Elementary 
 
 Inorganic and Organic. 
 
 HEWITT and POPE 
 
 LONDON: WHJTTAKER & CO. 
 
GIFT OF 
 
 . W.B, memo 
 

 ELEMENTARY 
 PRACTICAL CHEMISTRY. 
 
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ELEMENTARY 
 PRACTICAL CHEMISTRY. 
 
 INORGANIC AND ORGANIC. 
 
 BY 
 
 J. T. HEWITT, M.A., D.Sc., Ph.D., F.C.S., 
 
 Professor of Chemistry ; 
 AND 
 
 F. G. POPE, 
 
 Assistant Lecturer and Demonstrator in the 
 People s Palace Technical Schools. 
 
 fanban: 
 WHITTAKER AND CO., PATERNOSTER SQUARE, E.C. 
 
 NEW YORK: 66, FIFTH AVENUE. 
 
PREFACE 
 
 THIS small work on qualitative analysis is in- 
 tended to supply a text-book for students work- 
 ing according to the syllabus of the elementary 
 stage of Practical Inorganic and Organic Chem- 
 istry. The substances for which tests are given 
 are those contained in the new syllabus (1894), 
 but it is hoped that the methods given for 
 their detection and separation are such that the 
 student will have nothing to unlearn when he 
 proceeds to a more advanced course of qualita- 
 tive analysis. 
 
 Directions are given in the making up of 
 reagents for students who are working without 
 the aid of a teacher. 
 
 Objection may be taken by some to the way 
 in which it is recommended that results should 
 be stated, but the authors find after several 
 years practical experience in laboratory teach- 
 ing, that this method leads to clearness of 
 expression, and the rapid examination of a 
 student's work. 
 
 J. T. H. 
 
 Chemical Laboratory, F. G. P. 
 
 People's Palace, E. 
 
 237571 
 
HINTS FOR LABORATORY WORK. 
 
 IT is necessary that all apparatus should be 
 kept scrupulously clean, as good results cannot 
 be expected if dirty apparatus is used. 
 
 Reagent bottles should be replaced on the 
 shelves directly after use, and the stoppers 
 should on no account be mixed. 
 
 Write down the results observed as soon as 
 an experiment is made : it is hard to remember 
 all the work done when an analysis is finished. 
 Do not leave out an account of an experiment 
 because it has yielded a negative result. 
 
 Before systematic analysis is begun, 'pre- 
 liminary tests should be made. 
 
 Distilled water should always be used both 
 for making up reagents and for analytical pur- 
 poses. 
 
 Silver and platinum residues should not be 
 thrown away, but put into separate stock-bottles 
 for recovery. 
 
 Students should practise using small quantities 
 of substance and reagents, as much time is 
 wasted in having large quantities to filter. 
 
 Equations should be given wherever possible, 
 to illustrate the reactions that occur. 
 
 For the method of stating the results of an 
 analysis, see the sample analyses given at the 
 end of the analytical tables. 
 
'ELEMENTARY -'PRACTICAL CHEMISTRY. 
 
 REACTIONS OF THE METALS. 
 
 Lead Dry reaction. Heated on charcoal in 
 the reducing flame, lead compounds give a bead 
 of the metal. This is malleable, and marks 
 paper. 
 
 Wet reactions.- Use a solution of lead nitrate 
 Pb (NO,)* 
 
 Hydrochloric acid gives a white precipitate 
 (PbCL). 
 
 Pb(N0 3 ) 2 + 2HC1 = PbCl 2 + 2HN0 3 . 
 
 The precipitate is soluble in boiling water, 
 and crystallizes out again on cooling. 
 
 Hydrogen sulphide gives a black precipitate of 
 lead sulphide (PbS). 
 
 Pb(NO 3 ) 2 + H 2 S = PbS + 2 HNO 3 . 
 
 In presence of much HC1 the precipitate may 
 be red. If so, dilute and pass more gas. 
 
 Sulphuric acid precipitates white lead sulphate 
 (PbS0 4 ). 
 
 Pb(NO 3 ) 2 + H 2 SO 4 = PbSO 4 + 2 HNO 3 . 
 
 Potassium chromate gives a yellow precipitate 
 of yellow lead chromate (PbCrO 4 ). 
 
 Pb(NO 3 ) 2 + K 2 CrO 4 = PbCrO 4 + 2KNO 3 . 
 
 Potassium iodide precipitates yellow lead 
 iodide (PbI 2 ). 
 
 Pb(NO 3 ) 2 + 2KI = PbI 2 + 2 KNO 3 . 
 
REACTIONS OF THE METALS. 7 
 
 The precipitate dissolves in much boiling 
 water, and separates as yellow scales on cooling. 
 
 Mercury. The salts of mercury are of two 
 sorts : mercurous salts, corresponding to mer- 
 curous oxide HgoO ; and mercuric salts, cor- 
 responding to mercuric oxide HgO. The w_t 
 reactions of these two series of salts differ. 
 
 Dry reactions. Mercury salts volatilize when 
 heated on charcoal in the blowpipe flame. 
 
 Heated with sodium carbonate in a dry tube, 
 a mirror of metallic mercury is formed. 
 
 Wet reactions Mercurous salts. Use a so- 
 lution of mercurous nitrate (HgNO 3 ). 
 
 Hydrochloric acid gives a white precipitate of 
 mercurous chloride (calomel). 
 
 HgNO 3 + HC1 = HgCl + HNO 3 . 
 
 The precipitate is insoluble in boiling water, 
 and turned black by ammonia. 
 
 2 HgCl + 2NH 3 = NH 4 C1 + NH a Hg 2 Cl. 
 
 Mercuric salts. Use a solution of mercuric 
 chloride (HgCl., ; corrosive sublimate). 
 
 \Note. Mercuric chloride, unlike mercurous 
 chloride, is soluble in water ; hence mercuric 
 salts are not precipitated by addition of hydro- 
 chloric acid.] 
 
 Hydrogen Sulphide gives a grayish ppt, 
 passing through yellow to black mercuric sul- 
 phide (HgS). 
 
 HgCL, + H 2 S = HgS + 2HC1. 
 
5 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 This precipitate does not dissolve in hot 
 dilute nitric acid ; but if boiled with HC1 and 
 Bromine-water, a solution of HgCL is obtained. 
 
 Copper turnings become coated with a white 
 shining deposit of metallic mercury. 
 
 Potassium iodide gives a red precipitate of 
 mercuric iodide (HgL). 
 
 HgCl 3 + 2KI = HgI 2 4-2KCl. 
 
 This precipitate is soluble in excess of po- 
 tassium iodide. 
 
 HgI 2 + 2 KI = K 2 HgI 4 . 
 
 Soda and potash precipitate yellow mercuric 
 oxide. 
 
 HgCl 2 + 2 KOH = HgO + H 2 O + 2KC1. 
 
 Ammonia gives a white precipitate. 
 HgCl 2 + 2 NH 3 = NH 2 HgCl + NH 4 C1. 
 
 Stannous chloride gives a precipitate at first 
 white (HgCl), then turning gray (Hg). 
 
