A sample of iron ore weighing 0.962 g was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions. The solution required 32.32 mL of 0.0475M KMnO4 for titration. Fill in the table and calculate the % by mass of iron in the ore. Balance the equation: Fe +2 + MnO4 → Fe+3 + MnO2 Computation Name of analyte Iron ore Mass of analyte 0.2792 g Name of titrant KMnO4 Volume of titrant 23.30 mL Milliequivalents of the titrant 2.260 milliequivalents Mass of the analyte 0.125 g % Fe in analyte 44.81%

A sample of iron ore weighing 0.962 g was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions. The solution required 32.32 mL of 0.0475M KMnO4 for titration. Fill in the table and calculate the % by mass of iron in the ore. Balance the equation: Fe +2 + MnO4 → Fe+3 + MnO2 Computation Name of analyte Iron ore Mass of analyte 0.2792 g Name of titrant KMnO4 Volume of titrant 23.30 mL Milliequivalents of the titrant 2.260 milliequivalents Mass of the analyte 0.125 g % Fe in analyte 44.81%

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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