384 



BULLETIN OF THE UNIVERSITY OF WISCONSIN. 



[D. C. = 62] of the latter. But solutions of hydrochloric acid 

 in this solvent show but slight dissociation. Nernst 1 in refer- 

 ring to this case assumes that some specific influence of the sol- 

 vent comes into play, probably the association of the ions with 

 the molecules of the solvent. 



Another exception is noted by Franklin and Kraus 2 in their 

 researches on the electrical conductivity of liquid ammonia solu- 

 tions. Mercuric cyanide, according to Ostwald, 3 is not at all 

 dissociated in water, but Franklin and Kraus find that in ammo- 

 nia it forms a solution which possesses a distinct conductivity. 

 Again, the phenols yield good conducting solutions in ammonia, 

 while in water they form solutions which have relatively low 

 conductivity. The following table illustrates this point. It 

 gives the molecular conductivities of orthonitro-phenol in water 

 at 18° C. and in liquid ammonia at — 38° C. 



Table X. 



Choral and ethyl acetate, according to Drade, 6 have the values 

 6.67 and 5.85, respectively, for their dielectric constants. The 

 former, according to Kahlenberg and Lincoln, 7 yields solutions 

 with ferric chloride which show no appreciable conduction, 

 while the latter yields solutions with it, which show a distinct 

 conductivity. 



From the work of the same investigators we see 



1 " TheoretLsehe Chemie," p. 365. (Dritte AufHageJ. 



2 Am Chem. Journal, 23, 207, (1900 .>. 



3 Grundlinien der anorg. Chem. p. 657. 



4 Bader: Zeit. phys. Chem. 6, p. 206, (1890). 



5 Am. Chem. Jour. 23, p. 29."), (1900). 

 • Zeit. phys. Chem. 23, p. 309, (1897). 

 7 Jour. Phys. Chem. 3, 12, (1899). 



