pg. 1
,CHEM 210 Biochemistry: Module 1–8 & Final Exam Practice Bank (2026/2027)
Note on sourcing: This examination is an original, professionally developed practice test built to
reflect the scope and terminology of Portage Learning CHEM 210 Biochemistry. It is not an actual
Portage Learning exam, and no claim of official verification or “guaranteed pass” is made or
supported. The title supplied in your prompt references third-party study documents; the questions
below are newly written for educational preparation and do not reproduce those documents. Use
this bank alongside your official course materials.
Examination Overview
This 200-question multiple-choice examination covers the full scope of a two-semester
undergraduate biochemistry sequence organized into eight modules plus a comprehensive final
examination. Content includes the chemical foundations of biochemistry (water, pH, buffers,
functional groups), the structure and function of the four major classes of biomolecules
(carbohydrates, lipids, proteins, nucleic acids), enzyme kinetics and inhibition, bioenergetics and
metabolism, and the integration of metabolic pathways. Questions progress from foundational recall
through application, analysis, and clinical/biochemical problem-solving. All questions have a single
best answer and are accompanied by a rationale.
Table of Contents
Section Topic Area Questions
Foundations: Water, pH, Buffers, Functional
1 Q1–Q25
Groups
2 Amino Acids and Protein Structure Q26–Q55
Protein Function: Myoglobin, Hemoglobin,
3 Q56–Q85
Enzymes
4 Carbohydrates and Glycobiology Q86–Q110
5 Lipids, Membranes, and Transport Q111–Q135
Nucleic Acids and Molecular Biology
6 Q136–Q155
Foundations
7 Bioenergetics and Carbohydrate Metabolism Q156–Q180
pg. 2
,Section Topic Area Questions
8 Lipid and Amino Acid Metabolism; Integration Q181–Q195
Comprehensive Final Examination
9 Q196–Q200
(Integrated)
Questions 1–200
SECTION 1: Foundations (Q1–Q25)
Q1. Which property of carbon is most directly responsible for the vast diversity of organic molecules
found in living organisms?
A. Its ability to form ionic bonds with oxygen
B. Its capacity to form four stable covalent bonds and bond to itself in chains and rings
C. Its low atomic mass relative to other biologically relevant elements
D. Its tendency to exist as a diatomic gas under physiological conditions
Correct Answer: B. Its capacity to form four stable covalent bonds and bond to itself in chains and
rings
Rationale: Carbon’s tetravalency and ability to catenate (bond to other carbon atoms) allow for
linear, branched, and cyclic skeletons with diverse functional groups. Ionic bonding (A) is not
characteristic of carbon in biomolecules; low mass (C) is not the primary driver of diversity; and
carbon is not a diatomic gas in biological contexts (D).
Q2. A solution has a hydrogen ion concentration of 2.5×10−52.5×10−5 M. What is its pH?
A. 4.60
B. 5.40
C. 5.00
D. 9.40
Correct Answer: A. 4.60
Rationale: pH = −log(2.5 × 10⁻⁵) = −(log 2.5 + log 10⁻⁵) = −(0.398 − 5) = 4.602. Option B reverses a sign
error; C ignores the coefficient; D is the pOH, not the pH.
Q3. Which statement best explains why water is an effective solvent for ionic compounds?
A. Water has a low dielectric constant, which strengthens ionic interactions.
B. Water’s high polarity and high dielectric constant shield electrostatic interactions between ions.
C. Water forms covalent bonds with dissolved ions, stabilizing them.
D. Water’s nonpolar O–H bonds interact favorably with nonpolar solutes.
pg. 3
, Correct Answer: B. Water’s high polarity and high dielectric constant shield electrostatic
interactions between ions.
Rationale: Water’s high dielectric constant (~78 at 25 °C) reduces the electrostatic attraction
between oppositely charged ions, allowing them to dissociate. A is the opposite of the truth; C is
incorrect because water does not form covalent bonds with simple ions; D is false—O–H bonds are
polar, not nonpolar.
Q4. A buffer is prepared from acetic acid (pKa = 4.76) and sodium acetate. At which pH will this
buffer have the greatest buffering capacity?
A. pH 2.76
B. pH 4.76
C. pH 6.76
D. pH 7.40
Correct Answer: B. pH 4.76
Rationale: Buffering capacity is maximal when pH = pKa because the concentrations of the weak acid
and conjugate base are equal (Henderson–Hasselbalch: pH = pKa + log([A⁻]/[HA]); when [A⁻] = [HA],
log(1) = 0). A and C are ±2 units from the pKa, and D is physiological pH but far from acetate’s pKa.
Q5. Which functional group is present in all amino acids and confers basic properties?
A. Carboxyl group
B. Sulfhydryl group
C. Amino group
D. Hydroxyl group
Correct Answer: C. Amino group
Rationale: The α-amino group (–NH₂, protonated to –NH₃⁺ at physiological pH) is a defining feature
of amino acids and contributes to their basic character. The carboxyl group (A) is acidic, not basic;
sulfhydryl (B) is present only in cysteine; hydroxyl (D) is present in serine, threonine, and tyrosine
but is not universal.
Q6. The Henderson–Hasselbalch equation is pH = pKa + log([A⁻]/[HA]). If a buffer contains 0.10 M
weak acid and 0.010 M conjugate base, and the pKa is 6.0, what is the approximate pH?
