56S 
 
 SB 314 135 
 
EXCHANGE 
 
The Conductivities, Temperature Coeffi- 
 cients of Conductivity and Dissociation of 
 Certain Electrolytes from to 35, 
 and of Certain Other Elec- 
 trolytes from 35 to 65. 
 
 DISSERTATION. 
 
 SUBMITTED TO THE BOARD OF UNIVERSITY STUDIES OF THE JOHNS 
 HOPKINS UNIVERSITY IN CONFORMITY WITH THE REQUIRE- 
 MENTS FOR THE DEGREE OF DOCTOR OF PHILOSOPHY. 
 
 BY 
 HENRY HALLOCK HOSFORD, 
 
 J9U 
 
 EASTON, PA.: 
 
 KSCHENBACH PRINTING COMPANY 
 I9II. 
 
The Conductivities, 1 emperature Coeffi- 
 cients of Conductivity and Dissociation of 
 Certain Electrolytes from to 35, 
 and of Certain Other Elec- 
 trolytes from 35 to 65. 
 
 DISSERTATION. 
 
 SUBMITTED TO THE BOARD OF UNIVERSITY STUDIES OF THE JOHNS 
 HOPKINS UNIVERSITY IN CONFORMITY WITH THE REQUIRE- 
 MENTS FOR THE DEGREE OF DOCTOR OF PHILOSOPHY. 
 
 BY 
 
 HENRY HALLOCK HOSFORD. 
 
 H 
 J9JJ 
 
 EASTON, PA.: 
 
 ESCHENBACH PRINTING COMPANY 
 1911. 
 
5(0 
 
ACKNOWLEDGMENT. 
 
 The author wishes to offer his sincere thanks for instruction 
 in lecture room and laboratory to President Remsen, Pro- 
 fessors H. N. Morse, H. C. Jones, Renouf, Bliss, Associate Pro- 
 fessor Acree and Dr. Pfund. 
 
 This investigation was undertaken at the suggestion of Pro- 
 fessor H. C. Jones and was carried out under his supervision. 
 
 251847 
 
CONTENTS. 
 
 Acknowledgment 3 
 
 Historical Review 5 
 
 Purpose of This Investigation 6 
 
 Preparation of Material 6 
 
 Apparatus and Method 7 
 
 Experimental Results 9 
 
 Salts Studied from o to 35 9 
 
 Ammonium Aluminium Sulphate 9 
 
 Ammonium Chromium Sulphate (Violet Variety) 10 
 
 Ammonium Chromium Sulphate (Green Variety) 10 
 
 Ammonium Copper Sulphate 1 1 
 
 Sodium Ferrocyanide 12 
 
 Potassium Sodium Sulphate \2 
 
 Potassium Aluminium Sulphate 13 
 
 Potassium Nickel Sulphate 14 
 
 Potassium Chromium Sulphate (Violet Variety) 15 
 
 Potassium Chromium Sulphate (Green Variety) J 15 
 
 Calcium Formate 16 
 
 Calcium Chromate 17 
 
 Zinc Nitrate 17 
 
 Zinc Acetate 18 
 
 Lead Acetate 19 
 
 Salts Studied from 35 to 65 20 
 
 Ammonium Aluminium Sulphate 20 
 
 Disodium Phosphate 21 
 
 Sodium Tetraborate 21 
 
 Potassium Aluminium Sulphate 22 
 
 Potassium Sulphocyanate 22 
 
 Monopotassium Phosphate 23 
 
 Potassium Acetate 23 
 
 Calcium Chloride 24 
 
 Magnesium Chloride 24 
 
 Manganese Sulphate 25 
 
 Ferric Chloride . '.^. /*., ....:,./.;, ; ...<;. . 26 
 
 Chromium Sulpha te "(Green Variety;.'//. 26 
 
 Nickel Nitrate.?,. .;.;. ..?.,. j...*. .;. ?. . ? . .*. .'.*.' 27 
 
 Nickel Sulphate , .:/. \ .'! ; : . { /.: . ( . . 1 /A .../ 27 
 
 Cobalt Sulphate 28 
 
 Copper Sulphate 28 
 
 Discussion of Results 29 
 
 Summary 41 
 
 Biography 43 
 
THE CONDUCTIVITIES, TEMPERATURE COEFFI- 
 CIENTS OF CONDUCTIVITY AND DISSOCIA- 
 TION OF CERTAIN ELECTROLYTES 
 
 HISTORICAL REVIEW 
 
 Volta, at the end of the eighteenth century, distinguished 
 two classes of conductors of the then recently discovered 
 galvanism. The first class comprised those substances, such 
 as metals, which conduct without chemical change; while 
 conductors of the second class were decomposed by the passage 
 of the current. A few years later, by electrolyzing conduc- 
 tors of the second class, Davy isolated the previously unknown 
 metals of the alkalies and the alkaline earths. Faraday, 1 in 
 1832, published his laws showing the relation between the 
 amount of electricity passed through the electrolyte and the 
 amount of the electrolyte decomposed. 
 
 Measurements of the resistance of solutions of electrolytes 
 were soon made by many investigators. Of these early re- 
 searches those of Hankel, 2 Becquerel, 3 Horsford, 4 Wiedeman, 5 
 Becker, 8 and Beetz 7 may be especially noted. Brief dis- 
 cussions of these and other investigations can be found in 
 Wiedemann's book. 8 
 
 The earlier methods were very imperfect. The continuous 
 current was used, causing polarization of the electrodes, ex- 
 cept in some special cases, as when the metal of the salt was 
 used for the electrodes. The standard method now used 
 practically eliminates polarization by using the alternating 
 current. This method was first developed and used by Kohl- 
 rausch and his coworkers in a series of researches 9 that were 
 far more comprehensive than any preceding investigations. 
 
 1 Exp. Researches, III, Ser. No. 373 (1832). 
 
 2 Pogg. Ann., 69, 255 (1846). 
 
 3 Ann. chim. phys., [3] 17, 267 (1846). 
 
 4 Pogg. Ann., 70, 238 (1847). 
 
 5 Ibid., 99, 225 (1856). 
 
 e Ann. Chem. (Liebig), 73, 1 (1850); 75, 94 (1851). 
 i Pogg. Ann., 117, 1 (1862). 
 
 8 G. Wiedemann: Die Lehre von der Elektricitat, Band I (Braunschweig, 1882). 
 9 For brief discussions and references to original publications see Wiedemann: 
 Loc. cit. 
 
The dissociation theory of Arrhenius 1 imparted new life to 
 conductivity measurements of electrolytes as affording a 
 basis for the accurate determination of the degree of ioniza- 
 tion. 
 
 Following Kohlrausch, many investigations in this field 
 have been carried out, but in most cases with some special 
 object in view which has limited the scope of the work. The 
 researches were concerned with a few substances only, or were 
 confined to a narrow range of temperature and concentration. 
 
 PURPOSE OF THIS INVESTIGATION 
 
 It has seemed desirable to secure conductivity data relative 
 to all the substances in more common use by the chemist, 
 and under the conditions of temperature and dilution at which 
 they are usually employed in chemical work. With this end 
 in view, a systematic study of the electrical conductivities and 
 allied relations of acids, bases and salts in aqueous as well as 
 in nonaqueous solutions, and at various temperatures and 
 concentrations, has been in progress in this laboratory for ten 
 years. Six papers 1 dealing solely with aqueous solutions 
 have been published and other investigations are in progress. 
 
 The work herein described was undertaken as a continua- 
 tion of that already carried out on the general problem. It 
 includes the determination of the electrical conductivities, 
 temperature coefficients of conductivity and percentage dis- 
 sociation of a number of inorganic salts at dilutions ranging 
 from N/2 to N/4O96. Some of the measurements were made 
 over a range of temperature from o to 35, and a part from 
 35 to 65. 
 
 PREPARATION OF MATERIAL 
 
 The salts used were the purest available. In nearly all 
 cases Kahlbaum's chemicals were employed. These were re- 
 crystallized from one to five times, the final crystallizations 
 in all cases being made from water of special purity or so-called 
 "conductivity water." Any deviations from this general 
 
 Z. physik. Chem., 1, 631 (1881). Scientific Memoirs, Series IV, p. 47. 
 
 2 Jones and Douglas: Am. Chem. J., 26, 428 (1901). Jones and West: Ibid., 34, 
 357 (1905). Jones and Jacobson: Ibid., 40, 355 (1908). Clover and Jones: Ibid., 43, 
 187 (1910). White and Jones: Ibid., 44, 159 (1910). West and Jones; Ibid., 44, 
 508 (1910). 
 
procedure are stated in connection with the experimental 
 data under each salt. 
 
 The water used in making up the solutions was prepared 
 by a modification of the method of Jones and Mackay, 1 i. e., by 
 subjecting the distilled water of the laboratory to three ad- 
 ditional distillations: first in the presence of potassium di- 
 chromate and sulphuric acid to oxidize organic matter and re- 
 tain ammonia, and twice with barium hydroxide to absorb 
 carbon dioxide. The conductivity of such water varies from , 
 i.o to 1.5 X io~". The correction of the molecular conduc- 
 tivity due to this cause is negligible in the greater concentra- 
 tions, but was calculated and applied to the conductivity 
 values obtained for the dilute solutions. 
 
 APPARATUS AND METHOD 
 
 The Kohlrausch method was used in this investigation. 
 In the work from 35 to 65 a slide- wire bridge of the usual 
 type was employed, while measurements from o to 35 were 
 made by means of an improved slide-wire bridge made by 
 Leeds and Northrup, the wire being about five meters long. 
 The bridges and resistance coils were standardized by Leeds 
 and Northrup and also by means of resistances which had been 
 corrected by the U. S. Bureau of Standards. 
 
 The conductivity cells were of the type used and described 
 by Clover and Jones 2 and Jones and West. 3 The constants 
 of these cells were determined at short intervals. In connec- 
 tion with the work from o to 35 the following method of 
 determining the constants was employed. A 0.02 N solution 
 of carefully purified potassium chloride was prepared, using 
 water of special purity. The molecular conductivity of this 
 solution at 25 was assumed to have Kohlrausch's value of 
 129.7, an( i this solution was used to determine the constants 
 of the cells designed for concentrated solutions. A 0.002 N 
 solution of potassium chloride was also prepared, and its 
 molecular conductivity found by means of a cell whose con- 
 stant had been determined as explained above. This 0.002 N 
 
 i Z. physik. Chem., 14, 317 (1894). Am. Chem. J., If, 91 (1897). 
 a Am. Chem. J., 43, 192 (1910). 
 4, 510 (1910). 
 
8 
 
 solution was then used in finding the constants of the cells 
 intended for the more dilute solutions. 
 
 In connection with the work from o to 35, a slightly differ- 
 ent plan was adopted. Solutions of potassium chloride of 
 0.02 N and 0.002 N concentration were prepared and used as de- 
 scribed; but a fixed value of 136.5 at 25 was taken for the 
 molecular conductivity of the 0.002 N solution. This value is 
 based on repeated measurements made in this laboratory. 
 
 So far as possible the initial or mother solution of each salt 
 was prepared by direct weighing of the properly purified sub- 
 stance. If this was impracticable a mother solution of con- 
 venient strength was made up and standardized by analysis. 
 From the mother solution the various concentrations were 
 prepared by dilution. In the case of the work from o to 35, 
 solutions were made up at 20 and were used without correc- 
 tions at the various temperatures at which measurements 
 were made, the correction being less than the known experi- 
 mental error. When working from 35 to 65 solutions were 
 prepared at 50, and a factor was employed in the reduction 
 of all measurements made at 35 and 65 to correct for the 
 change in concentration due to change in volume. The cor- 
 rection factor for the molecular conductivity of solutions 
 made at 50 and used at 35 is 0.994; f r those made at 50 
 and used at 65 the value is i .0076. The burettes and meas- 
 uring flasks used in making up solutions were carefully cali- 
 brated for the temperature at which they were to be used. 
 
 For the work at o an ice bath was employed in which the 
 cells were supported so as to be immersed as deeply as possi- 
 ble in the crushed ice and water. A shallow vessel filled with 
 ice and water covered the ice baths when in use. Connections 
 were made through openings closed with perforated stoppers 
 carrying the conducting wires. The baths for higher tem- 
 peratures were properly sheathed with asbestos cement, and 
 in the case of the 50 and 65 baths efficient covers were pro- 
 vided to retain the heat. Hot-air engines were used to stir 
 the baths. It was found easy to keep the temperature of the 
 baths constant to within o.02 or o.o3 by hand regulation, 
 and this method was adopted. 
 
From two to four independent measurements of the con- 
 ductivity were made for each concentration at each tempera- 
 ture. If there was not close agreement in the results, or if any 
 abnormally large errors were suspected, the measurements 
 were repeated. So far as possible my results were compared 
 with those obtained by other workers. In most cases there is 
 reasonable agreement. When wide discrepancies appeared 
 my work was duplicated. 
 
 Concentrations are indicated under the heading V, or 
 the number of liters which would contain one gram- 
 molecular weight of the salt. Molecular conductivities are 
 expressed in Siemens' units. The temperature coefficients 
 and dissociation were calculated in the usual way. On ac- 
 count of hydrolysis or other causes, the maximum value of 
 the molecular conductivity (p^) was not found for certain 
 salts at the greatest dilution worked with. In such cases the 
 dissociation was not calculated. 
 
