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
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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
Chapter1: Chemical Foundations
Section: Chapter Questions
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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 0.3100 M potassium permanganate (\( \text{KMnO}_4 \)) solution.
The balanced chemical equation for the reaction is:
\[ 8 \text{H}^+ (aq) + 5 \text{Fe}^{2+} (aq) + \text{MnO}_4^- (aq) \rightarrow 5 \text{Fe}^{3+} (aq) + \text{Mn}^{2+} (aq) + 4 \text{H}_2\text{O} (l) \]
### What kind of reaction is this?
- Precipitation
- Acid-base
- Redox
The checkbox has been marked for "precipitation" (Note: In this case, the correct answer is "redox").
### Questions:
1. **If you said this was a precipitation reaction, enter the chemical formula of the precipitate.**
2. **If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base.**
3. **If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized.**
4. **Calculate the mass percent of \( \text{Fe} \) in the sample. Be sure your answer has the correct number of significant digits.**
\[ \_\_\_\_ \% \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12c0a0e9-4d98-45bb-8c42-bb6fd08d9097%2Fc73ab758-4380-482a-a915-aa617bd4a02f%2Fntv7pfq_processed.png&w=3840&q=75)
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 0.3100 M potassium permanganate (\( \text{KMnO}_4 \)) solution.
The balanced chemical equation for the reaction is:
\[ 8 \text{H}^+ (aq) + 5 \text{Fe}^{2+} (aq) + \text{MnO}_4^- (aq) \rightarrow 5 \text{Fe}^{3+} (aq) + \text{Mn}^{2+} (aq) + 4 \text{H}_2\text{O} (l) \]
### What kind of reaction is this?
- Precipitation
- Acid-base
- Redox
The checkbox has been marked for "precipitation" (Note: In this case, the correct answer is "redox").
### Questions:
1. **If you said this was a precipitation reaction, enter the chemical formula of the precipitate.**
2. **If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base.**
3. **If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized.**
4. **Calculate the mass percent of \( \text{Fe} \) in the sample. Be sure your answer has the correct number of significant digits.**
\[ \_\_\_\_ \% \]
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