Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(d)
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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 11c
Identify the acid from which the following conjugate bases were formed. [The most basic atom is indicated.]
(c) 
Verified step by step guidance1
Step 1: Understand the concept of conjugate bases. A conjugate base is formed when an acid donates a proton (H⁺). To identify the acid, you need to add a proton back to the conjugate base.
Step 2: Examine the structure of the conjugate base provided in the problem. Identify the most basic atom, as this is the site where the proton was removed.
Step 3: Add a proton (H⁺) to the most basic atom in the conjugate base. This will reverse the deprotonation process and reconstruct the original acid.
Step 4: Write the chemical formula or structure of the acid formed after adding the proton. Ensure the valency and bonding are correct.
Step 5: Verify the acid by considering its chemical properties and ensuring it matches the expected acid that corresponds to the given conjugate base.
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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 concept is crucial for identifying conjugate acids and bases, as the conjugate base is formed when an acid donates a proton.
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The Lewis definition of acids and bases.
Conjugate Acid-Base Pairs
Conjugate acid-base pairs consist of two species that differ by the presence or absence of a proton. When an acid donates a proton, it becomes its conjugate base, and the base that accepts the proton becomes its conjugate acid. Recognizing these pairs helps in determining the original acid from which a conjugate base is derived.
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Basicity and Electronegativity
Basicity refers to the ability of a species to accept protons, which is influenced by the electronegativity of the atoms involved. The most basic atom in a conjugate base is typically the one that can stabilize the negative charge most effectively. Understanding the relationship between basicity and electronegativity is essential for identifying the original acid based on the properties of its conjugate base.
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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.]
(d)
1
views
Textbook Question
What is the conjugate acid of each of the following bases? [The most basic atom is indicated.]
(d)
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)
1
views
Textbook Question
Identify the base from which the following conjugate acids were formed. [The most acidic proton is indicated.]
(c)