Question 1

The acid solubility product, Kspa, for PbS refers to which of the following reactions?

Accepted Answer

A) PbS(s)+ 2H2O(l)   H+(aq)+ Pb(OH)2(s)+ HS-(l) 
B) PbS(s)+ 2H2O(aq)   H+(aq)+ Pb(OH)2(s)+ HS-(aq) 
C) PbS(s)+ 2H2O(l)   H+(l)+ Pb(OH)2(s) 
D) PbS(s)+ 2H+(aq)   Pb2+(aq)+ H2S(aq) 
E) PbS(s)+ 2H+(l)   H+(aq)+ Pb(OH)2(s)+ HS-(aq) 
A) PbS(s)+ 2H2O(l)   H+(aq)+ Pb(OH)2(s)+ HS-(l) 
B) PbS(s)+ 2H2O(aq)   H+(aq)+ Pb(OH)2(s)+ HS-(aq) 
C) PbS(s)+ 2H2O(l)   H+(l)+ Pb(OH)2(s) 
D) PbS(s)+ 2H+(aq)   Pb2+(aq)+ H2S(aq) 
E) PbS(s)+ 2H+(l)   H+(aq)+ Pb(OH)2(s)+ HS-(aq)

Question 2

How many grams of AgCl can dissolve in 1.00 L of 1.50 M NH3?The Ksp of AgCl is 1.80 × 10-10, and the formation constant of [Ag(NH3)2]+ is 1.60 × 107.Hint: Combine the formation and solubility reactions to find the overall reaction and its equilibrium constant and account for the presence of a common ion.

Accepted Answer

We need to consider two balanced chemica

Question 3

Which one of the compounds below has the highest molar solubility in water?

Accepted Answer

A) SrF2, Ksp = 2.8 × 10-9 
B) Sr(IO3)2, Ksp = 3.3 × 10-7 
C) Fe(OH)2, Ksp = 8.0 × 10-16 
D) PbCl2, Ksp = 1.6 × 10-5 
E) PbBr2, Ksp = 3.9 × 10-5 
A) SrF2, Ksp = 2.8 × 10-9 
B) Sr(IO3)2, Ksp = 3.3 × 10-7 
C) Fe(OH)2, Ksp = 8.0 × 10-16 
D) PbCl2, Ksp = 1.6 × 10-5 
E) PbBr2, Ksp = 3.9 × 10-5

Question 4

What is the molar solubility of AgCl in a 0.450 M solution of KCl? The Ksp of AgCl is 1.8 × 10-10.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

Accepted Answer

The K_sp expression in this problem is K_sp =

Question 5

The solubility product for BaSO4 is 1.1 × 10-10. Calculate the solubility of BaSO4 in pure water.

Accepted Answer

A) 5.5 × 10-11 mol L-1 
B) 1.0 × 10-5 mol L-1 
C) 2.1 × 10-5 mol L-1 
D) 1.1 × 10-10 mol L-1 
E) 2.2 × 10-10 mol L-1 
A) 5.5 × 10-11 mol L-1 
B) 1.0 × 10-5 mol L-1 
C) 2.1 × 10-5 mol L-1 
D) 1.1 × 10-10 mol L-1 
E) 2.2 × 10-10 mol L-1

Question 6

Zinc carbonate, a slightly soluble substance, is most soluble in which of the following solvents?

Accepted Answer

A) water 
B) 0.1 M ZnCl2(aq) 
C) 0.1 M NaOH(aq) 
D) 0.1 M HCl(aq) 
E) 0.2 M Na2CO3(aq) 
A) water 
B) 0.1 M ZnCl2(aq) 
C) 0.1 M NaOH(aq) 
D) 0.1 M HCl(aq) 
E) 0.2 M Na2CO3(aq)

Question 7

Group II and group III cations (acid-insoluble and base-insoluble sulfides)can be separated out by forming a precipitate of acid-insoluble cations at low ________.

Accepted Answer

The answer of Group II and group III cations (acid-insoluble...

Question 8

The Ksp of calcium fluoride is 3.9 × 10-11. A 0.420 g sample of NaF and a 1.110 g sample of calcium chloride were added to a 1.000 liter volumetric flask, and distilled water was added to the mark. After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, how many grams of precipitate, if any, would be formed?Hint: Find Q and compare to Ksp.

