when CaF₂ dissolves, it dissociates as follows; CaF₂ --> Ca²⁺ + 2F⁻ If molar solubility of CaF₂ is x, then molar solubility of Ca²⁺ is x and F⁻ is 2x. ksp is solubility product constant and it can be calculated as follows; ksp = [Ca²⁺][F⁻]² ksp = (x)(2x)² ksp = 4x³ 4x³ = 1.5 x 10⁻¹⁰ x³ = 0.375 x 10⁻¹⁰ x = 3.3 x 10⁻⁴ M To calculate solubility in terms of g/L, we have to know the molar mass of CaF₂. Solubility of CaF₂ is 3.3 x 10⁻⁴ mol/L x 78 g/mol = 0.0257 g/L
