To determine the amount of magnetite (Fe3O4) in an impure ore, a 1.7832 g sample is dissolved in concentrated HCl, giving a mixture of Fe2+ and Fe3+. Then, Fe2+ is oxidized to Fe3+ by adding HNO3 and diluting with water. Fe3+ is precipitated as Fe(OH)3 by adding NH3. Filtering, rinsing and igniting the precipitate provides 0.9179 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
To determine the amount of magnetite (Fe3O4) in an impure ore, a 1.7832 g sample is dissolved in concentrated HCl, giving a mixture of Fe2+ and Fe3+. Then, Fe2+ is oxidized to Fe3+ by adding HNO3 and diluting with water. Fe3+ is precipitated as Fe(OH)3 by adding NH3. Filtering, rinsing and igniting the precipitate provides 0.9179 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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To determine the amount of magnetite (Fe3O4) in an impure ore, a 1.7832 g sample is dissolved in concentrated HCl, giving a mixture of Fe2+ and Fe3+. Then, Fe2+ is oxidized to Fe3+ by adding HNO3 and diluting with water. Fe3+ is precipitated as Fe(OH)3 by adding NH3. Filtering, rinsing and igniting the precipitate provides 0.9179 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
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