SOLUBILITIES OF INORGANIC AND ORGANIC SUBSTANCES A HANDBOOK OF THE MOST RELIABLE QUANTITATIVE SOLUBILITY DETERMINA TIONS RECALCULATED AND COMPILED BY ATHERTON SEIDELL, PH.D. (J-H.U.) Chemist, Division of Pharmacology, Hygienic Laboratory of the U. S Public Health and Marine-Hospital Service, Washington, D. C~ Formerly Assistant Chemist, Bureau of Chemistry U. S. Department of Agriculture FOURTH PRINTING CORRECTED NEW YORK D. VAN NOSTRAND COMPANY 25 PARK PLACE 1917 COPYRIGHT, 1907 AND 1911 BY D. VAN NOSTRAND COMPANY Stanhope preea N. OILBON COMPANY BOBTO N. U. S. A. PREFACE DURING the years which have elapsed since Professor Arthur M. Comey's admirable "Dictionary of Chemical Solubilities" went to press (March, 1894), the literature upon solubilities has grown to such an extent that it has appeared desirable to make a new compilation of it. Soon after beginning work upon this volume the author realized that it would not be possible to prepare a com- pilation of solubility results which would fulfill completely the various requirements of theoretical, technical, analytical, and other classes of chemists, and he has therefore endeavored to meet some of the needs of all chemists rather than provide information especially arranged for any particular class. The following features have been considered of chief impor- tance in preparing the present compilation: completeness of the data, reliability of the determinations, uniformity in expression of results, convenience of arrangement of material, and the index- ing of the cross-references to tables. The material has been collected almost entirely from the origi- nal sources, and not from text-books or works of reference. The plan followed has been to search diligently the tables of con- tents or indices of twenty -five of the principal chemical journals issued since 1875, and to consult all articles in these as well as in other journals to which references could be obtained. In this connection, however, it should be stated that indexed references to work on solubility usually appear under the name of the sub- stance employed, and not under the heading "solubility." Fur- thermore, solubility determinations are often incidental to other investigations, and consequently are not indicated in the title of the article or included in the index of the journal. Consid- ering these difficulties there can be little hope of making such a compilation complete in every detail, and in the present case the best that can be said is that an earnest effort has been made to omit nothing of importance. This has been done not only for the author's personal satisfaction in perfecting the work, but also to give the reader a reasonable assurance that the ab- sence from these pages of results upon a particular substance is good evidence that such determinations of satisfactory reliability iii 395316 PREFACE are not readily obtainable from the usually accessible chemical journals. Although at the time Professor Comey compiled his book it appeared inadvisable to attempt, in the majority of cases, to select the most reliable determinations of the solubility of the same substance reported by different investigators, the present author believes that this can now be done with advantage. The selections have been made in all cases by calculating the avail- able determinations to a common basis and drawing curves through the points plotted on cross-section paper. A comparison of the curves, together with a study of the details of the methods by which the determinations were made in the several cases, has usually furnished clear evidence for a reliable selection. For some substances, however, this plan could not be followed, and it has therefore been necessary to present two or more sets of disagreeing results. In many instances the calculations and study necessary to ascertain the most reliable figures have required much labor, and perhaps in some cases the author has not succeeded in selecting the ones nearest the truth; but it is believed that the economy of space required to present the material, and the saving of the time of the reader in making the necessary selections him- self, will far overbalance the disadvantage resulting from the accidental inaccuracies introduced through extended computa- tions. An additional advantage resulting from the recalculation of different determinations to a common basis is the increased uniformity in the expression of results throughout the volume. On this account it has been possible to give the solubility of most substances for regular intervals of temperature and in terms of weight of dissolved substance per given weight of solvent or of solution. Quantitative results alone have been included in this com- pilation, since it is assumed that qualitative determinations, if desired, can be readily made by simple tests in the laboratory, and therefore the effort necessary to collect such observations from the literature is out of proportion to the value of the inform- ation obtained. In regard to the names and formulas of the compounds in- cluded, the author wishes to say that they are, for the most part, given as found in the original papers from which they were taken ; and in some cases a lack of uniformity in the manner of their iv PREFACE expression will be noted. This is especially true of the molecules of water of crystallization in the formulas given in connection with the guide names placed in heavy type at the head of the tables for all substances considered. As is well known, many compounds, besides gaining or losing water in air, also crystal- lize with different numbers of molecules of water even at the ordinary temperature, and it was therefore thought best to include such information at the proper place in the tables under the heading "Solid Phase" rather than to select in doubtful cases the number of molecules of water which the particular substance was considered to carry under ordinary conditions. Although the arrangement of the material is alphabetical accord- ing to the customary English names, an index has been added which also provides for those cases where there appears a doubt as to which name is preferable, and furnishes cross-references to those tables which contain results upon more than one substance. A glance through the pages of this book will show the incom- pleteness of the data for many of the most common chemical compounds. Furthermore many of the results given are of doubtful accuracy, although the best available. It is hoped, therefore, that a realization of the present incomplete state of our information concerning solubilities as evidenced in these pages will stimulate investigations of many of those substances which have hitherto been studied incompletely or not at all. This volume went to press January ist, 1907, and the subject matter is brought up to November, 1906. In conclusion, the author begs all indulgence for errors and omissions, and will thank any one for calling them to his attention or making suggestions such as would improve a possible future edition of this "Handbook." A. S. WASHINGTON, D.C., Feb. 22, 1907. ABBREVIATIONS Abs. Absolute. Abs. Coef . Absorption Coefficient. Aq. or a.q. Aqueous. At. Atmosphere. b. pt. Boiling Point. cc. Cubic Centimeter. cone. Concentrated. d. Dextro. dt. Density. f. pt. Freezing Point. G., g., or gm. Gram. Gms. or gms. Grams. G.M. or Gm. Mol. Gram Molecule. /. Laevo. m. Meta. Mg. or mg. Milligram. Mgs. or mgs. Milligrams. Mg. Mol. Milligram Molecule. Millimols. Milligram Molecules. Mol. Molecule. m. pt. Melting Point. N. or n. Normal. o. Ortho. ord. Ordinary. p. Para. ppt. Precipitate. pptd. Precipitated. pt. Part. sat. Saturated. sol. Solution. Sp. Gr. Specific Gravity. t. Temperature in degrees C. temp. Temperature. vol. Volume. wt. Weight. vii ABBREVIATIONS OF TITLES OF JOURNALS Am. Ch. J. The American Chemical Journal, Baltimore. Am. J. Sci. American Journal of Science and Arts, New Haven. Analyst. The Analyst, London. Ann. See Liebig's Ann. Ann. chim. anal. appl. Annales de chimie analytique applique"e, Paris. Ann. chim. phys. Annales de chimie et de physique, Paris. Ann. Physik. A^nnalen der Physik und Chemie, Leipzig. See also Pogg. Ann. and Wied. Ann. Apoth.-Ztg. Apotheker Zeitung, Berlin. Arch. Pharm. Archiv der Pharmacie, Halle. Ber. Berichte der deutschen chemischen Gesellschaft, Berlin. Biedermann's Centr. Biedermann's Centralblatt fur Agrikulturchemie, u. s. w., Leipzig. Bull. soc. chim. Bulletin de la socie'te' chimique de Paris. Chem. Centralbl. Chemisches Centralblatt, Berlin. Chem. Ind. Die Chemische Industrie, Berlin. Chem. News. The Chemical News, London. Chem.-Ztg. Chemiker Zeitung, Cothen. Compt. rend. Comptes rendus hebdomadaires des Seances de 1'Academie des Sciences, Paris. Dingier pol. J. Dingier' s polytechnisch.es Journal, Stuttgart. Gazz. chim. ital. Gazzeta chimica italiana, Palermo. Jahresber. Chem. Jahresbericht iiber die Fortschritte der Chemie, Giessen. J. Am. Chem. Soc. Journal of the American Chemical Society, Easton. J. Anal. Chem. The Journal of Analytical and Applied Chemistry, Easton. T. Chem. Soc. Journal of the Chemical Society of London. '. pharm. chim. Journal de pharmacie et de chimie, Paris. r . Physic. Chem. Journal of Physical Chemistry, Cornell. : . pr. Chem. Journal fiir praktische chemie, Leipzig. \. russ. phys. chem. Ges. Journal of the Russian Chemical Society, St. Petersburg. J. Soc. Chem. Ind. Journal of the Society of Chemical Industry, London. Landw. Vers-Stat. Landwirthschaftlichen Versuchs-Stationen, Berlin. Liebig's Annalen. Justus Liebig's Annalen der Chemie, Leipzig. Monatsh. Ch. Monatshefte fur Chemie, u. s. w., Vienna. Mon. Sci. Le Moniteur Scientifique, Paris. Mulder. Scheikundige Verhandelingen en Onderzoekingen, Vol. 3, Pt. 3. Bijdragen tot de Geschiedenis van Het Scheikungig Gebonden Water by G. J. Mulder, Rotterdam, 1864. Pharm. J. Pharmaceutical Journal and Transactions, London. Phil. Mag. The Philosophical Magazine, London. Physic. Rev. Physical Review, Cornell. Pogg. Ann. Annalen der Physik und Chemie, edited by Poggendorf. See also Ann. Physik and Wied. Ann. Proc. Am. Acad. Proceedings of the American Academy of Arts and Sciences, Boston. Proc. Roy. Soc. Proceedings of the Royal Society of London. Rec. trav. chim. Recueil des travaux chimiques des Pays-Bas, Leiden. Sitzber. Akad. Wiss. Berlin. Sitzungsbericnte der koniglichen preussischen Akademie der Wissenschaften zu Berlin. Sitzber. Akad. Wiss. Wien. Sitzungsberichte der mathematische naturwissen- schaftlichen classe der kaiserlichen Akademie der Wissenschaften zu Wien. U. S. P. Pharmacopoeia of the United States, 8th Revision, 1900. ix ABBREVIATIONS OF TITLES OF JOURNALS Wied. Ann. Annalen der Physik und Chemie, edited by Wiederman. See also Pogg. Ann. and Ann. Physik. Wiss. Abh. p. t. Reichanstalt. Wissenschaftlichen Abhandlung der physik- alische technische Reichstalt, Charlottenburg. Z. anal. Chem. Zeitschrift fiir analytische Chemie, Wiesbaden. Z. angew. Chem. Zeitschrift fiir angewandte Chemie, Berlin. Z. anorg. Chem. Zeitschrift fur anorganische Chemie, Hamburg and Leipzig. Z. Elektrochem. Zeitschrift fiir Elektrochemie, Halle. Z. Krystallogr. Zeitschrift fiir Krystallographie und Mineralogie, Leipzig. Z. physik. Chem. Zeitschrift fiir pnysikalische Chemie, Leipzig. Z. Ver. Zuckerind. Zeitschrift fiir Rubenzucker-Industrie, Berlin. The above abbreviations with a few necessary exceptions are taken from the list adopted by the editor of the Journal of the American Chemical Society for the new abstract journal, "Chemical Abstracts," and will in general be familiar to many of those who use this volume. In a large number of in- stances Chem. has been contracted to Ch., but with this exception, and possibly a few inaccuracies which have slipped in, the abbreviations of journal titles used in this book conform to the above list. AOENAPHTHENE C 12 H 10 . SOLUBILITY IN SEVERAL ORGANIC SOLVENTS. (Speyers Am. J . Set. [4] 14, 294, 1902.) NOTE. In the original paper the results are given in terms of gram molecules of acenaphthene, acetamide, acetanilide, etc., per 100 gram molecules of solvent, at temperatures which varied with each solvent and with each weighing of the solutions. The tabulated results here given were obtained by recalculating and reading the figures from curves plotted on cross section paper. In Methyl Alcohol. In Ethyl Alcohol. In Propyl^Alcohol. t . ' (a)* (b)* (c)*" (a) (b) (c) ' (a) (b) (c) O 8l 33 1. 80 O 39 81 .1 1-9 o-57 82.3 2.26 0.88 IO 80 .40 1.70 O .38 80 3 2.8 0.84 8! .8 2.40 I .00 20 79 .60 2.25 O .48 79 .6 4.0 1.20 81.4 3-40 1 .35 30 79 .00 3-50 .72 79 .1 5-6 1.70 80.9 4-75 1.90 40 78 45 6.00 I .20 78 7 8.4 2.60 80.6 7.10 2.90 50 78 9.00 I 77 78 .8 13.2 3-90 80.7 II. 10 4.40 60 78 30 ii .70 2 35 79 4 23-2 7-00 81.5 19.60 8.20 70 78 .60 14.30 2 .90 80.75 40-5 I2.5O 83-9 37.00 16.20 In Chloroform. In Toluene. t . (a) (b) (c) (a) (ft) (c) 143 ,8 16.4 12.7 90.7 13.18 7-9 10 140 I 20.6 16.0 90.8 18.0 10.7 20 136 3 27.0 19-5 91.0 24-5 14-5 30 132 4 34-o 25.0 91.8 33-5 20.5 40 128 42-5 32.0 92.7 47-o 28.0 50 123, 4 40.0 94-o 60.5 35-7 60 119-3 62.5 50-0 95 5 74-o 43-5 70 97.2 89.0 52-5 AOETAMIDE CH 3 CO.NH 2 . SOLUBILITY IN WATER AND IN ALCOHOL. (Speyers.) In Water. In Ethyl Alcohol. t 8 . (a) (*) (c) (a) (b) W 105 5 70.8 29.6 85.62 17-3 18.5 10 104 9 81.0 34-o 86.2 24.0 26.0 20 104 3 97-5 40.8 87-3 31-5 33-8 30 103 7 114.0 47-7 88.8 40-5 43-o , 40 103 o 133 .0 55-5 90.7 50.0 53-5 SO 102 3 154.0 64.0 93 o 6s .0 64-5 . 60 101 6 177 5 74-o 95-5 72.0 76-5 ACETANILIDE C 6 H 5 NH.COCH 3 . 100 grams H 2 O dissolve 0.55 gram at 25, and 5.55 grams at b. pt. * (o) Weight of 100 cc. solution in grains. * (b) Grams dissolved substance per zoo grams solvent. * (c) Gram molecules of dissolved substance per ioc gram molecules of solvent. AOETAKILIDS t ' a SOLUBILITY OF ACETANILIDE IN ORGANIC SOLVENTS. (Speyers.) In Methyl Alcohol. In Ethyl, Alcohol. In Chloroform. O 10 20 30 40 50 60 (a) 86.0 86.4 87-5 89.2 91.1 93-2 95 7 (ft) 22-7 30-0 41 -o 54-0 75-5 107.0 145.0 (0 5-4 7-o 9.8 13.2 18.0 25.2 84 84 85 86 87 89 92 .2 4 -O .0 4 5 .0 (ft) 14.7 20-0 27.0 36.0 49.0 65.0 87-0 (c) 5-o 6.6 9-0 12.2 16.2 22. 30-0 (a) 147 144 139 131 127 3 5 .8 -4 4 .2 (ft) 3-66 7-80 12.00 17.0 23.0 31.0 41-0 (c) " 3-24 7.00 10.50 15-0 20.4 27.6 36-0 SOLUBILITY IN MIXTURES OF ETHYL ALCOHOL AND WATER AT 25. (Holleman and Antusch Rec. trav. chim 13, 293, 1894.) Vol. % Gms. CgHgNO per ~ Pr AlcohS. loo Gms. Solvent. S P' Gr ' Vol. % Gms. CgHsNO per c ~ Alcohol. loo Gms. Solvent. &p ' (jT ' 100 32-93 0.8512 55 13 13 0-9335 95 36.65 0-8737 9-74 0.9396 93 38.04 0.8813 45 7-25 0.9449 90 38.20 0.8896 40 5.10 0.9508 87 37.80 0-8959 35 3-58 0.9567 85 36.83 0.8996 3 1 2.56 0.9617 80 33-62 0.9072 25 1.73 0.9683 75 29.25 0.9133 20 1.30 0.9736 24-73 0.9185 IS 1.03 o 9795 65 20.42 0.9185 10 o 94 0.9845 60 16.51 0.9287 0-54 0.9970 ACETIC ACID CH 3 COOH. SOLUBILITY IN WATER. (Dahms Ann. Phys. [4] 60, 122, '97.) t o Gms. CHaCOOH per Solid ,0 Gms. CHaCOOH per Solid * ' 100 Cms. Solution. Phase. 100 Gms. Solution. Phase. -5 15.1 Ice -20 66.3 CHaCOOH -10 28.2 " -io 76.7 -15 39.5 " - o 87.0 -20 49.5 +10 90.8 25 57.0 " 16.5 ioo-otr.pt. " -26.6 58.9 Ice-fCH 3 COOH DISTRIBUTION OF ACETIC ACID BETWEEN: Water and Amyl Alcohol at 20. Water and Benzene at 25. (Herz and Fischer Ber. 37, 4747, '04) (H. and F. Ber. 38, 1140, '05.) Cms. CHaCOOH per 100 cc. G. M. CHaCOOH per 100 cc. Gms. CH S COOH per loo cc. G. M. per CHaCOOH 1OO CC. H a O Alcoholic HaO Alcoholic H 2 O QH H20 CoH Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. I 0.923 0.01 0.0095 5 0.130 0.05 0.0014 2 1.847 0-03 0.0280 10 0.417 o.io 0.0005 3 2-741 0-05 0.0460 20 -55 O-2O O.OO3O 4 3.694 0-07 0-0645 30 3 03 0.30 0.0290 5 4.587 0-09 0.0830 40 4.95 0.50 0.051 6 5-475 O.II IOIO 0-70 0.090 7 6-434 0.13 0-1190 8 . . . AOETIO AOID DISTRIBUTION OF ACETIC ACID BETWEEN WATER AND BENZENE. (Waddell J. Phys. Ch. 2, 237, 1898.) Results in terms of grams per 100 grams solution. Upper Layer. Lower Layer. t. CHaCOOH. C 6 H a . H 2 6. 25 o .46 99 52 .02 25 3 .10 96 75 o 1$ 25 5 .20 94 55 o 25 25 8 7 90 .88 o -42 25 16 3 82 .91 o 79 25 30 5 67 37 2 13 25 5 39 .60 7 .60 35 i .2 98 .68 o .08 35 5 7 93 97 o 33 35 9 .0 90 .42 58 35 45 .0 49 .00 6 .0 35 5 2 .2 39 4 8 4 CHaCOOH . CeHa. H 2 0. 9-4 0.18 90.42 28.2 o-53 71.27 37-7 0.84 61.46 48-3 1.82 49-88 61 .4 6.1 32-5 66.0 13-8 20-2 52-8 39-6 7 .6 16.4 0.62 89.98 36.8 1.42 62.78 49.0 2.10 48.90 61-3 25-5 13.2 52.2 39-4 8. 4 DISTRIBUTION OF ACETIC ACID BETWEEN WATER AND CHLOROFORM: At Room Temperature. At 25. (Wright, Thomson and Leon Proc. Roy. Soc-49, 185, 1891-) Results in parts per 100 parts of solution. Upper Layer. Lower Layer. (HerzandLewy;Rol Cms. CHaCOOH per TOO cc. CHaCOOH. CHC1 3 . H 2 O. CH 3 COOH . CHC1 3 . H 2 0. Layer. CHC1 3 Layer. O ,84 99 .16 o 99- OI 0. 99 2 0.089 6.46 o. 92 92 .62 1.04 98. 24 0. 72 4 0.313 17.69 0. 79 81 S 2 3-83 94- 98 I . 19 6 0.596 25.10 I. 21 73 .69 6.77 91. 85 I. 38 8 0.974 33-71 2. 97 63 32 11.05 87- 82 I. 13 10 1.430 44.12 t 30 4 8 58 17.72 80.00 2. 28 12 1.982 50.18 IS- ii 34 25-75 70. 13 4- 12 20 5-10 30 10.2 40 15-3 50 21-9 52-3 39-54 G. M. CHaCOOH per 100 cc. CHC1, Layer. 0.0032 O.0062 0.0100 H 2 Layer. 0.05 0.075 O.IOO 0.150 0.0198 0.175 0.0260 0.0325 0.070 0.170 0.275 o-335 0.200 0.30 0.50 O.70 0.80 0.87 0.659 The figures in the table for 25 were read from the curve plotted from the results of H. and L., Z. electro. Ch. u, 818, 1905, and of R. and W., Z. phys. Ch. 40, 623, 1902. The influence of electrolytes upon the distribution of acetic acid between the aqueous and chloroform layers was investigated by Rothmund and Wilsmore, and the following results expressed in gram molecules per liter at 25 were obtained: Cone, of Cone, of CHaCOOH Cone* Cone, of Cone. CH 3 COOH Cone.* ectro- I Electrolyte n CHaCOOl * Electro- * .lectrolyte in' C H 3 COOH lyte. Aq. Aq. CHC1 3 " H 2 O lyte. Aq. , \q. C :HC1 3 ' H 2 O Layer. Layer. Layer. Layer. Layer. L ayer. ] -ayer. Layer. ICl 0.463 0.876 0.0907 0.946 i H 2 SO 4 0.514 I. 099 1315 I.I68 0.463 I-538 0.2435 1.680 " 1.029 i. 555 .2714 1.787 0.926 0-813 0.0938 0.966 0.926 1.586 0.2902 1.858 NH 4 NO a I.O i. 136 o I 3 I 3 1.168 NO, 0.316 0.936 0.0927 0.958 " I.O i. 991 o .3481 2-053 0.316 1.694 0.2537 1.720 LiNO 3 I.O 892 .1005 I.OOO 0.633 0.965 0.0981 0.988 * * I.O I. 513 o .2581 1-737 0.633 1.631 0.2486 1.702 * Calculated from table above. ACETIC ACID 4 DISTRIBUTION OF ACETIC ACID AT 25 BETWEEN: Water and Carbon Bisulphide. Water and Carbon Tetrachloride. (Herz and Lewy.) (Herz and Lewy.) Gms. CHaCOOH G. M. CHaCOOH Gms. CHaCOOH G. M. CHaCOOH per ipo cc. per 100 cc. per 100 cc. per ipo cc. HjO CST H 2 O CIST H 2 O CCk ' H 2 O CC1 4 Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. 65 2.64 i.i 0.45 30 1.8 0.5 0.03 70 3.0 1.2 0.55 40 3.0 0-7 0.055 75 3-3 1-2 0.80 50 4.8 0.9 0.095 80 5.4 1-35 o-97 60 5.8 i.i 0.155 85 6.4 1-4 1-3 70 12.0 1.2 0.235 76.2 25.2 1.27 0.420 DISTRIBUTION OF ACETIC ACID AT 25 BETWEEN: Water and Bromoform. Water and Toluene. (H. and L. Z. electro. Ch. n, 818, '05.) (H. and F. Ber. 38, 1140, '05.) Gms. CHaCOOH G. M. CHaCOOH Gms. CHaCOOH G. M. CH 3 COOH per IPO cc. per ipo cc. per ipo cc. per 100 cc. 1*5 CHBra" ' H 2 O CHBr 3 'H 2 O CeHsCHa ' H 2 O C 6 H 6 CH3 Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. 20 1.5 0.4 0.035 5 0.119 o.i 0.0025 30 3.0 0.6 0.070 10 0.328 0.2 0.0075 4O 4-8 0.8 0.120 20 I.I32 0-4 0.0260 50 7.8 i.o 0.20 30 2.265 0.6 0.0530 60 12. o i.i 0.28 40 3-725 0.8 0.090 65 15.6 1.15 0.395 5 5-841 i.o 0.140 70 27.0 60 8.344 DISTRIBUTION OF ACETIC ACID AT 25 BETWEEN: Water and o or p Xylene. Water and m Xylene. (Herz and Fischer.) (Herz and Fischer.) Gms. CH 8 COOH G. M. CHaCOOH Gms. CHaCOOH G. M. CH 3 COOH per IPO cc. per 100 cc. per 100 cc. per 100 cc. TTO .? 9 r P wn 5 0.24 o.i 0.004 5 0-06 o.i 0.0015 10 0.48 0-2 O-OIO 10 0-30 0-2 0.007 20 1.13 0.4 0.025 20 o 95 0.4 0.022 30 2.15 0.6 0-047 30 1.91 0.6 0.042 40 3.40 0.8 0-079 4 3 4 0-8 0-072 50 5-10 I.O 0-122 50 4-65 I.O O.III 60 7-27 1.2 O.23O 60 6.65 1.2 70 12.52 NOTE. The distribution results as presented in the original papers to which references are given in the above tables, are reported in millimolecules per 10 cc. portions of each layer in the several cases. To obtain the figures given in the above tables, the original results be- fore and after calculating to gram quantities were plotted on cross- section paper, and from the curves thus obtained, readings for regular intervals of concentration of acetic acid in the aqueous layer were selected. 5 Chlor ACETIC ACID Chlor ACETIC ACID CH 2 C1COOH. DISTRIBUTION OF CHLORACETIC ACID BETWEEN: (Herz and Fischer.) Water and Benzene at 25. Water and Toluene at 25. 3ms. CH 2 C1COOH per 100 cc. G. M. CH 2 C1COOH per ipo cc. Gms. CH 2 C1COOH per 100 cc. G. M. CH 2 C1COOH per 100 cc. H 2 Layer. Layer. H 2 Layer. Layer. H 2 Layer. Layer* H 2 Layer. C 6 H 5 CH 3 Layer. 0.25* 8.69 O.OO25 O .090 O .!* 5 .22 O OOI 0-055 o-5 15-59 O.OO5 O r 55 O 5 20 31 O .005 O-2O I.O 27.87 O-OIO O .28 I .0 34 .87 O OIO 0.36 IS 41.10 0.015 415 I 5 49 14 O .015 0.50 2.0 52.90 0-02 54 2 .0 60 .46 .02 O.62 3-o 68.01 0.03 O .70 3 .0 72 .28 03 0-77 4-0 76.52 O.O4 O 79 4 .0 81 .72 O .04 0.85 5 .0 86 94 O 05 0.90 DISTRIBUTION OF CHLORACETIC ACID BETWEEN: (Herz and Lewy.) Water and Chloroform at 25* Water and Bromoform at 25. Gms. CH2C1COOH G. M. CH 2 C1COOH Gms. CH 2 C1COOH G. M. CH 2 C1COOH per 100 cc. per ipo cc. per loo cc. per 100 cc. H 2 O CHC1 3 Layer. Layer. 'H 2 O CHC1 3 ' Layer. Layer. H 2 O CHBrs Layer. Layer. H 2 O CHBra Layer. Layer. 5* 0.283 0.05 0.0025 40* 0.850 0.45 o.on 10 0.614 o.io 0.0060 50 1.889 0.50 0.0165 20 I. 088 O.2O O.OI35 60 2.994 O.6o O.O28 4O 2 . 948 O.4O O.O29 70 4.241 0.70 O.O4O 50 3.684 0.60 0-045 80 5 . 620 0.8o 0.053 60 4-440 0.70 0.061 90 7.560 0.90 0.067 70 7.086 0.75 0-077 91.6 II-340 0-97 0.120 DISTRIBUTION OF CHLORACETIC ACID BETWEEN: (Herz and Lewy.) Water and Carbon Bisulphide at 25. Water and Carbon Tetra- chloride at 25. Gms. CH2C1COOH per 100 cc. G. M. CH 2 C1COOH per 100 cc. Gms. CH 2 C1COOH per 100 cc. G. M. CH 2 C1COOH per 100 cc. H^ CS 2 HzO cs^ H 2 ecu H 2 ecu" Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. 60* 0.426 0.6 O.OO42 90* I.4I7 o-95 0.0150 80 0.691 0.8 O.OO7 95 2.031 1. 00 0.0195 90 0-803 I.O O.OO9 100 2.645 1.05 O.O27O 100 1.040 1.05 0.0105 I0 5 4.26 1. 10 0.0415 105 1.464 1. 10 0.015 106.7 5-19 1-13 0.0550 106.7 1.890 1-13 O-020 * See Note, page 4. Chlor ACETIC ACIDS SOLUBILITY OF MONOCHLOR, DICHLOR, AND OF TRICHLORACETIC ESTER IN AQUEOUS ALCOHOL AT ROOM TEMPERATURE. (Bancroft Phys. Rev. 3, 193, 1895-96, from results of PfcifLr, Z. physik. chem. 9, 469, '92.) cc. Elhyl Alcohol in Mixtures. cc. H2O added to cause separation of a second phase in mixtures of the given amts. of Alcohol and 3 cc. of : CH2C1COOC 2 H 5 . CHCl2COOC 2 H 3 CCbCOOQjHfi. 3 1.32 O.QO 0.65 6 4-OI 2-45 1. 80 9 7-30 4-33 3-02 12 10.78 6.60 4-50 15 16.16 9-20 6.50 18 22.16 ... t 21 28.74 . . . a AOETNAPHTHALIDE C 2 H,ONH(C 10 H 7 ). SOLUBILITY IN MIXTURES OF ALCOHOL AND WATER AT 25. (Holleman and Antusch Rec. trav. chim. 13, 289, 1894.) Vol.% Alcohol. Gms. per 100 Gms. Solvent. Sp. Gr. of Solutions. Alcohol Gms. per 100 Gms. Solvent. Sp. Gr. of Solutions. 100 4-02 0.7916 65 I. 7 8 0.8977 95 4-31 0.8150 60 1-44 0.9091 90 4-II 0.8344 55 I .02 0.9201 85 3-69 0.8485 5o 0-71 0-9290 80 3 .l8 0.8624 35 0.25 Q-9537 75 2-73 0.8761 20 O.O9 0.9717 70 2.31 0.8798 10 O-O4 0.9841 ACETONE (CH 3 ) 2 CO. SOLUBILITY OF ACETONE AT 25 IN AQUEOUS SOLUTIONS OF: Electrolytes. Non-Electrolytes. (Bell J. Phys. Ch. 9, 544, 1005; Linebarger Am. Ch. J. 14, 380, 1892.) Gms. Electro- lyte per Gms. (CH 3 ) 2 CO per 100 Gms. Solvent in Solutions of: Gms. Non- Gms. (CH 3 ) 2 CO per too Gms Electrolyte Solvent in Solutions of: 100 Gms. Aq Solution. K 3 C0 3 Na 2 CO 3 (NH4) 2 CO 3 MgCO 3 Aq. Solution. C^Hg* Anethol* (C 6 H 5 ) 2 CO, I 2 5 . . . . 83-5 5 92-5 103.0 90.0 2 50 51.0 no O 65 -o 10 117.0 I2 3 .0 108.5 5 CO 65.0 38.0 73 5 47-o 20 137.0 144 5 126.0 7 5 46.5 27-5 57 O 38.0 30 14^-5 155 .0 133 .0 10 34-5 19-5 44 5 29.0 40 155-5 162 O 136.0 12 5 25-5 14.0 35 .0 . . . 5 159-5 1 66 .0 135-5 15 .0 18.0 9-0 28 .0 . . . 00 160-2 165 .0 131 .5 20 o 8.0 2-7 . . . 70 155-0 158 .0 123.0 25 O 3-7 . . . . . 80 108.5 30 .0 1.6 90 82.0 * Anethol - p Propenylanisol CHs.CHrCHUJQ^OCHj. Naphthalene results at 35. NOTE. The original results were recalculated and plotted on cross- section paper. From the curves so obtained the above table was constructed. See also Note, page 7. ACETONE SOLUBILITY OF ACETONE IN AQUEOUS SOLUTIONS OP CARBOHYDRATES (Krug and McElroy J. Anal. Ch. 6. 184, '92; Bell J. Phys. Ch. 9, 547. '05.) Per cent Sugar. 10 20 30 35 40 45 50 55 60 65 70 In Aqueous Solutions of Cane Sugar. Cms. (CH 3 ) 2 CO per too Cms. Sugar Solution at: is. 30. 2S- 30. 35 40. 597-2 581.8 574-8 272.5 250.0 251.8 172.4 150.0 150.6 . . . . . . . . . 110 . . . 96.4 92.8 89.8 85 . . . 71.9 68.8 65-7 62 50.8 48.1 45-9 42 35-8 33-8 32-5 29 25.2 24.2 23-4 . . . 18.3 17.7 17.0 13.2 12.8 12.5 In Aqueous Dextrose Solutions. In Aqueous Maltose Solutions. Per cent Gms. (CH 3 ) 2 CO per Solvent at: ioo Gms. Per cent Gms. (CH 3 ) 2 CO per ioo Gms. Solvent at: Dextrose. ' 15. 25- 3S- Maltose. "iS. 25. 3S." 10 73 6 7 747 9 76I-5 10 353 .6 348 .1 342-0 2O 255 3 247 7 24O.8 20 I8 5 4 181 .2 176.9 30 157 5 149 .8 142.5 30 119 9 116 O II2.4 40 86 9 79 .6 74-0 40 78 4 74 7 70-5 50 36 .2 33 .0 31.2 50 4 6 .2 42 9 39-8 NOTE. The above determinations were made by adding successive small quantities of acetone to mixtures of known amounts of water and the carbohydrate, and noting the point at which a clouding due to the separation of a second phase occurred. This method was also used for the solubility of acetone in the aqueous electrolyte solutions (see previous page). In the case of the aqueous non-electrolyte solutions, however, successive small amounts of water were added to mixtures of known amounts of acetone and the non-electrolyte. DISTRIBUTION OF ACETONE BETWEEN WATER AND BENZENE AT 25. (Herz and Fischer Ber. 38, 1142, '05.) Gms. (CH 3 ) 2 CO per ioo cc. G. M. (CH 3 ) 2 CO per ioo cc. Aq. Layer. CH Layer. ' Aq. Layer. QH, Layer. I* I .20 0.025* 0.025 5 4.17 0.05 0.047 10 10.15 o.io o-975 15 15-59 0.15 0.150 20 22.50 O-2O 0.215 0.25 0.275 * See Note, page 4. ACET-PHENETIDINE 8 ACET-PHENETIDINE p (PHENAOETINE) C H 4 (OC 2 H 5 )NHCH 3 CO. SOLUBILITY IN WATER, ALCOHOL, ETC. (U. S. P.) Cms. C 6 H4(OC2H5)NHCH 3 CO per 100 Cms. b.pt. H 2 0. CzHeOH. (CH 3 ) 2 0. CHCl,. 0.108 8-33 I -59 S-oo i-43 50.0 ACET-TOLUIDE p CH 3 .C 6 H 4 NH.C 2 H 3 O. SOLUBILITY IN MIXTURES OF ALCOHOL AND WATER AT 25. (Holleman and Antusch Rec. trav. chim. 13, 288, '94.) Alcohol. Gms. per 100 Gms. Solvent. Sp. Gr. of Solutions. 100 I0.l8 0.8074 95 10-79 0.8276 90 IO.62 o . 8440 85 9.62 0-8576 80 8-43 0.8685 75 7.04 0.8803 70 5-81 o . 8904 65 4-39 0.9021 60 3-59 0.9115 55 2.69 0.9207 Alcoho?. Gms. per loo Gms. Solvent. Sp. Gr. of Solutions. 50 1.92 0.9306 45 I.4I 0.9380 40 0.96 o . 9460 35 0.66 0.9544 2 5 0.31 0.9668 20 0.23 0.9725 15 0.16 0.9780 5 0.13 0.9903 0.12 0-9979 ACETYLENE C 2 H 2 . SOLUBILITY IN WATER. (Winkler ; see Landolt and Bernstein's Tabellen, sd ed. p. 604, t e . O 5 10 20 25 3 73 49 3 1 03 o-93 0.84 O.2O O.I7 O.I5 0.13 0-12 O-II 0.09 a, " Absorption Coefficient," = the volume of gas (reduced to o and 760 mm. pressure) taken up by one volume of the liquid at the given temperature when the partial pressure of the gas equals 760 mm. mercury. <7, " Solubility," = the amount of gas in grams which is taken up by 100 grams of the pure solvent at the given temperature if the total pressure, i.e., the partial pressure of the gas plus the vapor pressure of the liquid at the absorption temperature is 760 mm. 9 AOETYLAOETONE ACETYLACETONE CH 3 COCH 2 COCH . SOLUBILITY IN "WATER. (Rothmund Z. phys. Ch. 26, 475, '98.) Cms. CH S COCH,COCH 8 per too Cms. to ' H 2 Acetyl Acetone Layer. Layer. 30 15.46 95-02 40 I7-58 93.68 5<> 2O.22 91.90 60 23-23 89.41 70 27.10 85-77 80 33-92 78.82 87. 7 (crit. temp.) 56.8 NOTE. Weighed amounts of water and acetylacetone were placed in small glass tubes, which were then sealed and slowly heated until the contained mixtures became homogeneous. The temperature was then allowed to fall very gradually and the point noted at which cloudiness appeared. This point was accurately established for each tube by repeated trials. The curve plotted from these determinations shows two percentage amounts of acetylacetone which cause cloudiness at each temperature below the critical point. Of these two points, for each temperature, one represents the aqueous layer, i.e., the solubility of acetylacetone in water; and the other represents the acetylacetone layer, i.e., the solubility of water in acetylacetone. This method is known as the " Synthetic Method," and yields results in harmony with those obtained by the analytical method, i.e., by analyzing each layer after complete separation occurs. ACONITINE (Amorphous) C3 4 H 47 NO n . SOLUBILITY IN SEVERAL SOLVENTS. (At 25 U.S.P.; at i8-22, Miiller Apoth.-Ztg. 18, 2, '03.) Cms. C3iH 4 7NOi per Cms. CaJL^NOn per Solvent. IPO Gms. Solvent at: Solvent. 100 Gms.^Solvent at: i8-22. 25? i8-22. 25. " Water . . . 0-054 0.031 Benzene *7 -&S Alcohol 4-54 * Carbon Tetrachloride i . 99 Ether ... 1.44 2.27 Petroleum Ether . . 0-023 0.028 ADIPIO ACID (Normal) (CH 2 ) 4 (COOH) 2 . 100 grams H 2 O dissolve 1.44 grams adipic acid at 15. (Henry Compt. rend. 99* 1157, '84; Lamowoux Ibid. 128, 908, '99.) AIR. 10 AIR SOLUBILITY IN WATER. (Winkler Her. 34, 1409, '01; see also Peterson and Sondern Ber. 22, 1439, '89.) cc.* of atmospheric O and N per liter of: Dist. H 2 O (at 760 mm.). Sea Water (at 760 mm.). t". B. Oxygen. Nitrogen. Oxygen. Nitrogen. o 0.02881 0.02864 IO.I9 18.45 7-77 I4-85 5 02543 .02521 8.91 16.30 6-93 13.32 10 .02264 .02237 7.87 14.50 6.29 12 .06 15 .02045 .02011 7-04 13.07 5-7o 11.05 20 .01869 .01826 6-35 II .91 IO.25 25 .01724 .01671 5-75 10.96 9.62 30 .Ol6o6 01539 5-24 10.15 40 .OI4l8 OI3I5 4.48 8.67 50 .01297 .01140 3-85 7-55 60 OI2l6 .00978 3-25 6.50 80 .OII26 .00600 1.97 4-03 100 .01105 .OOOOO o.oo 0-00 B = " Coefficient of Absorption," i.e., the amount of gas dissolved by the liquid when the pressure of the gas itself without the tension of the liquid amounts to 760 mm. B r = " Solubility," i.e., the amount of gas, reduced to o and 760 mm., which is absorbed by one volume of the liquid when the barometer indicates 760 mm. pressure. * Reduced to o and 760 mm. SOLUBILITY OF AIR IN AQUEOUS SULPHURIC ACID AT 18 AND 760 MM. (Tower Z. anorg. Ch. 50, 382, '06.) Wt. % H 2 SO 4 98 90 80 70 60 50 Solubility Coef. 0.0173 0.0107 0.0069 0.0055 0.0059 0.0076 SOLUBILITY OF AIR IN ALCOHOL, ETC. (Robinet Compt. rend. 58, 608, '64.) Solvent . Alcohol (95 . i%) . . 14.1 Oil of Lavender . ... 6.9 Petroleum 6.8 Oil of Turpentine . . . 24.2 Benzene 14.0 Solvent. Vols. Air per io< Vols. Solvent. Vols. Air per 100 Vols. Solvent. ALANINE (a Aminopropionic Acid) CH 3 CH(NH 2 )COOH. SOLUBILITY IN MIXTURES OF ALCOHOL AND WATER AT 25. (Holleman and Antusch Rec. trav. chim. 13, 297, '94.) Vol.% Alcohol. Gms. per 100 Gms. Solvent. Sp. Gr. of Solutions. 16.47 I .0421 5 14-37 I.03II 10 12.43 I -O2OO IS 10.49 I -OIOI 20 8.48 0.9984 25 7.11 0.9886 31 5-53 0-9761 Vol. % Alcohol. Gms. per 100 Gms. Solvent. Sp. Gr. of Solutions. 35 4.91 0.9670 40 3 -89 o-9577 50 2-38 o-9355 60 i-57 0.9102 70 0.85 0.8836 80 o-37 o 8556 ii ALDEHYDE ALDEHYDE. SOLUBILITY OF p FORMALDEHYDE (TRIOXYMETHYLENE) IN AQUEOUS SODIUM SULPHITE SOLUTIONS AT 20. (Lumiere and Seyewetz Bull. soc. chim. [3] 27, 1213, 'oa.) Grams Sodium Sulphite per 100 cc. H 2 O 5 10 20 28 Gms. Trioxymethylene per 100 cc. solution 22 24 26 27 100 gms. H 2 O dissolve 12.5 paraldehyde at 25, and 6.6 gms. at b. pt. ALCOHOLS. SOLUBILITY OF AMYL ALCOHOL IN WATER AT 22. (Herz Ber. 31, 2671, '98.) ioo cc. water dissolve 3.284 cc. amyl alcohol. Sp. Gr. of solu- tion = 0.9949, Volume = 102.99 cc. ioo cc. amyl alcohol dissolve 2.214 cc. water. Sp. Gr. of solu- tion = 0.8248, Volume = 101.28 cc. Sp. Gr. of H 2 O at 22 = 0.9980; Sp. Gr. of amyl alcohol at 22= 0.8133. SOLUBILITY OF AMYL ALCOHOL IN WATER AT DIFFERENT TEMPERA- TURES, " SYNTHETIC METHOD" (see Note, page 9). (Alexejew Ann. phys. Chem. 28, 305, '86.) Gms. CsHuOH per ioo Gms. Gms. CsHnOH per ioo Gms. t o Aqueous Alcoholic t o ' Aqueous Alcoholic ' Layer. Layer. Layer. Layer. o 97 ioo 2.0 80 20 6 94 120 4.0 77 40 4 9 J 4o 7.0 73 60 2 87 150 9.0 72 80 1.5 83 SOLUBILITY OF AMYL ALCOHOL IN AQ. ETHYL ALCOHOL SOLUTIONS. (Bancroft Phys. Rev. 3, 193, '95-96.) cr Fthvl cc.H 2 O added to cause Separation of a AV*2a Second Phase in Mixtures of the given in \!KT?. Amounts of Ethyl Alcohol and 3 cc. Portions of Amyl Alcohol at: ' 9-1. 19- 2.' 3 13-21 3-50 6 10 .35 10.80 9 18.34 19.10 12 27.47 29.15 15 41-25 43-15 NOTE. The effect of various amounts of a large number of salts upon the temperature (39.8) at which a mixture of 20 cc. of amyl alcohol + 20 cc. of ethyl alcohol + 32.9 cc. of water becomes homo- geneous has been investigated by PfeifTer (Z. phys. Ch. 9, 444, '92). The results are no doubt of interest from a solubility standpoint, but their recalculation to terms suitable for presentation in the present compilation has not been attempted. SOLUBILITY OF ISOAMYL ALCOHOL IN WATER. Gms. Iso Amyl Alcohol per ioo Gms. H20 Layer. 'Alcoholic Layer. 13 .7 2.0 Balbrano Ber. 9, 1437, '76 16.5 2.5 92.9 Wittstein Jahrb. 408, '62 22 2-61 97-36 Herz Ber. 31, 2669, '98 f. 'Aqueous Layer. Alcoholic Layer. 20 27 66 10 28 00 27-5 56 10 26.0 57 20 22.5 00 30 18 63-5 40 16 65-5 60 13 67 80 15 63 IOO 20 S 2 107 crit. temp. 33 120 ALCOHOLS 12 SOLUBILITY OF QUTY.L ALCOHOLS IN WATER, " SYNTHETIC METHOD " (see Note, page 9). (Alexejew Ann. phys. Chem. 28, 305, '86.) Secondary Butyl Alcohol I so Butyl Alcohol and Water. and Water. Cms. Secondary Butyl Alcohol per 100 Cms. Cms. Iso Butyl Alcohol per too Gms. Aqueous Alcoholic Layer. Layer. 13 85 9 84 7-5 83 7 82 7 77-5 8 72 . . . ... 16 62 130 28 50 133 crit. temp. 40 DISTRIBUTION OF ETHYL ALCOHOL BETWEEN WATER AND BENZENE AT 25. (Taylor J. Phys. Ch. x, 468, '97.) Composition of 10 cc. of Upper Layer. Composition of 10 cc. Lower Layer. 5.92 o. 2 6o 3.48 4-37 i-o7 4-5 6 6.43 0.48 3.09 3.54 1-41 S-5 7.40 0.29 2.31 2.04 2.27 5.69 8.13 0-17 1.70 i. 08 3.22 8.70 8.65 o.io 1.25 0.59 4-06 5.35 9.05 0.06 0.89 0.28 4.99 4.73 ALUMINIUM CHLORIDE A1C1 3 6 H 2 O. SOLUBILITY IN WATER. (Gerlach Z. anal. Ch. 8, 250, '69.) ioo gms. saturated solution contain 41.13 gms. A1C1 3 at 15, Sp. Gr. of solution = 1.354. ALUMINIUM SULPHATE A1 2 (S0 4 ) 3 18 H 2 O. SOLUBILITY IN WATER. (Poggiale Ann. chim. phys. [3] 8, 467, '43.) Gms. A1 2 (SO 4 )3 per 100 Gms. Gms. Al 2 (SO 4 )a. per ioo Gms. t*. Water. Solution. t. Water. Solution. o 31.3 23.8 60 59.1 37-2 J o 33-5 25.1 70 66.2 39.8 20 36.1 26.7 80 73-1 42 2 30 40.4 28.8 90 80.8 44.7 40 45-7 3 I -4 ioo 89.1 47.1 50 52.1 34.3 ioo gms. of a saturated solution of aluminium sulphate in glycol con- tain 14.4 gms. A1 2 (SO 4 ) 3 . (de Coninck Bull. acad. roy. Belgique, 3 S9, '05-) ALUMS ALUMS. SOLUBILITY OF AMMONIUM ALUM AND OF POTASSIUM ALUM IN WATER. (Mulder; Poggiale Ann. chim. phys. [3] 8, 467, '43; Locke Am.Ch. J.z6, 174, '01; Marino Gazz. chim. ital. 35, II, 351, '05; Berkeley Trans. Roy. Soc. 203 A, 214, '04.) Ammonium Alum. Potassium Alum. t. Gms. (NH 4 ) 2 A1 2 (S0 4 ) 4 Gms. (NH*)* A1 2 (S0 4 ) 424 H 2 G.M.(NH 4 ) 3 A1 2 (S0 4 ) 4 Gms. K 2 A1 2 (S0 4 ) 4 Gms. K 2 A1 2 (S0 4 ) 4 2 4 H 2 G. M. K 2 A1 2 (S0 4 ) 4 per 100 g. per 100 g. per 100 g. per loo g. per 100 g. per loo g. H 2 0. H 2 O. H 2 0. H 2 O. H 2 O. H^. 2.IO 3-90 O.OO44 3.0 5-65 0-0058 5 3-50 6.91 O.OO74 3-5 6.62 O.OO68 10 4-99 9-52 O.OIO5 4-0 7.60 0.0077 IS 6-25 12.66 0.0132 5 - 9-59 0.0097 20 7-74 15.13 0-0163 5-9 11.40 O.OII4 2 5 9.19 19.19 O.OI94 7-23 14.14 O.OI4O 30 10.94 22 -OI O.O23I 8-39 16.58 O.OI62 40 14.88 30.92 0.0314 ii .70 23-83 O.O227 50 20. 10 44-10 0.0424 17.00 36.40 0.0329 60 26.70 66.65 0.0569 24-75 57-35 0.0479 70 40.0 110.5 0.0774 80 71.0 321-3 0.1374 90 109.0 2275.0 O-2IIO 92 5 119.0 oo 0.2313 95 109.7 00 0.2312 NOTE. The potassium alum figures in the preceding table were taken from a curve plotted from the closely agreeing determinations of Mulder, Locke, Berkeley, and Marino. For the higher temperatures (above 60), however, the results of Marino are lower than those of the other investigators, and are omitted from the average curve. Locke called attention in his paper to the fact that Poggiale's results upon ammonium and potassium alum had evidently become inter- changed through some mistake. This explanation is entirely sub- stantiated, not only by Locke's determinations, but also by those of Mulder and Berkeley. The ammonium alum figures given above were therefore read from Poggiale's potassium alum curve, with which Locke's determination of the solubility of ammonium alum at 25 is in entire harmony. SOLUBILITY OF AMMONIUM ALUM IN PRESENCE OF AMMONIUM SUL- PHATE AND IN PRESENCE OF ALUMINIUM SULPHATE IN WATER. Mixture Used. (Rudorff Ber. 18, 1160, '85.) TOO Gms. Saturated Solution Contain: Grams (NH 4 ) 2 SO 4 + Grams A1 2 (SO 4 ) 3 . Saturated Ammonium Alum at 18.5 1.42 3-69 20 cc. above sol. + 6 gms. cryst. A1 2 (SO 4 ) 3 . . . 0.45 16.09 20 cc. above sol. -f 4 gms. cryst. (NH 4 ) 2 SO 4 . . . 20.81 0.29 ALUMS SOLUBILITY OF MIXTURES OF POTASSIUM ALUM AND ALUMINIUM SUL- PHATE AND OF POTASSIUM ALUM AND POTASSIUM SULPHATE IN WATER. (Marino Gazz. chim. ital. 35, II, 351, '05.) Gms. per logo Gms. H 2 O. K 2 S0 4 . 243-73 23-45 O.I 20 824.25 30.85 I 5- 1 35 911 .02 35-29 24.1 5o 1243.21 59-55 33-5 65 1598.00 ii9-43 43.1 77 1872.11 183.80 50-5 5.06 75.83 O.I 0.5 8.66 75.18 0.2 5- 16.07 85.78 0-4 10 18.52 96.50 o-5 15 20.56 109.30 0-55 30 39.60 147.8 I .0 40 73-88 163.1 1.9 50 126.0 195-4 3-4 60 249-7 238-8 6-7 70 529.0 3 2 3 7 14.2 80 1044.0 517-27 28.1 Gm. Mols. per i OOP Mols. H 2 O. Al 2 (S0 4 ) 3 .i8H 2 0. K 2 S0 4 / 2-3 3-6 6.1 12.6 18.9 7-8 7-7 8.8 99 II. 2 15.2 16.8 20. i 24.6 32.6 53-4 Solid Phase. K 2 A1 2 (S0 4 ) 2 . 24 H 2 + A1 2 (S0 4 ), K 2 A1 2 (S0 4 ) 2 . 24 H 2 + K 2 S0 4 SOLUBILITY OF MIXTURES OF POTASSIUM ALUM AND OF THALLIUM ALUM IN WATER AT 25. (Fock Z. Kryst. Min. 28, 397, '97.) K 2 A1 2 (S0 4 ) 4 .2 4 H 2 ; T1 2 A1 2 (SO 4 ) 4 .2 4 H 2 O. Composition of Solution. Solid Phase Mol. % of Potassium KAl(SO 4 ) 2 j>er Liter. T1A1(SO 4 ) 2 per Liter. Mol. % Sp. Gr. of Grams. Mg. Mols. Grams. Mg. Mols. KA1(SO 4 ) 2 . Solutions. Alum. 69.90 270.5 o.oo 0-00 100 .0591 100. 74-56 288.2 0.48 I-I3 99.61 ] .0601 99 32 67.90 262.8 1.72 4.07 98.48 3 .0598 96.84 65-30 252.7 4.52 10-67 95-95 i .0603 90-84 64-95 251.4 9.60 22.67 91.73 .] 0605 82.94 53-23 205.9 18.44 43.56 82.54 i .0609 68.24 45-32 175-4 24.60 58.10 7S-" 0609 58.23 38.02 147.2 32.48 76.75 65.73 1.0611 46.72 34-54 133-6 35-59 84.10 61.36 1.0611 44-23 28-35 109.7 42.99 101.60 51.93 1.0623 32.07 10.94 42-4 66.12 156.2 21.34 1-0654 7-94 O-OO O-O 75-46 178-3 o.oo 1.0674 0-00 ALUMS SOLUBILITY OF SODIUM ALUM IN WATER. 100 gms. H 2 O dissolve 51.0 gms. (?anhy.) Al 2 Na 2 (SO 4 ) 4 .24H 2 O at 16. (Auge Compt. rend, no, 1139, '90.) ioo gms. H 2 O dissolve no.o gms. Al 2 Na 2 (SO 4 ) 4 .24H 2 O at o. (Tilden J. Ch. Soc. (Lond.) 45, 269, '84.) SOLUBILITY OF CAESIUM ALUM, RUBIDIUM ALUM, AND OF THALLIUM ALUM IN WATER. (Setterburg Liebig's Annalen, 211, 104, '82; Locke Am. Ch. J. 26, 183, '01; Berkeley Trans. Roy. Soc. 203 A, 215, '04.) Caesium Alum. Rubidium Alum. Thallium Alum. Gms. per ioo Gms. HaO. Gms. per ioo Gms. H2O. Gms. per ioo Gms. H 2 O. Al2Cs 2 (S0 4 ) 4 . A1 .f 4 % ( 2 S (? 4) * Al 2 Rb 2 (S0 4 ) 4 . A1 f 4 ^)* A1 2 T1 2 (S0 4 ) 4 . A1 {|(J> 0-21 0.34 0.72 I. 21 3- I 5 4-84 5 0-25 0-40 0.86 1.48 3 .80 5.86 10 0.30 0-49 1.05 1.81 4.60 7-12 2O o . 40 o . 65 1.50 2.59 6.40 10.00 25 0.50 0.81 i. 80 3.12 7.60 11.95 30 0-60 0.97 2.20 3.82 9.38 14.89 40 0.85 1.38 3 2 5 5.69 14.40 23.57 50 1.30 2. II 4.80 8.50 22.50 38.41 60 2.00 3.27 7.40 13.36 35-36 65.19 70 3-20 5.27 12.40 23.25 80 5.40 9-01 21. 60 43.25 ... ... 90 10.50 i8.ii ... IOO 22.70 42-54 ... ... NOTE. Curves were plotted from the closely agreeing determina- tions recorded by the above named investigators and the table con- structed from the curves. AMINES. METHYL AMINE AND TRI METHYL Water and Amyl Alcohol. (Herz and Fischer Ber. 37, 4751, '04.) AMINE, DISTRIBUTION BETWEEN: Water and Benzene. (Herz and Fischer Ber. 38, 1143, '05.) Gms. NH 2 (CH 3 ) per ioo cc. Millimols NH 3 (CH 3 ) per 10 cc. Gms. N(CH3) 3 per i po cc. Millimols N(CH 3 ) 3 per^io cc. Aq. Alcoholic Aq. Alcoholic Aq. i CeH* Aq. CaHe Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. o-37 O-I2 1.155 .3804 O 345 O .174 O 5 8 4 0.295 0.94 o 33 3-036 I .070 O .812 O 396 I 377 0-670 i .57 o-54 5-054 I 759 I 075 545 I .819 0.921 i.8 9 0.69 6.083 2 .219 I .462 731 2 474 1.237 2.00 0.72 6.429 2 .315 2 139 I .077 3 .619 1.823 2-53 0.92 8.126 2 981 2 757 I 376 4 .663 2.328 3-30 1.24 10.613 3 974 3 .292 z 683 5 .568 2.847 3 996 2 053 6 .760 3-474 6 582 3 465 ii 5.861 AMINES 16 SOLUBILITIES OF Di ETHYL AMINE AND WATER.* (Lattey Phil. Mag. [6] 10, 398, '05.) Cms. NH(C2Hs) 2 per 100 Gms. t. 155 ISO 148 146 145 144 Aqueous Layer. 21-7 23-6 24.8 26-3 28.0 3 I.O Amine Layer. S9-o 55-5 53-5 51.0 49.0 45-o DISTRIBUTION OF TRI ETHYL AMINE BETWEEN WATER AND AMYL ALCOHOL AT 25. (Herz and Fischer Her. 37, 4751, '04.) Gms. N(C 2 Hc) 3 Millimols N(C2H6) S per zoo cc. per 10 cc. Aqueous Layer. Alcoholic Layer. Aqueous Layer. Alcoholic Layer. 0.0885 0.1683 o . 1866 0.2502 2.299 4-457 4.922 6.491 0.0875 o . 1664 0-1846 0.2474 2.273 4-408 4.868 6.418 143.5 (crit-t) 37-4 Tri Ethyl AMINE N(C 3 H 5 ) 3 . SOLUBILITY IN WATER. (Rothmund Z. phys. Ch. 26, 433, '98.) h o Gms. N(C 2 Hs)s per too Gms. 1 Gms. N(C2H 6 )3 per 100 Gms. Aq. Layer. Amine Layer. Aq. Layer. Amine Layer. 18.6 (crit. temp.) 51 9 40 3-65 96.48 20 14.24 72.0 50 2.8 7 96.4 25 7-30 95.18 55 2-57 96.3 30 5-80 96.60 60 2.23 9 6 3 35 4.58 9 6 -5 65 1.97 96 3 SOLUBILITY OF TRI ETHYL AMINE IN MIXTURES OF WATER AND ETHYL ALCOHOL AT DIFFERENT TEMPERATURES.* (Meerburg Z. phys. Ch. 40, 647, '02.) o% Alcohol. 13-33% .Alcohol. 28.08% Alcohol. 38.84% .Alcohol. 60.16% Alcohol t . per loo t. G. NCCaHjOa G. N( per 100 t . per CgHs' 100 13 G. N(< t. per -2Hs] 100 3 G. N(C 2 H 6 ) 3 t . per 100 g.sol. g.sol. g.sol. g.sol. g. sol. 69.2 i-7 38-3 8.2 54-5 22 .8 73 4 31 .2 76-77 71.2 30.8 5-6 13-9 29 .8 65 4 33 3 74-75 75-o 23.1 8-5 28.0 21.6 33-4 51 .1 5i .6 40 .6 72-73 80.0 I8. 7 25-8 26.4 30.6 63 7 42 -i So .6 I8. 7 37-2 24.9 40.5 30-3 68 5 40 9 54 7 19-5 51-8 24.2 49-8 28.5 82 .2 34 .2 70 .6 20-5 68.6 24.1 60.7 35-o 9i .8 33 O 77 5 20-5 84.0 24.0 69.7 34 7 88 20.5 89.7 23-5 73-6 40 5 91 .3 21-4 92.4 24.0 81-5 25-8 95-5 24.2 87.4 26-5 96.1 25.0 92.0 NOTE. Results for Tri Ethyl Amine, Water and Ethyl Ether, and for Tri Ethyl Amine, Water and Phenol are also given by Meerburg. 100 gms. abs. methyl alcohol dissolve 57.5 grams NH(C 6 H S ) 2 at 19.5. 100 gms. abs. ethyl alcohol dissolve 56.0 grams NH(C 6 Hg) 2 at 19.5. (de Bruyn Z. phys. Ch. 10, 784, 1802.) * Determinations made by " Synthetic Method," see Note, page 9. i; AMINES SOLUBILITY OP Di PHENYL AMINE AND ALSO OF TRI PHENYL AMINE IN CARBON BISULPHIDE. (Arctowski Compt. rend. 121, 123, '5.) NH(C6H 5 ) 2 in CS 2 . N(C 6 H 5 ) 3 in CS* A.O Gms. per 100 . o Gms per 100 Cms. Solution. Gms. Solution. -88i 0.87 -83 1.91 -117 0-37 -91 1.56 ~ IO2 1.24 -II3i 0.98 SOLUBILITY OF Di PHENYL AMINE IN HEXANE AND IN CARBON BISULPHIDE. (Etard Ann. chim. phys. [7] 2, 570, '94.) Gms. NH(C6H 8 ) 2 Gms. NHCCeHsk per IPO Gms. Sol, in: per 100 Gms. Sol, in; Hexane. CS^ Hexane. CS^ 60 ... 1.3 o 2.6 33.7 50 ... 2.2 +10 3.8 46.8 40 ... 3.8 20 6.7 60-9 ~30 0-5 7-2 30 13.8 76.0 20 0.8 12.5 40 47.0 io 1.4 21.6 50 94.0 AMMONIA NH 3 . SOLUBILITY OF AMMONIA IN WATER. (Roscoe and Dittmar Liebig's Annalen, 112, 334, '50; Raoult - Am. Ch. J. 19, 807, '97.) - Ann. chim. [5] i. *6a, '74; Mallet At 760 mm. Pressure. At 760 mm. Pressure. t tt . G. NH 3 per 100 g. H 2 0. Vol. NHa per i g. H 2 0. t. GJSTHa per TOO g. H 2 0. Vol. NHa per i g. %0. -40 -30 20 294.6 278.1 176.8 ... 20 2$ 30 52.6 46.0 40-3 710 635 595 (28) io III-5 87-5 1299 35 40 35-5 30-7 5 10 15 77-5 67.9 60.0 1019 910 802 45 5o 56 27.0 22.9 18.5 ... SOLUBILITY OF AMMONIA IN AQUEOUS SALT SOLUTIONS. (Raoult.) la Calcium Nitrate Solutions In Potassium Hydroxide Solutions Gms. NH 3 per too Gms. NHa per 100 Gms. Solvent in: Gms. Solvent in: cS&. IBfP o 96.25 104-5 72-0 49.5 8 78.50 84.75 57-o 37-5 16 65.00 70.5 46.0 28.5 24 ... ... 37-3 21.8 AMMONIA 18 MUTUAL SOLUBILITY OP AQUEOUS AMMONIA AND POTASSIUM CARBON- ATE SOLUTIONS. (Newth J. Chem. Soc. 77, 7?6, 1900.) The solutions used were: Potassium Carbonate saturated at 15 (contained 57.2 grams K 2 CO 3 per 100 cc.). Aqueous Ammonia of 0.885 Sp. Gr. (contained about 33 per cent ammonia). The determina- tions were made by adding successive small quantities of one of the solutions to a measured volume of the other, and observing the point at which opalescence appeared. Saturated K 2 COa in Aq. Ammonia. Aq. Ammonia in Saturated K 2 COs. t. cc. KzCOs per %K 2 CO 3 Solution cc. Ammonia %K 2 CO 3 Solution 100 cc. Ammonia. in Mixture. in 100 cc. K 2 COa. in Mixture. I 2.0 2.0 37-5 72.7 6 3.0 3.0 47-5 6 7-6 ii 5.0 4-7 5 2 5 6 5-o 16 6.5 6.1 60-0 63.0 21 8.5 8.0 77.5 56.3 26 10.5 9.5 105-0 49.0 31 12.5 ii. i 152.5 39.0 38 20.0 16.6 195 .o 33.0 39 21.0 17.0 220-0 31.0 42 25.0 20- o 250-0 28.5 43 35.0 26.0 285.0 26.5 Above 43 the solutions are completely miscible. If 10 per cent of water is added to each solution the temperature of complete miscibility is lowered to 25. The mutual solubilities are: Per cent K 2 CO 3 Solution in: t. Ammonia K 2 CO 3 Sol. Layer. Layer. o 8 62 10 ii 52 20 15 38 25 (crit. pt.) 25 With the addition of 12.9 per cent of water to each solution the temperature of complete miscibility (crit. pt.) is lowered to 10. With the addition of 18.1 per cent water this temperature becomes o. SOLUBILITY OF AMMONIA IN ABSOLUTE ETHYL ALCOHOL. (Delepine J. pharm. chim. [5) 25, 496, 1892; de Bruyn Rec. trav. chim. ii, 112, '92-) A O Cms . NH 3 Cms. NHs per 100 Gms. Solution. Gms. NHs per 100 Gms. Alcohol t . Density. per loo cc. Solution. (Delepine.) (de Bruyn.) (Delepine.) (de Bruyn.) 0-782 !3 OS 20 95 19 7 26 5 24 5 5 0-784 12 OO 19 .00 17 5 23 .0 21 .2 10 0-787 10 85 16 43 15 .0 19 .6 17 .8 IS 0.789 9 .20 13 .00 13 .2 15 o *s .2 20 0.791 7 SO 10 .66 II 5 II 9 13 .2 25 0-794 6 OO 10 o 10 .0 II .0 II .2 30 0.798 5 IS 9 7 8 .8 10 7 9 5 AMMONIA SOLUBILITY OF AMMONIA IN AQUEOUS ETHYL ALCOHOL. (Delepine.) In 96%. Alcohol. In 90%. Alcohol. In 8o% A Alcohol. t. Sp. Gr. Solution. G. NH 3 per' 100 Gms. Sol. Sp. Gr. Solution. G. NH 8 per too Gms. Sol. Sp. Gr. Solution. G. NH S per loo Gms. Sol. O 0.783 24-5 0.800 30.25 0.8o8 39-o 10 0.803 18.6 Q-794 28.8 O.8OO 28.8 20 0.788 14.8 0-795 15-8 0.821 19.1 30 0.791 10.7 0.796 II.4 0.826 12.2 In 60% Alcohol. In 50% Alcohol. t. Sp. Gr. G. NH 3 per Solution. 100 Gms. Sol O 0.830 50-45 IO 0.831 37-3 20 0.842 26.1 30 0-846 21 .2 Sp. Gr. Solution. 0.835 0-850 0.869 0.883 G. NHs per 100 Gms. Sol. 69.77 43-86 33-8 25 -2 SOLUBILITY OF AMMONIA IN ABSOLUTE METHYL ALCOHOL. (de Bruyn Rec. trav. chim. n, 112, '92.) . G. NHs per 100 Grams. G. NH 3 per^ioo Grams. Solution. Alcohol. o 29.3 41.5 5 26.5 36.4 10 24.2 31.8 15 21.6 27.8 20 25 30 Solution. 19.2 I6. S 14-0 Alcohol. 23-8 2O. O 16.0 DISTRIBUTION OF AMMONIA BETWEEN: Water and Amyl Alcohol at 20' (Herz and Fischer Ber. 37t 4747, '04.) Water and Chloroform at 20. (Dawson and McCrae J. Ch. Soc. ?g, 496, '01; see also Hantsch and Sebaldt Z.phys.Ch.ao, 258, '99.) Gms.NHsperioocc. G . M. NHs per 100 cc. Gms. NHs per 100 cc. G. M. NH$ per 100 cc. Aq. Alcoholic Aa. Alcoholic Aq. CHClg Aq. CHC1 3 Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. o-5 0.072 2 5 0.0035 0.2 O.OO7 O .01 .00038 I .0 0-147 50 0.0073 0-4 0.015 O .02 .00073 2 -O O.272 I OO 0-0148 0.6 0.023 O 03 O OOII4 3-o 0.438 2 OO 0-0295 0.8 0.031 O .04 .OOI52 4-0 o-595 3 OO 0-0460 I.O 0-039 O 05 .00193 5-o 0.756 I .2 0-046 .06 .00232 1-4 0-055 O -08 .00311 1.6 0-063 O .10 O .00396 NOTE. The influence of a large number of electrolytes upon the distribution of ammonia between water and chloroform was also investigated. For calculations of above distribution results, see Note, page 4. AMMONIUM ARSENATES 20 SOLUBILITY OF AMMONIUM CALCIUM ARSENATE AND AMMONIUM MAGNESIUM ARSENATE IN WATER, ETC. (Field J. Ch. Soc. u, 6, '73.) Grams per too Grams Solvent. Solvent. NH4CaAs0 4 *H,0 . . _____ Water 0.02 o 014 Aq. Ammonia 10% (Sp. Gr. 0.88) o.ooi 0.007 Aq.NH 4 Cl 5% 0.415 Aq. NH 4 Cl 10% . . 0.095 AMMONIUM BENZOATE NH 4 C 7 H 6 O 2 . SOLUBILITY IN WATER AND IN ALCOHOL. Gms. NH 4 C7HsO2 per ioo Gms. Solvent in : t. Water. Alcohol.' 25 9.52 4.0 b- pt. 83.33 13.2 AMMONIUM BROMO PLATINATE (NH 4 ) 2 PtBr 6 . ioo gms. sat. aq. solution contain 0.59 gm. (NH 4 ) 2 PtBr 6 at 20. (Halberstadt Ber. 17, 2965, '84.) AMMONIUM BROMIDE NH 4 Br. SOLUBILITY IN WATER. (Eder Abh. K. Akad. Wiss. (Berlin) 82 ii, 1284, '80.) Gms. NH 4 Br. per ioo Grams. Gms. NH 4 Br. per ioo Grams. t. 'Solution. Water." t. Solution. Water. 10 39.8 66.2 50 48-5 94-3 20 42.5 74-0 60 50.2 IOI.O 30 44.8 81.3 80 53.5 II5.0 40 46.7 87.5 ioo 56.1 128.2 SOLUBILITY OF AMMONIUM BROMIDE IN ABSOLUTE ETHYL ALCOHOL, METHYL ALCOHOL, AND IN ETHER. (Eder; de Bruyn Z. phys. Ch. 10, 783, '92-) In Ethyl Alcohol. In Methyl Alcohol. In Ether (0.729 Sp. Gr.). Gms. NH^r Gms. NH^r Gms. NH^r per ioo Grams. per ioo Grams. per ioo Grams. t. Solution. Alcohol. Solution. Alcohol. Ether. 15 2.97 3.06 0.123 19 3-12 3.22 II. I 12.5 78 9-5 10.50 *;" Solubility of Tetra Ethyl AMMONIUM BROMIDE N(C 2 H 5 ) 4 Br, and of Tetra Methyl Ammonium Bromide N(CH 3 ) 4 Br in Acetonitril. (Walden Z. phys. Ch. 55, 712, '06.) ioo cc. sat. solution in CH 3 CN contain 9.59 gms. N(C 2 H 5 ) 4 Br at 25. ioo cc. sat. solution in CH 3 CN contain 0.17 gm. N(CH 3 ) 4 Br at 25. AMMONIUM CADMIUM BROMIDE NH 4 Br.CdBr 2 .H 2 O. ioo parts of water dissolve 137.0 parts NH 4 Br.CdBr 2 .iH 3 O. ioo parts of alcohol dissolve 18.8 parts NH 4 Br.CdBr 2 .$H 2 O. ioo parts of ether dissolve 0.36 part NH 4 Br.CdBr 2 .$H 2 O. (Eder Dingier polyt. J. 221, 89, *76.> 21 AMMONIUM CARBONATE AMMONIUM CARBONATE (NH 4 ) 2 CO 3 . 100 grams H 2 O dissolve 100 grams (NH 4 ) 2 CO 3 H 2 O at 15. 100 grams glycerine dissolve 20 grams (NH 4 ) 2 CO 3 at 15. (Divers J. Ch. Soc. 23t 171, J ?o.) AMMONIUM BICARBONATE NH 4 HCO 3 . SOLUBILITY IN WATER. (Dibbits J. pr. Ch. [2] 10, 417. '74 ) 9 Cms. NILJICOs per 100 Grams. Solution. Water'. O 10.6 II-9 20 5 I2 -i I 3-7 25 10 13.7 i5- 8 30 15 J 5-5 l8 -3 Grams NHjNCOs per TOO Grama. Solution. Wate?. 17.4 21.0 19.3 23.9 21.3 27.0 SOLUBILITY OP AMMONIUM BICARBONATE IN AQUEOUS SOLUTIONS OP AMMONIUM CHLORIDE SATURATED WITH CO 2 . (Fedotieff Z. phys. Ch. 49, 168, '04.) Per 1000 cc. Solution. Per 1000 Grams HjO. 4.0 Wt.OI * i cc. Sol. o G. NP M. uci. G. M. Gms. NILJICOs. NH4C1. Gms NILJI COa. G. M. NH4C1. o.o G. M. NILJICO I .22 Gms. 3. NIL^Cl. o.o Gms. NILJICOs. II9.0 o 1.077 4 .41 o-37 235-9 2 9 .2 5-42 0.46 290.8 36.0 15 .064 .0 2.12 o.o I6 7 .2 o.o 2.36 o.o 186.4 15 .063 o 5 1.84 26.8 145 .2 0.56 2.06 29.9 162.9 15 .O62 I .0 I .59 53-5 125 5 1-13 1. 80 60.6 142.2 15 .062 I .41 1.42 75-4 112 .2 I .60 85-1 126.9 15 -06 5 I .89 4.28 100.8 101 .1 2.18 1.48 II6.8 II6.8 15 .069 2 .87 0-99 153-3 78 .2 3-42 1.18 183.0 93-3 15 .076 3 .84 0-79 205.2 62 5 5-03 0.98 269.3 77-3 15 .085 4 .82 0.65 257-9 5 1 4 6.21 0.84 332.5 66.4 085 4 95 O.62 264.8 48 9 6.40 0.81 343-5 64.2 3 ... o.o 3-42 o.o 270.0 7O 7.4 i .ic 107.0 OI.O SOLUBILITY OF AMMONIUM BICARBONATE IN AQUEOUS SOLUTIONS OP SODIUM BICARBONATE SATURATED WITH CO 2 . (Fedotieff.) Per looo cc. Solution. Per 1000 Grams H^O. t. o o 15 15 7O Wt ' f , r G. M. G. M. Gms. Gms. i cc. bol. NaHCC , 3 . NILJICOa. NaHCO 3 . NILJICOs. G. M. G. M. Gms. NaHCOs. NILJICOs. NaHCO 3 . o.o 1.51 o.o 0.58 1.39 48.2 o.o 2.36 o.o 0.71 2.16 59-2 o.o 3.42 o.o 0.8.1 2.01 70-0 Gms. II9.0 109.4 186.4 170.6 270.0 210-0 1.072 0.53 1.064 o.o 1.090 0.63 1.28 2.12 1.92 44.6 o.o 52.5 101.4 167.2 151-3 AMMONIUM BICARBONATE 22 SOLUBILITY OF MIXTURES OF AMMONIUM BICARBONATE, SODIUM BICARBONATE, AND AMMONIUM CHLORIDE IN WATER SATURATED WITH CO 2 . (Fedotieff.) Solid Phase. a -h c u t o Wt.of * icc. Sol. o 1.114 Gms HaO. Gms ' *** IOO Gms ' H2 ' NaHC0 3 . NaCl. O-59 0.96 NH*U. 4.92 NaHC0 3 . 49.61 NaCl. 56.16 NH4C1. 263.4 o 1.187 O .12 4 83 2 74 10 .09 282.6 146.7 15 1.116 93 5 1 6 .28 78 .18 29.84 336.2 15 1.178 O .18 4 44 3 73 15 13 259.8 199.6 15 .151 O 30 3 .09 4 56 25 .22 l8o.8 244.1 .128 5 1 z 68 5 45 42 87 98.28 291.7 15 .112 O 99 o 35 5 65 83 .22 20-47 302.4 15 .I08 I .07 20 5 .21 89 95 11.70 278.9 15 .IO6 I .12 ii 4 .92 94 .14 6.44 263.4 r 5 .101 I .16 o 14 4 OO 97 52 8.19 2I4.I .090 O 93 o 95 2 03 78 .18 55-58 108.6 a = NaHCO 3 , b = NH 4 HCO 3 , c = NH 4 C1. AMMONIUM URANYL CARBONATE 2 (NH 4 ) 2 CO 3 UO 2 CO 3 . (Ebelmen.) 100 grams H 2 O dissolve 5 grains of the salt at 15. AMMONIUM LEAD COBALTICYANIDE NH 4 PbCo(CN) 6 .3H 2 O. (Schuler Sitz. Ber. K. Akad. W. (Berlin) 79, 302.) 100 grams H 2 O dissolve 12.0 grams of the salt at 18. AMMONIUM CHLORIDE NH 4 C1. SOLUBILITY IN WATER. (Mulder; below o, Meerburg Z. anorg. Ch. 37, 203, 1003.) Gms. NH4C1 per 100 Gms. Gms. NH 4 C1 per TOO Cms. Solution. Water. Solution. Water. -15 19.7 24.5 40 31-4 45-8 -10.9 20-3 25.5 50 33.5 50.4 -5.7 21.7 27.7 60 35.6 55.2 o 22.7 29.4 70 37.6 60.2 + 5 23.8 31.2 80 39-6 65.6 10 24.9 33.3 90 41-6 7i-3 15 26.0 35.2 100 43 - 6 77-3 20 27.1 37.2 no 45-6 83.8 25 28.2 39.3 115.6 46.6 87.3 30 29.3 41.4 Density of saturated solution at o = 1.088, at 15 = 1.077, at I 9 < - 1.075. 23 AMMONIUM CHLORIDE SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS AMMONIUM BI- CARBONATE SOLUTIONS SATURATED WITH CO 2 . (Fedotieff Z. phys. Ch. 49, 169, 1904.) Wt f Per 1000 cc. Solution. Per 1000 Gms. H 2 O. t p . i cc. Sol. G.M. G . M. Gms. Gms. G.M. G . M. Gms. Gms. NH 4 HCO 3 . NI NH 4 HCO 3 . NH4C1. NH4HC03. NP NHHC1. NH4C1. o I .069 O-O 4 .60 o.o 246.1 o.o 5- 57 0-0 298.0 I .077 o-37 4 41 29.2 235.9 0.46 5- 42 36.0 290-8 15 I .077 o.o 5 29 o.o 283.1 o.o 6. 64 0-0 355-o 15 I 085 0.62 4 95 48.9 264.8 0.81 6. 40 64.2 343-5 30 0-0 7- 78 O-O 416.4 2O I .IS 7 . 40 OI .0 307 .0 SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE SATURATED WITH CO 2 . (Fedotieff.) Per 1000 cc. Solution. Per 1000 Gms. H 2 O. t. Wt. of G. M. G. M. Gms. Gms. G. M. G. M. Gms. Gms ^ i cc. Sol. NaCl. NH4C1. NaCl. NH4C1. NaCl. NH 4 C1. NaCl. NH 4 C1. I .069 O .0 4.60 o.o 246.1 O O 5- 57 o.o 298. o o 1.085 4 .04 2 .26 236.5 121 -O 4 .89 2. 73 286.4 146. i 15 1.077 o O 5.29 o-o 283.1 o .0 6. 64 o.o 355- 15 1.097 .81 4.71 47.5 252.1 I .02 5- 9i 59-8 316- 4 15 I .I2O I .68 4.13 98.0 221-7 2 .09 5- 18 122.4 277. o 15 I - I 53 2 .87 3.38 168.0 180.7 3 57 4- 20 208.9 224. 7 15 I - I 75 3 65 2.98 213.5 159.4 4 55 3- 72 266.8 198. 8 30 .0 7- 78 o.o 416. 4 30 1.166 3 30 3.70 193.0 198.0 4 .26 4- 77 249.0 255- 4 45 O 9- 03 o-o 483- 7 45 4 .0 6. 02 233-9 322. i SOLUBILITY OP AMMONIUM CHLORIDE IN AQUEOUS SOLUTIONS OP HYDROCHLORIC ACID AT 0. (Engel Ann. chim. phys. [6] 13, 379, '88.) Sp. Gr. of Solutions. Milligram Molecules per 10 cc. Solution. Grams per 100 cc. Solution. HC1. NH4C1. 'HC1. NH4C1. i .076 o-o 46.12 .0 24.61 i .069 2.9 43 - 6 I 05 23.16 i .070 5-5 4i-o I 99 21.78 i .071 7-85 39 -!5 2 .84 20.79 i 073 10.85 36.45 3 93 19.36 i .078 21.4 27.37 7 74 14-54 i .106 53.0 10.87 19 .18 5-78 I .114 61.0 8.8 22 .07 4.67 Sat. HClati2 3. 7 at 17 AMMONIUM OHLORIDE 24 SOLUBILITY IN AQUEOUS AMMONIA SOLUTIONS AT o. (Engel Bull. soc. chim. [3] 6, 17, 1891.) Sp. Gr. of Solutions. 1.067 1.054 1.031 1.025 I .017 0-993 0.992 0-983 o-953 0.931 Milligram Molecules per 10 cc. Solution. NH 3 . NH4C1. 5-37 45-8 12.02 45-5 38.0 44-5 47-0 44.0 54-5 43 -63 80.0 43.12 90.0 44.0 95-5 44-37 130.0 49-75 169-75 60-0 Grams per 100 cc. Solution. NH40H. NH4C1. 0.92 24.52 2.05 6.48 8.02 24-35 23.82 9-30 13-66 23-35 23-09 16.29 22.18 28.97 23 75 26.63 32.14 SOLUBILITIES OF MIXTURES OF AMMONIUM CHLORIDE AND OTHER SALTS IN WATER. (Riidorff, Karsten, Mulder.) Both salts present in solid phase. AO Grams per 100 Grams H2O. <> Grams per 100 Grams H 2 O. 19.5 29 . 2 NH 4 C1+ 1 74 . o NH 4 NO 3 R 21.5 26.8 " + 4 6.5(NH 4 ) 2 SO 4 R 20.0 33.8 " + n.6BaCl 2 R 18.5 39.2 " + i7.oBa(NO 3 ) 2 K 15.0 28.9 " + I6.9KC1 R 22.0 30.4 " -f- 19.1 KC1 R b.pt. 67.7NH 4 Cl+2i. 9 KCl M 14.8 38.8 " + 34 .2KNO 3 K 18.5 39.8 " + 3 8.6KN0 3 K 14.0 36.8 " H-i 4 .iK 2 S0 4 R 18.7 37.9 " +i 3 . 3 K 2 S0 4 K 18.7 22.9 " +23. 9 NaCl R SOLUBILITY OF AMMONIUM CHLORIDE IN ABSOLUTE ETHYL AND METHYL ALCOHOL AT 19 AND IN AQUEOUS ETHYL ALCOHOL SOLUTIONS. 100 grams absolute ethyl alcohol dissolve 0.62 grams NH 4 C1. 100 grams absolute methyl alcohol dissolve 3.35 grams NH 4 C1. (de Bruyn Rec. trav. chim. u, 156, '92.) In Aqueous Alcohol at 30. (Bathrick J. Physic. Chem. i, 159, '96.) Wt. per cent Alcohol. G. NH 4 C1 per 100 g. Alcohol. Wt. per cent Alcohol. G. NH 4 C1 per 100 g. Alcohol. 40.4 45-9 17-0 8.3 35-3 54-3 14.0 16.9 3i-8 65 -o 9 .6 25-9 27-5 75-6 6. 4 34-4 21.7 87.9 2-9 In Aq. Alcohol of 45 Wt. %. (Gerardin Ann. chim. phys. [4] 5, 147, '65.) f ~ G. NH 4 C1 t . per 100 g. Alcohol. 4 II .2 8 12 .6 27 19.4 38 23-6 56 30.1 AMMONIUM CHLORIDE SOLUBILITY OF AMMONIUM CHLORIDE IN AQUEOUS GLYCERINE SOLU- TIONS AND IN AQUEOUS ACETONE SOLUTIONS AT 25. (Herz and Knoch Z. anorg. Chem. 45, 263, 267, '05.) In Aqueous Glycerine. (Sp. Gr. of Glycerine 1.255, Impurity about 1.5%.) In Aqueous Acetone. Wt.% NKUCl per 100 cc. Sp. Gr. Solution. 25 AceloiT NH 4 C1 per 100 cc. Solution. Sp. Gr. .25 Glycenne. ^u^^ o. 585.1 Grams. 3I-32 4 0793 Millimols 585-I . Grams. 3I-32 r I 0793 13.28 544-6 29.16 .0947 10 534 .1 28.59 I -O6l8 25.98 502.9 26.93 .1127 20 464 .6 24.87 I 0451 45 -3 6 434-4 23.26 .1452 30 396 7 21.23 I 0263 54-23 403-5 21 .60 .1606 40 328 5 *7-59 9998 83.84 291.4 15.60 2225 * 4 6 5 L 283 7 O 9800 IOO-OO 228.4 12.23 .2617 *8 5 -7 U 18 9 1. 01 O .8390 90 9 4 0.50 o 8274 * Between these two concentrations of acetone, lower layer, U indicates tipper layer. the solution separates into two layers L indicates Solubility of Tetra Ethyl AMMONIUM CHLORIDE N(C 2 H 5 ) 4 C1, and also of Tetra Methyl Ammonium Chloride N(CH 3 ) 4 C1 in Acetonitril. 100 cc. sat. solution in CH 3 CN contain 29.31 gms. N(C 2 H S ) 4 C1 at 25. 100 cc. sat. solution in CH S CN contain 0.265 gms. N(CH 3 ) 4 C1 at 25. (Walden Z. physik. Chem. 55, 712, '06.) AMMONIUM CHROMATES. SOLUBILITY IN WATER AT 30. (Schreinemaker Z. physic. Chem. 55, 89, '06.) Composition in Wt. per cent of: Solid Phase. (NH 4 ) 2 CrO (NH 4 ) 2 Cr0 4 + (NH 4 ) 2 Cr 2 7 (NH 4 ) 2 Cr 2 O 7 (NH 4 ) 2 Cr 2 O 7 + (NH 4 )aCr,O lto (NH 4 ) 2 Cr 3 10 U (NH 4 ) 2 Cr 3 10 +(NH 4 ) 2 Cr 4 18 (NH 4 ) 2 Cr 4 3 (NH 4 ) 2 Cr 4 O J3 +CrO, Cr0 3 CrOa 100 gms. of the sat. aq. solution contain 28.80 gms.(NH 4 ) 2 CrO 4 at 30. 100 gms. of thesat. aq. solution contain 32. 05 gms. (NH 4 ) 2 Cr 2 O 7 at 30. The Solution. The Residue. % Cr0 3 . % NH 3 . % Cr0 3 . % NH 3 . 6-933 22.23 9.966 16-53 47-59 20-44 16.973 8.20 . . . 22-53 6-37 38.03 12.15 27.09 6.87 48.02 12.01 26.19 5-7 47-38 8.81 25-99 5.10 41.56 7-58 30.16 3.50 38.89 3.10 61.08 8.80 42.44 59-72 6.75 44-08 2.27 54-90 4.14 52.91 i .11 60.88 3-09 54-56 1.03 63.07 3-09 56-57 o-97 65-70 2-95 58.87 0.65 69.74 3-24 62.48 0.46 71-93 O 63.60 0.40 73-68 1.18 63.66 0.41 71-47 2.07 62.94 O.2I . . . 62.28 0-0 . . . AMMONIUM FLUOBORIDE 26 AMMONIUM FLUOBORIDE NH 4 3BF 3 . 100 parts of water dissolve 25 parts salt at 16, and about 97 parts at b. pt. (Stolba Chem. Techn. Cent. Anz. 7, 459.; AMMONIUM FORMATE HCOONH 4 , and also Ammonium Acid Formate. SOLUBILITY IN WATER. (Groschuff Her. 36, 4351, '03.) Solid. Phase. 2O O 20 40 60 80 Gms. HCOONH* per i go Gms. Solution. Water. 41.9 72 HCOONH 4 IO2 " 50-5 67.1 204 75-7 3" 84. 2 531 116 f. pt. \jms. per ioo \jrns. t. Solution. Solid. HCOONH-J + HCOOH: - 6.5 46.7 34-1 HCOONH 4 .HCOOH + i-5 49.6 36.2 H 6.0 37-4 a 8.5 52.1 38.0 " - 7 49.6 36.2 HCOONH 4 labil. + 13 S3- 38.6 stabil. 29 55-8 40.7 39 57.8 42.2 H,O free solution. SOLUBILITY OF AMMONIUM FORMATE IN FORMIC ACID SOLUTIONS. (Groschuff.) 30 grams of HCOONH 4 dissolved in weighed amounts of formic acid and cooled to the point at which a solid phase separated. Gms. G. M. HCOONH 4 HCOONH4 t. per per ioo Gms. xooG.M. Solid Phase. ~ 3 + 8.5 21-5 Solution. 35-3 40.6 50.0 HCOOH. 39.9 HCOONH 4 . ii HCOOH 39 49-9 7 8 Gms. G. M. HCOONH 4 HCOONH 4 per per ioo Gms. ioo G. M. Solution. HCOOH. HCOONH 4 labil. Solid Phase. 50.0 73.0 57. 73- 116 m.pt. 100.0 IOO.O 199.0 00 stabil. AMMONIUM IODATE NHJO 3 . ioo parts H 2 O dissolve 2.6 parts salt at 15 and 14.5 parts at 100. (Rammelsberg Pogg. Ann. 44, 555, 1838.) Tetra Methyl AMMONIUM IODIDE N(CH 8 )J. SOLUBILITY IN SEVERAL SOLVENTS. (Walden Z. physik. Chem. 55. 708, '06.) o Sp. Gr. of Gms. N(CH 3 ) 4 I per ioo. Solreat. Formula. Solution. cc . Solution. Gms. Solution. Water H 2 O I .0188 2 .01 I 97 Water H 2 25 I 0155 5 .31-5 .89 5 .22 Methyl Alcohol CH 3 OH O o .8025 .l8-0 .22 .22 Methyl Alcohol CHaOH 25 .7920 .38-0 .42 . 4 8 Ethyl Alcohol C 2 H 5 OH 25 .7894 .09 Glycol (CH 2 OH), O I .OI4 Glycol (CH 2 OH) 8 25 X .0678 .240 .224 Acetonitril CHsCN 25 o .650 Nitro Methane CHaNO, o I 1387 .25-0 32 o .22 Nitro Methane CH 3 N0 2 25 I .1285 34-0 38 .21 Acetone (CH 3 ) 2 CO . . . o .118 Acetone (CH 3 ) 2 CO 25 . . . o .187 Salicyl Aldehyde C 6 H 4 .OH.COH o I .1492 .302 '.'063 Salicyl Aldehyde C 6 H 4 .OH.COH 25 I 1379 0.510 .484 AMMONIUM IODIDE Tetra Ethyl AMMONIUM IODIDE N(C 2 H S )J. SOLUBILITY IN SEVERAL SOLVENTS. (Walden Z. physik. Chem. 55. 6pS, '06.) Solvent. Formula. t o Sp.Gr.of ' Solution. Cms. N(C2H 5 ) 4 I per 100. cc. Solution. Gms. Solution. Water H 2 o I .0470 16 31 15 58 Water H 2 2 5 I .IO2I 36 33(35-5) 44 Methyl Alcohol CH 3 OH o .8326 3 7-4-3 4 44 Methyl Alcohol CHsOH 25 .8463 10 5 (10.7) 12 .29 Ethyl Alcohol C 2 H 5 OH .7928 348 439 Ethyl Alcohol C 2 H 5 OH 25 .7844 .98 (0.88) I .249 Glycol (CH 2 OH) 2 o I .1039 3 27 2 97 Glycol (CH 2 OH) 2 25 I .0904 7 63(7-55) 7 .00 Acetonitril CH 3 CN o .8163 2 .24 2 74 Acetonitril CH 3 CN 25 7929 3 04 (3-54) 3 83 Propionitril CH 3 CH 2 CN o .8059 .618 .767 Propionitril CH 3 CH 2 CN 25 .7830 .81-1.01 i .29 Benzonitril C 6 H 5 CN 25 .467 Methyl Sulphocyanide CH 3 SCN 25 I .0828 4 .40 4 .06 Ethyl Sulphocyanide C 2 H 5 SCN 25 I OOI2 475 47 Nitro Methane CHgNO 2 o I .1658 3 59 3 .004 Nitro Methane CH 3 NO 2 25 I .1476 5 .61-6.27 5 .61 Nitroso Dimethylin (CH 3 ) 2 N.NO 25 I .0059 2 .67 2 .66 Acetyl Acetone CH 3 COCH 2 COOCH 3 25 .268 Furfurol C 4 H 3 O.COH o I 1738 3 .91 3 33 Furfurol C 4 H 3 O.COH 25 I .1692 5 33 4 55 Benzaldehyde C C H 5 COH 25 43 Salicylaldehyde C 6 H 4 .OH.COH 25 change- able-17-7 Anisaldehyde C6H 4 .OCH 3 .COH 25 . . . 59 . . . Acetone (CH 3 ) 2 CO o o -799I .174 o 218 Acetone (CH 3 ) 2 CO 25 .249 o. 218 Ethyl Acetate CH 3 COOC 2 H 5 25 .00039 . . Ethyl Nitrate C 2 H 6 ON0 2 25 I, 0984 .062 o. 056 Benzoyl Ethyl Acetate C 6 H 5 COCH 2 COOC 2 H 5 25 I. *303 .321 o. 284 Di-Methyl Malonate CH 2 (COOCH 3 ) 2 25 I . 040 o. 035 Methyl Cyan Acetate CH 2 CNCOOCH 3 o I. 1341 1.82 I . 605 Methyl Cyan Acetate CH-jCNCOOCHa 25 ... 2.83 Ethyl" Cyan Acetate CH 2 CNCOOC 2 H 6 I . 0760 I. 057 o. 981 Ethyl Cyan Acetate CH 2 CNCOOC 2 H 6 25 I . 0607 I . I . 4i AMMONIUM IODIDE 28 Tetra Propyl AMMONIUM IODIDE N(C 3 H 7 )J. SOLUBILITY IN SEVERAL SOLVENTS. (Walden Z. phyaik. Chem. 55, 709, '06 .) Q ,, . Cms. N(C 3 H 7 ) 4 I per too. ap. or. ot i f Solvent. Formula. A. O Op. VJi . Ul ' Solution. cc. Solution. Gms. Solution. Methyl Alcohol CH 3 OH o 0.9756 40 .92 41- 94 Methyl Alcohol CH 3 OH 25 1.0187 56 .42 55- 37 Ethyl Alcohol C 2 H 6 OH o 0.8349 6 .5-6.8 8. 14 Ethyl Alcohol C 2 H 6 OH 25 0.8716 19 .88-20.29 2 3- 28 Acetonitril CH 3 CN o 0.8553 13 03 IS- 24 Acetonitril CH 3 CN 25 0-8584 18 .69 21. 77 Propionitril C 2 H 5 CN o 0.8280 6 37 7- 66 Propionitril CjjHjiCN 25 0.8191 9 65 ii . 76 Benzonitril C 6 H 6 CN 25 1.0199 8 44 8. 35 Nitro Methane CHgNOa o .181 14 79 12 . 5 2 Nitro Methane CH 3 NO 2 25 .158 22 .24 19. 21 Nitro Benzol C 6 H 5 NO 2 25 .193 5 7 1 4- 79 Benzaldehyde CeHfiCOH o .0581 7 .06 6. 67 Benzaldehyde C 6 HcCOH 25 0549 9 .87 9- 35 Anisaldehyde C 6 H 5 .OCH 3 .COH o .1114 5 .60 5- 04 Anisaldehyde C 6 H 5 .OCH 8 .COH 25 .1004 6 75 6. 14 Salicylaldehyde C 6 H 6 .OH.COH 52 39 .28 . . . Ethylnitrite C 6 H 5 ON0 2 o .1207 0.522 O- 466 Ethylnitrite C 6 H S ON0 2 25 .1025 o 653 o. 592 Di-Methyl Malonate CH 2 (COOCH 3 ) 2 1532 o .298 o. 259 Di-Methyl Malonate CH 2 (COOCH 3 ) 2 25 I 34S o .320 o. 282 Acetone (CH 8 ) 2 C o 0.8259 2 .692 3 26 Acetone (CH 3 ) 2 CO 25 0.8049 3 944 4.90 Ethyl Acetate CH 3 COOC 2 H 6 25 0.8975 o .0063 o 007 AMMONIUM NITRATE NH 4 NO 3 . SOLUBILITY IN WATER. (Schwarz Ostwald's Lehrbuch, xd ed. p. 425; Muller and Kaufmann Z. phjsik.Chem. 42, 497. 'oi-'o2.) t. Sp. Gr. Solution. G. Mols. NH 4 N0 3 per zoo Mols. H 2 C Gms. NH4NO 3 per 100 Gms. Solid Phase. * Solution. Water. o 26-63 54 19 118 3 NH 4 NO 3 rhomb, ft 12 2 1-2945 34 50 60 53 *$3 4 a 2O .2 .3116 43 30 65 80 192 4 2 5 O 3 J 97 4 8 .19 68 i7 214 2 tt 30 O 3299 54 .40 70 73 241 8 (i 32 .1 3344 57 .60 7i 97 256 9 NH 4 NO 3 rhomb, ft + rhomb, a 35 .0 3394 59 .80 72 64 265 8 NH 4 NO 3 rhomb. 4o .0 3464 66 .80 74 82 297 O ti 50 .0 77 .41 77 49 344 M 60 .0 94 73 80 81 421 .0 tt 70 .0 112 30 83 32 499 O tt 80 .0 *3o So 85 2 5 580 .0 tt 90 .0 166 So 88 08 740 NH 4 NO 3 rhombohedral ? 100 .0 196 oo 89 7i 871 O 29 AMMONIUM NITRATE SOLUBILITIES OF MIXTURES OF AMMONIUM NITRATE AND OTHER SALTS. (Riidorff Mulder.) ioo gms. H 2 O dissolve 162.9 gms. NH 4 NO 3 + 77.1 gms. NaNO, at i6R. ioo gms. H 2 O dissolve 88.8 gms. NH 4 NO 3 + 40.6 gms. KNO. at 9 M. ioo gms. H 2 O dissolve 101.3 gms. NH 4 NO 3 + 6.2 gms. Ba(NO 8 ) 2 at 9M. SOLUBILITY OF AMMONIUM NITRATE IN AMMONIA. (Kuriloff Z. physik. Chem. 25, 109, '98.) Gms. Mols. NILJSTOs Gms. per ioo Mols. Gms. Mols. NH^Os Gms. Der TOO MnU. f. NH 3 . NH 4 NO 3 t. + NH 3 . NH4NOS. NH 3 . NI^NOg + NH a . -80 O IOO O .0 33 3 O 9358 O 2352 45-9 -60 1.3918 4.4327 6 25 35 9 .7746 O 1857 47-o -44-5 0.9526 1-2457 13 9 68 .8 4 .2615 7747 53-8 -30 0.8308 0.3700 32 3 94 O 6439 .0665 67-3 -10.5 0.9675 0-35*5 36 9 190 .8 o 7578 .0588 74-2 o o . 7600 o . 2607 38 3 168 .0 IOO-O t temperature of equilibrium between solution and solid phase. SOLUBILITY OF AMMONIUM NITRATE IN NITRIC ACID. (Groschuff Ber. 37, 1488, '04.) Determinations by the " Synthetic Method," see Note, page 9. Gms. Mols. Gms. Mols. Solid t o NH 4 NO 3 NH 4 NOa Solid per ioo per ioo Phase. per ioo per ioo Phase. Gms. Sol. Mols. HNO 8 . Gms. Sol. Mols. HNO 3 . 8 21. 1 21. 1 NI^NOa^HNOa n.o 51.7 84.3 NH.NO 8 .HNO S 23 28.7 31.6 a 12.0 54.7 95.1 " labil. 29. 5m.pt. 38. 8 50.0 11.5 57.6 108.0 " b 27.5 44.6 63.4 b 11.5 54.0 92.4 NI^NOa kbit. 23.5 49.4 76.8 17.0 54.7 95.1 " stabil. 17.5 54.0 92.4 27.0 56.2 101.0 16.5 54-3 93-5 vmxTrTiiwr* 4 9' 6 '4 120.0 4.0 45-8 66.7 NHtfWfcJWO^ 79 o 68>I l6g Q a= solution in HNO 8 , 6 = solution in NH NO,. SOLUBILITY OF AMMONIUM TRI-NITRATE IN WATER. (Groschuff.) Gms. NI^NOa Gms. HNO 3 Mols. NH4NO3* Mols. NH^Oa to per ioo per ioo per ioo per ioo Solid . Gms. Gms. Mols. total Mols. Phase Solution. Solution. H20. Solution. -8 34-2 53-9 22.0 NH.NO3.2HNO3 -2.5 34-8 54-8 75 - 1 23-1 35-4 55-8 90.0 24-3 8^5 36.6 5 6 -9 113.0 25-7 19-5 37-4 58-9 225 .0 29.0 25.0 38-1 60.0 450.0 31.0 29.5 m. pt. 38.8 61.2 o.o 00 (I * or NH*NO 8 . 2 HNO 8 . AMMONIUM NITRATE 30 SOLUBILITY OF AMMONIUM NITRATE IN AQUEOUS ETHYL ALCOHOL. (Fleckcnstcin Physic. Z. 6, 419, '05.) Grams of NH4NO 3 Dissolved per 100 Grams Aq. Alcohol of (Wt.%). V . 100%. 86.77%. 76.12%. 51.65%. 25.81%. 0%. 20 2-5 II. 23.0 70-0 140 J 95 30 4.0 14.0 32.0 90.0 165 230 40 5-o 18.0 43 - 115.0 196 277 50 6.0 24.0 5S-o 144-0 244 365 60 7-5 30.0 70.0 183.0 320 70 9.0 41 .0 93-o 230.0 80 10.5 56.0 NOTE. The figures in the preceding table were read from curves shown in the abridged report of the work, and are therefore only approximately correct. Determinations of the solubility in methyl alcohol solutions were also made but not quoted in the abstract. The " Synthetic Method" (see Note, page 9) was used. 100 grams absolute ethyl alcohol dissolve 4.6 grams NH 4 NO 3 at 14 and 3.8 grams at 20.5. 100 grams absolute methyl alcohol dissolve 14.6 grams NH 4 NO 3 at 14 and 17.1 grams at 20.5. (Schiff and Monsacchi Z. physik. Chem. 21, 277, '96; at 20.5 de Bruyn Ibid., 10, 783, '92.) AMMONIUM MAGNESIUM NITRATE 2NH 4 NO 3 .Mg(NOa) 2 . 100 parts water dissolve 10 parts salt at 12.5. (Foucroy.) AMMONIUM MANGANIC MOLYBDATE 5(NH 4 ) 2 MoO 4 .Mn 2 (Mo 2 O 7 ) 3 . i 2 H 2 0. 100 parts water dissolve 0.98 Darts salt at 17. (Struve J. pr. Chem. 61, 460, '54 ,) AMMONIUM OXALATE (NH 4 ) 2 C 2 O 4 . 100 grams H 2 O dissolve 2.215 grams (NH 4 ) 2 C 2 O 4 at o Sp. Gr. of solution = 1.0105. (Engel Ann. chim. phys. [6] 13, 359- '88.> SOLUBILITY OF NEUTRAL AMMONIUM OXALATE IN AQUEOUS SOLU TIONS OF ACID AMMONIUM OXALATE. (Engel.) i Milligram Mols. per 10 Grams per 100 cc. cc. Solution. Solution. (NH 4 ) 2 C 2 O 4 3.54 o.o 2.19 o.o 2.65 1.45 1.63 0.77 2-475 2 -5 2 5 1-5* T -34 2.38 2 90 1.47 1-54 * Both salts present in solid phase AMMONIUM OXALATE SOLUBILITY OP AMMONIUM OXALATE AND OXALIC ACID IN WATER AT 25. (Walden Am. Ch. J. 34, 149, '05.) Mixtures of the two substances were dissolved in warm water and the solutions allowed to cool in a thermostadt held at 25. Composition of Solution. Solid Phase. HaO and (NH) 2 C 2 O 4 .3H 2 C2O 4 .4H 3 O Double salt, Grams per 100 Gms. Solution. Mols. per 100 Mols. H 2 0. (NH^aCaO*. H 2 Ca0 4 : (NH4)2C204 . HaC 2 4 . 0.28 10-20 0.045 2.281 0.46 7.24 0.072 1-570^ 2-44 2-59 0.372 0-546 3-65 2.80 0.566 0-599 4-99 3-41 0.791 Q-745 ) 5.20 3-55 0.824 0.781 5-36 3-38 0.853 0.741 i 6.27 3-4 1. 00 0.671 5 7-03 2.90 1-13 0.645 > 7.08 2.70 I.I4 0-599 6.92 Q-775 (N rH 4 ) 2 C 2 4 . 3 H 2 C 2 4 . 4 H 2 (NH 4 ) 2 C 2 4 .H 2 C 2 4 .H 2 and Double salt, (NH 4 ) 2 .CaO 4 .H 2 C 2 O 4 .HaO (NH 4 ) 2 C 2 O 4 .H 2 C 2 O 4 (NH 4 ) 2 C 2 4 AMMONIUM HYDROGEN PHOSPHITE (NH 4 H)HPO 3 . 100 grams water dissolve 171 grams (NH 4 H)HPO 3 at o, 190 grams at 14.5 and 260 grams at 31. (Amat. Compt. rend. 105, 809, '87.' AMMONIUM PERMANGANATE NH 4 MnO 4 . 100 parts water dissolve approximately 8 parts of NH 4 MnO 4 at 15. (Aschoff.) AMMONIUM FLUO SILICATE (NH 4 ) 2 SiF 6 . 100 parts water dissolve 18.5 parts (NH 4 ) 2 SiF e at 17.5, Sp. Gr. 1.096. (Stolba Chem. Centr. 418, 1877.) AMMONIUM SALICYLATE C 6 H 4 (OH)COONH 4 . 100 parts H 2 O dissolve ui.i parts C 6 H 4 (OH)COONH 4 at 25; 100 parts alcohol dissolve 43.5 parts at 25 and 100 parts at the b. pt. (U. S. P.) AMMONIUM SULPHATE (NH 4 ) 2 SO 4 . SOLUBILITY IN WATER. (Mulder.) Grams (NHi) 2 SO 4 per 100 Grams. Grams (NH 4 ) 2 SO 4 per too Grams. 'Water. Solution. * * Water. Solution. o 70.6 41.4 30 78.0 43-8 5 7 1.8 41.8 40 81.0 44.8 10 73-o 42.2 60 88.0 46.8 15 74-2 42.6 80 95 3 48.8 20 75-4 43-o 100 103-3 50 8 25 76.7 43-4 108.9 107-5 5i-8 Sp. Gr. of saturated solution at 15 1.248; at 19 = 1.241. AMMONIUM SULPHATE 32 SOLUBILITY OF MIXTURES OF AMMONIUM SULPHATE AND COPPER SULPHATE AT 16, AND OF AMMONIUM SULPHATE AND POTASSIUM SULPHATE AT 19.1. (Riidorff Ber. 6, 482, '73.) + CuSO 4 . G. per i oo g. Solution. . . G. per ioo g. Solution Preparation of Solution. f -^^^ Preparation of Solution. ^_ cr> ^ gA Both salts in excess 8.55 7.12 Both salts in excess 39.3 37.97 1 5 cc. sat. sol. + 3 gms. 1 5 cc. sat. sol. + 4 g. (NH 4 ) 2 SO 4 1.77 18.16 K 2 SO 4 4 -94 33-26 15 cc. sat. soL + 3 gms. 15 cc. sat. sol. + 4 g. CuSO 4 .sH 2 O 15.85 5.65 (NH 4 ) 2 SO 4 2.05 40.80 SOLUBILITY OF AMMONIUM SULPHATE IN AQUEOUS ETHYL ALCOHOL SOLUTIONS. (Traube and Neuberg Z, physik. Chem. i, 510, '87; Bodlander Ibid. 7, 318, '91; Schreinemaker Ibid. 23, 657, '97 ; deBruyn Ibid. 32, 68, 'oo; Linebarger Am. Ch. J. 14, 380, '92.) Upper Layer Results. Lower Layer Results. Grams per 100 Gms. Solu- Gms. QHsOH Gms - (NH 4 ) 2 SO 4 per ioo g. tion at io-4o. pe r IOO Gms. Solution at: C 2 H 6 OH. (NH 4 ) 2 SO 4 . Solution. 6 . 5 <>. 15 <> ^^ ioo o.o o 42.0 42.6 44 80 o.i 2.5 39.0 40.2 ? 70 0-3 5-0 36.2 37.2 ? 60 1.4 7-5 33-2 34-5 42 50 3.2 10. o 30.0 31.0 35 45 4.8 12.5 27.2 28.0 ? 40 6.6 15-0 24.6 25.2 ? 35 9.2 17.5 22.0 22.4 ? 30 12.2 2O. O 2O. O 2O. O ? 25 14.6 NOTE. When ammonium sulphate is added to aqueous solutions of alcohol, it is found that for certain concentrations and temperatures the solutions separate into two liquid layers, the upper of which con- tains the larger percentage of alcohol. Most of the determinations which have been made upon this system, as contained in the papers referred to above, are given in terms of grams of ammonium sulphate, of alcohol and of water per ioo grams of these three components taken together. Those results which are given in other terms can be readily calculated to this basis, and it is therefore possible to make a comparison of the several sets of de- terminations by plotting on cross-section paper and drawing curves through the points. In the present case the grams of alcohol per ioo grams of solution were taken as ordinates, and the grams of ammo- nium sulphate in the same quantity of each solution taken as abscissae. It was found that a single curve could be drawn through practi- cally all the points representing the upper layer solutions at the several temperatures, but the points for the solutions containing the larger amounts of water gave curves which diverged with increase of temperature. The results given for 33 in the above table are not to be accepted as correct until further work has been done. 33 AMMONIUM SULPHATE SOLUBILITY OF AMMONIUM SULPHATE IN AQUEOUS PROPYL ALCOHOL SOLUTIONS AT 20. (Linebarger Am. Ch. J. 14, 380, '92.) Gms. per ioo Gms. Solution. Gms. per ioo Gms. Solution. CsHjOH. (NH 4 ) 2 SO 4 .' C 3 H 7 OH. (NH4) 2 SO 4 ; 70 60 50 0.4 1.0 2.0 40 30 20 3-2 4-8 6. 7 AMMONIUM CADMIUM SULPHATE (NH 4 ) 2 Cd(SO 4 ) 2 6H 2 O. 100 cc. H 2 O dissolve 72.3 grams (NH 4 ) 2 Cd(SO 4 ) 2 at 25. (Locke Am. Ch. J. 27 459. *ox.) AMMONIUM CHROMIUM SULPHATE (Alum) (NH 4 ) 2 Cr 2 (SO 4 ) 4 . 2 4 H 2 0. loocc. H 2 O dissolve 10.78 grams anhydrous or 21.21 grams hydrated salt at 25. (Locke Am. Ch. J. 26, 174, '01.) AMMONIUM COBALT SULPHATE (NH 4 ) 2 Co(SO 4 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Tobler Liebig's t. O 10 20 25 30 AnnalenQS, 193, '<;<;; v. Hauer J. pr. Chem. 74* 433. '58; at 25, Locke Am. Ch. J. 27, 459. '01.) Gms. (NH 4 ) 2 Co(SO 4 ) 2 Gms. (NH4) 2 Co(SO 4 ) 2 per 100 Gms. 4. per 100 Gms. \Vater. 6.0 9-5 13.0 14.72 17.0 Solution. 5-7 8.7 "5 12.8 14-5 40 So 60 70 80 Water. 22 -O 27.0 33-5 40.0 49.0 Solution. 18.0 21-3 25-1 28.6 32-9 NOTE. The determinations reported by the above named inves- tigators were plotted on cross-section paper and although considerable variations were noted, an average curve which probably represents very nearly the true conditions was drawn through them, and the above table made from this curve. AMMONIUM COPPER SULPHATE (NH 4 ) 2 Cu(SO 4 ) 2 .6H 2 O. ioo grams H 2 O dissolve 26.6 grams salt at 19, Sp. Gr. of sol. =1.1336 (Schiff Liebig's Ann. 109, 326, '59.) AMMONIUM IRON SULPHATE (Alum) (NH 4 ) 2 Fe 2 (SO 4 ) 4 .2 4 H 2 O. ioo cc. H 2 O dissolve 44.15 gms. anhydrous or 124.40 gms. hydrated salt at 25. Sp. Gr. of saturated solution at 15 = 1.203. (Locke Am. Ch. J. 26, 174, 'oi.J AMMONIUM IRON SULPHATE (ferrous) (NH 4 ) 2 Fe(SO 4 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Tobler; at 25, Locke Am. Ch. J. 27, 459. '01.) t o G. (NH 4 ) 2 Fe(S0 4 ) 2 t o G. (NH 4 ) 2 Fe(SO 4 ) 2 t o G. (NH 4 ) 2 Fe(SO 4 ) 2 per ioo g. H 2 O. per ioo g. H 2 O. per ioo g. H 2 O. o 12.5 25 25.0 (T) 50 40 15 20.0 25 35.1 (L) 70 52 40 33-o AMMONIUM INDIUM 34 SULPHATE AMMONIUM INDIUM SULPHATE (NH 4 ) 2 In 2 (SO 4 ) 4 .2 4 H 2 O. 100 g. H 2 O dissolve 200 gms. salt at 16 and 400 gms. at 30. (Rossler J. pr. Chem. [2] 7, 14, '73.) AMMONIUM MAGNESIUM SULPHATE (NH 4 ) 2 Mg(SO 4 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Average curve, from results of Mulder, Tobler, Locke, at 25.) G. (NI I 4 ) 2 Mg(SO 4 ) 2 G. (NH 4 ) 2 Mg(SO 4 ) 2 t. per 100 Gms. t. per 100 Gms. Water. Solution. Water. Solution. 9.0 8.8 40 27.0 21.3 10 13.0 "5 50 32.0 24.4 20 18.0 60 37.0 27.0 25 19.9 16.6 70 42.0 29.6 30 22 -O 18.0 80 47-0 32.0 AMMONIUM MANGANESE SULPHATE (NH 4 ) 2 Mn(SO 4 ) 2 .6H 2 O. 100 cc. water dissolve 37.2 gms. (NH 4 ) 2 Mn(SO 4 ) 2 at 25. (Locke Am. Ch. J. 27. 