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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
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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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