1908-9.] Hydrolysis of Salts of Amphoteric Electrolytes. 655 
The values for the hydrolysis constant of a non-amphoteric electrolyte 
as obtained from the two methods are thus seen to agree comparatively 
well with each other. 
V. 
Conductivity. 
g Catalysis. 
16 
174-8 
173-6 
32 
198-2 
190 
Evidently the theory holds good so long as the base is non-amphoteric, 
and either method is equally good as a gauge of the hydrolysis. 
The Ratio of Distribution of a base between two solvents has been used 
by Farmer * as a method of estimating the basic constant. His value for 
o-amidobenzoic acid at 25° corresponds very well with that obtained from 
the rate of catalysis of methyl acetate, viz. ^- = 118. 
The Solubility of the amphoteric base in water and in acid of different 
concentrations was then investigated, as giving a measure of the 
hydrolysis. Bottles of resistance-glass were used for these estimations. 
They were almost filled with the solvent, the air above which was 
replaced by nitrogen in order to preclude oxidation. The liquids were 
shaken up with recrystallised anthranilic acid in a thermostat at 25° C. 
At intervals of some hours portions of the liquids were siphoned off 
through a filter into weighed flasks and titrated against twentieth-normal 
caustic soda solution. 
In the acid solutions it is assumed that the concentration of free base is 
the same as the concentration of the saturated aqueous solution, and that 
the extra base dissolved is therefore all in the form of combined hydro- 
chloride. The values obtained in this way for ^ are not constant for the 
different strengths of acid used, but at v = 16 especially seems to approximate 
most closely to the catalysis value. 
The solutions containing hydrochloric acid became saturated compara- 
tively quickly, but the o.-amidobenzoic acid dissolved in the water very 
slowly, the acidity still increasing slightly after several days’ shaking. 
* Journal Chem. Soc., vol. 79, p. 863 ; vol. 85, p. 1713. 
