Chemistry - Ionic Equilibrium Question with Solution | TestHub

A specialized laboratory buffer is strictly maintained at a pH of 5.0 . To this buffer, an excess of the sparingly soluble solid silver oxalate. ${\mathrm{Ag}}_2{\mathrm{C}}_2{\mathrm{O}}_4(\mathrm{s})$, is added. The solubility product of silver oxalate is ${\mathrm{K}}_{\mathrm{sp}}=1.6\times 10^{-8}$. ${\mathrm{C}}_2{\mathrm{O}}_4^{-2}$ produced further convert in oxalic acid by suitable equilibriums. Oxalic acid $\left({\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4\right)$, a weak diprotic acid have dissociation constants ${\mathrm{K}}_{{\mathrm{a}}_1}=1.0\times 10^{-2}$ and ${\mathrm{K}}_{{\mathrm{a}}_2}=1.0\times 10^{-5}$. If the molar solubility of ${\mathrm{Ag}}_2{\mathrm{C}}_2{\mathrm{O}}_4$ in this buffer is found to be exactly $\mathrm{x}\times 10^{-3}\mathrm{M}$. Calculate the integer value of x .