The pH of 0.1 M solution of the following sa | vedclass

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(A) $HCl$ is a strong acid,so its $pH$ is the lowest $(pH \approx 1)$.$NH_4Cl$ is a salt of a strong acid $(HCl)$ and a weak base $(NH_4OH)$,so it und

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$HCl < NH_4Cl < NaCl < NaCN$

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(A) $HCl$ is a strong acid,so its $pH$ is the lowest $(pH \approx 1)$.$NH_4Cl$ is a salt of a strong acid $(HCl)$ and a weak base $(NH_4OH)$,so it undergoes cationic hydrolysis,resulting in an acidic solution $(pH $NaCl$ is a salt of a strong acid $(HCl)$ and a strong base $(NaOH)$,so it is neutral $(pH = 7)$.$NaCN$ is a salt of a weak acid $(HCN)$ and a strong base $(NaOH)$,so it undergoes anionic hydrolysis,resulting in a basic solution $(pH > 7)$.Therefore,the order of increasing $pH$ is: $HCl < NH_4Cl < NaCl < NaCN$.

The $pH$ of $0.1 \ M$ solution of the following salts increases in the order:

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