Question 1

The acid solubility product, Kspa, for metal sulfides is always larger in value than non-sulfides.

Accepted Answer

A) True 
 B)False  True

Question 2

Which of the following is the expression for the solubility product of copper(II)hydroxide?

Accepted Answer

A) Ksp = [Cu2+][2 OH] 
B) Ksp = [Cu2+] 2[OH]2 
C) Ksp = [Cu2+]2[OH] 
D) Ksp = [Cu2+][OH]2 
E) Ksp = [Cu2+] ½[OH]2 
A) Ksp = [Cu2+][2 OH] 
B) Ksp = [Cu2+] 2[OH]2 
C) Ksp = [Cu2+]2[OH] 
D) Ksp = [Cu2+][OH]2 
E) Ksp = [Cu2+] ½[OH]2 D

Question 3

The solubility of lead(II)fluoride, PbF2, in pure water is 2.1 × 10-3 moles per liter. Calculate the value of Ksp for lead(II)fluoride from this data.

Accepted Answer

A) 1.3 × 10-7 
B) 1.9 × 10-8 
C) 3.7 × 10-8 
D) 1.6 × 10-9 
E) 9.3 × 10-9 
A) 1.3 × 10-7 
B) 1.9 × 10-8 
C) 3.7 × 10-8 
D) 1.6 × 10-9 
E) 9.3 × 10-9 C

Question 4

In an aqueous solution, silver ions can form Ag(NH3)2+(aq), in the presence of ammonia. In Ag(NH3)2+(aq),

Accepted Answer

A) Ag(NH3)2+(aq)is a ligand; NH3 is a donor atom; Ag+ is a ligand. 
B) Ag(NH3)2+(aq)is a complex ion; NH3 is a ligand; Ag+ is a complex ion. 
C) Ag(NH3)2+(aq)is a complex ion; NH3 is a donor atom; Ag+ is a ligand. 
D) Ag(NH3)2+(aq)is an acceptor ion; NH3 is a ligand; Ag+ is a complex ion. 
E) Ag(NH3)2+(aq)is a complex ion; NH3 is a ligand; Ag+ is an acceptor. 
A) Ag(NH3)2+(aq)is a ligand; NH3 is a donor atom; Ag+ is a ligand. 
B) Ag(NH3)2+(aq)is a complex ion; NH3 is a ligand; Ag+ is a complex ion. 
C) Ag(NH3)2+(aq)is a complex ion; NH3 is a donor atom; Ag+ is a ligand. 
D) Ag(NH3)2+(aq)is an acceptor ion; NH3 is a ligand; Ag+ is a complex ion. 
E) Ag(NH3)2+(aq)is a complex ion; NH3 is a ligand; Ag+ is an acceptor.

Question 5

For the formation of Fe(H2O)63+(aq)by Fe+3(aq)+ 6H2O(aq)→ Fe(H2O)63+(aq)Which reactant acts as a Lewis acid, and which acts as a Lewis base?

Accepted Answer

Fe⁺³ acts as a Lewis a

Question 6

Which one of the compounds below has the highest solubility in water, expressed in moles per liter?

Accepted Answer

A) SrF2, Ksp = 2.8 × 10-9 
B) Sr(IO3)2, Ksp = 3.3 × 10-7 
C) MgF2, Ksp = 6.5 × 10-9 
D) PbCl2, Ksp = 1.6 × 10-5 
E) BaF2, Ksp = 1.7 × 10-6 
A) SrF2, Ksp = 2.8 × 10-9 
B) Sr(IO3)2, Ksp = 3.3 × 10-7 
C) MgF2, Ksp = 6.5 × 10-9 
D) PbCl2, Ksp = 1.6 × 10-5 
E) BaF2, Ksp = 1.7 × 10-6

Question 7

The formation constant for the bis(thiosulfato)argentate(I)ion, [Ag(S2O3)2]3-, is 2.0 × 1013, while the solubility product constant for silver iodide is 8.3 × 10-17. A 0.200 molar solution of Na2S2O3 is saturated with AgI. What is the concentration of free iodide ion in the saturated solution?Hint: Combine the formation and solubility reactions to find the overall reaction and its equilibrium constant.

Accepted Answer

Question 8

The solubility of silver sulfate (Ag2SO4), can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

Accepted Answer

A) solubility = 2[Ag+] 
B) solubility = [Ag+] 
C) solubility = [2Ag+] 
D) solubility = 2[SO42] 
E) solubility = [SO42] 
A) solubility = 2[Ag+] 
B) solubility = [Ag+] 
C) solubility = [2Ag+] 
D) solubility = 2[SO42] 
E) solubility = [SO42]

Question 9

Consider the equilibrium,AgCl(s)+ Br(aq)   AgBr(s)+ Cl-(aq)whose equilibrium constant is related to Ksp(AgCl)= 1.8 × 10-10 and Ksp(AgBr)= 5.0 × 10-13. Calculate the equilibrium constant for the reaction and indicate whether AgCl will react with 1.00 M KBr(aq)to a significant extent.

