Balance the following redox reaction in basic aqueous solution.

Cl2 (g) → Cl− (aq) + ClO− (aq)

Question

Balance the following redox reaction in basic aqueous solution.

Cl2 (g) → Cl− (aq) + ClO− (aq)

BlackTom AI · Accepted Answer

Disproportionation of chlorine in basic solution produces chloride (Cl−) and hypochlorite (ClO−). Use half‑reaction balancing in basic solution.

1) Relevant knowledge points
- Redox half‑reactions must conserve mass and charge.
- In basic solution, balance O with H2O and H with OH− (add OH− to neutralize H+).
- Electrons lost in oxidation must equal electrons gained in reduction.

2) Step‑by‑step reasoning (half‑reaction method)
Reduction half (chlorine reduced to chloride):
Cl2 + 2 e− → 2 Cl−
(Here one Cl2 accepts 2 e− to give two Cl−.)

Oxidation half (chloride → hypochlorite; note Cl− → ClO− is loss of 2 e−):
Cl− + H2O → ClO− + 2 H+ + 2 e−

3) Combine halves (show intermediate steps)
Add the two half‑reactions so electrons cancel:
Cl2 + (Cl− + H2O) → 2 Cl− + (ClO− + 2 H+)

Cancel one Cl− on each side:
Cl2 + H2O → Cl− + ClO− + 2 H+

Convert to basic medium by adding 2 OH− to both sides (to neutralize 2 H+):
Cl2 + H2O + 2 OH− → Cl− + ClO− + 2 H2O

Cancel one H2O from both sides:
Cl2 + 2 OH− → Cl− + ClO− + H2O

This is the balanced equation in basic solution.

4) Why this is correct
Mass and charge are balanced: LHS has 2 Cl, 2 O, net charge −2; RHS has 2 Cl, 2 O (one in ClO− and one in H2O), net charge −2. Electron transfer was accounted for via half‑reactions.

5) Why other choices are incorrect
- Option A (2 Cl2 + 4 OH− → 2 Cl− + 2 ClO− + 2 H2O) is simply twice the correct equation—chemically equivalent but not the single‑molecule form given as the answer.
- Option C includes both OH− and excess H+ and extra waters, producing inconsistent charge/mass balance.
- Option D places extra waters and OH− on the wrong sides and is not balanced overall.
- Option E has too few OH− for the number of Cl2 molecules (charge and O/H balance fail).

6) Conclusion
The balanced basic‑solution equation is Cl2 (g) + 2 OH− (aq) → Cl− (aq) + ClO− (aq) + H2O (l), which matches the provided answer.

Balance the following redox reaction in basic aqueous solution. Cl2 (g) → Cl− (aq) + ClO− (aq)Single choice

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