2. Kindly solve this and show your solution. 2. A 0.450 g of steel contains manganese as an impurity. The sample is dissolved in acidicsolution and the Mn is oxidized to the permanganate ion MnO4. The MnO4 ion isreduced to Mn2+ by reacting with 50 mL of 0.0800 M FeSO4 solution. The excess Fe2+ions are then oxidized to Fe3* by 22.4 mL of 0.01 M K2C12O7. Calculate the percent bymass of Mn in the sample.

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Answered: ions are then oxidized to Fe3+ by 22.4…

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ions are then oxidized to Fe3+ by 22.4 mL of 0.01 M K2C12O7. Calculate the percent by mass of Mn 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

Chapter20: Chemistry Of The Metals

Section: Chapter Questions

Problem 43QAP

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Question

2. Kindly solve this and show your solution.

2. A 0.450 g of steel contains manganese as an impurity. The sample is dissolved in acidic
solution and the Mn is oxidized to the permanganate ion MnO4. The MnO4 ion is
reduced to Mn2+ by reacting with 50 mL of 0.0800 M FeSO4 solution. The excess Fe2+
ions are then oxidized to Fe3* by 22.4 mL of 0.01 M K2C12O7. Calculate the percent by
mass of Mn in the sample.

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