The iron (II) in an acidified solution is titrated with 0.0317M solution of KMnO4: 5Fe2+ +MnO4- +8H → 5 Fe3+ +Mn2+ + 4H2O If the titration required 51.3 ml, how many mg of iron ore are in the solution?
The iron (II) in an acidified solution is titrated with 0.0317M solution of KMnO4: 5Fe2+ +MnO4- +8H → 5 Fe3+ +Mn2+ + 4H2O If the titration required 51.3 ml, how many mg of iron ore are in the solution?
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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The iron (II) in an acidified solution is titrated with 0.0317M solution of KMnO4:
5Fe2+ +MnO4- +8H → 5 Fe3+ +Mn2+ + 4H2O
If the titration required 51.3 ml, how many mg of iron ore are in the solution?
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