All iron in 4.00 g of iron ore sample, which was dissolved in an acid solution, was converted to Fe2+ which was then titrated with 0.200 M KMNO4 solution. In this titration all iron is oxidized to Fe3+ and MnO4 to Mn²*. If 27.45 mL of KMNO4 solution is required to the end point, determine 1. How many grams of iron content is in the iron ore sample. 2. The yield percentage of iron in the sample. 3. If the iron in the sample is present as Fe2O3, what is the mass percentage of Fe2O3 in the sample.
All iron in 4.00 g of iron ore sample, which was dissolved in an acid solution, was converted to Fe2+ which was then titrated with 0.200 M KMNO4 solution. In this titration all iron is oxidized to Fe3+ and MnO4 to Mn²*. If 27.45 mL of KMNO4 solution is required to the end point, determine 1. How many grams of iron content is in the iron ore sample. 2. The yield percentage of iron in the sample. 3. If the iron in the sample is present as Fe2O3, what is the mass percentage of Fe2O3 in the sample.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 58QAP: The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing...
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Transcribed Image Text:All iron in 4.00 g of iron ore sample, which was dissolved in an acid
solution, was converted to Fe2+ which was then titrated with 0.200 M
KMNO4 solution. In this titration all iron is oxidized to Fe3+ and MnO4
to Mn2+. If 27.45 mL of KMNO4 solution is required to the end point,
determine
1. How many grams of iron content is in the iron ore sample.
2. The yield percentage of iron in the sample.
3. If the iron in the sample is present as Fe2O3, what is the mass
percentage of Fe2O3 in the sample.
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