Jhemical Experiment!' 
 
 General and uivtical 
 
 Yv'illiams 
 
 
i of Olivias Lry 
 
 LIBRARY 
 
 OF THE 
 
 UNIVERSITY OF CALIFORNIA 
 
 01 FT OP" 
 
 x? ^ 
 
 Received 
 Accession No.> Sl5~~ . C/<25S A/b 
 
CHEMICAL EXPERIMENTS 
 
 GENERAL AND ANALYTICAL 
 
 FOR USE WITH ANY TEXT-BOOK OF CHEMISTRY, OR 
 WITHOUT A TEXT-BOOK 
 
 K. P. WILLIAMS 
 
 N x 
 
 Instructor in Chemistry, English High School, Boston, and 
 
 Author of " Introduction to Chemical Science," 
 
 " Laboratory Manual," etc. 
 
 OS t 
 
 t_ 
 . _ . __ 
 
 BOSTON, U.S.A., AND LONDON 
 
 PUBLISHED BY GINN & COMPANY 
 
 1895 
 
COPYRIGHT, 1895 
 BY R. P. WILLIAMS 
 
 ALL BIGHTS RESERVED 
 
PEEFAOE. 
 
 THE rapid growth of the laboratory method of teaching chem- 
 istry since the author's Manual was issued in 1888 has called for a 
 larger and more comprehensive work of a similar sort for high 
 schools, academies, and colleges. To such a call tfre present book 
 is a response. 
 
 In preparing the experiments the author has endeavored, first, 
 to select such as are most instructive and best illustrate the subject 
 without being too elaborate ; second, to arrange them in an order 
 calculated to lead up by the most natural and easiest steps to a 
 knowledge of the science ; third, to make the subject fascinating 
 by giving just enough information and suggestion to interest the 
 experimenter, and to make him work for the knowledge to be 
 gained. Finally, the author has aimed to make the book simple 
 enough for the dull and slow pupil, and by the introduction of 
 supplementary and original work elaborate enough for the most 
 acute. Great care has been taken to give minute and accurate 
 directions for performing the experiments. " Terms " at the end 
 of experiments are for pupils to study outside the laboratory, and 
 are often repeated. They may also be discussed in the laboratory. 
 
 Metal analysis has received a somewhat unique treatment. 
 Each metal of a group is first taken separately, and the analytical 
 reactions are given. This method shows the pupil at once why a 
 given re-agent is added, and what its effect is. The product is 
 given when the substance is in solution as well as when it is 
 precipitated. The group is next treated in the same way. This 
 method clarifies the subject greatly in the pupil's mind, and is 
 believed to be a valuable departure in teaching analysis. 
 
iv PREFACE. 
 
 The new orthography recommended by the Chemical Section 
 of the A. A. A. S. has been adopted, as a step towards uniformity 
 and progress. 
 
 It is recommended that wherever it is possible each laboratory 
 period cover the space of two hours (even if there can be only one 
 period per week), and that the last 20 or 30 minutes be taken to 
 question the class rapidly on the work of the day, discuss and 
 explain the use of terms, etc. The books should be inspected 
 after each exercise, or perhaps after each experiment has been 
 written out. 
 
 It is by no means necessary to perform every experiment, or to 
 follow the order here given, if the teacher prefers to do otherwise. 
 A diversity of opinion exists among teachers, and a diversity of 
 time and talent among pupils and classes. In no place better than 
 in the laboratory, under a competent instructor, can a " cast-iron 
 rule " be done away with, and variety of arrangement and method 
 be adopted. 
 
 The author would be glad to receive criticisms, as well as 
 suggestions as to other methods, or experiments, or different ways 
 of performing experiments. Especially would he be glad to know 
 what it has been difficult, in the matter of directions or principles, 
 for pupils to understand. 
 
 The author desires to acknowledge valuable suggestions in the 
 preparation of this work from the following persons : Messrs. J. Y. 
 Bergen, Jr., C. W. Gerould, E. F. Holden, A. S. Perkins, K S. 
 French, H. I. Lord, E. S. Chapin ; and Misses D. M. Stickney, 
 M. L. Foster, and others. 
 
 CAMBRIDGE, 
 
 December 1, 1895. 
 
INDIVIDUAL APPARATUS. 
 
 Each pupil should be provided with the apparatus given below, but in cases 
 where great economy must be exercised different pupils may, by working at 
 different times, use the same set. The author has selected apparatus specially 
 adapted, as to exact dimensions, quality, and cheapness, for performing in the 
 best way the experiments herein described, and sets or separate pieces of this, 
 together with other apparatus and chemicals, can be had of the L. E. Knott 
 Apparatus Co., 14 Ashburton Place, Boston, to which firm teachers are referred 
 for catalogs. 
 
 4 re-agent bottles, 250 cc. glass stop- 
 pers, blown labels: NH 4 OH, 
 HC1, HNO 3 , H 2 S0 4 . 
 
 1 pneumatic trough. 
 
 1 Hessian crucible. 
 
 2 beakers. 
 
 2 pieces wire gauze. 
 
 1 piece platinum wire. 
 
 1 mouth blowpipe. 
 
 6 pieces glass tubing. 
 
 4 pieces hard glass tubing. 
 
 1 test-tube brush. 
 
 1 small tube brush. 
 
 1 doz. test tubes. 
 
 4 cork stoppers, for tubes. 
 
 1 fish-tail attachment for Bunsen 
 
 burner. 
 
 1 blowpipe attachment with rest for 
 Bunsen burner. 
 
 piece sheet copper. 
 
 glass retort. 
 
 tumbler. 
 
 piece cobalt glass. 
 
 horn spatula. 
 
 sheet litmus paper. 
 00 filter papers. 
 
 bunch splints. 
 
 sheet turmeric paper. 
 
 1 camel's-hair brush. 
 
 1 magnet. 
 
 4 wide-mouthed bottles. 
 
 1 2-holed rubber stopper to fit above. 
 
 4 pieces window-glass. 
 
 glass funnel. 
 
 porcelain evap. dish. 
 
 asbestos board. 
 
 sand bath. 
 
 pair iron forceps. 
 
 triangular file. 
 
 round file. 
 
 piece copper wire. 
 1 piece lead wire. 
 1 piece zinc wire. 
 1 wooden test-tube holder. 
 1 wire test-tube rack. 
 1 thistle tube. 
 1 Bohemian flask. 
 1 2-holed rubber stopper to fit flask. 
 
 Bunsen burner, 
 iron ring stand. 
 
 2 ft. rubber tubing. 
 1 ft. " " 
 1 metric ruler. 
 1 graduate. 
 1 small leaden dish. 
 
GENERAL APPARATUS. 
 
 The requirements of general apparatus for a laboratory are too numerous 
 and varied to be given here. A few of the pieces in more general demand for 
 experiments in this book are as follows : 
 
 Glass-stoppered bottles. 
 
 Graduates. 
 
 Funnels. 
 
 Fruit jars (for making solutions). 
 
 Scales, with metric weights. 
 
 Ignition tubes. 
 
 Beakers. 
 
 Filter-stands. 
 
 Glass and rubber tubing. 
 
 Steel glass-cutters. 
 
 Steel wire-cutters. 
 
 Mortars and pestles. 
 
 Flasks. 
 
 Filter papers, etc., etc. 
 
 CHEMICALS. 
 
 ESTIMATE FOR A CLASS OF TWENTY IN GENERAL CHEMISTRY AND ANALYTICAL 
 REACTIONS, NOT INCLUDING GENERAL REACTIONS AND SUPPLEMENTARY 
 WORK. 
 
 Acid, acetic, HC 2 H 3 O 2 4 Ib. 
 
 " boric, H 3 B0 3 i " 
 
 " hydrochloric, HC1 25 " 
 
 " hydrofluoric, HF i " 
 
 " hydrofluosilicic, H 2 SiF 6 .... i " 
 
 " nitric, HNO 3 12 " 
 
 " oxalic, H 2 C 2 4 f " 
 
 " phosphoric, H 3 PO4 J " 
 
 " sulfuric, H 2 S0 4 18 " 
 
 " tartaric, H 2 C 4 H 4 6 i " 
 
 Alcohol, C 2 H 5 OH 1 qt. 
 
 Alum, K 2 A1 2 (SO 4 ) 4 1 Ib. 
 
 Aluminum chlorid, A1C1 3 -J- " 
 
 Ammonium carbon., (NH 4 ) 2 C0 3 1 " 
 
 chlorid, NH 4 C1 2 " 
 
 " hydroxid, NH 4 OH..20 " 
 
 " nitrate, NH 4 NO 3 1 " 
 
 " oxalate, (NH 4 ) 2 C 2 4 i " 
 
 " sulfate, (NH 4 ) 2 S0 4 .. i " 
 
 Antimony cryst., Sb ^ " ' 
 
 " chlorid, SbCl 3 i " 
 
 Arsenious oxid, As 4 O 6 1 oz. 
 
 Arsenopyrite, FeAsS Jib. 
 
 Barium chlorid, BaCl 2 i " 
 
 " hydroxid, Ba(OH) 2 i " 
 
 Bismuth oxychlorid, BiOCl i " 
 
 Calcium chlorid, CaCl 2 i ' 
 
 " fluorid, powdered, CaF 2 k " 
 " hypochlorite, CaCl 2 0.... i " 
 
 " sulfate, CaS0 4 i " 
 
 " oxid, CaO 2 " 
 
 Carbon bisulfid, CS 2 i 
 
 Charcoal, animal, gran., C 1 " 
 
 ' " powdered, C.. 1 " 
 " wood, u C.. 1 " 
 * C 20 pieces 
 
 Cobalt chlorid, CoCl 2 i Ib. 
 
 " nitrate, Co(N0 3 ) 2 .... 
 
 Cochineal 
 
 Copper, turnings, Cu 
 
 " sheet, Cu i 
 
 " chlorid, CuCl 2 1 
 
 " nitrate, Cu(NO 3 ) 2 i 
 
 ** oxid, CuO 1 
 
 i " 
 i " 
 3 " 
 
 VI 
 
CHEMICALS. 
 
 Vii 
 
 Copper sulfate, CuSO 4 i Ib. 
 
 Ether, (C 2 H 5 ) 2 i " 
 
 Gold leaf, Au 1 bk. 
 
 Indigo i Ib. 
 
 lodin, 1 2oz. 
 
 Iron, fine turnings, Fe 1 Ib. 
 
 " by hydrogen, Fe , -J- " 
 
 " perchlorid, FeCl 3 1 " 
 
 " protosulfid, FeS 5 " 
 
 " pyrite, FeS 2 i " 
 
 " sulfate, FeSO 4 1 " 
 
 Lead, sheet, Pb 1 " 
 
 " wire, i in. diam., Pb 12 ft. 
 
 " acetate, Pb(C 2 H 3 02)2 i Ib. 
 
 " chlorid, PbCl 2 i " 
 
 " nitrate, Pb(N0 3 ) 2 2 " 
 
 " protoxid, PbO i " 
 
 " tetroxid (red), Pb 3 4 i " 
 
 Litmus, cubes 1 oz. 
 
 Marble chips, CaC0 3 3 Ib. 
 
 Magnesium ribbon, Mg 10 ft. 
 
 " chlorid, MgCl 2 i Ib. 
 
 sulfate, MgSO 4 " 
 
 Manganese chlorid, MnCl 2 " 
 
 " dioxid, gran., Mn0 2 .. " 
 " powd.,Mn0 2 li " 
 
 Mercury, Hg $ " 
 
 " bichlorid, HgCl 2 " 
 
 " protochlorid, HgCl " 
 
 " pernitrate, Hg(N0 3 ) 2 .... i " 
 " protonitrate, HgN0 3 .... i " 
 
 " oxid, HgO 1 " 
 
 Nessler's sol i " 
 
 Phosphorus, P 2 oz. 
 
 Picture wire 1 roll 
 
 Platinum chlorid, sol., PtCl 4 loz. 
 
 Potassium, metallic, K " 
 
 " bromid, KBr Ib. 
 
 " carbonate, K 2 C0 3 1-J- " 
 
 " chlorid, KI " 
 
 u chlorate, KC1O 3 2 " 
 
 " chromate, K 2 CrO 4 .... i " 
 " cyanid, KCN " 
 
 Potassium, dichromate, K 2 Cr 2 O 7 1 Ib. 
 " ferrocy., K 4 Fe(CN) 6 .. 1 " 
 ' ferricy., K 3 Fe(CN) 6 .. f " 
 
 iodid,KI 1 " 
 
 " hydroxid, KOH 1 " 
 
 " nitrate, KN0 3 1 " 
 
 u nitrite, KN0 2 i " 
 
 *' permangan., KMnO 4 i " 
 " sulfocyanid, KSCN.... i " 
 " tartrate, K 2 C 4 H 4 6 .... i " 
 
 Silica, powdered, Si0 2 i " 
 
 Silver nitrate, AgNO 3 4 oz. 
 
 Sodium, metallic, Na fa " 
 
 " acetate, NaC 2 H 3 O 2 i Ib. 
 
 . " arsenite, HNa 2 As0 3 | " 
 
 " bicarbonate, HNaC0 3 .... i " 
 
 " bisulfate, HNaS0 4 i 
 
 " borate, Na 2 B 4 O 7 -J- " 
 
 " carbonate, Na 2 C0 3 3 * 
 
 " chlorid, NaCl 4 " 
 
 u hydroxid (caust.),NaOH 3 " 
 
 " nitrate, NaNO 3 2 " 
 
 " nitrite, NaNO 2 -J- 
 
 * oxalate, Na 2 C 2 O 4 \ " 
 
 " phosphate, HNa 2 P0 4 1 " 
 
 sulfate, Na 2 S0 4 
 
 " sulfid, Na 2 S 
 
 " sulfite, Na 2 S0 3 
 
 " thiosulfate, Na 2 S 2 3 
 
 Starch, C 6 Hi O 5 
 
 Strontium chlorid, SrCl 2 
 
 Sugar, Ci 2 H 22 On 
 
 Sulfur, brimstone, S 2 " 
 
 ** flowers, S 1 
 
 Tin bichlorid, SnCl 2 i " 
 
 Turmeric paper 1 sheet 
 
 Turpentine, Ci Hi 6 loz. 
 
 Zinc, gran., Zn 3 Ib. 
 
 " wire, i in. diam 12ft. 
 
 " (arsenic-free) lib. 
 
 " chlorid, ZnCl 2 i " 
 
 u nitrate, Zn(N0 3 ) 2 i u 
 
 Litmus paper i quire 
 
 1 
 
 I " 
 
 i " 
 
 1 " 
 
 i " 
 i" 
 
 1 " 
 
SOLUTIONS, ETC. 
 
 In making solutions for metal analysis, chlorids of the metals are usually 
 taken (except in Group I, in which nitrates are used, the chlorids being insol- 
 uble). From 25 e to 50 & of solids are usually dissolved hi 500 cc of distilled 
 water, and filtered if necessary. Many are sat., as Ca(O H) 2 . Substances for 
 analysis, as well as acids and other re-agents, should be C. P. Concentrated 
 acids are used unless the dilute are called for. 
 A few exceptional sols, are given below : 
 
 HNa2P0 4 , 40. (NH 4 ) 2 C0 3 , 100. (NH 4 ) 2 S0 4 , 5. 
 
 KCy, 50. KNO 2 , 50. NH 4 C1, 60. 
 
 K 2 Cr 2 7 , 25. KOH, 60. NaOH, 60. 
 
 Dilute acids are made by mixing one volume of concentrated acid with four 
 
 volumes of water. 
 NH 4 OH. If NH 4 OH of 26 is obtained, it should be diluted with three times its 
 
 volume of water before using. 
 HgN0 3 is best prepared by putting into a large e.d. say 25s of Hg, and adding 
 
 to it a mixture of 25 cc HNO 3 and 25 cc of H 2 O, and letting it stand till 
 
 action stops, then adding 400 cc or 500 cc of H 2 O. More Hg should be used 
 
 than will dissolve, and some should be left in the bottle. 
 PbCl 2 is only slightly soluble in water. A saturated sol. should be used. 
 BiClg is prepared by adding water and HC1 to oxychlorid of bismuth, BiOCl. 
 
 First add the H 2 O, then acidulate it with the acid, say 1 vol. of H Cl to 20 
 
 of H 2 O, it being insol. in H 2 O alone. 
 AsCl s . Add H 2 to sodium arsenite HNa 2 AsO 3 , then add HC1 with stirring till 
 
 effervescence stops. 
 SbCl 3 . Pour a little butter of antimony, SbCl 3 , into H 2 0, then acidulate with 
 
 HC1. 
 SnC^. This must also be acidulated with HC1, and a little Sn should be left hi 
 
 the bottom of the bottle. 
 CrCl 3 , This may be made from K 2 Cr 2 7 sol. by adding some HC1 (say ^) and a 
 
 little alcohol, boiling some time and letting it stand, when it turns from red 
 
 to green. 
 (NH 4 ) 2 S. Pass H 2 S gas into dilute NH 4 OH till the sol. gives no ppt. with 
 
 MgSO 4 sol., then filter. It should be nearly colorless. 
 (NH 4 ) 2 S X (ammonium polysulfid). Stir sulfur flowers in the (NH 4 ) 2 S, as above 
 
 prepared, then filter. It is yellow. 
 Cochineal sol, Grind up a handful of cochineal in a mortar, and add water, stir, 
 
 and filter. 
 
 Litmus sol. Pulverize litmus cubes, and add water. 
 Indigo sol. (sulfindigotic acid). Slowly mix and stir 5s indigo with 25 CC H 2 SO 4 
 
 (or better H 2 S 2 O 7 , fuming sulfuric acid) in a beaker immersed in cold 
 
 water. Cover the beaker, and after 48 hours add 500 cc H 2 0, stir and filter. 
 Many substances in sol. easily break up on standing, and hence should be freshly 
 
 prepared. 
 For acid radicals compounds of Na or K are commonly used, as they are 
 
 soluble. 
 
 vin 
 
RULES AND SUGGESTIONS FOR PUPILS. 
 
 Pupils should read .these rules carefully, and should refer to them whenever in 
 
 doubt on any point. 
 
 1. Each pupil should provide himself with a towel, to keep his bench clean, 
 and any apron or other clothing desired for protection in the laboratory. 
 A long linen duster or duck coat reaching to the feet is the best protection. 
 Without something of the sort clothing may be injured at any moment. 
 
 2. The bench at which the pupil works must be left clean and dry after 
 every laboratory exercise. Wipe off a ring-stand, lamp, or other apparatus on 
 which a re-agent has fallen, wipe out a p.t. after using it, and keep re-agent 
 bottles, apparatus, books, and lockers clean. 
 
 3. Pupils are held responsible for apparatus, and should replace anything 
 that is lost or broken. 
 
 4. In experimenting have your apparatus neatly arranged without artificial 
 props, wedges, or uncouth-looking material. Have every d.t. and stopper fit 
 tightly to prevent leakage of gas. If a gas generates well, but does not pass 
 into the rec. , there is some leakage, due probably to loose bearings. 
 
 5. In heating a t.t. on the r.s. hold the lamp in the hand, move it slowly, 
 and now and then take it away from the tube for a moment, to prevent 
 melting and breaking the latter. 
 
 6. Mixtures of solids should be made on paper. Be careful not to mix 
 chemicals or re-agents except as directed. 
 
 7. To shake the contents of a t.t. cover its mouth with the thumb (Exp. 4, 
 Fig. 10), or the hand, or a stopper, hold it away from the bench, and shake it 
 vigorously. 
 
 8. Never put down a stopper when using a re-agent bottle, but hold it 
 between the first and second fingers (Exp. 6, Fig. 11), and replace it when you 
 put down the bottle. Do not pour back any excess of a re-agent from a t.t. or 
 other rec. into a re-agent bottle, and do not dip a stirring rod into a re-agent 
 bottle. 
 
 9. In pouring a liquid into a t.t. (or graduate) hold the latter on a level with 
 the eye, and towards the light, so as to see any change. The thumb-nail may 
 be placed at the upper limit to which it is desired the liquid should reach. 
 When much heat is liberated, as when sulfuric acid is poured into water, a 
 tube-holder should be used ; paper folded several times serves for this purpose. 
 
 10. Pour only liquids, fine powders, or soluble salts into the sinks, always 
 opening the faucet first to let the water run. Other solids should be thrown 
 into the jars. Great care must be taken not to clog the discharge-pipes. 
 
 11. Have flasks and tubes perfectly dry on the outside before applying heat. 
 Tubes of thick glass, if they contain no liquid, should be heated gradually at 
 
 ix 
 
TABLE OF COMMON ELEMENTS. 
 
 ARRANGED ACCORDING TO ELECTRO-CHEMICAL ORDER. 
 
 NAME. 
 
 SYMBOL. 
 
 Oxygen 
 
 0" 
 
 Sulfur 
 
 S", iv (vi) 
 
 Nitrogen 
 
 N'", v - etc. 
 
 Fluorin 
 
 F', 00 
 
 Chlorin 
 
 Cl', 00 
 
 Bromin 
 
 Br', CO 
 
 lodin 
 
 T, (v) 
 
 Phosphorus 
 
 P"', 'V 
 
 Arsenic 
 
 As'", v 
 
 Chromium 
 
 Cr", '", vi 
 
 Boron 
 
 B"' 
 
 Carbon 
 
 CD, iv 
 
 Antimony 
 
 Sb"', v 
 
 Silicon 
 
 Si" 
 
 Hydrogen 
 
 H' 
 
 Gold 
 
 Au('), "' 
 
 Platinum 
 
 Pt("), IV 
 
 Mercury 
 
 Hg', " 
 
 Silver 
 
 Ag 7 
 
 Copper 
 
 Cu('), " 
 
 Bismuth 
 
 Bi'", ( v > 
 
 Tin 
 
 Sn", 'v 
 
 Cadmium 
 
 Cd" 
 
 Cobalt 
 
 Co", ('") 
 
 Nickel 
 
 Ni", ('") 
 
 Lead 
 
 Pb", OT, 
 
 Iron 
 
 Fe", "' 
 
 Zinc 
 
 Zn" 
 
 Manganese 
 
 Mn", ("') 
 
 Aluminum 
 
 Al'" 
 
 Magnesium 
 
 Mg" 
 
 Calcium 
 
 Ca" 
 
 Strontium 
 
 Sr" 
 
 Barium 
 
 Ba" 
 
 Sodium 
 
 Na' 
 
 Potassium 
 
 K' 
 
 AT. WT. 
 
 VAPOR DENSITY. 
 
 STATE, 
 
 16 
 
 16 
 
 G 
 
 32 
 
 32 
 
 S 
 
 14 
 
 14 
 
 G 
 
 19 
 
 
 G 
 
 35.5 
 
 35.5 
 
 G 
 
 80 
 
 80 
 
 L 
 
 127 
 
 127 
 
 S 
 
 31 
 
 62 
 
 S 
 
 75 
 
 150 
 
 S 
 
 52 
 
 
 S 
 
 11 
 
 
 S 
 
 12 
 
 
 S 
 
 120 
 
 
 S 
 
 28 
 
 
 S 
 
 1 
 
 1 
 
 G 
 
 197 
 
 
 S 
 
 197 
 
 
 S 
 
 200 
 
 100 
 
 L 
 
 108 
 
 
 S 
 
 63 
 
 
 S 
 
 207 
 
 
 S 
 
 117 
 
 
 S 
 
 112 
 
 56 
 
 S 
 
 59 
 
 
 S 
 
 58 
 
 
 S 
 
 206 
 
 
 S 
 
 56 
 
 
 S 
 
 65 
 
 32i 
 
 S 
 
 55 
 
 
 S 
 
 27 
 
 
 S 
 
 24 
 
 
 S 
 
 40 
 
 
 S 
 
 87 
 
 
 S- 
 
 137 
 
 
 S 
 
 23 
 
 
 S 
 
 39 
 
 
 S 
 
 A ( ) indicates a rare valence. Atomic weights are only approximate. 
 
 xii 
 
ABBREVIATIONS. 
 
 Ac. acetate, C 2 H 8 2 . 
 
 gr. green. 
 
 alk. alkali or alkaline. 
 
 insol. insoluble. 
 
 Am. ammonium, NH 4 . 
 
 i.t. ignition tube. 
 
 app. apparatus. 
 
 M. metal (valence 1). 
 
 b. black. 
 
 . o.f. oxidizing flame. 
 
 B.B. before the blowpipe. 
 
 Ox. oxalate. 
 
 B.B.C.C. before the blowpipe on 
 
 ppd. precipitated. 
 
 charcoal. 
 
 ppg. precipitating. 
 
 bl. blue. 
 
 ppn. precipitation. 
 
 cc. cubic centimeters. 
 
 ppt. precipitate. 
 
 cm. centimeters. 
 
 p.t. pneumatic trough. 
 
 col. color. 
 
 qcm. square centimeters. 
 
 cone. concentrated. 
 
 re-agt. re-agent. 
 
 cpd. compound. 
 
 rec. receiver. 
 
 cryst. crystalline. 
 
 res. residue. 
 
 Cy. cyanid, CN. 
 
 r.f. reducing flame. 
 
 dil. dilute. 
 
 r.s. ring stand. 
 
 dis. dissolve. 
 
 sat. saturate. 
 
 dist. distinguish. 
 
 sep. separate. 
 
 d.s. deflagrating spoon. 
 
 si. slight or slightly. 
 
 d.t. delivery tube. 
 
 sol. solution or soluble. 
 
 e.d. evaporating dish. 
 
 sp. gr. specific gravity. 
 
 evap. evaporate. 
 
 s.r. stirring rod. 
 
 ex. excess. 
 
 Tr. tartrate. 
 
 Exp. experiment. 
 
 t.t. test tube. 
 
 fil. filtrate. 
 
 up. disp. upward displacement. 
 
 g. grams. 
 
 v. vide, see. 
 
 gel. gelatinous. 
 
 vol. volume. 
 
 gen. generator. 
 
 yel. yellow. 
 
 Xlll 
 
INDEX TO EXPERIMENTS. 
 
 1. Metric Measurements. 
 
 35. Oxids of Nitrogen. 
 
 69. Manganese. 
 
 2. Glass Manipulation. 
 
 36. Carbon Dioxid. 
 
 70. Zinc. 
 
 3. " " 
 
 37. Chlorin. 
 
 71. Group IV. 
 
 4. Physical Changes. 
 
 38. Euchlorin. 
 
 72. Barium. 
 
 5. 
 
 39. Bromin. 
 
 73. Strontium. 
 
 6. Chemical " 
 
 40. lodin. 
 
 74. Calcium. 
 
 7. Elements and Compounds. 
 
 41. Sulfur. 
 
 75. Magnesium. 
 
 8. Oxygen, Preparation. 
 
 42. Hydrogen Sulfid. 
 
 76. Group V. 
 
 9. " Combustion. 
 
 43. Phosphorus. 
 
 77. Sodium. 
 
 10. 
 
 44. Arsenic. 
 
 78. Potassium. 
 
 11. Nitrogen, Separation. 
 
 45. Compounds of Boron. 
 
 79. Ammonium t 
 
 12. " and Air. 
 
 46. " " Silicon. 
 
 80. Group VI. 
 
 13. Hydrogen from Acids. 
 
 47. Oxidation and Reduction. 
 
 81. Borates. 
 
 14. " " Water. 
 
 48. Lead. 
 
 82. Nitrates. 
 
 15. Carbon, Preparation. 
 
 49. Silver. 
 
 83. Nitrites. 
 
 16. " Properties. 
 
 50. Mercury. 
 
 84. Chlorates. 
 
 17. Combustion. 
 
 51. Group I. 
 
 85. Carbonates. 
 
 18. " 
 
 52. Mercury. 
 
 86. Sulfids. 
 
 19. Positive and Negative Elements. 
 
 53. Lead. 
 
 87. Sulfltes. 
 
 20. Acids, Bases, Salts. 
 
 54. Bismuth. 
 
 88. Thiosulfates. 
 
 21. Acid, Alkaline, Neutral Reactions. 
 
 55. Cadmium. 
 
 89. Fluorids. 
 
 22. Soluble Salts by Neutralization. 
 
 56. Copper. 
 
 90. Chlorids. 
 
 23. " " from Metals. 
 
 57. Group H, A. 
 
 91. Bromids. 
 
 24. " " " Carbonates, etc. 
 
 58. Arsenic. 
 
 92. lodids. 
 
 25. Insoluble Salts by Precipitation. 
 
 59. Tin. 
 
 93. Acetates. 
 
 26. Hydrochloric Acid. 
 
 60. Antimony. 
 
 94. Cyanids. 
 
 27. " " 
 
 61. Group H,B. 
 
 95. Tartrates. 
 
 28. Hydrofluoric 
 
 62. Iron. 
 
 96. Oxalates. 
 
 29. Nitric 
 
 63. " 
 
 97. Silicates. 
 
 30. Aqua Regia. 
 
 64. Aluminum. 
 
 98. Ferrocyanids. 
 
 31. Sulfuric Acid. 
 
 65. Chromium. 
 
 99. Ferricyanids. 
 
 32. Ammonium Hydroxid. 
 
 66. Group in. 
 
 100. Sulfates. 
 
 33. Fixed Alkalies. 
 
 67. Cobalt. 
 
 101. Chromates. 
 
 34. Oxids of Nitrogen. 
 
 68. Nickel. 
 
 102. Phosphates. 
 
 xiv 
 
XT 
 
1. METRIC MEASUREMENTS. 
 
 I. Length. 
 
 Note the length of 10 cm on a metric ruler, then estimate by the 
 eye alone this length on the cover of a book, and on various objects, 
 verifying each result till you can carry in mind 10 cm . Estimate 
 the number of inches it covers, and verify. In the same way 
 experiment with l cm . Measure the perpendicular distance between 
 the blue lines on a sheet of foolscap paper. Measure the diameter 
 of the older nickel five-cent piece. Make a drawing of the fol- 
 lowing measurements on the opposite page : one square decimeter, 
 i.e. 10 cm on a side ; l qcm . 
 
 II. Volume. 
 
 Measure in a graduate 10 CC of water, then pour it into a t.t. 
 Note, without marking, what proportion of the t.t. is filled. Make 
 a drawing of it on the opposite page. Pour out the water, then 
 pour into the t.t. as near the same volume as possible, estimating 
 by the eye alone. Verify the result by pouring the water into the 
 graduate. Kepeat this till you can estimate quite accurately. Try 
 it with a t.t. of another size. Estimate l cc of the liquid in the 
 same way. Draw a figure of a cube l cm on a side. 
 
 In future experiments estimate volumes, without measuring, unless 
 special accuracy is required. 
 
 III. Weight. 
 
 Balance a piece of paper on each pan of a pair of scales. On 
 one pan put a 10 g weight and balance this with fine salt or sugar. 
 Note with the eye the quantity of the substance, then remove it. 
 Now estimate a like quantity and verify by weighing it. Repeat 
 the experiment several times. Weigh 1 or 2 g and estimate as 
 before. See if l g can be piled on a one-cent coin. Weigh one of 
 the old nickel five-cent pieces. In subsequent experiments estimate 
 quantity of solids, unless accuracy is desired. 
 
 Supplementary. Commit to memory the metric tables for length, volume 
 and weight (v. Physics). How many cc in a liter ? How many grams should a 
 liter of water weigh ? 10 CC of water ? Hg weighs 13.6 times as much as water. 
 What will 5| cc of Hg weigh ? A rectangular block of marble is 3 X 4 X 2 cm 
 and has sp. gr. 2.5. What does it weigh in grams ? 
 
2. GLASS MANIPULATION. 
 
 I. Ignition Tubes. 
 
 Take a piece of ignition tubing 20 or 25 cm long, 
 hold it steadily in a Bunsen flame just above the inner 
 greenish cone (Fig. 1), and rotate it. When it begins 
 to soften draw it out slightly (Fig. 2, a) and raise it 
 a little in the flame. Do not pull or twist the glass 
 but let the heat gradually separate it, so as not to 
 have long threads attached. The ends may be rounded 
 (Fig. 2, b) by holding in the edge of the flame (Fig. 3). 
 Finally anneal the glass by closing the lower open- 
 ings of the lamp and holding the heated end 
 in the flame to cover it with soot, then letting 
 Fi it cool gradually without touching any object. 
 
 Unless great care is taken in this, the glass 
 
 will break when next put into the flame. Save the tubes for sub- 
 sequent experiments. 
 
 II. Stirring Rod. 
 
 Weld the ends of a piece of glass tubing about 
 lo cm long and or ij- cm in diameter by holding each 
 end successively in a Bunsen flame above the green 
 cone (Fig. 3), and rotating till the openings are 
 sealed. Use care in cooling as before. 
 
 Fig. 3. 
 
 Supplementary. Bulb Tubes. Draw out a piece 
 of tubing as in 1, then melt the closed ends by holding 
 and rotating as in Fig. 3. When the glass is sufficiently 
 Fig. 4. softened, blow moderately into the open end, repeating 
 
 the operation till the tube assumes the desired shape (Fig. 4). 
 
3. GLASS MANIPULATION. 
 
 III. Connecting Tubes, 
 
 Use an ordinary gas flame (or a fish-tail attachment to a Bunsen 
 burner) for bending glass, as the Bunsen 
 flame is too hot. Turn down the gas till 
 the flame is about 5 cm across, then bend 
 each of 3 pieces of tubing, 16 cm long, in the 
 middle and at right angles, by letting the 
 glass rest lightly in the fingers of both 
 hands and holding it lengthwise of the flame 
 and just above the dark part (Fig. 5). Ko- 
 tate it slowly and hold very steadily. When 
 it begins to soften take it quickly from the 
 flame and holding it between the eye and 
 a window frame bend it at right angles. 
 If it does not bend easily, heat it again. Bend also one piece of 
 tubing (50 cm long), 5 or 6 cm from one end. Kound the sharp 
 corners of each by holding the tip ends of the tubes in the edge of 
 a Bunsen flame for a minute (Fig. 3). Do not let any part of the 
 heated glass touch any object and avoid wiping off the soot till the 
 glass is cool enough to handle, when it should be cleaned. 
 
 IV. Delivery Tubes, 
 
 Examine the angles (all obtuse) and the relative lengths of the 
 
 parts in Fig. 6 and in a model, 
 noting that the bends a and c are 
 very near the ends, and a and b 
 are close together. Do this work 
 very carefully. Use a piece of 
 glass tubing 50 cm long, holding it 
 as before. Make the bends in the 
 order a, b, c. Hold the glass con- 
 stantly in the flame, turning it 
 6 occasionally to heat both sides. 
 
 When it yields remove and bend it 
 out of the flame. To make the bends at b and c, turn the glass 
 quickly and closing one eye sight along the tube so as to 
 have all parts lie in the same plane. Round the sharp edges 1 
 and 2 in the flame, as before, and cool with care. Show all results 
 to the instructor. 
 
 V. Perforating Corks. 
 
 Fit a cork to a t.t., remove it and with a round file bore a hole 
 in it holding the cork in the left hand and pressing the end of 
 the file against its larger surface. Observe constantly during the 
 operation whether the perforation is perpendicular to the surface of 
 the cork. The orifice must be perfectly circular and a little smaller 
 than the tube it is to receive. When completed, adjust to the d.t. 
 and t.t. Detach the stopper from the t.t., not from the d.t. 
 
4. PHYSICAL CHANGES. 
 
 Fig. 7. 
 
 Solution. 
 
 See whether crystals of granulated sugar, C 12 (H 2 0) U , can be 
 crushed. Put into a t.t. 5 g or more of the 
 sugar, just cover it with water, H 2 0, and boil 
 in a Bunsen flame for a minute, using a t.t. 
 holder of wood, metal, or paper (Fig. 7), till 
 the sugar dissolves. Cool it by holding the 
 tube under a jet of water, and when cool taste 
 a drop of the liquid. Have the sugar particles 
 been divided by dissolving? How do you 
 know? Arrange a filter paper (Fig. 8) and 
 filter the sol., using a filter stand and collect- 
 ing the filtrate in another t.t. 
 (Fig. 9). Touch a drop of 
 the filtrate to the tongue with 
 a stirring rod (s.r.). Note 
 whether the sugar has gone 
 through the filter paper. 
 Divide the liquid into two parts. Save one for 
 Exp. 6, and dilute the other with an equal vol. 
 of H 2 ; then cover the t.t. with the thumb or 
 hand, invert it (Fig. 10) and, holding it away 
 from the table, shake the contents vigorously. 
 Taste a drop of the sol. Note whether the 
 Fig 9 sugar particles have been further, divided. 
 
 Supplementary, Read very carefully Rule 14 and the Model for Taking 
 Notes, (a) Dis. a little CuCl 2 or Cu(NO 3 ) 2 in water, 
 boiling as before, and filter but do not taste the sol. 
 (b) Dis. also a little NaCl, filter and taste the filtrate. 
 Evaporate. Do substances in sol. pass through a 
 filter paper ? Many substances like SiO 2 and BaS 0* 
 are not sol. in water or acids, others, like Zn, Cu, 
 etc., are sol. hi acids only, (c) Heat a platinum 
 wire in a Bunsen flame. Note if it undergoes 
 change. 
 
 Fig. 8. 
 
 Fig. 10. 
 
 Terms: Physical division, physical solution, insoluble, dilution, molecule, 
 evaporation, properties, filtrate, residue. 
 
5. PHYSICAL CHANGES. 
 
 Solution and Crystallization. 
 
 1. Fill an e.d. f full of water, heat it, and add small pieces of 
 alum until the liquid becomes thick. Replace the water lost by evap- 
 oration. Now put in a narrow piece of cotton cloth so that it lies 
 in the liquid but does not touch the bottom of the dish, and set the 
 latter aside to cool. Observe occasionally, meantime doing the 
 following : 
 
 2. Cautiously boil about 5 g copper sulfate in 5 CC H 2 in a t.t. 
 until it is dissolved. Then place the t.t. in an oblique position 
 and let the liquid cool. If necessary, leave till the next laboratory 
 hour. Note the formation of crystals in 1 and 2, and observe their 
 form, color, luster, angles, etc. Are these illustrations of physical 
 or of chemical changes, and why ? Trace each step in the process. 
 Which seems more soluble, alum or sulfate of copper ? Are they 
 more soluble in hot or in cold water ? 
 
 3. Put a few crystals of copper sulfate into an i.t. or small t.t. 
 and slowly heat. Observe the sides of the tube and any change of 
 color, luster, hardness, and form in the crystals. Explain. When 
 the tube is cool add a drop of water. 
 
 4. Experiment in the same way with some of the crystals of 
 alum, tasting the powder obtained by heating. 
 
 5. Put a crystal of sodium sulfate and a small piece of calcium 
 chlorid on separate pieces of paper and leave them in the locker 
 exposed to the air till the next exercise. Describe the result with 
 explanation. 
 
 Supplementary. (a) Put into an e.d. as much powdered S as will stay on 
 the point of a very small knife blade. Cover it with a very little C S 2 (keep the 
 flame at a distance from this substance) so as to dis. the S, let it evaporate in a 
 draft of air, then watch closely as the C S 2 evaporates. Describe and explain the 
 phenomena. Put a drop of this sol. on a microscopic slide and watch it closely 
 under the microscope as the CS 2 evaporates, (b) Dissolve and re-crystallize 
 Na 2 SO 4 . (c) Mix sols, of alum and CuSO 4 and try to crystallize the two 
 substances together. Are the above salts soluble or insoluble ? 
 
