Question

The solubility product of $BaSO_{4}$ at $25^\circ C$ is $1.0\times 10^{- 9}$ what would be the concentration of $H_{2}SO_{4}$ to precipitate $BaSO_{4}$ from a solution of $0.01MBa^{2 +}$ ions ?

• A. $10^{- 9}M$
• B. $10^{- 8}M$
• C. $10^{- 6}M$
• D. $10^{- 10}M$

Answer 1

Answer: (C)

$BaSO_{4}\rightleftharpoonsBa^{+ 2}+SO_{4}^{- 2}$
$I.P>K_{sp}$ for precipitation
$\left[Ba^{+ 2}\right]\left[SO_{4}^{- 2}\right]>K_{sp}$
$\left(0 . 01\right)\left(SO_{4}^{- 2}\right)>\left(10\right)^{- 9}$
$\left(SO_{4}^{- 2}\right)>\left(10\right)^{- 7}$
$10^{- 6}$