Chapter 5, Problem 127RQ

A solution containing 0.1244 g of ${\text{K}}_{\text{2}}{\text{C}}_{\text{2}}\text{O4}$ was acidified, changing the ${\text{C}}_{\text{2}}{\text{O}}_{\text{4}}{}^{\text{2-}}$ ions to ${\text{H}}_{\text{2}}{\text{C}}_{\text{2}}{\text{O}}_{\text{4}}$. The solution was then titrated with 13.93 mL of a ${\text{KMnO}}_{\text{4}}$ solution to reach a faint pink end point. In the reaction, ${\text{H}}_{\text{2}}{\text{C}}_{\text{2}}\text{O4}$ was oxidized to ${\text{CO}}_{\text{2}}$ and ${\text{MnO}}_4{}^{\text{-}}$ was reduced to ${\text{Mn}}^{\text{2+}}$. What was the molarity of the ${\text{KMnO}}_{\text{4}}$ solution used in the titration?