(B) According to the $BRONSTED-LOWRY$ theory,an acid is a proton donor and a base is a proton acceptor.In the reaction: $HCl_{(aq)} + H_2O_{(l)} \righ

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(B) According to the $BRONSTED-LOWRY$ theory,an acid is a proton donor and a base is a proton acceptor.In the reaction: $HCl_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O_{(aq)}^{+} + Cl_{(aq)}^{-}$$HCl$ acts as $Acid-1$ and donates a proton to $H_2O$,which acts as $Base-2$.After donating the proton,$HCl$ becomes $Cl^-$ $(Base-1)$ and $H_2O$ becomes $H_3O^+$ $(Acid-2)$.Therefore,$H_2O_{(l)}$ is the base $2$.

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium Acids and Bases

Medium

Identify base $2$ for the following equation according to the $BRONSTED-LOWRY$ theory.
$HCl_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O_{(aq)}^{+} + Cl_{(aq)}^{-}$

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A
$H_3O_{(aq)}^{+}$
B
$H_2O_{(l)}$
C
$Cl_{(aq)}^{-}$
D
$HCl_{(aq)}$

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Chapter

2 Equilibrium: Ionic Equilibrium

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Acids and Bases

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

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

Identify base $2$ for the following equation according to the $BRONSTED-LOWRY$ theory.$HCl_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O_{(aq)}^{+} + Cl_{(aq)}^{-}$

Similar Questions

Would gaseous $HCl$ be considered as an Arrhenius acid?

Which among the following is the conjugate base of $HClO_4$?

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:

What is the increasing order of basic strength for $Cl^{-}, CH_3COO^{-}, OH^{-},$ and $F^{-}$?

Which of the following are Lewis acids? $H_2O, BF_3, H^{+}, NH_4^{+}$

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Identify base $2$ for the following equation according to the $BRONSTED-LOWRY$ theory.
$HCl_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O_{(aq)}^{+} + Cl_{(aq)}^{-}$

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: