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Earlier studies of the dissociation constants of monoethanolammonium and diethanolammonium ions and the thermodynamic constants for the dissociation processes have been supplemented by a similar study of triethanolammonium ion from 0° to 50° C. The dissociation constant ( K bh  ) is given by the formula    -  logK   b  h    =  1341.16  /  T  +  4.6252  -  0.0045666  T    where T is in degrees Kelvin. The order of acidic strengths of the ions is as follows: Triethanolammonium &gt;diethanolammonium&gt;monethanolammonium. Conversely, monoethanolamine is the strongest of the three bases. The thermodynamic constants for the dissociation of one mole of triethanolammonium ion in the standard state at 25° C are as follows: Heat content change (Δ H °) 33.450 joule mole -1 ; entropy change (Δ S °), -36.4 joule deg -1 mole -1 ; heat-capacity change    (   Δ   C  p  °    )    , 52 joule deg -1 mole -1 .

Acid dissociation constant and related thermodynamic quantities for triethanolammonium ion in water from 0 to 50 C