An iron ore was analyzed by dissolving a 1.957-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe2O3·xH2O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.6009 g of pure Fe2O3. Calculate (a) the % Fe and (b) the % Fe3O4 in the sample.
An iron ore was analyzed by dissolving a 1.957-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe2O3·xH2O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.6009 g of pure Fe2O3. Calculate (a) the % Fe and (b) the % Fe3O4 in the sample.
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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An iron ore was analyzed by dissolving a 1.957-g sample in concentrated HCl. The
resulting solution was diluted with water, and the iron(III) was precipitated as the
hydrous oxide Fe2O3·xH2O by the addition of NH3. After filtration and washing, the
residue was ignited at a high temperature to give 0.6009 g of pure Fe2O3. Calculate (a)
the % Fe and (b) the % Fe3O4 in the sample.
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