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ple of an iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 38.55 mL of 0.02500 M Mn04 - şolution. The oxidation-reduction reaction that occurs during titration is as follows: Mn04 - (ag) + 5FE2+(ag) + 8H+ (ag) à Mn2+(ag) + 5FE3+(ag) + 4H2O(I) a. How many moles of MnO4 - were added to the solution? A sample b. How many moles of Fe2+ were in the sample?

ple of an iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 38.55 mL of 0.02500 M Mn04 - şolution. The oxidation-reduction reaction that occurs during titration is as follows: Mn04 - (ag) + 5FE2+(ag) + 8H+ (ag) à Mn2+(ag) + 5FE3+(ag) + 4H2O(I) a. How many moles of MnO4 - were added to the solution? A sample b. How many moles of Fe2+ were in the sample?

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.103QE
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A sample of an iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 38.55 mL of 0.02500 M Mn04 - şolution. The oxidation-reduction reacțion that occurs during titration is as follows: Mn04 - (ag) + 5FE2+(ag) + 8H+ (ag) à Mn2+(ag) + 5Fe3+(ag) + 4H2O(1) a. How many moles of Mn04 - were added to the solution? b. How many moles of Fe2+ were in the sample?
Transcribed Image Text:A sample of an iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 38.55 mL of 0.02500 M Mn04 - şolution. The oxidation-reduction reacțion that occurs during titration is as follows: Mn04 - (ag) + 5FE2+(ag) + 8H+ (ag) à Mn2+(ag) + 5Fe3+(ag) + 4H2O(1) a. How many moles of Mn04 - were added to the solution? b. How many moles of Fe2+ were in the sample?
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