Which of the following statements is correct?

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(C) $1$. In aqueous medium,$HCl$ is a stronger acid than $HF$ due to the higher bond dissociation energy of the $H-F$ bond compared to $H-Cl$. Thus,op

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$HNO_3$ is a stronger acid than $HNO_2$.

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(C) $1$. In aqueous medium,$HCl$ is a stronger acid than $HF$ due to the higher bond dissociation energy of the $H-F$ bond compared to $H-Cl$. Thus,option $A$ is incorrect.$2$. The acidity of oxoacids increases with the oxidation state of the central atom. In $HClO_4$,the oxidation state of $Cl$ is $+7$,while in $HClO_3$,it is $+5$. Therefore,$HClO_4$ is a stronger acid than $HClO_3$. Thus,option $B$ is incorrect.$3$. In $HNO_3$,the oxidation state of $N$ is $+5$,and in $HNO_2$,it is $+3$. Higher oxidation state and more resonance-stabilized conjugate base make $HNO_3$ a stronger acid than $HNO_2$. Thus,option $C$ is correct.$4$. $H_2SO_3$ is a stronger acid than $H_3PO_3$ because $S$ is more electronegative than $P$,leading to greater polarization of the $O-H$ bond. Thus,option $D$ is incorrect.

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