(B) The strength of an acid is determined by its ability to donate protons ($H^+$ ions) in an aqueous solution. $H_2SO_4$ (sulfuric acid) is a strong

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(B) The strength of an acid is determined by its ability to donate protons ($H^+$ ions) in an aqueous solution. $H_2SO_4$ (sulfuric acid) is a strong mineral acid that undergoes complete dissociation in water. $H_3PO_4$ and $HNO_2$ are weak acids,and $CH_3COOH$ is a weak organic acid. Therefore,$H_2SO_4$ is the strongest acid among the given options.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Acids and Bases

Easy

Which of the following is the strongest acid?

A
$H_3PO_4$
B
$H_2SO_4$
C
$HNO_2$
D
$CH_3COOH$

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Class 11

Chemistry Questions

Chapter

6-2.Equilibrium-II (Ionic Equilibrium)

Subtopic

Acids and Bases

In the following ionic equilibrium,the conjugate acid of $H_2O_2$ is ........
$H_2O_2 + H_2O \rightleftharpoons H_3O^+ + HO_2^-$

Medium

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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	$II$. $3.0 \times 10^{-8}$
$C$. $HClO$	$III$. $1.0 \times 10^{-10}$
$D$. $CH_3COOH$	$IV$. $6.5 \times 10^{-5}$
	$V$. $1.75 \times 10^{-5}$