SCH3U GRADE 11 CHEMISTRY UNIT 3 SOLUTIONS
TEST |COMPLETE QUESTIONS AND WORKED
ANSWERS | ONTARIO VIRTUAL SCHOOL | 2026.
90 Questions with Answers and Detailed Rationales
100 PERCENT GUARANTEED PASS
INSTANT DOWNLOAD ANSWERS INCLUDED
IMPORTANCE OF THIS DOCUMENT
This comprehensive examination preparation guide has been meticulously developed to help you succeed in the
SCH3U GRADE 11 CHEMISTRY UNIT 3 SOLUTIONS TEST |COMPLETE QUESTIONS AND WORKED
ANSWERS | ONTARIO VIRTUAL SCHOOL | 2026.. It contains 90 carefully selected questions that reflect the
most current exam content and testing strategies. Each question is accompanied by a correct answer and a
detailed rationale that explains the underlying pathophysiology, pharmacology, or clinical reasoning.
Self-Assessment – Test your knowledge and Exam Preparation – Familiarize yourself with the
identify areas requiring further question format and content
study areas
Concept Reinforcement – Deepen your Confidence Building – Develop test-taking
understanding through strategies and reduce
evidence-based exam anxiety
rationales
Time Management – Practice answering
questions under simulated
exam conditions
Review Summary 90 Questions
Foundations - Application - Sch3u Grade 11 Chemistry UNIT 3 Solutions Complete AND Worked Ontario
Virtual School 2026 Sch3u Grade 11 Chemistry UNIT 3 Solutions Complete AND Worked Ontario Virtual
School 2026 University
All answers with rationales
,Table of Contents
Content Area Questions Key Topics
Solutions AND Their 1-15 Solution, Water, Solubility, Prepared, Resulting
Properties
Concentration AND Molarity 16-30 Solution, Solubility, Water, First, Molar
Solubility AND Factors 31-45 Solution, Water, Solubility, Prepared, Dissolving
Affecting Solubility
Solution Stoichiometry 46-60 Solution, Point, Water, Prepared, Mixing
Dilutions AND Preparing 61-75 Solution, Solubility, Prepared, Water, Mixing
Solutions
Electrolytes AND 76-90 Solution, Solubility, Water, Statements, Point
Nonelectrolytes
TOTAL 90 All questions include answers and detailed rationales
,Section A - Solutions AND Their Properties
Q1.
A solution is prepared by dissolving 58.44 g of NaCl in 500.0 g of water. The density of the
resulting solution is 1.12 g/mL. Calculate the molality of the solution.
A. 1.00 m B. 2.00 m
C. 0.500 m D. 1.50 m
Correct: B - 2.00 m
Rationale:Moles of NaCl = 58.44 g / 58.44 g/mol = 1.00 mol. Mass of water = 0.500 kg.
Molality = 1.00 mol / 0.500 kg = 2.00 m. Option A uses kg of solution instead of solvent; C
uses total mass incorrectly; D is a miscalculation.
Q2.
Which of the following processes is endothermic when a solute dissolves in water, yet the
overall dissolution is spontaneous?
A. Ion-dipole attractions between solute and B. The entropy change of the system is
water are weaker than solute-solute and negative, but the enthalpy change is highly
water-water attractions. exothermic.
C. The enthalpy of hydration is negative and D. The entropy increase of the surroundings
the lattice energy is positive, with the due to heat release compensates for a
hydration energy exceeding the lattice decrease in system entropy.
energy.
Correct: A - Ion-dipole attractions between solute and water are weaker than solute-solute
and water-water attractions.
Rationale:Dissolution can be endothermic (”H positive) if the energy cost to separate solute
and solvent exceeds the energy released on mixing, but spontaneity arises from a large
positive entropy change (S positive). Option B is endothermic but non-spontaneous unless
entropy compensates; C describes an exothermic process; D incorrectly attributes
spontaneity to surroundings in an endothermic case.
Q3.
A 0.10 M solution of a weak acid HA has a pH of 3.50. What is the percent ionization of
HA?
A. 0.32% B. 3.2%
C. 0.032% D. 0.50%
Page 3
, Section A - Solutions AND Their Properties
Correct: A - 0.32%
Rationale:[H+] = 10^-3.50 = 3.16 × 10^-4 M. Percent ionization = ([H+]/[HA]0) × 100 = (3.16 ×
10^-.10) × 100 = 0.316% 0.32%. Option B uses 10^-pH as a percentage without dividing
by concentration; C is a decimal error; D is an arbitrary value.
