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 dissociation constant values aren't shown in your question. However, I can explain the general principle: **To identify the strongest acid, look for the largest $K_a$ value.** The dissociation constant $K_a$ quantifies acid strength: $$K_a = \frac{[H^+][A^-]}{[HA]}$$ A larger $K_a$ means the equilibrium favors ionization, producing more $H^+$ ions, making the acid stronger. **Step-by-step reasoning:** 1. **Compare $K_a$ values** of all given acids 2. **The acid with the highest $K_a$** dissociates most completely in water 3. **Greater dissociation** = greater concentration of $H^+$ ions = stronger acid **Example:** If option A has $K_a = 1.8 \times 10^{-4}$ while others have smaller values like $K_a = 1.3 \times 10^{-5}$, then A is strongest. --- **To verify your answer:** Share the $K_a$ values given in the options, and I can confirm which one corresponds to the strongest acid.