 Ammonium Aluminium Sulphate, NH 4 Al(SO 4 ) 2 .i2H 2 O 
 The mother solution was standardized by determining 
 aluminium as aluminium oxide. 
 
 Table I. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35* 
 
 8 
 
 8o.o 
 
 II0.9 
 
 H3 -I 
 
 168.8 
 
 32 
 
 IO2 .5 
 
 I43-I 
 
 185-5 
 
 22O-4 
 
 128 
 
 I30.I 
 
 182.7 
 
 238.8 
 
 284.8 
 
 512 
 
 l62 .2 
 
 230.9 
 
 304-5 
 
 365-9 
 
 1024 
 
 iSl.O 
 
 257-5 
 
 342-4 
 
 4 I 5-i 
 
 2048 
 
 201.8 
 
 288.2 
 
 386.4 
 
 485.8 
 
 4096 
 
 224. I 
 
 322.8 
 
 437-6 
 
 540-3 
 
 Table II. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 2.47 
 
 3-09 
 
 2.58 
 
 2-33 
 
 2-57 
 
 I. 80 
 
 32 
 
 3-25 
 
 3-17 
 
 3-39 
 
 2-37 
 
 3-49 
 
 1.88 
 
 128 
 
 4.21 
 
 3-24 
 
 4-49 
 
 2 .46 
 
 4.60 
 
 i-93 
 
 512 
 
 5-50 
 
 3-39 
 
 5-89 
 
 2-55 
 
 6. 14 
 
 2 .02 
 
 1024 
 
 6.12 
 
 3-38 
 
 6.79 
 
 2.64 
 
 7.27 
 
 2 . 12 
 
 2048 
 
 6.91 
 
 3-42 
 
 7.86 
 
 2 - 73 
 
 9-94 
 
 2-57 
 
 4096 
 
 7.90 
 
 3-53 
 
 8.38 
 
 2 .60 
 
 10.27 
 
 2-35 
 
10 
 
 Ammonium Chromium Sulphate (Violet Variety), 
 NH 4 Cr($O 4 ) 2 .i2H 2 
 
 The mother solution was standardized in the same manner 
 as in the case of the potassium salt. 
 
 Table HI. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 8 
 
 77-5 
 
 106.4 
 
 137-3 
 
 162.7 
 
 16 
 
 88.9 
 
 123.2 
 
 159-5 
 
 188.3 
 
 32 
 
 100.8 
 
 140.3 
 
 182.2 
 
 216.0 
 
 128 
 
 129-5 
 
 183.0 
 
 240.2 
 
 285.9 
 
 512 
 
 165 5 
 
 238.0 
 
 321.0 
 
 385.9 
 
 1024 
 
 187.0 
 
 272.0 
 
 372.0 
 
 455-7 
 
 2048 
 
 211 .9 
 
 310.7 
 
 428.5 
 
 530-0 
 
 4096 
 
 240.7 
 
 355-6 
 
 492.2 
 
 617.0 
 
 Table IV. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35 < 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 2.31 
 
 2. 9 8 
 
 2.47 
 
 2.32 
 
 2-54 
 
 1-85 
 
 16 
 
 2.74 
 
 3.08 
 
 2 .90 
 
 2-35 
 
 2.88 
 
 1.81 
 
 32 
 
 3-16 
 
 3-H 
 
 3-35 
 
 2-39 
 
 3.38 
 
 1.86 
 
 128 
 
 4.28 
 
 3-31 
 
 4-57 
 
 2.5 
 
 4-57 
 
 1.90 
 
 512 
 
 5.80 
 
 3-51 
 
 6.64 
 
 2.79 
 
 6.49 
 
 2 .02 
 
 1024 
 
 6.80 
 
 3-64 
 
 8.00 
 
 2-94 
 
 8-37 
 
 2-25 
 
 2048 
 
 7.90 
 
 3-73 
 
 9.40 
 
 3-03 
 
 10. 15 
 
 2-37 
 
 4096 9.19 3.82 10.93 3.07 12.48 2.54 
 
 Ammonium Chromium Sulphate (Green Variety) 
 
 The mother solution was prepared by heating a portion of 
 the mother solution of the violet variety to 70 for about 
 seven hours in a stoppered bottle. 
 
 Table V. Molecular Conductivity 
 
 V 
 
 o 9 
 
 12. 5 
 
 25 
 
 35 
 
 8 
 
 103.6 
 
 133-2 
 
 162.9 
 
 185.3 
 
 16 
 
 119.7 
 
 155-4 
 
 190.6 
 
 219.3 
 
 32 
 
 136.4 
 
 178.2 
 
 220.8 
 
 255-1 
 
 128 
 
 172.3 
 
 228.4 
 
 288.1 
 
 336.4 
 
 512 
 
 202.6 
 
 274.4 
 
 355-7 
 
 423.2 
 
 1024 
 
 215.6 
 
 294.2 
 
 386.2 
 
 471.2 
 
 2048 
 
 222.0 
 
 3I3-5 
 
 414.0 
 
 518.4 
 
 4096 
 
 234-4 
 
 328. 4 
 
 458.1 
 
 593-8 
 
1 1 
 
 Table VI. Temperature Coefficients 
 
 0-12.5 
 
 12. 5-25 
 
 25-35 a 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 2-37 
 
 2.29 
 
 2. 3 8 
 
 1.79 
 
 2.24 
 
 I. 3 8 
 
 2.70 
 
 2 .26 
 
 2.82 
 
 1.82 
 
 2.87 
 
 I-5I 
 
 3-34 
 
 2-45 
 
 3-41 
 
 I.9I 
 
 3-43 
 
 i-55 
 
 4-49 
 
 2.6l 
 
 4.78 
 
 2.09 
 
 4-83 
 
 1.68 
 
 5-74 
 
 2.8 3 
 
 6. so 
 
 2-37 
 
 6-75 
 
 i .90 
 
 6. 29 
 
 2.92 
 
 7.36 
 
 2.50 
 
 8.50 
 
 2.20 
 
 7-32 
 
 3-37 
 
 8.04 
 
 2-57 
 
 10.44 
 
 2.52 
 
 7-52 
 
 3-21 
 
 10.38 
 
 3.16 
 
 13-57 
 
 2.96 
 
 V 
 
 8 
 
 16 
 
 32 
 
 128 
 
 512 
 
 1024 
 
 2048 
 
 4096 
 
 Ammonium Copper Sulphate, (NH 4 ) 2 Cu(SO 4 ) 2 .6H 2 O 
 
 The mother solution was standardized by determining the 
 sulphuric acid as barium sulphate, and the copper was also 
 determined as copper oxide. 
 
 Table VII. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25' 
 
 35- 
 
 4 
 
 106.3 
 
 146.6 
 
 190.4 
 
 225.7 
 
 8 
 
 122.7 
 
 169.9 
 
 220. 7 
 
 262.2 
 
 32 
 
 153-5 
 
 213.8 
 
 280.2 
 
 334-3 
 
 128 
 
 187.8 
 
 262.4 
 
 346.7 
 
 412 .6 
 
 512 
 
 221 .6 
 
 312 . I 
 
 411.7 
 
 495-7 
 
 1024 
 
 236.0 
 
 333-5 
 
 442.6 
 
 532.5 
 
 2048 
 
 246.4 
 
 347-9 
 
 463.6 
 
 560.0 
 
 4096 
 
 259 4 
 
 367-3 
 
 494.0 
 
 597-3 
 
 Table VI II. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35* 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 3-22 
 
 3 03 
 
 3 50 
 
 2-39 
 
 3-53 
 
 1-85 
 
 8 
 
 3-78 
 
 3.08 
 
 4.06 
 
 2-39 
 
 4-15 
 
 1.88 
 
 32 
 
 4.82 
 
 3-H 
 
 5-3i 
 
 2.48 
 
 5-4 1 
 
 i 93 
 
 128 5.97 3.18 6.74 2.57 6.59 1.90 
 
 512 7.24 3.27 7.97 2.55 8.40 2.04 
 
 1024 7.80 3.31 8.73 2.62 8.99 2.03 
 
 2048 8.12 3.30 9.26 2.66 9.64 2.08 
 
 4096 8.63 3.33 10.14 2.76 10.33 2.09 
 
12 
 
 Sodium Ferrocyanide, Na 4 Fe(CN) 6 . i2H 2 O 
 
 The mother solution was made up by direct weighing of the 
 anhydrous salt. 
 
 Table IX. Molecular Conductivity 
 
 V 12. 5 25 35 
 
 8 
 
 136.7 
 
 194.9 
 
 259.2 
 
 3I3-4 
 
 i6 
 
 I5I-3 
 
 215-5 
 
 287.0 
 
 347 7 
 
 32 
 
 167. i 
 
 238-5 
 
 318.5 
 
 386.2 
 
 128 
 
 203.5 
 
 289.6 
 
 385-9 
 
 464.5 
 
 512 
 
 234.2 
 
 334-1 
 
 446.4 
 
 543-2 
 
 1024 
 
 253-4 
 
 361.7 
 
 482.4 
 
 581.2 
 
 2048 
 
 266.4 
 
 380.3 
 
 504.0 
 
 612 .0 
 
 4096 
 
 275-7 
 
 398.1 
 
 527-1 
 
 632.2 
 
 Table X. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 4.66 
 
 3-41 
 
 5-14 
 
 2 .64 
 
 5-42 
 
 2 .09 
 
 16 
 
 5-H 
 
 3-40 
 
 5-72 
 
 2.6 5 
 
 6.07 
 
 2. 12 
 
 32 
 
 5-71 
 
 3-42 
 
 6.40 
 
 2.68 
 
 6.77 
 
 2.13 
 
 128 
 
 6.89 
 
 3-39 
 
 7.70 
 
 2.66 
 
 7.86 
 
 2.04 
 
 512 
 
 7-99 
 
 3-4i 
 
 8.98 
 
 2.69 
 
 9.68 
 
 2.17 
 
 1024 
 
 8.66 
 
 3-42 
 
 9.66 
 
 2.67 
 
 9.88 
 
 2-05 
 
 2048 
 
 9.11 
 
 3-42 
 
 9.90 
 
 2.60 
 
 10.80 
 
 2.14 
 
 4096 
 
 9-79 
 
 3-55 
 
 10.32 
 
 2-59 
 
 10.51 
 
 2.00 
 
 Table XL Percentage Disssociation 
 
 12. 5 25 35 
 
 8 49.58 48.96 49.18 49.57 
 
 16 
 
 54-88 
 
 54-13 
 
 54-45 
 
 55-00 
 
 32 
 
 60. 61 
 
 59-91 
 
 60.43 
 
 61 .09 
 
 128 
 
 73-8i 
 
 72.74 
 
 73-21 
 
 73-47 
 
 512 
 
 84-95 
 
 83.92 
 
 84.69 
 
 85-92 
 
 1024 
 
 91.91 
 
 90.86 
 
 9I-52 
 
 91-93 
 
 2048 
 
 96.63 
 
 95-53 
 
 95.62 
 
 96.81 
 
 4096 100.00 loo.oo loo.oo 100.00 
 
 Potassium Sodium Sulphate, KNaSO 4 
 
 The mother solution was standardized by determining 
 sulphuric acid as barium sulphate. 
 
13 
 Table XII. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 88.4 
 
 122.5 
 
 159-0 
 
 189.6 
 
 8 
 
 96. i 
 
 146.6 
 
 170.6 
 
 2O9. I 
 
 32 
 
 113.0 
 
 I58.I 
 
 2O7.2 
 
 249.7 
 
 128 
 
 128.8 
 
 179.0 
 
 236.1 
 
 284.5 
 
 512 
 
 135-6 
 
 189.6 
 
 250.8 
 
 301.0 
 
 1024 
 
 140.8 
 
 I97.I 
 
 259-2 
 
 3I3-2 
 
 2048 
 
 140.9 
 
 198.2 
 
 26l .4 
 
 316.2 
 
 4096 144-3 202.6 267.6 322.1 
 
 Table XIII. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 2-73 
 
 3-09 
 
 2 .92 
 
 2.38 
 
 3.06 
 
 1.92 
 
 8 
 
 4.04 
 
 4-30 
 
 1.92 
 
 1.30 
 
 3-85 
 
 I 79 
 
 32 
 
 3-68 
 
 3-26 
 
 3-93 
 
 2-49 
 
 4-25 
 
 2.05 
 
 128 
 
 4.02 
 
 3.12 
 
 4-57 
 
 2-55 
 
 4.84 
 
 2.05 
 
 512 
 
 4-32 
 
 3-19 
 
 4.90 
 
 2.58 
 
 5.02 
 
 2 .OO 
 
 1024 
 
 4-50 
 
 3-20 
 
 4-97 
 
 2.52 
 
 5-4 
 
 2.08 
 
 2048 
 
 4-58 
 
 3-25 
 
 5.06 
 
 2-55 
 
 5-48 
 
 2. 10 
 
 4096 4.66 3.23 5.20 2.56 5.45 2.04 
 Table XIV. Percentage Dissociation 
 
 V 12. 5 25 35 
 
 4 61.26 60.46 59-42 58.88 
 
 8 66.60 72.36 63.75 64.93 
 
 32 
 
 78.31 
 
 78.03 
 
 77-43 
 
 77-54 
 
 128 
 
 89.26 
 
 88.35 
 
 88.23 
 
 88-35 
 
 512 
 
 93-97 
 
 93.58 
 
 93-72 
 
 93-47 
 
 1024 
 
 97-57 
 
 97.28 
 
 96.86 
 
 97.26 
 
 2048 
 
 97.64 
 
 97-83 
 
 97-68 
 
 98.19 
 
 4096 
 
 100.00 
 
 IOO.OO 
 
 100.00 
 
 100.00 
 
 Potassium Aluminium Sulphate, KAl(SO 4 ) 2 .i2H 2 O 
 The mother solution was standardized by determining 
 aluminium as aluminium oxide. 
 
