Question

The solubility product (K_sp) of solid barium sulphate at 298 K is 1.1 × 10^-10. The molar solubility, S of \[\ce{Ba^{2+} and [SO^{2-}_4]}\] are ______.

Options

• 1.05 × 10^-7 mol L^-1

• 1.05 × 10^-10 mol L^-1

• 1.05 × 10^-6 mol L^-1

• 1.05 × 10^-5 mol L^-1

Answer 1

The solubility product (K_sp) of solid barium sulphate at 298 K is 1.1 × 10^-10. The molar solubility, S of \[\ce{Ba^{2+} and [SO^{2-}_4]}\] are 1.05 × 10^-5 mol L^-1.

Explanation:

\[\ce{BaSO4(s) <=> \underset{(S)}{Ba^{2+}(aq)} + \underset{(S)}{SO^{2-}_4 (aq)}}\]

K_sp = S × S = S²

1.1 × 10^-10 = S²

S = 1.05 × 10^-5 mol L^-1