A. 5.0
B. 6.0
C. 7.0
D. 8.0
Correct Answer: A. 5.0
Rationale: log(0.010/0.10) = log(0.1) = −1. pH = 6.0 + (−1) = 5.0. B assumes equal concentrations; C
and D incorrectly add rather than subtract the log term.
pg. 4
,CHEM 210 Biochemistry: Module 1–8 & Final Exam Practice Bank (2026/2027)
Note on sourcing: This examination is an original, professionally developed practice test built to
reflect the scope and terminology of Portage Learning CHEM 210 Biochemistry. It is not an actual
Portage Learning exam, and no claim of official verification or “guaranteed pass” is made or
supported. The title supplied in your prompt references third-party study documents; the questions
below are newly written for educational preparation and do not reproduce those documents. Use
this bank alongside your official course materials.
Examination Overview
This 200-question multiple-choice examination covers the full scope of a two-semester
undergraduate biochemistry sequence organized into eight modules plus a comprehensive final
examination. Content includes the chemical foundations of biochemistry (water, pH, buffers,
functional groups), the structure and function of the four major classes of biomolecules
(carbohydrates, lipids, proteins, nucleic acids), enzyme kinetics and inhibition, bioenergetics and
metabolism, and the integration of metabolic pathways. Questions progress from foundational recall
through application, analysis, and clinical/biochemical problem-solving. All questions have a single
best answer and are accompanied by a rationale.
Table of Contents
Section Topic Area Questions
Foundations: Water, pH, Buffers, Functional
1 Q1–Q25
Groups
2 Amino Acids and Protein Structure Q26–Q55
Protein Function: Myoglobin, Hemoglobin,
3 Q56–Q85
Enzymes
4 Carbohydrates and Glycobiology Q86–Q110
5 Lipids, Membranes, and Transport Q111–Q135
Nucleic Acids and Molecular Biology
6 Q136–Q155
Foundations
7 Bioenergetics and Carbohydrate Metabolism Q156–Q180
pg. 2
,Section Topic Area Questions
8 Lipid and Amino Acid Metabolism; Integration Q181–Q195
Comprehensive Final Examination
9 Q196–Q200
(Integrated)
Questions 1–200
SECTION 1: Foundations (Q1–Q25)
Q1. Which property of carbon is most directly responsible for the vast diversity of organic molecules
found in living organisms?
A. Its ability to form ionic bonds with oxygen
B. Its capacity to form four stable covalent bonds and bond to itself in chains and rings
C. Its low atomic mass relative to other biologically relevant elements
D. Its tendency to exist as a diatomic gas under physiological conditions
Correct Answer: B. Its capacity to form four stable covalent bonds and bond to itself in chains and
rings
Rationale: Carbon’s tetravalency and ability to catenate (bond to other carbon atoms) allow for
linear, branched, and cyclic skeletons with diverse functional groups. Ionic bonding (A) is not
characteristic of carbon in biomolecules; low mass (C) is not the primary driver of diversity; and
carbon is not a diatomic gas in biological contexts (D).
Q2. A solution has a hydrogen ion concentration of 2.5×10−52.5×10−5 M. What is its pH?
A. 4.60
B. 5.40
C. 5.00
D. 9.40
Correct Answer: A. 4.60
Rationale: pH = −log(2.5 × 10⁻⁵) = −(log 2.5 + log 10⁻⁵) = −(0.398 − 5) = 4.602. Option B reverses a sign
error; C ignores the coefficient; D is the pOH, not the pH.
Q3. Which statement best explains why water is an effective solvent for ionic compounds?
A. Water has a low dielectric constant, which strengthens ionic interactions.
B. Water’s high polarity and high dielectric constant shield electrostatic interactions between ions.
C. Water forms covalent bonds with dissolved ions, stabilizing them.
D. Water’s nonpolar O–H bonds interact favorably with nonpolar solutes.
pg. 3
, Correct Answer: B. Water’s high polarity and high dielectric constant shield electrostatic
interactions between ions.
Rationale: Water’s high dielectric constant (~78 at 25 °C) reduces the electrostatic attraction
between oppositely charged ions, allowing them to dissociate. A is the opposite of the truth; C is
incorrect because water does not form covalent bonds with simple ions; D is false—O–H bonds are
polar, not nonpolar.
Q4. A buffer is prepared from acetic acid (pKa = 4.76) and sodium acetate. At which pH will this
buffer have the greatest buffering capacity?
A. pH 2.76
B. pH 4.76
C. pH 6.76
D. pH 7.40
Correct Answer: B. pH 4.76
Rationale: Buffering capacity is maximal when pH = pKa because the concentrations of the weak acid
and conjugate base are equal (Henderson–Hasselbalch: pH = pKa + log([A⁻]/[HA]); when [A⁻] = [HA],
log(1) = 0). A and C are ±2 units from the pKa, and D is physiological pH but far from acetate’s pKa.
Q5. Which functional group is present in all amino acids and confers basic properties?
A. Carboxyl group
B. Sulfhydryl group
C. Amino group
D. Hydroxyl group
Correct Answer: C. Amino group
Rationale: The α-amino group (–NH₂, protonated to –NH₃⁺ at physiological pH) is a defining feature
of amino acids and contributes to their basic character. The carboxyl group (A) is acidic, not basic;
sulfhydryl (B) is present only in cysteine; hydroxyl (D) is present in serine, threonine, and tyrosine
but is not universal.
Q6. The Henderson–Hasselbalch equation is pH = pKa + log([A⁻]/[HA]). If a buffer contains 0.10 M
weak acid and 0.010 M conjugate base, and the pKa is 6.0, what is the approximate pH?
A. 5.0
B. 6.0
C. 7.0
D. 8.0
Correct Answer: A. 5.0
Rationale: log(0.010/0.10) = log(0.1) = −1. pH = 6.0 + (−1) = 5.0. B assumes equal concentrations; C
and D incorrectly add rather than subtract the log term.
pg. 4
