QUALITATIVE ANALYSIS TABLES, 
 
 AND THK 
 
 REACTIONS OF CERTAIN ORGANIC SUBSTANCES, 
 
 LETTS 
 
LIBRARY 
 
 OF THE 
 
 UNIVERSITY OF CALIFORNIA. 
 
 Class 
 
 >. 
 
QUALITATIVE ANALYSIS TABLES, 
 
 AND THE 
 
 REACTIONS OF CERTAIN ORGANIC SUBSTANCES. 
 
QUALITATIVE ANALYSIS TABLES, 
 
 AND THE 
 
 REACTIONS OF CERTAIN ORGANIC SUBSTANCES 
 
 BY 
 
 E. A. LETTS, D.Sc., PH.D., F.R.S.E., F.C.S., &C., 
 
 x 
 
 PROFESSOR OF CHEMISTRY IN QUEEN'S COLLEGE, BELFAST. 
 
 LONDON: MACMILLAN AND Co. 
 
 BELFAST : MAYNE & BOYD. 
 
 [ALL RIGHTS RESERVED.] 
 
L4- 
 
 PUINTEI) HY MAYNK & BOYI), PKINTEKS TO QUEEN'S COLLEGE, BELFAST. 
 
PREFACE 
 
 THIS little book has been written chiefly for my own students, but I shall be glad if it prove of service 
 to others also. 
 
 The plan which I have always adopted in teaching qualitative analysis, has been to demonstrate in 
 the class-room the reactions of the metals, acids, &c., embraced in the course, and to write on the board 
 the explanatory reaction, and also in words the characteristic phenomena, in each case. Then when 
 we came to the detection of unknown substances, I have also demonstrated the actual process and have 
 written on the board the scheme my students being instructed to carefully observe all that I do. to 
 copy in their note books all that I write, and to repeat in the laboratory for themselves, what they have 
 seen done in the class-room. In this way they gradually write their own text books part passu 
 with their work in the laboratory ; my object being to teach them to observe accurately, and at the 
 same time to make them understand the scientific explanation of each process which they are per- 
 forming. 
 
 I have always found this method of teaching satisfactory, and that a sound knowledge of the 
 subject is both acquired and retained, infinitely better and more readily than if a text book is placed in 
 the student's hands and he is told to make use of it. 
 
 The labour to the teacher by this method is, however, severe ; so I have decided to abate it some- 
 what by placing in the hands of my students a series of tables which shall embody the essence of the 
 demonstrations they actually see. There are also other reasons for doing this, as experience has 
 taught me that students never take down these tables accurately, and that there are many notes, &c., 
 to the latter, which it is impossible to deal with on the board. Moreover, there is a lot of matter which 
 medical students (and the book is largely, though by no means entirely, written for them) ought to 
 have some knowledge of, which it is impossible to teach in a three months' course ; and although very 
 anxious that they should pass their professional examinations, I have done my utmost to discourage the 
 " cram " system. 
 
 So much by way of apology for adding yet another to the many similar books on the subject. 
 
 Every teacher has his own methods acquired not only from his experience, but also largely 
 through the researches of others and this book embodies mine. 
 
 111732 
 
I have worked out all the different schemes repeatedly, and have had the very salutory comments 
 of many hundreds of students who have gone through them. 
 
 Table VIII. is founded on what I believe to be the best quantitative method for separating the 
 phosphate, and although somewhat tedious in carrying out it has always proved satisfactory. 
 
 Considerable trouble has been taken with Table IX., which as every chemist knows, embodies a 
 very difficult and unsatisfactory subject, and the same remark applies to Table X. (Solubility Table), 
 which has been re-written with the aid of Storer's Dictionary, Fresenius, and special experiments of 
 my own. The subject though of great importance in qualitative analysis is often nearly ignored by 
 both teachers and students, and although from the conflicting statements as to solubilities I feel sure 
 that the table here given may be open to many criticisms, I trust that it may be an improvement on 
 its predecessors. 
 
 The following are my authorities on certain special subjects treated of in this book, Fresenius, 
 Dittmar, Barfoed, Neubauer and Vogel, Otto, Roberts, Tollens, and Storer. 
 
 In conclusion, my best thanks are due to my assistant, MR. R. F. BLAKE, for the great care and 
 attention he has exercised in correcting and revising the proof sheets. 
 
 E. A. LETTS. 
 QUEEN'S COLLEGE, BELFAST, 
 JUNE, 1892. 
 
ANALYTICAL CLASSIFICATION OF THE METALS. 
 
 IN THIS BOOK THE METALS ARE ARRANGED AS FOLLOWS : 
 
 GROUP I. Metals precipitated by sulphuretted hydrogen from acidulated solutions of their 
 salts. 
 
 Sub-Groups : 
 
 1. Metals forming insoluble, or sparingly soluble chlorides 
 
 Silver, Lead, Mercurous Mercury. 
 
 2. Metals whose sulphides are soluble in (yellow) sulphide of ammonium 
 
 Tin, Antimony, Arsenic. 
 
 3. Metals not belonging to either of the first two sub-groups 
 
 Copper, Bismuth, Cadmium, Mercuric Mercury, (Lead). 
 
 GROUP II. Metals precipitated by sulphide of ammonium from solutions of their salts (or by 
 sulphuretted hydrogen and an alkali). 
 
 GROUP III. Metals not precipitated by sulphuretted hydrogen from solutions of their salts, 
 under any conditions. 
 
 Sub-Groups : 
 
 1. Metals precipitated by carbonate of ammonium (as carbonates), after adding chloride of 
 
 ammonium and ammonia to solutions of their salts 
 Barium, Strontium, Calcium. 
 
 2. Magnesium not precipitated under the above conditions by carbonate of ammonium, 
 
 but which gives a precipitate with a soluble phosphate. 
 
 3. Metals which give no precipitate with any of the above reagents 
 
 Potassium, Sodium, (Ammonium). 
 
EEACTIONS AND PROPERTIES OF SOME OF THE MOKE IMPORTANT 
 ORGANIC SUBSTANCES WITH TABLES FOR THEIR DETECTION. 
 
 ALKALOIDS. PAGE. 
 
 General Reagents for the Detection of Alkaloids, . . . . .60 
 
 Quinine, Reactions and Properties of, . . . .61 
 
 Cinchonine, . . . . .61 
 
 Strychnine, ,, . . . . .61 
 
 Brucine, ..... 62 
 
 Morphine, ..... 62 
 
 TABLE XL 
 Examination for a Single Alkaloid in a Solution (after Fresenius), . . .63 
 
 TABLE XII. 
 Reactions of Alkaloids, ........ 66 
 
 HEALTHY AND MORBID URINE. 
 
 Chief Constituents of Healthy Urine : 
 
 Urea, Reactions and Properties of, . . 
 
 Uric Acid, ., ,,..... 
 
 Hippuric Acid, ,, ...... 
 
 Chief Constituents of Morbid Urine : 
 
 Albumen, Reactions and Properties of, . . . . .71 
 
 Blood, 72 
 
 Bile, . 72 
 
 Sugar, . 72 
 
 Urinary Sediments and Calculi, ....... 73 
 
 TABLE XIII. 
 Examination of Morbid Urine, ....... 74 
 
 TABLE XIV. 
 Examination of Urinary Sediments, ...... 76 
 
TABLE XV. 
 
 Examination of Calculi containing One Constituent, ..... 77 
 
 TABLE XVI. 
 Examination of Calculi containing Several Constituents, . . . .78 
 
 TABLE XVII. 
 
 Examination of Complex Organic Mixtures, such as Articles of Food, the Contents of the 
 
 Stomach, etc., for Poisons, ...... 79 
 
 PROPERTIES AND REACTIONS OF CERTAIN OTHER ORGANIC BODIES. 
 
 Formic Acid, .... 82 
 
 Butyric ,,....... 82 
 
 Lactic ........ 83 
 
 Succinic ,,....... 83 
 
 Malic ,,....... 83 
 
 Benzoic ........ 84 
 
 Glucoses, ...... 84 
 
 Saccharoses, . . . . . . .85 
 
 Amyloids, ....... 85 
 
 Alcohol, ....... 86 
 
 Chloroform, ...... 87 
 
 Chloral Hydrate, ..... 87 
 
 Glycerine, 
 
 Albumenoid Bodies, 
 
 Blood, ...... 89 
 
 Tannins, ... . 9 
 
 Gallic Acid, ..... 9 
 
 Pyrogallic Acid, .... 9 1 
 
 Phenol, ..... 91 
 
 Salicylic Acid, ...... 9 J 
 
QUALITATIVE ANALYSIS TABLES 
 
 WITH NOTES AND EXPLANATIONS. 
 
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 HH 5) d. 
 
 00 
 
 O 
 
 a 
 
 02 
 
 I 
 S 
 
 o 
 
 s 
 
 Ex 
 
 he 
 
 Jpo 
 
 c ^ 
 
 K- 
 
 
 
 & 
 
 
 Q, 
 
 
 ^ <u 
 
 PI U 
 
 ** - y* 
 
 "2 
 SJ 
 
 N rt 
 
 j3 
 
 3 
 _* 
 
 "? 
 
 
 ffi g 
 
 
 ta&< 
 
 
 3 o 
 
 o o 
 
 S 
 
 S 
 
 
 
 
 c 
 
 j.j'^-i-tr*!^-* *- "^ 4-* 
 
 02 
 O 
 
 S 
 
 w 
 
 w 
 
 l 
 
 
 
 
 g 
 
 9 
 
 wo 
 
 w 
 
 02 
 
 w 
 
 <J 
 
 O 
 
 w 
 
 P3 
 
 2 c 
 
 4|- 
 
 bfl 
 
 (/! 
 
ued. 
 
 
 
 <3 
 
 uj 
 _i 
 m 
 
 o 
 
 h- 
 
 co 
 
 LU 
 
 I- 
 
 o 
 
 r-; 
 
 
 13 
 
 
 aT 
 
 * 
 
 c 
 
 oT 
 
 - 
 
 >~> 
 
 10 
 
 u-, 
 
 cu 
 
 be 
 
 
 
 CO 
 
 O 
 
 ^- 
 
 
 CO 
 
 rt 
 
 "c 
 
 Cu 
 
 4-1 
 
 rt 
 cj 
 
 bo 
 
 13 
 
 4-1 
 
 rt 
 13 
 
 4-1 
 
 
 
 ammonia adde 
 
 
 4-1 
 
 cd 
 
 'to 
 
 o" 
 
 O 
 
 _C 
 O 
 
 is insoluble i 
 
 4-1 
 
 rt 
 
 j^ 
 Cu 
 
 CO 
 
 O 
 
 J5 
 Cu 
 rt 
 u-, 
 
 t i 
 
 ttf 
 
 13 
 JO 
 
 3 
 
 g 
 
 V 
 
 4-1 
 
 13 
 
 CO 
 
 f a phosphate : 
 
 able quantity c 
 
 cS 
 
 'o 
 
 CU 
 J3 
 
 13 
 C 
 rt 
 
 CO 
 
 of 
 
 O 
 
 3 
 
 m 
 
 rt 
 
 13 
 O 
 
 00 
 
 3 
 
 4-> 
 
 rt 
 13 
 
 O 
 
 C 
 rt 
 
 H- 1 
 
 HCI, neutraliz 
 
 U 
 
 K 
 
 CO 
 
 CO 
 
 CU 
 
 c 
 
 
 'S 
 
 "3 
 rt 
 
 C 
 
 o 
 
 c 
 
 JO 
 
 "o 
 
 c 
 
 o 
 
 4-1 
 
 JO 
 
 
 4-1 
 
 rt 
 
 
 JO 
 
 'o 
 
 CU 
 
 CO 
 
 rt 
 O 
 
 js 
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 CU 
 
 13 
 
 4-1 
 
 monium 
 
 fluoride 
 
 i 
 
 > 5 
 i i 
 t 
 
 consider 
 
 E 
 
 o 
 
 13 
 cu 
 I- 
 
 of 
 
 m 
 
 CU 
 
 carbonat 
 
 13 
 
 j> 
 o 
 
 13 
 O 
 
 4-1 
 C 
 
 
 
 >. 
 
 rt 
 
 S 
 
 "c 
 
 CU 
 
 to 
 
 
 iT 
 rt 
 
 CU 
 
 4-1 
 CO 
 
 3 
 rt 
 
 <u 
 
 E 
 
 rt 
 
 CU 
 JO 
 
 rt 
 13 
 
 CU 
 
 4-1 
 
 4-1 
 CS 
 
 E 
 
 4-1 
 
 4-1 
 
 rt 
 
 Q 
 
 O 
 
 
 ^ 
 
 c 
 
 CL, 
 
 
 CL, 
 
 a 
 
 , 
 
 CJ 
 
 O 
 
 jo 
 
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 H 
 
 13 
 rt 
 
 r* 
 
 S 
 
 ^ 
 
 ^ 
 
 CU 
 
 3 
 
 
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 4-1 
 
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 CO 
 
 O 
 
 
 r*^ 
 
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 x 
 
 ^ 
 
 c^ 
 
 U 
 
 4-1 
 
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 J3 
 
 4-1 
 
 3 
 
 JO 
 
 13 
 c 
 
 Q 
 
 13 
 
 
 *o 
 
 rt 
 
 s 
 
 !_ 
 
 4-1 
 
 
 CL, 
 
 CU 
 
 0) 
 
 
 13 
 
 3" 
 
 c 
 
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 4-1 
 
 CO 
 
 2 
 
 3 
 
 CU 
 
 C 
 
 oo 
 
 4-1 
 CU 
 
 JO 
 U 
 
 rt 
 
 c 
 
 
 bb 
 
 
 
 CO 
 
 2 
 3 
 
 
 rt 
 O 
 
 OO 
 
 o 
 
 O 
 
 'o 
 rt 
 
 tj 
 
 4-1 
 
 CU 
 
 ^O 
 
 cu 
 
 'E 
 pj 
 
 'bb 
 
 E 
 
 CJ 
 
 rt 
 
 ' 
 o 
 
 
 ' 
 
 
 o 
 
 
 4-> 
 
 
 
 . 
 
 ^CJ 
 
 U 
 
 
 ^i 
 
 4-* 
 
 X 
 
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 CU 
 
 O 
 
 CU 
 
 
 2 
 
 "* 
 
 JH 
 
 
 ^_^ 
 
 CU 
 
 ex 
 
 P*H 
 
 CO 
 
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 ^Q. 
 
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 t, , 
 
 cu 
 
 o 
 
 ifl 
 
 4-1 
 
 
 
 CO 
 <+-, 
 
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 13 
 
 CU 
 
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 rt 
 
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 00 
 
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 C 
 bO 
 rt 
 
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 fl 
 
 
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 3 
 13 
 
 CU 
 JO 
 
 rt 
 
 E 
 
 13 
 
 13 
 
 c 
 
 rt 
 
 E 
 
 o 
 
 also the precipitate 
 
 rt 
 
 4-1 
 
 O 
 
 ex 
 
 CJ 
 
 4-> 
 CO 
 
 3 
 rt 
 
 CJ 
 
 13 
 C 
 
 C 
 
 ex 
 i 
 
 fs" 
 
 3 
 
 _o 
 
 'C 
 
 3 
 
 ^ex 
 
 to 
 
 C 
 rt 
 
 'o 
 rt 
 
 3 
 3 
 
 C 
 rt 
 3 
 CT 1 
 
 3 
 O 
 
 4-1 
 
 rt 
 
 OJ 
 
 O 
 
 1-1 
 rt 
 
 a 
 
 cu 
 13 
 
 13 
 C 
 
 4-1 
 
 3 
 
 13 
 
 onia precipitate (or 
 
 4-1 
 4-1 
 
 c 
 
 rt 
 
 'S 
 
 O 
 
 E 
 
 dness to convert it ir 
 
 present, evaporate t 
 
 C 
 
 Cu 
 
 rt 
 
 00 
 CO 
 
 4-1 
 
 rt 
 
 
 ffi 
 
 'co 
 
 < 
 
 
 to 
 IM 
 
 
 ^o" 
 
 <u 
 
 CJ 
 
 rt 
 
 E 
 
 E 
 
 rt 
 
 CU 
 
 00 
 
 _o 
 
 rt 
 r-, 
 
 ^_^ 
 
 'CX 
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 CU 
 
 
 
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 \-, 
 O 
 
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 13 
 
 C 
 
 Q 
 
 1 
 
 3 
 
 C 
 
 'C 
 
 _cf 
 
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 rt 
 
 j=: 
 
 4-1 
 
 3 
 
 13 
 
 1 
 
 ^3 
 
 T> 
 
 rt 
 
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 1* 
 
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 13 
 
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 rt 
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 agnesium ; < 
 
 3 
 3 
 
 G 
 O 
 l_ 
 
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 r the original 
 
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 jSo 
 
 C 
 
 13 
 C 
 rt 
 
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 E 
 
 rt 
 
 13 
 
 13 
 as 
 
 J^ 
 
 4-1 
 4-T 
 
 C 
 CU 
 
 Neutralize v 
 
 substance) tc 
 
 rt 
 
 t i 
 
 O 
 
 00 
 CO 
 
 rt 
 
 13 
 
 
 
 4-1 
 
 co 
 
 CL, 
 O 
 
 4-1 
 
 
 "o 
 
 C 
 
 13 
 
 E 
 o 
 
 o 
 
 ^3 
 3 
 
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 _CJ 
 
 ^ 
 
 .2 
 
 o 
 
 o 
 
 "u 
 rt 
 
 13 
 _c 
 
 ^~ 
 
 cx 
 
 U 
 
 _c 
 
 13 
 C 
 rt 
 
 
 JO 
 
 t) 
 
 CU 
 
 < 
 <U 
 
 rt 
 
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 a 
 
 
 C 
 rt 
 
 .2 
 
 E" 
 
 _3 
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 4-1 
 
 co 
 
 13 
 _c 
 
 'bb 
 
 ^o 
 
 o 
 
 mmon 
 
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 4-1 
 
 rt 
 
 4-1 
 
 cu 
 
 13' 
 
 cu 
 
 13 
 o 
 
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 1 
 
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 i-. 
 
 
 
 CU 
 
 rt 
 
 
 
 'c 
 
 
 o 
 
 
 "o 
 
 
 _o 
 
 c 
 
 rt 
 
 ex 
 
 >-(-, 
 
 >^ 
 
 
 3 
 
 cu 
 
 13 
 
 J3 
 
 !* 
 s 
 
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 O 
 
 C 
 
 ! 
 
 13 
 rt 
 
 JU 
 
 <*- 
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 CO 
 
 C! 
 
 Q 
 
 'o 
 
 V 
 
 (X 
 
 to 
 
 C 
 
 13 
 
 
 
 3 
 to 
 
 O 
 
 adding chloride of ammo 
 
 >? 
 