Accepted Answer

A) 0.00 g 
B) 0.039 g 
C) 0.39 g 
D) 0.41 g 
E) 0.77 g 
A) 0.00 g 
B) 0.039 g 
C) 0.39 g 
D) 0.41 g 
E) 0.77 g

Question 9

The formation constant for the bis(thiosulfato)argentate(I)ion is 2.0 × 1013, while the solubility product constant for silver bromide is 5.0 × 10-13. What would be the equilibrium constant for the reaction below?AgBr(s)+ 2 S2O32-(aq)   Ag(S2O3)23-(aq)+ Br-(aq)

Accepted Answer

A) 2.0 × 1013 
B) 5.0 × 10-1 
C) 4.0 × 1025 
D) 5.0 × 10-13 
E) 10 
A) 2.0 × 1013 
B) 5.0 × 10-1 
C) 4.0 × 1025 
D) 5.0 × 10-13 
E) 10

Question 10

A solution contains Ba2+ (1.0 × 10-3 M), Ca2+ (1.0 × 10-3 M)and K+ (1.0 × 10-3 M). Drops of a 5.0 × 10-1 M solution of NaF were added through a microburet until the [F-] in the solution mix reached 6.0 × 10-3 M. Should a precipitate form? If so, what is the precipitate? The Ksp values are BaF2: 1.0 × 10-6, CaF2: 5.3 × 10-9. (Neglect the slight change in volume resulting from the added NaF solution.)

Accepted Answer

A) a precipitate consisting of BaF2 only should form 
B) a precipitate consisting of CaF2 and KF should form 
C) a precipitate consisting of BaF2 and CaF2 should form 
D) a precipitate consisting of CaF2 only should form 
E) No precipitate should form. 
A) a precipitate consisting of BaF2 only should form 
B) a precipitate consisting of CaF2 and KF should form 
C) a precipitate consisting of BaF2 and CaF2 should form 
D) a precipitate consisting of CaF2 only should form 
E) No precipitate should form.

Question 11

The solubility product for PbBr2 is: Ksp = 6.6 × 10-6. Which of the following represents the solubility of PbBr2?

Accepted Answer

A) 4.7 × 10-1 g/L 
B) 2.4 × 10-3 g/L 
C) 6.0 × 10-4 g/L 
D) 4.3 g/L 
E) 6.1 × 10-4 g/L 
A) 4.7 × 10-1 g/L 
B) 2.4 × 10-3 g/L 
C) 6.0 × 10-4 g/L 
D) 4.3 g/L 
E) 6.1 × 10-4 g/L

Question 12

What is the solubility, in moles per liter, of BaSO4 (Ksp = 1.1 × 10-10), in 0.0100 M Na2SO4 solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

Accepted Answer

A) 1.1 × 10-8 
B) 1.1 × 10-6 
C) 1.1 × 10-7 
D) 1.1 × 10-5 
E) 1.1 × 10-4 
A) 1.1 × 10-8 
B) 1.1 × 10-6 
C) 1.1 × 10-7 
D) 1.1 × 10-5 
E) 1.1 × 10-4

Question 13

The value of the solubility product constant for barium carbonate is 5.0 × 10-9 and that of barium chromate is 2.1 × 10-10. From this data, what is the value of Kc for the reaction below?   Hint: Combine reactions and Ksp values like all other reactions and equilibrium constants.

Accepted Answer

A) 1.1 × 10-18 
B) 4.2 × 10-2 
C) 4.8 × 10-9  
D) 4.9 
E) 24 
A) 1.1 × 10-18 
B) 4.2 × 10-2 
C) 4.8 × 10-9  
D) 4.9 
E) 24

Question 14

PbCO3, PbCl2, PbI2, and PbS are all only very slightly soluble in pure water. Which one (ones)should be significantly more soluble in acidic solution than in pure water?

Accepted Answer

A) PbI2, PbS and PbCO3 
B) only PbCO3 and PbS 
C) only PbCl2 and PbI2 
D) only PbCO3 
E) All four are significantly more soluble in acidic solution. 
A) PbI2, PbS and PbCO3 
B) only PbCO3 and PbS 
C) only PbCl2 and PbI2 
D) only PbCO3 
E) All four are significantly more soluble in acidic solution.

Question 15

The solubility of calcium fluoride, CaF2, in pure water is 2.15 × 10-4 moles per liter. Calculate the value of Ksp for calcium fluoride from this data.

Accepted Answer

A) 1.85 × 10-7 
B) 9.28 × 10-8 
C) 1.99 × 10-11 
D) 3.98 × 10-11 
E) 9.94 × 10-12 
A) 1.85 × 10-7 
B) 9.28 × 10-8 
C) 1.99 × 10-11 
D) 3.98 × 10-11 
E) 9.94 × 10-12

Question 16

Given the following information:   What is the equilibrium constant for the reaction,MgCO3(s)+ H+(aq)   Mg2+(aq)+ HCO3-(aq)

Accepted Answer

Question 17

The solubility of copper(II)iodate, Cu(IO3)2, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

Accepted Answer

A) solubility = 2[Cu2+] 
B) solubility = [Cu2+] 
C) solubility = [2 Cu2+] 
D) solubility = 2[IO3] 
E) solubility = [IO3]2 
A) solubility = 2[Cu2+] 
B) solubility = [Cu2+] 
C) solubility = [2 Cu2+] 
D) solubility = 2[IO3] 
E) solubility = [IO3]2

Question 18

The solubility product for Mg3(PO4)2 is 6.3 × 10-26. What is the solubility of Mg3(PO4)2 in pure water, in grams per liter?

