A 0.5962 g sample of iron ore is dissolved in perchloric acid (HClO4 ). All iron present is oxidized to Fe3+ . The solution is filtered to remove solid matrix materials and made basic with addition of ammonium hydroxide. The iron precipitates as the Fe(OH)3 • x H2O gel. The precipitate is collected in a cistern crucible and ignited to produce Fe2O3 . What is the percent by weight of iron in the sample if the analysis produced 0.3210 g Fe2O3?
A 0.5962 g sample of iron ore is dissolved in perchloric acid (HClO4 ). All iron present is oxidized to Fe3+ . The solution is filtered to remove solid matrix materials and made basic with addition of ammonium hydroxide. The iron precipitates as the Fe(OH)3 • x H2O gel. The precipitate is collected in a cistern crucible and ignited to produce Fe2O3 . What is the percent by weight of iron in the sample if the analysis produced 0.3210 g 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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6. A 0.5962 g sample of iron ore is dissolved in perchloric acid (HClO4 ). All iron present is oxidized to Fe3+ . The solution is filtered to remove solid matrix materials and made basic with addition of ammonium hydroxide. The iron precipitates as the Fe(OH)3 • x H2O gel. The precipitate is collected in a cistern crucible and ignited to produce Fe2O3 . What is the percent by weight of iron in the sample if the analysis produced 0.3210 g Fe2O3?
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