To measure the concentration of an aqueous solution of H2O2, an analytical chemist adds strong acid to a 48.00g sample of the solution and titrates it to the endpoint with 81.1mL of 0.290M potassium permanganate KMnO4 solution. The balanced chemical equation for the reaction is: 6H+(aq) + 5H2O2(aq) + 2MnO−4(aq) -> 5O2(g) + 2Mn2+(aq)  8H2O(l) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of H2O2 in the sample. Be sure your answer has the correct number of significant digits.

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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To measure the concentration of an aqueous solution of H2O2, an analytical chemist adds strong acid to a 48.00g sample of the solution and titrates it to the endpoint with 81.1mL of 0.290M potassium permanganate KMnO4 solution.

The balanced chemical equation for the reaction is:

6H+(aq) + 5H2O2(aq) + 2MnO−4(aq) -> 5O2(g) + 2Mn2+(aq)  8H2O(l)

What kind of reaction is this?

If you said this was a precipitation reaction, enter the chemical formula of the precipitate.

If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base.

If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized.

Calculate the mass percent of H2O2 in the sample. Be sure your answer has the correct number of significant digits.

 

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