SEVENTH ANNUAL MEETING 83 



7. The hindering of a reaction by adding something which does 

 not give like ions. 



8. Faraday's Law holds for non-aqueous solutions. 



9. The equation for degree of ionization calculated on the basis 

 of concentration does not always hold, even for typical salts. 



These are only a few of the reasons, and many more might 

 be given on each side. 



Let us now consider some of the recent work, more in detail. 



The work of Walden of Rega apparently showed that there 

 was a direct parallelism between the dissociation power as in- 

 dicated by the conductivity and the dielectric constant. With- 

 out a doubt, this was true for the one solute that he used, but 

 it has been equally well established by work done at Wisconsin 

 and by some unpublished work done in our laboratory, that this 

 relation does not hold in all cases. 



Creighton of Halifax on the other hand gives results in a 

 recent paper which show that for aniline in acetophenone the 

 Nernst-Thomsen rule does hold. Also Davis of Dalhousie Col- 

 lege found the same relations for rosaniline hydrochloride in 

 organic solvents, as Walden did for his solute. 



Thornton of the University of Durham, says in explana- 

 tion of some high values for the dielectric constant obtained 

 for some liquids such as water, that it is an effect depending 

 on the electrical conductivity. 



To get his results Walden assumed that the conductivity 

 of the solvents which he had especially purified was due to 

 ionization. This is likely not the case for the reason that the 

 conductivity is dependent upon the mode of purification. In 

 this connection I will recite the recent work of Corvallo, pub- 

 lished in C. R., in which he states that he obtains ether so pure 

 that its conduction is very likely due to impurities. 



Viscosity is recognized as having considerable influence on 

 the conductivity of a solution. Lloyd of Alabama has recently 

 showed that he gets entirely different maxima at 50° C. than 

 he does at 100° C. for the same solutions, and this difference 

 he attributes to changes in viscosity. Pratolongo of Milan de- 

 termined the conductivity of a solution of citric acid with 

 hydrochloride, arsinous, or phosphoric acids dissolved in it, and 

 found that each addition reduces the specific conductivity. 

 This effect is ascribed in part to an increase of the viscosity of 

 the solution by these additions. 



Some very interesting results have been obtained by the 

 prolonged passage of an electric current through ammonia or 