 Terms: Crystal, amorphous substance, mother liquor, saturation, super- 
 saturation, water of crystallization, deliquescent, efflorescent, luster. 
 
6. CHEMICAL, CHANGES. 
 
 I. Sulfuric Acid and Sugar. 
 
 To the sol. saved from Exp. 4 slowly add sulf uric acid, H 2 S 4 , 
 in a small stream, holding the tube with a t.t. 
 holder, and the bottle as in Fig. 11 (read Rule 
 9), till the substance changes color. Add a little 
 more acid, and if the sugar solution is strong 
 enough it will cause the substance to swell and 
 run over the tube. Observe the color, odor, and 
 temperature, but do not taste it. Does it appear 
 Fig. 11. to be a solid or a liquid ? Sugar is a compound 
 
 of C and H 2 0. H 2 S0 4 has great affinity for 
 
 water. From these facts explain the phenomena. Clean the tube 
 
 with water, using a brush if necessary. 
 
 II. Heat and Sugar. 
 
 See whether heat will break up sugar, by dipping a short piece 
 of glass tubing moistened with water into a little sugar and 
 holding it in a Bunsen flame. Describe all you see, note the odor, 
 and state your conclusions. What produced the chemical change ? 
 
 III. Combustion of Wood. 
 
 Hold a small stick in a flame. State whether the changes 
 observed are chemical, or physical, with reasons. 
 
 IV. Changes in Solutions. 
 
 Add a little hydrogen chlorid, HC1, to 5 CC Pb(N0 8 ) a sol. The 
 hydrogen chlorid and the lead nitrate have become lead chlorid 
 and hydrogen nitrate. The former product is insoluble and is 
 therefore thrown down (precipitated). To 5 CC of CuCl 2 sol. add a 
 little N H 4 H ammonium hydroxid and notice any evidence of 
 change. 
 
 Supplementary. (a) To 5 CC of HgCl 2 sol. add a few drops of KI sol. 
 (b) Add a few drops of KI sol. to 5 CC of Pb(NO 3 )2 sol. (c) On a few bits of Cu 
 in an e.d. pour a few drops of nitric acid, HNOa. Describe all you see. Are 
 these chemical, or physical changes ? Why ? 
 
 Terms : Combustion, chemical solution, affinity, precipitation, chemical 
 
7. ELEMENTS AND COMPOUNDS. 
 
 Fig. 12. 
 
 Synthesis. 
 
 Fill an i.t. (from Exp. 2) not over -j- full of an intimate 
 mixture of one part by weight of S (finely pow- 
 dered brimstone, or flowers of S) with two parts 
 of fine Cu filings. Observe that the two elements 
 are entirely distinct, and note the color and 
 luster of each. Now heat the tube very slowly 
 for a minute (moving it alternately out of the 
 flame and into it, so as not to break the glass) 
 then heat very strongly, 'the upper part first 
 (Fig. 12). Watch the contents of the tube for 
 evidence of a chemical change. What is the 
 evidence ? When this change has taken place throughout the 
 whole mass let the tube cool for a minute, then heat an instant, 
 break the -tube with a jet of water, and examine the substance. 
 Note whether it resembles Cu or S in color or luster. Describe 
 fully what you saw, state what is supposed to have taken place, 
 and give an equation to express it. 
 
 Supplementary. (a) Mix Fe filings and S (in about the same proportion as 
 Cu and S), try to separate the Fe with a magnet and the S with C S 2 from a 
 part, then heat the other part in an i.t. Test the product with magnet and 
 CS 2 ; also by adding a little H 2 O and then HC1 in an e.d. An offensive gas is 
 liberated which either element alone would not give if similarly treated. 
 Describe fully with equations, (b) Light a match, and as it burns watch the 
 colors of the flame and see if there is any evidence of a product being formed. 
 The match contains the elements P, S, and C, which combine with the element 
 O in the air to form compounds called oxids of P, S, and C (v. Exp. 9). 
 (c) Burn a piece of charcoal and observe. The products are for the most part 
 invisible gases, (d) Heat in an i.t. a little granular pyrite, FeS 2 , and finally 
 test the residue with a magnet. 
 
 Terms: Synthesis, sulfid, oxid, binary compound, element, gas, luster, 
 residue. 
 
Fig. 13. 
 
 8. PREPARATION OF OXYGEN. 
 
 Fill 4 or 5 wide-mouthed bottles recs. with water, invert 
 
 them on the shelf of a p.t. 
 in which the water is 3 or 
 4 cm above the shelf. Mix on 
 a paper 5 or 10 g KC10 a 
 (not pulverized) and 3 or 4 
 of powdered Mn0 2 . Put 
 the mixture into a large dry 
 t.t. which should not be over 
 J- full. Adjust a stopper and 
 d.t. and hang the app. on a 
 r.s. (Fig. 13). Direct a 
 
 Bunsen flame against the t.t., holding the lamp and slowly moving 
 it. Avoid heating too long in one place (take it away from the 
 tube occasionally for a few seconds), or the tube will melt. Watch 
 the bubbles in the d.t., collect the escaping gas in the recs., and 
 notice the bubbles as they burst, and whether the gas 
 has color. Explain, and after a time observe again. 
 Is there evidence of a gas, or a solid, or both ? As 
 soon as the flame is taken away remove the d.t. from the 
 trough to prevent the water drawing back and break- 
 ing the tube. Why is there this back action ? Let 
 the recs. remain on the shelf till wanted, or, if taken 
 out, keep them covered with glass plates (Fig. 14). 
 After doing Exp. 9 clean the t.t. by covering the residue with 
 water, closing the mouth of the tube with the thumb or hand, and 
 shaking the contents vigorously, holding it away from the table. 
 
 Supplementary. Does the O occupy more, or less, volume than the factors 
 from which it was obtained ? Why ? Would it weigh more, or less ? Why ? 
 The MnO 2 takes no part in the reaction, but is used to distribute and equalize 
 the heat and lower the temperature of dissociation. Name all the substances 
 in the t.t. at the end of the exp. 
 
 Fig. 14. 
 
 Terms : Factors, products, dissociation. 
 
9. COMBUSTION IN OXYGEN. 
 
 1. Put a burning splinter into a rec. of for an instant, note 
 the color and vigor of the flame, then remove, blow out the flame 
 and put in the glowing stick. Repeat till there is no effect. State 
 accurately everything you saw and heard. Wood consists largely 
 of C. Explain the combustion and write an equation for it. Test 
 the product by adding 4 or 5 CC of lime water, Ca(OH) 2 sol.; shake 
 it well and notice the effect. 
 
 2. Make a d.s. by hollowing out the end of a crayon, or electric 
 
 light carbon, and attaching a Cu wire. Put into it a 
 bit of S, hold the whole in a flame till the S burns, 
 then lower it into a rec. of (Fig. 15). Notice the 
 color and vigor of the flame, and the color and state of 
 the product, explain what you see and write the equa- 
 tion. Name the product and test it by cautiously 
 noting the odor, and also by putting a drop of K 2 Cr 2 7 
 sol. on paper and holding it in the gas, noting any 
 Fig - 15 - change of color. 
 
 3. Put into an e.d. with a pair of forceps (don't handle it) 
 a piece of P, half as large as a pea. Dry it by rolling it lightly on 
 paper, then put it into a d.s. Heat for an instant the end of a 
 wire or file, touch the P with it and lower the spoon at once into a 
 rec. of 0. Observe the color of the flame and of the product. 
 Describe, also write the equations. When combustion stops burn 
 every bit of the P by holding the d.s. in a flame. Add a few cc of 
 H 2 to the rec., shake it well and drop in a piece of blue litmus 
 paper. 
 
 Supplementary. What became of the in the above cases ? Would the 
 product in each case weigh more or less than the C, S, P ? How do you 
 know ? (a) Cover the bottom of a rec. of O with sand or H 2 1 or 2 cm deep. 
 With forceps hold for an instant in a flame one end of a picture-cord wire 5 or 
 10 cm long, then dip it into a bit of powdered S. Hold it again in the flame till 
 the S burns, then thrust it into the rec. of O. If the Fe does not burn try it 
 again, or repeat with another rec. (have but little S on the wire). Describe the 
 combustion and the product, and give the equation, (b) With forceps hold in 
 the flame a piece of Mg ribbon till it begins to burn, then instantly thrust it into 
 a rec. of O. (c) Try Zn tipped with S. 
 
 Terms : Supporter of combustion, combustible, kindling point. 
 
1O. OXYGEN. 
 
 Fig. 16. 
 
 I. Oxygen from Oxids. 
 
 Heat strongly 1 or 2 g of HgO in a t.t. 
 or i.t. and thrust a glowing splinter into 
 the tube while still holding it in the 
 flame (Fig. 16). Note the color of the 
 HgO while it is being heated, observe the 
 sides of the tube, and finally pour out and 
 carefully examine the contents. Explain, 
 and give the reaction. Save the residue. 
 
 II. Oxygen from Nitrates. 
 
 Put into a t.t. about 1 of Pb (N0 8 ) 2 , 
 
 heat it and test the gas as before. Note any snapping, the color of 
 the fumes, which are N 2 and (the O being colorless), and the 
 color of the residue, PbO. Also write the equation. 
 
 III. Oxygen from Chlorates. 
 
 Try to obtain oxygen in the same way by heating a few crystals 
 of K C10 3 . Test as before, and write full notes. 
 
 Supplementary. What 3 classes of substances have you found which yield 
 O ? From which is the oxygen obtained most easily ? N 2 O will also support 
 combustion of C, S, P, but not as readily as pure O. Heat and test : (a) 
 (b) NaNO 3 . 
 
 Terms: Oxid, chlorate, chlorid, nitrate, residue. 
 
11. SEPARATION OF NITROGEN. 
 
 Fill a p.t. with water 3 or 4 CC above the shelf. Prepare a d.s. 
 with a wire bent sharply 5 or 6 cm from the 
 crayon. Pass the wire through the orifice in 
 the shelf so that it will reach half way up an 
 inverted rec., fasten it there (so as to be easily 
 removable) with the mouth of the rec. under 
 water (Fig. 17). When adjusted remove the 
 rec., leaving the wire. Using forceps and e.d. 
 put a piece of P (the size of half a pea) into 
 Fi s- 17 - the spoon. Touch it with a warm (but not too 
 
 hot) wire or file handle, and instantly invert the rec. over it as be- 
 fore, pressing the latter down and holding it steadily with the hand 
 till combustion ceases. Was there any escape of gas ? Before re- 
 moving the d.s. be sure the combustion has stopped, and let no air 
 enter. Compare the combustion and the product with the same in 
 the oxygen exp. Describe fully with equation. Finally remove 
 the crayon without admitting air or disturbing the rec. Burn any 
 remaining P in a flame and leave the rec. till the gas becomes toler- 
 ably clear, then remove with a glass plate, turning the rec. right 
 side up and keeping the water in the bottom. Set this aside for 
 Exp. 12. 
 
 Supplementary. (a) Try to separate the N in air with S in a d.s., setting 
 the S on fire by holding a flame over the adjusted spoon, (b) Try paper or 
 charcoal. What elements do these exps. show to exist in the. air ? N may also 
 be separated by forcing air over red hot Cu, which forms CuO. It may be 
 obtained from compounds, such as nitrates and ammonia. 
 
12. NITROGEN AND AIR. 
 
 I. Properties of N. 
 
 (1) Put a burning stick into the rec. of N (Exp. 11), sliding 
 along the glass cover enough to admit it. Note the effect on the 
 stick and on the gas. Try it with a glowing stick. Is the spark 
 rekindled, or extinguished ? (2) See whether the P, S, and C on 
 the end of a match will burn in the gas. Is there any equation ? 
 Why ? Is N a combustible ? A supporter of combustion ? (3) Test 
 the liquid with blue litmus paper. Describe and explain. 
 
 II, Composition of Air. 
 
 Measure accurately the water in the rec. of N by pouring it into 
 a graduate and recording the volume in cc. Then measure the 
 total capacity of the rec. in the same way, and compute the percentage 
 of and of N (by volume) in the air, giving the computation and 
 remembering that the first vol. of water represents the vol. of 
 burned. If any air was forced out in Exp. 11, will the per cent 
 of found be too large or too small ? Explain. 
 
 Supplementary. Compare the properties of N with those of 0. Air con- 
 tains also C 2 (tested for by Exp. 36) and H 2 O (shown by setting a pitcher of 
 cold water in a warm room). Make tests for each and explain. From the per- 
 centage of N there must be subtracted about 1% of the recently discovered ele- 
 ment argon, A, a gas more inert than N. 
 
 Terms: Inert substance, percentage by volume and by weight, acid, litmus 
 paper. 
 
13. HYDROGEN FROM ACIDS. 
 
 Fig. 19. 
 
 I. Preparation. 
 
 Fill 4 or 5 recs. with water and invert in a 
 p.t., then put into the gen. (Fig. 18) (or use 
 the same app. as for making 0) 8 or 10 g granu- 
 lated Zn, cover with H 2 and add 5 CC of HC1 
 through the thistle tube. Have the bearings 
 perfectly tight, and, without applying heat, 
 collect the gas like 0. Observe and describe 
 the action and note any heat. If action stops 
 add more H Cl. Leave the recs. of gas in the ^s- is. 
 
 p.t. till wanted in II (or if removed keep them inverted, Fig. 19). 
 Has the gas any color ? Why ? Clean the app. and 
 save the Zn. 
 
 II. Tests. 
 
 (1) Lift a small rec. of H, hold it inverted, and 
 thrust a burning stick into the gas. Note any explo- 
 sion and whether the gas or splinter burns. (2) Try 
 it with another rec. and then cautiously look into the 
 open mouth of the latter, noting the colors of flame. Explain fully 
 the explosion, combustion, etc., with equation. Note the (3) color 
 and (4) odor of (the impure) H. (5) Collect by up. disp. a t.t. of 
 H, and test by putting it mouth to mouth with a t.t. of air and then 
 bringing the two open tubes successively to a flame. 
 
 Supplementary. (a) Put 2 or 3 small pieces of Zn into a t.t. (use a t.t. 
 holder), cover it with water and add a little H 2 S0 4 . Notice the action, test the 
 combustibility of the gas, and write the equations, (b) Put into a 
 t.t. a few Fe filings, add H 2 O and HC1. Test the gas as before, 
 (c) Try Fe and H 2 SO 4 . Make a complete record of all work. 
 From what class of substances has H been obtained, and how ? 
 Is H a combustible ? A supporter ? (d) Try the action of Zn and 
 H 2 S O 4 , without H 2 O, cautiously noting the odor, (e) Pass H into 
 euchlorin (Exp. 38). (f) Fill a rec. half full of water, invert it in 
 a p.t., letting air fill the upper half. Now fill the rest with H from 
 a gen., then bring the mouth of the rec. to a flame, (g) Make a 
 philosopher's lamp (Fig. 20), but before lighting the hydrogen, test 
 the gas by collecting a t.t. full by upward displacement and bring- 
 ing it to a flame. If a sharp sound ensues there is danger, as the 
 gen. contains air. If only a low muffled sound, the gas may be lighted. Lower 
 a larger open glass tube over the flame. Other flames give the same result. 
 
 Terms : Upward and downward displacement, philosopher's lamp, singing 
 flame. 
 
 Fig. 20. 
 
14. HYDROGEN FROM WATER. 
 
 I, Action of Na on H 2 0. 
 
 (1) Put into a clean rec. 15 or 20 CC of H 2 O. Have a cover of 
 paper or cardboard, not glass. Observe the color and 
 luster of freshly cut Na; take a small piece from 
 the naphtha in which it is kept (using forceps and 
 dry e.d.), drop it into the rec., and cover the latter at 
 once (Fig. 21). Describe the action, note any fumes 
 or gas (try to ignite it), and write equations. When 
 action stops take off the cover and bring the fumes 
 near a Bunsen flame, or hold the lower openings of 
 the burner close to the mouth of the rec. and notice the color im- 
 parted to the flame. This is the flame test for Na and its cpds. 
 Are the fumes solid or gaseous, and what becomes of them ? 
 (2) Hold a piece of moist red litmus paper in the fumes, also put 
 one into the liquid. Test the liquid by adding a little to these 
 sols.: (3) FeCl 3 ; (4)FeS0 4 ; (5) A1C1 8 . 
 
 (6) Try the action of Na on hot H 2 by boiling a little H 2 O in a 
 t.t. and pouring it into a rec., then dropping a piece of Na on it and 
 covering it at once. Note all the phenomena and write equations 
 for : (a) the action of Na on H 2 ; (b) the combustion of H, and 
 (c) Na ; (d) the sol. of Na 2 0. 
 
 II, Action of K on H 2 0. 
 
 Perform the exp. as above, using K and cold H 2 0, and making 
 similar observations, notes, and tests, including flame tests. 
 
 Supplementary. Which has greater affinity for H 2 0, Na or K ? (a) Col- 
 lect H by putting a small piece of Na in a wire cage and quickly thrust it under 
 an inverted t.t. full of H 2 O in a p.t. Test the gas. What proportion of H in 
 water is replaced by K or Na ? Are the metals heavier or lighter than H 2 O ? 
 (a) Moisten a piece of paper, put it into a rec. and drop on the moist paper a 
 bit of Na and cover it. When action stops try to light the fumes by bringing a 
 Bunsen flame to the mouth of the rec. (b) Try the same with K. 
 
15. AMORPHOUS CARBON. 
 
 I. Carbon from Wood. 
 
 Put 2 or 3 small, thin pieces of wood into a small Hessian cruci- 
 ble and cover them with sand (Fig. 22). Apply a 
 Bunsen flame for half an hour, or until gases 
 cease to come off (meanwhile do II, III, and 
 Exp. 16). Notice any gases rising and try to 
 kindle them. Observe the color and odor. Finally 
 remove the carbon with forceps and save the sand. 
 Examine the carbon as to color, weight, volume, 
 porosity, and brittleness (compare with the original 
 22 wood). See whether it burns with flame or only 
 
 glows, on igniting it in a flame. 
 
 II. Carbon from Candle, Oil, Gas. 
 
 Hold a short piece of white crayon, or of glass tubing, in the 
 flame of a Bunsen burner, with the lower openings closed, then 
 open the orifices and try to burn off the deposit. Try to collect C 
 from a candle flame and from that of a kerosene lamp in the same 
 way. The candle, oil, and gas consist mainly of cpds. of C and H. 
 Which seems to burn at the lower temperature, C or H ? 
 
 III. Carbon from Sugar, Starch. 
 
 Heat in a narrow tube a very little sugar, also starch. State 
 what you see and conclude. 
 
 Supplementary. Gases burn with flame. Solids glow. What has the 
 destructive distillation of wood in I. done ? Cpds. of C and H (called hydro- 
 carbons) are solid, liquid, or gaseous, (a) Try to obtain carbon in any other 
 way, (b) Hold a piece of charcoal in water for a minute, (c) Weigh a piece 
 of wood, then distil it, and finally weigh the product, (d) Put some small 
 pieces of wood into an i.t., attach a d.t. and heat. Collect the gas (Fig. 13). 
 (e) Test the gas. 
 
 Terms : Amorphous, crystalline, dimorphous, trimorphous, porosity, specific 
 gravity. 
 
16. PROPERTIES OF CHARCOAL,, 
 
 I. Carbon a Reducing Agent, 
 
 Fill an i.t. not over full of an intimate mixture of CuO and C 
 (powdered charcoal), about 7 parts CuO to 1 part C by weight. 
 Heat it very cautiously at first, then strongly till you see evidence 
 of a chemical change. What is the evidence ? What caused the 
 mixture to rise? After the action stops is there any change in 
 color ? When sure that no more action will ensue, cool it for a 
 minute and pour the contents into a dry e.d. Examine it carefully 
 as to color and luster. Explain, giving an equation to express the 
 chemical change. 
 
 Finally test the residue by adding 2 or 3 CC HN0 3 , noting the 
 color of the fumes and of the residue. See whether HN0 8 has a 
 similar effect on the original mixture of CuO and C. What does 
 the test show ? 
 
 II. Carbon a Decolorizer. 
 
 Shake up 5 or 10 g of bone black animal charcoal in a t.t, 
 or rec. with 10 or 20 CC cochineal sol., then filter and notice the color 
 of the liquid. If not perfectly colorless pour it again on the same 
 filter, using more carbon if needed. Try in the same way sols, of 
 indigo and litmus ; also of K 2 Cr 2 7 and K Mn0 4 . Can you draw 
 any general inference of the decolorizing action on animal, vege- 
 table, and mineral pigments, the first three being animal or vege- 
 table, the last two mineral ? K 2 Cr 2 7 may be turned slightly yellow 
 by alkali in the bone black. 
 
 III. Carbon a Deodorizer or Disinfectant. 
 
 Prepare a sol. of H 2 S (Exp. 42). Notice the odor of the gas and 
 its solubility. Put into a rec. 5 or 10 g of powdered charcoal and 
 pour upon it 10 or 20 CC H 2 S sol. and shake the mixture well. Then 
 pour the whole on a filter, collect the filtrate in a clean t.t. and see 
 if any odor remains ; if so, mix and filter again, using more char- 
 coal if necessary. The H 2 S has been absorbed physically into the 
 pores of the coal and partially oxidized there. This illustrates the 
 absorbent action of charcoal on gases, animal effluvia, and micro- 
 organisms in the sick room. 
 
17. EXPERIMENTS IN COMBUSTION. 
 
 I. Structure of Flame. 
 
 (1) Make a careful examination of the parts and colors of a 
 candle flame, and make a drawing to show them. Move the candle 
 slightly in the air to show the outer flame. This is best seen in a 
 dark room. Describe fully. (2) Examine the structure of a 
 Bunsen burner (unscrew the top if necessary), make a drawing to 
 show the orifices, and state what use they subserve. Keplace the 
 tube and light the gas. Hold the flame in front of a dark object 
 (as a blackboard), examine the parts, make a drawing, give a brief 
 description, and state the color of each part. If possible, put the 
 flame in direct sunlight, and study the parts from its shadow, to 
 confirm your results. 
 
 II. Combustion of Flame, 
 
 (1) Put a moist stick across the base of the Bunsen flame for an 
 instant, and notice what parts are burned. Hold a stick just above 
 the inner cone of the flame. Make sketches of results. (2) Press 
 quickly down on the flame with a paper, or pasteboard, remove 
 before it burns, and notice the shape of the charred part, or press 
 down on the flame with a fine wire gauze, and observe by the 
 glowing of the wire where the heat is most intense. Sketch. 
 
 (3) Put one end of a small d.t. into the inner blue cone, not into 
 the lamp, and try to light the gas at the other end. (4) Thrust a 
 match quickly into the inner cone near the bottom. If done quickly 
 the phosphorus will not take fire. The match contains a supporter 
 and a combustible. Why does it not burn ? In what parts of the 
 flame does combustion occur ? 
 
 Supplementary. Examine : (a) an ordinary gas flame ; (b) the flame of a 
 kerosene lamp ; (c) the flame of a burning splinter, or match, holding it vertical 
 and breaking off the charred part as fast as it forms. Have all flames practi- 
 cally the same structure ? 
 
18. EXPERIMENTS IN COMBUSTION. 
 
 III. Light of Flame. 
 
 (1) Sprinkle a very little charcoal dust into a Bunsen flame, 
 and note any change of light or color, or, better, dip a fine splinter 
 into powdered charcoal and thrust it into the openings at the base. 
 Notice flame. (2) File a nail or other metallic substance over the 
 flame, or sprinkle in CuO, or " iron by hydrogen." (3) Also stir 
 up the dust near the flame, or tap the lamp with the fingers. What 
 produces flame ? What is the cause of light in a flame, and what 
 flames give light ? (4) Close the orifices at the base of the burner, 
 and explain the change of light. (5) Set fire to a small piece of 
 charcoal, by holding it in a flame, and see whether it burns with 
 flame or only glows. What does this show ? 
 
 IV. Kindling Point. 
 
 (1) Light the gas and hold a fine wire gauze 3 or 4 cm above the 
 burner. Why does it not burn above the wire ? (2) Extinguish, 
 then relight the gas above the gauze. Result and explanation. 
 Gradually lift the wire till the gas will not burn. (3) Again light 
 the gas above the gauze, and hold another gauze above the flame, so 
 as to confine it above and below. State three conditions of combus- 
 tion, define each, and show how this exp. illustrates them. 
 
 Supplementary. Why does a lamp smoke ? Why does phosphorus take 
 fire spontaneously ? Why does gunpowder explode ? Why will it burn with- 
 out air ? Why do we exclude the air to put out a fire ? Why does blowing a 
 flame sometimes cause it to burn, and sometimes extinguish it ? Why does 
 cannel coal burn with flame ? When will a mixture of H and air not explode ? 
 Why will some substances burn in water ? See which has the lower kindling 
 point, P or S, by putting each on one end of a piece of iron at equal distances 
 from a flame which heats the other end. 
 
 Terms : Kindling temperature, spontaneous combustion, combustible, sup- 
 porter. 
 
19. POSITIVE AND NEGATIVE ELEMENTS. 
 
 I. Dis, Ag in HN0 3 and ppt. Ag with Cu. 
 
 Put a ten-cent silver coin into an e.d. and add 10 or 20 drops of 
 HN0 3 . Warm it, if necessary, over asbestos, and 
 watch the result as to action, color of liquid, color of 
 fumes, etc., and give the reason for each, with equa- 
 tion. When action stops, or the coin is dissolved, add 
 10 CC H 2 0, then pour it into a t.t. and put in a copper 
 wire (Fig. 23). Leave for 10 to 30 minutes. At 
 this point begin II., but observe any deposit on the 
 wire, noting its color, luster, texture, crystalline 
 form, and any change in the color of the liquid. Ex- 
 plain, giving equation. Save the Ag. Which has 
 greater affinity for N 3 , H, or Ag ? Why is H not set free ? 
 
 II. Dis. Cu in HN0 3 and ppt. Cn with Pb. 
 
 Put into a t.t. or e.d. a thin piece of sheet Cu, say l<i cm ; add 10 or 
 20 drops HN0 3 . Make as accurate observations and notes as be- 
 fore, including equation. After dissolving the Cu add 10 CC H a O, 
 and put in a Pb wire (or other piece of Pb), made bright with a 
 file or by just dipping it into a little HN0 3 . Leave it for some 
 time in the Cu (NO 3 ) 2 sol., and begin III. Afterwards notice the 
 deposit, the color of liquid, etc., as before, and take full notes with 
 equations. Which has more affinity for N 3 , Cu, or Ag ? 
 
 III. Dis. Pb in HN0 3 and ppt. Pb. with Zn. 
 
 Dis. part of a small piece of Pb in a few drops of H N 3 , heat- 
 ing if necessary, and when Action ceases add 10 CC H 2 ; pour the 
 liquid into a t.t. and put in a piece of Zn. There should be scarcely 
 any free acid when the Zn is introduced, or violent effervescent 
 action will ensue and both Pb and Zn will dissolve. Make full 
 notes as before, including equations. 
 
 Supplementary. (a) Obtain crystals of pure AgN0 3 from a coin, (b) Of 
 Pb(NO 3 ) 2 from Pb. (c) Of Cu(NO 3 ) 2 from Cu. (d) Make CuSO 4 from Cu with 
 dil. acid, (e) See whether Zn will ppt. Cu from CuSO 4 . (f) From CuCl 2 . 
 With l oz of pure Ag, how much AgNO 3 could be made ? How much Ag will 
 5s of Cu replace from a sol. of AgN O 3 ? 
 
 Terms: Chemical solution, physical solution, precipitation, stochiornetry. 
 
2O. ACIDS, BASES, SALTS. 
 
 I. Acids, 
 
 (1) Pour into an e.d. a few drops of HC1, add 4 or 5 CC H 2 0, stir 
 
 it, taste a drop from the s.r. 
 (Fig. 24). Dip the end of a 
 strip of blue litmus paper into 
 it. State results. (2) Einse 
 the e.d., then put in a few- 
 drops HN0 8 and 5 CC H 2 0, stir 
 24. and test as before, (3) Test 
 
 in like manner H 2 S 4 . What do these exps. teach you of acids ? 
 
 II. Bases. 
 
 (1) Pour into an e.d. 1 or 2 CC NH 4 OH, add 4 or 5 CC H 2 0, stir it, 
 and taste a drop. If it has no taste add more NH 4 OH. Dip the 
 end of a piece of red litmus paper into it. (To redden blue litmus 
 hold it in the fumes of H Cl. To turn red litmus paper blue hold 
 it in NH 3 fumes.) (2) Einse the e.d. and test NaOH sol. in the 
 same way. Also (3) KOH sol. What do these exps. teach con- 
 cerning bases ? 
 
 III. Salts. 
 
 (1) Pour into a clean e.d. 1 or 2 CC of Nad sol., taste a drop of 
 it, and test it with litmus, red and blue. Test in the same way 
 (2) KN0 8 sol., also (3) a sol. of (N H 4 ) 2 S 4 . What is the usual 
 action of salts on litmus ? Test, however, these sols, with both 
 colors: (4) Na 2 C0 3 ; (5)CuS0 4 ; (6) HNaC0 3 ; (7) HNaS0 4 . 
 
 Supplementary. Test sols, of: (a) H 3 PO 4 ; (b) H 2 C 2 4 ; (c)HC 2 H 3 O 2 r 
 (d) Ca (OH) 2 ; (e) Ba (OH) 2 ; (f) HNa 2 PO 4 ; (g) Na 2 B 4 7 ; (h) 
 
 Terms : Acid, base, salt, acid salt, normal salt, alkaline salt, neutral salt, 
 salt acid to litmus, alkali, fixed alkali, volatile alkali, alkaline carbonate. 
 
21. ACID, ALKALINE, AND NEUTRAL REACTIONS. 
 
 Put into a small beaker or a t.t. 5 CC of an aqueous sol. of blue 
 litmus. (1) Pour a few drops of HC1 into an e.d., beaker, or t.t. 
 and dip a s.r. into this (never dip a rod into a reagent bottle), then 
 stir the litmus solution with it, noting any change of color. If 
 none occurs add another drop of acid with the rod. (2) Pour a 
 few drops of NH 4 OH into a clean e.d. or t.t., dip the s.r. into it, 
 then stir the litmus solution with this. If the color is unchanged 
 repeat till blue is again obtained. (3) In the same way put a drop 
 (or more, if necessary) of HN0 3 from an e.d. into the same blue 
 solution. (4) When it is reddened add a drop or more of NaO H 
 sol. until it becomes blue. (5) Change it again to red with a drop 
 of H 2 S0 4> and (6) restore the color with KOH sol. 
 
 Supplementary. (a) Add a few drops of H 2 O to a sol. of red litmus, and 
 also to one of blue, (b) Add to both red and blue litmus sols, a sol. of NaCl. 
 (c) Try N H 4 C1 sol. (d) K N 8 sol. (e) H NaC O 3 sol. (f ) H K S O 4 . (g) CuS O 4 . 
 
 Terms : Acid, alkaline, and neutral reactions. 
 
22. SOLUBLE SALTS BY NEUTRALIZATION. 
 
 I. Sodium Chlorid. 
 
 Pour into an e.d. not over 5 CC NaOH sol., and into a clean t.t. or 
 
 beaker 4 or 5 CC HC1. Now add 
 some of this latter, a little at a 
 time (Fig. 25), to the NaOH 
 sol., stirring it meantime till 
 the product is neutral to litmus 
 paper ; when nearly neutral 
 add a drop at a time with a 
 
 s.r. and test with both colors, using only the end of the paper and 
 keeping it on the side of the e.d. If blue litmus 
 paper is reddened by the sol., add NaOH sol., a few 
 drops at a time. If red litmus is turned blue add a 
 drop of H Cl. When the sol. does not affect either 
 red or blue litmus left in it for a minute, show it 
 with both papers in it to the instructor, then filter 
 and evaporate the liquid to dryness by boiling it over 
 a plate and abestos paper (Fig. 26). When it is cool, 
 examine the residue and taste it. What is the object 
 of evaporation ? Explain what took place when the acid and base 
 were mixed, and give the equation to express it. Sift a little of 
 the salt into the flame. The color shows a cpd. of Na. Test for 
 Cl by Exp. 27. 
 
 II. Potassium Sulfate. 
 
 Into an e.d. put 5 CC KOH sol. and neutralize it with dilute 
 H 2 S0 4 , using both test papers. When sure it is neutral, evaporate 
 most of the water and taste the product. Explain the action, giving 
 the equation. Sift a little into a flame. The color shows a K cpd. 
 (best seen through blue glass). Test S0 4 by Exp. 31. 
 
 III. Ammonium Nitrate. 
 
 Neutralize NH 4 OH with HN0 3 (preferably dilute) in the same 
 way as before. Stop evaporation when dense fumes begin to ap- 
 pear. These fumes indicate a decomposition of the salt by heat 
 (v. Exp. 34). 
 
 Supplementary. How would you make by neutralization NaN Os, 
 K N O 3 , K Cl, N H 4 C1, (N H 4 ) 2 S O 4 ? Write also equation for each. Weak acids 
 will not neutralize strong bases, and vice versa. Hence, salts like NaaC O 8 are 
 not neutral. How do these exps. illustrate the law of definite proportion ? 
 
 Terms : Neutralization, double decomposition, definite proportion, evapora- 
 tion, fumes. 
 
23. SOLUBLE SALTS FROM METALS. 
 
 I. Zinc Chlorid. 
 
 To a piece of Zn in a t.t. add water and a little HC1. Describe 
 and explain the action, and when it ceases, pour the liquid into an 
 e.d. and evaporate to dryness. Observe and taste the salt. Name 
 it and write the equation. To test the salt, add a little H 2 O to dis- 
 solve it and divide the sol. into 4 parts. Test for Cl by Exp. 27, 
 and for Zn by Exp. 70. 
 
 II. Iron Sulfate. 
 
 Dissolve as above a few Fe filings in dil. H 2 S 4 . When action 
 stops add H 2 O, filter, and evaporate the filtrate. Then dissolve the 
 salt in water after having examined it. Name it and write the 
 equation. Test it for Fe by Exp. 63, and for S 4 by Exp. 31. 
 
 III. Copper Nitrate. 
 
 Dissolve a little Cu in dil. H N 3 , pour off the liquid, evaporate, 
 and then add H 2 0. Test for Cu by Exp. 56. and for N0 3 by 82. 
 Make full notes. 
 
 Supplementary. The salts in Exps. 22, 23 are sol. in water. Insoluble 
 salts are not made in this way. PbCl 2 is only partially insoluble, hence HC1 
 will not dissolve much Pb. Table A shows that there are but two soluble salts 
 of Pb ; hence most acids do not act upon that metal. By reference to this 
 table you can judge what acids will probably act on a given metal. Will H 2 S O 4 
 dis. Ba? Pb? Cu? Will H Cl probably dis. Sn ? Ag? Hg? Mg? Will H 3 P0 4 
 dis. Pb? Ca? Ag? (a) Try any of the above. (b) Try .to dis. Pb in 
 HC 2 H 8 O 2 . Compare chemical sol., as shown in 23, with physical sol., Exp. 4. 
 What two processes in chemical sol.? 
 
 Terms : Insoluble, soluble, saturation, supersaturation. 
 
24. SOLUBLE SALTS FROM CARBONATES, 
 HYDROXIDS, OXLDS. 
 
 I, Carbonates. 
 
 (1) To a piece of CaC0 3 (marble or limestone) in a t.t. add 
 H 2 0, and a little H Cl. When the action stops, pour a little of the 
 liquid into an e.d., evaporate and notice the residue. See if it will 
 dis. in H 2 0. State your observations and the reaction. Test for 
 the presence of Ca by Exp. 74. (2) Try Na 2 C0 3 (or HNaC0 3 ) 
 with HC1. (3) CaC0 3 may be tried with H 2 S0 4 or HN0 3 . 
 
 II. Hydroxids. 
 
 (1) To some Fe(OH) 3 (made by adding NH 4 OH to FeCl 3 sol., 
 and pouring off the supernatant liquid after the ppt. settles) add 
 drop by drop just enough HC1 to dissolve it. (2) Try also HNO 3 
 and H 2 S0 4 on separate ppts. of Fe(OH) 3 . Evaporate and dis. in 
 H 2 as before. Test for Fe by Exp. 63. (3) Try A1(OH) 3 (made 
 from A1C1 3 sol. and NH 4 OH) with HC1. Evaporate, dis. in H 2 O, 
 and test for Al by Exp. 64. 
 
 HE. Oxids. 
 
 To 28 PbO (litharge) in an e.d. add some dil. HN0 3 and heat 
 it. Decant on a filter, partly evap. the filtrate, add H 2 0, and test 
 for Pb by Exp. 48. 
 
 Supplementary. Notice from Table A what carbonates and hydroxids are 
 soluble, (a) Add H 2 to a little Na 2 CO 3 (or K 2 C0 3 ) in a t.t. and boil a 
 minute, (b) In another tube cautiously add HC1 to Na^COs.. Explain the 
 difference between (a) and (b). (c) Into (a) pour cautiously a little H Cl. De- 
 scribe the action and explain it with reaction. Sol. salts may be made from 
 many other classes of cpds. besides the above. 
 
 Terms : Physical and chemical solution, decantation. 
 
25. INSOLUBLE SALTS BY PRECIPITATION. 
 
 Insol. Salts of Pb. 
 
 (1) Pour into a t.t. 5 CC Pb(N0 3 ) 2 sol. and add a few drops HC1. 
 (2) Try it again, substituting Nad sol. for HC1. (3) Use also a 
 sol. of N H 4 C1. Record results and write equations. (4) Now in 
 place of Pb(NO 3 ) 2 use a sol. of Pb(C 2 H 3 2 ) 2 , try the action of the 
 same three reagents as previously used, and make a similar record. 
 What is the ppt. in each case ? Could you obtain the same ppt. by 
 putting together any other sols., and if so, what ones ? 
 
 To 5 CC of each of the following sols, in a t.t. add a little sol. of 
 Pb(N 3 ) 2 or Pb(C 2 H 3 2 ) 2 and write the equation, underlining the 
 ppt. and writing the color above. (5) K 2 O0 4 . (6) K I. (7) K Br. 
 (8) NaOH. (9) Na 2 C0 3 . (10) Na 2 S0 4 . (11) K 4 FeCy 6 . 
 
 Supplementary. What are the only two soluble salts of Pb ? Law of 
 Ppn. : Whenever a mixture is made of two sols., one of which contains the positive 
 part and the other the negative part of an insoluble cpd., a ppt. of the insol. cpd. 
 will always form. 
 
 From Table A what salts of Ba are insol. ? (a) Try to make some of them 
 by the application of the above law. (b) Also try Fe(0 H) 3 . (c) Make HgS. 
 (d) Try to make MnS. (e) Make CaC O 8 . 
 
 Terms: Insoluble, precipitation, positive, negative. 
 
26. HYDROCHLORIC ACII>, HC1. 
 
 Preparation. 
 
