Textbook Question
Write the formula for the conjugate base of each acid. a. H2SO4
Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Chapter 17, Problem 34c
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. c. CO32–(aq) + H2O(l) ⇌ HCO3–(aq) + OH–(aq)
Verified step by step guidance1
Identify the species that donates a proton (H⁺) in the reaction. This species is the Brønsted–Lowry acid.
Identify the species that accepts a proton (H⁺) in the reaction. This species is the Brønsted–Lowry base.
Determine the conjugate acid, which is the species formed when the Brønsted–Lowry base gains a proton.
Determine the conjugate base, which is the species formed when the Brønsted–Lowry acid loses a proton.
Write out the reaction showing the transfer of the proton and label each species as the Brønsted–Lowry acid, base, conjugate acid, and conjugate base.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Brønsted–Lowry Acid-Base Theory
The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework allows for the identification of acid-base reactions based on the transfer of protons (H+ ions) between species. Understanding this theory is essential for analyzing reactions and determining the roles of different substances in the reaction.
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02:08
Bronsted-Lowry Acid-Base Theory
Conjugate Acid-Base Pairs
In the context of Brønsted–Lowry theory, a conjugate acid is formed when a base accepts a proton, while a conjugate base is formed when an acid donates a proton. These pairs are crucial for understanding the equilibrium of acid-base reactions, as they illustrate how substances can interchange roles depending on the reaction conditions.
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01:30Conjugate Acid-Base Pairs
Chemical Equilibrium
Chemical equilibrium refers to the state in which the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In acid-base reactions, this concept helps explain how the presence of acids and bases can shift the equilibrium position, affecting the concentrations of conjugate acids and bases in solution.
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04:21Chemical Equilibrium Concepts
Related Practice
Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. CH3NH2(aq) + H2O(l) ⇌ CH3NH3+(aq) + OH–(aq)
Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH–(aq)
Textbook Question
Write the formula for the conjugate acid of each base. c. HCO3–
Textbook Question
Write the formula for the conjugate base of each acid. b. HBr
Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. d. C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH–(aq)