UNIVERSITY OF NEW ENGLAND CHEM 1011 GENERAL CHEMISTRY II FINAL EXAM QUESTIONS & … EXAM
P R O F E S S I O N A L P R A C T I C E M AT E R I A L S
University of New England CHEM
1011 General Chemistry II Final
Exam Questions & Answers
Weeks 9-16 2026-2027
(Rationales)
Verified Answers Exam Ready With Rationales
90 QUESTIONS
DOCUMENT OVERVIEW
This document contains 90 exam questions with correct answers and detailed rationales focused on general
chemistry concepts. It serves as a comprehensive resource for students seeking to enhance their
understanding of chemical principles. The material is ideal for study sessions, review, and preparation for
certification exams in chemistry.
CONTENTS
01 Solubility and Ksp Q1–Q10
02 Thermodynamics Concepts Q11–Q22
03 Entropy and Microstates Q23–Q33
04 Gibbs Free Energy Q34–Q44
05 Electrochemistry Q45–Q55
06 Periodic Trends and Elements Q56–Q66
Page 1
, 07 Organic Chemistry Structures Q67–Q77
08 Nuclear Chemistry Q78–Q90
E XA M Q U EST I O N S
Q1 QUESTION 1 OF 90
W9, Q9
A solid ionic compound, such as KCl in water, that is classified as soluble
A) Will not dissociate if added to a saturated solution
B) Will always dissociate completely
C) Will not dissociate at all
D) Will form a homogeneous solution without dissociation
CORRECT ANSWER
Will not dissociate if added to a saturated solution
RATIONALE
Ionic compounds like KCl dissociate into their constituent ions in solution; however, if the solution is already saturated, no additional
dissociation occurs since the solubility limit has been reached, preventing further ionization. This principle highlights the dynamic
equilibrium between dissolved ions and undissolved solid in a saturated solution.
Q2 QUESTION 2 OF 90
W9, Q9
The solubility product expression for the dissolution of Ba3(PO4)2 is
A) Ksp = [Ba2+][PO43-]
B) Ksp = [Ba2+]3[PO43-]
C) Ksp = [Ba2+]3[PO43-]2
D) Ksp = [Ba2+]2[PO43-]3
CORRECT ANSWER
Ksp= [Ba^2+]3[PO4^3-]2
RATIONALE
The solubility product constant (Ksp) for Ba3(PO4)2 incorporates the stoichiometry of the dissolution reaction, which yields three barium
ions and two phosphate ions per formula unit. Therefore, the Ksp expression is correctly represented as Ksp = [Ba2+]^3[PO43-]^2, reflecting
the coefficients from the balanced equation.
Q3 QUESTION 3 OF 90
W9, Q9
The solubility of CaS will be greatest in
A) 0.05 M Ca(NO3)2
Page 2
,B) 0.1 M Mg(NO3)2
C) 0.1 M CaBr2
D) 0.1 M Li2S
CORRECT ANSWER
0.1 M Mg(NO3)2
RATIONALE
Common ion effect reduces the solubility of salts, so CaS will be least soluble in solutions containing Ca²⁺ ions like Ca(NO3)2 or CaBr2. In
contrast, Mg(NO3)2 provides no common ions, allowing for maximum solubility of CaS.
Q4 QUESTION 4 OF 90
W9, Q9
What is the effect of adding NaOH to a saturated solution of Ca(OH)2?
A) [Ca2+] will decrease, [OH-] will decrease, there will be less Ca(OH)2(s)
B) [Ca2+] will decrease, [OH-] will increase, there will be more Ca(OH)2(s)
C) [Ca2+] will increase, [OH-] will decrease, there will be more Ca(OH)2(s)
D) There will be no change in [Ca2+], [OH-], or Ca(OH)2(s)
CORRECT ANSWER
[Ca2+] will decrease, [OH-] will increase, and there will be more Ca(OH)2 (s)
RATIONALE
Adding NaOH to a saturated Ca(OH)2 solution increases the hydroxide ion concentration, shifting the equilibrium to the left according to Le
Chatelier's principle, which promotes the precipitation of more solid Ca(OH)2 and decreases the concentration of dissolved calcium ions.
This dynamic illustrates the common ion effect, where the addition of a common ion (OH-) suppresses the solubility of the salt.
Q5 QUESTION 5 OF 90
W9, Q9
Marble is a type of rock composed primarily of calcium carbonate. Statues and buildings made from marble are particularly
susceptible to damage from acid rain, which is partially caused by the conversion of NO2 gas from industrial emissions into nitric
acid.
Three of the reactions relevant to this damage are:
(Rxn 1) 4 NO2(g) + 2 H2O(l) + O2(g) ⇌ 4 HNO3(aq)
(Rxn 2) HNO3(aq) + H2O(l) ⟶ H3O+ + NO3-(aq)
(Rxn 3) CaCO3(s) + 2 H3O+(aq) ⇌ Ca2+(aq) + CO2(g) + H2O(l)
Which of the following is true of this coupled equilibrium system?