 Table XV. Molecular Conductivity 
 
 V 12. 5 25 35 
 
 78.9 108.9 I 4-3 l6 5-3 
 
 32 
 
 101 .2 
 
 140.8 
 
 182.2 
 
 215-7 
 
 128 
 
 127.6 
 
 177.7 
 
 232.9 
 
 283.7 
 
 512 
 
 158.8 
 
 223.7 
 
 294.9 
 
 358.3 
 
 1024 
 
 177-8 
 
 250.5 
 
 332-7 
 
 402.8 
 
 2048 
 
 197-5 
 
 281.8 
 
 378.4 
 
 470.0 
 
 4096 
 
 218.8 
 
 3I4-7 
 
 425.5 
 
 528.8 
 
14 
 Table XVI. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 2.40 
 
 3-04 
 
 2-51 
 
 2.30 
 
 2.50 
 
 1.78 
 
 32 
 
 3-17 
 
 3-13 
 
 3-31 
 
 2-35 
 
 3-35 
 
 1.84 
 
 128 
 
 4.01 
 
 3-14 
 
 4.42 
 
 2 49 
 
 5.08 
 
 2.18 
 
 512 
 
 5-19 
 
 3-27 
 
 5-69 
 
 2-54 
 
 6-34 
 
 2.15 
 
 1024 
 
 5-81 
 
 3-27 
 
 6-57 
 
 2.62 
 
 7.01 
 
 2 . II 
 
 2048 
 
 6.74 
 
 3-41 
 
 7-73 
 
 2.74 
 
 9. 16 
 
 2.42 
 
 4096 
 
 7.67 
 
 3-51 
 
 8.86 
 
 2.82 
 
 10-33 
 
 2-43 
 
 Potassium Nickel Sulphate, K 2 Ni(SO 4 ) 2 .6H 2 O 
 The mother solution was standardized by determining 
 sulphuric acid as barium sulphate and also by determining 
 nickel as oxide. 
 
 Table XVII. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 8 
 
 122 .6 
 
 170.7 
 
 221 .9 
 
 265.3 
 
 32 
 
 155-4 
 
 217.0 
 
 28 3 -8 
 
 339-7 
 
 128 
 
 187-5 
 
 263.0 
 
 344-8 
 
 414.1 
 
 512 
 
 219.6 
 
 309 3 
 
 407.7 
 
 490.7 
 
 1024 
 
 235-5 
 
 331-2 
 
 437-1 
 
 527-1 
 
 2048 
 
 249 5 
 
 349-9 
 
 463.0 
 
 560.1 
 
 4096 
 
 26o.8 
 
 367-9 
 
 487.4 
 
 588.1 
 
 Table XVIII. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35< 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 3-85 
 
 3-14 
 
 4. 10 
 
 2.40 
 
 4-34 
 
 1.96 
 
 32 
 
 4 93 
 
 3.17 
 
 5-32 
 
 2-45 
 
 5-59 
 
 i-97 
 
 128 
 
 6.04 
 
 3.22 
 
 6-54 
 
 2.48 
 
 6-93 
 
 2.01 
 
 512 
 
 7-18 
 
 3-27 
 
 7-87 
 
 2-54 
 
 8.30 
 
 2.O4 
 
 1024 
 
 7.66 
 
 3-25 
 
 8.47 
 
 2.56 
 
 9.00 
 
 2.06 
 
 2048 
 
 8.03 
 
 3.22 
 
 9 05 
 
 2-59 
 
 9.71 
 
 2.09 
 
 4096 8.57 3.29 9.56 2.60 10.07 2.07 
 Table XIX. Percentage Dissociation 
 
 V 12. 5 25 35 
 
 47.01 46.40 45.53 45.11 
 
 32 
 
 59-59 
 
 58.98 
 
 58.23 
 
 57-76 
 
 128 
 
 71.89 
 
 71.49 
 
 70.74 
 
 70.41 
 
 512 
 
 84.20 
 
 84-07 
 
 83.65 
 
 83.44 
 
 1024 
 
 90.30 
 
 90.02 
 
 89.68 
 
 89.63 
 
 2048 
 
 95 67 
 
 95 ii 
 
 94-99 
 
 95-24 
 
 4096 
 
 IOO.OO 
 
 IOO.OO 
 
 IOO.OO 
 
 100.00 
 
15 
 
 Potassium Chromium Sulphate ( Violet Variety) , 
 KCr(SO 4 ) a .i2H a O 
 
 The mother solution was standardized by determining 
 chromium as chromic oxide and also by determining sulphuric 
 acid as barium sulphate. 
 
 
 Table XX. 
 
 Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 8 
 
 75-8 
 
 105.0 
 
 135-3 
 
 159 4 
 
 16 
 
 87-3 
 
 121 .2 
 
 157-3 
 
 185.3 
 
 32 
 
 99.0 
 
 I38.I 
 
 179.6 
 
 2II.3 
 
 128 
 
 127.0 
 
 179-5 
 
 236.7 
 
 279.9 
 
 512 
 
 161 . i 
 
 232.0 
 
 3II-5 
 
 374-5 
 
 1024 
 
 186.6 
 
 271 .6 
 
 369.6 
 
 443-8 
 
 2048 
 
 213-3 
 
 3I4-2 
 
 428.8 
 
 520.6 
 
 4096 
 
 245.8 
 
 364.8 
 
 500.1 
 
 613.9 
 
 Table XXI. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35' 
 
 Cond. Per Cond. Per Cond. Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 2-34 
 
 3.09 
 
 2.42 
 
 2.31 
 
 2. 4 I 
 
 1.78 
 
 16 
 
 2.71 
 
 3.10 
 
 2.89 
 
 2. 3 8 
 
 2.80 
 
 1.78 
 
 32 
 
 3-13 
 
 3 .I6 
 
 3-32 
 
 2.40 
 
 3-17 
 
 1.77 
 
 128 
 
 4.20 
 
 3.31 
 
 4-58 
 
 2-55 
 
 4-32 
 
 1.82 
 
 512 
 
 5.67 
 
 3-52 
 
 6.36 
 
 2.74 
 
 6.30 
 
 2 .02 
 
 1024 
 
 6.80 
 
 3-64 
 
 7-84 
 
 2.89 
 
 7-42 
 
 2.01 
 
 2048 
 
 8.07 
 
 3-78 
 
 9.17 
 
 2 .92 
 
 9.18 
 
 2.14 
 
 4096 
 
 9 52 
 
 3-87 
 
 10.82 
 
 2.97 
 
 11.38 
 
 2.28 
 
 Potassium Chromium Sulphate (Green Variety) 
 The mother solution was prepared by heating a portion of 
 the mother solution of the violet variety to 70 for about seven 
 hours in a stoppered bottle. 
 
 Table XXII. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 8 
 
 101 .0 
 
 I30.I 
 
 158.4 
 
 179.6 
 
 16 
 
 H9 3 
 
 154.0 
 
 I88.I 
 
 213.2 
 
 32 
 
 137 8 
 
 179 3 
 
 219-5 
 
 249-3 
 
 128 
 
 177.7 
 
 234 4 
 
 290.6 
 
 333-5 
 
 512 
 
 210.9 
 
 283-5 
 
 359-i 
 
 426.6 
 
 1024 
 
 229.7 
 
 310.9 
 
 399 -6 
 
 479-0 
 
 2048 
 
 247.0 
 
 339-5 
 
 441-3 
 
 539-1 
 
 4096 
 
 273.1 
 
 379-4 
 
 500.3 
 
 616.2 
 
i6 
 
 Table XXIII. 
 
 Temperature Coefficients 
 
 
 0-12 
 
 . 5 
 
 12. 5-25 
 
 25-35 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 2-33 
 
 2.31 
 
 2.26 
 
 1.74 
 
 2 . 12 
 
 i-34 
 
 16 
 
 2.78 
 
 2-33 
 
 2-73 
 
 1.77 
 
 2.51 
 
 i-33 
 
 32 
 
 3-32 
 
 2. 4 I 
 
 3-22 
 
 I. 80 
 
 2.98 
 
 1.36 
 
 128 
 
 4-54 
 
 2-55 
 
 4-50 
 
 1.92 
 
 4.29 
 
 1.48 
 
 512 
 
 5-8i 
 
 2.76 
 
 6.05 
 
 2.13 
 
 6-75 
 
 1.88 
 
 1024 
 
 6.50 
 
 2.8 3 
 
 7.10 
 
 2.28 
 
 7-94 
 
 1.99 
 
 2048 
 
 7.40 
 
 3.00 
 
 8.14 
 
 2.40 
 
 9-78 
 
 2.22 
 
 4096 
 
 8.50 
 
 3 -ii 
 
 9.67 
 
 2-55 
 
 11 -59 
 
 2.32 
 
 Calcium Formate, Ca(OOCH) 2 
 
 The mother solution was standardized by determining 
 calcium as the sulphate. 
 
 Table XXIV. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 58.4 
 
 81.7 
 
 IO7 . I 
 
 128.6 ' 
 
 8 
 
 67.2 
 
 94 4 
 
 124.5 
 
 149-7 
 
 32 
 
 81 .4 
 
 II5-3 
 
 I53-I 
 
 184.7 
 
 128 
 
 92.2 
 
 131.2 
 
 174-3 
 
 211 .6 
 
 512 
 
 95-7 
 
 135-5 
 
 l8l.9 
 
 223-5 
 
 2048 
 
 101 .4 
 
 144.6 
 
 190.4 
 
 230.6 
 
 4096 
 
 101.3 
 
 145-4 
 
 190.6 
 
 229.2 
 
 Table XXV . Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35< 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 
 I 
 
 .86 
 
 3 
 
 19 
 
 2.03 
 
 2-49 
 
 2 
 
 15 
 
 2 
 
 .01 
 
 8 
 
 
 2 
 
 .18 
 
 O 
 
 24 
 
 2.41 
 
 2-55 
 
 2 
 
 52 
 
 2 
 
 .02 
 
 32 
 
 
 2 
 
 .70 
 
 o 
 
 32 
 
 3.02 
 
 2.62 
 
 3 
 
 .16 
 
 2 
 
 .06 
 
 128 
 
 
 3 
 
 . 12 
 
 ^ 
 
 .38 
 
 3-45 
 
 2.63 
 
 3 
 
 73 
 
 2 
 
 H 
 
 512 
 
 
 3 
 
 .18 
 
 o 
 
 32 
 
 3-7i 
 
 2-74 
 
 4 
 
 .16 
 
 2 
 
 .29 
 
 2048 
 
 
 3 
 
 .46 
 
 3 
 
 .41 
 
 3-66 
 
 2-53 
 
 4 
 
 .02 
 
 2 
 
 . II 
 
 4096 
 
 
 3 
 
 53 
 
 3 
 
 48 
 
 3-62 
 
 2-49 
 
 3 
 
 .86 
 
 2 
 
 03 
 
 Table XXVL 
 
 Percentage Dissociation 
 
 
 V 
 
 
 
 
 o 
 
 
 12. 5 
 
 25 
 
 35 
 
 
 4 
 
 
 57- 
 
 65 
 
 
 56-19 
 
 56.19 
 
 
 56 
 
 . II 
 
 
 
 8 
 
 
 66. 
 
 34 
 
 
 64.92 
 
 65-32 
 
 
 65 
 
 31 
 
 
 
 32 
 
 
 80. 
 
 36 
 
 
 79-30 
 
 80-33 
 
 80.58 
 
 
 128 
 
 
 9i- 
 
 02 
 
 
 90.23 
 
 91-45 
 
 
 92 
 
 32 
 
 
 
 512 
 
 
 94- 
 
 47 
 
 
 93-19 
 
 95-44 
 
 
 97 
 
 51 
 
 
 2048 loo.oo 99-45 99-89 100.00 
 4096 .... 100.00 loo.oo 
 
17 
 
 Calcium Chromate, CaCrO 4 
 
 The mother solution was standardized by titrating with 
 ferrous ammonium alum. 
 
 Table XXV 1 1. Molecular Conductivity 
 
 V 12. 5 25 35 
 
 8 57.7 80.9 105.8 125.4 
 
 1 6 64.6 90.4 118.5 I 4-9 
 
 32 72.2 101.4 I 33- 1 158.2 
 
 128 91.2 126.9 *67-5 200.8 
 
 512 106.7 150-0 198-7 239.5 
 
 1024 i i i. 6 157-3 208.8 253.3 
 
 2048 114 .4 160.8 214.0 264.0 
 
 4096 116.1 162.5 216. i 261.6 
 
 v 
 8 
 
 16 
 
 32 
 
 128 
 
 512 
 
 1024 
 
 2048 
 
 4096 
 
 Table XXIX Percentage Dissociation 
 
 V 12. 5 25 35 
 
 8 49.70 49.78 48.96 47.94 
 
 16 55-64 55-63 54-85 53-86 
 
 32 62.19 62.40 61.59 60.47 
 
 128 78.55 78.09 77.51 76.76 
 
 512 91.90 92.31 91.95 91.55 
 
 1024 96 . I 2 96 . 80 96 . 62 96 . 83 
 
 2048 98.54 98.95 99 -3 100.00 
 4096 100.00 100.00 100.00 .... 
 
