Thermodynamics Research Center / ThermoML | Fluid Phase Equilibria

ABSTRACT

In this investigation, the thermodynamic properties of aqueous solutions Na, K or NH4 dihydrogenphosphate were determined at various temperatures ranging from 298.15 K to 353.15 K. The measurements of water activity were performed in the molality range from dilution to saturation using the hygrometric method. The modeling approach based on the ion interaction model was developed to determine the thermodynamic properties. From these measurements of phosphate salts, mixing parameters in binary solutions were evaluated at various temperatures, without considering formation of aqueous complexes. The osmotic and activity coefficients were determined for these aqueous solutions of orthophosphate salts. The measurements of the binary systems were combined with reference pure water, NaH2PO4(s), KH2PO4(s) and (NH4)H2PO4(s) solubility data to construct a chemical model that calculates solute and solvent activities from dilute to saturated solution concentration from 298.15 to 353.15 K respectively up to m_max(NaH2PO4(s)) = 7.90 to 18.29 mol kg-1; m_max(KH2PO4(s)) = 1.83 to 5.10 mol kg-1; and m_max((NH4)H2PO4(s)) = 4.93 to 12.62 mol kg-1. The thermodynamic characteristics, solubility products K_sp and the standard molar Gibbs energy of dissolution were also given.