CHEM 210 BIOCHEMISTRY
Comprehensive Exam Bank: Modules 1-8 & Final Exam
TABLE OF CONTENTS
Section Module
1 Module 1 Water, pH, and Buffers
2 Module 2 Amino Acids and Proteins
3 Module 3 Protein Structure and Function
4 Module 4 Enzymes and Enzyme Kinetics
5 Module 5 Carbohydrates and Glycobiology
6 Module 6 Lipids and Membranes
7 Module 7 Metabolism: Glycolysis and TCA Cycle
8 Module 8 Oxidative Phosphorylation and Bioenergetics
,MODULE 1 EXAM
Water, pH, and Buffers
Instructions: Choose the BEST answer for each question. Each question is worth 2 points.
1. Which of the following properties of water is MOST responsible for its high boiling point relative to
other molecules of similar molecular weight?
A) Its high specific heat capacity
B) Hydrogen bonding between water molecules
C) Its ability to act as both acid and base
D) Its high dielectric constant
E) Van der Waals interactions
Answer:B
2. The ionization constant of water (Kw) at 25°C is:
A) 1.0 × 10⁻⁷
B) 1.0 × 10⁻¹⁴
C) 1.0 × 10⁻⁷ M²
D) 1.0 × 10⁻¹⁴ M²
E) 7.0 × 10⁻⁸
Answer:D
3. A solution has a hydroxide ion concentration [OH⁻] of 1.0 × 10⁻³ M. What is the pH of this solution?
A) 3
B) 11
C) 7
,D) 4
E) 10
Answer:B
4. Which of the following statements about hydrogen bonds in water is CORRECT?
A) Each water molecule can form a maximum of two hydrogen bonds
B) Hydrogen bonds in water are stronger than covalent O-H bonds
C) Each water molecule can donate two and accept two hydrogen bonds
D) Hydrogen bonds in water are permanent and do not break
E) Only one hydrogen bond can form per water molecule
Answer:C
5. The Henderson-Hasselbalch equation is written as:
A) pH = Ka + log([A⁻]/[HA])
B) pH = pKa + log([HA]/[A⁻])
C) pH = pKa + log([A⁻]/[HA])
D) pH = pKa - log([A⁻]/[HA])
E) pH = pKa × log([A⁻]/[HA])
Answer:C
6. Which of the following is the BEST definition of a buffer?
A) A solution that prevents any pH change
B) A solution that resists changes in pH when small amounts of acid or base are added
C) A solution with a pH of exactly 7.0
D) A solution containing equal concentrations of acid and base
E) A solution that neutralizes all acids and bases
, Answer:B
7. A weak acid (HA) has a pKa of 4.76. What ratio of [A⁻]/[HA] would give a pH of 5.76?
A) 1:1
B) 2:1
C) 10:1
D) 1:10
E) 100:1
Answer:C
8. Which of the following is NOT a noncovalent interaction important in biochemistry?
A) Hydrogen bonds
B) Ionic interactions
C) Peptide bonds
D) Van der Waals interactions
E) Hydrophobic interactions
Answer:C
9. The hydrophobic effect is BEST described as:
A) Attraction between nonpolar molecules and water
B) The tendency of nonpolar molecules to associate with each other in aqueous solution to minimize
disruption of water structure
C) Repulsion between water molecules and polar groups
D) The formation of hydrogen bonds between nonpolar molecules
E) Increased entropy when nonpolar molecules interact with water
Answer:B
Comprehensive Exam Bank: Modules 1-8 & Final Exam
TABLE OF CONTENTS
Section Module
1 Module 1 Water, pH, and Buffers
2 Module 2 Amino Acids and Proteins
3 Module 3 Protein Structure and Function
4 Module 4 Enzymes and Enzyme Kinetics
5 Module 5 Carbohydrates and Glycobiology
6 Module 6 Lipids and Membranes
7 Module 7 Metabolism: Glycolysis and TCA Cycle
8 Module 8 Oxidative Phosphorylation and Bioenergetics
,MODULE 1 EXAM
Water, pH, and Buffers
Instructions: Choose the BEST answer for each question. Each question is worth 2 points.
1. Which of the following properties of water is MOST responsible for its high boiling point relative to
other molecules of similar molecular weight?
A) Its high specific heat capacity
B) Hydrogen bonding between water molecules
C) Its ability to act as both acid and base
D) Its high dielectric constant
E) Van der Waals interactions
Answer:B
2. The ionization constant of water (Kw) at 25°C is:
A) 1.0 × 10⁻⁷
B) 1.0 × 10⁻¹⁴
C) 1.0 × 10⁻⁷ M²
D) 1.0 × 10⁻¹⁴ M²
E) 7.0 × 10⁻⁸
Answer:D
3. A solution has a hydroxide ion concentration [OH⁻] of 1.0 × 10⁻³ M. What is the pH of this solution?
A) 3
B) 11
C) 7
,D) 4
E) 10
Answer:B
4. Which of the following statements about hydrogen bonds in water is CORRECT?
A) Each water molecule can form a maximum of two hydrogen bonds
B) Hydrogen bonds in water are stronger than covalent O-H bonds
C) Each water molecule can donate two and accept two hydrogen bonds
D) Hydrogen bonds in water are permanent and do not break
E) Only one hydrogen bond can form per water molecule
Answer:C
5. The Henderson-Hasselbalch equation is written as:
A) pH = Ka + log([A⁻]/[HA])
B) pH = pKa + log([HA]/[A⁻])
C) pH = pKa + log([A⁻]/[HA])
D) pH = pKa - log([A⁻]/[HA])
E) pH = pKa × log([A⁻]/[HA])
Answer:C
6. Which of the following is the BEST definition of a buffer?
A) A solution that prevents any pH change
B) A solution that resists changes in pH when small amounts of acid or base are added
C) A solution with a pH of exactly 7.0
D) A solution containing equal concentrations of acid and base
E) A solution that neutralizes all acids and bases
, Answer:B
7. A weak acid (HA) has a pKa of 4.76. What ratio of [A⁻]/[HA] would give a pH of 5.76?
A) 1:1
B) 2:1
C) 10:1
D) 1:10
E) 100:1
Answer:C
8. Which of the following is NOT a noncovalent interaction important in biochemistry?
A) Hydrogen bonds
B) Ionic interactions
C) Peptide bonds
D) Van der Waals interactions
E) Hydrophobic interactions
Answer:C
9. The hydrophobic effect is BEST described as:
A) Attraction between nonpolar molecules and water
B) The tendency of nonpolar molecules to associate with each other in aqueous solution to minimize
disruption of water structure
C) Repulsion between water molecules and polar groups
D) The formation of hydrogen bonds between nonpolar molecules
E) Increased entropy when nonpolar molecules interact with water
Answer:B