 Zinc Nitrate, Zn(NO 3 ) 2 .6H 2 O 
 
 The mother solution was standardized by determining zinc 
 as zinc oxide. 
 
 Table XXVIII. Temperature Coefficients 
 
 0-12.5 
 
 12. 5-25 
 
 25-35 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 1-85 
 
 3-21 
 
 1.99 
 
 2.46 
 
 I .96 
 
 1.85 
 
 2 .06 
 
 3-19 
 
 2.25 
 
 2-49 
 
 2.2 4 
 
 1.89 
 
 2-33 
 
 3-23 
 
 2-54 
 
 2-51 
 
 2.51 
 
 1.89 
 
 2.86 
 
 3-14 
 
 3-25 
 
 2.56 
 
 3-33 
 
 i 99 
 
 3-46 
 
 3-24 
 
 3-90 
 
 2.60 
 
 4.08 
 
 2.05 
 
 3-66 
 
 3.28 
 
 4.12 
 
 2.62 
 
 4-45 
 
 2.13 
 
 3-71 
 
 3-24 
 
 4.26 
 
 2.6 5 
 
 5-oo 
 
 2-34 
 
 3-7i 
 
 3-20 
 
 4.29 
 
 2.64 
 
 4-55 
 
 2. II 
 
i8 
 Table XXX. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 80.6 
 
 1 10 . 8 
 
 146.6 
 
 I7I.2 
 
 i 
 
 87.6 
 
 121 .2 
 
 157 2 
 
 188.5 
 
 32 
 
 IOO.O 
 
 139.2 
 
 I82.I 
 
 2I9.O 
 
 128 
 
 110.4 
 
 I54-I 
 
 202 .6 
 
 243-5 
 
 512 
 
 114. 1 
 
 164.9 
 
 210. I 
 
 254-3 
 
 1024 
 
 117.1 
 
 165.0 
 
 216.6 
 
 261.3 
 
 2048 
 
 120.4 
 
 169.2 
 
 222 .4 
 
 270.2 
 
 4096 
 
 124.4 
 
 175 -0 
 
 229. I 
 
 279.4 
 
 Table XX XL Temperature Coefficients * 
 
 0-12.5 12. 5-25 25-35' 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 2.42 
 
 .3-00 
 
 2.86 
 
 2.58 
 
 2 .46 
 
 1.68 
 
 8 
 
 2.69 
 
 3-07 
 
 2.88 
 
 2.38 
 
 3-13 
 
 i 99 
 
 32 
 
 3-34 
 
 3-34 
 
 3-43 
 
 2 .46 
 
 3-69 
 
 2.03 
 
 128 
 
 3-50 
 
 3-17 
 
 3.88 
 
 2.52 
 
 4.09 
 
 2 .02 
 
 512 
 
 4.06 
 
 3-56 
 
 3.62 
 
 2 .20 
 
 4.42 
 
 2. 10 
 
 1024 
 
 3-83 
 
 3-27 
 
 4-13 
 
 2.50 
 
 4-47 
 
 2.06 
 
 2048 
 
 3-90 
 
 3-24 
 
 4.26 
 
 2.52 
 
 4.78 
 
 2.15 
 
 4096 
 
 4-05 
 
 3-26 
 
 4-33 
 
 2-47 
 
 5-03 
 
 2. 2O 
 
 Table XXXIL Percentage Dissociation 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 64.79 
 
 63-3I 
 
 63-99 
 
 61 .27 
 
 8 
 
 70.42 
 
 69.26 
 
 68.62 
 
 67.47 
 
 32 
 
 80.39 
 
 79-54 
 
 79.48 
 
 78.38 
 
 128 
 
 88.75 
 
 88.06 
 
 88.43 
 
 87.15 
 
 512 
 
 91.92 
 
 94-23 
 
 91.71 
 
 91 .02 
 
 1024 
 
 94 13 
 
 94.29 
 
 94-54 
 
 93-52 
 
 2048 
 
 96.78 
 
 96.68 
 
 97.07 
 
 96.71 
 
 4096 IOO.OO IOO.OO IOO.OO IOO.OO 
 
 Zinc Acetate, Zn(C2H 3 O 2 ) 2 
 
 The mother solution was standardized by determining zinc 
 as zinc oxide. 
 
 Table XXXI 1 1. Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 27.8 
 
 38.0 
 
 48.0 
 
 55-0 
 
 8 
 
 37-7 
 
 52.2 
 
 66.6 
 
 77-2 
 
 32 
 
 55-5 
 
 78.6 
 
 103.0 
 
 122.4 
 
 128 
 
 70.0 
 
 IOO-7 
 
 134-2 
 
 162.1 
 
 512 
 
 78.6 
 
 II3-7 
 
 153-2 
 
 185-5 
 
 1024 
 
 79 9 
 
 116. i 
 
 156-7 
 
 191 .6 
 
 2048 
 
 83-2 
 
 120.8 
 
 163.2 
 
 200. i 
 
 4096 
 
 83.8 
 
 121.3 
 
 163.4 
 
 2OI . I 
 
19 
 
 Table XXXIV. 
 
 0-12.5 
 
 , Temperature Coefficients 
 
 12. 5-25 25 
 
 -35 
 
 Cond. 
 
 Per 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 
 
 .81 
 
 2 
 
 91 
 
 
 0.80 
 
 2. II 
 
 o 
 
 .70 
 
 I 
 
 -46 
 
 8 
 
 I 
 
 .16 
 
 3 
 
 .08 
 
 
 1. 15 
 
 2.20 
 
 I 
 
 .06 
 
 I 
 
 -59 
 
 32 
 
 I 
 
 -85 
 
 3 
 
 33 
 
 
 i 95 
 
 2.48 
 
 I 
 
 94 
 
 I 
 
 .88 
 
 128 
 
 2 
 
 45 
 
 3 
 
 50 
 
 
 2.68 
 
 2.66 
 
 2 
 
 79 
 
 2 
 
 .08 
 
 512 
 
 2 
 
 .81 
 
 3 
 
 58 
 
 
 3.16 
 
 2.78 
 
 3 
 
 23 
 
 2 
 
 . ii 
 
 1024 
 
 2 
 
 90 
 
 3 
 
 63 
 
 
 3-25 
 
 2.79 
 
 3 
 
 49 
 
 2 
 
 23 
 
 2048 
 
 o 
 
 OI 
 
 3 
 
 .61 
 
 
 3-39 
 
 2.81 
 
 3 
 
 .69 
 
 2 
 
 .26 
 
 4096 
 
 3 
 
 00 
 
 3 
 
 58 
 
 
 3-37 
 
 2.78 
 
 3 
 
 -77 
 
 2 
 
 3i 
 
 Table XXXV. 
 
 Percentage Dissociation 
 
 V 
 
 
 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 
 33- 
 
 17 
 
 
 3i 
 
 33 
 
 29.38 
 
 
 27 
 
 35 
 
 
 8 
 
 
 44- 
 
 99 
 
 
 43 
 
 03 
 
 40.76 
 
 
 38 
 
 39 
 
 
 32 
 
 
 66. 
 
 23 
 
 
 64 
 
 .80 
 
 63-03 
 
 
 60 
 
 -87 
 
 
 128 
 
 
 83- 
 
 53 
 
 
 83 
 
 .02 
 
 82.13 
 
 
 80 
 
 .61 
 
 
 512 
 
 
 93- 
 
 79 
 
 
 93 
 
 73 
 
 93-76 
 
 
 92 
 
 .24 
 
 
 1024 
 
 
 95- 
 
 34 
 
 
 95 
 
 7i 
 
 95-9P 
 
 
 95 
 
 .28 
 
 
 2048 
 
 
 99- 
 
 28 
 
 
 99 
 
 59 
 
 99.86 
 
 
 99 
 
 50 
 
 
 4096 
 
 
 100. 
 
 00 
 
 
 100 
 
 .00 
 
 100.00 
 
 
 IOO 
 
 .00 
 
 
 Lead Acetate, 
 
 The mother solution was standardized by determining 
 lead as lead sulphate. 
 
 Table XXXVI. -Molecular Conductivity 
 
 V 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 II .2 
 
 16.4 
 
 22 . I 
 
 27.0 
 
 8 
 
 16.0 
 
 23-3 
 
 31.2 
 
 37-8 
 
 32 
 
 28.8 
 
 41.4 
 
 54-9 
 
 66.2 
 
 128 
 
 46.4 
 
 66.3 
 
 87.1 
 
 104.2 
 
 512 
 
 65.3 
 
 92.7 
 
 I23.I 
 
 146.2 
 
 1024 
 
 74-5 
 
 108.2 
 
 I39-I 
 
 167.2 
 
 2048 
 
 84-3 
 
 II9.4 
 
 156.8 
 
 189.1 
 
 4096 
 
 87.8 
 
 124.6 
 
 165.5 
 
 198.7 
 
20 
 
 Table XX XV II. Temperature Coefficients 
 
 0-12.5 12. 5-25 25-35 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 
 
 .41 
 
 3 
 
 .66 
 
 0.46 
 
 2.8l 
 
 
 0. 
 
 49 
 
 2 
 
 .22 
 
 8 
 
 
 
 58 
 
 3 
 
 -63 
 
 0.63 
 
 2.70 
 
 
 o. 
 
 66 
 
 2 
 
 . 12 
 
 3 2 
 
 I 
 
 .01 
 
 3 
 
 50 
 
 I. 08 
 
 2.61 
 
 
 I , 
 
 13 
 
 2 
 
 .06 
 
 128 
 
 I 
 
 59 
 
 3 
 
 42 
 
 1.66 
 
 2.50 
 
 
 I , 
 
 71 
 
 T 
 
 .96 
 
 512 
 
 2 
 
 19 
 
 3 
 
 35 
 
 2-43 
 
 2.62 
 
 
 2 , 
 
 31 
 
 i 
 
 .88 
 
 1024 
 
 2 
 
 .70 
 
 3 
 
 .62 
 
 2.47 
 
 2.28 
 
 
 2, 
 
 81 
 
 2 
 
 .02 
 
 2048 
 
 2 
 
 .81 
 
 3 
 
 34 
 
 2.99 
 
 2.50 
 
 
 o 
 
 23 
 
 2 
 
 .06 
 
 4096 
 
 2 
 
 94 
 
 3 
 
 35 
 
 3-27 
 
 2.62 
 
 
 3 
 
 32 
 
 2 
 
 15 
 
 Table XXXVIII. 
 
 Percentage Dissociation 
 
 V 
 
 
 
 
 
 
 
 12. 5 
 
 25 
 
 35 
 
 4 
 
 
 12 
 
 .76 
 
 
 13.16 
 
 13- 
 
 35 
 
 
 13- 
 
 59 
 
 
 8 
 
 
 18 
 
 .22 
 
 
 18.70 
 
 18. 
 
 85 
 
 
 19- 
 
 02 
 
 
 32 
 
 
 32 
 
 .80 
 
 
 33-23 
 
 33- 
 
 17 
 
 
 33- 
 
 32 
 
 
 128 
 
 
 52 
 
 -85 
 
 
 53-21 
 
 52. 
 
 63 
 
 
 52. 
 
 44 
 
 
 512 
 
 
 74 
 
 -38 
 
 
 74.40 
 
 74- 
 
 38 
 
 
 73- 
 
 58 
 
 
 1024 
 
 
 84 
 
 .86 
 
 
 86.84 
 
 84- 
 
 05 
 
 
 84. 
 
 15 
 
 
 2048 
 
 
 96 
 
 .02 
 
 
 95-83 
 
 94- 
 
 74 
 
 
 95- 
 
 *7 
 
 
 4096 
 
 
 100 
 
 .00 
 
 100.00 
 
 100. 
 
 oo 
 
 
 100. 
 
 00 
 
 
 Ammonium Aluminium Sulphate, NH 4 Al(SO 4 ) 2 .i2H 2 O 
 The mother solution was standardized by determining sul- 
 phuric acid as barium sulphate. 
 
 v 
 
 8 
 
 16 
 
 64 
 
 128 
 
 512 
 
 2048 
 
 Table XXXIX. 
 
 35 
 
 168.8 
 202.3 
 261.5 
 284.8 
 
 485-8 
 
 -Molecular Conductivity 
 
 50 65 
 
 203 .5 236 . 5 
 
 247.5 288.0 
 
 325-8 384-8 
 
 347-5 426.3 
 
 477-5 573-5 
 
 643-1 831.5 
 
 Table XL. Temperature Coefficients 
 
 35-50 50-65 
 
 
 Cond 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units. 
 
 cent. 
 
 units 
 
 cent. 
 
 8 
 
 2.31 
 
 1-37 
 
 2 .20 
 
 .08 
 
 16 
 
 3.01 
 
 1.48 
 
 2 . 70 
 
 .09 
 
 64 
 
 4 29 
 
 I .64 
 
 3-93 'i 
 
 .21 
 
 128 
 
 4.18 
 
 i-47 
 
 5 25 
 
 51 
 
 512 
 
 7-44 
 
 2.03 
 
 6.40 
 
 34 
 
 2048 
 
 10.49 
 
 2.16 
 
 12.56 
 
 95 
 
21 
 
 Disodium Phosphate, HNa2PO 4 .i2H 2 O 
 
 The mother solution was standardized by determining the 
 phosphoric acid as magnesium pyrophosphate. 
 
