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Arrehenius Theory of Acids and Bases

20 mL of 0.1 ...

Question

20 mL of 0.1 M $H_{2} S O_{4}$ solution is added to 30 mL of 0.2 M $N H_{4} O H$ solution. The pH of the resultant mixture is: [ $p K_{b}$ of $N H_{4} O H$ = 4.7]

9.4

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5.02

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9.0

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5.2

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Solution

The correct option is C 9.0
$20 m L o f 0.1 M H_{2} S O_{4} \Rightarrow n_{H +} = 4 m m o l 30 m L o f 0.2 M N H_{4} O H \Rightarrow n_{N H_{4} O H} = 6 m m o l$

The given mixture is basic buffer

$p O H = p K_{b} + l o g \frac{[N H_{4}^{+}]}{[N H_{4} O H]} = 4.7 + l o g 2 = 4.7 + 0.3 = 5$
$p H = 14 - 5 = 9$

Hence, option (c) is correct.

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