A) A decrease in HNO3(aq) will lead to an increase in Ca2+(aq)
B) A decrease in NO2(g) will lead to a decrease in Ca2+(aq)
C) An increase in NO2(g) will lead to a decrease in CO2(g)
D) An increase in HNO3(aq) will lead to a decrease in CO2(g)
CORRECT ANSWER
A decrease in NO2(g) will lead to a decrease in Ca2+(aq)
Page 3
, RATIONALE
A reduction in NO2(g) decreases the production of HNO3(aq) via reaction 1, subsequently reducing H3O+(aq) and shifting reaction 3 left,
thus lowering the concentration of Ca2+(aq) released from marble dissolution. This illustrates Le Chatelier's principle, where a change in
reactant concentration affects the equilibrium position of the system.
Q6 QUESTION 6 OF 90
W9, Q9
The Ksp of CuCl is 1.2 x 10-6 at 25 °C.
What is the molar solubility of CuCl at 25 °C?
A) 1.2 x 10-6 M
B) 1.1 x 10-2 M
C) 3.7 x 10-4 M
D) 1.1 x 10-3 M
CORRECT ANSWER
1.1 x 10-3 M
RATIONALE
The solubility product constant (Ksp) represents the equilibrium between a solid and its ions in solution, where Ksp = [Cu^+] [Cl^-]. For CuCl,
dissociation yields one mole of Cu^+ and one mole of Cl^- per mole of CuCl, making the molar solubility equal to the square root of Ksp,
yielding 1.1 x 10^-3 M.
Q7 QUESTION 7 OF 90
W9, Q9
The solubility of ZnCO3 in water is 0.0023 g/100 mL at 25°C. What is the Ksp for ZnCO3 at 25 °C?
A) 3.4 x 10-8
B) 2.6 x 10-9
C) 1.8 x 10-15
D) 1.1 x 10-15
CORRECT ANSWER
3.4 x 10-8
RATIONALE
4 x 10⁻⁸. This reflects the principle that Ksp quantifies the extent of dissolution of a sparingly soluble salt.
Q8 QUESTION 8 OF 90
W9, Q9
What is the molar solubility of AgCl in a 0.050 M NaCl solution? The Ksp of AgCl is 1.6 x 10-10. (Assume that the contribution of
[Cl-] from AgCl is negligible relative to the [Cl-] from NaCl)
A) 6.4 x 10-10 M
Page 4
P R O F E S S I O N A L P R A C T I C E M AT E R I A L S
University of New England CHEM
1011 General Chemistry II Final
Exam Questions & Answers
Weeks 9-16 2026-2027
(Rationales)
Verified Answers Exam Ready With Rationales
90 QUESTIONS
DOCUMENT OVERVIEW
This document contains 90 exam questions with correct answers and detailed rationales focused on general
chemistry concepts. It serves as a comprehensive resource for students seeking to enhance their
understanding of chemical principles. The material is ideal for study sessions, review, and preparation for
certification exams in chemistry.
CONTENTS
01 Solubility and Ksp Q1–Q10
02 Thermodynamics Concepts Q11–Q22
03 Entropy and Microstates Q23–Q33
04 Gibbs Free Energy Q34–Q44
05 Electrochemistry Q45–Q55
06 Periodic Trends and Elements Q56–Q66
Page 1
, 07 Organic Chemistry Structures Q67–Q77
08 Nuclear Chemistry Q78–Q90
E XA M Q U EST I O N S
Q1 QUESTION 1 OF 90
W9, Q9
A solid ionic compound, such as KCl in water, that is classified as soluble
A) Will not dissociate if added to a saturated solution
B) Will always dissociate completely
C) Will not dissociate at all
D) Will form a homogeneous solution without dissociation
CORRECT ANSWER
Will not dissociate if added to a saturated solution
RATIONALE
Ionic compounds like KCl dissociate into their constituent ions in solution; however, if the solution is already saturated, no additional
dissociation occurs since the solubility limit has been reached, preventing further ionization. This principle highlights the dynamic
equilibrium between dissolved ions and undissolved solid in a saturated solution.
Q2 QUESTION 2 OF 90
W9, Q9
The solubility product expression for the dissolution of Ba3(PO4)2 is
A) Ksp = [Ba2+][PO43-]
B) Ksp = [Ba2+]3[PO43-]
C) Ksp = [Ba2+]3[PO43-]2
D) Ksp = [Ba2+]2[PO43-]3
CORRECT ANSWER
Ksp= [Ba^2+]3[PO4^3-]2
RATIONALE
The solubility product constant (Ksp) for Ba3(PO4)2 incorporates the stoichiometry of the dissolution reaction, which yields three barium
ions and two phosphate ions per formula unit. Therefore, the Ksp expression is correctly represented as Ksp = [Ba2+]^3[PO43-]^2, reflecting
the coefficients from the balanced equation.