Accepted Answer

A) 1.7 × 10-23 g L-1 
B) 3.4 × 10-7 g L-1 
C) 9.4 × 10-4 g L-1 
D) 1.2 × 10-3 g L-1 
E) 2.4 × 10-3 g L-1 
A) 1.7 × 10-23 g L-1 
B) 3.4 × 10-7 g L-1 
C) 9.4 × 10-4 g L-1 
D) 1.2 × 10-3 g L-1 
E) 2.4 × 10-3 g L-1

Question 19

The solubility product for chromium(III)fluoride is Ksp = 6.6 × 10-11. Using this information, what is the molar solubility of chromium(III)fluoride?

Accepted Answer

Question 20

What is the solubility, in moles per liter, of Fe(OH)2 (Ksp = 7.9 × 10-16), in 0.0500 molar NaOH solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

Accepted Answer

A) 3.16 × 10-13 
B) 3.13 × 10-16 
C) 1.58 × 10-14 
D) 1.14 × 10-14 
E) 3.16 × 10-16 
A) 3.16 × 10-13 
B) 3.13 × 10-16 
C) 1.58 × 10-14 
D) 1.14 × 10-14 
E) 3.16 × 10-16

The acid solubility product, K_spa, for PbS refers to which of the following reactions?

Which one of the compounds below has the highest molar solubility in water?

What is the molar solubility of AgCl in a 0.450 M solution of KCl? The K_sp of AgCl is 1.8 × 10^-10.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

The solubility product for BaSO₄ is 1.1 × 10^-¹⁰. Calculate the solubility of BaSO₄ in pure water.

Zinc carbonate, a slightly soluble substance, is most soluble in which of the following solvents?

Group II and group III cations (acid-insoluble and base-insoluble sulfides)can be separated out by forming a precipitate of acid-insoluble cations at low ________.

The formation constant for the bis(thiosulfato)argentate(I)ion is 2.0 × 10¹³, while the solubility product constant for silver bromide is 5.0 × 10^-¹³. What would be the equilibrium constant for the reaction below?AgBr(s)+ 2 S₂O₃²^-(aq) Ag(S₂O₃)₂³^-(aq)+ Br^-(aq)

The solubility product for PbBr₂ is: K_sp = 6.6 × 10^-⁶. Which of the following represents the solubility of PbBr₂?

What is the solubility, in moles per liter, of BaSO₄ (K_sp = 1.1 × 10^-10), in 0.0100 M Na₂SO₄ solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

The value of the solubility product constant for barium carbonate is 5.0 × 10^-9 and that of barium chromate is 2.1 × 10^-10. From this data, what is the value of K_c for the reaction below? Hint: Combine reactions and K_sp values like all other reactions and equilibrium constants.

PbCO₃, PbCl₂, PbI₂, and PbS are all only very slightly soluble in pure water. Which one (ones)should be significantly more soluble in acidic solution than in pure water?

The solubility of calcium fluoride, CaF₂, in pure water is 2.15 × 10^-⁴ moles per liter. Calculate the value of K_sp for calcium fluoride from this data.

Given the following information: What is the equilibrium constant for the reaction,MgCO₃(s)+ H⁺(aq) Mg²⁺(aq)+ HCO₃^-(aq)

The solubility of copper(II)iodate, Cu(IO₃)₂, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

The solubility product for Mg₃(PO₄)₂ is 6.3 × 10^-²⁶. What is the solubility of Mg₃(PO₄)₂ in pure water, in grams per liter?

The solubility product for chromium(III)fluoride is K_sp = 6.6 × 10^-11. Using this information, what is the molar solubility of chromium(III)fluoride?

What is the solubility, in moles per liter, of Fe(OH)₂ (K_sp = 7.9 × 10^-¹⁶), in 0.0500 molar NaOH solution?^{Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.}

A Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Mixtures at the Molecular Level: Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

Exam 18: Solubility and Simultaneous Equilibria

The acid solubility product, Kspa, for PbS refers to which of the following reactions?

Which one of the compounds below has the highest molar solubility in water?

