Which of the following is most acidic?

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(B) The acidity of carboxylic acids depends on the stability of the conjugate base (carboxylate ion). Electron-withdrawing groups $(EWG)$ stabilize th

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Chloroacetic acid

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(B) The acidity of carboxylic acids depends on the stability of the conjugate base (carboxylate ion). Electron-withdrawing groups $(EWG)$ stabilize the carboxylate ion through the inductive effect ($-I$ effect),thereby increasing acidity.$1$. $CH_3CH_2COOH$ (Propionic acid): Contains an electron-donating alkyl group ($+I$ effect),which decreases acidity.$2$. $CH_3COOH$ (Acetic acid): Contains a methyl group ($+I$ effect),which is less electron-donating than the ethyl group in propionic acid.$3$. $HCOOH$ (Formic acid): No alkyl group attached to the carboxyl group.$4$. $ClCH_2COOH$ (Chloroacetic acid): Contains a chlorine atom,which is a strong electron-withdrawing group ($-I$ effect). This significantly stabilizes the carboxylate ion,making it the most acidic among the given options.

Similar Questions

Arrange the following compounds in increasing order of their acidic strength:
$(A)$ $CH_3COOH$
$(B)$ $Ph-CH_2-COOH$
$(C)$ $Br-CH_2-COOH$
$(D)$ $O_2N-CH_2-COOH$

Assign the structure of the major product $(X)$ of the reaction given below:
$C_6H_5-CH(OH)-COOH$ $\xrightarrow{CH_3CH_2OH, HCl(g), \Delta}$ $\xrightarrow{SOCl_2, \Delta} (X)$

Which among the following has the lowest boiling point?

The product of the Perkin reaction is:

Which among the following compounds has the highest boiling point?

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