Accepted Answer

Question 10

Which of the following is the expression for the solubility product of Ba3(AsO4)2?

Accepted Answer

A) Ksp = [Ba2+]3[AsO43]2 
B) Ksp = [3 × Ba2+]3[2AsO43]2 
C) Ksp = 3[Ba2+] 2[AsO43] 
D) Ksp = 3[Ba2+]3 + 2[AsO43]2 
E) Ksp = [Ba3+]3[AsO42]2 
A) Ksp = [Ba2+]3[AsO43]2 
B) Ksp = [3 × Ba2+]3[2AsO43]2 
C) Ksp = 3[Ba2+] 2[AsO43] 
D) Ksp = 3[Ba2+]3 + 2[AsO43]2 
E) Ksp = [Ba3+]3[AsO42]2

Question 11

The pH of a saturated solution of Mg(OH)2, whose Ksp is 7.1 × 10-12, is ________.

Accepted Answer

Question 12

Will a precipitate of MgF2 form when 300 mL of 1.1 × 10-3 M MgCl2 solution is added to 500 mL of 1.2 × 10-3 M NaF? The Ksp of MgF2 is 6.9 × 10-9.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

Accepted Answer

A) yes, because the ion product, Q > Ksp 
B) no, because the ion product, Q sp 
C) no, because the ion product, Q = Ksp 
D) yes, because the ion product, Q sp 
E) no, because the ion product, Q > Ksp 
A) yes, because the ion product, Q > Ksp 
B) no, because the ion product, Q sp 
C) no, because the ion product, Q = Ksp 
D) yes, because the ion product, Q sp 
E) no, because the ion product, Q > Ksp

Question 13

For the H2CO3/ HCO3/CO32- system at room temperature Ka1 = 4.5 × 10-7, whileKa2 = 4.7 × 10-11. The Ksp for BaCO3 is 5.0 × 10-9.Calculate the equilibrium constant for the reaction,BaCO3(s)+ H+(aq)   Ba2+(aq)+ HCO3-(aq)

Accepted Answer

Question 14

Calculate the concentration of bromide ions in a saturated solution of lead(II)bromide. The Ksp = 6.6 × 10-6.

Accepted Answer

A) 1.2 × 10-2 M 
B) 2.2 × 10-2 M 
C) 2.0 × 10-2 M 
D) 1.2 × 10-1 M 
E) 2.1 × 10-3 M 
A) 1.2 × 10-2 M 
B) 2.2 × 10-2 M 
C) 2.0 × 10-2 M 
D) 1.2 × 10-1 M 
E) 2.1 × 10-3 M

Question 15

Hydrazine, N2H4, is a weak molecular base with a value of 9.6 × 10-7 for Kb. An aqueous solution contains 0.200 M N2H4 and 0.376 M N2H5Cl per liter as the only solutes. If the Ksp of Fe(OH)2 is 7.9 × 10-16, what is the maximum [Fe2+] that can coexist with these solutes in the solution? Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, then use that to find [OH-].

Accepted Answer

A) 1.5 × 10-9 M 
B) 4.1 × 10-9 M 
C) 0.00024 M 
D) 0.00086 M 
E) 0.0030 M 
A) 1.5 × 10-9 M 
B) 4.1 × 10-9 M 
C) 0.00024 M 
D) 0.00086 M 
E) 0.0030 M

Question 16

The solubility product for Ag3PO4 is: Ksp = 2.8 × 10-18. What is the solubility of Ag3PO4 in water?

Accepted Answer

A) 1.8 × 10-5 M 
B) 2.5 × 10-5 M 
C) 1.9 × 10-86 M 
D) 3.1 × 10-5 M 
E) 4.1 × 10-5 M 
A) 1.8 × 10-5 M 
B) 2.5 × 10-5 M 
C) 1.9 × 10-86 M 
D) 3.1 × 10-5 M 
E) 4.1 × 10-5 M

Question 17

What is the solubility, in moles per liter, of MgCO3 (Ksp = 3.5 × 10-8), in 0.0200 M Na2CO3 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) 4.4 × 10-6 
B) 8.1 × 10-4 
C) 4.4 × 10-3 
D) 8.8 × 10-5 
E) 1.8 × 10-6 
A) 4.4 × 10-6 
B) 8.1 × 10-4 
C) 4.4 × 10-3 
D) 8.8 × 10-5 
E) 1.8 × 10-6

Question 18

During an experiment, 300 mL of 2.0 × 10-5 M AgNO3 is going to be added to 200 mL of 2.5 × 10-9 M NaI. Will a precipitate form? What is the precipitate? The Ksp forAgI is 8.3 × 10-17.Hint: Find the concentration of each ion and use those concentrations to find Q for any insoluble compounds that might form.

