Solubility product of BaS{O₄} is 1.5 × {10^{ - 9}}. precipitation in a 0.01 ,M,,B{a^{2 + }} solut

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6-2.Equilibrium-II (Ionic Equilibrium)

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The solubility product of $BaS{O_4}$ is $1.5 \times {10^{ - 9}}.$ The precipitation in a $0.01 \,M\,\,B{a^{2 + }}$solution will start, on adding ${H_2}S{O_4}$ of concentration

A

${10^{ - 9}}\,M$

B

${10^{ - 8}}\,M$

C

${10^{ - 7}}\,M$

D

${10^{ - 6}}\,M$

Solution

(c) ${K_{sp}}$ of $BaS{O_4} = 1.5 \times {10^{ – 9}}$;

$B{a^{ + + }} = 0.01\,M$

$SO_4^{ – \, – } = \frac{{1.5 \times {{10}^{ – 9}}}}{{0.01}} = 1.5 \times {10^{ – 7}}$

Standard 11

Chemistry

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