Abstract
The dissociation constants, pKa, of monoethanolamine (MEA), N-methyldiethanolamine (MDEA), 2-amino-2-methyl-1-propanol (AMP), 2(2-aminoethyl)etanolamine (AEEA), and piperazine (Pz) were measured by potentiometric titration over the temperature range (298.15 to 363.15)K. Enthalpies of protonation, ΔHp, were measured calorimetrically at temperatures from (298.15 to 393.15)K for MEA, MDEA, and AMP, and from (298.15 to 353.15)K for AEEA and Pz. In addition, the effect of the ionic strength of the solutions on the protonation of MDEA was studied using NaCl as background salt {(0 to 5.5)mol/kg-H2O)}. Correlations for the reaction equilibrium constants for proton dissociation are proposed for the studied amines based on the experimental data from literature and from this work. Both experimental enthalpy data and dissociation constants were used for fitting. The results from this work may be used for thermodynamic modeling of CO2 capture processes using amines.
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