A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7. The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the iron in the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,it required 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Show your solution why 77.86% is the iron content of the ore as %w/w Fe2O3.
A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7. The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the iron in the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,it required 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Show your solution why 77.86% is the iron content of the ore as %w/w 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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A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.
The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the iron
in the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,it
required 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Show your solution why 77.86% is the iron content of the ore as %w/w Fe2O3.
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