A 1.362 g sample of an iron ore that contained FegO4was dissolved in acid and all of the iron was reduced to Fe2*. The solution was then acidified with H2SO4and titrated with 39.42 mL of 0.0281 M KMNO4, which oxidized the iron to Fet. The net ionic equation for the reaction is 5FE2+ + MnO4 +8H* 5FE3+ + Mn2+ + 4H2O What was the percentage by mass of iron in the ore? What was the percentage by mass of FegO4in the ore? Part 1 * Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used Part 2 Using the previous answer and the balanced equation, find the number of moles of Fe2+. mol Fe2+

A 1.362 g sample of an iron ore that contained FegO4was dissolved in acid and all of the iron was reduced to Fe2. The solution was then acidified with H2SO4and titrated with 39.42 mL of 0.0281 M KMNO4, which oxidized the iron to Fet. The net ionic equation for the reaction is 5FE2+ + MnO4 +8H 5FE3+ + Mn2+ + 4H2O What was the percentage by mass of iron in the ore? What was the percentage by mass of FegO4in the ore? Part 1 * Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used Part 2 Using the previous answer and the balanced equation, find the number of moles of Fe2+. mol Fe2+

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 74QAP: A solution contains both iron(II) and iron(III) ions. A sample Of the solution is titrated with 35.0...

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