 Table XLI. Molecular Conductivity and Dissociation 
 
 35 50 65 
 
 V 
 
 8 
 32 
 
 128 
 512 
 
 2048 
 
 V 
 
 8 
 32 
 
 128 
 
 512 
 
 2048 
 
 Hv 
 
 141.8 
 176.8 
 206.5 
 224.3 
 229.5 
 
 Table 
 
 a flv a Pv 
 6l.8 184.1 6l-5 228.0 
 77.0 228.2 76.3 287.9 
 
 90.9 269.0 89.8 334-4 
 97.8 292.7 97.8 376.1 
 loo.o 299.3 loo.o (355.4) 
 
 XLII. Temperature Coefficients 
 
 35-50 50-65 
 
 ; i 
 60 
 76 
 88 
 
 IOO 
 
 i 
 
 .6 
 .6 
 9 
 
 .0 
 
 Cond. 
 units 
 
 2.82 
 
 3-43 
 4.17 
 
 4-56 
 4-65 
 
 Per 
 cent. 
 
 1.99 
 
 i 94 
 
 2 .02 
 2.03 
 2.03 
 
 
 Cond. 
 units 
 
 2-93 
 3-98 
 4-36 
 5-56 
 4-65 
 
 Per 
 
 cent. 
 
 i-59 
 1.74 
 1.62 
 i .90 
 
 Sodium Tetraborate, 
 The mother solution was standardized as the anhydrous 
 salt. 
 
 Table XL/77. Molecular Conductivity and Dissociation 
 
 35 50 65 
 
 V 
 
 16 
 
 
 141 3 
 
 
 a 
 70.9 
 
 P-v a 
 182.8 67.6 
 
 231-3 
 
 
 a 
 6 4 
 
 4 
 
 32 
 
 
 I57-I 
 
 
 78.8 
 
 204.0 75 
 
 5 
 
 256.2 
 
 
 71 
 
 3 
 
 128 
 
 
 172.4 
 
 
 86. 5 
 
 224.1 82 
 
 9 
 
 281.6 
 
 
 7 8 
 
 4 
 
 512 
 
 
 186.7 
 
 
 93-6 
 
 247.8 91 
 
 -7 
 
 316.7 
 
 
 88 
 
 ,1 
 
 2048 
 
 
 199.4 
 
 
 IOO.O 
 
 270.3 loo 
 
 .0 
 
 359-3 
 
 
 IOO 
 
 .0 
 
 Table XLIV .Temperature 
 
 Coefficients 
 
 
 
 
 
 35-50 
 
 
 
 50-65 
 
 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 
 16 
 
 
 2 
 
 77 
 
 I. 9 6 
 
 3-23 
 
 
 I 
 
 .76 
 
 
 
 32 
 
 
 3 
 
 13 
 
 1.99 
 
 3-48 
 
 
 I 
 
 -7i 
 
 
 
 128 
 
 
 *J 
 
 45 
 
 2.OO 
 
 3-83 
 
 
 I 
 
 7i 
 
 
 
 512 
 
 
 4 
 
 01 
 
 2-15 
 
 4-59 
 
 
 I 
 
 -85 
 
 
 2048 
 
 4 
 
 73 
 
 2-37 
 
 5-93 
 
 
 2 
 
 19 
 
 
22 
 
 Potassium Aluminium Sulphate, KAl(SO 4 ) 2 .i2H 2 O 
 The mother solution was standardized by determining sul- 
 phuric acid as barium sulphate. 
 
 v 
 
 4 
 
 8 
 
 32 
 
 128 
 
 512 
 
 2048 
 
 Table XLV. Molecular Conductivity 
 
 35 50 65 
 
 142.3 172.5 196.1 
 
 165.3 207.5 240.6 
 
 215 7 255.1 317.4 
 
 283.7 
 358.3 
 
 470.0 
 
 356.9 
 446.9 
 626.4 
 
 426.2 
 
 557-1 
 796.4 
 
 Table XLV I. Temperature Coefficients 
 
 3S-50 
 
 50-65 
 
 
 Cond. Per 
 
 Cond. Per 
 
 V 
 
 units cent. 
 
 units cent. 
 
 4 
 
 2.01 .41 
 
 i-57 0.87 
 
 8 
 
 2 . 8 i .70 
 
 2.21 .06 
 
 32 
 
 2.63 .22 
 
 4-15 -63 
 
 128 
 
 4.88 .72 
 
 4.62 .29 
 
 512 
 
 5 9i 65 
 
 7-35 -64 
 
 2048 
 
 10.42 2.22 
 
 11.33 -81 
 
 Potassium Sulphocyanate, KCNS 
 
 The mother solution was prepared by direct weighing. 
 Table XLV II. Molecular Conductivity and Dissociation 
 
 35 ( 
 
 50 C 
 
 65' 
 
 V 
 
 n v 
 
 a 
 
 Pv 
 
 a 
 
 V-V 
 
 a 
 
 4 
 
 127.6 
 
 79 2 
 
 160.2 
 
 77-6 
 
 191 . 1 
 
 76.2 
 
 8 
 
 132.9 
 
 82.4 
 
 166.7 
 
 80.8 
 
 201 .8 
 
 80.4 
 
 32 
 
 142-3 
 
 88.3 
 
 179.6 
 
 87.0 
 
 219.6 
 
 87-5 
 
 128 
 
 H9-3 
 
 92.6 
 
 190.0 
 
 92.1 
 
 232.4 
 
 92 .6 
 
 512 
 
 153-7 
 
 95-4 
 
 192.6 
 
 93 3 
 
 239-3 
 
 95-4 
 
 2048 
 
 161 .2 
 
 100. 
 
 206.4 
 
 100. 
 
 250.9 
 
 IOO.O 
 
 Table XLV III. Temperature Coefficients 
 
 35-50 
 
 50-65 
 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 4 
 
 2.17 
 
 .70 
 
 8 
 
 2.25 
 
 .69 
 
 32 
 
 2-49 
 
 75 
 
 128 
 
 2.74 
 
 .84 
 
 512 
 
 2.60 
 
 .69 
 
 2048 
 
 3.01 
 
 .86 
 
 Cond. 
 
 Per 
 
 units 
 
 cent. 
 
 2.06 
 
 I .29 
 
 2-34 
 
 I .40 
 
 2.67 
 
 1-49 
 
 2.83 
 
 i 49 
 
 3 ii 
 
 1.62 
 
 2.97 
 
 1.44 
 
23 
 
 Monopotassium Phosphate, H 2 KPO 4 
 
 The mother solution was standardized by determining phos- 
 phoric acid as magnesium pyrophosphate. 
 
 Table XLIX. Molecular Conductivity and Dissociation 
 
 35 50 65 
 
 V 
 
 V-v 
 
 a 
 
 fiv 
 
 a 
 
 P-v 
 
 a. 
 
 8 
 
 310.4 
 
 63-8 
 
 391.6 
 
 64-5 
 
 477-2 
 
 61.2 
 
 32 
 
 380.0 
 
 7 8.1 
 
 481.2 
 
 79-2 
 
 588.4 
 
 75-5 
 
 128 
 
 424-3 
 
 8 7 .2 
 
 537-6 
 
 88.5 
 
 661.2 
 
 84.8 
 
 512 
 
 452.3 
 
 93 -o 
 
 573-1 
 
 94-4 
 
 708.2 
 
 90.9 
 
 2048 
 
 471-5 
 
 96.9 
 
 599-9 
 
 98.8 
 
 740.9 
 
 95-1 
 
 8192 
 
 486.4 
 
 100. 
 
 621 .4 
 
 IOO.O 
 
 779-4 
 
 IOO.O 
 
 Table L. Temperature Coefficients 
 
 35-50 50-65 
 
 Cond. Per Cond. Per 
 
 units cent. units cent. 
 
 8 
 
 5-41 
 
 i 74 
 
 5-7i 
 
 i .46 
 
 32 
 
 6-75 
 
 1.78 
 
 7-15 
 
 i 49 
 
 128 
 
 7-55 
 
 1.78 
 
 8.24 
 
 i-53 
 
 512 
 
 8.05 
 
 1.78 
 
 9.01 
 
 i-57 
 
 2048 
 
 8.56 
 
 1.81 
 
 9.40 
 
 1-58 
 
 8192 
 
 9.00 
 
 1.82 
 
 io-53 
 
 i .69 
 
 Potassium Acetate, KC 2 H 3 O 2 
 
 The mother solution was standardized by determining 
 potassium as the sulphate. 
 
 Table LL Molecular Conductivity and Dissociation 
 
 35 50 65 
 
 V 
 
 Hv 
 
 
 a 
 
 
 lh) 
 
 a 
 
 
 V-v 
 
 
 a. 
 
 
 4 
 
 94- 
 
 4 
 
 75- 
 
 40 
 
 125.6 
 
 7 8. 
 
 84 
 
 142 
 
 . I 
 
 72. 
 
 13 
 
 8 
 
 102 . 
 
 7 
 
 82. 
 
 03 
 
 131.6 
 
 82. 
 
 61 
 
 1 60 
 
 4 . 
 
 81. 
 
 42 
 
 32 
 
 112 . 
 
 o 
 
 89. 
 
 46 
 
 147.0 
 
 92 
 
 28 
 
 1 80 
 
 .8 
 
 91. 
 
 78 
 
 128 
 
 118. 
 
 7 
 
 94- 
 
 81 
 
 154.6 
 
 97 
 
 05 
 
 184 
 
 5 
 
 93 
 
 66 
 
 512 
 
 125. 
 
 2 
 
 100. 
 
 00 
 
 159 3 
 
 IOO. 
 
 00 
 
 194 
 
 9 
 
 98. 
 
 94 
 
 2048 
 
 .123. 
 
 3 
 
 
 
 
 157-7 
 
 
 
 197 
 
 .0 
 
 IOO. 
 
 00 
 
Table LI I. Temperature Coefficients 
 
 35-50 
 
 50-65 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 2.08 
 
 2.20 
 
 I . 10 ( 
 
 ).88 
 
 8 
 
 i-93 
 
 1.88 
 
 I .92 
 
 .46 
 
 32 
 
 2-33 
 
 2.08 
 
 2.25 
 
 53 
 
 128 
 
 2.40 
 
 2.02 
 
 2.00 
 
 .29 
 
 512 
 
 2.27 
 
 1.81 
 
 2-37 
 
 49 
 
 2048 
 
 2.29 
 
 1.86 
 
 2.62 
 
 .66 
 
 Calcium Chloride, 
 
 The mother solution was standardized by determining cal- 
 cium as carbonate and chlorine by Mohr's method. 
 
 Table LIII. Molecular Conductivity and Dissociation 
 
 35 50 65 
 
 V 
 
 Vv 
 
 a 
 
 ftv 
 
 
 a 
 
 Hv 
 
 
 
 a 
 
 4 
 
 189 
 
 . I 
 
 63 
 
 41 
 
 237 
 
 -7 
 
 62 . 22 
 
 29O. 
 
 4 
 
 61 
 
 16 
 
 8 
 
 208 
 
 . I 
 
 69, 
 
 78 
 
 258 
 
 5 
 
 67-67 
 
 3 l8. 
 
 7 
 
 67 
 
 12 
 
 32 
 
 242 
 
 .0 
 
 81 
 
 15 
 
 306 
 
 5 
 
 80.24 
 
 378- 
 
 5 
 
 79 
 
 .72 
 
 128 
 
 267 
 
 . I 
 
 89 
 
 57 
 
 34 
 
 .8 
 
 89.21 
 
 418. 
 
 9 
 
 88 
 
 .22 
 
 512 
 
 283 
 
 5 
 
 95 
 
 .07 
 
 362 
 
 4 
 
 94.87 
 
 452. 
 
 5 
 
 95 
 
 30 
 
 2048 298.2 100.0 382.0 100.00 474.8 100.00 
 Table LIV. Temperature Coefficients 
 
 35-50 50-65 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units c 
 
 ent. 
 
 units 
 
 cent. 
 
 4 
 
 3-24 ';) 
 
 [-71 
 
 3-51 
 
 1.48 
 
 8 
 
 3-36 
 
 .62 
 
 4-OI 
 
 i-55 
 
 32 
 
 4-3 :1 
 
 .78 
 
 4.80 
 
 i-57 
 
 128 
 
 4.91 
 
 .84 
 
 5-21 
 
 i-53 
 
 512 
 
 5-26 
 
 .86 
 
 6.01 
 
 1.66 
 
 2048 
 
 5-59 :i 'i 
 
 .88 
 
 6. 19 
 
 1.62 
 
 Magnesium Chloride, MgCl 2 .6H 2 O 
 
 The mother solution was standardized by determining 
 magnesium as magnesium pyrophosphate and chlorine by 
 Mohr's method. 
 
Table LV. Molecular Conductivity and Dissociation 
 
 35' 
 
 50 c 
 
 65' 
 
 4 
 
 179-8 
 
 62 . 17 
 
 228.0 
 
 61 .09 
 
 280.6 
 
 60.27 
 
 8 
 
 196-5 
 
 67-95 
 
 249.7 
 
 66.91 
 
 303.8 
 
 65-25 
 
 32 
 
 231.6 
 
 8o.o8 
 
 294.7 
 
 78.97 
 
 364.8 
 
 78.35 
 
 128 
 
 249-8 
 
 86.37 
 
 3II.8 
 
 83-55 
 
 401 .6 
 
 86.25 
 
 512 
 
 269-9 
 
 91 .20 
 
 348.3 
 
 93-33 
 
 433-1 
 
 93.02 
 
 2048 
 
 289.2 
 
 IOO.OO 
 
 373-2 
 
 100.00 
 
 465-6 
 
 100.00 
 
 Table LVL Temperature Coefficients 
 
 35-50 50-65 
 
 Cond. 
 
