The permanganate ion (MnO4- ) is often used in redox titrations. The strongly colored (violet) the permanganate ion forms the slightly pink Mn2+ ion upon reaction in acidic solution. Permanganate solutions are prepared by dissolving solid potassium permanganate. At preparation and storage of the solution, however, often forms brownstone (MnO 2 (s)) which must filtered before use. The concentration of the solution is therefore determined directly before use by titration in sulfuric acid solution against sodium oxalate (Na2 C2 O4 ; easily soluble salt that serves as the primary standard) whereby the oxalic acid forms carbon dioxide (gas). Calculate the concentration of a potassium permanganate solution from the following data. 0.6501 gram of sodium oxalate is weighed and consumes 20.00 mL of the prepared the potassium permanganate solution.
The permanganate ion (MnO4- ) is often used in redox titrations. The strongly colored (violet) the permanganate ion forms the slightly pink Mn2+ ion upon reaction in acidic solution. Permanganate solutions are prepared by dissolving solid potassium permanganate. At preparation and storage of the solution, however, often forms brownstone (MnO 2 (s)) which must filtered before use. The concentration of the solution is therefore determined directly before use by titration in sulfuric acid solution against sodium oxalate (Na2 C2 O4 ; easily soluble salt that serves as the primary standard) whereby the oxalic acid forms carbon dioxide (gas). Calculate the concentration of a potassium permanganate solution from the following data. 0.6501 gram of sodium oxalate is weighed and consumes 20.00 mL of the prepared the potassium permanganate solution.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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The permanganate ion (MnO4- ) is often used in redox titrations. The strongly colored (violet)
the permanganate ion forms the slightly pink Mn2+ ion upon reaction in acidic solution.
Permanganate solutions are prepared by dissolving solid potassium permanganate. At
preparation and storage of the solution, however, often forms brownstone (MnO 2 (s)) which must
filtered before use. The concentration of the solution is therefore determined directly before
use by titration in sulfuric acid solution against sodium oxalate (Na2 C2 O4 ;
easily soluble salt that serves as the primary standard) whereby the oxalic acid forms carbon dioxide (gas).
Calculate the concentration of a potassium permanganate solution from the following data.
0.6501 gram of sodium oxalate is weighed and consumes 20.00 mL of the prepared
the potassium permanganate solution.
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