459, *oi.) AMMONIUM NICKEL SULPHATE (NH 4 ) 2 Ni(SO 4 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Average curve from Tobler, Locke, at 25.) G. (NH 4 ) 2 Ni(S0 4 ) 2 G. (NH4) 2 Ni(S0 4 ) 2 t. per loo Gms. t . per loo Gms. Water. Solution. Water. Solution. i.o o-99 40 12.0 10.72 10 4.0 3.85 50 14-5 12.96 20 6.5 6.10 60 17-0 14-53 25 7-57 7-04 70 2O- O 16.66 30 9.0 8.45 AMMONIUM SODIUM SULPHATE NH 4 NaSO 4 . 2 H 2 O. 100 gms. water dissolve 46.6 gms. NH 4 .NaSO 4 .2H 2 O at 15, Sp. Gr. Sol. = 1.1749. . AMMONIUM VANADIUM SULPHATE (Alum) (NH 4 ) 2 V 2 (SO 4 ) 4 . 2 4 H 2 0. 100 cc. H 2 O dissolve 31.69 gms. anhydrous or 78.50 gms. hydrated Salt at 25. (Locke.) AMMONIUM ZINC SULPHATE (NH 4 ) 2 Zn(SO 4 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Average curve, see Note, p. 33, Tobler, Locke, at 25.) G. (NH 4 ) 2 Zn(S0 4 ) 3 G. (NH 4 ) 2 Zn(S0 4 ) 2 t. per TOO Gms. t. per 100 Gms. Solution. Water.' Solution. Water. " O 6-54 7-0 40 16.66 20 10 8.67 9-5 So 20-0 25 20 II .11 12.5 60 23.1 30 25 12.36 14.1 70 25-9 35 30 13-79 16.0 80 29.6 42 35 AMMONIUM PERSULPHATE AMMONIUM PERSULPHATE (NH 4 ) 2 S a O 8 . 100 parts H a O dissolve 58.2 parts (NH 4 ) 2 S 2 O 8 at o. (Marshall J. Chem. Soc. 59. 77L '91.) AMMONIUM SODIUM HYDROGEN SULPHITE (NH 4 )Na 2 H(SO 8 ) 2 4H 2 O. 100 gms. H 2 O dissolve 42.3 gms. salt at 12.4 and 48.5 gms. at 15. (Schwincker Ber. 22, 1732, '89.) AMMONIUM SULPHOCYANIDE NH 4 SCN. 100 parts water dissolve 128.1 parts NH 4 SCN at o and 162.2 parts at 20. (Clowes Z. Ch. 190, 1866.) AMYL ACETATE BUTYRATE, FORMATE, etc. SOLUBILITY IN WATER AND IN AQUEOUS ALCOHOL AT 20. (Bancroft Phys. Rev. 3. 131, 196, 205, '95- '06; Traube. Ber. 17, 2304, '84.) T? t , cc. Ester per Sp. Gr. v . cc. Ester per Sp. Gr. loocc. H 2 0. of Ester. 100 cc. H 2 O. of Ester. Amyl acetate 0.2 0.88 Amyl propionate o.i 0.88 Iso amyl acetate 0.2(1.2?) ... Iso amyl formate 0.3 (gms. at 22) Amyl butyrate o . 06 0.85 Solubility of Iso Amyl Acetate Solubility of Amyl Acetate and Amy] in Aq. Alcohol Mixtures. Formate in Aq. Alcohol Mixtures. cc. H 2 O added to cause separation of second phase in mixtures of the rr given amounts of alcohol and 3 cc. in Mixture Per 5 cc. C 2 H 5 OH. * portions of : 7 o-4 6 0.7 5 i-3 3.61 3.0 3.01 4.0 2.60 5.0 Amyl Amyl Formate. Acetate. 3 i. 80 I. 7 6 9 8.77 9-03 15 17.01 I7-52 21 27.06 26.99 27 38-3I 37-23 33 50-7I 48.41 39 65.21 45 85.10 48 94-20 ANETHOL (p Propylanisol) CH 3 CHCH[ 4 ]C 6 H 4 OCH 3 . SOLUBILITY IN AQ. ALCOHOL AT 20. (Schimmel and Co. Reports, Oct 1895, p. 6 ) Vol. per cent alcohol = 20 25 30 40 50 Gm. Anethol per liter aq. alcohol=o.i2 0.20 0.32 0.86 2.30 ANILINE 36 ANILINE C 6 H 5 (NH 2 ). SOLUBILITY IN WATER AT 22. (Herz Ber. 31, 2671, '98; see also Vaubel J. pr. Chem.f2) 52, 72, '95: Aignan and Dugas Compt. rend. 129, 643, 99.) ioo cc. H 2 O dissolve 3.481 cc. C 6 H 6 (NH 2 ) Vol. of Sol. = 103.48, Sp. Gr. = 0.9986. ioo cc. C 6 H 6 (NH 2 ) dissolve 5.22 cc. H 2 O Vol. of Sol. = 104.96, Sp. Gr. = 1.0175. SOLUBILITY OF ANILINE IN WATER AT DIFFERENT TEMPERATURES. (Alexejew Ann. Physik. Chem. 28, 305, '86; calc. by Rothmund Z. physic. Chem. 26, 475, '98.) Determinations by " Synthetic Method " see Note, p. 9. Figures read from curve. Cms. C H S (NH 2 ) per TOO Grams. i0 Cms. CeH5NH 2 per ioo Grams. Aq. Layer. Aniline Layer. Aq. Layer. Aniline Layer. 20 3-2 95-5 140 13-0 83-5 40 3-5 95-o 150 18.0 79.0 60 3-8 94-7 160 27-5 71.0 80 4-5 93-5 165 36.0 63.0 ioo 6.0 92.0 167.5(0-11. temp.) 48.6 120 8-5 88-5 SOLUBILITY OF ANILINE IN AQUEOUS SALT SOLUTIONS AT 18. (Euler Z. physik. Chem. 40, 307, '04.) Aq. & -.lutinn * jms> aau ms - ^* n slution. pgj. liter p^ JQO g , H 2 alone o 3.61 *N KC1 37-3 3-i5 N KC1 74-6 . 2.68 N NaCl 58.5 2-55 Aq. Cms. Salt G Solution. per liter, per ioo g. sol vent. N NaOH 40.06 1.90 N LiCl N CuCl 42.48 67.25 2.80 3.00 SOLUBILITY OF ANILINE IN AQUEOUS ANILINE HYDROCHLORIDE SOLUTIONS AT 18. (Lidow J. russ. phys. chem. Ges. 15, 420, '83; Ber. 16, 2297, '83.) Per cent CeHcNKfeHCl Gms. C6N 6 NH 2 per ioo g. Sol vent. 3-8 Per cent QHeNHa-HCl in Solvent. Cms. per loog. Sol vent. insolvent, 5 3- 30 39-2 12 5-3 35 50-4 25 l8 -3 DISTRIBUTION OF ANILINE BETWEEN: (Vaubel J. pr. Chem. [2] 67, 477. '3-) Water and Ether. Water and Carbon Tetrachloride. Composition of Solutions. Gms. CsHcNHjin: Composition of Solutions. Gms.CeHsNI^ in: 1.24^8 1.2478 1.2478 50 cc. H 2 O -f 2occ. Ether 50 cc. H 2 O + 5occ. Ether 50 cc. H 2 O -f ioo cc. Ether 0.1671 0.0835 0.0594 1.0807 1.1643 1.1884 0.3478 1.2478 1.2478 50 cc. H 2 O + 20CC.CC1 4 50 cc. H 2 O + 50 cc. CC1 4 50 cc. H 2 O + ioocc.CC! 4 ] 0. 0. o. 3358 2767 1845 0.012 I.97I 1.063 SOLUBILITY OF ANILINE IN SULPHUR. (Alexejew Ann. Physik. Chem. 28, 305, '86.) IOO no 120 Gms.C6H6NH 2 per loog. S. Layer. Anilin Layer". 4 75 6 70 10 64 Gms. CflH s NH 2 per ioog. S. Layer. W J 5 135 17-5 138 (crit. temp.) Anilin Layer'. 5 8 47 23 . . 37 ANILINE DISTRIBUTION OF ANILINE BETWEEN WATER AND TOLUENE AND BETWEEN AQUEOUS SALT SOLUTIONS AND TOLUENE AT 25 (RbcLl Z. physik. Chem. 56, 243, '06.) NOTE. Mixtures of Aniline and Toluene were shaken with water or with aqueous salt solutions, and after separation of the two layers the Sp. Gr. of the A : T mixture (layer) was determined and also the amount of Aniline in each layer. Solution Shaken with A : T Mixture. Vol. per cent ! Aniline : Toluene in Mixtures Used. Sp. Gr. of A : T Mixture after Separation. Cms. C 6 H 5 N1 ^2 in 100 cc. of: A : T Layer. Aq. Layer. H 2 50:50 0.9257 41-5 2.14 " 25:75 0.8928 20-7 I .5 " 12.5:87.5 0-8737 8.62 0.86 " 0.8661 3-87 0-45 M 2.5:97.5 0.8627 1.68 O-2I o.xN *i 50:50 0.9297 44-o 2-09 2 14 25:75 0-8901 19.03 1.38 ' 12.5:87.5 0.8739 8-77 0.81 M 5-5:94-5 0.8663 3-94 0.42 M 0-8629 1.81 0.21 o.iN KBO 2 50:50 0-9257 41 .61 2. II M 25:75 0.8870 17.08 i-34 14 12.5:87.5 0.8748 9-34 0.92 ii 0.8661 3-85 o-44 11 2-5:97-5 0.8627 1.72 0.21 XT Ba(OH) O.OIOQ4N > ' 2 50:50 0-9334 46.52 2.IO 2 11 25:75 0.8929 20.78 I .46 ft 12.5:87.5 0.8749 9.41 0.88 11 5-5:94 5 0.8663 3 96 o-43 it 2-5:97-5 0.8628 1.72 O-2O XT Sr(OH) 2 o.io4N s 50:50 o-9333 46-45 2.13 2 M 25:75 0.8929 20.78 1.46 XT Sr(OH). o . I044N \ L L i2. 5 :8 7 -5 0.8750 9.46 0.88 2 M 5-5:94-5 0.8662 3-96 0-43 f XT or(Oxr) o.io63N s fl L 2.5:97.5 0.8628 i-75 O-2O 2 . 04 N Ca ( QH )2 50:50 0-9333 46.18 2. 2O 2 " 25:75 0.8925 20.59 1.51 II 12.5:87.5 0.8749 9-43 0.91 " 0.8662 3 -89 0-44 M 2.5:97.5 0.8627 1.70 0-21 ioo cc. aqueous solution contain 3.607 gms. Aniline at 25. ANILINE SOLUBILITY OF ANILINE, PHENOL MIXTURES IN WATER. (Schreinemaker Z. physik. Chem. 29, 584; 30, 460, 'go.) Mixture used = 50 Mols. Aniline + 50 Mols. Phenol Gms. of Mixture per 100 Gms. 40 60 80 100 no 104 (crit. temp.) 33 Mixture used = 2<;.4 Mols. Aniline + 74 6 Mols. Phenol Gms. of Mixture per 100 Gms. * Aq. Layer. 5-5 8.0 12.5 19.0 A. + P. Layer. 86.0 4 82.0 8 77.0 10 67.0 12 5 6 -5 13 '35 Aq. Layer. 4-0 5-5 8.0 A. + P. Layer. 91-5 85-5 82.0 *3-5 19.0 23-5 73-5 66.0 58-0 140 (crit. temp.) 35 Determinations" in above" table by "Synthetic Method," see NOTE, p. 9. Schreinemaker gives results for several other mixtures of Aniline and Phenol which yield curves entirely similar to those for the two mixtures here shown. NitrANILINES C 6 H 4 NH 2 NO 2 . o, m, and p. SOLUBILITY IN WATER. (Carnelly and Thomson J. Chem. Soc. 53, 768, '88; Vaubel J. pr. Chem. [2] 52, 73, '95; above ao Lowenherz Z. physik. Chem. 25, 407, '98.) Grams NHraniline per Liter of Solution. 20 24.2 27.3 Ortho Nitranilinc. 1.25(25) Mcta Nitraniline. I.I4-I.67 1.205 1-422 Para Nitraniline. 0.77-0.80 SOLUBILITY OF ORTHO AND OF META NITRANILINE IN HYDROCHLORIC ACID. (Lowenherz.) Ortho Nitraniline at 25. G. Mols. per Liter. Grams per Liter Meta Nitraniline. G. Mols. per Liter. Grams per Liter. 'HCl CeHsNHa. TJ/~M C* U VT LJ " ri.V^.1 i^grT^INri^. 'HCl C 6 H 5 NH 2 . HCl C 6 H 5 NH 2 . ]O2(o) NO 2 (o) NO 2 (w) N0 2 (m) o.o .0091 O .0 i 2 5 (25) o.o .OO9I o.o 1.20 0.63 O .0143 22 97 ' i 97 (26. 5) 0.0125 .0183 0.46 2-53 0.95 .0174 34 63 2 .40 (23. 3) 0.0247 .0274 0.90 3-85 1.26 .0215 45 94 a 97 SOLUBILITY OF META AND OF PARA NITRANILINE IN ORGANIC SOLVENTS AT 20. (Carnelly and Thomson.) Solvent. Methyl Alcohol Ethyl Alcohol Propyl Alcohol Iso Butyl Alcohol Iso Amyl Alcohol Ethyl Ether Gms. per Liter. Meta. no. 6 70-5 56.5 26.4 85-1 78.9 Para. 95-9 58-4 43-5 19.1 62.9 61 .o Solvent. Benzene Toluene Cumene Chloroform Carbon Tetra Chloride Carbon Bisulphide Gms. per Liter. Meta. 24-5 I7.I "5 30.1 2.1 3-3 Para. 19.8 9-0 23.1 2.6 ANISIC ACID (p-Methoxybenzoic acid) CH 3 O.C G H 4 .COOH. See also p. 61. 100 cc. sat. aq. solution contain 0.2263 8 m - Anisic acid at 25. (Paul Z. physik. Chem. 14, xn, '94.) 39 ANTHRACENE ANTHRACENE C U H 10 . SOLUBILITY IN LIQUID SULPHUR DIOXIDE IN (Centnerswer and Teletow Z. Electrochem. Weighed amounts of anthracene and liquid tubes which were then sealed, rotated at temperature and the point at which the solid THE CRITICAL REGION* 9. 799. '03.) SO 2 were placed in glass a gradually increasing disappeared, observed. 40.1 45-8 47-9 Gms. C M H 10 per 100 g. Solution. 2. II 2.48 2 .65 Gms. per 100 g. Solution. 65.0 7 8.2 88.0 4-0 5 .66 7.14 98.0 99-1 106.5 Gms. C u H 10 per 100 g. Solution. 9-95 12.78 SOLUBILITY OF ANTHRACENE IN ABSOLUTE ETHYL AND METHYL ALCOHOLS. (v. Becchi; at 19.5, de Bruyn Z. physik. Chem. 10, 784, '92.) Grams C u HIO per 100 Grams Alcohol at; In Ethyl Alcohol In Methyl Alcohol 16. 0.076 19-5. 1.90 1. 80 b. pt. 0.83 SOLUBILITY OF ANTHRACENE IN BENZENE. (Findlay J. Chem. Soc. 81, 1221, '02.) Gms. C M H 10 per 100 Gms. Mols. C M H 10 per 100 Mols. C 6 He- CeHe. 0-979 0.429 1.118 0-49 1 I .296 0.567 !-53 2 0.673 1-830 0.803 I-95 1 0.856 2-175 0-954 5 10 20 25 26 30 12.94 parts at 100 (v. Becchi). t< Gms. C M H, s . per 100 Gms. Mols. C M H, per too Mols. 38 4 2.773 I.2I3 40 .0 2.987 I.3I2 44 .6 3.368 1-473 50 3.928 60 4.941 2.164 70 6.041 2.649 80 7-175 3- J 43 irt s anthracene at 16.5 and SOLUBILITY OF ANTHRACENE IN ALCOHOLIC PICRIC ACID SOLUTIONS AT 25. (Behrend Z. physik. Chem. 15, 187, *94-) ; per Solu ilution. Picric Acid. O I-OI7 2.071 2.673 3-233 Anthracene . 0.176 0.190 O.2O6 O.2I5 0.228 3.469 0.236 Solid Phase. Anthracene tt Anthracene and Anthracene Picrate Grams per 100 Gms. Solution. Picric Acid. 3-999 5.087 5-843 6.727 7-5 11 7-452 Anthracene. O.2O2 0.180 O.l62 O.I5I 0.149 Solid Phase, Anthracene Picrate Anthracene Picrate H- Picric Acid Picric Acid ANTHRAQUINONE 40 ANTHRAQUINONE (C 6 H 4 ) 2 (CO) 2 . SOLUBILITY IN LIQUID SULPHUR DIOXIDE IN THE CRITICAL REGION. (Centnerswer and Teletow Z. Electrochem. 9, 799, '08.) (See Anthracene, page 39). _ _ Cms. CuHgOj Cms. C M H 8 O 3 t. per zoo g. t. per 100 g. t. per ipo g. Solution. Solution. Solution. 39.6 0.64 92.1 2.81 118.5 S-6o 51.5 0.88 101.4 3.67 141.6 7.53 67.9 1.73 106.3 4.23 160.0 9.60 82.4 2.24 108.7 4.40 J 79-o 12.70 183.7 18.30 100 parts of absolute ethyl alcohol dissolve 0.05 part anthroquinone at 18 and 2.249 parts at b. pt. (v. Becchi). SOLUBILITY OF ANTHRAQUINONE IN ETHER. (Smits Z. Electrochem. g, 663, '03.) Weighed amounts of ether and anthraquinone were placed in glass tubes which were then sealed. The temperature noted at which the anthraquinone disappeared and also at which the liquid phase disap- peared (critical temp.). The two curves cross at 195 and again at 241. Between these two temperatures the critical curve lies below the solubility curve, hence for this range of temperature no solubility curve is shown. The following figures were read from the curves, and are therefore only approximately correct. Cms. CuHjAi Cms. CuHgOz Cms. t. per loo g. t. per 100 g. t^ per 100 g. Solution. Solution. Solution. 130 3 241 30 260 80 150 4 245 40 270 90 170 4-5 2 47 50 275 100 195 5.0 250 60 100 parts of toluene dissolve 0.19 part anthraquinone at 15 and 5.56 parts at 100 (v. Becchi). ANTIMONY TRICHLORIDE SbCl s . SOLUBILITY IN WATER. SOLID PHASE SbCl 3 . (Meerburg Z. anorg. Chem. 33, 299, 1903.) Mols. SbCls Cms. SbCU Mols. SbOa Cms. SbCl t. per loo per 100 t. per 100 per 100 Mols.H 2 0. gVHaO. % Mols. H 2 O. g. H^. o 47-9 601.6 35 91.6 1152.0 15 64.9 815.8 40 108.8 1368.0 (72.4 910.1 50 152.5 - 1917.0 (74.1 931-5 60 360.4 453 I -o 25 78.6 988.1 72 oo o 30 84.9 1068. o 4 i ANTIMONY TRICHLORIDE SOLUBILITY OF ANTIMONY TRICHLORIDE IN AQUEOUS HYDROCHLORIC ACID. SOLID PHASE SbCl 3 . TEMP. 20. (Meerburg.) Mols. per 100 Mok. H 2 O. Cms. per 100 g. H 2 O. Mols. per 100 Mols. H 2 O. Gms. per 100 g. HjO. HC1. SbCls/ o 72.4 2.4 71.2 6.1 69 . 9 8.3 68.2 "HC1. SbCl 3 . O-O QIOiI 4-86 895.4 12-34 879.0 16.80 857.6 fid. SbCla". ' 9-1 68.9 11.7 68.1 28.7 62.8 HC1. SbCW 18.41 866.4 23.68 856.3 58.08 789.8 ioo grams absolute acetone dissolve 537.6 grams SbCl 3 at 18. (Naumann Ber. 37, 4332, '04.) ANTIMONY TRI IODIDE SbI 3 . SOLUBILITY IN METHYLENE IODIDE AT 12. (Retgers Z. anorg. Ch. 3, 344, '93.) ioo parts CH 2 I 2 dissolve 1 1.3 parts SbI 3 . Sp. Gr. of solution = 3.453. ANTIMONY POTASSIUM TARTRATE K(SbO)C 4 H 4 O 6 .iH 2 O. ioo grams glycerine dissolve 5.5 grams of the tartrate at 15.5. ARGON, A. t o Cor. Bar. SOLUBILITY IN WATER. (Estreicher Z. physik. Chem. 31, 184, '99.) Vol. Vol. Absorbed Absorption Coefficients.* Solubility. Pressure. HafJ. Argon. a. /. q. . . .0578 O-OIO2 I 764 9 77 .40 4 34 o 0561 0561 O.OO99 5 765 .0 77 39 3 .92 .0507 .0508 0.0090 10 765 3 77 .41 3 49 .0450 0453 0.0079 15 762 4 77 .46 3 .13 .0404 o .0410 0.0072 20 757 .6 77 53 2 .86 o .0369 0379 O.OO66 25 766 7 77 .62 2 .64 o 0339 0347 O.OO6O 30 760 .6 77 73 2 43 o .0312 .0326 0-0056 35 757 .1 77 .86 2 .24 .0288 0305 0.0052 40 758 3 77 99 2 .07 o .0265 .0286 0.0048 45 756 4 78 I .92 o .0246 .0273 0-0045 5 747 .6 78 3 1 I 73 o O22I o .0257 O.OO4I a = under barometric pressure minus tension of H 2 O vapor. / under 760 mm. pressure. q = grams argon per ioo g.H 2 O when total pressure is equal to 760 mm. * See Acetylene, page 8. ARSENIC PENTOXIDE As 2 O 6 . ioo parts H 2 O dissolve .244.8 parts As 2 O 4 302.3 parts HaAsO 4 at 12.5. Sp. Gr. of solution = 2.18 at 15. (Vogel.) ARSENIC IODIDE AsI 3 . SOLUBILITY IN METHYLENE IODIDE AT 12. (Retgers Z. anorg. Chem. 3, 344, 1893.) ioo grams CH 2 I 2 dissolve 17.4 gms. AsI 3 . Sp. Gr. of solution 3.449. ARSENIC TRIOXIDE ARSENIO TRIOXIDE 42 As 2 3 . SOLUBILITY OF THE: Crystallized Modification. Amorphous Modification. In Water. In Water. A.O Gms. As 2 O 3 per 100 cc.H 2 O. ord. temp. 3 . 7 b. pt. 11.86 In Alcohol, Ether and CS 2 . G. As 2 O 3 per 100 g. Solvent. Alcohol o . 446 Ether 0.454 CS 2 o.ooi (Winkler J. pr. Chem. [2] 31, 347, '85-) Gms. AsgOa t. per TOO cc. Sat. Solution. 2 I -2OI 15 I-657 25 2.038 39-8 2.930 b. pt. 6.+ (Bruner and St. Tolloczko Z. anorg. Chem. 37, 456, '03; Chodounsky Listy. Chem. 13, 114, '88.) ASPARAGINE C 4 H 8 N 2 O 3 .H 2 O. SOLUBILITY /S-/-ASPARAGINE C 4 H 8 N 2 O 3 .H,O AND OF /S-/-ASPARAGINIC ACID C 4 H 7 NO 4 IN WATER. Determined by " Synthetic Method," see Note, page 9. (Bresler Z. physik. Chem. 47, 613, '04.) /3-/-Asparaginic Acid. /3-J-Asparagine. O 7' 28, 41. 7 9 4 Gms. : 4 H 8 N 2 3 .H 2 C per 100 g. H 2 0. 0.9546 I .4260 2.1400 3.I7IO 5.6500 55 87 98 5 7 .0 .0 Gms. C 4 H8N 2 3 .H 2 per 100 g. H 2 0. 10.650 19.838 36-564 52-475 *~ Gms. Gms. t. C 4 H 7 NO 4 t. C 4 H 7 N0 4 per 100 g. per 100 g. H 2 0. H 2 0. 0.2 0.2674 51.0 1.2746 9-5 o . 4042 63-5 1.8147 16.4 0.5176 70.0 2.3500 31 .5 0-75*4 80.5 3.2106 40.0 0.9258 97-4 5-3746 ATROPINE C 17 H 23 NO 3 . SOLUBILITY OF ATROPINE C 17 H 23 NO 3 AND OF ATROPINE SULPHATE (Ci 7 H,3NO 3 ) 2 .SO 2 (OH) 2 IN WATER AND OTHER SOLVENTS. (U. S. P. ; Miiller Apoth.-Ztg. 18, 244, '03.) Grams Atro- Grams Atropine per 100 Grams. pine Sulphate Solvent. t. , * N per TOO Grams Solution. Solvent. (U. S. P.) Solvent. (U. S. P.) 263.1 454-5 27.0 52-6 0.047 0.161 Water 25 1.782 (20) 0.222 Water 80 "S Alcohol 2 5 . . . 68.44 Alcohol 60 III .11 Ether 25 2-21 (20) 6. 02 Chloroform 2 5 68.03 (20) 64.10 Benzene 20 3-99 . . . Carbon Tetrachloride 20 0.661 1.136 Ethyl Acetate 20 3.88 . . . Petroleum Ether 2O 0.83 . . . Glycerine IS 3-o * Schnidelmeiser Chem. Ztg. 25, 129, '01. 43 AZELAIO ACID AZELAIC ACID C 7 H 14 (COOH) 2 . SOLUBILITY IN WATER. (Lamouroux Compt. rend. 128, 998, '99.) t= o 15 20 35 50 65 Gms. C 7 H U (CO9H) 2 per 100 cc. solution = o.io 0.15 0.24 0.45 0.82 2.20 AZOPHENETOL (/>) C 6 H 5 N 2 .C 6 H 4 .OC 2 H 5 . SOLUBILITY IN 100 PER CENT ACETIC ACID. (Dreyer and Rotarski Chem. Centr. 76, II, 1016, '05.) t= 89.2 91 93 95.6 97.2 99.6 Mols. per liter. 0.153 0.176 0.185 0.209 0.232 0.252 A knick at 94.7 corresponds to the transition temperature of the a modification into the modification. BARIUM ACETATE Ba(CH 3 COO) 2 . SOLUBILITY IN WATER. (Walker and Fyffe J. Ch. Soc. 83, 179, '03; Krasnicki Monatsh. Chem. 8, 597, '87.) Solid Phase. Ba(C 2 H 3 2 ) a Gms. Ba(CH 3 COO) 2 t o < per 100 Gms. Solid Phase. t Gms. Ba(CH 3 COO) 2 . per 100 Gms. Water. Solution. Water. Solution. 3 58.8 37 .0 Ba(C 2 H 3 2 ) 2 . 3 H 2 40 5 79 .0 44 .1 I 7 9 61 6 38 .1 u 4i 5 78 7 44 .0 J 7 5 69.2 40 9 u 44 5 77 9 43 .8 21 .6 72.8 42 .1 5i .8 76 5 43 4 24 . i 78.1 43 9 (4 63 .0 74 .6 42 7 26 .2 76.4 43-3 Ba(C 2 H 3 2 ) 2 .H 2 73 .0 73 5 42 4 30 .6 75-i 42 9 it 84 .0 74 42 5 35 .0 75-8 43 .i (i 99 .2 74 .8 42 .8 39 .6 77-9 43 .8 a Transition temperatures 24.7 and 41' BAEIUM ARSENATE Ba 3 (AsO 4 ) 2 . 100 gms. H 2 O dissolve 0.055 gm. Ba 3 (AsO 4 ) 2 ; 100 gms. 5% NH 4 C1 dissolve 0.195 gm., and 100 gms. 10% NH 4 OH dissolve 0.003 S 10 - Ba 3 (AsO 4 ) 2 (Field J. Ch. Soc. n 6, 1850-) BARIUM BROMATE 44 BARIUM BROMATE SOLUBILITY IN WATER. (Trantz and Anschiitz Z. physik. Chem. 56, 238, '06; Rammelsberg Pogg. Ann. 52, 81, '41-) Cms. Ba(BrO 3 ) 2 Gms. Ba(BrO 3 ) 2 Gms. Ba(BrO 3 )j t. per 100 Gms t. per 100 Gms. t. per 100 Gms. Solution. Solution. Solution. 0.034 0.28 30 0.95 70 2.922 o 0.286 40 1.31 80 3-521 -Mo 0.439 5 *-7 2 9 4-26 20 0.652 60 2.271 98.7 S- 2 56 25 0.788 99.65 5.39 BARIUM BROMIDE BaBr 2 . 2 H 2 O. SOLUBILITY IN WATER. (Kremers Pogg. Ann. 99, 47, '56; Etard Ann. chim. phys. [7] 2, 540, '94.) Gms. BaBr 2 per TOO Grams. Gms. BaBr 2 per TOO Grams. t. 'Water. Solution. t. ' Water. Solution. (Kremers.) (Kremers.) (Etard.) (Kremers.) (Kremers.) (Etard.) 20 . . . 45- 6 40 114 53-2 S^S O 98 49-5 47-5 So 118 54-i 52-5 10 101 50.2 48-5 60 123 55-i 53-5 20 104 51.0 49-5 70 128 56-1 54-5 25 106 5i-4 50.0 80 J 35 57-4 55-5 30 109 52-i 50.6 IOO 149 60.0 57-8 140 59-4 Sp. Gr. of saturated solution at 19.5 = 1.710. The results of Kremers and Etard are both given, since it is uncer- tain which is the more correct. SOLUBILITY OF MIXTURES OF BARIUM BROMIDE AND BARIUM IODIDE IN WATER AT DIFFERENT TEMPERATURES. (Etard.) e Grams per i oo Gms. Solution. Grams per ioo^Gms. Solution. BaBr 2 . " BaI 2 . BaBr 2 . Bal^. 16 4.8 58.4 170 ii. o 67.4 +60 5.5 66.0 210 14-9 6 7-7 135 9.2 67 . 2 Both salts present in solid phase. SOLUBILITY OF BARIUM BROMIDE IN METHYL AND ETHYL ALCOHOLS. We Bruyn Z. physik. Chem. 10, 783, 92 ; Richards Z. anorg. Chem. 3, 455, '93 ; Rohland Ibid. 15 412, '97.) Parts BaBr 2 per 100 Parts BaBr 2 .2H 2 O per 100 t o parts Aq. C 2 H 6 OH of: parts of Aq. CH 3 OH of: 100%. 97%- 87%. 100%. 93-5%' SG%. 15.0 .- 0.48 (BaBr 2 .2H 2 O) .. 45.9 27.3 4-O 22.5 3 6 56.1 BARIUM BUTYRATE Ba(C 4 H 7 O 2 ) 2 .2H 2 O. SOLUBILITY IN WATER. (Deszathy Monatsh. Chem. 14, 249, '93.) e Gms. Ba(C 4 H 7 O 2 ) a per 100 Gms. Gms. Ba(C 4 H 7 Q 2 ) 2 per 100 Gms. Water. Solution". Water. Solution. o 37.42 27.24 50 36.44 26.77 10 36.65 26.82 60 37-68 27.36 20 36.12 26.55 70 39.58 28.36 30 35 - 8 5 26.38 80 42.13 29.64 40 35 -82 26.37 45 BARIUM CAPROATE BARIUM GAPROATE AND BARIUM ISO CAPROATE. SOLUBILITY IN WATER. (Kulisch Monatsh. Chem. 14, 567, '93.) (Konig Monatsh. Chem. 15, 23, '94.) Barium Caproate (Methyl 3 Pentan.) Barium Iso Caproate (Methyl 2 Pentan ) Ba(CH3.CH 2 CH(CH 3 )CH 2 COO) 2 . Ba(CH3CH(CHg)CH 2 .CH 2 COO) 2 . Gms.Ba(C 6 H u 2 ) 2 t 8 . per TOO Gms. Solid Phase. Gms. Ba(C 6 H n O 2 ) 2 per TOO Gms. Solid Phase. Water. Solution. Water. Solution. II 7i 10 .49 BaCQHuOa^iHaO 14. 34 12 54 *'< i(C6H u 2 ). 4 HaO 10 8 38 7 73 13- 33 II 77 " 20 6 .89 6 45 12 . 67 II .26 " 30 5 87 5 55 12. 37 II .01 40 50 5-79 6.63 5 6 47 .21 12 . 12. 42 83 II II 3 :: 60 8 39 7 74 13 . 63 II 99 70 ii .09 9 .98 14. 68 12 .80 44 80 14 12 .82 16. 24 13 , 97 44 00 19 .28 16 .16 17- 95 I5-23 BARIUM CARBONATE BaCO,. SOLUBILITY IN WATER. (Holleman, Kohlrausch and Rose Z. physik. Chem. 12, 139, 241, '93.) Electrolytic conductivity method used. i liter H 2 O dissolves 0.016 g. BaCO 3 at 8.8, 0.022 g. at 18, and 0.024 g- at 24.2. SOLUBILITY OF BARIUM CARBONATE IN WATER CONTAINING CO 2 . The average of several determinations at about 10, by Bineau, Lassaigne, Foucroy and Bergmann is i.io gms. BaCO 3 per liter water. Wagner (Z. anal. Ch. 6, 167, '67) gives 7.25 gms. BaCO 3 per liter of water saturated with CO 2 at 4-6 atmospheres pressure. BARIUM CHLORATE BajClO^H a O. SOLUBILITY IN WATER. (Tfantz and Anschiitz Z. physik. Chem 56, 238, '06; Kremers Pogg. Ann. 99, 43, '56; Tilden and Shenstone Trans. Roy. Soc. 34, '84.) Gms. Ba(ClO 3 ) 2 Gms. Ba(ClO 3 ) 2 Gms. BaCClOs)* t. per too Gms. t. per too Gms. t. oer 100 Gms. Solution. Solution Solution. ~ 2-75 15.28 30 29 43 90 4 8 .70 O 16.90 40 33 -16 99.1 5 1 I 7 4-10 21.23 5 36-69 105 52.62 20 25.26 60 40-05 116 66.0 25 27-53 7o 43-04 146 78.0 80 45-90 BARIUM CHLORIDE 46 BARIUM CHLORIDE BaCl 2 . 2 H 2 O. SOLUBILITY IN WATER. (Mulder; Engel Ann. chim. phys. [6] 13, 372, '88; Etard Ibid. [7] 2, 535, '94-) A0 Gms. BaCl 2 l )er ioo Gms. A0 Gms. BaCh per ioo Gms. * Water. Solution! ' 'Water. Solution. 31-6 24.0 60 46.4 3 I -3 10 33-3 25.0 70 49.4 33- 1 20 35-7 26.3 80 52-4 34-4 25 37-o 27.0 IOO 5 8.8 37.0 30 38.2 27.7 130 59-5 37-3 40 40.7 28.9 160 63.6 38-9 50 43-6 30-4 215 75-9 43 - 1 Sp. Gr. of solution saturated at o - 1-25; at 20 = 1.27. SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND BARIUM NITRATE IN WATER. Both salts present in solid phase. (Etard.) o Grams per ioo Gms. Solution. Grams per ioo Gms. Solution. BaCl 2 . Ba(N0 3 ) 2 . BaCl 2 . Ba(NO 3 ) 2 . o 22.5 4.3 ioo 31 14 20 24.5 6.0 140 32 20 40 26.5 7.5 180 33 26 60 28.5 9.5 210 32 32 SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND MERCURIC CHLORIDE IN WATER. (Foote and Bristol Am. Ch. J. 32, 248, '04.) t. Gms. per ioo Gms. Solution . Solid Phase. t. Gms. per ioo Gms. Solution. Solid Phase. BaCl 2 . HgCl 2 . BaCl 2 . HgCl 2 . 10.4 23-58 50.54 I BaCl,2H,O+ Hg'd 2 ' 10.4 22. IO 51.66] Brctl I . e 3 H a ga 2 .6H 2 0. 10.4 10.4 23-44 22.58 50-74 51-23 Double Salt BaC^HgCl, IO.4 25 21.64 23.02 5i-74 54.83 BaCI,.2H,O+HgCl,. 10.4 22.48 5 I -4i SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND POTASSIUM CHLORIDE IN WATER. (Foote Am. Ch. J. 32, 253, '04.) ioo grams saturated solution contain 13.83 grams BaCl 2 + 18.97 grams KC1 at 25. SOLUBILITY OF MIXTURES OF BARIUM CHLORIDE AND SODIUM CHLORIDE IN WATER. (Precht and Wittgen Ber. 14, 1667, '81; Rudorff Ber. 18, 1161, '85.) , Gms. per ioo Gms. H 2 O. Gms. per ioo Gms. Solution. BaO^ NaCl. BaCl 2 . NaCl. 20 4-1 33-8 2.9 25.0 40 6.3 33.6 4-5 2 3-o 60 9.7 33-5 6 - 8 2 3-4 80 13.9 33-6 9.4 22.8 IOO 17-9 33-6 II .8 22.2 47 BARIUM CHLORIDE SOLUBILITY OF BARIUM CHLORIDE IN AQUEOUS SOLUTIONS OP HYDROCHLORIC ACID AT o. (Engel Ann. chim. phys. [6] 13, 371, '88.) >. Gr. of 10 cc. Sol.' Gms. per 100 CC. Sol. Gms. per ioo g. So! )lutions. HC1. iBaCW 'HC1. BaCl 2 . 'HC1. BaCl 2 . 1.250 O 28.90 30.10 24.07 1.242 I .1 27.80 0.40 28.95 0.32 23-3I 1.228 2.8 26.07 1.02 27-I5 0.83 22.11 I .2IO 5-o 23.40 1.82 24.36 *-5* 2O.I4 143 14.4 I4.0O 5-24 J 4-57 4-58 12.76 .Il8 18.8 10.20 6.84 10.47 6.13 9-37 .099 22.7 6.67 8. 99 6-95 7-55 6-33 .079 32.0 2.74 11.66 2.85 10.81 2.64 .088 5o-5 0.29 18.41 0-30 16.92 0.28 Less than i part of BaCl 2 is soluble in 20,000 parts of concentrated HC1 and in 120,000 parts of cone. HC1 containing $ volume of ether. (Mar Am. J. Sd.[ 3 ] 43, 521, '92.) SOLUBILITY OF BARIUM CHLORIDE IN ABSOLUTE METHYL ALCOHOL AND IN GLYCERINE. (In Alcohol, de Bruyn Z. physik. Chern. 10, 783, '92.) ioo parts of CH 3 OH dissolve 2.18 parts BaCl 2 at 15.5, and 7.3 parts BaCl 2 .2H 2 O at 6. ioo parts by weight of glycerine dissolve 10 parts of BaCl 2 at 15.5. SOLUBILITY OF BARIUM CHLORIDE IN AQUEOUS ETHYL ALCOHOL AT 15. (Schiff Liebig's Ann. 118, 365, '61; Rohland Z. anorg. Ch. 15, 412, '97.) Wt. per cent alcohol 10 20 30 40 60 80 97 Gms.BaCl 2 .2H 2 Oper ioo g. aq. alcohol 31.1 21.9 14.7 10.2 3.5 0.5 0-014 BARIUM CHROMATE BaCrO 4 . SOLUBILITY IN WATER AND IN SALT SOLUTIONS. t. Solvent. Gms " 1 ** U ** Observer. ( (Kohlrausch & Rose 18 Water 0.0038 ]z. physic. Ch. 12, 241, ( '93-) ord. temp. o . 0062 (ignited BaCrO 4 ) ( (Schweitzer z. anal. ord. temp. " o.o ioo (not ignited) j ch. 29, 4M, '90.) V\ i-kt " ^ I^AI ( (Mescherzerski Z. D - P l - o .043 j ^ ch ai 399> , 8a } Ord. temp. 1.5% Am. Acetate O.O2O (Fresenius - Z. anal. ord. temp. 0.5% Am. Nitrate o .022 ( Ch - 2 * 418, V-) BARIUM CITRATE Ba 3 (C 6 H 6 O 7 ) 2 .7H 2 O. SOLUBILITY IN WATER AND IN ALCOHOL. ioo grams water dissolve 0.0406 gram Ba 3 (C 6 H s O 7 )2.7H 2 O at 18, and 0.0572 gm. at 25. ioo grams 95% alcohol dissolve 0.0044 gram Ba 3 (C 6 H s O 7 ) 2 .7H 2 O at 18, and 0.0058 gm. at 25. (Partheil and Hiibner Archiv. Pharm. 241, 413, '03.) BARIUM CYANIDE 48 BARIUM CYANIDE Ba(CN) 2 . SOLUBILITY IN WATER AND IN ALCOHOL AT 14. (Joannis Ann. chim. phys. [5] 26, 489, '82.) ioo parts water dissolve 80 parts Ba(CN) 2 . 100 parts 70% alcohol dissolve 18 parts Ba(CN) 2 . BARIUM FERROOYANIDE AND BARIUM POTASSIUM FERRO- CYANIDE. (Wyrouboff Ann. chim. phys. [4] 16, 292, '69.) ioo parts water dissolve o.i part Ba 2 Fe(CN) 6 .6H 2 O at 15, and i.o part at 75. ioo parts water dissolve 0.33 part BaK 2 Fe(CN) 6 .5H 2 O at ord. temp. BARIUM FLUORIDE BaF 2 . (Kohlrausch Z. physik. Chem. 50, 365, 'o4~'os.) i liter of water dissolves 1.63 gms. BaF 2 at 18. Electrolytic conduc- tivity method. BARIUM FORMATE Ba(HCOO) 2 .2H 2 O. SOLUBILITY IN WATER. (Krasnicki Monatsh. Chem. 8, 597, '87.) t o Gms . Ba(HCOO) 2 per i oo Gms. t <> Gms. Ba(HCOO) 2 per too Gms. Water. Solution. Water. Solution. o 27.76 21.72 40 34-81 25.82 10 28.46 21.15 50 37-14 27.10 20 30.11 23.15 00 38.97 28.03 25 31-20 23.80 70 39-95 28.54 30 32.34 24.45 80 39.71 28.42 BARIUM HYDROXIDE Ba(OH) 2 . SOLUBILITY IN WATER. SOLID PHASE Ba(OH) 2 .8H 2 O. (Rosenthiel and Riihlmann Jahresber. Chem. 314, '70.) t o Gms. Ba(OH) 2 per ioo Gms. t o Gms. Ba(OH) 2 per ioo Gms. 'Water. Solution." Water. Solution o 1-67 1.65 30 5.59 5.29 5 1.95 1.92 40 8.22 7.60 10 2.48 2.42 50 13.12 ii. 61 15 3.23 3.13 60 20.94 17-32 20 3.89 3.74 75 03-5 1 38-85 25 4.68 4.47 So 101.40 50.35 SOLUBILITY OF BARIUM HYDROXIDE IN AQUEOUS ACETONE AT 25. (Herz and Knoch Z. anorg. Chem. 41, 321, '04.) Ba(OH) 2 per ioo cc. Sat. Gms. Ba(OH) 2 Sp. Gr.of Vol.% Solution. Per Solutions. Acetone. / " > ioo Gms. Millimols. Grams. Solution. 1.0479 55 -8 4-722 4-506 i. 0168 10 31-84 2.730 2.686 0.9927 20 17.79 1-525 I -53<5 0.9763 30 9.10 0.779 0.798 0.9561 40 4-75 -407 0.426 0-939* 50 i-54 0.132 0.141 0.9179 60 0.48 0.041 0-045 0-8956 70 0-08 0.007 0-018 . 49 BARIUM IODATE BARIUM HTOATE Ba(IO 3 ) 2 .H 2 O. SOLUBILITY IN WATER. (Trantz and Anschutz Z. physik. Chem. 56, 238, '06.) t o Cms. Ba(IO 3 ) 2 per t<3 Gms. Ba(IO 3 ) per t o Gms. Ba(IO 3 ) 2 per 100 Gms. Solution. 100 Gms. Solution. 100 Gms. Solution. - 0.046 O.OOS 30 0.031 70 0.093 -f 10 0.014 40 0.041 80 0.115 2O O-O22 5O 0-056 9O O.I4I 25 0.028 60 0-074 100 o- J 97 BARIUM IODIDE BaI 2 . SOLUBILITY IN WATER. (Kremers Pogg. Ann. 103, 66, 1858; Etard Ann. chim. phys. [7] 2, 544, '94.) Gms BaI 2 per loo Gms. t. G ' Bal2 ^"ooGms. Water. Solution. Water. Solution. -20 143-9 59.0 BaI 2 .6H 2 O 40 231.9 69.8 BaI 2 .2 H 2 O o 170.2 63.0 60 247.3 7 1 - 2 4-10 185.7 65.0 80 261.0 72.3 20 203.1 67.0 100 271.7 73.1 " 25 212.5 68.0 120 281.7 73.8 30 219.6 68.7 " 160 294.8 74.6 " Sp. Gr. of saturated solution at 19. 5 = 2.24. For method of interpolating above results, see Note, page 33. 100 grams 97% Ethyl Alcohol dissolve 1.07 g. BaI 2 .2H 2 O at 15. (Rohland Z. anorg. Chem. 15, 417, 1807.) BARIUM MALATE BaC 4 H 4 O 5 . SOLUBILITY IN WATER. (Cantoni and Basadonna Bull. soc. chim. [3] 35, 731, '06.) t o per 100 cc. Sol. per 100 cc. Sol. per 100 cc. 20 0.883 35 0.895 60 i. on 25 0.901 4O 0-896 7O I.O4I 30 0.903 50 0.942 80 1.044 SOLUBILITY IN WATER AND IN ALCOHOL. (Bartheil and Hiibner Archiv. Pharm. 241, 413, '03.) ioo grams water dissolve 1.24 gms. BaC 4 H 4 O 5 at 18, and 1.3631 gms. at 25. too grams 95% alcohol dissolve 0.0038 gms. BaC 4 H 4 O 8 at 18, and 0.0039 g m - a ^ 2 5- BARIUM MALONATE BaC 3 H 2 O 4 .N 2 O. SOLUBILITY IN WATER. (Miczynski Monatsh. Chem. 7t 263, '86.) Gms. BaC 3 H 2 O 4 per ioo Gms. Gms. BaC8H 2 O 4 per ioo Gms. Water. "" Solution. Water. Solution. o 0.143 0.143 50 0.287 0.285 10 0.179 0.179 60 0.304 0.303 20 0-212 0-2II 70 0.317 0.316 3O O.24I O.24O 80 0.326 0-325 4O O.266 0.265 BARIUM MOLYBDATE BaMoO 4 . ioo parts water dissolve 0.0058 part BaMoO 4 at 23. (Smith and Bradbury Ber. 24, 3930, '91.) BARIUM NITRATE 50 BARIUM NITRATE Ba(NO 3 ) 2 . SOLUBILITY IN WATER. (Mulder; Gay Lussac; Etard Ann.chim. phys.f?] 2, 528, 94; Euler Z. physik. Chem. 49, 3is,'o4.) Cms. Ba(N0 3 ) 2 Gms. Ba(NO 3 ) 2 t. per 100 Gms. t. per 100 Gms. Water. Solution. Water. Solution. 5-0 4.8 80 27.0 21-3 10 7.0 6.5 100 34-2 25.5 20 9-2 8. 4 120 42.0 29.6 25 10.4 9-4 140 5o-o 33-3 30 n. 6 10.6 160 58.0 36.7 40 14.2 12.4 180 67.0 40.1 50 17.1 14.6 200 76.0 43-2 60 20.3 16.9 215 84.5 45-8 Sp. Gr. of saturated solution at 19.5 = 1.072. SOLUBILITY OF MIXTURES OF BARIUM NITRATE AND LEAD NITRATE IN WATER AT 25. (Fock. Z. Kryst. Min. 28, 365, '97; at 17, Euler Z. phyisk. Chem. 49, 315, '04.) J.11 O01UUU11. A In Solid Phase Sp. Gr. of Solution. Gms. per Liter. Mg. Mols. per Liter. Mol.% Ba(NO 3 ) 2 . Mol.% Ba(N0 3 ) 2 Ba(NO 3 ) 2 . Pb(N0 3 ) 2 . Ba(N0 3 ) 2 . Pb(N0 3 ) 2 ' 1.079 102.2 O 391.0 O 100 IOO 1. 088 54-9 I7-63 2IO.I 53-3 79.78 98.30 I.IOS 86.5 49.80 330-7 !5o-7 68.70 96.74 I .119 79-7 68.10 304-9 205.7 59-69 94.80 I .140 77.0 97.20 294.4 293.6 50.09 93.62 1.163 69.8 130.7 266.8 395-o 40.31 92-49 1.198 66.0 177-3 252.5 535-6 32-03 90.07 1.252 57-5 247-7 222 .6 748.5 22.91 83-47 1.294 25-9 334-3 99-2 1010.3 8. ii 75-44 I-376 28.8 429.7 IIO-3 1298.0 7-77 35-n *-459 553-8 O-O 1673.0 0-0 o.o Tables of results are also given for 15, 30, and 47. SOLUBILITY OF MIXTURES OF BARIUM NITRATE AND POTASSIUM NITRATE IN WATER AT 25. (Foote Am. Ch. J. 32, 252, '04.) Per TOO Grams Solution. ' Pm K>in Grams ' Solid Phase. Gms. KN0 3 . B a (N0 8 ) 2 . 14 .89 6 .62 Ba(NO 3 ) 2 and 2 KNO 3 .Ba(NO 3 , 2 1 6 . 30 5 . 49 \ Double salt, 21 99 3 .04 J 2 KN0 3 .Ba(N0 3 ) 2 27 . 76 2 .04 KN0 3 and 2 KNO 3 .Ba(NO 3 ) 2 BARIUM NITRATE SOLUBILITY OF BARIUM NITRATE IN AQUEOUS PHENOL SOLUTIONS AT 25. (Rothmund and Wilsmore Z. phyisk. Chem. 40, 620, '02.) G. Mols. per Liter. Gms. per Liter. G. Mols. per Liter. Gms. per Liter. CflHcOH 'Ba(N0 3 ) 2 . C 8 H 5 OH. Ba(NO 3 ) 2 .' C 6 H 5 OH. Ba(NO 3 ) 2 . 0-000 0.3835 0.0 100.2 0.310 0.3492 0.045 0.3785 4.23 98.97 0.401 0.3400 0.082 0.3746 7.71 97-95 0.501 0.3299 0.146 0.3664 13-73 95 - 8 29.12 9 I -3 I 37.73 88.90 47.11 86.26 0.728 (sat.) 0.3098 68.45 81.00 BARIUM NITRITE Ba(NO 2 ) 2 .H 2 O. SOLUBILITY IN WATER. (Vogel Z. anorg. Chem. 35. 389, '03.) Gms. Ba(NO 2 ) 2 per 100 gms. H 2 O 58 20 C 63 30 82 35 97 BARIUM OXALATE BaC 2 O 4 . SOLUBILITY OF THE THREE HYDRATES IN WATER. (Groschuff Ber. 34, 3318, '01.) BaC 2 43 *H 2 0. BaC 2 O 4 .2HoQ. t . Gms.BaC 2 O 4 G.M.BaC 2 O 4 per per 100 Mol. Gms. BaC 2 O 4 per G. M. BaC 2 O 4 per 100 G. M. 1000 g. Sol. H 2 O. looo g. Sol. H 2 0. O 0.058 O.OOO46 0-053 O.OOO42 9-5 0.082 o .00066 18 O.II2 O.OOO9O 0-089 O.OOO7I 3 0.170 0.00136 O-I2I O.OOO97 40 0.152 O-OOI22 45 0.169 0-00135 50 55 O-2I2 O.OOI70 60 . . . 65 0.250 0-OO2OO 73 0.285 0.00228 75 90 100 . . . . BaC 2 O 4 .}H 2 O. Gms.BaC 2 O< G.M. BaC 2 O 4 per per 100 Mol. 1000 g. Sol. H 2 O. 0-089 O.OOO7O 0.124 0.00099 O.I4O O-OOII2 O.I5I O.OOI2I 0.164 O.OOI3I 0.175 0.00140 0.188 O-2OO O.2II O.OOI5I O.OOI6O 0.00169 SOLUBILITY OF BARIUM OXALATE (BaC 2 O 4 .$H 2 O) IN AQUEOUS ACETIC ACID AT 26-27. (Herz and Muhs. Ber. 36, 3715, '03.) of Acetic Acid. per S see CHaCOOH. Oj ^j ate of Acetic Acid. per 50 cc. CHaCOOH. Ba Oxalate O O ,0077 o.oo .0154 3-85 O .0564 23 .12 O.II27 0-565 O .0423 3-39 .0845 5-79 .0511 34 .76 0-I02I I-425 O .0520 8-55 .1039 O .0048 103 .90 0-0096 2.85 055 6 17.11 .1111 * Dried at 70. BARIUM AOID OXALATE 52 BARIUM AOID OXALATE BaC 2 O 4 .H 2 C 2 O 4 . 2 H 2 O. SOLUBILITY IN WATER. (Groschuff.) Gms. per 100 Gms. Solution. ll . H 2 C 2 4 . BaC 2 4 : H 2 C 2 4 . BaC 2 4 . ' per i Mol.Ba< 0.27 0.030 0-054 O.OO24 22 18 0.66 0.070 0.130 0.0056 24 20.5 0.76 0.076 0.15 0-0061 25 38 1.61 0.16 o-33 0.013 25 41 1.82 0.18 o-37 O.OI5 25 53 2 .92 0.31 0.60 O.O26 24 60 3.60 0.40 o-75 0-033 22-5 80 6.21 0.81 O.O7O 19 90 7.96 i .11 1.75 0-098 18 99 10.50 i .55 2-39 O.I4I 17 BARIUM PROPIONATE Ba(C 3 H 6 O 2 ) 2 .H 2 O. also 6H 2 O. SOLUBILITY IN WATER. (Krasnicki Monatsh. Chem. 8, 597, '87.) Gms. Ba(CaH 5 O 2 ) 2 Gms. Ba(C 3 H 5 O 2 ) 2 t e . per loqGtns. t. per 100 Gms. Water. Solution. Water. Solution. o 47 -9 8 3 2 -4i 50 62.74 38.57 10 5 J -5 6 34-02 60 64.76 39-3 1 20 54-82 35.42 70 66.46 39.93 30 57-77 3 6 - 6 5 8o 6 7-85 40-42 40 60.41 37.66 BARIUM SULPHATE BaSO 4 . SOLUBILITY IN WATER. Electrolytic Conductivity Method. (Holleman; Kohlrausch and Rose Z. physik. Chem. 12, 131, 241, '93.) t 2 10 19 26 34 37-7 Gm. BaSO 4 per liter 0.0017 0.0020 0.0023 0.0026 0.0029 0.0031 SOLUBILITY OF BARIUM SULPHATE IN AQUEOUS SOLUTIONS OF HYDRO- CHLORIC AND OF NITRIC ACIDS. (Banthisch J. pr. Chem. 29, 54, 1884.) In Hydrochloric Acid. In Nitric Acid. ^ _^ / A, _^ cc. containing Mgs. BaSO 4 Gms. per 100 cc. cc . containing Mgs. BaSO 4 Gms. per 100 cc. iMg.Equiv. per i Mg. Equiv. Solution. i Mg.Equiv. per i Mg.Equiv. Solution. ofHCl ofHCl. HC1. BaS0 4 : of HNO 3 . of HNO 3 . HNO 3 . BaSO 4 . 2.0 0.133 1.82 0.0067 2.0 0.140 3- J 5 0.0070 i.o 0.089 3.65 0.0089 i.o 0.107 6.31 0.0107 0.5 0.056 7.29 o.oioi 0.5 0.085 12. 61 0.0170 O-2 O.OI7 18.23 O.OO86 O-2 0.048 3I-52 O.O24I 100 cc. HBr dissolve 0.04 gms. BaSO 4 ; 100 cc. HI dissolve 0.0016 gms. BaSO 4 at the boiling point. (Haslam Chem. News 53, 87, '86.) 53 BARIUM SULPHATE SOLUBILITY OF BARIUM SULPHATE IN AQUEOUS SOLUTIONS OF IRON, ALUMINUM AND MAGNESIUM CHLORIDES AT 20 25. (Fraps. Am. Ch. J. 27, 290, '01.) Cms. Chloride Milligran is BaSO 4 per Liter in: Cms. Chloride Mgs. BaSO 4 per Liter in: per Liter. Aq. FeCla- Aq. AlCla- Aq. MgCl 2 . per Liter. Aq. FeCl 3 . Aq. AlCla. Aq.MgCl 2 . I 58 33 30 25 J 5o 116 50 4 72 43 30 50 160 170 50 5 "5 60 33 100 170 J 75 SO 10 123 94 33 BARIUM PerSULPHATE BaS 2 O 8 . 4 H 2 O. TOO parts water dissolve 39.1 parts BaS 2 O 8 or 52.2 parts BaS 2 O 8 . 4H 2 O at o. (Marshall J. Ch. Soc. 59, 771, '91. BARIUM SULPHITE BaSO 3 . SOLUBILITY IN WATER AND IN AQUEOUS SUGAR SOLUTIONS. (Rogowicz Z. Ver Zuckerind. 938, 1905.) Cone, of Gm. BaSC ) 4 per 100 cc. Sol. Cone, of Gm. BaSO 4 per 100 CC. Sol. Sugar Sol. at 20. at 80. Sugar Sol. at 20. at 80. oBx 0.0197 0.00177 40 Bx 0-0048 0.00158 10 " O-OIO4 0-00335 50 " O.OO3O O.OOI49 20 " 0-0097 0.00289 60 " (sat.) O.OO22 0-OOII2 30 " 0-0078 0.00223 BARIUM SUGGINATE AND BARIUM ISO SUGGINATE Ba.CH 2 CH 2 (COO) 2 . Ba.CH 3 CH 2 (COO) 2 . SOLUBILITY OF EACH IN WATER. (Miczynski Monatsh. Chem. 7, 263, 1886.) Gms. Ba. Iso Succinate per IPO Gms. Gms. Ba. Succinate t. per zoo Gms. Water. Solution. 0.421 0.420 10 0.432 0.430 20 0.418 0.417 30 o-393 0.392 40 0.366 0-365 50 o-337 0.336 60 0.306 0-305 70 0.273 0.272 80 0-237 0.237 Water. Solution. 1.884 1.849 2.852 2.774 3 .6l8 3-493 4.l8l 4-014 4-542 4-346 4-700 4-594 4.656 4-450 4-410 4.224 3.962 3.810 100 gms. H 2 O dissolve 0.396 gms. Ba Succinate at 18 and 0.410 gms. at 25. 100 gms. 95% alcohol dissolve 0.0015 gms. Ba Succinate at 18 and 0.0016 gms. at 25. (Partheil and Hiibner Archiv. Pharm. 241, 413, '03.) BARIUM TARTRATE Ba(C 2 H 2 O 3 ) 2 . SOLUBILITY IN WATER. (Cantoni and Zachoder Bull. soc. chim. [3] 33, 751, '05; see also Partheil and Hiibner.) Gms. Gms. Ba(C 2 H 2 O 3 ) 2 t . per loo cc. Solution. t . per 100 cc. Solution. o O.O2O5 30 0-0315 10 20 25 O.O242 0.0279 0.0297 40 50 60 0.0352 0-0389 O.O44O 70 80 90 Gms. Ba(C 2 H 2 O a )2 per 100 cc. Solution. o . 0480 0.0527 0.0541 BARIUM TARTRATE 54 SOLUBILITY OF BARIUM TARTRATE IN AQUEOUS ACETIC ACID SOLUTIONS at 26-2j. (Herz and Muhs Ber. 36, 3715, '03.) Ul rVL-CUC Acid. per 50 VK* Sol. CHaCOOH. Ba tartrate.' Add per 50 cc. Sol. CH 3 COOH. Ba tartrate O O .0328 O-O 0655 3-77 .1866 22 .62 0.3728 0.565 O .1151 3-39 .2300 5-65 O .1865 33 .90 0.3726 1.425 - ^-559 8-55 3 JI 5 16.85 O .02l8 101 .10 0.0436 2 -85 o . 17 39 17.11 o 3475 . * Dried at 70. ioo grams 95% alcohol dissolve 0.032 gm. Ba tartrate at 18 and 0-035 6 m - at 2 5- (Partheiland Hiibner.) BENZALDEHYDE C 6 H 6 COH. ioo gms. H 2 O dissolve 0.3 gm. benzaldehyde at room temperature. (Fluckiger Arch. Pharm. [3] 7, 103, '75.) BENZAMIDE C 6 H 5 CONH 2 . SOLUBILITY IN ETHYL ALCOHOL. (Speyers Am. J. Sci. [4] 14, 295, '02.) t. G.M. Gms. Sp. Gr. of C 6 H 6 CONH 2 C 6 H 5 CONH 2 t o Solutions, per ioo G.M. per ioo Gms. Sp. Gr. of Solutions. G.M. C 6 H 6 CONH 2 per ioo G.M. C 2 H 5 OH. Gms. C 6 H 5 CONH 2 per ioo Gms. 0-833 3 .1 8 J 5 40 0.848 II 28.92 10 0.832 4 .2 ii .04 5o 0.862 14 2 37 34 20 0.833 5 9 J 5 52 60 0.881 J 7 2 45 .22 25 0.835 6 .8 17 87 70 0.913 20 4 53 63 30 0.838 8 .2 21 56 . SOLUBILITY OF BENZAMIDE IN MIXTURES OF ALCOHOL AND WATEP AT 25. (Holleman and Antusch Rec. trav. chim. 13, 294, '94.) Alcohol. IOO 95 90 85 83 80 75 BENZENE C 6 H,. SOLUBILITY IN WATER AT 22. (Herz Ber. 31, 2671, '98.) ioo cc. water dissolve 0.082 cc. C 6 H 6 , Vol. of Sol. 100.082, Sp. Gr. = 0.9979. ioo cc. C 6 H 6 dissolve 0.211 cc. H 2 O, Vol. of sol. = 100.135, Sp. Gr. = 0.8768. Gms. Gms. C 6 HeCONH 2 per ioo Gms. Sp. Gr. of Solutions. Vol. % Alcohol. C 6 H 6 CONH 2 per ioo Gms. Sp. Gr. of Solutions. Solvent. Solvent. 17.03 0.830 70 2 3 -87 0.925 21 .12 0.856 60 18.98 0-939 24.50 0.878 50 13-74 0.949 26.15 0-895 40 8.62 0-958 26.63 0.900 31 5-33 0.967 26.43 0-907 2.28 0.912 25.41 0.917 o i-35 o-999 55 BENZENE BENZENE, ACETIC ACID, WATER MIXTURES. (Lincoln J. Physic. Chem. 8, 251, '04.) NOTE. To mixtures of known amounts of acetic acid and benzene, water was gradually added until clouding occurred. The same degree of clouding did not represent the end point in all cases, as was assumed by Waddel. (J, Physic. Chem. 4, 161, 'oo.) _ At 25. _ ^ _ At 35. _ cc. cc. cc. cc. cc. cc. CHaCOOH. C 6 H 6 . H 2 O. CH 3 COOH. C 6 H. H 2 O. 5 10. 06 0.45 ioo 18.10 1.14 5 8.04 0.55 ioo 16.09 I - 22 5 6.03 0.64 ioo 10.06 1.55 5 3.02 0.98 ioo 6.03 2.17 5 2 .01 1.28 ioo 4.02 2.77 5 i .01 1.89 ioo 3.01 3.26 5 0.60 2.80 ioo i .00 7.01 5 0.35 4-54 ioo 0.65 10.10 5 o- 1 ? 9-53 I0 o-47 J 3- 6 4 BENZENE, AQ. ALCOHOL MIXTURES; BENZENE, AQ. ACETONE MIX- TURES AT 20. H 2 O added to mixtures of known amounts of the other two and appearance of clouding noted. (Bancroft Phys. Rev. 3, 31, 1895.96.) C 6 H 6 ,C 2 H 5 OH and H 2 O C 6 H 6 ,CH 3 OHandH 2 O C 6 H 5 ,(CH 3 ) 2 COandH 2 O Per 5 cc. C 2 H 5 OH. Per 5 cc. CH 3 OH. Per 5 cc. (CH 3 ) 2 CO. cc. H 2 O. cc. C 6 H C .~ 8.O O-IO 3-o Q-395 2.O 0-69 1.3 i.o 0-51 2.0 0.295 3.0 O.2 4.0 0.15 5-0 MUTUAL SOLUBILITY OF BENZENE AND /3 NAPHTHALENE PICRATE C 6 H 2 (N0 2 ) 3 OH.C 10 H 7 OH. " Synthetic Method " used see Note, p. 9. (Kuriloff Z. physik. Chem. 24, 442, '97.) cc. HzO. cc. C 6 H. 'cc. H 2 0. cc. C 6 H: 20 0.03 5-o 0.15 8 0.13 3-o 0.215 4 o-39 2.O 0.59 2 1.17 1.4 1 .0 i-5 1.87 I.O 1.9 i.o 3-57 0.8 3-o 0.605 8.0 0.69 4.0 0.34 20. o 0.49 8.0 t o Gms. Gms. e Gms. Gms. Picrate. Benzene a Picrate. Benzene. ct. 157 IOO O . . . 100.0 in .6 i 173 I 37 19 2 148.4 2 .128 O.II5 79-3 102 .0 i .087 I .780 II. 2 137-4 I .274 0.170 61.1 29 5 390 8 430 o-95 134.2 I 384 0-297 49-3 4 .6 i 3 2 9 21 .80 0.48 126.8 I .019 0-343 38-3 5 .02 IOO o a = Mols. Naphthalene Picrate per ioo Mols. of Napthalene Picrate plus Benzene. Determinations for a large number of isothermes are also given. BENZENE 56 SOLUBILITY OF BENZENE IN SULPHUR. By " Synthetic Method, " see Note, p. 9. (Alexejew Ann. Physik. Chem. 28, 305, '86.) t o Gms. C 6 He per 100 Gms. t <> Cms. C 6 H 8 per 100 Gms. S Layer. C 6 H Layer. S Layer. C 8 H Layer. loo 6 75 140 16 61 no 8 72.5 150 19 55 120 10 70 160 25 45 130 12 66 164 (crit temp.) 35 Di Brom BENZENE (p) C 6 H 4 Br 2 . SOLUBILITY IN ETHYL, PROPYL, Iso BUTYL ALCOHOLS, ETC. (Schroder Z. physik. Chem. n, 456, '93.) Determinations by " Synthetic Method" see Note, p. 9. Grams C 6 H 4 Br 2 (/>) per 100 Grams Sat. Solution in: 1 . C 2 H 6 OH. CjjHyOH. (CH 3 )CH.CH 2 OH. (C 2 H 6 ) 2 0. CS 2 . C 6 H 6 . C 6 H 6 Br. 27 10 30 34 34 22 20 38 43 43 29 30 14 '5 47 53 53 36 40 *9 2O 57 62 62 45 50 26 27 30 67 72 7i 54 00 38 40 44 77 81 80 67 70 57-6 67 65 87 90 88 79 75 80.5 85 77 . . 84 80 94-4 95 94.6 90 Chlor BENZENE C.H.Q. SOLUBILITY OF CHLOR BENZENE IN SULPHUR. " Synthetic Method, " see page 9. (Alexejew.) Grams C 8 H S C1 per 100 Grams. ** Sulphur Chlor Beri- Layer. zene Layer. 00 13 70 ioo 18.5 63 no 27 53 116 (crit. temp.) 38 For the solubility of Mixtures of di Chlor Benzene and di Brom Benzene in aqueous Ethyl Alcohol solutions see Thiel. (Z. physik. Chem. 43, 656, 1903.) Di Nitro BENZENE (m) C 6 H 4 (NO 2 ) 2 . SOLUBILITY IN BENZENE, BROM BENZENE AND IN CHLOROFORM. " Synthetic Method." (Schroder.) Gms. C 6 H4(NO 2 ) 2 per ioo Gms. C 6 H4(NO,) 2 per t. Gms. Sol, in: jo ioo Gms. Sol, in: CH 6 . C 6 H 6 Br. CHClg. C 6 H 6 . C 6 H 5 Br. 15 17.5 ... 22.2 40 52.0 38.0 42.0 20 26.0 18.5 25.0 50 62.5 47.5 52.5 2 5 33-o 23.7 29.0 60 71.0 57.0 65.0 30 40-0 28.7 33.0 ...... ..... 57 BENZENES Solubilities of Di-Nitro BENZENES and of Tri-Nitro BENZENES in Several Solvents. , (de Bruyn Rec. trav. chim. 13, 116, 150, '94.) Grams per 100 Grams Solvent. Solvent. **' (N(Sv ( <$$r $8fir (NO!': wcwo* Methyl Alcohol Ethyl Alcohol 20 2O. 5 5 3 i. 3<> 9 6 3- 75 5 0.69 0.4 4 i 9 9 (16) 16.2 (15.5) (16) 5.45 (IS. 5) Propyl Alcohol 2O. 5 i . 00 2. 4 0.298 9 Carbon Bi-Sulphide 17. 6 0.236 I. 35 0.148 25 Chloroform 17- 6 27. i 3 2 - 4 1.82 6 .1 Benzene 18. 2 5.66 39- 45 2.56 6 .2 (16) Ether 17' 5 . . . .. i 5 Ethyl Acetate 18. * 12. 96 36- 27 3-56 t Toluene 16. 2 3- 62 66 2.36 fm Carbon Tetra Chloride 16. 2 0. J 43 i. 18 0.12 , Water (ord.) O. 014 o. 5 2 5 0.008 .. . Symmetrical Tri-Nitro BENZENE. SOLUBILITY IN AQUEOUS ALCOHOL AT 25. (Holleman and Antusch Rec. trav. chim. 13, 206, '94.) Vol.% Alcohol. G. C 6 H 3 (N0 3 )3(5) per 100 g. Solvent. Sp. Gr. of Solutions. Vol.% Alcohol. G. C 8 H 3 (N0 8 )3to per roo g. Solvent. Sp. Gr. of Solutions. 100 2-34 Q-7957 80 o-57 0.8582 95 i-57 0.8131 75 o-47 0.8708 90 1. 12 0.8288 70 o-37 0.88o8 85 0-79 0.8436 60 0.23 0.9064 BENZOYL PHENYL HYDRAZINE C 6 H 5 .NH.NH.C 7 H e O. SOLUBILITY IN AQUEOUS ALCOHOL. (Holleman and Antusch Rec. trav. chim. 13, 291, '94.) Vol.% Alcoho IGms. Hydrazine per loo g. Solvent. Sp. Gr. Solutions. 100 2-39 0-793 95 2.43 0.814 93 3. co 0.822 90 2.26 0.831 Vol.% Alcohol. Gms. Hydrazine per 100 g. Solvent. Sp. Gr. Solutions. 80 70 1 59 1. 08 0.859 0.884 55 40 0.51 0.16 0.917 0.946 BENZO SULPHONIG ACIDS. SOLUBILITY IN WATER. (Bahlman Liebig's Ann. 186, 309, '77.) Name of Acid. 0- Amido benzo sulphonic acid. Amido brom benzo sulphonic acid. Mono brom amido benzo sulphonic acid. Barium di-brom benzo sulphonic acid. Barium nitro brom benzo sulphonic acid (hydrated). Barium nitro brom benzo sulphonic acid (anhydrous). * At 18 = i. Gms. Sulphonic Acid per 100 Gms. Solution at: 11 = 1.301 8 = 0.737 12 = 0.431 14 =L7I3 16 0.527 8 = 0.156 15 = 1.436 16 = 1.131* 15 = 0.463 9 = 1.098 30 = 0.914 BENZINE 58 BENZINE (Petroleum) C 6 H 12 C 6 H 14 . ioo parts of alcohol dissolve about 16 parts benzine of 0.638 0.660 Sp. Gr., at 25. BENZOIO ACID C 6 H 8 COOH. SOLUBILITY IN WATER. (Bourgoin Ann. chim. phys. [5] 15, 171, '78.) Grams. QHsCOOH Grams. C 6 HsCOOH t. per ioo Gms. t. per ioo Gms. Water. Solution. Water. Solution. o 0.170 0.170 40 0.555 0-55 1 10 0.210 0.209 50 0.775 0.768 20 0.290 0.289 60 I - I 55 1.142 25 0.345 0.343 80 2.715 2.643 30 0.410 0.408 ioo 5- 8 75 5-549 ioo grams saturated aqueous solution contains 0.340 gram C 6 H 6 COOH at 25; 0.353 g ra m at 2 6.4 ; 0.667 gram at 45. (Paul Z. physik. Ch. 14, in, '94; Noyes and Chapin Ibid. 27, 443, '08; Hoffman and Langbeck Ibid. 51, 393, '05; Philip J. Ch. Soc. 87, 992, '05 ; see also Alexejew Ann. Phys. Ch. 28, 305, '86; Ost J.pr. Ch.[2] 17, 232, '78; Vaubel Ibid.\2\ 52, 73, '95.) SOLUBILITY OF MIXTURES OF LIQUID BENZOIC ACID AND WATER. (Alexejew.) Determinations by " Synthetic Method," see Note, p. 9. Figures read from curve. Gms. C r ,H 5 COOH per ioo Gms. e Gms. C 6 H 5 COOH per ioo Gms. Aq. Layer. Benzoic Ac. Layer. Aq. Layer. Benzoic Ac. Layer. 70 6 83 ioo 12. o 69.0 80 7.5 79.5 no 18.0 59.0 90 8.5 76 116 (crit. temp.) 35 SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF: (Hoffman and Langbeck.) Nor- mality Potassium Chloride at 25. J!f- Dissolved CfiHsCOOH. ^~ v Potassium Nitrate at 25. ^335; Dissolved QHgCOOH. of Aq. KC1 LJJ^ Mol. Cone. Wt. per cent. KNOs per Liter. Mol. Cone Wt. per cent. 0-02 1-49 5 . 0254-10"* 0. 339 O.02 2. 02 5.0326-10-* 0.340 0.05 3-73 4.9801 o. 333 0.05 5- 06 5.0421 a 0.341 0.20 14.92 4-7639 o. 322 0.20 20. 24 5.0297 ft 0.340 0.50 37-30 4-3632 o. 295 0.50 50- 59 4.9400 if 0-334 I -OO IOI . 19 4 . 7646 0.322 SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF: (Hoffmann and Langbeck.) Sodium Chloride. Sodium Nitrate. Nor- mality of Aq Gms. NaCI Gms. CfiHsCOOH per ioo Gms. Sol. Nor- mality of Aq NaNC-3 Gms. CgHgCOOH per ioo Gms. Sol. NaCI.' liter. at 25- at 45. NaNO 3 . L^ter. at 25. at 45: o.oo .00 O- 340 o. 667 0-02 1.70 340 0.666 O-O2 I 17 0- 339 o. 663 0-05 8. 5 I O 339 0.663 O.O5 2 93 O- 335 o. 654 O-2O 17 .02 O 333 0.647 0.20 II .70 o. 336 o. 6l 7 0.50 42-54 3i9 0.613 0.50 29 25 0- 282 o. 546 I.OO 85.09 o .294 . . . I.OO 58 50 . o- 449 59 BENZOIO ACID SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF SODIUM ACETATE, FORMATE, BUTYRATE, AND SALICYLATE. (Noyes and Chapin Z. physik. Chem. 27, 443, '98; Philip J. Ch. Soc. 87. 993, '05.) Grams Gram: s QjH 5 COOH per Liter of S< )lution in: Sodium Salt per CHaCOONa. HCOONa. CaHrCOONa. CoH^OH.COi Liter. At 25. At 26. 4 6 . At 25. At 26.4. At 26.4. At 26.4". O 3-41 3-53 3-41 3-53 3-53 3-53 I 4-65 4-75 4-25 4-35 4.50 3-62 2 5-7 5-85 4-75 4.85 5-40 3 6.70 6.90 5-20 5-30 6-15 3-8o 4 7.60 7-85 5-6o 6.90 3-87 6 8.40 4.00 8 4-10 Sodium Salt per Liter. O-OO O-OI O-O2 0.03 0-04 O-o6 CH 3 COONa. HCOONa. CaH 7 COONa. At 26.4. 0.0289 0.0376 0.0455 0.0525 0-0596 CaH4OH.COONa At 26.4. 0.0289 0.0300 0.0312 0.0321 0.0328 0.0342 At 25. 0.0279 0-0362 o . 0440 0.0508 0.0572 At o. O- o. o. o. 26.4. 0289 0370 0448 0518 0586 At 25. 0.0279 0.0330 0-0364 0.0392 O.O4I6 0-0460 At 26.4. 0.0289 0.0336 0.0372 0-0398 0.0423 0-0466 SOLUBILITY OF BENZOIC ACID IN ABSOLUTE ALCOHOLS. (Tirrofeiew Compt. rend. 112, 1137, '91; at 15, Bourgoin Ann. chim. phys., [5] 13, 406, '78.) In Methyl Alcohol. In Ethyl Alcohol. G. CeH 6 COOH per IPO Cms. G. CeH 5 COOH per 100 Gms. In Propyl Alcohol. G. QH 6 COOH per 100 Gms. 3 '5 21 CHaOH. 50-16 Solution. 33-39 69.29 40.93 C 2 H 5 OH. 40.16 46.70 54-09 Solution. 28.65 31.80 35 -io CaH 7 OH. 29.88 Solution. 23.00 40.64 28.90 SOLUBILITY OF BENZOIC ACID IN 90% ALCOHOL, IN ETHER AND IN CHLOROFORM. (Bourgoin.) Solvent. 90% Alcohol Ether Chloroform Gms. CgHsCOOH per 100 Grams. Solvent. Solution." 15 41.62 29.39 15 3 r -35 23.86 25 14-30 12.50 SOLUBILITY OF BENZOIC ACID IN AQUEOUS SOLUTIONS OF DEXTROSE. Normality of iier 01 ooiuuon in: per Liter. C 3 H 7 COONa. CH 3 COONa. HCOONa. C 6 H4.OH.COONa. O 7-85 7-85 7-85 7-85 o-5 8-35 8-50 8.60 8-35 I.O 8.90 9-15 9-50 8.70 2 IO-O I0.8o "$ 9-4 3 II .2 12-55 13-5 II. 4 12-4 i4-5 I 5 .6 "5 6 15-2 SOLUBILITY OF ORTHO NITRO BENZOIC ACID IN AQUEOUS SOLUTIONS OF DEXTROSE, SODIUM CHLORIDE, AND OF SODIUM NITRATE. Original results in molecular quantities. (Hoffman and Langbeck Z. physik. Chem. 51, 412, '05.) In Dextrose. In NaCl. In NaNO 3 . 1 G. CeH l2 8 per 100 cc. G.(o)C 6 H4N0 2 .COOH G. NaCl. per 100 g. Solvent. WI IOO cc G.&OC.EUN02.COOH G .NaNO 3 . per loo g. Solvent. pe r I00 cc . G.(o)C6H 4 N0 2 .COOH per TOO g. Solvent. Solution. At 25. At 35. Solution. At 25. At 35. Solution. At 25. At 35. 0-0 0.736 -063 O.II7 O 743 I .072 .170 .746 1.074 0.36 0.736 .064 0.195 O .746 1-075 .284 754 I.OSO 1. 80 0.732 O6l 0.585 O 749 I .O7O .851 .767 I -096 9-50 O.722 .051 2.425 .688 0.967 4 255 774 1.097 20-00 0.703 .030 5.80 o 597 0.831 8 .510 748 1.047 BENZOIO SULPHINIDE (Saccharine) C 6 H 4 <^Q 2 >NH. 100 parts water dissolve 0.4 part at 25 and 4.17 parts at 100. loo parts alcohol dissolve 4 parts at 25 (U. S. P.). BENZOPHENONE BENZOPHENONE (C 8 H 5 ) 2 CO. SOLUBILITY IN AQUEOUS ALCOHOL AND IN OTHER SOLVENTS. (Derrien Compt. rend. 130, 722, 'oo; Bell J. Physic. Chem. 9, 550, '05.) In Aqueous Alcohol at 40. (Bell.) Akoh?l Cms. (CoH 6 ) 2 CO per loo^Gms. in Solvent. Solvent. Solution. 40 2 1-9 45 5 4-8 SO 8 8-3 55 II 99 60 16 13-8 65 28 22.6 Wt.% Gms. (CH 8 ) 2 CO Alcohol per 100 Gms. in Solvent. Solvent. Solution. 67-5 39 28.1 70 5 6 359 71 67 39.2 72 90 47-4 72-5 105 51.2 73 156 61.0 In Aqueous Alcohol and other Solvents. (Derrien.) Solvent. 97% Ethyl Alcohol 17 8500. 97% Alcohol + i5CC.H 3 O " 80" " +20" 75" " +26" Methyl Alcohol (pure) 9 .8 15.0 Acetic Ether (pure) 9.6 Carbon Bisulphide 16.1 Gms. (C6H 6 ) 2 CO per 100 g. Solvent. 13-5 3-8 2 .2 II .O 14-3 19 .2 66.6 Solvent. Benzene Xylene Nitro Benzene Chloroform (com.) Bromoform Toluene Ligroine II* 15-8 16.5 17-3 I? 'A 14.6 Gms. (CeH 5 ) 2 CO per 100 g. Solvent. 76.9 38.4 58.8 55-5 33-3 55-5 6.7 BERYLLIUM HYDROXIDE Be(OH) 2 (See also Glucinium, page 140). SOLUBILITY IN AQUEOUS SOLUTIONS OF SODIUM HYDROXIDE. (Rubenbauer Z. anorg. Chem. 30 334, '02.) Moist Be(OH) 2 used, solutions shaken 5 hours, temperature prob- ably about 20. Molecular Gms. per IOQ^CC. Solution. 'NaOH. Be(OH) 2 ." Per 20 cc. Solution. Dilution of the NaOH. 0.68 o-53 0.27 Gms. Na. o-335 8 0.6716 0.8725 I-7346 Gms. Be. 0.0358 0.0882 O.II75 0-2847 2.917 5.840 18.310 BERYLLIUM SULPHATE BeSO,. SOLUBILITY IN WATER. (Levi, Malvano Z. anorg. Chem. 48, 446, '06.) 0.850 2.094 2.789 6.760 Mols. H 2 O per i M ol Gms. BeSCu per 100 Gms. Solid Mols. H 2 4. o per i Mol. Gms. BeSO 4 per 100 Gms. Solid t. BeS0 4 . " Water. Solution. Phase. * ' BeS0 4 . Water. Solution. Phase. 31 ii. 18 52-23 34-32 BeSO 4 .6H,O 95-4 6.44 90.63 47-55 BeSO. 4 H O 5 9.62 60.67 37-77 " 107.2 5.06 ^5-3 53.58 ' 72.2 7-79 74-94 42-85 in 4-55 I2-S.3 56.19 77-4 7- J 3 81.87 45.01 80 6.89 84.76 45-87 BeSO .2H,C 3 13.33 43.78 3-45 BeSO 4 H,0 91.4 5-97 97-77 49.42 * 40 12.49 46.74 * IO 5 4-93 118.4 54.21 68 9.42 61.95 38-27 1 119 3-9 1 149-3 59-88 1 85 7-65 76.30 43-28 * BISMUTH 64 BISMUTH Bi. MUTUAL SOLUBILITY OP BISMUTH AND ZINC. (Spring and Romanoff Z. anorg. Chem. 13, 34, '06.) 266 419 475 Upper Layer. Lower^ Layer. 584 650 75o Upper Layer. Lower Layer. %Bi. %Zn." 86 14 84 16 %Bi. %Zn. 3 97 5 95 %Bi. %Zn. 80 20 77 23 70 30 %Bi. %Zn. 10 90 15 85 27 73 810-820 (crit. temp.) BISMUTH CHLORIDE BiCl 3 . 100 grams absolute acetone dissolve 17.9 grams BiCl 3 at 18. (Naumann Ber. 37, 4332, 1004.) BISMUTH IODIDE BiI 3 . 100 grams absolute alcohol dissolve 3.5 grams BiI 3 at 20. (Gott and Muir J. Chem. Soc. 57. 138, '90.) ioo grams methylene iodide CH 2 I 2 dissolve 0.15 gram BiI 3 at 12. (Retgers Z. anorg. Chem. 3, 343, '93.) BISMUTH NITRATE Bi(NO 3 ) 8 .5H 2 O. ioo grams acetone dissolve 48.66 grams Bi(NO 3 ) 3 .5H 2 O at o, and 41.7 grams at 19. (von Laszczynski Ber. 27, 2285, '94.) BISMUTH OXIDE Bi 2 O 3 . SOLUBILITY OF BISMUTH OXIDE IN AQUEOUS NITRIC ACID AT 26. (Rutten and van Bemmelen Z. anorg. Chem. 30, 386, '02.) Present in Shaker Flask. Gms. per ioo Gms. Solution. Mols. per ioo Mols. H 2 O. Solid Per i part Bi 2 O 3 . 3N 2 O 5 .ioH 2 O. Bi 2 O 3 N 2 5 Bi 2 3 N 2 5 R 1N 2 B 2 , 3 Phase. 24.4 parts H a O 3.2 parts H 2 O 0-321 6-37 0.963 7.17 o 126 2.844 1.61 13.82 J j 12.8 4.8 Bi 2 8 .N,0 6 .2H,0 Dilute HNO, Dilute HNO 3 18.74 31.48 15-9 2 3-7 10.50 27.2 I 3-6 3.0 J Bi s O,N 1 5 .H,0 Dilute HNO 3 = 6.13% N 2 6 32-93 24.83 30.15 97.97 I 3-2 f Bi 2 O 3 .N 2 Oj5.H,O and Bi 2 O s .3N,O 6 .ioH 2 O 6.816% N 2 5 32.67 24.70 ' 29.70 96.57 j 3-2] 24.0% N 2 O 6 51.0% N 2 O 5 24.16 11.66 28.25 46.62 19.65 10.81 98.76 186.23 X I 5-0 17.2 -Bi 2 O s .3N 2 O 5 .ioH,O 70.0% N 2 O 5 20.76 53-75 33-51 355.87 I 10.6, 27.85 51.02 51.0 403.0 I 7-9 Bi 2 O 8 .3N 2 O 5 .ioH 2 O and Bi 2 O s .3N 2 O s .3H 2 O Anyhdrous HNO Bi 3 O 3 + " 38.56 4.05 68.28 74.90 14.35 7.45 492.0 592-9 I j 34-3 79.5 Bi,0,. 3 N,Os.3H,0 Results are also given for 9, 30, and 65. 65 BORIC AOID BOEIO ACID (Ortho) H 3 BO 3 . SOLUBILITY IN WATER. (Ditte Corapt. rend. 85, 1069, 77; Herz and Knoch Z. anorg. Chem. 41, 319, '04.) Gms. H 3 BO 3 per jo_ 100 Gms. Gms. B 2 O 3 penooGms. t. Gms. HsBO 3 per loo Gms. Gms. B2C per 100 Gn Water. Solution. H 2 O. Water. Solution. H2O. O I 95 I .91 I .1 40 7-0 6 54 3-95 IO 2 .70 2 63 I 5 5 8.8 8 .09 5-o8 20 4 .0 3 85 2 25 60 II. 9 .91 6.2 25 4 7 4 49 2 65 80 16.8 14 38 9-5 30 5 4 5 .12 3 05 IOC 27-5 21 57 I 5-5 2 The above results of Ditte are probably low. Herz and Knoch find for 13, 3.845 grams H 3 BO 3 per 100 cc. solution, for 20, 4-99> 2 5> 5-593' and 26 > 5- 6 37- Bogdan finds 5.753 grams H 3 BO 3 per 100 grams H 2 O at 25. SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OP HYDROCHLORIC, SULPHURIC, AND NITRIC ACIDS AT 26. (Herz Z. anorg. Chem. 33, 355, 34, 205, '03.) Normality of the TToSO HfM Normality of Dissolved. Gms. Strong Acid Gms. B(OH) 3 per 100 cc. Solution. ine xi2ov^/4, riv^i or HNO 3 . B(OH) 3 . Solution. In HC1. In H 2 SO 4 . In HNO 3 . O 0-91 O 5- 6 4 5- 6 4 5.64 o-S 0-78 5 4-0 4.25 4-50 I .0 0.71 10 3-2 3-6 3-9 2.O 0.58 15 2-45 3-o 3-35 3-0 0-49 20 1.8 2-5 2-9 4-0 0-41 25 2.0 2-55 5 - o-35 30 *-55 2.1 6.0 0.26 35 1-75 The determinations given in the original tables in terms of normal solutions when plotted together lay close to an average curve drawn through them. The figures in the tables here shown 'were read (and calculated) from the average curve. SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF ELECTROLYTES Gms. Electro- AT 25. (Bogdan Ann. Scient. Univ. Jassy, 2, 47, 'o2-'o3.) Grams H 3 BO 3 per too Gms. H2O in Aq. Solutions of: lytc per 100 Gms. H 2 O. NaCl. KCl. NaNO 3 . KNO 3 . Na 2 SO 4 . K 2 S0 4 . O 5-75 5-75 5-75 5-75 5-75 5-75 IO 5-75 5.80 5-78 5.81 5-88 5-92 20 5-74 5.86 5.81 5-88 6.00 6.10 40 5-72 5-98 5-87 6.04 6.33 6.50 60 5-72 6.12 5-95 6. 20 6.70 6.92 80 5-7i 6.29 6. 02 6.37 7.10 7.40 Interpolated from the original. 100 parts alcohol dissolve 6.5 parts H 3 BO 3 at 25 and 23 parts at b. pt. (U. S. P.). BORIC ACID 66 SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF UREA, ACE- TONE, AND OF PROPYL ALCOHOL AT 25. (Bogdan.) Grams of CO(NH 2 )2,(CH3) 2 CO or of CsHyOH per 100 Gms. H 2 O. 10 20 40 60 Gms. HaBOs per 100 g. H 2 O in Aq. Solutions of: JL CO(NH 2 ) 2 5-75 5-84 5-93 6-13 6.31 (CH 3 ) 2 CO. 5-75 5-84 5-93 6.12 6.29 C3H 7 OH, 5-75 5-8o 5-85 5-94 6.03 SOLUBILITY OF BORIC ACID IN AQUEOUS SOLUTIONS OF : Acetic Acid at 26. (Herz Z. anorg. Chem. 34, 205, '03.) Acetone at 20. (Herz and Knoch Ibid. 41, 319, '04.) Normality of Solutions. Gms. per TOO cc. Solution. cc. Acetone B(OH)s per 100 cc. Solutioi CH 3 COOHT B(OH) 3 . CHsCOOH. B(OH) 3 . per 100 cc. Solvent. ^lillimols. Grams! 0-91 5- 6 4 O 79 -15 4.91 I 0.82 5 4-7 20 81.71 5-07 2 0.65 10 4.2 30 83-35 4 0-42 20 3- 40 82.72 5 - J 3 6 0.25 30 2.0 50 81.62 5.06 60 76.40 4-74 70 67.62 4.19 80 55-05 3-4i IOO 8.06 0.50 SOLUBILITY OF BORIC ACID IN: Pure Glycerine (Sp.Gr. =1.260 at 15.5). (Hooper Pharm. J. Trans. [3] 13, 258, '82.) Aq. Solutions of Glycerine at 25. (Herz and Knoch Z. anorg. Chem. 45, 268, '05.) Gms. B2O 3 t o 3H 2 Oper TOO CC. Glycerine - Gms. B(OH) 3 per 100 Gms. Wt. % Millimols Glycerine B(OH) 3 per in Solvent. 100 cc. Sol. Sp. Gr. *: Gms. B(OH) 3 per 100 Glycerine. Solution. cc. Solution Gms.So- ' lution. O 20 I5-87 J 3 17 90.1 1.017 5 59 5-50 10 24 19.04 16 CO 7 *5 9O.I 1.038 5 59 5-38 20 28 22 .22 18 .21 20 44 90.6 1.063 5 .62 5.28 30 33 26.19 20 75 31 55 92.9 i .090 5 .76 5-29 40 38 30.16 23 i7 40 95 97-0 1.113 6 .02 5-41 50 44 34-92 25 95 48.7 103.0 i-i33 6 39 5- 6 4 60 50 39.68 28 .41 6 9 .2 I4O.2 1.187 8 .69 7-32 70 56 44-65 30 72 IOO .0 390-3 1.272 24 .20 19.02 80 61 48.41 32 .61 90 67 53-18 34 .70 IOO 72 57-14 36 36 6; BORIC ACID DISTRIBUTION OF BORIC ACID BETWEEN WATER AND AMYL ALCOHOL AT 25. (Fox Z. anorg. Chern. 35, 130, '03.) Millimols B(OH) 3 in Cms. B(OH) 3 in 100 cc. Millimols B(OH) 3 in Gms. B(OH) 3 in TOO cc Aq. Alcoholic Aq. Alcoholic Aq Alcoholic Aq. Alcoholic Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. 265.8 7 6 .6 1.648 O 475 8 7 9 33-2 545 O.2O6 196.5 59 5 I .219 3 6 9 75 .2 22.7 .466 O.I4I 159.6 47 5 0.990 o .294 64 .6 19.76 .400 0.123 126.0 37 .1 0.781 O 230 BORIC ACID (Tetra) H 2 B 4 O 7 . 100 grains water dissolve 2.69 grams H 2 B 4 O 7 at 15, Sp. Gr. == 1.015. (Gerkcb Z. anal. Chem. 28, 473, '89.) BORON TRI-FLUORIDE BF 3 . i cc. H 2 O absorbs 1.057 cc. BF 3 at o and 762 mm., i cc. cone. H 2 SO 4 (Sp. Gr. 1.85) absorbs 50 cc. BF 3 . BROMINE Br. SOLUBILITY IN WATER. (Winkler Chem. Ztg. 23, 687, '99; Roozeboom Rec. trav. chim. 3, 29, 59, 73, 84, '84; Dancer J. Chem. Soc. 15, 477, '62; at 15, Dietze Pharm. Ztg. 43, 200, '98.) Grams Bromine per 100 Grams. ** Water. Solution. (W.) (R. D. & D.) (W.) (R. D. & D.) 4.17 4.22 3.98 4-05 5 10 2O 3-92 3-74 3-65 3-58 3-7 3-4 3-25 3.20 3-77 3.61 3-52 3 46 3-57 3-29 3.10 25 3 -48 3-17 3 ^6 3 -7 30 3-44 3 I 3 3-32 3-03 40 3-45 3-33 50 60 3-52 . . . 3-40 . . . 80 . . . . . . . . . * "Solubility."* a. q. 60.5 43-1 45.8 32.4 35.1 24.8 27.0 I9.O 21-3 14.8 17.0 II.; 13.8 9.4 9.4 6.2 6.5 4.0 4.9 2.8 3.0 I.I * For " Absorption Coefficient " a and " Solubility " q. of Bromine Vapor in water, see Acetylene, page 9. BROMINE 68 SOLUBILITY OF BROMINE IN AQUEOUS SOLUTIONS OF POTASSIUM SUL- PHATE, SODIUM SULPHATE, AND OF SODIUM NITRATE AT 25. (Jakowkin Z. physik. Chem. 20, 38, '96.) v t InK 2 SO 4 ^"fution GmS ' ^ Liter ' In Na 2 SO 4 Gms. per Liter. In NaNOa Gms. per Liter. \ 91.18 i 45-59 i 22.79 i n-39 A 5-69 Br. 25.14 29.44 31.46 32.70 Na 2 SO 4 . 63-55 15.88 7-94 3-97 Br. ' 25.07 29.20 31-33 32-94 32.26 NaNO 3 . 85.09 42.54 21.27 10.63 5-3 1 Br. 28.80 31-35 32.62 33-33 33-74 SOLUBILITY OF BROMIN& IN NORMAL AQUEOUS SALT SOLUTIONS AT 25. (McLauchlan Z. physik. Chem. 44, 617, '03.) Gms. Normality Gms. Gms. Normality Gms. Salt. Salt per of Dis- Br. per .Salt. Salt per of Dis- Br. per Liter. solved Br. Liter. Liter. solved Br. Liter. Water O.O 0.424 33-95 NH 4 NO 3 80. II 0.688 55-15 Na 2 SO 4 63-55 0.286 23-9 NaCl 58-50 o .701 55-90 K 2 S0 4 91 .l8 0.310 24.8 KC1 74.60 0.718 57-40 (NH 4 ) 2 S0 4 70.04 0.971 77-7 NH 4 C1 53-5 2 1.028 82.2 NaNO 3 85.09 0-3495 28.0 CH 3 COONH 4 77.09 4-26 340.5 KNO 3 IOI.I9 0.362 28.95 H 2 S0 4 * 49-03 0.366 29.26 Wildeman. SOLUBILITY OF BROMINE IN AQUEOUS POTASSIUM BROMIDE SOLUTIONS. (Worley J. Chem. Soc. 87, 1107, '05; see also Wildeman Z. physik. Chem. n, 421, '93.) Gram Mols. KBr Gms. KBr Br. per Liter Dissolved at 26.5. Br. per Liter Dissolved at 18.5. per Liter. per Liter. G. Mols. Grams. G. Mols. Grams. o.oo o.oo 0.4282 34.23 0.4448 35.56 O.O2 2.l8 0-4671 37-35 0.4823 38.56 0.04 4.38 0.5101 40.79 0.5243 41.91 0-06 6.55 0.5530 44-21 0.5668 45.31 0.08 8.76 0.5920 47.33 0.6059 48.44 o.io 10.91 0.6488 51.87 0-6533 52.23 0.20 21.82 0.8591 68.69 0.8718 69.69 0.40 43-82 1.2704 101.60 I.3I24 104.90 0.60 65.46 1.6717 133-70 I.77I2 I4I.6o 0.80 87.64 2.1029 168.10 2.2354 178.70 0.90 98.19 2.3349 186.20 2.4851 198.70 ioo grams saturated solution of Bromine in Carbon Bisulphide con- tain 45.4 grams Br at " 95 39 grams at - no. 5, and 36.9 grams at - 116. (Arctowski Z. anorg. Chem. u, 274, *95-'o6.) BROMINE DISTRIBUTION OP BROMINE AT 25 BETWEEN WATER AND: (Jakowkin Z. physik. Chem. 18, 588, '95.) Carbon Bisulphide. Bromoform. Carbon Tetra Chloride. Gms. Br. per Liter of: Gms. Br. jxr Liter of: Gms. Br. per Liter of: Aq. Layer. CSa Layer. Aq. Layer. CHBr 3 Layer. Aq. Layer. CC1 4 Layer. 0-5 36 o-5 33 -5 IS I 80 i 66 i 28 2 163 2 136 2 60 3 240 3 206 3 90 4 330 4 276 4 123 5 420 5 346 5 156 6 515 6 415 6 190 7 62O ... 8 2OO 10 340 12 430 14 520 BRUCINE C 21 H 20 (OCH 3 ) 2 N 2 2 . 4 H 2 0. SOLUBILITY IN SEVERAL SOLVENTS AT i8-22. (Muller Apoth. Ztg. 18, 232, '03.) Solvent. Water Ether Acetic Ether Benzene Gms. Brucine per 100 Gms. Solution. 0.0563 0-749 4-255 I. II Solvent. Gms. Brucine per 100 Gms. Solution. Petroleum Ether 0.088 Carbon Tetra Chloride 0.078 Carbon Tetra Chloride* i .937 Glycerine 2 . 2 * Schindelmeiser Chem. Ztg. 25, 129, '01. BUTANE C 4 H 10 . SOLUBILITY IN WATER AT t. AND 760 MM. Vois. per ioo vols. o 4 10 15 20 3 . 147 2.77 Iso BUTYL ACETATE, etc. SOLUBILITY IN WATER. (Traube Ber. 17, 2304, '84; at 20, Vaubel J. pr. Chem. 59, 30, '99.) 22 22 20 Compound. Grams Com- pound per 100 Grams HaO. Iso Butyl Acelate 0.5 Iso Butyl Formate i . o Normal Butyric Aldehyde 3.6 Iso Butyric Aldehyde 10.0 BUTYL ACETATE 70 SOLUBILITY OF BUTYL ACETATE AND OF BUTYL FORMATE IN MIXTURES OF ALCOHOL AND WATER. (Bancroft Calc. from Pfeiffer Phys. Rev. 3, 205, '95- '96.) cc. HjjO added to cause separation of a Alcohol second phase in mixtures of the given in Mixture quantity of alcohol and 3 cc. portions of: Butyl Formate. Butyl Acetate. 3 3-45 2.08 6 8.83 6.08 9 14-75 10.46 12 21.45 15-37 15 29.65 20.42 i8 39-o 25.60 21 51 .8 31 .49 24 00 37-48 27 43-75 30 50-74 33 s 59-97 100 cc. H 2 O dissolve 0.7 cc. iso butyl acetate at 25 (Bancroft) Iso BUTYRIC ACID (CH 3 ) 2 CH.COOH. SOLUBILITY IN WATER. (Rothmund Z. physik. Chem. 26, 475, '98.) Synthetic Method used, see Note, p. 9. Gms. Iso Butyric Acid per 100 Gms. i . Aq. Layer. Iso Butyric Ac. Layer. 5 16.4 73-4 10 17.5 68.5 15 19.4 62.5 20 22.6 53-9 22 25.8 49.6 24-7 (crit. temp.) 36.3 CADMIUM BROMIDE CdBr, SOLUBILITY IN WATER. (Dietz Ber. 32, 95, '99; Z. anorg. Chem. 20, 260, '99; Wiss. Abh. p.t. Reichanstalt, 3, 433, 'oo; see alsf Eder Dingier polyt. J. 221, 189, '76; Etard Ann. chim. phys. [7] 2, 536, '94.) Gms. CdBr 2 Mols. CdBr 2 Gms. CdBr 2 Mols. CdBr 2 t. per 100 Gms. per 100 Solid Phase. t. per looGms. per 100 Solid Phase. Solution. Mols. H 2 O. Solution. Mols. H2O. o 37.92 4.04 CdBr 2 .4H 2 O 40 60.65 10.20 CdBr 2 .H 2 O 18 48.90 6.21 45 60.75 10.24 30 56.90 8.73 60 61.10 10.39 38 61.84 10.73 8o 62 - 2 9 10.48 35 60.29 10.05 CdBr 2 .H 2 O 100 61.63 IO - 6 3 Density of saturated solution at 18= 1.683. 7i CADMIUM BROMIDE SOLUBILITY OF CADMIUM BROMIDE IN ALCOHOL, ETHER, AND IN ACETONE. ioo gms. sat. solution of CdBr 2 .4H 2 O in abs. alcohol contain 20.93 gms. CdBr 2 at 15 (Eder). ioo gms. sat. solution of CdBr 2 .4H 2 O in abs. ether contain 0.4 gm. CdBr 2 at 15 (Eder). ioo gms. absolute acetone dissolve 1.559 S ms - CdBr 2 at 18. (Naumann Ber.37, 4332, '04.) CADMIUM (Mono) AMMONIUM BROMIDE CdBr 2 .NH 4 Br. SOLUBILITY IN WATER. (Rimbach Ber. 38, 1553, '05; Eder.) A0 ioo Grams Solution contain Gms. Atomic Relation . G. CdBra-NHJSr Cd. Br. NH 4 . Cd : Br : NH 4 '. |Jti. n-nj VJrilia* Solution. 1.0 16.33 34.87 2.6 3 I 3 I 53-82 14.8 17.40 37-15 2.80 I 3 I 58.01 52 -2 19.79 42.38 3-21 I 3 I 65-3I IIO- 1 22 .99 49.17 3-72 I 3 I 75 -98 ioo gms. sat. solution of CdBr 2 .NH 4 Br in abs. alcohol contain 15.8 gms. double salt at 15 (Eder). ioo gms. sat. solution of CdBr 2 .NH 4 Br in abs. ether contain 0.36 gm. double salt at 15 (Eder). CADMIUM (Tetra) AMMONIUM BROMIDE CdBr 2 .4NH 4 Br. SOLUBILITY IN WATER. (Rimbach.) The double salt is decomposed by water at temperatures below 160. ii . c d. i r. NH4. ' C d : Br : NH,. ' Cd : E r : NH 4 . 0.8 H .72 5 .46 6.67 : 4.82 2.82 I 10 .02 8.02 13.0 14 95 5 1 .48 6.85 4-85 2.85 I II 57 9-57 44.0 15 .01 53 85 7-35 5-4 3-04 I 6 .84 4.84 76.4 14 .6 54 .28 7.80 .3 5-32 3-32 I 6 63 4-63 123-5 15 .5 59 5 8-45 5-38 3-38 I 7 40 5-40 160.0 14 7 62 67 9-43 5-99 3-99 I 6 03 4-03 CADMIUM (Mono) POTASSIUM BROMIDE CdBr 2 .KBr.H a O. SOLUBILITY IN WATER. (Rimbach; see also Eder.) ^ ioo Gms. Solution contain Gms. Atomic Relation in Sol. Gms.CdBr 2 .KBr Cd. Br. K. Cd : Br : K". per ioo Gms* Solution. 0-4 I5-4I 33-o 5-42 I 3 I 53-63 15 .8 16.85 35-96 5-86 I 3 I 58.61 50.0 19.58 41.86 6-85 I 3 I 67.87 112.5 22.24 48.28 8.14 0.98 3 1.03 78.11 CADMIUM BROMIDE 72 CADMIUM Tetra POTASSIUM BROMIDE is decomposed by water at ordinary temperatures. CADMIUM (Mono) RHUBIDIUM BROMIDE CdBr 2 .RbBr. SOLUBILITY IN WATER. (Rimbach.) ioo Cms. Solution contain Gms. Atomic Relation in Sol . Gms. CdBr 2 .RbBr t. per ioo Gms. Cd. Br. Rb. Cd : Br Rb. Solution. 0.4 8-37 17-93 6-43 I 3 1. 01 32- 6 5 14.5 10.72 23.02 8.30 0.99 3 1. 01 41-87 49.2 15.01 3 2 -!3 11.51 I 3 I S8-54 ^7-5 19.65 41.12 14.06 I .02 3 0.96 75-77 CADMIUM (Tetra) RHUBIDIUM BROMIDE CdBr 2 .4RbBr. SOLUBILITY IN WATER. (Rimbach.) ioo Gms. Solution contain Gms. Atomic Relation in Sol. Gms.CdBr 2 .4RbBr I . ' Cd Br Rb. ' Cd : Br : Rb. per ioo \jrrn Solution. o-5 5-70 24.94 17.97 0.98 6 4-05 47-95 13-5 6-55 28. 7 4 20.74 0-97 6 4-05 55-J7 Si'S 8-25 35-5 1 25-39 0.99 6 4-02 68.82 H4-5 9-5o 40.67 29.00 1. 00 6 4-0 79.04 CADMIUM (Mono) SODIUM BROMIDE CdBr 2 .NaBr 2 iH,O. SOLUBILITY IN WATER, ETC., AT 15. (Eder Ding, polyt. J. 221, i8g, '76.) Gms. CdBr 2 .NaBr per ioo Gms. Solid S lvCnt - 'Solution. ' Solvent.' Phase. Water 49.0 96.1 CdBr 2 .NaBr.2iH 2 O Absolute Alcohol 21.2 27.0 Absolute Ether 0.52 0.53 " CADMIUM CHLORATE Cd(ClO 3 ) 2 .2H 2 O. SOLUBILITY IN WATER. (Meusser Ber. 35, 1422, '02.) Gms. Mols. Gms. Mols. t o Cd(C10a) 2 Cd(C10,) 2 solid Phase t Cd(ClO 3 ) 2 Cd(ClO 3 ) 2 Solid Phase. 1 per ioo Gms. per ioo Mols. aoua rnasc. * ' per looGms. per ioo Solution. HzO. Solution. Mols. HzO. -20 72.18 22.47 Cd(ClO 3 ) 2 .2H 2 O 18 76.36 27.98Cd(ClO 8 ) 2 .2H 2 O -15 72-53 22.87 49 80.08 34.82 o 74.95 25.92 65 82.95 42.14 Density of the saturated solution at 18 = 2.284. 73 CADMIUM CHLORIDE SOLUBILITY IN WATER. (Dietz W. Abh. p. t. Reichanstalt 3, 433, 'oo; above 100, Etard Ann. chim.phys-t?] 2, 536, '04.) G. CdCl 2 perMols.CdCl 2 Solid G.CdCUper t . ioo Gms. oer ioo ^ " t . 100 Gms. Mols.CdCl, per ioo Solution. Mols.H 2 0. Solution. MSs.H.0. - 9 43.58 7-5' + 10 57-47 13.3' o 49-39 9.6 f~*Af~*] .TT f) 2O 57-35 13.2 + 10 55-58 12.3 4O 57-51 13-3 15 59.12 I4-2J 60 57-7i 13-4 10 44-35 7-8 80 58.41 13-8 o 47-37 9.0 IOO 59-52 14-4. + 18 52-53 10.9 CdCl 2 . 2 JH 2 O 150 64.8 30 56.91 12.8 (monoclinic) 2OO 72.0 36 57-91 J 3-5. 270 77-7 T>UOC Phaae ' Density of saturated solution at 18= 1.741. 100 gms. abs. ethyl alcohol dissolve 1.52 gms. CdCl 2 at 15. 5. 100 gms. abs. methyl alcohol dissolve 1.71 gms. CdCl 2 at 15. 5. (de Bruyn Z. physik. Chem. 10, 783, 'pa.) CADMIUM AMMONIUM CHLORIDE CdCl 2 .NH 4 Cl. SOLUBILITY IN WATER. (Rimbach Ber. 30, 3075, 1897.) IOQ Gms. Solution contain Gms. Gms. per 100 Gms. I . Cd. Cl. Nrt . Solution. Water. ' 2.4 14.26 13-44 2.24 29.94 42.74 16.0 15.82 15-07 2-56 33-45 50.26 41.2 18.61 17.46 2.89 38.96 63-83 63.8 20.92 19-73 3-34 43-99 78.54 105.9 24.70 23-5 2 4-oi 52-23 109-33 CADMIUM (Tetra) AMMONIUM CHLORIDE CdCl 2 .4NH 4 Cl. IN CONTACT WITH WATER. The salt is decomposed in aqueous solution. (Rimbach.) . ioo Gms. Solution contain Gms. Atomic Relation in Solution. * Cd. Cl. NH 4 . 3-9 5-75 18.17 7-37 16.1 6.96 20.26 7 97 40.2 9.91 23.84 8.92 58-5 12.50 26-53 9-35 112.9 16.66 31-79 10.78 ii3-9 16.51 32-71 11.30 Cd Cl 9.96 9-2O 7 .6i 6. 7 i 6. 02 6.26 NH*. 7.96 7-13 5-61 4-66 4.02 4.26 SOLUBILITY OF MIXTURES OF CADMIUM TETRA AMMONIUM CHLORIDE AND CADMIUM AMMONIUM CHLORIDE IN WATER. (Rimbach Ber. 35, 1300, '02.) t ioo Gms. Solution contain Gms. Atomic Relation. Solid Phase, Mol. per cent of: Cd. Cl. NH4. Cd : Cl : NH*. CdCla. CdCla. 4NH4C I .1 5 34 17 .62 7.27 i 10-47 8.50 49-6 50-4 M 7 .12 19 .86 7-84 i 8.84 6.87 47-o 53-o 40 7 10 .24 23 .82 8.85 i 7-37 5-37 77.0 23 o 53 5 12 50 26 53 9-35 i 6. 7 I 4.66 CADMIUM CHLORIDE 74 SOLUBILITY OF MIXTURES OP CADMIUM TETRA AMMONIUM CHLORIDE AND AMMONIUM CHLORIDE IN WATER. (Rimbach.) ioo Gms. Solution t*^ contain Gms. Atomic Relation Solid Phase, Mol. per cent of: Cd. Cl. NH. Cd : Cl : NH 4 . ' NH 4 C1. CdCl 2 . 4 NH 4 d. 1.0 2.82 17 .11 7 .82 I 19.21 17.28 59-o 4i .0 !3-2 2. 7 6 18 .84 8 7 1 I 21 .62 19.62 74-o 26 .0 40.1 3-16 22 56 10 49 I 22 .65 20.74 71.0 29 .0 58-2 3-51 25 .21 II .72 I 22.79 20.89 69.0 3i .0 OADMIUM BARIUM CHLORIDE 2(CdCl 2 ).BaCl 2 .5H 2 O. SOLUBILITY IN WATER. (Rimbach Ber. 30, 3083, '97.) t. 22.6 41-3 53-9 62.2 69-5 107.2 CADMIUM t 8 . 22.5 3 2 -9 41.4 53-4 62.0 97.8 108.3 109.2 100 Gms. Solution contain Gms. Gms. 2(CdCl 2 ).BaCl 2 per 100 Gms. 'Cd. Cl. Ba. Solution. Water. 17.71 16.89 ii -o 45-6o 83.82 19.22 18.15 n-77 49 I 4 96.62 19.85 18.75 12.41 51-04 104.25 20.59 19.66 12.83 53- 08 II 3- I 3 21.20 20.18 13-09 54-47 119-64 24.25 23.23 14.90 62.38 165.85 BARIUM CHLORIDE CdCl 2 .BaCl 2 .4H 2 O. SOLUBILITY IN WATER. (Rimbach.) 100 Gms. Solution Gms. CdCl 2 .BaClj contain Gms. per 100 Gms. Cd. Cl. Ba. 11.98 15-19 I 4-7 I 12.40 16.18 16.09 13.05 16-95 16.81 13.96 18.21 18.13 14.73 l8 -8i l8 -74 17.57 22.48 22.00 18-53 23.51 22 -79 18.67 23.69 29.95 Solution. Water. 41.88 72.06 44.67 80.73 46.81 88.01 50.30 IOI-2I 52.28 109.56 62.05 163.^0 64.83 184.33 65.31 188.27 OADMIUM MAGNESIUM CHLORIDE 2 (CdCl 2 )MgCl 2 .i2H 2 O. SOLUBILITY IN WATER. (Rimbach.) ioo Gms. Solution Gms. 2(CdCl 2 ).MeCl 2 contain Gms. per ioo Gms. Cd. Cl. Mg. Solution. Water. 2-4 22.14 21 .06 2.41 45.61 83-86 20.8 24.30 22.80 2-55 49.69 98. 77 45-5 26.24 24-55 2.72 53-5 1 115 .IO 67.2 28.45 26.71 2.98 58-14 I38.QO 121. 8 31-84 30-20 3-44 65.48 189.69 75 CADMIUM CHLORIDE CADMIUM (Mono) RHUBIDIUM CHLORIDE CdCl 2 .RbCl. SOLUBILITY OF CADMIUM MONO RHUBIDIUM CHLORIDE IN WATER. (Rimbach Ber. 35, 1303, '02.) 100 Gms. Solution ontain Gms. Gms. CdCl 2 .RbCl per 100 Gms. I . Cd. Cl. Rb. Solution. Water. I .2 4.80 4-53 3.63 12-97 14.90 14-5 6. 20 5-88 4-75 16.80 20.19 41.4 9-34 8.86 7.14 25 -3 1 33 -89 57-6 11.40 10.78 8.63 30-83 44-58 103.9 17.14 16.37 13.39 46.62 87.36 CADMIUM (Tetra) RHUBIDIUM CHLORIDE CdCl 2 . 4 RbCl. IN CONTACT WITH WATER. (Rimbach.) The double salt decomposes to CdCl 2 .RbCl and RbCl. t . ioo Gms. Solution contain Gms. Atomic Relation. Solid Phase, Mol. per cent of: Cd. Cl. Rb. Cd : Cl : Rb. CdClo. RbCl. CdCl 2 . " 4 RbCl. 0.7 O 65 6-52 14 73 I 31.88 2 9 .88 30 70 8.8 I 07 7-37 16 I 21.89 19 .89 24 7 6 13.8 I 32 7.86 16 93 I 18.88 16 83 16 84 42-4 3 .21 ii .35 22 45 I II .21 9 .21 14 86 59 o 4 .6l 13 .41 25 I 9-23 7 23 33 67 108.4 8 94 l8 -57 3 1 15 I 6-57 4 59 SOLUBILITY OF MIXTURES OF CdCl 2 .4RbCl AND RbCl IN WATER. (Rimbach.) Solid Phase, Mol. per cent of: ioo Gms. Solution contain Gms. Atomic Relation. Cd. 0.4 14.8 17.9 Cl. 12.86 13 .62 14.0 Rb. 30-97 32.81 33-71 Cd Cl : Rb. I I I I I I CdCl 2 . 4 RbCl RbCl. 55 45 67 33 80 20 THE EFFECT OF THE PRESENCE OF HC1, CaCl 2 AND OF LiCl UPON THE DECOMPOSITION OF CADMIUM TETRA RHUBIDIUM CHLORIDE BY WATER AT 16. (Rimbach Ber. 38, 1570, '05.) ioo Gms. Solution contain Gms. Mols ^ J00 Mf)ls HzO Molecular Ratio> Total Cl. Cl. HCl. c d. N Rb. C. :dci 2 . t .bCl. HCl. CdC :i 2 : Rbci: 36-44 0.84 36.61 41 i-39 .109 483 29.76 1 [ 4-43 28.45 0.80 28.44 35 1-38 o .082 .422 20-35 5-J5 12 .09 3-24 9.11 o 69 6.74 o 139 X 772 5.60 J2-75 Ca. CaCl 2 . CaCl 2 . 14-98 7-56 20.91 73 2.80 o 159 o 799 4-59 5-04 12.70 5-77 15.96 77 4.87 o 163 I 353 3-4i 8.31 10-85 3-78 14.47 l' oo 8.51 o .211 2 365 2.24 II .22 9-o8 1.84 5-10 I 24 12 .14 o .262 3 385 i -09 12.92 Li. Lid. Lid. 26.49 4.8 7 29-40 56 3-87I J 39 i .271 19.40 t 9 13 20-37 3-33 2O- 1 1 o 52 7.84 .122 2 433 12-54 [ 19.88 See Note on next page. CADMIUM CHLORIDE 76 CADMIUM (Mono) POTASSIUM CHLORIDE CdCl 2 .KCl.H a O. SOLUBILITY IN WATER. (Rimbach Ber. 30, 3079, '97; see also Croft Phil. Mag. [3] 21, 356, '42.) 100 Gms. Solution Gms. CdCb-KCl t. contain Gms. per ipo Gms. Cd. CT R. Solution. Water. 2.6 9.53 9.03 3.31 21.87 2 7-99 15.9 11.63 10.98 3.99 26.60 36.24 41-5 15-47 14-73 5-45 35 - 66 55-34 60.6 17.68 16.80 6.20 40.67 68.55 105.1 22.46 21.34 7.87 5*-67 106.91 CADMIUM (Tetra) POTASSIUM CHLORIDE CdCl 2 . 4 KCl. IN CONTACT WITH WATER. (Rimbach.) The double salt is decomposed when dissolved in water at ordinary temperature. zoo Grams Solution contain Gms. l> . Cd. Cl. K. 4 3- 6 4 9.84 8-31 23.6 5.66 14.02 11.52 50.2 9.10 18.09 13.60 108.9 11.94 23 .11 17.16 NOTE. The effect of the presence of certain chlorides upon the decomposition of cadmium tetra potassium chloride by water at 16 was investigated by Rimbach in a manner similar to that used in the case of cadmium tetra rhubidium chloride (see preceding page). The results, which show the extent to which increasing amounts of the several chlorides force back the decomposition of the double salt, were plotted on cross-section paper, and the points at which the decom- position was prevented, were determined by interpolation. These values which show the minimum amount of the added chlorides which must be present to insure the crystallization of the pure double salt are shown in the following table. /\aaea Chloride. CdCl 2 . KCl. Added! Chloride. jLeusuy 01 Solutions. CdCl 2 . KCl. Added Chloride. HC1 0.074 .296 19 .80 I .1403 0-033 o .132 8.828 LiCl 0-344 I 376 9 30 I .1380 0.166 .663 4.483 CaCl, 0-544 2 .176 3 .80 I 2333 0-270 I .808 1.887 KCl 1.034 6 514* 2 -378 I .214 0-507 3 .195* I .167 * Total. CADMIUM CYANIDE Cd(CN) 2 . 100 gms. H 2 O dissolve 1.7 gms. Cd(CN) 2 at 15. (Joannis Ann. chim. phys. [5] 26, 489, '82.) 77 CADMIUM FLUORIDE CADMIUM FLUORIDE CdF 2 . SOLUBILITY IN WATER. 100 cc. saturated aqueous solution contain 4.36 gms. CdF 2 at 25. (Jager Z. anorg. Chem. 27, 34, '01.) CADMIUM HYDROXIDE Cd(OH) 2 . SOLUBILITY IN WATER. i liter of aqueous solution contains 0.0026 gm. Cd(OH) 2 at 25. (Bodlander Z. physik. Chem. 27, 66, '98.) CADMIUM IODIDE CdI 2 . SOLUBILITY IN WATER. (Dietz W. Abh. p. t. Reichanstalt 3, 433, 'oo; see also Kremers Pogg. Ann. 103, 57, '58; Eder Dingl. polyt. J. 221, 189, '76; Etard Ann. chim. phys. [7] 2, 536, '94.) A0 Gms. CdI 2 per ioo Gms. Mols. CdI 2 Gms. CdI 2 r^er ioo Gms. Mols. CdI 2 Solution. Water. MoTs.'SzO. Solution. Water. Mob 1 U^O. O 44-4 79.8 3-9 30 47-3 89.7 4-43 10 45-4 83.2 4-1 40 48-4 93-8 4.6 15 45-8 84.5 4.17 50 49-35 97-4 4.8 18 46.02 85.2 4.2 75 52.65 III .2 5-4 20 46-3 86.2 4.26 IOO 56.08 127.6 6-3 25 46.8 87.9 4-34 Density of saturated solution at 18 = 1.590. SOLUBILITY OF CADMIUM IODIDE IN ORGANIC SOLVENTS. Observer. (Eder.) (Timofeiew Compt. rend. 112, 1224, '91.) (Timofeiew Compt. rend. 112, 1224, '91.) (Timofeiew Compt. rend. 112, 1224, '91.) (Eder.) (Naumann Ber.37, 4332, '04.) Solvent. t. Gms. CdI 2 per ioo Gms. Solution. Solvent. Absolute Alcohol 15 50 5 102 o Ethyl Alcohol 20 42 .6 74 .27 Methyl Alcohol 20 59 .0 J 43 7 Propyl Alcohol 20 28 9 40 .67 Absolute Ether 15 21 7 27 7 Absolute Acetone 18 20 25 .0 CADMIUM AMMONIUM IODIDES (Mono and Di) . SOLUBILITY IN WATER, ETC. (Rimbach Ber. 38. 155?. 'os; at 15 Eder Dingl. polyt. J. 221, 189, '76.) Cd. Mono Ammonium Iodide. Solvent. Water Abs. Alcohol Abs. Ether Gms. CdI 2 .NH4l per t > ioo Gms. 15 15 15 Solution. 52.6 53 29.4 Solvent. Ill .O "3 41.7 Cd. Di Ammonium Iodide. 14.5 15 Gms. CdI 2 .2NHJ per ioo Gms. Solution. 59 10 Solvent. 611.6 ii CADMIUM IODIDES 78 CADMIUM POTASSIUM IODIDES, Mono Di= CdI 2 .2KI. 2 H 2 O. CdI 2 .KI.H 2 O, CADMIUM Di SODIUM IODIDE Cdl2.2NaI.6H 2 O. SOLUBILITY IN WATER, ETC., AT 15. (Eder.) Gms. CdI 2 .KI Gms. CdI 2 . 2 KI Gms. CdI 2 .2NaI Solvent. ^ per IPO Gms. per 100 Gms. per 100 Gms. Solution. Solvent. Solution. Solvent. Solution. Solvent. Water 51.5 106 57-8 137 61-3 158.8 Abs. Alcohol . . . 41.7 71 53-7 116.2 Abs. Ether 39 4.1 9.0 99 CADMIUM NITRATE Cd(NO 3 ) 2 . SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichanstalt 3 440, 'oo.) Mols. Cd(NO 3 ) 2 Solid per 100 Mols. H 2 O. Phase. 4.55 Cd(N0 3 ) 2 . 9 H 2 6.85 8.50 8.37 Cd(N0 3 ) 2 . 4 H 2 9.61 10.7 12. 1 25.0 Density of saturated solution at 18 = 1.776. Gms. Cd(NO 3 ) 2 t o. per loo^Gms. -13 I Solution. 37-37 47-33 Water. 89.86 + I 52-73 in. 5 + 18 52-37 55-9 109.7 126.8 30 40 59-5 61 .42 76.54 140.4 159.2 326.3 CADMIUM OXALATE CdC 2 O 4 . 3 H 2 O. i liter of sat. aqueous solution contains 0.033 g m - CdC 2 O 4 at 18. (Kohlrausch Z. physik. Chem. 44, 197, '03.) CADMIUM SULPHATE CdSO 4 . SOLUBILITY IN WATER. (Mylius and Funk W. Abh. p. t. Reichanstalt 3, 444, 'oo; see also Kohnstamm and Cohn Wied Ann. 65, 344, '98; Steinwehr Ann. der Phys. (Drude) [4] 9. 1050, '02; Etard Ann. chim. phys [?] 