 2 HgCl 2 + SnCl 2 = 2 HgCl + SnCl 4 . 
 2HgCl + SnCl 2 = 2Hg + SnCl 4 . 
 
 Aluminium Dry reaction. Aluminium com- 
 pounds heated on charcoal in the oxidizing 
 flame yield a white mass of the oxide. If 
 this is moistened with cobalt nitrate solution 
 (Co(NO 8 )jj) and again heated, a blue mass is 
 produced. 
 
REACTIONS OF THE METALS. 9 
 
 Wet reactions. Use a solution of potash 
 alum, K 2 SO 4 . A1 2 (SO 4 ) 3 . 2 4 H 2 O. 
 
 Ammonia gives a white gelatinous precipitate 
 of aluminium hydroxide, A1(OH) 3 , insoluble in 
 excess. 
 
 A1 2 (SO 4 ) 3 + 6NH 4 OH = 2 A1(OH) 3 + 3(NH 4 ) 2 S0 4 . 
 
 Soda and potash give a similar precipitate, 
 soluble in excess. 
 
 A1(OH) 3 + 3 NaOH = Al(ONa), + sH 2 O. 
 
 The alkaline solution gives a precipitate of 
 A1(OH) 3 on boiling with ammonium chloride. 
 
 Al(ONa) 3 + 3 NH 4 C1-A1(OH), + sNaCl + 3 NH 3 . 
 
 Calcium Dry Reaction. Calcium salts 
 moistened with hydrochloric acid impart an 
 orange colour to the Bunsen flame. 
 
 Wet reactions. Use a solution of calcium 
 chloride, CaCl 2 . 
 
 Ammonium Carbonate gives a white precipi- 
 tate of calcium carbonate, CaCO 3 . 
 
 CaCl 2 + (NH 4 ) 2 CO 3 = CaCO 3 + 2 NH 4 C1. 
 
 Ammonium Oxalate precipitates white calcium 
 oxalate, CaC 2 O 4 . 
 
 CaCL + (NH 4 ) 2 C 2 O 4 = CaC 2 O 4 + 2NH 4 C1. 
 
 Sulphuric acid gives a precipitate of calcium 
 sulphate, CaSO 4 , in strong solutions, if, however 
 the solution be dilute, the precipitate will not 
 
10 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 appear, as calcium sulphate is slightly soluble 
 in water. 
 
 CaCLj + H,,SO 4 = CaSO 4 + 2HC1. 
 
 Magnesium Dry reaction. Heated before 
 the blowpipe, magnesium salts leave a white 
 residue of magnesium oxide, MgO. If this is 
 treated with a drop of cobalt nitrate solution 
 and again heated in the oxidizing flame a pink 
 mass is obtained. 
 
 Wet reactions. Use a solution of magnesium 
 sulphate, MgSO 4 . 
 
 The solution will give precipitates with ammo- 
 nium hydroxide and carbonate if ammonium 
 chloride is not present. If, however, ammonium 
 chloride be present, the double chloride of 
 ammonium and magnesium (2NH 4 C1, MgCL) 
 is formed, which gives no precipitate with these 
 reagents. 
 
 \N.B. In this way calcium and magnesium 
 may be separated. Mix solutions of calcium 
 and magnesium chlorides, add ammonium chlor- 
 ide, and then ammonia and ammonium carbon- 
 ate. The white precipitate will consist of calcium 
 carbonate, the magnesium remains in the solu- 
 tion.] 
 
 Caustic potash and soda produce white pre- 
 cipitates of magnesium hydroxide, Mg(OH) 2 . 
 
 MgS0 4 + 2KOH - Mg(OH) 2 + K 2 SO 4 . 
 
 The precipitate is soluble in ammonium 
 chloride ; magnesium hydroxide will not be 
 
REACTIONS OF THE METALS. II 
 
 thrown down if ammonium chloride is present 
 in the original solution. 
 
 Sodium phosphate added to a solution of a 
 magnesium salt which contains ammonium 
 chloride and ammonia gives a white crystalline 
 precipitate of magnesium ammonium phosphate. 
 
 MgSO 4 + Na,HPO 4 + NH 4 OH = Mg(NH 4 )PO 4 + 
 Na. 2 SO 4 
 
 Potassium Dry reaction. Potassium salt:> 
 colour the Bunsen flame violet. Lead salts 
 communicate a blueish violet colour to the flame, 
 hence, if lead salts are present, potassium must 
 be looked for in the residue left on ignition, 
 and not in the original mixture (see Table F). 
 
 Wet reactions. Use a solution of potassium 
 chloride, KC1. 
 
 Platinum chloride gives a yellow crystalline 
 precipitate of potassium chlorplatinate, K 2 PtCl (; 
 (the solution must not be too dilute). 
 
 Fluosilicic acid gives a white gelatinous pre- 
 cipitate of potassium fluosilicate, K 2 SiF 6 . 
 
 2 KC1 + H 3 SiF 6 = K 2 SiF 6 + 2 HC1. 
 
 Tartaric acid precipitates acid potassium tar- 
 trate from a fairly concentrated solution of a 
 potassium salt. 
 
 KC1 4- H 2 . C 4 H 4 O 6 = KH. C 4 H 4 O 6 + HC1. 
 
12 ELEMENTARY PRACTICAL CHEMISTRY 
 
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14 ELEMENTARY PRACTICAL CHEMISTRY. 
 
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 -SEPARATION OF THE 
 if possible if not, in i 
 ous chloride (Table B 
 ie well-cooled solution 
 the washings to the filt 
 
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REACTIONS OF THE METALS. 
 
 TABLE B. 
 
 The precipitate obtained by the addition of 
 HC1 may contain PbCL, and HgCl (Group I. 
 ppt). These chlorides may be separated by 
 treatment with boiling water ; the PbCl 2 dis- 
 solves, and the solution is filtered from the 
 insoluble HgCl. 
 
 The insoluble residue on 
 the filter consists of HgCl. 
 Confirm its composition by 
 adding ammonia, when it 
 will turn black from forma- 
 tion of NH 2 Hg 2 CL 
 
 Divide hot filtrate into three 
 parts. 
 
 (a) To one part add 
 K 2 CrO 4 . An immediate yel- 
 low ppt. consists of PbCrO 4 . 
 
 (b) Add KI to another 
 portion, and allow to cool. 
 PbI 2 separates in glistening 
 yellow scales on cooling. 
 
 (c) Cool and add HsSC^ ; 
 a white ppt. of PbSO 4 is 
 formed. 
 
 TABLE C. 
 
 The black ppt. obtained by the action of 
 may be tested for Pb and Hg(ic) in' the 
 following way. It is boiled with dilute HNCX, 
 which dissolves the PbS, forming Pb(NO 3 ) 2 ; 
 whilst HgS is not dissolved by this treatment. 
 Filter and wash. 
 
 To confirm the presence of 
 Hg in the residue, dissolve 
 it in HC1, with addition of a 
 little bromine-water ; boil off 
 the excess of Br,* and add a 
 solution of SnCl 2 . A ppt., 
 at first white (HgCl), then 
 turning gray (Hg), indicates 
 the presence of Hg. 
 
 Evaporate the filtrate to a 
 small bulk ; cool, and add a 
 few drops of dilute sulphuric 
 acid. A white ppt. of PbSO 4 
 indicates the presence of Pb. 
 Confirm the presence of Pb 
 by heating some of the orig- 
 inal substance on charcoal 
 in the reducing flame a 
 malleable metallic bead 
 should be obtained. 
 
