General Discussion of Results. 
435 
Table XXXV. 
y 
KBr 
NH 4 Br 
KT 
nh 4 i 
A 
B 
C 
A 
B 
C 
A 
B 
C 
A 
B 
C 
16 
123.1 
' 
59.82 
127.2 
65.43 
61.16 
124.5 
69.20 
62.13 
125.4 
72:24 
62.63 
32 
127.5 
69.02 
62.46 
131.8 
72.73 
63.81 
128.2 
76.35 
64.37 
129.6 
78.74 
65.04 
64 
130.5 
76.70 
65.36 
135.3 
79.56 
66.04 
130.5 
82.52 
66.01 
133.4 
85.0 
67.48 
128 
132.9 
83.60 
67.11 
138.6 
85.80 
67.45 
133.0 
88.69 
67.45 
135.9 
91.14 
69.28 
256 
136.4 
88.96 
69.26 
141.2 
90.88 
68.32 
135.8 
93.85 
68.28 
138.7 
96.20 
70.34 
512 
140.2 
93.26 
70.53 
143.5 
94.99 
69.10 
137.9 
98.19 
69.65 
141.3 
100.6 
71.12 
1024 
143.4 
97.25 
145.6 
98.24 
70.11 
140.9 
102.2 
70.55 
143.7 
104.7 
71.5? 
It will be noticed that the conductivity of the halogen salts 
of the alkalies in methyl alcohol (B) is considerably less than 
in aqueous solutions (A). When water is added to the extent 
of 50 per cent, even (C), the conductivity is somewhat less than 
it is in absolute methyl alcohol. Cohen and others have 
pointed out the same fact; that is, at 18° C. the conductivity 
of a mixture consisting of water and methyl alcohol, and con¬ 
taining more than 60 per. cent of alcohol, is less in dilute solu¬ 
tions than it is in absolute alcohol. This fact seems to be 
rather difficult to reconcile with the electrolytic dissociation 
theory, for here we have two solvents that possess dissocia¬ 
tive power in a high degree, and yet a salt dissolved in a mix¬ 
ture of equal parts of these yields a solution the conductivity 
of which is less than that of the solutions formed when dis¬ 
solved in either. 
Carrara 1 has shown that the electrolytic dissociation of water 
in methyl alcohol is greater than it is in aqueous solutions, 
while the reverse is the case in ethyl alcohol. It is also of in¬ 
terest to note that KOH and NaOH in methyl alcohol show 
the same conductivity as CH 3 OK and CH 3 ONa. 
1 Gazz., Chem. Ital., 27, I, 422; 1897. (Ref.) Jour. Chem. Soc., 72, ii, 
473; 1897. 