 _> 
 
 E 
 E 
 
 rt 
 
 13 
 .cu 
 CJ 
 
 3 
 13 
 O 
 U 
 
 CL, 
 
 CU 
 f 
 
 4-1 
 
 [a,' 
 
 , of barium, strontium, c 
 
 00 
 
 rt 
 
 i_ 
 
 __O^ 
 
 rs 
 
 rt 
 
 'bb 
 
 o 
 
 
 
 4-1 
 
 o 
 
 CU 
 
 N 
 "o 
 
 CU 
 to 
 rt 
 CJ 
 
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 ^0) 
 
 4-1 
 
 1- 
 
 
 ex 
 cu 
 
 "rt 
 >-i 
 rt 
 
 ex 
 
 CU 
 
 CO 
 
 4-1 
 CO 
 
 CU 
 
 4-1 
 
 0> 
 
 4-J 
 OJ 
 
 O 
 
 d, by the turmeric reactic 
 
 .e precipitate produced by 
 
 ;ssolve the ammonia preci 
 
 O 
 en 
 
 ex 
 o 
 
 T3 
 V 
 
 rt 
 
 "S 
 
 cu 
 C 
 
 aT 
 
 4-1 
 
 rt 
 
 4-1 
 CU 
 
 4-1 
 
 O 
 
 _q 
 
 4-1 
 00 
 
 'O 
 
 co 
 
 | 
 
 U-H 
 
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 (U 
 
 ttf 
 
 to 
 
 o 
 
 'C 
 o 
 
 i i 
 
 13 
 C 
 ctf 
 
 13 
 
 'co 
 CU 
 
 )-, 
 
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 ^> 
 3 
 
 CO 
 
 to 
 13 
 
 13 
 C 
 rt 
 
 i-T 
 cu 
 
 4-1 
 
 jat the ammonia precipitat 
 
 S 
 
 4-1 
 
 03 
 13 
 
 G 
 rt 
 
 .2*" 
 'S 
 o 
 
 ders the silica insoluble w 
 
 4-1 
 
 (0 
 
 M-* 
 
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 a 
 
 CU 
 
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 CU 
 
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 " 
 
 'g 
 
 ^c 
 
 rt 
 
 jc 
 
 4-1 
 
 13 
 
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 rt 
 
 O 
 
 ^ 
 
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 -G 
 
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 S 
 
 3 
 
 3 
 
 00 
 
 to 
 O 
 
 4-1 
 O 
 
 3 
 CT 1 
 <U 
 to 
 
 M 
 
 CL, 
 CU 
 
 4-1 
 
 13 
 
 X' 
 
 o 
 
 _'o 
 
 to 
 
 CO 
 
 CJ 
 
 1 
 
 bo 
 
 C 
 
 4-T 
 
 C 
 (U 
 CO 
 
 E 
 
 3 
 
 ex 
 
 CO 
 
 !U 
 4-1 
 
 1 
 
 4-T 
 
 C 
 cu 
 oo 
 
 S 
 
 rt 
 
 J^ 
 
 J3 
 
 CJ 
 
 D 
 
 4-1 
 
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 CU 
 
 C 
 
 
 
 CU 
 
 JO 
 
 3 
 co 
 
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 3 . 
 
 co 
 
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 "cu 
 
 
 JO 
 
 13 
 
 CU 
 
 ex 
 
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 JO 
 
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 CU 
 l_ 
 
 ex 
 
 '^ 
 
 jEi 
 
 -; 
 
 . 1 
 
 
 j=: 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 Q 
 
 
 H 
 
 
 <J 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 o" 
 
 
 hH 
 
 
 <*i 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
LU 
 
 _l 
 CD 
 < 
 I- 
 
 r 
 
 i| 
 
 > 
 
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 3 
 
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 ct i i 
 
 
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 x 2 
 
 3 o 
 
 3 <U 
 
 i <-> 
 
 o 
 
 C/D 2 
 
 
 
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 o ' o 
 
 o i 
 
 5 ^ S. 
 
 ^ 13 - 
 
 W 2 en 
 
 ^g S 
 
 ;|1 
 
 o-ffl 
 rt ^; 
 
 O T3 
 
 v- C <u 
 CX w C 
 
 -o a 
 
 <U 
 
 '2 
 
 E 55 | 
 S * 
 
 
 
 
 "c" 
 
 
 
 
 4-1 
 
 
 
 
 bfl OH 
 
 
 
 
 !a 
 
 
 
 d 
 
 fe J^H 
 
 
 
 .2 
 
 fc 
 
 
 
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 ^~l 
 
 
 
 
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 s ^ 
 
 
 
 . 
 
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 s 5, 
 
 h 
 
 
 1 
 
 tt - 
 
 
 
 
 .a 
 
 4) ^ 
 
 
 
 
 1 
 
 H --^ 
 
 1-1 
 
 
 
 
 H 
 
 T3 
 
 & 
 
 C 
 
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 b 
 
 5 
 
 ^^ o i 
 
 ri 
 
 4-1 
 
 cS 
 
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 p-'C 
 ^ -2^ 
 
 <M 
 
 c/3 
 
 g 
 
 
 
 
 
 
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 13 
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 13 
 
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 13 *"" "^ 
 >> <u u 
 
 - 
 
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 3 
 
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 9 
 
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 in 
 
 <n 
 
 
 
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 rt 
 
 
 
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 (J 
 
 
 
 H 
 
 
 
 
 N 
 *> 
 
 o> 
 
 1 
 
 T3 
 
 The Metal is : 
 
 BARIUM 
 STRONTIUM 
 CALCIUM 
 
 EH 
 
 
 
 
 
 
 
 M 'C 
 
 
 
 1 
 
 4-j o kD 
 
 
 
 J. 
 
 m o 
 
 
 
 i 
 
 ] , IS^ ^ 
 
 OH g O 
 
 
 
 u 
 
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 * o> o> 
 
 
 
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 "> ^ 
 
 
 
 ^ 
 
 <^ OH OT 
 
 
 
 CQ 
 
 "t? 'G 1r< 
 
 
 
 a 
 
 2 D -M 
 
 
 
 
 
 6 ~ "On 
 
 
 
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 ^ ^^ " f ~ l 
 
 
 
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 g 43 &, 
 
 
 
 
 C *** 4.^ 
 
 ^ 
 
 C ^ 
 <u o 
 
 X" fi bc 
 O O c 
 
 S 
 
 '- 
 
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 T3 . 
 
 tn C d. 
 
 Pi ""* *o 
 
 O (U <U 
 
 S 4J 9 
 
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 T3 
 rt 
 
 u 
 
 ffi 
 
 C 3 c^ 
 
 .5 "o ^ 
 
 O "" T3 
 
 S I 8 
 
 r -o 
 
 -y T3 x! 
 5 as ^ 
 
 ]&, 4J~ | 
 
 Sis 
 
 ^ 2 ^ 
 
 rt cr 
 
 CJ <-t-> "~ 
 
 '" O 
 
 P "c -^ 
 
 C ~- 
 
 <u oJ 
 
 ^ C 
 
 6 "2 o 
 
 .2 g >g 
 
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 ^G g 
 
 rt c 
 
 _< 
 
 &H 
 
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 55 -*-> rt 
 
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 c o 
 & 
 
 (L> 
 
 3 
 
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 O 4J I- 1 - * 
 
 o,S c ? 
 
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 TJ ^ CTj t/) 
 
 JJ C3 -4-J C/3 
 
 r^ C ^ R$ 
 
 'i 1 c & 
 
 -P ^ St <+- 
 
 c c^iz: 
 
 CD 
 
1 
 
 
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 LU 
 
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2 
 
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 *~^ ^ Q^ *^ ^ 
 
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 .t: y rt ig 
 
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 c 
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 t" 01-, 
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 |o f | f 
 
 1 2 c 
 
 
 
 to 
 i 
 
 ~s, 
 
 CS 
 
 C 
 
 H 
 
 S* cu 
 
 S CO ^ 
 
 0) I 
 
 3 J,^ 
 
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 o o .2 
 
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 ess 
 
 ^ "o + 
 
 
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 ^ S 
 4_) rt 
 
 S 
 a 
 
 t* 
 
 > "o (5^ 
 
 6+t 
 
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 C?^ 0) 
 
 TJ 
 ^CJ 
 
 t/2 
 
 D 
 
 _ -' ^ 
 
 c ^^ 
 
 
 j^ 1 G ( ; f-j 
 
 K^ ^^* r^ 
 
 a 
 
 2 jf 
 
 S 
 
 o 
 
 rt i ~ < 
 
 rt <u ^ -^ 
 
 iuu 
 
 ^ ^ ^-^ g 
 
 wj ^'-S 
 
 
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 u 
 
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 ^ r( <$ 
 
 <r^ sj ^ ^ b^ 
 
 << ^ o 
 
 ^ 
 
 ^ co 
 
 
 H-l CTJ 
 
 _^ O 
 
 1-1 ^ 
 
 <- 
 
 ^-v^v x~.^~s 
 
 Z'il 
 
 d 
 
 00 
 
 tM 
 
 O 
 
 
 _-/ 
 
 3^73 ^,-^3 
 
 M C^ CO 
 
 C/v^-'S ^3^ 
 
 >^ o ^^ 
 
 c^ 
 
 * 
 
 
 
 
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 en 
 
 o 
 
 ^-, 
 
 y 'd 
 
 
 rt 
 
 * 
 
 
 rt 
 
 
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 o .a 
 
 
 
 
 
 
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 ^ '^J\ V 
 
 c 
 
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 u 
 
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 5^ 
 
 0) 43 
 
 
 
 
 E 
 
 Q 
 
 4 
 
 2 
 
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 OH T3 
 
 1 ^ 
 
 i PRESENC 
 
 fe 
 O 
 
 PQ 
 N 
 
 i 
 
 I 
 
 P 
 
 
 D 
 
 02 
 
 o 3 
 
 "p 
 
 CO 
 
 o 
 
 0) be 
 
 v-< c 
 
 
 
 o 
 M 
 
 
 
 
 03 
 
 09 
 
 S^ 
 
 H 
 
 .-g 
 
 en VH 
 
 cc 
 
 
 
 
 
 
 M) 
 
 C 1 
 
 
 
 
 
 
 
 B 
 
 J" 
 
 
 
 
 
 
 
 g 
 
 '5 ^ 
 
 
 t/) >s, fj ~ 
 
 ^ 
 
 bD<j^ c ^ 
 
 
 3 O 
 
 to 
 
 O <U 
 
 o, 6 
 
 
 D ^1 ^ pi 
 
 **7" H '73 4n ^ 
 
 13 
 
 13 
 
 'i^c*' 
 
 
 B. 
 
 o *- 
 
 1 
 
 <u 3 
 
 
 O *S VH rt 
 
 H 
 
 rt y rt '" 
 
 
 U 
 
 
 rt "o 
 
 
 'o 2 vS'c 
 
 *s 
 
 ^ QH^ 
 
 
 ^ rt 
 
 ^ 
 
 1 ^ 
 
 
 So'o^'g 
 
 c 
 
 rt e 'o 
 f0 r* C v 
 
 
 c " 
 
 <U OJ 
 
 5 
 ^o 
 
 Q ^ 
 
 
 c'a 8-| 
 
 5 
 
 bjO^ a. 
 
 
 4-> 4-> 
 
 | 
 
 45 
 
 
 O 3 J* +5 
 "JU $ 'hri C 
 
 "o 
 
 >-i O 
 c o ^ 
 
 
 rt 
 
 3- 
 
 solution with about one-t 
 
 RESULT. 
 
 nee in the cold with evolu 
 ) characteristic odour, but c 
 ime- water suspended on a j 
 ured on to lime-water co 
 ds shaken with it). 
 
 nee in the co/c/ with ev 
 y a characteristic odour. 
 
 o^ -M i- dT 
 
 |1|;| 
 
 3 
 
 Oi 
 
 "3 
 
 be 
 
 'S 
 
 3 
 
 II 
 
 rt p^ 
 QJ r^ '^ 
 
 "o o -5* 
 
 .^- r-* 
 
 1/2 ** 00 
 
 S 
 
 * 
 
 u 
 
 
 0) J2 i O *~ 
 
 U 
 
 C ^ 3 <-i w 
 
 !_,_, 
 
 *" C 3 
 
 
 5 
 
 
 g** 8 s| 
 
 <u ^j 
 
 B'o ** a 
 
 O 
 
 V-, 
 
 .0 g 
 
 
 1 
 
 
 fc'> % 
 
 w*3 
 
 152lt 
 
 
 
 J^ 
 
 
 h 
 
 
 f^ 2 *^ tiD 
 WpC] 
 5/5 TO ^j "O 
 
 w 1 
 
 W D.-- J 
 
 
 
 co?^ 
 
 
 
 
 rt ^ f{ C 
 
 3 
 
 rt "T^ r^ "tji 
 
 
 3 S 
 
 
 S 
 
 
 bo -M rt 
 
 
 CL, p TJ 42 
 
 
 
 

 
 s !<->" 
 
 
 
 
 -II 
 
 
 
 ^ 6-5 
 
 
 
 
 ^^ 
 
 
 
 u .3 - 
 
 
 
 
 O" 3 .-5 
 < xl 
 
 
 
 trS C "~ 
 
 
 <D 
 
 
 Z ^ ^ 
 
 
 
 _.M O ^ 
 
 
 4-J 
 
 
 be a 
 
 
 
 OH CD 
 
 
 2 (D 
 
 
 <^ ^ t" 
 
 
 
 '5 ~ "td 
 
 
 'S^ *^ 
 
 OJ 
 
 "^S 'rt 
 
 
 
 c" 33 
 
 
 'u .ti 
 
 S 
 
 5 T3 'C 
 
 
 
 2 " r2 .^ 
 
 
 .?/ 
 
 .!&* 
 
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 J3 S o> *u 
 
 
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 *-> m . 
 
 u o o y 
 
 
 
 o O '"O ^ ..?* 
 
 
 "rt u fe^ 
 
 rt ^ D 
 
 'rt O L 
 
 
 
 "Q X <u Lt, 
 
 dj 
 
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 "- ^"rt 
 
 _4J N *-" 9f 
 
 
 
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 rt 
 
 &i 3 3 * 
 
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 O-.X T3 
 
 
 
 C ^ " 4 ~ ) *^ 
 
 .tn 
 
 'G ' o " - 
 
 'CJ 'CL, 
 
 "o "*"* ^ r^ 
 
 
 
 OO CO ***** 
 > "> 
 
 "o< 
 
 'o 
 
 D O Q OH 
 
 D (U .5. 
 
 !-<>-. O 
 
 O-bC w 
 
 O f'1 
 
 
 
 E be o J ^ 
 
 T^ 3 O 
 
 S 
 
 OH 
 
 3 I'| D ^ 
 
 ID x! O- 
 
 ^^ 0) 
 
 gJj-"3S 
 
 
 
 j & ^*r2 O 
 
 C 
 It 
 
 3 I C ^.^ 
 
 ^5 be 
 
 o O C 
 -5 rt 
 
 .> S ^ 
 
 
 
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 (i) AgNO 3 a yellowish precipitate which cu 
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 (i) AgNO 3 a yellowish precipitate which cu 
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 (i) AgNO 3 a white precipitate which does 
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 5 tests described on Table VI. 
 
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 5 
 
 sulphides, 
 cyanides, ferrocyanides 
 chromates, peroxides ai 
 
 hyposulphites, polysulphi 
 iodides, along with oxidis 
 
 benzoates. 
 
 silicates, 
 salts of silver, lead, merci 
 
 >rmation of precipitates of 
 hloride of silver (from silv 
 ariety of things which we: 
 
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 resence of an oxidizing agent or of SO 2 . Ferric chloride (yellow or brown solution) gives 
 becomes colourless (because a ferrous salt is produced). Chromates and bichromates 
 precipitate of sulphur and become green (because chromium chloride is produced). 
 mates (violet solution) also become colourless (because manganous chloride is formed). 
 
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 (umiuouiiut; jo a;iuDsaBqd|ns) !! S s V' r HN6=S ? (''HN) + (: S r ' s V ''^ 
 
 -salts of tin, antimony, and arsenic are decomposed, the sulphides of those metals being 
 
 JH 4 Cl+As,S,-r-H,S. Yellow sulphide of ammonium is decomposed by hydrochloric acid 
 
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 forming a mixture o 
 
 
 chloride to metallic t 
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a ^1 i: ? S^'*S ^^ r ^ w ^'^'^ "5 ^TS'C^^G '^^sj 
 
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 a c^c .2 y-^tv^- 1 '^ ^ S^ p ^C 1 s a '-S .2 S ^7"^ p a 'o u ^ 
 
 ts -^^^y rt u o ^ a^x 5 Sy'S-^^o ( *? 4 - > *- 1 
 
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 y ji .a u y Ji rl a r, r ^J . "" N a 
 
 ^ 
 
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 magnesium, should it 
 
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 144 
 
 
 
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 : indicates phosphor* 
 ~ CO 2 and the solutioi 
 soluble gelatinous res 
 
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 siderable quantities c 
 
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 5 - p .5 I^ w "S .ti || y - a a ^ v 
 10 ^ w^:'i--2 S^ "3*^*1 >> ^^ rt 
 
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 ie of ammonium is to prevent the precipit 
 
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 ess of molybdate of ammonium yellow p 
 d then KMnO 4 effervescence due to the 
 ryness, moistening with strong HCI, and v 
 
 u *- 
 
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 y be extracted as such from the (NH^)|S 
 te precipitate with (NH4) 2 CijO 4 proving tl 
 f ammonium proving the presence of pho; 
 
 CJ 
 
 55 
 
 y" 
 fe N 
 
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 0^2 
 c ^ 
 
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 s based on the fact that Fe 2 (OH) (j , Cr.(OK 
 y soluble, but are reprecipitated on boili 
 r partly especially in the presence of am 
 LC1O 3 , the chromium is converted into K s 
 soluble in vvater, while the iron is convert 
 Jtion of the fused mass eventually conta 
 -hich gives yellow chromate of lead with c 
 ZnS which is often dark coloured from 
 est (p. 26) or by redissolving it in dilute 
 ipitating with H 2 S when the precipitated 
 depends upon the following facts. Bott 
 ig respectively cobalto-cyanide of potassi 
 Ni(CN) 2 =K 2 Ni(CN) 4 . On adding brom 
 o(CN) 8 -(-2KBr. On now adding caustic ] 
 nee of the hypobromite) of black Ni 2 (OH) f 
 lution filtered from the black Ni 2 (OH) (i , t 
 need (mercurous colbalti-cyanide; which c 
 
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8 
 
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 Ammonium pre 
 
 Sulphide 
 
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 olutio 
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 the 
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 contain Z 
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 Solution (ma 
 
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 bo 
 
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 ZINC, 
 
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 TABLE VIM. ( 
 
 the solution filtered from the sulphide of ammonium precipita 
 ested by boiling with carbonate of ammonium. If no ppt. for 
 ,vith carbonate of ammonium, boiled, and filtered. The filt 
 that the whole of the metals have been precipitated. The pp; 
 
 Table for the Examination of the Precipitate produced by ( 
 
 'en 
 
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 Precipitate (may contain SrSO 4 and CaSO 4 
 
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 on filtered from the carbonate of ammonium precipitate, or in 
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 ence of magnesium the solution is tested for potassium and so< 
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 ht residue which may be left, and once more to evaporate to C 
 st for potassium (violet flame, crimson through blue glass), am 
 :he POTASSIUM confirmed in a portion of the solution b 
 of the solution by freshly prepared pyroantimoniate of potassi 
 
 him is present, it should be removed before testing for K an< 
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 natory test for the nitrite with starch, 
 sorb the liberated iodine. In such cases 
 and here the knowledge and ingenuity 
 emoved by nitrate of silver : the filtered 
 matory test for the nitrite. To remove 
 colour with starch, iodide of potassium, 
 
 
 
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 ows PRESENCE OF : 
 
 SULPHIDE 
 
 SULPHITE 
 
 YPOSULPHITE 
 
 (Thiosulphate) 
 
 BENZOATE 
 
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 CYANIDE* 
 
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 EREOCYANIDE 
 
 'EERICYANIDE 
 
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 RESULT. 
 