 * The excess of bromine must be carefully removed, or the stan- 
 nous chloride will be oxidized at the expense of the Br, and not by 
 the HgClo ; hence a ppt. of HgCl and Hg will not be obtained. 
 
1 6 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 TABLE D. 
 
 The ppt. obtained by addition of NH 4 C1, 
 NH 4 OH, and (NH 4 ),S, consists of A1(OH) 3 . 
 Note that it is the ammonia which effects the 
 precipitation, not the (NH 4 ) 3 S.* To confirm 
 the presence of Al, dissolve the ppt. in the least 
 possible quantity of dilute HC1, add NaOH in 
 slight excess, and then NH 4 C1, and boil. A 
 white gelatinous ppt. of A1(OH) 3 indicates the 
 presence of Al. 
 
 TABLE E. 
 
 The ppt. obtained by addition of (NH 4 XCO 3 
 consists of CaCO 3 . The calcium may be con- 
 firmed by dissolving a portion of the ppt. in HC1, 
 adding NH 4 C1, NH 4 OH, and (NH 4 ) 2 C 2 O 4 . A 
 white ppt. of CaC 2 O 4 is produced. 
 
 Another portion of the ppt. should be moist- 
 ened with HC1, and heated on wire in the 
 Bunsen flame the flame is coloured orange. 
 
 TABLE F. 
 
 The filtrate from the calcium ppt. contains 
 magnesium and potassium. Divide into two 
 parts. 
 
 To one part add Na 2 HPO 
 
 warm, and allow to stand. 
 A white cryst. ppt. ( Mg( N H 4 ) 
 PO 4 ) indicates Mg. 
 
 Evaporate the other por- 
 tion to dryness ; ignite to 
 expel ammonium salts, and 
 test the residue (if any), after 
 moistening with HC1 by the 
 flame test. 
 
 Violet flame = K. 
 
 * A ppt. will be obtained in this group, even if Al is not 
 present, if the metals Pb and Hg have not been completely 
 removed by H 2 S. 
 
REACTIONS OF THE COMMON ACIDS. IJ 
 
 THE REACTIONS OF THE 
 COMMON ACIDS. 
 
 H 2 CO 3 H.SO4 HNO 3 HC1. 
 
 These acids may be divided into four different 
 groups, viz.: 
 
 Group I. The acid precipitated by barium 
 chloride, but having its barium salt insoluble 
 in acid solution Sulphuric acid. 
 
 Group II. The acid precipitated from its 
 neutral solution by barium chloride, the 
 barium salt being insoluble in water Car- 
 bonic acid. 
 
 Group III. The acid precipitated by silver 
 nitrate, its silver salt being insoluble in dilute 
 HNO 3 Hydrochloric acid. 
 
 Group IV. The acid whose salts are all solu- 
 ble in water, and which, therefore, is not 
 precipitated by any reagent Nitric acid. 
 
 Reactions of Acid in Group I. 
 
 SULPHURIC ACID, H 2 SO 4 . 
 
 Sulphates are precipitated by barium chloride 
 in the presence of hydrochloric acid, as insoluble 
 barium sulphate. 
 
 Tests. i. Dry sulphates heated with solid 
 Na. 2 CO 3 on charcoal in the reducing flame are 
 converted into sodium sulphide, which when 
 
 B 
 
iS ELEMENTARY PRACTICAL CHEMISTRY. 
 
 placed on a silver coin and moistened with 
 water, gives a black stain (i.e., the silver is 
 converted into black silver sulphide, Ag 2 S). 
 
 2. Soluble sulphates give with 
 
 (A) Barium chloride or nitrate, a white precipi- 
 tate of barium sulphate (BaSO 4 ) insoluble in 
 hydrochloric acid, nitric acid, and ammonia. 
 
 BaCl 2 + H 2 SO 4 = BaSO 4 + 2HC1. 
 
 (B) Lead acetate gives a white precipitate of 
 lead sulphate, soluble in ammonium acetate. 
 
 Pb(C 2 H 3 2 ) 2 + H 2 S0 4 = PbS0 4 + 2 HC 2 H 3 O 2 . 
 
 Reactions of Acid in Group II. 
 
 CARBONIC ACID, H 2 CO 3 . 
 
 Carbonates are precipitated by barium chloride 
 in a neutral solution as insoluble barium car- 
 bonate. 
 
 Na 2 CO 3 + BaCl 2 = BaCO 3 + 2NaCl. 
 
 Tests. i. The addition of acids (e.g., HC1, 
 HNO 3 ) gives an evolution of carbonic acid gas 
 (CO 2 ), which on passing through lime-water 
 turns it milky, owing to formation of calcium 
 carbonate. 
 
 C0 2 + CaH 2 2 = CaC0 3 + H 2 O. 
 
 2. Barium chloride gives in neutral solutions 
 a white precipitate of barium carbonate, soluble 
 in dilute acids with effervescence. 
 
REACTIONS OF THE COMMON ACIDS. 1 9 
 
 Reactions of Acid in Group III. 
 
 HYDROCHLORIC ACID, HC1. 
 
 Chlorides are precipitated by silver nitrate as 
 insoluble silver chloride, e.g. 
 
 Nad + AgNO 3 = AgCl + NaNO,. 
 
 Tests. i. Dry chlorides on treating with 
 strong sulphuric acid evolve hydrochloric acid 
 gas, which turns blue litmus red, and gives 
 dense white fumes of ammonium chloride in 
 the presence of strong ammonia. 
 
 2. Dry chlorides heated with sulphuric acid 
 and potassium bichromate evolve chlorine, which 
 can be recognised by its smell, and by its bleach- 
 ing of moist red litmus paper. 
 
 3. Solutions of chlorides give with silver ni- 
 trate a white precipitate of silver chloride, 
 soluble in ammonia, and reprecipitated on- the 
 addition of excess of nitric acid. 
 
 4. Solutions of chlorides give with mercurous 
 nitrate a white precipitate of calomel, which is 
 turned blaek on the addition of ammonia. 
 
 Reactions of Acid in Group IV. 
 
 NITRIC ACID, HNO 3 . 
 
 This acid is not precipitated by any reagent, 
 as all its salts are soluble. 
 
 Tests. i. Solid nitrates evolve oxygen when 
 heated, and some evolve brown nitrous fumes as 
 well. The oxygen may be tested with a glowing 
 splinter. 
 
20 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 2. Solid nitrates heated with strong sulphuric 
 acid, an equal bulk of water, and a piece of 
 copper, give nitric oxide, turning brown on 
 exposure to the air. 
 
 3Cu + 8HNO 3 = 3Cu(NO 3 ) 2 + 2 NO + 4H 2 O. 
 
 3. Add to the dry substance some strong 
 sulphuric acid and mix well. Cool and add 
 carefully a cold solution of ferrous sulphate. If 
 nitric acid be present, a black ring is formed at 
 the junction of the two liquids. 
 
 [The H 2 SO 4 first liberates HNO 3 . Then the 
 nitric acid is reduced by some of the ferrous 
 sulphate to nitric oxide, which cannot escape 
 except by passing through the excess of ferrous 
 sulphate ; in this it dissolves, forming the black 
 compound. 
 