 (1) Fill 2 recs. % full of water. Connect the apparatus as in Fig. 
 27, observing how the tubes extend. (A 
 safety-tube may also be used if desired.) 
 Then put into a flask 10 g NaCl (preferably 
 fused) and 20 CC H 2 S0 4 which has previ- 
 ously been mixed with 5 CC of H 2 0. Be 
 sure you have enough acid, or the flask is 
 liable to crack. Heat slowly for 10 or 15 
 minutes over asbestos, but do not let the 
 froth extend to the neck of the flask. Look 
 for any current in the liquid of the rec. 
 and explain. (2) Detach the apparatus 
 (at a, Fig. 27) and pass some of the escap- 
 ing gas over a few drops of NH 4 OH in an e.d. (If much gas is 
 accidentally breathed, inhale NH 3 .) Describe the fumes (note 
 whether they have any odor different from H Cl or N H 3 ), name 
 them, state the color, and write the equation for their production. 
 This is the ammonia test for H Cl. Ascertain whether the product 
 is gaseous, or solid, by dipping a rod into strong H Cl and holding it 
 over a bottle of NH 4 OH. (3) Pass some of the gas from the gen. 
 into a sol. of blue litmus. What does this show as to the solubility 
 of HC1 ? What else does it show ? 
 
 Supplementary. How would you test for the presence of N H 8 ? Generate 
 HC1 if possible from : (a) KC1 ; (b) NH 4 C1, using an open t.t. and applying the 
 usual tests, (c) Try PbCl2. Law of Formation of Gases : When two substances, 
 which can react so as to liberate a gas, are put together, that reaction will always 
 take place and the gas be formed. 
 
 Fig. 27. 
 
 Terms : Wolff bottle, flask, safety -tube, muriatic acid. 
 
27. HYDROCHLORIC ACID, HC1. 
 
 Properties and Tests, 
 
 (1) Test the liquid in each bottle (Exp. 26) with blue litmus 
 paper. (2) Taste a drop, using a s.r. (3) Cautiously note the odor. 
 (4) Put a piece of Zn into a t.t. and pour over it 5 or 10 CC of the 
 contents of the first Wolff bottle. (5) If a gas escapes, test its 
 combustibility. Explain fully with observations and equations. 
 (6) Put into a t.t. 5 CC Pb(N 8 ) 2 sol. and add a little of the liquid 
 from the first bottle. If a ppt. falls, pour a small part of it into 
 another t.t., add a little H 2 0, and boil a minute. Does it dissolve ? 
 What does that show ? Now add a little K 2 Cr 2 7 (or K 2 Cr0 4 ) sol. 
 Explain. (7) To 5 CC AgN 3 sol. add a little of the acid. If a ppt. 
 falls let it settle, then pour off most of the supernatant liquid, 
 leaving the residue ; then add N H 4 H and shake it. Finally 
 acidify cautiously with HN0 3 . Explain all results. (8) Test 
 HgN 3 sol. in the same way, adding N H 4 H at the end, but not 
 HN0 3 . By any of the above exps. can you determine which bottle 
 contains the stronger acid ? 
 
 Supplementary. (a) Add HC1 to Cu(NO 3 ) 2 sol. and explain the result, 
 (b) Separate Ag from Cu in a mixture of solutions of their nitrates. Try the 
 action of HC1 on sols, of : (c) Co(NO 3 ) 2 ; (d) NaNO 3 ; (e) KN0 3 ; (f) MgSO 4 . 
 What 3 chlorids are insol. in H 2 O, and how are they made ? 
 
 Terms : Analysis, reagent, pungent, acidify, alkalize. 
 
28. ETCHING WITH HYDROFLUORIC ACID, HF. 
 
 Cover thinly with beeswax or paraffin one side of a small piece 
 of glass. Spread the wax evenly over the surface, 
 by warming the other side of the glass and pour- 
 ing off the excess of melted wax. With a sharp 
 metallic point, as the handle of a file, mark 
 Fig. 28. some design through the wax when cold (Fig. 
 
 28). Put into a lead dish (it will spoil a porce- 
 lain e.d.) a very little HF sol. (be exceedingly careful not to get 
 any on the flesh) and with a camel's-hair brush spread some of it 
 over the design on the glass. Do this several times. Finally, 
 after a few minutes wash away the acid from the glass, melt and 
 pour off the wax, wiping off what remains with a cloth wet in 
 naphtha, or alcohol. Examine closely the result and describe it. 
 By reason of its affinity for Si0 2 , HF acts on the glass and forms 
 SiF 4 . The equation should be written. 
 
 Supplementary. Etch a t.t. so as to make a graduate of it. Why cannot 
 H F sol. be kept in glass bottles ? H F is made by treating powdered CaF 2 
 (fluorite) with H 2 S 4 in a lead dish. Write the equation (v. Exp. 89 for other 
 tests). The fumes must not be inhaled. 
 
 Terms : Etching, fluor spar, fluorid, fluorite, silica. 
 
29. NITRIC ACID, HNO 8 . 
 
 Fig. 29. 
 
 I. Preparation. 
 
 Introduce into a glass retort through the tubulure, holding 
 
 the foi*mer so as not to have the 
 chemicals touch the neck of the 
 retort (Fig. 29), 10 or 15* fine 
 NaN0 8 (or KN0 3 ) and 20 or 25 CC 
 3 H 2 S0 4 . 
 
 Adjust the apparatus as in 
 Fig. 30, having the neck of the 
 retort pass to the bottom of a wide 
 t.t., which is surrounded by water 
 in a wide tumbler, or bottle. The 
 water is to cool and condense the 
 acid from the vaporous state in 
 which it passes over. Apply the 
 Bunsen flame, using a plate and as- 
 bestos, for 15 or 20 minutes. Notice 
 the liquid running down the neck of 
 the retort, also any colored fumes 
 name and account for the latter, and 
 see whether they increase with the 
 heat the color of the liquid in the 
 t.t., and the cause of it. Do the ordi- 
 nary reactions (which should be writ- 
 ten) account for the fumes ? Observe 
 also the color of the product in the 
 retort. Heat may have reduced some 
 of the white Na 2 S0 4 to dark-colored 
 Na 2 S. Use great care not to get any 
 of the acid on the hands. The anti- 
 dote, after thorough washing, is HNaC0 3 (v. Eule 19). 
 
 II. Tests. 
 
 (1) Test the vapor from the end of the retort with a few drops 
 of N H 4 H. (2) Put a drop or more of the acid on a very few Cu 
 filings in an e.d. Observe and explain with equation. (3) Try 
 with a s.r. the action of a drop on the finger-nail, then wash it off 
 and add a drop of NH 4 OH. This shows its action on animal mat- 
 ter. (4) Try it also on a feather or on silk. (5) Try its decolor- 
 izing action on 3 or 4 CC of indigo sol. in a t.t. Try its action on 
 insoluble salts, e.g.: (6) CuS ; (7) CaC0 8 ; (8) BiOCl. State what 
 this shows of the solubility of the respective nitrates (v. alsoExp. 82). 
 
 Supplementary. (a) Compare the action of H N O 3 and H 2 S O 4 on wood. 
 Could HNO 3 be made from Pb(NO 3 ) 2 ? How are nitrates made? (b) Make 
 Zn(NO 8 ) 2 . (c) Try to dis. a little Sn in HN 3 in an e.d. (d) Try Sb. (e) Put 
 a drop of commercial HNO 3 on writing paper, another on newspaper. The 
 latter contains wood pulp, (f) Try to decolorize anilin solutions. 
 
 Terms: Fuming nitric acid, metastannic acid, xanthoproteic acid, salt of 
 nitric acid, nitrate, tubulure. 
 
 Fig. 30. 
 
30. AQUA REGIA. 
 
 I. Preparation. 
 
 Pour 2 or 3 CC of HISTOg into a t.t. containing 6 or 8 CC of HC1. 
 If there is no evidence of chemical action, warm the mixture a 
 minute and observe. To what is the color due ? Give reaction. 
 
 II. Tests. 
 
 (1) Into a part of the aqua regia introduce a little gold leaf by 
 winding it around a moist s.r., not letting it touch the sides of the 
 t.t. (2) Into another part drop a bit of Pt foil, qcm . If no action 
 ensues, heat it. Pt does not dis. as readily as Au. Try the 
 solvent action of aqua regia on : (3) Zn ; (4) Fe ; (5) Cu ; (6) Pb. 
 Give the usual explanations, reactions, etc., for each of the above 
 exps. Why should not the 'acid act as well on Pb as on the others ? 
 
 Supplementary. See if Au will dis. in : (a) HC1, or (b) HNO 3 . Also try 
 (c) Pt. Try Hg in (d) H Cl, then in (e) aqua regia. (f ) Try Fe in each and 
 notice the color of each liquid after filtering. Explain, (g) Test the 2 chlorids 
 of Fe by Exp. 63. 
 
 Terms : Nitro-hydrochloric acid, gold chlorid, ferrous and ferric chlorids. 
 
31. SULFURIC ACID, 
 
 I, Preparation. 
 
 Burn a small piece of S in a rec. in which there is H 2 enough 
 to cover the bottom, using a d.s. and confining the fumes as much 
 as possible by covering the mouth of the rec. 
 
 Pour into an e.d. 1 or 2 CC HN0 3 , and dip into this a piece of 
 strong paper, or cloth, or a wood shaving, and lower it into the rec. 
 of S 2 , holding it there for some time without dropping any acid 
 from it into the rec. See whether the fumes change color. Repeat 
 the operation several times. Explain the phenomena and give all 
 reactions. Cover the rec. with the hand and shake the liquid and 
 the gases well together. 
 
 II. Tests. 
 
 (1) Apply the litmus test. (2) Put a drop of the liquid on 
 writing paper, and evaporate it so as not to burn the paper. See 
 whether the paper is charred, blackened, or made rotten by the 
 liquid. Explain. This is a test for free H 2 S0 4 . (3) Add a 
 little of the liquid to 5 or 10 CC BaCl 2 sol. (or Ba(N0 3 ) 2 ) in a t.t., 
 state the effect and give an equation. If you obtain a ppt., add a 
 little H Cl and shake it well. Does it dissolve ? (4) Pour into a 
 t.t. containing 5 CC H 2 O the same amount of H 2 S 4 from the shelf 
 bottles. Observe any thermal effects on this mixture and explain. 
 Save the dilute acid in a separate rec. (5) Apply tests (2) and (3) 
 above to this mixture. (6) Pour a few drops of concentrated acid 
 upon 1 or 2 g sugar in an e.d. (7) Dip a small stick into a t.t. which 
 contains 1 or 2 CC H 2 S O 4 . (8) Pulverize a bit of starch, add a few 
 drops of the acid. If no change occurs, cautiously heat it for a 
 minute. Sugar is C 12 (H 2 0)n ; starch is C 6 (H 2 0) 5 ; cellulose is 
 C 18 (H 2 0) 15 ; explain the action of the acid. 
 
 Supplementary. Why is commercial H 2 S O 4 liable to be of a brown color ? 
 
 (a) Measure accurately 10 CC of concentrated acid in a graduate, leave it in 
 an open t.t. or rec. for a week, then measure it carefully again. Explain the 
 result, (b) Test commercial acid for PbS0 4 by pouring a little into an equal 
 vol. of H 2 O in a t.t. BaSO 4 is the only salt of Ba that is not dis. by HC1. 
 (c) Test Na 2 SO 4 sol. with BaCl 2 . Explain, (d) Test a sol. of Na 2 SO 3 for 
 
 Terms : Salt of sulfuric acid, fuming sulfuric acid, sulfate, starch, cellulose. 
 
32. AMMONIUM HYDBOXID, NH 4 OH; AMMONIA, NH 3 . 
 
 I. Preparation, 
 
 Powder and put into a flask about 10* 
 NH 4 C1 and 7 Ca(OH) 2 (freshly slaked is 
 best). Add 20 CC H 2 and connect with 
 Wolff bottles containing H 2 (Fig. 31), 
 as in the HC1 exp. Heat 10 or 15 
 minutes, using a plate and asbestos paper. 
 Observe the phenomena, especially the 
 pressure in the different bottles and the 
 absorption of gas, and write the reaction. 
 While the mixture is heating, do III. 
 
 Fig. 31. 
 
 II, Tests. 
 
 (1) Disconnect the flask while the gas is escaping (a, Fig. 31) r 
 put 2 or 3 drops HC1 into an e.d., and pass the gas over it from the 
 gen. Observe the fumes, giving equation. (2) Let the flask cool 
 as it stands, and test the liquid in each bottle (odor and litmus). 
 Put sols. (5 CC each) of the following substances into separate tubes, 
 and add a little of the prepared liquid to each : (3) FeS 4 ; 
 (4) FeCl 3 ; (5) A1C1 8 . Observe colors, especially -of ferrous and 
 ferric cpds. (6) Test likewise CuCl 2 sol., first with very little 
 NH 4 OH, then with excess. State and explain all phenomena. 
 
 III. Ammonia. 
 
 Mix 2 or 3* of fine NH 4 N0 3 with an equal quantity of Ca(OH) 2 , 
 put them into a t.t., and warm it over a flame. See whether a gas 
 escapes by : (1) cautiously taking the odor ; (2) testing with red 
 litmus paper ; (3) with H Cl. 
 
 Supplementary. (a) Put into a t.t. a gram or two of either (NH 4 ) 2 SO 4r 
 N H 4 NO 3 , NH 4 C1, or (NH 4 ) 2 C 2 O 4 , and add a little NaOH (or KO H) sol., warm 
 it, and apply tests. What two classes of cpds. are used to obtain ammonia ? 
 Are the above examples of double decomposition, and why ? Relation between 
 ammonia and ammonium hydroxid ? (b) Fill a t.t. with NH 8 by upward dis- 
 placement, and invert it over a rec. of water. Observe and explain. 
 
 Terms : Volatile alkali, fixed alkali. 
 
33. FIXED ALKALIES. 
 
 I, Sodium Hydroxid, NaOH. 
 
 To 5 CC of a saturated sol. of Na 2 C0 3 add about an equal quantity 
 of Ca(0 H) 2 sol. Shake the mixture well and observe. If a ppt. 
 falls, name it and write the equation. What goes into solution ? 
 Let the ppt. settle, then add some of the supernatant liquid to sols. 
 of : (a) Fe(S0 4 ) ; (b) FeCl 3 ; (c) A1C1 3 . Effects, colors, and equa- 
 tions should be given in each case. If any effect different from 
 what is expected occurs, it should be noted and explained. 
 
 II. Potassium Hydroxid, KOH. 
 
 Treat a sat. sol. of K 2 C 8 in precisely the same way as Na 2 C 3 
 above, making close observations and taking full notes as before, 
 including all the tests given. 
 
 Supplementary. Compare the action of fixed alkalies with that of N H 4 O H 
 on sols, of Fe and Al salts, (a) Obtain some NaO H or KO H in the solid state. 
 In what other ways were NaO H and KOH made in the laboratory ? (b) Would 
 Ca(OH) 2 actonNaCltoformNaOH? (c) Ca(0 H) 2 on Na^S O 4 ? (d) Is FeCl 3 
 sol. acid, alkaline, or neutral ? (e) Is A1(O H) 3 soluble hi excess of NaO H or 
 KOH sol.? 
 
 Terms : Hydroxid, hydrate, alkali metals, metals of alkaline earths. 
 
Fig. 32. 
 
 34. OXIDS OF NITKOGEN. 
 
 I. Nitrogen Monoxid, N 2 (Nitrous Oxid). 
 
 (1) Put into a flask (of 200 CC capacity) 10* of NH 4 N 8 , not too 
 
 coarsely crystalline (so as not 
 to break the flask in melting). 
 Connect the flask with a large 
 t.t. (resting in a rec. of H 2 0, 
 Fig. 32), or with a rec. which 
 contains no water (Fig. 33), and 
 from this t.t. or rec. have a d.t. 
 leading to a p.t, so as to collect 
 the gas over water. Ha.ve the 
 joints tight and the tubes pass 
 through the stoppers. Apply 
 heat not too rapidly, notice the 
 order of changes and give the 
 main reaction. Are there any 
 fumes in the flask ? Is the gas 
 colored, and why ? Obtain 2 
 recs. of gas, then remove the 
 lamp and take the d.t. from the 
 water, letting the flask cool on 
 the r.s. (2) Taste a drop of the 
 liquid in the large t.t. or rec., 
 and also test with litmus, red and blue. Some NH 4 N0 3 will 
 probably have been driven over, also some NO, N0 2 , HN0 3 , etc., 
 formed by breaking up of NH 4 N0 3 . (3) Test the gas with a burn- 
 ing stick, also with a glowing one. (4) Test the combustibility of S 
 (well burning when introduced), and (5) of P. Compare the bril- 
 liancy of flame and the products obtained with those in 0, and write 
 all equations. 
 
 Supplementary. Compare the action of heat on NH 4 N0 3 with that on 
 Pb(N0 3 ) 2 in Exp. 10. Compare with the action of NaNO 3 + H 2 SO 4 (Exp. 29). 
 Learn the symbols and names of all the oxids of N. Try the action of heat 
 (using a t.t.) on: (a) KN0 3 ; (b) Hg(N0 3 ) 2 ; (c) Zn(NO 3 ) 2 ; (d) Pb(NO 3 ) 2 . 
 
 Fig. 33. 
 
 Terms : Laughing gas, nitrous oxid, nitrates, nitrites. 
 
35. OXIDS OF NITROGEN. 
 
 II. Nitrogen Dioxid NO or N 2 2 (nitric oxid). 
 
 (1) Arrange the app., with inverted recs., as for the hydrogen 
 exp. Then put into the gen. (or t.t.) 5 g Cu turnings, cover them 
 with water and add through the thistle tube 5 CC of HN0 3 . Collect 
 2 or 3 recs. of the gas. If action stops add a little HN0 3 (or Cu, if 
 necessary). Save any Cu that is left. Explain the different colors 
 of the gases and the color of the liquid. (2) Test the gas with a 
 burning stick. Explain the fumes. Test also with (3) S and (4) P 
 (well burning). In (4) see whether the solid gradually separates 
 from the gas. Take full notes. 
 
 III. Nitrogen Trioxid N 2 3 and Tetroxid N0 2 or N 2 4 (peroxid). 
 
 (1) Lift a rec. of the gas N 0, just prepared, from the shelf of 
 the p.t. What is the effect, what is the new gas, and how is it 
 formed ? (2) Heat 1 or 2 crystals of Pb(N0 3 ) 2 in a t.t., and while 
 the gas escapes insert a glowing stick into the tube. (3) Put a 
 fragment of starch into a t.t. and add a few drops of HN0 3 . Heat 
 cautiously. 
 
 Supplementary. State how the oxids of N are derived from H N O 3 and 
 nitrates. What action have heat and reducing agents on nitrates ? (a) Notice 
 the action of direct sunlight on strong H N O 3 in stoppered bottles, (b) Try the 
 action of heat on other nitrates, e.g., Cu(NO 3 ) 2 , KNO 3 . (c) Heat a bit of 
 powdered charcoal on a plate or asbestos, and when it is hot add a drop of 
 HN0 3 with a s.r. N 2 3 and N0 2 are both red and not distinguishable. Find 
 how N 2 Og is prepared, and its relation to HNO 3 . 
 
 Terms : Nitrous and nitric anhydrids, nitrogen peroxid, nitric oxid. 
 
36. CARBON DIOXED, CO 2 . 
 
 I. Preparation. 
 
 Put 10 or 15 g CaC 3 (marble, in lumps) into a 
 t.t. or gen. (Fig. 34), cover with H 2 O and after 
 having the app. all prepared add 5 CC HC1. Add 
 more of the reagents as needed. Enough must be 
 used to produce vigorous action. Attach a delivery 
 tube and collect a rec. of gas by downward displace- 
 ment, having the tube reach to the bottom of the rec. 
 Fig. 34. It will take only a minute. 
 
 II, Tests. 
 
 (1) Test the gas with a burning stick. (2) Let the gas 
 bubble from a d.t. into 5 CC Ca(OH) 2 sol. in another t.t. and look for 
 a ppt. Let the action continue until the liquid clears. (3) When 
 the sol. is clear, boil it for a minute and notice the reappear- 
 ance of the ppt. Explain all the phenomena very fully, giving 
 equations at the proper places. (4) Pass the gas 
 into a sol. of blue litmus. (5) Observe the Ca flame 
 (bring the open mouth of the C0 2 gen. close to a 
 Bunsen flame). Small particles of CaCl 2 are carried 
 up by the gas. (6) Also dip a stick into the sol., 
 hold it in the flame and notice the color. (7) Take 
 2 or 3 CC Ca(0 H) 2 sol. in a clean t.t. and breathe into 
 it through a glass tube. What does the result show ? 
 (8) Put a little lime water into an e.d. and look for 
 a scum after a few minutes ; or draw the air through 
 a rec. of lime water (Fig. 35), by suction, applying 
 The air enters at a, and any C 2 is drawn through 
 
 Fig. 35. 
 
 the lips at b. 
 
 the lime water. Explain. 
 
 Supplementary. (a) See whether you can obtain C 2 from Na 2 C 3 . Use 
 an open t.t. and test the gas with a drop of Ca(0 H) 2 sol. on a s.r. (b) Use also 
 HNaC0 3 . (c) K 2 CO 3 . (d) Test some oyster, clam, or other shells with a drop 
 of HC1, and see whether there is effervescence ; or put them into a gen. and 
 test the gas. (e) Obtain CaCl 2 from the C O 2 gen. (f ) Test that salt for Cl 
 (Exp. 90). (g) For Ca (Exp. 74). (h) Obtain CaSO 4 from CaC 8 . (i) Ca(NO 3 ) 2 . 
 
 Terms: Carbonate of lime, quicklime, slaked lime, lime water, milk of 
 lime, sulfate of lime. 
 
37. CHLOKIN. 
 
 I. Preparation from Hydrochloric Acid. 
 
 Put into a flask (or t.t.) 5 g Mn0 2 (preferably granulated) and 
 10 CC H Cl. Shake them well together, apply gentle heat, and avoid 
 inhaling the gas, but collect it by downward displacement in a rec. 
 loosely covered with paper. Add more HC1 if it is needed. Ob- 
 serve and describe, with equations. Note when the rec. is filled, to 
 avoid passing the gas into the room. If accidentally any is inhaled, 
 the antidote is vapor of alcohol (inhale from a handkerchief) ; or 
 NH 3 will do. State the color of the gas, its sp. gr. compared with 
 air, its effect on the nasal organs. 
 
 II. Tests and Properties, 
 
 (1) Drop into the rec. a piece of dry Turkey-red cloth (or of 
 calico), also bits of printed and written paper. If there is little 
 or no effect add a very little water, shake the gas, water, cloth and 
 paper well together, and note the effect. Which bleach better, wet 
 or dry fabrics ? (2) Into another rec. of Cl (dried if possible) file 
 a little Sb (or stibnite, Sb 2 S 3 ). Describe the result and give an 
 equation. Is this a case of ordinary combustion ? Pass some Cl 
 from the gen. into sols, of : (3) AgN0 3 ; (4) Pb(N0 3 ) 2 ; (5) H 2 S. 
 
 Supplementary. (a) Put into a small beaker 5s bleaching powder, CaCl 2 0, 
 set this into a larger rec. or beaker, putting into this last the substance to be 
 bleached. Cover the large rec. with pasteboard, through which passes a thistle- 
 tube into the smaller. Pour through the thistle- tube 5 CC dilute H 2 SO 4 (half 
 H 2 O and half acid). Add more, if needed, (b) Mix a gram of fine NaCl with 
 a gram of Mn0 2 , add in a t.t. 2 CC H 2 O and 3 c c H 2 SO 4 , and heat. Observe any 
 gas. Test it with N H 3 , or otherwise, (c) Dip some unglazed paper into oil of 
 turpentine, CioHie, in an e.d.; warm it by holding the paper near a flame for 
 an instant (or heat the turpentine in an e.d. over a waterbath), but do not set it 
 on fire. Then at once thrust the paper into a rec. of Cl. Explain the combustion 
 and describe all you saw, giving the equation. Clean the rec. with naphtha or 
 petroleum. 
 
 Terms : Bleaching, bleaching powder, calcium hypochlorite, chlorid of lime. 
 
38. EUCHLORIN, C1O 2 , CL 
 
 I. Preparation. 
 
 Drop into a t.t. 3 or 4 crystals of K C10 3 . Add a few drops 
 H 01, heat for an instant and then add 5 or 10 CC H 2 0. 
 
 II. Tests. 
 
 (1) Observe carefully the action, noting the color and odor 
 (cautiously), and give equation. (2) To 2 CC indigo sol. in a t.t. add 
 a little euchlorin. Is the color discharged ? Test in the same way 
 sols, of (3) litmus and of (4) cochineal. (5) Try K 2 O 2 7 sol. (a 
 mineral pigment ; the other three are vegetable or animal coloring 
 matters). What do you conclude from this ? (6) Very cautiously 
 add 2 or 3 drops of H 2 S 4 to 2 or 3 small crystals'of K C10 3 in 
 a t.t. at arm's length from the operator, then fill the t.t. with H 2 0. 
 Describe the result with equation. (7) Try to bleach a piece of 
 Turkey-red cloth or calico by putting it into some euchlorin and 
 leaving it a few minutes. 
 
 Supplementary. (a) Try to bleach K Mn0 4 sol. Will euchlorin dis. : 
 (b) Au ? (c) Zn ? (d) Cu ? Try its action on sols, of : (e) AgN0 3 ; 
 (f)Pb(N0 3 ) 2 ; (g)HgN0 3 . 
 
 Terms : Euchlorin, oxids of chlorin, detonation. 
 
y /v 
 
39. BKOMIN AND BROMIDS. 
 
 I. Preparation of Br. 
 
 (1) Make some starch paste by pulverizing a piece of starch not 
 larger than a pea, adding 10 CC H 2 and boiling several minutes in 
 a t.t.; cool it and dil. with 10 CC H 2 0, shaking it well. Boil again if 
 necessary. [Save part of this for subsequent exps.] (2) Mix 1 or 
 2 crystals of KBr with an equal quantity of Mn0 2 , put them into 
 a t.t. and add a few drops H 2 S0 4 . Heat the mixture and observe 
 carefully. Write the equation, and explain the action. 
 
 H, Tests. 
 
 (1) Dip a strip of paper into the starch paste, wind it around 
 the end of a s.r. and carefully put it into the t.t., so as not to touch 
 the sides. Then heat the mixture in the t.t. Observe the effect of 
 the Br on the starch. The product is supposed to be starch bromid. 
 Avoid getting much Br into the air in the room, or inhaling it. 
 Alcohol vapor, or ammonia, is the antidote, as for Cl. Do you 
 notice any effect of Br vapor on the eyes ? (2) To a sol. of KBr 
 add a few drops of euchlorin. Describe and explain, stating which 
 is the more stable or stronger cpd., KBr or KC1, and how this exp. 
 shows it. (3) Add to a few drops of starch paste 10 CC H 2 0, shake 
 it well, add a few drops of KBr sol. and one drop of euchlorin. 
 Describe and explain. 
 
 Supplementary. Liquid Br should be examined, (a) Try the action of 
 Br on a mixture of starch paste and KI sol. Try the action of H 2 S0 4 on (b) a 
 few drops of K Br sol. , also on (c) a crystal of K Br. (d) Pour a little Br vapor 
 from a gen. into 5 CC of KI sol. (e) Put a drop of CS 2 into a t.t. with a few 
 drops of KBr sol., then add a few drops of euchlorin and shake it. Notice the 
 color of the C S 2 at the bottom of the tube. The Br was set free and dis. by 
 the CS 2 . 
 
40. IODIN AND IODIDS. 
 
 I, Preparation of I. 
 
 Prepare I like Br in the previous exp., using KI instead of 
 KBr. Notice the difference in its action, color, state, etc., and give 
 a full description with equation. 
 
 II. Properties and Tests. 
 
 (1) Make the same tests with starch as in Exp. 39, noting the 
 different results. (2) Warm 1 or 2 crystals of I in a dry t.t. 
 Notice the color of vapor, and its relative weight (pour a little into 
 a dry e.d.). (3) While warming the tube hold a s.r. half way down 
 the t.t. Look for a sublimate on the rod and on the sides of the 
 tube, examining carefully its form, luster, and color. (4) Put into 
 a small t.t. 1 or 2 crystals of I, add 3 or 4 CC of alcohol, C 2 H 5 OH, 
 and warm a minute. Explain, then (5) add a drop of this with a 
 s.r. to a drop of starch sol. shaken up with 10 or 15 CC of H 2 0. Ob- 
 serve the color of the product (starch iodid), and boil it a moment 
 to see whether the color disappears. If not, too much I was used. 
 When it is cool (hold the tube under a jet of water) observe again. 
 
 Supplementary. (a) See whether a crystal of I will dis. in H 2 O. To de- 
 termine this apply the starch test, (b) To 5 or 10 CC H 2 O add a drop or two of 
 CS 2 and of KI sol. (examine), then one drop of euchlorin. Shake well, let 
 stand, and note the color of the C S 2 globule, (c) Test the solubility of I in 
 ether (C 2 H 5 ) 2 O, keeping the latter away from the flame, (d) Obtain crystals 
 by letting the ether sol. evaporate, (e) To 10 CC H 2 O add a few drops KI sol. 
 and a few drops of starch paste. Shake well together and note the color. Now 
 add one drop of euchlorin (Exp. 38). If too much euchlorin is added the sol. 
 becomes green or black (ppt. of I). Describe the coloration and explain fully, 
 (f) Repeat (e) of Exp. 39 with KI sol. 
 
 Terms : Sublimation, sublime, crystal, tincture. 
 
41. EXPERIMENTS WITH SULFUR. 
 
 I. Crystallization, 
 
 Into a small beaker or large t.t. put 10 or 15 g S, and slowly 
 melt it over a lamp (using sand bath or asbestos), not allowing it 
 to become darker than amber-color. When it is melted remove the 
 lamp, leave the beaker in position (or hold the t.t. in the hand), 
 and when crystals begin to shoot across the surface, pour the liquid 
 S remaining into water in an e.d. Explain. 
 
 Loosen the S by pouring round the edges a little H N 3 . Warm 
 if necessary, when the mass may be removed with a thin knife-blade. 
 
 II. Allotropy. 
 
 Put 10 g S into a t.t. and slowly melt it. Notice the yellow color, 
 and see that the liquid (now above 100) is very thin. Slowly 
 continue to heat it till it becomes black. Note that it is now very 
 thick and can scarcely be poured (about 200). Apply more heat 
 till it grows thin again (above 300). Now heat to boiling (over 
 400), note the color of the vapor, and any sublimate on the t.t. 
 If it takes fire (S burns at 230), cover the mouth of the tube 
 with paper or cardboard for a minute. Pour the S into an e.d. of 
 water. Pull it and note its elasticity. Is it now crystalline, or 
 amorphous ? See whether it afterward changes. Clean the t.t. as 
 before. 
 
 III. Solubility. 
 
 Place in an e.d. -J g pulverized brimstone and cover it with CS 2 
 (avoid a flame, as CS 2 is explosively inflammable). See whether 
 any dissolves. Let it stand till the C S 2 has evaporated, watching 
 it meantime. Describe fully the phenomena. 
 
 Supplementary. (a) Try to dis, a little S in ether, (C 2 H 5 ) 2 O, and let 'it 
 evaporate. Is S soluble in H 2 ? (b) Grind together on a brick with, a pestle 
 or other implement, not over a half gram of S and K C10 3 . (c) Make gunpowder 
 by mixing intimately very fine KNO 3 , C, and S (a small quantity of each). Pile 
 the mixture on a brick and cautiously set it on fire. If this reaction is correct, 
 in what proportion should the constituents be mixed :2KNO 3 + 3C + S = K 2 S 
 +3 CO 2 + 2 N ? (d) Obtain flowers of S by sublimation and see whether they 
 are crystalline or globular (use compound microscope), (e) Add HC1 to a sol. 
 of Na-jS^s and look for a S ppt. (f ) Obtain S O 2 from S, also from H 2 S 4 . 
 (g) Try to bleach with it a green leaf or a blue petal. 
 
 Terms : allotropy, allotropic, fusion, crystalline, globular, amorphous. 
 
42. HYDROGEN SULFLD. 
 
 Preparation and Tests. 
 
 (1) Put into a gen. (rec. or t.t.) 5*FeS, 10 CC H 2 0, and 5 ec HC1 
 
 (or H 2 S0 4 ). Adjust a d.t., having the 
 joints perfectly tight, and pass the gas 
 for a minute or two into 5 CC H 2 in an- 
 other t.t. or beaker (Fig. 36). Note the 
 odor. Can you determine whether 
 e gas is soluble in H 2 ? (2) See 
 whether the sol. is acid, alkaline, or 
 Fi g-36. neutral. With a s.r. put a drop of 
 
 H 2 S sol. on bright coins of (3) Ag and (4) Cu. State the effect, 
 products, reactions. (5) Put a drop of Pb(C 2 H 3 2 )2 sol. on paper and 
 pass the gas over it from the tube of the generator. Describe the 
 effect (this is the characteristic test for H 2 S) and write the equation. 
 Is there any other way in which you would recognize this gas ? 
 
 (6) Try the combustibility of H 2 S, using a philosopher's lamp. 
 
 (7) If it burns, hold a glass tube or a crayon in the flame. 
 Explain. 
 
 II. As a Reagent. 
 
 Add a little H 2 S sol. to 5 CC of each of the following sols., describe 
 the results, write equations where necessary, and explain why there 
 is no effect in certain cases : (1) HgCl 2 , (2) CuCl 2 , (3) BaCl 2 , 
 (4) CaCl 2 . (5) Next mix 3 or 4 CC CuCl 2 sol. and the same 
 quantity of BaCl 2 sol., add H 2 S sol., shake it well and filter. What 
 is the residue and what does the filtrate contain? (6) Now to the 
 filtrate add a sol. of Na 2 C0 3 . State the effect, give the reaction, 
 and explain how the Cu and the Ba have been separated. 
 
 III. Test for Sulfids. 
 
 To a little Na 2 S or CaS add H 2 S0 4 . If any gas arises (heat if 
 necessary) try the Pb(C 2 H 3 2 ) 2 test. 
 
 Supplementary. See whether you can separate (a) Cu from Ca ; (b) Ca 
 from Hg ; (c) Hg from Ba ; (d) Fe from Cu. How are some insol. sulfids made ? 
 (e) Test FeS for a sulfid ? What sulfids are insoluble ? 
 
 Terms : sulfuretted hydrogen, sugar of lead, sulfid. 
 
43. PHOSPHORUS. 
 
 Caution: Phosphorus must be handled with forceps, as the 
 burns from it heal very slowly, and all experiments with it must 
 be done cautiously. None should be dropped upon the floor, nor 
 left upon the apparatus, and all must finally be burned. C S 2 must 
 be kept away from the flame. 
 
 I. Spontaneous Combustion, 
 
 (1) Into an e.d. put 10 or 20 CC of C S 2 (for a class) and drop into 
 it 3 or 4 small pieces of P. Notice the odor of CS 2 and whether 
 the P dissolves in it. Also observe the color and luster of newly 
 cut P. (2) Dip a piece of unglazed paper into the sol., then place 
 it on the ring of a r.s. till it is dry, looking out for any action. If 
 such occurs state fully ivhat has caused it and whether it is a case 
 of ordinary combustion. 
 
 II, Combustion under Water. 
 
 Put into a large t.t. 4 or 5 crystals of KC10 3 , cover it with H 2 
 and add a small piece of P. Rest the t.t. in a rec., and then slowly 
 add 2 or 3 CC H 2 S O 4 through a thistle tube which reaches to the P 
 and K C10 3 . Account for the phenomena. What color is the liquid, 
 and what is the cause of it? HKS0 4 , HC10 4 , C10 2 and H 2 
 are formed. Write the equation for forming them, and for the 
 combustion. What compound of P is finally formed ? 
 
 Supplementary. (a) Put a small piece of P into a dry e.d. in a dark room, 
 observe, and explain the result, (b) Put a piece of P on a dry- plate or e.d., set 
 it on fire and at once cover with a dry inverted rec. When the fumes settle add 
 a very little water. Test the product with litmus, (c) Cover a small piece of 
 P with bone black in a plate, and leave for some time. If no action ensues 
 burn the P before leaving the Exp. 
 
 Terms : spontaneous combustion, phosphorescence. 
 
% w > : r <3 
 
 V^ * 
 
44. ARSENIC. 
 
 I. Marsh's Test. 
 
 Caution : AsH 3 is a deadly poison, and must not be inhaled. 
 If the H is ignited before introducing the As compound there is 
 little danger. 
 
 Prepare a hydrogen gen., with or without a CaCl 2 drying attach- 
 ment, and with lamp tube (Fig. 37, or model). Put in a few pieces 
 
 of arsenic-free Zn, some distilled 
 water, and C.P. HC1. After a few 
 minutes test the H gas (Exp. 13) 
 before lighting, and when no sharp 
 explosion occurs light the gas, and 
 observe the color of the flame. Test 
 37 - for As by holding an e.d. over the 
 
 flame. Now pour through the thistle tube 1 or 2 CC of a sol. that 
 may be supposed to contain some cpd. of As. This sol. may be 
 obtained either by dissolving HNa 2 As0 3 in H 2 with a little HC1, 
 or by immersing in HC1 a small piece of green paper tag from 
 which any As that may be present will dis. as AsCl 3 . Note any 
 change in the color of the flame; hold an e.d. or other cold body 
 in the flame and look for a deposit ; put a Bunsen flame under the 
 drawn out tube (Fig. 37) and look for a sublimate just beyond. 
 Absence of a sublimate in either 'case indicates absence of As. 
 Explain fully, writing all equations. 
 
 II. Reinsch's Test. 
 
 Into a sol. of an As salt (obtained by HC1 as above) in a beaker 
 or e.d. put a small strip of bright Cu foil and heat for a few 
 minutes. Notice that the foil changes color. After a few minutes 
 remove it, dry it by carefully pressing between folds of blotting 
 paper, cut it into strips, and put them into a t.t. ; heat the latter. 
 Notice the vapor and sublimate, As 4 6 , on the tube. This sublimate 
 may be examined under the microscope after first breaking the 
 tube. Explain all results, using equations. 
 
 Supplementary. (a) Reduce As 4 O 6 as follows : Mix intimately a bit of it 
 not larger than a wheat grain with as much powdered charcoal, put the mixture 
 into a small t.t. or i.t. and heat strongly. Note the vapor, color, sublimate, 
 (b) Make Scheele's green by mixing sols, of CuCl 2 and HNa^AsOs (or other sol. 
 cpds.) and having them nearly neutral, (c) Try the effect on these mixtures of 
 (d) excess of HC1, (e) excess of NH 4 OH. (f) See whether As 4 6 is very soluble 
 in H 2 by putting a very little into a t.t. and heating with H 2 0. (g) Heat a little 
 powdered arsenopyrite, FeAsS, in a t.t. and note the odor, (h) Test some 
 wall paper, or colored silk, for As. 
 
45. COMPOUNDS OF BORON. 
 
 I. Boric Acid. 
 
 Put 5* of Na 2 B 4 7 into a t.t., add 10 CC of dil. H 2 S0 4 and boil 
 till it is clear, adding more water if necessary. Then cool it by 
 holding the tube under a jet of water, keeping watch for crystals. 
 When it is cool pour off the supernatant liquid and rinse the 
 crystals once or twice with water to remove the H 2 S 4 , then put 
 them into an e.d. Add a very little water, and when the crystals 
 have dissolved dip into the sol. a piece of turmeric paper, which 
 should then be dried and the color noted. Describe fully the 
 results. 
 