 Evolution of a gas smelling of rot 
 paper moistened with acetate of lea 
 white or yellow precipitate of sulp! 
 the addition of, an acid to a sulph 
 latter has been long prepared.) 
 
 3 
 
 ( 
 be 
 
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 3 
 
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 O 
 
 13 
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 The solution remains clear for 
 becomes turbid from separation of 
 same time smells of burning sulphu 
 
 White crystalline precipitate, and 
 acid on warming. 
 
 White gelatinous precipitate. 
 
 Characteristic odour of hydrocyai 
 
 Evolution of a greenish-yellow 
 characteristic odour which bleaches 
 (The original solution also .smel 
 possesses bleaching properties.) 
 
 ^ - u 
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(i) Chlorates give no precipitate with silver nitrate, 
 but if their solutions are mixed with zinc and dilute sul- 
 phuric acid they are slowly changed to chlorides Which 
 then give a white precipitate with silver nitrate. 
 
 (i) Warmed with MnOj, and H 2 SO 4 , chlorine isevolved 
 as a greenish-yellow gas of characteristic odour, which 
 bleaches moist litmus paper. 
 (2) AgNO :j a white precipitate which curdles when 
 shaken, dissolves readily in ammonia, but isunsolitble in 
 nitric acid. 
 
 (i) Chlorine water a yellow to brown colour. On 
 shaking the mixture with chloroform, the latter becomes 
 coloured brown. 
 
 (i) Chlorine water (not in excess) a yellow to brown 
 colour. (A) On shaking the mixture with chloroform, 
 the latter becomes coloured violet. (B) On addingsome of 
 it to fresh starch solution, the latter becomes coloured blue. 
 (2) HgCl 2 a scarlet precipitate. 
 
 (i) CaCl 2 whitegelatinousprecipitate, soluble inHCl. 
 
 ( i ) The dry substance (or residue left when the solution 
 is evaporated to dryness) heated with solid arsenious 
 anhydride, gives the characteristic odour of kakodyl. 
 
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 on warming. (If the precipitate is dissolved in the 
 smallest possible quantity of ammonia, and the mixture 
 warmed, metallic silver is deposited on the tube as a 
 mirror.) 
 
 4-1 
 
 rt 
 
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 be 
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 CHLORATE 
 
 CHLORIDE 
 
 BROMIDE 
 
 IODIDE 
 
 FLUORIDE 
 
 ACETATE 
 
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 CITRATE 
 
 be 
 
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 ATORY TESTS 
 
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 ows PRESENCE or : 
 
 OXALATE 
 
 to 
 
 i * 
 
 OXALATE 
 
 CHLORIDE 
 
 BROMIDE 
 
 IODIDE 
 
 1 
 
 be 
 
 c 
 o 
 
 NITRATE* 
 
 :ralised solutior 
 Id chloride of b 
 
 SULPHATEt 
 
 IVERAL ACID 
 
 fl 
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 : carbonate, nitrite, fluoride, sulphate, 
 groups, (i) chloride, bromide, or iodide ; 
 ;) chlorate or chloride ; (6) acetate or 
 : ; (9) tartrate or citrate, etc. The 
 >vith the preliminary examination may 
 
 B. 
 
 eat the precipitate with acetic acid. A 
 ITRATE (partly) pass into solution, 
 soluble in hydrochloric acid, 
 recipitate. Filter, wash, then treat the 
 
 i, FERRIC YANIDE (orange), BROMIDE 
 
 ith nitric acid, 
 id FERROCYANIDE (white). 
 G, CHLORATE, ACETATE, possibly a 
 
 :e added), while a HYPOSULPHITE and 
 
 g the solution with excess of carbonate 
 
 
 
 i i 
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 (0 
 
 XI 
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 4-) 
 
 XJ 
 
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 'i 
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 excess of chlorine-water which oxidizes 
 carbon or chloroform. To test for the 
 lid taken), the dry residue well pounded 
 icentrated sulphuric acid from a small 
 
 c H ^ 
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 X! 
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 1 X . Continued. 
 
 ed the following with certaint 
 d one or more of the following 
 i chlorate or hypochlorite ; 
 , ferrocyanide, or ferricyanil 
 if necessary, and this coupled 
 n below : 
 
 W 
 EH 
 O 
 
 W 
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 & 
 
 
 
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 02 
 
 p 
 
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 CM 
 
 neutral). Filter, wash, and 
 OSPHATE, ARSENIATE, and 
 
 SULPHATE, and BORATE, al 
 
 1 from the nitrate of calcium 
 
 te), SULPHOCYANATE (whit 
 
 reprecipitated on acidulating 
 mmonia), SULPHIDE (black), 
 ntain a TARTRATE, CITRA 1 
 
 U 
 
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 means bromine and iodine ar 
 stils over, and is decomposed 
 1 iodine, and then tested with 
 
 LU 
 
 CO 
 
 h 
 
 preliminary examination will probably have indicat 
 e, hypochlorite, borate, chromate, silicate, benzoate, an 
 ate or nitrite ; (3) sulphite or hyposulphite ; (4) 
 yanate ; (7) phosphate or arseniate ; (8) cyanide 
 ig partial separation of acids may first be resorted to 
 : the necessity of one or other of the separations give 
 
 PARTIAL SEPARATION 0! 
 
 calcium to the original solution (which must be 
 NATE is here indicated by effervescence, while a PH 
 
 ay contain a FLUORIDE, OXALATE, TARTRATE, 
 
 ' silver and dilute nitric acid to the solution filterec 
 
 ate with strong ammonia, and filter : 
 nay contain a CHLORIDE (white), CYANIDE (whi 
 
 sh), and CHROMATE (crimson), all of which may be 
 ay contain an IODIDE (yellow but is whitened by a 
 iltered from the nitrate of silver precipitate may co 
 
 ATE, SULPHITE, NITRITE, and a NITRATE origin 
 HLORITE will have been destroyed. 
 
 :n be converted into sodium salts, and the silver i 
 and filtering from carbonates of silver and calcium v 
 
 SEPARATI 
 
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 . 
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 test for the BROMIDE in another portion of the sol 
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 vn precipitate indicating the HYPOCHLORITE. 
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 E 
 
 o 
 2 
 
 T3 
 >^ 
 
 XI 
 
 
 VN 
 o. 
 
 o 
 
 4-> 
 
 
 _0 
 
 rt 
 
 * 
 
 >r\ 
 
 O 
 
 
 ^H 
 
 
 '4-1 
 </> 
 
 3 
 
 y. 
 
 CM 
 
 o *- 
 d, -d 
 
 <u 
 ^> 
 
 
 rt 
 
 
 
 + 
 
 O 
 
 3 " 
 
 U 
 
 
 
 _0 
 
 
 "5) 
 
 IM 
 
 O 
 
 
 v 
 
 
 u 
 
 
 
 
 
 
 
 oJ 
 
 J3 
 
 *l_ 
 
 ^o 
 
 
 5J 
 
 
 
 
 ~ 
 
 
 
 t/5 
 
 s 
 
 
 c 
 
 
 
 
 rt 
 
 
 
 
 4 
 
 
 rt 
 
 
 
 
 
 '5 
 
 
 3 
 
 
 
 
 
 -a 
 
 
 T3 
 
 
 
 
 
 TD 
 
 Sulphocy 
 
 ate 
 
 6 
 
 ith soli 
 he blood 
 
 .ion is evaporated 
 YATE may be 
 
 CD CD 
 
 XI XJ 
 ^ h^ 
 
 sidue le 
 emitted. 
 acid to 
 
 e 
 
 s 
 
 dry substance (or r 
 ic odour of kadodyl is 
 ddition of hydrochlo 
 
 he 
 
 s 
 
 er 
 he a 
 
 be detected by hea 
 ride when the char 
 h ferric chloride, afte 
 
 CETATE may 
 
 arsenious anhyd 
 red colour wit 
 
 CD 
 
 H 
 
X 
 
 LU 
 
 CD 
 
 H 
 
 
 FC ?^ 
 
 ** CD 
 
 5 .S 
 
 c .2 
 
 r5 '5 
 o u 
 
 o - 
 >. -^ 
 
 " V4-C 
 
 "re 
 
 
 
 
 .5 
 o 
 
 X 
 
 o J 
 Q 
 
 p 
 
 1 
 ^3 
 
 
 rogen and hydrochloric acid in a 
 
 
 
 
 
 ^o 
 '-D 
 
 T3 
 
 C 
 re 
 
 o 
 
 CJ 
 
 eaction. To detect the FERRO- 
 ich precipitates the ferrocyanide as 
 
 s 
 
 'Sc 
 
 .d 
 
 ^ 
 
 _H 
 
 
 
 1-H 
 
 
 
 *5 S 
 
 = 
 
 s. 
 
 
 S^ 
 
 
 ^ 
 
 CU 
 
 rH 
 
 "i 
 
 w 
 
 
 (7.) Phosphate and Arseniate. 
 
 nee of the phosphate by the yellow precipitate formed 
 ric acid, or by Marsh's test. The PHOSPHATE in preset 
 
 
 ''5 
 
 CD 
 
 ^> 
 
 3 
 
 -M 
 
 en 
 
 _/-. 
 
 rt 
 
 M 
 
 a 
 
 re 
 ^ 
 
 re 
 
 _^ 
 
 /^v 
 
 en 
 f. 
 <U 
 C 
 > 
 
 -5 
 o 
 
 4-> 
 
 -a 
 
 CD 
 
 4-> 
 
 rt 
 
 
 
 dn 
 
 rt 
 
 CD 
 
 /. 
 
 C 
 
 _c 
 
 3 
 
 he fused mass into water phosphuretted hydrogen is gi 1 
 
 i-.' 
 
 
 
 
 TJ 
 O 
 
 osphate by prolonged treatment with sulphuretted h] 
 
 N 
 _O 
 
 T3 
 
 lide, Ferrocyanide, and Ferricyanide (as Alkaline Salts 
 
 turated with carbonic anhydride (which decomposes tl 
 
 4-1 
 3 
 
 So 
 
 2 5 
 
 
 
 ^ CJ 
 
 s 'E 
 
 cu < 
 
 *-s 
 
 *> en 
 
 - 3 
 
 ^ y 
 
 g 
 
 ^ J3 
 en .ti 
 
 
 
 C t3 
 O CD 
 
 - X 
 
 i 1 
 
 *-" .2 
 
 X^ 
 
 Jj en 
 rt 
 
 T3 S3 
 
 2 bfl 
 
 8.S 
 
 = 
 ^ ^ 
 
 JJ'-s 
 
 CD 
 
 ed from this precipitate is tested for the FERRICYANIE 
 
 
 
 <L> O 
 en - 
 
 CD ,C 
 
 CX O 
 
 C 
 ao 
 
 CD 
 
 j 
 
 M 
 
 c 
 
 O 
 
 4-1 
 
 y/ 
 'C 
 
 A 
 ex. 
 
 rt 
 
 ID 
 
 4-> 
 
 en 
 
 1 
 
 rt 
 en 
 
 en 
 
 &* 
 
 re 4-> 
 
 6 <s 
 
 V- 
 
 <u 
 
 4-J 
 S 
 
 
 
 s t 
 
 T3 J3 
 ^ T3 
 
 c 
 
 aj 
 -C 
 Z 
 
 '5c 
 c 
 'C 
 .Q 
 c 
 
 haracte 
 
 e 
 
 
 
 fc 
 
 1/3 
 1/3 
 CU 
 
 o 
 
 o 
 
 U 
 
 ex, 
 
 55- 
 
 C 
 
 .2 
 
 4-> 
 
 J3 
 
 1 ^ 
 
 s ;s 
 
 .J3 rt 
 
 C 
 
 _0 
 
 4-J 
 
 j3 
 
 ~ 
 
 
 
 O C 
 CD re 
 
 4-> 
 
 S 
 
 ni 
 
 
 
 CJ 
 
 m 
 
 T3 
 0) 
 
 tu 
 
 43 
 
 
 "o 
 
 H 
 
 -0 g 
 <u tu 
 
 j~. 
 CD 
 
 
 
 S S 
 
 js r 
 
 >^u 
 
 re ^~> 
 
 S ^ 
 
 r residue 1< 
 
 idescent. 
 
 4-j 
 
 JT 
 
 en 
 
 o 
 
 4-1 
 4-J 
 
 2 ~ 
 
 rt 3 
 1 1 
 
 en | 
 
 *.l 
 
 _C 
 
 4-1 
 
 g 
 
 1 1 
 
 . ^ 
 ^ T3 
 
 s i 
 
 73. ~ 
 
 'o D 
 
 ro rr 
 
 X 
 
 H 
 
 CJ 
 
 _3 
 
 :5 
 
 S 
 
 
 .RSENIATE 
 
 sulphuretted 
 
 substance (o 
 
 become incai 
 
 minute quan 
 
 U 
 
 4-1 
 
 '5 
 
 CD 
 en 
 
 4-1 
 
 'o 
 
 
 >H 
 
 
 
 CD 
 
 JZ 
 *-> 
 
 4-1 
 
 o 
 
 0) 
 
 hydrocyanic 
 CYANIDE, t 
 
 '' Prussian B 
 
 " Turnbull's 
 
 
 <3 
 
 
 
 
 l_ 
 
 
 
 "CD 
 
 
 
 
 
 
 
 
 
 rt 
 
 
 
 
 
 
 
 
 ^ 
 
 
 
 
 C 
 
 
 
 o 
 
 
 
 
 
 H 
 
 
 
 
 <3 
 
 
 
 H 
 
 
 
 
 cq 
 
 
 EH 
 S 
 
 4-> 
 
 H 
 
 e/3 
 
 O 
 
 'e 
 
 'o " 
 
 CD lT 
 
 S S 
 
 -5 '-2 
 
 c S 
 
 v, 
 en 
 
 4-1 
 " 4J 
 
 'rt "^ 
 
 ^ S 
 
 D 
 
 X 
 
 i 
 
 4-> 
 
 rt 
 
 'G 
 
 <u 
 
 f. 
 
 U 
 
 g 
 "3 
 
 
 Bromide, Iodide. 
 
 i 
 
 CD 
 
 Cc 
 i-T 
 
 4-J 
 
 '5 
 X 
 
 = c 
 
 rt 
 C 
 
 en 
 
 O 
 
 S 
 c 
 
 
 
 "2 
 
 a 
 
 -c 
 
 _0 
 
 >-. 
 
 
 
 
 CD 
 X 
 
 O 
 
 C i- 
 
 .2 o 
 
 4-1 *-> 
 
 -C 
 
 
 
 o 
 
 rt 
 CD 
 
 
 Chloride, 
 
 "% 
 
 c 
 
 _cD 
 3 
 
 ^_o 
 
 rt 
 ^ 
 
 CD 
 
 X 
 
 4-1 
 ^ 
 
 -^J 
 
 S 
 
 V-' 
 
 -1 
 
 "rt 
 > 
 
 
 4^ 
 
 C 
 
 bfl 
 O 
 
 ^ 
 
 x 1 
 
 'S 
 
 ^ ^H 
 
 .Hf "^ 
 
 fcc 
 
 c 
 <u 
 
 4-J 
 
 rt 
 C 
 O 
 
 ^ 
 
 rt 
 
 precipitate. 
 
 
 
 
 
 oT 
 
 1? 
 a 
 
 
 O 
 en 
 
 CD 
 
 A 
 
 <u 
 
 re 
 
 ^5 
 ^ 
 
 3 
 
 en 
 
 C 
 
 ^H 
 
 bfi 
 
 .5 
 
 'o 
 
 ^ 
 
 ^ 
 t-> 
 
 ^ 
 
 
 i 
 
 
 
 4-> JO 
 
 > 
 
 <u 
 
 t 
 
 'E, 
 
 E 
 
 f- 
 
 
 1 
 
 | 
 
 o 'o 
 
 *~O rt 
 
 CD 
 
 
 4-1 
 
 ^5 
 ? 
 
 
 
 I 
 
 'u c 
 
 S a 
 
 D.'O 
 
 mass 
 
 
 (9.) Tartrate 
 
 O 
 ^1 
 
 <u 
 
 be removed. 1 
 ^ol, add some acel 
 
 S 
 
 J^ 
 
 en 
 rt 
 -j 
 3 
 DH 
 
 <+H 
 
 
 
 
 *J 
 
 ro 
 
 4-1 
 
 .C 
 
 4-J 
 
 '5 
 
 o 
 > 
 
 'So 
 u 
 
 Ferricyanide, Su 
 
 om HALOIDS. 
 
 n: 
 
 CD 
 
 
 
 re 
 
 V- 
 
 CJ 
 
 > 
 
 'en 
 ^-i 
 O 
 M 
 
 -a 
 
 CU 
 y/ 
 
 a 
 
 V 
 
 ^ 
 
 4-> 
 
 4-> 
 
 en 
 CU 
 
 ofl 
 
 '-3 
 
 
 
 
 
 rt 
 
 
 
 i_ 
 
 CD 
 
 
 
 
 'o 
 
 rt 
 
 ^ 
 <u 
 
 e/3 
 
 <L> 
 
 C- 
 
 _c 
 
 I 8 
 
 13 
 
 3 
 
 G T3 
 <U 
 
 ro en 
 
 ~ T3 
 D ^_, 
 
 w rt 
 " fc 
 
 is precipitated as bitartr 
 
 IS 
 
 ^ 
 
 <*- 
 
 o 
 
 XI 
 
 4-J 
 
 o 
 
 JD 
 
 B 
 _2 
 
 "C 
 H 
 
 ,0 
 
 <H- 
 O 
 
 <u 
 
 Cyanide, Ferrocyanide, 
 
 DOUBLE CYANIDES f 
 
 "2 
 
 'S 
 
 rt 
 ^ 
 
 CJ 
 CD 
 
 12 
 
 ? 
 c 
 
 
 T3 
 
 S 
 rt 
 
 en 
 
 D 
 
 ~2 
 '5 
 
 e with carbonate of soda 
 
 
 
 t 
 
 " o 
 
 4-J CD 
 
 u 
 
 "rt 
 -, 
 
 ttf 
 
 4-J 
 
 <L> 
 CJ 
 
 o 
 
 T3 
 
 C 
 rt 
 
 re 
 >> 
 
 CJ 
 
 CD 
 
 "re 
 j 
 
 'H 
 
 U 
 
 r2 
 
 
 1 
 
 rt nj 
 
 4-> 
 
 '-*- CD 
 
 rt 
 
 IN 
 
 O 
 
 
 CQ 
 
 H 
 
 X 
 
 H 
 
 G 
 
 i 
 
 -3 
 
 o 
 
 
 cu 
 
 O cj 
 
 <U ^ H O.T3 
 
 
 
 cu 
 
 r C^ 
 
 D 
 
 
 i2 
 
 
 ~ 
 
 a- 
 
 
 en 
 
 CJ <*- 
 
 c o 
 
 w 
 
 
 
 ^l 
 < 
 
 U 
 
 u 
 
 rt 
 
 
 H 
 
 3 
 
 EH 
 
 - 
 en C 
 
 cL'- 
 
 u 
 
 3 
 X 
 
 i 
 
 
 g 
 
 0> 
 
 S 
 
 rt 
 '- 
 
 'G 
 u 
 
 '5 
 .E/- 
 o 
 
 A 
 
 iromide, 
 
 
 
 .S e/3 
 
 
 
 -U 
 
 
 PS 
 
 . 
 
