(C) According to the Bronsted-Lowry theory,a base is a proton $(H^+)$ acceptor.In the given options,$NH_{3(aq)}$ acts as a Bronsted-Lowry base because

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(C) According to the Bronsted-Lowry theory,a base is a proton $(H^+)$ acceptor.In the given options,$NH_{3(aq)}$ acts as a Bronsted-Lowry base because it accepts a proton from the water molecule.The reaction is: $H_2O_{(\ell)} + NH_{3(aq)} \rightleftharpoons NH_{4(aq)}^+ + OH^-_{(aq)}$

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium Acids and Bases

Easy

Which of the following compounds accepts a proton from a water molecule according to the Bronsted-Lowry theory?

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A
$NaOH_{(aq)}$
B
$HCl_{(aq)}$
C
$NH_{3(aq)}$
D
$NH_4OH_{(aq)}$

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Chapter

2 Equilibrium: Ionic Equilibrium

Subtopic

Acids and Bases

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The concentration of which ion is decreased when $NH_3$ solution is added?

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What is a Lewis acid?

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The conjugate acid of $HPO_3^{2-}$ is

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Match the following acids in List-$I$ with their respective acid dissociation constants $(K_a)$ in List-$II$:
List-$I$ (Acid) List-$II$ $(K_a)$
$A$. Phenol $I$. $1 \times 10^{-13}$
$B$. Benzoic acid $II$. $3.0 \times 10^{-8}$
$C$. $HClO$ $III$. $1.0 \times 10^{-10}$
$D$. $CH_3COOH$ $IV$. $6.5 \times 10^{-5}$
$V$. $1.75 \times 10^{-5}$

The correct match is:

List-$I$ (Acid)	List-$II$ $(K_a)$
$A$. Phenol	$I$. $1 \times 10^{-13}$
$B$. Benzoic acid	$II$. $3.0 \times 10^{-8}$
$C$. $HClO$	$III$. $1.0 \times 10^{-10}$
$D$. $CH_3COOH$	$IV$. $6.5 \times 10^{-5}$
	$V$. $1.75 \times 10^{-5}$