The solubility of $BaSO_4$ in water is $2.42 \times 10^{-3} gL^{-1}$ at 298 K. The value of its solubility product $(K_{sp})$ will be <br> (Given molar mass of $BaSO_4 = 233 \; g\;mol^{-1}$ )

Question

( A ) $1.08 \times 10^{-10}\;mol^2 L^{-2}$
( B ) $1.08 \times 10^{-12}\;mol^2 L^{-2}$
( C ) $1.08 \times 10^{-8}\;mol^2 L^{-2}$
( D ) $1.08 \times 10^{-14}\;mol^2 L^{-2}$