 * ' 
 
 _u 
 
 
 2 
 
 
 
 
 
 C- 
 
 
 
 
 
 EH 
 
 
 
 
 
 en 
 
 /-S 
 
 
 
 
TABLE > 
 
 W signifies soluble in water. 
 
 A ,, insoluble in water, but soluble in nitric and in hydrochloric acid. 
 
 I ,, ,, ,, and in both nitric and hydrochloric acid. 
 
 slightly soluble in the particular solvent against which it is placed. 
 
 
 K 1 
 
 NH/ 
 
 Na 1 
 
 Mg 
 
 Ba 
 
 Sr 
 
 Ca 
 
 Fe" 
 
 Fe"' 
 
 Ni 
 
 Co 
 
 Al 
 
 ACETATE 8 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 ARSENIATE 
 
 W 
 
 W 
 
 W 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 ARSENITE 
 
 W 
 
 W 
 
 W 
 
 A 
 
 W S -A 
 
 W S -A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 
 
 BENZOATE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W s 
 
 W 
 
 A 
 
 W 
 
 W 
 
 W 
 
 W 
 
 BORATE 
 
 W 
 
 W 
 
 W 
 
 W S -A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 BROMIDE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 CARBONATE 
 
 W 
 
 W 
 
 W 
 
 A 
 
 A 
 
 A 
 
 A 
 
 
 
 A 
 
 A 
 
 A 
 
 A 
 
 CITRATE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 A 
 
 A 
 
 W 8 -A 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 CHLORIDE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 CHLORATE 9 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 CHROMATE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 A 
 
 W S -A 
 
 W 8 -A 
 
 w 
 
 
 
 A 
 
 A 
 
 A 
 
 CYANIDE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W S -A 
 
 W 
 
 W 
 
 w 
 
 A 8 -I 
 
 A*-I 
 
 A S -I 
 
 
 
 FLUORIDE 
 
 W 
 
 W 
 
 W 
 
 A 
 
 W 8 -A 
 
 W S -A 
 
 A-I 19 
 
 w 
 
 W 
 
 W 
 
 W 
 
 W&I 20 
 
 FORMIATE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 w 
 
 W 
 
 W 8 
 
 W S -A 
 
 W 
 
 FERROCYANIDE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W S -A 
 
 W 
 
 W 
 
 I 
 
 I 
 
 I 
 
 I 
 
 w 
 
 FERRICYANIDE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 
 
 w 
 
 w 
 
 I 
 
 I 
 
 I 
 
 
 
 HYDRATE 
 
 W 
 
 W 
 
 W 
 
 W S -A 
 
 W 
 
 W 
 
 w s 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 HYPOSULPHITE 10 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W s 
 
 W 
 
 w 
 
 
 
 W 
 
 W 
 
 W 
 
 
 
 HYPOCHLORITE 13 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 w 
 
 
 
 
 
 
 
 
 
 
 
 IODIDE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 \v 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 NITRATE 17 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 w 
 
 w 
 
 W 
 
 W 
 
 W 
 
 w 
 
 NITRITE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 w 
 
 
 
 
 
 w 
 
 
 
 
 
 OXALATE 
 
 W 
 
 W 
 
 W 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 OXIDE 
 
 W 
 
 W 
 
 W 
 
 A-I 19 
 
 W 
 
 W 
 
 w s 
 
 A-A 8 
 
 A-A 8 
 
 A 
 
 A 
 
 A-I 19 
 
 PHOSPHATE 
 
 W 
 
 W 
 
 W 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 SILICATE 21 
 
 W 
 
 
 
 W 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 SULPHATE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 I 
 
 I. 
 
 W S -A 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 SULPHITE 
 
 W 
 
 W 
 
 W 
 
 W 8 
 
 A 
 
 A 
 
 W 
 
 W S -A 
 
 W 8 -A 
 
 A 
 
 A 
 
 W 
 
 SULPHIDE 
 
 W 
 
 W 
 
 W 
 
 W 8 -A 
 
 W 
 
 W 
 
 W S -A 
 
 A 
 
 A 
 
 A N 
 
 A* 
 
 A 
 
 SULPHOCYANATE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 TARTRATE 
 
 W 
 
 W 
 
 W 
 
 W 8 -A 
 
 A 
 
 A 
 
 A 
 
 W 
 
 W S -A 
 
 A 
 
 W 
 
 W 
 
 
 K 1 
 
 NH 4 X 
 
 Na 1 
 
 Mg 
 
 Ba 
 
 Sr 
 
 Ca 
 
 Fe" 
 
 Fe" 7 
 
 Ni 
 
 Co 
 
 Al 
 
 * To find the solubility of any compound of one of the metals whose symbol is placed at the head 
 find the solubility of mercurous chloride, glance down the last vertical column (headed 
 insoluble in water, and only sparingly soluble in nitric acid. 
 
 56 
 
 of the v 
 
 Hg 2 ) un 
 
olubility Table.* 
 
 signifies soluble in nitric acid alone, or appears to be. 
 
 M ,, hydrochloric acid alone, or appears to be. 
 
 that the substance either does not exist, or that no record of its solubility can be found. 
 
 Mn, 
 
 Or 
 
 Hg 
 
 Pb 2 Bi 3 Cu Od 
 
 Sb 4 Sn'' Sn"" As s 
 
 Ag 6 
 
 Hg, 7 
 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 
 
 W s 
 
 \V 8 -A N 
 
 ACETATE 8 
 
 A 
 
 A 
 
 A 
 
 A N 
 
 A H 
 
 A 
 
 
 
 A-I 20 
 
 A 
 
 A 
 
 
 
 A N 
 
 A N 
 
 AESENIATE 
 
 A 
 
 
 
 A 
 
 A N 
 
 
 
 A 
 
 
 
 W 
 
 A? 
 
 A? 
 
 
 
 A N 
 
 A N 
 
 ARSENITE 
 
 W 
 
 W 
 
 W S -A X 
 
 W S -A N 
 
 W 
 
 W S -A 
 
 W 
 
 W 
 
 W 8 
 
 W 8 
 
 
 
 W S -A- V 
 
 A* 
 
 BENZOATE 
 
 A 
 
 A 
 
 
 
 A* 
 
 A 
 
 A 
 
 W 8 -A 
 
 
 
 A 
 
 
 
 
 
 W S -A N 
 
 
 
 BORATE 
 
 W 
 
 W 
 
 W 
 
 \V S -A N 
 
 W S -A 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 I 
 
 A N8 
 
 BROMIDE 
 
 A 
 
 
 
 A 
 
 A* 
 
 A 
 
 A 
 
 A 
 
 
 
 A 
 
 
 
 
 
 A" 
 
 A* 
 
 CARBONATE 
 
 A 
 
 W 
 
 W S -A 
 
 A s 
 
 
 
 W 
 
 A 
 
 
 
 
 
 
 
 
 
 A" 
 
 A N 
 
 CITRATE 
 
 W 
 
 W&A 
 
 W 
 
 \V 8 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 I 
 
 \ N * 
 
 CHLORIDE 
 
 W 
 
 W 
 
 W 
 
 w 
 
 W . 
 
 W 
 
 W 
 
 
 
 W 
 
 
 
 
 
 W 
 
 W 
 
 CHLORATE 9 
 
 W 
 
 A 
 
 W 8 -A 
 
 A N -I 
 
 A 
 
 W 
 
 A 
 
 A 
 
 A 
 
 A 
 
 
 
 A NS 
 
 A N 
 
 CHROMATE 
 
 A 
 
 A 
 
 W 
 
 A" 
 
 A 
 
 A 
 
 A 
 
 
 
 
 
 
 
 
 
 I 
 
 
 
 CYANIDE 
 
 A 
 
 W 
 
 W 
 W 
 
 W 8 -A 
 W 
 
 A N 
 W s 
 
 W 
 W 
 
 A 
 W 
 
 W--A 
 W 
 
 W 
 
 W 
 
 A? 
 
 W? 
 
 W 
 
 W 
 W 
 
 A N 
 
 W 8 
 
 FLUORIDE 
 FORMIATE 
 
 A 
 
 W 
 
 A 
 
 A* 
 
 I? 
 
 I 
 
 A 
 
 
 
 A-I? 
 
 I? 
 
 
 
 I 
 
 
 
 FERROCYANIDE 
 
 I 
 
 
 
 W 
 
 W S -A S 
 
 I 
 
 I 
 
 A 
 
 
 
 I 
 
 
 
 
 
 I 
 
 
 
 FERRICYANIDE 
 
 A 
 
 t 
 
 A 
 
 A* 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 
 
 A N 
 
 A N 
 
 HYDRATE 
 
 W 
 
 
 
 
 
 W s 
 
 
 
 W 
 
 W 
 
 
 
 W 
 
 
 
 
 
 A* 11 
 
 12 - 
 
 HYPOSULPHITE 10 
 
 14 
 
 
 
 
 
 W 
 
 
 
 W 
 
 
 
 
 
 
 
 
 
 
 
 W 15 
 
 
 
 HYPOCHLORITE 18 
 
 W 
 
 W 
 
 A 
 
 W S -A S 
 
 A 
 
 16 
 
 W 
 
 W 8 -A 
 
 VV 
 
 W? 
 
 W 
 
 I 
 
 I 
 
 IODIDE 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 W 
 
 
 
 W 
 
 W 
 
 NITRATE 17 
 
 W 
 
 
 
 
 
 W 8 -A* 
 
 
 
 W 
 
 
 
 
 
 
 
 
 
 
 
 w s 
 
 18 
 
 NITRITE 
 
 P-A 
 
 W 8 -A 
 
 A 
 
 A N 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 W 
 
 
 
 A N 
 
 A N 
 
 OXALATE 
 
 A 
 
 A-I 20 
 
 A 
 
 A N 
 
 A 
 
 A 
 
 A 
 
 A 20 
 
 A 
 
 I 
 
 W 8 -A 
 
 A N 
 
 A N 
 
 OXIDE 
 
 A 
 
 A 
 
 A 
 
 A N 
 
 A 
 
 A 
 
 A 
 
 A 
 
 A 
 
 I? 
 
 
 
 A N 
 
 A N 
 
 PHOSPHATE 
 
 A 
 
 A 
 
 
 
 A N 
 
 
 
 A 
 
 A 
 
 
 
 
 
 
 
 
 
 
 
 
 
 SILICATE 21 
 
 W 
 
 W 
 
 W 
 
 A N -I 
 
 W 
 
 W 
 
 W 
 
 A 
 
 W 
 
 W 
 
 
 
 W 8 
 
 W 8 -A N 
 
 SULPHATE 
 
 7 8 -A 
 
 
 
 W 
 
 A N 
 
 A 
 
 W 
 
 W 9 -A? 
 
 A? 
 
 W 
 
 
 
 
 
 A N 
 
 
 
 SULPHITE 
 
 A 
 
 A 
 
 A" 
 
 A N 
 
 A 
 
 A N 
 
 A 
 
 A H 
 
 A H 
 
 A H 
 
 A 
 
 A N 
 
 A 22 
 
 SULPHIDE 
 
 W 
 
 ~ 
 
 W? 
 
 W S -A? 
 
 A 
 
 W 
 
 W s 
 
 
 
 W? 
 
 
 
 
 
 I 
 
 A S -I 
 
 SULPHOCYANATE 
 
 / 8 -A 
 
 W 
 
 A 
 
 A N 
 
 A 
 
 W 
 
 W 8 -A 
 
 A 
 
 A 
 
 
 
 
 
 A N 
 
 A N 
 
 TARTRATE 
 
 Mn 
 
 Cr 
 
 Hg 
 
 Pb 2 
 
 Bi 3 
 
 Cu 
 
 Cd 
 
 Sb 4 
 
 Sn" 
 
 Sn"" 
 
 As 5 
 
 Ag 6 
 
 Hg/ 
 
 
 lumns, glance down the column until the horizontal line is reached corresponding with the acid. Thus, to 
 [LORIDE (ninth) horizontal line is reached. Here "A NS " is printed signifying that mercurous chloride is 
 
 57 
 
NOTES TO TABLE X Solubility Table. 
 
 1. All the ordinary salts of the alkali metals are soluble. 
 
 2. As salts of lead are precipitated by hydrochloric acid, the solubility of those salts which are insoluble 
 
 in water, but soluble in acids are marked " N " signifying that they give a clear solution with 
 nitric acid. 
 
 3. Bismuth salts are as a rule decomposed by water giving basic compounds soluble in nitric and 
 
 hydrochloric acids. 
 
 4. Antimony salts are as a rule decomposed by water giving basic compounds soluble in acids. 
 
 5. Very few salts of arsenic are known. 
 
 6. As salts of silver are precipitated by hydrochloric acid, those salts which are insoluble in water, bul 
 
 soluble in acids are marked " N " signifying that they give a clear solution with nitric acid. 
 
 7. The same note as 6 applies to mercurous salts. 
 
 8. Probably all normal acetates are soluble in water, but basic acetates often are not. 
 
 9. Probably all chlorates are soluble in water. 
 
 10. Hyposulphites are decomposed by acids with precipitation of sulphur. 
 
 11. Hyposulphite of silver is white, but changes rapidly, becoming yellow, orange, brown, and finally 
 
 black Ag 2 S 2 O 3 +H 2 O=:Ag 2 S-f-H 2 SO4. It is soluble in excess of alkaline hyposulphites. 
 
 12. A mercurous salt gives a black precipitate, with a soluble hyposulphite, of mercurous sulphide 
 
 Hg 2 (NO 3 ) 2 + Na 2 S 2 O :i + H 2 O = Hg 2 S + H 2 ^SO 4 + 2NaNO s . 
 
 13. Ordinary hypochlorites always contain chlorides in addition. 
 
 14. A manganese salt gives a brown precipitate of hydrated manganese peroxide with a hypochlorite 
 
 MnCl 2 +NaClO + 2NaHO=MnO 2 ,H 2 O + 3NaCl. 
 
 15. Hypochlorite of silver is soluble, but decomposes spontaneously into chlorate (soluble) and chloride 
 
 (insoluble) 3AgClO=AgClO s +2AgCl. 
 
 1 6. A cupric salt when mixed with a soluble iodide, gives a precipitate consisting of a mixture of cuprous 
 
 iodide and free iodine 2CuSO 4 +4KI=Cu s I 1 +2K 2 SO 4 +I 2 . 
 
 1 7. Probably all nitrates are soluble in water. 
 
 1 8. A solution of a mercurous salt when mixed with a nitrite, gives a grey precipitate of metallic mercury 
 
 Hg 2 (N0 3 ) 2 + KNO 2 +H 2 0-2HN0 3 +KN0 3 +2Hg. 
 
 19. The native compound is insoluble in water and acids. 
 
 20. After ignition it is insoluble in acids. 
 
 21. Most natural silicates are insoluble in water and acids, but artificial silicates are often soluble in 
 
 dilute acids. Such solutions when concentrated yield a gelatinous mass of silica and a soluble 
 salt of the metal. 
 
 22. Soluble in aqua regia only, or in a mixture of hydrochloric acid and chlorate of potash. 
 
 58 
 
REACTIONS AND PROPERTIES 
 
 OF SOME OF THE MORE 
 
 IMPORTANT ORGANIC SUBSTANCES, 
 
 WITH TABLES FOR THEIR DETECTION. 
 
Alkaloids. 
 
 The alkaloids form a series of natural principles, mostly derived from vegetable sources. They 
 always contain nitrogen and are more or less closely allied to ammonia. Some contain carbon, hydrogen, 
 and nitrogen only while others contain oxygen in addition. The former are as a rule volatile, while 
 the latter generally, but not always, decompose when heated. The alkaloids frequently have a bitter 
 taste and generaly have a powerful physiological action, many of them being violent poisons. They 
 neutralize acids, forming as a rule crystallizable salts. Most of them are sparingly soluble in water, but 
 readily dissolve in alcohol. There are certain general reagents which react in a similar manner with all 
 alkaloids, among which are the following : 
 
 1 . Chloride of platinum combines with the hydrochlorates of the alkaloids, forming compounds 
 
 analogous to the double chloride of ammonium and platinum 2NH 4 C1, PtCl 4 . They 
 are best obtained (if not insoluble) by evaporating the mixed solution of chloride of 
 platinum and hydrochlorate of the alkaloid to dryness, and adding alcohol to the residue. 
 
 2. Solution of iodine in iodide of potassium, (best decinormal solution) throws down all the 
 
 alkaloids from solutions of their salts in the form of yellow, brown or reddish-brown pre- 
 cipitates consisting of their polyiodides. If these precipitates are well washed, and then 
 evaporated to dryness on a water bath with excess of sulphurous acid, the pure sulphate of 
 the alkaloid remains. 
 
 3. Solution of iodide of mercury in iodide of potassium* throws down all the alkaloids from their 
 
 solutions in the form of white or yellowish-white precipitates. 
 
 4. Solution of the iodides of cadmium and potassium! precipitates the alkaloids after their 
 
 solutions have been acidulated with sulphuric acid. The precipitates are all white and 
 amorphous at first, but some of them become crystalline on standing. 
 
 :. Solution of the iodides of bismuth and potassium gives with most (but not all) alkaloids floc- 
 culent orange coloured precipitates. 
 
 6. Phospho-molybdic acidt precipitates all the alkaloids, even when their quantity is very minute. 
 
 The precipitates are bright yellow, ochreous, or brownish-yellow in colour, and have an 
 analogous composition to phospho-molybdate of ammonium. On warming the precipitate 
 with caustic potash or soda, the alkaloid separates in the free state, and may be removed 
 by extracting the solution with ether, amyl alcohol, benzol, &c. 
 
