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Some Partial Pressures of Hydrogen Chloride 1189 potassium hydroxide in 50% aqueous ethyl alcohol. This extends the observations of Barnett and his co-workers to more drastic conditions.Two interpretations of this and similar facts are considered, that a Walden inversion must attend such a replacement reaction, or that a carbonium ion must be formed in which the central carbon atom and the three atoms directly combined with it lie in a common plane. The latter concept, advocated previously by Bartlett and Knox by analogy to boron compounds, is here correlated with the resonance normally present in an arylated carbonium ion. This interpre-tation is favored but not conclusively proved.The bromine can be replaced by hydrogen by means of reduction with sodium and alcohol. Maleic anhydride has been added to ethyl N-9*• anthrylcarbamate to yield a bridged-ring urethan (VII) which is readily hydrolyzed to the aminodibasic acid related to II. Nitrous acid converts this into a compound which is probably the dibasic acid with hydroxyl on the bridge-head. As expected by Barnett, this compound is very unstable to alkali. Its decomposition is interpreted as ketol cleavage. Cambridge, Massachusetts

the most frequently studied three-component systems are those consisting of water and two electrolytes having a common ion (1), it has seemed desirable to provide an experiment for the introductory physical chemistry course involving a system of this kind. Such an experiment not only illustrates the use of triangular coordinates, but also the indirect method employed in determining the composition of the solid phase (2). A study of the system, potassium chloride-hydrogen chloride-water, has been used and found suitable for this purpose. Since the solutions come to equilibrium quickly, and since they may be analyzed volumetrically, the amount of time consumed in the performance of the experiment is not excessive, a pair of students being able to obtain enough satisfactory data in from six to eight hours in the laboratory.The experimental procedure involves an adaptation of the usual method employed in physical chemistry

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This paper attempts to answer two questions concerning the hydrolysis of a salt derived from a weak acid and a weak base which are greatly emphasized by a treatment of salt hydrolysis in terms of the modern theory of acids and bases. The questions are:(1) To what are the values cited in the literature for the degree of hydrolysis of salts of this kind referred; and (2) should not the degree of hydrolysis be stated separately for each ion? It is shown that the degree of hydrolysis need not be determined separately for each ion except for very low salt concentrations; that it is possible to determine the degree of hydrolysis for the ions individually by methods employing measurements of hydronium-ion activities or of distribution ratios.The available data in the literature for the hydrolysis of salts derived from weak acids and bases at room temperatures is compiled.