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(D) The $pH$ of the aqueous solution of these salts depends on the strength of the corresponding conjugate acid formed upon hydrolysis.When these salt

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$NaClO_{4}$

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(D) The $pH$ of the aqueous solution of these salts depends on the strength of the corresponding conjugate acid formed upon hydrolysis.When these salts react with water,they form $NaOH$ (a strong base) and the corresponding oxoacid of chlorine.The reactions are:$NaClO + H_{2}O \rightarrow NaOH + HClO$$NaClO_{2} + H_{2}O \rightarrow NaOH + HClO_{2}$$NaClO_{3} + H_{2}O \rightarrow NaOH + HClO_{3}$$NaClO_{4} + H_{2}O \rightarrow NaOH + HClO_{4}$Since $NaOH$ is common to all,the $pH$ is determined by the acidity of the resulting acid.$HClO_{4}$ is the strongest acid among the given options $(HClO Therefore,the solution of $NaClO_{4}$ will have the highest concentration of $H^{+}$ ions,resulting in the lowest $pH$ value.

The aqueous solution of the following salt will have the lowest $pH$:

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