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)
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 14b
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.
(b) 
Verified step by step guidance1
Step 1: Identify the acid and base on the left side of the equation. The acid is the species that donates a proton (H⁺), and the base is the species that accepts the proton. In this reaction, HBr is the acid because it donates a proton, and the alkyne (CH≡CH) is the base because it accepts the proton.
Step 2: Determine the conjugate acid and conjugate base on the right side of the equation. The conjugate acid is the species formed when the base gains a proton, and the conjugate base is the species formed when the acid loses a proton. Here, the conjugate acid is the carbocation (CH₂=CH⁺), and the conjugate base is the bromide ion (Br⁻).
Step 3: Label the acid, base, conjugate acid, and conjugate base in the chemical equation. On the left side, HBr is labeled as the acid, and CH≡CH is labeled as the base. On the right side, CH₂=CH⁺ is labeled as the conjugate acid, and Br⁻ is labeled as the conjugate base.
Step 4: Understand the proton transfer mechanism. The proton (H⁺) from HBr is transferred to the alkyne (CH≡CH), resulting in the formation of the carbocation (CH₂=CH⁺) and bromide ion (Br⁻). This is a typical acid-base reaction.
Step 5: Verify the reaction follows the Bronsted-Lowry acid-base theory. The acid (HBr) donates a proton, and the base (CH≡CH) accepts it, forming the conjugate acid (CH₂=CH⁺) and conjugate base (Br⁻). This confirms the labeling is consistent with the theory.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Brønsted-Lowry Acid-Base Theory
The Brønsted-Lowry theory defines acids as proton donors and bases as proton acceptors. In a chemical reaction, the acid donates a hydrogen ion (H+) to the base, which accepts it. This theory helps in identifying the roles of substances in acid-base reactions, making it essential for labeling acids and bases in chemical equations.
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The Bronsted-Lowry definition of acids and bases.
Conjugate Acid-Base Pairs
A conjugate acid-base pair consists of two species that differ by the presence of a single proton. When an acid donates a proton, it forms its conjugate base, while the base that accepts the proton becomes its conjugate acid. Understanding these pairs is crucial for identifying the products of acid-base reactions and labeling them correctly.
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Chemical Equation Representation
Chemical equations represent the reactants and products of a reaction, showing how substances interact. In the context of acid-base reactions, the left side typically contains the acid and base, while the right side shows the conjugate acid and conjugate base. Familiarity with this representation is vital for accurately labeling the components in the given reactions.
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Related Practice
Textbook Question
Based on the one species that is identified for you, label the remaining molecules as acid, base, conjugate acid, or conjugate base.
(a)
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Textbook Question
Based on the one species that is identified for you, label the remaining molecules as acid, base, conjugate acid, or conjugate base.
(b)
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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
Identify the base from which the following conjugate acids were formed. [The most acidic proton is indicated.]
(c)
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.
(c)