 TABLE G. 
 DETECTION OF ACIDS. 
 
 Test separate portions of the original sub- 
 stance for chlorides, nitrates, sulphates, and 
 carbonates, as follows : 
 
 (A) To the original substance add dilute HNO 3 . 
 Effervescence without smell, with a white 
 precipitate formed on passing the gas into 
 lime-water, indicates a carbonate. 
 
 (B) To the original substance add strong H 2 SO 4 , 
 cool and add a solution of FeSO 4 , a black 
 
REACTIONS OF THE COMMON ACIDS. 21 
 
 ring at the junction of the two liquids indi- 
 cates a nitrate. Confirm by warming the 
 original substance with sulphuric acid and 
 a strip of metallic copper. Brown fumes 
 evolved. 
 
 (C) Dissolve the original substance in HC1 
 (filter if a precipitate is formed), and add 
 BaCL. A white precipitate insoluble in HC1 
 and HNO 3 indicates a sulphate. Confirm 
 by dry test. 
 
 (D) Dissolve the original substance in HNO 3 , 
 and add AgNO 3 . A white precipitate soluble 
 in NH 4 OH indicates a chloride. Confirm by 
 the preliminary tests. 
 
 Reactions of Organic Compounds. 
 METHYL ALCOHOL, CH 3 OH. 
 
 1. Heat with soda lime and it is converted 
 into formic acid. 
 
 2. Distil over zinc-dust and it yields CO and H. 
 
 CH,OH = CO + 2H a . 
 
 3. Heat with sodium acetate and strong sul- 
 phuric acid and it yields methyl acetate. 
 
 CH 3 OH + CH 3 COONa + H 2 SO 4 = 
 CH 3 COOCH 3 + NaHSO 4 + H 2 O. 
 
 ETHYL ALCOHOL, C 2 H 5 OH. 
 
 i. Heat with K,Cr 2 O 7 and H.SO 4 and alde- 
 hyde is evolved. 
 
 C 2 H 5 OH + O = CH 3 CHO + H 2 O. 
 
22 ELEiMENTARY PRACTICAL CHEMISTRY. 
 
 2. Add KHO, a strong solution of I in KI, 
 till faint brown colour is produced, and then a 
 drop or two of KHO till colour is destroyed, 
 boil, and a yellow ppt. of iodoform (CHI 3 ) falls. 
 
 3. Heat with sodium acetate and strong sul- 
 phuric acid it yields ethyl acetate. 
 
 C 2 H 5 OH + CH 3 COONa + H 2 SO 4 = 
 CH 3 COOC 2 H 5 + H 2 O + H 2 SO 4 . 
 
 GLYCERIN, QH 5 (OH) 3 . 
 
 i. Evaporate to small bulk and heat with dry 
 KHSO 4 , and acrolein is evolved, recognised by 
 its sharp and penetrating smell. 
 
 FORMIC ACID, HCOOH. 
 
 1. Solid formates heated with strong H 2 SO 4 
 evolve CO, which burns with a blue flame, form- 
 ing CO 2 . No charring takes place. 
 
 HCOOH = H 2 + CO. 
 
 2. To a solution of a formate add FeCl 3 , a 
 deep brown red colour is formed, and, on boil- 
 ing, a reddish ppt. of basic ferric formate is 
 formed. 
 
 3. AgNO 3 in strong neutral solutions gives a 
 white ppt. of silver formate, which is decom- 
 posed on warming, with the deposition of metallic 
 silver on the tube. 
 
 AgNO 3 + NaCHO 2 = AgCHO 2 + NaNO 3 . 
 2AgCHO, = HCOoH + 2 Ag + CO 2 . 
 
REACTIONS OF THE COMMON ACIDS. 23 
 
 4. HgCl 2 gives a white ppt. of HgCl, which 
 on heating is decomposed, and Hg is deposited 
 as a black powder. 
 
 HCOOH + 2HgCl 2 = 2HgCl + 2HC1 + CCX. 
 HCOOH + 2HgCl = 2Hg + 2HC1 + CO 2 . 
 
 5. A solution of KMnO 4 is at once decolor- 
 ized by a formate. 
 
 ACETIC ACID, CH 3 CO,H. 
 
 1. Solid acetates heated with H 2 SO 4 give off 
 acetic acid, recognised by its smell. 
 
 2. Solid acetates heated with strong H 2 SO 4 
 and a drop or two of absolute alcohol give off 
 ethyl acetate. 
 
 CH 3 COONa + C 2 H 5 OH + H 2 S0 4 = 
 CH 3 COOC 2 H 5 + NaHSO 4 + H 2 O. 
 
 3. FeCl 3 in strong solutions gives a red color- 
 ation, which, on boiling, forms a deep brown 
 red ppt. of basic ferric acetate, 
 
 [The normal acetate, Fe(C 2 H 3 O 2 )3, is first 
 formed, and this is decomposed on boiling by 
 the excess of water, thus : 
 
 2HC.H.O,.] 
 
 4. AgNO 3 gives a white ppt. of AgC 2 H 3 O 2 , 
 not decomposed on boiling. 
 
 AgN0 3 + QH 3 2 Na = AgC 2 H 3 O 2 + NaNO 3 . 
 
 OXALIC ACID COOH. 
 COOH. 
 
 i. Solid oxalates on heating with strong 
 
24 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 H 2 SO 4 evolve CO and CO,, and do not 
 char. 
 
 2. CaCl 2 in neutral solutions gives a white 
 ppt. of CaC 2 O 4 , readily soluble in HC1. 
 
 Na 2 C 2 4 + CaCl 2 = 2 NaCl + CaC 2 O 4 . 
 
 3. AgNO 3 gives a white ppt of Ag 2 C 2 O 4 , 
 soluble in acids and ammonia. 
 
 Na 2 C 2 O 4 + 2 AgNO 3 = 2NaNO 3 + Ag 2 C 2 O 4 . 
 
 TARTARIC ACID, CH(OH)CO 2 H. 
 CH(OH)CO 2 H. 
 
 1. Solid tartrates, on heating in a tube, blacken 
 and give off a smell of burnt sugar. 
 
 2. Solid tartrates, heated with strong H 2 SO 4 , 
 blacken and evolve CO and CO 2 . 
 
 3. CaCl 2 in neutral solutions gives a white 
 ppt. of CaC 4 H 4 O 6 , soluble in HC1 ; also in cold 
 strong KHO, but repptd. on boiling. 
 
 Na 2 C 4 H 4 O 6 + CaCl 2 = 2NaCl + CaC 4 H 4 O 6 . 
 
 4. AgNO 3 in neutral solutions gives a white 
 ppt. of Ag 2 C 4 H 4 O 6 . If this ppt. be washed and 
 dissolved in the least possible quantity of 
 NH 4 OH and the solution warmed, Ag will be 
 deposited on the tube. 
 
 2 AgNO 3 + Na 2 C 4 H 4 O 6 - 2 NaNO 3 + Ag 2 C 4 H 4 O 6 . 
 
 5. KC1 in presence of a little alcohol gives a 
 white ppt. of KHC 4 H 4 O 6 . 
 
 KC1 + C 4 H 4 O 6 = KHC 4 H 4 O 6 + HC1. 
 
