Chem 104 Final Exam (Hill) STUDY GUIDE 2026
COMPLETE QUESTIONS WITH CORRECT
DETAILED ANSWERS || 100% GUARANTEED
PASS <RECENT VERSION>
Chapter 12: Solutions
1. Which of the following is NOT a colligative property?
A. Vapor pressure lowering
B. Boiling point elevation
C. Freezing point depression
D. Increased solubility
2. A solution is prepared by dissolving 10.0 g of glucose (C₆H₁₂O₆, MW=180.2 g/mol) in
250 g of water. What is the molality of the solution?
A. 0.0222 m
B. 0.222 m
C. 0.0400 m
D. 0.400 m
3. The Henry's Law constant for O₂ in water at 25°C is 1.3 x 10⁻³ M/atm. What is the
concentration of O₂ in water exposed to air at 0.21 atm O₂?
A. 2.7 x 10⁻⁴ M
B. 6.2 x 10⁻³ M
C. 1.3 x 10⁻³ M
D. 0.21 M
4. For an ideal solution, which statement is TRUE?
A. ΔH_solution = 0
B. ΔS_solution = 0
C. Raoult's Law is always obeyed for both components.
D. The vapor pressure is always higher than predicted.
5. Case Study: A solution contains 0.100 mol of a nonvolatile, nonelectrolyte solute in
500.0 g of benzene (K_b = 2.53 °C/m, K_f = 5.12 °C/m, normal bp = 80.1°C, normal fp =
5.5°C). What is the boiling point of the solution?
A. 80.1°C
,B. 80.6°C
C. 81.1°C
D. 5.0°C
Chapter 13: Chemical Kinetics
6. For a reaction 2A → B, the rate is found to be Rate = k[A]². What is the overall order
of the reaction?
A. 0
B. 1
C. 2
D. 3
7. The half-life for a first-order reaction is 25.0 minutes. What is the rate constant k (in
min⁻¹)?
A. 0.0277 min⁻¹
B. 0.693 min⁻¹
C. 0.0277 s⁻¹
D. 25.0 min⁻¹
8. Which factor does NOT affect the rate of a chemical reaction?
A. Concentration of reactants
B. Activation energy
C. Temperature
D. Equilibrium constant
9. The Arrhenius equation describes the relationship between:
A. Rate and concentration.
B. Rate constant and temperature.
C. Half-life and initial concentration.
D. Order and molecularity.
10. Case Study: A plot of ln[A] vs. time for a reaction A → products yields a straight line
with a slope of -0.045 s⁻¹. What is the concentration of A after 20.0 seconds if the
initial concentration was 0.50 M?
A. 0.20 M
B. 0.11 M
C. 0.30 M
D. 0.41 M
Chapter 14: Chemical Equilibrium
,11. For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the equilibrium constant expression Kc
is:
A. [NH₃] / ([N₂][H₂])
B. [NH₃]² / ([N₂][H₂]³)
C. 2[NH₃] / (3[H₂][N₂])
D. ([N₂][H₂]³) / [NH₃]²
12. If Kc for a reaction is 1.5 x 10⁻³ at 25°C, what can be said about the reaction at
equilibrium?
A. Products predominate.
B. Reactants predominate.
C. Equal amounts of reactants and products.
D. Cannot determine.
13. Le Chatelier's Principle states that if a stress is applied to a system at equilibrium,
the system will:
A. Shift to counteract the stress.
B. Shift to increase the stress.
C. Remain unchanged.
D. Change the value of K.
14. For which reaction does Kp = Kc?
A. N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
B. H₂(g) + I₂(g) ⇌ 2HI(g)
C. 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
D. CaCO₃(s) ⇌ CaO(s) + CO₂(g)
15. Case Study: For the reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g), Kc = 4.0 at 500 K. An
initial mixture contains 1.0 M CO and 1.0 M H₂O. What is the equilibrium
concentration of CO₂?
A. 0.33 M
B. 0.50 M
C. 0.67 M
D. 0.75 M
Chapter 15: Acids and Bases
16. According to the Brønsted-Lowry definition, an acid is a:
A. Proton donor.
B. Proton acceptor.
, C. Electron pair donor.
D. Hydroxide ion producer.
17. What is the conjugate base of H₂PO₄⁻?
A. H₃PO₄
B. HPO₄²⁻
C. PO₄³⁻
D. H₂PO₄
18. In pure water at 25°C, which is true?
A. [H₃O⁺] = [OH⁻] = 1.0 x 10⁻⁷ M
B. [H₃O⁺] > [OH⁻]
C. pH = 7.0, pOH = 8.0
D. K_w = 1.0 x 10⁻¹⁴ only in acids.
19. Which of the following is a strong acid?
A. HF
B. H₃PO₄
C. HClO₄
D. H₂CO₃
20. Case Study: A 0.10 M solution of a weak acid HA has a pH of 2.87. What is the Ka
for HA?
A. 1.3 x 10⁻³
B. 1.8 x 10⁻⁵
C. 1.3 x 10⁻⁴
D. 1.8 x 10⁻⁴
Chapter 16: Acid-Base Equilibria (Buffers, Titrations)
21. A buffer solution is most effective when:
A. [Acid] >> [Conjugate base]
B. [Acid] = [Conjugate base]
C. pH = 7
D. It contains a strong acid and its salt.
22. The Henderson-Hasselbalch equation for a weak acid buffer is:
A. pH = pKa + log([base]/[acid])
B. pH = pKa - log([acid]/[base])
C. pOH = pKb + log([acid]/[base])
D. pH = -log[H⁺]
COMPLETE QUESTIONS WITH CORRECT
DETAILED ANSWERS || 100% GUARANTEED
PASS <RECENT VERSION>
Chapter 12: Solutions
1. Which of the following is NOT a colligative property?
A. Vapor pressure lowering
B. Boiling point elevation
C. Freezing point depression
D. Increased solubility
2. A solution is prepared by dissolving 10.0 g of glucose (C₆H₁₂O₆, MW=180.2 g/mol) in
250 g of water. What is the molality of the solution?