3 536, '94-) Solid Phase. Gms. CdS0 4 t . per TOO Gms. Solution. Water. -17 44-5 80.2 -10 4 6.1 85-5 5 48.5 94.2 18 43-35 76.52 10 43-27 76.28 o 43 - OI 76.48 + 10 43-18 76.00 20 43-37 76.60 CdSO 4 .7H 2 O CdSO 4 .|H 2 O Gms. CdSO 4 t. per TOO Gms. Solid Solution. Water. ase. 40 43-99 78.54 CdSO 4 .fH 2 O. 60 44-99 83.68 " 73-5 46.6 87.28 M 74-5 46.7 87.62 CdSO 4 .H 2 O 77 42.2 73.02 a 85 39-6 " 90 38.7 63.13 tt 100 37-8 60.77 tt 79 CADMIUM SULPHATE SOLUBILITY OF CADMIUM SULPHATE IN AQUEOUS SOLUTIONS OF SUL- PHURIC ACID AT o. (Engel Compt. rend. 104, 507, '87.) Equivalents per 10 Gms. H2O. Density Grams per 100 Grams H 2 O. HaS0 4 . CdS0 4 . of Solutions. H 2 SO 4 . CdSCv " o. 71.6 1.609 - 74 -61 3.87 70.9 1.591 1.90 73.87 12.6 62.4 I -545 6.18 65.03 28.1 50.6 1.476 13.78 52.73 43.3 40.8 1.435 21.23 42-52 47.6 37.0 1.421 23.34 38.56 53.8 32.7 1.407 26.38 34.07 71.5 23.0 1.379 35.06 23.96 SOLUBILITY OF MIXED CRYSTALS OF CADMIUM SULPHATE AND FERROUS SULPHATE IN WATER AT 25. (Stortenbecker Z. physik. Chem. 34, 109, 'oo.) i^om position 01 ooiunoii. _ . . . ^ ^ JL Mnl n*r rent PH in Gms. per too Gms. H 2 O. Mols. per 100 Mols. H 2 0. Mol. % Cd. in Sol. Crystals of Solid Phase. CdSO 4 . FeSO 4 . ' Cd. Fe. ' Crystals with 2 Mols. H 2 O. 76.02 o.o 6-57 o.o 100 100 57-61 10.63 4.98 1.26 79-8 99 .0 Crystals with 7 Mols. H 2 0. 57-61 10.63 4.98 1.26 79-8 3 6.6 78-5 34-6 . . . . . . . . . . . . 44.6 n. i . . . . . . . . . . . . 24.4 4-8 o.o 26.60 o.o 3 -165 o.o o.o CADMIUM POTASSIUM SULPHATE CdK 2 (SO 4 ) 2 . SOLUBILITY IN WATER. (Wyrouboff Bull. soc. chim. [3] 25, 121, f oi.) ,o G. CdK t (SO 4 ) 2 per Solid 100 Gms. H 2 O. Phase. t o G. CdK 2 (SO 4 ) 2 Solid ' per 100 Gms. H^. Phase. 16 42.89 CdK 2 (S0 4 ) 2 . 2 H 2 26 42.50 CdK 2 (S0 4 ) 2 .iiH 2 3i 46.82 u 3 1 42.80 40 47-40 u 40 43-45 a 6 4 44.90 u CADMIUM SODIUM SULPHATE 80 CADMIUM SODIUM SULPHATE CdNa 2 (SO 4 ) 2 . 2 H 3 O. SOLUBILITY IN WATER, ALSO WITH THE ADDITION OF CADMIUM SUL- PHATE AND OF SODIUM SULPHATE. (Koppel, Gumpery Z. physik. Chem. 52, 413, '05.) Gms. per 100 Gms. t. Solution. Gms. per 100 Gms. H 2 O. Mols. per 100 Mols. H ?- Solid Phase. CdSO 4 . Na 2 S0 4 . CdSO 4 . Na 2 S0 4 . CdSO 4 . Na 2 S0 4 . 24 22 25 15 .07 35 49 24 .04 3 .07 3-05) 30 22 55 15 .29 36 .28 24 .60 3 .14 3.12 VCdNa 2 (S0 4 ) 2 . 2 H 2 O 40 22 .89 15 65 37 .24 25 45 3 .22 3-28J 40 32 4 85 73 54 8 85 6 36 10 39 .91 5 .24 72 77 9 55 6 30 .2i)cdNa 2 (S0 4 ) 2 . 2 H 2 20 40 .26 5 .16 73 81 9 45 6 39 .20 1 +CdSO 4 -fH 2 O 40 39 .89 7 .18 75 38 13 56 6 52 7*1 14.8 40 .18 4 .60 72 68 8 32 6 .29 / ' s i o 10 20 37 32 22 3o 53 .69 6 8 14 53 .69 66 55 32 34 ii 14 23 .62 .78 52 5 4 3 74 79 .14 \'V 1 CdNa 2 (S0 4 ) 2 . 2 H 2 lyi + Na 2 S0 4 .ioH 2 25 16 33 19 .82 25 60 .06 2 .21 3-94' 30 9 .21 27 .80 14 62 44 .14 I .26 4 59 1 /""fl^ji fQO ^ oTT (~l 35 40 8 9 .26 .98 29 28 35 .27 16 26 24 47 46 .06 .27 I I .41 If 6 j +*W CAESIUM ALUMS SOLUBILITY OF CAESIUM CHROMIUM ALUM, CAESIUM IRON ALUM, CAESIUM INDIUM ALUM, AND OF CAESIUM VANADIUM ALUM IN WATER. (Locke Am. Ch. J. 27, 174. *oi.) Formula of Alum. Cs 2 Cr 2 (S0 4 ) 4 . 24 H 2 C S- Fe 2 (S0 4 ) 4 . 24 H 2 Cs 2 In 2 (S0 4 ) 4 . 24 H 2 Cs 2 V 2 (S0 4 ) 2 .2 4 H 2 25 30 35 40 25 35 40 25 2 5 Gms. per 100 cc. H^. Anhydrous Salt. Hydrated" Salt. o-57 0.96 i .206 o 94 !-52 1.91 i .53 2-43 1.71 2.72 2.52 3-75 6.04 4-oi 6.01 9.80 7-57 ii .73 0.771 1 -3 1 Gram Mols. Salt per zoo cc. H^. O.OOI5I 0.0025 0.0032 0.00405 0.0045 O.OO66 O-OO99 0.0156 0.0172 O.OO2O4 8 1 CAESIUM CHLORAURATE OAESIUM CHLORAURATE CsAuCl 4 . SOLUBILITY IN WATER. (Rosenbladt Her. 19, 2537, '86.) ... Gms. CsAuC^ per 100 Gms. Solution. Gms. CsAuCU t. per TOO Gms. t. Solution. Gms. CsAuOt per 100 Gms. Solution. 10 o-5 40 3-2 80 16.3 20 0.8 SO 5-4 00 21.7 30 1.7 60 8.2 100 27-5 70 12.0 OAESIUM FLUOBORIDE CsBFl 4 . 100 grams water dissolve 0.92 gram CsBFl 4 at 20, and 0.04 gram at 100. (Godeffroy Ber. 0, 1367, '76.) CAESIUM MERCURIC BROMIDE CsBr. 2 HgBr 2 . 100 grams saturated aqueous solution contain 0.807 gram CsBr. 2HgBr 2 at l6. (Wells Am. J. Sci. [3} 44. 221, '92.) CAESIUM CARBONATE Cs 2 CO 3 . 100 grams absolute alcohol dissolve u.i grams Cs 2 CO*at 19, and 20.1 grams at b. pt. (Bunsen.) OAESIUM CHLORIDE CsCl. SOLUBILITY IN WATER. (Berkeley Trans. Roy. Soc. (Lond.) 203 A, 208, '04; see also Hinrichsen and Sachsel Z. physik. Chem. 50, 99, '04- '05; at 25, Foote.) G. CsCl per IPO Gms. G.Mol.CsCl t o G. CsCl per 100 Gms. G. Mol. CsCl Solution, Water. per Liter. Solution . Water. per Liter. O 61 7 161 4 6 74 60 69.7 229 7 8.28 IO 63 .6 174 7 7 .11 70 70.6 239 5 8.46 20 65 .1 186 5 7 38 80 71.4 250 o 8.64 3 66 4 I 97 3 7 63 90 72.2 260 .1 8.80 40 67 5 208 .0 7 .86 100 73-o 270 5 8.96 50 68 .6 218 5 8 .07 119.4 74-4 200 o 9-22 SOLUBILITY OF MIXTURES OF CAESIUM CHLORIDE AND MERCURIC CHLORIDE IN WATER AT 25. (Foote Am. Ch. J. 30, 340, '03.) Gms. per 100 Gms. Gms. per 100 Gms. Solution. Solid Phase. Solution. 5^4 p^^. CsCl^ HgCl 2 . CsCl 2 . HgCl 2 . 65.61 o.o CsCl 38.63 1.32 ) 65.78 0.215 CsCl + Cs,HgCl B 17.03 0. 5 i ( gBWkSjg^OCi 62.36 0.32 ) Double Salt 1-53 0.42 ) 57.01 0.64 > CssHgCl 6 0.6i 2.64 CsHg +CsHg,Cl s 52.35 1.23 ) -65-1% CsCl . 49 2<9I 1 DoubleSalt 51.08 1.44 Cs s HgCl 5 + CsjHgCl* 0.40 3.78 J CsHgjCls = 23.7% CsCl 49.30 1.49 I DoubleSalt 0.44 4.63 CsHg,Cl 6 + CsHgsClu 45.95 !- 6 9 ) Cs H gCU = 55.4%CsCl 0.41 4-68 ) DoubleSalt 45-23 1-73 Cs,HgCU + CsHgCl, 0.25 5.65 J CsHfoCU^n.^CBCl . 1 8 7.09 CsHg B Cl u + HgCl, o.o 6.90 HgCl, CAESIUM CHLORTELLURATE 82 CAESIUM CHLORTELLURATE CsTeCl 6 . SOLUBILITY IN AQUEOUS HYDROCHLORIC ACID. (Wheeler Am. J. Sci. [3] 45. 267, '93-) ioo parts HC1 (Sp. Gr. 1.2) dissolve 0.05 part CsTeCl 6 at 22. 100 parts HC1 (Sp. Gr. 1.05) dissolve 0.78 part CsTeCl 6 at 22. CAESIUM THALLIC CHLORIDE 3 CsCl.TlCl 3 .2H 2 O. ioo parts H 2 O dissolve 2.76 parts 3CsCl.TlCl 3 .2H 2 O at 17, and 33.3 parts at I00. (Godeffroy Z. Osterr. Apoth. Ver. No. 9, 1886). CAESIUM IODATE CsIO 3 . ioo parts H 2 O dissolve 2.6 parts CsIO 3 at 24, and 2.5 parts 2CsIO 3 . I 2 O fi at 21 (Wheeler Am. J. Sci. [3] 44, 123, '92.) CAESIUM IODIDE Csl. SOLUBILITY OF MIXTURES OF CAESIUM IODIDE AND IODINE IN WATER. (Foote Am. Ch. J. 29, 210, '03.) t. -4 -4 -4 0.2 Gms. per ioo Gms. Solution. 35-6 35-6 35-6 35-6 Gms. per ioo Gms. Solution. Solid Phase at Csl Csl and CsI 3 CsI 3 and CsI 5 CsI 5 and I Csl. I. 27.68 o.o 27.52 0.09 3.18 0.31 0.85 0-34 Csl. I. 51.48 o.o 51.66 0.71 10.72 1.78 3.74 I. 60 t . 52- S 2 - 52- 52- 73 73 73 Gms. per ioo Solution. Gms. 2 2 2 2 Csl. 16.75 6.69 6.72 6.65 26.98 16.66 6.27 4 3 3 3 15 10 ' 4 I. 36 32 45 .07 50 .08 In Separated Heavy Solution Gms. per ioo Gms. Solution. ^? Csl. I. . . . CsI 3 and CsI 5 . . . CsI 5 and I 22.94 73-72 CsI 5 22.80 74-63 I CsI 3 and CsI B 27.56 68.40 Csl. 17.68 80.02 I CAESIUM (Tri) IODIDE CsI 3 . ioo cc. saturated aqueous caesium iodide (about 17 per cent Csl) solution contain 0.97 gram CsI 3 at 20, density of solution = 1.154. (Wells Am. J. Sci. [3] 44, 221, '92.) CAESIUM NITRATE CsNO 3 . SOLUBILITY IN WATER. (Berkeley Trans. Roy. Soc. (Lond.) 203 A, 213, '04.) Gms. CsNOs per t. ioo Gms. G. Mols. CsN0 3 t . per Liter. Gms. CsNOs per ioo Gms. G. Mols CsNOt per Liter. Solution. Water. Solution. Water". 8-54 9 33 ,476 60 45 .6 83 .8 3-41 10 12.97 14 9 O 725 70 5 1 7 107 O 4-10 20 18.7 2 3 .0 I .11 80 57 3 134 .0 4-8l 30 25-3 33 9 j 58 90 62 .0 I6 3 .0 5-50 40 32.1 47 .2 2 .12 IOO 66 3 197 .0 6.19 50 39-2 64 4 2 73 106.2 68 .8 220 3 6.58 CAESIUM OXALATE CAESIUM OXALATE Cs 2 C 2 O 4 .H 3 O. SOLUBILITY OF MIXTURES OP CAESIUM OXALATE AND OXALIC ACID IN WATER AT 25. (Foote and Andrew Am. Ch. J. 34 156, '05.) Varying amounts of the two substances were dissolved in hot watei and the solutions allowed to cool in a thermostadt held at 25. Solid Phase. H 2 C 2 4 .2H 2 0+H 3 Cs(C 2 4 ) 2 . 2 H 2 Double Salt. H 3 Cs(C 2 4 ) 2 .2H,0 H 3 Cs(C 2 4 ) 2 2H 2 + H 4 Cs 2 (C 2 4 ) 3 Double Salt. H 4 Cs 2 (C 2 4 ) 3 H 4 Cs 2 (C 2 4 ) 3 +HCsC 2 4 Double Salt. HCsC 2 O 4 HCsC 2 4 +H 6 Cs 8 (C 2 4 ) 7 Double Salt. H 6 Cs 8 (C 2 4 ) 7 H 6 Cs 8 (C 2 4 ) 7 +Cs 2 C 2 4 .H 2 Cs 2 C 2 O 4 .H 2 O Gms. per 100 G. Mols. per 100 Gms. Solution. G. Mols. H 2 O. Hi Cs 2 Cs6 4 . H 2 C 2 4 . Cs^zO*. 10 .20 . 2.274 10 .29 O .61 2.314 O 035 7 .90 9 .92 924 O 614 { 4 .11 2 5 .12 ] .162 I 81 J 4 32 27 55 .279 2 06 4 27 28 30 .267 2 14 I 4 40 35 .90 .476 3 07 J 4 -82 40 .10 752 3 .71 4 45 42 32 .672 4 05 ) 3 05 48 .80 1.268 5 16 [ i .04 68 .69 0.688 ii 56 ) o .91 71 .24 o . 648 13 06 77 73 45 0.598 14 5 1 I 75 74 .04 0.596 14 .96 J 74 75 .20 0.625 15-93 .0 75 .82 o.o IS 97 CAESIUM PERMANGANATE CsMnO 4 . 100 cc. sat. aqueous solution contain 0.097 gm. CsMnO 4 at i, 0.23 gm. at 19, and 1.25 gms. at 59. (Patterson J. Am. Chem. Soc. 28, 1735, '6.) CAESIUM SELENATE Cs 2 SeO 4 . 100 grams H 2 O dissolve 245 grams Cs 2 SeO 4 at 12. (Tutton J. Chem. Soc. 7L 850, '97 ) CAESIUM SULPHATE Cs 2 SO 4 . SOLUBILITY IN WATER. (Berkeley Trans. Roy. Soc. (Lond.) 203 A, 210, '04.) Gms. Cs 2 SO 4 per G. Mols. Gms. Cs 2 SO 4 per G. Mols. J. too^Gms. Cs 2 S0 4 t. 100 Gms. C S2 S0 4 Solution. Water. per Liter. Solution. Water. per Liter. 62.6 I6 7 .1 3 .42 60 66 7 199 9 3-78 10 63-4 173 .1 3 .49 70 67 .2 205 O 3-83 20 64.1 I 7 8 7 3 56 80 67 .8 2IO 3 3-88 30 64.8 184 .1 3 .62 00 68 3 214 9 3-92 40 65-5 189 9 3 .68 100 68 .8 220 3 3-97 5 66.1 194 9 3 73 108.6 69 .2 224 5 4.00 CAESIUM DOUBLE 84 SULPHATES SOLUBILITY OF CAESIUM DOUBLE SULPHATES IN WATER AT 25. (Locke Am. Ch. J. 27. 459, 'ox.) Cms. Anhydrous Salt G m. Mols. Name. Formula. per 100 Gms. Salt per 100 Solution. Water. Gms. H 2 O. Caesium Cadmium Sulphate Cs 2 cd(sO4) 2 .6H 2 o 58.16 139.9 0.2455 Caesium Cobalt Sulphate CszCoCso^-eHzO 29.52 41.9 0.081 Caesium Copper Sulphate Cs,Cu(so 4 ) 2 .6H 2 o 31-49 46.0 0.0882 Caesium Iron Sulphate Cs 2 Fe(so 4 ) 2 .6H 2 o 50.29 101.1 0.1967 Caesium Magnesium Sulphate CsjsMgtso^HaO 34-77 53-3 o . 1 106 Caesium Manganese Sulphate Cs2Mn(SO 4 ) 2 .6H2O 44-58 80 . 4 0.157 Caesium Nickel Sulphate Cs2Ni(so 4 )2.6H 2 o 20.37 25.6 0.0495 Caesium Zinc Sulphate Cs2Zn(so 4 ) 2 .6H 2 o 27.87 38.6 0.0738 CAFFEINE C 6 H(CH 3 ) 3 N 4 2 .H 2 0. SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P. ; Gockel J. Chem. Soc. 74 32?, '98; CommaiUe Compt. rend. 8x, 819, '75.) Grams Caffeine per 100 Grams Solvent at: Solvent. 25. 80. U.S. P. 18. Gockel. b.pt. is .17 b. CommaiUe. pt. Water 2.19 19-23 . . . . I 3 T J 45- 54 Alcohol 1.88 5.85* , . .6iJ 3. Ether 0.267 o. 119 2 95 O 044| o. 3^1 Chloroform 12.5 II . 77 15 12 97t 19. 02% Benzene - . . ... o. 911 5 .29 . , Carbon Tetra Chloride ... ... o. 089 .702 . Carbon Bisulphide ... . 0585* o. 454J * 60. t 65. t Gms. anhydrous caffeine. Abs. alcohol and abs . ether. CALCIUM ACETATE Ca(CH 3 COO) 2 . 2 H 2 O. SOLUBILITY IN WATER. (Lumsden J. Chem. Soc. 81, 355. '02-, Krasnicki Monatsh. Chem. 8, 597, '87.) Gms. CaCCHaCOOa Gms. Ca(CH 3 COO) 2 t. per IPO Gms. Solid Phase. t. per 100 Gms. Solid Phase. Solution. Water. Solution. Water. O 27.2 37.4 Ca(CH 3 COO) 2 .2H 2 O 60 24.6 32.7 Ca(CH 3 COO) 2 .2H 2 O 10 26.5 36.0 Ca(CH 3 COO) 2 .2H 2 O 80 25.! 33.5 Ca(CH3COO) 2 .2H 2 O 20 25.8 34.7 Ca(CH 3 COO) 2 . 2 H 2 O 84 25.3 33.8 Ca(CH 3 COO) 2 .2H 2 O' 2 5 25.5 34.2 Ca(CH3COO) 2 .2H20 85 24.7 32.9 Ca(CH 3 COO) 2 .H 2 O 3 2 5-3 33 " 8 Ca(CH 3 COO) 2 . 2 H 2 90 23.7 31.1 Ca(CH 3 COO) 2 .H 2 O 40 24.9 33.2 Ca(CH 3 COO) 2 . 2 H 2 IOO 22-9 29.7 Ca(CH3COO) 2 .H,O SOLUBILITY OP CALCIUM ACETATE IN AN AQUEOUS SATURATED SOLU- TION OF SUGAR AT 31.25. (Kohler Z. Ver. Zuckerind. 47, 447, *97-) TOO gms. solution contain 8.29 gms. Ca(CH 3 COO) 2 + 60.12 gms. sugar, loo gms. water dissolve 26.3 gms. Ca(CH 3 COO) 2 + 190.3 gms sugar. CALCIUM ACETATES CALCIUM (Tri) Methyl ACETATE Ca[(CH 3 ) 3 CCOO] 3 . CALCIUM (Di) Ethyl ACETATE Ca[(C 2 H 5 ) 2 CHCOO] 2 . CALCIUM Methyl Ethyl ACETATE Ca[CH 3 (C 2 H 6 ).CHCOO] 2 . SOLUBILITY OF EACH IN WATER. (Landau Monatsh. Chem. 14, 717, '93; Keppish Ibid. 9, 600, '88; Sedlitzki Hid. 8, 573, '87-j Ca. Tri Methyl Acetate. Ca. Di Ethyl Acetate. Ca. Methyl Ethyl. Acetate. Gms. Ca(C 5 H 9 O 2 )2 Gms. Ca(C6H n O2) 2 Gms. ( :a(C5H 9 2 ) s 4 o per 100 Gms. per loo Gms. per loo Gms. Water. Solution. 'Water , Solution. Water. Solution. O 7-30 6.81 30-3 23.22 28.78 22-35 10 6.84 6.40 27.8 31 .71 24.07 20 6-54 6.14 25.6 20-38 33.76 25.23 30 6.40 6.01 23-7 19.16 34-92 25.89 40 6.44 6.05 22 .1 I8.IO 35-20 26.04 50 6.64 6.22 20-8 17.22 34.60 25-7I 60 6.86 6.42 19.9 16.60 33 .11 24.89 70 7.11 6-64 19.2 16.11 30-74 23.41 80 7-38 6.87 27.49 21 .56 CALCIUM Methyl Propyl ACETATE Ca[CH 3 (C 3 H 7 ).CHCOO],. CALCIUM (Di) Propyl ACETATE Ca[(C 3 H 7 ) 2 CHCOO] 2 . CALCIUM (Iso) Butyl ACETATE Ca[(CH 3 ) 2 CH(CH 2 ) 2 COO] 2 . SOLUBILITY OF EACH IN WATER. (Stiassny Monatsh. Chem. 12, 596, '91; Furth Ibid. 9. 313. '88; Konig Ibid. 15, 22, '94.) Ca. Methyl Propyl Acetate. Ca. Di Propyl Acetate. Ca. Iso Butyl Acetate. Gms. Ca(C 8 H 15 O 2 ) 2 per IPO Gms. Water. Solution. 9-57 8.73 8-35 7.19 6. ii Gms. Ca(C 6 H u O 2 )2 t o. per 100 Gms. Water. Solution. O 16.58 14.22 10 15.80 I3-65 20 15.14 13.15 30 I4.6l 12-75 40 14.21 12-45 50 J 3-94 12 .24 60 13-79 12.13 70 I3-78 12.12 80 13.89 12.20 90 7.71 6.71 5-77 5.09 4.84 4.14 3.98 $*$ 2-38 per iop Gms. Water. Solution. 7.48 6.96 6.38 5.99 5-66 5-36 5-3 1 5-04 3-25 2-44 1-65 5.68 6.41 1.62 5-04 5-37 6.02 7.51 6.98 8.97 8.23 10.79 9-74 CALCIUM BROMIDE CaBr 2 . SOLUBILITY IN WATER. (Kremers Pogg. Ann. 103, 65, '58; Etard Ann. chim. phys. [7] 2, 532, '94, gives results which yield an irregular curve and are evidently less accurate than those of Kremers.) Gms. CaBr 2 per TOO Gms. Gms. CaBr 2 per 100 Gms. Water. Solution. Water. Solution. ioi 50.5 34-2 185 65 22 O 10 20 25 I2 5 132 55-5 57.0 143 58-8 153 60.5 34-2 40 60 80 105 213 278 295 312 68.1 73-5 74-7 75-7 Density of saturated solution at 20 = 1.82. CALCIUM BUTTRATE 86 CALCIUM (Normal) BUTTEATE Ca[CH 3 (CH 2 ) 2 eOO] 2 .H 2 O. CALCIUM (Iso) BUTYRATE Ca[(CH 3 ) 2 CH.COO] 2 .sH 2 O. SOLUBILITY OF EACH IN WATER. (Lumsden J. Chem. Soc. 81, 355, '02; see also Chancel and Parmentier Compt. rend. 104, 474, '87; Deszathy Monatsh. Chem. 14, 251, '93, and also Hecht Liebig's Annalen 213, 72, '82, give results for the normal salt which are somewhat below those of Lumsden for the lower temperatures. SedHtzki Monatsh. Chem. 8, 566, '87, gives slightly different results for the iso salt.) Calcium Normal Butyrate. Calcium Iso Butyrate. Gms. Ca(C 4 H 7 2 ) 2 t . per 100 Gms. t. Gms. Ca(C 4 H 7 O 2 ) 2 per 100 Gms. Solid PttftM Water. Solution. Water. Solution. iDclSC. O 20 3i 16 .89 2O IO 16 .78 Ca(C 4 H 7 2 ) : , 5 H 2 10 19 .15 16 .08 20 22 40 18 30 fi 20 18 .20 J 5 39 30 23 .80 !9 23 ii 25 17 .72 15 5 40 25 .28 20 65 K 30 17 25 14 7i 60 28 40 22 .12 t( 40 16 .40 14 .09 62 28 .70 22 30 a 60 15 .15 J 3 .16 65 28 25 22 03 Ca(C 4 H 7 3 ) 2 .H,0 80 *4-95 13 .01 80 27 OO 21 .26 100 J 5 85 13 .69 100 26 .10 20 .69 M CALCIUM CAPROATE Ca[CH 3 (CH 2 ) 4 COO] 2 .H 2 O. CALCIUM 3 Methyl PENTANATE Ca[CH 3 .CH 2 .CH(CH 3 )CH,. COO] 2 . 3 H 2 0. CALCIUM CAPRYLATE Ca[CH 3 (CH 2 ) 6 COO] 2 .H 2 O. SOLUBILITY OF EACH IN WATER. (Lumsden; the Pentanate, Kulish Monatsh. Chem. 14, 566, '93; see also Keppish Ibid. 9, 594, '88, and Altschul Ibid. 17, 571, '96, for results on the Caproate.) Ca. Caproate. Gms. Ca(C6H u 2 ) 2 per 100 Gms. H 2 0. O 20 40 50 60 80 100 18 15 2 .23 2 2 , 2.10 2-15 2.30 2-57 Ca. 3 Methyl Pentanate. Gms. Ca(C5HnO 2 ) 2 per 100 Gms, Water. 12-33 I7.I8 18.99 18-73 17.71 *3-37 9-94 Solution. 10.98 14.66 J 5-97 I5-78 15.04 11.80 9.04 Ca. Caprylate. Gms. Ca(C 8 H 15 O 2 ) s per 100 Gms. H 2 0. . o-33 0.31 0.28 0.26 0.24 0.32 0.50 CALCIUM CARBONATE CaCO,. SOLUBILITY IN WATER, AS DETERMINED BY THE ELECTROLYTIC CONDUCTIVITY METHOD. (Holleman, Kohlrausch, and Rose Z. physik. Chem. 12, 129, 241, '93.) i liter solution contains o.oi gram CaCO 3 at 8.7, and 0.012 gram at 20. 87 CALCIUM BICARBONATE CALCIUM BICARBONATE Ca(HCO 3 ) 2 . SOLUBILITY IN WATER AT 15. Calcium carbonate in presence of water, free from and containing carbon dioxide, dissolves as the hydrogen carbonate. (Among the investigators who have reported results upon the solubility of calcium bicarbonate may be mentioned, Cossa Z. anal. Chem. 8, 145, '69; Schloesing Com pt. rend. 74, 1522, '72; Caro Arch. Pharm. [3] 4, 145, '74; Reid Proc. Roy. Soc. (Edin.) 15, 151, '87- '88^ Irving and Young J. Chem. " Ann. chim. phys. L'Orosi 19, 217, '96, ippear ot most interest and reliability are the following by Tread- well and Reuter Z. anorg. Chem. 07, 185, '96.) cc. CO 2 per 100 cc. Partial Pres- Gms. per 100 cc. Saturated Solution. sure of COa (o and 760 mm.). in mm. Hg. Free CO 2 . Ca(HC0 3 ) 2 . Ca."" 8.94 67.9 0.1574 0.1872 0.0462 6-O4 45-9 0.0863 0-1755 0-0433 5-45 41.4 0-0528 0.0394 2.18 16.6 0-0485 0-I540 0.0380 1.89 14.4 0-0347 0.1492 0.0368 1.72 13 .1 0.0243 0-I33 1 0.0329 o 79 6.0 O.OI45 o . i 249 0.0308 0.41 3- 1 0-0047 0.0821 O.O2O3 0-25 1.9 O.OO29 0-0595 O.OI47 0.08 0.6 0.0402 O.OO99 0.0385 0.0095 Therefore i liter sat. solution at 15 and o partial pressure of CO 2 contains 0.385 gram Ca(HCO 3 ) 2 . SOLUBILITY OF CALCIUM BICARBONATE IN AQUEOUS SODIUM CHLORIDE SOLUTION AT 15. (Tread well and Reuter.) The NaCl solution contained about 5 grams per liter, and was there- fore approximately T V normal. cc. CO 2 per 100 cc. Gaseous Phase (o and 760 mm.). 16.95 11-47 6.07 3-16 0.50 Partial Pres- sure of CO 2 in mm. Hg. 128.8 8 7 .2 46.1 24.0 3 * 3-4 Grams per 100 cc. Saturated Solution. Free CO 2 . Ca(HC0 3 ) 2 . Ca. 0.1325 0.2184 0-0539 O-IIOI 0.2143 0.0529 0.0235 0.1492 0.0368 0.0135 0.1183 0.0292 O.OO27 0-0739 O.Ol82 0.0003 0.0400 O-OI2I 0.0349 0.0086 0.0332 0.0082 CALCIUM BICARBONATE 88 SOLUBILITY OF CALCIUM BICARBONATE IN AQUEOUS SOLUTIONS op AMMONIUM NITRATE, SODIUM CHLORIDE AND OF SODIUM SULPHATE. (Cameron and Seidell J. Physic. Chem. 6, 50, '02; Berju and Kosminiko Landw. Vers. Stat. 60, 422, '04.) In NH4NG-3 Solutions at 18. Grams per Liter Solution. In NaCl Solutions at 25. Grams per Liter Solution. In Na2SO 4 Solutions at 24. Grams per Liter Solution. fHUNOs . Ca(HC0 3 ) 2 . NaCl. Ca(HC0 3 ) 2 . Na 2 S0 4 . Ca(HCO 3 ) 2 total. Ca(HCO 3 ) 2 . 0.210 O o . 1046 O 0.092 0.092 5 10 20 0.340 0.415 o-547 5 10 20 0.150 O.lSo 0.210 5 10 20 0-175 0.232 0.277 0-175 O.22O O.262 40 80 0.744 0.940 40 80 O.225 O-22O 40 80 0.332 0.4OO 0.307 0-347 100 150 2OO 0.215 0.192 0.170 100 200 0.432 0.510 O.6OO o-355 0.382 0.400 250 0.137 250 0.725 0-435 CALCIUM CHLORATE Ca(ClO 3 ) 2 .2H 2 O. 100 grams saturated aqueous solution contain 64.0 grams Ca(ClO 3 )L at 1 8. Density of solution is 1.729. (Mylius and Funk Ber. 30, 1718, '97.) CALCIUM CHLORIDE CaCl 2 . SOLUBILITY IN WATER. (Roozeboom Z. physik. Chem. 4, 42, '80; see also Mulder; Ditte Compt. rend. 92, 242, '81; Eng*' Ann. chim. physic. [6JI3, 381, '88; Etard Ibid. [7] 2, 532, '94.) Gms. CaCl 2 per $0. ioo Gms. Solid t>u<. t. Gms. CaCl 2 per ioo Gms. Solid Phase. Water. Solution. Water. Solution. 55 42 5 29. 8 Ice -f CaCl 2 .6H 2 O 60 I 3 6 .8 57 .8 CaCl 2 .2H 2 25 50 .0 33- 3 CaCl 2 .6H2O 70 141 7 58 .6 CaCl 2 . 2 H 2 O o 59 5 37- 3 CaCl 2 .6H 2 O 80 147 -0 59 -5 CaCl 2 .2H 2 O 10 65 .0 39- 4 CaCl 2 .6H 2 O 90 152 7 60 .6 CaCl 2 .2H 2 O 20 74 5 42. 7 CaCl 2 .6H2O IOO X 59 .0 61 4 CaCl 2 . 2 H 2 O 30.2 IO2 7 7 CaCl 2 .6H 2 O 1 20 *73 .0 63-4 CaCl 2 . 2 H 2 O 20 91 .0 47- 6 CaCl 2 . 4 H 2 Oa 140 191 .0 65 .6 CaCl 2 . 2 H 2 O 29.8 IOO .6 50. i ^H 2 O a -f .6H 2 O 160 222 5 69 O CaCl 2 . 2 H 2 40 IJ 5 3 53- 4 .4H 2 Oa 170 2 55 7 1 .8 CaCl 2 . 2 H 2 20 104 5 5 1 - i CaCl 2 4H 2 O ft J75-5 297 .0 74 .8] ! -r CaClz-ii^ 29.2 112 .8 53 wiH 2 O 6 + .6H 2 O 180 300 .0 75 .0 CaCl 2 .H 2 O 35 122 5 55 wtH 2 O8 200 3" .0 75 7 CaCl a .H2O 38-4 127 5 56 o ^H 2 0/3+CaCl 2 .2H 2 235 332 -O 76 .8 CaC^.HzO 45-3 130 .2 56 6 -4H2O a + CaCl 2 . 2 H2O 260 347 .0 77 .6 CaCl 2 .H 2 Density of saturated solution at o = 1.417. 1.367, at 15= 1.399* at l8 ' 8 9 CALCIUM CHLORIDE SOLUBILITY OF CALCIUM CHLORIDE IN AQUEOUS SOLUTIONS OP HYDROCHLORIC ACID AT o. (Engel Compt. rend. 104, 434, '87.) G. Mols. in Mgs. per 10 cc. Solution. *CaCl 2 . 92.7 83-7 77.1 66.25 53-75 HCl. O.O 9-1 16.0 29.25 43-45 36-25 63.5 20.3 95.0 Density of Solutions. 1.367 1-344 1.326 i .310 1.283 1.250 1.238 Grams per 100 cc. Solution. CaCl 2 . HCl. 5^45 O.O 46.45 3-32 42.80 5-83 3 6 -77 10.66 29.84 15.84 2O- 12 23-I5 II .29 34.62 SOLUBILITY OP MIXTURES OF CALCIUM CHLORIDE AND ALKALI CHLORIDES. (Mulder; Riidorff.) ioo grams H 2 O dissolve 63.5 grams CaCl 2 +4.9 grams KC1 at 7 (M) 100 grams H 2 O dissolve 57.6 grams CaCl 2 + 2.4 grams NaCl at 4 (M) ioo grams H 2 O dissolve 59.5 grams CaCl 2 +4.6 grams NaCl at 7(M) ioo grams H 2 O dissolve 72.6 grams CaCl 2 + 16.0 grams NaCl at i5(R) SOLUBILITY OF CALCIUM CHLORIDE IN AQUEOUS ALCOHOL AT ROOM TEMPERATURE. (Bodtker Z. physik. Chem. 22, 570, '97.) Solution Used. 15 Cms. CaCl 2 .6H 2 O + 20 cc. alcohol 15 Gms. CaCl 2 .6H 2 O + 20 cc. alcohol 15 Gms. CaCl 2 .6H 2 O + 20 cc. alcohol 15 Gms. CaCl 2 .6H 2 O + i Gm. CaCL Vol. per cent Alcohol. 9 2 -3 97-3 99-3 99-3 Gms. CaCl 2 1.430 1.409 1.429 1.529 Solution Used. 15 Gms. CaCl 2 .6H 2 O +20 cc. alcohol + 2 Gms. CaC^ " +3 " " +4 " " +5 " Vol. per cent Alcohol. " 3 Gms. CaCl 2 ."si* 1.561 1.590 1.641 1.709 SOLUBILITY OF CALCIUM CHLORIDE IN A SATURATED SOLUTION OP SUGAR AT 31.25. (Kohler Z. Ver. Zuckerind. 47, 447, '97.) ioo grams saturated solution contain 42.84 grams sugar + 25.25 grams CaCl 2 , or ioo grams water dissolve 135.1 grams sugar + 79.9 grams CaCl 2 . CALCIUM CITRATE Ca 3 (C 6 H 6 O 7 ) 2 . 4 H 2 O. SOLUBILITY IN WATER AND IN ALCOHOL AT 18 AND AT 25. (Partheil and Hiibner Archiv. Pharm. 241, 413, '03.) Solvent. Grams per ioo Water Alcohol (Sp. Gr. 0.8092 = 95%) 18. 0.08496 0.0065 2S- 0.0959 0-0089 CALCIUM OHROMATE 90 CALCIUM CHROMATE CaCrO 4 . SOLUBILITY OP THE SEVERAL HYDRATES IN WATER. (Mylius and Wrochem Wiss. Abh. p. t. Reichanstalt 3, 462, 'oo.) ft o Gms. CaCrO 4 per 100 Gms. Mols. CaCr0 4 Gms. CaCrO 4 per looGms. Mols.CaCrO 4 1 /-=; : > per 100 Mols. * ' Water. Solution. H 2 O. Solid Phase, a CaCrO 4 .2H 2 O. (Monoclinic.) O 17.3 14-75 2.0 18 16.68 14.3 1.93 20 16.6 14.22 i-93 30 16.5 13.89 1.85 45 14-3 I2 -53 J - 6 5 Solid Phase, /5 CaCrO 4 . 2 H 2 O (Rhombic.) O 18 40 O 18 25 40 00 75 100 10.9 9.8 11.5 10.3 ii. 6 10.4 Solid Phase, CaCrO 4 .H 2 O. 1.25 i-33 i-34 13.0 10.6 10. o 8-5 6.1 4.8 3-2 "5 9.6 9.1 7.8 5-7 4-6 50 22 0.98 O.7O 0.56 o-37 Water. Solution. per 100 o H 2 O. Solid Phase, CaCrO 4 .*H 2 O. 7-3 6.8 0.84 18 4-8 4-4 0.51 31 3-84 3-7 0-44 38.5 2.67 2.6 0.31 50 1-63 1.6 0.19 00 1-13 i.i 0.13 100 0.81 0.8 0.09 Solid Phase, CaCr0 4 . , 4-5 4-3 ' 0.52 18 2.32 2.27 0.27 3i 2.92 1.89 0.22 50 1. 12 I. II 0.13 00 0.83 0.82 O.II 70 0.80 0-79 O.O9 100 0.42 O.42 O.O5 Densities of the saturated solutions of the above several hydrates at 18 are: a CaCrO 4 .2H 2 O, 1.149; CaCrO 4 .2H 2 O, 1.105; CaCrO 4 .H 2 O, 1.096; CaCrO 4 .iH 2 O, 1.044; CaCrO 4 , 1.023. 100 cc. 29% alcohol dissolve 1.206 grams CaCrO 4 . 100 cc. 53% alcohol dissolve 0.88 gram CaCrO 4 . (Fresenius Z. anal. Chem. 30, 672, '91.) CALCIUM POTASSIUM FERROCYANIDE CaK 2 Fe(CN) 6 . 3 H 2 O. 100 parts H 2 O dissolve 0.125 part salt at 15, and 0.69 part at b. pt. (Kunheim and Zimmerman Dingt. polyt. J. 252, 478, '84.) CALCIUM FLUORIDE CaF 2 . i liter of saturated aqueous solution contains 0.016 gram CaF 2 at 1 8. Determined by the electrolytic method. (Kohlrausch Z. physik. Chem. 44. 197, '03.) CALCIUM FORMATE Ca(HCOO),. SOLUBILITY IN WATER. (Lumsden J. Chem. Soc. 81, 355, '02; see also Krasnicki Monatsh. Chem. 8, 597, '87.) Gms.Ca(HCOO) 2 ^^ per loo Gms. 4 Gms.Ca(HCOO) 2 per loo Gms. 20 40 Water. 16.15 16.60 17-05 Solution. 13.90 14.22 14.56 60 80 100 Water. I7-50 17-95 18.40 Solution. 14.89 15.22 15-53 9 i CALCIUM HEPTOATE CALCIUM HEPTOATE (Oenanthate) Ca[CH 3 (CH 2 ) 6 COO] 2 .H 2 O. SOLUBILITY IN WATER. (Lumsden J. Chem. Soc. 81, 355, '02; see also Landau Monatsh. Chem. 14, 712, '93; Altschul Ibid. 17, 575, '96.) t. o. 20. 40. 60. 80. ioo. G. Ca(C 7 H 13 O 2 ) 2 per i oo gms. solution 0.94 0.85 0.81 0.81 0.97 1.24 CALCIUM HYDROXIDE Ca(OH) ? . SOLUBILITY IN WATER. (Average curve from the results of Lamy Ann. chim. phys. [5] 14, 145, '78; Mahen Pharm. J. Trans [3] 14, S5, '83-84; Herzfeld Z. Ver Zuckerind. 34 820, '97, and Guthrie J. Soc. Chem. Ind. 20, 224, 'ox.) Grams per 100 Grams HjO. Grams, per TOO Grams H2O. Ca(OH) 2 . CaO. ' Ca(OH) 2 . CaO. ' o 0.185 0.140 50 0.128 0.097 10 0.176 0.133 60 0.116 0.088 20 0.165 0.125 70 '0.106 0.080 25 - I 59 0.120 80 0.094 0.071 30 o<1 53 0.116 90 0.085 0.064 40 0.141 0-.I07 100 0.077 0-058 SOLUBILITY QF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OP AMMONIUM CHLORIDE AT 25. (Noyes and Chapin Z. physik. Chem. 28, 520, '99.) Millimols per Liter. Grams per Liter of Saturated Solution. NH 4 C1. Ca(OH) 2 . NI^Cl. c7(OH) 2 = CaO. o.oo 20.22 o.oo 1-50 1.13 21.76 29.08 1-165 2.16 1.63 43-52 39-23 2.330 2.91 2.20 83-07 59-68 4.447 4-42 3-45 SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF CALCIUM CHLORIDE. (Zahorsky Z. anorg. Chem. 3, 41, '93; Lunge J. Soc. Chem. Ind. n, 882, '92.) Concentration Grams CaO Dissolved per 100 cc. Solvent at; of CaCb Solutions, Wt.%. O 5 10 15 20 25 30 * Indicates cases in which a precipitate of calcium oxychloride separated and thus removed some of the CaCl 2 from solution. The results in o% CaCl 2 solutions, i.e., in pure water, are high when compared with the average results given above. 4 20. 40. 00. 80. 100. c. 1374 .Il62 O .IO26 .0845 .0664 ,1370 .Il6o .1020 .0936 .0906 ,1661 o .1419 1313 1328 .1389 o 1993 .I78l .1706 .1736 o .1842 o .1857* .2249 o .22O4 2295 o 2325 .1661* o .3020* o .2989 3261 .3710 1630* .3680* .3664 .4122 .4922 CALCIUM HYDROXIDE 92 SOLUBILITY OP CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OP POTASSIUM CHLORIDE AND OF SODIUM CHLORIDE. (Cabot J. Soc. Chem. Ind. 16, 417, '97.) In KC1 Solutions. In NaCl Solutions. Gms. of the Chloride Gms. CaO per Liter at: Gms. CaO per Liter at: per Liter. o. 15- 99*. o. 15. 09. i. 3 6 1.31 635 .36 3 3 1 0-635 30 I .701 1.658 o .788 ] .813 703 0.969 60 I-72S 1.674 o .876 .824 I .004 120 I.7I8 i. 606 o .894 1 .86 .722 I.OI5 240 1.248 1.199 .617 37 .274 0.771 320 .054 0.929 0-583 SOLUBILITY OF LIME IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE ALONE AND CONTAINING SODIUM HYDROXIDE. (Margiet Bull. soc. chim. [3] 33, 631, '05.) G. NaCl per Liter Gms. CaO per Liter of Solution. G. NaCl. per Liter. W W Gms. CaO per Liter of Solution. Without o.8 9 .NaOH 4 .o 9 .NaOH NaOH. per Liter. per Liter. ithout aOH. o.8 9 .NaOH per Liter. 4.09.NaOH per Liter. O I 3 O .8 0.22 J 5o 65 I 25 0-44 5 I 4 9 175 .6 I .2 . . . 10 I .6 I .0 182 .6 I .2 25 I 7 I .1 225 4 I O . . . 50 I .8 I 25 250 3 9 75 I 9 I 4 0.55 300 .1 O 7 0.22 IOO I 85 I 4 SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF SODIUM HYDROXIDE. (d'Anselme Bull. soc. chim. [3] 29, 938, '03.) Concentration of NaOH: Grams CaO per Liter Sat. Solution at: Normality. Gms. per Liter N/ioo 0-4 N/2 5 1.6 N/i5 2.66 N/8 5-oo N/5 8.00 N/2 20-00 20. 50. 70. 100. 1.170 0.94 0.880 0.65 o-75 o-53 o-54 o-35 o-57 o-35 0.225 0.14 o 39 0.18 0-20 O-o6 O.II 0-04 0.05 O-OI O.II O-O2 o.oi trace 0.02 trace o.oo 0-00 For results upon mixtures of calcium hydroxide and alkali carbonates and hydroxides, see Bodlander Z. angew. Chem. 18, 1138, '05. 93 CALCIUM HYDROXIDE SOLUBILITY OF CALCIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF GLYCERINE AT 25" deter Arch. Phann. [3] 4, 558, '74.) (Herz and Knoch Z. anorg. Chem. 46, 193, '05; for older determinations, see Berthelot Ann. chim. phys. [3] 46, 176; and Carles , density of Solutions Wt. per cent Glycerine in Solution. MilUmols *Ca(OH) 2 per 100 cc. Solution. I .0003 .0244 o.o 4-3 8.13 0537 .0842 20-44 14.9 22.5 1137 1356 .2072 40.95 48.7 69.2 40.1 44.0 95-8 Gms. per 100 cc. Solution. Ca(OH) 2 = CaO. 0.1593 o.i 206 0.3013 O.228l 0.5522 0.4180 0-8339 0.6313 1.486 I.I25 1 1631 1.234 3-550 2.687 SOLUBILITY OF LIME IN AQUEOUS SOLUTIONS OF SUGAR. (Weisberg Bull. soc. chim. [3] 21, 775, '99.) The original results were plotted on cross-section paper and the following table constructed from the curves. ist series, t = i6'-i7. 2d, series t = 15. Gms. per Solu 100 Gms. tion. G. CaO per 100 Gms. Sugar in Sol. Gms. per 100 Gms. Solution. G, CaO per 100 Gms. Sugar in Sol. Sugar. CaO. Sugar. CaO. I 0.30 35- I 0.50 62.5 2 0-56 28. 7 2 0-75 36.0 3 0.85 28. o 3 1.02 32-5 4 I .12 27. 7 4 1.22 30.2 5 1.40 27. 5 5 i-45 28.5 6 1.65 27. 5 6 1.67 27.7 8 2.22 27. 5 8 2.22 27-5 10 2.77 27. 5 10 2-77 27-5 12 3-27 27. 5 12 3-27 27-5 14 3-85 27. 5 14 3-85 27-5 In the second series a very much larger excess of lime was used than in the first series. The author gives results in a subsequent paper, Bull. soc. chim. [3] 23, 740, 'oo, which show that the solubility is also affected by the condition of the calcium compound used, i.e., whether the oxide, hydrate, or milk of lime is added to the sugar solutions. CALCIUM IODATE 94 CALCIUM IODATE Ca(IO 3 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Mylius and Funk Ber. 30, 1724, '97; W. Abb. p. t. Reichanstalt 3, 448, 'oo.) Cms. Mols. Gms. Mols. t o Ca(I0 3 ) 2 Ca(10 3 ) 2 Solid t Ca(IO 3 ) 2 Ca(IO 3 ) 2 Solid per 100 per 100 Phase. ' per ioo per 100 Phase. Gms. Sol. Mols. H 2 O. Gms. Sol. Mols. H^. o o.io 0.0044 Ca(IO 3 ).6H 2 O 21 0.37 0.016 Ca(IO 3 ) 2 .H 2 O 10 0.17 0.0075 35 0-48 0.021 18 0.25 o.oii 40 0.52 0.023 30 0.42 0.019 45 0.54 0.024 40 0.61 0.027 50 0.59 0.026 50 0.89 0.040 60 0-65 0.029 54 1.04 0.046 80 0.79 0.034 60 1.36 0.063 " 100 0.94 0.042 " Density of solution saturated at 18 = i.oo. CALCIUM IODIDE CaI 2 . SOLUBILITY IN WATER. (Average curve from the results of Kremers Pogg. Ann. 103, 65, '58; Etard Ann. chim. phys. [7] 2, 532, '94-) . o Gms. CaI 2 per TOO t Gms. CaI 2 per 100 . Gms. CaI 2 per 100 Gms. Solution. Gms. Solution. Gms. Solution. o 64.6 30 69 80 78 10 66.0 40 70.8 loo 81 20 67.6 60 74 Density of solution saturated at 20 = 2.125. CALCIUM (Neutral) MALATE Ca(C 4 H 4 O 5 ).3H 2 O. CALCIUM (Acid) MALATE Ca(C 4 H 5 O 5 ) 2 .6H 2 O. CALCIUM MALONATE Ca(C 3 H 2 O 4 ).4H 2 O. SOLUBILITY OF EACH IN WATER. (Iwig and Hecht Liebig's Ann. 233. 167, '86; Cantoni and Basadonna Bull. soc. chim. [3] 35, 731, '06; the malonate, Miczynski Monatsh. Chem. 7, 261, '86.) Ca. Neutral Malate. Ca. Acid Malate. Ca. Malonate. Gms. Ca(C 4 H 4 O 5 ) per 100. Gms. Ca(C 4 H 5 O5)3 Gms. Ca(C 3 H 2 O 4 ) t. Gml G cTSoT . *** I0 ? Gms - . pP" 1 ^ HzO. Sol. (CandB). Water. Solution. Gms. H 2 O. o ... ... ... ... ... o . 290 10 0.85 0.84 1.8 1.77 0.330 20 0.82 0.81 0.907 1.5 1.48 0-365 30 0.78 0-77 0.835 2.0 1.96 0.396 40 0.74 0.73 0.816 5.2 4.94 0.422 50 0.66 0.65 0.809 15.0 13-09 0.443 57 0.57 0.56 32.24 24.29 60 0.58 0.58 0.804 26.0 20.64 0.460 70 0.63 0.63 0.795 II - 9-9 1 0.472 80 0.71 0.70 0.754 6.8 6.37 0.479 90 ... o . 740 SOLUBILITY OF CALCIUM MALATE IN WATER AND IN ALCOHOL. (Partheil and Hiibner Archiv. Pharm. 241, 413, '03.) ioo grams H 2 O dissolve 0.9214 gram CaC 4 H 4 O 5 .H 2 O at 18, and 0.8552 gram at 25. ioo grams 95% alcohol dissolve 0.0049 gram CaC 4 H 4 O c .H 2 O at 18, and 0.00586 gram at 25. 95 CALCIUM NITRATE CALCIUM NITRATE Ca(NO 3 ) 2 .2H 2 O. SOLUBILITY IN WATER AT 18. (Mylius and Funk Ber. 30, 1718, '97.) ioo grams saturated solution contain 54.8 grams Ca(NO 3 ) 2 . Density of solution, 1.548. CALCIUM OXALATE Ca(COO) 2 .H 2 O. SOLUBILITY IN WATER, BY ELECTROLYTIC CONDUCTIVITY METHOD. (Holleman, Kohlrausch, and Rose Z. physik. Chem. 12, 129, 241, '93; Richards, McCaffrey, and Bisbee Z. anorg. Chem. 28, 85, '01.) . Cms. CaC 2 O 4 per t o Cms. CaC 2 O 4 per Liter of Solution. Liter of Solution. 13 0.0067 (H) 25 0.0068 (R, McC and B) 18 0.0056 (K and R) 50 0.0095 24 0.0080 (H) 95 0.0140 " SOLUBILITY OF CALCIUM OXALATE IN AQUEOUS SOLUTIONS OF ACETIC ACID AT 26-27. (Herz and Muhs Ber. 36, 3715, '03.) Normality of Acetic Acid. G. CH 3 COOH per ioo cc. Sol. Residue from 50.052 cc. Solution. O-OO O.OOI7 0.58 3-48 O.OO48 2.89 J 7-34 0.0058 5-79 34-74 O.OOO4 The residues were dried at 70 C. CALCIUM OXIDE. See Calcium Hydroxide, p. 91. CALCIUM PHOSPHATE (Tribasic) Ca 3 (PO 4 ) 2 . SOLUBILITY IN WATER. The determinations of the solubility of this salt in water, as stated in the literature, are found to vary within rather wide limits, due, no doubt, to the fact that so-called tribasic calcium phosphate is apparently a solid solution of the dibasic salt and calcium oxide, and therefore analyses of individual samples may show an excess of either lime or phosphoric acid. When placed in contact with water, more PO 4 ions enter solution than Ca ions, the resulting solution being acid in reaction and the solid phase richer in lime than it was, previous to being added to the water. For material having a composition approximating closely that represented by the formula Ca 3 (PO 4 ) 2 the amount which is dissolved by CO 2 free water at the ordinary temperature, as cal- culated from the calcium determination, is o.oi to o.io gram per liter, depending upon the conditions of the experiment. Water saturated with CO 2 dissolves 0.15 to 0.30 gram per liter. A list of references to papers on this subject is given by Cameron and Hurst J. Am. Chem. Soc. 26, 903, '04; see also Cameron and Bell, Ibid. 27, 1512, '05. CALCIUM PHOSPHATE 96 CALCIUM PHOSPHATE (Dibasic) CaHPO 4 .2H a O. SOLUBILITY IN WATER. (Cameron and Seidell J. Am. Chem. Soc. 26, 1460, '04; see also Rindell Compt. rend. 134, ua, 'oa; Magnanini Gazz. chim. ital. 31, II, 544, *oi.) i liter of CO 2 free water dissolves 0.136 gram CaHPO 4 at 25. i liter of water sat. with CO 2 dissolves 0.561 gram CaHPO 4 at 25. SOLUBILITY OF Di CALCIUM PHOSPHATE AND OF MONO CALCIUM PHOS- PHATE IN AQUEOUS SOLUTIONS OF PHOSPHORIC ACID AT 25. (Cameron and Seidell J. Am. Chem. Soc. 27, 1508, '05; Causse Compt. rend. 114, 414, '92.) Grams per Liter of Solution. Gms. per Liter Calc. frOP 1 r*aO FminrT PzO 6 per Liter tt E combLe f d Solid Phase. CaO. F 2 Os. with Ca. I.7I 4.69 4.15 CaHPO 4 2-53 CaHP0 4 . 2 H 2 n-57 36.14 28.05 tt 21-5 (4 23 -3 1 75-95 56.53 tt 46.45 tt 39.81 139.6 97-oi tt 89.0 11 49.76 191.0 120.7 tt 128.0 If 59-40 234.6 144.1 tt J 59-4 ft 70-3 1 279.7 170.6 tl 190.7 tt 77.00 317.0 (174.2 (321.3 CaHP0 4 or CaH 4 (P0 4 ) 2 226.0 122 .2 CaHP0 4 .2H,0 CaH 4 (PO ) a .H, + 72.30 3S x "-9 301.6 CaH 4 (P0 4 ) 2 169.0 CaH 4 (P0 4 ) 2 .H 2 69.33 361 .1 289.3 tt 186.1 tt 59-98 419.7 250.2 11 267.9 tt 53-59 451 .7 223.7 it 316.1 tt 44-52 505-8 185.8 it 393-1 tt 39-89 538.3 166.4 it 437-4 " Density of the solution in contact with both salts at 25 = i. 29. SOLUBILITY OF Di CALCIUM PHOSPHATE IN AQUEOUS N/2oo SOLUTION OF ACID POTASSIUM TARTRATE AT 25. (Magnanini .) i liter of the solution contains 0.08 gram Ca = 0.235 gram CaHPO 4 . CALCIUM PHOSPHATE (Monobasic) CaH 4 (PO 4 ) 2 .H 2 O. SOLUBILITY IN WATER. This salt is stable in contact with the aqueous solution only when there is present free phosphoric acid to the extent indicated by the above table. CALCIUM PEL ARGON ATE (Nonate) Ca[CH 3 (CH 2 ) 7 COO] 2 .H 2 O. CALCIUM PROPIONATE Ca(CH 3 .CH 2 COO) 2 .H 2 O. SOLUBILITY OF EACH IN WATER. (Lumsden J. Chem. Soc. 81, 355, '02; Krasnicki Monatsh. Chem. 8, 597, '87.) Calcium Pelargonate. Grams t. Ca[CH 8 (CH 2 )7COO]2 per loo Grams H 2 O. o 0.16 20 0.14 40 0.13 60 0.12 80 0.15 90 0.18 100 . 26 Calcium Propionate. Grams Ca(CH 3 .CH 2 COO) 2 per 100 Grams. Water. Solution. 42.80 29.97 39.85 28.48 38.45 27.76 38.25 27.67 39.85 28.48 42.15 29.66 48.44 32-63 97 CALCIUM SELENATE CALCIUM SELENATE CaSeO 4 . SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 532, '94.) t. -i. +5. 20. 37. Gms. per ioo gms. sol. 7.4 7.3 7.6 6.8 The accuracy of these results appears questionable. 67. 5.1 CALCIUM SILICATE CaSiO 3 . SOLUBILITY IN WATER AND IN AQUEOUS SUGAR SOLUTIONS AT 17. (Weisberg Bull. soc. chim. [3] 15, 1097, '96.) The sample of calcium silicate was air dried. Grams per ioo cc. Saturated Solution. Solvent. Water 10% sugar sol. 20% sugar sol. At 17. After Boiling and Filtering Hot. CaO(det.) 0.0046 0.0065 0-0076 CaSiO 3 (calc.) 0.0095 0.0135 0.0157 CaO(det.) 0.0094 O-OI2O CaSiO s (calc.) 0.0195 O.O249 (JALCIUM SUCCINATE Ca(C 2 H 2 O 2 ) 2 . CALCIUM (Iso) SUCCINATE CaCH 3 .CHC 2 O 4 .H 2 O. SOLUBILITY OF EACH IN WATER. (Miczynski Monatsh. Chem. 7, 261, '86.) Calcium Succinate. Calcium Iso Succinate. t. Gms. Ca(C 2 H 2 2 ) 2 per ioo Gms. Gms. t o Ca(C 2 H 2 O 2 ) 2 ' per ioo Gms. Gms. t o Ca(C 2 H 2 2 ) 2 " per ioo Gms. Gms. t o Ca(C 2 H 2 2 ) 2 ' per ioo Gms. H 2 0. H 2 0. H 2 H 2 0. o I.I27 50 I .029 .522 50 O .440 10 I .220 60 O .894 10 O 524 60 o 396 20 I .276 70 O .770 20 o 5*7 70 342 40 I.I77 80 657 40 o 475 80 o 279 ioo cc. H 2 O dissolve 1.424 grams succinate (CaC 4 H 4 O 4 .H 2 O) at i8 t and 1.436 grams at 25. ioo cc. 95% alcohol dissolve 0.00136 gram succinate (CaC 4 H 4 O 4 . H 2 O) at 18, and 0.00136 gram at 25. (Partheil and Hubner Archiv. Pharm. 241, 413, '03.) CALCIUM SULPHATE CaSO 4 . 2 H 2 O. SOLUBILITY IN WATER. and Allen, also Euler Z. physik. Chem. 49, 313, '04. Determinations by the electrolytic conductivity method Holleman, Kohlrausch and Rose Z. physik. Chem. 12, 129, 241, '93.) Gms. CaSO 4 Millimols. Density of t o Gms. CaSO 4 Millimols Density of t. per ioo cc. Solution. per Liter. Solutions. per ioo cc. Solution. per Liter. Solutions. O 0-1759 12.926 I .00197 40 O .2097 15 413 O 99439 10 0.1928 14.177 I .00173 55 O .2009 14 .765 O ,98796 18 0.2016 14.817 I .00059 65 3 o .1932 14 2OO o ,98256 2 5 o . 2080 I5-295 O .99911 75 O .1847 13 575 o 97772 30 o . 2090 I5-36I O .99789 IOO O .1619 II .900 35 o . 2096 I5-405 .99789 107 II 390 CALCIUM SULPHATE 98 SOLUBILITY OP CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF HYDRO- CHLORIC, NITRIC, CHLOR ACETIC, AND FORMIC ACIDS. (Banthisch J. pr. Chem. 29, 52, '84; Lunge J. Soc. Chem. Ind. 4, 32, '85.) In Hydrochloric. In Nitric. In Chlor Acetic. In Formic. Grams Acid Grams CaSO 4 per per 100 cc. 100 cc. Sol. Gms. CaSO 4 per 100 cc. Solution Gms. CaSO 4 per 100 cc. Sol. Gms. CaSO 4 per zoo cc. Sol. Solution. at 25. at io2 6 . at 25. at 25. at 25. 0.208 0.160 0.208 O.2O8 0.208 I 0.72 1.38 0.56 . . . ... 2 I .02 2-38 0.82 3 1.25 3.20 1.02 4 1.42 3- 6 4 1.20 0.22 0.24 6 I.6 S 4-65 1.48 . . . 8 1-74 1.70 . . . 10 1.84 0.25 12 . . . ... I .08 ... SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF PHOS- PHORIC ACID AT 25. (Taber page 61, Bull. 33, Bureau of Soils U. S. Dept. Agr., 1906.) Gms. per Liter. o.o 5-o 10.5 21.4 46-3 CaS0 4 . 2.126 3- I 43 3-734 4-45 6 5.760 Sp. Gr. of Solutions at $f . 0.9991 Gms. per Liter. Sp. Gr. of Solutions at f . 1.106 P 2 5 . 145 - 1 CaSCV 7.920 1.002 205.0 8-383 I - I 45 1.007 I .Ol6 I -35 395-8 494.6 6.848 5-572 I .221 1.280 1-344 I -75 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF SUL- PHURIC ACID. (Cameron and Breazeale J. Physic. Chem. 7, 574, '03.) Grams H 2 SCu Results at 25. per Liter of Solution. Gms. CaSO 4 per Liter. Wt. of i cc. Sol. O .00 2 .126 0.9991 grams O .48 2 .128 0025 n 4 .87 2 .144 ] .OO26 a 8 .11 2 203 3 .0051 (i 16 .22 2 .382 "I .0098 u 48 .67 2 .727 .0302 (I 75 OO 2 .841 1-0435 It 97 35 2 779 ' [-0756 (I 146 .01 2 571 ft 194 .70 2 3*3 ] [.1134 11 243 35 I .901 1.1418 292 .02 I .541 1.1681 11 Results at 35. Gms. CaSO 4 per Liter. Results at 43. Gms. CaSO 4 per Liter. 2-145 2.209 2.236 2.451 2.456 2.760 3.II6 3-397 3-843 4.146 3.606 3-i5o 4-139 3-55 1 2-959 . - , 2.481 99 CALCIUM SULPHATE SOLUBILITY OP CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF AMMONIUM SALTS. (In NH^Cl and NH 4 NO3, Cameron and Brown J. Physic. Chem. 9, 210, '05 ; In (NH 4 ) 2 SO 4 at 25*, Sullivan J. Am. Chem. Soc. 27, 529, '05; In (NH 4 ) 2 SO 4 at 50, Bell and Tabor J. Physic. Chem. 10, 119, '06.) In NH 4 C1 In NH 4 NO 3 In NH 4 C1 In NH 4 NO 3 at 25. at 25. at 25. at 25. Cms. Ammo- G.CaSO 4 G. CaSO 4 nium Salt Dissolved Dissolved Gms. Ammo- G. CaSO 4 nium Salt Dissolved G. CaS0 4 Dissolved per Liter. per Liter. per Liter - per Liter. per Liter. per Liter. O 2 . 08 2 . 08 300 10.10 I0.8o 20 5-00 3.70 375 7-40 40 7-00 5-10 400 11-40 60 8.00 6.05 600 12.15 80 8.50 7-00 800 12.10 100 9.10 7.65 IOOO II.Sl 150 10.30 8.88 1400 IO-O2 200 10-85 9.85 sat. 7-55 In (NH 4 ) 2 SO 4 at 25. In (NH 4 ) 7 SO 4 at 50. Grams per Liter Sol. \vt. of 100 cc. Grams per Liter Sol. Sp. Gr. (NH 4 ) 2 S0 4 . CaS0 4 . Sat. Sol. (NH 4 ) 2 S0 4 . CaSO 4 . ' of Solutions. o-oo 0-208 99-91 o-oo 2.168 0.129 0-204 99-9I 15.65 1.609 .0026 0.258 0.199 99-92 30-67 1.750 .0113 0.821 0.181 99-95 91.6 2.542 .0440 1.643 0.166 99-99 160.4 3-402 .0819 3.287 0.154 100.10 221.6 4.068 .II08 6.575 0.144 100.34 340-6 5-084 1653 13.15 0.146 100.82 416.5 5-354 .1964 26.30 0.162 101.76 428.4 4-632 .2043 84.9 0.233 105.34 53O.8 2.152 1-2437 169.8 0.333 110.32 566.0 I .08 1.2508 339.6 0.450 H9-J5 566.7 o.oo 1.2510 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF CALCIUM SALTS AT 25. 1 J. Physic. Chem. 5, 643, '01; Seldell and Smith Ibid. 8, 493, '04; Cameron and Bell J. Am. Chem. Soc. 28, 1220, '06.) (Cameron and Seidell In Calcium Chloride. Grams per Liter Sol. In Calcium Nitrate. Gms. per Liter Sol. Wt. of In Calcium Hydroxide and vice versa. Gms. per Liter Sol. Solid CaCl 2 . ^ CaSO 4 . Ca(N0 3 ) 2 . CaSO 4 . r cc. Sol. CaO. CaS0 4 . Phase. o.oo 2 .06 O-O 2.08 O .998 O O 2 .126 CaS0 4 . 2 H 2 7-49 I .24 25 1.24 I 014 .062 2 .030 ** ii .96 I .18 50 1.20 I .032 O .176 I .918 M 25-77 I .10 100 I .13 I .067 O 349 I 853 M 32-05 I .08 2OO o-93 I 137 O .61 I. .722 (t 51-53 I .02 300 I .204 o 939 j 634 it 97.02 O .84 4OO o-57 I .265 I .222 I .588 1 CaS0..2lLO+ t Ca(OH). 192.71 47 500 0.40 I .328 I .242 I .214 Ca(OH), 280.30 o .20 544 o-35 I 352 I .150 .666 " 367-85 03 I .166 O .00 M CALCIUM SULPHATE 100 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS op MAGNESIUM CHLORIDE AND OF MAGNESIUM NITRATE AT 25. (Cameron, Seidell, and Smith.) In Magnesium Chloride. Grams per Liter of Sat. Solution. MgCl 2 . CaS0 4 . H 2 6. o.o 2.08 997-9 8.50 4.26 19.18 5.69 994-5 46.64 7-59 989.1 121.38 8.62 972.2 206.98 6-57 949-9 337-o 2-77 908.7 441.1 1.39 878.6 In Magnesium Nitrate. Gms. per Liter Sol. \y t. of i cc. >olution. Mg(N0 3 ) 2 . CaS0 4 .' o.o 2 . 08 O . 998 I 25 5-77 1.0205 50 7-88 1.0398 100 9 . 9 2 .0786 200 13-34 .1498 300 14.00 1 .2190 400 14.68 .2821 5*4 15.04 3553 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF MAG- NESIUM SULPHATE AT 25. (Cameron and Bell J. Physic. Chem. 10, 210, '06.) Grams per Liter Solution. MgS0 4 . CaSO 4 . 0-0 J 2.046 3-20 J .620 6-39 507 10.64 .471 21.36 .478 42.68 558 64.14 .608 85.67 : [.617 128.28 3 c .627 Sp. Gr. of Solutions at sf. 1.0032 1-0055 .0090 -OIl8 .O226 .0419 .0626 0833 .II9O Grams per Liter Solution. Sp. Gr. of MgS0 4 . 149.67 l6 5-7 CaS0 4 . i-597 1-549 Solutions at i I-I377 I. 1479 171 .2 198.8 1.474 i .422 I - I 537 1.1813 232.1 265.6 298.0 330-6 1.254 1.070 0.860 0.647 1.2095 1.2382 i .2624 1.2877 355-o 0.501 1-3023 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF POTAS- SIUM CHLORIDE, BROMIDE, AND IODIDE AT 21. (Ditte Ann. chim. phys. [7] 14, 294, '98.) In KC1 Solutions. In KBr Solutions. In KJ Solutions. Grams of the Potassium Salt per Liter. Gms. CaSO 4 per Liter. O 10 2.05 3-6 20 40 60 4-5 5-8 6.6 80 7-2 100 I2 5 7-5 double salt 200 250 300 Gms. CaSO 4 per Liter. 2.05 3-i 3-6 4-5 5- 2 5-9 6-3 6.7 7-o 7-3 double salt Gms. CaSO 4 per Liter. 2.O5 2.8 3- 2 3-9 4-5 4-85 5- 1 5-45 5-8 5-95 6.00 double salt 101 CALCIUM SULPHATE SOLUBILITY OP CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF POTAS- SIUM NITRATE AND OF POTASSIUM SULPHATE AT 25. (Seidell and Smith J. Physic. Chem. 8, 493, '04; Cameron and Breazeale 7Wd.8, 335, '04.) In Potassium Nitrate. In Potassium Sulphate. Gms. per Liter Solution. Wt.of ice. Solution. KN0 3 . CaS0 4 . o-o 2.08 0.9981 12-5 3.28 I .0081 25.0 4-08 I.OI54 50.0 5.26 I.032I ioo. o 6.86 I .0625 150 7.91 1.0924 200 8.69 I .1224 260 syngenite I-I539 Gms. per Solutior " ter v ft. of i cc. Solution K 2 S0 4 . ( : a so 4 . 0-0 J z.o8 < 5.9981 4.88 .60 3 .0036 5-09 .56 ] .0038 9-85 45 J .0075 19-57 49 .0151 28-35 55 J .0229 30-66 57 .0236 32-47 .58* * Solid phase syngenite. Results for the solubility of syngenite in solutions of potassium sulphate are also given in the original paper. SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE AT 26. (Cameron J. Physic. Chem. 5, 5 phys. chem. Ges. 37. 949. '02 372, '03.) Grams per ioo cc. Solution. [56, '01; see this pa] ; Cloez Bull, soc Wt. of i cc. Solution. 0.9998 I . 0644 1.0981 I .IOI2 >er for references to other work, a . chim. [3] 29, 167, '03; d'Anse Grams per ioo cc. Solution. IsoOrloff T.russ- Ime Ibid. [3] 29* Wt.of ice. Solution. 1.1196 I.I488 I.I707 1.2034 NaCl. 0-00 9-II5 14-399 14.834 CaSO 4 . O.2I2I 0.666 0.718 0.716 ' NaCl. 17.650 22.876 26.417 32.049 CaS0 4 . ' 0.712 0.679 0-650 0.572 SOLUBILITY OF MIXTURES OF CALCIUM SULPHATE AND CALCIUM CAR- BONATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE AT 23. (Cameron and Seidell J. Physic. Chem. 5, 643, '01.) Grams per Liter Solution. Grams per Liter Solution. NaCl. Ca(HC0 3 ) 2 . CaSO 4 . o.oo 0.060 1-930 3-63 0.072 2.720 11.49 0-089 3-446 39.62 O-IOI 5-I56 NaCl. Ca(HC0 3 ) 2 . CaSO 4 . 79-52 O.o6o 6.424 121 .90 0.056 5.272 193.80 0-048 4-786 267 .60 O.O4O 4.462 SOLUBILITY OF MIXTURES OF CALCIUM SULPHATE AND SILVER SUL- PHATE IN WATER. (Euler Z. physik. Chem. 49, 313. '04.) ... Per Liter of Solution. Total Salt per ioo Gms. Solution. Sp. Gr. of Solutions. Gms. Salt. Gms. Equiv. Salt. ^ojCaSO, 2.31 7-235 0-034 0-0464 Q-9473 1.0083 jCaS0 4 25 Ug 8 S0 4 2.61 8. ii 0.0383 O.O52O 1.062 1. 010 CALCIUM SULPHATE 102 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SOLUTIONS OF SODIUM NITRATE AND OF SODIUM SULPHATE AT 25. (Seidell, Smith, Cameron, Breazeale.) In Sodium Nitrate. In Sodium Sulphate. Grams per Liter Solution. \\TJ of i cc Grams per Liter Solution. \Vt. of i cc. NaNO 3 . CaSO 4 . Solution. Na;zSO 4 . CaSO 4 . Solution. o 2.08 0.9981 2.39 1.65 1.0013 25 4.25 1.0163 9.54 1-45 1.0076 So 5-50 1-0340 14-13 J -39 1-0115 ioo 7.10 1.0684 24.37 1.47 1.0205 2OO 8.79 1.1336 46.I5 1-65 I.O39I 300 9.28 1.1916 115.08 2.10 1-0965 600 7.89 i-3 6 39 146.61 2.23 1.1427 655 7.24 L3904 257.10 2.65 1. 2120 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS AND ALCOHOLIC MONO POTASSIUM TARTRATE SOLUTIONS AT 20. (Magnanini Gazz. chim.ital.3i, II, 544, '.) Gms. CaSO 4 Gms. CaSO. 4 Solvent. per ioo Gms. Solvent. per ioo Gms. Solution. Solution Water 0.2238 10% alcoholic N/ 2 oo KHC 2 H 4 O 6 0.0866 Aq. N/200 KHC 4 H 4 O. o . 2323 Aq. N/2OO KHC 2 H 4 O 6 + 5% 10 per cent alcohol 0.0970 tartaric ac. 0.2566 10% ale. N/400 KHC^Os + 5% tartaric ac. 0.1086 SOLUBILITY OF CALCIUM SULPHATE IN AQUEOUS SUGAR SOLUTIONS. (Stolle Z. Ver. Zuckerind. 50, 331, 'oo.) Per cent Concen- Grams CaSO 4 Dissolved by i Liter of the Sugar Solutions at: tration of Sugar Solutions. O 10 20 27 35 42 49 55 CALCIUM SULPHIDE CaS. SOLUBILITY IN AQUEOUS SUGAR SOLUTIONS. (Stolle.) r 30. 40. 50. 60. 70. 80. 2 J 57 i 730 ' i 730 i .652 i ,710 2 .041 I 730 i 730 i 574 i 574 i ,613 I .808 I .652 i .419 i .380 i .419 i .263 I 550 I 438 i .361 i -283 i .283 972 I .263 I 050 i .088 i .108 .914 I .030 777 o .816 855 o .729 564 739 o 5 6 4 .603 o 486 .486 505 .486 3 6 9 0.330 Per cent Concen- Grams CaS Dissolved per Liter of the JL Sugar Solutions at: tration ot ougar f Solutions. 30. 4 o. 50. 60. 70. 80. 90. O i .982 2 .123 I 235 I 390 I .696 2.032 2.496 10 i .866 1.316 I .441 I 673 I .560 1.634 1-544 20 2 .187 1.696 I .802 I 905 I .879 1.892 1.930 27 2 522 2.097 2 059 a .226 2 342 2.304 2-357 35 2 .689 2.265 2 304 2 .406 2 342 2-857 2-947 42 2 342 2.136 2 .226 2 .522 2 574 2.509 2.689 49 2 445 2.290 2 458 2 .638 2 .728 2.818 3-063 55 2 509 2 .226 2 "340 2 .882 2 .766 2.972 3.616 103 CALCIUM SULPHITE CALCIUM SULPHITE CaSO,. SOLUBILITY IN WATER AND IN AQUEOUS SUGAR SOLUTIONS AT 18. (Weisberg Bull. soc. chim. [3] 15, 1097, '96.) Grams CaSO 3 per 100 cc. Solution. Solent. ' . R0 After Boiling Solution 2 Hours. Water 0.0043 10 Per cent Sugar 0-0083 0.0066 30 Per cent Sugar o . 0080 o . 0069 CALCIUM TARTRATE CaC 4 H 4 O 6 .4H 2 O. SOLUBILITY IN WATER. (Cantoni and Zachoder Bull. soc. chim. [3] 33, 747, '05.) t o Gms. CaC 4 H 4 O 6 .4HjO t o Gms. CaC^Qj -411,0 t o Gms. CaC^Oa.^sO per 100 cc. Sol. per 100 cc. Sol. per 100 cc. Sol. o 0.0365 30 0.0631 70 0.1430 10 0.0401 40 0-0875 80 0.1798 20 0.0475 5 o.noo 85 0.2190 25 0.0525 60 0.1262 ioo gins. aq. Ca. tartrate solution contain 0.0185 g. CaC 4 H 4 O 6 .4H 2 O at 18, and 0.029489 at 25. ioo gms. 95% alcohol solution contain 0.0187 g. CaC 4 H 4 O 6 .4H 2 O at l8, and 0.02352 at 25. (Partheil and Hiibner Archiv. Pharm. 241, 413, '03.) ioo gms. aq. Ca. tartrate solution contain 0.0364 g. CaC 4 H 4 O 6 at 20. ioo gms. 10% alcohol solution contain 0.0160 g. CaC 4 H 4 O 6 at 20. ioo gms. 10% alcohol 4- 5% tartaric acid solution contain 0.1632 g. CaC 4 H 4 O 6 at 20 . (Magnanini Gazz. chim. ital. 31, II, 544, '01.) SOLUBILITY OF CALCIUM TARTRATE IN AQUEOUS ACETIC ACID SOLUTIONS AT 26-27. (Herz and Muhs Ber. 36, 3715, '03; see also Enell Pharm. Centrallh. 38, 181; Z. anal. Chem. 38, 368, '99.) Normality of Gms.CH 3 COOH Residue from Normality of Gms.CH 3 COOH Residue from Acetic Acid. per ioo cc. Sol. 50x552 cc. Sol. Acetic Acid, per ioo cc. Sol. 50.052 cc. Sol. o o 0.0217 3 .80 22.80 0.2042 0.57 3.42 0.1082 5.70 34-20 0.1844 I -42$ 8.55 0.1635 10.09 60.54 0.1160 2.85 17.10 0.1970 16.505 93.03 0.0337 The residue was dried at 70 C. CALCIUM BITARTRATE CaH 2 (C 4 H 4 O 6 ) 2 . SOLUBILITY IN WATER AND IN AQUEOUS SOLUTIONS OF ACIDS AND OF SALTS. (Warington J. Chem. Soc. 28, 946, '75.) In Hydrochloric Acid. In other Acids and in Salt Solutions at 14. CO Gms f p?r CI G.n Acid or Salt Gms. Acid or Salt Gms. CaH 2 (C 4 H 4 O 6 ) a ioo Gms. Sol. "At 22. ' At So / ^ I0 C ' S L *** IO CC - SoL o 0.600 4.027 Acetic Acid 0.81 0.422 0.68 3-01 5-35 Tartaric Acid 1.03 0.322 2.15 6.88 n-35 Citric Acid 0.84 0.546 4.26 11.19 20.23 Sulphuric Acid 0.685 1.701 8.36 22.75 4 -93 Hydrochloric Acid 0.504 1-947 16.13 48-31 80.12 Nitric Acid 0.845 1.969 Potassium Acetate i . 387 o . 744 Potassium Citrate 1.397 0.843 CALCIUM VALERATE 104 CALCIUM VALERATE Ca[CH 3 (CH 2 ) 3 COO] 2 .H 2 O. CALCIUM (Iso) VALERATE Ca[(CH 3 ) 2 .CH.CH 2 .COO] 2 . 3 H 2 O. SOLUBILITY OP EACH IN WATER. (Lumsden T. Chem. Soc. 81. 355, '02: see also Furth Monatsh. Chem. 9, 313, '88; Sedlitzky /Wd,8, 566, '87.) Calcium Valerate. Gms. Ca(C5H 8 C>2)2 t* per TOO Gms. 40. Calcium Iso Valerate. Gms. Ca(C 5 H 9 2 ) 2 ... per 100. Gms. Solid Water. Solution. Water. Solution. O 9 .82 8 94 26 05 20 .66 Ca(C 5 H 9 O 2 ) 2 . 10 9 25 8 47 10 22.7O 18 5 20 8 .80 8 .09 2O 21 .80 17 .90 30 8 .40 7 75 30 21 .68 17 .82 40 8 05 7 45 40 22 .00 18 .18 50 7 85 7 .28 45-5 22 35 18 .42 " 57 7 75 7 .19 50 19 95 16 .63 Ca(C 5 H 9 2 ) 2 . 60 7 .78 7 .22 60 18 38 15 52 70 7 .80 7 .24 70 17 .40 14 .82 80 7 95 7 36 80 16 .88 14 44 " 90 8 .20 7 58 90 16 65 14 .28 100 8 .78 8 .07 100 16 55 14 .20 CAOUTCHOUC. SOLUBILITY IN ORGANIC SOLVENTS. (Hanausek J. pharm. chim. [5] 15, 509, '87.) Grams. Caoutchouc Dissolved per 100 Gms. Solvent. Ceara. Tete Noire. Sierra Leone. 2-5 3-6 4-5 4-5 5-o 4.6 3-o 3-7 3 - i .5 4-5 4-0 4-4 5- 4-7 0.4 o.o o.o Solvent. Ether Turpentine Chloroform Petroleum Benzene Carbon Bisulphide CAMPHORIC ACID C 8 H 14 (COOH) 2 . 100 grams of water dissolve 0.8 gram C 8 H 14 (COOH) 2 at 25, and 10 grams at the b. pt. (U.S. P.) CARBAZOLE (Di Phenylene imid) (C 6 H 4 ) 2 NH. 100 grams abs. alcohol dissolve 0.92 gms. (C 6 H 4 ) 2 NH at 14, and 3.88 grams at b. pt. 100 grams toluene dissolve 0.55 gm. (C 6 H 4 ) 2 NH at 16.5, and 5.46 grams at b. pt. CARBAMIDES. * SOLUBILITY IN SEVERAL SOLVENTS. as Methyl Phenyl Carbamide (m. pt. 82), Benzyl Carbamide (m. pt. 149). o Tolyl Carbamide(m.pt. 185) and Tolyl Carbamide (m.pt. 173). (Walker and Wood J. Chem. Soc. 73, 626, '08.) Grams Carbamide per 100 cc. Sat. Solution. aoivem. i as Methyl Phenyl. Benzyl. P Tolyl. Tolyl. Water 45 74 j 71 O 307 o .251 Acetone 23 29. 4 3 .10 2 .66 O .462 Ether 22 5 2 . 28 o 053 .062 O .Ol62 Benzene 44 .2 12 . 4 0597 O 043 0155 CARBON DIOXIDE V . 3. ft. i. 0-335 1 -7*3 5 0.277 1.424 10 0.231 1.194 15 0.197 i .019 1.070 20 0.169 0.878 . . . 25 0.145 0-759 0.826 30 0.126 0.665 40 0.097 0-530 50 0.076 0.436 60 0.058 0-359 In 17.62% NaCl. CARBON DIOXIDE CO 2 . SOLUBILITY IN WATER AND IN AQUEOUS SODIUM CHLORIDE SOLUTIONS. (Bohr Wied. Ann. Physik. [3] 68, 303, '99; Geffcken Z.physik.Chem. 49, 271, '04; Just Ibid. 37, 354, *oi-) Solubility in Water. ^tci^ "ft. 0.675 0-577 0-503 0.442 o-393 0-352 0.319 0.263 0-235 ft. 1.234 1.024 0.875 o-755 0.664 0-583 0-5*7 0.414 0.370 0-305 183 q *= wt. of gas dissolved by i oo grams of solvent at a total pressure of 7 60 mm. p = the Bunsen Absorption Coefficient which signifies the volume (v) of the gas (reduced to o and 760 mm.) taken up by unit volume (V) of the liquid when the pressure of the gas itself minus the vapor tension of the solvent is 760 mm. _ v * = V(i + 0.00367 i) ' I = the Ostwald Solubility Expression which represents the ratio of the volume (v) of gas absorbed at any pressure and temperature, to the volume (V) of the absorbing liquid, i.e. / = p This expression differs from the Bunsen Absorption Coefficient, p, in that the volume (v) of the dissolved gas is not reduced to o and 760 mm. The solubility / is therefore the volume of gas dissolved by unit volume of the solvent at the temperature of the experiment. The two expressions are related thus: / = p (i + 0.00367 /), p = - ; . (i + 0.00367 /) SOLUBILITY IN WATER AT PRESSURES ABOVE ONE ATMOSPHERE. (Wroblewski Compt. rend. 94, 1335, '82.) ^Pressure in Atrnos- Coefficient of Saturation * at: Pressure in Atmos- Coefficient of Saturation * at : pheres. - 12.4. pheres. o . 12.4. I 1-797 I .086 2O 21 65 17.11 5 8.65 5 .15 25 30 55 20.31 10 16.03 9 65 30 33 74 23-25 * Coefficient of Absorption is no doubt intended. SOLUBILITY OP CO 2 IN AQUEOUS SOLUTIONS OP ACIDS AND SALTS (Geffcken.) Aq. Cms Acid C0 2 Dissolved, / at: Aq. Cms Salt COa Dissolved, / at: Solvent. per Liter. 15. 25. Solvent. per Liter. 15. 25 HC1 18 23 043 0.8o6 CsCl 8 4 17 I .006 O .781 " 36 .46 .028 o-799 KC1 37 30 .976 759 (4 72 .92 coo o-795 KC1 74 .60 O .897 .700 HNO S 3i 52 .078 0.840 KI 83 .06 .992 775 * 63 .086 0-853 KI 166 .12 923 727 " 126 .10 .100 0.877 KBr 59 55 .986 o .768 H0 t 24 5 2 .018 0.794 KBr 119 .11 .914 7i3 tt 49 .04 0.978 0.770 KN0 3 50 59 ' I 005 .784 tt 98 .08 0-917 0.730 KNO 3 IOI .19 946 o 749 t( 147 .11 0.870 0.698 RbCl 60 47 .989 o .769 tt 196 .15 0.828 0.667 RbCl 120 95 o .921 o .788 CARBON DIOXIDE 106 SOLUBILITY IN AQUEOUS SOLUTIONS OP SALTS. (Mackenzie Wied. Ann. Physik. [2] i, 450, '77.) Salt in Solution. Gms. Salt per zoo Gms. Solution. Density of Solution 15. Absorption Coefficient a at: ' 8. i S . 22 r KC1 6.05 I .021 0.988 0.777 0.670 it 8.646 1-053 0.918 0.777 0.649 " 11.974 I .080 0.864 0.720 0.597 " 22 .506 1-549 0-688 0.571 0.480 NaCl 7-062 1.038 0-899(6.4) 0-735 M 12.995 1.080 0-633(6.4) 0.557 0.482 " 17.42 1.123 0.518(6.4) 0.431 0.389 " 26.00 0-347(6-4) 0-297 0.263 NH 4 C1 6.465 1. 021 1.023 0-825 0.718 " 8.723 1-047 i .000 0.791 0.702 " 12.727 1-053 0.922 0.798 0.684 " 24-233 1.072 0.813(10) 0.738 0.600 8. l6.S. 22. 30. BaCI, 7.316 i. 068 0-969 O-744 O-68O 0.566 " 9-753 i .092 I- O2 I O.645 O.6O7 0.543 " 14.030 i .137 0.618 0.524 0.467 u 25 215 1.273 0.495 0-618 0.383 0.315 SrCL, 9-5 11 1.087 0.779 0-663 0.581 0.508 tt 12-325 1.1159 o-737 0.586 0.507 0.539 tl I7-7I3 i .173 0-606 0.473 0.444 0.367 11 3 I - I 94 1-343 0.285 0.245 0.247 0.223 CaCL, 4-365 1.036 0-942 0-759 0.673 0.596 " 5-739 1.049 0-855 0.726 0-616 0.527 H 8.045 i. 068 0-838 0-674 0.581 0.500 " 15-793 I - I 39 0.632 0.520 0.471 0.400 SOLUBILITY OF CARBON DIOXIDE IN ALCOHOL. (Bohr Wied. Ann. Physik [4] i, 247, 'oo.) In 99 per cent Alcohol. In 98.7 per cent Alcohol. cc. CC>2 (at o and 760 mm.) per i cc. cc. CO2 (at o and 760 mm.) per i cc. Alcohol. Sat. Solution. Alcohol. Sat. Solution. -65 38-41 35-93 39.89 37.22 2O 7-5i 7.41 7-25 7.16 10 5-75 5-69 5-43 5-38 o 4-44 4.40 4-35 4-3i + 10 3-57 3-55 20 2.98 2 .96 25 2.76 2-74 30 2-57 2.56 ... ... 40 2.20 2 .19 45 2.01 2.00 ... ... 107 CARBON DIOXIDE SOLUBILITY IN AQUEOUS ALCOHOL AT 20. (Muller Wied. Ann. Physik. [2] 37t 39. '89; Lubarsch Ibid. [2] 37, 525, '89.) Density of Per cent Alcohol Abs. Coef. Density of Per cent Alec Alcohol. By Wt. Of CO2, *. Alcohol. By Wt. 0-998 1.07 0.861 0.922 49-o 0-969 22 .76 0.841 0-870(18.8) 71.1 0-960 (22.4) 28.46 0.792 0.835(16) 85-3 0.956 3 I - I 7 0.801 o-79S to ) 99-7 0-935(17) 42.15 0.877 Of C0 2) a. 0.982 1.293 1-974 2.719 SOLUBILITY OF CARBON DIOXIDE IN ORGANIC SOLVENTS. (Just Z. physik. Chem. 37t 354. *oi.) Sol . of CO 2 , Ostwald Expression * Sol . of CO 2 , Ostwald Expression * Solvent. > Solvent. aoiveni. IK- ISO- /15- /26- fe. /i*. CS 2 .870 .889 945 C 3 H 7 OH 2 .498 C.H.NH, I 324 1 434 i 531 C 2 H 5 OH( 95 %) 2 -706 2 923 3-I30 C.HUOH I 8 3 I i .941 2 .058 C 6 H 5 COH .841 3 057 3-304 C 6 H 5 Br I .842 i .964 2 .092 CHClg 3 -430 3 .681 3-958 CC1 4 2 .294 2 .502 2 .603 CH 3 OH 3 837 4 .205 4-606 G^CEt, 2 305 2 .426 2 , 557 CHjCOOH 4 691 5 .129 5.614 C.H. 2 425 2 540 2 . 716 (CH 3 CO) 2 5 .206 5 .720 6.18 C.H.NO, 2 45 6 2 655 2 . 845 (CH 3 ) 2 CO 6 295 6 .921 * See p. 105. Determinations are also given for the solubility in glycerine, iod benzene, o and m toluidine, eugenol, benzene tri chloride, cumol, carvene, di chlor hydrine, iso butyl alcohol, benzyl chloride, meta xylol, ethylene bromide, chlor benzene, propylene bromide, amyl bromide, carvol, amyl chloride, iso butyl chloride, butyric acid, ethylene chloride, pyridine, amyl formate, propionic acid, amyl acetate, iso butyl acetate, and in methyl acetate. See Woukoloff Compt. rend. 108, 674; 109, 62, '89, for the solubility of CO 2 in CS 2 and CHC1 3 at different pressures. CARBON MONOXIDE CO. SOLUBILITY IN WATER. (Winkler Ber. 34, 1416, '01.) t. ft, "Absorp, Coef." . * 1', " Solu- bility." t. /3 , "Absorp. Coef." ft :', "Solu- bility." 9- o 0-03537 0.03516 .0044 40 01775 01647 0.0021 5 0.03149 O .03122 O 0039 50 .01615 O .OI42O 0-OOlS 10 O.O28l6 O .02782 o 0035 60 O .01488 O OII97 O.OOI5 15 0.02543 o .02501 .0031 70 o .OI44O o 00998 O.OOI3 20 0-02319 o .O2266 o .0028 80 o 01430 o .00762 O-OOIO 25 0.02142 o .02076 .0026 90 o .OI42O .00438 0.0006 30 0.01998 o .01915 o .0024 100 .01410 o OOOOO o.oooo /? = vol. of CO absorbed by i volume of the liquid at a partial pres- sure of 760 mm. See page 105. /8' = vol. of CO (reduced to o and 760 mm.) absorbed by i volume of the liquid under a total pressure of 760 mm. q = grams of CO dissolved by 100 grams H 2 O at a total pressure of 760 mm. CARBON MONOXIDE 1 08 SOLUBILITY OF CARBON MONOXIDE IN AQUEOUS ALCOHOL SOLUTIONS AT 20 AND 760 MM. PRESSURE. (Lubarsch Wied. Annalen Physik. [2] 37, 525, '89.) Wt.% Alcohol. Vol.% Absorbed CO. Wt.% Alcohol. Vol. % Absorbed CO. o-oo 9-09 16.67 23.08 2.41 1-87 J-75 1.68 28.57 33-33 50.00 1.50 !-94 3.20 SOLUBILITY OP CARBON MONOXIDE IN ORGANIC SOLVENTS. (Just Z. physik. Chem. 37, 361, 'or.) Results in terms of the Ostwald Solubility Expression, see p. 105. Solvent. /25. /20. Solvent. /25. / 20- Water . 02404 .02586 Toluene 0. 1808 0. 1742 Anilin 05358 o 555 Ethyl Alcohol 0. 1921 0. IOOI Carbon Bisulphide .08314 .08112 Chloroform 0. 1954 o. 1897 Nitro Benzene .09366 .09105 Methyl Alcohol 0. 1955 0. 1830 Benzene o .1707 o .1645 Amylacetate o. 2140 o. 2108 Acetic Acid .1714 .1689 Acetone 0. 2225 0. 2128 Amyl Alcohol .1714 o. 1706 Iso Butyl Acetate 0. 2365 0. 2314 Xylene o .1781 1744 Ethyl Acetate 0. 2516 0. 2419 ioo volumes of petroleum absorb 12.3 vols. CO at 20, and 13.4 vols. at 10. (Guiewasz and Walfisz Z. physik. Chem. I, 70, '87.) SOLUBILITY OP CARBON MONOXIDE IN MIXTURES OF ACETIC ACID AND OTHER SOLVENTS AT 25. (Skirrow Z. physik. Chem. 41, 148, '02.) Results in terms of the Ostwald Solubility Expression, see p. 105. Mixture of Acetic Ac. and /< 7 V^AJ. inM ixture. CO. ! ' By Wt. By Vof. Anilin IOO .0 IOO .0 o 173 tt 86 5 90 .8 .110 " 58 3 68 5 o .070 " 13 .8 25 .1 o .058 " o O 053 Benzene 67 5 63 4 o .199 tt 33 .6 29 .6 .198 tt 19 .2 16 5 .190 " .0 o o .174 Mixture of Acetic Ac. and : % CH 3 COOH in Mixture. CO. ByWt. By Vol. Chloroform 56 4 64 .5 o .196 11 O .0 .0 .206 Nitro Benzene 88 4 84 .8 o .156 tt 49 .0 66 3 .130 tt o .0 .0 093 Toluene 74 7 7i .0 .191 tt 56 9 52 .6 195 fl 20 5 17 .8 o .190 tt .0 .182 109 CARBON MONOXIDE SOLUBILITY OP CARBON MONOXIDE IN MIXTURES OF ACETONE AND OTHER SOLVENTS AT 25. (Skirrow.) Mixture of %(CH 3 ) 2 CO in Mixture. CO. Acetone and: By Wt. By Vol. fcs- Mixture of Acetone and: %(CH 3 ) 2 CO in Mixture. CO. 7_. By Wt. By Vol. '"' Anilin 100.0 IOO. o o. 238 Chloroform 66. 6 78. 9 0.226 " 79.2 85. 9 0. 179 " 26. 5 40. 4 0.212 " 44.9 56. 7 0. no 11 o. O. o 0.207 " O.O 0. 0. 053 ft Naphthol 86. 93- 9 0.190 Carbon Bisulphide 82.0 83. 8 o. 236 " 73- i 87- i 0.169 " 50-5 61. 8 0. 227 Nitro Benzene 78. 4 88. 5 0.207 u 26.0 35- 7 o. 187 tt 46. 8 69. 5 - I 57 H *4- 5 21. 2 0. 144 " o. 0. 0.090 tt 0.0 O.O 0. 096 Phenanthrene 87- 2 95- 4 0.205 Naphthalene 86.7 93- 5 0. 199 " 75- 90. 2 0.183 '* 72.6 85- 4 o. 187 SOLUBILITY OF CARBON MONOXIDE IN MIXTURES OF BENZENE AND OTHER SOLVENTS AT 25. (Skirrow Z. physik. Chem. 41, 144, '02.) The solubility of the CO given in terms of the Ostwald Expression, see p. 105. Mixture of Benzene and: %C6H 6 in Mixture. CO. }~, Mixture of Benzene and: %C 6 H 6 in Mixture. CO. By Wt. By Vol. ByWt . By Vol. Naphthalene 100.0 IOO. o .174 Anilin 87. 3 89.1 .156 " 88.5 92. 6 .164 " 71- 7 75-2 131 " 66.2 76. 3 .141 tt 42. 6 47.0 095 Phenanthrene 89.2 95- i 0.144 tt 21. 2 24-3 .068 " 72.6 8 0.127 O. O O.O 053 a Naphthalene 96-5 98.' i .149 Nitro Benzene 71. 8 80. 1 152 " 87.9 93- i 139 " 45. i 5 6 -4 o .127 Ethyl Alcohol 47-7 44- 9 o .181 H O.O O.O 093 O.O 0. o .192 SOLUBILITY OF CARBON MONOXIDE IN MIXTURES OF TOLUENE AND OTHER SOLVENTS AT 25. (Skirrow.) Mixture of 5 CH 3 in ture. 1 CO. / Mixture of Toluene mid* %CoHsCH3 in Mixture. CO. /. Toluene and: B'y Wt. By Vol. *zo 'By Wt. By Vol. *O* Anilin 100.0 IOO-O .182 a Naphthol 95- 5 97-1 .171 tt 94-4 93 5 .169 u 2 94-2 l62 " 80. i 80-3 .148 Nitro Benzene 81. 7 85-7 .160 tt 55-4 55-6 o .115 tt 5- 8 58.1 o 131 " 25-4 25.6 o .077 " 23- 7 29-3 o .108 tt o.o o 053 " o. o O-O 093 Naphthalene 92.9 94 .8 .169 Phenanthrene 94- 4 97.0 .170 " 84.9 88 7 .161 tf 88. 8 93-9 .l6l " 77-3 82 5 .153 " 78. 4 87.5 .147 CARBON MONOXIDE no SOLUBILITY OF CARBON MONOXIDE IN MIXTURES OF ORGANIC SOLVENTS AT 25. (Skirrow.) Mixture Composed of: % of Latter in Mixture. C O. By Wt. By Vol. fee- Chloroform and Methyl Alcohol o . o o . 207 " " 13-0 0.202 " " 100 0.196 Carbon Bisulphide and Ethyl Di Chloride 100 o . 147 75 0.157 51 0.160 18.4 0.140 o.o 0.083 Methyl Alcohol and Glycerine o.o o.o 0.196 39.6 30.1 0.096 " " 60.5 50.1 0.052 77.1 68.9 0.025 " " 100. o 100. o very small NOTE. From the results shown in the preceding five tables, it is concluded that the solubility of carbon monoxide in various mixtures of organic solvents is, in general, an additive function. CARBON BISULPHIDE CS 2 . SOLUBILITY IN WATER. (Chancel and Parmentier Compt. rend. 100, 773, 85; Rex Z. physik. Chem. 55, 355, '06.) Grams CSg per 100 Grams CS2 pe 1 100 ** cc. Solu- Cms. H 2 O t . cc. Solu- Gms. H 2 O tion. (Rex). tion. (Rex). o 0.204 0.258 30 0.155 0.195 5 - I 99 35 o- x 37 10 0.194 0.239 40 o.in 15 0.187 ... 45 0.070 20 0.179 o.ioi 49 0.014 25 0.169 100 cc. H 2 O dissolve o.i 74 cc. CS 2 at 22; Vol. of solution = 100.208, Sp. Gr. = 0.9981. 100 cc. CS 2 dissolve 0.961 cc. H 2 O at 22; Vol. of solution= 100.961, Sp. Gr. = 1.253. (Herz Ber. 31, 2670, '98.) SOLUBILITY OF CARBON BISULPHIDE IN: Aq. Solutions of Ethyl Alcohol at 17. Methyl Alcohol. (Tuchschmidt and Folleuins Ber. 4, 583, '71.) (Rothmund Z. physik. Chem. 26, 475, '08.) Wt. per Gms. CS2 Wt. per Gms. CS 2 Wt. per centCS 2 in: cent per 100 cc. cent per 100 cc. t . CHaOH GST" 1 Alcohol. Solvent. Alcohol. Solvent. Lajer. La7 er . loo oo 91.37 50 10 45-i 9 8 -3 98.5 l82 84.12 30 20 50.8 97.2 98.15 132 76.02 20 25 54.2 96.4 96.95 100 48.40 2 30 58.4 95.5 93-54 7o 47-90 o 35 64.0 93.5 40.5 (crit. temp.) 80.5 Ill CARBON OXYSULPHIDE SOLUBILITY OP CARBON OXYSULPHIDE IN WATER. (Winkler; see Landolt and Bernstein's Tabellen, sd ed. p. 602, 1906.) O 5 10 15 1-333 i .056 0-835 0.677 0-356 20 0.561 0.147 0.28l 25 0.468 0.122 O-22I 3O 0.403 O.IO4 0-179 For /3 and q see Carbon Dioxide, page 105. CARBON TETRACHLORIDE. See p. 201. CARVOXIME C 10 H 4 :NOH. SOLUBILITY IN r LIMONENE. (Goldschmidt and Cooper Z. physik. Chem. 26, 714, '98.) Gms. CinH:NOH Gms. CioHUiNOH t . per 100 Gms. Solid Phase. t. per 100 Gms. Solid Phase. r Limonene. r Limonene. 24.6 44-6 / Carvoxime 4 8 198.7 / Carvoxime 30.0 59-2 / Carvoxime 49-4 199.7 r Carvoxime 30-3 63-3 r Carvoxime 55-4 325-I ' I Carvoxime 38.4 104.3 / Carvoxime 55-9 346.6 r Carvoxime 39-4 103.1 r Carvoxime 58.8 560-0 r Carvoxime 43 - 1 130.8 / Carvoxime 63.2 126.93 r Carvoxime CERIUM ACETATE, BUTYRATE, FORMATE, etc. SOLUBILITY IN WATER. (Wolff Z. anorg. Chem. 45, 102, '05.) Grams Anhydrous Salt per 100 Gms. Solution at: Salt. Acetate Butyrate Iso Butyrate Formate Propionate Formula. Ce(C 2 H 3 2 ) 3 .i$H 2 Ce(C 4 H 7 2 ) 3 , and 3 H 2 Ce(C 4 H 7 2 ) 3 . 3 H 2 Ce(CH0 2 ) 3 Ce(C 3 H 5 O 2 ) 3 .H 2 O, an 3-544 15 19.61 3.406 6.603(20.4) 18.99 76. 12.97 1.984 3-39 0-374(75-3) 15-93 CERIUM AMMONIUM NITRATE (Ceri) Ce(NO 3 ) 4 .2NH 4 NO 3 . SOLUBILITY IN WATER. (Wolff.) f. Gms. per 100 Gms. Solution. * Atomic Gms.Ce(N0 3 )4.2NH 4 NO 3 Relation. per 100 Gms. NIL,. Ce. NIL, : Ce. Solution. Water. 25 4.065 15.16 2.08 i 58.49 140.9 35-2 4-273 16.10 2 .06 i 61.79 161.7 45-3 4.489 16.69 2.08 i 64.51 174.9 64-5 4.625 (i7-4oCe ( 15. 03 Ce IV 2.06 2-39 LCe iCelV 66.84 201.6 85.6 4 .7 7 8 (i8.i6Ce 1 15 -79 Ce IV 2 .04 2-34 i Ce iCe IV 69.40 226.8 22.82 Ce 2.08 iCe 112 .117 i6.22CeIV 2-95 iCelV 88-03 735-4 CERIUM AMMONIUM NITRATE 112 CERIUM AMMONIUM NITRATE (Cero) Ce(NO 3 ) 3 .2NH 4 NO,. 4 H a O. SOLUBILITY IN WATER. (Wolff.) t. Gms. per 100 Gms. Solution. Atomic Relation. Gms. Ce(NO 3 ) 2 .2NH per 100 Gms. NH 4 . Ce. " NIL. Ue. Solution. Water." 8 75 4 .787 18 56 I 999 I 70 .2 235-5 25 .0 5 .09 19 .80 I 995 I 74 .8 296.8 45 .0 5 53 21 .06 2 037 I 80 4 410.2 60 6 .01 22 77 2 054 I 87 .2 681.2 65 06 6 .11 23 .42 2 .022 I 89 .1 817.4 CERIUM AMMONIUM SULPHATE Ce 2 (SO 4 ) 3 .(NH 4 ) 2 SO 4 .8H 2 O. SOLUBILITY IN WATER. (Wolff.) Gms. _ Ce 2 (S0 4 ) 3 .(NH 4 ) 2 S0 4 1 per 100 Gms. Solid Phase. .8H 2 ( Solution. Water. 22.3 5.06 5.33 35.1 4.93 5.18 45-2 4.76 4.99 45-o 55-25 75-4 85-2 Gms. Ce 2 (S0 4 ) 3 .(NH 4 ) 2 S0 4 per 100 Gms. Solution. Water. 2.91 2.99 2.16 2.21 I . 46 I . 48 1.17 1.18 Solid Phase. Anhydride CERIUM SULPHATE Ce 2 (SO 4 ) 3 . SOLUBILITY OF THE SEVERAL HYDRATES IN WATER. (Koppel Z. anorg anorg. Chem. 16, 455, to be inaccurate.) Gms. Ce2(S0 4 ) 3 - ( t. per 100 ** . Chem. 41, 377, '04; the previous determinations '98, and by Wyrouboff Bull. soc. chim. [3] 25, Mols. CerfSC>4)s i 8 ?^? 61 " Solid Phase. t. oer 10^ ' by 121 2e*( Muthman and Rolig Z. , '01, are shown by Koppel Mols. Gms. Solution. H 2 0. SoluTion. H2 ' 14 .20 O .525 Ce2(S0 4 ) 3 .i 2 H20 20-5 8 .69 O .302 Ce 2 (S0 4 ) 3 .8H 2 O 18.8 14 .91 555 40 5 .613 .188 " 19.2 IS .04 .561 60 3 .88 .129 " o 17 35 o . 665 Ce5(SO 4 ) 3 .9H 2 O 45 8 .116 .280 Cej(S0 4 ) 3 .sH30 15 10 .61 .376 60 3 145 o .103 " 21 8 .863 o .308 80 I .19 .0382 " 31-6 6 .686 o .227 100.5 .46 .0149 45-6 4 .910 . 164 35 7 .8 o .27 Ce 2 (S0 4 ) 3 . 4 H,0 50 4 465 . 148 40 5 .71 .19 60 3 73 .123 5 a .31 .11 " 65 3 47 .114 65 I, 85 o .06 " o 15 95 . 605 Ce 2 (SO 4 ) 3 .8H 2 O 82 o 9 8 .032 " 15 9 95 o 350 100.5 o 42 014 H3 CHLORAL HYDRATE CHLORAL HYDRATE C 2 HC1 3 O.H 2 O. SOLUBILITY IN WATER, ETHYL ALCOHOL, CHLOROFORM, AND IN TOLUENE. . (Speyers Am. J. Sci. [4] 14* 294, '02.) Calculated from the original results, which are given in terms of gram molecules of chloral hydrate per 100 gram mols. of solvent. In Chloroform. In Toluene. I . / w. s. W. s w. s. w S. o 433 189-7 [ -II 123 3 1-530 3- 7 o. 898 3-2 5 .460 233-o [.16 130 o 1 .515 4- o o. 900 4.0 10 485 275.0 23 140 o 1 .510 5- o o. 910 7-o 15 .510 330.0 30 160 1-505 9- o o. 915 II. 20 535 383-0 36 185 o 1.510 19. o. 94 21.0 25 555 433-o .42 215 o 1.520 34- o o. 97 36.0 30 .580 480 . o ] 49 245 o 1.540 56. o I. 02 56.0 35 59 516.0 J 55 280 1.570 80. o I . 13 80.0 40 .605 ] [.60 320 1.590 no. I. 40 no.o 45 J .620 . W = wt. of i cc. grams solvent. saturated solution, S = Gms. C 2 HC1 3 .H 2 O per 100 CHLORINE Cl. SOLUBILITY IN WATER. (Winkler Landolt and Bernstein's Tabellen, 3d ed. p. 532, 601, '06; Roozeboom Rec. trav. chirn. 3t 59. :ems labellen, 3d ed. p. <;32, ooi, 06; Kooze '84; 4, 69, '85; Z. physik. them. 2, 452, '88.) Gms. Cl per Solid * - " 9- * 100 Gms. H^. Phase. o 4.610 1.46 0.24 0.492 Ice+C1.8aq. 3 3-947 1-25 o 0-507-0.560 C1.8 aq. 6 3-4H 1. 08 2 0.644 tt 9 3-031 0.96 4 0.732 tt 9.6 2.980 o-94 6 0-823 " 12,0 2.778 0.88 8 0.917 10 3-095 o-997 9 0.965-0.908 tt IS 2-635 0.849 20 I-8 S tt 20 2 .260 0-729 28.7 tt 25 1.985 0.641 30 1.769 o-572 40 I.4I4 0-459 50 1.204 o-393 60 1. 006 0-329 70 0-848 0.279 80 0.672 0.223 90 0.380 0.127 100 o.ooo o.ooo ft' = vol. of Cl (red. to o and 760 mm.) absorbed by i vol. H 2 O at total pressure of 760 mm. q = Gms. Cl per 100 gms. H 2 O at a total pressure of 760 mm. CHLORINE 114 SOLUBILITY IN WATER. (Goodwin Ber. 15, 3039, '82.) The saturated aqueous solution of the chlorine was cooled until chlorhydrate separated; the temperature was then gradually raised and portions withdrawn for analysis at intervals. Slightly different results were obtained for solutions in contact with much, little, or no chlorhydrate. The following results are taken from an average curve. ^o Solubility t o Solubility .<> Solubility Coefficient. Coefficient. Coefficient. 2-5 1.76 II 3-0 25 2.06 5.0 2.00 12.5 2.75 30 1.8 7.5 2.25 15 2.6 40 1.35 10 2-7 20 2-3 50 1.0 SOLUBILITY OF CHLORINE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC ACID AND OF POTASSIUM CHLORIDE. (Goodwin.) Coefficient of Solubility in: t. HC1 HC1 HCl KCl (1.046 Sp. Gr.). (1.08 Sp. Gr.). (1.125 Sp. Gr.). (20 g. per 100 cc.). o 4-i 6. 4 7-3 i-5 5 5-i 5-2 6.7 2.0 10 4.1 4-5 6.1 2.2 IS 3-5 3-9 5-5 1.6 20 3-o 3-4 4-7 I .2 25 2 -5 3-o 4-0 1.0 30 2.O 2.4 0-9 40 1.25 1.6 Goodwin also gives results for solutions of NaCl, CaCl 2 , MgCl 2 , SrCl 2 , Fe 2 Cl 2 , CoCl ? , NiCl 2 , MnCl 2 , CdCl 2 , LiCl, and in mixtures of some of these, but the concentrations of the salt solutions are not stated. SOLUBILITY OF CHLORINE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE. (Kumpf Wied. Ann. Beibl. 6, 276, '82; Kohn and O'Brien J. Soc. Chem. Ind. 17, 100, '08.) Coefficient of Solubility in: l> . 9-97% NaCl. i6.oi%NaCl. 19-66% NaCl. 26 .39% NaCl. o 2-3 1-9 1.7 0.5 5 2.0 1.6 1.4 0.44 10 I .7 I .3 I .15 0.4 15 1.4 1. 06 o-95 0.36 20 I .2 0-9 0.8 0.34 2$ 0-94 0-75 0.65 o-3 50 O.2 80 . . . 0.05 ioo cc. of 6.2 per cent CaCl 2 solution dissolve 0.245 gram Cl at 12. 100 cc. of 6.2 per cent MgCl 2 solution dissolve 0.233 gram Cl at 12. ioo cc. of 6.2 per cent MnCl 2 solution dissolve 0.200 gram Cl at 12. For coefficient of solubility see page 105. ii5 CHLORINE MONOXIDE CHLORINE MONOXIDE C1,O. ioo volumes of water at o absorb 200 volumes of C1 2 O gas. CHLORINE TRIOXIDE C1 2 O 3 . SOLUBILITY IN WATER AT APPROX. 760 MM. PRESSURE. (Brandan Liebig's Ann. 151, 340, '69.) t. 8.5. 14-0. 21. 93". Gms. Cl^Og per ioo gms. ILfl 4-7^5 5-012 5-445 5.651 Garzarolli and Thurnbalk Liebig's Ann. 209, 184, '81, say that C1 2 O 3 does not exist, and above figures are for mixtures of C1 2 O and Cl. CHLOROFORM CHC1 3 . SOLUBILITY IN WATER. (Chancel and Parmentier Compt. rend, ioo, 473, 85; Rex Z. physik. Chem. 55, 355, '06.) t o Gms. CHC1 3 ioo Gms. H 2 O t. Gms. CHC1 3 per Liter of Solution, Density of Solutions. o 9.8 7 1.00378 3-2 8.90 17-4 7-12 1.00284 29.4 7-05 I .00280 41.6 7.12 I .00284 54-9 7-75 I .00309 O 10 20 30 1.062 0.895 0.822 0.776 ioo cc. H 2 O dissolve 0.42 cc. CHC1 3 at 22; Vol. of sol. = 100.39 cc - Sp. Gr. = 1.0002. ioo cc. CHC1 3 dissolve 0.152 cc. H 2 O at 22; Vol. of sol. = 99.62 cc., Sp. Gr. = 1.4831. (Herz Ber. 31, 2670, '98.) SOLUBILITY OF CHLOROFORM IN AQUEOUS ETHYL ALCOHOL, METHYL ALCOHOL, AND ACETONE MIXTURES AT 20. (Bancroft Phys. Rev. 3, 29, '95, '96.) In Ethyl Alcohol. In Methyl Alcohol. Per 5 cc. C 2 H 5 OH. Per 5 cc. CH 3 OH. cc. H 2 O. 10 cc. CHC1 3 . O.2O 8 -3 6 0-5 1 ! 4 *-*3 2 I 2-51 4.60 0.91 0.76 6.0 O-55 8.0 0.425 IO.O 0.20 20. o 0.125 30.24 cc. H 2 0. cc. CHC1 3 . IO O.IO 5 4 0.48 0.8o 2 4-0 1.49 7-0 8.0 I .12 IO.O In Acetone. Per 5 cc. (CH 3 ) 2 CO cc. H 2 O. cc. CHC1 3 . 0.16 4-0 O-22 2 .O o-33 0.58 I.O 0-955 o-79 0-505 1. 12 1. 60 0.30 2.50 0.21 3-50 0.19 0.16 4-0 5-o 0.12 IO.O CHROMIUM ALUMS 116 SOLUBILITY OP CHROMIUM ALUMS IN WATER AT 25. (Locke Am. Ch. J. 26, 174, 'ox.) Per IPO cc. Water. Mum. Formula. 'Grams Grams Gram " Anhdyrous. Hydrated. Mok. Potassium Chromium Alum KjCr^SO^. 241^0 12.51 24.39 0.0441 Tellurium Chromium Alum Te 2 Cr 2 (SO 4 ) 4 .24H 2 O 10.41 16.38 0.0212 CHROMIUM CHLORIDE (ic) CrCl 3 .6iH 2 O. 100 grams H 2 O dissolve 130 grams (green modification) at 15. (Recoura Compt. rend. 102, 518, '86.) CHROMIUM DOUBLE SALTS. SOLUBILITY IN WATER. (Jorgensen J. pr. Chem. [2] 20, 105, '79; [2] 30, i, '84; [2] 42, 208, '90; Struve Ibid. [2] 61, 457, '99.) Gms. per Name of Salt. Formula. t . too Gms. H 2 O. Chloro Tetra Amine Chromium Chloride CrCl(NH 3 ) 4 (OH 2 )Cl 2 15 6.3 Chloro Purpureo Chromium Chloride CrCl(NH 3 ) 5 Cl 2 16 0.65 Luteo Chromium Nitrate Cr(NH 3 ) 6 (NO 3 ) 3 ? 2.6 Chloro Purpureo Chromium Nitrate CrCl(NH 3 ) 5 (NO 3 ) 2 17.5 1.4 Chromic Potassium Molybdate 3K 2 O.Cr 2 O 3 .i2MoO 3 .2oH 2 O 17 2.5 CHROMIUM TRIOXIDE CrO 3 . SOLUBILITY IN WATER. (Mylius and Funk Wiss. Abh. p. t. Reichanstalt, 3, 451, 'oo.) o 15 18 50 99 7 39 37 - 1 Density of solution saturated at 18 = 1.705. CHROMIUM SULPHATES (ous and ic). SOLUBILITY m WATER (ous at o). Salt. G 5i. P H 2 a Solid Phase. Authority. ChromOUS 12.35 CrSO 4 .7H 2 O (Moissan Bull. soc. chim. [2] 37. 206, '8a ) Chromic 1 20 . Cr 2 (SO 4 ) 3 . iSH^O (Etard Compt. rend. 84, 1090, '77.) CHRYSAROBIN CH at O 7 . SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.) Gms. CrOa per 100 g. Solution. Mols. CrO 3 per 100 Mols. H 2 O. Solid Phase. 62.08 29.4 CrO, 62.38 29.8 62.45 29.91 it 6 4-55 32-7 tt Water 0.021 0.046 Chloroform 5-55 Alcohol 0.324 0.363 (60) Ether 0.873 Benzene 4.0 ... Amyl Alcohol 3.33 Carbon Bisulphide 0-43 ii; OHRTSEN OHBYSEN C 18 H 12 . SOLUBILITY IN TOLUENE AND IN ABS. ALCOHOL. (v. Becchi.) ioo gms. toluene dissolve 0.24 gm. C 18 H 12 at 18, and 5.39 gms. at 100. ioo gms. abs. alcohol dissolve 0.097 gm. C 18 H 12 at 16, and 0.170 gm. at b. pt. CINCHONA ALKALOIDS. (See also Quinine, p. 269.) SOLUBILITY OF CINCHONINE, CINCHONIDINE, QUININE, AND QUINIDINE IN SEVERAL SOLVENTS AT i8-22. (Miiller Apoth.-Ztg. 18, 233, '03; see also Prunier J. pharm. chim. [4] 39, 136, '79.) Grams of the Alkaloid per ioo Grams Solution. Solvent. i x Quinine Cinchonine C* U XT C\ Cinchonidine CH N O r* IT CjoH; M N,O,. Quinidine P H M O Cl9MNt->. 19^23-^2^. Hydrate. Anhydride. <-204 i>l a'-'- Ether 0-10 O.2II I .619 0.876 0.776 Ether sat. with H.,0 0.123 0.523 5.6l8 2.794 1.629 Hp sat. with Ether O.O25 0.0306 0.0667 0.0847 0.031 Benzene 0-0545 0.099 O.2O54 I .700 2.451 Chloroform 0.6979 9.301 100 + 100 + 100 + Acetic Ether .0.0719 0.3003 4.65 2.469 1.761 Petroleum Ether 0-0335 0-0475 O.OIO3 O-O2II O.O24I Carbon Tetra Chloride 0-0361 0.0508 0.203 0.529 0-565 Water 0.0239 0-0255 o-574 0.0506 0-0202 Glycerine (15.5) 0.50 0.50 ioo grams chloroform dissolve 0.565 gm. cinchonine at 50. ioo grams abs. ether dissolve 0.264 gm. cinchonidine at 32. (Kohler Z. anal. Ch. 18, 242, '79.) SOLUBILITY OF CINCHONINE AND CINCHOTINE SULPHATE, TARTRATE, BlTARTRATE, OXALATE, AND HYDROCHLORIDE IN WATER. (Forst and Bohringer Ber. 14, 1266, '81.) Cinchonine Salts. Cinchotine Salts. Gms. per Formula. t . ioo Gms. Formula. 2 (C 19 H 22 N 2 0)S0 4 H 2 . 2 H 2 2 (C 19 H 22 N 2 O) C 4 H 6 O 6 . 2 H 2 O wa.... (C 19 H 22 N 2 O) .C 2 H 4 O 4 .H 2 O 19 H 22 N 2 O.HC1. 2 H 2 O 13 1 6 1 6 20 10 1.52 2(C 19 H 24 N 2 0)S0 4 H 2 . 2 H 2 13 3.0 2(C 19 H 24 N 2 O)C 4 H 6 O 6 . 2 H 2 O 1 6 0.99 C 19 H 24 N 2 O.C 4 H 6 6 . 4 H 2 16 0.06 2 (CjgH^NaO) .C 2 H 2 O 4 .H 2 O 10 4.16 C 19 H 24 N 2 O.HC1. 2 H 2 O 10 Gms. pet ioo Gms. H 2 0. 3.28 1.76 1.28 1.16 2.12 SOLUBILITY OF CINCHONINE SULPHATE AND OF CINCHONIDINE SUL- PHATE IN SEVERAL SOLVENTS. Solvent. (U. S. P.) Gms. (C 19 H22N 2 2 ) 2 H 2 S04.2H 2 per ioo Gms. Solvent. ' At 25. At 80. " Water 1.72 3- 1 Alcohol 10. 19.2(60) Ether 0.04 . . . Chloroform i-45 . . . Glycerine 6-7 (i5) i ... Gms. (C 1 oH 22 N 2 O) !! .H 2 S04.3H 2 O per ioo Gms. Solvent. At 25 1. 