 Per 
 
 units 
 
 cent. 
 
 3-21 
 
 79 
 
 3-55 
 
 .81 
 
 4.21 l 
 
 .82 
 
 4-13 
 
 65 
 
 5-23 
 
 94 
 
 5.60 
 
 94 
 
 Cond. 
 
 Per 
 
 units 
 
 cent. 
 
 3-51 
 
 54 
 
 3 .6l 
 
 45 
 
 4.67 
 
 58 
 
 5-93 
 
 .90 
 
 5-65 
 
 .62 
 
 6.16 
 
 65 
 
 V 
 
 4 
 
 8 
 
 32 
 128 
 512 
 
 2048 
 
 Manganese Sulphate, MnSO 4 .4H 2 O 
 
 The mother solution was standardized by determining 
 manganese as manganous pyrophosphate and sulphuric acid 
 as barium sulphate. 
 
 Table LVIL Molecular Conductivity 
 
 V 
 
 35 
 
 50 
 
 65 
 
 
 
 4 
 
 
 78. 
 
 
 
 
 
 88. 
 
 
 
 
 108 
 
 3 
 
 8 
 
 
 92 
 
 6 
 
 
 
 112. 
 
 8 
 
 
 130 
 
 .0 
 
 32 
 
 
 128. 
 
 5 
 
 
 
 156. 
 
 4 
 
 
 181 
 
 .8 
 
 128 
 
 
 166 
 
 7 
 
 
 
 204. 
 
 I 
 
 
 241 
 
 9 
 
 512 
 
 
 219. 
 
 4 
 
 
 
 277. 
 
 5 
 
 
 338 
 
 7 
 
 2048 
 
 
 246. 
 
 
 
 
 
 326. 
 
 7 
 
 
 404 
 
 .6 
 
 Table LVIII 
 
 . Temperature 
 
 Coefficients 
 
 35-50 
 
 50-65 
 
 * 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units 
 
 cent. 
 
 4 
 
 
 
 6 7 
 
 
 O 
 
 .86 
 
 
 I 
 
 35 
 
 
 
 53 
 
 8 
 
 I 
 
 35 
 
 
 I 
 
 46 
 
 
 I 
 
 15 
 
 
 
 04 
 
 32 
 
 I 
 
 86 
 
 
 I 
 
 45 
 
 
 I 
 
 6 9 
 
 
 
 08 
 
 128 
 
 2 
 
 49 
 
 
 I 
 
 49 
 
 
 2 
 
 52 
 
 
 
 24 
 
 512 
 
 o 
 
 87 
 
 
 I 
 
 76 
 
 
 4 
 
 08 
 
 
 
 47 
 
 2048 
 
 c 
 
 38 
 
 
 2 
 
 19 
 
 
 5 
 
 19 
 
 
 
 
 59 
 
26 
 
 Ferric Chloride, FeCl 3 .6H 2 O 
 
 The mother solution was standardized by determining iron 
 as ferric oxide. 
 
 Table LIX. Molecular Conductivity and Dissociation 
 
 35 50 65 
 
 V 
 
 I'v 
 
 
 
 a 
 
 4 
 
 214 
 
 -J 
 
 16 
 
 92 
 
 8 
 
 276 
 
 5 
 
 21 
 
 83 
 
 32 
 
 424 
 
 1 
 
 33 
 
 52 
 
 128 
 
 827 
 
 i 
 
 65 
 
 .29 
 
 512 
 
 1050 
 
 7 
 
 82 
 
 94 
 
 2048 
 
 1266 
 
 8 
 
 100 
 
 .00 
 
 269.5 
 
 346-9 
 515.8 
 
 1037.6 
 1405.4 
 
 17.71 
 
 23-32 
 34.68 
 
 69.75 
 
 94.48 
 
 1487.5 100.00 
 
 327.0 19.39 
 
 I5I2.5 89.71 
 
 1685.9 ioo. oo 
 
 1673.6 
 
 Table LX. Temperature Coefficients 
 
 35-50 50-65 
 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 4 
 
 3-68 
 
 1.72 
 
 8 
 
 4.69 
 
 1.70 
 
 32 
 
 6.07 
 
 i-43 
 
 128 
 
 14.00 
 
 i .69 
 
 512 
 
 23-6 
 
 2.25 
 
 2048 
 
 14.7 
 
 i .60 
 
 Cond. 
 
 units 
 
 3.83 
 
 31-7 
 I8. 7 
 I2. 4 
 
 Per 
 cent. 
 
 1.42 
 
 3-85 
 
 i-33 
 0.83 
 
 Chromium Sulphate (Green Variety) 
 
 The mother solution was standardized by determining 
 chromium as chromic oxide. 
 
 Table LXL Molecular Conductivity 
 
 V 
 
 35 
 
 50 
 
 65 
 
 4 
 
 128.2 
 
 160.0 
 
 189.6 
 
 8 
 
 183.5 
 
 227.8 
 
 262 .9 
 
 32 
 
 302.0 
 
 354-4 
 
 417.4 
 
 128 
 
 433-9 
 
 522.7 
 
 606.0 
 
 512 
 
 673-3 
 
 811.1 
 
 977-3 
 
 2048 
 
 961 . i 
 
 1207.8 
 
 1534-7 
 
 Table LXII. Temperature Coefficients 
 
 
 35-50 
 
 50-65 
 
 
 Cond. 
 
 Per Cond. 
 
 Per 
 
 V 
 
 units cent. units - 
 
 cent. 
 
 4 
 
 2. 12 
 
 65 i 97 
 
 23 
 
 8 
 
 2-95 
 
 -61 2.34 
 
 03 
 
 32 
 
 3-49 
 
 .16 4.20 
 
 19 
 
 128 
 
 5 92 
 
 -34 5-55 
 
 .06 
 
 512 
 
 9.19 
 
 -37 ii. oS 
 
 37 
 
 2048 
 
 16.45 
 
 .71 21.79 
 
 .80 
 
Nickel Nitrate, Ni(NO 3 ) 2 .6H 2 O 
 The* mother solution was standardized by determining 
 
 AM 
 
 nickel as nickel oxide. 
 
 Table LXIII. Molecular Conductivity and Dissociation 
 
 35 c 
 
 50 C 
 
 65' 
 
 V 
 
 Ai 
 
 a 
 
 V-v 
 
 a 
 
 V-v 
 
 a 
 
 4 
 
 200.8 
 
 61 .0 
 
 252.4 
 
 60. I 
 
 306.6 
 
 59 4 
 
 8 
 
 216.8 
 
 65-8 
 
 276.3 
 
 65-6 
 
 343-5 
 
 66.6 
 
 32 
 
 260. 1 
 
 79-0 
 
 330.3 
 
 78.6 
 
 402.4 
 
 78.0 
 
 128 
 
 289.7 
 
 89.8 
 
 369.2 
 
 87.9 
 
 453-2 
 
 87.8 
 
 512 
 
 314-2 
 
 95-4 
 
 399-7 
 
 95-2 
 
 494.8 
 
 95-9 
 
 2048 329.3 ioo. o 420.0 ioo. o 516.0 loo. o 
 Table LXIV .Temperature Coefficients 
 
 35-50 
 
 50-65< 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 units c 
 
 ent. 
 
 4 
 
 3-44 i 
 
 [-71 
 
 3-6i 
 
 43 
 
 8 
 
 3-97 
 
 -83 
 
 4.48 
 
 .62 
 
 32 
 
 4.68 
 
 .80 
 
 4.81 
 
 .46 
 
 128 
 
 5-30 | 
 
 -83 
 
 5.60 
 
 52 
 
 512 
 
 5-70 
 
 .81 
 
 6-34 
 
 59 
 
 2048 
 
 6.05 
 
 .84 
 
 6.40 
 
 52 
 
 Nickel Sulphate, NiSO 4 .6H 2 O 
 
 The mother solution was standardized by determining 
 sulphuric acid as barium sulphate. 
 
 Table LXV. Molecular Conductivity 
 
 V 35 50 
 
 4 78.6 95.5 
 
 8 93-i ii5-5 
 
 32 127.0 158.2 
 
 128 171.8 215.6 
 
 512 219.4 278.9 
 
 2048 264.0 34 T -3 
 
 65 
 
 in. 8 
 
 135-7 
 187.8 
 259.8 
 339-7 
 425-7 
 
 * Table LXV I. Temperature Coefficients 
 
 35-50 
 
 50-65< 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units < 
 
 :ent. 
 
 units < 
 
 :ent. 
 
 4 
 
 I 13 
 
 44 
 
 1.0 9 
 
 .14 
 
 8 
 
 i 49 
 
 .60 
 
 i-35 
 
 -17 
 
 32 
 
 2.08 
 
 .64 
 
 i 97 
 
 25 
 
 128 
 
 2 .92 
 
 .70 
 
 2-95 
 
 37 
 
 512 
 
 3-97 
 
 .81 
 
 4-05 
 
 45 
 
 2048 
 
 5 15 
 
 95 
 
 5-63 
 
 65 
 
28 
 
 Cobalt Sulphate, CoSO 4 .7H 2 O 
 
 The mother solution was standardized by determining sul- 
 phuric acid as barium sulphate. 
 
 Table LXVII. Molecular Conductivity 
 
 v 
 
 4 
 
 8 
 
 32 
 
 128 
 
 512 
 
 2048 
 
 35 
 80.0 
 
 94-9 
 129. i 
 
 172.5 
 229.8 
 264.8 
 
 50 
 
 95-6 
 
 117.2 
 160.0 
 203.4 
 2.90.7 
 340-3 
 
 65 
 II2.7 
 
 137-5 
 189.6 
 256.6 
 346.0 
 
 421 .6 
 
 Table LXVIIL Temperature Coefficients 
 
 35-50 50-65 
 
 
 Cond. 
 
 Per 
 
 V 
 
 units 
 
 cent. 
 
 4 
 
 I .04 
 
 1.30 
 
 8 
 
 I 49 
 
 i-57 
 
 32 
 
 2.06 
 
 i-59 
 
 128 
 
 2.06 
 
 i., 1.9 
 
 512 
 
 4.06 
 
 1.76 
 
 2048 
 
 5-03 
 
 i .90 
 
 Cond. 
 units 
 
 Per 
 cent. 
 
 I . 14 
 
 19 
 
 1-35 
 
 15 
 
 i 97 
 
 23 
 
 3-55 
 
 74 
 
 3-49 
 
 .20 
 
 5-42 i 
 
 t-59 
 
 Copper Sulphate, CuSO 4 -5H 2 O 
 
 The mother solution was standardized by determining copper 
 as copper oxide and sulphuric acid as barium sulphate. 
 
 Table LXIX. Molecular Conductivity 
 
 V 35 50 65 
 
 4 75-6 93-8 107.4 
 
 8 90.5 109.1 124.5 
 
 126.1 152.7 173.8 
 
 170.7 210.3 247.3 
 
 222.7 279.1 337-7 
 
 266.3 343-3 422.7 
 
 Table LXX. Temperature Coefficients 
 
 32 
 
 128 
 
 512 
 
 2048 
 
 35-50 
 
 50-65 
 
 
 Cond. 
 
 Per 
 
 Cond. 
 
 Per 
 
 V 
 
 units c 
 
 ent. 
 
 units 
 
 cent. 
 
 4 
 
 I .21 3 
 
 .60 
 
 0.91 
 
 0.97 
 
 8 
 
 1.24 3 
 
 37 
 
 I .02 
 
 o-93 
 
 32 
 
 i-77 'J 
 
 .40 
 
 I.4I 
 
 0.92 
 
 128 
 
 2.64 
 
 55 
 
 2-45 
 
 1.16 
 
 512 
 
 3-76 
 
 .69 
 
 3 9i 
 
 i .40 
 
 2048 
 
 5-13 
 
 i-93 
 
 5-29 
 
 i-54 
 
DISCUSSION OF 
 
 Salts Studied from o to 35 
 
 The conductivity data (Tables XXIV to XXXVIII) for 
 the salts derived from diacid bases are of the same general 
 character. This is best seen by drawing curves. Fig. I shows 
 
 32 128 512 1024 
 
 Concentration 
 Fig. I. Zinc acetate 
 
 2048 
 
 conductivity-concentration curves for zinc acetate, which 
 may be taken as an example of these salts. The diagrams for 
 the other members of the group are similar, except that the 
 curve is much flattened in the cases of lead acetate and calcium 
 chromate. This is apparent in Fig. II, which gives the 
 conductivity-concentration curves for lead acetate. 
 
 Lead acetate presents a number of exceptions. In concen- 
 trated solutions it has the smallest molecular conductivity 
 and dissociation of any of the salts studied. At infinite 
 dilution, however, the conductivity is nearly the same at all 
 temperatures as for zinc acetate. Again, lead acetate shows 
 the smallest temperature coefficients of conductivity at high 
 temperatures, and the most rapid increase with dilution of 
 any of the salts brought within the scope of this investigation. 
 
 It has been known that dissociation seems to be nearly 
 independent of temperature over the range of temperature at 
 
30 
 
 which my work was done, but in general decreases as the tem- 
 perature rises. This is true of all but four of the salts included 
 in this investigation. 
 