Q3 QUESTION 3 OF 90
W9, Q9
The solubility of CaS will be greatest in
A) 0.05 M Ca(NO3)2
Page 2
,B) 0.1 M Mg(NO3)2
C) 0.1 M CaBr2
D) 0.1 M Li2S
CORRECT ANSWER
0.1 M Mg(NO3)2
RATIONALE
Common ion effect reduces the solubility of salts, so CaS will be least soluble in solutions containing Ca²⁺ ions like Ca(NO3)2 or CaBr2. In
contrast, Mg(NO3)2 provides no common ions, allowing for maximum solubility of CaS.
Q4 QUESTION 4 OF 90
W9, Q9
What is the effect of adding NaOH to a saturated solution of Ca(OH)2?
A) [Ca2+] will decrease, [OH-] will decrease, there will be less Ca(OH)2(s)
B) [Ca2+] will decrease, [OH-] will increase, there will be more Ca(OH)2(s)
C) [Ca2+] will increase, [OH-] will decrease, there will be more Ca(OH)2(s)
D) There will be no change in [Ca2+], [OH-], or Ca(OH)2(s)
CORRECT ANSWER
[Ca2+] will decrease, [OH-] will increase, and there will be more Ca(OH)2 (s)
RATIONALE
Adding NaOH to a saturated Ca(OH)2 solution increases the hydroxide ion concentration, shifting the equilibrium to the left according to Le
Chatelier's principle, which promotes the precipitation of more solid Ca(OH)2 and decreases the concentration of dissolved calcium ions.
This dynamic illustrates the common ion effect, where the addition of a common ion (OH-) suppresses the solubility of the salt.
Q5 QUESTION 5 OF 90
W9, Q9
Marble is a type of rock composed primarily of calcium carbonate. Statues and buildings made from marble are particularly
susceptible to damage from acid rain, which is partially caused by the conversion of NO2 gas from industrial emissions into nitric
acid.
Three of the reactions relevant to this damage are:
(Rxn 1) 4 NO2(g) + 2 H2O(l) + O2(g) ⇌ 4 HNO3(aq)
(Rxn 2) HNO3(aq) + H2O(l) ⟶ H3O+ + NO3-(aq)
(Rxn 3) CaCO3(s) + 2 H3O+(aq) ⇌ Ca2+(aq) + CO2(g) + H2O(l)
Which of the following is true of this coupled equilibrium system?
A) A decrease in HNO3(aq) will lead to an increase in Ca2+(aq)
B) A decrease in NO2(g) will lead to a decrease in Ca2+(aq)
C) An increase in NO2(g) will lead to a decrease in CO2(g)
D) An increase in HNO3(aq) will lead to a decrease in CO2(g)
CORRECT ANSWER
A decrease in NO2(g) will lead to a decrease in Ca2+(aq)
Page 3
, RATIONALE
A reduction in NO2(g) decreases the production of HNO3(aq) via reaction 1, subsequently reducing H3O+(aq) and shifting reaction 3 left,
thus lowering the concentration of Ca2+(aq) released from marble dissolution. This illustrates Le Chatelier's principle, where a change in
reactant concentration affects the equilibrium position of the system.
Q6 QUESTION 6 OF 90
W9, Q9
The Ksp of CuCl is 1.2 x 10-6 at 25 °C.
What is the molar solubility of CuCl at 25 °C?
A) 1.2 x 10-6 M
B) 1.1 x 10-2 M
C) 3.7 x 10-4 M
D) 1.1 x 10-3 M
CORRECT ANSWER
1.1 x 10-3 M
RATIONALE
The solubility product constant (Ksp) represents the equilibrium between a solid and its ions in solution, where Ksp = [Cu^+] [Cl^-]. For CuCl,
dissociation yields one mole of Cu^+ and one mole of Cl^- per mole of CuCl, making the molar solubility equal to the square root of Ksp,
yielding 1.1 x 10^-3 M.
Q7 QUESTION 7 OF 90
W9, Q9
The solubility of ZnCO3 in water is 0.0023 g/100 mL at 25°C. What is the Ksp for ZnCO3 at 25 °C?
A) 3.4 x 10-8
B) 2.6 x 10-9
C) 1.8 x 10-15
D) 1.1 x 10-15
CORRECT ANSWER
3.4 x 10-8
RATIONALE
4 x 10⁻⁸. This reflects the principle that Ksp quantifies the extent of dissolution of a sparingly soluble salt.
Q8 QUESTION 8 OF 90
W9, Q9
What is the molar solubility of AgCl in a 0.050 M NaCl solution? The Ksp of AgCl is 1.6 x 10-10. (Assume that the contribution of
[Cl-] from AgCl is negligible relative to the [Cl-] from NaCl)
A) 6.4 x 10-10 M
Page 4
