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To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 31.00 g sample in strong acid and titrates it to the endpoint with 20.1 mL of 0.3100M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 8H* (aq) + 5Fe²+ (aq) + MnO4(aq) → 5Fe³+ (aq). + What kind of reaction is this? Mn²+ (aq) + 4H₂0 (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 Fe in the sample. Be sure correct number of significant digits. answer has the Oprecipitation O acid-base O redox 0 0 0 % 4 X 2 On x10

To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 31.00 g sample in strong acid and titrates it to the endpoint with 20.1 mL of 0.3100M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 8H* (aq) + 5Fe²+ (aq) + MnO4(aq) → 5Fe³+ (aq). + What kind of reaction is this? Mn²+ (aq) + 4H₂0 (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 Fe in the sample. Be sure correct number of significant digits. answer has the Oprecipitation O acid-base O redox 0 0 0 % 4 X 2 On x10

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 57QRT
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To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 31.00 g sample in strong acid and titrates it to the endpoint with 20.1 mL of 0.3100M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 8H* (aq) + 5Fe²+ (aq) + MnO4 (aq) What kind of reaction is this? 5Fe³+ (aq) + Mn²+ (aq) + 4H₂0 (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 Fe in the sample. Be sure your answer has the correct number of significant digits. Oprecipitation O acid-base O redox 0 0 0 0% 4 X 5 ☐
Transcribed Image Text:To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 31.00 g sample in strong acid and titrates it to the endpoint with 20.1 mL of 0.3100M potassium permanganate (KMnO4) solution. The balanced chemical equation for the reaction is: 8H* (aq) + 5Fe²+ (aq) + MnO4 (aq) What kind of reaction is this? 5Fe³+ (aq) + Mn²+ (aq) + 4H₂0 (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 Fe in the sample. Be sure your answer has the correct number of significant digits. Oprecipitation O acid-base O redox 0 0 0 0% 4 X 5 ☐
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