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Salt of Strong Acid and Weak Base

40 ml of 0.1 ...

Question

40 ml of 0.1 M ammonia solution is mixed with 20 mL of 0.1 M HCl. What is the pH of a mixture? ( $p K_{b}$ of ammonia solution is 4.74)

A

4.74

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B

2.26

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C

9.26

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D

5

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Solution

The correct option is C 9.26

At half stage of titration, $[s a l t] = [b a s e]$
Use the Henderson - Hasselbalch Equation:
$p O H = p K_{b} + l o g [\frac{[salt]}{[base]}]$
$p O H = p K_{b} + l o g [\frac{[N H_{4} C l]}{[N H_{3}]}]$
$p O H = p K_{b} = 4.74 (∵ [s a l t] = [b a s e])$
$∴ p H = 14 - p O H$
$p H = 14 - 4.74 = 9.26$

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Salt of Strong Acid and Weak Base

Standard XII Chemistry

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