CHEM134 C001 Final Exam Spring 2026 Actual
Exam 2026/2027 | Complete Exam-Style
Questions with Detailed Rationales | Pass
Guaranteed – A+ Graded
SECTION I: Foundational Concepts & Definitions (Brønsted-Lowry
Acid-Base Theory, Amphiprotic Substances, Conjugate Acid-Base
Pairs)
Q1: According to the Brønsted-Lowry definition, an acid is a substance that:
A. donates an electron pair to form a coordinate covalent bond
B. accepts a proton (H⁺) from another substance
C. donates a proton (H⁺) to another substance [CORRECT]
D. increases the concentration of OH⁻ in aqueous solution
Correct Answer: C
Rationale: Correct because the Brønsted-Lowry definition states that an acid is a proton
donor. This matches CHEM134 C001 curriculum on acid-base theory.
Q2: According to the Brønsted-Lowry definition, a base is a substance that:
A. donates a proton (H⁺) to another substance
B. accepts a proton (H⁺) from another substance [CORRECT]
C. donates an electron pair to form a coordinate covalent bond
D. increases the concentration of H⁺ in aqueous solution
Correct Answer: B
Rationale: Correct because the Brønsted-Lowry definition states that a base is a proton
acceptor. This is the fundamental definition taught in CHEM134 C001.
Q3: A substance that can act as both an acid and a base is called:
A. amphoteric
,B. amphiprotic [CORRECT]
C. polyprotic
D. conjugate
Correct Answer: B
Rationale: Correct because amphiprotic substances can both donate and accept
protons, such as H₂O, HCO₃⁻, and H₂PO₄⁻. This matches CHEM134 C001 curriculum.
Q4: Which of the following substances is amphiprotic?
A. HCl
B. NaOH
C. H₂O [CORRECT]
D. NH₄⁺
Correct Answer: C
Rationale: Correct because water can act as a Brønsted-Lowry acid (donating H⁺ to
form OH⁻) or as a base (accepting H⁺ to form H₃O⁺), making it amphiprotic.
Q5: The conjugate base of H₂PO₄⁻ is:
A. H₃PO₄
B. HPO₄²⁻ [CORRECT]
C. PO₄³⁻
D. H₂PO₄²⁻
Correct Answer: B
Rationale: Correct because removing one proton (H⁺) from H₂PO₄⁻ yields HPO₄²⁻. The
conjugate base always has one less H⁺ and one more negative charge.
Q6: In the reaction NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq), the two Brønsted-Lowry
bases are:
A. NH₃ and H₂O
B. NH₄⁺ and OH⁻
C. NH₃ and OH⁻ [CORRECT]
D. H₂O and NH₄⁺
Correct Answer: C
, Rationale: Correct because NH₃ accepts a proton from H₂O to become NH₄⁺, and OH⁻
accepts a proton in the reverse reaction. Both are proton acceptors.
Q7: In the reaction NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq), the two Brønsted-Lowry
acids are:
A. NH₃ and H₂O
B. NH₄⁺ and OH⁻
C. NH₃ and OH⁻
D. H₂O and NH₄⁺ [CORRECT]
Correct Answer: D
Rationale: Correct because H₂O donates a proton to NH₃ to form OH⁻, and NH₄⁺ donates
a proton to OH⁻ in the reverse reaction. Both are proton donors.
Q8: Which of the following is NOT an amphiprotic species?
A. HCO₃⁻
B. H₂PO₄⁻
C. HSO₄⁻
D. SO₄²⁻ [CORRECT]
Correct Answer: D
Rationale: Correct because SO₄²⁻ has no protons to donate and can only accept protons,
making it solely a base, not amphiprotic.
Q9: The conjugate acid of HCO₃⁻ is:
A. CO₃²⁻
B. H₂CO₃ [CORRECT]
C. CO₂
D. HCO₃²⁻
Correct Answer: B
Rationale: Correct because adding one proton (H⁺) to HCO₃⁻ yields H₂CO₃. The
conjugate acid always has one more H⁺ and one less negative charge.
Q10: In the reaction HCO₃⁻ + H₂O ⇌ H₂CO₃ + OH⁻, which species is acting as a
Brønsted-Lowry base?
