Write the conjugate acid or base for the following species :
`HClO_4 , OH^(-) , F^(-) , CO_3^(2-) , S^(2-)`

Answer

To find the conjugate acids and bases for the given species, we can follow these steps:

### Step 1: Identify the species and determine if they can act as acids or bases.
- **HClO₄**: This is a strong acid and can lose a proton (H⁺).
- **OH⁻**: This is a base and can either accept a proton or lose a proton.
- **F⁻**: This is a base and can accept a proton.
- **CO₃²⁻**: This is a base and can accept a proton.
- **S²⁻**: This is a base and can accept a proton.

### Step 2: Write the conjugate acid or base for each species.
1. **HClO₄**:
- As an acid, it can lose H⁺ to form its conjugate base.
- **Conjugate Base**: ClO₄⁻

2. **OH⁻**:
- As a base, it can accept H⁺ to form its conjugate acid.
- **Conjugate Acid**: H₂O
- It can also lose H⁺ to form its conjugate base.
- **Conjugate Base**: O²⁻

3. **F⁻**:
- As a base, it can accept H⁺ to form its conjugate acid.
- **Conjugate Acid**: HF

4. **CO₃²⁻**:
- As a base, it can accept H⁺ to form its conjugate acid.
- **Conjugate Acid**: HCO₃⁻

5. **S²⁻**:
- As a base, it can accept H⁺ to form its conjugate acid.
- **Conjugate Acid**: HS⁻

### Summary of Conjugate Acids and Bases:
- HClO₄ → Conjugate Base: ClO₄⁻
- OH⁻ → Conjugate Acid: H₂O, Conjugate Base: O²⁻
- F⁻ → Conjugate Acid: HF
- CO₃²⁻ → Conjugate Acid: HCO₃⁻
- S²⁻ → Conjugate Acid: HS⁻