An iron ore sample which weighs 1.097 g is dissolved, the iron reduced to Fe*2, and the resulting solution titrated with 0.0210 M , 37.63 ml standard KMNO4 solution. The reaction is: 2KMNO4+10FESO4 +8H2SO4 = 2MNSO4 +K2SO4 +10CO2 + 5Fe2(SO4)3 + 8H2O Compute the percentage of iron as Fe2O3.

An iron ore sample which weighs 1.097 g is dissolved, the iron reduced to Fe*2, and the resulting solution titrated with 0.0210 M , 37.63 ml standard KMNO4 solution. The reaction is: 2KMNO4+10FESO4 +8H2SO4 = 2MNSO4 +K2SO4 +10CO2 + 5Fe2(SO4)3 + 8H2O Compute the percentage of iron as Fe2O3.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter19: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 11E: Iron (II) can be oxidized to iron (III) by dichromate ion, which is reduced to chromium (III) in...

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Question

Q2) An iron ore sample which weighs 1.097 g is dissolved, the iron reduced to Fe*2, and the
resulting solution titrated with 0.0210 M , 37.63 ml standard KMNO4 solution. The reaction
is:
2KMNO4+10FeSO4 +8H2SO4 2MNSO4 +K2SO4 +10CO2 + 5FE2(SO4)3 + 8H2O
Compute the percentage of iron as Fe2O3.

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