 II. Borax Beads. 
 
 Make a loop in the end of a Pt wire (which is welded into a 
 
 short glass tube, Fig. 38) . Moisten 
 
 c=s=s=^ o the loop end and dip it into some 
 
 powdered borax, Na 2 B 4 7 . Now 
 heat it, using the mouth blowpipe, 
 
 dipping it again into the borax if more is wanted, and heating till 
 a clear transparent bead is obtained. Describe and explain the 
 phenomena. Beads may be colored as follows : If blue is wanted 
 dip the clear bead into a very dil. sol. of some Co salt, as CoCl 2 , and 
 fuse again. -(If too much Co is used it will look dark.) For other 
 colors v. Table G. Detach the beads by suddenly jerking the Pt 
 wire while the bead is fused. Save the beads, and label them, 
 stating the coloring material. 
 
 Supplementary. (a) See whether H 3 B 3 is more, or less, soluble in hot 
 water than in cold, (b) Make a bead of H 3 B 3 if possible, (c) Stir a little 
 H 3 B O 3 in an e.d. with a few drops of CgHsOH. Then take some of the mixture 
 on a short glass tube and hold it in a Bunsen flame, noting the color imparted 
 to the latter, (d) Try the same with Na^O?, (e) then with Na2B 4 O 7 to which 
 has been added a few drops of H 2 S0 4 . 
 
 Terms: borax bead, flux. 
 
46. COMPOUNDS OF SILICON. 
 
 I. Silicic Acid and Silica. 
 
 Pour a few cubic centimeters of water glass, H 4 Si0 4 , into an e.d. 
 and add a little H Cl. Note the phenomena, describe the result and 
 write the equation. Pour off the extra HC1 and rinse the residue, 
 H 4 Si0 4 , 2 or 3 times with H 2 0. Now heat it over a Bunsen flame, 
 with stirring. This leaves Si0 2 . Write the equation, and note how 
 the product feels when rolled between the fingers. Is silicic acid 
 made differently from other acids ? Pulverize (in a mortar if 
 necessary) some of the Si0 2 obtained, to use in the following. 
 
 II. Silicates by Solution. 
 
 Make a strong sol. of NaO H (or K H) and add to it some of 
 the Si0 2 obtained above, very finely powdered. Heat and stir 
 the mixture for some time. See whether the Si0 2 dissolves, and 
 write an equation. 
 
 III. Silicates by Fusion, Glass. 
 
 Make a small mixture of equal parts of powdered Na 2 C0 3 
 and K 2 C0 3 and fuse the mixture into a bead as in the case of borax. 
 Note that the bead is opaque when cold. Is it so when hot ? Dip 
 this bead when hot into a little Si0 2 powdered very finely, then 
 heat again more strongly in the hottest part of the flame. If it is 
 not transparent when cold, dip it again into the Si0 2 and heat more 
 strongly than before. See whether it now resembles glass. Describe 
 all phenomena and write the equations. Colors may be obtained as 
 in borax beads, Table G. 
 
 Supplementary. (a) Try to dis. finely powdered Si0 2 in a strong sol. of 
 Na 2 CO 3 , boiling the mixture, (b) Try to fuse Si0 2 in a borax bead. 
 
 Terms: fusible, infusible, fusion, transparent, opaque, silica, silicate, glass, 
 water glass. 
 
47. OXIDATION AND REDUCTION. 
 
 I. Oxidation. 
 
 (1) Into each of two tubes put 5 CC FeS0 4 sol. (freshly dissolved). 
 
 To one of these add a few drops HN0 3 and boil a minute, then cool. 
 
 To each of the tubes add 5 CC NaO H sol. (or NH 4 OH). Observe the 
 
 color effects, explain their causes, and give equations for the ppts. 
 
 Explain the action of H]ST0 3 . 
 
 (2) Put a small fragment of Pb on a piece 
 of charcoal, slightly hollowed out with the 
 handle of the forceps. Fit a metallic tube to 
 a Bunsen burner, and with a mouth blow-pipe 
 blow the oxidizing flame (outer) strongly and 
 steadily against the Pb for 4 or 5 minutes 
 (Fig. 39). What first takes place? As you 
 stop blowing, notice the yellow vapor that 
 escapes from the globule of Pb : also the yellow 
 
 a, red^Snfflame. coating of Pb on the charcoal. Explain fully, 
 
 b, oxidizing flame. using equations. 
 
 II. Reduction. 
 
 (1) Pour a little FeCl 3 sol. into two tubes. Pass S 2 gas, or 
 H, from a gen. into one of these for a few minutes. Next add 
 NH 4 OH to each. Compare the products and explain, with 
 equations. What action has the S0 2 ortheH? Try the action 
 of Zn and H, or of Zn alone. 
 
 (2) Put g PbO on a piece of charcoal hollowed out as before. 
 With the blow-pipe blow the reducing flame (inner) steadily against 
 it for some time, or until a metallic globule is obtained. What is 
 it? Explain fully, with equation. See whether the globule is 
 sectile (can be cut) or malleable (can be flattened by pressure). 
 Extinguish the fire, if the coal still glows, with a drop of water. 
 
 Supplementary. Notice that the action of the flames here is like that of 
 oxidizing and reducing agents generally, (a) Experiment with other metals and 
 oxids. (b) See whether Fe(OH) 2 or Fe(OH) 3 tends to change to the other on 
 standing. Which is the more stable cpd. ? (c) Try sols, of FeS 4 and FeCl 3 
 in the same way. (d) Try to oxidize FeSO 4 sol. with a little euchlorine. 
 (e) Oxidize HgN0 3 with HNO 3 . (f) Try to reduce K 2 Cr 2 O 7 sol. to CrCl 3 with 
 a little HC1, C 2 H 5 OH and heat. Note the change in color, also test by Exp. 48. 
 Are these oxidizing, or reducing agents: (g) KC10 3 , (h) KNO 3 , (i) C, (j) Cu ? 
 (k) Pulverize about a gram of K N O 3 and mix it with a like quantity of fine 
 charcoal. Put into a dry i.t. and heat. (1) Try KNO 3 and S in the same way. 
 
 Terms: Oxidation, reduction, oxidizing agent, reducing agent, oxidizing 
 flame, reducing flame. 
 
48. LEAD, Pb". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. PbCl 2 (v, Ag, Hg'). 
 
 
 
 
 To Pb(N0 3 ) 2 sol. add HC1, filter 
 (test fil.), wash, reject washing 
 (and fil. if no more PbCl2 falls). 
 
 (1) PbCl 2 
 
 white 
 
 
 2. Dis. PbCl 2 in hot H 2 0. (v. Ag, 
 
 Hg')- 
 
 
 
 
 Pour on res. (1) boiling H 2 from 
 t.t. Save fil. 
 Repeat this several times. 
 
 
 
 (a) PbCl 2 
 
 3. Final test for Pb. 
 
 
 
 
 To first filtrate (a) add K 2 Cr 2 7 
 sol. (or K 2 Cr0 4 ). 
 
 (2) PbCr0 4 
 
 yellow 
 
 
 Supplementary. 1. PbCl 2 is somewhat sol. in H 2 0, hence traces of it are 
 tested for in Grp. II. 3. If there is much free acid in a sol. the K 2 Cr 2 7 test is 
 not to be relied on. H 2 S 4 should then be used. What other Pb salt might be 
 used for sol. (Table A) ? (a) Allow some of the hot water sol. of PbCl 2 to cool 
 in a t.t. and look for crystals. Explain, (b) See which is the stronger cpd. 
 PbCl 2 or PbCr0 4 . (c) Make several other final tests for Pb. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENT. 
 
 REMARKS. 
 
 1 
 
 2 
 
 AmOH 
 NaOH 
 
 Pb 2 0(OH) 2 
 Pb(OH) 2 
 
 white 
 u 
 
 ( NaOH (ex.), 
 
 With PbAc 2 no ppt., 
 Pb 2 OAc 2 being sol. 
 
 8 
 
 Am 2 C0 3 
 
 Pb 3 (C0 3 ) 2 (OH) 2 
 
 u 
 
 
 STaOH (ex.), 
 
 
 4 
 
 NfeCOa 
 
 Pb 3 (C0 8 ) 2 (OH) 2 
 
 u 
 
 
 INO 
 
 
 5 
 
 HC1 
 
 PbCl 2 
 
 (i 
 
 ]_ 
 
 I 2 (boiling) 
 FTfll (sL) 
 
 Re-ppts., cryst., on cooling. 
 
 G 
 
 H 2 S 
 
 PbS 
 
 black 
 
 dil. HNO.t 
 
 HN0 3 (str.) forms PbS0 4 . 
 
 
 
 
 
 
 H 2 S + HX0 8 ppts. S. 
 
 7 
 
 Am 2 S 
 
 PbS 
 
 u 
 
 dil. HNOs 
 
 HN0 8 (str.) forms PbS0 4 . 
 
 
 
 
 
 
 Am 2 S + HX0 8 ppts. S. 
 
 8 
 
 KI 
 
 PbI 2 
 
 yellow 
 
 H 2 boiling 
 
 Re-ppts., cryst., on cooling. 
 
 9 
 
 H 2 S0 4 
 
 PbS0 4 
 
 white 
 
 
 TaOH'(ex ) 
 
 Dis.by Na 2 S 2 O 3 (v. BaS0 4 ). 
 
 10 
 
 K 2 Cr 2 7 
 
 PbCr0 4 
 
 yellow 
 
 
 
 gaUS 
 
 HC1 changes ppt. to PbCl 2 . 
 
 11 
 
 Am 2 0x 
 
 PbOx 
 
 white 
 
 
 WE*^ 
 
 
 12 
 
 HNa 2 P0 4 
 
 Pb 3 (P0 4 ), 
 
 (4 
 
 
 
 'JaOH (ex.), 
 
 
 13 
 
 KCy 
 
 PbCy 2 
 
 U 
 
 KCy (ex), 
 
 Boiling re-ppts. 
 
 14 
 
 KiFeCy,, 
 
 Pb^eCy* 
 
 *' 
 
 
 
 15 
 
 Zn 
 
 Pb 
 
 metallic 
 
 dil. HNOs 
 
 Also Al, Cd, Co, Mg. 
 
 16 
 
 Mb. } 
 
 Pb 
 
 " 
 
 dil. HN0 3 
 
 Yel. PbO on C.C. 
 
49. SILVER, AgT- 
 
 ANALYTICAL REACTIONS. 
 
 BISECTIONS. 
 
 PPT. 
 
 COLOB. 
 
 SOL. 
 
 1. Ppt.AgCl(v. Pb, HgO 
 
 
 
 
 To AgN0 3 sol. add HC1, filter (test 
 fil.), wash res., reject fil. and 
 washings. 
 
 (l)AgCl 
 
 white 
 
 
 2. Dis. AgCl in NH 4 OH (v. Hg', Pb). 
 
 
 
 
 To (1) add NH 4 OH on filter, and 
 catch fil. in t.t. 
 
 
 
 (a) 
 (NH 3 ) 3 (AgCl) 2 
 
 3. Be-ppt. AgCl. 
 
 
 
 
 Cautiously acidify (a) with HN0 3 
 
 (2) AgCl 
 
 white 
 
 
 Supplementary. 1. Strong HC1 dis. AgCl (and HgCl somewhat) ; hence 
 avoid excess. 2. In testing for trace of Ag, evap. NH 3 before adding HN0 3 . 
 3. Never add the latter in large excess. AgCl is not re-ppd. by H Cl except in 
 cone. sols, (a) Sep. Ag from Pb. Are most salts of Ag soluble (Table A) ? 
 Can these exist together in sol: (b) AgN0 3 and HgCl 2 ? (c) AgNO 3 and CuCl 2 ? 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENT. 
 
 EEMABKS. 
 
 1 
 
 AmOH 
 
 
 brown 
 
 (AmOHx.,, 
 
 AgOH is not known. 
 
 
 
 
 
 ( HAc',H 2 S04 3> 
 
 
 2 
 
 NaOH 
 
 
 ' ' 
 
 n 
 
 
 3 
 
 Am 2 C0 3 
 
 Ag 2 C0 3 
 
 white 
 
 Am.oCOs (ex.), 
 AmOH,HN0 3 
 
 
 4 
 
 TflTflrfifO 
 
 ** 
 
 u 
 
 
 
 5 
 6 
 
 HCl 
 H 2 S 
 
 AgCl 
 Ag 2 S 
 
 black 
 
 |AmOH,KCy, 
 
 (Na^Os 
 
 boilingHNO, 
 
 HN0 3 re-ppts. Light re- 
 duces to Ag 2 Cl, violet, 
 black. 
 
 7 
 
 Am,S 
 
 " 
 
 u 
 
 
 
 
 8 
 
 KBr 
 
 AgBr 
 
 white 
 
 AmOH (si.) 
 
 
 9 
 
 El 
 
 Agl 
 
 (yellow- 
 jwhite 
 
 KI (ex.) 
 
 Insol. in AmOH. 
 
 10 
 
 K 2 Cr s O T 
 
 Ag,Cr04 
 
 (dark 
 
 (AmOH, 
 \HN0 8 
 
 HCl changes it to AgCl. 
 
 11 
 
 Am 2 0x 
 
 Ag 2 0x 
 
 white 
 
 AmOH 
 
 
 12 
 
 HNa 2 P0 4 
 
 Ag 3 P0 4 
 
 yellow 
 
 ( AmOH, 
 (HNOs 
 
 
 13 
 
 KCy 
 
 AgCy 
 
 white 
 
 KCy (ex.) 
 
 
 14 
 
 
 Ag 4 FeCVrt 
 
 {yellow- 
 
 
 Boiling gives metallic Ag. 
 
 
 
 
 
 j white 
 
 
 
 15 
 
 Zn 
 
 Ag 
 
 gray 
 
 dil. HNO< 
 
 Also Bi, Cu, Fe, Hg, Pb. 
 
 16 
 
 Na 2 C0 3 , ) 
 B.B.C.C. ) 
 
 Ag 
 
 it 
 
 HNOs 
 
 Metallic globule. 
 
50. MERCURY (ous), Hg'. 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. HgCl (v. Ag, Pb). 
 ToHgN0 3 sol. add HC1, filter (test 
 fil.), wash, reject fil. and wash- 
 ings. 
 
 (l)HgCl 
 
 white 
 
 
 2. AmOE on HgCl (v. Ag, Pb). 
 On (1) pour a little AmOH, wash 
 and reject washings. 
 
 (2)NH 2 Hg 2 Cl 
 
 black 
 
 
 3. Dis. NH 2 Hg 2 Cl in aqua regia. 
 On (2) pour a few drops aqua regia, 
 save fil. 
 
 
 
 (a) HgCl 2 
 
 4. Ee-ppt.Hgd. 
 
 Dilute (a), add SnCl 2 sol. 
 
 (3) HgCl 
 Hg 
 
 white 
 gray 
 
 
 Supplementary. 1. Hg', not Hg", must be used as HgCl 2 is sol. 3. The 
 smallest quantity of aqua regia that will dis. the ppt. must be used. 4. SnCl 2 
 sol. must be newly prepared, and with plenty of HC1, or it will oxidize to SnCU 
 and Sn 2 O C1 2 . (a) Sep. Hg' from Ag. (b) Hg / from Pb. Explain action of 
 SnCl 2 on HgCl 2 . (c) Can HgN O 3 and CuCl 2 exist in sol. together ? (d) HgN 3 
 andCdC! 2 ? 
 
 GENERAL REACTIONS. 
 
 
 RK-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 NHjHg 2 N0 3 
 
 black 
 
 HN0 3 ,aq.reg. 
 
 
 2 
 
 NaOH 
 
 Hg 2 
 
 ( brown- 
 ] black 
 
 
 
 Hg 2 O (instable) = Hg + 
 HgO. HgOH not known. 
 
 3 
 
 Am,C0 3 
 
 NH,Hg 2 N0 3 
 
 black 
 
 Acids, 
 
 
 4 
 
 NazCOs 
 
 HgzCOs 
 
 gray 
 
 
 Forms black Hg 2 on boil- 
 
 
 
 
 
 
 ing. 
 
 5 
 
 HC1 
 
 HgCl 
 
 white 
 
 HNO, 
 
 With AmOH = NH 2 Hg 2 Cl 
 
 
 
 
 
 
 (black). 
 
 6 
 
 H 2 S 
 
 Hg 8 S 
 
 black 
 
 aq.reg. 
 
 Hg 2 S (instable) - HgS+ Hg 
 
 7 
 
 Am 2 S 
 
 
 
 1 1 
 
 
 
 
 8 
 
 El 
 
 Hgl 
 
 (yellow- 
 ] green 
 
 KI (ex). 
 
 Ex. forms HgI 2 (sol.) + Hg. 
 Acids decompose it. 
 
 9 
 
 H 2 S0 4 
 
 Hg 2 S0 4 
 
 white 
 
 HNOs 
 
 In strong sol. only. 
 
 10 
 
 K 2 Cr 2 7 
 
 Hg 2 CrO* 
 
 yellow 
 
 HN0 3 
 
 
 11 
 
 AmoOx 
 
 Hg 2 0x 
 
 white 
 
 
 
 
 12 
 
 HNa 2 F0 4 
 
 HgsPO* 
 
 
 
 
 
 
 13 
 
 ZCy 
 
 HgCy 2 + Hg 
 
 gray 
 
 H 2 
 
 Hg ppd. 
 
 14 
 
 K.FeCyB 
 
 Hg4FeCy fi 
 
 white 
 
 HNOs 
 
 
 15 
 
 Zn. 
 
 Hg 
 
 gray 
 
 HNOs, aq.reg. 
 
 Also Al, Bi, Cd, Cu, Mg. 
 Sn amalgamates with M. 
 
 1 A 
 
 Na,C0 8 , ) 
 
 He- 
 
 a 
 
 
 
 Heat in tube with Na 2 C0 3 
 
 lo 
 
 B.B.C.C. ) 
 
 **& 
 
 
 
 + C, and Hg sublimes. 
 
51. GROUP I. - Pb", Ag , Hg . 
 
 ANALYTICAL REACTIONS. 
 PPT. 
 
 DIRECTIONS. 
 
 SOL. 
 
 1. Fpt. PbCl 2 , AgCl, HgCl. 
 
 Sat. sol. with HC1, filter, wash, 
 reject washings. 
 
 2. Sep. Pb from Ag.Hg. 
 
 On (1) pour boiling H 2 0. Repeat 
 till last fil. gives no ppt. with 
 K 2 Cr 2 O 7 sol. 
 
 3. Final test for Pb. 
 
 To (a) add K 2 Cr 2 O 7 sol. (or 
 K 2 Cr 2 O 4 ). 
 
 4. Sep. Ag. from Hg. 
 
 On (2) pour warm AmOH two or 
 three times. 
 
 5. Final test for Ag. 
 
 Acidify (b) with HN0 3 . 
 
 6. Dis. NH 2 Hg 2 Cl. 
 
 To (4) add very little aqua regia. 
 
 7. Final test for Hg. 
 
 To (c) add SnCl 2 sol. 
 
 (l)PbCl 2 ,AgCl,HgCl 
 
 (2) AgCl, HgCl 
 
 (3) PbCr0 4 
 
 (4) NHoHg 2 Cl 
 
 (5) AgCl 
 
 (6) HgCl, Hg 
 
 (a) PbCl 2 
 
 (b)(NH 3 ) 3 (AgCl) 
 
 (c) HgCl, 
 
 Supplementary. 1. Avoid large excess of HC1, as it may interfere with 
 the ppts. of H 2 S, Grp. II- AgCl is less sol. than HgCl, HgCl than PbCl 2 . H Cl 
 may give a ppt. outside of Group I as follows : of S, if a sulfid or thiosulfate is 
 present ; of BaCl 2 (sat. sol.) which is sol. in H 2 O but insol. in strong HC1 ; of 
 BiOCl, SbOCl, Sn 2 OCl 2 , from sols, acidified with other acids than HC1 (these 
 are sol. in excess of HC1); of As 2 S 3 , Sb 2 S 3 , SnS 2 , AgCy, XiCy 2 , H 4 Si0 4 , 
 H 3 B0 3 , Zn(OH) 2 , A1(OH) 3 , from an alk. sol. In any of the above cases if an 
 appreciable ppt. falls, insol. in H 2 or HC1, dis. and analyze separately. 
 2. PbCl 2 should all be removed by successive additions of hot H 2 (test the last 
 fil. with a drop of AgNO 3 sol.), as NH 4 OH changes it to white insol. Pb 2 OCl 2 , 
 some of which appears in the fil. H N O 3 however dis. it. It may be better to 
 boil the liquid which holds the first ppt. before filtering, then filter and test the 
 fil. for Pb. 3. What other reagent might be used here ? 4. Why is not AgN0 3 
 formed ? I have a white powder which is PbCl 2 , HgCl, or AgCl. What 
 reagent will determine which it is ? 
 
52. MERCURY (ic), Hgr'. 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. HgS(v.Pb,Bi,Cd,Cu,As,Sn,Sb). 
 
 
 
 
 Sat. sol. with H 2 S gas, filter (test 
 
 
 
 
 fil.), wash. 
 
 (1) HgS 
 
 black 
 
 
 2. HgS insol. in Am 2 S, (v. As, Sn, Sb). 
 
 
 
 
 To (1) in e.d. add Am 2 S x , stir, boil, 1 
 
 
 
 decant, wash. 
 
 (2) HgS 
 
 u 
 
 
 3. HgS insol. in dil. HN0 3 (v.Pb,Bi,Cd, 
 
 
 
 
 Cu). 
 
 
 
 
 Cover (2) with dil. HNO 3 , boil a 
 
 
 
 
 minute, decant. 
 
 (3) HgS 
 
 u 
 
 
 4. Dis. HgS in aqua regia (v. Hg'). 
 
 
 
 
 
 To (3) add little aqua regia, stir, 
 
 
 
 
 boil if necessary. 
 
 (S) 
 
 
 (a) HgCl 2 
 
 5. Ppt. HgCl and Hg with SnCl 2 (v. Hg', 
 
 
 
 
 Sn"). 
 
 
 
 
 Boil (a) to expel all Cl, add SnCl 2 
 
 
 
 
 sol. 
 
 (4) HgCl 
 
 white 
 
 
 
 Hg 
 
 gray 
 
 
 Supplementary. 1. Hg" salts often give with H 2 S a ppt. first white, then 
 yellow, red, brown, black. Double salts., e.g. HgCl 2 (HgS) 2 are first formed. 
 3. Strong HN0 3 may convert HgS into Hg(N0 8 ) 2 (HgS) 2 , white, insoluble ; 
 hence test a white res. for Hg. 4. In dis. HgS use the smallest quantity of aqua 
 regia (usually only a few drops). The sol. may afterwards be diluted. 5. SnClj 
 sol. is pearly, and must not be confounded with a Hg ppt. How detect HgN 3 in 
 a mixture with Hg(N0 3 ) 2 ? Hg(N0 3 ) 2 in presence of HgNO 3 ? Explain the 
 action of SnCl 2 on HgCl 2 . Is HgS sol. in strong H N0 3 ? Why is Hg" not put 
 into Group I ? 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 I 
 
 AmOH 
 
 NH 2 HgCl 
 
 white 
 
 AmOH, HC1 
 
 Hg(N0 3 ) 2 gives NHg 2 N0 8 . 
 
 2 
 
 NaOH 
 
 HgO 
 
 y el. -red 
 
 HN0 3 
 
 Hg(OH) 2 not known. 
 
 3 
 
 Am 2 C0 3 
 
 NH 2 HgCl 
 
 white 
 
 AmOH, HC1 
 
 
 4 
 
 NfeCOs 
 
 (HgO) 3 HgC0 3 
 
 (var.) 
 
 C red 
 j white 
 
 
 Forms HgO on boiling. 
 
 5 
 
 SnCl; 
 
 HgCl, Hg 
 
 gray 
 
 HN0 3 ,aq.reg. 
 
 
 6 
 
 H 2 S 
 
 HgS 
 
 black 
 
 aqua regia 
 
 May be first white, then 
 
 7 
 
 Am 2 S 
 
 (i 
 
 a 
 
 
 
 red, brown, black. 
 
 8 
 
 KBr 
 
 HgBr 2 
 
 white 
 
 hot H 2 
 
 
 
 
 El 
 
 HgI 2 
 
 red 
 
 1 HgCl 2 
 \ KI (ex.), HC1 
 
 
 10 
 
 K 2 Cr 2 7 
 
 HgCr0 4 
 
 orange 
 
 HNOs 
 
 
 11 
 
 Am : 0x 
 
 HgOx 
 
 white 
 
 dil. HN0 3 
 
 With HgCl 2 no ppt. forms. 
 
 12 
 
 HNazPO* 
 
 Hg3(P0 4 )j 
 
 (i 
 
 acids, Am. salts 
 
 
 13 
 
 KCy 
 
 HgCy 2 
 
 it 
 
 KCy (ex.) 
 
 
 14 
 
 K4FeCy 6 
 
 Hg 2 FeCy 6 
 
 K 
 
 
 On stand, becomes Pruss. blue. 
 
 15 
 
 Zn 
 
 Hg 
 
 gray 
 
 
 Forms amalgam with the metal 
 
 1 /> 
 
 Na 2 C0 3 \ 
 
 TT-_ 
 
 u 
 
 
 (v. Exp. 50). 
 
 16 B.B.C.C.J 
 
 Hg 
 
 
 
 
53. L.EAD, Pb". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. PbS (v. Hg", Bi, Cd, Cu, As, 
 Sn, Sb). 
 
 
 
 
 Sat. sol. with H 2 S, filter (testfil.), 
 wash. 
 
 2. PbS insol. in Am 2 S x (v. As, Sn, Sb). 
 
 (1) PbS 
 
 ( brown- 
 ( black 
 
 
 To (1) in e.d. add Am 2 S x , warm, 
 decant, wash. 
 
 (2) PbS 
 
 u 
 
 
 3. Dis. PbS in HN0 3 (v. Kg"). 
 
 
 
 
 Boil (2) with dil. HN0 3 , evap., 
 add H 2 0. 
 
 
 
 (a) Pb(N0 3 ) 2 
 
 4. Ppt. PbS0 4 (v. Bi, Cd, Cu). 
 
 
 
 
 To (a) add dil. H 2 S04+C 2 H 6 OH, 
 and shake it. 
 
 (3) PbS0 4 
 
 white 
 
 
 Supplementary. 1. Pb sometimes gives colored ppts. at first, like Hg", if 
 much HC1 is present. If there is much mineral acid, it must be diluted or 
 partly neutralized before H 2 S will give a ppt. 3. Strong HNO 3 oxidizes PbS to 
 PbSO 4 , and dil. acid does so somewhat. Some PbSO 4 dis. in HN0 3 , and some 
 may be left with HgS. Test the latter with boiling AmAc sol., filter and add 
 HAc + K 2 Cr 2 7 sol. Before adding H 2 SO 4 all HN0 3 should be expelled by 
 evaporation, (a) Sep. Hg" from Pb. Test the relative solubility in water of 
 (b) PbCl 2 , (c) PbS, (d) PbSO 4 . Can these salts exist together in a sol.: 
 (e) Pb(NO 3 ) 2 + MgS0 4 ? (f) Pb(NO 3 ) 2 + Na 2 CrO 4 ? (g) Pb(NO 3 ) 2 + NaCl ? 
 Explain. Exp. 48 gives General Reactions for Pb. 
 
54. BISMUTH, Ei'". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. Bi 2 S 3 (v. Hg, Pb, Cd, Cu, As, 
 Sb, Sn). 
 Sat. sol. with H 2 S, filter, wash. 
 
 2. Bi 2 S 3 insol. in Am 2 S x (v. As, Sn, Sb). 
 To (1) add Am 2 S x . 
 
 (1) Bi 2 S 3 
 (2) Bi 2 S 3 
 
 ( brown- 
 j black 
 
 u 
 
 
 3. Dis. Bi 2 S 3 in HN0 3 (v. Hg.). 
 To (2) add dil. HNO 3 , boil a min- 
 ute, filter. 
 
 (S) 
 
 
 (a) Bi(N0 3 ) 3 
 
 4. Bi not ppt. by H 2 S0 4 (v. Pb). 
 To (a) add few drops H 2 S0 4 . 
 
 
 
 (b) Bi(N0 3 ) 3 
 
 5. Final test for Bi (v. Cd, Cu). 
 To (b) add excess AmOH, shake, 
 let stand. 
 
 (3) Bi(OH) 3 
 
 white 
 
 
 Supplementary. 1. Diluting an acid sol. of Bi may ppt. BiOCl, BiON0 3 , 
 etc., but H 2 S changes these to Bi 2 S 8 . 5. NH 4 OH must be added in excess, 
 otherwise Bi will not ppt. here, but with Cd (v. Group II, A), (a) Pour a few 
 drops of the BiCl 3 sol. into a t.t. of H 2 O. BiCl 3 reacts with H 2 O, and forms 
 insoluble BiOCl (v. Sb). (b) Test Bi(NO 3 ) 3 sol. in the same way. BiNO 3 (OH) 2 
 (variable) is ppd. Name the ppts. Try to dis. them with acids: (c) HC1, 
 (d) HNO 3 , (e) HAc. Most salts of Bi react with H 2 O. This confirmatory test 
 may be tried in analysis. Ppt. (f) a Bi salt and (g) a Pb salt (in 2 tubes) with 
 K 2 Cr 2 O 7 sol., and test solubility of each in NaOH sol. What would this 
 
 reaction distinguish ? Now add 
 (i) Bi from Pb ; (j) Bi from Ag. 
 
 SnCl 2 sol. to each, (h) Sep. Bi from Hg"; 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Bi OH*; white 
 
 Acids 
 
 Boil, gives Bi 2 O 3 (yel.-wh.). 
 
 2 
 
 NaOH 
 
 <( 
 
 " 
 
 
 
 No. ppt. with H 2 Tr or H 3 Ci. 
 
 3 
 
 AmgCOs 
 
 Bi 2 2 C0 3 
 
 " 
 
 
 
 
 4 
 
 Na 2 CO s 
 
 ti 
 
 u 
 
 d 
 
 
 5 
 
 SnClo 
 
 BiO 
 
 black 
 
 
 With excess NaOH (T. Cl). 
 
 6 
 
 Ht8 
 
 BiA 
 
 u 
 
 HN0 3 (dil.) 
 
 Insol. in Am 2 S x . 
 
 7 
 
 Am 2 S 
 
 
 
 t( 
 
 d 
 
 u u u 
 
 
 KI 
 
 \ (BiOD 
 
 (dark 
 
 HC1 
 
 
 
 
 / Bil . 
 
 (brown 
 
 
 
 9 
 
 H 2 
 
 BiOCl 
 
 white 
 
 HC1 
 
 Others give basic salt. 
 
 10 
 11 
 
 K 2 Cr 2 7 j 
 or Z 2 Cr0 4 ) 
 
 Bi 2 0(Cr0 4 ) 2 
 
 yellow 
 
 HNO 
 
 Insol. in NaOH (v. Pb). 
 
 12 
 
 Am 2 0x 
 
 Bi 2 0xs 
 
 white 
 
 HN0 3 
 
 
 13 
 
 HN^POi 
 
 BiP0 4 
 
 " 
 
 HC1 
 
 Insol. in HNO 3 or HAc. 
 
 14 
 
 KCy 
 
 Bi(OH) 3 
 
 " 
 
 Acids 
 
 Insol. in excess KCy., 
 
 15 
 
 K 4 FeCy 
 
 BuFeCyis 
 
 ( yellow- 
 1 white 
 
 HNO 
 
 Reppts. on boiling. 
 
 16 
 
 Zn 
 
 Bi 
 
 spongy 
 
 " 
 
 Also Cu, Fe, Pb, Sn. 
 
 17 
 
 B.B.C.C. i 
 
 Bi 
 
 dark 
 
 " 
 
 Incrustation yellow. 
 
 
 i 
 
 
 
 
55. CAI>MIUM, Cd". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. CdS (v. Hg, Pb, Bi, Cu, As, Sb, 
 Sn). 
 Sat. sol. with H 2 S; filter, wash. 
 
 (1) CdS 
 
 yellow 
 
 
 2. CdS insol. in Am 2 S x (v. As, Sb, Sn). 
 To (1) add Am 2 S x in e.d.; stir. 
 
 (2) CdS 
 
 yellow 
 
 
 3. Dis. CdS in HN0 3 (v. Hg). 
 Boil (2) a minute with dil. HNO 3 . 
 Filter if necessary. 
 
 (S) 
 
 
 (a) Cd(N0 3 ) 2 
 
 4. Cd not ppd. by H 2 S0 4 (v. Pb). 
 To (a) add a drop or two dil. 
 H 2 S0 4 . 
 
 
 
 (b) Cd(N0 3 ) 2 
 
 5. Cd(OH) 2 dis. by excess AmOH (v. Bi). 
 To (b) add excess. AmOH. 
 
 
 
 (c) 
 (NH 3 ) 2 CdO(AmN0 3 )2 
 
 6. Cd not ppd. by KCy (v. Cu). 
 To (c) add little KCy sol. 
 
 
 
 (d) (KCy) 2 CdCy 2 
 
 7. Ke-ppt. CdS (v. Cu). 
 Sat. (d) with H 2 S. 
 
 (3) CdS 
 
 yellow 
 
 
 Supplementary. 1. If a large excess of acid is present the sol. must be 
 diluted before H 2 S will act. (a) Sep. Cd from Bi. (b) Sep. Cd from Hg". 
 (c) Sep. Cd from Pb. What sol. salts, if any, of Cd have the corresponding salts 
 of Cu insol. , or vice versa (v. Table A) ? (e) Devise any method of separating 
 Cd from Cu, dependent upon this, and try it. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Cd(OH) 2 
 
 white 
 
 AmOH(ex) 
 
 
 2 
 
 NaOH 
 
 it 
 
 
 
 Acids 
 
 Insol. in excess. 
 
 3 
 
 Am 2 C0 3 
 
 CdC0 3 
 
 
 
 
 
 4 
 
 NfeCOs 
 
 
 
 u 
 
 
 
 Free Am prevents, ppt. 
 
 5 
 
 H 2 S 
 
 CdS 
 
 yellow 
 
 i Hot, dil. 
 iHNOs 
 
 
 6 
 
 Am 2 S 
 
 u 
 
 n 
 
 
 
 
 7 
 
 K 2 Cr 2 OT 
 
 CdCrO* 
 
 It 
 
 HNO. 
 
 In concentrated sols. only. 
 
 8 
 
 Am 2 0x 
 
 CdOx 
 
 white 
 
 Acids (si.) 
 
 
 9 
 
 HNa^ 
 
 Cd3(P0 4 ) 2 
 
 u 
 
 Acids 
 
 
 10 
 
 KCy 
 
 CdCy 2 
 
 u 
 
 KCy (ex.) 
 
 Re-ppd. by H 2 S. 
 
 11 
 
 K^FeCyB 
 
 Cd 2 FeCy B 
 
 u 
 
 (HC1 
 1 AmOH 
 
 
 12 
 
 KaFeCyr, 
 
 Cd 3 Fe a Cy 12 
 
 yellow 
 
 i AmOH 
 IHC1 
 
 
 13 
 
 Zn 
 
 Cd 
 
 gray 
 
 
 Also Al, Mg. 
 
 14 
 
 Na.COs ) 
 B.B.C.C. \ 
 
 CdO 
 
 ( brown- 
 ! yellow 
 
 
 Incrustation, no globule. 
 
 
 
 
56. COPPER, Cu". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. CuS (v. Hg, Pb, Bi, Cd, As, Sb, 
 Sn). 
 Sat. sol. with H 2 S, filter, wash. 
 
 2. CuS insol. in Am 2 S x (v. As, Sb, Sn). 
 To (1) add Arn 2 S x ; stir. 
 
 3. Dis. CuS in HN0 3 (v. Hg). 
 To (2) add dil. HNO 3 , boil a min- 
 ute, filter if necessary. 
 
 (1) CuS 
 (2) CuS 
 
 (S) 
 
 ( brown- 
 I black 
 
 ( brown- 
 l black 
 
 (a) Cu(N0 3 ) 2 
 
 4. Cu not ppd, by H 2 S0 4 (v. Pb). 
 To (a) add a drop or two H 2 SO 4 . 
 
 
 
 (b) Cu(N0 3 ) 2 
 
 5. Cu salts sol. in excess AmOH (v. Bi). 
 To (b) add excess AmOH. 
 
 
 
 (c) 
 (NH 3 ) 2 CuO(AmN0 3 ) 2 
 
 6. Action of KCy on Cu salts (v. Cd.). 
 To (c) add KCy sol. until blue 
 color disappears. 
 
 
 
 (d) (KCy) 2 CuCy.> 
 
 7. Inaction of H 2 S on (KCy) 2 CuCyo 
 (v. Cd). 
 Pass H 2 S into (d). 
 
 
 
 (e) (KCy) 2 CuCy. 2 
 
 8. Final test for Cu. 
 To (e) add HC1. 
 
 (3) CuS 
 
 { brown- 
 ( black 
 
 
 Supplementary. 5. If the sol. does not become blue on adding NH 4 OH, 
 Cu is absent. 2. CuS dis. slightly in (NH 4 ) 2 S X . Neutralizing such a sol. with 
 HC1 gives a liver-colored ppt. (a) Sep. Cu and Pb; (b) Cu and Hg"; (c) Cu 
 and Bi. (d) Can CuCl 2 exist in sol. with Na^COa ? (e) Cu(NO 3 ) 2 and Na 2 S ? 
 (f) CuCl 2 and MgSO 4 ? 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Cu(OH) 2 
 
 blue 
 
 AmOH (ex.) 
 
 Unsat., pale-blue basic. 
 
 2 
 
 NaOH 
 
 
 
 u 
 
 
 
 Boiling gives black CuO. 
 
 3 
 
 Am 2 C0 3 
 
 Cu 2 (OH) 2 C0 3 
 
 u 
 
 Am 2 C0 3 (ex.) 
 
 it U U U 
 
 4 
 
 H 2 S 
 
 CuS 
 
 black 
 
 HNOs, KCy 
 
 
 5 
 
 Am 2 S 
 
 u 
 
 " 
 
 d 
 
 
 6 
 
 KI 
 
 CuI,I 
 
 yel.-wh. 
 
 KI(ex.) 
 
 
 7 
 
 K 2 Cr0 4 
 
 Cu 2 Cr0 4 (OH) 2 
 
 red-br. 
 
 
 
 8 
 
 Am 2 0x 
 
 CuOx 
 
 ( blue- 
 i white 
 
 j M. acids 
 
 i Am 2 0x(ex.) 
 
 
 9 
 
 HNa 2 P0 4 
 
 HCuP0 4 
 
 U ' 
 
 Acids 
 
 Cu (ex.) gives Cu 3 (PO 4 ) 2 . 
 
 10 
 
 KCy 
 
 CuCy 2 
 
 gr.-yel. 
 
 KCy (ex.) 
 
 H 2 S has no effect on KCy. 
 
 11 
 
 
 Cu 2 FeCy 6 
 
 red-br. 
 
 AmOH 
 
 Dil. sol. gives red color. 
 
 12 
 
 KBr+H 6 2 S0 4 
 
 None. 
 
 red 
 
 
 A drop or two of each. 
 
