Posted by **Meso** on Sunday, May 22, 2011 at 1:55pm.

Suppose 22.93mL of KMnO4 solution used in the question above (KMnO4 solution in above question 36.00mL and concentration of 0.02036M)are needed to oxidize Fe(2+) to Fe(3+) in a 0.4927g pill. What is the mass percent of FeSO4 (dot) 7H2O (molar mass 278.03g/mol) in the pill?

What I would do is take the concentration of KMnO4 and then using the 22.93mL find the mols and then divide the 0.4927g by them. This gives me the molar mass of the pill. Then i find the percent by dividing the molar mass of FeSO4 (dot) H2O by the pill molar mass to find the percent. Is that correct?

Thank you :)

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