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Standard XII

Chemistry

Basic Buffer Action

A weak acid ...

Question

A weak acid $H A$ is found to be $10 %$ ionized in $0.01 M$ aqueous solution. Calculate the pH of a solution which is $0.1 M$ in $H A$ and $0.05 M$ in $N a A$ .

5.365

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6.355

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3.653

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6.593

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Solution

The correct option is D $3.653$
$α = 0.1 a n d C = 0.01 M$

$K_{a} = \frac{α^{2} C}{1 - α} = \frac{{(0.1)}^{2} \times (0.01)}{1 - 0.1} = 1.11 \times 10^{- 4}$

$p K_{a} = - log 1.11 \times 10^{- 4} = 3.9542$

$p H = p K_{a} + log \frac{[s a l t]}{[a c i d]}$

$= 3.9542 + log [\frac{0.05}{0.10}] = 3.653$

Option (C) is correct.

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A weak acid HA is found to be 10% ionized in 0.01 M aqueous solution. Calculate the pH of a solution which is 0.1 M in HA and 0.05 M in NaA.

The correct option is D 3.653α=0.1 and C=0.01 MKa=α2C1−α=(0.1)2×(0.01)1−0.1=1.11×10−4pKa=−log1.11×10−4=3.9542pH=pKa+log[salt][acid]=3.9542+log[0.050.10]=3.653Option (C) is correct.

A weak acid $H A$ is found to be $10 %$ ionized in $0.01 M$ aqueous solution. Calculate the pH of a solution which is $0.1 M$ in $H A$ and $0.05 M$ in $N a A$ .