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Salt of Strong Acid and Weak Base

40 ml of 0....

Question

$40 m l$ of $0.1 M$ ammonia solution is mixed with $20 m l$ of $0.1 M H C l$ . What is the pH of the mixture?
[Given: $p K_{b}$ of ammonia solution is $4.74$ ]

4.74

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2.26

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9.26

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5.00

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Solution

The correct option is B $9.26$
Volume of the solution= 40 + 20= 60 ml

$N H_{3} + H C l \to N H_{4} C l$

$p O H = p k_{b} + l o g \frac{[S a l t]}{[B a s e]}$

$p O H = 4.74 + l o g \frac{0.1 / 60}{0.1 / 60}$

$p O H = 4.74 + 0 = 4.74$

$p H = 14 - 4.74 = 9.26$

Option (C) is correct.

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