664 
Proceedings of the Royal Society of Edinburgh. [Sess. 
and still more from the results of catalysis. We find, however, that those 
methods of ascertaining the hydrolysis of o-amidobenzoic salts which depend 
directly on the concentration of liydrion in the solution agree fairly well 
with each other, i.e. catalysis of methyl acetate by the hydrochloride, and 
of diazoacetic ester by the nitrate, and the electro-motive force. The 
solubility and distribution between two solvents also point to the same 
value being correct, The question is, then, why should not the more 
indirect methods — conductivity and freezing-point — lead to the same 
result ? 
The molecular conductivity of a sixteenth normal solution of antlira- 
nilic hydrochloride is 173. The amount contributed to this by the 
liydrion present is, according to the catalysis value for the hydrolysis, 
392 
•313 X X 352 — 102*7. Then, assuming the chloride to be ionised to about 
the same extent, the conductivity supplied by chloridion is *9x68 = 6T2. 
Thus there is left for the anthranilic ion M = 173 — (102 - 7 + 6T2) = 9, 
which is not nearly enough to correspond with 68‘7 per cent, of 
chloridion. 
Or we can account for the specific conductivity of the solution in this 
way. 
The total specific conductivity is 
173 
16 
10*8. The hydrochloric acid 
present supplies *313 x 
392 
16 
= 7*6. 
This leaves a specific conductivity for 
the salt of 32, i.e. a molecular conductivity of 51 ‘2 — not nearly enough for 
the 68 ‘7 per cent, of anthranilic hydrochloride. 
Evidently the method of calculating the hydrolysis from conductivity 
and freezing-point data is not legitimate, on account of some factor 
being overlooked, or perhaps unknown. We assume, for example, that 
the degrees of ionisation of the acid and salt, and the speeds of their 
ions, are quite normal, and that the water itself acts quite normally 
even in presence of the large quantities of ions formed from the strong 
electrolytes present. 
In accounting for the conductivity, the small amount left for the hydro- 
chloride seems to point to its ionisation being abnormally small. If this 
were so in the comparatively dilute sixteenth-normal solution, it would show 
up much more in a more concentrated, say half-normal, solution, where the 
ionisation would probably be reduced to zero, and the hydrolysis, as calculated 
from the conductivity at that concentration, would therefore appear to differ 
still more from the catalysis value. 