 13 
 
 Zn 
 
 Cu 
 
 " 
 
 HNOs 
 
 Also Al, Bi, Fe, Ni, Pb, Sn. 
 
 14 
 
 B.B.C.C. i 
 
 " 
 
 u 
 
 " 
 
 No incrustation. 
 
57. GROUP II, A.-Ug 9 Pb, Bi, Cd, Cu. 
 
 ANALYTICAL PEACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 SOL. 
 
 1. Ppt. HgS, PbS, Bi. 2 S;j, CdS, CuS 
 
 {v?As,~Sn, Sb). 
 Sat. sol. with H 2 S gas, filter, 
 test filtrate, wash residue 
 until washings give no 
 ppt. with a drop AgNO 3 . 
 
 2. Separate Hg from Pb, Bi, Cd, 
 
 Cu. 
 
 To (1) add little dil. HN0 3 , 
 boil a minute, decant, leave 
 residue. 
 
 3. Dis. HgS in aqua regia. 
 
 To (2) add a few drops aqua 
 regia, stir, warm if neces- 
 sary. 
 
 4. Final test for Hg (v. Hg", Sn). 
 
 Boil to expel all free Cl, add 
 SnCl 2 sol. 
 
 5. Sep. Pb from Bi, Cd, Cu. 
 
 Expel all HNO 3 from (a), add 
 little dil. H 2 S0 4 +C 2 H 5 OH, 
 shake, let stand, filter, test 
 fil. 
 
 6. Sep. Bi from Cd, Cu. 
 
 To (c) add AmOH, shake, 
 let stand, filter. 
 
 7. Sep. Cd from Cu. 
 
 To (d) add KCy sol. until 
 any blue color disappears, 
 then sat. (e) with H 2 S. 
 
 8. Final test for Cu. 
 
 Acidify (f) with HC1. 
 
 (1) HgS, PbS, 
 Bi 2 S 3 , CdS, CuS 
 
 (2) HgS (S) 
 
 (S) 
 
 (3) HgCl, Hg 
 
 (4) PbS0 4 
 
 (5) Bi(OH) 3 
 
 (6) CdS 
 
 (7) CuS 
 
 (a) 
 
 Pb(N0 3 ) 2 , Bi(N0 3 ) 3 
 Cd(N0 3 ) 2l Cu(N0 3 ) 2 
 
 (b) HgCl 2 
 
 (c) Bi(N0 3 ) 3 
 Cd(N0 3 ) 2 
 Cu(N0 3 ) 2 
 
 (d) 
 
 (NH 3 ) 2 CdO(AmN0 3 ) 2 
 (NH 3 ) 2 CuO(AmN0 3 ) 2 
 
 (e) (KCy) 2 CdCy 2 
 (KCy) 2 CuCy 2 
 
 (f) (KCy) 2 CuCy 2 
 
 Supplementary. 1. Acidulate the original sol. with HC1 (not HNO 3 , 
 which, like other oxidizing agents, decomposes H 2 S). Unless the sol. is acid, 
 Co, Ni, Zn are liable to ppt. if present. If too acid, Cd, Pb, etc., will not ppt. 
 If no ppt. falls, dil. the sol. 1. Be sure the sol. is sat. with H 2 S ; to ascertain 
 this test the fil. 2. A black res. may not be HgS, but S with enclosed particles 
 of PbS, Bi 2 S 3 , CuS. Hence confirm by SnCl 2 . 5. Test a small part of the sol. 
 for Pb at first. 6. Excess of AinO H must be used to ppt. all the Bi (which 
 otherwise may appear in the final Cd test) and to dis. Cu(OH) 2 and Cd(OH) 2 at 
 first formed. Bi may be confirmed by dis. ppt. in a few drops of HC1, evapo- 
 rating free acid and adding to H 2 0. 6. If the color is not blue on adding 
 AmO H no appreciable Cu is present. Unless previously removed Pb will ppt. 
 with AmOH. 7. The final Cd ppt. must be yellow. If not, some of the other 
 metals have failed to ppt. at the right place, and will appear here. 
 
 As, Sn, Sb Group II, B are omitted here for brevity. They are ppd. 
 by H 2 S, and may be separated from the whole of Group II by dissolving in 
 Am 2 S x (v. Exp. 61). If Group I metals were not removed by HC1, would they 
 ppt. with Group II (test each with H 2 S) ? 
 
58. ARSENIC, As'". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. As 2 S 3 (v. Group II, A; Sn, Sb). 
 Sat. sol. with H 2 S, filter (test fil.), 
 wash. 
 
 (1) As 2 S 3 
 
 yellow 
 
 
 2. As 2 S 3 insol. in HC1 (v. Sn, Sb). 
 Cover (1) with HC1, boil a min- 
 ute, filter, wash. 
 
 (2) As 2 S 3 
 
 yellow 
 
 
 3. Dis. As 2 S 3 in Am 2 S x . 
 To (2) add Am 2 S x , boil, filter if 
 necessary. 
 
 (S) 
 
 
 (a) Am 3 AsS 3 
 
 4. Re-ppt. As 2 S 3 . 
 Cautiously acidify (a) with HC1. 
 
 (3) As 2 S 3 ,(S) 
 
 yellow 
 
 
 Supplementary. The original sol. should be acidified with H Cl. (a) Try 
 a neutral sol. with H 2 S, also (b) an alkaline. H 2 S acts very slowly on As v , but 
 more rapidly when hot than when cold, ppg. As 2 S 3 + S. Test (c) an acid, (d) a 
 neutral, (e) an alkaline sol. of As salts with a sol. of a Cu salt. What 2 yellow 
 ppte. formed by H 2 S ? (f) Test the solubility of each in Am 2 S x . 
 
 GENERAL REACTIONS. 
 
 
 RB-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 
 
 
 
 fAmfVH 
 
 
 1 
 
 AgNO, 
 
 AgsAsOs 
 
 yellow 
 
 1 AJliUXl 
 
 < dil. HCl 
 LAmCl 
 
 As v (neutral) + AgNO 3 = 
 Ag 3 AsO 4 (red-brown). 
 
 2 
 
 H,S 
 
 ASaS., 
 
 ( lemon- 
 / yellow 
 
 fAm 2 CO s 
 4 Am 2 S x 
 LNaOH 
 
 Re-ppd. by HCl. 
 
 3 
 
 AmcS 
 
 
 
 d 
 
 
 
 
 4 
 
 CnS0 4 
 
 HCuAsOs 
 
 green 
 
 (AmOH 
 I ail. acids 
 
 Scheele's green (Paris green). 
 
 5 
 
 KMnO* 
 
 
 
 
 Decolorized. 
 
 
 
 f!n A /* 
 
 ( CuCXAsoOv* 
 
 u 
 
 (AmOH 
 
 Schweinfurt green. 
 
 U 
 
 vQAUl 
 
 iCuACj 
 
 
 land acids 
 
 Paris green. 
 
 7 
 
 Cu 
 
 As 
 
 gray 
 
 aq. reg, 
 
 Heated with HCl (Reinsch's 
 
 
 
 
 
 
 test). 
 
 8 
 
 H (nascent) 
 
 AsH 3 (ga) 
 
 
 
 Burns with pale-white flame. 
 
 
 
 
 
 
 Deposits As on porcelain. 
 
 
 
 
 
 
 AsH 3 very poisonous 
 
 
 
 
 
 
 (Marsh's test). 
 
 9 
 
 Na,C0 8 +KCy 
 
 As 
 
 gray 
 
 HCl 
 
 Sublimed if heated dry. 
 
 10 
 
 *C (heated) 
 
 
 
 u 
 
 
 
 Garlic odor. 
 
 11 
 
 lAmCPAmOH 
 1 +MgS0 4 
 
 AmMgAs0 4 
 
 white 
 
 
 
 For Asv only. 
 
 12 
 
 Am 3 MoO, 
 
 AmAs'MoO;, 
 
 yellow 
 
 
 
 Composition uncertain (v. 
 
 
 
 
 
 
 M 8 P0 4 ). 
 
59. TIN, Sn' . 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. SnS (v. Group II, A ; As, Sb). 
 Sat. sol. with H 2 S, filter, wash. 
 
 (1) SnS 
 
 chocolate 
 
 
 2. Dis. SnS in HC1 (v. As). 
 To (1) add HC1, boil, filter if 
 necessary. 
 
 (S) 
 
 
 (a) SnCl 2 
 
 3. Hg test for Sn. 
 To (a) add HgCl 2 sol. 
 
 (2) HgCl, 
 Hg 
 
 white 
 gray 
 
 
 Supplementary. SnCl2 sol. should be freshly prepared, and both Sn and 
 H Cl left in the sol. Otherwise SnCl 4 and Sn 2 O C1 2 are formed. Sn iv with H 2 S 
 gives yellow SnS 2 , sol. in Am 2 S x , or Am 2 CO 3 . (a) Try to dis. Sn in HN0 3 
 (strong and dil.). Try to dis. part of the res. in (b) HC1, part in (c) aqua regia. 
 What metals have no nitrates? Which of the following can exist in sol. 
 together ? (d) SnCl 2 and HgCl ; (e) SnCl 4 and HgCl ; (f) SnCl 4 and HgCl 2 . 
 (g) Change SnCl 2 to SnCl 4 ; (h) SnCl 4 to SnCl 2 . Give proof of the change in 
 both cases, (i) Sep. Sn from As. (j) Can SnCl 2 and AgN0 3 exist in sol. 
 together ? (k) SnCl 2 and PbCl 2 ? 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Sn(OH) 2 
 
 white 
 
 NaOH 
 
 Ppt. from Sn iv is SnO(OH) 2 , 
 
 
 
 
 
 
 white. 
 
 2 
 
 NaOH 
 
 " 
 
 " 
 
 ii 
 
 Boiling gives SnO. Boiling 
 
 
 
 
 
 
 NaOH+HoTr gives Sn 
 
 
 
 
 
 
 (black). 
 
 3 
 
 Am.CO 
 
 " 
 
 it 
 
 " 
 
 Insol. in excess (v. Sb"'). 
 
 4 
 
 Na ; CO 
 
 
 
 " 
 
 
 
 " ' " 
 
 5 
 
 HgCl 2 
 
 HgCl+Hg 
 
 }white, 
 
 
 If dil. HgCl, if strong Hg. 
 
 
 
 
 
 {WoATT 
 
 {Normal Am 2 S does not 
 
 6 
 
 H 2 S 
 
 SnS 
 
 brown 
 
 il d wil 
 
 HC1 
 
 dis. SnS. 
 If Sniv i s present, ppt. is 
 
 
 
 
 
 XX vl 
 
 SnS 2 (yellow). 
 
 7 
 
 El 
 
 SnI 2 
 
 yellow 
 
 HC1, NaOH 
 
 In neutral, concentr. sol. 
 
 8 
 
 Am 2 0x 
 
 SnOx 
 
 white 
 
 HC1 
 
 
 9 
 
 HN^PO, 
 
 SH3(P0 4 ) 2 
 
 " 
 
 Acids 
 
 
 10 
 
 ECy 
 
 Sn(OH) 2 
 
 " 
 
 HC1, NaOH 
 
 HCy (very poisonous) is 
 
 
 
 
 
 
 evolved. 
 
 11 
 
 E4FeCy6 
 
 Sn 2 FeCy B 
 
 ' 
 
 
 
 12 
 
 HN0 3 , Cl 
 
 
 
 
 Oxidizes Sn" to Sn iv . 
 
 13 
 
 or H,0 
 
 Sn 2 OCl- 
 
 white 
 
 HC1 
 
 SnCl 4 also formed and dis- 
 
 
 
 
 
 
 solved. Sn and HC1 add- 
 
 
 
 
 
 
 ed retard action. 
 
 14 
 
 Zn 
 
 Sn 
 
 igray, 
 I spongy 
 
 * 
 
 Also Al, Cd, Mg. 
 
 
 Na 2 COs ) 
 
 
 
 
 Use excess Na 2 C0 3 and 
 
 15 
 
 B.B.C.C. ) 
 
 
 
 
 little KCy. 
 
6O. ANTIMONY, Sb'". 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. Sb 2 S 3 (v. Group II, A-, As, Sn). 
 Sat. sol. with H 2 S, filter, wash. 
 
 2. Dis. Sb 2 S 3 in HC1 (v. As). 
 To (1) add HC1, boil, filter if 
 necessary. 
 
 3. Inaction of HgCl 2 on SbCl s (v. Sn). 
 Divide (a), to half add HgCl 2 sol. 
 
 4. Ke-ppt. Sb 2 S 3 . 
 Dilute other half (a), add H 2 S. 
 
 (1) Sb 2 S 3 
 Sb 2 S 3 
 
 orange 
 
 
 (a) SbCl:; 
 (b) SbCl 3 
 
 Supplementary. Sb 2 S 8 will not ppt. from too acid or too alkaline sols., 
 and only imperfectly from neutral. SbCl 3 is insol. in H 2 O, reacting with it to 
 form insol. SbOCl (which H 2 S changes to Sb 2 S 3 ). It should be acidulated with 
 HC1. Try to dis. Sb in HNO 3 . If not sol., test the res. (a) with HC1, (b) with 
 aqua regia. (c) Add HgCl 2 sol. to SbCl 3 sol. Explain, (d) Apply the "spot 
 test," i.e. Marsh's test (Exp. 44), to Sb. (e) Sep. Sb from Sn ; (f) Sb from As. 
 Would you be likely to find SbCl 3 in sol. with the first group metals ? With a 
 purely aqueous sol. of Group II, A ? 
 
 GENERAL REACTIONS. 
 
 
 KE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 BM, 
 
 white 
 
 (Hot NaOH (ex.), 
 I HC1 
 
 Sol. should be slight- 
 ly acid. 
 
 2 
 
 NaOH 
 
 (( 
 
 tt 
 
 
 
 " " " 
 
 3 
 
 Am 2 CO: 
 
 f( 
 
 u 
 
 
 
 (1 U U 
 
 4" 
 
 
 
 
 (HC1, 
 
 u u u 
 
 
 AftilAJa 
 
 
 
 1 hot Am 2 C0 3 
 
 
 5 
 
 H 2 
 
 SbOCl (var.) 
 
 u 
 
 Acids 
 
 Part only ppts. 
 
 
 
 
 
 fAm 2 Sx, 
 
 
 6 
 
 Hs8 
 
 Sb 2 S 3 
 
 orange 
 
 j NaOH, 
 
 
 
 
 
 
 IhotHCl 
 
 
 7 
 
 Am 2 S 
 
 u 
 
 u 
 
 i< 
 
 If too acid or too al- 
 
 
 
 
 
 
 kaline, no ppt. 
 
 8 
 
 El 
 
 no ppt. 
 
 yellow 
 
 
 Sb v ppts. I. 
 
 9 
 
 Am 2 0x 
 
 Sb(NH s ) 3 Ox 3 
 
 white 
 
 
 Ppts. slowly. 
 
 10 
 
 ECy 
 
 uncertain 
 
 " 
 
 
 
 11 
 
 EtFeCye 
 
 u 
 
 u 
 
 
 Insol. in acids. 
 
 12 
 
 Zn 
 
 Sb 
 
 black 
 
 aqua regia 
 
 Also Bi, Cu, Mg, Fe, 
 
 
 
 
 
 
 Sn. 
 
 
 
 
 
 
 rMetallic, brittle, 
 
 13 
 
 Na,CO, 1 
 B.B.C.C. i 
 
 " 
 
 " 
 
 aqua regia 
 
 1 white incrust., 
 1 green flame, white 
 I fumes (Sb 2 O 3 ). 
 
61. GROUP II, B. As, Sn, Sb. 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 SOL. 
 
 1. Ppt. As 2 S 3 , SnS, Sb.>S 3 (v. Group II, 
 
 ^)- 
 Sat. sol. with H 2 S, filter, wash. 
 
 2. Sep. Sn and Sb from As. 
 
 Warm (1) in e.d. some time with 
 HC1, decant on filter. 
 
 3. Dis. As 2 S 3 . 
 
 To (2) add Am 2 S x , boil, filter if 
 necessary. 
 
 4. Final test for As. 
 
 Cautiously acidify (b) with HC1. 
 
 5. Final test for Sn. 
 
 Divide (a), to half add HgCl 2 
 sol. 
 
 6. Final test for Sb. 
 
 Dilute other half (a), add H 2 S. 
 
 (1) As 2 S 3 , SnS, Sb 2 S 3 
 
 (2) As 2 S 3 (S) 
 
 (S) 
 
 (3) As 2 S 3 (S) 
 
 (4) HgCl, Hg. 
 
 (5) Sb. 2 S ; > 
 
 (a) SnCl 2 , SbCl 3 
 
 (b) Am 3 AsS, 
 
 Supplementary. 1. If there is very much HC1 in the sol., Sb and Sn may 
 not ppt. To determine this, dilute a little of the sol., and test with H 2 S. 
 2. The sol. should be warmed with H Cl in excess some time, not boiled, or As 
 will go into solution. As 2 S3 may be dis. by a sat. sol. of Am 2 CO 3 (made 
 without AmOH), warmed, and sep. from Sb and Sn ; then ppt. As 2 S 3 with 
 HC1 (cautiously). 3. If no appreciable res. is left in 2 except S, omit 3. 6. If 
 Sb is present, an orange ppt. will appear first, followed later (if Sn is also there) 
 by chocolate SnS. Metals of Group II, J3, are sep. from those of Group II, J., 
 by dis. the sulfids of the former in Am 2 S x (not Am 2 S). A white ppt. , on adding 
 HC1 is liable to be S. (a) Sep. SbCl 3 from CuCl 2 ; (b) SnCl 2 from BiCl 3 . 
 
62. IRON (ic), Fe'". 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. Fe(OH) 3 (v. Cr, Al). 
 
 
 
 
 To sol. add AmCl sol. , AmOH, warm, 
 
 
 
 
 filter, wash res. 
 
 (1) Fe(OH) 3 
 
 red 
 I brown 
 
 
 2. Dis. Fe(OH) 3 in HC1 (v. Cr, Al). 
 
 
 
 
 To (1) in e.d. add dil. HC1, stir. 
 
 
 
 (a) FeCl 3 
 
 3. Be-ppt. Fe(OH) 3 with NaOH (v. Cr, Al). 
 To (a) add excess NaOH sol. 
 
 (2) Fe(OH) 3 
 
 (red 
 1 brown 
 
 
 Supplementary. To reduce Fe'" to Fe" v. Exp. 47. To oxidize Fe" to 
 Fe'" v. Exp. 47. Test FeCl 3 sol. (Fe'") in t.t. with a few drops of (a) K 4 FeCy 6 , 
 (b) K 3 FeCy 6 , (c) KSCy, (d) NaOH. (e) Test also FeS0 4 sol. (Fe") with the 
 same reagents, and tabulate results. Then state what will distinguish Fe" 
 from Fe'". (f) Dis. a little Fe in dil. H 2 SO 4 , nearly evap., add H 2 O, and then 
 determine whether FeS0 4 or Fe 2 (SO 4 ) 3 is found, (g) Dis. a little Fe in aqua 
 regia, evap., dil., test as before, (h) Test also the product after dis. in HC1. 
 (i) Sep. Fe'" from Cu"; (j) Fe" from Bi'". (It is better to oxidize Fe" to Fe'" 
 before separation.) (k) Can a sol. contain both FeCl 3 and HgNO 3 ? (1) FeS0 4 
 and Cu(NO 3 ) 2 ? (m) Make FeP0 4 . Will H 2 S ppt. FeS ? Fe 2 S 3 is not formed 
 in aqueous analysis. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Fe(OH) 3 
 
 (red 
 ( brown 
 
 Acids 
 
 Variable to Fe 2 2 (OH) 2 . 
 
 2 
 
 NaOH 
 
 
 
 a 
 
 it 
 
 U .<( li 
 
 8 
 
 Am 2 C0 3 
 
 it 
 
 it 
 
 it 
 
 a u it 
 
 
 
 
 
 
 Traces Fe 2 (C0 3 ) 3 . 
 
 4 
 
 NaaCOs 
 
 K 
 
 n 
 
 
 
 Variable to Fe 2 2 (OH) 2 . 
 
 5 
 
 HNaPO* 
 
 FeP0 4 
 
 white 
 
 M. acids 
 
 Fe" x (except FeAc 3 ) ppt. 
 
 
 
 
 
 
 by this and NaAc (v. 
 
 
 
 
 
 
 M 3 P0 4 ). 
 
 6 
 
 AmaOx 
 
 Fe 2 0x 3 
 
 u 
 
 Acids 
 
 
 7 
 
 KCy 
 
 Fe(OH) 3 
 
 |red 
 I brown 
 
 d 
 
 HCy formed (very poi- 
 sonous). 
 
 8 
 
 Z4FeCy 6 
 
 Fe4Fe s Cy 18 
 
 blue 
 
 H 2 SO* 
 
 Prussian blue. NaOH + 
 
 
 
 
 
 
 ppt. = Fe(OH) 3 . 
 
 9 
 
 KsFeCye 
 
 
 
 
 No action; distinguishes 
 
 
 
 
 
 
 Fe'" from Fe". 
 
 10 
 
 KSCy 
 
 FeCy 3 S 3 
 
 ( blood- 
 ied 
 
 
 Color only, no ppt. 
 Disting. Fe'" from Fe". 
 
 11 
 
 H 2 S 
 
 S 
 
 white 
 
 
 Reduces Fe"' to Fe". 
 
 12 
 
 Am,S 
 
 FeS+S 
 
 black 
 
 Acids 
 
 First reduces Fe'" to Fe". 
 
 13 
 
 j Tannic acid 
 ( and galls. 
 
 Fe'" tannate 
 
 it 
 
 
 Basis of writing ink. 
 
 14 
 
 NaAc 
 
 Fe 2 Ac 3 (OH) 3 
 
 red 
 
 
 
 15 
 
 ( SO,, H 8 S 
 1 Zn, SnCl 2 
 
 
 
 
 Reduce Fe'" to Fe". 
 
63. IRON, Fe". 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AuiOH 
 
 Fe(OH) 2 
 
 (green 
 i black 
 
 ( AmCl (si.), 
 ( Acids 
 
 White, if pure. Oxidizes 
 to Fe(OH) 3 , red-brown. 
 
 2 
 
 NaOH 
 
 (C 
 
 a 
 
 u 
 
 u u u 
 
 3 
 
 Am 2 C0 3 
 
 FeC0 3 
 
 white 
 
 u 
 
 Oxidizes to Fe(OH) 3 . 
 
 4 
 
 NaoCO; 
 
 
 
 u 
 
 " 
 
 11 U U 
 
 5 
 
 H,S 
 
 FeS 
 
 black 
 
 u 
 
 With FeAc 2 only a slight 
 
 
 
 
 
 
 ppt. 
 
 6 
 
 Am_>S 
 
 u 
 
 u 
 
 it 
 
 Oxidizes to FeO(S0 4 ) 2 . 
 
 7 
 
 Am,0x 
 
 FeOx 
 
 yellow- 
 white 
 
 M, acids 
 
 
 
 
 
 Kino 
 
 
 
 8 
 
 HNa2P0 4 
 
 HFeP0 4 
 
 Diue- 
 white 
 
 Acids 
 
 Fe 3 (PO 4 ) 2 also formed. 
 
 9 
 
 KCy 
 
 FeCy 2 
 
 yellow- 
 red 
 
 KCy (ex.) 
 
 
 10 
 
 K4FeCy 6 
 
 K 2 Fe 2 Cy 6 
 
 blue- 
 white 
 
 
 Oxidizes in air to Prus- 
 sian blue. 
 
 11 
 
 K-FeCy, 
 
 Fe 3 Fe 2 Cyi2 
 
 blue 
 
 
 Distinguishes Fe" from 
 
 
 
 
 
 
 Fe"'. 
 
 12 
 
 KSCy 
 
 no effect 
 
 
 
 a u u 
 
 13 
 
 HN0 3 , KC10 3 
 
 
 
 
 
 14 
 
 Cl, &c. 
 
 Fe'" (no ppt.) 
 
 red 
 
 
 Oxidizes Fe" to Fe'". 
 
 15 
 
 f Tannic acid 
 i + tincture 
 I gaUs 
 
 Fe" tannate 
 
 ( white to 
 I black 
 
 
 Oxidizes to Fe'" tannate 
 (black ink). 
 
 Supplementary. In the separation of Fe" it is first oxidized to Fe'", and 
 then tested as in Group III. To ascertain whether you have a ferrous (Fe") or 
 a ferric (Fe'") salt, test the original sol. by the table below, (a) Prepare some 
 Prussian blue ; (b) Everitt's salt ; (c) Turnbull's blue ; (d) black ink. 
 
 TESTS FOR FERROUS AND FERRIC IRON. 
 
 RE-AGT. 
 
 FE". 
 
 FE"'. 
 
 K4FeCy 6 
 
 Z 2 FeFeCy 6 (bluish white). 
 Potassium ferrous-ferro-cya- 
 nid or Everitt's salt. 
 
 Fe4Fe 3 Cyi8 (deep-blue). 
 Ferric-ferro-cyanid or Prus- 
 sian blue. 
 
 ZsFeCye 
 
 Fe 3 Fe 2 Cyi 2 (dark-blue). 
 Ferrous-ferri-cyanid or Turn- 
 bull's blue. 
 
 FeFeCy 6 (green or brown color 
 only). 
 Ferric-f erri-cy anid . 
 
 KSCy 
 
 No effect. 
 
 Fe(SCy) 3 (blood-red color only). 
 Ferric-sulpho-cyanid. 
 
 KOH 
 
 Fe(OH) 2 (white to dirty green). 
 Ferrous hydroxid. 
 
 Fe(OH) 8 (red-brown). 
 Ferric hydroxid. 
 
64. ALUMINUM, Al"'. 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. A1(OH) 3 (v. Fe, Cr). 
 To sol. add AmCl sol. , AmOH, 
 boil, filter. 
 
 (1) A1(OH) 3 
 
 white 
 
 
 2. Dis. A1(OH) 3 in HC1 (v. Fe, Cr). 
 To (1) add dil. HC1, stir. 
 
 
 
 (a) A1C1 3 
 
 3. Dis. A1(OH) 3 in NaOH (v. Fe, Cr, Zn). 
 To (a) add excess, strong NaOH 
 sol., shake. 
 
 
 
 (b) Na2Al 2 4 
 
 4. A1(OH) 3 insol. in AmOH. 
 
 Acidify (b) with HC1, add 
 AmOH. 
 
 (2) A1(OH) 3 
 
 u 
 
 
 Supplementary. 3. NaO H sol. must be in excess, and strong enough to dis. 
 the A1(OH) 3 first formed, (a) Sep. Fe from Al. (b) Test action of limited 
 NaO H sol. on Al. (c) Is A1 2 S 3 formed in aqueous analysis [try H 2 S and Am 2 S ; 
 a ppt. is A1(OH) 3 ] ? (d) Test Al'" and AmCl sol. with NaOH sol. (e) Now 
 ppt. A1(OH) 3 with AmCl and NaOH, and try to dis. it in excess, (f) Sep. Cu 
 and Al ; (g) Bi and Al. (h) Obtain A1C1 3 from several cpds. of Al, in two or 
 three different ways, (i) Obtain alum crystals by mixing sols, of sulfates of Al 
 and K (Exp. 5). Try to dis. Al in (j) HC1, (k) HNO 3 . 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 
 
 
 
 
 rNaOH(ex.) forms 
 
 1 
 
 AmOH 
 
 A1(OH) 3 
 
 (gray 
 ( white 
 
 NaOH, acids 
 
 I Na2Al 2 O 4 ,notre- 
 I ppd. by boiling 
 
 
 
 
 
 
 I (v. Zn). 
 
 
 
 
 
 
 f NaOH (ex.) forms 
 
 2 
 
 NaOH 
 
 ti 
 
 u 
 
 u 
 
 ^ Na2Al 2 4 ; AmCl 
 
 
 
 
 
 
 [ re-ppts. it. 
 
 3 
 
 Am 2 C0 3 
 
 u 
 
 
 Na 2 C0 3 
 
 Liberates CO 2 . 
 
 4 
 
 Na-COs 
 
 " 
 
 
 NazCOs (ex.) 
 
 u u 
 
 5 
 
 Am,S 
 
 (( 
 
 white 
 
 Acids 
 
 H 2 S evolved. 
 
 
 
 KJeCye 
 
 uncertain 
 
 
 it 
 
 
 7 
 
 HNa,POi 
 
 A1P0 4 
 
 
 NaOH, HC1 
 
 
 8 
 
 NasStOs 
 
 A1(OH) 3 +S 
 
 
 Acids 
 
 S0 2 liberated. 
 
 
 
 
 
 
 TFirst heat : infus. 
 
 9 
 
 | B.B.C.C 7 . 
 
 I + Co(N0 3 ) 2 
 
 
 blue 
 
 
 Add a drop of 
 Co(N0 3 ) 2 sol., 
 I heat: blue. 
 
ii iff r- 
 
 |U 
 
65. CHROMIUM (ic), Cr"'. 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. Cr(OH) 3 (v. Fe, Al). 
 To sol. add AmCl sol., AmOH; 
 warm. 
 
 (1) Cr(OH) 3 
 
 green 
 
 
 2. Dis. Cr(OH) 3 in HC1 (v, Fe, Al). 
 To (1) add dil. HC1, stir, filter if 
 necessary. 
 
 
 
 (a) CrCl 3 
 
 3. Oxidize Cr'" to Cr vi . 
 
 Evap. (a) almost to dryness, then 
 add 1 or 2 crystals KC10 3 , and 
 evap. to dryness ; add H 2 O, 
 filter if necessary. 
 
 
 
 (b) K 2 Cr 2 7 
 
 4. Action of NaOH on KoCr_,0 7 . 
 To (b) add NaOH sol. 
 
 
 
 (c) K 2 Cr0 4 
 
 5. Ppt. PbCr0 4 . 
 
 Acidify (c) with HAc, add 
 Pb(N0 3 ) 2 sol. 
 
 (2) PbCr0 4 
 
 yellow 
 
 
 Supplementary. 1. Cr(OH) 3 may dis. in cold water, but re-ppts. on 
 boiling. 3. Cr"' must be oxidized to Cr, or it will ppt. with NaOH sol. 
 (a) Sep. Cr"' from AY", (b) To K 2 Cr 2 7 sol. add successive small portions of 
 AmOH, shaking each time, till the color becomes yellow. Alkalies reduce red 
 dichromates to yellow chromates; acids have the reverse effect, (c) Slowly 
 acidify the chromate with HC1. (d) Will Cr(OH) 3 ppt. from K 2 Cr 2 O 7 sol.? 
 (e) Reduce Cr vi to Cr'". (f ) Sep. Cr'" and Fe'" ; (g) Cr"' and Cd. (h) Make 
 Cr 2 (S0 4 ) 3 from K 2 Cr 2 7 . (i) Make Cr(NO 3 ) 3 . 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Cr(OH) 3 
 
 j blue- 
 \ green 
 
 ( NaOH(ex.) 
 1 Acids 
 
 Re-ppt. by hot AmCl or by 
 boiling. 
 
 2 
 
 NaOH 
 
 '* 
 
 " 
 
 NaOH (ex.) 
 
 it a n tt 
 
 3 
 
 AmoCO; 
 
 " 
 
 " 
 
 Na 2 C0 3 (ex.) 
 
 tt tt tt it 
 
 4 
 
 Na-CO;: 
 
 a 
 
 tt 
 
 u 
 
 tt it tt n 
 
 
 
 
 
 
 CO 2 formed. Slight ppt. 
 
 5 
 
 H 2 S 
 
 Cr 2 2 Cr0 4 
 
 
 
 Reduces Cr vi to Cr'" in pres- 
 
 
 
 
 
 
 ence of HC1. 
 
 6 
 
 Am 2 S 
 
 Cr(OH) 3 
 
 u 
 
 Acids 
 
 Forms slowly if dilute ; H 2 S 
 
 
 
 
 
 
 liberated. 
 
 7 
 
 HNaJ?0 4 
 
 CrP0 4 
 
 green 
 
 M. acids 
 
 
 8 
 
 H 2 S0 4 +H 2 2 
 
 undeterm. 
 
 blue 
 
 (C2Hs)aO 
 
 Blue liquid rises to surface 
 
 
 
 
 
 
 with Cr vi only. 
 
 9 
 
 KCy 
 
 Cr(OH) 3 
 
 ( blue- 
 
 NaOH 
 
 HCy liberated. 
 
 
 
 
 ( green 
 
 
 
 10 
 
 KC10 3 , Cl, &c, 
 
 
 
 
 Cr'" oxidized to Cr vi (yellow- 
 
 
 
 
 
 
 red) with heat. 
 
 11 
 
 NazCOg+KClOa 
 
 i K 2 Cr0 4 
 
 yellow 
 
 H 2 
 
 Fused on Pt foil. 
 
 12 
 
 Na2C0 3 (bead) 
 
 
 green 
 
 
 V. Table G. 
 
66. GROUP III.-Fe, Al, Cr. 
 
 SEPARATION. 
 
 DIRECTIONS. 
 
 PPT. 
 
 SOL. 
 
 1. Ppt. Fe(OH) 3 , A1(OH) 3 , Cr(OH) 3 . 
 
 
 
 To sol. add AmCl sol., AmOH, 
 
 (1) 
 
 
 boil a minute, filter, wash. 
 
 | Fe(OH) 3 , A1(OH) 3 , 
 
 
 
 ( Cr(OH) 3 
 
 
 2. Dis. Fe(OH) 3 , A1(OH) 3 , Cr(OH) 3 in 
 
 
 
 HN0 3 . 
 
 
 (a) 
 
 To (1) add dil. HNO 3 . 
 
 
 (Fe(N0 3 ) 3 ,Al(N0 3 ) 3 , 
 
 3. Oxidize Cr(N0 3 ) 3 to K 2 Cr 2 7 . 
 
 
 I Cr(N0 3 ) 3 
 
 Evap. (a) to dryness; when al- 
 
 
 
 most evap. add 1 or 2 small 
 
 
 
 crystals KC1O 3 . When evap. 
 
 
 
 dis. in H 2 O ; decant on filter 
 
 
 
 and add to res. a few drops 
 HNO 3 ; pour on same filter. 
 
 
 (Fe(N0 3 ) 3 ,Al(N0 3 ) 3 , 
 
 
 
 i KoCr 2 7 
 
 4. Sep. Fe from Al and Cr. 
 
 
 
 To (b) add excess strong NaOH 
 
 
 (e) 
 
 sol., shake, filter. 
 
 (2) Fe(OH) 3 
 
 Na. : AL0 4 , K. 2 Cr0 4 
 
 5. Sep. Al from Cr. 
 
 
 
 Acidify (c) with HC1, add AmOH, 
 
 
 
 filter. 
 
 (3) A1(OH) 3 
 
 (d) K 2 Cr0 4 
 
 6. Final test for Cr. 
 
 
 
 Partly evap. (d), dil., acidify with 
 
 
 
 HAc, add Pb(N0 3 ) 2 sol. 
 
 (4) PbCr0 4 
 
 
 Supplementary. 1. AmCl prevents ppn. by AmOH of Mg, Mn, Zn, Co, Ni 
 (Fe" partially), aids ppn. of Al, and does not affect Fe"' and Cr. Considerable 
 AmCl is needed. AmO H at first ppts. Co, Ni, Zn, if present, all of which are 
 sol. in excess. If only one of these Fe'", Al, Cr, is present, the color determines 
 which. Cr(OH) 3 dis. in cold H 2 0, but is re-ppd. on boiling. Fe" should be 
 oxidized to Fe'" by boiling with a few drops of HN0 3 . H 2 S must all be 
 removed by boiling before adding AmO H, to prevent formation of Am 2 S and 
 ppn. of Co, Ni, Mn, Zn. Cr"" is reduced by H 2 S to Cr'", and hence ppd. here. 
 3. Cr"' must all be oxidized to Cr or it will ppt. with Fe. 4. Fe should be 
 tested in the original sol. for Fe" or Fe'" by K 4 FeCy 6 , K 3 FeCy 6 , KSCy. 
 6. NaO H dis. some SiO 2 from the containing bottles, and there may be a ppt. 
 of H 4 Si0 4 , similar to A1(OH) 3 , small in quantity and sinking sooner than 
 A1(OH) 3 . 6. A white ppt. of PbCl 2 will always appear if no Cr is present. 
 The yellow color alone indicates Cr. 
 
67. COBALT, Co". 
 
 ANALYTICAL REACTIONS. 
 
 BISECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. CoS (v. Ni, Mn, Zn). 
 To sol. add AmCl sol., Am 2 S, 
 shake, warm, filter, wash res. 
 with hot H 2 O, adding to it a 
 few drops Ani2S. 
 
 (1) COS 
 
 black 
 
 
 2. CoS insol. in HC1 (v. Mn, Zn). 
 To (1) add dil. HC1, stir, decant. 
 
 (2) CoS 
 
 
 
 
 3. Dis. CoS in aqua regia (v. Ni). 
 To (2) add a few drops of aqua 
 reg., stir, filter, evap. acid, dil. 
 
 (S) 
 
 
 (a) CoCl 2 
 
 4. Ppt. K 6 Co 2 0(N0 2 )i . 
 
 To (a) add HAc, KN0 2 sol. 
 
 (3) 
 
 K 6 Co. 2 0(N0 2 ) 10 
 
 yellow 
 
 
 Supplementary. 1. Am 2 S (colorless) must be used, not Am 2 S x (yellow). 
 2. CoS is sol. in strong, hot H Cl, and slightly in cold, as is NiS. 3. K 6 CoO(N 2 )io 
 is broken up by alkalies, or HC1, but not by HC 2 H 3 O 2 . 1. CoS and NiS are 
 liable to oxidize to the soluble sulfates if exposed long to the air, hence they 
 must be filtered and washed at once. 4. Some ppt. may occur at once in 4, but 
 to be sure all the Co is thrown down 24 hours is needed, and enough KNO 2 
 must be used. What sulfid in Group II was sol. in aqua regia only ? Why is 
 not CoS ppd. by H 2 S with Group II ? (a) To Co salts add H 2 S, then AmO H. 
 How is Am 2 S made ? (b) Make a borax bead by fusing with the blow-pipe a 
 little Na 2 B 4 O 7 in the loop of a Pt. wire until it becomes clear. Dip this bead 
 into a very weak sol. of CoCl 2 and fuse again. The blue color if the sol. was 
 not too strong is very characteristic of Co. (c) Can AgN O 3 and CoCl 2 exist 
 in sol. together ? Sep. (d) Co and Cd; (e) Co and Cr. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Co(OH) 2 
 
 red 
 
 J AmOH (ex.), 
 ' AmCl, &c. 
 
 f Blue bas. ppt. first formed. 
 4 On stand, forms Co(OH),. 
 i. Oxidizes to Co(OH) 3 . 
 
 2 
 
 NaOH 
 
 u 
 
 u 
 
 " 
 
 Insol. in NaOH (ex.). 
 
 3 
 
 Am 2 CO s 
 
 Co 2 OC0 3 
 
 it 
 
 Am 2 C0 3 (ex.) 
 
 Violet or blue by heating. 
 
 4 
 
 Na 2 C0 3 
 
 " 
 
 " 
 
 
 Insol. in excess Na 2 CO 3 . 
 