60 1-4 0-02 O-II At 80 4.80 (60) CINNAMIC ACID 118 OINNAMIO ACID C 6 H 5 CH:CH.COOH. SOLUBILITY OF CINNAMIC ACID IN AQUEOUS SOLUTIONS OF SODIUM ACETATE, BUTYRATE, FORMATE, AND SALICYLATE AT 26.4. (Philip J. Chem. Soc. 87, 992, '05.) Calculated from the original results, which are given in terms of molecular quantities per liter. Gms Na Salt Gms> CaH 5 CH:CH.COOH per Liter in Solutions of: per Liter. O I 2 3 4 8 ... ... ... 0.90 i liter of aqueous solution contains 0.491 gm. C 6 H 5 CH:CH.COOH at 25 (Paul). SOLUBILITY OF CINNAMIC ACID IN AQUEOUS SOLUTIONS OF ANILIN AND OF PARA TOLUIDIN AT 25. (Lowenherz Z. physik. Chem. 25, 394, '98.) Original results in terms of molecular quantities per liter. In Aqueous Anilin. In Aqueous p Toluidin. Grams per Liter. Grams per Liter. CH 3 COONa. CaHyCOONa. HCOONa. Ce^.OH.COONa. 0.56 0.56 0.56 0-56 1.50 1.30 0.92 0.62 2.12 1.85 I .12 0.70 2.52 2-25 1.27 o-73 2.85 2.60 1.40 0.77 3-05 2.90 i-47 0.80 : CHCOOH. C^CHgNHa. C 6 H 5 CH :CHCOOH. 0.49 o 0.49 1 1.20 I 1.52 2 1-65 2 2.20 3 2.02 3 2.83 4 2.35 4 3-35 6 2.92 5 3.80 SOLUBILITY OF CINNAMIC ACID IN METHYL, ETHYL, AND PROPYL ALCOHOLS. (Timofeiew Compt. rend. 112, 1137, '91.) Grams C 6 H 5 CH:CH.COOH per 100 Grams of: CHaOH. C 2 H 6 OH. o 20.65 15-61 10.63 19.5 28.91 22.03 I 5-4i SOLUBILITY OF BROM CINNAMIC ACIDS. a Brom and ft Brom Cinnamic Acid a Brom Cinnamic Acid in Aq. in Water at 25. Solutions of Oxalic Acid at 25. (Paul Z. physik. Chem. 14, in, '94.) (Noyes Z. physik. Chem. 6, 245, '90.) Per 1000 cc. Solution. Normality of Solutions. Grams per Liter. Acid. Grams. Millimols. ' (COOH) 2 . CeH 6 CH': (COOH) 2 . QHsCH^ CBr:COOH. CBrCOOH. a, C 6 H 6 CH: CBrCOOH 3.9325 *7'3 2 0.0176 o.o 3.995 ft C 6 H 5 CBr: CHCOOH 0.5255 2.315 0.0275 0.0140 2.448 3.178 0.0524 0.0129 4.716 2.928 1 1 9 CITRIC AOID OITBIO AOID C 3 H 4 (OH)(COOH) 3 .H 2 O. SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.; Bourgoin Ann. chim. phys. [5] 13, 406, '78.) _ . Cms. C3H 4 (OH)(COOH)3.H 2 per 100 Cms. bolvent. t . - ; > solution. bolvent. Water 25 64.8 185 Water b. pt. 70.3 250 Alcohol (90%) 25 34.6 75.9 Alcohol (U.S.P.) " 39-2 64.5 Alcohol (Abs.) 43.2 52.8 Ether " 2.21 2.26 Ether (U.S.P.) " 5-2 5-55 COBALT BROMIDE CoBix SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 537, '94.) t. 59. 75. 97. Gms. CoBr 2 per 100 gms. solution 66.7 66.8 68.1 (blue) COBALT DOUBLE SALTS. SOLUBILITY IN WATER. (Jorgensen J.pr. Chem. [2] 18, 205, '78; iQt 49. '795 Kurnakoff J. russ. phys. chem. Ges. 24, 629, '92.) Gms. Salt Name. Formula. t. per zoo Gms. H 2 O Chloro purpureo cobaltic bromide CoCl(NH 3 ) 5 Br 2 14.3 0.467 Bromo purpureo cobaltic bromide CoBr(NH 3 ) 5 Br 2 16 0.19 Chloro tetra amine cobaltic chloride CoCl(NH 3 ) 4 (OH 2 )Cl 2 2 . 50 Chloro purpureo cobaltic chloride CoClCNH.,)^^ o 0.232 Chloro purpureo cobaltic chloride CoCl(NH 3 ) 5 CL5 I 5-S 0.41 Chloro purpureo cobaltic chloride CoCl(NH 3 ) 5 Cl2 46 6 i .03 Luteo cobaltic chloride Co(NH 3 ) 6 Cl 3 o 4.26 Luteo cobaltic chloride Co(NH 3 ) 6 CL, 46.6 12.74 Roseo cobaltic chloride Co(NH 3 ) 5 (OH 2 )Cl s o 16.12 Roseo cobaltic chloride Co(NH 3 ) 5 (OH 2 )Cl 3 16 . 2 24 .87 Chloro purpureo cobaltic iodide CoC^NH,,)^ 19.2 2.0 Chloro purpureo cobaltic nitrate CoCl(NH 3 ) 5 (NO 3 ) 2 15 1.25 Chloro purpureo cobaltic sulphate CoCl(NH 3 ) 5 SO 4 .2H 2 O 17.3 0.75 Nitrato purpureo cobaltic nitrate Co(NO 3 )(NH3)(NO 3 ) 2 16 0.36 COBALT CHLORATE Co(ClO 3 ) 2 . SOLUBILITY IN WATER. (Meusser Ber. 35, 1419, '02.) Mols. Solid Phase. Co(C10 3 ) 3 .4H 2 0. t Gms. Co(C10a) 2 Mols. Co(C10 3 ) 2 Solid Gms. Co(C10 3 ) 2 Mols. Co(C10 3 ) 2 per 100 Gms. Solution. per 100 Phase. Mols.HaO. ' per 100 Gms Solution. per 100 Mols. H 2 O. 12 2 9 97 3 .41 Ice 18 6 4 .19 14 .28 21 53 30 9 .08 Co(ClO 8 ) 2 .6H 2 O . 21 6 4 39 14 51 -19 53 .61 9 .20 35 6 7 - 09 16 10 O 57 45 IO 75 " 47 6 9 . 66 18 29 10.5 61 83 12 .90 " 61 7 6. 12 25 39 Density of solution saturated at 18 = 1.861. COBALT CHLORIDE 120 COBALT CHLORIDE CoCl 2 . SOLUBILITY IN WATER. (Etard Compt. rend. 113, 699, '91; Ann. chim. phys. [7] 2, 537, '94-) Cms. Cms. t o CoCl 2 per Solid CoCl 2 per Solid 100 Cms. Phase. 100 Gms. Phase. Solution, Solution. -io 27.0 CoO^HjO (red) 35 38.0 CoCl 2 .H 2 O (violet) o 29.5 40 41.0 + 10 3 J -5 5o 47-o 20 33-5 60 47-5 CoOyHjO (blue) 25 34-5 80 49-5 30 35.5 100 51.0 SOLUBILITY OP COBALT AMMONIUM CHLORIDES IN WATER. (Kurnakoff J. russ. phys. chem. Ges. 24, 629, '93; J. Chem. Soc. 64, ii, 509, '93.) c . Grams per 100 Grams H 2 O at: salt. / v o. 16.9. 46.6' 0.232 ... 1.031 16.12 24.87 ... CoClg.6NH 3 4.26 ... 12.74 SOLUBILITY OF COBALT CHLORIDE IN AQUEOUS HYDROCHLORIC ACID SOLUTIONS AT o. (Engel Ann. chim. phys. [6] 7, 355, '89.) Milligram Mols. per 10 cc. Sol. Sp. Gr. of Ss%1iitirkn 2 . SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichanstalt 3, 439, 'oo.) t -26 20-5 21 IO - 4 o + 18 Gms. Mols. Co(N0 3 ) 2 Co(N0 3 ) 2 per_ioo Gms. per 100 Solution. 39-45 42.77 4i-55 43-69 44-85 45-66 49-73 Solid Phase. H 2 0. 6.40 Co(NOs) 2 .9H 2 35 Co(NO 8 ) 2 .6H2O 7 6.98 7.64 7-99 8.26 9.71 t. Gms. Co(N0 3 ) 2 per ioo Gms. Mol Co(NC per i Solution. Mols.E 41 55-96 12.5 56 62.88 I6. 7 55 61.74 15-8 62 62.88 I6. 7 70 64-89 18.2 84 68.84 21-7 91 77-21 33-3 Co(NO,) 2 .6H 8 Co(N03) 2 . 3 H,0 Density of solution saturated at 18 = 1.575. COBALT NITRATE 122 SOLUBILITY OF COBALT NITRATE IN GLYCOL. (de Coninck Bull. acad. roy. Belgique, 359, '05.) 100 grams saturated solution contain 80 gms. Cobalt Nitrate. COBALT RUBIDIUM NITRITE Rb 3 Co(NO 2 ) 6 .H 2 O. 100 grams H 2 O dissolve 0.005 gram of the salt. (Rosenbladt Ber. 19, 2531, '86. COBALT SULPHATE CoSO 4 .7H 2 O. SOLUBILITY IN WATER. (Mulder; Tobler Liebig's Ann. 95, 193, '55; Koppel VVetzel Z. physik. Chem. 52, 395, '05.) Gms. CoSO 4 t. per 100 Gms. Mols. CoS0 4 per 100 t. Gms. CoSO 4 Mols. CoSO 4 per 100 Gms. p^ I00 Solution. Water. Mols. t! 2 U. Solution. Water. Mols. H;zO. o 20:35 25.55 2.958 35 31.40 45-80 5.31 5 21.90 28.03 3-251 40 32-81 48.85 5-664 10 23.40 30.55 3.540 50 35.56 55.2 15 24.83 33.05 3.831 60 37.65 60.4 20 26.58 36.21 4-199 7 39-66 65.7 25 28.24 39.37 4.560 80 41.18 70.0 30 29.70 42.26 4-903 I0 45-35 83.0 SOLUBILITY OF MIXTURES OF CoSO 4 .7H 2 O AND Na 2 SO 4 .ioH 2 O IN WATER. (Koppel; Wetzel.) Gms. per Gms. per Mols. per $. 100 Gms. Solution. 100 Gms. H 2 O. 100 Mols. H 2 O. Solid Phase. 'CoS0 4 . N a2 S0 4 . CoSO 4 . Na 2 SO 4 . CoSO 4 . Na 2 S0 4 . 5 16.56 17.46 7 9 63 59 21 23 85 94 10 .07 2 2 54 77 1.27 1.6 7 CoS0 4 . 7 H 2 + Na 2 S0 4 .ioH 2 O 10 17.90 ii 73 25 .41 16 67 2 94 2. II M 20 17-59 16 43 26 65 24 .91 3 .09 3-15 CoNa 2 (S0 4 ) 2 . 4 H 2 25 17.06 15 70 25 36 23 32 2 95 2-97 30 15-94 14 93 23 21 .61 2 .70 2.74 " 35 15-73 14 52 22 54 20 85 2 .62 2 .64 " 40 14-87 14 .22 2O .98 20 05 2 .46 2-53 . " 18.5 18-75 15 .61 28 .61 23 .82 3 32 3.02 CoNa 2 (S0 4 ) 2 . 4 H 2 20 19.30 15 .10 29 .42 23 .01 3 .41 2.92 + CoS0 4 . 7 H 2 O 2 5 20-30 13 .60 30 74 2O 58 3 56 2 .6l 3o 21.67 12 05 32 .70 18 .17 3 79 2.30 < 35 22.76 IO 43 34 .06 15 .61 3 95 I. 9 8 " 40 24-05 9 .16 35 OI 13 72 4 .81 1.74 44 , 18.5 16.87 16 97 2 5 5o 25 65 2 .96 3-25 CoNa 2 (S0 4 ) 2 . 4 H2O 20 I5-4I 18 .12 23 .18 27 .26 2 .69 3-45 +Na 2 SO 4 .ioH 2 O 25 10.63 23 .26 16 .07 35 .17 I .86 4.46 4 , 30 6.01 28 .6 7 9 .20 43 74 I .07 5-54 35 40 4-56 4.72 3i .14 .78 7 7 .19 45 5o 79 . 10 835 .864 6.44 6-34 CoNauCSOJz^HjO + Na 2 S0 4 COBALT SULPHATE SOLUBILITY OF COBALT SULPHATE IN METHYL AND ETHYL ALCOHOL AND IN GLYCOL. Solvent. Gms. per 100 Gms. Solvent. 'CoSO 4 . Observer. Methyl Alcohol (abs.) CoSO 4 .7H 2 O. 42 . 8 (de Bruyn Z. physik. Ch. 10, 784, '92.) 50.9 54-5 13-3 1.8 3 15 18 1.04 (93-5%) 3 ." (50%) 3 Ethyl Alcohol (abs.) 3 ... 2.5 Glycol . .(penoogms. solution) 3 . i COCAINE C 17 H 21 NO 4 . COCAINE HYDROCHLORIDE C 17 H 21 NO 4 .HC1. SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.; at i8-22; Mttller Apoth.-Ztg. 18, 248, '03.) Gms. per too Gms. Solvent. (de Coninck Bull, a cad. roy. Belgique, 359. '05.) Gms. L.i7rl 2l J\(J 4 . Ci7ri2i-l->*~'4""*-'J- per zoo Gms. Solvent. Water 25 0.17 250 Ether +KLO 18-22 34-o Water 80 0-38 1000 11,0+ Ether 18-22 0.254 Alcohol 25 2O-O 38 Benzene 1 8-2 2 100 Ether (U.S.P.) 25 26-3 CC1 4 17 18.5 Ether 18-22 ii. 6 Acetic Ether 1 8-2 2 5 8 -99 Chloroform 18-22 100 + Petroleum Ether 1 8-2 2 2-37 CODEINE C 18 H 21 NO 3 .H 2 O, also the Phosphate and Sulphate. COLCHICINE C 22 H 25 N0 6 . SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.; at i8-22, Miiller.) Grams, per 100 Grams Solvent. Solvent. t. Codeine Codeine ~** c 'i8H2iNO3H 2 O. H 2 SO 4 .s Aq. C 22 H 25 NO 6 . Water 18-22 9.616 Water 25 I .13 44-9 3-3 4-5 Water 80 1.70 217.0 16.0 5.0 Alcohol 25 62.5 0.383 0.096 Alcohol 60 108.7 1.03 0.27 Ether 25 8.0 0.075 0.64 Ether 18-22 . . . . . . 0.126 Ether sat. with H^O 18-22 . . . ... . . . 0.18 H 2 O sat. with Ether 18-22 12.05 Benzene 18-22 0-939 Benzene 25 1.15 Chloroform 25 151 .5 0-015 100 + Carbon Tetra Chloride 17 1.328 O.I2I Acetic Ether 18-22 . . 1.342 Petroleum Ether 18-22 0.058 'COLLIDINE 124 COLLIDINE (2, 4, 6, Tri Methyl Pyridine) C 6 H 2 N(CH,) a . SOLUBILITY IN WATER. (Rothmund Z. physik. Chem. 26, 433, '98.) Gms. Collidin per 100 Gms. Gms. Collidin ^per 100 Gms. Aq. Layer. Collidin Layer. Aq. Layer. Collidin Layer. 5.7 (crit.t.) 17.20 10 7.82 41.66 80 1.73 86.12 20 3.42 54-92 100 1.78 88.07 30 2.51 62.80 120 1.82 88.98 40 1.93 70.03 140 2.19 89.10 60 1.76 80.19 160 2.93 87.2 180 3.67 COPPER ACETATE Cu(C 2 H 3 O 2 ) 2 .H 2 O. 100 grams of glycerine dissolve 10 grams of copper acetate at 15.5. COPPER BROMIDB (ous) Cu 2 Br 2 . SOLUBILITY OP CUPROUS BROMIDE IN AQUEOUS SOLUTIONS OF POTAS- SIUM BROMIDE AT i8-2o. (Bodlander and Storbeck Z. anorg. Chem. 31, 460, '02.) Millimols per Liter. Grams, per Liter. KBr. Total Cu. Total Br. Cu (ic). Cu (ous). KBr. Total Cu. Cu (ic). Cu (ous). 0.3157 0.4320 o. 2096 O .1061 O 0.0201 .0133 0.0067 25 0.119 0. OI2 .107 2. 98 0.0076 .0007 0.0068 40 O.200 0. 013 O .187 4- 76 0.0127 o .0007 0.0119 60 0.310 0. 025 .285 7- i5 0.0197 .0015 0.0181 80 0.423 0. 012 .411 9- 53 0.0266 .0007 0.0261 IOO 0.584 ... o .584 n. 0.0371 0.0371 120 0.693 ... .693 14. 29 0.0441 0.0441 500 8.719 ... 8 .719 59- 55 0.5540 0.5540 COPPER CHLORATE (ic) Cu(ClO 3 ) 2 . 4 H 2 O. SOLUBILITY IN WATER. (Meusser Ber. 35, 1420, '02.) Gms. Mols. Gms. Mols. t Cu(ClO 3 ) 2 Cu(ClO 3 ) 2 Solid t <> Cu(ClO 3 ) 2 Cu(ClO 3 ) 2 Solid per i oo Gms. per 100 Mols. Phase. per 100 Gms. per 100 Mols. Phase. Solution. H 2 0. Solution. H 2 O. 12 30.53 3.43 Ice l8 62.17 12.84 Cu(ClO3) 2 .4H2O 31 54-59 9-39 Cu(ci03) 2 .4H20 45 66.17 15.28 2i 57-12 10.41 " 59.6 69.42 17.73 -ho. 8 58.51 11.02 " 71 76.9 25.57 Density of solution saturated at 18 = 1.695. COPPER CHLORIDE (ic) CuCl 2 . SOLUBILITY IN WATER. (Reicher and Deventer Z. physik. Chem. 5, 560, '90; see also Etard Ann. chim. phys. (7] 2, 528, '94.) Gms. CuCl 2 Gms. CuCl 2 Gms. CuClj t. per loo Gms. t. per 100 Gms. t. per 100 Gms. Solution. Solution. Solution. o 41-4 25 44.0 50 46.65 10 42-45 3 44-55 6o 47-7 20 43.5 40 45.6 80 49 -8 TOO 51.9 Density of solution saturated at o = 1.511, at 17.5 = 1.579. 125 COPPER CHLORIDE SOLUBILITY OF CUPRIC CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO- CHLORIC ACID AT o. (Engel Ann. chim. phys. [6] 17, 351, '89.) Milligram Mols. per 10 cc. Sol. Sp Gr. of Gms. per too cc. Sol. Gms. per too Gms. Sol. *CuCl 2 . HC1. Solutions. CuCl 2 . HCf. CuCl 2 . HCI: 9 J -75 O I 49 61 .70 o. o 41 41 o.o 86.8 4 5 I 475 58 37 I . 64 39 58 1 .11 83-2 7 .8 I 458 55 95 2. 84 38 37 J-95 79-35 10 5 I 435 53 37 3- 83 37 .19 2.67 68.4 20 25 I 389 46 .01 7- 38 33 .11 5-3 1 50.0 37 5 I 3 J 9 33 .62 *3- 67 25 5o 10.37 22.8 70 2 S I .231 IS 33 25- 61 12 .46 20.80 23-5 102 5 I .288 I 5 .81 37- 36 12 .27 29.00 26.7 128 .0 I 323 *7 .96 46. 66 J 3 57 35-26 29 o Sat . HC1 SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF HYDRO- CHLORIC ACID. (Engel Ibid. [6] 17. 372, '89; Compt. rend. 121, 520, '95.) Milligram Mols . per 10 cc. Sol. So. Gr. of Gms. per TOO cc. Sol. Gms. per 100 Gms. Sol iCu 2 C! 2 . HCI. Solutions. C U2 C1 2 . HCI. CU;>C1 2 . HCl- Results at o. O 475 8 975 1-05 O 471 327 448 0.312 I 5 17 I 486 .638 I .418 0.6o8 2 9 26 .0 i .065 2 8 7 2 .948 2 .697 0.932 4 5 34 5 .080 4 457 I 257 4 .127 I .164 8 2 5 47 .8 .135 8 172 I 743 7 .199 I -S3S 15 5 68 5 .261 15 7 2 497 12 .46 1.980 33 .0 104 .0 345 32 68 3 .827 24 .30 2.845 Results at 15-! 6. 7 4 54 4 .19 7 33 i 983 6 159 1.666 10 .8 68 9 .27 10 69 2 5 11 8 .422 1.977 12 .8 75 o .29 12 68 2 734 9 .826 2.119 16 92 .0 1.38 IS .84 3 346 ii .48 2.424 COPPER CHLORIDE, AMMONIUM CHLORIDE MIXTURES IN AQUEOUS SOLUTION AT 30. (Meerburg Z. anorg. Chem. 45. 3. 'osO Grams per 100 Gms. Sat. Solution. CuCl 2 . O 1.9 3-6 NH4C1. 29-5 28.6 25-9 10.5 16.5 19.9 9-4 29.4 4.9 41.4 2.1 43-2 2-0 43-9 Grams per 100 Gms. Solid Phase. CuCl 2 . 6.0 37-o 21.7 28.5 35- 1 NEUCl. 4 8-2 34-9 23-1 18.4 15-3 13-3 6.6 Solid Phase NH4C1 NH4C1 + CuCl-s-aNEUCl ^HjO CuClj - aH^ + CuCl 2 .2H 2 O COPPER AMMONIUM 126 CHLORIDE COPPER AMMONIUM CHLORIDE CuCl 2 .2NH 4 C1.2H,O. SOLUBILITY IN WATER. (Meerburg.) Gms. t . CuCl 2 . 2 NH 4 Cl Solid oer 100 Gms. Phase. Gms. t o CuCl2.2NHCl ' per 100 Gms. Solution. Solution. 10.5 3- 87 Ice 30 27 .70 ( 10.8 20. 12 Ice 40 3 47 ii 20. 3 Ice + CuCl 2 .2NH 4 Cl. 2 H 2 O 50 33 .24 10 20. 46 CuCl i .2NH 4 C1.2H 2 60 36 13 22. 02 *' 70 39 35 12 24. 26 " 80 43 .36 20 25. 95 u Solid Phase. CuCl 2 .2NH 4 Cl. 2 H 2 O SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF CUPRIC SULPHATE AT ABOUT 20. (Bodlander and Storbeck Z. anorg. Chem. 31, 22, '02.) Millimols per Liter. Grams per Liter. CuSO 4 . Total Cu. Total Cl. Cu(ic). Cu(ous). CuS0 4 . Total Cu. Total Cl. Cu(ic). Cu(ous). 2.880 5-3 12 2.258 O.622 o. o O. 183 0.188 0.143 O.O4O 0.987 3.602 4.908 3-145 0-457 0. 158 0. 229 0.174 O. 2OO 0.029 1-975 4-553 4.687 4-I3 1 0.422 0. 3 I 5 O. 290 0.166 0.263 0.027 2.962 5-*93 4.256 4.625 0.509 0. 473 0. 330 0.151 0.292 0.032 4-937 7.276 4-329 6.546 0.730 0. 788 0. 463 0.154 0.416 0.046 SOLUBILITY OF CUPROUS CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM CHLORIDE AT i8-2o EXCEPT DETERMINATIONS IN 3RD, 7TH, STH, AND LAST LINE, WHICH ARE AT 1 6. (Bodlander and Storbeck.) Millimols per Liter. Grams per Liter. KC1 . Total Cu. Total Cl. Cu(ic). Cu(ous). KC1. Total Cu. Total Cl. Cu(ic). Cu(ous) 2.851 5.436 2.222 0.629 0. O.lSl 0.193 o. 141 O.O4O 2. 5 I -955 6.015 I.42I 534 0. 186 O.I24 0.213 O.OOO 0.034 5 1.522 7.525 1.008 5M 0. 373 0.097 0.267 0,069 0.033 10 1.236 n-735 0.475 o .761 0. 746 0.079 0.416 0.030 0.048 20 1.446 21.356 0.324 I .122 I. 492 0.092 0.759 0.021 O.O7I 5 2.411 not det. 0. 1088 2 .302 3- 730 0.153 not det. O.OO7 o. 146 100 4.702 M o.ooo 4 .702 7- 460 0.299 n 0.000 0.209 2OO 9-485 11 0.000 9 .485 14- 920 0.603 it 0.000 0.603 1000 97.0 it 0.000 97 .O 74- 60 6.170 ft 0.000 6.170 2OOO 384.0 tt 0.000 384 .0 149. 2 24.42 tt 0.000 24.420 SOLUBILITY OF COPPER CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE. (Hunt Am. J. Sci. [2] 49, 154, '70.) Grams CuCl 2 per 100 cc. Solution of: II 40 90 Sat. NaCl. 8.9 11.9 16.9 15% NaCl. 5% NaCl. I.I 2.6 127 COPPER CHLORIDE SOLUBILITY OP COPPER CHLORIDE AND POTASSIUM CHLORIDE DOUBLE SALTS AND MIXTURES IN WATER. (Meyerhoffer Z. physik. Chem. 5, 102, '90.) 39-4 49-9 60.4 79.1 90-5 93-7 98.8 o 39-6 50.1 5 2 -9 60.2 72.6 64.2 72-5 Cl per i Gram Solution. Present as Present as' CuCl 2 . KC1. O.I2O o . 107 0.129 O.II5 0.142 0.125 0.168 0.142 0.188 0.154 0.194 0.156 0.197 O.l62 0.214 0.021 0.232 O.O49 0-233 0-059 0.241 O.O62 0.246 0.066 0-255 0.063 Mols.penoqMols.HzO. CuCl 2 . KCl. 5.56 9-93 6 39 ii. 4 7.71 13.6 n. i 18.8 14.9 24.4 16.2 26.0 17.5 28.7 9.84 1.94 12.9 5-44 13-7 6.90 14.8 7-63 15.8 8.49 16.8 8-35 14.9 n. 6 14.8 15.0 Solid Phase. CuCl 2 .2KC1.2H 2 + Kd CuCl 2 .KCl + KC1 CuCl 2 .2KC1.2H 2 H- Cud 2 .2H 2 O CuCl 2 .KCl + CuCl 2 . 2 H 2 O CuCl 2 . 2 KC1.2H 2 O + CuCl 2 .KCl CuCl 2 JCCl SOLUBILITY OP CUPRIC CHLORIDE IN SEVERAL SOLVENTS. (Etard Ann. chim. phys. [7] 2, 564, '94; de Bruyn Z. physik. Chem. 10, 783, '92; de Coninck Compt.rend. 131, 59, 'oo; St. von Laszczynski Ber. 27 2285, '94.) Solvent. Methyl Alcohol Ethyl Alcohol Propyl Alcohol Iso Propyl Alcohol n Butyl Alcohol Allyl Alcohol Ethyl Formate Ethyl Acetate Acetone (abs.) Acetone (80%) Ether * (CuCl 2 .2 Aq.) For the solubility of cupric chloride in mixtures of a number of organic solvents, see de Coninck. Grams CuCl 2 per 100 Grams Sat. Solution at: 0. 15. 20. 4 0. 80. 36 40. 5 (de B.) 36 5 37 O 32 35- o (deB.) 35 7 39 O 29 30 5 30 5 . . . ... * 16 o 30 .0 15 15 3 16 .0 16 5 23 23 .0 . 10 9 .0 8. o ... . . . 3 .0 2 5 I 3 ( 72) 8.86* 8. 9 2 t 2 .88 (18) .. i .40 (56; 18 9* . o. 043 () o .11 . q.) f (CuCl 2 .2 Aq.) t (23 CuCl 2 .2 Aq.) COPPER CHLORIDE 128 IN AQUEOUS ALCOHOL AT 11.5. Chem. 22, 507, '97.) indicated amounts of CuCl 2 were The solutions shaken two hours, SOLUBILITY OF CUPRIC CHLORIDE (Bodtker Z. physik. 10 gms. of CuCl 2 2H 2 O and the added to 20 cc. portions of alcohol. 5 cc. portions withdrawn. Vol.% Gms.CuCl 2 Gms. per 5 cc. Solution. Alcohol. Added. H 2 O. CuCl 2 ." 89.3 o.o 0.794 I - I 37 92.0 o.o 0.648 1.090 96.3 o.o 0.478 1.116 99.3 o.o 0.369 i. 208 COPPER NITRATE (ic) Cu(NO 3 ) 2 . SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichanstalt, 3, 440, 'oo.) Vol. % Gms. CuCl 2 Alcohol. Added. Gms. per 5 cc. Solution. H 2 0. CuCl 2 . ' 99-3 0.223 0.330 1.295 99-3 0.887 0.247 1.639 99-3 1.540 O.I9I 2.086 99-3 i-957 0.164 2.400 Gms. Mols. Gms. Mols. Cu(N0 3 ) 2 Cu(N0 3 ) 2 t . per 100 Gms. per 100 Solid Phase. Solution. Mols. H 2 O. Cu(N0 3 ) 2 Cu(N0 3 ) 2 t . per 100 Gms. per 100 Solid Phase. Solution. Mols. H 2 O. 23 36 .08 5 , 42 Cu(NO3)2^H2O 20 55 58 12 .0 Cu(NO 3 ) 2 .6H 2 O 20 40 .92 6 .65 26.4 63 39 16 7 " . 21 39 S 2 6 27 Cu(N03) 2 .6H 2 25 60 .01 14 4 Cu(N0 3 ) 2 . 3 H20 45 .00 7 ,8 7 40 61 5i I 5 .2 " + 10 48 79 9 J 5 60 64 17 17 .2 18 53 ,86 ii 20 80 67 5i 20 O II4-5 77 59 33 3 to Density of solution saturated at 18 = 1.681. COPPER SULPHATE CuSO 4 .5H 2 O. SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 528, '94; Patrick and Aubert Trans. Kansas Acad. Sci. 19, '74 ; 15, Cohen Z. Electrochem. 9, 433, '03; at 25, Trevor Z. physik. Chem. 7, 470, '91.) Gms. CuSO 4 per too Gms. I . 10 Solution. 12-5 14.8 Water. 14-3 17.4 20 25 17.2 I8. 5 20-7 22-7 30 40 20-0 22-5 25.0 28-5 50 25.0 33-3 i . Solution. Water. 60 28.5 40-0 80 35-5 55-o 100 43-o 75-4 120 44-o 78.6 140 44-5 80.2 160 44.0 78.6 180 43-o 75-4 SOLUBILITY OF COPPER SULPHATE IN AQUEOUS SOLUTIONS OF SUL- PHURIC ACID AT o. (Engel Compt. rend. 104, 507, '87.) Grams per 100 Grams Milligram Equiv. per 10 Gms. H 2 O. Sp. Gr. of H 2 SO 4 . CuSO 4 . OU1UUU11S. H 2 S0 4 . CuSO 4 . o.o 18.6 1.144 o.oo 14-85 4.14 17.9 1. 143 2.03 14.29 14.6 19.6 1.158 7.16 15.65 31-0 12.4 1.170 15.20 9.90 54-2 8.06 1-195 26.57 6-43 5 6 -25 7-75 I. 211 27-57 6.19 71.8 5-o 1.224 35-2 3-99 1 29 COPPER SULPHATE SOLUBILITY OF COPPER SULPHATE IN AQCJEOUS SOLUTIONS OP AMMO- NIUM SULPHATE AT o. (Engel Compt. rend. 102, 114, '86.) Milligram Equiv. per Grams per 10 cc. Solution. fP- ^ r - 100 cc. Solution. Solutions. (NH 4 ) 2 SO 4 . CuSO 4 . (NH 4 ) 2 SO 4 . CuSO 4 . o.o 18.52 5-45 20.15 7.0 10.5 7.4 9.1 8.45 6.425 n-35 3-7 18.6 1.178 31.2 i.o .144 o.o 14-79 .190 3.61 16.09 .108 4.63 8.38 099 4.90 7.26 8l 5 5-59 5-13 .071 7.51 2.95 .082 12.31 0.94 .116 20.65 0.80 MIXTURES OF COPPER AMMONIUM SULPHATE AND NICKEL AMMONIUM SULPHATE IN WATER AT 13 1 4. (Fock Z. Kryst. Min. 28, 394, '97.) CuSO 4 .(NH 4 ) 2 SO 4 .6H 2 O NiSO 4 .(NH 4 ) 2 SO 4 .6H 2 O. Mol. % in Solution. Mols. per 100 Mols. H 2 O. Mol. % in Solid Phase. CuT Salt. Ni Salt. Cu Salt. Ni Salt. ' Cu. Salt. Ni Salt. o OO 100 .00 O .00 O .521 O .00 100 OO 33 34 66 .66 .1476 0.295 10 .29 8 9 71 56 05 43 95 O .2664 .2089 30-59 6 9 -41 73 .89 26 .20 .4165 .1449 52 23 47 77 79 .92 20 .08 o .4785 .1202 78 .80 21 .20 100 .00 O OO I 0350 o .00 100 .0 O .00 MIXTURES OF COPPER AMMONIUM SULPHATE AND ZINC AMMONIUM SULPHATE IN WATER AT i3-i4. (Fock.) CuSO 4 .(NH 4 ) 2 SO 4 .6H 2 O ZnSO 4 .(NHJ 2 SO 4 .6H 2 O. Mol.% in Solution. Mols. per TOO Mols. H 2 O. Mol. % in Solid Phase. Cu. Salt. Zn Salt. ' Cu Salt. Zn Salt." Cu. Salt. Zn Salt.' 4-97 95-03 0.0422 0.8069 2.39 97-61 10.65 89.35 0.0666 0.5638 4.52 95.48 19.24 80.76 0.1218 0.5115 9.03 90.97 30.19 69.81 0.2130 0.4924 14-67 85.33 44.44 55.56 0.3216 0.4022 22.62 77.38 100.00 o.oo I -35 o.ooo 100 o-ooo SOLUBILITY OF COPPER SULPHATE IN AQUEOUS SOLUTIONS OF MAGNESIUM SULPHATE AT o. (Diacon Jahresber. Chem. 61, '66.) Grams per 100 Gms.HzO. Solid Grams per ioo Gms. HzO. Solid CuS0 4 . "MgS0 4 . ' CuS0 4 . MgS0 4 . O 26.37 MgSO 4 .6H2O 12.03 15-67 CuSO 4 .sH20 2.64 25.91 " I3-6l 8.64 4.75 25.30 " 14-99 o.oo 9-01 23 . 30 MgSO 4 .6H2O + CuSO^sHaO COPPER SULPHATE 130 COPPER SULPHATE, MANGANESE SULPHATE, MIXED CRYSTALS AT 25. (Stortenbecker Z. physik. Chem. 34, 112, 'oo.) Gms. per 100 Gms. H 2 O. CuSO 4 . MnSOl. Triclinic Crystals with sH 2 O. 20. 2 O 19.76 3.69 I3-65 3I-52 ii. 61 39.41 Mols. per 100 Mols. H 2 O. Mn. ' Cu. 2.282 2.23 Mol. % Cu in Solution. Mol. % Cu in Crystals. I-3 1 O 0-44 3-76 4-70 9-39 46.77 i. 06 5-59 6.47 53-39 o-73 6-37 3.01 58 93 o-34 7-03 o.o 61.83 o.o 7-375 100 100 90.5 83-5 99-3 74.1 97-3 57-7 31.0 81 29.0 26.1 21.8 70.4 21 .2 42.6 20. o 34-4 15-9 13-45* 22.9 15.2* 10.27 10.5 4*6 4-9 2.31 2-15 o.o IOO.O Monoclinic Crystals with 7H 2 O. 9-39 46 77 i -06 6-47 53-39 -73 O-O o.o 5-58 6-37 8* 20. o J 3-45 10.27 4.6* o.o 28.2 23-5 20.8 16.0 S-8* 100 Indicates points of labil equilibrium. COPPER SULPHATE, ZINC SULPHATE, MIXED CRYSTALS IN WATER. (Stortenbecker Z. physik. Chem. 22, 62, '97.) Triclinic Crystals with sH 2 O. ols. per TOO I Aols. H 2 O. Mol.% Cu Mol.% Cu Cu. Zn. in Solution. in Crystals. 2.28 O 100 100 83 2.08 46.8 94-9 -41 3-60 28.1 86.4 .19 5-oi 19.2 77-9 .86 3-36 36.2 40.4 .22 4-45 21-5 29-5-3I-9 -01 4-72 17.6 24.1-28. 0.82 5-03 14.0 19.0-22. 0.51 5-59 8.36 12.4-14.9 0.30 5-56 4.87 7.02 o.o 6.42 o.o o 1.19 5-oi 19 2 5.01 0.51 5-59 8.^6 1.97 0.267 5-77 4.42 I-I5 o.o 5-94 o.o 0-00 Monoclinic Crystals with 7H 2 O. Rhombic Crystals with 7H 2 O. COPPER SULPHATE SOLUBILITY OF COPPER SULPHATE, SODIUM SULPHATE MIXTURES IN WATER. (Koppel Z. physik. Chem. 42, 8, 'oi-'o2; Massol and Maldes Compt. rend. 133, 287, '01.) Mols. per 100 Mols. . per Sol CuSO 4 . Na,S0 4 . CuS0 4 . Na 2 SO 4 . 13 .40 6 23 I .88 .98 10 14 .90 9 .46 2 23 I 56 15 15 .18 ii .64 2 23 2 .02 17 7 14 34 13 34 2 .24 2 34 23 .0 14.36 12 .76 2 23 2 .21 40 15 13-73 12 .26 2 .10 2 .10 17 7 14 99 13 .48 2 37 2 39 23 16 .41 II 35 2 57 I 99 40 .15 20 56 8 .0 3 -25 I 47 18 13 53 13 .84 2 .10 2 .41 20 II 34 15 .70 I .76 2 73 25 6 .28 21 .20 O .98 3 .70 30 2 .607 28 38 O 43 5 .21 33 9 I 475 32 30 O 25 6 .18 37 .2 I 494 3 1 .96 O 25 6 .08 30 5 38 22 17 .1 3 .69 25 37 3 i 57 32 .09 Solid Phase. CuSO 4 . 5 H 2 O + Na 2 S0 4 .ioH 2 O CuSO 4 .Na 2 SO 4 .6HjO 44 CuSO 4 .Na 2 S0 4 .6H2O + CuSO^sHzO CuSO 4 .Na 2 S0 4 .6H 2 O + Na,SO 4 .ioH 2 O CuSO 4 .Na 2 SO 4 .6H 2 O + increasing amts. of Na 2 SO 4 .ioH 2 O SOLUBILITY OF COPPER POTASSIUM SULPHATE CuK 2 (SO 4 ) 2 .6H 2 O m WATER AT 25. 100 grns. H 2 O dissolve 11.14 gms. CuK 2 (SO 4 ) 2 . (Trevor Z. physik. Chem. 7, 470, '91. SOLUBILITY OF COPPER SULPHATE IN METHYL AND ETHYL ALCOHOL, ETC. (de Bruyn Z. physik. Chem. 10, 786, '92; de Coninck Bull. acad. roy. Belgique, 257, '05.) Gms. per 100 Gms. Solvent. SOLUBILITY IN AQUEOUS Cuso 4 . CuS0 4 . 5 H 2 o. ALCOHOL AT i5 P . I .05 15 .6 (Schiff Liebig's Ann. 118, 365, '6i/> 0.93 0.40 Solvent. Methyl Alcohol Abs. 18 93-5% 18 50% 18 Abs. 3 Ethyl Alcohol Abs. 3 Glycol 14.6 Glycerine 15.5 Alcohof. Gms. CuSO 4 . 5 H 2 O per 100 g. Solvent. ... I.I ... 7 .6* 30.0 * Per 100 g. sol. 10 20 40 3-2 0.25 COPPER SULPHIDE CuS. SOLUBILITY IN AQUEOUS SUGAR SOLUTIONS. (Stolle Z. Ver. Zuckerind. 50, 340, f oo.) % Sugar in Solvent. Gms. per .Liter ol Aq. sugar ooiuuon M; ^i7-5. 45. 7S- 10 30 50 0.5672 0.8632 0-9076 0.3659 O.722O 1.0589 I-I345 1-2033 I . 2809 COPPEB TARTRATE 132 COPPER TARTRATE CuC 4 O 6 H 4 . 3 H 2 O. SOLUBILITY IN WATER. (Cantoni and Zachoder Bull. soc. chim. [3] 33, 7^1, '05.) t<>. Cms. per ioo cc. t. C Cms. :uC 4 6 H 4 . 3 H 2 per ioo cc. tv Cms. CuC 4 6 H 4 . 3 H 2 per ioo cc. Solution. Solution. Solution. 15 0.0197 40 0.1420 65 0.1767 20 o . 0420 45 0.1708 70 0.1640 25 0.0690 50 O.I92O 75 '. 0.1566 30 0-0890 55 0.2124 80 0.1440 35 0.1205 60 0.1970 85 0.1370 ORE80L C 6 H 4 (OH).CH 3 o, m and p. SOLUBILITY IN WATER AT 20. (Vauhel J. pr. Chem. [2] 52, 72, 'PS-) * ioo grams of the saturated aqueous solution contain : ^_ . * ^ 2.45 grams o cresol, 2.18 grams m cresol, 1.^94 grams p cresol. DISTRIBUTION OF CRESOL BETWEEN WATER AND ETHER. (Vaubel J. pr. Chem. [2] 67, 472. '03.) Composition of Solvent. Cms. Cresol in JJ 2 O Layer. In Ether Layer. 200 cc. H 2 O+ ioo cc. Ether -5Jf. I -0760 200 cc. 1^0 + 200 c.c. Ether o.oi^o i .1144 OUMINIC ACID C 3 H 7 C 6 H 4 .COOH (p Iso Propyl Benzoic Acid). SOLUBILITY IN WATER AT 25. (Paul Z. physik. Chem. 14, in, '94.) 1000 cc. sat. solution contain 0.1519 gm. or 0.926 millimol Cuminic Acid. PseudoOUMIDINE (CH ;! ) 3 .C 6 H 2 .NH 2 (sym. 5 Ammo, i, 2, 4, Trimethyl benzene). SOLUBILITY IN WATER. (Lowenherz Z. physik. Ch. 35, 412. *98.) t. 19.4. 23.7. 28.7. Cms. ^ Cumidine per liter H 2 O i . 198 j . 330 i .498 CYANOGEN CN. SOLUBILITY IN SEVERAL SOLVENTS AT 20. (Gay Lussac.) Solvent. Vols. CN per i Vol. Solvent. Water 4.5 Alcohol 23.0 Ether 5.0 Oil of Turpentine 5 -o 133 DIDYMIUM SULPHATE DIDYMIUM SULPHATE Di 2 (SO 4 ) 3 . SOLUBILITY IN WATER. (Marigrac Ann. chim. phys. [3] 38, 170, '53.) o t ._ Gins.HaO. 12 43-1 18 25.8 25 20.6 38 13.0 50 n. o " Gms.HjsO. Phase. ? 19 34-o II.7 Di,(S0 4 ) 3 .6H 2 O Di 2 (S0 4 ) 3 .8H 2 40 8.8 H 50 6.5 tt IOO 1.8 tt DIDYMIUM POTASSIUM SULPHATE K 2 SO 4 .Di 2 (SO 4 ),. 2 H 2 O. (Marignac.) ioo gms. H 2 O dissolve 1.6 grams double salt at 18. ERBIUM SULPHATE Er 2 (SO 4 ) 8 . SOLUBILITY IN WATER. (Hoglund.) ioo gms. H 2 O dissolve 43.0 gms. Er 2 (SO 4 ) 3 at o. ioo gms. H 2 O dissolve 23.0 gms. Er 2 (SO 4 ) 3 .8H 2 O at 20. EBYTHRITE CH 2 OH(CHOH) 2 CH 2 OH. ioo grams saturated solution in pyridine contain 250 gms. at 26. (Holty J. Physic. Chem. 9, 764, '35 v ETHANE C 2 H fl . SOLUBILITY IN WATER. (Winkler Ber. 34, 1421, 'ox.) t. ft. p. . 9 8 7 o O .8 0.74 o 54 7.0 .0 8 .0 O 5 1 1. 00 o 44 10. 03 10 -0 o 25 2.00 o .29 5-00 * Saturated 'with ethyl acetate. t Saturated with water. ioo cc. H 2 O dissolve 7.26 g. ethyl acetate at 28. (Euler Z. physik. Chem. 31, 360, '99.) ioo cc. H 2 O dissolve 9.26 cc. ethyl acetate at 20. ioo cc. ethyl acetate dissolve 2.94 cc. water at 20. ETHYL BUTYRATE C 3 H 7 COOC 2 H 6 . SOLUBILITY IN WATER AND IN AQUEOUS ETHYL ALCOHOL MIXTURES AT 20. ioo g. H 2 O dissolve 0.5 g. ethyl butyrate at 22. (Traube Ber. 17, 2304, '84.) ioo cc. H 2 O dissolve 0.8 cc. ethyl butyrate at 20. (Bancroft.) ioo cc. ethyl butyrate dissolve 0.4 0.5 cc. H 2 O at 20. Per 5 cc. ( cc. H 2 O 10 6 4 2.96 2.10 Ethyl Alcohol ( cc. C 3 H 7 COOC 2 H 5 0.34 0.96 2.47 4.00 6.0 ETHYL FORMATE HCOOC 2 H 5 . ioo grams water dissolve 10 grams'ethyl formate at 22. (Traube.) ETHYL PROPIONATE C 2 H 5 COOC 2 H 6 . SOLUBILITY IN WATER AND IN AQUEOUS ETHYL ALCOHOL MIXTURES. (Bancroft.) ioo grams H 2 O dissolve 1.7 grams ethyl propionate at 22. (Traube.> .... cc. HaO to cause separation of a second phase in cc. Aicoi ixtures of the given amounts of Alcohol and 3 cc. in Mixture. portions of Ethyl Propionate. 3 2 -32 6 6.87 9 I2 35 12 19-17 27.12 36.84 21 50.42 24 oo 3 1.42 39 53 -13 9 7.18 45 63.60 J S 14-13 57 90-53 21 22.40 72 131.0 27 31.62 81 180.0 33 41 .62 i 3 7 ETHTL VALERATE ETHYL VALERATE C 4 H 8 COOC 2 H 6 . ETHYL (Iso) VALERATE (CH,) 2 .CH.CH 2 COOC 2 H 6 . SOLUBILITY OF EACH IN WATER AND IN AQUEOUS ALCOHOL MIXTURES AT 20. (Bancroft.) ioo cc. water dissolve 0.3 cc. ethyl valerate at 25. 100 cc. water dissolve 0.2 cc. ethyl iso valerate at 20. ioo cc. ethyl iso valerate dissolve 0.4+ cc. water at 20. Mixtures of Ethyl Alcohol, Mixtures of Ethyl Alcohol, Ethyl Valerate and Water. Ethyl Iso Valerate and Water. Per 5 cc. Ethyl Alcohol. ec. Alcohol* cc.H20.t cc. Alcohol* cc.H^.f ' ~ " C c Ethyl " cc.H 2 0. IsoVal / rate . 10 0-15 8 0.23 6 0.46 5 0.72 4 1-23 * cc. Alcohol in mixture. t cc. H^ added to cause the separation of a second phase in mixtures of the given amounts of alcohol and 3 cc. portions of ethyl valerate. Di ETHYL KETONE (3 Pentanon) (C 2 H 5 ) 2 CO. SOLUBILITY IN WATER. (Rothmund Z. physik. Ch. 26, 433, '08 ) Determinations made by Synthetic Method, see page 9. Cms. Di Ethyl Ketone Cms. Di Ethyl Ketone t. per ioo Gms. t. per TOO Cms. Aq. Layer. Ketone Layer. Aq. Layer. Ketone Layer. 20 4 . 60 ... ioo 3 . 68 93-io 40 3-43 97-42 120 4-05 90.18 60 3.08 96.18 140 4.76 87.01 80 3.20 94-92 ioo 6.10 83.33 ETHYL BROMIDE C 2 H 6 Br. SOLUBILITY IN ETHER. (Parmentier Compt. rend. 114, 1002, '92.) t. 13. o. 12. 22.5. 32. G. C 2 H 5 Br per ioo gms. Ether 632 561 462 302 253 SOLUBILITY OF ETHYL BROMIDE, ETC., IN WATER. (Rex Z. physik. Chem. 55, 355, '06.) Grams per ioo Grams H 2 O at: Dissolved Substance. o. 10. 20. 30. Ethyl Bromide 1.067 0.965 0.914 0.896 Ethyl Iodide 0.441 0.414 0.403 0.415 Ethylene Chloride 0.922 o . 885 o . 869 o . 894 Ethylidene Chloride 0.656 0.595 0.550 0.540 ETHYL OARBAMATE 138 ETHYL OARBAMATE CO(OC 2 H 5 )NH 2 . (See also Urethane, p. 347.) SOLUBILITY IN SEVERAL SOLVENTS AT 25. (U. S. P.) Solvent. Water. Alcohol. Ether. Chloroform. Glycerine. Cms. CO(OC 2 H 5 )NH 2 ,, per 100 gms. solvent Ioo+ l66 77 33 ETHYLENE C 2 H 4 . SOLUBILITY IN WATER AND IN ALCOHOL. (Bunsen and Carius; Winkler Landolt and Bornstein, Tabellen, jd ed. p. 604, '06.) * - ft - Solubility in Alcohol, o 0.226 0.0281 . ~ t o Vols. C2H 4 per 5 O.IQI O.O237 100 Vols. Alcohol. 10 0.162 0.0200 o 359-5 15 0.139 0.0171 4 337.5 2O O.I22 O.OI5O IO 308.6 25 0.108 0.0131 15 288.2 30 0.098 0.0118 20 271.3 For )3 and q see Ethane, page 133. SOLUBILITY OF ETHYLENE IN METHYL ALCOHOL AND IN ACETONE. (Levi Gazz. chim. ital. 31, II, 513, '01.) Results in terms of the Ostwald Solubility Expression /. See p. 105. t. In Methyl Alcohol. In Acetone. t. In Methyl Alcohol. In Acetone. o 3-3924 4.0652 30 1-8585 1. 8680 10 2.8831 3-3580 40 I -343 2 1.0852 20 2.3718 2.6278 50 0.8259 0.2772 25 2.II54 2.2500 60 0.3506 The formulas from which the above figures were calculated are: In Methyl Alcohol, / = 3 .3924 0.05083 / o.ooooi t z . In Acetone, / = 4.0652 0.06946 / 0.000126 t 2 . FATS. SOLUBILITY OF THE FATTY ACIDS OBTAINED FROM SEVERAL SOURCES IN ALCOHOL AND IN BENZENE. (Dubois and Fade Bull. soc. chim. [2] 44, '85.) r* T?_i r* AI__ Gms. Fats per 100 Gms. Benzene at 12. 14.70 15.89 26.08 27.30 69.61 13-53 Crude Fatty Acid of: rai per 100 ^ Alcohol at: Tins. rt.DS. 0. 10. 26. Mutton 2,48 , S-o 2 ^7.96 Beef 2.51 6.05 8/T23 Veal 5.00 13-78 137.10 Pork 5-6 3 11.23 118.98 Butter 10. 61 24.81 158.2 Margarine 2-37 4-94 47.06 139 FUMARIO AOID FUMARIC ACID COOH.CH:CH.COOH. MALEIC ACID (CH) 2 (COOH) 2 . SOLUBILITY IN WATER. (Vaubel J. pr. Chem. [2] 59, 30, '99-) ioo gms. water dissolve 0.672 gram fumaric acid at 165. 100 gms. water dissolve 50.0 grains maleic acid at 100. FURFUROL C 4 H 3 OCHO. SOLUBILITY IN WATER. (Rothmund Z. physik. Chem. 26, 475, '98.) Determinations by Synthetic Method, for which see page 9. t o Gms. C 4 H3OCHO per ioo Gms. t02 2.55 Wt. % Alcohol. Vol. % Absorbed H. Wt. % Alcoh o.oo i-93 28.57 9.09 16.67 23.08 i-43 1.29 1.17 33-33 50-0 66.67 149 HYDROGEN SOLUBILITY OP HYDROGEN IN AQUEOUS SUGAR SOLUTIONS AT 15. (Gordon Z. physik. Chem. 18, 14, '95.) Gms. xoo Gms. C. 16.67 30.08 Gm. Mols. Sugar per Liter. 0.520 o-993 1.699 Absorption Coefficient of H. 0.01561 0.01284 0.00892 SOLUBILITY OF HYDROGEN IN WATER AND IN ORGANIC SOLVENTS. Results in terms of the Ostwald Expression, see page 105. (Just Z. physik. Chem. 37, 359, f oi.) Solvent. /25- /so. Amyl Acetate 0.0774 0.0743 Xylene 0.0819 0.0783 Ethyl Acetate 0.0852 0.0788 Toluene 0.0874 0.0838 Ethyl Alcohol (98.8%) o. 0894 o. 0862 Methyl Alcohol 0.0945 0.0902 Iso Butyl Alcohol 0.0976 0.0929 Solvent. Water Anilin Amyl Alcohol Nitro Benzene Carbon Bisulphide Acetic Acid Benzene Acetone /26- 0.0199 0.0285 0.0301 0.0371 0.0375 0.0633 0.0756 0.0764 0.0200 0.0303 0.0353 0.0353 0.0336 0.0617 0.0707 0.0703 SOLUBILITY OP HYDROGEN IN CHLORAL HYDRATE AT 20. SOLUTIONS (Knopp.) P. Normality (per 1000 Gms. H a O). Molecular Concentration. Absorption Coefficient of H. Density of Solutions. 4.91 0.310 0.005594 0.01839 I .O2O2 7.69 0.504 0.008992 0.01802 1.0320 14.56 1.030 0.018223 O.OI7I2 1.0669 29-50 2 -530 0-043601 0.01542 I.I466 38.42 3-770 0.063647 O.OI44O 1.1982 49-79 6.000 0.097493 0-01353 1.2724 63.90 10.700 o. 161660 0.01307 1-3743 SOLUBILITY OF HYDROGEN IN PROPIONIC ACID SOLUTIONS. (Braun.) G. C 2 HcCOOH Coefficient of Absorption of Hydrogen at: per 100 Gms. Solution. ' 5. 10. IS - 20. 25. 2.63 O.O2245 0.0214 O-O2OO 0.0188 0.0172 3-37 O.O222 O.O2I2 0.0199 0.0187 0.0171 5-27 0-0224 O-O2I2 0.0198 0.0184 0.0171 6.50 0.0218 o . 0209 0.0193 0.0183 0.0169 9.91 0.0213 0.0203 O.OI9I 0.0178 0.0160 SOLUBILITY OP HYDROGEN IN PETROLEUM. (Griewasz and Walfisz Z. physik. Chem. I, 70, '&J./ Coefficient of absorption at 20 0.0582, at 10 0.0652. HYDROGEN SULPHIDE {50 HYDROGEN SULPHIDE H 2 S. SOLUBILITY IN WATER AND IN ALCOHOL AT t AND 760 MM. PRESSURE. (Bunsen and Carius; Fauser Math, u Natur. W. Ber. (Ungarn.) 6, 154, '88.) In Alcohol. i Vol. Alcohol Absorbs 1 7 . 89 Vols. H 2 S(at o and 760 mm.) 14-78 11.99 9-54 7.42 5-96 (24) For ft and q see Ethane, page 133. SOLUBILITY OF HYDROGEN SULPHIDE IN AQUEOUS SALT SOLUTIONS In Water. t. i Vol . H 2 Absorbs /3. 3 . o 4-37 Vols. H 2 S(ato and 760 mm.) 4-686 0.710 5 3-97 M 4.063 0.6l5 10 3-59 H 3-520 0-530 15 3-23 H 3-056 0-458 20 2 .91 u 2.672 0.398 25 2 -6l " 30 2-33 It 35 2.08 " . . . 40 1.86 " AT 25. (McLauchlan Z. physik. Chem. 44 615, '03.) NOTE. The original results are given in terms of y which is the ^0 iodine titer (/) of the H 2 S dissolved in the salt solution divided by the titer (/ ) of the H 2 S dissolved in pure water. These figures were multi- plied by 2. 6 1 (see 25 results in preceding table) and the products recorded in the following table as volumes of H 2 S absorbed by i vol. of aqueous solution. Solution. Grams Salt I Vols. H 2 S per Liter, fo. per i Vol. Sol . Solution. Gms^Salt I Vols. H 2 S /. per i Vol .Sol n NH 4 Br 9 8. I. 00 2.61 n KBr 119.0 0. 945 2.47 n NH 4 C1 53- 4 0. 96 2.40 n KC1 74-5 0. 853 2. 22 n NH 4 NO 3 80. 0. 99 2.58 n KN0 3 IOI.O O. 913 2.38 in (NH 4 ) 2 SO 4 33- 0. 82 2.14 in K 2 S0 4 43-5 0. 78 2.04 In (NH 4 ) 2 S0 4 16. 5 0. 9i 2.37 in K 2 SO 4 21.7 0. 89 2.32 n NH 4 C 2 H 3 2 77- i I. 09 2.84 n KI 166.0 o. 98 2. 5 6 n (NH 2 ) 2 CO 60. i I. 02 2.66 n NaBr 103.0 0. 935 2.44 InHCl 18. 22 0. 975 2-54 n NaCl 58.5 o. 847 2. 21 n H 2 SO 4 24. 52 0. 905 2.36 in NaCl 29.2 0. 93 2.42 n C 4 H 6 O 6 150. 0. 944 2.46 n NaNO 3 85.0 0. 893 2.32 3 n C 4 H 6 O 6 45 0. 858 2.24 in Na 2 SO 4 35-5 0. 73 1.90 Pure C 3 H 5 (OH) 3 IOCX). o. 863 2.26 in Na 2 S0 4 17.8 0. 89 2.32 HYDROQUINONS C 6 H 4 (OH) 2 1:4, also Resorcin C 6 H 4 (OH) 2 1:3 and Pyrocatechin C 6 H 4 (OH) 2 1:2. SOLUBILITY IN WATER. (Vaubel J. pr. Chem. [2] 59, 30, 'oo.) ioo grams solution contain 6.7 grams hydroquinone at 20. Sp. Gr. of sol. = i. 01 2. ioo grams solution contain 63.7 grams resorcin at 20. TOO grams solution contain 31.1 grams pyrocatechin at 20. IS* HYDEOQUINONE SOLUBILITY OF HYDROQUINONE IN SULPHUR DIOXIDE IN THE CRITICAL VICINITY. (Centnerswer and Teletow Z. Electrochem. 9, 799, '03.) Determinations made by the Synthetic Method, for which see Note page 9. t o Cms. Hydroquinone t o Cms. Hydroquinone ^o Cms. Hydroquinone per IOQ Cms. Sol. per 100 Cms. Sol. per 100 Cms. Solution. 63 0.89 117.6 4.46 136.7 10.31 73-5 1-22 123.3 5-66 141-4 13-3 89.2 2.18 134.2 8.31 145.0 14.9 HYDROXYLAMINE NH 2 (OH). HYDROXYLAMINB HYDRO- CHLORIDE NH 2 (OH).HC1. SOLUBILITY IN SEVERAL SOLVENTS. (de Bpuyn Rec. trav. chim. n, 18, '92; Z. physik. Chem. 10, 783, 'yt.) Grams NH 2 OH Grams NH 2 (OH).HCl Solvent. t. per 100 Cms. t. per 100 Gms. Solution. Solvent. Methyl Alcohol (abs.) 5 35.0 19 .75 16.4 Ethyl Alcohol (abs.) 15 15.0 19-75 4-43 Ether (dry) (b. pt.) 1.2 Ethyl Acetate (b. pt.) 1.6 For densities of NH 2 (OH).HC1 solutions, see Schiff and Monsacchi Z. physik. Ch. 21, 277, '96. HYOSCYAMINE C 17 H 21 NO 3 . SOLUBILITY IN SEVERAL SOLVENTS AT i8-22. (Miiller Apoth.-Ztg. 18, 249, '03.) Gms. CnHnNOs Gms. Solvent. per 100 Gms. Solvent. per 100 Gms. Solution. Solution. Water -355 Chloroform 100+ Ether 2.02 Acetic Ether 4-903 Ether sat. with HO 3.913 Petroleum Ether 0.098 Water sat. with Ether 3.125 Carbon Tetra Chloride 0.059 Benzene o . 769 HYOSOINE HYDROBROMIDE, etc. SOLUBILITY IN SEVERAL SOLVENTS AT 25. (U.S. P.) . Grams per 100 Grams Solvent. Solvent. Hyoscine Hyoscyamine Hyoscyamine Hydrobromide C,7H 21 N04.HBr.3H 2 O. Hydrobromide CnHaNOa-HBr. Sulphate (C,7H 23 N0 3 ) 2 .H 2 S04. Water 66.6 very soluble very soluble Alcohol 6 . 2 So is-6 Ether 0-062 0.04 Chloroform o . 133 40.0 0.043 IODINE IODINE I. to Gms. I per Liter . Solution. 15 0.272-0.283 25 0.279 25 0.304 25 o-339 25 0.340 30 o-457 152 SOLUBILITY IN WATER. Authority. (Dietz Pharm. Ztg. 43, 290, '98.) (McLauchlan Z. physik. Chem. 44, 617, '03.) (Herz and Knoch Z. anorg. Chem. 45, 269, '05.) (Jakowkin Z. physik. Chem. 18, 590, '95.) (Noyes and Seidensticker Z. physik. Chem. 27, 359, '98.) (Dietz.) SOLUBILITY OF IODINE IN AQUEOUS POTASSIUM IODIDE SOLUTIONS AT 25. (Noyes and Seidensticker; Bruner Z. physik. Chem. 2<5 147, '98.) Millimols per Liter. KI. (I 2 ). o.ooo 1.342 0.830 I.8I4 1.661 2-235 3-322 3-052 6.643 4-667 13.29 8.003 26.57 14.68 53-15 28.03 106.3 55-28 Gms. per Liter. KI. 0.00 2-75 11.03 22.07 44-I5 88.3 176.6 I. 0.340 0.461 0.568 0-775 i 2 3 7 14.04 185 .032 .728 .119 Results by Bruner. Gms. KI per Gms. I 1000 g. Sol. per Liter. 10 0.78* 20 I 60 40 3-25 60 5 04 80 6.94 ioo 8.96 * There is some uncertainty in regard to the position of the decimal point in this column, lation from the original it should be one place further to the right. By calcu SOLUBILITY OF IODINE IN AQUEOUS SALT SOLUTIONS AT 25. (McLauchlan.) Salt. Gms. Salt Gms. Dissolved I per Liter. per Liter. Salt. Gms. Salt Gms. Dissolved I per Liter. per Liter. Na 2 S0 4 2 9 77 o .160 NH 4 C1 53 4 735 K 2 S0 4 43 5 o .238 NaBr 103 .0 3 .29 (NH 4 ) 2 S0 4 33 .0 .246 KBr 119 .0 3 .801 NaNO 3 -85 .0 o 257 NH 4 Br 98 .0 4 .003 KN0 3 101 .2 o .266 NH 4 C 2 H 3 2 77 .1 o .440 NH 4 NO 3 80 O 375 (NH 4 ) 2 C 2 H 4 86 9 o .980 NaCI 58 5 o 575 H 3 B0 3 55 .8 300 KC1 73 .6 o .658 SOLUBILITY OF IODINE IN ARSENIC TRI CHLORIDE. (Sloan and Mallet Chem. News, 46, 194, '82.) t. o. 15. 96. Gms. I per ioo gms. AsCl 3 8.42 11.88 36.89 153 IODINE SOLUBILITY OF IODINE IN AQUEOUS ETHYL AND NORMAL PROPYL ALCOHOL SOLUTIONS AT 15. (Bruner Z. physik. Chem. 26, 147, '08.) In Aq. Ethyl Alcohol. In Aq. Propyl Alcohol. Gms. Gms. Gms. Gms. Gms. Gms. Gms. Gms. per loo Gms. I per 100 CC. per 100 Gn ! I per IS. 100 CC. CsHyOH per 100 Gms. I per 100 CC. CsH 7 OH per 100 Gms. I per 100 CC. Solvent. Solution. Solvent. Sol. Solvent. Sol. Solvent. Sol. IO O.O5 60 I.I4 IO 0-05 60 2.71 2O O.o6 70 2-33 2O O.II 70 4-10 30 o.io 80 4.20 30 0-40 80 6.05 40 O.26 90 7-47 40 0-94 90 9.17 50 0-88 ICO x 5- 6 7 50 I .64 100 14-93 SOLUBILITY OF IODINE IN BENZENE, CHLOROFORM, AND IN ETHER. (Arctowski Z. anorg. Chem. n, 276, '95-'o6.) In Benzene. In Chloroform. In Ether. t o Gms. I per ioo Gms. Solution. A o Gms. * ' Gms. I per ioo Solution. A o Gms. I per ioo Gms. Solution. 4-7 8 .08 -49 o .188 -83 15. 39 6.6 8 63 -55* o .144 -90 14. 58 10.5 9 .60 -60 .129 -108 15 . 09 13-7 IO 44 -6 9 i o .089 16.3 ii 23 -73* o .080 + 10 I .76 per ioo gms. CHCL, (Duncan - - Pharm. J. Trans. 22, 544, 'pi-' SOLUBILITY OF IODINE IN BROMOFORM, CARBON TETRA CHLORIDE, AND IN CARBON BISULPHIDE AT 25. (Jakowkin Z. physik. Chem. 18, 590, '95.) i liter of saturated solution in CHBr 3 contains 189.55 i liter of saturated solution in CC1 4 contains 30.33 gms. I. i liter of saturated solution in CS 2 contains 230.0 gms. I. SOLUBILITY OF IODINE IN CARBON BISULPHIDE SOLUTIONS. (Arctowski Z. anorg. Chem. 6, 404, '94.) . o Gms. I per ioo ^ o Gms. Solution. Gms. I per ioo Gms. Solution. t. Gms. I per ioo Gms. Solution. IOO 0.32 7.89 30 19.26 -80 0.51 10 10.51 36 22.67 -63 1.26 15 12-35 40 25.22 2O 4.14 20 14.62 42 26.75 IO 5-52 25 16.92 IODINE 154 SOLUBILITY OF IODINE IN MIXTURES OF CHLOROFORM AND ETHYL ALCOHOL, CHLOROFORM AND NORMAL PROPYL ALCOHOL, CHLOROFORM AND BENZENE, AND CHLOROFORM AND CARBON BISULPHIDE AT 15. (Bruner.) Cms. CHC1 3 Grams I Dissolved per ioo cc. of Mixtures of: of Mixtures. C Hda+CaHfl OH. CH 3 C1 + C 3 H 7 OH . CHgCl + CeHfi. CH 3 CI -f CS 2 . IS-67 14-93 IO.4O 17.63 10 9-43 13.16 9.84 J 5-93 2O 8.69 II .20 8.78 14.20 30 7.80 8.98 7-74 12 .l6 40 7.09 8.09 6.96 10.20 50 6.62 7-82 6.20 9.08 60 6.24 7.09 5-34 7-72 70 5-77 6.42 4.89 6.42 80 5-o6 5-54 4-53 5-27 90 4-34 4-52 4.07 4-32 IOO 3.62 3-62 3-62 3.62 SOLUBILITY OF IODINE IN MIXTURES OF CARBON TETRA CHLORIDE AND BENZENE AND IN MIXTURES OF CARBON TETRA CHLORIDE AND CARBON BISULPHIDE AT 15. (Bruner.) Gms.CCUper Cms. I per loocc. of Mixture of: Gms.CCUper Gms.Iper loocc. of Mixture TSNTH Cl-mc r\f ^ A -w^^. nvo nf _ ^ Mixtures. CCU+CeHe. CC1 4 + CS 2 . J.UU VJII1S. Ul Mixtures. CCU + C 6 H 6 . CC1 4 +CS 2 . 10-40 17.6 60 4.90 5-55 10 9.44 14.44 70 4.09 4-5 20 8-53 "33 80 3-4i 3-37 30 7-77 10.34 90 2.74 2.60 40 6.63 8.60 IOO 2.06 2.06 50 5-7o 6.83 SOLUBILITY OF IODINE IN AQUEOUS GLYCERINE SOLUTIONS AT 25. (Herz and Knoch Z. anorg. Chem. 45, 269, '05.) Density of glycerine at 25/4 1-2555; impurities about 1.5%. Wt.% Glycerine Millimols I Grams I per Density of in Solvent, per ioo cc. Solution, ioo cc. Solution. Solutions at 2S/4. o 0.24 0.0304 Q-9979 7.15 0.27 0.0342 1.0198 20.44 0-38 0-0482 1.0471 31.55 0.49 0.0621 1-0750 40.95 0.69 0.0875 1-0995 48.7 1.07 0.135 1.1207 69.2 2. 2O 0.278 1.1765 100.0 9.70 1-223 1.2646 155 IODINE DISTRIBUTION OP IODINE BETWEEN CARBON BISULPHIDE AND AQ. POTASSIUM OXALATE. (Dawson Z. physik. Chem. 56, 610, '06; Dawson and McRae J. Chem. Soc. 8x, 1086, '02.) Concentration of .o Equiv. .o " .o " .2 Gms. I per Liter of Aq. Layer. 2.408 3-555 5.766 6.861 CS-z Layer. 10.82 16.32 27.91 34-Qi 17.07 Vol. of Solution which Contains i Mol. I. Fraction of I Uncombined in Solution. 105-3 71-37 0.005495 0.00561 43-99 36.98 71.97 0.005915 0.000055 0.005645 DISTRIBUTION OP IODINE BETWEEN AMYL ALCOHOL AND WATER AND BETWEEN AMYL ALCOHOL AND AQUEOUS POTASSIUM IODIDE SOLUTIONS AT 25. (Herz and Fischer Ber. 37, 4752, '04.) The original results were plotted on cross-section paper, and the following tables made from the curves. Millimols I per 10 cc. of H 2 O and of Aq. KI Layers. Amyl Alcohol Layer ~ N 2N N 4N ioN ""* in Each Case. HoO. K I . KI. KI* KI. *" " KJ 10 10 10 10 10 2-5 O-OI2 0-135 0.160 O.I7O O.I7O . . . 3-o O-OI4 0.150 0.185 O.2OO 0.200 0.160 4-0 0-OlS 0.180 0-235 0-255 0.270 0.240 5 O.O2I O.2IO 0.280 0-340 0-315 6 O.O25 0.230 0-330 o-375 O.4IO 0.390 7 O.O29 0.250 0-375 0.430 0.480 0.470 8 0.260 0.420 0.490 0-550 o-555 9 0.270 0.45 o-55o O.62O 0.640 10 0.280 0.470 0.605 0.690 0.720 12 0.490 0.700 0.830 0.900 14 0.510 0.790 0.980 1.200 20 0-575 Gms. I per loocc. Gms. I per ioo cc. of H 2 O and of KI Layers. Amyl Alcohol Layer f~ N aN ^N 4N ioN "^ in Each Case. HoO. KI. KI. KI ^~ yy KI IO IO 10 IO 10 3 0.014 O.l64 0.20 0.21 0.21 4 0.016 0.196 0.24 O.26 0.26 0.21 6 0.026 0.252 o-34 0-38 0.40 o-37 8 0-033 0-297 o-43 0-49 o-54 0.51 10 0-040 0.328 0.51 0.61 0.67 0.69 12 . . . 0.341 0.58 -73 0.81 0.84 14 0.60 0-83 o-95 1. 00 16 0.63 0.91 1.09 1.20 18 0.64 25 0.71 The original figures for sN/io and xoN/io KI solutions give prac- tically identical curves. Results for the distribution of Iodine between N/io KI solutions on the one hand, and mixtures in various proportions of C 8 H e + CS 2> C 6 H 5 CH 8 +CS 2 , C 6 H 6 +C 6 H 6 CH 3 , C 6 H 6 + light petroleum, CS 2 + light petroleum, CS 2 +CHC1 3 , CHC1 3 + C 6 H 6 , CC1 4 + CS 2 and CC1 4 + C 8 H 6 CH 3 on the other hand, are given by Dawson J. Chem. Soc., 81, 1086, '02, IODINE 156 DISTRIBUTION OF IODINE BETWEEN WATER AND BROMOFORM, WATER AND CARBON BISULPHIDE, AND WATER AND CARBON TETRA CHLORIDE AT 25. (Jakowkin Z. physik. Chem. 18, 590, '95.) Original results plotted on cross-section paper and table made from curves. Jakowkin points out that the results of Berthelot and Jungfleisch Ann. chim. phys. [4] 26, 400, '72, are incorrect on account of the presence of HI. Grams I per Liter of Grams I per Liter ot^ HjO Layer in Each Case. 0.05 O.IO 0.15 0.20 0.25 IODOFORM CHI 3 , IODOL CJ 4 NH (Tetra lodo Pyrrol). SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.; Vulpius Pharm. Centrh. 34, 117, '93.) CHBrs Layer. CS 2 Layer. CCU Layer. 2O 3<> 4-0 45 60 8-5 71 91 13.0 IOO 126 17-5 130 160 22.0 Solvent. t . Water 25 Alcohol 25 Alcohol b. pt. Ether 25 Chloroform 25 Grams per ioo^Grams Solvent. LaL CJ4NH. 0.0106 0.0204 2.14 (i .43 gms. (V.)) 1 1. 1 (lo.ogms. (V.)) ... 19.2 (!6.6gms. (V.)) 66.6 0.95 IRIDIUM DOUBLE Double Salt. Irido Pentamine Bromide " Bromonitrate " Tri Chloride " Chloro Bromide Chloro Iodide " Chloro Nitrate " Chloro Sulphate " Nitrate Aquo Pentamine Bromide Chloride " " Nitrate SALTS. SOLUBILITY IN WATER. (Palmaer Ber. 23, 3817; 24, 2090, '91.) Formula. Ir(NH 3 ) 6 Br 3 Ir(NH 3 ) 6 Br(N0 3 ) 2 Ir(NH 3 ) 5 Cl 3 Ir(NH 3 ) 6 ClBr 2 Ir(NH 3 ) 5 ClI 2 Ir(NH 3 ) 5 Cl(N0 3 ) 2 Ir(NH 3 ) s ClSO 4 .2H 2 O Ir(NH 3 ) 6 (N0 3 ) 3 Ir(NH 3 ) 5 (OH 2 )Br 3 Ir(NH 3 ) s (OH 2 )Cl 3 Ir(NH 3 ) 5 (OH 2 )(N0 3 ), Gms, per 100 t . Gms. HjjO. 12.5 0.284 18 5.58 15.1 6-53 15 0.47 15 o-95 15-4 1.94 15.0 0.74 16 0.28 ord. temp. 25.0 ord. temp. 74-7 17 IO.O IEON BROMIDE (Ferrous) FeBr2.6H 2 O. SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 537. '94-) t o Gms. FeBr 2 t <> per loo Gms. Sol. Gms. FeBr 2 t Gms. FeBr 2 per zoo Gms. Sol. per 100 Gms. Sol. 20 47-0 30 55-o 60 59 -o 50-5 40 56-2 80 61 .5 20 53-5 IOO 64.0 IRON CARBONATE (Ferrous) FeCO 3 . TOO gms. HjO saturated with CO 2 at 6-8 atmospheres dissolve 0.073 gram FeCO,. (Wagner Jahresber. Chem. 135, '67.) 157 IRON CHLORIDE IRON CHLORIDE (Ferrous) FeCl 2 . 4 H 2 O. (Etard.) SOLUBILITY IN WATER. 10 15 25 30 40 So Gms. FeCfe per loo Gms. Solution. 39-2 40.0 4i-5 42.2 43-6 45-2 Solid Phase. 60 80 87 90 100 1 20 Gms. FeCla per 100 Gms. Solution. 47-0 50.0 51.2 51-3 51-4 51-8 Solid Phase. FeCl 2 SOLUBILITY OF IRON CHLORIDE (Roozeboom Z. physik. (FERRIC) Fe 2 Cl 6 IN WATER. Chem, 10, 477, '92.) Mols. Fe 2 Cl Gms. FeCl 3 per 100 t. Der 100 Mols. Gms. H 2 0. H 2 0. Solution. Solid Phase, Fe-sCla.izHaO. -55 2 75 49 52 33 .12 -27 2 .98 53 .00 34 93 4 13 74 39 42 .66 + 20 5 .10 9i 85 47 .88 30 5 93 106 .8 5 1 .64 37 8 33 150 .0 60. 01 30 ii .20 2OI 7 66 85 20 12 83 231 .1 69 79 8 J 3 7 246 7 7i *5 Solid Phase, Fe 2 Cl6. 7 H 2 0. 20 ii 35 2O4 4 67 .14 32 13 55 244 .0 70 .92 30 15 .12 272 4 73 J 3 25 15 54 280 o 73 .69 Solid Phase, Fe 2 Cl6.5H 2 0. 12 12 .87 231 .8 69 87 27 14 85 267 5 72 .78 Mols. Fe 2 Cl6 Gms. FeCl 3 per 100 t. per 100 Mols. Gms. HaO. HaO. Solution. Solid Phase, FeaCle-sH zO (con.). 35 15 .64 28l .6 73 79 50 17 50 315 .2 75 .91 55 19 15 344 .8 77 52 55 20 32 365 9 78 54 Solid Phase, FeaCIe^HaO. 50 19 .96 359 3 78 23 55 20 32 365 9 78 54 60 20 .70 372 .8 78 .86 69 21 53 387 7 79 5o 73-5 25 .0 450 .2 81 .81 70 27 9 502 4 83 .41 66 29 .2 525 9 84 03 Solid Phase, Fe 2 Cle. 66 29.2 525.9 84.03 75 28.42 511.4 83.66 80 29.20 525.9 84.03 100 29.75 535-8 84.26 SOLUBILITY OF FERRIC CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM CHLORIDE AT 25, 35, AND 45. (Mohr Z. physik. Chem. 27, 197, '08.) Results at 25. Results at 35. Results at 45. Mols. per 100 Mols. HaO. Mols. per 100 Mols. H 2 O. Mols. per 100 Mols. H 2 O. . .Solid Phase NH4C1. O 10.98 NHiCl. O FeaCU. I3-36 NH4C1. o.o 33-4 FeaCU-iaHaO (s-HaO at 4 S) I .57 10.74 I.4I I3-05 Hydrate + Double Salt 2.48 9.02 3-08 9.28 4.08 9-58 Double Salt 5-28 7-73 6.98 7.64 - 9-59 6.77 10.76 6.70 13.09 6.31 H 9-83 6.70 II .60 6-52 13-54 6.28 Double Salt + Mixed Crystals 9-65 6.07 12.28 6.08 12.91 5-49 Mixed Crystals 9-93 5-23 II .57 3 -98 13-49 4.84 9.92 3-97 11.89 3-38 13.46 4-99 10.31 2.05 I3-23 i 38 * x 3-3 o.o 14-79 o.o 16.28 o.o NH*a IRON CHLORIDE IS8 SOLUBILITY OF FERRIC CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM CHLORIDE AT 15. (Roozeboom Z. physik. Ch. 10, 148, '92.) Mols.per TOO Mols.H2O. Grams per ipo Gms.H 2 O. Solid NH4C1. FeCl 3 . " NHiCl. FeCla,' Phase. O.O 9-30 0.0 83.88 FerClo.^HaO I -9 9-57 3- 2 4 86.32 J -3 6 9-93 4-03 9I.6l Fe2Cl6.i2H 2 -f- Double Salt 2 . OO 9.27 5 9 2 83 . 64 Double Salt 2.79 8.71 8. 3 I 78.77 4.05 8.09 12. 08 73-2O 6.41 7.18 19.12 64.83 10.78 6.21 32.04 56.00 7 .82 6.75 23 . 21 60 .83 Mixed Crystals containing 7.29% FeQ 3 7.62 5.94 22.63 53-47 " " 5.55 " 7.70 5.03 22.90 45-42 " " 4-4 " 7-8i 4-34 23.23 39.13 3 .8 (i 8.52 2.82 25.33 25.43 x . 64 10.95 - 68 32-55 6 - I 5 - - o. 3 i 11.88 0.0 35-30 0.0 NH4C1 SOLUBILITY OF FERRIC CHLORIDE IN AQUEOUS HYDROCHLORIC ACID SOLUTIONS AT DIFFERENT TEMPERATURES. (Roozeboom and Schreinemaker Z. physik. Chem. 15, 633, '94.) Mols. per too Mols. Gms. per 100 Gms. Mols. per 100 Mols. Gms. per 100 Gms. H,0. H 2 0. Solid H 2 0. H 2 0. Solid HC1. FeCl 3 . HC1. FeCl 3 . -^hase. HC1. FeCl 3 . HC1. FeCl a Phase Results at o. Results at 25 (con.). o 8.25 o 74-3' o.o 29.00 o.o 261.1" 7.52 6.51 15.22 58.62 7.5 29.75 15.18 267.9 - FC2 %> 13-37 6.33 27.06 57.01 19-5 35-25 39-46 317. 4 j 5-"2v-' 16.80 8.70 33.99 78-34 *9-5 35- 2 5 39.46 317. 4 > 18.45 J0.23 37-34 92-10 20.40 15.40 41.28 138.7 Fe 2 Cl 6 20.6 35-34 41-68 318.3 I2H2 3 I -34 41-58 63.42 374.4 Fe 2 Cl 6 20.10 16.00 40.67 144.1 33-oo 43-oo 66.77 387-3 19-95 J 7-70 40.37 J 59-4 34.65 44.80 70.11 403.4^ 19.00 22.75 38-45 2 4- 8 40.41 40.25 81.77 362.4' 18.05 23.41 36.53 210.8 J 39.03 41.38 78.98 372.7 * 62 .2HC1 18.05 23.40 36.53 210.8 ; Fe 2 Cl6 35.74 45-24 72.33 407.4- + 4H2O 19.50 25.93 39.55 233.5 \ 7H2O Results at 40. 24.12 30.04 48.81 270.5 26.00 32.16 52.60 289.6 26.00 32.16 52.60 289.6 34.60 38.11 70.01 343.2 37.27 36.60 75.41 329.6 , 34.60 38.11 70.01 343.2 ; ^HaO 32.4 0.0 291.7 ., _. 13-4 37-45 27.11 337.3 2 .4H 2 o I 3-4 37-45 27.11 337.3 Fe 2 Cl 6 2 7- 50.80 54.64 457.5 .2HC1 58.0 0.0 522.3' + 4 H20 27 5Q g 54 64 457 5 L Fe 2 Cl Results at 25. 42.01 48.64 85.00 438.0, 1 o.o 10.90 o.o 98. 151 42.50 47.52 86.72 428.0 2-33 23.72 4.715 213.6 K.^042.01 48.64 85.00 438.0 Fe 2 Cl 6 . 2 HC1 + 4 H 2 O.O 24.5 0.0 220. 7 J o.o 23.5 o.o 211. 6^| Results for other temperatures 2.33 23.72 4.715 213.4 |Fe 2 ci are also given in the 7.50 29.75 I 5- I 8 267.9 f - 7H2 paper. original o.o 31.50 o.o 283.6 J 159 IRON CHLORIDE SOLUBILITY OP THE SALT PAIR FeCl a .NaCl IN WATER AT 21. (Hinrichsen and Sachsel Z. physik. Chem. 50, 94, *o4-'os.) Grams Used. Gms. per 100 Gms. Solution. G. Mols. per iooMols.H 2 0. Solid FeCI a . NaCl. FeCl 3 . NaCl. ' Feds- " NaCl.' o 3.6 o 36.10 O 1 1 2 NaCl 1.8 3.0 24.27 9-10 2 . 69 2.8 Mix Crystals 3-6 2.5 25.40 8.45 2.8l 2.6 5-5 2.0 26.40 5 .25 2.93 2-54 7.2 1.5 3 8 - I 5 3-9o 4.23 1.22 9.0 i.o 45 -3 8 2.45 5-03 o-75 10.8 0.5 46.75 2. ii 5.18 0.65 10.8 o.o 83.39 o.o 9.3 O.O FeCli SOLUBILITY OF THE SALT PAIR FeCl 5 ,.KC1 IN WATER AT 21. (H. and S.) Grams Used. Gms. per xoo Gms. Solution. Gm. Mols. per 100 Mols. H 2 0. SoM Feda. KC1. FeCl 3 . KC1. FeCl 3 . " KCi: o 35 o 34-97 8.45 KCI 13 28 13.44 24.45 I . 49 5 9O Mix Crystals 18 21 23.18 16.54 2-57 3-99 23 i8-5 28.05 11-69 3-II 2.82 28 16 35.72 11.68 3.96 2.82 3i 10.5 36.62 11.19 4 . 06 2 . 70 Double Salt 36.2 9 37-35 r 3-67 4-14 3-30 46.5 6 5!- 6 9 7-54 5-73 1-82 J5-5 o 83.89 o.o 9.3 0.0 FeCl 3 SOLUBILITY OF THE SALT PAIR FeCl 3 .CsCl IN WATER AT 21. (H. and S.) Grams Used. Gms. per 100 Gms. Solution. Gm. Mols. per 100 Mols. H 2 O. Sond FeCli. CsCll ' FeCl 3 . CsCl. " 'Fed,.' CsCL o 65 o.o 65.0 O-O 6.95 CsCl 0.6 II. 6 0-45 55- 18 -5 5-9 FeCl 3 .CsCl.H 2 O 1.4 IO.2 2.1 5 2 -3 8 0.23 5.6 2.2 8.8 5.24 51.44 o-57 5-5 2.0 7.4 7.8 47-70 0.86 5.1 FeCl 3 .2CsCl.H 2 3.8 6.0 8.93 41.15 0.99 4.4 4.6 4.6 15-34 25.25 1.70 2.7 5-4 2.8 21.65 14.96 2.40 1.6 6.2 1.4 27.96 8.42 3.10 0.9 35.0 0.2 48.71 0.94 5.40 o.i 35.0 o.o 83.89 o.o 9.3 0.0 FeCls ioo gms. abs. acetone dissolve 62.9 gms. FeCl 3 at 18. (Naumann Ber.37, 4332, 04.) IBON NITRATE 160 IRON NITRATE (Ferrous) Fe(NO 3 ) 2 . Cms. SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichanstalt 3, 438, 'oo.) Mols. Cms. Mols. Fe(N0 3 ) 2 Fe(N0 3 ) 2 MM Fe(N0 3 ) 2 Fe(N0 3 ) 2 Solid t. per 100 Cms. per 100 Mols. Phase. t . per 100 Cms. per 100 Mols. Phase. Sol. H 2 0. Sol. H 2 0. -27 35-66 5-54 Fe(N0 3 ) 2 .oH 2 -9 39-68 6-57 Fe(NO 3 ) 2 .6H 2 O -21.5 36.10 5-64 u 41-53 7.10 -19 36-56 5-76 18 45-14 8-23 > - x s-s 37-17 5-9i M 24 46.51 8.70 " 60.5 62 .50 16.67 M Density of solution saturated at 18 = 1.497. IRON OXIDES, HYDROXIDE and SULPHIDE. 7n Suear in Sol- SOLUBILITY IN AQUEOUS SUGAR SOLUTIONS. (Stolle Z. Ver Zuckerind. 50, 340, 'oo.) One Liter of Sugar Solutions Dissolves Milligrams of: Fe 2 (OH) 6 at; FegOa at: Fe 3 O 4 at: FeS at: vent. 17.4. 45. 75. 17.5. 45. 17-5. 45. 75: ' 17.5. 45. 75. IO 3-4 3-4 6.1 1.4 2.0 10.3 10-3 12.4 3-8 3-8 5-3 30 2 -3 2.7 3-8 1-4 12-4 10-3 12.4 7-i 9.1 7.2 50 2-3 1.9 3-4 0.8 I .1 14-5 10-3 14-5 9-9 19.8 9.1 IRON PHOSPHATE Fe 2 (PO 4 ) 3 . THE ACTION OF WATER AND OF AQUEOUS SALT SOLUTIONS UPON FERRIC PHOSPHATE. (Lachowicz Monatsh. Chem. 13, 357, '92; Cameron and Hurst J. Am. Chem. Soc. 26, 888, '04.) The experiments show that the ordinary precipitation methods for the production of ferric phosphate give products which do not conform to the formula Fe 2 (PO 4 ) 3 . By digesting such samples with water very little is dissolved, but the material is decomposed to an extent depending upon the relative amounts of solid and solvent used. The amount of PO 4 dissolved per gram of Fe 2 (PO 4 ) 3 varies from about 0.0026 gram removed by 5 cc. H 2 O to 0.0182 gram removed by 800 cc. H 2 O at the ordinary temperature. IRON SULPHATE (Ferrous) FeSO 4 .7H 2 O. SOLUBILITY IN WATER. (Franckel Heidelberg '05, Landolt and Bernstein's Tabellen, 3d ed. p. 537, f o<5.) Gms. FeSO 4 , ,. . t . per 100 g ld Gms. H 2 O. Phase - 56.6 54-58 FeSO 4 .7H 2 + FeSO 4 .4H 2 O 00 70 75-8 80 90 t. Gms. FeS0 4 -,., oKSSb. St. -1.82 14.98 Ice+FeS0 4 .7H 2 O o 15.62 FeSO 4 .7H 2 O 10 20.85 20 26.42 30 33.00 40 40 . 20 5 48.55 55-02 56.04 56.8 FeSO 4 .4H 2 O -f FeSO 4 H 2 O 50.6 FeSCu-HjO 43.0 ioo grams sat. solution in Glycol contain 6.0 grams FeSO 4 at ordi- nary temperature. (de Coninck.) 161 IRON POTASSIUM SULPHATE IEON POTASSIUM SULPHATE (Ferrous) FeSO 4 .K 2 SO 4 .6H 2 O. SOLUBILITY IN WATER. (Tobler Liebig's Ann. 95, 193, '55.) 35 40 55 65 70 t. Cms. K2Fe(SO 4 ) 2 per 100 Grams H 2 0. o 19.6 10 24-5 14.5 29.1 16 30-9 25 36.5 per 100 Grams HjjO. 41 .o 45-o 56.0 57-3 64.2 SOLUBILITY OF MIXTURES OF FERROUS SULPHATE FeSO 4 .7H 2 O AND SODIUM SULPHATE Na 2 SO 4 .ioH 2 O IN WATER. (Koppel Z. physik. Chem. 52, 405, '05.) Cms. per 100 Gms. Cms. per 100 Cms. t. Solution. H 2 O. Solid Phase. FeS0 4 . Na 2 S0 4 . FeS0 4 . Na 2 s6 4 . O 14 54 4 93 18 .06 6 .11 FeSQ 4 .7H 2 O + Na 2 SO 4 .ioHaO 15-5 17 .76 II 32 25 05 15 97 21.8 16 57 15 32 24 34 22 5 1 FeNa-zCSO^^H^ 24.92 16 .21 15 13 23 .62 22 .04 " 35 16 35 14 .98 23 .91 21 83 " 40 16.37 15 .42 24 .01 22 .62 " 18.8 18 13 13 .8 26 63 2O .28 FeNa 2 (SO 4 )2-4H 2 O + FeSO^HjO 23 19 58 12 5 28 .82 18 4 27 20 97 II 3 30 95 16 .64 " 31 22 .91 9 .71 33 99 14 .41 4 < 35 23 85 9 .26 35 .61 13 85 4 ti 40 26 32 7 85 39-98 II .92 18.8 18 23 14 83 27 - 2 3 22 .16 FeNa 2 (SO 4 ) 2 4H 2 O + N a2 SO 4 .ioH 2 O 23 13 83 18 .04 20 .31 26 .48 28 7 .66 24 .41 ii .28 35 94 > 31 4 58 29 50 6 95 44 75 1C 35 4 .04 30-49 6 .16 46 58 FeNa 2 SO 4 4H 2 O + NaaSO 4 40 4 .10 30 .60 6 .27 46 99 M ti LANTHANUM BROMATE 162 LANTHANUM BROMATE La(BrO 3 ) 3 . 9 H 2 O. 100 gms. H 2 O dissolve 28.5 gms. lanthanum bromate at 15. (Marignac.) LANTHANUM SULPHATE La 2 (SO 4 ) 3 . -f 4/f y6 SOLUBILITY IN WATER. (Muthmann and Rolig Ber. 31, 1723, '98.) t. c rms.LaiiCSO^a per 100 Gms. Solution. Water. >ms. La 2 (SO 4 )3 per 100 Gms. Solution. Water. o 14 30 2.91 2-53 2.6 1.9 50 75 100 1.47 o-95 0.68 0.96 0.69 LEAD Pb. MUTUAL SOLUBILITY OF LEAD AND ZINC. (Spring and Romanoff Z. anorg. Chem. 13, 34, 'p6.) Upper Layer. Lower Layer. Upper Layer. Lower Layer. * jox %P 08 b. .8 %Zn/ I .2 % Pb. % Zn. %Pb. %Zn.' 6CO &2 O 1*7 O %P b. /-\ %Zn. c\ *? r\ 66** y u^u t^ . \j i i . 27 33 (3) 40 69.4 75 .0 41.9 10 44 4 48 3 31 .6 5 78.7 85 .0 45.0 17 50 .0 54 34 .2 60 88.0 95 .0 47-8 2O S 2 3 56 5 35 .2 80 107.6 "5 o 52-7 25 56 4 60 .6 36 9 100 127.0 138 .8 30 60 7 66 .0 38 .8 17 52.76* 34-54 51 * Euler. (i) Mulder, (2) Kremers, (3) Average of M and K. Density of saturated solution at 17 = 1.405. (Euler.) SOLUBILITY OP LEAD NITRATE IN ETHYL AND METHYL ALCOHOL. Cms. Pb(NO 3 ) 2 per 100 Grams Solvent at: Solvent. / * -v 4. 8. 22. 40. 50. Aq. C 2 H 6 OH (Sp. Gr. .9282) 4.96 5.82 8.77 12.8 14.9 (G) Abs. C 2 H 6 OH o. 04 (20.5) (de B) Abs. CH 3 OH 1.37 " (Gerardin Ann. chim. phys. [4] 5, 129, '65; de Bruyn Z. physik. Chem. 10, 783, '92.) SOLUBILITY OF MIXED CRYSTALS OF LEAD NITRATE AND STRONTIUM NITRATE IN WATER AT 25. (Fock Z. Kryst. Min. 28, 372, '97.) Mol. per cent in Solution. Cms. per 100 cc. Solution. Sp. Gr. of Mol. per cent in Solid Phase. Pb(N0 3 ) 2 . Sr(N0 3 ) 2 . Pb(N0 3 ) 2 . Sr(N0 3 ) 2 . Solutions. Pb(N0 3 ) 2 . Sr(N0 3 ) 2 . 100 .0 4 6 31 o.o I 4472 100 O .0 87.41 12 39 50 47 4-5 6 I 4336 99 05 95 78.68 21 32 53 .92 8.14 I .4288 9 8 .11 I .89 5 6 -39 43 .61 45 34 17.81 I .4263 97 .02 2 .98 60.29 39 7 1 44 .48 18.74 I 4245 96 .06 3 94 33-70 66 30 25 23 35-03 I .4468 83 .84 16 .16 24-58 75 .42 19 !3 37-54 I .4867 32 .88 67 .12 o.o 100 o o .0 71.04 I 5*41 100 .00 LEAD OXALATE PbC 2 O 4 . One liter of water dissolves 0.0015 gm. PbC 2 O 4 at 18 (conductivity method). (Bottger Z. physik. Chem. 46, 602, '03; Kohlrausch Ibid 50, 356, W-'os.) LEAD OXIDES. SOLUBILITY IN WATER. (Bottger; Ruer Z. anorg. Chem. 50, 273, '06.) No - Description of Oxide. " pe?L?ter. 1. Yellow Oxide, by boiling Pb hydroxide with 10% NaOH i . 03 X io~* o. 023 2. Red Oxide, by boiling Pb hydroxide with cone. NaOH 0.56X10"* 0.012 3. Yellow Oxide, by heating No. i to 630 1.05X10"* 0.023 4. Yellow Oxide, by heating No. 2 to 740 i.ooXio" 4 0.022 5. Yellow Oxide, by heating com. yellow brown oxide to 620 i . 09 X io~ 4 o. 024 6. Yellow Brown Oxide commercially pure i.ioXio" 4 0.024 7. Yellow Brown Oxide, by long rubbing of No. 5. 1.12X10"* 0.025 Bottger gives for three samples of lead oxide, 0.017, 0.021, and 0.013 gm. per liter respectively. i6 9 LEAD PALMITATE LEAD PALMITATE, LEAD STEARATE. 100 cc. absolute ether dissolve 0.0138 gm. palmitate and 0.0148 gm. stearate. (Lidoff Bull. soc. chim. [3] 10, 356, '93.) LEAD PHOSPHATE (Ortho) Pb 3 (PO 4 ) 2 . One liter of 4.97 per cent aqueous acetic acid solution dissolves 1.27 gms. Pb 3 (P0 4 ) 2 . (Bertrand Monit. Scknt. [3] io, 477. '68.) LEAD SUCCINATE PbC 4 H 4 O 4 . SOLUBILITY IN WATER AND IN ALCOHOL. (Partheil and Hxibner Archiv. Pharm. 241, 413, '03.) ioo gms. H 2 O dissolve 0.0253 gm. PbC 4 H 4 O 4 at 18, and 0.0285 gm. at 25. ioo gms. 95% alcohol dissolve 0.00275 gm. PbC 4 H 4 O 4 at 18, and 0.003 g m - a "k 2 5- Density of alcohol used = 0.8092. LEAD SULPHATE PbSO 4 . One liter of water dissolves 0.041 gm. PbSO 4 , by conductivity method. (Kohlrausch; Bottger. Dibbits Z. anal. Chem. 13, 139, '74, finds 0.038 gram by gravimetric method.) SOLUBILITY OF LEAD SULPHATE IN AQUEOUS SOLUTIONS OF STRONG ACIDS. (Schultz Pogg. Ann. 113, 137, '61; Rodwell J. Chem. Soc. 15, 59, '62.) In Aq. H 2 SO 4 . In Aq. HC1. In Aq. HNO 3 . (a). (&). (c). (a). (i). (c). (a). (6). (c). 1.540 63.4 0-003 J -793 85.7 O.OII 1.841 97.0 0.039 .05 10.6 0.14 i. 08 ii. 6 0.33 .08 16.3 0-35 1. 12 17.5 0-59 II 22.0 0.95 1.25 34.0 0.78 .14 27.5 2. II 1.42 6o.O I. 01 .16 31.6 2.86 (a) Sp. Gr. of Aq. Acid. (6) Gms. Acid per ioo Gms. Solution, (c) Gms.PbSO 4 per ioo Gms. Solvent. SOLUBILITY OF LEAD SULPHATE IN AQUEOUS SOLUTIONS OF AMMO- NIUM ACETATE AND OF SODIUM ACETATE. (Noyes and Whitcomb J. Am. Chem. Soc. 27, 756, '05; Dunnington and Long Am. Ch. J. 22, 217, '99; Dibbits Z. anal. Chem. 13, 139, '74.) In Ammonium Acetate. In Sodium Acetate. At 25 (N. and W.). At 100 (D. and L.). (D.). Millimols per Liter. Grams per Liter. ^ }.NH 4 C 2 H 3 O 2 G.PbSO 4 per ioo cc. per ioo g. Solution. Solution. Gms. per ioo Gms. H 2 O. z . PbSO 4 . NH 4 C 2 H 3 6 2 . PbS0 4 . NaC 2 H 8 O 2 . PbSO 4 . o.o 2O7.I 0.134 2.IO 4-55 o.o 7.98 15.96 O.O4I 0-636 L38 28 32 37 7.12 9.88 10.58 2.05 8.2 41.0 0.054 0.853 11.23 4I4.I 10.10 31.92 3.02 45 ii .10 LEAD (Hypo) SULPHATE 170 SOLUBILITY OP MIXTURES OF LEAD HYPOSULPHATE AND STRONTIUM HYPOSULPHATE AT 25. (Fock Z. Kryst. Min. 28. 389. '97 ) Mol. per cent in Solution. Grams per Liter. Sp. Gr. of Mol. per cent in Solid Phase PbSg. SrSzO." PbS 2 6 . SrS 2 6 . Solutions. PbS 2 6 SrSjOe ^HzO. -4H 2 O. .4!!^. 0.0 100. o.o 145.6 I .1126 o.o IOO-O 1.05 98.95 2-97 I5I.2 I .1184 0.30 99 7 15 .31 84-69 40.82 152.5 I-I503 3-87 96.13 46.80 53-20 149.2 II4-5 I.2I47 9.84 90.16 62.30 37-70 256.1 85.0 1.2889 19.26 80.74 75-75 24.25 310.3 67.0 I-3252 23-73 76.27 78.09 21 .91 373-7 70-8 1.3726 32.24 67.76 88.29 11.71 509-5 45 - 6 1.4671 49-97 50-I3 IOO-O O-OO 374-3 o.o 1.6817 o.oo 0-00 LEAD TARTRATE PbC 4 O 6 H 4 . SOLUBILITY IN WATER. (Cantoni and Zachoder Bull. soc. chim. [3] 33, 751, '05; Partheil and Hiibner Archiv. Pharm. 241, 413. '03-) f0 Cms. PbC 4 OeH4 per t o Gms. PbC 4 C>6H 4 per t o Cms. PbC 4 O . Water. Solution. O 151 60.2 10 157 61.1 20 165 62.2 25 I6 7 62.6 171 63.1 I Water. Solution. 40 179 64.2 5 I8 7 65-2 60 2O2 66.9 70 230 69.7 75 263 72-5 ioo grams sat. solution in Glycol (C 2 H 4 (OH) 2 .H 2 O) contain 28.0 grams Lil at 15.3. (de Coninck Chem. Centrb. 76, II, 883, '05.) ioo cc. saturated solution in Furfurol (C 4 H 3 O.COH) contain 45.86 gms. Lil at 25. ioo cc. saturated solution in Nitro Methane (CH 3 NO 2 ) contain 1.219 g ms - Lil at o, and 2.519 gms. at 25. (Walden Z. physik. Ch. 55, 713, 718, '06.) LITHIUM NITRATE LiNO 3 . SOLUBILITY IN WATER. (Donnan and Burt J. Chem. Soc. 83, 335, '03.) t o Gms.LiNO 3 per Solid ioo Gms. Solution. Phase. O.I 34-8 LiNO 3 .3H 2 10-5 12. 1 37-9 38-2 13-75 39-3 " 19.05 40.4 " 21 .1 42.9 " 27-55 47-3 " 29.47- 29.78 55-09 it t o Gms. LiNO 3 per Solid i oo G ms . Solution . Phase . 29.87 56.42 LiN0 3 .3H20 29.86 56.68 " 29.64 57-48 " 29-55 58-03 43 - 6 60.8 LiNOa.iHaO 5o-5 61.3 " 55-o 63.0 " 60.0 63.6 64.2 64.9 LiNOa 70.9 66.1 Cryohydrate point of the trihydrate, 17.8. Transition points, 29.6 and 61.1. LITHIUM OXALATE Li 2 C 2 O 4 . SOLUBILITY OF MIXTURES OF LITHIUM OXALATE AND OXALIC ACID IN WATER AT 25. (Foote and Andrew Am. Ch. J. 34, 153, '05.) Mixtures of the two substances were dissolved in water, and the solutions cooled in a thermostadt to 25. Gms. per ioo Gms. Solution. H 2 C 2 4 . ' Li 2 C 2 4 . 10.20 10.66 iQ-55 8.08 2.60 2.16 Mols. per ioo Mols. H 2 O. Solid 2.12 2 .96 3- 11 3 .l8 5-03 6-54 1.61 5-87 H 2 C 2 4 . Li 2 C 2 4 .' Phase. 2.274 H2C 2 4 .2H 2 2-457 O.622 H 2 C 2 4 .H 2 and HLiC 2 O 4 .I 1.823 o-5 6 3 0-633) 0.962) Double Salt HLiC 2 4 . 4 H 2 = 39.2H 2 C 2 O 4 and 44 -7 Li ; 0.469 1.273 HLiC 2 O 4 .H 2 O and Li 2 C 2 O 4 I .90! Li 2 C 2 4 LITHIUM PHOSPHATE 176 LITHIUM PHOSPHATE Li 3 PO 4 . 100 grams H 2 O dissolve 0.04 gram Li 3 PO 4 . (Mayer Liebig's Ann. 98. 193, '56.) LITHIUM (Hypo) PHOSPHATE Li 4 P 2 O 6 .7H 2 O. 100 grams H 2 O dissolve 0.83 gram hypophosphate at ord. temp. (Rammelsberg J. pr. Ch. [2] 45, 153, '92.) LITHIUM PERMANGANATE LiMnO 4 .3H 2 O. 100 grams water dissolve 71.4 grams permanganate at 16. (Ashoff.) LITHIUM SALTS of Fatty Acids. SOLUBILITY IN WATER AND IN ALCOHOL OF 0.797 SP. GR. AT 18 AND AT 25. (Partheil and Ferie Archiv. Pharm. 241, 554, '03.) Grams Salt per 100 cc. Sat. Solution in: Salt. Formula. Water at Alcohol at 18. 25. 18. 25. Stearate C 17 H 35 COOLi o.oio o.on 0.041 0.0532 Palmitate C 15 H 31 COOLi o-on 0.018 0.0796 0.0956 Myristate C 13 H 27 COOLi 0.0232 0.0234 0.184 0.2100 Laurinate C n H 23 COOLi 0.158 0.1726 0.418 0.4424 Oleate C^HggCOOLi 0.0674 0.1320 0.9084 i.oio LITHIUM SULPHATE Li 2 SO 4 . SOLUBILITY IN WATER. (Average curve from Kremers Pogg. Ann. 95, 468, '55; Etard Ann. chim. phys. [7] 2, 547, '94.) t o Gms. Li 2 SO 4 per 100 Gms. Solution t o Gms. Li 2 SO 4 per . zoo Gms. Solution t o Gms. Li 2 SO 4 per . 100 Gms. Solution. 2O 18.4 2O 25-S 50 24-5 10 24.2 25 25'3 60 24.2 O 26.1 30 25-1 80 23-5 IO 25-9 40 24-7 100 23.0 NOTE. For equilibrium between lithium sulphate ammonia and water, see Schreinemaker and Cochert Chem. Weekblad. 2, 771; 3, 157, '06. EQUILIBRIUM BETWEEN LITHIUM SULPHATE, ALUMINUM SULPHATE, AND WATER AT 30. (Schreinemaker and De Waal Chem. Weekblad. 3, 539, '06.) Composition in Weight per cent: Of Solution. Of Residue. Solid Phase. % Li 2 S0 4 . % A1 2 (S0 4 ) 3 . % Li 2 SO 4 . % A1 2 (S0 4 ) 3 . 25.1 O Li 2 SO 4 .H2O 21-93 5-34 ' 16.10 14.89 63.70 4-02 13-63 20.76 14.72 3 I -*7 | Li 2 S0 4 .H 2 + \ Al 2 (S0 4 ) 3 .i8H 2 13.24 21.71 61 .24 7.22 ii .73 22 .08 6.92 33-54 Al 2 (SO 4 ) 3 .i8H2O 6-75 24-34 3-77 37.06 3-44 26.12 o.o 28.0 ... NOTE. For solubility of lithium sulphate in mixtures of alcohol and water at 30, see Schreinemaker and Van Dorp, ]r. Chem. Week- blad. 3, 557, '06. I 7 7 MAGNESIUM BROMATE MAGNESIUM BROMATE Mg(BrO 3 ) 2 .6H 2 O. 100 cc. sat. solution contain 42 grams Mg(BrO 3 ) 2 , or 0.15 grammols. at 1 8. (Kohlrausch Sitzb. K. Akad. Wiss. (Berlin), i, 90, 'o?J MAGNESIUM BROMIDE MgBr 2 .6H 2 O. SOLUBILITY IN WATER. (Menschutkin Chem. Centrb. 77, I. 646, '06; at 18, Mylius and Funk Ber. 30, 1718, '97.) Grams MgBr 2 per 100 Gms. Grams MgBr 2 per icx> Grams. Solution. Water. Solution. Water. io 47.2 89.4 40 50.4 101.6 o 47-9 9 I -9 5 5 1 - I0 4-i io 48.6 94.5 60 51.8 107.5 18 49.0 96.1 80 53.2 113.7 18 50.8 103.4 (M. and F.) 100 54-6 120.2 20 49.1 96.5 120 56.0 127.5 25 49.4 97.6 140 58.0 138-1 30 49.8 99.2 . 160 62.0 163.1 Density of saturated solution at 18 = 1.655 ( M - and ?.) Etard Ann. chim. phys. [7] 2, 541, '94, gives solubility results which are evidently too high. SOLUBILITY or MAGNESIUM BROMIDE ALCOHOL COMPOUNDS IN THE CORRESPONDING ALCOHOLS. (Menschutkin Chem. Centrb. 77, I, 334, 647, '06.) In the Corresponding Alcohols. Results Expressed in Mols. per cent. . A -_v MgBr 2 .6CH 3 OH MgBr 2 .6C 2 H 5 OH in CH 3 OH. in C 2 H 6 OH. 6.0 2.0 20 6.4 4 .6 40 6.9 8. 4 50 7.2 10-9 60 7-5 I4.I 80 8-25 22.1 100 9.6 3 8.6 150 16.7 IOO.O (108.5) 190 IOO.O Determinations are also given for the solubility of MgBr 2 .6C 3 H 7 OH in C 3 H 7 OH, of MgBr 2 .6(CH 3 ) 2 C 2 H 3 OH in (CH 3 ) 2 C 2 H 3 .OH, and of MgBr 2 . 6(CH 3 ) 2 C 2 H 3 OH in (CH 3 ) 2 C 2 H 3 OH, also of MgBr 2 . 4 (CH 3 ) 2 ,CHOH in iso propyl alcohol and in tri methyl carbinol. For the solubility magnesium bromide mono etherate (MgBr 2 . (C 2 H 6 ) 2 O) in ethyl ether, see Menschutkin Chem. Centrb. 77, 1, 1868, '06; also Z. anorg. Ch. 49, 208, '06. For magnesium bromide di etherate (MgBr 2 .2C 4 H 10 O) in ethyl ether, see Menschutkin Z. anorg. Ch. 49, 35, '06. For magnesium bromide hexa formic acid and mag- nesium bromide hexa acetic acid compounds in anhydrous solutions of the corresponding acids, see Iswietja d. Petersburger, Polytechn. Inst. 5, 293, '06; Chem. Centrb. 77, II, 1482, '06. MAGNESIUM CARBONATE 178 MAGNESIUM CARBONATE MgCO,. SOLUBILITY IN WATER IN PRESENCE OF CARBON DIOXIDE AT 15* (Treadwell and Reuter Z. anorg. Ch. 17, 200, '08.) cc. CO2 per 100 cc. Gas Phase (at o and 760 mm.). Partial Pressure of CO S in mm. Hg. Grams per too cc. Solution. /"""" * Free CO 2 . MgC0 3 . Mg(HC0 3 ) 2 . Total Mg. 18.86 143-3 O.IIQO I.2I05 0.2016 5-47 41 .6 0.0866 I.2I05 0.2016 4-47 33-8 0.0035 I .2105 0.2016 i-54 11.7 0-0773 I .0766 0.2016 i-35 10.3 0-0765 0.7629 0.1492 1.07 8.2 . . . 0-0807 0-595 2 O.I224 0.62 4-7 . . . 0.0701 0.3663 0.0865 0.60 4-6 0-0758 0.3417 0.0788 o-33 2-5 0-0748 0.2632 0-0655 0.21 1.6 0.0771 O.2229 0-0594 0-14 i.i 0.0710 0.2169 0-0566 0.03 o-3 0.07II o . 2036 0-0545 0.0685 0.2033 0.0536 . . . 0-0702 0.1960 0.0529 0-0625 o . 2036 O.O52O 0-0616 0.1954 0.05II 0-0641 0.1954 0.0518 Therefore at o partial pressure of CO 2 and at 1 5 and mean barometric pressure, one liter of saturated aqueous solution contains 0.641 gram of MgCO 3 plus 1.954 grams Mg(HCO 3 ) 2 . SOLUBILITY OF MAGNESIUM CARBONATE IN WATER CHARGED WITH CAR- BON DIOXIDE AT PRESSURES GREATER THAN ONE ATMOSPHERE. (Engel and Ville Compt. rend. 93, 340. '81; Engel Ann. chim. phys. [6] 13, 349, '88.) Pressure of CO 2 in G. M :f?CO 3 * per Liter. Pressure of G. MgCO 3 * per Liter. Atmospheres. At 12. 0-5 20-5 At 19. Atmospheres. At 4.0 42 12. .8 At 19. I .0 26.5 25 .8 4 7 43 5 2-0 34-2 33 .1(2. i At.) 6 .0 5o .6 48 .5(6.2 At.) 3-o 39-o 37 2(3 .2 At.) 9 .0 56 .6 SOLUBILITY IN WATER SATURATED WITH CO 2 AT ONE ATMOSPHERE. (Engel.) t o Cms. MgCO 3 * t o Cms. MgCO 3 * t o Gms. MgCO 3 * per Liter. per Liter. per Liter. 5 3 6 3 2I 6o I]C 10 31 40 17 80 5 20 26 100 O * Dissolved as Mg(HCO 3 ) 2 . 179 MAGNESIUM CARBONATE SOLUBILITY OF MAGNESIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM CARBONATE AT 25. The solutions being in equilibrium with an atmosphere free from CO 2 . (Cameron and Seidell J. Physic. Ch. 7, 588, '03.) Wt. of i Liter Grams per Liter. Reacting Weights per Liter. of Solution. N a2 C0 3 . MgCOa. " NazCOs. MgC0 3 . 996.8 o.oo 0.223 o.ooo O.OO266 1019.9 23.12 0.288 0.220 0.00344 1047-7 50-75 0.510 0.482 O.OO62O 1082.5 86.42 0.879 O.82O 0.01027 1118.9 127.3 1-3*4 I .209 0.01570 1147.7 160.8 1.636 I .526 0.01955 1166.1 181.9 1.972 1.727 0.02357 1189.4 213 .2 2.317 2.024 0.02770 SOLUBILITY OF MAGNESIUM Bi CARBONATE AND OF MAGNESIUM CAR- BONATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE AT 23. The solutions being in equilibrium with an atmosphere of CO 2 in the one case, and in equilibrium with air free from CO 2 in the other. (C. and S.) In Presence of CO 2 as Gas Phase. In Presence of Air Free from CO 2 . Cms. NaCl per Liter. Gms. Mg(HCO 3 ) 2 per Liter. Wt. of i Liter. Gms. NaCl per Liter. Gms. MgCO 3 per Liter. 7-0 30.64 996.9 o.o 0.176 56.5 30.18 IOI6.8 28.0 0.418 119.7 27.88 I04I.I 59-5 0.527 163.9 24.96 1070.5 106.3 0.585 224.8 20.78 1094-5 147-4 0-544 306.6 10.75 II42.5 23I.I 0.460 II70.I 272.9 0-393 II99-3 331-4 0.293 SOLUBILITY OF MAGNESIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM SULPHATE AT 24 AND AT 35.5. The solutions being in equilibrium with an atmosphere free from CO 2 . (Cameron and Seidell.) Results at 24. Results at 35.5. Wt. of Gms. Na 2 SO 4 Gms. MgCO 3 Wt. of Gms. Na^O^ Gms. MgCO 3 i Liter. per Liter. per Liter. i Liter. per Liter. per Liter. 997.5 o.oo 0.216 995- 1 -3 2 0.131 1021.2 25.12 0.586 1032.9 41.84 0.577 1047.6 54-76 0.828 1067.2 81.84 o-753 1080.9 95-68 i .020 1094.8 116.56 0.904 1133.8 160.8 i .230 1120.4 I 48-56 0.962 1157.3 191.9 1.280 1151-7 l86 -7 1-047 1206.0 254.6 2.338 1179.8 224.0 i. 088 1242.0 305.1 1.388 1236.5 299.2 1.130 MAGNESIUM CHLORATE 180 MAGNESIUM CHLORATE Mg(ClO 3 ) 3 . SOLUBILITY IN WATER. (Meusser Ber. 35, 1416, '02.) Cms. Mols. Mg(C10 8 ) 2 Mg(C10 8 ) 2 pencx>Gms. per 100 Solution. Mols. H 2 O. 18 o 18 29 35 51.64 S3- 2 7 56-50 60.23 63-65 10.05 10.73 12.22 14.25 16.48 Solid Phase. Mg(C10 8 ) 8 .6H a O t. Gms. o Mg(C10 3 ) 2 Mols. Mg(C10 8 ) 2 Solid. * per 100 Gms Solution. per 100 Mols.H 2 O. Phase. 42 63 .82 16 .16 M g (C10 3 ) 3 ^H 3 65 5 69 .12 20 .08 " 39 5 65 37 17 -76 Mg(C10 8 ) a .aH 2 61 .0 6 9 46 21 40 it 68 70 .69 22 .69 93 (73 (26 38) M Sp. Gr. of saturated sol. at + 18 = 1.564. MAGNESIUM CHLORIDE MgCl 2 . SOLUBILITY IN WATER. (van "t Hoff and Meyerhoffer Z. physik. Chem. 27, 75, '98; Engel; Lowenherz. Results quoted from Landolt and Bornstein Tabellen, sd, ed. p. 549, '06.) Gms. MgClgper TOO Gms Solid t". Gms. MgC^penoo Gms" Solid * Solution. Water. Phase. Solution. Water. Phase. 10 ii .1 12 5 Ice O 34 5 52.8 MgCl 2 .6H 2 O 2O 16 .0 19 .0 " 10 34 9 53-5 " 30 19 4 24 .0 11 20 35 3 54-5 " 33- 6 20 .6 26 .0 Ice+MgCl 2 .i2H 2 O 22 35 .6 55-2 " 12 26 7 36 5 MgCl 2 .i 2 H 2 25 36 .2 56.7 " 16. 4 30 .6 44 f.pt. 40 36-5 57-5 " 16. 8 31 .6 46 .2 ( MgCl 2 .i2H 2 O + ( MgCl 2 .8H 2 O a 60 37 9 61.0 " 17- 19. 9- 3- 4 4 6 4 32 33 33 34 3 3 9 4 47 49 5 1 S 2 .6 9 3 3 ( MgCl 2 .i2H 2 O-f- \ MgCl 2 .8H 2 O/3 JMgCl 2 .i 2 H 2 + ( MgCl 2 .6H 2 O j MgCl 2 .8H 2 /3 t + MgCl 2 .6H 2 ( MgCl 2 .8H 2 O a + 1 MgCl 2 .6H 2 O about 80 100 116 152 181 39 42 7 46 6 49 5 55 .8 .2 .2 .1 .8 66.0 73-o 85-5 96.4 126.0 ( MgCl 2 .6H 2 O + { MgCl 2 . 4 H 2 G MgCl 2 . 4 H 2 f MgCl 2 .4H 2 + \ MgCl 2 . 2 H 2 186 56 .1 128.0 MgClz.aHaO SOLUBILITY OF MAGNESIUM CHLORIDE IN AQUEOUS SOLUTIONS OP HYDROCHLORIC ACID AT o. (Engel Compt. rend. 104, 433, '87.) Grams per Liter of Solution. Milligram Mols. per i occ. Solution. So.Gr of HC1. *MgCl 2 . Solutions. o.o 99-55 362 4-095 95-5 354 9-5 90.0 344 17.0 82.5 .300 20.5 79-o .297 28.5 71.0 .281 42 .0 60.125 58 v75 46.25 76.0 32.0 HCl. MgCW o.o 474.2 14.93 454-8 34.63 428.6 61.97 393-o 74-74 376.2 103.9 338.3 153 - 1 286.4 214.2 220.3 277.1 152.0 sat. HCl (Ditte) 6-S 181 MAGNESIUM CHLORIDE SOLUBILITY OP MIXTURES OF MAGNESIUM CHLORIDE AND OTHER SALTS IN WATER AT 25. (LSwenherz Z. physik. Chem. 13. 479, '94.) Mixture. MgCl 2 .6H 2 O + MgSO 4 .6H 2 O Gram Mols. per 1000 Mols. H2O. Gms. per Liter of Solution. 104 MgCL, + 14 MgSO 4 25.0 Cl + 4.4 SO 4 M g Cl2.7H 2 0-t-MgS0 4 .6H 2 73 +15 19.5 "+5.3 MgCl 2 .6H 2 + M g Cl 2 .KC1.6H 2 106 Cl+i K 2 +io 5 Mg 26.9 C1+ 0.3 K+ 45-7 SO 4 Results for the remaining possible combinations of magnesium sulphate and potassium chloride are also given. MAGNESIUM CHROMATE MgCrO 4 -7H 2 O. 100 grams H 2 O dissolve 72.3 grams MgCrO 4 at 18, or 100 grams solution contain 42.0 grams. Sp. Gr. = 1.422. (Mylius and Funk Ber. 30, 1718, '97.) MAGNESIUM POTASSIUM OHROMATE MgCrO 4 .K 2 CrO 4 .2H 2 O. 100 grams H 2 O dissolve 28.2 grams at 20, and 34.3 grams at 60. MAGNESIUM PLATINIC CYANIDE MgPt(CN) 4 . SOLUBILITY IN WATER. (Buxhoevden and Tamman Z. anorg. Ch. 15, 319, '97.) Gms.MgPt(CN) 4 t. per loo Gms. Solid Phase. Gms. MgPt(CN) 4 t . per 100 Gms. Solid Phase. Solution. Solution. -4.12 24.90 MgPt(CN) 4 .6.8-8.iH2O 48.7 40.89 MgPt(CN) 4 . 4 H 2 o-5 26.9 " (Red) 55 41-33 (1 5-5 28.65 " 58-1 42.15 II 18.0 32.46 " 69.0 43-49 36.6 39-53 77 .8 44.90 " 4S-o 4i-33 87.4 45-5 2 46.2 42 .0 " 9O.O 45-05 " 42.2 40.21 MgPt(CN) 4 . 4 H20 93-o 45-04 46-3 39-85 " (Bright Green) 96.4 44-33 MgPt(CN) 4 .aH 2 100. 44.0 (White) MAGNESIUM FLUORIDE MgF 2 . One liter of water dissolves 0.076 gram MgF 2 at 18 by conductivity method. (Kohlrausch Z. physik. Ch. 50, 356/04- '05. MAGNESIUM HYDROXIDE Mg(OH) 2 . One liter of water dissolves 0.008 0.009 S m - Mg(OH) 2 at 18 by Conductivity method. (Dupre and Brutus Z. angew. Ch. x6> SS, W SOLUBILITY OF MAGNESIUM OXIDE IN AQUEOUS SOLUTIONS CONTAINING SODIUM CHLORIDE AND SODIUM HYDROXIDE. (Maigret Bull. soc. chim. 33, 631, '05.) Grams MgO per Liter Solution with Added: per Liter. 125 140 160 0.8 g. NaOH per Liter. O.O7 0-045 none 4.0 g. NaOH per Liter. 0.03 none MAGNESIUM HYDROXIDE 182 SOLUBILITY OF MAGNESIUM HYDROXIDE IN AQUEOUS SOLUTIONS OF AMMONIUM CHLORIDE AND OF AMMONIUM NITRATE AT 29. (Herz and Muhs Z. anorg. Ch. 38, 140, '04.) NOTE. Pure Mg(OH) 2 was prepared and an excess shaken with solutions of ammonium chloride and of ammonium nitrate of different concentrations. Concentration of NHjCl or of NH4NO 3 Acid Required for Liberated Normality of: (Normal.) ' NH 4 OHin2SCC. (Normal.) Mg(OH) 2 . NH 4 C1. 7 (NH 4 C1) 0.09835 0.156 0.388 o . 466 O.IIOS O.IO8 0.250 o-35 0.09835 0-089 0.172 0-233 O.IIOS 0.0638 0.106 o-i75 O.IIOS 0.049 O.O77I 0.35 (NEUNO8) O.IIOS 0.0833 0.1834 0.175 " O.IIOS 0-0495 0.076 Grams per Liter. Mg(OH) 2 . NH^Cl. 4-55 2 .60 1.86 i-43 20.86 13-39 9.21 5-67 4-13 i-45 6 -o9 MAGNESIUM IODATE Mg(IO 3 ) 2 . SOLUBILITY IN WATER. (Mylius and Funk Ber. 30, 1722, '97; Wiss. Abh. p. t. Reichanstalt 3, 446, 'oo.) Gms. Mols. Gms. Mols. t o Mg(T6 3 ) 2 Mg(I0 3 ) 2 Solid per 100 per 100 Mols. Phase. Gms. Solution. H 2 O. t o Mg(I0 3 ) 2 Mg(I0 3 ) 2 Solid per 100 per i oo Mols. Phase. Gms. Solution. H 2 O. O 3- 1 0.15 Mg(IO 8 )2.ioH 2 O O 6.8 o-34 Mg(I0 3 ) 2 . 4 H 2 20 IO.2 0-55 IO 6.4 0.30 " 30 17.4 I .01 18 7.6 0.40 " 35 21. 9 i-35 20 7-7 0.40 M 50 67-5 IO-O 35 8.9 0.47 " 63 12.6 0.69 " 100 19-3 I-I3 " Sp. Gr. of solution sat. at 18= 1.078. MAGNESIUM IODIDE MgI 2 . SOLUBILITY IN WATER. (Menschutkin Chem. Centrb. 77, I, 646, '06; at 18, Mylius and Funk Ber. 30, 1718, '97.) t o Grams MgI 2 per Solid " 100 Grams Solution. Phase. t o Gms. Mgla per ' 100 Grams Solution. 