Problem: Enter your answer in the provided box.A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe2+ in acid and then titrating the Fe 2+ with MnO4-.  A 1.4771-g sample was dissolved in acid and then titrated with 31.38 mL of 0.0194M KMnO4. The balanced equation is 8H+(aq) + 5Fe2+(aq) + MnO4-(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) Calculate the mass percent of iron in the ore. 

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A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe2+ in acid and then titrating the Fe 2+ with MnO4-.  A 1.4771-g sample was dissolved in acid and then titrated with 31.38 mL of 0.0194M KMnO4. The balanced equation is 

8H+(aq) + 5Fe2+(aq) + MnO4-(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) 

Calculate the mass percent of iron in the ore. 


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Based on our data, we think this problem is relevant for Professor Aken's class at GMU.