48 ROYAL SOCIETY OF CANADA 



From tliese values it will be seen that the conductivit}^ of a silver 



nitrate solution steadily increased with the concentration. 



N 

 Summary. — 1. Tables I-III shew that as a , ^^^ ■ solution of 

 ^ 10000 



HCl was added to water there was, at first, very little change in the 



conductivity of the solution, but as the HCl solution became more 



concentrated the conductivity gradually increased. 



2. Tables IV-IX shew that on the addition of HCl to AgNOg of 

 various dilutions a drop in the conductivity was observed. When, 

 however, a 39.5 x 10"'^ normal silver nitrate solution was reached this 

 effect disappeared, 



3. A similar drop in the conductivity was observed when a 

 dilute nitric acid solution was added to a dilute silver chloride solu- 

 tion. Also, when a dilute silver nitric solution was added to a dilute 

 solution of hydrochloric acid. 



4. In the case of the silver nitrate solution (Experiment VII) the 

 conductivity steadily increased with the concentration. 



Explanation. — Two explanations may be given of the above 

 phenomenon (1) The fact that, in Experiment III, the conductivity 

 remains steady at first, may be due to the absorption of hydrogen by 

 the platinum electrodes, and (2) The drop in conductivity indicated 

 in Experiments IV, V, VI may be due to the hydrogen ion attracting 

 to itself the neutral AgCl, and becoming loaded. Its mobility might, 

 thereby, be decreased so as to have a value below that of the silver 

 ion which it displaced. 



Up to the present the results obtained are not sufficient to dis- 

 criminate between these two explanations, and it is hoped that with 

 additional observations the problem raised may be cleared up. In 

 conclusion I wish to thank Mr. E. F. Burton for his kind assistance 

 in the course of these experiments. 



