A 1.362 g sample of an iron ore that contained Fe304was 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* + MnO4 + 8H* 5FE3+ + Mn2* + 4H20 What was the percentage by mass of iron in the ore? What was the percentage by mass of Fe304in the ore?

A 1.362 g sample of an iron ore that contained Fe304was 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* + MnO4 + 8H* 5FE3+ + Mn2* + 4H20 What was the percentage by mass of iron in the ore? What was the percentage by mass of Fe304in the ore?

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 50QAP

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