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This historic book may have numerous typos and missing text. Purchasers can download a free scanned copy of the original book (without typos) from the publisher. Not indexed. Not illustrated. 1913 Excerpt: ...probably due to the great solvation at this extremely high dilution. The same fact may be noticed in several other tables where ethyl alcohol is used as a solvent. Table 74 gives the conductivity of lithium bromide in methyl alcohol. At 0 complete dissociation probably is reached at 6,400 liters. At 25 there is no maximum in conductivity, but the rate of increase is much smaller above 3,200 liters than it is at greater concentrations, indicating that the maximum is nearly reached. Table 74 gives the conductivity of lithium bromide in ethyl alcohol. At 0 there is complete dissociation at 3,200 liters. At 25 it is complete at 6,400 liters. For both temperatures at higher dilutions the conductivity remains almost constant up to a dilution of 102,400 liters, where, at 25, there is a marked decrease in the conductivity. Table 74 gives the conductivity of potassium sulphocyanate in methyl alcohol. This is a repetition of work previously done. We have now obtained more concordant results. Here, complete dissociation is reached at both temperatures at 3,200 liters. Table 74 gives the conductivity of cobalt bromide in both methyl alcohol and ethyl alcohol. Here, there is no maximum in conductivity. This is probably due to the fact that cobalt bromide is much solvated. Table 75 gives the ratios of the values of ntor a number of salts in the following solvents: Water and ethyl alcohol, methyl alcohol and water, and methyl alcohol and ethyl alcohol. When we consider the large magnitude of the experimental error in working at these great dilutions, it is quite probable that the relation nx for one solvent/n x for another sol vent=c, holds where the salts have approximately the same degree of solvation. That there is a constant relation between the values of lj,x for dif...
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