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 notice the question references specific acid dissociation constants, but the actual $K_a$ values and answer options (A, B, C, D) aren't provided in your prompt. However, I can explain the general principle: **Key Concept:** The strongest acid has the **largest $K_a$ value** (or smallest $pK_a$ value). $$K_a = \frac{[H^+][A^-]}{[HA]}$$ A larger $K_a$ means the acid dissociates more completely, releasing more $H^+$ ions in solution. **To determine the strongest acid:** 1. Compare the given $K_a$ values for all options 2. The acid with the **highest $K_a$** is the strongest 3. Alternatively, calculate $pK_a = -\log K_a$ — the **lowest $pK_a$** indicates the strongest acid **Why A is correct:** Option A must have the largest $K_a$ value (or smallest $pK_a$) compared to options B, C, and D. --- **Please provide the actual $K_a$ values** so I can show the specific numerical comparison and confirm why A is strongest among the given acids.