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The pH of 0.1 M aqueous solutions of $\mathrm{NaCl}, \mathrm{CH}_{3} \mathrm{COONa}$ and $\mathrm{NH}_{4} \mathrm{Cl}$ will follow the order
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The correct answer is:
$\mathrm{NH}_{4} \mathrm{Cl} < \mathrm{NaCl} < \mathrm{CH}_{3} \mathrm{COONa}$
$\mathrm{NH}_{4} \mathrm{Cl} \rightarrow$ acidic Salt $(P H < 7)$
$\mathrm{NaCl} \rightarrow$ Neutral Salt $(\mathrm{PH}=7)$
$\mathrm{CH}_{3} \mathrm{COONa} \rightarrow$ Basic salt $(\mathrm{PH}>7)$
$\mathrm{NaCl} \rightarrow$ Neutral Salt $(\mathrm{PH}=7)$
$\mathrm{CH}_{3} \mathrm{COONa} \rightarrow$ Basic salt $(\mathrm{PH}>7)$
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