The $p H$ of $0.1$ M aqueous solutions of $N a C l$ , $C H_{3} C O O N a$ and $N H_{4} C l$ will follow the order:

N a C l < C H_{3} C O O N a < N H_{4} C l

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N H_{4} C l < N a C l < C H_{3} C O O N a

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N H_{4} C l < C H_{3} C O O N a < N a C l

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N a C l < N H_{4} C l < C H_{3} C O O N a

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Solution

The correct option is C $N H_{4} C l < N a C l < C H_{3} C O O N a$
The order of pH is $N H_{4} C l ( less than 7) < N a C l (7) < C H_{3} C O O N a ( more than 7)$
Hence, the option (B) is correct answer.
$N H_{4} C l$ is a salt of weak base and strong acid. Its solution is acidic.
$C H_{3} C O O N a$ is a salt of weak acid and strong base. Its solution is basic.
$N a C l$ is a salt of strong base and strong acid. Its solution is neutral.

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The pH of 0.1M aqueous solutions of NaCl, $C H_{3}$ COONa and $N H_{4}$ Cl will follow the order

C H_{3} C O O N a + C H_{3} C O O H

N a C l + N a O H

N H_{4} C l + N H_{4} O H

N a_{2} S O_{4} + H_{2} S O_{4}

N H_{3}

N H_{4} C l

C H_{3} C O O H

C H_{3} C O O N a

H C l

N a C l

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