A. 0.0222 m
B. 0.222 m
C. 0.0400 m
D. 0.400 m
3. The Henry's Law constant for O₂ in water at 25°C is 1.3 x 10⁻³ M/atm. What is the
concentration of O₂ in water exposed to air at 0.21 atm O₂?
A. 2.7 x 10⁻⁴ M
B. 6.2 x 10⁻³ M
C. 1.3 x 10⁻³ M
D. 0.21 M
4. For an ideal solution, which statement is TRUE?
A. ΔH_solution = 0
B. ΔS_solution = 0
C. Raoult's Law is always obeyed for both components.
D. The vapor pressure is always higher than predicted.
5. Case Study: A solution contains 0.100 mol of a nonvolatile, nonelectrolyte solute in
500.0 g of benzene (K_b = 2.53 °C/m, K_f = 5.12 °C/m, normal bp = 80.1°C, normal fp =
5.5°C). What is the boiling point of the solution?
A. 80.1°C
,B. 80.6°C
C. 81.1°C
D. 5.0°C
Chapter 13: Chemical Kinetics
6. For a reaction 2A → B, the rate is found to be Rate = k[A]². What is the overall order
of the reaction?
A. 0
B. 1
C. 2
D. 3
7. The half-life for a first-order reaction is 25.0 minutes. What is the rate constant k (in
min⁻¹)?
A. 0.0277 min⁻¹
B. 0.693 min⁻¹
C. 0.0277 s⁻¹
D. 25.0 min⁻¹
8. Which factor does NOT affect the rate of a chemical reaction?
A. Concentration of reactants
B. Activation energy
C. Temperature
D. Equilibrium constant
9. The Arrhenius equation describes the relationship between:
A. Rate and concentration.
B. Rate constant and temperature.
C. Half-life and initial concentration.
D. Order and molecularity.
10. Case Study: A plot of ln[A] vs. time for a reaction A → products yields a straight line
with a slope of -0.045 s⁻¹. What is the concentration of A after 20.0 seconds if the
initial concentration was 0.50 M?
A. 0.20 M
B. 0.11 M
C. 0.30 M
D. 0.41 M
Chapter 14: Chemical Equilibrium
,11. For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the equilibrium constant expression Kc
is:
A. [NH₃] / ([N₂][H₂])
B. [NH₃]² / ([N₂][H₂]³)
C. 2[NH₃] / (3[H₂][N₂])
D. ([N₂][H₂]³) / [NH₃]²
12. If Kc for a reaction is 1.5 x 10⁻³ at 25°C, what can be said about the reaction at
equilibrium?
A. Products predominate.
B. Reactants predominate.
C. Equal amounts of reactants and products.
D. Cannot determine.
13. Le Chatelier's Principle states that if a stress is applied to a system at equilibrium,
the system will:
A. Shift to counteract the stress.
B. Shift to increase the stress.
C. Remain unchanged.
D. Change the value of K.
14. For which reaction does Kp = Kc?
A. N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
B. H₂(g) + I₂(g) ⇌ 2HI(g)
C. 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)
D. CaCO₃(s) ⇌ CaO(s) + CO₂(g)
15. Case Study: For the reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g), Kc = 4.0 at 500 K. An
initial mixture contains 1.0 M CO and 1.0 M H₂O. What is the equilibrium
concentration of CO₂?
A. 0.33 M
B. 0.50 M
C. 0.67 M
D. 0.75 M
Chapter 15: Acids and Bases
16. According to the Brønsted-Lowry definition, an acid is a:
A. Proton donor.
B. Proton acceptor.
, C. Electron pair donor.
D. Hydroxide ion producer.
17. What is the conjugate base of H₂PO₄⁻?
A. H₃PO₄
B. HPO₄²⁻
C. PO₄³⁻
D. H₂PO₄
18. In pure water at 25°C, which is true?
A. [H₃O⁺] = [OH⁻] = 1.0 x 10⁻⁷ M
B. [H₃O⁺] > [OH⁻]
C. pH = 7.0, pOH = 8.0
D. K_w = 1.0 x 10⁻¹⁴ only in acids.
19. Which of the following is a strong acid?
A. HF
B. H₃PO₄
C. HClO₄
D. H₂CO₃
20. Case Study: A 0.10 M solution of a weak acid HA has a pH of 2.87. What is the Ka
for HA?
A. 1.3 x 10⁻³
B. 1.8 x 10⁻⁵
C. 1.3 x 10⁻⁴
D. 1.8 x 10⁻⁴
Chapter 16: Acid-Base Equilibria (Buffers, Titrations)
21. A buffer solution is most effective when:
A. [Acid] >> [Conjugate base]
B. [Acid] = [Conjugate base]
C. pH = 7
D. It contains a strong acid and its salt.
22. The Henderson-Hasselbalch equation for a weak acid buffer is:
A. pH = pKa + log([base]/[acid])
B. pH = pKa - log([acid]/[base])
C. pOH = pKb + log([acid]/[base])
D. pH = -log[H⁺]
