Question

The solubility of $BaS{O}_4$ in pure water $\left(ing{L}^{-1}\right)$ is closest to [Given : $K_{sp}forBaS{O}_{4}is1.0\times {10}^{–10}at{25}^{o}C.$ Molecular weight of $BaS{O}_{4}is233gmo{l}^{–1}$]

• A. $1.0\times {10}^{–5}$
• B. $1.0\times {10}^{–3}$
• C. $2.3\times {10}^{–5}$
• D. $2.3\times {10}^{–3}$

Answer 1

The correct option is D $2.3\times {10}^{–3}$

$BaS{O}_4\to B{a}^{2+}+S{O}_4^{2-}$
s
- s s
$K_{sp}\left(BaS{O}_4\right)=\left[B{a}^{2+}\right]\left[S{O}_4^{2-}\right]$
$K_{sp}\left(BaS{O}_4\right)=s^2$
$s=\sqrt{K_{sp}}=\sqrt{1\times {10}^{-10}}={10}^{–5}mol{L}^{-1}$
$Solubility\left(s\right)={10}^{–5}\times molecularmass={10}^{–5}mol{L}^{-1}\times 233gmo{l}^{–1}=2.33\times {10}^{–3}g{L}^{–1}$