`H_2O_2` cannot act as reducing agent. True or False

Explanation

To determine whether the statement "H₂O₂ cannot act as a reducing agent" is true or false, we can analyze the properties of hydrogen peroxide (H₂O₂) and its behavior in chemical reactions.

### Step-by-Step Solution:

1. **Understanding Hydrogen Peroxide (H₂O₂)**:
- Hydrogen peroxide is a chemical compound with the formula H₂O₂. It consists of two hydrogen atoms and two oxygen atoms.

2. **Oxidation States**:
- In H₂O₂, the oxidation state of hydrogen is +1 and the oxidation state of oxygen is -1. This can be represented as:
- H: +1
- O: -1 (for each oxygen atom)

3. **Oxidizing and Reducing Agent**:
- A reducing agent is a substance that donates electrons in a chemical reaction and gets oxidized itself.
- An oxidizing agent is a substance that accepts electrons and gets reduced.

4. **Behavior of H₂O₂**:
- H₂O₂ can act as both an oxidizing agent and a reducing agent. This dual behavior is due to the fact that it can either gain or lose electrons depending on the reaction conditions.

5. **Reactions Demonstrating Reducing Character**:
- In acidic medium:
- H₂O₂ + 2 H⁺ → O₂ + 2 e⁻
- In basic medium:
- H₂O₂ + 2 OH⁻ → 2 H₂O + O₂ + 2 e⁻
- In both cases, H₂O₂ donates electrons, demonstrating its reducing properties.

6. **Conclusion**:
- Since H₂O₂ can act as a reducing agent in various reactions, the statement "H₂O₂ cannot act as a reducing agent" is **False**.

### Final Answer:
**False** - H₂O₂ can act as a reducing agent.