Barium peroxide when dissolved in water forms a substance which has oxidizing as well as bleaching properties. The Bronsted acid in this reaction

Options

A. `O_(2)^(-)`
B. `O_(2)^(2-)`
C. `OH^(-)`
D. `H_(2)O`

Answer

To determine the Bronsted acid in the reaction of barium peroxide when dissolved in water, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction**: When barium peroxide (BaO2) is dissolved in water, it dissociates to form barium ions (Ba²⁺) and peroxide ions (O2²⁻). The peroxide ions can further react with water.

2. **Understand the Role of Water**: Water (H2O) can act both as an acid and a base. In this context, we need to identify which component donates a proton (H⁺) and which one accepts it.

3. **Identify the Oxidizing Agent**: The peroxide ion (O2²⁻) acts as a strong oxidizing agent. When it reacts with water, it can release nascent oxygen (O), which is responsible for its bleaching properties.

4. **Determine the Bronsted Acid**: In the reaction, water donates a proton (H⁺) to the peroxide ion. Since the substance that donates a proton is defined as a Bronsted acid, we conclude that water acts as the Bronsted acid in this reaction.

5. **Final Conclusion**: Therefore, the Bronsted acid in the reaction of barium peroxide dissolved in water is water (H2O).

### Summary:
- The Bronsted acid in the reaction is **water (H2O)**, as it donates a proton (H⁺) to the peroxide ion.