Calculate the molar solubility of magnesium fluoride (K_sp = 6.9 × 10^-9)in a solution that also 0.010 M NaF.

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The presence of NaF in the solution will decrease the solubility of MgF2 due to the common ion effect. The molar solubility of MgF2 in a solution that also contains 0.010 M NaF can be calculated using the following expression:Ksp = [Mg2+][F-]^26.9 × 10^-9 = [Mg2+][0.010 + 2x]^2[Mg2+] = 6.9 × 10^-9 / (0.010 + 2x)^2Assuming x is small compared to 0.010, we can simplify the expression to:[Mg2+] = 6.9 × 10^-9 / (0.010)^2[Mg2+] = 6.9 × 10^-5 MTherefore, the molar solubility of MgF2 in a solution that also contains 0.010 M NaF is 6.9 × 10^-5 M.

Calculate the Molar Solubility of Magnesium Fluoride (Ksp = 6

Calculate the Molar Solubility of Magnesium Fluoride (K_sp = 6