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
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 158IP: The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with...
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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 Fe. The net ionic equation for
the reaction is
5F22+ + MnO4+8H*
5FE3+ + Mn2- + 4H20
What was the percentage by mass of iron in the ore?
What was the percentage by mass of Fe3O in the ore?
Part 1
Calculate the number of moles of permanganate ion in the solution given.
moles MnO4
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Part 2
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