177 



NH4CI. . . .Very soluble with evolution of ammonia. 



LiCl Soluble. 



FeCls Slightly soluble. 



S11CI2 Insoluble, unchanged. 



C0CI2 . . . .Reacts with evolution of heat, forming greenish yellow precipitate. 

 PbBr2 . . . .Reacts, forming white precipitate which afterward redissolves. 



KI Insoluble, unchanged. 



Cdl2 Reacts, forming white, insoluble precipitate. 



AgCN . . . .Slightly soluble. 



Hg(CN)2. .Slightly soluble. 



AgN03 . . .Soluble with evolution of much heat. 



NaN03 . . . Insoluble, unchanged. 



Pb(N03)2.. Reacts, forming white, insoluble precipitate. 



It is thus seen that, in all cases where the salt dissolves appreciably, 

 there is evidence of chemical action, either through the evolution of heat 

 or the formation of a precipitate, or both. In the case of ammonium 

 chloride the well known action of evolution of ammonia was observed. 

 There is, therefore, every reason for expecting that complex salts will be 

 formed in every case excepting the last, where no doubt ethyl amine 

 hydrochloride is produced, as Shinn has pointed out. If this be true, the 

 question still remains as to whether the reaction is complete as soon as 

 the salt is all in solution, so that henceforth all physical properties 

 will be those of a solution in ethyl amine of a definite double or complex 

 salt, changing with dilution only with respect to the degree of ionization. 

 With the investigations of Hofmann and Marburg and of Bonnefoi in 

 mind, the answer to this question would certainly he negative. We should 

 expect that the ratio of ethyl amine to simple salt combined with it would 

 not only change with lowering of temperature, hut that it would increase 

 with decreasing concentration, because as dilution progresses the ratio 

 of amine to salt in solution increases. If the conductivity of the complex 

 salt is much less than that of the simple salt the change in molecular 

 conductivity with change in concentration would be the resultant of two 

 influences, i. e., change in ionization and change in complexity of the 

 ions. The migration velocity of a complex cation containing one or more 

 molecules of ethyl amine could not be very high, and it is not likely that 

 such a compound would possess a very high degree of ionization. This 

 fact would then result in a more or less gradual tendency toward falling 

 off in the molecular conductivity with increasing dilution, since we are 

 actually dealing not only with more complex compounds, whose ioniza- 



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