Solubility of silver chromate in 0.01 ,M {K₂}Cr{O₄} is 2 × {10^{ - 8}},mol,d{m^{ - 3}} . solubi

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6-2.Equilibrium-II (Ionic Equilibrium)

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The solubility of silver chromate in $0.01 \,M$ ${K_2}Cr{O_4}$ is $2 \times {10^{ - 8}}\,mol\,d{m^{ - 3}}$. The solubility product of silver chromate will be

A

$8 \times {10^{ - 24}}$

B

$16 \times {10^{ - 24}}$

C

$1.6 \times {10^{ - 18}}$

D

$16 \times {10^{ - 18}}$

Solution

(d) ${K_{sp}} = {[A{g^ + }]^2}[Cro_4^{ – \, – }] = {[2S]^2}[0.01]$

=$4{S^2}[0.01] = 4{[2 \times {10^{ – 8}}]^2} \times 0.01$$ = \,\,16 \times {10^{ – 18}}$ .

Standard 11

Chemistry

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