Write the formula of the conjugate base of each of the following:
`H_2O , HSO_4^(-), NH_4^(+), CH_3COOH,H_3PO_4, CH_3NH_3^+`

Answer

To find the conjugate base of each given species, we need to remove a proton (H⁺) from each acid. The conjugate base is what remains after the acid has donated a proton. Here’s the step-by-step solution:

1. **Identify the species**: We have the following acids: H₂O, HSO₄⁻, NH₄⁺, CH₃COOH, H₃PO₄, and CH₃NH₃⁺.

2. **Remove a proton (H⁺)**: For each acid, we will remove one H⁺ ion to find the conjugate base.

- **For H₂O**:
- Remove H⁺: H₂O → OH⁻
- **Conjugate Base**: OH⁻

- **For HSO₄⁻**:
- Remove H⁺: HSO₄⁻ → SO₄²⁻
- **Conjugate Base**: SO₄²⁻

- **For NH₄⁺**:
- Remove H⁺: NH₄⁺ → NH₃
- **Conjugate Base**: NH₃

- **For CH₃COOH**:
- Remove H⁺: CH₃COOH → CH₃COO⁻
- **Conjugate Base**: CH₃COO⁻

- **For H₃PO₄**:
- Remove H⁺: H₃PO₄ → H₂PO₄⁻
- **Conjugate Base**: H₂PO₄⁻

- **For CH₃NH₃⁺**:
- Remove H⁺: CH₃NH₃⁺ → CH₃NH₂
- **Conjugate Base**: CH₃NH₂

3. **Final List of Conjugate Bases**:
- H₂O → OH⁻
- HSO₄⁻ → SO₄²⁻
- NH₄⁺ → NH₃
- CH₃COOH → CH₃COO⁻
- H₃PO₄ → H₂PO₄⁻
- CH₃NH₃⁺ → CH₃NH₂