SYSTEM OF INSTRUCTION rsr QUANTITATIVE CHEMICAL ANALYSIS. BY DR. C. KEMIGIUS FRESENIUS, PROFESSOR OF CHEMISTRY AND NATURAL PHILOSOPHY, WIESBADEN. tet ($tt0U01i and EDITED BY 0. D. ALLEN, PH.D., PROFESSOR OF ANALYTICAL CHEMISTRY AND METALLURGY IN THE SHEFFIELD SCIENTIFIC SCHOOL YALE COLLEGE. WITH THE COOPERATION OF SAMUEL W. JOHNSON, M.A., PROFESSOR OF THEORETICAL AND AGRICULTURAL CHEMISTRY IN THE SHEFFIELD SCIENTIFIC SCHOOL. NEW YORK: JOHN WILEY & SONS, 15 ASTOR PLACE. 1881. tf> ol COPYRIGHT, 1881, BY JOHN WILEY & SONS. S. W. GRMN'S SON, Printer, Electrotyper and Binder, 74 Beekman Street, New York. EDITORS PKEFACE TO THE SECOND AMERICAN EDITIOK IN the preparation of this edition of Fresenius' Quantitative Analysis, the general plan announced by the editor of the first American edition in the preceding preface has been followed. Although the original work, as it appears in the last foreign editions, has been somewhat abridged, it is believed that little which is useful to the student has been omitted from the present work. All processes which are described are given with the full details, and, with few exceptions, as far as practicable in the lan- guage used by the author. The desired reduction of the bulk of the original treatise has been effected by the omission of one or more processes when several are given for the same purpose, or more rarely by the entire omission of a whole subject. The subjects omitted, in addition to those mentioned in the preceding preface, are : " The Determination of the Equivalent of Organic Compounds," "The Assay of Silver Ores," and "The Assay of Gold Ores." On the other hand, many new processes and modifications of old processes appearing in the recently pub- lished first volume of the sixth German edition are included, and may be regarded as valuable additions to the General Part. Additions made by the editors are usually distinguished by en- closure in brackets [ ]. The more important additions of this kind are in those chap- ters (in the Special Part) which treat of the analysis of products pertaining to the Metallurgy of Iron and to Commercial Fertilizers. The entire chapter on the latter subject has been prepared by Professor S. W. Johnson and Dr. E. H. Jenkins, Chemist of the Connecticut Agricultural Experiment Station. It describes the 374258 IV PREFACE. methods and plans of analysis adopted in that institution after much experience and research. The new system of chemical notation and nomenclature is employed throughout the book, although the old system is still retained even in the last foreign editions. It is confidently be- lieved that this change, so long deferred for reasons perhaps sufficiently valid, can at the present time be made with advantage -to the student and instructor. The editor is under obligation to Messrs. W. J. Comstock and A. B. Howe, Ph.D., instructors in the Sheffield Laboratory, and to Professor W. G. Mixter, of the Sheffield Scientific School, for information and advice which their experience has en; bL'd them to give regarding many processes, and for valuable assistance in various other ways. The task of preparing this edition was undertaken and carried out with the generous co-operation of Professor S. W. Johnson. To him, therefore, most . especially are due thanks from the editor and from those who may believe that they find any advantage in the possession of the book in its present form. O. D. ALLEN. SHEFFIELD LABORATORY OF YALE COLLEGE, Feb., 1881. EDITOK'S PKEFACE TO THE FIKST AMEKICAN EDITIOK IN preparing this edition of Fresenius' Quantitative Chemical Analysis, the editor has sought by various changes to adapt it to the wants of the American student. The foreign editions have attained such encyclopedic dimen- sions as to occasion the beginner no little confusion and embarrass- ment. For this reason the bulk of the work has been considerably reduced. A few processes which the editor's experience has con- vinced him are untrustworthy, and many more that can well be spared because they are tedious or unnecessary, have been omitted. The entire chapter on Analysis of Mineral Waters, excellent as it is, has been suppressed on account of its length, and because the few who have occasion to make detailed investigations in th^t direction have access to the original sources of information. The section on Organic Analysis has been reduced from sixty to thirty pages, mainly by the omission of processes which, from their antiquity or inferiority, are more curious than useful. The chapters on Acidimetry and Alkalimetry have been likewise greatly condensed, and all that especially relates to Soils and Ashes of Plants has been left out. The recent appearance of an excellent special treatise on " Agricultural Chemical Analysis " by Professor Caldwell, of Cornell University, justifies the last-mentioned omis- sion. On the other hand, some important matter has been added. Bunsen's invaluable new methods of treating precipitates are described in his own (translated) words. Yarious new methods of estimation and separation are incorporated in their proper places. The editor thankfully acknowledges his indebtedness to several gentlemen for special contributions to this work, viz. : To Dr. J". Lawrence Smith, who has kindly furnished a manuscript account Vi PREFACE. of his admirable method of fluxing silicates for the estimation of alkalies. To O. D. Allen, Esq., late chemist to the Freedom Iron Works, Lewistown, Pennsylvania, for copious notes of his exten- sive experience in the analyses of steel, iron, and iron ores, which have been freely employed in 229. To Mr. William G. Mixter, chief assistant in the Sheffield Laboratory, for the account of the .gold and silver assay. To Professor Brush, of Yale College, Pro- fessor Collier, of Vermont University, and B. S. Burton, Esq., of Philadelphia, for various important facts and suggestions. Just before going to press, Dr. Wolcott Gibbs has communicated an account of his new method of finding at once the total correction for temperature, pressure, and moisture in absolute determinations of nitrogen or other gases, which, from its simplicity, convenience, and accuracy, must prove of the highest service in chemistry. It will be found in the Appendix, p. 838. The additions which have been made to the methods of exam- ining ores, it is believed, adapt the work to meet all the ordinary requirements of the metallurgical and mining student. The editor's additions are distinguished; in all important cases, by enclosure in brackets, [ ]. While fully recognizing the necessity of teaching the new notation and nomenclature of chemistry, the editor has in this book retained the old system, because it is identified with the chemical literature of the century, and cannot be speedily forgot- ten by practical men. At a time when the most elementary text- books are framed on the " modern" system, it is important to keep the student exercised in the language of the old masters of the science, which is still, and must for some time remain, a part of the vernacular of the physician, the apothecary, the metallurgist, and the manufacturer. SAMUEL W. JOHNSON. SHEFFIELD LABORATORY OF YALE COLLEGE, Dec., 1869. CONTENTS. PAGX INTRODUCTION , ,....,... 1 PART I. SECTION I. Operations, 1 11 I. Determination of quantity, 2 , 11 1. Weighing, 3 11 a. The balance 12 Accuracy, 4 12 Sensibility, 5 14 Testing, 6 and 7 17 b. The weights, 8 18 c. The process of weighing, 9 20 Rules, 10 22 2. Measuring, 11 24 a. The measuring of gases, 12 25 Correct reading-off, 13 27 Influence of temperature, 14 28 Influence of pressure, 15 29 Influence of moisture, 16 29 b. The measuring of fluids, 17 30 a. Measuring vessels graduated to hold certain volumes of fluid. aa. Vessels serving to measure out one definite volume of fluid. 1. Measuring flasks, 18 30 bb. Vessels serving to measure out different volumes of fluid. 2. The graduated cylinder, 19 32 ft. Measuring vessels graduated to deliver certain volumes of fluid. eta. Vessels serving to measure out one definite volume of fluid. viii CONTENTS. PAGE 3. The graduated pipette, 20 33 bb. Vessels serving to measure out different volumes of fluid. 4. The Burette. I. Mohr's burette, 21 36 II. Gay-Lussac's burette, 22 40 III, Geissler's burette, 23 41 II. Preliminary operations. Preparation of substances for the processes of quantitative analysis. 1. Selection of the sample, 24 42 2. Mechanical division, 25 43 3. Drying, 26 46 Desiccators, 27 , 48 Water-baths, 28 49 Air-baths, 29 52 Parafflne-baths, 30 54 III. General procedure in quantitative analysis, 32 55 1. Weighing the substance, 33 56 2. Estimation of water, 34 57 a. Estimation of water by loss of weight, 35 58 b. Estimation of water by direct weighing, 36 60 3. Solution of substances, 37 63 a. Direct solution, 38 64 b. Decomposition by fluxing, 39 65 4. Conversion of the dissolved substance into a weighable form, 40 66 a. Evaporation, 41 66 Weighing of residues, 42 72 b. Precipitation, 43 74 a. Separation of precipitates by decantation, 44 75 /?. Separation of precipitates by filtration, 45 76 aa. Filtering apparatus 77 bb. Rules to be observed in the process of filtration, 46 79 cc. Washing of precipitates, 47 81 y. Separation of precipitates by decantation and filtra- tion combined, 48 82 Further treatment of precipitates preparatory to weigh- ing, 49 83 aa. Drying of precipitates, 50 84 bb. Ignition of precipitates, 51 85 First method, 52 88 Second method, 53 90 Bunsen's method of rapid filtration, 53, a 91 Bunsen's simplified exhausting apparatus, 53, b 97 Bunsen's method of igniting precipitates, 53, c 98 Use of asbestos filters, 53, d 100 5. Volumetric analysis, 54 102 CONTENTS. IX SECTION II. PAGE Reagents, 55 105 A. Reagents for gravimetric analysis in the wet way. I. Simple solvents, 56 105 II. Acids and halogens. a. Oxygen acids, 57 106 b. Hydrogen acids and halogens, 58 107 c. Sulpho-acids 109 III. Bases and metals. a. Oxygen bases and metals. a. Alkalies, and ft. Alkaline earths, 59 109 y. Heavy metals and oxides of heavy metals, 60 110 b. Sulpho-bases Ill IV. Salts. a. Salts of the alkalies, 61 Ill b. Salts of the alkali-earth metals, 62 112 c. Salts of the heavy metals, 63 113 B. Reagents for gravimetric analysis in the dry way, 64 114 C. Reagents for volumetric analysis, 65 117 D. Reagents for organic analysis, 66 123 SECTION HI. Forms and combinations in which substances are separated from each other, or weighed, 67 130 A. BASIC RADICALS. FIRST GROUP. 1. Potassium, 68 132 2. Sodium, 69 135 3. Ammonium, 70 137 SECOND GROUP. 1. Barium, 71 138 2. Strontium, 72 '. 141 3. Calcium, 73 143 4. Magnesium, 74 146 THIRD GROUP. 1. Aluminium, 75 149 2. Chromium, 76 151 FOURTH GROUP. 1. Zinc, 77 153 2. Manganese, 78 155 X CONTENTS. PAGE 3. Nickel, 79 159 4. Cobalt, 80 161 5. Ferrous iron ; and 6. Ferric iron, 81 164 FIFTH GROUP. 1. Silver, 82 167 2. Lead, 83 170 3. Mercury in mercurous; and 4. in mercuric compounds, 84 174 5. Copper, 85 177 6. Bismuth,86 180 7. Cadmium, 87. 182 SIXTH GROUP. 1. Gold,88 184 2. Platinum, 89 184 3. Antimony, 90 185 4. Tin in stannous; and 5. in stannic compounds, 91 188 6. Arsenious acid; and 7. Arsenic acid, 92 190 B. ACIDS. FIRST GROUP, 93. 1. Arsenious and arsenic acids. 2. Chromic acid 193 3. Sulphuric acid 195 4. Phosphoric acid 195 5 Boracic acid 200 6. Oxalic acid 200 7. Hydrofluoric acid 200 8. Carbonic acid 201 9. Silicic acid 201 SECOND GROUP, 94. 1. Hydrochloric acid 203 2. Hydrobromic acid 203 3. Hydriodic acid 204 4. Hydrocyanic acid 205 5. Hydrosulphuric acid 205 THIRD GROUP, 95. 1. Nitric acid 206 2. Chloric acid 206 SECTION IV. Determination of radicals, 96 207 I. Determination of basic radicals 210 FIRST GROUP. 1. Potassium, 97 210 2. Sodium, 98 215 CONTENTS. Xl PAGE 3. Ammonium, 99 217 Supplement to first group, 100. 4. Lithium 226 SECOND GROUP. 1. Barium, 101 227 2. Strontium, 102 230 3. Calcium, 103 232 4. Magnesium, 104 237 THIRD GROUP. 1. Aluminium, 105 240 2. Chromium, 106 1 243 Supplement to third group, 107. 3. Titanium 245 FOURTH GROUP. 1. Zinc, 108 247 2. Manganese, 109 251 3. Nickel, 110 258 4. Cobalt, 111 262 5. Ferrous iron, 112 265 6. Ferric iron, 113 275 Supplement to fourth group, 114 7. Uranium 281 FIFTH GROUP. 1. Silver, 115 283 2. Lead, 116 297 3. Mercury in mercurous compounds, 117 304 4. Mercury in mercuroic compounds, 118 306 5. Copper, 119 31 1 6. Bismuth, 120 318 7. Cadmium, 121 323 Supplement to fifth group, 122. 8. Palladium 325 SIXTH GROUP. 1. Gold, 123 326 2. Platinum, 124 329 3. Antimony, 125 831 4. Tin in stannous; and 5. in stannic compounds, 126 338 6. Arsenious acid ; and 7. Arsenic acid, 127 344 Supplement to sixth group, 128. 8. Molybdic acid 353 II. Estimation of the acids. FIRST GROUP. First Division. 1. Arsenious and arsenic acids, 129 355 xii CONTENTS. PAGE 2. Chromic acid, 130 355 Supplement, 131. 1. Selenious acid 361 2. Sulphurous acid . 363 3. Thiosulplmric acid 364 4. lodic acid 364 5. Nitrous acid 365 Second Division. Sulphuric acid, 132 366 Supplement, 133. Hydrofluosilicic acid 372 Third Division. 1. Phosphoric acid. I. Determination, 134 373 II. Separation from the bases, 135 383 2. Boric acid, 136 389 3. Oxalic acid, 137 394 4. Hydrofluoric acid, 138 396 Fourth Division. 1. Carbonic acid, 139 403 2. Silicic acid, 140 419 SECOND GROUP. 1. Chlorine (Hydrochloric acid), 141 428 Supplement: free chlorine, 142 434 2. Bromine (Hydrobromic acid), 143 436 Supplement: free bromine, 144 439 3. Iodine (Hydriodic acid), 145 439 Supplement : free iodine, 146 44 B 4. Cyanogen (Hydrocyanic acid), 147 449 5. Sulphur (Hydrosulphuric acid), 148 457 THIRD GROUP. 1. Nitric acid, 149 469 2. Chloric acid, 150. 476 SECTION V. Separation of bodies, 151 478 I. SEPARATION OF BASIC RADICALS FROM EACH OTHER. FIRST GROUP. Separation of the alkalies from each other, 152 481 SECOND GROUP. I. Separation of the basic radicals of the second group from those of the first, 153 ; 488 CONTENTS. PAGE II. Separation of the basic radicals of the second group from eacn other, 154 . 493 THIRD GROUP. I. Separation of aluminium and chromium from the alkalies, 155 499 II. Separation of aluminium and chromium from the alkali-earth metals, 156 500 III. Separation of aluminium and chromium from each other, 157 506 FOURTH GROUP. I. Separation of the metals of the fourth group from the alkalies, 158. . 507 II. Separation of the metals of the fourth group from those of the second, 159 509 III. Separation of the metals of the fourth group from those of the third and from each other, 160 512 IV. Separation of iron, aluminium, manganese, calcium, magnesium, potas- sium, and sodium, 161 529 Separation of uranium from the metals of groups I. IV 532 FIFTH GROUP. I. Separation of the metals of the fifth group from those of the preced- ing four groups, 162 536 II. Separation of the metals of the fifth group from each other, 163 543 SIXTH GROUP. I. Separation of the metals of the sixth group from Lhose of the first five groups, 164 554 II. Separation of the metals of the sixth group from each other, 165. . . 569 IL SEPARATION OF ACIDS FROM EACH OTHER. FIRST GROUP. Separation of the acids of the first group from each other, 166 580 SECOND GROUP. I. Separation of the acids of the second group from those of the first, 167 588 Supplement. Analysis of compounds containing sulphides of the alkali metals, carbonates, sulphates, and thiosulphates, 168 591 II. Separation of the acids of the second group from each other, 169. . . 532 THIRD GROUP. I. Separation of the acids of the third group from those of the two first groups, 170 602 II. Separation of the acids of the third group from each other 603 CONTENTS. SECTION VI. PAGE Ultimate analysis of organic bodies, 171 604 I. Qualitative, 172 606 II. Quantitative, 173 609 A. Substances consisting of carbon and hydrogen, or of carbon, hydro- gen, and oxygen. a. Solid bodies. Combustion with oxide of copper, 174 610 Completion of the combustion by oxygen gas, 176 620 Combustion with lead chromate (and potassium dichromate) 177 620 Combustion with oxide of copper and oxygen gas, 178 621 Volatile bodies, or bodies undergoing alteration at 100, 179. 627 b. Liquid bodies. a. Volatile bodies, 180 627 ft. Non-volatile bodies, 181 630 Supplement to A. Modified apparatus for absorption of carbonic acid, 182 631 B. Substances consisting of carbon, hydrogen, oxygen, and nitrogen. a. Estimation of carbon and hydrogen, 183 633 b. Estimation of nitrogen. a. From the volume, 184 635 /?. By conversion into ammonia, after Varrentrapp and Will, 185 644 C. Analysis of bodies containing sulphur, 186 649 D. Estimation of phosphorus in organic bodies, 187. 660 E. Analysis of substances containing chlorine, bromine, or iodine, 188 661 F. Analysis of organic substances containing inorganic bodies, 189.. 664 PART II. SPJCCI^JL, 1. Analysis of fresh water, 190 ..................................... 669 2. Acidimetry. A. Estimation by specific gravity, 191 .......................... 675 B. Determination of the acid by saturation with an alkaline fluid of known strength, 192 .................. ................. 675 Kiefer's modification of the process, 193 ................ 689 3. Alkalimetry. A. Estimation of potassa, soda, or ammonia, from the density of their solutions, 194 ...................................... 691 B. Estimation of the amount of caustic and carbonated alkali in commercial alkalies ................. 691 CONTENTS. XV / PAGE Method of Descroizilles and Gay-Lussac, 195. . . 692 Modification by Mobr, 196 694 C. Estimation of caustic alkali in the presence of carbonates, 197. 695 D. Estimation of sodium carbonate in presence of potassium car- bonate 696 4. Estimation of alkali-earth metals by the alkalimetric method, 198. . . 697 5. Chlorimetry, 199. 698 Preparation of the solution of chloride of lime 699 A. Penot's method, 200 699 B. Otto's method, 201 701 Modification 703 C. Bunsen's method 703 6. Valuation of manganese, 202 704 I. Drying the sample 704 II. Determination of the manganese dioxide, 203 705 A. Fresenius and Will's method 705 B. Bunsen's method 709 C. Method by means of iron 709 III. Estimation of moisture in manganese, 204 710 IV. Estimation of the amount of hydrochloric acid required for the complete decomposition of a manganese, 205 711 7. Analysis of common salt, 206 711 8. Analysis of gunpowder, 207 713 9. Analysis of silicates and siliceous rocks, 208 714 10. Separation of silicates decomposable from those undecomposable by acids, 209 719 11. Analysis of limestones, dolomites, marls, &c 720 A. Complete analysis, 210 721 B. Volumetric determination of calcium carbonate, &c., 211 726 12. Assay of copper ores, 212 728 13. Assay of lead ores, 213 730 14. Determination of nickel and cobalt in ores, &c., 214 731 15. Assay of zinc ores, 215 737 16. Partial analysis of iron ores, 216 740 17. Complete analysis of iron ores, 217 753 18. Analysis of pig iron, steel, and wrought iron, 218 758 I. Pigiron 758 II. Steel and wrought iron 765 19. Analysis of coal and peat, 219 765 20. Analysis of commercial fertilizers, 220 767 21. Analysis of atmospheric air, 221 772 A. Determination of water and carbonic acid, 222 , 772 B. Determination of oxygen and nitrogen, 223 779 22. Detection and estimation of arsenic in organic matter, 224 781 XVl CONTENTS. PAET III. PAGE Exercises for practice 789 APPENDIX. Analytical experiments 809 Calculation of analyses 834 I. Calculation of the constituent sought from the compound produced, and exhibition of the results in per-cents 834 1. When the substance sought has been separated in the free state. a. Solid bodies, liquids, or gases, which have been determined by weight 834 b. Gases which have been measured 835 2. When the substance sought has been separated in combination with another 839 3. Calculation of indirect analyses 841 Supplement to I. Remarks on loss and excess, and on taking the average 842 II. Deduction of formulae 844 Tables for the calculation of analyses 849 872 I. Atomic weights of the elements 849 II. Composition of basic and acid oxides 849 III. Reduction of compounds found to constituents sought by simple multiplication or division 854 IV. Amount of constituent sought for each number of compound found 856 V. Specific gravity and absolute weight of several gases 872 VI. Comparison of degrees of mercurial thermometer with those of air thermometer. . 872 INTRODUCTION. As we have already seen in the " Manual of Qualitative Analy- sis," to which the present work may be regarded as the sequel, Chemical Analysis comprises two branches, viz. : qualitative analysis and quantitative analysis, the object of the former being to ascertain the nature, that of the latter to determine the amount, of the several component parts of any compound. By QUALITATIVE ANALYSIS we convert the unknown constituents of a body into certain known forms and combinations ; and we are thus enabled to draw correct inferences respecting the nature of these unknown constituents. Quantitative analysis attains its ob- ject, according to circumstances, often by very different ways ; the two methods most widely differing from each other, are analysis by weight, or gravimetric analysis, and analysis lyy measure, or volumetric analysis. GRAVIMETRIC ANALYSIS has for its object to convert the known constituents orf a substance into forms or combinations which will admit of the most exact determination of their weight, and of which, moreover, the composition is accurately known. These new forms or combinations may be either educts from the analyzed sub- stance, or they may be products. In the former case the ascer- tained weight of the eliminated substance is the direct expression of the amount in which it existed in the compound under exami- nation ; whilst in the latter case, that is, when we have to deal with products, the quantity in which the eliminated constituent was ori- ginally present in the analyzed compound, has to be deduced by calculation from the quantity in which it exists in its new com- bination. The following example will serve to illustrate these points : Suppose we wish to determine the quantity of mercury contained 2 INO/RODUCTION. in the chloride of that metal ; now, we may do this, either by pre- cipitating the metallic mercury from the solution of the chloride, say by means of stannous chloride ; or we may attain our object by precipitating the solution by sulphuretted hydrogen, and weighing the precipitated mercuric sulphide. 100 parts of mercuric chloride consist of 73*82 of mercury and 26*18 of chlorine ; consequently, if the process is conducted with absolute accuracy, the precipitation of mercury in 100 parts of mercuric chloride by stannous chloride will yield 73*82 parts of metallic mercury. With equally exact manipulation the other method yields 85*634 parts of mercuric sulphide. Now, in the former case we find the number 73*82 directly ; in the latter case we have to deduce it by calculation : (100 parts of mercuric sulphide contain 86*207 parts of mercury ; how much mercury do 85*634 parts contain ?) 100 : 85*634:: 86*207 : x x = 73'82. As already hinted, it is absolutely indispensable that the forms into which bodies are converted for the purpose of estimation by weight should fulfil two conditions : first, they must be capable of being weighed exactly; secondly, they must be of s known composi- tion, for it is quite obvious, on the one hand, that accurate quan- titative analysis must be altogether impossible if the substance the quantity of which it is intended to ascertain, does not admit of correct weighing; and on the other hand, it is equally evident that if we do not know the exact composition of a new product, we lack the necessary basis of our calculation. YOLUMETRIC ANALYSIS is based upon a very different principle from that of gravimetric analysis ; viz., it effects the quantitative determination of a body, by converting it from a certain definite state to another equally definite state, by means of a fluid of accu- rately known power of action, and under circumstances which per- mit the analyst to mark with rigorous precision the exact point when the conversion is accomplished. The following example will serve to illustrate the principle of this method : Potassium per- manganate added to a solution of ferrous sulphate, acidified with sulphuric acid, immediately converts the ferrous sulphate into fer- ric sulphate ; the permanganic acid, which is characterized by its intense color, yielding np oxygen and forming with the free sul- INTRODUCTION. 3 phuric acid present colorless manganous sulphate. If, therefore, to an acidified fluid containing a ferrous salt we add, drop by drop, a solution of potassium permanganate, its red color continues for some time to disappear upon stirring ; but at last a point is reached when the coloration imparted to the fluid by the last drop added remains ; this point marks the termination of the conversion of the ferrous salt into a ferric salt. If now we convert a known weight of iron into a ferrous sul- phate by dissolving it in dilute sulphuric acid, and ascertain by suitable measuring apparatus the volume of a solution of potassium permanganate required to convert the ferrous sulphate to ferric sulphate, we can by means of this permanganate solution determine unknown quantities of ferrous iron in a solution. This is accom- plished by adding the permanganate solution until the above de- scribed reaction is completed, and noting the volume used. The amount of iron present can now be calculated by comparing the volume used with that used when a known quantity of iron was present, as the weight of iron must in both cases be proportional to volume of permanganate used. To this brief intimation of the general purport and object of quantitative analysis, and the general mode of proceeding in ana- lytical researches', I have to add that certain qualifications are essen- tial to those who would devote themselves successfully to the pursuit of this branch. These qualifications are, 1, theoretical knowledge ; 2, skill in manipulation ; and 3, strict conscientious- ness. The preliminary knowledge required consists in an acquaintance with qualitative analysis, the stoichiornetric laws, and simple arith- metic. Thus prepared, we shall understand the method by which bodies are separated and determined, and we shall be in a position to perform our calculations, by which, on the one hand, the formu- lae of compounds are deduced from the analytical results, and, on the other hand, the correctness of the adopted methods is tested, and the results obtained are controlled. To this knowledge must be joined the ability of performing the necessary practical opera- tions. This axiom generally holds good for all applied sciences, but if it is true of one more than another, quantitative analysis is that one. The most extensive and solid theoretical acquirements will not enable us, for instance, to determine the amount of com- mon salt present in a solution, if we are without the requisite dex- 4 INTRODUCTION. teritj to transfer a fluid from one vessel to another without the smallest loss by spirting, running down the side, &c. The various operations of quantitative analysis demand great aptitude and man- ual skill, which can be acquired only by practice. But even the possession of the greatest practical skill in manipulation, joined to a thorough theoretical knowledge, will still prove insufficient to insure a successful pursuit of quantitative researches, unless also combined with a sincere love of truth and a firm determination to accept none but thoroughly confirmed results. Every one who has been engaged in quantitative analysis knows that cases will sometimes occur, especially when commencing the study, in which doubts may be entertained as to whether the result will turn out correct, or in which even the operator is positively convinced that it cannot be quite correct. Thus, for instance, a small portion of the substance under investigation may be spilled ; or some of it lost by decrepitation ; or the analyst may have reason to doubt the accuracy of his weighing ; or it may happen that two analyses of the same substance do not exactly agree. In all such cases it is indispensable that the operator should be conscientious enough to repeat the whole process over again. He who is not possessed of this self-command who shirks trouble where truth is at stake who would be satisfied with mere assumptions and guess- work, where the attainment of positive certainty is the object, must be pronounced just as deficient in the necessary qualifications for quantitative analytical researches as he who is wanting in knowl- edge or skill. He, therefore, who cannot fully trust his work r who cannot swear to the correctness of his results, may indeed oc- cupy himself with quantitative analysis by way of practice, but he ought on no account to publish or use his results as if they were positive, since such proceeding could not conduce to his own ad- vantage, and would certainly be mischievous as regards the science. The domain of quantitative analysis may be said to extend over all matter that is, in other words, anything corporeal may become the object of quantitative investigation. The present work, how- ever, is intended to embrace only the substances used in pharmacy, arts, trades, and agriculture. Quantitative analysis may be subdivided into two branches, viz., analysis of mixtures, and analysis of chemical compounds. This division may appear at first sight of very small moment, yet it is necessary that we should establish and maintain it, if we would INTRODUCTION. 5 form a clear conception of the value and utility of quantitative research. The quantitative analysis of mixtures, too, has not the same aim as that of chemical compounds ; and the method applied to secure the correctness of the results in the former case is dif- ferent from that adopted in the latter. The quantitative analysis of chemical compounds also rather suttserves the purposes of the science, whilst that of mixtures belongs to the practical purposes of life. If, for instance, I analyze the salt of an acid, the result of the analysis will give me the constitution of that acid, its com- bining proportion, saturating capacity, &c. ; or, in other words, the results obtained will enable me to answer a series of questions of which the solution is important for the theory of chemical science : but if, on the other hand, I analyze gunpowder, alloys, medicinal mixtures, ashes of plants, &c., &c., I have a very different object in view ; I do not want in such cases to apply the results which I may obtain to the solution of any theoretical question in chemistry, but I want to render a practical service either to the arts and industries, or to some other science. If in the analysis of a chemi- cal compound I wish to control the results obtained, I may do this in most cases by means of calculations based on stoi'chiometric data, but in the case of a mixture a second analysis is necessary to confirm the correctness of the results afforded by the first. The preceding remarks clearly show the immense importance of quantitative analysis. It may, indeed, be averred that chemistry owes to this branch its elevation to the rank of a science, since quantitative researches have led us to discover and determine the laws which govern the combinations and transpositions of the ele- ments. Stoichiometry is entirely based upon the results of quan- titative investigations ; all rational views respecting the constitution of compounds rest upon them as the only safe and solid basis. Quantitative analysis, therefore, forms the strongest and most powerful lever for chemistry as a science, and not less so for chemis- try in its applications to the practical purposes of life, to trades, arts, manufactures, and likewise in its application to other sciences. It teaches the mineralogist the true nature of minerals, and suggests to him principles and rules for their recognition and classification. It is an indispensable auxiliary to the physiologist ; and agriculture has already derived much benefit from it ; but far greater benefits may be predicted. We need not expatiate here upon the advan- tages which medicine, pharmacy, and every branch of industry 6 INTRODUCTION. derive, either directly or indirectly, from the practical application of its results. On the other hand, the benefit thus bestowed by quantitative analysis upon the various sciences, arts, etc., has been in a measure reciprocated by some of them. Thus whilst stoichio- metry owes its establishment to quantitative analysis, the stoichio- metric laws afford us the means of controlling the results of our analyses so accurately as to justify the reliance which we now gen- erally place on them. Again, whilst quantitative analysis has advanced the progress of arts and industry, our manufacturers in return supply us with the most perfect platinum, glass, and por- celain vessels, and with articles of india-rubber, without which it would be next to impossible to conduct our analytical operations with the minuteness and accuracy which we have now attained. Although the aid which quantitative analysis thus derives from stoichiometry, and the arts and manufactures, greatly facilitates its practice, and although many determinations are con- siderably abbreviated by volumetric analysis, it must be admitted, notwithstanding, that the pursuit of this branch of chemistry requires considerable expenditure of time. This remark applies especially to those who are commencing the study, for they must not allow their attention to be divided upon many things at one time, otherwise the accuracy of their results will be more or less injured. I would therefore advise every one desirous of becoming an analytical chemist to arm himself with a considerable share of patience, reminding him that it is not at one bound, but gradually, and step by step, that the student may hope to attain the neces- sary certainty in his work, the indispensable self -reliance which can alone be founded on one's own results. However mechanical, protracted, and tedious the operations of quantitative analysis may appear to be, the attainment of accuracy will amply compensate for the time and labor bestowed upon them ; whilst, on the other hand, nothing can be more disagreeable than to find, after a long and laborious process, that our results are incorrect or uncertain. Let him, therefore, who would render the study of quantitative analysis agreeable to himself, from the very outset endeavor, by strict, nay, scrupulous adherence to the conditions laid down, to attain correct results, at any sacrifice of time. 1 scarcely know a better and more immediate reward of labor than that which springs from the attainment of accurate results and perfectly correspond- ing analyses. The satisfaction enjoyed at the success of our efforts INTRODUCTION. 7 is surely in itself a sufficient motive for the necessary expenditure of time and labor, even without looking to the practical benefits which we may derive from our operations. The following are the substances treated of in this work : I. METALLOIDS, or NON -METALLIC ELEMENTS. Oxygen, Hydrogen, Sulphur, [Selenium,] Phosphorus, Chlo- rine, Iodine, Bromine, Fluorine, Nitrogen, Boron, Silicon, Car- bon. II. METALS. Potassium, Sodium, [Lithium,'] Barium, Strontium, Calcium, Magnesium, Aluminium, Chromium, [Titanium,] Zinc, Manga- nese, Nickel, Cobalt, Iron, [Uranium,'] Silver, Mercury, Lead, Copper, Bismuth, Cadmium, [Palladium,'] Gold, Platinum, Tin, Antimony, Arsenic, [Molybdenum]. (The elements enclosed within brackets are considered in sup- plementary paragraphs, and more briefly than the rest.) I have divided my subject into three parts. In the first, I treat of quantitative analysis generally ; describing the execution of anal- ysis. In the second, I give a detailed description of several special analytical processes. And in the third, a number of carefully se- lected examples, which may serve as exercises for the groundwork of the study of quantitative analysis. The following table will afford the reader a clear and definite notion of the contents of the whole work : I. GENERAL PART. 1. Operations. 2. Reagents. 3. Forms and combinations in which bodies are separated from others, or in which their weight is determined. 4. Determination of bodies in simple compounds. 5. Separation of bodies. 6. Organic elementary analysis. 8 INTRODUCTION. II. SPECIAL PAET. 1. Analysis of waters. 2. Analysis of such minerals and technical products as are most frequently brought under the notice of the chemist ; including methods for ascertaining their commercial value. 3. Analysis of atmospheric air. III. EXERCISES FOR PRACTICE. APPENDIX. 1. Analytical experiments. 2. Calculation of analyses. 3. Tables for calculation. TP.AJRT I. GENERAL PART, THE EXECUTION OF ANALYSIS. SECTION I. OPERATIONS. 1. MOST of the operations performed in quantitative research are the same as in qualitative analysis, and have been accordingly described in my work on that branch of analytical science. With respect to such operations I shall, therefore, confine myself here to pointing out any modifications they may require to adapt them for applica- tion in the quantitative branch ; but I shall, of course, give a full description of such as are resorted to exclusively in quantitative investigations. Operations forming merely part of certain speci- fic processes will be found described in the proper place, under the head of such processes. I. DETERMINATION OF QUANTITY. 2. The quantity of solids is usually determined by weight / the quantity of gases and fluids, in many cases by measure upon the care and accuracy with which these operations are performed, de- pends the value of all our results ; I shall therefore dwell minutely upon them. O O. 1. WEIGHING. To enable us to determine with precision the correct weight of a substance, it is indispensable that we should possess, 1st, a good BALANCE, and 2d. accurate WEIGHTS. 12 OPERATIONS. a. THE BALANCE. Fig. 1 represents a form of balance well adapted for analytical purposes. There are several points respecting the construction and properties of a good balance, which it is absolutely necessary for every chemist to understand. The usefulness of this instrument depends upon two points : 1st, its accuracy r , and 2d, its sensibility or delicacy. 4- The ACCURACY of a balance depends upon the following condi- tions : a. The fulcrum or the point on which the beam rests must lie above the centre of gravity of the balance. Fig. 1. This is in fact a condition essential to every balance. If the fulcrum were placed in the centre of gravity of the balance, the beam would not oscillate, but remain in any position in which it is placed, assuming the scales to be equally loaded. If the fulcrum be placed below the centre of gravity, the balance will be overset by the slightest impulse. When the fulcrum is above the centre of gravity the balance represents a pendulum, the length of which is equal to that of the line uniting the fulcrum with the centre of gravity, and this line forms right angles with the beam, in whatever position the latter may be placed. Now if we impart an impetus to a ball suspended by a thread, the ball, after having terminated its vibrations, will WEIGHING. 13 invariably rest in its original perpendicular position under the pointof suspension. It is the same with a properly adjusted bal- ance impart an impetus to it, and it will oscillate for some time, but it will invariably return to its original position ; in other words, its centre of gravity will finally fall back into its perpen- dicular position under the fulcrum, and the beam must consequently reassume the horizontal position. But to judge correctly of the force with which this is accom- plished, it must be borne in mind that a balance is not a simple pendulum, but a compound one, i. e., a pendulum in which not one, but many material points move round the turning point. The inert mass to be moved is accordingly equal to the sum of these ppints, and the moving force is equal to the excess of the material points below, over those above the fulcrum. ft. The points of suspension of the scales must ~be on an exact level with the fulcrum. If the fulcrum be placed below the line joining the points of suspension, increased loading of the scales will continually tend to raise the centre of gravity of the whole svstem, so as to bring it nearer and nearer the fulcrum ; the weight which presses upon the scales combining in the relatively high- placed points of suspension ; at last, when the scales have been loaded to a certain degree, the centre of gravity will shift alto- gether to the fulcrum, and the balance will consequently cease to vibrate any further addition of weight will finally overset the beam by placing the centre of gravity above the fulcrum. If, on the other hand, the fulcrum be placed above the line joining the points of suspension, the centre of gravity will become more and more depressed in proportion as the loading of the scales is in- creased ; the line of the pendulum will consequently be length- ened, and a greater force will be required to produce an equal turn ; in other words, the balance will grow less sensitive the greater the load. But when the three edges are in one plane, in- creased loading of the scales will, indeed, continually tend to raise the centre of gravity towards the fulcrum, but the former can in this case never entirely reach the latter, and consequently the bal- ance will never altogether cease to vibrate upon the further addi- tion of weight, nor will its sensibility be lessened ; on the contrary speaking theoretically a greater degree of sensibility is im- parted to it. This increase of sensibility is, however, compensated for by other circumstancas. (See 5.) 14 OPERATIONS. y. The beam must be sufficiently rigid to bear without bending the greatest weight that the construction of the balance admits of ; since the bending of the beam would of course depress the points of suspension so as to place them below the fulcrum, and this would, as we have just seen, tend to diminish the sensibility of the balance in proportion to the increase of the load. It is, therefore, necessary to avoid this fault by a proper construction of the beam. The form best adapted for beams is that of an isosceles obtuse- angled triangle, or of a rhombus. d. The arms of the balance must be of equal length, i. e., the points of suspension must be equidistant from thefulcru7n^ for if the arms are of unequal length the balance will not be in equili- brium, supposing the scales to be loaded with equal weights, but there will be preponderance on the side of the longer arm. 5. The SENSIBILITY of a balance depends principally upon the three following conditions : a. The friction of the edges upon their supports must be as slight as possible. The greater or less friction of the edges upon their supports depends upon both the form and material of those parts of the balance. The edges must be made of good steel, the supports may be made of the same material ; it is better, however, that the centre edge at least should rest upon an agate plane. To form a clear conception of how necessary it is that even the end edges should have as little friction as possible, we need simply reflect upon what would happen were we to fix the scales immov- bly to the beam by means of rigid rods. Such a contrivance would at once altogether annihilate the sensibility of a balance, for if a weight were placed upon one scale, this certainly would have a tendency to sink ; but at the same time the connecting rods be- ing compelled to form constantly a right angle with the beam, the weighted scale would incline inwards, whilst the other scale would turn outwards, and thus the arms would become unequal, the shorter arm being on the side of the weighted scale, whereby the tendency of the latter to sink would be immediately compensated for. The more considerable the friction becomes at the end edges of a balance, the more the latter approaches the state just now described, and consequently the more is its sensibility impaired. /?. The centre of gravity must be as near as possible to theful- WEIGHING. 15 crum. The nearer the centre of gravity approaches the fulcrum, the shorter becomes the pendulum. If we take two balls, the one suspended by a short and the other by a long thread, and impart the same impetus to both, the former will naturally swing at a far greater angle from its perpendicular position than the latter. The same must of course happen with a balance ; the same weight will cause the scale upon which it is placed to turn the more rapidly and completely, the shorter the distance between the centre of gravity and the fulcrum. We have seen above, that in a balance where the three edges are on a level with each other, increased loading of the scales will continually tend to raise the centre of gravity towards the fulcrum. A good balance will therefore be- come more delicate in proportion to the increase of weights placed upon its scales ; but, on the other hand, its sensibility will be di- minished in about the same proportion by the increment of the mass to be moved, and by the increased friction attendant upon the increase of load ; in other words, the delicacy of a good balance will remain the same, whatever may be the load placed upon it. The nearer the centre of gravity lies to the fulcrum, the slower are the oscillations of the balance. Hence in regulating the position of the centre of gravity we must not go too far, for if it ap- proaches the fulcrum too nearly, the operation of weighing will take too much time. y. The beam must be as light as possible. The remarks which we have just now made will likewise show how far the weight of the beam may influence the sensibility of a balance. We have seen that if a balance is not actually to become less delicate on increased loading, it must on the one hand have a tendency to become more delicate by the continual approach of the centre of gravity to the fulcrum. ]N"ow it is evident, that the more considerable the weight of the beam is, the less will an equal load placed upon both scales alter the centre of gravity of the whole system, the more slowly will the centre of gravity approach the fulcrum, the less will the increased friction be neutralized, and consequently the less sensi- bility will the balance possess. Another point to be taken into account here is, that the moving forces being equal, a lesser mass or weight is more readily moved than a greater. ( 4 a.) 6. We will now proceed, first, to give the student a few general 16 OPERATIONS. rules to guide him in the purchase of a balance intended for the purposes of quantitative analysis ; and, secondly, to point out the best method of testing the accuracy and sensibility of a balance. 1. A balance able to bear YO or 80 grammes in each scale, suf- fices for most purposes. 2. The balance must be enclosed in a glass case to protect it from dust. This case ought to be sufficiently large, and, more especially, its sides should not approach too near the scales. It must be constructed in a manner to admit of its being opened and closed with facility, and thus to allow the operation of weighing to be effected without any disturbing influence from currents of air. Therefore, either the front part of the case should consist of three parts, viz., a fixed centre part and two lateral parts, open- ing like doors ; or, if the front part happens to be made of one piece, and arranged as a sliding-door, the two sides of the case must be provided each with a door. 3. The balance must be provided with a proper contrivance to render it immovable whilst the weights are being placed upon the scale. This is most commonly effected by an arrangement which enables the operator to lift up the beam and thus to remove the middle edge from its support, whilst the scales remain suspended. It is highly advisable to have the case of the balance so arranged that the contrivances for lifting the beam and fixing the scales can be worked while the case remains closed, and consequently from without. 4. It is necessary that the balance should be provided with an index to mark its oscillations ; this index is appropriately placed at the bottom of the balance. 5. The balance must be provided with a spirit level, to enable the operator to place the three edges on an exactly horizontal level ; it is best also for this purpose that the case should rest upon three screws. 6. It is very desirable that the beam should be graduated into tenths, so as to enable the operator to weigh the milligramme and its fractions with a centigramme " rider."* 7. The balance must be provided with a screw to regulate the centre of gravity, and likewise with two screws to regulate the * [Becker's later balances have beams graduated to twelfths, and a rider weighing 12 mgrs. This enables the operator to use nearly the whole of the graduation.] .7] WEIGHING. 17 equality of the arms, and finally with screws to restore the equi- librium of the scales, should this have been disturbed. The following experiments serve to test the accuracy and sensi- bility of a balance. . 1. The balance is, in the first place, accurately adjusted, if necessary, either by the regulating screws, or by means of tinfoil, and a milligramme weight is then placed in one of the scales. A good and practically useful balance must turn very distinctly with this weight ; a delicate chemical balance should indicate the -^ of a milligramme with perfect 'distinctness. 2. Both scales are loaded with the maximum weight the con- struction of the balance will admit of the balance is then accu- rately adjusted, and a milligramme added to the weight in the one scale. This ought to cause the balance to turn to the same extent as in 1. In most balances, however, it shows somewhat less on the index. It follows from 5 ft that the balance will oscillate more slowly in this than in the first experiment. 3. The balance is accurately adjusted (should it be necessary to establish a perfect equilibrium between the scales by loading the one with a minute portion of tinfoil, this tinfoil must be left re- maining upon the scale during the experiment) ; both scales are then equally loaded, say, with fifty grammes each, and, if neces- sary, the balance is again adjusted (by the addition of small weights). The load of the two scales is then interchanged, so as to transfer that of the right scale to the left, and vice versa. A bal- ance with perfectly equal arms must maintain its absolute equilib- rium upon this interchange of the weights of the two scales. 4. The balance is accurately adjusted ; it is then arrested and again set in motion ; the same process should be repeated several times. A good balance must invariably reassume its original equi- librium. A balance the end edges of which afford too much play to the hook resting upon them, so as to allow the latter slightly to alter its position, will show perceptible differences in different trials. This fault, however, is possible only with balances of defec- tive construction. A balance to be practically useful for the purposes of quantita- tive analysis must stand the first, second, and last of these tests. A slight inequality of the arms is of no great consequence, as the 18 OPERATIONS. [ 8. error that it would occasion may be completely prevented by the manner of weighing. As the sensibility of a balance will speedily decrease if the steel edges are allowed to get rusty, delicate balances should never be kept in the laboratory, but always in a separate room. It is also advisable to place within the case of the balance a vessel half filled with calcined carbonate of potassa, to keep the air dry. I need hardly add that this salt must be re-calcined as soon as it gets, moist. b. THE WEIGHTS. 1. The French gramme is the best standard for calculation. A set of weights ranging from fifty grammes to one milligramme may be considered sufficient for all practical purposes. With re- gard to the set of weights, it is generally a matter of indifference for scientific purposes whether the gramme, its multiples arid frac- tions, are really and perfectly equal to the accurately adjusted nor- mal weights of the corresponding denominations ; * but it is abso- lutely necessary that they should agree perfectly with each other, i. 0., the centigramme weight must be exactly the one hundredth part of the gramme weight of the set, etc. etc. 2. The whole of the set of weights should be kept in a suitable, well-closing box ; and it is desirable likewise that a distinct com- partment be appropriated to every one even of the smaller weights. 3. As to the shape best adapted for weights, I think that of short frusta of ' cones inverted, with a handle at the top, the most convenient and practical form for the large weights ; square pieces of foil, turned up at one corner, are best adapted for the small weights. The foil used for this purpose should not be too thin, and the compartments adapted for the reception of the several smaller weights in the box, should be large enough to admit of their con- tents being taken out of them with facility, or else the smaller weights will soon get cracked, bruised, and indistinct. Every one * Still it would be desirable that mechanicians who make gramme-weights intended for the use of the chemist, should endeavor to procure normal Aveights. It is very inconvenient, in many cases, to find notable differences between weights of the same denomination, but coming from different makers; as I my- self have often had occasion to discover. 8.] WEIGHING. 19 of the weights (with the exception of the milligramme) should be distinctly marked. 4. With respect to the material most suitable for the manufac- ture of weights, we commonly rest satisfied with having the smaller weights only, from 1 or 0'5 gramme downwards, made of plati- num or aluminium foil, using brass weights for all the higher-de- nominations. Brass weights must be carefully shielded from the contact of acid or other vapors, or their correctness will be in- paired ; nor should they ever be touched with the fingers, but always with small pincers. But it is an erroneous notion to sup- pose that weights slightly tarnished are unfit for use. It is, in- deed, hardly possible to prevent weights for any very great length of time from getting slightly tarnished. I have carefully examined many weights of this description, and have found them as exactly corresponding with one another in their relative proportions as they were when first used. The tarnishing coat, or incrustation, is so extremely thin, that even a very delicate balance will gener- ally fail to point out any perceptible difference in the weight. The following is the proper way of testing the weights : One scale of a delicate balance is loaded with a one-gramme weight, and the balance is then completely equipoised by taring with small pieces of brass, and finally tinfoil (not paper, since this absorbs moisture). The weight is then removed, and replaced suc- cessively by the other gramme weights, and afterwards by the same amount of weight in pieces of lower denominations. The balance is carefully scrutinized each time, and any devi- ation from the exact equilibrium marked. In the same way it is seen whether the two-gramme piece weighs the same as two single grammes, the five-gramme piece the same as three single grammes and the two-gramme piece, &c. In the comparison of the smaller weights thus among themselves, they must not show the least dif- ference on a balance turning with ^ of a milligramme. In com- paring the larger weights with all the small ones, differences of jig- to T 2 o- of a milligramme may be passed over. If you wish them to be more accurate, you must adjust them yourself. In the purchase of weights chemists ought always to bear in mind that an accurate weight is truly valuable, whilst an inaccurate one is absolutely worthless. It is the safest way for the chemist to test every weight he purchases, no matter how high the reputation of the maker. 20 OPERATIONS. [ 9. 9- c. THE PROCESS OF WEIGHING. We 'have two different methods of determining the weight of substances ; the one might be termed direct weighing, the other is called weighing by substitution. In direct weighing, the substance is placed upon one scale, and the weight upon the other. If we possess a balance, the arms of which are of equal length, and the scales in a perfect state of equilibrium, it is indifferent upon which scale the substance is placed in the several weighings required during an analytical pro- cess ; i.e., we may weigh upon the right or upon the left side, and change sides at pleasure, without endangering the accuracy of our results. But if, on the contrary, the arms of our balance are not perfectly equal, or if the scales are not in a state of perfect equili- brium, we are compelled to weigh invariably upon the same scale, otherwise the correctness of our results will be more or less materi- ally impaired. Suppose we want to weigh one gramme of a substance, and to divide this amount subsequently into two equal parts. Let us assume our balance to be in a state of perfect equilibrium, but with unequal arms, the left being 99 millimetres, the right 100 millimetres long ; we place a gramme weight upon the left scale, and against this, on the right scale, as much of the substance to be weighed as will restore the equilibrium of the balance. According to the axiom, "masses are in equilibrium upon a lever, if the products of their weights into their distances from the fulcrum are equal," we have consequently upon the right scale 0'99 grm. of substance, since 99xl'00=100x0'99. If we now, for the purpose of weighing one half the quantity, remove the whole weight from the left scale, substituting a 0'5 grm. weight for it, and then take off part of the substance from the right scale, until the balance recovers its equilibrium, there will remain 0'495 grm. ; and this is exactly the amount we have removed from the scale : we have consequently accomplished our object with respect to the relative weight ; and as we have already remarked, the absolute weight is not generally of so much importance in scientific work. But if we attempted to halve the substance which we have on the right scale, by first removing both the weiglit and the substance 9.] WEIGHING. 21 from the scales, and placing subsequently a O5 grm. weight upon the right scale, and part of the substance upon the left, until the balance recovers its equilibrium, we should have 0*505 of substance upon the left scale, since 100x0-500=99x0.505; and conse- quently, instead of exact halves, we should have one part of the substance amounting to 0'505, the other only to 0-485. If the scales of our balance are not in a state of absolute equili- brium, we are obliged to weigh our substances in vessels to insure accurate results (although the arms of the balance be perfectly equal). It is self-evident that the weights in this case must like- wise be invariably placed upon one and the same scale, and that the difference between the two scales must not undergo the slighest variation during the whole course of a series of experi- ments. From these remarks result the two following rules : 1. It is, under all circumstances, advisable to place the sub- stance invariably upon one and the same scale most conveniently upon the left. 2. If the operator happens to possess a balance for his own private and exclusive use, there is no need that he should adjust it at the commencement of every analysis ; but if the balance be used in common by several persons, it is absolutely necessary to ascer- tain, before every operation, whether the state of absolute equili- brium may not have been disturbed. Weighing by substitution yields not only relatively, but also absolutely accurate results; no matter whether the arms of the balance be of exactly equal lengths or not, or whether the scales be in perfect equipoise or not. The process is conducted as follows : the material to be weighed say a platinum crucible is placed upon one scale, and the other scale is accurately counterpoised against it. The plati- num crucible is then removed, and the equilibrium of the balance restored by substituting weights for the removed crucible. It is perfectly obvious that the substituted weights will invariably express the real weight of the crucible with absolute accuracy. We weigh by substitution whenever we require the greatest pos- sible accuracy; as, for instance, in the determination of atomic weights. The process may be materially shortened by first placing a tare (which must of course be heavier than the substance to be weighed) upon one scale, say the left, and loading the other scale 22 OPERATIONS. [ 10. with weights until equilibrium is produced. This tare is always retained on the left scale. The weights after being noted are removed. The substance is placed on the right scale, together with the smaller weights requisite to restore the equilibrium of the balance. The sum of the weights added is then subtracted from the noted weight of the counterpoise : the remainder will at once indicate the absolute weight of the substance. Let us sup- pose, for instance, we have on the left scale a tare requiring a weight of fifty grammes to counterpoise it. We place a platinum crucible on the right scale, and find that it requires an addition of weight to the extent of 10 grammes to counterpoise the tare on the left. Accordingly, the crucible weighs 50 minus 10=40 grammes. 10. The following rules will be found useful in performing the process of weighing : 1. The safest and most expeditious way of ascertaining the exact weight of a substance, is to avoid trying weights at random ; instead of this, a strictly systematic course ought to be pursued in counterpoising substances on the balance. Suppose, for instance, we want to weigh a crucible, the weight of which subsequently turns out to be 6.627 grammes ; well, we place 10 grammes on the other scale against it, and we find this is too much ; we place the weight next in succession, i.e., 5 grammes, and find this too little ; next Y, too much; 6, too little ; 6'5, too little ; 6'7, too much ; 6'6, too little ; 6-65, too much ; 6'62, too little ; 6'63, too much ; 6'625, too little ; 6-627, right. I have selected here, for the sake of illustration, a most com- plicated case ; but this systematic way of laying on the weights will in most instances lead to the desired end, in half the time required when weights are tried at random. After a little prac- tice a few minutes will suffice to ascertain the weight of a sub- stance to within the y^ of a milligramme, provided the balance does not oscillate too slowly. 2. The milligrammes and fractions of milligrammes are deter- mined by a centigramme rider (to be placed on or between the divisions on the beam) far more expeditiously and conveniently than by the use of the weights themselves, and at the same time with equal accuracy. 10.] WEIGHING. 23 3. Particular care and attention should be bestowed on enter- ing the weights in the book. The best way is to write down the weights first by inference from the blanks, or gaps in the weight box, and to control the entry subsequently by removing the weights from the scale, and replacing them in their respective -compartments in the box. The student should from the com- mencement make it a rule to enter the number to be deducted in the lower line ; thus, in the upper line, the weight of the cruci- ble + the substance ; in the lower line, the weight of the empty crucible. 4. The balance ought to be arrested every time any change is contemplated, such as removing weights, substituting one weight for another, tfcc. etc., or it will soon get spoiled. 5. Substances (except, perhaps, pieces of metal, or some other bodies of the kind) must never be placed directly upon the scales, but ought to be weighed in appropriate vessels of platinum, silver, glass, porcelain, &c., never on paper or card, since these, being liable to attract moisture, are apt to alter in weight. * The most common method is to weigh in the first instance the vessel by itself, and to introduce subsequently the substance into it ; to weigh again, and subtract the former weight from the latter. In many instances, and more especially where several portions of the same substance are to be weighed, the united weight of the vessel and of its contents is first ascertained ; a portion of the contents is then shaken out, and the vessel weighed again ; the loss of weight expresses the amount of the portion taken out of the vessel. 6. Substances liable to attract moisture from the air, must be weighed invariably in closed vessels (in covered cru'cibles, for instance, or between two watch-glasses, or in a closed glass tube); fluids are to be weighed in small bottles closed with glass stoppers. 7. A vessel ought never to be weighed whilst warm, since it will in that case invariably weigh lighter than it really is. This is owing to two circumstances. In the first place, every body con- denses upon its surface a certain amount of air and moisture, the quantity of which depends upon the temperature and hygroscopic state of the air, and likewise on its own temperature. Now sup- pose a crucible has been weighed cold at the commencement of the operation, and is subsequently weighed again whilst hot, together with the substance it contains, and the weight of which we wish to determine. If we subtract for this purpose the 24 OPERATIONS. [ 11. weight of the cold crucible, ascertained in the former instance, from the weight found in the latter, we shall subtract too much, and consequently we shall set down less than the real weight for the substance. In the second place, bodies at a high temperature are constantly communicating heat to the air immediately around them; the heated air expands and ascends, and the denser and colder air, flowing towards the space which the former leaves, pro- duces a current which tends to raise the scale, making it thus appear lighter than it really is. 8. If we suspend from the end edges of a correct balance respectively 10 grammes of platinum and 10 grammes of glass, by wires of equal weight, the balance will assume a state of equili- brium ; but if we subsequently immerse the platinum and glass completely in water, this equilibrium will at once cease, owing to the different specific gravity of the two substances ; since, as is well known, substances immersed in water lose of their weight a quantity equal to the weight of their own bulk of water. If this be borne in mind, it must be obvious to every one that weighing in the air is likewise defective, inasmuch as the bulk of the -substance weighed is not the same with that of the weight. This defect, however, is so very insignificant, owing to the trifling specific gravity of the air in proportion to that of solid substances, that we may generally disregard it alto- gether in analytical experiments. In cases, however, where absolutely accurate results are required, the bulk both of the substance examined, and of the weight, must be taken into account, and the weight of the corresponding volume of air added respectively to that of the substance and of the weight, making thus the process equivalent to weighing in vacua. 11. 2. MEASURING. The process of measuring is confined in analytical researches mostly to gases and liquids. The method of measuring gases has been brought to such perfection that it may be said to equal in accuracy the method of weighing. However, such accurate meas- urements demand an expenditure of time and care, which can be 12.] MEASUKIX(T OF (4 ASKS. 25 bestowed only on the nicest and most delicate scientific investiga- tions.* The measuring of liquids in analytical investigations was resorted to first by DESCROIZILLES (" Alkali meter," 1806). GAY-LUSSAC materially improved the process, and indeed brought it to the highest degree of perfection (measuring of the solution of chloride of sodium in the assay of silver in the wet way). More recently F. MOHR+ has bestowed much care and ingenuity upon the pro- duction of appropriate and convenient measuring apparatus, and has added to our store the eminently practical compression stop- cock burette. The process is now resorted to even in most accurate scientific investigations, since it requires much less time than the process of weighing. The accuracy of all measurings depends upon the proper con- struction of the measuring vessels, and also upon the manner in which the process is conducted. a. THE MEASURING OF GASES. We use for the measuring of gases graduated tubes of greater or less capacity, made of strong glass, and closed by fusion at one end, which should be rounded. The following tubes will be found sufficient for all the processes of gas measuring required in organic elementary analyses. 1. A bell-glass capable of holding from 150 to 250 c. c., and about 4 centimetres in diameter ; divided into cubic centimetres. 2. Five or six glass tubes, about 12 to 15 millimetres in diam- eter in the clear, and capable of holding from 30 to 40 c. c. each, divided into -^ c. c. The sides of these tubes should be pretty thick, otherwise they will be liable to break, especially when used to measure over mer- cury. The sides of the bell-glass should be about 3, of the tubes about 2 millimetres thick. , The most important point, however, in connection with meas- * [The student who will practise the accurate measurement of gases in any but the simplest cases, must refer for all details to Bunsen's "Gasometry" (translated by Roscoe), and Russell, Jour. Chem. Soc., 1868, p. 128, as the sub- ject is too extensive for the limits of this volume.] t "Lehrbuch der Titrirmethode," by Dr. Fr. Mohr. Brunswick, 1855. 26 OPERATIONS. [ 12, uring instruments is that the} 7 be correctly graduated, since upon this of course depends the accuracy of the results. For the method of graduating I refer to GREVILLE WILLIAMS' u Chemical Mani- pulation."* In testing the measuring tubes we have to consider three things. 1. Do the divisions of a tube correspond with each other? 2. Do the divisions of each tube correspond with those of the other tubes ? 3. Do the volumes expressed by the graduation lines corre- spond with the weights used by the analyst ? These three questions are answered by the following experi- ments : a. The tube which it is intended to examine is placed in a per- pendicular position, and filled gradually with accurately measured small quantities of mercury, care being taken to ascertain with the utmost precision w T hether the graduation of the tube is proportion- ate to the equal volumes of mercury poured in. The measuring- off of the mercury is effected by means of a small glass tube, sealed at one end, and ground perfectly even and smooth at the other. This tube is filled to overflowing by immersion under mercury, care being taken to allow no air bubbles to remain in it ; the excess of mercury is then removed by pressing a small glass plate down on the smooth edge of the tube.f 5. Different quantities of mercury are successively measured off in one of the smaller tubes, and then transferred into the other tubes. The tubes may be considered in perfect accordance with each other, if the mercury reaches invariably the same divisional point in every one of them. Such tubes as are intended simply to determine the relative volume of different gases, need only pass these two experiments ; but in cases where we want to calculate the weight of a gas from its yolume, it is necessary also to obtain an answer to the third question. For this purpose c. One of the tubes is accurately weighed and then filled with * [See also Gary Lea, Am. Jour. Sci. and Arts, 2d ser., vol. 42, p. 375.] f As warming the metal is to be carefully avoided in this process, it is advi- sable not to hold the tube with the hand in immersing it in the mercury, but to fasten it in a small wooden holder. 13.J MEASURING OF GASKS. 27 distilled water of a temperature of 16 to the last mark of the graduated scale ; the weight of the water is then accurately deter- mined. If the tube agrees with the weights, every 100 c. c. of water of 16 must weigh 99*9 grrn. But should it not agree, no matter whether the error lie in the graduation of the tube or in the adjustment of the weights, we must apply a correction to the volume observed before calculating the weight of a gas therefrom. Let us suppose, for instance, that we find 100 c. c. to weigh only 99'6 grm. : assuming our weights to be correct, the c. c. of our scale are accordingly too small ; and to convert 100 of these c. c. into normal c. c. we say : 99-9 :.99-6 :: luO : ,/. In the measuring of gases we must have regard to the follow- ing points : 1. Correct reading-off. 2. The temperature of the gas. 3. The degree of pressure operating upon it. And 4. The circumstance whether it is dry or moist. The three latter points will be readily understood, if it be borne in mind that any alteration in the tem- perature of a gas, or in the pressure acting upon it, or in the ten- sion of the admixed aqueous vapor, involves likewise a consider- able alteration in its volume. 13. 1. CORRECT READING-OFF. This is rather difficult, since mercury in a cylinder has a con- vex surface (especially observable with a narrow tube), owing to its own cohesion; whilst water, on the other hand, under the same circumstances has a concave surface, owing to the attraction which the walls of the tube exercise upon it. The cylinder should invariably be placed in a perfectly perpendicular position, and the eye of the operator brought to a level with the surface of the fluid. In reading-off over water, the middle of the dark zone formed by that portion of the liquid that is drawn up around the inner walls of the tube, is assumed to be the real surface ; whilst when operating with mercury, we have to place the real surface in a plane exactly in the middle between thp highest point of the sur- face of the mercury, and the points at which the latter is in actual 28 OPERATIONS. [ 14. contact with the walls of the tube. However, the results obtained in this way are only approximate. Absolutely accurate results cannot be arrived at, in measuring over water or any other fluid that adheres to glass. But over mer- cury they may be arrived at if the error of the meniscus be deter- mined and the mercury be read off at the highest point. The determination of the error of the meniscus is performed for each tube, once for all, in the following manner : some mercury is poured into the tube, and its height read-off right on a level with the top of the convex surface exhibited by it; a few drops of solu- tion of chloride of mercury are then poured on the top of the metal ; this causes the convexity to disappear ; the height of the mercury in the tube is now read-off again and the difference noted. In the process of graduation, the tube stands upright, in that of measuring gases, it is placed upside down ; the difference observed must accordingly be doubled, and the sum added to each volume of gas read off. 14. 2. INFLUENCE OF TEMPERATURE. The temperature of gases to be measured is determined either by making it correspond with that of the confining fluid, and ascertaining the latter, or by suspending a delicate thermometer by the side of the gas to be measured, and noting the degree which it indicates. If the construction of the pneumatic apparatus permits the total immersion of the cylinder in the confining fluid, uniformity of temperature between the latter and the gas which it is intended to measure, is most readily and speedily obtained ; but in the reverse case, the operator must always, after every manipulation, allow half an hour or, in operations combined with much heating, even an entire hour to elapse, before proceeding to observe the state of the mercury in the cylinder, and in the thermometer. Proper care must also be taken, after the temperature of the gas has been duly adjusted, to prevent re-expansion during the reading-off ; all injurious influences in this respect must accord- ingly be carefully guarded against, and the operator should, more especially, avoid laying hold of the tube with his hand (in pressing it down, for instance, into the confining fluid) ; making use, instead, of a wooden Holder. 15, 16.J MEASUKIXG OF GASES. 29 15. 3. INFLUENCE OF PRESSURE. With regard to the third point, the gas is under the actual pressure of the atmosphere if the confining fluid stands on an exact level both in and outside the cylinder ; the degree of pres- sure exerted upon it may therefore at once be ascertained by con- sulting the barometer. But if the confining fluid stands higher in the cylinder than outside, the gas is under less pressure, if lower, it is under greater pressure than that of the atmosphere ; in the latter case, the perfect level of the fluid inside and outside the cylinder may readily be restored by raising the tube ; if the fluid stands higher in the cylinder than outside, the level may be restored by depressing the tube ; this however can only be done in cases where we have a trough of sufficient depth. When oper- ating over water, the level may in most cases be readily adjusted ; when operating o'ver mercury, it is, more especially with wide tubes, often impossible to bring the fluid to a perfect level inside and outside the cylinder. 16. 4. INFLUENCE OF MOISTURE. In measuring gases saturated with aqueous vapor, it must be taken into account that the vapor, by virtue of its tension, exerts a pressure upon the confining fluid. The necessary correction is simple, since we know r the respective tension of aqueous vapor for the various degrees of temperature. But before this correction can be applied, it is, of course, necessary that the gas should be actually saturated with the vapor. It is, therefore, indispensable in measuring gases to take care to have the gas thoroughly satu- rated with aqueous vapor, or else absolutely dry. It is quite obvious from the preceding remarks, that volumes of gases can be compared only if measured at the same temper- ature, under the same pressure, and in the same hygroscopic state. They are generally reduced to 0, 0'76 met. barometer, and abso- lute dryness. How this is effected, as well as the manner in which we deduce the weight of gases from their volume, will be found in the chapter on the calculation of analyses. 30 OPERATIONS. [ 17, 18. 17. b. THE MEASURING OF FLUIDS. In consequence of the vast development which volumetric analysis has of late acquired, the measuring of fluids has become an operation of very frequent occurrence. According to the different objects in view, various kinds of measuring vessels are employed. The operator must, in the case of every measuring vessel, carefully distinguish whether it is graduated for holding or for delivering the exact number of c. c. marked on it. If you have made use of a vessel of the former description in measuring off 100 c. c. of a fluid, and wish to transfer the latter completely to another vessel, you must, after emptying your measuring vessel, rinse it, and add the rinsings 'to the fluid transferred ; whereas, if you have made use 'of a measuring vessel of the latter description, there must be no rinsing. a. MEASURING VESSELS GRADUATED FOR HOLDING THE EXACT MEAS- URE OF FLUID MARKED ON THEM. aa. Measuring vessels which serve to measure out one definite quantity of fluid. We use for this purpose 18. 1. Measuring Flasks. Fig. 2 represents a measuring flask of the most practical and convenient form. Measuring flasks of various sizes are sold in the shops, holding respectively 200, 250, 500, 1000, 2000, &c., c. c. As a general rule, they have no ground-glass stoppers ; it 'is, however, very desirable, in certain cases, to have measuring flasks with ground stoppers. The flasks must be made of well-annealed glass of uni- form thickness, so that fluids may be heated in them. The line- mark should be placed within the lower third, or at least within the lower half, of the neck. 18.] MEASURING OF FLUIDS. 31 Measuring flasks, before they can properly be employed in analytical operations, must first be carefully tested. The best and simplest way of effecting this is to proceed thus : Put the flask, perfectly dry inside and outside, on the one scale of a sufficiently delicate bal- ance, together with a weight of 1000 grm. in the case of a litre flask, 500 grm. in the case of a half -litre flask, etc., restore the equilibrium by placing the requisite quan- tity of shot and tinfoil on the other scale, then remove the flask and the weight from the balance, put the flask on a perfectly level surface, and pour in distilled water of 16,* until the lower border of the dark zone formed by the top of the water around the inner walls corresponds with the line-mark. After having thoroughly dried the neck of the flask above the mark, replace it upon the scale : if this restores the perfect equilibrium of the bal- ance, the water in the flask w r eighs, in the case of a litre measure, exactly 1000 grm. If the scale bearing the flask sinks, the water in it weighs as much above 1000 grm. as the additional weights amount to which you have to put in the other scale to restore the equilibrium ; if it rises, on the other hand, the water weighs as much less as the weights amount to which you have to put in the scale with the flask to effect the same end. *To use water in the state of its highest density, viz., of 4, 1 c. c. of which weighs exactly 1 grm., and, accordingly, 1 litre, exactly 1000 grms., is less prac- tical, as the operations must in that case be conducted in a room as cold ; since, in a warmer room, the outside of the flask would immediately become covered with moisture, in consequence of the air cooling below dew-point. Nor can I recommend F Mohr's suggestion to make litre-flasks, and measuring vessels in general, upon a plan to make the litre-flask, for instance, hold, not 1000 grm. water at 4, but 1000 grm. at 16, since in an arrangement of the kind proper regard is not paid to the actual meaning of the term "litre" in the scientific world ; and measuring vessels of the same nominal capacity, made by different instrument-makers, are thus liable to differ to a greater or less extent. One litre- flask, according to Mohr, holds 1001 '2 standard c. c. I consider it impractical to give to the c. c. another signification in vessels intended for measuring fluids than in vessels used for the measuring of gases, which latter demand strict ad- hesion to the standard c. c. , as it is often required to deduce the weight of a gas by calculating from the volume. OPERATIONS. [ If the water in the litre measure weighs 999 grm.,* in the half- litre measure, 499'5 grm., &c., the measuring flasks are correct. Differences up to O'lOO grm., in the litre measure, up to 0.070 grm. in the half-litre measure, and up to 0'050 grm. in the quarter-litre measure, are not taken into account, as one and the same measur- ing flask will be found to offer variation to the extent indicated, in repeated consecutive weighings, though filled each .time exactly up to the mark with water of the same temperature. Though a flask should, upon examination, turn out not to hold the exact quantity of water which it is stated to contain, it may yet possibly agree with the other measuring vessels, and may accordingly still be perfectly fit for use for most purposes. Two measuring vessels agree among themselves if the marked Nos. of c. c. bear the same proportion to each other as the weights found ; thus, for instance, supposing your litre- measure to hold 998 grm. water of 16, and your 50 c. c. pipette to deliver 49'9 grm. water of the same temperature, the two measures agree, since 100 90 80 70 60 50 40 1000 : 50 = 998 : 49-9. To prepare or correct a measuring flask, tare the dry litre, half-litre, or quarter-litre flask, and then weigh into it, by substitution, ( 9) 999 grrn., or, as the case may be, the half or quarter of that quantity of distilled water of 16. Put the flask on a perfectly horizontal support, place your eye on an exact level with the surface of the water, and mark the lower border of the dark zone by two little dots made on the glass with a point dipped into thick asphaltum varnish, or some other substance of the kind. Now pour out the water, place the flask in a convenient position, and cut with a diamond a fine distinct line into the glass from one dot to the other. lib. Measuring vessels which serve to measure out any quanti- ties of fluid cut will. * With absolute accuracy, 998-981 grm. ^ 19, 20.] MEASURING OF FLUIDS. 33 ' 19- 2. The Graduated Cylinder. This instrument, represented in fig. 3, should be from 2 to 3 cm. wide, of a capacity of 100 300 c. c., and divided into single c. c. It must be ground at the top, that it may be covered quite close with a ground-glass plate. The measuring with such cylinders is not quite so accurate as with measuring flasks, as in the latter the volume is read off in a narrower part. The accuracy of measuring cylinders may be tested in the same way as in the case of measuring flasks, viz., by weighing into them water of 16 ; or, also, very well, by letting definite quantities of fluid flow into the cylinder from a correct pipette, or burette graduated for delivering, and observing whether or not they are correctly indi- cated by the scale of the cylinder. ft. MEASURING VESSELS GRADUATED FOR DELIVERING THE EXACT MEASURE OF FLUID MARKED ON THEM (graduated d Pecoiilemeitt i. aa. Measuring vessels which serve to measure out one definite quantity of fluid. 20. 3. TJie Graduated Pipette. This instrument serves to take out a definite volume of a fluid from one vessel, and to transfer it to another ; it must accordingly be of a suitable shape to admit of its being freely inserted into flasks and bottles. We use pipettes of 1, 5, 10, 20, 50, 100, 150, and 200 c. c. capacity. The proper shape for pipettes up to 20 c. c. capacity is represented in fig. 4 ; fig. 5 shows the most practical form for lar- ger ones. To fill a pipette suction is applied to the upper aper- ture, either directly with the lips or through a caoutchouc tube, until the fluid stands above the mark ; the upper orifice (which is somewhat narrowed and ground) is then closed with the first finger of the right hand (the point of which should be a little moist) ; the outside is then wiped dry, if required, and, the pipette being held in a perfectly vertical direction, the fluid Is made to drop out, by lifting the . finger a little, till it has OPERATIONS; [ 20. fallen to the required level; the loose drop is carefully wiped off, and the contents of the tube are then finally transferred to the other vessel. In this process it is found that the fluid does not run out completely, but that a small portion of it remains adhering to the glass in the point of the pipette ; after a time, as this becomes increased by other minute particles of fluid trickling down from the upper part of the tube, a drop gathers at the lower orifice, which may be allowed to fall off from its own weight, or may be made to drop off by a slight shake. If, after this, the point of the pipette be laid against a moist portion of the inner side of the vessel, another minute portion of fluid will trickle out, and, lastly, another trifling droplet or so may be got out by blowing into the pipette. Now, supposing the operator follows no fixed rule in this respect, letting the fluid, for instance, in one operation simply run out, whilst in another operation he lets it drain afterwards, and in a third blows out the last particles of it from the pipette, it is evident that the respective quantities of fluid delivered in the several operations cannot be quite equal. I prefer in all cases the second method, viz., to lay the point of the pipette, whilst drain^ ing, finally against a moist portion of the side of the vessel, which I have always found to give the most accurately corresponding measurements. The correctness of a pipette is tested by filling it up to the mark with distilled water of 16, letting the water run out, in Fig. 4. Fig. 5. Fig. 6. t } ie manner j lis t stated, into a tared vessel, and weighing ; the pipette may be pronounced correct if 100 c. c. of water of 16 weigh 99*9 grin. Testing in like manner the accuracy of the measurements made with a simple hand pipette, we find that one and the same pipette will in repeated consecutive weighings of the contents, though 20.] MEASURING OF FLUIDS. 35 tilled and emptied each time with the minutest care, show differ- ences up to O010 grin, for 10 c. c. capacity, up to 0*00 grm. for 50 c. c. capacity. The accuracy of the measurements made with a pipette may be heightened by giving the instrument the form and construction shown in fig. 6, and fixing it to a holder. It will be seen from the drawing that these pipettes are emptied only to a certain mark in the lower tube, and that they are provided with a compression stop-cock, a contrivance which we shall have occasion to describe in detail when oh the subject of burettes. This contrivance reduces the differences of measure- ments with one and the same 50 c. c. pipette to 0'005 grm. Pipettes are used more especially in cases where it is intended to estimate different constituents of a substance in separate por- tions of the same : for instance, 10 grm. of the substance under examination are dissolved in a 250 c. c. flask, the solution is dilu- ted up to the mark, shaken, and 2, 3, or 4 several portions are then taken out with a 50 c. c. pipette. Each portion consists of \ part of the whole, and accordingly contains 2 grm. of the substance. Of course the pipette and the flask must be in perfect harmony. Whether they are may be ascertained by, for instance, emptying the 50 c. c. pipette 5 times into the 250 c. c. flask, and observing if the lower edge of the dark zone of fluid coincides with the mark. If it does not, you may make a fresh mark, which, no matter whether it is really correct or not, will bring the two instru- ments in question into conformity with each other. Cylindrical pipettes, graduated throughout their entire length, may be used also to measure out any given quantities of liquid ; however, these instruments can properly be employed only in pro- cesses where minute accuracy is not indispensable, as the limits of error in reading off the divisions in the wider part of the tube are not inconsiderable. For smaller quantities of liquid this inaccu- racy may be avoided by making the pipettes of tubes of uniform width, having a small diameter only, and narrowed at both ends. (FR. MOHR'S measuring pipettes.) When a fluid runs out of a pipette, drops sometimes remain here and there adhering to the tube ; this arises from a film of fat on the inside ; it may be removed by keeping the instrument some time filled with a solution of bichromate of potassa mixed with sulphuric acid. 36 OPERATIONS. [21. bb. Measuring vessels which serve to measure out quantities of fluid at will. 4. The Burette. Of the various forms and dispositions of this instrument, the following appear to me the most convenient : I. Mohr's Burette, (Compression cock burette). For this excellent measuring apparatus, which is represented in fig. 7, we are indebted to FR. MOHR. It consists of a cylindrical tube, narrower towards the lower end for about an inch, with a 21.] MEASURING OF FLUIDS. 37 slight widening, however, at the extreme point, in order that the caoutchouc connector may take a firm hold. I only use burettes of two sizes, viz.. of 30 c. c., divided into ^ c. c.; and of 50 c. c., divided into J c. c. The former I employ principally in scientific, the latter chiefly in technical investigations. The usual length of my 30 c. c. burette is about 50 cm.; the graduated portion occupies about 49 cm. The diameter of the tube is accordingly about 10 mm. in the clear ; the upper orifice is, for the convenience of filling, widened in form of a funnel, measuring 20 mm. in diameter ; the width of the lower orifice is 5 mm. For very delicate processes, the length of the graduated portion may be extended to 50 or 52 cm., leaving thus intervals of nearly 2 mm. between the small divisional lines. In my 50 c. c. burettes the graduated portion of the tube is generally 40 cm., long. To make the instrument ready for .use, the narrowed lower end of the tube is warmed a little, and greased with tallow ; a caout- chouc tube, about 30 mm. long, and having a diameter of 3 mm. in the clear, is then drawn over it ; into the other end of this is inserted a tube of pretty thick glass, about 40 mm. long, and drawn out to a tolerably fine point; it is advisable to slightly widen the upper end of this tube also, and to cover it with a thin coat of tallow ; and also to tie linen-thread, or twine, round both ends of the con- nector, to insure perfect tight- ness. The space between the lower orifice of the burette and the upper orifice of the small de- livery tube should be about 15 mm. The India rubber tube is now pressed together between the ends of the tubes by the com- pression-cock (or clip). This latter instrument is usually made outof brass wire; the form represented in fig. 8 was given by Mo HE. A good clip must pinch so tight that not a particle of fluid can make its way through the connector when compressed by it ; it must be so const racted that the analyst may work it with perfect facility and exactness, so as to regulate the outflow of the liquid with the most rigorous accuracy, by bringing a higher or less degree of pressure to bear upon it. 38 OPERATIONS. [ 21. For supporting MOHR'S burettes, I use the holder represented in tig. 7 ; this instrument, whilst securely confining the tube, per- mits its being moved up and down with perfect freedom, and also its being taken out, without interfering with the compression-cock. The position of the burette must be strictly perpendicular, to insure which, care must be taken to have the grooves of the cork lining, which are intended to receive the tube, perfectly vertical, with the lower board of the stand in a horizontal position. To charge the burette for a volumetrical operation, the point of the instrument is immersed in the liquid, the compression-cock opened, and a little liquid, sufficient at least to reach into the burette tube, sucked up by applying the mouth to the upper end ; the cock is then closed, and the liquid poured into the burette ' until it reaches up to a little above the top mark. The burette having, if required, been duly adjusted in the proper vertical posi- tion, the liquid is allowed to drop out to the exact level of the top mark. The instrument is now ready for use. When as much liquid has flowed out as is required to attain the desired object, the analyst, before proceeding to read off the volume used, has to wait a few minutes, to give the particles of fluid adhering to the sides of the emptied portion of the tube proper time to run down. This is an indispensable part of the operation in accurate measure- ments, since, if neglected, an experiment in which the standard liquid in the burette is added slowly to the fluid under examina- tion (in w T hich, accordingly, the minute particles of fluid adhering to the glass have proper time afforded them during the operation itself to run down), will, of course, give slightly different results from those arrived at in another experiment, where the larger por- tion of the standand fluid is applied rapidly, and the last few drops alone are added slowly. The way in which the reading-off is effected, is a matter of great importance in volumetric analysis ; the first requisite is to bring the eye to a level with the top of the fluid. We must con- sequently settle the question What is to be considered the top ? If you hold a burette, partly filled with water, between the eye and a strongly illumined wall, the surface of the fluid presents the appearance shown in fig. 10 ; if you hold close behind the tube a sheet of white paper, with a strong light falling on it, the sur- face of the fluid presents the appearance shown in fig. 9. In the one as well as in the other case, you have to read off at MEASTJBING OF FLUIDS. 39 the lower border of the dark zone, this being the most distinctly marked line. FR. MOIIR recommends the following device for reading-off : Paste on a sheet of very white paper a broad strip of black paper, and, when reading-off, hold this close behind the burette, in a position to place the border line between white and black from 2 to 3 mm. below the lower border of the dark zone, as -shown in fig. 11 ; read-off at the lower border of the dark zone. Great care must be taken to hold the paper invariably in the same position, since, if it be held lower down, the lower border of the black sone will move higher up. Fig. 9. Fig. 10. Fig. 11. I prefer to read-off in a light which causes the appearance rep- resented in fig. 9. By the use of ERDMANN'S float * all uncertainties in reading-off may be avoided. Fig. 12 represents a burette thus provided. In this case we always read off the degree of the burette which coin- cideswith the circle in the middle of the float. The float must be- so fitted to the width of the burette that when placed in' the filled burette, it will, on allowing the fluid to run out gradually, sink down with the same without wavering, and when it has been pressed down into the fluid of the closed burette, it will slowly rise again. The weight of the float must, if necessary, be so regu- * Journ. f. prakt. Chem. 71, 194. 40 OPERATIONS. [ 22. lated by mercury that when placed in the filled tube it may cut the fluid with its top uniformly all round. A further important condition of the float is that its axis should coincide as nearly as pos- sible with that of the burette tube, so that the division-mark on the burette may be always parallel with the circular line on the float. The correctness of the graduation of a burette is tested in the most simple way, as follows : fill the instrument up to the highest division with water of 16, then let 10 c. c. of the liquid flow out into an accurately weighed flask, and weigh; then let another quantity of 10 c. c. flow out, and weigh again, and repeat the oper- ation until the contents of the burette are ex- hausted. If the instrument is correctly graduated,, every 10 c. c. of water of 16 must weigh 9*990 grm. Differences up to 0*010 grm. may be dis- regarded, since even with the greatest care bestowed on the process of reading-off, deviations to that extent will occur in repeated measurements of the uppermost 10 c. c. of one and the same burette. With the float-burettes the weighings agree much more accurately, and the differences for 10 c. c. do not exceed 0-002 grm. MOHR'S burette is unquestionably the best and most convenient instrument of the kind, and ought to be employed in the measurement of all liquids which are not injuriously affected by contact with caoutchouc. Of the standard solutions used at present in volumetric analysis, that of perman- ganate of potassa alone cannot bear contact with caoutchouc. 22. II. Gay-Lussarfs Burette. Fig. 13 represents this instrument in, as I believe, its most practical form. I make use of two sizes, one of 50 c. c. divided into % c. c.> the other of 30 c. c. divided into -^ c. c. The former is about 33 cm. long ; the graduated portion occupies about 25 cm.; the internal diameter of the wide tube measures 15 mm. ; that of 23.] MEASURING OF FLUIDS. 41 the narrow tube 4 mm., which in the upper bent end gradually decreases to 2 mm. The graduated portion of the smaller burette is about 28 cm. long, and has accordingly an internal diameter of about 11 mm. The stand which I make use of to rest my burettes in, consists of a disk of solid wood, from 5 to 6 cm. high, and from 10 to 12 cm. in diameter, with holes made with the auger and chisel, of proper size to receive the bot- tom part of the burettes. To complete the instrument, MOHK suggests the use of a perforated cork, bearing a short glass tube bent at aright angle. The cork being inserted into the mouth of the wide tube, a piece of caoutchouc is drawn over the short glass tube ; by blowing into this with greater or less force, the outflow of the liquid from the spout of the slightly slanting burette may be regulated at pleasure. The reading-off of the height of the liquid is effected in the same way as explained in 21. I prefer, however, placing the burette firmly against a perpendicular partition, either a strongly illumined door, or the pane of a window, to insure the vertical position of the instrument. It is only when opera- IflfiSSO ting with more highly concentrated, and accordingly opaque solutions of permanganate of potassa, that the method of reading-off requires modification ; in that case, the upper border of the liquid is noted ; and the best way is to place the burette against a white background, and read off by reflected light. 23. III. Geissler^s Burette. In this instrument, which is represented in fig. 14, the narrow tube is placed inside the wide tube instead of outside, as in GAY- LUSSAC'S burette. The part of the inner tube projecting beyond the wide tube is thick in the glass ; whilst the part inside, which is of the same inside width, is made of very thin glass. . This is a very convenient instrument, and less liable to frac- ture than GAY-LUSSAC'S burette. OPERATIONS. [ 24. II. PRELIMINARY OPERATIONS. PREPARATION OF SUBSTANCES FOR THE PROCESSES OF QUANTITATIVE ANALYSIS. 1. THE SELECTION OF THE SAMPLE. Before the analyst proceeds to make the quantitative analysis of a body, he cannot too carefully consider whether the desired result is fully attained if lie simply knows the respective quantity of every individual constituent of that body. This pri- mary point is but too frequently disregarded, and thus false impressions are made, even by the most careful analysis. This remark applies both to scientific and to technical investigations. Therefore, if you have to determine the constitution of a mineral, take the greatest pos- sible care to remove in the first place every particle of gangue, and disseminated impuri- ties ; remove any adherent matter by wiping or washing, then wrap the substance up in a sheet of thick paper, and crush it to pieces on a steel anvil ; and pick out with a pair of small pincers the cleanest pieces. Crystalline substances, prepared artificially, ought to be purified by re- crystallization ; precipitates by thorough wash- ing, &c., &c. In technical investigations, when called upon, for instance, to determine the amount of peroxide presentin a manganese ore, or the amount of iron present in an iron ore, the first point for consideration ought to be whether the samples selected correspond as much as possible to the average quality of the ore. What would it serve, indeed, to the purchaser of a manganese mine to know the amount of peroxide present In a "select, possibly particularly rich, sample ? These few observations will suffice to show that no universally applicable and valid rules to guide the analyst in the selection of the sample can be laid down ; he must in every individual case, Fig. 14. 25.] MECHANICAL DIVISION. 43 on the one hand, examine the substance carefully, and more par- ticularly also under the microscope, or through a lens ; and, on the other hand, keep clearly in view the object of the investigation, and then take his measures accordingly. 25. 2. MECHANICAL DIVISION. In order to prepare a substance for analysis, i.e., to render it accessible to the action of solvents or fluxes, it is generally indis- pensable, in the first place, to divide it into minute parts, since this will create abundant points of contact for the solvent, and will counteract, and, as far as practicable, remove the adverse influences of the power of cohesion, thus fulfilling all the condi- tions necessary to effect a complete and speedy solution. The means employed to attain this object vary according to the nature of the different bodies we have to operate upon. In many- cases, simple crushing or pounding is sufficient ; in other cases it is necessary to reduce the powder to the very highest degree of fineness, by sifting or by elutriation. The operation of powdering is conducted in mortars ; the first and most indispensable condition is, that the material of the mor- tar be considerably harder than the substance to be pulverized, so as to prevent, as far as practicable, the latter from being contami- nated with any particles of the former. Thus, for pounding salts and other substances possessing no very considerable degree of hardness, porcelain mortars may be used, whilst the pounding of harder substances (of most minerals, for instance,) requires vessels of agate, chalcedony, or flint. In such cases, the larger pieces are first reduced to a coarse powder ; this is best effected by wrapping them up in several sheets of writing-paper, and striking them with a hammer upon a steel or iron plate ; the coarse powder thus obtained is then pulverized, in small portions at a time, in an agate mortar, until it is reduced to the state of an impalpable powder. If we have but a small portion of a mineral to operate upon, and indeed in all cases where we are desirous of avoiding loss, it is advisable to use a steel mortar (fig. 15) for the preparatory reduc- tion of the mineral to coarse powder. ab and cd represent the two parts of the mortar ; these may 1 >e readilv taken asunder. The substance to be crushed (having, if 44 OPERATIONS. [ 25. practicable, -first been broken into small pieces), is placed in the cylindrical chamber ef ; the steel cylinder, which fits somewhat loosely into the chamber, serves as pestle. The mortar is placed upon a solid support, and perpendicular blows are repeatedly struck upon the pestle with a hammer until the object in view is attained. Minerals which are very difficult to pulverize should be strongly ignited, and then suddenly plunged into cold water, and subsequently again ignited. This process is of course applicable only to minerals which lose no essential con- stituent on ignition, and are perfectly insoluble in water. In the purchase of agate mortars, especial care ought to be taken that they have no palpable cracks or indentations ; very slight cracks, however, that cannot be felt, do not render the mortar useless, although they impair its durability. Minerals insoluble in acids, and which consequently require fusing, must especially be finely divided, otherwise we cannot calcu- late upon complete decomposition. This object may be obtained either by triturating the pounded mineral with water, or by elutri- ation, or by sifting; the two former processes, however, can be resorted to only in the case of substances which are not attacked by water. It is quite clear that analysts must in future be much more cautious in this point than has hitherto been the case, since we know now that many substances which are usually held to be insoluble in water are, when in a state of minute division, strongly affected by that solvent; thus, for instance, water, acting upon some sorts of finely pulverized glass, is found to rapidly dissolve from 2 to 3 per cent, of powder even in the cold. (PELOUZE.*) Thus, again, finely divided feldspar, granite, trachyte and porphyry give up to water both alkali and silica. (H. LuDwiG.f) Trituration with water (levigation). Add a little water to the pounded mineral in the mortar, and triturate the paste until all crepitation ceases, or, which is a more expeditious process, transfer * Compt. Rend., t. xliii. pp. 117-123. f Archiv der Pharm. 91, 147. 25.] MEASURING OF FLUIDS. 45 the mineral paste from the mortar to an agate or flint slab, and tritu- rate it thereon with a muller. Rinse the paste off, with the wash- ing bottle, into a smooth porcelain basin of hemispheric form, evaporate the water on the water-bath, and mix the residue most carefully with the pestle. (The paste may be dried also in the agate mortar, but at a very gentle heat, since otherwise the mortar might crack.) To perform the process of elutriation^ the pasty mass, having first been very finely triturated with water, is washed off into a beaker, and stirred with distilled water ; the mixture is then allowed to stand a minute or so, after which the supernatant turbid fluid is poured oif into another beaker. The sediment, which contains the coarser parts, is then again subjected to the process of trituration, etc., and the same operation repeated until the whole quantity is elutriated. The turbid fluid is allowed to stand at rest until the minute particles of the substance held in suspension have subsided, which generally takes many hours. The water is then finally decanted, and the powder dried in the beaker. The process of sifting is conducted as follows : a piece of fine, well-washed, and thoroughly dry linen is placed over the mouth of a bottle about 10 cm. high, and pressed down a little into the mouth, so as to form a kind of bag ; a portion of the finely triturated sub- stance is put into the bag, and a piece of soft leather stretched tightly over the top by way of cover. By drumming with the finger on the leather cover, a shaking motion is imparted to the bag, which makes the finer particles of the powder gradually pass through the linen. The portion remaining in the bag is subjected again to trituration in an agate mortar, and, together with a fresh portion of the powder, sifted again; and the same process is continued until the entire mass has pass through the bag into the glass. When operating on substances consisting of different com- pounds it would be a grave error indeed to use for analysis the powder resulting from the first process of elutriation or sifting, since this will contain the more readily pulverizable constituents in a greater proportion to the more resisting ones than is the case with the original substance. Great care must, therefore, also be taken to avoid a loss of substance in the process of elutriation or sifting, as this loss is likely to be distributed unequally among the several component parts. 46 OPERATIONS. [ 26. In cases where it is intended to ascertain the average composi- tion of a heterogeneous substance, of an iron ore for instance, a large average sample is selected, and reduced to a coarse powder ; the latter is thoroughly intermixed, a portion of it powdered more finely, and mixed uniformly, and finally the quantity required for analysis is reduced to the finest powder. The most convenient instrument for the crushing and coarse pounding of large samples of ore, &c., is a steel anvil and hammer. The anvil in my own laboratory consists of a wood pillar, 85 cm. high and 26 cm. in diameter, into which a steel plate, 3 cm. thick and 20 cm. in diameter, is let to the depth of one-half of its thickness. A brass ring, 5 cm. high, fits round the upper projecting part of the steel plate. The hammer, which is well steeled, has a striking surface of 5 cm. diameter. An. anvil and hammer of this kind afford, among others, this advantage, that their steel surfaces admit most readily of cleaning. To convert the coarse powder into a finer, a smooth-turned steel mortar of about 130 mm. upper diameter and 74 mm. deep is used the final trituration is conducted in an agate mortar. 26. 3. DRYING. Bodies which it is intended to analyze quantitatively must be, when weighed, in a definite state, in a condition in which they can be always obtained again. Now, the essential constituents of a substance are usually accom- panied by an unessential one, viz., a greater or less amount of water, enclosed either within its lamellae, or adhering to it from the mode of its preparation, or absorbed by it from the atmosphere. It is perfectly obvious that to estimate correctly the quantity of a substance, we must, in the first place, remove this variable amount of water. Most solid bodies, therefore, require to be dried before they can be quantitatively analyzed. The operation of drying is of the very highest importance for the correctness of the results ; indeed it may safely be averred that many of the differences observed in analytical researches proceed entirely from the fact that substances are analyzed in different states of moisture. Many bodies contain, as is well known, water which is proper xj 26. J DESICCATION. 47 to them either as inherent in their constitution or as so-called water of crystallization. In contradistinction to this, we will employ the term moisture to designate that variable adherent or mechanically enclosed water, with the removal of which the operation of drying in the sense here in view is alone concerned. In the drying of substances for quantitative analysis, our object is to remove all moisture, without interfering in the slightest degree with combined water or any other constituent of the body. To accomplish this object, it is absolutely requisite that we should know the properties which the substance under examination mani- fests in the dry state, and whether it loses water or other constitu- ents at a red heat, or at 100, or in dried air, or even simply in contact with the atmosphere. These data will serve to guide us in the selection of the process of desiccation best suited to each sub- stance.* The following classification may accordingly be adopted : a. Xnl.Hftances which lose water even in simple contact with the atitwxplu -re ; such as sodium sulphate, crystallized sodium carbon- ate, etc. Substances of this kind turn dull and opaque when exposed to the air, and finally crumble wholly or partially to a white powder. They are more difficult to dry than many other bodies. The process best adapted for the purpose, is to press the pulverized salts with some degree of force between thick layers of fine white blotting-paper, repeating the operation with fresh paper until the last sheets remain absolutely dry. It is generally advisable in the course of this operation to repow- der the salt. ~b. Substances which do not yield water to the atmosphere (unless if 1$ perfectly dry\ but effloresce in art (-fir nil h/ tfried air such as magnesium sulphate, sodium potassium tartrate (Rochelle salt), etc. Salts of this kind are reduced to powder, which, if it be very moist, is pressed between sheets of blotting-paper, as in a after this operation, it must be allowed to remain for some time spread in a thin layer upon a sheet of blotting-paper, effectually protected against dust, and shielded from the direct rays of the sun. * The dried substance should always at once be transferred to a well-closed vessel ; glass tubes, sealed at one end, and of sufficiently thick glass to bear the firm insertion of tight-fitting smooth corks weighing-tubes are usually employed for this purpose. 48 OPERATIONS. [27. c. Substances which undergo no alteration in dried air, but lose water at 100 ; calcium tartrate, for instance. These are finely pulverized ; the powder is put in a thin layer into a watch-glass or shallow dish, and the latter placed inside a chamber in which the air is kept dry by means of sulphuric aciol. This process is usually conducted in one of the following apparatuses, which are termed desiccators, and subserve still another purpose besides that of dry- ing, viz., that of allowing hot crucibles, dishes, etc., to cool in dry air. In fig. 16, a represents a glass plate (ground-glass plates answer the purpose best), ~b, a bell jar with ground rim, which is greased with tallow ; c is a glass basin with sulphuric acid ; d, a round iron Fig. 16. Fig. 17. plate, supported on three feet, with circular holes of various sizes, for the reception of the watch-glasses, crucibles, etc., containing the substance. In fig. 17, a represents a beaker with ground and greased rim, and filled to one-fourth or one-third with concentrated sulphuric acid ; ~b is a ground-glass plate ; c is a bent wire of lead, which serves to support the watch-glass containing the substance. Fig. 18 represents a readily portable desiccator, used more par- ticularly to receive crucibles in course of cooling, and carry them to the balance. The instrument consists of a box made of strong glass ; the lid must be ground to shut air-tight ; the place on which it joins is greased with tallow. The outer diameter of my boxes 28.] DESICCATION. 49 Fig. 18. is 105 mm. ; the sides are 6 mm. thick. The aperture has a diam- eter of 80 mm. ; the box up to the small part is 65 mm. high ; the lid has the same height ; the small part itself is 15 mm. high, and ground to a slightly conical shape. A brass ring, with rim, fits exactly into the aperture ; the rim must not project beyond the glass. The ring bears a triangle of iron, or, better, platinum wire, intended for the reception of crucibles, &c. The body which it is intended to dry is kept exposed to the action of the dry air in the glass, until it shows no further diminution of weight. Sub- stances upon which the oxygen of the air exercises a modifying influence are dried in a similar manner, under the exhausted receiver of an air-pump. Substances which, though losing no water in dry air, yet give off ammonia, are dried over cuicklime, mixed with some chloride of ammonium in powder, and consequently in an anhydrous ammoniacal atmo- sphere. 28. d. Substances which at 100 completely lose their moisture, without suffering any other alteration, such as hydrogen potas- sium tartrate, sugar, etc. These are dried in the water-bath ; in the case of slow-drying substances, or where it is wished to expe- dite the operation, with the aid of a cur- rent of dry air. Fig. 19 represents the water-bath most commonly used. It is made of sheet copper. The engraving renders a detailed description unnecessary. The inner chamber, c, is surrounded on five sides by the outer case or jacket, d e, without communicating with it. The Fi 19 object of the apertures g and h is to effect change of air, which purpose they answer sufficiently well. When 50 OPERATIONS. [ 28. it is intended to use the apparatus, the outer case is filled to about one-half with rain-water, and the aperture a is closed with a perfor- ated cork, into which a glass tube is fitted ; the aperture b is entirely closed. If the apparatus is intended to be heated over charcoal, it should have a length of about 20 cm. from d to f ; but if over a gas-, spirit-, or oil-lamp, it should be only about 13 cm. long. In the former case, the inner chamber is 17 cm. deep, 14 cm. broad, and 10 cm. high ; in the latter case, it is 10 cm. deep, 9 cm. broad r and 6 cm. high. The temperature in the inner chamber never quite reaches 100 ; to bring it up to 100, F. ROCHLEDEK has sug- gested to close I with a double-limbed tube, the outer longer limb of which dips into a cylinder filled with water; a is in that case closed with a perforated cork bearing a sufficiently tall funnel tube, which fits air-tight in the cork. The lower end of this tube reaches down to one inch from the bottom. In large analytical laboratories water is usually kept boiling all day long, for the production of distilled water. The boilers used in my own laboratory have the shape of somewhat oblong square boxes, about 120 cm. long, 60 cm. broad, and 24 cm. high ; the front of the boiler has soldered into it, one above the other, two rows of drying chambers, of the kind shown in fig. 19. This gives so many ovens that almost every student may have one for his special use. Most of these ovens are from 11 to 12 cm. deep and broad, and 8 cm. high ; some of them, however, are 16 cm. deep and broad, to enable them to receive large-sized dishes. The substances to be dried are usually put on double watch-glasses, laid one within the other, which are placed in the oven, and the door is then closed. In the subsequent process of weighing, the upper glassj which contains the substance, is covered with the lower one. The glasses must be -quite cold before they are placed on the scale. In cases where we have to deal with hygroscopic substances, the reabsorption of water upon cooling is prevented by the selection of close-fitting glasses, which are held tight together by a clasp (fig. 20), and allowed to cool with their contents under a bell- glass over sulphuric acid (see fig. 16). These latter instructions 28.] DESICCATION. 51 apply equally to the process of drying conducted in other appa- ratus. The clasp used for keeping the watch-glasses pressed together and which in all cases where it is intended to ascertain the loss of weight which a substance suffers on desiccation, is to be looked upon as belonging to the glasses, and must accordingly be weighed with them is constructed of two strips of thin brass plate, about 10 cm. long, and 1 cm. wide, which are laid the one over the other, and soldered together at the ends, to the extent of 5 to 6 mm. The following apparatus (fig. 21) serves for drying substances in a current of air : 21. a represents a flask filled to one-third with concentrated sul- phuric acid ; c a glass vessel (commonly called a LIEBIG'S drying- tube), and d a tin vessel provided with a stop-cock at e, and arranged in other respects as the cut shows. A, , represents a small tin vessel, containing water and covered with a lid ; two apertures are cut into the border of the latter, to receive the ascending limbs of c. The tube c is first weighed with the substance, then placed in the water-bath, h, i, which is placed over a spirit- or gas-lamp ; the aspirator d is then filled with water, and c connected with the flask a by the perforated cork g. and with d by means of a caout- chouc tube,/. If the stop-cock e be now opened so as to cause the water to drop from d, the air will pass through the tube , and after being dehydrated by the sulphuric acid, will pass over the heated substance in c. After the operation has been continued for some time, it is interrupted for the purpose of weighing the 52 OPERATIONS. [29. tube c and its contents, and then resumed again, and continued until the weight of c (and its contents) remains stationary. The current of cold air exercising its constant cooling action upon the substance, the latter never really reaches 100. It is, therefore, sometimes advisable to substitute for the water in the bath a satu- rated solution of common salt. With this substitution, the apparatus represented in fig. 21 will be found to effect its purpose the most expeditiously. It is not adapted, however, for drying such substances as have a ten- dency to fuse or agglutinate at 100. 29. e. Substances which persistently retain moisture at 100, or become completely dry only after a very long time but which are decomposed by a red heat. t The desiccation of such substances is effected in the air-bath or oil-bath, the temperature being raised to 110-120, and still higher, and, according to circumstances, with or without application of a current of air, carbon dioxide, or hydrogen. Figs. 22 and 23 represent two air-baths of simple construction ; the former (fig. 22) adapted for the desiccation of a single sub- stance, the latter suited for the simultaneous drying of several substances. In fig. 22, A is a box of strong sheet copper, about 11 cm. high, and 9 cm. in diameter. The box is closed with the loose-fitting cover B, which is provided with a narrow rim, and has two aper- tures, C and E '; C is intended to receive the thermometer _Z>, which is fitted into it by a per- forated cork, ^affords an exit to the aqueous vapors, and is. ac- cording to circumstances, either left open, or loosely closed. In 29.] DESICCATION. 53 the interior of the box, about half-way up, are fixed three pins, supporting a triangle of moderately stout wire, upon which the crucible with the substance is placed uncovered. The bulb of the thermometer approaches the crucible as closely as possible, but without touching the triangle. The heating is effected by means of a gas- or spirit-lamp. When the apparatus has cooled sufficient- ly to aUow its being laid hold of without inconvenience, the lid i.s removed, the crucible, which is still warm, taken out, covered, and allowed to cool in a desiccator ; and weighed when cold. In fig. 23, a b is a case of strong sheet copper, with riveted or locked joints, of a width and depth of 15 to 20 cm., and corresponding height. The aperture c is intended to receive a perforated cork, into which is fixed a thermometer, d, which reaches into the interior of the case ; within is a shelf, on which are placed the watch-glasses with the substances to be dried. The case is heated by means of a gas-, spirit-, or oil-lamp. When the temperature has once reached the intended point, it is easy to maintain it pretty constant, by regu- Fig. 28. lating the flame.* In order to limit as much as possible the cooling from without, it is advisable to put over the whole apparatus a pasteboard hood with a movable front. [The air-bath, fig. 23, by a slight alteration, may serve for de- siccating in a stream of dry air. For this purpose, cut a circular orifice, 35 mm. wide, in each end of the copper chamber, and rivet over each orifice a copper tube or ring of corresponding diameter, and 25 mm. long. Fit a glass tube of 20 mm. diameter, by means of perforated corks, into these openings, so that it shall traverse the chamber and project 40-50 mm. beyond the corks at each end. * With a gas-lamp, Kemp's regulator improved by Bunsen, may advanta- geously be used to obtain constant temperatures. 54 OPERATIONS. [ 30. The copper tubes should be so adjusted that the glass tube shall stand horizontally in the chamber, at the same height as the ther- mometer bulb and just behind it. To produce the current of dry air one of the projecting ends of the wide tube is connected by a narrow glass tube and perforated cork, with an aspirator as in fig. 21, the other with a large calcium chloride tube ; the water of the aspirator is allowed to run off somewhat rapidly at first, more slowly afterwards. The end of the tube that delivers the air into the wide tube is recurved, so that the substance within shall not be carried away in the current. The substance to be dried is weighed out in a tray of platinum or porcelain, fig. 24, which is pushed within the wide glass tube by help of a wire. When the sub- stance is hygroscopic, the tray is placed horizontally within a test- tube, which is corked while the weight is being ascertained. The substance and tray, after drying, may be cooled in the same test-tube ; in that case just before put- ting on the balance, the cork should be removed momentarily to allow the tube to fill with air.] 30. The copper apparatus represented in fig. 19, when made with brazed joints, can be employed also as a paraffin e-bath ; w r hen used for that purpose, the outer case is tilled to two-thirds with par- affine. To note the temperature, a thermometer is inserted, by means of a perforated cork, in the aperture a ; with the bulb reaching nearly to the bottom, or, at all events, entirely immersed in the paraifine. Many organic substances, when dried at a somewhat high tem- perature, suffer alteration by the action of the atmospheric oxygen. In the desiccation of such substances, oxygen must accordingly be excluded. [The drying of such bodies is conducted as just described in the modified air-bath, but in a stream of dried and purified hydro- gen or carbonic acid (see 29). The gas is evolved from a self- regulating generator (see fig. 50), 108. 31, 32.] DESICCATION. o:> 31. f. Substances which suffer no alteration at a red heat, such as barium sulphate, pearlash, etc., are very readily freed from mois- ture. They need simply be heated in a platinum or porcelain crucible over a gas or spirit-lamp until the desired end is attained. The crucible, having first been allowed to cool a little, is put, still hot, under a desiccator, and finally weighed when cold. III. GENERAL PROCEDURE IN QUANTITATIVE ANALYSES. 32. It is important, in the first place, to observe that we embrace in the following general analytical method only the separation and determination of the metals and their combinations with the metalloids, and of the inorganic acids and salts. With respect to the quantitative analysis of other compounds, it is not easy to lay down a universally applicable method, except that their constitu- ents usually require to be converted first into acids or bases, before their separation and estimation can be attempted ; this is the case, for instance, with phosphorus sulphide, sulphur chloride, iodine chloride, nitrogen sulphide, &c. The quantitative analysis of a substance presupposes an accurate knowledge of the properties of the same, and of the nature of its several constituents. These data will enable the operator at once to decide whether the direct estimation of each individual constitu- ent is necessary ; whether he need operate only on one portion of the substance, or whether it would be advantageous to deter- mine each constituent in different portions. Let us suppose, for instance, we have a mixture of sodium chloride and anhydrous sodium sulphate, and wish to ascertain the proportion in which these two substances are mixed. Here it would be superfluous to determine each constituent directly, since the determination either of the quantity of the chlorine, or of the sulphuric acid, is quite sufficient to answer the purpose ; still the estimation of both the chlorine and the sulphur trioxide will afford us an infallible con- trol for the correctness of our analysis ; since the united weights of these two substances, added to the sodium and soda respectively equivalent to them, must be equal to the weight of the substance taken. 56 OPERATIONS. [ 33. These estimations may be made, either in one and the same portion of the mixture, by first precipitating the sulphuric acid with barium nitrate, and subsequently the hydrochloric acid from the filtrate with solution of silver nitrate ; or a separate portion of the mixture may be appropriated to each of these two operations. Unless there is some objection to its use (e.g., deficiency or hetero- geneousness of substance), the latter method is more convenient and generally yields more accurate results ; since, in the former method, the unavoidable washing of the first precipitate swells the amount of liquid so considerably that the analysis is thereby delayed, and, moreover, loss of substance less easily guarded against. Before beginning all analyses, at least those of a more complex nature, the student should write out an exact plan, and accurately note on paper, during the entire process, everything that he does. It is in the highest degree unwise to rely on the memory in a com- plicated analysis. When students, who imagine they can do so, come, a week or a fortnight after they have begun their analysis, to work out the results, they find generally too late that they have forgotten much, which now appears to them of importance to know. The intelligent pursuit of chemical analysis consists in the projecting and accurate testing of the plan ; acuteness and the power of passing in review all the influencing chemical relations must here support each other. He who works without a thor- oughly thought-out plan, has no right to say he is practising chem- istry ; for a mere unthinking stringing together of a series of filtra- tions, evaporations, ignitions, and weighings, howsoever well these several operations may be performed, is not chemistry. We will now proceed to describe the various operations consti- tuting the process of quantitative analysis. 33. 1. WEIGHING THE SUBSTANCE. The amount of matter required for the quantitative analysis of a substance depends upon the nature of its constituents ; it is, there- fore, impossible to lay down rules for guidance on this point. Half a gramme of sodium chloride, and even less, is sufficient to effect the estimation of the chlorine. For the quantitative analy- sis of a mixture of common salt and anhydrous sodium sulphate, 1 34.] ESTIMATION OF WATER! 57 gramme will suffice ; whereas, in the case of ashes of plants, com- plex minerals, &c., 3 or 4 grammes, and even more, are required. 1 to 3 grm. can therefore be indicated as the average quantity suitable in most cases. For the estimation of constituents present in very minute proportions only, as, for instance, sodium and potassium in limestones, phosphorus or sulphur in cast-iron, &c., much greater quantities are often required 10, 20, or 50 grammes. The greater the amount of substance taken the more accurate will be the analysis ; the smaller the quantity, the sooner, as a rule, will the analysis be finished. We would advise the student to endeavor to combine accuracy with economy of time. The less substance he takes to operate upon, the more carefully he ought to weigh ; the larger the amount of substance, the less harm can result from slight inaccuracies in weighing. Somewhat large quantities of substance are generally weighed to 1 milligramme ; minute quantities, to y 1 ^ of a milligramme. If one portion of a substance is to be weighed off, we first weigh two watch-glasses which fit on each other, or else an empty platinum crucible with lid, then we put some substance in, and weigh again ; the difference between the two weighings gives the weight of the substance taken. If several quantities of a substance are to be operated upon, the best way is to weigh off the several portions successively ; which may be accomplished most readily by weighing in a glass tube, or other appropriate vessel, the whole amount of substance, and then shaking out of the tube the quantities required one after another into appropriate vessels, weighing the tube after each time. The work may often also be materially lightened, by weighing off a larger portion of the substance, dissolving this to , -J or 1 litre, and taking out for the several estimations aliquot parts, with the 50 or 100 c.c. pipette. The first and most essential condition of this proceeding, of course, is that the pipettes must accurately correspond with the measuring flasks ( 18 and 20). 34. 2. ESTIMATION OF THE WATER. If the substance to be examined after having been freed from moisture by a suitable drying process ( 26-32) contains water, 58 OPERATIONS. [ 35. it is usual to begin by determining the amount of this water. This operation is generally simple ; in some instances, however, it has its difficulties. This depends upon various circumstances, viz., whether the compounds intended for analysis yield their water readily or not ; whether they can bear a red heat without suffering decomposition ; or whether, on the contrary, they give off other volatile substances, besides water, even at a lower temperature. The correct knowledge of the constitution of a compound depends frequently upon the accurate estimation of the water con- tained in it ; in many cases for instance, in the analysis of the salts of known acids the estimation of the water contained in the analyzed compound suffices to enable us to deduce the formula. The estimation of the water contained in a substance is, therefore, one of the most important, as well as most frequently occurring operations of quantitative analysis. The proportion of water con- tained in a substance may be determined in two ways, viz., a, from the diminution of weight consequent upon the expulsion of the water ; &, by weighing the amount of water expelled. 35. a. ESTIMATION OF THE WATER FROM THE Loss OF WEIGHT. This method, on account of its simplicity, is most frequently employed. The modus operandi depends upon the nature of the substance under examination. a. The substance hears ignition without losing other Constituents hesides Water, and without absorbing Oxygen. The substance is weighed in a platinum or porcelain crucible, and placed over the gas- or spirit-lamp ; the heat should be very gentle at first, and gradually increased. When the crucible has been maintained some time at a red heat, it is allowed to cool a little, put still warm under the desiccator, and finally weighed when cold. The ignition is then repeated, and the weight again ascer- tained. If no further diminution of w r eight has taken place, the process is at at end, the desired object being fully attained. But if the weight is less than after the first heating, the operation must be repeated until the weight remains constant. In the case of silicates, the heat must be raised to a very high g 35.] ESTIMATION OF WATER. 59 degree, since many of them (e.g. talc, steatite, nephrite) only begin at a red heat to give off water, and require a yellow heat for the complete expulsion of that constituent. (Tn. SCHEERER.*) Such bodies are therefore ignited over a blast-lamp. In the case of substances that have a tendency to puff off, or to spirt, a small flask or retort may sometimes be advantageously sub- stituted for the crucible. Care must be taken to remove the last traces of aqueous vapor from the vessel, by suction through a glass tube. Decrepitating salts (sodium chloride, for instance) are put- finely pulverized, if possible in a small covered platinum crucible, which is then placed in a large one, also covered ; the whole is weighed, then heated, gently at iirst for some time, then more strongly ; finally, after cooling, weighed agaiu. /3. The substance loses on ignition other Constituents besides Water (Boracic Acid, Sulphuric Acid, Silicon Fluoride, dkc.). Here the analyst has to consider, in the first place, whether the water may not be expelled at a lower degree of heat, which does not involve the loss of other constituents. If this may be done, the substance is heated either in the water-bath, or where a higher temperature is required, in the air-bath or oil-bath, the tempera- ture being regulated by the thermometer. The expulsion of the water may be promoted by the co-operation of a current of air (compare 29 and 30) ; or by the addition of pure dry sand to the substance, to keep it porous.f The process must be continued under these circumstances also, until the weight remains constant. In cases where, for some reason or other, such gentle heating is insufficient, the analyst has to consider whether the desired end may not be attained at a red heat, by adding some substance that will retain the volatile constituent whose loss is apprehended. Thus, for instance, the crystallized sulphate of alumina loses at a red heat, besides water, also sulphuric acid ; now, the loss of the latter constituent may be guarded against by adding to the sul- phate an excess (about six times the quantity) of finely pulverized, recently ignited, pure lead oxide. But the addition of this sub- stance will not prevent the escape of silicon fluoride from silicates when exposed to a red heat * Jahresber. von Liebig u. Kopp, 1851, 610. f Ann. d. Chem. u. Pharm. 53, 233. \ Ibid. 81, 189. 60 OPERATIONS. Thus again, the amount of water in commercial iodine may be determined by' triturating the iodine together with eight times the quantity of mercury, and drying the mixture at 100 (BOLLEY*). y. The substance contains several differently combined quantities of Water which require different Degrees of Temperature for Expulsion. Substances of this nature are heated first in the water-bath, until their weight remains constant ; they are then exposed in the oil- or air-bath to 150, 200, or 250, &c., and finally, when prac- ticable, ignited over a gas- or spirit-lamp. [In such experiments, it is best to proceed as described, 29, p. 53, viz., to heat in a cur- rent of dried air, hydrogen, or carbon dioxide.] In this manner differently combined quantities of water may be distinguished, and their respective amounts correctly estimated. Thus, for instance, crystallized sulphate of copper contains 28-87 per cent, of water, which escapes at a temperature below 140, and 7*22 per cent., which escapes only at a temperature between 220 and 260. tf. When the substance has a tendency to absorb oxygen (from the presence of ferrous compounds, for instance) the water is bet- ter determined in the direct way, than by the loss. ( 36.) 36. l>. ESTIMATION OF WATER BY DIRECT WEIGHING. This method is resorted to by way of control, or in the case of substances which, upon ignition, lose, besides water, other con- stituents, which cannot be retained even by the addition of some other substance (e.g., carbon dioxide, oxygen), or in the case of substances containing bodies inclined to oxidation (e.g., ferrous compounds). The principle of the method is to expel the water by the application of a red heat, so as to admit of the condensa- tion of the aqueous vapor, and the collection of the condensed water in an appropriate apparatus, partly physically, partly by the agency of some hygroscopic substance. The increase in the weight of this apparatus represents the quantity of the water expelled. The operation may be conducted in various ways ; the follow- ing is one of the most appropriate : *Dingler's Polyt. Journ., 126, 39. 36.] ESTIMATION OF AVATEK. 61 B, fig. 25 represents a gasometer filled with air ; b a flask half- filled with concentrated sulphuric acid; c and a oare calcium chlo- ride tubes ; d is a bulb-tube. Fig. 25. The substance intended for examination is weighed in the per fectlj dry tube d* which is then connected with c and the weighed calcium chloride tube ao. by means of sound and well- dried perforated corks. The operation is commenced by opening the stop-cock of the gasometer a little, to allow the air, which loses all its moisture in ~b and c, to pass slowly through d ; the tube d is then heated to be- yond the boiling-point of water, by holding a lamp towards f, taking care not to burn the cork ; and finally, the bulb which con- tains the substance is exposed to a low red heat, the temperature at/ being maintained all the while at the point indicated. When the expulsion of the water has been accomplished, a slow current of air is still kept up till the bulb-tube is cold ; the apparatus is then disconnected, and the calcium chloride tube ao, weighed. The increase in the weight of this tube represents the quantity of water originally present in the substance examined. * [It is usually better to weigh off the substance into a tray or boat of porce- lain or platinum, and place this within a straight tube of hard glass and ignite by means of a tube furnace.] OPERATIONS. 36. j The empty bulb #, in which the greater portion of the water collects, has not only for its object to prevent the liquefaction of the calcium chloride, but enables the analyst also to test the con- densed water as to its reaction and purity. The apparatus may, of course, be modified in various ways ; thus, the chloride of calcium tubes may be U-shaped ; a U-tube, filled with pieces of pumice-stone saturated with sulphuric acid, may be substituted for the flask with sulphuric acid ; and the gaso- meter may be replaced by an aspirator (fig. 21) joined to o. The expulsion of the aqueous vapor from the tube containing the substance under examination, into the calcium chloride tube, may be effected also by other means than a current of air sup- plied by a gasometer or aspirator ; viz., the substance under ex- amination may be heated to redness in a perfectly dry tube, to- gether with lead carbonate, since the carbon dioxide escaping from the latter at a red heat, serves here the same purpose as a stream of air. This method is principally applied in cases where it is desirable to retain an acid which otherwise would volatilize together with the water ; thus, it is applied, for instance, for the direct estimation of the water contained in acid potassium sulphate. Fig. 26. Fig. 26. represents the disposition of the apparatus. a 1) is a common combustion furnace ; cf a tube filled as fol- lows: from c to d with lead carbonate,* from d to e the substance intimately mixed with lead carbonate, and from e tof pure lead car- bonate. The calcium chloride tube UXSEN'S gas-lamp may be used most advantageously in opera- tions of this kind ; a little wire-gauze cap, loosely fitted upon the tube of the lamp, is a material improvement. By means of tli is simple arrangement it is easy to produce even the smallest flame, without the least apprehension of ignition of the gas within the tube. If the evaporation is to be effected on the water-bath, and the operator happens to possess a BEINDORF, or other similarly-con- structed steam apparatus, the evaporating- dish may be placed simply into an opening corresponding in size. Otherwise recourse must be had to the water-bath, illustrated by % 2T -. It is made of strong sheet copper, and when used is half filled with water, which is kept boiling over a gas-, spirit-, or oil-lamp. The breadth from a to b should be from 12 to 18 cm. Various flat rings of the same outside diameter as the top of the bath, and adapted to receive dishes and crucibles of different sizes, are essential adjuncts to the bath. These rings when required are simply laid on the bath. It will occasionally happen that the water in the bath com- pletely evaporates ; in such cases, residues are heated to a higher degree than is desirable, concentrated solutions spirt, &c. To avoid these inconveniences, water-baths have been devised with an arrangement for maintaining a constant level of water. 68 OPERATIONS. [41. If the operator can conduct his processes of evaporation in a room set apart for the purpose, where he may easily guard against any occurrence tending to suspend dust in the air, he will find it no very difficult task to keep the evaporating fluid clean ; in this case it is best to leave the dishes uncovered. But in a large laboratory, frequented by many people, or in a room exposed to draughts of air, or in which coal fires are burning, the greatest caution is required to protect the evaporating fluid from contami- nation by dust or ashes. For this purpose the evaporating dish is either covered' with a sheet of filtering-paper turned down over the edges, or a glass rod twisted into a triangular shape (fig. 28) is laid upon it, and a sheet of filtering-paper spread over it, which is kept in position by a glass rod laid across, the latter again being kept from rolling down by the slightly turned up ends, a and Z, of the triangle. The best way, however, is the following : Take two small thin wooden hoops (fig. 29), one of which fits loosely in the other ; spread a sheet of blotting-paper over the smaller one, and push the other over it. This forms a cover admirably adapted to the purpose ; and whilst in no way interfering with the operation, it completely protects the evaporating fluid from dust, and may be readily taken off ; the paper cannot dip into the fluid ; the cover lasts a long time, and may, moreover, at any time be easily renewed. It must be borne in mind, however, that the common filtering- paper contains always certain substances soluble in acids, such as lime, ferric oxide, &c., which, were covers of the kind just described used over evaporating dishes containing a fluid evolving acid vapors, would infallibly dissolve in these vapors, and the solu- tion dripping down into the evaporating fluid, would speedily con- taminate it. Care must be taken, therefore, in such cases, to use only such filtering-paper as has been freed by washing from sub- stances soluble in acids. Evaporation for the purpose of concentration may be effected also in flasks; these are only half filled, and placed in a slanting position. The process may be conducted on the sand-bath, or over a gas- or spirit-lamp, or even, and with equal propriety, over a char- 41.] EVAPORATION. 69 coal fire. In cases where the. operation is conducted over a lamp or a charcoal fire, it is the safest way to place the flasks on wire ganze. Gentle ebullition of the fluid can do no harm here, since the slanting position of the flask guards effectively against risk of loss from the spirting of the liquid. Still better than in flasks, the object may be attained by evaporating in tubulated retorts with open tubulure and neck directed obliquely upwards. The latter acts as a chimney, and the constant change of air thus effected is extremely favorable to evaporation. The evaporation of fluids containing a precipitate is best con- ducted on the water-bath ; since on the sand-bath, or over the lamp, it is next to impossible to guard against loss from bumping. This Fig. 30. bumping is occasioned by slight explosions of steam, arising from the sediment impeding the uniform diffusion of the heat. Still there remains another, though less safe way, viz., to conduct the evaporation in a crucible placed in a slanting position, as illus- trated in fig. 30. In this process, the flame is made to play upon the crucible above the level of the fluid. Where a fluid has to be evaporated to dryness, as is so often the case, the operation should always, if possible, be terminated on the water-bath. In cases where the nature of the dissolved sub- stance precludes the application of the water-bath, the object in view may often be most readily attained by heating the contents 70 OPERATIONS. [ 41. of the dish from the top, which is effected by placing the dish in a proper position in a drying closet, whose upper plate is heated by a flame (that of the water- or sand-bath) passing over it. If the substance is in a covered platinum dish or crucible, place the gas- lamp in such a position that the flame may act on the cover from above. In cases where the heat has to be applied from the bottom, a method must be chosen which admits of an equal diffusion and ready regulation of the heat. An air-bath is well adapted for this purpose, i.e.. a dish of iron plate, in which the porcelain or platinum dish is to be placed on a wire triangle, so that the two vessels may be at all points i to |- inch distant from each other. The copper apparatus, flg. 27, may 7 also serve as an air-bath, although I must not omit to mention that this mode of application will in the end seriously injure it. If the operation has to be conducted over a lamp, the dish should be placed high above the flame ; best on wire gauze, since this will greatly contribute to an equal diffusion of the, heat. The use of the sand-bath is objectionable here, because with that apparatus we cannot reduce the heat so speedily as may be desirable. An iron plate heated by gas may perhaps be used with advantage. But no matter which method be employed, this rule applies equally to all of them ; that the operator must watch the process, from the moment that the residue begins to thicken, in order to prevent spirting, by reducing the heat, and breaking the pellicles which form on the surface, with a glass rod, or a platinum wire or spatula. Saline solutions that have a tendency ', upon their evaporation, to creep up the sides of the vessel, and may thus finally pass over the brim of the latter, thereby involving the risk of a loss of substance, should be heated from the top, in the way just indicated ; since by that means the sides of the vessel will get heated sufficiently to cause the instantaneous evaporation of the ascending liquid, pre- venting thus its overflowing the brim. The inconvenience just alluded to may, however, be obviated also, in most cases, by cover- ing the brim, and the uppermost part of the inner side of the ves- sel, with a very thin coat of tallow, thus diminishing the adhesion between the fluid and the vessel. In the case of liquids evolving gas-bubbles upon evaporating, particular caution is required to guard against loss from spirting. The safest way is to heat such liquids in an obliquely-placed 41.] EVAPORATION. 71 flask, or in a beaker covered with a large watch-glass ; the latter is removed as soon as the evolution of gas-bubbles has ceased, and the fluid that may have spirted up against it is carefully rinsed into the glass, by means of a washing-bottle. If the evaporation has to be conducted in a dish, a rather capacious one should be selected, and a very moderate degree of heat applied at first, and until the evolution of gas has nearly ceased. If a fluid has to be evaporated vnth exclusion of air, the best way is to place the dish under the bell of an air-pump, over a ves- sel with sulphuric acid, and to exhaust; or a tubulated retort may be used through whose tubulure hydrogen or carbon dioxide is passed by the acid of a tube not quite reaching to the surface of the fluid. The material of the evaporating vesxel* may exercise a much greater influence on the results of an analysis than is generally believed. Many rather startling phenomena that are observed in analytical processes may arise simply from a contamination of the evaporated liquid by the material of the vessel ; great errors may also spring from the same source. The importance of this point has induced me to subject it to a searching investigation (see Appendix, Analytical Experiments, 1 4), of which I will here briefly intimate the results. Distilled water kept boiling for some length of time in glass I flasks of Bohemian glass) dissolves very appreciable traces of that material. This is owing to the formation of soluble silicates ; the particles dissolved consist chiefly of potassa, or soda and lime, in combination with silicic acid. A much larger proportion of the glass is dissolved by water containing caustic or carbonated alkali ; boiling solution of ammonium chloride also strongly attacks glass vessels. Boiling dilute acids, witli the exception, of course, of hydrofluoric and hydrofluosilicilic acids, exercise a less powerful solvent action on glass than pure- water. Porcelain (Berlin dishes) is much less affected by water than glass ; alkaline liquids also exercise a less powerful solvent action on porcelain than on glass ; the quantity dissolved is, however, still notable. Solution of ammonium chloride acts on porcelain as strongly as on glass; dilute acids, though exercising no very powerful solvent action on porcelain, yet attack that material more strongly than glass. It results from these data, that in analyses pretending to a high degree of accuracy, platinum or platinum-indium or silver dishes 72 OPERATIONS. [ 4 W 2. should always be preferred. The former may be used in all cases where no free chlorine, bromine, or iodine is present in the fluid, or can be formed during evaporation. Fluids containing caustic alkalies may safely be evaporated in platinum, but not to the point of fusion of the residue. Silver vessels should never be used to evaporate acid fluids nor liquids containing alkaline sulphides ; but they are admirably suited for solutions of alkali hydroxides and carbonates, as well as of most normal salts. 42. We come now to weighing the residues remaining upon the evaporation of fluids. We allude here simply to such as are soluble in water ; those which are separated by filtration will be treated of afterwards. Residues are generally weighed in the same vessel in which the evaporation has been completed, for which purpose platinum dishes, from 4 to 8 cm. in diameter, pro- vided with light covers, or large platinum cruci- bles, are best adapted, since they are lighter than porcelain vessels of the same capacity. However, in most cases, the amount of liquid to be evaporated is too large for so small a vessel, and its evaporation in portions would occupy too much time. The best way, in cases of this kind, is to concentrate the liquid first in a larger vessel, and to terminate the operation afterwards in the smaller weighing vessel. In transferring the fluid from the large;- to the smaller vessel, the lip of the former is slightly greased, and the liquid made to run down a glass rod. (See fig. 31.) Finally the large vessel is carefully rinsed with a washing- bottle, until a drop of the last rinsing leaves no longer a residue upon evaporation on a platinum knife. When the fluid has thus been transferred to the weighing-vessel, the evaporation is com- pleted on the water-bath and the residuary substance finally ignited, provided, of course, it will admit of this process. For this pur- pose the dish is covered with a lid of thin platinum (or a thin glass plate), and then placed high over the flame of a lamp, and heated very gently until all the water which may still adhere to the sub- stance is expelled ; the dish is now exposed to a stronger, and finally to a red heat. (Where a glass plate is used, this must, of course, be EVAPORATION. 73 removed before igniting.) In this case it is also well to make the flame play obliquely on the cover from above, so as to ran as little risk as possible of loss by spirting. After cooling in a desic- cator, the covered dish is weighed with its contents. When oper- ating upon substances which decrepitate, such as sodium chloride, for instance, it is advisable to expose them after their removal from the water-bath, and previously to the application of a naked flame to a temperature somewhat above 100, either in the air- bath, or on a sand-bath, or on a common stove. If the residue does not admit of ignition, as is the case, for instance, with organic substances, ammonium salts, f which we want to ascertain, in presence of a comparatively large amount of an ammonium salt, which has been mixed with it in the course of the analytical process, I prefer the following method : The saline mass is thoroughly dried, in a large dish, on the water- bath, or, towards the end of the process, at a temperature some- what exceeding 100. The dry mass is then, with the aid of a platinum spatula, transferred to a small glass dish, which is put aside for a time in a desiccator. The last traces of the salt left adhering to the sides and bottom "of the large dish are rinsed off with a little water into the small dish, or the large crucible, in which it is intended to weigh the salt ; the water is then evaporated, and the dry contents of the glass dish are added to the residue : the ammonium salts are now expelled by ignition, and the residu- ary fixed salts finally weighed. Should some traces of the saline mass adhere to the smaller glass dish, they ought to be removed and transferred to the weighing vessel, with the aid of a little pounded ammonium chloride, or some other ammonium salt, as the moistening again with water would involve an almost certain loss of substance. 74 OPERATIONS. [ 43. 43 J. PRECIPITATION. Precipitation is resorted to in quantitative analysis far more frequently than evaporation, since it serves not merely to convert substances into forms adapted for weighing, but also, and more especially, to separate them from one another. The principal in- tention in precipitation, for the purpose of quantitative estimations, is to convert the substance in solution into a form in which it is insoluble in the menstruum present. The result will, therefore, cceteris parifms, be the more accurate, the more the precipitated body deserves the epithet insoluble, and in cases where precipi- tates are of the same degree of solubility, that one will suffer the least loss which comes in contact w r ith the smallest amount of solvent. Hence it follows, first, that in all cases where other circum- stances do not interfere, it is preferable to precipitate substances in their most insoluble form ; thus, for instance, barium had better be precipitated as sulphate than as carbonate ;- secondly, that when we have to deal with precipitates that are not quite insoluble in the menstruum present, we must endeavor to remove that men- struum, as far as practicable, by evaporation ; thus a dilute solution of strontium should be concentrated, before proceeding to precipi- tate the strontium with sulphuric acid ; and, thirdly, that when we have to deal with precipitates slightly soluble in the liquid present, but insoluble in another menstruum, into which the former may be converted by the addition of some substance or other, we ought to endeavor to bring about this modification of the menstruum. Thus, for instance, alcohol may be added to "water, to induce com- plete precipitation of ammonium platinic chloride, lead chloride, calcium sulphate, &c.; thus again, ammonium magnesium phosphate may be rendered insoluble in an aqueous menstruum by adding ammonia to the latter, &c. Precipitation is generally effected in beakers. In cases, how- ever, where we have to precipitate from fluids in a state of ebulli- tion, or where the precipitate requires to be kept boiling for some time with the fluid, flasks or dishes are substituted for beakers, with due regard always to the material of which they are made (see Evaporation, 41, at the end). 44.] DECANTATIOX. 75 The separation of precipitates from the fluid in which they are suspended, is effected either by deccuitation or filtration, or by both these processes jointly. But, before proceeding to the sepa- ration of the precipitate by any of these methods, the operator must know whether the precipitant has been added in sufficient quantity, and whether the precipitate is completely formed. To determine the latter point, an accurate knowledge of the properties of the various precipitates must be attained, which we shall en- deavor to supply in the third section. To decide the former ques- tion. it is usually sufficient to add to the fluid (after the precipitate has settled) cautiously a fresh portion of the precipitant, and to note if a further turbidity ensues. This test, however, is not infallible, when the precipitate has not the property of forming immediately ; as, for instance, is the case with ammonium phos- pho-molybdate. When this is apprehended, pour out (or transfer with a pipette) a small quantity of the clear supernatant fluid into another vessel, add some of the precipitant, warm if necessary ; and after some time look and see whether a fresh precipitate has formed. As a general rule, the precipitated liquid should be allowed to stand at rest for several hours, before proceeding to the separation of the precipitate. This rule applies more particularly to crvstalline, pulverulent, and gelatinous precipitates, whilst curdy and flocculent precipitates, more particularly when the precipitation was effected at a boiling temperature, may often be filtered off im- mediately. However, we must observe here, that all general rules, in this respect, are of limited application. a. SEPARATION OF PRECIPITATES BY DECANTATIOX. When a precipitate subsides so completely and speedily in a fluid that the latter may be decanted off perfectly clear, or drawn off with a syphon, or removed by means of a pipette, and that the washing of the precipitate does not require a very long time, decantation is often resorted to for its separation and washing ; this is the case, for instance, with chloride of silver, metallic mer- cury, cv;c. Decantation will always be found a very expeditious and accu- rate method of separation, if the' process be conducted with due care ; it is necessary, however, in most cases, to promote the speedy 76 OPERATIONS. [ 45. and complete subsidence of the precipitate ; and it may be laid down as a general rule, that heating the precipitate with the fluid will produce the desired effect. Nevertheless, there are instances in which the simple application of heat will not suffice ; in some cases, as with silver chloride, for instance, agitation must be resorted to ; in other cases, some reagent or other is to be added hydrochloric acid, for instance, in the precipitation of mercury, &c. We shall have occasion, subsequently, in the fourth section, to discuss this point more fully, when we shall also mention the vessels best adapted for the application of this process to the various precipitates. After having washed the precipitate repeatedly with fresh quantities of the proper fluid, until there is no trace of a dissolved substance to be detected in the last rinsings, it is placed in a crucible or dish, if not already in a vessel of that description ; the fluid still adhering to it is poured off as far as practicable, and the precipitate is then, according to its nature, either simply dried, or heated to redness. A far larger amount of water being required for washing pre- cipitates by decantation than on filters, the former process can be expected to yield accurate results only where the precipitates are absolutely insoluble. For the same reason, decantation is riot ordi- narily resorted to in cases where we have to determine other con- stituents in the decanted fluid. The decanted fluid must be allowed to stand at rest from twelve to twenty-four hours, to make quite sure that it contains no particles of the precipitate ; if, after the lapse of this time, no precipitate is visible, the fluid may be thrown away ; but if a pre- cipitate has subsided, this had better be estimated by itself, and the weight added to the main amount ; the precipitate may, in such cases, be separated from the supernatant fluid by decantation, or by filtration. 45. /3. SEPARATION OF PRECIPITATES BY FILTRATION. This operation is resorted to whenever decantation is imprac- ticable, and, consequently, in the great majority of cases ; provided always the precipitate is of a nature to admit of its being com- pletely freed, by mere washing on the filter, from all foreign substances. Where this is not the case, more particularly, there- fore, with gelatinous precipitates, aluminium hydroxide for in- 45.] FILTRATION. 7? stance, a combination of decantation and filtration is resorted to ( 4)- aa. FILTERING APPARATUS. Filtration, as a process of quantitative analysis, is almost exclusively effected by means of paper. Plain circular filters are most generally employed ; plaited fil- ters are only occasionally used. Much depends upon the quality of the paper. Good filtering paper must possess the three follow- ing properties: 1. It must completely retain the finest precipi- tates ; 2. It must filter rapidly ; and 3. It must be as free as possible from any admixture of inorganic bodies, but more espe- cially from such as are soluble in acid or alkaline fluids. It is a matter of some difficulty, however, to procure paper fullv answering these conditions. The Swedish filtering, paper, with the water-mark J. H. MUNKTELL, is considered the best, and, consequently, fetches the highest price ; but even this answers only the first two conditions, being by no means sufficiently pure for very accurate analyses, since it leaves upon incineration about 0*3 per cent, of ash,* and yields to acids perceptible traces of lime, mag- nesia, and ferric oxide. For exact experiments it is, consequently, necessary first to extract the paper with dilute hydrochloric acid, then to wash the acid completely out with water, and finally to dry the paper. In the case of very fine filtering paper, the best way to perform this operation is to place the ready-cut filters, several together, in a funnel, exactly the same way as if intended for immediate filtration ; they are then moistened with a mixture of one part of ordinary pure hydrochloric acid with two parts of water, which is allowed to act on them for about ten minutes : after this all traces of the acid are carefully removed by washing the filters in the funnel repeatedly with warm water. The funnel being then covered with a piece of paper, turned over the edges, is put in a warm place until the filters are dry. Compare the instruction given in the "Qual. Anal.," Am. Ed., p. 8, on the preparation of washed filters. Filter paper containing lead, and which is consequently blackened by sulphuretted hydrogen, should be rejected. * Plantamour found the ash of Swedish filtering paper to consist of 63 '23 silicic acid, 12'83 lime, 6 '21 magnesia, 2'94 alumina, and 13'92 ferric oxide, in 100 parts. 78 OPERATIONS. [45. Heady-cut filters of various sizes should always be kept on hand. Filters are either cut by circular patterns of pasteboard or tin, or, still better, by MOHB'S filter- patterns, fig. 32. This little apparatus is made of tin-plate, and consists of two parts. is a quadrant fitting in A, whose straight edges are turned up, 32 and which is slightly smaller than B. T.he sheets of filter- paper are first cut up into squares, which are folded in quarters, and placed in A, then B is placed on the top, and the free edge of the paper is cut off with scissors. Filters cut in this way are per- fectly circular, and of equal size. Several pairs of these patterns of various sizes (3, 4, 5, 6, 6*5, and 8 cm. radius) should be procured. In taking a filter for a given operation, you should always choose One which, after the fluid has run through, will not be more than half filled with the precipitate. As to the funnels, they should be inclined at the angle of 60% and not bulge at the sides. Glass is the most suitable material for them. Fig. 33. Fig. 34. The filter should never protrude beyond the funnel. It should come up to one or two lines from the edge of the latter. 46.] FILTRATION. 79 The lilter is firmly pressed into the funnel, to make the paper fit closely to the side of the latter; it is then moistened with water ; any extra water is not poured out, but allowed to drop through. The stands shown in figs. 33 and 34 complete the apparatus for filtering. The stands are made of hard wood. The arm holding the funnel or funnels must slide easily up and down, and be fixable by the screw. The holes for the funnels must be cut conically, to keep the funnels steadily in their place. These stands are very convenient, and may be readily moved about without interfering with the operation. 46. 1>1>. RULES TO BE OBSERVED IN THE PROCESS OF FlLTRATION. In the ease of curdy, flocculent, gelatinous, or crystalline pre- cipitates there is no danger of the fluid passing turbid through the filter. But with fine pulverulent precipitates it is generally n> .sv//-y, and always advisable, to let the precipitate subside, and then filter the supernatant liquid, before proceeding to place the precipi- tate upon the filter. We generally proceed in this way also wit]) other kinds of precipitates, especially with those that require to stand long before they completely separate. Precipitates which have been thrown down hot, are most properly filtered off before cooling (provided always there be no objections 'to this course), since hot fluids run through the filter more speedily than cold ones. S< .me precipitates have a tendency to be carried through the filter along with the fluid ; this may be prevented in some instances by modifying the latter. Thus barium sulphate, when filtered from an aqueous solution, passes rather easily through the filter the addition of hydrochloric acid or ammonium chloride prevents this in a great measure. If the operator finds, during a filtration, that the filter would be much more than half filled by the precipitate, he would better use an additional filter, and thus distribute the precipitate over the two ; for, if the first were too full, the precipitate could not be properly washed. The fluid ought never to be poured directly upon the filter, but always down a glass rod, and the lip or rim of the vessel from 80 OPERATIONS. [ 40. which the fluid is poured should always be slightly greased with tallow.* The stream ought invariably to be directed towards the sides \of the filter, never to the centre, since this might occasion loss by splashing. In cases where the fluid has to be filtered off, with the least possible disturbance of the precipitate, the glass rod must not be placed, during the intervals, in the vessel containing the precipitate ; but it may conveniently be put into a clean glass, which is finally rinsed with the wash-water. The filtrate is received either in flasks, beakers, or dishes, according to the various purposes for which it may be intended. Strict care should be taken that the drops of fluid filtering through glide down the side of the receiving vessel ; they should never be allowed to fall into the centre of the filtrate, since this again might occasion loss by splashing. The best method is that shown in fig. 34, viz., to rest the point of the funnel against the upper part of the inside of the receiving vessel. If the process of filtration is conducted in a place perfectly free from dust, there is no necessity to cover the funnel, nor the vessel receiving the filtrate ; however, as this is but rarely the case, it is generally indispensable to cover both. This is best effected with round plates of sheet-glass. The plate used for covering the receiving vessel should have a small U-shaped piece cut out of its edge, large enough for the funnel-tube to go through. The effect desired may be produced by cautiously chipping out the glass bit by bit with the aid of a key. Plates perforated in the centre are worthless as regards the object in view. After the fluid and precipitate have been transferred to the filter, and the vessel which originally contained them has been, rinsed repeatedly with water, it happens generally that small par- ticles of the precipitate remain adhering to the vessel, which can- not be removed with the glass rod. From beakers or dishes these particles may be readily removed by means of a feather prepared for the purpose by tearing off nearly the whole of the plumules, leaving only a small piece at the end which should be cut per- fectly straight. From flasks, minute portions of heavy precipitates which are not adherent, are readily removed by blowing a jet of water into the flask, held inverted over the funnel ; this is effected * The tallow may be kept under the edge of the work-table at a convenient point, where it will adhere by a little pressure. The best way of applying the tallow to the lip of a vessel is with the greased finger. 47.] FILTEATIO^. 81 by means of the washing-bottle shown in fig. 36. If the minute adhering particles of a precipitate cannot be removed by mechani- cal means, solution in an appropriate menstruum must be resorted to, followed by re-precipitation. Bodies for which we possess no solvent, such as barium sulphate, for instance, must not be precipi- tated in flasks, 47. cc. WASHING OF PRECIPITATES. After having transferred the precipitate completely to the fil- ter, we have next to perform the operation of washing ; this is effected by means of one of the well-known washing-bottles, of which I prefer the one represented in fig. 35 in every respect. The doubly perforated stoppers are of vulcanized rubber. Fig. 35. Fig. 36. Fig. 37. Care must always be taken to properly regulate the jet, as too impetuous a stream of water might occasion loss of substance. In cases where a precipitate has to be washed with great cau- tion, the apparatus illustrated in fig. 37 will be found to answer very well. The construction of this apparatus requires no explanation. When the flask is inverted, it supplies a fine continuous jet of water. Precipitates requiring washing with water, are washed most expeditiously with hot water, provided always there be no special reason against its use. The washing-bottle shown in fig. 35 is particularly well adapted for this purpose. The cork which is fastened to the neck of the flask with wire serves to facilitate holding it. 82 OPERATIONS. [ 48. It is a rule in washing precipitates not to add fresh wash-water to the filter till the old has quite run through. In applying the jet of water you have to take care on the one hand that the upper edge of the filter is properly washed, and on the other hand that no canals are formed in the precipitate, through which the fluid runs off, without coming in contact with the whole of the precipi- tate. If such canals have formed and cannot be broken up by the jet, the precipitate must be stirred cautiously with a small platinum knife or glass rod. The washing may be considered completed w r hen all soluble matter that is to be removed has been got rid of. The beginner who devotes proper attention to the completion of this operation shuns one of the rocks which he is most likely to encounter. Whether the precipitate has been completely washed may generally be ascertained by slowly evaporating a drop of the last washings upon a platinum knife, and observing if a residue is left. But in cases where the precipitate is not altogether insoluble in water (strontium sulphate, for instance), recourse must be had to more special tests, which we shall have occasion to point out in the course of the work. The student should never discontinue the washing of a precipitate because he simply imagines it is finished he must be certain. 48. y. SEPARATION OF PRECIPITATES BY DECANT ATION AND FILTRATION COMBINED. In the case of precipitates which, from their gelatinous nature, or from the firm adhesion of certain coprecipitated salts, oppose insuperable, or, at all events, considerable obstacles to perfect wash- ing on the filter, the following method is resorted to : Let the precipitate subside as far as practicable, pour the nearly clear super- natant liquid on the filter, stir the precipitate up w T ith the washing fluid (in certain cases, where such a course is indicated, heat to boiling), let it subside again, and repeat this operation until the precipitate is almost thoroughly washed. Transfer it now to the filter, and complete the operation with, the washing-bottle (see 47). This method is highly to be recommended; there are many precipitates that can be thoroughly \vashed only by its application. 