50.0 10 51 .65 18 53-o(59-7 M - andF -> 20 53-4 2 5 54-4 30 55-4 40 57-8 45 59-9 Solid Phase. MgI 2 .8H 2 O 50 70 90 110 140 160 200 6l.6 61.85 62.1 62 .25 62 .5 63.0 64.1 MgI 2 -6H 2 Density of saturated solution at 18= 1.909. (M. andF.) 183 MAGNESIUM IODIDE SOLUBILITY OF MAGNESIUM IODIDE ALCOHOL COMPOUNDS IN THE CORRESPONDING ALCOHOLS. (Menschutkin Chem. Centrb. 77, I, 335, '06.) Results expressed in molecular per cent. t o MgI 2 .6CH 3 OH MgI 2 .6C 2 H 5 OH t > MgI 2 .6CH 3 OH MgI 2 .6C 2 H 5 OH ' * ' in CH 3 OH. inC 2 H 8 OH. * ' in CH 3 OH. inQHjOH. o 6.3 2.3 ioo 10.5 19.7 10 6.6 3-1 120 II. 8 28.2 20 7.0 4.0 140 13.4 S3- 6 40 7.8 6.2 160 15.7 80.3(145) 60 8.6 9.3 180 18.7 100-0(146.5) 80 9.5 13.5 200 23.1 SOLUBILITY OF MAGNESIUM IODIDE Di ETHERATE (MgI 2 .2C 4 H 10 O) IN ETHYL ETHER. (Menschutkin Z. anorg. Ch. 49, 46, '06.) Synthetic Method used, see Results in the Critical page 9. Vicinity. Grams per TOO pms. Solution. Gms. per ioo Gms. Solution. MgI 2 . MgI 2 .2C4H 10 O. " ' MgI 2 . 5.4 1.45 2.2 37.3 19.4 29.3 ii. 8 2.43 3.7 38.5 22.45 34-4 15.6 3.46 5.3 38.5 26.07 39.9 18.1 5.4 8.3 38.5 29.8 45.7 20.4 7-55 "-6 3 8 32-8 5-3 22.2 11.28 17.3 Two liquid phases appear near the melting point of the magnesium iodide di etherate. The lower may be considered as a solution of ether in di etherate, and the upper as a solution of the lower layer in ether. The critical temperature is 38.5. Lower Layer. Upper Layer. Gms. per ioo Gms. Solution. Gms. per ioo Gms. Solution I . MgI 2 . MgI 2 . 2 C 4 H 10 0. ' i . MgI 2 . MgI 2 . 2 C 4 H lo O. 14.8 35-5 54-4 18.6 13-57 20.8 20. 35-8 54-8 23.2 14.4 22 . 1 28.4 35-5 54-4 24.4 14.6 22-4 33 35-7 54-7 32-4 15.82 24.2 35 35-3 54-i The solubility of double compounds of magnesium iodide and alkyl esters in the corresponding acetates is given by Menschutkin Chem. Centrb. 77, I, 647, '06. For the solubility of magnesium iodide hexa acetic acid compound in anhydrous acetic acid solutions, see Chem. Centrb. 77, II, 1482, '06. MAGNESIUM NITRATE 184 MAGNESIUM NITRATE Mg(NO 8 ) 2 . SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichanstalt 3, 437, 'oo.) Gms. Mols. Gms. Mols. Mg(N03) 2 Mg(NO ? ) 2 Solid Mg(N0 3 ) 2 Mg(N0 3 ) 2 Solid t per ioo Gms. Solution. per ioo Mols. Phase. t. per ioo Gms. Solution. per ioo Mols. H 2 0. Phase. -23 35-44 6 . 6 Mg(NOg) 2 .9H2O 40 45-87 10-3 Mg (N0s) 2 .6: 20 36.19 7-o 80 53.69 14.6 " -18 38-03 7-4 90 57-81 16.7 " -18 38-03 7.37 Mg(N0 3 ) 2 .6H20 8 9 63.14 2O-9 | - 4 5 39-50 7.92 77 5 65-67 23.2 V * o 39.96 8.08 67 67-55 25-1 ) + 18 42-33 8. 9 * Reverse curve. Sp. Gr. of solution saturated at 18 = 1.384. MAGNESIUM OXALATE Mg.C 2 O 4 .2H 2 O. One liter of water dissolves 0.3 gram MgC 2 O 4 at 18 (conductivity method) . (Kohlrausch Z. physik. Ch. 50, 356, '05.) MAGNESIUM (Hypo) PHOSPHATE Mg 2 P 2 O 6 .i2H 2 O. One liter of water dissolves 0.066 gram hypophosphate. (Salzer Liebig's Ann. 232, 114, '86.) One liter of water dissolves 5.0 grams magnesium hydrogen hypophosphate MgH 2 P 2 O 6 .4H 2 O. (Salzer.) MAGNESIUM SALICYLATE Mg(C 7 H 5 O 3 ) 2 . 4 H 2 O. One liter of saturated solution contains 8.015 grams of the salt. (Barthe Bull. soc. chim. [3] n, 519, '94.) MAGNESIUM FLUOSILICATE MgSiF 6 .6H 2 O. One liter of water dissolves 652 grams of the salt at 17.5. Sp. Gr. Of Solution = 1.235. (Stolba Chem. Centrb. 578, '??.) MAGNESIUM SULPHATE MgSO 4 . SOLUBILITY IN WATER. (Mulder; Tilden J. Ch. Soc. 45, 409, '84; Etard Compt. rend. 106, 741, '88.) Etard's results for the lower temperatures are somewhat low. Mulder's and Tilden' s results agree very well. Gms. MgSOj per 100 Gms. Solid t<5 Gms. MgSO 4 per 100 Gms. g^d Solution. Water. Phase. Solution. Water. Phase. O 21.2 26.9 MgSO 4 .7H 2 O 50 33.5 50.3 MgSO^HzO 10 24.0 31.5 " 60 35.5 55.0 20 26.5 36.2 70 37.5 59.6 25 28.2 38.5 80 39-1 64.2 30 29.0 4O.9 " 9O 4O.7 .68.9 40 31.2 45.6 ioo 42.5 73.8 no 45-5 8 3-6 For temperatures between 123 and 190, grams MgSO 4 per ioo grams solution =48.5 0.4403 t. (Etard). For densities of aqueous solutions of MgSO 4 , see Barnes and Scott J. Physic. Ch. 2, 542, 'q8. 185 MAGNESIUM SULPHATE SOLUBILITY OF MAGNESIUM SULPHATE IN METHYL AND ETHYL ALCOHOLS. (de Bruyn Rec. trav. chim. n, 112, '92.) Solvent. t. Per 100 Gms. Solvent. Solvent. t. Per 100 Cms. Solvent. Abs. CH 3 OH 18 1.18 gms. MgSO 4 93% Methyl Ale. 17 9.7 gms.MgSO 4 .7H2O 17 41-0 " MgS0 4 . 7 H 2 50% " " 3-4 4.1 " 3-4 29.0 " " Abs. C 2 H 5 OH 3 1.3 " SOLUBILITY IN AQUEOUS ETHYL ALCOHOL. (Schiff Liebig's Ann. 118, 365, '61.) Wt. per cent Alcohol 10 20 40 G. MgSO 4 .7H 2 O per 100 gms. solvent 64.7 27.1 i .65 SOLUBILITY OF MAGNESIUM SULPHATE IN SATURATED SUGAR SOLUTION AT 31.25. (Kohler Z. Ver. Zuckerind. 47, 447, *97.) ioo grams saturated aqueous solution contain 46.52 grams sugar + 14.0 grams MgSO 4 . ioo grams water dissolve 119.6 grams sugar + 36.0 grams MgSO 4 . MAGNESIUM POTASSIUM SULPHATE MgK 2 (SO 4 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Tobler Liebig's Ann. 95, 193, '55.) t.-o 20 30 45 60 75 Gms. MgK 2 (S0 4 ) 2 per ioo gms. H 2 O 14.1 25.0 30.4 40.5 50.2 59.8 MAGNESIUM SULPHITE MgSO 3 .6H 2 O. ioo grams cold water dissolve 1.25 grams sulphite; ioo grams boil- ing water dissolve 0.83 gram. (Hager Chem. Centrb. 135, '75.) MALONIC ACID CH 2 (COOH) 2 . SOLUBILITY IN WATER. (Klobbie Z. physik. Chem. 24, 622, '97; Miczynski Monatsh. Ch. 7, 259, '86; Henry Compt. rend, 99, 1157, '84; Lamouroux Ibid. 128, '998, '99.) Grams CH 2 (COOH) 2 per ioo Grams CH 2 (COOH) 2 per ioo Gms. Solution.* cc. Solution (L.). Gms. Solution.* cc. Solution (L.). o 52-0 61.0 50 71.0 93 -o 10 56.5 67.0 60 74.5 loo.o 20 60.5 73 .o 70 ... 106.0 25 62.2 76.3 80 82.0 30 64.0 80.0 ioo 89.0 40 68. o 86.5 132 (m. pt.) 100-0 * Average curve from results of K., M., and H. MALONIC AOID 186 SOLUBILITY OP MALONIC ACID IN ETHER. (Klobbie.) fc. Gms. CH2. Gms. MnBrj per ioo Gms. Solution. Solid Phase. 20 52-3 MnBr^HaO 40 62.8 MnBr 2 . 4 H 2 O 10 54-2 " So 64-S 56-0 " 60 66.3 10 57-6 M 70 68.0 M 20 59-5 " 80 69.2 MnBr. 2 H 2 O 25 60.2 M 90 693 61.1 ioo 695 i8; MANGANESE CHLORIDE MANGANESE CHLORIDE MnCl 2 . 4 H 2 O. SOLUBILITY IN WATER. (Etard; Dawson and Williams Z. physik. Chem. 31, 63, '09.) f. 20 IO O + 10 2O 25 30 40 60 70 80 90 IOO 120 140 Sp. Gr. of Grams MnCl 2 per ioo Grams Jutions. Water. Solution. . . . 53-8 35-o . . . 58-7 37-o 63-4 38.8 68.1 40-5 73-9 42-5 4991 77.18 43-55 5049 80.71 44-68 5348 88.59 46.96 5744 98.15 49-53 .6097 105.4 5*-33 .6108 108.6 52.06 1.6134 no. 6 52-52 112.7 52.98 114.1 53-2 115 .3 53-5 118.8 54-3 119-5 55-o Mols. MnC! 2 per ioo Mols. H 2 O. II. 08 n-55 12.69 14.05 15.10 15-55 I5-85 16.14 Solid Phase. MnCl2.2H.jO One liter of water dissolves 87.0 grams MnCl 2 . One liter of sat. HC1 dissolves 19.0 grams MnCl 2 at i2 c (Ditte Compt. rend. 92, 242, '81.) MANGANESE FLUO SILICATE MnSiF 6 .6H 2 O. ioo grams H 2 O dissolve 140 grams salt at 17.5. Sp. Gr. of solution = 1.448. (Stolba Chem. Centrb. 292, '83.) MANGANESE NITRATE Mn(NO 3 ) 2 .6H 2 O. SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichanstalt 3, 438, f oo.) t. Gms. Mn(N0 3 ) 2 Mols. Mn(NO 3 ) 2 Solid per ioo Gms. Sol. per ioo Phase. Mols. H 2 0. -29 42.29 7-37 Mn(NO 3 ) 2 .6H 2 O. -26 43-15 7-63 " 21 44-30 8.0 " -16 45-52 8.4 - 5 48.88 9.61 M o 50-49 10.2 " + 11 54-50 12.0 " Sp. Gr. of solution saturated at 18 t. Gms. Mn(N03) 2 Mols. Mn(NO3) 2 per ioo Gms. Sol. per ioo Mols.H 2 O. 18 57-33 13.5 25 62.37 !6. 7 27 65.66 19.2 29 66.99 20.4 30 67.38 20.7 34 71 .31 24.9 35-5 76.82 33-3 DO 1.624. Solid Phase. Mn(NO 3 ) 2 .6H 2 O. MANGANESE (Hypo) PHOSPHITE Mn(PH 2 O 2 ) 2 H 2 O. ioo grams H 2 O dissolve 15.15 grams salt at 25, and 16.6 grams at b. pt. MANGANESE SULPHATE 188 MANGANESE SULPHATE MnSO 4 .5H 2 O. SOLUBILITY IN WATER. (Cottrell J. Physic. Ch. 4, 651, '01; Richards and Fraprie Am. Ch. J. 26, 77, *oi. The results f Linebarger Am. Ch. J. 15, 225, '93, were shown to be incorrect by Cottrell, and this conclusion as confirmed by R. and F.) Grams MnSO 4 per Grams MnSO 4 per t. ico^Gms. Solid Phase. t. 100 Gms. Solid Phase Water. Solution. ' Water. Solution r 10 47-96 32 .40 MnSO 4 .7H 2 O 16 63 94 38 99 MnSO 4 ^H 2 O 53-23 34 73 18 5 6 4 .19 39 .10 " 5 56.24 35 99 25 65 32 39 53 it 9 59-33 37 .24 3 66 -44 39 93 1 12 61.77 38 .19 39 9 68 .81 40 77 " 14-3 39 .00 " 49 9 72 6 3 42 .08 " 5 58.06 36 . 69 MnSO 4 .sH 2 O 41 4 60 87 37 .84 MnSO 4 .H 2 O 9 59 -!9 37 .18 5 58 17 36 .76 " 15 61.08 37 .91 60 55 .0 35 .49 M 25 64-78 39 .31 70 52 o 34 .22 " 67.76 40 .38 80 48 .0 3 2 43 35-5 71.61 4i 74 90 42 5 29 83 " 100 32 .0 24 .24 " SOLUBILITY OP MANGANESE SULPHATE, COPPER SULPHATE MIXED CRYSTALS IN WATER AT 18. (Stortenbecker Z. physik. Chem. 34, 112, 'oo.) Mols. per 100 Mols. Mol. per cent H 8 0. Cu in : 'Cu. Mn. Solution. Crystals. Solid Phase, CuMnSO 4 . S H 2 O, Triclinic. 2.282 2.23 1-54 Mols. per 100 Mols. H 2 0. Mol. per cent Cu in: ^ ciT Mn. Solution. Crystals- Solid Phase, CuMnSO 4 . S H 2 O. Triclinic. [1.06 O 100 100 . . . 90.5 0.44 83-5 74.1 97-3 57-7 95 - 1 . . . 31.0 81.3 3-76 29.0 26.1 70.4 4.70 21.8 21 .2 42 .6 20-0 34-4 5.58 15-9 22.9] 13 9 15-2* [0.73 -34 6.37 7-3 10.27 5.0 10.5] 4-9 2.15 2.31 7*^7^ O O O O / \j t %} Solid Phase. CuMnSO 4 . Monoclinic. ?H 2 O. 20-4 28.2* [1.06 5.58 15.9 23.5] 20.8 16.0] [o-73 6 -37 12-45 10.27 O-O 5-8* o.o * Indicates meta stabil points. CuMnSO 4 .5H 2 O = 100-90.8 and 2.11-0 mol. percent Cu. CuMnSO 4 .7H 2 O 37.8-4.92 mol. per cent Cu. SOLUBILITY OF MANGANESE SULPHATE IN GLYCOL. 100 grams saturated solution contain 0.5 gram MnSO 4 . (de Coninck Bui. acad roy. Belgique, 359, '05.) i8 9 MANGANESE SULPHATE SOLUBILITY OF MANGANESE SULPHATE IN AQUEOUS ETHYL AND PROPYL ALCOHOL SOLUTIONS AT 20. (Linebarger Am. Ch. J. 14, 380, '92; Snell J. Physic. Ch. 2, 474, '98.) Cone, of Alcohol Cms. MnSO 4 per 100 Cms. Aq. Cone, of Alcohol Gms. MnSO 4 per 100 Cms. Aq. in Wt. per cent. Ethyl Ale. Propyl Ale. in Wt. per cent. Ethyl Ale. Propyl Ale." 34 9-5 6 - 44 3-3 i-9 36 7.2 4.6 48 2.2 1.4 38 5.8 3.5 52 1.4 i.i 40 4-7 2.8 MANGANESE POTASSIUM VANADATE MnKV 6 O u .8H 2 O. 100 grains H 2 O dissolve 1.7 grams salt at 18. (Radan Liebig's Ann. 251, 120, '89.) MANNITE C 6 H 8 (OH) 6 . SOLUBILITY IN WATER. (Campetti Abs. in Z. physik. Chem. 41, 109, '02.) Grams CH8(OH)6 per 100 Grams. ' Water. Solution. " 10 13.94 12.78 15 16.18 14-63 20 18.98 16.86 100 grams of saturated solution of mannite in Pyridine contain 0.47 gram C 6 H 8 (OH) 6 at 26. (Holty- J. Physic. Ch. 9. 764, '05.) MANNITOL C 6 H 8 (OH) 6 . SOLUBILITY IN WATER. (Findlay J. Ch. Soc. 81, 1219, '02.) Gms. G.M. t o Wt. of i cc. Mannitol Mannitol t <> Wt. of i cc. in Grams. per 100 per 100 in Grams. Gms. Mannitol per loo G. M. Mannitol per loo Gms. H 2 0. G.M .H 2 0. Gms.H 2 O. G.M.H 2 0. O 1.044 7 59 O 75 50 1.099 (47-7) 47 .01 4.65 IO II 63 I . 60 60 .01 5-94 15 1.05 14 38 I 42 70 1.148 (68) 74 50 7-35 20 17 I 75 80 5 9.04 25 21 39 2 ii 9 1.207 (85-9) no .8 10.96 30 1.076(31.1 ) 2 5 .40 2 5 1 IOO 133 .1 I 3- I 7 40 35 .40 3 5 NOTE. In the original paper the author writes, " grams of sub- stance in zoo grams of solvent (percentage solubility) " and " moles of substance in 100 mols of solvent (percentage molar solubility)," thus implying equivalence of the terms and giving rise to uncertainty as to which is really intended. MERCURY BROMIDE (ic) HgBr 2 . SOLUBILITY IN WATER. g I .06 (Lassaigne J. chim. med. 12, 177, '76.) 25 O . 6l (Sherrill Z. physik. Ch. 43, 727. '03-) IOO 2O-25 (Lassaigne.) MERCURY BROMIDE 190 SOLUBILITY OF MERCURIC BROMIDE ORGANIC SOLVENTS. In Carbon Bisulphide. In Other Solvents at i8-2o. (Arctowski Z. anorg. Ch. 6, 267, '94.) t*. Cms. HgBr 2 per 100 Gms. Solution. t. Gms.HgBr 2 per 100 Gms. Solution. 10 - 5 0.049 0.068 0.087 I 5 20 25 0.140 0.187 0.232 + 5 0.105 30 0.274 10 0.122 (Sulc. Ibid. 25, 401, 'oo.) Solvent. Chloroform Bromoform Tetra Chlor Methane Ethyl Bromide Cms. HgBr 2 Formula. periooGms. Solvent . O.I26 0.679 0.003 2.31 CHC1 3 CHBr 3 CC1 4 C 2 H 5 Br Ethylene Di Bromide C 2 H 4 Br 2 2.34 Mercurous bromide Hg 2 Br 2 . One liter of saturated aqueous solution contains 0.000039 gram Hg 2 Br 2 at 25. (Shemii) MERCURY CHLORIDE (ic) HgCl 2 . SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 563, '94; at 25, Foote and Levy Am. Ch. J temp. Rohland Z. anorg. Ch. 18, 328' '98; see also Poggiale Ann. chim. 35t 238, '06; at room phys. [3] 8, 468, '43.) t . Gms. HgCl 2 per loo Gms. Solution. t. Gms. HgCl 2 per zoo Gms. Solution. t. Gms. HgCl 2 per 100 Gms. Solution. O 3-5 30 7-2 100 38.0 10 20 25 4-5 5 . 4 (6.88,R. 6.9 (F.andL.) 40 60 80 9-3 14.0 23.1 120 I4O J 5o 59-o 77.0 78-5 SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE. (Homeyer and Ritsert Pharm. Ztg. 33, 738, '88.) Per cent Concentration Gms ' H * C1 * ** I0 Gn - NaC1 ^"^ at: of NaCl Solutions. o-5 1.0 IO-O 25.0 26.0 (saturated) 128 ^5 65 100 10 13 44 14 18 48 3 36 64 58 68 no I2O 142 196 128 152 208 SOLUBILITY OF MERCURIC CHLORIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC ACID AT: (Engel - Mg. Mols. per 0. Ann. chim. phys. [6] 17, 100 cc. Sol. Gms. per 20-25 (?). 362, '89.) (Ditte Ibid. [5] 22, 551, '81 .) 100 cc. Sol. S p. Gr. of Parts HC1 Part _ s HgCl2 HC1. *HgCl. HCl. Hg0 2 . Solutions. per 100 Parts H 2 0. per 100 Parts Solution. 4-3 9-7 i-57 I3.II .117 O-O 6.8 9.9 19.8 3.61 18.04 .238 5-6 46.8 I 7 .8 35-5 6.49 3 2 -44 .427 10- I 73-7 26.9 55-6 9.81 49.04 .665 13-8 87.8 32-25 68.9 n .76 58.80 .811 21 .1 127.4 34-25 72.4 12.48 62 .40 .874 31.0 141.9 41-5 85 5 i$-i3 75.65 2-023 50.0 148.0 48.1 88 6 17-54 87.70 2.066 6o.o 154.0 70-9 95-7 25.84 129.20 2.198 191 MERCURIC CHLORIDE SOLUBILITY OF MIXTURES OP SODIUM AND MERCURIC CHLORIDE IN WATER AT 25. (Foote and Levy Am. Ch. J. 35, 239, '06.) Gms. per loo Gms. Solution. Gms. per 100 Gms. Undissolved Residue. Solid NaCl. HgCl 2 . NaCl. HgCl 2 . H 2 0. 26-5 none IOO none none NaCl 18.66 5!-35 . . . 16.39 18.71 18.64 5*-32 51.42 21.98 65.42 NaCl and NaCl.HgCl 2 .2H 2 O 18.87 51 .26 71 .25 14-97 57-74 i6'. 3 8 74.18 9.44 ' Double Salt 14.03 13-25 59-69 62.16 16.36 16.16 74-21 74.70 9-43 9.14 NaCl.HgCl 2 .2H 2 O ' Calc. Comp. = 16.01% NaC! 74-14% HgC1.9.8s% H,0 13 .17 62.59 15.96 74.76 9.28 . 12.97 *3-M 62 .50 62.48 78.20 88.64 1 NaCl.HgCl 2 . 2 H 2 O f and HgCl 2 13 -15 62-55 90-83 ... J Two determinations made at 10.3 gave: 19.46 46.49 67.46 29.19 3-35 19.48 46.50 22.83 68.85 8.32 SOLUBILITY OF MIXTURES OF POTASSIUM AND MERCURIC CHLORIDES IN WATER AT 25. (Foote and Levy.) Composition of Solution. Grams per 100 Grams Solution. Percentage Composition of Undissolved Residue Solid Phase. ' KC1. 26.46 26.24 26.43 26.33 HgCl 2 . none 15 .04 15 .02 15.02 K'Cl. IOO HgCl 2 . none 3-63 26.15 52.01 H 2 0. ill] KC1 KC1 and 2KCl.HgCl 3 .H 2 O 26 33 14.92 61 .04' 23 74 18.91 34 .61 61 .66 3- 73) 2 KCl.HgCl 2 .H 2 O 22 21 36 39 21.39 23.88 34 34 77 05 62 61 .02 .84 3- 3- Calc. Composition 34.05% KC1, 6i.8 4 %HgCl 2 , 4.11% H 2 20.32 2O.26 27 .62 27.38 65 73 .24 . 9 8 ;; j 2 KCl.HgCl 2 .H 2 and KCl.HgCl 2 .H 2 O 17 85 25-34 21 '.89 75 .10 3- on 9 .26 18.95 21 .02 73 36 5- 6 2 | KC1.H S C1 2 .H 2 7 '6 .80 .84 19.56 22.81 2O 20 7.6 75 73 74 .06 54 6. 4- 18 71 ,. Calc. Composition 20.52%KC1, 74-53% HgCl 2 , 5.47% H 2 6 .66 24.32 20 54 73 99 5- 47, 6 6 52 .64 25- x 3 25.16 76 80 .46 .60 KCl.HgCl 2 .H 2 O and KC1.2HgCl 2 . 2 H 2 6 27 2 5 -ii 12 .09 83 .20 4- ?i KC1.2HgCl 2 . 2 H 2 O Calc. Composition 5 77 24-73 II .87 83 . 18 4- 95 n.43%KCl, 83.os%HgCl 2 .5.52%H 2 4 .68 24-75 . ' 84 .46 4 .66 25- J 7 . . . 93 .68 . KC1.2HgCl 2 .2H 3 and HgC; a 4 .69 24.82 . 98 5o - none 6.90 none IOO .00 none Hga 2 MERCURIC CHLORIDE 192 SOLUBILITY OF MIXTURES OF RUBIDIUM AND MERCURIC CHLORIDES IN WATER AT 25. (Foote and Levy.) Composition of Solution. Grams per 100 Grams. Solution. Percentage Composition of Undissolved Residue. Solid Phase. RbCl. HgCl 2 . RbCl. HgCl 2 . H 2 6. 48.57 none IOO.O none none RbCl 46.76 9.18 88.04 ii .24 0.72 ] 47-54 47-55 9-49 9-39 60.33 37-5 1 40-75 2.16 2.66 - RbCl and 2 RbCl.HgCl 2 .H 2 47-3 9-47 46.73 49-38 3.88 J 47-65 10-35 19.58 46.50 50.92 50.80 2-58 } 3-22 : 2RbCl.HgCl 2 .H 2 O Calc. Com- position 45.55% RbCl.si 05% HgCl 2 .3-4%H 2 O 34-77 19.94 43-07 52-44 4-49 2RbCl.HgCl 2 .H 2 Oand 3 RbCl. 34.76 20-10 41 .10 55.36 3-54 2HgCl 2 .2H 2 O 30.27 29.20 27-38 20.17 20-55 20.63 39-07 39.10 38.67 57-34 57-47 57-40 3-59 3-43 . 3-93 3 RbC1.2HgCl ? .2H 2 O Calc. Composition 3 8. 5 5%RbCl, 57.62%HgCl 2 . 3 .82%H 2 26.83 27.09 20.87 20.97 38.48 31.40 57-36 64-35 4- J 6 I 3 RbC1.2HgCl 2 . 2 H 2 O and 4.25 RbCl.HgCl 2 .H2O 26.15 20.58 30-34 65.48 4.18 J 23.81 18.71 30.87 65.10 . ~ ^ RbCl.HgCl 2 .H 2 O 4-3 Calc. Composition 18.10 14.25 29.87 65.28 4.8? \ 2 9 .49%RbCl, 66.11% HgCl 2 , D 4.40%H 2 O 10.87 10.42 29-33 66.15 4-52 J 10.68 10.56 28.59 67-99 3-42 RbCl.HgCl 2 -H 2 O and 3 RbCl 10. 06 10.05 26.22 72 .20 1.58 4 HgCl 2 .H 2 io.c6 9.86 25.28 73-38 0-84 8.48 8.46 8.71 8.80 25-30 25-44 73-15 73-67 i-55 0.89 3KbCl. 4 HgCl 2 .H 2 O Calc. Composition ' 24.76% RbCl, 74-01% HgCl* 5-68 8.70 25.09 73-46 i-45 i.2 3 %H 2 O 5.10 8-33 24.92 73-93 i .15 3-43 8-25 22.79 75-72 i-49 3 RbCl. 4 HgCl 2 .H 2 Oand RbCl sHgC! 2 3-38 8.00 12.68 86.74 0-58 ^ 2.98 1.89 1.50 7.71 7-64 7-55 8.40 8.38 8.30 91.24 91.78 91.81 RbCl. S HgCl 2 Calc. Composition ' 8 .20% RbCl, 9 1 -8% HgCl 2 I .10 7.21 8.07 91.58 o-79 7.16 6.91 93 -15 RbCl.sHgCl 2 and HgCl 2 0.84 7.42 2.27 97-09 none 6.90 none IOO.O HgCl 2 i 9 3 MERCURIC CHLORIDE SOLUBILITY OF MERCURIC CHLORIDE IN METHYL, ETHYL PROPYL, w BUTYL, Iso BUTYL AND ALLYL ALCOHOLS. (Etard Ann. chim. phys. [7] 2, 563, '94.) NOTE. For the solubility in Me, Et, and propyl alcohols at room temperature, see Rohland Z. anorg. Ch. 18, 328, '98; at 8.5, 20 and 38. 2, see Timofejew Compt. rend. 112, 1224, '91; in Me and Et alcohols at 25, see de Bruyn Z. physik. Ch. 10, 783, '92. The deter- minations of these investigators agree well with those of Etard, which are given below. Grams HgC! 2 per 100 Grams Saturated Solution in: l> . CHaOH. C 2 H 5 OH. C-jHzOH. CH 3 (CH 2 ) 3 OH. (CH3) 2 CHCH 2 OH. CH 2 .CH.CH,OH. -30 14-5 15.0 ... 20 20.1 15-7 13-5 21.0 10 15-2 26-5 16-5 13-7 25-5 20.1 29.8 17.4 14.0 5-2 30.0 + 10 26. 3 30.6 18.0 14-3 6.0 37-5 20 34-o 32.0 18.8 14.6 6.8 46-5 25 40.0 32-5 I9-S *5 5 7.2 30 44.4 33-7 20.0 16.5 7-5 40 58.6 35-6 23.0 19.6 9-7 . . . 60 62.5 41.2 29.8 26.5 17.0 . . . 80 66.0 47-5 36.8 33-o 24.9 . . . 100 70.1 54-3 43-8 3 I -7 . . . 120 73-5 61-5 50.6 39-2 150 78-5 SOLUBILITY OF MERCURIC CHLORIDE IN ACETIC ACID. (Etard.) Cms. Gms. Gms. t. HgCl 2 per 100 Cms. t. HgCl 2 per zoo Gms. t. HgCJ 2 per loo Gms. Solution. Solution. Solution. 20 2-5 70 8-5 no 13-6 30 3-5 80 9-7 120 I6. 5 40 4-7 90 II -O I 3 20.7 50 6.0 IOO 12.4 140 25.2 60 7-2 1 60 34-8 SOLUBILITY OF MERCURIC CHLORIDE AND SODIUM CHLORIDE IN ETHYL ACETATE AT 40. (Linebarger Am. Ch. J. 16, 214, '94.) Solid HgCl 2 Mols. per 100 Mols. Acetate. Gms. per 100 Gms. Acetate. Gms. per 100 Gms. Solution. NaCl. HgCl 2 . NaCl. H g ci 2 : NaCl. H g ci 2 : 0.8 12-9 0.53 39-7 o-53 28.4 2.3 12-4 I .53 38-15 27.61 4-3 I6. 4 2 .8 S 5 -44 2 '.78 33-54 9.1 22.85 6.05 86.14 5-6o 46.28 18.5 34-9 12 .29 107.4 10.95 5!-7 6 20. o 40.0 13.29 123.0 II -73 55.18 The double salt (HgCl 2 ) 2 .NaCl is formed under proper conditions. MERCURIC CHLORIDE 194 SOLUBILITY OF MERCURIC CHLORIDE IN ETHYL ACETATE AND IN ACETONE. (Etard; von Laszcynski Ber. 27, 2285, '94; Krug and McElroy J. Anal. Ch. 6, 186, '92; Linebar- ger Am. Ch. J. 16, 214, 94; Aten Z. physik. Ch. 54, 121, '05.) NOTE. The results obtained by the above named investigators were calculated to a common basis and plotted on cross-section paper. The variations which were noted could not be satisfactorily harmonized, and therefore all the results are included in the following table. SOLUBILITY. In Ethyl Acetate. In Acetone. Grams HgCl 2 per TOO Grams Solution. Gms. HgCl2 per TOO Gms. Solution. Laszcynski. Aten. Lanebarger. Etard . K and McE . Laszcynski . Aten . Etard k 10 23- O 40 44.0* 57- 22 .O 23- 2 32 .0 40 49-7 43 .0 * 61. 7 + 10 22.2 23- 5 32 5 40 52.0 51.0 *- 5 8. 9 f 61. 7 20 22-5 23- 4 32 7 40 54 58- 5 t 61. 7 25 22 .7 23 5 33 -O 40 37-4 55-2 5 8. 2 t 61. 7 30 23.0 . 33 .2 40 ... ... 61. 7 40 23-5 33 5 40 61. 7 50 24.0 . 33 5 41 ... ... 61. 7 60 24-7 42 5 ... ... 61. 7 80 26.0 45 .2 ... ... 61. 7 100 . . . . . . . . 48 .0 ... ... . . 1 20 . 50 .8 ... . 150 55 .0 ... . (*) Solid phase HgCl 2 (CH 3 ) 2 CO. (t) Solid Phase HgCl 2 . 100 grams absolute acetone dissolve 143 grams HgCl 2 at 18. (Naumann Ber. 37, 4332, '04.) SOLUBILITY OF MERCURIC CHLORIDE IN SEVERAL SOLVENTS. (Arctowski Z. anorg. Ch. 6, 267, '94; von Laszcynski; Sulc. Z. anorg. Ch. 25, 401, 'oo.) In Carbon Bisul- phide (A.). Gms. HgCl 2 t V per 100 Gms. Solution. 10 O-OIO 0-018 10 0.026 15 0.032 20 O.O42 25 0-053 30 0-063 In Benzene (von L.). In Several Solvents at 18-20 (S.). Gms. HgCl 2 Gms. HgCl 2 t. per 100 Gms. Solution. Solvent. per loo Gms. Solvent. 15 o-537 CHBr 3 0.486 41 0.616 CHC1 3 0.106 55 0.843 CC1 4 0.002 84 1.769 C,H 5 Br 2 -OIO C 2 H 4 Br 2 1-530 I 9 5 MERCURIC CHLORIDE SOLUBILITY OF MERCURIC CHLORIDE IN ABSOLUTE ETHYL ETHER. (Etard; Laszcynski ; Kohler Z. anal. Ch. 18, 242, '79.) t o Gms. HgCl 2 per t <> Gms. HgCl 2 per t <> Gms. HgCl 2 per 100 Gms. Solution. ' 100 Gms. Solution. 100 Gms. Solution. 6.0 60 6.0 90 7.5 6.0 70 6.4 100 8.0 6.0 80 7.0 no 8.5 SOLUBILITY OF MERCURIC CHLORIDE AND OF DOUBLE MERCURIC AND TETRA METHYL AMINE CHLORIDE (CH 3 ) 4 NC1.6HgCl 2 IN AQ. ETHER AT I 7. (Stromholm J. pr. Ch. [2] 66, 443, '02; Z. physik. Chem. 44, 64, '03.) Molecular Concentration per Liter. Grams per Liter of Solution. H 2 O. HgCl 2 (*). HgCl 2 (t). H 2 0. HgCl 2 (*). HgCl 2 (f). O-O o-i5 J 5 0.0342 O 4I.I6 9.26 0-0656 o-i795 0.0428 1.18 48.64 II. 60 O.I3II o . 2069 0-0516 2.36 56-08 I4.OO 0.1956 0.2339 0-0603 3-5 2 63.38 16.34 0.26II 0.2489 0-0690 4.70 70-16 18.70 0.3267 o . 2849 0.0779 5.88 77-20 21.10 0.3922 0.3100 0.0866 7.06 84.02 23.48 - ^J-y - *J -^ -1 (*) Results in this column are for solutions in contact with the Solid Phase HgCfe. (t) Results in this column are for solutions in contact with the Solid Phase (CH 3 ) 4 NC1.6HgCl2. SOLUBILITY OF MERCURIC CHLORIDE AND OF DOUBLE MERCURIC AND TETRA METHYL AMINE CHLORIDE IN ALCOHOL-ETHER SOLUTIONS AT 17. (Stromholm.) Grams C 2 H 5 OH per Liter. Grams HgCI 2 (*) per Liter. Grams HgCl 2 (t) per Liter. o.o 41.16 9.26 4.58 50.00 11.87 9-l6 58.76 14-38 13.74 66.96 16.90 SOLUBILITY OF DOUBLE MERCURIC CHLORIDES IN AQUEOUS AND PURE ETHER AT 16.6. (Stromholm.) Mol. Cone, of HgCl 2 per Liter of: Gms. HgCl 2 per Liter of: Pure Aq. Aq. Aq. Pure Aq. Aq. Aq. 1 h 'J Ether. Ether Ether Ether Ether. Ether Ether Ether Fhase> (i). (2). (3). (4). (S). (6). 0.1515 0.2387 0.2647 0.3196 41.04 64.69 71.71 86.58 HgCl 2 0.0673 0.0673 - I2 93 -i 6 i7 l8 - 2 3 l8 - 2 3 35-5 43-79 (CH 3 .CH 3 C 2 H 4 ) 2 SC1.6HgCl2 0.0404 0.0720 0.0835 0.1034 10.95 I 9-5 I 22.61 28.01 (CH 3 .C 2 H 5 CH3C 2 H4) 2 SC1.6HgClt 0.0342 . . . 0.0706 . . . 9.26 ... 19.10 ... (CH3) 4 NC1.6HgCl 2 0.0264 . . . 0.0568 . . . 7.14 . . . 15.39 . . (C 2 H 6 ) 3 SC1.6HgCl 2 0.0209 0.0400 0.0460 0.0594 5.66 10.83 12.48 16.10 (CH 3 .C 2 H 5 ) 2 SC1.6HgCI 2 0.0063 ... 0.0144 i'7 ... 3-90 ... (CH 3 ) 2 .H 2 NC1.2HgCl2 (i) containing 0.21055 m ol- H 2 O pec liter. (2) 0.2756 mol. H 2 O per liter. (3) 0.421 mol. H 2 O per lite* (4) containing 3.79 gms. H 2 O per liter. (5) 4.97 gms. H 2 O per liter. (6) 7.59 gms. H 2 O per liter. MERCURIC CHLORIDE 196 DISTRIBUTION OF MERCURIC CHLORIDE BETWEEN WATER AND TOLUENE AT 24. (Brown J. Physic. Ch. 2, 50, '98.) Cms. HgCJ 2 per 100 cc. Gms. HgCIg per TOO cc. Layer. C*H 6 CH 3 Layer. H 2 O Layer. Layer . 0.442 O.O27O 1.816 0.130 0.732 0.0488 3.766 0.292 0.780 0.0542 3-754 0.298 I.I92 0.0812 6.688* 0.528* * This solution saturated. MERCUROUS CHLORIDE HgCl. One liter water dissolves 0.002 gram HgCl at 18, by conductivity method. (Kohlrausch Z. physik. Ch. 50, 356, '04- '05.) SOLUBILITY OF MERCUROUS CHLORIDE (CALOMEL) IN AQUEOUS SOLU- TIONS OF SODIUM CHLORIDE, BARIUM CHLORIDE, CALCIUM CHLORIDE AND OF HYDROCHLORIC ACID AT 25. (Richards and Archibald Proc. Am. Acad. 37, 345, 'oi-'o2.) Solid phase in each case. Calomel -f about o.i gram of mercury. In Aqueous NaCl. In Aqueous BaCl 2 . 3. Gr. of Grams per Liter. Sp. Gr. of Grams per Liter. >olutions. ' NaCl. HgCl 2 . ' Solutions. BaCl 2 . HgCl 2 . 5-85 O.OO4I 1. 088 104.15 O-O44 .040 58-50 0.041 I-I34 156.22 0.088 .078 119.00 0.129 I.I74 208.30 0.107 093 148.25 0.194 1.263 312.45 0.231 .142 222.3 0.380 .188 292.5 0.643 In Aqueous CaCl 2 In Aqueous HC1. >. Gr. of Grams per Liter. gp. Gr. of Grams per Liter. >lutions. ' CaCl 2 . HgCl 2 . Solutions. HC1. H g ci 2 : 39-96 O.O22 31.69 0.034 55-5 0.033 36.46 0.048 .064 III .0 O.oSl .042 95-43 0.207 .105 138.75 O.IlS .069 158.4 o-399 iS* I95-36 0.231 .091 209.2 0.548 .205 257-52 0.322 .114 267.3 0-654 243 324.67 0.430 .119 278.7 0.675 3*5 432-9 0.518 .132 3*7-3 0.670 I-358 499-5 0.510 J 53 364.6 0.673 100 grams bromoform, CHBr 3 , dissolve 0.055 gram HgCl at i8-2o. (Sulc. Z. anorg. Ch. 25, 401, *oo.) i 9 7 MERCURIC OTANIDE MERCURIC CYANIDE Hg(CN) 2 . Solvent. Water Abs. Ethyl Alcohol Abs. Methyl Alcohol Glycerine SOLUBILITY IN SEVERAL SOLVENTS. Observer. (Guthrie Phil. Mag. [5] 6, 40, '78.) (Wittstein.) (Griffiths.) (de Bruyn Z.physik. Ch. 10, 784, '92.) t. Gms. Hg(CN) 2 per 100 Gms. Solvent. -0.45 15.2 about ii .0 8.0 101 .1 53.85 19-5 10. 1 19-5 44.2 15-5 27.0 SOLUBILITIES OF MERCURIC CYANIDE DOUBLE SALTS IN WATER AND IN ALCOHOL. Double Salt. Hg(CN) 2 . 2 KCN Hg(CN) 2 . 2 TlCN Hg(CN) 2 . 2 TlCN 2 Hg(CN) 2 .CaBr 2 . 5 H 2 cold 2Hg(CN) 2 .CaBr 2 .5H 2 O boiling Hg(CN) 2 .KCl.H 2 Hg(CN) 2 .KBr.2H 2 O Hg(CN) 2 .KBr. 2 H 2 Hg(CN) 2 .BaI 2 . 4 H 2 Hg(CN) 2 .BaI 2 .4H 2 Hg(CN) 2 .KI Hg(CN) 2 .NaI.2H 2 O Hg(CN) 2 .SrI 2 .6H 2 * . Water. cold 22.7 i 12.6 10 9-7 cold 100. boiling 400.0 18 14.81 18 7-49 boiling 100.0 + cold 6.42 boiling 250.0 cold 6.2 18 22.2 18 14-3 Gms. per 100 Grams. 'Alcohol. ' 50.0 100. O Observer. (Fromuller Ber. n, 92, 's80 (Custer.) (Brett.) 4.42 (Custer.) 62.5 (90% Ale.) 1. 04 (34 B Ale.) (Caillot.) 15.4 (90% Ale.) (Custer.) 25.0 (90% Ale.) SOLUBILITY OF MERCURIC CYANIDE IN ORGANIC SOLVENTS AT l8-20. (Suk Z. anorg. Ch. 25, 401, 'oo.) Solvent. Formula. CHBr 3 CC1 4 C 2 H 5 Br C 2 H 4 Br 2 Bromoform Carbon Tetra Chloride Ethyl Bromide Ethylene Di Bromide G. Hg(CN) 2 per 100 Gms. Solvent. O.OO5 O-OOI 0.013 0.001 MERCURY FULMINATE C 2 HgN 2 O 2 . One liter of water dissolves 1.738 -1.784 grams C 2 HgN 2 O 2 at 12. (Holleman Rec. trav. chim. 15, 159, '96.) MERCURIC IODIDE HgI 2 . SOLUBILITY IN WATER. t . Grams Hglj per Liter. Observer. 1 8 O.OOO4 (conductivity method) (Kohlrausch Z. physik. Ch. 50, 356, 'o4-'os.) 17.5 O . O4O (Bourgoin Bull. soc. chim. [2] 42, '84.) 22 0.054 (Rohland Z. anorg. Ch. 18, 328, '08.) MERCURIC IODIDE 198 SOLUBILITY OF MERCURIC IODIDE IN ALCOHOLS. Alcohol. Formula. Methyl CH 3 OH (i Ethyl C 2 H 5 OH Propyl C 3 H 7 OH Amyl C 5 H U OH Iso Propyl (CH 3 ) 2 CH.OH Iso Butyl (CH 3 ) 2 CHCH 2 OH io 5 -io7~(b. pt.) ... 2.433 ... Sp.Gr.of Solution. G. HgI 2 per 100 Gms. Alcohol. Observer. 15-20 0.799 3-24 (Rohland.) 19-5 3-16 (de Bruyn.) 66 (b. pt.) 6.512 (Sulc.) 15-20 O.SlO 1.42 (Rohland.) 18 1.48 (Bourgoin.) 19-5 2.09 (de Bruyn.) 25 0.803 2.19 (HerzandKnoch.) 78 (b. pt.) 4.325 (Sulc.) 1520 0.816 0.826 (Rohland.) 13 0.66 (Laszcynski.) 3.66 " 100 5-30 M 133-5 81 (b. pt.) 9-57 2.266 (Suk.) SOLUBILITY OF MERCURIC IODIDE IN AQUEOUS ETHYL ALCOHOL: At 1 8. At 25. (Bourgoin.) (Herz and Knoch Z. anorg. Ch. 45, 266, '05.) Solvent. Gms. HgI 2 per Liter. Wt.% Alcohol in Solvent. HgI 2 per loo cc. Solution. Sp. Gr. of olutions as /, Millimols. Grams. Abs. Alcohol 11.86 100 3 .86 I 754 O 8033 HO + 80% 90 Ale. 2-857 95 .82 2 56 I .162 O .8095 H 2 O+io% 90 Ale. 0.086 92 44 I .92 873 O .8154 86 74 I 38 O 623 O .8300 78 75 O 935 425 O .8405 67 63 45 .204 O .8721 SOLUBILITY OF MERCURIC IODIDE IN ACETONE IN ETHYL ACETATE AND IN BENZENE. (Sulc; Krug and McElroy J. Anal. Ch. 6, 186, '92; Laszcynski Ber. 27, 2285, '94.) In Acetone. In Ethyl Acetate. Gms. HgI 2 Gms. HgI 2 t. per 100 Gms. t per loo Gms. (CH 3 ) 2 CO. ( :H 3 COOC2H 6< I 2.83 20 1-49 18 3-36 +17.5 1.56 25 2 .09 (K.andMcE.) 21 1.64 40 4-73 40 2-53 58 6.07 55 3.19 56 (b.pt.) 3 . 249 (Sulc.) 76 4-3 1 In Benzene. Gms. HgI 2 per zoo Gms. 15 0.22 60 0.88 6 5 0.95 84 1.24 80 (b.pt.) 0.825 (Sulc.) 74-78 (b.pt.) 4 . 20 (Sulc.) I 9 9 MERCURIC IODIDE SOLUBILITY OF MERCURIC IODIDE IN CARBON BISULPHIDE. (Linebarger Am. Ch. J. 16, 214, '94; Arctowski Z. anorg. Ch. 6, 267, '94; n, 274, '95.) f0 Cms. HgI 2 per t o Cms. HgI 2 per t o Cms. HgI 2 per io3 Gms. Solution. 100 Cms. Solution. 100 Cms. Solution. 116 0.017 5 0.141 15 0.271 93 0.023 o 0.173 20 0.320 86.5 0.024 + 5 0.207 25 0.382 10 0.107 10 0.239 30 0.445 SOLUBILITY OF MERCURIC IODIDE IN SEVERAL ORGANIC SOLVENTS. (Sulc Z. anorg. Ch. 25, 401, 'oo.) Solent. Formula. t". Chloroform CHC1 3 18-20 0.040 Chloroform CHC1 3 61 (b. pt.) 0.163 Bromoform CHBr 3 18-20 0.486 Tetra Chlor Methane CC1 4 18-20 0.006 Tetra Chlor Methane CC1 4 75 (b. pt.) 0.094 Ethyl Bromide C 2 H 5 Br 18-20 0.643 Ethyl Bromide C 2 H 5 Br 38 (b. pt.) 0.773 Ethylene Di Bromide C 2 H 4 Br 2 18-20 0.748 Ethyl Iodide C 2 H 5 I 18-20 2.041 Ethylene Di Chloride C 2 H 4 Cl2 85.5 (b. pt.) i .200 Iso Butyl Chloride (CH 3 ) .CHCH 2 C1 69 " 0.328 Methyl Formate HCOOCH 3 36-38 " 1.166 Ethyl Formate HCOOC 2 H 6 52-55 " 2.150 Methyl Acetate CH 3 COOCH 3 56-59 " 2.500 Acetal CH 3 CH(OC 2 H 5 ) 2 105 " 2.000 Epi Chlor Hydrine CH 2 .O.CH.CH 2 C1 117 " 6.113 Hexane C C H 14 67 ... 0.072 SOLUBILITY OF MERCURIC IODIDE IN ETHER AND IN METHYLENE IODIDE. In Ether. In Methylene Iodide. (Sulc; Laszcynski.) (Retgers Z. anorg. Ch. 3, 253, '93.) ^.0 Gms. HgI 2 per 100 ^.o Gms. HgI 2 per 100 Gms. (C 2 H 8 ) 2 O. Gms. CR 2 I t . o 0.62 15 2.5 36 0.97 loo 16.6 35 (b.pt.) 0.47 (Sulc) 180 58.0 SOLUBILITY OF MERCURIC IODIDE IN FATTY BODIES. (Mehu J. pharm. chim. [5] 12, 249, '85.) *o Gms. HgI 2 per Cni wn t *o Gms. HgI 2 per * ' 100 Gms. Solvent. * ' 100 Gms. Solvent. Bitter Almond Oil 25 0.5 Vaseline 25 0.025 Bitter Almond Oil 100 i . 3 Vaseline 100 o . 20 Castor Oil 25 4.0 Poppy Oil 25 i .o Castor Oil 100 20.0 Olive Oil 25 0.4 Nut Oil 100 1.3 Carbolic Acid 100 2.0 100 grams oil of bitter almonds dissolve 5.0 grams HgI 2 .KI at 25. (Mehu.) MERCURY OXIDE 200 MERCURY OXIDE HgO. SOLUBILITY IN WATER. (Schick Z. physik. Ch. 42* 163, 'oi-'oa.) * Grams per 1000 cc. Solution. 25 100 0.0518 yellow HgO 0.410 yellow HgO 0-0513 red HgO 0.3 79 red HgO EQUILIBRIUM IN THE SYSTEM, MERCURY OXIDE, SULPHUR TRI- OXIDE, WATER. (Hoitsema Z. physik. Chem. 17, 651, '95.) Results expressed in molecules per sum of 100 molecules of the three components of the system. Results at 25. Results at 50. Liquid Phase. Solid Liq uid Phas ie. Solid H 2 0. S0 3 . HgO. * Phase. H 2 0. S0 3 . HgO. Phase. 98-5 I .24 o-33 3HgO.SO$ 9 8 9 0.96 O 17 3 HgO.SO, 96.6 2 .49 0.92 N 9 6 O 3 05 O 93 94.4 3 93 1-65 41 93 .2 4 .92 I .90 " 93-9 4 .24 1-85} 3 HgO.SO 3 and 92 .8 5 10 2 .09 " 94.4 4 52 2.12 j 3 HgO.2SO8.2H 2 O 92 .8 5 ,16 2 .06 " 93-4 4 65 1-94 3 HgO.2SO 3 .2H2O 92 5 5 34 2 .12 " 92.9* 4 .81 2.29 3 HgO.SO 3 92 .2 5 57 2 .20 3 HgO.SO 3 and 92.9 5 .11 I. 9 8 3 HgO. 2 SO 3 .2H2O 3 Hg0.2S0 3 . 2 H 2 92.3* 5 .20 2-54 3 HgO.S0 3 92 .1 5 75 2 .11 3 HgO. 2 SO 3 .2H 2 O 9 2 -3 5 58 2.09 3 HgO. 2 SO 3 .2H 2 O 92 O 5 ,80 2 .16 " 92.1 5 .81 2.08 " 9 1 .2* 6 27 2 56 3 HgO.SO 3 and 91.9 5 97 2.90 3 HgO.S03 HgO.S0 3 91.9 6 i5 2.05 3 Hg0.2S0 3 .2H 2 9i 5 6 34 2 .19 3 HgO.2SO a . 2 H 2 O 9 J -3 6 54 2.13 and HgO.SO 3 91 .2 6 77 2.02 HgO.S03.H20 9 1 3* 6 37 2 30 HgO.SO 8 9 J -3 6 .90 1. 80 9i .6 6 .69 I 75 9!-3 7 .67 1. 01 9i .1 8 3 2 57 " 9i-3 91 -o 7 8 .84 36 0.8 9 j o.6 9 j HgO.SO 3 .H 2 O and HgO-SOa 89 3i .6 .6 10 68 .2 4 0.23 0.03 n 4 90-5 8 95 o-53 HgO.S0 3 89.2 10 .6 0.22 75-8 24 .2 trace 39-2 60 7 trace " * Indicates unstable equilibrium. MEROUROUS SULPHATE Hg 2 SO 4 . SOLUBILITY IN WATER, IN SULPHURIC ACID AND IN POTASSIUM SULPHATE AT 25. (Drucker Z. anorg. Ch. 28, 3 62, '01; Wright and Thomson Phil. Mag. [5] 17, 288; 19, i, '&4-'&s; Wilsmore Z. physik. Ch. 35, 3 os, 'oo.) Solvent. Water Aq.H 2 SO 4 ( i .96 gms. per liter) Aq.H 2 SO 4 ( 4.90 gms. per liter) Aq.H 2 SO 4 (9.80 gms. per liter) 4 (34.87 gms. per liter) Hg 2 SO 4 per Liter. Gram Mols. Grams. 11.71 I0~* O . 058(0.047 W.and T^ 0.059 W.) 8.31 " O.O4I 8.78 " 0.044 8.04 " O.O4O 9.05 " 0.045 2OI METHANE METHANE CH 4 . SOLUBILITY IN WATER. (Winkler Ber. 34, 1418, 'ox.) t . /5. 0'. ? t. /. ft'. 9. 0.05563 05530 0.00396 40 .02369 .02198 .00159 5 0.04805 .04764 0.00341 50 .02134 .01876 .00136 10 0.04177 o .04127 0-00296 60 .01954 .01571 .00115 J S 0-03690 o .03628 O.OO26O 70 .01825 .01265 .00093 20 0.03308 o 03233 O.OO232 80 .01770 o .00944 o .00070 25 O.O3OO6 .02913 0.00209 90 01735 00535 o .00040 30 O.O2762 .02648 O.OOI9I 100 .01700 o .00000 .00000 For the values otp,p' and q see Ethane, page 133. SOLUBILITY OF METHANE IN METHYL ALCOHOL AND IN ACETONE. (Levi Gazz. chim. ital. II, 513, *oi; abs. in Z. physik. Ch. 41, no, '02.) In methyl alcohol / (Ostwald expression, see page 105) 0.5644 0.0046 J o. 00004 i 2 . In acetone / (Ostwald expression) = 0.5906 0.00613* ~~ 0.0000146*'. From which is calculated the following values: In Methyl Alcohol. In Acetone. o 0.5644 10 0.5144 20 0.4564 30 0.3904 40 0.3164 50 0.2344 60 0.1444 70 o . 0464 o o . 5906 10 0.5278 20 0.4622 30 0.3936 40 0.3220 50 0.2476 60 0.1702 70 0.0900 Tetra Chlor METHANE CC1 4 (Carbon Tetra Chloride). SOLUBILITY IN WATER. (Rex Z. physik. Chem. 55, 355, '06.) t. o. 10. 20. Grams CC1 4 per 100 gms. H 2 O i .097 0.083 0.080 Tri Phenyl METHANE CH(C 6 H 5 ) 3 . SOLUBILITY IN ANILIN. (Hartley and Thomas J. Ch. Soc. 89, 1026, '06.) By synthetic method, see page 9. Gms. 30. 0.085 t . per zoo ' Gms. So- j Mol. per cent CH(CH 5 ) 3 . Solid Phase. lution. 23.0 5-4 1.85 a rhombs 35-3 9-5 3-8 43-o 13-5 5-6 " 52.1 21.9 9-7 " 61 .4 36-5 17.8 66.0 47.2 25-4 44 68.7 54-8 31-6 M 70.1 64.6 40.9 M Gms. t. C^CaHc) per 100 Gms. So- 3 Mol. per cent CH(CeH 6 ) 3 . Solid Phase. lution. 71-3 67.9 44.6 CH < v*6"6/3 .V^il^IM 112 rhombs 71.6 71 .7 49-1 71 .2 76-3 55.1 t 70.6 78.3 57-9 71.6 82.1 63 . 5 CH(CeHa) 3 monoclinic 74-3 84-9 68.2 tt 82.1 91 .7 80.9 87-3 96.1 00.2 44 Tri Phenyl METHANE 202 SOLUBILITY OF TRI PHENYL METHANE IN BENZENE. (Linebarger Am. Ch. J. 15, 45, '93.) Gms. QHa. 3-9 3-90 QH + CH(CflH 4.0 4.06 CH(C ft H 6 ) 3 .C 6 H, 12. 5 5-18 " 16.1 6.83 44 19.4 7.24 " 23-1 8-95 44 37-5 10.48 + CH(CeH5) 3 42 .0 19.61 CH(CeH 6 ) 3 44.6 22.64 44 50.1 30.64 44 55-5 40-51 44 71.0 I4O.OO 44 76.2 319.67 " (Hartley and Thomas.) Gins . \>r/\i CHCCaffi). f2 nt per ioo Gms. rmr H \ Solution. CH(QH 6 ) 8 . Solid Phase. 33 12.6 4-4 CH(C6H 6 ) 3 .QHj 49-4 24.0 8.8 44 65.6 38-9 17.2 44 73-8 57-5 30.2 14 77.1 67-4 39-7 " 77-9 76.3 5o-7 44 77-5 80.2 56-4 " 76.2 84.1 62.8 44 74.6 87-5 69.1 CH(C6H 5 ) 3 monoclinic 76.0 89.0 72.2 44 78.8 9o-5 75-3 " 82.3 93- 1 81-3 " 86.6 95-7 87.8 " NOTE. Hartley and Thomas call attention to the inaccuracy of Linebarger's results and the cor- rectness of Kuriloff 's determinations (Z. physik. Chem. 22, 547, J 97)- Gms. CH(CeHs) 3 Gms. CH(CH 5 ) 3 t. per ioo Gms. Solution. t. per ioo Gms. Solution. II3.C 1 0-98 -40 7-5 IO2 1.24 20 13 -7 - 91 I. 5 6 25.8 - 8 3 I.9I + 10 38-7 ~ 60 3-4 20 43-2 30 5 2 -9 SOLUBILITY OF TRI PHENYL METHANE IN CARBON BISULPHIDE. (Etard Ann. chim. phys. [7] 2, 570, '94; below-8o, Arctowski Z. anorg. Ch. n, 273, '95-) 40 50 60 70 80 Gms. per ioo Gms. Solution. 63-7 72-4 78.6 85.6 92.2 SOLUBILITY OF TRI PHENYL METHANE IN HEXANE AND IN CHLOROFORM. (Etard.) Gms. ioo Gms. Solution in: l> . Hexane. Chloroform. -50 10-5 -30 I .2 IS' 2 2O 1.6 19.0 10 2 -2 23-5 O 3-5 28.9 + 10 5-6 35 -o 20 8-3 4i-5 Gms. CH(C 6 H 5 ) 3 per ioo Gms. Solution in: Hexane. Chloroform. 30 12-5 48.8 40 20. o 5 6.1 50 2 5 .8 6 3 .8 00 45-7 71-7 70 62.0 79.8 80 78-5 8 7 .2 90 97.0 20 3 Tri Phenyl METHANE SOLUBILITY OF TRI PHENYL METHANE IN PYRIDINE. (Hartley and Thomas J. Ch. Soc. 89, 1028, '06.) Synthetic method used, see note, page 9. 22.8 3i-7 37-9 48.7 Cms. Mol. CH(CcH 6 )3 per Solid per 100 Gms. cent Phase. Solution. CH(C6H S ) 3 . 46.2 53-3 57-6 66.6 70.1 22.0 27.2 30-7 39-5 43-5 CH(C6H 5 ) 3 monoclimc Gms. Mol. CH(CH 6 ) 3 per per 100 Gms. cent. Solution. CH(C 8 H 5 ) 3 . 59-3 67.8 72.8 80.6 86.8 75-6 81.9 85-7 9i-5 95-8 50-3 59-7 66.4 77.2 88.1 Solid Phase. SOLUBILITY OF TRI PHENYL METHANE IN: (Hartley and Thomas.) Pyrrole. Gms. Mol. t o CH(CHe)3 Per Solid " per loo Gms. cent Phase. Thiophene. Gms. Mol. t o CH(C6H 6 ) 3 per Solid " per i oo Gms. cent Phase. Sol. CH(CH 5 ) 3 . Solution. CH(C6H 5 ) 3 . 24.6 24 3 8 .1 CH(C 6 H 6 ) 3 .CANH 25 7 26 .0 10 .8 CH(C ft H 6 ) 3 .C 4 H 4 S ,, rhombs 29.0 29 .8 IO 4 33 5 3 1 .1 13 5 3 r -5 33 4 12 .1 44 .0 43 .6 21 .1 " 36.8 40 .6 15 .8 CH(C6H6) 8 monoclinic 47 .6 48 4 24 4 " 42.7 49 i 20 9 53 5 58 7 32 9 " 46.9 56 .0 25 9 57 4 70 .2 44 7 " 53-2 63 9 32 .8 57 .6 74 .8 50.6 60.0 72 76 3 7 41 47 4 62 67 7 .0 78 81 7 9 56 60 .0 .8 CH(CH 5 ) 3 ,, monoclinic 68^5 81 9 55 .6 67 .2 82 .1 61 3 " 71.1 84 4 59 .8 74 .2 87 4 70 5 " 80.0 9 1 5 74 o 4i 79 O 90 3 76 3 " 89.2 97 .6 Q tt 87 .2 96 .2 89 9 " METHYL ACETATE, Butyrate and Propionate. SOLUBILITY IN WATER AT 22. (Traube Ber. 17, 2304, '84.) 100 grams H 2 O dissolve 25.0 grams CH 3 COOCH 3 ; 1.7 grams C 3 H 7 COOCH 3 ; 5.0 grams C 2 H 6 COOCH 3 . METHYL IODIDE, Methylene Chloride and Methylene Bromide. SOLUBILITY OF EACH IN WATER. (Rex Z. physik. Chem. 55, 355, '06.) Grams per 100 Grams H2O. O 10 20 30 CH 3 I. CH 2 C1 2 . CH 2 Br 2 . i-5 6 5 2-363 I-I73 1.446 2.122 I .146 1.419 2 .OOO I.T48 1.429 1.969 I.I76 METHYL BUTYRATE, 204 METHYL BUTYRATE, METHYL VALERATE. SOLUBILITY OF EACH IN AQUEOUS ALCOHOL MIXTURES. (Bancroft Phys. Rev. 3, 193, '95.) ioo cc. H 2 O dissolve 1.15 cc. methyl butyrate at 20. cc. Alcohol cc. H 2 O Added* in Mixture. Butyrate. Valerate. 3 2-34 1.66 6 6.96 5-o6 9 12 .62 9-03 12 I9'45 13.40 15 28.13 18.41 18 33-80 24.00 21 55- 6 4 30.09 24 00 36.72 cc. Alcohol in Mixture. cc. H 2 O Added * Valerate. 27 4I-I5 30 33 36 52-37 62.25 74.15 39 91-45 42 00 * cc. HjO added to cause the separation of a second phase in mixtures of the given amounts of ethyl alcohol and 3 cc. portions of methyl butyrate and of methyl valerate respectively. METHYL ETHYL KETONE CH 3 .CO.C 2 H 5 . SOLUBILITY IN WATER. (Rothmund Z. physik. Chem. 26, 475, '08.) By synthetic method, see Note, page 9. 0> Cms. Ketone per ioo Cms. Aq. Layer. Ketone Layer. -io 34-5 8 9-7 + 10 26.1 90.0 30 21.9 89.9 50 17.5 89.0 70 16.2 85.7 90 no 130 140 Cms. Ketone per ioo Gms. Aq. Layer. Ketone Layer, 16.1 84.8 17.7 80.0 21.8 71 .9 26.0 64.0 151 .8 (crit. temp.)44.2 MOLYBDENUM TRIOXIDE MoO 3 . ioo gins, cold H 2 O dissolve 0.187 gm. MoO 3 . (Dumas; Buchlolz.) ioo ems. hot H 2 O dissolve 0.104 gm. MoO 3 . (Hatchett.) MORPHINE C 17 H 19 N0 3 .H 2 0. SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.; Muller Apoth.-Ztg. 18, 257, '03.) Solvent. Gms. Morphine per ioo Gms. Solution. At i8-22. At 25. At8o d . Solvent. Gms. Morphine per ioo Gms. Solution. 0.0283 Water Alcohol Ether Ether sat. with H,O 0.0094 H,O sat. with Ether 0.0447 Benzene 0.0625 0.030 0.600 0.0131 0.0224 0.0961 Chloroform i .3 1 (60) Amyl Alcohol At l8-22. 0.0655 Ethyl Acetate 0.1861 Petroleum Ether 0.0854 Carbon Tetra Chloride 0.0156 Glycerine 0.45 (15.5) At 25. 0-0555 0.88 10 0.1905 0.032 (17) 205 MORPHINE SOLUBILITY OF MORPHINE IN AQUEOUS SOLUTIONS OF SALTS AND BASES AT ROOM TEMPERATURE, SHAKEN EIGHT DAYS. (Dieterich Pharm. Centrh. 31, 395, '90.) In N/io Salt or Base. In N/i Salt or Base. Grams per Liter. Grams per Liter. [. sa.ii or case. < Salt or Base. Morphine. Salt or Base. Morphine. ' NH 4 OH 3-51 0.20 35-08 0-505 (NH 4 ) 2 CO, 4.80 0.031 48.03 O.O4O KOH 4.62 2.78 46.16 K 2 C0 3 6.92 0.20 69.15 0-379 KHCO 3 10.02 0.024 ioo. 16 0.040 NaOH 4-OO 3-33 40.05 . . . Na 2 CO 3 5-30 0.09 53-03 0.14 NaHCOg 8.41 0.032 84.06 0.044 Ca(OH) 2 (sat.) 1.00(25) MORPHINE ACETATE CHaCOOH.C^H^NC^^HA Morphine Hydrochloride HC1.C 17 H 18 NO 3 . 3 H 2 O, Morphine Sulphate H 2 SO 4 . (C 17 H 19 NO 3 ) 2 .5H 2 O, and Apo Morphine Hydrochloride HC1.C 17 H 17 NO 2 . SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.) Grams per ioo Grams of Solvent. Solrent. Water Alcohol Chloroform Ether Glycerine Acetate. Hydrochloride. Sulphate . Apo M . Hydrochloride . 25 44. 4- 0. 19. 9 6 21 2 80. 50.O 40.0* 25. 2.4 20. Of * 60. 80. 25. 2OO.O 6.53 2.8* 0.22 80. " 166.6 0-53* 2-53 2.62 0.026 0-053 & 6. 3- 25 33 t 15-5. ioo gms. H 2 O dissolve 1.69 gms. apo morphine hydrochloride at 15.5, and 2.04 gms. at 25. ioo gms. 90% alcohol dissolve 1.96 gms. apo morphine hydro Chlorde at 2 5 . (Dolt Pharm. J . [4] 22. 345, '75 ) ioo gms. H 2 O dissolve 4.17 gms. morphine sulphate at 15. (Power Am. J. Pharm. March, '82.) MUSTARD OIL Allyl Isosulphocyanic Ester CS:NC 3 H 5 SOLUBILITY IN SULPHUR BY SYNTHETIC METHOD. See Note, p. 9. (Alexejew Ann. Physik. Chem. 28, 305, '86.) Grams Mustard Oil per ioo grams. Sulphur Layer. Mustard Oil Layer. 90 10 72 IOO 12 67 no 15 62 120 23 51 124 (crit. temp.) 35 NAPHTHYLAMINE 206 a NAPHTHYLAMINE p Sulphonic Acid (Naphtion Acid), i : 4 C, H 6 NH 2 .SO 2 H and a Naphthalamine o Sulphonic Acid, i : 2 a C 10 H 6 NH 2 .SO 2 H-. SOLUBILITY OF EACH IN WATER. (Dolinski Ber-38, 1836, '05.) Gms. per 100 Gms. H 2 O. Gms. per zoojGms. H 2 O. t. p Sulphonic o Sulphonic t. p Sulphonic o Sulphonic Ac. Ac. Ac. Ac. O.O27 O.24 50 0.059 0.81 10 O.O29 0.32 60 0-075 I .OI 20 0.031 0-41 70 0.097 I .37 30 0.037 0.52 80 0.130 1. 80 40 0-048 0.65 90 0.175 2 .40 100 0.228 3- J 9 NAPHTHALENE C 10 H 8 . SOLUBILITY IN METHYL, ETHYL, AND PROPYL ALCOHOLS. (Speyers Am. J. Sci. [4] 14, 294, '02 ; at 19.5, de Bruyn Z. physik.Chem. 10, 784, '92 ; at 11, Timo feiew Compt.rend. 112, 1137, '91.) The original results were calculated to a common basis, plotted on cross-section paper, and the following table read from the curves. In Methyl Alcohol. In Ethyl Alcohol. In Propyl Alcohol. f . W lu f tion CC - I CH^CH 1 * 5 Wt. of i cc. Solution. Gms. CioHg lift nf T re per 100 Gms . W r> Gms. C 10 H t. per 100 Gms. Solution. per 100 Gms. Solution. per 100 Gms. Solution. wr. 01 i cc Solution. per 100 Gms. QHs.CHa. -50 o-3 20 1-9 5-5 0.9124 + 10 27-5 24-0 9.0 0.9126 I 5 .0 2O 36.0 3 I.O 14.0 0-9*35 28.0 25 40-5 35-o J 7-5 o-9 J 55 36.0 30 45-5 39-o 21 .O 0.9180 42.0 40 54-0 48.0 30.8 0.9250 56.0 50 65.0 57-5 43-7 0-935 69-5 60 77-5 7o-5 60.6 Q-9475 83.0 70 88.0 85.0 78.8 o . 9640 97-5 80 0.9770 in .0 NAPHTHOIC ACID C 10 H 7 COOH. One liter of aqueous solution contains 0.058 gram C 10 H 7 COOH at 5. (Paul Z. physik. Ch. 14, in, '94.) ft NAPHTHOL 208 ft NAPHTHOL C 10 H 7 OH. 100 grams H 2 O dissolve 0.105 gram at 25, and 1.33 grams at b. pt.; 100 grams alcohol dissolve 164.0 grams at 25. NAROEINE. 100 grams pure carbon tetra chloride dissolve o.on gram narceine at 17. (Schindelmeiser Chem.-Ztg. 25, 129, 'ox.) NEODYMIUM CHLORIDE NdCl 3 . 100 grams H 2 O dissolve 98.7 grams NdCl 3 at 13, and 140. 4 grams at IOO . (Matignon Compt. rend. 133, 289, '01 ) NEODYMIUM SULPHATE Nd 2 (SO 4 ) 3 . SOLUBILITY IN WATER. (Muthmann and Rolig Ber. 31, 1728, '08.) Gms. Nd 2 (SO 4 ) 3 per 100 Gms. Gms. Nd 2 (SO^) 3 per 100 Gms. Solution. Water. Solution. Water. o 8.7 9.5 50 3.5 3.7 16 6.6 7.1 80 2.6 2.7 30 4.7 5.0 108 2.2 2.3 NICKEL BROMATE Ni(BrO 3 ) 2 .6H 2 O. loo grams cold water dissolve 27.6 grams nickel bromate. NICKEL BROMIDE NiBr 2 . SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 539, '94.) t o G ms.NiBr 2 per t o Gms. NiBr 2 per t <> Gms. NiBr 2 per loo Gms. Solution. too Gms. Solution. 100 Gms. Solution. -20 47-7 25 57.3 80 60.6 io 50.5 30 58.0 loo 60.8 o 53.0 40 59 - 1 120 60.9 + 10 55 -o 50 60.0 140 61 .o 20 56.7 60 60.4 NICKEL CHLORATE Ni(ClO 3 ) 2 . SOLUBILITY IN WATER. (Meusser Ber. 35, 1410, '02.) Gms. Mols. Gms. Mols. ft0 Ni(ClO 3 ) 2 Ni(ClO 3 ) 2 Solid t <> Ni(ClO 3 ) 2 Ni(ClOs) 2 Solid ' per 100 Gms. per 100 Phase. penooGms. per 100 Phase. Solution. Mols.H 2 O. Solution. Mols.H 2 O. 18 49-55 7^4 Ni(ClO 3 ) 2 .6H2O 48 67.60 16.65 N(ClOs)f.4HiO - 8 51.52 8.49 " 55 68.78 17.59 o 52.66 8.88 " 65 69.05 18.01 H-i8 56.74 10.47 " 79-5 75-50 24.68 40 64-47 15-35 M -*3-5 3 r -85 3-73 Ice 9 26.62 2.90 Sp. Gr. of solution saturated at + 18 = 1.661. 20 9 NICKEL CHLORIDE NICKEL CHLORIDE NiCL. SOLUBILITY IN WATER. (Etard; at 12, Ditte Compt. rend. 92, 242, '81.) t o Gms. NiCl 2 per t Gms. NiCl 2 per t o Cms. NiCfe per 100 Gms. Solution. 100 Gms. Solution. 100 Gms. Solution. -17 29.7 2 5 40.0 60 45-i 35-o 30 40.8 70 46.0 + 10 37-3 40 42-3 78 46.6 20 39-i So 43-9 100 46.7 1000 cc. sat. HC1 solution dissolve 4.0 grams NiCl 2 at 12. 100 grams abs. alcohol dissolve 53.71 grams NiCl 2 .6H 2 O at room temperature. 100 grams abs. alcohol dissolve 10.05 grams NiCl 2 at room temperature. (Bodtkcr Z. physik. Chem. 22, 511, '97.) 100 grams abs. alcohol dissolve 2.16 grams NiCl 2 .7H 2 O at 17, and 1.4 grams at 3' (de Bruyn Rec. trav. chim. n, 156, '92.) 100 grams saturated solution in glycol contain 16.2 grams NiCl 2 at room temperature. (de Coninck Bui. acad. roy. Belgique, 359, '05.) NICKEL IODATE Ni(I0 3 ) 2 . SOLUBILITY IN WATER. (Meusser Ber. 34, 2440, f oi.) Gms. Mols. Ni(I0 3 ) 2 Ni(I0 3 ) 2 Solid per 100 Gms. per 100 Mols. Phase. Ni(IO 3 ) 2 . 4 H 2 O Ni(I03) 2 .2H 2 (i) Solution. H 2 0. o o-73 0-033 18 i .01 0.045 3o 1.41 0.063 o o-53 0.023 18 0.68 0.030 30 0.86 0.039 50 1.78 O.oSo 8 0.52 0.023 Ni(I0 3 ) 2 . 2 H 2 (2) (i) a Dihydrate. Gms. t o Ni(I0 3 ) 2 ' per 100 Gms, Mols. Ni(IOa)2 , per 100 Mol: S Solid Phase. Solution. H 2 0. 18 o-55 0-0245 Ni(IO,) 2 .2E 5 0.81 0-035 " 75 1.03 0.045 " 80 I .12 0-049 14 3 I-I35 0.050 Ni(I0 3 ) 8 5 1.07 0-046 " 75 1.02 0.045 " 90 0.988 O.O44 44 (2) /3 Dihydrate. NICKEL IODIDE NiI 2 . SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 546, '94.) f o Gms. NiI 2 per 100 Gms. Solution. t o Gms. NiI 2 per 100 Gms. Solution 2O 52.0 2 5 60.7 O 55-4 30 61.7 10 57-5 40 63-5 20 59-7 So 64.7 60 70 80 90 Gms. NiI 2 per 100 Gms. Solution. 64.8 65.0 65-2 653 NIOKEL NITRATE 210 NIOKEL NITRATE Ni(NO 3 ) 2 . SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichaastalt, 3, 439, 'oo.) Gms. Mols. o Ni(NO 3 ) 2 Ni(NO 3 ) 2 Solid per ioo Gms. per 100 Mols. Phase. Solution. H 2 O. 23 39 .02 6-31 Ni(N0 3 ) 2 . 9 H 2 21 39 .48 6-43 M 10 5 44 13 7-79 " 21 39 94 6-55 Ni(NO 3 ) 2 .6H 2 O 12 5 4 1 59 7.01 " 10 42 .11 7.16 " 6 43 .00 7-44 " 44 32 7.86 " 18 48 59 9-3 " Cms. Mols. Ni(N0 3 ) 2 Ni(N0 3 ) 2 Solid per 100 Gms. per 100 Mols. Phase. Solution. H 2 O. Ni(NO 3 ) 2 .6H 2 O Ni(NO 3 ) 3 .3H 2 O 2O 49-06 9-49 41 55-22 12. 1 56 7 62.76 I6. 7 58 61.61 15-9 60 61.99 16.0 6 4 62.76 16.6 70 6 3-95 17.6 90 70.16 23.1 95 77.12 33-3 100 grams sat. solution in glycol contain 7.5 grams Ni(NO 3 ) at room temperature. (d e Coninck.) NICKEL SULPHATE NiSO 4 . SOLUBILITY IN WATER. (Steele and Johnson J. Ch. Soc. 85, 116, '04; see also Etard and Mulder.) Grams NiSO 4 per t_ ioo Gms. 5 Solution. 20.47 Water. ' 25-74 o 21.40 27.22 9 22 .6 30 23-99 27.48 29.99 31-55 37-90 42.46 32-3 33 30-57 3I-38 44-02 45-74 34 31.20 45-5 32-3 30-35 43-57 33-o 34-o 30.25 30-49 43-35 43-83 Solid Phase. NiSO 4 .6H 2 O " (blue) Transition points, hepta hydrate <= hexa hydrate = 31.5* Hexa hydrate (blue) + hexa hydrate (green) = 53.3. Grams NiSO 4 per t. ioo Gms. 35-6 44-7 Solution. 30-25 30-45 32-45 Water. 43-35 43-79 48.05 50.0 53-o 33-39 34-38 50.15 52-34 54-5 57-o 60 34-43 34-81 35-43 52.50 53-40 54.80 7o 80 99 37-29 38.71 43-42 59-44 63.17 76.71 Solid NiSO 4 .6H 2 O 4 (blue) (green) 211 NICKEL SULPHATE SOLUBILITY OF MIXTURES OF NICKEL SULPHATE AND COPPER SULPHATE. Results Gms. per 100 at 35. Gms. HuO. ^JPMVfc^^* Jvjyai* i^iiu. . Mol. per cent in Solution. * J/ y/'j Mol . per cent in Solid Phase. Crystal CuS0 4 . NiS0 4 . ' CuS0 4 . NiS0 4 . CuS0 4 . NiS0 4 . " Form. 9.62 583-9 I .57 98.43 o-35 99-65 Rhombic 41.66 484.4 7.69 92.31 2 .12 97.88 " 75-39 553-5 11.66 88.34 4-77 95-23 Tetragonal 106.40 506-5 16.92 83.08 6.52 93-48 " 172 .0 483.8 2 5 -63 74-37 13.88 86.17 " 186.9 468.0 27.90 72.10 (18.77 (94.91 81.23 5-09 Tetragonal Triclinic Results at 67. 20.04 729-3 2-65 97-35 o-93 99.07 Monoclinic 66.01 706.2 8-31 91.69 2.86 97.14 " 88.08 501.6 J 3-55 86.45 3-92 96.08 47-94 675.0 16:39 83.61 6.66 93-34 " 249-9 747-8 24.46 75-54 22.32 77-68 {Triclf^ 1 " SOLUBILITY OF MIXTURES OF NICKEL SULPHATE AND SODIUM SUL- PHATE, ETC. (Koppel; Wetzel Z. physik. Chem. 52, 401, '05.) t. Gms. per too Gms. Solution. Gms. per 100 Gms. H 2 O. Mols. per 100 Mols. H 2 O. J*>lid NiS0 4 . Na 2 S0 4 . NiS0 4 . Na 2 S0 4 ." NiS0 4 . Na 2 S0 4 . ' O 16 94 7 .6l 22 .46 IO.OQ 2 .61 I .28 ] 5 17 99 10.85 25 .28 15 .24 2 94 I !NiS0 4 . 7 H20 + 93 f Na 2 S0 4 .ioH 2 O 10 18 97 I3-85 28 .26 2O .64 3 .29 2 * * ^ v .61 J 20 18 76 17.21 29 3i 26 87 3 .410 3 .404 NiNa 2 (S0 4 ) 2 . 4 H 2 25 17 85 16.54 27 33 25 33 3 .l8l 3 .208 30 16 74 J5-34 24 .64 22 58 2 .868 2 .861 35 16 .28 14.91 23 .66 21 -67 2 753 2 744 40 15 35 14.49 21 .88 2O 65 2 546 2 .616 18.5 *9 .61 16.49 30 .70 2 5 .80 3 .56 3 .27 ' 20 20 *3 16.15 31 59 25 35 3 .67 3 .21 2 5 21 .20 14.77 33 .11 23 .06 3 85 2 92 NiNa 2 (SO 4 ) 2 . 4 H 2 O -f- 30 22 .60 12.80 34.98 19 .82 4 .07 2 59 35 23 .62 10.78 36 .01 16 43 4 .19 2 .08 40 24 .92 9-39 37 93 14 .29 4 .41 I .81 J 18.5 16 .80 18.93 26 .14 29 45 3 .04 3 .72 1 20 25 15 10 .48 .92 20.18 24.12 24 16 .06 .81 3i 37 37 13 2 I .80 .96 3 4 .07 1 NiNa^SO^jMHoO -f ^ NasSO.-ioH^ 30 6 .40 28.71 9 .87 44 25 I X 5 5 .60 J 35 4 54 31-65 7 J 3 49 59 .838 6 28 ) NiNa 2 (S0 4 ) 2 ^H 2 + 40 4 63 31-37 7 .24 49-03 843 6 2I j Na 2 S0 4 NICKEL SULPHATE 212 SOLUBILITY OF NICKEL POTASSIUM SULPHATE NiK 2 (SO 4 ) 2 .6H 2 O IN WATER. (Tobler Liebig's Ann. 95. 93. 'SSJ v. Hauer J. pr. Ch. 74, 433, '58.) Grams NiK 2 (SO 4 ) 2 Grams NiK^SO^a t o per IPO Gms. H2O. t o per 100 Cms. HaO. (Tobler.) (v. Hauer.) (Tobler.) (v. Hauer.)' o 5.3 ... 50 30 10 8.9 60 35.4 20.47 20 13.8 9.53 70 42-0 30 18.6 80 46.0 28.2 40 . 24-0 I4-03 SOLUBILITY OF NICKEL SULPHATE IN METHYL AND ETHYL ALCOHOLS. (de Bruyn Z. physik. Ch. 10, 783, '92.) ioo grams abs. ethyl alcohol dissolve 1.3 grams NiSO 4 .7H 2 O at 17. 100 grams abs. methyl alcohol dissolve 46.0 grams NiSO 4 .7H 2 O at 17, and 24.7 grams at 4. ioo grams abs. methyl alcohol dissolve 0.5 gram NiSO 4 at 18. ioo grams abs. methyl alcohol dissolve 31.6 grams NiSO 4 .6H 2 O at 17. ioo grams 93.5% methyl alcohol dissolve 10.1 grams NiSO 4 .7H 2 O at 4, and 7.8 grams NiSO 4 .6H 2 O at 18. ioo grams 50.0% methyl alcohol dissolve 2.0 grams NiSO 4 .7H 2 O at 4, and 1.9 grams NiSO 4 .6H 2 O at 18. ioo grams sat. solution in glycol contain 9.7 grams NiSO 4 at room temperature. (de Coninck Bull. acad. roy. Belgique 359, '05.) NICOTINE C 10 H 14 N 2 . SOLUBILITY IN WATER. (Hudson Z. physik. Chem. 47, 114, '04.) Determinations made by Synthetic Method, for which see Note, page 9. Below 60 and above 210 both liquids are miscible in all propor- tions; likewise with percentages of nicotine less than 6.8 and above 82 per cent the liquid does not show two layers at any temperature. Below 94 the upper layer is water. Above 94 the upper layer is nicotine. The curve plotted from the following results makes a com- plete circle. in the Mixture. 6.8 94 95 7-8 89 155 10. o 75 14-8 65 200 32.2 61 210 49-o 64 205 66.8 72 190 80.2 87 170 82.0 129 130 2i 3 NITROGEN NITROGEN N. SOLUBILITY IN WATER. iraun Z. physik. 44, 318, t o " Coefficient of Absorption " ft . (Winkler Her. 24, 3606, '91; Braun Z. physik. Chem. 33, 732, 'oo; Bohr and Bock Wied. Ann. 44, 318. 'pi-) 0.0235* o-02 39 t ...t 0.0233* 0.00239' 5 0-0208 0-0215 0.0217 0.0206 0.00259 10 0.0186 0-0196 0-0200 0.0183 0.00230 i5 0-0168 0-0179 0.0179 0.0165 0.00208 2O 0-0154 0-0164 0.0162 0.0151 0.00189 25 0-0143 0-0150 0-0143 0.0139 0.00174 30 0-0134 0-0138 . . . 0.0128 o. 00161 35 0-0125 0.0127 0.0118 0.00148 40 0-0118 0.0118 O-OIIO 0.00139 5 0-0109 0-0106 . . . 0.0096 O-OOI2I 60 O-OIO2 O-OIOO . . . 0.0082 0.00105 80 0.0096 0.0051 0.00069 100 0-0095 O-OIOO o.oooo O-OOOOO * W. t B. and B. $ B. For values of J3, ft' t and q, see Ethane, page 133. SOLUBILITY OF NITROGEN IN AQUEOUS SALT SOLUTIONS. (Braun.) Coefficient of Absorption of N in Barium Chloride Solutions of: t. 13-83 11.92 6.00 3-87 3-33 per cent. per cent. per cent. per cent. per cent. 5 0.0127 0-0137 0-0160 O-Ol8o 0-0183 10 O.OII7 O.OI25 O-OI47 0.0166 0-01^8 15 O-OIO4 0-OII4 0.0132 0.0148 0-0150 20 O.OO92 0-0098 O-OIlS 0.0132 0.0135 25 0-0078 0-0086 0-0104 O-OII4 O-OII9 Coefficient of Absorption of N in Sodium Chloride Solutions of: t. "73 8.14 6.4 2.12 0.67 per cent. per cent. per cent. per cent. per cent. 5 O-OIO2 0-0127 0.0138 O.OI79 O-O2OO 10 0.0093 0-OII3 O.OI26 0-0164 0.0185 !<; 0-OoSl O.OIOI O.OII3 0.0147 0.0164 20 O.OO66 0.0087 0.0098 O.OI3I 0-0148 25 O-OO47 0.0075 0.0083 O.OH3 O.OI3O SOLUBILITY OF NITROGEN IN ALCOHOL. (Bunsen.) t o 5 10 15 20 24 Vols. N * 0.1263 0.1244 0.1228 0.1214 0.1204 0.1198 dissolved by i Vol. Alcohol. * At o and 760 mm. NITROQFN 214 SOLUBILITY OF NITROGEN IN MIXTURES OP ALCOHOL AND WATER AT 2 5 . (Just Z. physik. Ch. 37, 361, 'ox.) Results in terms of the Ostwald solubility expression, see page 105, Vol. H 2 O in Mixture. Vol. Alcohol in Mixture. Dissolved N fa). 100 o 0.01634 80 20 0.01536 67 33 0.01719 o ioo (99 . 8 % Alcohol) o . 1 43 2 SOLUBILITY OF NITROGEN IN SEVERAL SOLVENTS AT 20 AND 25. (Just.) Solvent. /25- ^20- Toluene 0.1235 o. 1186 Chloroform 0.1348 0.1282 Methyl Alcohol o. 1415 o. 1348 Ethyl Alcohol (99.8%) o. 1432 o. 1400 Acetone o. 1460 o. 1383 Amyl Acetate 0.1542 0.1512 Ethyl Acetate o. 1727 o. 1678 Iso Butyl Acetate 0.1734 0.1701 Solvent. Water Aniline Sulphur Dioxide Nitro Benzene Benzene Acetic Acid Xylene Amyl Alcohol b. 0.01634 0.03074 0.05860 0.06255 0.1159 o. 1190 o. 1217 0.1225 fe. 0.01705 0.02992 0.05290 0.06082 0.1114 0.1172 o. 1185 o. 1208 SOLUBILITY OF NITROGEN IN PETROLEUM. COEFFICIENT OF ABSORP- TION AT 10 = 0.135, AT 20 = O.II7. (Gniewasz and Walfisz Z. physik. Ch. i, 70, '87 ) SOLUBILITY OF NITROGEN IN AQUEOUS PROPIONIC ACID AND UREA SOLUTIONS. (Braun.) Coefficient of Absorption of N in C 2 H 6 COOH Solutions of: fc . 11.22 per cent. 9.54 per cent. 6.07 per cent. 4.08 per cent. 3-82 per cent. 5 10 I 5 20 o. o. o. o. 0195 0178 0159 0146 O O O .O2O4 .0182 .0163 .0147 O O o o .0208 .0186 .0164 .0148 O O o .0210 .OI92 .0169 .0154 o .O2O9 0191 .0167 o I 55 25 o. 0130 .0134 o .0134 o .0137 o .0137 Coefficient of Absorption of N in CO(NH 2 ) 2 Solutions of: * . 15.65 percent. 1 1 .9 per cent . 9. 4 2 per cent. 6.90 per cent. 5.15 per cent. 2 .28 per cent . 5 10 '5 20 0.0175 O.Ol62 O.OI5O O.OI4O O.OI79 0-0167 O.OI49 0.0139 O.OI9O 0.0176 0-0158 O.OI46 0.0198 0.0183 0.0165 O.OI5I 0.0197 O.Ol82 0.0165 O.OI5I O.OI99 0-0184 O.OI7I 0.0155 25 0.0130 O.OI30 0.0133 0.0137 0.0135 0.0139 215 NITROUS OXIDE NITROUS OXIDE N 2 CX SOLUBILITY IN WATER. (Bunsen; Gordon Z. physik. Ch. 18, 9, '95; Roth Ibid. 24, 123, '97; Knopp Ibid. 48,106, '04 Geffcken Ibid. 49, 276, '04.) Coefficient of Absorption ft. t. (B.) (G.) (R.) (K.) 9 CR.) (K.) (G.) 5 1.0950 1-0955 i .1403 0.205 i .161 I .067 10 0.9196 0.9200 0.9479 . . . 0.171 0.9815 0.9101 15 0.7778 0.7787 0.7896 0.143 0-8315 0.7784 20 o . 6700 0.6700 0.6654 0.6270 O.I2I o 7131 0.6739 0.6756 2 5 0.5961 ... -575 2 0.104 0.6281 0.5992 * Calculated by Geffcken. NOTE. Knopp and also Geffcken call attention to the fact thsfct Roth in making his determinations used a rubber tube between the gas burette and the shaking flask, and give this as an explanation of the high results which he obtained. SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SULPHURIC ACID. (Lunge Ber. 14, 2188, '81; see also Geffcken 's results.) Sp. Gr. of H 2 SO 4 i .84 i .80 i .705 i .45 i .25 Vols. N 2 O dissolved by 100 vols. H 2 SO 4 75-7 66.0 39.1 41.6 33 -o 100 vols. of KOH solution of 1.12 Sp. Gr. absorb 18.7 vols. N 2 O. 100 vols. of NaOH solution of i.io Sp. Gr. absorb 23.1 vols. N 2 O. SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF ACIDS. (Geffcken.) Results in terms of the Ostwald Solubility Expression (/). See p. 105, In Hydrochloric Acid. In Nitric Acid. In Sulphuric Acid. Cms. HC1 N 2 O Dissolved Gms.HNOa N 2 O Dissolved Gms. H 2 SO* N zO Dissolved per Liter. , b. / 25 . ' per Liter. ' / 15 . /25- per Liter. / 15 . /PS-" 18.22 0. 755 0-577 36. 52 0.777 0-597 2 4 . 52 0.734 0.566 36.45 O. 738 0.568 63- 05 0.777 0.602 49- 04 0.699 o-543 72.90 0. 716 0-557 126. 10 0-775 0.611 98. 08 0.645 0.509 147- 12 0.602 0.482 196. 16 0.562 0.463 SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF: (Roth.) Phosphoric Acid. Oxalic Acid. t Coefficient of ADS. in H 3 PO 4 Solutions of: Coefficient of Abs. in (COOH)2jolutions of: 3-38%. 4-72%. 8.84%. 9.89%. 13.35%. 0.812%. 3.70%. 5 1-057 I 0365 .9883 o 9635 0.9171 I .1450 1.1094 10 0.8827 .8665 .8296 .8101 0.7711 .9526 0.9264 15 0-7388 7258 .6977 .6826 0.6505 O .7940 0.7745 20 0.6253 .6147 .5926 .5810 0-5555 o .6694 0.6538 25 0.5427 5329 5*43 5054 o . 4860 o 5784 0-5643 NITROUS OXIDE 216 SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF PROPIONIC ACID AT 20. (Knopp.) Gms. C 2 H 6 COOH per liter 15 .15 60.42 Coef. of Absorp- tion of N 2 O 0.6323 0.6369 158.4 176.6 344.0 0.6504 0.6534 0.7219 SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SALT SOLUTIONS. Results by Geffcken page 105. Salt. Ammonium Chloride Ammonium Chloride Caesium Chloride Lithium Chloride Lithium Chloride Potassium Bromide Potassium Bromide Potassium Chloride Potassium Chloride Potassium Iodide Potassium Iodide Potassium Hydroxide Potassium Hydroxide Rubidium Chloride Rubidium Chloride in terms of the Ostwald expression (/). See Fnrrrmli Cone, of Salt per Liter. Solubility of N 2 O. l* ormuia, * Gram Equiv. Grams. /IS- /26- NH 4 C1 o-S 26.76 0.730 0-557 NH 4 C1 I .0 53-5 2 O.69I 0.529 CsCl o-5 84.17 0.710 0-544 LiCl o-5 21 .24 0.697 o-535 LiCl i.o 42.48 0.623 0.483 KBr o-5 59-55 0.697 o-53 6 KBr i .0 119.11 0.627 0.485 KC1 o-5 37-3 0.686 0.527 KC1 i .0 74.6 0.616 o-475 KI o-5 83.06 0.702 0.541 KI I.O 166.12 0-633 0.492 KOH o-5 28.08 0.668 0.514 KOH I .0 56.16 o-559 0.436 RbCl o-S 60.47 0.695 o-533 RbCl i .0 120.95 0.625 0.483 Results by Knopp, in terms of the coefficient of absorption. See page 105. Salt. Formula. Potassium Nitrate KNO, Sodium Nitrate NaNO Cone, of Salt per Liter. Coef. of Absorption Normality. Grams. of N 2 O at 20. 0.1061 10-74 0.6173 0.2764 27.94 0.6002 0.5630 56-97 0-57I3 1.1683 118.2 0-5196 0.1336 n-37 0.6089 0.3052 25-97 0.5876 0.6286 53-50 0.5465 1. 1200 95-30 0.4926 Results by Roth, in terms of the coefficient of absorption. Grams NaCl per 100 Grams Solution. o-99 1. 808 3.886 5-865 Coefficient of Absorption of N 2 O at: A 5. I .0609 1.0032 0.9I3I 0.8428 10. 15. 20. 0.8812 0.7339 0.6191 0.8383 0.7026 0.5962 0.7699 0.6495 0.5520 0.7090 0.5976 0.5088 25. 0.5363 0.5190 0-4475 0.4224 2i 7 NITROUS OXIDE SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SALT SOLUTIONS. Results by Gordon in terms of coefficient of absorption. See p. 105. Concentration of Salt. Coefficient of Absorption of N 2 O at: Salt. Grams per Gram 100 Grams Mols. 5. 10. 15. Solution. per Liter. Calcium Chloride 5-79 -547 0.819 0.697 0.591 0.500 9.86 0.964 0.668 0.586 0.509 0.435 " J 3-99 1-416 0.510 0.441 0.380 0.328 Lithium Chloride 1.35 0.319 0.986 0.831 0.700 0.594 " 3.85 0.928 0.878 0.743 0.629 0.536 11.48 2.883 0.606 0.512 0.437 0.382 Lithium Sulphate 2.37 0.219 0.934 0.792 0.670 0.569 5.46 0.521 0.795 0.665 0.557 0.474 8.56 0.836 0-646 0.555 0.477 0.415 Magnesium Sulphate 5.90 0.521 0.766 0.664 0.561 0.471 7.66 0.687 0.708 0.586 0.488 0.414 10.78 0.997 0.569 0.491 0.417 0.346 Potassium Chloride 4.90 0.676 0.879 0.751 0.643 0.555 7.64 1.037 o-799 0-693 0591 0.494 " 14-58 2.147 0.654 0.574 0.500 0.430 22.08 3.414 0.544 0.459 0.390 0.339 Potassium Sulphate 2.62 0.154 0.986 0.831 0.701 0.605 " 4.78 0.285 0.918 0.763 0.637 0.542 Sodium Chloride 6.20 1.107 0.800 0.682 0.585 0.509 8.88 1.614 -7 I 3 0-603 0.510 0.434 12.78 2.391 0.634 0.532 0.449 0.386 Sodium Sulphate 5.76 0.427 0.808 0.677 0.584 0.495 8-53 0.646 0.692 0.574 0.482 0.416 " 12.44 0.974 0.559 0.486 0.417 0.354 Strontium Chloride 3.31 0.215 0.928 0.788 0.671 0.578 5.73 0.380 0.848 0.709 0.610 0.550 13.24 0.939 0.644 0.547 0.463 0.390 SOLUBILITY OF NITROUS OXIDE IN ALCOHOL AND IN AQUEOUS CHLORAL HYDRATE SOLUTIONS AT 20. (Bunsen; Knopp Z. physik. Ch. 48, 106, '04.) In Alcohol (B.). In Aq. Chloral Hydrate (K.). Vols. N 2 t . (at o and 760 mm .) peri Vol. Alcohol. Normality C 2 HCl3O.H 2 0. Cms. C 2 HC1 3 O.H 2 O per Liter. Coef . of Abs. of NaO. O 4.178 0.184 30-43 0.618 5 3-844 0-445 73.60 0-613 IO 3-541 0.942 155-8 0-596 15 3.268 1 .165 192.7 0.589 20 3-025 1.474 243-8 0-579 24 2.853 1 .911 316.4 0.567 SOLUBILITY OF NITROUS OXIDE IN PETROLEUM. COEFFICIENT OF ABSORPTION AT 10 = 2.49, AT 20 = 2.11. (Gniewasz and WaJfisz Z. physik. Ch. I, 70, '87.) NITROUS OXIDE 218 SOLUBILITY OF NITROUS OXIDE IN AQUEOUS SOLUTIONS OF GLYCERINE AND OF UREA. (Roth.) Coefficient of Absorption of N2O in Glycerine Solutions of: t . 5 10 r 5 20 25 3.46 per cent. 6.73 per cent. 12.12 per cent. 16.24 per cent. 1.097 1-055 0-999 0.959 0.917 0.887 0.841 0.810 0.767 0.745 0.710 0.686 0.647 0.630 0.605 0.585 0.556 0.542 0.527 0.508 Coefficient of Absorption of N 2 O in Urea Solutions of: 3.31 per cent. 4.97 per cent. 6.37 per cent. 7.30 per cent 5 1.104 1.096 i. 088 i.ioi 10 0.921 0.920 0.909 0.921 15 0.771 0.773 0-76I 0.772 20 0.653 0.656 0.644 0.655 25 0.569 0.567 0-559 0.570 NITRIC OXIDE NO. SOLUBILITY IN WATER. (Winkler Ber. 34, I4T4, '01.) 9.97 per cent. I .069 0.901 0.761 0.651 0.569 t. ft P'. 9- t. ft. r. 7- O .0738 0734 0-00984 40 035 1 0325 O.OO4 5 .0646 .0641 O.OO86O 50 o 0315 .0277 O.OO3 10 0571 .0564 0.00757 60 .0295 0237 0.003 15 o 0515 .0506 O.OO68O 70 .0281 .0195 O.OO2 20 .0471 .0460 0.0o6l8 80 .0270 .0144 O-OOI 25 o .0430 .0419 0-00564 90 .0265 .0082 0.001 30 .0400 .0384 O.OO5I7 100 .0263 OOOO o.ooo For values oi ft, ft' and q, see Ethane, page 133. SOLUBILITY OF NITRIC OXIDE IN AQUEOUS SULPHURIC ACID SOLUTIONS AT 18. (Lunge Ber. 18, 1391, '85; Tower Z. anorg. Ch. 50, 382, '06.) Wt. per cent H 2 SO 4 in Solution. 9 8 90 80 70 60 SO Sp. Gr. at 15. 1.8 4 1.82 i-733 1.616 1 399 Tension of H 2 O Vapor. o.i mm. 0.4 " 6.2 Solubility Coefficient * of NO at 18. 0.0227 (0.035, L.) 0.0193 O.OII7 O.OII3 0.0118 (0.017, L. O.OI2O * Volume of NO (at 760 mm.) per i volume of aqueous H 2 SO 4 . SOLUBILITY OF NITRIC OXIDE IN ALCOHOL. (Bunsen.) t o 5 10 15 20 Vols. NO* 0.316 0.300 0.286 0.275 0.266 absorbed by i vol. Ale. 24 0.261 * At o and 760 mm. 2i 9 OXALIC ACID OXALIC ACID (COOH) 2 . 2 H 2 O. SOLUBILITY IN WATER. (Average curve from results of Alluard; Miczynski Monatsh. Ch. 7, 258, '86; Henry Compt. rend. 9 H57 '84; Lamouroux Ibid. 128, 998, 'oo; at 25, Foote and Andrew Am. Ch. J. 34, 154, '05.) Grams (COOH) 2 per 100 Grams ^ Grams (COOH) 2 per 100 Grams H 2 O. Solution. H 2 O. Solution. o 3-45 3-33 40 21.15 17.46 10 5-55 5-26 50 31-53 23.97 20 8.78 8.07 60 45.55 31-37 25 II-36 10.21 70 63.82 38.95 30 13-77 II -9 I SOLUBILITY OF OXALIC ACID IN ALCOHOLS. (Timofeiew Compt. rend. 112, 1137, '91; Bourgoin Ann. chim. phys. [5] 13, 406, '78). Grams (COOH) 2 per 100 Grams of: Methyl Alcohol. Ethyl Alcohol. Propyl Alcohol. i 36.26 20.25 9-73 + 20 47-24 26.23 I5-I4 SOLUBILITY OF OXALIC ACID IN ABSOLUTE AND IN AQ. ETHER AT 25. (Bodtker Z. physik. Ch. 22, 512, '97; Bourgoin.) ioo grams absolute ether dissolve 1.47 grams (COOH) 2 .2H 2 O. 100 grams absolute ether dissolve 23.59 grams (COOH) 2 . In Aqueous Ether Solutions. Gms. Solid Acid Added per ioo cc. Ether Solution. Grams per ioo cc. Ether Solution. (COOH) 2 . 2 H 2 O. (COOH) 2 . H 2 O. (COOH) 2 . (1) 5.0 o.o 1-250 0.742 (2) 5.0 o.o 0.788 0.720 5.0 o.o 0.418 1.044 S-o 2.44 0.360 3.388 5.0 4.82 0.484 6.038 5-o 7-i4 0.558 8.538 5.0 9.42 0.632 10.996 5.0 11.63 0.676 13-316 5.0 13.79 0.761 15-684 5.0 18.18 0.816 17.818 5.0 22.73 0.816 17.818 (i) Ether saturated with water. (2) Ether containing 0.694 per cent water. ioo grams glycerine dissolve 15 grams oxalic acid at 15.5. DISTRIBUTION OF OXALIC ACID BETWEEN WATER AND AMYL ALCOHOL AT 20. (Herz and Fischer Ber. 37. 4748, '04.) Millimols i(COOH) 2 per 10 cc. Grams (COOH) a per ioo cc. Aq. Layer. Alcoholic Layer. Aq. Layer. Alcoholic Layer. o.68c6 O.I45I 0.306 0.0653 2.364 0.7233 1.064 0.320 6.699 2-550 3-015 I.I48 10.029 4.300 4-5" 1-934 OXYGEN 220 OXYGEN O. SOLUBILITY IN WATER. (Winkler Ber. 34, 3609, '91; Bohr and Bock Wied. Ann. [2] 44. 318, '91.) t. Coef. of Absorpdon /3. 9> cc. O per Liter HzO. 10.187 8.907 7.873 7.038 6.356 5.776 5.255 1 tB t. Coef. of Absorpdon ft. ?< O 5 10 15 20 25 30 0.0489* 0.0429 0.0380 0.0342 O.O3IO 0.0283 O.O26l 0.0496! 0.0439 0.0390 0.0350 0.0317 O.029O 0.0268 0.00695 0.00607 0.00537 0.00480 0.00434 0.00393 0.00359 *W. 40 o. 50 o. 60 o. 70 o. 80 o. 90 o. :oo o. . and B. 0231* 0209 0195 0183 0176 0172 0170 0.0233! O.O207 0.0189 0.0178 O.OI72 0.0169 0.0168 o. o. 0. 0. 0. 0. o. 00308 00266 00227 00186 00138 00079 ooooo For values of ft and q see Ethane, page 133. SOLUBILITY OF THE OXYGEN OF AIR IN WATER. t. 5.2 5-65 14-78 24.8 Solubility* 8.856 8.744 7.08 5.762 * cc. Oxygen per 1000 cc. H 2 O saturated with air at 760 mm. SOLUBILITY OF OXYGEN IN WATER AND IN AQUEOUS SOLUTIONS OF ACIDS, BASES AND SALTS. (Geffcken Z. physik. Ch. 49, 269, '04.) Aq. Solution of: Concentration per Liter. Solubility of Oxygen.* Gram Equiv. Grams. / 15 . /26- Water alone ... ... 0-0363 0.0308 Hydrochloric Acid 0-5 18.22 0.0344 O.O296 " i -o 36-45 0.0327 0.0287 " 2.0 72.90 O.O299 0.0267 Nitric Acid -5 36-52 0.0348 O.O3O2 u i.o 63.05 0.0336 0.0295 (I 2.O I26.IO 0-0315 O.0284 Sulphuric Acid 0.5 24.52 0-0338 0.0288 " i.o 49-04 0.0319 0.0275 " 2.0 98.08 0-0335 O.O25I " 3-o i47- I 2 0.0256 O.O229 " 4.0 196.16 0.0233 0.0209 5.0 245.20 0.0231 O.OI94 Potassium Hydroxide 0.5 28.08 O.O29I O.O252 " i.o 56.16 0.0234 O.O2O6 Sodium Hydroxide 0.5 20.03 0.0288 O.O250 " i.o 40.06 0.0231 O.O2O4 " 2.0 80. I 2 O.OI52 0.0133 Potassium Sulphate o-5 43-59 0.0294 0,0253 " i.o 87.18 0.0237 O.O2O7 Sodium Chloride o-5 29.25 O.O262 n i.o 58.5 O.O26o O.O223 u 2.0 H9.0 0.0182 O.OI58 * In terms of the Ostwald Solubility Expressions . See page 105 SOLUBILITY OF OXYGEN IN AQ. POTASSIUM CYANIDE SOLUTIONS AT 20. (Maclaurin J. Ch. Soc 63, 737, '93.) Cms. KCN per 100 gms. sol. i 10 20 30 50 Coefficient of absorption of O 0.029 0.018 0.013 0.008 0.003 221 OXYGEN SOLUBILITY OF OXYGEN IN ETHYL ALCOHOL, METHYL ALCOHOL AND IN ACETONE. (Timofejew Z. physik. Ch. 6, 151, '90; Levi Gazz. chim. ital. 31, II, 513, 'ox.) t0 In Ethyl Alcohol of 99.7% (T.). Atohofci'!) In Acetone (L.) P fj / = o 0.2337 0.2297 0.31864 0.2997 5 0.2301 0.2247 0.30506 0.2835 10 0.2266 0.2194 0.29005 0.2667 15 0.2232 0.2137 0.27361 0.2493 20 0.2201 0.2073 0.25574 0.2313 25 0.2177 (24) 0.2017 (24) 0.23642 0.2127 30 ... 0.21569 0.1935 40 ... ... 0.16990 0.1533 50 ... ... 0.11840 0.1057 For values of /3 and p', see Ethane, page 133. / Ostwald Solu- bility Expression. Seepage 105. The formulae expressing the solubility of oxygen in methyl alcohol and in acetone as shown in the above table are as follows: In Methyl Alcohol / = 0.31864 0.002572 t 0.00002866 1*. In Acetone /= 0.2997 0.00318* 0.000012**. SOLUBILITY OF OXYGEN IN AQUEOUS ALCOHOL AT 20 AND 760 MM. (Lubarsch Wied. Ann. [2] 37. 5S. '89.) yss!* Vol. per cent Absorbed O. Wt. per cent Alcohol. Vol. per cent Absorbed O. Wt. per cent Alcohol. Vol. per cent Absorbed O. o.oo 9.09 16.67 2.98 2.78 2.63 23.08 28.57 33-33 2.52 2-49 2.6 7 50.0 66.67 8o.O 3-50 4-95 5.66 SOLUBILITY OF OXYGEN IN PETROLEUM. COEFFICIENT OF ABSORP- TION AT 10 = 0.229, AT 20 = 0.202. (Gniewasz and Walfisz Z. physik. Ch. I, 70, '87.) OZONE O,. SOLUBILITY IN WATER. (von Mailfert Compt. rend. H9t 051, W. Carius; Schone Ber. 6, 1194, '73.) t. W. G. R. t*. W. G. R. o 39.4 61.5 0.641 27 13.9 51.4 0.270 6 34.3 61.0 0.562 33 7.7 39.5 0.195 ii. 8 29.9 59.6 0.500 40 4.2 37.6 0.112 13.0 28.0 58.1 0.482 47 2.4 31.2 0.077 15-0 25.9 56.8 0.456 55 - 6 J 9-3 0-Q3 1 19.0 21. o 55-2 0.381 60 o.o 12.3 o.ooo W Milligrams Ozone dissolved per liter water. G Milligrams Ozone in one liter of the gas phase above the solutions. R = Ratio of the dissolved to undissolved Ozone ( W -3- G) . PARAFFINE 222 SOLUBILITY OF OZOKERITE PARAFFINE OF MELTING POINT 64-6s ( AND SP. GR. AT 20 = 0.917 IN SEVERAL SOLVENTS AT 2O. (Pawlewski and Filemonowicz Ber. 21, 2973, ' 88 -) Solvent. Carbon Bisulphide Benzine, boiling below 75 Turpentine, b.pt. i58-i66 Cumol, com. b.pt. 160 " frac. 150-! 60 Xylene, com.b.pt. 135- " frac. i35-i38 Toluene, com.b.pt. io8-i 10 " frac. io8-io9 Chloroform Benzene Ethyl Ether Iso Butyl Alcohol, com. Gms. Paraffine per 100 Gms. cc. Solvent. Solvent. Solvent. 12.99 Acetone ' 11-73 8] 4 8 Ethyl Acetate 3 6.06 5-21 " Alcohol 4.26 3-7 2 Amyl Alcohol 3-99 3 3-95 3-39 3-43 Propionic Acid Propyl Alcohol 4-39 3-77 Methyl Alcohol 10 3.88 3-34 Methyl Formate 3-92 2.42 3-4i 3.61 Acetic Acid " Anhydride 1.99 J -75 Formic Acid Ethyl Alcohol 75% Gms.Paraffine per TOO 0.285 0.228 Gms. cc. Solvent. Solvent. o. 262 o. 209 0.238 o. 219 O. 2O2 o. 164 0.165 o. 141 O.O7I 0.056 O.O60 O.O6O 0.063 O.O25 0.013 o. 015 o. 0003 PAPAVERINE C 20 H 21 N0 4 . 100 grams pure carbon tetra chloride dissolve 0.203 gram at 17. (Schindelmeiser Chem.-Ztg. 25, 129, '01.) PHENANTHRENE C 14 H 10 . SOLUBILITY IN ALCOHOL AND IN TOLUENE.* (Speyers Am. J. Sci. [4] 14, 295, '02.) In Alcohol. In Toluene. t Gms. CuHio pe 100 Grams r Sp. Gr. of Solutions Gms. Ci 4 Hi per 100 Grams Sp. Gr. of Solutions CjjHsOH. (H20 at 4 .) C 6 H 6 .CH3 (H 2 at 4-) o 3-65 0.8l4 23.0 0.925 10 3 .80 0-807 30-0 0.929 20 4-6 O.Soi 42 .O 0-934 25 5-5 o-799 5- 0-939 30 6.4 0-797 5 8.0 0-943 40 8.2 o-795 76.0 o-955 50 10.6 o-794 95-o 0.971 60 15-6 0-797 115.0 0.989 70 0.815 135 .0 i .007 80 0.865 (76. 4) ISS-O 1.027 * Calculated from the original results which are given in terms of gram molecules of Phenanthrene per 100 gram molecules of solvent, and for irregular intervals of temperature. Behrend Z. physik. Ch. 10, 265, '92, finds 2.77 grams phenan- threne per 100 grams alcohol at 12.3, and 3.09 grams at 14.8. 223 PHENANTHRENE SOLUBILITY OF PHENANTHRENE PICRATE IN ABSOLUTE ALCOHOL. (Behrend Z. physik. Ch. 10, 205, '92.) Grams per 100 Grams Saturated Solution. , Picric Acid H h Phenanthrene = Phenanthrene Picrate. 12-3 0.91 0.71 1.62 14-3 1. 00 0.78 1.78 17-5 1.05 0.82 1.87 SOLUBILITY OF PHENANTHRENE PICRATE IN ALCOHOLIC SOLUTIONS CONTAINING PICRIC ACID AND ALSO PHENANTHRENE. (Behrend.) Grams Added to 62 cc. Abs. Alcohol. Gms. per 100 Cms. Sat. Solution. P. Picrate + Picric Ac. -j- Phenanthrene. Picric Ac. + Phenanthrene P. Picrate. 12-3 1.4 o o-5 o-534 1-413 1-947 12-3 1.4 0.9 0.409 2.141 2 -550 12.3 0.8 o 2.1 o-354 2.77 3.124 I2. 3 0.8 4-0 0.139 5.626 5-765 17-5 1.4 O.I I - I 59 o-75 I.9I 17-5 1.4 0.2 O 1.285 0.68 1.97 17-5 1.4 1.0 o 2-45 o-37 2.82 J 7-5 1.4 4.0 6.15 0.195 6-345 17-5 1.4 0-0 2.2 0.423 3.276 3- 6 99 PHENOL C 6 H 5 OH. SOLUBILITY IN WATER. (Alexejew Wied. Ann. 28, 305, '86; Schreinemaker Z. physik. Ch. 33, 79, 'oo; Rothmund Ibid 26, 474. '98-) Determinations were made by the " Synthetic Method," for which see Note, page 9. Grams Phenol per 100 Grams 10 20 30 40 50 55 60 65 68.3 (crit. temp.) 33.4 Vaubel J. pr. Ch. [2] 62, 73, '95, states that 100 grams sat. aque- rus solution contain 6.1 grams phenol at 20. Sp. Gr. of solution 1.0057. SOLUBILITY OF PHENIC ACID (PHENOL, C 6 H 5 OH) IN PARAFPINE AND IN BENZENE. (Schweissinger Pharm. Ztg. '84-'8s.) Grams CaH 5 OH per 100 Grams Solvent at: Solvent. f *- > 16. 21. 25. 43. Paraffine 1.66 ... ... 5.0 Benzene 2.5 8.33 10.0 100.0 Aqueous Layer. Phenol Layer. 7-5 75 .0 8-3 72 .1 8.8 6 9 .8 9.6 66 9 12.0 62 7 I4-I 59 5 I6. 7 55 4 21-9 49 .2 PHENOL 224 SOLUBILITY OF PHENOL IN AQUEOUS ACETONE SOLUTIONS. (Schreinemaker.) In 4.24 % Acetone. In 12.2% Acetone. In 24.4% Acetone. Grams Phenol per Gms. Phenol per Gms. Phenol per to ioo Gms. ioo Gms ioo Gms. . Aq. Acetone Phenol Aq . Acetone Phenol Aq. Acetone Phenol Layer. Layer. Layer. Layer. Layer. Layer. 20 . ... . . . . . 3 5.0 74.0 4.0 71.0 6.0 69.5 40 5-5 70.0 5 60 1.1 67.0 61.0 5 : 67.0 8.0 64.0 70 9.0 51.0 7-5 57-5 19.0 57- 80 14.0 34-0 10.5 49-5 14.0 52-5 (84) 22.5 20. 4* 30-5* 23- of 47. ot (90. 3) 25-0 26. 5t 44.0$ (9- 5) 35- o go t8 5 t87.s 45 In 59-9% Acetone. Gms. Phenol per ioo Gms. Aq . Acetone Phenol Layer. Layer 26. O 60. 5 28.5 57.0 32.0 52.0 34.5$ 49- c 36.511 46.50 (49.5) 41.5 !l47.S The figures in the above table were read from curves plotted from the original results. SOLUBILITY OF PHENOL IN AQUEOUS SOLUTIONS d TARTARIC ACID. (Schreinemaker.) In 5.093% Acid. Gms. Phenol per ioo Gms. In 19.34% Acid. Gms. Phenol per ioo Gms. In 40.9% Acid. Gms.Phenol per ioo Gms. Aq. Acid Phenol ~~ Layer. Layer. 13.0 16.5 77.0 20.0 74.0 26.5 71.0 39-o 63.5 54-0 30 50 60 65 I 7 ' 5 69 Aq. Acid Layer. 7-5 10.5 i4.5 19-5 25.0 47- Phenol Layer. 72.5 65.5 58.0 48.5 5 60 70 75 77 Aq. Acid Layer. 10. 12-5 19.0 29.0 47.0 Phenol Layer. 77.0 72.0 64.0 56.0 70 80 85 90 95 97 DISTRIBUTION OF PHENOL BETWEEN: AMYL ALCOHOL AND WATER AT 25. (Herz and Fischer Ber. 37, 4747, '04.) Millimols Phenol per lo cc. Gms. Phenol per ioo cc. Volumes of Solvents Alcoholic Aqueous Layer. Layer. Alcoholic Aqueous Layer. Layer. used per i Gm. Phenol o. 75 o. 047 o. 705 o. 0441 5occ.H 2 O+ 5occ.C a I 0.9 0.05 o. 846 o. 047 " +IOOCC. " i.i 0.07 1.035 0.066 " +15000. " 2. 6 o. 16 2.445 - X 5 " +200CC. 54- r 3.83 50.88 3.601 5 6 -3 3-9 52.93 3.667 BENZENE AND WATER AT 2oc (Vaubel J. pr. Ch. [2] 67. 476. V 3.) Gms. Phenol in- 'H 2 CeHo ' Layer. Layer O. 286 o. 714 o. 1188 0.8212 0.0893 0.9107 0.0893 0.9107 22 5 PHENOL DISTRIBUTION OP PHENOL BETWEEN WATER AND BENZENE AND BETWEEN AQUEOUS K 2 SO 4 SOLUTIONS AND BENZENE AT 25. (Rothmund and Wilsmore Z. physik. Ch. 40, 623, '02.) NOTE. The original results, which are given in terms of gram mols. per liter, were calculated to grams per liter, and plotted on cross- section paper. The following figures were read from the curves obtained. Between H 2 O and CaHa. Effect of K 2 SO 4 upon the Distribution. Grams C WHsOH Cms. K 2 SO 4 (i) Cms. CsHsOH (a)Gms. CH 6 OH per Liter of: per Liter per Liter of: per Liter of: fi,0 Layer. CeH, Layer. Aq. Solution. Aq. Layer. Layer. Aq. Layer. Layer. 5 10 1.36 17.08 59-96 9-52 26.28 10 28 2.72 16.92 60.63 9-50 26.38 15 52 5-44 16.85 60.92 9.46 26.55 20 84 10.89 16.44 62.73 9-35 27.06 25 128 21.79 15.89 65.19 9.09 28.27 30 200 43-59 14-85 69.71 8.68 30.21 35 300 87.18 12.92 78.00 7-79 34.38 40 410 45 520 50 610 (i) First series. (*) Second series. DISTRIBUTION OF PHENOL AT 25 BETWEEN: (Herz and Fischer Ber. 38, 1143, '05.) Water and Toluene. Water and m Xylene. Millimols Cel^OR per 10 cc. Grams CeHsOH per TOO cc. Millimols CftHsOH per 10 cc. Grams QjHeOH per 100 cc_ C 8 H,CH 3 Layer. H 2 O Layer. CH 5 CH3 Layer. H 2 O Layer. '*% ELXCHg) ayer. t H 2 0* Layer. mCH4(CH3) Layer. 2 H 2 0' Layer. 1.244 0.724 I .169 0.681 I 6lO I .071 I 5 J 4 1.007 3-047 1.469 2 .865 1.381 4 .787 2 .726 4 .501 2-563 4.667 2.2OO 4 .389 2.068 12 .210 5 .168 II .22 4.860 6.446 2.861 6 .061 2 .691 22 .718 6 994 21 36 6-577 14.960 4-750 14 07 4.467 34 .827 8 .124 32 75 7.640 I7-725 5-346 16 .69 5.027 5 1 352 9 .123 4 8 .28 8.578 47-003 7.706 44 .20 7.246 77 703 10 .050 73 .07 9-450 53 -783 8.087 50 58 7.604 90.287 9.651 84 .89 9.074 DISTRIBUTION OF PHENOL BETWEEN WATER AND CARBON TETRA CHLORIDE AT 20. (Vaubel J. pr. Ch. [2] 67, 4?6, '03.) Grams Phenol in: Gms. Phenol Used. Volumes of Solvents. 50 cc. H 2 O+ 10 cc. CC1 4 + 20 CC. + 30 cc. + 50 cc. -f 100 CC. H-I50CC. + 200 CC. H:zO Layer. CCL, Layer. 0.8605 0.1285 0.7990 0.1900 0.7275 0.2015 0.6435 0.3455 o . 4680 0.5210 0.3645 0.6245 0.3240 0.6650 PHENOLATE 226 PHENOLATE of Phenyl Ammonium. SOLUBILITY IN WATER. Figures read from Curve. (Alexejew Wied. Ann. 28, 305, '86.) By Synthetic Method, See page 9. Gms. Phenolate per 100 Gms. Gms. Phenolate per 100 Gms. Aq. Layer. Phenolate Layer. Aq. Layer. Phenolate Layer. 10 3 94 no 9 76 30 4 93 120 12 69 50 5 91 130 17.5 60 70 6 87.5 140 (crit. temp.) 40 90 7 83 PHENYL (Di) AMINES C 6 H 4 (NH 2 ) 2 . SOLUBILITY IN WATER AT 20. (Vaubel J. pr. Ch. [2] 52, 73, '95-) Aminp Gms. per 100 Sp. Gr. of Gms. Solution. Solution. m Phenyl di Amine 23.8 1.0317 P 3-7 1-0038 Nitro PHENOLS C 6 H 4 .OH.NO 2 . 100 grams saturated aqueous solution contain: 0.208 gram ortho, 2.14 grams meta, 1.32 grams para nitro phenol at 20. (Vaubel.) Di Nitro PHENOL C 6 H 3 .OH.(NO 2 ) 2 . SOLUBILITY IN ALCOHOLS AT 19.5. (de Bruyn Z. physik. Ch. 10, 784, '92.) ioo grams abs. methyl alcohol dissolve 6.3 grams C 6 H 3 .OH.(NO 2 ) 2 . 100 grams abs. ethyl alcohol dissolve 3.9 grams C 6 H 3 .OH.