(Solved): A solution of permanganate is standardized by titration with oxalic acid (H2C2O4). It req ...

A solution of permanganate is standardized by titration with oxalic acid $\left({\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4\right)$. It required $34.54\mathrm{mL}$ of the permanganate solution to react completely with $0.5999\mathrm{g}$ of oxalic acid. The unbalanced equation for the reaction is ${\mathrm{MnO}}_4^{?}(aq)+{\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4(aq)\stackrel{\text{ Acidic }}{?}{\mathrm{Mn}}^{2+}(aq)+{\mathrm{CO}}_2(g)$ What is the molarity of the permanganate solution? $\text{ Molarity }=?M$ The vanadium in a sample of ore is converted to ${\mathrm{VO}}^{2+}$. The ${\mathrm{VO}}^{2+}$ ion is subsequently titrated with ${\mathrm{MnO}}_4{}^{?}$in acidic solution to form $\mathrm{V}(\mathrm{OH}{)}_4{}^{+}$and manganese(II) ion. To titrate the solution, $28.74\mathrm{mL}$ of $0.07240\mathrm{M}{\mathrm{MnO}}_4{}^{?}$was required. If the mass percent of vanadium in the ore was $65.1\%$, what was the mass of the ore sample? Mass $=$ $\mathrm{g}$