Exam 2026/2027 | Complete Exam-Style
Questions with Detailed Rationales | Pass
Guaranteed – A+ Graded
SECTION I: Foundational Concepts & Definitions (Brønsted-Lowry
Acid-Base Theory, Amphiprotic Substances, Conjugate Acid-Base
Pairs)
Q1: According to the Brønsted-Lowry definition, an acid is a substance that:
A. donates an electron pair to form a coordinate covalent bond
B. accepts a proton (H⁺) from another substance
C. donates a proton (H⁺) to another substance [CORRECT]
D. increases the concentration of OH⁻ in aqueous solution
Correct Answer: C
Rationale: Correct because the Brønsted-Lowry definition states that an acid is a proton
donor. This matches CHEM134 C001 curriculum on acid-base theory.
Q2: According to the Brønsted-Lowry definition, a base is a substance that:
A. donates a proton (H⁺) to another substance
B. accepts a proton (H⁺) from another substance [CORRECT]
C. donates an electron pair to form a coordinate covalent bond
D. increases the concentration of H⁺ in aqueous solution
Correct Answer: B
Rationale: Correct because the Brønsted-Lowry definition states that a base is a proton
acceptor. This is the fundamental definition taught in CHEM134 C001.
Q3: A substance that can act as both an acid and a base is called:
A. amphoteric
,B. amphiprotic [CORRECT]
C. polyprotic
D. conjugate
Correct Answer: B
Rationale: Correct because amphiprotic substances can both donate and accept
protons, such as H₂O, HCO₃⁻, and H₂PO₄⁻. This matches CHEM134 C001 curriculum.
Q4: Which of the following substances is amphiprotic?
A. HCl
B. NaOH
C. H₂O [CORRECT]
D. NH₄⁺
Correct Answer: C
Rationale: Correct because water can act as a Brønsted-Lowry acid (donating H⁺ to
form OH⁻) or as a base (accepting H⁺ to form H₃O⁺), making it amphiprotic.
Q5: The conjugate base of H₂PO₄⁻ is:
A. H₃PO₄
B. HPO₄²⁻ [CORRECT]
C. PO₄³⁻
D. H₂PO₄²⁻
Correct Answer: B
Rationale: Correct because removing one proton (H⁺) from H₂PO₄⁻ yields HPO₄²⁻. The
conjugate base always has one less H⁺ and one more negative charge.
Q6: In the reaction NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq), the two Brønsted-Lowry
bases are:
A. NH₃ and H₂O
B. NH₄⁺ and OH⁻
C. NH₃ and OH⁻ [CORRECT]
D. H₂O and NH₄⁺
Correct Answer: C
, Rationale: Correct because NH₃ accepts a proton from H₂O to become NH₄⁺, and OH⁻
accepts a proton in the reverse reaction. Both are proton acceptors.
Q7: In the reaction NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq), the two Brønsted-Lowry
acids are:
A. NH₃ and H₂O
B. NH₄⁺ and OH⁻
C. NH₃ and OH⁻
D. H₂O and NH₄⁺ [CORRECT]
Correct Answer: D
Rationale: Correct because H₂O donates a proton to NH₃ to form OH⁻, and NH₄⁺ donates
a proton to OH⁻ in the reverse reaction. Both are proton donors.
Q8: Which of the following is NOT an amphiprotic species?
A. HCO₃⁻
B. H₂PO₄⁻
C. HSO₄⁻
D. SO₄²⁻ [CORRECT]
Correct Answer: D
Rationale: Correct because SO₄²⁻ has no protons to donate and can only accept protons,
making it solely a base, not amphiprotic.
Q9: The conjugate acid of HCO₃⁻ is:
A. CO₃²⁻
B. H₂CO₃ [CORRECT]
C. CO₂
D. HCO₃²⁻
Correct Answer: B
Rationale: Correct because adding one proton (H⁺) to HCO₃⁻ yields H₂CO₃. The
conjugate acid always has one more H⁺ and one less negative charge.
Q10: In the reaction HCO₃⁻ + H₂O ⇌ H₂CO₃ + OH⁻, which species is acting as a
Brønsted-Lowry base?