(NO 2 ) 2 . SOLUBILITY OF MIXTURES OF 5 TRI BROM PHENOL AND 5 TRI CHLOR PHENOL IN METHYL ALCOHOL AT 25. (Thiel Z. physik. Ch. 43, 667, '03; from Wurfel Dissertation Marburg, '96.) Molecular per cent C 6 H 2 .OH.Br 3 n Solubility of ^ In Solid. In Solution. C 6 Ho.OH.CJ 3 . C 6 H 2 .OH.Br 3 . O O O.204 O O.2O4 4-49 3-59 0.194 O.OO7 0.201 10.13 7-58 0.191 0.016 0.206 16.28 12.15 0.172 0.024 0.196 62.44 13.07 0.204 0.031 0-235 69.88 15.86 0.150 0.028 0.178 81.76 19.01 0.096 0.023 O.IlS 84.66 24.05 0.069 O.O22 O.O9I 87-53 32.46 0-043 O-O2I 0.063 93.62 47-87 O-O2I O.OI9 O.O4O 100.0 IOO.O O-O O.OI9 O.OI9 227 PHENYL SALIOYLATE PHENYL SALICYLATE (Salol) C 6 H 4 (OH).COOC 6 H 5 i: 2 . TOO grams H 2 O dissolve 0.043 gram salicylate at 25. 100 grams alcohol dissolve 20.0 grams at 25. (u. s. P.) Di PHENYL C 6 H 5 .C,H 6 . 100 grams absolute methyl alcohol dissolve 6.57 grams at 19.5. 100 grams abs. ethyl alcohol dissolve 9.98 grams at 19.5. (de Bruyn Z. physik. Ch. 10, 784, '92.) PHOSPHO MOLYBDIC ACID P 2 O 5 .2oMoO 3 .5 2 H 2 O. SOLUBILITY IN ETHER. ((Parmentier Compt. rend. 104, 686, '87.) t o 8.1 19.3 27. 4 C Gms. Acid per ioo gms. Ether 80.6 84.7 96.7 103.9 107.9 PHOSPHORUS P. (yellow) SOLUBILITY IN BENZENE. (Christomanos Z. anorg, Ch. 45, 136, '05.) t. Gms. P p ioo Gms. C er Sp. Gr. ofj 5 H s : &**. Gms. P per t . ioo Gms. (C 2 H 6 ) 2 0. O 0-434 . . . 15 0.90 0.723 28 i. 60 5 O.62 . . . 18 I .01 0.719 30 i .75 8 0-79 0.732 20 I .04 0.718 33 i. 80 10 0.85 0.729 23 I .12 0.722 35 2 -OO 25 i-39 0.728 ioo grams CS 2 dissolve about 1750 grams yellow P at room temper- ature. (Vogel Jahresber. Chem. 149, '68.) ioo grams alcohol of 0.799 Sp. Gr. dissolve 0.312 gram P cold and 0.416 gram hot. (Buchner) PHOSPHORUS 228 SOLUBILITY OP YELLOW PHOSPHORUS IN SEVERAL SOLVENTS AT 15. (Stich Pharm. Ztg. 48, 343, '03.) Solvent. Cms. P per 100 Cms. Solution. Almond Oil 1.25 Oleic Acid i -06 Paraffine i -45 Water 0.0003 Acetic Acid o . 105 PHTHALIO ACIDS C 6 H 4 (COOH) 2 . SOLUBILITY IN WATER. (Vaubel J. pr. Ch. [2] 52, 73, '95; 59. 3. '99-) Acid. t . Cms. per 100 Cms. Solution. o Phthalic Acid 14 0.54 Iso Phthalic Acid 25 0.013 Tere Phthalic Acid . . almost insoluble SOLUBILITY OF o PHTHALIC ACID IN ALCOHOL AND IN ETHER AT 15* (Bourgoin Ann. chim. phys. [5] 13, 406, '78.) Grams QHUCCOOH^ o per 100 Grams Solution. Solvent.' Absolute Alcohol 9 . 1 56 1 1 . 70 90 per cent Alcohol 10.478 10.08 Ether 0.679 0.684 CO PHTHALIO ANHYDRIDE C 6 H 4 - SOLUBILITY IN WATER. (van der Stadt Z. physik. Ch. 41, 358, '02.) All determinations, except first three, made by the Synthetic Method. See page 9. 1 Grams C 8 H 4 O3 per 100 Gms. Mol. i >er cent t Grams CsI^Oa per 100 Gms. J^ ^ Water. Solution. C 8H43- w Water. Solution. CsHtOz O 0.00295 . 00295 .00036 189. 5 1076 QI. 66 5 6 -73 25 0.6194 .6150 0.0754 188. 8 1265 92. 68 60.63 5 1.630 I .604 .198 187. X 1474 93- 65 64.22 94-3 4 8 54 10 3 181. 8 2332 95- 88 73-95 165.4 210. O 6 7 75 20 36 176. 2 3334 97- 07 80.23 179-4 3I9-3 76 13 27 .98 169. 4 5745 98. 28 87.49 186.2 449.6 81 .81 35 37 130. 9 37570 99- 72 97.89 189.6 546.1 84 50 39 93 83010 99- 86 99.02 191.0 821.5 89 .19 50 .00 131. 2 00 100. 00 100.00 190.4 863.4 89 .62 24 On page 362 of the original paper the solubility of C 8 H 4 O, at o is given as 0.2722 gram per 100 grams of solution. 229 PHTHALIC ANHYDRIDE SOLUBILITY OF PHTHALIC ANHYDRIDE IN CARBON BISULPHIDE. (Arctowski Compt. rend. 121, 123, '95; Etard Ann. chim. phys. [7] 2, 570, '94-) Gms. CgHjOa Gms. C 8 H4O 3 Gms. CgH 4 O3 t. per ioo Gms. t. per ioo Gms. t. per ioo Gms. Solution. Solution. Solution. 112.5 0.013 + 10 o-3 70 2-3 - 93 0.013 20 0.7 90 3-7 - 77-5 0.016 30 0.8 IOO 5-o - 40 0.03 40 1.2 120 8.0 20 0.06 50 -3 I4O J 3-3 10 o.io 60 i-7 160 20.7 O.2O 180 30.2 PHYSOSTIGMINE SALIOYLATE C 6 H 4 (OH)COOH.C 16 H tl N,O 2 and Physostigmine Sulphate H 2 SO 4 (C 1S H 21 N 3 O 2 ) 2 . SOLUBILITY IN WATER, ALCOHOL, ETC. (U. S. P.) e Gms. per 100 Gms. Solvent. "Salicylate. Sulphate/ Water 25 1.38 very soluble Water 80 6.66 Alcohol 25 7.87 " Alcohol 60 25.00 Chloroform 25 n.6 Ether 25 0.57 0.083 PICRIC ACID C 6 H 2 .OH.(NO 2 ) 3 . SOLUBILITY IN WATER. (Dolinski Ber. 38, 1836, '05; Findlay J. Ch. Soc. 81, 1219, '02.) Gms. CeHgNgOr per 100 Grams Gms. QjHsNgOr per 100 Grams Solution. Water. Solution. Water. O 0.67(D.) 0.68 (D.) 1.05 (F.) 60 2-77(D.) 2.8KD.) 3.I7(F4 10 .80 0.81 i. 10 70 3.35 3.47 3- 8 9 20 1. 10 I. II 1.22 80 4-22 4.41 4.66 30 1.38 1.40 1.55 oo 5.44 5-72 5-49 40 1.75 1.78 1.98 100 6.75 7.24 6.33 50 2.15 2.19 2.53 Dolinski does not refer to the previous determinations of Findlay. PICRIC ACID 230 SOLUBILITY OF PICRIC ACID IN WATER AND IN AQUEOUS SALT SOLUTIONS AT 25. (Levin Z. physik. Ch. 55, 520, '06.) One liter of aqueous solution contains 0.05328 gram mols. = 12.20 grams C e H 2 .OH(NO 2 ) 3 at 25. Gm. Mols. Salt per j-.uer in /\ * q- oomuuiis 01 per Liter. NaCl. NaNQs. Na 2 SO 4 . LiCl. Li 2 S0 4 . NItiCl. 0.01 0.05524 0.05529 o .05604 0.05480 0.05661 0.05487 O.O2 0-05559 0.05872 o 05872 0-05558 0.06053 0.05540 O.O5 0.05729 0.06632 o .06632 0.05703 0.06691 0.05771 0.07 0.05862 0.07093 o .07093 0.05878 0.07013 0.05865 O.IO 0.05902 0.07670 o .07670 0.06132 0.07437 0.50 O.O79O 0.123 I .OO O-IlSo 0.149 Gm. Mols. Grams Picric Acid per Liter in Aq. Solutions of: Salt per Liter NaCl. NaN0 3 . Na 2 SO. LiCl. Li 2 S0 4 . NH4C1. O.OI 12.66 12.67 12.83 I2 -55 12-97 12-57 O-O2 12.74 13-45 13-45 12.74 I3-87 12.69 O.O5 13.12 i5- J 9 15 -!9 13.06 15-33 13.22 0.07 13-43 16.25 16.25 13-47 16.06 13-44 O.IO I3-5 2 17-57 17-57 14.05 17.04 0.50 18.09 28.18 I .00 26.98 34-14 Solubility in Aq. Cane Sugar. Solubility in Aq. Grape Sugar. Gm. Mols. Sugar per Liter. Picric Ac. per Liter Solution. Sp. Gr. Solution. Gm. Mols. Grape Sugar per Liter. Picric Acid per Liter Sol. Gm. Mols. Gms. G. Mols. Gms. O.IO 0.05202 II .92 I .0122 O.IO 0-0530 12.14 0.25 0-04978 II .40 I.03I9 0.25 0.0521 n-93 0.50 0.0482 II .04 I .0654 0.50 0.0509 11.66 I -OO 0-0443 IO.I5 I.I294 1. 00 0.0474 10.86 SOLUBILITY OF PICRIC ACID IN ABSOLUTE ALCOHOL. (Behrend Z. physik. Ch. 10, 265, '92.) TOO gms. sat. solution contain 5.53 grams CeHgNgOy at 12.3, and 5.92 grams at 14.8. Sp. Gr. of the latter solution = 0.8255. SOLUBILITY OF PICRIC ACID IN BENZENE. Gms. Mols. ^HsNsOr C 6 H 3 N 3 7 per 100 per 100 "viols. C 6 H 6 . (Findlay.) t Gms. Mols. per_ioo Gms. i per 100 Mols.CeHe. 5 10 *5 20 25 26. 35 5 7 9 12 37 29 56 ,66 21.38 1.26 1.83 2.48 3-25 4-30 4.60 7. .6 38.4 26.15 8.88 45 33-57 ii .40 55 50-65 17.21 58-7 58.42 19.83 65 71 .31 24.20 75 96.77 32.92 231 PICRIC AOID SOLUBILITY OP PICRIC ACID IN ETHER. (Bougault J. pharm. chim. [6] 18, 116, '03; Apoth.-Ztg. 21, 74, '06.) Solvent. Ether of Sp. Gr. 0.721 Ether of Sp. Gr. o . 725 (0.8 pt. H 2 O per 100) Ether of Sp. Gr. 0.726 (i.o pt. H 2 O per 100) Ether saturated with H 2 O H 2 O saturated with Ether t. Gms. CeHaNa C>7 per Liter. 13 10.8 (B.) 13 36.8 M 13, 4O.O M *5 51-2 15 13-8 DISTRIBUTION OF PICRIC Water and Amyl Alcohol. (Herz and Fischer Ber. 37, 4747, '04.) ACID AT 25 BETWEEN: Water and Toluene, (H. and F. Ber. 38. 1142, '05.) Millimols CeHsNgO? per 10 cc. Gms. Cs-HsNgOY per 100 cc. Millimols CeHgNaOr per 10 cc. Gms. CsHaNsOy per loo cc. Aq. Alcohol Aq. Alcohol Aq. Toluene Aq. Toluene Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. 0-0553 0.0930 O .127 O 213 O 075 O.I26 o. 172 0.289 0.0920 0.1850 O .211 .424 O .109 0.230 o. 250 0.527 0.1613 0.4127 O 369 .946 O .163 0.482 o. 374 I .IO4 0.1869 0.5182 .428 I .188 O .244 I .026 o. 559 2-351 0.3161 1.079 O 724 2 473 O 389 2-347 o. 891 0.4471 1.638 I .024 3 753 .496 3-747 I . 137 8.586 0.5624 2.189 I .288 5 .017 .583 5-135 I . 336 11.770 0.6423 2-549 I .472 5 839 DISTRIBUTION OP PICRIC ACID AT 25 BETWEEN: Water and Bromoform. (Herz and Lewy Z. Electrochem. n, 820, '05.) Water and Chloroform. (H. and L.) Millimols CeHsNsO? Gms. CVHjNsCV Millimc Is CoHaNaOr Gms. CoHsNgOr per 10 cc. per IOO CC. per 10 CC. per IOO CC. Aq. Bromoform Aq. Bromoform Aq. Chloroform Aq. Chloroform Layer. Layer. Layer. Layer. Layer. Layer. Layer. Layer. 0.321 0-365 0.736 0-836 0.207 0.254 0-474 0.582 0.401 Q -5*S 0.919 I.lSo 0.329 o-547 0-754 I - 2 53 o-475 - 6 55 1. 088 I.50I 0.488 1.09 1.118 2.498 o-575 0.871 I-3I7 J-995 0.561 1.41 1.285 3-230 0.674 1.14 i-545 2 .6l2 0-588 i-53 1-348 3-505 PILOCARPINE HYDROCHLORIDE C n H 16 N 2 O 2 .HCl, Pilocarpine Ni- trate C n H 16 N 2 O 2 .HNO 3 , and Piperine C 17 H 19 NO 3 in Several Solvents. (U. s. P.) Grams per 100 Grams Solvent. *-! _ A. ft OU1VCLH. i> . C U H 16 N 2 2 .HC1. ( :nH 16 N20 2 .HN( >a. CnHwNoV Water 25 333 25 insoluble Alcohol 25 4-35 1.66 6.66 Alcohol 60 9-09 6.2 22.7 Chloroform 2 5 0.18 . . . 58.8 Ether 25 2.8 PLATINUM ALLOYS 232 SOLUBILITY OF PLATINUM ALLOYS IN NITRIC ACID. (Winkler Z. anal. Ch. 13, 369, '74-) j Alloy. I Pt ^pprox. Grams Alloy Dissolved per 100 Grams HNOs Solution ot in AUoy. i. 39 8Sp.Gr. i.2o8Sp.Gr. i.igoSp.Gr. i.2o8Sp.Gr.: Pt and Silver 10 57 44 6 9 37 11 5 69 57 51 35 tt 2-5 62 61 69 " i 75 70 7 6 Pt and Copper 10 46 27 II 51 " 5 36 34 14 4i " 2-5 5 1 40 30 " i 52 4 1 37 Pt and Lead 10 7 9 8 u 5 8 9 10 u 2-5 22 17 ii It 21 18 23 Pt and Bismuth 10 14 19 4 3 n 5 21 20 6 18 (l 2-5 25 42 8 (l I 49 6 4 10 Pt and Zinc 10 10 II 19 5 " 5 16 12 6 ii " 2-5 16 24 19 " I 20 32 37 PLATINUM BROMIDE PtBr 4 . 100 grams sat. aqueous solution contain 0.41 gram PtBr4 at 20. (Halberstadt Ber. 17, 2962, '84.) PLATINIC POTASSIUM BROMIDE K 2 PtBr 6 . 100 grams sat. aqueous solution contain 2.02 grams K 2 PtBr 6 at 20. (Halberstadt.) PLATINIC DOUBLE CHLORIDES of Ammonium, Caesium, Potas- sium, Rubidium and Thallium. SOLUBILITY IN WATER. (Crookes Chem. News 9, 37, 205, '64; Bunsen Pogg. Ann. 113, 337, *6i.) Grams per 100 Grams Water. o 10 0.024 0.666 (15) 0.050 0.74 0.90 Rb 2 PtCl6. 0.184 0.154 0.0064(15) 20 25 0.079 0.095 I .12 1.26 0.141 0.143 . . . 30 40 O.IIO 0.142 I.4I I. 7 6 0.145 0.166 '.". 50 60 0.177 0.213 2.17 2.64 0.203 0-253 70 80 0.251 0.291 3-79 0-329 0.417 90 100 0.332 1.25 0.377 4-45 0.521 0.634 0.050 233 PLATINIC CHLORIDES SOLUBILITY OF AMMONIUM PLATINIC CHLORIDE AND OF POTASSIUM PLATINIC CHLORIDE IN ALCOHOL AT i5-2o. (Fresenius: Peligot Z. aaal. Ch. 36, 322, '97.) Gms. per Liter Solution. Cms, per Liter Solution. " ' (NHifcPtO* 55% Alcohol 0.150 ... 95% Alcohol 0.0037 0.030 76 " 0.067 0.026 Abs. " ... 0.0082-0.0023 85 " ... 0.180 80 Vol.% Alcohol + 20 Vol. % Ether ... 0.027 90 " ... o. 100 Abs. Methyl Alcohol ... 0.072 PLATINO AMINES. SOLUBILITY IN WATER. (Cleve.) Amine. Formula. S-LJ-TT \ f*i Gms. per ioo Gms. H 2 O. Platino Semi Di Amine Chloride Pt Sp. Gr. of Grams per Liter. Sp. Gr. of Grams per Liter. Solutions. KC1. KC10 3 ". Solutions. KC1. KC10 3 '. 1.050 O 7I.I 1.098 120 24-5 1.050 10 58.0 I.IOS 140 22-5 1.050 20 49.0 I .119 1 60 21 .0 1.054 40 39-5 I.I30 180 20-0 1.064 60 34-o I .140 200 20-0 1-075 80 30.0 1.168 250 20. o 1. 086 100 27.0 SOLUBILITY OF POTASSIUM CHLORATE IN AQUEOUS SOLUTIONS OF POTASSIUM NITRATE. (Arrhenius Z. physik. Chem. n, 397, '93.) Results at 19.85' Mols. per Liter. Grams r^er Liter. Results at 23.87. Mols. per Liter. Grams per Liter. KN0 3 . KC10,/ KNO 3 . KC10 3 KN0 3 . KC10 3 ' KNO 8 . K< O O O 570 o.o 6 9 .88 .0 0.645 o.o 79 .09 O .125 529 12.65 6 4 .86 5 -5 I 5 50.59 63 .14 2 5 492 25.29 60 33 I .0 374 101 .19 45 85 2 -O 328 202.38 40 .22 241 POTASSIUM CHLORATE SOLUBILITY OF POTASSIUM CHLORATE: (Taylor J. Physic. Chem. i, 720, '96- '97; see also Gerardin Ann. chim. phys. [4] 5, 148, '65.) In Aqueous Alcohol. In Aqueous Acetone. Wt. per cent _ A * A?X Alcohol or Gms. KC10 3 per of Acetone 1O Gms - Gr At 40. as. KC1O 3 per 100 Gms. At 30. At 40. Gms. KC1O 3 per Gms. KC1O 3 per 100 Gms. ioo Gms. mSolvent. Solution . Water. Solution. Water. Solution. Water. Solution. Water. o 9-23 IO.I7 12 23 J 3 93 9-23 10.17 II 23 *3-93 5 7.72 8.80 10 .48 12 33 8.32 9-5 6 II .10 13.11 10 6.44 7^5 8 .84 IO 77 7.63* 9.09 10 .28* 12. 60 20 4-51 5-90 6 .40 8 56 6.09 8.10 8 .27 II .26 30 3.21 4-74 4 .67 7 .00 4-93 7.40 6 .69 IO.24 40 2-35 4.00 3 -4T v) ,88 3-90 6.76 5 36 9-45 50 i .64 3-33 2 .41 4 94 2.90 5-98 4 03 8.40 60 I .01 2-53 I .41 2 .69 2.03 5-i7 2 .86 7-35 70 0-54 1.82 O .78 2 63 1.24 4.18 I .68 5.68 80 0.24 I .22 34 I 73 o-57 2.88 79 3-97 90 0.06 O.62 o .12 I , 17 0.18 1.82 O .24 2-45 * Solvent, 9.09 Wt. per cent Acetone. ioo grams glycerine dissolve 3.5 grams KC1O 3 at 15.5. ioo grams sat. solution of KC1O 3 in glycol contain 0.9 gram KC1O 3 . (de Coninck Bui. acad. roy. Belgiquc, 359, '05.) POTASSIUM (Per) CHLORATE KC1O 4 . SOLUBILITY IN WATER AND IN ALCOHOL. (Muir Chem. News, 33, 15, '76; Wenze Z. angew. Ch. 5, 691, '91 .) In Water. (M.) In Alcohol. (W.) to. Gms.KClO 4 per iooGms.H 2 O. Sp. Gr. of Solutions. Wt . per cent Gms . KC1O 4 per Alcohol. ioo Gms. Alcohol. 6 0-7 1.0005 97.2 0.0156 2 5 1.9 I.OI23 95-8 0.020 6-45 1.0181 90.0 0-036 00 20.0 i .0660 POTASSIUM CHLORIDE KC1. SOLUBILITY IN WATER. (Average curve from the results of Meusser Z. anorg. Chem. 44, 79, '05; at 31.25, Kohler 2 Ver. Zuckerind. 47, 447, '97; Andrae J. pr. Chem. [2] 2Q, 456, '84; Gerardin Ann. chim. phy: [4] 5. i37. '65; de Coppet Ibid. [5] 30, 411, '83; Etard Ibid. [7] 2,526, '94; Mulder; above 100, Tilde and Shenstone Proc. Roy. Soc. (Lond.) 35, 345, '83.) A0 Gms. KCl per too Gms. A0 Gms. KCl per ioo Gms. Gms. KCl per ioo Gms. Solution. Water. Solution. Water. ' Solution. Water. -9 19-3 23 9 40 28 .6 4O.O 147 41 5 70.8 -4-5 20. 6 5 29 9 42.6 180 43 7 77-5 o 21.6 27 .6 60 31 3 45-5 Solid Phase Ice 5 22.7 29 3 70 32 .6 48-3 -9 19 3 23-9 10 23-7 3 1 .0 80 33 .8 5 1 - 1 -8 17 7 21 .5 15 24-5 3 2 4 90 35 .1 54-o -8 16 7 20. o 20 25-4 34-o IOO 36 .2 56-7 -7 14 9 I7-S 2 5 26.2 35 5 130 39 .8 66.0 -6 13 .6 15-7 30 27.1 37 .0 -5 5 I2 5 14 3 Sp. Gr. of solution sat. at o = i.iso; at 15 = 1.172. POTASSIUM CHLORIDE 242 SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND AMMONIUM CHLORIDE IN WATER AT 25. (Fock Z. Kryst. Min. 28, 353, '97.) Grams per Liter Solution. KCl. 3II-3 293-3 278.7 273.2 234.6 204-2 157-7 II6.8 123.0 III .O 102.2 53-16 3 J -24 o.oo Grams per Liter Solution. Mol. per cent in Solution. NH 4 C1. KCl. o.oo 100.0 9.41 90.59 15.04 84.96 34.26 65.74 46.59 53-44 5 J - 6 3 48.37 63-56 36-44 73-49 26.51 73-48 26.52 79.10 20.90 82.14 17.86' 87.96 12.04 93-45 6.55 100.00 o.oo Sp. Gr. of Solutions. Mol. per cent in Solid Phase. 1807 1716 1678 *493 1461 i i i i i i i . 1.1326 1.1329 1.1245 I .1212 I .1009 I .O9I2 1.0768 NH4C1. 0-0 1 .21 2 -II 6.18 8.90 J o-53 17.86 60.20 76.88 97-5 1 97-79 98-85 99-33 100.0 KCl. IOO 98.79 97.89 93.82 91 .10 89.47 82.14 39.80 23 -12 2-49 2.21 1*1$ 0.67 o.oo NH4C1. O.OO 22 -8l 35-39 89.17 127.8 147.2 197-3 232-5 244-5 261 .9 259.0 278.6 320.7 273-5 SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND POTASSIUM BROMIDE AT 25. (Fock.) Milligram Mols. Mo i. p^ cent Mo i. _,. cent per Liter. KCl in P KCl in KB7 KCl. Solution. 4686.2 o.o o.o I -3756 4462.7 314.2 6.16 1.3700 4228.5 624.3 12.86 1-3648 3817.8 1108.0 22.49 J-3544 3188.1 1830.7 36.48 1.3320 2727.6 2237.4 45-06 1-3119 1830.2 2868.0 60.30 1.2689 uSi.i 3363.9 74.01 1.2455 291.7 398.8 3911.4 85.22 1-1977 311.3 o.o 4173-1 100.00 1-1756 KBr. 558.1 531-5 503-6 454-6 KCl. O-OO 23-44 46.57 82.62 379.6 136.6 324.8 166.9 213.9 250.9 218.0 140.7 47-5 o.o Solid Phase. O.OO O.OO 8.2 3 15.68 33-66 63-5 1 82.29 88.04 96.98 100.00 SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC ACID AT o. (Jeannel Compt. rend. 103, 381, '86; Engel Ann. chim. phys. [6] 13, 377, '88.) ram Mols. per 10 cc. < Srams per 100 cc. Solution, Sp. Gr. of KCl. HCI: KCl. HCI. Solutions. 34-5 o.o 25-73 O-O I-I59 30.41 3-9 22.69 1.42 I.I52 27-95 6.6 20.84 2.41 I.I50 27-5 7-i 20.51 2-59 I.I47 23-75 ii .1 17.71 4-05 I-I37 16.0 23.0 11 -93 8-39 I. Ill 10. 34-o 7.46 12 .40 I . IO5 7-5 41.0 5 60 T 4-95 I.I05 2.O 65-5 i-49 23.88 I .121 2-4 148.8 (sat.) 1.52 54.26 I .224 TOO cc. saturated HCI solution dissolve 1.9 grams KCl at 17. (Ditte Compt. rend. 92, 142, '86.) 243 POTASSIUM CHLORIDE SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS POTASSIUM HYDROXIDE SOLUTIONS. (Engel Bull. soc. chim. [3] 6, 16, '91; Winteler Z. Electrochem. 7, 360, 'oo.) Resu < Mg. Mols. per 10 cc. Solution Sp. Its at Engel.) Gr. of >lution. 0. Gms. per 100 cc. Solution. Results at (Winteler Gms. per zoo cc. Solution. 20. > Sp. Gr. of Solution. KC1. KOH. KC1. KOH. KCl. KOH." 35-5 O 159 26.83 O o 29 3 I .0 1.185 31.0 2 375 .146 23-44 I 33 21 .1 10 o I. 210 28.3 4 *53 21.39 2 .64 14 .8 2O .0 1.245 23.0 9 9 .172 17-39 5 56 10 4 30 .0 1.295 18.38 15 i ^95 13.89 8 .46 6 .8 40 .0 I -345 *4-43 20 1. 2l6 10.91 ii 2 3 4 .0 50 .0 x -397 n-43 24 .63 1.239 8.64 13 83 2 .2 60 .0 1.450 8.98 29.25 1.261 6-78 16 43 I 4 70 .0 1.500 6.28 35 .13 1.294 4-74 19 72 1 .1 80 .0 J -55o O 9 85 .0 1.580 SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND POTASSIUM IODIDE IN WATER. (Etard Ann. chim. phys. [7] 3, 275, '94.) Grams per too Gms. Solution. Grams per 100 Gms. Solution. ** KCl. KI. & KCl. KI. o 3-7 50-5 100 6.2 61 .0 20 4.2 53-o 140 7-3 63-7 40 4-7 55-3 180 8-3 65-5 60 S- 2 57-5 220 9-4 66 3 80 5-7 59-4 245 10.0 66.5 SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS MAGNESIUM CHLORIDE SOLUTIONS. (Precht and Wittgen Ber. 14, 1667, '81.) Grams KCl per 100 Grams Sat. Solution in: t. 11% Mcrru. MgClo. 21-2% 30% MgClo. McrCl->. 20% MgCl 2 . 10 14 3 9 9 5' \J 1.9 4 .2 KC1+5-7 NaCl 20 15 9 ii 3 6 5 2.6 6 .0 1 +5-9 M 30 17 5 12 7 * ,6 3-4 6 9 " +6.0 u 40 19 .0 14 .2 8 .8 4.2 7 9 " +6.1 M 50 20 5 IS .6 10 .0 5-o 8 9 " +6.3 tt 60 21 9 17 .0 ii .2 5-8 9 9 " +6.4 (I 80 24 5 .5 13 .6 7-3 10 9 " +6.6 11 90 25 .8 2O .8 14 7 8.1 ii 9 " +6.7 tt 100 27 .1 22 .1 15 9 8.9 *3 .0 " +6.9 Ii POTASSIUM CHLORIDE 244 SOLUBILITY OP POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM NITRATE, AND OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF POTASSIUM CHLORIDE, AT SEVERAL TEMPERATURES. (Touren Compt. rend. 130, 908, 'oo; Bodlander Z. physik. Ch. 7, 360, '91; Nicol Phil. Mag. (Lond.) 31, 369, '91; Soch J. Physic. Ch. 2, 46, '98.) KC1 in Aq. KNO 3 Solutions at: 14.5 (T.). KNO. O 20.64 32.18 62.23 82.77 115.9 II9.I 123.4 KCI. 288.3 284.2 282.1 276.8 273-5 270.7 268.3 267.2 I 7-5 (B.). 25-2 (T.). ofctSns Gms. per Liter. Gms. per Liter. 'KN0 3 . KCI". kNo 3 . KCI: .173 o.o 293.9 o.o 311.8 . 198 65.8 275.0 13.76 306.6 .2IO 88-3 273.4 32.18 303.6 .225 124.8 265.3 91.26 293.2 .236 148.3 259.8 122.7 287.2 - 2 39 152.2 259.6 141.4 284.2 239 154.9 259.5 182.7 276.0 .241 153.3 262.4 20, etc. (N.). Gms. per 1000 Gms. H 2 0. KN0 3 . O.OO 56.18 168.54 at 21 225.8 KCI. 345-2 342.15 334-39 341-3 at 80 1175.0 402.0 KNO 3 in Aq. KCI Solutions at: 14-5. Grams per Liter Solution. KCI. O.O 31-63 65.64 132.6 164.4 196.5 236.9 KNO 3 . 225.4 219.8 208.2 185.2 I S9-5 144.0 25-2". Grams per Liter Solution. KCI. KN0 3 . O.O 32C.C 49.22 100.7 J 55-2 207.3 226.8 3 I2 288 -3 .7 254.0 224.4 203.9 196.9 20' Grams per ioooGms.H 2 O. KCI. KN0 3 . " 0.0 82.9 165.8 248.7 310.8 311.1 256.8 221.7 2O2.O 501.6 KNO 3 in Aq. KCI at 20.5 (B.), KCI in Aq. KNO 3 at 20.5 (B.). Gms. per ioo Gms. Solution. Sp. Gr. of ci. KNO,. 0.0 27.68 1.1625 4.72 24-39 .1700 7-74 22.44 J 1765 12.23 20.23 .1895 J 5-i5 18.96 .1983 19.61 17.67 ] .2150 22.17 I7-II .2265 24-96 16 79 1.2400 Gms. per Solu ioo Gms. tion. Sp. Gr. of " 1 *.' KN0 3 . KCI. Solutions. O.O 29-39 .1730 6.58 27.50 .1980 8.88 27-34 .2100 12.48 26-53 .2250 14.83 25.98 .2360 15.22 25-96 .2390 15-49 25-95 .2388 15-33 26.24 : [.2410 245 POTASSIUM CHLORIDE SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND POTASSIUM SULPHATE IN WATER. t. 10 15.8 20 25 30 Gms. per too Gms. H 2 0. KCI 28 33 36 4 .1 K 2 SO. 1.32 2-3 i-43 2-93 Observer. (Precht and Wittgen.) (Kopp.) (P.and W.) (Van't Hoff and Meyerhoffer.) (P. and W.) t e . Gms. per roo Gms. H 2 0. KCI -i - K 2 so;. 40 38.7 1.68 5 41-3 1.82 60 43-8 i-94 80 49.2 2.21 100 54-5 2-53 Observer. (P. and W.) SOLUBILITY OF MIXTURES OF POTASSIUM CHLORIDE AND SODIUM CHLORIDE IN WATER. ( (i) Precht and Wittgen Ber. 14, 1667, '81; at 25 and'at 80, (3) Soch T. Physic. Ch. 2. *6 '08 (2) Etard Ann. chim. phys. [7] 3, 275, '97-) Grams per 100 Grams H 2 O. KCI. NaCl. Grams per 100 Grams H 2 O. KCI. NaCl. * 22.0(1)19.0(2) 27.7(1)32.3(2) 24.6 20.6 27.2 32.8 27-3 32-5 26.8 34.1 30.0(3)25.2(3) 26.4(3)34.0 32.9 28.4 26.1 32.3 34-7 32-3 25.8 30.6 NOTE. Page and Keightly, Rudorff and also Nicol, give single determinations which lie nearer the results of Precht and Wittgen than to those of Etard. o II. 2(1 )n .2(2' > 30, oO [ )3O 0(2) 5 10 12. 5 12.3 29 7 30 5 60 20 14. 7 13 .8 29 .2 3 1 .0 70 25 15.8(3)14 5 29 .0(3)31 3 80 30 17- 2 15 4 28 7 3 1 5 90 40 19. 5 .0 28 .2 9 100 SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OP SODIUM CHLORIDE, AND OF SODIUM CHLORIDE IN AQUEOUS SOLU- TIONS OF POTASSIUM CHLORIDE, AT 20. (Nicol Phil. Mag. (Lond.) 31, 369, '91.) KCI in Aq. NaCl Solutions. Grams per 100 Grams H 2 O. ' NaCl. KCI. O-O 6-5 13.0 34-52 29-37 4-71 .42 NaCl in Aq. KCI Solutions. Grams per 100 Grams H>O. KCI. o.o 4-i4 8.29 12.42 35.91 34-39 32.71 3 I -3 100 gms. 40 per cent by wt. alcohol dissolve 5.87 gms, KCI + 12.25 gms. NaCl at 25. 100 gms. 40 per cent by wt. alcohol dissolve 5.29 gms. KNO 3 + 10.06 gms. KCI at 2 5. ( s ch - j. physk. Ch. 2, 4 6, '98.) 100 gms. abs. ethyl alcohol dissolve 0.034 gm. KCI at 18.5. 100 srrns. abs. methyl alcohol dissolve 0.5 gm. KCI at 18.5. (de Bruyn Z. physik. Ch. 10, 783, '92; Rohland Z. anorg. Ch. 18, 327, '98,) POTASSIUM CHLORIDE 246 SOLUBILITY OP POTASSIUM CHLORIDE IN AQUEOUS ALCOHOL. (Gerardin Ann. chim. phys. [4] 5, 140, '65.) Interpolated from the original results. Grams KCl per 100 Gms. Aq. Alcohol of Sp. Gr.: t. 0.9004 = 5-5 0.9848 9-35 0.9793 = 13.6 0.9726 = 19.1 0.9573 30 0.939 = 40 0.8967 = 60 v 0.8244 = 90 Wt.%. Wt.%. Wt.%. Wt.%. Wt.%. Wt.%. Wt.%. Wt.%. o 23-4 19-5 15-5 "$ 7.0 4.0 i-7 o.o 5 25.0 21 .0 16.8 12.8 8.0 4.8 2 .2 o.o 10 26.4 22.5 18.0 14.0 9.0 5-6 2.7 o.o J 5 26.8 24.0 19.2 15.2 IO-O 6.4 3-i 0.04 20 29.1 25-3 20.3 16.1 10.8 7.2 3-5 0.06 2 5 30-4 26.8 21-5 17.1 n. 6 7-9 3-9 0.08 3 31-7 28.0 22 .6 18.2 12.5 8-5 4.2 O-IO 40 34-3 30-8 24.8 20. o 14.0 9-9 4.8 O.20 5 37-o 33-5 27.0 21.8 15-5 10.8 5- 2 0.30 60 16.8 ii. 8 5-5 O.4O SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS ALCOHOL AT i5- 14.5. (Schiff Liebig's Ann. 118, 365, '61.) (Bodlander Z. physik. Ch. 7, 316, f px-> Sp. Gr. Wt. G. KCl per of per cent 100 cr AQ Sp. Gr. of Sat. Grams per 100 cc. Solution. Alcohol. Alcohol. Alcohol. Solutions. C 2 H 6 OH. H 2 O. KCl. 0.984 10 19.8 I.I720 ... 88.10 29.10 O.972 2O 14.7 I.I542 2.79 85.78 26.85 0.958 30 10-7 I .1365 4.98 84.00 24.67 0.940 40 7.7 I.I075 10.56 79-63 20-56 0.918 50 5.0 I .1085 15-57 75-24 17.24 0.896 60 2.8 1-0545 2O.66 70.52 14.27 o . 848 80 o . 45 i -0455 24.25 67.05 I3-25 Gerardin's results at 15 agree 0.9695 40.42 50.18 6-35 well with the above deter- -93!5 48.73 40.60 3.82 minations. 0.8448 68.63 15-55 0.30 30 and 40. (Bathrick J. Physic. Chem. I, 160, '96.) Wt. per cent Gms. KCl per 100 Gms. Aq. Alcohol. Wt. per cent Gms. KCl per 100 Gn Aq. Alcohol. Alcohol. At 30. At 40. Alcohol. At 30. At 40. O 38.9 41.8 43.1 II. I I3-I 5-28 33-9 35-9 55-9 6.8 8.2 9-43 30.2 33-3 65 9 3-6 4.1 16.9 24.9 27 .6 78.1 i-3 1.6 2 5-i 19.2 21.8 86.2 0.4 o-5 IS -6 17.2 247 POTASSIUM CHLORIDE SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS ACETONE SOLUTIONS. (Snett J. Physic. Ch. 2, 484, '98; at 20, Herz and Knoch Z. anorg. Ch. 41, 317, '04.) Per cent Acetone in KCl At 20. per loo cc. Solution. At 30. Gms. per 100 Gms. Solution. At 40. Gms. per 100 Gms. Solution. At 50. Gms. per 100 Gms. Solution . Solvent. Millimols. Grams. Acetone. KCl. Acetone. KCl. Acetone. KCl. O 410, 5 3- 62 O. O 27.27 O. o 28.69 0.0 30.0 9.1 351 , 7 26. 23 6.96 23.42 6. 79 25-33 . . . . 2O 286 .6 21. 38 16.22 18.90 15- 75 21.28 . . . 30 223. , 7 16. 69 25-45 15.06 two layers 25.67 14.42 40 166. r 12. 42 35-52 11.31 36.03 9-93 50 i*5 4 8. 61 45.98 8.04 a 46.46 7.07 60 7 1 , 2 5. 31 56.91 5-i2 " 57-37 4-38 70 38. 5 2. 87 68.18 2.60 " 68.56 2.22 80 12, 9 0. 96 78.43 0.76 79- 34 0.58 79.25 0.94 9 2 ,0 0. J 5 89.88 0.13 89. 84 o. 16 8i+sat.sol. IOO O ,o o. 100.0 0.00 IOO. 00 0.00 NOTE. For the 20 results the per cent acetone in the solvent is stated in terms of volume per cent, and the concentration of the second solution is 10 per cent instead of 9.1 which is the concentration of the solvent for the corresponding results at the other temperatures. AT THE TEMPERATURE 40 AND FOR CONCENTRATIONS OF ACETONE BETWEEN 20 AND 80 PER CENT THE SATURATED SOLUTION SEPAR- ATES INTO Two LAYERS HAVING THE FOLLOWING COMPOSITIONS: Upper Layer. Grams per 100 Grams Solution. HgO. (CH 3 ) 2 CO. KCl. 55-2 31.82 12.99 53-27 35-44 ii .29 51 .23 48-50 10.27 50.3 + 39-88 9-77 48.O2 43.18 8-79 46.49 45-34 8.17 58.99 25.24 15-77 Lower Layer. Grams per 100 Grams Solution. H 2 0. (CH 3 ) 2 CO. KCl. 28.14 69.42 2-44 30.96 65-97 3-07 32.64 63-79 3-56 34-07 62.01 3-92 37-44 57-67 4.89 38-. 68 56-I7 5-25 23.66 74-91 1-43 zoo cc. sat. solution of potassium chloride in furfurol (C 4 H 3 O.COH) contain 0.085 gm. KCl at 25. (Walden Z. physik. Ch. 55, 7i3,'o6.) POTASSIUM CHLORIDE 248 SOLUBILITY OF POTASSIUM CHLORIDE IN AQUEOUS SOLUTIONS OP GLYCERINE AT 25. (Herz and Knoch Z. anorg. Ch. 45, 267, '05.) Sp. Gr. of Glycerine at 25/4 = I - 2 555- Impurity about 1.5%. Wt. per cent Glycerine in Solvent. KCl per ioo cc. Solution. Sp. Gr. of Solutions. Wt. per cenl Glycerine ii Solvent, KCl per ioo cc. ! Solution Sp. Gr. of Solutions. Millimols. Grams. Millimols. Grams. 424 5 3 1 ,66 I.lSo 54-23 238.5 17.79 I .219 13.28 383 4 28, .61 1.185 83.84 149.0 II. II I 259 25.98 339 3 25 3 1 I.I94 100.00 no. 6 8.25 I .286 45-36 271 4 20 .24 I .211 ioo grams H 2 O dissolve 246.5 grams sugar 4- 44.8 grams KCl at 31.25, or ioo grams of the sat. solution contain 62.28 grams sugar + 11.33 grams KCl. (Kohler Z. Ver. Zuckerind. 47. 447. '97 ) POTASSIUM CHEOMATE K 2 CrO 4 . POTASSIUM (Di) CHEOMATE K 2 Cr 2 O 7 . SOLUBILITY OF EACH IN WATER. (Alluard Compt. rend. 50, 500, '64; Nordenskjold and Lindstrom Pogg. Ann. 136, 314, '69; Etard Ann. chim. phys. [7] 2, 527, '94; Kremers Pogg. Ann. 92, 497, '54; Tilden and Shenstone Phil. Trans. 23, 1884.) Potassium Chromate. Grams per ioo Grams Water. Potassium Di Chromate. o 5 8.2* 59 -3t 60.2$ 10 6o.O 61.2 62.5 20 61.7 63.2 64-5 25 62.5 64.2 64-5 30 63.4 65-2 66.5 40 65 .2 67.0 68.6 50 66.8 69.0 70.6 6 68.6 71.0 72.7 70 70.4 73-o 74-8 80 72.1 75-o 76.9 90 73-9 77.0 79.0 IOO 75-6 79.0 82.2 '25 79.0 15 83.0 Grams per ioo Grams Water. 5* S 7 7 12 12 16 16 20 20 26 27 34 37 43 47 52 58 61 70 70 82 80 97 no 145 H3 205 * Etard. t Alluard. $ N. and L. A., K., T. and S. 249 POTASSIUM CHROMATE SOLUBILITY OF POTASSIUM CHROMATES IN WATER AT 30. (Schreinemaker Z. physik Ch. 55, 83, '06.) Composition in Wt. per cent of: The Solution. The Residue. 'er cent CrO 3 < Per cent KjO. Per cent CrO 3 . Per cent KaO. O 47 o.o 47.16 12.59 47-54 0.1775 34.602 10-93 37-47 I-35 1 26.602 16.482 32.532 20.584 37-I3I 39-922 15-407 19.225 27.966 29.377 20-67 19.17 . . . 19.096 17.30 37 . 64 22 .6l I]C -35 7.88 17-93 3.412 2 C 8<\ 7 .82 43.51 3.01 49-45 9.91 44.46 3-245 53-94 12 .40 46.368 2.823 60.314 12 .935 49-357 2-353 63.044 11.684 53-215 1.360 62.958 8.002 62-55 0.796 67.944 6.731 0.621 70.0 4-0 62.28 o.o . . . . . . Solid Phase. KOH-aHaO K 2 Cr0 4 +K 2 Cr 2 0, K 2 Cr 4 O l3 -hCrO, CrO 3 ioo gms. sat. solution in glycol C 2 H 4 (OH) 2 .H 2 O contain 1.7 gms. K 2 CrO 4 at 15.4. ioo gms. sat. solution in glycol C 2 H 4 (OH) 2 .H 2 O contain 6.0 gms. K 2 Cr 2 O 7 at 14.6. (d e Coninck Bull. acad. roy. Belgique, 25?. '05.) POTASSIUM CITRATE C 3 H 4 (OH)(COOK) 3 .H 2 O. SOLUBILITY IN WATER AND IN SATURATED SUGAR SOLUTION AT 31.25. (Kohler Z. Ver. Zuckerind. 47, 447, '97.) ioo gms. H 2 O dissolve 169.7 gms. C 6 H 5 O 7 K 3 , or ioo gms. sat. solu- tion contain 61.11 gms. ioo gms. H 2 O dissolve 198.3 gms. C 6 H 5 O 7 K 3 4- 303.9 gms. sugar, or ioo gms. sat. solution contain 32.83 gms. C 6 H 5 O 7 K 3 4- 50.3 gms. sugar. POTASSIUM CYANATE KCNO. SOLUBILITY IN ALCOHOLIC MIXTURES. (Erdmann Ber. 26, 2439, '93.) o _. _ t Grams KCNO per 3olvent - Liter Solvent at bYpt. 80 per cent Alcohol + 20 per cent Water 62 80 per cent Alcohol +20 per cent Methyl Alcohol 76 80 per cent Alcohol + 10 per cent Acetone 82 POTASSIUM CYANIDE KCN. ioo gms. H 2 O dissolve 122.2 gms. KCN, or ioo gms. sat. solution contain 55.0 gms. KCN at 103.3. (Griffiths.) ioo gms. abs. ethyl alcohol dissolve 0.87 gm. KCN at 19.5. ioo gms. abs. methyl alcohol dissolve 4.91 gms. KCN at 19.5. (de Bruyn Z. physik, Ch. 10, 783, '93.) ioo gms. glycerine dissolve 32 gms. KCN at 15.5. POTASSIUM CYANIDES 250 POTASSIUM OHROMOCYANIDE K 3 Cr(CN) 6 . 100 gms. H 2 O dissolve 32.33 gms. K 3 Cr(CN) 6 at 20. (Moissan Ann. chim. phys. [6] 4, 136, '85; Christensen J. pr. Ch. [2] 31, i66,'3s.) POTASSIUM OHROMISULPHOCYANIDE K 2 Cr(SCN) 6 . 4 H 2 O. 100 gms. H 3 O dissolve 139 gms. salt. (Karsten Ann. Suppl. 3, 170.) POTASSIUM CARBONYL FERROOYANIDE K 3 FeCO(CN) 5 . 3 m,O. 100 gms. H 2 O dissolve 148 gms. salt at 16. (Muller Com pt. rend. 104, 992, '87.) POTASSIUM FERRICYANIDE K 3 Fe(CN) 6 . POTASSIUM FERROCYANIDE K 4 Fe(CN) 6 . 3 H 2 O. SOLUBILITY OF EACH IN WATER. (Wallace J. Ch. Soc. 7. 8, '85 ; Etard Ann. chim. phys. [7] 2, 526, '94; Schiff Liebig's Ann. H3t 35 '60; Michel and Krafft Ann. chim. phys. [3] 41, 478, '58; Thomsen.) NOTE. The available determinations fall very irregularly when plotted on cross- section paper, and the following figures, which are averages, are therefore hardly more than rough approximations to the true amounts. The figures under K 4 Fe(CN) 6 show the limits between which the correct values probably lie. Grams per 100 Gms. H2O. Grams per TOO Gms. HuO. K3Fe(CN) 6 . K 4 Fe(CN) 6 . KaFe(CN) 6 . o 31 13 ... 40 60 38 70 10 36 20 20 60 66 52 83 20 43 25 40 80 ... 66 89 25 46 28 48 100 ... 76 91 30 50 32 57 104.4 82.6 POTASSIUM FLUORIDE KF.2H 2 O. 100 gms. H 2 O dissolve 92.3 gms. KF, or 100 gms. sat. solution contain 48 gms. KF at 18. Sp. Gr. of solution =1.502. (Mylius and Funk Ber. 30, 1718, '97.) SOLUBILITY OF POTASSIUM FLUORIDE IN HYDROFLUORIC ACID AT 21. (Ditte Compt. rend. 123, 1282, '96.) Gms. per 100 Gms. H^O. Gms. per 100 Gms. HoO. Gms. per TOO Gms. H2O. HF. KF. o.o 96.3 I. 21 72.0 1.61 61 .o 3-73 40-4 4-03 32.5 6.05 30.4 HF. KF. HF. KF. 9-25 29.9 20.68 38.4 11.36 29.6 28.60 46.9 12 .50 30-5 41.98 61.8 13 ,95 53-71 74.8 15.98 33-4 74-20 105.0 17.69 35 - 62 119.20 169.5 25 1 POTASSIUM FORMATE HCOOK. POTASSIUM FORMATE SOLUBILITY OF POTASSIUM FORMATE AND OF THE ACID SALT IN WATER. (Groschuff Ber. 36, 1785, 1903.) Solid Phase : HCOOK Solid Phase : HCOOK. HCOOH. Gms. HCOOK t. per ioo Gms. Mols. HCOOK per ioo Mols. Gms. HCOOK Gms. .HCOOH HCOOK t . per ioo per ioo t . Gms. Gms. Gms, HCOOK per ioo Gms Mols. HCOOH Solution. H 2 0. Solution. Solution. Solution . HCOOK. 20 7 2.8 57 4 O 60.4 39 o o 36 3 3-21 + 18 76.8 o 25 69.8 45 .1 19-5 38 .2 2 .96 50 80.7 89 .8 50 79.2 5 1 .2 39-3 40 .8 2.65 90 86.8 141 .0 80 90.7 58 .6 60 44 .0 2-33 1 2O 92.0 247 .0 70 45 9 2 .l6 140 96.0 90 S 2 .1 1.68 n;7 IOO.O 00 Sp. Gr. of sat. sol. at 18= 1.573. NOTE. Since the acid salt is less soluble at ordinary temperatures than the neutral salt, it can be precipitated from the solution of the neutral salt by addition of aqueous formic acid. Proceeding in this way an impure product is obtained, giving solubility values (expressed in HCOOK) as shown in the last three columns above. POTASSIUM FLUOGERMANATE K 2 GeF 6 . SOLUBILITY IN WATER. (Winkler; Kruss and Nilson Ber. 20, 1696, '87.) ioo gms. H 2 O dissolve 173.98 gms.ICGeF 6 at 18, and 34.07 gms. at 100 (W. ). ioo gms. H.,O dissolve 184.61 gms. K 2 GeF e at 18, and 38. 76 gms. at 100 (K. and N.). POTASSIUM HYDROXIDE KOH. SOLUBILITY IN WATER. (Pickering J. Ch. Soc. 63, 908, '93; at 15, Ferchland Z. anorg. Ch. 30, 133, '02.) Solid Phase. KOH. 2 H 2 t fl Gms. KOH ', per ioo Gms. Solid T>U^. Gms. KOH t o. per ioo Gm?. Water. Solution. Water. Solution. 22 3 7 3 .6 Ice 15 107 5 1 7 20 ,7 22 5 18 4 " 20 112 S 2 .8 -65 2 44 5 3 .8 30 126 55 .76 -36 .2 36 .2 26 .6 KOH. 4 H 2 O 32-5 135 57 44 -32 7 77 94 43 .8 50 I4O 58 33 -33 80 44 4 KOH^HizO+KOH.aHjjO IOO I 7 8 64 03 -23 2 85 45 9 KOH. 2 H 2 O 125 213 68 .06 o 97 49 .2 " 143 3 11 7 75 73 10 I0 3 50 7 < KOH.2H; [20 + KOH-HzO KOH.H 2 Sp. Gr. of sat. solution at 15 = 1.5355. POTASSIUM IODATE 252 POTASSIUM IODATE KIO 3 . SOLUBILITY IN WATER. (Kremers Pogg. Ann. 97, 5. '56; at 30, Meerburg Ch. Weekbl. I, 474, '04.) t 20 30 40 60 80 100 Cms. KIO 3 per 100 gms. H 2 O 4.73 8.13 11.73 I2 -8 18.5 24.8 32.2 100 gms. H 2 O dissolve 1.3 gms. potassium hydrogen iodate(KH(IO s ) 2 at 15, and 5.4 gms. at 17. (Serullas - Ann. chim. phys. 22, 118.) ioo gms. H 2 O dissolve 4.0 gms. potassium di hydrogen iodate KH 2 (IO 3 ) 2 at 1 5. (Meineke Liebig's Ann. 261. 360, '91 ,) POTASSIUM IODIDE KI. SOLUBILITY IN WATER. (Mulder; de Coppet-j- Ann. chim. phys. [5] 30, 417, '83; Etard Ibid. [7] 2. 526, '94; Meusser Z. anorg. Ch. 44, 80, '05; see also Tilden and Shenstone Phil. Trans. 23, J 84; Schreinemaker Z. physik. Chem. 9, 71, '92.) Gms. KI per ioo Gms. Gms. KI per ioo Gms. Water. Solution. *- Water. Solution. -io 115.1 53.5 80 192 65.8 - 5 119.8 54.5 90 200 66.7 - I 122.2 55.0 IOO 208 67 5 o 127.5 5 6 - no 215 68 3 10 136 57.6 120 223 69 O 20 144 59.0 25 148 59.7 Ice Curve 30 152 60.3 - 5 25.7 22 5 40 160 61.5 7 42.6 29.9 50 168 62.7 - 9.5 51.5 34.0 60 176 63.7 -H-5 6 4-7 39-3 70 184 64.8 14 75-8 4 2 7 SOLUBILITY OF POTASSIUM IODIDE IN ABSOLUTE ALCOHOLS. (de Bruyn Z. physik. Ch. io, 783, '92; Rohland Z. anorg. Ch. 18, 327, '98.) ioo gms. methyl alcohol dissolve 16.5 gms. KI at 20.5. ioo gms. ethyl alcohol dissolve 1.75 gms. KI at 20.5. ioo gms. propyl alcohol dissolve 0.46 gm. KI at i5-2o (R.) SOLUBILITY OF POTASSIUM IODIDE IN: Ethyl Alcohol of 0.9496 Sp. Gr. Aqueous Ethyl Alcohol at 1 8. f ~ Gms. KI per Sp. Gr. Weight Gms. KI Sp. Gr. Weight Gms. KI t 8 . IOO Gms. Alcohol of Alcohol. per cent Alcohol. per ioo Gms. Alcohol. of Alcohol. per cent per ioo Gms Alcohol. Alcohol. 8 67.4 0.9904 5- 2 I30-5 0.9390 45 66.4 13 69.2 0-9851 9-8 119.4 0.9088 59 48-2 2 5 75- 1 0.9726 23.0 IOO. I 0.8464 86 11.4 46 84.7 0.9665 29.0 89.9 0.8322 91 6.2 55 87-5 0.9528 38.0 76.9 62 90.2 (Gerardin Ann. chim. phys. [4] 5, 155, '65.) 253 POTASSIUM IODIDE SOLUBILITY OF POTASSIUM IODIDE IN ACETONE AND IN PYRIDINE. (von Laszcynski Ber. 27, 2285, '94; at 25, Krug and McElroy J. Anal. Ch. 6, 184,, '92.) Solvent. Gms. KI per 100 Gms. Solvent at: -2.5. 10. 22. 25. 56. 119. Acetone 3-08 ... 2.38 2.93 1.21 Pyridine ... 0.26 ... ... ... o-ii 100 gms. glycerine dissolve 40 gms. KI at 15.5. SOLUBILITY OF POTASSIUM IODIDE IN SEVERAL SOLVENTS. (Walden Z. physik. Ch. 55, 714, '06.) Solvent . Formula t |P- G .r. of Gms. KI per too ' Solution. cc. Solution. Gms. Solution . Water H 2 O O I . 6699 94 5 56.32 Water H 2 25 L7254 102 .70 59-54 Methyl Alcohol CH 3 OH o 0.8964 II .6l I2 .95 Methyl Alcohol CH 3 OH 25 0.9003 13 5-14.3 14.97 Ethyl Alcohol C 2 H 5 OH o 0.8085 I .197 1.479 Ethyl Alcohol C 2 H 5 OH 25 o. 7908 I .520 1.922 Glycol (CH 2 OH) 2 o 1.3954 43 .28 31-03 Glycol (CH 2 OH) 2 25 1.3888 47 23 33-oi Acetonitril CH 3 CN o 0.8198 1.852 2-259 Acetonitril CH 3 CN 25 0.7938 I 57 2.003 Propionitril C 2 H 5 CN o 0.8005 o 34-0.41 0.0429 Propionitril C 2 H 5 CN 25 0.7821 .32-0.36 0.0404 Benzonitril C 6 H 5 CN 25 I . 0076 o .051 0.0506 Nitro Methane CH 3 NO 2 o 1.1627 .314-0.366 0-315 Nitro Methane CH 3 N0 2 25 1.1367 o 289-0.349 0.307 Nitro Benzene C 6 H 5 N0 2 25 .0019 Acetone (CH 3 ) 2 CO o 0.8227 I 732 2.105 Acetone (CH 3 ) 2 CO 25 o. 7968 I .038 1.302 Furfural C 4 H 3 O.COH . . . 15 .10 . . . Furfural C 4 H 3 O.COH 25 .2014 5 93 4.94 Benzaldehyde C 6 H 6 COH 25 .0446 343 0.328 Salicyl aldehyde C 6 H 4 .OH.COH .1501 I 257 1.093 Salicyl aldehyde C 6 H 4 .OH.COH 25 1373 549 0.483 Anis aldehyde C 6 H 4 .OCH 3 .COH .1223 I .520 1-355 Anis aldehyde C 6 H 4 .OCH 3 .COH 25 .1180 .720 0.644 Ethyl Acetate CH 3 COOC 2 H 5 25 o .0013 Methyl Cyan Acetate CH 2 CNCOOCH 3 .1521 3.256 2.827 Methyl Cyan Acetate CH 2 CNCOOCH 3 25 .1358 2 459 2.165 Ethyl Cyan Acetate CH 2 CNCOOC 2 H a 25 .0628 O .989 0.930 POTASSIUM NITRITE 254 POTASSIUM NITRITE KNO 2 . 100 gms. H 2 O dissolve about 300 gms. KNO 2 at 15.5. (Divers J. Ch. Soc. 75. 86, '99-) POTASSIUM NITRATE KNO,. SOLUBILITY IN WATER. (Mulder; Andrae J. pr. Ch. [2] 29, 456, '84; Gerardin Ann. chim. phys. [4] 5, 150, '65; Etard Ibid. [7] 2, 526, '94; Ost J.pr. Ch-feTi?, 233, '78; at 31-25. Kohler Z. Ver. Zuckerind. 47, 447, '97; Euler Z. physik. Ch-49, 315, '04; Tilden and Shenstone Phil. Trans. 23, '84;Berkeley Trans. Roy. Soc. 203 A, 213, '04.) Average Curve. Gms. KNOa per ioo Gms. Gms.KNO 3 per TOO Gms. Water. Solution. Water. Solution. o 13-3 11.7 70 138 58.0 10 20.9 17.3 80 169 62.8 20 31.6 24.0 00 202 66.9 25 37.3 27.2 ioo 246 71.1 30 45-8 3 x -4 no 300 75.0 40 63.9 39.0 120 394 79.8 50 85.5 44.0 125 493 83.1 60 no.o 52.0 SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND BARIUM NITRATE IN WATER. (Euler Z. physik. Ch. 49, 313, '04.) t. Sp. Gr. of Sat. Solution. Grams per ioo Grams HaO. 17 1. 120 i3.26KNO 3 + 6.31 Ba(NO 3 ) 2 21.5 ... 17.00 " + 7.58 30 1.191 24.04 " 4- 9-99 " 50 49-34 +18.09 SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF NITRIC ACID AT o. (Engel Compt. rend. 104, 913, '87.) Sp. Gr. of Equivalents per 10 cc. Solution. Grams per ioo cc. Solution. Solutions* 1.079 i2.5KNO 3 o HNO 3 i2.65KNO 3 o.ooHNO 8 9.9 " 5-87 10.02 " 3-7 1 " 1.093 8.28 " 13-2 8. 3 8 " 8.38 tt 1.117 7-4 " 2i-55 7-49 13-58 Is 1.144 7-4 31.1 " 7-49 " 19.47 H i .202 7.6 48.0 7.68 " 30.04 M 1.289 10.3 " 68.0 10.42 " 42.86 M 1.498 28.3 " 120.5 " 28.64 " 75-95 M 255 POTASSIUM NITRATE SOLUBILITY OF POTASSIUM NITRATE AND OF ACID POTASSIUM NITRATES IN NITRIC ACID. (Groschuff Ber. 37, 1490, '04.) NOTE. - Determinations made by the so-called thermometric method, i.e., by observing the temperature of the disappearance of the separated, finely divided solid from solutions of known concen- tration. Grams per 100 Gms. Gms. per 100 Gms. t . Solution. Solid Phase. t . Solution. Solid T>Un KNO 3 . HN0 3 . KNO 3 . HN0 3 . .rnase. - 6 24.4 75-41 KN0 3 . 2 HNO 8 (i) 22-5 47-2 52-93 KNO 3 .HNO 3 + 14 32-6 67.42 (stabil) 47-8 52.11 " (stabil) 17 34-8 65.04 44 25-5 48.6 51.46 " 19 5 37-2 62 .90 44 27.0 49-4 50.78 44 22 44-5 55-46 44 29.0 50.1 49-94 KN0 3 .HN0 3 21 5 47-8 52.11 KN0 3 . 2 HN0 3 (2) 30-5 5-9 49-15 (labil) 21 5 48.6 51.46 (labil) 21 .O 49-4 50.78 KNO 8 (labil) 20 50-9 49-15 44 39-o 5 -9 49-15 " (stabil) - 4 37-2 62.81 KNO 3 .HNO 8 5o 51 .7 48-32 -16 5 44-5 55-46 (labil) C> Solution in HNOs. (') Solution in KNO 3 . CONDUCT OF ACID POTASSIUM NITRATE TOWARDS WATER. Gms. per 100 Gms. t. Solution. Solid Phase. Gms. per 100 Gms. t_ Solution. Solid Phase. KN0 3 . HN0 3 . KN0 3 . HN0 3 . 22 44-5 55-5 KNO 3 .2HNO 8 50 38.7 48.3 KNOj 20 5 44-i 55-o 44 61 36.0 44 .8 44 18 43-8 54-5 41 63 34-5 43 - 44 12 43 - 53-6 60.5 30.9 39-5 41 6 42-3 52-7 44 56 27 .6 34-4 44 41 .6 51-8 44 43 20.8 25-9 44 J 2 4i-3 51 .4 KNO 3 17 ii. 7 16.6 44 22 40.9 51-0 44 -5 5-54 6.91 44 40 39-9 49-8 44 SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND POTASSIUM CHLORIDE IN WATER. (Etard Ann. chim. phys. [7] 3, 283, '94; at 20, Riidorff Ber. 6, 482, '73; Nicol Phil. Mag. [5] 31, 385, '91.) Gms. per 100 Gms. t. Solution. Gms. per 100 Gms. t. Solution. Gms. per 100 Gms. t. Solution. KN0 3 . KCl. KN0 3 . KCl. KN0 3 . KCl. O 5-o 2O O 30 16 .0 21 .2 70 39-5 17-5 10 8.0 2O .8 40 21 -0 21 80 45-5 15-8 20 12.6 21 .2 50 27 20 O 100 57-5 ii. 6 25 14-0 21 3 60 33 5 19 O 120 69.0 7-7 POTASSIUM NITRATE 256 SOLUBILITY OP POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF: (Touren Compt. rend. 131, 259, 'oo.) Potassium Carbonate. Potassium Bi Carbonate. Results at 14.5. Results at 14.5. Mols. per Liter. Gms. per Liter. Mols. per Liter. Grams per Liter. KaCO,. KN0 3 . KjC0 3 . KJ\0 3 . KHC0 3 . KN0 3 . KHCOs. KN0 3 . o.o 2 .228 o o 225 O 2 33 0.0 236 0-48 I 85 66 4 188 39 2 i7 39-o 22O I - 2 5 I 39 172 9 141 O .76 2 03 76.0 205 2.58 .86 356 9 87 I .16 I .92 116 194 3-94 .64 544 9 65 I 55 I .81 J 55 I8 3 Results at 35. Results at 35. o.o 3 .217 o o 326 o .0 3 .28 o.o 332 o-59 2 .62 81 .6 265 .89 2 .84 8 9 287 i-35 I 97 186 7 199 I 33 2 65 J 33 268 2 .IO I .46 290 5 148 I .91 2 45 191 249 2.70 I .14 373 .6 "5 3-58 0.79 495 .1 80 SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND POTASSIUM SULPHATE IN WATER. (Euler Z. physik. Ch. 49, 313, '04.) t". Sp. Gr. of Sat. Solution. Grams per 100 Grams Water. 15 1.165 24.12 KNO 3 " 5.65K 2 SO 4 20 ... 30.10 " 5.58 " 25 I. 210 3 6.12 5.58 SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND SODIUM CHLORIDE IN WATER. (Etard Ann. chim. phys. [7] 3, 283, '94; agree well with those of Etard.) Gms. per 100 Gms. t. Solution. t t the older determinations of Riidorff, Karsten, Mulder, etc, Gms. per 100 Gms. Gms. per 100 Gms. Solution. t. Solution. KNOs. NaCl KN0 3 . NaCl.' KN0 3 . NaCl. O 13 24 40 30-5 19 120 73 8 .0 10 16 23 5o 36 17 140 77 7 .0 20 20 22 00 42-5 15 160 79 5 6 .0 25 23 21 5 80 55 12 170 80 5 c 5 30 25 20 5 100 67 9-5 SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM NITRATE AND VICE VERSA AT 20. (Carnelly and Thomson J. Ch. Soc. 53, 782, '88; Nicol Phil. Mag. 31, 369, '91.) KNO a in Aq. NaNO 3 Solutions. NaNO 3 in Aq. KNO 3 Solutions. Grams per TOO Grams HgO. Grams per 100 Grams I^O. NaN0 3 . KN0 3 " KNO 3 . " NaNOa. " o 31.6 o 88 10 30 .5 10 90 20 31 .0 20 92 40 33-o 25 93 60 35.5 30 94 80 41-0 35 96 257 POTASSIUM NITRATE SOLUBILITY OF MIXTURES OF POTASSIUM NITRATE AND SILVER NITRATE IN WATER. (Etard Ann. chim. phys. [7] 3, 283, '94.) Gms. per 100 Gms. Sol. A Gms. per 100 Gms. Sol. t . Gms. per 100 Gms.S t . KN0 3 . AgNOa. KN0 3 - AgNO 3 . ' KNO 3 . AgN0 3 . *3-5 43 O 30 26 .8 49 4 80 36.2 55-i 10 IQ.O 44 7 40 29 .6 51 5 100 38.3 55-3 20 23.0 47 .0 SO 3 2 .0 54 .0 120 4O.O 55-6 2 5 25.0 48 .0 60 33 5 54 .8 I4O 41-5 55-8 SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM NITRATE AND SILVER NITRATE IN WATER AT 25. (Herz Inaug. Diss. (Berlin) '05; Calc. by Fock Z. Kryst. Min. 28, 405, '97.) Grams per Liter. Mg. Mols. per Liter. Mol. per cent AgNO 3 in Solution. Mol. per cei AgN0 3 in Solid Phas, AgN0 3 . KNO 3 . AgN0 3 . KNO 3 . 45-9 321.8 270 3 l8o 7-83 0-2896 IIO-7 322.6 65!-3 3^4 16.96 o . 6006 176.8 333-7 IO4O 3298 23-97 o 9040 259.6 364.0 1528 3597 29.81 1.054 365-6 456-4 2151 45 11 32 .28 I .604 57-9 387.2 2988 3816 43^5 2-439 745-9 398.6 4388 3960 52.70 8.294 SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM NITRATE AND THAL- LIUM NITRATE IN WATER AT 25. (Fock.) Grams per Liter. Mg. Mols. per Liter. Mol. per cent T1NO 3 Sp. Gr. of Mol. per cent T1NO TlNOg. KNO 3 . T1N0 3 . KN0 3 . in Solution. Solutions, in Solid Phas;. O-OO 35 I -o o.o 3468.2 o.oo I .2632 O-OO 2-37 329.0 8. 9 325I-5 0-43 1.1903 0.08 6.15 332-4 23.1 3285.1 0.70 1.1956 O.2O 17.64 333-7 66.3 3298.1 1.97 I .2050 o-57 49-74 333-3 186.9 3294.4 5-37 I .2196 1.78 63.60 321.0 239.0 3172.4 7.01 1.2436 2.19 86.18 330-5 323 .8 3265-8 9.02 I .2617 2-77 123.8 428.3 465.2 4232.6 9.90 1.2950 {6.00 27.04 101 .3 245.1 380.6 2423-3 I3-58 I .2050 93-33 116.1 O-O 463.1 o.o IOO. 00 I .0964 100.00 SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL SOLUTIONS (Gerardin Ann. chim. phys. [4] 5, 151, '65.) Grams KNO 3 per 100 Grams Aqueous Alcohol of Sp. Gr.: t . 0.9904 0.9843 0.9793 0.9726 09571 0-939 0.8967 0.8429 w\ 5 %. Wt'f. = 13.6 Wt.%. = 19.1 Wt.%. =30 Wt.%. = 40 Wt.%. = 60 Wt.%. =90 Wt.%. IO 17 13 10 7 4-5 3 I O-2 18 22-5 18.5 14-5 10 6.2 4-5 1.6 o-3 20 24 20 16 ii 7.0 5 2 o-3 25 29 24-5 20 13 .5 9.0 6-5 2-5 0.4 30 36 30 25 17 8 o-5 40 52 43 36 27 ll'.s ii 4 0.6 50 72 61 38 23.0 16 6 o-7 60 93 79 69 5 2 31.0 21 8 i .1 POTASSIUM NITRATE 258 SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL AT 18, (Bodlander Z. physik. Ch. 7, 316, '91.) Sp. Gr. of Gms. per 100 re. Solution. gp .. Gr. of Gms. per IOCD cc. Solution. Solution. C 2 H 6 OH. H 2 O. KN0 3 . alution. C 2 H 6 OH. H 2 O. KN0 3 . I .1480 89.80 2 5 O i .0120 23 33 69.81 8.06 1.1085 3 3o 87-44 2O .11 9935 28 . ii 64-74 6.50 I .IOIO 5 .24 86.26 18 .60 9585 37 53 54-21 4-II 1.0805 8 .69 83.18 16 .18 O 9450 42 .98 48.15 3-37 I -755 9 .06 83.10 IS 39 O .9050 5 1 23 27-32 i-95 1-0655 14 .08 77-93 14 54 O .8722 61 65 24.74 0.83 i .0490 16 .27 76.36 12 .27 8375 69 .60 13-95 0.20 1-0375 *9 97 72.93 10 85 SOLUBILITY OF POTASSIUM NITRATE IN AQUEOUS ALCOHOL AND IN AQUEOUS ACETONE. (Bathrick J. Physic. Ch. i, 160, '96.) In Aqueous Alcohol. In Aqueous Acetone at 40. Wt. per cent Gms. KNO 3 per 100 Gms. Aq. Alcohol. Wt. per cent Gms ' Alcohol. At3Q o At4QO> Acetone. ^Solvent. o 45-6 64.5 o 64.5 8-25 32.3 47.1 8.5 51.3 17.0 22.4 33.3 16.8 38.9 25.7 15.1 24.1 25.2 22.8 35-0 11.4(34.4) 16-7 34.3 24-7 44.9 7.0 11.6(44) 44-i i7-o 54-3 4-5 7-2(55) 53-9 "-9 65.0 2.7 4.4 64.8 7.2 75-6 i-3 2.0(76.3) 76.0 3.0 88.0 0.4 0.6(88.5) 87.6 0.7 100 grams H 2 O saturated with sugar and KNO 3 dissolve 224.7 gms. sugar + 41 .9 gms. KNO 3 , or 100 gms. of the saturated solution contain 61.36 gms. sugar + 11.45 g ms - KNOa at 31.25. (Kohler Z. Ver Zuckerind. 47, 447, '97.) POTASSIUM OXALATE K 2 C 2 O 4 . 4 H 2 O. SOLUBILITY OF MIXTURES OF POTASSIUM OXALATE AND OXALIC ACID IN WATER AT 25. (Foote and Andrew Am. Ch. J. 34, 155, '05.) Gms. per 100 Gms. Solution. Mols. per too Mols. H 2 O. ' n-,^ " -F7T ' wr n " v r n Solid Phase. xl 2 C 2 (J 4 . Jv 2 C 2 U 4 . rl 2 L. 2 (J 4 . JV2C 2 (J 4 . 10.2 2.274 H2C 2 4 . 2 H 2 10.31 O.O4 2. 302 O- CO5 H 2 C 2 O 4 . 2 H 2 O + H 3 K(C 2 O 4 ) 2 .2H 2 O 9.26 O-I3 2.O46 O-Ol6 ) ~ ,, lTTT^//-/-,\ TT/-V J } Double salt H 3 K(C 2 O 4 ) 2 -2H 2 O 3-39 0.63 0.707 0.071 i 2 . 06 4.26 O 440 O 495 H 3 K(C 2 O 4 ) .2H 2 O + HKC 2 O 4 1.16 ii. so 0.266 1-427 I _ , ' I Double salt HKC 2 O 4 0.99 16.93 0.240 2.235 ' 0.85 2 1. 08 0-221 2.928 HKC 2 4 +H 2 K 4 (C 2 4 ) 3 . 2 H 2 O.82 21-49 O-2II 2.998 "j O 64 23.52 O . 169 3 36l f Double salt H 2 K 4 (C 2 O 4 ) 3 .2H 2 O 0-57 24.88 0.153 3-6I7 j 0.43 27.52 0-122 4-14 H 2 K 4 (C 2 O 4 ) 3 .2H 2 O + K 2 C 2 O 4 .H 2 O 27 -40 ... 4.09 K 2 C 2 4 .H 2 259 POTASSIUM OXALATE SOLUBILITY OF POTASSIUM OXALATE AND ACID POTASSIUM OXALATE IN WATER. (Alluard; results at o, Engel Ann. chim. phys. [6] 13, 362, '88.) ioo gms. H 2 O dissolve 25.24 gms. K 2 C 2 O 4 , or 100 gms. of sat. solu- tion contain 20.62 gms. K 2 C 2 O 4 at o. Sp. Gr. of solution = 1.161. Acid Oxalate in Solutions of Neutral Oxalate at o. Acid Oxalate in Water n H 2 SO 4 Corre- n KOH Corre- Q ^ r, ~t Gms. per Gms. KHC 2 O 4 sponding to K spending to Free ^imiVinT I0 C 9 - ^'- t. per ioo Gms. T T /~\ K 2 C2O 4 . H 2 C 2 4 . H 2 O. 28 5 4 1.164 23 53 18 o 2 2 10 .8 O 925 8 9i O 41 IO 3 I 6 .8 I 075 .042 5 61 O 48 20 5 2 4 78 I 25 .031 3 94 o 56 40 10 5 3 83 I .025 3 16 o 65 60 20 5 3 35 I 53 .022 2 76 o 68 80 34 7 2 .6 (i) I 85 .018 2 !5 o 83 IOO 2 o (2) 2 .25 1.007 I 65 I oo 45(3) I .25 1.004 37 56 (i) Sat. with acid potassium oxalate. (2) Sat. with both acid oxalate and tetroxalate. (3) Sat. with tetroxalate. POTASSIUM PERMANGANATE KMnO 4 . SOLUBILITY IN WATER. (Baxter, Boylston, and Hubbard J. Am. Ch. Soc. 28, 1343, >o6 Patterson Ibid, 28, 1735, '06.) Grams KMnO 4 per ioo : Grams KMnO 4 per ioo : Gms. Solution . Gms. H 2 O . cc. Solution (P). Gms. Solution. Gms. H 2 O. 2-75 2.83 2.84 34-8 9.64 10.6; 9-8 4-13 4.31 . . . 40 ii. 16 12.56 15.0 . . . . . . 5-22 45 12.73 14.58 19.8 5-96 6-34 5o 14-45 16.89 24.8 7.06 7 59 . . . 55 16.20 r 9-33 29.8 8.28 9-03 8.69 65 20-02 25-03 Sp. Gr. of saturated solution at 15 = 1-035. SOLUBILITY OF POTASSIUM PERMANGANATE IN: Water. Aqueous Acetone Solutions at 1 3. (Voerman Chem. Centrb. 77, I, 125, '06.) (Herz and Knoch Z. anorg. Ch. 41, 317 '04.) t Gms. KMnO 4 per ioo Gms. Solid cc. Acetone KMnO 4 per ioo cc. per ioo cc. Solution. Solution. Water. Solvent. Millimols. Grams. .18 o 58 .58 Ice O I 4 8 5 4 .70 27 o 99 I .01 10 162 .2 5 13 .48 I .98 2 O2 " 20 177 3 5 .61 58 2 .91 3 00 Ice + KMnO 4 30 208 .2 6 59 -f 10 o 4 OI 4 22 KMnO 4 40 257 4 8 .14 *5 4 95 5 .20 " 50 28 9 7 9 .16 25 7 .00 7 53 60 316 .8 10 .02 40 10 .40 ii .61 70 328 .0 IO 38 So 14 35 16 75 80 312 5 9 .89 90 227.0 7 .18 IOO 6 7 .0 a .14 POTASSIUM PERMAN- 260 GANATE SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM PERMANGANATE AND POTASSIUM PERCHLORATE AT 7. (Muthmann and Kuntze Z. Kryst. Min. 23, 368, '94; recalculated by Fock Ibid. 28, 402, '97.) Milligram Mols. per Liter. Grams per Liter. KMn0 4 . KC10 3 . KMnO 4 . KC1O 4 . " Crystals of Solid Phase. o.o 63.91 o.oo 8.86 o.oo 29.37 54.48 4.65 7.55 2.84 67-73 42-75 10.71 5-93 9-78 79-04 39-59 12.50 5.49 10.81 99.81 38.63 15.79 5.36 15.96 122.24 34-39 19-34 4-77 23.56 119.21 38-91 18.84 5-39 24.28 128.08 33-77 20.26 4.68 26.40 I44-46 33-14 22.86 4.59 34.32 167.81 29.53 26.55 4-09 44-42 183.09 25.19 28.97 3.49 67.33 197.82 20.16 3!-3o 2.80 77-95 233-75 28.26 36.98 3.92 94.37 264.27 o.oo 41.81 o.oo 100-00 SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM PERMANGANATE AND RUBIDIUM PERMANGANATE AT 7. (Muthmann and Kuntze, calc. by Fock.) Milligram Mols. per Liter. Grams ger Liter. KMnO 4 in KMnO 4 . RbMnO 4 . KMnO 4 . RbMnO/. Crystals of Solid Phase. 27.04 22.69 4- 2 8 4-64 3-50 75.00 22.22 11.84 4-54 13-75 120.26 31-29 J 9-o3 6.40 34-29 188.30 38.98 29.80 7.97 71.45 198.36 41-29 31.39 8.44 92.50 205.76 42-50 32-56 8.69 99-47 225.12 26.00 35.61 5.32 99.32 264.27 o-oo 41.81 o.oo loo.oo POTASSIUM PHOSPHATE KH 2 PO 4 (Monobasic). One liter aqueous solution contains 249.9 grams at 7. (Muthmann and Kuntze.) POTASSIUM HYPOPHOSPHATE, etc. SOLUBILITY IN WATER. (Salzer Liebig's Ann. 211, i, 82.) Salt. Formula. Gms - Cms. Salt per i H 2 0. Cold. Hot. Potassium Hypophosphate K 4 P 2 O 6 .8H 2 O 400 " Hydrogen Hypophosphate K 3 HP 2 O 6 .3H 2 O 200 " Di Hydrogen Hypophosphate K 2 H 2 P 2 O 6 .3H 2 O 33 100 Tri Hydrogen Hypophosphate KH 3 P 2 O 6 66.6 200 " Penta Hydrogen Hypophosphate K 3 H 5 (P 2 O 6 ) 2 . 2H 2 O 40 125 " Hydrogen Phosphite KH 2 PO 3 172 (20) " Hypophosphite KH 2 PO 2 200(25) 333 Hypophosphite KH 2 PO 2 * 14.3(25) 28 * Solvent alcohol. 261 POTASSIUM PHOSPHO- MOLYBDATE POTASSIUM PHOSPHOMOLYBDATE K 3 PO 4 .nMoO 3 .iiH 2 O. 100 gms. H 2 O dissolve 0.007 gms. at 30. 100 gms. aqueous 10 % HNO 3 dissolve 0.204 gms. at 30. (Donk Proc. Assoc. Official Agrl. Chemists Bull. No. oo, Bureau of Chemistry, U. S. Dept. of Agr., '05.) POTASSIUM SELINATE K 2 SeO 4 . SOLUBILITY IN WATER. t. -20. -5. +5. 18. 97. Gms. K 2 SeO 4 per 100 gms. solution 51.5 51. 7 52. o 52. 6 54.9 (Etard Ann. Chim. phys. [7] 2, 550, '94.) POTASSIUM STANNATE K 2 SnO 3 .3H 2 O. 100 gms. H 2 O dissolve 106.6 gms. at 10, and 110.5 g ms - at 20 Sp. Gr. at 10 = 1.618 at 20 = 1.627. (Ordway Am. J. Sci. [2] 40, 173, '65.) POTASSIUM SULPHATE K 2 SO 4 . SOLUBILITY IN WATER. (Mulder; Andrae J. pr. Ch. 20,456, '84; Trevor Z. physik. Ch. 7, 468,01; TUdenand Shenstone - Phil. Trans. 31, '84; Berkeley Trans. Roy. Soc. 203 A, 209, '04; see also Etard Ann. chim. phys. [?] 2, 549, '94-) Gms. K 2 SO 4 per ioo Gms Gms. K 2 SO 4 per ioo Gms. Gms. K 2 SO 4 per ioo Gms Water. Solution. Water. Solution. I , Water. Solution. O 7-35 6.85 40 14.76 12.86 90 22.8 18-57 10 9.22 8-44 5 16.50 14.16 IOO 24.1 19.42 2O ii .11 10.00 60 18.17 I5-38 120 26-5 20-94 2 5 12 .04 10.75 7o 19-75 16.49 143 28.8 22.36 30 12-97 11.48 80 21-4 17.63 170 32-9 24.76 Sp. Gr. of solution saturated at 18 = 1.083. SOLUBILITY OP POTASSIUM SULPHATE IN AQUEOUS AMMONIA SOLUTIONS AT 20. (Girard Bull. soc. chim. [2] 43, 552, '85.) Gms. NH 3 per i oo cc. solution o 6.086 15-37 24.69 31-02 Gms. K 2 SO 4 per i oo cc. solution 10-80 4.10 0-83 0-14 0-04 SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM SULPHATE AND AMMONIUM SULPHATE AT 25. (Fock Z. Kryst. Min. 28, 375, '97.) Grams per Liter. Milligram Mols. per Liter. K 2 S0 4 . (NH 4 ) 2 S0 4 - ' Mol. per cent K 2 SO 4 in Solution. Sp. Gr. of Solution. Mol. per cent K 2 SO 4 in Solid Phase. KjjSO*. (NH 4 ) 2 S0 4 . 127.9 O-O 734 o.o IOO 1. 086 IOO 135-7 II5-7 778.5 874.6 47-1 I.I49 91.28 84.20 28l.I 483 2126 18.5 1.200 80-05 59.28 355-o 340 2685 11.13 1.226 68.63 40.27 482.7 231 3650 1.246 27-53 o.oo 542-3 o.o 4100 o.oo 1.245 o.oo Results are also given for 14, 15, 16, 30, 46, and 47. POTASSIUM SULPHATE 262 SOLUBILITY OF MIXED CRYSTALS OF POTASSIUM COPPER SULPHATE AND AMMONIUM COPPER SULPHATE IN WATER. CuSO 4 .K 2 SO 4 .6H 2 O and CuSO 4 (NH 4 ) 2 SO 4 .6H 2 O at i3-i4. (Fock.) Mols. per IPO Mols. H 2 O Mol. per cent K Salt Mols. per 100 Mols. H 2 O Mol. per cent K Salt K~Sair 'NH 4 Salt: m Solution, in Solid. K Salt. ' NH* Salt. ' in Solution. ' in Solid. ' o-oo I -O35 o.oo o.oo 0.2946 0.5096 36.63 58.20 0.0897 0.8618 5.06 10.34 0.3339 0.3319 50.15 75.34 0.2269 0.6490 16.76 33-05 0.4560 0.1961 69.93 83.86 0-2570 0.5887 30.40 46.22 0.4374 o.oo 100.00 100-00 SOLUBILITY OF SOME POTASSIUM DOUBLE SULPHATES IN WATER AT 25. (Locke Am. Ch. J. 27, 459, 'ox.) D "*le Salt- Formula. j Potassium Cobalt Sulphate K 2 CO(SO 4 ) 2 .6H 2 O 12.88 Copper " K 2 Cu(SO 4 ) 2 .6H 2 O 11.69 Nickel " K 2 Ni(SO 4 ),.6H 2 O 6.88 Zinc " K 2 Zn(S0 4 ) 2 .6H 2 O 13.19 SOLUBILITY OF POTASSIUM NICKEL SULPHATE AND ALSO OF POTASSIUM ZINC SULPHATE IN WATER AT DIFFERENT TEMPERATURES. Grams per 100 Gms. H 2 O. Grams per TOO Grams HjjO. *- ' K2Ni(S0 4 ) 2 K2Zn(S0 4 ) 2 ' *- 'K 2 Ni(SO 4 ) 2 K 2 Zn(SO 4 ) 2 ' .6H;}O. .6H 2 O. .6H 2 O. .6HO 2 . o 6 13 40 23 45 10 9 19 50 28 56 20 14 26 60 35 72 25 16 30 70 43 88 30 l8 35 SOLUBILITY OF THE THREE HYDRATES OF POTASSIUM FERRO SULPHATE IN WATER AT DIFFERENT TEMPERATURES. (Kuster and Thiel Z. anorg. Ch. ax, 116, '99.) K ? SO 4 .FeS0 4 .6H 2 0. K 2 SO 4 .FeSO 4 .4H 2 O. K 2 SO 4 .FeSO 4 .2H 2 O. t< cc.N/ioKMnO 4 Gms. K 2 SO 4 cc.N/ioKMnO 4 Gms.K 2 SO 4 cc.N/ioKMnO 4 Gms.K 2 SO per 2cc. Solution. .FeSO 4 per 100 cc. Sol. per 2 cc. Solution. .FeSO 4 per 100 cc. Sol. per 2 cc. Solution. .FeS0 4 per loo cc. Sol. o-5 12.4 18.36 15-5 22-94 15-4 22.79 17.2 17.0 25 .16 18.1 26.79 21.6 31.98 40.1 2 4 .8 36.72 21 .9 32.41 27 .6 40.86 60 29.0 42-93 24-1 35-68 28.8 42.63 80 30.6 45-29 27-3 40.46 28.6 42.34 90 29.6 43-82 28.9 42.73 95 29.8 44.11 27.7 41 .01 263 POTASSIUM SULPHATE SOLUBILITY OF POTASSIUM SULPHATE IN AQUEOUS SOLUTIONS OP POTASSIUM CHLORIDE, BROMIDE, AND IODIDE. (Blarez Compt. rend. 112, 939, '91.) Interpolated from the original results. Gram K2SO 4 per 100 cc. in Aq. Grams Halogen Solutions of: Salt per 100 cc. Solution. O 2 4 6 8 10 12 SOLUBILITY OP MIXED CRYSTALS OF POTASSIUM SULPHATE AND POTASSIUM CHROMATE AT 25. (Fock Z. Kryst. Min. 28, 379, '97.) KC1 KBr KI at 12.5. at 14. at 12.5. 9.9 10.16 9-9 8-3 9.1 9-2 7.0 8.2 8. 4 5-7 7-4 7-7 4.6 6.6 7-2 3-5 6.0 6.6 5-5 6.0 Milligram Mols. per Liter Grams per Liter. Mol. per cent K 2 S0 4 in Solution. Sp. Gr. of Solution. Mol. per cent K2S0 4 in Solid Phase. K 2 SO 4 . K 2 Cr0 4 . K 2 S0 4 . K 2 Cr0 4 . 618.1 o.o 107-7 O-OO IOO.O 1.083 IOO.O 608.4 103 106.0 2O.O2 85-51 I .092 99.65 341.0 691.8 59-46 134-5 33-oi I .141 97-30 174.8 1496.0 30-47 290.5 10.50 I.23I 91.97 110.7 2523 19.30 490-5 4.21 I-356 28.43 100.6 2687 17-54 5 2 2-3 3.60 i-377 2.41 o.o 2847 o.o 553-5 o.oo 1.398 o.oo 734-o o.o 127.9 o.o IOO.O i .0863 IOO.O 617 .0 103.4 107.6 20.1 85-65 i .0934 99.78 463 452-7 80.72 88.0 55-55 I - I2 35 98-49 279 948.2 48.64 184.4 22.72 1.1700 96.07 153 1469 26.68 285.6 9.41 1-2255 85-77 296 2681 51.61 521 .2 21 .09 1.3688 25 -73 o.o 2715 o.oo 527.8 o.oo 1.3781 o.oo SOLUBILITY OF POTASSIUM SODIUM SULPHATES IN WATER. Double Salt. t. Gm's.^cT Authority. 3K 9 SO 4 .Na 9 SO 4 103 . 5 40 . 8 (Penny Phil. Mag. [4] 10, 401, 'SS-) 5K 2 SO 4 .Na 2 SO 4 4.4 9.2 (Gladstone J. Ch. Soc. 6, it, '54.) 12.7 10.1 " 100.0 25.0 POTASSIUM SULPHATE 264 SOLUBILITY OF POTASSIUM SULPHATE IN AQUEOUS ALCOHOL. (Gerardin Ann. chim. phys. [4] 5, 147, '65; Schiff Liebig's Ann. 118, 362, *6i.) In Aq. Alcohol of 0.939 Sp. Gr.= 4o Wt. %. Alcohol of Different Strengths at 15. 40 80 60 Cms. K 2 SO 4 per 100 Gms. Alcohol. 0.16 O.2I 0.92 Weight per cent Alcohol. Gms. K 2 SO 4 per ioo Gms. Sat. Sol. 10 20 30 3-90 I .46 0.56 40 0-21 100 gms. glycerine of 1.255 temp. - Gr. dissolve 1.316 gms. K 2 SO 4 at ord. (Vogel Neues Report, Pharm. 16, 557 '67.) SOLUBILITY OF POTASSIUM SULPHATE IN AQUEOUS ACETIC ACID AND IN AQUEOUS PHENOL SOLUTIONS AT 25. (Rothmund and Wilsmore Z. physik. Ch. 40, 619, '02.) In Aq. Phenol. Mols. per Liter. Grams per Later. CH 3 COOH K 2 SO 4 . CeHfiOH. K 2 S0 4 . C 6 H 5 OH. K 2 S0 4 . O o 117 .0 .0 o .6714 o. o 1X7 .0 4 .2 "5 4 o .032 o .6598 3- 01 S .0 8 .22 114 4 .064 .6502 6. 02 .3 19 .68 no .8 o .127 o .6310 II . 94 no .0 34 .68 106 3 .236 .6042 22 . J 9 !05 3 69 .06 96 .87 o .308 5834 28. 97 101 7 128 58 82 .70 .409 o 5572 38. 46 97 .2 .464 .5480 43- 63 95-5 .498 (sat.) 5377 46. 82 93 .8 In Aq. Acetic Acid. Mols. per Liter. Grams per Liter. CHaCOOH.' KzS0 4 . o.o 0.6714 0.07 0-6619 0.137 0-6559 0.328 0-6350 0.578 0.6097 1.151 0.5556 2.183 -4743 100 grams water dissolve 10.4 grams K 2 SO 4 + 219.0 grams sugar at 31.25, or 100 grams sat. solution contain 3.18 grams K 2 SO 4 + 66.74 grams Sugar. (Kahler Z. Ver. Zuckerind. 47, 447, '97.) POTASSIUM ACID SULPHATE KHSO 4 . SOLUBILITY IN WATER. (Kremers Liebig's Ann. 92, 497, '54.) t 20 40 100 Gms. KHSO 4 per ioo gms. H 2 O 36.3 51.4 67.3 121.6 POTASSIUM PERSULPHATE K 2 S 2 O 8 . ioo gms. H 2 O dissolve 1.77 gms. K 2 S 2 O 8 at o. (Marshall J. Ch. Soc. 59, 771, '91.) POTASSIUM SODIUM THIOSULPHATE KNaS 2 O 3 .2H 2 O. POTASSIUM SODIUM HYDROGEN SULPHITE KNa 2 H(SO 3 ) 2 . 4 H 2 0. ioo grams H 2 O dissolve 213.7 grams KNaS 2 O 3 .2H 2 O (a) at 15. ioo grams H 2 O dissolve 205.3 grams KNaS 2 O 3 .2H 2 O (b) at 15. ioo grams H 3 O dissolve 69.0 grams KNa 2 H(SO 3 ) 2 .4H 2 O at 15. (Schwicker Ber. 22, 1731, '89.) 20 265 POTASSIUM SULPHO- CYANIDE. POTASSIUM SULPHOCYANIDE KSCN. 100 grams H 2 O dissolve 177.2 grams K*SCN at o, and 217.0 grams at ' (Rxidorff Her. 2, 68, '69.) SOLUBILITY OF POTASSIUM SULPHOCYANIDE IN ACETONE, AMYL ALCOHOL, ETC. (von Laszcynski Ber. 27, 2285, '94.) In Acetone. In Amyl Alcohol. In Ethyl Acetate. In Pyridine. Gms. KSCN per Gms. KSCN per Gms. KSCN per Gms. KSCN per t. 100 Gms. t. 100 Gms. t. 100 Gms. t. 100 Gms. (CH 3 ) 2 CO. CsHnOH. CH 3 COOC 2 H6. CgHijN. 22 20-75 13 0.18 o 0.44 O 6-75 58 20.40 65 i-34 14 0.40 20 6-15 100 2.14 79 0.20 58 4-97 133-5 3-15 97 3-88 "5 3.21 POTASSIUM (Bi) TARTBATE (Mono) KHC 4 H 4 O 6 Cream of Tartar. SOLUBILITY OF MONO POTASSIUM TARTRATE IN WATER. F" (Alluard Liebig's Ann. 133, 292, '65; Roelofsen Am. Ch. J. 16, 466, '94; Blarez 2, 434, '91; at 20, Magnanini Gazz. chim. ital. 31, II, 542, '01; at 25, Noyes an physik. Ch. 13, 413, '94.) Compt. rend, and Clement Gms. KHC4.ri.4Oft Gms. KHC^HjOft t. per 100 Gms. Solution. t. per loo Gms. Sol !ution. o. 3 o(R.) 0.32 (A) o.35 (B.) 4O 0.96 i3 1.29 IO o-37 0.40 0.42 50 1-25 1.8 I. 80 20 0.49 o-53(M.) 0.60 60 2.4 25 30 0.58 0.69 o.654(N. and C.) 0.9 (A.) 0.74 0.89 80 IOO .... 4.4 6-5 SOLUBILITY OF POTASSIUM ACID TARTRATE (KHC 4 H 4 O 6 ) IN NORMAL SOLUTIONS OF ACIDS AT 20. (Ostwald; Huecke J. pr. Ch. [2] 29, 49, '84.) Purified tartrate was added in excess to normal solutions of the acids, and after shaking clear i cc. portions of each solution were withdrawn and titrated with approximately N/io Ba(OH) 2 solution; i cc. normal acid requiring 10.63 cc - f tne Ba(OH) 2 solution. Acid. Gms. Acid cc. N/io Ba(OH) 2 Gms. KHC4H4O, 1 Acid Gms. cc. N/io Gms Acid Ba(OH) 2 KHC 4 H 4 O 8 per loo cc. Solvent. per i cc. Solution. per loocc. Solution. per loo cc. Solvent. per i cc. per icocc Solution. Solution' HN0 3 6. 31 5- 77* 10. 21 C 2 H 5 SO 3 H II. O 5 .01* 8.87 HC1 3- 65 5- 32 9- 42 HO.(CH 2 ) 2 SO 3 H 12. 6l 5 33 9-43 HBr 8. IO 5- 38 9- 75 C 6 H 5 S0 3 H 15.81 5 25 9.29 HI 12. 80 5- 43 9- 61 HCOOH 4.60 45 0.80 H,S0 4 4- 00 3- 97 7- 03 CH 3 COOH 6.00 .27 0.48 HCH,SO 4 ii. 21 5- 58 12. 44 CH 2 C1COOH 9-45 i .01 1.79 HC 2 H 6 S0 4 12. 61 5- 9- 58 C 2 H 5 COOH 7.40 o .24 0.42 HC 3 H 7 S0 4 14. 01 5- 21 9- 22 C 3 H 7 COOH 8.8! 0, 23 0.41 * The figures in this column show the amount of the Ba(OH)z solution in excess of that which would have bsen required by the normal acid solution alone in each case, viz., 10.63 cc. They, therefore, corre- spond to the amount of KHC^H^Oe dissolved in i cc. of each saturated solution, and when multiplied by i-77give the grams of KHC^Oa per 100 cc. solution. POTASSIUM TARTRATE. 266 SOLUBILITY OF MONO POTASSIUM TARTRATE (KHC 4 H 4 O 8 ) IN AQUEOUS SOLUTIONS OP ELECTROLYTES AT 25. (Noyes and Clement Z. physik. Ch. 13, 413, '94; Magnanini Gazz. chim. ital. 31, II, 542, f oi.) Gms. Equiv. Gms. per Gm. Equiv. Grams per Electro- per Liter. 100 CC. Electro- per Liter. IOO CC. lyte. Electro- KHC 4 Electro- KHCi lyte. Electro- KHC," Electro- KHC 4 lyte. H 4 6 . lyte. IL^OS. lyte. lyte. ILXV KC1 0.025 0.0254 1.86 0.4788 CH 3 COOK 0.05 0.0410 4.91 0.7718 " 0.05 0.0196 3-73 0.3680 " O.IO 0.0504 9.82 0.9486 (( O.IO 0.0133 7-46 0.2509 " O.2O 0.0634 19.63 1.1930 " O.2O 0.0087 14.92 0.1636 KHS0 4 (20) O-OI 0-0375 1.36 0.706 KC10 3 O.025 0.0256 3.06 0.4821 " O.02 0.0500 2.72 0.941 M 0.05 0.0197 6.13 0.3716 it O.IO 0-1597 13.62 3.006 " O.IO 0.0138 12.26 0.2601 KHC 2 O 4 * (20) o.oi 0.0369 1.28 0.694 " O.2O 0.0092 24.52 0.1728 " O.O2 0.0424 2.56 0.798 KBr O.O5 0.0197 5-95 0.3699 " O.IO O.II32 12.82 2.130 M O.IO 0.0134 11.91 0.2517 HC1 0.013 0.0367 o-45 0.690 " O.2O 0.0087 23.82 0.1629 M 0.025 0.0428 0.91 0.806 KI 0.05 0.0196 8.30 0.3687 tt 0.050 0.0589 1.82 1.109 " O.IO 0.0132 16.61 0.2492 NaCl 0.05 0.0376 2.92 0.708 ii O.2O 0.0086 33-22 0.1619 M O.IO 0.0397 0.748 KNO 3 O.O5 0.0195 0.3676 ii O.2O 0.0428 11.70 0.80^ " O.IO 0.0136 10.12 0-2551 NaClOs 0.05 0.0382 5-32 0.718 " O.2O 0.0090 2O.24 0.1696 11 O.IO 0.0405 10.65 0.763 K 2 S0 4 O.O5 0.0208 4.36 0.3921 " O.2O 0.0446 21.30 0.840 " O.IO 0.0147 8. 7 2 0.2769 * Acid potassium oxalate. '* 0^20 O.OIOO 17.44 0.1881 SOLUBILITY OF MONO POTASSIUM TARTRATE IN AQUEOUS ALCOHOL SOLUTIONS. (Roelofsen Am. Ch. J. 16, 466, '94; Wenger Ibid. 14, 624, '92-) NOTE. The original results were plotted on cross-section paper and the following figures read from the curves. Milligrams KHC 4 H < O 6 per 10 cc. of Aq. Alcohol of: If . 10 20 3 40 60 - N 80 per cent. per cent. per cent. per cent. per cent. per cent. o 17 II 7 6 6 6 10 22 14 8 7 6 6 20 29 18 ii 8 6 6 2 5 34 21 12 9-5 6-5 5-5 30 40 2 5 J 3 ii 7 5-5 40 55 36 J 9 14 7-5 5 50 87 55 29 19 8 5 POTASSIUM FLUO TITANATE K 2 TiF 6 .H 2 O. SOLUBILITY IN WATER. (Marignac Ann. chim. phys. [4] 8, 65, '66.) t o 3 6 10 14 20 Gms. K 2 TiF e per 100 gms. H 2 O 0.55 0.67 0.77 O.QI 1.04 1.28 26; POTASSIUM VANADATE POTASSIUM VANADATE K 3 V 6 O 14 .5H 2 O. 100 grams H 2 O dissolve 19.2 grams at 17.5. (Radan Uebig's Ann. 351, xao, "89.) POTASSIUM ZINC VANADATE KZnV 5 O 14 .8H 2 O. 100 grams H 2 O dissolve 0.41 gram of the salt (Radan). PRASEODYMIUM SULPHATE Pr 2 (SO 4 ) 3 . SOLUBILITY IN WATER. (Muthmann and Rolig Ber. 31, 1727, '98.) Gms. Pr 2 (SO 4 >3 t . per 100 Gms. Solid ft0 Phase. Gms. Pr 2 (SO 4 ) 3 per 100 Gms. Solid Phase. Solution. Water.' Solution. Water. O I6. 5 19.8 Pi 2 (SO 4 ) 3 .8H 2 O 75 4-0 4-2 Pr 2 (S0 4 ) 3 .8H 2 18 12-3 I4-I 85 J -5 *-55 Pr 2 (S0 4 ) 3 .8H 2 -f- 35 9-4 10-4 " 55 6.6 7- 1 95 1.0 I .01 PraCSO^.sHzO PROPIONIO ALDEHYDE C 2 H 5 COH. 100 grams H 2 O dissolve 16 grams aldehyde at 20. (Vaubel J. pr. Ch. 59. 30, '99-) PROPIONITRIL C 2 H 5 CN. SOLUBILITY IN WATER. Synthetic method used. See Note, page 9. (Rothmund Z. physik. Ch. 26, 474, '98.) Wt. per cent C 2 H 6 CN in; Wt. per cent CjjHfiCN in: * ' Aq. C2H 6 CN ** A^ C 2 H 6 CN Layer. Layer. Layer. Layer. 40 10.7 92.1 95 19.6 78.0 50 ii. 6 90.5 ioo 22.4 75.5 60 12.7 88.5 105 26.0 72.1 70 13.2 86.1 no 32.0 66.5 80 14.9 83.4 113.1 (crit. temp.) 48.3 90 17.6 80.2 PROPYL ACETATE, Butyrate and Propionate. SOLUBILITY OF EACH IN AQUEOUS ALCOHOL MIXTURES. (Bancroft Phys. Rev. 3, 205, '95, calc. from Pfeiffer.) cc. H 2 O Added to Cause Separation* in: Vb4 .TVH.U- hoi in P. Ace- P. Buty- P. Propio- cc. /uco- hoi in P. Ace- P. Buty- P. Propio- Mixture. tate. rate. nate. Mixture. tate. rate. nate. 3 4-50 I.I9 1-58 21 58.71 19.68 27.83 6 10.48 3-55 4.70 24 oo 23.72 33-75 9 17.80 6.13 8-35 30 32.10 47-15 12 26.OO 9-05 12.54 36 41-55 63.18 15 35 -63 12.31 17 .15 42 51 .60 83.05 18 47-50 15.90 22.27 48 62 .40 107.46 54 73-85 * cc. HsO added to cause the separation of a second phase in mixtures of the given amounts of alcohol and 3 cc. portions of propyl acetate, butyrate and propionate. PROPYL ACETATE 268 SOLUBILITY OP PROPYL ACETATE, FORMATE, AND PROPIONATE IN WATER. 100 cc. H 2 O dissolve 1.7 gms. propyl acetate at 22. 100 cc. H 2 O dissolve 2.1 gms. propyl formate at 22. (Traube Ber. 17, 2304, '84.) ioo cc. H 2 O dissolve 0.6 cc. propyl propionate at 25. (Bancroft.) PEOPYL OHLORIDE, Bromide, etc. SOLUBILITY IN WATER. (Rex Z. physik. Ch. 55, 355. '06.) Grams P. Compound per too Gms. H2O at: Propyl Compound. (normal) 0.376 0.323 0.272 0.277 CH 3 CH 2 CH2Br " 0.298 0-263 0.245 0.247 CH 3 CH 2 CH 2 I " 0.114 0.103 0.107 0.103 (CH 3 ) 2 CHC1 (iso) o . 440 o . 363 o . 305 o . 304 (CH 3 ) 2 CHBr 0.418 0.365 0.318 0.318 (CH 3 ) 2 CHI " 0.167 0.143 0.140 0.134 PROPYLENE C 3 H 6 . SOLUBILITY IN WATER. (Than Liebig's Ann. 123, 187, '62.) t. p. ? 0.4465 0.0834 5 0-3493 0.06504 10 0.2796 0.0519 15 0.2366 0.0437 20 0.2205 0.0405 and q, see Ethane, page 133- For values of PYRENE C 16 H 10 SOLUBILITY IN TOLUENE AND IN ABSOLUTE ALCOHOL. ioo gms. toluene dissolve 16.54 gms. pyrene at 18. ioo gms. absolute alcohol dissolve 1.37 gms. pyrene at 10 and 3.08 gms. at b. pt. PYROGALLOL C 6 H 3 (OH) 3 i, 2, 3. SOLUBILITY IN WATER, ETC. (U. S. P.) ioo gms. water dissolve 62.5 gms. C 6 H 3 (OH) 3 at 25. ioo gms. alcohol dissolve 100.0 gms. C 6 H 3 (OH) 3 at 25. ioo gms. ether dissolve 90.9 gms. C 6 H 3 (OH) 3 at 25, 269 QUININE QUININE C 20 H 24 N 2 O 2 . (See also Cinchona alkaloids, p. 117.) SOLUBILITY OF QUININE AND OF QUININE SALTS IN WATER AND OTHER SOLVENTS. (U. S. P.) Grams. Quinine Compound per 100 Grams Solvent in: Compound. C 20 H 24 N 2 2 C 20 H 24 N 2 2 . 3 H 2 C 20 H 24 N 2 O 2 HC1.H 2 O C 20 H 24 .N 2 2 . 2 C 6 H 4 (OH). COOH.H 2 O (C 20 H 24 N 2 2 ) 2 .H 2 S0 4 . 7 H 2 C 20 H 24 N 2 2 .H 2 S0 4 .7H 2 C 20 H 24 N 2 2 .HBr.H 2 Water. Alcohol. Ether. Chloroform. Glycerine. At *5. At 80.' At 25. At 25 - At 25. At 25. 0. 057 0. 123 166. 6 22 .2 52- 6 O. 633 0. 06 5 0. 129 166. 6 7 6 9 62. 5 .472 5 55 250. 166. 6 .417 122. 12 .2 I 30 2. 86 9- 09 .91 2. ,70 6 25 0. i39 2. 22 i. 16 . O. 25 2 .78 II. 77 117. 7 5- 55 .056 0. 109 5-55 2. 5 33- 3 149. 2 6 .2 . 12 5 SOLUBILITY OF QUININE IN AQUEOUS SOLUTIONS OF CAUSTIC ALKALIES. (Doumer and Deraux J. pharm. chim. [6] i, 50, '95.) METHOD. A one per cent solution of quinine sulphate containing a very small amount of HC1 was gradually added to 200 cc. portions of the caustic alkali solutions of the various concentrations stated, and the point noted at which a precipitate of the appearance cor- responding to that of i cc. of milk in 100 cc. of water, remained undissolved. In Aq. Ammonia. In Aq. Sodium Hydrate. In Aq. Pot. Hydrate. Gms.NHa per 200 cc. Solution. Gms. Anhydrous Quinine Dissolved. Gms. NaOH per 200 cc. Solution. Gms. Anhydrous Quinine Dissolved. Gms.KOH per 200 cc. Solution. Gms. Anhydrous Quinine Dissolved. 0.52 0-084 O.OO7 O.O92 0.612 0.088 0.65 0.084 O-OI2 0.091 I.5I2 0.082 4-59 0.096 0.740 O.O9O 3-456 0.068 13.08 O.I22 2.l6o 0.079 10.944 0.039 18.88 0.144 3.188 0.056 44 74 O.OO6 25.19 0.174 6.172 0.044 35-79 0.184 8-537 0.021 17.074 0.015 SOLUBILITY OF QUININE SALTS IN WATER. (Regnault and Willejean Chem. Centralb. 18, 252, '87.) Salt. Brom Hydrate (basic) (neutral) Chlor Hydrate (basic) Lactate t. Gms. Salt per iooGms.H 2 O. Salt. t. Gms. Salt per 100 Gms. H 2 O 14 2 .06 Salicylate (basic) 15 O .114 12 12 33 Sulphate " 14 o. 139 14 13 .19 a tt 16 o. 16 14 79 a 18 o. 160 15 14 .20 " (neutral) 15 8. 50 12 3 .80 it n 17 8. 90 14 4 .14 it tt 18 9- 62 IS 4 2 5 Valerate (basic) I2-l6 2. 59 15 10 03 37 16 .18 RESORCINOL. 270 RESOROINOL C 6 H 4 (OH) 2 i, 3. SOLUBILITY IN: Water. Ethyl Alcohol. (Speyers Am. J. Sci. [4] 14, 294, '02.) (Speyers.) . Sp. Gr.of Gms.CoHtCOH);; per 100 Gms. Sp .Gr.of Gms. GjH4(OH) 2 per 100 Gms. Solutions. Water. Solution. Solutions. Alcohol. Solution. O I .101 60 37-5 I 033 2IO 6 7 .8 10 I .118 8l 44-8 I .036 223 6 9 .0 20 I 134 103 50-7 I .041 236 70 3 25 I .142 117 53-9 I 045 243 70 .8 30 I .148 I3 1 56-7 I .048 250 71 4 40 I .157 161 58.9 I 056 266 72 7 50 I .165 198 66.5 I 065 286 74 i 60 I .172 246 71.1 I 075 311 75 7 70 I .176 320 76.2 I .087 341 77 3 80 I .179 487 82.9 I .104 375 78 9 NOTE. The original results of Speyers are given in terms of mols. per 100 mols. H 2 O. According to Vaubel, 100 gms. H 2 O dissolve 175.5 ms - C 6 H 4 (OH) 2 , or 100 gms. sat. solution contain 63.7 gms. at 20. Sp. Gr. of sol. = I - I 335- (J. pr. Ch. [2] 52, 73. '95-) SOLUBILITY OF RESORCINOL IN BENZENE. (Rothmund Z. physik. Ch. 26, 475, '98.) Synthetic method used. See Note, p. 9. Gms. C6H4(OH) 2 per 100 Gms. Gms. QH^OIty; per 100 Gms. CeHe Layer. C 6 H4(OH) 2 Layer. C 6 H 6 Layer. 60 4.8 79.4 90 13.0 71.3 70 6.6 77.5 ioo 19.5 65.7 80 9.2 75 .o 105 24.6 60.7 109.3 ( cr it- temp.) 42.4 DISTRIBUTION OF RESORCINOL BETWEEN WATER AND ORGANIC SOLVENTS AT ORDINARY TEMPERATURE. (Vaubel J. pr. Ch. [2] 67, 478, '03.) Gms. Gms. CeH^OH) in: C 6 H4(OH) 2 Solvents. Organic Used. H 2 Layer. S o\v?llyer. 1.191 6occ. H 2 O+ 30 cc. Ether 0.2014 0.9896 1.191 60 cc. H 2 O + 60 cc. Ether 0.2475 0.9525 0-800 40 cc. H 2 O+ 40 cc. Benzene 0.5873 0.2127 0.800 40 cc. H 2 O+ 80 cc. Benzene 0-5773 0.2227 0.500 50 cc. H 2 O+ 50 cc. CC1 4 0.4885 0.0115 0.500 50 cc. H 2 O+ioo cc. CC1 4 0.4880 0.0120 0.500 50 cc. H 2 O+i5o cc. CC1 4 0.4880 0.0120 RHODIUM SALTS. SOLUBILITY IN WATER. (Jorgensen J. pr. Ch. [2] 27, 433. '83; 34. 394. '86; 44, 51. '91-) Salt. Formula. t Chloro Purpureo Rhodium Chloride ClRh(NH 3 ) 5 Cl 2 17 0.56 Luteo Rhodium Chloride Rh(NH 3 ) 6 Cl 3 8 13.3 Luteo Rhodium Nitrate Rh(NH 3 ) 6 (NO 3 ) 3 ord. t. 2.1 Luteo Rhodium Sulphate [Rh(NH 3 ) 6 ] 2 (SO 4 ) 3 .5H 2 O 20 2.3 2 7 I RUBIDIUM ALUMS formula. i . Anhydrous . Hydrated. G. Mols. RbAl(SO 4 ) 2 .i2H 2 O 25 1.81 3-15 0.0059 (4 3 2.19 0.0072 <( 35 2.66 0.0087 11 40 3.22 . 0.0106 RbCr(SO 4 ) 2 .i2H 2 O 25 2-57 4-34 0.0079 M 3 3-17 . . . 0.0096 " 35 4.11 0.0128 40 5-97 0.0181 RbV(S0 4 ) 2 .i2H 2 RbFe(SO 4 ) 2 .i2H 2 O 25 25 5-79 9-74 9-93 16.98 0.0177 0.0294 " 3 20. 24 0.0617 RUBIDIUM ALUMS. SOLUBILITY IN WATER. (Locke Am. Ch. J. 27, 174, '01.) Gms. Alum per 100 Gms. HjO. Alum. Rb. Aluminum Alum Rb. Chromium Alum Rb. Vanadium Alum Rb. Iron Alum Biltz and Wilke (Z. anorg. Ch. 48, 299, '06) find for the solubility of rubidium iron alum in water, at 6.6, 4.55 gms. per 100 cc. solution; at 25, 29.0 gms.; and at 40, 52.6 gms. RUBIDIUM FLUOBORIDE RbBF 4 . 100 gms. H 2 O dissolve 0.55 gm. RbBF 4 at 20, and i.o gram at 100. (Godeffroy Ber. 9, 1337, '76.) RUBIDIUM BROMIDE RbBr. SOLUBILITY IN WATER. (Rimbach Ber. 38, 1557, '05.) Gms. RbBr per 100 Gms. Gms. RbBr per 100 Gms. ' Water. Solution. Water. Solution. 0.5 89.6 47-26 39.7 131-85 5 6 - 8 7 5.0 98.0 49-5 57-5 i5 2 -47 60.39 16.0 104.8 51-17 113-5 205.21 67.24 RUBIDIUM CARBONATE Rb 2 CO 3 . 100 gms. absolute alcohol dissolve 0.74 gm. Rb 2 CO 3 . (Bunsen.) RUBIDIUM CHLORATE RbClO 3 . SOLUBILITY IN WATER. (Reissig Liebig's Ann. 127. 33. '63-) t. 4.7. 13-0 '. 18.2*. 19-0. Gms. RbClO 3 per 100 grams H 2 O 2.8 3.9 4-9 5 - 1 RUBIDIUM (Per) CHLORATE RbClO 4 . 100 grams H 2 O dissolve 1.08 grams RbClO 4 at 21.3. (Longuimine Liebig's Ann. 121, 123, '62.) RUBIDIUM CHLORIDE 272 t RUBIDIUM CHLORIDE RbCl. SOLUBILITY IN WATER. (Rimbach Ber. 35, 1304, '02; Berkeley Trans. Roy. Soc. (Lond.) 203 A, 207, '04.) * Mols. RbCl Gms. RbCl per 100 Gms. t *. Mols. RbCl Gms. RbCl per 100 Gm * per Liter. Water. Solution. per Liter. Water. Solution. 5.17 77-0 43-5 60 6.90 "5-5 536 10 5-55 84.4 45-8 70 7-12 121 .4 54-8 20 5-88 9I.I 47-7 80 7-33 127.2 56.0 3 6.17 97.6 49-4 90 7-52 133 - 1 57-i 40 6-43 103-5 50-9 100 7.71 138.9 58-9 So 6.67 109.3 52.2 112.9 7-95 146.6 59 5 RUBIDIUM TELLURIUM CHLORIDE Rb 2 TeCl,. 100 gms. Aq. HC1 of 1.2 Sp. Gr. dissolve 0.34 gm. Rb 2 TeCl 6 at 23. 100 gms. Aq. HC1 of 1.05 Sp. Gr. dissolve 13.09 gms. Rb 2 TeCl 6 at 23. (Wheeler Am. J. Sti. [3] 45. 267, '93-) RUBIDIUM THALLIUM CHLORIDE 3RbClTlCl 3 .2H 2 O. 100 gms. H 3 O dissolve 13.3 gms. at 18, and 62.5 gms. at 100. (Godeffroy Zeit. allgem. Oster. Apoth. No. 9, '80.) RUBIDIUM GHROMATE (Mono) Rb 2 CrO 4 . SOLUBILITY IN WATER. (Schreinemaker and Filippo Chem. Centralb. 77, I, 1321, '06.) Gms. RbCrO 4 Gms. RbCrC-4 Gms. RbCrOv t. per zoo t . per 100 t. per 100 Gms. Solution. Gms. Solution. Gms. Solutioi - 7 36.65 50 47-44 2.40 J 5-58 o 3 8.27 60.4 48.90 3.25 20-03 10 40.23 Solid Phase, Ice 4.14 24.28 20 42.42 0.6 6.95 -5-55 3<>- I 5 30 44.11 i.i 7.22 -6.71 34-3 1 40 46.13 -1.57 9.87 about 7 36.65 RUBIDIUM (Di) CHROMATE Rb 2 Cr 2 O 7 . 100 grams saturated aqueous solution contain 9.47 grams Rb 2 Cr 2 O 7 at 30. (Schreinemaker and Filippo.) RUBIDIUM HYDROXIDE RbOH. 100 grams sat. aqueous solution contain 63.39 grams RbOH at 30. (Schreinemaker and Filippo.) RUBIDIUM IODATE RbIO 3 . 100 grams H 2 O dissolve 2.1 grams RbIO 3 at 23. (Wheeler Am. J. Sci. [3] 44. "3. '92-) RUBIDIUM IODIDE Rbl. 100 grams H 2 O dissolve 137.5 grams Rbl at 6.9, and 152.0 grams at 17-4. (Reissig Liebig's Ann. 127. 33. '63-) 273 RUBIDIUM IODIDE SOLUBILITY OF RUBIDIUM IODIDE IN ORGANIC SOLVENTS. (Walden Z. physik. Ch. 55, 713, 718, '06.) Solvent. Acetonitril Propionitril Nitromethane Acetone Furfurol Formula. CH 3 CN C 2 H 5 CN CH 3 N0 2 (CH 3 ) 2 CO C 4 H 3 O.COH Grams Rbl per 100 cc. Solution. 1.478 at o 0.274 " 0-567 " 0.960 " i. 350 at 25 0-305 " 0.518 " 0.674 " 4-930 " RUBIDIUM BROM IODIDE RbBrJ. loo gms. sat. aq. solution contain about 44.0 gms. RbBr 2 I, and the Sp. Gr. of the solution is 3.84. (Wells and Wheeler Am. J. Sci. [3] 43, 475, '92.) RUBIDIUM NITRATE RbNO 3 . SOLUBILITY IN WATER. (Berkeley Trans. Roy. Soc. (Lond.) 203 A, 207, '04.) Mols. OramsRhNO, rv>r rooGms. Mols. K. DIN 03 ' Per Liter. Water. Solution. i\i)iM\J3 Per Liter. Water. Solution . 1.27 19-5 16.3 60 7-99 200 66.7 10 2 .04 33-o 24.8 70 9.02 2$I 71 .5 20 3-10 53-3 34-6 80 9-93 309 75-6 30 4-34 81.3 44.8 90 10.77 375 78.9 40 5.68 116.7 53-9 IOO n-54 452 81.9 50 6.88 I 55- 6 60.9 118.3 12 .76 617 86.1 RUBIDIUM PERMANGANATE RbMnO 4 . One liter of aqueous solution contains 6.03 grams RbMnO 4 at 7. (Muthmann and Kuntze Z. Kryst. Min. 23, 377, '94.) loo cc. sat. aq. solution contain 0.46 gm. RbMnO 4 at 2, 1.06 gms. at 19 and 4.68 gms. at 60. (Patterson J. Am. Ch. Soc. 28, 1735, '06.) RUBIDIUM SELENATE Rb 2 SeO 4 . loo grams H 2 O dissolve 158.9 grams Rb 2 SeO 4 at 12. (Tutton J. Ch. Soc. 71, 850, '97-) RUBIDIUM FLUO SILICATE Rb 2 SiF 6 . loo gms. H 2 O dissolve 0.16 gm. Rb 2 SiF 6 at o, and 1.36 gms. at 100. (Stolba J. pr. Ch. 101, i, '67.) RUBIDIUM SILICO TUNGSTATE Rb 8 SiW 12 O 42 . loo gms. H 2 O dissolve 0.65 gm. Rb 8 SiW 12 O 42 at 20, and 5.1 gms. at I OO. (Godeffroy Ber. 9, 1363, '76.) RUBIDIUM SULPHATE Rb 2 SO 4 . SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 550, '94; Berkeley Trans. Roy. Soc. (Lond.) 203 A, 207, '04.) t*. Mols. c RW50, * per Liter. ims. Rb 2 SO 4 per 100 Gms. A0 Mols. Gms. Rb 2 SO 4 per 100 Gms. Water. Solution. per Liter. Water. Solution. o 1.27 3 6 -4 27-3 60 2.15 67.4 40-3 10 I. 4 6 42 .6 29.9 7 2.25 71.4 41.7 20 I .64 48.2 32-5 80 2-34 75 - 42.9 30 1-79 53-5 34-9 90 2.42 78.7 44-o 40 I .92 58-5 36.9 IOO 2.49 81.8 45 -o SO 2 -O4 63-1 38.7 102.4 2 -SO 82.6 45-2 RUBIDIUM SULPHATE 274 SOLUBILITY OF RUBIDIUM DOUBLE SULPHATES IN WATER AT 25. (Locke Am. Ch. J. 27, 459, '01.) Formula. Rb 2 Cd(S0 4 ) 2 .6H 2 Rb 2 Co(S0 4 ) 2 .6H 2 Rb 2 Cu(S0 4 ) 2 .6H 2 Rb 2 Fe(SO 4 ) 2 .6H 2 O Per IPO cc. H 2 O. Gms. Mols. Anh. Salt. Salt. 76.7 0.1615 9.28 0.022 IO.28 O.O24I 24.28 0.0579 Formula. Rb 2 Mn(SO 4 ) 2 .6H 2 O Rb 2 Mg(S0 4 ) 2 .6H 2 Rb 2 Ni(S0 4 ) 2 .6H 2 Rb 2 Zn(SO 4 ) 2 .6H 2 O Per IPO cc. H 2 O. Gms. Mols. nh. Salt. Salt. 35-7 20.2 5.98 10.10 0.0857 0.0521 0.0142 0.0236 SALICYLIC ACID C 6 H 4 .OH.COOH 1:2. SOLUBILITY IN WATER. (See also p. 61.) .. 315. '9; tummann ana i^angoeck iota. 51 with the following, see Alexejew -Ann. Physik. Chem. 28, 305, '86; Bourgion IS* 165, '?8; Ost. J. pr. Ch. [2] 17, 232, '78.) O 10 20 Gms. Cel^OHCOOH per Liter Solution. 0.8 I .2 1.8 25 30 40 50 Gms. Q,H 4 OH.COOH per Liter Solution. 2.2 2-7 3-7 5-4 60 70 80 Ann. chim. phys. [5] Gms. CeH 4 OH.COOH per Liter Solution. 8.2 I 3 .2 20-5 SOLUBILITY OF SALICYLIC ACID (LIQUID) IN WATER. (Alexejew.) Determinations by Synthetic Method. See Note, page 9. Figures read from curve. Gms. CeH 4 OHCOOH per 100 Gms. 60 70 80 00 95 temp.) Aqueous Layer. Salicylic Acid Laver. 