REACTIONS OF THE COMMON ACIDS. 25 
 
 6. Tartrates with a strongly alkaline solution 
 of KMnO 4 give a pink colouration, which on 
 boiling forms a brown ppt. 
 
 CITRIC ACID, CH 2 . COOH. 
 COH. COOH. 
 CH 2 . COOH. 
 
 1. Solid citrates on heating blacken and give 
 off unpleasant fumes. 
 
 2. Solid citrates on heating with strong 
 H 2 SO 4 , evolve CO, then blacken, evolving CO 2 , 
 acetone, &c. 
 
 3. CaCl 2 in neutral solutions gives a white 
 ppt. of Ca 3 (C 6 H 5 O 7 ) 2 on boiling. 
 
 3CaCl 2 + 2Na 3 C 6 H 5 O 7 = 6NaCl + Ca 3 (C 6 H 5 O 7 ) 2 . 
 No ppt. is formed in the cold. 
 
 4. AgNO 3 gives a white ppt. of Ag 3 C 6 H 5 O 7 
 soluble in NH 4 OH, but it is not reduce'd on 
 heating. 
 
 3 AgN0 3 + Na 3 C 6 H 5 7 = Ag 3 C 6 H 5 O 7 + 3NaNO 3 . 
 
 5. Citrates boiled with a strongly alkaline 
 solution of KMnO 4 give a green coloration, but 
 no ppt. 
 
 SALICYLIC ACID, C 6 H 4 (OH)COOH. 
 
 1. Solid salicylates heated with CaO yield 
 phenol, recognised by smell. 
 
 C 6 H 4 OH COOH + CaO = C 6 H 5 OH + CaCO 3 . 
 
 2. FeCl 3 gives a deep purple coloration, even 
 in very dilute solutions. 
 
 3. Bromine- water gives a white ppt. 
 
26 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 Before proceeding with the systematic analysis, 
 the following preliminary tests should be made : 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 i. Heat a small 
 
 (A) Substance 
 
 Presence of a tar- 
 
 portion of the sub- 
 
 blackens, swells, 
 
 trate or citrate. 
 
 stance in a small 
 
 and gives odour of 
 
 
 dry tube. 
 
 burnt sugar. 
 
 
 
 (B) A white sub- 
 
 Presence of an 
 
 
 limate is formed. 
 
 oxalate. 
 
 
 (C) Smell of phe- 
 
 Presence of a sali- 
 
 
 nol.* 
 
 cylate. 
 
 2. Heat a small 
 
 (A)Noblackening 
 
 Absence of tar- 
 
 portion of sub- 
 
 after long heating. 
 
 trates and citrates. 
 
 stance in a dry tube 
 with strong H 2 SO 4 . 
 
 (B) Rapid effer- 
 vescence with char- 
 
 Presence of a tar- 
 
 
 ring, and CO, CO 2 , 
 
 trate or citrate. 
 
 
 and ultimately SO a f 
 
 
 
 given off. 
 
 
 
 (C) COJ only ev- 
 
 Presence of a 
 
 
 olved ; no charring. 
 
 formate. 
 
 
 (D)COandCOjJI 
 
 Presence of an 
 
 
 evolved; no char- 
 
 oxalate. 
 
 
 ring. 
 (E) Odour of 
 
 Presence of an 
 
 
 acetic acid ; no 
 
 acetate. 
 
 
 charring. 
 
 
 * Salicylic acid is decomposed on rapid heating, thus : 
 C 6 H 4 (OH)CO a H = C 6 H 5 OH + C0 2 . 
 
 t The carbon present acts on the sulphuric acid, reducing it, thus : 
 C + 2H-jSO 4 =-CO 2 + 2H 2 O + 2SO i . 
 
 I Formic acid is decomposed thus : 
 
 HC0 2 H = CO + H J O. 
 
 || Oxalic acid is decomposed thus : 
 
 If the substance given is a liquid, it should 
 
 be tested for methyl and ethyl alcohols and 
 
 glycerine in the following manner : 
 
 (A) Methyl and ethyl alcohols. Should the mix- 
 
 ture smell of alcohol, make it alkaline with 
 
 NaOH and distil a large portion, collect the 
 
REACTIONS OF THE COMMON ACIDS. 2J 
 
 distillate and redistil it over half its bulk of 
 freshly ignited K 2 CO 3 . Repeat the operation 
 and take first portion of distillate only. Now 
 note the boiling point of the liquid. 
 
 Methyl alcohol boils at 67C and ethyl 
 alcohol at 78C. 
 
 The liquid should give a smell of aldehyde 
 when heated with dilute H 2 SO 4 and K 2 Cr 2 O 7 . 
 (B) Glycerine. Evaporate liquid to small bulk 
 on water bath. A thick viscid liquid remains, 
 which on heating with dry KHSO 4 gives 
 pungent smell of acrolein. 
 
 C 3 H 5 (OH) 3 = C 3 H 4 + 2 H 2 0. 
 
 PREPARATION OF SOLUTION TO BE TESTED FOR 
 ORGANIC ACIDS. 
 
 I. Dissolve small portion of substance in a 
 little water if possible. If solution is neutral 
 and does not contain heavy metals (i.e., gives no 
 ppt. on treating portions with HC1, H 2 S and 
 Na 2 CO 3 ) it can be used at once for the detection 
 of the acids. 
 
 II. If substance does not dissolve in water or 
 if it contains heavy metals, dissolve it in HNO 3 , 
 add H 2 S, and if a ppt. is formed pass H 2 S in 
 excess and filter, boil filtrate to expel H 2 S and 
 add solid Na^COg till very alkaline, boil, and if 
 necessary, filter. To solution add litmus and 
 slight excess HNO 3 , boil off CO 2 , add ammonia 
 till slightly alkaline and boil till excess of ammo- 
 nia is expelled. Solution should now be neutral. 
 
 [H 2 S is added to ppt., AS and Sb, and 
 Na 2 CO 3 to remove all remaining metals, except 
 those of Group V.] 
 
28 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 SEPAR 
 
 bo 
 
 
 E II 
 
 I Ji 
 
 2 '8 
 
 ^ l 
 
 eutral 
 stand 
 
 II 
 
 O C 
 H rt 
 
 L- 
 
 QJ D 
 
 -E 
 
 1 1 
 
 & 
 
 4 
 
 
 
 ll 
 
 I 
 
 !* 
 ?1 
 
 E rt^; 
 
 fl? 
 
 
 aj JD 
 ij "o 
 
 O 'r^ i* 
 
 ^ IS 
 
 2P rt S 
 
 ^ ijtc 
 
 S 'o E 
 
 g a 
 
 ^c o 
 
 H.S ffl 
 
 .3* 
 
 2 
 h ^ 
 
 saafi, 
 
 cd rt c3 
 
REACTIONS OF THE COMMON ACIDS. 29 
 
 To TEST FOR FORMIC ACID. 
 
 (A) In absence of tartaric or citric acids. To 
 solution add strong AgNO 3 solution. A white 
 ppt. is formed which immediately blackens on 
 heating the solution, owing to reduction ~>f 
 AgN0 3 to Ag. 
 
 (B) In presence of tartaric and citric acids. 
 Distil a portion of the substance with dilute 
 H 2 SO 4 , stopping the distillation before black- 
 ening occurs.* Neutralize distillate and test 
 as above. 
 
