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UNE GENERAL CHEMISTRY II MIDTERM
EXAMINATION | 300 QUESTIONS AND VERIFIED
ANSWERS | ALREADY GRADED A+ | Plus
RATIONALES | BRAND NEW!
Course Name: General Chemistry II
Course Code: CHEM 1011 / General Chemistry II
Subject: General Chemistry II
Assessment Type: Comprehensive Midterm Practice Examination
Total Questions: 300
SECTION 1 — QUESTIONS 1–100
1. Which property of a solution is directly related to the amount of
dissolved solute particles rather than their chemical identity?
A. Color
B. Density
C. Osmotic pressure
D. Electrical conductivity
❖ Expert Explanation: Osmotic pressure is a colligative property and
depends primarily on the number of dissolved particles present.
2. A solution contains 0.500 mol NaCl dissolved in 2.00 L of solution.
What is its molarity?
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A. 0.100 M
B. 0.250 M
C. 1.00 M
D. 2.50 M
❖ Expert Explanation: Molarity equals moles of solute divided by
liters of solution: 0.500/2.00 = 0.250 M.
3. Which process is most likely to increase the solubility of a solid ionic
compound in water?
A. Decreasing temperature for an endothermic dissolution
B. Removing solvent
C. Increasing temperature when dissolution is endothermic
D. Adding a nonpolar solvent
❖ Expert Explanation: For an endothermic dissolution, adding heat
favors dissolution according to Le Châtelier’s principle.
4. A 25.0-mL sample of 0.200 M HCl is diluted to 100.0 mL. What is the
final concentration?
A. 0.800 M
B. 0.200 M
C. 0.0500 M
D. 0.00500 M
❖ Expert Explanation: Using M₁V₁ = M₂V₂ gives M₂ =
(0.200)(25.0)/100.0 = 0.0500 M.
5. Which substance is expected to have the greatest solubility in water?
A. CH₄
B. C₆H₆
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C. I₂
D. NaNO₃
❖ Expert Explanation: Sodium nitrate is an ionic compound whose
charged particles interact strongly with polar water molecules.
6. A student prepares a solution by dissolving 5.85 g NaCl (58.44 g/mol)
in enough water to make 500.0 mL. What is the approximate molarity?
A. 0.0100 M
B. 0.200 M
C. 0.500 M
D. 2.00 M
❖ Expert Explanation: 5.85/58.44 = 0.100 mol; 0.100 mol/0.500 L =
0.200 M.
7. Which statement best describes a saturated solution?
A. It contains no dissolved solute.
B. It contains only solvent.
C. It contains the maximum dissolved solute at a specified
temperature.
D. It must contain an undissolved solid.
❖ Expert Explanation: Saturation represents equilibrium between
dissolved and undissolved solute at a particular temperature.
8. Which factor generally has the greatest effect on the solubility of a
gas in a liquid?
A. Solute color
B. Pressure
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C. Solute molar mass only
D. Container shape
❖ Expert Explanation: Gas solubility increases as the partial pressure
of that gas above the solution increases.
9. Henry's law relates gas solubility primarily to:
A. Temperature only
B. Volume of the container only
C. Partial pressure of the gas
D. Molecular geometry
❖ Expert Explanation: Henry's law states that dissolved gas
concentration is proportional to the gas's partial pressure above
the solution.
10. Why does carbonated water lose CO₂ more rapidly after a bottle is
opened?
A. CO₂ becomes more polar.
B. Water becomes less dense.
C. The CO₂ partial pressure above the solution decreases.
D. The temperature automatically reaches 0°C.
❖ Expert Explanation: Opening the container lowers CO₂ pressure,
shifting the dissolution equilibrium toward CO₂ escaping from
solution.
11. Which concentration unit is most useful for calculations involving
boiling-point elevation?
A. Mole fraction only
B. Molarity only
UNE GENERAL CHEMISTRY II MIDTERM
EXAMINATION | 300 QUESTIONS AND VERIFIED
ANSWERS | ALREADY GRADED A+ | Plus
RATIONALES | BRAND NEW!
Course Name: General Chemistry II
Course Code: CHEM 1011 / General Chemistry II
Subject: General Chemistry II
Assessment Type: Comprehensive Midterm Practice Examination
Total Questions: 300
SECTION 1 — QUESTIONS 1–100
1. Which property of a solution is directly related to the amount of
dissolved solute particles rather than their chemical identity?
A. Color
B. Density
C. Osmotic pressure
D. Electrical conductivity
❖ Expert Explanation: Osmotic pressure is a colligative property and
depends primarily on the number of dissolved particles present.
2. A solution contains 0.500 mol NaCl dissolved in 2.00 L of solution.
What is its molarity?
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A. 0.100 M
B. 0.250 M
C. 1.00 M
D. 2.50 M
❖ Expert Explanation: Molarity equals moles of solute divided by
liters of solution: 0.500/2.00 = 0.250 M.
3. Which process is most likely to increase the solubility of a solid ionic
compound in water?
A. Decreasing temperature for an endothermic dissolution
B. Removing solvent
C. Increasing temperature when dissolution is endothermic
D. Adding a nonpolar solvent
❖ Expert Explanation: For an endothermic dissolution, adding heat
favors dissolution according to Le Châtelier’s principle.
4. A 25.0-mL sample of 0.200 M HCl is diluted to 100.0 mL. What is the
final concentration?
A. 0.800 M
B. 0.200 M
C. 0.0500 M
D. 0.00500 M
❖ Expert Explanation: Using M₁V₁ = M₂V₂ gives M₂ =
(0.200)(25.0)/100.0 = 0.0500 M.
5. Which substance is expected to have the greatest solubility in water?
A. CH₄
B. C₆H₆
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C. I₂
D. NaNO₃
❖ Expert Explanation: Sodium nitrate is an ionic compound whose
charged particles interact strongly with polar water molecules.
6. A student prepares a solution by dissolving 5.85 g NaCl (58.44 g/mol)
in enough water to make 500.0 mL. What is the approximate molarity?
A. 0.0100 M
B. 0.200 M
C. 0.500 M
D. 2.00 M
❖ Expert Explanation: 5.85/58.44 = 0.100 mol; 0.100 mol/0.500 L =
0.200 M.
7. Which statement best describes a saturated solution?
A. It contains no dissolved solute.
B. It contains only solvent.
C. It contains the maximum dissolved solute at a specified
temperature.
D. It must contain an undissolved solid.
❖ Expert Explanation: Saturation represents equilibrium between
dissolved and undissolved solute at a particular temperature.
8. Which factor generally has the greatest effect on the solubility of a
gas in a liquid?
A. Solute color
B. Pressure
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C. Solute molar mass only
D. Container shape
❖ Expert Explanation: Gas solubility increases as the partial pressure
of that gas above the solution increases.
9. Henry's law relates gas solubility primarily to:
A. Temperature only
B. Volume of the container only
C. Partial pressure of the gas
D. Molecular geometry
❖ Expert Explanation: Henry's law states that dissolved gas
concentration is proportional to the gas's partial pressure above
the solution.
10. Why does carbonated water lose CO₂ more rapidly after a bottle is
opened?
A. CO₂ becomes more polar.
B. Water becomes less dense.
C. The CO₂ partial pressure above the solution decreases.
D. The temperature automatically reaches 0°C.
❖ Expert Explanation: Opening the container lowers CO₂ pressure,
shifting the dissolution equilibrium toward CO₂ escaping from
solution.
11. Which concentration unit is most useful for calculations involving
boiling-point elevation?
A. Mole fraction only
B. Molarity only
