OTHER PROPERTIES OF ELECTROLYTIC SOLUTIONS 285 



sity of the salt. In Table CXII are given values of B C , so calculated, 

 together with values of B & as experimentally determined by Heydweiller 

 for different salts in water. 



TABLE CXII. 



COMPARISON OF EXPERIMENTAL AND CALCULATED VALUES OF B. 

 Salt B e B c Salt B e B C 



NH 4 I 8.38 8.55 LiN0 3 3.71 4.02 



NaCl 3.36 3.15 LiCl 2.06 2.17 



NaN0 3 4.88 4.74 Nal 10.45 10.77 



KN0 3 5.21 5.30 1/2 CaI 2 .... 11.55 11.70 



1/2 K 2 S0 4 . .. 5.73 5.45 1/2 BaBr 2 . . . 11.80 11.75 



KC10 3 6.73 7.00 1/2 BaI 2 15.56 15.58 



AgN0 3 13.28 13.04 1/2 CdN0 3 . . 9.21 9.15 



From an inspection of the table it appears that the values of B e and 

 # are in remarkably good agreement. The differences probably do not 



G 



exceed the experimental error. The values calculated in this way, how- 

 ever, do not in all cases agree as well as those appearing in the above 

 table. In the case of salts which show a marked tendency to form 

 hydrates, Heydweiller has employed the density of the hydrated salt 

 rather than that of the anhydrous salt and has obtained excellent agree- 

 ment between the observed and the calculated values of the constant B, 

 while in another group of electrolytes the values of B as calculated are 

 not in close agreement with those as measured. This is illustrated in the 

 following table. 



TABLE CXIII. 



COMPARISON OF EXPERIMENTAL AND CALCULATED VALUES OF B. 

 Salt B p B r Salt fl fl 



\j c 



NH 4 C1 0.42 1.83 KC1 2.94 3.71 



NH 4 Br 4.45 5.69 KBr 6.65 7.48 



NH 4 NO, 2.60 3.39 KI 10.56 11.20 



1/2 N 2 H 8 S0 4 . 2.49 2.87 KCNS 3.70 4.57 



Lil 9.53 10.10 1/2 K 2 Cr0 4 . . 5.83 6.16 



LiBr 5.84 6.19 RbCl 6.24 7.79 



CsCl 10.36 12.62 



While there is a marked deviation between the values of B as derived 

 from the experimental curves and as calculated from the density of these 



