A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink end point. The balacned redox reaction is shown below. 8H++MnO4 - +5Fe2+------>Mn2++5Fe3++4H2O1.) How many moles MnO4 - were used in the titration?2.) How many grams of Fe are there in the sample3.) How many moles Fe2+ are there in the sample?4.) What is the percentage of Fe(by mass) in the sample?

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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 solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink end point. The balacned redox reaction is shown below.

8H⁺+MnO₄ ^- +5Fe²⁺------>Mn²⁺+5Fe³⁺+4H₂O

1.) How many moles MnO₄ ^- were used in the titration?

2.) How many grams of Fe are there in the sample

3.) How many moles Fe²⁺ are there in the sample?

4.) What is the percentage of Fe(by mass) in the sample?

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