Chemistry - Redox Reactions Question with Solution | TestHub

The reaction involves the oxidation of oxalate by $KMn{O}_4$ in acidic medium. The balanced equation helps determine the stoichiometry. The milliequivalents of $K_{x}H(C_2{O}_4{)}_y$ equals milliequivalents of $KMn{O}_4$. $10\times 0.2\times (2y)=8\times 0.2\times 5$. Solving for $y$, we get $y=2$. Since the compound is $K_{x}H(C_2{O}_4{)}_2$, the total negative charge is -4. Therefore, $x+1=4$, so $x=3$.