Q4.
Which of the following 0.10 M aqueous solutions will have the highest boiling point?
A. NaCl B. CaCl2
C. C6H12O6 (glucose) D. CH3COOH (acetic acid)
Correct: B - CaCl2
Rationale:Boiling point elevation depends on the van't Hoff factor (i). CaCl2 dissociates into 3
ions (i=3), giving the highest effective particle concentration. NaCl has i=2, glucose i=1, and
acetic acid partially ionizes (i1.0). Therefore CaCl2 produces the greatest boiling point
elevation.
Q5.
A student prepares a saturated solution of PbCl2 in pure water and measures [Pb2+] =
0.016 M. What is the Ksp of PbCl2?
A. 1.6 × 10^-5 B. 4.1 × 10^-6
C. 2.6 × 10^-4 D. 1.0 × 10^-5
Correct: A - 1.6 × 10^-5
Rationale:PbCl2(s) !Ì Pb2+ + 2Cl-. If [Pb2+] = 0.016 M, then [Cl-] = 2 × 0.016 = 0.032 M. Ksp
= [Pb2+][Cl-]^2 = 0.016 × (0.032)^2 = 1.64 × 10^-5 1.6 × 10^-5. Option B cubes the
concentration; C uses wrong stoichiometry; D is a miscalculation.
Q6.
Which of the following best explains why a solution of NaCl in water conducts electricity,
but a solution of sucrose in water does not?
A. NaCl is a strong electrolyte, dissociating B. NaCl is a covalent compound that forms
into ions, while sucrose is a non-electrolyte, charged particles in solution, while sucrose
remaining as neutral molecules. is ionic and remains neutral.
C. Water molecules break down NaCl into D. Sucrose dissolves by forming hydrogen
charged particles, but they cannot break bonds, which prevents any charged species
down sucrose because it is too large. from forming.
Correct: A - NaCl is a strong electrolyte, dissociating into ions, while sucrose is a
non-electrolyte, remaining as neutral molecules.
Page 4
TEST |COMPLETE QUESTIONS AND WORKED
ANSWERS | ONTARIO VIRTUAL SCHOOL | 2026.
90 Questions with Answers and Detailed Rationales
100 PERCENT GUARANTEED PASS
INSTANT DOWNLOAD ANSWERS INCLUDED
IMPORTANCE OF THIS DOCUMENT
This comprehensive examination preparation guide has been meticulously developed to help you succeed in the
SCH3U GRADE 11 CHEMISTRY UNIT 3 SOLUTIONS TEST |COMPLETE QUESTIONS AND WORKED
ANSWERS | ONTARIO VIRTUAL SCHOOL | 2026.. It contains 90 carefully selected questions that reflect the
most current exam content and testing strategies. Each question is accompanied by a correct answer and a
detailed rationale that explains the underlying pathophysiology, pharmacology, or clinical reasoning.
Self-Assessment – Test your knowledge and Exam Preparation – Familiarize yourself with the
identify areas requiring further question format and content
study areas
Concept Reinforcement – Deepen your Confidence Building – Develop test-taking
understanding through strategies and reduce
evidence-based exam anxiety
rationales
Time Management – Practice answering
questions under simulated
exam conditions
Review Summary 90 Questions
Foundations - Application - Sch3u Grade 11 Chemistry UNIT 3 Solutions Complete AND Worked Ontario
Virtual School 2026 Sch3u Grade 11 Chemistry UNIT 3 Solutions Complete AND Worked Ontario Virtual
School 2026 University
All answers with rationales
,Table of Contents
Content Area Questions Key Topics
Solutions AND Their 1-15 Solution, Water, Solubility, Prepared, Resulting
Properties
Concentration AND Molarity 16-30 Solution, Solubility, Water, First, Molar
Solubility AND Factors 31-45 Solution, Water, Solubility, Prepared, Dissolving
Affecting Solubility
Solution Stoichiometry 46-60 Solution, Point, Water, Prepared, Mixing
Dilutions AND Preparing 61-75 Solution, Solubility, Prepared, Water, Mixing
Solutions
Electrolytes AND 76-90 Solution, Solubility, Water, Statements, Point
Nonelectrolytes
TOTAL 90 All questions include answers and detailed rationales
,Section A - Solutions AND Their Properties
Q1.
