WORK OF H. R. KREIDER. 103 



These facts make it appear probable that there is approximately such a constant 

 for binary electrolytes and another for ternary electrolytes. These data are not suffi- 

 cient, however, to give a final value to such constants. Further investigations will 

 be required for this purpose. Most of these maxima occur at dilutions of V = 12,800 

 to V= 51,200. At these dilutions it is very difficult to obtain accurate results, and 

 the values for the constant are probably within the limits of experimental error. 



The value for the constant between methyl and ethyl alcohols for binary elec- 

 trolytes appears to be very nearly 2.37. We have obtained but one value for ternary 

 electrolytes, which is 3.68. That is nearly 1.5 X 2.37. The latter value (3.56) is prob- 

 ably the more nearly correct. The factor 1.5 is employed, since this expresses the 

 ratio of ions present between binary and ternary electrolytes at complete dissociation. 



With the data in hand we proceeded to test further the accuracy of the above 

 equation, by supplying by calculation in table 70 those fx x values which could not 

 be determined experimentally. The value of the constant was taken as 2.37 for 

 binary electrolytes, and 3.56 for ternary electrolytes. The calculated value for 

 potassium iodide in methyl alcohol at from the value in ethyl alcohol would be 

 77.5. An examination of table 64 reveals the fact that this value is probably very 

 nearly correct. For 25 it would be 112.6. Again, from the same table this is 

 probably correct. Ammonium bromide in ethyl alcohol at would be equal to 

 30.3. This, too, as indicated by table 64, is probably nearly correct. Potassium 

 sulphocyanate in methyl alcohol at 25 would have a value of 110.4. Table 64 

 indicates that this value is probably correct to within the limits of experimental 

 error. Lithium nitrate gives a value of 96.7 in methyl alcohol at 25; compared 

 with table 64 this would seem to be nearly correct. 



With ternary electrolytes there are only three cases to which this equation can 

 be applied. Copper chloride in ethyl alcohol at would give a value of 24.8, and 

 cobalt chloride in ethyl alcohol at 25 would give 46.7 as the value for the maximum 

 in conductivity. In table 64, at 0, a maximum is reached at V= 25,600. The 

 maxima at the different temperatures as a rule do not occur very far apart. We 

 believe that the value 46.7 is very nearly correct for the maximum for cobalt chlo- 

 ride in ethyl alcohol at 25. The only two values which do not fit into the table are 

 those for potassium cyanide in methyl alcohol at 0, and for copper chloride in ethyl 

 alcohol at 25. The latter, however, is not far from what we might expect it to be. 



We believe from the above results that the ratio between the maxima in molecular 

 conductivity for different salts in methyl alcohol, and the maxima for the same salts 

 in ethyl alcohol is probably constant for all binary electrolytes; that for all ternary 

 electrolytes it is a constant of different value, and that there is a definite relation 

 bet ween these two constants. 



Jones, in an article on "The Electrolytic Dissociation of Certain Salts in Methyl 

 and Ethyl Alcohols, as Measured by the Boiling-Point Method," gives table 72, 

 which expresses "the dissociation values of the above alcohols as calculated from 

 data obtained by the boiling-point method." The ratios of these values were cal- 

 culated and are also expressed in the table. 



Leaving out the value 1.8 for sodium iodide, which is evidently erroneous, we 

 find as a mean from the other values of the binary electrolytes 2.37, which, it will be 



