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    Lab: Analysis of Hydrogen Peroxide Solutions

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    Fill a burette with 50 mL of 0.2M potassium permanganate solution. Add 10 mL of NEW hydrogen peroxide and 2 mL of 6M sulfuric acid to a flask. Titrate the hydrogen peroxide with the KMnO4 solution to the purple endpoint of excess MnO4- ion.

    Questions:
    (a) Volume of potassium permanganate used in each titration (mL):50mL
    (b) The volume of potassium permanganate required to titrate 10 mL of the new hydrogen peroxide (mL):20mL
    (c) Calculate the concentration of H2O2 from the volume of KMnO4 used and the stoichiometry of the reaction (MW of H2O2 is 34.01).

    In these calculations I got lost.
    -I found 0.12655 mol KMnO4. Is this the amount in mol of KMnO4 which reacted? So now how I get the concentration of the H2O2?
    -2(C2x0.02L)KMnO4=5(34.01xV1)H2O2. What is C2 and V1?

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    https://brainmass.com/chemistry/acid-and-base-organic-chemistry/lab-analysis-hydrogen-peroxide-solutions-399278

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    Lab: Analysis of Hydrogen Peroxide Solutions
    Fill a burette with 50 mL of 0.2M potassium permanganate solution. Add 10 mL of NEW hydrogen peroxide and 2 mL of 6M sulfuric acid to a flask. Titrate the hydrogen peroxide with the KMnO4 solution to the purple endpoint of excess MnO4- ion.

    Questions:
    (a) Volume of potassium permanganate used in each titration (mL):50mL
    (b) The volume of potassium permanganate required to titrate ...

    Solution Summary

    An analysis of hydrogen peroxide solutions are examined.

    $2.19

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