Chapter 4, Problem 4.146MP

Iron content in ores can be determined by a redox procedure in which the sample is first reduced with ${\text{Sn}}^{\text{2}+}$ , as in Problem4.130, and then titrated with ${\text{KmO}}_{\text{4}}$ to oxidize the ${\text{Fe}}^{\text{2}+}$ to ${\text{Fe}}^{\text{3}+}$ . The balanced equation is
${\text{MnO}}_4{}^{-}\left(aq\right)+5{\text{Fe}}^{2+}\left(aq\right)+8{\text{H}}^{+}\left(aq\right)\to {\text{Mn}}^{2+}\left(aq\right)+5{\text{Fe}}^{3+}\left(aq\right)+4{\text{H}}_{\text{2}}\text{O}\left(l\right)$
What is the mass percent Fe in a 2.368 g sample if 48.39 mLof a $0.{\text{1116 M KMnO}}_{\text{4}}$ solution is needed to titrate the ${\text{Fe}}^{\text{3}+}$ ?