Textbook Question
Use the acid-dissociation constants in Table 16.3 to arrange these oxyanions from strongest base to weakest: SO42-, CO32-, SO32-, and PO43-.
Ch.16 - Acid-Base Equilibria
Chapter 16, Problem 77b
Which is the stronger base, the acetate ion or the hypochlorite ion?
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Identify the chemical formulas for the acetate ion (CH₃COO⁻) and the hypochlorite ion (ClO⁻).
Recall that the strength of a base is related to its ability to accept protons (H⁺) and is inversely related to the strength of its conjugate acid.
Determine the conjugate acids of the acetate ion and the hypochlorite ion: acetic acid (CH₃COOH) and hypochlorous acid (HClO), respectively.
Compare the acid dissociation constants (Ka) of acetic acid and hypochlorous acid. The weaker the conjugate acid (lower Ka), the stronger the base.
Conclude which ion is the stronger base by identifying which conjugate acid has the lower Ka value, indicating a weaker acid and thus a stronger base.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Theory
Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, acids are proton donors and bases are proton acceptors. The strength of a base is determined by its ability to accept protons, which is influenced by the stability of the conjugate acid formed after the base accepts a proton.
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Bronsted-Lowry Acid-Base Theory
Conjugate Acid Stability
The strength of a base is often related to the stability of its conjugate acid. A more stable conjugate acid indicates a stronger base, as the equilibrium will favor the formation of the base. Factors affecting stability include electronegativity, resonance, and inductive effects, which can help predict the relative strengths of different bases.
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01:30Conjugate Acid-Base Pairs
Comparative Base Strengths
To compare the strengths of the acetate ion (CH3COO-) and the hypochlorite ion (ClO-), one must consider their conjugate acids: acetic acid (CH3COOH) and hypochlorous acid (HClO). The relative acidity of these acids can be assessed using pKa values; a higher pKa indicates a weaker acid and thus a stronger conjugate base. This comparison allows for determining which ion is the stronger base.
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Related Practice
Textbook Question
Given that Ka for acetic acid is 1.8 * 10-5 and that for hypochlorous acid is 3.0 * 10-8, which is the stronger acid?
Textbook Question
Calculate Kb values for CH3COO- and ClO-.
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Textbook Question
Given that Kb for ammonia is 1.8 × 10-5 and that for hydroxylamine is 1.1 × 10-8, which is the stronger base?
Textbook Question
Which is the stronger acid, the ammonium ion or the hydroxylammonium ion?