The solubility of magnesium fluoride is 1.17 × 10^-3 M.Find the value of K_sp for this compound. A)1.17 × 10^-3 B)(1.17 × 10^-3)² C)4(1.17 × 10^-3)³ D)(1.17 × 10^-3)³ E)3(1.17 × 10^-3)³

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Quizplus · Accepted Answer

The solubility product (Ksp) for magnesium fluoride (MgF2) can be calculated using the formula Ksp = [Mg2+][F-]^2, where [Mg2+] is the concentration of magnesium ions and [F-] is the concentration of fluoride ions in a saturated solution. Given the solubility of magnesium fluoride is 1.17 × 10^-3 M, the concentration of Mg2+ ions is 1.17 × 10^-3 M, and the concentration of F- ions is 2(1.17 × 10^-3 M) due to the 1:2 stoichiometry of MgF2. Therefore, Ksp = (1.17 × 10^-3)^1(2 × 1.17 × 10^-3)^2 = 4(1.17 × 10^-3)^3.

The Solubility of Magnesium Fluoride Is 1