Question

The solubility of silver sulphate is 1.85 x 10^-2 mol dm^-3. Calculate solubility product of silver sulphate.

Answer 1

\[\ce{AgSO4(s) <=> 2Ag+(aq) + SO^2-_4(aq)}\]

\[\ce{k_{sp} = [Ag^+]^2 [SO^2-_4]}\]

If S is solubility, \[\ce{[Ag^+] = 2S and [SO^2-_4] = S}\]

K_s = (2S)² × S = 4S³

∴ K_s = 4 × (1.85 × 10 ^-2)³ = 2.53 × 10^-5