What is the primary reason for the acidity of chloroacetic acid compared to acet

What is the primary reason for the acidity of chloroacetic acid compared to acetic acid?

What is the primary reason for the acidity of chloroacetic acid compared to acetic acid?

Step 1: Understand that acidity refers to how easily a substance can donate a proton (H+).
Step 2: Know that acetic acid (CH3COOH) has a methyl group (CH3) attached to the carboxylic acid (-COOH).
Step 3: Recognize that chloroacetic acid (ClCH2COOH) has a chlorine atom (-Cl) attached to the carbon next to the carboxylic acid.
Step 4: Learn about the inductive effect, which is the influence of electronegative atoms (like Cl) on nearby atoms.
Step 5: Realize that the chlorine atom pulls electron density away from the carboxylic acid group in chloroacetic acid.
Step 6: Understand that this electron withdrawal stabilizes the negative charge that forms when the acid donates a proton.
Step 7: Conclude that because chloroacetic acid can stabilize the negative charge better than acetic acid, it is more acidic.

No concepts available.