Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 36m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

6. Chemical Quantities & Aqueous Reactions

Balancing Redox Reactions: Basic Solutions

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Balancing Redox Reactions: Basic Solutions

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Multiple Choice

What is the balanced redox reaction for Cl2(g) + Mn2+(aq) → MnO2(s) + Cl-(aq) in a basic solution?

Cl2(g) + Mn2+(aq) + 4OH-(aq) → MnO2(s) + Cl-(aq) + 2H2O(l)

Cl2(g) + Mn2+(aq) + 2H2O(l) → MnO2(s) + 2Cl-(aq) + 2OH-(aq)

Cl2(g) + Mn2+(aq) + 2OH-(aq) → MnO2(s) + 2Cl-(aq) + H2O(l)

Cl2(g) + 2Mn2+(aq) + 4OH-(aq) → 2MnO2(s) + 2Cl-(aq) + 2H2O(l)

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Verified step by step guidance

Identify the oxidation and reduction half-reactions. Chlorine (Cl2) is reduced to chloride ions (Cl-), and manganese ions (Mn2+) are oxidized to manganese dioxide (MnO2).

Write the reduction half-reaction for chlorine: Cl2(g) → 2Cl-(aq). Balance the atoms and charges by adding electrons: Cl2(g) + 2e- → 2Cl-(aq).

Write the oxidation half-reaction for manganese: Mn2+(aq) → MnO2(s). Balance the oxygen atoms by adding water molecules: Mn2+(aq) + 2H2O(l) → MnO2(s). Balance the hydrogen atoms by adding hydroxide ions: Mn2+(aq) + 2H2O(l) → MnO2(s) + 4OH-(aq). Balance the charges by adding electrons: Mn2+(aq) + 2H2O(l) → MnO2(s) + 4OH-(aq) + 2e-.

Combine the balanced half-reactions. Ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction. Add the two half-reactions: Cl2(g) + 2e- + Mn2+(aq) + 2H2O(l) → 2Cl-(aq) + MnO2(s) + 4OH-(aq) + 2e-.

Cancel out the electrons and any other species that appear on both sides of the equation. The final balanced redox reaction in a basic solution is: Cl2(g) + Mn2+(aq) + 2OH-(aq) → MnO2(s) + 2Cl-(aq) + H2O(l).