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Which of the following compounds would h...

Which of the following compounds would have the smallest value for `pK_(a)`?

A

`CHF_(2)CH_(2)CH_(2)COOH`

B

`CH_(3)CH_(2)CF_(2)COOH`

C

`CH_(2)FCHFCH_(2)COOH`

D

`CH_(3)CF_(2)CH_(2)COOH`

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given compounds has the smallest value for \( pK_a \), we need to analyze the acidic strength of each compound based on the position of the electron-withdrawing groups relative to the functional group. ### Step-by-Step Solution: 1. **Understanding \( pK_a \)**: - The \( pK_a \) value is a measure of the acidity of a compound. A lower \( pK_a \) value indicates a stronger acid. Therefore, we are looking for the compound with the highest acidity. 2. **Identifying the Functional Group**: - In this case, the functional group we are focusing on is the carboxylic acid group (-COOH). 3. **Analyzing the Compounds**: - We need to look at the compounds provided in the options and identify where the electron-withdrawing groups (EWGs) are located in relation to the carboxylic acid group. - The presence of electron-withdrawing groups increases the acidity of carboxylic acids by stabilizing the negative charge on the conjugate base after deprotonation. 4. **Position of the Electron-Withdrawing Groups**: - For each option, identify the position of the electron-withdrawing groups (like -F or -Cl) relative to the carboxylic acid group. - The closer the EWG is to the carboxylic acid group, the stronger the acid will be. 5. **Comparing the Options**: - **Option 1**: EWG at the 3rd position from the -COOH group. - **Option 2**: EWG at the 1st position from the -COOH group (closest). - **Option 3**: EWG at the 2nd position from the -COOH group. - **Option 4**: EWG at the 2nd position from the -COOH group (similar to option 3 but different EWG). 6. **Determining the Strongest Acid**: - Since option 2 has the EWG closest to the carboxylic acid group, it will have the highest acidic strength. - Therefore, option 2 will have the smallest \( pK_a \) value. ### Conclusion: The compound with the smallest value for \( pK_a \) is **Option 2**.

To determine which of the given compounds has the smallest value for \( pK_a \), we need to analyze the acidic strength of each compound based on the position of the electron-withdrawing groups relative to the functional group. ### Step-by-Step Solution: 1. **Understanding \( pK_a \)**: - The \( pK_a \) value is a measure of the acidity of a compound. A lower \( pK_a \) value indicates a stronger acid. Therefore, we are looking for the compound with the highest acidity. 2. **Identifying the Functional Group**: ...
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  • Which of the following compounds have a dipole moment?

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    A
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    B
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