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a sample of iron ore (m=0,330g)consisting of a mixture of FeO and Fe2O3 was dissolved in...

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Chemistry

a sample of iron ore (m=0,330g)consisting of a mixture of FeOand Fe2O3 was dissolved in dilute sulfuric acid and titrated with apotassium permanganate solution containing 0.0200g of KMnO4 perlitre, and required 20,3 mL for complete reaction. The secondsample of iron ore (m=0,370g)was dissolved in dilute sulfuric acidsolution and fe3+ is reduced to fe2+ then titrated with the samepotassium permanganate solution. 42,6mL was required for the secondtitration. Calculate the mass of each iron oxide in the originalsample.
im not sure about chemical reactions because Fe2o3 is not reactingwith KMno4

Answer & Explanation Solved by verified expert
3.7 Ratings (620 Votes)
Ans Part A Concentration of KMnO4 solution Number of moles of KMnO4 solution in 00200 g sample mass molar mass 00200 g 15809 g mol1 12651 x 104 moles Molarity number of moles of solute liter of solution Since 0020 g 12651 x 104 moles dissolved in 1 L Molarity of KMnO4 solution 12651 x    See Answer
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