 7. Metatungstic acid (or a solution of tungstate of soda) to which phosphoric acid has been added 
 
 precipitates all the alkaloids from their solutions. The precipitates are white and floccu- 
 lent, and the reaction is very delicate. To obtain the free alkaloid from the precipitate 
 the latter is digested with lime or baryta, when insoluble phospho-tungstate of lime or 
 baryta and the alkaloid separate. 
 
 8. Picric acid throws down nearly all the alkaloids in the form of yellow precipitates, insoluble in 
 
 excess of the precipitant. 
 
 * A solution of iodide of potassium to which mercuric chloride has been added until the precipitate first formed just ceases to 
 be redissolved on shaking. 
 
 t Prepared by saturating a boiling concentrated solution of iodide of potassium with iodide of cadmium, and adding an equal 
 volume of iodide of potassium. 
 
 J Prepared as follows : A boiling solution of ordinary molybdate of ammonium is precipitated with phosphate of soda ; the 
 precipitate is well washed, suspended in water, and warmed with a solution of carbonate of soda until it is completely dissolved. 
 The solution is evaporated to dryness, the residue ignited, and if reduction has taken place it is moistened with nitric acid and 
 ignited again. The product is warmed with water, and dissolved by adding nitric acid in considerable excess (one part of the 
 residue should make ten parts of solution). 
 
 60 
 
QUININE CocH^NA, 3H,O 
 
 Occurs in the bark of the cinchona tree along with cinchonine. The free alkaloid is crystalline 
 sparingly soluble in cold more readily in hot water. It is easily soluble in alcohol and chloroform, but 
 less so in ether. Solutions both of the free alkaloid and of its salts have an intense bitter taste. 
 
 1. Solutions of quinine salts which contain an oxygen acid (especially the sulphate) show a very 
 
 characteristic blue fluorescence. 
 
 2. Caustic potash and soda, ammonia, and the carbonates and bicarbonates of potash and soda pre- 
 
 cipitate the free alkaloid from solutions of its salts. The precipitate is white and amor- 
 phous when first formed, but becomes crystalline after some time. 
 
 3. On adding chlorine-water and then excess of ammonia, solutions of quinine salts give an 
 
 emerald-green colour. If, before adding ammonia, a few drops of ferrocyanide of potassium 
 are added, a deep red coloration is produced. These reactions are delicate and highly 
 characteristic. 
 
 CINCHONINE C 19 H 2 ,N 2 O 
 
 Accompanies quinine in cinchona bark. The free alkaloid is crystalline, very sparingly soluble in 
 cold and in hot water. It is more readily soluble in alcohol, and also dissolves in ether and chloroform. 
 It has a bitter taste. When heated cautiously the alkaloid sublimes unchanged. 
 
 1. Caustic potash or soda, ammonia, and the carbonates and bicarbonates of potash and soda pre- 
 
 cipitate the free alkaloid from solutions of its salts. The precipitate does not present a 
 crystalline appearance unless produced in very weak solution. 
 
 2. On adding ferrocyanide of potassium to a neutral solution of a salt of cinchonine, a flocculent 
 
 precipitate of the ferrocyanide of the alkaloid is thrown down. If this is warmed with a 
 slight excess of the precipitant it redissolves, and on cooling separates in brilliant golden 
 yellow scales or needles. 
 
 STRYCHNINE C^NA 
 
 Occurs in the different varieties of strychnos, especially in mix vomica, the St. fgnatius bean, and in 
 false angostnra bark. It is always accompanied by the alkaloid brucine. The free alkaloid is crystalline,, 
 and has an intensely bitter taste (appreciable in a solution containing i part of the alkaloid in 700,000 
 of water). It dissolves readily in boiling chloroform, benzol, and amyl alcohol. But it is almost 
 insoluble in cold water, and even boiling water dissolves only minute quantities. 
 
 Its salts are as a rule insoluble in water, and all have a very bitter taste, and like the free alkaloid 
 are extremely poisonous. 
 
 i . Caustic potash or soda and their carbonates produce a white crystalline precipitate with solu- 
 tions of the salts of strychnine. Ammonia gives the same precipitate, but it is soluble 
 in excess. After some time, however, the free alkaloid again separates out from the 
 ammoniacal solution in crystalline needles. 
 
 3. If strong sulphuric acid is added to a salt of strychnine, or to the free base, and then a fragment 
 
 , of bichromate of potash added, a magnificent violet colour is produced. The reaction is 
 delicate and highly characteristic. 
 
 61 
 
3. Sulphocyanate of potassium produces a white precipitate with solutions of strychnine salts, con- 
 
 sisting of the sulphocyanate of the alkaloid. The precipitate is somewhat soluble in excess 
 of the precipitant, and only appears after some time in dilute solutions. 
 
 4. Strong chlorine-water produces in solutions of strychnine salts a white precipitate, soluble in 
 
 ammonia to a colourless fluid. 
 
 BRUCINE C^U^NA 4H 2 O 
 
 Accompanies strychnine in nature. The free alkaloid is colourless and crystalline. It is far more 
 soluble in water than strychnine. It dissolves very readily in alcohol, amyl alcohol, chloroform, and 
 benzol, but it is almost insoluble in ether. When cautiously heated it first loses its water of crystallization, 
 and then sublimes' unchanged. Both the free alkaloid and its salts have a strong bitter taste. 
 
 1. Caustic potash and soda, and their carbonates precipitate the free alkaloid from solutions of its 
 
 salts. Ammonia behaves similarly, but the precipitate when first produced redissolves 
 in excess of the precipitant, but is thrown down again after the lapse of some time. 
 
 2. Strong nitric acid dissolves brucine and its salts, forming a blood-red solution which becomes 
 
 yellow on heating. On adding stannous chloride or sulphide of ammonium (either to 
 the diluted or undiluted fluid) it acquires an intense violet colour. 
 
 3. Concentrated sulphuric acid dissolves brucine and its salts to a faint rose coloured solution. 
 
 The smallest trace of nitric acid causes the development of a transient red colour, eventually 
 changing to yellow. This reaction is delicate and highly characteristic. 
 
 4. Chlorine-water when added to a solution of a brucine salt colours it red. On addition of 
 
 ammonia the solution becomes yellowish brown. 
 
 5. Sulphocyanate of potassium reacts as with strychnine salts. 
 
 MORPHINE C 17 H 19 NO 3 , H 2 O 
 
 Occurs in the juice of the poppy, along with several other less important alkaloids and meconic acid. 
 The free alkaloid is crystalline, has a bitter taste, is sparingly soluble in cold, but more readily in hot 
 water. It is also soluble in alcohol, and amyl alcohol, but scarcely dissolves in ether or chloroform. 
 
 1. Caustic potash and soda, also ammonia, as well as the carbonates and bicarbonates of potash and 
 
 soda precipitate the free alkaloid from solutions of its salts (if nat too dilute). The 
 precipitate dissolves easily in excess of potash or soda, but is much more sparingly 
 soluble in ammonia. 
 
 2. lodic acid is decomposed by solutions of morphine and its salts, with separation of iodine. The 
 
 latter may be detected by the violet colour which it imparts to chloroform or bisulphide of 
 carbon, or by the blue colour which it strikes with starch paste. 
 
 3. Neutral ferric chloride gives a deep indigo-blue colour with (concentrated) neutral solutions of 
 
 salts of morphine. This reaction is characteristic. 
 
 4. Strong sulphuric acid when warmed with the free alkaloid or its salts gives no colour, 
 
 but on adding to the cooled solution a minute quantity of nitric acid, it assumes a red 
 colour (heating promotes the reaction). If a fragment of bichromate of potash is now 
 placed in the liquid, it acquires an intense mahogany-brown colour. 
 
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 (i) Solutions of strychnine salts give a white cry: 
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 (3) Physiological action. 
 
 (i) Solutions of the acid salts of quinine contaii 
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 (2) Solutions of quinine salts when mixed first i 
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 brown. 
 
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 (i) Ferric chloride colours solutions of salicin a 
 brown, but on boiling, the mixture becomes colour 
 while a dull yellow precipitate is formed. 
 (2) On heating a solution of salicin with nitrat 
 silver to which excess of ammonia has been added 
 either caustic potash or soda, the silver is reduced, 
 a brilliant mirror of metallic silver is formed. 
 
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 cyanide of potassium is added be: 
 ammonia, the solution becomes < 
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 (i) Cinchonine when cautiously 
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 dense, giving crystalline needles. 
 (2) Neutral solutions of cinchoni 
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 (i) Physiological action. 
 
 (i) Chlorine-water (or better 
 colours solutions of brucine salts i 
 adding ammonia the colour becc 
 brown. 
 
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 (i) A peculiar odour of flowers is 
 when atropine or its salts are he 
 sulphuric acid, or chromic acid. 
 (2) Physiological action on the 
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 ( i ) The alkaloid when mixed in 
 with cane sugar and concentrated 
 acid becomes at first yellow, th 
 green, and finally blue. 
 
 
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 added to this solution it becon 
 coloured violet. 
 
 Little or no immediate chan 
 
 Dissolves to a colourless fk 
 (If the alkaloid is evaporated 
 dryness with fuming nitric a 
 and alcoholic potash added to t 
 colourless residue, a violet cok 
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 characteristic.) 
 
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 resinous lumps, which aft 
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 OTHER CHARACTERISTIC REACTIONS. 
 
 (i) Frohde's reagent dissolves codeine at 
 first with a yellow colour, which rapidly 
 becomes deep green, and finally blue. 
 (2) When heated with water, codeine 
 melts and forms oily drops. 
 (3) Dissolved in chlorine-water, codeine 
 gives a colourless solution, which becomes 
 yellow-red on adding ammonia. 
 
 (i) Frohde's reagent dissolves thebaine, 
 forming a blood-red solution. 
 (2) A solution of the alkaloid in chlorine- 
 water becomes coloured an intense red- 
 brown on adding ammonia. 
 (3) Sulphuric acid containing nitric acid is 
 coloured by the alkaloid dark-red or orange. 
 
 (i) Frohde's reagent dissolves narceine, 
 giving at first a brown-green colour, which 
 soon becomes olive-green, and finally blood- 
 red. 
 (2) Iodine-water colours the solid alkaloid 
 an intense blue. 
 (3) Thealkaloid whenstirred withchlorine- 
 water, and then a drop or two of ammonia, 
 gives a deep red solution. 
 
 (i) Frohde's reagent dissolves papaverine 
 in the cold, giving a green colour. On 
 warming, the solution shows a transient blue, 
 and finally a cherry-red colour. 
 (2) Iodine-water colours the alkaloid dark- 
 red, then brick-red, and then dark-red again. 
 (3) With chlorine-water and ammonia the 
 alkaloid gives at first a red-brown, and finally 
 nearly a black-brown solution. 
 
 
 
 
 
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(i) Heated with concentrated sulphuric 
 acid until red, and afterwards mixed with 
 ferric chloride, a violet coloration is at first 
 produced, gradually becoming cherry-red. 
 (2) Frohde's reagent gives the same re- 
 action as with papaverine. 
 (3) Chlorine-water added to a solution of 
 narcotine gives a yellow colour, slightly in- 
 clining to green. On the addition of ammonia 
 a yellowish-red colour is produced. 
 
 (i) Frohde's reagent colours the alkaloid 
 deep chocolate-brown. If a drop of strong 
 hydrochloric acid is added quickly to the 
 mixture, a blue colour is immediately pro- 
 duced, which soon passes into a green. 
 (2) Physiological action (emetic). 
 
 (i) Bleaching powder colours a solution of 
 the alkaloid at first red, but on adding 
 more of the reagent the colour disappears. 
 (2) Bromine-water produces a yellow pre- 
 cipitate in an aqueous solution of the base. 
 (3) Physiological action (contraction of the 
 pupil of the eye). 
 
 (r) Behaves with concentrated sulphuric 
 acid and bichromate of potash, like strychnine, 
 but the colour is more permanent. 
 (2) Physiological action (paralysis of the 
 voluntary muscles.) 
 
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02 
 
 Reactions of the Chief Constituents of Healthy and Morbid 
 
 Urine. 
 
 Human urine when freshly voided is an amber coloured liquid, having a faint acid reaction, a 
 sp. gr. about 1020, and a peculiar characteristic smell. It contains about 95'5 per cent, of water, and 4/5 
 per cent of solids. 
 
 The following table shows the names and average amount of the different solid substances present 
 (Roberts) : 
 
 Urea, ... ... ... ... ... 2-157 
 
 Uric acid, ... ... ... ... ... '036 
 
 " Creatine, ... 
 Creatinine, 
 Ammonia, 
 Hippuric acid, 
 Xanthine, 
 Hypoxanthine, 
 Sarcine, 
 
 . Pigments, etc., 
 Chlorine, ... ... ... ... ... '457 
 
 Sulphuric acid, ... ... ... ... '131 
 
 Phosphoric acid, ... ... ... ... "209 
 
 Potash, ... ... ... ... ... '140 
 
 Soda, -719 
 
 Lime, ... ... ... ... ... 'Oil 
 
 .Magnesia, ... ... ... ... ... '012 
 
 4-525 
 
 w 
 
 02 
 
 Q 
 W 
 
 H 
 
 FM 
 
 653 
 
 The colour, sp. gr., reaction, and odour of normal urine are subject to considerable variations, depending 
 on the nature of the food taken, the amount of liquid consumed, the period at which the urine is 
 voided, the action of certain drugs, etc. Morbid urine may either contain abnormally large proportions 
 of the above constituents or else bodies, such as albumen, sugar, spermatozoa, fat, cystine, pus, etc. 
 
 UREA CO(NH 2 ) 2 
 
 Crystallizes in colourless four-sided prisms. It has a cooling bitter taste like saltpetre. It dissolves 
 readily in water and alcohol. It combines with acids, bases, and salts. 
 
 1 . A concentrated solution of urea is precipitated by strong nitric acid as the nitrate of urea, 
 
 CO(NH 2 )i, HNO 3 , in white glistening plates or scales. 
 A strong solution of oxalic acid throws down the oxalate 2CO(NH 2 ) 2 , C 2 H 2 O 4 . 
 
 2. A dilute solution of urea is precipitated by mercuric nitrate (compounds of mercuric oxide 
 
 and urea being formed). The precipitate is white and flocculent, soluble in a small 
 quantity of common salt solution, but again precipitated on addition of mercuric nitrate. 
 
 3. A solution of urea is decomposed by nitrous acid (or a solution of potassium nitrite, to which 
 
 a drop or two of nitric acid have been added). Effervescence occurs, and the escaping 
 gases consist of nitrogen and carbonic anhydride. The latter can be detected by lime- 
 water CO(NH 2 ) 2 +N 2 O 3 =2N 2 +C(Vf-2H 2 O. 
 
 70 
 
4. Urea is decomposed by potassium hypobromite (made by adding bromine to cold caustic 
 
 potash solution until it ceases to be decolorized), with effervescence, into the same products 
 CO(NH 2 ) 2 + 3KBrO=CO 2 + 2H 2 O + N 2 +3KBr. Only the nitrogen escapes, as the carbonic 
 anhydride is retained in solution as potassium carbonate. 
 
 5. Dry urea when cautiously heated in a dry test tube until it melts, and just begins to disengage 
 
 ammoniacal fumes, is converted into biuret. On dissolving the biuret in water, adding 
 excess of caustic soda, and then drop by drop, a dilute solution of copper sulphate, the 
 solution becomes coloured first red, then red-violet, and finally violet, (biuret reaction). 
 
 UEIC ACID C 5 H 4 N 4 O 3 . 
 
 Pure uric acid is a white powder, very insoluble in water (1 part dissolves in 14,00015,000 of 
 cold, and in 1,800 1,900 of boiling water). It is insoluble in alcohol and ether, but dissolves in caustic 
 potash or soda, and in solutions of. their carbonates and phosphates. It is insoluble in ammonia. It 
 forms two classes of salts, acid and normal, according as one or two of its hydrogen atoms are replaced 
 by metals. From solutions of these it is precipitated by acids. 
 
 I . The most characteristic reaction of uric acid is based upon the production of murexide. 
 
 A few grains of solid uric acid, or a urate, are heated with strong nitric acid, when a brisk 
 effervescence occurs. On evaporating to dryness on a water bath, and exposing the residue 
 (colour either yellow or brick-red ) to the fumes of ammonia, a violet colour is produced 
 (due to the production of murexide or purpurate of ammonium C 8 H 4 NH 4 N 5 O 6 ). 
 
 HIPPURIC ACID C 9 H 9 NO 3 
 
 Crystallizes in white four-sided prisms. Slightly soluble in cold, -more readily in hot water. Soluble with 
 ease in alcohol ; also soluble, though less easily, in ether. It combines readily with bases to form salts, 
 which for the greater part are soluble. When boiled with hydrating agents it is converted into 
 glycocoll and benzoic acid C 9 H 9 NO 3 + H 2 O=C 7 H 6 O 2 +C 2 H 5 NO 2 . 
 
 i. Solid hippuric acid, when gently warmed in a test tube, melts to an oily liquid, then grows red, 
 and is decomposed, giving a sublimate of benzoic acid, and an odour like bitter almonds 
 (benzo-nitrile). 
 
 ALBUMEN. 
 
 Albumen in urine can be detected as follows : 
 
 1 . The urine is boiled in a tube, and a few drops of strong nitric acid are added, (so that the 
 
 mixture has a well marked acid reaction). The presence of albumen is indicated by a 
 flocculent precipitate. (This test is open to the objection that urates may be also 
 precipitated, and also it is not very delicate.) 
 
 2. Concentrated nitric acid is poured cautiously down the side of a test tube containing the urine. 
 
 If albumen is present, a sharply defined cloudy ring appears at the junction of the two fluids 
 (Heller). 
 
 3. The urine is acidulated strongly with acetic acid, then about an equal part of a saturated 
 
 solution of common salt is added, and the mixture boiled. The presence of albumen is 
 indicated by a flocculent precipitate. 
 
 4. The urine is acidulated strongly with acetic acid, and a few drops of ferrocyanide of potassium 
 
 are added. A thick white precipitate is then produced if albumen is present. 
 
 5. On adding albumenous urine to a solution of picric acid, (saturated in the cold) a white 
 
 precipitate is produced. 
 
 71 
 
6. The urine is saturated in the cold with crystallized sulphate of magnesium, then filtered from 
 the undissolved portion, strongly acidulated with acetic acid, and boiled. A flocculent 
 precipitate indicates albumen.* 
 
 BLOOD. 
 
 Blood in urine generally colours the excretion red, brown, or black, and causes it to be turbid. 
 
 1. On examining a test tube full of the urine placed before the slit of the spectroscope two well 
 
 defined absorption bands are seen. 
 
 2. The urine when boiled gives a precipitate of albumen, which is coloured more or less brown. 
 
 3. The urine is made strongly alkaline with caustic soda, and boiled. The haemoglobin of the 
 
 blood is converted into haematin, which adheres to the precipitated earthy phosphates 
 colouring them brown. (This is a very delicate reaction.) 
 
