An iron ore sample weighing 0.9132 g is dissolved in HCl (aq), and the iron is obtained as Fe²⁺ (aq). This solution is then titrated with 28.72 mL of 0.05051 M K₂Cr₂O₇ . What is th... An iron ore sample weighing 0.9132 g is dissolved in HCl (aq), and the iron is obtained as Fe²⁺ (aq). This solution is then titrated with 28.72 mL of 0.05051 M K₂Cr₂O₇ . What is the mass percent Fe in the ore sample?
Understand the Problem
The question is asking us to calculate the mass percent of iron (Fe) in an iron ore sample. We are given the mass of the ore sample, the volume and molarity of the K₂Cr₂O₇ solution used in the titration, and the fact that iron is present as Fe²⁺. We will need to use stoichiometry based on the titration data to find the mass of iron and then calculate the mass percent.
Answer
53.2%
The mass percent of Fe in the ore sample is 53.2%.
Answer for screen readers
The mass percent of Fe in the ore sample is 53.2%.
More Information
To calculate the mass percent of iron in the ore sample, a titration method is used. The iron ore is dissolved in hydrochloric acid, resulting in Fe2+ ions. These ions are then titrated with a known concentration of potassium dichromate (K2Cr2O7). The reaction between Fe2+ and Cr2O72- is a redox reaction, where iron is oxidized to Fe3+ and chromium is reduced to Cr3+. By using the stoichiometry of the reaction and the volume and concentration of K2Cr2O7 used in the titration, the amount of iron in the original sample can be determined, and thus the mass percent of iron can be calculated.
Tips
Make sure the chemical equation is balanced properly before proceeding with the calculation.
Sources
- PDF] CHEM 130 Name Quiz 5 - blamp.sites.truman.edu
- Solved 3. An iron ore sample weighing 0.9132 g is dissolved - Chegg - chegg.com
- Problem 65 An iron ore sample weighing \(0.... [FREE SOLUTION] - vaia.com
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