The values of dissociation constants of some acids (at 25°C) are as follows. Indicate which is the s — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

I don't see the specific dissociation constant values or options listed in your question. However, I can explain the principle: **To identify the strongest acid:** The **strongest acid has the largest $K_a$ value** (or smallest $pK_a$). $$K_a = \frac{[H^+][A^-]}{[HA]}$$ A larger $K_a$ means the acid dissociates more completely, releasing more $H^+$ ions and thus being stronger. Alternatively, using $pK_a$: $$pK_a = -\log K_a$$ The **strongest acid has the smallest $pK_a$** (most negative or least positive value). **Example reasoning:** - If option A has $K_a = 1.8 \times 10^{-4}$ (or $pK_a ≈ 3.74$) - And other options have $K_a$ values like $10^{-5}$, $10^{-6}$, etc. - Then **A is strongest** because $10^{-4} > 10^{-5}$ (larger $K_a$) **Please provide the actual $K_a$ values** from your question, and I can confirm which acid is strongest and explain why the others are weaker.