A weak monobasic acid has undergone dissociation to the extent of $2 %$ when the concentration is 0.01M at 250C. Calculate the dissociation constant of the acid.

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Solution

The correct option is C

$\begin{matrix} H A ⇌ H^{+} + A^{-} c (1 - α) c α c α 0.01 (1.0 - 0.02) 0.01 \times 0.02 0.01 \times 0.02 \end{matrix} K_{B} = \frac{c^{2} α^{2}}{c (1 - α)} = \frac{c α^{2}}{1 - α} = \frac{0.01 \times (0.02)^{2}}{1 - 0.02} = 4.08 \times 10^{- 6}$

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