146 Conductivities and Viscosities in Pure and in Mixed Solvents. 



suggested as the cause of these high values. He also shows that the 

 conductivity of most organic acids is a parabolic function of the tem- 

 perature, but concludes that no general statement can be made con- 

 cerning the change in dissociation with temperature change, since the 

 behavior of solutions of organic acid is not in accord with the Thompson- 

 Nernst hypothesis connecting dissociating power and dielectric constant. 



Clover 1 continued this work, but over a wider range of temperature. 

 Some measurements were made at a temperature of 80. West 2 and 

 Wightman 3 also did work in this field. The results obtained by these 

 investigators were in accord with the findings of their predecessors. 



Alum and other soluble salts were studied by Hosford and Jones. 

 They found that the conductivity of an alum is less than the conduc- 

 tivity of the constituent salts. This is evidence in favor of a theory 

 advanced by Jones regarding the existence of double salts, as such, in 

 concentrated solutions. 



While studying the conductivity of a number of electrolytes in 

 aqueous solutions, Winston and Jones 4 found apparent exceptions to 

 the earlier work, viz, an increase in percentage dissociation with rise 

 in temperature, and large temperature coefficients when there were no 

 indications of large hydration. This led Winston to advance the theory 

 that inductive action takes place through the solvent between charged 

 ions and neutral molecules, giving rise to complex molecules and ions 

 in solution. 



Wightman, 6 Springer, 6 and Smith 7 extended the work previously 

 done in this laboratory on organic acids. The last-named investigator 

 found that Euler's equation 



holds in every case studied, and calls attention to the fact that isomeric 

 acids do not behave similarly with regard to change in dissociation. 

 That the migration velocity of anions is a function of the number of 

 atoms constituting the anion was indicated by his experimental work. 



Howard 8 and Shaeffer 9 have each published papers on conductivity 

 work carried out under the direction of Jones. 



In this brief review of the conductivity studies made in this labora- 

 tory, attention has been called to work done only on aqueous solutions. 

 Similar work has been carried out by Jones and his collaborators, using 

 glycerol, ethyl alcohol, and formamid as solvents. A considerable 

 number of investigations involving various mixtures of different solvents 

 have been carried out. For a full account of this work, Publications 

 80, 180, and 210 of the Carnegie Institution of Washington should be 

 consulted. 



1 Amer. Chem. Journ., 43, 187 (1910). *Ibid., 46, 368 (1911). ''Ibid., 50, 1 (1913). 

 *Ibid., 44, 508 (1910). 6 Ibid., 48, 320 (1912). *Ibid., 48, 500 (1912). 



*Ibid., 46, 56 (1911). Ibid., 48, 411 (1912). 9 Jbid., 49, 207 (1913). 



