Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(c)
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 9a
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(a) 
Verified step by step guidance1
Identify the acid in the problem: The given acid is H₃O⁺ (hydronium ion), and the most acidic proton is indicated by the arrow.
Recall the definition of a conjugate base: The conjugate base is formed when the acid donates a proton (H⁺).
Remove the most acidic proton (H⁺) from H₃O⁺. This results in the chemical species H₂O (water).
Verify the charge: When H₃O⁺ loses a proton (H⁺), the positive charge is neutralized, resulting in a neutral molecule, H₂O.
Conclude that the conjugate base of H₃O⁺ is H₂O, as it is the species formed after the loss of the most acidic proton.
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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 forms its conjugate base, while the species that accepts the proton becomes the conjugate acid. Understanding these pairs is essential for predicting the outcome of acid-base reactions.
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Base Pairing Concept 1
Acidity and pKa
Acidity refers to the tendency of a substance to donate protons in a solution. The strength of an acid is often measured by its pKa value, which is the negative logarithm of its acid dissociation constant (Ka). A lower pKa indicates a stronger acid, meaning it more readily donates protons, which is crucial for identifying the most acidic proton in a molecule.
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07:45Identifying pKa values
Hydronium Ion (H3O+)
The hydronium ion (H3O+) is formed when an acid donates a proton to water, resulting in a positively charged ion. It is a key player in acid-base chemistry, as it represents the presence of protons in aqueous solutions. Recognizing H3O+ is vital for determining the conjugate base formed when it loses a proton, which in this case would be water (H2O).
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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.
Textbook Question
What is the conjugate base of each of the following acids? [The most acidic proton is indicated.]
(d)
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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.
(b)
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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)
Textbook Question
What is the conjugate acid of each of the following bases? [The most basic atom is indicated.]
(a)
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