Textbook Question
(a) The isoelectric point (pI) of phenylalanine is pH 5.5. Draw the structure of the major form of phenylalanine at pH values of 1, 5.5, and 11.
2534
views
Ch. 24 - Amino Acids, Peptides, and Proteins
Wade9th EditionOrganic ChemistryISBN: 9780135213728
Not the one you use?Change textbookSelect a different textbook
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 24, Problem 27c
The isoelectric point of glutamic acid is pH 3.2. Draw the structures of the major forms of glutamic acid at pH values of 1, 3.2, 7, and 11. Explain why the side-chain carboxylic acid is a weaker acid than the acid group next to the α-carbon atom.
Verified step by step guidance1
Step 1: Understand the isoelectric point (pI) of glutamic acid. The isoelectric point is the pH at which the molecule has no net charge. For glutamic acid, this occurs at pH 3.2. At this pH, the amino group (-NH3+) is protonated, the α-carboxylic acid group (-COO-) is deprotonated, and the side-chain carboxylic acid group (-COOH) is also deprotonated.
Step 2: Analyze the structure of glutamic acid at pH 1. At this low pH, the environment is highly acidic, so all acidic groups will be protonated. The amino group will be in its protonated form (-NH3+), the α-carboxylic acid group will be in its protonated form (-COOH), and the side-chain carboxylic acid group will also be in its protonated form (-COOH).
Step 3: Analyze the structure of glutamic acid at pH 3.2. At this pH (the isoelectric point), the amino group remains protonated (-NH3+), the α-carboxylic acid group is deprotonated (-COO-), and the side-chain carboxylic acid group is also deprotonated (-COO-). The molecule has no net charge at this pH.
Step 4: Analyze the structure of glutamic acid at pH 7. At this neutral pH, the amino group remains protonated (-NH3+), the α-carboxylic acid group is deprotonated (-COO-), and the side-chain carboxylic acid group is also deprotonated (-COO-). The molecule carries a net negative charge due to the two deprotonated carboxylate groups.
Step 5: Analyze the structure of glutamic acid at pH 11. At this high pH, the environment is basic, so the amino group will lose its proton and become neutral (-NH2), while both the α-carboxylic acid group and the side-chain carboxylic acid group remain deprotonated (-COO-). The molecule carries a net charge of -2. The side-chain carboxylic acid is a weaker acid than the α-carboxylic acid because the α-carboxylic acid is closer to the electron-withdrawing amino group, which stabilizes the negative charge on the conjugate base, making it easier to lose a proton.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
4mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Isoelectric Point (pI)
The isoelectric point (pI) is the pH at which a molecule, such as an amino acid, carries no net electrical charge. For glutamic acid, this occurs at pH 3.2, where the amino group is protonated, and the carboxyl groups are in their zwitterionic form. Understanding pI is crucial for predicting the charge state of amino acids at different pH levels, which influences their solubility and interactions in biological systems.
Recommended video:
Guided course
03:19
Definition of Isoelectric Point
Acid-Base Properties of Amino Acids
Amino acids possess both acidic and basic functional groups, allowing them to act as buffers in biological systems. The carboxylic acid groups can donate protons (H+), while the amino group can accept protons. The strength of these acids can vary; in glutamic acid, the α-carboxylic acid is stronger than the side-chain carboxylic acid due to the proximity of the α-amino group, which stabilizes the conjugate base formed after deprotonation.
Recommended video:
Guided course
04:10The 7 Ionizable Amino Acids
Structural Forms of Amino Acids at Different pH Levels
The structure of amino acids changes with pH due to protonation and deprotonation of functional groups. At low pH (1), glutamic acid is fully protonated; at its pI (3.2), it exists as a zwitterion; at neutral pH (7), it has a net negative charge; and at high pH (11), it is fully deprotonated. Understanding these structural changes is essential for predicting the behavior of amino acids in various biochemical environments.
Recommended video:
Guided course
11:14Charged Amino Acids
Related Practice
Textbook Question
Propose a mechanism for the coupling of acetic acid and aniline using DCC as a coupling agent.
166
views
Textbook Question
Predict the products of the following reactions.
(b)
1189
views
Textbook Question
Predict the products of the following reactions.
(d)
564
views
Textbook Question
Draw the structure of the phenylthiohydantoin derivatives of
(c) lysine.
839
views
Textbook Question
Predict the products of the following reactions.
(c)
908
views