Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(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 9c
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(c) 
Verified step by step guidance1
Identify the acid in the given problem and locate the most acidic proton as indicated in the question.
Recall the definition of a conjugate base: it is formed when an acid donates a proton (H⁺). This means you need to remove the most acidic proton from the acid.
Write the chemical structure of the acid and remove the indicated proton. This will result in a species with one less hydrogen atom and a negative charge on the atom that was bonded to the proton.
Ensure that the resulting conjugate base is correctly represented, including the formal charge and any resonance structures if applicable.
Double-check the structure of the conjugate base to confirm that it is consistent with the removal of the most acidic proton and that the negative charge is placed on the appropriate atom.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Conjugate Acid-Base Pair
A conjugate acid-base pair consists of two species that differ by the presence or absence of a proton (H+). When an acid donates a proton, it forms 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 an acid.
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Base Pairing Concept 1
Acidity and pKa
Acidity refers to the tendency of a substance to donate protons, and it is quantitatively expressed by the pKa value. The lower the pKa, the stronger the acid, indicating a greater ability to lose a proton. Recognizing the most acidic proton in a molecule helps in determining which proton will be removed to form the conjugate base.
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Proton Transfer Mechanism
The proton transfer mechanism is a fundamental process in acid-base chemistry where a proton is transferred from an acid to a base. This mechanism is essential for understanding how acids and bases interact in solution, and it aids in predicting the formation of conjugate bases when acids lose protons.
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Related Practice
Textbook Question
Sulfuric acid is a very strong acid. Show how the following equation can be used to explain that sulfuric acid is at once an Arrhenius, Brønsted–Lowry, and Lewis acid.
780
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Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(d)
1157
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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
Sodium amide (NaNH2) dissociates to give a sodium cation (Na+) and amide ion (NH2-) a very strong base. In the following three equations, identify which definition of base is being exemplified.
(c)
1327
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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
views