104 



WORK OF H. It. KREIDEK. 



remembered, is the same as the value obtained above by the conductivity method 

 for the ratio between the maxima in the different alcohols. The figure in this table 

 for the one ternary electrolyte is not so great as that determined by the conductivity 

 method, and yet it is possible that more data would give comparable values. 



Table 72. Dissociation in Methyl and Ethyl Alcohols. 



Substance. 



KI 



Nal 



NaBr 



NH 4 Br 



CH3COOK. 

 CHsCOOXa 

 Ca(N0 3 ) 2 ... 



Dissociation j Dissociation 



in ethyl Ratio, 

 alcohol. alcohol. 



Dilution 



normal. I "W^ 1 



p. ct. 

 25 

 33 

 24 

 21 

 16 

 14 

 5 



2.08 



1.8 



2.5 



.3 



.3 



.7 



.0 



2. 

 2. 

 2. 

 3. 



The boiling-point data in this work were obtained by means of the boiling-point 

 apparatus used by Jones. 1 Both solvents were carefully purified and dried. 



Table 73 gives the dissociation of certain salts as calculated by both the conduc- 

 tivity and boiling-point methods. 



It will readily be seen from table 73 that the dissociation values as determined by 

 conductivity are higher than those found by the boiling-point method in both methyl 

 and ethyl alcohols. This may possibly be due to a polymerization of the undisso- 

 ciated molecules in the solvent in question. This would give too low dissociation 

 as measured by the boiling-point method, since this method takes into account both 

 the molecules and the ions, while the conductivity method deals only with the ions. 



Table 73. Dissociation of Salts as Determined by the Conductivity and Boiling-point Methods. 



Salt. 



Solvent. 



Dissociation from 



conductivity 



method. 



Dissociation from 



boiling-point 



method. 



KI Methvl. 



KI Ethyl. 



Nal Methyl. 



NH.Br Methyl. 



NHJBr I Ethyl. 



p. ct. 

 65 

 49 

 75 

 71 

 40 



p. ct. 

 49 

 26 

 61 

 47 

 20 



SUMMARY. 



We have measured the conductivity of various salts in pure methyl and ethyl 

 alcohols at very high dilutions, and also in mixtures of methyl and ethyl alcohols 

 with water. In many of these measurements we have found the value of /jl x . 



Many of these values were found to occur at concentrations between V = 3,200 

 and 7 = 51,200. 



A constant ratio was found between the values of fi x for several binary electro- 

 lytes in methyl alcohol and in ethyl alcohol, and the ratio for one ternary electrolyte 



'Zeit. pbye. Cliom., 31, 114 (1809) (JubclLnnd zu van't Hofl"). 



