470 Dr. Harry 0. Jones on the 



The results with the three alkalies cannot be regarded as so 

 accurate as those with the acids and salts. The solutions were 

 of necessity in contact with the air and must have absorbed 

 small amounts of carbon dioxide. The solutions were, how- 

 ever, so very dilute that the magnitude of the error could 

 not have been great. 



The Results with Electrolytes. 



On account of the method of preparing the solutions, the 

 concentrations actually investigated are not those which are 

 commonly employed in work : they are not simple fractional 

 parts of a normal solution. The results with the solutions 

 used have already been partly recorded *, and the remainder 

 will appear later in the same journal. For convenience in 

 comparison and for future work, the results obtained have 

 been plotted as curves, and the lowering of the freezing- 

 point for simple decimal parts of a normal solution read off 

 from the curves. The remaining values for each concentra- 

 tion have been calculated from this lowering. 



In the Tables, column 1 contains the strength of the solu- 

 tions in terms of gram-molecular normal. This was employed 

 instead of gram-equivalent normal, because a molecule pro- 

 duces the same lowering of the freezing-point whatever the 

 equivalence of the acid or base may be. Column 2 contains 

 the corrected lowerings of the freezing-point. Column 3, the 

 lowerings of the freezing-point which would have been pro- 

 duced by a gram-molecular weight of the compound = gram- 

 molecular lowering. Column 4, the different values for i, 



. &T. molec. lowering 



e = — -y 



1-89 



1/89 being the constant for water, i. e. the amount of the 

 lowering of the freezing-point of water produced by a gram- 

 molecular normal solution of a completely undissociated 

 compound. Column 5, the dissociation, = i— 1 when the 



2 — 1 



molecule dissociates into two ions, and — ^- when the molecule 

 dissociates into three. 



When the molecule yields two ions the dissociation is 

 calculated thus : 



1 — a + 2a = i, 

 a = i — l. 



* Jones, Zeits. phys. Chem. xi. pp. 112, 536. 



