Textbook Question
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(a) ClO2- or ClO3-
(b) HSO4- or HSeO4-
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Ch.16 - Aqueous Equilibria: Acids & Bases
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 16, Problem 65d
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(d) HS- or Br-
Verified step by step guidance1
Identify the conjugate acids of each base: HS^- is the conjugate base of H2S, and Br^- is the conjugate base of HBr.
Recall that the strength of a base is inversely related to the strength of its conjugate acid. A weaker conjugate acid means a stronger base.
Compare the acid strengths: H2S is a weaker acid than HBr, as HBr is a strong acid and H2S is a weak acid.
Since H2S is weaker than HBr, its conjugate base (HS^-) is stronger than the conjugate base of HBr (Br^-).
Conclude that HS^- is the stronger base compared to Br^- because it is derived from the weaker acid, H2S.
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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, an acid is a proton donor, while a base is a proton acceptor. Understanding this theory is crucial for determining the strength of bases, as it helps identify which species can more readily accept protons.
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Bronsted-Lowry Acid-Base Theory
Conjugate Acid-Base Pairs
Conjugate acid-base pairs consist of two species that differ by the presence of a proton. For example, HS⁻ is the conjugate base of H₂S, while Br⁻ is the conjugate base of HBr. The strength of a base can often be inferred from the strength of its conjugate acid; a stronger conjugate acid corresponds to a weaker base.
Electronegativity and Basicity
Electronegativity refers to the tendency of an atom to attract electrons in a bond. In the context of basicity, a less electronegative atom is generally better at donating electron density to accept protons. Comparing HS⁻ and Br⁻, sulfur is less electronegative than bromine, making HS⁻ a stronger base due to its greater ability to share electron density.
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Related Practice
Textbook Question
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(c) HS- or OH-
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Textbook Question
Identify the stronger acid in each of the following pairs.Explain your reasoning.(b) H3PO4 or H3AsO4
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Textbook Question
Which of the indicators given in Figure 16.5, methyl violet, bromcresol green, phenol red, or thymolphthalein, would be most appropriate to detect a pH change from: (b) 8 to 10?
359
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Textbook Question
Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25
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