The solubility product (K_{ {sp}}) of solid barium sulphate at 298 {K} is 1.1 \times 10^{-10}. The molar solubility, S of [ {Ba}^{2+}] and [ {SO}_{4}^{2-}] is

Correct Answer is : 1.05×10−5molL−1

1.05 \times 10^{-7} {mol} {L}^{-1}

1.05 \times 10^{-10} {mol} {L}^{-1}

1.05 \times 10^{-6} {mol} {L}^{-1}

1.05 \times 10^{-5} {mol} {L}^{-1}

MHT CET 2021 Chemistry Solved Paper

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The solubility product (Ksp) of solid barium sulphate at 298K is 1.1×10−10. The molar solubility, S of [Ba2+] and [SO42−] is

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