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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
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...
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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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