What is the molar solubility of AgCl in a 0.450 M solution of KCl? The Ksp of AgCl is 1.8 × 10-10.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

The solubility product for BaSO4 is 1.1 × 10-10. Calculate the solubility of BaSO4 in pure water.

Zinc carbonate, a slightly soluble substance, is most soluble in which of the following solvents?

Group II and group III cations (acid-insoluble and base-insoluble sulfides)can be separated out by forming a precipitate of acid-insoluble cations at low ________.

The formation constant for the bis(thiosulfato)argentate(I)ion is 2.0 × 1013, while the solubility product constant for silver bromide is 5.0 × 10-13. What would be the equilibrium constant for the reaction below?AgBr(s)+ 2 S2O32-(aq) Ag(S2O3)23-(aq)+ Br-(aq)

The solubility product for PbBr2 is: Ksp = 6.6 × 10-6. Which of the following represents the solubility of PbBr2?

What is the solubility, in moles per liter, of BaSO4 (Ksp = 1.1 × 10-10), in 0.0100 M Na2SO4 solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

The value of the solubility product constant for barium carbonate is 5.0 × 10-9 and that of barium chromate is 2.1 × 10-10. From this data, what is the value of Kc for the reaction below? Hint: Combine reactions and Ksp values like all other reactions and equilibrium constants.

PbCO3, PbCl2, PbI2, and PbS are all only very slightly soluble in pure water. Which one (ones)should be significantly more soluble in acidic solution than in pure water?

The solubility of calcium fluoride, CaF2, in pure water is 2.15 × 10-4 moles per liter. Calculate the value of Ksp for calcium fluoride from this data.

Given the following information: What is the equilibrium constant for the reaction,MgCO3(s)+ H+(aq) Mg2+(aq)+ HCO3-(aq)

The solubility of copper(II)iodate, Cu(IO3)2, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

The solubility product for Mg3(PO4)2 is 6.3 × 10-26. What is the solubility of Mg3(PO4)2 in pure water, in grams per liter?

The solubility product for chromium(III)fluoride is Ksp = 6.6 × 10-11. Using this information, what is the molar solubility of chromium(III)fluoride?

What is the solubility, in moles per liter, of Fe(OH)2 (Ksp = 7.9 × 10-16), in 0.0500 molar NaOH solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

A Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Mixtures at the Molecular Level: Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

The acid solubility product, K_spa, for PbS refers to which of the following reactions?

What is the molar solubility of AgCl in a 0.450 M solution of KCl? The K_sp of AgCl is 1.8 × 10^-10.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

The solubility product for BaSO₄ is 1.1 × 10^-¹⁰. Calculate the solubility of BaSO₄ in pure water.

The formation constant for the bis(thiosulfato)argentate(I)ion is 2.0 × 10¹³, while the solubility product constant for silver bromide is 5.0 × 10^-¹³. What would be the equilibrium constant for the reaction below?AgBr(s)+ 2 S₂O₃²^-(aq) Ag(S₂O₃)₂³^-(aq)+ Br^-(aq)

The solubility product for PbBr₂ is: K_sp = 6.6 × 10^-⁶. Which of the following represents the solubility of PbBr₂?

What is the solubility, in moles per liter, of BaSO₄ (K_sp = 1.1 × 10^-10), in 0.0100 M Na₂SO₄ solution?Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.

The value of the solubility product constant for barium carbonate is 5.0 × 10^-9 and that of barium chromate is 2.1 × 10^-10. From this data, what is the value of K_c for the reaction below? Hint: Combine reactions and K_sp values like all other reactions and equilibrium constants.

PbCO₃, PbCl₂, PbI₂, and PbS are all only very slightly soluble in pure water. Which one (ones)should be significantly more soluble in acidic solution than in pure water?

The solubility of calcium fluoride, CaF₂, in pure water is 2.15 × 10^-⁴ moles per liter. Calculate the value of K_sp for calcium fluoride from this data.

Given the following information: What is the equilibrium constant for the reaction,MgCO₃(s)+ H⁺(aq) Mg²⁺(aq)+ HCO₃^-(aq)

The solubility of copper(II)iodate, Cu(IO₃)₂, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

The solubility product for Mg₃(PO₄)₂ is 6.3 × 10^-²⁶. What is the solubility of Mg₃(PO₄)₂ in pure water, in grams per liter?

The solubility product for chromium(III)fluoride is K_sp = 6.6 × 10^-11. Using this information, what is the molar solubility of chromium(III)fluoride?

What is the solubility, in moles per liter, of Fe(OH)₂ (K_sp = 7.9 × 10^-¹⁶), in 0.0500 molar NaOH solution?^{Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math because the solubility is very low.}