49.] FILTRATION". 83 In cases where it is not intended to weigh the precipitate washed by decantation, but to dissolve it again, the operation of washing is entirely completed by decantation, and the precipitate not even transferred to the filter. The re-solution of the bulk of the precipitate being effected in the vessel containing it, the filter is placed over the latter, and the solvent passed through it. Although the termination of the operation of washing may be usually ascertained by testing a sample of the washings for one of the substances originally present in the solution which has to be removed (for hydrochloric acid, for instance, with nitrate of silver), still there are cases in which this mode of proceeding is inapplicable. In such cases, and indeed in processes of washing by decantation generally, BUNSEN'S method will be found convenient viz., to continue the process of washing until the fluid which had remained in the beaker, after the first decantation, has under- gone a ten thousand- fold dilution. To effect this, measure with a slip of paper the height from the bottom of this beaker to the surface of the fluid remaining in it, together with the precipitate, after the first decantation; then fill the beaker with water, if possible, boiling, and measure the entire height of the fluid; divide the length of the second column by that of the first. Go through the same process each time you add fresh water, and always multiply the quotient found witli the number obtained in the preceding calculation, until you reach 10000. 49. FURTHER TREATMENT OF PRECIPITATES. Before proceeding to weigh a precipitate, it still remains to convert it into a form of accurately known composition. This is done either by igniting or by drying. The latter proceeding is more protracted and tedious than the former, and is, moreover, apt to give less accurate results. The process of drying is, therefore, ;is a general rule, applied only to precipitates which cannot bear exposure to a red heat without undergoing total or partial volatili- zation ; or whose residues left upon ignition have no constant com- position ; thus, for instance, drying is resorted to in the case of mercuric sulphide, arsenious sulphide, and other metallic sulphides ; and also in the case of silver cyanide, potassium platinic chloride, etc. 84 OPERATIONS. [ 50. But whenever the nature of the precipitate (!. U>. Ignition of Precipitates. In this process it is necessarv to burn the filter and substract the weight of the filter ash from the total weight found. If care be taken to make the filters always of the same paper, * Turned down over the rim. Or more neatly as follows: Wet a common cut filter, stretch it over the ground top of the funnel, and then gently tear off the superfluous paper. The cover thus formed continues to adhere after drying with some force. 86 OPEKATIONS. [ 51. and to cut every size by a pattern, the quantity of ash which each size yields upon incineration may be readily determined. It is necessary, however, to determine separately the quantity of ash left by ordinary filters, and that left by filters which have been washed with hydrochloric acid and water ; on an average the latter leave about half as much ash as the former. To determine the fil- ter ash take ten filters (or an equal weight of cuttings from the same paper), burn them in an obliquely-placed platinum crucible, and ignite until every trace of carbon is consumed ; then weigh the ash, and divide the amount found by ten; the quotient ex- presses, with sufficient precision, the average quantity of ash which every individual filter leaves upon incineration. In the ignition of precipitates, the following four points have to be more particularly regarded: 1. No loss of substance must be incurred ; 2. The ignited precipitates must really be the bodies they are represented to be in the calculation of the results ; 3. The incineration of the filters must be complete ; 4. The crucibles must not be attacked. The following two methods seem to me the simplest and most appropriate of all that have as yet been proposed. The selection of either depends upon certain circumstances, which I shall imme- diately have occasion to point out. But no matter which method is resorted to, the precipitate must always be thoroughly dried, before it can properly be exposed to a red heat. The application of a red heat to moist precipitates, more particularly to such as are very light and loose in the dry state (silicic acid, for instance), involves always a risk of loss from the impetuously escaping aqueous vapors carrying away with them minute particles of the substance. Some other substances, as aluminium hydroxide or ferric hydroxide, for instance, form small hard lumps ; if such lumps are ignited while still moist within they are liable to fly about with great violence. The best method of drying precipitates as a preliminary to ignition is as described in 50, the last paragraph. Respecting the ignition, the degree of heat to be applied and the duration of the process must, of course, depend upon the nature of the precipitate and upon its deportment at a red heat. As a general rule, a moderate red heat, applied for about five minutes, is found sufficient to effect the purpose ; there are, how- 51.] IGNITIC^ OF PRECIPITATES. 87 ever, many exceptions to this rule which will be indicated where- ever they occur. Whenever the choice is permitted between porcelain and platinum crucibles, the latter are always preferred, on account of their comparative lightness and infrangibility, and because they are more readily heated to redness. The crucible .selected should always be of sufficient capacity, as the use of crucibles deficient in size involves the risk of loss of substance. The proper size, in most cases, is 4 cm. in height, and 3*5 cm. in diameter. That the crucible must be perfectly clean, both inside and outside, need hardly be mentioned. The analyst should acquire the habit of cleaning and polishing the platinum crucible always after using it. This should be done by friction with moist sea-sand whose grains are all round and do not scratch. The sand is rubbed on with the finger, and the desired effect is produced in a few minutes. The adoption of this habit is attended with the pleasure of always working with a bright crucible and the profit of prolonging its existence. This mode of cleaning is all the more necessary, when one ignites over gas-lamps, since at this high temperature crucibles soon acquire a gray coating, which arises from a superficial loosen- ing of the platinum. A little burnishing with sea-sand readily removes the appearance in question, without causing any notable diminution of the weight of the crucible. The foregoing remarks on platinum crucibles refer equally to those of iridium-platinum which, by the by, are now much used, and very highly to be recom- mended only the restoration of the polish is somewhat more diffi- cult with the latter, on account of the greater hardness of the alloy. If there are spots on the platinum or iridium-platinum crucibles, which cannot be removed by the sand without wearing away too much of the metal, a little potassium disulphate is fused in the crucible, the fluid mass shaken about inside, allowed to cool, and the crucible finally boiled with water. There are two ways of cleaning crucibles soiled outside ; either the crucible is placed in a larger one, and the interspace filled with potassium disulphate, which is then heated to fusion ; or the crucible is placed on a platinum-wire triangle, heated to redness, and then sprinkled over with powdered potassium disulphate. Instead of the sulphate you may use borax, ^ever forget at last to polish the crucible with sea-sand again. When the crucible is clean, it is placed upon a clean platinum- 88 OPERATIONS. [ 52, wire triangle (fig. 40), ignited, allowed to cool in the desiccator, and weighed. This operation, though not indispensable, is still always advisable, that the weighing of the empty and filled crucible may be performed under as nearly as possible the same circum- stances. The empty crucible may of course be weighed after the ignition of the precipitate ; however, it is preferable in most cases to weigh it before. The ignition is effected with a BERZELIUS spirit-lamp or a gas-lamp, or else in a muffle. In igniting reducible substances over lamps, the analyst must always be on his guard against the contact of unconsumed hydro- carbons even in covered crucibles. When gas-lamps are used there is especial need of caution in this respect. Reduction will be avoided if the flame is made no larger than necessary, if the crucible is supported in the upper part of the flame, and if, when the crucible is in a slanting position, it is heated from behind. We pass on now to the description of the special methods. FIRST METHOD. (Ignition of the Precipitate with the Filter.) This method is resorted to in cases where there is no danger of a reduction of the precipitate by the action of the carbon of the filter. The mode of proceeding is as follows : The perfectly dry filter, with the precipitate, is removed from the funnel, and its sides are gathered together at the top, so that the precipitate lies enclosed as in a small bag. The filter is now put into the crucible, which is then covered and heated over a spirit-lamp with double draught, or over gas very gently, to effect the slow charring of the filter; the cover is now removed, the crucible placed obliquely, and a stronger degree of heat applied, until complete incineration of the filter is effected ; the lid, which had in the meantime best be kept on a porcelain plate, or in a por- celain crucible, is put on again, and a red heat applied for some time longer, if needed ; the crucible is now allowed to cool a little, and is then, while still hot, though no longer red hot,* taken off * Taking hold of a red Jwt crucible with brass tongs might cause the formation of black rings round it. 52.] IGXITIOX OF PRECIPITATES. 89 with a pair of tongs of brass or polished iron (fig. -tl), and put in the desiccator, where it is left to cool ; it is finally weighed. The combustion of the carbon of the filter may be promoted, in cases where it proceeds too slowly, by pushing the non-consumed particles, with a smooth and rather stout platinum wire, within the focus of the strongest action of the heat and air. And the oper- ator may also increase the draught of ail* by leaning the lid of the crucible against the latter in the manner illustrated in fig. 42. It will occasionally happen that particles of the carbon of the filter obstinately resist incineration. In such cases the operation may be promoted by putting a small lump of fused, dry ammonium Fig. 41. Fig. 42. nitrate into the crucible, placing on the lid and applying a gentle heat at first, which is gradually increased. However, as this way of proceeding is apt to involve some loss of substance, its applica- tion should not be made a general rule. In cases where the bulk of the precipitate is easily detached from the filter, the preceding method is occasionally modified in this, that the precipitate is put into the crucible, and the filter, with the still adhering particles, folded loosely together, and laid over the precipitate. In other respects, the operation is conducted in the manner above described. 90 OPERATIONS. SECOND METHOD. (Ignition of the Precipitate apart from the Filter.) This method is resorted to in cases where a reduction of the precipitate from the action of the carbon of the filter is appre- hended; and also where the ignited precipitate is required for further examination, which the presence of the filter ash might embarrass. It may be employed also, instead of the first method, in all cases where the precipitate is easily detached from the filter. The mode of proceeding is as follows : The crucible intended to receive the precipitate is placed upon a sheet of glazed paper ; the perfectly dry filter with the precipi- tate is taken out of the funnel, and gently pressed together over the paper, to detach the precipitate from the filter ; the precipitate is now shaken into the crucible, and the particles still adhering to the filter are removed from it, as far as practicable, by further pressing or gentle rubbing together of the folded filter, and are then also transferred to the crucible. The filter is now spread open upon the sheet of glazed paper, and then folded in form of a little square box, enclosed on all sides by the parts turned up ; any minute particles of the precipitate that may have dropped on the glazed paper are brushed into this little box, with the aid of a small feather ; the box is closed again, rolled up, and one end of a long platinum wire spirally wound round it. The crucible being placed on or above a porcelain plate, the little roll is lighted, and, during its combustion, held over the crucible, so that the falling particles of the precipitate or filter ash may drop into it, or, at least, into the porcelain plate. In this way, and by occasionally holding the little roll again in or against the flame, the incineration of the filter is readily and safely eifected. "When the operation is terminated, a slight tap will suffice to drop the ash and the remain- ing particles of the precipitate into the crucible, which is then cov- ered, and the ignition completed as in 52. "Where it is intended to keep the ash separate from the precipitate, it is made to drop into the lid of the crucible, in which case it is better to ignite the crucible with the principal portion of the precipitate first. This method of incinerating the filter, devised by BTJNSEN, is preferable to the method formerly in use, in which the filter, freed, as far as 53, a.] BUNSEN'S METHOD OF RAPID FILTKATION. 91 practicable, from the precipitate, was burnt either whole or cut up into little bits on the lid of the crucible, the operation being pro- moted when necessary by gently pressing the still unconsumed particles with a platinum wire, or platinum spatula, against the red-hot lid. Xo matter which method of incineration is resorted to. the operation must always be conducted in a spot entirely pro- tected from draughts. Certain precipitates suffer some essential modification in their properties, in their solubility, for instance, from ignition. In cases where a portion of a substance of the kind is required, after the weighing, for some other purpose with which the effects of a red heat would interfere, the two operations of drying and igniting may be combined in the following way : The precipitate is col- lected on a filter dried at 100 ; it is then also dried, at 100, and weighed (' 50). A portion of the dry precipitate is put into a tared crucible, and its exact weight ascertained ; it is then exposed to a red heat, allowed to cool in the usual way, and weighed again ; the diminution of weight which it has undergone is calculated on the whole amount of the precipitate. SKX'S MKTHOD OF RAPID FILTRATION.* .V precipitate is washed either by filtration or by decantation : in the former case the portion of liquid not mechanically retained is allowed to drain from the precipitate ; in the latter it is sepa- rated by simply pouring it away, the foreign substances contained in the precipitate being then removed by the repeated addition of some washing-fluid, in each successive portion of which the pre- cipitate is, as far as possible, uniformly suspended, this process being continued until the amount of impurity becomes so minute that its presence may be entirely disregarded. In the process of filtration as hitherto conducted, the time re- quired is so long and the quantity of wash-water needed so great that some simplification of this continually recurring operation is in the highest degree desirable. The following method, which de- pends not upon the removal of the impurity by simple attenuation, but upon its displacement by forcing the wash- water through the * Ann. derChem. imdPharm., vol. cxlviii. p. 269; Am. Jour. Sci., xlvii. p. 321. 92 OPERATIONS. [ 53, a. precipitate, appears to me to combine all the requisite conditions and therefore to satisfy the need. / The rapidity with which a liquid filters depends, cceteris paribus, upon the difference which exists between the pressure upon its upper and lower surfaces. Supposing the filter to consist of a solid substance, the pores of which suffer no alteration by pres- sure, or by any other influence, then the volume of liquid filtered in the unit of time is nearly proportional to the difference in pres- sure : this is clearly shown by the following experiments, made with pure water and a filter consisting of a thin plate of artificial pumice-stone. The thin plate of pumice was hermetically fastened into a funnel consisting of a graduated cylindrical glass vessel, the lower end of which was connected with a large thick flask by means of a tightly fitting caoutchouc cork. The pressure in the flask was then reduced by rarefying the air by means of a method to be described upon another occasion ; and for each difference of pressure^, measured by a mercury column, the number of seconds t was observed which a given quantity of water occupied in passing through the filter. The following are the results : I. p. t. pt. metre. 0-179 91-7 16-4 0-190 81-0 15-4 0-282 52-9 14-9 0-472 33-0 15-6 In the ordinary process of filtration, p on the average amounts to no more than 0-.004 to 0-008 metre. The advantage gained, therefore, is easily perceived when we can succeed by some simple, practicable, and easily attainable method in multiplying this differ- ence in pressure one or two hundred times, or, say, to an entire atmosphere, without running any risk of breaking the filter. The solution of this problem is very easy : an ordinary glass funnel has only to be so arranged that the filter can be completely adjusted to its side even to the very apex of the cone. For this purpose a glass funnel is chosen possessing an angle of 60, or as nearly 60 as possible, the walls of which must be completely free from ine- qualities of every description; and into it is placed a second funnel made of exceedingly thin platinum-foil, and the sides of 53, a.] BUNSEN'S METHOD OF RAPID FILTRATION . 93 which possess exactly the same inclination as those of the glass funnel. An ordinary paper filter is then introduced into this coin- pound funnel in the usual manner ; when carefully moistened and so adjusted that no air-bubbles are visible between it and the glass, this filter, when filled with a liquid, will support the pressure of an extra atmosphere without ever breaking. Fig. 43. The platinum funnel is easily made from thin platinum-foil in the following manner : In the carefully chosen glass funnel is placed a perfectly accurately fitting filter made of writing-paper; this is kept in position by dropping a little melted sealing-wax between its upper edge and the glass ; the paper is next saturated with oil and filled with liquid plaster of Paris, and before the mixture solidifies a small wooden handle is placed in the centre. 94: OPERATIONS. [ 53, a. After an hour or so tlie plaster cone with the adhering paper filter can be withdrawn by means of the handle from the funnel, to which it accurately corresponds. The paper on the outside of the cone is again covered with oil, and the whole carefully inserted into liquid plaster of Paris contained in a small crucible 4 or 5 centims. in height. After the mixture has solidified, the cone may be easily withdrawn; the adhering paper filter is then detached, and any small pieces of paper still remaining removed by gentle rubbing with the linger. In this manner a solid cone is ob- tained accurately fitting into a hollow cone, and of which the angle of inclination perfectly corresponds with that of the glass funnel. Fig. 43, 1, represents the cones. By their help the small plati- num funnel is made. A piece of platinum (shown three-fourths of the natural size in fig. 44)* is cut from foil of such a thickness that one square centimetre weighs | / about O154 grm., and from the centre a a vertical 5 incision is made by the scissors to the edge c I d is then closely pressed upon the plaster, and the remaining portion of the platinum wrapped as equally and as closely as possible around the cone. On again heating the foil to redness, pressing it once more upon the cone, and inserting the whole into the hollow cone, and turning it round once or twice under a gentle pressure, the proper shape is completed. The platinum funnel, which should not allow of the transmission of light through its extreme point, even now possesses such sta- bility that it may be immediately employed for any purpose. If desired, it may be made still stronger by soldering down the over- lapping portion in one spot only to the upper edge of the foil by means of a grain or two of gold and borax ; in general, however, this precaution is unnecessary. If the shape has in any degree altered during this latter process, it is simply necessary to drop the platinum funnel into the hollow cone and then to insert the solid cone, when by one or two turns of the latter the proper form * The diameter of a in the original drawing is 2 '5 centimetres. Perforated platinum cones admirably adapted for use with the BUNSEN filtering apparatus can now be purchased of dealers in chemical apparatus, or of the manufacturer, Mr. J. Bishop, Sugartown, Chester Co., Pa. 53, a.] BUNSEN'S METHOD OF RAPID FILTRATION. 95 may be immediately restored. The platinum funnel is placed in the bottom of the glass funnel, the dry paper filter then introduced in the ordinary manner, moistened, and freed from all adhering air-bubbles by pressure with the finger. A filter so arranged and in perfect contact with the glass, when filled with a liquid will support the pressure of an entire atmosphere without the least danger of breaking ; and the- interspace between the folds of the platinum foil is perfectly sufficient to allow of the passage of a continuous stream of water. In order to be able to produce the additional pressure of an atmosphere, the filtered liquid is received in a strong glass flask instead of in beakers.* This flask is closed by means of a doubly perforated caoutchouc cork, through one of the holes of which the neck of the glass funnel is passed to a depth oifrmn 5 to 8 ceht't- n Litres (tig. 43, #); through the other is fitted a narrow tube open at both ends, the lower end of which is brought exactly to ///> len-l of the lowrr surface of the cork* to the other is adapted the caoutchouc tube connected with the apparatus destined to produce the requisite difference in pressure : this apparatus will be de- scribed immediately. The flasks are placed in a metallic or porce- lain vessel, in the conical contraction of wdiich several strips of cloth are fastened. This method of supporting the flask has the advantage that, in one and the same vivsi-1, tlasks varying in size from 0'5 to 2*5 litres stand equally weP <*nd that by simply laying a cloth over the mouth of the vesse/, the consequences of an explosion (which through inexperience or carelessness is possible) are rendered harmless. It is impossible to employ any of the air-pumps at present in use to create the difference in pressure, since the filtrate not unfre- quently contains chlorine, sulphurous acid, hydric sulphide, and other substances which would act injuriously upon the metallic portions of these instruments. I therefore employ a water air- pump constructed on the principle of SPRENGEL'S mercury-pump, and which appears to me preferable to all other forms of air-pump for chemical purposes, since it effects a rarefaction to within 6 or 12 millimetres pressure of mercury. Fig. 43 shows the arrangement of this pump. On opening the pinch-cock . Common alcohol of various degrees of strength. 3. ETHEK. The application of ether as a solvent is very limited. It is more frequently used mixed with alcohol, in order to diminish the solvent, power of the latter for certain substances, e.g., ammonium platinic chloride. The ordinary ether of the shops will answer the purpose. 4. CARBON BISULPHIDE (see " Qual. Anal."). II. ACIDS AND HALOGENS. a. Oxygen Acids. 1. SULPHURIC ACID. a. Concentrated sulphuric acid of the shops. J. Concentrated pure sulphuric acid. c. Bilute sulphuric acid. See "Qual. Anal." 2. NITRIC ACID. a. Pure nitric acid of 1-2 sp. gr. (see " Qual. Anal."). J. Red fuming nitric acid (concentrated nitric acid containing some hyponitric acid). Preparation. Two parts of pure, dry potassium nitrate are introduced into a capacious retort, and one part of concentrated sulphuric acid is added either through the tubulure of the retort, or if a common non-tubulated one is used, through the neck by means of a long funnel-tube bent at the lower end, carefully avoid- ing soiling the neck of the retort. The latter being put into a ves- sel filled with sand, or, better still, with iron turnings, is then con- nected with a receiver, but not quite aiivtight. The distillation is conducted at a gradually increased heat, and carried to dryness. The cooling of the receiver must be properly attended to during the distillation. In the preparation of small quantities, the retort 58.] REAGENTS. 107 is placed on a piece of wire-gauze, and heated with charcoal ; in this process it is always advisable to coat the retort by repeated application of a thin paste made of clay and water ; a little borax or sodium carbonate should be added to the water used for making the paste. Tests. Red fuming nitric acid must be in a state of the greatest possible concentration, and perfectly free from sulphuric acid. In order to detect minute traces of the latter, evaporate a few c. c. of the specimen in a porcelain dish nearly to dryness, dilute the resi- due with water, add some barium chloride, and observe whether a precipitate forms on standing. Uses. A powerful oxidizing agent and solvent ; it serves more especially to convert sulphur and metallic sulphides into sulphuric acid and sulphates respectively. 3. ACETIC ACID (see " Qual. Anal."). 4. TARTARIC ACID (see " Qual. Anal."). b. Hydrogen Acids and Hologens. 58. 1. HYDROCHLORIC Aero. a. Pure hydrochloric acid of 1*12 sp. gr. (see "Qual. Anal."). b. Pure fuming hydrochloric acid of about 1*18 sp. gr. Preparation. As in " Qual. Anal." 26, with this modifica- tion, however, that only 3 or 4 parts of water, instead of 6, are put into the receiver, to 4 parts of sodium chloride in the retort. The greatest care must be taken to keep the receiver cool, and to change it as soon as the tube through which the gas is conducted into it- begins to get hot, since it is now no longer hydrochloric acid gas which passes over, but an aqueous solution of the gas, in form of vapor, which would simply weaken the fuming acid, if it were allowed to mix with it. Tests. The fuming acid must, for many purposes, be perfectly free from chlorine and sulphurous acid. For the mode of testing for these impurities, see " Qual Anal." loc. cit. Test for sulphuric acid as under Nitric Acid, above. Uses. Fuming hydrochloric acid has a much more energetic action than the dilute acid ; it is, therefore, used instead of the latter in cases where a more rapid and energetic action is desirable. 108 KEAGENTS. [ 58. 2. HYDROFLUORIC ACID. This is employed for the decomposition of silicates and borates, sometimes in the gaseous form, sometimes in the condition of aqueous solution. In the first case, the substance to be decomposed is introduced into the leaden box, in which the hydrofluoric gas is being generated ; in the latter case, we must first prepare the aque- ous acid. The raw material employed is fluor spar or kryolite (LUBOLDT*). Both are first finely powdered, and then treated with concentrated sulphuric acid. To 1 part kryolite, 2-J parts sulphuric acid are used ; to 1 part fluor spar, 2 parts sulphuric acid are used. If the latter is employed, allow the mixture to stand in a dry place for several days, stirring every now and then, so that the silicic acid (which is generally contained in fluor spar) may first escape in the form of fluosilicic gas. Convenient distil- latory apparatus have been described by LUBOLDT (loc. cit.) and by H. BRiEGLEB.f The latter commends itself especially on account of its relatively small cost. It consists of a leaden retort, with a movable leaden top, which can be luted on. The receiver belong- ing to it is a box of lead, with a tubulure at the side, into which the neck of the retort just enters. The cover of the receiver is raised conical, and is provided at the top with an exit tube of lead. In the receiver a platinum dish containing water is placed, all joints are luted, and the retort is carefully heated in a sand-bath. The aqueous hydrofluoric acid found at the end of the operation in the platinum dish is perfectly pure. The small quantity of impure hydrofluoric acid which collects on the bottom of the receiver is thrown away. The hydrofluoric acid must entirely volatilize when heated in a platinum dish on a water-bath. The pure acid gives no precipitate when neutralized with potash, while potassium silico- fluoride separates if the acid contains hydrofluosilicic acid. The acid is best preserved in gutta-percha bottles, as recommended by STADELER. The greatest caution must be observed in preparing this acid, since, whether in the fluid or gaseous condition, it is one of the most injurious substances. 3. CHLORINE AND CHLORINE-WATER (see " Qual. Anal"). 4. NITRO-HYDROCHLORIC ACID (see " Qual. Anal."). 5. HYDROFLUOSILICIC ACID (see " Qual. Anal."). * Journ. furprakt. Chem., 76/330. f Annal. d. Chem. u. Pharm., Ill, 380. 59.] REAGENTS. 109 c. Sulphur Acids. 1. HYDROSULPHURIC ACID (see " Qual. Anal."). HI. BASES AND METALS. a. Oxygen Bases and Metals. 59. a. Alkali Bases. 1. POTASSIUM HYDROXIDE OR POTASSA AND SODIUM HYDROXIDE OR SODA (see " Qual. Anal."). All the four sorts of the caustic alkalies mentioned in the quali- tative part are required in quantitative analysis, viz., common solu- tion of soda, potassa purified with alcohol, solution of potassa pre- pared with baryta, and absolutely pure soda. Pure solution of potassa may be obtained also by heating to redness for half an hour in a copper crucible, a mixture of 1 part of potassium nitrate, and 2 or 3 parts of thin sheet copper cut into small pieces, treating the mass with water, allowing the oxide of copper to subside in a tall vessel, and removing the supernatant clear fluid by means of a syphon (WOHLER).* 2. AMMONIA (see " Qual. Anal."). ft. Alkali-earth Bases. 1. BARIUM HYDROXIDE OR BARYTA (see " Qual. Anal."). 2. CALCIUM HYDROXDDE OR LIME. Finely divided calcium hydroxide mixed with water (milk of lime), is used more particularly to effect the separation of magne- sium, &c., from the alkali metals. Milk of lime intended to be used for that purpose must, of course, be perfectly free from alka- lies. To insure this the slaked lime should be thoroughly washed, by repeated boiling with fresh quantities of distilled water. This operation is conducted best in a silver dish. When cold, the milk of lime so prepared is kept in a well-stoppered bottle. * Sodium hydroxide, made by acting on pure water by pure sodium and fusing in silver vessels, is to be had cheaply of the Magnesium Metal Company, Salford, Manchester, England. 110 REAGENTS. [ 60. y. Heavy Metals, and their Oxides. 60. 1. ZINC. Zinc has of late been much used as a reagent in quantitative analy- sis. It serves more especially to effect the reduction of ferric to ferrous salts, and also the precipitation of copper from solutions of its salts. Zinc intended to be used for the former purpose must be free from iron, for the latter free from lead, copper, and other metals which remain undissolved upon treating the zinc with dilute acids. To procure zinc which leaves no residue upon solution in dilute sulphuric acid, there is commonly no other resource but to re-distil the commercial article. This is effected in a retort made of the material of Hessian or black-lead crucibles. The operation is conducted in a wind-furnace with good draught. The neck of the retort must hang down as perpendicular as possible. Under the neck is placed a basin or small tub, filled with water. The distillation begins as soon as the retort is at a bright red heat. As the neck of the retort is very liable to become choked up with zinc, or oxide of zinc, it is neces- sary to keep it constantly free by means of a pipe-stem. The zinc obtained by this re-distillation is nearly or quite free from lead. Tests. The following is the simplest way of testing the purity of zinc : dissolve the metal in dilute sulphuric acid in a small flask provided with a gas-evolution tube, place the outer limb of the tube under water, and w T hen the solution is completed, let the water entirely or partly recede into the flask ; after cooling, add to the fluid, drop by drop, a sufficiently dilute solution of potassium per- manganate. If a drop of that solution imparts the same red tint to the zinc solution as to an equal volume of water, the zinc may be considered free from iron. I prefer this way of testing the purity of zinc to other methods, as it affords, at the same time, an ap- proximate, or, if the zinc has been weighed, and the permanganate solution (which, in that case, must be considerably diluted) measured, an accurate and precise knowledge of the quantity of iron present. If lead or copper are present, these metals remain undissolved upon solution of the zinc. 2. LEAD OXIDE. Precipitate pure lead nitrate or acetate with ammonium car- 61.] KEAGENTS. HI bonate, wash the precipitate, dry, and ignite gently to complete decomposition. Lead oxide is often used to fix an acid, so that it is not expelled even by a red heat. b. Sulphur Bases. 1. AMMONIUM SULPHIDE (see " Qual. Anal."). We require both the colorless monosulphide, and the yellow polysulphide. 2. SODIUM SULPHIDE (sep " Qual. Anal."). IV. SALTS. a. Salts of the Alkalies. 61. 1. POTASSIUM SULPHATE (see " Qual. Anal."). 2. AMMONIUM OXALATE (see " Qual. Anal."). 3. SODIUM ACETATE (see " Qual. Anal."). 4. AMMONIUM SUCCTNATE. Preparation. Saturate succinic acid, which has been purified by dissolving in nitric acid and recrystallizing, with dilute ammo- nia. The reaction of the new compound should be rather slightly alkaline than acid. Uses. This reagent serves occasionally to separate ferric iron from other metals. 5. SODIUM CARBONATE (see " Qual. Anal."). This reagent is required both in solution and in pure crystals ; in the latter form to neutralize an excess of acid in a fluid which it is desirable not to dilute too much. 6. AMMONIUM CARBONATE (see "Qual. Anal."). 7. SODIUM HYDROGEN SULPHITE (see " Qual. Anal."). 8. SODIUM THIOSULPHATE (HYPOSULPHITE), N 2 S 2 O 3 . This salt occurs in commerce. It should be dry. clear, well crystallized, completely and with ease soluble in water. The solu- tion must give with silver nitrate at first a white precipitate, must not effervesce with acetic acid, and when acidified must give no pre- cipitate with barium chloride, or at most, only a slight turbidity. The acidified solution must, after a short time, become milky from separation of sulphur. EEAGENTS. [ 62. Uses. Sodium thiosulphate is used for the precipitation of several metals, as sulphides, particularly in separations, for instance, of copper from zinc ; it also serves as solvent for several salts (sil- ver chloride, calcium sulphate, &c.) ; lastly, it is employed in volu- metric analysis, its use here depending on the reaction 2(Na 2 S a O 3 ) 9. POTASSIUM NITRITE (see " Qual. Anal."). 10. POTASSIUM DICHROMATE (see " Qual. Anal."). 11. AMMONIUM MOLYBDATE (see " Qual. Anal."). 12. AMMONIUM CHLORIDE (see "Qual. Anal."). 13. POTASSIUM CYANIDE (see " Qual. Anal."). b. Salts of the Alkali-earth Metals. 62. 1. BARIUM CHLORIDE (see " Qual. Anal."). The following process gives a very pure barium chloride, free from calcium and strontium : Transmit through a concentrated solution of impure barium chloride hydrochloric gas, as long as a precipitate continues to form. Nearly the whole of the barium chloride present is by this means separated from the solution, in form of a crystalline powder. Collect this on a filter, let the adhering liquid drain off, wash the powder repeatedly with small quantities of pure hydrochloric acid, until a sample of the wash- ings, diluted with water, and precipitated with sulphuric acid, gives a filtrate which, upon evaporation in a platinum dish, leaves no residue. The hydrochloric mother-liquor serves to dissolve fresh portions of witherite. I make use of the barium chloride so obtained, principally for the preparation of perfectly pure barium carbonate, which is often required in quantitative analyses. 2. BARIUM ACETATE. Preparation. Dissolve pure barium carbonate in moderately dilute acetic acid, filter, and evaporate to crystallization. Tests. Dilute solution of barium acetate must not be rendered turbid by solution of silver nitrate. See also " Qual. Anal.," Barium chloride, the same tests being also used to ascertain the purity of the acetate. Uses. Barium acetate is used instead of barium chloride, to effect the precipitation of sulphuric acid, in cases where it is desir- 63.] REAGENTS. 113 able to avoid the introduction of a chloride into the solution, or to convert the base into an acetate. As the reagent is seldom required, it is best kept in crystals. 3. BARIUM CARBONATE (see "Qual. Anal."). 4. STRONTIUM CHLORIDE. Preparation. Strontium chloride is prepared from strontian- ite or celestine, by the same processes as barium chloride. The pure crystals obtained are dissolved in alcohol of 96 per cent., the solution is filtered, and kept for use. Uses. The alcoholic solution of strontium chloride is used to effect the conversion of alkali sulphates into chlorides, in cases where it is desirable to avoid the introduction into the fluid of a salt insoluble in alcohol. 5. CALCIUM CHLORIDE (see " Qual. Anal."). 6. MAGNESIUM CHLORIDE OR MAGNESIUM MIXTURE. Dissolve 11 parts crystallized magnesium chloride (MgCl, + 6 H 3 O) and 28 parts ammonium chloride in 130 parts water, add 70 parts dilute ammonia solution (sp. gr. 0'96). Allow the mix- ture to stand one or two days and filter. This solution, commonly called " magnesia mixture," is used to precipitate phosphoric acid. An excess is required to effect complete precipitation. Prepared as here described, about 10 c. c. should be used in ordinary cases for every O'l gramme P,O 5 . A solution containing the same per cent, (approximately) of magnesium chloride and other constituents may also be prepared from common calcined magnesia (MgO), provided it is free from the other alkali-earth metals, as follows : Add to 11 parts magnesia sufficient hydrochloric acid to effect solution, next add a slight ex- cess of magnesia and boil to separate traces of iron ; filter, and add 140 parts ammonium chloride and 350 parts dilute ammonia. Dilute with water until volume equals 1000 c. c. for every 11 grammes of MgO used. Allow the mixture to stand two or three days, and filter if necessary. c. Salts of the Heavy Metals. 63. 1. FERROUS SULPHATE (see "Qual. Anal."). 2. FERRIC CHLORIDE (see " Qual. Anal."). 3. URANIC ACETATE. 114 REAGENTS. [ 64. Heat finely powdered pitchblende with dilute nitric acid, filter the fluid from the undissolved portion, and treat the filtrate with hydrosulphuric acid to remove the lead, copper, and arsenic; filter again, evaporate to dryness, extract the residue with water, and fil- ter the solution from the oxides of iron, cobalt, and manganese. Uranic nitrate crystallizes from the filtrate ; purify this by recrys- tallization, and then heat the crystals until a small portion of uranic oxide is reduced. Warm the yellowish-red mass thus obtained with acetic acid, filter and let the filtrate crystallize. The crystals are uranic acetate, and the mother-liquor contains the undecom- posed nitrate (WERTHEIM). Tests. Solution of uranic acetate after acidification with hydrochloric acid must not be altered by hydrosulphuric acid; ammonium carbonate must produce in it a precipitate, soluble in an excess of the precipitant. Use-s. Uranic acetate may serve, in many cases, to effect the separation and determination of phosphoric acid. 4. SILVER NITRATE (see " Qual. Anal."). 5. LEAD ACETATE (see " Qual. Anal."). 6. MERCURIC CHLORIDE (see " Qual. Anal."). 7. STANNOUS CHLORIDE (see " Qual. Anal."). 8. PLATINIC CHLORIDE (see " Qual. Anal."). 9. SODIUM PALLADIO-CHLORIDE (see " Qual. Anal."). B. REAGENTS FOR GRA VIMETRIC ANAL YSIS IN THE DR Y WA Y. 64. 1. SODIUM CARBONATE, pure anhydrous (see " Qual. Anal."). 2. MIXED SODIUM AND POTASSIUM CARBONATES (see " Qual. Anal."). 3. BARIUM HYDROXIDE OR BARYTA (see " Qual. Anal." and 59). 4. POTASSIUM NITRATE (see " Qual. Anal."). 5. SODIUM NITRATE (see " Qual. Anal."). G. BORAX (fused). Preparation. Heat crystallized borax (see " Qual. Anal.) in a platinum or porcelain dish, until there is no further intumescence; reduce the porous mass to powder, and heat this in a platinum cru- cible until it is fused to a transparent mass. Pour the semi-fluid, 64.] EEAGENTS. 115 viscid mass upon a fragment of porcelain. A better way is to fuse the borax in a net of platinum gauze, bj making the gas blowpipe- flame act upon it. The drops are collected in a platinum dish. The vitrified borax obtained is kept in a well-stoppered bottle. But as it is always necessary to heat the vitrified borax previous to use, to make quite sure that it is perfectly anhydrous, the best way is to prepare it only when required. Uses. Vitrified borax is used to effect the expulsion of car- bonic acid and other volatile acids, at a red heat. 7. POTASSIUM DISULPHATE. Preparation. Mix 87 parts of normal potassium sulphate (see " Qual. Anal."), in a platinum' crucible, with 49 parts of concen- trated pure sulphuric acid, and heat to gentle redness until the mass is in a state of uniform and limpid fusion. Pour the fused salt on a fragment of porcelain, or into a platinum dish standing in cold water. After cooling, break the mass into pieces, and keep for use.* Uses. This reagent serves as a flux for certain native com- pounds of alumina and chromic oxide. Potassium disulphate is used also, as we have already had occasion to state, for the cleansing of platinum crucibles; for this latter purpose, however, the salt which is obtained in the preparation of nitric acid will be found sufficiently pure. 8. AMMONIUM CARBONATE (solid). Preparation. See " Qual. Anal." This reagent serves to con- vert the acid alkali sulphates into normal salts. It must com- pletely volatilize when heated in a platinum dish. 9. AMMONIUM TITRATE. Preparation. Neutralize pure ammonium carbonate with pure nitric acid, warm, and add ammonia to slightly alkaline reaction ; filter, if necessary, and let the filtrate crystallize. Fuse the crys- tals in a platinum dish, and pour the fused mass upon a piece of porcelain ; break into pieces whilst still warm, and keep in a well- stoppered bottle. Tests. Ammonium nitrate must leave no residue when heated in a platinum dish. * [J. Lawrence Smith advises the use of sodium disulphate for fluxing alumi- nous compounds, as the fused mass is much more readily soluble in water.] 116 REAGENTS. [ 64. Uses. Ammonium nitrate serves as an oxidizing agent ; for instance, to convert lead into lead oxide, or to effect the com- bustion of carbon, in cases where it is desired to avoid the use of iixed salts- 10. AMMONIUM CHLORIDE. Preparation and Tests. See " Qual. Anal." Uses. Ammonium chloride is often used to convert metallic oxides and acids, e.g., lead oxide, zinc oxide, stannic oxide, arsenic acid, antimonic acid, &c., into chlorides (ammonia and water escape in the process). Many metallic chlorides being volatile, and others volatilizing in presence of ammonium chloride fumes, they may be completely removed by igniting them with ammonium chloride in excess, and thus many compounds, e.g., alkali antimonates, may be easily and expeditiously analyzed. Ammonium chloride is also used to convert various salts of other acids into chlorides, e.g., small quantities of alkali sulphates. 11. HYDROGEN GAS. Preparation. Hydrogen gas is evolved when dilute sulphuric acid is added to granulated zinc. It may be purified from traces of foreign gases either by passing first through mercuric chloride solution, then through potash solution, or as recommended by STENHOUSE, by passing through a tube filled with pieces of char- coal. If the gas is desired dry, pass through sulphuric acid or a calcium chloride tube. Tests. Pure hydrogen gas is inodorous. It ought to burn with a colorless flame, which, when cooled by depressing a porcelain dish upon it, must deposit nothing on the surface of the dish except pure water (free from acid reaction). Uses. Hydrogen gas is frequently used, in quantitative analy- sis, to reduce oxides, chlorides, sulphides, &c., to the metallic state. 12. CHLORINE. Preparation. See " Qual. Anal." Chlorine gas is purified and dried by transmitting it through concentrated sulphuric acid, or a calcium chloride tube. Uses. Chlorine gas serves principally to produce chlorides, and to separate the volatile from the non-volatile chlorides; it is also used to displace and indirectly determine bromine and iodine. 65.] KEAGENTS. 11? G. REAGENTS USED IN VOLUMETRIC ANALYSIS. 65. Under this head are arranged the most important of those substances, which serve for the preparation and testing of the fluids required in volumetric analysis, and have not been given sub A and B. 1. PUKE CRYSTALLIZED OXALIC ACID, H a C 3 O 4 -f- 2H a O. The introduction of crystallized oxalic acid as a basis for alkali- metry and acidiraetry is due to FR. MOHR. It is also employed to determine the strength of, or to standardize, a solution of potas- sium permanganate, 1 molecule of potassium permanganate being required, in the presence of free sulphuric acid, to convert 5 mole cules of oxalic acid into carbon dioxide and water (K a Mn a O 8 -(- 5H a C a 4 + 3H a S0 4 = K a S0 4 + 2MnSO 4 + 8H 2 O + lOCO,). We use in most cases the pure crystallized acid which has the formula H a C 2 O 4 -j- 2H a O, and of which the molecular weight is accordingly 126. Preparation. See " Qual. Anal.," under Ammonium Oxalate. Tests. The crystals of oxalic acid must not show the least sign of efflorescence (to which they are liable even at 20 in a dry atmosphere) ; they must dissolve in water to a perfectly clear fluid ; when heated in a platinum dish, they must leave no fixed and incombustible residue (calcium carbonate, potassium carbonate, &c.). If the acid obtained by a first crystallization fails to satisfy these requirements, it must be recrystallized. 2. TINCTURE OF LITMUS. Preparation. Digest 1 part of litmus of commerce with 6 parts of water, on the water-bath, for some time, filter, divide the blue fluid into 2 portions, and saturate in one half the free alkali, by stirring repeatedly with a glass rod dipped in very dilute nitric acid, until the color just appears red ; add the remaining blue half, together with 1 part of strong spirit of wine, and 'keep the tincture which is now ready for use, in a small open bottle, not quite full, in a place protected from dust. In a stoppered bottle the tincture would speedily lose color. Tests. Litmus tincture is tested by coloring with about 100 cubic centimetres of water distinctly blue, dividing the fluid into 118 KEAGENTS. [ 65. two portions, and adding to the one the least quantity of a dilute acid, to the other a trace of solution of soda. If the one portion acquires a distinct red, the other a distinct blue tint, the litmus tincture is fit for use, as neither acid nor alkali predominates. 3. POTASSIUM PERMANGANATE. Preparation. Mix 8 parts of very finely powdered pure pyro- lusite, or manganese binoxide, with 7 parts of potassium chlorate, put the mixture into a shallow cast-iron pot, and add 37 parts of a solution of potassa of 1*27 specific gravity (the same solution as is used in organic analysis *) ; evaporate to dry ness, stirring the mixture during the operation ; put the residue before it has ab- sorbed moisture, into an iron or Hessian crucible, and expose to a dull-red heat, with frequent stirring with an iron rod or iron spa- tula, until no more aqueous vapors escape and the mass is in a faint glow. Remove the crucible now from the fire, and transfer the friable mass to an iron pot. Reduce to coarse powder, and transfer this, in small portions at a time, to an iron vessel containing 100 parts of boiling water; keep boiling, replacing the evaporating water, and passing a stream of carbon dioxide through the fluid ( MULDER f). The originally dark-green solution of potassium manganate soon changes, with separation of hydrated manganese binoxide, to the deep violet-red of the permanganate. When it is considered that the conversion is complete, allow to settle, take out a small quantity of the clear liquid, boil and pass carbon dioxide through it. If a precipitate forms, the conversion is not yet complete. The solution may be filtered through gun-cotton. Evaporate, crystallize, and dry the crystals on a porous tile. The pure salt is now to be obtained in commerce. 4. AMMONIUM FERROUS SULPHATE. FeS0 4 .(KE 4 ) 2 S0 4 + 6H 3 O. FR. MOHR has proposed to employ this double salt, which is not liable to efflorescence and oxidation, as an agent to determine the strength of the permanganate solution. Preparation. Take two equal portions of dilute sulphuric * Or instead of the solution, use 10 parts of the hydroxide KOH. In this case fuse the potash and the chlorate together first; and then project the manganese into the crucible. f Jahresbericht von Kopp und Will, 1858, 581. 65.] REAGENTS. 119 acid, and warm the one with a moderate excess of small iron nails free from rust, until the evolution of hydrogen gas has alto- gether or very nearly ceased ; neutralize the other portion exactly with ammonium carbonate, and then add to it a few drops of dilute sulphuric acid. Filter the solution of the ferrous sulphate into that of the ammonium sulphate, evaporate the mixture a little, if neces- sary, and then allow the salt to crystallize. Let the crystals, which are hard and of a pale-green color, drain in a funnel, then wash them in a little water, dry thoroughly on blotting-paper in the air, and keep for use. The molecular weight of the salt (392) is exactly 7 times the atomic weight of iron (56). The solution of the salt in water which has been just acidified with sulphuric acid must not become red on the addition of potassium sulphocyanate. 5. AMMONIA-IKON-ALUM. Preparation. Bring into a large porcelain dish 58 grms. of pure crystallized ferrous sulphate (see Fresenius' "Qual. Anal." Am. ed., p. 73), together with a quantity of oil of vitriol equiva- lent to 8-3 grms. of sulphuric anhydride (SO 8 ), (see Table, 1 ( J1). Heat upon a sand-bath, adding nitric acid from time to time, in small portions, until the iron has all passed into ferric sulphate, or until a drop of the solution gives no blue coloration with potassium ferricyanide. Heat further, and evaporate until the excess of nitric acid is expelled, then add 14 grms. of ammonium sulphate,* and, if need be, hot water sufficient to bring the salt into solution ; filter into a porcelain capsule and set aside, under cover, to crys- tallize. The iron-alum separates in cubo-octahedrons, which may be yel- lowish, lilac, or colorless. If dark in color, dissolve in warm water, add a few drops of oil of vitriol, and crystallize again. Rinse the pale or colorless crystals, after separation from the mother-liquor, with cold water, wrap up closely in filter paper, and allow them to dry at the ordinary temperature.f * If not on hand, this salt may be prepared by saturating oil of vitriol with ammonium carbonate and evaporating to dryness. 30 grammes of oil of vitriol give somewhat more than is required above. f Examinations of iron-alum thus prepared show that the variations in the 120 REAGENTS. [ 65. The yield should be about 80 grms. The dry salt should be pulverized, pressed between folds of paper until freed from mechanically adhering water, and preserved in a well-stoppered bottle. Uses. Ammonia-iron-alum furnishes the best means of obtain- ing a definite quantity of iron in a ferric salt for making standard solutions, being easily obtained pure and inalterable if kept away from acid vapors. Its purity may be readily controlled by ascertaining the loss on careful ignition, which should leave a resi- due of 16*6 per cent, of ferric oxide of iron, corresponding to 11*62 per cent, of metallic iron. 6. PUKE IODINE. Preparation. Triturate iodine of commerce with -J part of its- weight of potassium iodide, dry the mass in a large watch-glass with ground rim, warm this gently on a sand-bath, or on an iron plate, and as soon as violet fumes begin to escape, cover it with another watch-glass of the same size. Continue the application of heat until all the iodine is sublimed, and keep in a well-closed glass bottle. The chlorine or bromine, which is often found in iodine of commerce, combines, in this process, with the potassium, and remains in the lower watch-glass, together with the excess of potassium iodide. Tests. Iodine purified by the process just now described, must leave no fixed residue when heated on a watch-glass. But, even supposing it should leave a trace on the glass, it would be of no great consequence, as the small portion intended for use has to be resublimed immediately before weighing. color of the salt, from colorless to rose, are not connected with appreciable differences of composition. J. H. Grove, of the Sheffield Laboratory, obtained the following results in the examination of ammonia-iron-alum crystals, the ferric oxide being estimated by ignition : Fe 2 3 ( 16-59 1st \ 16-55 ( 16-59 2d 16-53 3d 16-57 4th 16-57 5th 16-58 fith J 6tn \ 16-56 7th 16-55 Calculated 16'60 65.] REAGENTS. Uses. Pure iodine is used to determine the amount of iodine contained in the solution of iodine in potassium iodide, employed in many volumetric processes. 7. POTASSIUM IODIDE. Small quantities of this article may be procured cheaper in commerce than prepared in the laboratory. For the preparation of potassium iodide intended for analytical purposes I recommend BAUP'S method, improved by FREDERKING, because the product obtained by this process is free from iodic acid. Tests. Put a sample of the salt in dilute sulphuric acid. If the iodide is pure, it will dissolve without coloring the fluid ; but if it contain potassium iodate, the fluid will acquire a brown tint, from the presence of free iodine, the sulphuric acid setting free iodic and hydriodic acids which react on each other (HIO 3 -f- (HI) 5 = (H 2 O) 3 -f- I 6 ) with liberation of iodine which remains in solution. Mix the solution of another sample with silver nitrate, as long as a precipitate continues to form ; add solution of ammonia in excess, shake the mixture, filter, and supersaturate the filtrate with nitric acid. The formation of a white, curdy precipitate indicates the presence of chloride in the potassium iodide. Presence of potassium sulphate is detected by means of solution of barium chloride, with addition of some hydrochloric acid. Uses. Potassium iodide is used as a solvent for iodine in the preparation of standard solutions of iodine ; it is employed also to absorb free chlorine. In the latter case every atom of chlorine lib- erates an atom of iodine, which is retained in solution by the agency of the excess of potassium iodide. The potassium iodide intended for these uses must be free from potassium iodate and carbonate; the presence of trifling traces of potassium chloride or potassium sulphate is of no consequence. 8. ARSENIOUS OXIDE (As 3 O 3 ). The arsenious oxide sold in the shops in large pieces, externally opaque, but often still vitreous within, is generally quite pure. The purity of the article is tested by moderately heating it in a glass tube, open at both ends, through which a feeble current of air is transmitted. Pure arsenious oxide must completely volatilize in this process ; no residue must be left in the tube upon the expulsion of the sublimate from it. If a non-volatile residue is left which, when heated in a current of hydrogen gas, turns black, the 122 EEAGENTS. [ 65. arsenious oxide contains antimony teroxicle, and is unfit for use in analytical processes. Dissolve about 10 grms. of the arsenious oxide to be tested in soda, and add 1 2 drops lead acetate. If a brownish color is produced, the arsenious oxide contains arsenious sulphide and cannot be used. Arsenious oxide dissolves in a solution of sodium carbonate forming sodium arsenite which is used to determine hypochlorous acid, free chlorine, iodine, &c. 9. SODIUM CIILOKIDE. Perfectly pure rock-salt is best suited for analytical purposes. It must dissolve in water to a clear fluid ; ammonium oxalate, sodium phosphate, and barium chloride must not trouble the solution. Pure sodium chloride may be prepared also by MAKGUERITTE'S process, viz., conduct into a concentrated solution of common salt hydrochloric gas to saturation, collect the small crystals of sodium chloride which separate on a funnel, let them thoroughly drain, wash with hydrochloric acid, and dry the sodium chloride finally in a porcelain dish, until the hydrochloric acid adhering to it has completely evaporated. The mother-liquor contains the small quantities of calcium sulphate, magnesium chloride, &c., originally present in the salt. Uses. Sodium chloride serves as a volumetric precipitating agent in the determination of silver, and also to determine the strength of solutions of silver intended for the estimation of chlo- rine. We usually fuse it before weighing. The operation must be conducted with caution, and must not be continued longer than necessary ; for if the gas-flame acts on the salt, hydrochloric acid escapes, -while sodium carbonate is formed. 10. METALLIC SHAVER. The silver obtained by the proper reduction of the pure chlo- ride of the metal alone can be called chemically pure. The silver precipitated by copper is never absolutely pure, but contains gener- ally about yoVjj f copper. Chemically pure silver is only used in small quantity to prepare the dilute solution employed for the determination of silver. The solution of silver required for the estimation of chlorine need not be made with absolutely pure silver, as the strength of this solu- tion had always best be determined after the preparation, by means of pure sodium chloride. 66.] REAGENTS. , 123 D. REAGENTS USED IN ORGANIC ANALYSIS. 66.- 1.' CUPRIC OXIDE. Preparation. Stir pure* copper scales (which should first be ignited in a muffle) with pure nitric acid in a porcelain dish to a thick paste ; after the effervescence has ceased, heat gently on the sand-bath until the mass is perfectly dry. Transfer the green basic salt produced to a Hessian crucible, and heat to a moderate redness, until no more fumes of hyponitric acid escape ; this may be known by the smell, or by introducing a small portion of the mass into a test tube, closing the latter with the finger, heating to redness, and then looking through the tube lengthways. The uniform decom- position of the salt in the crucible may be promoted by stirring the mass from time to time with a hot glass rod. When the cruci- ble has cooled a little, reduce the mass, which now consists of pure cupric oxide, to a tolerably fine powder, by triturating it in a brass or porcelain mortar ; pass through a metal sieve, and keep in a well-stoppered bottle for use. It is always advisable to leave a small portion of the oxide in the crucible, and to expose this again to an intense red heat. This agglutinated portion is not pounded, but simply broken into small fragments. Another method is to dissolve pure copper in pure nitric acid, evaporate to dryness in a porcelain dish, ignite the copper nitrate thus obtained in a Hessian crucible until no fumes arise on stirring the top of the mass with a rod. A portion in the bottom of the crucible will be sintered if a proper heat has been applied, while the upper part will be pulverulent. Treat the sintered portion as above, and reserve each separately. This method gives a reliable product. . Tests. Pure cupric oxide is a compact, heavy, deep-black pow- der, gritty to the touch ; upon exposure to a red heat it must evolve no hyponitric acid fumes, nor carbon dioxide ; the latter would indicate presence of fragments of charcoal, or particles of dust. It must contain nothing soluble in water. That portion of the oxide which has been exposed to an intense red heat should be hard, and of a grayish-black color. * If the scales contain lime, digest them with water, containing a little nitric acid, for a long time, wash, and then proceed as above. 124 REAGENTS. [ 00. Uses. Cupric oxide serves to oxidize the carbon and hydrogen of organic substances, yielding up its oxygen wholly or in part, according to circumstances. That portion of the oxide which has been heated to the most intense redness is particularly useful in the analysis of volatile fluids. JST.B. The cupric oxide, after use, may be regenerated by oxi- dation with nitric acid, and subsequent ignition. Should it have become mixed with alkali salts in the course of the analytical pro- cess, it is first digested with very dilute cold nitric acid, and washed afterwards with water. To purify cupric oxide containing chlo- ride, E. EKLENMEYER recommends to ignite it in a tube, first in a stream of moist air, and finally, when the escaping gas ceases to redden litmus paper, in dry air. By these operations any oxides of nitrogen that may have remained are also removed. 2. LEAD CHROMATE. Preparation. Precipitate a clear filtered solution of lead ace- tate, slightly acidulated with acetic acid, with a small excess of potassium dichromate ; wash the precipitate by decantation, and at last on a linen strainer ; dry, put in a Hessian crucible, and heat to bright redness until the mass is fairly in fusion. Pour out upon a stone slab or iron plate, break, pulverize, pass through a fine metallic sieve, and keep the tolerably fine powder for use. Tests. Lead chromate is a heavy powder, of a dirty yellowish- brown color. ~It must evolve no carbon dioxide upon the applica- tion of a red heat ; the evolution of carbon dioxide would indicate contamination with organic matter, dust, &c. It must contain nothing soluble in water. Uses. Lead chromate serves, the same as cupric oxide, for the combustion of organic substances. It is converted, in the pro- cess of combustion, into chromic oxide and basic lead chromate. It suffers the same decomposition, with evolution of oxygen, when heated by itself above its point of fusion. The property of lead chromate to fuse at a red heat renders it preferable to cupric oxide as an oxidizing agent, in cases where we have to act upon difficultly combustible substances. N.B. Lead chromate may be used a second time. For this purpose it is fused again (being first roasted, if necessary), and then powdered. After having been twice used it is powdered, moistened with nitric acid, dried, and fused. In this way the 66.] REAGENTS. 125 lead chromate may be used over and over agaia indefinitely (VOHL*). 3. OXYGEN GAS. Preparation. Triturate 100 grammes of potassium chlorate with 5 grammes of finely pulverized manganese binoxide, and introduce the mixture into a plain retort, which must not be more than half full ; expose the retort over a charcoal fire or a gas-lamp, at first to a gentle, and then to a gradually increased heat. As soon as the salt begins to fuse, shake the retort a little, that the contents may be uniformly heated. The evolution of oxygen speedily commences, and proceeds rapidly at a relatively low tem- perature, provided the above proportions be adhered to. As soon as the air is expelled from the retort, connect the glass tube fixed in the neck of the retort by means of a tight-fitting cork, with an india-rubber tube inserted in the lower orifice of the gasometer ; the glass tube must be sufficiently wide, and there must be sufficient space left around the india-rubber to permit the free efflux of dis- placed water. Continue the application of heat to the retort till the evolution of gas has ceased. 100 grammes of potassium chlorate give about 27 litres of oxygen. The oxygen produced by this process is moist, and may con- tain traces of carbon dioxide, and also of chlorine. These impuri- ties must be removed and the oxygen thoroughly dried, before it can be used in organic analysis. The gas is therefore passed from the gasometer first through a solution of potassa of 1'27 sp. gr., then through U tubes containing granulated soda lime, and finally, according to circumstances, through U tubes containing calcium chloride or pumice-stone moistened with sulphuric acid. Tests. A chip of wood which has been kindled and blown out so as to leave a spark at the extremity must immediately burst into flame in oxygen gas. The gas must not render lime-water or a solution of silver nitrate turbid when transmitted through these fluids. 4. SODA-LIME. Preparation. Take solution of soda N"aOH), ascertain its specific gravity, weigh out a certain quantity, calculate the weight of sodium hydroxide present, add twice this latter weight of the best quick-lime, allow the lime to slake, and then evaporate to dryness * Annalen d. Chem. u. Pharm., 106, 127. 126 KEAGENTS. [ 66. in an iron vessel. Heat the residue in an iron or Hessian crucible ; keep for some time at a low red heat. Break up while still warm in an iron mortar, and pass the whole through a sieve with meshes about 3 mm. wide. Reject the finest portion (removing it with a fine sieve) and keep the granulated product in a well-closed bottle. JJ S6t Granulated soda-lime prepared as above described forms an excellent absorbent for carbon dioxide. It was formerly also used for nitrogen determination instead of the following : 5. SODA-LIME FOK NITROGEN DETERMINATIONS.* Preparation. Equal weights of sal-soda in clean (washed) large crystals and of good white promptly slaking quick-lime are separately so far pulverized as to pass through holes of y 1 ^ inch, then well mixed together, placed in an iron pot which should not be more than half filled, and gently heated, at first without stir- ring. The lime soon begins to combine with the crystal w r ater of the sodium carbonate, the whole mass heats strongly, swells up, and in a short time yields a fine powder, which may then be stirred to effect intimate mixttire and to drive off the excess of water so that the mass is not perceptibly moist and yet short of the point at which it rises in dust on handling. "When cold it is secured in well-closed bottles or fruit jars, and is ready for use. 6. METALLIC COPPER. Metallic copper serves, in the analysis of nitrogenous substances, to effect the reduction of the nitric oxide gas that may form in the course of the analytical process. It is used either in the form of turnings, or copper scales reduced by hydrogen ; or of small rolls made of fine copper wire gauze. A length of from 7 to 10 centimetres is given to 'the spirals or rolls, and just sufficient thickness to admit of their being inserted into the combustion tube. To have it perfectly free from dust, oxide, &c., it is first heated to redness in the open air, in a crucible, until the surface is oxidized ; it is then put into a glass or porcelain tube, through which an uninterrupted current of dry hydrogen gas is transmitted; and when all atmospheric air has been expelled from the evolution apparatus and the tube, the latter is in its whole length heated to redness. The operator should * S. W. Johnson. Report of the Conn. Agr. Expr. Station, 1878, p. 111. 66.] REAGENTS. 127 make sure that the atmospheric air has been thoroughly expelled, before lie proceeds to apply heat to the tube ; neglect of this pre- caution may lead to an explosion. 7. POTASSIUM HYDROXIDE OR POTASSA. a. Solution of Potassa. Solution of potassa is prepared from the carbonate, with the aid of milk of lime, in the way described in the " Qualitative Analysis," for the preparation of solution of soda. The propor- tions are 1 part of potassium carbonate to 12 pails of water, and f part of lime, slaked to paste with three times the quantity of warm water. The decanted clear solution is evaporated, in an iron vessel, over a strong fire, until it has a specific gravity of 1*27 ; it is then, whilst still warm, poured into a bottle, which is well closed, and allowed to stand at rest until all solid particles have subsided. The clear solution is finally drawn off from the deposit, and kept for use. b. Fused Potassa (common). The commercial potassa in sticks (impure KOH usually com- bined with more or less H 2 O) will answer the purpose. If you wish to prepare it, evaporate solution of potassa (a) in a silver ves- sel, over a strong fire, until the residuary hydroxide flows like oil, and white fumes begin to rise from the surface. Pour the fused mass out on a clean iron plate, and break it up into small pieces. Keep in a well-stoppered bottle for use. c. Potassa (purified with alcohol), see " Qual. Anal.," p. 43. Uses. Solution of potassa serves for the absorption, and at the same time for the estimation of carbon dioxide. In many cases, a tube filled with fragments of fused potassa is used, in addition to the apparatus filled with solution of potassa. Potassa purified with alcohol, which is perfectly free from potassium sul- phate, is employed for the determination of sulphur in organic substances. 8. CALCIUM CHLORIDE. a. Pure Calcium Chloride. Preparation. Dissolve marble in commercial hydrochloric acid diluted with four or five times its volume of water. (The waste solution resulting from the preparation of carbon dioxide 128 KEAGENTS. [ 66. \ may be used.) Add to this solution with stirring lime, slaked with sufficient water to give it the consistency of thin paste until it gives an alkaline reaction and a pellicle of calcium carbonate forms on the surface on standing exposed to the air. Iron, man- ganese, and especially magnesium are usually present in such a solution, and are precipitated by the calcium hydroxide the iron, however, not completely. After a few hours, filter and pass hydro- gen sulphide through the alkaline solution until a filtered portion is no longer blackened by this reagent. Let the solution stand for twelve hours, then filter from the iron sulphide. Add next hydro- chloric acid to strongly acid reaction to convert the calcium sul- phide and calcium oxy chloride which may be present into chloride. Concentrate in a porcelain dish. If sulphur separates, after a short time filter again, and continue the evaporation to dry ness with addition of a little more hydrochloric acid toward the end of the process. Finally expose the residue to a tolerably strong heat about (200) on the sand-bath, until it is changed throughout to a white porous perfectly opaque mass, which point can be ascertained by breaking up a piece detached from the top. The product is CaCl 2 -f- (H 2 O) 2 . Reduce while still hot to granules of the proper size (-J- to -^ of an inch) by means of suitable sieves and a mortar previously warmed, and keep in well-closed bottles. b. Crude fused Calcium Chloride. Preparation. Neutralize the alkaline solution obtained in a (without separating the little iron present with H 2 S) exactly with hydrochloric acid, and evaporate to dryness in an iron pan ; fuse the residue in an iron or Hessian crucible, pour out the fused mass, and break into pieces. Preserve it in well-stoppered bottles. Uses. The crude fused calcium chloride serves to dry moist gases ; the pure chloride is used in elementary organic analysis for the absorption and estimation of water formed by the hydrogen contained in the analyzed substance. A solution of the pure cal- cium chloride should not show an alkaline reaction. A calcium chloride tube filled with it should not gain weight when a very slow current of perfectly dry carbon dioxide is passed through it an hour. 9. POTASSIUM BICHROMATE. Bichromate of potassa of commerce is purified by repeated recry stall ization, until barium chloride produces, in the solution of 66.] REAGENTS. 129 a sample of it in water, a precipitate which completely dissolves in hydrochloric acid. Potassium dichromate thus perfectly free from sulphuric acid is required more particularly for the oxidation of organic substances with a view to the estimation of the sulphur contained in them. "Where the salt is intended for other purposes, e.g., to determine the carbon of organic bodies, by heating them with potassium dichromate and sulphuric acid, one recrystallization is sufficient. SECTION III. FOEMS AND COMBINATIONS IN WHICH SUB- STANCES AKE SEPAEATED FEOM EACH OTHER, OR IN WHICH THEIR WEIGHT IS DETERMINED. 67. THE quantitative analysis of a compound substance requires, as the first and most indispensable condition, a correct and accurate knowledge of the composition and properties of the new combina- tions into which it is intended to convert its several individual constituents, for the purpose of separating them from one another, and determining their several weights. Regarding the properties of the new compounds, we have to inquire more particularly, in the first place, how they behave with solvents ; secondly, what is their deportment in the air ; and, thirdly, what is their behavior on ignition ? It may be laid down as a general rule, that compounds are the better adapted for quantitative determination the more insoluble they are, and the less alteration they undergo upon exposure to air or to a high temperature. With respect to the composition of a compound, it is better adapted to the quantitative determination of a body the less it contains relatively of that body ; since any error in weighing or loss of the compound to be weighed will have the less influence on the accuracy of the results the less the percentage it contains of the substance to be determined. In this section those combinations of the several bodies which are best adapted for their quantitative determination are enumer- ated and described. The description given of the external form and appearance of the new compounds relates more particularly to the state in which they are obtained in our analyses. With regard to the properties of the new compounds, we shall confine ourselves to the enumeration of those which bear upon the special objects we have more immediately in view. [The percentage compositions of these compounds are stated in connection with their description. For this purpose the symbols $ 67.] FORMULA. 131 of the constituent elements of the compounds in many cases (viz. : when they are oxygen salts) are grouped in a manner different from that used to express their chemical constitution. This grouping constitutes a kind of formulae differing from either the empirical or rational in ordinary use in modern text-books of chemistry, but identical with that formerly in general use (the old system). These formulae are based upon the fact that in all oxygen salts, whether normal, acid, basic, ortho-, meta-, or pyro- salts, there is just enough oxygen to form with the radicals present, both basic and acid, their corresponding oxides or anhydrides, and with hydrogen, if present, water. They represent oxides (and water) jointly equivalent in weight to the radicals, hydrogen, and remaining oxygen, which rational formulae represent as existing in oxygen salts. EXAMPLES. OTT Potassium sulphate, SO 2 < QK = ^A^O,. Hydrogen potassium sulphate, 8(80, < g|) = K,0,H,0,2SO, Potassium disulphate, < SO! - OK = K A2SO,. Ammonium magnesium phosphate, ^ O Magnesium pyrophosphate, PO < 2 > Mg Most analytical chemists prefer to present the results of analyses of oxygen salts in percentages of oxides (or anhydrides) and water on account of the simplicity of computations required. Accord- 132 FORMS. [ 68. ingly, in the following section, the percentage composition of oxygen salts is given in this manner, accompanied by correspond- ing formulae and molecular weights. These formulae are in every case preceded by rational formulae constructed in accordance with the theory of the constitution of oxygen salts which is now generally accepted.] A. FORMS IN WHICH THE BASIC RADICALS ARE WEIGHED OR PRECIPITA TED. BASIC RADICALS OF THE FIRST GROUP. 68. 1. POTASSIUM. The combinations best suited for the weighing of potassium are POTASSIUM SULPHATE, POTASSIUM CHLORIDE, and POTASSIUM PLATINIC CHLORIDE. a. Potassium sulphate crystallizes usually in small, hard, straight, four-sided prisms, or in double six-sided pyramids ; in the analytical process it is obtained as a white crystalline mass. It dissolves with some difficulty in water (1 part requiring 10 parts of water of 12), it is almost absolutely insoluble in pure alcohol, but slightly more soluble in alcohol containing sulphuric acid (Expt. No. 6). It does not affect vegetable colors ; it is unalter- able in the air. The crystals decrepitate strongly when heated, yielding at the same time a little water, which they hold mechani- cally confined. The decrepitation of crystals that have been kept long drying is less marked. At a good red heat the salt fuses without volatilizing or decomposing. At a white heat a little of the salt volatilizes and also some sulphuric acid, so that the residue possesses an alkaline reaction (AL. MITSCHERLICH,* BoussiNGAULTf). When exposed to a red heat, in conjunction with ammonium chloride, potassium sulphate is partly, and, upon repeated applica- tion of the process, wholly converted, with effervescence, into potassium chloride (H. KOSE). * Journ. f. prakt. Chem. 83, 486. f Zeitschr. f. anal. Chem. 7, 244. 68.] BASES OF GROUP I. 133 COMPOSITION. K 3 O . . . 94-26 54-09 ~ SO, 80-00 45-91 174-26 100-00 The acid potassium sulphate (KHSO 4 ), which is produced when the normal salt is evaporated to dryness with free sulphuric acid, is readily soluble in water, and fusible even at a moderate heat. At a red heat it loses sulphuric acid, and is converted into normal potassium sulphate, but not readily the complete conversion of the acid into the normal salt requiring the long-continued applica- tion of an intense red heat. However, when heated in an atmos- phere of ammonium carbonate which may be readily procured by repeatedly throwing into the faint red-hot crucible containing the acid sulphate small lumps of pure ammonium carbonate, and putting on the lid the acid salt changes readily and quickly to the normal sulphate. The transformation may be considered complete as soon as the salt, which was so readily fusible before, is perfectly solid at a faint red heat. b. Potassium: chloride crystallizes usually in cubes, often lengthened to columns ; rarely in octahedra. In analysis we obtain it either in the former shape, or as a crystalline mass. It is readily soluble in water, but much less so in dilute hydrochloric acid ; in absolute alcohol it is nearly insoluble, and but slightly soluble in common alcohol. It does not affect vegetable colors, and is unalterable in the air. When heated, it decrepitates, unless it has been kept long drying, with expulsion of a little water mechanically confined in it. At a moderate red heat, it fuses unaltered and without diminution of weight ; when exposed to a higher temperature, it volatilizes in white fumes ; this volatilization proceeds the more slowly the more effectually the access of air is prevented (Expt. No. 7). When repeatedly evaporated with solution of oxalic acid in excess, it is converted into potassium oxalate. When evaporated with excess of nitric acid, it is con- verted readily and completely into nitrate. On ignition with ammonium oxalate, potassium carbonate and potassium cyanide are formed in noticeable quantities. 134 FORMS. [ 68. COMPOSITION. K . . . . 39-13 52-46 Cl 35-46 47-54 74-59 100-00 c. Potassium platinic chloride presents either small reddish- yellow octahedra, or a lemon-colored powder. It is difficultly soluble in cold, more readily in hot water; nearly insoluble in absolute alcohol, and but sparingly soluble in common alcohol- one part requiring for its solution, respectively, 12083 parts of absolute alcohol, 3775 parts of alcohol of 76 per cent, and 1053 parts of alcohol of 55 per cent. (Expt. No. 8, a.) Presence of free hydrochloric acid sensibly increases the solubility (Expt. No. 8, b). In caustic potassa it dissolves completely to a yellow fluid. It is unalterable in the air, and at 100. On exposure to an intense red heat, four atoms of chlorine escape, metallic plati- num and potassium chloride being left ; but even after long-con- tinued fusion, there remains always a little potassium platinic chloride which resists decomposition. Complete decomposition is easily effected, by igniting the double salt in a current of hydrogen gas, or with some oxalic acid. According to ANDREWS, potassium platinic chloride, even though dried at a temperature considerably exceeding 100, retains still "0055 of its weight of water. COMPOSITION. (KC1), . . . 149-18 30-56 K 2 . . . 78-26 16-03 PtCl 4 ... 339-02 69-44 Pt . . . 197-18 40-39 01. . . . 212-76 43-58 488-20 100-00 488-20 100-00 d. Potassium silicqfluoride is obtained on mixing a solution of a potassium salt with hydrofluosilicic acid in the form of a trans- lucent iridescent precipitate, which increases and completely separates, when an equal volume of strong alcohol is added to the fluid. After being filtered off, washed with weak alcohol and dried, it is a soft white powder. It is difficultly soluble in cold water, far more readily in boiling water, not at all or in merest traces soluble in a mixture of water and strong alcohol in equal parts, but it is 69.] BASES OF GROUP I. 135 decidedly more soluble in the presence of any considerable quan- tity of free acid, especially hydrochloric or sulphuric acid. When potassa is added to the boiling aqueous solution of the salt the following change takes place : (KF) 2 SiF 4 + 4KOH = 6KF + Si(OH) 4 , the solution turning from acid to neutral (principle of STOLBA ? S volumetric method of estimating potassium). As soon as it is ignited the salt fuses, gives off silicon fluoride and leaves potassium fluoride. 69. 2. SODIUM. Sodium is usually weighed as SODIUM SULPHATE, SODIFM CHLO- RIDE, or SODIUM CARBONATE. It is separated from potassium in the form of SODIUM PLATINIC CHLORIDE, from other bodies occasionally in the form of sodium silicofluoride. a. Anhydrous normal sodium sulphate is a white powder or a white very friable mass. It dissolves readily in water ; but is sparingly soluble in absolute alcohol ; presence of free sulphuric acid slightly increases its solubility in that menstrum ; it is some- what more readily soluble in common alcohol (Expt. No. 9). It does not affect vegetable colors ; upon exposure to moist air, it slowly absorbs water (Expt. No. 10). At a gentle heat it is un- altered, at a strong red heat it fuses without decomposition or lo>s of weight. At a white heat it loses weight by volatilization of sodium sulphate and also of sulphuric acid (Ai.. MITSCHERLK n, BOUSSINGAULT). When ignited with ammonium chloride, it be- haves like potassium sulphate. COMPOSITION. OKa _ Na,O .... 62-08 43-69 ONa - SO 3 .... 80-00 . 56-31 142-08 100- 00 The acid sodium sulphate (sodium hydrogen sulphate, NaHSO 4 ) which is always produced upon the evaporation of a solution of the normal salt with sulphuric acid in excess, fuses even at a gentle heat ; it may be readily converted into the normal salt in the same manner as the acid potassium sulphate (see 68, a). b. Sodium chloride crystallizes in cubes, octahedra, and hollow 136 FORMS. [ 69. four-sided pyramids. In analysis it is frequently obtained as an amorphous mass. It dissolves readily in water, but is much less soluble in hydrochloric acid ; it is nearly insoluble in absolute alcohol, and but sparingly soluble in common alcohol ; 100 parts of alcohol of 75 per cent, dissolve, at a temperature of 15, '7 part ("WAGNER). It is neutral to A r egetable colors. Exposed to a somewhat moist atmosphere, it slowly absorbs water (Expt. No. 12). Crystals of this salt that have not been kept drying a considerable time decrepitate when heated, yielding a little water, which they hold mechanically confined. The salt fuses at a red heat without decomposition ; at a white heat, and in open vessels even at a bright red heat, it volatilizes in white fumes (Expt. No. 13). If a carburetted hydrogen name acts on fusing sodium chloride, hydro- chloric acid escapes, and some sodium carbonate is formed. On evaporation with oxalic or nitric acid as well as by ignition with ammonium oxalate, it behaves like the corresponding potassium salt. COMPOSITION. Na ..... 23-04 39-38 Cl 35-46 60-62 58-50 100-00 c. Anhydrous sodium carbonate is a w r hite powder or a white very friable mass. It dissolves readily in water, but much less so in solution of ammonia (MAEGUERITTE) ; it is insoluble in alcohol. Its reaction is strongly alkaline. Exposed to the air, it absorbs water slowly. On moderate ignition to incipient fusion it scarcely loses weight ; on long fusion, however, it volatilizes to a consider- able extent (Comp. Expt. 14). COMPOSITION. . ONa _ Na 2 O 62-08 58-52 -~ . . . 44-00 41-48 106-08 100-00 d. Sodium platinic chloride crystallizes with 6 mol. water (NaCl) 3 . PtCl 4 + 6 H 2 O, in light yellow, transparent, prismatic crystals which dissolve readily both in water and in common alcohol. 70.] BASES OF (iJK)UP I. 137 e. Sodium silicofluoride is similar in properties to the corre- sponding potassium salt. It has an analogous composition, and is decomposed in the same way by alkalies. It is, however, con- siderably more soluble in water and in diluted alcohol. 3. AMMONIUM. Ammonium is most appropriately weighed as AMMONIUM CHLORIDE, or as AMMONIUM pLATiNic CHLORIDE, or it may be esti- mated from the weight of the PLATINUM in the latter compound. Under certain circumstances ammonium may also be estimated from the volume of the NITROGEN GAS eliminated from it ; and it is frequently estimated by alkalimetry. a. Ammonium chloride crystallizes in cubes and octahedra, but more frequently in feathery crystals. In analysis we obtain it uniformly as a white mass. It dissolves readily in water, but is difficultly soluble in common* alcohol. It does not alter vegetable colors, and remains unaltered in the air. Solution of ammonium chloride, when evaporated on the water-bath, loses a small quantity of ammonia, and becomes slightly acid. The diminution of weight occasioned by this loss of ammonia is very trifling (Expt. Xo. 15). At 100 ammonium chloride loses nothing, or very little of its weight (comp. same Expt.). At a higher temperature it volatilizes readily, and without undergoing decomposition. COMPOSITION. XII 18-04 33-72 NH 3 . . 17-04 31-85 Cl , 35-46 66-28 HC1 . . 36-46 68-15 53-50 100-00 53-50 100-00 100*parts of ammonium chloride correspond to 48 67 parts of ammonium oxide. J. Ammonium platinic chloride occurs either as a heavy, lemon-colored powder, or in small, hard octahedral crystals of a bright yellow colon It is difficultly soluble in cold, but more readily in hot water. It is very sparingly soluble in absolute alcohol, but more readily in common alcohol 1 part requiring of absolute alcohol, 26535 parts; of alcohol of 76 per cent., 14<><'> 138 FORMS. [ 71. parts; of alcohol of 55 per cent., 665 parts. The presence of free acid sensibly increases its solubility (Expt. No. 16). It remains unaltered in the air, and at 100. It loses a little water between 100 and 125. Upon ignition chlorine and ammonium chloride escape, leaving the metallic platinum as a porous mass (spongy platinum). However, if due care be not taken, in this process, to apply the heat gradually, the escaping fumes will carry off particles of platinum, which will coat the lid of the crucible. For properties of metallic platinum, see 89, a. COMPOSITION. (NH 4 Cl) a . . 107-00 23-99 (NH 4 ) 2 . . 36-08 8-09 PtCl 4 . . .339-02 76-01 Pt . . . .197-18 44-21 01. ... 212-76 47-70 446-02 100-00 446-02 100-00 N, ... 28-08 6-295 (NH,) S . . 34-08 7-64 H 8 . . . 8-00 1-794 Pt ... 197-18 44-209 (HOI), . . 72-92 16-35 Ol, . . .212-76 47-702 PtCl 4 . . . 339-02 76-01 446-02 100-000 446-02 100-00 100 parts of ammonium platinic chloride correspond to 11-677 parts of ammonium oxide. c. Nitrogen gas is colorless, tasteless, and inodorous ; it mixes with air, without producing the slightest coloration ; it does not affect vegetable colors. Its specific gravity is -97137 (REGNAULT). One litre weighs at 0, and '76 metre bar., 1-25617 grm. It is difficultly soluble in water, 1 volume of water absorbing, at 0, and 76 pressure, -02035 vol.; at 10, -01607 vol.; at 15, -01478 vol. of nitrogen gas (BUNSEN). BASIC RADICALS OF THE SECOND GROUP. 71. 1. BARIUM. . Barium is weighed as BARIUM SULPHATE/ BARIUM CARBONATE, and BARIUM SILICOFLUORIDE. a. Artificially prepared 'barium sulphate presents the appear- ance is of a fine white powder. When recently precipitated, it 71.] BASES OF GROUP II. 139 difficult to obtain a clear filtrate, especially if the precipitation was effected in the cold, and the solution contains neither hydrochloric acid nor ammonium chloride. It is as good as insoluble in cold and in hot water. (1 part of the salt requires more than 400,< >< >< > parts of water for solution.) It has a great tendency, upon pre- cipitation, to carry down with it other substances contained in the solution from which it separates, more particularly barium nitrate, nitrates and chlorates of the alkali metals, ferric oxide, &c. Several of the impurities, such, for instance, as potassium or sodium chlo- rates, may be removed by igniting the barium sulphate, moistening with hydrochloric acid, evaporating the latter off and exhausting the residue with water ; other impurities again, such as potassium or sodium nitrates, cannot be removed" by this treatment. Even the precipitate obtained from a solution of barium chloride by means of sulphuric acid in excess contains traces of barium chloride, which it is impossible to remove, even by washing with boiling water, but which are dissolved by nitric acid (SIEGLE). Cold dilute acids dissolve trifling, yet appreciable traces of barium sulphate ; for instance, 1000 parts of nitric acid of 1/032 sp. giv dissolve '062 parts (CALVERT). 1000 parrs of hydrochloric acid containing 3 per cent, dissolve ()(> parts.* Cold concentrated acids dissolve consid- erably more ; thus, 1000 parts of nitric acid of 1'167 sp. gr. dis- solve 2 parts (CALVERT). Boiling hydrochloric acid also dissolves appreciable traces; thus 230 c.c. hydrochloric acid of 1/02. sp. gr. were found, after a quarter of an hour's boiling with '679 grm. barium sulphate, to have dissolved of it -048 grm. Acetic acid dissolves less barium sulphate than the other acids; thus, 80 c.c. acetic acid of 1*02 sp. gr. were found, after a quarter of an hour's boiling with ! grm., to have dissolved only -002 grm. (SIEGLE). Free chlorine considerably increases its solubility (O. L. ERDMANN). Several salts more particularly interfere with the precipitation of barium by sulphuric acid. I observed this some time ago with magnesium chloride, but ammonium nitrate (MITTENTZWEY), alkali nitrates generally,* and more particularly alkali citrates (SPILLER), possess this property in a high degree. In the last case the pre- cipitate appears on the addition of hydrochloric acid. If a fluid contains metaphosphoric acid, barium cannot be completely pre- cipitated out of it by means of sulphuric acid ; the resulting pre- cipitate too contains phosphoric acid (SCHEERER, RUBE). Barium * Zeitschr. f . anal. Chem. 9, 62. 140 FOKMS. [71. sulphate dissolves in tolerable quantity in concentrated sulphuric acid, but separates again on dilution. It is as good as insoluble in a boiling solution of ammonium sulphate (1 in 4). Barium sulphate remains quite unaltered in the air, at 100, and even at a red heat. At a strong white heat it loses sulphuric acid (Bous- SINGAULT).* On ignition with charcoal, or under the influence of reducing gases, it is converted comparatively easily, but as a rule only partially, into barium sulphide. On ignition with ammonium chloride, barium sulphate undergoes partial decomposition. It is not affected, or affected but very slightly, by cold solutions of the hydrogen carbonates of the alkali metals or of ammonium carbo- nate ; solutions of normal sodium and potassium carbonates when cold have only a slight decomposing action upon it ; but when boiling, and upon repeated application, they effect at last the complete decomposition of the salt (H. KOSE). By fusion with sodium or potassium carbonate, barium sulphate is readily decom- posed. COMPOSITION. Ba .... 153 65.67 go 80 34 . 33 233 100-00 1). Artificially prepared barium carbonate presents the appear- ance of a white powder. It dissolves in 14137 parts of cold, and in 15421 parts of boiling water (Expt. No. 17). It dissolves far more readily in solutions of ammonium chloride or ammonium nitrate ; from these solutions it is, however, precipitated again, though not completely, by caustic ammonia. In water containing free carbonic acid, barium carbonate dissolves to an acid carbonate. In water con- taining ammonia and ammonium carbonate, it is nearly insoluble, one part requiring about 141000 parts (Expt. No. 18). Its solution in water has a very faint alkaline reaction. Alkali citrates and metaphosphates impede the precipitation of barium by ammonium carbonate. It is unalterable in the air, and at a red heat. When exposed to the strongest heat of a blast-furnace, it slowly yields up the whole of its carbonic acid ; this expulsion of the carbonic acid is promoted by the simultaneous action of aqueous vapor. Upon heating it to redness with charcoal, caustic baryta is formed, with evolution of carbon monoxide. * Zeitschr. f. anal. Chem. 7, 244. 72.] BASES OF GROUP II. 141 COMPOSITION. O^-R BaO . . . 153 77-67 >tJa -CO 3 .... 44 22-33 197 100-00 c. Itarium silicofiuoride forms small, hard, and colorless crys- tals, or (more generally) a crystalline powder. It dissolves in 3800 parts of cold water ; in hot water it is more readily soluble (Expt. No. 19). The presence of free hydrochloric acid increases its solu- bility considerably (Expt. No. 20). Ammonium chloride acts also in the same way (1 part silicofluoride of barium dissolves in 428 parts of saturated, and 589 parts of dilute solution of ammonium chloride. J. "W. MALLET). In common alcohol it is almost insoluble. It is unalterable in the air, and at 100 ; when ignited, it is decom- posed into silicon fluoride, which escapes, and barium fluoride, which remains. COMPOSITION. BaF a . . . 175 62-72 Ba . . . 137 49-10 SiF 4 ... 104 37-28 Si ... 28 10-04 F. . . . 114 40-86 279 100-00 279 100-00 72. 2. STRONTIUM. Strontium is weighed either as STRONTIUM SULPHATE, or as STRONTIUM CARBONATE. a. Strontium sulphate, artificially prepared, is a white powder, sometimes dense arid crystalline, sometimes loose and bulky. It dissolves in 6895 parts of cold, and 9638 parts of boiling water {Expt. No. 21). In water containing sulphuric acid, it is still more difficultly soluble, requiring from 11000 to 12000 parts (Expt. No: 22). Of cold hydrochloric acid of 8-5 per cent., it requires 474 parts ; of cold nitric acid of 4'8 per cent., 432 parts ; of cold acetic acid of 15-6 percent, of HC 2 H 3 O a , as much as 7843 parts (Expt. No. 23). It dissolves in solutions of potassium chloride and magnesium chlo- ride, in quantity which increases with the concentration, also in solu- tions of sodium chloride and calcium chloride in greatest quantity 142 FORMS. [ 72. when the solutions are of medium concentration (A. VIRCK*) ; it it is precipitated from these solutions by sulphuric acid. Meta- phosphoric acid (SCHEEBEB, RUBE), and also alkali citrates, but not free citric acid (SPILLEK), impede the precipitation of strontium by sulphuric acid. It is as good as insoluble in absolute alcohol, in common alcohol, and in a boiling solution of ammonium sulphate (1 in 4). It does not alter vegetable colors ; and remains unaltered in the air, and at a red heat. When exposed to a most intense red heat, it fuses, with loss of a small quantity of sulphuric acid (M. , DAKMSTADT f) ; all the sulphuric acid will escape on very strong ignition continued for a length of time (BOUSSINGAULT $). When ignited with charcoal, or under the influence of reducing gases, it is converted into strontium sulphide. Solutions of acid and nor- mal carbonates of potassium, sodium, and ammonium decompose strontium sulphate completely at the common temperature, even when considerable quantities of alkali sulphates are present (H. HOSE). Boiling promotes the decomposition. COMPOSITION. /O _SrO 103-5 56-40 ' U *I;M. Presence of free oxalic acid and acetic acid slightly increases the solubility of calcium oxalate. The stronger acids (hydrochloric acid, nitric acid) dissolve it readily ; from these solutions it is precipitated again unaltered, by alkalies, and also (provided the excess of acid be not too great) by alkali oxalates or acetates added in excess. Calcium oxalate does not dissolve in solutions of potassium chloride, sodium chlo- ride, ammonium chloride, barium chloride, calcium chloride, and strontium chloride, even though these solutions be hot and concen- trated ; but, on the other hand, it dissolves readily and in appreci- able quantities, in hot solutions of the salts belonging to the mag- nesium group. From these solutions it is reprecipitated by an excess of alkali oxalate (SOUCHAY and LENSSEN). Alkali citrates (SPILLER) and metaphosphates (RUBE) impede the precipitation of lime by alkali oxalates. When treated with solutions of many of the heavy metals, e.g., with solution of cupric chloride, silver nitrate, tfcc., calcium oxalate suffers decomposition, a soluble cal- cium salt being formed, and an oxalate of the heavy metal, which separates immediately, or after some time (REYNOSO). Calcium oxalate is unalterable in the air, and at 100. Dried at the latter temperature, it has invariably the following composition (Expt. No. 28, also SOUCHAY and LENSSEN *). CO-O V CaO ... 56 38-36 | X Ca -1- H,0 = C 2 3 ... 72 49-32 CO-O/ H,O ... 18 12-32 146 100-00 At 205 calcium oxalate loses its water, without undergoing decomposition ; at a somewhat higher temperature, still scarcely reaching dull redness, the anhydrous salt is decomposed, without actual separation of carbon, into carbon monoxide and calcium carbonate. The powder, which was previously of snowy whiteness, * Anal. d. Chem. und Pharm. 100, 322. 146 FORMS. [_ 74. transiently assumes a gray color in the course of this process, even though the oxalate be perfectly pure. Upon continued applica- tion of heat this gray color disappears again. If the calcium oxalate is heated in small, coherent fragments, such as are obtained upon drying the precipitated salt on a filter, the commencement and progress of the decomposition can be readily traced by this transient appearance of gray. If the process of heating be con- ducted properly, the residue will not contain a trace of calcium oxide. Hydrated calcium oxalate exposed suddenly to a dull-red heat, is decomposed with considerable separation of carbon. By ignition over the gas blowpipe calcium oxalate is converted into calcium oxide. d. Calcium oxide obtained by continued strong ignition of the oxalate or carbonate appears as a white, infusible powder, unalter- able by ignition. By standing in the air it attracts water and car- bonic acid, but not rapidly enough to interfere with accurate weighing. By treatment with a little water calcium hydroxide is formed with evolution of much heat ; on igniting again the water of hydration is readily and completely removed. Pure calcium oxide dissolves in dilute hydrochloric acid with evolution of heat, but without effervescence. Y4. 4. MAGNESIUM. Magnesium is weighed as MAGNESIUM SULPHATE, MAGNESIUM PYKOPHOSPHATE, or MAGNESIUM OXIDE. To convert it into the pyro- phosphate, it is precipitated as NORMAL AMMONIUM MAGNESIUM PHOS- PHATE. a. Anhydrous magnesium sulphate presents the appearance of a white, opaque mass. It dissolves readily in water. It is nearly altogether insoluble in absolute alcohol, but it is somewhat soluble in common alcohol. It does not alter vegetable colors. Exposed to the air it absorbs w r ater rapidly. At a moderate red heat, it remains unaltered ; but when heated to intense redness, it undergoes partial decomposition, losing part of its acid, after which it is no longer perfectly soluble in water. By means of a gas blowpipe it as tolerably easy to expel S$ 74.] BASKS OF <;iiorp n. 147 the whole of the sulphuric acid from small quantities of magne- sium sulphate (Expt. No. 30). Ignited with ammonium chloride magnesium sulphate is not decomposed. COMPOSITION. so /O M MgO .... 40 33-33 ' '<0 >M S-S0 3 .... 80 66-67 120 100-00 b. Ammonium magnesium phosphate is a white crystalline powder. It dissolves, at the common temperature, in 15293 parts of cold water (Expt. Xo. 31). In water containing ammonia, it is much more insoluble. 1000 grm. of a mixture of 3 parts water and 1 part ammonia solution, dissolved only a quantity correspond- ing to '004 grm. pyrophosphate (KISSEL*) ; the salt was consid- erably more soluble when ammonium chloride was also present ; thus, in one of KISSEL'S experiments a quantity corresponding to Oil grm. pyrophosphate w T as dissolved by 1000 grm. fluid con- taining IS grm. ammonium chloride. Presence of excess of mag- nesium sulphate diminishes the solubility in dilute ammonia, even in the presence of ammonium chloride, to such an extent that the quantity dissolved by 1000 grm. fluid cannot be estimated (KISSEL); the precipitate, under these circumstances, is liable, especially in the absence of much ammonium chloride, and when a large excess of magnesium sulphate is present, to contain some magnesium hydroxide or basic magnesium sulphate (KuBEL,f KISSEL). Sodium phosphate also diminishes (to about the same extent as magnesium sulphate) the solubility of the salt in water containing ammonium chloride and ammonia (W. HEINTZ :). It dissolves readily in acids, even in acetic acid. Its composition is expressed by the formula XII 4 MgPO 4 + 6H 2 O. 5 mol. of water escape at 100, the remain- ing water together with ammonia are expelled, at a red heat, leav- ing Mg 2 P 2 O 7 . On the application of a stronger heat the mass passes through a state of incandescence, if the salt were pure ; the weight of the residue is not affected. The incandescence may not take place at all in the presence of small quantities of calcium salts, * Zeitschr. f. anal. Chem. 8, 173. f Ib. 8, 125. \ Ib. 9, 16. 148 FOKM-S. [ 74. of other magnesium salts, or of silicic acid. It is occasioned not by the passage of the orthophosphate into the pyrophosphate, but by the passage from the crystalline to the amorphous condi- tion (O. POPP*). If ammonium magnesium phosphate is dissolved in dilute hydrochloric or nitric acid and ammonia be then added to the solution, the salt is reprecipitated completely, or more cor- rectly, only so much remains in solution as corresponds to its ordinary solubility in water containing ammonia and ammonium salt. c. Magnesium pyrophoyphcvte presents the appearance of a white mass, often slightly inclining to gray. It is barely soluble in water, but readily so in hydrochloric acid, and in nitric acid. It remains unaltered in the air, and at a red heat \. at a very intense heat it fuses unaltered. Exposed at a white heat to the action of hydrogen, Mg 3 (PO 4 ) 2 is formed, while PH 3 , P and P. 2 O 3 escape. 3(Mg 2 P 2 7 ) = 2(Mg,(P0 4 ) 1 + P.O. (STRuvEf). It leaves the color of moist turmeric-, and of reddened litmus-paper unchanged. If we dissolve it in hydrochloric or nitric acid, add water to the solu- tion, boil for some time, and then precipitate wi.h ammonia in excess, we obtain a precipitate of ammonium magnesium phosphate which, after ignition, affords less Mg 2 P 2 O 7 , than was originally employed. WEBEB J gives the loss as from 1-3 to 2'3 per cent. By long-continued fusion with mixed potassium and sodium car- bonates, magnesium pyrophosphate is completely decomposed, the pyrophosphoric acid being re-converted into orthophosphoric. If, therefore, we treat the fused mass with hydrochloric acid, and then add water and ammonia, we re-obtain on igniting the precipitate the whole quantity of the salt used. If the solution of magnesium pyrophosphate in nitric acid is evaporated to dryness a white resi- due is left ; if this is heated more strongly hyponitric acid is liber- ated, and the residue turns the color of cinnamon ; on cooling it is yellowish-white. By heating still more strongly to incipient red- ness, rapid decomposition sets in, more hyponitric acid is evolved, and pure-white magnesium pyrophosphate is left. Unless the heat is applied with care the evolution of gas may be so rapid as to carry away particles of the substance (E. LUCK). * Zeitschr. f. anal. Chem. 13, 305. | Jour. f. prakt. Chem. 79, 349. \ Pogg. Ann. 73, 146. 75.] BASES OF <;non> in. 149 p ( ) V O^ J ^_2MgO . . . So 36-04 V/ N. /~\ T~ /" v -t t *. .^^ ^ ~ L'L^ 100-00 <:/. Magnesium oxide is a white, light, loose powder. It dis- solves in 55,368 parts of cold, and in the same proportion of boil- ing water (Expt. 2so. 37). Its aqueous solution has a very slightly alkaline reaction. It dissolves in hydrochloric and in other acids, without evolution of gas. Magnesium oxide dissolves readily and in quantity, in solutions of normal ammonium salts, and also in solutions of potassium chloride and sodium chloride (Expt. No. 38) and potassium sulphate and sodium sulphate (It. WARIXGTON, Jr.) it is more soluble than in water. Exposed to the air, it slowly absorbs carbonic acid and water. Magnesium oxide is highly infusi- ble, remaining unaltered at a strong red heat, and fusing super- ficially only at the very highest temperature. < OM POSITION. Mg 24 60 O 16 40 40 100 BASIC RADICALS OF THE THIRD GROUP; T5. 1. ALUMINIUM. Aluminium is usually precipitated as HYDROXIDE, occasionally as BASIC ACETATE or BASIC FORMATE, and always weighed as ALUMINIUM OXIDE. ft. Aluminium hydroxide, recently precipitated from a solu- tion of an aluminium salt by an alkali is translucent, and when dried at 100 has the formula, A1 2 (OH) 6 . The precipitate inva- riably retains a minute proportion of the acid with which the aluminium was previously combined, as well as of the alkali which has served as the precipitant ; it is freed with difficulty from these admixtures by repeated washing. It is insoluble in pure water ; 150 FORMS. [ 75. but it readily dissolves in soda, potassa, and ethylamine (SONNEN- BCHEIN) ; it is sparingly soluble in ammonia, and insoluble in am- monium carbonate ; presence of ammonium salts greatly diminishes its solubility in ammonia (Expt. No. 39). The correctness of this statement of mine in the first edition of the present work, has been amply confirmed since by MALAGUTI and DUBOCHER ;* and also by experiments made by my former assistant, Mr. J. FUCHS. The former chemists state also that, when a solution of aluminium is precipitated with ammonium sulphide, the fluid may be filtered off five minutes after, without a trace of aluminium in it. FUCHS did not find this to be the case (Expt. No. 40). Aluminium hydroxide, recently precipitated, dissolves readily in hydrochloric or nitric acid ; but after filtration, or after having remained for some time in the fluid from which it has been precipitated, it does not dissolve in these acids without considerable difficulty, and long digestion. Aluminium hydroxide shrinks considerably on drying, and then presents the appearance of a hard, translucent, yellowish, or of a white, earthy mass. When ignited, it loses water, and this loss is frequently attended with slight decrepitation, arid invariably with considerable diminution of bulk. Aluminium hydroxide precipitated .from a solution of aluminium in potassa or soda by ammonium chloride is milk-white, denser, easier to wash, and much less soluble in ammonia than the variety above de- scribed. When dried at 100, it has the formula A1 2 O 3 + (H a O) a (J. LowEf). b. Aluminium oxide or alumina, prepared by heating the hydroxide to a moderate degree of redness, is a loose and soft mass ; but upon the application of a very intense degree of heat, it con- cretes into small, hard lumps. At the most intense white heat, it fuses to a clear glass. Ignited alumina is dissolved by dilute acids with very great difficulty ; in fuming hydrochloric acid, it dis- solves upon long-continued digestion in a warm place, slowly, but completely. It dissolves tolerably easily and quickly by first heat- ing with a mixture of 8 parts of concentrated sulphuric acid and 3 parts of water, and then adding water (A. MITSCHERLICH^). Ignition in a current of hydrogen gas leaves it unaltered. By fusion with potassium disulphate, it is rendered soluble in water. Upon igniting alumina with ammonium chloride, aluminium * Ann. de Chim. et de Phys. 3 Ser. 17, 421. f Zeitschr. f. anal. Chem. 4, 350. J Journ. f. prakt. Chem. 81, 110. 70).] BASES OF GROTP III. 151 chloride escapes ; but the process fails to effect complete volatili- zation of the alumina (H. ROSE). When alumina is fused at a very high temperature, with ten times its quantity of sodium car- bonate, sodium aluminate is formed, which is soluble in water (R. RICHTER). Placed upon moist red litmus-paper, pure alumina does not change the color to blue. t'OMFOSITK >X. A1 2 55-00 53-40 O 3 48-00 46-60 10?,. oo 100-00 c. If to the solution of a salt of aluminium, sodium carbonate or ammonium carbonate be added, till the resulting precipitate only just redissolves on stirring, and then sodium acetate or ammonium acetate poured in in abundance and the mixture boiled some time, the aluminium is precipitated almost completely as basic acetate in the form of translucent nocks, so that if the filtrate be boiled with ammonium chloride and ammonia, only unweighable traces of aluminium hydroxide separate. If the quantity of sodium acetate employed be too small, the precipitate appears more granular, the filtrate would then contain a larger amount of aluminium. The precipitate cannot be very conveniently filtered and washed. In washing it is best to use boiling water, containing a little sodium acetate or ammonium acetate. The precipitate is readily soluble in hydrochloric acid. d. If, instead of the acetates mentioned in . Manganous hydroxide recently thrown down forms a white, flocculent precipitate, barely soluble in water and alkalies, but soluble in ammonium chloride ; it immediately absorbs oxygen from the air, and turns brown, owing to the formation of hydrated protosesquioxide. On drying it in the air, a brown pow r der is obtained which, when heated to intense redness, with free access of air, is converted into protosesquioxide, and on ignition with sulphur, in a stream of hydrogen, is converted into sulphide. c. Protosesquioxide of manganese^ artificially produced, is a brown powder. All the oxides of manganese are finally converted into this by strong ignition in the air. Each time it is heated it assumes a darker color, but its weight remains unaltered. It is insoluble in water, and does not alter vegetable colors. If ignited with ammonium chloride, it is converted into the manganous chloride. When heated with concentrated hydrochloric acid, it dissolves to chloride with evolution of chlorine (Mn 3 O 4 -|- 8IIC1 3MnCl 2 + 2C1 -f- 4H 2 O). On ignition with sulphur in a stream of hydrogen it is converted into sulphide (H. ROSE). On ignition in oxygen it is converted into manganic oxide (SCHNEIDER). On ignition in hydrogen it is converted into manganous oxide. COMPOSITION. Mn 3 .... 165-00 72-05 O 4 64-00 27-95 229-00 100-00 d. Manganese dioxide is occasionally produced in analysis by exposing a concentrated solution of manganous nitrate to a gradually increased temperature. At 140 brown flakes separate, at 155 much nitrous acid is disengaged, and the whole of the manganese separates as anhydrous dioxide. It is brownish-black, and is deposited on the sides of the vessel, with metallic lustre. It is insoluble in weak nitric acid, but dissolves to a small amount in 78.] BASES OF GROUP IV. IT)? hot and concentrated nitric acid (DEVILLE). In hydrochloric acid it dissolves with evolution of chlorine, in concentrated sulphuric acid with liberation of oxygen. The dioxide is also sometimes obtained in the hydrated condition in analytical separations, thus when we precipitate a solution of a mangaiious salt with sodium hypochlorite, or, after addition of sodium acetate, with bromine or chlorine in the heat. The brownish-black flocculent precipitate thus obtained, contains alkali, from whicli it cannot be well freed by washing. ' e. Manganese sulphide, prepared in the wet way, generally forms a flesh-colored precipitate. I must make a few remarks with reference to its precipitation.* This is effected but incom- pletely if we add to a pure manganous solution only ammonium sulphide, no matter whether it be colorless or yellow, while it is perfectly effected if ammonium chloride be used in addition. A large quantity even of ammonium chloride does not impede the precipitation. Ammonia in small quantity is not injurious, but in large quantity it interferes with complete precipitation, especially in the presence of ammonium polysulphide (A. CLASSEN-)-). In all cases we must allow to stand at least 24 hours, and with very dilute solutions 48 hours, before filtering. Colorless or slightly yellow ammonium sulphide is the most appropriate precipitant. In the presence of ammonium chloride even a large excess of ammonium sulphide is uninjurious. If the precipitation is con- ducted as directed, the manganese can be precipitated from solu- tions which contain an amount equivalent to only ^^Wo ^ tne manganous oxide. If the flesh-colored hydrated sulphide remains some time under the fluid, from which it was precipitated, it sometimes becomes converted into the green anhydrous sulphide.:): This conversion is more likely to take place when a large excess of ammonium sulphide has been used; heating favors it, ammonium chloride hinders it. The conversion is occasionally rapid. The green sulphide thus obtained consists of eight-sided tables dis- tinctly visible under the microscope (F. MUCK). In acMs (hydro- chloric, sulphuric, acetic, (fee.) the hydrated sulphide dissolves with evolution of hydrogen sulphide. If the precipitate, while still moist, is exposed to the air, or washed with water impregnated with air, it changes to brown, hydrated protosesquioxide of manganese * Journ. f. prakt. Chem. 82, 265. f Zeitschr. f. anal. Chem. 8, 370. \ Journ. f. prakt. Chem. 82, 268. ? Zeitschr. f. Chem. N. F. 6, 6. 158 FORMS. [ 78. being formed, together with a small portion of manganous sulphate. Hence in washing the hydrate we always add some ammonium sul- phide to the wash-water, and keep the filter as full as possible with the same. We guard against the filtrate running through turbid, by adding gradually decreasing quantities of ammonium chloride to the wash-water (at last none). (Expt. No. 44.) On igniting the precipitate mixed with sulphur in a stream of hydrogen the anhydrous sulphide remains. If we have gently ignited during this process, the product is ' light green ; if we have strongly ignited, it is dark green to black. Neither the green nor the black sulphide attracts oxygen or water quickly from the air (H. ROSE). The anhydrous sulphide is also readily soluble in dilute acids. COMPOSITION. Mn .... 55-00 63-22 S 32-00 36-78 87-00 100-00 f. Anhydrous manganous sulphate, produced by exposing the crystallized salt to the action of heat, is a white, friable mass, readily soluble in water. It resists a very faint red heat ; but upon exposure to a more intense red heat, it suffers more or less complete decomposition oxygen, sulphur dioxide, and sulphur trioxide being evolved, and protosesquioxide of manganese re- maining behind. Ignited with sulphur in a stream of hydrogen it is transformed into sulphide (H. ROSE). COMPOSITION. ^O ^^ Mn Mn ' 71 ' 47 ' 2 >u ' < O ' SO, , . . 80 ' 00 52 ' 98 151-00 100-00 g. Ammonium manganese phosphate. GIBBS* says that this precipitate is insoluble in boiling water, but I have not found this to be the case. My results are that 1 part dissolves in 32092 parts of cold water, in 20122 parts boiling water, and 17755 parts of water containing -^ of ammonium chloride. It has the formula * SILLIM. Amer. Journ. (ii.) 44, 216. , ~i) I BASES OF GROUP IV. 159 7S T II 4 MnPO 4 + II.,O. It presents pale pink scales of pearly lustre, which sometimes turn reddish on the filter. On ignition it is converted into manganese pyrophosphate. //. Mdnganese pyro/phosphdie is the white residue left on the ignition of the preceding. COMPOSITION. / PO< 0> Mn _2MnO .142 50 ^POMn~ P <> _^ 284 100 T9. 3. NICKEL. Xickel is precipitated as HYDROXIDE, and as SULPHIDE. It is weighed in the form of NICKELOUS OXIDE, of METALLIC NICKEL, or of anhydrous NICKELOUS SULPHATE. a. Nickelous hydroxide forms an apple-green precipitate, almost absolutely insoluble in water. When precipitated from a solution of the chloride or sulphate, it retains some of the acid even after long washing (TEICHMANN*). It is also very difficult to remove the last traces of alkali. It dissolves with some difficulty in ammonia and ammonium carbonate, far more readily in the presence of an ammonium salt. From these solutions it is com- pletely precipitated by excess of potassa or soda ; application of heat promotes the precipitation. It is unalterable in the air ; on ignition, it passes into nickelous oxide. b. Niehelous oxide is a dirty grayish-green powder. When obtained by heating the nitrate to redness, it always contains some nickelic oxide, and requires very strong and protracted ignition for conversion into the pure green nickelous oxide (W. J. EUSSELL). It is insoluble in water, but readily soluble in hydrochloric acid. It does not affect vegetable colors. It suffers no variation of weight upon ignition with free access of air. Mixed with am- monium chloride and ignited, it is reduced to metallic nickel (II. "ROSE); it is also easily reduced by ignition in hydrogen or carbon monoxide. * Aunal. d. Chera. u. Pliarm. 156, 17. 160 FORMS. [ '/. COMPOSITION. M .... 59 78- 6T O 16 21-33 75 100-00 c. Metallic nickel obtained by the reduction of nickelous oxide with hydrogen has the form of a gray powder, or if the^ heat has been very strong, and it has melted, it is lustrous and white like silver. It is unaltered in weight by ignition in hydrogen, when ignited in the air it is superficially oxidized. It is attracted by the magnet. It is dissolved slowly by hydrochloric acid and dilute .sulphuric acid, and readily by moderately strong nitric acid. d. Anhydrous nickelous sulphate obtained by evaporating a solution of the chloride, nitrate, &c., with sulphuric acid is yellow, soluble in water to a green fluid. The hydrous salt may be rendered anhydrous without loss of acid by cautious heating in a platinum dish, but at low redness it begins to blacken at the edges and loses acid (F. GAIT HE*). e. Hydrated nickelous sulphide, prepared in the wet way, forms a black precipitate, insoluble in water. I must make some observations on its precipitation. f In order to precitate the nickel from a pure solution completely and with ease, ammonium chloride must be present ; it is not enough to add ammonium sulphide alone. A large quantity even of ammonium chloride produces no injurious effect. In the presence of free ammonia, on the con- trary, some nickel remains in solution. In this case, the super- natant fluid appears brown. As precipitant, colorless or ligl it- yellow ammonium sulphide containing no free ammonia should be used, a large excess must be avoided. If the directions given are adhered to allowing to stand 48 hours the nickel may be pre- cipitated by means of ammonium sulphide, from solutions con- taining only 8~o-o^o-o ^ ^ e ox ide. ^ s tne precipitate is liable to take up oxygen from the air, being transformed into sulphate, a little ammonium sulphide is mixed with the wash-water, to which also it is advisable to add ammonium chloride (less and less at last none) ; the filter should be kept full' (Expt. 'No. 45). Brown filtrates, containing nickel sulphide in solution, may be freed from the latter by acidulation with acetic acid, and boiling some time. * Zeitschr. f. anal. Chem. 4, 190. f Journ. f. prakt. Chem. 82, 257. 80.] BASES OF GROl'P IV. 161 The sulphide falls down, and may now be filtered off. It is very sparingly soluble in concentrated acetic acid, somewhat more soluble in hydrochloric acid. It is more readily soluble still in nitric acid, but its best solvent is nitro-hydrochloric acid. It loses its water upon the application of a red heat ; when ignited in the air, it is trans- formed into a basic compound of nickelous oxide with sulphuric acid. Mixed with sulphur and ignited in a stream of hydrogen, a fused mass remains, of pale yellow color and metallic lustre. This consists of Xi 2 S, but its composition is not perfectly constant (F. GAUHE*). [Xickel may be precipitated as a sulphide, dense in form, easy to wash, and not readily oxidizing by contact with air, by proceed- ing as follows : To the solution, which should be concentrated and contain a liberal quantity of ammonium salts, add ammonia (if necessary) to alkaline reaction, then acetic acid to slight acid reac- tion, also ammonium or sodium acetate, and heat, to bolting. Transmit H,S gas through the boiling solution. Since much free acetic acid prevents complete precipitation, it is necessary some- times when much nickel is present to partially neutralize once or twice the acid set free during the process.] Xickel sulphide may be converted into nickelous sulphate bv dissolving in nitric acid and evaporating with sulphuric acid. 80. 4. COBALT. Cobalt is weighed in the PURE METALLIC state, or as COBALTOUS SULPHATE. Besides the properties of these substances, we have to study also those of COBALTOUS HYDROXIDE, of the SULPHIDE, and of the TRIPOTASSIUM COBALTIC NITRITE. a. Cobaltous hydroxide. Upon precipitating a solution of a cobaltous salt with potassa, a blue precipitate (a basic salt) is formed at first, which, upon boiling with potassa in excess, exclud- ed from contact of air. changes to light red cobaltous hydroxide ; if, on the contrary, this process is conducted with free access of air. the precipitate becomes discolored, and finally black, part of the cobaltous hydroxide being converted into cobaltic hydroxide. But the hydroxide prepared in this way, retains always a certain quantity of the acid, and, even after the most thorough washing Zeitschr. f. anal. Chem. 4, 191. 162 FORMS. [ 80. with hot water, also a small amount of the alkaline precipitant. .The latter, however, is not enough to spoil the accuracy of the results (H. ROSE, F. GATJIIE*). Cobaltous hydroxide is insoluble in water, and also in dilute potassa ; it is somewhat soluble in very concentrated potassa, and readily in ammonium salts. When dried in the air, it absorbs oxygen, and acquires a brownish color. By strong ignition it is converted into cobaltous oxide (even if some higher oxide had formed from boiling or drying in the air) ; if cooled with exclusion of air, as in a current of carbon dioxide, pure light.brown cobaltous oxide will be left ; if cooled, on the contrary, with access of air, it is more or less changed to black protosesquioxide (cobaltoso-cobaltic oxide) (W. J. RUSSELL!). By ignition in a current of hydrogen, metallic cobalt is left, from which any traces of alkali may now be almost completely removed by boiling water. I. The metallic cobalt obtained according to a, or by igniting the chloride or the protosesquioxide (produced by igniting the nitrate) in hydrogen is a grayish-black powder, which is attracted by the magnet, and is more difficultly fusible than gold. If the reduction has been effected at a faint heat, the finely divided metal burns in the air to protosesquioxide of cobalt, which is not the case if the reduction has been effected at an intense heat. Cobalt does not decompose water, either at the common temperature, or upon ebullition except sulphuric acid be present, in which case decomposition will ensue. Heated with concentrated sul- phuric acid, it forms cobaltous sulphate, with evolution of sulphur dioxide. In nitric acid it dissolves readily to cobaltous nitrate. c. Cobalt sulphide, produced in the wet way, forms a black precipitate, insoluble in water, alkalies, and alkali sulphides. With regard to its precipitation, this is effected but slowly and im- perfectly by ammonium sulphide alone ; in the presence of am- monium chloride however, it takes place quickly and completely. Free ammonia is not injurious ; it is all one, whether colorless or yellow ammonium sulphide is employed. If the directions given are observed, cobalt may be precipitated from a solution contain- ing no more than innAnnr f *he protoxide. In the moist con- dition, exposed to the air, it oxidizes to sulphate. In washing it, therefore, water containing ammonium sulphide is employed, and * Zeitschr. f. anal. Chem. 4, 54. f Journ. Chem. Soc. (2) 1, 51. \ Journ. f. prakt. Chera. 82, 262. BASES OF GROUP IV. 163 the filter is kept full. It is advisable also to mix a little ammo- nium chloride with the wash-water, but its quantity should be gradually decreased, and the last water used must contain none. It is but sparingly soluble in acetic acid and in dilute mineral acids, more readily in concentrated mineral acids, and most readily in warm nitro-hydrochloric acid. Mixed with sulphur and ignited in a stream of hydrogen, we obtain a product which varies in composition according to the temperature employed. The residue is therefore not suited for the determination of cobalt (H. ROSE). Cobalt can be precipitated as sulphide completely in the presence of a very small amount of free acetic acid by hydrogen sulphide in the same manner as nickel (see 79, e). Cobalt sulphide may be converted into cobaltous sulphate by heating in the air, moistening with nitric acid, evaporating with sulphuric acid and igniting. d. CqbciUous sulphate crystallizes, in combination with 7 aq., slowly in oblique rhombic prisms of a fine red color. The crystals yield the whole of the water, at a moderate heat, and are con- verted into a rose-colored anhydrous salt, which bears the applica- tion of a low red heat without losing acid. At a stronger heat the edges become black and some sulphuric acid escapes (F. GAUHE*). It dissolves rather difficultly in cold, but more readily in hot water. COMPOSITION. O ^ CoO . . .75 48-39 * < O - ~S0 3 80 51-61 155 100-00 e. Tripotassiv.m cobaltie nitrite. If a solution of a cobalt salt (not too dilute) is mixed with excess of potassa and then with acetic acid till the precipitate is redissolved, and a concentrated solution of potassium nitrite previously acidified with acetic acid is added, first a dirty, brownish precipitate forms which gradually turns yellow and crystalline, especially on the application of a gentle heat (X. ~W. FISCHER!). The composition of this precipi- tate corresponds to the formula (KNO 2 ) 6 Co 3 (!N"O 2 ) 6 + aq. x (SADT- LER). Dried at 100 its composition is somewhat variable (STKO- MEYER, EnmiAxx;}:). It is decidedly soluble in water, less in potassium acetate whether neutral or acidified with acetic acid, * Zeitschr. f. anal. Chem. 4, 55. fPogg. Ann. 72, 477. \ Journ. f. prakt. Chem. 97, 385. 164 FORMS. [ 81. not in potassium acetate to which some potassium nitrite has been added, not in potassium nitrite, nor in alcohol of 80 per cent. On washing with water or solution of potassium acetate, unless potassium nitrite is added, nitric oxide is constantly evolved in small quantities. It is decomposed with separation of brown cobaltic hydroxide, with difficulty by solution of potassa, with ease by soda or baryta. On being moistened with sulphuric acid and ignited (finally with addition' of ammonium carbonate) it leaves 2(CoSO 4 ) + 3(K 2 SO 4 ), but there is a difficulty in driving off all the excess of acid without decomposing the cobaltous sulphate. The yellow salt is soluble in hydrochloric acid, potassa precipitates the whole of the cobalt from this solution as hydroxide. 81. 5. FERROUS IRON ; and 6. FERRIC IRON. Iron is ifsually weighed in the form of FERRIC OXIDE, occasion- ally as SULPHIDE. We have to study also the FERRIC HYDROXIDE, the FERRIC SUCCINATE, the FERRIC ACETATE, and the FERRIC FORMATE. a. Ferric hydroxide, recently prepared, is a reddish-brown precipitate, insoluble in water, in dilute alkalies, and in ammonium salts, but readily soluble in acids ; it shrinks very greatly on drying. When dry, it presents a brown, hard mass, with shining conchoidal fracture. If the precipitant alkali is not used in excess, the precipitate contains basic salt ; on the other hand, if the alkali has been used in excess, a portion of it is invariably carried down in combination with the ferric hydroxide, on which account ammonia alone can properly be used in analysis for this purpose. Under certain circumstances, for instance, by protracted heating of a solution of ferric acetate on the water-bath (which turns the solution from blood-red to brick-red, and makes it appear turbid by reflected light), and subsequent addition of some sulphuric acid or salt of an alkali, a reddish-brown hydrated ferric oxide is pro- duced, which is insoluble in cold acids, even though concentrated, and is not attacked even by boiling nitric acid (L. PEAN DE ST. GILLES*). Closely allied to ferric hydroxide are the highly basic salts obtained by mixing dilute cold solutions of ferric salts, best ferric chloride, with much ammonium chloride, cautiously adding am- * Journ. f. prakt. Chem. 66, 137. g 81.] BASKS OF GROUP IV. 165 monimn carbonate till the fluid on standing in the cold instead of becoming clear turns more turbid if anything, and then boiling. The precipitates, thus produced in the fluid which still retains its acid reaction, contain the whole of the iron present and play an important part in analytical separations. They should be washed with boiling water containing ammonium chloride, being soluble to a slight extent in pure water. They are not suitable for ignition, as ferric chloride might occasionally escape from them. I. Ferric hydroxide is, upon ignition, converted into ferric o.i'ide. If the hydroxide has been superficially dried only, the violent escape of steam from the lumps is likely to occasion loss ; but if it has been dried as much as possible by suction and still remains moist, it may be ignited without fear of loss. Pure ferric oxide, when placed upon moist reddened litmus-paper, does not change the color to blue. It dissolves slowly in dilute, but more rapidly in concentrated hydrochloric acid ; the application of a moderate degree of heat effects this solution more readily than boiling. With a mixture of 8 parts concentrated sulphuric acid and 3 parts water, it behaves in the same manner as alumina. The weight of ferric oxide does not vary upon ignition in the air; when ignited with ammonium chloride, ferric chloride escapes. Ignition with charcoal, in a closed vessel, reduces it more or less. Strongly ignited with sulphur in a stream of hydrogen, it is trans- formed into ferrous sulphide. COMPOSITION. Fe a 112 70-00 O 3 48 30-00 160 100. on c. Ferrous sulphide, produced in the wet way, forms a black precipitate. The following facts are to be noticed with regard to its precipitation.-)- Ammonium sulphide used alone, whether colorless or yellow, precipitates pure neutral solutions of ferrous salts, but slowly and imperfectly. Ammonium chloride acts very favorably ; a large excess even is not attended with inconvenience. Ammonia has no injurious action. It is all the same whether the ammonium sulphide be colorless or light yellow. If the direc- ., 82, 268. 166 FORMS. [ 81. tions given are observed, iron may be precipitated by means of ammonium sulphide, from solutions containing only TF ^ ^-5-5- of ferrous oxide. In such a case, however, it is necessary to allow to stand forty-eight hours. Since the precipitate rapidly oxidizes in contact with air, ammonium sulphide is to be added to the wash- water, and the filter kept full. It is well also to mix a little ammonium chloride with the wash-water, but the quantity should be continually reduced, and the last water used should contain none. In mineral acids, even when very dilute, the hydrated sulphide dissolves readily. Mixed with sulphur, and strongly ignited in a stream of hydrogen, anhydrous ferrous sulphide re- mains (H. HOSE). COMPOSITION. Fe 56 63-64 S 32 36-36 88 100-00 d. When a neutral solution of a ferric salt is mixed with a neutral solution of an alkali succinate, a cinnamon-colored precipi- tate of a brighter or darker tint of a basic ferric succinate is formed, succinic acid being set free. The free succinic acid does not exercise any perceptible solvent action upon the precipitate in a cold and highly dilute solution, but it redissolves the precipitate a little more readily in a warm solution. The precipitate must therefore be filtered cold, if we want to guard against re-solution. Formerly the precipitate was erroneously supposed to consist of a normal salt, decomposable by hot water into an insoluble basic and a soluble acid compound. Basic ferric succinate is insoluble in cold, and but sparingly soluble in hot water. It dissolves readily in mineral acids. Ammonia, especially if w^arm, deprives it of the greater portion of its acid, leaving compounds which are highly basic ferric succiiiates (DOPPING). e. If to a solution of a ferric salt, sodium carbonate be added in the cold, till the fluid contains no more free acid, and in consequence of the formation of basic salt has become deep red, but remains still perfectly clear, and then sodium acetate be poured in and the mixture boiled, the whole of the iron will be precipi- tated as basic ferric acetate. f. Instead of the sodium or ammonium acetate used in n. 00 d. Lead sulphate is a heavy white powder. It dissolves, at the common temperature, in 22800 parts of pure water (Expt. Xo. 49*) ; it is less soluble in water containing sulphuric acid (1 part requiring 36500 parts Expt. Xo. 50) ; it is far more readily solu- ble in water containing ammonium salts ; from this solution it may be precipitated again by adding sulphuric acid in excess (Expt. Xo. 51). It is almost entirely insoluble in common alcohol. Of the ammonium salts, the nitrate, acetate, and tartrate are more espe- cially suited to serve as solvents for lead sulphate : the two latter salts are made strongly alkaline by addition of ammonia, previous to use (WACKENRODER). Lead sulphate dissolves in concentrated hydrochloric acid, upon heating. In nitric acid it dissolves the more readily, the more concentrated and hotter the acid ; water fails to precipitate it from its solution in nitric acid ; but the addi- tion of a copious amount of dilute sulphuric acid causes its precipi- * According to G. F. RODWELL 1 part dissolves in 31696 parts water at 15 (Chem. News, 1866, 50). 172 FORMS. [ 83. tation from this solution. The more nitric acid the solution con- tains, the more sulphuric acid is required. It dissolves sparingly in concentrated sulphuric acid, and the dissolved portion precipi- tates again upon diluting with water (more completely upon addi- tion of alcohol). A moderately concentrated solution of sodium thiosulphate dissolves lead sulphate completely even if cold, more readily if warmed. On boiling, the solution becomes black, from separation of a small quantity of lead sulphide (J. LOWE*). The solutions of alkali carbonates and alkali hydrogen carbonates con- vert lead sulphate, even at the common temperature, completely into lead carbonate. The solutions of the normal alkali carbonates, but not those of the alkali hydrogen carbonates, dissolve some lead oxide in this process (H. RosEf). Lead sulphate dissolves readily in hot solutions of potassa or soda. It is unalterable in the air, and at a gentle red heat ; when exposed to a full red heat, it fuses with- out decomposition (Expt. No. 52), provided always reducing gases be completely excluded for, if this is not the case, the weight will continually diminish, owing to reduction to sulphide (EKDMANN^:). At a white heat the whole of the sulphuric acid gradually escapes (BoussiNGAuivr ). When it is ignited with charcoal, lead sulphide is formed at first ; if the heat be raised, this sulphide reacts on undecomposed sulphate, metallic lead and sulphur dioxide being produced. Fusion with potassium cyanide reduces the whole of the lead to the metallic state. Lead sulphate mixed with sulphur and exposed to intense ignition in a current of hydrogen yields the sulphide, but loss can scarcely be avoided (compare f). COMPOSITION. PbO . . . . 223 73.60 SO.. 80 26-40 303 100-00 e. Lead chloride obtained by precipitation is a white crystalline powder. It separates in needles from a hot solution containing a certain quantity of hydrochloric acid; occasionally it presents wedge-shaped crystals, or when separated from a strong hydro- chloric solution, hexagonal tables. At 1Y'7 water dissolves '946 * Journ. f . prakt. Chem, 74, 348. f Pogg. Annal. 95, 426. \ Journ. f. prakt. Chem. 62, 381. Zeitschr. f. anal. Chem. 7, 244. 83.] BASES OF GROUP V. per cent.; a fluid containing 15 per cent, of hydrochloric acid of 1-162 sp. gr. dissolves -090 ; a fluid containing 20 per cent, acid dissolves '111 per cent.; a fluid containing 80 per cent, acid dis- solves 1-498 per cent. Pure hydrochloric acid of the above strength dissolves 2'900 per cent. (J. CARTER BELL*). Lead chloride is less soluble in water containing nitric acid than in water (1 part requires 1636 parts, BISCHOF). It is extremely sparingly soluble in alcohol of TO to 80 per cent,, and altogether insoluble in absolute alcohol. It is unalterable in the air.- It fuses at a temperature below red heat, without loss of weight. "When exposed to a higher temperature, with access of air, it volatilizes slowly, being partially decomposed : chlorine gas escapes, and a mixture of lead oxide and chloride remains. COMPOSITION. Pb 207-00 74-48 01, 70-92 25-52 277-92 100-00 f. Lead sulphide, prepared in the wet way, is a black precipi- tate, insoluble in water, dilute acids, alkalies, and alkali sulphides. In precipitating it from a solution containing free hydrochloric acid, it is necessary to dilute plentifully, otherwise the precipitation will be incomplete. Eveii if a fluid only contain 2*5 per cent. HC1, the whole of the lead will not be precipitated (M. MARTIN f). It is unalterable in the air; it cannot be dried at 100 without -decomposition. According to H. ROSE it increases perceptibly in weight by oxidation ; in the case of long-protracted drying even becoming a few per-cents heavier. I have confirmed his state- ment (see Expt. X>. :>3 1. If lead sulphide mixed with sulphur is heated gently in a current of hydrogen, so that the lower quarter of the crucible is red hot, lead sulphide is left without loss of weight. By continuing a gentle heat the weight gradually dimin- ishes; by strong ignition the loss is rapid. This loss is partly owing to volatilization of lead sulphide, but mainly to escape of sulphur in the form of hydrogen sulphide and formation of Pb 2 S, or even of lead (A. SOUOHAY). It dissolves in concentrated hot * Jour. Chem. Soc. (2) 6, 355. t Journ. f. prakt. Chem. 67, 374. \ Pogg. Annal. 91, 110; and 110, 134. Zeitschr. f. anal. Chem. 4, 63. 174 FORMS. [ 84. hydrochloric acid, with evolution of hydrogen sulphide. In mod- erately strong nitric acid lead sulphide dissolves, upon the applica- tion of heat, with separation of sulphur ; if the acid is rather con- centrated, a small portion of lead sulphate is also formed. Fuming nitric acid acts energetically upon lead sulphide, and converts it into sulphate without separation of sulphur. COMPOSITION. Pb ........ 207 86-61 S . 32 13-39 239 100-00 g. For the composition and properties of lead chromate, see Chromic acid, 93. 84. 3. MERCURY IN MERCUROUS COMPOUNDS ; and 4. MERCURY IN MERCURIC COMPOUNDS. Mercury is weighed either in the METALLIC STATE, as MERCUROUS CHLORIDE, or as SULPHIDE, or occasionally as MERCURIC OXIDE. a. Metallic mercury is liquid at the common temperature ; it has a tin-white color. When pure, it presents a perfectly bright surface. It is quite unalterable in the air at the common tempera- ture. It boils at 360. It evaporates, but very slowly, at the ordinary temperature of summer. Upon ]ong-continued boiling with water, a small portion of mercury volatilizes, and traces escape along with the aqueous vapor, whilst a very minute proportion remains suspended (not dissolved) in the water (comp. Expt. 'No. 54). This suspended portion of mercury subsides completely after long standing. When mercury is precipitated from a fluid, in a very minutely divided state, the small globules will readily unite to a large one if the mercury be perfectly pure ; but even the slightest trace of extraneous matter, such as fat, etc., adhering to the mercury will prevent the union of the globules. Mercury does not dissolve in hydrochloric acid, even in concentrated ; it is barely soluble in dilute cold sulphuric acid, but dissolves readily in nitric acid. h. Mercurous chloride, prepared in the wet way, is a heavy 84.] BASES OF GROUP V. 175 white powder. It is almost absolutely insoluble in cold water ; in boiling water it is gradually decomposed, the water taking up chlorine and mercury ; upon continued boiling, the residue acquires a gray color. Highly dilute hydrochloric acid fails to dissolve it at the common temperature, but dissolves it slowly at a higher temperature ; upon ebullition, with access of air, the whole of the mercurous chloride is gradually dissolved ; the solution contains mer- curic chloride (Hg 2 Cl 2 + 2HC1 + O-=2HgCl a + H 2 O). When acted upon by boiling concentrated hydrochloric acid, it is rather speedily decomposed into mercury, which remains undissolved, and mer- curic chloride, which dissolves. Boiling nitric acid dissolves it to mercuric chloride and nitrate. Chlorine water and nitrohydrochlo- ric acid dissolve it to mercuric chloride, even in the cold. Solutions of ammonium chloride, sodium chloride, and potassium chloride, decompose it into metallic mercury and mercuric chloride, which latter dissolves ; in the cold, this decomposition is but slight ; heat promotes the action. It is soluble in hot solution of mercurous nitrate, and still more in that of mercuric nitrate ; on cooling it crystallizes out almost completely (DEBRAY*). It does not affect vegetable colors ; it is unalterable in the air, and may be dried at 100, without loss of weight ; when exposed to a higher degree of heat, though still below redness, it volatilizes completely, without previous fusion. COMPOSITION. Hg 2 400-00 84-94 Cl, 70-92 15-06 470-92 100-00 c. Mercuric sulphide, prepared in the wet way, is a black pow- der, insoluble in water. Dilute hydrochloric acid and dilute nitric acid fail to dissolve it, hot concentrated nitric acid scarcely attacks it, boiling hydrochloric acid has no action on it. By prolonged heating with red fuming nitric acid it is finally converted into a white compound, 2HgS + Hg(NO 3 ) 2 , which is insoluble, or barely soluble, in nitric acid. It dissolves readily in nitrohydrochloric acid. From a solution of mercuric chloride containing much free hydrochloric acid, the whole of the metal cannot be precipitated as * Compt. Rend. 70, 995. 176 FORMS. [ 84. sulphide by means of hydrogen sulphide, until the solution is prop- erly diluted. Should such a solution be very concentrated, mer- curous chloride and sulphur are precipitated (M. MARTIN*). Solu- tion of potassa, even boiling, fails to dissolve it. It dissolves in potassium sulphide, but readily only in presence of free alkali. It is insoluble in potassium hydrosulphide and in the corresponding -sodium compound, and is therefore precipitated from its solution in potassium or sodium sulphide by hydrogen sulphide or by ammonium hydrosulphide (C. BARFOEDf). Small but distinctly perceptible traces dissolve on cold digestion with yellowish or yel-~ low ammonium sulphide, but after hot digestion- it is scarcely possi- ble to detect any traces in solution.;}: Potassium cyanide and sodium sulphite do not dissolve it. On account of the solubility of mer- curic sulphide in potassium sulphide, it is impossible to precipitate mercury by means of ammonium sulphide completely from solutions containing potassium or sodium hydroxides or carbonates. Such solutions may occur, for instance, when a solution of mercuric chloride contains much potassium chloride, or sodium chloride, for, in this case, no mercuric oxide would be precipitated on the addi- tion of potassa or soda (H. ROSE). In the air it is unalterable, even in the moist state, and at 100. When exposed -to a higher temperature, it sublimes completely and unaltered. COMPOSITION. Hg 200 86-21 S 32 13-79 232 100-00 d. Mercuric oxide, prepared in the dry way, is a crystalline brick-colored powder, which, when exposed to the action of heat, changes to the color of cinnabar, and subsequently to a violet-black tint. It bears a tolerably strong heat without decomposition ; but when heated to incipient redness, it is decomposed into mercury and oxygen ; perfectly pure mercuric oxide leaves no residue upon ignition. Its escaping fumes also should not redden litmus-paper. Water takes up a trace of mercuric oxide, acquiring thereby a very weak alkaline reaction. Hydrochloric or nitric acid dissolves it readily. * Journ. f. prakt. Chem. 67, 376- f Zeitschr. f. anal. Chem. 4, 436. \ Ib. 3, 140. Pogg. Annal. 110, 141. 85.] BASES OF GROUP V. 177 COMPOSITION. Hg 200 92-59 O 16 7-41 216 100-00 ' 85. 5. COPPER. Copper is usually weighed in the METALLIC STATE, or in the form of CUPRIC OXIDE, or of CUPROUS SULPHIDE. Besides these forms, we have to examine CUPRIC SULPHIDE, CUPROUS OXIDE, and CUPROUS SULPHOCYANATE. a. Copper, in the pure state, is a metal of a peculiar well- known color. It fuses only at a white heat. Exposure to dry air, or to moist air, free from carbon dioxide, leaves the fused metal unaltered; but upon exposure to moist air impregnated with carbon dioxide, it becomes gradually tarnished and coated with a film, first of a blackish-gray, finally of a bluish-green color. Pre- cipitated finely divided copper, in contact with water and air, oxidizes far more quickly, especially at an elevated temperature. On igniting copper in the air, it oxidizes superficially to a varying mixture of cuprous and cupric oxide. In hydrochloric acid,- in the cold, it does not dissolve if air be excluded ; in the heat it dissolves but slightly if the metal is in a compact state. Finely divided copper on the contrary dissolves slowly when heated with strong hydrochloric acid, hydrogen being evolved and cuprous chloride being formed (WELTZIEN*). Copper dissolves readily in nitric acid. In ammonia it dissolves slowly if free access is given to the air ; but it remains insoluble if the air is excluded. Metallic copper brought into contact in a closed vessel with solution of cupric chloride in hydrochloric acid, reduces the cupric to cuprous chloride, an atom of metal being dissolved for every molecule of chloride. b. Cupric oxide. If a dilute, cold, aqueous solution of a cupric salt is mixed with solution of potassa or soda in excess, a light blue precipitate of cupric hydroxide, Cu(OH),, is formed, which it is found difficult to wash. If the precipitate be left in the fluid *Ann. d. Cbem. u. Pharm. 136, 109. 178 FORMS. [ 85. from which it has been precipitated, it will, even at a summer heat, gradually change to brownish-black, passing, with separation of water, into 6CuO -f- H 2 O (SOUCHAY). This transformation is immediate upon heating the fluid nearly to boiling. The fluid filtered off from the black precipitate is free from copper. It follows from this that the black precipitate is insoluble in dilute potassa. Concentrated potassa or soda on the contrary dissolves the hydroxide, and on long warming even the black oxide (O. Low*). The resulting blue solutions remain clear on boiling, even if mixed with some water ; but if boiled after being much diluted the whole of the copper will separate as black oxide. If a solution of a cupric salt contains non-volatile organic substances, the addition of alkali in excess will, even upon boiling, fail to precipitate the whole of the copper. The hydrated cupric oxide, 6CuO -f- H 2 O, precipitated with potassa or soda from hot dilute solutions obsti- nately retains a portion of the precipitant ; it may, however, be completely freed from this by washing with boiling water. The precipitated oxide after ignition, or the oxide prepared by decom- posing cupric carbonate or nitrate by heat, is a brownish-black, or black powder, the weight of which remains unaltered even upon strong ignition over the gas- or spirit-lamp, provided all reducing gases be excluded (Expt. No. 56). If cupric oxide is exposed to a heat approaching the fusing point of metallic copper, it fuses, yields oxygen, and becomes Cu 5 O 3 (FAVRE and MAUMENE). It is very readily reduced by ignition with charcoal, or under the in- fluence of reducing gases ; heated in the air for a long time, the reduced metallic copper re-oxidizes. Mixed with sulphur and ignited in a current of hydrogen, towards the end strongly, cupric oxide passes into cuprous sulphide (Cu 2 S H. ROSE). Cupric oxide, in contact with the atmosphere, absorbs water ; less rapidly after being strongly ignited (Expt. No. 57). It is nearly insoluble in water; but it dissolves readily in hydrochloric acid, nitric acid, &c.; less readily in ammonia, It does not affect vegetable colors. COMPOSITION. Cu 63-40 79-85 O 16-00 20-15 79-40 100-00 * Zeitschr. f. anal. Chem. 9, 463, 85.J BASES OF GROUP V. 179 c. Cupric sulphide, prepared in the wet way, is a brownish- Muck, or black precipitate, almost absolutely insoluble in water.* When exposed to the air in a moist state, it acquires a greenish tint and the property of reddening litmus paper, cupric sulphate being formed. Hence the sulphide must be washed with water containing hydrogen sulphide. It dissolves readily in boiling nitric acid, with separation of sulphur. Hydrochloric acid dis- solves it with difficulty. This is the reason why hydrogen sulphide precipitates copper entirely from solutions which contain even a very large amount of free hydrochloric acid (GnuNDMANNf). Only when we dissolve a copper salt directly in pure hydrochloric acid of 1*1 sp. gr. does any copper remain unprecipitated (M. MARTINA). It does not dissolve in solutions of potassa and of potassium sulphide, particularly if these solutions be boiling; it dissolves perceptibly in colorless, and much more readily in hot yellow ammonium sulphide. Potassium cyanide dissolves the freshly pre- cipitated sulphide readily and completely. Upon intense ignition in a current of hydrogen it is converted into pure Cu,S. d. If the blue solution which is obtained upon adding to solu- tion of copper tartaric acid and then soda in excess, is mixed with solution of grape sugar or sugar of milk, and heat applied, an orange-yellow precipitate of cuprous hydroxide is formed, which contains the whole of the copper originally present in the solu- tion, and after a short time, more particularly upon the applica- tion of a stronger heat, turns red, owing to the conversion of the hydroxide into anhydrous cuprous oxide (Cu 2 O). The precipitate, which is insoluble in water, retains a portion of alkali with con- siderable tenacity. When treated with dilute sulphuric acid, it gives cupric sulphate which dissolves, and metallic copper which separates. e. Cuprous sulphocyanate, Cu 2 (CNS) a , which is always formed when potassium sulphocyanate is added to a solution of copper, mixed with sulphurous or hypophosphorous acid, is a white precipitate in- soluble in water, as well as in dilute hydrochloric or sulphuric acid. Dried at 115, the salt retains from 1 to 3 per cent, of water, which is driven off only by heating to incipient decomposition ; it is, therefore, not well adapted for direct weighing. When * In some experiments that I made when examining the Weilbach water, I found that about 950000 parts of water are required to dissolve 1 part of CuS. f Journ. f. prakt. Chem. 73, 241. \ Ib. 67, 375, 180 FORMS. [ 86. ignited- with sulphur, with exclusion of air, it changes to Cu 2 S (RivoT*). When heated, with hydrochloric acid and potassium chlorate, or with sulphuric acid and nitric acid, it is dissolved and suffers decomposition. Solutions of potassa and soda separate hydrated cuprous oxide, with formation of sulphocyanate of the alkali metal. f. Cuprous sulphide, produced by heating CuS in a current of hydrogen or Cu,(GN"S) a with sulphur, is a grayish-black crystalline mass, which may be ignited and fused without decomposition if the air is excluded. COMPOSITION. Cu, .... 126-80 79-85 S . 32-00 20-15 158-80 100-00 86. 6. BISMUTH. Bismuth is weighed as OXIDE, as METAL, or as CHKOMATE (Bi a O,2CrO 4 ). Besides these compounds, we have to study here the BASIC CARBONATE, the BASIC NITRATE, the BASIC CHLORIDE, and the SULPHIDE. a. Bismuth trioxide, prepared by igniting the carbonate or nitrate, is a pale lemon-yellow powder which, under the influence of heat, assumes transiently a dark yellow or reddish-brown color. When heated to intense redness, it fuses, without alteration of weight. Ignition with charcoal, or in a current of carbon mon- oxide, reduces it to the metallic state. Fusion with potassium cyanide also effects its complete reduction (II. RosEf). It is in- soluble in water, and does not affect vegetable colors. It dissolves readily in those acids which form soluble salts with it. When ignited with ammonium chloride it gives metallic bismuth, the reduction being attended with deflagration. COMPOSITION. Bi a . . . . . 416 89-655 O 3 48 10-345 464 100-000 *Ib. 62, 252. f Journ. f. prakt. Ohem. 61, 188. 86.] EASES OF GROUP V. 181 b. Metallic bismuth is white, with a reddish tinge, moderately hard, brittle, with a tendency to crystallize. It fuses at 264, and at a low white heat volatilizes. It does not oxidize in the air at the ordinary temperature, but with the co-operation of water it oxidizes slowly, more speedily on fusion. It dissolves in dilute nitric acid. c. Bismuth carbonate. Upon adding ammonium carbonate in excess to a solution of bismuth, free from hydrochloric acid, a white precipitate of basic bismuth carbonate (Bi 3 O z CO 3 ) is imme- diately formed ; part of this precipitate, however, redissolves in the excess of the precipitant. But if the fluid with the precipitate be heated before filtration, the filtrate will be free from bismuth. (Potassium carbonate likewise precipitates solutions of bismuth completely ; but the precipitate in this case invariably contains traces of potassium, which it is very difficult to remove by wash- ing. Sodium carbonate precipitates solutions of bismuth less completely.) The precipitate is easily Avashed; it is practically insoluble in water, but dissolves readily, with effervescence, in hydrochloric and nitric acids. Upon ignition it leaves the oxide. d. The basic bismuth nitrate, which is obtained by mixing with water a solution of the nitrate containing little or no free acid, presents a white, crystalline powder. It cannot be washed with pure cold water without suffering a decided alteration. It becomes more basic, while the washings show an acid reaction, and contain bismuth. If the basic salt, however, be washed with cold water containing -^-^ of ammonium nitrate, no bismuth passes through the filter. The solution of ammonium nitrate must not be warm. These remarks only apply in the absence of free nitric acid (J. LOWE*). On ignition the basic nitrate passes into the oxide. e. Basic bi.$m >>th- Morifo, formed by adding much water to solution of bismuth containing hydrochloric acid or sodium chloride, is a brilliant white powder (BiOCl after drying at 100). It is insoluble in water, but dissolves in concentrated hydrochloric or nitric acid. Fused with potassium cyanide it gives metallic bismuth. f. Bismuth chromate (Bi 2 O 3 ,2CrO 3 ), which is produced by adding potassium dichromate, slightly in excess, to a solution of * Ib. 74. 341. 182 FOBMS. [ 87. bismuth nitrate as neutral as possible, is an orange-yellow, dense, readily-subsiding precipitate, insoluble in water, even in presence of some free chromic acid, but soluble in hydrochloric acid and nitric acid. It may be dried at 100-112 without decomposition (LOWE*). COMPOSITION. o o / Q>v"v,, Bi ^ 464-00 69-78 ^ O x 664-96 100-00 g. Bismuth trisulphide, prepared in the wet way, is a brownish black, or black precipitate, insoluble in water, dilute acids, alkalies, alkali sulphides, sodium sulphite, and potassium cyanide. In moderately concentrated nitric acid it dissolves, especially on warming, to nitrate, with separation of sulphur. Hence in pre- cipitating bismuth from a nitric acid solution, care should be taken to dilute sufficiently. Hydrochloric acid impedes the pre- cipitation by hydrogen sulphide only when a very large excess is present, and the fluid is quite concentrated. The sulphide does not change in the air. Dried at 100, it continually takes up oxygen and increases slightly in weight ; if the drying is protracted this increase may be considerable (Expt. No. 58). Fused with potassium cyanide, it is completely reduced (H. ROSE). Reduction takes place more slowly by ignition in a current of hydrogen. COMPOSITION. Bi, 416 81-25 S $ 96 18-75 512 100-00 87. 7. CADMIUM. Cadmium is weighed either as OXIDE or as SULPHIDE. Besides these substances, we have to examine CADMIUM CARBON AT K. a. Cadmium oxide, produced by igniting the carbonate or nitrate, is a yellowish-brown or reddish-brown powder. The appli- * Journ. f. prakt. Chem. 67, 291. 87.] BASES OF GROTP V. 183 cation of a white heat fails to fuse, volatilize, or decompose it ; it is insoluble in water, hut dissolves readily in acids ; it does not alter vegetable colors. Ignition with charcoal, or in a current of hydrogen, carbon monoxide, or carburetted hydrogen, reduces it readily, the metallic cadmium escaping in the form of vapor. COMPOSITION. Cd ! . . . . 112 87-50 O 16 12-50 128 100-00 l>. Cadmium carbonate is a white precipitate, insoluble in water and the fixed alkali carbonates, and extremely sparingly soluble in ammonium carbonate. It loses its water completely upon drying. Ignition converts it into oxide. c. Cadmium sulphide, produced in the wet way, is a lemon- yellow to orange-yellow precipitate, insoluble in water, dilute acids, alkalies, alkali sulphides, sodium sulphite, and potassium cyanide (Expt. No. 59). It dissolves readily in concentrated hydrochloric- acid, with evolution of hydrogen sulphide. In precipitating, there- fore, with hydrogen sulphide, a cadmium solution should not contain too much hydrochloric acid, and should be sufficiently diluted. The sulphide dissolves readily in dilute sulphuric acid on heating. It dissolves in moderately concentrated nitric acid, with separation of sulphur. It may be washed, and dried at 100 or 105, without decomposition. Even on gentle ignition in a current of hydrogen, it volatilizes in appreciable amount (H. ROSE*), partially unchanged, partially as metallic vapor. COMPOSITION. Cd 112 77-78 S ... 32 22-22 100-00 Pogg. Annal. 110, 134 184 FORMS. [ 88, 89. METALS OF THE SIXTH GROUP. 88. 1. GOLD. Gold is always weighed in the metallic state. Besides METALLIC GOLD, we have to consider the TKISULPHIDE or AURIC SULPHIDE. a.. Metallic gold, obtained by precipitation, presents a blackish- brown powder, destitute of metallic lustre, which it assumes, how- ever, upon pressure or friction ; when coherent in a compact mass, it exhibits the well-known bright yellow color peculiar to it. It fuses only at a white heat, and resists, accordingly, all attempts at fusion over a spirit-lamp. It remains wholly unaltered in the air and at a red heat, and is not in the slightest degree affected by water, nor by any simple acid. Nitrohydrochloric acid dissolves it to trichloride. Hot concentrated sulphuric acid containing a little nitric acid dissolves gold, especially if in a finely divided condition, to a yellow fluid, from which it is thrown down again by water (J. SPILLED). 1. Auric sulphide. When hydrogen sulphide is transmitted through a cold dilute solution of auric chloride, the whole of the gold separates as auric sulphide. Au 2 S 3 , in form of a brownish- black precipitate. If this precipitate is left in the fluid, it is gradually transformed into metallic gold and free sulphuric acid. Upon transmitting hydrogen sulphide through a warm solution of auric chloride, aurous sulphide Au 2 S precipitates, with formation of sulphuric and hydrochloric acids. Auric sulphide is insoluble in water, hydrochloric acid, and nitric acid, but dissolves in nitrohydrochloric acid. Colorless am- monium sulphide fails to dissolve it; but it dissolves almost entirely in yellow ammonium sulphide, and completely upon addition of potassa. It dissolves in potassa, with separation of gold. Yellow potassium sulphide dissolves it completely. It dis- solves in potassium cyanide. Exposure to a moderate heat reduces it to the metallic state. 89. 2. PLATINUM. Platinum is invariably weighed in the METALLIC STATE ; it is f Chern. News, 14, 256. 90.] METALS OF <;Korp vi. 185 generally precipitated as AMMOXITM PLATINIC CHLORIDE, or as POTASSIUM PLATINIC CHLORIDE, rarely as PLATINIC SULPHIDE. a. Metallic platinum, produced by igniting ammonium platinic chloride, or potassium platinic chloride, presents the appearance of a gray, lustreless, porous mass (spongy platinum). The fusion of platinum can be effected only at the very highest degrees of heat. It remains wholly unaltered in the air, and in the most powerful furnaces. It is not attacked by water, or simple acids, and scarcely by aqueous solutions of the alkalies. Nitrohydrochloric acid dis- solves it to platinic chloride. J. The properties of potassium platinic chloride, and those of ammonium platinic chloride, have been given already in 68 and TO respectively. c. Platinic sulphide. When a concentrated solution of pla- tinic chloride is mixed with hydrogen sulphide water, or when hydrogen sulphide gas is transmitted through a rather dilute solution of the chloride, no precipitate forms at first ; after stand- ing some time, however, the solution turns brown, and finally a precipitate subsides. But if the mixture of solution of platinic chloride, with hydrogen sulphide in excess, is gradually heated (finally to ebullition), the whole of the platinum separates as platinic sulphide (free from any admixture of platinic chloride). Platinic sulphide is insoluble in water and in simple acids ; but it dissolves in nitrohydrochloric acid. It dissolves partly in caustic alkalies, with separation of platinum, and completely in alkali sulphides, especially the polysulphides if used in sufficient excess. When hydrogen sulphide is transmitted through water holding minutely divided .platinic sulphide in suspension, the sulphide, absorbing hydrogen sulphide, acquires a light grayish-brown color ; the hydrogen sulphide thus absorbed, separates again upon exposure to the air. When moist platinic sulphide is exposed to the air, it is gradually decomposed, being converted into metallic platinum and sulphuric acid. Ignition in the air reduces platinic sulphide to metallic platinum. 90. 3. ANTIMONY. Antimony is weighed as ANTIMONIOUS SULPHIDE, as ANTIMONY TETROXIDE (or ANTIMONIOUS ANTIMONATE), or more rarely in the METALLIC state. 186 FORMS. [ 90. a. Upon transmitting hydrogen sulphide through a solution of antimonious chloride mixed with tartaric acid, an orange precipi- tate of amorphous antimonious sulphide is obtained, mixed at first with a small portion of basic antimony chloride. However, if the fiuid is thoroughly saturated with hydrogen sulphide, and a gentle heat applied, the chloride mixed with the precipitate is decom- posed, and pure antimonious sulphide obtained. Antimonious sulphide is insoluble in water and dilute acids ; it dissolves in con- centrated hydrochloric acid, with evolution of hydrogen sulphide. In precipitating with hydrogen sulphide, therefore, antimony solutions should not contain too much free hydrochloric acid, and should be sufficiently diluted. The amorphous antimonious sul- phide dissolves readily in dilute potassa, ammonium sulphide, and potassium sulphide, sparingly in ammonia, very slightly in ammo- nium carbonate, and not at all in hydrogen potassium sulphite. The amorphous sulphide, dried in the desiccator at the ordinary temperature, loses very little weight at 100; if kept for some time at this latter temperature its weight remains constant. But it still retains a little water, which does not perfectly escape even at 190, but at 200 the sulphide becomes anhydrous, turning black and crystalline (II. KOBE* and Expt. No. 60). Ignited gently in a stream of carbon dioxide, the weight of this anhydrous sulphide remains constant; at a stronger heat a small amount volatilizes. The amorphous sulphide, if long exposed to the action of air, in presence of water, slowly takes up oxygen, so that on treatment with tartaric acid it yields a filtrate containing anti- mony. Antimonic sulphide is insoluble in water, also in water con- taining hydrogen sulphide. It dissolves completely in ammonia, especially on warming; traces only dissolve in ammonium car- bonate. On heating dried antimonic sulphide in a current of carbon dioxide 2 atoms of sulphur escape, black crystalline anti- monious sulphide remaining. On treating antimonious or antimonic sulphide with fuming nitric acid violent oxidation sets in. We obtain first antimonic acid and pulverulent sulphur ; on evaporating to dryness antimonic acid and sulphuric acid ; and lastly on igniting antimony tetroxide. The same antimony tetroxide is obtained by igniting the sulphide * Journ. f. prakt. Chem. 59, 331. 90. J METALS OF GROUP VI. 187 with 30 to 50 times its amount of mercuric oxide [According to later investigations of BuxsEN,t the temperature necessary to reduce Sb 2 O. to Sb 2 O 4 lies so near that which reduces Sb a O 4 to Sb 3 O 3 that it is not easy to bring antimony into Sb a O 4 for weighing. It is possible only by using a large covered platinum or rather large open porcelain crucible (by suitable choice of size of crucible and intensity of flame) and heating with a gas blast lamp so that the bottom only of the crucible reaches a strong red heat, to drive off exactly one atom of oxygen from Sb 3 O 6 .] Ignition in a current of hydrogen converts the sulphides of antimony into the metallic state. COMPOSITION. Sb, . . . . 244-00 71-77 S 8 .... 96-00 28-23 340-00 100-00 b. Antimony tetroxide is a white powder, which, when heated, acquires transiently a yellow tint ; it is infusible ; it loses weight when ignited intensely in a small platinum crucible with a gas blast flame (BuNSENf). It is almost insoluble in water, and dis- solves in hydrochloric acid with very great difficulty. It undergoes no alteration on treatment with ammonium sulphide. It manifests an acid reaction when placed upon moist litmus-paper. COMPOSITION. Sb a 244 79-22 64 20-78 308 100-00 c. Metallic antimony* produced in the wet way, by precipita- tion, presents a lustreless black powder. It may be dried at 100 without alteration. It fuses at a moderate red heat. Upon ignition in a current of gas, e.g., hydrogen, it volatilizes, without formation of antimonetted hydrogen. Hydrochloric acid has very little action on it, even when concentrated and boiling. Nitric acid converts it into antimonious oxide, mixed with more or less * Annal. de Chem. u. Pharm. 106, 3. f Zeitschr. f . anal. Chem. 1879, 268. 188 FORMS. [g 91. antimony tetroxide, according to the concentration of the nitric acid. 91. 4. TIN IN STANNOUS COMPOUNDS ; and 5. TIN IN STANNIC COMPOUNDS. Tin is generally weighed in the form of STANNIC OXIDE ; be- sides stannic oxide, we have to examine stanuous sulphide and stannic sulphide. a. Stannic oxide. If a solution of an alkali, sodium sulphate or ammonium nitrate is added to a solution of stannic chloride, stannic acid (H 2 SnO 3 ) is precipitated. This precipitate is soluble in excess of soda, and does not separate again even on the addition of a large quantity of soda (C. F. BAKFOED*). It is also readily soluble in hydrochloric acid. By the action of nitric acid on metallic tin, or by evaporating a solution of tin with an excess of nitric acid, a white. residue is obtained which is metastannic acid (Sn 6 H 10 O 16 ?). This residue is insoluble in water, but very slightly soluble in nitric acid, or sulphuric acid. By heating with hydrochloric acid it does not dissolve, but is changed to metastannic chloride, which is soluble in water after removal of the excess of hydrochloric acid. Soda added to a solution of metastannic chloride precipitates sodium metastaiinate, which is insoluble in excess of soda and in weak alcohol. Upon intense ignition, both stannic and metastannic acids are converted into stannic oxide. Mere heating to redness is not sufficient to expel all the water (DuMAsf). Stannic oxide is a straw-colored powder, which under the influence of heat, transiently assumes a different tint, varying from bright yellow to brown. It is insoluble in water and acids, and does not alter the color of litmus-paper. Mixed with ammonium chloride in excess, and ignited, it volatilizes completely as stannic chloride. If stannic oxide is fused with potassium cyanide, all the tin is obtained in form of metallic globules, which may be com- pletely, and without the least loss of metal, freed from the adhering slag, by extracting with dilute alcohol, and rapidly decanting the fluid from the tin globules (H. ROSE;):). * Zeitschr. f. anal. Chem. 7, 260. f Annal. d. Chem. u. Pharm. 105, 104. \ Journ. f. prakt. Chem. 61, 189. 91.] METALS OF GROUP VI. 189 COMPOSITION. Sn 118 78-67 O, 32 21-33 150 100-00 b. Hydrated stannous sulphide forms a brown precipitate, insoluble in water, hydrogen sulphide water, and dilute acids. In precipitating tin from stannous solutions by means of hydrogen sulphide, free hydrochloric acid must not be present in too large amount, and the solution must be diluted sufficiently. Ammonia fails to dissolve it ; but it dissolves pretty readily in yellow ammo- nium sulphide, and in yellow potassium sulphide ; it dissolves readily in hot concentrated hydrochloric acid. Heated, with exclu- sion of air, it loses its water, and is rendered anhydrous; when ex- posed to the continued action of a gentle heat, with free access of air, it is converted into sulphur dioxide, which escapes, and stannic oxide, which remains. c. Hydrated stannic sulphide, precipitated by acids from the solution of its alkali sulphur salts, is a light-yellow precipitate. In washing with pure water, it is inclined to yield a turbid filtrate and to stop up the pores of the filter ; this annoyance is got over by washing with water containing sodium chloride, ammonium acetate, or the like (BuxsEx). On drying, the precipitate assumes a darker tint. It is insoluble in water ; it dissolves with difficulty in ammonia, but readily in potassa, alkali sulphides, and hot con- centrated hydrochloric acid. It is insoluble in hydrogen potassium sulphite. In precipitating tin from, stannic solutions by hydrogen sulphide, the solution should not contain too much free hydro- chloric acid, and should be sufficiently diluted. According to C. F. BARFOED* the precipitates thus produced are not pure hydrated stannic sulphide, but a mixture of this with stannic or metastannic acid, as the case may be. The precipitate thrown down from ordinary stannic chloride keeps its yellow color even after long standing in the fluid, and dissolves completely in excess of soda ; that thrown down from the metastannic chloride is first white and becomes gradually yellow, it turns brown on standing in the fluid and dissolves in excess of soda, leaving, however, a considerable residue of sodium metastannate. When heated, with * Zeitschr. f. anal. Chem. 7, 261. 190 FORMS. [ 92. exclusion of air, stannic sulphide loses its water of hydration, and, at the same time, according to the degree of heat, one-half or one- fourth of its sulphur, becoming converted either into stannous sulphide or the sesquisulphide of tin ; when heated very slowly, -with free access of air, it is converted into stannic oxide, with dis- engagement of sulphur dioxide. 92. 6. ARSENIC OF ARSENIOUS COMPOUNDS ; and 7. ARSENIC OF ARSENIC COMPOUNDS. ARSENIC is weighed either as LEAD ARSENATE, as ARSENIOUS SULPHIDE, aS AMMONIUM MAGNESIUM ARSENATE, as MAGNESIUM PYRO- ARSENATE, or as URANYL PYROARSENATE ; besides these forms, we have here to examine also ARSENIO-MOLYBDATE OF AMMONIUM. a. Lead arsenate, in the pure state, is a white powder, which agglutinates when exposed to a gentle red heat, at the same time transitorily acquiring a yellow tint ; it fuses when exposed to a higher degree of heat. When strongly ignited, it suffers a slight diminution of weight, losing a small proportion of arsenic acid, which escapes as arsenious oxide and oxygen. In analysis we have never occasion to operate upon the pure lead arsenate, but upon a mixture of it with lead oxide. 1). A.rsenious sulphide forms a precipitate of a rich yellow color; it is insoluble in water,* and also in hydrogen sulphide water. When boiled with water, or left for several days in con- tact with that fluid, it undergoes a very trifling decomposition : a trace of arsenious acid dissolves in the water, and a minute pro- portion of hydrogen sulphide is disengaged. This does not in the least interfere, however, with the washing of the precipitate. The precipitate may be dried at 100, without decomposition ; the whole of the water which it contains is expelled at that tempera- ture. When exposed to a stronger heat, it transitorily assumes a brownish-red color, fuses, and finally rises in vapor, without decomposition. It dissolves readily in alkalies, alkali carbonates, * In some experiments which I had occasion to make, in the course of an analysis of the springs of Weilbach (Chemische Untersuchung der wichtigsten Nassauischen Mineralwasser von Dr. Fresenius, V. Schwefelquelle zu Weilbach. Weisbaden, Kreidel und Niedner. 1856), I found that one part of As 2 Sa dis- solves in about one million parts of water. 92.] METALS OF GROUP VI. 191 alkali sulphides, potassium hydrogen sulphite, and nitrohydro- chloric acid ; but it is scarcely soluble in boiling concentrated hydrochloric acid. Hed fuming nitric acid converts it into arsenic acid and sulphuric acid. It is insoluble in carbon disulphide. COMPOSITION. As a 150 60-98 S, , 96 39-02 246 100-00 c. Ammonium magnesium ar senate forms a white, somewhat transparent, finely crystalline precipitate, which when dried in a desiccator has the formula NH 4 MgAsO 4 + 6H 2 O. After drying at 100, its composition is (NH 4 MgAsO 4 ) 2 + H 2 O. At a higher temperature, say 105 110, more water escapes, and at 130 this loss is considerable (PULLER*). Upon ignition it loses water and ammonia, and changes to magnesium pyroarsenate, Mg 3 As 2 O 7 . On rapid ignition the escaping ammonia has a reducing action on the arsenic acid, and a notable loss is occasioned (H. EOSE) ; by raising the heat very gradually reduction may be avoided (H. 11 WrrrsTEiMjt PULLER), or by passing a current of dry oxygen during the ignition. Ammonium magnesium arsenate dissolves very sparingly in water, one part of the salt dried at 100, requir- ing 2656, one part of the anhydrous salt, 2788 parts of water of 15. It is far less soluble in ammoniated water, one part of the salt dried at 100 requiring 15038, one part of the anhydrous salt, 15T86 parts of a mixture of one part of solution of ammonia ('96 sp. gr.), and 3 parts of water at 15. In water containing ammonium chloride, it is much more readily soluble, one part of the anhydrous salt requiring 886 parts of a solution of one part of ammonium chloride in 7 parts of water. Presence of ammonia diminishes the solvent capacity of the ammonium chloride ; one part of the anhydrous salt requires 3014 parts of a mixture of 60 parts of water, 10 of solution of ammonia (-96 sp. gr.) and one of ammonium chloride.