CHEM134 C002 DIGITAL TITRATION OF ACIDS &
BASES (BEYOND LABZ) SPRING 2026 UPDATED |
Fully Solved Lab Answers, Step-by-Step Solutions
& Verified Results | INSTANT PDF DOWNLOAD
• This document contains 200 fully solved, verified multiple-choice questions for
CHEM134 Digital Titration of Acids & Bases (Beyond Labz), complete with bolded
correct answers and detailed EXPERT RATIONALE for every question.
• Use it by attempting each question independently first, then checking the
highlighted answer and EXPERT RATIONALE below it to solidify your understanding
of every concept tested.
CHEM134 C002 – SPRING 2026
DIGITAL TITRATION OF ACIDS & BASES – BEYOND LABZ
200 FULLY SOLVED MULTIPLE CHOICE QUESTIONS
SECTION 1: ACID-BASE THEORIES
1. Which acid-base theory defines an acid as a proton donor and a base as a
proton acceptor?
A) Arrhenius theory
B) Lewis theory
C) Lux-Flood theory
D) Solvent system theory
E) Brønsted-Lowry theory
✓ Correct Answer: E) Brønsted-Lowry theory
EXPERT RATIONALE: Brønsted-Lowry (1923) defines acids as H⁺ donors and bases
as H⁺ acceptors. This is broader than Arrhenius, which restricts acids and bases to
aqueous solutions only.
,2. According to the Arrhenius definition, which of the following is classified as
a base?
A) HCl dissolved in water
B) CH₃COOH dissolved in water
C) CO₂ dissolved in water
D) NaOH dissolved in water
E) NH₄Cl dissolved in water
✓ Correct Answer: D) NaOH dissolved in water
EXPERT RATIONALE: Arrhenius bases produce OH⁻ ions in aqueous solution. NaOH
dissociates completely to give Na⁺ and OH⁻, fitting the Arrhenius base definition
perfectly.
3. In the Lewis acid-base theory, a Lewis acid is defined as:
A) A proton donor
B) A hydroxide ion producer
C) An electron pair acceptor
D) An electron pair donor
E) A substance that increases pH
✓ Correct Answer: C) An electron pair acceptor
EXPERT RATIONALE: Lewis acids accept electron pairs to form coordinate covalent
bonds. This definition is the broadest of all acid-base theories and includes species
that have no protons at all (e.g., BF₃).
4. Which of the following is the conjugate base of H₂SO₄?
,A) SO₄²⁻
B) H₃SO₄⁺
C) HSO₄⁻
D) H₂O
E) OH⁻
✓ Correct Answer: C) HSO₄⁻
EXPERT RATIONALE: When H₂SO₄ donates one proton, it becomes HSO₄⁻, which is
its conjugate base. The conjugate base always has one fewer proton than the
parent acid.
5. In the reaction NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, which species is acting as the
Brønsted-Lowry acid?
A) NH₃
B) H₂O
C) NH₄⁺
D) OH⁻
E) None of the above
✓ Correct Answer: B) H₂O
EXPERT RATIONALE: H₂O donates a proton to NH₃, making it the Brønsted-Lowry
acid in this reaction. NH₃ accepts the proton and is therefore the base.
6. What is the conjugate acid of the base NH₃?
A) NH₂⁻
B) N₂H₄
C) NH₄⁺
, D) NH₂OH
E) H₂N⁻
✓ Correct Answer: C) NH₄⁺
EXPERT RATIONALE: A conjugate acid is formed when a base gains a proton. NH₃ +
H⁺ → NH₄⁺. Therefore NH₄⁺ is the conjugate acid of NH₃.
7. Water acting as both an acid and a base in the autoionization reaction is an
example of:
A) Hydrolysis
B) Neutralization
C) Amphoterism
D) Disproportionation
E) Conjugation
✓ Correct Answer: C) Amphoterism
EXPERT RATIONALE: An amphoteric substance can act as either an acid or a base.
Water autoionizes: H₂O + H₂O ⇌ H₃O⁺ + OH⁻, where one water molecule donates a
proton (acid) and one accepts it (base).