 4. Small quantities of blood in urine are precipitated by tannin. The precipitate may be collected, 
 
 dried in the air, and examined as described at page 89 (under " Blood," test 3). 
 
 BILE. 
 
 Urine containing biliary matters is coloured yellow, brown, or green, and froths when shaken. The 
 following tests for bile pigments may be employed : 
 
 1 . A few cubic centimetres of strong nitric acid (having a yellow colour) are placed in a test tube ; 
 
 the latter is then held in a slanting position, and the urine is carefully poured down 
 the side of the tube, so that it forms a distinct layer above the nitric acid. At the point 
 of junction of the two fluids, a play of colours becomes apparent. If this at any time 
 is green, biliary matters are present (Gmelin). 
 
 2. On adding to the suspected urine a few drops of tincture of iodine, an emerald-green colour is 
 
 produced (Trousseau and Dumontpallier). Bromine-water may be substituted for iodine 
 (Maly). 
 Bile acids may be detected thus : 
 
 A few cubic centimetres of the urine are placed in a test tube along with a fragment of loaf 
 sugar. A small quantity of concentrated sulphuric acid is then poured carefully down the 
 side of the tube, so that it forms a distinct layer at the bottom. At the line of contact of 
 the two liquids a deep purple colour is produced, after a few minutes, if bile acids are 
 present (Pettenkofer and Harley). 
 
 SUGAE. 
 
 Grape Sugar (dextrose) C 6 H 12 O 6 occurs abundantly in the urine of patients suffering from 
 diabetes. In such cases large quantities of urine are often voided. 
 The following tests may be employed : 
 
 1 . The urine is made strongly alkaline with caustic potash or soda, and then boiled for some time. 
 
 If the colour darkens considerably sugar is present (Moore and Heller). Normal urine 
 darkens slightly when boiled with alkalies, and the presence of lead in the latter also 
 causes them to give a dark colour with urine ; so that this test is not very trustworthy in 
 doubtful cases. 
 
 2. As in i, the urine is made strongly alkaline with caustic potash or soda, then rather dilute 
 
 sulphate of copper solution is added drop by drop, (the mixture being shaken vigorously all 
 the time), until a very little of the precipitated hydrate of copper remains undissolved. On 
 
 * Globulin behaves like albumen in all the tests given with the exception of this one. 
 
 72 
 
warming, a yellow or red precipitate of cuprous oxide separates, (if sugar is present) bejore 
 the mixture boils. The heating is then interrupted, and the reduction proceeds by itself 
 (Trommer).* 
 
 3. The urine is made alkaline as before, a solution of nitrate of bismuth is then added until a fair 
 
 amount of precipitate is produced, and the mixture warmed. The precipitate darkens 
 rapidly if sugar is present, and the liquid itself becomes brown (Bottger). 
 
 4. The urine is mixed with a few crumbs of German yeast. A test tube is filled to the brim with 
 
 the mixture, then closed with the thumb, and inverted in a dish or basin containing more 
 of the urine. The tube and basin are then set aside in a warm place (say on the mantel- 
 piece). If sugar is present, fermentation soon occurs and carbonic anhydride is formed, 
 which gradually displaces the urine in the tube (Fermentation test).t 
 
 Urinary Sediments and Calculi. 
 
 Very frequently freshly voided urine is cloudy, or rapidly becomes so on standing, and eventually 
 deposits a sediment. The sediment is caused by the separation of some normal or abnormal constituent 
 the former in excess of normal amount. Should the deposition occur gradually within the bladder or 
 kidney, it not unfrequently happens that the separated particles become agglomerated into a hard mass> 
 which is called a " stone " or u calculus." Urinary sediments may consist of the following : 
 
 1. Uric acid and urates. 
 
 2. Phosphate of lime. 
 
 3. Oxalate of lime. 
 
 4. Phosphate of ammonia and magnesia. 
 
 5. Carbonate of lime. 
 
 6. Cystine. 
 
 7. Fat globules. 
 
 p 
 
 w 
 
 a 
 
 r 
 
 
 
 o 
 
 8. Epithelium. 
 
 9. Mucus. 
 
 10. Pus. 
 
 11. Blood. 
 
 12. Spermatozoa. 
 
 13. Micro-organisms. 
 
 14. Casts of uriniferous tubes. 
 .15. Hydatids. 
 
 and a few other bodies, such as indigo, xanthine, leucine, tyrosine, hippuric acid, sulphate of lime r 
 phosphate of magnesia, etc. Urinary calculi contain the same substances as those present in non- 
 organised sediments, with the exception of hippuric acid and tyrosine. 
 
 * Instead of applying the "reduction test" as above, the following modification may be used if greater certainty is desired: Fill 
 a test tube to the depth of J of an inch or so with "Fehling's solution" (p. 84, footnote), heat until it begins to boil, and then 
 add a drop or two of the suspected urine. If it is ordinary diabetic urine, the mixture after an interval of a few seconds, 
 will suddenly turn to an intense opaque-yellow colour, and in a short time an abundant yellow or red sediment falls to the 
 bottom. If, however, the quantity of sugar present is small, the suspected urine is added more freely, but not beyond a 
 volume equal to that of the test employed. In this latter case it is necessary to raise the mixture once more to the boiling 
 point. It is then allowed to cool slowly. If no suboxide has been thrown down when it has become cold, then the urine 
 mar with certainty be pronounced sugar free (Eoberts). 
 
 t This is often \ised by physicians as a quantitative test the difference in Sp. Gr. before and after fermentation roughly representing 
 the amount of sugar per ounce (Roberts). 
 
 73 
 
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 74 
 
 
 
 
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 Dllowing substances are t 
 
 .R according to p. 72 
 
 o3 
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 chloroform, and then a 
 If indican is present, th< 
 
 must be removed from 
 
 HURETTED HYDROGE 
 
 CD 
 
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 paper, which becomes b 
 
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 with bromine water, p. 
 
 ONE. Urine occasionall 
 
 16 
 
 id 
 
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 large quantities of the 
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 ORGANIZED. 
 
 AMORPHOU 
 
 
 
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 HATE OF LIME. 
 
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CD 
 
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 bJD 
 
 
 IDENTIFICATION. 
 
 t burns when heated, leaving only a 
 
 ered, it dissolves on warming withcaustic 
 m of NH 3 indicates urate of ammonium), 
 murexide reaction, p. 71. 
 
 ble when heated, but a fragment is : 
 when heated on platinum foil before 
 owpipe, if it consists of phosphate of 
 nium and magnesium. 
 e before the blowpipe, if it consists 
 sphate of calcium. 
 Ted calculus dissolves in hydrochloric 
 ition can be tested in the ordinary way 
 ia, and phosphoric acid. 
 
 : when heated does not burn, but dis- 
 in hydrochloric acid with effervescence, 
 gives no precipitate with ammonia, 
 red calculus dissolves without efferves- 
 hloric acid, and the solution gives a 
 with ammonia. 
 
 t burns when heated, and leaves but 
 
 red calculus dissolves in ammonia, and 
 s characteristic crystals on spontaneous 
 
 be extracted from the powdered calculus 
 ia. The solution is filtered and evapor- 
 The residue (well washed with water) 
 stic crystalline compounds (i) when 
 c acid and nitrate of silver, and (2} when 
 rochloric acid. 
 
 'pearance. 
 
 
 C 13 ." 
 
 1 0,3 ~ 
 bfl CX o o 
 
 ^ -d .c ^'3 
 6* ^"o 
 
 CX 
 
 Jl 11 !^! 
 
 (i) A fragment 
 solves afterwards 
 and the solution 
 (2) The powdei 
 cence in hydroc 
 white precipitate 
 
 (i) A fragmen 
 little ash. 
 (2} The powde 
 the solution give 
 evaporation. 
 
 Xanthine may 
 by dilute ammon 
 ated to dryness. 
 gives character! 
 heated with nitri 
 treated with hyd 
 
 OH 
 
 _o 
 
 
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 :h as phosphorus, hydrocyanic acid, alcohol, chloroform, 
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 PRELIMINARY EXAMINATION. 
 
 nd draw what conclusions you can. 
 appearance of the suspected matter, and see whether it is 
 
 t arsenic, stir some of the substance in a roomy beaker \ 
 "rom time to time for hard grains of arsenious anhydride. 
 
 SYTEMATIC EXAMINATION. 
 
 poisons : Reserve from one-third to two-thirds (accordin 
 is follows : 
 
 tion for PHOSPHORUS by placing the suspected mixture 
 oistened with nitrate of silver solution, the other with 
 
 dark and observe whether one or both of the papers are 
 but if both papers are changed, the blackening may be d 
 
 umonia is present the luminosity may be prevented, but acidulation with 
 
 
 
 
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Properties and Reactions of certain other Organic Bodies. 
 
 FORMIC ACID H,CO 2 . 
 
 When pure, formic acid is a slightly fuming liquid, having a pungent and characteristic odour. It 
 boils at 99C, and is miscible in all proportions with water, alcohol, and ether. Its salts are as a rule 
 readily soluble formiate of lead being the least so. Both the free acid and its salts are powerful 
 reducing agents. 
 
 1. Formic acid and its salts (in the solid state) are decomposed when heated with strong sulphuric 
 
 acid, carbonic oxide being formed. Thus : CH 2 O 2 H 2 O=CO. 
 
 2. On warming a solution of a formiate with dilute sulphuric acid, formic acid is liberated and 
 
 may be recognized by its odour ; also by suspending a piece of paper moistened with 
 nitrate of silver in the fumes, which becomes blackened owing to the reduction of the 
 silver. 
 
 3. On warming a formiate with alcohol and strong sulphuric acid, formic ether is produced 
 
 CHO 2 (C 2 H 5 ), which has a characteristic odour resembling rum. 
 
 4. Solutions of formiates when warmed with nitrate of silver give a black precipitate of metallic 
 
 silver. 
 
 5. Solutions of formiates when warmed with mercuric chloride give either a white precipitate of 
 
 calomel, or a grey precipitate of metallic mercury. 
 
 6. Formiates behave with ferric chloride, like acetates. 
 
 BUTYRIC ACIDS C 4 HA- 
 
 The normal acid CH 3 CH,, CH 2 COOH is a colourless oily liquid having a powerful and 
 characteristic odour. It boils at 163C. The iso acid (CH 3 ) 2 =CH COOH much resembles the normal 
 body, but boils at 154C. Both are only sparingly soluble in water. 
 
 1. On warming a butyrate with sulphuric acid, butyric acid is set free, and is easily recognized 
 
 by its odour. 
 
 2. On warming a butyrate with alcohol and strong sulphuric acid, butyric ether C 4 H 7 O L ,(C L ,H 5 ) is 
 
 produced, having a very characteristic odour like pine apples. 
 
 3. Acetate of lead gives a white precipitate with solutions of butyrates (CJE^O^Pb, which on 
 
 warming melts to an oil. 
 
 4. Nitrate of silver gives a white, cheesy or crystalline precipitate C 4 H 7 O 2 Ag. 
 
 5. Ferric chloride gives a brownish-yellow precipitate. 
 
 82 
 
LACTIC ACIDS C 3 H 6 O 3 . 
 
 Three isomers are known (i) ordinary or fermentation lactic acid (a-oxypropionic acid), or 
 ethylidene lactic acid, CH ;t CH(OH) COOH, optically active; (2) sarko-lactic acid, which only 
 differs in being inactive; (3) ethylene lactic acid, (/3-oxypropionic acid), CH 2 (OH) CH., COOH. 
 All three are syrupy liquids having no odour. They are soluble in all proportions in water and alcohol, 
 and dissolve readily in ether also. Heated to 130 150 C. the first two lose water, and give suffocating 
 vapouis of the anhydrides: The reactions of ordinary lactic acid are as follows : 
 
 1. Heated with dilute sulphuric acid, lactic acid, and lactates, yield acetaldehyde and formic acid. 
 
 2. Heated with strong sulphuric acid, carbonic oxide is evolved. 
 
 3. The most characteristic salts are the calcium salt, crystallizing in tufts of needles, and soluble 
 
 in about 10 parts of cold water ; the zinc salt, crystallizing in needles and club-shaped 
 crystals, soluble in about 60 parts of cold water ; the magnesium salt, crystallizing much 
 like the zinc salt, and soluble in about 30 parts of cold water. 
 
 SUCCINIC ACIDS C 4 H 6 O 4 . 
 
 Of these, ethylene succinic acid HOOC CH., CH., COOH is alone of importance. It is solid, 
 and crystallizes in colourless monoclinic prisms. It is soluble in about 23 parts of water at ordinary 
 temperatures, and in about 4 parts of boiling water. When heated, it partly sublimes, and partly loses 
 water to give the anhydride. 
 
 1 . On cautiously warming a solid succinate with about twice as much bisulphate of potash, free 
 
 succinic acid is formed, and condenses in the cold part of the tube, partly in crystals, partly 
 in the form of oily drops which solidify on cooling. 
 
 2. Chloride of barium precipitates moderately strong solutions of succinates when the mixture is 
 
 stirred. The separated crystals have a very characteristic appearance when examined 
 under the microscope. With dilute solutions of succinates, 1 2 volumes of alcohol must 
 be added in order to obtain the barium salt. 
 
 3. Ferric chloride gives a pale rust coloured gelatinous precipitate of basic ferric succinate. 
 
 4. Acetate of lead gives a white amorphous precipitate which redissolves both in excess of the 
 
 succinate and in acetate of lead. On standing, however, the salt soon separates in the 
 crystalline state. 
 
 MALIC ACID C 4 H 6 O 5 . 
 
 The acid is a solid crystalline substance, and dissolves readily in water and in alcohol. When 
 heated, it is resolved into water, maleic acid, and fumaric acid, the two last forming a crystalline 
 sublimate in the upper part of the tube. 
 
 1. Malic acid and its salts when heated with sulphuric acid evolve carbonic oxide and carbonic 
 
 anhydride. The fluid then darkens, and ultimately becomes black. 
 
 2. Chloride of calcium gives no precipitate with malic acid or malates, even when the mixture is 
 
 boiled (unless the solution is very strong). On adding 2 volumes of alcohol, a voluminous 
 white precipitate of malate of calcium is thrown down (C 4 H 4 O 5 )Ca, 3H 2 O. 
 
 83 
 
;. Acetate of lead throws down a white precipitate C 4 H 4 O 5 Pb, 3H...O, which fuses when heated to 
 
 a resinous mass. 
 4. Nitrate of silver gives a white precipitate C 4 H 4 O 5 Ag 2 , which on long standing, or on warming, 
 
 turns somewhat grey. 
 
 BENZOIC ACID C 7 H 6 O a . 
 
 Benzoic acid forms white feathery crystals, which melt at 12r4C, and volatilize slowly even at 
 lower temperatures. The vapour of benzoic acid has a very characteristic aromatic odour. The acid is 
 very sparingly soluble in cold water, more readily in hot water, and dissolves easily in alcohol, ether, 
 alkalies, and to some extent in solution of phosphate of soda. Most benzoates are soluble in water. 
 
 1. Solid benzoic acid and benzoates when distilled with lime evolve benzol : 
 
 C (i H 5 -COOH+CaO=C 6 H 6 +CaCO :J . 
 
 2. Solutions of benzoates, unless very dilute, give a precipitate of benzoic acid with sulphuric 
 
 acid (or other mineral acid), and on warming the mixture, the characteristic odour of 
 benzoic acid is evolved. 
 
 3. Solutions of benzoates when heated with alcohol and strong sulphuric acid emit the charac- 
 
 teristic odour of benzoic ether (C 7 H 5 O 2 )C 2 H 5 . 
 
 4. Solutions of benzoates give (in neutral solutions) a buff coloured precipitate of basic ferric 
 
 benzoate Fe 2 (C 7 H 5 O 2 ) 6 , Fe 2 O 3 . 
 
 5. Solutions of benzoates give a white flocculent precipitate (C 7 H 5 O 2 ) 2 Pb, H-jO, soluble in excess 
 
 of acetate of lead and in acetic acid. 
 
 Carbohydrates. 
 
 Form an important group of organic compounds chiefly of vegetable origin. In addition to carbon 
 they all contain hydrogen and oxygen in the proportions necessary to form water whence their name. 
 All carbohydrates contain either six atoms of carbon or a multiple of six. 
 
 As a class they possess the following characteristic properties, either before or after hydrolysis : 
 i . They reduce easily reducible metals from their solutions. 
 
 2. They give a yellow colour with alkalies. 
 
 3. Heated with sulphuric or hydrochloric acid they decompose giving laevulinic acid, humus-like 
 
 substances, and formic acid. 
 
 4. They give with acetate of phenyl hydrazine, after a short time, a precipitate which usually 
 
 consists of yellow needles. 
 
 5. Nearly (and perhaps) all carbohydrates rotate the plane of a ray of polarized light. 
 
 GLUCOSES C 6 H 12 O 6 . . 
 
 Dextrose (grape sugar) soluble in water and in alcohol. It rotates the ray of polarized light to 
 the right. 
 
 i. Reduces Fehling's solution* at once when the mixture is warmed, red Cu-^O being precipitated. 
 
 " 1 s solution prepared by mixing equal volumes of the following solutions just prior to use : 
 
 1. 34-64 grams, of pure sulphate of copper dissolved in water, so that the mixture occupies (just) oOO cc. 
 
 2. 173 grams of Eochelle salt and 60 grams of caustic soda dissolved in water, so that the mixture occupies 500 cc. 
 
 84 
 
2. Concentrated sulphuric acid does not blacken solid dextrose. 
 
 3. Heated with strong caustic potash solution the mixture turns brown. 
 
 4. Readily ferments with yeast. 
 
 5. Allowed to stand at ordinary temperatures with normal acetate of copper, or warmed with a 
 
 mixture of that salt and acetic acid, and then allowed to stand, reduction and precipitation 
 of cuprous oxide occurs. 
 
 LaBVUlOSe resembles dextrose in most of its properties, but rotates the ray of polarized light to 
 the left. 
 
 SACCHAROSES C 12 H M O n . 
 
 Cane Sugar or sucrose crystallizes in colourless monoclinic prisms (sugar candy), and has a very 
 sweet taste. Easily soluble in water, and sparingly soluble in alcohol. Heated it melts, and on cooling 
 solidifies to a glassy mass (barley sugar). Heated more strongly it turns brown, and decomposes, 
 evolving vapours of characteristic odour. It rotates the ray of polarized light to the right. 
 
 1. When warmed with Fehling*s sohition no change occurs at first, but on prolonged boiling, 
 
 very slow reduction occurs. 
 
 2. Concentrated sulphuric acid blackens solid cane sugar and its strong aqueous solution. 
 
 3. Heated with strong caustic potash solution the mixture does not turn brown. 
 
 4. Allowed to stand at ordinary temperatures with normal acetate of copper solution, or warmed 
 
 with a mixture of that salt and acetic acid and then allowed to stand, no reduction occurs. 
 
 Milk Sugar or lactose C^H^On, H. 2 O forms hard prisms which are not so sweet as cane sugar. 
 It is less soluble in water. Like cane sugar it is dextro-rotatory. 
 
