Textbook Question
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)
Ch.16 - Acids and Bases
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Chapter 16, Problem 37a
Write the formula for the conjugate base of each acid. a. HCl
Verified step by step guidance1
Identify the acid in the problem: HCl.
Recall that a conjugate base is formed by removing a proton (H⁺) from the acid.
Remove one hydrogen ion (H⁺) from HCl, which leaves you with Cl⁻.
Recognize that the remaining species, Cl⁻, is the conjugate base of HCl.
Write the formula for the conjugate base: Cl⁻.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Conjugate Acid-Base Pairs
In acid-base chemistry, a conjugate acid-base pair consists of two species that differ by the presence of a proton (H+). When an acid donates a proton, it transforms into its conjugate base, while the base that accepts the proton becomes its conjugate acid. Understanding this relationship is crucial for identifying the conjugate base of any given acid.
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Conjugate Acid-Base Pairs
Strong Acids and Their Conjugate Bases
Strong acids, such as hydrochloric acid (HCl), completely dissociate in water, meaning they release all their protons. The conjugate base of a strong acid is typically a weak base, which does not readily accept protons. For HCl, the conjugate base is Cl-, which is stable and does not react significantly with water to form HCl again.
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Chemical Notation and Formulas
Chemical notation is a system of symbols used to represent elements and compounds. The formula for a conjugate base is derived from the acid's formula by removing one hydrogen atom and adjusting the charge accordingly. For HCl, the removal of H+ results in the formula Cl-, indicating the chloride ion as the conjugate base.
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Related Practice
Textbook Question
Write the formula for the conjugate base of each acid. d. HF
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
Write the formula for the conjugate base of each acid. c. HCHO2
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Write the formula for the conjugate base of each acid. b. H2SO3
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)