 The four apparent exceptions are potassium acetate, cal- 
 cium formate, lead acetate and sodium ferrocyanide. Potas- 
 sium acetate shows no well-marked change in the dissocia- 
 tion with temperature. Dissociation apparently increases as 
 the temperature rises in the cases of calcium formate and 
 sodium ferrocyanide. The same is true of lead acetate in 
 concentrated solutions. It is intended to study farther the 
 dissociation of these apparently exceptional salts. 
 
 J2 128 5/2 T024 2O48 
 
 Concentration 
 Fig. II. I<ead acetate 
 
 The complex salt sodium ferrocyanide has high conduc- 
 tivity and large temperature coefficients of conductivity. The 
 percentage coefficients are remarkably constant at the various 
 dilutions. The value for //^ was hardly reached at the high- 
 est dilution used, which is probably due, in part at least, to 
 the breaking down into simpler ions in the more dilute solutions. 
 Hydrolysis also probably takes place. 
 
 The remaining salts studied over the lower range in tem- 
 perature are double salts and all are sulphates. Ammonium 
 copper sulphate and potassium nickel sulphate yield very 
 similar conductivity data. In the stronger solutions the 
 
nickel salt shows the greater conductivity, but at higher dilu- 
 tion the molecular conductivity and the temperature coeffi- 
 cients of these two salts are almost identical. Conductivity 
 in these cases is probably somewhat affected by hydrolysis. 
 
 A comparison of the data for the violet and green varie- 
 ties of ammonium chrome alum shows that in the more con- 
 centrated solutions the green variety has much higher con- 
 ductivity. At higher dilutions the reverse is true; the violet 
 conducts better than the green form. The same general 
 relation is shown in the case of potassium chrome alum, though 
 fi v for the green variety does not actually fall below the n v 
 value for the violet form at the highest dilution employed. 
 This relation between the two varieties appears in Fig. III. 
 
 600 
 
 500 
 
 400 
 
 300 
 
 32 128 5/2 1024 
 
 2048 
 
 Concentration 
 
 4036 
 
 _,. TTT f X X X Violet variety 
 
 Fig. III.-Ammomum chromium sulphate j_Q_Q_Q_ Green Tariety 
 
 The violet form of the chromium salts is transformed into 
 the green variety by heating the solid salt or its solution for 
 some time at about 70. The relation between the two forms 
 
32 
 
 has been the subject of many investigations. Monti 1 ob- 
 served that the change was accompanied by an increase in 
 the conductivity of the solution. Recoura, 2 in an elaborate 
 investigation, explained the change as hydrolytic, resulting 
 in the formation of free sulphuric acid and a basic salt. This 
 conclusion was confirmed by Whitney. 3 Jones and Mackay 4 
 showed by conductivity measurements that the transforma- 
 tion was continuous as the temperature rose slowly from 
 37. 5 to 90. 
 
 In the light of the conclusions of these workers, the explana- 
 tion of the relative conductivity of the two forms of ammonium 
 chrome alum would seem to be that the green modification, 
 by virtue of the hydrolysis caused by heating, has the higher 
 initial conductivity, but when diluted it is incapable of further 
 hydrolysis to the same extent as appears to occur in the case 
 of the normal violet variety. 
 
 Salts Studied from 35 to 65 
 
 Before considering in detail the salts studied from 35 to 
 65 some general relations should be discussed. It was found 
 by Jones and Ota 5 and by Jones and Knight 6 that concen- 
 trated solutions of certain salts in water often show abnormally 
 great depressions of the freezing point of the solvent. It was 
 also shown to be true in many cases that the molecular lower- 
 ing of the freezing point increased from a certain concentra- 
 tion both with dilution and with increased concentration. 
 The subject was further studied by Jones and Chambers 7 
 and by Jones and Getman. 8 It was found that the molecular 
 conductivities of solutions of the substances which showed a 
 minimum in the value of the molecular lowering were per- 
 fectly normal at all concentrations. 
 
 1 Z. anorg. Chem., 12, 75 (1896). 
 
 2 Ann. chim. phys., [7] 4, 494 (1895). 
 
 3 Z. physik. Chem., 20, 40 (1896). 
 * Am. Chem. J., 19, 103 (1897). 
 
 6 Ibid., 22, 5 (1899). 
 *Ibid., 22, 110 (1899). 
 
 7 Ibid., 23, 89 (1900). 
 
 Z. physik. Chem., 46, 244 (1903). 
 
33 
 
 To account for the facts, Jones 1 offered the suggestion that 
 the molecules of the dissolved substance form complex com- 
 pounds or hydrates with a portion of the water, thus virtually 
 increasing the concentration of the solution. The freezing 
 point is thus abnormally depressed. It was also pointed out 
 that substances which give these abnormal results are often 
 hygroscopic and that, when dehydrated, they readily com- 
 bine with water. Jones and his assistants have collected a 
 large amount of evidence, 2 by several independent methods, 
 which supports the theory of hydration. A method 3 was de- 
 veloped by which the approximate composition of the hy- 
 drates of many substances was calculated. 
 
 It was pointed out by Jones 4 that the breaking down of the 
 hydrated molecules, or of the hydrated ions, by a rise in 
 temperature would diminish the mass of the ion and thus in- 
 crease the conductivity. The more complex the hydrates 
 the greater would be the change in hydration and, conse- 
 quently, the greater the change in conductivity. Therefore 
 "we should expect to find those ions with the largest hydrating 
 power having the largest temperature coefficients of conduc- 
 tivity."* An examination of the experimental results of Jones 
 and West 6 led to the following conclusions : 
 
 1. The temperature coefficients of conductivity of aqueous 
 solutions of electrolytes are greater, the greater the hydra- 
 ting power of the electrolyte. 
 
 2. The temperature coefficients of conductivity of aqueous 
 solutions of electrolytes are of the same order of magnitude 
 for those substances having, approximately, the same hydra- 
 ting power. 
 
 3 . The temperature coefficients of conductivity, for any 
 given substance, increase with the dilution of the solution, 
 and the increase is greatest for those substances with large 
 hydrating power. 7 
 
 1 Am. Chem. J., 23, 103 (1900). 
 
 2 See Hydrates in Aqueous Solution; Carnegie Institution of Washington, Publica- 
 tion No. 60. 
 
 * Ibid., pp. 28-145. 
 
 4 Am. Chem. J., 35, 445 (1906). 
 
 5 Loc. cit., p. 447. 
 
 6 Am. Chem. J., 34, 357 (1905). 
 
 7 Ibid., 35, 450 (1906). 
 
34 
 
 Similar results were obtained by Jones and Clover. 1 
 The composition of the hydrates formed by some of the 
 substances which were brought within the scope of this inves- 
 tigation has been approximately determined by Jones 2 and 
 his assistants. In general, the hydrating power may be taken 
 as roughly proportional to the amount of water of crystallization. 
 The substances named in Table LXXI crystallize with little 
 or no water, and have slight hydrating power. They are 
 seen to have small temperature coefficients of conductivity. 
 The substances named in Table LXXII have large hydrating 
 power and also have large temperature coefficients of conduc- 
 tivity. 
 
 Table LXXI. Substances with Slight Hydrating Power 
 
 Temperature coefficients in conductivity units 
 
 V V Temp, range 
 
 KCNS 4 2.17 2048 3.01 35-50 
 
 KC 2 H 3 O 2 4 2.08 2048 2.29 35-50 
 
 Ca(OOCH) 2 4 2.15 2048 4.02 25-35 
 
 Zn(C 2 H 3 2 ), 4 0.70 2048 3.69 2 5 -35 
 
 Pb(C 2 H 3 2 ) 2 . 3 H 2 4 0.49 2048 3.23 2 5 -35 
 
 CaCrO 4 .2H 2 O 8 1.96 2048 5.00 25-35 
 
 Table LXXII. Substances with Large Hydrating Power 
 
 Temperature coefficients in conductivity units 
 
 V V Temp, range 
 
 Ni(N0 3 ) 2 .6H 2 4 3.44 2048 6.05 35-50 
 
 CaCl 2 .6H 2 4 3.24 2048 5 -59 35^5O 
 
 MgCl 2 .6H 2 4 3.21 2048 5.60 35-5 
 
 Zn(NO 3 ) 2 .6H 2 4 2.46 2048 4.78 25 - 3 5 
 
 FeCl 3 .6H 2 4 3.68 2048 14.7 35-5O 
 
 HNa 2 PO 4 .i2H 2 O 8 2.82 2048 4.65 35-5O 
 
 H 2 KP0 4 8 5.41 2048 8.56 35-50 
 
 Na 2 B 4 7 . 5 H 2 16 2.77 2048 4 73 35-5O 
 
 The values used in these tables are not strictly compara- 
 ble, since the concentrations and the ranges of temperatures 
 at which the temperature coefficients were determined are 
 not the same throughout, but the agreement is sufficiently 
 close to warrant their use in showing the general relations. 
 
 * Am. Chem. J., 43, 215 (1906). 
 
 2 Hydrates in Aqueous Solution; Carnegie Institution of Washington, No. SO. 
 
35 
 
 My results confirm the conclusion of Jones cited above, and 
 are in perfect accord with the theory of hydration advanced 
 by him. 
 
 The sulphates which I have studied in this investigation 
 are omitted from Tables LXXI and LXXII, because, as shown 
 by Jones and his coworkers, 1 the sulphates usually show ab- 
 normal results. In general, sulphates have very small tem- 
 perature coefficients of conductivity, and appear to have 
 small hydra ting power in solution. There is evidence that 
 some sulphates, at least, are polymerized in concentrated 
 solutions. 
 
 Sodium tetraborate gives normal conductivity results at 
 35, but at higher temperatures the increase in conductivity 
 with dilution is exceptionally rapid. The salt also has large 
 temperature coefficients of conductivity, and is undoubtedly 
 hydrated in solution. Boric acid being little dissociated and, 
 therefore, a weak acid, the sodium salt would certainly undergo 
 hydrolysis. By assuming both hydration and hydrolysis to 
 take place, the behavior of the salt is easily accounted for. 
 At the lower temperatures the hydrolysis, due to increasing 
 dilution, is balanced by the increasing complexity of the 
 fairly stable hydrates. As the temperature rises the hydrates 
 break down, while hydrolysis continues unchecked so that 
 the conductivity increases rapidly. 
 
 Calcium and magnesium chlorides give almost identical 
 results, except that the molecular conductivity of the cal- 
 cium salt is about ten conductivity units above that of magne- 
 sium chloride. The latter salt shows greater increase in the 
 value of fi v with dilution at 56, which accords with its greater 
 hydration, as shown by Jones and Bassett. 2 
 
 Nickel nitrate also shows large temperature coefficients. 
 It is known 3 to possess marked power of hydration. 
 
 The conductivity data for the sulphates of nickel, cobalt, 
 copper, and manganese are remarkably similar in every re- 
 
 1 Hydrates in Aqueous Solution; Carnegie Institution of Washington, Publica- 
 tion No. 60, pp. 80, 136, 148. 
 
 2 Am. Chem. J., 33, 555 (1905). 
 
 3 Jones: Hydrates in Aqueous Solution; Carnegie Institution of Washington, 
 Publication No. 60, p. 78. 
 
36 
 
 spect. There is little indication of an approach to p.^ at the 
 highest dilution employed. The temperature coefficients are 
 not large in concentrated solutions, but increase rapidly with 
 dilution. This behavior is probably due, in part at least, to 
 the polymerization of the sulphates in concentrated solu- 
 tions. 
 
 The molecular conductivity of the quaternary electrolytes, 
 chromium sulphate and ferric chloride, increases very rapidly 
 with dilution and also, in dilute solutions, with rise in tem- 
 perature. Hydrolysis undoubtedly plays a prominent part. 
 In the case of ferric chloride distinct precipitation, due to 
 hydrolysis, occurred at 65 in the N/8 and N/32 solutions. 
 The conductivity curve of this salt is interesting (Fig. IV). 
 
 65 5o 35 
 
 1024 
 
 512 
 
 128 
 32 
 
 idoo I5OO I4OO I3OO I2OO IIOO IOOO QOO 800 7OO 6OO 5OO 400 300 200 
 
 Conductivity 
 Fig. IV. Ferric chloride 
 
 The abrupt bend in the curve for 50 and 65 at the N/5I2 
 concentration indicates that the cause of the increasing con- 
 ductivity presumably hydrolysis is rapidly becoming less 
 effective. It would seem that under these conditions of tem- 
 perature and dilution the hydrolysis of the salt is very 
 great. 
 
 The ammonium and potassium alums were studied through 
 both ranges of temperature (o-35 and 35-65), and the 
 
37 
 
 values of p v recorded for 35 were deduced from all the read- 
 ings made at this temperature. Fig. V shows the conduc- 
 
 Conductivity 
 
 
 tivity-temperature curves for potassium alum through the 
 entire range of temperature. In strong solutions, at ordinary 
 
temperatures, molecular conductivity is nearly a linear func- 
 tion of temperature ; but at greater dilutions the curve in para- 
 bolic. 1 All of the salts studied in this investigation yield 
 conductivity-temperature curves of this same general charac- 
 ter. 
 