 1. Readily reduces Fehling's solution on warming, cuprous oxide being precipitated. 
 
 2. Concentrated sulphuric acid chars it, but less readily than cane sugar. 
 
 3. Heated with strong caustic potash solution, the mixture turns brown. 
 
 4. Allowed to stand at ordinary temperatures with normal acetate of copper solution, no reduction 
 
 occurs. If a little acetic acid is added, the mixture boiled for a short time, and then allowed 
 to stand, there is also no reduction if the solution is not too concentrated. 
 
 AMYLOIDS (C 6 H 10 5 ),,. 
 
 Starch forms a white amorphous powder. When examined with the microscope it shows a charac- 
 teristic structure, each granule showing concentric laminae, and resembling to a certain extent an oyster 
 shell. The size of the granules varies considerably with the different varieties of starch. When starch 
 is rubbed into a thin paste with cold water, the granules burst and discharge their contents, forming a 
 thick translucent gelatinous mass or if very little of the starch is present a translucent fluid. 
 
 1. Boiled starch paste is precipitated by alcohol ; also by basic acetate of lead, baryta water, lime 
 
 water, tannin, &c. 
 
 2. Starch, especially after it has been boiled with water, gives a deep blue colour, with free iodine. 
 
 The colour is destroyed by heat. This is the most delicate and characteristic test for 
 starch. 
 
 85 
 
3. Starch when boiled with dilute mineral acids, gives a mixture of dextrin and dextrose, or when 
 
 treated with diastase, and certain other unorganized ferments dextrin and maltose. The 
 formation of dextrose occurs according to the equation (C 6 H u A5)n + nH 2 O=n(C 6 H 12 O 6 ). 
 
 4. When heated to 150C, starch is converted into dextrin which readily dissolves in water, and 
 
 gives no blue colour with iodine. 
 
 Dextrin an amorphous powder, readily soluble in water, forming a mucilaginous solution. It 
 has no sweet taste. There are probably several varieties. 
 
 1 . Dextrin (obtained by heating starch) gives a wine-red colour with free iodine. 
 
 2. Allowed to stand at ordinary temperatures with normal acetate of copper, no reduction occurs, 
 
 but on warming, gradual reduction takes place. If a little acetic acid is added to the mixture 
 and it is boiled for a short time, and then allowed to stand, no change takes place. 
 
 3. When boiled with dilute mineral acids, dextrin is converted into dextrose. Thus : 
 
 (CH 10 O e ) n + nH 8 0=n(C 6 H 12 8 ). 
 
 4. Fehling's solution behaves with dextrin as with dextrose, but reduction does not occur quite 
 
 so rapidly. 
 
 Cellulose Solid substance, retaining the structure of the plant fibre from which it has been 
 obtained (e.g., cotton wool). Insoluble in all liquids, except strong sulphuric acid (which dissolves it in 
 the cold, and cupric hydrate dissolved in ammonia). 
 
 i. When dissolved in strong sulphuric acid, and the mixture diluted and boiled, cellulose is 
 converted into dextrose. Thus : (C 6 H 10 O 5 ), 1 +nH 2 O=n(C li H 12 O 6 ). 
 
 Gum (arabic) consists of compounds of arabic acid (C B H U A at 1 20C, C^H^On at 1 00C) with lime 
 and potash. It forms white or slightly yellow transparent or translucent masses. It is soluble with ease in 
 water, forming a mucilaginous liquid, and this solution (if fairly strong) gives a white precipitate with 
 strong alcohol of the original substance. But if hydrochloric acid is previously added, the precipitate 
 consists of arabic acid. Iodine gives no colour with gum, thus distinguishing it from dextrin. 
 
 1. On adding to a gum solution a few drops of sulphate of copper, and then excess of caustic 
 
 soda, a bluish precipitate is produced, which when boiled is not reduced nor blackened. 
 (This reaction distinguishes gum from dextrin and the sugars.) 
 
 2. Basic acetate of lead gives a white gelatinous precipitate a reaction which distinguishes gum 
 
 from dextrin, the sugars, and gelatine. 
 
 ALCOHOL C 2 H (i O 
 
 Is a colourless liquid, lighter than water. Has a burning taste and characteristic odour. It boils at 
 78-4C, and burns when ignited with a blue flame. It is miscible with water and with ether in all 
 proportions, and when pure, with bisulphide of carbon also. 
 
 1. When warmed with bichromate of potash and sulphuric acid, the characteristic odour of 
 
 aldehyde C 2 H 4 O is emitted, and the solution turns green. 
 
 2. When warmed with a solution of iodine in iodide of potassium, and then just enough caustic 
 
 soda solution added to decolorize the mixture, iodoform CHI 3 is produced as a yellow 
 crystalline precipitate. This has a very characteristic appearance when examined with 
 the microscope, the crystals consisting of hexagonal plates or six rayed stars. The crystals 
 and the fluid from which they separate have also a very characteristic saffron-like odour. 
 This reaction is not absolutely characteristic of alcohol, as aldehyde, acetone, acetic ether, 
 and some other substances, also yield iodoform. 
 
 86 
 
3- If strong alcohol is mixed with a solid alkaline, acetate, benzoate, or formiate, and strong 
 sulphuric acid, the mixture when warmed evolves the characteristic odours of the 
 respective ethers. 
 
 4. If bisulphide of carbon is mixed with a solution of caustic potash in pretty strong alcohol, a 
 yellow solution of xanthate of potash is produced 
 
 On adding sulphate of copper, and slightly acidulating with hydrochloric acid, a yellow 
 precipitate of xanthate of copper is produced. 
 
 [Tests 3 and 4 succeed only with strong alcohol. This can be separated from a weak solution 
 by distillation the first portions which pass over being rectified two or three times, if 
 necessary, from solid carbonate of potash.] 
 
 CHLOROFORM CHC1 3 
 
 Is a colourless mobile liquid which is not combustible. It has a characteristic odour and a burning 
 taste. It boils at G1'2C, and dissolves in alcohol and ether in all proportions, but is almost insoluble in 
 water. 
 
 i . On warming chloroform with a strong aqueous solution of caustic potash or soda, to which about 
 ten times as much alcohol has been added, it is rapidly decomposed, giving a mixture of 
 chloride and formiate of the alkali CHC1 3 +4KHO=3KC1 + CHKO 2 + 2H 2 O. The 
 formic acid may be separated by boiling off the spirit, and distilling the residue with 
 dilute sulphuric acid. 
 
 2. On warming a drop or two of chloroform with a mixture of alcoholic potash, and a drop or 
 two of aniline, the intense and disagreeable, but characteristic odour of phenyl iso-nitrile 
 is evolved CHC1 3 +NH(C B H 5 )+3KHO=CN(C 6 H 5 
 
 The purity of chloroform is known by the following properties : 
 
 1. When evaporated on the hand or in a watch glass it should leave no residue and no odour. 
 
 2. When shaken with nitrate of silver solution it should not cause any turbidity. 
 
 3. It should not redden litmus. 
 
 4. It should not colour a mixture of bichromate of potash and sulphuric acid green in the cold. 
 
 5. When boiled with bright metallic sodium the lustre of the metal should not be dimmed. 
 
 6. It should not be coloured brown by caustic potash, nor by strong sulphuric acid. 
 
 CHLORAL HYDRATE CHad-A 
 
 Is a solid crystalline body, which when rubbed in the hand has a fatty feel. It has a strong and 
 characteristic odour and a nauseoxis bitter taste. When heated it melts, then boils, and its vapour 
 condenses in oily drops, which crystallize on cooling. It dissolves easily in water, alcohol, and ether. 
 When thrown on to water, the particles of chloral hydrate gyrate and move about the surface. 
 
 i. On adding caustic potash or soda to a fairly strong solution of chloral hydrate, the fluid 
 becomes milky from the separation of chloroform, the odour of which becomes apparent on 
 warming 
 
 C,H 3 C1 3 O 
 
 87 
 
2. On adding nitrate of silver to a cold solution of chloral hydrate very little if any effect is 
 
 produced, but on adding a little ammonia the odour of chloroform becomes apparent, and 
 the silver is reduced partly in the form of a mirror. 
 
 3. Chloral hydrate when warmed with aniline and alcoholic caustic potash gives the characteristic 
 
 odour of phenyl iso-nitrile. 
 
 GLYCERINE C,H S O 
 
 When pure, is a colourless syrupy liquid, having a sweet taste. It attracts moisture from the air, and is 
 miscible in all proportions with water and alcohol. It is almost insoluble in ether, but dissolves 
 abundantly in a mixture of alcohol and ether. 
 
 1. On moistening a piece of paper with a drop of glycerine the paper becomes marked as with a 
 
 grease spot, but on washing the paper with water and then drying, the spot is removed. 
 
 2. On heating glycerine in a test tube with bisulphate of potash or phosphoric acid, suffocating 
 
 vapours of very characteristic odour are produced. They consist of acroleine C 3 H 4 O. 
 
 [If a solution has to be tested for glycerine it must first be concentrated as far as possible on 
 a water bath.] 
 
 ALBUMENOID BODIES. 
 
 These form the chief part of the organic constituents of animals, and some occur in vegetables also. 
 They contain carbon, hydrogen, nitrogen, oxygen, and sulphur, and there can be no doubt have an 
 exceedingly complex composition. They are usually amorphous, and their solutions are laevorotatory. 
 With the exception of peptones they do not diffuse. They may be divided into the following groups : 
 
 Albumens (serum, egg, plant albumen, &c.) Soluble in water, and coagulated by heat. 
 
 Peptones Soluble in water, and not coagulated by heat. (Peptones are formed by the action 
 of gastric juice, pancreatic ferment, etc., or of boiling dilute acids and alkalies on 
 albumenoid bodies.) 
 
 Globlllines (myosine, globuline, fibrinogen, &c.) Insoluble in water, but soluble in dilute salt 
 solution. 
 
 Derived Albumens (Albumenates) (acid albumen, alkali albumen, caseme, &c.) Insoluble 
 in water and in salt solution. Soluble in dilute acids and alkalies. 
 
 Fibrins Insoluble in water, sparingly soluble in dilute acids, alkalies, and in neutral saline 
 solutions. 
 
 The following reactions are general for all albumenoid bodies : 
 
 i. When heated they char, and evolve vapours having the odour of singed hair, and containing 
 abundance of ammonia. The vapours condense in part on a cold surface, and give reddish 
 oily drops. 
 
 88 
 
2. When boiled with strong alkalies, ammonia is disengaged and the residual solution contains 
 
 an alkaline sulphide. Hence it evolves sulphuretted hydrogen when treated with an 
 excess of acid, and gives a violet colour with nitro-prusside of sodium. 
 
 3. Strong acetic acid dissolves nearly all albumenoids when warmed with them, and from the 
 
 solutions thus obtained ferrocyanide of potassium throws down a white precipitate. 
 
 4. Fairly strong hydrochloric acid when heated with albumenoid bodies decomposes them, the 
 
 fluid becoming violet, and finally brown. 
 
 q. Strong nitric acid colours albumenoids yellow, and on moistening the stain with alkalies, the 
 colour becoming brownish-yellow. (Xantho-proteine reaction.) 
 
 6. When an albumenoid body is mixed with a cold solution containing 2 3 volumes of strong 
 
 sulphuric acid to 1 volume of water and a few drops of a strong solution of cane sugar, a 
 red colour gradually appears (in about half-an-hour), and in 24 hours the mixture is 
 nearly black. 
 
 7. When warmed with Milloris reagent* albumenoid bodies acquire at first a yellow, then a red 
 
 colour. 
 
 8 On adding a drop of sulphate of copper solution to an albumenoid dissolved in caustic soda, 
 and shaking the mixture, the hydrate of copper redissolves and colours the fluid violet. 
 The colour does not disappear on boiling. 
 
 BLOOD. 
 
 1. Blood when examined under the microscope presents a very characteristic appearance. 
 
 Numerous discs or corpuscles are then seen to be floating in a colourless liquid. The size 
 of the corpuscles varies in different animals. Addition of water changes their form, but 
 solutions of certain salts do not do so. A solution of iodide of potassium in four times its 
 weight of water is most suitable for the purpose. Linen, &c., stained with blood may be 
 macerated in this solution, and after remaining three or four hours the corpuscles can be 
 seen in a drop of the liquid squeezed out. 
 
 2. Alkalies decompose the haemoglobin of blood into globulin and haematin. If a few drops of 
 
 caustic potash or soda are added to a mixture of water and blood, the solution exhibits 
 dichroism, being red by reflected, and green by transmitted, light. 
 
 3. If dried blood is warmed with glacial acetic acid, and a very little common salt, haemin 
 
 (hydrochlorate of haematin C 32 H 30 N 4 Fe 2 O 3 , HC1) is produced. A drop of the solution 
 when allowed to evaporate spontaneously gives minute, but highly characteristic, crystals 
 ( Teichmanrfs crystals), which are brown, or brown-red, by transmitted light, but violet > 
 or bluish-black, by reflected light, with a metallic lustre. Crystals of haemin are further 
 characterized by being insoluble in water, alcohol, ether, &c., but they dissolve in caustic 
 soda, forming a solution which is greenish in thin layers. 
 
 This test is delicate and characteristic, and is frequently employed for recognizing blood spots 
 and stains. 
 
 4. A solution of blood, even when very dilute, exhibits two very characteristic absorption bands 
 
 when examined with the spectroscope. 
 
 Prepared by gently warming mercury with an equal volume of strong nitric acid until it is dissolved, then diluting the liquid 
 with twice its bulk of water, and allowing the fluid to settle. Or by adding to a neutral solution of mercuric nitrate a drop 
 or two of red fuming nitric acid. 
 
 89 
 
5- When blood is added, even in veiy minute quantity, to a mixture of equal volumes of 
 turpentine and tincture of guiacum a blue colour is produced almost instantly. (The blue 
 colour is caused by the oxidation of the resin contained in the guiacum tincture, and is 
 produced even when blood is diluted with 10,000 times its volume of water ; but it is not 
 absolutely characteristic, as many inorganic and organic substances-: such as flour, gum, 
 milk, etc., give it also.) 
 
 TANNINS 
 
 Are abundantly distributed in the vegetable kingdom, and cause the astringency of plants. Their 
 reactions are not quite identical, though similar the most important is ordinary tannin : 
 
 Digallic Acid (gallotannic acid) C 14 H 10 O 9 . which when pure forms a pale yellow powder, having 
 an astringent taste. It dissolves easily in water and in alcohol, and to a less extent in ether, though it 
 is easily soluble in acetic ether. It combines with bases, forming salts, which for the greater part are 
 insoluble. Its alkaline salts are exceptions to this rule. Acids precipitate its aqueous solution. 
 
 1. When cautiously warmed, tannin melts and yields (among other bodies) pyrogallic acid, which 
 
 volatilizes and condenses in yellowish drops, becoming crystalline on cooling. 
 
 2. When warmed with strong sulphuric acid to 150C tannin is converted into rufigallic acid 
 
 and other bodies. The mixture is thrown into water, and the turbid liquid thus obtained 
 shaken with acetic ether. The acetic ether is then drawn off, washed by shaking with 
 water, and evaporated to dryness on a water bath. By this means tolerably pure rufigallic 
 acid is obtained. It is characterized by giving a carmine-red solution with cold sulphuric 
 acid, and a transient blue colour with strong caustic potash solution. 
 
 3. On adding an excess of caustic soda to a solution of tannin, a reddish-yellow colour is produced, 
 
 which rapidly changes on contact with air through various shades of red-brown, red, 
 brown-yellow, and yellow. The reaction is delicate. 
 
 4. Ferric chloride gives a blue-black precipitate in a solution of tannin, or if the latter is very 
 
 weak a blue-black colour. (This reaction does not succeed if the tannin solution contains 
 acids or alkalies.) 
 
 5. Sulphate of cinchonine precipitates nearly the whole of the tannin from a solution, in the 
 
 form of a white compound. 
 
 6. A freshly prepared solution of gelatine gives with a solution of tannin a white ropy precipitate, 
 
 which, after washing, is coloured black by ferric chloride, and red by caustic soda. 
 
 GALLIC ACID C 7 H 6 O 5 , H 2 O 
 
 Crystallizes in slender needles. Dissolves with great ease in boiling water, but less readily in cold water. 
 Soluble readily in alcohol, but with difficulty in ether. Acetic ether also dissolves it When heated, it 
 behaves in much the same manner as tannin. 
 
 1. When heated with strong sulphuric acid to 150C it is, like tannin, converted into rufigallic 
 
 acid (see tannin) 2C 7 H 6 O 5 C U H 8 O 8 +2H.O. 
 
 2. It behaves with ferric chloride like tannin. 
 
 90 
 
3. It differs from tannin in being crystalline ; in not being precipitated from aqueous solutions 
 by acids ; and in giving no precipitate with gelatine or sulphate of cinchonine.. 
 
 PYROGALLIC ACID (trioxyphenol) C 6 H 6 O 3 
 
 Forms bulky, colourless needles. Soluble in water, alcohol, and ether. Melts when heated, and 
 volatilizes nearly unchanged. 
 
 1. Nitric acid when warmed with pyrogallic acid attacks it energetically, giving off abundance 
 
 of red fumes, and producing a yellow solution of extraordinary tinctorial power. 1 part 
 of this solution will colour from 2 3 million parts of water yellow. 
 
 2. In the absence of air or oxygen alkalies give a colourless solution with pyrogallic acid, but in 
 
 their presence the solutions almost instantly become yellow or brown. 
 
 3. Lime-water gives a violet colour, which, however, soon becomes red or brown. 
 
 4. A solution of ferrous sulphate (free from ferric salts) gives a colourless solution with pyrogallic 
 
 acid, but if the mixture is vigorously shaken it becomes blue. If a trace of caustic soda is 
 previously added to the pyrogallic solution, ferrous sulphate gives a red liquid, which on 
 shaking becomes violet-blue. 
 
 5. Nitrate of silver is almost instantly reduced by pyrogallic acid. 
 
 PHENOL (carbolic acid^ C 6 H 6 O 
 
 When pure, forms colourless deliquescent crystals, melting at 41 C, and boiling at 183C. It has a 
 persistent and characteristic odour. It is sparingly soluble in water, but dissolves easily in alcohol, 
 ether, chloroform, and alkalies. It volatilizes with steam. 
 
 1. Bromine-water gives a white or yellowish precipitate of tribromo-phenol C 6 H 3 Br 3 O, even in 
 
 very dilute solutions (1 in 60,000). 
 
 2. Ferric chloride gives a violet coloration. 
 
 3. When mixed with nitrite of potassium and strong sulphuric acid, it gives a brown colour, 
 
 changing to green, and finally to blue. 
 
 4. When heated with ammonia and a drop or two of bleaching powder solution, a deep blue 
 
 colour is produced (green in dilute solutions), changed to red by acids. 
 
