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Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.16 - Acid-Base EquilibriaProblema 5b
Capitolo 16, Problema 5b

The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+.(b) Which acid would have the smallest aciddissociation constant, Ka?
Diagrams of three acids, HA, HB, and HC, showing their molecular structures for acid dissociation analysis.

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Identify the degree of dissociation for each acid by counting the number of dissociated ions (H+ and the corresponding anion) in each diagram.
Compare the number of dissociated ions for each acid. The acid with the fewest dissociated ions has the smallest degree of dissociation.
Recall that the acid dissociation constant, Ka, is a measure of the strength of an acid in solution. A smaller degree of dissociation indicates a weaker acid and thus a smaller Ka value.
Determine which acid (HA, HB, or HC) has the smallest degree of dissociation based on the diagrams.
Conclude that the acid with the smallest degree of dissociation has the smallest Ka value.

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Acid Dissociation Constant (Ka)

The acid dissociation constant, Ka, quantifies the strength of an acid in solution. It is defined as the equilibrium constant for the dissociation of an acid into its conjugate base and a proton (H+). A higher Ka value indicates a stronger acid that dissociates more completely in solution, while a lower Ka value suggests a weaker acid with less dissociation.
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Characteristics of Ka and Kb

Strength of Acids

The strength of an acid is determined by its ability to donate protons (H+) in an aqueous solution. Strong acids, such as hydrochloric acid (HCl), dissociate completely, while weak acids, like acetic acid (CH3COOH), only partially dissociate. The relative strength of the acids represented in the diagrams can be inferred from their molecular structures and the presence of electronegative atoms that stabilize the conjugate base.
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Binary Acid Strengths

Molecular Structure and Electronegativity

The molecular structure of an acid, including the presence of electronegative atoms, significantly influences its acidity. Electronegativity affects the stability of the conjugate base formed after dissociation; more electronegative atoms can stabilize negative charge better, leading to a stronger acid. Analyzing the diagrams, one can assess which acid has a structure that would likely result in a lower Ka value based on these principles.
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Electronegativity Trends
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