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The solubility of silver chromate in $0.01 \mathrm{M} \mathrm{K}_2 \mathrm{CrO}_4$ is $2 \times 10^{-8} \mathrm{~mol} \mathrm{dm}^{-3}$. The solubility product of silver chromate will be
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$16 \times 10^{-18}$
$K_{s p}=\left[\mathrm{Ag}^{+}\right]^2\left[\mathrm{CrO}_4^{2-}\right]=[2 S]^2[0.01]$
$=4 S^2[0.01]=4\left[2 \times 10^{-8}\right]^2 \times 0.01=16 \times 10^{-18}$
$=4 S^2[0.01]=4\left[2 \times 10^{-8}\right]^2 \times 0.01=16 \times 10^{-18}$
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