The pH of 0.1M aqueous solutions of NaCl, $C H_{3}$ COONa and $N H_{4}$ Cl 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 B
$N H_{4} C l < N a C l < C H_{3} C O O N a$

$N H_{4}$ Cl $\to$ acidic Salt (PH<7)

NaCl $\to$ Neutral Salt (PH = 7)

$C H_{3}$ COONa $\to$ Basic salt (PH>7)

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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

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Which of the following salt solutions ( $0.1 M$ each) will have the lowest pH values?

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