Textbook Question
Write the formula for the conjugate acid of each base. a. NH3 b. ClO4– c. HSO4– d. CO32–
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Ch.17 - Acids and Bases
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving93
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities44
- Ch.5 - Introduction to Solutions and Aqueous Solutions69
- Ch.6 - Gases97
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom48
- Ch.9 - Periodic Properties of the Elements73
- Ch.10 - Chemical Bonding I: The Lewis Model76
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory70
- Ch.12 - Liquids, Solids & Intermolecular Forces41
- Ch.13 - Solids & Modern Materials40
- Ch.14 - Solutions76
- Ch.15 - Chemical Kinetics90
- Ch.16 - Chemical Equilibrium56
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium127
- Ch.19 - Free Energy & Thermodynamics78
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry60
- Ch.22 - Organic Chemistry115
Chapter 17, Problem 37b
Write the formula for the conjugate base of each acid. b. H2SO3
Verified step by step guidance1
Identify the acid given in the problem: \( \text{H}_2\text{SO}_3 \).
Recall that a conjugate base is formed by removing one proton (\( \text{H}^+ \)) from the acid.
Remove one \( \text{H}^+ \) from \( \text{H}_2\text{SO}_3 \) to form the conjugate base.
After removing \( \text{H}^+ \), the remaining species is \( \text{HSO}_3^- \).
Thus, the formula for the conjugate base of \( \text{H}_2\text{SO}_3 \) is \( \text{HSO}_3^- \).
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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 base is formed when an acid donates a proton (H+). The relationship between an acid and its conjugate base is fundamental to understanding acid-base reactions, as it illustrates how substances can interchange between donating and accepting protons.
Sulfurous Acid (H2SO3)
Sulfurous acid (H2SO3) is a weak diprotic acid that can donate two protons. When it loses one proton, it forms its conjugate base, bisulfite (HSO3-), and if it loses both protons, it forms sulfite (SO3^2-). Understanding the structure and behavior of sulfurous acid is essential for identifying its conjugate base.
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Acid-Base Equilibrium
Acid-base equilibrium refers to the balance between acids and their conjugate bases in solution. This concept is crucial for predicting the direction of acid-base reactions and understanding the strength of acids and bases, which is determined by their ability to donate or accept protons in a chemical reaction.
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Related Practice
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)
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Textbook Question
Write the formula for the conjugate base of each acid. d. HF
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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)
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Textbook Question
Write the formula for the conjugate base of each acid. c. HCHO2
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Textbook Question
Write the formula for the conjugate base of each acid. a. HCl
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