A 1.362 g sample of an iron ore that contained FezOawas 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 Fe. The net ionic equation for the reaction is 5FE2+ + MnO+ 8H* 5F 3+ + Mn2 +4H20 What was the percentage by mass of iron in the ore? What was the percentage by mass of Fe30gin the ore? Part 1 X Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used
A 1.362 g sample of an iron ore that contained FezOawas 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 Fe. The net ionic equation for the reaction is 5FE2+ + MnO+ 8H* 5F 3+ + Mn2 +4H20 What was the percentage by mass of iron in the ore? What was the percentage by mass of Fe30gin the ore? Part 1 X Your answer is incorrect. Calculate the number of moles of permanganate ion in the solution given. moles MnO4 Attempts: 1 of 1 used
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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