OnlineCBT
Chemistry · EQUILIBRIUM
हिन्दीTwo weak acids \( \text{HA}_1 \) and \( \text{HA}_2 \) have dissociation constants \( K_{a1} = 3.0 \times 10^{-4} \) and \( K_{a2} = 1.2 \times 10^{-5} \) respectively. At equimolar concentrations, what is the ratio of their degrees of dissociation \( \frac{\alpha_1}{\alpha_2} \)?
Correct answer · Option 1
\( 5 : 1 \)
Explanation
For weak electrolytes, \( \alpha = \sqrt{\frac{K_a}{c}} \). Therefore, \( \frac{\alpha_1}{\alpha_2} = \sqrt{\frac{K_{a1}}{K_{a2}}} = \sqrt{\frac{3.0 \times 10^{-4}}{1.2 \times 10^{-5}}} = \sqrt{25} = 5 \).
