In the context of your question, a strong acid will produce a greater number of \( \text{H}_3\text{O}^+ \) ions at equilibrium compared to a weak base when the same quantity of each solute is added to water.
Explanation:
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Strong Acid: A strong acid completely dissociates in water. For example, if you add hydrochloric acid (\( \text{HCl} \)), it will dissociate completely into \( \text{H}^+ \) (or \( \text{H}_3\text{O}^+ \)) and \( \text{Cl}^- \). Therefore, all of the acid will contribute to the \( \text{H}_3\text{O}^+ \) concentration, resulting in a high concentration of hydronium ions.
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Weak Base: A weak base partially accepts protons from water, resulting in fewer \( \text{H}_3\text{O}^+ \) ions compared to a strong acid. Because the weak base does not fully dissociate, the amount of \( \text{H}_3\text{O}^+ \) generated will be significantly less than the amount produced by a strong acid.
Hence, the conclusion is that a strong acid will yield the greatest number of \( \text{H}_3\text{O}^+ \) ions at equilibrium.