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Question

The $$pH$$ of $$0.1$$M aqueous solutions of $$NaCl$$, $$CH_3COONa$$ and $$NH_4Cl$$ will follow the order:


A
NaCl<CH3COONa<NH4Cl
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B
NH4Cl<NaCl<CH3COONa
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C
NH4Cl<CH3COONa<NaCl
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D
NaCl<NH4Cl<CH3COONa
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Solution

The correct option is C $$NH_4Cl < NaCl < CH_3COONa$$
The order of pH is $$\displaystyle NH_4Cl \text {( less than 7)}  <  NaCl  (7) < CH_3COONa  \text {( more than 7)} $$
Hence, the option (B) is correct answer.
$$\displaystyle NH_4Cl $$ is a salt of weak base and strong acid. Its solution is acidic.
$$\displaystyle CH_3COONa   $$  is a salt of weak acid and strong base. Its solution is basic.
$$\displaystyle NaCl$$  is a salt of strong base and strong acid. Its solution is neutral.

Chemistry

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