with definit acidic and basic properties, it is not a t all strange that the heat of neutralization should vary considerably from solvent to solvent. Summary. I. Measurements of heats of reaction in non-aqueous solutions have been made and reported for the first time. 2. The amount of heat liberated for a given reaction in different solvents has been found to vary greatly from solvent to solvent. 3. These considerable differences cannot be explained as being due to any electrolytic dissociation of the acetate, nor are they due to differences in the heats of solution of the acetate in the different solvents. 4. The chemical nature of the solvents does not seein to give any clue as to the magnitude of the heat of neutralization in the cases investigated, nor of the magnitude or sign of the heat of solution of the resulting acetate. It is proposed to continue this line of work, using such other reactions as may be found available.
I~o', which is the boiling point of a solution having approximately the composition CaC12.6H20. The liquid was then transferred to a shallow tray where it solidified. This material is quite hard and we passed it through a grinder before use. In winter weather, when the laboratory air is dry, the material does not deliquesce in the open tray. LOG. d., pp. 591-592. I 106 I€. W. FOOTE AND BLAIR SAXTON. With none present, all three coincide in one straight line practically parallel with AB. This is the case, for instance, when a mixture of sand and water is frozen, and the first sample of alumina (Fig. I) approximates this condition. We have already shown that freezing and time both tend to diminish capillary water. Our present investigation has shown that heating a hydrogel with water affects capillary water more than either long standing or freezing and this effect has therefore received much attention. We have also determined the amounts of combined water in several samples prepared under other conditions, and have duplicated some of our previous determinations where this seemed desirable.
The solubilities of potassium perchlorate and potassium nitrate have been measured in the presence of several added salts in pure glacial acetic acid.The observed solubilities agree with those predicted by the interionic attraction theory if a sufficiently large ion diameter is assumed.An empirical relationship from which the value of the activity coefficient may be calculated has been pointed out.A somewhat better agreement is obtained with the extended theory of Gronwall, La Her and Sandved than with the original Debye-Htickel development.It is concluded that explanation of the properties of salt solutions requires that other properties of the solvent in addition to its dielectric constant must be considered.
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