Consider the equilibrium equation, `CH_(3)COOH+HI leftrightarrowCH_(3)COOH_(2)^(+) + I^(-) ` which of the following statements is/are incorrect?

Options

A. `I^(-)` is the conjugate base of HI.
B. `I^(-)`is the conjugate base of `CH_(3)COOH`
C. `CH_(3)COOH`, is the conjugate acid of `CH_(3)COOH`
D. `CH_(3)COOH`, is the conjugate acid of `CH_(3)COOH_(2)^(+)`

Explanation

To determine which statements are incorrect regarding the equilibrium equation:

\[ \text{CH}_3\text{COOH} + \text{HI} \leftrightarrow \text{CH}_3\text{COOH}_2^+ + \text{I}^- \]

we need to analyze the roles of the species involved in the reaction and identify their conjugate acids and bases.

### Step-by-Step Solution:

1. **Identify the Acid and Base:**
- In the given equilibrium, **HI** donates a proton (H⁺) to **CH₃COOH** (acetic acid). Therefore, **HI** acts as an acid, and **CH₃COOH** acts as a base.

2. **Determine the Conjugate Acid and Base:**
- When **CH₃COOH** accepts a proton from **HI**, it forms **CH₃COOH₂⁺**. Thus, **CH₃COOH₂⁺** is the conjugate acid of **CH₃COOH**.
- The conjugate base of **HI** is **I⁻**, as it is what remains after HI donates a proton.

3. **Evaluate Each Statement:**
- **Option 1:** "I⁻ is a conjugate base of HI."
- This statement is **correct** because after HI donates a proton, I⁻ remains.

- **Option 2:** "I⁻ is a conjugate base of CH₃COOH."
- This statement is **incorrect**. I⁻ is not related to CH₃COOH; it is the conjugate base of HI.

- **Option 3:** "CH₃COOH is a conjugate acid of CH₃COOH."
- This statement is **incorrect**. CH₃COOH cannot be its own conjugate acid; it is the acid itself.

- **Option 4:** "CH₃COOH is a conjugate acid of CH₃COOH₂⁺."
- This statement is **incorrect**. CH₃COOH₂⁺ is the conjugate acid of CH₃COOH, not the other way around.

4. **Conclusion:**
- The incorrect statements are **Option 2**, **Option 3**, and **Option 4**.

### Final Answer:
The incorrect statements are **Option 2**, **Option 3**, and **Option 4**.

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