`H_2O_2` is prepared in laboratory by action of `H_2SO_4` with

Options

A. `Na_2O_2`
B. `BaO_2`
C. `BaO_2`.8`H_2O`
D. Both A and C

Answer

To prepare hydrogen peroxide (H₂O₂) in the laboratory using sulfuric acid (H₂SO₄), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reactants**:
- The main reactant is sulfuric acid (H₂SO₄).
- We need to choose a suitable metal peroxide that can react with sulfuric acid to produce hydrogen peroxide.

2. **Choose the Metal Peroxide**:
- Common metal peroxides include sodium peroxide (Na₂O₂) and barium peroxide (BaO₂).
- Sodium peroxide is a good candidate because it reacts with sulfuric acid to produce hydrogen peroxide.

3. **Write the Reaction for Sodium Peroxide**:
- The reaction can be represented as:
\[ \text{Na}_2\text{O}_2 + \text{H}_2\text{SO}_4 \rightarrow \text{H}_2\text{O}_2 + \text{Na}_2\text{SO}_4 \]
- This shows that sodium peroxide reacts with sulfuric acid to yield hydrogen peroxide and sodium sulfate.

4. **Consider Barium Peroxide**:
- Barium peroxide (BaO₂) can also be used, but it must be in hydrated form (BaO₂·8H₂O) to avoid issues with precipitate formation.
- The reaction for hydrated barium peroxide is:
\[ \text{BaO}_2 \cdot 8\text{H}_2\text{O} + \text{H}_2\text{SO}_4 \rightarrow \text{H}_2\text{O}_2 + \text{BaSO}_4 + 8\text{H}_2\text{O} \]
- Here, barium sulfate (BaSO₄) precipitates out, and the presence of water helps to prevent the BaSO₄ from coating the BaO₂, allowing the reaction to proceed effectively.

5. **Conclusion**:
- Both sodium peroxide and hydrated barium peroxide can be used to prepare hydrogen peroxide in the laboratory.
- Therefore, the correct answer to the question is that H₂O₂ is prepared in the laboratory by the action of H₂SO₄ with both Na₂O₂ and BaO₂·8H₂O.

### Final Answer:
- The answer is **D**: Both A (Na₂O₂) and C (BaO₂·8H₂O) are correct.