Abstract
The crystal structure of 1-decylammonium hydrobromide was determined by X-ray crystallography. Lattice potential energy and molar volumes of the solid compound and its cation were obtained respectively. The ionic radius of the cation can be calculated from the corresponding effective volume of the cation. The molar enthalpies of dissolution of the compound at different concentrations m/(mol·kg−1) at T=298.15K were measured by an isoperibol solution-reaction calorimeter at T=298.15K. According to the Pitzer’s electrolyte solution theory, the molar enthalpy of dissolution of the compound at infinite dilution (ΔsHm∞) and Pitzer parameters (βMX(0)L and βMX(1)L) were obtained. The values of apparent relative molar enthalpies (ΦL) of the title compound and relative partial molar enthalpies (L2¯ and L1¯) of the solute and the solvent at different concentrations were derived from the experimental values of the enthalpy of dissolution of the compound. Finally, hydration enthalpies of the compound and its cation were calculated by designing a thermochemical cycle in accordance with lattice potential energy and the molar enthalpy of dissolution of the title compound at infinite dilution.
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