^ A solution of ammonium chloride, ammonia and magnesium sulphate dissolves much less of the salt than ammoniated water; thus, PULLER (loc. cit.) found that one * Zeitschr. f. anal. Chera. 10, 62. f Ib. 2, 19. $ Zeitschr. f. anal. Chem. 3, 206. PULLER obtained almost the same numbers (Ib. 10, 53). 192 FORMS. [92. part of the anhydrous salt dissolved in 32827 parts of a fluid con- taining -^ of magnesia mixture (p. 113). Excess of alkali arsenate still more diminishes the solubility of the salt in water containing ammonia and ammonium chloride (PULLER). V COMPOSITION OF AMMONIUM MAGNESIUM ARSENATE DRIED AT 100. 2MgO. . , 80-00 21-05 . . 52.08 13-68 /AsO/O ' \- l AsU M I 7 A g 2 O 5 . . . 230-00 60-53 H 2 . . . 18-00 4.74 +H 2 380-08 100-00 d. Magnesium pyr oar senate, obtained by careful ignition of the preceding salt, is white, infusible by ignition in a porcelain crucible even over the blowpipe, but agglutinating at a still higher temperature, and finally fusing. After ignition in a porcelain crucible it dissolves readily in hydrochloric acid : ammonia pre- cipitates ammonium magnesium arsenate from the solution in a crystalline form. COMPOSITION. 2MgO ... 80 25-81 As 2 O 5 ... 230 74-19 310 100-00 e. Uranyl pyroarsenate. If a solution of arsenic acid is mixed with potash in slight excess, then with acetic acid to strongly acid reaction, and finally with uranyl acetate, the whole of the arsenic is thrown down as UO 2 HAsO 4 + 4H 2 O. In the presence of salts of ammonia the precipitate also contains the whole of the arsenic, and consists of UO 2 NH 4 AsO 4 + water. Both precipitates are pale yellowish-green, slimy, insoluble in water, acetic acid and saline solutions, such as ammonium chloride, soluble in mineral acids. Boiling favors the separation of the precipitate, addition of a few drops of chloroform will help it to settle, the washing is to be effected by boiling up and decanting. Both precipitates give (UO 2 ) 2 As 2 O 7 on ignition. The latter is a light yellow residue ; if it has turned greenish from the action of reducing gases, it may be restored to its proper color by moistening with nitric acid and 93.] Anns OF GROTP i. 393 re-igniting. On igniting the ammonium uranyl arsenate, the ammonia must first be expelled by cautious heating, or a current of oxygen must be passed during the ignition, otherwise the arsenic acid will be partially reduced, and arsenic will be lost (PULLER*). COMPOSITION. AsO < g > 1 JO, 2UO a O . . 571 - 2 71-29 AsO < g > 1 TO, As 9 O 5 . . 230-0 28-71 801-2 100-00 f. Arsenic-mol ybdate of ammonium. If a fluid containing arsenic acid is mixed with excess of the nitric acid solution of ammonium molybdate, the fluid remains clear in the cold, but on heating a yellow precipitate of arsenio-molybdate of ammonium separates. This precipitate comports itself with solvents like the analogous compound of phosphoric acid ; it is, like the latter, insoluble in water, nitric acid, dilute sulphuric acid and salts, pro- vided an excess of solution of ammonium molybdate, mixed with acid in moderate excess, be present. Hydrochloric acid or metallic chlorides, when present in large quantity, interfere with the thoroughness of the precipitation. SELiasoHNf found it to be composed of 87*666 per cent, of molybdic acid, 6*308 arsenic acid, 4*258 ammonia, and 1*768 water. R FORMS IN WHICH THE ACID RADICALS ARE WEIGHED OR PRECIPITATED. ACIDS OF THE FIRST GROUP. 93, 1. ARSENIOUS ACID and ARSENIC ACID. See 92. 2. CHROMIC ACID. Chromic acid is weighed either as CHROMIC OXIDE, or as LEAD CHROMATE, or BARIUM CHROMATE. We have also to consider MER- CUROUS CHROMATE. a. Chromic oxide. See 76. b. Lead chromate obtained by precipitation forms a bright-yel- * Zeitschr. f. anal. Chem. 10, 72. f Journ. f. prakt, ('hem. 67, 481. 194 FOKMS. [ 93. low precipitate, insoluble in water and acetic acid, barely soluble in dilute nitric acid, readily in solution of potassa. When lead cliro- mate is boiled with concentrated hydrochloric acid, it is readily decomposed, lead chloride and chromic chloride being formed. Addition of alcohol tends to promote this decomposition. Lead chromate is unalterable in the air. It dries thoroughly at 100. Under the influence of heat it transitorily acquires a reddish-brown tint ; it fuses at a red heat ; when heated beyond its point of fusion, it loses oxygen, and is transformed into a mixture of chro- mic oxide and basic lead chromate. Heated in contact with organic substances, it readily yields oxygen to the latter. COMPOSITION. 223-00 68-94 100-48 31-06 323-48 100-00 c. Barium chromate is obtained as a light-yellow precipitate on mixing a solution of an alkali chromate with barium chloride. It dissolves in hydrochloric and in nitric acid, but not in acetic acid. On washing with pure water, the latter begins to dissolve it slightly, as soon as all soluble salts are removed, to such an extent that the washings run off yellow. The precipitate is insoluble in saline solutions. Hence it is best to use a solution of ammonium acetate for washing (PEARSON and RICHARDS*). It is not decom- posed by moderate ignition. COMPOSITION. BaO - - 153-00 60-36 100-48 39-64 253-48 100-00 d. Mercurous chromate obtained by adding mercurous nitrate to an alkali chromate is a brilliant-red precipitate, which turns black by the action of light. It dissolves very slightly in cold water, more in boiling water, being partially converted into a mer- curic salt ; it dissolves slightly in dilute nitric acid. For washing, *Zeitschr. f. anal. Chem. 9, 108. 93.] ACIDS OF GROUP I. 195 it is best to use a dilute solution of mercurous nitrate containing but little free acid ; in this solution it is insoluble (H. ROSE*). 3. SULPHURIC ACID. Sulphuric acid is determined best in the form of BARIUM suir PHATE, for the properties of which see 71. 4. PHOSPHORIC ACID. The principal forms into which phosphoric acid is converted are as follows : LEAD PHOSPHATE, MAGNESIUM PYROPHOSPHATE, MAGNE- SIUM PHOSPHATE Mg 3 (PO 4 ) 3 , FERRIC PHOSPHATE, URANYL PYROPHOS- PHATE, STANNIC PHOSPHATE, and SILVER PHOSPHATE. Besides these compounds, we have to examine MERCUROUS PHOSPHATE and PHOSPHO-MOLYBDATE OF AMMONIUM. a. The lead phosphate obtained in the course of analysis is rarely pure, but is generally mixed with free lead oxide. In this mixture we have accordingly the normal lead phosphate Pb 3 (PO 4 ) a ; in the pure state, this presents the appearance of a white powder;^ it is insoluble in water, acetic acid, and ammonia. It dissolves readily in nitric acid. When heated it fuses without decomposi- tion. b. Magnesium pyrophosphate. See 74. c. Magnesium phosphate (Mg 3 (PO 4 ) 3 ). A mixture of this com- pound with excess of magnesia is produced by mixing a solution of an alkali phosphate, containing ammonium chloride, with magnesia, evaporating, heating until the ammonium chloride is expelled, and finally treating with water. It is practically insoluble in water and in solutions of salts of the alkalies (FR. SCHULZE|). d. Ferric phosphate. If a solution of phosphoric acid or of calcium phosphate in acetic acid is carefully precipitated with a solution of ferric acetate, or with a mixture of iron-alum and sodium acetate, so that the iron salt may just predominate, the pre- cipitate always contains 1 mol. P a O 5 to 1 mol. Fe 2 O 3 corresponding to the formula of normal ferric phosphate, Fe 2 (PO 4 ) a (RAWSKY, AViTTSTEiN, E. DAVY:):) ; if, on the other hand, the ferric acetate is in larger excess, the precipitate is more basic. WITTSTEIN obtained, by using a considerable -excess of ferric acetate, a precipitate con- taining 3P 2 O 5 to 4Fe 2 O 3 . Precipitates obtained with a small excess of the precipitant possess a composition varying between the above- * Pogg. Ann. 53, 124. f Journ. f. prakt. Chem. 63, 440. t Phil. Mag. 19, 181. 196 FORMS. [ 93o mentioned limits. RAMMKLSBERG obtained Fe 2 fPO 4 ) 2 -|- 4FI 2 O, and WITTSTEIN subsequently the same compound (with 8II () instead of 4) upon mixing ferric sulphate with sodium phosphate in excess ; with an insufficient quantity of sodium phosphate the latter chem- ist obtained a more yellowish precipitate which had a composition corresponding to the formula -3 Fe 2 (PO 4 ) 2 + Fe a (OH) 6 + 8H,(). If an acid fluid containing a considerable excess of phosphoric acid is mixed with a small quantity of a ferric solution, and an alkali acetate is added, a precipitate of the formula, Fe a (PO 4 ) a -|- water, is invariably obtained, which accordingly leaves upon ignition Fe a (PO 4 ) a = Fe a O 8 -|~ P a O 6 (WITTSTEIN). Fresh experiments which I have made upon this subject have convinced me of the perfect correctness of this statement. MOHR obtained the same results.* The precipitate is insoluble in a fluid containing salts, but when washing, as soon as the soluble salts are nearly removed, the pre- cipitate begins to dissolve. The filtrate has an acid reaction, and contains iron and phosphoric acid. The precipitate, under these circumstances, alters in composition, and this explains why different results were obtained in the analysis of precipitates which had been washing for different lengths of time (FR. MOHR). COMPOSITION. _P 2 5 ... 142 47-02 ~Fe,O 3 . . . 160 52-98 PO---O- IV 302 If we dissolve ferric phosphate in hydrochloric acid, supersatu- rate the solution with ammonia, and apply heat, we obtain more basic salts, viz., 3Fe a O,,2P a O B (RAMMELSBEKG) ; 2Fe 2 O 3 ,P 2 O 5 (WITT- STEIN after long washing). In WITTSTEIN'S experiment, the wash- water contained phosphoric acid. The white ferric phosphate does not dissolve in acetic acid, but it dissolves in a solution of ferric acetate. Upon boiling the latter solution (of ferric phosphate in ferric acetate), the whole of the phosphoric, acid precipitates, with basic ferric acetate, as hyperbasic ferric phosphate. Similar extremely basic combinations are invariably obtained (often mixed with ferric hydroxide), upon precipitating with ammonia or barium * Zeitschr. f. anal. Cheni. 2, 250. 93.] ACIDS OF GROUP I. 197 carbonate, a solution containing phosphoric acid and an excess of a ferric salt. The precipitate obtained by barium carbonate can be conveniently filtered off and washed, the filtrate is perfectly free from either iron or phosphoric acid ; on the contrary, the precipi- tate obtained by ammonia, especially if the latter were much in excess, is slimy, and therefore difficult to wash, and the filtrate always contains small traces of both iron and phosphoric acid. e. Uranyl pyrophosphate. If the hot aqueous solution of a phosphate soluble in water or acetic acid is mixed, in presence of free acetic acid, with uranyl acetate, a precipitate of uranyl hydro- gen phosphate is immediately formed. If the fluid contains much ammonium salt, the precipitate contains also uranyl ammonium phosphate. The same precipitate forms also if aluminium or ferric salts are present; but in that case it is always mixed with more or less aluminium or ferric iphosphate. Presence of potassium or sodium salts, on the contrary, or of salts of the alkali-earth metals, has no influence on the composition of the precipitate. Ammonium uranyl phosphate (UO a y II 4 PO 4 -f- #H S O) is a somewhat gelatinous, whitish-yellow precipitate, with a tinge of green. The best way of washing it, at least so far as the principal part of the operation is concerned, is by boiling with water and decanting. If, after having allowed the fluid in which the precipitate is suspended to cool a little, a few drops of chloroform are added, and the mixture is shaken or boiled up, the precipitate subsides much more readily than without this addition. The precipitate is insoluble in water and in acetic acid ; but it dissolves in mineral acids ; ammonium acetate, added in sufficient excess, completely re-precipitates it from this solution, upon appli- cation of heat. Upon igniting the precipitate, no matter whether containing ammonium or not, uranyl pyrophosphate of the for- mula (UO 2 ) 2 P 2 O 7 is produced. This has the color of the yolk of an egg. If the precipitate is ignited in presence of charcoal or of some reducing gas, partial reduction to uranous phosphate ensues, owing to which the ignited mass acquires a greenish tint ; however, upon warming the greenish residue with some nitric acid, the green ura- nous salt is readily reconverted into the yellow uranyl salt. Uranyl pyrophosphate is not hygroscopic, and may therefore be ignited and weighed in an open platinum dish (A. AREXDT and "W. KNOP*). * Chemisches Centralblatt, 1856, 769, 803; and 1857, 177. 198 FOEMS. [ 93. PO<9>UO a 2UO 2 O . .571-2 80-09 < ^POUO, P a O 5 . ...142-0 19-91 713-2 100 00 The one-fifth part of the precipitate may accordingly be cal- culated as phosphoric anhydride in ordinary analyses.* f. Stannic phosphate is never obtained in the pure state in the analytical process, but contains always an admixture of hydrated metastannic acid in excess, which, upon ignition, changes to meta- stannic acid. It has, generally speaking, the same properties as hydrated metastannic acid, and is more particularly, like the latter, insoluble in nitric acid. Upon heating with concentrated solution of potassa, potassium phosphate and rnetastannate are formed. g. Normal silver phosphate is a yellow powder ; it is insoluble in water, but readily soluble in nitric acid, and also in ammonia. In ammonium salts, it is difficultly soluble. It is unalterable in the air. Upon ignition, it acquires transiently a reddish-brown color ; at an intense red heat, it fuses without decomposition. . . 695-82 83-05 142-00 16-95 837-82 100-00 h. Mercurous phosphate. This compound is employed for the purpose of effecting the separation of phosphoric acid from many bases, after H. ROSE'S method. Mercurous phosphate presents the appearance of a white crys- talline mass, or of a white powder. It is insoluble in water, but dissolves in nitric acid. The action of a red heat converts it into fused mercuric phosphate, with evolution of vapor of mercury. Upon fusion with alkali carbonates, alkali phosphates are pro- duced, and mercury, oxygen, and carbon dioxide escape. i. Phospho-molybdate of ammonium. This compound also * The atomic weight of uranium is here taken as 237*6, according to Ebel- men. If we take it according to Peligot, as 240, the ignited phosphate would contain 80'22 UO 3 , and 19*78 P 2 O 6 . W. Knop and Arendt found in four experiments 20*13, 20*06, 20*04, and 20*04 respectively (in another 20*77). It will be seen that these numbers agree better with the composition as reckoned from Ebelmen's than from Peligot's atomic weight. 93.] ACIDS OF GROUP i. 199 serves to effect the separation of phosphoric acid from other bodies ; it is of the utmost importance in this respect. Phospho-molybdate of ammonium forms a bright yellow, readily subsiding precipitate. Dried at 100, it has, according to SELIG- SOHN, the following (average) composition : MoO 3 90-744 P 2 O 5 . 3-142 CN"H 4 ) f O 3'- 570 H,O . . ' 2-544 100-000* In the pure state, it dissolves but sparingly in cold water (1 in 10000 EGGERTZ) ; but it is soluble in hot water. It is readily soluble even in the cold, in caustic alkalies, alkali carbonates and phosphates, ammonium chloride, and ammonium oxalate. It dis- solves sparingly in ammonium sulphate, potassium nitrate, and potassium chloride ; and very sparingly in ammonium nitrate. It is soluble in potassium sulphate and sodium sulphate, sodium chloride and magnesium chloride, and sulphuric, hydrochloric and nitric acids (concentrated and dilute). Water, containing 1 per cent, of common nitric acid, dissolves ^Vfr (EGGERTZ). Appli- cation of heat does not check the solvent action of these substances. Presence of ammonium molybdate totally changes its deportment with acid fluids. Dilute nitric or sulphuric acid containing ammonium molybdate does not dissolve it ; but much hydro- chloric acid, even in the presence of ammonium molybdate, has a solvent action, and this acid consequently interferes with the complete precipitation of phosphoric acid by nitric acid solution of ammonium molybdate. The solution of the phospho-molybdate of ammonium in acids is probably attended, in all cases, with decomposition and separation of the rnolybdic acid, which cannot take place in the presence of ammonium molybdate (J. CRAW)+ . Tartaric acid and similar organic substances entirely prevent the * From the varying results of different analysts it is plain that the precipi- tate, prepared under apparently the same circumstances, has not always exactly the same composition. SONNENSCHEIX (Journ. f . prakt. Chem. 53, 342) found in the precipitate dried at 120, 2'93 3'12 P 2 O 5 ; LIPOWITZ (Pogg. Annal. 109, 135), in the precipitate dried at from 20 to 30, 3'607 P 2 O 5 ; EGGERTZ (Journ. f. prakt. Chem. 79, 496), 3 '7 to 3 "8 $. f Chem. Gaz. 1852, 216. 200 FORMS. [ 93. precipitation of the phospho-molybdate of ammonium (EGGERTZ). In the presence of an iodide instead of a yellow precipitate, a green precipitate or a green fluid is formed, resulting from the reducing action of the hydriodic acid on the molybdic acid (J. W. BILL*). Other substances which reduce molybdic acid have of course a similar action. 5. BORACIC ACID. POTASSIUM BOROFLUORIDE is the best form to convert boracic acid into for the purpose of the direct estimation of the acid. This compound is produced by mixing the solution of an alkali borate, in presence of a sufficient quantity of potassa, with hydrofluoric acid in excess, in a silver or platinum dish, and evaporating to dry- ness. The gelatinous precipitate which forms in the cold, dissolves upon application of heat, and separates from the solution subse- quently, upon evaporation, in small, hard, transparent crystals. The compound has the formula KF,BF 3 . It is soluble in water arid also in dilute alcohol ; but strong alcohol fails to dissolve it t * it is insoluble also in concentrated solution of potassium acetate. It may be dried at 100, without decomposition (AuG. STRO- MEYERf). COMPOSITION. K 39-13 31-02 B 11-00 8-72 F 76-00 60-26 126-13 100-00 6. OXALIC ACID. When oxalic acid is to be directly determined it is usually pre- cipitated in the form of CALCIUM OXALATE ; and its weight is inferred from the CALCIUM CARBONATE or CALCIUM OXIDE produced from the oxalate by ignition. For the properties of these bodies see 73. 7. HYDROFLUORIC ACID. The direct estimation of hydrofluoric acid is usually effected by weighing the acid in the form of CALCIUM FLUORIDE. Calcium fluoride forms a gelatinous precipitate, which it is found difficult to wash. If digested with ammonia, previous to * Sillim. Journ., July, 1858. \ Annal. d. Chem. u. Pharm. 100, 82. 93.] ACIDS OF GROUP I. 201 filtration, it is rendered denser and less gelatinous. It is not alto- gether insoluble in water ; aqueous solutions of the alkalies fail to decompose it. It is very slightly soluble in dilute, but more readily in concentrated hydrochloric acid. When acted upon by sulphuric acid, it is decomposed, and calcium sulphate and hydro- fluoric acid are formed. Calcium fluoride is unalterable in the air, and at a red heat. Exposed to a very intense heat, it fuses. Upon intense ignition in moist air, it is slowly and partially decomposed into calcium oxide and hydrofluoric acid. Mixed with ammonium chloride, and exposed to a red heat, calcium fluoride suffers a con- tinual loss of weight ; but the decomposition is incomplete. COMPOSITION. Ca ...!.. 40 51-28 F, 38 48.72 78 100-00 We often determine fluorine, more particularly in presence of silicic acid, by converting it into silicon fluoride (SiF 4 ). This is a colorless gas, fuming in the air, with suffocating odor, of sp. gr. 3'574, which decomposes when mixed with water forming silica and hydrofluosilicic acid thus : 3SiF 4 + 2H.O = 2H 2 SiF.+ SiO 2 . 8. CARBONIC Aero. The direct estimation of carbonic acid which, however, is only rarely resorted to is usually effected by weighing the acid in the form of CALCIUM CARBONATE. For the properties of the lattefr substance, see 73. 9. SILICIC ACID.* When silicic acid is separated by acids from aqueous solutions of alkali silicates, it is at first perfectly soluble in water. It be- comes insoluble or rather difficultly soluble when it coagulates. Coagulation is a permanent change and is furthered by concentra- tion and by elevation of temperature. Silicic acid solution con- taining 10 or 12 per cent, of SiO 2 coagulates at the ordinary tem- perature in a few hours, and immediately if heated. A solution of * Free silicic acid in solution is assumed to have the composition expressed by the formula Si(OH) 4 . Silicic anhydride (SiO 2 ) is usually called "silica." Compounds of SiO 3 with less water than corresponds to the formula Si(OH) 4 = SiO 2 (H 3 O) 2 are here called " hydrates of silica." 202 FORMS. [ 93. 5 per cent, may be preserved without coagulating for five or six days, one of 2 per cent, for two or three months, and one of 1 per cent, for several years, and solutions containing ^ per cent, or less are not appreciably altered by time. Solid matter in powder such as graphite, hastens coagulation, alkali salts induce it rapidly. Aque- ous solutions of silicic acid may, on the contrary, be mixed with hydrochloric acid, nitric acid, acetic acid, tartaric acid and alcohol without coagulating. The gelatinous silicic acid produced by coagulation may contain more or less water, and it appears to be the more difficultly soluble in water, the less water it contains; thus a jelly of silicic acid containing 1 per cent, of silica (SiO 2 ) gives a solution with cold water containing 1 part of silica in about 5000 rparts. a jelly of 5 per cent, gives a solution containing 1 part of silica in about 10000 parts of water. A jelly containing less water is still less soluble, and when the jelly, is dried up to a gummy mass it is barely soluble at all ; this is also the case with the pulverulent hydrate of silica obtained in the analysis of silicates by drying a jelly containing much salts at 100 (GrRAHAM*). The hydrated silica dried at 100 dissolves but very slightly in acids (with the exception of hydrofluoric acid) ; it dissolves, however, in solutions of fixed alkalies and alkali carbonates, especially on heating. Aque- ous ammonia dissolves the jelly in tolerable quantity and the dry hydrate in very notable quantity (PRiBRAM)f. Regarding the amount of water in the hydrate dried at given temperatures chem- ists do not agree.;}; On ignition all the hydrates pass into anhydrous silica. As the vapor escapes small particles of the extremely fine powder are liable to whirl up. This may be avoided by moistening the hydrate in the crucible with water, evaporating to dry ness on a water bath, and then applying at first a slight and then a gradu- ally increased heat. The silica obtained by igniting the hydrate appears in the amorphous condition, with a sp. gr. of 2'2 to 2*3. It forms a * Pogg. Annal. 123, 529. f Zeitschr. f. anal. Chem. 6, 119. \ DOVERI (Annal. de Chim. et de Phys. 21, 40; Annal. d. Chem. u. Pharm. 64, 256) found in the air-dried hydrate 16'9 to 17*8 I water; J. FUCHS (Annal. d. Chem. u. Pharm. 82, 119 to 123), 9'1 to 9'6; G. LIPPERT, 9'28 to 9'95. DOVERI found in the hydrate ' dried at 100, 8'3 to 9*4; J. FUCHS, 6 '63 to 6'96; G. LIP- PERT 4-97 to 5'52. H. ROSE (Pogg. Annal. 108. 1; Journ. fur prakt. Chem. 81, 227) found in the hydrate obtained by digesting stilbite with concentrated hydrochloric acid, and dried at 150, 4 '85 $ water. 94.] ACIDS OF GROUP II. 203 white powder insoluble in water, and acids (hydrofluoric excepted), soluble in solutions of the fixed alkalies and their carbonates, especially in the heat. Hydrofluoric acid readily dissolves amor- phous silica; the solution leaves no residue on evaporation in platinum, if the silica was pure. The amorphous silica, when heated with ammonium fluoride in a platinum crucible, readily volatilizes. The ignited amorphous silica, exposed to the air, eagerly absorbs water, which it will not give up at from 100 to 150 (H. HOSE). The lower the heat during ignition the more hygroscopic is the residue (SOUCHAY*). Silica fuses at the strong- est heat ; the mass obtained being vitreous and amorphous. Amor- phous silica ignited with ammonium chloride, at first loses weight, and then, when the ignition has rendered it denser, the weight remains constant. The amorphous silica must be distinguished from the crystallized or crystalline variety, which occurs as rock crystal, quartz, sand, &c. This has a sp. gr. of 2*6 (SCHAFFGOTSCH), and is far more difficultly, and in far less amount, dissolved by potash solution or solution of fixed alkali carbonates ; it is also more slowly attacked by hydro- fluoric acid, or ammonium fluoride. Crystallized silica is not hygro- scopic, whether strongly or gently ignited (SOUCHAY). Vegetable colors are not changed either by silica or its hydrates. COMPOSITION. Si 28-00 46-67 O, 32-00 53-33 60-00 100-00 ACID RADICALS OF THE SECOND GROUP. 94. 1. HYDROCHLORIC ACID. Hydrochloric acid is almost invariably weighed in the form of SILVER CHLORIDE for the properties of which see 82. 2. HYDROBROMIC Acn>. * Hydrobromic acid is always weighed in the form of SILVER BROMIDE. * Zeitschr. f. anal. Chem. 8, 423. 204 FORMS. [ 94. Silver bromide, prepared in the wet way, forms a yellowish- white precipitate. It is wholly insoluble in water and in nitric acid, tolerably soluble in ammonia, readily soluble in sodium thio- sulphate and potassium cyanide. Concentrated solutions of potas- sium, sodium, and ammonium chlorides arid bromides dissolve it to a very perceptible amount, while in very dilute solutions of these salts it is entirely insoluble. Traces only dissolve in the alkali nitrates. It dissolves abundantly in a concentrated warm solution of mercuric nitrate. On digestion with excess of potassium iodide solution it is completely converted into silver iodide (FIELD). On ignition in a current of chlorine silver bromide is transformed into chloride ; on ignition in a current of hydrogen it is converted into metallic silver. Exposed to the light it gradually turns gray, and finally black. Under the influence of heat, it fuses to a reddish liquid, which, upon cooling, solidifies to a yellow, horn-like mass. Brought into contact with zinc and water, it is decomposed : a spongy mass of metallic silver forms, and the solution contains zinc bromide. COMPOSITION. Ag . . . . 107-93 57-45 Br 79-95 42-55 187-88 100-00 3. HYDRIODIC ACID. Hydriodic acid is usually determined in the form of SILVER IODIDE, and occasionally also in that of PALLADIOUS IODIDE. a. Silver iodide, produced in the wet way, forms a light-yellow precipitate, insoluble in water, and in dilute nitric acid," and very slightly soluble in ammonia. One part dissolves, according to WALLACE and LAMONT* in 2493 parts of aqueous ammonia sp. gr. 89, according to MARTINI, in 2510 parts of *96 sp. gr. It is copi- ously taken up by concentrated solution of potassium iodide, but it is insoluble in very dilute ; it dissolves readily in sodium thiosul- phate and in potassium cyanide ; traces only are dissolved by alkali nitrates. In concentrated warm solution of mercuric nitrate it is- copiously soluble. Hot concentrated nitric and sulphuric acids convert it, but with some difficulty, into silver nitrate and sulphate respectively, with expulsion of the iodine. Silver iodide acquires a Chem Gaz. 1859, 137. 94.] ACIDS OF GROUP II. 205 black color when exposed^ to the light. When heated, it fuses without decomposition to a reddish fluid, which, upon cooling, solidifies to a yellow mass, that may be cut with a knife. Under the influence of excess of chlorine in the heat it is completely con- verted into silver chloride; ignition in hydrogen reduces it but incompletely to the metallic state. When brought into contact with zinc and water, it is decomposed but incompletely : zinc iodide is formed, and metallic silver separates. COMPOSITION. Ag . . . . 107-93 45- 97 I 126-85 54-03 234-78 100-00 1. Palladious iodide, produced by mixing an alkali iodide with palladious chloride, is a deep brownish-black, flocculent pre- cipitate, insoluble in water, and in dilute hydrochloric acid, but slightly soluble in saline solutions (sodium chloride, magnesium chloride, calcium chloride, &c.). It is unalterable in the air. Dried simply in the air it retains one molecule of water =5-05 per cent. Dried long in vaciw, or at a rather high temperature (70 to 80), it yields the whole of this water, without the least loss of iodine. Dried at 100, it loses a trace of iodine ; at from 300 to 400, the whole of the iodine is expelled. It may be washed with hot water, without loss of iodine. COMPOSITION. Pd 106-58 29-58 I, 253-70 70-42 360-28 100-00 4. HYDROCYANIC Aero. Hydrocyanic acid, if determined gravimetrically and directly, is always converted into SILVEK CYANIDE for the properties of which compound see 82. 5. HYDROSULPHURIC ACID. The forms into which the sulphur in hydrogen sulphide or metallic sulphides, is converted for the purpose of being weighed, 206 FORMS. [ 95. are ARSENIOUS SULPHIDE, SILVER SULPHIDE, COPPER SULPHIDE, and BARIUM SULPHATE. For the properties of the sulphides named, see 82, 85, 92 ; for those of barium sulphate, see 71. ACID RADICALS OF THE THIRD GROUP. 95. 1. NITRIC ACID ; and 2. CHLORIC Aero. These two acids are never determined directly that is to say, in compounds containing them, but always in an indirect way ; generally volumetrically. SECTION IV. THE DETERMINATION (OR ESTIMATION) OF RADICALS. 96. IN the preceding Section we have examined the composition and properties of the various forms and combinations in which radicals are separated from each other, or in which they are weighed. We have now to consider the special means and methods of con- verting them into such forms and combinations. For the sake of greater clearness and simplicity, we shall, in the present Section, confine our attention to the various methods applied to effect the determination of single radicals, deferring to the next Section the consideration of the means adopted for sepa- rating them from each other. As in the " Qualitative Analysis," the acids of arsenic will be treated of among the bases, on account of their behavior to hydro- gen sulphide. In the quantitative analysis of a compound we have to study first, the most appropriate method of dissolving it ; and, secondly, the 'modes of determining the quantity of one or more of its cqn- stituents. With regard to the latter point, we have to turn our attention, first, to the performance; and secondly, to the accuracy of the methods. It happens very rarely in quantitative analyses that the amount of a substance, as determined by the analytical process, corresponds exactly with the amount theoretically calculated or actually pres- ent ; and if it does happen, it is merely by chance. It is of importance to inquire what is the reason of this fact, and what are the limits of inaccuracy in the several methods. The cause of this almost invariably occurring discrepancy between the quantity present and that actually found, is to be ascribed either exclusively to the twcution* or it lies partly in the method itself. 208 DETERMINATION. [ 96. The execution of the analytical processes and operations can never be absolutely accurate, even though the greatest care and .attention be bestowed on the most trifling minutiae. To account for this, we need only bear in mind that our weights and measures are never absolutely correct, nor our balances absolutely accurate, nor our reagents absolutely pure ; and, moreover, that we do not weigh m vacuo ; and that, even if we deduce the weight in vacuo from the weight we actually obtain by weighing in the air, the very volumes on which the calculation is based are but approxi- mately known ; that the hygroscopic state of the air is liable to vary between the weighing of the empty crucible and of the cru- cible -j- the substance ; that we know the weight of a filter ash only approximately y .that we can never succeed in completely keeping off dust, &c. With regard to the methods, many of them are not entirely free from certain unavoidable sources of error ; precipitates are not absolutely insoluble; compounds which require ignition are not absolutely fixed ; others, which require drying, have a slight tendency to volatilize ; the final reaction in volumetric analyses is usually pi'oduced only by a small excess of the standard fluid, which is occasionally liable to vary with the degree of dilution, the temperature, the potassium may be separated in the first form, and then titrated as the latter (STOLBA, loc. cit.). 98. 2. SODIUM. a. Solution. See 97, a solution of potassa sodium all the directions given in that place applying equally to the solution of soda and sodium salts. b. Determination. Sodium is determined either as sodium sulphate, as sodium chloride, or as sodium carbonate ( 69). For the alkalimetric esti- mation of caustic soda and sodium carbonate, see 195 and 196. We may convert into 1. SODIUM SULPHATE; 2. SODIUM CHLORIDE. In general the sodium salts corresponding to the potassium salts specified under the analogous potassium compounds, 97. 3. SODIUM CARBONATE. Caustic soda, sodium hydrogen carbonate, and sodium salts of organic acids, also sodium nitrate and sodium chloride. In sodium borate the sodium is estimated best as sodium sul- phate ( 136) ; in the phosphate, as sodium chloride, or sodium carbonate ( 135). Sodium salts of organic acids are determined either, like the corresponding potassium compounds, as chloride, or by preference as carbonate. (This latter method is not so well adapted for potassium salts.) The analyst must here bear in mind, that when carbon acts on fusing sodium carbonate, carbon monoxide escapes, and caustic soda in not inconsiderable quantity is formed. 1. Determination as Sodium Sulphate. If alone and in v aqueous solution, evaporate to dryiiess, ignite and weigh the residue in a covered platinum crucible ( 42). The process does not involve any risk of loss by decrepitation, as in the case of potassium sulphate. If free sulphuric acid happens to be 216 DETERMINATION. [ 98. present, this is removed in the same way as in the case of potas- sium sulphate. With regard to the conversion of sodium chloride, &c., into sodium sulphate, see 97, &, 1. For properties- of the residue, see 69. The method is easy, and gives accurate results. 2. Determination as Sodium Chloride. Same method as described in 1. The rules given and the observations made in 97, >, 2, apply equally here. For properties of the residue, see 69. The methods of converting sodium sulphate, chromate, chlorate, and silicate into sodium chloride, will be found in Part II. of this Section, under the respective heads of the acids which these salts contain. 3. Determination as Sodium Carbonate. Evaporate the aqueous solution, ignite moderately, and weigh. The results are perfectly accurate. For properties of the residue, see 69. Caustic soda is converted into the carbonate by adding to its aqueous solution ammonium carbonate in excess, evaporating at a gentle heat, and igniting the residue. Sodium hydrogen carbonate, if in the dry state, is converted into the normal carbonate by ignition. The heat must be very gradually increased, and the crucible kept well covered. If in aqueous solution, it is evaporated to dryness, in a capacious silver or platinum dish, and the residue ignited. Sodium salts of organic acids are converted into the carbonate by ignition in a covered platinum crucible, from which the lid is removed after a time. The heat must be increased very gradually. When the mass has ceased to swell, the crucible is placed obliquely, with the lid leaning against it (see 52, fig. 42), and a dull red heat applied until the carbon is consumed as far as practicable. The contents of the crucible are then warmed with water, and the fluid is filtered off from the residuary carbon, which is carefully washed. The filtrate and rinsings are evaporated to dryness with the addition of a little ammonium carbonate, and the residue is ignited and weighed. The ammonium carbonate is added, to con- vert any caustic soda that may have been formed into carbonate. The method, if carefully conducted, gives accurate results ; how- ever, a small loss of soda on carbonization is not to be avoided. 99.] AMMOXH.M. 217 Sodium nitrate, or sodium chloride, may be converted into car- bonate, by adding to their aqueous solution perfectly pure oxalic acid in moderate excess, and evaporating several times to dryness, with repeated renewal of the water. All the nitric acid of the sodium nitrate escapes in this- process (partly decomposed, partly undecomposed) ; and equally so all the hydrochloric acid in the case of sodium chloride. If the residue is now ignited until the excess of oxalic acid is removed, sodium carbonate is left. 99. 3. AMMONIUM. a. Solution. Ammonia is soluble in water, as are all ammonium salts of those acids which claim our attention here. It is not always necessary, however, to dissolve ammonium salts for the purpose of determin- ing the amount of ammonium contained in them. 5. Determination. Ammonium is weighed, as stated TO, either in the form of ammonium chloride^ or in that of ammonium platinic chlori'f' . Into these forms it may be converted either directly or Indirectly (i.e., after expulsion as ammonia, and re-combination with an acid). Ammonium is also frequently determined by volumetric analysis, and its quantity is sometimes inferred, from the volume of nitrogen. We convert directly into 1. AMMONIUM CHLORIDE. Ammonia gas and its aqueous solution, and also ammonium salts of weak volatile acids (ammonium carbonate, ammonium sulphide, &c.). 2. AMMONIUM PLATINIC CHLORIDE. Ammonium salts of acids soluble in alcohol, such as ammonium sulphate, ammonium phosphate, &c. 3. The methods based on the EXPULSION OF AMMONIA from ammonium compounds, and also that of inferring the amount of ammonium from the volume of nitrogen eliminated in the dry way, are equally applicable to all ammonium salts. The expulsion of ammonia in the dry way (by ignition witli soda-lime), and its estimation from the volume of nitrogen elimi- nated in the dry way, being effected in the same manner as the 218 DETERMINATION. [ 99. estimation of the nitrogen in organic compounds, I refer the stu- dent to the Section on organic analysis. Here I shall only give the methods based upon the expulsion of ammonia and of nitrogen in the wet way. For the alkalinietric estimation of free ammonia, see 195 and 196. 1. Determination as Ammonium Chloride. Evaporate the aqueous solution of the ammonium chloride on the w^ater-bath, and dry the residue at 100 until the weight remains constant ( 4-2). The results are accurate. The volatili- zation of the chloride is very trifling. A direct experiment gave 99-94 instead of 100. (See Expt. 15.) The presence of free hydrochloric acid makes no difference ; the conversion of caustic ammonia into ammonium chloride may accordingly be effected by supersaturating with hydrochloric acid. The same applies to the conversion of the carbonate, with this addition only, that the process of supersaturation must be conducted in an obliquely-placed flask, and the mixture heated in the same, till the carbonic acid is driven off. In the analysis of ammonium sulphide we proceed in the same way, taking care simply, after the expulsion of the hydrogen sulphide, and before proceeding to evaporate, to filter off the sul- phur which may have separated. Instead of weighing the ammo- nium chloride, its quantity may be inferred by the determination of its chlorine according to 14-1, n. (Coinp. potassium chloride, 97, 5, 3.) 2. Determination, as Ammonium Platinic Chloride, a. Ammoniacal salts with volatile acids. Same method as described in 97, b, 3, a (potassium platiiiic chloride). ft. Ammonium salts of non-volatile acids. Same method as described 97, b, 3, ft (potassium platinic chloride). The results obtained by these methods are accurate. If you wish to control the results,* ignite the double chloride, wrapped up in the filter, in a covered crucible, and calculate the amount of ammonium from that of the residuary platinum. The results must agree. The heat must be increased very gradually.! * If the ammonium platinic chloride is pure, which may be known by its color and general appearance, this control may be dispensed with. f The best way is to continue the application of a moderate heat for a long time, then to remove the lid, place the crucible obliquely, with the lid leaning against it, and burn the charred filter at a gradually-increased heat (H. ROSE). 99.] AMMONIUM. 219 Want of due caution in this respect is apt to lead to loss, from particles of the double salt being carried away with the ammonium chloride. Very small quantities of ammonium platinic chloride are collected on an unweighed filter, dried, and at once reduced to platinum by ignition.* 3. Estimation by Expulsion of the Ammonia in the Wet Way. This method, which is applicable in aU cases, may be effected in two different ways, viz. : a. EXPULSION OF THE AMMONIA BY DISTILLATION WITH SOLUTION OF POTASSA, or SODA, or with MILK OF LIME. Applicable in all cases where no nitrogenous organic matters from which ammonia might be evolved upon boiling with solution of potassa, &c., are present with the ammonium salts. Weigh the substance under examination in a small glass tube, three centimetres long and one wide, and put the tube, with the substance in it, into a flask containing a suitable quantity of mod- erately concentrated solution of potassa or soda, or milk of lime, from which every trace of ammonia has been removed by protracted ebullition, but which has been allowed to get thoroughly cold again ; place the flask in a slanting position on wire-gauze, and immediately connect it by means of a glass tube bent at an obtuse angle, with the glass tube of a small cooling apparatus. Connect the lower end of this tube, by means of a tight-fitting perforated cork, with a sufficiently large tubulated receiver which is in its turn connected with a U-tube by means of a bent tube passing through its tubulure. If you wish to determine voluinetrically the quantity of ammo- IL in- expelled, introduce the larger portion of a measured quantity of standard solution of acid (sulphuric, hydrochloric, or oxalic, 192), into the receiver, the remainder into the U-tube ; add to the portion of fluid in the latter a little water, and color the liquids in the receiver and U-tube red with 1 or 2 c. c. of tincture of lit- mus. The cooling-tube must not dip into the fluid in the receiver; the fluid in the ll-tube must completely fill the lower part, but it must not rise high, as otherwise the passage of air bubbles might * In a series of experiments to get the platinum from pure and perfectly anhydrous ammonium platinic chloride, by very cautious ignition, Mr. Lucius, one of my pupils, obtained from 44*1 to 44 3 per cent, of the metal, instead of 44-3. 220 DETERMINATION. [ 99. easily occasion loss by spirting. The quantity of acid used must of course be more than sufficient to fix the whole of the ammonia expelled. When the apparatus is fully arranged, and you have ascertained that all the joints are perfectly tight, heat the contents of the flask to gentle ebullition, and continue the application of the same degree of heat until the drops, as they fall into the receiver, have for some time altogether ceased to impart the least tint of blue to the portion of the fluid with which they first come in contact. Loosen the cork of the flask, allow to stand half an hour, pour the contents of the receiver and U-tube into a beaker, rinsing out with small quantities of water, determine finally with a standard solution of alkali the quantity of acid still free, which, by simple subtraction, will give the amount of acid which has combined with the ammonia ; and from this you may now calculate the amount of the latter ( 192). Kesults accurate.* If you wish to determine by the gravimetric method the quan- tity of ammonia expelled, receive the ammonia evolved in a quan- tity of hydrochloric acid more than sufficient to fix the whole of it, and determine the ammonium chloride formed, either by simple evaporation, after the directions of 1, or as ammonium platinic chloride, after the directions of 2. b. EXPULSION OF THE AMMONIA BY MILK OF LIMP:, WITHOUT APPLICATION OF HEAT. This method, recommended by SCHLOSING, is based upon the fact that an aqueous solution containing free ammonia gives off the latter completely, and in a comparatively short time, when exposed in a shallow vessel to the air, at the com- mon temperature. It finds application in cases where the presence of organic nitrogenous substances, decomposable by boiling alkalies, forbids the use of the method described in 3, a ; thus, for instance, in the estimation of the ammonia in urine, manures, &c. The fluid containing the ammonia, the volume of which must not exceed 35 c. c., is introduced into a shallow flat-bottomed ves- sel from 10 to 12 centimetres in diameter; this vessel is put on a plate filled with mercury. A tripod, made of a massive glass rod, is placed in the vessel which contains the solution of the ammonium salt, and a saucer or shallow dish with 10 c. c. of the normal solu- tion of oxalic or sulphuric acid ( 192) put on it. A beaker is now * [In thus estimating minute quantities of ammonia, the condensing tube must be of tin, since glass yields a sensible amount of alkali to hot-water vapor.] 99.] AMMONIUM. 221 inverted over the whole. The beaker is lifted up on one side as far as is required, and a sufficient quantity of milk of lime added by means of a pipette (which should not be drawn out at the lower end): The beaker is then rapidly pressed down, and weighted with a stone slab. After forty-eight hours the glass is lifted up, and a slip of moist reddened litmus paper placed in it ; if no change of color is observable, this is a sign that the expulsion of the ammo- nia is complete ; in the contrary case, the glass must be replaced. Instead of the beaker and plate with mercury, a bell-jar, with a ground and greased rim, placed air-tight on a level glass plate, may be used. A bell-jar, having at the top a tubular opening, furnished with a close-fitting glass stopper, answers the purpose best, as it permits the introduction of a slip of red litmus paper suspended from a thread ; thus enabling the operator to see whether the com- bination of the ammonia with the acid is completed, without the necessity of removing the bell-jar. According to SCHLUSIXG, forty- eight hours are always sufficient to expel O'l to 1 gramme of ammo- nia from 25 to 35 c. c. of solution. However, I caii admit this statement only as regards quantities up to 0*3 grm. ; quantities above this often require a longer time. I, therefore, always prefer operating with quantities of substance containing no more than 0-3 grm. ammonia at the most. When all the ammonia has been expelled, and has entered into combination with the acid, the quantity of acid left free is deter- mined bv means of standard solution of alkali, and the amount of the ammonia calculated from the result ( 192). 4. Estimation by Expulsion of the Nitrogen in the Wet Way. A process for determining ammonium by means of the azo- tometer has been given by "W. KNOP.* It depends on the sepa- ration of the nitrogen by a bromized and strongly alkaline solution of sodium hypochlorite.f [The simplest azotometer is that described by RUMPF.^; It * Chem. Centralbl. 1860, 244. f This is prepared as follows: Dissolve 1 part of sodium carbonate in 15 parts of water, cool the fluid with ice, saturate perfectly with chlorine,, keeping cold all the while, and add strong soda solution (of 25 per cent.) till the mixture on rubbing between the fingers makes the skin slippery. Before using, add to the quantity required for the series of experiments bromine in the proportion of 2-3 grm. to the litre, and shake. \ Fres. Zeit., VI. 398. 222 DETERMINATION. consists of a burette of 50 or 100 c. c. stationed in a glass cylinder nearly filled with mercury, and connected by a stout caoutchouc tube with a small bottle, a, fig. 49, to which is fitted a soft, thrice- perforated caoutchouc stopper. The stopper carries a thermometer and two short glass tubes, one of which joins it to the burette, and the other has attached a short bit of caoutchouc tubing and a pinch- cock, e. The weighed ammonium salt (not more than 0'4 grm.) is placed in the tube, f, with 10 c c. of water, and 50 c. c. of the bromized hypochlorite solution are brought into the bottle, a. The cock, e, being open, the stopper is firmly fixed in its place, and the burette is depressed in the mercury un- til its uppermost degree exactly coincides with the surface of the metal. The cock is then closed, and the bottle is inclined to bring the two substances in contact. The ammonium salt is speedily decomposed. When no further evolution of gas takes place the burette is so adjusted that the level of the mercury without and within it shall nearly coincide, and the operator waits 10-20 minutes, or until the thermometer in a indicates the same temperature as the sur- rounding air. Then the adjustment of the burette to exact coincidence of the mercury level, within and without, is effected, and the volume of the gas is read off. The stand of the thermometer and barometer are also noted, and the recorded volume of nitrogen is corrected by use of the tables on pp. 223 and 224-225, by DIETRICH. The first table gives a correction for the nitrogen which is absorbed by the 60 c. c. of liquid in the bottle a. The amount varies with the relative volumes of air and nitrogen, and is determined empirically by decomposing known quantities of ammonia and noting the difference between the obtained and the theoretical volume of nitrogen. The correction holds strictly, of course, only for a solution of such strength as that employed by DIETRICH and at the mean temperatures. The second table serves to spare the labor of calculation. The weight of 1 c. c. of nitrogen, measured e. g. at T54 mm. of barome- PJg. 49. 99.] TABLE OF ABSORPTION OF NITROGEN GAS. 223 1 I 1 8 T-l s 3 8 8 8 8. T-< OJ _ 1 1 Cft 10 8 5 g 2 e s o 2 9. 1 % 2 S 8 l-H 1 5 5 O 1 B 9 s s TH - 2 S 9. 1 s s? iH s 2 2 S 5 8 1 s 2 g S ^ 85 5 * ii s s S : 00 cc *-; o 1 s ^ . 1 1 5 2 : ^ W < i 224 TABLE OF WEIGHTS. [99. II. TABLE OF THE WEIGHT OF A In Milligrammes for Pressures from 720 to 770 mm/ MILLIMETRES. 720 722 724 726 728 i 730 732 I 734 I 736 I 738 ! 740 742 744 10* 1.18880 1,18699 1.14018 1.14337 1.146561.14975 1.15294 1.15613 1.16988 1.16261 1.16570 1.16889 1.17208 i i i ; - j i i 11 1.13881 1 1.18199 1.13517,1.13835 1.14153 1.144711. 14789;!. 15107 1.154241.15742 1.16060 1.16378 1.16696 i ; 12 1.12376 1.12693 1.13010J1.13326 1.13643'l.l3960 1.14277 1.14593 ! 1.14910^1. 152271. 15543 1.15860 1.16177 I ! 1.11875 1.12191 1.12506:1.12822 1.13138; 1.13454 1.13769 1.14085 1.1440l|l.l4716 1.15032 1.15348 1.15663 14 1.1186911.11684 1.1199911.1231311.12628 1. 12942 ! 1.13257 1.13572 ' 1.18886 1.14201 1.14515 1.14830 1.15145 1.10346 1.10658'1.10971'1.11283!1.115961.11908 1.12220 1.12533 1.12845'l.l3158il. 13470 1.13782J1.14095 15 1.10859(1.11172 1.11486!!. 11799 1.12113 1.12426 1.12739 1.13053 1.13366' 1.13680 1.13993 1.14306! 1.14620 I I 17 1.09828 1.10139 1.10450 1.10761 1.11078 1.li884 1.11695 1.12006 1.12317:1.12629 1.12940 1.13251; 1.13562 18 1.09304 1.09614 1.09924 i l. 10234 1.10544 1.10854 1.11165 1.11475 1.11785 1.120951.12405 1.12715 1.13025 i r- Vt - -f I 19 1.08744 1.09083 1.09392:1.09702 1.10011 1.10320 1.106291.10938 1.11248 1.11557 1.118661.12175 1.12484 | i | i j I l | i | 20|l.08246il.08554 1.08862|l.09170 1.094781.09786|1.100941. 10402 1.107101.11018 1.11327 1.11635 1.11943 i i : i 21 1.077081.080151.08322 1. 08629k 08936 J. 09243; 1.09550 1.09857 1.10165|1. 10472 1.107791. 11086 ! 1. 11393 22 1.071661. 074721.07778!l.080841.083901.08696 1.090021.09308 1.096141.09921 1.10227 1.10533 1.10839 r. i II 23 1.06616, 1.06921 1.07226 1.07531 1.078361.08141 ! 21. 1.06061 1.063651.06669 1.06973 1.07277 1.07581 i | 1.05499 1.058011.06104 1.06407 '1.06710 1.07013 1.073161.07619 1.07922 1.08225 1.08528 1.08831 1.08446 1.08751 1.09056 1.09361 1.09666 1.09971 1.078851.081891.08493 1 1.08796 1.091001.09404 1.10276 1.09708 1.09134 720 722 ! 724 726 728 730 732 734 736 738 740 742 744 MILLIMETRES. 99.] TABLE OF WEIGHTS. 225 CUBIC CENTIMETRE OF NITROGEN. of Mercury, and for Temperatures from 10 to 25 C. MILLIMETRES. 746 748 | 750 752 754 756 758 760 762 764 766 768 770 ; i 1.17527 1.17846' 1.18165 1.18484 1.18803 1.19122 1. 19441 jl. 19760 1.20079 1.20398 1.20717 1.21036 1.21355; ioi 1.17014:1.17332 1.17650 1.17168 1.18286 1.18603 1.18921J1.192394.19557 1.19875 1.201931.20511 1.20829; 11- 1.16493 1.16810 1.17127 1. 174444. 17760 1.18077 1.18394 1.18710 1.19027 1.19344 1.196601.19977 1.20294J 12 1.15979 1.16295 1.16611 1.16926 1.17242 1.17558 1.17873 1.18189 1.18505 1.18820 1.191361.19452 1.19768 13<> 1.15459 1.15774 1.16088 1.16403 1.16718 1.17032J1.17347 1.17661 1.17976 118291 1.186051.18920 1.19234 14 1.14933 1.15247 1.15560 1.15873 1.16187 1.16500 1.16814 1.17127 1.17440 1.17754 1.18067 1.18381 1.18694 15 1.144071.147201.150321.15344 1.15657 1.15969 1.16282 1.16594 1.16906 1.17219 1.17531 1.17844 1. 18156 | 16 1.13873 '1.14185 1.14496 1.14807 1.15118 1.15429 1.15741 1.16052 1.163631.16674 1.16985 1.17297 1.1700S 17- 1.13335 1.13645 1.13955 1.14266 1.14576 1.148861.15196 1.15506 ; 1.15816 1.16126 1.16436 1.16746 1.17056, 18 1.12794 1.13103 1.13412 1.13721 1.14340 1.14649 1.14958 1.15267 1.15576 1.15886 1.16195 1.16504 19 1.12251 1.12559 1.12867 1.13175 1.13483 1.13791 1.14099 1.14406;!. 14716 1.15024 1.15332 1.15640 1.15948; 20 1.11700 1.12007 1.12314 1.12621 1.12928 1.13236 1.13543 1.13850 1.14157 1.14464 1.14771 1.15078 1.15385J 21; 1 1.11145 1.11451 1.11757 1.12063 1.12369 1.12675 1.12982 1.13288 1.13594:1.13900 1.14206 1.14512 1.14818| 22 1.10581 1.10886 1.11191 1.11496 1.11801 1.12106 1,12411 1.12716 1.13021 1.133261.13631 1.13936 1.14241) 23 | 1.10012 1.10316 1.10620 1.10924 1.11228 1.11532J1.11835 1.12139 1.12443,1.12747:1.13051 .1.13355 1.13659 24 1.09437 1.09740 1.10043 1.10346 1.10649 1.10952 1.11255 1.11558 1.11861 1.12164 1.12467 1.12770 1.13073J 25 ] 746 748 750 752 754 756 758 760 762 764 766 768 770 MILLIMETRES. 226 DETERMINATION. [ 100. ter and 15 C., is found at the intersection of the vertical column 754 with the horizontal column 15, is, viz., 1-16187. To the observed volume of nitrogen add the amount absorbed as per Table L, and correct the total by Table II. It scarcely requires to be mentioned that good results can only be obtained in an apartment where the temperature is uniform, and when care is exercised to avoid warming the apparatus in handling. See DIET- KICH'S papers.* 100. Supplement to the First Group. LITHIUM. In the absence of other bases, lithium may, like potassium and sodium, be converted into anhydrous SULPHATE, and weighed in that form (Li 2 SO 4 ). As lithium forms no acid sulphate, the excess of sulphuric acid may be readily removed by simple igni- tion. LITHIUM CARBONATE also, which is difficultly soluble in water, and fuses at a- red heat without suffering decomposition, is well suited for weighing ; whilst lithium chloride, which deliquesces in the air, and is by ignition in moist air converted into hydro- chloric acid and lithium oxide, is unfit for the estimation of lithium. In presence of other alkali metals, lithium is best converted into LITHIUM PHOSPHATE (Li 3 PO 4 ), and weighed in that form. This is effected by the following process: add to the solution a sufficient quantity of sodium phosphate (which must be perfectly free from phosphates of the alkali-earth metals), and enough soda* to keep the reaction alkaline, and evaporate the mixture to dry ness ; pour water over the residue, in sufficient quantity to dissolve the soluble salts with the aid of a gentle heat, add an equal volume of solution of ammonia, "digest at a gentle heat, filter after twelve hours, and wash the precipitate with a mixture of equal volumes of water and solution of ammonia. Evaporate the filtrate and first washings to dryness, and treat the residue in the same way as before. If some more lithium phosphate is thereby obtained, add this to the prin- cipal quantity. The process gives, on an average, 99*61 for 100 parts of lithium oxide. * Fres. Zeit. III. 162; IV. 141, and V. 36. 101.] BARIUM. 227 If the quantity of lithium present is relatively very small, the larger portion of the potassa or soda compounds should first be removed by addition of absolute alcohol to the most highly con- centrated solution of the salts (chlorides, bromides, iodides, or nitrates, but not sulphates) ; since this, by lessening the amount of water required to effect the separation of the lithium phosphate from the soluble salts, will prevent loss of lithium (W. MAYER).* The precipitated normal lithium phosphate has the formula 2Li 3 PO 4 + H 3 O. It dissolves in 2539 parts of pure, and 3920 parts of ammoniated water ; at 100, it completely loses its water ; if pure, it does not cake at a moderate red heat (MAYER). The objections raised by KAMMELSBERof to MAYER'S method of estimating lithia I find to be ungrounded. According to my own experience, it appears that the filtrate and wash- water must be evaporated in a platinum dish not only once, but at least twice in fact, till a residue is obtained which is completely soluble in dilute ammonia. Lithium phosphate may be dried at 100, or ignited according to 53, before being weighed. In the latter case, care must be taken to free the filter as much as possible from the precipitate before proceeding to incinerate it. I have thus obtained, J instead of 100 parts lithium carbonate, by drying at 100, 99-84, 99-89, 100-41, by "igniting 99*66 and 100-05. The lithium phosphate obtained was free from sodium. Second Group. BARIUM STRONTIUM CALCIUM MAGNESIUM. 101. 1. BARIUM. a. Solution. Caustic baryta is soluble in water, as are many barium salts. Barium salts which are insoluble in water are, with almost the single exception of the sulphate, readily dissolved by dilute hydro- chloric acid. The solution of the sulphate is effected by fusion with sodium carbonate, &c. (See 132.) * Annal. der Chem. u. Pharm. 98, 193, where Mayer has also demonstrated the non-existence of a sodium lithium phosphate of fixed composition (Berzelius), or of varying composition (Rammelsberg). f Pogg. Annal. 102, 443. \ Zeitschr. f. Analyt. Chem. 1, 42. 228 DETERMINATION. [ 101. b. Determination. Barium is weighed either as sulphate or as carbonate, rarely (in the separation from strontia) as barium silico-fluoride ( 71). Barium oxide or hydroxide, also barium carbonate, may also be determined by the volumetric (alkalimetric) method. Comp. 198. We may convert into 1. BARIUM SULPHATE. a. By Precipitation. b. By Evaporation*. All barium compounds with- All barium salts of volatile out exception. acids, if no other non-volatile body is present. 2. BAKIUM CARBONATE. a. All barium salts soluble in water. b. Barium salts of organic acids. Barium is both precipitated and weighed, by far the most fre- quently as sulphate, the more so as this is the form in which it is most conveniently separated from other bases. The determination by means of evaporation (1, b) is, in cases where it can be applied, and where we are not obliged to evaporate large quantities of fluid, very exact and convenient. Barium is determined as carbonate in the wet way, when from any reason it is not possible or not desir- able to precipitate it as sulphate. If a fluid or dry substance con- tains bodies which impede the precipitation of barium as sulphate or carbonate (alkali citrates, metaphosphoric acid, see 71, a and b\ such bodies must of course be got rid of, before proceeding to precipitation. 1. Determination as Barium, Sulphate. a. By Precipitation. Heat the moderately dilute solution of barium, which must not contain too much free acid (and must, therefore, if necessary, first be freed therefrom by evaporation or addition of sodium carbo- nate), in a platinum or porcelain dish, or in a glass vessel, to incipi- ent ebullition, add dilute sulphuric acid, as long as a precipitate forms, keep the mixture for some time at a temperature very near the boiling point, stirring if not on a water-bath, and allow the precipitate to subside ; decant the almost clear supernatant fluid on a filter, boil the precipitate once with water and a little dilute sul- 101.] BARIUM. 229 phuric acid, then three or four times with water, then transfer it to the filter, and wash with boiling water, until the filtrate is no longer rendered turbid by barium chloride. Dry the precipitate, and treat it as directed in 53. If the precipitate has been properly washed in the manner here directed, it is perfectly pure. In the presence of alkali salts, however, the precipitate will still contain small quantities of alkali sulphate. b. By Evaporation. Add to the solution, in a weighed platinum dish, pure sulphuric acid very slightly in excess, and evaporate on the water-bath; expel the excess of sulphuric acid by cautious application of heat, and ignite the residue. For the properties of barium sulphate, see 71. Both methods, if properly and carefully executed, give almost absolutely accurate results. 2. Determination as Barium Carbonate. a. In Solutions. Mix the moderately dilute solution of the barium salt in a beaker with ammonia, add ammonium carbonate in slight excess, and let the mixture stand several hours in a warm place. Filter, wash the precipitate with water mixed with a little ammonia, dry, fljid ignite ( 53). For the properties of the precipitate, see 71. This method involves a trifling loss of substance, as barium carbonate is not absolutely insoluble in water. The direct experiment, No. 62, gave 99-79 instead of 100. If the solution contains a notable quantity of ammonium salts, the loss incurred is much more considerable, since the presence of such salts greatly increases the solubility of barium carbonate. b. In Barium Salts of Organic Acids. Heat the salt slowly in a covered platinum crucible, until' no more fumes are evolved; place the crucible obliquely, with the lid leaning against it, and ignite, until the whole of the carbon is consumed, and the residue presents a perfectly white appear- ance : moisten the residue with a concentrated solution of ammo- nium carbonate, evaporate, ignite gently, and weigh. The results obtained by this method are quite satisfactory. A direct experi- ment, No. 63, gave 99'61 instead of 100. The loss of substance which almost invariably attends this method is owing to particles 230 DETERMINATION. [ 102. of the salt being carried away with the fumes evolved upon igni- tion, and is accordingly the less considerable, the more slowly and gradually the heat is increased. Omission of the moistening of the residue with ammonium carbonate would involve a further loss of substance, as the ignition of barium carbonate in contact with carbon is attended with formation of some caustic baryta, carbon monoxide gas being evolved. 102. 2. STRONTIUM. a. Solution. See the preceding paragraph ( 101, a. Solution of baryta and barium salts), the directions there given apply equally here. b. Determination. Strontium is weighed either as strontium sulphate or as stron- tium carbonate ( 72). Strontium in the form of oxide, hydrox- ide, or carbonate, may be determined also by the volumetric (alkalimetric) method. Comp. 198. We may convert into 1. STRONTIUM SULPHATE. a. J3y Precipitation. All compounds of strontium without exception. ft. By' Evaporation. All strontium salts of volatile acids, if 110 other non-volatile body is present. 2. STRONTIUM CARBONATE. a. All strontium compounds soluble in water. /3. Strontium salts of organic acids. The method based on the precipitation of strontium with sul- phuric acid yields accurate results only in cases where the fluid from which the strontium is to be precipitated may be mixed, without injury, with alcohol. Where this cannot be done, and where the method based on the evaporation of the solution of strontium with sulphuric acid is equally inapplicable, the conver- sion into the carbonate ought to be resorted to in preference, if admissible. As in the case of barium, so here, we have to be on our guard against the presence of substances which would impede precipitation. 102.] STRONTIUM. 231 1. Determination as Strontium Sulphate. a. By Precipitation. Mix the solution of the strontium salt (which must not be too dilute, nor contain much free hydrochloric or nitric acid) with dilute sulphuric acid in excess, in a beaker, and add at least an equal volume of alcohol; let the mixture stand twelve hours, and filter ; wash the precipitate with dilute alcohol, dry and ignite ( 53). If the circumstances of the case prevent the use of alcohol, the fluid must be precipitated in a tolerably concentrated state, allowed to stand in the cold for at least twenty-four hours, filtered, and the precipitate washed with cold water, until the last rinsings manifest no longer an acid reaction, and leave no perceptible residue upon evaporation. If traces of free sulphuric acid remain adhering to the filter, the latter turns black on drying, and crumbles to pieces ; too protracted washing of the precipitate, on the other hand, tends to increase the loss of substance. Care must be taken that the precipitate be thoroughly dry, before proceeding to ignite it ; otherwise it will be apt to throw off fine particles during the latter process. The filter, which is to be burnt apart from the precipitate, must be as clean as possible, or some loss of substance will be incurred ; as may be clearly seen from the depth of the carmine tint of the flame with which the filter burns if the precipitate has not been properly removed. For the properties of the precipitate, see 72. When alcohol is used and the directions given are properly adhered to, the results are very accurate ; when the sulphate of strontium is precipitated from an aqueous solution, on the contrary, a certain amount of loss is unavoidable, as strontium sulphate is not absolutely insoluble in water. The direct experiments, No. 64, gave only 98'12 and 98*02 instead of 100. However, the error may be rectified, by calculat- ing the amount of strontium sulphate dissolved in the filtrate and the wash-water, basing the calculation upon the known degree of solubility of strontium sulphate in pure and acidified water. See Expt. No. 65, which, with this correction, gave 99'77 instead of 100. The necessity for making the correction may be obviated by washing with 1 part sulphuric acid mixed with 20 parts water till all substances precipitable by alcohol are removed, then with alco- hol till all the sulphuric acid is removed. Strontium sulphate also carries down sulphates of other strong bases in small quantities. 232 DETERMINATION. [ 103. b. By Evaporation. The same method as described for barium, 101, 1, b. 2. Determination as Strontium Carbonate. a. In Solutions. The same method as described 101, 2, a. For the proper- ties of the precipitate, see 72. The method gives very accurate results, as strontium carbonate is nearly absolutely insoluble in water containing ammonia and ammonium carbonate. A direct experiment, No. 66, gave 99*82 instead of 100. Presence of ammonium salts exercises here a less adverse influence than the precipitation of barium carbonate. b. In Salts of Organic Acids. The same method as described 101, 2, b. The remarks made there, respecting the accuracy of the results, apply equally here. 103. 3. CALCIUM. a. Solution. See 101, a. Solution of barium. Calcium fluoride is, by means of sulphuric acid, converted into calcium sulphate, and the latter again, if necessary, decomposed by boiling or fusing with an alkali carbonate (132). [Calcium sulphate dissolves readily in moderately dilute hydrochloric acid. It is much less soluble in strong hydrochloric acid.] b. Determination. Calcium is weighed either as calcium sulphate, as calcium carbonate, or calcium oxide ( 73). Calcium in the form of oxide, hydroxide, or carbonate, may be determined also by the volumetric (alkalimetric) method. Comp. 198.' We may convert into 1. CALCIUM SULPHATE. a. By Precipitation. All calcium salts of acids soluble in alcohol, provided no other substance insoluble in alcohol be present. b. By Evaporation. All calcium salts of volatile acids, provided no non- volatile body be present. 103.] ( ALCIUM. 233 2. CALCIUM CARBONATE. a. By Precipitation with Ammon Carbonate. All calcium salts soluble in water. b. By Precipitation with A nun oitium, Oxalate. All calcium salts soluble in water or in hydrochloric acid with- out exception. c. By Ignition. ( 'alcium salts of organic acids. Of these several methods, 2, b (precipitation with ammonium oxalate) is the one most frequently resorted to. This, and the method 1, J, give the most accurate results. The method, 1, a, is usually resorted to only to effect the separation of calcium from other basic radicals ; 2, #, generally only to effect the separation of calcium together with the other alkali-earth metals from the alkalies. As many bodies (alkali citrates, and metaphosphates) interfere with the precipitation of calcium by the precipitants given, these, if present, must be first removed. 1. Determination of Calcium Sulphate. a. By Precipitation. Mix the solution of calcium salt in a beaker, with dilute sul- phuric acid in excess, and add twice the volume of alcohol ; let the mixture stand twelve hours, filter, and thoroughly wash the precipitate with alcohol, dry. and ignite moderately ( 53). For the properties of the precipitate, see 73. The results are very accurate. A direct experiment, No. 67, gave 99'64 instead of 100. b. By Evaporation. The same method as described 101, 1, b. 2. Determination as Calcium Carbonate or Calcium Oxide. a. By Precipitation with Ammonium Carbonate. The same method as described 101, 2, a. The precipitate can be most conveniently weighed as calcium carbonate. It must be exposed only to a very gentle red heat, but this must be con- tinued for some time. For the properties of the precipitate, see 73. This method gives very accurate results, the loss of substance incurred being hardly worth mentioning. If the solution contains ammonium chloride or similar ammo- 234 DETERMINATION. [ 103. niurn salts in considerable proportion, the loss of substance incurred is far greater. The same is the case if the precipitate is washed with pure instead of ammoniacal water. A direct experiment, No. 68, in which pure water was used, gave 99*17 instead of 100 parts of lime. J. J3y Precipitation with A.?nnionium Oxalate. a. The Calcium Salt is soluble in Water. To the hot solution in a beaker, add ammonium oxalate in moderate excess, and then ammonia sufficient to impart an ammo- niacal smell to the fluid; cover the glass, and let it stand in a warm place until the precipitate has completely subsided, which will require twelve hours, at least. Pour the clear fluid gently and cautiously, so as to leave the precipitate undisturbed, on a filter ; wash the precipitate two or three times by decantation with hot water ; lastly, transfer the precipitate also to the filter, by rinsing with hot water, taking care, before the addition of a fresh portion, to wait until the fluid has completely passed through the filter. Small particles of the precipitate, adhering firmly to the glass, are removed with a feather. If this fails to effect their complete removal, they should be dissolved in a few drops of highly dilute hydrochloric acid, ammonia added to the solution, and the oxalate obtained added to the first precipitate. Deviations from the rules laid down here will generally give rise to the passing of a turbid fluid through the filter. After having washed the precipitate, dry it on the filter in the funnel, and transfer the dry precipitate to a platinum crucible, taking care to remove it as completely as possible from the filter; burn the filter on a piece of platinum wire, letting the ash drop into the hollow of the lid ; put the latter, now inverted, on the crucible, so that the filter ash may not mix with the precipitate ; heat at first very gently, then more strongly, until the bottom of the crucible is heated to very faint redness. Keep it at that temperature from ten to fifteen minutes, removing the lid from time to time. I am accustomed during this operation to move the lamp backwards and forwards under the crucible with the hand, since, if you allow it to stand, the heat may very easily get too high. Finally allow to cool in the desic- cator and weigh. After weighing, moisten the contents of the crucible, which must be perfectly white, or barely show the least tinge of gray, with a little water, and test this after a time with a 103.] CALCIUM. 235 minute slip of turmeric paper. Should the paper turn brown a sign that the heat applied was too strong rinse off the fluid adhering to the paper with a little water into the crucible, throw in a small lump of pure ammonium carbonate, evaporate to dry- ness (best in the water-bath), heat to very faint redness, and weigh the residue. If the weight has increased, repeat the same opera- tion until the weight remains constant. This method gives nearly absolutely accurate results; and if the application of heat is properly managed, there is no need of the tedious evaporation with ammonium carbonate. A direct experiment, No. 69, gave 99-99 instead of 100. If a gas blowpipe is at hand, or any other arrangement by means of which a platinum crucible may be raised to a white heat, the calcium oxalate may be converted into CAUSTIC LIME with results almost equally accurate; and I believe that this method, which requires less patience than the other, is more certain to yield good results in the hands of many persons. The calcium oxalate and the filte^ ash are transferred to a moderate-sized platinum crucible, which is ignited first over the BI.NSKX. and then over the blowpipe. The crucible is then weighed, and ignited again over the blowpipe. The second ignition over the blowpipe should not reduce the weight. The duration of the ignition necessary varies from 5 to 15 or more minutes, according to intensity of heat and quantity of the precipitate. It is well to weigh the empty crucible again at the end of the operation, as platinum sometimes loses weight after violent and prolonged ignition. The results obtained by FRITZSCHE, COSSA,* and SOUCHAY scarcely differ from the calcu- lated numbers. For properties of calcium oxide, see 73. The calcium oxalate may also be converted into SULPHATE. SCHROTTER ignites in a covered platinum crucible with pure ammo- nium sulphate. Or you may ignite in a covered platinum dish till the precipitate is for the most part converted into oxide, add a little water, then hydrochloric acid to effect solution, then pure .sulphuric acid in excess, evaporate and ignite moderately. This process is also quite accurate. Instead of converting calcium oxalate into carbonate or oxide for weighing, the quantity of calcium present in the salt may be determined also by two different volumetric methods. * FRITZSCHE (Zeitschr. f. anal. Chem. 3, 179) and A. COSSA (Ib. 8, 141). 236 DETERMINATION. [ a. Ignite the oxalate T converting it thus into a mixture of cal- cium carbonate and oxide, and determine the quantity of the cal- cium by the alkalimetric method described in 198 ; or, b. Determine the oxalic acid in the well-washed but still moist calcium oxalate by means of potassium permanganate ( 137). With proper care, both these volumetric methods give as accu- rate results as those obtained by weighing. (Comp. Expt. No. 71.) They deserve to be recommended more particularly in cases- where an entire series of quantitative estimations of calcium has to be made. Under certain circumstances it may also prove advantageous to precipitate calcium with a measured quantity of a standard solution of oxalic acid, filter, and determine the excess of oxalic acid in the filtrate, or an aliquot part of the same. (KRAUT.*) /?. The Salt is insoluble in Water. Dissolve the salt in dilute hydrochloric acid. If the acid of the calcium salt is of a nature to escape in this operation (e.g., cai bonic acid), or to admit of its separation by evaporation (e.g., silicic acid), proceed, after the removal of the acid, as directed in a. But if the acid cannot thus be readily got rid of (e.g., phosphoric acid), proceed as follows : Add ammonia until a precipitate begins to form, re-dissolve this with a drop of hydrochloric acid, add ammo- nium oxalate in excess, and finally sodium acetate; allow the precipitate to subside, and proceed for the remainder of the opera- tion as directed in a. In this process the free hydrochloric acid present reacts on the sodium acetate and ammonium oxalate, forming sodium and ammonium chlorides, with liberation of a corresponding amount of oxalic and acetic acids in which calcium oxalate is nearly insoluble. The method yields accurate results. A direct experiment, No. 72, gave 99'78 instead of 100. c. By Ignition. The same method as described 101, 2, b (barium). The resi- due remaining upon evaporation with ammonium carbonate (which operation it is advisable to perform twice) must be ignited very gently. The remarks made in 101, 2, #, in reference to the accuracy of the results, apply equally here. By way of control, the calcium carbonate may be converted into oxide or into calcium sulphate (see 5, <*), or it may be determined alkalimetrically ( 198). * Chem. Centralblatt, 1856, 316. ;> 104.] MAGNESIUM. 237 104. 4. MAGNESIUM. a. Solution. Many magnesium salts are soluble in water ; those which are insoluble in that menstruum dissolve in hydrochloric acid, with the exception of some silicates and aluminates. I. Determination. Magnesium is weighed ( 74) either as sulphate or as pyro- phozphate, or as magnesium oxide. In the form of oxide or car- bonate, it may be determined also by the alkalimetric method described in 198. We may convert into 1. MAGNESIUM SULPHATE. a. Directly. b. Indirectly. All magnesium salts of vola- All magnesium salts soluble tile acids, provided no other in water, and also those which, non- volatile substance be pres- insoluble in that menstruum, ii t. dissolve in hydrochloric acid, with separation of their acid (provided no ammonium salts be present). 2. MAGNESIUM PYROPHOSPHATE. All magnesium compounds without exception. 3. MAGNESIUM OXIDE. a. Magnesium salts of organic acids, or of readily volatile inor- ganic oxygen acids. b. Magnesium chloride, and magnesium compounds convertible into that salt. . The direct determination as magnesium sulphate is highly recommended in all cases where it is applicable. The indirect con- version into the sulphate serves only in the case of certain separa- tions, and is hardly ever had recourse to where it can possibly be avoided. The determination as pyrophosphate is most generally resorted to ; especially also in the separation of magnesium from other bases. The method based on the conversion of magnesium chloride into oxide is usually resorted to only to effect the separa- 238 DETERMINATION. [ 104. tion of magnesium from the alkali metals. Magnesium phosphates are analyzed as 135 directs. 1. Determination as Magnesium Sulphate. Add to the solution excess of pure dilute sulphuric acid, evapo- rate to dryness, in a weighed platinum dish, on the water-bath ; then heat at lirst cautiously, afterwards, with the cover on more strongly here it is advisable to place the lamp so that the flame may play obliquely on the cover from above until the excess of sulphuric acid is completely expelled ; lastly, ignite gently over the lamp for some time; allow to cool, and weigh. Should no fumes of hydrated sulphuric acid escape upon the application of a strongish heat, this may be looked upon as a sure sign that the sulphuric acid has not been added in sufficient quantity, in which case, after allowing to cool, a fresh portion of sulphuric acid is added. The method yields very accurate results. Care must be taken not to use a very large excess of sulphuric acid. The resi- due must be exposed to a moderate red heat only, and weighed rapidly. For the properties of the residue, see 74. 2. Determination as Magnesium Pyrophosphate.. The solution of the magnesium salt is mixed, in a beaker, with ammonium chloride, and ammonia added in slight excess. Should a precipitate form upon the addition of ammonia, this may be con- sidered a sign that a sufficient amount of ammonium chloride has not been used ; a fresh amount of that salt must consequently be added, sufficient to effect the re-solution of the precipitate formed. The clear fluid is then mixed w T ith a solution of sodium phosphate or sodium ammonium phosphate* in excess, and the mixture stirred, taking care to avoid touching the sides of the beaker with the stir- ring-rod ; otherwise particles of the precipitate are apt to adhere so firmly to the rubbed parts of the beaker, that it will be found difficult to remove them ; the beaker is then covered, and allowed to stand at rest for twelve hours, without warming ; after that time the fluid is filtered, and the precipitate collected on the filter, the last particles of it being rinsed out of the glass with a portion of the filtrate, with the aid of a feather ; when the fluid has completely passed through, the precipitate is washed with a mixture of 3 parts of water, and 1 part of solution of ammonia of 0*96 sp. gr., the * According to MOHB (NaNH 4 H)PO4 is preferable to (Na 2 H)PO 4 as a pre- cipitant. (See Zeitschr. f. Anal. Chem. 12, 36.) 104.1 MAGNESIUM. 239 operation being continued until a few drops of the fluid passing through the filter mixed with nitric acid and a drop of silver nitrate show only a very slight opalescence. The precipitate is now thoroughly dried, and then transferred to a platinum crucible ( 53); the latter, with the lid on, is exposed for some time to a very gentle heat, which is finally increased to intense redness. The filter, as clean as practicable, is incinerated in a spiral of platinum wire, and the ash transferred to the cru- cible, which is then once more exposed to a red heat, allowed to cool, and weighed. If the magnesium pyrophosphate is dark colored, moisten with a few drops of nitric acid, warm till dry, and ignite again. For the properties of the precipitate and residue, see 74. This method, if properly executed, yields most accurate results. The precipitate must be washed completely, but not over-washed, and the washing water must always contain the requisite quantity of ammonia. Direct experiments, No. 73, a and 5, gave respectively 100-43 and 100-30 instead of 100. 3. Determination as Magnesium Oxide. a. In Magnesium Salts of Organic or Volatile Inorganic Acid*. The magnesium salt is gently heated in a covered platinum crucible, increasing the temperature gradually, until no more fumes escape ; the lid is then removed, and the crucible placed in an oblique position, with the lid leaning against it. A red heat is now applied, until the residue is perfectly white. For the prop- erties of the residue, see 74. The method gives the more accu- rate results the more slowly the salt is heated from the beginning. Some loss of substance is usually sustained, owing to traces of the salt being carried off with the empyreumatic products. Mag- nesium salts of readily volatile oxygen acids (carbonic acid, nitric acid), may be transformed into magnesium oxide in a similar way, by simple ignition. Even magnesium sulphate loses the whole of its sulphuric acid when exposed, in a platinum crucible, to the heat of the gas blowpipe-flame (SONNENSCHEIN). As regards small quan- tities of magnesium sulphate, I can fully confirm this statement. b. Conversion of Magnesium Chloride into Magnesium Oxide. See ^ 153. 4, y. 240 DETERMINATION. [ 105. THIRD GROUP OF BASIC RADICALS. AL UMINI UM C H ROMIUM (TITANIUM). 105. 1. ALUMINIUM. a. Solution. Aluminium compounds which are insoluble in water, dissolve, for the most part, in hydrochloric acid. Native crystallized alu- minium oxide (sapphire, ruby, corundum, &c.), and many native aluminium compounds, and also artificially produced aluminium oxide after intense ignition, require fusing with sodium carbonate, caustic potassa, or barium hydroxide, as a preliminary step to their solution in hydrochloric acid. Many aluminium compounds which resist the action of concentrated hydrochloric acid, may be decom- posed by protracted heating with moderately concentrated sul- phuric acid, or by fusion with potassium disulphate ; e.g., common clay. b. Determination. Aluminium is invariably weighed as aluminium oxide ( 75). The several aluminium salts are converted into aluminium oxide, either by precipitation as aluminium hydroxide, and subsequent ignition, or by simple ignition. Precipitation as basic acetate or basic formate is resorted to only in cases of separation. We may convert into ALUMINIUM OXIDE. a. By Precipitation. b. By Heating or Ignition. All aluminium salts soluble a. All aluminium salts of in water, and those which, insolu- readily volatile oxygen acids ble in that menstruum, dissolve (e.g., aluminium nitrate). in hydrochloric acid, with sepa- /?. All aluminium salts of ration of their acid. organic acids. With regard to the method a, it must be remembered that the solution must contain no organic substances, which would inter- fere with the precipitation e.g., tartaric acid, sugar, &c. Should such be present, the solution must be mixed with sodium carbo- nate and potassium nitrate, evaporated to dryness in a platinum dish, the residue fused, then softened with water, transferred to a 105.] ALUMINIUM. 241 beaker, digested with hydrochloric acid, and the solution filtered, and then, but not before, precipitated. The methods , a and ft, are applicable only in cases where no other fixed substances are present. The methods of determining aluminium in its combinations with phosphoric, boracic, silicic, and chromic acids, will be found in Part II. of this Section, under the heads of these several acids. Determination as Aluminium Oxide. a. By Precipitation. Mix the moderately dilute hot solution of the aluminium salt, in a beaker or dish, with a tolerable quantity of ammonium chlo- ride, if that salt is not already present ; add ammonia slightly in excess, boil gently till the fluid gives a neutral or barely alkaline reaction (the fluid adhering to the test paper must be washed back). The fluid must not be heated too long, or it may become acid through decomposition of ammonium chloride, and some of the precipitate may redissolve ; allow to settle ; then decant the clear supernatant fluid on to a filter, taking care not to disturb the pre- cipitate ; pour boiling water on the latter in the beaker, stir, let the precipitate subside, decant again, and repeat this operation of washing by decantation a second and a third time; transfer the precipitate now to the filter, finish the washing with boiling water, dry thoroughly, ignite ( 52), and weigh. The heat applied should be very gentle at first, and the crucible kept well covered, to guard against the risk of loss of substance from spirting, which is always to be apprehended if the precipitate is not thoroughly dry ; towards the end of the process the heat should be raised to intense redness. In the case of aluminium sulphate the foregoing process is apt to leave some sulphuric acid in the precipitate, which, of course, vitiates the result. To insure the removal of this sulphuric acid, the precipitate should be exposed for 510 min. to the heat of the gas blowpipe flame. If there are difficulties in the way, prevent- ing this proceeding, the precipitate, either simply washed or mod- erately ignited, must be re-dissolved in hydrochloric acid (wliich requires protracted warming with strong acid), and then precipi- tated again with ammonia ; or the sulphate must first be converted into nitrate by decomposing it with lead nitrate, added in very slight excess, the excess of lead removed by means of hydrostil- phuric acid, and the further process conducted according to the 242 DETERMINATION. [ 106. directions of a or J. For the properties of aluminium hydroxide and ignited aluminium oxide, see 75. The method, if properly executed, gives very accurate results. But if a considerable excess of ammonia is used, more particularly in the absence of ammo- nium salts, and the liquid is filtered without boiling or long stand- ing in a warm place to remove the ammonia, no trifling loss may be incurred. This loss is the greater, the more dilute the solution, and the larger the excess of ammonia. The precipitate cannot well be sufficiently washed on the filter on account of its gelatinous nature ; on the other hand, if it be entirely washed by decantation, a very large quantity of wash-water must be used, hence it is advis- able to combine the two methods, as directed.* In case the BUNSEN filtering apparatus is used for washing aluminium hydroxide, for which operation it is particularly desirable, the precipitate may be brought into the filter without washing by decantation, and may be ignited without previous drying. See 53, b. b. By Ignition. a. Aluminium Salts of Volatile Oxygen Acids. Ignite the salt (or the residue of the evaporated solution) in a platinum crucible, gently at first, then gradually to the very high- est degree of intensity, until the weight remains constant. For the properties of the residue, see 75. Its purity must be care- fully tested. There are no sources of error. ft. AliwYiinium Salts of Organic Acids. The same method as described 104, 3, a (Magnesium). 106. 2. CHROMIUM. a. Solution. Many chromic salts are soluble in water. Chromic hydroxide, and most of the salts insoluble in water, dissolve in hydrochloric acid. Ignition renders chromic oxide and many chromium salts insoluble in acids ; this insoluble modification must be prepared for * [When a solution of aluminium hydroxide in potassium or sodium hydrox- ide is boiled with excess of ammonium chloride, the aluminium separates com- pletely as a hydrated oxide with two mol. of water, which may be washed with comparative ease. In certain cases, as where aluminium is separated from ferric iron by boiling their hydroxides with soda, this fact may be taken advantage of. LOWE, Fres. Zeitschrift, IV. 315.] 106.] CHROMIUM. 243 solution in hydrochloric acid, by fusing with 3 or 4 parts of potassa. In the process of fusing a small quantity of potassium chromate is formed by the action of air; this, however, can be decomposed by heating with hydrochloric acid with formation of chromic chloride. Addition of alcohol greatly promotes the reduction to chromic chloride. Instead of this fusing with potassa, we frequently prefer to adopt a treatment, whereby the chromium is at once oxidized and converted into an alkali chromate (see 2). For the solution of chromic iron, see 160. b. Determination. Chromium is always, when directly determined, weighed as chromic oxide. It is brought into this form either by precipitation as hydroxide and ignition, or by simple ignition. It may, how- ever, also be estimated, by conversion into chromic acid, and deter- mination as such. We may convert into 1. CHROMIC OXIDE. a. By Precipitation. b. By Ignition. All chromic salts soluble in a. All chromic salts of vola- water, and also those which, in- tile oxygen acids, provided no soluble in that menstruum, dis- non-volatile substances be pres- solve in hydrochloric acid, with ent. separation of their acid. Pro- fi. Chromic salts of organic vided always that no organic acids, substances (such as tartaric acid, oxalic acid, &c.) which interfere with the precipitation be present. 2. CHROMIC ACID, or. more correctly speaking, ALKALI CHROMATE. Chromic oxide and all chromic salts. The methods of analyzing chromic phosphates, borates, silicates, and chromic chromate, will be found in Part II. of this Section, under the heads of the several acids of these compounds. 1. Determination as Chromic Oxide. a. By Precipitation. The solution, which must not be too highly concentrated, is heated to 100 in a platinum or porcelain dish. If the precipita- tion is effected in a glass vessel, considerable error is caused by contamination of the precipitate with silica. If porcelain is used, 244 DETERMINATION. [ 106. this error is slight. Ammonia is then added slightly in excess, and the mixture exposed to a temperature approaching boiling, until the fluid over the precipitate is perfectly colorless, presenting no longer the least shade of red ; let the solid particles subside, wash three times by decantation, and lastly on the filter, with hot water, dry thoroughly, and ignite ( 52). The heat in the latter process must be increased gradually, and the crucible kept covered, other- wise some loss of substance is likely to arise from spirting upon the incandescence of the chromic oxide which marks the passing of the soluble into the insoluble modification. For the properties of the precipitate and residue, see 76. This method, if properly executed, gives accurate results. b. By Ignition. a. Chromic salts of Volatile Oxygen Acids. The same method as described, 105, Z>, a (Aluminium). 1). Chromic salts of Organic Acids. The same method as described, 104, 3, a (Magnesium). 2. CONVERSION OF CHROMIUM IN CHROMIC COMPOUNDS INTO ALKALI CHROMATE. (For the estimation of chromic*acid, see 130.) The following methods have been proposed with this view : a. The solution of the chromic salt is mixed with solution of potassa or soda in excess, until the chromic hydroxide, which forms at first, is redissolved. Chlorine gas is then conducted into the cold fluid until it acquires a yellowish-red tint ; it is then mixed with potassa or soda in excess, and the mixture evaporated to dry- ness ; the residue is ignited in a platinum crucible. The whole of the potassium (or sodium) chlorate formed is decomposed by this process, and the residue consists, therefore, now of an alkali chro- mate and potassium (or sodium) chloride. (YoHL.) 1). Potassium hydroxide is heated in a silver crucible to calm fusion ; the heat is then somewhat moderated, and the perfectly dry chromic compound projected into the crucible. When the substance is thoroughly moistened with the potassa, small lumps of fused potassium chlorate are added. A lively effervescence ensues, from the escape of oxygen ; at the same time the mass acquires a more and more yellow color, and finally becomes clear and trans- parent. Loss of substance must be carefully guarded against (II. SCHWABZ). 107.] TITANIUM. 245 c. Dissolve chromic hydroxide in solution of potassa or soda, add lead dioxide in sufficient excess, and warm. The yellow fluid produced contains all the chromium as lead chromate in alkaline solution. Filter from the excess of lead dioxide, add to the filtrate acetic acid to acid reaction, and determine the weight of the pre- cipitated lead chromate (G. CHANCEL*). \KTKUM1NATION. [ 112. b. Determination. Ferrous iron may be estimated 1, by dissolving, converting into ferric iron, and determining the latter gravimetrically or volu- , metrically; 2, by precipitating as sulphide, and weighing it as such, or determining it after conversion into a ferric salt ; 3, by a direct volumetric method. The methods 1 and 2 are, of course, only applicable when no ferric compound is present; the method 2 is scarcely ever used except for separations. The methods included under 3 are adapted to most cases, and, in absence of other reducing substances, are especially worthy of recommendation. As the determination of iron as ferric oxide belongs to 113, and as the process for precipitating ferrous iron as sulphide is the same as that for precipitating ferric iron in this form, nothing remains for us here but to describe the methods of converting ferrous into ferric salts and the processes included under 3. . 1. Methods of converting Ferrous into Ferric Iron. a. Methods, applicable in all cases. Heat the solution of the ferrous salt with hydrochloric acid and add small portions of potassium chlorate, till the fluid, even after warming for some time, still smells strongly of chlorine. Our object may be also attained by passing chlorine gas or in the case of small quantities by addition of chlorine water, or very con- veniently by adding solution of bromine in hydrochloric acid. If the solution is required to be free from excess of chlorine or bromine, it is finally heated, till all odor of chlorine or bromine has disappeared. h. Methods which are only suitable when the iron is to be subse- quently precipitated hy ammonia* as ferric hydroxide. Mix the solution of the ferrous salt in a flask with a little hydrochloric acid, if it does not already contain any ; add some nitric acid, and heat the mixture for some time to incipient ebulli- tion. The color of the fluid will show whether the nitric acid has been added in sufficient quantity. Though an excess of nitric acid does no harm, still it is better to avoid adding too much on account of the subsequent precipitation. In concentrated solutions, the addition of nitric acid produces a dark-brown color, which disap- pears upon heating. This color is owing to the nitrogen dioxide 112.] FEKKOUS IIJOX. 267 (N 2 O 2 ) formed dissolving in the portion of the solution which still contains ferrous salt. c. Methods which can be employed only when the ferric iron is to be determined volumetrieally . Add to the hydrochloric solution small quantities of artificially prepared iron-free manganese dioxide, till the solution is of a dark olive-green color from the formation of manganic chloride ; boil till this coloration and the odor of chlorine have disappeared (Fit. MOHR) ; or you may add pure potassium permanganate (in crystals or concentrated solution) till the fluid is just red and then boil, till the red color and chlorine-odor have vanished. These methods present the advantage of permitting complete conversion of ferrous into ferric salts without the use of any considerable excess of the oxidizing agent. 2. Volumetric Determination. a. MARGUERITE'S Method. If we add to a solution of ferrous salt, containing an excess of sulphuric acid, potassium permanganate, the former is converted into a ferric salt by the oxidizing action of the latter (10FeSO 4 -|- 8H 2 SO 4 + K,Mn 2 6 8 = 5Fe f (S0 4 ), + K,SO 4 + 2MnSO 4 + 8H 2 O). Now if we possess a solution of potassium permanganate, and know how much iron 100 c.c. of it can convert from the ferrous to the ferric condition, we can, with this, readily determine an unknown quan- tity of iron ; we have simply, for this purpose, to dissolve the iron in acid, in the form of a ferrous salt, to oxidize the solution accu- rately, and note how many c.c. of the solution of potassium per- manganate have been used to accomplish that object. In the presence of hydrochloric acid (see y), the change is not exactly in accordance with the above equation (LOWENTHAL and LENSSEN*). a. Tit/ration of tlie Solution of Potassium Permangan- ate. Dissolve 5 grin, (roughly weighed) of pure crystallized potas- sium permanganate in distilled water by the aid of heat, dilute to 1 litre, and preserve in a stoppered bottle. Action of direct sunlight on the solution should be avoided. The solution, if carefully kept, does not alter, but still it is well to titrate it afresh occasionally. * Zeitschr. f. anal. Chem. 1, 329. 268 DETERMINATION. [ 112. aa. Titration l>y Metallic Iron. Weigh off accurately about 1 gnu. thin soft iron wire, previ- ously cleaned with emery paper, transfer to a J litre measuring flask, containing 100 c.c. dilute sulphuric acid (1 to 5), add about 1 rin. sodium bicarbonate, to produce carbonic acid and expel the air, and then close the flask with an india-rubber stopper, provided with an evolution tube, as shown in flg. 51 ; < contains 20 or 30 c.c. water. Heat the flask at first gently, finally to gentle boiling till the iron is dissolved. The clip l> is open, and the hydro- gen escapes through the water in <: Meanwhile boil about 300 c.c. distilled water, to drive out all the air it contains, and then allow it to cool. As soon as the iron is entirely dissolved, remove the lamp and close the evolution tube with the clip. When the iron solution has cooled a little loose the clip, and allow the water in c to recede, pour the boiled water into c, and allow this also to recede till the solution nearly reaches the mark. Take out the evolution tube and close the flask with an unperforated stopper, allow to cool to the temperature of the room, fill with water to the mark, shake and allow to stand, so that the particles of carbon usually present may deposit. Now take out with a pipette 50 c.c. of the clear and nearly colorless fluid (containing ^ of the iron weighed off), transfer to a 400 c.c. beaker, and dilute till the beaker is half full. Place the beaker on a sheet of white paper, or better, on a sheet of glass, with white paper underneath. Fill a GAY-LUSSAC'S or GKJSSLEB'S burette of 30 c.c. capacity, divided into -fa c.c. (see p. 41, figs. 13 and 14), up to zero, with solu- tion of potassium permanganate, of which take care to have ready a sufficient quantity, perfectly clear and uniformly mixed. Now add the permanganate to the ferrous solution, starring the latter all the while with a glass rod. At first the red drops dis- appear very rapidly, then more slowly. The fluid, which at first was nearly colorless, gradually acquires a yellowish tint. From the instant the red drops begin to disappear more slowly, add the permanganate with more caution and in single drops, until the last drop imparts to the fluid a faint, but unmistakable reddish color, 112.] FERROUS IRON. 269 which remains on stirring. A little practice will enable you readily to hit the right point. As soon as the fluid in the burette has sufficiently collected again read off, and mark the number of c.c. used. The reading off must be performed with the greatest exact- ness (see 22) ; the whole error should not amount to ^ c.c. The amount of permanganate solution used should be about 20 c.c. Repeat the experiment with another 50 c.c. of the iron solution. The difference between the permanganate used in the two cases should not be more than -1 c.c. ; if it is, make one more experiment and when the results are sufficiently near take the mean. Now calculate what quantity of iron is represented by 100 <-.e. of the permanganate. To this end first divide the iron weighed off by 5, and then multiply by '996, since soft iron wire contains on the average *4 per cent, carbon, &c. ; this gives the quantity of pure iron contained in 50 c.c. of the solution. Suppose we took 1-050 grm. iron wire, and used a mean of 21'3 c.c. per- manganate, J -" 7r 5 - - = '210, -210 X "996 = -20910. And then by rule of three : 21-3 : -20916:: 100 : x * = -98197; therefore, 100 c.c. permanganate = -98197 pure iron. If there is a deficiency of free acid in the solution of iron, the fluid acquires a brown color, turns turbid, and deposits a brown precipitate (manganese dioxide and ferric hydroxide). The same may happen also if the solution of potassium permanganate is added too quickly, or if the proper stirring of the iron solution is omitted or interrupted. Experiments attended with abnormal manifestations of the kind had always better be rejected. That the fluid reddened by the last drop of solution of potassium permanganate added, loses its color again after a time, need create no surprise or uneasiness; this decolorization is, in fact, quite inevitable, as a dilute solution of free permanganic acid cannot keep long undecomposed. 55. Titration by Ammonium Ferrous Sulphate. Weigh off, with the greatest accuracy, about 1-4 grin, of the pure salt prepared according to the directions given in 65, 4, dissolve in about 200 c.c. distilled water, previously mixed with about 20 c.c. dilute sulphuric acid, and proceed as in aa. By dividing the amount of salt weighed off by 7' 0014 (or where 270 DETERMINATION. [ 112. great accuracy is not required by 7) we obtain the quantity of iron corresponding. If the salt is not pure, if, for instance, it contains basic radicals isomorphous with ferrous iron (manganese, magnesium, &c.) ; or if it contains ferric iron, or is moist, the result will of course be too high. cc. Titration by Oxalic Acid. If solution of potassium permanganate is added to a warm solution of oxalic acid, mixed with sulphuric acid, the liberated permanganic acid oxidizes the oxalic acid to carbon dioxide and water [5H 2 C 2 O 4 + K 2 Mn 2 O 8 + 3H 2 SO 4 ^ K 2 S() 4 + 2MnSO 4 + 10CO, + 8H 2 O]. For the oxidation of 1 mol. oxalic acid (H 2 C 2 O 4 ) and 2 at. iron (in the ferrous state) equal quantities of permanganic acid are accordingly required ; therefore, 126 parts (1 mol.) of crystallized oxalic acid correspond, in reference to the oxidizing action of permanganic acid, to 112 parts (2 at.) of iron. A solution of oxalic acid is altered by the action of light ; it is, therefore, well only to dissolve as much as will be required for immediate use. Dissolve 1 to 1*2 grm. pure acid prepared by 65, 1, to 250 c.c. ; 50 c.c. of this solution are introduced into a beaker, diluted with about 100 c.c. water, from 6 to 8 c.c. cone, sulphuric acid added, and the fluid heated to about 60. The beaker is then placed on a sheet of white paper, and permanganate added from the burette, with stirring. The red drops do not disappear at first very rapidly, but when once the reaction has fairly set in, they continue for some time to vanish instantaneously. As soon as the red drops begin to disappear more slowly, the solution of potassium permanganate must be added with great caution; if proper care is taken in this respect, it is easy to complete the reaction with a single drop of permanganate ; this completion of the reaction is indicated with beautiful distinctness in the colorless fluid. To find the iron corresponding to the permanganate used, multiply the amount of crystallized oxalic acid in the 50 c.c. by 8 and divide by 9. If the oxalic acid was not perfectly dry, or not quite pure, the result of the experiment will, of course, lead to fixing the strength of the solution of potassium permanganate too high. Instead of pure oxalic acid, SAINT-GILLES has proposed to use crystallized oxalate of ammonium (NH 4 ) 2 C 2 O 4 + H a O). This can easily be pre- pared in the pure state," keeps well, and can be weighed with 112.] FERROUS IRON. 271 accuracy. 142'08 parts of the crystallized salt correspond to 112 parts iron. Of the foregoing three methods of standardizing solution of potassium permanganate, the first is the one originally proposed by MARGUERITE. Ammonium ferrous sulphate was first proposed by FR. MOHR, and oxalic acid by HEMPEL, as agents suitable for the purpose. With absolutely pure and thoroughly dry reagents, and proper attention, all three methods give correct results. For myself, I prefer the first method, as the most direct and positive, the only doubtful point about it being the question whether the assumption that the iron wire contains 99-6 per cent, of chemically pure iron is quite correct ; this, however, is of very trilling importance, as the error could not exceed y 1 ^ or y 2 ^ per- cent.* The other two methods are, as may readily be seen, some- what more convenient, but they are not so trustworthy unless you can insure the purity and dryness of the preparations. For the analysis of very dilute solutions of iron, e.g., chalybeate water, in which the amount of iron may be very approximately determined with great expedition, by direct oxidization with per- manganate, a very dilute standard solution must be prepared. Such a solution may be made by diluting the previous solution with 9 parts of water or by dissolving -5 grin crystals of potassium permanganate in 1 litre of water. It is to be directly standardized with correspondingly small quantities of iron, ferrous salt, or oxalic acid. In experiments of this kind, the fact that a certain quantity of permanganate is required to impart a distinct color to pure acidi- fied water (which is of no consequence in operations where the concentrated solution is used) must be taken into consideration ; for where the solution used is so highly dilute, it takes indeed a measur- able quantity of it to impart the desired reddish tint to the amount of water employed. In such cases, the volume of the solution of iron used for standardizing the permanganate and the volume of the w r eak ferruginous solution subjected to analysis should be the same, and either the two solutions should contain about the same quantity of iron, or by means of a special experiment, it is ascer- tained how many y 1 ^ c.c. of the permanganate are required to * If you are ofton making iron determinations, you may of course procure a quantity of wire and determine the amount of the foreign matter in it. 272 DETERMINATION. [ impart the desired pale red color to the same volume of acidified water. In the latter case, these ^ c.c. will be deducted from the amount of permanganate used in the regular experiments. Fig. 52. ft. Performance of the Analytical Process. This has been fully indicated in a. The compound to be examined is dissolved, preferably with application of a current of carbon dioxide* (see fig. 52). in dilute sulphuric acid, allowed to cool in the current of carbon dioxide, and suitably diluted (if prac- ticable, the solution of a substance containing about '2 grm. iron should be diluted to about 200 c.c.) ; if free acid is not present in sufficient quantity, dilute sulphuric acid is added till about 20 c. c. are present altogether, and then standard permanganate from the burette, to incipient reddening of the fluid. The volume of stand- ard solution used is then read off. The strength of the solution of permanganate being known, the quantity of iron present in the examined fluid is found by a very simple calculation. Suppose 100 c. c. of solution of potassium permanganate to correspond to 98 grm. iron, and 25 c.c. of the solution to have been used to effect the oxidation of the ferrous compound examined, then 100 : 25:: -98 : a?; x = '245. * If commercial hydrochloric acid is used for the preparation of CO 2 by action on marble, it must be free from sulphurous acid an impurity which it often contains. 112.] FEKKOUS IKON. 273 The quantity of ferrous iron originally present amounted accordingly to '245 grm. For the method of determining the total amount of iron present in a solution containing both ferrous and ferric salts, I refer to 113 ; for that of determining the amount in each con- dition separately, to Section Y. y. Process to be used with hydrochloric solutions of Iron. In titrating hydrochloric acid solutions of iron with perman- ganate, it is essential that the standardizing of the reagent and the actual analysis be performed under the same circumstances as regards dilution, amount of acird, and temperature. Besides the proper reaction lOFeCI, + K,Mn,O 8 + 16HC1 = 5Fe 2 Cl 6 + 2KC1 + 2MnCl, + 8H,O, the collateral reaction K a Mn 3 O 8 + 16HC1 = 2KC1 -f- 2MnCl a -f- 8H 3 O -f- 10C1 also takes place, in consequence of which a little chlorine is liberated. This chlorine does not combine with the ferrous chloride to form ferric chloride in the case of considerable dilution, but there occurs a condition of equilibrium in the fluid containing ferrous chloride, chlorine, and hydrochloric acid, which is destroyed by addition of a further quantity of either body (LOWENTHAL and LENSSEN*). But since it is difficult to observe the above conditions of obtaining correct results, the determination in presence of hydrochloric acid is always less trustworthy than it is in sulphuric acid solutions. The following method I have, however, found f to give the best results : Standardize the permanganate by means of iron dissolved in dilute sulphuric acid, make the iron solution to be tested up to J litre, add 50 c.c. to a large quantity of water acidified with sul- phuric acid (about 1 litre), titrate with permanganate, then again add 50 c.c. of the iron solution, and titrate again, &c. &c. The num- bers obtained at the third and fourth time are taken. These are constant, while the number obtained the first time, and sometimes also the second time, differs. The result multiplied by 5 gives exactly the quantity of permanganate proportional to the amount of ferrous iron present. J. PENNY'S Method (recommended subsequently by SCHABUS). If potassium dichromate is added to a solution of a ferrous salt in presence of a strong free acid, the ferrous salt is converted into * Zeitschr. f. anal. Chem. 1. 329. \ Ib. 1, 361. 274 DETERMINATION. [ 112.. ferric salt, whilst a potassium, and a chromic salt of the free acid is formed (6FeSO 4 + K 3 Cr 2 O 7 + 7H 2 SO 4 =3Fe 2 (SO 4 ) 3 + K,SO 4 + Or,. (SOO.+7H.O). Now, witli 29*522 gr. potassium dichromate dissolved to 2 litres of fluid, 33'6 gr. iron may be changed from a ferrous to a ferric salt, (295-22 being the mol. weight of K a O 2 O 7 , and 336 being 6 times the at. weight of iron ;) 50 c.c. of the above solution corre- spond accordingly to '84 grin. iron. Care must be taken to use perfectly pure potassium dichromate ; the salt is heated in a porcelain crucible until it is just fused ; it is then allowed to cool under the desiccator, and the required quan- tity weighed off when cold. Besides the above solution, another should also be prepared, ten times more dilute. It is always advisable to test the correctness of the standard solution of potassium dichromate, by oxidizing with it a known amount of pure iron dissolved to a ferrous salt (see p. 268, aa). The ferrous solution is sufficiently diluted, mixed with a suf- ficient quantity of dilute sulphuric acid, and the standard solution of potassium dichromate slowly added from the burette, the liquid being stirred all the while with a thin glass rod. The fluid, which is at first nearly colorless, speedily acquires a pale green tint, which changes gradually to a darker chrome-green. A very small drop of the mixture is now from time to time taken out by means of the stirring-rod, and brought into contact with a drop of a solution of potassium ferricyanide (free from f errocyanide) on a porcelain plate, which has been spotted with several of such drops. When the blue color thereby produced begins to lose the intensity which it exhibited on the first trials, and to assume a paler tint, the addition of the solution of potassium dichromate must be more carefully regulated than at first, and towards the end of the process, a fresh essay must be made, and with larger drops than at first, after each new addition of two drops, and finally, even of a single drop ; drops must also be left for some time in contact before the observation is taken. When no further blue coloration ensues, the oxidation is terminated. From the remarkable sensitiveness of the reaction, the exact point may be easily hit to a drop. To heighten the accuracy of the results, the dilute (ten times weaker) standard fluid should, just at the end of the process, be substituted for the concentrated solution of potassium dichromate. For the manner of proceeding in presence of ferric salts. 113. j FERRIC IRON. 275 1 refer to 113. If there is- a deficiency of free acid in the solution, brown chromic chromate may form, upon which the solution of ferrous salt exercises no longer a deoxidizing action. This method is usually preferred to the preceding when hydro- chloric acid is. unavoidably present. 113. 6. FERRIC IRON. a. Solution. Many ferric compounds are soluble in water. Ferric oxide and most ferric compounds which are insoluble in water, dissolve in hydrochloric acid, but many of them only slowly and with diffi- culty ; compounds of this nature are best dissolved in concentrated hydrochloric acid, in a flask, with the aid of heat ; which, however, should not be allowed to reach the boiling-point ; the compound must, moreover, be finely powdered, and even then it will often take many hours to effect complete solution. Fusion with sodium carbonate or potassium disulphate must sometimes be resorted to in case of native ferric compounds. / b. Determination. The iron of ferric compounds is usually weighed as ferric oxide, but sometimes as ferrous sulphide ( 81). It may, however, be estimated also indirectly, and also by volumetric analysis, both directly and after reduction to ferrous iron. The conversion of compounds of iron into ferric oxide is effected either by precipita- tion as ferric hydroxide, preceded in some cases by precipitation as ferrous sulphide, or as basic ferric acetate, succinate, or formate ; or by ignition. While the volumetric and the now seldom-used indirect methods are applicable in almost all cases, we may convert into 1. FERRIC OXIDE. a. By Precipitation as Ferric Hydroxide. All salts soluble in water of inorganic or volatile organic acids, and likewise those which, insoluble in water, dissolve in hydro- chloric acid, with separation of their acid. 5. By Precipitation as Ferrous Sulphide. All compounds 'of iron without exception. c. By ignition. All ferric salts of volatile oxygen acids. 276 DETERMINATION. [ 113. 2. FERROUS SULPHIDE. All compounds of iron without exception. The method 1, c, is the most expeditious and accurate, and is therefore preferred in all cases where its application is admissible. The method 1, #, is the most generally used. The methods 1, &, and 2, serve principally to effect the separation of the iron from other bases ; they are resorted to also in certain instances where a is inapplicable, especially in cases where sugar or other non-volatile organic substances are present ; and also to determine iron in ferric phosphates and borates. For the manner of determining iron in ferric chromate and silicate, I refer to 130 and 140. The volu- metric methods for estimating the iron of ferric compounds are used in technical work almost to the exclusion of all others, and are very frequently employed in scientific analyses. 1. Determination as Ferric Oxide. a. By Precipitation as Ferric Hydroxide. Mix the solution in a dish or beaker with ammonia in excess, heat nearly to boiling, decant repeatedly on to a filter, wash the precipitate carefully with hot water, dry thoroughly (which very greatly reduces the bulk of the precipitate), and ignite in the manner directed in 53. For the properties of the precipitate and residue, see 81. The method is free from sources of error. The precipitate, under all circumstances, even if there are no fixed bodies to be washed out, must be most carefully and thoroughly washed, since, should it retain any traces of ammonium chloride, a portion of the iron would volatilize in the form qf ferric chloride. It is also highly advisable to dissolve the weighed residue, or a portion of it, in strong hydrochloric acid, to see whether it is quite free from silicic acid. The solution is most readily effected in hydrochloric acid if the oxide is previously -reduced to metallic iron by ignition in hydrogen. 1). By Precipitatioii as Ferrous Sulphide. The solution, in a not too large flask, is mixed with ammonia, till all the free acid is neutralized. (In the absence of organic, non- volatile substances, this leads to the precipitation of a little ferric hydroxide, which, however, is of no consequence.) Add ammonium chloride, if not already present in sufficient quantity, then colorless or yellowish ammonium sulphide in moderate excess, 113.] FERRIC IRON. 277 lastly water, till the fluid reaches to the neck of the flask. Cork it up and stand in a warm place till the precipitate has subsided, and the supernatant fluid has a clear yellowish appearance (without a tinge of green). Wash as directed in the case of manganese sulphide ( 109, 1, - tracted from the total amount of iron found. {Reduction by Hydrogen Sulphide. Pass hydrogen sulphide through the cold ferric solution in a flask. The solution should occupy about two-thirds of the capacity of the flask, and should not contain much more than *2 gr. iron per 100 c.c., but may be more dilute when but little iron is present. Continue the treatment with hydrogen sulphide at least 10 minutes after the color due to the ferric salt has disappeared, or until the solution appears to be well saturated with that gas. Heat, at first cautiously, to boiling. Escape of hydrogen sulphide at this period indicates that enough of that reagent has been applied. Continue boiling so rapidly that air cannot enter the flask, the mouth of which may be partially closed by a loose roll of filter paper, or other means, until the solution is reduced to one half its first volume. This will insure the removal of excess of hydrogen sulphide. (The escaping vapor will cease to blacken paper dipped in an alkaline lead solution somewhat before this point is reached.) During the boiling, let the flask be inclined so as to prevent mechanical loss. When the boiling is discontinued fill the flask immediately with old water to within an inch of the mouth, close with a stopper, and cool in a stream of water. Before reducing the ferric solution by either of the above pro- cesses, it is desirable to remove hydrochloric acid, if it is present, so that the iron after reduction can be satisfactorily determined by means of potassium permanganate. Chlorides can be decomposed and hydrochloric acid removed by evaporating the solution with excess of sulphuric acid so long as hydrochloric acid vapors are given off at a temperature slightly exceeding 100 C. A liberal excess of sulphuric acid is advan;iv- geous. After cooling add water and digest till the ferric sulphate is dissolved. This treatment is simple and safe when nothing is present which is thereby converted into a compound insoluble in dilute sulphuric acid (silicic acid, barium, strontium, much cal- 280 DETERMINATION. [ llo. cium, . In the Dry Way. This method serves more exclusively for the analysis of silver bromide and iodide, although it can be applied in the case of other compounds. Fig. 53. The process is conducted in the apparatus illustrated by fig. 53, leaving off the U tube e, and employing a straight bulb- tube or a plain tube with porcelain tray instead of the bent tube d. a is a flask for disengaging chlorine, it is completely filled with pieces of pvrolusite (native manganese dioxide) of the size of hazel- nuts, and half filled with strong hydrochloric acid. The chlorine is conducted to the bottom of c, which contains a layer of sulphuric acid and is filled above with pumice-stone moistened with strong sulphuric acid. The flow of chlorine may be regulated by the stop-cock, while any excess accidentally produced is conducted by a second tube to the bottom of the cylinder 5, in which it is absorbed by a soda solution ; d is a bulb-tube intended for the reception 286 DETERMINATION. [ 1L"). of the silver iodide or bromide. The operation is commenced by introducing the compound to be analyzed into the bulb, and applying heat to the latter until its contents are fused ; when cold, the tube is weighed and connected with the apparatus. Chlorine gas is then evolved from a ; when the evolution of the gas has proceeded for some time, the contents of the bulb are heated to fusion, and kept in this state for about fifteen minutes, agitating now and then the fused mass. The bulb-tube is then removed from the apparatus, allowed to cool, and held in a slanting position to replace the chlorine by atmospheric air; it is subsequently weighed, then again connected with the apparatus, and the former process repeated, keeping the contents of d in a state of fusion for a few minutes. By means of a light glass tube attached by a piece of rubber tube to the end of d the chlorine escaping during the operation may be conducted into the open air or into a flue. The operation may, in ordinary cases, be considered concluded if the weight of the tube suffers no variation by the repetition of the process. If the highest degree of accuracy is to be attained, heat the silver chloride again to fusion, passing at the same time a slow stream of pure, dry carbon dioxide through the tube, in order to drive out the traces of chlorine absorbed by the fused chloride. Allow to cool, hold obliquely for a short time, so as to replace the carbon dioxide by air, and finally weigh. See 82. 2. Determination as Silver Sulphide. Hydrogen sulphide precipitates silver completely from acid, neutral, and alkaline solutions ; ammonium sulphide precipitates it from neutral and alkaline solutions. The precipitate does not settle clearly and rapidly except a free acid or salt be present (such as nitric acid or ah alkali nitrate). Eecently prepared perfectly clear solution of hydrogen sulphide may be employed to precipitate small quantities of silver ; to precipitate larger quantities, the solu- tion of the salt of silver (which must not be too acid) is moderately diluted, and washed hydrogen sulphide gas conducted into it. After complete precipitation has been effected, and the silver sul- phide has perfectly subsided (with exclusion of air), it is collected on a weighed filter, washed, dried at 100, and weighed. For the properties of the precipitate, see 82. This method, if properly executed, gives accurate results. The operator must take care to filter quickly, and to prevent the access of air as much as possible 115.] SILVER. 287 during the filtration, since, if this precaution be neglected, sulphur is likely to separate from the hydrogen sulphide water, which, of course, would add falsely to the weight of the silver sulphide. If the presence of a minute quantity of sulphur in the precipitate is suspected, treat it after drying with pure carbon disulphide on the filter repeatedly, till the fluid running through gives no residue on evaporation in a watch-glass ; dry and weigh. The sulphide must, however, never be weighed as just described, unless the analyst is satisfied that no considerable amount of sul- phur has fallen down with it, as would occur if the fluid contained hyponitiic acid, a ferric salt, or any other substance which decom- poses hydrogen sulphide. In case the precipitate does contain much admixed sulphur, the simplest process is to convert it into metallic silver (H. HOSE*). For this purpose it is transferred to a weighed porcelain crucible, the filter ash is added, and the whole is heated to redness in a stream of hydrogen, the apparatus- described in 108 being employed. Results accurate. Should the apparatus in question not be at the operators dis- posal, he may, after complete washing of the precipitate, carefully rinse it into a porcelain dish (without injuring the weighed filter), heat it once or twice with a moderately strong solution of pure sodium sulphite, retransfer the precipitate (now freed from admixed sulphur) to the old filter, wash well, dry and weigh (J. LOWE+ > ; or lie may treat the dried precipitate, together with the filter-ash, with moderately dilute chlorine-free nitric acid at a gentle heat, till complete decomposition has been effected (till the undissolved sulphur has a clean yellow appearance), filter, wash well, and pro- ceed according to 1. a. 3. Determination as Silver Cyanide. Mix the neutral solution of silver with potassium cyanide, until the precipitate of silver cyanide which forms at first is redissolved ; add nitric acid in slight excess, and apply a gentle heat. If the solution contains free acid, this must be first neutralized with pot- ash or sodium carbonate. After some time, collect the precipitated silver cyanide on a weighed filter, wash, dry at 100, and weigh. For the properties of the precipitate, see 82. The results are accurate. * Pogg. Annal. 110, 139. f Journ. f. prakt. Chem. 77, 73. 288 DETERMINATION. [ 115. 4. Determination as Metallic Silver. Silver oxide, silver carbonate, &c., are easily reduced by simple ignition in a porcelain crucible. In the reduction of salts of organic acids, the crucible is kept covered at first, and a moder- ate heat applied ; after a time the lid is removed, and the heat increased, until the whole of the carbon is consumed. For the properties of the residue, see 82. The results are absolutely accurate, except as regards silver salts of organic acids; in the analysis of the latter, it not unfrequently happens that the reduced silver contains a minute portion of carbon, which increases the weight of the residue to a trifling extent. If it is desired to transform silver chloride, bromide, or sulphide into metallic silver, for the purpose of analysis, they are heated in a current of pure hydrogen to redness, till the weight remains constant. The process may be conducted in a porcelain crucible or a bulb-tube. In the former case, the apparatus described p. 251, 108, is used; in the latter the apparatus represented p. 285, with the substitution, of course, of hydrogen for chlorine. If the bulb-tube is used, it must, after cooling and before being weighed, be held in an inclined position, so that the hydrogen may be replaced by air. The results are perfectly accurate. Silver iodide cannot be reduced in this way. 5. Volumetric Methods. I. GAY-LUSSAC'S. This, the most exact of all known volumetric processes, was introduced by GAY-LUSSAC as a substitute for the assay of silver by cupellation, was thoroughly investigated by him, and will be found fully described in his work on the subject. This method has been rendered still more precise by the researches of G. J. MULDER, to whose exhaustive monograph* I refer the special student of this branch. I shall here confine myself to giving the process so far as to suit the requirements of the chemical laboratory, taking only for granted that the analyst has the ordinary measuring apparatus, &c., at his disposal. MULDER'S results will be made use of to the full extent possible under these circumstances. a. EEQUISTTES. a. SOLUTION OF SODIUM CHLORIDE. Take chemically pure * Die Silberprobirmethode (see note p. 167). 115.] SILVER. 289 sodium chloride either artificially prepared or pure rock-salt powder it roughly and ignite moderately (not to fusion*). Now dissolve 5*4202 grm. in distilled water to 1 litre, measured at 16. 100 c.c. of this solution contains a quantity of sodium chloride equivalent to 1 grm. of silver. The solution is kept in a stoppered bottle and shaken before use. ft. DECIMAL SOLUTION OF SODIUM CHLORIDE. Transfer 50 c.c. of the solution described in a to a 500 c.c. measuring flask, fill up to the mark with distilled water and shake. Each c.c. of this decimal solution corresponds to '001 grm. silver. The measuring must be performed at 16. The solution is kept as the other. y. DECIMAL SILVER SOLUTION. Dissolve '5 grm. chemically pure silver f in 2 to 3 c.c. pure nitric acid of 1*2 sp. gr., and dilute the solution with water exactly to 500 c.c. measured at 16. Each c.c. contains '001 grm. silver. The solution is kept in a stoppered bottle and protected against the influence of light. d. TEST-BOTTLES. These should be of colorless glass, holding easily 200 c.c., closed with well-ground glass-stoppers, running to a point below. The bottles fit into cases blackened on the inside, and reaching up to their necks. In order to protect the latter also from the action of light, a black-cloth cover is employed. b. PRINCIPLE. Suppose we know T the value of a solution of sodium chloride, i.e., the quantity that is necessary to precipitate a given amount of silver, say 1 grm., we are in the position, with the aid of this solu- * On fusion, if the flame can in the least way act upon it, it takes an alkaline reaction, since under the influence of vapor of water and carbon dioxide, a little hydrochloric acid is formed and escapes, while a corresponding quantity of sodium carbonate remains. f For the preparation of pure silver STAS recommends the following method: Take crude silver nitrate containing copper, fuse in order to decompose any platinum nitrate which may be present, dissolve in dilute ammonia, allow to stand 48 hours, filter and dilute till the fluid does not contain more than 2 per cent, silver. Add ammonium sulphite in excess. To ascertain how much sul- phite will be required make a small preliminary test; as soon as after heating the blue solution loses all color, you may be sure that enough of the sulphide has been added. Warm on a water-bath to 60 or 70, when all the silver will be thrown down as a metallic powder, allow to cool and wash by decantation with diluted ammonia till the washings are free from copper and sulphuric acid. Now digest the metal for several days with strong ammonia, wash, dry, and fuse with a flux of borax and sodium nitrate. 290 DETERMINATION. [ 115. tion, to determine an unknown amount of silver, for if we put x for the unknown amount of silver, then c.c. of solution used for 1 grm. : c.c. used for x : : 1 grm. : x. But if we examine whether 1 mol. sodium chloride dissolved in water actually precipitates 1 at. of silver dissolved in nitric acid exactly, we find that this is not the case.* On the contrary, the clear supernatant fluid gives a small precipitate both on the addition of a little solution of sodium chloride, and on the addition of a little silver solution, as MULDER has most accurately determined. The value of a solution of sodium chloride in the sense explained above cannot, therefore, be reckoned from the amount of salt it contains, b^ calculating 1 at. silver for 1 mol. sodium chloride, but it can only be obtained by experiment. MULDEK has shown that the temperature and the degree of dilution have some influence, and also that this fact is to be explained on the ground of the sol- vent power of the sodium nitrate produced on the silver chloride. In the solution thus formed we have to imagine NaNO 3 and NaCl with AgXO 3 in a certain state of equilibrium, which on the addition of either Nad or AgNO 3 is destroyed, silver chloride being pre- cipitated. From this interesting observation it follows, that if to a silver- solution we add at first concentrated solution of sodium chloride, then decimal solution drop by drop, till the exact point is reached when no more precipitate appears, now, on addition of decimal silver-solution, a small precipitate will be again produced ; and if we add the latter drop by drop, till the last drop occasions no tur- bidity, then again decimal solution of sodium chloride will give a small precipitate. On noticing the number of drops of both deci- mal solutions which are required to pass from one limit to the other, we find that the same number of each are used. Let us suppose that we had added decimal solution of sodium chloride till it ceased to react, and had then used 20 dropsf of decimal silver- solution, till this ceased to produce a further turbidity, we must now again add 20 drops of decimal solution of sodium chloride, in * If sodium bromide or potassium bromide is used, complete precipitation would ensue on addition of an equivalent quantity of silver solution, since bro- mide of silver is not at all soluble in the supernatant fluid (STAS Compt rend 67, 1107). f Twenty drops from MULDER'S dropping apparatus are equal to 1 c.c. 115.] SILVER. 291 order to reach the point at which this ceases to react. Were we to add only 10 instead of these 20 drops, we have the neutral point, as MULDER calls it, i.e., the point at which both silver and sodium chloride produce equal precipitates. We have, therefore, 3 different points to choose from for our final reaction : a, the point at which sodium chloride has just ceased to precipitate the silver ; 5, the neutral point ; c, the point at which silver-solution has just ceased to precipitate sodium chloride. Whichever we may choose, we must keep to it, l.e., we must not use a different point in standardizing the sodium chloride solution and in performing an analysis. The difference obtained, by using first a and then b is, according to MULDER, for 1 grin, silver, at 16, about '5 mgrm. silver; by employing first a and then c, as was permitted in the original process of GAY-LUSSAC, the difference is increased to 1 mgrm. For our object, it appears most convenient to consider, once for all, the point a as the end, and never to finish with the silver- solution. If the point has been overstepped by the addition of too large an amount of decimal solution of sodium chloride, 2 or 3 c.c. of decimal silver-solution should be added all at once. The end-point is then found by carefully adding decimal solution of sodium chloride again, and the quantity of silver in the silver-solu- tion added is added to the original amount of silver weighed off. c. PERFORMANCE OF THE PROCESS. This is divided into two operations a, the tit-ration of the sodium chloride solution; /?, the assay of the silver alloy to be examined. (Y. TlTRATION OF THE SODIUM C'lILORIDE SOLUTION. Weigh off exactly from Tool to 1*003 grm. chemically pure silver,* put it into a test-bottle, add 5 c.c. perfectly pure nitric acid, of 1/2 sp. gr., and heat the bottle in an inclined position in a water- or sand-bath till complete solution is effected. Xow blow out the nitrons f nines from the upper part of the bottle, and after it has cooled a little, place it in a stream of water, the temperature of which is about 16, and let it remain there till its contents are cooled to this degree, wipe it dry, and place it in its case. Now fill the 100 c.c. pipette with the concentrated solution of sodium chloride, which is then allowed to flow into the test-bottle * See note, p. 289. 292 DETERMINATION. [ 115. containing the silver-solution*. Insert the glass-stopper firmly (after moistening it with water), cover the neck of the bottle with the cap of black stuff belonging to it, and shake violently without delay, till the silver chloride settles, leaving the fluid perfectly clear. Then take the stopper out, rub it on the neck, so as to remove all silver chloride, replace it firmly, and by giving the bottle a few dexterous turns, rinse the chloride down from the upper part. After allowing to rest a little, again remove the stopper, and add, from a burette divided into T J c.c., decimal sodium chloride solution, allowing the drops to fall against the lower part of the neck, the bottle being held in an inclined position. If, as above directed, 1*001 to 1*008 grm. silver have been employed, the portions of sodium chloride solution at first added may be c.c. After each addition, raise the bottle a little out of its case, observe the amount of precipitate produced, shake till the fluid has become clear again, and proceed as above, before adding each fresh quantity of sodium chloride solution. The smaller the precipitate produced, the smaller should be the quan- tity of sodium chloride next added ; towards the end only two drops should be added each time ; and quite at the end read off the height of the fluid in the burette before each further addition. When the last two drops give no more precipitate, the previous reading is the correct one. If by chance the point has been overstepped, and the time has been missed for the proper reading off of the burette, add 2 to 3 c.c. of the decimal silver solution (the silver in which is to be added to the quantity first weighed), and try again to hit the point exactly by careful addition of decimal sodium chloride solution. The value of the sodium chloride solution is now known. Reckon it to 1 grm. silver. Suppose we had used for 1*002 grm. silver, 100 c.c. of concen- trated and 3 c.c. of decimal sodium chloride solution ; this makes altogether 100*3 of concentrated ; then 1*002 : 1*000 :: 100*3 : a? v. = 100*0998 We may without scruple put 100*1 for this number. We now * The pipette, having been filled above the mark, should be fixed in a support, before the excess is allowed to run out, otherwise the measurings will not be suffi- ciently accurate. 115.] SILVER. 293 know that 100*1 c.c. of the concentrated solution of sodium chloride, measured at 16. exactly precipitates 1 grin, of silver. This relationship serves as the foundation of the calculation in actual assaying, and must be re-examined whenever there is reason to imagine that the strength of the sodium chloride solution may have altered. ft. THE ACTUAL ASSAY OF THE SlLVEK-ALLOY. Weigh oif so much as contains about 1 grm. of silver, or better, a few mgrm. more ;* dissolve in a test-bottle in 5 to 7 c.c. nitric acid, and proceed in all respects exactly as in a. Suppose we had taken 1-116 grm. of the alloy, and in addition to the 100 c.c. of concentrated sodium chloride solution, had used 5 c.c. of the dilute (= *5 concentrated), how much silver would the alloy contain ? Presuming that we use the same sodium chloride solution which served as our example in a, 100*1 c.c. of which = 1 grm. silver, then 100-1 : 100-5 : : 1-000 : x x = 1-003996 (say (1-004). We may also arrive at the same result in the following manner : Nad Solution. For the precipitation of the silver in the alloy were used 100*5 c.c. For 1 grm. silver are necessary 100*1 c.c. Difference -4 c.c. There are, therefore, 4 mgrm. of silrer present more than a grm., on the presumption that -1 of the concentrated sodium chloride solution ( 1 c.c. of the decimal solution) corresponds to 1 mgrm. * In coins containing 9 parts of silver and 1 part of copper, therefore take about 1*115 or 1*120. In weighing off alloys of silver and copper, which do not correspond to the formula Ag 3 Cu 2 (standard VoW ) = we must remember that they are never homogeneous in the mass ; thus, for instance, the pieces of metal, from which coins are stamped, often show 1-5 to 17 in a thousand more silver in the middle than at the edges. In assaying alloys, then, portions from various parts of the mass must be taken, in order to get a correct result. The inaccuracy, however, proceeding trom the cause above-mentioned, can only be completely overcome by fusing the alloy and taking out a portion from the well-stirred mass for the assay. 294 DETERMINATION. [ 115. silver. This supposition, although not absolutely correct, may he safely made, for the inexactness it involves is too minute, as is evident from the previous calculation. Before we can execute this process exactly, we must know the quantity of silver the alloy contains very approximately. In assaying coins of known value this is the case, bnt with other silver alloys it is usually not so. Under the latter circumstances an approximate estimation must precede the regular assay. This is performed by weighing off \ grin, (or in the case of alloys that are poor in silver, 1 grm.), dissolving in 3 to 6 c.c. nitric acid, and adding from the burette sodium chloride solution, first in larger, then in smaller quantities till the last drops produce no further turbidity. The last drops are not reckoned with the rest. The operation is conducted, as regards shaking/ &c., as previously given. Suppose we had weighed off *5 grm. of the alloy, and employed 25 c.c. of the sodium chloride solution taking the above supposed value of the latter- We have 100-1 : 25 : : 1-000 : x x = -249T that is, the silver in '5 grm. of the alloy ; and as to the quantity of alloy we have to w r eigh off for the assay proper, We have '2497 : 1-003 : : -5 : x x = 2-008. This quantity will, of course, require more nitric acid for solution than was previously used (use 10 c.c.). In cases where the highest degree of accuracy is not required, the results afforded by this rough preliminary estimation will be accurate enough, if the experiment is carefully conducted, since they give the quantity of silver present to within ^^ or ^ F . With alloys which contain sulphur, and with such as consist of gold and silver, and contain a little tin, LEVOL* employs concen- trated sulphuric acid (about 25 grm.) as solvent. The portion of the alloy is boiled with it till dissolved ; after cooling, the fluid is treated in the usual manner. As, however, concentrated sulphuric, acid fails to dissolve all the silver when there is much copper present, MAscAzziNif digests the weighed portion of alloy (which * Annal. de Chim. et de Phys. (3) 44, 347. \ Chem. Centralbl. 1857, 300. 115.j SILVKK. 295 may contain small quantities of lead, tin, and antimony, besides gold) first with the least possible amount of nitric acid, as long as red vapors are formed; he then adds concentrated sulphuric acid, hoils till the gold has settled well together, adds water after <-ooling, and then titrates. In the presence of mercury, tli chloride of that metal is carried down with the silver, render hi"- n the method inaccurate. If the quantity of mercury is but small, yon may get over the difficulty by adding 25 c.c. ammonia and 20 c.c. acetic acid (LEVOL). The ammonium acetate acts by decomposing the mercuric chloride, and thus preventing its precipitation (DEBRAY*). If the quantity of mercury is large the addition of an alkali acetate is not effective, and DEBRAY recom- mends to drive off the mercury by igniting for four hours in a small crucible of gas carbon in a muffle. The presence of other volatile metals, such as zinc, does not interfere with this oper- ation. II. PISANI'S METHOD.! This process depends on the following reaction : a solution of iodide of starch added to a very dilute neutral solution of silver nitrate, forms silver iodide and silver hypoiodite. The blue color consequently vanishes, and on continued addition of the iodide of starch, the fluid does not become permanently blue till all the sil- ver nitrate present is decomposed in the above manner. The iodide of starch solution used is therefore proportional to the quan- tity of silver nitrate. Hence, if the value of the iodide of starch solution be determined, by allowing it to act on a certain amount of silver solution of known strength, we shall be able to estimate unknown quantities of silver with the greatest ease, provided that the silver solution is free from all other substances which exert a decomposing action on the iodide of starch. Besides the ordinary reducing agents, the following salts must be especially mentioned as possessing this power : mercurous and mercuric salts, stannous salts, manganous, ferrous, and antimonious salts, also auric chloride and arsenites ; lead and copper salts, on the other hand, do not affect iodide of starch. The iodide of starch is prepared as follows : make an intimate * Compt. rend. 70, 849. f Annal. d. Min. 10, 83. 296 DETEKMI-NATION. [ mixture in a mortar of 2 grm. iodine and 15 grm. .starch with the addition of 6 to 8 drops of water, and heat the slightly-moist mix- ture in a closed flask in a water-bath, till the original violet-blue color has passed into dark grayish-blue it takes about an hour. The iodide of starch thus prepared is then digested with water ; it dissolves completely to a deep bluish-black fluid. The value of this fluid is determined 'by allowing it to act on 10 c.c. of a neutral solution of silver nitrate, containing 1 grm. of pure silver in 1 litre the silver solution is mixed with a little pure precipitated calcium carbonate before adding the iodide of starch. The strength of this latter is right, if 50 to 60 c.c. are used in this experiment. On adding it, at lirst the blue color dis- appears rapidly, and the fluid becomes yellowish from the silver iodide. The end of the operation is attained as soon as the fluid is bluish-green. The point is pretty easy to hit, and an error of '5 c.c. is of no importance, as it only corresponds to about '0001 grm. silver. The calcium carbonate, besides neutralizing the free acid, has the effect of rendering the final change of the color more dis- tinctly observable. To analyze an alloy of silver and copper, dis- solve about '5 grm. in nitric acid, dilute to 100 c.c. to lower the color of the copper, saturate 5 c.c. with calcium carbonate, and add iodide of starch till the coloration appears. Or you may deter- mine very approximately the amount of silver in 2 c.c. of the solu-~ tion, then precipitate the greater part (about 9 9f) of the silver from 50 c.c. of the solution with standard solution of potassium iodide, and without filtering estimate the remainder of the silver by means of iodide of starch. If the amount of silver to be deter- mined is more than '020 grm., it is always better to employ the latter method. In the case of a nitric acid solution containing sil- ver with lead, the latter metal is first precipitated with sulphuric acid and filtered off, calcium carbonate is added to the filtrate till all free acid is neutralized, the fluid is filtered again (if necessary), and lastly, more calcium carbonate is added, and then the iodide of starch. Very dilute solutions must be concentrated, so that one may have no more than from 50 to 100 c.c. to deal with. The method is worthy of notice and specially suited for the estimation of small quantities of silver. "With such it has afforded me perfectly satis- factory results. Instead of the standard iodide of starch, a dilute standard solution of iodine in potassium iodide may be equally well 116.] LEAD. . 297 employed with addition of starch solution (FIELD*). If this is used you must bear in mind that any substance which decomposes potassium iodide with separation of iodine will interfere. III. METHOD DEPENDING ON THE ACTION OF SILVER NITRATE ON SODIUM CHLORIDE IN THE PRESENCE OF POTASSIUM CHROMATE. This is the reverse of the method for the estimation of -chlorine 141 I, a, and will be described in that place. 116. 2. LEAD. a. Solution. Few of the lead salts are soluble in water. Metallic lead, lead oxide, and most of the lead salts that are insoluble in water dissolve in dilute nitric acid. Concentrated nitric acid effects neither com- plete decomposition nor complete solution, since, owing to the insolubility of lead nitrate in concentrated nitric acid, the first por- tions of nitrate formed protect the yet undecomposed parts of the salt from the action of the acid. For the solubility of lead chloride and sulphate, see 83. As we shall see below, the analysis of these compounds may be effected without dissolving them, lead iodide dissolves readily in moderately dilute nitric acid upon appli- cation of heat, with separation of iodine. Solution of potassa is the only menstruum in which lead chromate dissolves without decomposition. b. Determination. Lead may be determined as oxide, sulphate, chromate, or sul- phide also by volumetric analysis. We may convert into 1. LEAD OXIDE : a. By Precipitation. All lead salts soluble in water, and those of its salts which, insoluble in that menstruum, dissolve in nitric acid, wiih separa- tion of their acid. b. By Ignition. a. Lead salts of readily volatile or decomposable inorganic acids. /?. Lead salts of organic acids. * Chem. News, 2, 17. 298 DETERMINATION. [ 116. 2. LEAD SULPHIDE : All lead salts in solution. 3. LEAD SULPHATE: a. By Precipitation. The salts that are insoluble in water, but soluble in nitric acid, whose acid cannot be separated from the solution. b. By Evaporation. a. All the oxides of lead, and also the lead salts of volatile acids. ft. Many of the organic compounds of lead. 4. LEAD CHROMATE: The compounds of lead soluble in water or nitric acid. The application of these several methods must not be under- stood to be rigorously confined to the compounds specially enu- merated under their respective heads ; thus, for instance, all the compounds enumerated sub 1, may likewise be determined as lead sulphate ; and, as above mentioned, all soluble compounds of lead may be converted into lead sulphide ; also, in lead sulphate the lead may be without difficulty determined as sulphide, Lead chloride, bromide, and iodide are most conveniently reduced to the metallic state in a current of hydrogen gas, in the manner described 115 (Reduction of silver chloride), if it is not deemed preferable to dis- solve them in water, or to decompose them by a boiling solution of sodium carbonate. If the reduction method is resorted to, the heat applied should not be too intense, since this might cause some lead chloride to volatilize. The higher oxides of lead are reduced by ignition to the state of lead monoxide, and may thus be readily analyzed and dissolved. Should the operator wish to avoid having recourse to ignition, the most simple mode of dissolving the higher oxides of lead is to act upon them with dilute nitric acid, with the addition of alcohol. For the methods of analyzing lead sulphate, chromate, iodide, and bromide, I refer to the paragraphs treating of the corresponding acids, in the second part of this section. To effect the estimation of lead in the oxide and in many lead salts, especially also in the sulphate, the compound under examination may be fused with potassium cyanide, and the metallic lead obtained well washed, and weighed. From the sulphide also the greater portion of the lead 116.] LEAD. 299 may be separated by this method, but never the whole (II. ROSE*). 1. Determination as Oxide. a. By Precipitation. Mix the moderately dilute solution with ammonium carbonated slightly in excess, add some caustic ammonia, apply a gentle heat, allow to cool and filter through a small thin filter. Wash with pure water, dry, and transfer the precipitate to a watch-glass, removing it as completely as possible from the filter ; burn the latter in a weighed porcelain crucible. After the crucible is cold, moisten the ash with nitric acid, allow it to evaporate, ignite gently, allow to cool, add the precipitate and ignite gently till all the car- bonic acid is driven off. For the properties of the precipitate and residue, see 83. The results are very satisfactory, although gen- erally a trifle too low, owing to lead carbonate not being absolutely insoluble, particularly in fluids rich in ammonium salts (Expt. No. 47, b). b. By Ignition. Compounds like lead carbonate or nitrate are cautiously ignited in a porcelain crucible, until the weight remains constant. In case of lead salts of organic acids, the substance is very gently heated in a small covered porcelain crucible, which is included within a large one, also covered, until the organic matter is completely carbonized ; the lids are then removed, when the mass begins to ignite, and a mixture of lead oxide with metallic lead results, which may still contain unconsumed carbon. A few pieces of recently fused ammonium nitrate are now thrown into the inner crucible, which has previously been removed from the flame, and both are again covered. The salt fuses, oxidizes the lead, and converts it partly into nitrate. The whole is now very gradually raised to a red heat, until no more fumes of hyponitric acid escape. The residuary oxide is then weighed. The results are satisfactory. 2. Determination as Sulphide. Lead may be completely precipitated from acid, neutral and * Pogg. Annal. 91, 144. f Ammonium oxalate, which has been so highly recommended as a precipi- tant for lead, is not so delicate as the carbonate. My experience in this respect coincides with F. Mohr's (Expt. No. 48). 300 DETERMINATION. [ 116. alkaline solutions by hydrogen sulphide, and also from neutral and alkaline solutions by ammonium sulphide. Precipitation from acid solution is usually employed, especially in separations. A large excess of acid and also warming should both be avoided. The former is prejudicial to complete precipitation ( 83, y), the latter may readily occasion the re-solution of the sulphide that has already been precipitated. In order to guard against incomplete precipitation, before filtering, test a portion of the supernatant fluid by mixing with a relatively large quantity of strong hydrogen sulphide water. If the fluid contained no hydrochloric acid or metallic chloride, the lead sulphide is pure. After it has been filtered off, washed with cold water and dried, it is transferred, together with the filter-ash, to a porcelain crucible, a little sulphur added, and ignited in hydrogen at gentle redness till its weight is constant. It should always be allowed to cool in a current of the gas, before being weighed. As regards the apparatus, see 108, 2, fig. 50. For the properties of the residue, see 83, y. The results are satisfactory (II. ROSE). The heat of the ignition must not be too low, or the residue will contain too much sulphur, nor too high, or the lead sulphide will begin to volatilize, and lead disulphide will also be formed with loss of hydrogen sulphide. Drying the precipitate at 100 cannot be recommended ( 83, y). If the fluid, on the contrary, contained hydrochloric acid or a metallic chloride, the lead sulphide contains chloride which cannot be removed even by boiling the precipitate with ammonium sulphide. If the precipi- tate were treated as above, we should obtain a tolerably pure sulphide, but not without loss from volatilization of chloride. A precipitate of this kind must therefore be decomposed with strong hydrochloric acid, the solution evaporated to dryness, the residue dissolved by heating with a concentrated solution of sodium acetate, and this solution diluted and poured with stirring into excess of strong hydrogen sulphide water. Or the lead chloride obtained may be evaporated, heated to 200, and weighed as such (FlNKENER*). 3. Determination as Sulphate, a. By Precipitation. . Determination. Copper may be weighed in the form of cupric oxide, or in the metallic state, or as cuprous sulphide (85). Into the form of. cupric oxide it is converted by precipitation, or ignition, sometimes with previous precipitation as sulphide. The determination as cuprous sulphide is preceded usually by precipitation either as cupric sulphide or as cuprous sulphocyanate. Copper may be deter- mined also by various volumetric and indirect methods. We may convert into 1. CUPRIC OXIDE : a. By Precipitation as hydrated cupric oxide and subsequent ignition : All cupric salts soluble in water, and also those insoluble salts, the acids of which may be removed upon solution in nitric acid, provided no non-volatile organic substances be present. 1. By Precipitation, preceded by Ignition of the compound : Such of the salts enumerated under a as contain a non-vblatile organic substance, thus more particularly cupric salts of non-vola- tile organic acids. c. By Ignition : Cupric salts of oxygen acids that are readily volatile or decomposable at a high temperature (cupric carbonate, cupric nitrate). 2. METALLIC COPPER : Copper in all solutions free from other metals precipitable by zinc or the galvanic current, also the oxides of copper. 3. CUPROUS SULPHIDE : Copper in all cases in which no other metals are present that are precipitable by hydrogen sulphide or potassium sulphocyanate. 312 DETERMINATION. [ 119. Of the several methods of effecting the estimation of copper, No. 3 is particularly to be recommended for use in laboratories ; method 2 is also very convenient, and well adapted for assaying. Of the volumetric methods, one is suited for technical purposes, the other for the estimation of small quantities of copper. For technical purposes there are, besides, also several colorimetric methods, proposed by HEINE., VON HUBERT, JACQUELAIN, A. MUL- LER, and others, which are, all of them, based upon the comparison of an ammoniacal solution of copper, of unknown strength, with others of known strength.* LEVOL'S indirect method of estimating copper, which is based upon the diminution of weight suffered by a strip of copper when digested in a close-stoppered flask with ammoniacal solution of copper till decolorization is effected, takes too much time, and is apt to give false results (PHILLIPS, f EKDMANN^;). The latter remark applies also to the indirect method proposed by RUNGE, which con- sists in boiling the solution of copper, free from nitric acid and ferric salts, in presence of some free hydrochloric acid, in a flask,, with a weighed strip of copper, and, after decolorization of the fluid, determining the loss of weight suffered by the copper. 1. Determination as Oupric Oxide. a. By direct Precipitation as Oxide. Heat the rather dilute neutral or acid solution in a platinum or porcelain dish, to incipient ebullition, add a somewhat dilute solu- tion of pure soda or potassa until the formation of a precipitate ceases, and keep the mixture a few minutes longer at a tempera- ture near boiling. Allow to subside, filter, wash by decantation twice or thrice, boiling up each time, then collect it on the filter,, wash thoroughly with hot water, dry, and ignite in a porcelain or platinum crucible, as directed 53. Do not use the blow-pipe- After ignition, and having added the ash of the filter, let the crucible cool in the desiccator, and weigh. The action of reducing gases must be carefully guarded against in the process of ignition. It will sometimes happen, though mostly from want of proper attention to the directions here given, that particles of the precipi- * This subject hardly comes within the scope of the present work. I there- fore refer to AL. MULLER, das Complemcntarcolorimeter, Chemnitz, 1854; Bo- DEMANN'S Probirkunst von KERL, 222; also to DEHMS, Zeitschr. f. anal. Chem. 3, 218, and GUSTAV BISCHOF, jun., Ib. 6, 459. f Annal. d. Chem. u. Pharm. 81, 208. \ Jour. f. prakt. Chem. 75, 211. 119.] COPPER. 313 tate adhere so tenaciously to the dish as to be mechanically irremov- able. In a case of this kind, after washing the dish thoroughly, dissolve the adhering particles with a few drops of nitric acid, and evaporate the solution over the principal mass of the precipitated oxide, before you proceed to ignite the latter. Should the solution be rather copious, it must first be concentrated by evaporation, until only very little of it is left. For the properties of the pre- cipitate, see 85. With proper attention to the directions here given, the results obtained by this method are quite accurate, otherwise they may be either too high or too low. Thus, if the solution be not sufficiently dilute, the precipitant will fail to throw down the whole of the copper ; or if the precipitate be not thoroughly washed with hot water, it will retain a portion of the alkali ; or if the ignited pre- cipitate be allowed to stand exposed to the air before it is weighed, an increase of weight will be the result ; and so, on the other hand, a diminution of weight, if the oxide be ignited with the filter or under the influence of reducing gases, as thereby cuprous oxide would be formed. Should a portion of the oxide have suffered reduction, it must be reoxidized by moistening with nitric acid, evaporating cautiously to dry ness, and exposing the residue to a gentle heat, increasing this gradually to a high degree of intensity. Let it be an invariable rule to test the filtrate for copper with hydrogen sulphide water. If , notwithstanding the strictest compli- ance with the directions here given, the addition of this reagent produces a precipitate, or imparts a brown tint to the fluid, this is to be attributed to the presence of organic matter ; in that case, concentrate the filtrate and wash-water by evaporation, acidify, precipitate with hydrogen sulphide water, filter, incinerate the filter, heat with nitric acid, dilute, filter, concentrate, precipitate with soda, and add the oxide obtained to the main quantity. Never neglect to test the cupric oxide after weighing for alkali or alkali salt by boiling it with water. If either is present, the oxide must be exhausted with hot water, and then reignited and reweighed. Finally, dissolve the oxide in hydrochloric acid to detect and if necessary to estimate any silicic acid it may contain. In default of sufficiently pure potash or soda, the carbonate* may be used, but the solution must not contain more than 1 grin, copper in the litre; the alkali carbonate must only be added slightly in excess, and the mixture must be boiled for half an hour. 314 I) KT V. K M I .\ A T ION. [ 1 1 9. The bluish-green precipitate will tlien turn dark brown and gran- ular, and may be easily washed (GIBBS*). From ammoniacal solutions, also, copper may be precipitated l)y soda or potassa. In the main, the process is conducted as above. After precipitation the mixture is heated, until the supernatant fluid has become perfectly colorless ; the fluid is then filtered off with the greatest possible expedition. If allowed to cool with the precipitate in it, a small portion of the latter would redissolve. b. By Precipitation ax Oxide, preceded by Ignition of the Substance. Heat the substance in a porcelain crucible, until the organic matter present is totally destroyed ; dissolve the residue in dilute nitric acid, filter if necessary, and treat the clear solution as directed in a. c. By Ignition. The salt is put into a platinum or porcelain crucible, and exposed to a very gentle heat, which is gradually increased to intense redness; the residue is then weighed. As cupric nitrate spirts strongly when ignited, it is always advisable to put it into a small covered platinum crucible, and to place the latter in a large one, also covered. With proper care, the results are accurate Cupric salts of organic acids may also be con verted into cupric oxide by simple ignition. To this end, the residue iirst obtained, which contains cuprous oxide, is completely oxidized by ignition with mercuric oxide (which leaves no residue on ignition), or, with less advantage, by repeated moistening with nitric acid, and ignition. A loss of substance is generally incurred by the use of nitric acid from the difficulty of avoiding spirting. 2. Determination at* Metallic Copper, a. By Precipitation with Zinc or Cadmium.^ Introduce the solution of copper, after having, if required, first freed it from nitric acid, by evaporation with hydrochloric acid or * Zeitschr. f. anal. Chem. 7, 258. f The method of precipitating copper by iron or zinc, and weighing it in the metallic form, was proposed long ago ; see PFAFF'S Handbuch der analytischen Chemie, Altoua, 1822, 2, 269; where the reasons are given for preferring zinc as a precipitant, and hydrogen sulphide is recommended as a test for ascertaining whether the precipitation is complete. I mention this with reference to F. MOHR'S paper in the Annal. d. Chem. u. Pharm. 96, 215, and BODEMANN'S Probirkunst von KERL, 220.' 119.] COPPER. 315 sulphuric acid, into a weighed platinum dish , dilute, if necessary with some water, throw in a piece of zinc (soluble in hydrochloric acid without residue), and add, if necessary, hydrochloric acid in sufficient quantity to produce a moderate evolution of hydrogen. If, on the other hand, this evolution should be too brisk, owing to too large excess of acid, add a little water. Cover the dish with a watch-glass, which is afterwards rinsed into the dish with the aid of a washing-bottle. The separation of the copper begins imme- diately ; a large proportion of it is deposited on the platinum in form of a solid coating; another portion separates, more particu- larly from concentrated solutions, in the form of red spongy masses. Application of heat, though it promotes the reaction, is not abso- lutely necessary ; but there must always be sufficient free acid present to keep up the evolution of hydrogen. After the lapse of about an hour or two, the whole of the copper has separated. To make sure of this, test a small portion of the supernatant fluid with hydrogen sulphide water ; if this fails to impart a brown tint to it, you may safely assume that the precipitation of the copper is complete. Ascertain now, also, whether the zinc is entirely dis- solved, by feeling about for any hard lumps with a glass rod, and observing whether renewed evolution of hydrogen will take place upon addition of some 'hydrochloric acid. If the results are satis- factory in this respect also, press the copper together with the glass rod, decant the clear fluid, which is an easy operation, pour, with- out loss of time, boiling water into the dish, decant again, and repeat this operation until the washings are quite free from hydro- chloric acid. Decant the water now as far as practicable, rinse the dish with strong alcohol, dry at 100, let it cool, and weigh. If you have no platinum dish, the precipitation may be effected also in a porcelain crucible or glass dish ; but it will, in that case, take a longer time ; and the whole of the copper will be obtained in loose masses, and not firmly adhering to the sides of the crucible or dish, as in the case of precipitation in platinum vessels. The results are very accurate. The direct experiment, No. 78, gave 10OO and 100-06, instead of 100. FK. MOHR (loc. cit.) obtained equally satisfactory results by precipitating in a porcelain crucible.* * STOKER (On the alloys of copper and zinc, Cambridge, 1860, p. 47) says that the precipitated copper retains water, but I have not found this to be the case. 316 DKT.KKMINAT10N. [ Zinc being sometimes difficult to obtain of sufficient purity, cadmium may be used instead; it dissolves with less violence in strongly acid copper solutions. It maybe used in the form of rod in which it usually occurs in commerce (CLASSEN*). 1). I>y Precipitation with tlte Galvanic Current. This method makes us independent of pure zinc or cadmium, and yields the copper in a compact form, readily washed and deter- mined. It is now largely used in copper works, constant batteries have been employed for it, and the whole process has been organ- ized for use on a large scale by LUCKOW, and adopted by the Mans- feld Ober-Berg-und Hut ten-Direction in Eisleben.f A small elec- trolytic apparatus without separate battery, for single precipitations,, has been described by ULLGKEN.J: c. By Ignition in Hydrogen. The oxides of copper when ignited in a current of pure hydro- gen are converted into metallic copper, and may thus be conven- iently analyzed. Occasionally the cupric oxide obtained by 1, a or b, is reduced either at once, or after weighing ; in the latter case the reduction serves as a control. 3. Determination as Cuprous Sulphide. a. By Precipitation as Cupric Sulphide. Precipitate the solution which is best moderately acid, but should not contain a great excess of nitric acid according to the quantity of copper present, either by the addition of strong hydro- gen sulphide water, or bypassing the gas. In the absence of nitric acid it is well to heat nearly to boiling while the gas is passing, as this makes the precipitate denser, and it is more easily washed. When the precipitate has fully subsided, and you have made sure that the supernatant fluid is no longer colored or precipitated by strong hydrogen xulphide water, filter quickly, wasli the precipi- tate without intermission with water containing hydrogen sulphide, and dry on the filter with some expedition. Transfer to a weighed porcelain crucible, add the filter-ash and some pure powdered sul- phur, and ignite strongly in a stream of hydrogen ( 108, fig. 50). It is advisable to use a glass blow-pipe. The results are very accu- rate (H. EOSE). * Journ. f. prakt. Chem. 96, 259. f Zeitschr. f. anal. Chem. 8, 23 and 11, 1. Compare also GIBBS, Ib. 3, 334, and LECOQ DE BOISBAUDAN, Ib. 7, 253. t /'> ?> 442. Pogg. Annal. 110, 138. 119. ] COPPER. 317 This method, which was recommended by BERZELIUS, and after- wards by BRUNNER, has only lately received a very practical form, from the apparatus introduced by H. ROSE. I feel great pleasure in recommending it. In my own laboratory it is in frequent use. o. By Precipitation as Cuprous Sulphocyanate^ after RIVOT.* The solution should be as free as possible from nitric acid and free chlorine, and should contain little or no free acid. Add sul- phurous or hypophosphorous acid in sufficient quantity, and then solution of potassium sulphocyanate in the least possible excess. The copper precipitates as white cuprous sulphocyanate. It is filtered after standing some time, washed and dried, mixed with sulphur, ignited in hydrogen in the apparatus mentioned in #, and this ignition with sulphur is repeated till the weight is constant. The precipitate may also be collected on a weighed filter, dried at 100, and then weighed. The experiment, Xo. 80, conducted in the latter way, gave 99'66 instead of 100. The process yields satisfactory results, but they are always inclined to be a little too low, as the cuprous sulphocyanate is not absolutely insoluble. The loss is larger in the presence of much free acid. c. Cuprous and cupric oxide, cupric sulphate, and many other salts of copper (but not chloride, bromide, or iodide) may be directly converted into cuprous sulphide, by mixing with sulphur and igniting in hydrogen as in a (H. ROSE, loo. rit.). The results are thoroughly satisfactory. 4. Volumetric Methods. a. DE HAEN'S METHOD.! I recommend this method, which was devised in my own laboratory, as more especially applicable in cases where small quantities of copper are to be estimated in an expeditious way. The method is based upon the fact that, when a cupric salt in solution is mixed with potassium iodide in excess, cuprous iodide and free iodine are formed, the latter remaining dissolved in the solution of potassium iodide : CuSO 4 + 2KI =. Cul + K 2 SO 4 + I. Now, by estimating the iodine by BUNSEN'S method, or with sodium thiosulphate ( 146), we learn the quantity of copper, as 1 at, iodine (126-85) corresponds to 1 at. copper (63-4). The following is the most convenient way of proceeding: Dissolve the compound *Compt. Rend. 38, 868; Journ. f. prakt. Chem. 62, 252. f Annal. d. Chem. u. Pharm. 91, 237. 318 DETERMINATION. |$12<). of copper in sulphuric acid, best to a neutral solution ; a moderate excess of free sulphuric acid, however, does not injuriously affect the process. Dilute the solution, in a measuring flask, to a defi- nite volume; 100 c.c. should contain from 1 to 2 grin, of copper. Introduce now about 10 c.c. of potassium iodide solution (1 in 10) into a stoppered bottle, add 10 c.c. of the copper solution, mix, allow to stand 10 minutes, and then determine the separated iodine, either with sulphurous acid and iodine ( 146, 1), or with sodium thiosulphate ( 146, 2). The copper solution must be free from ferric salts and other bodies w r hich decompose potassium iodide, also free nitric acid, and free hydrochloric acid ; and the solution must not be allowed to stand too long before titration. With strict attention to these rules, the results are accurate. I)E HAEN obtained, for instance, "3567 instead of '3566 of cupric sul- phate, 99;89 and lOO'l instead of 100 of metallic copper. Further experiments (No. 81) have convinced me, however, that, though the results attainable by this method are satisfactory, they are not always quite so accurate as would be supposed from the above figures given by DE HAEN. Acting upon FR. MOHK'S suggestion, I tried to counteract the injurious influence of the presence of nitric acid, by adding to the solution containing nitric acid, first, ammonia in excess, then hydrochloric acid to slight excess; the result was by no means satisfactory. The reason of this is that a solution of ammonium nitrate, mixed with some hydrochloric acid, will, even after a short time, begin to liberate iodine from solution of potassium iodide. 120. 6. BISMUTH. a. Solution. Metallic bismuth, bismuth trioxide, and all other compounds of that metal, are dissolved best in nitric acid, more or less diluted. It must be borne in mind that hydrochloric acid solutions of bismuth, if concentrated, cannot be evaporated without loss of bismuth chloride. ~b. Determination. Bismuth is weighed in the form of trioxide, of chromate, of sulphide, or in the metallic state. The compounds of bismuth are converted into trioxide by ignition, by precipitation as basic car- 120.] BISMUTH. 319 bonate, or by repeated evaporation of the nitric solution. These are sometimes preceded by separation as sulphide. The deter- mination as metallic bismuth is frequently preceded by precipita- tion as sulphide or as basic chloride. We may convert into 1. BISMUTH TRIOXIDE: a. By Precipitation as basic Bismuth Carbonate. All com- pounds of bismuth which dissolve in nitric acid to nitrate, no other acid remaining in the solution. b. By Ignition. a. Bismuth salts pf readily volatile oxygen acids. ft. Bismuth salts of organic acids. c. By Evaporation. Bismuth in nitric acid solution. d. By Precipitation as Bismuth Trisulphide. All compounds of bismuth without exception. 