7 68 8 64 12 58 19 49 32 SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SALT SOLUTIONS AT 25* AND AT 35. (Hoffmann and Langbeck Z. physik. Ch. 51, 407, '05.) Salt. KC1 KN0 3 NaCl Normality of Salt Gms. C^OHCOOH < dissolved at 25. dissolved at 35. Solution. Liter. Gms. per 1000 G. Molecular Gms. per 1000 G. Molecular gms. Sat. Sol. percentage, gms. Sat. Sol. percentage. o .0 O. 2 .206 2.8851 3 .197 .020 I 49 2 .24 2 .9216- ICT 4 3 23 4 .2206. 10" 100 7 .46 2 25 2-9377 " 3 23 4 .2203 n .492 36 73 2 .02 2.6321 " 3 .9268 tt I .004 74 .92 I .89 2-4759 2 .68 3 5003 u .020 2 .02 2 25 3.9351 " 3 25 4 2499 tt .100 10 .12 2 30 3-OJ03 " 3 32 4 3334 it o 504 5 1 .10 2 38 3.1061 " 3 38 4 .4123 tt I .004 101 .60 2 39 3.1249 3 36 4 .3848 it .020 i .19 2 23 2.9110 3 .22 4 .2062 tt .100 5 95 2 .22 2.9027 " 3 .20 4 .1806 tt 497 29 .50 2 OO 2.6128 2 85 3 .7171 tt o .988 58 .80 I 72 2.2487 " 2 43 3 .1596 it 275 SALICYLIC ACID SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SOLUTIONS OF SODIUM FORMATE, ACETATE, AND BUTYRATE AT 26.4. (Philip J. Ch. Soc. 87, 992, '05.) *_i_ Mols. Per Liter in: 100 per Liter. i<_nj HCOONa. CH 3 COONa. C :3H 7 COONa^ O I.7I I.7I I.7I I 2-35 2.47 2.50 2 3-05 3-35 3 -48 3 3-7 4-2 4-35 4 5 4-3 5- 1 48 6.1 5-3 63 Per Liter in: Ocfcll per Liter. O I 2 3 4 5 HCOONa. CHsCOONa. C 3 H 7 COONa 2-36 2.36 2.36 3-7 3-6 5-o 5.2 6.2 6.75 7.2 8.3 3-3 4-5 5-65 6.85 8.1 SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SOLUTIONS OF SODIUM SALICYLATE AT 20.1. (Hoitsema Z. physik. Ch. 27. 315, '98.) Gram Mols. per Liter. D. Gr. Grams per Liter. CsttiOH COOH. C6H4OH of COONa. Solutions. Cfitt^OH COOH. C6H 4 OH COONa. Solid Phase. O .0132 1.002 I -823 O .0 C^OHCOOH OII2 -017 .003 I 55 2 705 " O -OI24 .113 .009 I 7i 17 .98 O 0143 O .226 .016 I 97 35 .96 i 0164 344 .024 2 .26 54 74 " 0203 .500 034 2 .80 79 56 " 062 I .70 1 .098 8 56 270.1; o 095 2 .11 137 13 .11 335 f Cel^OHCOOH.Cel^OHCOONa 7 ( + CH40HCOOH o OQI 2 .19 .144 12 56 348 4 CH4OHCOOH.CH40HCOONa o 086 3 .41 1.215 II .88 542 .6 o 081 4 .23 1.263 II .19 673 ^ J CaHUOHCOOH.C^OHCOONa ( +C6H4OHCOONa o 048 4 .18 1-259 6.63 665 .1 CH4QHCOONa 021 4 .12 1-258 2 .90 665 5 OO 4 r 5 1-257 O .0 660 3 SOLUBILITY OF SALICYLIC ACID IN ALCOHOLS IN ETHER AND IN ACETONE. (Timofeiew Compt. rend. 112. 1137, '91; at 15, Bourgoin Ann. chim. phys. [5] 13, 405, '78; at 17 and 23, Walker and Wood J. Ch. Soc. 73, 6>, '98.) Solvent. CH 3 OH CH 3 OH C 2 H 5 OH C 2 H 5 OH C 2 H 5 OH CpHUOH 90% t. -3 -f 21 -3 + 15 21 15 Cms. Ce^OHCOOH per loo Gms. Solvent. C 3 H 7 OH() C 3 H 7 OH() (CH 3 ) 2 (CH 3 ) 2 (CH 3 ) 2 CO * Per Gms. CH4OHCOOH 4 t per 100 Gms. Solvent. Solution. 40.67 28.91 62.48 38.46 36.12 26.29 49.63 33-17 53-53 34.87 42.09 29.62 Solvent. Solution, 3 26.12 20.71 + 21 37.69 27.36 15 50.47 33-55 17 23.4* 23 3i 3* ioo cc. Sat. Solution. SALICYLIC ACID 276 SOLUBILITY OF SALICYLIC ACID IN AQUEOUS SOLUTIONS OP ETHYL ALCOHOL, Iso BUTYL ALCOHOL, DEXTROSE, CANE SUGAR, AND OF LEVULOSE AT 25 AND AT 35. (Hoffmann and Langbeck Z. physik. Ch. 51, 400, '05.) Aq. Solvent. H 2 O C,H 5 OH u II ll C 4 H 9 OH (iso) ii ii C 6 H 12 8 Cone, of Solvent. CH 4 OHCOOH dis- solved at 25. C 8 H 4 OHCOOH dis- solved at 35. Normality. O.O Gms. per Liter. 0.0 Grams Grams Grams molecular per ioo gms. molecular percentage. sat. solution, percentage 2.8851 0.22064.1844 Grams per ioo gms. sat. solution. 0.3197 O. 0249 I. 146 2. 8966. 10~ 4 0.222 4 .2044.IO""" 4 0. 322 O. 0560 2. 578 2. 9150 " 0.223 4 .2348 ii 0. 324 0. 1747 8. 04 2. 9901 0.229 0. 2399 II. 05 4 4341 ii 0. 339 I. 03 47- 4 3- 5279 " 0.270 5 .28l6 ii 0. 404 I. 638 75- 44 3- 9253 0.300 O. O2O i. 496 2. 909 0.223 4 .229 ii 0. 324 0. 051 3- 74 2. 955 0.226 4 .289 ii 0. 329 0. IOO 7- 48 3- 033 0.232 4 435 ii O. 339 0. 5 21 38. 60 3- 718 " 0.285 5 .624 ii O. 0. 02 6 2. 886 " 0.221 4 .184 n 0. 321 0. IO 18. 2. 898 O. 222 4 .202 ii 0. 322 O. 50 89. 6 2. 954 0.226 4 .263 ii O. 326 I. 00 180. 3- 015 " 0.231 4 .360 ii 0. 334 O. 02 6. 88 2. 885 " O. 221 4 .206 ii 0. 322 0. IO 34- 97 2. 964 " 0.227 4 .28 7 ii O. 328 0. 50 172. 3- 239 0.248 4 .697 ii 0. 360 I. 10 376. 3 3- 633 " 0,278 5 .236 ii 0. 401 0. 02 3-6 2. 888 " 0.221 . . . 0. 06 10. 8 2. 895 " 0.221 . . . 0. 25 45- 2. 944 " C.225 C 6 .H 12 O a SOLUBILITY OF SALICYLIC ACID IN BENZENE. (Walker and Wood J. Ch. Soc. 73, 620, '98.) Gms. Gms. Gms. t o QjIL^OHCOOH t o C6H4OHCOOH t <, C^OHCOOH per ioo Gms. per ioo Gms. per ioo Gms. r* TT r* XT r* TT eerie. i^6"6- v^ng. II-7 0.460 30.5 0.991 49.4 2.380 18.2 0.579 34.6 1.261 64.2 4.40 36.6 1.430 SELENIUM Se. SOLUBILITY IN CARBON BISULPHIDE. (Marc Z. anorg. Ch. 48, 425, '06.) ioo cc. CS 2 dissolve 0.065 g m - amorphous Se at room temperature. Se which is heated to 180 for 6-7 hours is insoluble in CS 2 . Se crystal- lized from the melt at 200 is insoluble in CS 2 . Se heated once quickly to 140 is very slightly soluble in CS 2 . ioo gms. methylene iodide (CH 2 I 2 ) dissolve 1.3 gms. Se at 12. (Retgers Z. anorg. Ch. 3, 346, '93.) 277 SELENIOUS ACID SELENIOUS ACID H 2 SeO 3 . SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 551, '94.) Cms. H 2 SeO 3 100 Gms. Soli 10 O + 10 20 per ution. 42.2 47-4 55-o 62 .5 t o Gms. H 2 SeO3 per 100 Gms. Solution t Gms. HjSeOs per * 100 Gms. Solution. 2 5 67.0 60 79-3 30 40 70.2 77-5 70 80 79-3 79-3 50 79.2 90 79-4 SILICON Si. SOLUBILITY IN LEAD AND IN ZINC. (Moissan and Siemens Ber. 37, 2088, '04.) In Lead. t. Gms. Si per 100 Gms. Solution. 1250 0-024 1330 0.070 1400 0-150 1450 !55 O-2IO 0.780 600 650 730 800 850 In Zinc. Gms. Si per 100 Gms. Solution. 0-o6 o-57 0.92 i .62 SILICON IODIDES Si 2 I 6 , SiI 4 . SOLUBILITY IN CARBON BISULPHIDE. (Friedel and Lachburg Bull. soc. chim. [2] 12, 92, '69; Friedel Liebig's Ann. 149, 96, '69.) ioo gms. CS 2 dissolve 19 gms. Si 2 I 6 at 19. 100 gms. CS 2 dissolve 26 gms. Si 2 I 6 at 27. ioo gms. CS 2 dissolve 2.2 gms. SiI 4 at 27. SILICO TUNGSTIC ACID H 8 SiW 12 O 42 . ioo gms. H 2 O dissolve 961.5 crystallized silico tungstic acid at 18, and solution has Sp. Gr. 2.843. SILVER 278 For equilibrium between metallic Silver and mercury (Silver amai gam) and mixed aqueous solutions of their nitrates, determined foe mixtures of the two metals in all proportions, see Reinders Z. physik. Ch. 64, 609, '06. SILVER ACETATE CH 3 COOAg. SOLUBILITY IN WATER. (Nernst Z. physik. Ch. 4, 379,' 89; Nauman and Rucker Ber. 38, 2293 Arrhenius Ibid, u, 396, '93; Goldschmidt Ibid. 25, 93, '98, , '05; Raupenstrauch Monatsh. Ch. 6, 585, '85; Wright and Thompson Phil. Mag. [5] 17, 288, '8 4; 19, it '85. ) t o Gms . Ag( C 2 H 3 O 2 ) 1 per Liter. Gms.Ag(C 2 H 3 O 2 ) per Liter. f. Gms. Ag(C 2 H 3 O 2 ) per Liter. O 7-22 25 II. 2 50 16.4 10 8-75 30 12 .1 60 18.9 15 9-4 40 I4-I 70 21.8 2O 10.4 80 25.2 SOLUBILITY OF SILVER ACETATE IN AQUEOUS SOLUTIONS OP: Silver Nitrate. Sodium Acetate. Gms^ Gms. CH 3 COOAg per Liter at: CHaCOONa Gms - CH 3 COOHg per Liter at: pe/Liter. 16 (Nernst). i9.8(Arrhenius). per Liter * 16 (N.,N.andR.). i8.6(A.). ' o 10.05 9-85 o Jo- 05 9.9 5 8.2 7.9 5 6.3 6.6 10 7.0 6.6 10 4.6 4.9 15 6 -4 5-5 X 5 3-8 4-i 20 5-7 4-5 20 3.3 3.5 30 4-4 30 2.8 40 3.2 ... 40 ... 2.4 SILVER Mono Chlor ACETATE CH 2 ClCOOAg. One liter aqueous solution contains 12.97 grams CH 2 ClCOOAg at 16.9. (Arrhenius) SOLUBILITY OF SILVER MONO CHLOR ACETATE AT 16.9 IN AQUEOUS SOLUTIONS OF: Silver Nitrate. Sodium Chlor Acetate. Gms. AgN0 3 per Liter. Gms. CH 2 ClCOOAg per Liter. Gms. CH 2 ClCOONa per Liter. Gms. CH 2 ClCOOAg per Liter. o.o 9 .6 17.0 12-97 10.05 7-55 O-O 3-88 7-77 !5-53 12.97 10.05 8.16 6.02 31.07 58.26 4.19 3.26 SILVER Di Propyl ACETATE AgC 8 H 15 O 2 . 100 gms. H 2 O dissolve 0.123 m - AgC 8 H 15 O 2 at 11.7, and 0.190 gm. at 72. (Fiirth Monatsh. Ch. 9. 311, '88.) 279 SILVER ACETATES SILVER Methyl Ethyl ACETATE Ag.CH 3 .CH 2 .CH(CH 3 )COO. SILVER Di Ethyl ACETATE Ag.[(C 2 H 5 ) 2 CH.COOj. SILVER Tri Methyl ACETATE Ag.(CH 3 ) 3 CCOO.* SOLUBILITY OF EACH WATER. (Sedlitzky Monatsh. Ch. 8, 563, '87; Keppish Ibid, g, 589, '88; Stiassny Ibid. 12, 601, '91.) Gms. per 100 Gms. H2O. Gms. per 100 Gms. H2O. I/ . Ag.C 5 H 9 O 2 . AgC 6 H n 2 . AgC 5 H 9 O 2 * It . AgC 5 H 9 2 . AgQHnOs. AgC6H 9 O 2 * o I .112 0.402 1. 10 50 I .602 0-536" i-47 IO I .126 0.413 I - I 5 60 1.827 0-585 i-57 20 I.l82 0.432 1.22 70 2.093 0.643 1.68 30 1.280 0.458 I .22 80 2.402 i. 80 40 I .420 0.494 I -37 SILVER BENZOATE C 6 H 6 COOAg. One liter of aqueous solution contains 1.763 gms. C 6 H 5 COOAg at 14.5, and 2.607 gms. at 25. (Holleman Z. physik. Ch. 12, 129, '93; Noyes and Schwartz Ibid. 27, 287, '98.) SOLUBILITY OF SILVER BENZOATE AT 25 IN AQUEOUS SOLUTIONS OF: Nitric Acid (N. and S.). Chlor Acetic Acid (N. and S.). Millimols^per Liter. Grams per Liter. Millimols per Liter. Grams per Liter. HN0 3 . COOAg. HN 3- COOAg. C1COOH. COOAg. C1COOH. COOAg, o.o 0.01144 o.o 2.607 -o 0.01144 o.o 2.607 0.004435 0.01395 0.280 3.195 0.00394 0.01385 0.371 3.172 0.00887 0.01698 0.559 3-889 0.00787 o 01612 0.744 3.691 0.00892 0.01715 0.562 3.926 0.01574 0.02093 1.487 4.792 0.01774 0.02324 1.118 5.321 0.02674 0.03071 1.686 7-031 One liter of cold alcohol dissolves 0.169 g m - C 6 H 5 COOAg; one liter Of boiling alcohol dissolves 0.465 gram. (Liebermann Ber. 35, 1094, '02.) SILVER BORATE AgBO 2 . One liter of aqueous solution contains about 9.05 gms. AgBO 2 at 25. (Abegg and Cox Z. physik. Ch. 46, n, '03.) SILVER BROMATE AgBrO 3 . SOLUBILITY IN WATER. t. Gms. AgBrO 3 per Liter. Authority. 2O I .586 (Bottger Z. physik. Ch.46, 602, '03.) 24.5 I.9II (Noyes Z. physik. Ch. 6, 246, '90.) 25 I . 68 (Longi Gazz. chim. ital. 13, 87, '83.) SOLUBILITY OF SILVER BROMATE IN AQUEOUS AMMONIA AND NITRIC ACID SOLUTIONS AT 25. (Longi.) Grams AgBrOs per Solvent. 1000 cc. Sol. 1000 Gms. Sol. Ammonia Sp. Gr. 0.998=5% 35 .10 35-54 Ammonia Sp. Gr. 0.96 =10% 443.6 462.5 Nitric Acid Sp. Gr. 1.21 =35% 3.81 3.12 SILVER BROMATE 280 SOLUBILITY OF SILVER BROMATE AT 24.5 IN AQUEOUS SOLUTIONS OF: Silver Nitrate (Noyes). Potassium Bromate (N.). Normal ^Content. Gms. per Liter. Normal Content. Cms, per Liter. AgN0 3 . AgBr0 3 .' AgNO 3 . AgBrO 3 . KBrO 3 . AgBrO 3 . KBrO 3 . AgBrOs- o.o 0.0081 o.o 1.911 o.o 0.0081 o.o 1.911 0.0085 0.0051 1-445 I - 20 3 0.0085 0.00519 1.42 1.225 0-0346 0-0022 5.882 0.510 0-0346 0.00227 5.78 0-536 SILVER BROMIDE AgBr. SOLUBILITY IN WATER. t . Gms. AgBr per Liter. Authority. 2O O - 000084 (Bottger Z. physik. Ch. 46, 602, '03.) 25 O .OOOI37 (Abegg and Cox Z. physik. Ch. 46, xi, '03.) 100 O .00370 (Bottger Z. physik. Ch. 56, 93. '06.) (See also Holleman Z. physik. Ch. 12, 129, '93; Kohlrausch Ibid. 50, 365, '05.) SOLUBILITY OF SILVER BROMIDE IN AQUEOUS AMMONIA SOLUTIONS. (Longi Gazz. chim. ital. 13, 87, '83; at 80, Pohl Sitzber. Akad. Wiss. Wien, 41, 267, '60.) Gms. AgBr at 12 per G ras. AgBr at 80 per Solvent. I000 cc . 1000 Gms. o Gms. Solvent. Solvent. Solvent. Ammonia Sp. Gr. 0.998=5% 0.114 0.114 Ammonia Sp. Gr. o . 96 =10% 3 .33-4-0 3-47 Ammonia Sp. Gr. 0.986 ... ... 0.51* I .ot * Dried AgBr. t Freshly pptd. SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF: Ammonia at o. Monq Methyl Amine at 11.5. (Jarry Ann. chim. phys. [7] 17, 363. *99-) (Jarry.) Grams per 100 cc. Solution. Gms. per 100 cc. Solution. AgBr. NH 3 Gas. AgBr. NH 2 CH 3 . AgBr. 3.07 0.080 26.27 1.067 ii. 01 0-07 4.88 0.096 31-26 1-568 13-17 0.12 6.69 0.172 33.89 1.987 15.13 0.16 8.29 0.212 36.52 2.669 J 7-97 - 2 8 11.51 0.349 37-22 2.888 32.58 0.55 J 5-32 0.557 37.70 2.930 35.62 0.73 18.09 0.722 39-26 2.892 43-n 1-27 19.53 0.741 39-95 2.852 48-44 2.89 SOLUBILITY OF SILVER BROMIDE IN AQUEOUS SOLUTIONS OF SODIUM THIO SULPHATE AT 35. (Richards and Faber Am. Ch. J. 21, 186, '99.) Gms. Cryst. Na Thio Sulphate Gms. AgBr Dissolved Mols. AgBr Dissolved per Liter. per Gram of Thio Sulphate. per Mol. of ioo 0.376 0.496 200 0.390 o-5 I S 300 0.397 0.524 400 0.427 0.564 281 SILVER BROMIDE SOLUBILITY OP SILVER BROMIDE IN AQUEOUS SALT SOLUTIONS. (Valenta Monatsh. Ch. 15, 250, '94; see also Cohn Z. physik. Ch. 18, 61, '95.) Gms.AgBr per 100 Cms. Aq. Solution of Concentration: Salt Solution. t. / ^- N 1:100. 5:100. 10: 100. 15:100. 20:100. Sodium Thio Sulphate 20 0.35 1.90 3.50 4.20 5.80 " Calc. by Cohn 20 0.50 2.40 4.59 6.58 8.40 Sodium Sulphite 25 0.04 ... 0.08 Potassium Cyanide 25 ... 6.55 " Calc. by Cohn 25 ... 6.85 Potassium Sulphocyanide 25 ... ... o . 73 Ammonium Sulphocyanide 20 ... 0.21 2.04 5-30 Calcium Sulphocyanide 25 0.53 Barium Sulphocyanide 25 ... ... 0.35 Aluminum Sulphocyanide 25 ... ... 4-50 Thio Carbamide 25 ... ... i .87 Thio Cyanime 25 0.08 0.35 0.72 NOTE. Cohn shows that the lower results obtained by Valenta are due to the excess of solid AgBr used and the consequent formation of the less soluble di salt 3(AgS 2 O 3 Na) 2 instead of the more soluble salt (AgS 2 O 3 Na) 2 Na 2 S 2 O 3 . TOO cc. H 2 O containing 10 per cent of normal mercuric acetate, Hg(C 2 H 3 O 2 )2 + Aq., dissolve 0.0122 gram AgBr at 20. 100 gms. NaCl in cone. aq. solution dissolve 0.474 gm. AgBr at 15. 100 gms. NaCl in 21 per cent solution dissolve 0.182 gm. AgBr at 15. 100 gms. KBr in cone, solution dissolve 3.019 gms. AgBr at 15. 95 gms. NaCl + 10 gms. KBr in --cone. aq. solution dissolve 0.075 gm. AgBr at 15. (Schierholz Sitzber. K. Akad. Wiss. (Vienna) xox. 2b, 4, '90-) SILVER BUTYRATE C 3 H 7 COOAg. SILVER (Iso) BUTYRATE (CH 3 ) 2 CHCOOAg. SOLUBILITY OF EACH IN WATER. Ch. 25, 93, '98; Arrhenius Ibid. II, 396, '93'. R' Ch. 6, 589, '85.) Gms. per 100 Grams H 2 O. Grams per 100 Gms. H 2 O. (Goldschmidt Z. physik. Ch. 25, 93, '98; Arrhenius Ibid, u, 396, '93'. Raupenstrauch Monatsh Ch. 6, 589, '85-) Butyrate. Iso Butyrate. Butyrate. Iso Butyrate. o 0.363 0.796 30 0.561(1.1020.) 1. 060 10 0.419 0.874 40 0.647 17.8 0.432 (A.) ... 50 0.742 1.313 18.8 0.445 (A.) 60 0.848 20 0-484(0.9990.) 0-961 70 0.901 1.670 25 ... (1.0440.) ... 80 1.14 1-898 SILVER BUTYRATE 282 SOLUBILITY OF SILVER BUTYRATE IN AQ. SOLUTIONS OF SILVER ACETATE, SILVER NITRATE AND OF SODIUM BUTYRATE. (Arrhenius Z. physik. Ch. n, 396, '93.) In Silver Acetate at 17.8. G. Mols. per Liter. Grams per Liter CH 3 C 3 H 7 COOAg. COOAg. O-O O-O22I 0.0270 0.0139 0-0506 O.OIO3 G. Mols. per Liter. COONa. O.O O . OO66 0-0164 0.0329 C 3 H 7 COOAg. O.O224 O.OI99 0.0169 O.OI3I CH 3 C 3 H 7 Airivro COOAg. COOAg. o.o 4-32 o.o 4.51 2.71 0.0667 8.45 2.01 O.IOO In Sodium Butyrate at Grams per Liter. G. Mols. O.O228 0.0078 0.0062 18.2. per Liter. ' C 3 H 7 C 3 H 7 ' COONa. COOAg. o.o 4-363 0-73 3-881 1.81 3-296 3:^2 2.555 ' C 3 H 7 COONa. 0-0658 0.263 0-493 C 3 H 7 COOAg. O.OO9I o . 0060 0.0040 O.OO27 In Silver Nitrate at 18.8. G. Mols. per Liter. Grams per Liter. AgNO 3 . o.o 4.445 11 -33 I -52i 17.00 1.209 Grams per Liter. ' C 3 H 7 C 3 H 7 COONa. COOAg. 7.24 1.774 14.47 I-I70 28.96 0.780 54.28 0.526 SILVER CAPROATES Ag(C 6 H n O 2 ). SOLUBILITY IN WATER. (Keppish Monatsh. Ch. 9, 589, '88; Stiassny Ibid. 12, 596, '91; Ibid. 15, 26, '94; Altschul Ibid. 17, ; Kulisch Ibid. 14, 570, '93; Konig 568, '96.) Results in terms of grams salt per 100 grams H 2 O. 2 Methyl Pentan M A Normal Caproate \ C JH *- CH 3 (CH 2 ) 4 COOAg. CHa.CH.CHa ethyl 3 Pentan 4 Methyl Pentan Acid 4 4 Acid CH 3 .CH 2 CH 3 (CH 2 ) 2 CH(CH 3 ) :H 3 CH 2 COOAg. .COOAg. .(CH 2 ) 2 COOAg. .CH( 0.076 (A.) -078(Keppisch) o . l68 (Konig) 0-88o(Kulish) 0.510 (Stiassny) IO 0.085 0-089 0-162 0.858 0-528 20 o.ioo 0.107 0.163 0-849 0-550 30 0.123 O.I3I O.I7O 0.854 o-574 40 0.154 0.161 0.183 0-871 0.602 50 0.193 0.198 0.203 0-902 0-632 60 0.240 0.243 0.229 0.946 0.666 70 0.295 o . 288 o . 263 1.003 0.702 80 o-354 0.300 1.073 0.742 90 0-347 I-I57 SILVER CARBONATE Ag 2 CO 3 . SOLUBILITY IN WATER. t. Gms. Ag 2 CO 3 per Liter. Authority. 15 .031 (Kremers Pogg. Ann. 85, 248, '52.) 25 O -033 (o- 00012 S m ' atoms Ag.) (Abegg and Cox Z. physik. Ch. 46, n, '03.) IOO O 50 (Joulin Ann. chim. phys. [4] 30, 260, '73.) 15 O .85 (inH 2 O sat. with CO 2 ) (Johnson Ch. News, 54, 75, *86.) SILVER CHLORATE AgClO 3 . loo grams cold water dissolve 10 grams AgClO 3 (Vauquelin) ; 20 gms. AgClO 3 (Wachter). 283 SILVER CHLORIDE SILVER CHLORIDE AgCl. SOLUBILITY IN WATER. (A large number of determinations are quoted by Abegg and Cox Z. physik. Ch. 46, n, '03; see also Kohlrausch Ibid. 50, 356, 04- '05; BSttger Ibid. 46, 602, '03, 56, 93, '06.) t. i4- 20. 25. 42. loo*. Gms. AgCl per liter 0-0014 0.0016 0.0020 0.0040 0.0218 SOLUBILITY OP SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF: Ammonia at o. Mono Methyl Amine at 11.5. (Jarry Ann. chim. phys. [7] 17, 342, '99.) (Jarry.) Grams per 100 Grams Solution. Gms. per 100 Gms. Solution. NH 3 Gas. AgCl. NH 3 Gas. AgCl. NH 2 CH 3 . AgCl. i-45 0.49 28.16 6 -59 I. 7 8 0.16 1-94 1.36 29.80 7.09 4-44 0.62 5 .60 3-44 30.19 7-25 5-51 0.83 6.24 4.00 32-43 5-87 7.66 1.32 11-77 4.68 34-5 6 4-77 I3-70 3-29 16.36 5-i8 37-48 3-90 18.69 5-43 36.69 9-93 SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIA. (Longi Gazz chim. ital. 13. 87, '83; at 25, Valenta Monatsh. Ch. 15, 250, '94; at 80, Pohl Sitzber. Akad. Wiss, Wien, 41, 627, '60.) Aq. Ammonia of 0.998 Sp. Gr. = 5% 12 0.233 0.96 Sp. Gr. = 10% 18 7.84 0.986 Sp. Gr. 80 1.49 = 3% 25 1.40 = 15% 25 7.58 SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM CHLORIDE. (Schierholz Sitzber. K. Akad. Wiss. (Vienna) 101, 2b, 8, '90; see also Vogel N. Rep. Pharm. 23, 335, '74. Hahn Wyandotte Silver Smelting Wks., 1877.) Solubility at 15. Solubility at Different Temperatures. Grams per 100 Gms. Solution. t o Gms. per 100 Gms. Solution. frHCl. AgCl. NH4C1. AgCl. 10-00 0-0050 15 26.31 0-276 14 29 o 0143 40 0.329 17.70 0-0354 60 0-421 19-23 0.0577 80 0.592 21.98 O.I 10 90 0.7II 25-31 0.228 IOO 0.856 28-45 0.340 (24.5) no 1-053 Sat. at ord. temp. 0.157 Sp. Gr, of 26.31 % NH 4 C1 solution at iS = i.o8. SILVER CHLORIDE 284 SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OP ALUMINUM AND AMMONIUM SALTS. (Valenta; see also Cohn Z. physik. Ch. 18, 61, '95-) Gms. AgCl per 100 Gms. Solvent of Concentration- Aq. Salt Solution. Aluminum Surphocyanide Ammonium Carbonate Sulphocyanide " Thio Sulphate i . r i : 100. s IOO. 10 : IOO. k 2 5 2 .02 le 25 20 . . . o. 08 O 05 54 te Calc. 20 by Cohn* o-57 0.64 I. 3- 32 07 3 5 .92 .86 * See Note, p. 281. SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS HYDROCHLORIC ACID SOLUTIONS AT ORDINARY TEMPERATURE. (Pierre J. pharm. chim. [3] 12, 237, '47; Vogel.) Solvent. kq. i vol. Cone. HC1 + i vol. H,O Sat.HCl. Sp.Gr.i.i6 5 Gms. AgCl per Liter. Solvent. Gms. AgCl per Liter. S-o ioo vol. sat. HC1 -f 10 vol. H 2 0.56 1.6 + ?o " " 0.18 2.98 " + 30 " " 0.09 ) 5-6o " + 5 " o-35 SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SALT SOLUTIONS. (Vogel; Hahn; Valenta ) Salt Solution. Barium Chloride Barium Chloride Barium Sulphocyanide Calcium Sulphocyanide Calcium Chloride Calcium Chloride Copper Chloride Ferrous Chloride Ferric Chloride Manganese Chloride Magnesium Chloride Magnesium Chloride Magnesium Chloride Strontium Chloride Zinc Chloride Potassium Chloride Potassium Chloride Potassium Cyanide Potassium Cyanide Potassium Sulphocyanide Sodium Chloride Sodium Chloride Cone, of Salt. t. Gms. AgCl per zoo Gms. Solution. 27-32% 24-5 0.057 (H.) saturated ord. temp. 0.014 (Vg.) 10 : 100 2 5 O-2O (VI.) 10 : loo 2 5 0.15 (VI.) 41-26% 24-5 0-571 (H.) saturated ord. temp. 0.093 (Vg.) u 24-5 0-053 (H.) u 0.169 (H.) It O.OO6 (H.) C( ti O.OI3 (H.) 50 : 100 25 0.50 (VI.) 36.35% 24-5 0-53 1 (H.) saturated ord. temp. 0.171 (Vg.) a 0.088 (Vg.) a 24-5 0-0134 (H.) u ord. temp. 0-0475 (Vg.) 24.95% 19.6 0.0776 (H.) 5: ioo 25 2-75 (VI.) 5 ' I0 25 5-24 (Cohn*) 10 : ioo 2 5 O.II (VI.) saturated ord. temp. 0-095 (Vg.) 25-95% 19.6 0.105 (H.) * See Note, page 281. SILVER CHLORIDE SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF POTASSIUM CHLORIDE AT 15. (Schierholz Sitzber. K. Akad. Wiss. (Vienna) 101, 20, 8, '90.) Grams per 100 Grams Grams loo Grams lution. er 100 Grams >lution. KC1. IO.O 14.29 16.66 20-00 AgCl. O-OOO 0-004 O-OOS O.O2O KC1. AgCl. 22-47 0.045 24.0 O.O72 25.0 0.084 Sp. Gr. of 25% KC1 sol,= 1.179 MIXTURES OF SILVER CHLORIDE AND SILVER HYDROXIDE IN EQUI- LIBRIUM WITH AQ. POTASSIUM HYDROXIDE SOLUTIONS AT 25. (Noyes and Kohr J. Am. Ch. Soc. 24, 1144, '02.) Normality Millimols per Liter. Grams per Liter. ofKOH. KC1. KOH," KC1. KOH. Agfcl. o-333 3-4I4 347-8 0.255 10.05 0.4896 0.065 0.598 65.0 0-0446 2.OO 0.0828 SOLUBILITY OF SILVER CHLORIDE IN AQ. SOL. OF SODIUM CHLORIDE. (Schierholz; Vogel; Hahn.) Solubility at 15. Gms. per 100 Gms. Solution. NaCl. IO-O AgCl. O.OO25 14.29 18.18 O.OO7I O.Ol82 21.98 2 3-53 25.64 26.31 0.0439 0.0706 0.103 O.I27 Solubility at Different Temperatures. Cms. AgCl per 100 Gms. Solution in: Sp. Gr. of 26.31% NaCl sol. = 1.207. 109 14% NaCl 26.3% NaCl. 15 0.007 0.128 30 O-OII 0.132 40 0.014 0.158 So 0.023 0.184 70 0-042 0.263 80 0.054 0.315 90 0.069 0.368 100 0.090 0.460 109 0.107 (104) 0.571 SOLUBILITY AT 20, 50, AND 90 (CALC. FROM ORIGINAL). Gms. NaCl per zoo cc. Solution. (Barlow J. Am. Chem, Soc, 28, 1446, '06,) Gms, NaCl Gms. AgCl dissolved per 100 cc. Solution at: 20. O-OOOlS 5 . 0.0016 per 100 cc. Solution. Gms. AgCl dissolved per 100 cc. Solution at: 15-3 20". O.OC3I o . 0090 50. O.OI24 O.OI9I 90. 0.0436 0.0732 90. 3.43 o.ooois o.ooio 0.0067 4.60 0-00025 0.0025 o.oioo 5.75 0.00047 0.0034 0.0135 7.67 0-00125 0-0058 0.0236 Results are also given for the solubility of silver chloride in aqueous sodium chloride solutions containing hydrochloric acid. 23.0 0.0313 0.0889 0.1706 SOLUBILITY OF SILVER CHLORIDE IN AQ. SODIUM NITRATE SOLUTIONS. 30 45-55 Gms. per 100 Gms. H2O. NaNO 3 . AgCl. 0.787 O.OOO86 0.787 O.OOI46 0-787 0.00233 0-787 0.00399 I5-2O a Gms. per TOO Gms. H2O. NaN0 3 . AgCl. ' O-393 0-00096 0-787 0.00133 2.787 0.00253 (Mulder,) SILVER CHLORIDE 286 SOLUBILITY OF SILVER CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM THIO SULPHATE, ETC. (Valenta ; Cohn ; Richards and Faber Am. Ch. J. 2i> 168, '99.) Gms. AgCl per ioo Gms. Aq. Solutions of Concentration: Salt Solution. t. , < i : ioo. 5:100. 10 : ioo. 15:100. 20:100. Sodium Sulphite 25 ... ... 0.44 ... 0.95 Sodium Thio Sulphate 20 0.40 2.00 4.10 5-50 6.10 " Calc. by Cohn* 0.38 1.83 3.50 5.02 6.41 Sodium Thio Sulphate 35 ... 9.08 f Thio Carbamide 25 ... ... 0.83 Thio Cyanime 25 0.40 1.90 3.90 * See Note, page 281. f Gms. per ioo cc. solution (R. and F.). SILVER CHROMATE Ag 2 CrO 4 . One liter of water dissolves 0.026 gm. Ag 2 CrO 4 at 18, and gm. at 25. (Abegg and Cox Z. physik.[Ch. 46, n, '03; Kohlrausch Ibid 50, 356, '04^ SOLUBILITY OF SILVER CHROMATE IN AQUEOUS SOLUTIONS OF NITRATES AT 100. (Carpenter J. Soc. Chem. Ind. 5t 286, '86.) c , Gms. Salt Gms. Ag 2 CrO 4 per ioo cc. HjjO. per ioo cc. Solution. Water o 0.064 Sodium Nitrate 50 0.064 Potassium Nitrate 50 o . 192 Ammonium Nitrate 50 0.320 Magnesium Nitrate 50 0.256 SILVER (Di) CHROMATE Ag 2 Cr 2 O 7 . One liter of aqueous solution contains 0.00019 gram mols. or 0.083 gram Ag 2 Cr 2 O 7 at 15. (Mayer - Ber. 36, 1741, '03) SILVER CITRATE C 6 H 5 O 7 Ag 3 . ioo gms. H 2 O dissolve 0.0277 gm. C 6 H 5 O 7 Ag 3 at 18, and 0.0284 gm. at 2 5. (Partheil and Hubner Archiv. Pharm. 241, 413, ; o 3 .) SILVER CYANIDE AgCN. One liter of aqueous solution contains 0.000043 gm. AgCN at 17.5 and 0.00022 gm. at 20 (by Conductivity Method). (Abegg and Cox Bottger Z. physik. Ch. 46, 602, '03.) SOLUBILITY OF SILVER CYANIDE IN AQUEOUS AMMONIA SOLUTIONS. (Longi Gazz. chem. ital. 139 87, '83.) ioo gms. aq. ammonia of 0.998 Sp. Gr. = 5% dissolve 0.232 gm. AgCN at 12. ioo gms. aq. ammonia of 0.96 Sp. Gr. = 10% dissolve 0.542 gm. AgCN at 18. SILVER SODIUM CYANIDE AgCN.NaCN. ioo gms. H 2 O dissolve 20 gms. at 20, and more at a higher tem- perature, ioo gms. 85% alcohol dissolve 4.1 gms. at 20. (Baup Ann. chim. phys. [3] 53, 468, 58.) SILVER THALLOUS CYANIDE AgCN.TlCN. ioo gms. H 2 O dissolve 4.7 gms. at o, and 7.4 gms. at 16. (Fronmiller Ber 11. 92, '78 J 287 SILVER FLUORIDE SILVER FLUORIDE AgF. 100 gms. H 2 O dissolve 181.8 gms. at 15.8. Sp. Gr. of sol. = 2.61. (Gore Proc. Roy. Soc. 18, 158, '70.) SILVER FULMINATE CAg 2 (NO 2 )CN. One liter of aqueous solution contains 0.075 g*n. C2Ag 2 N 2 O 2 at 13, and O.lSo gm. at 30. (Holleman - Rec. trav. chim. 15, 159, '96.) SILVER HEPTOATE (Onanthylate) AgC 7 H 13 O 2 , SOLUBILITY IN WATER. (Laudau Monatsh. Ch. 14, 709, '93; Altschul Ibid. 17, 568, '96.) t o Gms. AgC 7 Hi 3 O2 per 100 Gms. H 2 O. ^ Gms. AgC 7 H l3 O2 per 100 Gms. H2O. O O -0635 (Landau) O .0436 (Altschul) 50 O . 1652 (Landau) o .0858 (Altschul) 10 0-0817 0.0494 60 0.1906 0.1036 20 0.1007 -555 7 0.2185 0.1351 30 0.1206 0.0617 80 0.2495 0.1688 40 0.1420 0.0714 SILVER IODATE AgIO 3 . One liter of aqueous solution contains 0.04 gram or 0.00014 g- mols. at i8-2o, and 0.05334 gm. or 0.000189 g. mols. at 25. (Longi; Bottger; Kohlrausch; Noyes and Kohr J. Am. Ch. Soc. 24, 1141, '02.) SOLUBILITY OF SILVER IODATE IN AQUEOUS SOLUTIONS OP AMMONIA AND OF NITRIC ACID AT 25. (Longi Gazz. chim. ital. 13, 87, '83.) ioo gms. aq. ammonia of 0.998 Sp. Gr. = 5% dissolve 2.36 gms. AgIO 3 . 100 gms. aq. ammonia of 0.96 Sp. Gr. = 10% dissolve 45.41 gms. AgI0 3 . ioo gms. aq. nitric acid of 1.21 Sp. Gr. = 35% dissolve 0.096 gm. AgI0 3 . SILVER IODIDE Agl. One liter of aqueous solution contains 0.0000028 gm. Agl at 2o-25. (Average of several determinations by Kohlrausch, Abegg and Cox, etc. Holleman gives higher figures.) i liter of aq. ammonia of 0.96 Sp. Gr. = 10% dissolve 0.035 gm. Agl at 12. (Longi.) SOLUBILITY OF SILVER IODIDE IN AQUEOUS SALT SOLUTIONS. ' (Valenta Monatsh. Chem. 15, 250, '94; Cohn Z. physik. Ch. 18, 61, '95.) Gms. Agl per ioo Gms. Aq. Solution of Concentration: Aq. Salt Solution. t. / * N i : ioo. 5 : ioo. 10 : ioo. 15 : ioo. 20 : ioo. Sodium Thio Sulphate 20 0.03 0.15 0.30 0.40 0.60 " Calc. by Cohn* 0.623 2.996 5.726 8.218 10.493 Potassium Cyanide 25 ... 8.28 " Calc. by Cohn* ... 8.568 ... Sodium Sulphite 25 ... ... o.oi ... 0.02 Ammonium Sulphocyanide 20 ... 0-02 0.08 0.13 Calcium 25 ... 0.03 Barium " 25 0.02 Aluminum " 25 0.02 Thio Carbamide 25 ... ... 0.79 Thio Cyan ime 25 0.008 0.05 0.09 * See Note, page 281. SILVER IODIDE 288 SOLUBILITY OF SILVER IODIDE IN AQUEOUS SOLUTIONS OP SODIUM CHLORIDE, POTASSIUM BROMIDE AND OP POTASSIUM IODIDE AT 15. (Schierholz Sitzb. K. Akad. Wiss. (Vienna) 101, ab, 10, '90.) In Sodium Chloride. In Potassium Iodide. Cms. per 100 Gms. Solution. Gms. per 100 Gins. Solution. NlCL AgL ' KL AgL 26.31 0.0244 59.16 53.13 25.00 0.00072 57- J 5 40-0 50.0 25.0 40.0 13.0 In Potassium Bromide. |3 3 \ ' 33 Gms. per 100 Gms. Solution. 2 5 ' z '75 KBr Agl 21-74 1-576 30.77 0.132 20-0 O 80 ioo gms. sat. silver nitrate solution dissolve 2.3 gms. Agl at 11, and 12.3 gms. at b. pt. ioo gms. pyridine dissolve o.io gm. Agl at 10, and 8.60 gms. at 121 . (von Laszcynski Ber. 27, 2285, '94.) SILVER MALATE C 4 H 4 O.Ag.. ioo gms. H 2 O dissolve 0.0119 gm. at 18, and 0.1216 gm. at 25. (Partheil and Hiibner Archiv. Pharm. 241, 413, '03.) SILVER NITRATE AgNO 3 . SOLUBILITY IN WATER. (Etard Ann. chim. phys. [7] 2, 526, '94; Kremers Pogg. Ann. 92, 497, '54; Tilden and Shenstone Phil. Trans. 23, '84.) Grams AgNOg per ioo Gms. Grams AgNO 3 per ioo Gms. Solution. Water. Solution. Water. 5 48 (Etard) . . ... 50 79 (Etard) 82 455 o 53 55 122 60 81.5 84 525 10 62 63 170 80 85.5 87 669 20 68 69 222 ioo 88.5 90^ 952 25 70.5 72 257 120 91 95 1900 30 7 2 -5 75 3oo 140 93-5 40 76-5 79 376 160 95 ioo gms. 2HNO 3> 3H 2 O dissolve 3.33 gms. AgNO 3 at 20, and 16.6 gms. at 100. ioo gms. cone. HNO 3 dissolve 0.2 gm. AgNO 3 . (Schultz Zeit. Chem. [2] 5, 531, '69.) MUTUAL SOLUBILITY OF SILVER NITRATE AND SODIUM NITRATE IN AQ. ETHYL ALCOHOL. (Hissnik Z. physik. Ch. 32, 557, 'oo.) Results at 25. Results at 50. (In Aq. Alcohol of rf, 0.945 = 37 wt. %.) (In Aq. Alcohol of dn 0839 - 75 wt. %.) Gms. per ioo Gms. Sol. Wt. per cent in Mix Crystals. Gms. per too Gms. Sol. Wt. per cent in Mix Crystals. AgN0 3 - NaN0 3 . AgN0 3 . NaNO 3 . AgN0 3 . NaNO 3 . AgN0 3 . NaNOa". 47-32 O O IOO o.o 29 .78 O o IOO o.o 44-01 8 >7 8 99-1 0-9 27 9 2 5 99 5 0-5 3 6. 7 8 20 .42 42.9 57-i 26 4 4 .2 99 3 0-7 29.97 23 .2 33-6 66.4 23 o 6 3 42 9 57-i 24.56 24 .82 27.6 72.4 18 3 7 .1 3 1 .0 69.0 8.02 26 .41 9-9 90.1 9 5 8 3 17 5 82.5 o.o 26 77 o.o 100.0 .0 8 54 .0 100.0 289 SILVER NITRATE SOLUBILITY OF SILVER NITRATE IN ALCOHOLS. (de Bruyn Z. physik. Ch. 10, 783, '92.) ioo gms. abs. methyl alcohol dissolve 3.72 gms. AgNO 3 at 19. ioo gms. abs. ethyl alcohol dissolve 3.10 gms. AgNO 3 at 19. SOLUBILITY OF SILVER NITRATE IN AQUEOUS ETHYL ALCOHOL. (Eder J. pr. Ch, [2] 17, 45. '78.) Sp. Gr.of Aq. Volume Gms. AgNO 3 per ioo Gms. Aq. Alcohol at: Alcoholic per cent t * \ Mixture. Alcohol. 15. 50. 75. 0.815 95 3.8 7.3 18.3 0.863 80 10-3 ... 42.0 0-889 7O 22.1 0.912 60 30.5 58.1 89.0 o-933 5o 35 - 8 0.951 40 56.4 98.3 160.0 0.964 30 73.7 0.975 2O 107.0 214.0 340-0 0.986 10 158-0 ioo gms. of a mixture of i vol. (95%) alcohol + i vol. ether dis- solve 1.6 gms. AgNO 3 at 15. ioo gms. of a mixture of 2 vols. (95%) alcohol + i vol. ether dis- solve 2.3 gms. AgNO 3 at 15. ioo gms. H 2 O sat. with ether dissolve 88.4 gms. AgNO 3 at 15. (Eder.) ioo gms. acetone dissolve 0.35 gm. AgNO 3 at 14, and 0.44 gm, &t Io . (von Lasczynski Ber. 27^ 2285, '94; Naumann Ber, 37, 4332, '04.) SILVER NITRITE AgNO 2 . SOLUBILITY IN AQUEOUS SOLUTIONS OF SILVER NITRATE AT 18. (Naumann and Rucker Ber. 385 2293, '05.) Mols. per Liter, Grams per Liter. Mols. per Liter Grams per Liter. AgNO 3 . AgNO 2 . AgNO 3 . AgNO 2 . AgNO 3 . AgNO 2 . AgNO 3 . AgNO 2 . 0.0000 0.02067 0-000 3-184 0.02067 0.01435 3.512 2.201 0.00258 0.01975 0.439 3.042 0.04134 o. 01168 7.024 1.799 0.00517 0.01900 0.878 2.926 0.08268 0.00961 14.048 1.480 0.01033 0.01689 1-756 2.601 SILVER OXALATE C 2 O 4 Ag 2 . One liter of H 2 O dissolves 0.035 gm. at 18, and 0.0365 gm. at 20. (Bottger; Kohlrausch.) SILVER OXIDE Ag 2 O. One liter of H 2 O dissolves 0.021 gm. at 20, and 0,025 gm. at 25. (Noyes and Kohr; Bottger; Abegg and Cox.) SILVER PERMANGANATE AgMnO 4 . ioo gms. cold water dissolve 0.92 gm.; hot water dissolves more. (Mitscherlich Pogg. Ann. 25. 301, '3*.} SILVER PHOSPHATE Ag 3 PO 4 . One liter ot water dissolves 0.00644 grn. at 20. (Bottger 2. physik. Chi 46, 6oa, '05.) SILVER PBOPIONATE 290 SILVER PROPIONATE C 2 H 6 COOAg. SOLUBILITY IN WATER. (Raupenstrauch Monatsh. Ch. 6- 587, '85; Arrhenius Z. pfaysik. Ch. 1 1, 396, '93; Goldschmidt Ibid. 25, 93. '98.) t o Cms. C 3 H s O 2 Ag t o Cms. CsHsOgAg Gms. C 8 H 6 O2Ag per Liter. per Liter. per Liter. O 5.12 20 8.36(8.48) 50 13.35 10 6.78 25 9.06 70 17-64 18.2 8. 36 (A.) 30 9-93(9-7o) 80 20.30 SOLUBILITY OF SILVER PROPIONATE IN AQUEOUS SOLUTIONS OF: (Arrhenius.) Silver Nitrate at 19.7. Sodium Propionate at i8.2 u Mols. per Liter. Grams per Liter. Mols. per Liter. Grams per Liter. AgN0 3 . Q [HsOaAg. AgN0 3 . C3Hr,O 2 Ag. C 3 H5O2Na. CjjH^OaAg. C3HsO 2 Na. CsHsOsAj o.o O .0471 o.o 8 .519 .0 0.0462 O .O 8.362 0.0133 .0415 2.289 7 5 11 o .0167 0-0393 I .607 7.114 0.0267 0379 4-577 6 .86 o 0333 0.0345 3 .215 6.244 0-0533 O .0307 9-059 5 556 .0667 0.0258 6 .429 4-670 o.ioo O222 16.997 4 .019 o 1333 0.0191 12 859 3-45 6 o .2667 0.0131 25 .718 2.371 .5000 O-OIOI 4 8 77 1.828 SILVER SALIC YLATE C 6 H 4 .OH.COOAg 1,2. One liter of aqueous solution contains 0.95 gm. at 23. (Holleman Z. physik. Ch. 12, 129, '93.) SILVER SUCCINATE C 4 H 4 O 4 Ag 2 . 100 gms. H 2 O dissolve 0.0176 gm. at 18, and 0.0199 g m - a "t 2 5- (Partheil and Hiibner Archiv. Pharm. 241, 413: '03 } SILVER SULPHATE Ag 2 SO 4 . SOLUBILITY IN WATER. (Euler Z. physik. Ch. 49, 314, '04; Wright and Thomson Phil. Mag. Is] 17, 288, '84; Wentzel Dammer's "Handbuch " II, 2, 858; Drucker Z. anorg. Ch. 28, 362, *oi.) t. Gms. Ag 2 SO 4 per Liter, Gm. Mols. Ag 2 SO 4 per Liter. 17 7.70 0.0247 (Euler.) 18 7.28 0-0233 (W. andT.) 25 8.01 0.0257 (D.) ioo 14.60 ... (w.) One liter of aqueous solution in contact with a mixture of silver sulphate and silver acetate contains 3.95 gms. Ag 2 SO 4 + 8.30 gms. CH 3 COOAg at 17. Sp. Gr. of solution = 1.0094. (Euler.) SOLUBILITY OF SILVER SULPHATE AT 25 IN AQUEOUS SOLUTIONS OF: (Drucker.) Sulphuric Acid. Potassium Sulphate. Mols. per Liter. Grams per Liter. Mols. per Liter. Grams per Liter. 'Ag 2 SO 4 . H 2 SO 4 ." Ag 2 SO 4 . H 2 SO 4 ". ' Ag 2 SO 4 . K 2 SO 4 ." Ag 2 SO 4 . K 2 SO 4 . 0.0260 0.02 8. ii 0.98 0.0246 0.02 7-67 i-74 0.0264 0.04 8.23 1.96 0-0236 0-04 7.36 3.49 0-0271 o.io 8.45 4.90 0-0231 o.io 7.20 8.72 0-0275 0.20 8.58 9.81 0-0232 0.20 7-24 17-44 291 SILVER SULPHATE SOLUBILITY OF SILVER SULPHATE AT 18 IN AQUEOUS SOLU- TIONS OF: (Eder J. pr. Ch. [2] 17, 44, '?8.) Gms. per ioo Gms. Solution . Gms. per 100 Gms. Solution. Gms. per 100 Gms Solution. (NH) 2 S04. Ag 2 S0 4 . K 2 SO 4 . Ag 2 SO 4 . Na 2 S0 4 . Ag 2 S0 4 . 5 0.66 6 0.60 12 0.65 15 0.85 18 0.76 32 0.8o SILVER SULPHOCYANIDE AgSCN. One liter of aqueous solution contains 0.0002 gm. at 25, and 0.0064 gm. at 100. (Abegg and Cox Z. physik. Ch. 46, n, '03; Bottger Ibid. 46, 60, '05; 56, 93, '06.) SOLUBILITY OF MIXTURES OF SILVER THIOCYANATE AND POTAS- SIUM THIOCYANATE IN WATER AT 25. (Foote Am. Ch. J. 30, 332, '03.) ms. per ioo Gms. Solution. Mols. per ioo Mols. H 2 O. Solid KSCN. AgSCN. KSCN. AgSCN. Phase. 70-53 44 -3 6 KSCN 66-55 9-32 5i-i3 4.19 KSCN + 2 KSCN.AgSCN 64.47 IO.62 47-98 4-60] 61.25 58-34 11.76 13-55 42.07 38.47 4-72 I 5-23| Double Salt. 2 KSCN.AgSCN 53. 92% KSCN 53-21 50.68 17-53 20-43 33-71 32-52 6. 5 oJ 7.67 2 KSCN.AgSCN+ KSCN.AgSCN 49-43 20.32 30.29 7-28] Double Salt. 32-5 1 18.34 12.26 4-o5f KSCN.AgSCN - 36.9% KSCN 24.68 16.41 7-77 3-2 J 23.86 16.07 7-3 6 2.90 KSCNAgSCN + AgSCN SILVER TARTRATE C 4 H 4 O 6 Ag 2 . ioo gms. H 2 O dissolve 0.2012 gm. C 4 H 4 O 6 Ag 2 at 18, and 0.2031 gm. at 25. (Partheil and Httbner Archiv. Pharm. 341, 413, '03.) SILVER VALERATES AgC 5 H 9 O 2 . SOLUBILITY IN WATER. Normal Valerate I so Valerate CH 3 (CH 2 ) 3 .COOAg. CH 3 .CH(CH 3 ) 2 CH 2 COOAg. (Furth Monatsh. Ch. 9, 3". '88; Sedlitzky Ibid. 8, 563, '87-) Gms. per ioo Gms. H 2 O. Gms. per ioo Gms. H 2 O. i . Normal V. IsoV. O.229 0-177 10 0-259 O-2II 20 0.300 0.246 30 0-349 0.283 40 0.408 0.321 t . Normal V. Iso V. 50 0-474 0-360 60 O-SS 2 O-4OI 70 0-636 0-443 80 . . . 0-486 ioo gms. H 2 O dissolve 0.73 gm. silver valerate at 20. (Markwald Ber. 32, 1089, '99.) SILVER VALERATE 292 SOLUBILITY OF SILVER VALERATE IN AQUEOUS SOLUTIONS OF SILVER ACETATE, SILVER NITRATE AND OF SODIUM VALERATE. (Arrhenius Z. physik. Ch. n 396, '93.) In Silver Acetate at 17.8. In Silver Nitrate at 16.5. Mols. per Liter. Gms. per Liter. Mols. per Liter. Gms. per Liter. CuHgOjjAg. 0-0 0-0067 0.0135 0.0270 0-0505 C 5 H 9 O 2 Ag. CizHgO-jAg. C-jHgOj^ 0-0094 o.o 1.96 0.0070 1.13 1.46 0.0057 2.27 1.19 0.0037 4-54 0.77 0.00265 8.48 0.55 In Sodium Mols. per Liter. . AgNOg. CsHijO^g. AgNOg. ( o.o 0.0094 o.o 0-0067 O.OO68 I.I4 O.OI33 O.OO5I 2.29 0-0267 O.OO3I 4.58 O.IOOO O-OOI2 17.00 Valerate at 18.6. Grams, per Liter. i .96 1.42 1.07 0.65 0.25 C2HgO 2 Na. C 5 H 9 O 2 Ag. o.o 0.0095 O.OI75 O.OO47 0.0349 0.0030 0-0698 0-00l8 0.1395 0.0015 C 2 H 3 2 Na. C5H 9 O 2 Ag. o.o i 986 2.17 0.982 4-32 0.627 8.65 0-376 I7-3 1 0.313 SILVER VANADATE Ag 6 V 4 O 13 . One liter of aqueous solution contains 0.047 gram at 14, and 0.073 gm. at 100. (Carnelly Liebig's Ann. 166, 155, '73.) SODIUM ACETATE CH 3 COONa. 3 H 2 O. SOLUBILITY IN WATER. Interpolated from original. (Schiavor Gazz. chim. ital. 32, II, 532, ? oz.) Gms. CHgCOONa Gms. CH 3 COONa * o per 100 Gms. + o per ioo Gms. Water. Solution. Water. Solution. o 34 25.4 25 53 34-7 10 41 29.1 30 57 36.3 20 49 32.9 40 65 39.4 100 gms. H 2 O dissolve 46.9 gms. CH 3 COONa at 31.5. (Kohler Z. Ver. Zuckerind. 47, 447, '97.) ioo cc. aqueous solution contain 41.11 gms. CH 3 COONa at 10. (Enklaar.) SOLUBILITY OF SODIUM ACETATE IN AQUEOUS SOLUTIONS OF ACETIC ACID. (Enklaar Rec. trav. chim. 20, 183, '01.) Gram Mols. per Liter. Grams per Liter. CH 3 COOH. CHgCOONa. CHgCOOH. CHgCOONa. o 5.0 o-o 411.1 0.085 5.0 5.1 410.3 0.12 5-0 7-2 410.4 SOLUBILITY OF SODIUM ACETATE IN ABSOLUTE ALCOHOL AT ROOM TEMPERATURE. (Bodtker Z. physik. Ch. 22, 510, '97.) ioo gms. alcohol dissolve 1.81 gms. CH 3 COONa or 7.49 gms. CH 3 COONa. 3 H 2 O. 293 SODIUM ACETATE SOLUBILITY OP SODIUM ACETATE IN AQUEOUS ALCOHOL: At Different Temperatures. (Schiavor.) At 1 8. (Gerardin Ann. chim. phys. [4] 5, 158, '65.) Wt. Gms.CHaCOONa per cent Alcohol. per ioo Gms. Aq. Alcohol. * ' S- 2 38.0 8 9 .8 35-9 12 23.0 29.8 19 29.0 27-5 II 38.0 23-5 13 45-o 20.4 15 14.6 18 86.0 3-9 21 91 .0 2.1 23 t . Degree M Gms. per ioo Gms. Alcohol. Alcohol. 'cHaCOONa. CH 3 COONa. 3 H2O.* 8 98.4 2.08 3-45 12 98.4 2.12 3-5 1 19 98.4 2-33 3-86 II 90 2.O7 3-42 13 00 2.13 3-52 15 63 13.46 22.32 18 63 13.88 23-03 21 63 14.65 24.30 23 40 28.50 47.27 100 gms. H 2 O dissolve 237.6 gms. sugar + 57.3 grams CH 3 COONa, or 100 gms. of the saturated solution contain 58.93 gms. sugar + 14.44 gms. CH 3 COONa at 31 . 25. (Kohier.) SODIUM ARSENATE N a3 AsO 4 .i2H 2 O. 100 grams aqueous solution contain 21.1 grams Na 3 AsO 4 .i2H 2 O. (=10.4 gms. NaaAsO 4 ) at 17. Sp. Gr. of solution = 1.1186. (Schiff Liebig's Ann. 113, 350, 'oo.) ioo grams glycerine dissolve 50 gms. sodium arsenate at 15.5. (Pharm. Centralh. No. 30, '81.) SODIUM HYDROGEN ARSENATE Na 2 HAsO 4 .i2H 2 O. ioo gms. H 2 O dissolve 17.2 gms. Na 2 HAsO 4 .i2H 2 O (= 7.3 gms. anhydrous) at o. 56.0 gms. (= 19.89 gms. anhydrous) at 14. Sp. Gr. 1.1722, 37.0 gms. anhydrous at 21, and 140.7 gms. hydrated at 30. (Schiff Liebig's Ann. 113, 350, '60; Tilden J. Ch. Soc. 45, 409, '84-) SODIUM BENZOATE C 6 H 6 .COONa. ioo gms. H 2 O dissolve 62 gms. at 25, and 77 gms. at b. pt. ioo gms. alcohol dissolve 2.3 gms. at 25, and 8.3 gms. at b. pt. (U. s. P.) SODIUM (Tetra) BORATE Na 2 B 4 O 7 .ioH 2 O (Borax). SOLUBILITY IN WATER. (Horn and Van Wagener Am. Ch. J. 30, 347, '"03.) Gms. 1 ^a 2 B40 7 Gms. Na 2 B 4 O 7 t. per ioo Gms. t . per ioo Gms. H>! 3. H 2 O. 5 .3 5 10-5 10 j .6 54 13-3 21. 5 2 .8 55 14.2 30 3 9 56 15.0 37 5 5 .6 57 16.0 45 8 .1 Gms. Na2B 4 Or per ioo Gms. H 2 0. 19.4 22 .O 22. 00 62 65 70 80 90 IOO Transition temperature Na 2 B 4 O 7 .ioH 2 O - imately 62. Sp. Gr. of saturated solution at 15 = 1.032. 20.3 20.7 21.9 24.4 3i-5 41.0 52-5 Na 2 B 4 O 7 .5H 2 O approx- SODIUM BORATES 294 SOLUBILITY OF SODIUM BORATES IN WATER AT 30. (Dukelski Z. anorg. Ch. 50, 42, '06, complete references given.) Solid Phase. NaOH.HjjO Cms. per ioo Gms. Solution. Gms. per ioo Gms. Residue KzO. B 2 O 3 . K 2 0. B 2 3 . 42.0 41-37 5.10 43-54 4.19 38.85 5-55 37-20 II. l8 34-44 3-73 33-52 I0.8o 29-39 2.51 29.63 IO.II 26.13 2-75 27-85 15.21 23.00 3-82 24.91 II .60 16.61 13.69 21 .29 20.64 21.58 4-63 24.52 19.04 20.58 4.69 21 .6l 16.59 I5-32 6.21 19.70 17.84 12.39 9.12 18.05 18.17 8.85 10.49 II .72 2O.62 5-8i 6.94 10.82 21.31 1.88 2.41 7-31 15.50 1.38 5 -*6 7.16 17.44 2 .02 7-79 6.24 16.38 4.08 17.20 8.96 29.20 3-79 15.84 5-68 28.19 2 .26 12.14 5-21 29.19 1.99 11.84 5-74 39.66 1.86 ii. iS i .06 28.78 0.64 6. ii 0.31 3 I - I 9 3-54 N a2 O.B 2 3 .4H20 -HNajO.B208.8H20 Na2O.B 2 03.8H 2 O N a2 O.2B 2 O 3 .ioH 2 O + Na2O.sB2O 3 .i Na 2 O.sB 2 O 3 .ioH 2 O N a2 O.2B2O 3 .ioH 2 O + B(OH) 3 B(OH) 3 ioo gms. alcohol of 0.941 Sp. Gr. dissolve 2.48 gms. sodium borate at 15.5. ioo gms. glycerine dissolve 60.3 gms. at 15.5! and ioo gms. at 80. (U.S. P.) Gaudolphe J. pharm. chim. [4] 22, 366, '75 says that glycerine dissolves its weight of sodium borate at ordinary temperatures. SODIUM BROMATE NaBrO 3 . SOLUBILITY IN WATER. (Kremers Pogg. Ann. 94, 271, 55; 97 5 's6-> t. o 20 40 60 80 100 Gms. NaBrO 3 per ioo Gms. H 2 O 27.5 34-5 5- 2 62.5 75.7 90.9 Sp. Gr. of saturated solution at 19.5 = 1.231. (Geriach.) 2 9 5 SODIUM BROMIDE SODIUM BROMIDE NaBr. 2 H 3 O. SOLUBILITY IN WATER. (Etard Compt. rend. 98, 1432, '84; de Coppet Ann. chim. phys. [5] 30, 411, '83.) LO Grams NaBr per 100 Gms. H 2 O. 20 57-5* 7i -4t 66 79-5 10 72 84-5 20 77 90-3 30 82.5 97-3 40 88.0 105.8 . o. Grams NaBr per 100 Gms. H 2 O. 50 95-112* n6f 00 112 117 80 113 119 IOO 114 121 1 2O 116 124 I4O 118 * Etard. t de Coppet. Transition temperature for NaBr.2H 2 O * NaBr is approximately 50. Kremers Pogg. Ann. 97, 14, '56 gives results which fall near those of de Coppet for the NaBr.2H 2 O, and near those of Etard for the NaBr section tf the curve. SOLUBILITY OF SODIUM BROMIDE IN AQUEOUS SOLUTIONS OF SODIUM HYDROXIDE AT 17. (Ditte Compt. rend. 124, 30, '97.) Gms. per 100 Gms. H 2 O. Gms. per 100 Gms. H 2 O. Gms. per 100 Gms. H2O. NaOH. NaBr'. NaOH. NaBr. NaOH. NaBr. o.o 91.38 17.17 63.06 28.43 48.00 3.26 79-86 19.12 62 .51 36.61 38.41 9.24 68.85 22-35 59.60 46.96 29-37 13-43 64.90 24.74 55-03 54-52 24.76 SOLUBILITY OF SODIUM BROMIDE IN ALCOHOLIC SOLUTIONS. (Rohland Z. anorg. Ch. 18 327, '98; Z. anal. Ch. 44, 252, '05; de Bruyn Z. physik. Ch. 10, 783 '92; Eder Dingl. polyt. 221, 89, '75.) Alcohol. Concentration of Aq. Alcohol. Methyl Alcohol ^15 = 0-799 Ethyl d 15 =o.8io Propyl " 7H 2 O (a). Gms. Na 2 CO 3 Gms. Na 2 CO 3 Gms. Na 2 CO 3 ^ e per 100 Gms. per 100 Gms. per 100 Gms. Water. Solution." Water. Solution. Water. So'ution. 7-0 6. 5 2O-4 16.9 32.0 24.2 5 9.5 6.9 23-2 18.8 35.0 25-9 10 12.5 II. I 26.2 20.8 37.8 27.4 15 16.4 14.1 29-5 22.8 41.2 29.2 20 21.5 17.7 33-5 25-1 45-5 31-3 25 28.2 (29.8*) 22 .O 38.0 27-5 37.8(40.9*) 27.4 43-5 30-3 32.5 46.2 31.6 (32.O46.6 3i-8 35 40 46.2 3 1 - 6 46.1(49.7*) 31-5 (33 -3) 48. 6 (34-5) 5i -3 32-7 33-9 60 46.0(46.4*) 3 J -5 Solid Phase Na 2 CO 3 .H 2 O 80 45.8(45.2*) 31.4 100 45-5 3 J -3 I0 5 45-2 3 1 - 1 * Epple Dissertation, Heidelberg, p. 26, 1899. Sp. Gr. of solution saturated at 17.5, 1.165 (Hager) ; at 18, 1.172 (Kohlrausch) ; at 23, 1.222 (Schiff) ; at 30, 1.342 (Lunge). See also Wegschroeder and Waller Monatsh. Chem. 26, 685, '05, for Sp. Gr. determinations at other temperatures. SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE AT 15. (Reich.) Gms. per 100 Gms. H 2 0. Gms. NaCl Gms. Na 2 CO 3 per 100 per 100 Gms. Gms. per too Gms. NaCl Gms. N a2 CO 3 Gms. H 2 U. per I00 p^ I00 Gms. NaCl. Na^O, .ioH 2 O Gms. Solution. NaCl Solution. NaCl. Na 2 C03 .ioH 2 0. Gms. Solution. NaCl Solution. o.o 61 .42 0.0 16.42 23.70 39.06 15.96 9.76 4-03 53-86 2.92 14.47 27-93 39-73 18.26 9.62 8.02 48.00 5-8o 12.87 3I-65 41.44 20.06 9-73 12 .02 43-78 8.61 II .62 35-46 43-77 2i-75 7-95 16.05 40.96 11.31 IO.7O 37-23 45.27* 22.46 10.13 19.82 39-46 i3-7i IO.II * Both salts in solid phase. SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF ETHYL AND OF PROPYL ALCOHOL AT 20. (Linebarger Am. Ch. J. 14, 380, '92.) Wt. per cent A1^ U 1 Gms. Na 2 COs per 100 Gms. Sol. Wt. per cent Alt- 1 Gms. Na 2 CO 3 per 100 Gms. Sol. Alcohol. In Ethyl. In Propyl'. Alcohol. In Ethyl. In Propyl, 28 4-4 4 8 0.9 1-3 38 2.7 50 . 84 1.2 44 1.7 1.7 54 0-8o 0-9 46 1.13 1.5 62 0.4 297 SODIUM CARBONATE SOLUBILITY OF SODIUM CARBONATE IN AQUEOUS SOLUTIONS OF ETHYL ALCOHOL. (Ketner Z. physik. Ch. 39, 646, 'oi-'o2.) NOTE. The mixtures were so made that an alcoholic and an aqueous layer were formed, and these were brought into equilibrium with the solid phase. Cms. per 100 Cms. Alcoholic Layer. Gms. per 100 Gms. Aq. Layer. C 2 H 5 OH. Na 2 CO 3 . H 2 O. C 2 HsOH. Na 2 CO 3 . H 2 0. Phase. 35 62 9 o-3 36 .8 I O 32-4 66.6 Na 2 C0 3 .H 2 40 61 .0 0-4 38 .6 I .2 31-9 66.9 " 49 61 -0 0-4 38 .6 I .2 31-5 67-3 " 68 55 .8 0.9 43 3 2 3 28.8 6$. 9 " 3 1 .2 5 2 4 0.8 46 .8 29-3 Na 2 C0 3 . 7 H 2 (b) 9 54 .8 0.7 44 5 I 7 29.8 68.5 " 32 3 56 .1 0.6 43 3 I 5 30.2 68.3 " 33 .2 58 .1 o-5 42 4 I 4 31.0 67.6 " 27.7 Crit. sol. 14% C 2 H 5 OHi 3 % Na 2 CO 3 7 3 % H 2 O 28.2 23.5 7.3 69.2 7.9 l8.6 73.5 Na 2 CO 3 .ioH2O 29-0 3 2 -7 3- 8 6 3-5 4-3 22.7 73.0 29.7 40-0 2.1 57.9 2.9 25.5 71.6 30.6 47.8 1.2 51.0 2.3 27.8 69.9 SOLUBILITY OF Na 2 CO 3 .ioH 2 O IN DILUTE ALCOHOL AT 21. (Ketner.) Grams per loo^Grams Solution. Grams per 100 Grains Solution. Na 2 C0 3 . cSsOH. H^O. Na 2 CO 3 . C 2 H 6 OH. H^. 18.5 0-0 81.5 1.2 39.2 59.6 12.7 6.2 81.1 0.2 58.2 41.6 6.9 15.3 77.8 o.i 67.1 32.8 3-2 26.1 70.7 0-06 73.3 26.64 zoo gms. saturated solution in glycol contain 3.28-3.4 gms. sodium Carbonate. (de Coninck Bull. acad. roy. Belgique, 359, '05.) ioo gms. H 2 O dissolve 229.2 gms. sugar + 24.4 gms. Na 2 CO 3 , or 100 gms. sat. aq. solution contain 64.73 S 1118 - sugar + 6.89 gms. Na 2 CO 3 . (Kohler Z. Ver. Zuckerind. 47, 447, '97.) SODIUM (Bi) CARBONATE NaHCO 3 . SOLUBILITY IN WATER. (Dibbits J. pr. Ch. [2] 10, 439, '74.) o Gms. NaHCOs per ioo Gms Gms. NaHCO per ioo Gms. Water. Solution. Water. Solution. o 6.9 6.5 30 ii. i 10.0 10 8.15 7.5 40 12.7 11.3 20 9.6 8.8 50 14-45 I2 -6 2 5 10-35 9-4 60 16.4 13.8 Sp. Gr. of sat. solution at 16 = 1.069. (Stolba.) ioo gms. alcohol of 0.941 Sp. Gr. dissolve 1.2 gms. NaHCO 3 at 15.5. ioo gms. glycerine dissolve 8 gms. NaHCO 3 at 15.5. SODIUM (Bi) CARBONATE 298 SOLUBILITY OF SODIUM BICARBONATE IN AQUEOUS AMMONIUM BICARBONATE SOLUTIONS SATURATED WITH CO 2 . (Fedotieff Z. physik. Ch. 49, 169, '04.) Solution. NH 4 HC0 3 . NaHCO 3 . 'NH 4 HC0 3 . NaHCOa. O 1.072 i-39 0.58 109.4 48.3 tt o.o 0.82 0-0 69.0 15 1.056 o.o 1.05 O-O 88.0 it i .061 0.29 0.95 23.0 80.0 tt i .065 0.56 0.89 44.0 74.6 ii 1.073 1 .08 0.79 85-7 66.7 it i .090 2.16 0.71 170.6 59-2 30 o.o 1.65 0-0 138.6 (4 2.91 0.83 23.0 70.0 SOLUBILITY OF SODIUM BICARBONATE IN AQUEOUS SOLUTIONS OF SODIUM CHLORIDE SATURATED WITH CO 2 . (Fedotieff; see also Reich Monatsh. Ch. 12, 464, '91.) t o Wt. of i cc. Mols.per loop Gms.H2O Grams per 1000 Gms. H2O. I . Solution. NaCl. NaHCO 3 . NaCl. NaHC0 3 . o O-O 0.82 0-0 69.0 " I. 208 6.0 O.O9 350-1 7-7 15 I .056 o.o 1.05 o.o 88.0 tt 1.063 0.52 0.82 30.2 68.6 tt 1.073 1.03 0-64 60. 1 53-6 tt I .096 2. II 0.41 123-1 34-8 tt I.I27 3.20 0.28 187.2 23.0 tt 1.158 4-39 O.I9 256.9 16.1 tt 1.203 6.06 O-I2 354-6 10. 30 1. 066 O-O I-3 1 0-0 IIO- 2 1.079 1 .02 0-87 59-9 7 2.8 It I .IOO 2.08 0.56 121 .9 47-3 tt I .127 3.18 0.38 186.3 32.0 tt I.I56 4.38 0.27 256.0 22-3 It I.I99 6.12 0.17 358-1 *3-9 45 1.077 o.o 1.65 O-O 138.6 1. 086 1 .04 I .12 60.7 94-o " I.II5 2.65 0.62 155 .2 52.0 " I.I27 3-24 0.52 189.4 43-4 I .155 4-38 0-37 256.1 30-7 " I.I98 6.18 0.23 3 6l -5 loo grams alcohol of 0.941 Sp. Gr. dissolve 5.55 grains sodium sulpho carbonate at 15.5. SODIUM CHLORATE NaClO 3 . SOLUBILITY IN WATER. (Kremers Pogg. Ann. 97, 4, '56.) t o Grams perjoo Grams 1 Grams per ^100 Grams Water. Solution. Water. Solution. o 81.9 45.0 60 147.1 59.5 12 89.3 47-2 80 175-6 63.7 20 99-0 49-7 IOO 232.6 69.9 40 123.5 55-3 I2 <> 333-3 7^-9 299 SODIUM CHLORATE SOLUBILITY OF SODIUM CHLORATE IN AQUEOUS SODIUM CHLORIDE SOLUTIONS AT 20. (Winteler Z. Electrochem. 7, 360, 'oo.) Volume Wt. Grams ger Liter. Volume Wt. Grams per Liter. of Solutions. jsf^CL NaCl6 3 . of Solutions. NaCL NaCl6 3 . .426 5 668 1.365 175 393 .419 25 638 1.345 200 338 .412 50 599 1.319 225 271 405 75 559 1-289 250 197 .398 100 522 1.256 275 120 .389 125 484 1-235 290 78 1-379 150 442 1-217 300 55 TOO gms. H 2 O dissolve 24.4 gms. NaCl + 50.75 gms. NaClO 3 at 12. 100 gms. H 2 O dissolve 11.5 gms. NaClH- 249.6 gms. NaClO 3 at 122. (Schlosing Compt. rend. 73, 1273, '71.) ioo gms. alcohol of 77 Wt. per cent dissolve 2.9 gms. NaClO 3 at 16. (Wittstein.) ioo gms. alcohol dissolve i gm. NaClO 3 at 25, and 2.5 gms. at b. pt. ioo gms. glycerine dissolve 20 gms. NaClO 8 at 15.5. SODIUM CHLORIDE NaCl. SOLUBILITY IN WATER. (Mulder ; de Coppet Ann. chim. phys. [5] 30, 411, '83; Andrae J. pr. Ch. [2] 29, 456, '84; above 100, Tilden and Shenstone Phil. Trans. 23, '84; Berkeley Trans. Roy. Soc. (Lond.) 203 A, 206, '04; Etard Ann. chim. phys. [7] 2, 527, '94, gives irregular results.) to Gms. NaCl per Gms _' NaCl Gms. NaCl. ner Gms. NaCl . ioo Gms. H2O. per ioo g. Sol. t . ioo Gms. H2O. per ioo g. Sol. 35-7* 35 6 3 t 26 .28f 70 37 .8* 37 Sit 27-27t 10 35-2 35 .69 26 .29 80 38 4 38 .00 27-54 20 36.0 35 .82 26 37 90 39 .0 38 5 2 t 27.80 25 36.12 35 .92 26 43 IOO 39 .8 39 "{ 28.12 36-3 36 03 26 -49 118 39 .8 28.46 40 36.6 36 32 26 65 140 42 .1 29.63 50 37-o 36 .67 26 83 160 43 .6 30-37 60 37-3 37 .06 27 .04 1 80 44 9 30.98 * M.; deC. t A. $ B . SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF AMMONIUM CHLORIDE. (Fedotieff Z. physik. Ch. 49, 170, '04.) o Wt. of i cc. Mols. per 1000 Gms. H 2 O. Grams per 1000 Gms. H2O. Solution. ' NH 4 C1. NaCl. N^Cl. NaCT. O ... O-O 6.09 Q.O 35^-3 " I-l85 2-73 4.89 146.1 286.4 15 1.200 o.o 6.12 o.o 357-6 1.191 1.07 5.58 57.3 326.4 1.183 2.22 5.13 Il8.9 300-0 " 1.176 3.48 4.64 186.4 271.6 I.I75 3-72 4-55 198.8 266.8 30 ... o.o 6.16 o.o 360.3 " 1.166 4-77 4-26 255.4 249.0 45 ... o.o 6.24 o.o 365-0 " ... 6.02 4.0 322.1 233.9 SODIUM CHLORIDE 300 SOLUBILITY OF SODIUM CHLORIDE IN HYDROCHLORIC (Engel Ann. chim. phys. [6] 13, 374, '88; Enklaar - At . (Engel.) AQUEOUS SOLUTIONS OF ACID. -Rec. trav. chim. 20, 183, f oi.) At io-io.5. (Enklaar.) g. Mols. per 10 cc. So. Gr. of Gms. per Liter. Mols. per Liter. Grams per Liter. HC1. NaCl. bolution. HC1. NaCl. HC1. NaCl. HC1. NaCl. O-O 54 7 1.207 32.0 0-0 6. II O 35-77 I -0 53 5 1-204 O 365 3*-3 0.27 5-77 9 8 4 33-76 1.8 5 52 2 .202 O .674 30-5 o-35 5-67 12 7 6 33- I 9 5-i 4 8 5 .196 I 859 28.4 o-43 5-59 15 68 32- 7 1 9.28 44.0 .185 3 38 25-7 o-57 5-43 20 78 3i-77 15-05 37 9 173 5 49 22.2 0.72 5-28 26 06 30.89 30-75 23 .5 .141 ii .20 13-7 2 .60 3-42 94 77 20. o i 56-35 6 .1 .119 20 54 3-6 2.80 3-i8 102 i 19.04 3-31 2.74 120 6 16.03 SOLUBILITY OF MIXTURES OF SODIUM CHLORIDE AND OTHER SALTS IN WATER, ETC. t o Gms. per 100 Gms. Solvent. Authority. Solvent. Water Alcohol (40%) 25 Water tt 17 26.4 NaCl+22.iNH 4 Cl* 17 34-5 " + 4.iBaCl 2 38-3 " +2 9 . 5 KN0 3 25 38-5 " +41-14 " . 80 39.81 " +168.8 " 25 I5-78 " +13-74 " 20 30-54 " +I3-95KC1 j, 25 28.90 " +16.12 " j (Karsten.) (Soch J. Physic. Ch. 2, 46, '98.) (Quoted by Euler Z. physik. Ch. 49, 315. '04-) * Sp. Gr. of solution at 17 = 1.179. SOLUBILITY OF MIXTURES OF SODIUM CHLORIDE AND POTASSIUM SULPHATE IN WATER AT VARIOUS TEMPERATURES. (Precht and Wittgen Ber. 15, 1666, '82.) 4.0 Grams per 100 Grams H 2 O. f o Grams per 100 Grams H 2 O. ' NaCl K 2 S0 4 KCl NaCl K 2 S0 4 KCl 10 33 4 8 .1 3 .2 60 36 4 xx .9 2-7 20 34 .0 8 9 3 .1 70 36 .6 12.8 3-2 30 34 .6 9 .6 2 9 80 36 .0 12.3 5 - 1 40 35 .2 10 4 2 .8 90 35 9 12.4 7.0 50 35 .8 ii .1 2 .8 100 35' 6 12.6 8.8 SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM BICARBONATE SATURATED WITH CO 2 . (Fedotieff.) Grams per 10000 Gms. HsO. t Wt. of i cc. Mols. per ipoo Gms. H; V Solution. NaHCO 3 . NaCl. ' o . . . 0-0 6.09 a 1. 208 O.O9 6.0 15 1.203 o.o 6.12 1.203 0-12 6.06 30 1.196 O-O 6.16 ft I.I99 0-17 6.12 45 1.189 o-o 6.24 tt 1.198 0.23 6.18 NaHC0 3 . NaCl. o.o 356 3 7-7 35O.I o.o 357-6 IO-O 354-6 0-0 360.3 13 9 358.1 o.o 356-0 0.23 361-5 3 oi SODIUM CHLORIDE SOLUBILITY OP SODIUM CHLORIDE IN AQUEOUS SODIUM HYDROXIDE SOLUTIONS. (Engel; Winteler Z. Electrochem. 7, 360, 'oo.) At o (Engel). At 20 (Winteler). Mg.Mols . per 10 cc. Sp. Gr. of Solutions. Grams per Liter. NaOH. NaCl." Gms. per Liter g x Gr. of lutions. Na 2 0. NaCl. " NaOH. NaCl. So O 54 7 I .207 o.o 320 .0 IO 308 .200 4 .8 49 38 I .221 38-4 288 9 50 297 .230 6 73 47 .21 I .225 53-8 276 .2 100 253 250 10 .41 42 38 I 2 3 6 183.2 247 9 J 5o 213 .270 M .78 39 55 I .249 118.2 231 4 200 I 39 305 30 5 24 95 I 295 244.0 146 .0 300 112 330 37 .88 19 3o I 314 303-0 112 9 400 61 375 53 25 9 .41 I .362 426,. o 55 .0 500 30 425 640 18 .490 SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF SODIUM NITRATE AND VICE VERSA. (Bodlander Z. physik. Ch. 7, 361, '91; Nicol Phil. Mag. [5] 3L 369, '91; results at 25 by Soch J. Physic. Ch. 2, 46, '98.) NaCl in Aqueous NaNO 3 . NaNO 3 in Aqueous NaCl. Results at 15.5 (B.). Results at 15 (B.). Sp. Gr. of Gms. per ioo cc. Sat. Solution. SD. Gr. of Gms. per ioo cc. Sat . Solution. Solutions. NaNO 3 . H 2 O. NaCl." Solutions. NaCl. H 2 0. NaNO 3 . I .2025 88 47 31 78 3720 74 .82 62.38 I 2 305 7-53 87 63 27 .89 3645 4-0 75 .69 5 6. 7 6 I .2580 13.24 86 25 26 3 1 3585 7.24 75 7i 52.09 I .2810 21.58 82 .66 2 3 .98 3530 II .36 76 .86 47-08 I .3090 28.18 80 .42 22 30 3495 15-33 76 .96 42.66 I 3345 33-80 79 25 20 .40 3485 I7.8l 77 .14 39-90 I 3465 37-88* 77 37 19 .40* 3485 18.97* 77 J 5 38.73* I 3465 37.64* 77 34 J 9 .67* 1.3485 19.34* 77 49 38.02* Results at 20 (N.). Grams per ioo Grams H 2 O. Grams per ioo Grams H 2 O. o NaNO 3 35.91 NaCl 14.17 " 32.82 " 28.33 " 29.78 42.50 " 26.91 " 54- 6 3 5 24.92 * o NaCl 87.65 NaNO 3 6-5 13.0 19.5 77-34 68.50 " 60.49 " ioo gms. H 2 O dissolve 43.66* gms. NaNO 3 + 26.58* gms. NaCl at 25. ioo gms. H 2 O dissolve 121.6* gms. NaNO 3 + 17.62* gms. NaCl at 80. ioo gms. aq. alcohol of 40 wt. per cent dissolve 22.78 gms. NaNO 3 -f 10.17 gms. NaCl at 25. * Indicates solutions saturated with both salts. SODIUM CHLORIDE 302 SOLUBILITY OF SODIUM CHLORIDE IN ALCOHOLS. (At 18.5, de Bruyn Z. physik. Ch. 10, 782, '92? Rohland Z. anorg. Ch. iB, 327, '08.) Gms. NaCl Gms. NaCl t. Alcohol. per ioo t. Alcohol per ioo Gms. Alcohol. Gms. Alcohol 18.5 Abs. Methyl 1.41 room temp. Methyl ^15= 0.799 I -33 " Ethyl 0.065 Ethyl ^ 5 =0.81 0.176 " Propyl d l6 =0.816 0.033 SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS ETHYL ALCOHOL SOLUTIONS. (Bodlander Z. physik. Ch. 7, 317, '91; Taylor J. Phys. Ch. i, 723, '97; also Bathrick Ibid. I, 159. '96.) Results at 11.5 (B.). Results at 13 (B.). Sp. Gr. of Gms. per ioo cc. Solution. Sp. Gr. of Gr ns. per ioo cc. So lutio n. Solutions. CzHeOH . H 2 0. NaCl. Solutions. C 2 H 5 OH. H 2 0. NaCl. 1-2035 O 86.62 31 73 I .2030 O 88.70 31 .60 I . 1865 2.86 86.14 29 .66 I 1348 II .Si 78.41 23 .26 I.I7IO 5-41 83 -93 27 77 I ,1144 15 99 74.64 2O .81 I.I548 7-93 81.50 26 05 I .0970 19 39 71-45 18 .86 I-I350 10.84 78-78 24 .28 I .0698 24 95 69.80 16.23 I.I390 II .22 78.62 23 65 I 0295 32 33 57 -96 12 .66 I. 1088 16.85 73-40 2O 63 .9880 40 33 49-34 9 .13 9445 49 .28 38-54 5 93 9075 57 .91 29-37 3 47 .8700 63 ,86 21 .62 i 52 .8400 72 ,26 II .24 50 Results at 30 and at 40 (T.) Wt. per ( Alcohol in S< :ent A alvent. t30, Gms.Ni iCl per ioo Gms. At 40 ', Gms. NaCl per ioo Gms. Solution. Water. Solution. Water. 26.50 36-05 26 .68 36.38 5 24-59 34-29 24 79 34.69 10 22 .66 32-57 22 .90 33-oo 20 19.05 29.40 19 .46 30.20 30 15-67 26.53 16 .02 27.25 40 12.45 23.70 12 75 24-37 50 9-34 20.60 9 .67 21 .42 60 6.36 16.96 6 65 17.82 70 3-36 12-75 3 -87 13.10 80 1-56 7 95 i .69 8.68 90 o-43 4-30 o 5 5.10 ioo gms. alcohol of 0.9282 Sp. Gr. = 54.0% by wt. dissolve at: 4 10 13 23 32 33 44 51 6o c 10.9 ii. i 11.43 "-9 I2 -3 I2 -5 I 3- 1 J 3 8 14 i gms. NaCl (Gerardin Ann. chim. phys. [4] 5, 146, '56.) ioo gms. of a mixture of equal parts of 96% alcohol and 98% ether dissolve o.n gm. NaCl. (Mayer Liebig's Ann. 98, 205, '56.) 3 o 3 SODIUM CHLORIDE SOLUBILITY OF SODIUM CHLORIDE IN AQUEOUS SOLUTIONS OF: Glycerine at 25. (H. and K. Ibid. 45. 267, '05.) Acetone at 20. (Herz and Knoch Z< anorg. Ch. 41, 318, '04.) cc. Acetone per 100 cc. Solvent. O 10 20 30 32 ) Lower layer 308 . 5 87 j Upper layer 88 90 Impurities about 1.5%. 100 gms. sat. solution in glycol contain 31.7 gms. NaCl at 14.8. (de Coninck Chem. Centralb. 76, II, 883, '05.) ioo gms. H 2 O dissolve 236.3 gms. sugar + 42.3 gms. NaCl at 31.25, or ioo gms. sat. aq. solution contain 62.17 gms. sugar + 11.13 g ms - NaCl. (Kohler Z. Ver. Zuckerind. 47, 447, '9?-) NaCl per ioo cc. Solution. Wt. per cent Glycerine in Solvent. NaCl per ioo cc. Solution s p. Gr. of olution. tfillimols. Grams. Millimols. Grams. 37 9 3 1 47 o. o 545 6 31. 93 .1960 64 .6 27 18 13 . 28 501 .z 29 3i .2048 94 .8 23 10 25- 98 448 4 26 23 2133 30 .1 19.32 45 36 37 .2 21 66 .2283 08 5 18 05 54 23 333 9 19 54 .2381 7 7 o 45 83 84 220 .8 12 91 1.2666 7 3 o 43 IOO 00* 167 .1 9 .78 1.2964 4-3 0.25 *Sp. Gr. of Glycerine, 1.2592. SODIUM CHROMATES (Mono, Di, etc.) SOLUBILITY IN WATER. (Mylius and Funk Wiss. Abh. p. t. Reichanstalt 3, 451, 'oo; see also Salkowski Ber. 34, 1948, '01.) Sodium Mono Chromate. Sodium Di Chromate. Gms. Na 2 Mols. Na 2 + o CrO 4 per CrO 4 per Solid t ioo Gms. ioo Mols Phase. Gms. Na 2 Mols. Na 2 o Cr 2 O 7 per Cr) 7 per ioo Gms. ioo Mols. Solid Phase. Solution. H 2 0. Solution. H 2 0. O 24 .07 3 .52 Na 2 CrO 4 .ioH2O o 61 .98 II .2 Na.jCr207.2H2* IO 33 .41 5 55 17 63 .82 12 .1 " 18* 40 .10 7 43 18:] : 6 3 .92 12 .16 " 18, 5 41 65 7 94 34 5 67 36 14 .2 " 19 5 44 .78 9 .01 52 71 . 7 6 17 4 * 21 47 .40 10 .00 72 76 9 22 .8 " 25 .6 46 .08 9 52Na 2 CrO 4 .4H 2 O 81 79 .8 27 .1 " 3 r 5 47 05 9 -90 93 81 .19 29 .6 NazCraOr 36 47 .98 10 .2 98 81 25 2 9 .8 " 40 48 97 IO .6 Sodium Tri Chromate. 45 50 .20 II " Gms. Na< Mols. Na 49 54 5 5 50-93 52.28 II 12 5 .2 " t. Cr 3 O, per too Gms. Solution. Cr 3 10 pe'r ioo Mols. H 2 Solid Phase. 59 5 53 39 12 7 O 80 03 J 9 9 65 55 23 13 7 Na2Cr0 4 15-1 \ 80 44 20 4 " 70 55 .15 13 .6 18 80 .60' 20 56 M 80 55 53 13 .8 55 82 .68 23 7 IOO 55 74 14 .0 99 85 78 2 9 9 " *Sp. Gr. of sat. sol. at 18 = 1.432. tSp. Gr. of sat. sol. at 18 = 2.059, |Sp. Gr. of sat. solution at 18 = 1.745. SODIUM CHROMATES 34 Sodium Tetra Chromate. Cms. o 16 18* 22 per 100 Gms. Solution. 72.96 74.19 74-60 76.01 Mols. Na 2 Cr 4 O, 3 per loo Mols.H 2 O. 10-5 II .2 11.27 12-3 Solid Phase. Na 2 Cr 4 O l3 . 4 H 2 * Sp. Gr. of sat. solution at 18= 1.926. Tetra Sodium Chromate. Gms. Mols. t Na 4 Cr0 6 Na 4 Cr0 5 Solid ' per looGms. Solution. per zoo Mols.H 2 O. Phase O 33-87 4-II 1 ^CrOg.i 10 35-58 4.42 " i8t 37-50 4.8l M 27.7 40.09 5-38 " 37 45-13 6.62 M t Sp. Gr. of sat. solution at 1 8 = 1.446. SOLUBILITY OF SODIUM CHROMATES IN WATER AT 30. (Schreinemaker Z. physik. Ch. 55, 91, '06.) Composition in weight per cent : Of Solution. Of Residue. Solid Phase. NaOH.H 2 O NaOH.H 2 O + Na 2 CrOi Na 2 Cr0 4 %Cr0 3 . %Na 2 0. %Cr0 3 . %Na 2 0. O 42 2.00 41.44 5-83 42.64 2.04 40.89 4-23 35-5 1 27.52 36.57 6.64 32-34 27.72 34.60 15 .19 27.06 37-07 32.20 IO.22 29-39 I5-48 28.41 8-93 28.49 18.09 26.89 8.62 26.91 13.12 23.91 18-57 25.92 18.44 22.86 . . . 19.26 22.98 21.54 25-3I 17.84 24.21 26.24 24.98 28.82 17.88 31-97 23-47 38.93 16.30 40-70 20.83 48.70 16.49 47-49 19-75 50.68 15-72 58.08 13.89 62.76 I7-38 66.13 13.70 69.48 16.06 65-98 14.15 69.46 15.15 68.46 10.95 73-88 13-38 66.88 9-85 71.27 10.67 70.06 11.85 83-95 9-57 69.04 11.04 81.80 6.43 67.84 9.81 82.85 5-42 64.48 4-5 1 79-49 2.71 62.28 o.o IOO-OO Na 2 Cr0 4 N^CrOs.iaHijO 5 .i 3 H 2 + Na 2 Cr0 4 . 4 H 2 N a2 CrO 4 . 4 H 2 O zH 2 O + Na-jCrsOio-HzO Na 2 Cr30 10 .H 2 O Na 2 Cr 3 Oio.H 2 O + Na 2 Cr 4 Q, 3 4H 2 O Cr0 3 100 gms. of a saturated aqueous solution contain at 30: 46.627 gms. Na 2 CrO 4 , or 100 gms. H 2 O dissolve 87.36 gms. Na 2 CrO 4 . 66.4 gms. Na 2 Cr 2 O 7 , or 100 gms. H 2 O dissolve 197.6 gms. Na 2 Cr 2 O T . 100 gms. absolute methyl alcohol dissolve 0.345 gm. Na 2 CrO 4 at 25. (de Bruyn Z. physik. Ch. 10, 783, '92.) 305 SODIUM CITRATE SODIUM CITRATE 2C 3 H 4 (OH)(COONa) 3 .nH 2 O. 100 gms. H 2 O dissolve 90.9 gms. citrate at 25, and 250 gms. at b. pt. (U.SP.) SODIUM (Ferro) CYANIDE Na 4 Fe(CN) 6 . SOLUBILITY IN WATER. (Conroy J. Soc. Chem. Ind. 17, 104, '98.) t 20. 42. 80. 98.5*. Gms. Na 4 Fe(CN) 6 per ioo gms. H 2 O 17.9 30.2 59.2 63.0 SODIUM FORMATE HCOONa. SOLUBILITY IN WATER. (Groschuff Ber. 36, 1788, '03.) Gms. Mols. Gms. Mols. t o HCOONa HCOONa Solid t HCOONa HCOONa Solid " per ioo Gms. per i oo Mols. Phase. per ioo Gms per ioo Mols. Phase. Solution. H 2 O. Solution. H 2 O. 20 22.8o 7.82 HCOONa. 3 H 2 O 25.5 $0.53 27.0 HCOONa. 2 H 2 O O 30.47 1 1. 6 " l8 49.22 25.65 HCOONa + 15 41.88 19.1 29 50.44 26.9 18 44-92 21.6 " 54 53-80 30.8 l8 44-73 2I -4 HCOONa.2H2O 74.5 56.82 34.8 21 46.86 23.3 100.5 6l -54 42-35 23 48.22 24.65 123 66.20 51-8 Sp. Gr. of the saturated solution of the dihydrate at 18= 1.317. SOLUBILITY OF SODIUM ACID FORMATE (EXPRESSED AS NEUTRAL SALT) IN AQUEOUS SOLUTIONS OF FORMIC ACID. (Groschuff.) Gms. Mols. Gms. Mols. t o HCOONa HCOONa Solid t o HCOONa HCOONa Solid per ioo Gms. per ioo Mols. Phase, * per ioo Gms. per ioo Mols. Phase. Solution. H 2 0. Solution. HjzO. O 22.35 J 9'5 HCOONa.HCOOH 45.5 38.85 43.! HCOONa 25.5 29.62 28.45 7o 41-27 47-5 66.5 41.08 47.1 85 43.09 51.2 SODIUM FLUORIDE NaF. ioo gms. sat. aq. solution contain 4.3 gms. NaF at 18. Sp. Gr. of Solution = 1.044. (Mylius and Funk Ber. 30, 1718, '97.) SOLUBILITY OF SODIUM FLUORIDE IN AQUEOUS SOLUTIONS OF HYDROFLUORIC ACID AT 21. (Ditte Compt. rend. 123, 1282, '96.) Grams per 1000 Grams HgO. Grams per 1000 Grams H 2 O. o.o HF 41. 7 NaF 83-8HF 22. 9 NaF io. o " 4i-4 " 129-7 " 23-8 " 45.8 " 22.5 " 596.4 " 48-8 " 56.5 " 22.7 " 777-4 ' 81.7 SODIUM FLUO SILICATE Na 2 SiF 6 . ioo gms. H a O dissolve 0.65 gm. at 17.5* and 2.45 gms. at 100. (Stolba Z. anal. Ch. u. ioo, '72.) SODIUM HYDROXIDE 306 SODIUM HYDROXIDE NaOH. SOLUBILITY IN WATER. (Pickering J. Ch. Soc. 63, 890, '93; Mylius and Funk (Dietz) Wiss. Abh. p. t. Reichaastalt 3, 450, 'oo.) t Gms. NaOH per TOO Gms. Solid Phase. Gms. NaOH t. per TOO Gms. Solid Solution . Water. Solution. Water 7 .8 8 -0 8 7 Ice 20 52 .2 109 NaOH.H 2 20 16 .0 I 9 .1 30 54 3 119 " -28 19 .0 23 5 Ice + NaOH. 7 H2O 40 56 3 129 " -24 22 .2 28 5 NaOH.7H 2 O + NaOH.sH 2 O 50 59 .2 145 41 ~I7 7 24 5 32 5 NaOH. 5 H 2 + NaOH^HaO a 60 63 5 174 " O 29 .6 42 .0 NaOH. 4 H 2 O a 6 4 369 222 3 "f-pt + 5 32 .2 47-5 NaOH. 4 H 2 a + NaOH 3 *H 2 61 .874 .2 288 NaOH.HoO + NaOH 10 34 5 1 5 NaOH. 3 *H 2 80 75 .8 313 NaOH (?) 15 5 38 9 63 53 f. pt. no 78 5 365 M 5 45 5 83 5 NaOH.siHzO + NaOH^H-zO 192 83 9 521 " 12 50 7 103 .0 NaOH. 2 H 2 O + NaOH.H 2 O Sp. Gr. of sat. solution at 18 = 1.539. For determinations of the Sp. Gr. of sodium hydroxide solution, see Kohlrausch Wied. Ann. i, 1879; Wegschnider and Waller Monatsh. Chem. 26, 685, '05. SODIUM IODATE NaIO 3 . SOLUBILITY IN WATER. (Gay-Lussac; Kremers Pogg. Ann. 97, 5, '56.) t. o. 20. 40. 60 80. 100. Gms. NaIO 3 per 100 gms. H 2 O 2.5 9 15 21 27 34 SODIUM IODIDE NaL2H 2 O. SOLUBILITY IN WATER. (de Copper Ann. chim. phys. [5] 30, 411, '83; see also Etard Compt. rend. 98, 1434, '84; and Kremers Pogg. Ann. 97, 14, '56.) Grams Nal per 100 Gms. Solution. 72.0 73-6 74.6 74.6 74-7 t Grams Nal per 100 Gms Solid Water. Solution. Phase. 20 148.0 59-7 NaI. 2 H 2 O O 158.7 61 .4 " IO 168.6 62.8 " 20 178.7 64.1 tc 25 184.2 64.8 M 30 190.3 65.6 " 40 205.0 67.2 II 50 227.8 69-5 Solid Phase 60 65 NaI. 2 H 2 Nal 70 80 100 1 2O 140 75-6 76.3 Water. 256.8 278.4 293 294 296 302 3 IO 3 2I SOLUBILITY OF SODIUM IODIDE IN SEVERAL SOLVENTS. de Bruyn Z. physik. Ch. 10, 783, '92; at ord. temp., Rohland Z. anorg. Ch. 18, 327, '98; Walden Z. physik. Ch. 55, 713. 7i8, '06.) Gms. Nal Gms. Nal per 100 Gms. per 100 Solvent. Solution. Gms. Solvent. ^ * j- 22.5 43-i Acetomtnl 22.09 J 8.43 ord. temp. 58.8 Propionitril 9.09 6.23 22.5 77.7 ord. temp. 83.3 ord. temp. 26.3 (At 22.5 Solvent. Absolute Ethyl Alcohol d l5 0.810 Ethyl Alcohol Absolute Methyl Alcohol d 15 o. 799 Methyl Alcohol d ls o. 816 Propyl Alcohol Solvent. Acetonitril Propionitril Nitro Methane Acetone Furfurol ato. 22.09 9.09 0.34 0.48 very soluble 25.10 307 SODIUM MOLYBDATE SODIUM MOLYBDATE Na 2 MoO 4 . SOLUBILITY IN WATER. (Funk Ber. 33, 3697, 'oo.) Gms. Mols, Gms. Mols. Na 2 MoO 4 Na 2 MoO 4 ,. . Na 2 MoO 4 Na 2 MoO 4 c ,. , t . per 100 per 100 p S"J| t . per too per 100 * lld Gms. Mols. Fhase - Gms. Mols. Phase " Solution. H 2 O. Solution. H 2 O. O 30-63 3 . 86 Na 2 MoO 4 .ioH 2 O 15.5 39-27 4 33.83 4.47 18 39.40 5.70 6 35-58 4.83 32 39.82 5.78 9 38.16 5.39 51.5 41-27 6.14 IO 39-28 5 . 65 Na 2 MoO 4 .2HaO IOO 45 '57 7 -32 zoo gms. H 2 O dissolve 3.878 gms. sodium tri molybdate Na 2 Mo 3 O 10 at 20 , and 13.7 gms. at 100. (Ullik Liebig's Ann. 144, 244, '67.) SODIUM NITRATE NaNO 3 . SOLUBILITY IN WATER. Trans. Roy '75; " " (Mulder; Berkeley Trans. Roy. Soc. (Lond.) 203 A, 211, '04; see also Ditte Compt. rend. 80, 1164, ;; Maumee Ibid. 58, 81, '64; Etard Ann. chim. phys. [7] 2, 527, '94-) Gms. NaNO 3i per 100 Gms. Mols. per t <> Gms. NaNO 3 per 100 Gms. Mols. per Solution. Water. Liter. Solution. Water. Liter. o 42.2 72.9-73.0* 6.71* 80 59.7 148.0-148.0* 10.35* 10 44.7 80.8-80.5 7.16 ioo 64.3 180.0-175.8 11.30 20 46.7 87.5- 88.0 7.60 120 68.6 218. 0-208. 8t 12.22! 25 47.6 91.0- 92.0 7.80 180 78.1 356.7 30 48.7 94.9-96.2 8.06 220 83.5 506.0 40 50.5 102.0-104.9 8.51 225 91.5 1076.0 50 52.8 112.0114.0 8.97 3i3m.pt. 100.0 oo 60 54.9 122.0-124.0 9.42 * Berkeley. t up - SOLUBILITY OF SODIUM NITRATE IN AQUEOUS SOLUTIONS OP NITRIC ACID AT o. (Engel Compt. rend. 104, 911, '87; see also Schultz Zeit. Ch. [2] 5, 531, '62.) Equivalents per 10 cc. Solution. Sp. Gr. of Grams per ioo cc. Solution. NaN0 3 . HNOY Solutions. NaNO 3 . HNO7- 66.4 o i-34i 56-5 o.oo 63.7 2.65 1.338 54.2 1.67 6o-5 5-7 I.33I 51-48 3-59 56.9 8.8 1.324 48.42 5.55 52.75 12-57 1.312 44.88 7.92 48.7 16.9 I-308 41-44 10-65 39-5 2 7- I - 2 9 I 33-6i 17-02 35.1 3 2 - 2 5 J - 28 5 29.86 20.33 31.1 37- 2 5 1.282 26.46 23.48 23.5 48.0 1.276 20.0 30.26 18.0 57.25 1.276 15.32 36.09 12.9 71.0 1.291 10.97 44-76 SODIUM NITRATE 308 SOLUBILITY OF MIXTURES OF SODIUM NITRATE AND POTASSIUM NITRATE IN WATER AT 20. (Carnelly and Thomson J. Ch. Soc. 53, 799, '88.) Per cent NaNO 3 in Mixtures Gins. per 100 Gms. H 2 O. Used. NaN0 3 . KNO 3 . 100 86.8 o 90 96.4 13.2 80 98.0 38-5 60 90.0 47-6 50 66.0 40-0 Per cent NaN0 3 in Mixtures Gms. per too Gms. H 2 0. Used. NaN0 3 . KNOa. 45-7 53-3 34-7 40 45-6 35-5 2O 20.8 33-3 10 9-4 3i-5 o O-O 33-6 ioo gms. H 2 O dissolve 24.9 gms. NaCl + 53.6 gms. NaNO 3 at 20. (Riidorff Ber. 6, 484, '73; Karsten; Nicol Phil. Mag. [5] 3L 386, '91.) SOLUBILITY OF SODIUM NITRATE IN AQUEOUS SOLUTIONS OF SODIUM HYDROXIDE AT o. (Engel Bull. soc. chim. [3] 6, 16, '91.) .Sp. Gr. of Solutions. I -341 I-338 1-333 1.327 i .326 1-332 i .401 SOLUBILITY OF SODIUM NITRATE IN ALCOHOLS. ioo gms. abs. methyl alcohol dissolve 0.41 gm. NaNO 3 at 25. ioo gms. abs. ethyl alcohol dissolve 0.036 gm. NaNO 3 at 25. (de Bruyn Z. physik. Ch. 10, 783, '92.) SOLUBILITY OF SODIUM NITRATE IN AQUEOUS ETHYL ALCOHOL AT DIFFERENT TEMPERATURES. (Bodlander Z. physik. Ch. 7, 317, '91; Taylor J. Physic. Ch. i, 723, '97; Bathrick Ibid, i, 162,796 ) Results at 13 (B.). Results at 16.5 (B.). Milligram Mols. per 10 cc. Solution. Na 2 O. NaN0 3 . o.o 66.4 2-875 62.5 6.1 57-15 12-75 47-5 26.0 29-5 39-o 17-5 45-88 13 -!9 60.88 6.05 Grams per ioo cc. Solution. NaOH. NaN0 3 . o.o 56.50 2.30 53 -!9 4.89 48.63 IO.2I 40.42 20.83 25 .IO 31.25 14.89 36. 7 6 II .22 48-75 5- J 5 >p. Gr. of Gms. per 100 cc. Solution. So.Gr.of Gms. per 100 cc. Solution. solutions. C 6 H 5 OH. H 2 0< NaNO 3 . Solutions. C 6 H 5 OH. H 2 O. NaN0 3 . .3700 O o 75 34 61 66 3745 o.o 75 25 62.20 3395 3 .08 73 53 57 34 .3162 6.16 70 .82 54-64 .3120 6 .01 7i .81 53 39 .2576 II .60 68 .IO 46.06 .2845 8 30 70 85 49 30 .2140 16.49 65 .04 39-87 .2580 IO .91 69 47 45 42 .1615 22.17 61 .67 32-3 1 2325 13 77 67 .12 42 36 0855 32.22 S 2 .92 23-41 .2010 16 .46 66 .16 37 .48 1-0558 37-23 48 50 19.85 i .0050 43-98 42 .78 13-74 0.9420 52.60 32 J 3 9-47 0.9030 6o-OO 2 5 65 4-65 0-8610 63.16 21 3i 1.63 39 SODIUM NITRATE Results at 30 (T.] Results at 40. (Bathrick.) Wt. per cent Alcohol in Gms. NaNO 3 per 100 Gms. Solvent. Solution. Water- O 49-10 96-45 5 46.41 9 I - I 5 10 43-50 85 -55 20 37-42 74-75 30 65.10 40 25.14 55-95 50 18.94 46-75 60 12.97 37-25 70 7 .8l 28.25 90 I .21 12.25 Wt. "per cent Alcohol. O 8.22 26.0 36.0 42.8 55-3 65-1 77-o 87-2 Gms. NaNOt per 100 Gms. Aq. Alcohol. 104.5 90.8 73-3 6l.6 48-4 40.6 27 18 i i 9-4 4.2 SOLUBILITY OF SODIUM NITRATE IN AQUEOUS SOLUTIONS OP ACETONE. Results at 30. (Taylor.) Results at 40. (Bathrick.) Wt. per cent Acetone in Gms. NaNO 3 per 100 Gms. Wt. per cent Gms. NaNOg per 100 Gms. Solvent. Solution. Water. Acetone. Aq. Acetone. 49-10 96.45 0-0 105 5 46.96 93-20 8-47 9 1.2 9.09 45 - 11 90.40 16.8 78.3 20 40.10 83-70 25.2 66.4 30 35.08 77.20 34-3 57-9 40 29.80 70.75 44.1 46.2 50 24-34 64.40 53-9 32-8 60 18.55 59-95 64.8 23.0 70 13 -is 50.50 76.0 10.8 80 7.10 38.20 87.6 3- 2 90 1.98 20-20 SODIUM NITRITE NaNO,. 100 gms. H 2 O dissolve 83.3 gms. at 15. (Divers J. Ch. Soc. 75, 86, "99.) 100 gms. abs. methyl alcohol dissolve 4.43 gms. NaNO 2 at 19.5. 100 gms. abs. ethyl alcohol dissolve 0.31 gm. NaNO 2 at 19.5. (de Bruyn Z. physik. Ch. 10, 783. 02.) SODIUM RHODO NITRITE Na 6 Rh 2 (NO 2 ) 12 . 100 gms. H 2 O dissolve 40 gms. at 17, and 100 gms. at 100. (Leidie Compt. rend, in, 107, '90.) SODIUM OXALATE C 2 O 4 Na 2 . SOLUBILITY IN WATER. (Souchay and Leussen Liebig's Ann. 99, 33, '56; Pohl J. pr. Ch. 56, ai6, '52.) t. 15-5. 2I-8 - 100. Gms. Na 2 C 2 O 4 per 100 gms. H 2 O 3 . 22 3 . 74 6 .33 SODIUM OXALATE 310 SOLUBILITY OP MIXTURES OF SODIUM OXALATE AND OXALIC ACID IN WATER AT 25. (Foote and Andrew Am. Ch. J. 34, 154, '05.) Gms. per 100 Gms. Mols. per 100 Mols. Solution. H 2 0. Na 2 C 2 4 . H 2 C 2 O 4 . Na 2 C 2 O 4 . IO-2O ... 2 .274 . . . H 2 C 2 O 4 .2H 2 O 10.50 0.83 2.370 0.130 H2Cj8O4.2H2O4-HNaCisO4.H2O 9.15 0.71 2.032 ^25 ^234 -I* Double Salt, HNaC.04^20 O-47 3. 2O 0-098 0.42 3.85 . 090 . 541 HNaC 2 O 4 .H 2 O + Na-jC^ 3.60 ... 0.502 Na 2 C 2 O 4 SODIUM p NITEO PHENOL C 6 H 4 .ONa(i).NO 2 ( 4 ). SOLUBILITY IN WATER AND IN AQUEOUS NORMAL SOLUTIONS OF NON ELECTROLYTES. (Goldschmidt Z. physik. Ch. 17, 154, '95.) Gms. CH4.ONa(i).NO2(4) per 100 Gms. Solution in: 1> Water. Alcohol. Urea. Glycerine. Acetone. Propionitril. Acetonitril . Urethane 23.7 5-597 5-6I5 6.244 6.188 6.225 6.257 6.065 6.520 28.6 6.721 6.874 7.489 7.440 7.498 7.571 7.328 7.88 9 30.6 7.256 . . . 33.6 8.125 8.318 9-000 9.025 9.025 9.066 8.886 9-57 35-9 8.851 36-1 8.883 9.683 9.688 9.665 9.9II 9.667 10.248 40.2 9.881 10. 147 10.666 10.777 10.695 10.905 10.667 TI -379 45-2 n-235' 11.513 12.068 12.229 12.869 12.730 13.133 13-555 13-785 The solid phase is C 6 H 4 ONa.NO 2 . 4 H 2 O below 36, and C 6 H 4 ON ai NO 2 .2H 2 O above 36 in each case. SODIUM PHOSPHATES, Ortho, Hydrogen, and Pyro. SOLUBILITY OF EACH IN WATER. (Mulder; Poggiale.) 4,0 Gms. per loo^Gms. Water. 4,0 Gms. per 100 Gms. H 2 O. NasPO 4 . Na 2 HPO 4 . Na 4 P 2 6 7 . NaaPO 4 . Na 2 HPO 4 . Na 4 P 2 6 7 . o 1.5 2.5 3.16 40 31.0 63.9 13-50 10 4-1 3-9 3-95 50 43-o 82.5 17.45 20 II. O 9.3 6.23 00 55-0 91.6 21.83 25 15.5 15-4 8.14 80 81.0 96.6 30.04 30 20.0 24.1 9.95 100 I08.0 99-0 40-26 Solid phases, Na 3 PO 4 .i2H 2 O, Na 2 HPO 4 .i2H 2 O and Na 4 P 2 O 7 .ioH 2 O respectively. Sp. Gr. of saturated solution of Na 2 HPO 4 at 15= 1.047, 100 gms. alcohol of 0.941 Sp. Gr. dissolve 0.33 gm. sodium phos- phate at 15.5. SODIUM (Double) PHOSPHATE, FLUORIDE Na 3 PO 4 .NaF.i 2 H 2 O. 100 gms. water dissolve 12 gms. of the double sodium salt at 25, and 57,5 gms. at 70. Sp. Gr. of solution at 25= 1.0329; at 70= (Briegleb Uebig's Ann. 97- 9S. 's6-> SODIUM PHOSPHITES SOLUBILITY OP SODIUM PHOSPHITES, ETC., IN WATER. Salt. Hydrogen Phosphite Formula. (NaH)HP0 3 . 2 JH 2 Gms. Salt per 100 Gms. H 2 0. Authority. Hypophosphate Hydrogen Hypophosphate Tri Hydrogen " Di Hydrogen " Di Hydrogen " Hypophosphite Hypophosphite SODIUM SELENATE Na 4 P 2 O 6 .ioH 2 Na 3 HP 2 6 . 9 H 2 NaH 3 P 2 O 63 H 2 Na 2 H 2 P 2 O 6 .6H 2 O Na 2 H 2 P 2 O 6 .6H 2 (NaH)HPO 2 .H 2 O (NaH)HPO 2 .H 2 O o 10 42 cold cold cold b. pt. b. pt. 66 193 3-3 6.7 2.2 2O. O 100. O 830 ( (Amat. Compt. . omp. rend. 106, 1351, '88.) (Salzer Liebig's Ann. a xx. 1,^82.) ] (Salzer Liebig's ) Ann. 187, 33L '77 (U. S. P.) Gms. Mols. Na 2 SeO 4 per 100 Gms. Na 2 SeO 4 per 100 Mols. Solid Phase. Solution. H 2 0. 11.74 1.26 Ni i2Se0 4 .ioI 25.01 3.18 M 29.00 3-90 u 36.91 5-57 44 39.18 6-13 44 Na 2 SeO 4 .ioH 2 O. SOLUBILITY IN WATER. (Funk Ber. 33, 3697, 'oo.) Gms. Mols. t o Na 2 SeO 4 per Na 2 SeO 4 per Solid loo Gms. loo Mols. Solution. HoO. Phase. O H-74 1.26 Na2SeO 4 .ioH2O 35-2 45-47 7-94 15 25.01 3.18 " 39.5 45.26 7.87 18 29.00 3.90 50 44-49 7-^3 25.2 36.91 5.57 75 42.83 7.14 27 39 .18 6.13 100 42.14 6.93 30 44-05 7.50 Sp. Gr. of saturated solution at 18 = 1.315. Na 2 Se0 4 SODIUM ST ANN ATE Na 2 SnO 3 .3H 2 O. 100 gms. H 2 O dissolve 67.4 gms. at o, and 61.3 gms. at 20. Gr. of solution at o = 1.472; at 20 = 1.438. Sp. SODIUM SULPHATE Na 2 SO 4 . (Ordway Am. J. Sci. [2] 40, 173, '65.) SOLUBILITY IN WATER. (Mulder; Lowel Ann.chim. phys. [3] 33, 382, '51; Tilden and Shenstone Proc. Ro; 35. 345. '83; Etard Ann. chim. phys. [7] 2, 527, '94; Funk Ber. 33, 3701, 'oo; Ber] Roy. Soc. (Lond.) 203 A, 209, '04.) Gms. Na 2 SO 4 per Mols. Q ,-j Gms. Na 2 SO 4 per Mols. t. TOO Gms. Na 2 SO*per ? hd t- 100 Gms. Na 2 SO 4 p Solution. Water. Liter (B.). Solution. Water. ^ter (L 4.76 5 o O .31 N a2 S0 4 .ioH20 50 31.8 4 6 7 2.92 5 6.0 6 4 " 60 31.2 45 3 2-83 10 8-3 9 .0 .631 80 3-4 43 7 2.69 15 ii. 8 13 4 IOO 29.8 42 5 2.60 20 16.3 19 4 I 32 1 20 29-5 4 1 95 25 21.9 28 o 140 29.6 42 27-5 25.6 34 .0 it 160 30-7 44 25 30 29.0 40 .8 2 .63 230 31 .7 46 4 30.6 44 o N o 16.3 19 5 32 32-3 47 .8 . . . ' 5 19.4 24 32-75 33-6 50 65 3 .11 10 23.1 30 33 33-6 5o .6 . . . N a2 SO 4 15 27.0 37 35 33-4 .2 ... " 20 30.6 44 40 32.8 48 .8 3 .01 2 5 34-6 53 ... Na,S0 4 NaaS0 4 .7H,0 SODIUM SULPHATE 312 SOLUBILITY OF MIXTURES OF SODIUM SULPHATE AND MAGNESIUM SULPHATE IN WATER (ASTRAKANITE) Na 2 Mg(So 4 ) 2 .4H 2 o. (Roozeboom Rec. trav. chim. 6, 342, '87; Z. physik. Ch. 2, 518, '88.) Solid Phase. Astrakanite Astrakanite -f Na2SO 4 Astrakanite + MgSO 4 Mols. per 100 Grams per 100 t. Mols. H 2 0. Grams ^20. Na 2 S0 4 . MgSO 4 . Na 2 S0 4 . MgSO 4 . 22 2-95 4-70 23-3 31-4 24-5 3-45 3-68 27.2 24.6 30 3-59 3-59 28.4 24.1 35 3-7i 3-7i 29.4 2 4 .8 47 3-6 3-6 28.4 24.1 22 2-95 4-70 23-3 31-4 24-5 3-45 3.62 27.2 24.2 30 4-58 2.91 36.1 I9.I 35 4-3 2.76 33-9 18.44 18.5 3-4i 4.27 43-o 45-5 22 2.85 4-63 35-2 48.9 24-5 2.68 4.76 32-5 5o-3 30 2-3 5-3i 25-9 55-o 35 i-73 5-88 23-5 59-4 SOLUBILITY OF MIXTURES OF SODIUM SULPHATE, POTASSIUM CHLORIDE, POTASSIUM SULPHATE, ETC., IN WATER. (Meyerhoffer and Saunders Z. physik. Ch. 28, 469; 31, 382, '99.) c f> t Mols. per 1000 Mols. H 2 O. f. &T.5L* , * N Solid Phase. Na a C1 2 *4-4 ... 5-42 14-39 5 T - 8 3 6o - 8 0.2 ... 3.35 12.78 50.93 60.36 NaaSO^xoHaO+KCl+NaCl -0.4 ... 3.59 16.38 40.75 53.54 Na 2 S0 4 .ioH 2 0+KCl+K 3 Na(S0 4 ) 2 16.3 ... 4.72 17.58 50.56 63.42 K 3 Na(SO 4 ) 2 +KCl+NaCl 24.8 1.2484 4.37 20.00 48.36 64.01 KsNa(SO 4 )a+KCH-NaCl *l6.3 ... 16.29 9- 16 6l.o6 53.93 K 3 Na(|0 4 ) 2 -hNaCl+Na 2 S0 4 .ioH 2 CH- 24.5 1.2625 14.45 9-90 58.46 53-91 K 3 Na 2 (S0 4 4)2+NaCl+Na 2 S0 4 0.3 ... 2.75 25.77 17.93 40-95 K3Na(S0 4 ) 2 +KCl+K 2 S0 4 25.0 1.2034 2.94 36.20 14.80 48.06 KsNa(SO 4 )2+KCl+K 2 SO 4 *l7-9 1.2474 13.84 0.0 62.57 48.70 Na 2 S0 4 .ioH 2 O+Na 2 SO 4 +NaCl *30.I 1.2890 50.41 10.08 40.33 0.0 K 3 Na(SO 4 ) 2 +Na 2 SO 4 .ioH 2 O+Na 2 SO 4 21.4 ... ... ... 46.61 46.36 NaC1.2H 2 O+Na 2 SO 4 .ioH 2 O -23.7 10.51 39.58 50.09 NaCl. 2 H 2 0+KCl -10.9 ... 1.45 30.68 ... 29.23 KC1+K 2 S0 4 ~3 ... 16.25 10.03 6 - 21 K 3 Na(S0 4 ) 2 +Na 2 SO 4 .ioH 2 O 3 ... 16.24 10.03 6 -2I ... K3Na(S0 4 )2-|-K 2 S0 4 -14 ... 1-39 25.59 8.78 32.94 K 3 Na(S0 4 ) 2 +Na 2 S0 4 .ioH 2 0+KCl -14 ... 1-39 25.59 8.78 32.94 K 3 Na(S0 4 ) 2 +K 2 S04+KCl -23.3 ... 0.41 15.15 44.20 58.97 Na 2 S0 4 .ioH 2 0+KCl+NaCl. 2 HaO * Indicates transition points. SODIUM SGLPHATB SOLUBILITY OP SODIUM SULPHATE IN AQUEOUS SOLUTIONS OP SULPHURIC ACID. (D'Ans, Shepherd and Gunther Z. anorg. Chem. 49, 356-61, '06.) Gms. per 1000 Cms. Solution. Mols. per 1000 gms. Solution. H.SO 4 Na,SO 4 H,SO 4 NaaS04 O.O 219.0 O.O I-54I 28.1 237-4 0.286 1.671 33-2 247-5 0.338 1.742 86.7 320.7 0.884 2.256 154.6 335-8 1.576 2.363 163.5 346.4 1.666 2-437 256.3 297.4 2.611 2.O9I '. Solid Phase. Na 2 SO4-ioH,O Na 2 SO 4 10 H 2 O + Na 2 SO 4 Na 3 H(SO4) -H 2 + Na 2 SO 4 Na 3 H(SO 4 ) 2 + Na 2 S0 4 NaH(SO 4 ) 2 + Na 3 H(SO 4 ) 2 - H a O SOLUBILITY OF SODIUM SULPHATE IN AQUEOUS SOLUTIONS OP SODIUM CHLORIDE AT DIFFERENT TEMPERATURES. Results at 10. (Seidell Am. Ch. J. 27, 52, '02.) Results at 21.5. Results at 27' Sp. Gr. of Gms. per TOO Gms. Sp. Gr. H 2 O. of Gms. per 100 Gms. Sp. Gr. H 2 O. O f Gms. per 100 Gms. Solutions. NaCl. Na 2 S0 4 . Solutions. ' NaCl. Na 2 S0 4 ." Solutions. NaCl. N aa SO 4 . I.oSo O.O 9 .14 1.164 O.O 21 33 .228 0-0 31.10 1.083 4.28 6 .42 .169 9-05 15 .48 .230 2.66 28.73 I .IO2 9.60 4 .76 .199 17.48 13 73 230 5-29 27.17 I.I50 I5-65 3 99 .214 20.41 13 .62 235 7.90 26.O2 I .164 21.82 3 97 243 26.01 15 05 259 16.13 24.83 I .192 28.13 4 *5 244 26.53 14 44 253 18.91 21-39 I .207 30.11 4 34 .244 27.74 13 39 249 19.64 20. 1 1 I .217 32.27 4 59 244 3I-25 10 .64 245 20-77 19.29 1.223 4 75 243 31.80 10 .28 238 32-33 9-53 245 32.10 8 43 .219 33.69 4 73 .212 34.08 2 77 .197 35-46 O .00 Results at 30. Results at 33. Results at 35. 5p. Gr. of Gms. per 100 Gms. SD Gr. HzO. of Gms. per 100 Gms. H 2 0. Sp. Gr. of Gms. per TOO Gms. Solutions. NaCl. Na 2 SO 4 . Solutions. NaCl. Na 2 SO 4 . Solutions. NaCl. Na 2 SO . I.28l 0.0 39 .70 1.329 O.O 48.48 I 324 .0 47-94 1.282 2-45 38 -25 1.323 I .22 46.49 I 2 .14 43-75 .284 S .6l 36 .50 1.318 1.99 45.16 I '256 13 57 26.26 .290 7.91 .96 1-315 2.64 44.09 I 238 18 78 19.74 .276 10.61 31 .64 1.309 3-47 42.6l I .231 31 .91 8.28 .270 12.36 29 .87 .265 12.14 29.32 I 193 35 .63 o.oo .258 15-65 25 .02 237 21.87 16.83 .249 18.44 21 30 234 32.84 8.76 .244 20.66 !9 .06 .217 33-99 4-63 .236 32-43 9 .06 .208 34-77 2-75 SODIUM SULPHATE 314 SOLUBILITY OF SODIUM SULPHATE IN AQUEOUS ETHYL ALCOHOL. (de Bruyn Z. physik. Chem. 32, 101, *oo.) .. Content of Alcohol. Gms. Na 2 SO 4 per 100 Gms. Aq. Alcohol. Gms. per 100 Gms. Solution. Solid H 2 0. C 2 H 5 OH. Na 2 SO 4 . Phase. 