A solution is prepared by dissolving 58.44 g of NaCl in 500.0 g of water. The density of the
resulting solution is 1.12 g/mL. Calculate the molality of the solution.
A. 1.00 m B. 2.00 m
C. 0.500 m D. 1.50 m
Correct: B - 2.00 m
Rationale:Moles of NaCl = 58.44 g / 58.44 g/mol = 1.00 mol. Mass of water = 0.500 kg.
Molality = 1.00 mol / 0.500 kg = 2.00 m. Option A uses kg of solution instead of solvent; C
uses total mass incorrectly; D is a miscalculation.
Q2.
Which of the following processes is endothermic when a solute dissolves in water, yet the
overall dissolution is spontaneous?
A. Ion-dipole attractions between solute and B. The entropy change of the system is
water are weaker than solute-solute and negative, but the enthalpy change is highly
water-water attractions. exothermic.
C. The enthalpy of hydration is negative and D. The entropy increase of the surroundings
the lattice energy is positive, with the due to heat release compensates for a
hydration energy exceeding the lattice decrease in system entropy.
energy.
Correct: A - Ion-dipole attractions between solute and water are weaker than solute-solute
and water-water attractions.
Rationale:Dissolution can be endothermic (”H positive) if the energy cost to separate solute
and solvent exceeds the energy released on mixing, but spontaneity arises from a large
positive entropy change (S positive). Option B is endothermic but non-spontaneous unless
entropy compensates; C describes an exothermic process; D incorrectly attributes
spontaneity to surroundings in an endothermic case.
Q3.
A 0.10 M solution of a weak acid HA has a pH of 3.50. What is the percent ionization of
HA?
A. 0.32% B. 3.2%
C. 0.032% D. 0.50%
Page 3
, Section A - Solutions AND Their Properties
Correct: A - 0.32%
Rationale:[H+] = 10^-3.50 = 3.16 × 10^-4 M. Percent ionization = ([H+]/[HA]0) × 100 = (3.16 ×
10^-.10) × 100 = 0.316% 0.32%. Option B uses 10^-pH as a percentage without dividing
by concentration; C is a decimal error; D is an arbitrary value.
Q4.
Which of the following 0.10 M aqueous solutions will have the highest boiling point?
A. NaCl B. CaCl2
C. C6H12O6 (glucose) D. CH3COOH (acetic acid)
Correct: B - CaCl2
Rationale:Boiling point elevation depends on the van't Hoff factor (i). CaCl2 dissociates into 3
ions (i=3), giving the highest effective particle concentration. NaCl has i=2, glucose i=1, and
acetic acid partially ionizes (i1.0). Therefore CaCl2 produces the greatest boiling point
elevation.
Q5.
A student prepares a saturated solution of PbCl2 in pure water and measures [Pb2+] =
0.016 M. What is the Ksp of PbCl2?
A. 1.6 × 10^-5 B. 4.1 × 10^-6
C. 2.6 × 10^-4 D. 1.0 × 10^-5
Correct: A - 1.6 × 10^-5
Rationale:PbCl2(s) !Ì Pb2+ + 2Cl-. If [Pb2+] = 0.016 M, then [Cl-] = 2 × 0.016 = 0.032 M. Ksp
= [Pb2+][Cl-]^2 = 0.016 × (0.032)^2 = 1.64 × 10^-5 1.6 × 10^-5. Option B cubes the
concentration; C uses wrong stoichiometry; D is a miscalculation.
Q6.
Which of the following best explains why a solution of NaCl in water conducts electricity,
but a solution of sucrose in water does not?
A. NaCl is a strong electrolyte, dissociating B. NaCl is a covalent compound that forms
into ions, while sucrose is a non-electrolyte, charged particles in solution, while sucrose
remaining as neutral molecules. is ionic and remains neutral.
C. Water molecules break down NaCl into D. Sucrose dissolves by forming hydrogen
charged particles, but they cannot break bonds, which prevents any charged species
down sucrose because it is too large. from forming.
Correct: A - NaCl is a strong electrolyte, dissociating into ions, while sucrose is a
non-electrolyte, remaining as neutral molecules.
Page 4