2. BISMUTH CHROMATE. All compounds named in 1, a. 3. BISMUTH TRISULPHIDE. The compounds *of bismuth without exception. 4. METALLIC BISMUTH : The trioxide and oxygen salts, the sulphide, the basic chloride, in which latter form the bismuth may be precipitated out of all its solutions. 1. Determination of Bismuth as Trioxide. a. By Precipitation as Bismuth Carbonate. If the solution is concentrated add water, taking no notice of any precipitate of basic nitrate that may be formed. Mix with ammonium carbonate in very slight excess, and heat for some time nearly to boiling ; filter, dry the precipitate, and ignite in the man- ner directed 116, 1 (Ignition of lead carbonate) ; the process of ignition serves to convert the carbonate into bismuth trioxide. For the properties of the precipitate and residue, see 86. The method gives accurate results, though generally a trifle too low, owing to the circumstance that bismuth carbonate is not absolutely insoluble in ammonium carbonate. Were you to attempt to precipitate bismuth, by means of ammonium carbonate, from solutions con- taining sulphuric acid or hydrochloric acid, you would obtain incorrect results, since with the basic carbonate, basic sulphate or basic chloride would be precipitated, which are not decomposed by excess of ammonium carbonate. Were you to filter off the precipi- tate without warming, a considerable loss would be sustained, as 320 DETERMINATION. [ 120. the whole of the basic carbonate would not have been separated .(Expt. No. 83). J. By Ignition. a. Compounds like bismuth carbonate or nitrate are ignited in a porcelain crucible until their weight remains constant. /?. Salts of organic acids are treated like the corresponding compounds of copper ( 119, 1, c). c. By Evaporation. The solution of the nitrate is evaporated, in a porcelain dish on the water-bath, till the neutral salt remains in syrupy solution ; add water, loosen the white crust that is formed with a glass rod from the sides, evaporate again on a water-bath, reprecipitate with water, and repeat the whole operation three or four times. After the dry mass on the water-bath has ceased to smell of nitric acid, it is allowed to cool thoroughly, and then treated with cold water containing a little ammonium nitrate (1 in 500) ; after the residue and fluid have been a short time together, filter, wash with the weak solution of ammonium nitrate, dry and ignite ( 53). Results very satisfactory (J. LOWE*). d. By Precipitation as Bismuth Trisulphide. Dilute the solution with water slightly acidulated with acetic acid (to prevent the precipitation of a basic salt), and precipitate with hydrogen sulphide water or gas ; allow the precipitate to subside, and test a portion of the supernatant fluid with hydrogen sulphide water: if it remains clear, which is a sign that the bismuth is completely precipitated, filter (the filtrate should smell strongly of H 3 S), and wash the precipitate with water containing hydrogen sulphide. Or mix with ammonia until the free acid is neutralized, then add ammonium sulphide in excess, and allow to digest for some time. The washed precipitate may now be weighed in three different forms, viz., as trisulphide, as metal, or as trioxide. The treatment in the two former cases will be described in 3 and 4 : in the latter case proceed as follows : Spread the filter out on a glass plate and remove the precipitate to a vessel by means of a jet of water from the wash-bottle or, if this is not practicable, put the precipitate and filter together into the vessel and heat gently with moderately strong nitric acid * Journ. f . prakt. Chem. 74, 344. 120.] BISMUTH. 321 until, complete decomposition is effected ; the solution is then diluted with water slightly acidulated with acetic or nitric acid, and filtered, the filter being washed with the acidulated water; the filtrate is then finally precipitated as directed in a. 2. Determination of Bismuth as Chromate (J. LOWE*). Pour the solution of bismuth, which must be as neutral as possible, and must, if necessary, be first freed from the excess of nitric acid by evaporation on the water-bath, into a warm solution of pure potassium dichromate in a porcelain dish, with stirring, and take care to leave the alkali chromate slightly in excess. Rinse the vessel which contained the solution of bismuth with water containing nitric acid into the porcelain dish. The precipi- tate formed must be orange-yellow, and dense throughout ; if it is nocculent, and has the color of the yolk of an egg, this is a sign that there is a deficiency of potassium dichromate ; in which case add a fresh quantity of this salt, taking care, however, to guard against too great an excess, and boil until the precipitate presents the proper appearance. Boil the contents of the dish for ten minutes, with stirring ; then wash the precipitate, first by repeated boiling with water and decantation on to a weighed filter, at last thoroughly on the latter with boiling water ; dry at about 120, and weigh. For the properties and composition of the precipitate, see 86. Results very satisfactory. 3. Determination of Bismuth as Trisulphide. Precipitate the bismuth as trisulphide according to 1, d. I? the precipitate contains free sulphur, extract the latter by boiling with solution of sodium sulphite, or by treatment with carbon disulphide (compare the determination of mercury as sulphide, 118, 3), collect on a weighed filter, dry at 100, and weigh. The drying must be conducted with caution. At first the precipitate loses weight, by the evaporation of water, then it gains weight, from the absorption of oxygen. Hence you should weigh every half hour, and take the lowest weight as the correct one. Compare Expt. No. 58. Properties and composition, 86, g. The bismuth sulphide cannot be conveniently converted into the metallic state by ignition in hydrogen, as its complete decom- position is a work of considerable time. As regards reduction with potassium cyanide, see 4. * Journ. f. prakt. Chem. 67, 464. 322 DETERMINATION. [ 120. 4. Determination of Bismuth as Metal. The oxide, sulphide, or basic chloride that are to be reduced are fused in a porcelain crucible with five times their quantity of ordinary potassium cyanide. The crucible must be large enough. In the case of oxide and basic chloride, the reduction is completed in a short time at a gentle heat ; sulphide, on the other hand, requires longer fusion and a higher temperature. The operation has been successful if on treatment with water metallic grains are obtained. These grains are first washed completely and rapidly with water, then with weak and lastly with strong alcohol, dried and weighed. If you have been reducing the sulphide, and on treating the fused mass with water a black powder (a mixture of bismuth with bismuth sulphide) is visible, besides the metallic grains, it is necessary to fuse the former again with potassium cyanide. It sometimes happens that the crucible is attacked, and particles of porcelain are found mixed with the metallic bismuth ; to prevent this from spoiling the analysis, weigh the crucible together with a small dried filter before the experiment, collect the rnetal on the filter, dry and weigh the crucible with the filter and bismuth again. Kesults good (H. ROSE*). The precipitation of bismuth as basic chloride, and the reduc- tion of the latter with potassium cyanide, has been recommended by II. RosE.f The process is conducted as follows : Nearly neu- tralize any large excess of acid that may be present with potassa, soda, or ammonia, add ammonium chloride in sufficient quantity (if hydrochloric acid is not already present), and then a rather large quantity of water. After allowing to stand some time, test whether a portion of the clear supernatant fluid is rendered turbid by a further addition of water ; and then, if required, add water to the whole till the precipitation is complete. Finally filter, wash com- pletely with cold water, dry and fuse according to the directions just given with potassium cyanide. It is less advisable to dry the precipitate at 100, weigh and calculate the metal present from the formula BiOCl, as washing causes a slight alteration in its com- position (unless a little hydrochloric acid is added to the wash- water, which is inconvenient when the precipitate is collected on a weighed filter), and if precipitated in the presence of sulphuric, phosphoric acids, &c., it is liable to contain small quantities of these acids. Results accurate. * Pogg. Annal. 91, 104, and 110, 136. f If). 110, 425. 121.] CADMIDM. 323 121. 7. CADMIUM. a. Solution. Cadmium, its oxide, and all the other compounds insoluble in water, are dissolved in hydrochloric acid or in nitric acid. b. Determination. Cadmium is weighed either in the form of oxide, or in that of sulphide ( 87). It may also be weighed as sulphate, and in the absence of other bases precipitable by oxalic acid, it may be esti- mated volumetrically. We may convert into 1. CADMIUM OXIDE: a. By Precipitation. The compounds of cadmium which are soluble in water ; the insoluble compounds, the acid of which is removed upon solution in hydrochloric acid ; cadmium salts of organic acids. o. By Ignition. Cadmium salts of readily volatile or easily decomposable inorganic oxygen acids. 2. CADMIUM SULPHDDE : All compounds of cadmium without exception. 3. CADMIUM SULPHATE : All compounds of cadmium, in the absence of other non-volatile substances. 1. Determination as Cadmium Oxide. a. By Precipitation. Precipitate with potassium carbonate, wash the precipitated cadmium carbonate, and convert it, by ignition, into oxide. The precipitation is conducted as in the case of zinc, 108, 1, a. The cadmium oxide which adheres to the filter may easily be reduced and volatilized ; it is therefore necessary to be cautious. In the first place choose a thin filter, transfer the dried precipitate as com- pletely as possible to the crucible, replace the filter in the funnel, and moisten it with ammonium nitrate solution, allow to dry, and then burn carefully in a coil of platinum wire. Let the ash fall into the crucible containing the mass of the precipitate, ignite carefully, avoiding the action of reducing gases, and finally weigh. It is difficult to remove the last portions of carbonic acid ; you must therefore repeat the ignition till the weight remains constant. 324 DETERMINATION. [121. Properties of precipitate and residue, 87. Results generally a little too low. Z>. By Ignition. Same process as for zinc, 108, 1, c. 2. Determination as Cadmium Sulphide. It is best to precipitate the moderately acid solution with hydro- gen sulphide water or gas, which must be used in sufficient excess. The presence of a considerable quantity of free hydrochloric or nitric acid may especially if the solution is not enough diluted prevent complete precipitation, hence such an excess should be avoided, and the clear supernatant fluid should in all cases be tested, by the addition of a relatively large amount of hydrogen sulphide water to a portion, before being filtered. Alkaline solutions of cadmium may be precipitated with ammonium sulphide. If the cadmium sulphide is free from admixed sulphur, it may be at once collected on a weighed filter, washed first with diluted hydrogen sulphide water mixed with a little hydrochloric acid, then with pure w r ater, dried at 100, and weighed ; if, on the contrary, it con- tains free sulphur, it may be purified by boiling with a solution of sodium sulphite, or by treatment with carbon di sulphide (see Mer- curic Sulphide, 118, 3). Results accurate. The precipitation of sulphur may occasionally be obviated by adding to the cadmium ;solution potassium cyanide till the precipitate first formed is redis- solved, and then precipitating this solution with hydrogen sulphide. If the cadmium sulphide is not to be weighed as such, warm it, together with the filter, with moderately strong hydrochloric acid, till the precipitate has dissolved and the odor of hydrogen sulphide is no longer perceptible, filter and precipitate the solution as in 1, #, after having removed the excess of free acid for the most part by evaporation. 3. Determination as Cadmium Sulphate. Same process as for magnesium ( 104, 1). The CdSO 4 may be rather strongly ignited without decomposition. 4. W. GIBBS* determines cadmium volumetrically by mixing the concentrated solution of the sulphate, nitrate, or chloride with excess of oxalic acid and a quantity of strong alcohol, filtering, washing with alcohol, dissolving in hot hydrochloric acid and *Zeitschr. f. anal. Chem.7, 259. 122.] PALLADIUM. 325 determining the oxalic acid with permanganate ( 137). "W. G. LEISON* obtained satisfactory results by this process. Supplement to the Fifth Group. 122. 8. PALLADIUM. Palladium is converted, for the purpose of estimation, into the metallic state or in many separations mto potassium palladia chloride. 1. Determination a>- Palladium. a. Neutralize the solution of palladious chloride almost com- pletely with sodium carbonate, mix with solution of mercuric cyanide ; and heat gently for some time, until the odor of hydro- cyanic acid has gone off. A yellowish-white precipitate of palladi- ous cyanide will subside ; from dilute solutions, only after the lapse of some time. Wash first by decantation, then on the filter, dry thoroughly, ignite cautiously, finally over the gas blowpipe till the palladium paracyanide first formed is decomposed, then ignite in hydrogen, since the palladium has been slightly oxidized As soon as the lamp is removed, stop the hydrogen to prevent absorption, and w r eigh the metal. If the solution contains palladious nitrate, evaporate it first with hydrochloric acid to dryness ; as otherwise the precipitate obtained deflagrates upon ignition (WOLLASTON). Results exact. b. Mix the solution of palladious chloride or nitrate with sodium or potassium formate, and warm until no more carbonic acid escapes. The palladium precipitates in brilliant scales (DoBE- REINER). c. Precipitate the acid solution of palladium with hydrogen sulphide, filter, w^ash with boiling water, roast, dissolve in hydro- chloric acid and nitric acid, and precipitate as in a. Exposed to a moderate red heat metallic palladium becomes covered with a film varying from violet to blue, but at a higher temperature it recovers its lustre, which it keeps after being sud- denly cooled, for instance, with cold water. This tarnishing and recovery of the metallic lustre is not attended with any percepti- * Zeitschr. f. anal. Chem. 10, 343. 326 DETEKMINATION. [ 123. ble difference of weight. Palladium which has taken up oxygen is immediately reduced in hydrogen ; when cooled in the current of gas, it retains some absorbed hydrogen. Palladium requires the very highest degree of heat for its fusion. It dissolves readily in nitrohydrochloric acid, with difficulty in pure nitric acid, more easily in nitric acid containing nitrous acid, with difficulty in boil- ing concentrated sulphuric acid. 2. Determination as Potassium Palladic Chloride. Evaporate the solution of palladic chloride with potassium chloride and nitric acid to dryness, and treat the mass when cold with alcohol of '833 sp. gr., in which the double salt is insoluble. Collect on a weighed filter, dry at 100, and weigh. Results a little too low, as traces of the double salt pass away with the alcohol washings (BEEZELIUS). Instead of weighing the double salt you may ignite in hydrogen, remove the potassium chloride with water and weigh the metal obtained. This method is indeed to be pre- ferred, as it prevents any potassiiim chloride in the precipitate from affecting the result. POTASSIUM PALLADIC CHLORIDE consists of microscopic octa- hedra ; it presents the appearance of a vermilion or, if the crystals are somewhat large, of a brown pow r der. It is very slightly solu- ble in cold water ; it is almost insoluble in cold alcohol of the above strength. It contains 26'806 palladium. Sixth Group. GOLD PLATINUM ANTIMONY TIN IN STANNIC COMPOUNDS TIN IN 8TANNOUS COMPOUNDS ARSENIOUS AND AKSENIC ACIDS ( MO- LYBDIC ACID). 123. 1. GOLD. a. Solution. Metallic gold, and all compounds of gold insoluble in water, are warmed with hydrochloric acid, and nitric acid is gradually added until complete solution is effected ; or they are repeatedly digested with strong chlorine water. The latter method is resorted to more especially in cases where the quantity of gold to be dis- solved is small, and mixed with foreign oxides which it is wished 123.]. GOLD. 327 to leave undissolved. According to W. SKEY* tincture of iodine, or, for larger quantities of gold, bromine water, is better than chlo- rine water. They give solutions freer from other metals than the chlorine water gives. b. Determination. Gold is always weighed in the metallic state. The compounds are brought into this form, either by ignition or by precipitation, as gold, or auric sulphide. We convert into METALLIC GOLD : a. By Ignition. All compounds of gold which contain no fixed acid, or other body. b. By Precipitation as metallic gold. All compounds of gold without exception in cases where a is inapplicable. c. By Precipitation as auric sulphide. This method serves to effect the separation of gold from certain other metals which may be mixed with it in a solution. Determination as Metallic Gold. a. By Ignition. Heat the compound, in a covered porcelain crucible, very gently at first, but finally to redness, and weigh the residuary pure gold. For properties of the residue, see 88. The results are most accurate. b. By Precipitation as Metallic Gold. a. The solution is free from Nitric Acid. Mix the solution with a little hydrochloric acid, if it does not already contain some of that acid in the free state, and add a clear solution of ferrous sulphate in excess ; heat gently for a few hours until the precipi- tated fine gold powder has completely subsided ; filter, wash, dry, and ignite according to 52. A porcelain dish is a more appro- priate vessel to effect the precipitation in than a beaker, as the heavy fine gold powder is more readily rinsed out of the former- than out of the latter. There are no sources of error inherent in the method. ft. The solution of Gold contains Nitric Acid. Evaporate the solution, on a water-bath, to the consistence of syrup, adding from time to time hydrochloric acid ; dissolve the residue in water con- * Zeitschr. f. anal. Chem. 10, 221. 328 DETERMINATION. [ 123. taining hydrochloric acid, and treat the solution as directed in a. It will sometimes happen that the residue does not dissolve to a clear fluid, in consequence of a partial decomposition of auric chlo- ride into aurous chloride and metallic gold ; however, this is a mat- ter of perfect indifference. y. In cases where it is wished to avoid the presence of iron in the filtrate, the gold may be reduced by means of oxalic acid. To this end, the dilute solution freed previously, if necessary, from nitric acid, in the manner directed in ft is mixed, in a beaker, with oxalic acid, or with ammonium oxalate in excess,, some sul- phuric acid added (if that acid is not already present in the free state), and the vessel, covered with a glass plate, is kept standing- for two days in a moderately warm place. At the end of that time, the whole of the gold will be found to have separated in small yellow scales, which are collected on a filter,, washed first with dilute hydrochloric acid, then with water, dried, and ignited.. If the gold solution contains a large excess of hydrochloric acid r the latter should be for the most part evaporated, before the solu- tion is diluted and the oxalic acid added. If the gold solution con- tains chlorides of alkali metals, it is necessary to dilute largely, and allow to stand for a long time, in order to effect complete precipi- tation (H. ROSE). &. The gold may also be thrown down in the metallic form by hydrate of chloral* in the presence of potash. Warm the solution, add the chloral, then pure potash in excess, and boil for a minute or so. The gold is precipitated with evolution of chloroform. . Finally, gold may be thrown down by many metals, such as zinc, cadmium, magnesium, &c. The latter has been recommended by ScHEiBLERf for the analysis of the gold salts of organic bases. The precipitate is first washed with hydrochloric acid, then with water. c. By Precipitation as Auric Sulphide. Hydrogen sulphide gas is transmitted in excess through the dilute solution containing some free acid; the precipitate formed is speedily filtered off, without heating, washed, dried, and ignited in a porcelain crucible. For the properties of the precipitate, see 88. No sources of error. * HAGEH'S pharmac. Centralhalle, 11, 393. f Ber. der dcutscli. chem. Gescllsch. 1869, 295. 124.] PLATINUM. 329 i 124. 2. PLATINUM. a. Solution. Metallic platinum, and the compounds of platinum which are insoluble in water, are dissolved by digestion, at a gentle heat, with nitrohydrochloric acid. b. Determination. Platinum is invariably weighed in the metallic state, to which condition its compounds are brought, either by precipitation aa ammonium platinic chloride, potassium platinic chloride, or pla- tinic sulphide, or by ignition, or by precipitation with reducing^ agents. All compounds of platinum, without exception, may, in most cases, be converted into platinum by either of these methods. Which is the most advantageous process to be pursued in special instances, depends entirely upon the circumstances. The reduc- tion to the 1 metallic state by simple ignition is preferable to the other methods, in all cases where admissible. The precipitation as platinic sulphide is resorted to exclusively to eifect the separation of platinum from other metals. Determination as Metallic Platinum. a. By Precipitation as Ammonium Platinic Chloride. The solution must be concentrated if necessary by evaporation on a water-bath. Mix, in a beaker, with ammonia until the excess of acid (that is, supposing an excess of acid to be present) is nearly saturated; add ammonium chloride in excess, and mix the fluid with a pretty large quantity of strong alcohol. Cover the beaker now with a glass plate, and let it stand for twenty-four hours, after which filter, wash the precipitate with alcohol of about '80 per cent., till the substances to be separated are removed, dry carefully, ignite according to 99, 2, and weigh. In the case of large quan- tities the final ignition is advantageously conducted in a stream of hydrogen ( 108, fig. 50), in, order to be quite sure of effecting complete decomposition. For the properties of the precipitate and residue, see 89. The results are satisfactory, though generally a little too low, as the ammonium platinic chloride is not altogether insoluble in alcohol of the above strength (Expt. No. 16), and as the fumes of ammonium chloride are liable to carry away traces of 330 DETERMINATION. [ 124. the jet nndecomposed double chloride, if the application of heat is not conducted with the greatest care. If the precipitated ammonium platinic chloride were weighed in that form, the results would be inaccurate, since, as I have con- vinced myself by direct experiments, it is impossible to completely free the double chloride, by washing with alcohol, from all traces of the ammonium chloride thrown down with it, without dissolving at the same time a notable portion of the double chloride. As a general rule, the results obtained by weighing the ammonium pla- tinic chloride in that form are one or two per cent, too high. b. By Precipitation as Potassium Platinic Chloride. Mix the solution, in a beaker, with potassa, until the greater part of the excess of acid (if there be any) is neutralized ; add potassium chloride slightly in excess, and finally a pretty large quantity of strong alcohol ; should your solution of platinum be very dilute, you must concentrate it previously to the addition of the alcohol. After twenty-four hours, collect the precipitate upon n rather small unweighed filter, wash with alcohol of 80 per cent., dry thoroughly at 100, and transfer to a porcelain crucible, dis- solving the portion which adheres to the filter, and evaporating the solution in the crucible. See 97, 3. Next, by igniting with hydrogen by means of apparatus described in 108, page 251, con- vert the compound into metallic platinum and potassium chloride. Reduction is best effected if the heat is very gradually applied, and does not at all quite reach the point at which potassium <;hloride fuses. After reduction, wash out the potassium chloride, ignite and weigh the platinum. For the properties of the precipitate :and residue, see 89. The results are more accurate than those obtained by method &, since, on the one hand, the potassium platinic chloride is more insoluble in alcohol than the corresponding ammonium salt ; and, on the other hand, loss of substance is less likely to occur during ignition. To weigh the potassium platinic chloride in that form would not be practicable, as it is impossible to remove, by washing with alcohol, all traces of the potassium chloride thrown down with it, without, at the same time, dissolving a portion of the double chloride. c. By Precipitation as Platinic Sulphide. Precipitate the solution with hydrogen sulphide water or gas, 125.] ANTIMONY. 331 according to circumstances, heat the mixture to incipient ebulli- tion, filter, wash the precipitate, dry, and ignite according to 52. For the properties of the precipitate and residue, see 89. The results are accurate. d. By Ignition. Same process as for gold, 123. For the properties of the residue, see 89. The results are most accurate. e. By Precipitation with Reducing Agents. Various reducing agents may be employed to precipitate plati- num from its solutions in the metallic state. The reduction is very promptly effected by ferrous sulphate and potassa or soda (the protosesquioxide of iron being removed by subsequent addi- tion of hydrochloric acid, HEMPEL), or by pure zinc or magnesium (the excess of which is removed by hydrochloric acid) ; somewhat more slowly, and only with application of heat, by alkali formiates. Mercurous nitrate also precipitates the whole of the platinum from solution of platinic chloride ; upon igniting the brown precipitate obtained, fumes of inercurous chloride escape, and metallic plati- num remains. 125. 3. ANTIMONY. a. Solution. Antimonious oxide, and the compounds of antimony which are insoluble in water, or are decomposed by that agent, are dissolved in more or less concentrated hydrochloric acid. Metallic antimony is dissolved best in nitrohydrochloric acid. The ebullition of a hydrochloric acid solution of antimonious chloride is attended with volatilization of traces of the latter ; the concentration of a solution of the kind by evaporation involves accordingly loss of substance. Solutions so highly dilute as to necessitate a recourse to evapora- tion must therefore previously be supersaturated with potassa. Solutions of antimonious chloride, which it is intended to dilute with water, must previously be mixed with tartaric acid, to prevent the separation of basic salt. In diluting an acid solution of anti- monic acid in hydrochloric acid, the water must not be added gradually and in small quantities at a time, which would make the fluid turbid, but in sufficient quantity at once, which will leave the fluid clear. 332 DETERMINATION. [ h. Determination . Antimony may be weighed as antmioiiious sulphide tetrod'Ule, \\\ separations it is sometimes weighed as metallic anti- mony , or it is estimated volumetrically. Antimony in solution is almost invariably first precipitated as sulphide, which is then, with the view of estimation, converted into anhydrous sulphide, or determined volnmetrically. 1. Precipitation a* Antiinon.iou# Sulphide. Add to the antimony solution hydrochloric acid, if not already present, then tartaric acid, and dilute with water, if necessary. Introduce the clear fluid into a flask, closed with a doubly perfo- rated cork ; through one of the perforations passes a tube y bent outside at a right angle, which nearly extends to the bottom of the flask ; through the other perf oration passes another tube, bent out- side twice at right angles, which reaches only a short way into the flask ; the outer end of this tube dips slightly under water. Con- duct through the first tube hydrogen sulphide gas, until it pre- dominates strongly; put the flask in a moderately warm place, and after some time conduct carbon dioxide into the fluid, until the excess of the other gas is almost completely removed. If there is no reason against it, from the presence of a large quantity of hydrochloric acid, or from the presence of nitric acid, it is well to- heat the solution during the passing of the gas, finally even boiling. The precipitate is then denser, and may be very easily washed (SHARPLES*). If the amount of the preet/pitate /* , the precipitate is subjected to the same treatment as in . 118, 17; and Zeitschr. f. anal. Chem. 2, 383. 336 DETERMINATION. [ 125. ft. Solution of Potassium Bichromate. Dissolve about 2*5 grm. to 1 litre. y. Solution of Ferrous Sulphate. Dissolve about 1/1 grm. iron wire in 20 c.c. dilute sulphuric acid (1 to 4), filter, and dilute to 1 litre. 8. Solution of Potassium Ferricyanide. Should be tolerably dilute and freshly prepared. 2. DETERMINATION OF THE SOLUTIONS. a f Relation betioeen the Solution of Chr ornate and the Solution of Ferrous Sulphate. Run into a beaker 10 c.c. of the chromate solution from the burette, add 5 c.c. of hydrochloric acid and 50 c.c. water, and then add iron solution from a burette till the fluid is green. Continue adding the iron solution, a c.c. at a time, test- ting after each addition whether a drop of the fluid, when brought in contact with a drop of the potassium ferricyanide, on a porcelain plate, manifesjts a distinct reaction for ferrous iron. As soon as this point is attained, add *5 c.c. of chromate solution and then iron solution two drops at a time, till the blue reaction just occurs. Now read off both burettes, and calculate how much chromate solution corresponds to 10 c.c. of iron solution. This experiment is to be repeated before every fresh series of analyses, as the iron solution gradually oxidizes. /?. Relation between the Chromate Solution and the Solution of Arsenious Acid. Transfer 10 c.c. of the arsenious solution to a beaker, add 20 c.c. hydrochloric acid of 1*2 sp. gr., and 80 100 c.c.* water, run in chromate solution till the yellow color of the fluid shows an excess, wait a few minutes, add excess of iron solu- tion, then again '5 chromate solution, and finally again iron solu- tion till the end-reaction appears (see above). Deduct from the total quantity of chromate solution employed, the amount corre- sponding to the iron used, and from the datum thus afforded calcu- late how much antimony corresponds to 100 c.c. of chromate solu- tion ; in other words, how much antimony is converted by the quantity of chromate mentioned from SbCl 3 into SbCl 6 . 3. THE ACTUAL ANALYSIS. In the absence of organic matter, heavy metallic oxides, and other * The water must he measured, for the action of chromic acid on arsenions acid (and also on antimonious chloride) is normal only if the fluid contains at least one sixth of its volume of hydrochloric acid of 1 '12 sp. gr. 125.] ANTIMONY. 337 bodies which are detrimental to the reaction, dissolve the antimo- nious compound at once in hydrochloric acid. The solution should contain not less than | of its volume of hydrochloric acid of 1-12 sp. gr. It is not advisable, on the other hand, that it should con- tain more than ^, otherwise the end-reaction with potassium ferri- cyanide is slower in making its appearance and loses its nicety. Tartaric acid cannot be employed as a solvent, since it interferes with the action of chromic acid on ferrous salts. Now proceed as directed in 2. If the direct determination of antimony in the hydrochloric acid solution is not practicable, precipitate it with hydrogen sulphide. Wash the precipitate, transfer it, together with the filter, to a small flask ; treat it with a sufficiency of hydro- chloric acid, dissolve by digestion on the water-bath, add a suffi- cient quantity of a nearly saturated solution of mercuric chloride in hydrochloric acid of 1*12 sp. gr. to remove the hydrogen sul- phide, and then proceed as directed. II. Titrcution with Potassium Permanganate. Here also the fluid must contain at least of its volume of hydrochloric acid of 1.12 sp. gr. The permanganate solution, which may contain about 1*5 grm. of the crystallized salt in a litre, is added to permanent reddening. The end-reaction is exact, and the conversion of antimonious to antiuionic chloride goes on uni- formly, although the degree of dilution may vary, provided the above relation between hydrochloric acid and water is kept up. It is not well that the hydrochloric acid should exceed J of the volume of the fluid, as in that qase the end-reaction would be too transitory. Tartaric acid, at least in the proportion to antimony in which it exists in tartar emetic, does not interfere with the reac- tion. Hence the permanganate may be standardized by the aid of solution of tartar emetic of known strength. If you have to analyze antimonious sulphide, proceed as directed I. 3 ; make the fluid mixed with mercuric chloride up to a certain volume, allow to settle, and use a measured portion of the perfectly clear solution for the experiment. My own experiments* have shown that KESSLER'S methods are also suitable for the estimation of very small quantities of anti- mony. * Zeitschr. f. anal. Chem. 8, 155. 338 DETEKMINATION. [ 126. J. Volumetric Estimation by determining the Hydrogen Sul- phide given up by the Sulphide (R. SCHNEIDER*). Both antimonions and antimonic sulphides yield under the action of boiling hydrochloric acid 3 mol. hydrogen sulphide for every 2 atoms of antimony. Hence, if the amount of the gas evolved under such circumstances is estimated, the amount of anti- mony is known. For decomposing the sulphide and absorbing the gas, the same apparatus serves as BUNSEN employs for his iodimetric analyses ( 130). The size of the boiling-flask should depend on the quan- tity of sulphide ; for quantities up to '4 grm. Sb Q S 3 , a flask of 100 c.c. is large enough ; for *4 1 grm., use a 200 c.c. flask. The body of the flask should be spherical, the neck rather narrow, long, and cylindrical. If the sulphide of antimony is on a filter, put both together into the flask. The hydrochloric acid should not be too concentrated. The determination of the hydrogen sulphide is best conducted according to the method given in 148, b. The results obtained by SCHNEIDER are satisfactory. If the precipitate contains anti- monious chloride, the results are of course false, and this would actually be the case if on precipitation with hydrogen sulphide the addition of the tartaric acid were omitted. 126. 4. TIN IN STANNOUS COMPOUNDS, and 5. TIN IN STANNIC COMPOUNDS. a. Solution. In dissolving compounds of tin soluble in water, a little hydro- chloric acid is added to insure a clear solution. Nearly all the compounds of tin insoluble in water dissolve in hydrochloric acid, or in aqua regia. The hydrate of metastannic acid may be dissolved by boiling with hydrochloric acid, decanting the fluid, and treating the residue with a large proportion of water. Ignited stannic oxide, and stannic compounds insoluble in acids, are prepared for solution in hydrochloric acid, by reducing them to the state of a fine pow- der, and fusing in a silver crucible with potassium or sodium hydroxide, in excess. Metallic tin is dissolved best in aqua regia ; the solution frequently contains metastannic chloride mixed with the stannic chloride (Tn. ScHEERERf). It is generally determined, * Pogg. Anna!. 110, 634. f Journ. f. prakt. Chcm. N. F. 3, 472. i^ 126.] TIN IX STANXOUS AND STANNIC COMPOUNDS. 339 however, by converting it into stannic oxide, without previous solution. Acid solutions of stannic salts, which contain hydrochlo- ric acid, or a chloride, cannot be concentrated by evaporation, not even after addition of nitric acid or sulphuric acid, without volatili- zation of stannic chloride taking place. b. Determination. Tin is weighed in the form of stannic oxide, into which it is converted, either by the agency of nitric acid, or by precipitation as stannic (or metastannic) acid, or by precipitation as sulphide. A great many volumetric methods of estimating tin have been pro- posed. They all depend on obtaining the tin in solution in the condition of stannous chloride, and converting this into stannic chloride either in alkaline or acid solution. A few only yield satis- factory results. We may convert into STANNIC OXIDE: a. By the Agency of Nitric Acid. Metallic tin, and those com- pounds of tin which contain no fixed acid, provided no compounds of chlorine be present. b. By Precipitation as Stannic (or Metastannic) Acid. All tin salts of volatile acids, provided no non- volatile organic .substances nor ferric salts be present. c. By Precipitation a$ Sulphide. All compounds of tin with- out exception. In methods a and c, it is quite indifferent whether the tin is present as a stannous or a stannic compound. The method b requires the tin to be present as a stannic salt. The volumetric methods may be employed in all cases ; but the estimation is simple and direct only where the tin is in solution as stannous chloride and free from other oxidizable bodies, or can readily be brought into this state. For the methods of determining stannous and stannic tin in presence of each other, I refer to Section Y. \ 1. Determination of Tin as Stannic Oxide. a. By Treating with Nitric Acid. This method is resorted to principally to convert the metallic tin into stannic oxide. For this purpose the finely-divided metal is put into a capacious flask, and moderately concentrated pure nitric acid (about 1'3 sp. gr.) gradually poured over it ; the flask is covered with a watch glass. "When the first tumultuous action of 340 DETERMINATION. [ 126. the acid lias somewhat abated, a gentle heat is applied until the metastannic acid formed appears of a pure white color, and further action of the acid is no longer perceptible. The contents of the flask are then transferred to a porcelain dish and evaporated on a water-bath nearly to dryness, water is then added, and the precipi- tate is collected on a filter, washed, till the washings scarcely red- den litmus paper, dried, ignited, and weighed. The ignition is effected best in a small porcelain crucible, according to 53 ; still a platinum crucible may also be used. A simple red heat is not sufficient to drive off all the water ; the ignition must therefore be finished over a gas blowpipe. Compounds of tin which contain no fixed substances may be converted into stannic oxide by treating them in a porcelain crucible with nitric acid, evaporating to dry- ness, and igniting the residue. If sulphuric acid be present, the expulsion of that acid may be promoted, in the last stages of the process, by ammonium carbonate, as in the case of acid potassium sulphate ( 97) ; here also the heat must be increased as much as possible at the end. For the properties of the residue, see 91. There are no inherent sources of error. Z>. By Precipitation as Stannic (or Metastannic) Acid. The application of this method presupposes the whole of the tin to be present in the state of stannic salts. Therefore, if a solu- tion contains stannous salts, either mix with chlorine water, or con- duct chlorine gas into it, or heat gently with chlorate of potassa, until the conversion of the stannous into stannic salts is effected. When this has been done, add ammonia until a permanent precipitate just begins to form, and then hydrochloric acid, drop by drop, until this precipitate is completely redissolved ; by this means a large excess of hydrochloric acid in the solution will be avoided. Add to the fluid so prepared a concentrated solution of ammonium nitrate (or sodium sulphate), and apply heat for some time, where- upon the whole of the tin will precipitate as stannic acid. Decant three times on to a filter, then collect the precipitate on the latter, wash thoroughly, dry, and ignite. To make quite sure that the whole of the tin has separated, you need simply, before proceeding to filter, add a few drops of the clear supernatant fluid to a hot solution of ammonium nitrate, or sodium sulphate, when the for- mation or non-formation of a precipitate will at once decide the question. The tin is also precipitated from metastannic chloride by the above reagents. 126. J TIN IN STANNOU8 AND STANNIC COMPOUNDS. 341 Tliis method, which we owe to J. LOWENTHAL, has been repeat- edly tested by him in my own laboratory,* is easy and convenient, and gives very accurate results. The decomposition is expressed by the equation, SnCl 4 + 4?s T a 3 SO 4 + 3H a O = H a SnO 3 + 4NaCl + 4NaHSO 4 , or in precipitating with ammonium nitrate : SnCl 4 + 4NH 4 NO 3 + 3H 2 O = HJSnO, + 4XH 4 C1 + 4HNO 3 . Tin may also, according to H. RosE,f be completely precipi- tated from stannic solutions by sulphuric acid. If the solution contains metastannic acid or metastannic chloride, the precipitation is effected without extraordinary dilution ; the other stannic com- pounds, however, require very considerable dilution. If free hydrochloric acid is absent, the precipitation is rapid ; in other cases 12 or 24 hours at least are required for perfect precipitation. Allow to settle thoroughly, before filtering, wash well (if hydro- chloric acid was present, till the washings give no turbidity with silver nitrate), dry and ignite, at last intensely with addition of some ammonium carbonate. The results obtained by OESTEN, and communicated by H. ROSE, are exact. c. By Precipitation as Stannotu or Stannic Sulphide. Precipitate the dilute moderately acid solution with hydrogen sulphide water or gas. If the tin was present in the solution as a stannous salt, and the precipitate consists accordingly of the brown stannous sulphide, keep the solution, supersaturated with hydrogen sulphide, standing for half an hour in a moderately warm place, and then filter. If, on the other hand, the solution contain a stan- nic salt, or metastannic acid, and the precipitate is yellow and consists of stannic sulphide mixed with stannic oxide, or yellowish brown and consists of hydrated metastannic sulphide mixed with meta- stannic acid {BAKFOED, p. 189, TH. SCHEEREK;*;), put the fluid, loosely covered, in a warm place, until the odor of hydrogen sul- phide has nearly gone off, and then filter. The washing of the stannic sulphide precipitate, which has a great inclination to pass through the filter, is best effected with a concentrated solution of sodium chloride, the remains of the latter being got rid of by a solution of ammonium acetate containing a small excess of acetic acid. If there is no objection to' having the latter salt in the fil- trate, the washing may be entirely effected by its means (BUNSEN). * Journ. f. prakt. Chem. 56, 366. f Pogg. Annal. 112, 164. \ Journ. f. prakt. Chem. N. F. 3, 472. Annal. d. Chem. u. Pharm. 106, 13. 342 DETERMINATION. [ 126. Transfer the dry precipitate as completely as possible to a watch glass, burn the filter carefully in a weighed porcelain crucible, moisten the ash with nitric acid, ignite, allow to cool, add the pre- cipitate, cover the crucible, heat gently for some time (slight decrep- itation often occurs), remove the lid and heat gently with access of air, till sulphur dioxide has almost ceased to be formed. (If too much heat is applied at first, stannic sulphide volatilizes, the fumes of which give stannic oxide.) Now heat strongly, allow to cool, and heat repeatedly with pieces of ammonium carbonate to a high degree, to drive out the last portions of sulphuric acid. When the weight remains constant the experiment is ended (H. HOSE). For the properties of the precipitates, see 91. The results are accu- rate. 2. Volumetric Methods. The determination of tin by the conversion of stannous into stannic chloride with the aid of oxidizing agents (potassium dichro- mate iodine, potassium permanganate, etc.) offers peculiar difficulties, inasmuch as on the one hand the stannous chloride takes up oxygen from the air and from the water used for dilution, with more or less rapidity, according to circumstances ; and on the other hand, the energy of the oxidizing agent is not always the same, being influenced by the state of dilution and the presence of a larger or smaller excess of acid. In the following methods, these sources of error are avoided or limited in such a manner as to render the results satisfactory. 1. Determination of Stannous Chloride ~by Iodine in Alkaline Solution (after LESSEN*). Dissolve the stannous salt or the metallic tinf in hydrochloric acid (preferably in a stream of carbon dioxide), add Rochelle salt, then sodium hydrogen carbonate in excess. To the clear slightly alkaline solution thus formed add some starch-solution, and after- wards the iodine solution of 146, till a permanent blue coloration appears. 2 at. free iodine used corresponds to 1 at. tin. .LENSSEN'S results are entirely satisfactory. * Journ. f. prakt. Chem. 78, 200; Annal. d. Chem. u. Pharm. 114, 113. f The solution of metallic tin is much assisted by the presence of platinum foil, which is accordingly added. LENSSEN found this addition of platinum to be objectionable; but no other experimenter has observed that it interferes with the accuracy of the results. 126.] TIN IX STANNOT'S AND STANNIC COMPOUNDS. 343 2. Determination of Stannous Chloride after addition, of Ferric Chloride. The fact that stannous chloride in acid solution can be far more accurately converted into stannic by oxidizing agents after being mixed with ferric chloride (or even with cupric chloride) than without this addition, was first settled by LOWENTHAL.* Sub- sequently SxROMEYERf published some experiments leading to the same results, together with practical remarks on the best way of carrying out the method in different cases. The processes thus originated, and which have been well tested, are as follows : a. The given substance is a stannous salt. Dissolve in pure ferric chloride (free from ferrous chloride) with addition of hydro- chloric acid, dilute and add standard permanganate from the burette. Kow make another experiment with the same quantity of water similarly colored with ferric chloride to ascertain how much permanganate is required to tinge the liquid, and subtract the quantity so used from the amount employed in the actual analysis, and from the remainder calculate the tin. The reaction between the tin salt and the iron solution is SnCl, -+-Fe 2 Cl 6 =SnCl 4 +2FeCl 2 . The solution thus contains ferrous chloride in the place of stannous salt, the former being, as is well known, far less susceptible of alteration from the action of free oxygen than the latter. 2 at. iron found correspond to 1 at. tin. It must not be forgotten that the titration takes place in presence of hydrochloric acid. The results cannot be considered accurate unless the standardizing of the permanganate and the analysis take place under similar conditions as regards dilution and amount of hydrochloric acid. b. The given substance is metallic tin. Either dissolve in hydrochloric acid preferably with addition of platinum and in an atmosphere of carbon dioxide and treat the solution according to ^, or place the substance at once in a concentrated solution of ferric chloride mixed with a little hydrochloric acid ; under these cir- cumstances it will, if finely divided, dissolve quickly even in the cold and without evolution of hydrogen. Gentle warming is unobjectionable. Now add the. permanganate. The reaction is Sii + 2Fe 2 Cl 6 =SnCl 4 + 4FeCl 2 , therefore every 4 at, iron found reduced correspond to 1 at. tin. The results are of course only * Journ. f. prakt. Chem. 76. 484. f Annal. d. Chem. u. Pharm. 117. 261. 344 DETERMINATION. [ 127. correct when iron is not present, Where this is the case, proceed with the impure tin solution according to c. c. The given substance is stannic chloride or stannic oxide, or a compound of tin containing iron. Dissolve in water with addition of hydrochloric acid, place a plate of zinc in the solution and allow to stand twelve hours, then remove the precipitated tin with a brush, wash it, dissolve in ferric chloride, and proceed as in b. d. The given substance is pure stannic sulphide, precipitated out of an acid stannic solution containing no stannous salt. Mix with ferric chloride, heat gently, filter off the sulphur, and then add the permanganate. 4 at. iron correspond to 1 at. tin, for Sn S 2 + 2Fe 2 Cl 6 SnCl 4 + 4FeCl 2 + 2S. The results obtained by STROMEYER are quite satisfactory. As regards the precipitated stannic sulphide, see BARFOED, p. 189. 127. 6. ARSENIOUS ACID, and 7. ARSENIC ACID. a. Solution. The compounds of arseiiious and arsenic acids which are not soluble in water are dissolved in hydrochloric acid or in nitrohydro- chloric acid. Some native arsenates require fusing with sodium carbonate. Metallic arsenic, arsenious sulphide, and metallic arsen- ides are dissolved in fuming nitric acid or nitrohydrochloric acid, or a solution of bromine in hydrochloric acid; those metallic arsenides which are insoluble in these menstrua are fused with sodium carbonate and potassium nitrate, by which means they are converted into soluble alkali arsenates and insoluble metallic oxides, or they may be suspended in potassa solution and treated with chlorine ( 164, 137 and 138). In this last manner, too, arsenious sulphide, dissolved in concentrated potassa, may be very easily ren- dered soluble. All solutions of compounds of arsenic which have been effected by long heating with fuming nitric acid, or by warm- ing with excess of nitrohydrochloric acid, or chlorine, contain arsenic acid. A solution of arsenious acid in hydrochloric acid cannot be concentrated by evaporation, since arsenious chloride would escape with the hydrochloric acid fumes. This, however, less readily takes place if the solution contains arsenic acid ; in fact, it only occurs in the presence of a large proportion of hydro- chloric acid (for instance, half the volume of hydrochloric acid of 127.] ARSENIOUS AND ARSENIC ACIDS. 345 1*12 sp. gr.*). It is therefore advisable in most cases where a hydrochloric acid solution containing arsenic is to be concentrated, previously to render the same alkaline. b. Determination. Arsenic is weighed as lead arsenate, a# ammonium magnesium arsenate, as magnesium pyroarsenate, as uranyl pyroarsenate, or as arsenious sulphide. The determination as ammonium magnesium arsenate is sometimes preceded by precipitation as ammonium arsenio-molybdate. The method recommended by BERTHIER and modified .by v. KOBELL of separating the arsenic as basic ferric arsenate is only used in separations. Arsenic may be estimated also in an indirect way, and by volumetric methods. We may convert into 1. LEAD ARSENATE : Arsenious and arsenic acids in aqueous or nitric acid solution. (Acids or halogens forming fixed salts with lead, and also ammonium salts, must not be present.) 2. AMMONIUM MAGNESIUM ARSENATE, or MAGNESIUM PYRO- ARSENATE I a. By direct Precipitation. Arsenic acid in all solutions free from bases or acids precipitable by magnesia or ammonia. b. Preceded by Precipitation as Ammonium Arsenio-molyb- date. Arsenic acids in all cases where no phosphoric acid is present, little or no hydrochloric acid, nor any substance which decomposes molybdic acid. 3. URANYL PYROARSENATE : Arsenic acid in all combinations soluble in water and acetic acid. 4. ARSENIOUS SULPHIDE : All compounds of arsenic without exception. Arsenic may be determined volumetrically in a simple and exact manner, whether present in the form of arsenious acid or an alkali arsenite, or as arsenic acid or an alkali arsenate. The volu- metric methods have now almost entirely superseded the indirect gravimetric methods formerly employed to effect the determination of arsenious acid. 1. Determination as Lead Arsenate. a. Arsenic Acid in Aqueous Solution. A weighed portion of the solution is put into a platinum or porcelain dish, and a weighed amount of recently ignited pure lead * Zeitschr. f. Chem. 1, 448. 346 DETERMINATION. [ 127. oxide added (about five or six times the supposed quantity of arse- nic acid present) ; the mixture is cautiously evaporated to dryness, and the residue heated to gentle redness, and maintained some time at this temperature. The residue is lead arsenate -f- lead oxide. The quantity of arsenic acid is now readily found by sub- tracting from the weight of the residue that of the oxide of lead added. For the properties of lead arsenate, see 92. The results are accurate, provided the residue be not heated beyond gentle red- ness. b. Arsenious Acid in Solution. Mix the solution with nitric acid, evaporate to a small bulk, add a weighed quantity of lead oxide in excess, evaporate to dry- ness, and ignite the residue most cautiously in a covered crucible, until the whole of the lead nitrate is decomposed. The residue consists here also of arsenic acid -(- lead oxide. This method requires considerable care to guard against loss by decrepitation upon ignition of the lead nitrate. 2. Estimation as Ammonium Magnesium Arsenate^ or Magnesium Pyroarsenate. a. By direct Precipitation. This method, which was first recommended by LEVOL, presup- poses the whole of the arsenic in the form of arsenic acid. Where this is not the case, the solution is gently heated, in a capacious flask, with hydrochloric acid, and potassium chlorate added in small portions, until the fluid emits a strong smell of chlorous acid ; it is then allowed to stand at a gentle heat until the odor of this gas is nearly gone off. The arsenic acid solution is now mixed with ammonia in excess, which must not produce turbidity, even after standing some time ; magnesia mixture is then added (p. 113, 62, 6). The fluid, which smells strongly of ammonia, is allowed to stand 24 or 48 hours in the cold, well covered, and then filtered through a weighed filter. The precipitate is then transferred to the filter, with the aid of portions of the filtrate, so as to use no more washing water than necessary, and washed with small quantities of a mixture of three parts water and one part ammonia, till the washings, on being mixed with nitric acid and silver nitrate, show no opalescence. The precipitate is dried at 102 to 103, and weighed. It has the for- 127.] ARSENIOUS AND ARSENIC ACIDS. 347 mula (MgNH 4 AsO 4 ) 3 -f-H 2 O.* As the drying of ammonium mag- nesium arsenate till its weight is constant, requires much time and repeated weighings, it is a great advantage that we can now con- vert it without loss of arsenic into magnesium pyroarsenate (Mg 2 As 2 O 7 ), thanks to the researches of H. RosE,f WITTSTEIN^: and PULLER. For this purpose first transfer the dried precipitate as completely as possible to a watch-glass, saturate the filter with a solution of ammonium nitrate, dry and burn it cautiously in a porcelain crucible. After cooling, transfer the precipitate to the crucible, heat in an air-bath to about 130, continue heating for 2 hours on a sand-bath, then heat for an hour or two on an iron plate a little more strongly, and when the ammonia has been thus entirely expelled ignite strongly for some time over the lamp. The pro- cess may be shortened by conducting the heating in a ROSE'S cruci- ble in a slow current of oxygen. 'The ammonia may then be driven off in 10 minutes, and after the precipitate has been at last strongly heated it will be ready to weigh. For the properties of the ammonium magnesium arsenate and magnesium pyroarsenate, see 92. The method yields satisfactory results, since the small loss of precipitate dissolved in the filtrate and washings is coun- terbalanced by the presence of a trace of basic magnesium sulphate (PULLER). PULLER with a quantity of -37 grm. ammonium mag- nesium arsenate lost only a fraction of a milligramme ; on the ad- dition of a large proportion of ammonium chloride the loss rose to about -002 grm. The correction for the solubility of the precipi- tate in the ammoniacal filtrate containining excess of magnesia mixture is -001 grm. of (MgNH 4 AsO 4 ) 2 -fH 2 O for 30 c.c. b. Preceded by Precipitation as Ammonium Arsenio-inolyb- date. Mix the acid solution, which must be free from phosphoric and silicic acids, with an excess of solution of ammonium molybdate. The ammonium molybdate solution should have been previously mixed with nitric acid in excess, and the whole process is con- ducted exactly as in the case of phosphoric acid see 134, b, fi. * If it is dried in a water-bath, the drying must be extremely prolonged, or otherwise more than 1 eq. will be left. After brief drying in the water-bath the compound contains between 1 and 3 eq. water. If it is dried between 105 and 110, part of the 1 eq. water is lost. f His Handbuch der anal. Chem. 6 Aufl. 2, 390. \ Zeitschr. f. anal. Chem. 2, 19. Ib. 10, 63. 348 DETERMINATION. [ 127. After dissolving the ammonium arsenio-molybdate in ammonia, neutralize the latter partially with hydrochloric acid. Treat the ammonium magnesium arsenate as in a. Results satisfactory. 3. Estimation as Uranyl Py roar senate. This method was first proposed by WERTHER.* It has been carefully studied by PuLLERf in my laboratory, and gives thor- oughly satisfactory results. Mix the arsenic acid solution with potash or ammonia in excess, and then a good excess of acetic acid, (If a precipitate of ferric or aluminium arsenate here remains insoluble, the method would be inapplicable.) Add uranyl acetate in excess, and boil. Wash the slimy precipitate of uranyl arsenate or of ammonium uranyl arsenate by decantation with boiling water, and then transfer to a filter. The addition of a few drops of chlo- roform to the partly cool fluid will hasten the deposition of the pre- cipitate. Dry, transfer the precipitate to a watch-glass, cleaning the filter as much as possible ; saturate the latter with ammonium nitrate, dry it, incinerate in a porcelain crucible, and add the pre- cipitate. If the precipitate contains ammonium, heat very cau- tiously, finally adding nitric acid, or ignite in oxygen. (See 2, a.) If the precipitate is free from ammonium, ignite in the ordinary way. Ammonium salts do not interfere. Properties of the pre- cipitate and residue, 92, e. 4. Estimation as Arsenioiis Sulphide. a. In solutions of Arsenious Acid or Arsenites free from Arsenic Acid. The solution should be strongly acid with hydrochloric acid. Precipitate with hydrogen sulphide and expel the excess with car- boii dioxide. Pass the latter through the solution for an hour, a longer time is useless. (See 125, 1.) Wash the precipitate thor- oughly and dry at 100 till the weight is constant. Particles of the precipitate which adhere so firmly to the glass that they can- not be removed mechanically are dissolved in ammonia and repre- cipitated with hydrocholric acid. Properties of the precipitate, 92. Do not omit to test a weighed portion to see whether it completely volatilizes on heating. If a residue remains it is to be weighed and the proportional quantity deducted from the total weight of the precipitate. Results accurate. * Journ. f. prakt. Chem. 43, 346. f Zeitschr. f. analyt. Chem. 10, 72. 127.] ARSENIQUS AND ARSENIC ACIDS. 349 If the solution contains any substance Which decomposes hydro- gen sulphide, such as ferric chloride, chromic acid, etc., the precip- itate produced in the cold contains an admixture of finely divided sulphur. It should be collected in the same manner on a filter dried at 100, and weighed, washed and dried. Extract the admixed sulphur with purified carbon disulphide (which should leave no residue on evaporation), continuing till the fluid which runs through leaves no residue. Dry at 100 till the weight is constant. From experiments made in my laboratory it appears that the results thus obtained are quite accurate, even when the amount of admixed sulphur is large ; but the precipitation must have been effected in the cold. If, on the contrary, heat is used, the sulphur is in the form of small agglutinated grains and cannot be completely extracted by cold carbon disulphide on the filter. However, it may be extracted by removing the precipitate from the filter and repeatedly digesting it with the disulphide on a water- bath (PULLER*). Instead of purifying the arsenious sulphide you may estimate the arsenic in the mixture of the sulphide with sulphur as follows : Dissolve the precipitate in strong potash, and pass chlorine into the solution ( 148, II. 2, b). The arsenic and the sulphur are con- verted into arsenic and sulphuric acid respectively ; the former may be estimated according to 2, a, or the latter according to 132. In the latter case, deduct the sulphur found from the weight of the arsenical precipitate. There is no loss of arsenic in this process from volatilization of the chloride, as the solution remains alkaline. The object may also be conveniently attained by the use of nitric acid. A very strong fuming acid, of 86 boiling point, is employed ; an acid of 1-42 sp. gr. which boils at a higher tempera- ture does not answer the purpose, as the separated sulphur would fuse, and its oxidation would be much retarded. The well dried precipitate is shaken into a small porcelain dish, treated with a tol- erably large excess of the fuming nitric acid, the dish immediately covered with a watch-glass, and as soon as the turbulence of the first action has somewhat abated, heated on a water-bath till all the sulphur has disappeared, and the nitric acid has evaporated to a small volume. The filter to which the unremovable traces of arsenious sulphide adhere is treated separately in the same manner, * Zeitschr. f. anal. Chem. 10, 46 et seq. 350 DETERMINATION. [_ 127. the complete destruction of the organic matter being finally effected by gently warming the somewhat dilute solution with potassium chlorate (BUNSEN*). Or the filter may instead be extracted with ammonia, the solution evaporated in a separate dish, and the resid- ual sulphide treated as above. In the mixed solution the arsenic acid is finally precipitated as ammonious magnesium arsenate. ( 127, 2, a). Treatment of the impure precipitate with ammonia, whereby the sulphide is dissolved, and the sulphur is supposed to remain behind, only gives approximate results, as the ammoniacal solution of arsenious sulphide takes up a little sulphur. b. In solutions of Arsenic Acid, or of a mixture of the two Oxides of Arsenic. Heat the solution in a flask (preferably on an iron plate) to about 70, and conduct hydrogen sulphide at the same time into the fluid, as long as precipitation takes place. The precipitate formed is always a mixture of sulphur and arsenious sulphide, since the arsenic acid is first reduced to arsenious acid with separation of sulphur, and then the latter is decomposed (H. Rossf). Only in the case when a sulphosalt containing pentasulphide of arsenic is decomposed with an acid, is the precipitate actually pentasulphide, and not merely a mixture of sulphur with arsenious sulphide (A. FUCHS^:). To convert this mixture of arsenious sulphide and granular sulphur into pure arsenious sulphide, suitable for weigh- ing, treat it a,s follows : Extract the washed and still moist pre- cipitate on the filter with ammonia, wash the residual sulphur, precipitate the solution with hydrochloric acid without heat, fil r ter, dry, extract with carbon disulphide, dry at 100, and weigh. Results accurate. The mixture of arsenious sulphide and sulphur obtained by hot precipitation may, of course, also be estimated directly or indirectly after one of the other methods in 4, a. 5. Volumetric Methods. a. Method which presupposes the presence of Arsenious Acid. BUNSEN'S method. This method is based upon the following facts : aa. If potassium dichromate is boiled with concentrated hydro- chloric acid, 6 at. chlorine are disengaged to every 2 mol. chromic acid 2CrO 3 + 12HC1 = Cr 2 Cl 6 + 6H 2 O -f- 601. * Annal. d. Chem. u. Pharm. 106, 10. f Pogg. Annal. 107, 186. JZeitschr. f. anal. Chem. 1, 189. Annal. d. Chem. u. Pharm. 86, 290. 127.] ARSENIOUS AND ARSENIC ACIDS. 351 bb. But if arsenious acid is present (not in excess) there is not the quantity of chlorine disengaged corresponding to the chromic acid, but so much less of that element as is required to convert the arsenious into arsenic acid (H 3 AsO 3 + 2C1 + H 2 O = H 3 AsO 4 -f 2 HC1). Consequently, for every 2 at. chlorine wanting is to be reckoned 1 mol. arsenious acid. cc. The quantity of chlorine is estimated by determining the quantity of iodine liberated by it from potassium iodide. These are the principles of BUNSEN'S method. For the manner of execution I refer to the Estimation of Chromic Acid. b. Method, which presupposes the presence of A. r seme Acid. This method depends on the precipitation of the arsenic acid by uranium solution and the recognition of the end of the reaction by means of potassium ferrocyanide. It is therefore the same as was suggested for phosphoric acid by LECOMTE, and brought into- use by NEUBAUER,* and afterwards by PiNcus.f BODEKER,^: who first employed the process for arsenic acid, recommends the employment of a solution of uranyl nitrate, as this is more permanent than the hitherto used acetate, which is gradually decomposed by the action of light. The uranium solution has the correct degree of dilution, if it contains about 17 grm. of uranium in 1 litre. It should contain as little free acid as possible. The determination of its value may be effected with the aid of pure sodium arsenate or by means of arsenious acid the latter is converted into arsenic acid by boiling with fuming nitric acid. The solution is rendered strongly alka- line with ammonia, and then distinctly acid with acetic acid. The uranium solution is now run in from the burette slowly, the liquid being well stirred all the while, till a drop of the mixture spread out on a porcelain plate, gives with a drop of potassium ferrocya- nide placed in its centre, a distinct reddish-brown line where the two fluids meet. The height of the fluid in the burette is now read off, the level of the mixture in the beaker is marked with a strip of gummed paper, and the beaker is emptied and washed, filled with water with addition of about as much ammonia and acetic acid as was before employed, and the uranium solution is cautiously dropped in from the burette, till a drop taken out of the beaker and tested as above, gives an equally distinct reaction. The * Archiv fur wissenschaftliche Heilkunde, 4, 228. f Journ. f. prakt. Chem. 76, 104. \ Anna!, de Chem. u. Pharm. 117, 195. 352 DETERMINATION. [ 127. quantity of uranium solution used in this last experiment is the excess, which must be added to make the end-reaction plain for the dilution adopted. This amount is subtracted from that used in the first experiment, and we then know the exact value of the uranium solution with reference to arsenic acid. In an actual analysis, the arsenic is first brought into the form of arsenic acid, a clear solution is obtained containing ammonium acetate and some free acetic acid,* and the process is conducted exactly as in determining the value of the standard solution. The experiment to ascertain the correction must not be omitted here, otherwise errors are sure to arise from the different degrees of dilu- tion of the arsenic acid solutions used in the determination of the value of the standard solution and in the actual analyses. The results of two determinations of arsenic given by BODEKEK are satisfactory. To execute the method well requires practice. The results are not exact enough unless the conditions as regards amount and quality of alkali salts are nearly similar in the standardizing of the uranium solution and in its use. Compare WArrz.f 6. Estimation of Arsenious Acid by Indirect Gravimet- ric Analysis. a. ROSE'S method. Add to the hydrochloric acid solution, in the preparation of which care must be taken to exclude oxidizing substances, a solution of sodium- or ammonium-auric chloride in excess, and digest the mixture for several days, in the cold, or, in the case of dilute solutions, at a gentle warmth ; then weigh the separated gold as directed in 123. Keep the filtrate to make quite sure that no more gold will separate. 2 at. gold correspond to 3 mol. arsenious acid. 1. YOIIL'S^ method. Mix the solution with a weighed quan- tity of potassium dichromate, and free sulphuric acid ; estimate the chromic acid still present by the method given in 130, y Volumetric Analysis. a. SCHWARZ'S method. The principle of this very accurate method is identical with that upon which PENNY'S method of determining iron is based ( 112, 2, b). The execution is simple : acidify the not too dilute solution of the chromate with sulphuric acid, add in excess a measured quan- tity of solution of a ferrous salt, the strength of which you have previously ascertained, according to the directions of 112, 2, , or &, or the solution of a weighed quantity of ammonium ferrous sul- phate, free from ferric salt, and then determine in the manner 130.] CHROMIC ACID. 357 directed 112, 2, a, or , the quantity of ferrous iron remaining. The difference shows the amount of iron that has been converted by the chromic acid from a ferrous to a ferric salt. 1 grm. of iron corresponds to 0-5981 of chromic anhydride (CrO s ). To determine the chromic acid in lead chromate, the latter is, after addition of the ammonium ferrous sulphate, most thoroughly triturated with hydrochloric acid, water added, and the analysis then proceeded with. ft. BUNSEN'S method* If a chromate is boiled with an excess of fuming hydrochloric acid, there are disengaged for every atom of chromium 3 at. chlo- rine ; for instance, K.Cr.O, + (HC1) 14 = (KC1), + Cr 2 Cl 6 + 601 + TH a O. If the escaping gas is conducted into solution of potassium iodide in exces, the 3 at. chlorine set free 3 at. iodine. The libera- ted iodine may next be determined as described in 146. 380'55 of iodine correspond to 100*48 of chromic anhydride (CrO 8 ). The analytical process is conducted as follows : Put the weighed sample of the chromate (say 3 to -1 grm.) into the little flask d, tig. 55 (blown before the lamp, and holding only from 36 to 40 c.c.), and nil the flask two thirds with pure fuming hydrochloric acid (free from Cl and SO,), add a compact lump of magne- site, to keep up a con- stant current of gas and prevent the fluid from receding. Connect the bulbed evolution tube a with the neck of the flask by means of a stout india-rubber tube c. As shown in the engraving, a is a bent pipette, drawn out at the lower end into an upturned point. A loss of chlorine need not be apprehended on adding the hydrochloric acid, as the disengage- ment of that gas begins only upon the application of heat. Insert the evolution tube into the neck of the retort, which is one-third filled with solution of potassium iodide. f This retort holds about * Annal. d. Chem. u. Pharm. 86, 279. t 1 part of pure potassium iodide, free from iodic acid, dissolved in 10 parts of water. The fluid must show no brown tint immediately after addition of dilute sulphuric acid. 358 DETERMINATION. [ 130. 160 c.c. The neck presents two small expansions, blown before the lamp, and intended, the lower one, to receive the liquid which is forced up during the operation, the upper one to serve as an additional guard against spirting. Apply heat now, cautiously, to the little flask. After two or three minutes ebullition the whole of the chlorine has passed over, and liberated its equivalent quan- tity of iodine in the potassium iodide solution. When the ebulli- tion is at an end, take hold of the caoutchouc tube c with the left hand, and, whilst steadily holding the lamp under the flask with the right, lift a so far out of the retort that the curved point is in the bulb h. Now remove first the lamp, then the flask, dip the retort in cold water to cool it, and shake the fluid in it about to effect the complete solution of the separated iodine in the excess of potas- sium iodide solution. When the fluid is quite cold, transfer it to a beaker, rinsing the retort into the beaker, and proceed as directed 146. The method gives very satisfactory results. The apparatus here recommended diifers slightly from that used by BUNSEN, the retort of the latter having only one bulb in the neck, and the evo- lution tube no bulb, being closed instead, at the lower end, by a glass or caoutchouc valve, which permits the exit of the gas from the tube, but opposes the entrance of the fluid into it. I think the modifications which I have made in BUNSEN'S apparatus are calcu- lated to facilitate the success of the operation. Instead of this apparatus, that described 142 may also be very conveniently used. II. SEPARATION OF CHROMIC ACID FROM THE BASIC RADICALS. a. Of the First Group. a. Reduce the chromic acid to a chromic salt, as directed in I., and separate the chromium from the alkalies as directed in 155. ft. Mix the potassium or sodium chromate with about 5 parts of dry pulverized ammonium chloride, and heat the mixture cau- tiously. The residue contains the chlorides of the alkali metals and chromic oxide, which may be separated by means of water. y. Precipitate the chromic acid according to I., , /?, and sep- arate the mercury and alkali metals in the filtrate by 1 02. h. Of the Second Group. a. Fuse the compound with 4 parts of sodium and potassium carbonates, and treat the fused mass with hot water, which dis- solves the chromic acid in the form of an alkali chromate. The 130.] CHROMIC ACID. 359 residue contains the alkali earth metals in the form of carbonates ; but as they contain alkali, they cannot be weighed directly. The chromic acid in the solution is determined as in I. Strontium and calcium chromates may be decomposed by boiling with potassium or sodium carbonate. Barium chromate may also be decomposed in the same way, but the boiling must be repeated a second time with fresh solution of alkali carbonate (H. KOSE). ft. Dissolve in hydrochloric acid, reduce the chromic acid according to I., #, and separate the chromium from the alkali earth metals according to 156. y. Magnesium chromate, as well as other chromates of the alkali earth metals soluble in water, may be easily decomposed also, by determining the chromic acid according to L, a, /?, or L, b, and separating the magnesium, etc., in the filtrate from the excess of the salt of mercury or lead as directed 162. d. Barium strontium and calcium chromates may also be decomposed by the method described II., , ft. Compare BAHK, Analysis of barium and calcium dichromates, etc.* c. Of the Third Group. a. from Aluminium. If you have chromic acid to separate from aluminium in acid solution, precipitate the aluminium with ammonia or ammonium carbonate ( 105, a) 7 and determine the chromic acid in the filtrate according to I. If the washed aluminium hydroxide has a yellow color, treat on the filter with ammonia, and wash with boiling water : this will remove the last traces of chromic acid. However, a little aluminium hydroxide dissolves in the ammonia, therefore heat the ammoniacal fluid in a platinum dish till it has almost lost its alkaline reaction, and collect on a filter the flocks of aluminium hydroxide which separate, and add them to the principal precip- itate. ft. From Chromium. aa. Determine in one portion the quantity of the chromic acid according to I., #, or I.,rf, OL, or ft, and in another portion the total amount of the chromium, by converting it into sesquioxide by cau- tious ignition with ammonium chloride, or by L, #, or by convert- ing it entirely into chromic acid by 106, 2. bb. In many cases the chromic acid may be precipitated accord- * Journ. f. prakt. Chem. 60, 60. 360 DETERMINATION. [ 130. ing to I., a, ft, or I., I. The chromium and mercury, or lead, in the filtrate, are separated as directed 162. cc. The hydrated compounds of sesquioxide of chromium with chromium trioxide, or chromic chromates, such as are obtained by precipitating a solution of chromic salt with potassium chromate, etc., may also be analyzed by ignition in a stream of dry air, in a bulb tube, to which a calcium chloride tube is attached (fig. 25, 36). The loss of weight represents the joint amount of oxygen and water that have escaped. If the increment of the CaCl 3 tube is deducted, we shall have the oxygen. Now every 3 at. oxygen correspond to 2 mol. CrO,. The amount of the latter being thus calculated, we have only to subtract its equivalent quantity of ses- quioxide from the weight of residue after the ignition, and the remainder is the quantity of sesquioxide originally present. VOGEL* and also STOKER and ELLioxf have employed this method. d. Of the Fourth Group. a. Proceed as directed in b, ot. Upon treating the fused mass with hot water, oxides of the basic metals are left. In the case of manganese the fusion must be effected in an atmosphere of carbon dioxide. Apparatus, fig. 50 in 108. ft. Reduce the chromic acid as directed in I., #, and separate the chromium from the metals in question, as directed in 160. e. Of the Fifth and Sixth Groups. a. Acidify the solution, and precipitate, either at once or after reduction of the chromic acid by sulphurous acid, with hydrogen sulphide. The metals of the fifth and sixth groups precipitate in conjunction with free sulphur ( 115 to 127), the chromic acid is reduced. Filter and determine the chromium in the filtrate, as directed in I., a. ft. Lead chromate may be conveniently decomposed by heating with hydrochloric acid and some alcohol ; the lead chloride and chromic chloride formed are subsequently separated by means of alcohol (compare 162). The alcoholic solution ought always to be tested with sulphuric acid ; should a precipitate of lead sulphate form, this must be filtered off, weighed, and taken into account. * Journ. f. prakt. Chem. 77, 484. f Proceedings of the American Academy, 5, 198. 131.] SELENIOUS ACID. 361 Supplement to the First Division. 131. 1. SELENIOUS ACID. From aqueous or hydrochloric acid solutions of selenious acid r the selenium is precipitated by sulphurous acid gas, or, in presence of an excess of acid, by sodium sulphite, or ammonium sulphite. The liquid containing the precipitate is heated to boiling for J hour, which changes the precipitate from its original red color to black, and makes it dense and heavy. The liquid is tested by a further addition of the reagent to see whether any more selenium will sep- arate ; the precipitate is finally collected on a weighed filter, dried at a temperature somewhat below 100, and weighed. Since H. ROSE* has shown that the presence of hydrochloric acid is an essen- tial condition to the complete reduction of selenious acid, the for- mer acid must be added, if not already present. To make quite sure that all the selenium has been removed, the filtrate is evapo- rated to a small volume, with addition of potassium or sodium chlo- ride, boiled with strong hydrochloric acid, so as to reduce any sele- nic acid to selenious acid, and tested once more with sulphurous acid. If the solution contains nitric acid it must be evaporated repeatedly with hydrochloric acid, with addition of sodium or potassium chloride. If the latter were omitted there would be considerable loss of selenious acid (RATHKEf). As regards the separation of selenious acid from basic radicals, the following brief directions will suffice : a. If the basic radicals are not liable to be altered by the action of sulphurous acid and hydrochloric acid, the selenium may be at once precipitated in the way just given ; the filtrate, when evap- orated with sulphuric acid, yields the base as sulphate. b. From basic metals which are not thrown down from acid solu- tion by hydrogen sulphide, the selenious acid may be separated by precipitation with that reagent. The precipitate (according to RATHKE^:, a mixture of SeS 2 , Se 2 S and S) contains 2 at. sulphur to 1 at. selenium. If it is dried at or a little below 100, the weight * Zeitschr. f. anal. Chem. 1, 73. f Journ. f. prakt. Chem. 108, 249; Zeitschr. f. anal. Chem. 9, 484. t Journ. f. prakt. Chem. 108, 252. 362 DP:TERMINATIOIV. [ 131. of the selenium may be accurately ascertained. Should, however, extra sulphur be mixed with the precipitate, the latter is oxidized while still moist with hydrochloric acid and potassium chlorate, or by treatment with potassa solution with simultaneous heating and transmission of chlorine. It is necessary here to oxidize the sul- phur completely, as it may enclose selenium, The solution now containing selenic acid is heated till it smells no longer of chlorine, hydrochloric acid is added, and the mixture is reheated. The sele- nic acid is hereby reduced to selenious acid, and when the solution has again ceased to smell of chlorine, the selenium is precip- itated with sulphurous acid. Instead of this process you may digest the precipitate of sulphur and selenium for some hours with con- centrated potassium cyanide, which will completely dissolve it, and then throw down the selenium from the dilute solution with hydro- chloric acid as in c (RATHKE, loc. cit.). c. In many selenites or selenates the selenium may also be determined by converting first into potassium selenocyanate, and precipitating the aqueous solution of the latter with hydrochloric acid (OppENHEiM*). To this end the substance is mixed with 7 or 8 times its quantity of ordinary potassium cyanide (containing cyanic acid), the mixture is put into a long-necked flask, or a porce- lain crucible, covered with a layer of potassium cyanide, and fused in a stream of hydrogen. The temperature is kept so low that the glass or porcelain is not attacked, and while cooling care must be taken to exclude atmospheric air. When cold, the brown mass is treated with water, and the colorless solution filtered, if neces- sary. The liquid should be somewhat but not immoderately diluted. Now boil some time (in order to convert the small quan- tity of potassium selenide that may be present into potassium sele- nocyanate, by the excess of potassium cyanide, allow to cool, super- saturate with hydrochloric acid, and heat again for some time. At the end of 12 or 24 hours all selenium will have separated, filter, dry at 100, and weigh. The results obtained by this process are accurate (H. RosEf). If the selenium agglomerates together on heating, it may enclose salts. In such cases, by way of control, it should be redissolved in nitric acid, and, after addition of hydro- chloric acid, precipitated with sulphurous acid. The fluid filtered from the selenium precipitate is, as a rule, free from selenium ; it Journ. f. prakt. Chem. 71, 280. f Zeitschr. f. anal. Chem. 1, 73. 131.] SULPHUROUS ACID. 363 is, however, always well to satisfy one's self on this point by the addition of sulphurous acid. d. From many basic radicals selenious acid (and also selenic acid) may be separated by fusing the compound with 2 parts of sodium carbonate and one part of potassium nitrate, extracting the fused mass thoroughly by boiling with water, saturating the nitrate, if necessary, with carbonic acid, to free it from lead which it might contain, then boiling down with hydrochloric acid in excess (to reduce the selenic acid and drive off the nitric acid), and precipi- tating finally with sulphurous acid. Selenium, if pure, must volatilize without residue when heated in a tube. 2. SULPHUROUS ACID. To estimate free sulphurous acid in a fluid which may contain also other acids (sulphuric acid, hydrochloric acid, acetic acid), a weighed quantity of the fluid is diluted with water, absolutely free from air,* until the diluted liquid contains not more than -05 per cent, by weight of sulphurous acid, the solution is poured with stirring into an excess of standard solution of iodine, the free iodine remaining is titrated with sodium thiosulphate, and the iodine used for the conversion of sulphurous into sulphuric acid is thus found. The reaction is expressed by the equation, SO, -f- 2H 2 O + 21 = H 2 SO 4 + 2HI. According to FINKENER, if the iodine is added to the sulphurous acid the reaction is not quite normal. Anyhow this method of operating prevents any loss of sulphurous acid. For the details, see 146. In case of sulphites soluble in water or acids, water perfectly free from air is poured over the substance, in sufficient quantity to attain the degree of dilution stated above, sulphuric or hydrochloric acid is added in excess, and then the titration is effected as above. The greatest care must be taken in this method, to use, for the purpose of dilution, water absolutely free from air. Sulphurous acid may also be determined in the gravimetric way, by conversion into sulphuric acid, and precipitation of the latter with barium chloride, according to 132. This method is espe- cially applicable in the case of sulphites quite free from sulphuric acid. The conversion of the sulphurous into sulphuric acid is * Prepared by iQng-continued boiling and subsequent cooling with exclusion of air. 364 DETERMINATION. [ 131. effected in the wet way, best by pouring the dilute solution with stirring into excess of chlorine or bromine water. Sulphites insolu- ble in water are decomposed by boiling with sodium carbonate, and the solution of sodium sulphite is treated as directed. After driv- ing off the excess of chlorine or bromine by heating, the moderately acid solution is precipitated with barium chloride. Sulphites may be oxidized in the dry way by heating in a platinum crucible, with 4 parts of a mixture of equal parts sodium carbonate and potassium nitrate. 3. THIOSULPHURIC ACID. Thiosulphuric acid, in form of soluble thiosulphates, may be determined by means of iodine, in a similar way to sulphurous acid. The reaction is represented by the equation, 2Na 2 S 2 O 3 -f- 21 = 2XaI -f- Na 2 S 4 O 6 . The salt under examination is dissolved in a large amount of water, starch-paste added, and then the neutral solution is titrated with iodine. That this method can give correct results only in cases where no other substances acting upon iodine are present, need hardly be mentioned. Thiosulphuric may like sulphurous acid be converted into sulphuric acid by means of chlo- rine or bromine water, and then determined. 4. IODIC ACID. lodic acid may be determined by the following easy method : Distil the free acid or iodate with an excess of pure fuming hydro- chloric acid, in the apparatus described in 1-30,6?, ft (chromic acid), receive the disengaged chlorine in solution of potassium iodide, and determine the separated iodine as directed in 130, I, d, ft. The decomposition of iodic acid by hydrochloric acid is represented by the equation, H1O 3 + 5HC1 = IC1 + 4C1 + 3H 2 O. Since the 4 at. Cl set free 4 at. I, the amount of iodic acid or iodic anhydride can be calculated from the weight of the latter ; 1014-8 iodine cor- respond to 333-7 iodic anhydride (I Q O 5 ) (BUNSEN*). The following method also yields good results. Mix the solution with dilute sul- phuric acid, add potassium iodide in excess, and determine the amount of liberated iodine, after 146. One sixth of the iodine thus formed is derived from the iodic acid (HIO 3 + 5HI = 3H 2 O + I 6 ). See RAMMELSBERG.f * Annal. d. Chem. u. Pharm. 86, 285. f Pogg. Annal. 135, 493 ; Zeitschr. f. anal. Chem. 8, 456. 131.] NITROUS ACID. 365 5. NITROUS ACID. The nitrous acid in nitrites which are free from nitrates may be estimated by converting the nitrogen into ammonia and deter- mining the latter, or by determining the oxidizing action on ferrous salt. This method is conducted exactly as described under nitric acid ( 149). When nitric acid is also present, nitrous acid may be determined very satisfactorily with a solution of pure potassium permanganate, provided the fluid be sufficiently diluted to prevent the nitrous acid, which is liberated by the addition of a stronger acid, being decomposed by water with formation of nitric acid and nitric oxide. For 1 part of nitrous anhydride at least 5000 parts of water should be present. The decomposition is repre- sented by the following equation, 5HNO, -f- K,Mn,O 8 -f- 3H,SO 4 = 5HNO 3 +K 2 SO 4 + 2MnSO 4 + 3H,O. If the permanganate be standardized with iron, 4 at. iron correspond to 1 raol. N 2 O 3 , since both of these require 2 at. oxygen. Nitrites are dissolved in very slightly acidulated water, the permanganate is added till the oxidation of the nitrous acid is nearly completed, the solution is then made strongly acid, and finally permanganate is added to ligl it- red coloration. To determine nitrogen tetroxide N,O 4 in red fuming nitric acid, transfer a few c.c. to about 500 c.c. cold pure distilled water with stirring, and determine the nitrous acid produced. 1 mol. nitrous anhydride found corresponds to 2 mol. nitrogen tetroxide, for the latter when mixed with such a large quantity of water as is indi- cated above is decomposed in accordance with the following equa- tion : N a O 4 + H 2 O = HNO 3 + HNO, (Sio. FELDHAUS*). Nitrous acid and nitrogen tetroxide in presence of nitric acid may also be estimated by the reduction of chromic acid. An excess of standard potassium dichromate is added, and the unde- composed residue of chromic acid is estimated with standard solu- tion of ferrous salt (F. MoHRf). As regards the estimation of nitrous acid with lead dioxide, comp. FELDHAUS, loc. tit. p. 431, also LANG^: and J. LOWENTHAL. * Zeitschr. f. anal. Chem. 1, 426. f His Lehrbuch der Titrirmethode. 3 Aufl. 236. \ Zeitschr. f. anal. Chem. 1, 485. Ib. 3, 176. 366 DETEBMIKATIO]*. [ 132. Second Division of the First Group of the Acids. SULPHURIC ACID ; (Hydrofluosilicic Acid). 132. SULPHURIC ACID. I. DETERMINATION. Sulphuric acid is usually determined in the gravimetric way as barium sulphate. The acid may, however, be estimated also by the acidimetric method ( 192), and by certain volumetric methods, based upon the insolubility of the barium sulphate (and lead sul- phate). 1. Gravimetric Method. The exact estimation of sulphuric acid as barium sulphate is by no means so simple and easy as it was formerly supposed to be, but requires, on the contrary, great care and attention. This arises from three causes : first, the barium sulphate is found to be far more soluble than was imagined in solutions of free acids and of many salts ; secondly, it is extremely liable to carry down with it foreign salts, which are of themselves soluble in water ; thirdly, when the precipitate has once separated in an impure state, it is often very difficult to purify it completely. The solution should contain but little free hydrochloric acid, and no nitric or chloric acid. If either of the two last are present, evaporate repeatedly, on the water-bath with pure hydrochloric acid. Dilute considerably, heat nearly to boiling, add barium chlo- ride in moderate excess, and allow to settle for a long time at a gentle heat. Decant the clear fluid through a filter, treat the pre- cipitate with boiling water, allow to settle, decant again, and so on, till the washings are free from chlorine. Finally transfer the pre- cipitate to the filter, dry and treat according to 53, using only a moderate red heat. After the precipitate has been weighed it is well to warm it for some time with dilute hydrochloric acid on the water-bath. Then pour off the hydrochloric acid through a small filter, wash the pre- cipitate by decantation with boiling water without removing it to the filter, evaporate the filtrate and washings nearly to dry ness in a platinum or porcelain dish, add water, collect the minute amount 132.] SULPHURIC ACID. 367 of barium sulphate here left undissolved upon the small filter, wash, dry, incinerate, add the ash to the bulk of the precipitate, ignite again, and weigh. If the precipitate has lost weight, this shows that it at first contained foreign salts. This method of purification sometimes fails when the precipi- tate contains ferric oxide or platinum (CLAUS*), and it invariably fails when the solution contained any notable quantity of nitric acid.t In such cases there is only one resource, namely, to fuse with about four parts of sodium carbonate, warm with water, filter, wash with boiling water, acidify the filtrate slightly with hydro- chloric acid, and determine the sulphuric acid again. The results are thoroughly satisfactory if these directions are attended to ; if not, the result may be two or three per cent, too high or too low. 2. Volumetric Methods. a. After CARL MOHK.;): We require a normal solution of barium chloride, containing 121*96 grm. of the pure crystallized salt in 1 litre, and also normal nitric or hydrochloric acid and normal soda ( 192, c. 6). Add to the fluid to be examined for sulphuric acid which, should it contain much free acid, is previ- ously to be nearly neutralized with pure sodium carbonate a meas- ured quantity of barium chloride solution, best a round number of cubic centimetres, in more than sufficient proportion to precipi- tate the sulphuric acid, but not in too great excess. Digest the mixture for some time in a warm place, then precipitate, without previous filtration, the excess of barium chloride with ammonium carbonate and a little ammonia, filter off the barium sulphate and carbonate, wash until the water running off acts no longer upon red litmus paper, and then determine the barium carbonate by the alkaliinetric method given in 198. Deduct the c.c. of normal acid used from the c.c. of barium chloride, and the remainder will be the c.c. of barium chloride corresponding to the sulphuric acid present. The results of this method are quite satisfactory, if the solution does not contain too much free acid ; but in presence of a large excess of free acid, the action of the salt of ammonia will retain barium carbonate in solution, which, of course, will make * Jahresber. von KOPP und WILL. 1861, 323, note, f Compare my paper in Zeitschr. f. anal. Chem. 9, 52. j Ann. der Chem. u. Pharm. 90, 165. 368 DETERMINATION. [ 132. the amount of sulphuric acid appear higher than is really the case. It need hardly be mentioned that this method is altogether inap- plicable in presence of phosphoric acid, oxalic acid, or any other acid precipitating barium salt from neutral solutions, and that no basic radicals except the alkalies may be present. b. After R. WILDENSTEIN.* Of all the methods for the volu- metric estimation of sulphuric acid, the simplest and that which is capable of the most general application, is to drop into the solution containing excess of hydrochloric acid, standard barium chloride solution, till the exact point is reached when no more precipitation takes place. This point is diffi- cult to hit, and hence the method has only found a very limited use. "WILDENSTEIN has given this method a practical form, which renders it possible to complete an analysis in about half an hour, and at the same time to obtain satisfactory results. He employs the ap- paratus, fig. 56. A is a bottle of white glass, whose bottom has been removed, it contains 900 950 c.c. B is a strong funnel-tube, with bell-shaped funnel, Flg - 56 * and bent as shown, provided below with a piece of india-rubber tube, a screw compression-cock, and a small piece of tubing not drawn out, The length from c to d is about 7-J-8, from d to e about 12 cm. The opening of the funnel-tube /", which should have a diameter of 2'5 to 3 crn., is covered as follows : Take a piece of fine new calico or muslin, free from sulphuric acid, and about 6 cm. square, lay on it two pieces of Swedish paper of the same size, and then another piece of stuff like the first, now bind these altogether over the opening/ 1 , carefully and without injuring the paper, by means of a strong linen thread which has been drawn a few times over wax, and cut it off even all round. We have now a small syphon-filter, which enables us to filter off a portion of fluid contained in A, and turbid from barium sulphate, clear and with comparative rapidity. On gradually adding barium chloride to the dilute acid solution of a sulphate a point occurs which may be compared to the neutral point in precipitating silver with sodium chloride (see 115, 5, 5.) ; .est effected by heating in platinum vessels, with concentrated sul- phuric acid ; silicon fluoride and hydrofluoric acid volatilize, the basic metals are left behind in the form of sulphates, and may, in many cases, after volatilization of the excess of sulphuric acid, be weighed :us such. If the metallic silicofluorides to be analyzed contain water, the latter cannot be estimated by mere ignition, since silicon fluoride would escape with the water. II. ROSE recommends the following method : Mix them most intimately with 6 parts of recently ignited lead oxide, cover the mixture in a small retort, with a layer of pure lead oxide, weigh the retort, heat cautiously until the contents begin to fuse together, remove the aqueous vapor still remaining in the vessel by suction, and weigh the retort again when cold. The diminution of weight shows the quantity of water expelled. Do not neglect testing the drops of the escaping water with litmus paper; the result is accurate only if they have no acid reaction. F. STOLBA* proposes the following process, at least for com- pounds soluble in water : Put into a crucible double as much inag- riesia as is necessary to decompose the silicofluoride to be analyzed, ignite it as strongly as possible, allow to cool, and weigh. Add water * Zeitschr. f . anal. Chem. 7, 93. 134.] PHOSPHORIC ACID. 373 to form a thick paste, and then the weighed silicofluoride ; if the amount of water present is not enough to dissolve the compound, add some more, mix with a platinum wire which must afterwards be wiped off clean, dry, ignite, and weigh. The increase in weight shows the amount of anhydrous silicofluoride, provided no oxide is present which takes up oxygen. Third Division of the First Group of the Acids. PHOSPHORIC ACID BORACIC ACID OXALIC ACID HYDROFLUORIC ACID. 134. 1. PHOSPHORIC ACID. I. DETERMINATION. Orthophosphoric acid may be determined in a great variety of ways. The forms in which this determination may be effected have been given already in 93, 4. The most appropriate forms for the purpose, however, are magnesium pyrophosphate and ura- nyl pyrophosphate. The determination as magnesium pyrophos- phate is frequently preceded by precipitation in another way, especially as ammonium phospho-molybdate, occasionally as stannic phosphate or mercurous phosphate. The other forms in which phosphoric acid may be determined give also, in part, very good results, but admit only of a more limited application. With respect to volumetric methods, those which depend upon the use of standard solution of uranium are the best. With regard to meta- and pyrophosphoric acids, I have simply to remark here that these acids cannot be determined by any of the methods given below. The best way to effect their determination is to convert them into orthophosporic acid, as follows : a. In the dry way. By protracted fusion with from 4 to 6 parts of mixed sodium and potassium carbonates. This method is, however, applicable only in the case of alkali meta- and pyrophos- phates, and of those metallic meta- or pyrophosphates which are completely decomposed by fusion with alkali carbonates ; it fails, accordingly, for instance, with the salts of the alkali-earth metals, magnesium excepted. ft. In the ivet way. The salt is heated for some time with a 374 DETERMINATION. [ 134. strong acid, best with concentrated sulphuric acid (WEBER*). This method leads only to the attainment of approximate results, in the case of all salts whose basic radicals form soluble salts of the acid added, since in these cases the meta- or pyrophosphoric acid is never completely liberated ; but the desired result may be fully attained by the use of any acid which forms insoluble salts compounds with the basic radicals present. Respecting the partial conversion in the former case, I bave found that it approaches the nearer to completeness the greater the quantity of free acid added,f and that the ebullition must be long continued. BUNCE'S statement,^ that phosphoric acid volatilizes when a phosphate is evaporated to dryness with hydrochloric or nitric acid and the residue heated a little, is quite erroneous (compare my paper on the subject, in Annal. der Chem. und Pharm., 86, 216). But, on the other hand, it must be borne in mind that; orthophos- phoric acid under these circumstances changes, not indeed at 100, but at a temperature still below 150, to pyrophosphoric acid ; thus, for instance, upon evaporating common hydrogen sodium phos- phate with hydrochloric acid in excess, and drying the residue at 150, we obtain 2 Nad + Na 2 H 2 P 2 O 7 . a. Determination as Lead Phosphate. Proceed as with arsenic acid, 127, 1, a ?>., evaporate with a weighed quantity of oxide of lead, and ignite. This method pre- supposes that no other acid 'is present in the aqueous or nitric acid solution; it has this great advantage, that it gives correct results, no matter whether ortho-, meta-, or pyrophosphoric acid is present. b. Determination as Magnesium Pyrophosphate. of. Direct determination. Suitable in all cases in which it is quite certain that the acid present is orthophosphorie, either free or combined as an alkali phosphate. The solution should be neutral, or only moderately ammoniacal. Add ammonium chloride, and then the usual magnesia mixture ( 62, 6), in sufficient but not too excessive quantity (see 62, 6). The precipitate being under these conditions somewhat slowly formed, appears distinctly crystalline. After some time add am- monia gradually to the amount of one third of the fluid. Allow * Pogg. Anna!. 73, 137. f There are, however, other considerations which forbid going too far in this respect, $ Sillim. .Tourn. May, 1851. 405. 134.] PHOSPHORIC ACID. 375 to stand 12 hours in a well-covered vessel in the cold, filter, test the filtrate with magnesia mixture and ammonia, and wash the pre- cipitate with ammonia diluted with 3 volumes of water till the washings, when acidified with nitric acid and tested with silver nitrate, are no longer rendered turbid ; proceed according to 104, 2. The precipitate is not absolutely insoluble in ammoniated water, therefore it is well to wash by suction, as this reduces the necessary amount of wash water to a minimum. The results are accurate (Expt. No. 89, also KISSEL*). If there is reason to sus- pect the purity of the precipitate, dissolve it in hydrochloric acid, and throw down again with ammonia, adding some magnesia mixture. If the magnesia mixture is omitted, the solution being free from magnesia will dissolve some of the precipitate. Com- pare KISSEL, loc. cit. Properties of the precipitate and residue, 74. If the solution contains pyrophosphoric acid, the precipi- tate is flocculent and dissolves to a notable degree in ammoniated water (WEBER). ft. Indirect determination, with previous precipitation as arfnno- nium phosphomolybdate, after SoiorENSCHEiN.f Applicable in all cases in which the phosphoric acid present is orthophosphoric, even in presence of salts of the alkali-earth metals, aluminium, ferric iron, &c. Tartaric acid, however, and similar! v acting organic substances must be absent. No considerable quan- tity of free hydrochloric acid may be present. Large quantities of ammonium chloride, and of metallic chlorides generally, also of certain ammonium salts, especially the oxalate and citrate (KoNiG)J, are to be avoided. Ammonium nitrate assists the precipitation and neutralizes the injurious action of very large quantities of nitrates and sulphates (E. RICHTERS). The molybdenum solution described u Qual. Anal.," 55, is employed as the precipitant. It contains 5 per cent, of molybdic acid. The fluid to be examined for phos- phoric acid should be concentrated, it may contain free nitric or free sulphuric acid. Transfer to a beaker and add a considerable quantity of the molybdenum solution. About 40 parts molybdic acid must be added for every 1 part phosphoric anhydride, there- fore 80 c.c. of the molybdic solution for -1 grm. Stir, without touching the sides, and keep covered 12 hours at about 40. Then remove a portion of the clear supernatant fluid with a pipette, mix * Zeitschr. f. anal. Chem. 8, 170. \ Journ. f. prakt. Chem. 53, 343. \ Zeitschr. f . anal. Chem. 10, 305. Ib. 10, 4G9. 376 DETERMINATION. [ 134. it with an equal volume of molybdenum solution, and allow it to stand some time at 40. If a further precipitation takes place, return the portion to the main quantity, add more molybdenum solution, allow to stand again 12 hours, and test again. When complete precipitation has been effected pour the fluid off through a small filter and wash the precipitate entirely by decantation, using a mixture of 100 parts molybdate, solution, 20 parts nitric acid of 1'2 sp. gr., and 80 parts water.* The washing must be thorough, and the last runnings must not be precipitated by excess of ammonia, even if lime, iron, &c., was present in the solution. Now dissolve the precipitate in the least quantity of ammonia, pour the fluid through the small filter, when the minute amount of precipitate thereon will be dissolved, wash the filter with ammonia diluted with three volumes of water, mix the filtrate and washings, and add hydrochloric acid carefully till the precipitate produced, instead of redissolving instantly, takes a little time to disappear ; finally throw down with magnesia mixture (compare a). If the ammonia leaves a small amount of the precipitate undissolved, treat the residue with nitric acid and test the filtrate with molybdic solution in order to save any phosphoric acid. Results accurate.f As this method requires so large a quantity of molybdic acid, it is usually resorted to only in cases where methods &, a, and c are inapplicable ; and the phosphoric acid in the quantity of substance taken is not allowed to exceed '3 grm. Arsenic acid and silicic acid,;): if present, must first be removed. Of all the methods for determining phosphoric acid which are admissible in the presence of ferric and aluminium salts, this is the best in my opinion, espe- cially for the estimation of small quantities of the acid in presence of large quantities of these salts. * According to E. RICHTERS (Zeitschr. f. anal. Chem. 10, 471) you may also wash with a solution of ammonium nitrate containing 15 grm. in 100 c.c. slightly acidified with nitric acid and containing a few per-cents of molybdic acid solution. f Zeitschr. f. anal. Chem. 3, 446, and 6, 403. \ Silicic acid may also be thrown down, in form of a yellow precipitate, by acid solution of ammonium molybdate, especially in presence of much ammo- nium chloride (W. KNOP, Chem. Centralb. 1857, 691). Mr. GRUNDMANN, who repeated KNOP'S experiments in my laboratory, obtained the same results. The precipitate dissolves in ammonia. If the solution, after addition of some ammo- nium chloride, is allowed to stand for some time, the silicic acid separates, and the phosphoric acid may then be precipitated from the filtrate with magnesia- mixture; it is, however, always the safer way to remove silicic acid first. 134.] PHOSPHORIC ACID. 377 y. Indirect determination, with previous precipitation as mer- curous phosphate, after H. HOSE.* Applicable for the separation of phosphoric acid (also of pyro^ and metaphosphoric acid) from all basic radicals, except aluminium. Comp. 135, L Dissolve the phosphate in neither too large nor too small a quantity of nitric 'acid, in a porcelain dish, add pure metallic mer- cury in sufficient quantity to leave a portion, even though only a small one, undissolved by the free acid. Evaporate on the water- bath to dryness. If the warm mass still evolves an odor of nitric acid, moisten it with water, and heat again on the water-bath, until it smells no longer of nitric acid. Add now hot water, pass through a small filter, and wash until the washings leave no longer a fixed residue upon platinum. Dry the filter, which, besides mercurous- phosphate, contains also basic mercurous nitrate and free mercury,, mix its contents, in a platinum crucible, with mixed sodium and potassium carbonates in excess, roll the filter into the shape of a ball, place it in a hollow made in the mixture, and cover the whole with a layer of the mixed carbonates. Expose the crucible, under a chimney with good draught, for about half an hour to a moderate heat, so that it does not get red-hot. At this temperature, the mercurous nitrate and the metallic mercury volatilize. Heat now over the lamp to bright redness, and treat the residue with hot' water, which will dissolve it completely, if no ferric oxide be present, and if no oxide of platinum has been formed. The latter may occur on account of too rapid heating, which might produce sodium nitrate, which would act upon the platinum. Supersatu- rate the clear (if necessary, filtered) solution with hydrochloric acid, add ammonia and magnesia-mixture, and proceed as in a. d. Indirect determination, with previous precipitation as stan- nic phosphate. After GiRAKD.f Dissolve the substance in highly concentrated nitric acid, remove all chlorine either by precipitation with silver nitrate or by repeated evaporation with nitric acid, add 8 times as- much tinfoil as there is phosphoric acid present, and warm the mixture 5 or 6 hours, until the precipitate has completely subsided, leaving the supernatant fluid clear. Wash with hot water by decantation and finally by filtration. The precipitate consists of * Pogg. Annal. 76, 218. f Compt. rend. 54, 468; Zeitschrift f analyt, Chem. I, 366. 378 DETERMINATION. [ 134. metastannic acid and stannic phosphate, together with a little ferric and aluminium phosphate. Heat it either at first with a small quantity of aqua regia, and then with ammonia and ammonium sulphide, or immediately with ammonium sulphide in excess. The last process is recommended by O. BABER,* on the ground that the former leaves a little phosphoric acid in the precipitate. The whole is digested about two hours, and then filtered ; the precipi- tate, consisting of ferrous sulphide and aluminium hydroxide, is washed with warm ammonium sulphide, then with water contain- ing a little ammonium sulphide, dissolved in nitric acid, and the solution thus formed mixed with the filtrate from the tin precipi- tate which contains the principal quantity of the basic metals. From the ammonium -sulphide filtrate, which contains stannic sul- phide and ammonium phosphate, the phosphoric acid is at once precipitated by magnesia-mixture. I may add that GIRARD con- siders 4 to 5 parts tin sufficient for 1 part P 2 O 5 . The results afforded by his test-analyses are unexceptionable. According to jANovsKY,f at least six parts of tin must be used. The tin should be free from arsenic. c. Determination as TJrcmyl Pyrophosphate. After LECONTE, A. ARENDT, and W. KNOP.^: (Very suitable in presence of alkali and alkali-earth metals, but not in presence of any notable amount of aluminium ; in presence of ferric iron, the method can be applied only with certain modifications. ) Where it is possible, prepare an acetic acid solution of the compound. If jou have a nitric or hydrochloric acid solution, remove the greater portion of the free acid by evaporation, add ammonia until red litmus paper dipped into it turns very distinctly blue, and then redissolve the precipitate formed in acetic acid. If mineral acids were present, add also some ammonium acetate ; this addition is beneficial under any circumstances. Mix the fluid now with solu- tion of uranyl acetate, and heat the mixture to boiling, which will cause the phosphoric acid to separate, in form of pale greenish- yellow ammonium uranyl phosphate. * Zeitschr. f. die gesammten Naturwissensch. 1864, 293. f Zeitschr. f. anal. Chem. 11, 157. \ LECONTE was the first to recommend the method of precipitating phospho- ric acid from acetic acid solutions by means of a salt of uranium (Jahresb. von LIEBIG und KOPP, fiir 1853, 642); A. ARENDT and W. KNOP have subsequently subjected k to a careful and searching examination (Chem. Centralbl. 1856, 769, 803; and 1857, 177). Chem. Centralbl. 1857, 182. 134.] PHOSPHORIC ACID. 379 Wash the precipitate, first by decantation, boiling up each time, then by filtration ; the operation may be materially facilitated by adding a few per-cents of ammonium nitrate to the water. Dry the precipitate, and ignite as directed 53. It is advisable to evaporate small quantities of nitric acid on the ignited precipitate repeatedly, and to reignite. The residue must have the color of the yolk of an egg. For the properties of the precipitate and resi- due, see 93, 4, e. Should it be necessary to dissolve the ignited residue again, for the purpose of reprecipitating it, this can be done only after fusing it with a large excess of mixed sodium and potas- sium carbonates, and thereby converting the pyrophosphoric into orthophosphoric acid. Results accurate ; compare the test-analyses given by the authors, Expt. No. 90, and KISSEL'S experiments.* d Deter minati potassium borqfluoride, alkalies only (preferably only potash) may be present. The process * Zeitschr. f. anal. Chem. 1, 405. 136.] BORIC ACID AND BORIC ANHYDRIDE. 391 is conducted as follows : Mix the fluid with pure solution of potassa, adding for each mol. boric acid supposed to be present, at least 1 mol. potassa ; add pure hydrofluoric acid (free from silicic acid) in excess, and evaporate, in a platinum dish, on the water-bath, to diyness. The fumes from the evaporating fluid should redden litmus paper, otherwise there is a deficiency of hydrofluoric acid. The residue consists now of KF,BF S and KF,HF. Treat the dry saline mass, at the common temperature, with a solution of 1 part of potassium acetate in 4: parts of water, let it stand a few hours, with stirring, then decant the fluid portion on to a weighed filter, and wash the precipitate repeatedly in the same way, finally on the filter, with solution of potassium acetate, until the last rinsings are no longer precipitated by calcium chloride. By this course of pro- ceeding, the hydrogen potassium fluoride is removed, without a particle of the potassium borofluoride being dissolved. To "remove the potassium acetate, wash the precipitate now with alcohol of 78 per cent., dry at 100, and weigh. As potassium chloride, -nitrate, and phosphate, sodium salts, and even, though with some difficulty, potassium sulphate, dissolve in solution of potassium acetate, the presence of these salts does not interfere with the estimation of the boric acid; however, sodium salts must not be present in consider- able proportion, as sodium fluoride dissolves with very great diffi- culty. The results obtained by this method are satisfactory. STKO- MEYER'S experiments gave from 97*5 to 10O7 instead of 100. When the amount of alkali salt to be removed is very large, the saline mass left on evaporation should be warmed with the solution of potassium acetate, allowed to stand 12 hours in the cold and then filtered. In this way the quantity of potassium acetate required will be much reduced. For the composition and proper- ties of potassium borofluoride, see 93, 5. As the salt is very likely to contain potassium silicofluoride it is indispensable to test it for that substance ; this is done by placing a small sample of it on moist blue litmus paper, and putting another sample into cold concentrated sulphuric acid. If the blue paper turns red, and effervescence ensues in the sulphuric acid, the salt is impure, and contains potassium silicofluoride. To remove this impurity, dis- solve the remainder of the salt, after weighing it, in boiling water, add ammonia, and evaporate, redissolve in boiling water, add ammonia, &c., repeating the same operation at least six times. Finally, after warming once more with ammonia, filter off the 392 DETERMINATION. [ 136. silicic acid, evaporate to dryness, and treat again with solution of potassium acetate and alcohol (A. STROMEYER).* I was obliged to modify STROMEYER'S method for effecting the separation of the silicic acid, the results of my experiments having convinced me that treating the salt only once with ammonia, as recommended by that chemist, is not sufficient to effect the object in view. II. Separation of Boric Acid from the Basic Radicals* a. from the Alkalies. Dissolve a weighed quantity of the borate in water, add an excess of hydrochloric acid, and evaporate the solution on the water-bath. Towards the end of the operation add a few more drops of hydrochloric acid, and keep the residue on the water-bath, until no more hydrochloric acid vapors escape. Determine now the chlorine in the residue ( 141), calculate from this the alkali, and you will find the boric acid from the difference. E. SOHWEIZER, with whom this method originated, states that it gave him very satisfactory results in the analysis of borax. It will answer also for the estimation of the basic metals in the case of some other borates. It is self-evident that the boric acid may be estimated, in another portion of the salt, by I., 1, c, or 2. If you have to estimate boric acid in presence of large proportions of alkali salts, make the fluid alkaline with potassa, evaporate to dry- ness, extract the residue with alcohol and some hydrochloric acid, add solution of potassa to strongly alkaline reaction, distil off the alcohol, and then proceed as in I., 1, #, or 2 (Auo. STROMEYER, loc. cit.). LuNGEf determined the soda in boronatrocalcite alkalimetri- cally, by dissolving the mineral in normal nitric acid and titrat- ing back with normal soda, till the tint of the litmus added becomes violet. 1). From Calcium. Dissolve in hydrochloric acid in the heat, avoiding too large an excess, neutralize with ammonia and precipitate with ammonium oxalate (LUNGE, loc. cit.). c. From almost all other Bases except Alkalies. The compounds are decomposed by boiling or fusing with potassium carbonate or hydroxide ; the precipitated base is filtered off, and the boric acid determined in the filtrate, according to I., 1, * Annal. d. Chem. u. Pharm. 100, 82. f Ib. 138, 53. 136.] BORIC ACID AND BORIC ANHYDRIDE. 393 d, or 2. If magnesium was present, a little of this is very likely to get into the filtrate, and if process L, 2, is employed upon neutralizing with hydrofluoric acid, this separates an insoluble magnesium fluoride, which may either be filtered off at once, or removed subsequently, by treating the potassium borofluoride with boiling water, in which that salt is soluble, and the magnesium fluoride insoluble. d. From the Metallic Oxides of the Fourth, Fifth, and Sixth Groups. The metallic oxides are precipitated by hydrogen sulphide, or T as the case may be, ammonium sulphide,* and determined by the appropriate methods. The quantity of boric acid may often be inferred from the loss. If it has to be estimated in the direct way, the filtrate, after addition of solution of potassa and some potassium nitrate, is evaporated to dry ness, the residue ignited, and the boric acid estimated by I., 1, d, or 2. In cases where the metal has been precipitated by hydrogen sulphide from acid or neutral solutions, the boric acid may also be determined in the filtrate in the absence of other acids by L, 1, a or b or c-, after the complete removal of the hydrogen sulphide by transmitting carbon dioxide through the fluid. e. From the whole of the Fixed Ba&ic Radicals. A portion of the very finely pulverized substance is weighed r put into a capacious platinum dish, and digested with a sufficient quantity of hydrofluoric acid (which leaves no residue when evapo- rated in a platinum dish) ; pure concentrated sulphuric acid is then gradually added, drop by drop, and the mixture heated, gently at first, then more strongly, until the excess of the sulphuric acid is completely expelled. In this operation the boric acid goes off in the form of fluoride of boron (B,O 3 + 6HF = 2BF 8 + 3H,O). The basic metals contained in the residue in the form of sulphates are determined by the appropriate methods, and the quantity of the boric acid is found by difference. It is of course taken for granted that the substance is decomposable by sulphuric acid. * Boric acid cannot be separated completely from aluminium by precipitation of the hydrochloric acid solution with ammonium sulphide or with ammonium carbonate (WOHLEB, Ann. d. Chem. u. Pharm. 141, 394 DETERMINATION. [ 137. 3. OXALIC ACID. I. Determination. Oxalic acid is either precipitated as calcium oxalate, and esti- mated after determination of the calcium in the latter as oxide, carbonate, or sulphate; or the amount contained in a compound is inferred from the quantity of solution of potassium permanga- nate required to effect its conversion into carbonic acid ; or from the quantity of gold which it reduces ; or from the amount of car- bonic acid which it affords by oxidization. a. Determination as Calcium Carbonate, <&c. Precipitate with solution of calcium acetate, added in moderate excess, and treat the precipitated calcium oxalate as directed in 103. If this method is to yield accurate results, the solution must be neutral or slightly acid with acetic acid / it must not con- tain salts of aluminium, chromium, or of the heavy metals, more especially cupric or ferric salts ; therefore, where these conditions do not exist, they must tirst be supplied. b. Determination by means of Solution of Potassium Perman- ganate. Standardize the solution of potassium permanganate, as directed 112, 2, a, cc, by means of oxalic acid ; then dissolve the substance in about 150 c.c. water, or acid and water (sulphuric acid is the best acid to use) ; add, if necessary, a further quantity of sulphuric acid (about 6 or 8 c.c. strong sulphuric acid should be present), heat to about 60, and then run in the permanganate, with constant stirring, until the fluid just shows a red tint. Knowing the quan- tity of oxalic acid which 100 c.c. of the standard permanganate will oxidize, a simple calculation will give the quantity of oxalic acid corresponding to the c.c. of permanganate used in the experi- ment. The results are very accurate. c. Determination from the reduced Gold (H. KOSE). a. In compounds soluble in water. Add to the solution of the oxalic acid or the oxalate a solution of sodium auric chloride, or ammonium auric chloride, and digest for some time at a tempera- ture near ebullition, with exclusion of direct sunlight. Collect the precipitated gold on a filter, wash, dry, ignite, and weigh. 2 at. 137.] OXALIC ACID. 395 Au. (196-71 X 2 = 393-42) correspond to 3 mol. C,O 3 (72 X 3 = 216). ft. In compounds insoluble in water. Dissolve in the least possible amount of hydrochloric acid, dilute with a very large quantity of water, in a capacious flask, cleaned previously with solution of soda ; add solution of gold in excess, boil the mixture some time, let the gold subside, taking care to exclude sunlight, and proceed as in a. d. Determination as Carbonic Add. This may be effected either, a. By the method of organic analysis ; or ft. By mixing the oxalic acid or oxalate with finely pulverized manganese dioxide in excess, and adding sulphuric acid to the mix- ture, in an apparatus so constructed that the disengaged CO, passes off perfectly dry. The theory of this method may be illustrated by the following equation : H,C 2 O 4 + MnO 3 + H,SO 4 = MnSO, -f- 2H,O + 2CO a . For the apparatus and process, I refer to the chapter on the examination of manganese ores, in the Special Part of this work. Here I may remark that free oxalic acid must first be prepared for the process by .slight supersaturation with alkali free from carbonic acid, and also that 9 parts of oxalic anhydride (C 2 O 3 ) require theoretically 11 parts of (pure) manganese dioxide. Since an excess of the latter substance does not interfere with the accuracy of the results, it is easy to find the amount to be added. The manganese dioxide need not be pure, but it must contain no carbonate. This method is expeditious, and gives very accurate results, if the process is conducted in an apparatus sufficiently light to admit of the use of a delicate balance. Instead of manganese dioxide, potassium chromate may be used (compare 130, 1, c), and instead of estimating the carbonic acid by loss it may be col- lected by an absorbent and weighed ( 139, II., e) ; the latter method is always to be preferred in the case of small quan- tities. II. /Separation of Oxalic Acid from the Basic Radicals. The most convenient way of analyzing oxalates is, in all cases, to determine in one portion the acid, by one of the methods given in I., in another portion the basic radical, particularly as the latter object may be generally effected by simple ignition in. the air, which reduces the salt either to the metallic state (e.g., silver oxa- 396 DETERMINATION. [ 138. late), or to pure oxide (e.g., lead oxalate), or to carbonate (e.g., the oxalates of the alkalies and alkali-earth metals). If the acid and basic radical have to be determined in one and the same portion of the oxalate, the following methods may be resorted to : a. The oxalic acid is determined by L, c, and the gold separated from the basic metals in the filtrate by the methods given in Sec- tion V. J. In many soluble salts the oxalic acid may be determined by the method L, a ; separating the basic metals afterwards from the excess of the calcium salt by the methods given in Section Y. c. Many oxalates of metals which are completely precipitated "as carbonates or oxides by excess of sodium or potassium carbonate, may be decomposed by boiling with excess of these reagents, metallic oxide or carbonate being formed, on the one, and alkali oxalate on the other side. d. All oxalates of the metals of the fourth, fifth, and sixth groups may be decomposed with hydrogen sulphide or ammonium sulphide. 138. 4. HYDROFLUORIC ACID. I. DETERMINATION. Free hydrofluoric acid in aqueous solution* is determined either with standard alkali or as calcium fluoride. In the latter case sodium carbonate is added in moderate excess, then the solution being boiled, calcium chloride is added as long as a precipitate con- tinues to form ; when the precipitate, which consists of calcium fluoride and carbonate, has subsided, it is washed, first by decanta- tion, afterwards on the filter, and dried ; when dry, it is ignited in a platinum crucible ( 53) ; water is then poured over it in a plati- num or porcelain dish, acetic acid added in slight excess, the mix- ture evaporated to dryness on the water-bath, and heated on the latter until all odor of acetic acid disappears. The residue, which consists of calcium fluoride and acetate, is heated with water, the * In analyzing fluorides you must always avoid bringing acid solutions in contact with glass or porcelain. If platinum or silver dishes of sufficient size are not at hand you may sometimes use gutta-percha vessels, or glass vessels coated with wax or paraffin. $ 138.] HYDROFLUORIC ACID. 397 calcium fluoride filtered off, washed, dried, ignited ( 53), and weighed. As a control of the purity of the calcium fluoride, it is well to convert it after weighing into sulphate. If the precipitate of calcium fluoride and carbonate were treated with acetic acid, without previous ignition, the washing of the fluoride would prove a difficult operation. Presence of nitric or hydrochloric acid in the aqueous solution of the hydrofluoric acid does not interfere with the process (H. ROSE). II. SEPARATION OF FLUORINE FROM THE METALS. 1. Fluorides Soluble in Water. If the solutions have an acid reaction, sodium carbonate is added in excess. If there is an odor of ammonia now, heat till the latter is expelled. If the sodium carbonate produces no precipitate, the fluorine is determined by the method given in L, and the metals in the filtrate are separated from calcium and sodium by the methods given in Section V. But if the sodium carbonate pro- duces a precipitate, the mixture is heated to boiling, then filtered, and the fluorine determined m the filtrate by the method given in I. ; the metals are in the precipitate, which must, however, first be tested, to make sure that it contains no fluorine. Neutral solutions are mixed with a sufficient quantity of calcium chloride, and the mixture heated to boiling in a platinum dish or, but less appropri- ately, in a porcelain dish ; the precipitate of calcium fluoride is allowed to subside, thoroughly washed with hot water by decanta- tion, transferred to the filter, dried, ignited, and weighed. The basic metals in the filtrate are then separated from the excess of the calcium salt by the usual methods. That the basic metals may be determined also in separate portions by the methods given in 2 #, need hardly be stated. 2. Insoluble Fluorides. a. Decomposition l>y Sulphuric Add (Indirect Estimation of the Fluorine). a. Anhydrous Compounds. The finely pulverized and weighed substance is heated for some time with pure concentrated sulphuric acid, and finally ignited until the free sulphuric acid is completely expelled. In the presence of alkalies, ammonium carbonate 'must be added during the igni- tion. The residuary sulphate is weighed, and the metal contained in it calculated ; the fluorine is estimated by loss. In cases where 398 DETERMINATION. [ 138. we have to deal with a metal whose sulphate gives off part of the sulphuric acid upon ignition, or where the residue contains several metals, it is necessary to subject the residue to analysis before this calculation can be made. In the case of many compounds, for instance of aluminium fluoride (which after ignition requires pro- longed heating with sulphuric acid for its decomposition), long continued strong ignition does not leave the sulphate, but the oxide in a pure state. Topaz (a silicate of aluminium in isomorphous mixture with aluminium silicofluoride) is not decomposed by boil- ing sulphuric acid, but it is decomposed by fusion with potassium disulphate. ft. Hydrated Fluorides. A sample of the substance is heated in a tube. aa. The Water expelled does not redden Litmus Paper. The water is determined by ignition ; the fluorine and metal as directed in a, a. lib. The Water expelled has an acid reaction. The substance is treated with sulphuric acid as directed in #, a, to determine the metal on the one hand, and the water -|- fluorine on .the other. Another weighed portion is then mixed, in a small retort, with about 6 parts of recently ignited lead oxide ; the mixture is covered with a layer of lead oxide, the retort weighed, and the water expelled by the application of heat, increased gradually to redness. No hydrofluoric acid escapes in this process. The weight of the expelled water is inferred from the loss. The first operation having given us the water -\- fluorine, and the second the water alone, the dif- ference is consequently the fluorine. b. Decomposition ~by Fusion with Alkali Carbonates. Many insoluble fluorides, aluminium fluoride for instance, may be completely decomposed by fusion with alkali carbonate alone ; others, such as calcium fluoride, require the addition of silicic acid. In the first case the fluorine is estimated in the aqueous solution of the fusion according to I., in the latter according to 166, 5. The temperature must not be too high, or some alkali fluoride may be lost. 3. Fluorides completely Decomposable by Sulphuric Acid. As might be inferred from 2, almost all fluorides are decom- posed by heating with sulphuric acid with evolution of hydroflu- 138.] HYDROFLUORIC ACID. 399 oric acid. If silica or silicate is added to the fluoride in sufficient quantity, silicon fluoride and water escape instead of hydrofluoric acid: SiO, + 4HF = SiF 4 + 2H.O. On this reaction methods of determining fluorine have been based. In the first, which I published some years ago,* the fluor- ide of silicon is determined by increase of weight of absorption tubes ; this I believe to be in many cases the only method which is applicable, and when carefully carried out yields ttie most accu- rate results. a. Estimation by Absorption of the evolved Fluoride Silicon. The method as here given is the result of a long series of experi- ments ; the conditions laid down must be most carefully attended to. The fluoride must be in the finest powder. As silicic acid we use finely powdered quartz, w r hich has been ignited in the air to destroy any organic admixture. The sulphuric acid should have a sp. gr. of 1 848, it must be colorless and free from oxides of nitro- gen and sulphurous acid. The gasometer must be filled with clean air, and not with air from the laboratory, for any dust of organic matter, traces of coal gas, &c., would interfere with the accuracy of the result. The apparatus required is shown fig. 57. A contains atmospheric air, b is half filled with sulphuric acid, c contains soda- lime with plugs of cotton, d pieces of glass moistened with sulphuric acid. The air is thus freed from carbonic acid and suspended mat- ter, and dried by sulphuric acid (p. 61). e is the decomposing flask ; it has a capacity of about 250 c.c. f is half filled with sulphuric acid ; its cork, which should not fit air-tight, bears a thermometer w T hose bulb dips into the acid, e andy should be so placed on the iron plate that the temperature in both may be equal, g is empty ; h contains fused calcium chloride in the first limb, and pumice impregnated with anhydrous cupric sulphate in the second. These U-tubes serve to retain the small amount of sulphuric acid and the hydrochloric acid which may accompany it. The calcium chloride and the cupric sulphate must both be anhydrous, or they will decompose and retain silicon fluoride. a, &, and I are the weighed absorption tubes; they are 10 or 12 cm. high, and about 12 mm. wide, i contains in the first limb pumice moistened with water between plugs of cotton, in the bend and half of the second limb soda- lime, in the upper half of the second limb fused calcium chloride *Zeitschr. f. anal. Chem. 5, 190. 400 DETERMINATION. [138. between pings of cotton. The tube after being charged weighs about 40 or 50 grm. ~k completes the absorption ; it is filled half with soda-lime and half with fused calcium chloride. I takes up again the small amount of water carried away from i and &; the bend is filled with pieces of glass moistened with sulphuric acid. These 138.] HYDROFLUORIC ACID. 401 absorption tubes retain the silicon fluoride, the carbonic acid which may be possibly evolved from the soda-lime by hydrofluosilicic acid, and the aqueous vapor ; and the air escapes through the unweighed guard tube m into the atmosphere. The latter contains in the first limb calcium chloride, in the second soda-lime. The flexible con- nections should not be long, and should be washed and dried before use. When the apparatus has been tested and found air-tight, place the weighed and very finely divided substance in e. The substance should be free from carbonic acid, and the quantity taken should give not less than -1 grm. silicon fluoride if possible. Add for every part of fluoride supposed to be present 10 or 15 parts of finely powdered quartz (previously strongly ignited in the air), and then 40 or 50 c.c. pure concentrated sulphuric acid. Connect e, on the one hand, with d, and, on the other, with g, and pass a moderate current of air, which should enter the fluid in the decomposing flask from the bottom. Heat the iron plate, shake e frequently and raise the temperature very gradually, till the thermometer in f indicates 150 to 160. The commencement of the decomposition shows itself not only by the appearance of bubbles of gas in the fluid, more particularly at the edge, but also by the separation of hydrated silica in i. The bubbles of gas will disappear on shaking the fluid ; as soon as they cease to form again remove the lamp ; the time usually occupied in the decomposition is one hour for small quantities of fluoride ( 1 grm.), two or three hours for large quantities (1 grm.). After a while shut off the current of air, remove the weighed tubes 2, &, and /, and during the weighing of these connect h with m by means of a glass tube. After weighing replace 2", &, and /, heat again to 150 or 160, and pass the air again for half an hour or an hour, weighing *, &, and I again. If any alteration of weight has occurred, the process must be continued. The increase in weight of the absorption tubes after deducting - 001 grm. for every hour during which the air has been passing (i.e., for every 6 litres of air) represents the amount of silicon fluoride. The small correction is necessary because air, even when it comes in contact only with short washed pieces of india-rubber, always gives traces of sulphurous and carbonic acid when passed through hot concentrated sulphuric acid. The results thus obtained are very satisfactory, and differ from the truth at the most by a few milligrammes. 402 DETERMINATION. [ 130. b. Other methods of Estimating the Silicon Fluoride expelled. a. Method of WOHLEE. Only applicable when the substance is readily decomposed by sulphuric acid, and the amount of fluorine is large. Transfer the very finely divided substance, if necessary, intimately mixed with 10 or 15 parts of ignited quartz powder, to a small flask, add pure sulphuric acid, close quickly with a cork fitted with a small tube filled with fused calcium chloride (or better still, half with fused calcium chloride and half with anhydrous cupric sulphate on pumice), weigh the whole apparatus as quickly as pos- sible, warm it till no more fumes of silicon fluoride escape, remove the last particles of gas in the apparatus by an air pump, allow to cool, and weigh. The loss of weight indicates the amount of silicon fluoride. ft. [S. L. PENFIELD* determines the amount of expelled silicon fluoride by an indirect volumetric method ; viz. : by passing it into a solution of potassium chloride, and titrating the hydrochloric acid which is set free with standard ammonia solution. 3SiF 4 -f- 2 H 2 = 2 H 2 F 2 SiF 4 + Si0 2 and H 2 F 2 SiF 4 + 2KC1 = (KF) 2 SiF 4 + 2 HC1. Two mol. HC1 thus liberated correspond to six at. F. ' The process of decomposing the fluorine compound is conducted as in , and the same apparatus may be used except that the four last U-tubes *, &, /, m, are replaced by two larger U-tubes for hold- ing the solution of potassium chloride. The aqueous solution of KC1 is mixed with an equal volume of alcohol to effect complete precipitation of the hydroflupsilicic acid. The titration may be either effected directly in U-tubes (the second of which will contain but a very small quantity of acid) or after transferring to a beaker and rinsing the tubes with alcohol and water. Care must be taken to loosen and break up the silicic acid and to have at least half of the final volume at the end of the titra- tion consist of alcohol. Kesults given by the author (loc. cit.) very satisfactory.] * American Chem. Journ. i. p. 27. 139.] CARBONIC ACID. . 403 Fourth Division of the First Group of the Adds. CARBONIC ACID SILICIC ACID. 139. 1. CARBONIC Aero. I. Determination. a. In a mixture of Gases. After thoroughly drying the gases with a ball of calcium chloride, or saturating with moisture ( 16), measure them accurately in a graduated tube over mercury, insert a ball of hydrate of potassa,* cast on a platinum wire in a pistol bullet-mould, take care that the end of the platinum wire remains under the surface of the mercury, leave in the tube for 24 hours, or until the volume of the gas ceases to show further diminution ; withdraw the ball, and measure the gas remaining, reinsert the same or a fresh ball of potassa, and repeat till no further absorption takes place. The carbonic acid gas is inferred from the difference, provided the gaseous mixture contained no other gas liable to absorption by potassa (compare 12-16). In very accurate analyses you must bear in mind that carbonic acid does not exactly follow the law of MARIOTTE. If the amount of carbonic acid is very small, this process does not yield sufficiently accurate results. In such cases one of the. methods recommended in "The Analysis of Atmospheric Air" should be employed. Several kinds of special apparatus are in use for the estimation of carbonic acid in coal gas and for the purposes of sugar works. I may mention those proposed by F. RuDORFFf and LEHMANN and H. WAHLERTJ: for the first purpose, and by C. SCHEIBLER and C. STAMMERJ! for the second. Besides these volu- metric methods the gravimetric processes given by myself for the analysis of gaseous mixtures^ may often be used with great advan- tage. * The ordinary hydrate is not adapted for the purpose. It should be fused with a quarter of its weight of water in a platinum crucible. f Pogg. Annal. 125, 71. f Zeitschr. f. anal. Chem. 7, 58. Dingler's polyt. Journ. 183, 306. | Ib. 102, 368. 11 Zeitschr. f. anal. Chem. 3, 343. 404 DETERMINATION. [ 139. J. In Aqueous Solution. a. WITH CALCIUM HYDROXIDE. Into a flask, holding about 300 c.c., put 2'5 to 3 grin, calcium hydroxide perfectly free from carbonate.* Provide the flask with a good india-rubber stopper, tare or weigh exactly, add the car- bonic acid water with gentle agitation till the flask is two thirds or three quarters fall, and close at once. In adding the carbonic acid water every care must of course be taken to guard against loss of carbonic acid. If the water flows from a pipe, it is allowed simply to run in. If it is in a jug or bottle, cool it to 4, and transfer the quantity required with a syphon.f If the water is in a basin or well, provide the flask with a stopper in which two glass tubes are inserted, one a few inches long, pushed down only to the lower surface of the stopper, the other extending through the stopper a short distance into the flask, but only to the upper surface of the stopper. Sink the flask into the water, and water will enter one tube and air escape through the other. Water which is not very rich in free carbonic acid may be removed from the basin or well by a plunging-syphon. Now weigh the flask with its stopper again, and you will find the quantity of water taken. No way of measuring the water is so accurate in retaining all the carbonic acid and in giving the quantity of water taken. If there is much interval between the mixing of the water and the lime and the estimation of the carbonic acid in the precipitate, the calcium carbonate, which is at first amorphous, passes spontane- ously into the crystalline condition ; but if the carbonic acid is to be determined soon after the mixing, heat for some time on the water-bath, raising the stopper occasionally, in order to hasten the change of the calcium carbonate. Now, without disturbing the precipitate, filter the clear fluid through a small plaited filter, which will take a very short time, throw the filter at once into the flask containing the precipitate and the rest of the fluid, and pro- ceed according to II., e. This process has been in use for 10 years in my laboratory for all mineral water analyses ; it is extremely * This is prepared by slaking freshly burnt lime with water in such a man- ner that the hydrate obtained appears dry and pulverulent. It is preserved in small bottles, the corks or stoppers of which are covered with sealing wax. f If the water is poured directly from the jug into the flask, carbonic acid gas is very likely to get into the latter as well as the water. 139. j CARBONIC ACID. 405 simple, and gives excellent results.* If the water contains alkali carbonate, put a quantity of calcium chloride sufficient to decom- pose the alkali carbonate with the lime in ' the flask before adding the water. ft. AFTER PETTEXKOFER.f The principle of this simple and expeditious process consists in mixing the carbonic acid water with a measured quantity of stand- ard lime water (or, under certain circumstances, baryta water) in excess. After complete separation of the calcium or barium carbo- nate, the excess of calcium or barium in the fluid is determined in an aliquot part by means of standard solution of oxalic acid ; the difference gives the calcium or barium precipitated by the carbonic acid, and consequently the amount of the latter present. If a water contains only free carbonic acid, the analyst has only to bear in mind if lime water is employed that the calcium car- bonate formed is at first, as long as it remains amorphous, very perceptibly soluble in water, to which it communicates an alkaline reaction. Hence the unprecipitated lime in the fluid cannot be estimated till the calcium carbonate has separated in the crystalline form, which takes 8 or 10 hours, unless the mixture is warmed to 70 or 80. On this account it is generally best to use baryta water (see " Analysis of Atmospheric Air"). If, on the contrary, a water contains an alkali carbonate or any other alkali salt whose acid would be precipitated by lime or baryta, a neutral solution of calcium or barium chloride must first be added to decompose the same. This addition, too, prevents any incon- venience arising from the presence of free alkali in the lime or baryta water, or of magnesium carbonate in the carbonic acid water; this inconvenience consists in the fact that oxalate of an alkali or of magnesium enters into double decomposition with cal- cium carbonate (which is seldom entirely absent from the fluid to be analyzed), forming calcium oxalate and carbonate of the alkali or of magnesium, which latter will of course again take up oxalic acid. In the presence of magnesium salts in the carbonic acid water, in order to avoid the precipitation of the magnesium, a little ammonium chloride must also be added, but in this case heat must * Zeitschr. f. anal. Chem. 2, 49 and 341. f BDCHXER'S neues Repert. 10, 1; Journ. f. prakt. Chem. 82, 32; Annal. d. Chem. u. Pharm. ii., Supplementb. 1 ; Zeitschr. f. anal. Chem. 1, 92. 406 DETERMINATION. [ 139. not be applied to induce the calcium carbonate to become more quickly crystalline, as ammonia would be thereby expelled. In making the determination the first thing to be done is to ascertain the relation between the lime or baryta water and a standard solution of oxalic acid. PETTENKOFER makes the latter solution by dissolving 2'8636 grm. pure uneffloresced dry crystal- lized oxalic acid to 1 litre ; 1 c.c. of this is equivalent to 1 mgrm. carbonic acid. The lime water is standardized as follows : Measure 45 c.c. into a little flask which can be closed by the thumb, and then run in from the burette the solution of oxalic acid till the alkaline reaction has just vanished. During the operation the flask is closed with the thumb and gently shaken. The end is attained as soon as a drop taken out with a glass rod and applied to delicate turmeric paper* produces no brown ring. The first experiment is a rough one, the second should be exact. The analysis of a carbonic acid water (a spring water, for instance) is performed by transferring 100 c.c. to a dry flask, add- ing 3 c.c. of a neutral and nearly saturated solution of calcium or barium chloride, and 2 c.c. of a saturated solution of ammonium chloride, then 45 c.c. of the standard lime or baryta water; close the flask with an india-rubber stopper, shake and allow to stand 12 hours. The fluid contents of the flask measure consequently 150 c.c. From the clear fluidf take out by means of a pipette two por- tions of 50 c.c. each, and determine the free lime or baryta by means of oxalic acid, in the first portion approximately, in the second exactly. Multiply the c.c. used in the last experiment by 3 and deduct the product from the c.c. of oxalic acid which corre- spond to 45 c.c. of lime or baryta water. The difference shows the lime or baryta precipitated by carbonic acid, each c.c. corresponds to 1 mgrm. carbonic acid. * For the preparation of this bibulous paper should be used, the ash of which is free from carbonate of lime. Swedish filtering-paper answers best. J. GOTT- LIEB (Journ. f. prakt. Chem. 107, 488; Zeitschr. f. anal. Chem. 9, 251) prefers aqueous tincture of litmus, prepared from litmus first exhausted with spirit and used in a very dilute state. E. SCHULZE and M. MARCKER (Zeitschr. f. anal. Chem. 9, 334) employ corallin or rosolic acid, which they say is specially adapted for Ihe purpose. The alcoholic solution is cautiously neutralized with potash, and a drop or two of this tincture is added. F. SCHULZE (Zeitschr. f. anal. Chem. 9, 292) recommends spirituous tincture of turmeric. f It is not admissible to use a filter (A. MULLER, Zeitschr. f anal. Chem 1 84). 139.] CARBONIC ACID. 407 The method is convenient and good ; it is especially to be recommended for dilute carbonic acid water. When calcium sul- phate or carbonate is present, as is almost always the case in spring water, you must always before titrating await the conversion of the amorphous calcium carbonate to the crystalline state, even if baryta water is used (K. KNAPP*).. Baryta water therefore possesses no advantages over lime water for the analysis of spring waters. II. Separation of Carbonic Acid from the Basic Radicals, and its Estimation in Carbonates. a. Estimation in Normal Alkali Carbonates and Alkali-earth Carbonates. If the salts are unquestionably normal carbonates, and there is no other salt with power to neutralize an acid present, we may determine the quantity of the basic radical by the alkalimetric method ( 196, 198), and calculate the amount of CO, necessary to form with it normal carbonate. b. Separation from Basic Metals in Salts which upon ignition readily and completely yield their Carbonic Acid. Such are, for instance, the carbonates of zinc, cadmium, lead, copper, magnesium, &c. a. Anhydrous Carbonates. Ignite the weighed substance, in a platinum crucible (cadmium and lead carbonates in a porcelain crucible), until the weight of the residue remains constant. The results are, of course, very accurate. Substances liable to absorb oxygen upon ignition in the air are ignited in a bulb-tube, through which a stream of dry carbon dioxide gas is conducted. The car- bonic acid is inferred from the loss. ft. Hydritted Carbonates. The substance is ignited in a bulb- tube through which dried air or, in presence of oxidizable sub- stances, carbon dioxide is transmitted, and which is connected with a calcium chloride tube, by means of a dry, close-fitting cork. During the ignition, the posterior end of the bulb-tube is, by means of a small lamp, kept sufficiently hot to prevent the con- densation of water in it, care being taken, however, to guard against burning the cork. The loss of weight of the tube gives the amount of the water -f- the carbonic acid ; the increase of weight gained by the calcium chloride tube gives the amount of the water, and the difference accordingly that of the carbonic acid. A somewhat * Annal. d. Chem. u. Pharm. 158, 112; Zeitschr. f. anal. Chem. 10, 861. 408 DETERMINATION. [ 139, wide glass tube may also be put in the place of the bulb-tube, and the substance introduced into it in a little boat, which is weighed before and after the operation. c. Separation from all fixed Basic Radicals, without exception, in Anhydrous Carbonates. Fuse vitrified borax in a weighed platinum crucible, allow to cool in the desiccator, weigh, then transfer the well-dried substance to the crucible and weigh again. The weights of both carbonate and borax are thus ascertained. They should be in about the pro- portion of 1 : 4-. Heat is then applied, which is gradually increased to redness, and maintained at this temperature until the contents of the crucible are in a state of calm fusion. The crucible is now allowed to cool, and weighed. The loss of weight is carbonic acid. The results are very accurate (SCHAFFGOTSCH). I must add that borax-glass may be kept in a state of fusion at a red heat for J to \ an hour without the occurrence of any vola- tilization, but that at a white heat (by igniting over the gas-bel- lows), even in a few minutes, it suffers a decided loss.* A few bubbles of carbonic acid remaining in the fusing mass are without any influence on the result. Instead of vitrilied borax fused potassium dichromate may be used, in the proportion of 5 to 1 of the carbonate (H. RosEf). The heat applied in this case must be low, and great caution must be used, or the dichromate will lose weight of itself.;): The carbonic acid may be expelled from alkali carbonates, by strong ignition with ignited silica (H. EOSE). d. Separation by decomposition with Acids. (Estimation from the loss of weight.) tv. Carbonates of metals which form Soluble Salts with Sulphuric Acid. The process is conducted in the apparatus illustrated by fig. 58. The size of the flask depends upon the capacity of the balance. B may be smaller than A. The tube a is closed at b with a little wax ball, or a small piece of india-rubber tube, stopped with half an inch of rod ; the other end of the tube a is open, as are also both ends of c and d. The flask B is nearly half filled with concentrated sulphuric acid, free from oxides of nitrogen and sulphurous acid. * Zeitschr. f. anal. Chem. 1, 65. f Pogg. Annal. 116, 131. \ Zeitschr. f. anal. Chem, 1, 188. Pogg. Annal. 116, 686. 139.J CAKBONIC ACIB. 409- The tubes must fit air-tight in the corks, and the latter equally *o in the flasks. The weighed substance is put into A ; this flask is then filled about one third with water, the cork properly inserted, and the apparatus tared on the balance. A few bubbles of air are now sucked out of d, by means of an india-rubber tube. This serves to rarefy the air in A also, and causes the sulphuric acid in B to ascend in the tube c. The latter is watched for some time, to ascertain whether the column of sulphuric acid in it remains stationary, which is a proof that the apparatus is air-tight. Air is then again sucked out of d, which causes a portion of the sulphuric acid to flow over into A. The carbonate in the latter flask is decomposed by the sulphuric acid, and the liberated carbonic acid, completely dried in its passage through the sulphuric acid in B 9 escapes through d. When the evolu- tion of the gas slackens a fresh portion of sulphuric acid is made to pass over into A. by renewed suction through d ; the operation being repeated until the whole of the carbonate is decom- posed. A more vigorous suction is now applied, to make a large amount of sulphuric acid pass over into A, whereby the contents of that flask are considerably heated ; when the evolu- tion of gas bubbles has completely ., . -, -, FIG. 58. ceased, the stopper on a is opened, and suction applied to d, until the air sucked out tastes no longer of carbonic acid.* When the apparatus is quite cold it is replaced upon the balance, and the equilibrium restored by additional weights. The sum of the weights so added indicates the amount of carbonic acid originally present in the substance. If the flasks A and B are selected of small size, the apparatus may be so constructed that, together with the contents, it need not weigh above TO grammes, admitting thus of being weighed on a delicate balance. The results obtained by the use of this apparatus, first suggested by WILL and myself, are very accurate, provided the quantity of the carbonic acid be not too trifling. Various * In accurate experiments, it is advisable to connect the end b of the tube a with a calcium chloride tube during the process of suction, and to use an aspira- tor or hydraulic air-pump instead of the mouth. 410 DETERMINATION". [ 139. modifications of the apparatus have been proposed, principally in order to make it lighter. If sulphites or sulphides are present, together with the carbon- ates, their injurious influence is best obviated by adding to the carbonate solution of normal potassium chromate in more than sufficient quantity to effect their oxidation. If chlorides are pres- ent, in order to prevent the evolution of hydrochloric acid, add to the evolution flask a sufficient quantity of silver sulphate in solu- tion, or connect the exit tube d with a small prepared U-tube, which is, of course, first tared with the apparatus, and afterwards weighed with it. This U-tube is prepared in accordance with the happy proposal of STOLBA by filling with fragments of pumice which have been boiled with an excess of concentrated solution of cupric sulphate, till the air has been expelled, and then dried and heated to complete dehydration of the copper salt. If the U-tube is only 8 cm. high and has a bore of 1 cm., it answers the purpose very well. The outer end is provided with a perforated cork and short glass tube. We apply suction to this by means of a flexible tube, instead of to d. ft. After S. W. JOHNSON.* All Carbonates which dis- solve freely in cold dilute acid. The apparatus may consist of a light flask or bottle with wide mouth which is closed by a soft rubber stopper, through which there passes, on the one hand, a calcium chloride tube, the lower bulb of which contains cotton, and, on the other, the neck of a vessel which contains the dilute acid. This acid reservoir is so constructed that on suitably inclining it, its contents will flow freely into the flask. For this purpose the tube connecting with the latter has an internal diameter of seven millimetres, and its extremity is cut off obliquely ; at its other end, the acid reservoir terminates in an upturned narrow tube. This and the upper termination of the calcium chloride tube are chosen of such diame- ter that they fit quite snugly into short, narrow, and thick-walled rubber connectors which are again provided with glass-rod stop- pers; all these joints must be gas-tight. In figure 59 the apparatus is represented in one third its proper dimensions. The weighed substance, in case of calcium carbonate, e.g., is placed at the bottom of the flask, most conveniently in the * American Journal of Science and Arts, vol. xlv. iii., July, 1869. CARBONIC ACID. 411 form of small fragments. The acid vessel is nearly filled witli hydrochloric acid of sp. gr. 1-1. It and the calcium chloride tube are tightly adjusted to the neck of the flask, and the glass-rod stoppers being removed, the apparatus is connected at with a self-regulat- ing generator of washed carbonic acid, and a rather rapid stream of the gas is transmitted through the apparatus for 15 minutes, or until the liquid is saturated and the air is thoroughly displaced. Then the opening at d is stopped and afterward the apparatus is disconnected with the carbonic acid generator and stopped at c. During these as well as the subsequent operations, the apparatus must be so handled that its temperature shall not change. It is immediately weighed. When removed from the balance, loosen the stopper at d, and, holding the flask by a wooden clamp, incline it so that the acid may flow over upon the carbonate. The decom- position should proceed slowly, so that the escaping gas may be thoroughly dried. As soon as solution of the carbonate is complete, replace the stopper at d, and weigh again. Should there be any leak in the apparatus the fact is made evident by a slow but steady loss of weight, when it is brought upon the balance. If all the joints are sufficiently tight, the weight remains the same for at least fifteen minutes. When properly executed the process gives extremely accurate results ; a slight change of temperature or of atmospheric pressure be- tween the two weighings of course greatly im- pairs the results or renders them worthless. Since the apparatus usually rises a little in temperature during the solution of the carbon- ate, it is better, as soon as the substance is de- composed, to stopper the CaCl, tube and let the whole stand fifteen minutes, then to connect as before with the gas-generator and pass dried CO a for a minute, and finally to stopper again and bring upon the balance. In seven analyses of pure calcite in quantities ranging from O5 to 0'9 grm., the follow- ing percentages of carbonic acid were obtained, viz. : 44*07, 44-07, 43-98, 44-01, 44-04, 44-11, 44-16 ; calculation requires 44-00. In case of alkali-carbonates which absorb carbonic acid gas, it is necessary to modify the apparatus. Instead of the light flask, FIG. 59. 412 DETERMINATION. [ 139. we may employ a small bottle of thick glass and wider mouth, and a thrice perforated rubber stopper. Through the third orifice pass a narrow tube 3 to 4 inches long enlarged below to a small bulb to contain the carbonate. This bulb must be so thin that on pushing down the tube within the bottle it shall be easily crushed to pieces against the bottom of the latter. The carbonate is weighed into the bulb-tube, the latter is wiped clean down to the bulb, corked and fixed in the stopper. The apparatus is filled as before with CO 2 and weighed. Then the bulb is broken and the process fin- ished as before described. In three estimations on sodium carbo- nate, 4:1-54, 4:1-64, and 41*58 percent, of CO 3 were obtained. Cal- culation requires 41 '51 per cent.] e. All Carbonates without exception (Determination by absorp- tion and weighing of CO 2 ), H. ROSE. The flask for decomposing the carbonate should be small (150 c.c.), in order to facilitate subsequent removal of carbonic acid by aspiration, unless the substance froths strongly during its decom- position, in which case a larger flask must be used. The end of the funnel tube, after it is inserted in the rubber stopper which is fitted to the flask, is drawn to a less diameter and bent upwards in the form of a hook, to prevent the entrance of gas-bubbles. Above the stop-cock its internal diameter should not be so small as to pre- vent water when poured in from filling it, and this portion should be so long that the pressure of the liquid filling it will suffice to force gas through the apparatus. A piece of glass tube bent at a right angle is fitted to the funnel by means of a piece of rubber tube slipped over it. The nearly horizontal glass tube (about 0*7 metre long) is of thin glass, and of a diameter not less than 12 millimetres. It is inclined to such extent that water condensing in it may flow back. The upper half is filled with granulated dried calcium chloride, secured in place by a little cotton or asbestos at each end. In the end of the large tube a small tube is fitted by means of a rubber stopper, and to this is joined by a' rubber tube the potash appara- tus and soda-lime tube (weighable either jointly or separately) charged with absorbents, as described 174, 175. The flask is removed to receive the weighed substance, and replaced without disturbing the position of the rest of the apparatus. It can now be ascertained whether the apparatus will leak gas by forcing a little air (free from carbonic acid) through the funnel tube, closing 139.] CARBONIC ACID. 413 the stop-cock, and observing whether the unequal height of liquid in the two limbs of the potash apparatus remains for a few minutes. Introduce a little water through the funnel tube, and next acid slowly by turning the stop-cock until evolution of CO 2 ceases. The small right-angled tube, to which is attached a large tube filled with fragments of potash (see 175), is now inserted in the glass funnel, and a slow current of air (1 bubble per second) is drawn through the apparatus by means of an aspirator (fig. 62) connected with the soda-lime tube. The aspirator should not be connected directly to the soda-lime tube, but to a calcium-chloride tube, which ought to be connected with the latter during the whole operation. As soon as the current of air is established, Fig. 60. apply the smallest possible flame of a Bunsen lamp, best main- tained constant by capping the burner with wire gauze until the fluid just boils. Keep up the gentle boiling a few minutes until water condenses in the tube, but not until condensed drops appear quite up to the calcium chloride. Remove then the lamp, and aspirate a while longer somewhat faster. The volume of air neces- sary to remove the carbonic acid depends upon the size of the decomposing flask. When the operation is completed, disconnect the absorbing apparatus, close the ends with caps of rubber tubing, and weigh after lapse of half an hour. For liberating the carbonic acid, sulphuric acid (the concen- trated diluted with 4 or 5 times its volume of water) is best 414 DETERMINATION. [ 139. adapted, provided it readily decomposes the substance without formation of insoluble sulphates. "When there are objections to using sulphuric acid, dilute hydro- chloric acid (containing about 10 per cent) may be used, or more rarely nitric acid. Nitric acid cannot be used when substances are present which cause its decomposition ; e.g., ferrous salts and sul- phides. When sulphuric acid is used, the evolution of H a S from sul- Fig. 62. phides, if present, may be prevented by adding first a solution of chromic acid or mercuric chloride. If sulphites are present, use chromic acid or potassium chromate. When hydrochloric acid is employed, the disturbing influence of compounds which cause evo- lution of chlorine may be prevented by allowing some concentrated solution of stannous chloride to run into the flask before addition of the acid. When hydrochloric acid is used, or even sulphuric in the presence of chlorides, it is best to guard against the possibility of carrying HC1 gas into the potash apparatus by substituting STOLBA'S preparation of anhydrous copper sulphate and pumice- 139.] CARBONIC ACID. 415 stone (see page 410) for that portion of the calcium chloride which fills 10-15 cm. of the end of the tube. A modification* of the above-described apparatus, possessing some obvious advantages, is shown by fig. 61. In place of the empty part of the long glass tube shown in fig. 60 is substituted a smaller strong tube, provided with a cooling apparatus through which water circulates. This is connected by a piece of close- fitting rubber tube with the remaining part d. Some suitable form of apparatus for absorbing CO, must, of course, be attached to d in the manner shown by fig. 60. The calcium-chloride tube, used to prevent moist air from entering the absorbing apparatus, is conveniently supported by attaching it to the aspirator (fig. 62). The aspirator may be connected with the apparatus from the beginning to the end of the operation, with its stop-cock so adjusted that water flows from it drop by drop. In conducting the operation, a little variation from the before described manipulation is admissible on ac- count of the presence of the condensing ap- paratus. After enough acid has been ad- mitted to effect decomposition, the stop-cock of a is closed, a little liquid still being al- lowed to remain above it. Heat is then applied as before directed, but continued longer until the CO 2 is almost or quite ex- pelled from the flask by steam. This point 7~ ~ is indicated by almost, or nearly, entire ces- sation of dropping of water from the aspi- rator. Diminish now the heat, and immediately after open the stop-cock of a and let air (free from CO a ) enter and replace the condensing steam. Boil again to expel the air which has entered, after which a small volume of air drawn through the apparatus by the aspirator will ensure the bringing of all the CO, into the absoib- ing apparatus. f. Estimation ~by Measuring the Gas. This process is applicable in the case of all salts which are * Devised by H. L. WELLS, of the Sheffield Laboratory. 416 DETERMINATION. [ 139. TABLE OF THE WEIGHT OF A CUBIC In Milligrammes, from 720 to 770 mm. ofpress- MlLLIMETRES. 720 722 724 726 728 730 732 734 736 738 740 742 744 IQo 1.77446 ! 1.77945'1.78445 1.78944 1.79443 1.79942 1.80441 1.80941 1.81440 1.81940 1.82438 1.82937 1.83437 11* 1.76668 1.77165 1.77662 1.78160 1.78657 1.79155 1.79652 1.80149 1.80647 1.81144 1.81642 1.82139 1.82636 12 1.75881 1.76377 1.76873 1.77368 1.77864 1.78359 1.78855 1.79351 1.79846 1.80342 1.80838 1.81333 1.81829 13 1.75092 1.75587 1.76081 1.76576 1.77070 1.77565 1.78059 1.78554 1.79048 1.79543 1.80037 1.80532 1.81026 14; 1.74301 1.74795 1.75288 1.75781 1.76275 1.76768 1.77261 1.77754 1.78248 1.78741 1.79234 1.79728 1.80221 150 1 1.73502 1.73993 1.74484 1.74974 1.75465 1.75955 1.76446 1.76937 1.77427 1.77918 1.78408 1.78899 1.79390 16 1.72699 1.73188 1.73677 1.74166 1.74655 1.75144 1.75633 1.76122 1.76611 1.77100 1.77590 1.78078 1.78567 17 1.71888 1.72376 1.72862 1.73349 1.73836 1.74322 1.74809 1.75296 1.75783 1.76269 1.76756 1.77243 1.77729 18 1.71069 1.71554 1.72040 1.72525 1.73011 1.73497 1.73982 1.74468 1.74953 1.75439 1.75925 1.76410 1.76896 j 19 1.70239 1.70723 1.71207 1.71691 1.72175 1.72659 1.73143 1.73627 1.74111 1.74595 1.75078 1.75562 1.76046 20 1.69412 1.69894 1.70377 1.70859 1.71341 1.71823 1.72305 1.72788 1.73270 1.73725 1.74234 1.74716 1.75199 21 1.68571 11.69051 1.69532 1.70012 1.70493 1.70974 1.71454 1.71935 1.72415 1.72896 1.73377 1.73857 1.74338 22 1.67722 1.68201 jl.68680 1.69151 1.69638 1.70117 1.70596 1.71075 1.71554 1.72033 1.72512 1.72991 1.73470 23 1.66862 1.67340 1.67817 1.68294 1.68772 1.69249 1.69727 1.70204 1.70681 1.71159 1.71636 1.72114 1.72591 24 1.65994,1.66470 1.66945 1.67421 1.67897 1.68372 1.68848 1.69324 1.69799 1.70275 1.70751 1.71227 1.71702 25 1.65113 1.65587I1.66081 1.66535 1.67009 1.67484 1.67958 1.68432 1.68906 1.69380 1.69854 1.70329 1.70803 720 722 724 726 728 730 732 734 736 738 740 742 744 MILLIMETRES. 139.] CAEBONIC ACID. 417 CENTIMETRE OF CARBONIC ACID. ure of mercury, and from 10 to 25 Cent. MILLIMETRES. 746 748' 750 752 754 756 ! 758 760 762 764 766 768 770 i 1 i j i 1.83936 1.84435 1.84934 1.85433 1.85933 1.86432 1.86931 1.87430 1.87930 1.884291.88928 1.894271.89926 10 . 1.831341.83631 1.84129 1.84626 1.85123 1.85621 1.86118 1.86616 1.87113 1.87610 1.88108 1.886051.89103 11 1.82324 1.82820 1.833151.83811 1.84307 1.84802 1.85298 1.85793 1.86289 1.86785 1.87280 1.87776 1.88271 12 1.81521 1.82015 1.825101.83004 1.83499 1.83993 1.84488 1.84982 1.85477 1.85971 1.86466 1.86960 1.87455 13 1.80714 1.81208 1.81701 1.82194 1.82687 1.83181 1.83674 1.84167 1.84661 1.85154 1.85647 1.86141 1.86634 14 1.79880 1.80371 1.80861 1.81352 1.81843 1.82333 1.82824 1.83314 1.83805 1.84296 1.84786 1.852771.85767 15 1.79056 1.79545 1.800341.80523 1.81012 1.81501 1.81990 1.82479 1.82968 1.83457 1.83946 1.84435 1.84924 16 1.78216 1.78703 1.79189 1.79676 1.80163 1.80650 1.81136 1.81623 1.82110 1.82596 1.83083 1.83570 1.&4056 170 1.77381 1.77867 1.783531.78838 1.79324 1.79809 1.80295 1.80781 1.81266 1.81752 1.82337 1.827231.83209 18 o 1.76530 1.77014 1.77498 1.77982 1.78466 1.78950 1.79434 1.79917 1.80401 1.80885 1.81369 1.81853 1.82337 19 1.75681 1.76113 1.766451.77127 1.77610 1.78092 1.78574 1.79056 1.79538 1.80021 1.80503 1.809851.81467 20 1.74818 I 1.75299 1.75780 1.76260 1.76741 1.77221 1.77702 1.78183 1.78663 1.79144 1.79624 1.80105 1.80586 21 1.73949 1.74428 1.74907 1.75386 1.75865 1.76344 1.76823 1.77302 1.77781 1.78260 1.78739 1.79218 1.79697 ft- 1.73068 1.73546 1.74023 1.74501 1.74978 1.75455 1.75933 1.76410 1.76888 1.77365 1.77842 1.78320 1.78797 23 1.72178 1.72654 1.73129 1.73605 1.74081 1.74556 1.75032 1.75508 1.75984 1.76459 1.76935 1.77411 1.77886 24 1.71277 1.71751 1.72225 1.72699 1.73173 1.73648 1.74122 1.74596 1.75070 1.75544 1.76018 1.76492 1.76967 25 746 748 750 752 754 756 758 760 762 764 766 768 770 MILLIMETRES. 418 DETERMINATION. [ 139. 8 5 8 S 8 $ 10 * 10 1 s JU CO ^ id 8 S 10 OS j^. 10' 8 1 00 22 T-H ^^ *' 8 1 00 i$ id 00 10' 8 CO s w . * 2 ^f id E e 10 o co" CO *~ *" 3 8 3 co 2 10 10 J> ^ 10 $> 1O S o 8 3 s o 1O CD OS id 8 5 8 3 00 CO 03 10 10* S -8 10' s 2 s s CO 8 3 ^ S OT id g 10' /v CO 8 5 CO c3 s id s s 10 id 3 i 1 ^ O5 id s a. CO 8 1 g 1 8 1 OS ? 8- co' 8 1 2 w id 8 3 8 1 00 "3 s . CO c5 10 S8 8. 10 8 1 8 S 00 a 3 s s id S 8 10 CO 00 10 CO OJ 8' 1 8. 10 g S 10 CO ^ id 10 ^ 8 1 $ 8 id JO | " id s 1 TH S t- ^J CO, id 50 id id CO CO """J 8 5 id CO CO * 10 s i y Hydrochloric or Nitric Acid, on digestion in open vessels. * Zcitschr. f. anal. Chem. 4, 163. 420 DETERMINATION. [ 140. To this class belong the silicates soluble in water, as well as many of the insoluble silicates, as, for instance, nearly all zeolites. Several minerals not decomposable of themselves by acids, become so by persistent ignition in a state of fine powder (F. MOHK*). If the ignition is too strong, particles of alkali may be lost. The substance is very finely powdered, f dried at 1 00, and put into a platinum or porcelain dish (in the case of silicates whose solu- tion might be attended with disengagement of chlorine, platinum cannot be used) ; a little water is then added, and the powder mixed to a uniform paste. Moderately concentrated hydrochloric acid, or if the substance contains lead or silver nitric acid, is now added, and the mixture digested at a very gentle heat, with con- stant stirring, until the substance is completely decomposed, in other terms, until the glass rod, which is rounded at the end, encounters no more gritty powder, and the stirring proceeds smoothly without the least grating. The silicates of this class do not all comport themselves in the same manner in this process, but show some differences ; thus most of them form a bulky gelatinous mass, whilst in the case of others the silicic acid separates as a light pulverulent precipitate ; again, many of them are decomposed readily and rapidly, whilst others require protracted digestion. When the decomposition is effected, the mixture is evaporated to dryness on the water-bath, and the residue heated, with frequent stirring, until all the small lumps have crumbled to pieces, and the whole mass is thoroughly dry, and until no more acid fumes escape. It is always the safest way to conduct the drying on the water-bath. Occasionally it is well to moisten the dry mass with water and evap- orate again. In cases where it appears desirable to accelerate the desiccation by the application of a stronger heat, an air-bath may be had recourse to ; which may be constructed in a simple way, by suspending the dish containing the substance, with the aid of wire, in a somewhat larger dish of silver or iron, in a manner to leave everywhere between the two dishes a small space of uniform width. Direct heating over the lamp is not advisable, as in the most strongly heated parts the silicic acid is liable to unite again with * Zeitschr. f. anal. Chem. 7, 293. t Very hard silicates cannot be powdered in an agate mortar without taking up silica; these must, therefore, be powdered in a steel mortar, sifted, and freed from particles of steel with the magnet. 140.] SILICIC ACID. 421 the separated bases to compounds which are not decomposed, or only imperfectly, by hydrochloric acid. When the mass is cold, it is brought to a state of semi-fluidity by thoroughly moistening it with hydrochloric acid ; after which it is allowed to stand for half an hour, then warmed on a water- bath, diluted with hot water, stirred, allowed to deposit, and the fluid decanted on to a filter ; the residuary silicic acid is again stirred with hydrochloric acid, warmed, diluted, and the fluid once more decanted ; after a third repetition of the same operation, the precipitate also is transferred to the filter, thoroughly washed with hot water, well dried, and ignited at last as strongly as possible, as directed in 52. For the properties of the residue, see 93, 9. The results are accurate. The basic metals, which are in the filtrate as chlorides, are determined by the methods given above. Devia- tions from the instructions here given are likely to entail loss of substance ; thus, for instance, if the mass is not thoroughly dried, a not inconsiderable portion of the silicic acid passes into the solu- tion, whereas, if the instructions are strictly complied with, only traces of the acid are dissolved ; in accurate analyses, however, even such minute traces must not be neglected, but should be separated from the metals precipitated from the solution. The separation may, as a rule, be readily effected by dissolving them, after ignition and weighing, in hydrochloric or sulphuric acid, by long digestion in the heat, the traces of silicic acid being left undissolved. Some- times it is better to fuse the metallic oxides with potassium disul- phate, or to reduce them to the metallic state by ignition in hydro- gen, and then to treat with hydrochloric acid. Again, if the silicic acid is not thoroughly dried previous to ignition, the aqueous vapor disengaged upon the rapid application of a strong heat may carry away particles of the light and loose silica. The silicic acid may be tested as follows : This testing must on no account be omitted if the silica has been separated in a pulveru- lent and not in a gelatinous form. Heat a portion on a water-bath with moderately concentrated solution of sodium carbonate for an hour in a platinum or silver dish ; with less advantage in a porce- lain dish. EGGERTZ"* recommends, for 1 grm. silicic acid, 6 c.c. of a saturated solution of sodium carbonate and 12 c.c. of water. Pure silica would dissolve. If a residue remains, pour off the clear * Zeitschr. f . anal. Chem. 7, 502. 