The dissociation constant of formic acid is — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

As derived in the previous step, the acid dissociation constant is calculated using the initial concentrations: $K_a = \frac{[\text{H}^+]^2}{C} = \frac{(8.0 \times 10^{-3})^2}{0.2} = \frac{64 \times 10^{-6}}{0.2} = 320 \times 10^{-6} = 3.2 \times 10^{-4}$. Therefore, correct answer is B.