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Chemistry | 12th Edition | ISBN: 9780078021510 | Authors: Raymond Chang; Kenneth Goldsby
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Solved: A quantity of 25.0 mL of a solution containing

Chapter 4, Problem 4.162

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QUESTION:

A quantity of 25.0 mL of a solution containing both Fe21 and Fe31 ions is titrated with 23.0 mL of 0.0200 M KMnO4 (in dilute sulfuric acid). As a result, all of the Fe21 ions are oxidized to Fe31 ions. Next, the solution is treated with Zn metal to convert all of the Fe31 ions to Fe21 ions. Finally, the solution containing only the Fe21 ions requires 40.0 mL of the same KMnO4 solution for oxidation to Fe31. Calculate the molar concentrations of Fe21 and Fe31 in the original solution. The net ionic equation is MnO4 2 1 5Fe21 1 8H1 Mn21 1 5Fe31 1 4H2O

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QUESTION:

A quantity of 25.0 mL of a solution containing both Fe21 and Fe31 ions is titrated with 23.0 mL of 0.0200 M KMnO4 (in dilute sulfuric acid). As a result, all of the Fe21 ions are oxidized to Fe31 ions. Next, the solution is treated with Zn metal to convert all of the Fe31 ions to Fe21 ions. Finally, the solution containing only the Fe21 ions requires 40.0 mL of the same KMnO4 solution for oxidation to Fe31. Calculate the molar concentrations of Fe21 and Fe31 in the original solution. The net ionic equation is MnO4 2 1 5Fe21 1 8H1 Mn21 1 5Fe31 1 4H2O

ANSWER:

Step 1 of 4

From the given,

Titration -1

Oxidizes ,  it will give us the amount of  in the solution.

Zinc is added to reduce  back to .

Titration - 2

Oxidized  to  

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