 To TEST FOR ACETIC ACID. 
 
 (A) In absence of formic acid. To solution add 
 FeCl 3 a brown coloration, giving a dark 
 brown ppt. on boiling, indicates acetic acid. 
 
 (B) In presence of formic acid and alcohol. If 
 alcohol be present, boil it off. Add dilute 
 H 2 SO 4 and distil off the acetic and formic 
 acids, boil distillate for some minutes with an 
 equal bulk of a solution of K 2 Cr 2 O 7 , and 
 dilute H 2 SO 4 in a flask with reflux tube.t 
 Distil, neutralize distillate, cool and add FeCl 3 
 brown coloration and brown ppt. on boiling 
 indicates acetic acid. 
 
 * If distillation is carried too far SO. 2 might be evolved, 
 and a black ppt. would be formed with AgXO 3 . 
 
 t This destroys formic acid and does not act on acetic. 
 
30 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 Typical Analyses. 
 
 Inorganic Mixtures. 
 (A) The substance is a white powder. 
 
 PRELIMINARY EXAMINATION FOR METALS 
 AND ACIDS. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 i. Heat some of 
 
 A white sublimate. 
 
 Presence of an 
 
 substance in bulb 
 
 
 ammonium salt. 
 
 tube. 
 
 
 
 2. Mix with dry 
 
 No metallic mirror. 
 
 Absence of a mer- 
 
 Na 2 CO 3 , and heat 
 
 
 cury salt. 
 
 in bulb tube. 
 
 
 
 3. Mix substance 
 
 A malleable me- 
 
 Presence of a lead 
 
 with dry Na 2 CO 3 , 
 
 tallic bead formed. 
 
 salt. 
 
 and heat on char- 
 
 
 
 coal in reducing 
 
 
 
 flame. 
 
 
 
 4. Heat on char- 
 
 (a) Yellow in- 
 
 Presence of a lead 
 
 coal in oxidizing 
 
 crustation. 
 
 salt. 
 
 flame. 
 
 (b) Substance de- 
 
 Presence of a ni- 
 
 
 flagrates. 
 
 trate. 
 
 5. Heat substance 
 
 A bluish -violet 
 
 Presence of a po- 
 
 moistened with HC1 
 
 flame coloration. 
 
 tassium or lead salt. 
 
 in Bunsen flame. 
 
 
 
 6. Warm some of 
 
 NH 3 given off. 
 
 Presence of an 
 
 substance in a tube 
 
 
 ammonium salt. 
 
 with NaOH solu- 
 
 
 
 tion. 
 
 
 
 7. Heat some of 
 
 Brownish fumes 
 
 Presence of a ni- 
 
 substance in a tube 
 
 evolved. 
 
 trate. 
 
 with strong H 2 SO 4 . 
 
 
 
 8. Add dilute 
 
 No effervescence. 
 
 Absence of a car- 
 
 HC1 to original 
 
 
 bonate. 
 
 substance. 
 
 
 
REACTIONS OF THE COMMON ACIDS. 
 
 c 
 
 U, 
 
 
 2.w> 
 
 
 
 Z 
 
 
 |1 P 
 
 HH 
 
 C 
 
 
 o^" g 
 
 -a 
 
 o 
 
 
 1*1 o S 
 
 'rt 
 
 i 
 
 
 w l*l z l 
 
 C 
 
 C3 
 
 
 ^ 
 
 rt 
 
 
 
 
 = -^ 
 
 ^ 
 
 EC 
 
 
 / jj 
 
 fcfi 
 
 *o 
 
 
 a u 
 
 9 
 
 u) rX 
 
 
 T3 00 
 
 
 
 0.^5 
 
 
 
 1 
 </> 
 
 11 
 
 add a few drc 
 a little (NH 4 
 
 (NH 4 ) 2 C0 3 . 
 
 to 
 
 cS 
 
 $ 
 
 1 ^ 
 
 .TJ 
 
 *! 
 
 3 
 
 O W 
 
 | 
 
 l 
 
 ^ 
 
 6 2 
 
 y 
 
 rf 
 
 (fr Z 
 
 e l 
 
 Z | 
 
 1 
 
 3 i *- 
 
 3 
 
 "rt ^ &. 
 
 C/3 
 
 "^ o 
 
 >, 
 
 rt u "o -- 
 
 'in 
 
 fc'.S 3*3 
 
 d 
 
 
 0> 
 
 >r ^ ^ c "M 
 
 s 
 
 S *2 3i 
 
 1 
 
 rv G_i 
 
 a 
 
 1 
 
 o <u 
 
 t/3 
 
 
 ^ W 
 
 "5 T3 OJ -* 
 
 X! 
 
 <1 | 
 
 
 2 o 
 
32 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 EXAMINATION OF GROUP I. PPT. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Wash ppt. with 
 cold H 2 O, and boil 
 with H 2 0. 
 
 Divide solution 
 into three parts : 
 To(i)addK 2 Cr0 4 . 
 (2) M KI. 
 ,, (3) Cool, and 
 add dilute H 2 SO 4 . 
 
 Ppt. completely 
 dissolves. 
 
 A yellow ppt. 
 A yellow ppt. 
 A white ppt. 
 
 Presence of Pb. 
 
 Presence of Pb. 
 Presence of Pb. 
 Presence of Pb. 
 
 EXAMINATION OF GROUP II. PPT. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Boil ppt. with di- 
 lute HNO 3 . 
 
 Evaporate solu- 
 tion to small bulk, 
 cool, and add di- 
 lute H 2 S0 4 . 
 
 Ppt. completely 
 dissolves. 
 
 A white ppt. 
 
 Presence of lead ; 
 absence of Hg. 
 
 Presence of Pb. 
 
 TEST ORIGINAL SUBSTANCE FOR AMMONIA. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE.. 
 
 Boil with NaOH. 
 
 Ammonia gas 
 evolved ; recognised 
 by smell and by 
 giving dense white 
 fumes (of NH 4 C1), 
 when a rod moist- 
 ened with strong 
 HC1 is brought 
 near. 
 
 Presence of am- 
 monium. 
 
REACTIONS OF THE COMMON ACIDS. 
 
 33 
 
 TEST FOR ACID. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 To substance add 
 strong H9SO 4 ; cool, 
 and add ~FeSO 4 so- 
 lution. 
 
 A black ring 
 formed at junction. 
 
 Presence of a ni- 
 trate. 
 
 Boil substance Brown 
 with sulphuric acid evolved, 
 and a strip of cop- 
 per. 
 
 fumes Presence of a ni- 
 trate. 
 
 Substance contains, therefore, lead, am- 
 monium, and nitric acid ; and is, therefore, 
 probably a mixture of lead and ammonium 
 
 nitrates. 
 
 (B) The substance is a white powder. 
 
 PRELIMINARY EXAMINATION FOR METALS 
 AND ACIDS. 
 
 EXPERIMENT. OBSERVATION. INFERENCE. 
 
 i. Heat sub- 
 stance in dry tube. 
 
 No sublimate. 
 Xo smell of am- 
 monia. 
 No metallic mir- 
 ror. 
 
 Abs. of mercury 
 or ammonium salts. 
 Abs. of an am- 
 monium salt. 
 Abs. of a mercury 
 salt. 
 