 6 
 
 Am 2 S 
 
 CoS 
 
 black 
 
 HN0 3 ,aq,reg. 
 
 Oxid. to CoSO 4 , which is sol. 
 
 6 
 
 KN0 2 
 
 KeCojO(N0 2 >io 
 
 yellow 
 
 HC1 
 
 Ppts. only in pres. of HAc. 
 
 7 
 
 KCy 
 
 CoCy 2 
 
 br.-wh. 
 
 KCy (ex.) 
 
 Dist. from Ni by hot HC1. 
 
 8 
 
 EUFeCye 
 
 Co 2 FeCy 6 
 
 
 
 Grayish green. 
 
 9 
 
 KaFeCye 
 
 CosTe.Cy. 
 
 J brown 
 (red 
 
 
 fin absence of Mn", or Ni, 
 4 AmCl+AmOH+K 3 FeCy 6 
 (^ + Co" = blood-red color . 
 
 10 
 
 HNa2P04 
 
 HCoPO ; 
 
 red 
 
 AmOH, acids 
 
 
 11 
 
 Heat (on paper) 
 
 
 blue 
 
 
 Dehydrated. 
 
 12 
 
 Na2B 4 7 (bead) 
 
 
 
 
 
 Blue bead in either flame. 
 
 13 
 
 Cl,Pb0 2 (warm) 
 
 
 white 
 
 
 Oxidizes Co" to Co'". 
 
 14 
 
 Zn 
 
 Co 
 
 a 
 
 HC1 
 
 Also Cd, Mg. 
 
 15 
 
 B.B.C.C. i 
 
 " 
 
 
 u 
 
 Magnetic. 
 
68. NICKEL,, Ni". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. NiS (v. Co, Mn, Zn). 
 To sol. add AmCl, Am 2 S, warm, 
 filter rapidly, wash res. with 
 hot H 2 O and a few drops of 
 Am 2 S. 
 
 (1) NiS 
 
 black 
 
 
 2. NiS insol. in HC1 (v. Mn, Zn). 
 To (1) add little dil. HC1, stir 
 and decant. 
 
 (2) NiS 
 
 a 
 
 
 3. Dis. NiS in aqua regia (v. Co). 
 To (2) add at once a few drops of 
 aqua regia, stir, filter, evap. 
 acid, and dilute. 
 
 (S) 
 
 
 (a) NiCLj 
 
 4. Inaction of KN0 2 on NiCl and HAc. 
 To (a) add little HAc, KNO 2 sol. ; 
 leave 24 hours. 
 
 
 
 (b) NiCl 2 
 
 5. Ppt. Ni(OH) 2 . 
 To (b) add excess strong NaOH 
 sol. ; boil if necessary. 
 
 (3) Ni(OH) 2 
 
 ( apple- 
 | green 
 
 
 Supplementary. 1. Ni has not been wholly removed if the fil. is brown or 
 has black particles in it. In that case acidify the fil. with HAc, boil, filter, and 
 test for Ni. 3. In using aqua regia the smallest quantity (usually a few drops) 
 that will suffice to dis. the substance must be employed. The sol. may after- 
 wards be diluted. Note the color of Ni salts. Sep. (a) Ni and Co ; (b) Ni and 
 Fe ; (c) Ni and Cu ; (d) Ni, Cu, Al ; (e) Ni, Bi, Sb. (f) Test Ni with borax 
 bead (v. Co and Table G). 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 Ni(OH) 2 
 
 pale green 
 
 i AmOH, 
 ' AmCl, &c. 
 
 Sol. NaOH re-ppts. slowly 
 (violet-blue). 
 
 2 
 
 NaOH 
 
 It 
 
 u 
 
 
 
 Insol. in NaOH (ex.). Un- 
 
 
 
 
 
 
 changed in air. 
 
 3 
 
 Am,CO 
 
 
 green 
 
 Am 2 CO s (ex.) 
 
 Sol. has blue-green color. 
 
 4 
 
 NajjCOs 
 
 ** 
 
 ' ' 
 
 Xi ftjvOs \^) 
 
 
 5 
 
 H 2 S 
 
 NiS 
 
 black 
 
 HN0 3 , aq. reg. 
 
 From neutral or alk. sol., 
 
 
 
 
 
 
 not acid. 
 
 6 
 
 AnijS 
 
 u 
 
 " 
 
 u 
 
 Sol. (si.) in Am 2 S (ex.). 
 
 7 
 
 KiFeCye 
 
 NiaFeCyc 
 
 green-white 
 
 AmOH 
 
 
 8 
 
 KsFeCye 
 
 Ni3Fe 2 Cyi 2 
 
 green-yel. 
 
 
 AmCl+AmOH+K 3 FeCy 6 + 
 Ni", boiled = red ppt. 
 
 9 
 
 HNa.PO, 
 
 Ni3(P0 4 ) 2 
 
 green-white 
 
 
 
 10 
 
 ZCy 
 
 NiCy 2 
 
 y el. -green 
 
 KCy (ex.) 
 
 Dist. from Co by HC1. 
 
 11 
 
 M,0x 
 
 NiOx 
 
 green 
 
 
 Leave 24 hours. 
 
 12 
 
 Na2B 4 7 (bead) 
 
 
 
 
 (V. Table G.) Co" obscures 
 
 
 
 
 
 
 test. 
 
 13 
 
 Cl, Br, &c. 
 
 
 
 
 Oxidizes Ni" to Ni'". 
 
 14 
 
 H 2 S, SO,, &c. 
 
 
 
 
 Reduces Ni 1 " to Ni". 
 
 15 
 
 Zn 
 
 Ni 
 
 white 
 
 
 Also Cd, Sn. 
 
 10 
 
 B.B.C.C. f 
 
 
 
 " 
 
 HNO 
 
 Magnetic powder. 
 
69. MANGANESE (ous), Mn". 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. MnS (v. Co, Ni, Zn). 
 To sol. add AmCl sol., Am 2 S, 
 warm, filter, wash in hot H 2 O 
 and Am 2 S. 
 
 (1) MnS 
 
 salmon 
 
 
 2. Dis. MnS in HC1 (v. Co, Ni). 
 To (1) add dil. HC1, stir, filter, 
 boil to expel all H 2 S, NH 3 , &c. 
 (test a little with PbAc 2 ). 
 
 (S) 
 
 
 (a) MnCL 
 
 3. Ppt. Mn(OH) 2 (v. Zn). 
 To (a) add excess strong NaOH 
 sol., warm. 
 
 (2) Mn(OH) 2 
 Mn 2 2 (OH) 2 
 
 white 
 brown 
 
 
 Supplementary. 3. Mn(OH) 2 will not ppt. with NaOH if AmCl and 
 AmO H are present. Mn(O H) 2 when pure is white, but it rapidly oxidizes to 
 brown Mn 2 O 2 (OH) 2 (variable). This should further be tested by fusing it with 
 a mixture of Na 2 CO 3 and KNO 3 , when bright green K 2 Mn0 4 and Na 2 Mn0 4 are 
 formed, (a) See whether Mn(OH) 2 or MnS forms in preference to the other. 
 Will these exist together hi sol. : (b) MnCl 2 + ZnS 4 ? (c) MnS O 4 + Cu(N 3 ) 2 ? 
 (d) MnCl 2 + K 2 Cr0 4 ? Sep. (e) Mn and Ni ; (f ) Mn and As ; (g) Mn, Cu, Cr ; 
 (h) Pb, Sr, Mn. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AmOH 
 
 w _ SVTT 
 
 Mn(OH) 2 
 
 white 
 
 AmCl, &c. 
 
 Quickly oxidizes to brown 
 Mn 2 O 2 (OH) 2 ; insoluble in 
 AmCl. 
 
 2 
 3 
 
 NaOH 
 Am,C0 3 
 
 MnCOs 
 
 u 
 
 u 
 
 U It U u 
 
 4 
 
 NazCOs 
 
 it 
 
 a 
 
 41 
 
 u . u u u 
 
 5 
 
 H 2 S 
 
 MnS 
 
 pink 
 
 HC1, HAc 
 
 MnS ppts. from MnAc 2 (un- 
 less HAc is present). Not 
 
 
 
 
 
 
 otherwise. 
 
 6 
 
 Am 2 S 
 
 (t 
 
 (t 
 
 
 
 
 7 
 
 ZiFeCye 
 
 Mn 2 FeCy 6 
 
 white 
 
 HC1 
 
 
 8 
 
 ZaFeCye 
 
 Mn3Fe 2 Cyi 2 
 
 brown 
 
 
 Insol. in acids. 
 
 9 
 
 HNaaPO* 
 
 Mns(P04) 2 
 
 white 
 
 Dil. acids 
 
 From AnuMnCL. etc. , forms 
 AmMnP0 4 . 
 
 10 
 
 KCy 
 
 MnCy 2 
 
 u 
 
 ZCy (ex.) 
 
 Darkens in air. 
 
 11 
 
 M 2 0x 
 
 MnOx 
 
 " 
 
 Acids 
 
 
 12 
 13 
 
 Na2B 4 7 (bead) 
 NaaCOs+KNO,, 1 
 ignited on Pt [ 
 foil 
 
 Z 2 Mn0 4 | 
 
 Na 2 MnO, ) 
 
 amethyst 
 green 
 
 
 In o. f . In r. f . colorless 
 (v. Table G). 
 ( NajjCOg bead (o. f .), same 
 { green color. 
 
 14 
 
 Cl, Br, &c. 
 
 
 
 
 Oxidizes to Mn'". 
 
 15 
 
 (H,S), S0 2 , &c. 
 
 
 
 
 Reduces Mn" to Mn", ppts. 
 S. 
 
 16 
 
 Zn 
 
 
 
 
 Reduces Mn'" to Mn" when 
 
 
 
 
 
 
 rightly acidulated. 
 
 17 
 
 HN0 8 +Pb0 2 (boil) 
 
 HMn0 4 (sol.) 
 
 red 
 
 
 Seen on settling of sediment. 
 
7O. ZINC, Zn". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. ZnS (v. Co, Ni, Mn). 
 To sol. add AmCl, Am 2 S, warm, 
 filter, wash with hot H 2 O and 
 a few drops of Am 2 S. 
 
 (1) ZnS 
 
 white 
 
 
 2. Dis. ZnS in HC1 (v. Co, Ni). 
 To (1) add dil. HC1, stir, filter. 
 
 (S) 
 
 
 (a) ZnClo 
 
 3. Zn(OH) 2 sol. in excess NaOH (v. Mn). 
 To (a) add excess strong NaOH 
 sol. 
 
 
 
 (b) NaoZnO., 
 
 4. Ee-ppt. ZnS. 
 Acidify (b) with HAc, add Am 2 S. 
 
 (2) ZnS 
 
 u 
 
 
 Supplementary. I. ZnS is the only white sulfid, but it must not be con- 
 founded with a white ppt. of S. 3. Zn(OH) 2 is not sol. in dil. sol. of NaOH, 
 especially if boiled. 4. ZnS is ppd. by H 2 S if the sol. is acidified with HAc. 
 Zn ppts. these metals from sols, of their salts : Pb, Ag, Hg, Bi, Cd, Cu, As, Sn, 
 Sb, Co, Ni, Fe. State color of each sulfid in Groups II and IV (tabulate). 
 What hydroxids are sol. in excess of NaO H ? Sep. (a) Zn and Al ; (b) Zn and 
 Co ; (c) Zn and Mn ; (d) Pb, Fe, Zn. 
 
 GENERAL REACTIONS. 
 
 
 RK-AQT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 I 
 
 AmOH 
 
 ZnOH 
 
 jgel. 
 1 white 
 
 AmOH (ex.) 
 
 Forms Am 2 ZnO 2 . Boil- 
 ing re-ppts. 
 
 2 
 
 NaOH 
 
 u 
 
 u 
 
 NaOH (ex.) 
 
 All Zn salts are sol. in 
 
 
 
 
 
 
 NaOH, except ZnS. 
 
 3 
 
 Am 2 C0 3 
 
 Zn5(OH) 6 (C0 8 )2 
 
 (( 
 
 AmOH 
 
 V 
 
 4 
 
 N^COs 
 
 tt 
 
 11 
 
 u 
 
 
 5 
 
 H 2 S 
 
 ZnS 
 
 white 
 
 
 From neutral sol. only, 
 
 
 
 
 
 
 and in part only. 
 
 6 
 
 Am-jS 
 
 K 
 
 
 
 HC1 
 
 Insol. in HAc (v. Mn"). 
 
 7 
 
 K4FeCy fi 
 
 Zn 2 FeCy 6 
 
 u 
 
 
 
 8 
 
 KaFeCye 
 
 Zn3Fe 2 Cyi 2 
 
 yellow 
 
 
 
 9 
 
 KCy 
 
 ZnCy 2 
 
 white 
 
 KCy (ex.) 
 
 
 10 
 
 NaAfcOxMid) 
 
 
 
 
 Hot, yellow ; cold, white. 
 
 
 
 
 
 
 {As incrustation. On cool- 
 
 11 
 
 Na,CO.. / 
 B.B.C.C. \ 
 
 ZnO, Zn 
 
 yellow 
 
 
 ing becomes white. 
 Co(NO 3 ) 2 makes green 
 
 
 
 
 
 
 color on heating again. 
 
71. GROUP IV. Co, Ni, Mn, Zn. 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 SOL. 
 
 1. Fpt. CoS, NiS, HnS, ZnS. 
 
 
 
 To sol. add AmCl, Am 2 S, shake, 
 warm (not boil), filter rapidly. 
 Pour on res. a few drops Am 2 S, 
 then wash with hot H 2 O. 
 
 (1) CoS, NiS, 
 MnS, ZnS 
 
 
 2. Sep. Co, Ni from Mn, Zn. 
 
 
 
 To (1) in e.d. add dil. HC1, stir 
 well, filter and wash. 
 
 (2) CoS, NiS 
 
 (a) MnCl 2 , ZnCl 2 
 
 3. Dis. CoS and NiS. 
 
 
 
 To (2) add at once very little aqua 
 regia. Evap. acid, dil. , add HAc. 
 
 (S) 
 
 (b) CoCl 2 , NiCl 2 
 
 4. Sep. Co from Ni. 
 
 
 
 To (b) add excess strong KN0 2 sol., 
 leave 24 hours, filter. 
 
 (3)KeCo 2 0(N0 2 ) 10 
 
 (c) NiCl 2 
 
 5. Final test for Ni. 
 
 
 
 To (c) add excess strong NaOH sol., 
 boil. 
 
 (4) Ni(OH) 2 
 
 
 6. To separate Mn from Zn. 
 
 
 
 Partly evap. (a) to concentrate the 
 sol. and expel all NH 3 , acidify 
 with HAc, add excess strong 
 NaOH sol., shake, let stand, 
 filter. 
 
 (5) Mn(OH) 2 , 
 Mn 2 2 (OH) 2 
 
 (d) Na 2 Zn0 2 
 
 7. Final test for Zn. 
 
 
 
 Acidify (d) with HAc, add Am 2 S. 
 
 (6) ZnS 
 
 
 Supplementary. 1. Am 2 S (colorless), not Am 2 S x (yellow), must be used. 
 CoS, NiS, etc. , oxidize to sulfates in air. Hence filter rapidly with H 2 having 
 a few drops of Am 2 S. Group II metals, if not all removed, may ppt. here. 
 2. CoS, NiS are dis. by strong hot HC1, and slightly by cold. 6. ZnS, MnS will 
 ppt. on adding XaO H if any H 2 S is present. Mn will not ppt. with NaO H if 
 AmCl and AmOH are present. Zn(OH) 2 is sol. in excess of strong cold NaOH 
 sol. only. Mn should be tested for by. fusing with Na 2 C 3 and K N O 3 . (a) What 
 members of Group III will Am 2 S ppt. ? (b) of Group II ? (c) Group I ? 
 
72. BARIUM, Ba". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Inaction of AraCl. AmOH on Ba salts 
 
 (v. Mg). 
 To sol. add AmCl sol. , AmOH. 
 
 
 
 (a) BaCl 2 
 
 2. Ppt. BaC0 3 (v. Sr, Ca, Mg). 
 To (a) add Am 2 CO 3 sol., warm, filter, 
 wash. 
 
 (1) BaCOg 
 
 white 
 
 
 3. Dis, BaC0 3 in HAc (v. Sr, Ca). 
 To (1) add little HAc. 
 
 
 
 (b) BaAca 
 
 4. Action o! K 2 Cr 2 7 on BaAc 2 (v. Sr, Ca). 
 To (b) add K 2 Cr 2 O 7 sol. 
 
 (2) BaCr0 4 
 
 yellow 
 
 
 Supplementary. Has AmO H any effect on sol. salts of Ba ? (a) Sep. Ba 
 and Mn ; (b) Ba and Fe'" ; (c) Ba and Bi ; (d) Ba and Hg"; (e) Ba and Hg 7 . 
 (f) What numbers of Group IV will Am 2 C O 3 ppt. ? (g) Group III ? (h) Group II ? 
 (i) Group I ? What Ba salt is insol. in HC1 (v. Exp. 100)? For what test i& 
 Ba(OH) 2 used? BaCO 8 occurs free in nature. How can other Ba salts be 
 made from it ? (g) Make several, (h) Test the Ba flame by dipping a Pt. wire 
 (or a splinter) into BaCl 2 and holding it in the edge of a Bunsen flame. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 I 
 
 NaOH 
 
 Ba(OH) 2 
 
 white 
 
 20 H,0, Acids 
 
 Must be very cone. sol. 
 
 2 
 
 Am 2 CO- 
 
 BaCOs 
 
 u 
 
 Acids 
 
 Slightly sol. in AmCl, aided by 
 
 
 XTrt OA 
 
 
 
 
 AmOH and heat. 
 
 4 
 
 .Ma^lsUs 
 
 HNa^O* 
 
 HBaP0 4 
 
 u 
 
 u 
 
 Also AmCl (si.). Must be neu- 
 
 
 
 
 
 
 tral or alkaline. 
 
 5 
 
 M 2 S0 4 
 
 BaS0 4 
 
 It 
 
 350,000 H.O 
 
 One of the most insol. of salts. 
 
 6 
 
 Z 2 Cr0 4 
 
 BaCrO 
 
 yellow 
 
 j HAc (si.), 
 ( HC1 (warm) 
 
 Re-ppd. by AmOH. 
 
 7 
 
 K 2 Cr 2 7 
 
 (t 
 
 u 
 
 
 
 U it 11 
 
 8 
 
 H 2 SiF, 
 
 BaSiF e 
 
 white 
 
 HC1, HN0 3 
 
 C 2 H 2 OH aids ppn., also stir- 
 
 
 
 
 
 
 ring, standing and boiling. 
 
 
 
 
 
 
 Sr not ppd. by H 2 SiF 6 . 
 
 9 
 
 AmjOx 
 
 BaOx 
 
 white 
 
 Acids 
 
 From cone. sols. 
 
 10 
 
 Flame test 
 
 
 jyellow- 
 1 green 
 
 
 Vis. through indigo sol.; blue- 
 green through green glass. 
 
73. STRONTIUM, Sr". 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COL. 
 
 SOL. 
 
 1. Inaction of AmCl and AmOH on Sr salts 
 (v. Mg). 
 To sol. add AmCl sol. , AmOH. 
 
 
 
 (a) SrCla 
 
 2. Ppt. SrC0 3 (v. Mg, Ba, Ca). 
 To sol. add Am 2 C03 sol. , warm, filter, 
 wash. 
 
 (1) SrC0 3 
 
 white 
 
 
 3. Dis. SrC0 3 in HAc (v. Ba, Ca). 
 Pour on (1) a little HAc. 
 
 
 
 (b) SrAc 2 
 
 4. Inaction of K 2 Cr 2 7 on SrAc 2 (v. Ba). 
 To (b) add little K 2 Cr 2 O 7 sol. 
 
 
 
 (c) SrAc2 
 
 5. Ppt. SrS0 4 with Am 2 S0 4 . 
 
 To (c) add Am 2 SO 4 sol., shake well, 
 let stand, filter, test filtrate. 
 
 (2) SrS0 4 
 
 
 
 
 Supplementary. (a) Test the Sr flame by dipping a Pt. wire (or a splinter) 
 into a Sr salt, and holding it in the edge of a Bunsen flame. Sep. : (b) Sr and 
 Ba; (c) Group IV and Sr; (d) Group III and Sr; (e) Group II and Sr; 
 (f) Group I and Sr. (g) If HC1 were used instead of HAc (in 3), would the 
 subsequent reaction take place just as well ? (h) See whether you can ascertain 
 which is more insol., SrS0 4 or BaS0 4 . 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 
 
 
 
 fApirlo 
 
 
 1 
 
 NaOH 
 
 Sr(OH) 2 
 
 white 
 
 60H 2 
 
 From cone. sol. 
 
 2 
 
 AniiCO: 
 
 SrCOs 
 
 " 
 
 Acids 
 
 From neutral or alkaline sol. 
 
 3 
 
 Na 2 CO;, 
 
 
 ' ' 
 
 ' ' 
 
 
 4 
 
 HNa 2 P0 4 
 
 HSrP0 4 
 
 " 
 
 M. acids 
 
 Partly sol. in AmCl. 
 
 6 
 
 M 2 S0 4 
 
 SrS0 4 
 
 " 
 
 ( 500HC1, 
 i 7000H 2 
 
 Let it stand some time. 
 
 6 
 
 Am 2 0z 
 
 SrOx 
 
 U 
 
 ( HC1, HN0 3 , 
 (AmCl 
 
 Slightly sol. in HAc. 
 
 7 
 
 K 2 Cr0 4 
 
 SrCr0 4 
 
 yellow 
 
 Acids 
 
 From cone. sol. 
 
 8 
 
 Flame test 
 
 
 crimson 
 
 
 Best with SrCl 2 . 
 
74. CALCIUM, Ca". 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COL. 
 
 SOL. 
 
 1. Inaction of AmCl and AmOH on Ca salts 
 
 
 
 
 (v. Mg). 
 
 
 
 
 To sol. add AmCl sol., AmOH. 
 
 
 
 (a) CaCL 
 
 2. Ppt. CaC0 3 (v. Mg). 
 
 
 
 
 To (a) add Am 2 C0 3 sol., warm, filter, 
 wash. 
 
 (1) CaC0 3 
 
 white 
 
 
 3. Dis. CaC0 3 in HAc (v. Ba, Sr). 
 
 
 
 
 Pour on (1) a little HAc. 
 
 
 
 (b) CaAc 2 
 
 4. Inaction of K 2 Cr 2 7 on CaAc 2 (v. Ba, Sr). 
 
 
 
 
 To (b) add K 2 Cr 2 7 sol. 
 
 
 
 (c) CaAca 
 
 5. Action of Am 2 S0 4 on CaAcjj (v. Sr). 
 
 
 
 
 To (c) add a little Am 2 S0 4 sol., very 
 dil. 
 
 
 
 (d) CaAc-j 
 
 6. Ppt. Ca with Am 2 0x. 
 
 
 
 
 To (d) add AmOH and Am 2 0x sol. 
 
 (2) CaOx 
 
 u 
 
 
 Supplementary. Sep. (a) Ca and Ba; (b) Ca and Sf; (c) Ca and Pb; 
 (d) Ca, Al, and Bi. CaCO 3 is the most abundant source of Ca salts, (e) Make 
 several Ca salts from it. (f) Test CaCl 2 with a strong sol. of Am 2 S0 4 , and 
 compare with SrCl 2 . This will show why very dil. Am 2 S0 4 must be used to sep. 
 Sr and Ca. (g) Test the Ca flame, as in the case of Sr, and compare the two. 
 (h) See whether CaSO 4 or SrSO 4 is more sol.; (i) BaSO 4 or CaS0 4 . 
 
 GENERAL REACTIONS. 
 
 
 RB-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 2 
 
 NaOH 
 Am,C0 3 
 
 Ca(OH) 2 
 CaCOs 
 
 white 
 u 
 
 ( 700H 2 0, 
 1 AmOH 
 Acids 
 
 Solubility decreased by heat. 
 Cone. sol. only. 
 Slightly sol. with AmCl. Neutral 
 or alkaline sol. 
 
 4 
 
 NasCOs 
 
 HNa.PO* 
 
 HCaFOi 
 
 u 
 
 u 
 
 
 5 
 
 MiSC-4 
 
 CaSO 
 
 (i 
 
 fH 2 0(sl.), 
 \ Acids (si.), 
 I Am 2 80 4 
 
 With dil. sol. use C 2 H 5 OH. 
 
 6 
 
 Am 2 0x 
 
 CaOx 
 
 II 
 
 M. acids 
 
 Insol. in HAc, H 2 0x. AmOH 
 aids ppn. 
 
75. MAGNESIUM, Mg ". 
 
 ANALYTICAL REACTIONS. 
 
 BISECTIONS. 
 
 PPT. 
 
 COL. 
 
 SOL. 
 
 1. Prevent ppn. of Mg(OH) 2 and 
 MgC0 3 (v. Ba, Sr, Ca). 
 To sol. add AmCl sol., 
 AmOH. 
 
 
 
 (a) (AmCl) 2 MgCl 2 
 
 2. Inaction of Am 2 C0 3 on 
 (AmCl) 2 MgCl 2 (v. Ba, Sr, Ca). 
 To (a) add Am 2 C0 3 sol. 
 
 
 
 (b) <AmCl) 2 MgCl 2 
 
 3. Ppt. AmMgP0 4 . 
 To (b) add HNa2P0 4 . 
 
 (1) AmMgP0 4 
 
 white 
 
 
 Supplementary. Unless enough AmCl sol. is present, AmO H ppts. half of 
 the Mg as Mg(0 H) 2 . AmMgPO 4 will not readily ppt. unless AmO H is present. 
 
 (a) Verify the above statements. To ppt. AmMgP0 4 from very dil. sols., warm 
 gently, stir with a glass rod, and let the sol. stand in a warm place some hours. 
 
 (b) Verify with dil. sol. (c) Test action of Am 2 C O 3 sol. on MgCl 2 sol. Does 
 any previous group re-agent ppt. Mg ? If so, how may ppn. be prevented ? 
 (d) Sep. Mg and Al ; (e) Mg and Fe'"; (f) Mg and Ba ; (g) Mg and Cu. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 BEMARKS. 
 
 1 
 
 AmOH 
 
 Mg(OH) 2 
 
 white 
 
 \ AmCl, 
 1 600H,0 
 
 Only half is ppd. , rest is 
 sol. as Am 2 Mg(S0 4 ) 2 - 
 
 
 
 
 
 ( Acids, 
 
 
 2 
 
 NaOH 
 
 (t 
 
 u 
 
 UmCl 
 
 
 3 
 
 NasCOs 
 
 Mg4(C0 3 )3(OH) 2 
 
 u 
 
 AmCl 
 
 Var.toMg 5 (C0 3 ) 4 (OH) 2 . 
 
 
 
 
 
 
 C0 2 liberated. 
 
 4 
 
 Am 2 CO: 
 
 Am,MglCO:-:, 
 
 u 
 
 Dil, HC1 
 
 Variable with strength 
 
 
 
 
 
 
 of sol. 
 
 5 
 
 HNa 2 P0 4 
 
 HMgF0 4 
 
 u 
 
 
 In cone. sol. only. 
 
 6 
 
 HNa^AsOi 
 
 u 
 
 u 
 
 
 Action is like HNai2PO 4 . 
 
 7 
 
 ( AmCl+AmOH 
 i +HNaaP04 
 
 AmMgPO* 
 
 (white 
 ( cryst. 
 
 ( Acids, 
 j 15,OOOH 2 
 
 
 8 
 
 B.B.C.C. 
 
 
 pink 
 
 
 Heat, add drop Co(N0 3 ) 2 
 
 
 
 
 
 
 sol., heat again; gives 
 
 
 
 
 
 
 pink color, when cool. 
 
76. GROUP V. Ba, Sr, Ca, 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 SOL. 
 
 1. Prevent ppn. of Mg(OH) 2 and 
 
 MgC0 3 . 
 
 To sol. add AmCl sol., then 
 AmOH. 
 
 2. Ppt. BaC0 3 , SrC0 3 , CaC0 8 . 
 
 To (a) add Am 2 C0 8 sol., 
 warm, filter, wash. 
 
 3. Final test for Mg. 
 
 To (b) add 
 
 4. Dis. BaCO,, , SrC0 3 , CaCO , in HAc. 
 
 Pour on (1) a little HAc and 
 stir it. 
 
 5. Sep. Ba from Sr, Ca, 
 
 To (c) add K 2 Cr 2 7 sol., 
 filter. 
 
 6. Ppt. SrC0 3 , CaC0 3 . 
 
 Alkalize (d) with AmOH, add 
 Am 2 CO 8 sol., boil, filter, 
 wash. 
 
 7. Dis. SrC0 3 , CaC0 8 in HAc. 
 
 Dis. (4) in little HAc and 
 dil. it. 
 
 8. Sep. Sr and Ca. 
 
 To (e) add very dil. Am 2 S0 4 
 sol., shake, let stand 2 
 hours, filter, test fil. 
 
 9. Final test for Ca. 
 
 Alkalize (f) with AmOH, add 
 Am 2 0x sol. 
 
 (1) BaC0 8 , SrC0 3 , 
 CaC0 8 
 
 (2) AmMgP0 4 
 
 (3) BaCr0 4 
 
 (4) SrCOs, CaC0 3 
 
 (a) BaClg, SrCl 2 , CaCl 2 , 
 (AmCl) 2 MgCl 2 
 
 (b) (AmCl)oMgCl 3 
 
 (c) BaAco, SrAcn, CaAc- : 
 
 (d) SrAc 2 , CaAc 2 
 
 (5) SrS0 4 
 
 (6) CaOx 
 
 (e) SrAcn, CaAc 2 
 
 (f) CaAc 2 , Ca80 4 
 
 Supplementary. 1. AmOH alone partially ppts. Mg(OH) 2 . AmCl forms 
 with Mg salts sol. (AmCl) 2 MgCl 2 , on which Am 2 CO 8 has no effect. A large 
 excess must be avoided. Mg really forms a group by itself, with a separate 
 re-agent. 4. HAc is used, instead of HC1, as K 2 Cr 2 7 sol. ppts. Sr, Ca, as well 
 as Ba from sol. in mineral acids. 5. Only a little of the sol. should first be 
 tested for Ba. If present, the whole must be treated, but if Ba is absent, the 
 rest may at once be tested for Sr (by 8). 5. BaCr0 3 must be removed (by 
 repeated filtration if necessary) to prevent interference with Sr test. 6. SrS O 4 
 is slightly sol. hi K 2 Cr 2 O 7 sol., hence it is better to re-ppt. Sr and Ca as carbon- 
 ates, and re-dis. by HAc before adding Am 2 SO 4 . 8. Very dil. Am 2 SO 4 must 
 be used to ppt. Sr, or Ca will be thrown down with it, as CaSO 4 is sol. in 400 
 pts. H 2 O. The sol. of Am 2 SO 4 should be tested with Ca sol. of a given strength, 
 and if after 2 hours no ppt. forms it is sufficiently dilute. 9. "All Sr must be 
 ppd. before testing for Ca. Make separate sols, of SrSO 4 , CaSO 4 , MgSO 4 . 
 (a) Try BaCl 2 sol. with each, (b) Try SrCl 2 sol. with each of the last two. 
 (c) Try CaCl 2 sol. with the last. Explain the results. 
 
77. SODIUM, Na'. 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOB. 
 
 1. Ppt. NaaSiFg (v. Am, K). 
 
 To a part of sol. add H 2 SiF 6 sol. 
 
 2. Inaction of H 2 Tr on Na salts (v. Am, K). 
 
 To part of original sol. add H 2 Tr. 
 
 3. Inaction of H 2 PtCl on Na salts (v. Am, K). 
 
 To part of original sol. add a few drops 
 of H 2 PtCl 6 . 
 
 4. Flame test lor Na (v. K). 
 
 Evap. part of original sol. to dryness, 
 test with Pt wire in outer edge of 
 Bunsen flame. Intercept flame with 
 blue glass (or indigo sol. in t.t.). 
 Hold sol. of K 2 Cr 2 O 7 in t.t. close to 
 Na flame. 
 
 5. Spectroscopic test for Na. 
 
 Test flame as above, using a spectro- 
 scope, and compare with a chart (v. 
 Physics). 
 
 (1) 
 
 white 
 
 No ppt. 
 
 deep yellow 
 colorless 
 
 decolorized 
 
 yellow lines, 
 etc. 
 
 Supplementary. No ppt. is obtained with H 2 SiF 6 unless the sol. is strong, 
 hence this is not a very good test. What salts of Na are sol. (v. Table A) ? 
 Why should the original sol. be used in each case, e.g. in the flame test? 
 Test the action of sol. Na salts on: (a) AgNO 3 sol.; (b) Pb(NO 8 )a sol. Since 
 Na salts are sol., explain the results. 
 
78. POTASSIUM, K'. 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 1. Ppt, K 2 PtCl 6 (v. Na). 
 To part of sol. add a few drops of H 2 PtCle. 
 
 (1) K 2 PtCl 
 
 yellow 
 
 2. Ppt. HZTr (v. Na). 
 To part of original sol. add H 2 Tr sol. and 
 C 2 H 5 OH. 
 
 (2) HKTr 
 
 white 
 
 3. Ppt, K 2 SiF 6 (v. Am, Na). 
 To part of original sol. add H 2 SiF 6 sol., 
 warm, let stand. 
 
 (3) K 2 SiF 6 
 
 u 
 
 4. Flame test for K (v. Na). 
 Evap. a little of original sol. , test with Pt 
 wire in the outer edge of a Bunsen flame. 
 Cover flame with blue glass (or with t.t. 
 of indigo sol.). 
 
 
 red-violet 
 
 5. Spectroscopic test for Z (v. Na). 
 Examine flame as above, using a spectro- 
 scope, and compare with a chart. 
 
 
 blue lines, 
 &c. 
 
 Supplementary. Neither H 2 Tr nor H 2 SiF 6 will cause a ppt. from dil. sols. 
 What of the common salts of K are insol. (v. Table) ? (a) Use several K salts 
 for the above tests, e.g. KC1, KC1O 3 , KN0 3 , etc. In which is the flame test 
 most distinct ? For flame tests use both solids and sols, (b) Dist. by the flame 
 test a mixture of NaCl and KC1. (c) Dist. K and Na by H t Tr sol. 
 
79. AMMONIUM, NH 4 ' (or Am). 
 
 ANALYTICAL REACTIONS. 
 
 DIRECTIONS. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 1. Ppt. Am 2 PtCl6 (v. Na, K). 
 To a part of the sol. add a few 
 drops of H 2 PtCle. Evap. and 
 ignite (1). 
 
 (1) Amj,PtCl 6 
 (2) Pt (spongy) 
 
 yellow 
 
 
 2. Ppt. HAmTr (v. Na, K). 
 To some original sol. add H 2 Tr 
 and C 2 H 5 OH. 
 
 (3) HAmTr 
 
 white 
 
 
 3. Generate NH 3 . 
 
 
 
 
 To some of original sol. (or solid) 
 add NaOH sol., heat, and test 
 gas (odor, litmus, HC1). 
 
 
 
 (a) NH S gas 
 
 4. Volatilization. 
 
 
 
 
 Heat, and ignite on Pt foil. 
 
 No residue 
 
 
 
 5. Nessler's test for NH 3 . 
 
 
 
 
 To part of original sol. add one 
 or two drops of Nessler's sol. 
 
 (4) NHg 2 IH 2 
 
 brown 
 
 
 6. Inaction of H 2 SiF on Am salts 
 (v. K, Na). 
 To part of original sol. add H 2 SiF 6 
 sol. 
 
 No ppt. 
 
 
 
 Supplementary. HAmTr will not ppt. unless a strong sol. is used. Test 
 several compounds of Am by 3 and 4, e.g. AmNOs, An^Ox, AmaSO*, etc. 
 
8O. GROUP VI. Na, K, Am. 
 
 TESTS. 
 
 RESULTS. 
 
 1. Test for Na. 
 
 (a) To part of original sol. add H 2 SiF 6 sol. 
 
 (b) Apply flame test with Pt wire. 
 
 (c) Apply spectroscope with Pt wire. 
 
 2. Tests for . 
 
 (a) To part of original sol. add H 2 PtCl 6 . 
 
 (b) " " " u " " H 2 Trsol. 
 
 (c) " " " " " " H 4 SiF 6 sol. 
 
 (d) Evap. part of original sol. and try flame test. 
 
 (e) " " " " " " spectrosc. test. 
 
 3. Tests for Am. 
 
 (a) To part of original sol. add H 2 PtCl 6 . 
 
 (b) " u " " u " H 2 Tr and C 2 H 5 OH. 
 
 (c) u " u " " " NaOH sol. , warm. 
 
 (d) Evap. part of original sol. and ignite. 
 
 (e) To part of original sol. add a drop of Nessler's sol. 
 
 Yellow flame. 
 Yellow lines. 
 
 K 2 PtCl 6 . 
 HKTr, 
 K 2 SiF 6 . 
 Purple flame. 
 Blue lines. 
 
 Am,PtCl. 
 HAmTr, 
 NH 3 gas. 
 
 NHg 2 IH 8 0. 
 
81. BOKATES, M 8 BO 8 , 
 
 TESTS. 
 
 RESULTS. 
 
 1. Flame test. 
 
 Mix a bit of powdered Na^O? (or 
 other borate) with a drop or two 
 of H 2 S0 4 . Dip a Pt wire (or glass 
 rod) in this, and hold it in the 
 edge of a Bunsen flame. The same 
 test may be applied by putting the 
 mixture in an e.d., stirring it with 
 a little C 2 H 5 OH, and setting the 
 latter on fire ; or by mixing a drop 
 or two of glycerin with it and test- 
 ing with the Pt wire. H 3 B0 8 gives 
 a green flame without the use of 
 H 2 S0 4 . 
 
 2. Turmeric test. 
 
 Add a very little HC1 to a sol. of 
 Na 2 B 4 O7 till it is just acidified, 
 then moisten a piece of turmeric 
 paper with it. 
 
 A green color is imparted to 
 the flame. 
 
 The color of the paper is red- 
 brown. On drying, the color 
 becomes deeper red. 
 
 Supplementary. Phosphates, salts of Cu and of Ba, except BaS0 4 , also 
 give a green flame, as does C 2 HsCl (formed by C 2 HgOH and MCI). In testing 
 for B, chlorids should first be removed by AgNO s , and also Cu by H 2 S. H 2 S04 
 reduces salts of Ba to BaS0 4 (which gives no green flame), and the flame of 
 phosphates is a very feeble green. H 3 B O 3 in sol. should be evaporated, after 
 first making alkaline to prevent volatilization. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 I 
 
 AgNOs 
 
 Ag 2 (BO,) 2 
 
 white 
 
 
 With normal borates. M 8 B0 8 
 
 
 
 
 
 
 also give Ag 2 O (brown). 
 
 2 
 
 PbACa 
 
 Pb(B0 2 ) 2 
 
 t 
 
 
 
 3 
 
 Cad: 
 
 Ca(B0 2 ) 2 
 
 ' 
 
 AmCl, acids 
 
 Not ppd. if dil. 
 
