Q.The solubility of $BaSO_4$ in water is $2.42 \times 10^{-3} \text{ g/L}$ at $298 \text{ K}$ . The value of its solubility product ( $K_{sp}$ ) is: (Molar mass of $BaSO_4 = 233 \text{ g/mol}$ )

1.08 \times 10^{-10}

1.08 \times 10^{-14}

1.04 \times 10^{-5}

2.42 \times 10^{-3}

The correct solution involves applying the fundamental concept to derive the final value step by step...

Already a member? Login here

Q.The solubility of BaSO4BaSO_4BaSO4​ in water is 2.42×10−3 g/L2.42 \times 10^{-3} \text{ g/L}2.42×10−3 g/L at 298 K298 \text{ K}298 K. The value of its solubility product (KspK_{sp}Ksp​) is: (Molar mass of BaSO4=233 g/molBaSO_4 = 233 \text{ g/mol}BaSO4​=233 g/mol)