The solubility of $$BaSO_{4}$$ in water is $$2.42 \times 10^{-3} gL^{-1}$$ at 298K. The value of its solubility product $$(K_{sp})$$ will be
(Given molar mass of $$BaSO_{4} = 233 g mol^{-1}$$

A

$$1.08 \times 10^{-8} mol^{2} L^{-2}$$

B

$$1.08 \times 10^{-14} mol^{2} L^{-2}$$

C

$$1.08 \times 10^{-12} mol^{2} L^{-2}$$

D

$$1.08 \times 10^{-10} mol^{2} L^{-2}$$