According to the Bronsted-Lowry concept,the c | vedclass

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(C) The relative strength of bases is inversely proportional to the strength of their conjugate acids.$1$. The conjugate acid of $OH^{-}$ is $H_2O$ $(

Vedclass · Accepted Answer

$OH^{-} > CH_3COO^{-} > Cl^{-}$

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(C) The relative strength of bases is inversely proportional to the strength of their conjugate acids.$1$. The conjugate acid of $OH^{-}$ is $H_2O$ $(K_a \approx 10^{-14})$.$2$. The conjugate acid of $CH_3COO^{-}$ is $CH_3COOH$ $(K_a \approx 1.8 	imes 10^{-5})$.$3$. The conjugate acid of $Cl^{-}$ is $HCl$ (a strong acid,$K_a$ is very high).Since the strength of conjugate acids follows the order $HCl > CH_3COOH > H_2O$,the strength of the corresponding conjugate bases follows the reverse order: $OH^{-} > CH_3COO^{-} > Cl^{-}$.

Acid	$K_a$
$HCN$	$6.2 \times 10^{-10}$
$HF$	$7.2 \times 10^{-4}$
$HNO_2$	$4.0 \times 10^{-4}$

According to the Bronsted-Lowry concept,the correct order of relative strength of bases follows the order:

Similar Questions

The conjugate base of $HCO_3^-$ is

Values of dissociation constant,$K_a$ are given as follows:
Acid $K_a$
$HCN$ $6.2 \times 10^{-10}$
$HF$ $7.2 \times 10^{-4}$
$HNO_2$ $4.0 \times 10^{-4}$

Correct order of increasing base strength of the bases $CN^{-}$,$F^{-}$ and $NO_2^-$ will be:

In the following reaction $HCO_3^{-} + H_2O \rightleftharpoons CO_3^{2-} + H_3O^{+}$,which two substances are Bronsted bases?

Which one is not an acid salt?

$HNO_3$ in aqueous solution yields:

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