422 DETERMINATION. [ 140. fluid and heat again with a small quantity of sodium carbonate. If a residue still remains, weigh the rest of the impure silica and treat it according to &, to estimate the amount of impurity. If you have pure hydrofluoric acid, you may also test the silicic acid in a very easy manner, by treating it with this acid and a few drops of sulphuric acid in a platinum dish ; upon the evaporation of the solution, the silicic acid, if pure, will volatilize completely (as fluoride of silicon). If a residue remains, moisten this once more with hydrofluoric acid, add a few drops of sulphuric acid, evaporate, arid ignite ; the residue consists of the sulphates of the metals retained by the silicic acid, as well as any titanic acid that was present (BEKZELIUS). Ammonium fluoride may be used instead of hydrofluoric acid. b. Compounds which are not decomposed "by Hydrochloric or Nitric Acid, on digestion in open vessels. a. Decomposition by fusion with Alkali Carbonate. Reduce the substance to an impalpable powder, by triturat'ion and, if necessary, sifting ( 25) ; transfer to a platinum crucible, and mix with about 4 times the weight of pure anhydrous sodium carbonate or sodium and potassium carbonate, with the aid of a rounded glass rod ; wipe the rod against a small portion of sodium carbonate on a card, and transfer this also from the card to the crucible. Cover the latter well, and heat, according to size, over a gas or spirit-lamp with double draught, or a blast gas-lamp ; or insert in a Hessian crucible, compactly filled up w r ith calcined magnesia, and heat in a charcoal fire. Apply at first a moderate heat for some time to make the mass simply agglutinate ; the carbonic acid will, in that case, escape from the porous mass with ease and unattended with spirting. Increase the heat afterwards, finally to a very high degree, and terminate the operation only when the mass appears in a state of calm fusion, and gives no more bubbles. The platinum crucible in which the fusion is conducted must not be too small ; in fact, the mixture should only half fill it. The larger the crucible, the less risk of loss of substance. As it is of importance to watch the progress of the operation, the lid must be easily removable ; a concave cover, simply lying on the top, is there- fore preferable to an overlapping lid. If the process is conducted over the spirit or simple gas-lamp, the mixed sodium and potas- 140.J SILICIC ACID. 423 siurn carbonates are preferable to sodium carbonate, as they fuse much more readily than the latter. In heating over a lamp, the crucible should always be supported on a triangle of platinum wire, with the opening just sufficiently wide to allow the crucible to drop into it fully one third, yet to retain it firmly, even with the wire at an intense red heat. When conducting the process over a spirit-lamp with double draught, or over a simple gas-lamp, it is also advisable, towards the end of the operation, when the heat is to be raised to the highest degree, to put a chimney over the cruci- ble, with the lower border resting on the ends of the iron triangle which supports the platinum triangle ; this chimney should be about 12 or 14 cm. high, and the upper opening measure about 4 cm. in diameter. The little clay chimneys recommended by O. L. ERDMAXX are still more serviceable (fig. 21, p. 24, " Qual. Anal."). When the fusion is ended, the red-hot crucible is removed with tongs, and placed on a cold, thick, clean iron plate, on which it will rapidly COQ! ; it is then generally easy to detach the fused cake in one piece. The cake (or the crucible with its contents) is put into a beaker, from 10 to 15 times the quantity of water poured over it, and heat applied for half an hour, then hydrochloric acid is gradually added, or, under certain circumstances, nitric acid; the beaker is kept covered with a glass plate, or, which is much better, with a large watch-glass or porcelain dish, perfectly clean outside, to prevent the loss of the drops of fluid which the escaping carbonic acid car- ries along with it ; the drops thus intercepted by the cover are afterwards rinsed into the beaker. The crucible is also rinsed with water mixed with dilute acid, and the solution obtained added to the fluid in the beaker. The solution is promoted by the application of a gentle heat, which is continued for some time after this is effected to insure the complete expulsion of the carbonic acid ; since otherwise some loss of substance might be incurred, in the subsequent process of evapo- ration, by spirting caused by the escape of that gas. If in the pro- cess of treating the fused mass with hydrochloric acid, a saline powder subsides (sodium or potassium chloride), this is a sign that more water is required. If the decomposition of the mineral has succeeded to the full extent, the hydrochloric acid solution is either perfectly clear, or light flakes of silicic acid only float in it. But if a heavy powder 424 DETEKMHSTATION. [ 140. subsides, which feels gritty under the glass rod, this consists of undecomposed mineral. The cause of such imperfect decomposi- tion is generally to be ascribed to imperfect pulverization. In such cases the undecomposed portion may be fused once more with alkali carbonate ; the better way, however, is to repeat the process with a fresh portion of mineral more finely pulverized. The hydrochloric or nitric acid solution obtained is poured, together with the precipitate of silicic acid, which is usually floating- in it, into a porcelain or, better, into a platinum dish, and treated as directed in II., a. That the fluid may not be too much diluted, the beaker should be rinsed only once, or not at all, and the few remaining drops of solution dried in it ; the trifling residue thus obtained is treated in the same way as the residue left in the evapo- rating basin. This is the method most commonly employed to effect the decomposition of silicates that are undecomposable by acids ; that it cannot be used to determine alkalies in silicates is self-evident. . Decomposition ly means of Hydrofluoric Acid. aa. By Aqueous Hydrofluoric Acid. The silicate should be finely pulverized, dried at 100 (in some cases ignition is advisable*). It is mixed, in a platinum dish, with rather concentrated, slightly fuming hydrofluoric acid, the acid being added gradually, and the mixture stirred with a thick plati- num wire. The mixture, which has the consistence of a thin paste, is digested some time on a water-bath at a gentle heat, and pure concentrated sulphuric acid, diluted with an equal quantity of water, is then added, drop by drop, in more than sufficent quantity to convert all the basic metals present into sulphates. The mixture is now evaporated on the water-bath, during which operation sili- con fluoride gas and hydrofluoric acid gas are continually volatiliz- ing ; then it is finally exposed to a stronger heat at some height above the lamp, until the excess of sulphuric acid is almost completely expelled. The mass, when cold, is thoroughly moistened with con- centrated hydrochloric acid, and allowed to stand at rest for one hour; water is then added, and a gentle heat applied. If the decomposition has fully succeeded, the whole must dissolve to a clear fluid. If an undissolved residue is left, the mixture is heated * Many minerals are much more readily decomposed by hydrofluoric acid also, if they are previously ignited in a state of fine division (HERMANN, RAM- MELSBERG, FR. HOUR, Zeitschr. f. anal. Chem. 7, 291). 140.] SILICIC ACID. 425 for some time on the water-bath, then allowed to deposit, the clear supernatant fluid decanted as far as practicable, the residue dried, and then treated again with hydrofluoric acid and sulphuric acid, and, lastly, with hydrochloric acid, which will now effect complete solution, provided the analyzed substance was very finely pulver- ized, and free from barium, strontium (and lead). The solution is added to the first. The basic metals in the solution (which con- tains them as sulphates, and contains also free hydrochloric acid) are determined by the methods which will be found in Section Y. This method, which is certainly one of the best to effect the decomposition of silicates, was proposed by BERZELIUS. It has been but little used hitherto, because we did not know how to pre- pare hydrofluoric acid, except with the aid of a distilling appa- ratus of platinum, or, at least, with a platinum head ; nor to keep it, except in platinum vessels. These difficulties can now be con- sidered as overcome, comp. 58, 2. Never omit testing the acid before using it. The hydrofluoric acid may also be employed in combination with hydrochloric acid ; thus 1 grm. of finely elutriated felspar, mixed with 40 c.c. water, 7 c.c. hydrochloric acid of 25^ and 3J c.c. hydrofluoric acid, and heated to near the boiling point, dissolves completely in three minutes. 4 c.c. sulphuric acid are then added, the barium sulphate which may separate is filtered off, and the filtrate evaporated till no more hydrofluoric acid escapes (AL. MlTSCHERLICH*). The execution of the method requires the greatest possible care, both the liquid and the gaseous hydrofluoric acid being most injurious substances. The treatment of the silicate with the acid and the evaporation must be conducted in the open air, otherwise the windows and all glass apparatus will be attacked. As the silicic acid is in this method simply inferred from the loss,+ a combination with method a is often resorted to. bb. By Ammonium Fluoride. Mix the very finely powdered substance in a platinum dish with four times its weight of ammonium fluoride, moisten well with concentrated sulphuric acid, heat on the water-bath till the * Journ. f. prakt. Chem. 81, 108. f The silicon escaping in the form of fluoride may sometimes be determined directly, by the method of STORY MASKELYNE (Zeitschr. f. anal. Chem. 9, 380), which, however, requires a platinum retort of peculiar construction. 426 DETERMINATION. [ 140. evolution of silicon fluoride and hydrofluoric acid slackens, add more sulphuric acid, heat again, finally somewhat more strongly till the greater part of the sulphuric acid has escaped, and treat the residue according to aa (L. v. BABO, J. POTYKA, R. HOFFMANN*). H. Kosfif first warms the silicate gently with seven times its amount of the fluoride and some water, then heats gradually to redness till no more fumes escape, and finally treats with sulphuric .acid. cc. By Fluoride of Hydrogen and Potassium, dec. In silicates, which more or less resist the action of hydrofluoric acid, such as zircon and beryl, the basic metals with the exception of the alkalies may be determined by fusing with fluoride of hydrogen and potassium (MARIGNAC, GiBBsf), or by mixing with 3 parts of sodium fluoride, adding 1 2 parts of potassium disulphate to the crucible, and then heating at first very gently, afterwards more strongly till the mass fuses calmly. The residue is dissolved in water or hydrochloric acid (CLAKKE). \y. .Decomposition by ignition with Calcium Carbonate and Ammonium Chloride. PROF. J. L. SMITH'S METHOD for separating alkalies. Mix 1 part of the pulverized silicate with 1 part of dry ammo- nium chloride, by gentle trituration in a smooth mortar, then add S parts of calcium carbonate (" Qual. Anal." p. 87) and mix inti- mately. Bring the mixture into a platinum crucible, rinsing the mortar with a little calcium carbonate. Warm the crucible gradu- ally over a small Bunsen burner until fumes of ammonium salts no longer appear, then heat with the flame of a Bunsen burner until the lower three-fourths only of the crucible are brought to a red heat. Keep this temperature constant from 40 to 60 minutes. The temperature desired is that which suffices to keep in state of fusion the calcium chloride formed by the reaction of ammonium chloride with calcium carbonate. The mass, however, does not become liquid since the fused calcium chloride is absorbed by the large quantity of calcium carbonate present. If the silicate is fused by application of too strong heat, disintegration of the mass at the end of the operation with water cannot be effected. More- over, too high a temperature causes volatilization of alkali chlo- * Zeitschr. f . anal. Chem. 6, 366. f Pogg. Annal. 108, 20. J Zeitschr. f. anal. Chem. 3, 399. Ib. 7, 463. 140.] SILICIC ACID. 427 rides. Certain silicates e.g., those which contain much ferrous i ron ma y f use when heated with the above mixture, even if no higher temperature is employed than is necessary to effect decom- position. If this occurs, it is better to repeat the ignition with a new portion of the silicate, using 8 to 10 parts of calcium carbo- nate. The mass contracts in volume during the ignition, and is usually easily detached from the crucible. Boil it in a covered porcelain dish, with 50-75 c.c. water, half an hour, replacing water lost by evaporation. Decant the solution from the residue upon a filter, boil the residue a few minutes with water, and decant again. If the residue is now all in a finely disintegrated state, it may be brought upon the filter and washed. But if, as is often the case, a portion remains coherent or in a coarsely granular state, it must be reduced to a fine state of division by trituration with a porcelain or agate pestle in the dish, and boiling with water again. By a few repetitions of the trituration, boiling and decanting, allowing the fine suspended portion to pass upon the filter each time, the whole can usually be transferred to the filter in properly disinte- grated condition in course of an hour. Xext wash until a few drops of the washings acidified with nitric acid give but a slight turbid- ity with silver nitrate. The filtrate now contains the alkalies of the silicate as chlorides together with calcium chloride and hydrox- ide. It is not advisable to concentrate this filtrate in a glass vessel, since it might take an appreciable quantity of sodium from the glass. Precipitate, therefore, the calcium at once with ammonium carbonate ; allow the precipitate to settle, and concentrate the supernatant solution in a porcelain (or platinum) dish, decanting it into the latter, portionwise if necessary, rinsing finally the precipi- tate into the porcelain dish. When the whole is thus reduced to about 30 c.c., add a little more ammonium carbonate and ammonia, heat and filter into a platinum (or porcelain) dish, evaporate to dry ness on a water-bath, expel ammonium chloride by ignition, dissolve the residual alkali chlorides in 3 to 5 c.c. of water. A little black or dark-brown flocculent matter usually remains undis- solved, while the solution may still contain traces of calcium. Add two or three drops of ammonium carbonate and ammonia, warm gently, and filter through a very small filter -into a weighable plati- num vessel. Evaporate to dryness on a water-bath, heat to in- cipient fusion of the alkali chlorides, and after cooling weigh. Prof. SMITH'S method is the most convenient of all methods 428 DETERMINATION. [ 141. for extracting alkalies from silicates, and is universally applicable, except perhaps in presence of boric acid. When carried out as here described, the results are sufficiently accurate in most cases. If, however, the silicate is rich in alkalies, a loss amounting to 0*1 or 0*2 per cent of the mineral is possible. If great accuracy is desired in such cases, a repetition of the whole process may be applied to the residue left by treatment of the ignited mass with water. It- need hardly be mentioned that unless care be takei) to use reagents perfectly free from soda and to avoid action of solutions on glass, an amount of soda may be introduced from these sources equal to 0*1 or 0'2 per cent of the silicate.] Second Group. CHLORINE BROMINE IODINE CYANOGEN SFLPHUB. 1. CHLORINE. I. Determination. Chlorine may be determined very accurately in the gravimetric as well as in the volumetric way.* a. Gravimetric Method. Determination as Silver Chloride. Solution of silver nitrate, mixed with some nitric acid, is added in excess to the solution of the chloride, the precipitated chloride is made to unite by heating and agitating, washed by decantation and nitration, dried, and ignited. The details of the process have been given in 115, 1, a. Care must be taken not to heat the solution mixed with nitric acid, before the nitrate of silver has been added in excess. As soon as the latter is present in excess, the silver chloride separates immediately and completely upon shaking or stirring, and the supernatant fluid becomes perfectly clear after standing a short time in a warm place. The determina- tion of chlorine by means of silver is therefore more readily effected than that of silver by means of hydrochloric acid. 1). Volumetric Methods. a. By Solution of Silver Nitrate. In 115, 5, we have seen how the silver in a fluid may be esti- mated by adding a standard solution of sodium chloride until no * For the acidimetric estimation of free hydrochloric acid, see 192. 141.] CHLORINE. 429 further precipitation ensues ; in the same way we may determine also, by means of a standard solution of silver, the amount of hydro- chloric acid in a fluid, or of chlorine in combination with a metal. PELOUZE has used this method for the determination of several atomic weights. LEVOL* proposed a modification which serves to indicate more readily the exact point of complete precipitation. To the fluid, which must be neutral, he added one tenth volume of a saturated solution of sodium phosphate. When the whole of the chlorine has been precipitated by the silver, the further addi- tion of the solution of silver produces a yellow precipitate which does not disappear upon shaking the vessel. FR. MOHR has since replaced, with the most complete success, the sodium phosphate by potassium chromate. This convenient and accurate method requires a perfectly neu- tral solution of silver nitrate of known value. The strength most convenient is, 1 litre = 1 at. Cl. I recommend the following method of preparation : Dissolve 18*80 to 18*85 grin, pure fused silver nitrate in 1100 c.c. water, and filter the solution if required ; the solution is purposely made too strong at first. Now weigh off exactly four portions of pure sodium chloride, each of *10 to *18 grin., one after another. The salt should be moderately ignited, not fused, powdered roughly while still warm, and introduced into a small dry tube, that can be well closed. The weighing off is per- formed by first weighing the filled tube, then shaking out into a dry beaker the quantity required, weighing again, dropping a second portion into beaker No. 2, weighing again, and so on. Each portion is dissolved in 20 to 30 c.c. water, and about 3 drops of a cold saturated solution of pure normal potassium chromate added. Fill a HOUR'S burette (in very accurate analysis an ERDMANN'S float should be used) with the silver solution, and run it slowly, with constant stirring, into the light yellow solution contained in one of the beakers. Each drop produces, where it falls, a red spot, which on stirring disappears, o \ving to the instant decomposition of the silver chromate with the sodium chloride. At last, how- ever, the slight red coloration remains. Now all chlorine has com- bined with silver, and a little silver chromate has been permanently formed. Read off the burette and reckon how much silver solu- * Journ. f. prakt. Chem. 60, 384. 430 DETERMINATION. [ 141. tion would have been required for -1 mol. sodium chloride, i.e., 5*85 grm. Suppose we have used to "110 sodium chloride 18*7 c.c. silver solution. 110 : 5-85 : : 18-7 : x; x = 994-5. E~ow, without throwing away the contents of the first beaker, make a second and third experiment in the same manner, of course always taking notice to regard the same shade of red as the sign of the end. The results of these are reckoned out in the same way as the first. Suppose they gave for 5'85 NaCl 995-0 and 993-0 respectively, we take the mean of the three numbers, which is 994*2, and we now know that we have only to take this number of c.c. of silver solution, and make it up to 1000 c.c. with 5*8 water, in order to obtain a solution of the required strength, i.e., 1000 c.c. -1 mol. JSTaCl. But if 994-2 requires 5-8 water, 1000 requires 5*83. Hence we fill a litre-flask (previously dried or rinsed with a small portion of the solution) up to the " holding " mark with the solution, add 5*83 c.c. water, insert a caoutchouc stopper, and shake. The solution must now be correct ; however, to make quite sure, we perform another experiment with it. To this end rinse the empty burette with the new solution, fill it with the same and test with the portion of salt in beaker No. 4. The c.c. used of silver solution must now, if multiplied by -00585, give exactly the weight of the salt. Being now in possession of a standard silver solution, and being practised in exactly hitting the transition from yellow to the shade of red, we are in the position to determine with precision chlorine in the form of hydrochloric acid or of a metallic chloride soluble in water. The fluid to be tested must be neutral free acids dissolve the silver chromate. The solution of the substance is therefore, if necessary, rendered neutral by addition of nitric acid or sodium carbonate (it should be rather alkaline than acid), about 3 drops of the solution of chromate added, and then silver from the burette, till the reddish coloration is just perceptible. The number of c.c. used has only to be multiplied by the atomic weight of chlorine or the mol. weight of the metallic chloride and divided by 10,000 to give the amount of these respectively present. If the operator fears he has added too much silver solution, i.e., if the red color is too strongly marked, he may add 1 c.c. of a solu- 141.] CHLORINE. 431 tion of sodium chloride containing 5*85 in a litre (and therefore corresponding to the silver solution), and then add the silver drop by drop again. Of course in this case 1 c.c. must be deducted from the amount of silver solution used. The results are very satisfactory. The fluid to be analyzed should be about the same volume as the solutions employed in standardizing the silver solution, and also about the same strength, otherwise the small quantity of silver which produces the colora- tion will not stand in the same proportion to the chlorine present. This small quantity of silver solution is extremely small, varying between -05 and '1 c.c.: the inaccuracy hereby arising even in the case of quantities of chlorine differing widely from that originally used in standardizing the silver solution is therefore almost incon- siderable. If the amount of silver solution necessary to impart the coloration always remained the same, we should have simply to deduct the amount in question with all experiments, in order to avoid this small inaccuracy entirely , since, however, the greater the quantity of silver chloride the more silver chromate is required for visible coloration, this method of proceeding would not increase the exactness of the results. ft. By Solution of Silver Nitrate and Iodide of Starch (PisAisn's method*). Add to the solution of the chloride, acidified with nitric acid, a slight excess of standard solution of silver nitrate, warm, and filter. Determine the excess of silver in the filtrate by means of solution of iodide of starch (see p. 295), and deduct this from the amount of silver solution used. The difference shows the quantity of silver which has combined with the chlorine; calculate from this the amount of the latter. Results satisfactory. Of these volumetric methods of estimating chlorine, the first deserves the preference in all ordinary cases. PISANI'S method (5, ft) is especially suited for the estimation of very minute quan- tities of chlorine, but is not applicable when as in nitre analyses- large quantities of alkaline nitrate are present (p. 290). II. Separation of Chlorine from the Metals, a. In Soluble Chlorides. The same method as in L, a. The metals in the filtrate are separated from the excess of the salt of silver by the methods * Annal. d. Mines, 10, 83 ; LTEBIG and KOPP'S Jahresbericht, 1856, 751. 432 DETERMINATION. [ 141. which will be found in Section Y. Chlorides soluble in water may also be completely decomposed by cold digestion with oxide or carbonate of silver. Silver chloride is obtained, while the metal combined with the chlorine is converted into oxide or carbonate and either remains in solution or falls down with the silver chlo- ride. Take care that no traces of oxide or carbonate of silver pass into the filtrate. Stannous chloride, mercuric chloride, platinic chloride, the chlorides of antimony, and the green chloride of chromium, form exceptions from the rule. ex. From stannic chloride, silver nitrate would precipitate, besides silver chloride, a compound of stannic oxide and silver oxide. To precipitate the tin, therefore, the solution is mixed with concentrated solution of ammonium nitrate, boiled, allowed to deposit, decanted, and filtered (compare 126, 1, Z>), and the chlo- rine in the filtrate is precipitated with solution of silver. LOWEN- THAL, the inventor of this method, has proved its accuracy.* ft. When mercuric chloride is precipitated with solution of silver nitrate, the silver chloride thrown down contains an admix- ture of mercury. The mercury is, therefore, first precipitated by hydrogen sulphide, and the chlorine in the filtrate determined as directed in 169. y. The chlorides of antimony are also decomposed in the man- ner described in ft. The separation of basic salt upon the addi- tion of water may be avoided by addition of tartaric acid. The antimonious sulphide should be tested for chlorine. #. Solution of silver fails to precipitate the whole of the chlo- rine from solution of the green chloride of chromium (PELIGOT). The chromium is, therefore, first precipitated with ammonia, the fluid filtered, and the chlorine in the filtrate precipitated as in I., a. f. From platinic chloride silver nitrate throws down a com- pound of platinous chloride and silver chloride (CoMAiLLEf). We may either ignite the platinic chloride in a current of hydrogen and. pass the hydrochloric acid produced into solution of silver (BON&DOBFF) ; or we may evaporate the solution with sodium car- bonate, fuse the residue in a platinum crucible and determine the chloride in the aqueous solution of the fusion. Or, thirdly, we may (after TOPSOE;};) digest the moderately dilute solution in the * Journ. f. prakt. Cliem. 66, 371. f Zeitschr. f. anal. Chem. 6, 121. t Zeitschr. f. anal. Chem. 9, 30. 141.] CHLORINE. 433 cold with zinc clippings till hydrogen ceases to escape, add ammo- nia in excess, heat on a water-bath till the fluid is fully decolorized, all the platinum being precipitated, and finally determine the chlo- rine in the filtrate. b. In Insoluble Chlorides. a. Chlorides soluble in Nitric Acid. Dissolve the chloride in nitric acid, without applying heat, and proceed as in I., a. fi. Chlorides insoluble in Nitric Acid (lead chloride, silver chloride, mercurous chloride). aa. Lead chloride is decomposed by digestion with alkali hydrogen carbonate and water. The process is exactly the same as for the decomposition of lead sulphate ( 132, II., b, /?). bb. Silver chloride is ignited in a porcelain crucible, with 3 parts of sodium and potassium carbonate, until the mass com- mences to agglutinate. Upon treating with water, the metallic silver is left undissolved ; the solution contains the alkali chloride, which is then treated as in I., a. Silver chloride may also be readily decomposed by long diges- tion with pure iron (reduced by hydrogen) and dilute sulphuric acid. Zinc may be used instead of iron, but it does not answer so well. The separated metallic silver may be washed, heated with dilute sulphuric acid, washed again and weighed ; it must after- wards be ascertained, however, whether it dissolves in nitric acid. The chlorine is determined in the chloride of iron or zinc as in I, a, cc. Mercurous chloride is decomposed by digestion with solu- tion of soda or potassa. The hydrochloric acid in the filtrate is determined as in I., a. The mercurous oxide is dissolved in nitric or nitrohydrochloric acid, and the mercury determined as directed in 117 or 118. c. The soluble chlorides of the metals of the fourth* fifth, and sixth groups may generally be decomposed also by hydrogen sul- phide or ammonium, sulphide. The chlorine in the filtrate is determined as in 169. It must not be omitted to test the pre- cipitated sulphides for chlorine. Several chlorides, cadmium chlo- ride for instance, give sulphides free from chlorine with ammonium sulphide, but not with hydrogen sulphide. d. In many metallic chlorides, for instance in those of the first and second groups, the chlorine may be determined also by evapo- 434 DETERMINATION. [ 142. rating with sulphuric acid, converting the metal thus into a sul- phate, which is then ignited and weighed as such ; the chlorine being calculated from the loss. This method is not applicable in the case of silver chloride and lead chloride, which are only imper- fectly and with difficulty decomposed by sulphuric acid ; nor in the case of mercuric chloride and stannic chloride, which sulphuric acid fails almost or altogether to decompose. Supplement. 142. DETERMINATION OF CHLORINE IN THE FREE STATE. Chlorine in the free state may be determined both in the volu- metric and in the gravimetric way. The volumetric methods, however, deserve the preference in most cases. They are very numerous. I shall only here adduce that one which is undoubtedly the most accurate and at the same time the most convenient.* 1. Volumetric Method. With Potassium Iodide (after BUNSEN). Bring the chlorine, in the gaseous form or in aqueous solution, into contact with an excess of solution of potassium iodide in water. Each at. chlorine liberates 1 at. iodine, which remains dissolved in the excess of potassium iodide. By determining the liberated iodine by means of sodium thiosulphate as in 146, you will accordingly learn the quantity of chlorine, and, in fact, with the greatest accuracy. If you have to determine the chlorine of chlorine water, measure a portion off with a pipette. So as to prevent any of the gas entering the mouth, connect the upper end of the pipette with a tube containing moist hydrate of potassa laid between cotton. When the pipette has been correctly filled allow its contents to flow, with stirring, into an excess of solution of potassium iodide (1 in 10). There is no difficulty about knowing whether the latter is sufficiently in excess, for if not, a black precipitate is formed. If the chlorine is evolved in the gaseous condition, you may employ either the apparatus given in 130, I., d, /?, or the following, which is especially suitable where the chlorine is not pure, but is mixed with other gases. * Compare " Chlorimetry" in the Special Part. 142.] CHLORINE. 435 a is a little flask, from which the chlorine is evolved by boiling the substance with hydrochloric acid, a small lump of magnesite being added ; it is connected with the tube, &, by means of a flexible tube. The latter must be free from sulphur should it contain sulphur it is well boiled with dilute potassa and then thoroughly washed. The thinner tube, , and c, which fit each other; weigh J and c together accurately. Put about 0'5 grm. pure dry iodine (prepared according to 65, 6) into , place it on an iron plate, heat gently, till dense fumes of iodine escape. Now cover it with I) and regu- late the heat so that the iodine may sublime entirely or almost entirely into o. Next remove b while still hot, and give it a gentle swing in the air to remove the still uncondensed iodine fumes and any traces of aqueous vapor, cover it with c, allow to cool under the desiccator, weigh and transfer the two watch-glasses together with the weighed iodine to a capacious beaker, containing a suffi- cient quantity of potassium iodide solution to dissolve the whole of the iodine to a clear fluid. Add water and then thiosulphate from a burette till the color is gone ; now add 3 or 4 c.c. of starch-paste and iodine solution (a, <*) from a second burette till a blue tinge just appears. Having read off both burettes, the following simple calculation will give you the iodine in the solution #, a : Suppose we had weighed off '150 grm. iodine, and used 29'5 c.c. thiosulphate and '3 c.c. iodine solution. * I filled several small well-stoppered bottles with some solution of iodine in potassium iodide, whose standard had been accurately determined, and placed them in a cellar. Even in the course of a few weeks the standard had altered. I now never rely on the strength of a solution of iodine, unless I have determined it shortly before. 146.] IODIDE. 447 From J, or, we know that 20 c.c. thiosulphate correspond to 20*2 c.c. iodine solution ; 29*5 c.c. therefore correspond to 29*8 c.c. Xow 29-5 c.c. thiosulphate correspond to '150 grm. iodine + -3 c.c. iodine solution. But 29-5 c.c. thiosulphate also correspond to 29*8 c.c. iodine solution. .*. -150 grm. iodine -f- '3 c.c. iodine solution = 29*8 c.c. iodine solution. .*. -150 grm. iodine = 29*5 c.c. iodine solution. .*. 1 c.c. iodine solution = -0050847 grm. iodine. The experiment just described is repeated and the mean of the two results taken, provided they exhibit sufficient uniformity. y. Dilution of the standard fluids to a convenient strength. With the aid of the iodine solution the strength of which we now know exactly, and the solution of sodium thiosulphate which stands in a known relation to the same, we might make any deter- minations of iodine. The calculation, although in principle ex- tremely simple, is yet somewhat hampered by reason of the long decimal which expresses the quantity of iodine in 1 c.c. of the solution. It is therefore convenient to dilute the iodine solution so that 1 c.c. may exactly contain -005 grm. iodine. This is done by filling a litre flask therewith, and adding the necessary quantity of water; in our case 16-94 c.c., for 5 : 5-0847 : : 1000 : 1016-94. If the litre flask will hold above the mark this 16*94 c.c., it is simply added, otherwise it is put into the dry bottle destined to receive the iodine solution, the iodine solution added, the whole shaken together, a portion of the fluid returned to the flask, shaken, poured back into the bottle, and the whole shaken again. The solution of thiosulphate may now be diluted in a corre- sponding manner. In our case we should have had to add 27*11 c.c. water to 1000 c.c. of the solution, as will be seen from the fol lowing consideration : 20-2 c.c. of the original iodine solution correspond to 20 c.c. of the thiosulphate solution. .-. 1000 c.c. correspond to 990-1 c.c. Now these 1000 c.c. were made up to 1016-94 by addition of water ; if therefore we make up 990*1 c.c. of the sodium thiosul- phate to the same bulk by addition of water we shall have equiva- lent solutions. Hence, to 990-1 c.c. we must add 26*84 c.c. water, or to 1000 c.c. 27*11 water. 448 DETERMINATION. [ 146. In such cases of dilution I always prefer to take exactly 1 litre instead of an uneven number of c.c., as in measuring the latter errors and inaccuracies may readily occur ; I have therefore above recommended the preparation of 1200 c.c. of the fluids, so that after their determination 1000 c.c. may be sure to remain. c. THE ACTUAL ANALYSIS. "Weigh the iodine to be determined in a glass-stoppered tube, dis- solve in potassium iodide solution as in 5, /?, add thiosulphate solution from the burette till decoloration is just produced, then 3 or 4 c.c. starch solution, then iodine solution from a second burette to incip- ient blueness. The substance contains the same amount of iodine as the c.c. of iodine solution corresponding to the thiosulphate used minus the c.c. of the former used to destroy the excess of the latter. Where the solutions are of equal value and 1 c.c. corre- sponds to '005 grm. iodine, the calculation is in the highest degree simple ; for suppose we had used 21 c.c. Na 3 S a O 3 and 1 c.c. iodine, the quantity of iodine present is '100 grm. 21 - 1 = 20, and 20 X '005 = -100. Where you are analyzing chromic acid or manganese dioxide by boiling with hydrochloric acid, and passing the chlorine evolved into potassium iodide, you must allow the solution to cool before titrating with thiosulphate ; for at a high temperature a portion of the sodium tetrathionate produced is converted into sodium sul- phate by the iodine (WRIGHT*). Free acid in the iodine solution to be estimated is not injuri- ous ; when such is present, however, the excess of the thiosulphate must be titrated without delay, or the free thiosulphuric acid may be decomposed before the iodine is added. d. KEEPING OF THE SOLUTIONS. The iodine solution and the thiosulphate solution are kept in glass-stoppered bottles in a cool, dark place. But the relation between the two solutions must be tested before each new series of experiments, and the iodine in the iodine solution must be rede- termined. If a fluid contains free iodine in presence of iodine in combina- tion, determine the former in one portion by the combined method, and the total quantity in another portion. For this purpose you * Zeitschr. f . anal. Chem. 9, 482. 147] CYANOGEN. 449 may either (1) add sulphurous acid to decoloration, precipitate with silver nitrate ( 145, 1., #, or), digest the precipitate with nitric acid to remove any silver sulphite which it may contain, filter, &c. ; or (2) distil with ferric chloride as directed, 145, I., b, y. 4. CYANOGEN.* I. Determination. y Silver Nitrate and Nitric Acid or Silver Nitrate and Ammonia. Digest for some time with a dilute solution of silver nitrate, stirring frequently,* then add nitric acid in moderate excess, and digest at a gentle heat, till the foreign cyanide is fully dissolved and the silver cyanide has become pure and quite white. Then add water and filter. As a precautionary measure it is well to test the metal obtained by long ignition of the silver cyanide, whether it is free from those metals which were combined with the cyano- gen. The filtrate is used for estimating the basic metals, the silver being first precipitated with hydrochloric acid. This method affords us an exact analysis of the double cyanides of potassium with nickel, copper, and zinc (H. ROSE). ~W. WEiTnf recommends a solution of silver nitrate in ammo- nia for the decomposition of many cyanogen compounds, such as potassium ferrocyanide, Prussian blue, and even potassium cobalti- cyauide. He digests them in sealed tubes at 100 (in the case of potassium cobalticyanide, 150) for 4 or 5 hours. Warm the con- tents of the tube gently in a dish, until the crystals of ammonio- cyanide of silver are dissolved, filter off the separated metallic * Double cyanide of Dickel and potassium yields by this process a mixture of silver cyanide with nickel cyanide. Like double cyanides are similarly decom- posed, f Zeitschr. f. anal. Chem. 9, 379. 452 DETEKMINATION. [ 147. oxide, wash it with ammonia, dilute, and precipitate the silver cyanide by acidifying with nitric acid. In the filtrate separate the silver from the alkalies, &c. In respect to the undissolved oxides it should be noted that metallic silver is always mixed with the ferric oxide. c. In Mercuric Cyanide. Precipitate the aqueous solution with hydrogen sulphide ; the mercuric sulphide may be filtered without difficulty if a little ammonia or hydrochloric acid be added ; it is determined accord- ing to 118, 3. If the compound is in the solid condition, the cyanogen may be determined in another portion by ignition with cupric oxide, the nitrogen and carbonic acid being collected and separated (comp. Organic Analysis). H. HOSE and FINKENER* have, after much trouble, succeeded in finding out a method for determining cyanogen with precision also in solutions of mercuric cyanide. Mix the solution of the mer- curic cyanide with zinc nitrate dissolved in ammonia. To 1 part of mercuric salt you may add about 2 parts of the zinc-salt. Add to the clear solution hydrogen sulphide water gradually till it pro- duces a perfectly white precipitate of zinc sulphide. The precipi- tate, which is a mixture of the mercuric and zinc sulphides, settles well. After a quarter of an hour filter it off and wash with very dilute ammonia. The filtrate contains zinc cyanide dissolved in ammonia, together with ammonium nitrate. It does not smell of hydrocyanic acid, and consequently no escape of the latter takes place. Mix it with silver nitrate and then add dilute sulphuric acid in excess. The silver cyanide is next washed a little by decantation, then to free it from any zinc cyanide simultaneously precipitated heated with a solution of silver nitrate, finally filtered off, washed, and determined after I., a. The precipitated sulphides may be dissolved in aqua regia, and the mercury precipitated as mercurous chloride according to 118, 2. The test-analyses com- municated by ROSE yielded excellent results. d. In compounds decomposable by Mercuric Oxide in the Wet Way. Many simple cyanides, and also double 'cyanides both of the character of the double cyanide of nickel and potassium, and of the ferro- or ferricyanides (not, however, cobalticyanides) may, as * Zeitschr. f. anal. Chem. 1, 288. 147] CYANOGEN. 453 is well known, be completely decomposed by boiling with excess of mercuric oxide and water, all cyanogen being obtained as mer- curic cyanide and the metals passing into oxides. H. HOSE (loc. cit.) has shown that Prussian blue, potassium ferro- and ferricyanide, more particularly, may be readily analyzed in this manner. Boil a few minutes with water and excess of mercuric oxide till complete decomposition is effected, add in order to render the ferric hydroxide and mercuric oxide removable by filtration nitric acid in small portions, till the alkaline reaction has nearly disap- peared, filter, wash with hot water, dry the precipitate, ignite very gradually raising the heat under a hood (with a good draught), and weigh the ferric oxide remaining. In the filtrate the cyanogen is determined according to c, and any potassium that may be present is determined in the filtrate from the silver cya- nide. e. Determination of Metals contained in Cyanides with decom- position and volatilization of the Cyanogen. Of the various means for completely decomposing compounds of cyanogen, especially also the double cyanides, according to H. ROSE (loc. cit.) three particularly are worthy of recommendation viz., concentrated sulphuric acid, mercuric sulphate, and ammo- nium chloride. The nitrates seemed decidedly less suitable on account of their too violent action. a. DECOMPOSITION BY SULPHURIC Aero. All cyanogen com- pounds, simple or double, are completely decomposed and con- verted into sulphates or oxides, as the case may be, if treated in a powdered condition in a platinum dish or a capacious platinum crucible with a mixture of about 3 parts concentrated sulphu- ric acid and 1 part water, and heated till almost all the sulphuric acid had been expelled. The residual mass is then free from cyan- ogen. It is dissolved in water, if necessary with addition of hydrochloric acid, and the metals determined by the usual methods. This way is not adapted for mercuric cyanide, as a little of the metal would escape with the fumes of the sulphuric acid. ft. DECOMPOSITION BY MERCURIC SULPHATE. Of the mercuric sulphates, those suitable to our present purpose are the normal and the basic (Turpeth mineral). The substance is mixed with fi parts of the latter, heated in a platinum crucible gradually, and finally maintained for a long time at a red-heat, till all the mercurv has 454 DETERMINATION. [ 147. volatilized, and the weight of the crucible remains constant. If alkalies are present, a little ammonium carbonate is added during the final ignition, from time to time, in order to convert the acid sulphates into normal. The residue may usually be analyzed by sim- ple treatment with water ; in the case of potassium f errocyanide, for instance, the potassium sulphate dissolves, and pure (alkali-free) ferric oxide remains behind. The test-analyses that have been communicated yielded excellent results. y. DECOMPOSITION BY AMMONIUM CHLORIDE. Mix the substance with twice or thrice the amount of this salt, and ignite the mixture moderately in a stream of hydrogen (apparatus, p. 251, fig. 5(W^). From the cooled mass water extracts alkaline chloride, while the reducible metals remain in the metallic state. The method is peculiarly adapted for the analysis of double cyanide of nickel and potassium and cobalticyanide of potassium, not so for iron com- pounds, since the iron obtained is not pure, but contains carbon. If one of the methods described in e is employed, the nitrogen and carbon (the cyanogen) must be determined by a combustion, if an estimation by the loss is not sufficient. f. Determination -of the- Alkalies, especially of Ammonia in Soluble Ferrocyanides. Mix the boiling solution with a solution of cupric chloride, in moderate excess, filter off the precipitated cupric f errocyanide, free the filtrate from copper by means of hydrogen sulphide, and then determine the alkalies (REINDEL*). g. Volumetric Determination of Ferro- and Ferricyanogen. a. After E. DE HAEN. This method, devised in my laboratory, is founded upon the simple fact that a solution of potassium ferro- cyanide acidified with sulphuric acid (and which may accordingly be assumed to contain free hydroferrocyanic acid) is by addition of potassium permanganate converted into the corresponding ferri- cyanide. If this conversion is effected in a very dilute fluid, con- taining about '2 grm. potassium ferrocyanide in from 100 to 200 c.c., the termination of the reaction is clearly and unmistakably indicated by the change of the originally pure yellow color of the fluid to reddish-yellow, f * Journ. f. prakt. Chem. 65, 452. f Instead of the permanganate you may use chromate of potash. The solu- tion is added till spots of sesquicbloride of iron on a plate are no longer colored blue or green, but brownish. E. MEYER, Zeitschr. f. anal. Chem. 8, 508. 147] CYANOGEN. 455 The process requires two test-fluids of known strength, viz. : 1. A solution of pure potassium ferrocyanide. 2. A solution of potassium permanganate. The former is prepared by dissolving 20 grin, perfectly pure and dry crystallized potassium ferrocyanide in water to 1 litre ; each c.c. therefore contains 20 mgrm. The latter is diluted so that somewhat less than a buretteful is required for 10 c.c. of the solu- tion of potassium ferrocyanide. To determine the strength of the potassium permanganate solu- tion in its action upon the potassium ferrocyanide, measure off, by means of a pipette, 10 c.c. of the solution of potassium ferrocyanide (containing '2 grm.), dilute with 100 to 200 c.c. water, acidify with sulphuric acid, place the glass on a sheet of white paper, and allow the permanganate to drop into the fluid, stirring it at the same time, until the change from yellow to reddish-jellow indicates that the conversion is complete.* Repetitions of the experiment always give very accurately corresponding results. If at any time you have reason to suspect that the permanganate has suffered altera- tion, recourse must be had again to this experiment. If after acidifying the potassium ferrocyanide with sulphuric acid you add a trace of ferric chloride to produce a bluish-green color, the latter will disappear at the end of the reaction, which is thus rendered very distinct (GrnTLf). To determine the amount of real potassium ferrocyanide con- tained in any given sample of the commercial article, dissolve 5 grm. to 250 c.c. ; take 10 c.c. of this solution, and examine as just directed. Suppose, in determining the strength of the permanga- nate, you have used 20 c.c., and you find now that 19 c.c. is suffi- cient, the simple rule-of -three sum, 20 : -2 : : 19 : x will inform you how much pure potassium ferrocyanide *2 grm. of the analyzed salt contains. And even this small calculation may be dispensed with, by diluting the permanganate so that exactly 50 c.c. correspond to *2 of potassium ferrocyanide, as, in that case, * If you wish at first for some additional evidence besides the change of color, add to a drop of the mixture on a plate, a drop of solution of sesquichloride of iron : if this fails to produce a blue tint, the conversion is accomplished. j- Zcitschr. f. anal. Chem. 6, 446. 456 DETERMINATION. [ 147. the number of half-c.c. consumed expresses directly the percentage of pure ferrocyanide. Instead of determining the strength of the permanganate by means of pure potassium ferrocyanide, which is unquestionably the best way, one of the methods given in 112, 2, may also be employed ; bearing in mind, in that case, that 2 mol. potassium ferrocyanide 885*52, 2 at. iron = 112, and 1 mol. oxalic acid 126 are equivalent in their action up6n solution of potassium per- manganate. The analysis of soluble ferricyanides by this method is effected by reducing them to ferrocyanides, acidifying, and then proceeding in the way described. The reduction is effected as follows : Mix the weighed ferricyanide with a solution of soda or potassa in excess, boil and add concentrated* solution of ferrous sulphate gradually, and in small portions, until the color of the precipitate appears black, which is a sign that protosesquioxide of iron has precipitated. Dilute now to 300 c.c., mix, filter, and proceed to determine the ferrocyanide in portions of 50 or 100 c.c. of the lluid. As the space occupied by the precipitate is not taken into account in this process, the results are not absolutely accurate ; the difference is so very trifling, however, that it may safely be disre- garded. GINTL (loc. cit.) suggests to put the neutral or alkaline fluid in a tall vessel and add a few lumps of sodium amalgam as big as peas : in ten minutes the reduction will be effected and with- out the aid of heat. Insoluble ferro- or ferricyanides, decomposable by boiling solu- tion of potassa (as are most of these compounds), are analyzed by boiling a weighed sample sufficiently long with an excess of solu- tion of potassa (adding, in the case of ferricyanides, ferrous sul- phate), and then proceeding as directed above. ft. After E. BOHLIG.* In the 'case of a fluid containing potassium ferrocyanide, and also sulphocyanide (for instance, the red liquor of the prussiate works), the method given in a cannot be employed, as the hydro- sulphocyanic acid also reduces permanganic acid. The following method depending on the precipitation of the ferrocyanogen with solution of cupric sulphate may then be used ; it is accurate enough for technical purposes. Dissolve 10 grm. pure cupric sul- * Polyteclm. Notizblatt, 16, 81. 148.] SULPHUR. 457 phate to 1 litre^also 4 grin, pure dry potassium ferrocyanide to 1 litre. Add to 50 c.c. of the latter solution (which contain -2 grm. potassium ferrocyanide) copper solution from a burette to complete precipitation of the ferrocyanogen. In order to hit this point exactly, from time to time dip a strip of filter-paper into the browriish-red fluid which will imbibe the clear filtrate, leaving the precipitate of copper ferrocyanide behind. At first the moist strips of paper, when touched with ferric chloride, become dark blue, the reaction gradually gets weaker and weaker, and finally vanishes altogether. We now know the value of the copper solution with reference to its action on potassium ferrocyanide, and can, there- fore, by its means test solutions containing unknown amounts of ferrocyanogen. If alkali sulphides are present, they are first removed by boiling with lead carbonate. After filtering off the lead sulphide, acidify with dilute sulphuric acid, and then proceed. 148. 5. SULPHUK. I. Determination. To determine hydrogen sulphide in a mixture of gases confined over mercury* it may be absorbed by a ball made of 2 parts precipi- tated lead phosphate and 3 parts plaster of Paris. The mixture is made into a paste with water, and pressed into a bullet mould in which the platinum wire is inserted. The mould should previously be oiled. The balls are dried at 100, saturated with concentrated phosphoric acid, and are then ready for use (LuDwiat). To determine sulphuretted hydrogen dissolved in^water the following methods are in use : a. The method of determining hydrogen sulphide volumetri- cally by solution of iodine, was employed first by DUPASQUIER ; it is very convenient and accurate. That chemist used alcoholic solu- tion of iodine. But as the action of the iodine upon the alcohol alters the composition of this solution somewhat rapidly, it is bet- ter to use a solution of iodine in potassium iodide. The decom- position is as follows : H a S + 21 = 2HI + S * When this gas remains long in contact with mercury, sulphide of mercury is liable to be formed. f Annal. d. Chem. u. Pharm. 162, 55. 458 DETERMINATION. [ 148. 2 at. I = 253-70 correspond, therefore, to 1 mol. H a S = 34. However, tins exact decomposition can be relied upon with cer- tainty only if the amount of hydrogen sulphide in the fluid does not exceed '04 per cent. (BUNSEN). Fluids containing a larger pro- portion of hydrogen sulphide must therefore first be diluted to the required degree with boiled w T ater cooled out of the contact of air. The iodine solution of 146 may be used for the estimation of larger quantities of hydrogen sulphide ; for weak solutions, e.g., sulphuretted mineral water, it is advisable to dilute the iodine solu- tion 5 times, so that 1 c.c. may contain -001 grm. iodine. The process is conducted as follows : Measure or weigh a certain quantity of the sulphuretted water, dilute, if required, in the manner directed, add some thin starch- paste, and then solution of iodine, with constant shaking or stir- ring, until the permanent blue color begins to appear. The result of this experiment indicates approximately, but not with positive accuracy, the relation between the examined water and the iodine solution. Suppose you have consumed, to 220 c.c. of the sulphu- retted water, 12 c.c. of a solution of iodine containing -000918 grm. iodine in the c.c.* Introduce now into a flask nearly the quantity of iodine solution required, add the sulphuretted water in quantity either already determined, or to be determined, by weight or measure ;f then to the colorless fluid add thin starch- paste, and after this iodine solution until the blue color just begins to show. By this course of proceeding, you avoid the loss of hydrogen sulphide which would otherwise be caused by evaporation and oxidation. In my analysis of the Weilbach water, 256 c.c. of the water required, in my second experiment, 16-26 c.c. of iodine solution, which, calculated to the quantity of sulphuretted water used in the first experiment, viz., 220 c.c., makes 13-9 c.c., or 1*9 c.c. more. But even now the experiment cannot yet be considered quite conclusive, when made with a solution of iodine so dilute ; it being still necessary to ascertain how much iodine solution is required to impart the same blue tint to the same quantity of ordinary water mixed with starch-paste, of the same temperature,^: and as nearly as possible in the same condition as the analyzed sulphuretted * The numbers here stated are those which I obtained in the analysis of the Weilbach water. t Compare Experiment No. 82. \ Annal. d. Chem. u. Pharm. 102, 186. In this connection I would recommend, in cases where the sulphuretted 148.] SULPHUR. 459 water, and to deduct this from the quantity of iodine solution used in the second experiment. Thus in the case mentioned, I had to deduct '5 c.c. from the 16'26 c.c. used. If the instructions here given are strictly followed, this method gives very accurate results. b. Mix the sulphuretted fluid with an excess of solution of sodium arsenite, add hydrochloric acid, allow to deposit, and deter- mine the arsenious sulphide as directed 127, 4. The results are accurate unless the solution is very dilute, in which case the slight solubility of arsenious sulphide occasions loss. c. If the hydrogen sulphide is evolved in the gaseous state, and large quantities are to be determined, the best way is to conduct it first through several bulbed U-tubes (fig. 64, p. 435), containing an alkaline solution of sodium arsenite, then through a tube connected with the exit of the last U-tube, which contains pieces of glass moistened with solution of soda ; to mix the fluids afterwards, and proceed as in b. If, on the other hand, we have to determine small quantities of hydrogen sulphide contained in a large amount of air, etc., it is well to pass the gaseous mixture in separate small bubbles through a very dilute solution of iodine in potassium iodide, of known volume and strength, which is contained in a long glass tube fixed in an inclined position and protected against sun- light. The free iodine remaining is finally estimated by means of a solution of sodium thiosulphate ( 146) ; the difference gives us the quantity of iodine which has been converted by hydrogen sulphide into hydriodic acid, and consequently corresponds to the amount of the hydrogen sulphide present. The volume of the gaseous mixture may be known by measuring the water which has escaped from the aspirator used. The arrangement of the absorp- tion tube is the same as is figured in connection with the Deter- mination of Carbonic Acid in Air ( 221). The thin glass tube con- ducting the gas into the absorption tube, however, must not be provided with an india-rubber elongation. From my own experiments* it appears that sulphuretted hydrogen whether in small or large quantities may be also estimated by the increase in weight of absorption tubes. We have only to take care that the mixture of gases is first thoroughly dried by passing over calcium chloride. To take up the hydrogen sulphide water contains bicarbonate of soda, to add to the ordinary water an equal quan- tity of this salt, as its presence has a slight influence on the appearance of the final reaction. *Zeitschr. f. anal. Chem. 10, 75. 460 DETERMINATION. [ 148. we use U-tubes, five sixths filled with copper sulphate on pumice, one sixth at the exit containing calcium chloride. To prepare the pumice with copper sulphate, proceed as follows. Treat 60 grm. pumice in lumps the size of peas in a small porcelain dish with a hot concentrated solution of 30 or 35 grm. copper sulphate, dry the whole with constant stirring, place the dish in an air or oil hath of the temperature of 150 to 160, and allow to remain therein four hours. A tube containing 14 grm. of this prepared pumice will absorb about '2 grm. hydrogen sulphide. It is w r ell always to employ two such tubes. If the prepared pumice is dried at a lower temperature it takes up much less of the gas, if dried at a higher temperature the gas is decomposed and sulphurous acid is formed. Finally, small quantities of hydrogen sulphide mixed with other gases may be estimated by passing through bromine water and con- verting into sulphuric acid. II. Separation and Determination of Sulphur in Sulphides. A. METHODS BASED ON THE CONVERSION OF THE SULPHUR INTO SULPHURIC ACID. 1. Methods in the Dry Way. a. Oxidation ~by Alkali Nitrates (applicable to all compounds of sulphur). If the sulphides do not lose any sulphur on heating, mix the pulverized and weighed substance with 6 parts of anhy- drous sodium carbonate and 4 of potassium nitrate, with the aid of a rounded glass rod, wipe the particles of the mixture which adhere to the rod carefully off against some sodium carbonate, and add this to the mixture. Heat in a platinum or porcelain crucible (which, however, is somewhat affected by the process), at a grad- ually increased temperature to fusion ;* keep the mass in that state for some time, then allow it to cool, heat the residue with water, filter the fluid, boil the residue with a solution of pure sodium car- bonate, filter, wash, remove all nitric acid from the filtrate by repeated evaporation with pure hydrochloric acid, and determine the sulphuric acid as directed in 132. The metal, metallic oxide, or carbonate, which remains undissolved, is determined, according to circumstances, either by direct weighing or in some other suit- able way. In the presence of lead, before filtering, pass carbonic * If gas not free from sulphur is used for heating, some sulphur is likely to be absorbed PRICE, Journ. Chem. Soc., (2) 2, 51. If a platinum crucible is used do not raise the heat more than necessary, or Ihe crucible will be attacked. 148.] SULPHUR. 461 acid through the solution of the fused mass, to precipitate the small quantity of that metal which has passed into the alkaline solution. Should the sulphides, on the contrary, lose sulphur on heating, the finely powdered compound is mixed with 4 parts sodium car- bonate, 8 parts nitre, and 24 parts pure and perfectly dry sodium chloride, and the process otherwise conducted as already given. b. Oxidation by Chlorine Gas (after BEEZELIUS and H. ROSE especially suitable for sulphosalts of complicated composition). The following apparatus (fig. 65), or one of similar construction, is used ; corks should be used, not india-rubber stoppers, and wher- ever there is an india-rubber connection, the glass tubes should be close to each other. The flask a is completely filled with pieces of pyrolusite (native manganese dioxide) of the size of hazelnuts, strong hydrochloric acid is poured in till the spaces between the pieces of pyrolusite are filled up to half the height of the body of the flask. The upper layer of pyrolusite, which should be rinsed with a little water after pouring in the hydrochloric acid, serves to purify the evolved chlorine almost completely from hydrochloric acid. When the stopcock in one of the tubes provided for conducting the chlorine is closed, the chlorine passes down into the cylinder b filled with rather dilute soda solution, by which it is completely absorbed. When the stopcock is opened the chlorine is conducted by a tube to the bottom of c into a layer of concentrated sulphuric acid, which serves to indicate the rapidity of the current ; c is moreover com- pletely filled with fragments of pumice-stone moistened with con- centrated sulphuric acid, for the purpose of drying the chlorine. The tube with the bulb d must be made of glass which is not too easily fusible, and must be adjusted, not horizontally, but a little inclined, so that heavy vapors may not pass back against the slow current of chlorine. The danger that vapors may pass back is further lessened by making the end of the bulb-tube at which chlorine enters no wider than is necessary for the introduction of the substance by means of a long, narrow, thin weighing tube. The part of the tube on the other side of the bulb should have a greater diameter, since it might otherwise be choked up by a sublimate, 462 DETERMINATION. [148. especially if the substance contains much antimony. It is narrowed at one point to facilitate subsequent fusion and drawing asunder. The downward bent end is fitted into the receiver e by means of a cork, or a piece of rubber tubing drawn over it. The receiver con- tains water or, if antimony is present in the substance, dilute hydro- chloric acid to which is also added a little tartaric acid (free from sulphuric acid). The volume of liquid should be only so large as to cause the passing gas to bubble through it in the narrow spaces at each end of the lower bulb, which should be large enough to hold 25 Fig. 65 to 30 c.c. when thus charged. It is well also to attach to the receiver a small U-tube charged with a small volume of the liquid absorbent in such a manner as to increase as little as possible the pressure in the interior of the apparatus. Finally, a long, light glass tube may be attached to the last U-tube for conducting the escaping chlorine into the open air or into a flue. When the substance has been introduced into the bulb-tube, and the whole apparatus is connected, the stopcock is first closed and 148.] SULPHUR. 463 evolution of chlorine is produced by application of gentle heat. A B soon as gas-bubbles following each other in quick succession appear in the soda solution, the heat is withdrawn. A constant evolution of chlorine will then go on for a long time without fur- ther application of heat. "When the gas-bubbles are nearly com- pletely absorbed by the soda solution, the stopcock is opened so wide that a slow current of gas enters c and after a while reaches the bulb d. If the substance is decomposed at the ordinary tem- perature (e.g., antimony sulphide), care must be taken to diminish the rapidity of the chemical action and consequent elevation of temperature, by partial closing of the stopcock, so that sulphur chloride may not distil over into the receiver at this stage of the process. For if sulphur chloride reaches the liquid in the receiver which is not yet saturated with chlorine, it is decomposed with separation of sulphur which is afterwards not easily converted into sulphuric acid by chlorine. "When the action of chlorine ceases to produce elevation of temperature or any apparent change of the substance, and the absorbing liquid has become charged with chlorine, the current is slightly increased and gentle, very gradu- ally increased heat is applied to the bulb, which, however, is not even at the end of the operation brought to redness. During this operation the flow of chlorine must not be so rapid as to carry visible fumes through the absorbing apparatus, and sulphur chloride must be distilled over so slowly that the absorbing liquid remains throughout well charged with chlorine. If the latter precaution, is neglected, unoxidized sulphur will remain at the close of the operation, which will render the subsequent part of the process more troublesome and probably less accurate. Besides sulphur chloride, the volatile metallic chlorides distil over. The portion of the tube beyond the bulb may be kept moderately heated so as to prevent it from being stopped up by a sublimate, especially at the narrowed part. When by gradually increased temperature no more volatile products arise from the mass in the bulb and con- dense in the cooler portion of the tube beyond it, except perhaps ferric chloride (giving a dark brown sublimate), the complete expulsion of which need not be awaited, the heating is extended so that the sublimate in the tube is gradually driven as far as prac- ticable into the receiver, or at least beyond the narrowed part. The stopcock is then closed while the bulb is still warm. "When, after a few minutes, the liquid in the receiver has receded some- 464 DETEKMINATION. [ 148. what, soften the narrow part of the tube with the flame of a Bnnsen burner aided by a blowpipe having a rather large jet, and at the same time draw the tube asunder. The drawn-off end of the tube containing anhydrous chlorides, which volatilize on exposure to the air, must not be withdrawn from the receiver until the chlorides are dissolved or have by long standing absorbed moisture. Their solution is easily effected pro- vided the tube extends well down into the receiver by inclining the latter so that liquid comes in contact with the end of the tube. The liquid then gradually rises in the tube, absorbing the chlorine gas and dissolving the chlorides in it ; meantime, if necessary, the cork may be slightly loosened to admit a little air and prevent the liquid from reaching it by absorption of chlorine. If one fails to effect a solution in the manner above described, the whole may be allowed to stand 24 hours, during which time the chlorides in the tube absorb moisture from the liquid in the receiver, so that the tube can then be withdrawn and the chlorides may be dissolved out with diluted hydrochloric acid and added with rinsings of the tube to the solution in the receiver. Finally, if it is intended to adopt this latter mode of proceeding, the tube may be cut off and immediately closed with a cork instead of being fused and drawn off. The solution of the chlorides obtained from the end of the tube, the solution in the receiver and that in the appended U-tube being united, a very gentle heat is applied until the free chlorine is expelled, and the fluid is then allowed to stand until the sulphur, if any is present, has solidified. The sulphur is filtered off on a weighed filter, washed, dried, and weighed. The filtrate is precipi- tated with barium chloride (132), by which operation the amount of that portion of the sulphur is determined which has been con- verted into sulphuric acid. The fluid filtered from the barium sul- phate contains, besides the excess of barium chloride added, also the volatile metallic chlorides ; which latter are finally determined in it by the proper methods, which will be found in Section Y. The chloride remaining in the bulb-tube is either at once weighed as such (silver chloride, lead chloride), or where this is impracticable as in the case of copper, for instance, which remains partly as cuprous, partly as cupric chloride it is dissolved in water, hydrochloric acid, nitrohydrochloric acid, or some other suitable solvent, and the metal or metals in the solution are determined by the methods already described, or which will be found in Section 148.] SULPHUR. 465 Y. To be enabled to ascertain the weight of the bulb-tube con- taining silver chloride, it is advisable to reduce the chloride by hydrogen gas, and then dissolve the metal in nitric acid. In cases where you have only to estimate the sulphur, say in substances containing also sulphuric acid, O. LLNDT* recommends conducting the chloride of sulphur and the volatile metallic chlorides into pure solution of soda, when decomposition immedi- ately takes place, producing sodium sulphide, sodium thiosulphate, sodium chloride, and hypochlorite. When the decomposition is over, continue passing the chlorine for two hours through the soda, evaporate then to dryness, ignite the residue cautiously to destroy the sodium chlorate, dissolve in water, and estimate the sulphuric acid according to 132. c. Oxidation ~by Oxide of Mercury (after BUNSEN). This method, which will be found in detail, 186, is particu- larly suited to the estimation of sulphur in volatile compounds, or in substances which when heated lose sulphur. 2. Methods in the Wet Way. a. Oxidation of the Sulphur by Acids yielding Oxygen, or ~by Halogens. f a. Weigh the finely pulverized sulphide in a small glass tube sealed at one end, and drop the tube into a tolerably capacious strong bottle with glass stopper, which contains red fuming nitric acid (perfectly free from sulphuric acidj) in more than sufficient quantity to effect the decomposition of the sulphide. Immediately after having dropped in the tube, close the bottle. When the action, which is very impetuous at first, has somewhat abated, shake the bottle a little ; as soon as this operation ceases to cause renewed action, and the fumes in the flask have condensed, take out the stopper, rinse this with a little nitric acid into the bottle, and then heat the latter gently. aa. The whole of the Sulphur has been oxidized, the Fluid is * Zeitschr. f. anal. Chem. 4, 370. f In presence of lead, barium, strontium, calcium, tin, and antimony, method b is preferable to a. $ To test for sulphuric acid in nitric or hydrochloric acid, it is necessary to evaporate on a water-bath nearly to dryness and take up with water before add- ing barium chloride. When the acid cannot be got pure, determine the sulphuric acid and allow for it. 466 DETERMINATION. [ 148. perfectly clear :* Evaporate with some sodium chloride, towards the end adding pure hydrochloric acid repeatedly, cooling the dish each time before adding the acid. Dilute with much water, and determine the sulphuric acid as directed 132. Make sure that the pre'cipitate is pure ; if it is not, purify it according to 132. Separate the bases in the filtrate from the excess of the barium salt by the methods given in Section Y. l)b . Undissolved Sulphur floats in the Fluid: Add potassium chlorate in small portions, or strong hydrochloric acid, and digest some time on a water-bath. This process will often succeed in dis- solving the whole of the sulphur. Should this not be the case, and the undissolved sulphur appear of a pure yellow color, dilute with water, collect on a weighed filter, wash carefully, dry, and weigh. After weighing, ignite the whole, or a portion of it, to ascertain whether it is perfectly pure. If a fixed residue remains (consisting commonly of quartz, gangue, &c., but possibly also of lead sul- phate, barium sulphate, &c.), deduct its weight from that of the impure sulphur. In the filtered fluid determine the sulphuric acid as in aa, calculate the sulphur in it, and add the amount to that of the undissolved sulphur. If the residue left upon the ignition of the undissolved sulphur contains an insoluble sulphate, decompose this as directed in 132, and add the sulphur found in it to the principal amount. In the presence of bismuth, the addition of potassium chlorate or of hydrochloric acid, is not advisable, as chlorine interferes with the determination of bismuth. /?. Mix the finely pulverized metallic sulphide in a dry flask, by shaking, with powdered potassium chlorate (free from sulphuric acid), and add moderately concentrated hydrochloric acid in small portions. Cover the flask with a watch-glass, or with an inverted small flask. After digestion in the cold for some time, heat gently, finally on the water-bath, until the fluid smells no longer of chlo- rine. Proceed now as directed in a, aa, or J, according as the sulphur is completely dissolved or not. In the latter case you must of course immediately dilute and filter. The oxidation of the sul- phur may be usually effected more quickly and completely by * This can of course be the case only in absence of metals forming insoluble salts with sulphuric acid. If such metals are present, proceed as in bb, as it is in that case less easy to judge whether complete oxidation of the sulphur has beer attained. 148.] SULPHUR. 467 warming with nitric acid of 1*36 sp. gr. on a water-bath, and add- ing potassium chlorate in small portions. Compare STOKER,* PEAR- SOX, and BowDiTCH.f y. Aqua regia is also frequently used. J. LEFORT^: recommends a mixture of 1 part strong hydrochloric acid and 3 parts strongest nitric acid. Complete conversion of sulphur into sulphuric acid, however, is rarely effected by aqua regia. 6". Bromine may also be used. Pyrites or blende is digested at a gentle heat with water, and bromine gradually added. If the sul- phides have been prepared in the wet way, good bromine water is sufficient to oxidize them. P. WAAGE prefers bromine to all other wet agents, and advises its purification by distillation in an appa- ratus from which all caoutchouc connections are excluded. J). Oxidation of the Sulphur by Chlorine in Alkaline Solution, after RIVOT, BEUDANT, and DAGUIN.|| (Suitable also for determining the sulphur in the crude article.) Heat the very finely pulverized sulphide or crude sulphur for several hours with solution of potassa free from sulphuric acid (which dissolves free sulphur, as well as the sulphides of arsenic and antimony), and then conduct chlorine into the fluid. This speedily oxidizes the sulphur ; the sulphuric acid formed combines with the potassa to sulphate, which dissolves in the fluid, whilst the metals converted into oxides remain undissolved. Filter, acid- ify the alkaline filtrate, and precipitate the sulphuric acid by barium chloride ( 132). Arsenic and antimony pass into the alkaline solution in the form of acids, but not so lead, which is converted into binoxide, and remains completely undissolved. This method is, therefore, particularly suitable in presence of lead sulphide. In presence of iron sulphide, potassium sulphate is formed at first, and ferric hydroxide, which, if the action of the chlorine is allowed to continue, begins to be converted into potassium ferrate. As soon, therefore, as the fluid commences to acquire a red tint the transmission of chlorine must be discontinued, and the fluid gently heated for a few moments with powdered quartz, to decompose the ferric acid. It occasionally happens, more particularly in presence of sand, iron pyrites, cupric oxide, &c., that the process is attended with impetuous disengagement of oxygen, which almost completely pre- * Zeitschr. f. anal. Chem. 9, 71. f Ib. 9, 82. J Ib. 9, 81. Ib. 10, 206. || Compt. Rend. 1835, 865 ; Journ. f. prakt. Chem. 61, 134. 468 DETERMINATION. [ 148. vents the oxidizing action of the chlorine. However, this accident may be guarded against by reducing the substance to the very finest powder. J2. METHODS BASED ON THE CONVERSION OF THE SULPHUR INTO HYDROGEN SULPHIDE, OK A METALLIC SULPHIDE. a. The determination of the sulphur in the sulphides of the metals of the alkalies and alkaline earths soluble in water is best effected provided they are free from excess of sulphur by L, l>. In the absence of acids of sulphur you may also convert the sulphur into sulphuric acid by bromine water. The bases are conveniently estimated in a separate portion, which is decomposed by evapora- tion with hydrochloric or sulphuric acid, or when none but alkali- metals are present by ignition with 5 parts of ammonium chloride in a porcelain crucible. If the compounds contain excess of sul- phur, they should be oxidized either by chlorine in alkaline solu- tion or treated according to B, c ; if they contain thiosulphate or sulphite, proceed according to 168. b. The sulphur contained in alkaline fluids as monosulphide or Iiydrosulphate of the sulphide may also be determined directly by volumetric analysis, by means of a standard ammoniacal silver or copper solution. In using the former, mix the solution with ammo- nia, heat and add the standard fluid till, on filtering off a small portion and adding silver solution, a mere opalescence is produced (LESTELLE*). In using the copper solution, mix the fluid to be tested with ammonia, heat to 50 or 60, and add the standard solu- tion, frequently shaking and boiling till no further precipitation of CuO, 5CuS is produced, and the solution begins to be blue (VER- STRAETf). To make a standard copper solution, 1 c.c. of which shall equal .01, E"a 2 S, dissolve 9.754 pure copper in 40 grm. nitric acid, boil, add 180 to 200 c.c. ammonia and water to 1 litre. These methods are well adapted for technical purposes, for the estimation of sulphide in soda lies for instance. It need hardly be added that precipitated silver, copper, or lead sulphide (if you have used a solution of oxide of lead in potash) may be estimated gravimetri- cally. c. If all the sulphur can be expelled from the substance in the form of sulphuretted hydrogen by heating with hydrochloric acid, the sulphide may be heated in a small flask with the concentrated * Zeitschr. f. anal. Chem. 2, 94. f Ib. 4, 216. g 149.] NITRIC ACID. 46t> acid to complete decomposition and expulsion of the hydrogen sul- phide the latter being determined according to I. In the case of polysulphides, the sulphur separated in the evolution flask is col- lected on a filter dried at 100, washed, dried first at 70, then for a short time at 100, and weighed. Third Group. NITKIC ACID. - CHLORIC ACID. 1. XITKIC ACID. . I. Determination. Free nitric acid in a solution containing no other acid is deter- mined most simply in the volumetric way, by neutralizing with a dilute solution of soda or ammonia of known strength (comp. Spe- cial Part, " Acidimetry"). The following method also effects the same purpose : Mix the solution with baryta-water, until the reac- * tion is just alkaline, evaporate slowly in the air, nearly to dryness, dilute the residue with water, filter the solution which has ceased to be alkaline, wash the barium carbonate formed by the action of the carbonic acid of the atmosphere upon the excess of the baryta- water, add the washings to the filtrate, and determine in the fluid the barium as directed in 101. Calculate for each 1 at. barium 2 mol. nitric acid. Lastly, free nitric acid may also be determined in a simple manner by supersaturating with ammonia, evaporating in a weighed platinum dish, drying the residue at 110 to 120, and weighing the NH 4 NO 3 (SCHAFFGOTSCII): II. Separation of nitric add from the basic radicals, and determination of the acid in nitrates. a. Methods based on the decomposition of Nitrates in the Dry Way. ex. In anhydrous metallic nitrates which leave upon ignition a metallic oxide of known and definite composition, the nitric acid may be determined by ignition and calculation from the weight of the residue. ft. In the case of nitrates, whose residue on ignition has no constant composition, or by whose ignition the crucible is much attacked (alkali and alkali-earth nitrates), fuse the substance (which 470 DETERMINATION. [ 149. must be anhydrous and also free from organic and other volatile bodies) with a noil- volatile flux, and estimate the nitric acid from the loss. Silicic acid is the best flux, as it may be readily procured, and the execution is the most easy and the most certain to succeed. I shall describe the method in its application to potassium or sodium nitrate. Fuse the latter at a low temperature, pour out on to a warm porcelain dish, powder, and dry again before weighing.. Now transfer to a platinum crucible 2 to 3 grin, powdered quartz, ignite well, and weigh after cooling. Add about 0*5 grm. of the salt prepared as above, mix well, and convince yourself by the balance that nothing has been lost during mixing. The covered crucible is then exposed to a low "red heat (just visible by day) for half an hour, and weighed after cooling with the cover. The loss of weight represents the quantity of K 9 O S . Sulphates or chlorides are not decomposed at the given temperature ; if a higher heat be applied, the latter may volatilize. The action of reducing gases must be avoided. The test-analyses, communicated by REICH,* as well as those performed in my own laboratory, f gave very satisfac- tory results. I). Method based on tJie distillation of Nitric Acid. All nitrates may be decomposed by distillation with moderately dilute sulphuric acid. The nitric acid passing into the receiver may then be determined, according to L, volumetrically or gravi- metrically. 1 to 2 grm. of the nitrate should be treated with a cooled mixture of 1 volume concentrated sulphuric acid and 2 vol- umes water. For 1 grm. nitre take 5 c.c. sulphuric acid and 10 c.c. water. The distillation may be performed either with a ther- mometer at 160 to 170 in a paraffin or sand bath (duration of the distillation for 1 to 2 grm. nitre, 3 to 4 hours), or in vacuo, with the use of a water-bath. The latter process is the best. In the former, the neck of the tubulated retort (which is drawn out and bent down) is connected with a bulbed TJ-tubeJ containing a meas- ured quantity of standard soda or potassa solution ( 192). The distillation in vacuo may be conducted, without the use of an air- pump, according to FINKENER,|| as follows: Transfer the measured * Berg- und Huttenmannische Zeitschrift, 1861, No. 21; Zeitschrifl f. analyt. Chem. 1, 86. t Zeitschr. f. anal. Chem, 1, 181. \ The bulbed U-tube will be found figured 185. || Zeitschrift f. analyt. Chem. 1, 309. 149.] NITRIC ACID. 471 quantity of water and concentrated sulphuric acid to the tubulated retort, and the necessary quantity of standard potassa or soda solu- tion, diluted to 30 c.c., to a flask with a narrow neck of about 200 c.c. capacity. Then, by means of an india-rubber tube, connect the flask with the retort air-tight, so that the drawn-out point of the latter may extend to the body of the flask, and with tubulure open heat the contents of the retort and of the flask to boiling. When the air has been expelled from the apparatus by long boil- ing, transfer the salt (weighed in a small tube) to the retort through the tubulure, close the latter immediately, and at the same time take away the lamp. The retort is then heated with a water-bath, the flask being kept cool. The quantity of nitric acid that has passed over is finally ascertained by determining the still free alkali with standard acid. If it is suspected that all the nitric acid has not been driven into the receiver by one distillation, you may by heating the flask and cooling the retort distil the water back into the latter, and then the distillation from the retort may be repeated. The distillate thus obtained is always free from sulphuric acid,, hence the results are very exact. The base remains as sulphate in* the retort. In the presence of chloride add to the contents of the retort a sufficiency of dissolved silver sulphate, or when much chloride is present moist silver oxide. The nitric acid is then obtained entirely free from chlorine. c. Methods based on the decomposition of* Nitrates by Alka- lies, &c. a. jSTitrates of metals which are completely precipitated by alkali hydroxides or carbonates provided basic salts are not pre- cipitated at the same time may be analyzed by simple boiling with an excess of standard potassa or soda or their carbonates. After cooling, dilute to J or ^ litre, mix, allow to settle, draw off a portion of the supernatant clear fluid, determine the free alkali remaining in it, and calculate therefrom the amount which has been converted into nitrate. HAYES obtained with silver and bis- muth nitrates good results; but with mercurous nitrate (using sodium carbonate) the results were not so satisfactory.* /?. In nitrates from which the basic metals are precipitated by barium or calcium hydroxides or their carbonates (or by barium sulphide), the nitric acid may be estimated with great accuracy by * H. Rose, Zeitschrift f. analyt. Chem. 1, 306. 472 DETERMINATION. [ 149. filtering, after precipitation lias been effected, warm or cold, pass- ing carbonic acid through the filtrate, if necessary, till all the barium is precipitated, warming, filtering, and determining the barium in the filtrate by sulphuric acid. 1 at. of the same corre- sponds to 1 mol. nitric anhydride (N~ a O 6 ). [In case of bismuth- salts, boil until the separated oxide is perfectly yellow. PAIGE.] y. In many nitrates whose bases are precipitable by sulphuret- ted hydrogen the nitric acid may be determined according to GIBB& by adding to the salt in solution about its own weight of some neutral organic salt, e.g., Rochelle salt, and throwing down the metal by H 2 S. The filtrate and w r ashings are brought to a definite bulk, and the free acid is determined in aliquot portions alkalimet- rically.* d. Methods based upon the decomposition of Nitric Acid by Ferrous Chloride. Method of PELouzEf and FRESENIUS. The decompositio n is a follows : 6FeCl 2 + 2KN0 3 + 8HC1 = 3Fe 2 Cl 6 + 2KC1 + 4H 2 O + N.O,- a. Select a tubulated retort of about 200 c.c. capacity, with a long neck, and fix it so that the latter is inclined a little upwards. Introduce into the body of the retort about 1-5 grin, fine piano- forte wire, accurately weighed, and add about 30 or 40 c.c. pure fuming hydrochloric acid. Conduct now through the tubulure, by means of a glass tube reaching only about 2 cm. into the retort,, hydrogen gas washed by solution of potassa, or pure carbonic acid,, and connect the neck of the retort with a U-tube containing some water. Place the body of the retort on a water-bath, and heat gently until the iron is dissolved. Let the contents of the retort cool in the current of hydrogen gas or carbonic acid ; increase the latter, and drop in, through the neck of the retort, into the body, a small tube containing a weighed portion of the nitrate under examination, which should not contain more than about 0*200 grin, of N 2 O 5 . After restoring the connection between the neck and the U-tube, heat the contents of the retort in the water-bath for about a quarter of an hour, then remove the water-bath, heat with the lamp to boiling, until the fluid, to which the nitric oxide had imparted a dark tint, shows the color of ferric chloride, and con- * Am. Jour..Sci., xliv. 209. \ Journ. f. prakt. Chem. 40, 324. 149.] MTKIC ACID. 473 tinue boiling for some minutes longer. Care must be taken to give the fluid an occasional shake, to prevent the deposition of dry salt on the sides of the retort. Before you discontinue boiling, increase the current of hydrogen or carbonic acid gas, that no air may enter through the U-tube when the lamp is removed. Let the contents cool in the current of gas, dilute copiously with water, and determine the iron still present as ferrous chloride volumetri- cally by potassium dichromate 336 of iron converted by the nitric acid from ferrous to ferric chloride correspond to 108 (K a O 6 ). My test-analyses of pure potassium nitrate gave 100*1 100*03 100*03, and 100*05, instead of 100.* [The iron remaining as ferric chloride may also be determined by sodium thiosulphate.] ft. SCHULZE'S Methodf modified by TIEMANN.^ The solution containing the nitrate is concentrated if necessary to a volume of about 50 c.c. and introduced into the flask A, which should have a capacity of about 200 c.c. This flask is provided with a rubber stopper, through which pass two bent tubes a b c and ef g. The first is drawn out to a point (not too small) at a, and projects through the stopper about 2 cm. ; the second terminates without diminution of size exactly at the lower surface of the stopper. These two tubes are connected by rubber tubes (bound with thread) at c and g with the glass tubes c d and g h. A rubber tube is drawn over the lower end of g h to protect it from fracture. B is a glass vessel containing 10 per cent, soda solution . A measuring tube graduated to 0*1 c.c., of not too great diameter, filled with previously boiled soda solution, is supported so that its open end is under the surface of the liquid in B. The solution of the nitrate in the flask is further concentrated by boiling, and finally the lower end of the tubeefg h is brought into the soda solution so that a part of the steam escapes through it. After a few minutes the rubber tube at g is pressed together with the fingers ; if the air has been completely displaced from the flask by boiling, the soda solution will rise suddenly in the tube as in a vacuum, and a slight blow against the finger will be percep- tible. In this case, the rubber tube at g is closed with a clamp and the steam is allowed to escape through abcdnniil only 10 c.c. * Annal. d. Chem. u. Pharm. 106, 217. f Zeitschr. fur anal. Chem. 1870, 400. | Anleitung zur Untersuchung von Wasser, von W. Kubel, Zweite Auflage von F. Tiemann, Braunschwerg bei Fr. Yieweg u. Sohn. 1870, s. 55. 474 DETERMINATION. [ 149. of fluid remain in the flask. The lamp is now removed and the rubber tube at c is closed with a clamp, and the tube c d filled by a jet of water. If an air bubble remains in the rubber tube at 0, it must be removed by pressure with the fingers. The graduated measuring tube is now brought over the upcurved end of the evo- lution tube efg h so that the end rises in it 2-3 cm. The flask must next be allowed to stand a few minutes until a partial vacuum is produced in it, which is manifested by a contraction of the rubber tubes at c and g. A nearly saturated solution of ferrous chloride is poured into a small beaker, the upper part of which is marked Fig. 67. so as to show the space occupied by 20 c.c. ; two other beakers must also be at hand partly filled with concentrated hydrochloric acid. The tube c d is now T dipped into the ferrous chloride solution, and the clamp at c is loosened until 15-20 c.c. are drawn into the flask. The ferrous chloride remaining in the tube is next removed by drawing in a small quantity of hydrochloric acid in two suc- cessive portions. Small bubbles may frequently be observed at 5, occasioned by evolution of hydrochloric gas caused by dimin- ished pressure in the flask. They disappear almost completely so soon as the pressure rises. g 149.] NITRIC ACID. 475 Heat is applied, at first very gently, until the rubber tubes at c and g are slightly expanded ; then the rubber tube at g is held com- pressed by the fingers, the clamp being removed, until the pressure becomes stronger, when the gas is allowed to pass over to the grad- uated tube. Toward the end of the operation heat is increased and distillation continued until the volume of gas in the measuring tube no longer increases. The hydrochloric gas, abundantly evolved in the last part of the process, is absorbed with violence by the soda solution with a peculiar clattering sound ; there is no danger, however, of breaking the evolution tube if care has been taken to enclose the lower end with a rubber tube as above directed. The measuring tube is brought into a large cylinder containing cold water, best of 15-18 C., and by means of some suitable fix- ture held wholly submerged in the same. The transfer is effected with the help of a small porcelain dish filled with soda solution. After 15-20 minutes, the temperature of the water in the cylinder is ascertained with a sensitive thermometer, and the state of the barometer is also observed. Then the tube is taken hold of at the upper end with a strip of paper or cloth, in order to avoid imparting heat to it by direct contact of the hand, and drawn up perpendicularly so far that the level of the fluids within and without it exactly coincide, and the volume of the gas is read off. From the data thus obtained, the volume which the dry gas would occupy at C. and 760 mm. bar. pressure is to be computed. (See p. 836, on Calculation of Analyses.) 1 c.c. JST a O, at C. and 760 mm. bar. pressure corresponds to 002413 grm. N 2 O S . A condition indispensable for the success of the operation is the complete expulsion of air from the apparatus in the beginning. When an abundant quantity of nitric acid is present in the sub- stance, enough to produce about 80 c.c. nitrogen dioxide is a suit- able quantity to use for its determination, and a somewhat larger quantity of ferrous chloride and hydrochloric acid than above indi- cated may be used. An unnecessary amount of these reagents should, however, be avoided, since it is difficult to boil a small quan- tity of nitrogen dioxide out of a large volume of liquid. This method is easy to carry out and gives satisfactory results. It has been selected for description and recommendation here out of a great number of methods, not mentioned in this volume, which have been proposed and more or less used for determination of nitric acid. 476 DETERMINATION. [ 150. e. Methods in which the Nitrogen of the Nitric Acid is sep- arated and measured in the gaseous form. These methods are more particularly suitable for analyzing nitrates which are decomposed by ignition into oxide or metal and oxides of nitrogen ; they will be found in the Section on the Ulti- mate Analysis of Organic Bodies, 184. MARIGNAC employed them to analyze rnercurous nitrates. BROMEIS analyzed nitrite, &c., of lead by a similar method, recommended by BUNSEN. In cases where it is intended to determine the water of the analyzed nitrate in the direct way, such methods are almost indispensable.* 150. 2. CHLORIC ACID. I. Determination. Free chloric acid in aqueous solution may be determined by converting it into hydrochloric acid by the agency of nascent hydrogen (II., &), and determining the acid formed, as directed in 141 ; or by saturating with solution of soda, evaporating the fluid, and treating the residue as directed in II., a or c. II. Separation of Chloric Acid from the Bases and Determination of the Acid in Chlorates. a. After BuNSEN.f "When warm hydrochloric acid acts upon chlorates, the latter are reduced ; as this reduction is not attended with separation of oxygen, the following decompositions may take place : C1 2 5 2 C1 2 6 3 C1 2 C1 2 5 2 C1 2 5 C1 2 5 12C1 2HC1 j g 1 ^ 3 4HC1 I 2 H 2 Q 6HC1 | Jg 1 ^ 8HC1 | g^Q 10HC1 ] 5H *<> Which of these products of decomposition may actually be formed, whether all or only certain of them, cannot be foreseen. But no matter which of them may be formed, they all of them agree in this, that, in contact with solution of potassium iodide, they liber- ate for every 2 mol. chloric acid (HC1O 3 ), or 1 mol. C1 2 O 5 in the chlorate, 12 at. iodine. 1522*2 of iodine liberated correspond accord- ingly to 150-92 C1 3 O 5 . The analytical process is conducted as des- cribed 142, 1. * See also Gibbs, Am. Journ. Sci., xxxvii. 350. f Annal. d. Chem. u. Pharm. 86, 282. jj 150.] CHLOKIC ACID. 477 l>. After SESTINI.* To the concentrated aqueous solution of the weighed chlorate add a piece of zinc and then some pure dilute sulphuric acid and allow to stand for some time (with 0.1 grin, potassium chlorate half an hour is sufficient). By the nas- cent hydrogen the chloric acid is converted into hydrochloric acid, which, after removal and rinsing of the zinc, is determined accord- ing to 141. To use the volumetric method ( 141, , a\ the sul- phuric acid is first precipitated with barium nitrate, then the zinc and excess of barium with sodium carbonate, the liquid is filtered and neutralized, then potassium chromate is added, and finally standard silver solution. c. The basic radicals are determined with advantage in a sepa- rate portion, by converting the chlorate either by very cautious ignition, or by warming with hydrochloric acid into chloride. The estimation of hypochlorous acid will be described in the Special Part, article " Chlorimetry." \ Zeitschrift f. analyt. Chem. 1, 500. SECTION V. SEPAKATION OF BODIES. 151. WHEN only one basic or one acid radical is present, the method of its determination has been considered in the previous Section. When more than one basic or more than one acid radical is pres- sent, the methods of separating and determining them will be described in the present Section. The separation of bodies may be effected in three ways : viz., #, by direct analysis ; b, by indirect analysis ; c, by estimation by difference. By direct analysis, we understand the actual separation of rad- icals or elements. Thus, we separate potassium from sodium by platinic chloride ; copper from tin by nitric acid ; arsenic from iron by hydrogen sulphide ; iodine from chlorine by palladious nitrate ; carbon from potassium nitrate by water, &c., &c. In direct analysis we render one body insoluble, while the others remain in solution, or vice versa, or we volatilize one body, leav- ing the others behind, or we effect actual separation in some other manner. This is the mode of analysis most frequently employed. It generally deserves the preference where choice is permitted. We term an analysis indirect if it does not effect the actual sep- aration of the bodies, but causes certain changes which enable us to calculate their quantity. Thus, the quantity of potassium and sodium in a mixture of compounds of the two may be determined by converting them into chlorides, weighing the latter, and deter- mining the chlorine ( 152, 3). Finally, if we weigh two bodies together, determine one of them, and subtract its weight from that of the two, we shall find the weight of the other body. In this case the second body is said to be estimated by difference. Thus, aluminium may be determined when its oxide is mixed with ferric oxide, by weighing the mix- ture and determining the iron volumetrically. [ 151. SEPARATION OF BODIES. 479 Indirect analysis and estimation by difference may be employed in an exceedingly large number of cases ; but their use is as a rule only to be recommended where good methods of true separation are wanting. The special cases in which they are preferable to direct analysis cannot be all foreseen ; those alone are pointed out which are of more frequent occurrence. As regards the calcu- lations required in indirect analysis, I have given general direc- tions under " the Calculation of Analysis ;" wherever it appeared judicious, I have added the necessary directions to the description of the method itself. I have retained our former subdivision into groups, and, as far as practicable, systematically arranged, first, the general separation of all the bodies belonging to one group from those of the preced- ing groups ; secondly, the separation of the individual bodies of one group from all or from certain bodies of the preceding groups ; and finally, the separation of bodies belonging to one and the same group from each other. I think I need scarcely observe that the general methods which serve to separate the whole of the bodies of one group from those of another group are also applicable to the separation of every individual body of the one group from one or several bodies of the other group. It must not be understood that the more special methods are necessarily in all cases preferable to the more general ones. As a rule, it must be left to individual chemists to decide for themselves in each special case which method should be adopted. With respect to the general methods for sepa- rating one group from another, I would observe that those adduced appeared to me more adapted to the purpose than others, but still there may be others that are equally suitable, and in special cases even more so. A wide field is here open to the ingenuity of the analyst. The methods given for the separation of both basic and acid radicals are generally based upon the supposition that they are in the form of free acids or bases, or in the form of salts soluble in water. Wherever this is not the case, special mention is made of the circumstance. From among the host of proposed methods, I have, as far as practicable, chosen those which have been sanctioned by experience and are distinguished for accurate results. In cases where two methods were on a par with each other as regards these two points, I have either given both or selected the more simple one. Methods 480 SEPARATION OF BODIES. [ 151. which experience has shown to be defective or fallacious have been altogether omitted. I have endeavored to point out, as far as pos- sible ? the particular circumstances under which either the one or the other of several methods deserves the preference. Where the accuracy of an analytical method has been estab- lished already, in Section IY., no furthur statements are made on the subject here. Paragraphs of former Sections deserving par- ticular attention are referred to in parentheses. > The extension of chemical science introduces almost every day new analytical methods of every description, which are, rightly or wrongly, preferred to the older methods; the present time may therefore be looked upon in this, as in so many other respects, as a period of transition, in which the new strives more than ever to overcome and supplant the old. I make this remark to show the impossibility of always adding to the description of a method an opinion of its usefulness and accuracy, and also to point out the importance, under such circumstances, of a proper systematic arrangement. I have in this Section generally arranged the vari- ous analytical methods upon the bases of their scientific principles, firmly persuaded that this will greatly tend to facilitate the study of the science, and will lead to endeavors to apply known princi- ples to the separation of other bodies besides those to which they are already applied, or to apply new principles where experience has proved the old ones fallacious, and the methods based on them defective. I conclude these introductory remarks with the important cau- tion to the student never to look upon a separation as successfully accomplished ~before he has convinced himself that the weighed pre- cipitates, <&c., are pure and more particularly free from those bodies from which it was intended to separate them. [ 152. BASES OF GROUP I. 481 I. SEPARATION OF THE BASIC RADICALS FROM EACH OTHER. First Group. POTASSIUM SODIUM AMMONIUM (LITHIUM). 152. INDEX. The numbers refer to those in the margin. Potassium from sodium, 1, 2, 6. " ammonium, 4, 5. Sodium from potassium, 1, 2, 6. " ammonium, 3, 4, 5. Ammonium from potassium, 4, 5. " sodium, 3, 4, 5. (Lithium from the other alkalies, 7, 8, 9.) 1. Methods based upon the different degrees of Solubility in Alcohol, of Sodium Platinic Chloride, and Potassium Platinic Chloride. a. POTASSIUM FROM SODIUM. It is an indispensable condition in this method that the 1 two alkalies should exist in the form of chlorides. If, there- fore, they are present in any other form, they must be first con- verted into chlorides, which in most cases may be effected by evaporation with hydrochloric acid in excess; in the case of nitrates, the evaporation with hydrochloric acid must be repeated 4 6 times till the weight of the gently ignited mass ceases to diminish. In presence of sulphuric acid, phosphoric acid, and boracic acid, this simple method will not answer. For the methods of separating the alkalies from the two latter acids and converting them into chlorides, see 135 and 136; The presence of sulphuric acid being a circumstance of rather fre- quent occurrence, the way of meeting this contingency is given below (2). Determine the total quantity of the sodium chloride and potassium chloride* ( 97, 98), dissolve in the least quantity * Never take the weight of the alkali chlorides without convincing yourself of their purity by dissolving them in water, which should give a clear solution, and testing the solution with ammonia and ammonium carbonate, which must throw down no precipitate. It may be thought, perhaps, that a matter so simple need not be mentioned here ; still I have found that neglect in this respect is by no means uncommon. 482 SEPARATION. [ 152. of water, add to the fluid in a porcelain dish an excess of a strong aqueous solution of platinic chloride as neutral as pos- sible. Enough platinum solution should be added to convert the sodium as well as the potassium into platinochloride. It is best to use a solution of known strength and to calculate roughly how much should be added. Evaporate on the water- bath nearly to dryness (the water in the bath should never actually boil, and the sodium platinic chloride should not lose its water of crystallization), treat the residue with alcohol of from -86 to *S7 sp. gr., cover the dish with a glass plate, and allow to stand a few hours, with occasional stirring. If the super- natant fluid is not deep yellow, this is a proof that the quantity of platinic chloride used is insufficient. When the precipitate has settled, pour off the clear fluid through a filter and exam- ine the precipitate most minutely, if necessary with the aid of a microscope. If it is a heavy yellow powder (sufficiently magnified, small octahedral crystals) it is the pure potassium pla- tinic chloride.* Then transfer it best with the aid of the fil- trate to the filter, wash it with spirit of '86 to '87 sp. gr. and proceed according to 97, 3 a. (Instead of weighing the double chloride or the platinum obtained from it, you may ignite gen- tly in hydrogen, extract the potassium chloride with water, and weigh this or titrate the chlorine in it by 141, I., 5, ). If, on the contrary, white saline particles (sodium chloride) are to be seen mixed with the yellow crystalline powder, pla- tinic chloride has been wanting, the whole of the sodium chlo- ride not having been completely converted into sodium platinic chloride. In this case the precipitate in the dish must be treated with some water, till all the sodium chloride is dis- solved, a fresh portion of platinic chloride is added, the whole evaporated nearly to dryness, and the above examination repeated. The quantity of the sodium is usually estimated by subtracting from the united weight of the sodium chloride and potassium chloride the weight of the latter, calculated from that of the potassium platinic chloride. To make quite sure that the potassium has completely sep- * If small tesseral crystals are visible of .a dark orange-yellow color, and relatively large size, and appearing transparent by transmitted light, then the double chloride contains lithium platinic chloride (JENZSCH, Pogg. Ann. 104, 102). 152.] BASES OF GROUP I. 483 sirated, it is advisable to add to the filtrate some water, some more platinic chloride, and if the quantity of sodium is only small, also some- sodium chloride ; evaporate on the water-bath nearly to dry ness, at a temperature not exceeding 75 (BISCHOF), and treat the residue in the manner just described. In order to diminish the solvent action of the alcohol on the potassium platinic chloride, J ether may be now mixed with it. Should this operation again leave a small undissolved residue of potas- sium platinic chloride, it is filtered off, best on a separate filter, and first washed with alcohol and ether. As, however, this remainder of the double salt is generally impure, dissolve it on the filter with boiling water, evaporate with a few drops of pla- tinic chloride, treat the residue with alcohol, and if any potas- sium salt remains, determine it either with the principal quan- tity or by itself. If you are not satisfied with an indirect estimation of the sodium, one- of the following direct methods may be employed, a. Evaporate the filtrate till the spirit has gone off, dilute, digest the solution with small pure iron filings till the platinum is all thrown down, filter, add chlorine water till the ferrous is converted into ferric chloride, precipitate with ammo- nia, filter off the ferric hydroxide, and determine the sodium chloride in the filtrate, ft. Evaporate the filtrate, finally in a porcelain crucible, to dryness, heat the residue to low redness in a current of hydrogen, extract with water, and determine the sodium chloride in the solution. For small quantities of fluid this method will be found convenient, y. A. MITSCHEK- LICH recommends to mix the filtrate with sulphuric acid, evapo- rate to dryness, ignite the residue, extract the sodium sul- phate with water, and determine it according to 98, 1. These methods, of course, yield the sodium salt in a pure condition only when the separation of the potassium has been perfect. They present the advantage that the sodium salt is brought under one's eyes and may be tested after weighing. Should the solution contain sulphuric acid, it may be in 2 presence of hydrochloric acid or of some volatile acid, convert the alkalies first into normal sulphates ( 97, 98), and weigh them as such. For the estimation of the potassium, one of tie two following methods may be used : a. First convert the sulphates into chlorides and then pro- 484 SEPARATION. [ 152. ceed as above. For this purpose barium salts were formerly employed, or, better, an alcoholic solution of strontium chloride. The barium sulphate, however, carries down considerable quan- tities of alkali salt, and the strontium sulphate noticeable quantities ; hence the employment of these reagents, more par- ticularly barium, cannot be recommended. H. ROSE advises repeated ignition of the alkali sulphates with ammonium chloride till the weight remains constant ; this process is simple and well adapted for small quantities ; no loss of alkali need be feared if the heat is not unnecessarily raised. L. SMITH advises the use of lead salts. Dissolve the alkali sulphate, precipitate with pure neutral lead acetate, avoiding a large excess, add some alcohol, filter, precipitate the excess of lead with sulphuric acid, and evaporate to dryness with addition of sulphuric acid. This method, when carefully conducted, yields excellent results. /?. Precipitate the potash directly out of the solution of the sulphates. R. FINKENER* gives the following process: To the rather dilute solution of the salts in a capacious porcelain dish add platinic chloride in quantity more than sufficient to throw down all the potassium, evaporate on a water-bath down to a few c.c., allow to cool, add, at first in small quantities, 20 times the volume of a mixture of 2 parts absolute alcohol and 1 part ether, with stirring ; filter after a short time, and wash the precipitate with alcohol and ether till the washings are colorless. If, when the alcohol and ether are first added, a strong aqueous solution of sodium sulphate separates, add some hydrochloric acid till the fluids mix. Dry the precipitate con- sisting of potassium platinic chloride and sodium sulphate, heat with the filter in a porcelain crucible till the filter is car- bonized, then in a current of hydrogen to scarcely visible redness extract the residue with hot water, ignite the platinum in the air, weigh and calculate from the weight the quantity of potassium. The separation of potassium from sodium by platinic chloride gives results which are fully satisfactory, and at all events far more exact than any method depending on another principle ; provided that the platinum solution is pure and the operations have been carefully performed in accordance with the directions. If you have any occasion to doubt the perfect * H. ROSE, Handbuch der anal. Chem. 6 Aufl. von FINKENER, ii. 923. BASES OF GROUP I. 485 purity of the weighed double salt, you may always dissolve it in boiling water, evaporate with addition of a little platinum solution, and reweigh the salt thus purified. I. AMMONIUM FROM SODIUM. The process is conducted exactly as in a, when the alka- 3 lies are present as chlorides. See also 99, 2. If potassium also is present, the precipitate produced by platinic chloride is a mixture of ammonium platinic chloride and potassium platinic chloride ; in which case the weighed precipitate is cautiously ignited for a sufficient length of time, but not too strongly, until the ammonium chloride is expelled, the gentle ignition continued in a stream of hydrogen or with addition of oxalic acid, the residue extracted with water, a few drops of hydro- chloric acid added if oxalic acid was employed, and the potas- sium chloride in the solution determined as directed 97, 2. The weight found is calculated into potassium platinic chloride, and the result deducted from the weight of the whole precipi- tate : the difference gives the ammmonium platinic chloride. The weighing of the separated platinum affords a good control. The method is seldom employed, as that given in 2 yields more exact results. 2. Methods based upon the Volatility of Ammonium /Salts and Ammonia. AMMONIUM FROM POTASSIUM AND SODIUM. a. The salts of the alkalies to be separated contain the same 4 volatile add, and admit of the total expulsion of their water by drying at 100, without losing ammonia (e.g., the chlorides). Weigh the total quantity of the salts in a platinum crucible, and heat, with the lid on, gently at first, but ultimately for some time to faint redness ; let the mass cool, and weigh. The decrease of weight gives the quantity of the ammonium salt. If the acid present is sulphuric acid, you must, in the first place, take care to heat very gradually, as otherwise you will suffer loss from the decrepitation of ammonium sulphate ; and, in the second place, bear in mind that part of the sulphuric acid of the ammonium sulphate remains with the fixed alkali sulphates, and that you must accordingly convert them into normal salts, by ignition in an atmosphere of ammonium car- 486 SEPARATION. [ 152. bonate, before proceeding to determine their weight (compare 97 and 98). Ammonium chloride cannot be separated in this manner from fixed alkali sulphates, as it converts them, upon ignition, partly or totally into chlorides. 1}. Some one or other of the conditions given in "a " is not fulfilled. If it is impracticable to alter the circumstances by simple 5 means, so as to make the method a applicable, the fixed alkalies and the ammonium must be determined separately in different portions of the substance. The portion in which it is intended to determine the potassium and sodium is gently ignited until ammonium is completely expelled. The fixed alkalies are con- verted, according to circumstances, into chlorides or sulphates, and treated as directed in 1, 2, or 6. The ammonium is esti- mated in another portion according to 99, 3. 3. Indirect Methods. Of course, a great many of these may be devised ; but the 6 following is the only one in general use. POTASSIUM FROM SODIUM. Convert both alkalies into chlorides ( 97 and 98), and weigh as such ; estimate chlorine ( 141) ; and from the amount of this calculate the quantities of the sodium and potassium (see " Calculation of Analysis" *). The indirect method of determining sodium and potassium is applicable only in the analysis of mixtures containing toler- ably large quantities of both bases ; but where this is the case, the process answers very well, affording also, more particularly, the advantage of expedition, if the chlorine in the weighed chlorides is titrated ( 141, I., 5). Supplement to the First Group. SEPARATION OF LITHIUM FROM THE OTHER ALKALIES. Lithium may be separated from. potassium and sodium in the 7 indirect way, and by two direct methods : a. Treat the nitrates or the chlorides, dried at 120, with a mixture of equal volumes of absolute alcohol and anhydrous ether, digest at least for 24 hours, with occasional shaking (the * Other methods are given by STOLBA (Zeitschr. f . anal. Chem. 2, 397) and MOIIR (7*. 7, 173). 152.] BASES OF GROUP I. 487 salts must be completely disintegrated), decant rapidly on to a filter covering the funnel, and treat the residue again several times with smaller portions of the mixture of alcohol and ether. Determine, on the one part, the undissolved potassium and sodium salts ; on the other, the dissolved lithium salt, by dis- tilling the fluid off, and converting the residue into sulphate. This method is apt to give too much lithium, as the potassium and sodium salts, especially the chlorides, are not absolutely insoluble in a mixture of alcohol and ether. The results may be rendered more accurate by treating the impure lithium salt, obtained by distilling off the ether and alcohol, once more with alcohol and ether, with addition of a drop of nitric or hydro- chloric acid, adding the residue left to the principal residue, and then converting the lithium salt into sulphate. If the salts, which it is intended to treat with alcohol and ether, have been ignited, however so gently, caustic lithia is formed in the case of the chloride by the action of water and lithium carbonate by attraction of carbonic acid ; in that case it is neces- sary, therefore, to add a few drops of nitric or, as the case may be, hydrochloric acid, in the process of digestion. If we have to separate the sulphates, they must be converted into nitrates or chlorides before they can be subjected to the above method. This conversion is best effected by means of lead salts, see 2. Ignition with ammonium chloride does not answer for lithium sulphate, nor can the sulphuric acid be removed by barium, or strontium, as the precipitated sulphates would contain lithium (DiEHL*). >. Weigh the mixed alkalies, best in form of sulphates, and 8 then determine the lithium as phosphate according to 100. If the quantity of lithium is relatively very small, convert the weighed sulphates into chlorides (7), separate, in the first place, the principal amount of the potassa and soda by means of alco- hol ( 100), and then determine the lithium (MAYER f). c. When exact results are required, the indirect method is 9 to be preferred. Proceed first according to rt, evaporate the spirituous solution of the lithium chloride containing the remain- der of the other chlorides to dryness, heat moderately, weigh, dissolve in water, estimate the chlorine, and calculate therefrom * Annal d. Chem. u. Pharm. 121, 98. \ Ib. 98, 193. 488 SEPARATION. [ 153. the lithium and sodium or potassium. BUNSEN * also applied the method to the indirect estimation of lithium in presence of potassium and sodium by removing the silver from the filtrate, and separating the potassium with platinum, But I must here point out, that according to JENZSCH f the potassium double salt will contain lithium apparently in the form of the platino- chloride of potassium and lithium. The sulphuric acid in weighed quantities of the sulphates of lithium, and of potassium and sodium, cannot be determined as barium sulphate (see end of 7). The separation of lithium from ammonium may be effected like that of potassium and sodium from ammonium (4 and 5). Second Group. BARIUM STRONTIUM CALCIUM -MAGNESIUM. I. SEPARATION OF THE BASIC RADICALS OF THE SECOND GROUP FROM THOSE OF THE FlRST. 153. INDEX. (The numbers refer to those in the margin.) Barium from potassium and sodium, 10, 12. ammonium, 11. Strontium from potassium and sodium, 10, 13. " ammonium, 11. Calcium from potassium and sodium, 10, 14. ammonium, 11. Magnesium from potassium and sodium, 15-18. " ammonium, 11. A. General Method. 1. THE WHOLE OF THE ALKALI-EARTH METALS FROM Po- TASSIUM AND SODIUM. Principle on which the method is based : Ammonium car- 10 donate precipitates, from a solution containing ammonium chloride, only barium, strontium, and calcium. Mix the solution, in which the metals are assumed to be contained in the form of chlorides, with a sufficient quantity of * Annal. d. Chem. u. Pharm. 122,348. f Pogg. Annal. 104, 102. 153] BASES OF GROUP II. 489 ammonium chloride to prevent the precipitation of the magne- sium by ammonia ; dilute rather considerably, add some ammo- nia, then ammonium carbonate in slight excess, let the mixture stand covered for an hour in a moderately warm place, filter, and wash the precipitate with water to which a few drops of ammonia have been added. The precipitate contains the barium, strontium, and cal- cium / the filtrate the magnesium and the alkalies. So at least we may assume in cases where the highest degree of accuracy is not required. Strictly speaking, however, the solution still contains exceedingly minute traces of calcium and somewhat more considerable traces of barium, as the car- bonates of these two metals are not absolutely insoluble in a fluid containing ammonium chloride; the precipitate also may contain possibly a little ammonium magnesium carbonate. Treat the precipitate according to 154, and the filtrate in rigorous analyses as follows : Add 3 or 4 drops (but not much more) of dilute sulphuric acid, then ammonium oxalate, and let the fluid stand again for 12 hours in a warm place. If a precipitate forms, collect this on a small filter, wash, and treat on the filter with some dilute hydrochloric acid, which dis- solves the calcium oxalate, and leaves the barium sulphate undissolved. Since a little magnesium oxalate may have sepa- rated with the former, add some ammonia to the hydrochloric solution, filter after the precipitate has settled, and mix the filtrate with the principal filtrate. Evaporate the fluid containing the magnesium and the alka- lies to dryness, and remove the ammonium salts by gentle igni- tion in a covered crucible, or in a small covered dish of platinum or porcelain.* In the residue, separate the magnesium from the alkalies by one of the methods given 15 18. 2. THE WHOLE OF THE ALKALI-EARTH METALS FROM AM- 11 MONITJM. The same principle and the same process as in the separation of potassium and sodium from ammonium (4 and 5). * This operation effects also the removal of the small quantity of sulphuric acid added to precipitate the traces of barium, as sulphates of the alkalies are converted into chlorides upon ignition in presence of a large proportion of ammonium chloride. 490 SEPARATION. [ 153. B. Special Methods. SINGLE ALKALI-EARTH METALS FROM POTASSIUM AND SO- DIUM. 1. BARIUM FROM POTASSIUM AND SODIUM. Precipitate the barium with dilute sulphuric acid ( 101, 1, a), 12 evaporate the filtrate to dryness, and ignite the residue, with addition towards the end of ammonium carbonate ( 97, 1 and 98, 1). Take care to add a sufficient quantity of sulphuric acid to convert the alkalies also completely into sulphates. In exact analyses, in order to save the alkali salts adhering to the barium sulphate, remove the dry barium sulphate from the filter, heat it with a sufficient quantity of pure strong sulphu- ric acid to dissolve it completely, allow to cool, dilute largely, collect the barium sulphate (now almost absolutely pure) on the first filter, ignite, and weigh. Evaporate the filtrate in a plati- num dish, drive off the sulphuric acid, and estimate the traces of the alkalies. This method is, on account of its greater accuracy, prefer- able to the one in A, in cases where the barium has to be sepa- rated only from one of the two fixed alkalies ; but if both alka- lies are present, the other method is more convenient, since the alkalies are then obtained as chlorides. 2. STRONTIUM FROM POTASSIUM AND SODIUM. Strontium may be separated from the alkalies like barium, 13 by means of sulphuric acid ; but this method is not preferable to the one in 10, in cases where the choice is permitted (comp. 102). 3. CALCIUM FROM POTASSIUM AND SODIUM. Precipitate the calcium with ammonium oxalate ( 103, 2, 14 Z>, a), evaporate the filtrate to dryness, and determine the alka- lies in the ignited residue. In determining the alkalies, dis- solve the residue, freed by ignition from the ammonium salts, in water, filter if necessary, acidify the filtrate, according to cir- cumstances, with hydrochloric acid or sulphuric acid, and then evaporate to dryness ; this treatment of the residue is neces- sary, because ammonium oxalate partially decomposes chlorides of the alkali metals upon ignition with formation of alkali car- bonates, except in presence of a large proportion of ammonium 153.] BASES OF GROUP II. 491 chloride. The results are still more accurate than in A, except where ammonium oxalate has been used, after the precipitation by ammonium carbonate, to remove the minute traces of lime from the filtrate. 4. MAGNESIUM FROM POTASSIUM AND SODIUM.* a. Methods based upon the sparing solubility of Magnesium Hydroxide in Water. a. Make the solution as neutral as possible, and free from 15 ammonium salts (it is a matter of indifference whether the mag- nesium and alkali metals are present as sulphates, chlorides, or nitrates), add baryta-water as long as a precipitate forms, heat to boiling, filter, and wash the precipitate with boiling water. The precipitate contains the magnesium as hydroxide. Dis- solve it in hydrochloric acid, precipitate the barium with sul- phuric acid, and then the magnesium as ammonium-magnesium phosphate ( 104, 2). The alkalies, which are contained in the solution, according to circumstances, as chlorides, nitrates, or caustic alkalies, are separated from the barium as directed in 10 or 12. LIEBIG, who w T as tjie first to employ this method, proposes crystallized barium sulphide as precipitant. The method is not very exact, as magnesium is somewhat more soluble in solutions of alkali salts than in water. On this account the weighed alkali salt must always be tested for magnesium, and the latter determined if required. fi. Precipitate the solution with a little pure milk of lime, 16 boil, filter, and wash. Separate the calcium and magnesium in the precipitate according to 24 ; the calcium and the alkalies in the filtrate according to 10 or 14. This method may be em- ployed when magnesium has to be removed from a fluid con- taining calcium and alkalies, provided the alkalies alone are to be determined. Minute quantities of magnesium also in this case remain with the alkali salt from the cause mentioned in a. y. Evaporate the solution of the chlorides (which must 17 contain no other acids) to dryness, and if ammonium chloride is present, ignite ; warm the residue with a little water (this will dissolve it with the exception of some magnesium oxide, which separates). Add mercuric oxide shaken up with water, * The methods a, a and ft, are suitable for the separation of magnesium from lithium. 492 SEPARATION. [ 153. evaporate to dryness on the water-bath with frequent stirring, dry thoroughly, ignite with increasing temperature till all the resulting mercuric chloride is volatilized. (Avoid inhaling the fumes.) There is no need to continue the ignition until the whole of the mercuric oxide is expelled ; on the contrary, part of it may be filtered off together with the magnesium oxide, and subsequently volatilized upon the ignition of the latter. Treat the residue with small quantities of hot water, filter off rapidly, and wash the magnesium oxide with hot water, using small quantities at a time, and not continuing the operation unnecessarily. The solution contains the alkalies in form of chlorides. This method, proposed by BERZELIUS, gives satis- factory results, and, as far as my experience goes, is the best of those given under a. Take care to add the mercuric oxide only in proper quantity, and always test the alkali chlorides for mag- nesium, a trace of which will generally be found. 1). Method based on the Precipitation of the Magnesium as Ammonium Magnesium Carbonate. Mix the solution of sulphates, nitrates, or chlorides (it must 18 be very concentrated) with an excess of a concentrated solution of sesquicarbonate of ammonia in water and ammonia (230 grm. of the salt, 360 c.c. solution of ammonia sp. gr. -96, and water to 1 litre). After twenty-four hours filter off the precipitate (MgCO 3 - (NH 4 ) 2 CO 3 + 4H 2 O), wash it with the solution of am- monia and ammonium carbonate used for the precipitation, dry, ignite strongly and for a sufncienfrlength of time, and weigh the magnesium oxide. Evaporate the filtrate to dryness (keeping the heat at first under 100, expel the ammonium salts, and de- termine the alkalies as chlorides or sulphates. When sodium alone is present the results are tolerably satisfactory. In the presence of potassium the ignited magnesium oxide must be extracted with water, before weighing, as it contains an appre- ciable quantity of potassium carbonate ; the washings are to be added to the principal filtrate. This last measure is unneces- sary in the absence of potassium. The magnesium is always a little too low. Mean error y^Vo (F. G. SCHAFFGOTSCH,* H. WEBER f). * Pogg. Annal. 104, 482. f Vierteljahresschrift f. prakt. Pharm. 8, 161. 154.] BASES OF GROUP II. 493 II. SEPARATION OF THE BASIC RADICALS OF THE SECOND GROUP FROM EACH OTHER. 154. INDEX. (The numbers icfer to those in the margin.) Barium from strontium, 20, 23, 32. calcium, 22, 23, 27, 32. " magnesium, 19, 21. Strontium from barium, 20, 23, 32. calcium, 26, 30, 31. magnesium, 19, 21. Calcium from barium, 20, 22, 23, 27, 32. strontium, 26, 30, 31 magnesium, 19, 24, 25, 28, 29. Magnesium from barium, 19, 21. strontium, 19, 21. calcium, 19, 24, 25, 28, 29. A. General Method. THE WHOLE OF THE ALKALI-EARTH METALS FROM EACH OTHER. Proceed as in 10. The magnesium is precipitated from the 19 filtrate as ammonium magnesium phosphate. The precipitated carbonates of barium, strontium, and calcium are dissolved in hydrochloric acid, and the bases separated as directed in 20. The traces of magnesium, which may be present in the ammo- nium carbonate precipitate, are obtained by evaporating the fil- trate from the strontium or calcium sulphate to dryness, taking up the residue with water, and precipitating the solution with sodium phosphate and ammonia. B. Special Methods. 1. Methods based upon the Insolubility of Barium Silicqfluoride. BARIUM FROM STRONTIUM AND FROM CALCIUM. Mix the neutral or slightly acid solution with hydrofluosili- 20 cic acid* in excess, add one third of the volume of alcohol of 81 sp. gr., let the mixture stand twelve hours, collect the pre- cipitate of barium silicofluoride on a weighed filter, wash with * If not kept in a gutta-percha bottle it should be freshly prepared. 494 SEPARATION. [ 154. a mixture of equal parts of water and alcohol until the wash- ings cease to show even the least trace of acid reaction (but no longer), and dry at 100. Precipitate the strontium or calcium from the filtrate by dilute sulphuric acid ( 102, 1, a, and 103, 1). The results are satisfactory. For the properties of barium silicofluoride, see 71. If both strontium and calcium are pres- ent, the sulphates are weighed, and then separated according to 26, or they are converted into carbonates ( 132, II,, b), and separated according to 31 or 30. 2. Methods based upon the Insolubility of Barium Sulphate or Strontium Sulphate, as the case may be, in Water and in Solution of Sodium T hiosulphate. a. BARIUM AND STRONTIUM FROM MAGNESIUM. Precipitate the barium and strontium with sulphuric acid 21 ( 101, 1, a and 102, 1, a\ and the magnesium from the fil-_ trate with ammonia and sodium ammonium phosphate ( 104, 2). b. BARIUM FROM CALCIUM. Mix the solution with hydrochloric acid, then with highly 22 dilute sulphuric acid (1 part acid to 300 water), as long as a pre- cipitate forms ; allow to deposit, and determine the barium sul- phate as directed 101, 1, a. Concentrate the washings by evaporation and add them to the filtrate, neutralize the acid with ammonia, and precipitate the calcium as oxalate ( 103, 2, b, a). The method is principally to be recommended when small quantities of barium have to be separated from much cal- cium. If we have to separate calcium sulphate from barium sulphate, the salts may (in the absence of free acids) be treated repeatedly with a solution of sodium thiosulphate at a gentle heat. The barium sulphate remains undissolved, the calcium sulphate dissolves. The calcium is precipitated from the fil- trate by ammonium oxalate (DIEHL*). 3. Method based upon the different deportment with Alkali Carbonates of Barium Sulphate on the one hand, and Strontium and Calcium Sulphates on the other. BARIUM FROM STRONTIUM AND CALCIUM. Digest the three precipitated sulphates for twelve hours at 23 * Journ. f. prakt. Chem. 79, 430. 154.] BASES OF GROUP II. 495 the common temperature (15 20), with frequent stirring, with a solution of ammonium carbonate, decant the fluid on to a filter, treat the residue repeatedly in the same way. wash finally with water, and in the still moist precipitate, separate the undecomposed barium sulphate by means of cold dilute hydrochloric acid from the strontium and calcium carbonates formed. To hasten the separation you may boil the sulphates for some time with a solution of potassium (not sodium) car- bonate, to which ^ the amount of the carbonate, or more, of potassium sulphate has been added. By this' process, also, the strontium and calcium sulphates are decomposed, the barium sulphate remaining unacted on. If the basic metals are in solu- tion, the above solution of potassium carbonate and sulphate is added in excess at once, and the whole boiled. The precipitate, consisting of barium sulphate and strontium and calcium car- bonates, is to be treated as above with cold hydrochloric acid (H. ROSE*). 4. Methods based on the Insolubility of Calcium /Sul- phate m Alcohol. CALCIUM FROM MAGNESIUM. a. Remove water and free hydrochloric from a solution of 24 the chlorides by evaporation, dissolve the residue in strong (but not absolute) alcohol, add a slight excess of pure strong sulphu- ric acid, digest in the cold, allow to stand for some hours, trans- fer the precipitate consisting of calcium sulphate and some magnesium sulphate to a filter, wash away the acid thoroughly with nearly absolute alcohol, and then continue the washing with alcohol sp. gr. *96 '95 till a few drops of the washings give no residue on evaporation. Weigh the calcium sulphate according to 103, 1. Evaporate the alcohol from the filtrate, and determine the magnesium according to 104, 2. The method is in itself not new, but A. CmzYNSKi,t adopting the precautions here given, has obtained excellent results, even in the presence of phosphoric acid. b. SMALL QUANTITIES OF CALCIUM FROM MUCH MAGNESIUM. 25 Convert into neutral sulphates, dissolve the mass in water, and add alcohol, with constant stirring, till a slight permanent tur- Pogg. Annal. 95, 286, 299, 427. f Zeitschr. f. anal. Chem. 4, 348. 496 SEPARATION. [ 154. bidity is produced, Wait a few hours and then filter, wash the precipitated calcium sulphate with alcohol which has been diluted with an equal volume of water, and determine it after 103, 1, a (in which case the weighed sulphate must be tested for magnesium), or dissolve the precipitate in water containing hydrochloric acid and separate the calcium from the small quan- tity of magnesium possibly coprecipitated according to 28 (SCHEERER*). 5. Methods based on the Insolubility of Strontium and Barium Sulphates in solution of Ammonium Sulphate. STRONTIUM FKOM CALCIUM. If the mixture is soluble, dissolve in the smallest quantity 26 of water, add about 50 times the quantity of the substance of ammonium sulphate dissolved in four times its weight of water, and either boil for some time with renewal of the water that evaporates and addition of a very little ammonia (as the solu- tion of ammonium sulphate becomes acid on boiling), or allow to stand at the ordinary temperature for twelve hours. Filter and wash the precipitate, which consists of strontium sulphate and a little ammonium strontium sulphate, with a concentrated solu- tion of ammonium sulphate, till the washings remain clear on addition of ammonium oxalate. The precipitate is cautiously ignited, moistened with a little dilute sulphuric acid (to convert the small quantity of strontium sulphide into sulphate), reig- nited and weighed. The highly dilute filtrate is precipitated with ammonium oxalate, and the calcium determined according to 103, 2, J, a. If you have the solid sulphates to analyze, they are very finely powdered and boiled with concentrated solu- tion of ammonium sulphate with renewal of the evaporated water and addition of a little ammonia. Results very close, e.g., 1-048 Sr(lSrO 3 ) 2 instead of .1-053, and -497 CaC0 3 , instead of -504 (H. RosEj). BARIUM may be separated FROM CALCIUM in the same way. 27 6. Methods based upon the Insolubility of Calcium Oxalate in Ammonium Chloride and in Acetic Acid. CALCIUM FROM MAGNESIUM. a. Mix the properly diluted solution with sufficient ammo- 28 * Annal. d. Chem. u. Pharm. 110, 237. $ Pogg. Annal. 110, 296. 154.] BASES OF GROUP II. 497 nium chloride to prevent the. formation of a precipitate by ammonia, which is added in slight excess ; add ammonium oxa- late as long as a precipitate forms, then a further portion of the same reagent, about sufficient to convert the magnesium also into oxalate (which remains in solution). This excess is abso- lutely indispensable to insure complete precipitation of the cal- cium, as calcium oxalate is slightly soluble in magnesium chlo- ride not mixed with ammonium oxalate (Expt. Xo. 92). Let the mixture stand twelve hours, decant the supernatant clear fluid, as far as practicable, from the precipitated calcium oxa- late, mixed with a little magnesium oxalate, on to a filter, wash the precipitate once in the same way by decantation, then dis- solve in hydrochloric acid, add water, then ammonia in slight excess, and a little ammonium oxalate. Let the fluid stand until the precipitate has completely subsided, then pour on to the previous filter, transfer the precipitate finally to the latter, and proceed exactly as directed 103, 2, 5, a. The first filtrate contains by far the larger portion of the magnesium, the second the remainder. Evaporate the second filtrate, acidified with hydrochloric acid, to a small volume, then mix the two fluids, and precipitate the magnesium with sodium ammonium phos- phate (HXaXH 4 )PO 4 ,*as directed 104, 2. If the quantity of ammonium salts present is considerable, the estimation of the magnesium is rendered more accurate by evaporating the fluids in a large platinum or porcelain dish to dryness, and igniting the residuary saline mass, in small portions at a time, in a smaller .platinum dish, until the ammonium salts are expelled. The residue is then treated with hydrochloric acid and water, warmed, allowed to cool, and rendered just alkaline with ammo- nia. If enough ammonium chloride is present, no magnesium hydroxide will fall down, but occasionally small flocks of silica or alumina are to be seen. Filter them off and finally precipi- tate with ammonia and (KN~aKH 4 )PO 4 . If the precipitate pro- duced by ammonia is at all considerable, dissolve it in hydro- chloric acid, evaporate the solution on a water-bath to dryness, treat the residue with hydrochloric acid and water, render alka- line with ammonia, filter, and add the filtrate to the principal solution. * This is preferable to sodium phosphate as a precipitant, see MOKR, Zeitschr. f. anal. Chem. 12, 36. 498 SEPARATION. [ 154. Numerous experiments have convinced me that this method, which is so frequently employed, gives accurate results only if the foregoing instructions are strictly complied with. It is only in cases where the quantity of magnesium present is relatively small that a single precipitation with ammonium oxalate may be found sufficient (comp. Expt. No. 93*). Z>. In the case of calcium and magnesium phosphates, dis- 29 solve in the least possible quantity of hydrochloric acid, add ammonia until a copious precipitate forms ; redissolve this by addition of acetic acid, and precipitate the calcium with an excess of ammonium oxalate. To determine the magnesium, precipitate the nitrate with ammonia and (HNaNH 4 )PO 4 . As free acetic acid by no means prevents the precipitation of small quantities of magnesium oxalate, the precipitate contains some magnesium, and as calcium oxalate is not quite insoluble in acetic acid, the nitrate contains some calcium ; these two sources of error compensate each other in some measure. In accurate analysis, however, these trifling admixtures of magnesium and calcium are afterwards separated from the weighed precipi- tates of calcium carbonate or oxide and magnesium pyrophos- phate respectively. 7. Method based upon the Insolubility of Strontium Nitrate in Alcohol and Ether. STRONTIUM FROM CALCIUM (after STROMEYER). Digest the perfectly dry nitrates in a closed flask with abso- 30 lute alcohol, to which an equal volume of ether should be added (H. ROSE). Filter off the undissolved strontium nitrate in a covered funnel, wash with the mixture of alcohol and ether, dis- solve in water, and determine as strontium sulphate ( 102, 1). Precipitate the calcium from the filtrate by sulphuric acid. The results are satisfactory. 8. Indirect Method. STRONTIUM FROM CALCIUM. Determine both bases first as carbonates or oxides, precipi- 31 * Further experiments will be found in Zeitschr. f . anal. Chem. 7, 310. Com- pare also WITTSTEIN, Zeitschr. f. anal. Chem. 2, 318, and COSSA, Ib. 8, 141. According to HAGER, Ib. 9, 254, the precipitate of calcium oxalate will be free from magnesium if filtered off immediately ; however, I fear that a little calcium might in this case be left in solution. 154.] BASES OF GROUP III. 499 fating them either with ammonium carbonate or oxalate ( 102, 103) ; then estimate the amount of carbonic acid in them, and calculate the amount of strontium and calcium as directed in " Calculation of Analyses." The determination of the carbonic acid may be effected by fusion with vitrified borax ( 139, II., y Barium Carbonate. FERRIC IRON, ALUMINIUM, AND CHROMIUM, FROM ALL OTHER BASIC RADICALS OF THE FOURTH GROUP. Mix the sufficiently dilute solution of the chlorides or 64 nitrates, but not sulphates, which must contain a little free , acid,* in a flask, with a moderate excess of barium carbonate diffused in water ; cork, and allow to stand some time in the cold, with occasional shaking. The ferric iron, aluminium, and chromium are completely separated,! whilst the other basic radicals remain in solution, with the exception perhaps of traces of cobalt and nickel, which will generally fall down with the precipitate. This may be prevented, at least as regards nickel, by addition of ammonium chloride to the fluid to be precipi- tated (SCHWARZENBERG^:). Decant, stir up with cold water, allow to deposit, decant again, filter, and wash with cold water. The precipitate contains, besides the precipitated metals, barium car- bonate ; and the filtrate, besides the non-precipitated metals, a barium salt. If ferrous iron is present, and it is wished to separate it by this method from ferric iron, etc., the air must be excluded during the whole of the operation. In that case, the solution of the substance, the precipitation, and the washing by decantation, are effected in a flask (A y fig. 68), through which carbonic acid is transmitted (d). The washing water, boiled free from air, and cooled out of con- tact of air (preferably in a current of carbonic acid), is poured in through a funnel tube (c), and the fluid drawn off by means of * If there is much free acid, the greater part of it must first be saturated with sodium carbonate. f The separation of the chromium requires the most time, t Annal. d. Chem. u. Pharm. 97, 216. Fig. 68. 514 SEPARATION. [ 160. a movable syphon (5) ; all the tubes are fitted air-tight into the cork ; they are smeared with tallow. 2. Method based upon the Precipitation of the Metals of the Fourth Group by Sodium Sulphide or Ammo- nium Sulphide, from Alkaline Solution effected with the aid of Tartaric Acid. ALUMINIUM AND CHROMIUM FROM THE METALS or THE FOURTH GROUP. Mix the solution with pure normal potassium tartrate,* then 65 with pure solution of soda or potassa until the fluid has cleared again ; f add sodium sulphide as long as a precipitate forms, allow it to deposit until the supernatant fluid no longer exhibits a greenish or brownish tint ; decant, stir the precipitate up with water containing sodium sulphide, decant again, transfer the precipitate, which contains all the metals of the fourth group, to a filter, wash with water containing sodium sulphide, and separate the metals as directed in B. Add to the filtrate potassium nitrate, and evaporate to dry ness ; fuse the residue in a platinum dish, and separate the aluminium from the chromic acid formed as directed 1 57". If you have merely to separate aluminium from the metals of the fourth group, it is better, after addition of potassium tartrate, to supersaturate with ammonia, add ammonium chloride, and precipitate in a flask with ammonium sulphide. When the precipitate has set- tled it is filtered off and washed with water containing ammo- nium sulphide. The filtrate is evaporated in a platinum dish with sodium carbonate and potassium nitrate to dryness, fused, and the aluminium determined in the residue. B. Special Methods. 1. Methods based upon the Solubility of Aluminium Hydroxide in Caustic Alkalies. a. ALUMINIUM FROM FERROUS AND FERRIC IRON, AND SMALL QUANTITIES OF MANGANESE (but not from nickel and cobalt). Mix the hydrochloric solution with sodium carbonate or 66 * Tartaric acid often contains aluminium, therefore this is best made from the acid tartrate. f Chromium and zinc cannot be obtained together in alkaline solution (CHANCEL, Compt. rend. 43, 927; Journ. f. prakt. Chem. 70, 378). ,^ 160.] BASES OF GROUP IV. 515 pure potash till the greater part of the free acid is neutralized, and pour the solution gradually into excess of pure potasli heated nearly to boiling in a platinum or silver dish, stirring all the while. Porcelain does not answer so well, and glass should on no account be used. The iron, if present as ferric chloride, separates ,as ferric hydroxide, while the aluminium remains in solution as alkali aluminate. Hydrated protosesquioxide of iron is more easy to wash than ferric hydroxide, hence when much iron is present it is better to reduce a part by cautiously adding sodium sulphite and heating, so that when the solution is added to the boiling potash a black granular precipitate may be formed. The iron precipitate is sure to contain alkali, and must be dissolved in hydrochloric acid, the solution boiled witli nitric acid if necessary, and reprecipitated with ammonia. To the alkaline filtrate add a few drops of hydrochloric acid. If the potash was present in sufficient excess the precipi- tate will redissolve readily on stirring. Continue adding hydro- chloric acid till in excess, boil with a little potassium chlorate (to destroy traces of organic matter), concentrate by evapora- tion, and throw down the aluminium according to 105, a. The above is the best method of procedure, but it is always to be feared that small quantities of aluminium will be retained by the iron precipitate. ~b. ALUMINIUM FROM FERROUS AND FEKRIC IRON, COBALT, AND NlCKEL. Fuse the oxides with potassium hydroxide in a silver era- 67 cible, boil the mass with water, and filter the alkaline fluid, which contains the aluminium, from the oxides, which are free from aluminium, but contain potassa (H. ROSE). 2. Methods based on the different behavior of Am- monia or Ammonium Carbonate in the presence of Chlo- ride with solutions of certain basic radical*. a. ALUMINIUM AND FERRIC IRON FROM COBALT AND NICKEL. Ferric iron may be completely separated from these metals 68 by mixing the hot solution with ammonium chloride, and then with excess of ammonia, digesting for several hours, washing the precipitate, redissolving in hydrochloric acid, reprecipitating with ammonia, and repeating the operation a third time. Nickel 516 SEPARATION. [ 160. and cobalt are to be precipitated from the filtrate after concen- tration to a small volume, as directed in 110, 1, &, /?. In separating iron and aluminium from nickel and cobalt, it is well to substitute ammonium carbonate for ammonia, so as to insure the complete precipitation of the aluminium. J. MANGANESE FROM NICKEL AND ZINC. The solution should be slightly acid and contain ammonium 69 chloride. Precipitate the manganese as white carbonate with ammonium carbonate, allow to settle in a warm place, filter through a thick paper, if necessary double, wash with hot water, dry the precipitate and convert it into protosesquioxide by igni- tion with access of air. This excellent method was proposed by TAMM,* and has given me good results, f It is not adapted to the separation of cobalt from manganese, as the former is partly precipitated with the latter. 3. Method 'based upon the different deportment of neutralized Solutions at boiling heat. a. FERRIC IRON FROM MANGANESE, NICKEL AND COBALT, AND OTHER STRONG BASIC METALS, AFTER HERSCHEL, J ScHWARZ- ENBERG, AND MY OWN EXPERIMENTS. Mix the dilute solution largely with ammonium chloride (at 70 least 40 of NH 4 C1 to 1 of MnO,NiO, &c.), add ammonium carbonate in small quantities, at last drop by drop and in very dilute solution, as long as the precipitated iron redissolves, which takes place promptly at first, but more slowly towards the end. As soon as the fluid has lost its transparency, without showing, however, the least trace of a distinct precipitate in it, and fails to recover its clearness after standing some time in the cold, but, on the contrary, becomes rather more turbid than other- wise, the reaction may be considered completed. When this point has been attained, heat slowly to boiling, and keep in ebullition for a short time after the carbonic acid has been entirely expelled. The iron separates as a basic ferric salt, which rapidly settles, if the solution was not too concentrated. Pour off the hot fluid through a filter and wash by decantation combined with filtration with boiling water containing a little * Chem. News, 26, 37. ' \ Annal. de Chim. et de Phys. 49, 306. f Zeitschr. 1 anal. Chem. 11, 425. Anna!, d. Chem. u. Pharm. 97, 216. 160.] BASES OF GKOUP IV. 517 ammonium chloride. It is well to redissolve the precipitate in hydrochloric acid, and throw down the iron with ammonia. The first filtrate should be mixed with excess of ammonia. If a small portion of ferric hydroxide is thrown down here, filter it off, dissolve in hydrochloric acid, precipitate with ammonia and thus free the small quantity of iron entirely from the strong basic metals ; if, on the other hand, a larger quantity of iron is thrown down, this is a sign that the operation has been con- ducted improperly, and the hydrochloric solution of the precipi- tate must be reprecipitated as above. The fluid should not contain more than 2 or 3 grm. of iron in the litre, and should be tolerably free from sulphuric acid, as when this is present it is impossible to hit the exact point of saturation. 4. Method based on the behavior of the Acetates at a foiling heat. FERRIC IKON AND ALUMINIUM FROM MANGANESE, ZINC, COBALT, NICKEL, AND FERROUS IRON. The metals should be present in the form of chlorides. The 71 solution should be in a flask. If much free acid is present first nearly neutralize with sodium or ammonium carbonate ; the solution should remain clear, but if there is much ferric chloride it should be of a deep red color. Add a concentrated solution of neutral sodium or ammonium acetate, not in large excess, and boil for a short time long-continued boiling would make the precipitate slimy. When the lamp is removed the precipitate should settle rapidly, leaving the supernatant fluid clear. Wash the precipitate immediately by decantation and filtration with boiling water containing a little sodium or ammonium acetate. In very particular analyses it would be well after washing the precipitate a little to redissolve it in hydrochloric acid and reprecipitate. In separating ferric from ferrous iron KEICHARDT* recom- mends a slight addition of ammonium chloride or of sodium chloride to prevent oxidation of the ferrous salt. The precipitate of basic ferric acetate or basic aluminium acetate is best dissolved in hydrochloric acid, in order to precipi- tate the basic metals from this solution again by ammonia. * Zeitsclir. f . anal. Chem. 5, 64 518 SEPARATION. [ 160 This method is more suitable to the separation of ferric iron or ferric iron and aluminium from the strong basic metals than to the separation of aluminium alone. It is a good method, and is very generally used. [The results obtained by this method depend greatly on the proper adjustment of free acetic acid to the volume of the solu- tion which is boiled. The solution at this point may contain about four per cent, (by volume) of acetic acid sp. gr. l'044r (JEWETT*). If too little acetic is present, zinc, manganese, nickel, and cobalt are precipitated in notable quantity along with the iron. If too much is present the precipitation of iron is incomplete. The operator may control the amount of acid within narrow limits by proceeding as follows. Add the alkali carbonate to the cold and preferably concentrated solution until a slight precipitate forms which no longer redissolves in four or five minutes with occasional shaking, but imparts a turbidity to the deep red solution ; HC1 is then added without further delay, slowly, drop by drop, until the fluid, though still dark, becomes clear. Next the amount of acetic acid required to form four per cent, of the final volume is added, then sodium acetate (about ten times as much of the crystallized salt as there is iron present, or more if but little iron is present). Dilute now to the final volume, which should amount to at least 100 c.c. per -1 grm. iron and heat to boiling. After boiling two or three minutes only, allow the iron precipitate to settle. Pour the clear liquid through a filter, then bring the precipitate upon the filter at once and wash as above directed. The iron pre- cipitate contains no zinc and but an inappreciable trace of man- ganese. Small quantities of cobalt and still more nickel will, however, be precipitated with the iron. When these two metals are present in considerable quantity a repetition of the process is indispensible when accuracy is required. Coprecipitation of nickel is lessened but not entirely prevented by presence of ammonium chloride, f In carrying out the process according to this plan great care must be taken in the preliminary neutralization with alkali carbonate to leave as little free mineral acid as possible without formation of a permanent precipitate, otherwise this free acid * Am. Cliem. Jour. I. 251. f Loc. tit. 160.] BASES OF GKOUP IV. 519 will liberate enough acetic acid from the eodium acetate to prevent (with that intentionally added) the precipitation of iron in a form easy to wash. In separating large quantities of iron from small quantities of manganese the addition of 2 or 3 per cent, of acetic acid will secure a separation satisfactory enough for most purposes (e.g. in iron and iron ores), and the danger that the acetic acid present may accidentally exceed the proper limit will of course be lessened.] 5. Method 'based on the different behavior of the Suc- cinates. FERRIC IRON (AND ALUMINIUM) FROM ZINC, MANGANESE, XlCKEL, AND COBAT. The solution should contain no considerable quantity of sul- 72 phuric acid. If acid, as is usually the case, add ammonia till the color is reddish brown, then sodium or ammonium acetate (H. HOSE) till the color is deep red, finally precipitate with neutral alkali succinate at a gentle heat, and when cool filter the ferric succinate from the solution which contains the rest of the metals. Wash the precipitate first with cold water, then with warm ammonia, which removes the greater part of the acid, leaving it darker in color. Dry and ignite, moisten with a little nitric acid, and ignite again. With proper care the sepa- ration is complete, and especially to be recommended when a relatively large quantity of iron is present. The method may also be used in the presence of aluminium. The latter falls down completely with the iron (E. MITSCHERLICH, PAGELS*). 6. Methods based upon the different deportment of the several Sulphides with Acids, or of Add Solutions with Hydrogen Sulphide. a. Zixc FROM ALUMINIUM AND MANGANESE. The solution of the acetates, which must be free from in- 73 organic acids, and must contain a sufficient excess of acetic acid, is precipitated with hydrogen sulphide, which throws down the zinc only ( 108, b). The metals are usually most readily obtained in the form of acetates, by converting them into * Jahresber. v. KOPP u. WILL. 1858, 617. 520 SEPARATION. [ 160. sulphates, and adding a sufficient quantity of barium acetate. Hydrogen sulphide is then conducted, without application of heat, into the unfiltered fluid, to which, if necessary, some more acetic acid has been added. The precipitate, which consists of a mixture of zinc sulphide and barium sulphate, is washed with water containing hydrogen sulphide. It is then heated with dilute hydrochloric acid, the solution filtered, and the zinc in the filtrate determined as directed 108, a. The other metals a-re determined in the fluid filtered from the zinc sul- phide, after removal of the barium by precipitation. BftuNNERf has proposed a modification of this process, especially for the separation of zinc from nickel. b. ZINC FKOM NICKEL, COBALT, AND MANGANESE. To the hydrochloric solution add sodium carbonate till a 74 permanent precipitate just forms, and then a drop or two of hydrochloric acid to redissolve the precipitate. Now pass hydrogen sulphide till the precipitate of zinc sulphide ceases to increase. Add a few drops of a very dilute solution of sodium acetate, and continue passing the gas for some time. When all the zinc is precipitated, allow to stand for twelve hours, filter, wash with hydrogen sulphide water, and determine the nickel and cobalt in the filtrate (SMITH and BRUNNER*) A good method ; compare KLAYE and DEus.f The method is also adapted for separating zinc from manganese. [Precautions. Bear in mind that Zn can be precipitated from solutions containing free HC1, but only in case the amount of the latter is very small.:): When ZnS is precipi- tated the amount of HC1 set free may be sufficient to prevent complete precipitation of the Zn. Addition of sodium acetate converts this HC1 into NaCl, and allows the formation of ZnS to continue. Care must be taken not to add enough sodium acetate to convert all the HC1 into NaCl, for in that case NiS and CoS will be precipitated.] c. ZINC FROM NICKEL COBALT, AND MANGANESE. [Zinc can be precipitated by hydrogen sulphide from a cold 75 solution containing a sufficient amount of free acetic acid to * Dingler's polyt. Journ. 150, 369; Chem. Centralbl. 1859, 26. . f Zeitschr. f. anal. Chem. 10, 200. \ STOKER and ELIOT, Mem. Am. Acad. Arts and Sciences, viii. 95. 160.] BASES OF GEOUP IV. 521 prevent precipitation of nickel and cobalt. To effect separation by this means* add sodium or potassium carbonate to the solu- tion till it is slightly alkaline. If a large quantity of any free volatile acid is present it may be previously removed by evaporation. Dissolve the . precipitate produced by the alkali carbonate (without filtering) in acetic acid, and add a large quantity more of acetic acid. Precipitate the zinc by passing H 2 S through the cold moderately diluted solution. Wash the sulphide of zinc with water to which hydrogen sulphide and a little ammonium acetate has been added. The zinc sulphide should not be dark-colored. This will only be the case when not enough acetic is present to prevent precipitation of nickel or cobalt. Cobalt and nickel may be best separated from the filtrate by evaporating till the greater part of the acetic acid is removed, then adding some ammonium chloride and ammonia to slight alkaline reaction, evaporating further till the reaction becomes acid, heating finally to boiling, and passing hydrogen sulphide through the solution, as directed in 110, 1, b, ft. A good method.] 7. Different deportment of the several Oxides with Hydrogen Gas at a red heat. FERRIC IRON FROM ALUMINIUM AND CHROMIUM. [Precipitate with ammonia, heat, filter, ignite, and weigh. 76 Triturate, and weigh off a portion in a porcelain crucible. Ignite to redness in a stream of hydrogen gas as long as water forms (about one hour). Then ignite over the blast-lamp in a current of mixed hydrogen and hydrochloric acid gases. This leaves aluminium and chromium oxides in a state of purity ; the iron volatilizes as ferrous chloride, and is determined by the loss. (Method of RIVOT and DEVILLE modified.) This method is further modified by COOKED who by means of a platinum boat in a platinum tube ignites the mixed oxides over a Bunsen lamp half an hour in a current of hydrogen, then alternately in HC1 gas and hydrogen till the light color shows that iron has been removed.] * ROSE and FINKENER, Anal. Chem. ii. 129 and 143. f Zeitschr. f. anal. Chem. 6, 226. SEPARATION [g 160. 8. Methods based upon the different capacity of the several Oxide to be converted ~by Oxidizing Agents into higher Oxides, or ly Chlorine into higher Chlorides. a. CHROMIUM FROM ALL THE METALS OF THE FOURTH GROUP, AND FROM ALUMINIUM. Fuse the oxides with potassium nitrate and sodium carbon- 77 ate (coinp. 51), boil the mass with water, add a small quantity of alcohol, and heat gently for several hours. Filter and deter- mine in the filtrate the chromium as directed 130, and in the residue the metals of the fourth group. The following is the theory of this process : the oxides of zinc, cobalt, nickel, iron, and partly that of manganese, separate upon the fusion, whilst, on the other hand, potassium manganate (perhaps also some ferrate) and chromate are formed. Upon boiling with water, part of the manganic acid of the potassium manganate is con- verted into permanganic acid at the expense of the oxygen of another part, which is reduced to the state of binoxide ; the latter separates, whilst the potassium salts are dissolved. The addition of alcohol, with the application of a gentle heat, effects the decomposition of the potassium manganate and permanga- nate, manganese binoxide being separated. Upon filtering the mixture, we have therefore now the whole of the chromium in the filtrate as alkali chromate, and all the oxides of the fourth group on the filter. Aluminium, if present, will be found partly in the residue, partly as alkali aluminate in the filtrate ; proceed with the latter according to 51. If you have to deal with the native compound of sesqui- oxide of chromium with protoxide of iron (chromic iron) the above method does not answer. This substance may be decom- posed by fusion with cryolite and potassium disulphate.* b. The radicals to be separated may be in the form of a 78 solution of their salts ; nearly neutralize the solution, add sodium acetate, heat and convert the chromium into chromic acid by passing chlorine, compare 53. If ferric iron and aluminium are present, they will separate during boiling by the action of the sodium acetate, while the chromic acid and any zinc will remain in solution. If manganese, nickel, and cobalt are present, the method loses its simplicity ; the manganese is precipitated as hydrated peroxide with a portion of the cobalt, * GIBBS and CLARK, Am. Jour. Sci. II ser. 48, 198. 160.] BASES OF GKOUP IV. 523 almost the whole of the nickel and some zinc, while the chromic acid remains in solution with the principal amount of the zinc and the rest of the cobalt and nickel (W. GIBBS). 9. Method based upon the different deportment of the Nitrites. COBALT FROM NICKEL, ALSO FROM MANGANESE AND ZINC. The separation of cobalt as tripotassium cobaltic nitrite was 79 recommended first by FISCHER,* afterwards by A. STROMEYER.+ GEXTH and GIBBS,^: H. ROSE, FR. GAUHE,[ and myself (com- pare last edition of this work). The results are quite satisfac- tory both in presence of much cobalt and little nickel, and in the presence of little cobalt and much nickel ; but the process is peculiarly good for the latter case. However, it is absolutely necessary that barium, strontium, and calcium should be absent, as in their presence nickel is thrown down as triple nitrite of nickel, potassium, and alkali-earth metal (KUNZEL, O. L. ERD- MANN^T). The best way of proceeding is as follows : The solution (from which any iron must first be separated) is evapo- rated to a small bulk, and then, if much free acid is present, neutralized with potassa. Then add a concentrated solution of potassium nitrite (previously neutralized with acetic acid and filtered from any flocks of silica and alumina that may have separated) in sufficient quantity, and finally acetic acid, till any flocculent precipitate that may have formed from excess of potassa has redissolved and the fluid is decidedly acid. Allow it to stand at least for twenty-four hours in a warm place, take out a portion of the supernatant fluid with a pipette, mix it with more potassium nitrite, and observe whether a further precipita- tion takes place in this after long standing. If no precipitate is formed the whole of the cobalt has fallen clown, otherwise the small portion must be returned to the principal solution, some more potassium nitrite added, and after long standing the same test applied. Thus, and thus alone, can the analyst be sure of the complete precipitation of the cobalt. Finally filter and treat the precipitate according to 111, 1, d. Boil the filtrate * Pogg. Anna}. 72, 477. } Ib. 104, 309. f Annal. d. Chem. u. Phann. 96, 218. Pogg. Annal. 110, 412. | Zeitschr. f . anal. Chem. 5, 74. y Zeitschr. f . anal. Chem. 3, 161 ; Journ. f . prakt. Chem. 97, 387. 524 SEPAKATION. [ 160. with excess of hydrochloric acid, precipitate with potash, redis- solve the precipitate in hydrochloric acid, throw down the nickel according to 110, 1, , a or /?, as sulphide, and then convert into metal. In this manner alone can the nickel be obtained pure, as the original nitrate contains so much alkali salt and also generally alumina and silica. [When nickel and cobalt are obtained in the form of sulphides in the process of separation from other metals, the mixed sulphides may be converted into metals without previous separation, by the same process that is described for nickel sulphide 110, 1, 5, and 2. Cobalt may then be separated from a nitric acid solution of the two metals and nickel estimated by difference.] 10. Methods based upon the different deportment with Potassium Cyanide. a. ALUMINIUM FROM ZINC, COBALT, AND NICKEL. Mix the solution with sodium carbonate, add potassium 80 cyanide in sufficient quantity, and digest in the cold, until the precipitated zinc, cobalt, and nickel carbonates are redissolved. Filter off the undissolved aluminium precipitate, wash, and remove the alkali which it contains, by resolution in hydro- chloric acid and reprecipitation by ammonia (FRESENIUS and HAIDLEN *). b. COBALT FROM NICKEL. LIEBIG'S method, f which depends upon the conversion of 81 the cobalt into potassium cobalticyanide, and of the nickel into double nickel and potassium cyanide, has been carefully studied in my laboratory by FR. GAUHE.^: It has been thus found that boiling the solution containing potassium cyanide and hydro- cyanic acid (LIEBIG'S first method) does not completely convert the double cobalt and potassium cyanide first formed into . potassium cobalticyanide, but that passing chlorine (LIEBIG'S second method) effects a ready and thorough conversion. The method then gives a very excellent separation, and is more par- ticularly to be recommended where the quantity of nickel is small in proportion to the cobalt. We proceed as follows, * Annal. d. Chem. u. Pharm. 43, 129. f lb., 65, 244, and 87, 128. \ Zeitschr. f. anal. Chem. 5, 75. 160.] BASES OF GROUP IV. 525 taking a hydrochloric solution of the metals : Remove the greater part of the free acid by evaporation or neutralize it by potash, add pure potassium cyanide till the precipitate first formed has redissolved ; then add more cyanide, dilute, boil for sorhe time or not, as you like, pass chlorine through the cold fluid, adding potash or soda occasionally, so that the fluid may remain strongly alkaline to the end. Bromine may be used instead of chlorine, and indeed is far more convenient. In the course of an hour the whole of the nickel will have precipi- tated as black hydrate of the sesquioxide. Having taken out a portion and satisfied yourself of this by addition of a further quantity of chlorine or bromine, filter, and wash with boiling water. The precipitate always retains alkali, and must be redis- solved in hydrochloric acid, and estimated according to 110, 1, a, or 2. As regards the cobalt, it is most convenient to estimate it by difference. But if you wish to make a direct estimation, it will be advisable, in consequence of the large quantity of salts present in solution, first to evaporate to dryness with excess of hydrochloric acid, to take up the residue with a little water, and to heat in a large platinum dish, with the addition of excess of pure concentrated sulphuric acid till the greater part of the sulphuric acid has escaped. The red mass, consisting principally of alkali disulphate, is then treated with water, and the cobalt estimated according to 111, 1, c. c. COBALT FROM ZINC. Add to the solution of the two metals, which must contain 82 Borne free hydrochloric acid, common potassium cyanide (pre- pared by LIEBIG'S method), in sufficient quantity to redissolve the precipitate of cobalt cyanide and zinc cyanide which forms at first ; then add a little more potassium cyanide, and boil some time, adding occasionally one or two drops of hydrochloric acid, but not in sufficient quantity to make the solution acid. After cooling add some chlorine or bromine, and digest for some time to complete the conversion of the cobalt into potassium cobalticyanide. Mix the solution with hydrochloric acid in an obliquely placed flask, and boil until the zinc cobalticyanide which precipitates at first is redissolved, and the hydrocyanic acid completely expelled. Add solution of soda or potassa in 526 SEPARATION. [ 160. excess, and boil until the fluid is clear ; the solution may now be assumed to contain all the cobalt as potassium cobalticyanide, and all the zinc as a compound of oxide of zinc and alkali. Precipitate the zinc by hydrogen sulphide ( 108). Filter, and determine the cobalt in the filtrate as in 81. The process is ' simple and the separation complete (FRESENIUS and HAIDLEN). 11. Methods based upon the Volumetric Determina- tion of one of the Metals , and the finding of the other from the difference. a. FERRIC IRON FROM ALUMINIUM, Precipitate both metals with ammonia ( 105, a, and 113, 83 1). Dissolve the weighed residue, or an aliquot part of it, by digestion with concentrated hydrochloric acid, or by fusion with bisulphate of potassa and treatment with water containing sul- phuric acid, and determine the iron volumetrically as directed 113, 3, a or ~b. The alumina is found from the difference. This is an excellent method, and to be recommended more par- ticularly in cases where the relative amount of iron is small. If you have enough substance, it is of course much more con- venient to divide the solution, by weighing or measuring, into 2 portions, and determine in the one the sesquioxide of iron -j- alumina, in the other the iron. 1). FERRIC IRON FROM FERROUS IRON (ZiNC AND NICKEL). oc. Determine in a portion of the substance the total amount 84 of the iron as sesquioxide, or by the volumetric way. Dissolve another portion by warming with sulphuric acid in a flask through which carbonic acid is conducted, to exclude the air ; dilute 'the solution, and determine the protoxide of iron volu- metrically ( 112, 2, a). The difference gives the quantity of the sesquioxide. Or, dissolve the compound in like manner in hydrochloric acid, and determine the ferric chloride with sodium thiosulphate according to 113, 3, ~b. In this case the difference gives the ferrous iron. If it is desired to determine the ferrous chloride in the hydrochloric solution directly, it will be well to use PENNY'S method ( 112, 2, &). If the compound in which the ferrous and ferric basic radicals are to be estimated is decomposed by acids with difficulty, heat it with a mixture of 4 parts sulphuric acid and 1 part water (or with hydrochloric 160.] BASES OF GROUP IV. 527 acid) in a sealed tube for 2 hours at 210 (MrrscHERLicHf). Or, if this is not enough, fuse it with borax (1 part mineral, 5 to 6 vitrified borax) in a small retort, connected with a flask containing nitrogen (produced by combustion of phosphorus in air) ; an atmosphere of carbonic acid is less suitable. Triturate the fused mass with the glass, and dissolve in boiling hydro- chloric acid in an atmosphere of carbonic acid (HERMANN v. KOBELL). Or, as will generally be the best way, you may dis- solve the substance in a mixture of hydrofluoric and hydro- chloric or hydrofluoric and sulphuric acids with exclusion of FIG. 69. air. COOKE * dissolves silicates in a mixture of sulphuric and hydrofluoric acids in an atmosphere of steam and carbonic acid, and determines the ferrous iron by means of potassium per- manganate. Fig. 69 exhibits his apparatus. To the sides of a copper water-bath are attached three tubes. The tube on the left con- nects with a Mariotte's flask to maintain the water at a constant level. The upper tube on the right connects with a carbonic acid gas generator, while the third tube carries off any overflow of water to the sink. On the cover of the water-bath close to the rim is a circular groove, which receives the edge of an inverted glass funnel. When the apparatus is in use this groove is kept full of water by the spray from the boiling liquid, and thus forms a perfect * Am. Jour. Science, 3d ser., 44, 347. - Jour. f. prnkt, Chem., 81. 108 and 83. 