TWf! nty-three butTer solu tions composed of approximately eCJual molal amounts of monoethanolamine (2-aminoethanol) and monoethanolammoniurn chloride ill water were studied by electromotive-force methods at 11 temperatures from 0° to 50° C. The values obtained for the acid ic dissociation constant, K bh , of the ethanolammonium ion are given in this range of temperatures by -log K bh = 2677.91/T + 0.3869 + 0.0004277T, where T is the temperature on t he K elvin scale.The changes of free energy, heat content, entropy, and heat capacity that accompany the dissociation of 1 mole of ethanolamm.oniumion in the standard state were calculated from the dissociation constant and its tem perature coefficient.Dissociation of a mol e of ethanolammonium ion resu lts in a small decrease of h eat capacity.In this r espect ethanolammonium ion resembles ammonium ion rathe r than the methyl-substitu ted ammonium ions, for which rather large increases of heat capacity on di ssociation have been found.
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Bates et al. (1951) studied this question.