Textbook Question
Using the convention that the acid and base are on the left side of the chemical equation, label the acid, base, conjugate acid, and conjugate base in the following reactions.
(a)
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Ch. 4 - Acids and Bases: Electron Flow
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
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Table of contents
- Ch. 2 - General Chemistry Translated: Finding the Electrons114
- Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis109
- Ch. 4 - Acids and Bases: Electron Flow144
- Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics118
- Ch. 6 - Stereoisomerism: Arrangement of Atoms in Space112
- Ch. 7 - Principles of Green (Organic) Chemistry3
- Ch. 8 - Alkenes I: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes II: Oxidation and Reduction150
- Ch. 10 - Alkynes: Electrophilic Addition and Redox Reactions101
- Ch. 11 - Properties and Synthesis of Alkyl Halides: Radical Reactions108
- Ch. 12 - Substitution and Elimination: Reactions of Haloalkanes172
- Ch. 13 - Alcohols, Ethers and Related Compounds: Substitution and Elimination239
- Ch. 14 - Structural Identification I: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification II: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution I: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution II: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems I: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems II: Pericyclic Reactions54
- Ch. 23 - Benzene I: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene II: Reactions Influenced by the Aromatic Ring62
- Ch. 25 - Amines: Structure, Reactions, and Synthesis27
- Ch. 26 - Amino Acids, Proteins, and Peptide Synthesis9
- Ch. 27 - Carbohydrates, Nucleic Acids, and Lipids54
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Not the one you use?Change textbook
Chapter 3, Problem 11d
Identify the acid from which the following conjugate bases were formed. [The most basic atom is indicated.]
(d) 
Verified step by step guidance1
Step 1: Recognize that the given structure represents the conjugate base of an acid. The conjugate base is formed when the acid donates a proton (H⁺).
Step 2: Analyze the structure provided. The image shows a chloride ion (Cl⁻), which is the conjugate base of hydrochloric acid (HCl).
Step 3: Recall the relationship between acids and their conjugate bases. Hydrochloric acid (HCl) donates a proton to form the chloride ion (Cl⁻).
Step 4: Understand that the most basic atom indicated in the image is the chloride ion (Cl⁻), which is negatively charged and stable due to its full octet of electrons.
Step 5: Conclude that the acid from which this conjugate base was formed is hydrochloric acid (HCl).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Conjugate Acids and Bases
In acid-base chemistry, a conjugate base is formed when an acid donates a proton (H+). The relationship between acids and their conjugate bases is fundamental, as it helps to understand the strength and behavior of acids in reactions. For example, when hydrochloric acid (HCl) donates a proton, it forms its conjugate base, Cl-. Identifying the original acid from a given conjugate base is crucial for understanding acid-base equilibria.
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Equilibrium constant and conjugates.
Acid Strength and Basicity
The strength of an acid is determined by its ability to donate protons, while the basicity of its conjugate base is determined by its ability to accept protons. Strong acids have weak conjugate bases, and vice versa. In the context of the question, recognizing the most basic atom in the conjugate base can help identify the original acid, as it indicates the proton that was lost during the acid-base reaction.
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06:21Understanding the difference between basicity and nucleophilicity.
Lewis Structures and Electron Configuration
Lewis structures are diagrams that represent the bonding between atoms and the lone pairs of electrons in a molecule. Understanding how to draw and interpret Lewis structures is essential for visualizing the electron distribution in acids and their conjugate bases. In the provided image, the arrangement of electrons around the chlorine atom can help deduce its behavior as an acid or base, aiding in the identification of the original acid.
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Related Practice
Textbook Question
Identify the acid from which the following conjugate bases were formed. [The most basic atom is indicated.]
(c)
1135
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Textbook Question
What is the conjugate acid of each of the following bases? [The most basic atom is indicated.]
(d)
933
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Textbook Question
When an atom loses a proton in an acid–base reaction, its formal charge is decreased by one. Thinking about the equation for calculating formal charge, explain this observation in your own words.
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Textbook Question
What is the conjugate acid of each of the following bases? [The most basic atom is indicated.]
(a)
1237
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Textbook Question
Identify the base from which the following conjugate acids were formed. [The most acidic proton is indicated.]
(c)
1158
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