Abstract
Using Solvent Evaporating and Atomic Emission Spectrophotometric methods, the solubility of NaF in water at 25 °C was determined. Comparing the value of the thermodynamic solubility product constant, K sp(th), ( K sp(th) = exp(− Δ G diss° / RT)) of NaF to the value which is obtained from the observed solubility, s/mol L −1 , and activity coefficients, f + and f −, which are estimated upon the extended Debye–Hückel law, K sp′ = [Na +][F −] f + f −, revealed a great difference. The difference has satisfactorily been explained using a combination of Debye–Hückel law and Ion-Association Theory.
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