455 528 SEPAEATION. [ 160. water-joint ; but in order to secure this result the bath must be kept nearly full of water, and holes for the ready escape of the steam and spray should be provided in the rings, which cover the bath and adapt it for vessels of various sizes. By this arrangement the funnel may be kept filled with an atmosphere of steam or of carbonic acid for an indefinite period. More- over, we can either pour in fresh quantities of solvent, or we can stir up the material, in the vessel within, introducing a tube-funnel or stirrer through the spout of the covering funnel. The finely pulverized substance (-J to 1 grm.) is placed in a large platinum crucible. Upon it pour a mixture of dilute sulphuric acid (sp. gr. 1*5) with as little hydrofluoric acid as experience may show is required to dissolve or decompose the substance, stirring up the material with a platinum spatula. The crucible is next transferred to the water-bath, the covering funnel put in place, water poured into the groove, the interior filled with carbonic acid, and the lamp lighted. As soon as the water boils, the supply of carbonic acid is stopped ; and if the water-level has been properly adjusted, the apparatus will take care of itself, the groove will be kept full of water, arid the interior of the funnel full of steam. If the materials cake on the bottom of the crucible, as is not unfrequently the case when a large amount of insoluble sulphate is formed, the lamp may be removed, the apparatus again filled with carbonic acid, and the contents of the crucible stirred up by aid of a stout platinum wire about two inches long, fused to the end of a glass tube. Anything adhering to the rod can easily be washed back into the crucible by directing the jet from the wash-bottle down the throat of the covering funnel. The lamp may then be replaced, the current of carbonic acid interrupted, and the process of digestion continued . When the decomposition is complete, the current of carbonic acid gas is re-established, the lamp extin- guished, and the air-tube of the Mariotte's flask raised until its lower end is above the level of the overflow. A slow current of water is thus caused to flow through the bath, which soon cools down the whole apparatus. The crucible may now be removed, its contents washed into a beaker-glass, and the solu- tion diluted with pure water until the volume is about 500 c.c., when the amount of ferrous iron present can be determined with a solution of potassium permanganate in the usual way. 161.] BASES OF GROUP IV. 529 Many iron compounds in fine powder are completely decom- posed by boiling a few minutes only with the mixed acids above mentioned. If a preliminary experiment shows this to be the case, a simple and satisfactory way of effecting a solu- tion is to boil the substance with the solvent acids in a platinum crucible of 40 to 50 c.c. capacity, provided with a well-fitting concave cover. By watching the escaping vapor, one y Ammonia or Ammonium Carbonate. COPPER FROM BISMUTH. Mix the (nitric acid) solution with ammonium carbonate 116 in excess, and warm gently. The bismuth separates as car- bonate, whilst the copper carbonate is redissolved by the excess of ammonium^ carbonate. As the precipitate, however, gen- erally retains a little copper, it is necessary to redissolve it, after washing, in nitric acid, and precipitate again with ammo- nium carbonate ; the same operation must be repeated a third time if required. Some solution of ammonium carbonate may be added to the water used for washing. Apply heat to the filtrate that the ammonium carbonate may volatilize, acidify cautiously with hydrochloric acid, and determine the copper as cuprous sulphide ( 119, 3). The oxide of bismuth thus * Pogg. Aniial. 110, 430. f Journ. f. prakt. Chem. 74, 345. 550 SEPARATION. [ 163. obtained is quite copper-free, but a little bismuth passes into the copper solution, hence the separation does not give such exact results as that in 114 (H. ROSE*). 6. Method based on the Precipitation of the Copper as Cuprous Sulphocyanate. COPPER FROM CADMIUM (and the metals of Groups I. IY., comp. 101). . Precipitate the copper according to 119, 3, Z>, as cuprous 117 sulphocyanate (RIVOT), and the cadmium from the filtrate as sulphide. Results good (H. ROSE). Palladium may also be separated from copper in this way Y. Method based upon the different deportment of the Chromates. BISMUTH FROM CADMIUM. Precipitate the bismuth as directed 120, 2. The filtrate 118 contains the whole of the cadmium. Concentrate by evapora- tion, and then precipitate the cadmium by the cautious addi- tion of sodium carbonate, as directed 121, 1, a (J. LowE,J "W. PEARSON). The results given are satisfactory. 8. Method based upon the different deportment of the Sulphides with Acids. a. MERCURICUM FROM SILVER, BISMUTH, COPPER, CADMIUM, AND (but less well) FROM LEAD. Boil the thoroughly washed precipitated sulphides with 119 perfectly pure moderately dilute nitric acid. The mercuric sulphide is left undissolved, the other sulphides are dissolved. No chlorine may be present, and it is necessary that the mer- curic sulphide should be pure, that is, free from finely divided mercury, which, as is well known, is precipitated when mer- curous salts are treated with hydrogen sulphide. G. v. RATH|| employed this method, which is so universally used in qualita- tive analysis; with perfect success for the separation of mer- cury from bismuth. * Pogg. Annal. 110, 430. f Annal. d. Chem. u. Pharm. 140, 144; Zeitschr. f. anal. Chem. 5, 403. t Journ. f. prakt. Chem. 67, 439. | Pogg. Anual. 96, 322. Phil. Mag. 11, 204. 163.] BASES OF GKOUP V. 551 b. COPPER FROM CADMIUM. Boil the well- washed precipitate of the sulphides with 120 dilute sulphuric acid (1 part concentrated acid and 5 parts water), and, after some time, filter the undissolved copper sul- phide, to be determined according to 119, 3, from the solu- tion containing the whole of the cadmium (A. "W. HOFMANN*). 9. Methods based upon the Volatility of some of the Metals, Oxides, Chlorides, or Sulphides at a high Tem- perature. a. MERCURY FROM SILVER, LEAD, COPPER (in general from the metals forming non- volatile chlorides). Precipitate with hydrogen sulphide, collect the precipi- 121 tated sulphides on a weighed filter, dry at 100, weigh, and mix uniformly. Introduce an aliquot part into the bulb d, FIG. 70. (fig. TO), pass a slow stream of chlorine gas, and apply a gen- tle heat to the bulb, increasing this gradually to faint redness. To ensure complete absorption it is well to have another small U-tube connected with e. The excess of chlorine escaping from the latter during the operation may be conducted into a flue or into a carboy containing moist slaked lime. First sul- phur chloride distils over, which decomposes with the water in e (p. 463) ; then the mercuric chloride formed volatilizes, condensing partly in e, partly in the hind part of d. Cut off * Annal. d. Chem. u. Pharm. 115, 286. 552 SEPARATION. [ 163. that part of the tube, rinse the sublimate with water into , and mix the contents of the latter with the water in the second U-tube (not shown by the figure). Mix the solution with excess of ammonia, warm gently till no more nitrogen is evolved, acidify with hydrochloric acid, and then determine in the fluid filtered from the sulphur, which may still remain undissolved, the mercury as directed 118, 3. If the residue consists of silver chloride alone, or lead chloride alone, you may' weigh it at once ; but if it contains several metals, you must reduce the chlorides by ignition in a stream of hydrogen, and dissolve the reduce^ metals in nitric acid, for their ulte- rior separation. Bear in mind that, in presence of lead, the sulphides and the chlorides must be heated gently ^ in the chlo- rine and hydrogen respectively, otherwise some lead chloride might volatilize. In alloys or mixtures of oxides the mercury may usually be determined with simplicity from the 'loss on ignition in the air or in hydrogen. b. BISMUTH FROM SILVER, LEAD, AND COPPER. The separation is effected exactly in the same way as that 122 of mercury from the same metals (121). The method is more especially convenient for the separation of the metals in alloys. Care must be taken not to heat too strongly, as other- wise lead chloride might volatilize ; nor to discontinue the application of heat too soon, as otherwise bismuth would remain in the residue. AUG. VOGEL * gives 360 to 370 as the best temperature. Put water containing hydrochloric acid in U-tubes, which serve as receivers (fig. 70), and determine the bismuth therein according to 120. 10. Precipitation of one Meted in the Metallic State lyy another or the lower Oxide of another, a. LEAD FROM BISMUTH. Precipitate the solution with ammonium carbonate ( 116, 123 1, a and 120, 1, a\ wash the precipitated carbonates, and dissolve in acetic acid, in a flask ; place a weighed rod of pure lead in the solution, and nearly fill up with water, so that the * Zeitscbr. f. anal. Chem. 13, 61. 163.] BASES OF GROUP V. 553 rod may be entirely covered by the fluid ; close the flask, and let it stand for about 12 hours, with occasional shaking. Wash the precipitated bismuth off from the lead rod, collect on a filter, wash, and dissolve in nitric acid ; evaporate the solution, and determine the bismuth as directed 120. Deter- mine the lead in the filtrate as directed 116. Dry the leaden rod, and weigh ; subtract the loss of weight which the rod has suffered in the process from the amount of the lead obtained from the filtrate (ULLGRE'N *). PATERA f recom- mends precipitating from dilute nitric solution, washing the precipitated bismuth first with water, then with alcohol, trans- ferring to a small filter, drying and weighing. If it is feared that the finely divided bismuth has undergone oxidation, it is well to fuse it with potassium cyanide ( 120, 4). 11. Separation of Silver by Cupellation. CUPELLATION was formerly the universal method of deter- 124 mining SILVER in alloys with COPPER, LEAD, etc. The alloy is fused with a sufficient quantity of pure lead to give to 1 part of silver 16 to 20 parts of lead, and the fused mass is heated, in a muffle, in a small cupel made of compressed bone-ash. Lead and copper are oxidized, and the oxides absorbed by the cupel, the silver being left behind in a state of purity. One part by weight of the cupel absorbs the oxide of about 2 parts of lead ; the quantity of the sample to be used in the experi- ment may be estimated accordingly. This method is only rarely employed in laboratories ; : I have given it a place here, however, because it is one of the safest processes to deter- mine very small quantities of silver in alloys. 12. Methods depending on the Volumetric Estima- tion of one Metal. a. COPPER OF CUPROUS COMPOUNDS IN PRESENCE OF CUPRIC COMPOUNDS.] Dissolve the substance, if necessary in a current of carbonic 125 * BERZELIUS' Jahresber. 31, 148. f Zeitschr. f. anal. Chem. 5, 226. $ For details of this process consult "Bodemann and Kerl's Assaying," translated by GOODYEAR ; or "Notes on Assaying," by P. DE RICKETTS. Compare MALAGUTI and DUROCHER, Comp. rend. 29, 689; DINGLER, 115, 376. Also W. HAMPE, Zeitschr. f. anal. Chem. 11, 221. | The method of COMMAILLE (Comp. rend. 56, 309) can no longer be relied 554 SEPARATION. [ 164, acid, in hydrochloric acid, and add ferric chloride. A volu- metric determination of the amount of iron reduced to fer- rous salt affords a basis for calculating the amount of copper present originally as a cuprous compound. Or if a known quantity of ferric chloride is used, a determination of the iron remaining in the state of a ferric salt suffices equally well. It. SILVER IN PRESENCE OF LEAD AND C/OPPER. Small quantities of silver may be estimated by PISANI'S method, 115, II. Sixth Group. GOLD PLATINUM TIN ANTIMONY (ANTIMONIC ACID) ARSENIOUS ACID AKSENIC ACID. I. SEPARATION OF THE METALS OF THE SIXTH GROUP FROM THOSE O 1 ? THE FIRST FlVE GROUPS. 164. INDEX. (The numbers refer to those in the margin.) - Gold from the metals of Groups I. III., 126, 131. Group IV., 126, 129, 131. silver, 129, 147. mercury, 129, 142. lead, 129, 152. copper, 129, 131. " bismuth, 129, 131, 152. " cadmium, 129, 131. Platinum from the metals of Groups I. III., 126, 132. Group IV., 126, 130, 132. silver, 130, 147. mercury, 130, 142. lead, 130. " copper, 130, 132. bismuth, 130, 132. cadmium, 130, 132. Tin from the metals of Groups I. and II., 126, 135, 141. Group III., 126, 135. upon, since STAS has shown that the finely divided silver thrown down by ammoniacal solution of cuprous chloride dissolves largely in ammonia with access of air. 164.] METALS OF GROUP VI. 555 Tin from zinc, 126, 128, 133, 135. manganese, 126, 128, 135. nickel and cobalt, 126, 128, 133, 135, 140. iron, 126, 128. silver, 127, 128, 133, 140. mercury, 127, 128, 133. lead, 127, 128, 133, 140. copper, 127, 128, 133, 135, 180. bismuth, 127, 128. cadmium, 127, 128, 133, 135. Antimony from the metals of Groups I. and II., 126. Group III., 126. zinc, 126, 128, 134. manganese, 126, 128. nickel and cobalt, 126, 128, 134, 139, 140. iron, 126, 128, 138. silver, 127, 128, 134, 140. mercury, 127, 128, 134, 136, 148. lead, 127, 128, 134, 140, 150. copper, 127, 128, 134, 138, 140, 151. bismuth, 127, 128. cadmium, 127, 128, 134. Arsenic from the metals of Group I., 126, 145, 146. " . " II., 126, 137, 145, 146. III., 126, 144, 145. zinc, 126, 128, 137, 143, 145, 146. manganese, 126, 128, 137, 143, 144, 145, 146. nickel and cobalt, 126, 128, 137, 139, 140, 143, 144, 145, 146. iron, 126, 128, 137, 138, 143, 144, 145. silver, 127, 128, 137, 140, 145. mercury, 127, 128, 145, 148. lead, 127, 128, 137, 140, 145, 149. copper, 127, 128, 137, 138, 140, 143, 144, 145, 151. bismuth, 127, 128, 137, 145. cadmium, 127, 128, 137, 144, 145. A. General Methods. 1. Method based upon the Precipitation of Metals of the Sixth Group from Acid Solutions by Sulphuretted Hydrogen. ALL METALS OF THE SIXTH GROUP FROM THOSE OF THE FIRST FOUR GROUPS. Conduct into the acid* solution hydrogen sulphide in 126 excess, and filter off the precipitated sulphides (corresponding to the oxides of the sixth group). * Hydrochloric acid answers best as acidifying agent. 556 SEPARATION. [ 164. The points mentioned 96, <*, /?, and 7, must also be attended to here. As regards 7, antimony and tin are to be inserted between cadmium and mercury, in the order of metals there given. With respect to the particular conditions required to secure the proper precipitation of certain metals of the sixth group, I refer to Section IY. I have to remark in addition : a. That hydrogen sulphide fails to separate arsenic acid from zinc, as, even in presence of a large excess of acid, the whole or at least a portion of the zinc precipitates with the arsenic (WOHLER). To secure the separation of the two bodies in a solution, the arsenic acid must first be converted into arsenious acid, by heating with sulphurous acid, before the hydrogen sulphide is conducted into the fluid. ft. That in presence of antimony, tartaric acid should be added, as otherwise the sulphide of antimony will contain chloride ; and that sulphide of antimony, when thrown down from a boiling solution by hydrogen sulphide, becomes black after a time, and so dense that it is deposited like sand, whereby the filtration and washing are much facilitated (S. P. SCHAFELER *). 2. Method based upon the Solubility of the Sulphides of the JHetals of the Sixth Group in Sulphides of ilie Alkali Metals. a. THE METALS OF GROUP VI. (with the exception of Gold and Platinum) FROM THOSE OF GROUP V. Precipitate the acid solution with hydrogen sulphide, pay- 127 ing due attention to the directions given in Section IV. under the heads of the several metals, and also to the remarks in 126. The precipitate consists of the sulphides of the metals of Groups V. and VI. Wash, and treat at once with yellow ammonium sulphide in excess. (It is usually best to spread out the filter in a porcelain dish, add the ammonium sulphide, cover with a large watch-glass, and place on a heated water- bath. Unnecessary exposure to air should be avoided.) Add some water, filter off the clear fluid, treat the residue again * Berichte der deutschen chem. Gesellsch. 1871, 279. I have myself con firmed these observations. 164.] METALS OF GROUP VI. 557 with ammonium sulphide, digest a short time, repeat the same operation, if necessary, a third and fourth time, filter, and wash the residuary sulphides of Group V . with water contain- ing ammonium sulphide. If stannous sulphide is present, some flowers of sulphur must be added to the ammonium sul- phide, unless the latter be very yellow. In presence of copper, the sulphide of which is a little soluble in ammonium sulphide, sodium sulphide should be used instead. However, this sub- stitution can be made only in the absence of mercury, since the sulphide of that metal is soluble in sodium sulphide. Add to the alkaline filtrate, gradually, hydrochloric acid in small portions, until the acid predominates ; allow to subside, and then filter off the sulphides of the metals of the sixth group, which are mixed with sulphur. If a solution contains much arsenic acid in presence of small quantities of copper, bismuth, &c., it is convenient to precipitate these metals (together with a very small amount of arsenious sulphide) by a brief treatment with hydrogen sul- phide. Filter, extract the precipitate with ammonium sulphide (or potassium sulphide), acidify the solution obtained, mix it with the former filtrate containing the principal quantity of the arsenic, and proceed to treat further with hydrogen sul- phide ( 127, 4, I). b. THE METALS OF GROUP VI. (with the exception of Gold and Platinum) FROM THOSE OF GROUPS IV. AND V. a. Neutralize the solution with ammonia, add ammonium 128 chloride, if necessary, and then yellow ammonium sulphide in excess ; digest in a closed flask, for some time at a moderate heat ; and then proceed as in 127. Repeated digestion with fresh quantities of ammonium sulphide is indispensable. On the filter, you have the sulphides of the metals of Groups IV and V. Wash with water containing ammonium sulphide. In presence of nickel, this method offers peculiar difficul- ties ; traces of mercuric sulphide, too, are liable to pass into the filtrate. In presence of copper (and absence of mer- cury), soda and sodium sulphide are substituted for ammonia and ammonium sulphide.* * The accuracy of this method has been called in question by BLOXAM (Quart. Journ. Chem. Soc. 5, 119). That chemist found that ammonium sulphide fails 558 SEPARATION. [ 164. /3. In the analysis of solid compounds (oxides or salts), it is in most cases preferable to fuse the substance with 3 parts of dry sodium carbonate and 3 of sulphur, in a covered porce- lain crucible. When the contents are completely fused, arid the excess of sulphur is volatilized, the mass is allowed to cool, and then treated with water, which dissolves the sulphosalts of the metals of the sixth group, leaving the sulphides of Groups IY. and Y. undissolved. By this means, even ignited stannic oxide may be readily tested for iron, &c., and the amount of the admixture determined (H. ROSE). The solu- tion of the sulphosalts is treated as in 127. In the presence of copper, traces of the sulphide may be dissolved with the sulphides of Group YI. Occasionally a little ferrous sulphide dissolves, coloring the solution green. In that case add some ammonium chloride, and digest till the solution has turned yellow. Instead of the mixture of sodium carbonate and sul- phur you may also use already prepared hepar sulphuris, or, as FROHDE* says, you may fuse the substance with 4 or 5 parts of sodium thiosulphate. B. Special Methods. 1. Methods based upon the Insolubility of some Metals of the Sixth Group in Acids. a. GOLD FROM METALS OF GROUPS IY. AND Y. IN ALLOYS. a. Boil the alloy with pure nitric acid (not too concen- 129 trated), or, according to circumstances, with hydrochloric acid. The other metals dissolve, the gold is left. The alloy must be reduced to filings, or rolled out into a thin sheet. If the alloy were treated, with concentrated nitric acid, and at a tem- perature below boiling, a little gold might dissolve in conse- quence of the co-operation of nitrous acid. In the presence of silver and lead, this method is only applicable when they to separate small quantities of stannic sulphide from large quantities of mercuric sulphide or cadmium sulphide (1 : 100); and that more especially the separation of copper from tin and antimony (also from arsenic) by this method is a failure, as nearly the whole of the tin remains with the copper. The latter statement I cannot confirm, for Mr. Lucius, in my laboratory, has succeeded in separating copper from tin by means of yellowish sodium sulphide completely; but it is indispensable to digest three or four times with sufficiently large quantities of the solvent, as stated in the text. * Zeitschr. f . anal. Chem. 5, 405. 164.] METALS OF GROUP VI. 559 amount to more than 80 per cent., since otherwise they are not completely dissolved. Alloys of silver and gold contain- ing less than 80 per cent, of silver are therefore fused with 3 parts of lead, before they are treated with nitric acid. The residuary gold is weighed ; but its purity must be ascertained, by dissolving in cold dilute nitrohydrochloric acid, not in con- centrated hot acid, as silver chloride also is soluble in the latter. In the presence of silver, a small quantity of its chloride is usually obtained here. If it can be weighed, it should be reduced and deducted. At the Mint Conference held at Vienna in 1857, the fol- lowing process was agreed upon for the mints in the several states of Germany. Add to 1 part of gold, supposed to be present, 2^ parts of pure silver ; wrap both the alloy and the silver in a paper together, and introduce into a cupel in which the requisite amount of lead is just fusing.* After the lead . has been absorbed,f the button is flattened by hammering or rolling, then ignited and rolled. The rolls are treated first with nitric acid of 1*2 sp. gr., afterwards with nitric acid of 1-3 sp. gr., rinsed, ignited, and weighed.^ Even after boiling again with nitric acid of 1*3 sp. gr., they retain -75 to *001 of silver which will remain as chloride if the rolls are treated with cold dilute aqua regia (H. ROSSLER, loc. cit.). ft. Heat the alloy (previously filed or rolled) in a capacious platinum dish with a mixture of 2 parts pure concentrated sulphuric acid and 1 part water, until the evolution of gas has ceased and the sulphuric, acid begins to volatilize ; or fuse the alloy with potassium disulphate (H. ROSE). Separate the gold from the sulphates of the other metals, by treating the mass with water which should finally be boiling. It is advisable to repeat the operation with the separated gold, and ultimately * If the weighed sample, say '25 grm., contains 98-92 gold, 3 grm. of lead are required; if 92-87'5, 4 grm. ; if 87 '5-75, 5 grm. ; if 75-60, 6 grm.; if 60-35, 7 grm. ; if less than 35, 8 grm. f A small quantity of gold from one to three thousandths is always lost in cupellation. The loss increases with the amount of lead, and is also depen- dent on the proportion of silver to gold. The more silver present the less is the loss of gold. In large buttons the loss is less than in small ones (H. ROSSLER, Ding, polyt. Journ. 206, 185; Zeitschr. f. anal. Chem. 13, 87). \ Kunst-und Gewerbeblatt f. Baiern, 1857, 151; Chem. Centralbl. 1857, 307 Polyt. Centralbl. 1857, 1151, 1471, 1639. 560 SEPARATION. [ 164. test the purity of the latter. In presence of lead this method is not good. y. The methods given in a and /? may be united, i.e., the cupelled and thinly-rolled rnetal may be first warmed with nitric acid of 1'2 sp. gr., then thoroughly washed, the gold boiled 5 minutes with concentrated sulphuric acid, washed again, and ignited (MASCAZZINI, BUGATTI). #. PLATINUM FKOM METALS OF GROUPS IY. AND Y. IN ALLOYS. The separation is effected by heating the alloy in filings 130 or foil with pure concentrated sulphuric acid, with addition of a little water, or by fusing with potassium disulphate (129, ft) ; but not with nitric acid, as platinum in alloys will, under cer- tain circumstances, dissolve in that acid. 2. Method based upon the Separation of Gold in the metallic state. GOLD FKOM ALL METALS OF GROUPS I. Y., with the excep- tion of LEAD, MERCURY, AND SILVER. Precipitate the hydrochloric acid solution with oxalic acid 131 as directed 123 5, y^ or with ferrous sulphate, 123, J, <*, and filter off the gold when it has completely separated. Take care to add a sufficient quantity of hydrochloric acid after the reduction to insure solution of any oxalates. In the presence of copper the addition of hydrochloric acid does not suffice, since the coprecipitated cupric oxalate will dissolve with diffi- culty in this acid. E. PURGOTTI* recommends in this case, after precipitation, adding potash cautiously to the boiling hot fluid till it is neutral, and then if necessary some normal potassium oxalate. Double oxalate of copper and potash will be formed which dissolves with a blue color. The gold after washing will now be pure. 3. Method based upon the Precipitation of Pla- tinum as Potassium Platinic, or Ammonium Platinic Chloride. PLATINUM FROM THE METALS OF GROUPS IY. AND Y., with the exception of MERCURY IN MERCUROUS COMPOUNDS, LEAD, AND SILVER. Precipitate the platinum with potassium chloride or 132 * Zeitschr. f . anal. Chem. 9, 128. 164.] METALS OF GROUP VI. 561 ammonium chloride as directed 124, and wash the precipi- tate thoroughly with alcohol. The platinum prepared from the precipitated ammonium or potassium salt is to be tested after being weighed, to see whether it yields any metal (especially iron) to fusing potassium disulphate. 4. Methods based upon the Separation of Oxides insoluble in Nitric Add. a. TIN FROM METALS OF GROUPS IY. AND Y. (not from Bismuth, Iron, or Manganese*) IN ALLOYS. Treat the finely divided alloy, or the metallic powder 133 obtained by reducing the oxides in a stream of hydrogen with nitric acid, as directed 126, 1, a. The filtrate contains the other metals as nitrates. As stannic oxide is liable to retain traces of copper and lead and iron, you must, in an accurate analysis, test an aliquot part of it for these bodies, and determine their amount as directed 128, ft. BRUNNER recommends the following course of proceeding, by which the presence of copper in the tin may be effectually guarded against. Dissolve the alloy in a mixture of 1 part of nitric acid, 4 parts of hydrochloric acid, and 5 parts of water ; dilute the solution largely with water, and heat gently. Add crystals of sodium carbonate until a distinct precipitate has formed, and boil. (In presence of copper, the precipitate must, in this operation, change from its original bluish-green to a brown or black tint.) When the fluid has been in ebulli- tion some 10 or 15 minutes, allow it to cool, and then add nitric acid, drop by drop, until the reaction is distinctly acid ; digest xhe precipitate for several hours, when it should have acquired a pure white color. The stannic oxide thus obtained is free from copper ; but it may contain some iron, which can be removed as directed in 128, ft. Before the stannic oxide can be considered pure, it must be tested also for silicic acid, as it frequently contains traces of this substance. To this end, an aliquot part' is fused in plati- * If the alloy of tin contains bismuth or manganese, there remains with the stannic oxide, bismuth trioxide or manganese sesquioxide, which cannot be extracted by nitric acid; if it contains iron, on the contrary, some stannic oxide always dissolves with the iron, and cannot be separated even by repeated evapo- ration (H. ROSE, Pogg. Annal. 112, 169, 170, 172). 562 SEPARATION. [ 164. mim with 3 4 parts of sodium and potassium carbonate, the fused mass boiled with water, and the solution filtered ; hydro- chloric acid is then added to the filtrate, and, should silicic acid separate, the fluid is filtered off from this substance. The tin ' is then precipitated by hydrogen sulphide, and the silicic acid still remaining in the filtrate is determined in the usual way ( 140). If hydrochloric acid has produced a precipitate of silicic acid, the last filtration is effected on the same filter (KHITTEL*). b. ANTIMONY FROM THE METALS OF GROUPS IV. AND Y. IN ALLOYS (not from Bismuth, Iron and Manganese). Proceed as in 133, filter off the precipitate, and convert it 134 by ignition into antimony tetroxide according to 125, 2. Results only approximate, as a little antimony dissolves. Alloys of antimony and lead, containing the former metal in excess, should be previously fused with a weighed quantity of pure lead (VARRENTRAppf). 5. Methods based on the Precipitation of Tin in Stannic Salts by Normal Salts (e.g., Sodium Sulphate) or by Sulphuric Acid. TIN FROM THE METALS OF GROUPS I., II., Ill, ; ALSO FROM MANGANESE, ZINC, NICKEL AND COBALT, COPPER, CADMIUM (GOLD). Precipitate the hydrochloric acid solution, which must 135 contain the tin entirely as stannic chloride, according to 126, 1, b, by ammonium nitrate or sodium sulphate (LOWENTHAL), or by sulphuric acid, which, H. ROSE says, answers equally well. Alloys are always treated as follows : First, oxidize by digestion with nitric acid ; when no more action takes place r evaporate the greater portion of the .nitric acid in a porcelain dish, moisten the mass with strong hydrochloric acid, and after half an hour add water, in which the metastannic chloride and the other chlorides dissolve. Alloys of tin and gold are dis- solved in aqua regia, the excess of acid evaporated, and the solution diluted with much water, before precipitating with sulphuric acid. It must be remembered that in this process any phosphoric * Chem. Centralbl. 1857, 929. f Dingler's polyt. Journ. 158, 316. 164.] MKTALS OF GROUP VI. 563 acid that may be present is precipitated entirely or partially with the tin. After the precipitate has been well washed by decantation, LOWENTHAL recommends to boil with a mixture of 1 part nitric acid (sp. gr. 1/2) and 9 parts water, then to transfer to the filter, and wash thoroughly. Results very satisfactory. If the fluid contains a ferric salt, a portion of the iron always falls down with the tin. Hence the stannic oxide must be tested for iron according to 128, /?, which, if present, must be determined and deducted. 6. Method based on, the Insolubility of Mercuric Sulphide in Hydrochloric Acid. MERCURY FROM ANTIMONY. Digest the precipitated sulphides with moderately strong 136 hydrochloric acid in a distilling apparatus. The sulphide of antimony dissolves, while the mercuric sulphide remains behind. Expel all the hydrogen sulphide, then add tartaric acid, dilute, filter, mix the filtrate with the distillate which contains a little antimony, and precipitate with hydrogen sulphide. The mercuric sulphide may be weighed as such (F. FIELD*). 7. Methods based upon the Conversion of Arsenic and Antimony into Alkali Arsenate and Antimonate. a. ARSENIC FROM THE METALS OF GROUPS II., IV., AND Y. If you have to do with arsenites or arsenates, fuse with 3 137 parts^of sodium and potassium carbonates and 1 part of potas-* sium nitrate ; if an alloy has to be analyzed it is fused with 3 parts of sodium carbonate and 3 parts of potassium nitrate. In either case the residue is boiled with water, and the solution, which contains the arsenates of the alkalies, filtered from the undissolved oxides or carbonates. The arsenic acid is deter- mined in the filtrate as directed 127, 2. If the quantity of arsenic is only small, a platinum crucible may be used, other- wise a porcelain crucible must be used, as platinum would be seriously injured. In the latter case, bear in mind that the fused mass is contaminated with silicic acid and alumina. If the alloy contains much arsenic a small quantity may be readily lost by volatilization, even though the operation be cautiously * Quart, Journ. Chein. Soc. 12, 32. 564 SEPARATION. [ 164. conducted. In such a case, therefore, it is better first to oxidize with nitric acid, then to evaporate, and to fuse the residue as above directed with sodium carbonate and potassium nitrate. b. ARSENIC AND ANTIMONY FROM COPPER AND IRON, especially in ores containing sulphur. Diffuse the very finely pulverized mineral through pure 138 solution of potassa, and conduct chlorine into the fluid (comp. p. 467). The iron and copper separate as oxides, the solution contains sulphate, arsenate, and antirnonate of potassium (B-ivoT, BEUDANT, and DAGUIN*). c. ARSENIC AND ANTIMONY FROM COBALT AND NICKEL. Dilute the nitric acid solution, add a large excess of potassa, 139 heat gently, and conduct chlorine into the fluid until the pre- cipitate is black. The solution contains the whole of the arsenic and antimony, the precipitate the nickel and cobalt as sesquioxides (RivoT, BEUDANT, and DAGUIN, loc. cit.) 8. Methods based upon the Volatility of certain Chlorides or Metals. a. TIN, ANTIMONY, ARSENIC FROM COPPER, SILVER, LEAD, COBALT, NICKEL. Treat the sulphides with a stream of perfectly dry chlorine, 140 proceeding exactly as directed in 121. In presence of anti- mony, fill the receiver e (fig. 70) with a solution of tartaric acid in water, mixed with hydrochloric acid. The metals may be also separated by this method in alloys. The alloy must be very finely divided. Arsenical alloys are only very slowly decomposed in this way. In separating arsenic and copper the temperature must not exceed 200, and chlorine water should be put into the receiver (PARNELLf). If tin and copper are separated in this manner, according to the experience of H. ROSE,:); a small trace of tin remains with the copper chloride. b. STANNIC OXIDE, ANTIMONIOUS OXIDE (AND ALSO ANTIMONIC ACID), ARSENIOUS AND ARSENIC ACIDS, FROM ALKALIES AND ALKALINE EARTHS. Mix the solid compound with 5 parts of pure ammonium 141 chloride in powder, in a porcelain crucible, cover this with a * Compt. rend. 1853, 835; Journ. f. prakt. Chem. 61, 133. f Chem. News, 21, 133. \ Pogg. Annal. 112, 169. 164.] METALS OF GKOUP VI. 565 concave platinum lid, on which some ammonium chloride is ' sprinkled, and ignite gently until all ammonium chloride is driven off ; mix the contents of the crucible with a fresh por- tion of that salt, and repeat the operation until the weight remains constant. In this process, the chlorides of tin, anti- mony, and arsenic escape, leaving the chlorides of the alkalies and alkali-earth metals. The decomposition proceeds most rapidly with alkali salts. With regard to salts of alkali-earth metals it is to be observed that those which contain antimonic acid or stannic oxide are generally decomposed completely by a double ignition w r ith ammonium chloride (magnesium alone cannot be separated perfectly from antimonic acid by this method). The arsenates of the alkali-earth metals are the most troublesome to decompose ; barium, stronium, and cal- cium salts usually require to be subjected 5 times to the opera- tion, before they are free from arsenic, and magnesium arsenate it is impossible thoroughly to decompose in this way (H. ROSE*). According to SALKowsxif barium arsenate may be . converted into chloride quite free from arsenic by one ignition with ammonium chloride ; however calcium arsenate was found to leave a residue containing arsenic acid even after six igni- tions with ammonium chloride. c. MERCURY FROM GOLD (SILVER, AND GENERALLY FROM THE NON-VOLATILE METALS). Heat the weighed alloy in a porcelain crucible, ignite till 142 the weight is constant, and determine the mercury from the loss. If it desired to estimate it directly, the apparatus, p. 307, fig. 54, may be used. In cases where the separation of mer- cury from metals that oxidize on ignition in the air is to be effected by this method, the operation must be conducted in an atmosphere of hydrogen (p. 251, fig. 50). 9. Methods based on the Volatility of Arsenious Sulphide. ARSENIC ACID FROM THE OXIDES, OF MANGANESE, IRON, ZINC, COPPER, NICKEL, COBALT (NOT so WELL FROM OXIDE OF LEAD, AND NOT FROM OXIDES OF SILVER, ALUMINUM, OR MAG- NESIUM). Mix the arsenic acid compound (no matter whether it has 143 * Pogg. Annal. 73, 582; 74, 578; 112, 173. f Journ. f. prakt, Chem. 104, 138. 566 SEPARATION. [ 164. been air-dried or gently ignited) with sulphur, and ignite under a good draught in an atmosphere of hydrogen (p. 251, fig. 50 ; the perforated lid must in this case be of porcelain ; platinum would not answer). The whole of the arsenic vola- tilizes, the sulphides of manganese, iron, zinc, lead, and copper remain behind ; they may be weighed directly. After weigh- ing, add a fresh quantity of sulphur to the residue, ignite as before, and weigh again ; repeat this operation until the weight remains constant. Usually, if the compound was intimately mixed with the sulphur, the conversion of the arsenate into sulphide is complete after the first ignition. Results very good. In separating nickel the analyst will remember that the residue cannot be weighed directly, since it does not possess a constant composition ; hence the ignition in hydrogen may be saved ; nickel arsenate loses all its arsenic on being simply mixed with sulphur and heated. The heat should be moderate and continued till no more red sulphide of arsenic is visible on the inside of the porcelain crucible. It is advisable to repeat the operation. The separation of arsenic from cobalt cannot be completely effected in this manner even by repeated treat- ment with sulphur, but it can be effected by oxidizing the resi- due with nitric acid, evaporating to dryness, mixing with sul- phur, and reigniting. Smaltine and cobaltine must be treated in the same manner (H. HOSE*). 1 should not forget to men- tion that EBELMEN,| a long while ago, noticed the separation of arsenic acid from sesquioxide of iron by ignition in a stream of hydrogen sulphide. 10. Method based upon the Separation of Arsenic as Ammonium Magnesium Arsenate. ARSENIC ACID FROM COPPER, CADMIUM, FERRIC IRON, MAN- GANESE, NICKEL, COBALT, ALUMINIUM. Mix the hydrochloric acid solution, which must contain 144 the whole of the arsenic in the form of arsenic acid, with enough tartaric acid to prevent precipitation by ammonia, pre- cipitate the arsenic acid according to 127", 2, as ammonium magnesium arsenate, allow to settle, filter, wash once with a * Zeitschr. f. anal. Chem. 1, 413. f Annal. de Chim. et de Phys. (3) 25, 98. 164.] METALS OF GROUP VI. 567 mixture of 3 parts water and 1 part ammonia, redissolve in hydrochloric acid, add a very minute quantity of tartaric acid, supersaturate again with ammonia, add some more magnesium chloride and ammonium chloride, allow to deposit, and deter- mine the now pure precipitate according to 127, 2. In the nitrate the bases of Groups IV. and V. may be precipitated by ammonium sulphide ; if aluminium is present, evaporate the iiltrate from the sulphides with addition of sodium carbonate and a little nitre to dryness, fuse, and estimate the aluminium in the residue. The method is more adapted to the separation of rather large than of very small quantities of arsenic from the above-named metals, since in the case of small quantities the minute portions of ammonium magnesium arsenate that remain in solution may exercise a considerable influence on the accu- racy of the result. 11. Method based upon the Separation of Arsenic as Ammonium Arsenio-molybdate. ARSENIC ACID FROM ALL METALS OF GROUPS I. V. Separate the arsenic acid as directed in 127, 2, I ; long 145 continued heating at 100 is indispensable. The determination of the basic metals is most conveniently effected in a special portion. 12. Method based upon the Insolubility of Ferric ~Arsenate. ARSEXIC ACID FROM THE METALS OF GROUPS I. AND II., AND FROM ZlXC, MANGANESE, KlCKEL, AND COBALT. Mix the hydrochloric solution with a sufficient quantity of 146 pure ferric chloride, neutralize the greater part of the free acid with sodium carbonate, and precipitate the iron and arse- nic acid together with barium carbonate in the cold or with sodium acetate at a boiling heat. The precipitate should be so basic as to have a brownish-red color. The method is espe- cially suitable for the separation of arsenic acid when its esti- mation is not required. However, the precipitate may be dis- solved in hydrochloric acid and the arsenic determined by precipitation with hydrogen sulphide. 568 SEPARATION. [ 164. 13. Methods based upon the Insolubility of some Chlorides. a. SILVER FKOM GOLD. Treat the alloy with cold dilute nitrohydrochloric acid, 147 dilute, and filter the solution of auric chloride from the undis- solved silver chloride. This method is applicable only if the alloy contains less than 15 per cent, of silver ; for if it contains a larger proportion, the silver chloride which forms protects the undecomposed part from the action of the acid. In the same way silver may be separated also from platinum. b. MERCURY FROM THE OXYGEN COMPOUNDS OF ARSENIC AND ANTIMONY. Precipitate the mercury from the hydrochloric solution by 148 means of phosphorous acid as mercurous chloride ( 118, 2). The tartaric acid, which in the presence of antimony must be added, does not interfere with the reaction (H. KOSE*). 14. Methods based upon the Insolubility of certain Sulphates in Water or Alcohol. a. ARSENIC ACID FROM BARIUM, STRONTIUM, CALCIUM, AND LEAD. Proceed as for the separation of phosphoric acid from the 149 same metals ( 135, b). The compounds of these basic radicals with arsenious acid are first converted into arsenates, before the sulphuric acid is added ; this conversion is effected by heating the hydrochloric acid solution with potassium chlo- rate or by means of bromine. b. ANTIMONY FROM LEAD. Treat the alloy with a mixture of nitric and tartaric acids. 150 The solution of both metals takes place rapidly and with ease. Precipitate the greater part of the lead as sulphate ( 116, 3), filter, precipitate with hydrogen sulphide, and treat the sul- phides according to 128, with ammonium sulphide, in order to separate the antimony from the lead left unprecipitated by the sulphuric acid (A. STRENGf). 15. Method based upon the Separation of Copper as Cuprous Sulphocyanate. COPPER FROM ARSENIC AND ANTIMONY. From the properly prepared solution precipitate the cop- 151 * Pogg. Annal. 110, 536. f Ding- polyt. Journ. 151, 389. 165.] METALS OF GROUP VI. 569 | per by 119, 3, 5, as cuprous 'sulphocyanate, allow to settle, filter, wash with water containing ammonium nitrate (to pre- vent the washings being muddy), and determine antimony and arsenic in the filtrate, precipitating first with hydrogen sulphide. Results good. 16. Method 'based upon the different deportment with Cyanide of Potassium.. GOLD FROM LEAD AND BISMUTH. These metals may be separated in solution by potassium 152 cyanide in the same way in which the separation of mercury from lead and bismuth is effected (see 110). The solution of the double cyanide of gold and potassium is decomposed by boiling with aqua regia, and, after expulsion of the hydrocyanic acid, the gold determined by one of the methods given in 123. II. SEPARATION OF THE METALS OF THE SIXTH GROUP FROM EACH OTHEE. 165. INDEX. (The numbers refer to those in the margin.) Platinum from gold, 153, 168. tin, antimony, and arsenic, 154. Gold from platinum, 153, 168. tin, 154, 167. " antimony and arsenic, 154 Tin from platinum, 154. gold, 154, 167. arsenic, 157, 162, 163, 164, 166, 169. antimony, 155, 158, 164, 165, 166. Tin in stannous, from tin in stannic compounds, 172. Antimony from platinum and gold, 154. " arsenic, 158. 159, 160. tin, 155, 158, 164, 165, 166. Antimony of antimonious compounds from antimonic acid, 171. Arsenic from platinum and gold, 154. tin, 157, 162, 163. 164, 166, 169. antimony, 158, 159, 160. Arsenious acid from arsenic acid, 156, 161, 170. 570 SEPARATION. [ 165. 1. Method based upon tfw Precipitation of Plati- num as Potassium Platinic Chloride. PLATINUM FROM GOLD. Precipitate from the solution of the chlorides the plati- 153 num as directed 124, , and determine the gold in the filtrate as directed 123, I. 2. Methods based upon the Volatility of the Chlo- rides of the inferior Metals. a. PLATINUM AND GOLD FROM TIN, ANTIMONY, AND ARSENIC. Heat the finely divided alloy or the sulphides in a stream 154 of chlorine gas. Gold and platinum are left, the chlorides of the other metals volatilize (compare 121). b. ANTIMONY FROM TIN. The tin should be present wholly as a stannous salt. 155 Precipitate with hydrogen sulphide, filter (preferably through an asbestos filtering tube), dry the precipitate, and pass through it a current of dry hydrochloric gas at the ordinary tempera- ture. The sulphides are converted into the corresponding chlorides ; the chloride of antimony alone escapes, and may be received in water. Dissolve the residual stannous chloride in water containing hydrochloric acid, and estimate the tin according to 126 (C. TOOKEY*). The method can only be used in rare cases, as it is difficult to obtain a precipitate quite free from stannic sulphide. c. ARSENIOUS ACID FROM ARSENIC ACID. The amount of substance taken should not contain more 156 than -2 grm. arsenious acid. Heat with 45 grm. sodium chloride, 135 grm. sulphuric acid (free from arsenic) of 1*61 sp. gr., and 30 grm. water in a tubulated retort containing a spiral of platinum, and provided with a thermometer. The temperature should rise to about 125. In order to condense the arsenious chloride in the products of distillation, a LIEBIG'S condenser is connected with the retort ; a tubulated receiver is connected with the condenser ; a U-tube is connected with the receiver, and finally a calcium chloride tube containing fragments of glass moistened with weak soda solution is fixed * Journ. Chem. Soc. 15, 462. 165.] METALS OF GROUP VI. 571 upright in the exit end of the U-tube. In the receiver and IJ-tube water is placed. At the end of the operation rinse the calcium chloride tube, and mix with the contents of the receiver. Determine the arsenic in the distillate according to jj 127, -1, #, in the residue according to 127, 4, h. The sul- phide obtained from the former corresponds to the arsenious. acid, from the latter to the arsenic acid. Results satisfactory (RiECKHER*). If the substance given is a dilute fluid, render slightly alkaline with sodium carbonate, and concentrate to about 20 c.c., finally in a tubulated retort. 3. Mrfltin/H based upon the Volatility of Arsenic am/ A /*> /tious Sulphide. a. AKSKXIC FROM Tix (H. ROSE). Convert into sulphides or oxides, dry at 100, and heat a 157 weighed portion with addition of a little sulphur in a bulb- tube, gently at first, but gradually 'more strongly, conducting a stream of dry hydrogen sulphide gas through the tube during the operation. Sulphur and arsenious sulphide vola- tilize ; sulphide of tin is left. The arsenious sulphide is received in U-tubes containing dilute ammonia, which are connected with the bulb-tube in the manner described in 121. When upon continued application of heat no sign of further sublimation is observed in the colder part of the bulb-tube, drive off the sublimate which has collected in the bulb, allow the tube to cool, and then cut it off above the coating. Divide the separated portion of the tube into pieces, and heat these with a little solution of soda until the sublimate is dissolved ; unite the solution with the ammoniacal fluid in the receivers, add hydrochloric acid, then, without filtering, potassium chlorate, and heat gently until the arsenious sulphide is com- pletely dissolved. Filter from the sulphur, and determine the arsenic acid as directed 127, 2. The quantity of tin cannot be calculated at once from the blackish-brown sulphide of tin in the bulb, since this contains more sulphur than SnS. It is therefore weighed, and the tin determined in a weighed por- tion of it, by converting it into stannic oxide, which is effected by moistening with nitric acid, and roasting ( 126, 1, c). * Pharm. Centrallialle, 11. 92. 572 SEPARATION. [ 165. Tin and arsenic in alloys are more conveniently converted into oxides by cautious treatment with nitric acid. If, how- ever, it is wished to convert them into sulphides, this may readily be effected by heating 1 part of the finely divided alloy with 5 parts of sodium carbonate and 5 parts of sulphur, in a covered porcelain crucible until the mass is in a state of calm fusion. It is then dissolved in water, the solution filtered from the ferrous sulphide, &c., which may possibly have formed, and then precipitated with hydrochloric acid. If the tin only in the alloy is to be estimated directly, while the arsenic is to be found from the difference, convert as above directed into sulphides or oxides, mix with sulphur and ignite in a porcelain crucible with perforated cover in a stream of hydrogen sulphide. The residual arsenic-free stannous sulphide is to be converted into stannic oxide and weighed as such. 4. Methods based upon the Insolubility of Sodium Metantimonate. a. ANTIMONY FROM TIN AND ARSENIC (H. ROSE). If the substance is metallic, oxidize the finely divided 158 weighed sample, in a porcelain crucible, with nitric acid of 1'4 sp. gr., adding the acid gradually. Dry the mass on the water-bath, transfer to a silver crucible, rinsing the last particles adhering to the porcelain into the silver crucible with solution of soda, dry again, add eight times the bulk of the mass of solid sodium hydroxide, and fuse for some time. Allow the mass to cool, and then treat with hot water until the undissolved residue presents the appearance of a fine powder ; dilute with some water, and add one-third the volume of alcohol of '83 sp. gr. Allow the mixture to stand for 24r hours, with frequent stirring; then filter, transfer the last adhering particles from the crucible to the filter by rinsing with dilute alcohol (1 vol. alcohol to 3 vol. water), and wash the undissolved residue on the filter, first with alcohol diluted with twice its volume of water, then with a mixture of equal volumes of alcohol and water, and finally with a mixture of 3 vol. alcohol and 1 vol. water. Add to each of the alcoholic fluids used for washing a few drops of solution of sodium carbonate. Continue the washing until the color of a portion 165.] METALS OF GROUP VI. 573 of the fluid running off remains unaltered upon being acidified with hydrochloric acid and mixed with hydrogen sulphide water. Rinse the sodium metantimonate from the filter, wash the latter with a mixture of hydrochloric and tartaric acids, dis- solve the metantimonate in this mixture, precipitate with hydrogen sulphide, and determine the antimony as directed 125, 1. In presence of much tin it is well to fuse the metantimonate again with caustic soda, &c. To the filtrate, which contains the tin and arsenic, add hydrochloric acid, which produces a precipitate of stannic arsenate ; conduct now into the unfiltered fluid hydrogen sulphide for some time, allow the mixture to stand at rest until the odor of that gas has almost completely gone off, and separate the weighed sulphides of the metals which contain free sulphur, as in 157. If the substance contains only antimony and arsenic, the alcoholic filtrate is heated, with repeated addition of water, until it scarcely retains the odor of alcohol ; hydrochloric acid is then added, and the arsenic acid determined as magnesium pyroarsenate ( 127, 2), or as arsenious sulphide ( 127, 4, b). b. Small quantities of the sulphides of arsenic and anti- 159 mony mixed with sulphur are often obtained in mineral analysis. The two metals may in this case be conveniently separated as follows : Exhaust the precipitate with bisulphide of carbon, oxidize with chlorine-free red fuming nitric acid, evaporate the solution nearly to dryness ; mix the residue with a copious excess of sodium carbonate, add some sodium nitrate, and treat the fused mass as given in #, 158. If, on the other hand, you have a mixture of sulphides of tin and antimony to analyze, oxidize it with nitric acid of 1*5 sp. gr., and treat the residue obtained on evaporation as given in a, 158. 5. Methods based upon the Precipitation of Arsenic as Ammonium Magnesium Arsenate. a. ARSENIC FROM ANTIMONY. Oxidize the metals or sulphides with nitrohydrochloric acid, 160 with hydrochloric acid and potassium chlorate, with bromine dissolved in hydrochloric acid, or with chlorine in alkaline solu- tion ; add tartaric acid, a large quantity of ammonium chloride, 574 SEPARATION. [ 165. and then ammonia in excess. (Should the addition of the latter reagent produce a precipitate, this is a proof that an insufficient quantity of ammonium chloride or of tartaric acid has been used, which error must be corrected before proceed- ing with the analysis.) Then precipitate the arsenic acid as directed 127, 2, and determine the antimony in the filtrate as directed in 125, 1. As basic magnesium tartrate might precipitate with the ammonium magnesium arsenate, the precipitate should always, after slight washing, be redissolved in hydrochloric acid, and reprecipitated with ammonia with addition of a little magnesia mixture an excellent method. b. ARSENIOUS ACID FROM ARSENIC ACID. Mix the sufficiently dilute solution with a large quantity 161 of ammonium chloride, precipitate the arsenic acid as directed 127, 2, and determine the arsenious acid in the filtrate by precipitation with hydrogen sulphide (127, 4). LUDWIG* has observed that if the solution is too concentrated, magne- sium arsenite falls down with the ammonium magnesium arsenate, hence it is necessary to dissolve the weighed magne- sium precipitate in hydrochloric acid and test the solution with hydrogen sulphide. The presence of arsenious acid will be betrayed by the immediate formation of a precipitate. c. TIN AND ANTIMONY FROM ARSENIC ACID. LENSSEN-J- separated tin from arsenic acid with good 162 results by digesting the oxides obtained by oxidation with nitric acid w T ith ammonia and yellow ammonium sulphide, and precipitating the arsenic acid from the clear solution accord- ing to 127, 2, as ammonium magnesium arsenate. On acidify- ing the filtrate the tin separates as stannic sulphide. The method can only give good results when the whole of the arsenic was present as arsenic acid before the addition of ammonium sulphide, for the arsenic in a solution of arsenious acid in yellow ammonium sulphide is not thrown down by magnesia mixture. The method also answers for separating antimony from arsenic. * Archiv fur Pharm. 97, 24. \ Annal. d. Chem. u. Pharm. 114, 116. 165.] METALS OF GROUP VI. 575 6. Methods based on the different behavior of the freshly Precipitated Sulphides towards Solution of Potassium Hydrogen Sulphite or Oxalic Acid. a. ARSENIC FROM ANTIMONY AND TIN (BuxsEN*). If freshly precipitated arsenious sulphide is digested with 163 sulphurous acid and potassium sulphite, the precipitate is dis- solved ; on boiling, the fluid becomes turbid from separated sulphur, which turbidity for the most part disappears again on long boiling. The fluid contains, after expulsion of the sul- phurous acid, potassium arsenite and thiosulphate. The sul- phides of antimony and tin do not exhibit this reaction. Both therefore may be separated from arsenious sulphide by diluting the solution of the three sulphides in potassium sulphide to about 500 c.c. and precipitating with a large excess (about a litre) of saturated aqueous sulphurous acid, digesting the whole for some time in a water-bath, and then boiling till one-third of the water and the whole of the sulphurous acid are expelled and the sulphur has disappeared ; this will take about an hour and a half. The residuary sulphide of antimony or tin is arsenic- free, the filtrate contains the whole of the arsenic and may be immediately precipitated with hydrogen sulphide. BUNSEN determines the arsenic by oxidizing the dried sulphide together with the filter with fuming nitric acid, diluting the solution a little, warming gently with a little potassium chlorate (in order to oxidize more fully the substances formed from the paper), and finally precipitating as ammonium magnesium arsenate. With regard to the separation of stannic sulphide from the solution of potassium arsenite, it is to be observed that the stannic sulphide must be washed with concentrated solution of sodium chloride, as, if water were used, the fluid would run through turbid. As soon as the precipitate is thoroughly washed with the sodium chloride, the latter is displaced by solution of ammonium acetate, containing a slight excess of acetic acid. These last washings must not be added to the first, as the ammonium acetate hinders the complete precipita tion of the arsenious acid by hydrogen sulphide. * Annal. d. Chem. u. Pharm. 106, 3. 576 SEPARATION. L The test-analyses adduced by BUNSEN show very satisfac- tory results. b. TlN FROM ARSENIC AND ANTIMONY (F. W. CLARKE*). Moist freshly precipitated bisulphide of tin completely dis- .solves on boiling for a moderate length of time with excess of oxalic acid, and therefore tin in the form of bichloride is not thrown down by hydrogen sulphide from a hot solution containing excess of oxalic acid. The sulphides of arsenic are barely affected by boiling with oxalic acid, and hydrogen sulphide immediately reprecipitates the traces dissolved. Sulphide of antimony dissolves more copiously on boiling with oxalic acid, but hydrogen sulphide reprecipitates the antimony from the solution. [These reactions form the basis of CLARKE'S method, which, with some important modifications, has been successfully applied to the separation of tin from antimony in alloys by F. P. DEWEY,f who proceeds as follows : Dissolve with a mixture of 1 part strong nitric acid, 4 parts strong hydrochloric acid, and 5 parts water. Since even small quantities of free mineral acids prevent complete precipitation of antimony, they are removed by evaporating to dryness on a water-bath, with previous addition of enough potassium chloride to form double salts with the tin and antimony chlor- ides present. The presence of the potassium chloride entirely prevents loss of tin and antimony by volatilization as chlorides during the evaporation. Add to the salts thus obtained a large quantity of pure oxalic acid (at least 20 parts crystallized acid to 1 part tin), and dilute with water to about 125 c.c. per *1 grin, antimony present. The salts dissolve readily. Boil and pass H 2 S through the boiling solution half an hour. Filter immediately while hot, and wash the greater part of the soluble matter out of the precipitate with hot water. The precipi- tated antimonious sulphide will contain a little stannic sulphide. Dissolve in ammonium sulphide, avoiding an unnecessary quantity of the solvent, and pour the solution into a strong hot solution of oxalic acid. A liberal excess of oxalic acid should be present after decomposition of the sulphur salts. Heat the oxalic solution with the suspended precipitate of antimonious * Chem. News, 21, 124. f Am. Chem. Journ. i. 244. 165.] METALS OF GROUP VI. 577 sulphide to boiling, and pass H,S gas ten minutes. Collect the Sb a S, now free from tin on a weighed filter, wash with hot water, and proceed to determine the antimony as directed in 125, 1, b. To recover tin from the filtrate, evaporate nearly to dryness, add strong sulphuric acid, and heat till all the oxalic acid present is decomposed and removed. Dilute largely, and precipitate the tin with hydrogen sulphide according to 126, 1, c.-] 7. Methods based 'upon the Separation of the Metals themselves, or, as the case may be, on the different deportment of the same with Acids. a. TIN FROM ANTIMONY (TooKEY,* improvements by CLASEN (loc. cit.) and AirFiELDf). The hydrochloric solution should be oxidized if necessary 165 with a few drops of nitric acid or a little potassium chlorate. Heat nearly to boiling and add iron as long as it dissolves. Either hoop-iron or fine bright wire will answer the purpose ; it should dissolve in dilute hydrochloric acid, leaving little or no residue. The antimony will be thrown down, the tin reduced to stannous chloride. As soon as all antimony appears to be precipitated and the iron to be dissolved, add more hydrochloric acid, allow to deposit, decant and test whether iron produces any further precipitate. In this way you will ensure the absence of any metallic iron and the complete pre- cipitation of the antimony. Wash the antimony with hot water, which should be at first acidified, then with alcohol, finally with ether, drying at 100. Throw down the tin with hydrogen sulphide ( 126, 1, c). With care the results are good ; compare CLASEN (loc. cit.). b. MUCH TIN FROM LITTLE ANTIMONY AND ARSENIC. If an alloy of the three metals is treated in a very finely 166 divided condition in a stream of carbonic acid with strong hydrochloric acid, the whole of the tin dissolves to stannous chloride. A part of the arsenic and antimony escapes as arsenetted and antimonetted hydrogen, whilst the rest remains behind in the state of metal, or, as the case may be, of a solid combination with hydrogen. Conduct the gas through several * Journ. Chem. Soc. 15, 402. f Zeitsckr. f. anal. Chem. 9, 107. 578 SEPARATION. [ 165, XT-tubes, containing a little chlorine-free red fuming nitric acid, whereby the arsenic and antimony will be oxidized. When the solution is effected, dilute the contents of the flask with air-free water to a certain volume, mix, allow to settle, and determine the tin in an aliquot part, either gravimetrically or volumetrically. Filter the rest of the fluid, wash the pre- cipitate thoroughly, dry the filter with its contents in a porce- lain crucible, add the contents of the U-tubes, evaporate to dryness, and in the residue separate the, antimony and arsenic as directed 158. It is well to treat an aliquot part of the hydrochloric solution with iron (165) to find, and, if necessary, estimate traces of antimony which may have passed into the hydrochloric acid solution. c. TIN FROM GOLD. Gold may be separated from excess of tin by boiling the 167 finely divided alloy with only slightly diluted sulphuric acid, to which hydrochloric acid has been cautiously added. The tin dissolves as stannous chloride. Heat is applied till the sulphuric acid begins to volatilize copiously. Stannic oxide is formed which dissolves in the concentrated sulphuric acid, while the gold remains behind. On addition of much water,, the stannic oxide falls, mixed with finely divided gold, in th form of a purple-red precipitate. On warming with concen- trated sulphuric acid, the stannic oxide finally redissolves, while the gold is left pure (H. HOSE*). d. PLATINUM FROM GOLD. The aqua regia solution is freed as far as possible from 168 nitric acid by evaporation with hydrochloric acid, and treated with a solution of ferrous chloride, the gold being determined as directed 123, &. The platinum may be precipitated from the filtrate by hydrogen sulphide according to 124, c. 8. Method based upon the Precipitation of Tin as Stannic Arsenate. TIN FROM ARSENIC. E. HlFFELYf has proposed the following method of deter- 169 mining both the tin and the arsenic in commercial sodium stannate, which often contains a large admixture -of sodium * Pogg. Annal. 112, 172. f Phil. Mag. 10, 220. 165.] METALS OF GROUP VI. -579 arsenate. Mix a weighed sample with a known quantity of sodium arsenate in excess, add nitric acid also in excess, boil, filter off the precipitate, which has the composition 2SnO 3 , As, O 6 -\- 10H 2 O, and wash ; expel the water by ignition, and weigh the residue, which consists of 2SnO a ,As a O 5 . In the filtrate determine the excess of arsenic acid .as directed 127, 2. The amount of the stannic oxide is found from the weight of the precipitate, that of the arsenic acid is obtained by add- ing the quantity in the precipitate to the quantity in the fil- trate, and deducting the quantity added. 9. Volumetric Methods. a. AKSENIOUS FROM ARSENIC Aero. Convert the whole of the arsenic in a portion of the sub- 170 stance into arsenic acid and determine the total amount of this as directed 127, 2 ; determine in another portion the arseni- ous acid as directed in 127, 5, #, and calculate the arsenic acid from the difference. &. ANTIMONY OF ANTIMONIOUS COMPOUNDS FROM ANTIMONIO ACID. Determine in a sample of the substance the total amount 171 of the antimony as directed 125, 1, in another portion esti- mate the antimony present as an antirnonious compound as directed 125, 3, and calculate the antiinonic acid from the difference. c. TIN OF STANNOUS, FROM TIN OF STANNIC COMPOUNDS. In one portion of the substance convert the whole of the 172 stannous into stannic salts by digestion with chlorine water or some other means, and determine the total quantity of tin as directed 126, 1, b ; in another portion, which, if necessary, is -to be dissolved in hydrochloric acid in a stream of carbonic acid, determine the stannous tin according to 126, 2. II. SEPARATION OF THE ACIDS FROM EACH OTHER. It must not be forgotten that the following methods of separation proceed generally upon the assumption that the acids exist either in the free state, or as alkali salts ; compare the introductory remarks, p. 479. Where several acids are to be determined in one and the same substance, we very often use 580 SEPARATION. [ 166. a separate portion for each. The methods here given do not embrace every imaginable case, but only the most important cases, and those of most frequent occurrence. First Group. ARSENIOUS ACID ARSENIC ACID CHROMIC ACID SULPHURIC ACID PHOSPHORIC ACID BORACIC ACID OXALIC ACID HYDROFLUORIC ACID SILICIC ACID CARBONIC ACID. 166. 1. ARSENIOUS ACID AND ARSENIC ACID FROM ALL OTHER ACIDS. Precipitate the arsenic from the solution by hydrogen sul- 173 phide ( 127, 4, a or &), filter, and determine the other acids in the filtrate. It must be remembered, that the arsenious sulphide will be obtained mixed with sulphur if chromic acid, ferric salts, or any other substances which decompose hydro- gen sulphide are present. The estimation of sulphuric acid in the filtrate cannot be accurate unless air is excluded, and oxidizers such as chromic acid are absent ; sulphuric acid is, therefore, best estimated in a separate portion (174). From those acids which form soluble magnesium salts, arsenic acid may be separated also by precipitation as ammonium magne- sium arsenate ( 127, 2). 2. SULPHURIC ACID FROM ALL THE OTHER ACIDS.* a. From Arsenious, Arsenic, Phosphoric^ Boracic,0xalic, and Carbonic Acids. Acidify the dilute solution strongly with hydrochloric acid, 174 mix with barium chloride, and filter the barium sulphate from the solution, which contains all the other acids. Determine the barium sulphate as directed 132. If acids are present' with which barium forms salts insoluble in water but soluble in acids, the barium sulphate is apt to carry down with it such salts, and this is all the more liable to happen, the longer the * With respect to the separation of sulphuric acid from selenic acid, comp. WOHLWILL (Annal. d. Chem. u. Pharm. 114, 183). f If metaphosphoric acid is present, it must first be converted into orthophos- phoric by fusion with alkali carbonate. 166.] ACIDS OF GROUP I. 581 precipitate is allowed to settle. This remark applies especially to barium oxalate, and tartrate, and the barium salts of other organic acids (H. ROSE). In such cases I would recom- mend, after washing, to stop up the neck of the funnel, and digest the precipitate with a solution of hydrogen sodium car- bonate, then to wash with water, with dilute hydrochloric acid, and again with water. In every case, however, the purity of the weighed barium sulphate must be tested as directed 132, 1. In the fluids filtered from the barium sulphate the other acids are determined according to the directions of the Fourth Section, after the removal of the excess of barium chloride. Or the other acids may be estimated in separate portions of the substance, which is indeed usually the best way, and for carbonic acid is of course the only way. ~b. From Hydrofluoric Acid. a. When sulphuric acid and hydrofluoric acid are present 175 in the free state in aqueous solution, it is best to estimate the acidity in one portion by means of standard soda ( 192), and the sulphuric acid in another ( 132, L, 1), finding the hydro- fluoric acid by difference. The barium sulphate should be purified by fusion with sodium carbonate ( 132, I., 1). ft. To estimate both acids in minerals or other dry sub- 176 stances, it is safest, provided the fluoride can be decomposed by sulphuric acid, to determine the fluorine in one portion according to 138, 3, , and to fuse another portion for a long time with four times its amount of sodium carbonate, which will decompose the sulphate thoroughly, the fluoride generally but partially. The fused mass is soaked in water, the solution filtered, acidified with hydrochloric acid and pre- cipitated with barium chloride. The barium sulphate thus obtained generally contains barium fluoride, and must be purified according to 132, I., 1, by fusion with sodium car- bonate, &c. y. An actual separation of both acids may be effected, 177 when both are in the form of alkali salts, by adding sodium carbonate if necessary, and then precipitating the fluorine according to 138, I., adding the calcium chloride cautiously in very slight excess. The sulphuric acid is for the most part 82 SEPARATION. [ found in the filtrate from the calcium carbonate and fluoride, a very small part is generally also found in the calcium acetate filtered from the calcium fluoride. Both filtrates are acidified and precipitated with barium chloride ( 132, I., 1. H. EOSE). d. Insoluble compounds may also be decomposed by fusion 178 with six parts of sodium and potassium carbonates, and two parts of silica. The fused mass, after cooling, is treated with water, the solution is mixed with ammonium carbonate, and heated, more ammonium carbonate is added to replace what evaporates, the silicic acid thrown down is filtered off and washed with water containing ammonium carbonate, a solu- tion of zinc oxide in ammonia is added to precipitate the remaining silica, the fluid is evaporated till all ammonia is driven off, filtered and the process concluded as in y. The precipitate produced by the zinc should be tested for sulphuric acid. c. From Chromic Acid. Boil the dry compound with strong hydrochloric acid 179 (p. 357, ft) and estimate the chromic acid from the evolved chlorine. Neutralize some of the acid with ammonia, dilute and precipitate the sulphuric acid by long boiling with excess of barium chloride. The barium sulphate thus obtained retains chromic oxide (H. KOSE) and must always be fused with sodium carbonate, &c. (p. 367). d. From Hydrofluosilicic Acid. First throw down the hydrofluosilicic acid according to 180 133, as potassium silicofluoride, then the sulphuric acid in the filtrate with barium chloride. e. From Silicic Acid. Compare 192. 3. PHOSPHORIC ACID FROM THE OTHER ACIDS. a. From the (icids of arsenic, see 173 : from sulphuric 181 acid, see 174 ; from silicic acid, see 192. b. From Chromic Acid. Precipitate the phosphoric acid by adding ammonium nitrate and ammonia, and then magnesium nitrate, and deter- 166. J ACIDS OF GROUP I. 583 mine the chromic acid in the filtrate as directed 130, I., #, ft or L, b. c. From I>oracic Acid. Precipitate the phosphoric acid with a solution of double 182 chloride of magnesium and ammonium ( 134, b, a), wash the precipitate partially, redissolve it in hydrochloric acid, repre- -cipitate with ammonia, adding a little magnesium and ammo- nium chloride, and estimate the phosphoric acid as magnesium pyrophosphate. In the filtrate estimate the boracic acid as magnesium borate ( 136, L, 1, d). d. From Oxalic Acid. a. If the two acids are to be determined in one portion, 183 the aqueous or hydrochloric solution is mixed with sodium :auric chloride in excess, heat applied, and the oxalic acid cal- culated from the reduced gold ( 137, c). The gold added in excess is separated from the filtrate by hydrogen sulphide, and the phosphoric acid then precipitated by double chloride of magnesium and ammonium. ft. If there is enough of the substance, the oxalic acid is 184 determined in one portion according to 137, &, or d, and the phosphoric acid in another portion. If the substance is solu- ble in water, and the quantity of oxalic acid inconsiderable, the phosphoric acid may be precipitated at once with magne- sium chloride, ammonium chloride, and ammonia : if not, the substance is ignited with potassium carbonate and sodium car- bonate, and the oxalic acid being thus destroyed, the phos- phoric acid is determined in the nitric acid solution of the residue according to 134, L, J, ft. e. From Hydrofluoric Acid. a. Phosphates and fluorides are frequently found together 185 in minerals. In the analysis of phosphorites, for instance, we have to estimate small quantities of fluorine, often too in the presence of aluminium and iron, which increase the difficulty. According to my own experience,* it is always safest in such cases to estimate in one portion the fluorine as silicon fluoride ( 138, II., 3, a), and in another portion the phosphoric acid. Regarding the first estimation, it must be mentioned that car- * Zeitschr. f. anal. Chem. 5, 190, and 6, 403. 584 SEPARATION. [ 166. bonic acid if present must first be removed. To this end heat the finely powdered weighed substance, with water, add acetic acid in slight excess, and also, if the fluoride present is soluble in water, some calcium acetate ; evaporate to dry ness on a water bath, treat with water, filter, wash the insoluble matter, dry, separate as far as possible from the filter, add the filter ash, weigh, test a small portion for carbonic acid by heating with hydrochloric acid, and weigh the rest for the fluorine estima- tion. For the estimation of the phosphoric acid, dissolve the finely powdered substance in hydrochloric acid, evaporate to dryness on a water-bath, moisten with a little hydrochloric acid, add nitric acid, warm, dilu-te, filter, evaporate filtrate and washings to dryness, dissolve in nitric acid, and proceed according to 134, I., >, ft. ft. Where you have an alkali phosphate and an alkali 186 fluoride together in aqueous solution the phosphoric acid may be separated according to 135, II., d, ft, as silver phosphate, or according to 135, II., &, as mercurou& phosphate. The fluoride will be all in the filtrate. If the former method is adopted the silver is removed from the filtrate by sodium chloride, and the fluorine estimated as calcium salt ( 138, 1.). If the latter method is adopted, as the solution is always acid, the use of glass and porcelain must be avoided. The mercury is removed from the filtrate by neutralizing with sodium car- bonate and without filtering passing hydrogen sulphide. The fluorine is estimated in the filtrate as calcium salt, accord- ing to 138, I. (II. KOSE). y. Substances which are insoluble in water, and cannot be 187 decomposed by acids, are fused with sodium carbonate and silica (178), the fused mass is treated with water, and the solu- tion with ammonium carbonate. In this way all the fluorine and all, or nearly all, the phosphoric acid will be brought into solution. The solution is treated as in 186, and any remainder of phosphoric acid in the undissolved residue is estimated according to 185. 4. HYDROFLUORIC ACID FROM OTHER ACIDS. a. fluorides from E orates. Mix the solution containing alkali borate and fluoride with 188 some sodium carbonate, and add calcium acetate in excess. A 166.] ACIDS OF GROUP I. 585 precipitate is formed, which contains the whole of the fluorine as calcium fluoride, and besides this, calcium carbonate and some calcium borate ; the greater portion of the latter having been redissolved by the excess of the calcium salt added. Determine the calcium fluoride in the precipitate as directed 138, 1. The small quantity of boracic acid in the precipitate is, in this process, partly volatilized, partly dissolved after evaporating the mass with acetic acid and extracting with water. It is therefore necessary to determine the boracic acid in a separate portion of the substance, according to 136, I., 2 (A. STROMEYER).* b. Fluorides from Silicic Acid and Silicates. A great many native silicates contain fluorides : care must, therefore, always be taken, in the analysis of minerals, not to overlook the latter. If the silicates containing fluoride are decomposable by acids which is only rarely the case and the silicic acid is separated in the usual way by evaporation, the whole of the fluorine may volatilize. a. BERZELIUS'S method. Fuse the elutriated substance 189 with 4 parts of sodium carbonate for some time at a strong red heat, digest the mass in water, boil, filter, and wash, first with boiling water, then with ammonium carbonate. The fil- trate contains all the fluorine as sodium fluoride, and, besides this, sodium carbonate, silicate, and aluminate. Mix the fil- trate with ammonium carbonate and heat the mixture, replac- ing the ammonium carbonate, which evaporates. Filter off the precipitate of hydrate of silicic acid and aluminium hydroxide, and wash with ammonium carbonate. To separate the last portions of silica from the filtrate add a solution of zinc oxide in ammonia, evaporate till no more ammonia escapes, and filter off the precipitate of zinc silicate and oxide. Determine the silica in this precipitate by dissolving in nitric acid, evaporating to dryness, taking up wdth nitric acid, and filtering off the undissolved silica. In the alkaline filtrate estimate the fluorine as calcium salt ( 138, I.). The residue, insoluble in water, and the precipitate produced by ammonium carbonate are finally treated with hydrochloric acid according to 140, II., , in order to separate the silica. * Annal d. Chem. u, Pharm. 100, 91 586 SEPARATION. [ 166. ft. In substances readily decomposed by sulphuric acid you 190 may also separate and weigh the silica according to 189 in one portion, and determine the fluorine in another portion accord- ing to 138, II., 3, a. c. Fluorides, /Silicates and Phosphates together. Compounds of this kind are not rare in nature, and may 191 be decomposed according to 189. We cannot always rely on complete decomposition of the phosphate, as, for instance, cal- cium phosphate is but partially decomposed on fusion with sodium carbonate. The solution, obtained after separation of the silica by ammonium carbonate and the zinc solution, is made up to a definite volume, and a portion is tested for phos- phoric acid with molybdic solution. If none is present the fluorine is estimated in the measured remainder of the fluid as fluoride of calcium ( 138, I.). If on the other hand phos- phoric acid is still present, treat the measured remainder of the fluid according to 186. In the original residue and the ammo- nium carbonate precipitate estimate the principal amounts of the silicic and phosphoric acids and the basic metals. In the zinc precipitate estimate the remainder of the silicic acid, and in the filtrate from the latter estimate the portion of the phosphoric acid which was thrown down by zinc oxide. As the phosphoric acid is so divided by this method, it is well to make a direct estimation of it in another portion of the substance, especially when only a small quantity is present. For this purpose decompose the silicate with hydrofluoric and hydrochloric acids, add enough but not too large an excess of sulphuric acid, and evaporate till all the fluorine has escaped as silicon fluoride arid hydrofluoric acid. Do not increase the heat to the escape of sulphuric acid, or phosphoric acid may be lost. Take up the residue with nitric acid, dilute, filter, and estimate the phosphoric acid in the filtrate by the molybdic method. If the substance can be easily decomposed with sulphuric acid, the fluorine may of course also be expelled as silicon fluoride and estimated according to 138, II., 3, a. 5. SILICIC Aero FKOM ALL OTHER ACIDS. a. In compounds which are decomposed by hydrochloric field. Decompose the substance by digestion with hydrochloric 192 166.] ACIDS OF (iiioi'p i. 587 or nitric acid, evaporate the whole on the water bath to dryness { 140, II., a), treat with water, hydrochloric acid or nitric acid according to circumstances, filter off the silica, and estimate the other acids in the filtrate. The following points require attention. a. In the presence of borates or fluorides this method cannot be used, employ 193. ft. In the presence of phosphoric acid the silica always retains a small portion, which cannot be extracted by washing with acidified water (H. ROSE, "W. SKEY*). After washing the silica with water, treat it repeatedly with ammonia, which will leave only a very minute quantity of the phosphoric acid. Evaporate the ammoniacal fluid, finally adding a little hydro- chloric acid, dissolve in water with addition of a little nitric acid, filter off the small amount of silica which was taken up by the ammonia, and estimate the remainder of the phosphoric acid in the filtrate. J. In compounds which are not decomposed by hydrochlo- ric acid. Fuse with carbonate of potash and soda (p. 422), and treat 193 the residue either at once cautiously with dilute hydrochloric or nitric acid, in order to proceed with the solution according to 192 (not applicable in presence of boracic acid or fluorine) ; or taking the fluid obtained by boiling the residue with water, precipitate the dissolved . silica by warming with ammonium carbonate, and throw down the last portion of silica from the filtrate by zinc oxide dissolved in ammonia (189j. The silicic acid is then found partly in the residue left undissolved by water, partly in the precipitate produced by ammonium carbonate, and partly in the precipitate produced by the zinc solution. Separate it according to 140, II., a. Boracic acid and fluorine will be found entirely in the last alkaline filtrate (189). Regarding phosphoric acid see 191. Sulphuric acid passes for the most part into the last alkaline filtrate, yet it is well also to examine the acid filtrates from the silica. 6. CARBONIC Aero FROM ALL OTHER ACIDS. When carbonates are heated with stronger acids, the car- 194 * Zeitschr. f. anal. Chem. 8, 70. 588 SEPARATION. [ 167. bonic acid is expelled ; the presence of carbonates, therefore, does not interfere with the estimation of most other acids. And as, on the other hand, the carbonic acid is determined by the -loss of weight or by combination of the expelled gas, the presence of salts of non-volatile acids does not interfere with the determination of the carbonic acid. Accordingly, with compounds containing carbonates, sulphates, phosphates, &c., either the carbonic acid is determined in one portion, and the other acids in another, or both estimations are performed on one portion. In the latter case the process described p. 412, e, may be used with advantage, the other acids being determined in the solution remaining in the decomposing flask. In pres- ence of fluorides, one of the weak non-volatile acids, such as tartaric acid or citric acid, must be employed to expel the carbonic acid ; since, were sulphuric or hydrochloric acid used, part of the liberated hydrofluoric acid would escape with the carbonic acid. If, as will occasionally happen in an analysis, a mixed precipitate of calcium fluoride and calcium carbonate is thrown down from a solution, the two salts may be separated by evaporating with acetic acid to dry ness, and extracting the residue with water ; the calcium acetate formed from the car- bonate is dissolved the calcium fluoride is left behind. Second Group. CHLORINE BROMINE IODINE CYANOGEN SULPHUR. I. SEPARATION OF THE ACIDS OF THE SECOND GROUP FROM THOSE OF THE FIRST. 167. a. All the Acids of the Second Group from those of the First. Mix the dilute solution with nitric acid, add silver nitrate 195 in excess, and filter off the insoluble chloride, bromide, iodide, &c., of silver. The filtrate contains the whole of the acids of the first group, the silver salts of these acids being soluble in water or nitric acid. Carbonic acid must, under all circum- stances, be determined in a separate portion ( 139, e). 167.] ACIDS OF GROUP II. 589 b. Some of the Acids of the Second Group from Acids of the First Group. As it is often inconvenient for the further separation of 196 the acids of the second group to have them all in the form of insoluble silver compounds, the analysis is sometimes effected by separating first the acid of the first group, then that of the second. If the quantity of substance is large enough, the most convenient way generally is to determine the several acids, e.g., sulphuric acid, phosphoric acid, chlorine, sulphur, . If you have to analyze a mixture of a nitrate or chlorate 228 with some other salt, determine in one portion the nitric or chloric acid volumetrically ( 149, II., d, a, or /?, or II., e, and 150), or the nitric acid by 149, II., a, ft ; and in another portion the other acid. I think I need hardly remark that no substances must be present which would interfere with the application of these methods. c. From the chlorides of many metals whose carbonates or 229 normal phosphates are insoluble, chlorates and nitrates may be separated also by digesting the solution with recently pre- cipitated thoroughly washed silver carbonate or normal silver phosphate in excess, and boiling the mixture. In this process, the chlorides react with the carbonate or phosphate silver chloride and carbonate or phosphate of the metal with which the chlorine was originally combined being formed, which both separate, together with the excess of the silver carbon- ate or phosphate, whilst the chlorates and nitrates remain in solution (H. ROSE, CHENEVIX, LASSAIGNE*). d. The estimation of an alkaline chlorate, in presence of 230 a chloride, may be effected also by precipitating one portion at once, and another portion after gentle ignition, with solu- tion of silver, and calculating the chloric acid from the differ- ence between the two precipitates. e. Where you have nitrate of soda or potash in presence of 231 * Journ. de Pharm. 16, 289; Pharm. Centralbl. 1850, 121. 170.] ACIDS OF GROUP III. 603 nitrite or carbonate, as for instance in the commercial alkali nitrites, estimate in one portion the carbonate by standard acid (see Special Part),* in another portion the nitrous acid by permanganate or chromate of potash (p. 365). The nitrate is found by difference. II. SEPARATION OF THE Acros OF THE THIRD GROUP FROM EACH OTHER. We have as yet no method to effect the direct separation 232 of nitric acid from chloric acid ; the only practicable way, therefore, is to determine the two acids jointly in a portion of the compound, by the method described for nitric acid, 149, II., dj a, bearing in mind that 12 atoms iron are converted from a ferrous to a ferric salt by 2 mol. chloric acid (HC1O 8 ) or 1 mol. chloric anhydride (C1 2 O 5 ). In another portion esti- mate the chloric acid, by adding sodium carbonate in excess, evaporating to dryness, fusing the residue until the chlorate is completely converted into chloride, and then determining the chlorine in the latter, taking care that the silver chloride contains no difficultly soluble nitrite. 2 mol. silver chloride produced from this corresponds to 2HC1O 3 or C1 2 O 6 , provided there was no chloride originally present. *The alkali nitrites have no alkaline reaction. SECTION" VI. OKGANIC ANALYSIS. 171. ORGANIC compounds contain comparatively only few of the ele- ments. A small number of them consist simply of 2 elements, viz., C and H ; the greater number contain 3 elements, viz., as a rule, C, H, and O ; most of the rest 4 elements, viz., generally, C, H, O, and N ; a small number 5 elements, viz., C, H, O, N, and S ; and a few, 6 elements, viz., C, H, O, N, S, and P. This applies to all the natural organic compounds which have as yet come under our notice. But we may artificially prepare organic compounds containing other elements besides those enu- merated ; thus we know many organic substances, which contain chlorine, iodine, or bromine ; others which contain arsenic, anti- mony, tin, zinc, platinum, iron, cobalt, etc.; and it is quite impos- sible to say which of the other elements may not be similarly capable of becoming more remote constituents of organic com- pounds (constituents of organic radicals). With these compounds we must not confound those in which organic acids are combined with inorganic bases, or organic bases with inorganic acids, such as tartrate of lead, for instance, silicic ether, borate of morphia, etc. ; 'since in such bodies any of the ele- ments may of course occur. Organic compounds may be analyzed either with a view simply to resolve them into their proximate constituents ; thus, for instance, a gum-resin into resin, gum, and ethereal oil ; or the analysis may have for its object the determination of the ultimate constituents (the elements) of the substance. The simple resolu- 171.] ORGANIC ANALYSIS. 605 tion of organic compounds into their proximate constituents is effected by methods perfectly similar to those used in the analysis of inorganic compounds ; that is, the operator endeavors to sepa- rate (by solvents, application of heat, etc.) the individual constitu- ents from one another, either directly, or after having converted them into appropriate forms. We disregard here altogether this kind of organic analysis of which the methods must be nearly as numerous and varied as the cases to which they are applied and proceed at once to treat of the second kind, which may be called the ultimate analysis of organic bodies. The ultimate analysis of organic bodies (here termed simply, organic analysis) has for its object, as stated above, the determi- nation of the elements contained in organic substances. It teaches us how to isolate these elements or to convert them into com- pounds of known composition, to separate the new compounds formed from one another, and to calculate from their several weights, or volumes, the quantities of the elements. Organic analysis, therefore, is based upon the same principle upon which rest most of the methods of separating and determining inorganic compounds. The conversion of most organic substances into distinctly characterized and readily separable products, the weights of which can be accurately determined, oilers no great difficulties, and organic analysis is therefore usually one of the more easy tasks of analytical chemistry ; and as, from the limited number of the ele- ments which constitute organic bodies, there is necessarily a great sameness in the products of their decomposition, the analytical process is always very similar, and a few methods suffice for all cases. It is principally ascribable to this latter circumstance that organic analysis has so speedily attained its present high degree of perfection : the constant examination and improvement of a few methods by a great number of chemists could not fail to produce this result. An organic analysis may have for its object either simply to ascertain the relative quantities of the constituent elements of a substance thus, for instance, woods may be analyzed to ascertain their heating power, fats to ascertain their illuminating power or to determine not only the relative quantities of the constituent elementary atoms, but also the number of atoms of carbon, hydro- gen, oxygen, &c., which constitute 1 molecule of the analyzed 606 ORGANIC ANALYSIS. [ 172. compound. In scientific investigations we have invariably the latter object in view, although we are not yet able to achieve it in all cases. These two objects cannot well be attained by one opera- tion ; each requires a distinct process. The methods by which we ascertain the proportions of the con- stituent elements of organic compounds may be called collectively the ultimate analysis of organic bodies, in a more restricted sense ; whilst the methods which reveal to us the absolute number of elementary atoms constituting the molecule of the analyzed compound may be styled the determination of the molecular weight of organic bodies. The success of an organic analysis depends both upon the method and its execution. The latter requires patience, circum- spection, and skill; whoever is moderately endowed with these gifts will soon become a proficient in this branch. The selection of the method depends upon the knowledge of the constituents of the substance, and the method selected may require certain modifi- cations, according to the properties and state of aggregation of the same. Before we can proceed, therefore, to describe the various methods applicable in the different cases that may occur, we have first to occupy ourselves here with the means of testing organic bodies qualitatively. I. QUALITATIVE EXAMINATION OF ORGANIC BODIES. It is not necessary, for the correct selection of the proper method, to know all the elements of an organic compound, since, for instance, the presence or absence of oxygen makes not the slighest difference to the method. But with regard to other ele- ments, such as nitrogen, sulphur, phosphorus, chlorine, iodine, bromine, . Fluids are treated with fuming nitric acid, or with a mixture of nitric acid and potassium chlorate, at first in the cold, finally with application of heat ; the solution is tested as in a. c. As the methods a and b serve simply to indicate the presence of sulphur in a general way, but afford no information regarding the state or form in which that element may be present, I add here another method, which serves to detect only -the sulphur in the non-oxidized state in organic compounds. Boil the substance with strong solution of potassa and evap- orate nearly to dryness. Dissolve the residue in a little water, and bring the solution into a small flask provided with a loosely-fitting stopper, through which passes a funnel tube reaching nearly to the bottom of the flask. Suspend from the lower surface of the stopper within the flask a strip of paper dipped first in lead acetate, then in ammonium carbonate solution. Add slowly dilute sulphuric acid, and observe whether the lead paper becomes brown ; or test the first alkaline solution by means of a polished surface of silver, or by nitroprusside of sodium, or by just acidifying the dilute solution with hydrochloric acid, and adding a few drops of a mixture of ferric chloride and potassium ferricyanide (see " Qual. Anal." 159). 3. Testing for Phosphorus. The methods described in 2, a and J, may likewise serve for phosphorus. The solutions obtained are tested for phosphoric acid with magnesium sulphate or chloride ; or with ferric chloride, with addition of sodium acetate ; or with solution of molybdie acid (comp. " Qual. Anal."). In method b, the greater part of the excess of nitric acid must first be removed by evaporation. 4. Testing for Inorganic Substances. A portion of the substance is heated on platinum foil, to see whether or not a residue remains. When acting upon difficultly combustible substances, the process may be accelerated by heating the spot which the substance occupies on the platinum foil to the 173.] . ORGANIC ANALYSIS. 609 most intense redness, by directing the flame of the blow-pipe upon it from below. The residue is then examined by the usual methods. That volatile metals in volatile organic compounds e.g., arsenic in kakodyl cannot be detected by this method need hardly be mentioned. These preliminary experiments should never be omitted, since neglect in this respect may give rise to very great errors. Thus, for instance, taurin, a substance in which a large proportion of sulphur was afterwards found to exist, had originally the formula C 4 JS T 2 H 14 O IO assigned to it. The preliminary examination of organic substances for chlorine, bromine, and iodine is generally unneces- sary, as these elements do not occur in native organic compounds, and as their presence in compounds artificially produced by the action of the halogens requires generally no further proof. Should it, however, be desirable to ascertain positively whether a substance does or does not contain chlorine, iodine, or bromine, this may be done by the methods given 188. II. DETERMINATION OF THE ELEMENTS IN ORGANIC BODIES.* 178. A. ANALYSIS OF COMPOUNDS WHICH CONSIST SIMPLY OF CARBON AND HYDROGEN, OR OF CARBON, HYDROGEN, AND OXYGEN. The principle of the method which serves to effect the quanti- tative analysis of such compounds is exceedingly simple. The substance is burned to carbonic acid and water ; these products are separated from each other and weighed, and the carbon of the substance is calculated from the weight of the carbonic acid, the hydrogen from that of the water. If the sum -of the carbon and hydrogen is equal to the original weight of the substance, the substance contains no oxygen ; if it is less than the weight of the substance, the difference expresses the amount of oxygen present. The combustion is effected either by igniting the organic sub- stance with oxygenized bodies which readily part with their oxygen (cupric oxide, lead chromate, &c.) ; or at the expense both of free and combined oxygen. a. SOLID BODIES. * [For Prof. Warren's admirable methods we must refer to his original papers in Am. Journ. Sci., 3d ser., vol. 38, p. 387, vol. 41, p. 40, and vol. 42, p. 156.] 610 ORGANIC ANALYSIS.. [ COMBUSTION WITH CUPRIC OXIDE. Applicable (with modification described in 176) to non-volatile organic compounds not containing chlorine, bromine, iodine, alkali metals, alkali-earth metals, nitrogen, or sulphur. 174. I. APPARATUS AND PREPARATIONS REQUIRED FOR THE ANALYSIS. 1. THE SUBSTANCE. This must be most finely pulverized and perfectly pure and dry ; for the method of drying, I refer to 26. 2. A TUBE IN WHICH TO WEIGH THE SUBSTANCE, made of thin glass about 20 cm. long, and of 7 mm. internal diameter ; one end of the tube is closed by fusion ; the other, during the operation of weighing, is stopped with a smooth cork. 3. THE COMBUSTION TUBE. A tube of difficultly fusible glass (potassa glass), about 2 mm. thick in the glass, 80 to 90 cm. in length, and from 12 to 14 mm. inner diameter, is softened in the middle before a glass-blower's lamp, drawn out as represented in fig. 71, and finally apart at b. The fine points of the two pieces. FIG. 71. are then sealed and thickened a little in the flame, and the sharp edges of the open ends, a and c, are slightly rounded by fusion, care being taken to leave the aperture perfectly round. The posterior part of .the tube should be shaped as shown in fig. 72, and not as in fig. 73. FIG. 72. FIG. 73. Two perfect combustion tubes are thus produced. The one intended for immediate use is cleaned with linen or paper attached to a piece of wire, and then thoroughly dried. This is effected either by laying the tube, with a piece of paper twisted over its 174. ORGANIC ANALYSIS. 611 mouth, for some time on a sand-bath, with occasional removal of the air from it by suction, with the aid of a glass tube, or (rapidly) by moving the tube to and fro over the flame of a gas or spirit lamp, heating its entire length, and continually removing the hot air by suction through the small glass tube (Fig. 74). FIG. 74. The combustion tube, when quite dry, is closed air-tight with a cork, and kept in a warm place until required for use. In default of glass tubes possessed of the proper degree of infusibility, thin brass or copper foil, or brass gauze, is rolled round the tube, and iron wire coiled round it. 4. THE POTASH BULBS (fig. 75). This apparatus, devised by LIEBIG, is filled to the extent indicated in the engraving, with a clear solution of caustic potassa of 1*27 S P- g r - ( 6$, '0- The introduction of the solution of potassa into the apparatus is effected by plunging the end a into a beaker or dish into which a little of the solution has been poured out, and apply- ing suction to b, by means of a caoutchouc tube. The two ends are then wiped per- fectly dry with twisted slips of paper, and the outside of the apparatus with a clean cloth. FlG - 75 - 5. THE CALCIUM CHLORIDE TUBE (fig. 76) is filled in the following manner : In the first place, the neck between the two bulbs of the tube is loosely stopped with a small cotton plug ; this is effected by introducing a loose cotton plug into the wide tube, and applying a sudden and energetic suction at the other end. The large bulb is then filled with lumps of calcium chloride ( 66, 8, #), and the tube with smaller fragments, intermixed with coarse powder of the same substance .; a loose cotton plug is then inserted, and the tube finally closed with a perforated cork, into which a small glass tube is fitted ; the protruding part of the cork 612 ORGANIC ANALYSIS. [ 174. is cut off, and the cut surface covered over with sealing-wax ; the edge of the little tube is slightly rounded by fusion. In using this tube a considerable quantity of the water con- denses in the empty bulb a, and at the close of the experiment FIG. 76. may be poured out. The operator is thus enabled to test it as to reaction, &c., and also to use the same tube far oftener without fresh filling than he could otherwise. 6. A SMALL TUBE OF VULCANIZED INDIA-RUBBER. This must be so narrow that it can only be pushed with difficulty over the tube of the calcium chloride tube on the one hand, and over the end of the potash bulbs on the other hand ; in which case there is no need of binding with silk cord. If the rubber tube should be a little too wide, it must be tied round with silk cord, or with ignited piano wire. It is self-evident that the narrow end of the calcium chloride tube should be of the same width as the tube a of the potash bulbs. The india-rubber tube is purified from any adherent sulphur, and dried in the water-bath previous to use. 7. CORKS. These should be soft and smooth, and as free as possible from visible pores. A cork should be selected which, .after careful squeezing, fits perfectly tight, and screws with some difficulty to one-third of its length, at the most, into the mouth of the combustion tube; a perfectly smooth and round hole, into which the end b of the chloride of calcium tube must fit perfectly air-tight, is then carefully bored through the axis of the cork. The cork is then kept for an hour of two in the water-bath. It is advisable always to have two corks of this description ready. Instead of ordinary corks, caoutchouc stoppers may be used with great advantage. 8. OXIDE OF COPPER. A Hessian crucible, of about 100 c.c. capacity, is nearly filled with oxide of copper prepared as directed in 66, 1 ; the crucible is covered with a well-fitting overlap- ping lid, and heated to dull redness with charcoal, or in a suitable gas-furnace ; it is then allowed to cool, so that by the time the oxide of copper is required for use, the hand can only just bear contact with it. 174.] OKGANIC ANALYSIS. 613 9. A WIDE GLASS TUBE sealed at one end, or a FLASK (fig. 77), in which the freshly ignited oxide of copper is allowed to cool, and from which it is transferred to the combustion tube, secure from the possible absorption of moisture from the air. The freshly ignited and still quite hot oxide of copper is transferred direct from the crucible to this filling tube, or flask, which is then closed air-tight with a cork. It saves time to fill in at once a sufficient quantity of oxide to last for several analyses. If the cork fits tight, the con- tents will remain several days fit for use, even though a portion has been taken out, and the tube repeatedly opened. Fi g- 77. 10. A MIXING WERE of copper (fig. 78) with ring at one end Fig. 78. for a handle and a single corkscrew turn at the other, which should taper smoothly to a point. D ^ 11. A COMBUSTION-FURNACE. Some time ago the only one used was LIEBIG'S, in which charcoal is the fuel.' Eecently gas combustion furnaces have been introduced into most laboratories, because they are Fig. 79. more cleanly and convenient. a. LIEBIG'S combustion-furnace is of sheet-iron. It has the form of a long box, open at the top and behind. It serves to heat the combustion tube with red-hot charcoal. Fig. 79 represents the furnace as seen from the top. It is from 50 to 60 cm. long, and from 7 to 8 deep ; the bot- tom, which, by cutting small slits in the sheet-iron, is converted into a grating, has a width of about 7 cm. The side walls are inclined slightly outward, so that at the top they stand about 12 Fig. 80. Fig. 81. cm. apart. A series of upright pieces of strong sheet-iron, having the form shown in Z>, fig. 80, and riveted on the bottom of the 614 ORGANIC ANALYSIS. [ 175. furnace at intervals of about 5 cm., serves to support the com- bustion tube. They must be of exactly corresponding height with the round aperture in the front piece of the furnace (fig. 80, A). This aperture must be sufficiently large to admit the com- bustion tube easily. Of the two screens used, one has the form shown in fig. 81, the other is a single plate precisely like the end piece of the furnace (fig. 79). The openings cut into the screens must be sufficiently large to receive the combustion tube without difficulty. The furnace is placed upon two bricks resting upon a flat surface, and is slightly raised at the farther end, by inserting a piece of wood between the supports (see fig. 84). The apertures of the grating at the anterior end of the furnace must not be blocked up by the supporting bricks. In cases where the combustion tubes are of good quality, the furnace may be raised by introducing a little iron rod between the furnace and the supporting brick. Placing the tube in a gutter of Kussia sheet- iron tends greatly to preserve it, but contact of the glass and iron must be prevented by an intervening layer of asbestos. I. Gas combustion furnaces of the most various descriptions have been proposed. 175. II. PERFORMANCE OF THE ANALYTICAL PROCESS. a. Weigh first the potash apparatus, then the calcium chloride tube. Introduce about 0'35 0'6 grin, of the substance under examination (more or less, according as it is rich or poor in oxygen) into the weighing tube,* which must be no longer warm, and weigh the latter accurately with its contents. The weight of the empty tube being approximately known, it is easy to take the right quantity of substance required for the analysis. Close the tube then with a smooth cork. ~b. The filling of the combustion tube is effected as follows : The perfectly dry tube is rinsed with some oxide of copper; a layer of oxide of copper, about 13 cm. long, is introduced into the posterior end of the combustion tube, by inserting the latter into the filling tube or flask containing the oxide of copper * Care must be taken that no particles of the substance adhere to the sides of the tube, at least not at the top. 175.] ORGANIC ANALYSIS. 615 (fig. 82), holding both tubes in an oblique direction, and giving a few gentle taps. Fig. 82. From the tube containing the substance remove the cork cautiously, to prevent the slightest loss of substance ; insert the open end of the tube as deep as possible into the combustion tube, and pour from it the requisite quantity of substance by giving it a few turns, pressing the rim all the while gently against the upper side of the combustion tube, to prevent its coming into contact with the powder already poured out ; the two tubes are, in this manipulation, held slightly inclined (see fig. 83). Fig. 83. When a sufficient quantity of the substance has been thus transferred from the weighing to the combustion tube, the latter is restored to the horizontal position, which gives to the former a gentle inclination with the closed end downwards. If the little tube is now slowly withdrawn, with a few turns, the powder near the border of the opening falls back into it, leaving the opening free for the cork. The tube is then immediately corked and weighed, the combustion tube also being meanwhile kept closed with a cork. The difference between the two weighings shows the quantity of substance transferred from the weighing to the combustion tube. The latter is then again opened, and a quantity of oxide of copper, equal to the first, transferred to it from the filling tube, or flask, taking care to rinse down with this the particles of the substance still adhering to the sides of the tube. 616 ORGANIC ANALYSIS. [ 175. There is now in the hind part of the tube a layer of oxide of copper, about 25 cm. long, with the substance in the middle. The next operation is the mixing : this is performed with the aid of the wire (fig. 78), which is pushed down to within 3 to 4 cm. of the end, and rapidly moved about in all directions until the mixture is complete and uniform, the tube being held nearly horizontal. Oxide of copper is then poured in to within 5 to 6 cm. of the open end,, and the tube is corked. c. A few gentle taps on the table will generally suffice to shake together the contents of the tube, so as to completely clear the tail from oxide of copper, and leave a free passage for the evolved gas from end to end. Should this fail, as will occasionally happen, owing to malformation of the tail, the object in view may be attained by striking the mouth of the tube several times against the side of a table. d. Connect the end b (fig. 84) of the weighed calcium chloride tube with the combustion tube by means of a dried perforated cork, lay the furnace upon its supports, with a slight inclination forward, and place the combustion tube in it ; connect the end Fig. 84. of the calcium chloride tube, by means of a vulcanized india- rubber tube, with the end m of the potash apparatus, and, if necessary, secure the connection with silk cord, taking care to press the joint of the two thumbs close together whilst tightening the cords, since otherwise, should one of the cords happen to give way, the whole apparatus might be broken. Rest the potash apparatus upon a folded piece of cloth. Fig. 84 shows the whole arrangement. e. To ascertain whether the joinings of the apparatus fit air- tight, put a piece of wood about the thickness of a finger (*), or a 175.] ORGANIC ANALYSIS. 617 cork or other body of the kind, undeT the bulb r of the potash apparatus, so as to raise that bulb slightly (see fig. 84). Heat the bulb m, by holding a piece of red-hot charcoal near it, until a certain amount of air is driven out of the apparatus ; then remove the piece of wood (), and allow the bulb m to cool. The solution of potassa will now rise into the bulb m, filling it more or less ; if the liquid in m preserves, for the space of a few minutes, the. same level which it has assumed after the perfect cooling of the bulb, the joinings may be considered perfect ; should the fluid, on the other hand, gradually regain its original level in both limbs of the apparatus, this is a positive proof that the joinings are not air- tight. (The few minutes which elapse between the two observa- tions may be advantageously employed in reweighing the little tube in which the substance intended for analysis was originally weighed.) f. Let the mouth of the combustion tube project a full inch beyond the furnace ; suspend the single screen over the anterior end of the furnace, as a protection to the cork ; put the double screen over the combustion tube about two inches farther on (see fig. 84), replace the little piece of wood (s) under r, and put small pieces of red-hot charcoal first under that portion of the tube which is separated by the screen ; surround this portion gradually altogether with ignited charcoal, and let it get red-hot ; then shift the screen an inch farther back, surround the newly exposed portion of the tube also with ignited charcoal, and let it get red- hot ; and proceed in this manner slowly and gradually extending the application of heat to the tail of the tube, taking care to wait always until the last exposed portion is red-hot before shifting the screen, and also to maintain the whole of the exposed portion of the tube before the screen in a state of ignition, and the projecting part of it so hot that the fingers can hardly bear the shortest con- tact with it. The whole process requires generally from f to 1 hour. It is quite superfluous, and even injudicious, to fan the charcoal constantly ; this should be done however when the process is draw- ing to an end, as we shall immediately have occasion to notice. The liquid in the potash bulbs is gradually displaced from the bulb in upon the application of heat to the anterior portion of the combustion tube, owing simply to the expansion of the heated air. The evolution of gas proceeds with greater briskness when the heat begins to reach the actual mixture ; the first bubbles are only 618 ORGANIC ANALYSIS. [ 175. partly absorbed, as the carbonic acid contains still an admixture of air ; but those which follow are so completely absorbed by the potassa, that a solitary air-bubble only escapes from time to time through the liquid. The process should be conducted in a manner to make the gas- bubbles follow each other at intervals of from to 1 second. Fig. 85 shows the oper position of the potash bulbs during the operation. It will be seen from this that an air- bubble entering through m passes first into the bulb &, thence to . 183. . 1. When nitrogenous substances are ignited with oxide of cop- per or with lead chromate, a portion of the nitrogen present escapes in the gaseous form, together with the carbonic acid and aqueous vapor; whilst another portion, minute indeed, still, in bodies abounding in oxygen, not quite insignificant, is converted into nitric oxide gas, which is subsequently transformed wholly or partially into nitrous acid by the air in the apparatus. The appli- cation of the methods described in 174, etc., in the analysis of nitrogenous substances would accordingly give too much carbon ; since the potash bulbs would retain, besides the carbonic acid, also the nitrous acid formed and a portion of the nitric oxide (which in the presence of potassa decomposes slowly into nitrous acid and nitrous oxide). This defect may be remedied by selecting a com- bustion tube about 12 15 cm. longer than those commonly employed, filling this in the usual way, but finishing with a loose layer, about 9 12 cm. long, of clean, fine copper turnings ( 66, 6), or a compact roll of copper wire-gauze. The roll of copper gauze in front of the oxide should not be previously oxidized (as is recommended for substances free from nitrogen chlorine and 634 ORGANIC ANALYSIS. [ 183. bromine), but should be in the metallic state*. The process is com- menced by heating these copper turnings to redness, in which state they are maintained during the whole course of the operation. These are the only modifications required to adapt the methods above described for the analysis of nitrogenous substances. The use of the metallic copper depends upon its property of decompos- ing, when in a state of intense ignition, all the oxides of nitrogen into oxygen, with which it combines, and into pure nitrogen gas. As the metal exercises this action only when in a state of intense ignition, care must be taken to maintain the anterior part of the tube in that state throughout the process. As metallic copper recently reduced retains hydrogen gas, and, when kept for some time, aqueous vapor condensed on the surface, the copper turnings intended for the process must be introduced into the tube hot as they come from the drying closet (which is heated to 100). v. LIEBIG recommends to compress the hot turnings in a tube into a cylindrical form, to facilitate their rapid introduction into the combustion tube. 2. If it is intended to burn nitrogenous bodies in the apparatus described in 178, care must be taken to keep at least the anterior half of the roll from oxidizing, both during the ignition in the current of air and during the actual process of combustion. When the operation is terminated, and the oxidation of the metallic copper is visibly progressing, the oxygen is turned off, and the cock of the air gasometer opened a little instead, to let the tube cool in a slow stream of atmospheric air. 3. Since the metallic copper is usually oxidized during each combustion and must be reduced again, STEmf uses silver instead of copper. Silver has the additional advantage that it retains also chlorine. According to the investigations of CALBERLA, silver at a red heat reduces oxides of nitrogen completely, while it does not exercise the least influence on carbonic acid. b. DETERMINATION OF THE NITROGEN IN ORGANIC COM- POUNDS. As already indicated, two essentially different methods are in * The copper turnings or gauze cannot be replaced by the metallic powder obtained by the reduction of the oxide with hydrogen, as this obstinately retains hydrogen, and consequently decomposes appreciable quantities of carbonic acid with formation of carbonic oxide. Schr5tter, Lautemann, Journ. f. prakt. Chem. 77, 316. f Zeitschrift f. anal. Chem. 8, 83. 184. J ORGANIC ANALYSIS. 635 use for effecting the determination of the nitrogen in organic com- pounds ; viz., the nitrogen is either separated in the pure form and its volume measured, or it is converted into ammonia, and this is determined either as ammonium platinic chloride, or volumetric- ally by neutralization. a. Determination of the Nitrogen from the Volume. 184. aa. DUMAS' Method, modified by Schiel. This method may be employed in the analysis of all organic compounds containing nitrogen. It requires a graduated glass cylinder of about 200 c.c. capacity, with a ground-glass plate to ver it. The combustion tube should be 60 or 70 cm. long, and drawn out at the posterior end to a stout open tail, which should have a small bulb or swell for the better fastening of a rubber tube to it. Introduce into it near the tail a plug of newly ignited asbestos, Fig. 93 then a layer of oxide of copper, 4 cm. long ; after this the intimate mixture of an accurately weighed portion of the substance (0*3 0*6 grm., or, in the case of compounds poor in nitrogen, a some- what larger quantity) with oxide of copper, then the oxide which lias served to rinse the mortar, followed by a layer of pure oxide, and, lastly, a layer of copper turnings, about 15 cm. long. Make a channel along the top of the tube by gentle tapping. Connect the tube with the bent delivery tube cf (fig. 93), and place in the furnace. Connect the tail by means of a stout tube of india-rub- ber with an apparatus for giving a continuous stream of washed carbonic acid gas. Transmit this slowly through the tube for half an hour, then immerse the end of the bent delivery tube under mercury, and invert over it a test tube filled with solution of 636 ORGANIC ANALYSIS. [ 184. potassa. If the gas bubbles entering the cylinder are completely absorbed by the solution of potassa, this is a proof that the air is thoroughly expelled from the tube. But should this not be the case, the evolution of carbonic acid must be continued until the desired point is attained. "When the gas is completely absorbed, close the communication between the CO 2 generator and the com. bustion tube by a screw clamp or stopcock, invert the graduated cylinder, filled -f with mercury, -J with concentrated solution of potassa, over the end of the delivery tube, with the aid of a ground-glass plate,* and proceed with the combustion in the usual way, heating first the anterior end of the tube to redness, and advancing gradually towards the farther end. In the last stage of the process, communication is reestablished with the CO 2 genera- tor, and thus the whole of the nitrogen gas which still remains in the tube is forced into the cylinder. Wait now until the volume of the gas in the cylinder no longer decreases, even upon shaking the latter (consequently, until the w T hole of the carbonic acid has been absorbed), then place the cylinder in a large and deep glass vessel filled with water, the transport from the mercurial trough to this vessel being effected by keeping the aperture closed with a small dish filled with mercury. The mercury and the solution of potassa sink to the bottom, and are replaced by water. Immerse the cylin- der, then raise it again until the water is inside and outside on an exact level ; read off the volume of the gas and mark the tempera- ture of the water and the state of the barometer ; calculate the weight of the nitrogen gas from its volume, after reduction to the normal temperature and pressure, and with due regard to the ten- sion of the aqueous vapor (comp. " Calculation of Analyses"). The results are generally somewhat too high, viz., by about O2 0*5 per cent. ; this is owing to the circumstance that even long-con- tinued transmission of carbonic acid through the tube fails to expel every trace of atmospheric air adhering to the oxide of copper. * The following is the best way of filling the cylinder and inverting it over the opening of the bent delivery tube : The mercury is introduced at first, and the air-bubbles which adhere to the walls of .the vessel are removed in the usual way. The solution of potassa is then poured in, leaving the top of the cylinder free to the extent of about 2 lines; this is cautiously filled up to the brim with pure water, and the ground-glass plate slided over it. The cylinder is now inverted, and the opening placed under the mercury in the trough ; the glass plate is then withdrawn from under the cylinder. In this manner the operation may be performed easily, and without soiling the fingers. 184.] ORGANIC ANALYSIS. 637 It is highly advisable, before making any nitrogen determina- tions with this method, to subject a non-nitrogenous substance, e.g., sugar, to the same process. The analyst thereby acquaints himself with the extent of the error to which he will be exposed. In such an experiment the quantity of unabsorbed gas should not exceed 1 or 1 c.c. To insure complete combustion of difficultly combustible bod- ies, STRECKER recommends the addition of arsenious oxide in pow- der to the oxide of copper with which the substance is to be mixed ; the arsenious oxide is volatilized by the action of the heat, the fumes burning the whole of the carbon like a current of oxygen. The arsenious oxide sublimes in the anterior part of the tube, arsenic remains in the copper. bb. By exhaustion of the combustion tube with an air pump, ami measurement of nitrogen in Schiff^s Azotometer. A process capable of giving much more accurate results than the preceding (ad) has been developed by FRANKLAXD and ARM- STRONG,* GIBBS \ and JOHNSON. It is described \ as follows : REAGENTS. 'Cupric oxide. " Copper scale," which may contain cuprous oxide, coal dust,' oil, &c., is mixed in an iron pot with 10 per cent. of potassium chlorate and enough water to make a thin paste. The mass is heated and stirred till dry, the heat is then raised to the point of ignition, and until the mass does not glow nor sparkle when stirred. The potassium chloride is washed out by decantation and the cupric oxide is dried and moderately ignited. Metallic copper. Granular copper oxide, or fine copper gauze, is suitable for its preparation. The granular copper is most con-, venient ; copper gauze must be made into rolls adapted to the combustion tube. The copper is reduced and cooled as usual in a stream of hydrogen. Potassium chlorate. Commercial potassium chlorate is fused in porcelain and pulverized. Sodium bicarbonate must contain no organic matter. * Jour. Chem. Soc. [ii], vol. vi. p. 77. f Ara.Journ.Sci. and Arts, vol. xlviii. J By JOHNSON and JENKINS, American Chemical Journal, ii. 27. 638 ORGANIC ANALYSIS. [ 184. Solution of Caustic Potash. Dissolve commercial " stick pot- ash" in less than its weight of water, making a solution so concen- trated that, on cooling, it deposits crystals of potassium hydrate. The same clear solution may be used for a number of combus- tions or until the absorption of carbonic acid gas is not quite prompt. APPARATUS. The Combustion tube should be of the best hard Bohemian glass, about 2 feet 4 inches long. The rear end is bent and sealed as in. fig. 96. It is best to protect the horizontal part with thin copper foil. The tube is connected with the pump by a close fitting rubber cork, smeared with glycerine. Azotometer. This is a modification of the apparatus invented and described by Schiif, Fres. Zeitschrift, Bd. 7, p. 430. It is represented in fig. 94. The gas is measured in an accurately calibrated cylinder (bu- rette) A of 120 c. c. capacity, graduated to . fifths of cubic centimetres, and closed at the upper end by a glass stopcock. The lower end is connected, by means of a perforated rubber stopper about 1J inches long and 1^ inches diameter, with another tube hav- ing two arms, one, D, to receive the delivery tube from the pump, the other connected by a rubber tube with a bulb of 200 c. c. capacity, F, through which potash solution is supplied. The graduated tube is en- closed in a water-jacket with an external diameter of about If inches. Its lower end is closed by the caoutchouc stopper that connects the two parts of the azotometer described above. The upper end of the jacket is closed by a thin rubber disc, slit radially and having four perforations : one in the centre, through which the neck of the graduated tube passes, and three others near the circumference. Through one of the latter, a glass tube, L, bent as in the figure, reaches to the bottom of the jacket, another short tube just passes Fig. 94. 184.] ORGANIC ANALYSIS. 639 through the disc, and the third hole is for supporting a thermo- meter. The azotometer is held upright and firm on a stand by rings fitting around the jacket and by cork wedges. The bulb for potash solution rests in a slotted, sliding ring. The air pump used is the Sprengel mercury pump, modified merely so as to be easily constructed and durable. Its essential parts are sketched in fig. 95. Some of them are exaggerated in order to show their construction more plainly. Through a rubber stopper wired into the nozzle of the mercury reser- voir, A, passes a glass tube, B, 4 inches long ; this connects by a caoutchouc tube with the straight tube D, 3 feet long. ^The rubber tube E, 6 inches long, connects D with a straight glass tube, F, of about the same length as D. G is a piece of combustion tube 1^ inches long, closed below by a doubly perforated soft rubber stopper admitting the tubes F and H, and above by a singly perforated rubber stopper into which a tube, I, is fitted. The tube H has a length of 45 inches. At the bottom it is connected by rubber with a straight tube of 3 inches, and this again with a tube, K, of 7 inches. The tubes H K should have an internal diameter of 1 millimetres, F may be 2 millimeters, and D still larger. We have used for H and F slender Bohemian glass tubes of 4 millimetres exterior diameter. Their elasticity compensates for their slenderness. If heavy barometer tubes be used, the stoppers and G must be of correspondingly larger dimensions. The joints at G must be made with the great- est care. It is best to insert the lower stopper for half its length into G, having the dimensions of the parts so related that it requires considerable effort to force the slightly greased tubes F and H to their places just through the stopper. The tube I must be of stout glass a decimetre in diameter. It is drawn out at either end to a long taper, and bent as in the figure, in order to bring its free extremity to the level of the combustion furnace. The hole in the upper rubber stopper has a diameter of 5 mm.. J| 640 ORGANIC ANALYSIS. [ 184. just sufficient to admit the narrowed end of the tube, which, after greasing or moistening with glycerine, is " screwed down" into the stopper. These three joints are the only ones belonging to the pump which have to resist diminished pressure, and require .extreme care in making. If not entirely secure they are to be trapped with glycerine. For this purpose it is needful to pass F and H through a stopper of half an inch greater diameter than G and correspondingly perforated before entering the latter. Then, previous to inserting I, a tube 4 inches long is slipped over G upon this wider stopper. When I has been inserted and the tubes have been secured to their support, the space between G and the outer tube is filled with the most concentrated glycerine, which is prevented from absorbing moisture by corking above. The two rubber tubes are both provided with stout screw clamps, to admit of exactly regulating the flow of mercury. The tubes D, F, H, and I are secured to a vertical plank framed below into a heavy horizontal wooden foot on which rests the mercury trough, and having above a horizontal shelf through an aperture of which passes the neck of A. The tubes D, F, H, and I are secured to the plank at several points by wooden or cork clamps, clasping the tubes and fastened by screws or wires. These fastenings are made elastic by the intervention of a thick rubber tube between the glass and wood. The connections C and E should be made of stout vulcanized rubber, those at the base of H K of fine black rubber. The latter should be soaked in melted tallow previous to use, all excess being carefully removed from the interior. The joints should be wound with waxed silk. A glass funnel is placed within A to prevent spattering of the mercury when it is filled. OPERATION. From 3 to 4 grains of potassium chlorate, according to the amount of carbon to be burned, are put into the tail of the com- bustion tube, fig. 96, followed by an asbestos plug just at the bend. The, substance to be analyzed (O6 0*8 grams) is well mixed in a mortar with enough cupric oxide that has been freshly ignited 184.] ORGANIC ANALYSIS. 641 and allowed to cool to make a layer 11 or 12 inches long in the tube. The mixture is introduced through a funnel and rinsed with enough cupric oxide to make a layer of 3 inches, a second asbestos plug, and upon it a layer of reduced copper of 4 or 5 inches long are put in, then a third asbestos plug, then 2 inches of cupric oxide, a fourth asbestos plug, then -8 to 1' grams of sodium bicarbonate. The remaining space in the tube is loosely filled with asbestos, to absorb the water which is formed during combustion, MIXTURE JRlNSINGSj Cu. jCuO ;co? j ASBESTUS j 1 a < j j 8cm. \ 30cm. | 8cm. I 12cm* iscmlacm! 10cm. j Fig. 96. and prevent it from flowing back upon the heated glass. The anterior part of the tube containing the cupric oxide and reduced copper is wound with copper foil, leaving, however, a little of the copper (Cu. in fig. 96) visible at its rear. The combustion tube is placed in the furnace at the bend of the tube I, and connected with the latter by a close-fitting rubber stopper smeared with glycerine. Care must be taken to make the joint perfectly tight. The combustion tube has its conical rubber stopper partly inserted, and is then forced and rotated upon the tapering and stout end of the tube I, the latter being supported by one hand applied at the lower bend. PREPARATION OF THE AZOTOMETER. Fill the bottom of the azotometer to about the level indicated by the dotted line G, with mercury. Close the arm D securely with a rubber stopper. Grease the stop-cock H and insert the plug, leaving the cock open. Pour potash solution into F till A is nearly full, and there is still some solution in the bulb F. Raise the bulb cautiously with one hand, holding the stop-cock H in the other hand. When the solution in A has risen very nearly to the glass cock, close the lat- ter, avoiding contact of the alkali with the ground glass bearings. Replace the bulb in the ring and lower it as far as may be. If the level of the solution in the azotometer does not fall in 15 or 20 minutes, it is tight. Place the delivery tube of the pump K in a mercury trough. 642 ORGANIC ANALYSIS. [ 184. Supply the vessel A with at least 500 c. c. of mercury. Cau- tiously open the clamps C and E. If the mercury does not start at once pinch the rubber at E repeatedly. The mercury should flow nearly as fast as it can be discharged at K, without filling the cylin- der G. Five to ten Minutes working of the pump will generally suffice to make a complete exhaustion of the combustion tube. If most of the mercury runs out before exhaustion is complete, close- the clamp C, return the mercury to A, and repeat the operation. When there is a complete exhaustion, the mercury falls with a rat- tling or clicking sound. After it has been distinctly heard for half a minute, close the clamp C. If the mercury column in H remains stationary for some minutes, the connections are proved to be tight. ADJUSTING THE AZOTOMETER. Remove the mercury trough, placing K in a capsule. Heat the part of the tube containing sodium bicarbonate. Water vapor and carbon dioxide are evolved, which fill the vacuum in H and expel the mercury. While this is being done place the azoto- meter near by, remove the bulb F from the ring and support it in a box near the level of D, so that the stopper may be removed from D without greatly changing the level of the mercury G, and so that the azotometer can be moved freely without disturbing it. When the cork in D has been removed fill D half full or more with water. As soon as the mercury has fully escaped from K insert the lat- ter in D. Let a few bubbles escape through the water and then pass the tube K down so that the escaping gas enters the azotome- ter. It will much facilitate the delivery of gas if the extremity of the tube K just touches the inside of the azotometer tube, and is kept, as near as possible, to the surface of the mercury. The carbon dioxide is absorbed in passing through the caustic potash solution. In spite of all precautions very minute bubbles of permanent gas will occasionally ascend, but, as will be seen on observing the amount of potash solution thus displaced, the error thereby occasioned is extremely small. THE COMBUSTION. First heat the anterior cupric oxide to full redness, and after- wards the copper. The fine gauze or pulverulent copper very com- 184.] OKGANIC ANALYSIS. 643 pletely reduces any oxides of nitrogen which might be produced in the combustion, and also retains any excess of oxygen which is evolved at the close of the process. The anterior cupric oxide burns the traces of hydrogen which may be held by the reduced copper, even when the tube is exhausted, and also destroys the carbon monoxide which is usually formed when steam and carbon dioxide pass together over reduced copper, if iron or carbon be present. Go on with the combustion as usual, bringing the heat up to a fair redness. The flow of gas may be made quite rapid, say one bubble a second, or a little faster. When the horizontal part of the -tube has all been heated, and the evolution of gas has nearly ceased, heat the potassium chlorate so that it boils vigorously from evolution of oxygen. The reoxidiza- tion of the reduced copper oxide and of any unburned carbon pro- ceeds rapidly. "When the oxygen, whose flow admits of easy regulation, begins to attack the anterior layer of reduced copper, stop its evolution and lower the flames all along the tube, keeping the reduced cop- per still faint red. After a few minutes start the pump, slowly at first, having some vessel under the tube D of the azotometer to receive the mercury. A few minutes pumping suffices to clear the tube. Remove the azotometer, close the tube D with its rubber stopper, then raise the bulb into its ring to such a height that the potash solution in it shall be at about the same level as that in the graduated tube. Con- nect L at its upper end with a water supply, insert a thermometer in the top of the water jacket and let the water run, until the tem- perature and the volume of gas are constant. Read off the volume of gas and temperature, after having accu- rately adjusted the level of the solution in the bulb to that in the azotometer. Read the barometer and make the calculations in the usual way. When 50 per cent, potash solution is used, no correction need be made for tension of aqueous vapor, as SCHIFF has shown. The calculation is somewhat shortened by the use of the table in Jour, of Chem. Soc., Yol. XVIII. (1865) p. 212. Very fair results are got by employing, with suitable precau- tion, a stream of carbon dioxide to displace the air of the combus- tion tube, but the process is very tedious, the sources of error are more numerous, and the results are apt to be higher and not so 644 ORGANIC ANALYSIS. [ 185. accordant as when the mercury pump is used to evacuate the tube. The pump above described has been in use for eighteen months without any repairs, and by its help two or even three analyses may be performed in a day. /3. Determination of Nitrogen l>y conversion into Ammonia. VAKRENTRAPP and WILL'S Method. 185. This method may be applied to all nitrogenous compounds, except those containing the nitrogen in the form of nitric acid, hyponitric acid, &c.* It is based upon the same principle as the method of examining organic bodies for nitrogen ( 172, 1, a\ viz., upon the circumstance that, when nitrogenous bodies are ignited with an alkali hydroxide, the latter is decomposed, yielding water, the oxygen of which combines with carbon to CO,, which remains in combination with the alkali as carbonate, whilst the hydrogen at the moment of its liberation combines with the whole of the nitrogen present to form ammonia. In the case of substances abounding in nitrogen, such as uric acid, mellon, &c., the whole of the nitrogen is not at once con- verted into ammonia in this process ; a portion of it combining with part of the carbon of the organic matter to cyanogen, which then combines, either in that form with the alkali metal, or in the form of cyanic acid with the alkali. Direct experiments have proved, however, that even in such cases the whole of the nitrogen is ultimately obtained as ammonia, if the alkali hydroxide is pres- ent in excess, and the heat applied sufficiently intense. As in all organic nitrogenous compounds the carbon prepon- derates over the nitrogen, the oxidation of the former, at the expense of the water, will invariably liberate a quantity of hydro- gen more than sufficient to convert the whole of the nitrogen pres- ent into ammonia ; for instance, CIS" + 2H 2 = CO, + ]STH 3 + H. [* Vegetable matters, as dried plants, containing not more than 3 per cent, of NO 5 may be analyzed by this method. In a case where 6 per cent, of N 2 O 5 was present, a loss of 0'2 per cent, of N took place in the experiments of E. Schulze. Fres. Zeitschrift vi. 387.] 185.] OKGANIC ANALYSIS. 645 The excess of the liberated hydrogen escapes either in the free state, or in combination with the not yet oxidized carbon, accord- ing to the relative proportions of the two elements and the tem- perature, as marsh gas, olefiant gas, or vapor of readily condensible hydrocarbons, which gases serve in a certain measure to dilute the ammonia. As a certain dilution of that product is necessary for the success of the operation, I will here at once state that sub- stances rich in nitrogen should be mixed with more or less of some non-nitrogenous body sugar, for instance so that there may be no deficiency of diluent gas. The ammonia is determined volumetrically, see 196. aa. Requisites. 1. The objects enumerated 174, and a PORCELAIN MORTAR for mixing the weighed substance. 2. A COMBUSTION TUBE of the kind described 174, 3 ; length about 40 cm., w r idth about 12 mm. The combustion is effected in an ordinary combustion furnace. 3. SODA-LIME ( 66, 5). It is advisable to gently heat in a platinum or porcelain dish, a quantity of the soda-lime sufficient to fill the combustion tube, so as to have it perfectly dry for the pro- cess of combustion. In the analysis of non- volatile substances, the best way is to use the soda-lime while still warm. 4. ASBESTOS. A small portion of this substance is ignited in a platinum crucible previous to use. 5. A VERRENTRAPP AND WILL'S BULB APPARATUS. This may be obtained from the shops. Fig. 97 shows its form. It is filled to the extent indicated in the drawing with standard sulphuric or Fig. 97. hydrochloric acid 192, of which 20 c.c. should be employed. The acid is introduced either by dipping the point into the acid, and applying suction to d, or by means of a burette. 646 OKGANIC ANALYSIS. [ 185. In order to guard against the receding of the acid into the combustion tube, ARENDT and KNOP have sug- gested the form indicated fig. 98. 6. A soft, well-perforated COKK, which fits the combustion tube air-tight, and in which the tube d of the bulb apparatus fits closely. 7. A SUCTION-TUBE of caoutchouc adapted to the point of the bulb apparatus. l)b. The Process. The combustion tube is half filled with soda-lime, which is then gradually transferred to the perfectly dry, and, if the nature of the substance permits, rather warm mortar, where it is most intimately mixed with the weighed substance, forcible pressure being care- fully avoided ; a layer of soda-lime, occupying about 3 cm., is now introduced into the posterior part of the combustion, tube, and the mixture filled in after ; the latter, which will occupy about 20 cm., is followed by a layer of about 5 cm. of soda-lime, which has been used to rinse the mortar, and this again by a layer of 12 cm. of pure soda-lime, leaving thus about 4 cm. of the tube clear. The tube is then closed with a loose plug of asbestos, and a free passage for the evolved gases formed by a few gentle taps ; it is then con- nected with the bulb apparatus by means of the perforated cork, and finally placed in the combustion furnace (see fig. 97). To ascertain whether the apparatus closes air-tight, some air is expelled by holding a piece of red hot charcoal to the bulb a, and the apparatus observed, to see whether the liquid will, upon cooling, permanently assume a higher position in a than in the other limb. The tube is then gradually surrounded with ignited charcoal, com- mencing at the anterior part, and progressing slowly towards the tail, the operation being conducted exactly as in an ordinary com- bustion ( 175). Care must be taken to keep the anterior part of the tube tolerably hot throughout the process, since this will almost entirely prevent the passage of liquid hydrocarbons, the presence of which in the standard acid would be inconvenient. The asbestos should be kept sufficiently hot to guard against its retaining water, and with this, ammonia. The combustion should be conducted so as to maintain a steady and uninterrupted evolu- tion of gas ; there is no fear of any ammonia escaping unabsorbed, even if the evolution is rather brisk ; but the operator must con- stantly be on his guard against the receding of the acid, which g 185.] OKGANIC ANALYSIS. 647 takes place the moment the evolution of gas ceases, and this, in some instances, with such impetuosity as to force the acid into the combustion tube, which of course spoils the whole analysis. This difficulty may be readily met, however, by mixing with the sub- stance an equal quantity of sugar, which will give rise to the evo- lution of more permanent gases diluting the ammonia. When the tube is ignited in its whole length, and the evolu- tion of gas has totally ceased,* the point of the combustion tube is broken off, and air to the extent of several times the volume of the gas in the tube is sucked through the apparatus, to force all the rest of the ammonia into the acid. Liquid nitrogenous compounds are weighed in small sealed glass bulbs, and the process is conducted as directed 180, with this difference, that soda-lime is substituted for oxide of copper. It is advisable to employ tubes of greater length for the combus- tion of liquids than are required for solid bodies. The best method of conducting the operation, is to heat first about one-third of the tube at the anterior end, and then to force the liquid from the bulbs into the tube by heating the hinder end of the latter ; the expelled liquid will thus become diffused in the central part of the tube, without being decomposed. By a progressive application of heat, proceeding slowly from the anterior to the posterior end, a steady and uniform evolution of gas may be easily maintained. When the combustion is terminated, the bulb apparatus is emptied, through the opening at the point, into a beaker, and rinsed with water until the rinsings cease to manifest acid reaction. The excess of acid is determined by means of standard potash or ammonia solution and cochineal tincture, or, if the acid is so colored that the point of neutralization cannot readily be decided by cochineal, employ slips of turmeric paper (see 196). It is advantageous to use a rather dilute acid, 1 c. c.= 0*005 grin, of nitrogen. The receiver (fig. 99) may be advantageously substi- tuted for the bulb-tube. The tube a previously provided with the caoutchouc stopper J is first connected by the aid of a good cork with the combustion tube, and then the U-tube c having been charged with the proper quantity of acid from a MOHK'S burette is added. At the termination of the combustion, when air has * This is indicated by the white color which the mixture reassumes when all the carbon deposited on the surface is oxidized. 648 OKGANIC ANALYSIS. [ 185. been drawn through the apparatus, the tube a is rinsed into the apparatus c, some tincture of cochineal added, and standard alkali run into the tube from a second burette, until the acid is almost neutralized. ~Now pour the contents of the apparatus into a beaker, rinse with water, and complete the neutralization. With this receiver neither receding nor spirting is possible. By not pouring out the fluid till the point of saturation is nearly attained, you require less water for rinsing the tube. This method- is rapid and accurate. [From the results of a critical investigation of Fi"99 this method by JOHNSON and JENKINS* the fol- lowing facts may be here added : 1. The efficiency of the " soda-lime" mixture described 66, 5, is fully confirmed. It is easier to prepare than the mixture of caus- tic lime and soda ( 66,4) formerly used for this purpose, and does not, like the latter, attract moisture readily from the air, and is not liable to swell and choke the tube during combustion. 2. Neither the highest heat possible to obtain in an EKLEN- MEYEK gas combustion furnace, nor a long layer of strongly heated soda-lime, nor these two conditions united, occasion any appreciable dissociation of the ammonia formed in combustion. 3. A suitable length of the anterior layer of soda-lime must be secured in order to get a good result. With O5 gram of sub- stances, such as are encountered in agricultural chemistry, contain- ing less than 8 per cent, of nitrogen, a glass tube of 12 to 14 inches is long enough. As the content of nitrogen increases to 10 per cent or over, the tubes should be made several inches longer. In the combustion of dried blood or egg-albumin a tube 20 25 inches long is preferred, and the mixture of soda-lime and substance should occupy rather less than half the tube, a layer of pure soda- lime of 12 or more inches long being essential for perfectly destroy- ing the volatile organic matters. 4. The* long anterior layer of pure soda-lime must be brought to SL full red heat before heating the mixture, and must be so kept throughout the combustion. 5. No fumes or tarry matters, indicative of incomplete combus- tion, should appear in bulb-tube or receiver. * Report of Connecticut Agr. Exp. Station, 1878, p. 111. 186.] ORGANIC ANALYSIS. 649 6. When the combustion proper is begun under the conditions above described, it can be carried on quite rapidly until completed. The contents of the tubes then show no sign of unburned carbon. 7. Equally good results are obtained whether the mixture is made intimately in a mortar, or more roughly by stirring with a spatula in a metallic capsule or scoop, or by mixing in the tube with a wire.] Iron gas tubes may be substituted for glass tubes. They are closed at the rear with a cork, carrying a bit of glass tube drawn out /to a sealed tail. The mixture is confined to its place by loose asbestos plugs. The corks are kept from charring by wrapping the end of the tube with two or three thicknesses of filter-paper, which is kept wet by a wash-flask, or by dipping the depending end into a vessel of water. The tubes should be 45 cm. long, and 5 cm. at each end should project from the fire and be protected with wet paper. C. ANALYSIS OF ORGANIC COMPOUNDS CONTAINING SULPHUR.* 186. The usuai method of determining the carbon in organic bodies viz., by combustion with oxide of copper or lead chromate would give results too high in the analysis of compounds contain- ing sulphur, since more especially if oxide of copper is used a portion of the sulphur would be converted in the process into sul- phurous acid, which would be absorbed with the carbonic acid in the potash bulbs. CARIUS recommends to burn substances contain- ing sulphur in a tube 60 80 cm. long, with lead chromate, care being taken that the anterior 10 20 cm., which contains pure lead chromate, are never heated above low redness. The lead chromate may be used again three or four times without refusion ; and, finally, if treated by YOHL'S method (p. 124), it is just as fit for use as if it had not been employed for the combustion of a sub- stance containing sulphur. The presence of sulphur demands no modification in the pro- cess described 184 and 185 for the determination of nitrogen. In substances containing oxygen in presence of sulphur, the oxygen is estimated from the loss. [* WARREX'S method of determining carbon, hydrogen, and sulphur in one operation is described in Am. Journ. Sci., vol. 41, 2d ser., p. 40.] 650 ORGANIC ANALYSIS. [ 186. As regards the estimation of the sulphur in organic compounds, that element is invariably weighed in the form of barium sulphate, into which it may be converted either in the dry or in the wet way. a. Methods in the Dry Way. 1. Method suitable , more particularly, to determine the sulphur in non-volatile Substances poor in Sulphur, e.g., in the so-called Protein Compounds (v. LIEBIG). Put some lumps of potassa, free from sulphuric acid ( 66, 7, c) into a capacious silver dish, add -J of pure potassium nitrate, and fuse the mixture, with addition of a few drops of water. When the mass is cold, add to it a weighed quantity of the finely pul- verized substance, fuse over the lamp, stir with a silver spatula, and increase the heat, continuing the operation until the color of the mass shows that the carbon separated at first has been com- pletely consumed. Should this occupy too much time, you may accelerate it by the addition of potassium nitrate in small portions. Let the mass cool, then dissolve in water, supersaturate the solu- tion with hydrochloric acid in a capacious beaker covered with a glass dish, and precipitate with barium chloride. Wash the pre- cipitate well with boiling water, first by decantation, then on the filter.- Dry and ignite. Treat the ignited barium sulphate as directed p. 367; if this latter operation is omitted, the result is almost always too high. A suitable alcohol lamp is preferable to a gas flame, since the latter may communicate sulphur to the fused mass. As it is by no means easy to obtain the required reagents perfectly free from sulphur, it is well to try a parallel experiment, using the same quantities of each that is used for the analysis, and if an appre- ciable amount of barium sulphate is obtained, make the necessary correction in the analysis. 2. Method adapted 'more particularly for the Analysis of non- volatile or difficultly volatile Substances containing more than 5 per cent, of Sulphur (KOLBE *). Introduce into the posterior part of a straight combustion tube,f 40 45 cm. long, a layer, 7 8 cm. long, of an intimate mixture of 8 parts of pure anhydrous sodium carbonate, and 1 part of pure * Supplemente zum Handworterbuch, 205. f Sealed and rounded at the end like a test tube. 186.] ORGANIC ANALYSIS. 651 potassium chlorate ; after tins introduce the weighed substance, then another layer, 7 or 8 cm. long, of the same mixture ; mix the organic compound intimately with the sodium carbonate and potas- sium chlorate, by means of the mixing wire (fig. 78, p. 613) ; fill up the still vacant part of the tube with anhydrous sodium carbon- ate or potassium carbonate mixed with a little potassium chlorate. Clear a wide passage from end to end by a few gentle taps, place the tube in a combustion furnace, heat the anterior part to redness, and then, progressing slowly toward the posterior part, proceed to surround with red-hot charcoal the part occupied b}^ the mixture. In the analysis of substances abounding in carbon, it is advisable to introduce into the posterior part of the tube a few lumps of pure potassium chlorate, to insure complete combustion of the car- bon, and perfect conversion into sulphates of the compounds of potassa with the lower oxides of sulphur that may have formed. The sulphuric acid in the contents of the tube is determined as in 1. 3. Method adapted for the Analysis both of non-volatile and volatile Substances, but more especially the latter (DEBUS *). Dissolve 149 parts of potassium dichromate purified by recrys- tallization, and 106 parts anhydrous sodium carbonate in water, evaporate the solution to dryness, reduce the lemon-colored saline mass to powder, heat to intense redness in a Hessian crucible, and transfer still hot to a filling-tube (fig. 77, p. 613).+ "When the powder is cold, introduce a layer of it, 7 10 cm. long, into a com- mon combustion tube ; then introduce the substance, and after this 1 another layer, 7 10 cm. long, of the powder. Mix intimately by means of the mixing wire, then fill the still unoccupied part of the tube with the saline mixture, and apply heat as in an ordinary ultimate analysis. When the entire mass is heated to redness, conduct a slow stream of dry oxygen gas over it for \ 1 hour. When cold, wipe the ash off the tube, cut the latter into several pieces over a sheet of paper, and treat them in a beaker with a suf- ficient quantity of water to dissolve the saline mass. Add hydro- chloric acid in tolerable excess, then some alcohol, and apply a * Annal. d. Chem. u. Pharm. 76, 90. f The saline mass must always first be tested for sulphur. For this purpose a small portion of it is reduced with hydrochloric acid and alcohol, barium chloride added, and the mixture allowed to stand 12 hours at rest. No trace of a precipitate should be discernible. 652 ORGANIC ANALYSIS. [ 186. gentle heat until the solution shows a beautiful green color ; filter off the chromic oxide produced by the combustion (this contains sulphuric acid) ; wash first with water containing hydrochloric acid, then with alcohol, dry, and transfer to a platinum crucible ; add the filter-ash, mix with 1 part of potassium chlorate and 2 parts of potassium (or sodium) carbonate, and ignite until the chromic oxide is completely converted into alkalin chromate. Dis- solve the fused mass in dilute hydrochloric acid, and reduce by heating with alcohol ; add the solution to the fluid filtered from the chromic oxide, heat the mixture to boiling, and precipitate the sulphuric acid with barium chloride. DEBUS'S test-analyses were very satisfactory ; thus he obtained 99*76 and 99'50 of sulphur for 100, again 30'2 of sulphur in xanthogenamide for 30 '4, &c. 4. Method equally adapted for the Analysis of Solid and Liquid Volatile Compounds. (W. J. RUSSELL ; * suggested by BUNSEN.) Introduce into a combustion tube, 40 cm. long, sealed at the posterior end, first 2 3 grm. pure mercuric oxide, then a mixture of equal parts of mercuric oxide and pure anhydrous sodium car- bonate, mixed with the substance, and fill up the tube with sodium carbonate mixed with a little mercuric oxide. Connect the open end of the tube with a gas delivery tube dipping under water, to effect the condensation of the mercurial fumes. Place a screen in front of the part of the tube occupied by the substance, then heat the anterior part to bright redness, and maintain this temperature during the entire process. At the same time, heat another portion of the tube, nearer to the end, but not to the same degree of inten- sity, so that there may be alternate parts in the tube in which the mercuric oxide is left undecomposed. When the part before the screen is at bright redness, remove the screen, heat the mixture containing the substance, regulating the application of heat so as to insure complete decomposition in the course of 10 15 minutes, and heat at the same time the still unheated parts of the tube, and lastly also the pure oxide of mercury at the extreme end. The gas must be tested from time to time, to ascertain whether it con- tains free oxygen. Dissolve the contents of the tube in water, add some mercuric chloride to decompose the sodium sulphide which may have formed, acidify with hydrochloric acid, oxidize the * Quart. Journ. Chem. Soc. 7, 212. 186.] ORGANIC ANALYSIS. 653 mercuric sulphide which may have formed with potassium chlo- rate, and finally precipitate the sulphuric acid with oarium chlo- ride. "W. J. RUSSELL obtained by this method very satisfactory results in the analysis of pure sulphur, potassium sulphocyanate, and carbon disulphide. b. Method in the Wet Way.* According to RIVOT, BEUDANT, and DAGUiN,t the sulphur in organic compounds may be readily determined by heating with pure solution of potassa, adding 2 volumes of water and conducting chlorine into the fluid. When the oxidation is effected, the solu- tion is acidified and freed from the excess of chlorine by applica- tion of heat, then filtered, and the filtrate precipitated by barium chloride. Mr. C. J. MEEZ, in my laboratory, has employed both this method and v. LIEBIG'S (#, 1) in the analysis of fine horn shavings. This process appears convenient and exact. \ Substances leaving an ash on incineration, and which may there- fore be presumed to contain sulphates, are boiled with hydrochloric acid ; the solution obtained is filtered, and the filtrate tested with barium chloride. If a precipitate of barium sulphate forms, the sulphur contained in it is deducted from the quantity found by one of the methods described above ; the difference gives the quan- tity of the sulphur which the analyzed substance contains in organic combination. [. In more readily decomposable compounds, e.g., in the sub- stitution products of acids, the halogen may also be determined by decomposing the substance by contact during several hours with water and sodium amalgam, acidifying the fluid with nitric acid, and precipitating with silver solution ( F. ANALYSIS OF ORGANIC COMPOUNDS CONTAINING INORGANIC BODIES. . 189. In the analysis of organic compounds containing inorganic bodies, it is, of course, necessary first to ascertain the quantity of the latter before proceeding to the determination of the carbon, &c., as otherwise the amount of the organic -body whose constitu- ents have furnished the carbonic acid, water, &c., not being known, it would be impossible to estimate the oxygen from the loss. If the substances in question are salts or similar compounds, their basic radicals are determined by the methods given in the Fourth Section ; but in cases where the inorganic bodies are of a nature to be regarded more or less as impurities (e.g., the ash in coal), they may usually be determined with sufficient accuracy by the combustion of a weighed portion of the substance, in an obliquely placed platinum crucible, or in a platinum dish. In the analysis of substances containing fusible salts, even long-continued ignition will often fail to effect complete combustion, as the carbon is protected by the fused salt from the action of the oxygen. In such cases, the best way to effect the purpose is to carbonize the substance, treat the mass with water, and incinerate the undissolved residue ; the aqueous solution is, of course, likewise evaporated to dryness, and the weight of the residue added to that of the ash. If organic compounds whose ash contains potassium, sodium, barium, strontium, or calcium are burnt with oxide of copper, part of the carbonic acid evolved remains as carbonate of these metals. As, in many cases, the amount of carbonic acid thus retained is not constant, and the results are, moreover, more accurate if the whole amount of the carbon is expelled and weighed as carbonic acid, the combustion is effected with lead chromate, with addition of -J- of potassium dichromate, according to the directions given in 177. * Jahresb. v. Kopp. u. Will. 1861, 832. 189 ] ORGANIC ANALYSIS. 665 Accurate experiments have shown that in this case not a trace of carbonic acid remains with the bases. If the substance is weighed in a porcelain or platinum boat, and the combustion is effected according to 178, the ash, carbon, and hydrogen may be determined in one portion. The amount of car- bonic acid contained in the ash is added to that found by the pro- cess of combustion ; if the carbonic acid in the ash cannot be cal- culated, as in the case of alkali carbonates, it may be determined by means of fused borax ( 139, II., c). In burning substances containing mercury, the arrival of any of the metal at the calcium chloride tube may be prevented by having a layer of copper-turnings in the anterior part of the combustion tube, and by not allowing the foremost portion to get too hot. II. SPECIAL PART. 1. ANALYSIS OF FKESH WATER (SPRING-WATER RIVER-WATER, &0.).* 190. THE analysis of the several kinds of fresh water is usually restricted to the quantitative estimation of the foDowing sub- stances : a. Basic metals : Sodium, calcium, magnesium. b. Acids: Sulphuric acid, nitric acid, silicic acid, carbonic acid, chlorine. c. Mechanically suspended Matters : Clay, &c. We confine ourselves, therefore, here to the estimation of these bodies. I. The Water is clear. 1. Determination of the Chlorine. This may be effected, either, a, in the gravimetric, or, b. in the volumetric way. a. Gravimetrically. Take 500 1000 grm. or c. c.f Acidify with nitric acid, and precipitate with silver nitrate. Filter when the precipitate has completely subsided ( 141, I., a). If the quantity of the chlorine is so inconsiderable that the solution of silver nitrate produces only a slight turbidity, evaporate a larger portion of the water to i> i> i> & c -> f its bulk, filter, wash the precipitate, and treat the filtrate as directed. b. Yolumetrically. Evaporate 1000 grm. or c. c. to a small bulk, and determine the chlorine in the residual fluid, without previous filtration, by solution of silver nitrate, with addition of potassium chromate ( 141, L, 8. ). ' . * Compare Qualitative Analysis, p. 320 et seq. See a paper recently read before the Chemical Society by Dr. Miller the Society's Journal (2), iii. 117 et seq.; also, Frankland, idem (2), iv. 239, and vi. 77; and Wanklyn, Chapman, and Smith, idem, vi. 152. f As the specific gravity of fresh water differs but little from that of pure water, the several quantities of water may safely be measured instead of weighed. The calculation is facilitated by taking a round number of c. c. 670 SPECIAL PART. [ 190. 2. Determination of the Sulphuric Acid. Take 1000 grm. or c. c. Acidify with hydrochloric acid and mix with barium chloride. Filter after the precipitate has completely subsided ( 132, I., 1). If the quantity of the sulphuric acid is very incon- siderable, evaporate the acidified water to , J, -J, &c., of the bulk, before adding the barium chloride. 3. Determination of Nitric Acid. If, on testing the residue on evaporation of a water for nitric acid, such a strong reaction is obtained that the presence of a determinable quantity of the acid may be inferred, evaporate according to the apparent quantity of nitric acid indicated by qualitative testing 500 to 1000 or 2000 c. c. of the water in a porcelain dish, wash the residue into a flask (it is immaterial whether any solid matter which- may have sepa- rated goes partially or not at all into the , flask), evaporate in the flask still further, if necessary, and in the small quantity of residual fluid determine the nitric acid according to 149, d, fi. 4. Determination of the /Silicic Acid, Calcium, and Mag- nesium. Evaporate 1000 grm. or c. c. to dryness after addition of some hydrochloric acid preferably in a platinum dish, treat the residue with hydrochloric acid and water, filter off the separated silicic acid, and treat the latter as directed 140, II., a. Deter- mine calcium and magnesium in the filtrate aS directed 154, 6, a (28). 5. Determination of the total Residue and of the Sodium. a. Evaporate 1000 grm. or c. c. of the water, with proper care, to dryness in a weighed platinum dish, first over a lamp, finally on the water-bath. Expose the residue, in the air-bath, to a temperature of about 180, until no further diminution of weight takes place. This gives the total amount of the salts. 1). Treat the residue with water, and add, cautiously, pure dilute sulphuric acid in moderate excess ; cover the vessel during this operation with a dish, to avoid loss from spirting ; then place on the water-bath, without removing the cover. After ten minutes, rinse the cover by means of a washing bottle, evaporate the con- tents of 'the dish to dryness, expel the free sulphuric acid, ignite the residue, in the last stage with addition of some ammonium car- bonate ( 97, 1), and weigh. The residue consists of sodium sul- phate, calcium sulphate, magnesium sulphate, and some separated 190.] ANALYSIS OF FKESH WATER. 671 silica. It must not redden moist litmus paper. The quantity of the sodium sulphate in the residue is now found by subtracting from the weight of the latter the known weight of the silica and the weight of the calcium and magnesium sulphates calculated from the quantities of these earths found in 4. 6. Direct Determination of the Sodium. The sodium may also be determined in the direct way, with comparative expedition, by the following method : Evaporate 1250 gnn. or c. c. of the water, in a dish, to about ^, and then add 2 3 c. c. of thin pure milk of lime, so as to impart a strongly alkaline reaction to the fluid ; heat for some time longer, then wash the contents of the dish into a quarter-litre flask. (It is not necessary to rinse every particle of the precipitate into the flask ; but the whole of the fluid must be transferred to it, and the particles of the precipitate adhering to the dish well washed, and the washings also added to the flask.) Allow the contents to cool,v dilute to the mark, shake, allow to deposit, filter through a dry filter, measure off 200 c. c. of the filtrate,- corresponding to 1000 grm. of the water, transfer to a quarter-litre flask, mix with ammonium car- bonate and some ammonium oxalate, add water up to the mark, shake, allow to deposit, filter through a dry filter, measure off 200 c. c., corresponding to 800 grm. of the water, add some ammonium chloride,* evaporate, ignite, and weigh the residual sodium chloride as directed 98, 2.f Or by the following method : Evaporate the filtrate from the barium sulphate obtained in 2 to dryness in a platinum dish (or if nitrates are present in porcelain) to remove free hydrochloric acid and separate silica. Digest the residue with a few c. c. water, and precipitate magnesium without previous filtration by addition of solution of barium hydroxide, avoiding a large excess. Enough has been added if a pellicle of barium carbonate forms upon the surface of the liquid on exposure a short time to the air. Filter and wash the usually slight precipi- tate. Heat the filtrate, and add ammonium carbonate to precipitate * To convert the still remaining sodium sulphate, on ignition, into sodium chloride. f This process, which entirely dispenses with washing, presents one source of error viz., the space occupied by the precipitates is not taken into account. The error resulting from this is, however, so trifling, that it may safely be disregarded, as the excess of weiht amounts to - at the most. 672 SPECIAL PART. [ 190. the barium introduced and the calcium originally present, filter from the precipitated carbonates, and evaporate the filtrate to dry- ness, and remove by- heating the ammonium chloride completely. Dissolve the sodium chloride in the residue with 4 or 5 c. c. water, warm, and add a few drops of ammonium carbonate and ammonia to separate possibly remaining traces of barium and calcium, filter again into a weighed platinum dish, evaporate to dryness, heat nearly to fusion, and weigh the sodium chloride. The sodium chloride obtained by either process will contain the potassium (as chloride) if any is present in the water. If enough alkali chloride is obtained it may, after weighing, be examined for potassium according to 152, 1, a. 7. Calculate the numbers found in 1 6 to 1000 parts of water, and determine from the data obtained the amount of carbonic acid in combination, as follows : Add together the quantities of SO 3 corresponding to the basic oxides found, and subtract from the sum, first, the amount of sulphuric acid SO 3 precipitated from the water by barium chloride (2), secondly, the amount equivalent to the nitric acid found, aird thirdly, the amount equivalent to the chlorine found ; the remain- der is equivalent to the carbonic acid combined with the bases in the form of normal carbonates. 80 parts of SO 3 remaining after sub- tracting the quantities just stated, correspond accordingly to 44 parts of CO 2 . If, by way of control, you wish to determine the combined car- bonic acid in the direct way, evaporate 1000 grm. or c. c. of the water, in a flask, to a small . bulk ; add tincture of cochineal, then standard nitric acid, and proceed as directed p. 698. 8. Control. If the quantities of the ^"a 2 O, CaO, MgO, SO 3 , N a O 6 , SiO 2 , CO, and Cl are added together, and an amount of oxygen equivalent to the chlorine (since this latter is combined with metal and not with oxide) is subtracted from the sum, the remainder must nearly correspond to the total amount of the salts found in 5, a. Perfect correspondence cannot be expected, since, 1, upon the evaporation of the water magnesium chloride is partially decomposed, and con- verted into a basic salt; 2, the -silicic acid expels some carbonic acid ; and 3, it being difficult to free magnesium carbonate from water without incurring loss of carbonic acid, the residue remain- ing upon the evaporation of the water contains the magnesium 190.] ANALYSIS OF FRESH WATEE. 673 carbonate as a basic salt, whereas, in our calculation, we have assumed the quantity of carbonic acid corresponding to the normal salt. 9. Determination of the free Carbonic Acid. ' In the case of well-water this may be conveniently executed by the process described 139, /3 (p. 405). We here obtain the carbonic acid which is contained in the water over and above the quantity corresponding to the normal carbonates, or in other words, the carbonic acid which is free and which is combined with the carbonates to bicarbonates. 10. Determination of the Organic Matter. Many fresh waters contain so much organic matter as to be quite yellow, others contain traces, and many again may be said to be free from such substances. The exact estimation of organic matter is by no means an easy task, and the method usually adopted viz., ignition of the residue of the water dried at 180, treatment with ammonium carbonate, gentle ignition again, and calculation of the organic matter from the loss of weight yields merely an approximate result, since we can never be sure as to the condition of the magnesium carbonate in the residue dried at 180 and in the same after ignition, and since the silicic acid expels some carbonic acid, which is not taken up again on treatment with ammonium carbonate, &c. [This approximation, however, will generally suffice, if the purpose of the analysis is to enable one to judge of the quality of the water with reference to its use in steam-boilers and for most manufacturing processes. But if it is desired to learn by analysis whether the water is fit or unfit for drinking, the case is quite different, for its quality as a potable water doubt- less depends greatly on the amount, and still more on the kind, of organic matter present. Detailed descriptions of methods used in the examination of the organic matter contained in water are to be found in Water Analysis," by J. A. WAKKLYN and E. T. CHAP- MAX, third edition, London, Truebner & Co., 1874: ; Anleitung znr Untersuchung von Wasser, von Kubel und Tiemann, 2 Aufl. ; also in several articles on the subject by WANKLYN, CHAPMAN, and SMITH, in Journal of the Chem. Soc.] II. The ivater is not clear. Fill a large flask of known capacity with the water, close with 674 SPECIAL PAKT. [ 190. a glass stopper, and allow the flask to stand in the cold until the suspended matter is deposited; draw off the clear water with a siphon as far as practicable, filter the bottoms, dry or ignite the contents of the filter, and weigh. Treat the clear water as directed in I. Eespecting the calculation of the analysis, I remark simply that the results are usually* arranged upon the following principles : The chlorine is combined with sodium ; if there is an excess, this is combined with calcium. If, on the other hand, there remains an excess of sodium, this is combined with sulphuric acid. The sulphuric acid, or the remainder of the sulphuric acid, as the case may be, is combined with calcium. The nitric acid is, as a rule, to be combined with calcium. The silicic acid is put down in the free state, the remainder of the calcium and the magnesium as carbonates, either normal or acid, according to circumstances. It must always be borne in mind that the results of the qualita- tive analysis may render another arrangement of the acids and bases necessary. For instance, if the evaporated water reacts strongly alkaline, sodium carbonate is present, generally in com- pany with sodium sulphate and sodium chloride, occasionally also with sodium nitrate. The calcium and magnesium are then to be entirely combined with carbonic acid. In the report, the quantities are represented in parts per 1000 (or 1000,000), and also in grains per gallon. For technical purposes, it is sometimes sufficient to estimate the hardness of the water (the relative amount of calcium and magne- sium in it) by means of a standard solution of soap. A detailed description of this method, which was first employed by CLAEK, may be found in BOLLEY & PAUL'S Handbook of Technical Analysis. See also STJTTON'S Yolumetric Analysis. * A certain latitude is here allowed to the analyst's discretion 192.] ACIDIMETRY. 675 2. ACIDIMETKY. A. ESTIMATION BY SPECIFIC GRAVITY. 191. Tables, based upon the results of exact experiments, have been drawn up, expressing in numbers the relation between the specific gravity of the aqueous solution of an acid, and the amount of real acid contained in it. Therefore, to know the amount of real acid contained in an aqueous solution of an acid, it suffices, in many cases, simply to determine its specific gravity. Of course the acids must, in that case, be free, or at least nearly free from admixtures of other substances dissolved in them. Now, as most common acids are volatile (sulphuric acid, hydrochloric acid, nitric acid, acetic acid), any non-volatile admixture may be readily detected by evaporating a sample of the acid in a small platinum or porcelain dish. The determination of the specific gravity is effected either by comparing the weight of equal volumes of water and acid, or by means of a good hydrometer. The estimations must, of course, be made at the temperature to which the Tables refer. The following Tables on pages 676 679 give the relations between the specific gravity and the strength for sulphuric acid, hydrochloric acid, nitric acid, and acetic acid. In all cases in which the determination of the specific gravity fails to attain the end in view, or which demand particular accuracy, the volumetric method described under B, is employed. B. ESTIMATION BY SATURATION WITH AN ALKALINE FLUID OF KNOWN STRENGTH.* 192. 1. This method requires : A dilute acid of known strength. Sulphuric or hydrochloric acid may be used. Nitric and oxalic acids are less frequently employed. * According to NICHOLSON and PRICE (Chem. Gaz., 1856, p. 30) the common method of acidimetry is not suited for determining free acetic acid, on account of the alkaline reaction of neutral sodium acetate; however, OTTO (Annal. d. Chem. u. Pharm. 102, 69) has clearly demonstrated that the error arising from this is so inconsiderable that it may safely be disregarded. 676 SPECIAL PART. [ 192. TABLE I. Showing the percentages of Acid (H 2 8O 4 ) and Anhydride (SO 3 ) corresponding to vari&us specific gravities of aqueous Sulphuric Acid by BINEAU ; calculated for 15, by OTTO. Specific gravity. Percentage Percentage ofH 2 SO 4 . ofSO 3 . Specific gravity. Percentage of H 2 SO 4 . Percentage of S0 3 . 1 8426 100 81-63 1-398 50 40-81 1-842 99 80-81 1-3886 49 40-00 1-8406 98 80-00 1-379 48 39-18 1-840 97 79-18 1-370 47 38-36 1-8384 96 78-36 1-361 46 37-55 1-8376 95 77-55 1-351 45 36-73' 1-8356 94 76-73 1-342 44 35-82 1-834 93 75-91 1-333 43 35-10 1-831 92 75-10 1-324 42 34-28 1-827 91 74-28 1-315 41 33-47 1-822 90 73-47 1-306 40 32-65 1-816 89 72-65 1-2976 39 31-83 1-809 88 71-83 1-289 38 31-02 1-802 87 71-02 1-281 37 30-20 1-794 86 70-10 1-272 36 29 38 1-786 85 69-38 1-264 35 28-57 1-777 84 68-57 1-256 34 . 