The percentage of pyridine () that forms pyridinium ion () in a aqueous pyridine solution ( for ) is — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

For a weak base, the degree of dissociation $\alpha = \sqrt{K_b / C}$. Substituting the given values: $\alpha = \sqrt{1.7 \times 10^{-9} / 0.10} = \sqrt{1.7 \times 10^{-8}} \approx 1.3 \times 10^{-4}$. To convert this to a percentage, multiply by 100: $1.3 \times 10^{-4} \times 100 = 1.3 \times 10^{-2}\% = 0.013\%$.