The metal content of iron in ores can be determined by a redox procedure in which the sample is first oxidized with Br2Br2 to convert all the iron to Fe3+Fe3+ and then titrated with Sn2+Sn2+ to reduce the Fe3+Fe3+ to Fe2+Fe2+. The balanced equation is 2Fe3+(aq)+Sn2+(aq)→2Fe2+(aq)+Sn4+(aq)   What is the mass percent FeFe in a 0.1840 gg sample if 13.52 mLmL of a 0.1015 MM Sn2+Sn2+ solution is needed to titrate the Fe3+Fe3+?

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The metal content of iron in ores can be determined by a redox procedure in which the sample is first oxidized with Br2Br2 to convert all the iron to Fe3+Fe3+ and then titrated with Sn2+Sn2+ to reduce the Fe3+Fe3+ to Fe2+Fe2+. The balanced equation is
2Fe3+(aq)+Sn2+(aq)→2Fe2+(aq)+Sn4+(aq)

 

What is the mass percent FeFe in a 0.1840 gg sample if 13.52 mLmL of a 0.1015 MM Sn2+Sn2+ solution is needed to titrate the Fe3+Fe3+?

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