 2. Heat with dry 
 Xa 2 CO 3 . 
 
 Xo metallic mir- 
 ror. 
 
 Abs. of a mercury 
 salt. 
 
34 
 
 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 PRELIMINARY EXAMINATION FOR METALS AND 
 ACIDS continued. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 3. Mix substance 
 with dry Na 2 CO 3 ; 
 heat on charcoal in 
 reducing flame. 
 
 4. Heat on char- 
 coal in oxidizing 
 flame. 
 
 Moisten white resi- 
 due with Co(NO 3 ) 2 , 
 and heat again. 
 
 5. Heat substance 
 moistened with HC1 
 in Bunsen flame. 
 
 6. Warm sub- 
 stance with NaOH 
 solution. 
 
 7. Heat substance 
 with strong H 2 SO 4 . 
 
 8. Add dilute HC1 
 to original sub- 
 stance. 
 
 (a) No metallic 
 bead. 
 
 ({>) Place residue 
 on a silver coin, 
 and moisten with 
 H 2 O. A black stain 
 on the silver. 
 
 No incrustation ; 
 white shining resi- 
 due. 
 
 No distinct co- 
 loration (i.e. , nei- 
 ther quite pink nor 
 quite blue). 
 
 No flame colora- 
 tion. 
 
 No NH 3 evolved. 
 
 No white fumes 
 evolved. 
 
 No brown fumes 
 evolved. 
 
 No effervescence. 
 
 Abs. of a lead 
 salt. 
 
 Presence of a sul- 
 phate. 
 
 Abs. of a lead 
 salt ; presence of 
 an aluminium, cal- 
 cium, or magnesium 
 salt. 
 
 (?) Presence of al- 
 uminium and mag- 
 nesium. 
 
 Abs. of potassium 
 and calcium salts. 
 
 Abs. of ammon- 
 ium salts. 
 
 Abs. of chlorides. 
 Abs. of nitrates. 
 
 Abs. of a carbon- 
 ate. 
 
REACTIONS OF THE COMMON ACIDS. 
 
 35 
 
 
 
 c 
 
 
 2 bfl 
 
 
 
 E 
 
 
 
 
 
 
 q 
 
 
 'S .J 
 
 
 
 E* 
 
 
 8.ffi ^*s 
 
 
 
 D 
 
 
 llj gd 
 
 
 
 
 
 o'S cj 
 
 ffi 
 
 
 | 
 
 
 
 
 2" bi 
 E ^ 
 
 rt 
 
 
 T3 
 C 
 
 - 
 
 1 s| 
 
 "c 
 
 
 ci 
 
 
 
 S i 
 
 rt 
 
 ^? 
 
 
 o^ 
 
 
 < ^s 
 
 
 
 * 
 
 1 
 
 ^ : 
 
 1 1 
 
 
 Ir 
 
 q 
 
 rt 
 
 
 
 13 o 
 
 
 > o 
 
 . 
 
 D. 
 
 G "S 
 
 
 53 < 
 
 
 
 ^c: 
 
 < 
 
 
 
 "rt 8 
 
 e 
 
 *0 
 
 | u 
 
 
 *.l 
 
 '~^ 
 
 G cj 
 
 
 te 
 
 fl 
 
 4-> rt 
 
 
 o I 
 
 
 (0 > 
 
 
 
 "%. S 
 
 (/) . 
 
 
 *| 
 
 ^S. 
 
 D 
 
 
 i\o 
 
 1 
 
 g 
 
 *a 
 
 "' "2 
 
 *tft 
 rt 
 
 | 
 
 Is 
 
 cu 
 
 cfl 
 
 
 ^"o 
 
 <u 
 
 cr; 
 
 o 
 
 *2 b/1 
 
 c 
 
 - *r^ 
 
 5 
 
 C/3 
 
 Xi 
 
 il 
 
36 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 EXAMINATION OF GROUP III. PPT. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Dissolve ppt. in 
 very small quantity 
 of dilute HC1, add 
 slight excess of 
 NaOH, and then 
 NH 4 C1, and boil. 
 Confirm ppt. by 
 heating on char- 
 coal, and moisten- 
 ing with Co(NO 3 ) 2 . 
 
 A white ppt. 
 A blue mass. 
 
 Presence of Al. 
 Confirms Al. 
 
 To CONFIRM Mg. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Heat ppt. on 
 charcoal moistened 
 with Co(NO 3 ). 2 . 
 
 A pink mass. 
 
 Presence of Mg. 
 
 TEST ORIGINAL SUBSTANCE FOR AMMONIUM. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Boil with NaOH. 
 
 No NH 8 evolved. 
 
 Abs. of NH 4 . 
 
 TEST FOR ACID. 
 
 EXPERIMENT. OBSERVATION. ; INFERENCE. 
 
 Dissolve sub- 
 stance in HC1, and 
 add BaCl 2 . 
 Confirm by dry 
 test. 
 
 A white ppt., in- 
 soluble in HC1 and 
 HN0 3 . 
 
 Presence of H 2 SO 4 . 
 
REACTIONS OF THE COMMON ACIDS. 
 
 37 
 
 Substance contains aluminium and magnesium 
 and sulphuric acid, and is therefore probably 
 a mixture of aluminium and magnesium sul- 
 phates. 
 
 Organic Mixtures. 
 
 (A) The substance is a white powder. 
 PRELIMINARY EXAMINATION. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Heat substance; Immediate black- Presence of a tar- 
 in a dry tube. cning and smell of trate or citrate, 
 burnt sugar. 
 
 Heat substance Rapid efferves- Presence of a tar- 
 vvith strong H 2 SO 4 . i cence.with charring trate or citrate, 
 and evolution of 
 CO, CO 2 , and ulti- ! 
 mately SO 2 . 
 
 Systematic Analysis. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 To a strong and 
 exactly neutral solu- 
 tion, free from heavy 
 metals, add CaCl 2 . 
 and allow to stand 
 for ten minutes. 
 
 Boil solution for 
 five minutes. 
 
 Filter, 
 FeCl 3 . 
 
 and add 
 
 No ppt. 
 
 White ppt. 
 
 Dark brown co- 
 loration and dark 
 brown ppt. on boil- 
 ing. 
 
 Absence of oxal- 
 ates and tartrates. 
 
 Presence of a ci- 
 trate. 
 
 Presence of a for- 
 mate or acetate. 
 
38 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 EXAMINATION OF PPT. PRODUCED BY CaCl 2 . 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Boil 
 
 }pt. with 
 
 PI 
 
 HC1. Confirm by 
 reactions, page 25' 
 
 It dissolves. 
 
 Presence of a ci- 
 trate. 
 
 To CONFIRM FORMIC OR ACETIC ACID. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 ~ Distil portion of j A white ppt. , Presence of a for- 
 original substance {blackening onj mate, 
 with dilute H 2 SO 4 , j warming, 
 stopping distillation 
 before blackening 
 occurs ; and to dis- 
 tillate add AgNO 3 . 
 
 Subtance was therefore a mixture of a for- 
 mate and a citrate. 
 
 (B) The substance is a colourless liquid. 
 
 EXPERIMENT. 
 
 OBSERVATION. 
 
 INFERENCE. 
 
