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(D) The strength of an acid is directly proportional to its acid dissociation constant,$K_a$.From the given data,$HI$ has the highest $K_a$ value $(3

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$HI$

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(D) The strength of an acid is directly proportional to its acid dissociation constant,$K_a$.From the given data,$HI$ has the highest $K_a$ value $(3 	imes 10^{11})$,which makes it the strongest Bronsted acid among the series.According to the Bronsted-Lowry theory,the conjugate base of a strong acid is a weak base,and the conjugate base of a very strong acid is the weakest.Therefore,since $HI$ is the strongest acid,its conjugate base $(I^-)$ is the weakest conjugate base.

Acid	$HF$	$HCl$	$HBr$	$HI$
$K_a$	$7.2 \times 10^{-4}$	$1 \times 10^6$	$1 \times 10^9$	$3 \times 10^{11}$

Consider the following data for a series of hydrogen halide Bronsted acids:-

Acid $HF$ $HCl$ $HBr$ $HI$

$K_a$ $7.2 \times 10^{-4}$ $1 \times 10^6$ $1 \times 10^9$ $3 \times 10^{11}$

Which of these Bronsted acids would have the weakest conjugate base?

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Consider the following data for a series of hydrogen halide Bronsted acids:- Acid $HF$ $HCl$ $HBr$ $HI$ $K_a$ $7.2 \times 10^{-4}$ $1 \times 10^6$ $1 \times 10^9$ $3 \times 10^{11}$ Which of these Bronsted acids would have the weakest conjugate base?