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Jack was asked to determine iron (55.845 g/mol) content in dietary supplement. He took few random tablets and ground them into fine powder. Next, he weighed 3.116 g of the fine powder. Sample was dissolved and iron was precipitated as Fe(OH)3 (106.867 g/mol). The precipitate was then ignited to a constant weight of 0.355 g as Fe2O3 (159.69 g/mol).

Jack was asked to determine iron (55.845 g/mol) content in dietary supplement. He took few random tablets and ground them into fine powder. Next, he weighed 3.116 g of the fine powder. Sample was dissolved and iron was precipitated as Fe(OH)3 (106.867 g/mol). The precipitate was then ignited to a constant weight of 0.355 g as Fe2O3 (159.69 g/mol).

Chemistry by OpenStax (2015-05-04)
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 14E: A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with...
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Jack was asked to determine iron (55.845 g/mol) content in dietary supplement. He took
few random tablets and ground them into fine powder. Next, he weighed 3.116 g of the
fine powder. Sample was dissolved and iron was precipitated as Fe(OH)3 (106.867 g/mol).
The precipitate was then ignited to a constant weight of 0.355 g as Fe2O3 (159.69 g/mol).
Report the iron content in dietary supplement as % w/w FeSO4·7H2O (278.01 g/mol).

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