교과서 질문
Calculate Kb values for CH3COO- and ClO-.
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Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
16장, 문제 77b
Which is the stronger base, the acetate ion or the hypochlorite ion?
검증된 단계별 안내1
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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주요 개념
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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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가이드 코스
02:08
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.
추천 영상:
가이드 코스
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.
추천 영상:
가이드 코스
01:58Comparing Binary Acid Strength
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Given that Kb for ammonia is 1.8 × 10-5 and that for hydroxylamine is 1.1 × 10-8, which is the stronger base?
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Which is the stronger acid, the ammonium ion or the hydroxylammonium ion?
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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?
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