Which of the following would be expected to be easily dissociated in water?

Options

A. `ClCH_2CH_2CH_2COOH`
B. `CH_3 C Cl_2CH_2COOH`
C. `CH_3CH_2C Cl_2 COOH`
D. `CH_3CH_2 CHClCOOH`

Explanation

To determine which of the given acids would be expected to be easily dissociated in water, we need to analyze the acidity of each compound based on their structure and the presence of electron-withdrawing or electron-donating groups.

### Step-by-Step Solution:

1. **Identify the Compounds**: First, we need to identify the acids provided in the question. Let's assume they are carboxylic acids, as mentioned in the transcript.

2. **Understand Acidity**: Acidity is the ability of a compound to donate a proton (H⁺). The more easily a compound can donate a proton, the stronger the acid it is.

3. **Role of Electron-Withdrawing and Electron-Donating Groups**:
- Electron-withdrawing groups (EWGs) stabilize the negative charge that forms when an acid donates a proton, making the acid stronger (more acidic).
- Electron-donating groups (EDGs) destabilize the negative charge, making the acid weaker (less acidic).

4. **Analyze the Compounds**:
- For each acid, check the presence of electron-withdrawing groups (like halogens, nitro groups, etc.) and electron-donating groups (like alkyl groups).
- The acid with more electron-withdrawing groups will be more acidic and thus will dissociate more easily in water.

5. **Compare Acidity**:
- If one acid has multiple electron-withdrawing groups compared to another acid with fewer or no such groups, the former will be expected to dissociate more easily in water.

6. **Conclusion**: After analyzing the compounds based on the presence of electron-withdrawing and electron-donating groups, identify the acid that is the strongest (most acidic) and thus expected to dissociate easily in water.