The solubility of BaSO4BaSO_4BaSO4 in water is 2.42×10−3 gL−12.42 \times 10^{-3} \text{ gL}^{-1}2.42×10−3 gL−1 at 298 K. The value of its solubility product (KspK_{sp}Ksp) will be (Given molar mass of BaSO4=233 g mol−1BaSO_4 = 233 \text{ g mol}^{-1}BaSO4=233 g mol−1)
1.08×10−14 mol2L−21.08 \times 10^{-14} \text{ mol}^2 \text{L}^{-2}1.08×10−14 mol2L−2
1.08×10−12 mol2L−21.08 \times 10^{-12} \text{ mol}^2 \text{L}^{-2}1.08×10−12 mol2L−2
1.08×10−10 mol2L−21.08 \times 10^{-10} \text{ mol}^2 \text{L}^{-2}1.08×10−10 mol2L−2
1.08×10−8 mol2L−21.08 \times 10^{-8} \text{ mol}^2 \text{L}^{-2}1.08×10−8 mol2L−2
Solubility of BaSO4BaSO_4BaSO4, s=2.42×10−3233 (mol L−1)=1.04×10−5 (mol L−1)s = \frac{2.42 \times 10^{-3}}{233} \text{ (mol L}^{-1}) = 1.04 \times 10^{-5} \text{ (mol L}^{-1})s=2332.42×10−3 (mol L−1)=1.04×10−5 (mol L−1). BaSO4(s)⇌Ba2+(aq)+SO42−(aq)BaSO_4(s) \rightleftharpoons Ba^{2+}(aq) + SO_4^{2-}(aq)BaSO4(s)⇌Ba2+(aq)+SO42−(aq). Ksp=[Ba2+][SO42−]=s2=(1.04×10−5)2=1.08×10−10 mol2L−2K_{sp} = [Ba^{2+}][SO_4^{2-}] = s^2 = (1.04 \times 10^{-5})^2 = 1.08 \times 10^{-10} \text{ mol}^2 \text{L}^{-2}Ksp=[Ba2+][SO42−]=s2=(1.04×10−5)2=1.08×10−10 mol2L−2.
Join thousands of students and practice with AI-generated mock tests.