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Abstract
The dependence on temperature of acid dissociation constants in water are examined for four systems. The final equation is based on a two-stage dissociation where the enthalpy terms are assumed to be independent of temperature. The relatively small overall enthalpy change for dissociation is shown to be a consequence of the enthalpy changes for the individual stages. The dependence of the overall heat-capacity quantity on temperature is marked, showing a minimum at a characteristic temperature. For acetic acid, the calculated dependence is in qualitative agreement with calorimetric data.
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Schedule a callMore From: Journal of the Chemical Society, Faraday Transactions 1: Physical Chemistry in Condensed Phases
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