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Concentration of the $Ag^+$ ions in a saturated solution of $Ag_2C_2O_4$ is $2.2 \times 10^{-4}\ mol\ L^{-1}$. Solubility product of $Ag_2C_2O_4$ is
Explanation
$[C_2O_4^{2-}] = [Ag^+]/2$; $K_{sp} = [Ag^+]^2[C_2O_4^{2-}]$.
Detailed Solution
$Ag_2C_2O_4(s) \rightleftharpoons 2Ag^+(aq) + C_2O_4^{2-}(aq)$, with concentrations 2s and s
$K_{SP} = [Ag^+]^2[C_2O_4^{2-}]$
$[Ag^+] = 2.2\times10^{-4}$ M
$\therefore [C_2O_4^{2-}] = \frac{2.2\times10^{-4}}{2}$ M $= 1.1\times10^{-4}$ M
$\therefore K_{SP} = (2.2\times10^{-4})^2(1.1\times10^{-4}) = 5.324\times10^{-12}$