Milk of Magnesia is actually a suspension (that's why instructions often mention shaking before use) of solid Mg(OH)2. 1.00 liter of solution of 0.055 moles of Mg2+ is held at a pH of 7.00. Would a precipitate form? If so, what fraction of the original 0.055 molar Mg2+ would precipitate at that pH? Ksp = 5.61 x10-12
Mg(OH)2 (s) → Mg2+ (aq) + 2 OH- (aq)
(B) At pH = 10.00, would there be precipitation? If so, what fraction of the original 0.055 M Mg2+ precipitate?