A chemical engineer determines the mass percent of iron in an ore sample by converting the $Fe$ to $F{e}^{2+}$ in acid and then titrating the $F{e}^{2+}$ with $Mn{O}_4^{-}.$ A $1\mathrm{.}2188-g$ sample was dissolved in acid and then titrated with $33\mathrm{.}71mL$ of $0\mathrm{.}04327MKMn{O}_4.$ The balanced equation is

$8H^{+}(aq)+5F{e}^{2+}(aq)+Mn{O}_4^{-}(aq)5F{e}^{3+}(aq)+M{n}^{2+}(aq)+4H_{2}O(l)$

Calculate the mass percent of iron in the ore. Be sure your answer has the correct number of significant figures.