Calculate the molar solubility of Mg(OH)₂ in a solution with pH = 12.20.(K_sp (Mg(OH)₂ = 1.2 x 10^-11)

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The solubility product (Ksp) of Mg(OH)2 is given as 1.2 x 10^-11. The dissolution of Mg(OH)2 in water can be represented as: Mg(OH)2(s) ⇌ Mg2+(aq) + 2OH-(aq). The Ksp expression is Ksp = [Mg2+][OH-]^2. Given the pH is 12.20, we can find the pOH = 14 - 12.20 = 1.80. The concentration of OH- can be calculated using [OH-] = 10^-pOH = 10^-1.80 = 1.58 x 10^-2 M. Substituting this into the Ksp expression and solving for [Mg2+], we get 1.2 x 10^-11 = [Mg2+](1.58 x 10^-2)^2. Solving for [Mg2+] gives [Mg2+] = 4.8 x 10^-8 M, which is the molar solubility of Mg(OH)2 in the solution.

Calculate the Molar Solubility of Mg(OH)2 in a Solution with PH

Calculate the Molar Solubility of Mg(OH)₂ in a Solution with PH