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Q.
At $25^{\circ}C$, if the concentration of $Ag^+$ ion is $1.5 \times 10^{-4}$ mol/L in the saturated solution of $Ag_2CrO_4$, then solubility product of $Ag_2CrO_4$ is
Solution:
$AgCro_{4}\left(s\right) {\rightleftharpoons}2Ag^{+}\left(aq\right)+CrO_{4}^{2-}\left(aq\right)$
In the saturated solution of $Ag_{2}CrO_{4}$
$[Ag^{+}]=1.5\times10^{-4}\,mol/L$
$\left[CrO_{4}^{2-}\right]=\frac{1.5\times10^{-4}}{2}=0.75\times10^{-4}$ mol/L
$K_{sp}=\left[Ag^{+}\right]\left[CrO_{4}^{2-}\right]=\left(1.5\times10^{-4}\right)^{2}\times0.75\times10^{-4}$
$=1.69\times10^{-12} mol^{3}L^{3}$