The solubility product (Ks p) of solid barium sulphate at 298 K is 1.1 × 10-10. The molar solubility, S of [ Ba 2+] and [ SO 42-] is

Question

The solubility product (Ks p) of solid barium sulphate at 298 K is 1.1 × 10-10. The molar solubility, S of [ Ba 2+] and [ SO 42-] is (A) 1.05 × 10-7 mol L -1 (B) 1.05 × 10-10 mol L -1 (C) 1.05 × 10-6 mol L -1 (D) 1.05 × 10-5 mol L -1

Tardigrade Admin · Accepted Answer

BaSO 4(s) leftharpoons sa 2+ undersets(a q)+S O42- undersets(a q) Ks p=S × S=S2 1.1 × 10-10=S2 S=1.05 × 10-5 mol L -1

Q. The solubility product $(K_{s p})$ of solid barium sulphate at $298 K$ is $1.1 \times 1 0^{- 10}$ . The molar solubility, $S$ of $[B a^{2 +}]$ and $[S O_{4}^{2 -}]$ is

$1.05 \times 1 0^{- 7} m o l L^{- 1}$

$1.05 \times 1 0^{- 10} m o l L^{- 1}$

$1.05 \times 1 0^{- 6} m o l L^{- 1}$

$1.05 \times 1 0^{- 5} m o l L^{- 1}$

$B a S O_{4} (s) ⇌ s a^{2 +} s (a q) + S O_{4}^{2 -} s (a q)$
$K_{s p} = S \times S = S^{2}$
$1.1 \times 1 0^{- 10} = S^{2}$
$S = 1.05 \times 1 0^{- 5} m o l L^{- 1}$

Q. The solubility product (Ksp​) of solid barium sulphate at 298K is 1.1×10−10. The molar solubility, S of [Ba2+] and [SO42−​] is

1.05×10−7molL−1

1.05×10−10molL−1

1.05×10−6molL−1

1.05×10−5molL−1