Chapter 5, Problem 129RQ

A 15.00 mL sample of a solution containing oxalic acid, ${\text{H}}_{\text{2}}{\text{C}}_{\text{2}}{\text{O}}_{\text{4}}$, was titrated with $0.02000M{\text{ KMnO}}_{\text{4}}$. The titration required 18.30 mL of the ${\text{KMnO}}_{\text{4}}$ solution. If 19.69 mL of a solution of $\text{NaOH}$ is needed to react completely with 25.00 mL of this same oxalic acid solution, what is the concentration of the $\text{NaOH}$ solution? In the reaction, oxalate ion $\left({\text{C2O}}_4^{2-}\right)$ is oxidized to ${\text{CO}}_{\text{2}}$ and ${\text{MnO}}_4^{-}$ is reduced to ${\text{Mn}}^{\text{2+}}$.