The interaction between NaCl-KCl salt of an equimolar composition and CaF2 was investigated in the 1023-1123 K temperature range. The solubility limit was determined as 2.1, 2.5, and 3.4 mol.% for 1023, 1073, and 1123 K, respectively. The linear dependence of the specific weight loss with time and the activation energy of the dissolution (124.6 +/- A 8.7 kJ/mol) indicate that CaF2 dissociation of the ions is the limiting stage of the process. Thermodynamic properties (partial enthalpy and entropy) of CaF2 in a dilute ternary -NaCl-KCl-CaF2 liquid solution were estimated using the values of the solubility limit and by applying a regular solution approach.