8. Which of the following pairs represents a conjugate acid-base pair?
A) HCl and NaOH
B) H₂SO₄ and SO₄²⁻
C) CH₃COOH and CH₃COO⁻
D) NH₃ and OH⁻
E) H₃O⁺ and H₂O₂
✓ Correct Answer: C) CH₃COOH and CH₃COO⁻
BASES (BEYOND LABZ) SPRING 2026 UPDATED |
Fully Solved Lab Answers, Step-by-Step Solutions
& Verified Results | INSTANT PDF DOWNLOAD
• This document contains 200 fully solved, verified multiple-choice questions for
CHEM134 Digital Titration of Acids & Bases (Beyond Labz), complete with bolded
correct answers and detailed EXPERT RATIONALE for every question.
• Use it by attempting each question independently first, then checking the
highlighted answer and EXPERT RATIONALE below it to solidify your understanding
of every concept tested.
CHEM134 C002 – SPRING 2026
DIGITAL TITRATION OF ACIDS & BASES – BEYOND LABZ
200 FULLY SOLVED MULTIPLE CHOICE QUESTIONS
SECTION 1: ACID-BASE THEORIES
1. Which acid-base theory defines an acid as a proton donor and a base as a
proton acceptor?
A) Arrhenius theory
B) Lewis theory
C) Lux-Flood theory
D) Solvent system theory
E) Brønsted-Lowry theory
✓ Correct Answer: E) Brønsted-Lowry theory
EXPERT RATIONALE: Brønsted-Lowry (1923) defines acids as H⁺ donors and bases
as H⁺ acceptors. This is broader than Arrhenius, which restricts acids and bases to
aqueous solutions only.
,2. According to the Arrhenius definition, which of the following is classified as
a base?
A) HCl dissolved in water
B) CH₃COOH dissolved in water
C) CO₂ dissolved in water
D) NaOH dissolved in water
E) NH₄Cl dissolved in water
✓ Correct Answer: D) NaOH dissolved in water
EXPERT RATIONALE: Arrhenius bases produce OH⁻ ions in aqueous solution. NaOH
dissociates completely to give Na⁺ and OH⁻, fitting the Arrhenius base definition
perfectly.
3. In the Lewis acid-base theory, a Lewis acid is defined as:
A) A proton donor
B) A hydroxide ion producer
C) An electron pair acceptor
D) An electron pair donor
E) A substance that increases pH
✓ Correct Answer: C) An electron pair acceptor
EXPERT RATIONALE: Lewis acids accept electron pairs to form coordinate covalent
bonds. This definition is the broadest of all acid-base theories and includes species
that have no protons at all (e.g., BF₃).
4. Which of the following is the conjugate base of H₂SO₄?
,A) SO₄²⁻
B) H₃SO₄⁺
C) HSO₄⁻
D) H₂O
E) OH⁻
✓ Correct Answer: C) HSO₄⁻
EXPERT RATIONALE: When H₂SO₄ donates one proton, it becomes HSO₄⁻, which is
its conjugate base. The conjugate base always has one fewer proton than the
parent acid.
5. In the reaction NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, which species is acting as the
Brønsted-Lowry acid?
A) NH₃
B) H₂O
C) NH₄⁺
D) OH⁻
E) None of the above
✓ Correct Answer: B) H₂O
EXPERT RATIONALE: H₂O donates a proton to NH₃, making it the Brønsted-Lowry
acid in this reaction. NH₃ accepts the proton and is therefore the base.
6. What is the conjugate acid of the base NH₃?
A) NH₂⁻
B) N₂H₄
C) NH₄⁺
, D) NH₂OH
E) H₂N⁻
✓ Correct Answer: C) NH₄⁺
EXPERT RATIONALE: A conjugate acid is formed when a base gains a proton. NH₃ +
H⁺ → NH₄⁺. Therefore NH₄⁺ is the conjugate acid of NH₃.
7. Water acting as both an acid and a base in the autoionization reaction is an
example of:
A) Hydrolysis
B) Neutralization
C) Amphoterism
D) Disproportionation
E) Conjugation
✓ Correct Answer: C) Amphoterism
EXPERT RATIONALE: An amphoteric substance can act as either an acid or a base.
Water autoionizes: H₂O + H₂O ⇌ H₃O⁺ + OH⁻, where one water molecule donates a
proton (acid) and one accepts it (base).
8. Which of the following pairs represents a conjugate acid-base pair?
A) HCl and NaOH
B) H₂SO₄ and SO₄²⁻
C) CH₃COOH and CH₃COO⁻
D) NH₃ and OH⁻
E) H₃O⁺ and H₂O₂
✓ Correct Answer: C) CH₃COOH and CH₃COO⁻
