Which of the following are the conjugate bases of the given acids?
`HClO_4, HCl, HBr, HI, HNO_3, H_2SO_4`

Options

A. `ClO_3^-, Cl^-, Br^-, I^-, NO_3^(2-), H_2SO_4^-`
B. `ClO_3^-, Cl^-, Br^-, I^-, NO_3^-, H_2SO_4^(-2)`
C. `ClO_4^-, Cl^-, Br^-, I^-, NO_3^-, H_2SO_4^(2-)`
D. `ClO_4^-, Cl^-, Br^-, I^-, NO_3^-, HSO_4^-`

Answer

To determine the conjugate bases of the given acids, we need to understand that when an acid donates a proton (H⁺), it forms its conjugate base. The conjugate base is the species that remains after the acid has lost a proton.

Let's analyze each acid provided in the question:

1. **HClO₄ (Perchloric acid)**:
- When HClO₄ donates a proton (H⁺), it becomes ClO₄⁻.
- **Conjugate base**: ClO₄⁻

2. **HCl (Hydrochloric acid)**:
- When HCl donates a proton (H⁺), it becomes Cl⁻.
- **Conjugate base**: Cl⁻

3. **HBr (Hydrobromic acid)**:
- When HBr donates a proton (H⁺), it becomes Br⁻.
- **Conjugate base**: Br⁻

4. **HI (Hydroiodic acid)**:
- When HI donates a proton (H⁺), it becomes I⁻.
- **Conjugate base**: I⁻

5. **HNO₃ (Nitric acid)**:
- When HNO₃ donates a proton (H⁺), it becomes NO₃⁻.
- **Conjugate base**: NO₃⁻

6. **H₂SO₄ (Sulfuric acid)**:
- When H₂SO₄ donates a proton (H⁺), it becomes HSO₄⁻.
- **Conjugate base**: HSO₄⁻

Now, we can summarize the conjugate bases for each acid:

- HClO₄ → ClO₄⁻
- HCl → Cl⁻
- HBr → Br⁻
- HI → I⁻
- HNO₃ → NO₃⁻
- H₂SO₄ → HSO₄⁻

### Final Answer:
The conjugate bases of the given acids are:
- HClO₄ → ClO₄⁻
- HCl → Cl⁻
- HBr → Br⁻
- HI → I⁻
- HNO₃ → NO₃⁻
- H₂SO₄ → HSO₄⁻