$0.0100$ mol of $\mathrm{FeC}{}_2\mathrm{O}{}_4$ is dissolved in dilute $\mathrm{H}{}_2\mathrm{SO}{}_4$. Consider titration with $0.0200\mathrm{M}$ $\mathrm{KMnO}{}_4$ (oxidises both $\mathrm{Fe}{}^{2+}$ and oxalate completely) and with $0.0200\mathrm{M}$ $\mathrm{K}{}_2\mathrm{Cr}{}_2\mathrm{O}{}_7$ (assume it oxidises only $\mathrm{Fe}{}^{2+}$). Which statements are correct?

1. AThe oxalate part consumes two-thirds of the total $\mathrm{KMnO}{}_4$ volume.
2. BThe $\mathrm{K}{}_2\mathrm{Cr}{}_2\mathrm{O}{}_7$ solution needed for the $\mathrm{Fe}{}^{2+}$ present is $83.3\mathrm{mL}$.
3. CComplete oxidation requires $300\mathrm{mL}$ of the $\mathrm{KMnO}{}_4$ solution.
4. DThe $\mathrm{Fe}{}^{2+}$ part alone consumes $200\mathrm{mL}$ of the $\mathrm{KMnO}{}_4$ solution.