In which of the solution hydrogen peroxide neither acts as oxidising agent nor reducing agent ?

Options

A. `PbS+H_(2)O_(2)rarr`
B. `SO_(3)^(-)+H_(2)O_(2)rarr`
C. `PbO_(2)+H_(2)O_(2)rarr`
D. `Na_(2)CO_(3)+H_(2)O_(2)rarr`

Answer

To determine in which solution hydrogen peroxide (H₂O₂) neither acts as an oxidizing agent nor a reducing agent, we will analyze the reactions provided in the question step by step.

### Step 1: Understanding Oxidizing and Reducing Agents
- An **oxidizing agent** gains electrons and gets reduced, leading to a decrease in its oxidation state.
- A **reducing agent** loses electrons and gets oxidized, leading to an increase in its oxidation state.

### Step 2: Analyzing Each Reaction
We will evaluate each of the four reactions given in the options:

1. **Reaction 1: PbS + H₂O₂**
- Products: PbSO₄ + H₂O
- Oxidation states:
- Pb in PbS: -2
- S in PbS: +2
- S in PbSO₄: +6
- Here, sulfur is oxidized from +2 to +6, indicating that H₂O₂ acts as an oxidizing agent (it gets reduced).

2. **Reaction 2: SO₃²⁻ + H₂O₂**
- Products: SO₄²⁻ + H₂O
- Oxidation states:
- S in SO₃²⁻: +4
- S in SO₄²⁻: +6
- Again, sulfur is oxidized from +4 to +6, indicating that H₂O₂ acts as an oxidizing agent (it gets reduced).

3. **Reaction 3: PbO₂ + H₂O₂**
- Products: PbO + H₂O + O₂
- Oxidation states:
- Pb in PbO₂: +4
- Pb in PbO: +2
- Here, lead is reduced from +4 to +2, indicating that H₂O₂ acts as a reducing agent (it gets oxidized).

4. **Reaction 4: Na₂CO₃ + H₂O₂**
- Products: Na₂O₂ + HCO₂ + H₂O
- This is primarily an acid-base reaction.
- In this case, H₂O₂ does not change its oxidation state and does not act as either an oxidizing or reducing agent.

### Conclusion
From the analysis, we find that in the fourth reaction (Na₂CO₃ + H₂O₂), hydrogen peroxide neither acts as an oxidizing agent nor as a reducing agent.

Thus, the correct answer is **Na₂CO₃ and H₂O₂**.

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