Comproportionationn occurs between:

Options

A. `Cl^(-)(aq.)+ClO^(-)(aq.)+OH^(-)(aq.)`
B. `PH_(3)(g)+H_(3)PO_(4)` acid
C. `Na_(2)S(aq.)+Na_(2)SO_(3)(aq.)`
D. `MNO_(4)^(2-)(aq.)+Mn^(2+)(aq.)+ZnSO_(4)(aq.)`

Explanation

To determine which reactions involve comproportionation, we need to analyze each reaction in terms of oxidation states of the elements involved. Comproportionation occurs when two reactants containing the same element in different oxidation states react to form a single product with an intermediate oxidation state.

### Step-by-Step Solution:

1. **Identify the Reactants and Their Oxidation States:**
- For each reaction, identify the oxidation states of the elements involved.

2. **Analyze the First Reaction:**
- **Reaction:** Cl⁻ (oxidation state -1) + ClO (oxidation state +1) → Cl₂ (oxidation state 0)
- **Change in Oxidation State:**
- Cl⁻ → Cl₂: oxidation state increases from -1 to 0 (oxidation)
- ClO → Cl₂: oxidation state decreases from +1 to 0 (reduction)
- **Conclusion:** This is a comproportionation reaction.

3. **Analyze the Second Reaction:**
- **Reaction:** H₃ (oxidation state -3) + H₃PO₄ (oxidation state +5) → H₄PO₃ (oxidation state +3)
- **Change in Oxidation State:**
- H₃ → H₄PO₃: oxidation state increases from -3 to +3 (oxidation)
- H₃PO₄ → H₄PO₃: oxidation state decreases from +5 to +3 (reduction)
- **Conclusion:** This is a comproportionation reaction.

4. **Analyze the Third Reaction:**
- **Reaction:** Ne₂S (oxidation state -2) + Ne₂SO₃ (oxidation state +4) → S (oxidation state 0)
- **Change in Oxidation State:**
- Ne₂S → S: oxidation state increases from -2 to 0 (oxidation)
- Ne₂SO₃ → S: oxidation state decreases from +4 to 0 (reduction)
- **Conclusion:** This is a comproportionation reaction.

5. **Analyze the Fourth Reaction:**
- **Reaction:** MnO₄²⁻ (oxidation state +7) + MnO₄²⁻ (oxidation state +2) → MnO₄²⁻ (oxidation state +6)
- **Change in Oxidation State:**
- MnO₄²⁻ (from +7) → MnO₄²⁻ (to +6): oxidation state decreases from +7 to +6 (reduction)
- MnO₄²⁻ (from +2) → MnO₄²⁻ (to +6): oxidation state increases from +2 to +6 (oxidation)
- **Conclusion:** This is a comproportionation reaction.

6. **Final Conclusion:**
- All four reactions involve comproportionation as they all involve the same element in different oxidation states reacting to form a product with an intermediate oxidation state.

### Answer:
Comproportionation occurs between all four reactions.

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