 4 
 
 BaCl 2 
 
 Ba(B02) 2 
 
 i 
 
 tl U 
 
 U It U tt 
 
 6 
 
 A1 2 (S04>3 
 
 A1(OH) 8 
 
 4 
 
 Acids 
 
 
 6 
 
 MgCl 2 
 
 Mg(B0 2 ) 2 
 
 < 
 
 AmCl, acids 
 
 
82. NITRATES, MNO 3 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Copperas test (v. MN0 2 ). 
 
 Mix in a t.t. a sol. of MN0 3 , or sol. 
 to be tested, with a fresh sol. of 
 FeSO 4 . When cold, introduce into 
 the bottom of the tube, with a glass 
 tube used as a pipette, a little 
 H 2 S0 4 . 
 
 2. Deflagration test (v. MNO 2 , MC10 3 ). 
 
 Heat B.B.C.C. a very little pow- 
 dered MNO 3 ; or mix with pow- 
 dered charcoal, and put into an i.t. 
 enough to cover a penknife point. 
 Heat cautiously. 
 
 3. Red fumes test (v. MN0 2 ). 
 
 Put into an i.t. very little MNO 3 , 
 heat. Insert a glowing splinter 
 into the tube while heating. 
 
 4. Free HN0 3 . 
 
 (a) Add a little indigo sol. 
 
 (b) Put a drop on the finger-nail, or 
 
 dip a feather into it. 
 
 (c) Pour a little on Cu and warm it. 
 
 (FeS0 4 ) 2 NO. Brown ring or 
 halo at junction of liquids. 
 
 Vigorous deflagration ensues. 
 
 N0 2 and N 2 3 (red) ; O (color- 
 less). Splinter burns. 
 
 Decolorizes, changing to red 
 
 isatin. 
 Turns animal matter yellow. 
 
 Bed fumes (N0 2 ), green liquid, 
 Cu(N0 3 ) 2 . 
 
 Supplementary. If a ppt. appears on adding H 2 SO 4 , let it settle, then 
 decant. H 2 SO 4 liberates HNO 3 from nitrates, and FeS0 4 reduces HN0 3 at 
 the surface of contact to N 0, which unites with FeS 4 . Let it stand an hour or 
 more if necessary. Heat decomposes this compound (FeSO 4 ) 2 NO, expelling 
 NO. The depth of color indicates the strength of nitrate. Heat decomposes 
 all nitrates ; from those of the alkali and alkaline earth metals are first formed 
 MNO 2 and O, then M 2 O, O, N. Nitrates of Ag and Hg reduce to the metal, 
 others to the oxid only. KNO 3 and NaNO 3 show faint fumes, best seen by 
 looking down the tube to a white background. Indigo is also decolorized by Cl, 
 Br, etc. Nitrates of Au and Sb are unknown. All nitrates are soluble except 
 Bi(N0 3 ) 3 , which reacts with H 2 O and ppts. Bi(OH) 2 N0 3 (variable), and to a less 
 extent Hg / , Hg", Sn", Sn iv . 
 
83. NITRITES, MNO 2 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Copperas test (v. MNO 3 ). 
 
 Apply this as in MNO 8 . 
 
 2. Bed fnmes test (v. MN0 3 ). 
 
 To a little MN0 2 add a few drops of 
 
 H 2 SO 4 . 
 Test the HNO 2 formed with iodo- 
 
 starch sol. 
 Test it also with KMn0 4 sol. 
 
 3. lodin test. 
 
 Add a few drops of KI sol. to 3 or 4 
 cc. H 2 O, then a few drops of dil. 
 H 2 SO 4 ; finally a little MN0 2 sol. 
 (or substance to be tested). 
 
 Test yellow liquid with starch sol. 
 
 4. Nitrate test (v. General Reactions). 
 
 Same result as in MNO 3 , but 
 more readily obtained. 
 
 N0 2 (red fumes) copiously 
 
 evolved ; also HN0 2 . 
 Starch iodid (blue) formed. 
 
 Decolorized. 
 
 HI first formed, then H 2 0, and 
 I set free by MN0 2 (yellow 
 color). 
 
 Iodid of starch (blue). 
 
 Supplementary. Indigo sol. is decolorized by nitrites, but not by nitrates 
 except by the addition of H 2 S0 4 , which forms HNO 3 . Apply the test. All 
 nitrites are soluble, but AgNO 2 and Pb(N0 3 ) 2 only slightly. Hence this test 
 cannot be applied in dil. sols. 
 
 GENERAL REACTIONS. 
 
 
 BE-AGT. 
 
 PPT. 
 
 CO LOB. 
 
 SOLVENTS. 
 
 REMAKKS. 
 
 1 
 
 AgNOs 
 
 AgN0 2 
 
 white 
 
 \ Acids, 
 i H 2 (ex.) 
 
 This distinguishes MN0 2 from 
 
 MNOg. 
 
 2 
 
 Pb(NO s ) 2 
 
 Pb(N0 2 ) 2 
 
 u 
 
 it 
 
 u it u a 
 
84. CHLORATES, MC1O 3 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Oxygen test (v. MN0 2 , MN0 3 ). 
 
 Heat a small quantity of the solid in 
 
 at.t. 
 
 Test the O with a glowing splinter. 
 Dis. the residue when cool, and test 
 
 for MCI with a drop of AgN0 3 sol. 
 
 2. Chlorin test (v. MN0 2 , MN0 3 ). 
 
 To a very little of the powder in a 
 t.t. add with great caution a few 
 drops of H 2 S0 4 . 
 
 3. Deflagration test (v. MN0 3 ). 
 
 Powder and heat B.B.C.C. 
 
 4. Bleaching test (v. MN0 2 , MN0 8 ). 
 
 To sol. of indigo add MC10 3 sol. , and 
 
 heat. 
 Mix sols, of MC10 3 and H 2 S0 3 , and 
 
 add to indigo sol., without heating. 
 
 5. Silver nitrate test (v. MAc, MN0 3 ). 
 
 To sol. add a few drops of AgNO 3 sol. 
 
 Melts, O escapes, MCI remains. 
 
 Re-kindles vigorously. 
 AgCl (white) ppts., sol. in 
 AmOH. 
 
 C10 2 (green-yellow, of charac- 
 teristic odor) liberated with 
 explosive violence. 
 
 Deflagrates. 
 
 Turned red (isatin). 
 
 No effect if the MC10 3 is pure. 
 
 Supplementary. All chlorates are soluble. Sb, Sn, and Au have no known 
 chlorates. The deflagration of chlorates is greater than of nitrates, (a) Test 
 this by scratching different kinds of matches. A few drops of HC1 added to a 
 few crystals of MC1O 3 , and heated, give C10 2 and Cl, of characteristic odor. 
 Heat liberates O with violence from chlorates, but the presence of certain oxids 
 (e.g. Mn0 2 ) causes it to be liberated more regularly, and at a lower temperature. 
 Dist. (b) KC10 3 and KC1; (c) KC10 3 and KNO 3 ; (d) KC1O 8 and KNO 2 . 
 
85. CARBONATES, M 2 CO 3 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Lime water test, 
 
 To the solid (or sol.) add a little dil. 
 HC1. Test the gas with a drop of 
 Ca(OH) 2 sol. on a s.r., or pass it 
 into Ca(OH) 2 sol., or shake the 
 lime water with the gas. 
 
 2. Barium hydroxid test, 
 
 Apply this hi the same way as the 
 lime water test, using Ba(OH) 2 sol. 
 instead of Ca(OH) 2 . 
 
 3. Flame test. 
 
 Put a burning splinter into the gas 
 generated, as above. 
 
 CO 2 gas (colorless) is formed, 
 which ppts. white CaCOs 
 with lime water. 
 
 White BaCO 3 fails, ppd. by 
 CO 2 gas, and dissolved with 
 effervescence by HC1. 
 
 The flame is extinguished. 
 
 Supplementary. Any acid (except H 2 S, H Cy) will act on any carbonate 
 and liberate C0 2 , but with varying intensity. H 2 CO 3 with a carbonate (e.g. 
 Na 2 CO 3 or CaCO 3 ) forms the bicarbonate (primary or acid carbonate), as 
 HNaC0 3 , H 2 Ca(CO 3 ) 2 . Most carbonates are insol. Heat breaks up many of 
 them, forming the metallic oxid and C 2 . CaC O 3 requires a red heat, and the 
 alk. carbonates are not decomposed at the temperature of the Bunsen flame 
 (v. oxalates). Try the action of various acids on carbonates, as: (a) HAc; 
 (b) H 2 Ox; (c) H 2 Tr. Na, K, Mg, burn in C0 2 , liberating C. (d) Pass C0 2 
 from a gen. into lime water till the ppt. clears, then boil. Dist. : (e) C O 2 and 
 SO 2 ; (f) CO 2 and H 2 S ; (g) CO 2 and N0 2 ; (h) M 2 CO 3 and M 2 Ox. Some 
 metallic salts with Na^C O 3 sol. give the primary carbonate, others the secondary, 
 and occasionally a basic salt is formed, as 2PbCO 3 .Pb(OH) 2 . Carbonates are 
 white in color. 
 
86. SULFIDS, M 2 S. 
 
 TESTS. 
 
 RESULTS. 
 
 1. Acid test. 
 
 To the solid (or sol.) add a little dil. 
 HC1 (or H 2 S0 4 ), and warm it. 
 Test the escaping gas (odor, PbAc 2 
 sol. on paper). 
 
 2. Coin test. 
 
 Put a drop of water on a silver coin, 
 and on this a soluble sulfid (if in- 
 sol., first fuse with Na 2 CO 3 ). (V. 
 M 2 S0 3 , M 2 S 2 3 , M 2 S0 4 .) 
 
 3. Ppn. tests (v. General Reactions). 
 
 H 2 S gas formed, with odor of 
 sewer-gas. Black, metallic 
 PbS formed. 
 
 Coin is blackened. by forma- 
 tion of Ag 2 S. 
 
 Supplementary. All sulfids, except those of the alkalies and alkaline 
 earths are insol. in H 2 O. Most are sol. in dil. acids. A few (FeS 2 , HgS, CoS, 
 NiS, etc.) are not acted on by acids, except aqua regia. In such cases H 2 S may 
 be made by nascent H, with the addition of a little Zn. No sulfid of Al or Cr 
 is known. Oxidizing agents with sulfids tend to form sulfates, or to liberate S 
 and S0 2 . (a) Test several with HN0 3 , or aqua regia. Metallic sulfids (includ- 
 ing Am 2 S) ppt. from sols, metals of the first four groups, except Cr and Al. 
 H 2 S ppts. only the first two groups. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 PPT. 
 
 COLOB. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 
 
 With H 2 S : 
 
 With. Am 2 S : 
 
 
 
 
 1 
 
 Pb(N0 3 ) 2 
 
 PbS 
 
 PbS 
 
 black 
 
 HotHNOa(dil.) 
 
 
 2 
 
 AgN0 3 
 
 Ag 2 S 
 
 Ag 2 S 
 
 <( 
 
 u u u 
 
 
 3 
 
 HgN0 3 
 
 Hg,S 
 
 Hg 2 S 
 
 u 
 
 aqua regia 
 
 Warming changes to 
 HgS and S. 
 
 4 
 
 HgCl 2 
 
 HgS 
 
 HgS 
 
 u 
 
 U i( 
 
 First white, then yel- 
 low, red, black. 
 
 5 
 
 BiCla 
 
 Bi 2 S 3 
 
 Bi 2 S 3 
 
 u 
 
 HotHNOaCdil.) 
 
 
 
 
 CdCl, 
 
 CdS 
 
 CdS 
 
 yellow 
 
 (( It 11 
 
 
 7 
 
 CuCl 2 
 
 CuS 
 
 CuS 
 
 ( brown- 
 f black 
 
 u u u 
 
 
 8 
 
 AsCla 
 
 AS 2 S 3 
 
 As 2 S 3 
 
 yellow 
 
 ( Am 2 S 2 (ex.), 
 1 Am 2 C0 3 
 
 Alkaline sol. not ppd. 
 with H 2 S. 
 
 9 
 
 SbCls 
 
 Sb,S 3 
 
 Sb 2 S 3 
 
 ( orange- 
 ( red 
 
 ( Am 2 Sx (ex.), 
 1 HC1 (hot) 
 
 Ppn. with Am 2 S is 
 imperfect. 
 
 10 
 
 SnCI- 
 
 SnS 
 
 SnS 
 
 j dark- 
 i brown 
 
 U 11 
 
 
 11 
 
 FeCls 
 
 none 
 
 FeS+S 
 
 black 
 
 Acids 
 
 
 12 
 
 CoCl 2 
 
 (t 
 
 CoS 
 
 u 
 
 aqua regia 
 
 AmCl aids ppn. 
 
 13 
 
 NiCl 2 
 
 
 
 NiS 
 
 11 
 
 u u 
 
 <( U U 
 
 14 
 
 MnCl= 
 
 u 
 
 MnS 
 
 pink 
 
 Acids 
 
 Turns dark -brown. 
 AmCl aids ppn. 
 
 16 
 
 ZnCls 
 
 (( 
 
 ZnS 
 
 white 
 
 ii 
 
 AmCl aids ppn. 
 

 
 
87. SULFITES, M 2 SO 3 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Acid test. 
 
 To the solid (or sol.) add a little HC1 
 (or dil. H 2 SO 4 ), and heat it. Test 
 the escaping gas (odor, K 2 Cr 2 O7 
 paper). 
 
 2. Zinc test. 
 
 To the original sol. add Zn and dil. 
 H 2 SO 4 . Test the escaping gas 
 (odor, PbAc 2 paper). 
 
 3. Coin test (v. M 2 S, M 2 S 2 O 3 , M 2 SO 4 ). 
 
 Heat the solid B. B. C. C. with Na 2 C0 3 , 
 also without. Put res. on Ag coin 
 on which is a drop of water. 
 
 4. Oxidation test (v. M 2 S0 4 ). 
 
 To some of the original sol. add a 
 little euchlorin (or HN0 3 ), and 
 heat. Test the product with HC1 
 and BaCl 2 sol. 
 
 S0 2 gas is liberated, reducing 
 K 2 Cr 2 7 to green O 2 (S0 4 ) 3 . 
 
 H 2 S is liberated, forming with 
 PbAc 2 black PbS. 
 
 Na 2 S is formed, and on the 
 coin black Ag 2 S. 
 
 M 2 S0 3 is oxidized to M 2 S0 4 , 
 and ppd. with BaCl 2 as 
 white BaSO 4 , insol. in HC1. 
 
 Supplementary. The alkaline sulfites are freely sol. in water. Most others 
 are but slightly sol., or are insol. Sulfites are decomposed by acids (except 
 H 2 C0 3 , H 3 B0 3 , H 2 S). (a) Ppt. BaS0 3 with BaCl 2 sol., dis. in HC1, filter if 
 necessary, then oxidize fil. with aqua regia, and try to dis. ppt. in HC1. Heat 
 changes sulfites to M 2 and SO 2 ; also to M 2 SO 4 and M 2 S. (b) Make the tests. 
 Sulfites are reducing agents, (c) Test action of SO 2 on FeCl 3 sol., then test sol. 
 for Fe" and Fe'". (d) Test HgCl 2 with S0 2 , then test sol. for Hg' or Hg". 
 (e) Generate H in a t.t., and test the gas for H 2 S with PbAc 2 paper, then add a 
 few drops of Na 2 SO 3 sol. and test again, (f) Bring together jets of S0 2 and 
 H 2 S. (g) Test the bleaching action of S 2 sol. by putting in it a colored flower, 
 or cambric, (h) Test with litmus sol. (i) Let some S0 2 sol. stand for a few 
 days in an open rec., and apply the BaCl 2 and HC1 test, (j) Try the action of 
 SO 2 sol. onCaCO 3 . 
 
 GENERAL REACTIONS. 
 
 
 KE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 BaCl> 
 
 BaSO; 
 
 white 
 
 HC1 (dil.) 
 
 (V. M 2 S0 4 .) 
 
 2 
 3 
 
 AgN0 3 
 
 Pb(N0 3 ) 2 
 
 Ag 2 S0 3 
 PbS0 3 
 
 u 
 
 u 
 
 HN0 3 (dil.) 
 
 u 
 
 Boiling ppts. dark-brown Ag. 
 Not blackened on boiling (v. 
 
 
 
 
 
 
 M 2 S 2 3 ). 
 
 4 
 
 FeCla 
 
 Fe 2 (SO) 3 
 
 red 
 
 
 Boiling forms green FeSO 4 . 
 
 6 
 
 HgCl> 
 
 HgCl 
 
 white 
 
 
 Boiling reduces to gray Hg. 
 
88. THIOSULFATES, M 2 S 2 O 3 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Bulb-tube test. 
 
 Heat the solid in a tube. 
 
 2. Acid test. 
 
 Add to the cone. sol. (or the solid) 
 
 HC1 (or H 2 S0 4 ), warm. 
 Test S0 2 (odor, K 2 CrO 4 ). 
 
 3. Beduction test (v. M 2 S0 3 ). 
 
 (1) To a sol. of starch and KI (made 
 
 blue by Cl) add a sol. of M 2 S 2 O 3 . 
 
 (2) To a sol. of starch and KI (un- 
 
 colored) add M 2 S 2 3 sol. with 
 which a little euchlorin is 
 mixed. 
 
 4. Coin test (v. M 2 S, M 2 S0 3 , M 2 S0 4 ). 
 
 Fuse B.B.C.C., put on Ag coin with 
 a drop of H 2 O. 
 
 5. Precipitation tests. 
 
 (V. General Reactions.) 
 
 Sublimate of H 2 O and S, and 
 liberation of S0 2 . 
 
 S ppts. (white), S0 2 formed. 
 
 Decolorized. 
 
 Uncolored, as Cl has oxidized 
 M 2 S 2 3 to M 2 S0 4 and HC1. 
 
 Coin is blackened (Ag 2 S). 
 
 Supplementary. Thiosulf ates, if mixed in a mortar with chlorates, explode 
 violently. They are strong reducing agents. They are mostly sol. in water, 
 except those of Ba, Pb, Ag. Dist. : . (a) M 2 S 2 O 3 and M 2 S ; (b) M 2 S 2 8 and 
 M 2 S0 3 ; (c) M 2 S 2 3 and M 2 S0 4 . 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 BaCl 2 
 
 BaS 2 3 
 
 white 
 
 Dil. acids 
 
 Acids ppt. S (white). 
 
 2 
 
 AgN0 3 
 
 Ag 2 S 2 3 
 
 (t 
 
 Na^Oz (ex.) 
 
 Boiling forms Ag 2 S (black). Forms 
 
 
 
 
 
 
 slowly on standing. 
 
 3 
 
 PbACa 
 
 PbS 2 3 
 
 t( 
 
 u u 
 
 Boiling forms PbS (black). Forms 
 
 
 
 
 
 
 slowly on standing. 
 
 4 
 
 HgN0 3 
 
 Hg 2 S 2 3 
 
 t( 
 
 tt u 
 
 Boiling forms Hg 2 S (black). Forms 
 
 
 
 
 
 
 slowly on standing. 
 
 5 
 
 FeCla 
 
 FeClo 
 
 
 
 Acts as reducing agent. 
 
 6 
 
 CaCl 2 
 
 none 
 
 
 
 Dist. from M 2 SO 3 . 
 
89. FL.UORIDS, MF. 
 
 TESTS. 
 
 RESULTS. 
 
 1. Glass- etching test, 
 
 (1) Put a little powdered CaF 2 into a 
 
 small lead dish, and mix with 
 enough H 2 SO 4 to make a thick 
 paste. Cover the dish with a piece 
 of glass (coated with wax if de- 
 sired, and a design scratched on 
 it) and let it stand in a warm place 
 for several hours. Remove the wax 
 by melting, and finally with a cloth 
 wet with alcohol, naphtha, or tur- 
 pentine. 
 
 (2) Mix a little CaF 2 with HKS0 4 , put 
 
 into a small t.t., and heat. 
 
 2. Turbidity test. 
 
 Mix a little CaF 2 , Si0 2 and H 2 SO 4 , 
 put into a t.t. and heat it, mean- 
 time holding in the tube on a s.r. 
 (or in the loop of a Pt wire) a drop 
 of H 2 0. 
 
 3. Free HF in sol. 
 
 Dip a brush into the liquid in a 
 leaden dish, and mark out a design 
 with it on a glass plate, going over 
 it several times. Avoid getting any 
 HF sol. on the flesh. 
 
 The glass will be etched where 
 exposed to the fumes of HF, 
 SiF 4 being formed. 
 
 The tube will be roughened 
 (or etched) by the HF. 
 
 The water is rendered turbid 
 by the SiF 4 gas, forming 
 H 2 SiF 6 . 
 
 The glass will be etched as 
 above. 
 
 Supplementary. Several of the fluorids are soluble. The most important 
 compounds of F are CaF 2 and HF. The latter corrodes glass, porcelain, and all 
 metals except Pb, Pt, and Au. CaCl 2 ppts. CaF 2 (transparent, gelatinous). 
 BaCl 2 ppts. BaF 2 (white). CaF 2 , which occurs in the earth as fluorite or fluor- 
 spar and cryolite, Na 3 AlFe, a mineral found in Greenland, are the main sources 
 of F compounds. 
 
9O. CHLOKIDS, MCI. 
 
 TESTS. 
 
 RESULTS. 
 
 1. HC1 test. 
 
 Add H 2 S0 4 to the solid in t.t., heat. 
 Test gas (odor, color, NH 3 ). 
 
 2. Cl test. 
 
 Mix the solid with MnO 2 , add H 2 SO 4 , 
 heat. Test gas (odor, color, NH 3 , 
 indigo paper). 
 
 3. Precipitation tests. 
 
 (a) To sol. add AgNO 3 sol. Expose part 
 
 to sunlight, add AmOH to the rest, 
 then HNO 3 . 
 
 (b) To sol. add HgNO 3 sol. ; then AmOH. 
 
 (c) To sol. add Pb(NO 3 ) 2 sol. boil with 
 
 plenty of H 2 0. 
 
 1IC1 is liberated. 
 
 Cl liberated, green - yellow ; 
 AmCl with NH 3 , indigo pa- 
 per bleached. 
 
 AgCl (white) ppts. ; blackens 
 
 in light ; sol. in AmOH ; re- 
 
 ppd. by HNO 3 . 
 HgCl (white) ppts. ; blackened 
 
 by AmOH. 
 PbCl 2 (white) ppts. ; sol. in 
 
 boiling H 2 0. 
 
 Supplementary. Most chlorids are soluble. Except. : Ag, Pb, Hg', Cu'. 
 SbCl 3 , BiCl 3 , SnCl 2 decompose water, forming SbO Cl, BiO Cl, Sn 2 O C1 2 . H 2 S O 4 
 frees HC1 from all chlorids, except HgCl and HgCl 2 (and not much from Ag, 
 Pb, Sn chlorids). HgCl 2 sol. fails to ppt. PbCl 2 from Pb(NO 3 ) 2 sol. (a) Test 
 the last statement. Dist.: (b) MCI and MC10 3 (cautiously); (c) MCI and 
 MNO 3 . (d) Take 5& KC1O 3 and divide into 2 parts. Dis. one in H 2 O and add 
 AgNO 3 sol. Heat the other a few minutes, then dis., and add AgNO 3 sol. 
 Compare the results. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AgN0 3 
 
 AgCl 
 
 white 
 
 AmOH, etc. 
 
 (v. Exp. 49.) 
 
 2 
 
 Pb(N0 3 ) 2 
 
 PbCl 2 
 
 u 
 
 Hot H 2 
 
 (v. Exp. 48.) 
 
 3 
 
 HgN0 3 
 
 HgCl 
 
 " 
 
 HN0 3 
 
 (V. Exp. 50.) 
 
91. BBOMII>S, MBr. 
 
 TESTS. 
 
 RESULTS. 
 
 1. Bromin test. 
 
 Mix Mn0 2 with the solid, add a little 
 
 H 2 SO 4 , heat. 
 Test the gas by holding in it a paper 
 
 dipped in starch-paste. 
 
 2. I o do- starch test. 
 
 Liberate Br as above, and hold in it 
 a paper dipped in a mixture of 
 starch-paste and KI sol. 
 
 3. CS, test. 
 
 To the sol. add a drop or two of 82 
 sol., and a drop of euchlorin, and 
 shake it. 
 
 4. Silver nitrate test. 
 
 To sol. add a drop or two of AgNOs 
 sol. Try to dis. part of ppt. in 
 HNO 8 , another part in AmOH. 
 
 Br (red gas) is liberated. 
 Colors starch yellow to orange. 
 
 Br combines with K in KI, lib- 
 erates I, which forms blue 
 starch-iodid. 
 
 Br is liberated and absorbed 
 by 82, which is colored 
 yellow. 
 
 AgBr, yellow- white, ppts., in- 
 sol. in HN0 3 , slowly sol. in 
 AmOH. 
 
 Supplementary. Bromids are soluble, except those of Ag, Hg', Hg", Cu', Pb. 
 BiBr 3 and SbBr 3 need acidulation. Dilute H 2 S04 acts on bromids to form 
 HBr; strong acid forms Br. (a) To a bromid sol. add euchlorin (very little), 
 and note the color, (b) Dist. MBr and MCI. (c) Pour a little Br vapor into 
 starch-paste, and shake., (d) Mix starch-paste and KBr sol. (very little), and 
 add a drop or two of euchlorin. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOL. 
 
 REMARKS. 
 
 I 
 
 AgN0 3 
 
 AgBr 
 
 pale yellow 
 
 AmOH 
 
 Only slightly sol. in AmOH. 
 
 2 
 
 PbAc2 
 
 PbBr 2 
 
 white 
 
 Hot H 2 
 
 Less sol. than AgCl in H 2 O. 
 
 8 
 
 HgN0 3 
 
 HgBr 
 
 yellow-white 
 
 KBr 
 
 
 
 
 
 
 
 
92. IODIDS, MI. 
 
 TESTS. 
 
 RESULTS. 
 
 1. Starch test. 
 
 Mix Mn0 2 with the solid, add H 2 S0 4 , 
 heat, and test with cold starch- 
 paste (v. Exp. 40). 
 
 2. CS 2 test. 
 
 Add to the sol. a drop of CS 2 [or 
 (C 2 H 5 ) 2 0], then 2 or 3 drops of 
 euchlorin (avoid excess), and shake 
 it well. 
 
 Violet I vapor appears, which 
 colors starch-paste blue. 
 
 CS 2 dis. the I set free by Cl, 
 and is colored violet at the 
 bottom of the tube. NaOH 
 destroys the color, forming 
 Nal and NaI0 3 . 
 
 Supplementary. Most iodids are sol. , except Pb, Hg 7 , Hg", Au. Sb, Bi, 
 Cu, Sn iv iodids need acidulation, as they react with H 2 0. The double iodids 
 (KIAgI, etc.) are formed and dis. with excess of KI with salts of Pb, Ag, Hg. 
 I may be liberated from an iodid by Zn and HNOs, HNO 2 being first formed. 
 Euchlorin or bromin acts the same. Iodids are broken up by oxidizing agents 
 more easily than bromids or chlorids. 
 
 GENERAL REACTIONS. 
 
 BE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AgN0 3 
 
 Agl 
 
 yellow-white 
 
 KCy, Na 2 S 2 3 
 
 Insol. in HNO 3 or ArnOH. 
 
 2 
 
 Pb(N0 3 ) 2 
 
 PbI 3 
 
 yellow 
 
 NaOH (ex.) 
 
 Dis. by HN0 3 . 
 
 8 
 
 HgNO s 
 
 Hgl 
 
 green-yellow 
 
 HgN0 3 (ex.) 
 
 u u u 
 
 4 
 
 Hg(NOs), 
 
 HgI 2 
 
 yellow-red 
 
 Hg(N0 3 ) 2 (ex.) 
 
 u it . u 
 
 5 
 
 CuSCM-HjSOs 
 
 Cul 
 
 white 
 
 H 8 (si.) 
 
 Insufficient reduc. agent 
 
 
 
 
 
 
 ppts. I. 
 
93. ACETATES, MC 2 H 3 O 2 (MAc). 
 
 TESTS. 
 
 RESULTS. 
 
 1 . Charring test ( v. M 2 Tr, M 2 0x) . 
 
 Heat a very little of the 
 solid in a t.t. , take odor. 
 
 2. Acetic acid test (v. M 2 Tr). 
 
 Add to the solid (or sol.) 
 H 2 SO 4 , heat, take the 
 odor, test with litmus. 
 
 3. Acetic ether test. 
 
 Add to the sol. a few drops 
 of C 2 H 5 OH and H 2 S0 4 , 
 warm, and take odor. 
 
 4. Ferric test, 
 
 To sol. add FeCl 3 sol. , boil. 
 
 5. Silver nitrate test (v. MNO 3 , 
 
 MC10 8 ). 
 
 To a dil. sol. add AgN0 3 
 
 sol. 
 To a strong sol. add AgNOs 
 
 sol. 
 
 6. Cacodyl test. 
 
 Heat with an alkali and 
 very little As^e ; take 
 odor. 
 
 Melts, expels H 2 O, turns black, gives odor 
 of acetone, C 3 H 6 O (inflammable). 
 
 HAc is formed, having characteristic odor, 
 and acid reaction. 
 
 C 2 H 5 Ac is formed, having characteristic 
 odor. 
 
 FeAc 3 (red sol.). Boiling ppts._ red-brown 
 basic acetate of Fe'". 
 
 No ppt. 
 
 AgAc (white) ppts. 
 
 Cacodyl oxid As 2 (CH 3 ) 4 evolved (intensely 
 offensive odor). 
 
 Supplementary. All acetates are sol., those of Ag and Hg' only partially. 
 No acetate of Au is known. Dist.: (a) MAc and M 2 Tr; (b) MAc and M 2 Ox. 
 (a) Try to make CH 4 in a t.t. by heating dry NaOH and an acetate, (b) Test 
 the combustibility of the gas. (c) Test some vinegar for acetic acid, (d) Make 
 some HgAc ; (e) AgAc. (f) See whether HAc will dis. Zn ; (g) Fe. (h) If so, 
 test the product for Fe" and Fe'". 
 
94. CYANIDS, MCN (MCy). 
 
 TESTS. 
 
 KESULTS. 
 
 1. HCy test. 
 
 Add to sol. a little H 2 SO 4 (or HC1). 
 Very cautiously take the odor by 
 fanning the gas to the face with 
 the hand. 
 
 2. Fe(CyS) 3 test. 
 
 Put a few drops in an e.d., add 
 equally Am 2 S x , evap. to dryness, 
 dis. in dil. HC1, add FeCl 8 sol. 
 
 3. Prussian blue test. 
 
 To sol. add equally a few drops of 
 NaOH sol. and FeS0 4 sol., shake 
 and warm it, add FeCl 3 . Dis. in 
 dil. HC1 (excess). 
 
 4. AgN0 3 test. 
 
 To sol. add a little A gN0 8 sol. Pour off 
 liquid, and boil with HNOg. If not 
 all dissolves, test liquid with HC1. 
 
 HCy is formed (very poison- 
 ous) ; odor of bitter aim onds. 
 
 MCyS is formed, sol. in HC1, 
 giving red Fe(CyS) 3 sol. 
 with FeClg. 
 
 FeCy2 (sol. in MCy excess), 
 Fe(OH) 2 , Fe(OH) 8 formed, 
 soluble in HC1, but ppg. 
 Fe 4 Fe 3 Cyi8, deep blue. 
 
 AgCy (white) ppts., sol. in hot 
 HN0 3 , re-ppd. by HC1. 
 
 Supplementary. Use great care in experimenting with cyanids, as they 
 are very poisonous. Cyanids are insol., except HgCy2 and those of the alkalies 
 and alkaline earths (BaCy 2 only slightly). The solutions are alkaline. The 
 ppd. cyanids are often sol. in excess of the cyanids, forming double salts, 
 (a) Make several by ppn., and then dissolve. Dist. : (b) MCy and MAc; 
 (c) MCy and MN0 3 . In the Prussian blue test the following equations indicate 
 the order of changes: (1) 2MCy+FeSO 4 = FeCy 2 +M 2 SO 4 ; (2) 4MCy+FeCy 2 = 
 M 4 FeCy 6 ; (3) FeS0 4 +2NaOH=Fe(OH) 2 -f NaaSO 4 ; (4) 2Fe(OH) 2 +H 2 0+0= 
 2Fe(OH) 3 ; (5) 2HCl+Fe(OH) 2 =FeCl 2 +2H 2 O; (6) 3HCl+Fe(OH) 3 =FeCl 3 + 
 3H 2 O; (7) 4FeCl 3 +3M 4 FeCy 6 =Fe 4 Fe 3 Cyi8+12MCl. The vapor of HCy is a 
 deadly poison, N H 3 or Cl inhaled being the antidote. As used in medicine the 
 acid contains only 2% H Cy. 
 
95. TABTKATES, 
 
 (M 2 Tr). 
 
 TESTS. 
 
 RESULTS. 
 
 1. Ignition test (v. M 2 0x, MAc). 
 
 Heat in i.t. Take odor, note res. 
 
 2. H 2 S0 4 test (v. MAc, M 2 Ox). 
 
 Heat in i.t. with little H 2 SO 4 . 
 
 3. Mirror test. 
 
 Add AgNO 3 sol. (to a neutral sol.). 
 Almost dis. ppt. with AmOH, then 
 heat gently in t.t. 
 
 4. Acetic acid test (v. MAc, M 2 0x). 
 
 Add to sol. BaCl 2 sol. Dis. the ppt. 
 
 in HAc. 
 Add to sol. CaCl 2 sol. Dis. the ppt. 
 
 in AmCl sol. 
 
 5. Potassium chlorid test. 
 
 Add KC1 sol. and C 2 H 5 OH to the sol., 
 stir with a glass rod. 
 
 Evolves fumes (white, then 
 brown), CO 2 , with odor of 
 burnt sugar, and black resi- 
 due, M 2 CO 3 , C. 
 
 CO, C0 2 , S0 2 , C. 
 
 Ag 2 Tr (white) ppts. Mirror of 
 Ag collects on the tube. 
 
 BaOx is sol. in HAc. 
 
 CaOx forms, sol. hi NaOH, 
 re-ppd. on boiling. 
 
 HKTr (white) ppts. from 
 strong sols. only. 
 
 Supplementary. Only the alkali tartrates are freely soluble, and the 
 bitartrates of the alkali metals are much less so than the normal ones (v. tests 
 for K and Am). Dist.: (a) M 2 Tr and M 2 0x; (b) M 2 Tr and MN0 2 . (c) Make 
 H AinTr. (d) Try the reducing action of H 2 Tr on K 2 Cr 2 7 sol. (e) See whether 
 CaTr is sol. 
 
96. OXAL.ATES, M 2 C 2 O 4 (M 2 Ox). 
 
 TESTS. 
 
 RESULTS. 
 
 1. Ignition test (v. M 2 Tr, MAc). 
 
 Heat the solid in an i.t. Test gas with 
 Ca(OH) 2 sol., also combustion of 
 CO. H 2 Ox decomposes with very 
 slight charring, and without res. 
 
 2. Acid test (v. MAc, M 2 Tr). 
 
 Heat the solid with H 2 SO 4 (which 
 absorbs the H 2 O). 
 
 3. Calcium suliate test. 
 
 Alkalize the sol. with AmOH, add a 
 little CaS0 4 sol. Try to dis. part 
 of the ppt. with HAc, the rest with 
 dil. HC1. 
 
 CO 2 , CO, M 2 O form. On pass- 
 ing the gas through NaOH 
 sol. to remove C0 2 , CO burns 
 with blue flame. 
 
 CO 2 , CO, M 2 form. Dil. HC1, 
 HN0 3 or H 2 S0 4 decomposes 
 M 2 0x, forming H 2 Ox. 
 
 CaOx (white) ppts. , sol. in dil. 
 HC1 without effervescence, 
 insol. in HAc. 
 
 Supplementary. On igniting oxalates, carbonates and CO first form, then 
 oxids and C 2 . Ag 2 Ox and HgOx (which easily decompose with heat) give the 
 metals as a final product. Ag 2 decomposes with explosion, (a) Test several 
 oxalates, first changing them to Ag 2 Ox. At moderate temperature H 2 0x 
 sublimes unchanged, except to give off its water of crystallization. Most 
 oxalates are insoluble, except those of the alkali metals and Cr. HC1, HNO 8 , or 
 H 2 S 4 forms H 2 0x from its salts. Oxalates are reducing agents, (b) (test with 
 KMn0 4 ), and are almost all white in color, (c) Make several oxalates. (d) vSee 
 whether H 2 0x will react with metals, e.g. Zn and Fe. 
 
 GENERAL REACTIONS. 
 
 
 RE-A.GT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 I 
 
 CaCl, 
 
 CaOx 
 
 white 
 
 HC1 (dil.) 
 
 2 
 
 FeSO* 
 
 FeOx 
 
 yellow-white 
 
 
 3 
 
 AgNO, 
 
 Ag 2 0x 
 
 white 
 
 
 4 
 
 Pb(N0 3 ) 2 
 
 PbOx 
 
 n 
 
 NaOH, HNO S 
 
97. SILICATES, M 4 SiO 4 , M 2 SiO 8 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Acid test. 
 
 To strong sol. add HC1 ; then evap. 
 Add HC1, boil, decant ; then add 
 to res. NaOH sol., boil. 
 
 2. Fusion test (insol. silicates). 
 
 Mix thoroughly 2 pts. dry K 2 C0 3 , 
 2 pts. Na 2 C0 3 , 1 pt. finely powdered 
 M 4 Si0 4 (e.g. slate, etc.), fuse thor- 
 oughly B.B.C.C. Pulverize, add 
 H 2 O, boil, filter. To fil. add HC1, 
 boil, evap. to dryness. Try to dis. 
 in boiling HC1, then in boiling 
 NaOH sol. The SiO 2 may also be 
 tested with CaF 2 and H 2 S0 4 in a 
 leaden dish (v. Exp. 28). 
 
 H 4 Si0 4 (gelat., white) formed. 
 Heat reduces to Si0 2 , insol. 
 in HC1; partially sol. in 
 NaOH sol. 
 
 K 4 Si0 4 , Na 4 Si0 4 , M 2 O (M 2 C0 3 ) 
 are formed. First two are 
 sep. by H 2 O, and changed by 
 HC1 to H 4 SiO 4 , and by heat 
 to SiO 2 (gritty); insol. in 
 HC1, slightly sol. in NaOH. 
 
 Supplementary. Silicates are insol., except those of the alkalies, which 
 are somewhat soluble. Some are dis. by acids, but many are not. SiO 2 is 
 insol., even in acids (except HF), and is also infusible in the blow-pipe flame, 
 but is fusible in the oxyhydrogen flame. There are two varieties of silica, the 
 amorphous and the crystalline. The former is sol. in NaOH or Na 2 CO 3 , the 
 latter not. In a bead of Na 2 C0 3 at very high temperature, B.B., SiO 2 and all 
 silicates fuse to a clear glass. They will not fuse in a bead of HNaAmPO 4 . 
 The best fusing mixture contains about half each of Na 2 C0 3 and K 2 C0 3 , the 
 mixture melting at a lower temperature than either alone. Test Si0 3 . 
 

98. FERROCYANIDS, H&FeCy* 
 
 TESTS. 
 