15 0-7 12.7 88.7 0-0 II-3 Na 2 S0 4 .ioH 2 O tt 9-2 6. 7 8 5 .I 8.6 6.3 tt 19.4 2.6 78.6 18.9 2.9 tl 39-7 0-5 6o.O 39-5 0-5 tl O.I 4I.I 58.8 o.i tt 72.0 o.o 28.0 72.0 o.o tt o.o 37-4 7 2.8 o.o 27.2 Na 2 S0 4 . 7 H2O tc II .2 16.3 76.5 9-5 14.0 tt 20.6 7.0 74-3 19.2 6.5 tt 30.2 2 .O 68.4 29.6 2.0 25 0-0 28.2 78.1 o.o 21-9 NajSO^ioHaO 10.6 13-9 78.5 9-3 12.2 tl 24.0 4-5 72.8 22.9 4-3 It 54-o 0.4 45-6 54-o 0.4 36 o.o 49-3 67.0 o.o 33 -o N a2 so 4 tt 8.8 29.2 70.6 6.8 22.6 tl 12.8 22.4 71.2 10.5 18.3 11 17.9 15-4 71.1 iS-5 13-4 It J 5-3 71.0 15-7 13-3 It 28.9 5-4 66.5 28.4 5- 1 tl 48.7 0.8 50-9 48-3 0.8 1? o.o 47-9 67.6 o.o 32.4 tt 9.0 27-5 71 .3 7 I 21.6 (I 14-5 19.2 7 i.8 12. 1 16,1 tl 20.6 12.3 70.6 18.4 IO.O ft 31.0 65.6 29-5 4-9 Between certain concentrations of the aqueous alcohol the liquid separates into two layers at 25, 36 and 45. 45 Upper Layer. Lower Layer. Gms. H 2 O. Gms.C 2 HOH. Gms. Na 2 SO 4 . Gms.H 2 O. Gms.C 2 H 5 OH. Gms. Na 2 SO 4 66.5 27-3 6.2 67.4 5-i 27-5 68.1 23-9 8.0 68. 5 6.0 25-5 68. 3 23.1 8.6 68.3 6. 7 25.0 66.6 4-1 29-3 57-7 38-4 3-9 65.0 28. 3 6.7 68.8 5-9 25-3 68.1 21 .2 10.7 68.9 9.4 21-7 61.8 32-9 5-3 65.8 25-3 8.9 68.4 8.8 22.8 66.0 2/1. IO.O 68.6 10. 1 21-3 3*5 SODIUM SULPHATE SOLUBILITY OF SODIUM SULPHATE IN AQUEOUS PROPYL ALCOHOL AT 20. (Linebarger Am. Ch. J. 14, 380, '92.) Gms. CsH 7 OH per ioo Gms. Alcohol-Water Mixture. 42.20 49-77 55 - 6 5 ioo gms. H 2 O dissolve 183.7 m s. sugar + 30.5 gms. Na 2 SO 4 at 31.25, or ioo gms. sat. solution contain 52.2 gms. sugar + 9.6 gms. Na 2 SO 4 . (K6hler Z. Ver. Zuckerind. 47, 447 , '97.) rms. Na 2 SO 4 per ioo Gms. Sat. Solution. Gms. CsH 7 OH per ioo Gms. Alcohol-Water Mixture. Gms. NajS' per ioo Gms. Sat. Solution. 1-99 0.72 60.64 62.81 0-44 0.38 SODIUM (Bi) SULPHATE NaHSO 4 . 100 gms. H 2 O dissolve 28.6 gms. at 25, and 50.0 gms. at 100. 100 gms. alcohol dissolve 1.4 gms. at 25. , 672, '91 > Cms. SrCrO 4 Gms.SrCrO* Solvent. per i oo Solvent. per ipo Cms. Solvent. Gms. Solvent. Water 0.12 Aq. Ethyl Alcohol (29%) 0.0132 Aq. NH 4 C1 (5 %) o . 195 Aq. Ethyl Alcohol (53 %) o .002 Aq. CH 3 COOH(i%) 1.57 STRONTIUM FLUORIDE SrF 2 . One liter of water dissolves 1.87 mg. equiv. or 0.117 gm. SrF 2 at 1 8, by conductivity method. (Kohlrausch Z. physik. Chem. 50, 356, 'o4-'os.) STRONTIUM HYDROXIDE Sr(OH) 2 . SOLUBILITY IN WATER. (Scheibler N. Z. Rubenzuckerind. 7. 257 ; abstract in J. pharm. chim. [5] 8, 540, '83.) Grams per 100 Grams Solution. Grams per TOO cc. Solution. ' SKX Sr(OH) 2 .8H 2 0." SrO. Sr(OH) 2 .8H 2 O. " o 0.35 0.90 0.35 0.90 10 0.48 1.23 0.48 1-23 20 0.68 1.74 0.68 1.74 30 i. oo 2.57 i .01 2.59 40 1.48 3-80 1.51 3-87 50 2.13 5.46 2.18 5.59 60 3.03 7.77 3-12 8.00 70 4-35 "- l6 4-55 JI - 6 7 80 6.56 16.83 7.02 18.01 90 12.0 30-78 i3- 6 4 34-99 100 18.6 47-7 1 22.85 58-61 STRONTIUM IODATE Sr(IO 3 ) 2 . TOO gms. H 2 O dissolve 0.026 gm. at 15, and 0.72-0.91 gm. at I OO. (Gay-Lussac; Rammelsberg Pogg. Ann. 44, 575, '38.) STRONTIUM IODIDE SrI 2 .6H 2 O. SOLUBILITY IN WATER. (Average curve from the results of Kremers Pogg. Ann. 103, 65, '58; and Etard Ann. chim. phys. [?] 2, 528, '74-) Gms. Srl 2 per too Gms Solid t o Gms. Srlg per 100 Gms. Solid ' ' Solution. ' Water. Phase. ' Solution. Water. Phase. O 62.3 165.3 SrI 2 .6H 2 O 90 78.5 365-2 SrI 2 .2H 2 O 20 64.0 177.8 " 100 79-3 383 .1 40 65.7 I9L5 " 120 80.7 4l8.I 60 68.5 217.5 " I 4 ^ 2 -5 47 x -5 80 73.0 270.4 " 175 85.6 594-4 Transition temperature about 90. Sp. Gr. of sat. solution at 20 =- 2.15. 100 gms. saturated solution of strontium iodide in absolute alcohol contain 2.6 gms. SrI 2 at 20, 3.1 gms. at + 4, 4.3 gms. at 39, and 4.7 gms. at 82. (Etard.) 319 STRONTIUM MALATE STRONTIUM MALATE SrC 4 H 4 O 6 . SOLUBILITY IN WATER. (Cantoni and Basadonna Bull. soc. chim. 35, 731. '06.) t Gms. per 100 cc. Solution. t. Gms. per 100 cc Solution- t o Gms. per 100 cc. Solution. 20 0.448 40 I-385 55 2 .460 25 0-550 45 1-743 60 2.821 30 0.752 ' So 2.098 65 3-I48 35 1.036 70 3-3 6 STRONTIUM MOLYBDATE SrMoO 4 . 100 gms. H 2 O dissolve 0.0104 gm. SrMoO 4 at 17. (Smith and Bradbury Ber. 24, 2930. '91.) STRONTIUM NITRATE Sr(NO 3 ) 2 . SOLUBILITY IN WATER. (Mulder; see also Etard for slightly lower results.) Gms. Sr(NO 3 ) 2 per 100 Gms. Solid t o Gms. Sr(NO 3 )? per 100 Gms. Solid 'Solution. Water. Phase. Solution. ' Water, Phase. O 28.3 39.5 Sr(N0 3 ) 2 .4H 2 40 47.7 91.3 Sr(NO3)t 10 35-5 54-9 5o 48-1 92.6 20 41-5 70.8 60 48.5 94 -o 25 44-1 79-o 80 49.3 97.2 30 46.7 87.6 " 100 50.3 101.1 Transition temperature about 31. Sp. Gr. of sat. solution at 20 = 1.44. 100 gms. absolute alcohol dissolve 0.024 gm. Sr(NO 3 ) 2 . 100 gms. rectified spirit dissolve 0.50 gm. Sr(NO 3 ) 2 . (Hill Pharm. J. Trans. [3] 19, 420, '88.) STRONTIUM OXALATE SrC 2 O 4 .H 2 O. One liter of aqueous solution contains 0.52 mg. equivalent SrC 2 O 4 or 0.046 gm. at 18, conductivity method. (Kohlrausch Z. physik. Chem. 50, 356, '04- '05.) SOLUBILITY OF STRONTIUM OXALATE IN AQUEOUS ACETIC ACID SOLUTIONS AT 26-27. (Herz and Muhs Ber., 36, 3715, '03.) Normality Gms. per 100 cc. Solution. Normality Gms. per 100 cc. Solution. of Acetic Acid. CH 3 COOH. Residue SrC 2 4 .H 2 0. of Acetic Acid. CEaCOOH. Residue SrC 2 4 .H 2 O, O-O o.o O.OO9 3-86 23.16 0.0898 0.58 3 -48 0.0526 5-79 34-74 0-0496 i-45 8.70 O.O622 16.26 97 -5 6 O.OO6O 2.89 17-34 0.0642 STRONTIUM SALIOYLATE Sr(C 6 H 4 OH.COO) 2 .2H 2 O. 100 gms. H 2 O dissolve 5.55 gms. at 25, and 28.6 gms. at b. pt. (U. S. P.) joo cc. aqueous solution contain 1.830 gms. anhydrous salt. (Barthe.) 100 gms. alcohol dissolve 1.5 gms. at 25, and 9.52 gms. at b. pt. (U. S. P. ; Barthe Bull. soc. chim. [3] i j, 519, '94.) STRONTIUM SULPHATE 320 STRONTIUM SULPHATE SrSO 4 . One liter of aqueous solution contains 1.24 mg. equivalents or 0.114 gm. SrSO 4 at 18, by conductivity method. (Kohlrausch Z. physik. Chem. 50, 356, '04 '05; Holleman Ibid. 12, 129, '93; Wolfmann Oster. Ung. Z. Zuckerind. 25, 997, '97.) SOLUBILITY OF STRONTIUM SULPHATE IN AQUEOUS SOLUTIONS OF HYDROCHLORIC, NITRIC, CHLORACETIC AND FORMIC ACIDS. (Banthisch J. pr. Chem. [2] 29, 52, '84.) cc. of Aq. Acid con- In Aq. HC1 Gms. per 100 cc. In Aq. HNO 3 Gms. per 100 cc. In Aq.CH 2 ClCOOH Gms. per 100 cc. Sol. In Aq. HCOOH Gms. per 100 cc. O 1 Mg. Equiv. in each case. So' So' [. ' CH 2 C1 COOH. SrS0 4 . Sol 'HC1. SrSO 4 . HN0 3 . SrS0 4 . HCOOH. SrSCv 0-2 18.23 0.161 3I-5 2 0.381 o-S 7.29 0.207 12. 6l 0.307 1.0 3-65 0.188 6.30 O.2I7 94-47 O.O26 46.02 O.O24 2.0 1.82 0.126 3-15 0.138 47-23 0.022 . . . IO.O 0.36 0.048 0.63 0.049 SOLUBILITY OF STRONTIUM SULPHATE IN SULPHURIC ACID SOLUTIONS. r f Gms. SrSO 4 t . w In Per 100 Authority. H2SO <- Gms. Acid. Ord. Concentrated $-68 (Struve Z. anal. Chem. 9, 34, 1870.) " fuming 9.77 91 % O .08 (Varenne and Paulean Compt. rend. 93, 1016, '81.) 70 Sp. Gr. 1 .843 = 99 / 14.0 (Garside Chem. News, 31. 245, '7S-) SOLUBILITY OF STRONTIUM SULPHATE IN AQUEOUS SALT SOLUTIONS. (Virck Chem. Centralb. 402, '62.) In Aq. NaCl. In Aq. KC1. In Aq. MgCl 2 . In Aq. CaCl 2 . (a.) (b.y (a.) (b.) (a.) (b.) (a.) (b.) 8-44 0.165 8. 22 O 193 i-59 o. 199 8.67 0.176 iS-54 0.219 12. 54 193 4-03 o. 2o6 16.51 0.185 22.17 0.181 18. 08 .251 J 3- 6 3 .242 33-70 0.171 (a) = Gms. salt per IOO gms. aq. solution. (6) = Gms. SrSO 4 per 100 gms . solvent. STRONTIUM TARTRATE SrC 4 H 4 O 6 . 3 H 2 O. SOLUBILITY IN WATER. (Cantoni and Zachoder BulL soc. chim. [3] 33, 751, '05.) Gms. Gms. Gms: SrC 4 H 4 O SrC 4 H 4 O 6 SrC^CV t . , 3 H 2 per t . . 3 H 2 O per t . . 3 H 2 O too cc. loo cc. per 100 cc. Solution. Solution. Solution. O O-II2 25 O.224 60 0.480 10 0.149 30 0.252 70 0.580 15 0.174 40 0-328 80 0.680 2O 0-200 50 0.407 85 0-755 32 1 STRONTIUM TARTRATE SOLUBILITY OF STRONTIUM TARTRATE IN AQUEOUS SOLUTIONS OF ACETIC ACID AT 26-27. (Herz and Muhs Ber. 36, 3715, '03.) Normality of Cms, per 100 cc. Solution. Normality of Gms. per 100 cc. Solution. Acetic Acid. CHaCOOH. SrC 4 H 4 O 6 . 3 H 2 O. Acetic Acid. CHgCOOH. o.o o.o 0.227 3.77 21.85 x -o5i o-5 6 5 3-39 o- 6 78 5- 6 5 33-90 0.982 1.425 8.15 0.864 16.89 101.34 0.184 2.85 17.10 0.996 STRONTIUM (Di) TUNGSTATE SrW 2 O 7 . 3 H 2 O. 100 cc. H 2 O dissolve 0.35 gm. at 15. (Lefort Ann. chim. phys. [5] 15, 326, '78.) STRYCHNINE C 21 H 22 N 2 O 2 . SOLUBILITY IN SEVERAL SOLVENTS. (U. S. P.; at 20, Mttller Apoth.-Ztg. 18 258, '03; Schindelmeiser.) Gms. C 2 iH 2 2N 2 O2 Gms. C 2 HazNaOa per 100 Gms. per 100 Gms. Solvent. < * Solvent. - Solution Solvent Solution Solvent at 20. at 25. at 20*. at 25. Water 0.021 0.016 Petroleum Ether 0.0093 Water Sat. with Ether 0.0166 ... Acetic Ether 0.1972 Ether 0.0432 0.0182 Carbon Tetra Chloride 0.158 o. 645(1 7) (S.) Ether Sat. with H 2 O 0.0513 ... Alcohol ... 0.909 Benzene o. 770 o. 666 Amyl Alcohol ... o. 555 Chloroform 100+ 16.6 Glycerine ... 0.25 (15) 100 gms. pyridine dissolve 1.24 gm. C 21 H 2 2N 2 O 2 at 26. (Holty J. Physic. Chem. 9, 764, '05.) SOLUBILITY OF STRYCHNINE NITRATE AND SULPHATE IN SEVERAL SOLVENTS. (U.S. P.) Strychnine Nitrate. Strychnine Sulphate. Gms. per 100 Gms. Solvent at: Gms. per too Gms. Solvent at: Solvent. , ^ 8o o. 25. 80. Water 2.38 12.5 3.23 16.6 Alcohol o . 83 i . 66 (60) 1.54 S-o (60) Chloroform 0.64 ... 0.31 Glycerine 1.66 4.0(15) 22.5(15) SUBERIC ACID C e H 12 (COOH) 2 . SOLUBILITY IN WATER. (Lamouroux Compt. rend. 128, 998, '99.) t. o. 15. 20*. 35*. SO* 65 Gms. C 8 H 12 (COOH) 2 per 100 cc. solution 0.08 0.13 0.16 0.45 0.98 2.22 SUCCINIC ACID 322 . SUCCINIC ACID (CH 2 ) 2 (COOH) 2 . SOLUBILITY IN WATER. (Miczynski Monatsh. Chem. 7, 263, '86; Van der Stadt Z. physik. Chem. 41, 355, '02; Lamouroux Compt. rend. 128, 998, '99; for other concordant results, see Bourgoin Bull. soc. chim. [2] 21, no '74; Henry Compt. rend. 99, 1157, '84.) Gms. Succinic Gms. (CH 2 ) 2 (COOH) 2 per 100 Anhydride (CH 2 )aCOCOO per Mol. per cent. ' Gms. H 2 O. cc. Solution. H 3 O. (CH 2 ) 2 COCOO. 100 Gms. H 2 O. 2.80 2 . 7 8(L.) 2-34 99.58 0.42 10 4-51 4-0 3.80 99-32 0.68 20 6.89 5-8 5-77 98.97 1.03 25 8.06 7-o 6.74 98.80 I .20 30 10-58 8-5 8-79 98.44 1-56 40 16.21 I2 -5 13.42 97.64 2. 3 6 50 24.42 18.0 !9 95 96.53 3-47 60 35.83 24-5 28.77 95 -7 4-93 70 51 .07 40.11 93.26 6-74 80 70.79 54-08 91 .12 8.88 89.4 95-45 70-62 88.71 ii .29 104.8 146.3 . . . IOI .2 84.57 15-43 115.1 188.5 126.8 8l-4 18.6 134.2 335-4 187.8 74.72 25.28 159-5 748.2 . . . 295.2 65.27 34-73 180.6 1839.0 408.5 57-6 42.4 182.8 00 . . . 542-3 50.0 5- 174.4 808.5 40.7 59-3 153-3 2239.0 19.86 80.14 128.0 . . . 8865.0 5-89 94.11 118.8-119 00 o-oo 100.00 SOLUBILITY OF SUCCINIC ACID IN ALCOHOLS AND IN ETHER. (Timofeiew Compt. rend. 112, 1137, '91; at 15, Bourgoin Ann. chim. phys. [5] 13, 405, '78.) Gms. (CH 2 ) 2 (COOH) 2 per 100 Gms. Solvent. / Solvent at: -i- +iS. +21.5. Abs. Methyl Alcohol 10.51 ... 1^9.40 Abs. Ethyl " 5.06 12.59 9.49 9 o% " 7-51 Abs. Propyl 2.11 ... 4-79 Abs. Ether ... 1.265 DISTRIBUTION OF SUCCINIC ACID BETWEEN WATER AND AMYL ALCOHOL AT 20. (Herz and Fischer Ber. 37, 4748, '04.) Millimols iC4H 6 O 4 per 10 cc. Gms. CHeO4 per 100 CC. Millimols iC4HeO 4 per 10 cc. Gms. C 4 H 6 O 4 per 100 cc. Alcohol Layer. 0.1888 0.3643 0.7077 1-440 2-7I5 Aq. Layer. 0.2684 0.5252 I -0373 2.1266 4-0495 Alcohol Layer. O-III4 0.215 0.418 0.850 1.603 Aq. Layer. 0.1584 0.310 0.612 I - 2 55 2.391 Alcohol Layer. 3-899 5- J 99 6-334 7.119 Aq. Layer. 6.0795 8.099 10.170 "555 Alcohol Layer. 2.302 3.069 3-739 4.202 Aq.- Layer. 3-588 4-779 6.000 6.821 323 SUCCINIC ACIE SOLUBILITY OP SUCCINIC ACID IN AQUEOUS ACETONE AT 20. (Herz and Knoch Z. anorg. Chem. 41, 320, '04.) cc. Acetone per C 4 H 6 O 4 per ipo cc. Solution. cc. Acetone per CJIeO* per too cc. Solution 100 cc. Solution. Millimols. Grams. ' 100 cc. Solution. Millimols. Grams. o 107.8 6.363 60 275.7 l6 -27 10 127.4 7.519 70 278.5 16.44 20 155-8 9.194 80 265.3 15.66 3O 186.7 II O2 90 2OI-9 11.91 40 225.4 13.30 loo 51.5 3.04 So 254.3 15.01 SOLUBILITY OP SUCCINIC ACID IN AQUEOUS GLYCERINE SOLUTIONS AT 25. (Herz and Knoch Z. anorg. Chem. 45, 268, '05.) Wt.% Glycerine 4^04 per 100 cc. Solution. Sp. Gr. of Wt.% Glycerine 4^04 per 100 cc. Solution. Sp. Gr. of in Solvent. Millimols. Grams. Solutions. in Solvent. Millimols. Grams. Solutions. O 133 4 7 .874 I O2I3 40 95 105 ..8 6.244 I .II2Q 7-15 128 .2 7 .566 I 0407 48 .70 99-9 5.896 I .1208 20-44 118 3 6 .982 I .0644 69 .20 88.5 I . 1804 31-55 109 7 6 .476 I .0897 IOO .00* 74.6 4.440 I-2530 * Sp. Gr. of Glycerine 1.2555. Impurity about 1.5 per cent. SUCCINIMID C 2 H 4 <>NH. SOLUBILITY IN WATER AND IN ETHYL ALCOHOL. Interpolated from original results. (Spey ers - Am. j. Sci. [ 4 ] 14, 204 , '02 ., In Water. In Ethyl Alcohol. t. Wt. of i cc. Mols. per Gms. per 100 Wt.oficc. Mols.penoo Gms. per 10 Solution. loo Mols. H 2 O. Gms. H 2 O. Solution. Mols.CjjHsOH. Gms.CtH 6 OH o 1.025 1.58 8.69 0.815 0.88 1.89 10 1.035 2.4 14.0 0.809 1.35 2.7 20 1-052 4-0 23.0 0.8o6 2.00 4-1 25 30 40 50 60 70 80 .067 5.9 33.0 0.805 2.5 5.3 .086 8.0 45.0 0.804 3.1 6.8 .120 12.8 70.0 0.809 4.9 10.5 145 17.8 96.0 0.816 7.8 16.0 .167 22.6 124.0 0-835 12.3 26 .189 27.5 152.0 0.873 .204 32.8 0.954 SUCCINIC NITBIL (Ethylene Cyanide) CNCH 2 CH 2 CN. The solubility of succinic nitril in water and also in aqueous sodium chloride solutions at various temperatures has been determined by Schreinemaker (Z. physik. Chem. 23, 439, '97), and the results presented in terms of mols. of nitril per 100 mols. of nitril + H 2 O. The following calculation of these results to gram quantities was made by Rothmund. (Landolt and Bornstein, 3d ed. p. 596, '06.) Gms. CNCH 2 CH 2 CN per 100 Gms. Gms. CNCH 2 CH 2 CN per 100 Gms^ Aq. Layer. Nitril Layer. . Aq. Layer. Nitril Layer. 18.5 10.2 92.0 53.5 33-2 66.4 20 ii. o 91.5 55 40-3 62.8 39 85 .2 55 .4 (crit. temp.) 51 .o 45 22.0 SUGAR 324 SUGAR C 12 H 22 O n (Cane Sugar.) SOLUBILITY IN WATER. (Herzfeld Z. Ver. Zuckcrind. 181, '92; see also Courtonne Ann. chim. phys. [5] 12, 569, '77.) Cms. dzH-BOn per t*. Cms. QaHuOu per ioo Gms. 100 Gms. Solution. Water. Solution. Water. o 64.18 179-2 40 70.42 238.1 5 64.87 184.7 45 7i-3 2 248-7 10 65.58 190-5 50 72.25 260.4 15 66.33 I 97- 74-i8 287.3 20 67.09 203.9 7 76.22 320.4 25 67.89 211.4 80 78.36 362.1 30 68.70 219.5 90 80. 61 415-7 35 6 9-55 228 -4 ioo 82.97 487-2 6p. Gr. of sat. solution at 15 = 1.329; at 25 = 1.340. SOLUBILITY OP SUGAR IN AQUEOUS SALT SOLUTIONS AT 30, 50. AND Interpolated from original results. AND 70. t. 30 ?f It tt tt to it (Schukow Z. Ver. Zuckerind. so, 313, 5 oo.) Gms. Ci2H22Oii per ioo grams EfeO in Aq. Solution of: ) 10 .0 ioo gms. oil of turpentine dissolve 1.35 gms. S at i6,and 16.2 gms. at b. pt. (Payen Compt. rend. 34. 356, '52.) 329 SULPHUR DIOXIDE SULPHUR DIOXIDE SO 2 . SOLUBILITY IN WATER. (Schonfeld Liebig's Ann. 95, 5, '55 Sims Ibid. 118, 340, '6x; Roozcboom Rec. trav. chim. 3. Schonfeld. Vols. SOa (at o and Qms. SO 2 per 760 mm.) per i Vol. IOO Qms, HaO Sims. SOa per i Gm. H,O. Roozeboom. SO 2 Dissolved per i pt. H 2 t. Sat. S0 2 + Aq. HaO. total pressure t . 760 mm. Gms. Vols. t . at 760 mm. pressure. O 68 .86 79 79 22 83 8 0.168 58.7 0.236 5 59 .82 67 .48 19 31 10 0.154 53-9 2 0.218 IO 5 1 38 56 65 16 .21 14 0.130 45-6 4 O.2OI I 5 43 56 47 .28 13 54 20 0.104 3 6 -4 6 0.184 20 36 .21 39 37 II .29 26 0.087 30-5 7 0.176 25 77 32 79 9 .41 30 0.078 27-3 8 0.168 30 25 .82 27 .16 7 .81 36 0.065 22.8 10 0.154 35 21 23 22 49 40 0-058 2O-4 40 17 .01 18 77 5 .41 46 0.050 17.4 12 O.I42 50 0.045 I5 .6 Sp. Gr. of sat. solution at - 1.061 o/-\ ; at 10, 1-055; at 20 i = 1.024. rv i gm. H 2 O dissolves 0.0909 gm. SO 2 = 34.73 cc. (measured at 25) at 25 and 748 mm. pressure. (Walden and Centnerszwer Z. physik. Chem. 42, 462, 'oi-'oa . SOLUBILITY OP SULPHUR DIOXIDE IN SULPHURIC ACID OP 1.84 SP. GR. Interpolated from original results. (Dunn Chem. News, 45, 272, '82.) Sp. Gr. Coefficient Sp. Gr. Coefficient t e . of Sat. Solution. of Absorp- tion (760 mm.). t. of Sat. Solution. of Absorp- tion (760 mm o . . . 53-o 50 1. 8l86 9-5 10 1.8232 35-o 60 1.8165 7.0 20 1.8225 25.0 70 I.8I40 5-5 25 I.822I 21.0 80 1.8112 4-5 30 I.82I6 18.0 90 I .8080 4-0 40 1.8205 13.0 SOLUBILITY OF SULPHUR DIOXIDE IN AQUEOUS SULPHURIC ACID SOLUTIONS. (Dunn; see also Kolb Bull. soc. ind. Mulhouse 222, '72.) Sp. Gr. of Approximate Coefficient t . HsSO* Per cent of Sp. Gr. of t. H 2 S0 4 Approximate Coefficient per cent of Solution H 2 SO 4 . Absorption. Solution. HaSO 4 . Absorption 6. 9 i T 39 20 48 67 15 .2 173 25 3 1 .82 6. 9 i .300 40 45 38 16 .8 .151 21 3 1 56 8.6 i .482 58 39 9 1 14 .8 277 36 30 .41 9.8 i 703 78 29 03 15 .1 458 56 29 .87 5-5 i .067 10 36 78 15 .6 '] .609 70 25 17 6.0 i .102 X 5 3.408 15 O 3 739 81 20 83 For Coefficient of Absorption, see Ethane page 133. SULPHUR DIOXIDE 330 SOLUBILITY OF SULPHUR DIOXIDE IN AQUEOUS SALT SOLUTIONS. (Fox Z. physik. Chem. 41, 461, '02.) Pesults in terms of the Ostwald Solubility Expression. See page 105. Aqueous Solubility Coefficient I of SO 2 in aq. Solutions of Concentrations: ilt Solution. 0.5 Normal 1.0 N. 1.5 N. 2.0 N. 2.5 N. 3.0 N. NH 4 C1 '25=34 58 36 37 38 .06 39 76 41 37 42.78 NH 4 Br '25=36 25 39 .46 42 78 46 .06 49 52-25 NH 4 CNS '25 = 37 .78 42 74 47 .26 5 2 .26 57 .01 61.46 NH 4 N0 3 '25 = 33 .96 35 .07 36 .28 37 .27 38 .01 39-14 NH 4 N0 3 '35=23 35 24 23 24 .78 25 57 26 .66 27-43 (NH 4 ) 2 S0 4 '25 = 33 35 33 .82 34 33 34 95 35 47 35 -96 (NH 4 ) 2 S0 4 '35=22 .91 23 .14 23 49 23 93 24 23 24.60 CdCl 2 .66 30 55 29 .46 28 .16 27 .09 26.06 CdCl 2 '35=21 73 21 23 20 55 20 .02 19 23 18.68 CdBr 2 '25 = 31 .91 31 .01 30 29 .27 28 15 27.46 CdBr 2 '35=21 .88 21 .46 2O .81 20 .60 19 .70 19.17 CdI 2 '25 = 33 27 33 76 34 .16 34 74 34 .98 35-77 CdI 2 '35=22 75 23 .06 23 36 23 23 99 24.30 CdS0 4 '25=3! .11 29 .71 28 .24 26 58 25 .14 23.76 CdSO 4 '35=21 45 20 43 19 .42 18 3 1 17 .41 16.25 KC1 '25 = 34 .42 36 05 37 76 39 32 40 .96 42.27 KC1 '35=23 74 25 26 54 27 94 28 93 30.02 KBr '25=35-94 39 .11 42 .41 44 .96 48 87 52.26 KBr '35=24 83 27 49 29 .64 3 1 93 34 .12 36.14 KCNS '25=37 57 42 38 47 .02 5 1 .81 55 .87 6 1 .26 KCNS '35=25 63 28 79 32 03 35 05 38 42-94 KI '25 = 38 .66 44 76 58 56 75 62 63 68.36 KI '35=26 3 30-25 34 .64 38 .04 41 .8 7 45-43 KNO 3 '25=33 .80 34 79 35 77 36 .66 37 57 38-52 KN0 3 '35=23 .27 24 03 24 79 25 72 26 54 27-33 K 2 SO 4 /,.= 77 .20 77 .61 2*~* v^ 4 NaBr 25 OO '25=33 76 OO 34 54 35 27 36 .26 36 .84 37-74 NaCl '25=32 .46 32 25 .96 .76 3 1 5 1 NaCNS '25=35 44 38 .24 40 78 43 37 45 .86 48.34 Na 2 S0 4 '25=3! .96 .14 30 45 29 5 1 28 .66 28.44 Na 2 S0 4 '35=21 .88 21 35 20 .81 20 .21 19 75 19.27 SOLUBILITY OF SULPHUR DIOXIDE IN ALCOHOLS AND IN OTHER SOLVENTS. (de Bruyn Rec. trav. chim. n, 128, '92; Schulze J. pr. Chem. [2] 24, 168, '81.) In Ethyl Alcohol In Methyl Alcohol In Several Solvents at 760 mm. at 760 mm. at o and 725 mm. (S.) to Gms. S(\per 100 Gms. Gms. SO 2 per 100 Gms. Solvent SC^per i Gm. Solvent. Solution. CjjHsOH. Solution. CH 3 OH.' Grams. Vols. ' o 53.5 115.0 71.1 246.0 Camphor 0.880 308 7 45.0 81 .o 59.9 149.4 CH 3 COOH 0.961 318 12.3 39.9 66.4 52.2 109.2 HCOOH 0.821 351 18.2 32.8 48.8 (17. 8) 44.0 78.6 (CH 3 ) 2 CO 2.07 589 26.0 244 32.3 31.7 46.4 SO 2 C1 2 0.323 189 33 1 SULPHUR DIOXIDE DISTRIBUTION OF SULPHUR DIOXIDE AT 20 BETWEEN: (McCrae and Wilson Z. anorg. Chem. 35, n, '03.) Water and Chloroform. Aq. HC1 and Chloroform. Gms. SOa per Liter in: Gm. Equiv. iSOj per Liter in: Cone. Gms. SOz per Liter in: Gm. Equiv. $SOj per Liter in: Aq. Layer. CHC1 3 Layer. Aq. Layer. CHC1 3 Layer. of HC1. Aq. Layer. CHClg Layer. Aq. Layer. CHCl," Layer. I-738 I .123 0-0543 O 035 1 O.O5 1.86 1.46 O .0581 0-0456 i-753 I .122 0.0547 O 0350 3-07 2.8 3 O .0960 0.0884 2.346 I 703 0.0732 O 0532 II 4.28 4-07 I 33 6 O.I27I 2.628 I .897 O.O82I O .0592 tt 5-34 5-42 .1667 0.1692 3-058 2 385 0-0955 0745 o.io 1.25 1.41 039 0-044 3-735 3 .062 0.1166 .0956 It 2.78 3-o8 .0868 o . 0962 4.226 3 .626 0.1319 .1132 (t 3-86 4-08 O .1199 0.1275 5.269 4 .798 0.1645 .1498 tt 5.161 5-72 O .1612 0.1784 6.588 6 I8 3 0.2057 O .1930 0.2 1.268 i-5i .0396 0.0471 31.92 33 .84 0.9968 I 056 tt 1.914 2.27 O 0597 0.0710 33-26 37 25 1.038 I 163 it 2.464 3-04 .0769 0.0949 tt 3-967 4.90 .1239 0.1530 0-4 i .202 1.61 .038 0-0504 tt 1.894 2.26 O 059 O.O7O6 TANNIC ACID C 13 H 9 O 7 COOH. 100 gms. H 2 O dissolve about 294 gms. at 25* dissolve about 439 gms. at 25. 100 gms. alcohol (U.S. P.) TAETAEIC ACID C 2 H 2 (OH) 2 (COOH) 2 . SOLUBILITY IN WATER. (Leidie Compt. rend. 95, 87, '82.) *. Grams Tartaric Acid per 100 Gms. KfeO. t. Gms. Tartaric Acid per 100 Gms. H 2 O. ' Dextro Racemic Racemic Dextro Racemic Racemic and Laevo Ac. Ac. and Laevo Ac. Ac. Acids. Anhydrous. Hydrated. Acids. Anhydrous. Hydrated o 115.04 8.16 9 23 5o 195.0 5- 59-54 10 125.72 12.32 14.00 60 217-55 64.52 78.33 20 139-44 18.0 20.60 7o 243.66 80.56 99-88 25 147.44 21.4 24.61 80 273-33 98.12 124.56 30 156.2 25.2 29.10 90 306.56 117.20 I52-74 40 176.0 37-o 43-32 100 343-35 137.80 184.91 SOLUBILITY OF TARTARIC ACID IN ALCOHOL AND IN ETHER AT 15. (Bourgoin Ann. chim. phys. [5] 13, 405, '78.) Gms. Tartaric Acid per 100 Gms. Solvent - Sat. Solution. Solvent. Absolute Alcohol 20 - 385 41 . 135 90% Alcohol 29 . 146 25 .604 Absolute Ether 0.389 0.40 TELLURIUM Te. 100 gms. methylene iodide CH 2 I 2 dissolve o.i gm. Te at 12. (Retgers Z. anorg. Chem. 3, 340, '93 TELLURIC ACID 33* TELLURIC AOID H,TeO 4 . 2 H 3 O. SOLUBILITY IN WATER. (Mylius Ber. 34, 2208, '01.) f. Cms. HjTeO 4 penoo Mols, H 2 TeO 4 per Solid 100 Mols. Phase. t. Gms. H a Te0 4 per 100 Mols. HTe0 4 per Solid xoo Mob. Phase. Cms. Sol. HaO. Gms. Sol. HjO. 13.92 1.51 H 2 TeO 4 .6HjO 30 33-36 4.67 HaTeCVaHaO 5 17.84 2.03 40 36.38 5-33 10 26.21 3-31 60 43-67 7-04 IS 32-79 4.41 80 51-55 9-93 IO 25.29 3.15 H 2 TeO 4 .aH 2 O 100 60.84 14-52 18 28.90 3-82 1 10 67.0 19.0 " TELLURIUM DOUBLE SALTS SOLUBILITY OP TELLURIUM DOUBLE BROMIDES AND CHLORIDES IN AQUEOUS HYDROCHLORIC AND HYDROBROMIC ACIDS AT 22. (Wheeler Z. anorg. Chem. 3, 432, '93.) Tellurium Double Salt. Formula. Solvent. Gms. Double Salt per 100 Gms. Solvent Te Caesium Bromide TeBr 4 .2CsBr Aq. HBr Te Potassium Bromide TeBr 4 .2KBr Te Rubidium Bromide Te Caesium Chloride Te Rubidium Chloride TeBr 4 . 2 RbBr TeCl 4 . 2 CsCl Aq. HC1* TeCl 4 . 2 RbCl * Sp. Gr. of Aq. HC1 solutions 1.2 and 1.05 respectively. THALLIUM ALUMS of i.4QSp.Gr. of i .08 Sp. Gr. 0.02 0.13 6-57 62.90 0.25 3-88 0.05 0.78 o-34 13.09 Alum. SOLUBILITY IN WATER AT 25 (Locke Am. Ch. J. 26. 174, f oi.) Salt per TOO Grams HjO. Formula. Tl Aluminum Alum Tl Vanadium Alum Tl Chromium Alum Tl Iron Alum Gms. Gms. Gm. Anhydrous. Hydrated. Mols. 7-5 11.78 0.0177 25-6 43 -3 1 0.0573 IO.48 16.38 0-0212 36-I5 64.6 0.0799 TlAl(S0 4 ) 2 .i 2 H 2 TlV(SO 4 ) 2 .i2H 2 O TlCr(S0 4 ) 2 . I2 H 2 TlFe(S0 4 ) 2 .i 2 H 2 THALLIUM BROMATE TlBrO 3 One liter saturated aqueous solution contains 3.463 gms. TIBrOj at 19.96 (B.), and 7.355 gms. at 39.75 (N. and A.). (Bottger Z. physik. Chem. 46, 602, '03; Noyes and Abbott Ibid. 16, 132, '95.) THALLIUM BROMIDE TIBr One liter saturated aqueous solution contains 0.42 gm. TIBr at 18, 0.476 gm. at 20, 0.57 gm. at 25, and 2.467 gms. at 68.5. (Kohlrausch Z. physik. Chem. 50, 356, '04; Noyes Ibid. 6, 248, '90; Bottger.) SOLUBILITY OF TIBr IN AQ. SOLUTIONS or T1NO 8 AT 68.5. (Noyes.) Gram Molecules per Liter. Grams per Liter. 0.0163 T1NO! 0.0294 " 0.0955 " 0.00410 TIBr 0.00289 " 0.00148 " 4.336 T1NO, 7.820 " 25-400 i . 164 TIBr 0.821 " 0.420 " 333 THALLIUM CHLORATE THALLIUM CARBONATE AND THALLIUM (Per) CHLORATE. THALLIUM CHLORATE T1C1O*. (See p. 338.) SOLUBILITY IN WATER. (Muir J. Chem. Soc. 29, 857, '76.) 20 50' 8o< ioo c Gms. T1C1O 3 per ioo gms. H^O 2.80 3.92 12.67 3 6 - 6 5 57 SOLUBILITY OP MIXED CRYSTALS OF THALLIUM CHLORATE AND POTASSIUM CHLORATE IN WATER AT 10. (Roozeboom Z. physik. Chem. 8, 532, '91.) NOTE. Solutions of the two salts were mixed in different pro- portions and allowed to crystallize, such amounts being taken that not more than one or two grams would separate from one liter. Grams per 1000 cc. Solution. Mg. Mols. per 1000 cc. Sp. Gr. Solution . o f Mol. per cent KC10 3 in Mixed TlClOa. KC10 3 . T1C10 3 . KC1O 3 . Solutions. Crystals. 25 637 8 9 .14 . . 1. 0210 19 637 6 .884 68 27 56 15 1.0222 2 .0 12 .001 26 .100 41 73 212 .89 1.0278 12 .61 9 036 40 .064 3 1 .42 326 79 0338 25 .01 7 7 .885 935 46 46 497 535 27 27 .42 .60 379 379 26 ] 57 J 0359 1 -0360 J ' 3 6 -30-97 93 6 .706 46 .410 23-32 378 55 0357 99 .28 6 729 47 .109 23 37 384 25 i 0363 99 .60 4 .858 47 .312 16 .89 385 .91 3 0345 99 .62 2 .769 47 9 63 384 .46 ] 0330 99.67 49 925 407 .22 ] 0330 IOO .00 SOLUBILITY OF MIXED CRYSTALS OF THALLIUM CHLORATE AND POTASSIUM CHLORATE IN WATER AT DIFFERENT TEMPERATURES. (Quoted by Rabe Z. anorg. Chem. 31, 156, '02.) ioo gms. H 2 O dissolve 2.8 gms. T1C1O 3 + 3.3 gms. KC1O 3 at o. ioo gms. H 2 O dissolve 10.0 gms. T1C1CX -f- 1 . 5 gms. KC1O 3 at 15. ioo gms. H 2 O dissolve 12.67 gms.,TlC!O 3 + 16.2 gms. KC1O 3 at 50. ioo gms. H 2 O dissolve 57.3 gms. T1C1O, + 48.2 gms. KClO,at 100. THALLIUM CHLORIDE T1C1. SOLUBILITY IN WATER. (Average curve from results of Noyes Z. physik. Chem. 9, 609, '92; Bottger Ibid. 46, 602, '03; Kohl- rausch Ibid. 50, 350, '04; Hebberling; Crookes; Lamy The results of Berkeley Trans. Roy. Soc. (Lond.) 203 A, 208, '04 are also given.) t o Gms. T1C1 per + Liter. o 2.1 (av.) 1.7 (B.) 25 10 2.5 2.4 30 20 3.3 3.4 40 50 Gms. T1C1 per .<> Gms. T1C1 per Liter. Liter. 3 .86 4 .0 60 8 .0 10 .2 4 .2 4 .6 80 12 o 16 -0 5 .2 6 .0 IOO 18 .0 24 .1 (99-3) 6 3 8 .0 THALLIUM CHLORIDE 334 THALLIUM CHLORIDE T1C1. SOLUBILITY IN WATER AND IN AQ. SALT SOLUTIONS AT 25. (Noyes; Noyes anji Abbott; Geffcken Z. physik. Chem. 49, 296, '04.) Aq. salt aoiuuon. Salt. T1C1. 'Salt. T1C1. Ammonium Nitrate NIL^NOj 0-0 o. 01612 o.o 3-86i (G.) M o-5 0.02587 40.02 6.209 %l I.O O.O3I2I 80.05 7-473 " 2.0 0-03966 160.10 9-497 Barium Chloride BaClj 0.0283 0.00857 5-895 2.052 (N.) o . 1468 0.00323 30-59 0-773 Cadmium Sulphate CdSC4 0.030 O.O2O6 6-255 4-933 (N.) " 0-0787 0.0254 16.41 6.081 " 0.1574 0.0309 32.82 7-399 Hydrochloric Acid HC1 0-0283 0.00836 1.032 2-002 (N.) " 0.0560 0.00565 2.043 1-353 || 0.1468 0.00316 5-357 0-757 Lithium Nitrate LiNOs o-5 O.O2542 34-53 6.085(0.) " I.O 0-03035 69.07 7.266 w 2-O 0-03785 138.14 9.063 " 3- 0.04438 207.21 10 . 630 Potassium Chlorate KClOa o-5 0.0237 61.28 5-674 (G.) Potassium Nitrate KNOs 0.015 O.OI7O i-5i7 4.070 (N.) " 0.030 0.0179 3-033 4.286 M 0-0787 0.0192 7-775 4-597 it 0-1574 O-O2I2 15.920 5.076 M o-5 0.0257 50-55 6-153(0.) (t I.O 0.0308 IOI.II 7-375 " 2.O 0.0390 202.22 9-340 Sodium Acetate CHsCOONa 0-015 0.0168 I.23I 4-023 (N.) " 0.030 0.0172 2.462 4.118 " 0-0787 0.0185 6. 4 6 4-43 0-1574 0.0196 12.92 4-693 Sodium Nitrate NaNO, o-5 0.02564 42.50 6.139 (G.) " i .0 0.03054 85.01 7-3I3 M 2-0 0.03851 170.02 9.221 " 3-o 0.04544 255-03 10.88 It 4.0 0.05128 340.12 12.28 Sodium Chlorate NaClOj o-5 0.02320 53-25 5-555 (GO '* 1.6 0.02687 106.5 6-433 M 2-0 0.03060 213.0 7.326 M 3-o 0-03303 3I9-5 7.909 ** 4-0 0.03850 426.0 9.215 Thallium Bromate TIBrOi (at 39.75*) O .01567 0-01959 5 201 4.690 (N.andA.) Thallium Nitrate TINOi 0.0283 0.0083 7.518 1.987 (N.) " 0-0560 0.00571 14.89 1.368 " o . 1468 0-00332 39.05 0-795 Thallium Sulphate TUSQi 0.0283 0.00886 14.27 2. 121 (N.) " 0.0560 0.00624 28.23 1-494 Thallium Sulphocyanide TiSCN Sat. 0.0119 Sat. 2.849(N.) * f= 59.60 1 : 1-40 : 0-45 Rb " 80.0 34.66+11.01 = 69.49 ' : 3-o * 1. 01 '* + 23-5N03. t + I9-74NO3. URANYL AMMONIUM PROPIONATE 2 UO 2 (C 3 H 5 O 2 ) 2 .NH 4 C 3 H 5 O 2 . 2H 2 O and Uranyl Potassium Propionate 2UO 2 (C 3 H 6 O 2 ) 2 .KC 3 H 6 O 2 . (Rimbach.) ioo gms. aq. solution contain 16.48 gms. 2UO 2 (C 3 H 5 O 2 ) 2 .NH 4 C 3 H,O 2 at 29.8. IQ-J gms. aq. solution contain 2.362 gms. UO 2 (C 3 H S O 2 )2 + 0.82 gm. KC 3 H C O 2 at 29.4, atomic relation, 1:1.29. TTRANYL SULPHATE 344 UEANYL SULPHATE (UO) 2 SO 4 . 3 H 2 O. SOLUBILITY IN WATER, ETC. (Buchdz; de Coninck Bull. Acad. Roy. Belgique, 350, p oi.) ioo gms. H 2 O dissolve 16.6 gms. UO 2 (SO 4 ).3H 2 O at 13.2, 17.4 gins, at 15.5, and 22.2 gms. at b. pt. ioo gms. abs. alcohol dissolve 4.0 gms. UO 2 (SO 4 ).3H 2 O at 18.2 and 5.0 gms. at b. pt. 100 gms. 85% alcohol dissolve 2.6 gms. UO 2 (SO 4 ).3H 2 O at 16. ioo gms. 16.2% alcohol dissolve 12.3 gms. UO 2 (SO 4 )-3H 2 O at 10. URANYL POTASSIUM SULPHATE UO 2 SO 4 .K 2 SO 4 .2H 2 O ioo gms. sat. aq. solution contain 10.41 gms. UO 2 SO 4 .K 2 SO 4 at 25 and 23.13 gms. at 70.5. (Rimbach.) SOLUBILITY OF UO 2 SO 4 .2K 2 SO 4 . 2 H 2 O + UO 2 SO 4 .K 2 SO 4 .2H 2 O IN WATER. Gms. per ioo Gms. Solution. Atomic Relation in Sol. Mol. % in Solid Phase. t . U0 2 . K. SO 4 . UO S . K. S0 4 . Mono Salt. Di Salt. 14 0.85 4.19 5-71 I 35-75 18.88 29 7 1 50 6.70 8.1 5 12.37 I 5.20 8.40 7 6 24 80 14.29 8-54 15-53 I 4-13 306 12 88 UREA CO(NH 2 ) 2 . SOLUBILITY IN WATER AND IN ALCOHOLS. (Campetti Abstract, Z. physic. Chem. 41, 109, '02; Speyers Am. J. Sci. [4] 14, 259, '02.) NOTE. Speyer's original results are in terms of Mols. CO(NH 2 ) 2 per ioo Mols. H 2 O at irregular temperatures. In Water. In Methyl Alcohol. In Ethyl Alcohol. . o Wt. of i cc. * ' Solution. Gms. CO(NH 2 ) 2 per w t . of i cc. ioo Gms. H 2 O. Solution. Gms. CO(NH 2 ) 2 XT ioo Gms. Gms. Wt. of ice. CO(NH 2 ) 2 Solution, per ioo Gms CH 3 OH. (J 2 H 5 UH. .121 55-9 0-861 138 0.8213 2 -5 10 ! 134 66.0 8s'o(C) 0.863 16.0 0.8l4 3-5 2O 1 .I 4 6 79.0 io8.2(C) 0.869 20. o 0-809 5-o 30 3 .156 93-o . . . 0.876 24.0 0.8o6 6-5 40 .165 106.0 . . . 0.890 30-0 0.804 8-5 50 173 I2O-O . . . 0.908 37-o 0.803 10.5 60 I.lSo 132.0 0.928 47-0 13.0 70 1.187 145.0 J 7-5 ioo gms. abs. methyl alcohol dissolve 21.8 gms. CO(NH 2 ) 2 at 19.5. ioo gms. abs. ethyl alcohol dissolve 5.06 gms. CO(NH 2 ) 2 at 19.5. (de Bruyn Z. physic. Chem. 10, 784, '92.) ioo gms. glycerine dissolve 50 gms. urea at 15.5. Phenyl Thio UREA (Phenyl thio carbamide) CS.NH 2 .NHC 8 H 6 . SOLUBILITY IN WATER. (Rothmund Z. physic. Ch. 33, 406, 'oo; Biltz Ibid. 43, 42, '03; Holeman and Antusch Rec. tray, chim. 13, 200, '94; Bogdan Ann. Scien. L'Univ. Jassy 2, 43, '02. '03.) One liter aq. solution contains 2.12 gms. CS(NH 2 ).NHCH 6 at 20 (B.), (R.) and 2.4 gms. at 25. (H. and A.). Bogdan gives 2.547 gms at 25. 345 Phenyl Thio UREA SOLUBILITY OF PHENYL THIO UREA IN AQUEOUS SALT SOLUTIONS AT 20. (Biltz; Rothmund.) Mfflimols and also Cms. CS(NH 2 )NHC8He Dissolved per Liter of Aqueous Salt Solution of Concentration: Salt 0.125 Normal 0.25 Normal o.s Normal I.O Normal Solution. Millimols . Cms. Millimols. Cms. Millimols. Gms. Millimols. Cms. iA!CI 3 12 95 1-97 12.82 I .96 12 03 1.8 3 10 .69 1.61 NH 4 NO 3 14 *7 2.15 14.4 2 .21 14 53 2.22 14 .91 2.27 i(NH 4 ) 2 S0 4 *3 5 1 2.05 12.84 1.96 II .78 1.79 9 .98 1.52 BaCl 2 13 12 1-99 12.92 1.97 12 .22 1.86 10 44 x -59 JBa(NO,) 2 13 9 8 2.13 I 3 . 9 8 2.13 13 -90 2.12 CsN0 3 14 53 2 .21 14.90 2.27 15 23 2-33 . . . LiN0 3 13 96 2.13 13.96 2.13 J 3 93 2 .12 *3 73 2.10 iMgS0 4 13 40 2.04 12.78 i-95 ii 54 75 9 43 i-43 KC 2 H 3 O 2 13 40 2 .04 12-95 1-97 12 .14 85 10 74 1.62 KBr 13 5o 2.05 13-35 2 .04 12 .80 95 ii .76 1.79 KC10 3 13 86 2. II 13 .60 2.O6 13 .12 99 . KC1 J 3 40 2.04 12-73 i-94 12 .19 85 IO 54 i .60 Kl 14 12 2.15 14.48 2.21 14 31 2.18 14 .60 2.23 KNO 3 I 3 8 9 2.12 I3-85 2. II 13 52 2.05 12 .82 i .96 KNO 2 14 5 2 2 .21 14.65 2.23 13 .80 2. II 12 5i i .92 iK 2 S0 4 13-25 2.03 12-49 I.9I II .11 I .69 8 73 *-33 RbNO 3 14 22 2.l6 14.44 2.19 14 39 2.18 14 .22 2.17 iNa 2 C0 3 J 3 .29 2.O4 12.52 I.9I II 05 1.68 8 58 1.32 NaClO 3 13 75 2.09 J 3- 6 5 2.08 13 .07 1.98 12 .21 1.86 NaC10 4 14 i5 2.15 14.05 2.14 13 58 2.06 12 56 i .92 NaCl I 3 28 2.02 12.83 i-95 II .90 1.81 IO .02 1.52 Nal 13 98 2-13 14.07 2.14 14 .29 2.18 13 .96 2.13 NaNO 3 !3 94 2 .12 13-77 2 .IO 13 32 2.04 12 57 i .92 NaNO 2 14 34 2.18 13.82 2. II 13 .06 1.98 II 52 J -75 }Na 2 S0 4 i3 .19 2.00 !2-35 1.87 IO 85 1-63 8 30 1.27 SOLUBILITY OF PHENYL THIO UREA AT 25 IN AQUEOUS SOLUTIONS OF. Potassium Nitrate. Sodium Nitrate. (Bogdan.) (Bogdan.) Gms. Mols. KN0 3 per Gms. looo Gms per H 2 0. Gms. Mols. NaNOa per Gms. per looo Gms. HjO. 1000 Gms. HaO. KNO 3 . CS(NH 2 ) .NHQjHs. 1000 Gms. H 2 0. NaNOa. CS(NH 2 ) .NHQjHfi. 1.045 105-7 2.38 I .024 87.14 2 .26 0.5123 5I-84 2.48 0.5065 43-10 2.46 O.2O26 20.50 2-54 0.2031 17.28 2.51 0.1007 10.19 2 -56 0.0986 8-39 2-53 0.0503 5-09 2-55 0.0540 4-59 2-54 0-0333 3-36 2-55 0-0335 2.84 2-54 Phenyl Thio UREA 346 SOLUBILITY OF PHENYL THIO UREA IN MIXTURES OF ETHYL ALCOHOL AND WATER AT 25. (Holleman and Antusch Rec. trav. chim. 13, 290, '94.) Cms. Gms. Vol. per cent CS(NH 2 ) NHQjHs Sp. Gr. of Vol. per cent CS(NH 2 ) NHQHs Sp.Gr. of Alcohol. per 100 Gms. Solutions. Alcohol. per 100 Gms. Solutions. Solvent. Solvent. ZOO 3-59 . . . 65 3-40 0.9018 95 4.44 0.8200 60 2.80 0-9128 90 4.69 0.8389 50 1.8 7 0.9317 85 4-99 0.8544 40 *-*3 0-9486 80 4.70 0-8679 25 0.56 0.9679 75 4-45 0.8810 15 0.38 0.9788 70 3-92 0.8915 O 0.24 0.9979 SOLUBILITY OF PHENYL THIO UREA IN AQUEOUS SOLUTIONS OF PROPYL AND OF ETHYL ALCOHOL AT 25. (Bagdan.) G. Mols. 1000 Gms. H 2 0. 0.5448 O.IO59 0.05526 0-04854 In Propyl Alcohol. Gms. per 1000 Gms. H 2 O C 3 H 7 OH. 62.10 32.688 6-354 CS(NH 2 ) NHCH 5 . 3.124 2.643 2-599 2.586 2.912 In Propyl Alcohol at o. I -OOO 60-06 I. 21 o.ioo 6.01 1-047 In G. Mols. C 2 H 5 OH per looo Gms. H 2 0. . Ethyl Alcohol. Gms. per rooo Gms.H 2 O C 2 HsOH. CS(NH 2 ) NHCeHs- I .1010 49.60 3- J 93 0-5355 o . 1094 0.05018 24.12 4-932 2.26 2.931 2 .629 2.589 0.03271 1-473 2-577 SOLUBILITY OF PHENYL THIO UREA IN AQUEOUS SOLUTIONS OF ACETONE, MANNITE, CANE SUGAR, DEXTROSE, AND UREA. (Bagdan.) Aqueous Non Electro- to Gms . per looo Gms. Aqueous Non Electro- * o Gms. per 1000 Gms. H 2 0. lyte. Non Elec- trolyte. CS(NH 2 ) NH.CcHs. lyte. Non Elec- trolyte. CS(NH 2 ) NHCeHs. (CH^CO 25 7 -478 2 .667 C 6 H 12 O fl 25 180 .40 3 .042 " 2 513 2 579 a ti 90 .46 2 83 " ft I .908 2 573 tt n 29 .29 2 .69 C,H 8 (OH). 11 182 .11 3 .04 it ti 18 .01 2 654 tt tt 91 05 2 .78 n it 9 554 2 .603 C^H^OH 25 338 .6 3 457 CCKNH,), 63 .08 3 .306 M It 170 4 3 .015 " " 29 93 2 .892 " (( 34 36 2 634 a a 6 .132 2 .6l8 " " 18 .28 2 -596 " " 4 .942 2 -60 5 " tt 10 .09 2 572 n tt 2 .009 2 572 it o 342 18 I 420 60 .11 I .310 " tt 34 .22 I 044 " " 6 .01 I .048 347 URETHANE URETHANE CO(NH 2 )OC 2 H 5 . SOLUBILITY IN SEVERAL SOLVENTS. (Speyers Am. J. Sci. [4] 14, 294, '02.) See also Ethyl Carbamate, p. 138. Interpolated and calculated from the original results which are given in terms of molecules Urethane per 100 Mols. solvent. Solubility in Water. Solubility in Methyl Alcohol. w* Mols. Gms / \\Tt- ~t Mols. Gms. CO(NH 2 ) CO(NH 2 ) Wt. ot CO(NH 2 ) t. lr OC 2 Hs per ioo Mols. OC 2 H 8 per ioo Gms. I CC. Solu- ioo Mols. OC^per ioo Gms. Uon - H 2 0. H 2 0. tion. CHaOH. CH 3 OH. o .023 3.61 I 7 .8 0.956 31.18 86.76 10 .033 6.0 29.7 0-977 41.0 II4.I 15 .042 15.0 74-2 0.989 47-5 132.1 20 -060 31 -O 153-3 i .000 54-5 25 -073 50.0 247-3 1.013 62.5 173-9 30 .078 65.0 321.4 1.024 72.0 200-3 40 .065 77.0 380.7 1.045 89.0 247-7 Solubility in Ethyl Alcohol. Solubility in Propyl Alcohol. w . nf Mols. Gms. TTfi - Mols. Gms. i cc CO(NH a ) CO(NH 2 ) Wt. Ot I CC. CO(NH 2 ) CO(NH 2 ) t. Solu- So^ScE* ioo Gms. Solu- ioo Mols. ioo Gms. C 2 H 5 OH.' tion. CaH 7 OH. o 0-8914 23.91 46.26 0.880 19.48 28.9 10 0-930 36.0 69.6 0.906 31-0 46.0 15 0.950 43-0 89.2 0-923 4O-O 59-3 20 0.968 50.0 96.7 0-942 51-0 75-7 25 0.985 59.0 II4.I 0-963 6o-0 89.0 30 I .001 70.0 135-4 0-983 68.0 100.9 40 1.035 88 -o 170.2 I .025 85.0 126.1 Solubility in Chloroform. Solubility in Toluene. .. Wf nf Mols. Wt of C 0(NH 2 ) So 0( *&? er Uon. X SJ8J?- Gms. CO(NH 2 ) OC 2 H, per ioo Gms. CHC1 3 . Wt.of I CC. Solu- tion. Mols. CO(NH 2 ) OC 2 H 6 per ioo Mols. Gms. CO(NH 2 ) OCaH per ioo Gms. o .404 27.56 20. 6 0.887 i 5 . 77 I.7I 10 .340 41 30.6 0-874 5-o 4-84 15 .310 46 34-4 0-875 10.0 9.68 20 280 53 39 6 0.883 16.0 15 -4 8 25 .240 60 44.8 0.902 25.0 24.18 30 .203 67 50.0 0-927 44.0 42.58 40 .125 80 59-7 o-995 85.0 82.24 URIC ACID C 6 H 4 N 4 O 3 . SOLUBILITY IN WATER. (Blarez and Deniges Compt. rend. 104, 1847, '87; at 15 Magnier 483, '75.) Bull. Soc. chim. [2] 23, Gms. CsIL^N^Og. Gms. C 5 H4N 4 O3 Gi us. GJLN^O t*. per ioo Gms. t. per ioo Gms. t. per ioo Gms. H 2 0. H 2 O. H^. O.OO2 30 o .0088 70 0-0305 10 0.0037 40 o OI22 80 0.0390 *S 0.0053 50 o .OI7O 90 0-0498 20 O.OO6 60 o .0230 IOO 0-0625 VALERIANIO ACID 348 VALEBIANIO ACID n CH,(CH 2 ) 3 COOH ( Propyl acetic acid Pentane acid) when shaken with water at 16 two layers are formed. 100 gms. of the aqueous layer contains 3.4 gms. CH 3 (CH 2 ) 3 COOH. 100 gms. of the acid layer contains 90.4 gms. CH 3 (CH 2 ) 3 COOH. (Lieben and Rossi Liebig's Ann. 159, 60, '71.) YTTRIUM IODATE Y(IO 3 ) 3 .3H 2 O. 100 gms. H 2 O dissolve 0.53 gm. yttrium iodate. (Berlin.) YTTRIUM SULPHATE Y 2 (SO 4 ) 3 . 100 gms. H 2 O dissolve 15.2 gms. Y 2 (SO 4 ) 3 at ord. temperature, 9.3 gms. Y 2 (SO 4 ) 3 .8H 2 O at ord. temp, and 4.8 gms. Y 2 (SO 4 ) 3 .8HO 2 at 100. (Cleve Bull. soc. chim. [2] ax, 344, '74.) YTTERBIUM SULPHATE Yb 2 (SO 4 ) 3 .8H 2 O. SOLUBILITY IN WATER. (Cleve Z. anorg. Chem. 32, 143, '02.) Gms. Yb2(SO 4 ) 3 Gms. Yb 2 (SO 4 ) 3 Gms. Yb2(SO 4 ) 3 t. per 100 gms. t. per 100 Gms. t. per 100 Gms. H 2 0. H 2 O. H 2 0. o 44-2 55 n-5 80 6.92 15.5 34.6 60 10.4 . 90 5.83 35 19.1 70 7.22 ico 4-67 ZINC ACETATE Zn(CH 3 COO) 2 .2H 2 O. 100 gms. H 2 O dissolve 40 gms. at 25 and 66.6 gms. at b. pt. 100 gms. alcohol dissolve 2.8 gms. at 25 and 166.0 gms. at b.pt. (u. s. P.) ZINC BENZOATE Zn(C 7 H 5 O 2 ) 2 . SOLUBILITY IN WATER. (Paietta Gazz. chim. ital. 36, II, 67, '06.) t. 15-9 17 27.8 31.3 37.5 49.8 59 Gms. Zn(C 7 H 5 O 2 ) 2 per loo gms. aq. solution 2.55 2.49 2.41 2.05 1.87 1.62 1.45 ZINC BROMIDE ZnBr 2 . SOLUBILITY IN WATER. (Dietz Wiss. Abh. p. t. Reizhanstalt 3, 431, 'oo; see also Etard Ann. chim. phys. [7] 2, 536, '94.) Gms. ZnBr 2 Mols. ZnBr 2 ,,.. Gms. ZnBr 2 Mols. ZnBr 2 ,... t. per TOO Gms. per 100 T * *- P 61 " I0 Gms - P 61 IO PV. ^Solution. Mols.H 2 0. Solution. Mols.H 2 O. !5 77 -*3 2 7' ZnBr 2 . 3 H2O 25 82.46 37.6 ZnBr 2 . 2 H 2 O io 78-45 2 9 - 1 3 84.08 42.3 - 5 80.64 33.3 37 86.20 50.0 --8 79-06 30-2 ZnBr 2 . 2 H a O 35 85.45 46.9 ZnBr 2 o 79-55 3 1 - 1 " 4o 85.53 47.4 + 13 80.76 33.5 60 86.08 49.5 18 81.46 35-1 80 86.57 51.5 ico 87.05 53.8 349 ZINC CARBONATE ZING CARBONATE ZnCO,. One liter H 2 O dissolves o.oi gm. at 15. One liter aq. 5.85 per cent NaCl solution dissolves 0.0586 gm. at 14. One liter aq. 7.45 per cent Nad solutions dissolves 0.0477 gm. at 14' (Cantoni and Passamanik Ann. chim. anal. appl. 10, 258, '05.) Gms. Zn(C10 3 ) 2 per i oo gms. Solution. -18 o 8 15 18 59 -!9 60.20 67.32 66.52 9.70 11.08 ii .72 15.96 15-39 Solid Phase. Zn(C10 3 ) 2 .6H 2 O Zn(C10 3 ) 2 . 4 H 2 Gms. Zn(C10 3 ) 2 per 100 Gms. Solution. ZINC CHLORATE ZnClO 3 . SOLUBILITY IN WATER. (Meusser Ber. 35, 1417, '02; at 18; Mylius and Funk Ber. 30, 1718, '97.) Mols. Zn(C10 3 ) 2 per too ols.H 2 O. 30 76.66 4O 69 . 06 55 75-44 Ice curve -13 30.27 9 26.54 Sp. Gr. of solution saturated at 18 = 1.916. Mols. Zn(C10 3 ) 2 per 100 Mols. H 2 O. 16.20 17.29 24.00 3-36 2.8o Solid Phase. Ice ZINC CHLORIDE ZnCl 2 . SOLUBILITY IN WATER. (Mylius and Dietz Z. anorg. Chem. 44, 217, '05; see also Dietz Wiss. Abh. p. t. Reichanstalt 3. 429, 'oo; Etard Ann. chim. phys. [?j 2, 536, '94.) Gms.ZnCl 2 per looGms. Solid .o Gms.ZnCl 2 per looGms. Solid Water. Solution. Phase. ' Water. Solution. Phase. 11 5 14 12 3 Ice 9 360 78 3 . 2 *H 2 0+.H 2 10 40 25 83 2O 45 .0 3 : J 385 2 9 8 79 74 4 9 ZnCl 2 . 2 }H 2 ZnCl 2 .i*H 2 -62 104 51 .0 Ice + ZnCl 2 .4H 2 O IO 330 76 .8 " "~1 5 XI 3 53 .0 ZnCl 2 . 4 H 2 O - 20 368 78 .6 " 40 127 55 9 26 423 80 9 .HH 2 0+ZnCl 2 .H 2 O -30 160 61 5 .4H 2 0+. 3 H 2 26.3 433 81 .2 .iJH 2 + ZnCl 2 10 189 65 4 ZnCl 2 . 3 H 2 O 342 77 4 ZnCl 2 .H 2 o 208 67 5 10 364 78 -4 " f 5 230 69 7 20 39 6 79 .8 " 6-5 252 4 7 1 .6 28 436 81 3 ZnCl 2 .H 2 -f ZnCl 2 5 282 73 .8 3 1 477 82 7 ZnCl 2 .H 2 O S^. o 309 75 5 . 3 H 2 O -f .iiH 2 O 25 432 81 .2 ZnCl 2 t o 2*< 7 .1 ZnCl2.2)HO 4O 452 81 9 " 6-5 OJ 252 7 1 .6 . 2 *H 2 O + -sHzO 60 488 83.0 10 272 73 .1 ZnCl^iHzO 80 543 84 4 " 12.5 303 75 .2 100 6 J 5 86 .0 " "5 335 77 O .2*H 2 + .liHjO 2 62 00 100 -0 it ZINC CYANIDE Zn(CN) 2 . 100 cc. concentrated Zn(C 2 H 3 O 2 ) 2 + Aq. dissolve 0.4 gm. Zn(CN) 2 . 100 cc. concentrated ZnSO 4 + Aq. dissolves 0.2 gm. (joannis.) ZINO CHLORIDE 350 SOLUBILITY OP ZINC CHLORIDE, AMMONIUM CHLORIDE MIXTURES IN WATER. (Meerburg Z. anorg. Ch^m. 37, 212, '03.) Isotherm for o. Isotherm for 20. Isotherm for 30. Gms. per ioo Gms. Gms. per too Gms. Gms. per ioo Gms. Solution. Solid Solution. Solid Solution. Solid *-. , , .. ,. TVirt, * Til . Tl_ _ ZnCl 2 . NH 4 C1." ' ZnCl 2 . NH 4 C1. ZnCl 2 . NH4C1. O 22.8 NH4C1 .0 26 9 NEUCl .0 29 5 NHa 3 5 23.0 5 .1 27 .1 9 .2 29 4 " 7 I 23-5 9 5 27 4 16 O 2 9 7 10 .2 23-9 12 7 27 5 20 .2 30 .1 " 15 I 24.7 15 7 27 7 24 7 30 4 18 .0 25-3 18 .0 27 9 26 3 30 .8 NH 4 Cl + < 22 4 26.O 23 5 29 .0 27 .2 30 .2 a 24 .2 26.1 26 .0 29 -5 NH 4 Cl + a 30 .1 2 9 .6 2 5 7 26-3 NH 4 Cl+a 29 5 28 .1 36 .8 28 2 " 27 5 26.4 32 3 27 7 42 4 27 3 " 30 7 25-7 35 .8 27 .0 43 .8 27 3 a + b 33 9 25-3 38 7 26 9 45 .0 24 4 b 38 .8 24.4 40 .2 26 .6 5 1 .2 17 .6 42 .6 24.6 a + b 41 9 26 3 61 9 IO 4 44 3 21-3 b 43 .2 26 .0 a + b 66 9 9 .2 ZnCl 2 -fi 49 .2 15-3 46 9 21 .0 b 75 .6 6 .1 ZnCl 2 5 2 .6 II-9 53 .2 14 5 70 3 7 .6 55 4 IO.O 58 4 II .1 78 5 3 .2 i 59 3 7-5 62 7 8 7 76 -9 3 5 14 62 .1 6.8 66.6 7 9 79 .8 i .6 to 81 .6 o .0 II a = ZnCl 2 .3NHCl 3 .. b = ZnCl 2 . 2 NH 4 Cl. ioo gms. abs. acetone dissolve 43.5 gms. ZnCl 2 at 18. (Naumann Ber. 37, 4332, '04.) ioo gms. glycerine dissolve 50 gms. ZnCl 2 at 15.5. ZINC FLUORIDE ZnF 2 . 4 H 2 O. One liter of water dissolves 16 gms. at 18. (Dietz.) ZINC HYDROXIDE Zn(OH) 2 . One liter of water dissolves 0.0042 gm. ZnO at 18, conductivity (Dupre and Bratas Z. angew. Chem, 16, 55, '03.) SOLUBILITY OF ZINC HYDROXIDE IN ONE PER CENT AQUEOUS SALT SOLUTIONS AT i6-2o. (Snyder Ber. n, 936, '78.) The CO 2 free Zn(OH) 2 dissolved is calculated as milligrams Zn per method. liter of the given salt solution, given. Additional determinations are also Aq. Salt Mgs. Zn per Solution. Liter Solution. NaCl KC1 CaCl 2 MgCl 2 BaCI, 5 1 43 57-5 65 38 Aq. Salt Mgs. Zn per Solution. Liter Solution. Aq. Salt Mgs. Zn per Solution. Liter Solution. K 2 S0 4 37-5 K 2 C0 3 o MgS0 4 27 NH 4 C1 95 KN0 3 J 7-5 NH 4 NO 3 77 Ba(N0 3 ) 2 25 (NH 4 ) 2 S0 4 88 ZING HYDROXIDE SOLUBILITY OF ZINC HYDROXIDE IN AQUEOUS SOLUTIONS OP: Ammonia and Ammonia Bases at i7-i9. (Herz Z. anorg. Chem. 30, 281, '02.) Sodium Hydroxide at Ord. Temp. (Rubenbauer Ibid. 30, 333, '02.) Normality Normality of of Dis- Gms. ZnO per 20 cc . Gms. per 20 cc. Solution Mol. the Base. solved Zn. Solution. Na. Zn. the NaOH. o . 0942NH 3 o . ooi i 0.00185 0-IOI2 0.0040 4.50 0.236 " o.oiio O.OlSo 0.1978 0.0150 2.33 0.707 " 0.059 0.0958 0.4278 0.0442 1. 06 o.o944NH 2 CH 3 0.0005 O.OOOS 0-6670 O.I77I 0.70 0.472 0.0081 O.OI32 0.9660 0.9630 0.48 0.944 " 0.03 0.0484 I.495I 0.2481 0.31 0.068 NH 2 C 2 H 5 0.0003 0.0005 2.9901 0.3700 0.16 0.51 " 0.0045 O.OO74 Moist Zn (OH) 2 used. So- 0.68 0.0098 O.OIOI lutions shaken 5 hours. Gms. ZnI 2 Mols. ZnI 2 per loo Gms. per 100 Mols. Solid Phase. ZnI 2 ZINC IODATE Zn(IO 3 ) 2 . loo gms. H 2 O dissolve 0.87 gm. Zn(IO 3 ) 2 cold and 1.31 gms. hot. (Rammelsberg Pogg. Ann, 43, 665, '38.) ZINC IODIDE ZnI 2 . SOLUBILITY IN WATER. (Dietz Wiss. Abh. p. t. Reichanstalt 3, 432, 'oo; see also Etard Ann. chim. phys. [7] 2, 526, '94.) Gms. ZnI 2 Mols. ZnI 2 t. per loo Gms. per 100 Solid Phase, t' Solution. Mols. H 2 O. 10 80.50 23.3 ZnI 2 . 2 H 2 O - 5 80.77 23.7 o 81.16 24.3 + 10 82.06 25.8 22 83.12 27.8 27 89.52 50.3 Sp. Gr. of sat. solution of the anhydrous salt at 18 = 2.725. loo gms. glycerine dissolve 40 gms. ZnI 2 at 15.5. ZINC NITRATE Zn(NO 3 ) 2 . SOLUBILITY IN WATER. (Funk Wiss. Abh. p. t. Reichanstalt, 3, 438, 'oo.) Solution. H 2 0. O 8i.ii 24.2 18 81.20 24.4 40 81.66 25.1 60 82.37 26.4 80 83-05 27-5 IOO 83.62 28. 7 Solid Phase. Gms. Mols. Zn(N0 3 ) 2 per ZnNO 3 per zoo Gms. loo Solution. Mols. H 2 O. 6.36 Zn(N0 3 ) 2 . 9 H 2 O l8 Gms. Mols. Zn(N0 3 ) 2 per Zn(NO 3 ) 2 per Solid -25 4O-I2 0-30 22-5 40-75 6-54 20 42.03 6.89 -18 43-59 7-34 -18 44-63 7.67 ~!5 45.26 7.86 -3 45 -5 1 7-94 12 45-75 8.01 O 48.66 9.01 + 12.5 52-0 10.3 t". loo Gms. IOO Phase. Solution. Mols. H 2 O. 18 53-50 IO.9 Zn(N03) 2 .6H,0 25 55-90 12 .O l 3 6 -4 63-63 I6. 7 " 36 64.63 17.4 " 33-5 65.83 18-3 " 37 66.38 18.8 Zn(N0 3 ) 2 .3H0 40 67.42 19.7 " 4i 68.21 20.4 " 43 69.26 21.4 M 45-5 77-77 33-3 ZINC OXALATE 352 ZINC OXALATE ZnC 2 O 4 . 2 H 2 O. One liter of water dissolve 0.083 Mg. equiv. = 0.0064 gm. ZnC 2 O 4 at 18. (Kohlrausch Z. physik. Chem. 50, 356, '04- '05.) ZINC SULPHATE ZnSO 4 . SOLUBILITY IN WATER. (Cohen Z. physik. Chem. 34, 189, 'oo; at 50; Callender and Barnes Proc. Roy. Soc. 62, 149, '97; Etard Ann. chim. phys. [7] 2, 536, '94; Poggiale Ibid. [3] 8, 467, '43; Mulder.) t . Gms. ZnS0 4 per ioo Gms. Solid t . Gms. ZnSO 4 per 100 Gms Solid Solution. Water'. Phase. Solution. Water. Phase. - 5 28 .21 39- 30 ZnSO 4 .7H 2 O 25 38 94 63 74 ZnS0 4 .6H 2 O O.I 29 54 93 39 41 .22 70 .06 .6H 2 O + .7H 2 O 9.1 32 OI 47- 09 5o 43 45 7 6 .84 ZnS0 4 .6H 2 O 15 33 .81 50- 88 70 47 5 88 7 .6H 2 + .H 2 O 2 5 36 .67 57- 90 80 46 4 86 .6 ZnSCvHzO 35 39 .98 66. 61 90 45 5 83 7 " 39 .21 70. 05 IOO 44 7 80 .8 " - 5 32 OO 47- 08 ZnS0 4 .6H 2 O 1 20 41 7 71 5 " OI 33 .09 49.48 140 38 .0 61 3 " 160 33 .0 49 3 " ioo gms. abs. methyl alcohol dissolve 0.65 gm. ZnSO 4 at 18, 5.90 gms. ZnSO 4 .7H 2 O at 18. ioo gms. 50 per cent methyl alcohol dissolve 15.7 gms. ZnSO.7H 2 O at 1 8. (de Bruyn Z. physik. Chem. 10, 783, '92.) SOLUBILITY OF ZINC SULPHATE IN AQUEOUS ETHYL ALCOHOL. (Schiff Liebig's Ann. 118, 365, '61.) Concentration of Alcohol 10 per cent 20 per cent 40 per cent Gms. ZnSO 4 .7H 2 O per ioo Gms. Solution 51.1 39.0 3.45 ioo gms. glycerine dissolve 35 gms. zinc sulphate at 15.5. 353 ZING SULPHATE SOLUBILITY OF ZINC SULPHATE SODIUM SULPHATE MIXTURES IN WATER. (Koppel Gumpery Z. physik. Chem. 52, 409, '05.) to Gms. per 100 Gms. Solution. Gms. per 100 Gms. H 2 O. Mols. per 100 Mols. H 2 0. Solid . ZnS0 4 Na 2 S0 4 ZnS0 4 . Na 2 S0 4 . ZnSO 4 . Na 2 S0 4 : Pnase - O 27.19 5-33 40.30 7-90 4-5 I .01 )ZnS0 4 . 7 H 2 + 5 2 7 -85 6.27 42.28 9-52 4.71 1. 21 ) Na 2SO 4 .ioH 2 O 25 I7-58 26.32 23.40 2-94 2.96 ZnNa 2 (S0 4 ) 2 .4H 2 30 17.66 I5-58 26.47 23-44 2-95 2.97 35 17-59 15 .70 26.36 23-52 2.94 2.98 40 J 7-75 I5-72 26.68 23-63 2.98 2.99 10 29.16 7.16 45-79 ii .24 5- 11 1-42 - IS 30.70 6.40 48.81 10.17 5-45 1.29 20 32- 5 1 5-36 52.34 8.62 5-84 1.09 ZnNa 2 (SO ) H O 25 34-36 4.41 56.15 7.22 6.27 0.91 -j-ZnSO/.rHzO 2 30 36.28 3-8o 60-55 6-34 6.76 0.81 35 38.18 3 .30 65-25 5-64 7.28 0.71 > 38 40 38-83 38.26 2 .90 2.78 66.64 64.89 4-98 4.71 7-44 7.24 0.63 o .60 10 27.91 7-92 43-50 12.34 4-85 I -5 6 5 15 24.28 10.90 36.92 16.71 4.12 2 .12 20 19,14 14.58 28.77 2i-95 3-21 2.79 ZnNa 2 (S0 4 ) 2 ^H 2 +Na 2 S0 4 .ioH 2 25 13 .31 19.94 19-93 29-87 2 .22 3 .785 30 6.96 27-75 10.67 42-51 I.I9 5-39 35 5 -61 30-03 8.72 46.61 0-971 ZnNa 2 (SO 4 ) 2 . 4 H 2 O 40 5-96 28.65 9.16 43-83 I .02 5-555 +Na 2 S0 4 ZINC SULPHITE ZnSO 3 . 2 H 2 O. 100 gms. H 2 O dissolve 0.16 gm. ZnSO 4 .2H 2 O. (Houston and Trichborne Brit. Med. Jour. 1063, '90 ZINC TARTRATE C 4 H 4 O 6 .Zn. 2 H 2 O. SOLUBILITY IN WATER. (Cantoni and Zachoder Bull. Soc. chim. [3] 33, 751, '05.) Gms. t. CAO6.Zn.2HzO per 100 cc. Solution. 15 O.OI9 2O O.O22 25 0-036 30 O.O4I 35 0-055 40 45 5o 55 60 Gms. C 4 H 4 O 6 .Zn. 2 H 2 O per 100 cc. Solution. 0-o6o 0.073 0.087 0.116 0.104 Gms. t. C 4 H 4 0.Zn.2H20 per i oocc. Solution. 65 o.ioo 70 0.088 75 0.078 80 0.050 85 0.041 ZINC VALERATE (C 4 H 9 COO) 2 Zn. 2 H 2 O. 100 gms. H 2 O dissolve 2 gms. (C 4 H,COO) z .Zn.2H 3 O at 35. 100 gms. alcohol dissolve 2.8 gms. at 25. (u. s. P.) ADDENDUM The distribution results shown in the following table were obtained by agitating together equal volumes of olive oil and aqueous solutions of the several narcotics, and determining the dissolved substance present in the aqueous layer before and after the agitation. The sum of the amount of substance in the oil and aqueous layers, as shown in the table, is the amount originally in 100 cc. of each aqueous solu- tion used. The work was done for the purpose of testing the Overton-Meyer Theory of Narcosis, that the anesthetic action of certain groups of narcotics is proportional to their distribution between water and the fatty material occurring in the nervous system, and olive oil was selected as the solvent best fulfilling the analytical requirements and at the same time offering a fair resemblance to the fatty substance of the nervous system. The results are believed to be of interest both as solubility studies and on account of their connection with the Theory of Narcosis. The author is indebted to Dr. Reid Hunt of the Hygienic Laboratory for calling his attention to the papers containing the distribution results here tabulated. 354 355 DISTRIBUTION OF SEVERAL SUBSTANCES BETWEEN WATER AND OLIVE OIL. (At ord. temp., Baum Archiv. exp. Pathql- u. Pharmakol, 42, 130, '99; at 3, 30 and 36; Meyer-* Ibid. 46, 344, '01; at 15, Harrass Archiv. internal. Pharmacodynamie et Therapie, xx, 458, '03.) Name of Substance. Sulfonal Trional Tetronal Di methyl sulphon di methyl methane Di ethyl sulphon me- thane Ethyl urethane Methyl urethane Formula. (CH 8 ) 2 C(S0 2 .C 2 H 6 ) 2 (CH 3 )(C 2 H 6 )C(S0 2 .C 2 H 6 ) 2 (CH 3 ) 2 C(S0 2 .CH 3 ) 2 CH 2 .(S0 2 .C 2 H 5 ) 2 NH 2 .C0 2 .C 2 H 5 NH 2 .CO 2 .CH 3 Tertiary butyl alcohol (CH 3 ) 2 C(OH)CHs Amylene hydrate (CH 3 )aC(OH)CH 2 .CH 3 Mono acetin C 3 H 6 (OH) 2 .(OC 2 H 3 O) Di acetin Tri acetin Bromal hydrate Butyl chloral hydrate Chloral hydrate Salicylamide Benzamide Ethyl alcohol Acetone C 3 H 5 (OH)(OC 2 H 3 0) 2 CBr 3 CH(OH) 2 C 3 H 4 C1 3 .CH(OH) 2 CClsCH(OH) 2 OH.CH4.CH 2 NHa C 7 H 6 ONH 2 (CH 3 )2CO Valeryl di ethyl amide CHs(CH 2 ) 3 cON(C3H6)2 Valeryl di methyl amide CHaCCH^sCONCCH^ Valeryl ethyl amide Valer amide Lactic acid di ethyl amide Sodium salicylate Gms. Substance per t o loo cc. C(f.) Water Olive Oil C(w.) layer (w.). layer (f.). ord. 0.0700 0.0686 0-979 tt 0.0404 o. 1646 4.074 ft 0.0462 0.1446 3-756 " 0.6072 0.0622 0.103 (( 0.610 0.092 0.151 " 4-52 0.615 . *36 " 7-50 0.275 0-037 " 8.744 !-539 0.176 M 6.605 6.605 I. 000 It 4.28 0.254 0.059 3 2-349 o. 229 0.099 36 2.417 0.161 0.066 ord. 3- o-7 0.234 tt 2.72 0.80 0.295 n 9.81 6.52 0.665 it 2.04 3-24 1.589 a 16.31 3.10 0.100 tt 4.12 0.91 0.22 3 1.34 0.08 0-053 3 1. 15 0.27 0.237 3 0.056 0.126 2.25 36 0-075 0.107. I.4O 3 1.062 0.706 0.66 36 1-235 0-533 0-43 3 3 2.69 3-90 0-09? 0.07$ 0.026 30 30 2.64 3.82 0.14 ) o.i6S 0.047 3 3.07 o. So') 3 4.14 0-52 > o. 146 3 3-92 0.61 ) 30 30 3 2-73 3.86 o.737 0.81 > 0.87) 0.235 15 0.231 1-339 5-797 15 0.911 0-379 0.416 15 1.029 0.261 0.254 15 0.769 o. 241 0-313 15 1.256 0.194 0.154 15 1.444 0.156 0.108 INDEX Acenaphthene, i. Acetamide, i. Acetanilide, i. Acetic acid, 2-4. in aq. benzene, 55. Acetnaphthalide, 6. Acetone, 6-7, 355. in aq. benzene, 55. in aq. ethyl acetate, 136. in aq. potassium chlorate, 241. in aq. potassium chloride, 247. in aq. potassium nitrate, 258. in aq. sugar, 326. Acetphenetidine, 8. Acet-toluide, 8. Acetyl acetone, 9. Acetylene, 8. Aconitine, 9. Adipic acid, 9. Air, 10. Alanine, 10. Aldehyde, n. propionic, 267. Alcohols, ii, 355. Alcohol in aq. benzene, 55. in aq. etner, 135. in aq. ethyl acetate, 136. in aq. ethyl butyrate, 136. in aq. ethyl propionate, 136. in aq. ethyl valerate, 137. in aq. methyl butyrate, 204. in aq. propyl acetate, 267 in aq. potassium carbonate, 239, in aq. potassium chlorate, 241. in aq. potassium nitrate, 258. in aq. sodium carbonate, 297. in aq. sodium nitrate, 308-9. in aq. sodium sulphate, 314. in aq. sugar, 325. Allyl isosulphocyanic ester, 205. Aluminum chloride, 12. rubidium alum, 271. sulphate, 12. sulphate + Lithium sulphate ,176. tellurium alum, 332. Alums, ammonium, potassium, etc., 13- caesium, 80. chromium, 116. iron ammonium, 33. rubidium, 271. tellurium, 332. Amalgam, 278. Amido benzoic acids, 60. benzo sulphonic acids, 60. Amido brom benzo sulphonic acid, 57, nitro benzoic acids, 60. propionic acid, 10. phenols, 60. Amines, methyl, etc., 15-17. Ammonia, 17-19. lithium sulphate, water, 176. Ammonium acid formate, 26. acid oxalate, 30. alum, 13. arsenate, 20. benzoate, 20. bicarbonate, 2122. bicarbonate + NaHCO,, 298. bichromate, 25. bromide, 20. bromide + KBr, 235. bromp platinate, 20. cadmium bromide, 20, 71. cadmium chloride, 73. cadmium iodides, 77. cadmium sulphate, 33. carbonate, 21. carbonate in acetone, 6. cerium nitrate, 111-112. cerium sulphate, 112. chloride, 22-25. chloride and CuCl 2 , 125-126. chloride and KC1, 242. chloride and NaCl, 299-300. chloride and ZnCl 2 , 350. chromates, 25. chromium sulphate, 33. cobalt chlorides, 120. cobalt sulphate, 33. copper sulphate, 33, 129, 262. fluo boride, 26. fluo silicate, 31. formate, 26. iodate, 26. iodide, 26-28. iridium sulphate, 34. iron sulphate, 33. lead cobalticyanide, 2 a. magnesium nitrate, 30. magnesium sulphate, 34. manganese molybdate, 30. manganese sulphate, 34. nickel sulphate, 34, 129. nitrate, 24, 28, 30. oxalate, 3031. permanganate, 31. persulphate, 35. phosphite, 31. platinic chloride, 232-233, 357 INDEX Ammonium salicylate, 31. sodium sulphate, 34. sodium sulphite, 35. sulphate, 24, 31-33. sulphate + K 2 SO 4 , 261. sulphocyanide, 35. tetra chromate, 25. tri chromate, 25. tri nitrate, 29. uranyl carbonate, 22. uranyl chlorides, 342. uranyl nitrate, 343. uranyl propionate, 343. vanadium sulphate, 34. zinc sulphate, 34, 129. Amyl acetate, 35. alcohol, ii. butyrate, 35. formate, 35. malonic acid, 186. propionate, 35. Amylene hydrate, 355. Anethol, 35. in aq. acetone, 6. Anilin, 36-38. Anis acid, 38, 61. Anthracene, 39. Anthraquinone, 40. Antimony potassium tartrate, 41. tri chloride, 40-41. tri iodide, 41. Apo morphine hydrochloride, 205. Argon, 41. Arsenic iodide, 41. pentoxide, 41. tri iodide, 42. Asparagine, 42. Astrakanite, 312. Atropine, 42. Aurous, auric, see Gold. Azelaic acid, 43. Azo phenetol, 43. Barium acetate, 43. acid oxalate, 52. arsenate, 43. bromate, 44. bromide, 44. butyrate, 44. cadmium chloride, 74. caproate, 45. carbonate, 45. chlorate, 45. chloride, 24, 4647. chloride + NaCl, 300. chromate, 47. citrate, 47. cyanide, 48. dibrom, etc., sulphonic acid, 57. ferrocyanide, 48. fluoride, 48. formate, 48, 165. hydroxide, 48. iodate, 49. Barium iodide, 49. iodide -f BaBr 2 , 44. iodide + Hg(CN) 2 , 197. iso caproate, 45. iso succinate, 53. malate, 49. malonate, 49. molybdate, 49. nitrate, 24, 29, 5051. nitrate + BaCl 2 , 46. nitrate + KNO 3 , 254. nitrite, 51. oxalate, 51. persulphate, 53. potassium ferrocyanide, 48. propionate, 52. succinate, 53. sulphate, 52-53. tartrate, 53-54- Benzamide, 54, 355. Benzaldehyde, 54. Benzene, 54-56. Benzine, 58. Benzoic acids, 58-62, 341. Benzoic sulphinide, 62. Benzophenone, 6, 63. Benzo sulphonic acids, 57, 60. Benzoyl phenyl hydrazine, 57. Benzyl carbamide, 104. Beryllium, see also Glucinium. Beryllium hydroxide, 63. salts, 140. sulphate, 63. Beta Naphthol, 208. Borax, 293. Boric acid, 65-67, 294. Boron tri-fluoride, 67. Bismuth, 64. and Pt alloys, 232. chloride, 64. iodide, 64. nitrate, 64. oxide, 64. Bromal hydrate, 355. Brom benzene (di) ,56. benzoic acid, 60. benzo sulphonic acid, 57. cinnamic acid, 118. phenols, 226. Bromine, 6769. Brucine, 69. Butane, 69. Butyl acetate, 69. alcohol, 12. alcohol tertiary, 355. chloral hydrate, 355. formate, 69-70. malonic acid, 186. Butyric acid (iso), 70. aldehyde, 69. Cadmium ammonium bromide, 20, 71. ammonium chloride, 73. ammonium iodides, 77. 358 INDEX Cadmium ammonium sulphate, 33. barium chloride, 74. bromide, 70-71. caesium sulphate, 84. chlorate, 72. cyanide, 76. fluoride, 77. hydroxide, 77. iodide, 77. magnesium chloride, 74. nitrate, 78. oxalate, 78. potassium bromide, 71. potassium chloride, 76. potassium iodide, 78. potassium sulphate, 79. rubidium bromide, 72. rubidium chloride, 75. rubidium sulphate, 274. sodium bromide, 72. sodium iodide, 78. sodium sulphate, 80. sulphate, 78-79. Caesium alums, 15, 80. cadmium sulphate, 84. carbonate, 81. chloraurate, 81. chloride, 81. chloride + FeCl 3 , 159. chlor tellurate, 82. chromium alum, 80. cobalt sulphate, 84. copper sulphate, 84. fluoboride, 81. gold chloride, 141. iodate, 82. iodide, 82. indium alum, 80. iron alum, 80. iron sulphate, 84. magnesium sulphate, 84. manganese sulphate, 84. mercuric bromide, 81. nickel sulphate, 84. nitrate, 82. oxalate, 83. permanganate, 83. platinic chloride, 232. selenate, 83. sulphate, 83. tellurium halides, 332. thallium chloride, 82. uranyl chloride, 342. uranyl nitrate, 343. vanadium alum, 80. zinc sulphate, 84. Caffeine, 84. Calcium acetate, 84-85. bicarbonate, 8788. bitartrate, 103. bromide, 85. bromide -f Hg(CN) 2 , 197. butyrate, 86. Calcium caproate, 86. caprylate, 86. carbonate, 86. chlorate, 88. chloride, 88-89. chromate, 90. citrate, 89. di ethyl acetate, 85. di propyl acetate, 85. fluoride, 90. formate, 90. heptoate, 91. hydroxide, 91. hydroxide + CaSO 4 , 99. iodate, 94. iodide, 94. iso butyrate, 86. iso butyl acetate, 85. iso .succinate, 97. iso valerate, 104. malate, 94. malonate, 94. methyl ethyl acetate, 85. methyl pentanate, 86. methyl propyl acetate, 85, nitrate, 95. nonate, 96. oenanthate, 91. oxalate, 95. oxide, 91. pelargonate, 96. phosphates, 95-96. potassium ferrocyanide, 90, potassium sulphate, 101. propionate, 96. selenate, 97. silicate, 97. succinate, 97. sulphate, 97-102. sulphide, 102. sulphite, 103. tartrate, 103. tri methyl acetate, 85. valerate, 104. Camphoric acid, 104. Cane sugar, 324-326. Caoutchouc, 104. Carbamides, 104. Carbazole, 104. Carbon bisulphide, no. dioxide, 105-107. monoxide, 107-110. oxysulphide, in. tetra chloride, 201. Carvoxime, in. Cerium acetate, 1 1 1 . ammonium nitrate, 111112. ammonium sulphate, 112. butyrate, in. formate, in. iso butyrate, in. propionate, in. sulphate, 112. Chinin, 117. 359 INDEX Chinidin, 117. Chlor acetic acid, 5. Chloral hydrate, 113, 355. hydrate butyl, 355. Chlor benzene, 56. benzoic acid, 60. Chlorine, 113-114. monoxide, 115. tri oxide, 115. Chloroform, 115. Chlor phenols, 226. Chromic acid, 25, 116, 304. Chromium alums, 116. ammonium sulphate, 33. caesium alum, 80. chloride, 116. double salts, 116. potassium cyanide, 250. potassium molybdate, 116. rubidium alum, 271. sulphate, 116. tellurium alum, 332. tri oxide, 25, 116, 304. Chrysarobin, 116. Chrysen, 117. Cinchona alkaloids, 117. alkaloids salts, 117. Cinnamic acid, 118. Citric acid, 119. Cobalt ammonium chlorides, 120. ammonium sulphate, 33. bromide, 119. caesium sulphate, 84. chlorate, 119. chloride, 120-121. double salts, 119. Cobalticyanide of NH 3 + Pb, 22. Cobalt iodate, 121. iodide, 121. lead cyanide, 165. lead potassium cyanide, 165. nitrate, 121-122." potassium sulphate, 262. rubidium nitrite, 122. rubidium sulphate, 274. sulphate, 122-123. Cocaine, 123. hydrochloride, 123. Codeine, 123. salts, 123. Colchicine, 123. Collidin, 124. Copper and Pt alloys, 232. acetate, 124. ammonium chloride, 125126. ammonium sulphate, 33, 129. bromide, 124. caesium sulphate, 84. chlorate, 124. chloride, 124128. nitrate, 128. potassium chloride, 127. potassium sulphate, 131, 262. Copper rubidium sulphate, 274. sodium sulphate, 131. sulphate, 32, 128-131. sulphate + CuCl 2 , 126. sulphate + MnSO 4 , 188. sulphate + NiSO 4 , 211. sulphide, 131. tartrate, 132. tellurium sulphate, 334. Cream of tartar, 265-266. Cresol, 131. Cumidin (pseudo), 132. Cuminic acid, 132. Cuprous, cupric, see Copper. Cyanogen, 132. Dextrose in aq. acetone, 7. Di acetin, 355. Di brom benzene, 56. Di chlor acetic acid, 6. Didymium potassium sulphate, 133. sulphate, 133. Di ethyl amine, 16. ethyl ketone, 137. ethyl sulphone, 355. Di methyl sulphone, 355. Di nitro benzenes, 56-57. nitro phenols, 226. Di phenyl, 227. phenyl amine, 17. Erbium sulphate, 133. Ervthrite, 133. Ethane, 133. Ether, 134-135- . in anthraquinone, 40. Ethyl acetate, 135-136. alcohol, see Alcohol. amines, 16. ammonium bromide, 20, ammonium chloride, 25. ammonium iodide, 27. bromide, 137. butyrate, 136. carbamate, 138. Ethylene, 138. chloride, 137. cyanide, 323. Ethyl formate, 136. Ethylidine chloride, 137. Ethyl iodide, 137. iso valerate, 137. ketone, 137. malonic acid, 186. methyl ketone, 204. propionate, 136. urethane, 355. valerate, 137. Fats, fatty acids, 138. Ferrous, ferric, see Iron. Ferri, ferrocyanide of potassium, 250. Formaldehyde, n. Fumaric acid, 139. Furfurol, 139. Gadolinium sulphate, 139. 360 INDEX Galactose, 139. Gallic acid, 139, Germanium dioxide, 140. potassium fluoride, 251. sulphide, 140. Glass, 140. Glucinium, see also Beryllium. Glucinium hydroxide, 63. salts, 140. sulphate, 63. Glutaric acid, 140. Glycolic acid, 140. Gold, 140. alkali chlorides, 140. caesium chlorides, 81. chloride, 141. phosphorus tri chloride, 141. Grape sugar, 325-326. Guaicol, 141. carbonate, 141. Guanidine, 141. Helium, 142. Hexane, 142. Hippuric acid, 142. Homatropine, hydrobromide, 143. Hydrastine, 143. chloride, 143. Hydrazine sulphate, 143. Hydriodic acid, 145. Hydrobromic acid, 143. Hydrochloric acid, 144. Hydrofluoric acid, 145. Hydrogen, 145149. sulphide, 150. Hydroquinone, 150-151. Hydroxy benzoic acids, 61. Hydroxylamine, 151. hydrochloride, 151. Hyoscyamine, 151. Hyoscine hydrobromide, 151. Indium ammonium sulphate, 34. caesium alum, 80. lodic acid, 145. Iodine, 152154. lodo benzoic acid, 60. Iron ammonium alum, 33. ammonium sulphate, 33. caesium alum, 80. caesium sulphate, 84. chloride, 157159. chloride mix crystals, 159. hydroxide, 160. lead cyanide, 165. nitrate, 160. oxide, 1 60. phosphate, 160. potassium sulphate, 161, 262. rubidium alum, 271. rubidium sulphate, 274. sulphate, 160. sulphate + CdSO 4 , 79. sulphate + Na 2 SO 4 , 161. sulphide, 160. Iron tellurium alum, 332. amyl acetate, 35. amyl alcohol, 1 1 . amyl formate, 35. amyl malonic acid, 186. Iso butyric acid, 70. butyric aldehyde, 69. butyl acetate, 6970. butyl alcohol, 12. phthalic acid, 228. propyl benzoic acid, 132. Ketone, di ethyl, 137. methyl ethyl, 204. Lactic acid di ethyl amide, 355. Lanthanum bromate, 162. sulphate, 162. Lead, 162. and Pt alloys, 232. acetate, 162. ammonium cobalticyanide, 22. benzoate, 162. bromate, 162. bromide, 163. carbonate, 163. chlorate, 163. chloride, 163-165. chroma te, 165. citrate, 165. cyanides, 165. fluoride, 165. formate, 165. hydroxide, 166. hyposulphate, 170, iodate, 166. iodide, 166-167. malate, 167. nitrate, 168. nitrate + Ba(NO 3 ) 8 , 50. oxalate, 168. oxides, 1 68. palmitate, 169. phosphate, 169. succinate, 169. sulphate, 169. tartrate, 170. Levulose, 170. Ligroin, 170. Lime, see Calcium hydroxide Lithium benzoate, 170. bicarbonate, 172. bichromate, 173. borate, 170. bromate, 171. bromide, 171. carbonate, 171. chlorate, 172. chloraurate, 172. chloride, 172. chromate, 173. citrate, 173. fluoride, 173. formate, 174. INDEX Lithium gold chloride, 141. hydroxide, 174. hypophosphate, 176. iooate, 174. iodide, 175. la urinate, 176. myristate, 176. nitrate, 175. oleate, 176. oxalate, 175. palmitate, 176. permanganate, 176. phosphate, 176. stearate, 176. sulphate, 176. Magnesium ammonium nitrate, 30. ammonium sulphate, 34. bicarbonate, 178-179. bromate, 177. bromide, 177. bromide alcoholates, 177. bromide aliphatic compounds, 177. bromide etherates, 177. cadmium chloride, 74. caesium sulphate, 84. carbonate, 178-179. carbonate in aq. acetone, 6. chlorate, 180. chloride, 180-181. chroma te, 181. fluoride, 181. fluosilicate, 184. hydroxide, 181-182. hypophosphate, 184. iodate, 182. iodide, 182-183. iodide alcoholate, 183. iodide, alkyl esters, 183. iodide, aliphatic compounds, 183. iodide etherate, 183. nitrate, 184. oxalate, 184. platinic chloride, 181. platinic chromate, 181. potassium sulphate, 185. salicylate, 184. sulpnate, 184-185. sulphate + MgCl 2 , 181. sulphate + Na 2 SO 4 , 312. sulphite, 185. Maleic acid, 139. Malonic acid, 185-186. Maltose in aq. acetone, 7. Manganese ammonium molybdate,3o. ammonium sulphate, 34. borate, 186. bromide, 186. caesium sulphate, 84. chloride, 187. fluo silicate, 187. hypophosphate, 187. nitrate, 187. Manganese potassium vanadate, 189. sulphate, 188-189. sulphate + CuSO 4 , 130. Mannite, 189. Mannitol, 189. Mercury, 278. bromide, 189-190. caesium bromide, 81. chloride (ic), 190-196. chloride (ous), 196. chloride + BaCl 2 , 46. chloride + CsCl, 81. cyanide, 197. fulminate, 197. iodide, 197199. oxide, 200. sulphate, 200. tetra methyl amine chloride, 1 95 . Methane, 200. Methoxy benzoic acid, 38. Methyl acetate, 203. alcohol, 136. amine, 15. amine HgCl ? , 195. ammonium iodide, 26. benzoic acids, 61, 341. butyrate, 203-204. Methylene bromide, 203. chloride, 203. Methyl ethyl ketone, 204. iodide, 203. malonic acid, 186. phenyl carbamide, 104. propionate, 203. urethane, 355. valerate, 204. Milk sugar, 325-326. Molybdenum trioxide, 204. Monoacetin, 355. Mono chlor acetic acid, 6. Morphine, 204-205. salts, 205. Mustard oil, 205. Naphthalene, 206-207. in aq. acetone, 6. j8-Naphthalene picrate, 55. Naphthoic acid, 207. Naphthol, 208. Naphthylamine sulphonic acid, 206. Naphtion acid, 206. Narceine, 208. Narcotics, 355. Neodymium chloride, 208. sulphate, 208. Nickel ammonium sulphate, 34, 129. bromate, 208. bromide, 208. caesium sulphate, 84. chloride, 208-209. iodate, 209. iodide, 209. nitrate, 210. potassium sulphate, 212, 262. 362 INDEX Nickel sulphate, 210-212. tellurium sulphate, 334. Nicotine, 212. Nitranilines, o, m, and p, 38. Nitric oxide, 218. Nitro benzene, 56-57. benzoic acids, 6162. Nitrogen, 213-214. Nitrous oxide, 215-218. Nitro phenols, 226. Olive oil as solvent, 355. Ortho boric acid, 65-67. Oxalic acid, 31, 175, 219, 310. Oxygen, 220-221. Ozone, 221. Papaverine, 222. Paraffine, 222. Pentane acid, 348. Pentanon, 137. Petroleum benzine, 58. Phenacetine, 8. Phenanthrene, 222-223. picrate, 223. Phenic acid, 223. Phenol, 223-225. Phenols (amido), 60. Phenol anilin mixtures, 38. Phenolate of phenyl ammonium, 226. Phenyl ammonium, phenolate, 226. amines, 17. di amines, 226. guanidine (tri), 141. nydrazine (benzoyl), 57. methane (tri), 201-203. salicylate, 227. thio carbamide, 344-346. thio urea, 344-346. Philocarpine salts, 231. Phosphorus, 227-228. Phosphomolybdic acid, 227. Phthalic acids, 228. anhydride, 228-229. Physostigmine salts, 229. Picric acid, 229231. Pipeline, 231. Platino amines, 233. Platinum alloys, 232. ammonium bromide, 20. bromide, 232. double chlorides, 232. potassium bromide, 232. Plumbic, see Lead. Potassium acetate, 233. acid formate, 251. acid nitrate, 257. acid oxalate, 259. acid sulphate, 264. alum, 13-14. antimony tartrate, 41. arsenate (di hydrogen), 233. barium ferrocyanide, 48. benzoate, 233. bicarbonate, 238-239. bitartrate, 265-266. Potassium borates, 234. boride (fluo), 234. bromate, 234-235. bromide, 235-238. bromide and chloride, 242. bromide + Hg(CN) 2 , 197. butyrate, 238. cadmium bromide, 71. cadmium chloride, 76. cadmium iodide, 78. cadmium sulphate, 79. calcium ferrocyanide, 90. carbonate, 238-239. carbonate in aq. acetone, 6. carbonate in aq. ammonia, 18 carbonyl ferrocyanide, 250. chlorate, 239-241. chlorate + T1C1O 3 , 335. chloride, 24, 241-248. chloride + BaCl 2 , 46. chloride + CaCl 2 , 89. chloride + FeCl 3 , 159. chloride + HgCl 2 , 191. chloride + Hg(CN) 2 , 197. chloride + KBr, 236. chloride + KNO 3 , 255. chloride + NaCl, 300. chloride + Na 2 SO 4 , 312. chromates, 248-249. chromates + K 2 SO 4 , 263. chromium alum, 116. chromium molybdate, 116. chromisulphocyanide, 250. chromocyanide. 250. cobalt sulphate, 262. copper chloride, 127. copper sulphate, 131, 262,, citrate, 249. cyanate, 249. cyanide, 249. di chromate, 248-249. didymium sulphate, 133. ferric yanide, 250. ferrocyanide, 250. ferrosulphate, 262. fluoride, 250. fluo boride, 234. fluo germanate, 251. fluo titanate, 266. formate, 251. gold chloride, 141. hippurate, 142. hydroxide, 251. hypophosphate, 260. hypophosphite, 260. iodate, 252. , iodide, 252-253. iodide and bromide, 236. iodide and chloride, 243. iodide and PbI 2 , 167. iodide and Hg(CN) 2 , 197. iron sulphate, 161. lead cobalticyanide, 165. 363 INDEX Potassium lead ferricyanide, 165. magnesium chloride, 181. magnesium chromate, 181. magnesium cyanide, 181. magnesium sulphate, 185. manganese vanadate, 189. mercuric cyanide, 197. nickel sulphate, 212, 262. nitrate, 24, 29, 254-258. nitrate + Ba(NOg) 2 , 50. nitrate + KBr, 237. nitrate + KC1, 244. nitrate + NaCl, 300. nitrate + NaNO 3 , 308. nitrite, 254. oxalate, 258-259. perchlorate, 241. perchlorate + KMnO 4 , 260. persulphate, 264. permanganate, 259-260. phosphate, 260. phosphite, 260. phosphomolybdate ,261. platinic bromide, 232. platinic chloride, 232-233. selinate, 261. sodium carbonate, 239. sodium sulphate, 263. sodium sulphite, 264. sodium thio sulphate, 264. stannate, 261. sulphate, 24, 32, 261-264. sulphate -f KC1, 245. sulphate + KNO 3 , 256, sulphate + NaCl, 300. sulphate + Na 2 SO 4 , 312. sulphocyanide, 265, 291. tartrate, 265-266. tellurium bromide, 332. thio cyanate, 291. tri chromate, 249. uranyl butyrate, 343. uranyl carbonate, 239. uranyl chloride, 342. uranyl nitrate, 343. uranyl sulphate, 344 vanadate, 266. zinc vanadate, 266. Praseodymium sulphate, 267- Propio nitril, 267. Propionic acid (amido), 10. aldehyde, 267. Propylene, 268. Propyl acetate, butyrate, etc., 267- 268. acetic acid, 348. alcohol in aq. K 2 CO 3 , 239. ammonium iodide (tetra), 28. anisol (/?), 35. bromide, chloride, etc., 268. formate, 268. malonic acid, 186. Pseudo cumidin, 132. Pyrene, 268. Pyrogallol, 268. Pyrotartaric acid, 140. guinine and salts, 117, 269. acemic acid, 331. Resorcinol, 270 Rhodium salts, 270. sodium nitrite, 309. Rubidium alums, 15, 271. bromide, 271. brom iodide, 273. cadmium bromide, 72, cadmium chloride, 75. cadmium sulphate, 274. carbonate, 271. chlorate, 271. chloride, 272. chromate, 272. cobalt nitrate, 122. cobalt sulphate, 274, copper sulphate, 274. di chromate, 272. fluo boride, 271. fluo silicate, 273. gold chloride, 141. hydroxide, 272. iodate, 272. iodide, 272-273. iron sulphate, 274. nitrate, 273. mercuric chlorides, 192. perchlorate, 271. permanganate, 273. permanganate + KM nO 4 , 260. platinic chloride, 232. selenate, 273. silico tungstate, 273. sulphate, 273274. tellurium bromide, 332. tellurium chloride, 272, 332 thallium chloride, 272. uranyl chloride, 342. uranyl nitrate, 343. Saccharine, 61. Salicylamid, 355. Salicylic acid, 61, 274-276. Salol, 227. Selenious acid, 277. Selenium, 276. Senfol, 205. Silicon, 277. Silico tungstic acid, 277. Silver, 278. and Pt alloys, 232. acetate, 278. benzoate, 279. borate, 279. bromate, 279280. bromide, 280281. butyrate, 281. caproates, 282. carbonate, 282. chlorate, 282. 364 INDEX Silver chloride, 283-286, chromate, 286. citrate, 286. cyanide, 286. di chromate, 286. di ethyl acetate, 279. di propyl acetate, 278. fluoride, 287. fulminate, 287. heptoate, 287. hydroxide -f AgCl, 285. iodate, 287. iodide, 277, 287-288. iso butyrate, 281. malate, 288. methyl ethyl acetate, 279. mono chlor acetate, 278. nitrate, 288-289. nitrate + KNO 3 , 257. nitrite, 289. onanthylate, 287. oxalate, 289. oxide, 289. permanganate, 289. phosphate, 289. propionate, 290. salicylate, 290. sodium cyanide, 286. succinate, 290. sulphate, 290291. sulphate + CaSO 4 , 101. sulphocyanide, 291. tartrate, 291. thallous cyanide, 286. thio cyanate, 291. tri methyl acetate, 279. valerates, 291292. vanadate, 292. Sodium acetate, 292-293. acid formate, 305. alum, 15. ammonium sulphate, 34. ammonium sulphite, 35. arsenate, 293. benzoate, 293. bicarbonate, 22, 297-298. bicarbonate + NaCl, 300. bisulphate, 315. borate, 294. bromate, 294. bromide, 295. cadmium bromide, 72. cadmium iodide, 78. cadmium sulphate, 80. carbonate, 296-297. carbonate in aq. acetone, 6. chlorate, 298-299. chloride, 24, 299-303. chloride + BaCl 2 , 46. chloride + CaCl 2 , 89. chloride + FeCl 3 , 159. chloride + Hg(CN) 2 , 191. chloride + KC1, 245. Sodium chloride + KNO 8 , 256. chloride + Na,CO s , 298. chloride + NaCIO,, 299. chroma tes, 303304. citrate, 305. copper sulphate, 131. ferrocyanide, 305. fluoride, 305. fluoride phosphate, 310. fluo silicate, 305. fluo zirconate, 316. formate, 305. gold chloride, 141. hydrogen arsenate, 293. hydroxide, 306. hydroxide + NaCl, 301. hypophosphates, 311. hypophosphite, 311. iodate, 306. iodide, 306. iodide + Hg(CN) 2 , 197. mercuric chloride, 193. mono chromate, 303-304. molybdate, 307. nitrate, 29, 307-309. nitrate -f KNO 3 , 256. nitrate 4- NaCl, 301. nitrate + AgNO 3 , 288. nitrite, 309. p nitro phenol, 310. oxalate, 309-310. phosphates, 310. phosphites, 311. potassium carbonate, 239. potassium sulphate, 263. potassium sulphite, 264. potassium thio sulphate, 264. rhodonitrite, 309. salicylate, 275, 355. selinate, 311. silver cyanide, 286. stannate, 311. sulphate, 311315. sulphate -f CoSO 4 , 122. sulphate + CuSO 4 , 131. sulphate + FeSO 4 . 161. sulphate + NiSO 4 , 211. sulphate + ZnSO 4 , 353. sulphite, 315. telluriate, 315. tetra borate, 293. tetra chromate, 304. thio sulphate, 315. tri molybdate, 307. tungstate, 316. uranyl chromate, 343. wolfromate, 316. Stannous, stannic, see Tin. Strontium benzoate, 316. bicarbonate, 316. bromate, 316. bromide, 316. carbonate, 316. 365 INDEX Strontium chlorate, 317. chloride, 317. chromate, 318. di tungstate, 321. fluoride, 318. hydroxide, 318. hyposulphate, 170. iodate, 318. iodide, 318. iodide + Hg(CN) 2 , 197. malate, 319. molybdate, 319. nitrate, 319. nitrate + Pb(NO 3 ) 2 , 168. oxalate, 319. salicylate, 319. sulphate, 320. tartrate, 320-321. tungstate (di), 321. Strychnine and salts, 321. Suberic acid, 321. Succinic acid, 322323. anhydride, 322. nitril, 323. Succinimid, 323. Sugar, 324-326. in aq. acetone, 7. + K. Butyrate, 238. + MgSO 4 , 185. Sulphanilic acid, 326. Sulphonal, 355. Sulphonic acids, 57. Sulphur, 327-328. in anilin, 36. in benzene, 56. dioxide, 329-331. trioxide, HgO and H 2 O, 200. Syngenite, 101. Tannic acid, 331. Tartar emetic, 41. Tartaric acid, 331. Telluric acid, 332. Tellurium, 331. caesium bromide, 332. caesium chloride, 82, 332. chromium alum, 116. mercuric cyanide, 197. potassium bromide, 332. rubidium bromide, 332. rubidium chloride, 272, 332. Terephthalic acid, 228. Tetra boric acid, 67. chlor methane, 201. ethyl ammonium bromide, 20. ethyl ammonium chloride, 25. ethyl ammonium iodide, 27. methyl ammonium iodide, 26. >, propyl ammonium iodide, 28. sodium chromate, 304. Tetronal, 355. Thallium alum, 14, 15, 332. bromate, 332. bromide, 332. caesium chloride, 82. carbonate, 338. chlorate, 333. chloride, 333~335- chromate, 335. copper sulphate, 338. cyanide, 336. fluoride, 336. iodate, 336. iodide, 336. nickel sulphate, 338. nitrate, 336. nitrate + KNO 3 , 257. oxalate, 336-337. perchlorate, 338. phosphate, 337. picrate, 337. ^ platinic chloride, 232. rubidium chloride, 272. silver cyanide, 286. sulphate, 338. sulphide, 338. sulphite, 339. sulphocyanide, 338. vanadates, 339. zinc sulphate, 338. Thallous tri chromate, 335. Thallo thallic chloride, 335. Theobromine, 339. Thio urea (phenyl), 344346. Thorium selenate, 339. sulphate, 339. Tin chloride, 340. hydroxide, 340. iodide, 340-341. sulphate, 341. Toluene, 341. Toluidine, 341-342. Toluyl acids, 341. Tolyl carbamide, 104. Tri acetin, 355. brom phenols, 226. chlor phenols, 226. chlor acetic acid, 6. ethyl amine,- 16. methyl amine, 15. nitro benzene, 57. oxymethylene, 1 1 . phenyl amine, 17. phenyl guanidine, 141. phenyl methane, 201. Trional, 355. Tungsto silicic acid, 277. Uranyl ammonium carbonate, 22. ammonium propionate, 343. chloride, 342. 366 INDEX Uranyl double chlorides, 342. double nitrates, 343. nitrate, 343. potassium butyrate, 343. potassium carbonate, 239. potassium sulphate, 344. sodium chromate, 343. sulphate, 344. Urea, 344-346. Urethane, 347. Uric acid, 347. Valerianic acid, 348. Valeramide, etc., 355. Vanadium ammonium sulphate, 34. caesium alum, 80. rubidium alum, 271. tellurium alum, 332. Ytterbium sulphate, 348. Yttrium iodate, 348. Zinc and Pt alloys, 232. Zinc acetate, 348. ammonium sulphate, 34, 129. Zinc benzoate, 348. bromide, 348. caesium sulphate, 84. carbonate, 349. chlorate, 349. chloride, 349-350. cyanide, 349. fluoride, 350. hydroxide, 350-351. iodate, 351. iodide, 351. nitrate, 351. oxalate, 352. potassium sulphate, 262. potassium vanadate, 266. sulphate, 352-353. sulphate + CuSO 4 , 130. sulphite, 353. tartrate, 353. tellurium sulphate, 334. valerate, 353. 367 YC 21994 THE UNIVERSITY OF CAUFORNIA LIBRARY