 The condition of double salts, when in solution, presents a 
 problem of interest. Investigators have sought for evidence 
 which would decide whether such salts, when dissolved, break 
 down into their constituent salts, which then dissociate in the 
 usual way; or whether they ionize to some extent as salts of 
 complex acids. Four investigations 2 bearing on the general 
 problem have been carried out in this laboratory. Jones and 
 Mackay compared the conductivity of certain alums with the 
 sum of the conductivities of the constituent salts. They 
 found the conductivity of the alums in dilute solutions to be 
 almost the same as the sum of the conductivities of the com- 
 ponents. In concentrated solutions the alums were found to 
 have a conductivity less than the sum of the conductivities of 
 the components, and the difference increased with the concen- 
 tration. The difference was greater than that observed when 
 mixtures of sulphates incapable of forming double salts were 
 compared. Similar methods were used by the other workers. 
 The general conclusion from these researches was that the 
 double salts in moderately concentrated solutions are not 
 wholly broken down into the simple salts. 
 
 In these investigations the conductivities were measured 
 at 25. As we now have at hand conductivity data over a 
 considerable range in temperature, it appears to be of interest 
 to apply the method of Jones and Mackay at other tempera- 
 tures. 
 
 The following is the table of Jones and Mackay 3 giving the 
 comparisons for potassium alum at 25: 
 
 1 Jones and Jacobson: Am. Chem. J., 40, 402 (1908). White and Jones: Ibid.. 
 44, 199 (1910). 
 
 2 Jones and Mackay: Ibid., 19, 83 (1897). Jones and Ota: Ibid., 22, 5 (1899). 
 Jones and Knight: Ibid., 22, 110 (1899). Jones and Caldwell: Ibid., 25, 349 (1901). 
 
 3 Ibid.. 34, 357 (1905). 
 
39 
 Table LXXIII. Potassium Alum, 25 (Jones and Mackay) 
 
 V 
 
 KaSO, 
 
 A1 2 (S0 4 ) 3 
 
 Sum/2 
 
 KA1SO 4 
 
 Diff. 
 Per cent. 
 
 5 
 
 172.7 
 
 108.0 
 
 140.3 
 
 133-9 
 
 4-5 
 
 8 
 
 183.3 
 
 124.2 
 
 153-7 
 
 149.2 
 
 3.0 
 
 20 
 
 205.1 
 
 I58.I 
 
 181.6 
 
 178.3 
 
 1.7 
 
 40 
 
 220.3 
 
 185.7 
 
 203.0 
 
 202.5 
 
 O.2 
 
 200 
 
 252.4 
 
 290.4 
 
 271.4 
 
 269.0 
 
 0.8 
 
 4OO 
 
 262 .2 
 
 342.6 
 
 302.4 
 
 305-2 
 
 + 0.9 
 
 This may be compared with Table LXXIV, which gives the 
 corresponding relations at o, 35, and 65. The values of 
 the conductivity of aluminum sulphate were kindly furnished 
 by Miss L. G. Winston. The conductivity values of potassium 
 sulphate are taken from the work of Jones and West. 1 
 
 Table LX XIV .Potassium Alum 
 
 V 
 
 K2SO 
 
 A1 2 (S0 4 ) 3 
 
 Sum/2 
 
 KA1SO 4 
 
 Diff, 
 
 
 Diff. 
 Per cent. 
 
 8 
 
 IOI . 
 
 9 
 
 65 
 
 2 
 
 83 
 
 .6 
 
 7 8. 
 
 9 
 
 4- 
 
 7 
 
 5-6 
 
 32 
 
 117. 
 
 9 
 
 89 
 
 5 
 
 103 
 
 7 
 
 IOI 
 
 .2 
 
 2 . 
 
 5 
 
 2.4 
 
 128 
 
 131 
 
 9 
 
 121 
 
 .8 
 
 126 
 
 9 
 
 127 
 
 .6 
 
 + 0. 
 
 7 
 
 + 0.5 
 
 512 
 
 142. 
 
 7 
 
 164 
 
 . i 
 
 153 
 
 4 
 
 158 
 
 .8 
 
 + 5- 
 
 4 
 
 + 3-5 
 
 
 
 
 
 
 
 35 
 
 
 
 
 
 
 8 
 
 220. 
 
 3 
 
 137 
 
 .2 
 
 I 7 8 
 
 .8 
 
 I6 5 
 
 3 
 
 -13- 
 
 5 
 
 7-5 
 
 32 
 
 259- 
 
 7 
 
 I 9 7 
 
 . I 
 
 228 
 
 4 
 
 215 
 
 7 
 
 12 . 
 
 7 
 
 5-5 
 
 128 
 
 296. 
 
 9 
 
 274 
 
 . I 
 
 285 
 
 5 
 
 283 
 
 7 
 
 - I . 
 
 8 
 
 0.6 
 
 512 
 
 3I9- 
 
 6 
 
 388 
 
 . I 
 
 353 
 
 9 
 
 358 
 
 3 
 
 + 4- 
 
 4 
 
 + 1.2 
 
 
 
 
 
 
 
 65 
 
 
 
 
 
 
 8 
 
 332- 
 
 8 
 
 188 
 
 4 
 
 260.6 
 
 240 
 
 ,6 
 
 20. 
 
 o 
 
 7-7 
 
 32 
 
 400. 
 
 
 
 264 
 
 .6 
 
 332 
 
 3 
 
 317 
 
 4 
 
 14. 
 
 9 
 
 4-5 
 
 218 
 
 456. 
 
 2 
 
 387 
 
 .6 
 
 421 
 
 9 
 
 426 
 
 .2 
 
 + 4- 
 
 3 
 
 1 .0 
 
 512 
 
 5 00. 
 
 7 
 
 581 
 
 .6 
 
 54i 
 
 . i 
 
 557 
 
 . I 
 
 + 16. 
 
 
 
 + 2.9 
 
 My values for "difference" in per cent, are of the same 
 order of magnitude as those obtained by Jones and Mackay, 
 and confirm their conclusions. It is noticeable that the per- 
 centage differences are nearly the same at the various tem- 
 peratures. This may be regarded as evidence that the break- 
 ing down of potassium alum in solution is little affected by 
 temperature, which, from other evidence, is known to be 
 true of dissociation in general. 
 
 i Am. Chem. J., 84, 357 (1905). 
 
40 
 
 In Table LXXV, from the work of Jones and Caldwell, 1 
 the conductivity of the double salt, potassium nickel sulphate, 
 is compared with the sum of the conductivities of the com- 
 ponents, all measurements being made at 25. Table LXXVI 
 shows the same relations for this salt at o and 35. The 
 values for the conductivity of nickel sulphate given in Table 
 LXXVI are taken from the work of Jones and Jacobson. 2 
 
 Table LXXV. Potassium Nickel Sulphate, 25 (Jones and 
 
 Caldwell) 
 
 
 
 
 
 
 
 Diff. 
 
 V 
 
 K2S0 4 
 
 NiS0 4 
 
 Sum 
 
 K 2 Ni(S0 4 ) 2 Diff. 
 
 Per cent. 
 
 8 
 
 182.4 
 
 77-9 
 
 260.3 
 
 219-5 
 
 40.8 
 
 -I 5 .6 
 
 40 
 
 22O.3 
 
 109.0 
 
 329-3 
 
 291 .6 
 
 37-7 
 
 II.4 
 
 80 
 
 237-9 
 
 122.8 
 
 360.7 
 
 323-7 
 
 37-0 
 
 10.3 
 
 400 
 
 262 .2 
 
 173-1 
 
 435-3 
 
 400.2 
 
 35-1 
 
 8.0 
 
 800 
 
 273.0 
 
 194.8 
 
 467.8 
 
 438.0 
 
 29.0 
 
 6.2 
 
 v 
 8 
 
 32 
 
 128 
 
 512 
 
 1024 
 
 8 
 
 32 
 
 128 
 
 512 
 
 1024 
 
 Table LXXVI. Potassium Nickel Sulphate 
 
 NiS0 4 
 40.4 
 
 54-8 
 
 73-9 
 
 93-i 
 
 100.4 
 
 90.9 
 123.0 
 168.4 
 
 213-5 
 234.6 
 
 IOI .9 
 II7.9 
 
 I3I-9 
 142.7 
 
 145-0 
 
 219.8 
 256.9 
 
 291 .o 
 
 318.4 
 325-0 
 
 
 
 
 
 Sum 
 
 K 2 Ni(S0 4 ) 2 
 
 Diff. 
 
 H2.3 
 
 122 .6 
 
 19.7 
 
 172.7 
 
 155-4 
 
 17-3 
 
 205.8 
 
 187.5 
 
 I8. 3 
 
 235-8 
 
 219.6 
 
 16.2 
 
 245-4 
 
 235-5 
 
 9.9 
 
 35 
 
 
 
 310.7 
 
 268.3 
 
 42.4 
 
 379-9 
 
 339-7 
 
 4O.2 
 
 459-4 
 
 414.1 
 
 45-3 
 
 531-9 
 
 490.7 
 
 41.2 
 
 559-6 
 
 527-1 
 
 32-5 
 
 Diff. 
 Per cent. 
 
 -I 3 .8 
 IO.O 
 -8. 9 
 
 9 
 .o 
 
 13-7 
 10.6 
 
 9-8 
 
 7-7 
 -5-8 
 
 The percentage "differences" at o and 35 agree closely 
 with those found by Jones and Caldwell at 25, showing that 
 the relations which they established as holding at 25 are also 
 true at higher and lower temperatures. My results also ac- 
 cord with the general law that dissociation is nearly independ- 
 ent of temperature. 
 
 1 Am. Chem. J., 25, 349 (1901). 
 
 2 Ibid., 40, 390 (1908). 
 
SUMMARY 
 
 1. The molecular conductivities of fifteen inorganic salts 
 from o to 35, and of sixteen inorganic salts from 35 to 65, 
 were measured by the Kohlrausch method. The tempera- 
 ture coefficients of conductivity, both in conductivity units 
 and in percentages, were calculated for these salts through the 
 ranges of temperature above stated. The percentage disso- 
 ciations were also calculated in all cases where the data were 
 sufficient. 
 
 2. Jones and his coworkers 1 have shown that the ions of 
 an electrolyte are hydra ted in aqueous solutions, and that the 
 complexes break down with rise in temperature, thus increas- 
 ing the conductivity. If this is true, substances of large 
 hydrating power should have large temperature coefficients 
 of conductivity. Jones 2 showed this to be true for the sub- 
 stances studied by Jones and West. 3 The substances which 
 I have studied show the same relations and my results are 
 in perfect accord with the theory of hydration. 
 
 3. Hydrolysis is evidently a frequent cause of abnormally 
 great conductivity. It is increased both by dilution and by 
 rise in temperature. 
 
 4. Another probable cause of abnormally rapid increase in 
 conductivity is decrease in polymerization. There is evidence 
 that sulphates are polymerized in concentrated solutions. 
 
 5. Observers have found an increase in the conductivity 
 of a solution of a chromium salt when it is changed from the 
 violet to the green variety. My results show that while the 
 conductivity is increased in concentrated solutions by this 
 change, the increase is relatively less at higher dilutions. 
 The conductivity of the green variety may even fall below 
 that of the violet variety. This would appear to show that 
 the green variety is not as susceptible to hydrolysis by dilu- 
 tion as is the normal violet form. 
 
 1 Hydates in Aqueous Solution; Carnegie Institution of Washington, Publication 
 No 60. 
 
 2 Am. Chem. J., 35, 445 (1906). 
 
 3 Ibid., 34, 357 (1905). 
 
42 
 
 6. Jones and his coworkers 1 found that the conductivities 
 of alums and other double salts were less than the sum of the 
 conductivities of the constituent salts. They inferred that 
 double salts exist as such to some extent in concentrated 
 solutions. Their work was done at 25. I have made 
 similar comparisons at other temperatures, and find that the 
 relations pointed out by them as holding at 25 also manifest 
 themselves from o to 65. In addition, my results show 
 that the breaking down or dissociation of double salts, like 
 dissociation in general, is little affected by temperature. 
 
 The following general relations, established by previous 
 investigators, are true of the salts which I have studied: 
 
 7. The temperature-conductivity curves for concentrated 
 solutions are nearly straight lines; at higher dilutions the 
 curves are often parabolic. 
 
 8. The percentage temperature coefficients increase with 
 dilution, but decrease with temperature. Temperature co- 
 efficients in conductivity units increase with dilution. 
 
 9. Dissociation decreases with temperature. Four salts 
 among those studied seem to be exceptions to the rule. 
 
 * Jones and Mackay: Am. Chem. J., 19, 83 (1897). Jones and Ota: Ibid., 22, 5 
 (1899). Jones and Knight: Ibid., 22, 110 (1899). Jones and Caldwell: Ibid., 25, 
 349 (1901). 
 
BIOGRAPHY. 
 
 Henry Hallock Hosford was born July 12, 1859, at Hudson, 
 Ohio. He prepared for college at Hudson and entered West- 
 ern Reserve College, graduating with the degree of Bachelor of 
 Arts in 1880. Three years later he received the degree of 
 Master of Arts from his Alma Mater. 
 
 After teaching for several years in Western Reserve Academy, 
 Mr. Hosford became professor of chemistry in Doane College, 
 Crete, Nebraska, which position he still occupies. In 1892 he 
 married Jennie Chamberlain, daughter of Dr. W. I. Chamber- 
 lain, of Hudson, Ohio. They have four children. 
 
 In October, 1909, Mr. Hosford entered Johns Hopkins 
 University as a graduate student in Chemistry with Physical 
 Chemistry and Physics as his subordinate subjects. 
 
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