The titration represented by the reaction below required $55\mathrm{.}0$ mL of $0\mathrm{.}100$ mol$/$L KMnO$4($aq$)$ to react completely with the Fe$2+($aq$).$ The mass of iron in the ore sample wasAn iron ore sample was crushed and treated in order to convert all the iron to

$F{e}^{2+}(aq).$ This solution was then titrated with $KMn{O}_{4(aq)}.$ The unbalanced redox

equation for the reaction is

$Mn{O}_4^{-}{?}_{(aq)}+H_{(aq)}^{+}+F{e}_{(aq)}^{2+}M{n}_{(aq)}^{2+}+H_2{O}_{(l)}+F{e}_{(aq)}^{3+}$