Chapter 16, Problem 33CI

Consider the reaction of sodium oxalate $\left({\text{Na}}_2{\text{C}}_2{\text{O}}_4\right)$ and potassium permanganate $\left({\text{KMnO}}_4\right)$ in acidic solution. The unbalanced equation is the following: $(9.2,9.3,12.4,$ , $12.5,15.2)$

${\text{MnO}}_4^{-}(aq)+{\text{C}}_2{\text{O}}_4^{2-}(aq)\to {\text{Mn}}^{2+}(aq)+{\text{CO}}_2(g)$

In an oxidation-reduction titration, the ${\text{KMnO}}_4$ from the buret reacts with ${\text{Na}}_2{\text{C}}_2{\text{O}}_4$

a. What is the balanced oxidation half-reaction?
b. What is the balanced reduction half-reaction?
c. What is the balanced ionic equation for the reaction?
d. If $24.6 \text{mL}$ of a ${\text{KMnO}}_4$ solution is needed to titrate a solution containing $0.758 \text{g}$ of sodium oxalate $\left({\text{Na}}_2{\text{C}}_2{\text{O}}_4\right)$ , what is the molarity of the ${\text{KMnO}}_4$ solution?