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Exam portage learning chem 103 general chemistry i
module 7 Newest Exam Preparation With Complete
Questions And Correct Answers With Rationales
Already Graded A+Brand New Version!!
1. What is the Arrhenius definition of a base?
A) A substance that produces OH⁻ ions in aqueous solution
B) A substance that produces H⁺ ions in aqueous solution
C) A substance that accepts a proton
D) A substance that donates an electron pair
Answer: A
Explanation: Svante Arrhenius defined bases as substances that
dissociate in water to produce hydroxide ions (OH⁻). Option B describes
an Arrhenius acid. Option C is the Brønsted-Lowry definition of a base.
Option D is the Lewis definition of a base.
2. According to the Brønsted-Lowry theory, an acid is a:
A) Proton donor
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B) Electron pair donor
C) Proton acceptor
D) Hydroxide ion producer
Answer: A
Explanation: The Brønsted-Lowry theory defines an acid as any species
that can donate a proton (H⁺ ion). Option B describes a Lewis base.
Option C describes a Brønsted-Lowry base. Option D describes an
Arrhenius base.
3. What is the pH of a 0.01 M solution of HCl?
A) 1.0
B) 2.0
C) 7.0
D) 12.0
Answer: B
Explanation: Hydrochloric acid (HCl) is a strong acid that dissociates
completely in water. Therefore, the concentration of H⁺ ions equals the
initial concentration of the acid, 0.01 M. pH = -log[H⁺] = -log(0.01) = 2.0.
4. Which of the following is the conjugate base of H₂SO₄?
A) HSO₄⁻
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B) H₃SO₄⁺
C) SO₄²⁻
D) OH⁻
Answer: A
Explanation: The conjugate base of an acid is formed by removing one
proton (H⁺) from the acid. Removing H⁺ from H₂SO₄ yields HSO₄⁻. Option
C would be the conjugate base of HSO₄⁻, not H₂SO₄.
5. What is the sum of pH and pOH for any aqueous solution at 25
degrees Celsius?
A) 14
B) 7
C) 10
D) 0
Answer: A
Explanation: At 25°C, the ion product constant of water (K_w) is 1.0 ×
10⁻¹⁴. Taking the negative logarithm of both sides of K_w = [H⁺][OH⁻]
yields pH + pOH = 14.
6. Which of the following is a polyprotic acid?
A) HCl
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B) HNO₃
C) CH₃COOH
D) H₂SO₄
Answer: D
Explanation: Polyprotic acids have more than one ionizable hydrogen
atom per molecule. Sulfuric acid (H₂SO₄) has two ionizable protons. HCl,
HNO₃, and CH₃COOH are all monoprotic acids.
7. If a solution has a pOH of 3.5, what is its pH?
A) 3.5
B) 7.0
C) 14.0
D) 10.5
Answer: D
Explanation: At 25°C, pH + pOH = 14. Therefore, pH = 14 - pOH = 14 - 3.5
= 10.5.
8. The equivalence point of a titration is defined as:
A) The point where the indicator changes color
B) The point where moles of acid equal moles of base
C) The point where the pH is exactly 7.0
Exam portage learning chem 103 general chemistry i
module 7 Newest Exam Preparation With Complete
Questions And Correct Answers With Rationales
Already Graded A+Brand New Version!!
1. What is the Arrhenius definition of a base?
A) A substance that produces OH⁻ ions in aqueous solution
B) A substance that produces H⁺ ions in aqueous solution
C) A substance that accepts a proton
D) A substance that donates an electron pair
Answer: A
Explanation: Svante Arrhenius defined bases as substances that
dissociate in water to produce hydroxide ions (OH⁻). Option B describes
an Arrhenius acid. Option C is the Brønsted-Lowry definition of a base.
Option D is the Lewis definition of a base.
2. According to the Brønsted-Lowry theory, an acid is a:
A) Proton donor
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B) Electron pair donor
C) Proton acceptor
D) Hydroxide ion producer
Answer: A
Explanation: The Brønsted-Lowry theory defines an acid as any species
that can donate a proton (H⁺ ion). Option B describes a Lewis base.
Option C describes a Brønsted-Lowry base. Option D describes an
Arrhenius base.
3. What is the pH of a 0.01 M solution of HCl?
A) 1.0
B) 2.0
C) 7.0
D) 12.0
Answer: B
Explanation: Hydrochloric acid (HCl) is a strong acid that dissociates
completely in water. Therefore, the concentration of H⁺ ions equals the
initial concentration of the acid, 0.01 M. pH = -log[H⁺] = -log(0.01) = 2.0.
4. Which of the following is the conjugate base of H₂SO₄?
A) HSO₄⁻
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B) H₃SO₄⁺
C) SO₄²⁻
D) OH⁻
Answer: A
Explanation: The conjugate base of an acid is formed by removing one
proton (H⁺) from the acid. Removing H⁺ from H₂SO₄ yields HSO₄⁻. Option
C would be the conjugate base of HSO₄⁻, not H₂SO₄.
5. What is the sum of pH and pOH for any aqueous solution at 25
degrees Celsius?
A) 14
B) 7
C) 10
D) 0
Answer: A
Explanation: At 25°C, the ion product constant of water (K_w) is 1.0 ×
10⁻¹⁴. Taking the negative logarithm of both sides of K_w = [H⁺][OH⁻]
yields pH + pOH = 14.
6. Which of the following is a polyprotic acid?
A) HCl
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B) HNO₃
C) CH₃COOH
D) H₂SO₄
Answer: D
Explanation: Polyprotic acids have more than one ionizable hydrogen
atom per molecule. Sulfuric acid (H₂SO₄) has two ionizable protons. HCl,
HNO₃, and CH₃COOH are all monoprotic acids.
7. If a solution has a pOH of 3.5, what is its pH?
A) 3.5
B) 7.0
C) 14.0
D) 10.5
Answer: D
Explanation: At 25°C, pH + pOH = 14. Therefore, pH = 14 - pOH = 14 - 3.5
= 10.5.
8. The equivalence point of a titration is defined as:
A) The point where the indicator changes color
B) The point where moles of acid equal moles of base
C) The point where the pH is exactly 7.0