27-75 1-767 83 67-75 1-2476 33 26-94 1-756 82 66-94 1-239 32 26-12 1-745 81 66-12 1-231 31 25-30 1-734 80 65-30 1-223 30 34-49 1-722 79 64-48 1-215 29 23-67 1-710 78 63-67 1-2066 28 22-85 1-698 77 62-85 1-198 27 22-03 1-686 76 62-04 1-190 26 21-22 1-675 75 61-22 1-182 25 20 40 1-663 74 60-40 1-174 24 19-58 1-651 73 59'59 1-167 23 18-77 1-639 72 58-77 1-159 22 17-95 1-627 71 57-95 1-1516 21 17-14 1-615 70 57-14 1-144 20 16-32 1-604 69 56-32 1-136 19 15-51 1-592 68 55-59 1-129 18 14-69 1-580 67 54-69 1-121 17 13-87 1-568 66 53-87 1-1136 16 13-06 1-557 65 53-05 1-106 15 12-24 1-545 64 52-24 1-098 14 11-42 1-534 63 51-42 1-091 13 10-61 1-523 62 50-61 1-083 12 9-79 1-512 61 49-79 1-0756 11 8-98 1-501 60 48-98 1-068 10 8-16 1-490 59 48-16 1-061 9 7-34 1-480 58 47-34 1-0536 8 6-53 1-469 57 46-53 1-0464 7 5-71 1-4586 56 45-71 1-039 6 4-89 1-448 55 44-89 1-032 5 4-08 1-438 54 44-07 1-0256 4 3-26 1-428 53 43-26 1-019 3 2-445 1-418 52 42-45 1-013 2 1-63 1-408 51 41-63 1-0064 1 0-816 192.] ACH)IMETBT. 677 TABLE II. Sliowing the percentages of Anhydrous Acid (HC1 ) corresponding to various specific gravities of Uqueous solutions of Hydrochloric Acid, by UBE. Tempera- ture 15. Specific gravity. Percentage of hydrochloric acid gas (HC1). Specific gravity. Percentage of hydrochloric acid gas (HC1). 1-2000 40-777 1-1000 20-388 1-1982 40-369 1-0980 19-980 1-1964 39-961 1-0960 19-572 1-1946 39-554 1-0939 19-165 1-1928 39-146 1-0919 18-757 1-1910 38-738 1-0899 18-349 1-1893 38-330 1-0879 17-941 1-1875 37-923 1-0859 17-534 1-1857 37-516 1-0838 17-126 1-1846 37-108 1-0818 16-718 1-1822 36-700 1-0798 16-310 1-1802 36-292 1-0778 15-902 1-1782 35-884 1-0758 15-494 1-1762 35-476 1-0738 15-087 1-1741 35-068 1-0718 14-679 1-1721 34-660 1-0697 14-271 1-1701 34-252 1-0677 13-863 1-1681 33-845 1-0657 13-456 1-1661 33-437 1-0637 13-049 1-1641 33-029 1-0617 12-641 1-1620 32-621 1-0597 12-233 1-1599 32-213 1-0577 11-825 1-1578 31-805 1-0557 11-418 1-1557 31-398 0537 11-010 1-1537 30-990 0517 10-602 1-1515 30-582 0497 10-194 1-1494 30-174 0477 9-786 1-1473 29-767 0457 9 379 1-1452 29-359 0437 8-971 1-1431 28-951 1-0417 8-563 1-1410 28-544 1-0397 8-155 1-1389 28-136 1-0377 7-747 1-1369 27-728 1-0357 7-340 V1349 27-321 1-0337 6-932 1-1328 26-913 1-0318 6-524 1-1308 26 505 1-0298 6-116 1-1287 26-098 1-0279 5-709 1-1267 25-690 1-0259 5-301 1-1247 25-282 1-0239 4-893 1-1226 24-874 1-0220 4-486 1-1206 24-466 1-0200 4-078 1-1185 24-058 1-0180 3-670 1-1164 23-650 1-0160 3-262 1-1143 23-242 1-0140 2-854 1-1123 22-834 1-0120 2-447 1-1102 22-426 1-0100 2-039 1-1082 22-019 1-0080 1-631 1-1061 21-611 1-0060 1-124 1-1041 21-203 1-0040 0-816 1 1020 20-796 1-0020 0-408 678 SPECIAL PAKT. [ 192. TABLE III. Showing the percentages of Nitric Anhydride (N 2 O 5 ) corresponding to various specific gvavities of aqueous Nitric Acid, by URE. Temperature 15. Specific gravity. Percentage of N a O 5 . Specific gravity. Percentage of N 8 O 5 . Specific gravity. Percentage of N a 6 . Specific gravity. Percentage of N a O 6 . 1-500 79-7 1-419 59-8 1-295 39-8 1-140 19-9 1-498 78-9 1-415 59-0 1-289 39-0 1-134 19-1 1-496 78-1 1-411 58-2 283 38-3 1-129 18-3 1-494 77-3 1-406 57-4 276 37-5 1-123 17-5 1-491 76-5 1-402 56-6 270 36-7 1-117 16-7 1-488 75-7 1-398 55-8 264 35-9 1-111 15-9 1-485 74-9 394 55-0 258 35-1 1-105 15-1 1-482 74-1 . -388 54-2 252 34-3 1-099 14-3 1-479 73 3 383 53-4 1-246 33-5 1-093 13-5 1-476 72-5 378 52-6 1-240 32-7 1-088 12-7 1-473 71-7 373 51-8 1-234 31-9 1-082 11-9 1-470 70-9 368 51-1 1-228 31-1 1-076 11-2 1-467 70-1 1-363 50 2 1-221 30-3 1-071 10-4 1-464 69-3 1-358 49-4 1 215 29-5 1-065 9-6 1-460 68-5 1-353 48'6 1 208 28'7 1-059 8-8 1-457 67-7 1-348 47-9 1-202 27'9 1-054 8-0 1-453 66-9 343 47-0 1-196 27-1 1-048 7-2 1-450 66-1 338 46-2 1-189 26-3 1-043 6-4 1-446 65-3 332 45-4 1-183 25'5 1-037 5-6 1-442 64-5 327 44-6 1-177 24-7 1-032 4-8 1-439 63-8 322 43-8 1-171 23-9 1-027 4-0 1-435 63-0 316 43-0 1-165 23-1 1-021 3-2 1-431 62-2 1-311 42-2 1-159 22-3 1-016 2-4 1-427 61-4 1-306 41-4 1 153 21-5 1-011 1-6 1-423 60-6 1-300 40-4 1-146 20-7 1-005 0-8 2. An alkaline fluid of known strength. Potassa or ammonia may be employed. a. PREPARATION OF THE SOLUTIONS. The solutions should be of suitable strength. As, the first step in the preparation of a dilute sulphuric acid, of convenient strength for ordinary use, dilute 20 cubic centimetres of oil of vit- riol with water to the volume of 2 litres. The standard alkali is made from commercial caustic potash ; this is dissolved in water and diluted until a given volume, e.g., 5. c. c., neutralizes 4 to 5 c. c. of the standard acid, as is determined by a few rough trials. The alkali solution thus obtained is heated to boiling in a flask, and a little freshly-slaked lime is added to decompose any potas- sium carbonate. The boiling is continued a few minutes and. 192.] ACIDIMETRY. 679 TABLE IV. Sliowing the percentages of Acetic Acid (HC 3 H 3 O ? ) corresponding to various specific gravities of aqueous solutions of Acetic Acid, by MOHK. Specific .gravity. Sa-j 3 c-HK Specific gravity. 111 | Specific gravity. fe c.2W Specific gravity. m 10 Specific gravity. 2s-* |i. If* li gS ll fig !& 1-0635 100 ' 1-0735 80 ' 1-067 60 1-051 40 1-027 20 1-0555 99 1-0735 79 1-066 59 1-050 39 1-026 19 1-0670 98 1-0732 78 1-066 58 ; 1-049 38 1-025 18 1-0680 97 1-0732 77 1-065 57 1-048 37 1-024 17 1-0690 96 1-0730 76 1-064 56 1-047 36 1-023 16 1-0700 95 1-0720 75 064 55 1-046 35 1-022 15 1-0706 94 ! 1-0720 74 063 54 1-045 34 1-020 14 1-0708 93 1-0720 73 063 53 1-044 33 1-018 13 1-0716 92 i 1-0710 72 062 52 1-042 32 1-017 12 1-0721 91 1-0710 71 061 51 1-041 31 1-016 11 1-0730 90 1-0700 70 060 50 1-040 30 1-015 10 1-0730 89 1-0700 69 059 49 1-039 99 1-013 9 1-0730 88 1-0700 68 058 48 088 28 1-012 8 1-0730 87 1-0690 67 056 47 036 27 1-010 7 1-0730 86 1-0690 66 1-055 46 035 26 1-008 6 1-0730 85 1-0680 65 1-055 45 034 25 1-007 5 1-0730 84 1-0680 64 1-054 44 033 24 1-005 4 1-0730 83 1-0680 63 1-053 43 032 23 1-004 3 1-0730 82 1-0670 62 1-052 42 031 22 1-002 2 1-0732 81 1-0670 61 1-051 41 1-029 21 1-001 1 1 finally, the lye is poured upon a filter, and the filtrate is collected in the bottle from which it is to be used. Care should be taken to bring upon the filter some of the excess of lime that is suspended in the liquid, so that the latter may acquire no carbonic acid from the air. This clear liquid thus obtained is a potash-lye containing lime in solution. If exposed to the air, the carbonic acid that is absorbed separates as calcium carbonate, leaving the liquid per- fectly caustic. It now remains to determine with the greatest accuracy, 1st, the volume of alkali which neutralizes a cubic centimetre of the acid, and, 2d, the amount of SO 3 contained in a cubic centimetre of the latter. As a means of recognizing the point of neutralization, tincture of cochineal possesses great advantages over solution of litmus. The knowledge of this fact is due to LUCKOW, who has detailed its application in Joum.fiir prakt. Chem., Ixxxiv. p. 424. Tincture 680 SPECIAL PART. [ 192. of cochineal is prepared by digesting and frequently agitating three grammes of pulverized cochineal in a mixture of 50 cubic centi- metres of strong alcohol with 200 c. c. of distilled water, at ordinary temperatures, for a day or two. The solution is decanted, or fil- tered through Swedish paper. The tincture thus prepared has a deep ruby-red color. On gradually diluting with pure water (free from ammonia), the color becomes orange and finally yellowish-orange. Alkalies and alkali- earths as well as their carbonates change the color to a carmine or violet-carmine. Solutions of strong acid and acid salts make it orange or yellowish-orange. To determine the volumetric relation of the alkali and acid, a given volume of the latter, e.g., 20 c. c., is measured off into a wide- mouthed flask, 10 drops of cochineal-tincture, and about 150 c.c. of water are added ; the alkali is now allowed to flow in from a burette, until the yellowish liquid in the flask, suddenly, and by a single drop, acquires a violet-carmine tinge. In nicer determinations, it is important to bring the liquid each time to a given volume, by adding water after the neutralization is nearly finished. For this purpose, two or more flasks of equal capacity are selected, and on the outside of each a strip of paper is gummed to indicate the level of the proper amount of liquid, e.g., 200 c. c. The same amount of coloring matter being thus always diffused in the same volume of the same water, the errors of vary- ing dilution and varying amount of ammonia (which is rarely absent from distilled water) are avoided. The contents of one flask, in which the neutralization has been satisfactorily effected, may be kept as a standard of color for the succeeding trials, as the tint remains constant for hours, being unaffected by the absorption of carbonic acid. The greatest convenience and accuracy of mea- surement' are obtained by using burettes provided with EKDMANN'S swimmer (see p. 40). When three or four accordant results have been obtained, the average is taken as expressing the relative strength of the acid and alkali. To ascertain the absolute standard, weigh off in a small plati- num crucible about 0'8 grm. of pure sodium carbonate, ignite to dull redness, cool and weigh accurately : bring the crucible with its contents into one of the wide-mouthed flasks and let flow from the burette a slight excess, e.g. 50 c. c., of standard acid. The solu- 192.] ACIDIMETRY. 681 tion of sodium carbonate is facilitated by wanning, and, finally, the contents of the flask are gently boiled for several minutes to expel carbonic acid. The solution is now allowed to become perfectly cold, then add ten drops of cochineal and lastly the standard alkali to neutralization, diluting to the proper volume. To illustrate the accuracy of the process and the calculations employed, the following actual data may be useful. The acid solu- tion was made by diluting 50 c. c. of oil of vitriol to the volume of ten litres and had half the strength above recommended. The alkali was from a stock on hand and more dilute than necessary. .Relation of acid to alkali. Exp. L, 20 c. c. H a SO 4 = 32-8 c. c. KOH, or 1 Exp. II., 20 c. c. H a SO 4 = 32 8 c. c. KOH, or 1 Exp. III., 40 c. c. H 3 SO 4 = 65-7 c. c. KOH, or 1 1-64 1-6425. We have accordingly : 1 c. c. H 3 SO 4 = 1-64 c. c. KOH and 1 c. c. KOH = 0-60976 c. c. H a SO, Absolute strength of acid and alkali. Exp. I. 0*4:177 grin, of sodium carbonate were treated with 44*2 c. c, of H a SO 4 solution. To neutralize -the excess of the acid were required 3'8 c. c. KOH, which correspond to 2*32 c. c. H a SO 4 (3-8 X 0-60976). Deducting this from the total amount of acid (44.2 2*32) we have 41 '88 c. c. of acid, neutralized by the sodium carbonate taken. 41-88 c. c. solution of H a SO 4 = 0-4177 grm. Ka,CO 3 . Exp. II. 0.4126 grm. Na.CO, treated with 44 c. c. H S SO 4 required 4*28 c. c. KOH. 4-28 X 0-60976 = 2'61 c. c. H 3 SO 4 . 44 - 2-61 = 41-39 c. c. H a SO 4 . 41-39 c. c. solution of H 2 SO 4 = 0-4126 grm. Na 2 CO 3 . Now, from the data obtained by each of these experiments, the absolute strength of the sulphuric acid solution may be calculated ; for when sodium carbonate and sulphuric acid exactly neutralize each other, one molecule or 106*08 pts. ISTa 2 CO 3 reacts with 1 molecule or 98 pts. H a SO 4 . mol. weight 98 mol. weight 106-08 H 2 S0 4 -j Na a C0 3 = NaJS0 4 + CO a + H a O. 682 SPECIAL PART. [ 192. Consequently that volume of a sulphuric acid solution which is found to exactly neutralize 1-0608 grm. Na a CO 3 must contain *98 grm. HJ30.. The volume of the sulphuric acid solution in the present case which would neutralize 1*0608 grm. Na a CO 3 is found by calcula- tion from the data furnished by the experiments to be : grms. Na 3 CQ 3 c. c. H 2 SO 4 solution L, -4177 : 1-0608 :: 41-88 : 106-35 II., -4126 : 1-0608 :: 41-39 : 106-41 According to Exp. L, 106-35 c. c.; according to Exp. II., 106-41 c. c. mean, 106-38 c. c. This volume therefore contains *98 grm. H a SO 4 . By dividing *98 grm. by 106-38 the weight of H a SO 4 in 1 c. c. would of course be found. But the already found volume of the sulphuric acid which con- tains a weight of H 2 SO 4 corresponding to its molecular weight is a more convenient basis for calculating the weight of any alkali neu- tralized by 1 c. c. Suppose it is desired, for instance, to find the weight of NH 4 OH, XH 3 , or N which corresponds to 1 c. c. of the .acid solution. One molecule of sulphuric acid neutralizes 2 mol. mol. weight 98 mol. weight 35 X 2 = 70 HS0 4 2JSTHOH = (NE^JSO, + (H,O) a . Hence 106-38 c. c. = -98 grm. H a SO 4 neutralize -70 grm. NH 4 OH, .and further, observing that 35 parts (1 mol.) of Mi 4 OH contain 14 pts. 1ST or 17 NH 3 I I i; O 16 35 and 70 pts. (2 mol.) twice these quantities 106 38 c. c. acid solution correspond to 34 grm. " " " " .28 " Finally find the weight of the substance which corresponds to 192.] ACIDIMETKY. 683 1 c. c. of the standard solution. For nitrogen, e.g., this is '28 grin. -h 106-38 = 0-002632 grm. We may then write on the label of the acid bottle the follow- ing data for calculation : 1 c. c. KOH = 0-60976 c. c. H a SO 4 , 1 c. c. H,SO 4 = 1-64 c. c. KOH, 1 c. c. H a SO 4 = 0-002632 grm. K In a like manner, we may calculate the weight of any base, or any constituent part of a base corresponding to 1 c. c. of the stan- dard acid, being careful to observe whether one or two molecules of the base are neutralized by one mol. H a SO 4 . To ascertain the absolute strength of the alkali solution. Is'o further experimental work is required for this purpose. For since 98 grm. H 2 SO 4 neutralize 1*1226 grm. KOH, as clearly seen from the formulae with appended molecular weights expressing the reaction, mol. weight 98 mol. weight 5613 X 2=112 "26 ~H0 4 V 2KOH ~"= K a SO 4 + (H a O) a , it follows that a volume of potash solution which exactly neutral- izes 106-38 c. c. sulphuric acid solution (i.e., the volume already found to contain -98 grm. H a SO 4 ) must contain 1-1226 grm. KOH. This volume of potash solution may be calculated from the already determined volumetric relation of the acid and alkali solutions, viz.: 1 c. c. H 2 SO 4 sol. = 1-64 c. c. KOH sol. 106-38 c. c. X 1-64 = 174-46 c. c. Accordingly 174'46 c. c. potash solution contain 1-1226 grm. KOH, or 112-26 centigrammes a number equal to twice the number which expresses the molecular weight of KOH. The weight of any acid neutralized by 1 c. c. of this alkali solution may now be readily calculated, bearing in mind that 2 mol. KOH neutralize 2 mol. of any monobasic and 1 mol. of any dibasic acid. For hydrochloric acid, e.g. : mol. weight 56-13 X 2 = 112-26 mol. weight 36'46 X 2 = 72.92 (KOH), eutrali (HCl) a 684 SPECIAL PART. [ 192. 176-46 c.c. sol. = 1-1226 grm. KOH neutralize '7292 grm. HC1. I c.c. alkali solution = -00418 grm. HC1. b. THE ACTUAL ANALYSIS. It is only necessary to weigh or measure off the acid to be examined, dilute to about 150 c. c. and ascertain how much of the standard alkali is required for its neu- tralization, proceeding just as detailed for ascertaining the volu- metric relation of the acid and alkali solutions. It is best to use for determination a quantity which will require 15 to 30 c. c., but not over a burette full of the standard alkali. It is often convenient in case of strong acids to weigh off about five times the amount required for a single trial, dilute to exactly 500 c. c. and make two or more determinations, using for each 100 c. c. tx. If the color of a fluid conceals the change of the dissolved cochineal, or if salts of iron be present, we use red litmus or turmeric paper to hit the point of neutralization, i.e., we add alkali till a strip of test paper dipped in just indicates a weak alkaline reaction. In this case more alkali will be employed than when cochineal can be used in solution, and in exact determinations it may be worth while to rectify the error by a correction. This may be done by taking a like quantity of water and adding alkali solu- tion, till the fluid just gives a reaction on the test paper in ques- tion, as strong as was obtained at the close of the first experiment. The quantity of alkali used is, of course, to be deducted from the quantity employed in the first experiment. ft. Determination of Acids by means of normal sodium car- bonate solution. See readily be proved by making two separate experiments, one with the decanted clear fluid, and the other with the residuary turbid mixture. Thus, for instance, in an experiment made in my own laboratory, the decanted clear fluid gave 22*6 of chlorine, the residu- ary mixture 25'0, the uniformly mixed turbid solution 24'5. 1 c. c. of the solution of chloride of lime so prepared corre- sponds to O'Ol grm. chloride of lime. A. PENOT'S Method.* 200. This method is based upon the conversion of arsenious acid into arsenic acid, or more strictly, an arsenite into an arsenate, since the conversion is effected in an alkaline solution. Potassium iodide- starch paper is employed to ascertain the exact point when the reac- tion is completed. * Bulletin de la Societe Industrielle de Mulhouse, 1852, No. 118. Dingler's Polytech. Journal, 127, 134. 700 SPECIAL PAKT. [ 200. a. Preparation of the Potassium Iodide-Starch Paper. The following method is preferable to the original one given by PENOT : Stir 3 grm. of potato starch in 250 c. c. of cold water, boil with stirring, add a solution of 1 grm. potassium iodide and 1 grin, crystallized sodium carbonate, and dilute to 500 c. c. Moisten strips of fine white unsized paper with this fluid, and dry. ' Keep in a closed bottle. 1). Preparation of the solution of Arsenious Acid. Dissolve 4-436 grrn. of pure arsenious oxide (As 2 O 3 ) and 13 grm, pure crystallized sodium carbonate in 600 700 c. c. water, with the aid of heat, let the solution cool, and then dilute to 1 liter. Each c. c. of this solution contains an amount of sodium arsenite equivalent to 0-004436 grm. arsenious oxide (As 3 O 3 ), which corresponds to 1 c. c. chlorine gas of and 760 mm. atmospheric pressure.* As sodium arsenite in alkaline solution is liable, when exposed to access of air, to be gradually converted into sodium arsenate, PENOT' s solution should be kept in small bottles with glass stoppers, filled to the top, and a fresh bottle used for every new series of experiments. According to Fr. MoHKf the solution keeps unchanged, if the arsenious oxide and the sodium carbonate are both absolutely free from oxidizable matters (arsenious sulphide,, sodium sulphide, and sodium sulphite). * Penot gives the quantity of arsenious oxide as 4'44; but I have corrected this number to 4'436, in accordance with the now received atomic weights of the substances and specific gravity of chlorine gas after the following propor- tion : 141-84 (4 at. 01): 198 (1. mol. As 2 O 8 ) :: 317763 (weight of 1 litre of chlorine gas):?/ x = 4 '436, i.e., the quantity of arsenious oxide which 1 litre of chlorine gas converts into arsenic acid. This solution is arranged to suit the foreign method of designating the strength of chloride of lime viz., in chlorimetrical degrees (each degree repre- sents 1 litre chlorine gas at and 760 mm. pressure in a kilogramme of the sub- stance). This method was proposed by Gay-Lussac. The degrees may readily be converted into per cents, and vice 'versa, thus: A sample of chloride of lime of 90 contains 90 X 317763 = 285'986 grm. chlorine in 1000 grm. or 28*59 in 100; and a sample containing 34'2 per cent, chlorine is of 107 '6, for 100 grm. of the substance contain 34'2 grm. chlorine; . . 1000 grm. of the substance contain 342 grm. chlorine, but 342 grm. chlorine = -S-TTT^ litres = 107 ' 6 litres; . . 1000 grm. of the substance contain 107'6 litres chlorine. f His Lehrbuch der Titrirmethode, 2 Aufl., S. 290. 201.] CHLORIMETRY. 701 c. The Process. Measure off, with a pipette, 50 c. c. of the solution of chloride of lime prepared according to the directions of 199, transfer to a beaker, and from a 50 c. c. burette add slowly, and at last drop by drop, the solution of arsenious acid, with constant stirring, until a drop of the mixture produces no longer a blue-colored spot on the iodized paper ; it is very easy to hit the point exactly, as the grad- ually increasing faintness of the blue spots made on the paper by the fluid dropped on it indicates the approaching termination of the reaction, and warns the operator to confine the further addition of the solution of arsenious acid to a single drop at a time. The num- ber of c. c. used indicates directly the number .of chlorirnetrical degrees (see note), as the following calculation shows : Suppose you have used 40 c. c. of solution of arsenious acid, then the quantity of chloride of lime used in the experiment contains 40 c. c. of chlorine gas. Now, the 50 c. c. of solution employed correspond to 0*5 grm. of chloride of lime ; therfore 0'5 grm. of chloride of lime contain 40 c. c. chlorine gas, therefore 1000 grm. contain 80000 c. c. = 80 litres^ This method gives very constant and accurate results, and appears to be particularly well suited for use in manufacturing establishments where there is no objection, on the score of danger, to the employment of arsenious acid. (Expt. No. 99.) B. OTTO'S Method. 201. The principle of this method is as follows : Two molecules of ferrous sulphate when brought in contact with chlorine in presence of water and free sulphuric acid, give 1 mol. ferric sulphate and 2 mol. HC1, the process consuming 2 at. chlorine. 2FeS0 4 + H 2 S0 4 + 2C1 = Fe(SO 4 ) 3 + 2HC1. 1 mol. crystallized ferrous sulphate : (FeS0 4 -7H 3 0) = 278 correspond to 35'46 of chlorine, or, in other terms, 0'7839 grm. crystallized ferrous sulphate correspond to 0*1 grm. chlorine. The ferrous sulphate required for these experiments is best pre- pared as follows : 702 SPECIAL PART. [ 201. Take iron nails, free from rust, and dissolve in dilute sulphuric acid, applying heat in the last stage of the operation : filter the solu- tion, still hot, into about twice its volume of common alcohol. The precipitate consists of 7H a O. Collect upon a filter, wash with common alcohol, spread upon a sheet of blotting paper, and dry in the air. When the mass smells no longer of alcohol, transfer to a bottle and keep this well corked. Instead of ferrous sulphate, ammonium ferrous sulphate (p. 118) may be used. 0*1 grin, of chlorine reacts with 1-1055 grm. of this double sulphate. The Process. Dissolve 3-1356 grm. (4 X '7839 grm.) of the precipitated fer- rous sulphate, or 4-422 grm. (4 X 1'1055 grm.) of ammonium fer- rous sulphate, with addition of a few drops of dilute sulphuric acid, in water, to 200 c. c. ; take out, with a pipette, 50 c. c., corre- sponding to 0*7839 grm. ferrous sulphate, or 1-1055 grm. ammonium ferrous sulphate, dilute with 150 200 c. c. water, add a sufficiency of pure hydrochloric acid, and run in from a 50 c. c. burette the freshly shaken solution of chloride of lime, prepared according to 199, until the ferrous sulphate is completely converted into ferric sulphate. To know the exact point when the reaction is completed, place a number of drops of a solution of potassium ferricyanide on a plate, and when the operation is drawing to an end apply some of the mixture with a stirring-rod to one of the drops on the plate, and observe whether it produces a blue precipitate ; repeat the experiment after every fresh addition of two drops of the solution of chloride of lime. When the mixture no longer produces a blue precipitate in the solution of potassium ferricyanide on the plate, read off the number of volumes used of the solution of chloride of lime. The amount of solution of chloride of lime used contained O'l grm. of chlorine. Suppose 40 c. c. have been used : as every c. c. corresponds to 0*10 grm. of chloride of lime, the percentage by weight of available chlorine in the chloride of lime is found by the following proportion : 0-40 : 0-10 :: 100 :; # = 25; or, by dividing 1000 by the number of c. c. used of the solution of chloride of lime. 201.] CHLORIMETRY. 703 This method also gives very satisfactory results, provided always that the ferrous salt is perfectly dry and free from ferric salt. Modification of the preceding Method. Instead of the solution of ferrous sulphate, a solution of ferrous chloride, prepared by dissolving pianoforte wire in hydrochloric acid (according to p. 268), may be used with the best results. If 0-6316 of pure metallic iron, i. e., 0'6335 of fine pianoforte wire (which may be assumed to contain 99'7 per cent, of iron), are dis- solved to 200 c. c., the solution so prepared contains exactly the same amount of iron as the solution of ferrous sulphate above men- tioned that is to say, 50 c. c. of it correspond to 0*1 gnu. chlorine. But as it is inconvenient to weigh off a definite quantity of iron wire, the following course may be pursued in preference : Weigh off accurately about 0'15 grin., dissolve, dilute the solution to about 200 c. c., convert the ferrous into ferric chloride with the solution of chloride of lime, prepared according to the directions of 199, and calculate the chlorine by the proportion 56 : 35*46 :: the quantity of iron used : x\ the x found corresponds to the chlorine contained in the amount used of the solution of chloride of lime. This calculation may be dispensed with by the application of the following formula, in which the carbon in the pianoforte wire is taken into account : Multiply the weight of the pianoforte wire by 6313, and divide the product by the number of c. c used of the solution of chloride of lime; the result expresses the percentage of chlorine by weight. This method gives very good results. I have described it here principally because it dispenses altogether with the use of standard fluids. It is therefore particularly well adapted for occasional examinations of samples of chloride of lime, and also by way of control. (See Expt. No. 99.) C. BTJNSEN'S Method. Pour 10 c. c. of the solution of chloride of lime, prepared accord- ing to the directions of 199 (containing O'l chloride of lime), into a beaker, and add about 6 c. c. of the solution of potassium iodide, prepared according to p. 445 (containing 0'6 KI) ; dilute the mix- 704 SPECIAL PAKT. [ 202. ture with about 100 c. c. of water, acidify with hydrochloric acid, and determine the liberated iodine as directed 146. As 1 at. iodine corresponds to 1 at. chlorine, the calculation is easy. This method gives excellent results. (Compare Expt. No 99.) 6. EXAMINATION OF BLACK OXIDE OF MANGANESE. 202. The native black oxide of manganese (as also the regenerated artificial product) is a mixture of manganese dioxide with lower oxides of that metal, and with ferric oxide, clay, &c., ; it also inva- riably contains moisture, and frequently chemically combined water. The commercial value of the article depends entirely upon the amount of dioxide (or, more correctly expressed, of available oxygen) which it contains. By " available oxygen " we understand the excess of oxygen contained in a manganese, over the 1 at. com- bined with the metal to monoxide ; upon treating the ore with hydrochloric acid, an amount of chlorine is obtained equivalent to this excess of oxygen. This available oxygen is always expressed in the form of manganese dioxide. 1 at. corresponds to 1 mol. man- ganese dioxide, since MnO 2 = MnO -|- O. I. DRYING THE SAMPLE. All analyses of manganese proceed, of course, upon the suppo- sition that the sample operated upon is a fair average specimen of the ore. A portion of a tolerably finely powdered average sample is generally sent for analysis to the chemist ; in the case of new lodes, however, a number of samples, taken from different parts of the mine, are also occasionally sent. If, in the latter case, the aver- age composition of the ore is to be ascertained, and not simply that of several samples, the following course must be resorted to : Crush the several samples of the ore, in an iron mortar, to coarse powder, and pass the whole of this through a rather coarse sieve. Mix uni- formly, then remove a sufficiently large portion of the coarse pow- der with a spoon, reduce it to powder in a steel mortar, passing the whole of this through a fine sieve. Mix the powder obtained by this second process of pulverization most intimately ; take about 8 10 grm. of it, and triturate this, in small portions at a time, in an agate mortar, to an impalpable powder. Average samples are 303."] EXAMINATION OF MANGANESE. 705 generally already sufficiently tine to require only the last opera- tion. As regards the temperature at which the powder is to be dried, if you desire to expel the whole of the moisture without dis- turbing any of the water of hydration, the temperature adopted must be 120 (this is the result of my own experiments, see Expt. ?s o. 100). But, as there appears to be at present an almost univer- sal understanding, in the manganese trade, to limit the drying tem- perature to 100, the fine powder is exposed, in a shallow copper or brass pan, for 6 hours, to the temperature of boiling water, in a water bath (p. 53, fig. 23.) When the samples have been dried, they are introduced, still hot, into glass tubes 12 14 cm. long and 8 10 mm. wide, sealed at one end ; these tubes are then corked and allowed to cool. In laboratories where whole series of analyses of different ores are of frequent occurrence, it is advisable to number the drying- pans and glass tubes, and to transfer the samples always from the pan to the tube of the corresponding number. II. DETERMINATION OF THE MANGANESE DIOXIDE. 203. Of the many methods that have been proposed for the valuation of manganese ores, I select three as the most expeditious and accu- rate. The first is more particularly adapted for technical pur- poses. A. FRESENIFS and WILL'S Method. a. If oxalic acid (or an oxalate) is brought into contact with manganese dioxide in presence of water and excess of sulphuric acid, manganous sulphate is formed, and carbon dioxide evolved, while the oxygen, which we may assume to exist in the manganese dioxide in combination with the monoxide, combines with the ele- ments of the oxalic acid, and thus converts the latter into carbon dioxide. Mn0 2 + H 2 S0 4 + H 2 C 2 4 = MnSO 4 -f 2H 2 O + 2CO 2 . Each atom of available oxygen, or, what amounts to the same, each mol. binoxide of manganese = 87. gives 2 mol. carbon dioxide = 88. 706 SPECIAL PAKT. [ 203. b. If this process is performed in a weighed apparatus from which nothing except the evolved carbonic acid can escape, and which, at the same time, permits the complete expulsion of that acid, the diminution of weight will at once show the amount of carbonic acid which has escaped, and consequently, by a very sim- ple calculation, the quantity of dioxide contained in the analyzed manganese ore. As 88 parts, by weight, of carbon dioxide corre- spond to 87 of manganese dioxide, the carbon dioxide found need simply be multiplied by 87, and the product divided by 88, or the carbon dioxide may be multiplied by ?_0-9887, 88~~ to find the corresponding amount of manganese dioxide. c. But even this calculation may be avoided by simply using in the operation the exact weight of ore which, if the latter con- sisted of pure dioxide, would give 100 parts of carbon dioxide. The number of parts evolved of carbon dioxide expresses, in that case, directly the number of parts of dioxide contained in 100 parts of the analyzed ore. It results from J that 98-87 is the number required. Suppose the experiment ' is made with 0*9887 grm. of the ore, the number of centigrammes of carbon dioxide evolved in the process expresses directly the percentage of dioxide contained in the analyzed manganese ore. Now, as the amount of carbon dioxide evolved from 0-9887 grm. of manganese would be rather small for accurate weigh- ing, it is advisable to take a multiple of this weight, and to divide afterwards the number of centigrammes of carbon dioxide evolved from this multiple weight by the same number by which the unit has been multiplied. The multiple which answers the pur- pose best for superior ores is the triple, = 2'966 ; for inferior ores, I recommend the quadruple, 3-955, or the quintuple, = 4-9435, The analytical process is performed in the apparatus illustrated in fig. 58, p. 409. The flask A should hold, up to the neck, about 120 c. c. ; B about 100 c. c. The latter is half filled with sulphuric acid ; the tube a is closed at l> with a little wax ball, or a very small piece of caoutchouc tubing, with a short piece of glass rod inserted in the other end. Place 2-966, or 3-955, or 4-9435 grm. according to the quality 203. J EXAMINATION OF MANGANESE. 707 of the ore in a watch-glass, and tare the latter most accurately on a delicate balance ; then remove the weights from the watch-glass, and replace them by manganese from the tube, very cautiously, with the aid of a gentle tap with the linger, until the equilibrium is exactly restored. Transfer the weighed sample, with the aid of a card, to the flask ^1, add 5 6 gnn. normal sodium oxalate, or about 7'5 grm. normal potassium oxalate, in powder, and as much water as will fill the flask to about one third. Insert the cork iuto A, and tare the apparatus on a strong but delicate balance, by means of shot, and lastly, tinfoil, not placed directly on the scale, but in an appropriate vessel. The tare is kept under a glass bell. Try whether the apparatus closes air-tight. Then make some sul- phuric acid flow from B into A, by applying suction to d, by means of a caoutchouc tube. The evolution of carbon dioxide com- mences immediately in a steady and uniform manner. When it begins to slacken, cause a fresh portion of sulphuric acid to pass into A, and repeat this until the manganese ore is completely decomposed, which, if the sample has been very finely pulverized, requires at the most about five minutes. The complete decompo- sition of the analyzed ore is indicated, on the one hand, by the ces- sation of the disengagement of carbon dioxide, and its non-renewal upon the influx of a fresh portion of sulphuric acid into A ; and, on the other hand, by the total disappearance of every trace of black powder from the bottom of A.* Xow cause some more sulphuric acid to pass from B into A, to heat the fluid in the latter, and expel the last traces of carbon dioxide therein dissolved ; remove the wax stopper, or india-rubber tube, from i, and apply gentle suction to d until the air drawn out tastes no longer of carbon dioxide. Let the apparatus cool com- pletely in the air, and place it on the balance, with the tare on the other scale, and restore equilibrium. The number of centigramme weights added, divided by 3, 4, or 5, according to the multiple of 0:9887 grm. used, expresses the percentage of dioxide contained in the analyzed ore. In experiments made with definite quantities of the ore, weigh- ing in an open watch-glass cannot well be avoided, and the dried manganese is thus exposed to the chance of a reabsorption of water * If the manganese ore has been pulverized in an iron niortar, a few black spots (particles of iron from the mortar) will often remain perceptible. 708 SPECIAL :PAKT. L from the air, which of course tends to interfere, to however so trifling an extent, with the accuracy of the results. In very pre- cise experiments, therefore, the best way is to analyze an indeter- minate quantity of the ore, and to calculate the percentage as shown above. For this purpose, one of the little corked tubes, filled with the dry pulverized ore, is accurately weighed, and about 3 to 5 grm. (according to the quality of the ore) are trans- ferred to the flask A. By now re weighing the tube, the exact quantity of ore in the flask is ascertained. To facilitate this opera- tion, it is advisable to scratch on the tube, with a iile, marks indi- cating approximately the various quantities which may be required for the analysis, according to the quality of the ore. With proper skill and patience on the part of the operator, a good balance and correct weights, this method gives most accurate and corresponding results, differing in two analyses of the same ore barely to the extent of (>2 per cent. If the results of two assays differed by more than 0*2 per cent., a third experiment should be made. In laboratories where analyses of manganese ores are matters of frequent occurrence, it will be found convenient to use an aspirator for sucking out the carbon dioxide. In the case of very moist air, the error which proceeds from the fact that the water in the air drawn through the appara- tus is retained, and which is usually quite inconsiderable, may now be increased to an important extent. Under such circumstances, connect the end of the tube b with a calcium chloride tube during the suction. Very accurate determinations may also be made by weighing the evolved carbon dioxide. For this purpose the apparatus described on page 414, fig. 61, is well adapted. From '5 to 1. grin, ore should be used for a determination. Introduce the ore and oxalic acid or oxalate into the decomposing flask, fill the flask about one third with water, connect the several parts of the apparatus as for the determination of carbonic acid, decompose the ore by admitting gradually strong sulphuric acid, remove the evolved CO 2 completely from the unweighed portion of the apparatus into the potash bulbs as described for the determination of CO 3 . Some ores of manganese contain carbonate* of the alkali-earth i net < ilx, which of course necessitates a modification of the foregoing process. To ascertain whether carbonates of the alkali-earth metals are present, boil a sample of the pulverized ore with water, and g 203.] EXAMINATION OF MANUANKSK. 709 add nitric acid. If any effervescence takes place, the process is modified as follows (RottR?): After the weighed portion of ore has been introduced into the liask ^4, treat it with water, so that the flask may be about i full, add a few drops of dilute sulphuric acid (1 part, by weight, sulphuric acid, to 5 parts water) and warm with agitation, prefer- ably in a water bath. After some time dip a rod in and test whether the fluid possesses a strongly acid reaction. If it does not, add more sulphuric acid. As soon as the whole of the car- bonates are decomposed by continued heating of the acidified fluid, completely neutralize the excess of acid with soda solution free from carbonic acid, allow to cool, add the usual quantity of sodium oxalate, and proceed as above. If you have no soda solution free from carbonic acid at hand, you may place the sodium oxalate or oxalic acid (about 3 grin.) in a small tube, and suspend this in the flask A by means of a thread fastened by the cork. When the apparatus is tared, and you have >atisfied yourself that it is air-tight, release the thread and proceed as above. B. BUNSEN'S Method. Reduce the ore to the very finest powder, weigh off about 0*4 grm., introduce this into the small flask #, illustrated in fig. 64, p. 435, and pour pure fuming hydrochloric acid over it ; conduct the process exactly as in the analysis of chromates. Boil until the ore is completely dissolved and all the chlorine expelled, which is effected in a few minutes. 2 atoms of iodine separated coriespond to 2 at. chlorine evolved, and accordingly to 1 mol. of manganese dioxide. For the estimation of the separated iodine, the method 140 may be employed. Results most accurate. C. Estimation of tJiy wean* of-I-run. Dissolve, in a small long- necked flask, placed in a slanting posi- tion, about 1 grm. pianoforte wire, accurately weighed, in moder- ately concentrated pure hydrochloric acid ; weigh off about 0'6 grm. of the sample of manganese ore in a little tube, drop this into the flask, with its contents, and heat cautiously until the ore is dis- solved. 1 mol. of manganese dioxide converts 2 at. of dissolved iron from the state of ferrous to ferric chloride. When complete * Zeitschr. f. anal. Them. 1, 48. 710 SPECIAL PART. [g - solution lias taken place, dilute the contents of the flask with water, allow to cool, rinse into a beaker, and determine the iron still remaining in the state of ferrous chloride with potassium dichro- mate (p. 274). Deduct this from the weight of the wire employed in the process ; the difference expresses the quantity of iron which has been converted by the oxygen of the manganese from ferrous to ferric chloride.* This difference multiplied by 4|^ 5 - or 0-7768 gives the amount of manganese dioxide in the analyzed ore. This method also, if carefully executed, gives very accurate results. The main reason why this method is less suitable for industrial use than the first lies in the fact that the analyst must work with much smaller quantities of substance. Hence to obtain results equally accurate with those yielded by A, far greater nicety in weighing and manipulating is required. Instead of metallic iron, weighed quantities of pure ferrous sulphate or ferrous ammonium, sulphate may be used. III. ESTIMATION OF MOISTURE IN MANGANESE, 204. In the purchase and sale of manganese, a certain proportion of moisture is usually assumed to be present, and often a percentage is fixed within which the moisture must be confined. In estimat- ing the moisture the same temperature should be employed, at which the drying for the purpose of determining the dioxide is effected ( 202, I.). As the amount of moisture in an ore may be altered by the operations of crushing and pulverizing, the experiment should be made with a sample of the mineral which has not yet been sub- jected to these processes. The drying must be continued until no further diminution of weight is observed ; at 100, this takes about 6 hours ; at 1 20, generally only 1 J hours. If the moisture in a manganese ore is not to be estimated on the spot, but in the labora- tory, a fair average sample of the ore should be forwarded to the chemist in a strong, perfectly dry, and well-corked bottle. * In very precise experiments, the weight of the iron must be multiplied by 0-997, since pianoforte wire ma}- always be assumed to contain about 0'003 impurities. 206.] ANALYSIS OF COMMON SALT. 711 IV. ESTIMATION OF THE AMOUNT OF HYDROCHLORIC Acn> REQUIRED FOR THK COMPLETE DECOMPOSITION OF A MANGANESE. 205. Different manganese ores, containing the same amount of avail- able oxygen, or, as it is usually expressed, of binoxide of manga- nese, may require very different quantities of hydrochloric acid to effect their decomposition and solution, so as to give an amount of -chlorine corresponding to the available oxygen in them ; thus, an ore consisting of 60 per cent, of binoxide of manganese and 40 per cent, of sand and clay requires 4 mol. hydrochloric acid to 1 at. of available oxygen; whereas an equally rich ore containing lower oxides of manganese, ferric oxide, or calcium carbonate requires a jnuch larger proportion of hydrochloric acid. The quantity of hydrochloric acid in question may be deter- in ined by the following process : Determine volumetrically the strength of a moderately strong hydrochloric acid (of, say, 1*10 sp. gr.). Warm 10 c. c. of the same acid with a weighed quantity (about 1 grm.) of the manganese, in a, small, long-necked flask, with a glass tube, about 3 feet long, fitted into the neck. Fix the flask in a position that the tube is directed obliquely upwards, and then gently heat the contents. As soon as the manganese is decomposed, apply a somewhat .stronger heat for a short time, to expel the chlorine which still remains in solution ; but carefully avoid continuing the application of heat longer than is absolutely necessary, as it is of importance to guard against the slightest loss of hydrochloric acid. Let the flask cool, dilute the contents with water, and determine the free hydrochloric acid remaining. Deduct the quantity found from that originally added ; the difference expresses the amount of hydrochloric acid required to effect the decomposition of the man- 1. ANALYSIS OF COMMON SALT. 206. I select this example to show how to analyze, with accuracy and tolerable expedition, salts which, with a predominant principal ingredient, contain small quantities of other substances. 712 SPECIAL PART. [ 206. a. Keduce the salt by trituration to a uniform powder, and put this into a stoppered bottle. b. Weigh off 10 grm. of the powder, and dissolve in a beaker by digestion with water ; filter the solution into a -J-litre flask, and thoroughly wash the small residue which generally remains. Finally, fill the flask with water up to the mark, and shake the fluid. If small white grains of calcium sulphate are left on dissolving the salt, reduce them to powder in a mortar, add water, let the mixture digest for some time, decant the clear supernatant fluid on to a filter, triturate the undissolved deposit again, add water, &c., and repeat the operation until complete solution is effected. c. Ignite and weigh the dried insoluble residue of b, and subject it to a qualitative examination, more especially with a view to ascer- tain whether it is perfectly free from calcium sulphate. (L Of the solution 5, measure off successively the following quantities : For e. 50 c. c. corresponding to 1 grm. of common salt. " /. 150 c. c. " 3 g. 150 c. c. " "3 " " " h. 50 c.c. I " " e. Determine in the 50 c. c. measured off, the chlorine as directed 141, L, a or I. f. Determine in the 150 c. c. measured off, sulphuric acid as directed 132, L, 1. g. Determine in the 150 c. c. measured off, the calcium and magnesium, as directed p. 496, 28. h. Mix the 50 c. c. measured off in a platinum dish, with about \ c. c. of pure concentrated sulphuric acid, and proceed as directed 98, 1. . The neutral residue contains the sulphates of sodium r calcium, and magnesium. Deduct from this the quantity of the two latter substances as resulting from g ; the remainder is sodium. sulphate. i. Determine in another weighed portion of the salt, the water as directed 35, a, a, at the end. k. Bromine and other bodies, of which only very minute traces are found in common salt, are determined by the methods described in Part I. 207.] ANALYSIS OF -GUNPOWDER. 713 8. ANALYSIS OF GUNPOWDER* 207. Gunpowder, as is well known, consists of nitre, sulphur, and char- coal, and, in the ordinary condition, invariably contains a small quan- tity of moisture. The analysis is frequently confined to the deter- mination of the three constituents and the moisture, but often the examination is extended to the nature of the charcoal, and the car- bon, hydrogen, oxygen, and ash therein are estimated. <(. Determination of the Moixtnre. Weigh 2 3 grm. of the substance (not reduced to powder) between two well-fitting watch-glasses, and dry in the desiccator, or at a gentle heat, not exceeding 60, till the weight remains con- stant. l>. Determination of the Nitre. Place an accurately weighed quantity (about 5 grm.) on a filter, moistened with water ; saturate with water, and, after some time, repeatedly pour small quantities of hot water upon it until the potassium nitrate is completely extracted. Receive the first filtrate in a small weighed platinum dish, the washings in a beaker or small flask. Evaporate the contents of the platinum dish cau- tiously, adding the washings from time to time, heat the residue cautiously to incipient fusion, and weigh it.f c. Determination of the Sulphur. Oxidize 2 3 grm. of the powder with pure concentrated nitric acid and potassium chlorate, the latter being added in small por- tions, while the fluid is maintained in gentle ebullition. If the operation is continued long enough, it usually happens that both the charcoal and sulphur are fully oxidized, and a clear solution is * As regards the determination of the sp. gr. of gunpowder, I refer to HEER- EN'S paper on the subject, in Mittheilungen des Gewerbevereins fur Hannover, 1856, 198178; Polyt. Centralbl. 1856, 1118. f The potassium nitrate may also be estimated in an expeditious manner, and with sufficient accuracy for technical purposes, by means of a hydrometer, which is constructed to indicate the percentage of this ingredient when floated in water containing a certain proportion of gunpowder in solution. A method based upon the same principle, proposed by Uchatius, is given in the Wiener akad. Ber. X. 748: also Anna!, d. ('hem. u. Pharm. 88, 395. 714 SPECIAL PAKT. [ 208. finally obtained. Evaporate with excess of pure hydrochloric acid on a water-bath to dryness, filter, if undissolved charcoal should render it necessary, and determine the sulphuric acid after 132, i, i. d. Determination of the Charcoal. Digest a weighed portion of the powder repeatedly with .ammonium sulphide, till all sulphur is dissolved, collect the char- coal on a filter dried at 100, wash it first with water containing ammonium sulphide, then with pure water, dry at 100, and weigh. The charcoal so obtained must, under all circumstances, be tested for sulphur by the method given under f silica. Treat the residue with strong hydrochloric acid 5 to lo minutes, add water and filter. The insoluble portion, consisting of silica and the undecomposed part of the rock, is ignited with the filter in a platinum crucible and fused with sodium carbonate. Silica is then separated in the usual manner, and the second solution of basic metals thus obtained is added to the first. Alkalies are determined in another portion by the method of J. L. Smith (page 426.) 2. Water. Silicates dried at 100 occasionally contain wut^r. This is determined by taking a weighed portion dried at 100 and igniting in a platinum crucible, or in presence of carbon, carbon- ates, or ferrous iron in a tube, through which a stream of dry air is drawn, the moisture expelled from the substance being retained by a weighed calcium chloride tube. If the escaping aqueous vapors manifest acid reaction, owing TO disengagement of hydrofluoric acid or silicon fluoride, mix the substance with 6 parts of finely triturated recently ignited lead oxide in a small retort, weigh, ignite, and weigh again. This method, however, cannot be used if carbonic acid as well as fluor- rine is present. In that case the method employed by L. SIPOCZ* may be used. Ignite 4 parts sodium carbonate in a platinum cru- cible till water is completely expelled, allow to cool to 50 or 60, mix intimately with a platinum wire with 1 part of the pulverized dried silicate, introduce the mixture into a capacious platinum boat, rinsing out the last adhering portions with sodium carbonate. The boat, provided with a cover, is now placed in the middle of a por- celain tube (glazed inside) and heated in an air bath an hour to 120 or 130 C. During this time every trace of moisture should be removed from the mixture by passing dried air by means of a gaso- meter through the tube. The end of the tube through which the current of air makes its exit is provided with a calcium chloride tube, which at the end of the drying process is replaced by a weighed F tube, containing glass beads moistened with pure strong sulphuric acid. The substance is now brought to a red heat in a combustion furnace, and a regulated current of air (dried by sul- *Zeitschr. f. anal. Chernie. 17, 207. 716 SPECIAL PART. [ 208. plmric acid) is passed over it about lialf an hour to carry the expelled water vapor into the absorbing apparatus. (It is obvious that this method can be used in any .case instead of ignition with lead oxide). 3. Carbonic acid and water. If it can be proved by a prelimi- nary experiment, that carbonic acid, as well as water, can be com- pletely removed by intense ignition, and no other constituents (ferrous iron, manganese, fluorine, sulphides, alkali fluorides, and chlorides, &c.) are present which will cause change of weight on ignition; the joint amount of water and carbonic acid may be determined by loss of weight on ignition, and carbonic acid in another portion according to 139, II., e. The amount of water present equals the difference between the two quantities thus found. If, as is usually the case, the nature of the substance does not allow the joint amount of water and carbonic acid to be deter- mined by loss on ignition, water may be determined by the method recommended by SIPOCZ (described above in 2). A much simpler and sufficiently accurate method, however, is to determine both water and carbonic acid at once by ignition of the substance with lead chromate mixed with y 1 ^ its weight of potassium dichromate in a combustion tube, collecting and weighing the evolved water and carbonic acid. The process is conducted precisely as in the combustion of organic compounds (see 177) except that it is not necessary (unless sulphides are present) to place lead chromate in front of the mixture of chromates with the pulverized rock. Heat should be applied toward the end of the process sufficient to fuse the mixture. It is desirable to use 2 grm. or even more of the sub- stance for the determination, and to take great care to avoid pres- ence of hygroscopic moisture in the chromates. Carbonaceous matter (rarely present in rocks) would of course interfere with the determination of CO a by this process.* 4. Ferrous iron is most readily determined by decomposing with a mixture of sulphuric and hydrofluoric acids and titration with potassium permanganate according to 160, 84, page 526. With a little skill and proper attention, the simple method of effecting the * Very satisfactory results were obtained both by myself and Mr. W. c. c. dilute sulphuric acid and evaporate till fumes of sul- phuric acid appear ; cool, add a little water, digest till sulphates, Arc., are dissolved, filter off and weigh the traces of silica, add the filtrate to the solution of titanic acid previously obtained. Add next to the solution, sodium carbonate until a slight precipi- tate is formed which does not redissolve on. stirring. Xext add 4 c. c. pure dilute sulphuric acid, which is designed to dissolve the slight precipitate and prevent precipitation of iron along with tita- nium in the subsequent part of the process (too much free acid would prevent complete precipitation of the titanic acid). Solu- tion of sulphurous acid is then added to reduce the iron to ferrous sulphate, the solution being exposed to a very gentle heat till it becomes nearly colorless, when it should be diluted to a volume of 700 to 800 c. c. and boiled two hours with occasional addition of a 718 SPECIAL PART. [ 208. i'ew c. c, dilute, previously heated, solution of sulphurous acid. Titanic acid if present will be precipitated. After filtering, iron may be determined in the filtrate by concentrating, reducing with 1 1. ,S, boiling out excess of H 2 S and titrating with standard potas- sium permanganate according to 113, 3, a. It may here be observed that by proceeding as above directed r in separating titanic acid from the silica the traces of alumina and possibly other basic oxides which may be retained by the silica are lost. This defect may be remedied, at the expense of some delay, by reserving the solution containing all the basic metals as first filtered from the separated' silica until the sulphuric acid solutions of the titanic acid and other impurities possibly present in the silica can be obtained and added to it. The iron and alumina precipitate will then contain all the titanic acid, and the traces of basic metals recovered from the silica will be united to the main portion. If this course is adopted, the use of an unnecessary amount of sodium carbonate and sulphuric acid in obtaining a solution of the residue from the silica should be avoided. The precipitate of aluminium and ferric hydroxides should, in order to eliminate basic sulphates, be dissolved and reprecipitated a proceeding which is always advisable, even in the absence of sulphates, when alkali-earth metals are present. Sulphur. If sulphides are present determine sulphur as in iron ores (see page 745). It must be borne in mind, however, that if barium, strontium, or lead is present a portion of the sulphuric acid formed may be retained in the undissolved residue. By pro- longed boiling of this residue with sodium carbonate and filtering, the sulphuric acid may be brought into solution as sodium sul- phate. This solution may also contain silica and lead, from which the sulphuric must be separated. If sulphates are present in the original material along with sul- phides, the sulphuric acid may be determined by boiling a separate portion a long time with sodium carbonate, filtering, acidifying the filtrate with HC1, and precipitating with BaCl 2 . The sulphur in the sulphuric acid thus found, deducted from the total amount existing in both sulphides and sulphates, leaves that belonging to the sulphides. Phosphoric acid may be determined as in iron ores (see p. 741). In careful investigations the residue insoluble in acids should be examined also by fusing it with sodium carbonate, separating silica 209.] SEPARATION OF SILICATES. 719 by drying down with nitric acid, redissolviiig with nitric acid and adding molybdic acid solution. The reagents used in this process must be free from the least trace of phosphoric acid.] 10. SEPARATION OF SILICATES DECOMPOSABLE FROM THOSE TOTDECOMPOSABLE BY ACIDS. 209. After the silicate has been very finely pulverized and dried at 100 it is usually treated for some time, at a gentle heat, with moderately concentrated hydrochloric acid, evaporated to dryness on the water-bath, the residue moistened with hydrochloric acid, water added, and the solution filtered ; it is often preferable, how- ever, to digest the powder with dilute hydrochloric acid (of about 1 5 per cent.) for some days at a gentle heat, and then at once filter the solution. Which of the two ways it is advisable to adopt, and indeed whether the method here described (which was first employed by CHR. GMELIX in the analysis of phonolites) may be resorted to, depends Upon the nature of the mixed minerals. The more readily decomposable the one of the constituent parts of the mixture is, and the less readily decomposable the other, the more constant the proportion between the undissolved and the dissolved part is found to remain in different experiments ; in other words, the less the undissolved part is affected by further treatment with hydrochloric acid, the more safely may this method of decomposi- tion be resorted to. The process gives : '/. A JtyrfrocMorie aci^l solution, containing, besides a little silicic acid, the basic metals of the decomposed silicate in the form of metallic chlorides, which are separated and determined by the proper methods. J. An Insoluble residue, which contains, besides the undecom- posed silicate, the silica separated from the decomposed silicate. After the latter has been well washed with water, to which a few drops of hydrochloric acid have been added, transfer it, still moist, in small portions at a time, to a boiling solution of sodium carbonate (free from silicic acid) contained in a platinum dish ; boil for some time, and filter off each time, still very hot, through a weighed filter. Finally, rinse the last particles of the residue 720 SPECIAL PART. [ 209. which still adhere to the filter completely into the dish, and pro- ceed .as before. Should this operation not fully succeed, dry and incinerate the filter, transfer the ash to the platinum dish, and boil repeatedly with the solution of sodium carbonate till a few drops of the fluid finally passing through the filter remain dear on warming with excess of ammonium chloride. "Wash the residue, first with hot water, then to insure the removal of every trace of sodium carbonate which may still adhere to it with water slightly acidified with hydrochloric acid, and finally again with pure water. Collect the washings in a separate vessel (H. ROSE). Acidify the alkaline filtrate with hydrochloric acid, and deter- mine in it the silicic acid which belongs to the silicate decomposed by hydrochloric acid, as directed 140, !!.,. To ascertain how much water the part decomposed by acid contains, the following data are required : The percentage which the decomposed part is of the whole, the percentage of water in the undecomposed part, the percentage of water in the original mixture of silicates. Dry the nndissolved silicate at 100 and weigh. Then calculate by difference the quantity of the dissolved silicate. Treat the undis- solved silicate as directed 140, II., ~b. For determination of water, ferrous iron, titanic acid, and other minor constituents, see 8 208. 11. ANALYSIS OF LIMESTONES, DOLOMITES, MARLS, &c. As the minerals containing calcium and magnesium carbonates play a very important part in manufactures and agriculture, the chemist is often called upon to analyze them. The analytical pro- cess differs according to the different object in view. For tech- nical purposes, it is sufficient to determine the principal constitu- ents ; the geologist takes an interest also in the matter present in smaller proportions ; whilst the agricultural chemist seeks a knowl- edge not only of the constituents, but also of the state of solubility, in different menstrua, in which they are severally present. I will give, in the first place, a process for effecting a complete and accurate analysis ; and, in the second place, the volumetric methods by which the calcium and magnesium carbonates may be determined. An accurate qualitative examination should always precede the quantitative analysis. 210. j ANALYSIS OF LIMESTONES, DOLOMITES, MARLS. 721 A. METHOD OF EFFECTING THE COMPLETE ANALYSIS. 210. a. Reduce a large piece of the mineral to powder, mix this uniformly, and dry at 100. 1. Treat about 2 grm., in a covered beaker, with dilute hydro- chloric acid in excess, evaporate to dryness in a platinum or por- celain dish, moisten the residue with hydrochloric acid, heat with water, filter on a dried and weighed filter, wash the insoluble residue, dry at 100, and weigh. It generally consists of separated .y///m, clay, and sand : but it often contains also hurtvu&like ?//, ), the aluminium pre- cipitate may be calculated as aluminium phosphate (A1 2 O 3 , P 2 O 5 ). If, on the contrary, no precipitate is formed, the phosphoric acid must be determined in the alumina precipitate as directed 134, i., i, ft. Precipitate III. consists principally of manganese sulphide. It may also contain traces of nickel, cobalt, and zinc sulphides, cal- cium carbonate, &c. Treat with moderately dilute acetic acid, heat the filtrate, to remove any carbonic acid, add ammonia, pre- cipitate with ammonium sulphide, allow to stand 24 hours, and determine the manyanese as sulphide ( 109, 2). If any residue was left insoluble in acetic acid, test it for the above-mentioned metals. The fluid filtered from the pure manganese sulphide is to be mixed with ammonium carbonate. If a precipitate forms it is to be treated with precipitate IY. Precipitate* IV., V.,VI. The united mass of these precipi- tates, together with the small portions of alkali-earth carbonates obtained during the treatment of precipitates I. and III. contain the whole of the strontium and the whole of the barium which originally passed into the hydrochloric acid solution. Ignite the dried precipitate (if necessary in portions) in a platinum crucible, most intensely over the gas blowpipe. By this means any barium * I may remind the operator that the residue, which contains nitric acid, can- not he heated with hydrochloric acid in a plntimim dish. 210.] AXALYSIS OF LIM*;STONKS, DOLOMITES, MARLS. 735 and strontium carbonate!?, and a part, at all events, of the calcium carbonate, are converted into oxides (ENGELBACH*). Boil the resi- due 5 or 6 times with small portions of water, pouring oif the solu- tion through a filter ; neutralize the solution with hydrochloric acid, evaporate to dry ness, and test a minute portion with the spectroscope this minute portion is afterwards added to the rest. If calcium and strontium alone are present, separate according to 26. If barium is present, separate the three alkali-earth metals after 23. l>b. Although it is possible in aa to test for metals precipitable by hydrogen sulphide from acid solution, e.g., copper, and if required to determine them, still it is more convenient to employ a fresh quarter of the hydrochloric acid solution for this purpose. The precipitate obtained by passing the gas into the warm dilute solution is washed, dried, and treated with carbon disulphide. If a residue remains it is to be examined. re. The remaining quarter of the dilute hydrochloric acid solu- tion is used for the estimation of the alkalies.^ Mix with chlo- rine water, then with ammonia and ammonium carbonate ; after allowing the mixture to stand for some time,~filter off the precipi- tate, evaporate the filtrate to dryness, ignite the residue in a plati- num dish to remove the ammonium salts, and finally separate the magnesium from the alkalies as directed p. 491, 15. The reagents must be most carefully tested for fixed alkalies, and the use of glass and porcelain vessels avoided as far as practicable. Should the limestone contain a sulphate soluble in hydrochloric acid, precipitate the sulphuric acid by a small excess of barium chloride, allow to settle, and filter off the barium sulphate (which is to be determined in the usual manner) before proceeding as above to the estimation of the alkalies. //. As calcite and aragonite may contain fluorides * Zeitschr. f. anal. Chem. 1, 474. \ The simplest way of ascertaining whether and what alkalies are present in a limestone, is the process given by ENGELBACH (Annal. d. Chem. u. Pharm. 123, 260) viz., ignite a portion of the triturated mineral strongly in a platinum cru- cible over the blast, boil with a little water, filter, neutralize with hydrochloric acid, precipitate with ammonia and ammonium carbonate, filter, evaporate the nitrate to dryness and examine with the spectroscope. The ammonium carbon- ate precipitate may be evaporated with hydrochloric acid to dryness, and exam ined in like manner for barium and strontium. J Pogg. Annal. 96, 145. 726 SPECIAL PAKT. [ 211. the possible presence of fluorine must not be disregarded in accu- rate analyses of limestones. Treat, therefore, a larger sample of the mineral with acetic acid until the calcium and magnesium car- bonates are decomposed ; evaporate to dryness until the excess of acetic acid is completely expelled, and extract the residue with water ( 138, I.). We have the fluorine in the residue. If it can be distinctly detected in a portion of the same,* the determination may be attempted after 138, II., 3, a. i. If the limestone under examination contains chlorides, treat a large sample with water and nitric acid, at a very gentle heat ; filter, and precipitate the chlorine from the filtrate by solution of silver nitrate. k. It is often interesting for agriculturists to know the degree of solubility of a sample of limestone or marl in the weaker solv- ents. This may be ascertained by treating the sample first with water, then with acetic acid, finally with hydrochloric acid, and examining each solution and the residue. The analysis of marls made by C. STRUCKMANNf were done in this manner. I. To effect the separation of the caustic or carbonated lime, in hydraulic limes, from the silicates, DEVILLED proposed to boil with solution of ammonium nitrate, which he stated would dissolve the caustic lime and carbonate of lime, without exercising a decom- posing action on the silicates. GUNNING found, however, that by this process the double silicates of aluminium and calcium are more or less decomposed, with separation of silicic acid. As yet no method is known by which the object here stated can be accom- plished with absolute accuracy ; the best way, perhaps, is treating the sample with dilute acetic acid ; C. KNAUSZ | recommends hydrochloric acid. B. VOLUMETRIC DETERMINATION OF CALCIUM CARBONATE AND MAG- NESIUM CARBONATE (for technical purposes). 211. a. If a mineral contains only calcium carbonate, the amount of the latter may be estimated from the quantity of acid required to * See Qual. Anal. 146, 6. f Annal. d. Chem. u. Pharm. 74, 170. \ Compt. rend. 37, 1001; Journ. f. prakt. Chem. 62, 81. Journ! f. prakt. Chem. 62, 318. I Gewerbeblatt aus Wttrtcmbera:, 1855, Nr. 4; Chem. Oentralbl., 1855, 244. ANALYSIS OF LIMESTONES, DOLOMITES, MARLS. 7*27 Affect its decomposition, the method described in 198 being employed for the purpose. Or the carbonic acid in the mineral may be determined, and 1 mol. calcium carbonate = 100 calculated for each mol. carbonic acid = 44. J>. But if the mineral contains, besides calcium carbonate, also magnesium carbonate, the results obtained by either process give the quantity of calcium carbonate -f- magnesium carbonate, the latter being expressed by its equivalent quantity of calcium car- bonate (/.<"., 100 of calcium carbonate for 84 of magnesium carbon- ate '). If, therefore, you desire to know the actual amount of each, YOU must, in addition to the above determination, determine one of the alkali-earth metals separately. For this purpose one of the two following methods may be employed : 1. Mix the dilute solution of 2 5 grm. of the mineral with ammonia and ammonium oxalate in excess, allow to stand for 12 hours and then filter. Ignite the precipitate of calcium oxalate, together with the filter, and treat the calcium carbonate produced as directed 198. This process gives the amount of calcium con- tained in the analyzed mineral ; the difference between this and the former result gives the calcium carbonate which is equivalent to the amount of magnesium carbonate present. To obtain per- fectly accurate results by this method, repeated precipitation is indispensable (see 154, 6, a). "2. Dissolve 2 5 grm. of the mineral in the least possible excess of hydrochloric acid, and add a solution of lime in sugar water as long as a precipitate forms. By this operation the mag- nesia only is precipitated. Filter, wash, and treat the precipitate as directed 198 ; the result represents the quantity of the magne- sium. Deduct the quantity of calcium carbonate equivalent thereto from the result of the total determination ; the remainder is the amount of calcium carbonate present. The method 2 is only suitable when the proportion of magne- sium is small. 728 SPECIAL PART. [ 212. [12. A8SAY OF COPPER ORES. 212. For the assayer who has occasion to determine the amount of copper in ores very frequently, the method of LTTCKOW* depending- on the electrolytic deposition of copper, and the method of STEIN- BECK^ (volumetric determination by means of potassium cyanide), are to be recommended. For the analytical chemist, who is only occasionally called upon to assay a copper ore, the processes below described may be useful, as they require no preparation of special reagents or apparatus. 1. When Arsenic, Antimony, Bismuth, (Cadmium, Tin) are not present. Take 1 grm. of the pulverized ore if rich, 3 to 5 if poor. Put it in a dry beaker (best of a diameter of 8 10 centimetres at the bottom), cover with a watch-glass. Mix in another glass vessel, which should be dry to avoid dilution, 1 pt. sulphuric with 3 to -t pts. nitric acid, both concentrated. Pour the mixed acids upon the ore. 40 50 c. c. will suffice if not more than 2 grm. ore are taken. The action is less violent if the requisite amount of acid is added at once than it is if added gradually. Heat the covered beaker 011 a sand-bath, to near 100 C. an hour or two, or until the action of the acids on the ore has apparently nearly ceased, raise then the watch- glass covering the beaker so far as to allow vapors to pass off freely by interposing between it and the beaker a triangle made of thick glass rod, and evaporate until nitric acid is completely removed. Copper exists in the residue as sulphate, mixed usually with other metallic sulphates, together with such constituents of the ore as are not decomposed by the acids. A small quantity of liquid (sulphuric acid) will still remain with the solid residue, and should not be removed by further elevation of temperature. After cooling, add about 100 c. c. of water to the residue and keep it warm on the sand-bath an hour to ensure solution of the anhydrous copper sul- phate. Complete solution of the copper in the residue may be effected in a few minutes by adding with the water a little hydro- chloric acid; but since hydrochloric acid dissolves notable quantities of lead sulphate, it should not be used for this purpose unless the ore is known to be free from lead. Filter from the undissolved Zeitschr. f. anal. Cliem. 8, 28., and 11, 1. \ Ib. 8, 9.. 212.] ASSAY OF COPPER ORES. part of the residue and wash it with hot water. If the residue contains lead sulphate, avoid the use of an unnecessary volume of water in washing, or use water acidified with sulphuric acid to pre- vent lead sulphate from being dissolved. Dilute the filtrate to about 500 c. c. If hydrochloric acid has not previously been used, add now 1 or 2 c. c. and heat to boiling and pass hydrogen sulphide through the solution until the copper is all precipitated, the tem- perature meanwhile being maintained nearly or quite to the boil- ing point. If a tolerably rapid current of H 2 S be passed into the solution through a tube contracted at the orifice to a diameter of 1 to 2 millimetres, so as to produce numerous and small bubbles, the precipitation is usually complete in course of 15 to 25 minutes. Wash the precipitate, dry, ignite in an atmosphere of hydrogen, and weigh the resulting' Cu a S according to directions in 111*. :>. , page 316. 2. When Antimony, Arsenic, (Bismuth, Cadmium, Tin \ - present. Arsenical or antimonial minerals are occasionally present in copper ores, bismuth compounds very rarely, while appreciable amounts of cadmium or tin can usually safely be assumed to be absent. If the ore to be assayed has not been pulverized and can be examined in large fragments, the assayer, with sufficient knowl- edge of mineralogy and experience in the use of the blowpipe, can usually decide whether arsenic, antimony, or even bismuth are present. If this cannot be done, qualitative testing in the wet way should be resorted to. If any of the metals which interfere with the process described in 1 are present, decompose the ore with aqua regia, adding also enough sulphuric acid to convert into sul- phates, on evaporation, any nitrates and chlorides which may be formed. An unnecessary excess of sulphuric should be avoided,, as it is difficult to remove by evaporation and, if allowed to remain in large amount, may render the subsequent precipitation of copper less perfect. After removing the nitric and hydrochloric acids- by evaporation, dissolve the copper sulphate in the residue by digestion with water, filter, add solution of sulphurous acid (100 200 c. c.), set in a warm, place ; if the solution ceases to smell of SO Z after half an hour, add more solution of sulphurous acid. Finally, after allowing the solution to stand in a warm place -t or 5 hours at least, precipitate the copper with ammonium or potassium sul- phocyanate and determine it as C'n,S as directed in 119, 3. I. 730 SPECIAL PART. [213. [13. ASSAY OF LEAD ORES 213. The commercial value of lead ore is often estimated from assays made in the dry way. These assays are not very exact even in rich ore, and still less so in poor ores. If the means for making a dry assay are not at hand, or a more accurate determination is required, the following method applicable to all ores (rich or poor, galenas or carbonates), not containing arsenic or antimony may be used. Decompose the finely pulverized ore 2 grin, if rich, 5 grm. if poor with a mixture of concentrated nitric and sulphuric acid precisely in the manner described for copper ores ( 212, 1). After free nitric acid has been removed by evaporation, the lead exists in the residue as lead sulphate, mixed, according to the char- acter of the ore, with different kinds and quantities of other metallic sulphates, and also such constituents of the ore as are not decomposed by the acids. Sulphuric acid, which may be used freely in the decomposing mixture, should remain also with this residue and not be driven off by evaporation. When, toward the close of the process of evaporation by gradually increasing tem- perature, dense white fumes of sulphuric acid begin to appeal-, or when, at a temperature little exceeding 100 C., no odor of nitric acid is perceptible, heat is removed and the residue allowed to cool. About 100 c. c. of water are then added. After digesting 2 hours to dissolve such metallic sulphates as are soluble in water,' the residue, containing lead sulphate and other insoluble matter (possibly, for example, quartz, native silicates, barium sulphate, calcium sulphate), is collected on a moderate sized filter and washed with water to which a little sulphuric acid has been added. The filter and its contents, without previous drying, are then placed in the bottom of a large beaker. Pour first ammonia (20 30 c. c.) upon the filter and residue, and next acetic acid to decided acid reac- tion, keep warm some 20 minutes with occasional stirring. The lead sulphate readily dissolves. Filter, wash the still remaining undissolved residue and filter, chiefly by decantation, adding to the wash water at first a little ammonium acetate. The filtrate may contain, besides lead, also calcium sulphate. To prevent the possi- $ 214.] NICKEL AND COBALT IN ORKS. 731 ble deposition of the latter during the subsequent precipitation of the lead, dilute the filtrate by adding ^ to 1 its volume of water, and add 1 or 2 c. c. dilute hydrochloric acid. Precipitate now the lead, either in the cold or slightly heated solution, with a current of hydrogen sulphide. Treat the precipitate according to 11(>, '2 page 299. In igniting in hydrogen, take care that only the bot- tom of the porcelain crucible is faintly red. Too high heat will cause loss by volatilization. If this ore contains arsenic and antimony, these elements, or at least the latter, will cause a small quantity of 'lead to remain undis- solved in the residue remaining after the treatment with ammo- nium acetate. In such a case, lead may be separated from the resi- due by means of methods of separation described in 164, or a wholly different course may be devised and applied to the original substance.] ' [14. DETERMINATION OF NICKEL AND COBALT IN ORES. SPEISS* AND MATTE.f 214. The separation of nickel and cobalt from other metals which accompany them in ores and determination of their joint amount precedes the separation of the two metals. The process requires great care throughout. A method is here given for determining these metals, and also copper and lead, in a " matte" containing, besides nickel and cobalt, copper, lead, iron, and accidental adhering parti- cles of sand and earthy silicates. To the description of this method will be appended modifications necessary or admissible in the examination of other products. 1. Decomposition and Separation of Lead. Decompose 2 gr. of the very finely pulverized material with a mixture of concentrated nitric and sulphuric acid, proceeding pre- cisely as recommended for decomposition of copper ores. (See ^ 212, 1.) It is, however, safer, after the nitric acid first employed * A product consisting chiefly of metallic arsenides obtained by smelting ores is called "speiss." . f A product consisting chiefly of metallic sulphides obtained by smelting ores is called "matte." 732 SPECIAL PABT. [ 214. has been expelled, to add to the residual sulphuric acid a fresh por- tion of concentrated nitric acid ; keep hot for some time, and finally evaporate off all the nitric acid a second time, allowing at least 8 or 10 hours for the whole process of decomposition. Add water (100 to 150 c.c.) to the cooled residue and digest 3 or 4 hours, and filter the solution of metallic sulphates obtained from the insolu- ble residue, which contains the lead as sulphate, together with par- ticles of sand, &c. Dissolve the lead sulphate in this residue with ammonium acetate and determine the lead as in the process of assay- ing lead ores, 213. Incinerate the filter containing the portion of the residue which ammonium acetate fails to dissolve in a porcelain crucible, and add to it in the crucible aqua regi# ; evaporate to a few drops. If the few drops of remaining liquid show no greenish color, it may be assumed that the residue so treated contains no nickel or cobalt. ' If the color indicates presence of these metals, rinse the contents of the crucible into the filtrate from the lead sulphate. Before throwing away the filtrate from the final lead precipitate (lead sulphide), prove that it contains no nickel or cobalt by adding ammo- nia to neutral reaction, and a few drops of ammonium sulphide. 2. Separation of Copper. Dilute the filtrate from the lead sulphate and other insoluble matter to about 500 c.c., and precipitate copper with hydrogen sul- phide and determine it, proceeding as directed in "Assay of Copper Ores," 212. 3. Separation of Iron. Concentrate the filtrate from the copper sulphide, add nitric acid enough to convert the iron into a ferric salt, and boil a few minutes. Allow the solution, which should now occupy a volume of about 300 c.c., to become nearly cold, and add a large twcss of ammonia at once, and let it stand in a warm place (50 to 70 C.) half an hour. Filter then into a porcelain casserole and wash the greater part of the saline matter out of the ferric hydroxide with hot water. Complete washing is needless. Although this filtrate contains the greater part of the nickel and cobalt, a very considerable quantity is retained by the ferric hydroxide. Even a second precipitation with ammonia cannot be relied upon for effecting a satisfactory sep- aration. Dissolve, therefore, the ferric hydroxide in hydrochloric acid, which may be used freely for this purpose, since it will be NICKEL AM) COBALT IX OKKS. 733 next converted into ammonium , chloride, which acts favorably, rather than otherwise, in the subsequent precipitation of iron ( 160, 71). Wash the filter from which the iron precipitate has been dissolved, neutralize the greater part of the free hydro- chloric acid in the solution with ammonia, proceed then care- fully to prepare the solution for precipitation of iron with sodium cwetate by neutralizing properly with sodium or ammonium car- bonate and addition of acetic acid, as described in 160, 71, p. 517. The iron precipitated thus a second time is still not absolutely free from a trace of nickel or cobalt, which may, however, be neglected unless extraordinary accuracy is required, or unless the original sub- stance was comparatively rich in these metals (containing over 2<> per cent). In that case, dissolve the iron precipitate in hydrochlo- ric acid and precipitate the iron again as basic ferric acetate and filter. Add the filtrate or filtrates, as the case may be, to the first ammoniacal filtrate, which should meanwhile have been concen- trated to expel free ammonia and reduce its volume. The mixed filtrates will now contain some free acetic acid. Concentrate in a porcelain dish to 300 or 400 c.c., and add ammonia to alkaline reac- tion. This will usually throw down a little ferric or aluminium hydroxide, which is to be filtered off. If the precipitate is very slight it may be thrown aw^ay. If considerable, dissolve in HC1, re precipitate with ammonia, filter, and add the filtrate to the main filtrate. 4. Precipitation <>f JT/V^v-/ //// (titration with standard sodium thiosulphate and iodine solutions). If ferrous iron is present, add, a little at a time, potassium chlorate (less than f gr. for 2 grm. ore usually suffices) until a minute portion of the 'solution taken out w r ith pointed glass rod and tested after dilution on a watch-glass with fresh solution of potassium ferricyanide gives no blue color. The unavoidable excess of potassium chlorate must now be decomposed by heating with hydrochloric acid, and the liberated chlorine removed by evaporating off about half the solu- tion. Next dilute to 500 c..c. and determine the iron by the process just mentioned. PHOSPHORUS. Take 5 grm. of the ore, unless it is known to contain a rather large quantity of phosphoric acicl, in which case 2 or 3 grm. should be used. Decompose with concentrated hydrochloric acid in a beaker having a diameter at the bottom of about 9 centimetres. The solution, without filtering from the insoluble residue, may be allowed to evaporate in a sand-bath nearly to dry ness, but before the liquid has been all removed, transfer the beaker to an air- * Some iron ores, especially magnetites, contain a small quantity of iron exist- ing as a constituent of a silicate (e.g.. hornblende or garnet), undecomposable by hydrochloric acid. In the assay of iron ores, the slight inaccuracy which on this account results is usually disregarded. 742 SPECIAL PART. [" 216. bath* provided with a thermometer, and continue the evaporation at a temperature of 130 to 140 C. until the mass is quite dry and appears no longer sticky, but brittle when touched with a glass rod. Then, after cooling, add concentrated nitric acid (40 to 50 c.c.) and heat on a sand-bath until the iron is again dissolved and only a residue similar in color and appearance to the original insoluble residue remains. This solution of the iron in nitric acid is easily effected, provided the heat used in the preceding drying operation has not exceeded the prescribed limit. The excess of nitric acid, however, which it is usually necessary to use for this purpose, if allowed to remain in the free state, retards the subsequent precipi- tation of phosphoric acid by molybdic acid solution, and may even cause an appreciable error by retaining a portion permanently in solution. Evaporate off, therefore, a part of the nitric acid, reduc- ing the volume to about 25 c.c. If the evaporation proceeds too far, basic ferric salts containing phosphoric acid will remain undis- solved on subsequent addition of water. After proper concentra- tion, add 100 c.c. of cold water, stir, and allow the insoluble residue, which must not show evidence of containing basic ferric salts, to settle. Filter into a tall narrow beaker, or better still into a cone- shaped flask. To the filtrate and washings, which need hardly exceed 200 c.c., add 100 c.c. of molybdic acid solution (prepared as directed in "Qual. Anal.," p. 72). Add next gradually ammonia so long as the reddish-brown precipitate, which it forms, dissolves very readily on stirring. A few cubic centimetres can usually be added at this point, without danger of forming a permanent iron precipitate, on account of the free nitric acid which the added molybdic acid solution contained. Stir well the solution, which should now occupy a volume of 300 to 350 c.c., and let it stand at a temperature of 40 to 50 C. at least 24 hours. The greater part of the solution standing over the precipitated ammonium phos- phomolybdate can be removed perfectly clear by means of a siphon. * A suitable air-bath may be easily constructed as follows : Procure an iron pot having its diameter greatest at the rim (about 12 inches), fit a sheet tin cover to it, cut circular holes (2 or 4) in the cover 10 centimetres in diameter to receive the beaker (which must be selected of a proper size), and also a small hole in the centre for inserting a thermometer. The pot is heated by setting it into a sheet- iron cylinder, made to fit it, down to the rim, and placing a Bunsen burner under it within the cylinder. 216.] PARTIAL ANALYSIS OF IKON ORES. 74:? Collect the precipitate on a small filter (2-J inches in diameter) and wash it with the same molybdic acid solution that is used for precipitation, diluted with an equal volume of water. Allow the filtrate and washings to stand in a warm place several hours to -ascertain whether any more phosphoric acid can be precipitated. The moist precipitate is to be dissolved on the filter with ammonia. It is advisable to have the ammonia used for this purpose in a .small graduated glass cylinder so that the quantity used may be observed. Pour 2 or 3 c.c. into the flask in which the precipita- tion has been effected in order to dissolve what may adhere to it, then pour from the flask upon the filter, and at the same time stir up the precipitate with a jet of hot water. Repeat this operation till complete solution takes place. By cautious use of ammonia solution (sp. gr. -95) its volume should be restricted to about 10 c.c. for small quantities of the precipitated phosphomolybdate, while for comparatively large quantities, such as are obtained from 4 gr. of ore containing upwards of '5 per cent, of phosphoric acid, more may be used. Usually the solution, after passing through the fil- ter remains clear or at most exhibits but a slight opalescence. Occa- sionally it is turbid to such extent that it is advisable to pass it through the same filter again. Wash the solution out of the filter paper with the smallest sufficient volume of hot water. Add now, according to the quantity of the dissolved precipitate, 6 to 12 c.c. of hydrochloric acid (sp. gr. 1-1). If this occasions (by super- saturation of the ammonia) a permanent precipitate of ammonium phosphomolybdate, redissolve it with a slight excess of ammonia, adding enough to give a perceptible odor of ammonia to the solu- tion when 'cold. This addition of a measured volume of hydro- chloric acid is designed to form a moderate quantity of ammonium chloride not enough to have a sensible solvent effect on the ammonium magnesium phosphate which is next to be precipitated, but sufficient to prevent the coprecipitation of other magnesium compounds. Xext precipitate the phosphoric acid with "mag- nesium mixture" (see p. 113). An excess of this solution is required to effect complete precipitation of phosphoric acid ; 8 to 10 c.c. may be used in any case, while more may be required if the ore is rich in phosphoric acid. Finally, to render the separa- tion of ammonium magnesium phosphate complete, add to the solution about one-tenth its volume of ammonia solution, and stir 744 SPECIAL PART. [ 216. well. The preceding operations should be conducted in such a manner as not to unnecessarily increase the volume of the solution. The iinal volume after addition of all reagents may amount to 40 to 60 c.c. in ordinary cases, or to 100 c.c. for ores containing an unusually large quantity of phosphorus. Filter the solution after standing 6 to 12 hours in the cold, wash the precipitate with dilute ammonia, dry, detach from the filter (unless the quantity is very small), incinerate the filter in an open platinum crucible, add the precipitate, ignite, weigh, and calculate the amount of phosphorus (or if required P 2 O f) ) in the ore. In view of the importance of accurate determinations of phos- phorus in iron ores, pig-iron, &c., for technical purposes, some further explanation may here be properly given of the causes of the possible errors which the above directions are intended to- obviate. If, in the beginning of the process, HC1 is not removed by evaporation to dryness, it may prevent complete precipitation of phosphoric acid by the molybdic acid solution/" The presence of a large quantity of free nitric acid also prevents precipitation of the last traces of phosphoric acid by the molybdic solution. If, in attempting to obviate this cause of error by evaporating the nitric acid, the evaporation is carried too far, basic ferric nitrate will be formed, which will retain 1 phosphoric acid. If too great heat is used in precipitating the ammonium phosphomolybdate, free molybdic acid will be deposited along with it. A slight deposition of molybdic acid, provided the precipitate remains pulverulent, may have no sensible injurious effect ; but a larger amount, espe- cially if deposited in the form of a crust, will retain iron which cannot be washed out on the filter. If then ammonia is applied to dissolve the precipitate on the filter, a ferric compound contain- ing phosphoric acid will remain on the filter undissolved. In order to insure the complete precipitation of phosphoric acid, it is necessary to use not only enough molybdic solution to * It is true that after evaporation and drying at a temperature between 130 and 140 C. some chlorine, still remains as ferric chloride, wh ich might be further decreased or entirely removed by evaporating again the nitric acid solution to- dryness. I have repeatedly taken this course and compared the results with those obtained without evaporating a second time ; but do not thereby obtain a larger amount of phosphorus, and conclude that this extra precaution is unnec- essarv. O. D. A. 216.] PARTIAL ANALYSIS OF IRON ORES. 745 convert it into ammonium phosphomolybdate, but a liberal excess proportional to the volume of the solution. It may occasionally hap- pen, in case of an ore or a sample of iron unexpectedly rich in phosphorus, that 100 c.c. will not suffice. But since more inolybdic solution is added in the process of washing the precipitate, the formation of an additional precipitate in the filtrate, which should l)e kept warm f> hours, will indicate any deficiency in the quantity of rnolybdic solution first used. If, in the final precipitation as ammonium magnesium phos- phate, a large amount of free ammonia, and no ammonium chloride, is present when the magnesia mixture is added, it is possible that magnesium oxide or basic magnesium phosphate may be coprecipi- tated ; while, on the other hand, a very large amount of ammonium chloride may retard the precipitation of phosphoric acid. If the precipitation is attempted in too large a volume of solution there is more danger that it may not be complete, and also more diffi- culty in removing the precipitate from the sides of the vessel, to which it may adhere in the form of minute transparent crystals. Finally, notwithstanding the use of all due precaution, the weighed magnesium pyrophosphate may contain a trace of silica so slight that it may in most cases be neglected. But if a very accurate determination of minute quantities of phosphorus in the purer kinds of ore, iron, &c., is required, it is advisable to dissolve the weighed precipitate in the crucible by warming with nitric or hydrochloric acid, collect any remaining residue on a very small filter, wash, return to the crucible, ignite, weigh, and deduct the weight of the crucible + silica from its weight + first ignited pyrophosphate. Sulphur. If any considerable quantity of metallic sulphides is visible on close inspection of the ore, take 5 grm. finely pul- verized. If no sulphides can be seen take 7 to 10 grin. Add to the ore in a large beaker about 20 c. c. of aqua regia for each gramme taken. Allow it to stand at common temperature of the room 6 hours, then 12 hours longer at 40 to 50 C. Finally evaporate to dryness, treat the residue with strong hydrochloric acid, dilute to 200 to 300 c.c., filter, concentrate to about 100 c.c.,, transfer to a small beaker, add while hot a few c.c. of barium chloride solution. If the ore contains much sulphur, the greater part of the sulphuric acid produced from it will be at once precipi- 746 SPECIAL PART. .[ 216. tated ; a quantity far too great to neglect, however, will remain in solution on account of the presence of free acids and ferric salts. If the ore contains a comparatively small though still determinable amount of sulphur, it may happen that no precipitate will appear at this stage. In either case, therefore, remove the free acid by evaporation, after the addition of barium chloride so far as it can be removed without the formation of basic ferric salts insoluble in water. The last part of the evaporation is carried on best by heat- ing the small beaker in an iron plate. The solution may usually be brought thus to a volume of 10 or 15 c.c. The formation of a xlark pellicle on the surface of the liquid at this stage can usually be observed, and is a sure indication that further evaporation would render the iron insoluble in water. After cooling, add cold water (about 100 c.c.) and 1 c.c. dilute HC1 to dissolve the soluble saline matter. If the ore contained sulphur, a residue of barium sulphate will now appear.* (If the preceding evaporation has been carried too far a bulky mass of ferric salts will remain undissolved, in which case add hydrochloric acid freely till it dis- solves, and repeat the evaporation.) The barium sulphate thus obtained usually contains iron and other impurities. Collect it on a filter, wash till the greater part of the saline matter is removed, ignite in an open platinum crucible till carbon is burned away, add a little sodium carbonate, fuse, warm the fused mass with water in the crucible until it becomes disintegrated ; pour the contents upon a small filter, wash the sodium sulphate out of the insoluble part, add IIC1 to the filtrate till it gives, after boiling, an acid reaction with test paper (avoiding much excess of acid), and precipitate w r hile boiling with barium chloride. The barium sul- phate thus obtained, after washing first by decantation 2 or 3 times, and afterwards 011 a filter with boiling water, may be assumed to be sufficiently pure. "Weigh it and calculate percentage of sulphur in the ore. * The nitric and hydrochloric acids used for the examination must always be tested for sulphuric acid as follows: Evaporate 200 c.c. (or the same volume used in analysis) of the mixed acids, with addition of a few centigrammes of pure Na 2 CO 3 till only some half dozen drops remain, dilute, add barium chloride while hot. If a weighable amount of BaSO 4 is formed, weigh it. If the weight of BaSO 4 from the 200 c.c. does not exceed '002 or -003 gr., the acids may be used with the required correction of result. 216.] PARTIAL ANALYSIS OF IKON ORES. 747 MANGANK*K. 1. Method suitable for ores not t/n usually rich in manganese. The most reliable methods of determining manganese in iron ores involve the precipitation of iron as basic ferric acetate. In order to avoid the tedious operation of washing a large quantity of iron precipitated in this form, the whole volume of the solution in which the precipitate is formed may be measured, and after the precipitate has settled a measured portion of the nearly clear supernatant liquid may be taken for the determination of man- ganese. A wide graduated cylinder of thin glass holding 1200 to 1400 c.c. is required for measuring the solution.* Take 4 or 5 grm. ore, decompose with strong hydrochloric acid, evaporate to dryness (with addition of nitric acid if ferrous iron is present), redissolve with strong hydrochloric acid, evaporate off the greater part of the excess of acid used for redissolving, dilute and filter into a flask capable of holding at least 1500 c.c., previously marked at a height corresponding to 1000 c.c. Precipitate now the iron by the successive addition of sodium carbonate, a little hycrochloric acid, acetic acid, sodium acetate, and boiling; according to directions given in 160, 71. The final vol- ume to which the solution is brought before boiling must in this case be limited to about 1000 c.c. After precipitation, pour the contents of the flask immediately without cooling into the gradu- ated vessel, rinse the flask with a small volume of water which must be carefully mixed from top to bottom with the main solu- tion by stirring with a long glass rod. When the precipitate has settled to such an extent that at least half of the solution can be drawn off nearly free from suspended matter, note the volume which it occupies, and siphon off the nearly clear solution. Note the volume remaining. Suppose, having used 5 gr. ore, the whole volume was 1140 c.c., and the remaining volume 420 c.c. The * If a suitable measuring vessel is not at hand, one which will suffice may be prepared in the following manner : Procure a tall narrow beaker (9 10 in. in height, 3 3| in. in diameter). Run 50 c.c. of water into it from a burette; mark the side of the beaker at the surface of the liquid with a writing diamond (or mark with a pencil a vertical strip of paper fastened to the beaker with shellac). Continue adding portions of 50 c.c. and marking till the vessel is filled. After- wards graduate the portion between 1000 c.c. and 1200 c.c., also between 300 c.c. and 500 c.c., into spaces corresponding each to 10 c.c. 748 SPECIAL PART. [ 216. volume drawn off is then 1140 420 = 720 c.c., corresponding to 720 - x 5 gr. ore ; or rather the 720 c.c. corresponds approximately to that amount of ore. For no account is taken of the volume occupied by the solid ferric acetate, nor can very accurate measure- ments be made in wide graduated glass vessels. But these sources of error have no appreciable influence on the final result unless the ore is comparatively rich in manganese (containing over 2 or 3 per cent.). For such ores it is, in fact, preferable to use 1 grm. for the determination, and wash the basic ferric acetate in the ordinary manner. The solution which is drawn off by means of a siphon may con- tain, besides a little suspended iron precipitate, a trace of iron still in solution, calcium and magnesium, and a large amount of saline matter. Concentrate without filtration by evaporation in a beaker, or, more expeditiously. by boiling in a flask to about 300 c.c. ; add sodium carbonate to alkaline reaction, boil and add a little sodium hydroxide. Manganese is thus precipitated along with iron calcium, &c. ; collect the precipitate on a filter, wash slightly and dissolve on the filter with the smallest possible quantity of hydrochloric acid. If the precipitate dissolves with difficulty on account of the presence of higher oxides of manganese, add a few drops of solution of sulphurous acid. Boil the filtrate to expel chlorine, or if sulphurous acid has been used, boil with addition of a few drops of nitric acid. Add sodium carbonate solution till a slight deepening of color, due to presence of ferric chloride, indi- cates that the solution is nearly neutral. (If sufficient iron is not already present to give this indication, two or three drops of ferric chloride solution may be added.) Add next sodium acetate and boil to precipitate the slight quantit}' of iron present, and filter the hot solution. If the preceding operations have been properly con- ducted, the filtrate and washings need rarely exceed 200 c.c. Pre- cipitate the manganese in it by adding aqueous solution of bromine and keeping it warm a few hours. When the excess of bromine has escaped, filter and wash with hot water. Test the filtrate for manganese by adding a little more bromine solution and also more sodium acetate. Ignite the precipitate and weigh as Mn 3 O 4 . The manganese protosesquioxide thus obtained may contain a trace of soda ; but when the quantity does not amount to more than 2 or % 216.] PARTIAL ANALYSIS OF JliOX ORES. 749 per cent, of the ore, it is not probable that greater accuracy would be attained by dissolving it and converting the manganese into another form for weighing. But it should, after weighing, be examined to ascertain whether it contains enough cobalt to cause an appreciable error in the estimation of manganese, since traces of cobalt are frequently present in iron ores, more especially in brown hematites. Dissolve it in hydrochloric acid, evaporate to a few drops. If the bright green color, which even a very small amount of cobalt would occasion, does not appear, it may be assumed that cobalt is not present in sufficient quantity to require any change in the percentage of manganese calculated from the weighed pro- tosesquioxide. But if the color indicates presence of cobalt, con- tinue the evaporation with heat not exceeding 100 C. until free acid is completely removed. Dissolve the residue in about 20 c.c. of water and acidify with not more than one or two drops of acetic- acid, add sodium acetate, heat and pass H 2 S through the solution. Cobalt will then be precipitated as sulpide. If the quantity is sufficient, the cobalt may be determined by converting it into cobalt sulphate (see p. -265); or manganese may be determined in the filtrate from the cobalt sulphide, by precipitating (after boiling out H 2 S) with sodium carbonate, igniting and weighing again as Mn,0, 2. Method suitable for Ores containing larger yminttfit-x <>f Manganese. Weigh out from '75 to 1* gr. and proceed as in the above- described process so far as the precipitation of iron as basic ferric acetate. Filter, wash the precipitate (best collected on two filters) with hot water containing 1 or 2 per cent, of sodium acetate. Boil the filtrate and washings, and filter again if any additional flocks of basic ferric acetate separate. Concentrate the filtrate to 600 800 c.c,, transfer about one-half of the solution into another beaker, nearly or quite neutralize the acetic acid which it contains with sodium carbonate, add to it the remainder of the solution which still contains free acid, and should dissolve any slight precipitate caused by sodium carbonate. Precipitate next manganese with hromine and treat the precipitate as above directed in 1, not omit- ting examination for cobalt ; or, if great accuracy is desired, the manganese may be converted into pyrophosphate for weighing. 750 SPECIAL PART. [ TITANIC ACID. Qualitative examination. Fuse about 1 grm. of \hQJvtiely pul- verized ore with potassium disulphate in the manner described below under " Quantitative determination." Treat the fused mass with boiling dilute hydrochloric acid, which readily dissolves the iron and titanic acid. Boil the solution, without filtering from the insoluble residue which usually remains, in a porcelain casserole with granulated tin. If the violet color indicating titanium does not sooner appear, concentrate by rapid boiling, with addition of more tin in case the first portion has dissolved, until saline matter begins to be deposited and but some half-dozen c. c. of liquid remain. If no decided violet color now appears it may be con- cluded that either no titanium or but very little is present. The only certain way to detect minute quantities is to proceed as in quantitative determinations, which indeed requires but little more time if the method of decomposing the ore with hydrofluoric acid is employed. Quantitative determination. Fuse 1 grm. of the very finely pulverized ore with potassium disulphate. The potassium disul- pliate has but little effect on the ore until the temperature approaches dull redness. If it contains too much sulphuric acid it will froth and occasion mechanical loss before the proper tem- perature is reached. If prepared strictly according to directions in g 64, 7, p. 115, this trouble will be obviated. After the bottom of the crucible is faint red, apply no more heat than is just sufficient to maintain the mass in a state of fusion. The temperature must be gradually increased, since the sulphate becomes more and more infusible as fumes of sulphuric acid escape with formation of nor- mal sulphate. When the mass is no longer fluid at a full red heat, allow it to cool ; add concentrated sulphuric acid (2 or 3 c. c.), heat very gradually until, aided by stirring with a platinum wire, the fused mass becomes disintegrated and mixed with the acid. The temperature may then be gradually increased as before. The progress of the decomposition may be ascertained by dip- ping a thick cold platinum wire or spatula to the bottom of the crucible, allowing it to cool and repeating the dipping a few times. By inspection of the sample thus taken up with a lens one can see whether undecomposed particles of magnetite are present. One addition of fresh sulphuric acid often suffices, but the addition of 216.] PARTIAL ANALYSIS OF IRON ORES. 751 acid and reheating may be repeated as often as required. It is advisable at the end of the operation, after the decomposition appears complete, to incorporate a liberal amount of sulphuric acid uniformly with the mass, and allow the greater part to remain in order to facilitate subsequent solution of the mass in water. After cooling, digest with 300 c. c. of cold water until all soluble matter (ferric sulphate, titanic acid) is taken up. This often requires a long time, usually 24 to 48 hours. If the ore contains quartz or silicates an insoluble residue is sure to remain, possibly retaining a small quantity of titanic acid. Collect it on a filter, incinerate the filter, and fuse the residue with a small quantity of potassium disulphate, and at the end of the operation add> after the mass has sufficiently cooled, concentrated sulphuric acid enough to retain the potassium salt and the titanic acid permanently in solution. Heat till the whole is liquid with exception of the undecomposable parts of the ore, cool, and put the crucible with its still liquid con- tents into a small beaker containing just sufficient water to cover it. If titanic is present it will now readily go into solution. The filtered solution can be treated for titanic separately like the main solution, or it may be added to the main solution. To separate titanic acid from the first solution, or from the two mixed solu- tions, add first sodium carbonate so long as it can be added without producing a permanent precipitate, then 3 c. c. of pure dilute sul- phuric acid and 100 to 150 c. c. strong solution of sulphurous acid ; expose to heat of 40 to 50 C. an hour. If the solution continues to smell of sulphurous acid enough of that reagent has been added, otherwise more should be added. Dilute to TOO to 800 c. c. in a large beaker and boil steadily 2 hours, covered with a watch-glass* A moderate quantity of free acid must be present to prevent iron from being precipitated. The iron must aiso be in the state of ferrous sulphate. Too much free acid prevents precipitation of titanic acid. When a considerable amount of titanic acid is present the formation of a precipitate on heating the solution, a little before the actual boiling begins, is an indication that the free acid present does not exceed the proper amount. - To compensate for the water lost by evaporation during the boiling, add from time to time hot water so gradually as not to check the boiling. A little solution of sulphurous acid should be mixed with the water thus, added to keep the iron in the state of ferrous sulphate. 752 SPECIAL PART. [216. Allow the precipitated titanic acid to settle till the solution above it is perfectly clear (12 to 24 hours). Filter (not with a Bunsen pump) through a filter carefully fitted to the funnel and stir the precipitate as little as possible during the washing, as it is somewhat inclined to pass through the pores of the filter paper ; if necessary, ammonium sulphate may be added to the water used for washing to prevent this tendency, Ignite the precipitate strongly, let the crucible partially cool, throw p a small lump of clean ammonium carbonate, and heat rapidly again to bright redness in order to remove traces of sulphuric acid. The weighed titanic acid, notwithstanding all precautions, is likely to contain a little ferric oxide. Fuse it with sodium carbonate, add gradually to the cold fused mass in the crucible 5 or 6 c. c. strong sulphuric acid, heat till evolution of CO 2 has ceased and the mass has dissolved. Add then more strong sulphuric acid (6 10 c. c.) and dilute with about 100 c. c. of water. Determine the iron in this solution by titration with potassium permanganate, with previous reduction by H 2 S according to 113, 3. (Zinc cannot in this case be employed for the reduction since it reduces also titanic acid.) Calculate the iron found as ferric oxide and subtract it from the impure titanic- acid weighed. If the t analyst has at hand hydrofluoric acid and a platinum dish capable of holding 100 to 200 c. c., the following method of decomposing the ore may be substituted, with great saving of time, for the fusion with disulphate. Heat the ore nearly to boiling in the platinum dish with a mixture of hydrofluoric and strong hydro- chloric acids. Magnetic iron ores, in which it is oftenest required to determine titanic acid, are thus usually decomposed in a few minutes. Add 20 to 25 c. c. concentrated sulphuric acid diluted with half its volume of water, and concentrate by means of a care- fully adjusted flame till fumes of sulphuric acid begin to escape. It is of utmost importance to remove every trace of hydrofluoric acid. The appearance of fumes of sulphuric acid can be considered as proof that this has been effected only when means are employed to protect the sides of the dish above the liquid from heat sufficient to volatilize sulphuric acid, since the mixed acids are attracted upward along the surface of the platinum. After cooling add nearly 100 c. c. of water. Either at once or in a few hours the whole dis- solves, with exception perhaps of a slight residue, which may, if it 217.] COMPLETE ANALYSIS OF IRON ORES. 753 appears too considerable to be neglected, be subjected again to the same treatment.* The solution of the ore obtained in this way is neutralized with sodium carbonate and further treated in the same manner as a solution obtained by decomposing with potassium disulphate.] [IT. COMPLETE ANALYSIS OF IKON OKES. 217. (Process adapted to all iron ores except such as contain a large amount of titanic acid.) 1. Silica, iron, aluminium, manganese, calcium, magnesium. Take about 1 grm. ore. Add concentrated hydrochloric acid and heat in a water bath or sand bath nearly to boiling one or two hours. Evaporate finally to dryness and expose the residue to a heat slightly exceeding 100 C. in order to render insoluble any silica which may have been dissolved. A porcelain dish may be used in this operation, but a beaker of 200 to 300 c.c. capacity is more convenient, especially if a suitable air bath is at hand for raising the temperature at the end to 120 to 130 C. Add two or three c.c. concentrated hydrochloric acid to the residue and warm till the iron is redissolved, and filter at oncef after suitable dilution, carefully removing every particle of the residue to the filter; wash and reserve the filtrate ; ignite the filter and its contents till carbon is burned away ; add then to the residue 5 or 6 times its weight of pure sodium carbonate and fuse ; disintegrate the fused mass by heating with water, acidify with hydrochloric acid, and separate silica by evaporation and drying in the usual manner. The filtrate from the silica is now added to the other reserved solution of basic metals. Another method of decomposing the ore and separating silica is to fuse directly with sodium carbonate, without previous treat- * If the ore contains much calcium, a residue of calcium sulphate insoluble in the limited amount of water above recommended must be expected. f By prolonged digestion of this residue with hydrochloric acid, traces of silica might be taken up from certain silicates which being very slowly acted on by acid may have escaped complete decomposition by -the first treatment with acid. 754 SPECIAL PART. [217. ment with hydrochloric acid, and separate silica from the fused mass in the ordinary manner. More time, however, is required to disintegrate the mass and separate the silica, more saline matter is introduced into the solution, and the platinum crucible used for the fusion is likely to become permeated with iron to such an extent that for a long time it is unsuitable for most other uses. These disadvantages overbalance the apparent greater simplicity of this mode of proceeding. From the solution of basic metals precipitate first, the iron as basic ferric acetate according to direction given in 160, 71, p. 517. The iron may be precipitated without concentration of the two mixed filtrates if care has been taken to avoid too large a vol- ume and the presence of an unnecessary amount of free acid r otherwise the solution should be concentrated until the greater part of the free acid is removed. It is usually best to collect the precipitated ferric acetate on two filters. Wash at first with boiling hot water containing 1 or 2 per cent, of sodium acetate until a few drops of the washings give but a slight turbidity when tested with silver nitrate. Reserve the filtrate and washings which contain manganese, calcium and magnesium, and continue without interruption to wash the precipitate with hot water to which a little ammonium acetate has been added until a drop of the washings leaves no residue on evaporation on platinum foil. The last washings containing ammonium acetate are thrown away. Dry the precipitate, which contains besides iron the aluminium and phosphoric acid of the ore, detach from the filters, incinerate the latter with prolonged exposure to the air at a full red heat in order to convert into ferric oxide the lower oxides of iron formed by reducing action of the filter paper. Add the precipitate and moisten it in the crucible with concentrated nitric acid, dry with gentle heat, repeat the moistening with nitric acid and drying, ignite and weigh. The weighed precipitate should exhibit no magnetic attraction when a magnet is applied externally to the bottom of the crucible.* Dissolve the weighed Fe a O 3 ,Al 2 O 3 and P 2 O 6 in strong hydro- * If the treatment with nitric acid is omitted, lower oxides of iron are usually formed by ignition of basic ferric acetate which are converted into ferric oxide with great difficulty by prolonged ignition. Even treatment with nitric acid lias but little oxidizing effect after the precipitate has once been ignited. 217.] COMPLETE ANALYSIS OF IRON ORES. 755 chloric acid, add 10 to 15 c.c. of pure dilute sulphuric acid, remove all the hydrochloric acid by evaporation, and dilute moderately with water. Occasionally, but not often, a residue of silica may be observed at this point, so considerable in quantity as to render it advisable to collect it in a small filter and deduct its weight from the precipitate which contained it and add it to that of the main portion of silica, It is necessary now, in order to estimate satisfac- torily the comparatively small amount of aluminium usually present, to determine very accurately the iron. Titration with potassium permanganate in the sulphuric acid solution is the best of all volumetric methods; previous reduction with hydrogen sulphide according to directions on p. 729 is to be recommended as a method of reduction involving least sources of error. The A1 2 O 3 is calculated by deducting Fe 2 O 3 found, and also P 3 O 5 * (determined in another portion of the ore) from the joint weight of the three substances. Concentrate the filtrate from the basic ferric acetate to about 600 c.c. and precipitate manganese with bromine water after partial neutralization of the free acetic acid as directed on p. 749 (second method of determining manganese). Neutralize the filtrate from the manganese dioxide with ammonia and precipitate calcium with ammonium oxalate. In the filtrate from calcium oxalate precipitate (without concentration unless the volume exceeds 600 c.c.) the magnesium with sodium phosphate adding a liberal quantity of ammonia and allowing 24 hours for complete separation of the ammonium magnesium phosphate. 2. Alkalies. Small quantities of potash or soda are sometimes found in magnetic iron ores owing to the presence of felspars. More rarely an appreciable amount of potash may be found in brown *If the amount of P 2 O 5 is very small, not exceeding say O'l per cent, the precipitate produced by boiling with sodium acetate, instead of being treated as here recommended, may be washed sufficiently to free it from appreciable quantities of manganese and alkali-earth metals, dissolved in hydrochloric acid and reprecipitated with ammonia. The ferric and aluminium hydroxides thus precipitated are easily washed free from saline matter, ignited and weighed. The phosphoric acid, however, is liable to be but partially precipitated by ammonia along with the iron, so that an error (not exceeding the amount of PS O 5 ) will result in calculating the A1 2 O 3 by difference. 756 SPECIAL PART. [ 217. hematite on account of intermixed micaceous minerals. For qualitative or quantitative examination use the method of J. L. SMITH. See p. 426. 3. Ferrous and Ferric Oxides. Decompose *5 grin, by boiling in a large covered platinum cruci- ble with a mixture of sulphuric and hydrofluoric acids, dilute and determine ferrous iron by titration with potassium permanganate. (See p. 529). The amount of ferric oxide can of course then be calculated, fhe total iron having being previously determined. 4. Carbonic Acid. Determine carbonic acid in 1 to 5 grm. according to the amount present by decomposing with hydrochloric acid and weighing the evolved CO 3 by the process described on p. 413. Or determine carbonic acid and water at the same time by igniting in a com- bustion tube with lead chromate and potassium chromate. (See Analysis of Silicates and Siliceous Rocks, 208, p. 716). The latter method, however, cannot be used when the ore contains carbonaceous matter. 5. Water. When carbonic acid and ferrous oxide are absent, water is determined by loss on ignition. Water should be determined in the same pulverized sample, kept carefully corked in a tube, which has been used for the determination of the chief constit- uents. If the sample has not been previously dried at 100 C., hygroscopic and combined water may be determined separately (if desired) by drying a weighed portion (about 1 grm.) at 100 C. to constant weight in a platinum crucible and afterwards igniting. In the presence of carbonic acid or ferrous oxide determine water by igniting 1 or 2 grm. in a platinum boat in a combustion tube and collecting the water in a calcium chloride tube, a slow current of dried air being meanwhile drawn through the apparatus by an aspirator. Or the water and at the same time carbonic acid may be determined as suggested above (under 4. Carbonic Acid). 6. Presence of carbonaceous or bituminous matter interferes with determination of water by either of the above methods, and also requires a modification of the processes used for determining some of the other constituents. Sulphur should be determined in 217.] COMPLETE ANALYSIS OF IKOX ORES. 757 the ore without previous ignition, as directed in 216 ; carbonic acid by decomposition with hydrochloric acid, and weighing the evolved CO 2 , as described p. 413. In determining phosphorous according to 216, ignite the portion weighed out in an open crucible till carbon is burned out before dissolving it. Treat also in the same manner the weighed portion in which silica and the other chief constituents are to be determined. For the estimation of ferrous &nd ferric oxides decompose *5 gr. with a mixture of hydrochloric and hydrofluoric acids, proceeding as in 3. Since presence of organic matter may interfere with the volumetric determination of either ferrous or ferric iron, separate ferric iron by barium carbonate with exclusion of air, according to 160, p. 513. Determine the amount of ferric iron thus precipi- tated by dissolving in sulphuric acid, reduction to ferrous sulphate, and titration with potassium permanganate. From the results of these several operations the composition of the ore in its original state can now be calculated, with the excep- tion of water and carbonaceous matter. 7. Titanic acid. It is rarely or never necessary to make complete analyses of iron ores containing over 5 or 6 per cent, of titanic acid, since such ores are usually rejected as unsuitable for smelting. When ores con- taining this amount or less are subjected to the above-described process of analysis, a portion of the titanic acid follows the silica and is weighed along with it. The remainder is precipitated with the basic ferric acetate and is weighed with ferric oxide. A method of separating the titanic acid from these two products is described in 208 (Analysis of Silicates and Siliceous Rocks), p. 717. In washing silica which contains titanic acid, the latter sometimes passes through the pores of the paper, making the filtrate turbid. This, however, will occasion no error if the filter retains the silica. 8. Phosphoric acid must be determined in a separate portion of the ore as in 216. 9. Sulphur must also be determined in a separate portion as in 216. 758 SPECIAL PART. [ 218. [18. ANALYSIS OF PIG-IKON, STEEL, AND WROUGHT IRON. 218. I. PIG-IRON. Preparation of the sample. The chemist usually receives for analysis a short section broken from a pig. If the iron is hard and brittle (white pig or spiegel), procure, by breaking on an anvil with a heavy hammer, some frag- ments free from the outer surface, to which sand or other impuri- ties may adhere. Pulverize these fragments to a coarse powder in a mortar of the hardest steel. If the sample is too tough to be crushed, it must be reduced to a suitable condition by drilling.* To obtain the necessary quantity (40 to 50 grm.) bore one or more holes in the clean broken end of the sample, at a distance half way between the centre and outside. Use no oil or water in the process, and cleanse the drill from oil before beginning. The borings may be taken up from time to time during the operation with a magnet and transferred to a bottle provided with a glass stopper. 1. Determination of the total amount of carbon. Method of BEKZELIUS (somewhat modified). The determination of carbon by the method here recommended requires the use of a special reagent, viz., a strong solution of cupric ammonium chloride containing no free acid. This solution may be prepared as follows : Dissolve common blue vitriol (crys- tallized cupric sulphate) in 10 to 15 times its weight of water, filter the solution, and heat to boiling in a copper kettle. Add solution of common sal soda gradually to alkaline reaction, keeping up meanwhile the boiling. Basic cupric carbonate (not entirely free from basic sulphate) is precipitated in a dense form easy to wash by decantation. Wash it by decantation until the sodium sul- phate is nearly all removed. Transfer to a glass or porcelain vessel. Reserve about one tenth, and dissolve the remainder in concentrated hydrochloric acid ; add the reserved portion which is * It is best if possible to employ the assistance of a machinist who can use a drill press run by steam. 21."- FKr-iRox, STP:KL. AXD WROUGHT IRON. 759 designed to neutralize the acid completely. Let the solution stand <3old several hours with occasional agitation. A portion of the basic carbonate should remain permanently undissolved. Filter, and add, for five parts blue vitriol used, two parts ammonium chloride previously dissolved in a small volume of hot water and filtered. Care should be taken to conduct the above operations so that the final solution obtained may not be too dilute. If its volume does not exceed twice the volume of the concentrated hydrochloric acid used in dissolving the carbonate, it is satisfactory in respect to strength. The Process. Pour at once, not gradually, at least 200 c.c. of the cupric ammonium, chloride solution upon the iron borings (3 or -i grm. may be taken) in a large beaker. The beaker should be set in a vessel of cold water, and the contents should be frequently stirred during the first 15 or 20 minutes to prevent too great ele- vation of temperature by the chemical action ; otherwise a slight evolution of hydrogen might take place, carrying off with it some hydrocarbon compound. (Evolution of hydrogen and loss of car- bon is sure to result if the cupric ammonium chloride contains free acid.) Afterwards the beaker is allowed to remain at the common temperature of the room. The iron dissolves as ferrous chloride with deposition of metallic copper, which, in presence of excess of cupric chloride, is converted into cuprous chloride. The latter is soluble in the cupric ammonium chloride. After the metallic iron has all dissolved, leaving a residue which crumbles under pressure (6 to 12 hours may be required according to fineness of the borings), add a few c.c. of hydrochloric acid to dissolve ferric compounds which may be deposited by the action of the air on the ferrous chloride in solution. If, after standing several hours longer, an accu- mulation of metallic copper or cuprous chloride is observed remain- ing persistently undissolved, more of the double chloride may be added. The complete solution of iron and copper is generally effected in 48 hours, and often much sooner. When nothing remains undissolved except a black carbonaceous residue, filter through an asbestos filter prepared by packing well-disintegrated asbestos, neither too closely nor too loosely,* in a tube 8 or 9 inches * Let the first 2 cm. of the filtering tube at the very bottom have a diameter of 4 cm. and the next 2 cm., above a diameter of about 1 cm. Leave the lower 2 cm. empty and fill with asbestos to a point a little above where the tube has its full diameter. After filling, pour water into the tube; if it runs through in a continuous stream, the packing is too loose, but it should drop rapidly. 700 SPECIAL PAKT. long and f of an inch in diameter, narrowed at one end. Wash the carbon residue until the copper solution is completely removed. It is not safe to apply an exhausting apparatus to hasten the filtration with a filter prepared in this manner.* Dilute the filtrate with dis- tilled (or perfectly clear) water, and observe whether particles of the- carbon residue have passed through. Dry the residue in the tube at 100, and determine the amount of carbon in it by combustion with lead chromate mixed with potassium dichromate according to ITT. Remove, for this purpose, the carbon residue together with the asbestos from the tube with the aid of a steel wire slightly curved at the end, introducing it through the narrow end of the tube, loosening and pushing the w^hole mass out into a small porce- lain mortar already containing some of the chromates. Rinse out the tube with the remainder of that portion of the chromates which is to be mixed with the substance, and mix with a pestle in the mortar till the asbestos is broken up to such an extent that the mixture can be introduced into the combustion tube through a funnel. 2. Determination of the graphite. Treat 4 grm. with moderately concentrated hydrochloric acid, at a gentle heat, until no more gas is evolved; filter the solution through an asbestos filter prepared as in 1 ; wash the undissolved- residue, first with boiling water, then with solution of potassa, after this with alcohol, and lastly with ether ; then dry, and burn after ITT. Deduct the graphite obtained here from the total amount of carbon found in 1 ; the difference gives the combined carbon. 3. Determination of Sulphur. The general plan adopted in all good methods of determining sulphur in iron is to dissolve the metal as completely as is prac- ticable in hydrochloric acid, whereby the greater part of the sul- phur, being converted into hydrogen sulphide, passes off along with a large volume of hydrogen which is conducted through some- liquid capable of absorbing the II 8 S. For this purpose bromine dissolved in hydrochloric acid, potassium permanganate solution,. * J. CREAGH SMITH has devised, and described in the America! Chemical Journal, vol. i.. p. 368, an asbestos filter for filtering carbon residues, which is simple in construction, and can be used with the BUNSEN pump. 218.] PIG-IKON, STEEL, AND WROUGHT IRON. 761 alkaline lead solution, ammoniacal cadmium solution, ammoniacal silver solution have all been employed, some suitable method in each case being devised for bringing the absorbed sulphur into a weighable form. Only the method in which an ammoniacal silver is used will here be described in detail. . A flask of 300 to 350 c.c. capacity is provided with a doubly perforated rubber stopper. Through one hole passes a funnel tube for the introduction of acid. The end of this tube, which should reach nearly to the bottom of the flask, is drawn out narrower and bent upward with a short curve to prevent gas bubbles from entering it and escaping. For absorbing the hydro- gen sulphide from the evolved gas a pair of connected U-tubes are used like those in fig. 64, p. 435. The absorbing tubes are con- nected with the flask by a strong (not too narrow) tube about & inches long, bent downward, and contracted if necessary, at each end, so as to fit into the perforation in the stopper. Treat the rubber stoppers used in making connection with warm soda solution, and carefully rub the loosened sulphur from the surface, not neglecting the perforations, till a clean black surface is obtained. The process. Dissolve a gramme or more of silver nitrate in 15 to 20 c.c. of ammonia solution. Pour at least 10 c.c. of this solution into the first U-tube and the remainder into the second. A little water may be added if the size and form of the U-tubes require it, in order to secure proper contact with the gas bubbles which are to pass through them. Introduce 10 grm. of the iron and 40 50 c.c. water into the flask. Adjust the funnel tube so that the lower end may be under the surface of the water. Connect the several parts of the apparatus, and add concentrated hydro- chloric acid in small portions at a time so as to produce as nearly as practicable a constant evolution of gas. The addition of acid may be regulated according to the appearance of the econd IT-tnbe. The first tube should absorb the hydrogen sulphide. If a blacken- ing of the solution in the second tube begins to appear, add the hydrochloric acid more gradually. When (usually after 4 or 5 hours) the addition of more hydrochloric acid fails to increase the very slow evolution of gas, heat the flask gently, but not to boiling, 20 or 30 minutes, with addition of more hydrochloric acid, taking care not to distil over enough acid to neutralize the ammonia in the first F-tube. Collect the precipitate formed in the first tube 762 SPECIAL PART. [ 218. on a small filter, wash slightly, and dry at 100 C. Dry also the U-tnbe, to which a portion of the precipitate invariably adheres. The second tube will not contain an appreciable quantity of silver sulphide unless too rapid a current of gas has been unintentionally produced. Place the dry filter and its contents in a small dry beaker. Dissolve or loosen the sulphide of silver from the U-tube by shaking with successive portions of aqua regia and pouring into a small beaker, using in all about 20 c.c. Then put into the beaker the dried silver sulphide with the filter. The insoluble residue in the flask, consisting chiefly of graphite and silica, often contains sulphur, and should never be neglected in the analysis of pig-irons. Collect it on a filter and wash out the free acid, dry on the filter thoroughly at 100, detach from the filter carefully, rub the mass to a powder in a beaker with a glass rod, and add aqua regia. Allow the aqua regia to act on the two products at the common temperature 6 hours, and afterwards 12 to 24 hours, at 40 to 54 C. Then concentrate to one third the first volume, dilute, and filter each through separate filters and unite the filtrates. After concentrating to about 50 c.c. add barium chloride, and continue the concentration not quite to dryness, but till only liquid enough remains to moisten the residue. Add a small volume of water and 5 or 6 drops of hydrochloric acid. Treat the residue of impure barium sulphate thus obtained as in the determination of sulphur in iron ores (p. 746). The aqua regia used for oxidizing the silver sulphide and the insoluble residue must be tested for sulphuric acid as directed in " Analysis of Iron Ores," p. 746. The process of dissolving the iron in the flask should be carried on without interruption. This method gives results agreeing with remarkable closeness when repeated determinations are made in the same sample. The substitution of a hydrochloric acid solution of bromine for the solution of silver nitrate in ammonia requires no essential change in the details of the process. The apparatus, however, must be modified so as to avoid much contact of rubber stoppers with the bromine vapor. The bromine solution at the close of the operation contains the sulphur which has been evolved at H a S already in the form of sulphuric acid, which can be determined simply by precipitation with barium chloride after evaporating off the hydrochloric acid to the proper extent. But since the insoluble 218.] PIG-IRON, STEEL, AND WROUGHT IROX. 763 residue, when accurate results are desired,* must be treated for sulphur, as before described, there is little saving of time or trouble by this shorter method of determining the sulphur which passes into the U-tube. 4. Determination of Phosphorus. If the iron is known to contain over 0*5 per cent, of phosphorus 2 grm. will suffice. If less is present 4 grm. may be taken for the determination. Dissolve with a mixture of equal parts of concentrated nitric and hydrochloric acids, using about 30 c.c. per gramme of iron taken, and pouring the whole quantity upon the iron at once.f Proceed further in all details precisely as directed for deter- mination of phosphorus in iron ores. 5. Determination of Silicon. The residue from the solution used for determining phosphorus may be used for determining silicon. Ignite it without separation from the filter until the graphite is partially burned away. Fuse with sodium carbonate mixed with a little potassium nitrate, suffi- cient to effect complete combustion of the carbon still present. Treat the fused mass first with boiling water, in which it readily dissolves, except some silica in light flocculent form, and traces of metallic oxides. Acidify with hydrochloric acid, or nitric acid in case the solution is to be in contact with platinum, and separate silica as usual. When the quantity of silica is not over 1 per cent., these operations may be most conveniently performed in a large platinum crucible without transferring the substance to any other vessel. 6. Determination of Manganese. Dissolve 3 grm. in aqua regia, evaporate to dryness to separate * I have frequently determined separately the sulphur remaining in the insoluble residue obtained by treating pig-iron as described in this process, and seldom find it to be free from a weighable quantity of sulphur; in spme cases amounting even to one third of the total amount found. O. D. A. f If the mixture of acids is gradually added to the iron, especially if a larger proportion of hydrochloric is used, a possible escape of phosphoretted hydrogen may be apprehended. 764 SPECIAL PART. [ 218, silica, redissolve with hydrochloric acid, filter, and determine man- ganese in the solution as in iron ores. Method 1, p. 747. In spiegel-iron the manganese may be more accurately deter- mined by dissolving *5 grm., evaporating to dryness, redissolving with hydrochloric acid, and proceeding with the solution as in Method 2 for iron ores (p. 749). 7. Determination of Copper. If a determination of the minute quantity of capper sometimes present in pig-iron is required, it may be done in the same portion used for sulphur. Dilute the filtrate from the first insoluble residue and pass hydrogen sulphide through it nearly an hour. More or less sulphur separates. Allow it several hours to settle. If the deposit is darker in color than pure sulphur, presence of copper is indicated. In that case collect it on a filter and wash with a dilute solution of hydrogen sulphide. Copper is also often found in the insoluble residue. When this residue is treated with aqua regia to extract the sulphur possibly retained by it, the copper is dissolved and goes finally into the filtrate from the impure barium sulphate first obtained. Pass H 2 S through this filtrate and filter off any precipitate which may result. Incinerate the two filters containing the copper precipitates in a porcelain crucible. Treat the residue in the crucible with aqua regia, add finally a few drops of sulphuric acid, remove the other acids by evaporation, take up the cupric sulphate in a small volume of water, filter and precipitate the copper again with H 3 S, and weigh it as cuprous sulphide. 8. Presence of Other Mements in Pig-Iron. Besides the above-mentioned elements, sodium, potassium, lithium, calcium, magnesium, aluminium, chromium, titanium, zinc, cobalt, nickel, tin, arsenic, antimony, vanadium, and, accord- ing to some authorities, nitrogen, may occur in minute quantities in pig-iron. Their determination, however, is rarely undertaken ; partly because it is not known whether they have any influence, good or bad, on the quality of the iron when present in such minute proportions, and partly because it is very difficult to determine them accurately on account of lack of sufficiently pure reagents, the action of solutions on the vessels used in the process, &c. 219.] ANALYSIS OF ^COAL AND PEAT. 765 II. STEEL AND WROUGHT IKON. Determine carbon, silicon, sulphur, phosphorus, and manganese as in pig-iron, with the following modifications only of the pro- cesses used for carbon, silicon, and sulphur. Silicon is best determined in a separate portion, since the quan- tity used for phosphorus does not afford enough silica to weigh accurately ; 10 grm. will suffice. Place the weighed quantity in a platinum (or porcelain) dish, add first 30 to 40 c. c. water ; next, gradually, concentrated hydrochloric acid until with aid of heat the metal is dissolved, leaving a residue of more or less carbona- ceous matter. Evaporate to dry ness, expose to a temperature of 120 to 150 C. in an air-bath, redissolve the iron by adding first concentrated hydrochloric acid, and next water. Filter through a small filter, incinerate the filter and burn the carbon out of the residue, fuse with sodium carbonate, disintegrate the fused mass with water, acidify with hydrochloric acid, and separate silica by evaporating in the crucible. The now pure silica is collected in a very small filter, washed and weighed in the usual manner. In the analysis of Bessemer steel, or any steel or iron which lias been melted, it may be assumed that the silica thus obtained is formed by oxidation, in the process of analysis, of silicon existing in the metal. In the analysis of ordinary wrought iron the silica obtained may come partly from silicon and partly from mechani- cally mixed particles of slag in which it existed as silica. Carbon. Use for determination 6 to 10 grm. of steel or 10 grm. of wrought iron. Sulphur. Treat the comparatively small quantity of insoluble residue collected on a small filter, washed and dried, directly with aqua regia without removing from the filter.] 19. ANALYSIS OF COAL AJSD PEAT. 219. For technical purposes, estimations of moisture, ash, coke, and volatile matters usually suffice. Determination of sulphur is less frequently required, and ultimate analysis is only resorted to in special cases. 766 SPECIAL PABT. [ 219. a. Moisture. The finely pulverized coal (3 5 grm.) is heated to 110 115 for an hour or more or until it ceases to lose weight (see 29). Many bituminous coals gain weight after a time from oxidation of sulphides or hydrocarbons (WHITNEY). According to HINKICHS,* drying the coal for one hour effects the maximum loss. I. Coke and volatile matters. The dried coal of a is sharply heated in a closed platinum, or, in presence of sulphides, in a porcelain crucible as long as combustible matters issue from it. It is then cooled quickly. The loss is set down as volatile matters. The residue, less the ash, is. coke. G. Ash. The residue of 5 is incinerated in a crucible placed aslant. d. Carbon and hydrogen are determined by combustion with chromate of lead and bichromate of potash, 177. e. Sulphur is best determined according to 186, 0, 2, a, p. 658. The method thus described gives the amount of ash as well as sulphur. Or the following simple method recommended by EscHKAf may be employed. About 1 grm. of the finely -pulverized substance is intimately mixed by stirring with a platinum wire with 1 grm. burned magnesia (MgO) and '5 grm. dry sodium carbonate in a platinum crucible. The uncovered crucible is then heated in an inclined position with an alcohol lamp so that only the lower half becomes red hot. In order to facilitate combustion, which requires, according to the nature of the substance, to 1 hour, the mixture is frequently stirred with a platinum wire. After the carbon is con- sumed and the color of the mass has changed to brownish or yellowish, \ to 1 grm. of pulverized anhydrous ammonium nitrate is added and intimately mixed with the contents of the crucible. The mixture is then ignited again, in the covered crucible, from 5 to 10 minutes. Any sulphites which may have been formed at first are hereby converted into sulphates. The mixture, which retains its pulverulent form, is next transferred to a beaker and warmed with 150 c. c. of water. The solution is filtered and acidi- fied with hydrochloric acid. Sulphuric acid is then precipitated with barium chloride. Chemical News, 19, 282. f Zeitschr. f. anal. Chem. 13, 344. 220.] ANALYSIS OF COMMERCIAL FERTILIZERS. 767 All the sulphur, whether existing in the form of calcium sul- phate or pyrites, in the coal is obtained by this method. The sulphur of calcium sulphate in coal may be separately determined by boiling 24 hours the finely powdered coal with an equal weight of sodium carbonate dissolved in water, filtering, acidifying with hydrochloric acid, and precipitating with barium chloride. The calcium sulphate is decomposed by the sodium carbonate, while sulphides of iron are not attacked. [20. ANALYSIS OF COMMERCIAL FERTILIZERS. 220. 1. Preparation of the sample. Mix the sample uniformly and, if need be, take a portion of 20 50 grms. which shall accurately represent the whole, for further pulverization. Bone, dried blood, guano, &c., should be ground or pounded fine enough to pas* through sieve meshes of -^ in. diameter. Superphosphates should be merely rubbed in a mortar to crush lumps and secure uniformity. Grinding of superphosphates may occasion a further action of the acid on the undissolved phosphate and increase the per cent, of soluble phosphoric acid. If the substance is very moist and coarse dry 20 to 50 grms. at 100, with addition of a weighed amount of oxalic acid if ammonia is likely to escape, till it can be easily handled, grind fine and weigh. Make nitrogen determinations in this portion and reckon the results back to the original material. ANALYSIS OF SUPERPHOSPHATE. 2. Soluble Phosphoric Acid. Bring 20 giro, into a litre flask with about 800 c. c. of water and shake frequently (every 10 min- utes) for 2 hours : then make up to volume of 1 litre ; mix thoroughly, pour on dry filter and measure off 100 c. c. = 2 grm. substance. 3. The determination of phosphoric acid in the solution thus obtained may be made most accurately by the molybdic method. (See p. 375). 4. A simpler, more rapid and for most purposes sufficiently 768 SPECIAL PART. [ 220. accurate process is the following " citric method," first published in its present form by PETERMANN, but worked out independently in the Connecticut Agricultural Experiment Station, as follows : To the solution add 55 c. c. solution of ammonium citrate,* (equivalent to 10 grin, of crystallized citric acid), 40 c. c. of mag- nesia mixturef in all cases use about four times as much as would be required to combine with the phosphoric acid and then add to the solution 75 c. c. of water and 90 c. c. of ammonia solu- tion of sp. gr. 0-96. The precipitate should be distinctly crystal- line ; a flocculent precipitate indicates that insufficient ammonium citrate has been added. Stir vigorously and repeatedly and after 12 hours filter, wash with dilute ammonia, ignite and weigh. The use of GOOCH'S as- bestus filter greatly facilitates the work. 5. Reverted Phosphoric Acid. Place 2 grm. of substance in a mortar. Take 100 c. c. of neutral or slight alkaline ammonium citrate solution, sp. gr. 1.09, (the commercial citrate is strongly acid), pour 50 c. c. on the substance, add dilute ammonia to slight alkaline reaction, pulverize the substance, let the coarser parts settle, pour off the turbid liquid into a flask, grind the residue to the finest powder and wash it with the remaining citrate solution into the flask, keep the contents of the latter at 30 40 for half an hour, with very frequent shaking, then dilute to 200 c. c., pour upon a dry filter, take 100 c. c. of filtrate =1 grm. substance, add 40 c. c. magnesia mixture, 120 c. c. water and 100 c. c. ammonia, stir, filter, ignite, etc., as under 4. Deducting the soluble phosphoric acid from that here found gives the amount of " reverted phosphoric acid" 6. Insoluble Phosphoric Acid. 5 grm. of the superphosphate are wet with 5 c. c. solution of magnesium nitrate, sp. gr. 1.3554 * Neutralize 185 grm. citric acid with ammonia or ammonium carbonate, in very slight excess, and bring to a volume of 1000 c. c. f HO grm. crystallized MgCl 2 6H 2 O, 140 grm. NH 4 C1, 700 c. c. solution of ammonia sp. gr. 0'96, and water to make 2 litres. Instead of MgCl 2 6H 2 O, 22 grm. of calcined magnesia may be dissolved in the equivalent quantity of HC1, the solution boiled with a little calcined magnesia in excess and filtered. \ Dissolve 160 grm. calcined MgO in the equivalent quantity of HNO 3 , boil with a little excess of MgO, filter and bring to volume of 1 litre. 5 c. c. of this solution is enough to prevent formation of pyrophosphate in 5 grm. of any com- mercial superphosphate. If not enough to destroy organic matters, moisten the residue of ignition with HNOs and heat again. 220.] ANALYSIS OF COMMERCIAL FERTILIZERS. 769 evaporated tp dryness and gently ignited. The residue is digested with hydrochloric acid, diluted to 500 c. c. and filtered on a dry filter. To 100 c. c. of filtrate (= 1 grm. substance) are added 4> c. c. ammonium citrate solution, 25 c. c. magnesium mixture, lUU c. c. water and 90 c. c. ammonia. The precipitate is treated as under 4. Subtracting the result of 5 from that of 6, gives the " insoluble phosphoric acid." 7. To apply the molybdic method to the analysis of superphos- phates, determine total phosphoric acid in 2 grm., first ignited with addition of magnesium nitrate, then treated with nitric acid to complete solution of the phosphates and diluted to 500 c. c. lot i c, c. of this solution are used. Determine "insoluble phos- phoric acid " in a suitable aliquot of the nitric solution of the insoluble residue of 5. Reverted phosphoric acid is found indirectly by subtracting from the total the sum of the soluble and insoluble. 8. Potash. Boil 10 grin, with water for 10 minutes, dilute the solution to 1000 c.c. and filter through a dry filter. The error of measurement due to the presence of undissolved matters is inconsiderable and may be neglected. Heat 100 c.c. of the filtrate to boiling, precipitate sulphuric acid by barium chloride and magnesium iron, &c., together with phosphoric acid by barium hydroxide and filter. In the filtrate, heated nearly to boiling, pre- cipitate the barium by ammonium carbonate and filter. Evaporate the filtrate to dryness, expel ammonium salts by ignition, dissolve the residue in a little water and determine the potash by excess of platinic chloride in the usual way. When the substance contains much soluble organic matters it is better to destroy these at the outset by heat, which should be very gentle at first and may finally reach faint redness. Nitrogen may exist in superphosphates either in organic com- bination, as ammonium salts, or as nitrates. 9. The nitrogen of ammonium salts is determined in all cases by distilling with calcined magnesia proceeding as directed p. 220, except that magnesia must be used instead of potash or lime. 10. The nitrogen in organic combination when alone or together with ammonium salts is determined by combustion with soda lime (p. 644), in the latter case subtracting from the result the amount of nitrogen already found to exist in ammonium salts. 11. Nitrogen in the form of nitrates is determined by SCHULZE'S method as described on p. 473. 770 SPECIAL PART. [ 220. 12. "When nitrates and nitrogenous organic matters occur together, it is necessary to determine the total nitrogen by the absolute method as described on p. 63755. The determination of soluble, reverted, and insoluble phosphoric acid, of potash and of nitrogen, is usually sufficient to fix the com- mercial value of a superphosphate. It is sometimes required, how- ever, to determine water, sulphuric acid and chlorine. 13. Water. Dry one gramme for three hours at 100. It is often impracticable, and for commercial purposes is unnecessary, to make an accurate water determination. Gypsum, which most superphosphates contain in considerable quantity, does not part with all its water readily or completely at 100, while a higher heat to some extent decomposes the organic matters. 14. Sulphuric acid. Boil one grm. with water acidulated with hydrochloric acid, filter, and determine sulphuric acid in the filtrate in the usual way. It is advisable in all cases to purify the precipitate as described on p. 366. 15. Chlorine is estimated by YOLHAKD'S method, or by precipi- tation with silver nitrate, in the clear hot water extract of 1 grm. GUANO. 16. The determinations of phosphoric acid, soluble, "reverted," and insoluble, are made precisely as in the case of a superphos- phate. The soluble phosphoric acid consists of phosphates of the alkalies, and the washings, except in the case of " rectified" guanos which have been treated with oil of vitriol, are alkaline. 17. Determine nitrogen as in superphosphates. Many guanos contain ammonium carbonate and therefore require care in manipula- tion to prevent its escape. If nitrates are present, add to the 0-5 gr. taken for combustion with soda lime an equal weight of pure sugar or oxalic acid. The quantity of nitrate is so small that with this precaution accurate results are obtained without resorting to the absolute method. 18. Potash is determined as in superphosphates. 19. If a determination of water is required, weigh the guano in a boat and introduce it into a tube which is heated to 100 in an air or water bath. One end of this tube is connected with a dry- ing apparatus containing oil of vitriol or calcium chloride. The other is provided with a U-tube and standard acid for receiving 220.] ANALYSIS OF COMMERCIAL FERTILIZERS. 771 ammonia, and an aspirator to maintain a current of dry air. The volatilized ammonia is measured with a standard alkali and taken into account in reckoning the loss of weight. BONE. 20. Water. Dry 1 grm. at 100, and determine water by loss. 21. Fat. Transfer the dry bone to an extraction apparatus and extract with absolute ether as long as anything is removed. Evaporate the ether extract, dry at 100 for two hours and weigh. 22. Carbonic acid. Determine carbonic acid in 1 grm. by the method described on p. 4120. 23. Ash. Incinerate 1 grm. till the ash is white or light gray. Moisten with ammonium carbonate solution, dry, ignite gently and weigh. 24-. Phosphoric acid. Dissolve the ash, prepared as above, in hydrochloric acid, filter, dilute to 250-300 c.c., add 12-15 grm. of citric acid as ammonium citrate and precipitate with magnesia mixture in the manner previously described, 4, or dissolve in nitric acid and proceed by the molybdic process. 25. Nitrogen. Determine nitrogen in 1 grm. by combustion with soda lime. For most purposes the determination of phosphoric acid and nitrogen in sufficient. POTASH SALTS. 26. Boil 5 grm. with water for 10 minutes, dilute to 1000 c.c. and determine potash in 100 c.c. as described under 8 or 29. 27. In another portion of 100 c.c., determine sulphuric acid by barium chloride, and in a third portion chlorine may be deter- mined by precipitation with silver nitrate, or more conveniently by VOLHARD'S method. 28. Determine water by heating 2-5 grm. in a platinum capsule to dull redness. 29. Potash. STOHMANN directs to boil 10 grm. of substance with about 300 c.c. of water, and to add dropwise BaCl 2 solution until no further precipitate appears, to let cool and dilute to 1000 c.c., and after subsidence or filtration to take 100 c.c. of the clear solution, add a large excess of PtCl 4 (equivalent to about 2 grm. 772 SPECIAL PART. [ 222. Pt), evaporate and proceed as usual with the precipitate. As the alkali-earth platinchlorides are all soluble in alcohol, the results are good. 21. ANALYSIS OF ATMOSPHEETC AIE. 221. In the analysis of atmospheric air we usually confine our at- tention to the following constituents : oxygen, nitrogen, carbonic acid, and aqueous vapor. It is only in exceptional cases that the exceedingly minute quantities of ammonia and other gases many of which may be assumed to be always present in infinitesimal traces are also determined. It does not come within the scope of the present work to de- scribe all the methods which have been employed in the capital investigations made in the last few years by BRUNNER, BUNSEN, DUMAS and BOUSSINGAULT, REGNAULT and REISET, and others. To these methods we are indebted for a more accurate knowledge of the composition of our atmosphere, and excellent descriptions of them will be found in the works below.* I confine myself to those methods which are found most con- venient in the analysis of the air for medical or technical purposes. A. DETERMINATION OF THE WATER AND CARBONIC ACID. 222. It was formerly the custom to effect these determinations by BRUNNER'S method, which consisted iii slowly drawing, by means of an aspirator, a measured volume of air through accurately weighed apparatuses filled with substances having the property of retaining the aqueous vapor and the .carbonic acid, and esti- mating these two constituents by the increased weights of the ap- paratuses. Fig. 103 represents the arrangement recommended by REG- NAULT. *Ausfiihrliches Handbuch der analytischen Chemie, von H. Rose, II. 853; Graham-Otto's Ausf uhrliches Lehrbuch der Chemie, Bd. II. Abth. 1, S. 102 et seq.; Handworterbuch der Chemie, von Liebig, Poggendorff und Wohler, 2 Aufl. Bd, II. S. 431 et seq.; and Bunsen's Gasometry. 222.] ANALYSIS OF ATMOSPHERIC AIR. 773 The vessel V is made of galvanized iron, or of sheet zinc ; it holds from 50 to 100 litres, and stands upon a strong tripod in a trough large enough to hold the whole of the water that V con- tains. At a a brass tube, c, with stopcock, is firmly fixed in with cement. Into the aperture &, which serves also to fill the appara- tus, a thermometer reaching down to the middle of V is fixed air- tight by means of a perforated cork soaked in wax. The efflux tube, 7', which is provided with a cock, is bent slightly upward, to guard against the least chance of air entering the vessel Fig. 103. from below. The capacity of the vessel is ascertained by filling it completely with water, and then accurately measuring the contents in graduated vessels. The end of the tube c is connected air-tight with F, by means of a caoutchouc tube ; the tubes A F are simi- larly connected with one another. J., -B, E, and F are filled with small pieces of glass moistened with pure concentrated sulphuric acid, C and D with moist slaked lime.* Finally, A is also con- * With regard to C and Z>, I have returned to lime, preferring it to purnice saturated with solution of potash, because, as Hlasiwetz (Chem. Centralbl. 1856, 575) has shown, the solution of potash absorbs not only carbonic acid, but also oxygen. Indeed, H. Rose had previously made a similar observation. With re- spect to the other tubes, I prefer the concentrated sulphuric acid to calcium chloride as the absorbent for water (see Pettenkofer, Sitzungsber. der bayer 774 SPECIAL PART. [ 222. nected with a long tube leading to tlie place from which the air intended for analysis is to be taken. The corks of the tubes are coated over with sealing-wax. The tubes A and B are intended to withdraw the moisture from the air ; they are weighed together. C, D, and E are also weighed jointly. C and D absorb the car- bonic acid ; E the aqueous vapor which may have been withdrawn from the hydrate of lime by the dry air. F need not be weighed ; it simply serves to protect E against the entrance of aqueous vapor from V. The aspirator is completely filled with water ; c is then con- nected with. F, and thus with the entire system of tubes ; the cock r is opened a little, just sufficiently to cause a slow efflux of water. As the height of the column of water in V is continually dimiii- ishing, the cock must from time to time be opened a little wider, to maintain as nearly as possible a uniform flow of water. "When V is completely emptied, the height of the thermometer and that of the barometer are noted, and the tubes A and B, and (7, Z>, and ^weighed again. As the increase of weight of A and B gives the amount of water, that of C, D, and E the amount of carbonic acid, in the air which has passed through them ; and as the volume of the latter (freed from water and carbonic acid) is accurately known from the ascertained capacity of V* the calculation is in itself very simple ; but it involves, at least in very accurate analyses, the following corrections : of. Reduction of the air in I 7 ", which is saturated with aqueous vapor, to dry air ; since the air which penetrates through c is dry. /?. Reduction of the volume of dry air so found to 0, and Y60 mm. When these calculations have been made (see " Calculations of Analyses," in Appendix), the weight of the air which has pene- trated into F is readily found from the datum in Table Y. at the Akad. 1862, II. Heft 1, S. 59). Hlasiwetz's statement, that concentrated sul- phuric acid also takes up carbonic acid, I nave found to be unwarranted. Calcium chloride does not dry the air completely, and, besides, Hlasiwetz says that when it is used a trace of chlorine is carried away corresponding to tne amount of ozone in the air (op. cit. p. 517). * Or from the quantity of water which has flown from V, as the experiment may be altered in this way, that a portion only of the water is allowed to run out, and received in a measuring vessel. g 2*22.] ANALYSIS OF ATMOSPHERIC AIR. 77.") end of the volume; and as the carbonic acid and water have also been weighed, the respective quantities of these constituents of the air may now be expressed in per cents, by weight, or, calculating the weights into volumes, in per cents, by measure. Considering the great weight and size of the absorption appara- tus, in comparison to the increase of weight by the process, at least 25,000 c. c. of air must be passed through ; the air inside the bal- ance-case must be kept as dry as possible by means of a sufficient quantity of calcium chloride, and the apparatus left for some time in the balance-case before proceeding to weigh. Neglect of these measures would lead to considerable errors, more particularly as regards the carbonic acid, the quantity of which in atmospheric air is, on an average, about 10 times less than that of the aqueous vapor (comp. HLASIWETZ, loc. cit.}. For the exact determination of the carbonic acid one of the fol- lowing methods is far better suited : a. Process suggested by FK. MOHR, applied and carefully tested l}ij H. v. GILM."* VON GILM employed in his experiments an aspira- tor holding at least 30 litres, which was arranged like that shown in fig. 103, but had a third aperture, bearing a small manometer. The air was drawn through a tube, 1 metre long and about 15 mm. wide ; this tube w r as drawn out thin at the upper end, and at the lower end bent at an angle of 140 150. It was more than half filled with coarse fragments of glass and perfectly clear baryta water, and fixed in such a position that the long part of it was inclined at an angle of 8 10 to the horizontal. A narrow glass tube, fitted into the undrawn-out end of the tube by means of a cork, served to admit the air. Two small flasks, filled with baryta water, were placed between the absorption tube and the aspirator ; these were intended as a control, to show that the whole of the carbonic acid had been retained. When about 60 litres of air had slowly passed through the absorption tube, the barium carbon- ate formed was filtered oft' out of contact of air, and the tube as well as the contents of the filter washed, first with distilled water saturated with barium carbonate, then with pure boiled water. The barium carbonate in the filter and in the tube was then dis- solved in dilute hydrochloric acid, the solution evaporated to dry- * Chem. Centralbl. 1857, 760. 776 SPECIAL PART. [ 222. Fig. 104. ness, the residue gently ignited, and the chlorine of the barium chloride determined as directed 141, 5, a. 2 atoms of chlorine represent 1 mol. carbonic acid. It is obvious that one may also determine the barium in the hydrochloric acid solution by precipi- tating with sulphuric acid. For filtering the barium carbonate, v. GILM employed a double funnel (fig. 104) ; the inner cork has, besides the perforation through which the neck of the funnel passes, a lateral slit, which establishes a commu- nication between the air in the outer funnel and the air in the bottle. As, with the absorption apparatus arranged as described, the air has to force its way through a column of fluid, the manometer is required to de- termine the actual volume of the air ; the height indicated by this instrument being deducted from the barometric pressure observed during the pro- cess. FR. MOHR * now recommends as the absorb- ent fluid a solution of barium hydroxide in pot- ash. -This is prepared by dissolving crystals of barium hydroxide in weak solution of potash with the aid of heat, and filtering off the barium carbonate, which invariably forms in small quantity. The clear filtrate is accordingly saturated with barium carbonate. MOHR now leaves out the fragments of glass. This method afforded v. GILM very harmonious results. Nev- ertheless, it involves one source of error. If clear baryta water is passed through paper with the most careful possible exclusion of air, and the filter is washed till the washings are free from baryta, and dilute hydrochloric acid is then poured upon the filter, and the filtrate thus obtained is evaporated, a small quantity of barium chloride will be left, showing that a little baryta was kept back by the paper. AL. MULLER f has already called attention to the capa- city of filter paper for retaining baryta. 1). M. PETTENKOFER'S process. \ a. Principle and Requisites. A known volume of air is made * Lehrbuch der Titrirmethode, 2d ed. 446. f Journ. f. prakt. Chem. 83, 384. \ Abhandl. der naturw. u. tcchn. Commission der k. bayer. Akad. der Wiss. II. 1; Annul, d. Chem. u. Pharm. II. Supplem. Bd. p. 1. 222.] ANALYSIS OF ATMOSPHERIC AIE. 777 to act upon a definite quantity of standard baryta water (standard- ized by oxalic acid solution), in such manner that the carbonic acid is completely bound by the baryta. The baryta water is then poured out into a cylinder, and allowed to deposit with exclusion of air, a part of the clear fluid is then removed, and the baryta remaining in solution is determined. The difference between the oxalic acid required for a certain quantity of baryta water before and after the action of the air represents the barium carbonate formed, and consequently the carbonic acid present. Two kinds of baryta water are used: one contains 21 grm. and the other 7 grm. crystallized barium hydroxide * in the litre ; these serve for the determination of larger and smaller quantities of car- bonic acid respectively. 1 c. c. of the stronger corresponds to about 3 ingrm. carbonic acid, of the weaker 1 c. c. corresponds to about 1 mgrm.f The oxalic acid solution which serves for standardizing the baryta water contains 2'8636 grm. cryst. oxalic acid in 1 litre. 1 c. c. corresponds to 1 mgrm. carbonic acid. The baryta water is standardized as follows: Transfer 30 c. c. of it to a flask, and then run in the oxalic acid from a MOHR'S burette with float ; shake the fluid from time to time, closing the mouth of the flask with the thumb. The vanishing point of the alkaline reaction is ascer- * The barium hydroxide must be entirely free from caustic potash, and soda, the smallest quantities of which render the volumetric estimation in the presence of barium carbonate impossible, since the normal alkali oxalates decompose the alkali-earth carbonates. When a trace even of barium carbonate is suspended in the fluid and this is always the case when a baryta water which has been used for the absorption of carbonic acid is not filtered the reaction continues alkaline if the smallest trace of potash or soda is present, because the alkali oxa- late formed immediately enters into decomposition with the barium carbonate. A fresh addition of oxalic acid converts the alkali carbonate again into oxalate. and the fluid is for a moment neutral, till, on shaking with air, the carbonic acid escapes, and any barium carbonate still present converts the alkali oxalate again into carbonate. To test a baryta water for caustic alkali, determine the alkalin- ity of a perfectly clear portion, and then of a portion that has been mixed with a little pure precipitated barium carbonate. If you use more oxalic acid in the second than in the first experiment, caustic alkali is present, and some barium chloride must be added to the baryta water before it can be used. f [The baryta water is kept in a bottle under a thin stratum of kerosene (MOHR). It is drawn off through a siphon supported in the stopper, the outer leg of which is recurved upwards and closed with a bit of rubber tube and clip. By having this leg of the siphon sufficiently long the burette may be filled by inserting its delivery end in the rubber tube and opening both clips.] 778 SPECIAL PART. [222. tained with delicate turmeric paper. * As soon as a drop of the fluid placed on the paper does not give a brown ring, the end is attained. If you were obliged, in the first experiment, to take out too many drops for testing with turmeric paper, consider the result as only approximate, and make a second experiment, adding at once the whole quantity of oxalic acid to within 1 or ^ c. c. and then beginning to test with paper. A third experiment would be found to agree with the second to ^ c. c. The reaction is so sen- sitive that all foreign alkaline matter, particles of ash, tobacco smoke, &c., must be carefully guarded against. /3. The actual Analysis. This may be effected in two differ- ent ways. aa. Take a perfectly dry bottle, of about 6 litres capacity, with well-fitting ground glass stopper, and accurately determine the capacity ; fill the bottle, by means of a pair of bellows, with the air to be analyzed ; add 45 c. c. of the dilute standard baryta w r ater, and cause the baryta water to spread over the inner surface of the bottle by turning the latter about, but without much shaking. In the course of about -J an hour the whole of the carbonic acid is absorbed. Pour the turbid baryta water into a cylinder, close securely, and allow to deposit ; then take out, by means of a pipette, 30 c. c. of the clear supernatant fluid, run in standard oxalic acid, multiply the volume used by 1*5 (as only 30 c. c. of the original 45 are em- ployed in this experiment), and deduct the product from the c. c. of oxalic acid used for 45 c. c. of the fresh baryta water; the dif- ference represents the quantity of baryta converted into carbonate, and consequently the amount of the carbonic acid. If the air is unusually rich in carbonic acid, the concentrated baryta water is employed. bb. Pass the air through a tube or through two tubes contain- ing measured quantities of standard baryta water and finish the experiment as in aa. For passing a definite quantity of air we should generally employ an. aspirator (p. 7Y3) ; PETTENKOFER in his experiments with the respiration apparatus forced the air by means of small mercurial pumps first through the tubes, and then through an apparatus for measuring the gas. The form and arrangement * Prepared with lime-free Swedish filter paper and tincture of turmeric. The spirit used in making the latter must be free from acid. Dry the paper in a dark room, and keep it protected from the light. It is lemon yellow. 223.] ANALYSIS OF ATMOSPHERIC AIU. 779 of the tubes is illustrated by tig. 105. Two such tubes were used ; the first was 1 metre, the second '3 metres long ; they were filled with baryta water the former with the stronger solution, the lat- ter with the weaker. The air is introduced through the short limbs of the tubes, and the glass tubes themselves are so inclined Fig. 105. that the bubbles of air move on with the necessary rapidity with- out uniting. The motion of the gas bubbles keeps up a constant mixing of the baryta water. B. DETERMINATION OF THE OXYGEN AND NITROGEN. 223. The method I shall give is that proposed by v. LIEBIG.* It is based upon the observation made by CHEVREUL and DOBEREINER, that pyrogallic acid, in alkaline solutions, has a powerful tendency to absorb oxygen. 1. A strong measuring tube, holding 30 c. c. and divided into ^ or yL c . c., is filled to f with the air intended for analysis. The remaining part of the tube is filled with mercury, and the tube is inverted over that fluid in a tall cylinder, widened at the top. 2. The volume of air confined is measured ( 12). If it is intended to determine the carbonic acid which can be done with sufficient accuracy only if the quantity of the acid amounts to several per cents. the air is dried by the introduction of a ball of cal- cium chloride before measuring. If it is not intended to determine Annal. d. Chem. u. Pharm. 77, 107. 780 SPECIAL PART. [ 223. the carbonic acid this operation is omitted. A quantity of solution of potassa of 1*4 sp. gr. (1 part of dry potassium hydroxide to 2 parts of water), amounting to from ^ to ^ of the volume of the air, is then introduced into the measuring tube by means of a pipette with the point bent upwards (fig. 106), and spread over the entire inner surface of the tube by shak- ing the latter ; when no further diminution of volume takes place, the decrease is read off. If the air has been dried Fig. 106. previously with calcium chloride, the diminution of the volume expresses exactly the amount of carbonic acid con- tained in the air ; but if it has not been dried with calcium chloride, the diminution in the volume cannot afford correct information as to the amount of the carbonic acid, since the strong solution of potassa absorbs aqueous vapor. 3. "When the carbonic acid has been removed, a solution of pyrogallic acid, containing 1 grm. of the acid* in 5 or 6 c. c. of water, is introduced into the same measuring tube by means of another pipette, similar to the one used in 2 (fig. 106) ; the quantity of pyrogallic acid employed should be half the volume of the solution of potassa used in 2. The mixed fluid (the pyrogallic acid and solution of potassa) is spread over the inner surface of the tube by shaking the latter, and, when no further diminution of volume is observed, the residuary nitrogen is measured. 4. The solution of pyrogallic acid mixing with the solution of potassa of course dilutes it, causing thus an error from the diminu- tion of its tension ; but this error is so trifling that it has no appreciable influence upon the results ; it may, besides, be readily corrected, by introducing into the tube, after the absorption of the oxygen, a small piece of hydrate of potassa corresponding to the amount of water in the solution of the pyrogallic acid. 5. There is another source of error in this method ; viz., on account of a portion of the fluid always adhering to the inner sur- face of the tube, the volume of the gas cannot be read off with absolute accuracy. In comparative analyses, the influence of this defect upon the results may be almost entirely neutralized, by taking nearly equal volumes of air in the several analyses.f * Liebig has described a very advantageous method of preparing pyrogallic acid. See Annal. d. Chem. u. Pharm. 101, 47. f Bunsen employs for the absorption of oxygen a papier-mache ball saturated 224.] ARSENIC IN ORGANIC MATTER. 781 6. Notwithstanding these sources of error, the results obtained by this method are very accurate and constant. In eleven analyses which v. LIEBIG reports, the greatest difference in the amount of oxygen found was between 20*75 and 21'03. The num- bers given express the actual and uncorrected results. [22. DETECTION AKD ESTIMATION OF AKSEXIC IX OBGAXIC MATTER GAUTIER'S Method simplified ty JOHNSON AND CHITTENDEN. The following method for the detection and estimation of arsenic in organic matter is a modification of the process recently described by GAITTIER.