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To measure the concentration of an aqueous solution of H₂O2, an analytical chemist adds strong acid to a 39.0 g sample of the solution and titrates it to the endpoint with 128. mL of 0.2900M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 6H* (aq) + 5H₂O₂(aq) + 2MnO4 (aq) What kind of reaction is this? - · 50₂(g) + 2Mn²+ (aq) + 8 H₂O (1) 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. O precipitation O acid-base O redox 0 0 0% % 5 2 品 G

To measure the concentration of an aqueous solution of H₂O2, an analytical chemist adds strong acid to a 39.0 g sample of the solution and titrates it to the endpoint with 128. mL of 0.2900M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 6H* (aq) + 5H₂O₂(aq) + 2MnO4 (aq) What kind of reaction is this? - · 50₂(g) + 2Mn²+ (aq) + 8 H₂O (1) 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. O precipitation O acid-base O redox 0 0 0% % 5 2 品 G

Chemistry
Chemistry
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ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Steven S. Zumdahl
Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
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To measure the concentration of an aqueous solution of H₂O2, an analytical chemist adds strong acid to a 39.0 g sample of the solution and titrates it to the endpoint with 128. mL of 0.2900M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 6H* (aq) + 5H₂O₂(aq) + 2MnO4 (aq) What kind of reaction is this? - · 50₂(g) + 2Mn²+ (aq) + 8 H₂O (1) 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. O precipitation O acid-base O redox 0 0 0% % 5 2 品 G
Transcribed Image Text:To measure the concentration of an aqueous solution of H₂O2, an analytical chemist adds strong acid to a 39.0 g sample of the solution and titrates it to the endpoint with 128. mL of 0.2900M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 6H* (aq) + 5H₂O₂(aq) + 2MnO4 (aq) What kind of reaction is this? - · 50₂(g) + 2Mn²+ (aq) + 8 H₂O (1) 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. O precipitation O acid-base O redox 0 0 0% % 5 2 品 G
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