Textbook Question
The following compounds can all react as bases.
a. For each compound, show its conjugate acid. Show any resonance forms if applicable.
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Ch. 2 - Acids and Bases; Functional Groups
Wade9th EditionOrganic ChemistryISBN: 9780135213728
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Table of contents
- Ch.1 - Structure and Bonding107
- Ch. 2 - Acids and Bases; Functional Groups115
- Ch.3 - Structure and Stereochemistry of Alkanes100
- Ch.4 - The Study of Chemical Reactions99
- Ch.5 - Stereochemistry93
- Ch.6 - Alkyl Halides; Nucleophilic Substitution118
- Ch. 7 - Structure and Synthesis of Alkenes; Elimination158
- Ch.8 - Reactions of Alkenes171
- Ch.9 - Alkynes91
- Ch.10 - Structure and Synthesis of Alcohols143
- Ch.11 - Reactions of Alcohols104
- Ch. 12 - Infrared Spectroscopy and Mass Spectrometry22
- Ch. 13 - Nuclear Magnetic Resonance Spectroscopy45
- Ch. 14 - Ethers, Epoxides, and Thioethers72
- Ch. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy89
- Ch. 16 - Aromatic Compounds74
- Ch. 17 - Reactions of Aromatic Compounds126
- Ch. 18 - Ketones and Aldehydes193
- Ch. 19 - Amines129
- Ch. 20 - Carboxylic Acids77
- Ch. 21 - Carboxylic Acid Derivatives141
- Ch. 22 - Condensations and Alpha Substitutions of Carbonyl Compounds175
- Ch. 23 - Carbohydrates and Nucleic Acids93
- Ch. 24 - Amino Acids, Peptides, and Proteins54
Chapter 2, Problem 45c
The following compounds can all react as acids.
c. Rank the original compounds in order, from strongest acid to weakest acid.
Verified step by step guidance1
Identify the functional groups in each compound: CH3COOH, CF3COOH, CF3CH2COOH, and CH3CH2OH. The first three are carboxylic acids, and the last one is an alcohol.
Understand that the acidity of a compound is influenced by the stability of its conjugate base. A more stable conjugate base corresponds to a stronger acid.
Consider the effect of electronegative substituents on acidity. Electronegative groups, like CF3, can stabilize the conjugate base through inductive effects, increasing acidity.
Rank the compounds based on the presence and position of electronegative groups: CF3COOH has the strongest electron-withdrawing group directly attached to the carboxyl group, making it the strongest acid.
Compare the remaining compounds: CF3CH2COOH is next due to the electron-withdrawing effect of CF3, followed by CH3COOH, and finally CH3CH2OH, which is the weakest acid due to the lack of electron-withdrawing groups and being an alcohol.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acidity and pKa
Acidity refers to the ability of a compound to donate a proton (H+) in a chemical reaction. The strength of an acid is often measured by its pKa value; lower pKa values indicate stronger acids. Understanding the relationship between structure and acidity is crucial for ranking acids, as factors like electronegativity and resonance can significantly influence a compound's ability to stabilize the negative charge after deprotonation.
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07:45
Identifying pKa values
Inductive Effect
The inductive effect describes how the presence of electronegative atoms or groups in a molecule can influence the acidity of nearby protons. Electronegative atoms, such as fluorine, can withdraw electron density through sigma bonds, stabilizing the negative charge on the conjugate base formed after deprotonation. This effect is particularly important in determining the relative acidity of compounds with different substituents.
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01:47Understanding the Inductive Effect.
Resonance Stabilization
Resonance stabilization occurs when a molecule can distribute its electron density across multiple structures, leading to increased stability of the conjugate base. In the context of acidity, compounds that can delocalize the negative charge through resonance after losing a proton will generally be stronger acids. Recognizing which structures can participate in resonance is essential for ranking the acidity of the given compounds.
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03:43The radical stability trend.
Related Practice
Textbook Question
The following compounds can all react as bases.
c. Rank the original compounds in order, from strongest base to weakest base.
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Textbook Question
The following compounds can all react as acids.
a. For each compound, show its conjugate base. Show any resonance forms if applicable. b. Rank the conjugate bases in the order you would predict, from most stable to least stable.
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Textbook Question
Compare the relative acidity of 1-molar aqueous solutions of the following acids.
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Textbook Question
Consider the following proposed Brønsted–Lowry acid–base reactions. In each case, draw the products of a transfer of the most acidic proton on the acid to the most basic site on the base. Use Appendix 4 to find or estimate the pKa values for the acids and the pKb values for the bases. Then determine which side of the reaction is favored, either reactants or products.
(a)
(b)
2188
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Textbook Question
The following compounds can all react as bases.
b. Rank the conjugate acids in the order you would predict, from most stable to least stable.
623
views