 Heat substance Liquid boils ; the 
 in a dry tube. vapour has an al- 
 
 j coholic smell. 
 
 Heat residual li- ' A very irritating 
 quid with strong odour of acrolein. 
 H 2 SO 4 . 
 
 Test reaction of Neutral. 
 original solution. 
 
 Burn a drop or No residue left, 
 two of liquid on Pt 
 foil. 
 
 Presence of me- 
 thyl or ethyl alco- 
 hol. 
 
 Presence of gly- 
 cerine. 
 
 No free organic 
 acid. 
 
 Absence of salts 
 of organic acids. 
 
REACTIONS OF THE COMMON ACIDS. 39 
 
 Distil a portion of the original liquid, collect 
 the distillate, redistil it over half its bulk of 
 freshly ignited K 2 CO 3 , repeat the process and 
 take the first portion of the distillate. Determine 
 its boiling point found to be 78. The sub- 
 stance is ethyl alcohol. 
 
 Test for glycerine in the residual liquid left 
 after distilling off the alcohol, by evaporating 
 with KHSO 4 and heating strongly. A pungent 
 odour of acrolein indicates glycerine. 
 
 The substance is therefore a mixture of gly- 
 cerine and ethyl alcohol. 
 
 Preparation of Reagents. 
 
 In making up reagents for use in the labora- 
 tory, distilled water must be always used. 
 
 Hydrochloric acid. The strong pure acid 
 should be diluted with three times its volume 
 of water. 
 
 Nitric acid. The strong pure acid should be 
 diluted with three times its volume of water. 
 
 Sulphuric acid. The strong pure acid should 
 be diluted with four times its volume of water, 
 allowed to stand overnight to allow the lead 
 sulphate to settle, and then siphoned off. [Care 
 must be taken to pour the strong acid into the 
 water, and NOT the water into the acid.] 
 
 Sodium hydrate. Dissolve one part by weight 
 of the solid in ten times its weight of water. 
 
 Ammonium hydrate. Dilute '880 ammonia 
 with three times its volume of water. 
 
40 ELEMENTARY PRACTICAL CHEMISTRY. 
 
 Lime-water. Shake up one part of slaked 
 lime with about one hundred times its weight of 
 water, allow to stand overnight and decant the 
 clear liquid. Preserve in a tightly stoppered 
 bottle. 
 
 Ammonium chloride. Dissolve one part by 
 weight of the solid in eight times its weight 
 of water. 
 
 Ammonium carbonate. Dissolve one part by 
 weight of the solid in five times its weight of 
 water, and add its own weight of '880 ammonia. 
 
 Barium chloride. Dissolve one part by weight 
 of the solid in ten times its weight of water. 
 
 Calcium chloride. Make a saturated solution. 
 
 Cobalt nitrate. Dissolve one part by weight 
 of the solid in ten times its weight of water. 
 
 Ferrous sulphate. Dissolve one part by weight 
 of the solid in ten times its weight of cold water, 
 and add a few drops of dilute sulphuric acid. 
 
 Ferric chloride. Dissolve one part by weight 
 of the solid in ten times its weight of water. 
 
 Potassium iodide. Dissolve one part by weight 
 of the solid in twenty times its weight of water. 
 
 Potassium chromafe. Dissolve one part by 
 weight of the solid in twenty times its weight 
 of water. 
 
 Sodium phosphate. Dissolve one part by 
 weight of the solid in ten times its weight 
 of water. 
 
REACTIONS O 
 
 Stannous chloride. Dissolve ore part by 
 weight of the solid in its own weight of strong 
 hydrochloric acid, and dilute with four times its 
 volume of water. A small piece of granulated 
 tin should always be kept in the solution. 
 
 Silver nitrate.. Dissolve one part by weight 
 of the solid in twenty times its weight of water. 
 
 For organic analysis dissolve one part by 
 weight of the solid in five times its weight 
 of water. 
 
 Platinum chloride. Dissolve one part by 
 weight of the solid in ten times its weight 
 of water. 
 
 Ammonium oxalate. Dissolve one part by 
 weight of the solid in twenty-four times its 
 weight of water. 
 
 Sulphuretted hydrogen. Make a saturated 
 solution of the gas. The gas should fir^t be 
 washed through water to free it from any small 
 quantities of acid present. 
 
 Bromine-water. Add about five grammes of 
 bromine to one hundred grammes of water, and 
 shake well. 
 
 Ammonium sulphide. Add to three volumes 
 of the strong solution twenty volumes of water 
 and two volumes of -880 ammonia. 
 
 Lead acetate. Dissolve one part by weight of 
 the solid in ten times its weight of water, and 
 add a little acetic acid. 
 
 Mercuric chloride. Dissolve one part by 
 weight of the solid in sixteen times its weight 
 of water. 
 
.fctf PRACTICAL CHEMISTRY. 
 TABLE OF SOLUBILITY OF SALTS. 
 
 
 a 
 
 E 
 
 
 
 E 
 
 3 
 
 O 
 
 ." 
 
 
 
 
 r5 
 
 9 
 
 
 3 
 
 
 
 
 
 E' 
 
 
 
 Aluminii 
 
 Ammoni 
 
 E 
 3 
 
 'o i *O 
 -= rt 
 
 ri a; 
 U J 
 
 i 
 
 & 
 
 3 
 
 >^ 
 d 
 B 
 
 
 
 ^ 
 
 >, 
 
 3 
 
 s 
 
 Potassiu 
 
 Sodium. 
 
 Acetate 
 
 (w) 
 
 w 
 
 W 
 
 \v vv 
 
 (vv) 
 
 W 
 
 w 
 
 w 
 
 Carbonate 
 
 
 w 
 
 a 
 
 a a 
 
 a 
 
 a 
 
 w 
 
 w 
 
 Citrate 
 
 w 
 
 vv a 
 
 a \v 
 
 a 
 
 a 
 
 w 
 
 w 
 
 Formate 
 
 
 w w 
 
 w w 
 
 vv 
 
 w 
 
 w 
 
 w 
 
 Chloride 
 
 vv 
 
 w vv 
 
 (w) vv 
 
 a 
 
 w 
 
 w 
 
 w 
 
 Nitrate 
 
 w 
 
 w 
 
 w 
 
 w 
 
 w 
 
 vv 
 
 w 
 
 w 
 
 w 
 
 Oxalate 
 
 a 
 
 vv 
 
 a 
 
 a 
 
 a 
 
 a 
 
 a 
 
 w 
 
 w 
 
 Salicylate 
 
 
 w 
 
 w 
 
 
 
 
 
 w 
 
 w 
 
 Sulphate 
 
 w 
 
 \v 
 
 (w) 
 
 i 
 
 vv 
 
 w 
 
 (w) 
 
 w 
 
 w 
 
 Tartrate 
 
 
 w 
 
 a 
 
 a 
 
 a 
 
 a 
 
 a 
 
 w 
 
 w 
 
 W signifies that the compound is soluble in water. 
 
 (w) signifies that the compound is difficultly soluble in water. 
 
 a signifies that the compound is soluble in acids. 
 
 i signifies that the compound is insoluble in water and acids. 
 
 JOSEPH THOMPSON', 6jK, TURNMILL STREET, LONDON, E.G. 
 
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