Abstract
The solubility of a zwitterionic compound has been determined as a function of pH and temperature. The data were used to determine the pK a, intrinsic solubility of the uncharged species and the thermodynamic quantities ΔG, ΔH, ΔS and ΔCp as a function of temperature. It was found that with an increase in temperature from 4°C to 45°C, pKa 1 decreased from 3.42 to 3.19 while pKa 2 decreased from 10.20 to 9.29. Over this same increase in temperature, the intrinsic solubility of the uncharged species increased from 1.28 to 3.40 mg ml . The thermodynamic quantities calculated were consistent with values found in the literature for similar compounds where ΔH for the equilibria are endothermic and the ΔS values indicate an increase in solution structure with dissociation. The intrinsic solubility of the uncharged species was found to decrease with the introduction of NaCl to the solution. This decrease is consistent with reported solubility effects of electrolytes upon non-electrolytes.
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