Calculate the molar solubility of CaF₂ in a 0.25 M solution of NaF(aq). (K_sp (CaF₂) = 4.0 x 10^-11)

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The correct answer is B because the molar solubility of CaF2 in a 0.25 M solution of NaF(aq) is 6.4 x 10-10 M. This can be calculated using the Ksp expression for CaF2, which is Ksp = [Ca2+][F-]2. Since NaF is a common ion, the [F-] concentration in the solution is 0.25 M. Substituting this value into the Ksp expression, we get Ksp = [Ca2+][0.25 M]2 = 4.0 x 10-11. Solving for [Ca2+], we get [Ca2+] = 6.4 x 10-10 M. Since the molar solubility of CaF2 is equal to the concentration of Ca2+ in the solution, the molar solubility of CaF2 is 6.4 x 10-10 M.

Calculate the Molar Solubility of CaF2 in a 0

Calculate the Molar Solubility of CaF₂ in a 0