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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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