 5. A pine shaving moistened with hydrochloric acid, is turned purple-red by phenol. 
 
 SALICYLIC ACID (orthoxybenzoic acid) C 7 H 6 O 3 
 
 Forms a white granular powder or prismatic crystals. Nearly insoluble in cold water. Soluble in hot 
 water, alcohol, ether, and alkalies. It melts at 155C. 
 
 1. Solid salicylic acid and its salts when distilled with lime yield phenol, which may be identified 
 
 by its odour, &c. 
 
 2. ^Ferric chloride gives a violet colour, even in very dilute solutions. The colour is destroyed 
 
 by acids or alkalies. 
 
 3. Bromine-water reacts as with phenol, but the reaction is far less delicate. 
 
 91 
 
INDEX 
 
 Acetates, detection, in simple solution, 14, 16, 18. 
 
 ,, ,, complex ,, 49, 51, 52, 53. 
 Acetone, detection, in urine, 75. 
 Acids, biliary, detection of, 72. 
 reactions of, 17. 
 separation of, 52. 
 detection, in simple solution, 12. 
 ,, ,, complex ,, 46. 
 ,, solids, 2, 28. 
 ,, by dry way tests, 20. 
 Aconitine, reactions of, 67. 
 Albumen, reactions of, 71. 
 in urine, 71, 74. 
 
 Albumenoid bodies, reactions of, 88. 
 Alcohol, reactions of, 86. 
 
 detection, in urine, 75. 
 Alkalies, detection of, 10, 20, 44. 
 Alkaline earths, detection of, 10, 20, 44. 
 Alkaloids, reactions of, 66. 
 
 general reagents for the detection of, 60. 
 detection, in simple solution, 63. 
 
 ,, ,, cases of poisoning, 80. 
 Alloys, analysis of, 29. 
 Aluminum, detection, in simple solution, 8. 
 
 ,, ,, complex ,, 40, 42. 
 ,, by dry way tests, 21. 
 Ammonia, detection, in urine, 75. 
 
 calculi, 77, 78. 
 Ammonium, detection, in simple solution, 4. 
 ,, ,, complex ,, 32. 
 ,, by dry way tests, 21, 22. 
 Amyloids, 85. 
 
 Antimony, detection, in simple solution, 6. 
 ,, ,, complex 36. 
 by dry way tests, 20, 21, 26, 27. 
 Arseniates, detection, in simple solution, 16, 19. 
 
 ,, ,, complex ., 51, 52, 54. 
 Arsenic, detection, in simple solution, 6. 
 ,, ,, complex ,, 36. 
 by dry way tests, 20, 21, 22, 26, 27. 
 ,, in cases of poisoning, 81. 
 Atropine, reactions of, 67. 
 
 detection, in simple solution, 63. 
 
 Barium, detection, in simple solution, 10. 
 ,, ,, complex ,, 44. 
 ,, by dry way tests, 20. 
 Bases, detection, in simple solution, 4. 
 ,, ,, complex ,, 32. 
 ,, by dry way tests, 20, 24. 
 ,, in solids, 2, 28. 
 Benzoates, detection, in simple solution, 13, 16, 19. 
 
 ,, ,, complex ,, 48, 51. 
 Benzoic acid, reactions of, 84. 
 Bile, reactions of, 72. 
 in urine, 72, 74. 
 
 Biliary acids, in urine, 72. 
 
 pigments, in urine, 72. 
 Bismuth, detection, in simple solution, 8. 
 ,, ,, complex ,, 38. 
 ,, by dry way testa, .21, 26, 27. 
 Blood, reactions of, 89. 
 in urine, 72, 74. 
 in urinary sediments, 73, 76. 
 Boracic acid, detection, by dry way tests, 20. 
 Borates, detection, in simple solution, 16, 18. 
 ,, complex ,, 51, 52. 
 Borax beads, 20, 27. 
 Bromides, detection, in simple solution, 14, 15, 17. 
 
 ,, complex ,, 49, 50, 52, 54. 
 ,, by dry way tests, 22. 
 Brucine, reactions of, 62, 67. 
 
 detection, in simple solution, 64. 
 Bunsen burner, 25. 
 flame, 25. 
 dry way tests, 24. 
 Butyric acids, reactions of, 82. 
 
 Cadmium, detection, in simple solution, 8. 
 ,, ,, complex ,, 38. 
 ,, by dry way tests, 26, 27. 
 Calcium, detection, in simple solution, 10. 
 ,, ,, complex ,, 44. 
 ,, by dry way tests, 20. 
 carbonate, detection, in urinary calculi, 78. 
 
 ,, sediments, 73, 76. 
 calculi, 77, 78. 
 ,, sediments, 73, 76. 
 simple solution, 8. 
 complex ,, 42. 
 
 oxalate, 
 
 
 phosphate, 
 
 urinary calculi, 77, 78. 
 sediments, 73, 76. 
 
 Calculi, urate, 77. 
 
 phosphate, 77. 
 oxalate, 77. 
 cystine, 77. 
 xanthine, 77. 
 urinary, 73. 
 
 examination of, 77, 78. 
 ammonia in, 77, 78. 
 calcium carbonate in, 78. 
 ,, sulphate in, 78. 
 ,, oxalate in, 77, 78. 
 ,, phosphate in, 77, 78. 
 cystine in, 77, 78. 
 magnesium phosphate in, 77, 78. 
 uric acid in, 77, 78. 
 xanthine in, 77, 78. 
 Cane sugar, reactions of, 85. 
 Carbohydrates, 84. 
 Carbolic acid, reactions of, 91. 
 
 detection, in cases of poisoning, 79. 
 
INDEX Continued 
 
 Carbonates, detection, in simple solution, 12, 17. 
 ,, ,, complex ,, 46, 52. 
 Casts, tube, in urinary sediments, 73, 76. 
 Cellulose, reactions of, 86. 
 Chloral hydrate, reactions of, 87. 
 Chlorates, detection, in simple solution, 13, 18. 
 
 ,, ,, complex ,, 49, 52, 53. 
 ,, by dry way tests, 21, 22. 
 Chlorides, detection, in simple solution, 13, 15, 17. 
 
 ,, ,, complex ,, 49, 50, 52, 53, 54. 
 ,, by dry way tests, 22. 
 Chloroform, reactions of, 87. 
 
 detection, in cases of poisoning, 79. 
 Chromates, detection, in simple solution, 15, 19. 
 ,, ,, complex ,, 50, 52. 
 
 Chrome iron ore, disintegration of, 31. 
 Chromium, detection, in simple solution, 8. 
 
 ,, complex ,, 40, 42. 
 ,, by dry -way tests,' 20. 
 Cinchonine, reactions of, 61, 66. 
 
 detection, in simple solution, 64. 
 Citrates, detection, in simple solution, 14, 19. 
 
 ,, ,, complex ,, 49, 52, 54. 
 Cobalt, detection in simple solution, 8. 
 
 ,, ,, complex ,, 40, 42. 
 ,, by dry way tests, 20. 
 separation of, from nickel, 41. 
 Codeine, reactions of, 68. 
 
 Complex mixtures, detection of bases in, 28, 32. 
 ,, acids ,, 28, 46. 
 ,, ,, poisons ,, 79. 
 Coniine, reactions of, 67. 
 
 detection, in simple solution, 63. 
 Copper, detection, in simple solution, 8. 
 ,, ,, complex ,, 38. 
 ,, by dry way tests, 20, 21. 
 Cyanides, detection, in simple solution, 13, 19. 
 
 ,, ,, complex ,, 48, 52, 54. 
 Cystine, detection, in urinary calculi, 77, 78. 
 
 ,, ,, ,, sediments, 73, 76. 
 Curarine, reactions of, 69. 
 
 Daturine, reactions of, 67. 
 
 Delphinine, ,, ,, 69. 
 
 Dextrin, ,, ,, 86. 
 
 Dextrose, ,, ,,84. 
 
 Diabetic urine, 72, 74. 
 
 Digallic acid, reactions of, 90. 
 
 Digitalin, detection, in simple solution, 65. 
 
 Dissolution of solids, 2, 28. 
 
 Diy way tests, 20. 
 
 Bunsen's, 24. 
 
 Emetine, reactions of, 69. 
 
 Epithelium, in urinary sediments, 73, 76. 
 
 Fat, in tirinary sediments, 73, 76. 
 Fehling's solution, preparation of, 84. 
 Ferricyanides, detection, in simple solution, 13, 19. 
 
 ,, ,, complex 48, 52, 54. 
 Ferrocyanides, detection, in simple solution, 13, 16, 19. 
 
 ,, complex 
 Fibrins, 88. 
 Films (Bunsen's dry way tests), 26. 
 
 action of reagents on, 27. 
 Flames, coloured, 20, 24. 
 structure of, 25. 
 
 48, 51, 52, 54. 
 
 Fluorides, detection, in simple solution, 14, 17. 
 
 ,, ,, complex ,, 49, 52. 
 
 ,, by dry way tests, 22. 
 Formiates, detection, in simple solution, lo. 
 
 ,, complex ,, 50. 
 
 Formic acid, reactions of, 82. 
 Frohde's reagent, preparation of, 66. 
 Fusion mixtures, 3 1 . 
 
 Gallic acid, reactions of, 90. 
 Globulines, 88. 
 Glucoses, 84. 
 
 Glycerine, reactions of, 88. 
 Grape sugar, reactions of, 84. 
 in urine, 72, 75. 
 Gum (arabic), reactions of, 86. 
 
 Hippuric acid, reactions of, 71. 
 
 in urine, 71. 
 Hypochlorites, detection, in simple solution, 13, 18. 
 
 ,, complex ,, 48, 52, 53. 
 
 by dry way tests, 22. 
 Hyposulphites, detection, in simple solution, 12, 18. 
 
 ,, ,, complex ,, 48, 52, 53. 
 
 Indican, detection, in urine, 75. 
 
 Insoluble bodies, 31. 
 
 Iodides, detection, in simple solution, 14, 15, 17. 
 
 ,, ,, complex ,, 49, 50, 52, 54. 
 ,, by dry way tests, 22. 
 Iron (ferrous), detection, in simple solution, 8. 
 (ferric), ,, . 8 - 
 
 detection, in complex solution, 40, 42. 
 ,, by dry way tests, 20. 
 
 Lactic acids, reactions of, 83. 
 
 Lactose, reactions of, 85. 
 
 Laevnlose, properties of, 85. 
 
 Lead, detection, in simple solution, 4, 8. 
 
 ,, ,, complex ,, 34, 38. 
 
 ,, by dry way tests, 20, 21, 26, 27. 
 
 Magnesium, detection, in simple solution, 10. 
 
 ,, ,, complex ,, 42, 44. 
 , , by dry way tests, 2 1 . 
 phosphate, in calculi, 77, 78. 
 phosphate of ammonium and, in urinary sediments, 
 
 73, 76. 
 
 Malic acid, reactions of, 83. 
 Manganese, detection, in simple solution, 8. 
 
 ,, ,, complex ,, 40, 42. 
 ,, by dry way te.sts, 20, 21. 
 Mercury (mercurous), detection, in simple solution, 4. 
 
 ,, ,, complex ,, 34. 
 (mercuric), ,, ,, simple solution, is. 
 
 ,, ,, conlplex ,, 38. 
 detection, by dry way tests, 21, 21, 26, 27. 
 Metals, detection, in simple solution, 4. 
 ,, ,, complex ,, 32. 
 ,, by dry way tests, 20. 
 ,, ,, ,, Bunsen's, 24. 
 
 ,, in solids, 2, 28. 
 reduction of, (Bunsen's dry way tests), 27. 
 
IN DEX Continued. 
 
 Micro-organisms, in urinary sediments, 73, 76. 
 Milk sugar, reactions of, 85. 
 Millon's reagent, preparation of, 89. 
 Morphine, reactions of, 62. 
 
 detection, in simple solution, 63, 66. 
 Mucus, in urinary sediments, 73, 76. 
 Murexide test for uric acid, 71. 
 
 Narceine, reactions of, 68. 
 Narcotine, reactions of, 69. 
 
 detection, in simple solution, 64. 
 Nickel, detection, in simple solution, 8. 
 
 ,, ,, complex ,, 40, 42. 
 ,, by dry way tests, 20. 
 Nicotine, reactions of, 67. 
 
 detection, in simple solution, 63. 
 Nitrates, detection, in simple solution, 15, 17. 
 
 ,, ,, complex ,, 50, 52, 53. 
 ,, by dry -\vay tests, 21, 22. 
 Nitrites, detection, in simple solution, 12, 17. 
 
 ,, ,, complex ,, 46, 52, 53. 
 
 Oxalates, detection, in simple solution, 14, 15. 18. 
 
 ,, ,, complex ,, 50, 52. 
 Oxalate of calcium, in urinary sediments, 73, 76. 
 ,, ,, calculi, 77, 78. 
 
 Papaverine, reactions of, 68. 
 
 Peptones, 88. 
 
 Phenol, reactions of, 91. 
 
 detection in urine, 75. 
 
 ,, in cases of poisoning, 80. 
 Phosphates, detection, in simple solution, 16, 19. 
 
 ,, ,, complex ,, 51, 52, 54. 
 ,, by dry way tests, 22. 
 Phosphate of calcium, in the ammonium sulphide precipitate, 
 
 8, 42. 
 
 in urinary sediments, 73, 76. 
 ,, ,, calculi, 77, 78. 
 Phosphate calculi, 77. 
 
 Phosphate of ammonium and magnesium, in i irinary sediments, 76 . 
 Phospho-molybdic acid, preparation of, 60. 
 Phosphorus, detection in cases of poisoning, 79. 
 Physostigmine, reactions of, 69. 
 Picrotoxin, detection, in simple solution, 65. 
 Poisons, detection of, in complex mixtures, 79. 
 Potassium, detection, in simple solution, 10. 
 ,, ,, complex ,, 44. 
 ,, by dry way tests, 20. 
 Pus, in urinary sediments, 73, 76. 
 Pyrogallic acid, reactions of, 91. 
 
 Quinine, reactions of, 61, 66. 
 
 detection, in simple solution, 64, 65. 
 
 Saccharoses, 85. 
 
 Salicin, detection, in simple solution, 65. 
 
 Salicylic ticid, reactions of, 91. 
 
 Sediments, urinary, 73, 7ti. 
 
 Selenium, detection of, by Him tests, 26, 27. 
 
 Semen, in urinary sediments, 76. 
 
 Separation of acids. 52. 
 
 Silicates, detection, in simple solution, 13, 16, 19. 
 ,, ,, complex ,, 48, 51. 
 ,, by dry way tests, 21. 
 insoluble, disintegration of, 31. 
 Silver, detection, in simple solution, 4. 
 ,, ,, complex ,, 34. 
 ,, by dry way tests, 21. 
 Sodium, detection, in simple solution, 10. 
 ,, ,, complex ,, 44. 
 
 ,, by dry way tests, 20. 
 Solids, dissolution of, 2, 28. 
 Solubility table, 56, 57. 
 
 notes to, 58. 
 Starch, reactions of, 85. 
 Strontium, detection, in simple solution, 10. 
 ,, ,, complex ,, 44. 
 
 ,, by dry way tests, 20. 
 Strychnine, reactions of. 61, 66. 
 
 detection, in simple solution, 65. 
 Succinic acids, reactions of, 83. 
 Sucrose, reactions of, 85. 
 Sugar, detection, in urine, 72, 75. 
 Sulphates, detection, in simple solution, 15, 17. 
 
 ,, ,, complex ,, 50, 52, 53. 
 ,, by dry way tests, 22. 
 Sulphides, detection, in simple solution, 12. 
 
 ,, ,, complex ,, 48, 52. 
 
 ,, by dry way tests, 21, 22. 
 
 Sulphites, detection, in simple solution, 12, 17. 
 
 ,, ,, complex ,, 48, 52, 53. 
 Sulphocyanates, detection, in simple solution, 16, 19. 
 
 ,, ,, complex ,, 51, 52, 53, 54. 
 Sulphuretted hydrogen, detection, in urine, 75. 
 
 Tables, analytical (see Con tents}. 
 
 Tannins, reactions of, 90. 
 
 Tartrates, detection, in simple solution, 14, 19. 
 
 ,, ,, complex ,, 49, 52, 54. 
 Tellurium, detection of, by film tests, 26, 27. 
 Thallium, 26, 27. 
 Thebaine, reactions of, 68. 
 Thiosulphates, detection, in simple solution, 12. 
 ,, ,, complex ,, 48. 
 Tin (stannous), detection, in simple solution, 6. 
 (stannic), ,, 6. 
 
 ,, ,, ,, complex ,, 36. 
 
 ,, ,, by dry M r ay tests, 21. 
 
 Toxicological analysis, 79. 
 Tube casts, in urinary sediments, 73, 76. 
 
 Urate calculi, 77. 
 
 Urates, detection, in urinary sediments. 76. 
 
 Urea, reactions of, 70. 
 
 in urine, 70. 
 
 Uric acid, reactions of, 71. 
 in calculi, 77, 78. 
 in urine, 7 1 . 
 
 detection, in urinary sediments, 76. 
 Urinary calculi, chief constituents of, 73. 
 examination of, 77, 78. 
 ammonia in, 77, 78. 
 calcium carbonate in, 78. 
 ,, sulphate in, 78. 
 ,, oxalate in, 77. 78. 
 ,, phosphate in, 77, 78. 
 cystine in, 77, 78. 
 magnesium phosphate in, 77, 
 uric acid in, 77, 78. 
 Aanthine in, 77, 78. 
 
INDEX Continued. 
 
 Urinary sediments, 73. 
 
 chief constituents of, 73. 
 examination of, 76. 
 detection of blood in, 76. 
 
 carbonate of calcium in, 76. 
 cystine in, 76. 
 epithelium in, 76. 
 fat in, 76. 
 
 micro-organisms in, 76. 
 mucus in, 76. 
 oxalate of calcium in, 76. 
 phosphate of ammonium and 
 
 magnesium in, 76. 
 phosphate of calcium in, 76. 
 pus in, 76. 
 semen in, 76. 
 tube casts in, 76. 
 urates in, 76. 
 uric acid in, 76. 
 Urine, general properties of healthy, 70. 
 chief constituents of healthy, 70. 
 ,, ,, morbid, 70. 
 
 general properties of morbid, 74. 
 examination of morbid, 74. 
 albumen in, 71, 74. 
 bile in, 72, 74. 
 blood in, 72, 74. 
 
 Urine, hippuric acid in, 71. 
 sugar in, 72, 75. 
 urea in, 70. 
 detection of bile acids in, 72. 
 
 ,, pigments in, 72. 
 
 blood in, 74. 
 
 biliary matter in, 74. 
 
 indican in, 75. 
 
 sulphuretted hydrogen in, 75. 
 
 ammonia in, 75. 
 
 phenol in, 75. 
 
 alcohol in. 75. 
 
 albumen in, 74. 
 
 Veratrine, reactions of, 67. 
 
 detection, in simple solution, 64. 
 
 Xanthine, in calculi, 77, 78. 
 
 Zinc, detection, in simple solution, 8. 
 
 ,, ,, complex 40, 42. 
 by dry way tests, 21, 26, 27. 
 
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