 RESULTS. 
 
 1. Ferrous test. 
 
 Add to the sol. acidi- 
 fied with HC1 a few 
 drops of FeS0 4 sol. 
 
 2. Ferric test. 
 
 Add to the sol. FeCl 3 sol. 
 
 3. Copper test. 
 
 Add to sol. CuS0 4 sol. 
 
 4. Silver test. 
 
 Add to sol. AgNO 3 sol. 
 
 White K 2 Fe 2 Cye ppts., changing quickly 
 to blue. Darkens by oxidation. 
 
 Prussian blue, Fe 4 Fe 3 Cyi 8 , ppts., sol. in 
 H 2 Ox (not HC1) to dark-blue liquid. 
 NaOH changes to red-brown Fe(OH) 3 . 
 
 Cu 2 Fe 2 Cy 6 (chocolate) ppts., insol. in HAc. 
 
 White Ag 4 Fe 2 Cy 6 ppts. , insol. in HNO 3 or 
 AmOH. Heated with HN0 3 the ppt. 
 forms Ag 3 Fe 2 Cye (orange-red), sol. in 
 AmOH. 
 
 Supplementary. Ferrocyanids are mostly insol., except those of the alkalies 
 and alkaline earths (Ba slightly). Ferrocyanids represent ferrous compounds, 
 ferricyanids are from ferric salts. The most important of the former is 
 K4FeCy, "yellow prussiate of potash." Make several ferrocyanids by the 
 following table. 
 
 GENERAL REACTIONS. 
 
 
 RH-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMABKS. 
 
 1 
 
 A1C1, 
 
 FeCy 2 +Al(OH) 8 
 
 white 
 
 NaOH 
 
 Forms slowly. 
 
 2 
 
 SbCl, 
 
 Sb 4 Fe 3 Cyi 8 
 
 u 
 
 u 
 
 
 3 
 
 Bid, 
 
 BuFesCyis 
 
 (( 
 
 u 
 
 
 4 
 
 CdCl, 
 
 Cd,FeCy 6 
 
 (( 
 
 HC1, NaOH 
 
 
 5 
 
 CaCl, 
 
 EsGaFeCye 
 
 u 
 
 NaOH 
 
 
 6 
 
 CoCl, 
 
 CosFeCye 
 
 green 
 
 (t 
 
 Becomes grad. gray. 
 
 7 
 
 CuCl, 
 
 CugFeCye 
 
 red-brown 
 
 u 
 
 
 8 
 
 FeS0 4 
 
 EsFeFeCye 
 
 white-blue 
 
 u 
 
 Rapidly changes from 
 
 
 
 
 
 
 white to blue. 
 
 9 
 
 FeCls 
 
 K4Fe s Cyi8 
 
 blue 
 
 u 
 
 
 10 
 
 Pb(N0 3 ) 2 
 
 Pb,FeCy6 
 
 white 
 
 (4 
 
 
 11 
 
 MgCl 2 
 
 AmjMgFeCye 
 
 
 
 U 
 
 With ammonium salts. 
 
 12 
 
 MnCl, 
 
 Mn 2 FeCy 6 
 
 u 
 
 NaOH, HC1 
 
 
 13 
 
 HgN0 3 
 
 Hg 4 FeCy 6 
 
 u 
 
 NaOH 
 
 
 14 
 
 Hg(N0 3 )2 
 
 Hg 2 FeCy 6 
 
 It 
 
 u 
 
 Changes to HgCy 2 and 
 
 
 
 
 
 
 Fe 3 Fe 2 Cyi2 (blue). 
 
 15 
 
 NiCl 2 
 
 NiaFeCye 
 
 green-white 
 
 u 
 
 
 16 
 
 AgN0 8 
 
 Ag 4 FeCy 6 
 
 white 
 
 u 
 
 Changes to blue. 
 
 17 
 
 ZnClc 
 
 Zn 2 FeCy 
 
 u 
 
 
 
srn 
 
 ^ t- 
 
 ^ 
 
 SITT. 
 
. FEBBICYANIDS, 
 
 TESTS. 
 
 RESULTS. 
 
 1. Ferrous test. 
 
 Add to some of the sol. 
 FeSO 4 sol. 
 
 2. Ferric test, 
 
 Add to some of the orig. 
 sol. FeCl 3 sol. Dilute 
 if necessary. 
 
 3. Copper test. 
 
 Add to some of the orig. 
 sol. CuSO 4 sol. 
 
 4. Silver test. 
 
 Add to some of the orig. 
 sol. AgNO 3 sol. 
 
 5. Zinc test, 
 
 Add to some of the orig. 
 sol. ZnCl 2 sol. 
 
 Turnbull's blue, Fe 3 Fe 2 Cyi 2 ppts. insol. in 
 acids. NaOH decolorizes it. 
 
 No ppt., but dark-green to brown color- 
 ation. 
 
 Yellow-green 
 HC1. 
 
 ppte., insol. in 
 
 Orange Ag 3 Fe 2 Cy 6 ppts., sol. in AmOH, 
 not in HN0 3 . 
 
 Orange Zn 3 Fe 2 Cyi 2 ppts., sol. in HC1 or 
 AmOH. 
 
 Supplementary. Ferricyanids are mostly insol., except those of alkalies 
 and alkaline earths. Alcohol does not ppt. the ferricyanid of Na or K from 
 sol. , and this also dist. it from the ferrocyanid. Make the test. K 3 FeCy was 
 formerly called red prussiate of potash. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 AgN0 3 
 
 AgsFeCye 
 
 red-brown 
 
 AmOH 
 
 
 2 
 
 Bid 
 
 BiFeCye 
 
 brown 
 
 
 
 3 
 
 CdCl 2 
 
 CdsFe 2 Cyi 2 
 
 yellow 
 
 AmOH, HC1 
 
 
 4 
 
 CoCla 
 
 Co 3 Fe 2 Cyi 2 
 
 red-brown 
 
 AmOH 
 
 Blood-red sol. with 
 
 
 
 
 
 
 AmOH and AmCl. 
 
 5 
 
 Cud; 
 
 CusFezCyw 
 
 yellow-green 
 
 
 
 6 
 
 FeS0 4 
 
 Fe 3 Fe 2 Cyi 2 
 
 dark-blue 
 
 
 
 7 
 
 Fed-, 
 
 none 
 
 
 
 Green to brown color. 
 
 8 
 
 Pb(NOs)* 
 
 uncertain 
 
 dark-brown 
 
 
 In cone. sols. only. 
 
 9 
 
 MnCl 2 
 
 Mn3Fe 2 Cyi2 
 
 brown 
 
 
 
 10 
 
 HgNOs 
 
 uncertain 
 
 red-brown 
 
 
 Turns white eventually. 
 
 11 
 
 Hg(N0 3 ) 2 
 
 none 
 
 
 
 (V. M4FeCy 6 .) 
 
 12 
 
 NiCl 2 
 
 NisFezCy^ 
 
 yellow-green 
 
 
 
 13 
 
 ZnCls 
 
 ZmFezCyw 
 
 orange 
 
 AmOH, HC1 
 
 (V. M 4 FeCy 6 .) 
 
1OO. SULFATES, M,SO 4 . 
 
 TESTS. 
 
 RB80LTS. 
 
 1. Barium test. 
 
 To a little of the sol. add BaCl 2 sol, 
 decant, and to the res. add dil. HC1. 
 
 2. Coin test (v. M 2 S, M 2 S0 8 , M 2 S 2 O 3 ). 
 
 Fuse some of the solid B.B.C.C. (r.f.) 
 with a mixture of Na 2 C0 3 . Place 
 the product on a silver coin with a 
 drop of water. 
 
 3. Insoluble sul fates. 
 
 Fuse 1 part of the solid with 2 parts 
 each of K 2 CO 3 and NaC0 3 (in Pt 
 crucible, if no Ag, Pb, or S is pres- 
 ent). Dis. what of the product will 
 dis. in H 2 O, the rest, separately, 
 in HC1. Test the former for SO 4 , 
 the latter for M. 
 
 4. Free H 2 S0 4 , 
 
 (1) Put a drop on paper, and evap. it 
 
 high above a flame, or over a water- 
 bath. 
 
 (2) Put a few drops on sugar in an e.d. 
 
 and evap. over a water-bath. 
 
 (3) Evap. some H 2 S0 4 nearly to dryness, 
 
 and add a little C 2 H 5 OH. 
 
 BaSO* ppts. , which is insol. in 
 HC1. 
 
 is formed, which dis. in 
 H 2 O and forms black Ag*S 
 with Ag. 
 
 K 3 S0 4 , NaaS0 4 , M 2 CO C are 
 formed. The first two are 
 sol. in H 2 O, the last in HC1. 
 The former contains the 
 radical, the latter the metal 
 of the original. 
 
 The paper is pulped, rotted, or 
 
 charred. Comp. with HC1, 
 
 HN0 3 . 
 Greenish -black substance is 
 
 formed. 
 
 is liberated, which burns 
 
 with a luminous flame. 
 
 Supplementary. In the barium test use dil. HC1 unless considerable 
 water is present for strong HC1 dis. a little BaS0 4 , and also ppts. BaClj from 
 sol. What sulfates are insol.? (a) Prepare some PbSO 4 , and test it as aboT 
 in 3. (b) Show that PbSO 4 exists in commercial H 2 S04 by diluting some witk 
 its vol. of water, (c) Make CuS0 4 , and test it. (d) Test NasSOs for trace* of 
 Na^S O 4 . Are most sulfates sol. or insol. ? 
 
 GENERAL REACTIONS. 
 
 
 KE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 Bad, 
 
 BaSO< 
 
 white 
 
 400,000 pts. H,0 
 
 The only salt of Ba (exc. 
 
 
 
 
 
 
 BaSLFe) insol. in dil. HC1. 
 
 2 
 
 Pb(NOs), 
 
 PbSO* 
 
 u 
 
 NaOH, Am Ac 
 
 C 2 H 5 OH aids ppn. 
 
 3 
 
 SrCl 2 
 
 8rSO 
 
 t( 
 
 7000 pts. H 2 
 
 Ppts. slowly in dil. sol. 
 
 4 
 
 CaCl, 
 
 CaS0 4 
 
 (( 
 
 400 pts. H 2 
 
 No ppt. in weak sol. 
 
1O1. CHKOMATES, M 2 CrO 4 . 
 
 TESTS. 
 
 RESULTS. 
 
 1. Borax bead test. 
 
 Make a bead of Na2B 4 O 7 or 
 HNaNH4P0 4 with Ft wire, dip 
 into sol., fuse in either flame. 
 
 2. Ppn. tests. 
 
 Apply the first three tests below 
 (General Reactions). 
 
 3. Hydrogen diozid test. 
 
 Acidulate the sol. with H 2 SO 4 , and 
 add a few drops of dil. H 2 O 2 sol. 
 Then add ether, and shake. This 
 will detect 1 part of chromate hi 
 40,000 of water. 
 
 Glass, yellow-green when hot, 
 emerald-green when cold. 
 
 A blue compound is formed 
 of uncertain composition, 
 which the ether dis. and car- 
 ries to the surface as a blue 
 liquid. 
 
 Supplementary. Most chromates are yellow, dichroinates are red. 
 Bichromates are confined to the alkali metals. K 2 Cr 2 O 7 , etc., ppt. normal 
 chromates, e.g. PbCrO 4 , BaCrO 4 from sol. Pb and Ba salts. In both the 
 normal and the dichromates Cr is a hexad, in ic salts it is a triad, in ous salts a 
 dyad. What other salts are yellow ? Acids change chromates to dichromates, 
 alkalies reverse this. Reducing agents (nascent H, SO 2 , H 2 S) change Cr to 
 Cr'" chromate to chromic salts. 
 
 GENERAL REACTIONS. 
 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 1 
 
 Bad, 
 
 BaCrO, 
 
 yellow 
 
 Dil. acids 
 
 
 2 
 
 Pb(N03) 2 
 
 PbCrO* 
 
 it 
 
 (HN0 3 (sl.), 
 f NaOH (si.) 
 
 Insol. in HAc. 
 
 8 
 
 AgN0 3 
 
 Ag 2 Cr0 4 
 
 dark-red {f^n^' 
 
 
 4 
 
 HgN0 3 
 
 Hg 2 Cr0 4 
 
 " i HN0 8 (8l.) 
 
 Ppt. ignited equals Cr 2 Og, 
 
 
 
 
 
 
 Hg, 0. 
 
 5 
 
 HgCl 2 
 
 HgCr04 
 
 orange 
 
 " 
 
 
 6 
 
 Bid, 
 
 BiiCCrCWs 
 
 yellow 
 
 " 
 
 
 7 
 
 CdCl t 
 
 CdCrO* 
 
 u 
 
 " 
 
 
 8 
 
 Acids 
 
 M 2 Cr 2 07 
 
 red sol. 
 
 
 Changed back by alkalies 
 
 
 
 
 
 
 to M 2 Cr0 4 (yellow). 
 
 9 
 
 H 2 S+HC1 
 
 S+CrCls 
 
 green sol. 
 
 
 Warming forms S0 2 , ppts. 
 
 
 
 
 
 
 Cr 2 O 2 Cr0 4 (brown). 
 
 10 
 
 Am,S 
 
 Cr(OH) s 
 
 green 
 
 Acids 
 
 
 11 
 
 CAOH+Hd 
 
 Crds 
 
 tt 
 
 
 On boiling. Odor of al- 
 
 
 
 
 
 
 dehyde. 
 
102. PHOSPHATES, 
 
 TESTS. 
 
 RESULTS. 
 
 1. Molybdate test. 
 
 To 1 or 2 cc. of sol. add a drop or 
 two of HN0 3 , then add 3 or 4 cc. 
 Am 2 Mo04 sol. , and let stand. 
 
 2. Magnesium sulfate test (v. As, Mg). 
 
 To sol. add AmCl sol. , AmOH, MgS0 4 
 sol., gently warm, stir, let stand. 
 
 3. Iron test. 
 
 To sol. add a drop of HAc, excess of 
 NaAc sol., and 1 or 2 drops of 
 FeCl 8 sol. 
 
 4. Cobalt test (v. SiO 2 , Al). 
 
 Heat the solid B.B.C.C., then on 
 white infusible mass put a drop of 
 CoCl 2 [or Co(N0 3 ) 2 ] sol., and heat 
 again. 
 
 5. Silver nitrate test. 
 
 To sol. add AgNO 3 sol. 
 
 Am 3 P04.12Mo0 8 (var., yel.) 
 ppts., sol. in M 8 PO 4 (ex.) or 
 in AmOH. 
 
 AmMgPO 4 (white, crystalline) 
 ppts. 
 
 FePO 4 (yellowish-white, gel.) 
 ppts., sol. in FeCl 8 (ex.). 
 
 Residue becomes blue. 
 
 Ag 3 P0 4 (yellow) ppte., sol. in 
 HN0 3 . 
 
 Supplementary. All phosphates are insoluble except those of the alkali 
 metals ; hence sols, of the other metallic salts ppt. phosphates. Most phosphates 
 are somewhat sol. in HC1. If insol. in H 2 0, they should be dis. in dil. HC1, 
 Am Ac (made from AmOH and HAc) added, then FeCl 3 till all the phosphate 
 is ppd. The fil. will now contain a chlorid of the original metal. This test 
 applies specially to phosphates of Ba, Sr, Ca, Mg. (a) Apply the test to each, 
 (b) Test bone-dust in this way. (c) Test samples of fertilizers. Phosphates (and 
 also oxalates) of Ba, Sr, Ca, Mg, if present, may ppt. with Fe, Cr, Al by AmOH. 
 To separate them dis. the ppt. in hot dil. HN0 3 , cool and add excess NaOH sol., 
 which ppts. only Fe and the phosphates (or oxalates). Dis. the ppt. in HNO, 
 add H 2 Tr and AmO H, which in excess ppts. the phosphates and oxalates, die- 
 solving the Fe. (For arseniates and arsenites, v. Exp. 58.) 
 
 GENERAL REACTIONS. 
 
 1 
 
 2 
 3 
 4 
 
 5 
 6 
 
 7 
 
 RE-AGT. 
 
 PPT. 
 
 COLOR. 
 
 SOLVENTS. 
 
 REMARKS. 
 
 Co(N0 8 ) 2 
 NiCl 2 
 BiCL 
 Cn(N0 8 ) 2 
 HgNOs 
 Hg(NOs) 2 
 Bad, 
 
 C03(P0 4 ) 2 
 Ni3(P0 4 ) 2 
 BiP0 4 
 Cus(P<>4) 2 
 HgsPO* 
 Hg 8 (P04) 
 Ba,(PO) I 
 
 red 
 
 light-green 
 white 
 blue-white 
 white 
 (i 
 
 it 
 
 AmOH, acids 
 
 n i< 
 
 HC1 
 HAc 
 
 HNO 
 Acids, Am salts 
 Dil. HC1 
 
 Insol. in HNO,. 
 HgCl 2 gives no ppt. 
 
|o 
 
 pipoi 
 
 pnnojg 
 
 r 
 
 
 
 B* ^"aT 
 
 Sflfe 
 
 S*||1 
 jj|g'S!ajJ 
 
 II II II II II II 
 
 iff 
 
 il 
 
 ..S c-^5o-r 
 
TABLE B. Tube Reactions. 
 
 Put into a small i.t. (or a bulb tube) a little of the powder, and heat it. 
 liefer the results to this table. 
 
 GASES. 
 
 SUBLIMATE, ETC. 
 
 FU- 
 SION. 
 
 RESIDUE. 
 
 INDICATION. 
 
 Red-brown, NO, 
 
 
 
 
 MNO MNO, 
 
 Yellow-gr. (rare) 
 
 
 
 
 
 Cl 
 
 
 
 
 (MCI) 
 
 Red, Br 
 
 
 
 
 MBr 
 
 Violet, I Black 
 
 
 
 MI 
 
 Odor, NH 3 ; HC1 
 
 
 
 
 tests White 
 
 
 
 NH, 
 
 Odor,SO,;K,Cr 2 7 
 
 
 
 M,S0 4 , M 2 SO S> 
 
 test 
 
 
 
 M,S 2 0:: 
 
 Odor,H,S; PbAc, 
 
 
 
 
 test Yel.-red, brown drops 
 
 X 
 
 
 MsS 
 
 Odor, Cy (flame 
 
 
 
 
 crimson) 
 
 
 
 
 (MCy) 
 
 CO 2 ; Ca(OH) a test 
 
 
 
 
 M,C0 3 , M,0x 
 
 CO (flame blue) 
 
 
 
 
 M 8 0x 
 
 O (splinter test) 
 
 
 
 
 MC10 3 , MNO,, 
 
 
 
 
 
 MO, 
 
 NjO " 
 
 
 X 
 
 All finally vaporizes 
 
 AmNO 
 
 
 Hot : yellow. Cold : 
 
 
 
 
 
 white 
 
 
 
 HgCl 
 
 ; White 
 
 X 
 
 
 HgCU 
 
 White, As 4 O Cryst. Heat and C = 
 
 
 
 
 (odor) mirror 
 
 
 
 AfcOe 
 
 White, needles 
 
 X 
 
 
 Sb,0, 
 
 O (splinter test) 
 
 Metallic Hg 
 
 
 Black, changing to red 
 
 HgO 
 
 
 Yel.-red-brown drops 
 
 X 
 
 
 8 
 
 Hot : red. Cool : yel. 
 
 
 
 As,Ss 
 
 
 Red when rubbed 
 
 
 
 HgI 2 
 
 
 Gray; white if rubbed 
 
 
 
 Hg 
 
 
 Black; red if rubbed 
 
 
 
 HgS 
 
 
 
 
 Black, tarry, burnt su- 
 
 
 
 
 
 gar odor 
 
 M 8 Tr 
 
 Heavy white 
 
 White cryst. 
 
 
 
 H,0x 
 
 
 
 
 Black; odor acetone 
 
 MAc 
 
 
 
 
 Hot: red-brown. Cold: 
 
 
 
 
 
 light yellow 
 
 Bi 2 s 
 
 
 
 
 Hot: black. Cold: red 
 
 Fe 2 8 
 
 
 
 
 Hot: red-brown. Cold: 
 
 
 
 
 
 yellow 
 
 PbO 
 
 
 
 
 Hot:yel.-brown. Cold: 
 
 
 
 
 
 yellow 
 
 SnO, 
 
 
 
 
 Hot: yel. Cold: white 
 
 ZnO 
 
 
 
 
 M 2 C0 8 , (M 2 0), (M) 
 
 Org. cpds.ofNa, 
 
 
 
 
 
 K,Am,Ba,Sr, 
 
 
 
 
 
 Ca,Mg 
 
 
 
 X 
 
 No decomposition 
 
 Cpds. of alka- 
 
 
 
 
 
 lies, + Cl, NO 3 
 
 
 
 
 
 cpds. of alk. 
 
 
 
 
 
 earths 
 
TABLE C. Action with H 2 SO 4 . 
 
 Tut a little of the powder into a t.t., and add a few drops of H-jSO*. Ualess 
 yiolent action ensues (as with K Cl O 8 ) heat it, and observe especially the gas. 
 
 OOIOB OF GAS. 
 
 ODOR. 
 
 REFERENCE. 
 
 REMARKS. 
 
 GAS. 
 
 INDICATION. 
 
 Violet 
 
 None 
 
 Exp. 92 
 
 Dark crystal, sub- 
 
 I 
 
 MI 
 
 
 
 
 limate. 
 
 
 
 Yellow 
 
 CIO, 
 
 " 84 
 
 Substance deto- 
 
 
 
 
 
 
 nates violently. 
 
 C10 2 
 
 MC10, 
 
 Red-brown 
 
 NO, 
 
 " 82, 83 
 
 
 N0 2 , N 2 3 
 
 MNO,,MNOo 
 
 Eed 
 
 Br 
 
 " 91 
 
 
 Br 
 
 MBr 
 
 None 
 
 HC1 
 
 " 90 
 
 
 HC1 
 
 MCI 
 
 ti 
 
 Stifling 
 
 " 89 
 
 Etches glass. 
 
 HF 
 
 MF 
 
 
 
 H,S 
 
 " 86 
 
 In tube open at both 
 
 
 
 
 
 
 ends gives SO 2 . 
 
 H,S 
 
 M,S 
 
 White 
 
 SO, 
 
 " 87 
 
 S not liberated. 
 
 SO, 
 
 M 2 S0 8 
 
 ti 
 
 ({ 
 
 " 88 
 
 S is liberated. 
 
 a 
 
 M,S,0, 
 
 None 
 
 HAc 
 
 " 93 
 
 
 HAc 
 
 MAc 
 
 
 
 HCy 
 
 " 94 
 
 
 HCy 
 
 MCy 
 
 K 
 
 CO 
 
 "' 96 
 
 
 CO 
 
 M 2 0x 
 
 
 
 None 
 
 " 10, 101 
 
 Kindles splinter. 
 
 
 
 MO,, M,Cr0 4 
 
 ti 
 
 K 
 
 " 85 
 
 White ppt. with 
 
 
 
 
 
 
 lime water. 
 
 CO, 
 
 M,CO, 
 
TABLE D. Heat on Charcoal (B.B.C.C.), 
 
 With the round end of the forceps make a slight depression in a piece of 
 harcoal, and put in a little of the powdered substance. With a mouth blow- 
 pipe blow the flame against it, cautiously at first, afterwards strongly. 
 
 RESULTS. 
 
 INDICATIONS. 
 
 1. Substance melts and runs into the coal. 
 
 3. Leaves white, infusible residue. 
 
 Add to this a drop of CoCl 2 sol. , and heat again. 
 The color may be : 
 Blue, 
 Green, 
 Pink. 
 
 S. Coats charcoal : 
 
 White, volatile, garlic odor, no globule. 
 44 " hard, brittle globule. 
 
 14 when cool, yellow when hot, no globule. 
 44 " " " " " globule malle- 
 
 able, but difficultly formed. 
 
 Yellow, globule easily formed, fusible, soft, malle- 
 able. 
 
 Yellow (orange when hot), globule hard, brittle. 
 
 Brown or red, no globule. 
 
 4. Deflagrates. 
 
 5. Volatilizes. 
 
 0. Gives odor. 
 
 Choking (SO*). 
 Garlic. 
 
 Salts of the alka- 
 lies, and some 
 alkaline earths 
 
 Al, 810., 
 
 Zn 
 
 Mg 
 
 As 
 Sb 
 Zn 
 
 Sn 
 
 Pb 
 Bi 
 Cd 
 
 MC10,, MNO, 
 Am 
 
 8 or M t S 
 As 
 
TABLE E. 
 Heat on Charcoal with Na2CO 8 (B.B.C.C., 
 
 Blow the inner flame (r.f.) for some time against a mixture of the powdered 
 substance, and dry, fine NaaCOs, using charcoal, as in Table D. 
 
 METALLIC I 
 GLOBULE. 
 
 No 
 GLOBULE. 
 
 INFUSIBLE 
 POWDER. | 
 
 COLORED ! 
 MASS. 
 
 SOLID RESIDUE. 
 
 INCRUSTATION. 
 
 INDICATION. 
 
 X 
 
 
 
 
 White, brilliant, malleable, 
 
 In strong o.f. red-brown. 
 
 Ag 
 
 
 
 
 
 non-oxidizable. 
 
 
 
 X 
 
 
 
 
 Hard, brilliant, oxidizable, 
 
 B.B. volatile. Hot, orange; 
 
 
 
 
 
 
 reddish-white. 
 
 cold, lemon-yellow. 
 
 Bi 
 
 X 
 
 
 
 
 Red, malleable ; oxidizes to 
 
 
 
 
 
 
 
 black ; green flame. 
 
 
 Cu 
 
 X 
 
 
 
 
 Easily formed, fusible, mal- 
 
 Hot, lemon-yellow ; cold, 
 
 
 
 
 
 
 leable, oxidizes to yel. 
 
 sulfur-yellow; vol. B.B. ; 
 
 
 
 
 
 
 
 O flame blue. 
 
 Pb 
 
 X 
 
 
 
 
 White, malleable, difficultly 
 
 Hot, yellow; cold, white 
 
 
 
 
 
 
 formed, easily oxidized. 
 
 near assay; non-vol. 
 
 Sn 
 
 
 X 
 
 
 
 
 White, volatile; light-blue 
 
 
 
 
 
 
 
 flame ; garlic odor. 
 
 As 
 
 
 X 
 
 
 
 
 Red-brown (like peacock 
 
 
 
 
 
 
 
 feather) ; vol. B.B, 
 
 Cd 
 
 X 
 
 (x) 
 
 
 
 White, brittle, oxidizable. 
 
 Hot, yel. ; cold, blue-white; 
 
 
 
 
 
 
 
 vol. B.B. pale green. 
 
 Sb 
 
 
 X 
 
 
 
 
 Hot, yellow; cold, white. 
 
 
 
 
 
 
 
 With Co(N0 8 ) 2 green. 
 
 Zn 
 
 
 
 X 
 
 
 Infusible magnetic powder, 
 white, gray, black. 
 
 
 Fe 
 
 
 
 X 
 
 
 It It tt it It 
 
 
 Co 
 
 
 
 X 
 
 
 tt It It It tt 
 
 
 Ni 
 
 
 
 
 X 
 
 Yellow mass. 
 
 
 Cr 
 
 
 
 
 x Green " 
 
 
 Mn 
 
TABLE F. Flame Reactions. 
 
 Fuse one end of a Pt wire into a short glass tube. Hold the wire in the 
 outer edge of a Bunsen flame till the latter loses the yellow color at first 
 imparted. Moisten the wire with H 2 O or HC1, and dip it into a little of the 
 salt, then hold it again in the flame, noting the color. Clean the wire with H Cl 
 and the flame. 
 
 FLAME COLOR. 
 
 REMARKS. 
 
 INDICATION. 
 
 1. Violet 
 
 Seen through blue glass looks red- 
 
 
 
 violet ; otherwise Na obscures it. 
 
 E 
 
 2. Bluish 
 
 
 As 
 
 3. Blue 
 
 
 Pb 
 
 4. Blue-green 
 
 Moistened with H 2 S0 4 . 
 
 M 3 P0 4 
 
 5. 
 
 First blue, then green. 
 
 Cu, espec. CuCl 2 
 
 6. Yellow-green 
 
 Moistened with H 2 S0 4 . 
 
 MsB0 3 
 
 7. 
 
 " HC1. 
 
 Ba 
 
 8. Greenish 
 
 Very slight color. 
 
 Sb 
 
 9. Bronze-green 
 
 " evanescent. 
 
 MNO- 
 
 10. Orange-yellow 
 
 Blue glass obscures the color. 
 
 Na 
 
 11. Orange-red 
 
 Obscured by Ba. 
 
 Ca 
 
 12. Crimson 
 
 " " " 
 
 Sr 
 
 TABLE G. Bead Reactions. 
 
 Make a loop in the end of a Pt wire (Fig. 38, Exp. 45), moisten and dip it 
 into some powdered borax, then hold it in the flame ; repeat till you have a 
 glass bead filling the loop. Test a weak sol. (or the smallest bit of powder) by 
 bringing the bead in contact with it, then blowing the flame against it with a 
 blowpipe. 
 
 OXIDIZING FLAME (o.f., outer). 
 
 REDUCING FLAME (r.f., inner). 
 
 
 
 
 INDI- 
 
 
 
 
 
 CATION. 
 
 Hot. 
 
 Co/d. 
 
 Hot. 
 
 Cold. 
 
 
 Blue 
 
 Blue 
 
 Blue 
 
 Blue 
 
 Co 
 
 Yellow-red 
 
 Green 
 
 Green 
 
 Green 
 
 Cr 
 
 Green 
 
 Blue-green 
 
 Colorless 
 
 Red-brown 
 
 Cu 
 
 Yellow-red 
 Violet 
 
 Yellow 
 Violet 
 
 Bottle-green 
 Colorless 
 
 Bottle-green 
 Colorless 
 
 Fe 
 Mn 
 
 l( 
 
 Red-brown 
 
 Gray, cloudy 
 
 Gray, cloudy 
 
 Ni 
 
 
 
 
 
 
TABLE H. Acil Radicals Resume. 
 
 SALTS. 
 
 f 
 
 w 
 
 BaCl 2 +HCl. 
 
 s 
 
 AgNO 8 +HNO 8 . 
 
 OTHER RE-AGENTS AND RESULTS. 
 
 For further explanation, v. Exps. 81-102. Abbrevi- 
 ations : b. black, bl. blue, br. brown, ch. chocolate, 
 d. dark, g. green, 1. light, o. orange, r. red, v. violet, 
 w. white, y. yellow. 
 
 M 2 S0 4 
 
 w. 
 
 W. 
 
 (w.) 
 
 
 Pb(N0 3 ) 2 : w. SrCl 2 : w. B.B.C.C. with Na 2 C0 3 
 
 
 
 
 
 
 on Ag: b. 
 
 M 2 S0 3 
 
 w. 
 
 
 w. 
 
 
 BaCl 2 + HC1 + Cl : BaS0 4 . HC1 : S0 2 [odor, 
 
 
 
 
 
 
 K 2 Cr 2 7 : g.]. 
 
 M 2 S 2 3 
 
 w. 
 
 
 w. 
 
 
 BaCl 2 +HCl: S. HC1: S+S0 2 [odor, KoO 2 O 7 : g.]. 
 
 M 2 C0 3 
 
 w. 
 
 
 w. 
 
 
 HC1: C0 2 [Ca(OH) 2 : w.]. Heat: (M 2 O, CO 2 ).^ ' 
 
 M 2 Cr0 4 
 
 i-y. 
 
 
 d.-r. 
 
 
 Pb(N0 3 ) 2 : y. HgN0 3 : d.-r. HgClo: o. BiCl 3 : y. 
 
 
 
 
 
 
 Cd(NO 3 ) 2 : y. H 2 S: y. Acids: r, which y. by alk. 
 
 M 3 POi 
 
 w. 
 
 
 i-y. 
 
 
 AmCl+AmOH+MgS0 4 : w. HN0 3 +Am 2 MoO 4 : 
 
 
 
 
 
 
 y. B.B.C.C. +Co(N0 3 ) 2 :bl. 
 
 M 3 As0 4 
 
 w. 
 
 
 ch.- 
 
 
 H 2 S, warm : y. AmCl + AmOH -f MgS0 4 : w. 
 
 
 
 
 br. 
 
 
 B.B.C.C.: As [garlic odor, white fumes]. 
 
 M 3 As0 3 
 
 w. 
 
 
 y.-w. 
 
 
 H 2 S+HCl:y. CuS0 4 (neutral): g. K 2 Cr0 4 +heat: 
 
 
 
 
 
 
 g. KMnO 4 : decol. C.C. + heat, t.t. : mirror. 
 
 M 3 B0 3 
 
 w. 
 
 
 w. 
 
 
 H 2 SO 4 , Pt wire: green flame. Turmeric paper + 
 
 
 
 
 
 
 H 3 B0 3 : br. H 2 SO 4 + C 2 H 5 OH : green flame. 
 
 M,0x 
 
 w. 
 
 
 w. 
 
 
 SrCl 2 : w. CaCl 2 : w. [sol. in HC1, insol. in HAc]. 
 
 
 
 
 
 
 Heat: CO, CO 2 , M 2 C0 3 , M 2 O or M, no char- 
 
 
 
 
 
 
 ring. H 2 SO 4 : effervesc., CO 2 . 
 
 M 2 Tr 
 
 w. 
 
 
 w. 
 
 
 CaCl 2 : w. [sol. in NaOH]. KC1: w. Heat: chars 
 
 M: ; SiO, 
 
 w. 
 
 
 i-y. 
 
 
 [odor]. AgN0 3 +AmOH: Ag mirror. 
 HCl+heat: Si0 2 . Na 2 C0 3 bead: effervesc., forms 
 
 
 
 
 
 
 glass. HNaAmP0 4 bead: insol. B.B.C.C.+ 
 
 
 
 
 
 
 HC1, evap. : SiO 2 , sol. in NaOH. 
 
 MN0 2 
 
 w. 
 
 
 w. 
 
 
 H 2 S0 4 : N0 2 . HAc+KMn0 4 : decol. HAc + 
 
 
 
 
 
 
 AgN0 3 : w. HAc +KI+ starch: bl. 
 
 MF 
 
 w. 
 
 
 
 
 H 2 S0 4 +heat: etches glass, makes H 2 turbid. 
 
 
 
 
 
 
 HKS0 4 + heat : green flame. 
 
 MCI 
 
 
 
 w. 
 
 W. 
 
 H 2 S0 4 : HC1. H 2 SO 4 +Mn0 2 : Cl. AgNX) 3 : w. 
 
 
 
 
 
 
 [sol. in AmOH, action of light]. Pb(N0 3 ) 2 : w. 
 
 MBr 
 
 
 
 y.-w. 
 
 y.-w. 
 
 PbAc 2 : w. CS 2 + Cl : y. H 2 S0 4 + Mn0 2 : Br 
 
 
 
 
 
 
 [starch, KI+ starch]. 
 
 MI 
 
 
 
 y.-w. 
 
 y.-w. 
 
 Pb(N0 3 ) 2 : y. HgN0 3 : y.-g. HgCl 2 : y.-r. CS 2 + 
 
 
 
 
 
 
 Cl : v. H 2 SO 4 + MnO 2 : I [starch test] . 
 
 MCy 
 
 
 
 y.-w. 
 
 y.-w. 
 
 CuS0 4 : y.-g. Co(N0 3 ) 2 : w.-br. NiClo : y.-g. 
 H 2 S0 4 : HCy [odor cautiously]. KOH+FeSO 4 
 
 
 
 
 
 
 + HCl:bl. 
 
 M,S 
 
 
 
 b. 
 
 b. 
 
 HC1: H 2 S [odor, PbAc 2 ]. B.B.C.C. on Ag: b. 
 
 M 4 FeCyo 
 
 
 
 w. 
 
 g-br 
 
 FeCl 3 : bl. FeS0 4 : bl.-w. CuSO 4 : br.-r. 
 
 M 3 FeCv fi 
 
 
 
 0. 
 
 o. 
 
 FeCl 3 : r.-br. CuSO 4 : g.-y. 
 
 MN0 3 
 
 
 
 
 
 Heat,i.t.:O,NO 2 . B.B.C.C.: deflagrates. H 2 S0 4 : 
 
 
 
 
 
 
 N0 2 . FeS0 4 +H 2 SO 4 : r.-br. H 2 S0 4 + indigo 
 
 
 
 
 
 
 sol.: decol. 
 
 MC10: 
 
 
 
 
 
 HCl+heat: g.-y. Heat, i.t. : O. H 2 S0 4 (very lit- 
 
 
 
 
 
 
 tle) : C1 2 4 [y. gas] . 
 
 MAc 
 
 
 
 
 
 Heat: blackens [odor]. H 2 S0 4 : HAc [odor]. 
 
 
 
 
 
 
 H 2 SO 4 + C 2 H 5 OH : C 2 H 5 Ac [odor]. FeCl 3 , 
 
 
 
 
 
 
 boil: r. 
 
TABLE I. Acid Radicals. 
 
 Arranged according to convenient method of detection. 
 
 1. Flame { H 3 B0 3 (M 3 B0 3 +H 2 S0 4 ). 
 
 f (with heat) { MN0 3 . 
 
 2. Gas J (with acid) { MN0 2 , MC10 3 , M 2 C0 3 , M 2 S, M 2 S0 3 , M 2 S 2 3 . 
 
 i (with heat and acid) { MF, MCI, MBr, MI, MAc, MCy. 
 
 o -a^ P j (with heat) { M 2 Tr, M 2 0x, 
 
 e ) (with heat and acid) { M 4 Si0 4 (M 2 Si0 3 ). 
 
 f (iron-cyanids) { M 4 FeCy 6 , M 3 FeCy 6 . 
 4. Precipitate 1 (insoluble) { M 2 S0 4 . 
 
 L (unclassed) { M 2 Cr0 4 , M 3 P0 4 , M 3 As0 4 , M 3 As0 3 . 
 
 COMPLETE ANALYSIS. 
 
 In making a complete analysis, i. e. analysis for the metal and acid radical, 
 the following order should be observed, and the pupil should begin with only 
 a single substance, such as Pb(N0 3 ) 2 , FeCl 3 , etc., and should make a careful 
 record under each head. 
 
 1. External properties: Color, luster, form (crystalline or amorphous), taste, 
 odor, deliquescent, efflorescent, etc. 
 
 2. Heat in glass tube (v. Table B). 
 
 3. Heat with H 2 S0 4 (v. Table C). 
 
 4. Heat B.B.C.C, (v. Table D). 
 
 5. Heat B.B.C.C. NaaCO-j (r.f.) (v. Table E). 
 
 6. Apply flame test (v. Table F). 
 
 7. Apply Borax bead test (v. Table G). 
 
 8. Test solubility (v. Table A). 
 
 9. Test for Metals (aqueous analysis) (v. Exps. 48-80). 
 
 10. Test for Acid radicals (v. Tables H, I). 
 
 11. State conclusion as to composition. 
 
UNIVERSITY OF CALIFORNIA LIBRARY 
 BERKELEY 
 
 Return to desk from which borrowed. 
 This book is DUE on the last date stamped below. 
 
 < 2 1948 
 23May'58 D 
 
 
 100m-9,'47(A5702sl6)476