Question

The solubility product of $BaS{O}_4$ is $1.5\times {10}^{-9}$. The precipitation in a $0.01M$ $B{a}^{2+}$ ions solution will start on adding $H_{2}S{O}_4$ of concentration -

• A. 10-9 M
• B.
• C. 1.5 x 10-7
• D. 10-6 M

Answer 1

The correct option is C

1.5 x 10-7

$\left[B{a}^{2+}\right]\left[S{O}_4^{2-}\right]$

= $1.5\times {10}^{-9}$ $\left(K_{sp}\right)$ and $\left[B{a}^{2+}\right]$ = $0.01M$

So required $\left[S{O}_4^{2-}\right]$ =$\frac{1.5\times {10}^{-9}}{0.01}$

= $1.5\times {10}^{-7}$

So $\left[H_{2}S{O}_4\right]>1.5\times {10}^{-7}$

for precipitation of $BaS{O}_4$