Which of the following acids will have the lo | vedclass

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(C) The acidity of carboxylic acids is influenced by the inductive effect of substituents. $1$. $\alpha$-halo acids are stronger than $\beta$-halo aci

Vedclass · Accepted Answer

$BrCH_2CH_2COOH$

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(C) The acidity of carboxylic acids is influenced by the inductive effect of substituents. $1$. $\alpha$-halo acids are stronger than $\beta$-halo acids because the electron-withdrawing group is closer to the carboxyl group. $2$. Fluorine $(F)$ has a stronger electron-withdrawing inductive effect than Bromine $(Br)$. $3$. Comparing the given options: - $CH_3CHFCOOH$ ($\alpha$-fluoro acid) is the strongest. - $CH_3CHBrCOOH$ ($\alpha$-bromo acid) is stronger than $\beta$-substituted acids. - Between $FCH_2CH_2COOH$ and $BrCH_2CH_2COOH$,both are $\beta$-substituted. Since $F$ is more electronegative than $Br$,$FCH_2CH_2COOH$ is stronger than $BrCH_2CH_2COOH$. Therefore,$BrCH_2CH_2COOH$ is the weakest acid and will have the lowest dissociation constant $(K_a)$.

Which of the following acids will have the lowest dissociation constant $(K_a)$?

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The descending order of acidity for the following carboxylic acids is:
$A.$ $CH_3COOH$
$B.$ $F_3C-COOH$
$C.$ $ClCH_2-COOH$
$D.$ $FCH_2-COOH$
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Choose the correct answer from the options given below:

The correct order of acidic strength is:

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