An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)

Answered: Image /qna-images/answer/2ad163e1-7e63-4724-8ea8-d40547c1ec83.jpg

Answered: An ore containing magnetite, Fe3O4, was…

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...

See similar textbooks

Related questions

Question

An ore containing magnetite, Fe₃O₄, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe²⁺ and Fe³⁺. After adding HNO₃ to oxidize any Fe²⁺ to Fe³⁺, the resulting solution was diluted with water and the Fe³⁺ precipitated as Fe(OH)₃ by adding NH₃. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe₂O₃. Calculate the %w/w Fe₃O₄ in the sample (Fe₃O₄ =231.54 g/mol, Fe₂O₃ = 159.69 g/mol)

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Extraction of Crude Metal from Concentrated Ore

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions