What is the solubility of m (oh) 2 in a 0.202 m solution of m (no3) 2? ksp 4.45*10^-12?

M (NO ₃) ₂ fully separates into M ²⁺ and NO ₃ ²⁻ and M (OH) ₂ partially separates as M ²⁺ and 2OH ⁻

M (NO ₃) ₂ → M ²⁺ + 2NO ₃²⁻

0.202 M 0.202 M

M (OH) ₂ (s) ↔ M ²⁺ (aq) + 2OH ⁻ (aq)

I - -

C - X + X + 2X

E X 2X

Ksp = [M ²⁺ (aq) ] [OH ⁻ (aq) ] ²

4.45 * 10∧-12 = (0.202 + X) (2X) ²

Since X is very small, (0.202 + X) = 0.202

4.45 * 10 - 12 = 0.202 * 4X ²

X = 2.347 * 10∧-6 M

Hence the solubility of M (OH) 2 is 2.347 * 10∧-6 M