The conjugate base is none O OH H O HSO4 O H2SO4 H20

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HSO4-(aq) + H2O(l) ⟷⟷ H2SO4(aq) + OH-(aq)

### Conjugate Bases

In the context of acid-base chemistry, a conjugate base is formed when an acid donates a proton (H⁺). The conjugate base is the species that remains after the acid has given up a proton. 

Examine the following multiple-choice question to test your understanding of conjugate bases:

**Question:** The conjugate base is

- ⬜ none
- ⬜ OH⁻
- ⬜ HSO₄⁻
- ⬜ H₂SO₄
- ⬜ H₂O

### Explanation of Options

- **none**: This choice implies that no conjugate base is formed, which is incorrect as every acid has a conjugate base.
- **OH⁻ (Hydroxide ion)**: This is the conjugate base of water (H₂O) when water acts as an acid.
- **HSO₄⁻ (Hydrogen sulfate ion)**: This is the conjugate base of sulfuric acid (H₂SO₄) when sulfuric acid donates a proton.
- **H₂SO₄ (Sulfuric acid)**: This is an acid, not a conjugate base.
- **H₂O (Water)**: Although water can act as both an acid and a base, it is not the conjugate base in this context.

The correct answer depends on the specific acid in question. For example, if H₂SO₄ (sulfuric acid) is the acid, its conjugate base would be HSO₄⁻. If water is the acid, its conjugate base would be OH⁻. Understanding the concept of conjugate acid-base pairs is fundamental in acid-base chemistry.
Transcribed Image Text:### Conjugate Bases In the context of acid-base chemistry, a conjugate base is formed when an acid donates a proton (H⁺). The conjugate base is the species that remains after the acid has given up a proton. Examine the following multiple-choice question to test your understanding of conjugate bases: **Question:** The conjugate base is - ⬜ none - ⬜ OH⁻ - ⬜ HSO₄⁻ - ⬜ H₂SO₄ - ⬜ H₂O ### Explanation of Options - **none**: This choice implies that no conjugate base is formed, which is incorrect as every acid has a conjugate base. - **OH⁻ (Hydroxide ion)**: This is the conjugate base of water (H₂O) when water acts as an acid. - **HSO₄⁻ (Hydrogen sulfate ion)**: This is the conjugate base of sulfuric acid (H₂SO₄) when sulfuric acid donates a proton. - **H₂SO₄ (Sulfuric acid)**: This is an acid, not a conjugate base. - **H₂O (Water)**: Although water can act as both an acid and a base, it is not the conjugate base in this context. The correct answer depends on the specific acid in question. For example, if H₂SO₄ (sulfuric acid) is the acid, its conjugate base would be HSO₄⁻. If water is the acid, its conjugate base would be OH⁻. Understanding the concept of conjugate acid-base pairs is fundamental in acid-base chemistry.
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