Conjugate base of `HO_(2)^(-)` is :

Options

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

Explanation

To determine the conjugate base of the ion \( \text{HO}_2^- \), we need to follow these steps:

### Step-by-Step Solution:

1. **Understand the Concept of Conjugate Bases**:
- A conjugate base is formed when an acid donates a proton (H⁺). The species that remains after the acid has lost a proton is the conjugate base.

2. **Identify the Given Species**:
- The species we are considering is \( \text{HO}_2^- \).

3. **Determine What Happens When \( \text{HO}_2^- \) Donates a Proton**:
- When \( \text{HO}_2^- \) donates a proton (H⁺), we need to find out what remains after this donation.

4. **Perform the Proton Donation**:
- \( \text{HO}_2^- \) → \( \text{O}_2^{2-} + \text{H}^+ \)

5. **Identify the Conjugate Base**:
- After the donation of H⁺, the remaining species is \( \text{O}_2^{2-} \). Therefore, \( \text{O}_2^{2-} \) is the conjugate base of \( \text{HO}_2^- \).

6. **Conclusion**:
- The conjugate base of \( \text{HO}_2^- \) is \( \text{O}_2^{2-} \).

### Final Answer:
The conjugate base of \( \text{HO}_2^- \) is \( \text{O}_2^{2-} \).

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