178 PROPERTIES OF ELECTRICALLY CONDUCTING SYSTEMS 



the metal has been transformed to the complex. This behavior is due 

 to the fact that the solutions of this complex possess a negative viscosity 

 relative to that of pure water, while solutions of the original salt possess 

 a positive viscosity with respect to pure water. 



In non-aqueous solutions, we find similar relations; that is, inter- 

 action often takes place between the second solvent component and the 

 electrolyte. Thus, the ionization of solutions of a large number of salts 

 appears to be greatly affected by the addition of a small amount of water. 

 This is particularly the case with electrolytes which exhibit a marked 

 tendency to form complexes with water. If a salt, which exhibits a 

 marked tendency to form hydrates, is dissolved in a medium, with 

 which this salt has little tendency to form a solvate complex, then 

 the salt will be relatively little ionized when dissolved in this solvent. 

 On addition of water to such a solution, the salt apparently forms a 

 complex with water, whose ionization in the original solvent is much 

 greater than that of the anhydrous salt. Solutions of potassium chloride 

 or iodide, for example, are highly ionized in acetone and their ionization, 

 and consequently their conductance, is but little affected by the addition 

 of water. On the other hand, lithium chloride, which shows a pronounced 

 tendency to form complexes with water, is ionized to only a relatively 

 slight degree in pure acetone. On the addition of water to a solution 

 of a lithium salt in acetone, the conductance is greatly increased. Similar 

 results have been obtained in the case of calcium chloride. 



2. Conductance of Salt Solutions on the Addition of Small Amounts 

 of Water. In Table LXIV are given values of the conductance of solu- 



TABLE LXIV. 

 CONDUCTANCE OF SALTS IN ANHYDROUS PROPYL ALCOHOL AT 25 . 1 



Nal 



CX10 3 



0.0623 



0.1581 



0.3902 



0.6591 



1.498 



2.310 



5.890 



13.26 



27.77 



53.40 



Ca(N0 3 ) 2 Anhydrous 

 C X 10 3 A mo i 



19.94 

 19.36 

 18.36 

 17.72 

 16.30 

 15.40 

 13.23 

 11.28 

 9.815 

 8.400 



0.363 



0.792 



1.617 



3.326 



5.908 



7.247 



14.320 



24.930 



43.290 



5.140 

 3.834 

 2.894 

 2.184 

 1.798 

 1.688 

 1.258 

 0.976 

 0.772 



*Kraua and Bishop, J. Am. Chem. Soc. 43, 1568 (1921). 



