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3. Balance the following in basic solution: a. So,2 (aq) + Cu(OH), (8) → So,²- (aq) + Cu(OH) (s) b. O2 (9) + Mn(OH), (8) - c. NO, (aq) + H, (9) - - MnOz (8) - NO (9) d. Al (s) + Cro, (aq) Al(OH), (s) + Cr(OH), (aq) 4. Identify the species that was oxidized, the species that was reduced, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem.

3. Balance the following in basic solution: a. So,2 (aq) + Cu(OH), (8) → So,²- (aq) + Cu(OH) (s) b. O2 (9) + Mn(OH), (8) - c. NO, (aq) + H, (9) - - MnOz (8) - NO (9) d. Al (s) + Cro, (aq) Al(OH), (s) + Cr(OH), (aq) 4. Identify the species that was oxidized, the species that was reduced, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.9: Corrosion: Redox Reactions In The Environment
Problem 2.4ACP: The overall reaction for the production of Cu(OH)2 from Cu in oxygenated water can be broken into...
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1. Balance the following in acidic solution: a. H2O2 + Sn²+ –→ H2O + Sn+ b. РЬО, + Hg + Hg, 2+ + Pb²+ c. Al + Cr,O,²- –→ Al³* + Cr³* 2. Identify the species that undergoes oxidation, the species that undergoes reduction, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem. 3. Balance the following in basic solution: a. SO,²- (aq) + Cu(OH), (s) → S0,²- (aq) + Cu(OH) (s) b. O2 (9) + Mn(OH), (8) · c. NO, (aq) + H2 (9) - d. Al (s) + CrO,²- (aq) → Al(OH), (8) + Cr(OH), (aq) - MnO2 (s) NO (9) 4. Identify the species that was oxidized, the species that was reduced, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem. 5. Why is it not possible for hydroxide ion (OH") to appear in either of the half-reactions or the overall equation when balancing oxidation-reduction reactions in acidic solution? 6. Why is it not possible for hydrogen ion (H*) to appear in either of the half-reactions or the overall equation when balancing oxidation-reduction reactions in basic solution? 7. Why must the charge balance in oxidation-reduction reactions?
Transcribed Image Text:1. Balance the following in acidic solution: a. H2O2 + Sn²+ –→ H2O + Sn+ b. РЬО, + Hg + Hg, 2+ + Pb²+ c. Al + Cr,O,²- –→ Al³* + Cr³* 2. Identify the species that undergoes oxidation, the species that undergoes reduction, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem. 3. Balance the following in basic solution: a. SO,²- (aq) + Cu(OH), (s) → S0,²- (aq) + Cu(OH) (s) b. O2 (9) + Mn(OH), (8) · c. NO, (aq) + H2 (9) - d. Al (s) + CrO,²- (aq) → Al(OH), (8) + Cr(OH), (aq) - MnO2 (s) NO (9) 4. Identify the species that was oxidized, the species that was reduced, the oxidizing agent, and the reducing agent in each of the reactions of the previous problem. 5. Why is it not possible for hydroxide ion (OH") to appear in either of the half-reactions or the overall equation when balancing oxidation-reduction reactions in acidic solution? 6. Why is it not possible for hydrogen ion (H*) to appear in either of the half-reactions or the overall equation when balancing oxidation-reduction reactions in basic solution? 7. Why must the charge balance in oxidation-reduction reactions?
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