* GAUTIER'S method consists in treating the substance with certain quantities of nitric acid, and afterwards of sulphuric acid, at a high temperature, whereby the organic matters are partly destroyed and converted into slightly soluble humus-like bodies, from which all the arsenic may be extracted by boiling water. Gautier treats the brown 'solution thus obtained with " sodium bi-snlphate, throws down the arsenic in the state of sul- phide, with hydrogen sulphide, transforms this sulphide into arsenic acid by known means," treats the solution thus obtained in the Marsh Apparatus, and finally weighs the arsenic in the metallic state as below described. JOHNSON and CHTITENDEN dispense with the use of all reagents but sulphuric acid, nitric acid, and zinc alloyed with a little pla- tinum, which are not difficult to obtain in a state of absolute free- dom from arsenic, and they, together with DONALDSON, have dem- onstrated that the method, thus essentially simplified, gives exact results. The following account of the process is from a paper by CHITTENDEN and DoNALDSON.f with a concentrated alkaline solution of potassium pyrogallate, "which he intro- duces into the gaseous mixture attached to a platinum wire. By adopting this proceeding the source of error mentioned in 5 is avoided. Bee also Russell, Jour. Chem. Soc. 1868, pp. 130, 131. * Bulletin de la Societe Chimique, 24, 250. f American Chemical Journal, vol. ii. p. 235. 782 SPECIAL PAKT. I. HEAGENTS AND APPARATUS. The reagents required are pure granulated zinc alloyed with a small quantity of platinum, pure concentrated nitric and sulphuric acids, and three dilute sulphuric acids of increasing strength, which, for the sake of convenience, may be prepared in considerable quan- tities. ISO c. c. pure cone. II 2 SO 4 - -1000 c. c. H 2 O. Acid No. 1. Acid No* 2. 260 c. c. pure cone. 1I 2 SO 4 +1000 c. c. H 2 O. Acid No. 3. 425 c. c. pure cone. H 2 SO 4 +1000 c. c. H 2 O. The form of MARSH apparatus used is shown by fig. 107. The flask, a BUNSEN'S wash-bottle of 200 c. c. capacity, is pro- Fig. 107. vided with a small separating funnel of 65 c. c. capacity, with glass stopcock. This is a very material aid to the obtaining of a slow and even evolution of gas, and is nearly indispensable in accurate quantitative work. The gas generated is dried by passing through a calcium chloride tube,* and then passes through a tube of hard glass, heated to a red heat by a fur- nace of three BUNSEN lamps with spread burners, so that a contin- uous flame of six inches is obtained, and with a proper length of * OTTO and also DRAGENDORFP recommend to pass the gas first over fragments of caustic potassa. We find, however, in accordance with DOREMTJS, that arse, nic is arrested by caustic alkali. S. W. J. and R. H. C. 224.] AESENIC IN OEGANIC 31 ATTEE. 783 cooled tube not a trace of arsenic passes by. The glass tube where heated is wound with a strip of wire gauze, both ends being sup- ported upon the edges of the lamp frame, so that the tube does not sink down when heated. The small furnace is provided with two appropriate side pieces of sheet metal, so that a steady flame is always obtained. When the quantity of arsenic is very small the tube is naturally so placed that the mirror is deposited in the nar- row portion, but when the arsenic is present to the extent of *005 grin, the tube should be 6 millimetres in inner diameter, and so arranged that fully two inches of this large tube are between the flame and the narrow portion. When the quantity of arsenic is less the tube can naturally be smaller. II. PROCESS. a. Method for the complete extraction of arsenic from organic matter. 100 grms of the material to be examined, cut into small pieces, are placed in a porcelain casserole of 600 c. c. capacity and provided with a stirring rod of stout glass. 23 c. c. of pure concentrated nitric acid are added, and the dish placed on a small air-bath* provided with a thermometer and a single BUXSEX burner. The m ixture is then heated at 150 160 C., with occasional stirring. At first the tissue takes on a yellowish color, then swells up somewhat, becoming finally quite thick ; soon changes again, becoming liquid, and then generally requires heating from \\ to 2 hours, the tem- perature sometimes being raised to 180 C. At this point the mass, being now quite thick again, usually takes on a deeper yellow color or orange shade. When this change of color is noticed the casserole is taken from the bath and 3 c. c. of pure concentrated sulphuric acid added and the mixture stirred vigorously. The addition of concentrated sulphuric acid to the viscid residue rich in nitric acid and nitro-com pounds naturally * For air-bath an ordinary flat-bottomed tin basin, 7 inches in diameter, 3 inches deep, is used with a cover provided with an opening 5 inches in dia- meter. This bath is set in an iron ring fastened to a stout lamp-stand, while the end of the thermometer passes through a small hole near the edge of the cover a short distance into the bath, so that the temperature can be regulated. 784 SPECIAL PART. [ 224. gives rise, especially at this temperature, to a considerable com- motion: the mass becomes brown, swells up, nitrous fumes are copiously evolved, immediately followed by dense white fumes of suffocating odor, while the residue in the dish is changed either into a dry carbonaceous mass or a black, sticky, tar-like mass. Although the oxidation is so powerful, no deflagration takes place, and the carbonization is effected in this manner without the volatilization of any arsenic. The casserole is again placed on the bath and heated for a few minutes at 180 C., then, while still on the bath, 8 c. c. of pure concentrated nitric acid are added drop by drop with continual stirring, the object being to destroy more completely the organic matter, arid at the same time the nitric acid falling drop by drop on the carbonaceous residue tends to prevent the formation of sulphurous acid and the consequent formation of insoluble arseni- ous sulphide. After the addition of the nitric acid the dish is heated at 200 C. for fifteen minutes, and when cold a hard carbonaceous residue is the result, entirely free from nitric acid. In w r or king with dif- ferent kinds of tissue, slight deviations from the above description will frequently be observed. When much bony matter is present the last residue takes on a somewhat different character, owing to the presence of calcium sulphate, and occasionally when the 3 c. c. of sulphuric acid are added the oxidation does not at once take place, but requires a little longer heating on the air-bath. "When such is the case the mixture needs constant watching in order to remove the dish from the bath at the first approach of the oxida- tion. The arsenic now exists as arsenic acid, readily soluble in w^ater. The carbonaceous residue is thoroughly extracted with boiling water, and in order to avoid all loss is not previously pul- verized, but the casserole in which the oxidation took place is filled with water and heated on the water-bath for several hours. The hard mass soon softens, and by repeated treatment in this manner readily gives up all its arsenic to the aqueous solution ; it is, however, bet- ter to have the carbonaceous residue in contact with different por- tions of warm water for about 24 hours to insure the complete extraction of the arsenic. The reddish-brown fluid containing some organic matter and arsenic acid is now evaporated on the water-bath to dryness, care being taken that the entire residue is finally obtained in one cas- 224.] ARSENIC IN ORGANIC MATTER. 785 serole. This residue* of organic matter and arsenic is warmed with 45 c. c. of sulphuric acid No. 1, and the clear solution so obtained, or, as more frequently happens, the fluid with organic matter in suspension, is then ready for introduction into the MARSH apparatus. J. Method for the conversion of arsenic acid into arsenetted hydrogen and then into metallic arsenic. 25-35 grms. of granulated zinc previously alloyed with a small quantity of platinum are placed in the generator, and everything being in position, the MARSH apparatus is filled with hydrogen by the use of a small quantity of acid No. 1. After a sufficient time has elapsed the gas is lighted at the jet and the glass tube heated to a bright redness. The 45 c. c. of acid No. 1 containing the arsenic is then poured into the separating funnel, from which it is allowed to flow into the generator at such a rate that the entire fluid is introduced in one hour or one hour and a half ; 40 c. c. of acid No. 2 are then poured into the casserole, to which considerable organic matter usually adheres, and then transferred to the separating fun- nel and allowed to flow slowly into the generator, and lastly 45 c. c. of acid No. 3. In this manner we are sure to have all of Jfche arsenic acid dissolved and thus carried into the generator, while at the same time the stronger acids Nos. 2 and 3 ser\ 7 e as a rinse fluid and thereby prevent mechanical loss, while, at the same time, the increasing strength of acid added counteracts the diluting effect of the reaction so that the strength of acid remains about the same during the entire process of 2^ to 3 hours and thereby insures a regular flow of gas. The amount of time required will vary with the amount of arsenic : 2 3 mgrms. of arsenic will require about two to three hours for the entire decomposition, while 4 5 * When the residue left by the evaporation of the water is quite large, it is sometimes better to reoxidize it. This is quickly accomplished by adding a few cubic centimetres of concentrated nitric acid to the contents of the casserole and heating on the air-bath at 150 180 C. until a reddish solution is obtained. Then 3 5 c. c. of concentrated sulphuric acid are added and the mixture heated at the above temperature until the nitric acid is completely driven off. The thin black fluid is then carefully mixed with the requisite quantity of No. 1 acid, and intro- duced into the Marsh apparatus. Frequently quite a heavy, flocculent precipitate separates from the sulphuric acid solution. This does not interfere, but is poured, together with the fluid, directly into the receiving bulb, which is purposely pro- vided with a delivery tube of large calibre. 786 SPECIAL PART. [ 224. ingrmes. will need perhaps three to four hours. "Where the amount of arsenic is small, only 25 grms. of zinc are needed, and but 45 c. c. of acid No. 1, 30 c. c. of acid No. 2, and 30 c. c. of acid No. -3 ; but when 4 5 mgrms. of arsenic are present it is better to take the first mentioned quantities of zinc and acids. The arsenic being thus collected as a large or small mirror of metal, the tube is cut at a safe distance from the mirror, so that a tube of perhaps 2 6 grms. weight is obtained. This is carefully weighed and then the arsenic removed by simple heating ; or, if the arsenic is to be saved as in a toxical case, dissolved out with strong nitric acid. The tube is then cleaned, dried, and again weighed, the difference giving the weight of metallic arsenic, from which by a simple calculation the amount of arsenious oxide can be obtained. The delicacy of the method is shown by the fact that -00001 grm. As 2 O 3 when introduced into 100 grms. of beef yielded by this method a distinct mirror of metallic arsenic. In a similar manner '000001 grm. As a O, yielded a faint mirror of arsenic, this amount appearing to be the limit. In conducting these experiments with organic matter, after the zinc is placed in the generator, 15 drops of olive oil are allowed to flow down the side, and this as the fluid is intro- duced floats on top and thereby prevents any troublesome frothing. The only other thing to be guarded against is the too rapid intro- duction of the acids, whereby loss as well as frothing of the mix- ture may ensue, and secondly the heating of the flask by the chemical reaction. If necessary this latter can be prevented by placing the generator in a glass or other dish so that a stream of cold water can continually play about it, which will keep the flask sufficiently cool to prevent the formation of any hydrogen sulphide which might sometimes show itself in slight quantity. The following results show the accuracy of the method : Wt. of Metallic Theoretical Wt. Quantity of Arsenic introduced. Arsenic found. Metallic Arsenic. 100 grms. beefsteak with .004 grm. As a 8 '00300 '00303 i < 004 004 003 005 005 00300 -00303 00290 -00303 00219 -00227 00369 -00378 00372 -00378] III. EXERCISES FOR PRACTICE. EXEEOISES FOE PRACTICE. THE principal point kept in view in the selection of these exer- cises has been that most of them, and more particularly the first, should permit an exact control of the results. This is of the utmost importance for students, since a well-grounded self-reliance is among the most indispensable requisites for a successful pursuit of quantitative investigations, and this is only to be attained by ascer- taining for one's self how near the results found approach the truth. Xow a rigorously accurate control is practicable only in the analysis of pure salts of known composition, or of mixtures com- posed of definite proportions of pure bodies. When the student has acquired, in the analysis of such substances, the necessary self- reliance, he may proceed to the analysis of minerals or products of industry in which such rigorous control is unattainable. The second point kept in view in the selection of these exer- cises has been to make them comprise both the more important analytical methods and the most important bodies, so as to afford the student the opportunity of acquiring a thorough knowledge of every branch of quantitative analysis. Organic analysis offers less variety than the analysis of inor- ganic substances ; the exercises relating to the former branch are therefore less numerous than those relating to the latter. I would advise the student to analyze the same substance re- peatedly, until the results are quite satisfactory. [It is a good habit always to carry on together duplicate analyses. It requires but little more time to make two analyses than to make one, and the operator's experience is thus very economically doubled.] It is by no means necessary for the student to go through the whole of these examples ; the time which he may require to attain proficiency in analysis depends, of course, upon his own abilities. One may be a good analyst without having tried every method or determined every body. A few substances well analyzed yield more profit than can be obtained from going over many processes in a superficial manner. 790 EXEKCISES FOK PRACTICE. Finally, the student is warned against prematurely attempting to discover new methods ; he should wait until he has attained a good degree of proficiency in general chemistry, and more particu- larly in practical analysis. EXEKCISES. A. SIMPLE DETERMINATIONS IN THE GRAVIMETRIC WAY, IN- TENDED TO PERFECT THE STUDENT IN THE PRACTICE OP THE MORE COMMON ANALYTICAL OPERATIONS. [Ws give here, in the first place, quite full details of all the steps in the estimation of chlorine in sodium chloride, including the preparation of this salt in a state of purity. This, it is hoped, will relieve much of the perplexity which the beginner must at first experience in making out a scheme of operations from the various separate paragraphs where the processes are described. The student should not fail, however, to study carefully the chapter on operations while carrying on the analysis, nor to examine every reference. 1. SODIUM CHLORIDE. Preparation. Sodium chloride is far less soluble in hydro- chloric acid than in water. On account of this property the crude product common salt may be purified from the magnesium chloride and calcium sulphate which it contains as follows : To 100 c. c. of a saturated solution add very gradually an equal vol- ume of pure concentrated hydrochloric acid. Drain the mass of fine crystals which separate on a funnel, the throat of which is loosely closed with filter paper. Wash with a small volume of pure dilute hydrochloric acid, and at last, in order to test the purity of the product, allow 5 or 6 c. c. of distilled water to pass through. Collect the water that runs through in a test tube separately, and add to it barium chloride. If no turbidity results, the sodium chloride is free from sulphates and may be assumed to be pure enough for analysis. Kemove it from the funnel and dry it in a porcelain dish. If not free from sulphates, the product may be subjected to a repetition of the process. This, however, will rarely be neces- sary.* * When large quantities of pure sodium chloride are required, it is more economical to prepare it from a solution of common salt by saturating the solu- tion with HC1 gas. EXERCISES FOR PRACTICE. 791 A portion* of the salt thus obtained is heated in a covered cru- cible until it ceases to decrepitate, but not to fusion, and preserved in a weighing tube (like a small test tube, but not flared at the mouth) that is closed with a soft, well-fitting, and smooth cork. ESTIMATION OF CHLORINE. 1. Weighing out the substance. The tube containing the pre- pared salt is wiped, if need be, from dust. The cork is taken out, and by means of a bit of thin paper, or a clean linen handkerchief, any particles of salt adhering to the cork, and to the inside of the tube as far as the cork reaches, are removed. The cork is replaced, and the whole is weighed (see 9 and 10), the weight being imme- diately recorded in the note-book. A clean beaker or assay-flask, of about 200 c. c. capacity, being ready, the weighing-tube is held over it and the cork carefully removed. A portion of substance is allowed to fall in the vessel, and, the cork being replaced, the tube is again counterpoised. If two to three decigrammes have been emptied, the operator is ready to proceed. If less, more should be transferred from the tube to the vessel. If more, or much more, it is better to begin anew, by weighing off another portion into another beaker or flask. In this manner weigh off two portions in separate vessels, so as to carry together duplicate analyses. Xow affix a piece of gummed paper to each vessel, and label them to correspond with their designation in the note-book. 2. Solution and precipitation. Dissolve the weighed portions, each in about 100 c. c. of cold distilled water, add a few drops of pure nitric acid, and, lastly, clear solution of silver nitratef until further addition no longer produces a precipitate. Agitate the mixture well, but with care to avoid loss. This can be done by shaking, if a flask be in use, or by stirring with a glass rod, if a beaker be employed. Set the vessel aside in a dark place, covered with paper or a watch-glass to exclude dust, and let stand for about 12 hours, or until the precipitate has subsided and the liquid above it is perfect! y clear, then add a drop of silver nitrate to make sure that the pre- cipitation is complete (if not complete, add more solution of silver, and let stand again for some hours). * Pure sodium chloride is needed in other analyses, and the chief part of what Is thus prepared should he carefully bottled and reserved for future use. f Solution of a silver coin in nitric acid answers for this purpose as well as pure nitrate, provided it be clear and contain but little free acid. 792 EXERCISES FOR PRACTICE. 3. Filtration. A filter is placed in a funnel at least J inch deeper than itself, and moistened with water, at the same time being carefully pressed down so that its edges touch the glass at all points. The funnel being supported on a stand, a- clean beaker or flask is put beneath it, and the operator proceeds to pour the liquid on whose surface some particles of silver chloride usually float into the filter, leaving the bulk of the precipitate undisturbed. To do this without loss the following precautions may be regarded : a. Touch the edge or lip of the vessel with a very slight coat of tallow (a small bit of which is kept at hand under the edge of the work- table, and is applied with the finger), b. Pour slowly over the greased place, along a glass rod held nearly vertical, so directing the stream that it shall strike against the side, not into the vertex of the filter, c. When the filter is filled to within J inch of the top discontinue the pouring, bringing the rod into the vessel con- taining the precipitate, after it has drained so that nothing will fall from it. The pouring-rod may be simply straight, and an inch longer than the diago- nal of the vessel, or when it is desirable not to disturb a precipitate, it may be 3 4 inches long and bent siphon fashion so as to hang on the edge of a beaker or flask. In either case its end should be rounded by fusion, and those portions along which the liquid flows must not be handled. The vessel containing the precipitate, as well as that which receives the filtrate, and likewise the funnel, should be kept covered as much as possible in all cases when nicety is required, to prevent access of dust, insects, &c. The most convenient covers are large watch-glasses, but square plates of glass, or even cards, will generally answer. The filtration of silver chloride should be conducted without exposing it to strong light, whereby it is blackened, with loss of chlorine, p. 168. 4. When all, or nearly all, the liquid has passed the filter, it remains to wash and to transfer the precipitate. These operations may be carried on as follows : pour about 100 c.c. of cold distilled water upon the precipitate, which mostly remains in the vessel where it was formed, and agitate vigorously, in order to break up and divide the lumpy silver chloride, and bring every part of it perfectly in contact with the water. EXERCISES FOR PRACTICE. 793 When in a beaker, the agitation must be made with great caution, by means of a glass stirring-rod ; when in a narrow-mouthed flanged flask, this may be tightly closed by a perfectly smooth cork (softened for the purpose by squeezing) and then shaken violently. The water and precipitate are now poured together upon the niter, with the precautions before detailed. The last portions of the precipitate are removed from the beaker or flask by repeated rins- ings, in which a wash-bottle like flg. 36, p. 81, may be conveniently employed. Any portions of precipitate that adhere to the sides of the ves- sel too strongly to be removed by a stream from the wash-bottle must be nibbed off. For this purpose the feather is employed. It is made from a goose-quill, by cutting off the extreme tip for an inch or so, and smoothly trimming away the beard, except a portion of one half-inch in length on the inside of the curve. The tubular part may be removed or not, to suit the depth of the dish which is to be washed. The dish being wiped clean, externally, a little water is put in it, and, it being held up to the light, its whole interior surface is gently nibbed with the feather, then rinsed, rubbed again and rinsed, so long as careful inspection discovers any portions of adhering pre- cipitate ; finally, the feather is rinsed in a stream of water, the rinsings in each case being poured upon the filter. The washing is now continued by help of the wash-bottle. A jet of cold water is directed, first, upon the interior of the funnel, just above the filter, then upon the edge of the filter itself. If thrown immediately against the paper, this is liable to be perfo- rated. The stream of water is carried around the edge of the filter until the latter is nearly full, and the liquid is then allowed to drain off. This process is repeated until a portion of the wash-water, collected to the depth of an inch in a test tube containing a drop of hydrochloric acid, gives no turbidity of silver chloride. When this is accomplished, the precipitate is washed down into the ver- tex of the filter. The funnel is then closely covered with paper (p. 85), labelled, allowed to drain thoroughly, and set away in a warm place for drying. 5. Drying the filter. In public laboratories a heated closet is usually provided for drying filters. Its temperature should not exceed 100 C. In default of such special arrangement, the dry- ing may be effected over the register of a hot-air furnace, or over a common stove or kitchen range. 794 EXERCISES FOR PRACTICE. The funnel may also be supported on a retort-stand over a sheet of iron, which is heated beneath by a lamp, or may be placed at once in the water-bath. See 50. 6. When the precipitate is perfectly dry we proceed to ignite it for weighing. A small porcelain crucible (platinum must not be used) is cleaned, gently ignited, and when cool (after 15 20 minutes) weighed. The work-table being clean, two small sheets of fine and smooth writing or glazed paper are opened and laid down side by side. The filter is removed from the funnel and carefully inverted upon one of the papers. The precipitate is loosened from the filter by squeezing and rubbing gently between the fingers, and when it has mostly separated the filter is lifted, reversed, and any portions of silver chloride still adhering are loosened by rubbing its sides together. What is thus detached is poured or shaken out on the paper. The filter is now spread out as a half -circle upon the other sheet of paper, and, beginning with the straight edge, is folded up into a narrow flattened roll, the two ends of which are then brought together. In this way those central portions of the filter to which particles of precipitate adhere are thoroughly enveloped by the exterior parts, so that in the subsequent burning nothing can -easily escape. The crucible being placed on the glazed paper, the filter is taken by the two free ends in a clean pincers or tongs, put to the flame of a lamp to set it on fire, and then held over the crucible until it is completely charred. It is then dropped into the crucible and moistened with two or three drops of nitric acid. The cruci- ble is covered and placed over a low flame until its contents are dry ; it is then heated somewhat stronger, whereby the carbon is nearly or entirely consumed. The crucible being allowed to cool, one more drop of nitric acid, and afterwards a drop of hydrochloric acid, is added to the residue, and it is heated cautiously, without the cover, until fumes cease to escape. This treatment with nitric acid serves to destroy carbon and convert any reduced silver to nitrate, which the hydro- ' -chloric acid in turn transforms into chloride. When the crucible is cool, it is placed again on the paper, and the precipitate is poured into it from the other sheet, the last particles being detached by EXERCISES FOR PRACTICE. 795 cautious tapping with the fingers underneath, or by the use of a clean camePs-hair pencil. The crucible is now put over a low flame and heated cautiously until the silver chloride begins to fuse on the edges. It is then covered and let cool. When cold it is weighed. Read 115, 1, and the references there made. 7. ^Record and calculation of results. The amount of silver chloride is learned by subtracting from the total the joint weight of the crucible and filter-ash. The quantity of chlorine is obtained by multiplying the amount of silver chloride by the decimal 0*2473. In order to compare results they are reduced to per cent, statements by the following proportion : Substance : chlorine in substance : : 100 : chlorine in 100 ; i.e. per cent. The record may be made as follows : It is well to work out the calculations in full in the weight-book, as in case of mistake the data are at hand for revision. No. 1. No. 2. NaCl and tube 6'615 6'180 " substance 6'180 5'765 Substance -435 Crucible, AgCl and Ash 15 '3630 Cr 14-298 ) u . 2 CO. f Cu < J > SO Q + 5H 2 O. t [Boil a solution of commercial blue vitriol with a little pure binoxide of lead to oxidize the iron, then with a little barium carbonate to precipitate it, filter and crystallize. H. WURTZ, Am. Jour. (2), XXVI. 367.] EXERCISES FOR PRACTICE. 799 a. Determination of Water of Crystallization. 1. Weigh off in a crucible 1 2 grm. of the salt, and, having first heated the air- bath (fig. 22, p. 52) so that the thermometer stands steadily at 120 140, introduce the crucible, uncovered, and maintain the heat for two hours. Then cool the crucible in a desiccator and weigh. Heat again as before, for an hour, and weigh. If need be, repeat the heating until no more loss occurs. The loss expresses the amount of water expelled at the temperature of 140, or four molecules. 2. Raise the temperature of the air-bath to between 250 260 and proceed as before. The loss is the one molecule of strongly combined water of crystallization, or, as some term it, water of halhydration. o. Determination of Sulphuric Acid. In another portion of the copper sulphate (about 1*5 grm.) determine the sulphuric acid according to 132, I., 1. d. Determination of Copper. In about 1-5 grm. determine the copper as cuprous sulphide, as directed 119, 3, a. CuO 79-40 31-83 SO, 80-00 32-08 H 2 O 18-00 7-22 4 a HO 72-00 28.87 249-40 100-00 9. CRYSTALLIZED HYDROGEN SODIUM PHOSPHATE.* a. Determination of the Water of Crystallization. Heat about 1 grm. of the pure uneffloresced salt in a platinum crucible, slowly and moderately, first in the water-bath, then in the air-bath, and finally some distance above the lamp (not to visible redness) ; the loss of weight gives the amount of water of crystallization. I. Determination of the Hydrogen in the Anhydrous Salt. Ignite the residue of a. The loss is water. c. Determination of Phosphoric Acid. a. Treat 1-5 2 grm. of the salt as directed 134, J, a. ft. Treat about 0'2 grm. of the salt as directed 134, , ft. I recommend the student to perform the determination by each of these methods, as they are both in common use in the analytical laboratory. * HO \ NaO - - PO -f 24H 2 O. XaO ^ 800 EXERCISES FOR PRACTICE. d. Determination of Sodium. Treat about 1*5 grm. of the salt, according to 135, , a. After the excess of lead has been separated with hydrogen sulphide, the fluid is to be evaporated to dryness and weighed in a platinum dish ; comp. 69, &, and 98, 2. P,0 142-00 19-83 2Na a O 124-16 IT'34 H a O 18-00 2-51 24H,O ..... 432-00 60-32 716-16 100-00 10. SILVER CHLORIDE. Ignite pure fused silver chloride in a stream of pure dry hydro- gen till complete decomposition is effected, and weigh the silver obtained. The ignition may be performed in a light bulb tube, or in a porcelain boat in a glass tube, or in a porcelain crucible with perforated cover ( 115, 4). The chlorine may be in this case estimated by difference ; if you want to determine it directly, proceed as directed 141, II., . Ag 107-93 75-27' 01 35-46 24-73 143-39 100-00 11. MERCURIC SULPHIDE. Reduce to a fine powder, and dry at 100. a. Determination of Sulphur. Treat about 0*5 grm., as directed 148, /?, p. 466, using nitric acid and potassium chlorate. Precipitate with barium chloride, and after decanting the clear liquid into a filter, boil the barium sulphate twice with dilute solution of ammonium acetate and finally wash with hot water. b. Determination of Mercury. Dissolve about 0*5 grm. as before, dilute, and allow to stand in a moderately warm place until the smell of chlorine has nearly gone off ; filter if necessary, add ammonia in excess, heat gently for some time, add hydro- chloric acid until the white precipitate of mercuric chloride and amide of mercury is redissolved, and treat the solution, which now no longer smells of chlorine, as directed 118, 3. Hg 200-00 86-21 S . . 32-00 13-79 232-00 100-00 EXERCISES FOR PRACTICE. 801 12. CRYSTALLIZED CALCIUM SULPHATE.* Select clean and pure cystals of selenite, triturate to a coarse powder, avoiding as much as possible exposure to the air, and cork up in a weighing tube. a. Determination of Water. After 35, a, a. o. Determination of Sulphuric Add and Calcium ( 132, II, &, a). CaO 56 32-56 SO, . '. 80 46-51 2H a O 36 20-93 172 100-00 C. SEPARATION OF TWO BASIC OR TWO ACID RADICALS FROM EACH OTHER, AND DETERMINATIONS IN THE VOLUMETRIC WAY. 13. SEPARATION OF IRON FROM MANGANESE. Dissolve in hydrochloric acid about 0'2 grm. fine pianoforte wire, and about the same quantity of ignited protosesquioxide of manganese (prepared as directed 109, 1, a) ; heat with a little nitric acid, and separate the two metals by means of sodium acetate (p. 517). Determine the manganese as directed 109, 3. 14. VOLUMETRIC DETERMINATION OF IRON BY SOLUTION OF POTASSIUM PERMANGANATE. a. Graduation of the Solution of Potassium Perman- ganate. a. By metallic iron (fine piano wire) dissolved in dilute sul- phuric acid (p. 268). ft. By ammonium oxalate (p. 270). o. Determination of Iron in Ammonium Ferrous Sul- phate. In solution acidified with sulphuric acid (p. 272, ft). The formula requires 18-37 per cent, of FeO. *Ca 802 EXERCISES FOR PRACTICE. c. .Determination of the Iron in a Limonite. Powder finely, dry at 100, weigh off 2 grm., heat with strong hydrochloric acid till the ferric oxide is completely dissolved, dilute the acid solution with twice its volume of water, filter, evaporate with sulphuric acid, dilute the ferric sulphate to 500 c.c., and in two or three portions of 100 c.c. each reduce ferric to ferrous sulphate, and determine iron as directed in 113, &, p. 278. i 15. VOLUMETRIC DETERMINATION OF IRON WITH SODIUM THIOSULPHATE. a. Graduation of the Solution of Sodium Thiosulphate. a. By solution of ferric chloride (p. 280). ft. By ammonia-iron-alum (p. 119). 2 grms. to be weighed off, dissolved in water with addition of hydrochloric acid. h. Determination of Iron in Limonite. Decompose 2 to 3 grms. with concentrated hydrochloric acid. Transfer to a 500 c.c. flask, mix well the solution diluted to 500 c.c., and determine repeatedly iron in portions of 100 c.c. each, after 113, 3, b. (If the ore contains ferrous iron, oxidize the hydrochloric acid solution with potassium chlorate, avoiding need- less excess, and concentrate it one half to remove excess of chlorine. See 112, 1, p. 266.) 16. DETERMINATION OF NITRIC ACID IN POTASSIUM NITRATE. Heat pure nitre, not to fusion, and transfer it to a tube provided with a cork. Treat 0*5 grm. as directed p. 4Y3, ft. K 2 O 94-26 46-59 N,O 108-08 53-41 202-34 . 100-00 IT. SEPARATION OF MAGNESIUM FROM SODIUM. Dissolve about 0-4 grm. pure recently ignited magnesia and about 0-5 grm. pure well-dried sodium chloride in dilute hydro- chloric acid (avoiding a large excess), and separate by one of the methods described in 153, 4. EXERCISES FOR PRACTICE. 803 18. SEPARATION or POTASSIUM FROM SODIUM. Triturate crystallized sodium potassium tartrate (Rochelle salt), press between blotting paper, weigh off about 1*5 grm., heat in a platinum crucible, gently at first, then for some time to gentle ignition. The carbonaceous residue is first extracted with water, finally with dilute hydrochloric acid, the acid fluid is evaporated in a weighed platinum dish, and the chlorides are weighed together ( 97, 2). Then separate them by platinic chloride (p. 481, 1), and calculate from the results the quantities of soda and potassa sever- ally contained in the Rochelle salt. K 3 O 94-26 16-70 Na 2 O 62-08 11-00 C 8 H 8 O 10 .... 264-00 46-78 8ILO 144-00 25-52 564-34 100-00 19. VOLUMETRIC DETERMINATION OF CHLORINE IN CHLORIDES. a. Preparation and examination of the solution of silver nitrate ( 141, L, J, ). ~b. Indirect determination of the sodium and potassium in Rochelle salt, by volumetric estimation of the chlorine in the alkali chlorides prepared as in No. 18. For calculation, see " Cal- culation of Analyses," in the Appendix. 20. ACIDIMETRY. a. Preparation of standard acid and alkali solutions. Sulphuric acid and potash, or hydrochloric acid and ammonia may be used ( 192). 5. Determination of acid in hydrochloric acid, by the specific gravity (p. 677). c. Determination of acid in the same hydrochloric acid, by an alkaline fluid of known strength (p. 684). d. Determination of acid in colored vinegar, by saturation with a standard alkaline solution. (Application of test-papers, p. 684). 21. ALKALIMETRY. a. Preparation of the normal acid after DESCROIZILLES and GAY-LUSSAC ( 195). 804 EXERCISES FOR PRACTICE. I. Valuation of a soda-ash after expulsion of the water by gentle ignition. a. After DESCROIZILLES and GAY-LUSSAC ( 195). /3. After MOHR ( 196). 22. DETERMINATION OF . AMMONIUM. Treat about O8 grm. chloride of ammonium as directed 99, 3, a. 4 . . 18-04 . . 33-72 NH 3 . . . 17'04 . . 31-85 Cl . 35-46 . . 66-28 HC1 . . . 36*46 . . 68-15 53-50 100-00 53-50 100-00 I). ANALYSIS OF ALLOYS, MINERALS, INDUSTRIAL PRODUCTS, &c., IN THE GRAVIMETRIC AND VOLUMETRIC WAY. 23. ANALYSIS OF BRASS. Brass consists of from 25 to 35 per cent, of zinc and from 75 to 65 per cent, of copper. It also contains usually small quantities of tin and lead, and occasionally traces of iron. Dissolve about 2 grm. in nitric acid, evaporate on the water- bath to dryness, moisten the residue with nitric acid, add some water, warm, dilute still further, and filter off any residual meta- stannic acid ( 126, 1, a). Add to the filtrate, or, if the quantity of tin is very inconsiderable, directly to the solution, about 20 c.c. dilute sulphuric acid ; evaporate to dryness on the water-bath, add 50 c.c. water, and apply heat. If a residue remains (lead sul- phate), filter it off, and treat it as directed 116, 3. In the filtrate, separate the copper from the zinc by sodium thiosulphate (p. 540). If the quantity of iron present can be determined, determine it in the weighed oxide of zinc ( 160). ^ 24. ANALYSIS OF SOLDER (TiN AND LEAD). Introduce about 1-5 grm. of the alloy, cut into small pieces, into a flask, treat it with nitric acid, and proceed as directed p. 339, to effect the separation and estimation of the tin. Mix the filtrate in a porcelain dish with pure dilute sulphuric acicf, evaporate the nitric acid on the water-bath, and proceed with the lead sulphate obtained as directed 116, 3. Test the fluid EXERCISES FOR PRACTICE. 805 filtered from the lead sulphate with hydrogen sulphide and ammo- nium sulphide for the other metals which the alloy might contain besides tin and lead. The stannic oxide may contain small quan- tities of iron or copper ; it is tested for these by fusion with sodium carbonate and sulphur (p. 558). 25. ANALYSIS OF A DOLOMITE. See 210. 26. ANALYSIS OF FELSPAR. a. Decomposition by sodium carbonate ( 140, II., b) ; removal of the silicic acid ; precipitation of the aluminium with the small quantity of iron as hydroxides by ammonia (in platinum or Berlin porcelain, not in glass vessels) after 156, 1, (37) ; separation of barium, if present, from the filtrate with dilute sulphuric acid, and then of calcium with ammonium oxalate, 154 (28). Finally, solu- tion of the weighed alumina in concentrated hydrochloric acid, separation and weighing of traces of silica if present ; evaporation with sulphuric acid and volumetric determination of iron, generally present in small quantities after 113, p. 279. b. Decomposition by SMITH'S method, p. 426. Separate the alkalies after 152, 1. - c. Determine loss by ignition. 27. ASSAY OF A CALAMINE OR SMrrHSONTTE. After 215. Volumetric determination of the zinc. 28. ASSAY OF GALENA. Determination of the lead, as directed 213. 29. VALUATION OF CHLORIDE OF LIME ( 199). a. After PENOT (p. 699). b. After OTTO (p. 701). 30. VALUATION OF MANGANESE ( 202). a. After FKESEXIUS and WILL (p. 705). The evolved CO, to be weighed (p. 708). b. After BUNSEN (p. 709). c. By means of iron (p. 709). 806 EXERCISES FOB PRACTICE. 31. COMPLETE ANALYSIS OF IRON ORE ( 217). E. DETERMINATION OF THE SOLUBILITY OF SALTS. 32. DETERMINATION OF THE DEGREE OF SOLUBILITY OF COMMON SALT. a. At boiling heat. Dissolve perfectly pure pulverized sodium chloride in distilled water, in a flask, heat to boiling, and keep in ebullition until part of the dissolved salt separates. Filter the fluid now with the greatest expedition, through a funnel surrounded with boiling water and covered with a glass plate, into an accu- rately tared capacious measuring flask. As soon as about 100 c.c. of fluid have passed into the flask, insert the cork, allow to cool, and weigh. Fill the flask now up to the mark with water, and determine the salt in an aliquot portion of the fluid, by evaporating in a platinum dish (best with addition of some ammonium chloride, which will, in some measure, prevent decrepitation) ; or by deter- mining the chlorine ( 141). b. At 14:. Allow the boiling saturated solution to cool down to this temperature with frequent shaking, and then proceed as in a. 100 parts of water dissolve at 109*7. . . .40*35 of sodium chloride. 100 " " 14 35*87 " " 33. DETERMINATION OF THE DEGREE OF SOLUBILITY OF CALCIUM SULPHATE. a. At 100. I. At 12. Digest pure pulverized calcium sulphate for some time with water, in the last stage of the process at 40 50 (at which tempera- ture sulphate of lime is most soluble) ; shake the mixture frequently during the process. Decant the clear solution, together with a little of the precipitate, into two flasks, and boil the fluid in one of them for some time ; allow that in the other to cool down to 12, with frequent shaking, and let it stand for some time at that temperature. Then filter both solutions, weigh the filtrates, and determine the amount of calcium sulphate respectively contained in them, by evaporating and igniting the residues. 100 parts of water dissolve at 100 0'217 of anhydrous calcium sulphate. 100 " " 12 0-233 34. ANALYSIS OF ATMOSPHERIC AIR. See 221. c 48 H . . 6 o 96 EXERCISES- FOR PRACTICE. 807 F. ORGANIC ANALYSIS AND ANALYSES IN WHICH ORGANIC ANALYSIS IS APPLIED. 35. ANALYSIS OF TARTARIC ACID. Select clean and white crystals. Powder and dry at 100. a. Burn with lead chromate after 177. For details of manipulation see 174 and 175. b. Burn with oxygen gas in a tray, 178. 32 4 64 150 100 36. DETERMINATION OF THE NITROGEN IN CRYSTALLIZED POTAS- SIUM FERROCYANIDE. Triturate the perfectly pure crystals, press in blotting paper, and determine the nitrogen as directed 185. (Combustion with soda lime.) The formula requires 19*93 per cent, of nitrogen. 37. ANALYSIS OF URIC ACID (or any other perfectly pure organic compound of carbon, hydrogen, oxygen, and nitrogen). Dry pure uric acid at 100. a. Determination of the carbon and hydrogen ( 183). b. Determination of the nitrogen. a. After 185. ft. After 184, II. C 5 60-00 35-68 N 4 56-16 33-40* H 4 4-00 2-38 O, 48-00 28-54 168-16 100-00 38. ANALYSIS OF A SUPERPHOSPHATE ( 220). 39. ANALYSIS OF COAL ( 219.) 40. ANALYSIS OF A CAST IRON. After 218. * Taking 14 for the atomic weight of N gives 33'33 per cent, of nitrogen. APPENDIX, ANALYTICAL EXPERIMENTS.* 1. ACTION OP WATER UPON GLASS AND PORCELAIN VESSELS, IN THE; PROCESS OP EVAPORATION (to 41). A large bottle was filled with water cautiously distilled from a copper boiler with a tin condensing tube. All the experiments in 1 were made with this water. a. 300 c.c., cautiously evaporated in a platinum dish, left a residue weighing, after ignition, 0*0005 grm. =0*0017 per 1000. b. 600 c.c. were evaporated, boiling, nearly to dryness, in a wide flask of Bohemian glass ; the residue was transferred to a platinum dish, and the flask rinsed with 100 c.c. distilled water, which was added to the residue in the dish ; the fluid in the latter was then evaporated to dryness, and the residue ignited. The residue weighed 0'0104 gnn. Deducting from this the quantity of fixed matter originally contained in the distilled water, viz .. 0'0012 " There remains substance taken up from the glass 0'0092 " =0-0153 per 1000. In three other experiments, made in the same manner, 300 c.c. left, in two 0-0049 grm., in the third 0'0037 grm. ; which, calculated for 600 c.c., gives art average of 0'0090 grm. And after a deduction of ..0-0012 " 0-0078 " =0-013 per 1000. We may therefore assume that 1 litre of water dissolves, when boiled down- to a small bulk in glass vessels, about 14 milligrammes of the constituents of the- glass. c. 600 c.c. were evaporated nearly to dryness in a dish of Berlin porcelain, and in all other respects treated as in b. The residue weighed 0*0015 grm. Deducting from this the quantity of fixed matter contained in the distilled water, viz 0'0012 " There remains substance taken up from the porcelain 0*0003 " =0-0005 per 1000. * The experiments are numbered as in the original edition, but some are omitted. 810 ANALYTICAL EXPERIMENTS. 2. ACTION OF HYDROCHLORIC, ACID UPON GLASS AND PORCELAIN VESSELS, IN THE PROCESS OF EVAPORATION (to 41). The distilled water used in 1 was mixed with y 1 ^ of pure hydrochloric acid. a. 300 grin., evaporated in a. platinum dish, left 0'002 grm. residue. b. 300 grm., evaporated first in Bohemian glass nearly to dryness, then in a platinum dish, left 0*0019 residue; the dilute hydrochloric acid, therefore, had not attacked the glass. c. 300 grm., evaporated in Berlin porcelain, &c., left 0*0036 grm., accordingly after deducting 0-002, 0-0016=0 '0053 per 1000. d. In a second experiment made in the same manner as in c., the residue amounted to 0'0034, accordingly after deducting 0*002, '0014=0-0047 per 1000. Hydrochloric acid, therefore, attacks glass much less than water, whilst porcelain is about equally affected by water and dilute hydrochloric acid. This shows that the action of water upon glass consists in the formation of soluble basic silicates. 3. ACTION OF SOLUTION OF AMMONIUM CHLORIDE UPON GLASS AND PORCELAIN VESSELS, IN THE PROCESS OF EVAPORATION (to 41). In the distilled water of 1, ^ of ammonium chloride was dissolved, and the solution filtered. a. 300 c.c., evaporated in a platinum dish, left O'OOG grm. fixed residue. b. 300 c.c., evaporated first nearly to dryness in Bohemian glass, then to dry ness in a platinum dish, left 0'0179 grm. ; deducting from this 0*006 grm., there remains substance taken up from the glass, 0-0119=0-0397 per iOOO. c. 300 c.c., treated in the same manner in Berlin porcelain, left 0-0178 deducting from this 0'006, there remains 0-0118=0-0393 per 1000. Solution of ammonium chloride, therefore, strongly attacks both glass and porcelain in the process of evaporation. 4. ACTION OF SOLUTION OF SODIUM CARBONATE UPON GLASP AND PORCE- LAIN VESSELS (to 41). In the distilled water of 1, T V of pure crystallized sodium carbonate was dis- solved. a. 300 c.c., supersaturated with hydrochloric acid and evaporated to dryness in a platinum dish, &c., gave 0'0026 grm. silica=0'0087 per 1000. b. 300 c.c. were gently boiled for three hours in a glass vessel, the evaporat- ing water being replaced from time to time; the tolerably concentrated liquid was then treated as in a; it left a residue weighing 0'1376 grm. ; deducting from this the 0-0026 grm. left in a, there remains 135 grm. =0 450 per 1000. c. 300 c.c., treated in the same manner as in b, in a porcelain vessel, left 0-0099; deducting from this 0*0026 grm., there re mains 0-0073=0-0243 per 1000. Which shows that boiling solution of sodium carbonate attacks glass very strongly, and porcelain also in a very marked manner. 5. WATER DISTILLED FROM GLASS VESSELS (to 56, 1). 42'41 grm. of water distilled with extreme caution from a tall flask with a LIEBIG'S condenser, left upon evaporation in a platinum dish, a residue weighing, after ignition, O'OOIS grm., consequently ANALYTICAL EXPERIMENTS. 811 6. POTASSIUM SULPHATE AND ALCOHOL (to 68, a). a. Ignited pure potassium sulphate was digested cold with absolute alcohol, for several days, with frequent shaking; the fluid was filtered off, the filtrate diluted with water, and then mixed with barium chloride. It remained perfectly clear upon the addition of this reagent, but after the lapse of a considerable tune it began to exhibit a slight opalescence. Upon evaporation to dryness, there remained a very trifling residue, which gave, however, distinct indications of the presence of sulphuric acid. b. The same salt treated in the same manner, with addition of some pure concentrated sulphuric acid, gave a filtrate which, upon evaporation in a plati- num dish, left a clearly perceptible fixed residue of potassium sulphate. 7. DEPORTMENT OF POTASSIUM CHLORIDE IN THE AIR AND AT A HIGH TEMPERATURE (to 68, b). (V9727 grm. of ignited (not fused) pure potassium chloride, heated for 10 minutes to dull redness in an open platinum dish, lost 0'0007 grm.; the salt was then kept for 10 minutes longer at the same temperature, when no further dimi- nution of weight was observed. Heated to bright redness and semi-fusion, the salt suffered a further loss of weight to the extent of 0'0009 grm. Ignited intensely and to perfect fusion, it lost 0-0034 grm. more. Eighteen hours' exposure to the air produced not the slightest increase of weight. 8. SOLUBILITY OF POTASSIUM PLATINIC CHLORIDE IN ALCOHOL (to 68, c). a. In absence of free Hydrochloric Acid. a. An excess of perfectly pure, recently precipitated potassium platinic chloride was digested for 6 days at 15 20, with alcohol of 97%5 per cent., in a stoppered bottle, with frequent shaking. 72'5 grm. of the perfectly colorless filtrate left upon evaporation in a platinum dish a residue which, dried at 100, weighed 0'006 grm.; 1 part of the salt requires therefore 12083 parts of alcohol of 97'5 per cent, for solution. ft. The same experiment was made with alcohol of 76 per cent. The filtrate might be said to be colorless; upon evaporation, slight blackening ensued, on which account the residue was determined as platinum. 75 '5 grm. yielded O'OOS grm. platinum, corresponding to 0'02 grm. of the salt. One part of the salt dissolves accordingly in 3775 parts of alcohol of 76 per cent. y. The same experiment was made with alcohol of 55 per cent. The filtrate was distinctly yellowish. 63'2 grm. left 0"0241 grm. platinum, corresponding to 0'06 grm. of the salt. One part of the salt dissolves accordingly in 1053 parts of alcohol of 55 per cent. b. In presence of free Hydrochloric Acid. Recently precipitated potassium platinic chloride was digested cold with alcohol of 76 per cent. , to which some hydrochloric acid had been added. The solution was yellowish; 67 grm. left 0'0146 grm. platinum, which corresponds to 0-0365 grm. of the salt. One part of the salt dissolves accordingly in 1835 parts of alcohol mixed with hydrochloric acid. 9. SODIUM SULPHATE AND ALCOHOL (to 69, a). Experiments made with pure anhydrous sodium sulphate, in the manner 812 ANALYTICAL EXPERIMENTS. described in 6, showed that this salt comports itself both with pure alcohol, and with alcohol containing sulphuric acid, exactly like potassium sulphate. 10. DEPORTMENT OP IGNITED SODIUM SULPHATE IN THE Am (to 69, a). 25169 grm. anhydrous sodium sulphate were exposed, in a watch-glass, to the open air on a hot summer day. The first few minutes passed without any increase of weight, but after the lapse of 5 hours there was an increase of 0*0061 grm. 12. DEPORTMENT OF SODIUM CHLORIDE IN THE AIR (to 69, b). 4-3281 grm. of chemically pure, moderately ignited (not fused) sodium chloride, which had been cooled under a bell-glass over sulphuric acid, acquired during 45 minutes' exposure to the (somewhat moist) air an increase of weight of 0-0009 grm. 13. DEPORTMENT OP SODIUM CHLORIDE UPON IGNITION BY ITSELF AND WITH AMMONIUM CHLORIDE (to 69, b). 4*3281 grm. chemically pure, ignited sodium chloride were dissolved in water, in a moderate-sized platinum dish, and pure ammonium chloride was added to the solution, which was then evaporated and the residue gently heated until the evolution of ammonium chloride fumes had apparently ceased. The residue weighed 4 '3334 grm. It was then very gently ignited for about 2 minutes, and after this re-weighed, when the weight was found to be 4*3314 grm. A few minutes' ignition at a red heat reduced the weight to 4*3275 grm., and 2 minutes' further ignition at a bright red heat (upon which occasion white fumes were seen to escape), to 4 '3249 grm. 14. DEPORTMENT OF SODIUM CARBONATE IN THE AIR AND ON IGNITION (to 69, c). 2*1061 grm. of moderately ignited chemically pure sodium carbonate were exposed to the air in an open platinum dish in July in bad weather; after 10 minutes the weight was 2-1078, after 1 hour, 21113, after 5 hours, 2-1257. 1 -4212 grm. of moderately ignited chemically pure sodium carbonate were ignited for 5 minutes in a covered platinum crucible ; no fusion took place, and the weight was unaltered. Heated more strongly for 5 minutes, it partially fused, and then weighed 1*4202. After being kept fusing for 5 minutes, it weighed 1-4135. 15. DEPORTMENT OF AMMONIUM CHLORIDE UPON EVAPORATION AND DRYING (to 70, a). 0"5625 grm. pure and perfectly dry ammonium chloride was dissolved in water in a platinum dish, evaporated to dryness in the water-bath and com- pletely dried; the weight was now found to be 0'5622 grm. (ratio 100:99'94). It was again heated for 15 minutes in the water-bath, and afterwards re-weighed, when the weight was found to be 0'5612 grm. (ratio 100:99-77). Exposed once more for 15 minutes to the same temperature, the residue weighed 0'5608 grm. (ratio 100:99-69). 16. SOLUBILITY OF AMMONIUM PLATINIC CHLORIDE IN ALCOHOL (to 70, 6). a. In absence of free Hydrochloric Acid. a. An excess of perfectly pure, recently precipitated ammonium platinic ANALYTICAL EXPERIMENTS. 813 chloride was digested for 6 days, at 15 20, with alcohol of 97'5 per cent., in a stoppered bottle, with frequent agitation. 74'3 grm. of the perfectly colorless nitrate left, upon evaporation and ignition in a platinum dish, O0012 grm. platinum, corresponding to 0'0028 of the salt. One part of the salt requires accordingly 26535 parts of alcohol of 97*5 per cent. ft. The same experiment was made with alcohol of 76 per cent. The filtrate was distinctly yellowish. 81 '75 grm. left 0'0257 platinum, which corresponds to 0-0584 grm. of the salt. One part of the salt dissolves accordingly in 1406 parts of alcohol of 76 per cent. y. The same experiment was made with alcohol of 55 per cent. The filtrate was distinctly yellow. Slight blackening ensued upon evaporation, and 56 '5 grm. left 0'0364 platinum, which corresponds to 0'08272 grm. of the salt. Con- sequently, 1 part of the salt dissolves in 665 parts of alcohol of 55 per cent. b. In presence of Hydrochloric Acid. The experiment described in ft was repeated, with this modification, that some hydrochloric acid was added to the alcohol. 76'5 grm. left 0'0501 grm. of platinum, which corresponds to 0'1139 grm. of the salt. 672 parts of the acidi- fied alcohol had therefore dissolved 1 part of the salt. 17. SOLUBILITY OF BARIUM CARBONATE IN WATER (to 71, b). a. In Cold Water. Perfectly pure, recently precipitated Ba CO 3 was digested for 5 days with water of 16 20, with frequent shaking. The mixture was filtered, and a portion of the filtrate tested with sulphuric acid, another portion with ammonia; the former reagent immediately produced turbidity in the fluid, the latter only after the lapse of a considerable time. 84*82 grm. of the solution left, upon evaporation, 0'0060 Ba CO 3 . One part of that salt dissolves conse- quently in 14137 parts of cold water. b. In Hot Water. The same barium carbonate being boiled for 10 minutes with pure distilled water, gave a filtrate manifesting the same reactions as that prepared with cold water, and remaining perfectly clear upon cooling. 84 '82 grm. of the hot solution left, upon evaporation, 0'0055 grm. of barium carbonate. One part of that salt dissolves therefore in 15421 parts of boiling water. 18. SOLUBILITY OF BARIUM CARBONATE IN WATER CONTAINING AMMONIA AND AMMONIUM CARBONATE (to 71, b). A solution of chemically pure barium chloride was mixed with ammonia and ammonium carbonate in excess, gently heated and allowed to stand at rest for 12 hours; the fluid was then filtered off; the filtrate remained perfectly clear upon addition of sulphuric acid; but after the lapse of a very considerable time, a hardly perceptible precipitate separated. 84 '82 grm. of the filtrate left, upon evaporation in a small platinum dish, and subsequent gentle ignition, 0'0006 grm. One part of the salt had consequently dissolved in 141000 parts of the fluid. 19. SOLUBILITY OF BARIUM SILICO-FLUORIDE IN WATER (to 71, c). a. Recently precipitated, thoroughly washed barium silico-fluoride was digested for 4 days in cold water, with frequent shaking; the fluid was then filtered off, and a portion of the filtrate tested with dilute sulphuric acid, another 814 ANALYTICAL EXPERIMENTS. portion with solution of calcium sulphate ; both reagents produced turbidity the former immediately, the latter after one or two seconds precipitates sepa- rated from both portions after the lapse of some time. 84.82 grm. of the filtrate left a residue which, after being thoroughly dried, weighed 0-0223 grm. One part of the salt had consequently required 3802 parts of cold water for its solu- tion. b. A portion of another sample of recently precipitated barium silico-fluoride was heated with water to boiling, and the solution allowed to cool (upon which a portion of the dissolved salt separated). The cold fluid was left for a consider- able time longer in contact with the undissolved salt, and was then filtered off. The filtrate showed the same deportment with solution of sulphate of lime as that of a. 84-82 grm. of it left '025 grm. One part of the salt had accordingly dissolved in 3392 parts of water. 20. SOLUBILITY OF BARIUM SILICO-FLUORIDE IN WATER ACIDIFIED WITH HYDROCHLORIC ACID (to 71, c). a. Recently precipitated pure barium silico-fluoride was digested with frequent agitation for 3 weeks with cold water acidified with hydrochloric acid. The filtrate gave with sulphuric acid a rather copious precipitate. 84'82 grm. left 01155 grm. of thoroughly dried residue, which, calculated as barium silico- fluoride, gives 733 parts of fluid to 1 part of that salt. b. Recently precipitated pure barium silico-fluoride was mixed with water very slightly acidified with hydrochloric acid, and the mixture heated to boiling. Cooled to 12, 84-82 grm. of the filtrate left a residue of 0*1322 grm., which gives 640 parts of fluid to 1 part of the salt. N.B. The solution of barium silico-fluoride in hydrochloric acid is not effected without decomposition; at least, the residue contained, even after ignition, a rather large proportion of barium chloride. 21. SOLUBILITY OF STRONTIUM SULPHATE IN WATER (to 72, a). a. In Water of 14. 84 '82 grm. of a solution prepared by 4 days' digestion of recently precipitated strontium sulphate with water at the common temperature, left 0'0123 grm. of strontium sulphate. One part of strontium sulphate dissolves consequently in 6895 parts of water. b. In Water of 100. 84 '82 grm. of a solution prepared by boiling recently precipitated strontium sulphate several hours with water, left 0'0088 grm. Consequently 1 part of strontium sulphate dissolves in 9638 parts of boiling water. 22. SOLUBILITY OF STRONTIUM SULPHATE IN WATER CONTAINING HYDRO- CHLORIC ACID AND SULPHURIC ACID (to 72, a). a. 84'82 grm. of a solution prepared by 3 days' digestion, left 0'0077 grm. SrSO 4 . b. 42-41 grm. of a solution prepared by 4 days' digestion, left 0-0036 grm. c. Pure strontium carbonate was dissolved in an excess of hydrochloric acid, and the solution precipitated with an excess of sulphuric acid and then allowed to stand in the cold for a fortnight. 84*82 grm. of the filtrate left 0'0066 grm. ANALYTICAL EXPERIMENTS. 815 In a. I part of SrSO 4 required 11016 parts. b. 1 " ". 11780 " c. 1 " " 12791 " Mean 11862 parts. 23. SOLUBILITY OF STRONTIUM SULPHATE IN DILUTE NITRIC Aero, HYDRO- CHLORIC ACID, AND ACETIC ACID (to 72, a). a. Recently precipitated pure strontium sulphate was digested for 2 days in the cold with nitric acid of 4*8 per cent. 150 gun. of the nitrate left 0*3431 grm. One part of the salt required accordingly 435 parts of the dilute acid for its solution ; in another experiment i part of the salt was found to require 429 parts of the dilute acid. Mean, 432 parts. b. The same. salt was digested for 2 days in the cold with hydrochloric acid 'of 8*5 per cent. 100 grm. left 0*2115, and in another experiment, 0'2104grm. One part of the salt requires, accordingly, in the mean, 474 parts of hydrochloric acid of 8*5 per cent, for its solution. c. The same salt was digested for 2 days in the cold with acetic acid of 15 '6 per cent. C 2 H 4 O 2 . 100 gnn. left 0*0126, and in another experiment, 0*0129 grm. One part of the salt requires, accordingly, in the mean, 7843 parts of acetic acid of 15*6 per cent. 24. SOLUBILITY OF STRONTIUM CARBONATE m COLD WATER (to 72, b). Recently precipitated, thoroughly washed strontium carbonate was digested several days with cold distilled water, with frequent shaking. 84*82 grm. of the filtrate left, upon evaporation, a residue weighing, after ignition, 0*0047 grni. One part of strontium carbonate requires therefore 18045 parts of water for its solution. 25. SOLUBILITY OF STRONTIUM CARBONATE IN WATER CONTAINING AMMONIA. AND AMMONIUM CARBONATE (to 72, b). Recently precipitated, thoroughly washed strontium carbonate was digested for 4 weeks with cold water containing ammonia and ammonium carbonate, with frequent shaking. 84*82 grm. of the filtrate left 0*0015 grm. SrCO 3 . Consequently, 1 part of the salt requires 56545 parts of this fluid for its solution. If solution of strontium chloride is precipitated with ammonium carbonate and ammonia as directed 102, 2, a, sulphuric acid produces no turbidity in the filtrate, after addition of alcohol. 26. SOLUBILITY OF CALCIUM CARBONATE LN COLD AND IN BOILING WATER (to 73, b). a. A solution prepared by boiling as in 26, b, was digested in the cold for 4 weeks, with frequent agitation, with the undissolved precipitate. 84*82 grm. left 0*0080 CaCO 3 . One part therefore required 10601 parts. b. Recently precipitated calcium carbonate was boiled for some time with distilled water. 42*41 grm. of the filtrate left, upon evaporation and gentle ignition of the residue, 0*0048 CaCO 3 . One part requires consequently 8834 parts of boiling water. S16 ANALYTICAL EXPERIMENTS. 27. SOLUBILITY OF CACO 3 IN WATER CONTAINING AMMONIA AND AMMO- NIUM CARBONATE (to 73, b). Pure dilute solution of calcium chloride was precipitated with ammonium carbonate and ammonia, allowed to stand 24 hours, and then filtered. 84 '82 grm. left 0*0013 grm. Ca CO 3 . One part requires consequently 65246 parts. 28. DEPORTMENT OF CALCIUM CARBONATE UPON IGNITION IN A PLATINUM CRUCIBLE (to 73, b). 0'7955 grm. of perfectly dry calcium carbonate was exposed, in a small and thin platinum crucible, to the gradually increased and finally most intense heat of a good BERZELIUS' lamp. The crucible was open and placed obliquely. After the first 15 minutes the mass weighed 0'6482 after half an hour 0'6256 after one hour 0*5927, which latter weight remained unaltered after 15 minutes' additional heating. This corresponds to 74 '5 per cent., whilst the proportion of CaO in the carbonate is calculated at 56 per cent. ; there remained therefore evidently still a considerable amount of the carbonic acid. 29. COMPOSITION OF CALCIUM OXALATE DRIED AT 100 (to 73, c). 0'8510 grm. of thoroughly dry pure calcium carbonate was dissolved in hydrochloric acid; the solution was precipitated with ammonium oxalate and ammonia, and the precipitate collected upon a weighed filter and dried at 100, until the weight remained constant. The calcium oxalate so produced weighed 1 -2461 grm. Calculating this as CaC 2 O 4 + H 2 O, the amount found contained 0-4772 CaO, which corresponds to 56 '07 per cent, in the calcium carbonate; the calculated proportion of CaO in the latter is 56 per cent. 30. DEPORTMENT OF MAGNESIUM SULPHATE IN THE AIR AND UPON IGNI- TION (to 74, a). 0'8135 grm. of perfectly pure anhydrous MgSO 4 in a covered platinum crucible acquired, on a fine and warm day in June, in half an hour, an increase of weight of 0'004 grm., and in the course of 12 hours, of 0'067 grm. The salt could not be accurately weighed in the open crucible, owing to continual increase of weight. 0'8135 grm., exposed for some time to a very moderate red heat, suffered no diminution of weight ; but after 5 minutes' exposure to an intense red heat, the substance was found to have lost 0'0075 grm'. , and the residue gave no longer a clear solution with water. About 0'2 grm. of pure magnesium sulphate exposed in a small platinum crucible, for 15 to 20 minutes, to the heat of a powerful blast gas lamp, gave, with dilute hydrochloric acid, a solution in which barium chloride failed to produce the least turbidity. 31. SOLUBILITY OF AMMONIUM MAGNESIUM PHOSPHATE IN PURE WATER (to 74, ft). a. Recently precipitated ammonium magnesium phosphate was thoroughly washed with water, then digested for 24 hours with water of about 15, with frequent shaking. 84-42 grm. of the filtrate left . . ; 0'0047 grm. of magnesium pyrophosphate. ANALYTICAL EXPERIMENTS. 817 b. The same precipitate was digested in the same manner for 72 hours. 84-42 grm. of the filtrate left 0-0043 " Mean 0'0045 " which corresponds to 0*00552 grm. of the anhydrous double salt. One part of that salt dissolves therefore in 15293 parts of pure water. The cold saturated solution gave, with ammonia, after the lapse of a short time, a distinctly perceptible crystalline precipitate; on the addition of sodium phosphate, it remained perfectly clear, and even after the lapse of 2 days no precipitate had formed; ammonium sodium phosphate produced a precipitate as large as that by ammonia. 32. SOLUBILITY OF AMMONIUM MAGNESIUM PHOSPHATE IN WATER CON- TAINING AMMONIA (to 74, b). a. Pure ammonium magnesium phosphate was dissolved in the least possible amount of nitric acid ; a large quantity of water was added to the solution, then ammonia in excess. The mixture was allowed to stand at rest for 24 hours, then filtered; its temperature was 14. 84 '42 grm. left O'OOIS magnesium pyro- phosphate, which corresponds to '00184 of the anhydrous double salt. Conse- quently 1 part of the latter requires 45880 parts of ammoniated water for its solution. b. Pure ammonium magnesium phosphate was digested for 4 weeks with ammoniated water, with frequent shaking; the fluid (temperature 14) was then filtered off; 126 '63 grm. left 0'0024 magnesium pyrophosphate, which corresponds to 0-00296 of the double salt. One part of it therefore dissolves in 42780 parts of ammoniated water. Taking the mean of a and b, 1 part of the double salt requires 44330 parts of ammoniated water for its solution. 33. ANOTHER EXPERIMENT ON THE $AME SUBJECT (to 74, b). Recently precipitated ammonium magnesium phosphate, most carefully washed with water containing ammonia, was dissolved in water acidified with hydrochloric acid, ammonia added in excess, and allowed to stand in the cold for 24 hours. 169 -64 grm. of the filtrate left 0'0031 magnesium pyrophosphate, corresponding to 0'0038 of anhydrous ammonium magnesium phosphate. One part of the double salt required therefore 44600 parts of the fluid. 34. SOLUBILITY OF AMMONIUM MAGNESIUM PHOSPHATE m WATER CON- TAINING AMMONIUM CHLORIDE (to* 74, b). Recently precipitated, thoroughly washed ammonium magnesium phosphate was digested in the cold with a solution of 1 part of ammonium chloride in 5 parts of water. 18 '4945 grm. of the filtrate left "002 magnesium pyrophosphate, which corresponds to '00245 of the double salt. One part of the salt dissolves therefore in 7548 parts of the fluid. 35. SOLUBILITY OF AMMONIUM MAGNESIUM PHOSPHATE IN WATER CON- TAINING AMMONIA AND AMMONIUM CHLORIDE (to 74, 6). Recently precipitated, thoroughly washed ammonium magnesium phosphate was digested in the cold with a solution of 1 part of ammonium chloride in 7 parts of ammoniated water. 23 1283 grm. of the filtrate left 0'0012 magnesium 818 ANALYTICAL EXPERIMENTS. pyrophosphate, which corresponds to '00148 of the double salt. One part of the double salt requires consequently 15627 parts of the fluid for its solution. 36. DEPORTMENT OF ACID SOLUTIONS of MAGNESIUM PYROPHOSPHATE WITH AMMONIA (to 74, c). 0'3985 grm. magnesium pyrophosphate was treated for several hours, at a high temperature, with concentrated sulphuric acid. This exercised no perceptible action. It was only after the addition of some water that the salt dissolved. The fluid, heated for some time, gave, upon addition of ammonia in excess, a crystalline precipitate, which was filtered off after 18 hours; the quantity of magnesium pyrophosphate obtained was 0'3805 grm., that is, 95 '48 per cent. Sodium phosphate produced in the filtrate a trifling precipitate, which gave 0*0150 grm. of magnesium pyrophosphate, that is, 3*76 per cent. 0-3565 grm. magnesium pyrophosphate was dissolved in 3 grm. nitric acid, of 1-2 sp. gr. ; the solution was heated, diluted, and precipitated with ammonia: the quantity of magnesium pyrophosphate obtained amounted to 0'3485 grm., that is, 98 '42 per cent.; 0"4975 grm. was treated in the same manner with 7'6 grm. of the same nitric acid: the quantity re-obtained was 0'4935 grm., that is, 99 '19 per cent. 0'786 grm. treated in the same manner with 16 '2 grm. of nitric acid, gave Q'7765 grm., that is, 98'79 per cent. The result of these experiments may be tabulated thus: Proportion of Mg 2 P 2 O to nitric acid. Re-obtained. Loss. 1: 9 98-42 per cent. 1-58 1 : 15 99-19 " 0-81 1 : 20 98-79 " 1'21 37. SOLUBILITY OF PURE MAGNESIA IN WATER (to 74, d). a. In Cold Water. Perfectly pure well-crystallized magnesium sulphate was dissolved in water, and the solution precipitated with ammonium carbonate and caustic ammonia ; the precipitate was thoroughly washed in spite of which it still retained a per- ceptible trace of sulphuric acid then dissolved in pure nitric acid, an excess of acid being carefully avoided. The solution was then re-precipitated with ammo- nium carbonate and caustic ammonia, and the precipitate thoroughly washed. The so-prepared perfectly pure magnesium carbonate was ignited in a platinum crucible until the weight remained constant. The residuary pure magnesia was then digested in the cold for 24 hours with distilled water, with frequent shaking. The distilled water used was perfectly free from chlorine, and left no fixed residue upon evaporation. a. 84*82 grm. of the filtrate, cautiously evaporated in a platinum dish, left a residue weighing, after ignition, 0*0015 grm. One part of the pure magnesia dissolved therefore in 56546 parts of cold water. The digestion was continued for 48 hours longer, when (3. 84-82 grm. left 0'0016 grm. One part required therefore 53012 y. 84-82 grm. left 0-0015 grm. One part required 56546 Average 55368 ANALYTICAL EXPERIMENTS. 819 The solution of magnesia prepared in the cold way has a feeble yet distinct alkaline reaction, which is most easily perceived upon the addition of very faintly reddened tincture of Jitmus; the alkaline reaction of the solution is perfectly manifest also with slightly reddened litmus paper, or with turmeric or dahlia paper, if these test-papers are left for some time in contact with the solution. Alkali carbonates fail to render the solution turbid, even upon boiling. Sodium phosphate also fails to impair the clearness of the solution, but if the fluid is mixed with a little ammonia and shaken, it speedily becomes turbid, and deposits after some time a perceptible precipitate of ammonium magnesium phosphate. b. In Hot Water. Upon boiling pure magnesia with water, a solution is obtained which com- ports itself in every respect like the cold-prepared solution of magnesia. A hot-prepared solution of magnesia does not become turbid upon cooling, nor does a cold-prepared solution upon boiling. 84*82 grm. of hot-prepared solution of magnesia left 0'0016 grm. MgO. 38. SOLUBILITY OP PURE MAGNESIA IN SOLUTIONS OF POTASSIUM CHLORIDE AND SODIUM CHLORIDE (to 74, d). 3 flasks of equal size were charged as follows : 1. With 1 grm. pure potassium chloride, 200 c.c. water and some perfectly pure magnesia. 2. With 1 grm. pure sodium chloride, 200 c.c. water and some pure magnesia. 3. With 200 c.c. water and some pure magnesia. The contents of the 3 flasks were kept boiling for 40 minutes, then filtered, and the clear filtrates mixed with equal quantities of a mixture of sodium phosphate, ammonium chloride and ammonia. After 12 hours a very slight precipitation was visible in 3, and a considerably larger precipitation had taken place in 1 and 2. 39. PRECIPITATION OP ALUMINIUM BY AMMONIA. ETC. (to 75, a). a. Ammonia produces in neutral solutions of aluminium salts or of alum, as is well known, a gelatinous precipitate of aluminium hydroxide. Upon further addition of ammonia in considerable excess, the precipitate redissolves gradually, but not completely. b. If a drop of a dilute solution of alum is added to a copious amount of ammonia, and the mixture shaken, the solution appears almost perfectly clear; however, after standing at rest for some time, slight flakes separate. c. If a solution of aluminium, mixed with a large amount of ammonia, is filtered, and . The filtrate boiled for a considerable time, flakes of aluminium hydroxide separate gradually in proportion as the excess of ammonia escapes. ft. The filtrate mixed with solution of ammonium chloride, a very percep- tible flocculent precipitate of aluminium hydroxide separates immediately; the whole of the aluminium present in the solution will thus separate if the ammonium chloride be added in sufficient quantity. y. The filtrate mixed with ammonium sesquicarbonate, the same reaction takes place as in ft. 820 ANALYTICAL EXPERIMENTS. 8. The filtrate mixed with solution of sodium chloride or of potassium , chloride, no precipitate separates, but, after several days' standing, slight flakes of aluminium hydroxide subside, owing to the loss of ammonia by evaporation. d. If a neutral solution of aluminium is precipitated with ammonium car bonate, or if a solution strongly acidified with hydrochloric or nitric acid is precipitated with pure ammonia, or if to a neutral solution a sufficient amount of ammonium chloride is added besides the ammonia; even a considerable excess of the precipitants will fail to redissolve the precipitated aluminium hydroxide, as appears from the continued perfect clearness of the filtrates upon protracted boiling and evaporation. 40. PRECIPITATION OP ALUMINIUM BY AMMONIUM SULPHIDE (to 75, a). (Experiments made by Mr. J. FUCHS, formerly Assistant in my Laboratory.) a. 50 c.c. of a solution of pure ammonium-alum, which contained 0'3939 A1 2 O 3 , were mixed with 50 c.c. water and 10 c.c. solution of ammonium sulphide, and filtered after ten minutes. The ignited precipitate weighed 0-3825 grm. b. The same experiment was repeated with 100 c.c. water; the precipitate weighed 0-3759 grm. c. The same experimeut was repeated with 200 c.c. water; the precipitate weighed 0*3642 grm. 41. PRECIPITATION OF CHROMIUM BY AMMONIA (to 76, a). Solutions of chromic chloride and of chrome-alum (concentrated and dilute, neutral and acidified with hydrochloric acid) were mixed with ammonia in excess. All the filtrates drawn off immediately after precipitation appeared red, but when filtered after ebullition, they all appeared colorless, if the ebullition had been sufficiently protracted. 42. SOLUBILITY OF THE BASIC ZINC CARBONATE IN WATER (to 77, a). Perfect^ pure, recently (hot) precipitated basic zinc carbonate was gently 'heated with distilled water, and subsequently digested cold for many weeks, with frequent shaking. The clear solution gave no precipitate with ammonium sulphide, not even after long standing. 84-82 grm. left 0'0014 grm. zinc oxide, which corresponds to 0'0019 basic zinc carbonate (74 per cent, of ZnO being assumed in this salt). One part of the basic carbonate requires therefore 44642 parts of water for solution. IN EACH OF THE THREE FOLLOWING NUMBERS THE SULPHIDE WAS PRECIPI- tated from the solution of the normal salt with addition of ammonium chloride by yellow ammonium sulphide, and allowed to stand in a closed vessel. After 24 hours the clear fluid was poured on to 6 filters of equal size, and the precipitate was then equally distributed among them. The washing was at once commenced and continued, without interruption, the following fluids being used: I. Pure water. II. Water containing hydrogen sulphide. III. Water containing ammonium sulphide. IV. Water containing ammonium chloride, afterwards pure water. ANALYTICAL EXPERIMENTS. 821 V. Water containing hydrogen sulphide and ammonium chloride, after- wards water containing hydrogen sulphide. VI. Water containing ammonium sulphide and ammonium chloride, after- wards water containing ammonium sulphide. 43. DEPORTMENT OF ZINC SULPHIDE ON WASHING (to 77, c). The filtrates were at first colorless and clear. On washing, the first three filtrates ran through turbid, the turbidity was strongest in II. and weakest in III. ; the last three remained quite clear. On adding ammonium sulphide no change took place; the turbidity of the first three was not increased, the clearness of the last three was not impaired. Ammonium chloride therefore decidedly exercises a favorable action, and the water containing it may be displaced by water containing ammonium sulphide. 44. DEPORTMENT OP MANGANESE SULPHIDE ON WASHING (to 78, e). The filtrates were at first clear and colorless. But after the washing had been continued some time, I. appeared colorless, slightly opalescent; II. whitish and turbid; III. yellowish and turbid; IV. colorless, slightly turbid; V. slightly yellowish, nearly clear; VI. clear, yellowish. To obtain a filtrate that remains clear, therefore, the wash-water must at first contain ammonium chloride. Addition of ammonium sulphide also cannot be dispensed with, as all the filtrates obtained without this addition gave distinct precipitates of manganese sulphide when the reagent was subsequently added to them. 45. DEPORTMENT OP NICKEL SULPHIDE (ALSO OP COBALT SULPHIDE AND FERROUS SULPHIDE) ON WASHING (to 79, e). In the experiments with nickel sulphide the clear filtrates were put aside, and then the washing was proceeded with. The washings of the first 3 ran through turbid, of the last three clear. When the washing was finished, I. was colorless and clear; II. blackish and clear; III. dirty yellow and clear; IV. colorless and clear; V. slightly opalescent; VI. slightly brownish and opal- escent. On addition of ammonium sulphide, I. became brown; II. remained unaltered; III. remained unaltered; IV. became black and opaque; V. became brown and clear; VI. became pure yellow and clear. Cobalt sulphide and ferrous sulphide behaved in an exactly similar manner. It is plain that these sulphides oxidize more rapidly when the wash-water con- tains ammonium chloride, unless ammonium sulphide is also present. Hence it is necessary to wash with a fluid containing ammonium sulphide; and the addition of ammonium chloride at first is much to be recommended, as this diminishes the likelihood of our obtaining a muddy filtrate. 46. DEPORTMENT OP COBALTOUS HYDROXIDE PRECIPITATED BY ALKALIES (to 80, a}. A. solution of cobaltous chloride was precipitated boiling with solution of soda, and the precipitate washed with boiling water until the filtrate gave no longer the least indication of presence of chlorine. The dried and ignited residue, heated with water, manifested no alkaline reaction. It was reduced by ignition in hydrogen gas, and the metallic cobalt digested hot with water. The decanted water manifested no alkaline reaction, even after considerable con- centration ; but the metallic cobalt, brought into contact, moist, with turmeric paper, imparted to the latter a strong brown color. '822 ANALYTICAL EXPERIMENTS. 47. SOLUBILITY OF LEAD CARBONATE (to 83, a). a. In pure Water. ' Recently precipitated and thoroughly washed pure lead carbonate was digested for 8 days with water at the common temperature, with frequent shaking. 84 '42 grm. of the filtrate were evaporated, with addition of some pure sulphuric acid; the residuary lead sulphate weighed 0'0019 grm., which corresponds to '00167 lead carbonate. One part of the latter salt dissolves therefore in 50551 parts of water. The solution, mixed with hydrogen sulphide water, remained perfectly colorless, not the least tint being detected in it, even upon looking through it from the top of the test-cylinder. b. In Water containing a little Ammonium Acetate and also Ammonium Carbonate and Ammonia. A highly dilute solution of pure lead acetate was mixed with ammonium carbonate and ammonia in excess, and the mixture gently heated and then allowed to stand at rest for several days. 84'42 grm. of the filtrate left, upon evaporation with a little sulphuric acid, 0'0041 grm. lead sulphate, which corresponds to 0'0036 of the carbonate. One part of the latter salt requires accordingly 23450 parts of the above fluid for solution. The solution was mixed with hydrogen sulphide water; when looking through the fluid from the top of the test-cylinder, a distinct coloration was visible; but when looking through the cylinder laterally, this coloration was hardly perceptible. Traces of lead sulphide separated after the lapse of some time. c. In Water containing a large propoi'tion of Ammonium Nitrate, together with Ammonium Carbonate and Caustic Ammonia. A highly dilute solution of lead acetate was mixed with nitric acid, then with ammonium carbonate and ammonia in excess; the mixture was gently heated, and allowed to stand at rest for 8 days. The filtrate, mixed with hydrogen sulphide, exhibited a very distinct brownish color upon looking through it from the top of the cylinder; but this color appeared very slight only when looking through the cylinder laterally. The amount of lead dissolved was unquestionably more considerable than in b. 48. SOLUBILITY OF LEAD OXALATE (to 83, b). A dilute solution of lead acetate was precipitated with ammonium oxalate and ammonia, the mixture allowed to stand at rest for some time, and then filtered. The filtrate, mixed with hydrogen sulphide, comported itself exactly like the filtrate of No. 47, b. The same deportment was observed in another similar experiment, in which ammonium nitrate had been added to the solution. 49. SOLUBILITY OF LEAD SULPHATE IN PURE WATER (to 83, d). Thoroughly washed and still moist lead sulphate was digested for 5 days with water, at 10 15, with frequent shaking. 84 '42 grm. of the filtrate (filtered off at 11) left 0-0037 grm. lead sulphate. Consequently 1 part of this salt requires 22816 parts of pure water of 11 for solution. The solution, mixed with hydrogen sulphide, exhibited a distinct brown color when viewed from the top of the cylinder, but this color appeared very slight upon looking through the cylinder laterally. ANALYTICAL EXPERIMENTS. 823 50. SOLUBILITY OF LEAD SULPHATE IN WATER CONTAINING SULPHURIC Acm (to 83, d). A highly dilute solution of lead acetate was mixed with an excess of dilute pure sulphuric acid; the mixture was very gently heated, and the precipitate allowed several days to subside. 80 '31 grm. of the filtrate left 0'0022 grm. lead sulphate. One part of this salt dissolves therefore in 36504 parts of water con- . taining sulphuric acid. The solution, mixed with hydrogen sulphide, appeared colorless to the eye looking through the cylinder laterally, and very little darker when viewed from the top of the cylinder. 51. SOLUBILITY OF LEAD SULPHATE IN WATER CONTAINING AMMONIUM SALTS AND FREE SULPHURIC ACID (to 83, d ). A highly dilute solution of lead acetate was mixed with a tolerably large amount of ammonium nitrate, and sulphuric acid in excess added. After several days' standing, the mixture was filtered. The filtrate was nearly indifferent to hydrogen sulphide water; viewed from the top of the cylinder, it looked hardly perceptibly darker than pure water. 52. DEPORTMENT OF LEAD SULPHATE UPON IGNITION (to 83, d). Speaking of the determination of the atomic weight of sulphur, ERDMANN and MARCHAND* state that lead sulphate loses some sulphuric acid upon ignition. In order to inform myself of the extent of this loss, and to ascertain how far it might impair the accuracy of the method of determining lead as a sulphate, I heated 2 '2151 grm. of absolutely pure PbSo* to the most intense redness, over a spirit-lamp with double draught, I could not perceive the slightest decrease of weight; at all events, the loss did not amount to '0001 grm. 53. DEPORTMENT OF LEAD SULPHIDE ON DRYING AT 100 (to 83, /). Lead sulphide was precipitated from a solution of pure lead acetate with hydrogen sulphide, and when dry, kept for a considerable time at 100 and weighed occasionally. The following numbers represent the results of the several weighings : I. 0-8154. II. 0-8164. III. 0'8313. IV. 0'8460. V. 0'864 54. DEPORTMENT OF METALLIC MERCURY AT THE COMMON TEMPERATURE AND UPON EBULLITION WITH WATER (to 84, a). To ascertain in what manner loss of metallic mercury occurs upon drying, and likewise upon boiling with water, and to determine which is the best method of drying, I made the following experiments: I treated 6'4418 grm. of perfectly pure mercury in a watch-glass, with dis- tilled water, removed the water again as far as practicable (by decantation and finally by means of blotting-paper), and weighed. I now had 6 '4412 grm. After several hours' exposure to the air, the mercury was reduced to 6 '4411. I placed these 6-4411 grm. under a bell- jar over sulphuric acid, the temperature being about 17. After the lapse of 24 hours the weight had not altered in the least. I introduced the 6*4411 grm. mercury into a flask, treated it with a copious quantity of distilled water, and boiled for 15 minutes violently. I then placed the mercury again upon the watch-glass, dried it most carefully with blotting - * Journ. fur Prakt. Chem. 31, 385. 824 ANALYTICAL EXPERIMENTS. paper, and weighed. The weight was now 6 '4402 grm. Finding that a trace of mercury had adhered to the paper, I repeated the same experiment with the 6*4402 grin. After 15 minutes' boiling with water, the mercury had again lost 0'0004 grm. The remaining 6'4398grm. were exposed to the air for 6 days (in summer, during very hot weather), after which they were found to have lost only 0-0005 grm. 55. DEPORTMENT OF MERCURIC SULPHIDE WITH SOLUTION OF POTASSA, AMMONIUM SULPHIDE, ETC. (to 84, c). a. If recently precipitated pure mercuric sulphide is boiled with pure solu- tion of potassa, not a trace of it dissolves in that fluid; hydrochloric acid produces no precipitate, nor even the least coloration, in the filtrate. b. If mercuric sulphide is boiled with solution of potassa, with addition of some hydrogen sulphide water, ammonium sulphide, or sulphur, complete solution is effected. c. If freshly precipitated mercuric sulphide is digested in the cold with yellowish or very yellow ammonium sulphide, slight but distinctly perceptible traces are dissolved, while in the case of hot digestion scarcely any traces of mercury can be detected in the solution.* d. Thoroughly washed mercuric sulphide, moistened with water, suffers no alteration upon exposure to the air ; at least, the fluid which I obtained by washing mercuric sulphide which had been thus exposed for 24 hours, did not manifest acid reaction, nor did it contain mercury or sulphuric acid. 56. DEPORTMENT OF CUPRIC OXIDE UPON IGNITION (to 85, b). Pure cupric oxide (prepared from cupric nitrate) was ignited in a platinum crucible, then cooled under a bell-jar over sulphuric acid, and finally weighed. The weight was 3 '542 grm. The oxide was then most intensely ignited for 5 minutes, over a BERZELIUS' lamp, and weighed as before, when the weight was found unaltered; the oxide was then once more ignited for 5 minutes, but with the same result. 57. DEPORTMENT OF CUPRIC OXIDE IN THE AIR (to 85, b}. A platinum crucible containing 4*3921 grm. of gently ignited cupric oxide (prepared from the nitrate) stood for 10 minutes, covered with the lid, in a warm room (in winter); the weight of the oxide was found to have increased to 4-3939 grm. The oxide was then intensely ignited over a spirit-lamp ; after 10 minutes' standing in the covered crucible, the weight had not perceptibly increased r after 24 hours' it had increased by 0*0036 grm. N 58. DEPORTMENT OF BISMUTH SULPHIDE UPON DRYING AT 100 (to 86, g).. 4558 grm. of bismuth sulphide prepared in the wet w T ay were placed in the desiccator on a watch-glass, and allowed to stand at the common tempera- ture. After 3 hours the weight was 0'4270, after 6 hours 0*4258, after 2 days- the same. 0*3602 grm. of the bismuth sulphide so dried was put into a water-bath, in 15 minutes it weighed 0*3596, half an hour afterwards 0'3599, in half an hour * Comp. my experiments in the Zeitschrift f. Anal. Chem. 3, 140. ANALYTICAL EXPERIMENTS. 825 more 0-3603, in two hours 0'3626. In a second experiment the drying was kept up for 4 days, and a continual increase of weight was observed. 0-5081 grm. of bismuth sulphide dried in the desiccator was heated in a boat iii a stream of carbonic acid. After gentle ignition the weight was 0'5002, after repeated heating 0'4992. The bismuth sulphide was visibly volatilized on ignition in the current of carbonic acid. 59. DEPORTMENT OF CADMIUM SULPHIDE WITH AMMONIA, ETC. (to 87, c). Recently precipitated pure cadmium sulphide was diffused through water, and the following experiments were made with the mixture : a. A portion was'digested cold with ammonia in excess, and filtered. The nitrate remained perfectly clear upon addition of hydrochloric acid. b. Another portion was digested hot with excess of ammonia, and filtered. This filtrate likewise remained perfectly clear upon addition of hydrochloric acid. c. Another portion was digested for some time with solution of potassium cyanide, and filtered. This filtrate also remained perfectly clear upon addition of hydrochloric acid. d. Another portion was digested with ammonium hydrosulphide, and filtered. The turbidity which hydrochloric acid imparted to this filtrate was pure white. (A remark made by WACKENRODER, in BUCHNER'S Repertor. d. Pharm., xlvi. 226, induced me to make these experiments.) 60. DEPORTMENT OF PRECIPITATED ANTIMONIOUS SULPHIDE ON DRYING (to 90, a). 0-2899 grm. of pure precipitated antimonious sulphide dried in the desiccator lost, when dried at 100, O'OOOT. 0*4457 grm. of the substance dried at 100 lost, when heated to blackening in a stream of carbonic acid, 0*0011 water. 0-1932 grm. of the substance dried at 100 gave up 0*0012, when heated to blackening in a stream of carbonic acid, and after stronger heating, during which fumes of antimony sulphide began to escape, the total loss amounted to 0-0022 grm. 0-1670 grm. of the substance dried at 100 lost O'OOOS grm. on being heated to blackening in a stream of carbonic acid. 61. AMOUNT OF WATER IN HYDRATED SILICA (to 93, 9). (Experiments made by my assistant, Mr. LIPPERT.) A dilute solution of soluble glass was slowly dropped into hydrochloric acid, as long as the precipitate continued to dissolve rapidly, then the clear fluid was heated in the water-bath, till it set to a transparent jelly. This jelly was dried as far as possible with blotting paper, diffused in water, and washed by decan- tation till the fluid altogether ceased to give the chlorine reaction. It was then transferred to a filter, and the latter spread on blotting paper and exposed till a crumbly mass was left from the spontaneous evaporation of water. One half (I.) was dried for 8 weeks in the desiccator over sulphuric acid, with occasional trituration, the other half (II.) was dried under similar circumstances, but in a vacuum. Both were transferred to closed tubes and these were kept in the desiccator. 826 ANALYTICAL EXPERIMENTS. The weighing of the substance dried at 100 was effected between watch glasses. For the purpose of igniting the residue, it was allowed to satiate itself with aqueous vapor by exposure to the air, otherwise a considerable quantity of the substance would have been lost, then water was dropped upon it in the watch-glass, then it was rinsed into a platinum crucible, dried in a water-bath, and ignited, at first cautiously, towards the end intensely. The substance I. contained Expt. i. Expt. 2. Water, escaping at or below 100 4*19 ^ q.no above 100 4*76 i Silica.. . 91-05 90-72 100-00 100-00 Consequently the hydrate dried at 100 consists of 4'97 water and 95 -03 silica. In the substance dried in the desiccator the oxygen of the total water : the oxygen of the silica (SiO 2 ), according to the first experiment : : 1 : 6*1, according to the second experiment : : 1 : 5 "86. And in the substance dried at 100 the oxygen of the water : the oxygen of the silica : : 1 : 11 '5. The substance II. contained Expt. 1. Expt. 2. Expt. 3. Water, escaping at or below 100 4'75 4'71 above 100 5*26 5 "21 Silica.. . 89-99 90'08 90'05 100-00 100-00 100-00 Consequently the hydrate dried at 100 consists on the average of 5 '49 water and 94*51 silica. In the substance dried in a vacuum over sulphuric acid the oxygen of the total water : the oxygen of the silica on an average : : 1 : 5'41. And in the substance dried at 100 the oxygen of the water : the oxygen of the .silica : : 1 : 10 '43. 62. DETERMINATION OF BARIUM BY PRECIPITATION WITH AMMONIUM CAR- BONATE (to 101, 2, a). 0*7553 grm. pure ignited barium chloride precipitated after 101, 2, a, gave 0-7142 BaCO 3 , which corresponds to 0'554719 BaO = 73'44 per cent. (100 parts of BaCl 2 ought to have given 73'59 parts). The result accordingly was 99 '79 instead of 100. 63. DETERMINATION OP BARIUM IN ORGANIC SALTS (to 101, 2, ft). 0'686 grm. barium racemate, treated according to 101, 2, b, gave 0*408 barium carbonate - 0'3169 BaO = 46'20 per cent, (calculated 46*38 percent.); i.e., 99*61 instead of 100. 64. DETERMINATION OF STRONTIUM AS STRONTIUM SULPHATE (to 102, 1, a). a. An aqueous solution of 1-2398 grm. SrCl 2 was precipitated with sulphuric acid in excess, and the precipitated strontium sulphate washed with water. It weighed 1-4113, which corresponds to 0'795408 SrO = 64*15 per cent, (calculated 65-38 per cent.); i.e., 98'12 instead of 100. b. 1 -1510 grm. SrCo 3 was dissolved in excess of hydrochloric acid, the sola- ANALYTICAL KXPKRI.M KNTS. 827 tion diluted, and then precipitated with sulphuric acid; the precipitated SrSO 4 was washed with water; it weighed 1*4024 = 0*79039 SrO = 68'68 per cent, (calculated 70 '07 per cent.); i.e., 98.02 instead of 100. 65. DETERMINATION OF STRONTIUM AS SULPHATE, WITH CORRECTION (to 102, 1, a). ^hQ filtrate obtained hi No. 64, b, weighed 190*84 grm. According to experi- ment No. 22, 11862 parts of water containing sulphuric acid dissolve 1 part of strontium sulphate; therefore, 190*84 grm.' dissolve 0*0161. The washing* weighed 63 '61 grm. According to experiment No. 21, 6895 parts of water dissolve 1 part of SrSO; therefore, 63*61 grm. dissolve 0*0092 grm. Adding 0*0161 and 0-0092 to the 1*4024 actually obtained, we find the total amount = 1*4277 grm., which corresponds to 0*80465 SrO = 69*91 per cent, in SrCO 3 (calculated 70 '07 per cent.); i.e., 99*77 instead of 100. 66. DETERMINATION OF STRONTIUM AS STRONTIUM CARBONATE (to 102, 2). 1*3104 grm. strontium chloride, precipitated according to 102, 2, gave 1*2204 SrCO 3 , containing 8551831 SrO = 65*26 per cent, (calculated 65*38); i.e., 99*82 instead of 100. IN THE FOUR FOLLOWING EXPERIMENTS, AND ALSO IN No. 72, PURE AIR- dried calcium carbonate was used, in a portion of which the amount of anhydrous carbonate had been determined by very cautious heating. 0*7647 grm. left 0*7581 grm., which weight remained unaltered upon further (extremely gentle) ignition; the air-dried carbonate contained accordingly 55 '516 per cent, of lime. 67. DETERMINATION OF CALCIUM AS CALCIUM SULPHATE BY PRECIPITATION (to g 103, 1, a). 1*186 grin, of "the air dried calcium carbonate" was dissolved in hydro- chloric acid, and the solution precipitated with sulphuric acid and alcohol, after 103, 1, a. Obtained 1*5949 grm. CaSO 4 , containing 0*65598 CaO, i.e., 55*31 per cent, (calculated 55*51), which gives 99*64 instead of 100. 68. DETERMINATION OF CALCIUM AS CaCO 3 , BY PRECIPITATION WITH AMMONIUM CARBONATE AND WASHING WITH PURE WATER (to 103, 2, a). A hydrochloric acid solution of 1*1437 grm. of "the air-dried calcium car- bonate" gave upon precipitation as directed, 1*1243 grin, anhydrous calcium carbonate, corresponding to 0*629608 CaO = 55*05 per cent, (calculated 55 "51 per cent.), which gives 99*17 instead of 100. 69. DETERMINATION OF CALCIUM AS CaCO 3 , BY PRECIPITATION WITH AMMO- NIUM OXALATE FROM ALKALINE SOLUTION (to 103, 2, b. a). 1*1734 grm. of "the air-dried calcium carbonate" dissolved in hydrochloric acid, and treated as directed 103, 2, b, a, gave 1*1632 grm. CaCO 3 (reaction not alkaline), containing 0*651392 of CaO = 55*513 per cent, (calculated 55*516 per cent.), which gives 99*99 instead of 100. 70. DETERMINATION OF CALCIUM AS OXALATE (to 103, 2, b, a). 0*857 grm. of "the air-dried calcium carbonate" were dissolved in hydro- chloric acid; the solution was precipitated with ammonium oxalate and 828 ANALYTICAL EXPERIMENTS. ammonia, the precipitate washed, and then dried at 100, until the weight remained constant, The precipitate (CaC 2 O 4 + H 2 O) weighed 1*2461 grm. con- taining G'477879 CaO 55*76 per cent, (calculated 55'516 per cent.), which gives 100-45 instead of 100. 71. VOLUMETRIC DETERMINATION OF CALCIUM PRECIPITATED AS OXALATE (to 103, 2, b, a). Six portions, of 10 c.c. each, were taken of a solution of pure calcium chloride ; in 2 portions the calcium was determined in the gravimetric way (by precipitation with ammonium oxalate, and weighing CaCO 3 ) ; in two by the alkalimetric method (p. 236), and in two by precipitation with ammonium oxalate, and estimation of the oxalic acid in the precipitate by solution of potas- sium permanganate. The following were the results obtained : a. In the gravimetric b By the alkalimetric c. By solution of potas- way. method. sium permanganate. 0*5617 CaCO 3 0'5614 0'5613 0-5620 " 0-5620 0'5620 72. DETERMINATION OF CALCIUM AS CaCO 3 BY PRECIPITATION AS CALCIUM OXALATE FROM ACID SOLUTION (to 103, 2, b, fi). 0*857 grm. of "the air-dried calcium carbonate" dissolved in hydrochloric acid and precipitated from this solution according to the directions of 103, 2, b, ft, gave 0'8476 calcium carbonate (which did not manifest alkaline reaction, and the weight of which did not vary in the least upon evaporation with ammonium carbonate), containing 0-474656 CaO = 55 -39 per cent, (calculated 55-51), which gives 99 '78 instead of 100. 73. DETERMINATION OF MAGNESIUM AS Mg 2 P 2 O 7 (to 104, 2). a. A solution of 1 -0587 grm. pure anhydrous magnesium sulphate in water, precipitated according to 104, 2, gave 0*9834 magnesium pyrophosphate, con- taining 0-35438 MgO = 33*476 per cent, (calculated 33'33 per cent.), which gives 100 -43 instead of 100. b. 0*9672 MgSO 4 gave 0*8974 Mg 2 P 2 O 7 = 33*43 per cent, of MgO (calculated 33*33, which gives 100-30 instead of 100. 74. PRECIPITATION OF ZINC ACETATE BY HYDROGEN SULPHIDE (to 108, b). a. A soluble of pure zinc acetate was treated with the gas in excess, allowed to stand at rest for some time, and then filtered. The filtrate was mixed with ammonia. It remained perfectly clear at first, and even after long standing a few hardly visible flakes only had separated. b. A solution of zinc acetate to which a tolerably large amount of acetic acid had been added previously to the precipitation with hydrogen sulphide, showed exactly the same deportment. 75. DETERMINATION OF IRON AS SULPHIDE (to 113, 2). 10 c.c. of a pure solution of ferric chloride was precipitated with ammonia; obtained 0*1453 Fe 2 O 3 = 0-10171 Fe. 10 c.c. was precipitated with ammonia and ammonium sulphide, and treated after 113, 2, obtained 0*1596 FeS 0*10157 Fe. 10 c.c. again yielded 0.1605 FeS = 0*1021 Fe. ANALYTICAL EXPERIMENTS. 829 76. DETERMINATION OF LEAD AS CHROMATE (to 116, 4). 1 '0083 grm. pure lead nitrate were treated according to 116, 4. The pre- cipitate was collected on a weighed filter, and dried at 100, obtained 0'9871 grm. = 0-67833 PbO. This gives 67 3 per cent. Calculation 67 '4. '9814 lead nitrate again yielded 0'9625 chromate = 67.4 per cent. 77. DETERMINATION OF MERCURY IN THE METALLIC STATE, IN THE WET WAY, BY MEANS OF STANNOUS CHLORIDE (to 118, 1, b). 2*01 grm. mercuric chloride gave 1*465 gnu. metallic mercury = 72 '88 per cent, (calculated 73 '83 per cent.), which gives 98 "71 instead of 100 (&CHAFFNER). The loss is not inherent in the method, i.e., it does not arise from mercury evaporating during the ebullition and desiccation (Expt. No. 54); but its origin lies in the fact that one usually does not allow sufficient time for the mercury to settle quite completely, and in general is not careful enough in decanting, and drying with paper, &c. 78. DETERMINATION OF COPPER BY PRECIPITATION WITH ZINC IN A PLA- TINUM DISH (to 119, 2). 30'882 grm. pure cupric sulphate were dissolved in water to 250 c.c.; 10 c.c. of the solution contained accordingly '31387 grm. metallic copper. a. 10 c.c. precipitated with zinc in a platinum dish, gave 0"3140 = 100 '06 per cent. b. In a second experiment 10 c.c. gave 0*3138 = 100 per cent. 80. DETERMINATION OF COPPER AS CUPROUS SULPHOCYANATE (to 119, 3, b). 0'5965 grm. of pure cupric sulphate was dissolved in a little water, and, after addition of an excess of sulphurous acid, precipitated with potassium sulphocy- anate. The well washed precipitate, dried at 100, weighed 0'2893, correspond- ing to 0-1892 CuO =31*72 percent. As cupric sulphate contains 31 '83 per cent., this gives 99'66 instead of 100. 81. DETERMINATION OF COPPER BY DE HAEN'S METHOD (to 119, 4, a). Four 10 c.c. -s of a solution of cupric sulphate, each 10 c.c., containing 0"0254 grm. Cu, were severally mixed with potassium iodide, then with 50 c.c. of a solution of sulphurous acid (50 c.c. corresponding to 12*94 c.c. iodine solution). After addition of starch paste, iodine solution was added until the fluid appeared blue. This required, In a, 4-09 b, 3-95 c, 4-06 d, 3-95 As 100 c.c. of iodine solution contained 0-58043 grrn. iodine, this gives For a, 0-0256 Cu instead of 0'0254 " b, 0-0260 " c, 0-0257 " d, 0-0260 Another experiment, made with 100 c.c. of the same solution of cupric sul- 830 ANALYTICAL EXPERIMENTS. phate, gave 0'2606 instead of 0*254 of copper. Ammonium nitrate having been added to 10 c.c. of the solution of cupric sulphate, then some dilute hydro- chloric acid, 3*4 and 3*5 c.c. of iodine solution were required instead of 4 c.c. a proof that considerably more iodine had separated than corresponded to the copper. 83. PRECIPITATION OF BISMUTH NITRATE BY AMMONIUM CARBONATE (to 120, 1, a). If a solution of bismuth nitrate, no matter whether containing much or little free nitric acid, is mixed with water, precipitated with ammonium carbonate and ammonia, and filtered without applying heat, the filtrate acquires, upon addition of hydrogen sulphide water, a blackish-brown color. But if the mixture before filtering is heated for a short time nearly to boiling, hydrogen sulphide fails to impart this color to the filtrate, or, at all events, the change of color is hardly visible to the eye looking through the full test-tube from the top. 84. DETERMINATION OP ANTIMONY AS SULPHIDE (to 125, 1). 0*559 grm. of pure air-dried tartar emetic, treated according to 125, 1, gave 0'2902 grm. antimonious sulphide dried at 100 = '2492 grm. or 44*58 per cent, of antimonious oxide. Heated to blackening in a current of carbonic acid, the precipitate lost 0"0079 grm. (reckoned from a part to the whole), leaving accord- ingly 0'2823 grm. of anhydrous antimonious sulphide, which corresponds to 0*24245 grm., or 43'37 per cent, of antimonious oxide. As the tartar emetic contains 43 '70 per cent, of antimonious oxide, the process gives, if the precipitate is dried at 100, 102*01; if heated to blackening, 99*22 instead of 100. 89. DETERMINATION OF PHOSPHORIC ACID AS MAGNESIUM PYROPHOSPHATE (to 134, b, a). 1-9159 and 2.0860 grm. pure crystallized sodium hydrogen phosphate, treated as directed 134, b, a, gave 0'5941 and 0*6494 grm. of magnesium pyrophos- phate respectively. These give 19 '83 and 19'91 per cent, of P 2 O 5 in sodium hydrogen phosphate, instead of 19*83 per cent. 90. DETERMINATION OF PHOSPHORIC ACID AS URANYL PYROPHOSPHATK (to 134, c). 30 c.c. of a solution of pure sodium hydrogen phosphate, treated with magnesium sulphate, ammonium chloride, and ammonia, as directed 134, b, a, gave 0*3269 grm. of magnesium pyrophosphate. 10 c.c. contained accordingly 0-06982 grm. of phosphoric anhydride. 10 c.c. of the same solution were then precipitated with uranyl acetate as directed 134, c. The ignited precipitate was treated with a little nitric acid, then again ignited ; after cooling, it weighed 0*3478 grm. corresponding to 0-06954 grm. of phosphoric anhydride. 91. DETERMINATION OF FREE HYDROGEN SULPHIDE BY MEANS OF SOLU- TION OF IODINE (to 148, I., a). The experiments were made to settle the following questions: ANALYTICAL EXPERIMENTS. 831 . Does the quantity of iodine required remain the same for solutions of hydrogen sulphide of different degrees of dilution? b. Does the equation H 2 S + 1 2 = 2HS -f S really represent the decomposition which takes place? The hydrogen sulphide water was contained in a flask closed by a doubly- perforated cork ; into one aperture a siphon with pinchcock was fitted, to draw off the fluid; into the other aperture a short open tube, which did not dip into the fluid. Question a. a. About 30 c.c. of iodine solution were introduced into a flask, which was then tared ; hydrogen sulphide water was added until the yellow color had just disappeared. The flask was then closed, weighed, starch paste added, and then solution of iodine until the fluid appeared blue. 70'2 grm. H 2 S water required 23'4 c.c. iodine solution, 100 accordingly 33-33 c.c. 68 '4 grm. required 22 '7 c.c. iodine solution, 100 accordingly 33 '20 c.c. ft. Same process; but the fluid was diluted with water free from air. 61 '5 grm. H 2 S water -f- 200 grm. water required 20"7 c.c. iodine solution, 100 accordingly 33 '65 c.c. 52 '4 grm. -j- 400 grm. water required 17.7 c.c. iodine solution, 100 accord- ingly 33-77. The iodine solution contained '00498 iodine in 1 c.c. Considering that addition of a larger volume of water necessarily involves a slight increase in the quantity of iodine solution, these results may be considered sufficiently corresponding. Question b. According to a, 100 grm. of the H 2 S water contained 0-02215 grm. H 2 S, assuming the proportion to be 100 : 33'2. 173 "6 grm. of the same water were, immediately after the experiments in a, drawn off into a hydrochloric acid solution of arsenious acid; after 24 hours, the arsenious sulphide was filtered off, dried at 100, and weighed. 0"0920 grm. were obtained, which corresponds to '03814 H 2 S, or a percentage of '02197. The second question also is therefore answered in the affirmative. 92. SOLUTION OF MAGNESIUM CHLORIDE DISSOLVES CALCIUM: OXALATE (to S 154, 6). If some calcium chloride is added to a solution of magnesium chloride, then a little ammonium oxalate, no precipitate is formed at first ; but upon slightly increasing the quantity of ammonium oxalate, a trifling precipitate gradually separates after some time. If an excess of ammonium oxalate is added, the whole of the calcium is thrown down, but the precipitate contains also magnesium oxalate. This shows that to effect the separation of the two bases by ammonium oxalate, the reagent must be added in excess; whilst, on the other hand, in the presence of much magnesium, the operator must expect to precipitate some of the magnesium, as the following experiments (No. 93) clearly show. 93. SEPARATION OP CALCIUM FROM MAGNESIUM (to 154, 6). The fluids employed in the following experiments were, a solution of calcium 832 ANALYTICAL EXPERIMENTS. chloride, 10 c.c. of which corresponded to '5618 CaCO 3 ; a solution of magne- sium chloride, containing 0*250 MgO in 10 c.c. ; a solution of ammonium chloride (1 : 8); solution of ammonia, containing 10 per cent. NH 3 ; solution of ammonium oxalate (1 : 24); acetic acid, containing 30 per cent. C 2 H 4 O 2 . The precipitation was effected at the common temperature; the precipitate of calcium oxalate was filtered off after 20 hours. a. Influence of the degree of dilution. a. 10 c. c. MgCl 2 , 10 c. c. CaCl 2 , 10 c. c. NH 4 C1, 4 drops JSTH 4 OH, 50 c.c. water, 20 c. c. (NH 4 ) 2 C 2 O 4 . Result, 0'5705 CaCO 3 . ft. Same as a, with 150 c.c, water instead of 50 c.c. Eesult, 0'5670 CaCO 3 . b. Influence of excess of ammonia. Same as a, ft + 10 c.c. NH 4 OH. Result, 0*5614 grin. CaCO 3 . c. Influence of excess of ammonium chloride. Same as a, ft + 40 c.c. NH 4 C1. Result, 0*5652 grm. d. Influence of excess of ammonia and ammonium chloride. Same as a, ft + 30 c.c. NH 4 C1 -f 10 c.c. NH 4 OH. Result, 0*5613 grm. e. Influence of free acetic acid. Same as a, ft, only with 6 drops C 2 H 4 O 2 , instead of the 4 drops NH 4 OH. Result, 0-5594 grm. /. Influence of excess of ammonium oxalate in feebly alkaline solution. Same as a, /? + 20 c.c. (NH 4 ) 2 C 2 O 4 . Result, 0'5644 grm. CaCO 3 ^ g. Influence of excess of ammonium oxalate in strongly alkaline solution. Same as a, ft, + 10 c.c. NH 4 OH + 20 c.c. (NH 4 ) 2 C 2 O 4 . Result, 0-5644. 7i. Influence of excess of ammonium oxalate in presence of much NH 4 C1 and NH 4 OH. Same as a, ft, -f 10 NH.OH + 30 NH 4 C1 + 20 (NH 4 ) a C 9 O 4 . Result, 0-5709 grm. i. Influence of excess of ammonium oxalate in solution slightly acidified with C 2 H 4 O 2 . Same as a, ft, - 4 drops NH 4 OH + 6 drops C 3 H 4 O 2 -f 20 c.c. (NH 4 ) 2 C 2 O 4 . Result, 0-5661 grm. Consequently, when a notable amount of magnesium is present there is always a chance of magnesium oxalate, or ammonium magnesium oxalate pre- cipitating along with the calcium oxalate. Another series of experiments in which a solution of magnesium oxalate in hydrochloric acid was mixed with ammonia under varying circumstances, proved also that, in presence of a notable quantity of magnesium, magnesium oxalate, or magnesium ammonium oxalate, will always separate after standing for some time, no matter whether in a cold or a warm place. In a third series of experiments, the separation was effected by double pre- cipitation, in accordance with 154, 28. The same solutions were employed as in the first series, with the exception of the magnesium chloride, for which a solution was substituted containing 0*2182 grm. MgO, in 10 c.c. 10 c.c. CaCl 2 -f 30 c.c. MgCl 2 + 20 c.c. NH 4 C1, + 300 c.c. water, + 6 drops ammonia, + a sufficient excess of ammonium oxalate. Results, in two experi- ments, 0-5621 and 0'5652, mean 0-5636, instead of 0'5618 CaCO 3 ; also 0'6660 and 0-6489 MgO, mean 0'6574, instead of 0'6546. ANALYTICAL EXPERIMENTS. 833 94. SEPARATION OF IODINE FKOM CHLORINE BY PISANI'S METHOD. 0-2338 grm. potassium iodide, dissolved in water, -f- \ c.c. of solution of iodide of starch, required 14 c.c. of decinormal silver solution = '2322 grm. potassium iodide. G'3025 grm. potassium iodide, mixed with about double the quantity of sodium chloride, required 18 '2 c.c. silver solution = 0'3021 KI. 0-2266 grm. potassium iodide, mixed with about 100 times as much sodium chloride, required 13 '7 c.c. silver solution = 0'2272 KI. 95. SEPARATION OF IODINE FROM BROMINE, BY PISANI'S METHOD. 0*3198 grm. potassium iodide, mixed with double the quantity of potassium bromide, required 19 '2 c.c. of decinormal silver solution = 0'3187 KI. 99. CHLORIMETRICAL EXPERIMENTS (to 199). 10 grm. of chloride of lime were rubbed up with water to one litre, with which the following experiments were made : a. By PENOT'S method ( 200); obtained 23 '5 and 23*5 per cent. b. By means of iron ( 201, modification); obtained 23'6 per cent c. By BUNSEN'S method ( 201); results, 23*6 23 '6 per cent. 100. DRYING OF MANGANESE (to 202, I.). Four small pans, containing each 8 grm. of manganese of 53 per cent., were first heated in the water-bath. After 3 hours, I. had lost 0145; after 6 hours, II. 0-15; after 9 hours, III. 015; after 12 hours, IV. 015 grm. I. and II. having been left standing, loosely covered, in the room for 12 hours, II. was found to weigh exactly as much as at first; I. wanted only O'Ol grm. of the original weight. The four pans were now heated for 2 hours to 120. . After cooling, they were found to have lost each 0180 of the original weight. I. and II. having been left standing, loosely covered, in the room for 60 hours, were found to have again acquired their original weight by attracting moisture. III. and IV. were heated for 2 hours to 150. The loss of weight in both cases was 0'215 grm. Having been left standing, loosely covered, in the room for 72 hours, both were found to weigh 0*05 less than at first. Assuming the hygroscopic moisture expelled to be reabsorbed by standing in the air, this shows that at 150 a little chemically combined water escapes along with the moisture, and accordingly that the tem- perature must not exceed 120. My experiments will be found described in detail in DINGLER'S polyt. Journ., 135, 277 et seq. 834 CALCULATION OF ANALYSIS. CALCULATION OF ANALYSES. THE calculation of the results obtained by an analysis presupposes, as an in- dispensable preliminary, a knowledge of the general laws of the combining proportions of bodies, on the one hand, and of the more simple rules of arith- metic on the other. It is a great error to suppose that the ability to make chemical calculations involves an extensive acquaintance with mathematics, a knowledge of decimal fractions and simple equations being for the most part sufficient. These remarks are not intended to dissuade students* of chemistry from pursuing the highly important study of mathematics; but merely to encourage those who have had no opportunity of entering more deeply into this science, and who, as experience has shown me, are often afraid to venture upon chemical calculations. For this reason, I have made the whole of the calculations given in the following paragraphs, in the most intelligible manner possible, and without logarithms. I. Calculation of the Constituents sought from the Compound obtained in ihe Analytical Process, and exhibition of the Result in Per-cents. The bodies the weight of which it is intended to determine, are separated, as we have seen in Division I., treating of the " Execution of Analysis," either in the free state, or and this most frequently in combinations of known com- position. The results are usually calculated upon 100 parts of the examined substance, since this gives a clearer and more intelligible view of the composi- tion. In cases where the several constituents have been separated in the free state, the calculation may be made at once ; but if the constituents have been separated in combination with other substances, they must first be calculated from the compounds obtained. 1. Calculation of the Results into Per-cents by Weight, in Cases where the Substance sought has been separated in the Free State. a. Solid Bodies, Liquids, and Gases, which have been determined by Weight. The calculation here is exceedingly simple. Suppose you have analyzed mercurous chloride, and separated the mercury in the metallic state. 2'945 grm. mercurous chloride have given say 2'499 grm, metallic mercury. 2-945 : 2-499 :: 100 : x x = 84-85, which means that your analysis shows 100 parts of mercurous chloride to con- tain 84-85 of mercury, and consequently 15*15 of chlorine. Now as mercurous chloride is known to consist of 2 at. mercury and 2 at. chlorine, and as the atomic weights, of both these elements are also known, the true percentage composition of the body may be readily calculated from these data. When analyzing substances of known composition for practice, the results theoretically calculated and those obtained by the analysis are usually placed in juxtaposition, as this enables the student at once to perceive the degree of accuracy with which the analysis has been performed. CALCULATION OF ANALYSIS. 835 Thus for instance Found. Calculated (compare 84, &). Mercury 84'85 84'94 Chlorine.. . 15'15 . . 15'06 100-00 100-00 b. Gases ichich have been determined by Measure. If a gas has been determined by measure, it is, of course, necessary first to ascertain the weight corresponding to the volume found, before the percentage by weight can be calculated. But as the exact weights of a definite volume of the various gases have been severally determined by accurate experiments, this calculation also is a simple rule-of-three question, if the gas may be measured under the same circumstances to which the known relation of weight to volume refers. The circumstances to be taken into consideration here, are: Temperature and Atmospheric Pressure. Besides these, the Tension of the Aqueous Vapor may also claim consideration in cases where water is used as the confining fluid, or generally where the gas has been measured in the moist state, The respective weights assigned in Table V.* to 1 litre of the gases there enumerated, refer to a temperature of 0, and an atmospheric pressure of 0*76 metre of mercury. We have, therefore, in the first place, to consider the manner in which volumes of gas measured at another temperature and another height of the barometer, are to be reduced to and - 76 of the barometer. a. Reduction of a Volume of Gas of any given Temperature to 0, or any other Temperature between and 100. The following propositions regarding the expansion of gases were formerly universally adopted: 1. All gases expand alike for an equal increase of temperature. The expansion of one and the same gas for each degree of the thermometer is independent of its original density. Although the correctness of these propositions has not been fully confirmed by the minute investigations of MAGNUS and REGNAULT, yet they may be safely followed in reductions of the temperature of those gases which are most frequently measured in the course of analytical processes, as the coefficients of expansion of these gases scarcely differ from each other, and as there is never any very considerable difference in the atmospheric pressure under which the gases are severally measured. The investigations just alluded to have given 0-3665 as the coefficient of the expansion of gases which comes nearest to the truth ; in other words, as the extent to which gases expand when heated from the freezing to the boiling point of water. They expand, therefore, for every degree of the centigrade thermometer, 0-3665 100 = 0-003665. * See Tables at the end of the volume. 836 CALCULATION OF ANALYSIS. If we wish to ascertain how much space 1 c. c. of gas at will occupy at 10, we find 1 X [1 -f (10 X 0-003665)] = 1 "03665. If we wish to ascertain how much space 100 c. c. at will occupy at 10, we find 100 X[l + (10X0 -003665)] = 100x1-03665-103-665. If we wish to know how much space 1 c. c. at 10 will occupy at 0, we find 1 + (10X 0-003665) How much space do 103*665 c. c. at 10 occupy at 0? 103-665 1 _|_ (10 x 0-003665) = 100. The general rule of these calculations may be expressed as follows: To calculate the volume of a gas from a lower to a higher temperature, we have in the first place to find the expansion for the volume unit, which is done by adding to 1 the product of the multiplication of the thermometrical difference by 0*003665; and then to multiply this by the number of volume units found in the analytical process. On the other hand, to reduce the volume of a gas from a higher to a lower temperature, we have to divide the number of volume units found in the analytical process, by 1 + the product of the multiplication of the thermometrical difference by '003665. ft. Reduction of the Volume of a Gas of a certain given Density to '76 Metre Barometric Pressure, or any other given Pressure. According to the law of MARIOTTE, the volume of a gas is inversely as the pressure to which it is exposed; in accordance with. this, a gas occupies the greater space the less the pressure upon it, and the less space the greater the pressure upon it. Thus, supposing a gas to occupy a space of 10 c. c. at a pressure of 1 atmos- phere, it will occupy 1 c. c. at a pressure of 10 atmospheres, and 100 c. c. at a pressure of T ^ atmosphere. Nothing, therefore, can be more easy than the reduction of a gas of a certain given tension to 760 mm. bar. pressure, or any other given pressure, e.g., 1000 mm., which is frequently used in the analysis of gases. Supposing a gas to occupy 100 c. c. at 780 mm. bar., how much space will it occupy at 760 mm. ? 760 : 780 :: 100 : x x = 102 -63. How much space will 100 c. c. at 750 mm. bar. occupy at 760 mm. ? 760 : 750 :: 100 : x x = 98-68. How much space will 150 c. c. at 760 mm. bar. occupy at 1000 mm.? 1000 : 760 :: 150 : x a; = 114. CALCULATION OF ANALYSIS. 837 y. Reduction of the Volume of a Ga# saturated with Aqueous Vapor, to its actual Volume in the Dry State. It is a well-known fact that water has a tendency, at all temperatures, to assume the gaseous state. The degree of this tendency (the tension of the aque- ous vapor) which is dependent solely and exclusively upon the temperature, and not upon the circumstance of the water being in vacua or in any gaseous atmosphere is usually expressed by the height of a column of mercury counter- balancing it. The following table indicates the amount of tension for the various temperatures at which analyses are likely to be made.* TABLE. Temperature (in degrees C.) Tension of the aqueous vapor expressed in Temperature (in degrees C.) Tension of the aqueous vapor expressed in millimetres. millimetres. 4-525 21 18-505 1 4-867 22 19-675 2 5-231 23 20-909 3 5-619 24 22-211 4 6-032 25 23-582 5 6-471 26 25-026 6 6-939 27 26-547 7 7-436 28 28-148 8 7-964 29 29-832 9 8-525 30 31-602 10 9-126 31 33-464 11 9-751 32 35-419 12 10-421 33 37-473 13 11-130 34 39-630 14 11-882 35 41-893 15 . 12-677 36 44-268 16 13-519 37 46-758 17 14-409 38 49-368 18 15-351 39 52-103 19 16-345 40 54-969 20 17-396 Therefore, if a gas is confined over water, its volume is, cateris paiibus, always greater than if it were confined over mercury; since a quantity of aque- ous vapor, proportional to the temperature of the water, mixes with the gas, and the tension of this partly counterbalances the column of air that presses upon the gas, and to that extent neutralizes the pressure. To ascertain the actual pressure upon the gas, we must therefore subtract from the apparent pressure so much as is neutralized by the tension of the aqueous vapor. Suppose we had found a gas to measure 100 c.c. at 759 mm. bar., the tempera- ture of the confining water being 15 ; how much space would this volume of gas occupy in the dry state and at 760 mm. of the barometer? Our table gives the tension of aqueous vapor at 15 = 12*677; the gas is con- sequently not under the apparent pressure of 759 mm. , but under the actual pressure of 759 - 12 '677 = 746-323 mm. * Compare Magnus, Pogg. Annal. 61, 247. 838 CALCULATION OF ANALYSIS. The calculation is now very simple; it proceeds in the manner shown in /?; we say, 760 : 746-323 :: 100 : x x = 98-20. When the volume of a gas has thus been adjusted by the calculations in a and ft, or y, to the thermometrical and barometrical conditions to which the data of Table V. refer, the percentage by weight may now be readily calculated by substituting the weight for the volume, and proceeding by simple rule of three. What is the percentage by weight of nitrogen in an analyzed substance, of which 0'5 grm. have yielded 30 c. c. of dry nitrogen gas at 0, and 760 mm. bar.? In Table V. we find that 1 litre (1000 c. c.) of nitrogen gas at 0, and 760 mm. bar., weighs 1-25456 grm. We say accordingly : 1000 : 1-25456 :: 30 : x x = 0-0376. And then : 0-5 : 0-0376 :: 100 : x x = 7-52. The analyzed substance contains consequently 7 '52 per cent, by weight of nitrogen. DR. GIBBS' method of finding at once the total correction for temperature, press- ure, and moisture in absolute determinations of nitrogen, or other gases: * "I take a graduated tube, which I fill with mercury, then displace about two-thirds of the mercury with air, and invert the tube into a cistern of mercury. Then I make four or five determinations of the volume of the included (moist) air in the usual manner, and find the volume of the air at and 760 mm. as a mean of all the determinations. This tube I call the companion tube, and it always hangs in the little room I use for gas analyses. Suppose the volume of (dry) air at and 760 mm. is 132 '35 c. c. "Now, in making an absolute nitrogen determination I collect the nitrogen moist over mercury in a graduated tube, and then suspend the measuring tube by the side of the companion tube. I then by a cord and pulley bring the level of the mercury in the two tubes to correspond exactly, and then read off the volume of air in the companion tube and the volume of nitrogen in the measur- ing tube. I ought to have stated that the two tubes hang in the same cistern of mercury. Suppose the volume of air in the companion tube to be 143 c. c. ; then the total correction for temperature, pressure, and moisture will be 143 132*35 = 10*65 c.c. The correction for the nitrogen will then be found by rule of three. As the observed volume of air in the companion tube is to the observed volume of nitrogen, so is (in this case) 10 '65 to the required correction. In this way, when the volume of air in the companion tube is once found, no further observations of temperature, pressure, or height of mercury above the mercury in the cistern are necessary. The companion tube lasts for an indefinite time. I have even used it filled with water, without any appreciable change in some weeks, but I prefer mercury. As the two tubes hang side by side, there is never an * Private communication. CALCULATION OF ANALYSIS. 839 appreciable difference of temperature. My results are most satisfactory. Wil- liamson & Russell have, as you know, used a companion tube for equating pressures, but not for finding the total value of the temperature and pressure correction at once ; and I believe that my process is wholly new. Certainly it is wonderfully convenient, and saves all tables and labor of computation." 2. Calculation of the Results into Per-cents by Weight, in Cases where the Body sought has been separated in Combination, or where a Compound has to be deter- mined from one of its -Constituents. If the body to be determined has not been weighed or measured hi its own form, but in some other form, e.g., carbonic acid as calcium carbonate, sulphur as barium sulphate, ammonia as nitrogen, chlorine by a standard solution of Iodine, &c., its quantity must first be reckoned from that of the compound found before the calculation described in 1 can be made. This may be accomplished either by rule of three or by some abridged method. Suppose we have weighed hydrogen in the form of water, and have found 1 grm. of water; how much hydrogen does this contain? A molecule of water consists of: Hydrogen 2 at. = 2 pts. Oxygen 1 at. = 16 " 18 " We say accordingly: 18 : 2 :: 1 : x x = 011111. Or, expressed in general terms: Water X 011111 = Hydrogen. EXAMPLE. 517 of water; how much hydrogen? 517 X 0-11111 = 57-444 The following equation results also from the above proportion: 18 l_ 2 := x 18 = 1 X I .'. X = - Or, expressed in general terms, Water divided by 9 = Hydrogen. EXAMPLE. 517 of water, how much hydrogen? f = 57-444. In this manner we may find for every compound constant numbers by which to multiply or divide the weight of the compound, in order to find the weight of the constituent sought (comp. Table III.*). * See Tables at the end of the volume. 840 CALCULATION OF ANALYSIS. Thus, for instance, the nitrogen contained in ammonium platinic chloride may be obtained by multiplying . the weight of the latter by 0*06296 ; thus the carbon may be calculated from carbonic acid by multiplying the weight of the latter by 0'2727, or dividing it by 3 '666. These numbers are by no means so simple, convenient, and easy to remember as in the case of hydrogen. It is therefore advisable, in the case of carbonic acid, for instance, to fix upon another general expression, viz., Carbonic acid X 3 _____ = Carbon ; 12 parts in 44 (= T 3 T ) in carbonic acid being carbon, as may be seen from the composition: C 12 O 2 32 44 The object in view may also be attained in a very simple manner, by refer- ence to Table IV.,* which gives the amount of the constituent sought for every number of the compound found, from 1 to 9 ; the operator need, therefore, simply add the several values together. As regards hydrogen, for instance, we find : TABLE. Found.) Sought, water j hydrogen 1 O'lllll 2 0-22222 3 0-33333 4 0-44444 5 0-55555 6 0-66667 0-77778 8 0-88889 9 i-ooooo From this table it is seen that 1 part of water contains 0-11111 of hydrogen, that 5 parts of water contain '55555 of hydrogen; 9 parts, 1 '00000, &c. Now if we wish to know, for instance, how much hydrogen is contained in 5'17 parts of water, we find this by adding the values for 5 parts, for ^ part, and for T ^ parts, thus : 0-55555 O'Olllll 0-0077778 0-5744388 Why the numbers are to be placed in this manner, and not as follows: 0-55555 0-11111 0-77778 1-44444 is self-evident, since arranging them in the latter way would be adding the value for 5, for 1, and for 7 (5 -f 1 -f 7 = 13), and not for 5'17. This reflection shows * See Tables at the end of the volume. CALCULATION OF ANALYSIS. 841 also that, to find the amount of hydrogen contained in 517 parts of water, the points must be transposed as follows : 55-555 1-1111 0-77778 57-44388 3. Calculation of the Results of Indirect Analyses into Per -cents by Weight. The import of th?, term " indirect analysis" as defined in 151, p. 478 shows sufficiently that no universally applicable rules can be laid down for the calcula- tions which have to be made in indirect analyses. The selection of the right way must be left in every special case to the intelligence of the analyst. I will here give the mode of calculating the results in the more important indirect separations described in Section V. They may serve as examples for other similar calculations. a. Indirect Determination of Sodium and Potassium. This is effected by determining the sum total of the chlorides, and the chlo- rine contained in them. The calculation may be made as follows: Suppose we have found 3 grm. of sodium and potassium chlorides, and in these 3 grm. 1*6877 of chlorine. At. Chlorine. Mol. KC1. Chlorine found. 35-46 : 74-59 :: 1-6877 : x x 3-55007. If all the chlorine present were combined with potassium, the weight of the chloride would amount to 3 - 55007. As the chloride weighs less, sodium chloride is present, and this in a quantity proportional to the difference (i.e., 3 '55007 3 = -55007), which is calculated as follows: The difference between the mol. weight of KC1 and that of NaCl (16 -09) is to the mol. weight of NaCl (58'50), as the difference found is to the sodium chloride present : 16-09 : 58-50 :: '55007 : x x = 2 NaCl and 3 - 2 = 1 KC1. From this the following short rule is derived: Multiply the quantity of chlorine in the mixture by 2 '1035, deduct from the product the sum of the chlorides, and multiply the remainder by 3 '6358; the product expresses the quantity of sodium chloride contained in the mixed chlo- ride. b. Indirect Determination of Strontium and Calcium. This may be effected by determining the sum total of the carbonates, and the carbonic acid contained in them ( 154, 31). Suppose we have found 2 giro, of mixed carbonate, and in these 2 grm. 0'7383 of carbonic acid. Mol. C0 2 Mol. SrCO 3 CO 2 found. 44 14750 :: 0'7383 : x x = 2-47498. 842 CALCULATION OF ANALYSIS. If, therefore, the whole of the carbonic acid were combined with strontia, the weight of the carbonate would amount to 2 '47498 grm. The deficiency, = 0-47498, is proportional to the calcium carbonate present, which is calculated as follows: The difference between the molecule of SrCO 3 and the molecule of CaCO 3 (47-50) is to the molecule of CaCO 3 (100) as the difference found is to the calcium carbonate contained in the mixed salt: ,-. 47-5 : 100 :: "47498 : x x = 1. The mixture, therefore, consists of 1 grm. calcium carbonate and 1 grm. strontium carbonate. From this the following short rule is derived : Multiply the carbonic acid found by 3 '3523, deduct from the product the sum of the carbonates, and multiply the difference by 2-10526; the product expresses the quantity of the calcium carbonate. c. Indirect Determination of Chlorine and Bromine ( 169, 1). Let us suppose the mixture of silver chloride and bromide to have weighed 2 grm., and the diminution of weight consequent upon the transmission of chlorine to have amounted to 01 grm. How much chlorine is there in the mixed salt,, and how much bromine? The decrease of weight here is simply the difference between the weight of the silver bromide originally present, and that of the silver chloride which has replaced it; if this is borne in mind, it is easy to understand the calculation which follows: The difference between the molecules of silver bromide and silver chloride is to the molecule of silver bromide as the ascertained decrease of weight is to x, i.e. , to the silver bromide originally present in the mixture : 44-49 : 187-88 :: O'l : x x = 0-422297. The 2 grm. of the mixture therefore contained 0*422297 grm. silver, bromide, and consequently 2 0-422297 1-577703 grm. silver chloride. It results from the above, that we need simply multiply the ascertained decrease of weight by to find the amount of silver bromide originally present in the analyzed mixture. And if we know this, we also know of course the amount of the silver chloride; and from these data we next calculate the quantities of chlorine and bromine in the ordinary way. SUPPLEMENT TO I. KEMARKS ON LOSS AND EXCESS IN ANALYSES, AND ON TAKING THE AVERAGE. If, in the analysis of a substance, one of the constituents is estimated from the loss, or, in other words, by subtracting from the original weight of the analyzed substance the ascertained united weight of the other constituents, it is evident that in the subsequent percentage calculation the sum total must invariably be 100. Every loss suffered or excess obtained in the determination of the several CALCULATION OF ANALYSIS. 843 constituents will, of course, fall exclusively upon the one constituent which is estimated from the loss. Hence estimations of this kind cannot be considered accurate, unless the other constituents have been determined by good methods, and with the greatest care. The accuracy of the results will, of course, be the greater, the less the number of constituents determined in the direct way. If, on the other hand, every constituent of the analyzed compound has been determined separately, it is obvious that, were the results absolutely accurate, the united weight of the several constituents must be exactly equal to the origi- nal weight of the analyzed substance. Since, however, as we have seen in 96, certain inaccuracies attach to every analysis, without exception, the sum total of the results in the percentage calculation will sometimes exceed, and sometimes fall short of, 100. In all cases of this description, the only proper way is to give the results as actually found. Thus, for instance, PELOUZE found, in his analysis of chromate of potassium chloride, Potassium 21 -8& Chlorine 19'41 Chromic acid. . 58 '21 99-50 BERZELITJS, in his analysis of potassium uranate, Potassa 12'8 Uranic oxide 86 '8 996 PLATTNER, in his analysis of pyrrhotite, Of Fahlun. Of Brasil. Iron 59-72 59'64 Sulphur 40-22 40'43 99-94 100-07 It is altogether inadmissible to distribute any chance deficiency or excess proportionately among the several constituents of the analyzed compound, as such deficiencj 7 or excess of course never arises from the several estimations in the same measure; moreover, such "doctoring" of the analysis deprives other chemists of the power of judging of its accuracy. No one need be ashamed to confess having obtained somewhat too little or somewhat too much in an analysis, provided, of course, the deficiency or excess be confined within certain limits, which differ in different analyses, and which the experienced chemist always knows how to fix properly. In cases where an analysis has been made twice, or several times, it is usual to take the mean as the most correct result. It is obvious that an average of the kind deserves the greater confidence the less the results of the several analyses differ. The results of the several analyses must, however, also be given, or, at all events, the maximum and minimum. Since the accuracy of an analysis is not dependent upon the quantity of sub- stance employed (provided always this quantity be not altogether too small), the average of the results of several analyses is to be taken quite independently of the quantities used ; in other words, you must not add together the quantities used, on the one hand, and the weights obtained in the several analyses on the 844 CALCULATION OF ANALYSIS. other, and deduce from these data the percentage amount; but you must cal culate the latter from the results of each analysis separately, and then take the mean of the numbers so obtained. Suppose a substance, which we will call AB, contains fifty per cent, of A; and suppose two analyses of this substance have given the following results : (1) 2 grm. AB gave 0'99 grm. of A. (2) 50 " " 24-00 " From 1, it results that AB contains 49*50 per cent, of A. " 2, 48-00 Total 97-50 Mean ,, 48*75 It would be quite erroneous to say 2 -f 50 = 52 of AB gaye 0*99 + 24 '00 = 24-99 of A, therefore 100 of AB contain 48 '06 of A; for it will be readily seen that this way of calculating destroys nearly altogether the influence of the more accurate analysis (1) upon the average, on account of the proportionally small amount of substance used. II. -DEDUCTION OF FORMULAE. 1. From the percentages of single elements in compounds. The process of deducing an empirical formula from the expression of the composition of a compound in parts per hundred of its constituents (i.e., its per- centage composition) will be readily understood by considering first the some- what simpler reverse process of calculating percentage compositions from formulae. Applying this latter process to the formula, for instance, of mannite, C 6 Hi 4 O 6 , we first compute from the relative number of atoms of the elements shown by the formula the relative quantities by weight of each, by means of their known atomic weights. Carbon 6 at. X 12 = 72 pts. by weight. Hydrogen.. 14 " X 1 = 14 " " Oxygen 6 " X 16 = 96 " 182 " " of mannite. Since 182 pts. of the compound contain 72 pts. of carbon, the number of pts. of carbon which 100 contain may be found by the rule of three: 182 : 100 r 72 : x ^ X 72 = 39-56 carbon, lo-c 100 In like manner - x 14 = 7-69 hydrogen. lo/4 ioH X 96 = 52-75 oxygen. 100-00 CALCULATION OF ANALYSIS. 845 Returning now to the first expression of the relative quantities, which was obtained by multiplying the relative number of atoms of carbon, oxygen, and hydrogen by their atomic weights, it is evident by dividing the relative quantities by the atomic weights, the relative number of atoms will again be obtained: Parts of carbon 72 -5- 12 = 6 carbon atoms. " " hydrogen 14 -s- 1 = 14 hydrogen " " "oxygen 96 -*- 16 = 6 oxygen " % It is moreover evident that if numbers obtained by increasing or diminishing 72, 14, and 96 proportionally, be divided by 12, 1, and 16 respectively, the resulting quotients will express the atomic ratio also : 100 Carbon 72 X ^n = 39 '56 *- 12 = 3 '296 carbon atoms. lo s 2 + 2H 2 O. b. When isomorphous constituents are present. In deducing formulae, it must be borne in mind that closely related elements or radicals, more especially the basic metals, may replace each other in all pro- portions. Elements of like quantivalence are oftenest found replacing each other, but in some cases equivalent amounts of elements having different valence appear to replace each other. The following example will illustrate the kind of formula and method of deducing it commonly used in such cases. S. L. PENFIELD found by analysis of triphylite the following composition: Molecular weights. Mol. ratio. At. ratio. P 2 5 44-76 -h 142 = -315 X 2 = P '630 FeO 26-40 -r- 72 = '366 Fe '3661 MnO 17-84 -*- 71 = '251 Mn '251 I _ . AQQ CaO -24 -r- 56 = '004 Ca '004 { McrO -47-^-40 = -012 Mg -012 J Li 2 O 9-36 -f- 30 = -312 X 2 = Li '624 f _ , .. Xa a O -35 -T- 78-08 = '005 X 2 = Na '010 f = H 2 -42 O 2-525 99-84 Disregarding the small amount of water, the relative numbers of molecules of the oxides (mol. ratio) are first found by dividing quantities by molecular weights, as in the preceding example. Next the atoms contained by the mole- cules are written in another column (at. ratio). This column, icith the adjoined symbols, is the empirical formula. It is apparent, or can be proved by trial, that the numbers of different atoms are not in any simple ratio. Such an atomic relation is to be expected when isomorphous constituents are present. It remains now to unite the atoms of such elements as are supposed to be capable of mutually replacing each other, and ascertain whether the numbers thus 848 CALCULATION OF ANALYSIS. obtained are in any simple proportion. For this purpose let R" represent one atom of any dyad basic metal and R' one atom of any monad basic metal present. The sum of the dyad atoms is '633 ; that of the monad atoms, '634, as above shown. The atomic ratio thus obtained is expressed by the formula R"633R' 6 34P63oO 2 5i5; or simpler, dividing by 630, almost exactly by R"R'PO 4 which is equal to \0-R', anhydrous normal lithium ferrous phosphate in which iron is partially replaced by manganese, magnesium, and calcium; and lithium to a slight extent by sodium. It may be here observed that in presenting atomic ratios in connection with analyses of natural oxygen salts (minerals), computation and statement of oxygen atoms is often omitted, since they may be deduced from a formula show ing the other constituents. Omitting oxygen in the above example we have R"R'P. By referring to the percentage composition it is seen that for two P five O must be present, for two R' one O, for one R" one O. Doubling R"R'P and appending to each constituent the required oxygen atoms, we have : R%O 2 R' 2 OP a O 6 = R" 2 R' a P 2 O 8 , and dividing by 2, R"RTO 4 , as before. TABLES FOR THE CALCULATION OF ANALYSIS. TABLE I. ATOMIC WEIGHTS OF THE ELEMENTS CONSIDERED IN THE PRESENT WORK.* Aluminium Antimony Arsenic Barium Bismuth Boron Bromine Cadmium Caesium Calcium Carbon Chlorine Chromium Cobalt Copper Fluorine Gold Hydrogen Iodine Iron Lead Lithium Alt Sbf As Ba Bi B Br Cd Cs Ca C Cl Cr Co Cu Fl Au H I Fe Pb Li 27-50 122-00 75-00 137-00 208-00 11-00 79-95 112-00 133-00 40-00 12-00 35-46 52-48 59-00 63-40 19-00 196-71 1-00 126-85 56-00 207-00 7-00 i I Magnesium ! Manganese | Mercury Molybdenum Nickel ; Nitrogen Oxygen Palladium Phosphorus Platinum Potassium , Rubidium Selenium Silicon Silver Sodium Strontium Sulphur Tin Titanium Uranium .Zinc Mg Mn Hg Mo Ni N O Pd P Pt K Rb Se Si Sr S Sn Ti Ur Zn 24-00 55-00 200-00 92-00 59-00 14-04 16-00 106-58 31-00 19718 39-13 85-40 79-00 28-00 107-93 23-04 8750 32-00 118-00 50-00 237-60 65-06 TABLE II COMPOSITION OF THE BASIC AND ACID OXIDES. GROUP I. a. BASIC OXIDES. Caesia Cs a . O.. Cs 2 O. .266-00 94-33 . 16-00.. 5-67 .282-00.. ..100-00 Rubidia Rb a . O.. .170-80 91-43 . 16-00.. 8-57 Rb 2 O 186.80.. ..100.00 * [The numbers here given are based on the atomic weights used in the sixth German edition, the atomic weights of the "old system" being doubled when necessary.] t Recent critical investigations by J. P. COOKE, on the atomic weight of antimony by J. W. MALLET, on that of aluminium, have conclusively shown that 120 and 27'02 respectively should be taken as the atomic weights of these elements. See Transactions of Am. Acad. Sci., 13, 15. Atomic Weight of Antimony, and Philosophical Transactions of the Royal Society (London), Revision of the Atomic Weight of Aluminium. 850 TABLE II. Potassa K a 78*26 83-03 O.. . 16-00.. . 16-97 K a O 94-26 100-00 Soda Na a 46-08 74-23 O.. . 16-00.. . 25-77 Na a O ................. 62-08 ........ 100-00 ..< ...................... Li 2 ................... 14-00 ........ 46-67 ..................... 16-00 ........ 53-33 Li 3 O .................. 30-00 ....... .100-00 Ammonium oxide ................. (NH 4 ) ................ 36-16 ....... . 69-28 O.. . 16-00.. . 30-72 (NH 4 ) a O 52-16 ...100-00 GBOUP II. Baryta Ba 137-00 89-54 O.. . 16-00.. . 10-46 BaO 153-00 100-00 Strontia Sr 87-50 84-54 O.. . 16-00.. . 15-46 SrO 103-50 100-00 Lime Ca 40-00 71-43 O.. . 16-00.. . 28-57 CaO 56-00 100-00 Mg 24-00 60-03 16-00 39-97 MgO... 40-00 100-00 GROUP III. Alumina Al a 55'00 53-40 O, 48-00.. . 46-60 Al a O 3 103-00 100-00 Chromic oxide Cr a 104-96 68*62 O 3 .. . 48-00.. . 31-38 Cr a O 3 152-96 100-00 GKOUP IV. Zinc oxide Zn 65*06 80-26 O.. . 16-00.. . 19-74 ZnO 81-06.. ..100-00 TABLE II. 851 Manganous oxide Mn 55-00 77-46 O. . . 16-00.. . 22-54 MnO 71-00 ...100-00 Manganic oxide Mn 3 110-00 69-62 O, .. 48-00 30-38 Mn,O 3 158-00 100-00 Nickelous oxide , Ni 59-00 78-67 16-00 21-33 NiO 75-00 100-00 Cobaltous oxide Co 59-00 78-67 O . 16-00.. . 21-33 CoO 75-00 100-00 Cobaltic oxide Co, 118-00 71-08 O s .. . 48-00 . . 28-92 Co,O, 166-00 100-00 Ferrous oxide Fe 56-00 77-78 O.. . 16-00.. FeO 72-00 100-00 Ferric oxide Fe a 112-00 70-00 O s . 48-00.. . 30-00 Fe 2 O, 160-00 100-00 GROUP V. Silver oxide Ag a 215*86 93-10 O . 16-00.. , 6-90 Ag a O 231-86 100-00 Lead oxide Pb 207-00 92-83 O . 16-00.. 7-17 PbO 223-00 100-00 Mercurous oxide Hg a 400-00 96-15 O.. . 16-00.. 3-85 Hg a O 416-00 100-00 Mercuric oxide Hg 200-00 92-59 O. . . 16-00.. 7-41 HgO 216-00 100-00 852 TABLE II. Cuprous oxide Cu 2 126*80 88-80 O . 16-00.. . 11-20 Cu a O 142-80 100-00 Cupric oxide Cu 63-40 79-85 O.. . 16-00.. . 20-15 CuO 79-40 100-00 Bismuth trioxide Bi a 416-00 89-66 O 3 48-00 10-34 Bi 2 O 3 464-00 100-00 Cadmium oxide Cd 112-00 87-50 O.. . 16-00.. . 12-50 CdO 128-00 100-00 GROUP VI. Auric oxide Au 2 392-00 89-09 O 3 48-00 10-91 Au 2 O 3 440-00 100-00 Platinic oxide Pt 197-18 86-04 O 2 32-00 13-96 PtO 2 229-18 100-00 Antimonious oxide Sb a 244-00 83-56 O 3 ... 48-00 16-44 Sb 2 O 3 292-00 100-00 Stannous oxide Sn 118-00 88'06 O... . 16-00 11-94 SnO 134-00 100-00 Stannic oxide Sn 118*00 78 -67 O 2 32-00 21-33 SnO 2 150-00 100-00 Arsenious oxide As 2 150-00 75-76 O 3 48-00 24-24 As 2 O 3 198-00 100-00 Arsenic oxide As 2 150-00 65-22 O 5 80-00 34-78 As 2 5 ... ..230-00 100-00 TABLE II. 853 b. ACID OXIDES (ANHYDRIDES). Chromic anhydride Or 52*48 52-23 O 3 ... . 48-00.. . 47-77 CrO 3 100 48 100-00 Sulphuric anhydride S 32-00 40 -.00 O 3 ... . 48-00.. . 60-00 SO 3 80-00 100-00 Phosphoric anhydride P 3 62-00 43'66 O 6 80-00 56-34 P a O 5 142-00 100-00 Boracic anhydride B 3 22-00. ....... 31-43 O 3 48-00.. . 68-57 B 3 O 3 70-00 100-00 Oxalic anhydride C 3 24-00 33-33 O 3 48-00 66-67 C 3 O 3 72-00 100-00 Carbonic anhydride C 12-00 27-27 O a 3200 72-73 CO 3 44-00 100-00 Silicic anhydride Si 28-00 46-67 O 2 32-00 53-33 SiO 3 ........... ....... 60-00 ........ 100-00 Nitric anhydride ................. N a .................... 28-08 ........ 25-98 . O 6 .... ................ 80-00 ........ 74-02 108-08 ........ 100-00 Chloric anhydride. ............... C1 3 ................ ... 70 92 ....... 46*99 O 6 .................... 80-00 ........ 53-01 C1,O... ..150-92.. ..100-00 854 TABLE III. TABLE III. REDUCTION OF COMPOUNDS FOUND TO CONSTITUENTS SOUGHT BY SIMPLE MULTIPLICATION OR DIVISION. This Table contains only some of the more frequently occurring compounds the formulae preceded by ! give absolutely accurate results. FOR INORGANIC ANALYSIS. CARBON DIOXIDE. ! Calcium Carbonate X 0.44 = Carbon dioxide. CHLORINE. Silver chloride X 0'2473 = Chlorine. COPPER. Cupric oxide X 0-79849 = Copper. IRON. ! Ferric oxide X 0'7 = Iron. ! Ferric oxide X 0'9 = Ferrous oxide. LEAD. Lead oxide X 0*9283 = Lead. MAGNESIA. Magnesium pyrophosphate X *36036 = Magnesia. MANGANESE. Protosesquioxide of manganese X 0-72052 = Manganese. Protosesquioxide of manganese X '9301 3 = Manganous oxide. PHOSPHORIC ANHYDRIDE (P 2 O 8 ). Magnesium pyrophosphate X 0'6396 = Phosphoric acid. Uranyl pyrophosphate ((UO 2 ) 3 P 2 O 7 ) X 01991 .-= P a O 6 . POTASSIUM. Potassium chloride X 0'5246 = Potassium. Potassium sulphate X '54092 = Potassa. Potassium platinic chloride X 0*30557. or Potassium platinic chloride Potassium chloride. 3-2725 Potassium platinic chloride X 019308 1 or I _ Potassium platinic chloride 5-179 TABLE III. SODA. Sodium chloride X 0'5306 = Soda. Sodium sulphate X 0-43694 = Soda. SULPHUR. Barium sulphate X '13734 = Sulphur. SULPHURIC ACID. Barium sulphate X 0'34335 = Sulphuric anhydride (S0). FOR ORGANIC ANALYSIS. CARBON. Carbon dioxide X 0'2727 or Carbon dioxide 855 3-666 or Carbon dioxide X 3 = Carbon. 11 HYDROGEN. Water X O'lllll or Water NITROGEN. Ammonium platinic chloride X -06296 = Nitrogen. Platinum X 01424 = Nitrogen. 856 TABLE IV. TABLE Showing the Amount of the Number of the Elements. Found. Sought. 1 Aluminium . . (Ammonium). Alumina A1 2 O 3 Ammonium chloride NH 4 C1 Ammonium platinic chloride (NH 4 Ciy PtCl 4 Aluminium Al Ammonia NH 3 Ammonium oxide (NH 4 ) 2 0.53398 0.31850 0.11677 Antimony. . . . Ammonium platinic chloride (NH 4 Cl) 2 -PtCl 4 Antimonious oxide Sb 2 O 3 Antimonious sulphide Sb 2 S 3 Ammonia NH 3 Antimony Sb Antimony Sb 0.07641 0.83562: 0.71765 Arsenic. . . . Antimonious sulphide Sb 8 S 3 Antimony tetroxide Sb 2 4 Arsenious oxide As 2 O 3 Antimonious oxide Sb 2 O 3 Antimonious oxide Sb 2 3 Arsenic As 0.85882' 0.94805 0. 7575$ Arsenic oxide As 2 O 5 Arsenic oxide As 2 O 6 Arsenious sulphide As 2 S 3 Arsenic As Arsenious oxide As 2 O 3 Arsenious oxide As 2 O 3 0.65217 0.86087 0.80488- Barium Arsenious sulphide As 2 S 3 Baryta Arsenic oxide As 2 O 5 Barium 0.93496. 89542 BaO Barium sulphate BaSO 4 Ba Baryta BaO 0.65665 TABLE IV. 85T IV. Constituent sought for every Compound found. * 1 4 5 7 8 9 1.06796 0.63701 0.23353 1.60194 0.95551 0.35030 2.13592 1.27402 0.46706 2.66990 1.59252 0.58383 3.20389 1.91103 0.70060 3.73787 2.22953 0.81736 4.27185 2.54804 0.93413 4.80583 2.86654 1.05089' 0.15282 1.67123 1.43529 0.22923 2.50685 2.15294 0.30564 3.34247 2.87059 0.38205 4.17808 3.58834 0.45846 5.01370 4.30588 0.53487 5.84932 5.02353 0.61128 6.68194 5.74118 0.68769 7.52055 6.45882 1.71765 1.89610 1.51516 2.57647 2.84416 2.27274 3.43530 3.79221 3.03032 4.29412 4.74026 3.78790 5.15294 5.68831 4.54548 6.01177 6.63636 5.30306 6.87059 7.58442 6.06064 7.72942 8.53247 6.81822 1.30435 1.72174 1.60975 1.95652 2.58261 2.41463 2.60870 3.44348 3.21951 3.26087 4.30435 4.02439 3.91304 5.16521 4.82927 4.56522 6.02608 5.63415 5.21739 6.88695 6.43902 5.86957 7.74782 7.24390 1.86992 1.79085 1.31330 2.80488 2.68627 1.96996 3.73984 3.58170 2.62661 4.67480 4.47712 3.28326 5.60975 5.37255 3.93991 6.54471 6.26797 4.59656 7.47967 7.16340 5.25322 8.41465 8.05882" 5.9098T 858 TABLE IV. TABLE IV. Elements. Found. Sought. Barium. Bismuth Boron Bromine... Cadmium. . . Calcium. . . Carbon Chlorine... Chromium . Cobalt. Barium carbonate BaCO 3 Barium silico-fluoride BaFVSiFl 4 Bismuth tri oxide Bi 2 O 3 Boracic anhydride B a 3 Silver bromide AgBr Cadmium oxide CdO Lime CaO Calcium sulphate CaSO 4 Calcium carbonate CaCO 3 Carbonic acid C0 2 Calcium carbonate CaCO 3 Silver chloride AgCl Silver chloride AgCl Chromic oxide Cr a O 3 Chromic oxide Cr 2 O 3 Lead chromate PbCrO 4 Cobalt Co Cobaltous sulphate CoSO 4 Baryta BaO Baryta BaO Bismuth Bi Boron B Bromine Br Cadmium Cd Calcium Ca- Lime CaO Lime CaO Carbon C Carbonic acid CO 2 Chlorine Cl Hydrochloric acid HC1 Chromium Cr Chromic anhydride CrO 3 Chromic anhydride Cr0 3 Cobaltous oxide CoO Cobaltous oxide CoO TABLE IV. 859 (Continued). 2 3 4 5 * 7 8 9 1.55330 2.32995 3.10660 3.88325 4.65990 5.43655 6.21320 6.98985 1.09677 1.64516 2.19355 2.74194 3.29032 3.83871 4.38710 4.93548 1.79310 2.68965 3.58620 4.48275 5.37930 6.27586 7.17240 8.06895 0.62857 0.94286 1.25714 1.57143 1.88572 2.20000 2.51429 2.82857 0.85107 1.27661 1.70215 2.12768 2.55322 2.97876 3.40430 3.82983 1.75000 2.62500 3.50000 4.37500 5.25000 6.12500 7.00000 7.87500 1.42857 2.14286 2.85714 3.57143 4.28571 5.00000 5.71429 6.42857 0.82353 1.23529 1.64706 2.05882 2.47059 2.88235 3.29412 3.70588 L 12000 1.68000 2.24000 2.80000 3.36000 3.92000 4.48000 5.04000 0.54546 0.81818 1.09091 1.36364 1.63636 1.90909 2.18181 2.45455 0.88000 1.32000 1.76000 2.20000 2.64000 3.08000 3.52000 3.96000 0.49460 0.74188 0.98919 1.23649 1.48378 1.73108 1.97838 2.22568 0.50854 0.76281 1.01708 1.27135 1.52563 1.77990 2.03417 2.28844 * 1.37238 2.05858 2.74477 3.43096 4.11715 4.80334 5.48954 6.17573 2.62762 3.94142 5.25523 6.56904 7.88285 9.19666 10.51046 11.82427 0.62124 0.93187 1.24249 1.55311 1.86373 2.17435 2.48498 2.79560 2,54237 3.81356 5.08474 6.35593 7.62712 8.89830 10.16949 11.44067 0.96774 1.45161 1.93548 2.41935 2.90323 3.38710 3.87097 4.35484 860 TABLE IV. TABLE IV. Elements. Found, Sought. Cobalt Copper Fluorine. Hydrogen. Iodine. . . . Iron Lead Lithium.. Cobaltous sulphate + potassium sulphate 2(CoSO 4 ) -|- 3(K 2 SO 4 ) Cobaltous sulphate + potassium sulphate 2(CoSO 4 )-f 3(K 3 SO 4 ) Cupric oxide CuO Cuprous sulphide Cu 2 S. Calcium fluoride CaFl 2 Silicon fluoride SiFl 4 Water H 2 O Silver iodide Agl Palladious iodide PdI 3 Ferric oxide Fe 2 O 3 Ferric oxide Fe 2 3 Ferrous sulphide FeS Lead oxide PbO Lead sulphate PbS0 4 Lead sulphate PbSO 4 Lead sulphide PbS Lithium carbonate Li 2 Co 3 Cobaltous oxide CoO Cobalt Co Copper Cu Copper Cu Fluorine Fl Fluorine Fl Hydrogen H Iodine I Iodine I Iron Fe Ferrous oxide FeO Iron Fe Lead Pb Lead oxide PbO Lead Pb Lead oxide PbO Lithia Li 2 TABLE IV 861 (Continued). 2 3 45678 9 0.36024 0.54036 0.72048 0.90060 1.08072 1.26084 1.44096 1.62108 0.28339 0.42508 0.56676 0.70847 0.85016 0.99186 1.13355 1.27525 1.59698 2.39547 3.19396 3.99244 4.79093 5.58942 6.38791 7.18640 1.59698 0.97436 2.39547 1.46154 3.19396 1.94872 3,99244 2.43590 4.79093 2.92307 5.58942 3.41027 6.38791 3.89743 7.18640 4.38461 1.46154 2.19231 2.92308 3.65385 4.38461 5.11538 5.84615 6.57692 0.22222 0.33333 0.44444 0.55555 0.66667 0.77778 0.88889 1.00000 1.08059 1.62088 2.16118 2.70147 3.24176 3.78206 4.32235 4.86264 1.40835 2.11252 2.81670 3.52087 4.22505 4.92922 5.63340 6.33757 1.40000 1.80000 2.10000 2.70000 2.80000 3.60000 3.50000 4.50000 4.20000 5.40000 4.90000 6.30000 5.60000 7.20000 6.30000 8.10000 1.27273 1.90909 2.54546 3.18182 3.81818 4.45455 5.09091 5.72728 1.85650 2.78475 3.71300 4.64126 5.56951 6.49776 7.42601 8.35426 1.47195 2.20792 2.94390 3.67987 4.41584 5.15182 5.88779 6.62377 1.36634 2.04950 2.73267 3.41584 4.09901 4.78218 5.46534 6.14851 1.86611 0.81081 2.79916 3.73222 1.21622 : 1.62162 4.66527 2.02703 5.59832 2.43243 6.53138 2.83784 7.46443 3.24324 8.39749 3.64865 862 TABLE IV TABLE IV. Elements. Found. Sought. Lithium Magnesium. Manganese. Mercury Nickel... Nitrogen. Lithium sulphate Li 2 SO 4 Lithium phosphate Li 3 PO 4 Magnesia MgO Magnesium sulphate MgS0 4 Magnesium pyrophosphate Mg 2 P 2 O 7 Manganous oxide MnO Protosesquioxide of manganese MnO + Mn 2 3 Manganic oxide Mn 2 O 3 Manganous sulphate MnS0 4 Manganous sulphide MnS Manganous sulphide MnS Mercury Hg Mercury Hg Mercurous chloride Hg 2 Cl 2 Mercuric sulphide HgS Nickelous oxide NiO Ammonium platinic chloride (NH 4 C1) 2 , PtCl 4 Platinum Pt Lithia Li 2 Lithia Li 2 O Magnesium Mg Magnesia MgO Magnesia MgO Manganese Mn Manganese Mn Manganese Mn Manganous oxide MnO Manganous oxide MnO Manganese Mn Mercurous oxide Hg 2 Mercuric oxide HgO Mercury M Hg Mercury Hg Nickel Ni Nitrogen N Nitrogen N TABLE IV. 863 ( Continued}. 2 3 4 5 7 8 9 ; 0.54545 0.81818 1.09091 1.36364 ! 1.63636 1.90909 2.18182 2.45454 0.77586 1.16379 1.55172 1.93966 2.32759 2.71552 3.10345 3.49138 1.20061 1.80091 2.40121 3.00151 3.60182 4.20212 4.8024-2 5.40273 0.66700 1.00051 1.33401 1.66751 2.00101 2.33451 2.66802 3.00152 0.72072 1.08108 1.44144 1.80180 2.16216 2.52252 2.88288 3.24324 1.54930 2.32394 3.09859 3.87324 4.64789 5.42254 6.19718 6.97183 1.44105 2.16157 2.88210 3.60262 4.32314 5.04367 5,76419 6.48472 1.39241 0.94040 2.08861 1.41060 2.78481 1.88080 3.48102 2.35099 4.17722 2.82119 4.87342 3.29139 5.56962 3.76159 6.26583 4.23179 1.63218 2.44828 3.26437 4.08046 4.89655 5.71264 6.52874 7.34483 1.26437 1.89655 2.52874 3.16092 3.79310 4.42529 5.05747 5.68966 2.08000 3.12000 4.16000 5.20000 6.24000 7.28000 8.32000 9.36000 2.16000 3.24000 4.32000 5.40000 6.48000 7.56000 8.64000 9.72000 1.69880 2.54820 3.39760 4.24701 5.09641 5.94581 6.79521 7.64461 1.72414 2.58621 3.44828 4.31034 5.17241 6.03448 6.89655 7.75862 1.57333 0.12591 2.36000 0.18887 3.14667 0.25182 3.93333 0.31478 4.72000 0.37774 5.50667 0.44069 6.29334 0.50365 7.08000 0.56660 0.28482 0.42722 0.56963 0.71204 0.85445 0.99686 1.13926 1.28167 864 TABLE IV. TABLE IV. Elements. Found. Sought. Nitrogen. . . Oxygen Silver cyanide AgCN Silver cyanide AgCN Alumina A1 2 O 3 Antimonious oxide Sb 2 O 3 Arsenious oxide As 2 O 3 Arsenic oxide As 2 O 5 Baryta BaO Bismuth trioxide Bi 2 3 Cadmium oxide CdO Chromic oxide Cr 2 3 Cobaltous oxide CoO Cupric oxide CuO Ferrous oxide FeO Ferric oxide Fe 2 O 3 Lead oxide PbO Lime CaO Magnesia MgO Manganous oxide MnO Cyanogen CN Hydrocyanic acid flCN Oxygen O Oxygen O Oxygen O Oxygen Oxygen Oxygen O ;n Oxygen O Oxygen O Oxygen O TABLE IV. 865 (Continued). 2 3 4 5 6 j 7 8 9 0.38874 0.40367 0.93204 0.58312 0.60551 1.39806 0.77749 0.80734 1.86408 0.97186 1.00918 2.33010 1.16623 1.21102 2.79611 1.36060 1.41285 3.26213 1.55498 1.61469 3.72815 1.74935 1.81652 4.19417 0.32877 0.48484 0.69565 0.49315 0.72726 1.04348 0.65754 0.96968 1.39130 0.82192 1.21210 1.73913 0.98630 1.45452 2.08696 1.15069 1.69694 2.43478 1.31507 1.93936 2.78261 1.47946 2.18178 3.13043 0.20915 0.20690 0.25000 0.31373 0.31035 0.37500 0.41830 0.41380 0.50000 0.52288 0.51725 0.62500 0.62745 0.62070 0.75000 0.73203 0.72415 0.87500 0.83660 0.82760 1.00000 0.94118 0.93105 1.12500 0.62762 0.42667 0.40302 0.94143 0.64000 0.60453 1.25524 0.85333 0.80604 1.56905 1.06667 1.00756 1.88286 1.28000 1.20907 2.19667 1.49333 1.41058 2.51048 1.70666 1.61209 2.82429 1.92000 1.81360 0.44444 0.60000 0.14350 0.66667 0.90000 0.21525 0.88889 1.2000Q 0.28700 1.11111 1.50000 0.35874 1.33333 1.80000 0.43049 1.55555 2.10000 0.50224 1.77778 2.40000 0.57399 2.00000 2.70000 0.64574 0.57143 0.79939 0.45070 0.85714 1.19909 0.67606 1.14286 1.59879 0.90141 1.42857 1.99849 1.12676 1.71429 2.39818 1.35211 2.00000 2.79788 1.57746 2.28571 3.19758 1.80282 2.57143 3.59727 2.02817 866 TABLE IV. TABLE IV. Elements. Found. Sought. Oxygen. Phosphorus... Protosesquioxide of Manganese MnO + Mn 2 O 3 Manganic oxide Mn 2 O 3 Mercurous oxide Hg 2 0' Mercuric oxide HgO Niekelous Oxide NiO Potassa K 2 O Silicic anhydride Si0 2 Silver oxide Ag 2 O Soda Na 2 O Strontia SrO Stannic oxide SnO 2 Water H 2 O Zinc oxide ZnO Phosphoric anhydride P 2 5 ium pyrophosphate M g2 P 2 7 Ferric phosphate FeP0 4 Silver phosphate Ag 3 PO 4 Uranyl pyrophosphate (U0 2 ) 2 P 2 7 ;en Oxygen Oxygen Oxygen Oxygen O Oxygen O Oxygen Oxygen O Oxygen Oxygen Oxygen O Oxygen Phosphorus P Phosphoric anhydride P 2 5 Phosphoric anhydride P 2 5 Phosphoric anhydride P 2 6 * Phosphoric anhydride P 2 5 TABLE IV. 867 (Continued). 2 3 4 5 6 7 8 9 0.55895 0.83843 1.11790 1.39738 1.67686 1.95633 2.23581 2.51528 0.60759 0.91139 1.21519 1.51899 1.82278 2.12658 2.43038 2.73417 0.07692 0.11539 0.15385 0.19231 0.23077 0.26923 0.30770 0.34616 0.14815 0.22222 0.29630 0.37037 0.44444 0.51852 0.59259 0.66667 0.42667 0.64000 0.85333 1.06667 1.28000 1.49333 1.70667 1.92000 0.33949 0.50923 0.67897 0.84871 1.01846 1.18820 1.35794 1.52768 1.06667 1.60000 2.13333 2.66667 3.20000 3.73333 4.26667 4.80000 0.13801 0.20702 0.27603 0.34503 0.41404 0.48305 0.55206 0.62106 0.51546 0.77320 1.03093 1.28866 1.54639 1.80412 2.06186 2.31959 0.30918 0.46377 0.61836 0.77295 0.92753 1.08212 1.23671 1.39130 0.42667 0.64000 0.85333 1.06667 1.28000 1.49333 1.70667 1.92000 1.77778 2.66667 3.55556 4.44445 5.33333 6.22222 7.11111 8.00000 0.39480 0.59220 0.78960 0.98700 1.18440 1.38180 1.57920 1.77660 0.87324 1.30986 1.74648 2.18309 2.61971 3.05633 3.49295 3.92957 1.27928 1.91892 2.55856 3.19820 3.83784 4.47748 5.11712 5.75676 0.94040 0.33907 1.41060 0.50860 1.88080 0.67814 2.35099 0.84767 2.82119 1.01721 3.29139 1.18674 3.76159 1.35628 4.23179 1.52581 0.39821 0.59731 0.79641 i 0.99551 1.19462 1.39372 1.59282 1.79192 868 TABLE IV TABLE IV. Elements. Found. Sought. 1 Potassium . . . Potassa Potassium 0.83026 K 2 O K Potassium sulphate Potassa 0.54091 K 2 SO 4 K 2 Potassium chloride Potassium 0.52460 KC1 K Potassium chloride Potassa 0.63185 KC1 K 2 Potassium platinic chloride Potassa 0.19308 (KCl) 2 PtCl 4 K 2 Potassium platinic chloride Potassium chloride 0.30557 (K01) 2 PtCl 4 KC1 Silicon Silicic anhydride Silicon 0.46667 SiO 2 Si Silver Silver chloride Silver 0.75270 AgCl Ag Silver chloride Silver oxide 0.80849 AgCl Ag 2 O Sodium . Soda Sodium 0.74227 Na 2 Na Sodium sulphate Soda 0.43694 Na 2 SO 4 Na 2 O Sodium chloride Soda 0.53060 Nad Na 2 O Sodium chloride Sodium 0.39384 NaCl Na Sodium carbonate Soda 0.58522 Na 2 CO 3 Na 2 Strontium. . . . Strontia Strontium 0.84541 SrO Sr Strontium sulphate Strontia 0.56403 SrSO 4 SrO Strontium carbonate Strontia 0.70169 SrCO 3 SrO Sulphur .... Barium sulphate Sulphur 0.13734 BaSO 4 S TABLE IV. 869 (Continued). 2 3 4 .56789 1.66051 1.08183 2.49077 1.62274 3.32103 2.16366 4.15128 2.70457 4.98154 i 5.81180 3.24549 ; 3.78640 6.64206 432732 7.47231 4.86823 1.04920 1.57380 2.09840 2.62300 3.14761 3.67221 419681 4.72141 1.26371 1.89556 2.52742 3.15927 3.79112 4.42298 5.05483 5.68669 0.38615 0.57923 0.77230 0.96538 1.15846 j 1.35153 1.54461 1.73768 0.61114 0.91671 1.22228 1.52785 1.83343 2.13900 2.44457 2.75014 0.93333 1.40001 1.86667 2.33333 2.80000 3.26667 3.73333 4.20000 1.50540 2.25811 3.01081 3.76351 4.51621 5.26891 6.02162 6 77432 1.61700 2.42548 3.23398 4.04247 485096 5.65946 6.46795 7.27645 1.48454 0.87387 2.22680 1.31081 2.96907 1.74775 3.71134 2.18468 4.45361 2.62162 5.19588 3.05856 5.93814 3.49550 6.68041 3.93243 1.06120 1.59179 2.12239 2.65299 3.18359 3.71419 4.24478 4.77538 0.78769 1.18154 1.57538 1.96923 2.36308 2.75692 3.15077 3.54461 1.17044 1.69082 1.75566 2.53623 2.34088 3.38164 2.92610 4.22705 3.51132 5.07247 4.09654 5.91788 4.68176 6.76329 5.26698 7.60870 1.12807 1.69210 2.25613 2.82017 3.38420 3.94823 4.51226 5.07630 1.40339 2.10508 2.80678 3.50848 4.21017 4.91186 5.61356 6.31526 0.27468 0.41202 0.54936 0.68670 0.82403 0.96137 1.09871 \ 1.23605 870 TABLE IV. TABLE IV. Elements. Found. Sought. 1 Sulphur Arsenious sulphide Sulphur 39024 As 2 S 3 S Barium sulphate BaSO 4 Sulphuric anhydride S0 3 0.34335 Tin Stannic oxide Tin 78667 SnO 2 Sn Stannic oxide Stannous oxide 0.89333 SnO 2 SnO Zinc Zinc oxide Zinc 80260 ZnO Zn Zinc sulphide Zinc oxide 0.83515 ZnS ZnO Zinc sulphide ZnS Zinc Zn 0.67031 TABLE IV. 871 (Continued). 2 u 4 5 6 7 8 9 0.78049 1.17073 1.56097 1.95122 2.34146 2.73170 3.12194 3.51219 0.68670 1.03004 1.37339 1.71674 2.06009 2.40344 2.74678 3. 09013 ' 1.57333 2.36000 3.14667 3.93333 472000 5.50667 629334 7.08000 1.78667 2.68000 3.57333 4.46667 5.36000 6.25333 7.14666 8.04000 1.60520 2.40780 3.21040 4.01300 4.81560 5.61820 6.42080 ' 7.22340 1.67031 2.50546 3.34062 4.17577 5.01092 5.84608 6.68123 7.51639 1.34061 2.01092 2.68123 3.35154 4.02184 4.69215 5.36246 6.03276 872 TABLES V. VI. TABLE V. SPECIFIC GRAVITY AND ABSOLUTE WEIGHT OF SEVERAL GASES. Atmospheric air Oxygen Hydrogen Water, vapor of Carbon, vapor of Carbon dioxide Carbon monoxide. . . . Marsh gas Elayl gas Phosphorus, vapor of. Sulphur, vapor of. . . . Hydrosulphuric acid. Iodine, vapor of Bromine, vapor of . . . . Chlorine Nitrogen Ammonia Cyanogen , Specific gravity, atmos- pheric air = 1 -0000. 1 litre (1000 cubic centi- metres) of gas at and 0*76 metre bar. pressure weighs grammes. 1-0000 1-10832 0-06927 0-62343 0-83124 1 -52394 0-96978 0-55416 0-96978 4-29474 6-64992 1-17759 8-78898 5-53952 2-45631 0-96978 0-58879 1-80102 1-29366 1-43379 0-08961 0-80651 1-07534 1-97146 1 -25456 0-71689 1-25456 5-55593 8-60273 1-52340 11-36995 7-16625 3-17763 1-25456 0-76169 2 32991 TABLE VI. COMPARISON OF THE DEGREES OF THE MERCURIAL THERMOMETER WITH THOSE OF THE AIR THERMOMETER. According to MAGNUS. Degrees of the mercurial thermometer. Degrees of the air thermometer. 100 100-00 150 148-74 200 197-49 250 245-39 300 294-51 330 . . 320-92 ALPHABETICAL INDEX, PAGE ACETIC Aero (reagent), see Qual. Anal, Table of specific gravities 679 Acidimetry 675 Air, analysis of atmospheric 722 Air-pump, Sprengel's mercury 639 Alcohol (reagent), see Qual. Anal, and 106 Alkalimetry 691 Aluminium 149* Determination 240 Basic acetate of 151 Basic formate of 151 Hydroxide 149 Oxide 150 Separation from alkali metals 499 alkali-earth metals 500 chromium 500 Ammonia (reagent) 109 Ammonium 137 Arsenio-molybdate , , 193 Carbonate (reagent), see Qual. Anal. Chloride ' 137 Chloride (reagent), see Qual. Anal. Determination , 217 Ferrous sulphate (reagent) 118 Molybdate (reagent), see Qual. Anal. Magnesium arsenate 191 Nitrate (reagent) 115 Oxalate (reagent), see Qual. Anal. Phosphomolybdate 198 Platinic chloride 137 Separation from metals of group IV. 507 other alkali metals 481 Sulphide (reagent), see Qual. Anal. Succinate (reagent), see Qual. Anal. Antimonious sulphide 186 874 ALPHABETICAL INDEX. PAGE Antimony 185 Determination 231 Separation from other metals of group VI 569 metals of groups I. V 554 Tetroxide 187 Arsenic, detection and estimation in presence, of organic matter 781 Arsenic (arsenious and arsenic acids). Separation from other metals of group VI 569 metals of groups I. V 554 Arsenic acid, determination 344 Separation from other acids 580 Arsenious acid, determination 344 Separation from other acids . 580 arsenic acid 574 Oxide 190 Sulphide 190 Asbestos filters 100 Auric sulphide 574 Azotometer, Schiff's 638 Balance. Barium 1 138 Acetate (reagent) 112 Carbonate (reagent), see Qual. Anal. Carbonate 140 Chloride (reagent) 112 Chromate 194 Hydroxide (reagent), see Qual. Anal. Determination 227 Separation from other alkali-earth metals 493 alkali metals 488 Silicofluoride 141 Sulphate 138 Bismuth 180 Basic chloride 181 Basic nitrate , 181 Carbonate 181 Chromate 181 Determination 318 Separation from other metals of group V 543 metals of groups I. IV 536 Trioxide 180 Trisulphide 182 Borax fused (reagent) 114 Boric acid 200 Determination 389 Separation from basic radicals 392 Bromine, determination 436 Separation from acid radicals of group 1 588 group II 592 ALPHABETICAL IXDEX. 875 PAGE Bunsen's filtering apparatus 93 Burette, Mohr's 36 Gay-Lussac's 40 Giessler's 41 Cadmium 182 Carbonate 182 Determination . . . 323' Oxide 182 Separation from other metals of group Y 543 metals of groups I. IY 536 Sulphide 183 Calcium 143 Carbonate 143 Chloride (reagent), see QuaL Anal, reagent for organic analysis 127 Determination 232 Fluoride 200 Hydroxide (reagent) 109 Oxalate 145 Oxide 146 Sulphate 143 Separation from the alkali metals 488 other alkali-earth metals 493 Calculation of analyses 834 Carbonic acid 201 Determination. ... 403 in atmospheric air 722 Separation from basic radicals 407 all other acids 587 Chloric acid 206 Determination 476 Separation from basic radicals 476 acids of groups I. and II 602 nitric acid 603 Chlorine, determination 428 in silicates 589 (Reagent) 116 Separation from basic radicals 431 other acids of group II 592 acids of group 1 588 fluorine 590 Chlorine water (reagent), see Qiial. Anal. Chlorimetry 698 Chromic acid 193 Determination 355 Separation from basic radicals 358 other acids of group 1 580 Chromium 151 Determination. . 242 876 ALPHABETICAL INDEX. PAGE Chromium Hydroxide 151 Oxide 152 Separation from alkali metals 499 alkali-earth metals 500 aluminium 499 Coal, analysis. 765 Cobalt ' -. 161 Determination . 262 Ore, assay 731 Cobaltous hydroxide * . < 161 Sulphate 163 Sulphide 162 (Cobaltic compound), tripotassium cobaltic nitrite 163 Combustion, see Organic Analysis. Copper 177 Metallic (reagent for organic analysis) 126 Determination 311 Ore, assay 728 Separation from other metals of group V 543 metals of groups I. IV. . . . : - 536 Cupric oxide 177 (Reagent for organic analysis) , 123 and 637 Sulphide 179 Cuprous oxide 179 Sulphide 180 Sulphocyanate 179 Cyanogen, determination 449- Separation from basic radicals 451 acid radicals of group II. 600 group 1 588 Cylinder, graduated 32 Distilled water. 105 Dolomite, analysis. 720 Drying precipitates r . . 84 Drying substances for analysis 46 55 Ether (reagent) 106 Errors in gravimetrical analyses 209 Evaporation 66 Ferric acetate (basic) 166 Chloride (reagent), see Qual. Anal. Hydroxide 164 Formate (basic) 166 Oxide 165 Phosphate 195 Succinate (basic) 166 Ferrous sulphate (reagent), see Qual. Anal. Sulphide 165 Ferro- and ferricyanogen, determination 454 Fertilizers, analysis 767 ALPHABETICAL INDEX. 877 PAGE Filtering apparatus 77 Formulae, calculations required for deducing 844 Gold 184 Determination 326 Separation from other metals of group VI 569 groups I. V 554 Gooch's method of filtering and igniting precipitates 100 Guano, analysis 770 Gunpowder, analysis 713 Hydriodic acid 204 Hydrobromic acid 203 Hydrochloric acid 203 (Reagent) 107 Hydrocyanic acid, 205 Hydrofluoric acid 200 Use for testing silica. 422 Hydrofluosilicic acid, determination 372 (Reagent), see Qual. Anal. Hydrosulphuric acid 205 Hydrogen gas (reagent), preparation of 116 Hydrogen sulphide (reagent), see QuaL Anal. Igniting precipitates 71 85 Bunsen's method 98 Gooch's method 100 lodic acid, determination 364 Iodine, determination 439 (Reagent) 120 Separation from basic radicals 442 acid radicals of group 1 588 group II 592 Iron 164 Determination in ferric compounds 275 Ferrous compounds 265 Separation from alkali-earth metals 509 metals of groups III. and IV 512 Determination of ferrous in presence of ferric 526 Iron ore, partial analysis 740 Complete analysis 753 Iron, wrought, analysis 765 Pig, analysis 758 Lead \ 170 Acetate (reagent), see QuaL Anal. Arsenate 190 Carbonate 170 Chloride 172 Chromate 193 Chromate (reagent for organic analysis) 124 Determination 297 Oxalate.. 170 878 ALPHABETICAL INDEX. PAGE Lead Oxide , 171 (Reagent) 110 Ore, assay 730 Phosphate , 195 Separation from other metals of group V 543 metals of groups I. IV 536 Sulphide. 173 Levigation 44 Limestone, analysis 720 Lithium carbonate 226 Determination 226 Phosphate 226 Separation from other alkali metals 481 Sulphate 226 Litmus 117 Litre flask . 31 Magnesia (or magnesium) mixture (reagent) 113 Magnesium 146 Ammonium magnesium phosphate 147 Determination 237 Oxide 149 Phosphate 195 Pyroarsenate 192 Pyrophosphate 148 Separation from other alkali-earth metals 493 the alkali metals 488 Sulphate 146 Manganese 155 Ammonium manganese phosphate 158 Carbonate 155 Determination 251 Dioxide 156 Hydroxide 156 Ore, estimation of oxygen in 705 Protosesquioxide 156 Pyrophosphate 159 Separation from alkali-earth metals 509 metals of groups III. and IV 512 Measuring of gases 25 Measuring of fluids 30 Mercuric chloride (reagent), see Qual. Anal. Oxide 1 76 Sulphide 176 Mercurous chromate 194 Chloride 174 Phosphate 193 Mercury 174 Determination in mercuric compounds 306 mercurous compounds 304 ALPHABETICAL INDEX. 879 PAGE Mercury Separation from other metals in group V 548 metals of groups I. IV 536 Metastannic acid 188 Metastannic chloride. . . . 188 Molybdic acid, determination 353 Nickel 159 Determination , 258 Hydroxide 159 Metallic 160 Oxide 159 Sulphate 160 Sulphide 160 Separation from alkali-earth metals 509 metals of groups III. and IV 512 Nickel ore, assay 731 Nitric acid 206 (Reage n t) 1 06 Determination 469 Separation from basic radicals 469 chloric acid 603 acids of groups I. and II 602 Nitrogen 138 Determination in organic compounds 634, 637 644, Nitrohydrochloric acid (reagent), see Qua!. Anal. Nitrous acid, determination 365 Normal solutions, mode of preparing 687 ORGANIC ANALYSIS 604 By combustion with cupric oxide 610 lead chromate 620 oxygen gas 621 Organic analysis of compounds containing nitrogen 631 alkalies 664 alkali-earth metals 664 halogens 661 sulphur 649 Organic analysis, qualitative 606 Oxalic acid 200 Pure (reagent) 117 Determination 394 Separation from basic radicals 395 Oxygen gas (reagent for organic analysis). ... 125 Palladious iodide 205 Palladium, determination 325 Phosphoric acid 195 Determination 373 Separation from basic radicals 383 all other acids 582 Phosphomorybdate of ammonium 198 Phosphorus, determination in organic compounds 660 880 ALPHABETICAL INDEX. PAGE Pipette, graduated 33 Platinic chloride (reagent), see Qual. Anal. Potassium platinic chloride 185 Sulphide 185 Platinum 184 Determination 329 t Separation from other metals of group VI 569 metals of groups I. V 554 Potassa (reagent) 109 (Fused reagent for organic analysis) 127 Solution (for organic analysis) 127 Potassium 132 Boro-fluoride. 200 Chloride , 133 Cyanide, see Qual. Anal. Determination 210 Dichromate (reagent), see Qual. Anal. Disulphate (reagent) 118 Iodide (reagent) 121 Nitrate (reagent), see Qual. Anal. Nitrite (reagent), see Qual. Anal. Permanganate (reagent) 118 Platinic chloride 134 Separation from other alkali metals 481 metals of group IV 508 Silicofluoride 134 Sulphate 132 (reagent), see Qual. Anal. Precipitates, separation from fluids 7576 Precipitation 74 Eeagents 105 Rocks, analysis 714 Salt, analysis of common 711 Samples, selection of 42 Mechanical division of. . . . , 43 Selenious acid, determination 361 Separation of acid radicals from each other 579 Sifting 45 .Silicates, analysis 714 719 Decomposition by fusion 422 Separation of alkalies from 426 Silicic acid. 201 Determination ... 419 Separation from basic radicals 419 other acids 586 Silver 167 Bromide 203 Chloride 167 Cyanide 170 ALPHABETICAL INDEX. 881 PAGE Silver Determination 283 Iodide 204 Metallic (reagent) 122 Nitrate (reagent), see Qual. Anal. Phosphate 198 Separation from other metals of group V 543 metals of groups I. IV 536 Sulphide -. 169 Soda lime 125 Soda lime for nitrogen determinations 126 Sodium 135 Acetate (reagent), see Qual. Anal. Carbonate (reagent), see Qual. Anal. Chloride (reagent) 122 Chloride 135 Determination 215 Hydrogen sulphide (reagent), see Qual. Anal. Nitrate (reagent), see Qual. Anal. Platinic chloride (reagent), see' Qual. Anal. Platinic chloride 136 Separation from other alkali metals 481 metals of group IV 508 Sulphate , 135 Thiosulphate (reagent) . Ill Solution of substances for analysis 63 Sprengel's mercury air-pump 639 Stannic oxide 188 Phosphate 198 Sulphide 189 Stannous chloride (reagent), see Qual. Anal. Sulphide 189 Steel analysis 765 Strontium 141 Carbonate 142 Chloride (reagent) 113 Determination 230 Separation from the alkali metals 488 other alkali-earth metals 493 Sulphate 141 Sulphur, determination 457 in organic compounds 649 658 in presence of carbonates 591 in silicates 590 Separation from metals 461 Sulphuric acid, determination 366 (Reagent), see Qual. Anal, and 106 Separation from basic radicals 370 other acids 580 Sulphurous acid, determination 363 882 ALPHABETICAL INDEX. PAGE TABLES showing Atomic weights 849 Absorption of nitrogen in bromized hypochlorite solution. 223 Weights of volumes of nitrogen 225 Composition of oxides 849 Strength of acids corresponding to various specific gravities. 676 Strength of alkalies corresponding to various specific gravi- ties . . 691 for Calculation of analyses 854 871 Tartaric acid (reagent), see Qual. Anal. Tin, determination 338 Thiosulphuric acid, determination 364 Uranium, determination 281 Uranyl (uranic) acetate (reagent) 114 Pyroarsenate 192 Pyrophosphate 197 Volumetric analysis (general) 102 VOLUMETRIC determination of Acids in the free state, see Acidimetry. Alkali hydroxides and carbonates, see Alka- limetry. Alkali-earth metals 697 Antimony 335 Arsenic acid 351, 579 Arsenious acid 350 Bromine (in bromides) 437 free 443 Cadmium 324 Calcium 235, 697 Copper 317 Chloric acid 476 Chlorine (in chlorides) 428 free 434 Chromic acid 356, 357 Cyanogen 450 Ferric iron 278280 Ferro- and ferricyanogen 454 Ferrous iron 267 Fluorine 402 Iodine (in iodides) 440 free 443 Lead 303 Manganese 257 Mercury 305, 310 Oxalic acid 394 Potassium 214 Phosphoric acid 380 Silver 288 Sulphuric acid ' 367 ALPHABETICAL INDEX. 883 PAGE VOLUMETRIC determination of Tin 343 Zinc 737 Zinc 152 Carbonate 152 Determination 247 Metallic (reagent) 110 Oxide 153 Ore, assay 737 Separation from alkali-earth metals 509 metals of groups III. and IV 512 Sulphide 154 RETURN CIRCULATION DEPARTMENT TO * 202 Main Library LOAN PERIOD 1 HOME USE 2 3 4 5 6 ALL BOOKS MAY BE RECALLED AFTER 7 DAYS 1 -month loans may be renewed by calling 642-3405 6-month loans may be recharged by bringing books to Circulation Desk Renewals and recharges may be made 4 days prior to due date DUE AS STAMPED BELOW NOV 2 3 1982 83; MAY 23 1983 " CT22 3 RECPIVFD A I If* on UNIVERSITY OF CALIFORNIA, BERKELEY FORM NO. 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