Q8 / 60 · KVPY 2014 (SA) · Chemistry

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

  • A
    $\mathrm{NaCl} < \mathrm{CH}_{3} \mathrm{COONa} < \mathrm{NH}_{4} \mathrm{Cl}$
  • Correct answer
    B
    $\mathrm{NH}_{4} \mathrm{Cl} < \mathrm{NaCl} < \mathrm{CH}_{3} \mathrm{COONa}$
  • C
    $\mathrm{NH}_{4} \mathrm{Cl} < \mathrm{CH}_{3} \mathrm{COONa} < \mathrm{Na}^{4} \mathrm{Cl}$
  • D
    $\mathrm{NaCl}^{4} \mid < \mathrm{NH}_{4} \mathrm{Cl} < \mathrm{CH}_{3}^{3} \mathrm{COONa}$

Solution

$\mathrm{NH}_{4} \mathrm{Cl} \rightarrow$ acidic Salt $(P H < 7)$ $\mathrm{NaCl} \rightarrow$ Neutral Salt $(\mathrm{PH}=7)$ $\mathrm{CH}_{3} \mathrm{COONa} \rightarrow$ Basic salt $(\mathrm{PH}>7)$

Hence, the correct answer is option: 'B'.

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