Rank the solutions in order of decreasing [H₃O⁺]: 0.10 M HCl; 0.10 M HF; 0.10 M HClO; 0.10 M HC₆H₅O.

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Identify that HCl is a strong acid, which means it completely dissociates in water, producing a high concentration of \([H_3O^+]\).

Recognize that HF, HClO, and HC6H5O are weak acids, which do not completely dissociate in water, resulting in lower \([H_3O^+]\) compared to strong acids.

Understand that the strength of weak acids can be compared using their acid dissociation constants \(K_a\). The larger the \(K_a\), the stronger the acid, and the higher the \([H_3O^+]\).

Research or recall the \(K_a\) values for HF, HClO, and HC6H5O to determine their relative strengths.

Rank the solutions based on the \([H_3O^+]\) concentration, starting with the highest for the strong acid and then in order of decreasing \(K_a\) for the weak acids.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Strong vs. Weak Acids

Strong acids, like HCl, completely dissociate in water, producing a high concentration of hydronium ions (H3O+). In contrast, weak acids, such as HF and HClO, only partially dissociate, resulting in a lower concentration of H3O+. Understanding this distinction is crucial for ranking the solutions based on their acidity.

Concentration of Solutions

The concentration of an acid solution, expressed in molarity (M), indicates the amount of acid present in a given volume of solution. In this question, all solutions have the same concentration of 0.10 M, but their ability to produce H3O+ varies based on their strength as acids, affecting the final ranking.

Acid Dissociation Constant (Ka)

The acid dissociation constant (Ka) quantifies the strength of a weak acid in solution. A higher Ka value indicates a stronger acid that dissociates more in water, leading to a greater concentration of H3O+. For the weak acids in the question, knowing their Ka values helps determine their relative acidity and thus their ranking based on H3O+ concentration.

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