Accepted Answer

A) yes, the ppt is AgNO3(s) 
B) yes, the ppt is NaNO3(s) 
C) yes, the ppt is NaI(s) 
D) yes, the ppt is AgI(s) 
E) no 
A) yes, the ppt is AgNO3(s) 
B) yes, the ppt is NaNO3(s) 
C) yes, the ppt is NaI(s) 
D) yes, the ppt is AgI(s) 
E) no

Question 19

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 is the equilibrium constant for the reaction,AgBr(s)+ 2 S2O32-(aq)   Ag(S2O3)23-(aq)+ Br(aq)?

Accepted Answer

Question 20

The acid-insoluble sulfides and base-insoluble sulfides can be separated from each other by changing the pH of the aqueous solution that contains them. At low pH, the acid-insoluble sulfides will precipitate out. What role does the acid play in this process?

Accepted Answer

A) The H+ ion is produced by the dissolving sulfide, so the presence of an acid hinders the dissolution process. 
B) The sulfide reacts with the H+ ion, forming the cation and H2S. 
C) The sulfide reacts with any OH- ions present, forming S(OH)2 and the cation. 
D) The sulfide forms a complex ion with the H+ provided by the acid. 
E) The acid does not play a role in the dissolution process of metal sulfides. 
A) The H+ ion is produced by the dissolving sulfide, so the presence of an acid hinders the dissolution process. 
B) The sulfide reacts with the H+ ion, forming the cation and H2S. 
C) The sulfide reacts with any OH- ions present, forming S(OH)2 and the cation. 
D) The sulfide forms a complex ion with the H+ provided by the acid. 
E) The acid does not play a role in the dissolution process of metal sulfides.

The acid solubility product, K_spa, for metal sulfides is always larger in value than non-sulfides.

Which of the following is the expression for the solubility product of copper(II)hydroxide?

The solubility of lead(II)fluoride, PbF₂, in pure water is 2.1 × 10^-³ moles per liter. Calculate the value of K_sp for lead(II)fluoride from this data.

In an aqueous solution, silver ions can form Ag(NH₃)₂⁺(aq), in the presence of ammonia. In Ag(NH₃)₂⁺(aq),

For the formation of Fe(H₂O)₆³⁺(aq)by Fe⁺³(aq)+ 6H₂O(aq)→ Fe(H₂O)₆³⁺(aq)Which reactant acts as a Lewis acid, and which acts as a Lewis base?

Which one of the compounds below has the highest solubility in water, expressed in moles per liter?

The solubility of silver sulfate (Ag₂SO₄), can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

Consider the equilibrium,AgCl(s)+ Br(aq) AgBr(s)+ Cl^-(aq)whose equilibrium constant is related to K_sp(AgCl)= 1.8 × 10^-10 and K_sp(AgBr)= 5.0 × 10^-13. Calculate the equilibrium constant for the reaction and indicate whether AgCl will react with 1.00 M KBr(aq)to a significant extent.

Which of the following is the expression for the solubility product of Ba₃(AsO₄)₂?

The pH of a saturated solution of Mg(OH)₂, whose K_sp is 7.1 × 10^-¹², is ________.

Will a precipitate of MgF₂ form when 300 mL of 1.1 × 10^-³ M MgCl₂ solution is added to 500 mL of 1.2 × 10^-³ M NaF? The K_sp of MgF₂ is 6.9 × 10^-⁹.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

For the H₂CO₃/ HCO₃/CO₃^2- system at room temperature K_a1 = 4.5 × 10^-⁷, whileK_a2 = 4.7 × 10^-11. The K_sp for BaCO₃ is 5.0 × 10^-9.Calculate the equilibrium constant for the reaction,BaCO₃(s)+ H⁺(aq) Ba²⁺(aq)+ HCO₃^-(aq)

Calculate the concentration of bromide ions in a saturated solution of lead(II)bromide. The K_sp = 6.6 × 10^-⁶.

The solubility product for Ag₃PO₄ is: K_sp = 2.8 × 10^-¹⁸. What is the solubility of Ag₃PO₄ in water?

What is the solubility, in moles per liter, of MgCO₃ (K_sp = 3.5 × 10^-8), in 0.0200 M Na₂CO₃ 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 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 is the equilibrium constant for the reaction,AgBr(s)+ 2 S₂O₃^2-(aq) Ag(S₂O₃)₂^3-(aq)+ Br(aq)?

The acid-insoluble sulfides and base-insoluble sulfides can be separated from each other by changing the pH of the aqueous solution that contains them. At low pH, the acid-insoluble sulfides will precipitate out. What role does the acid play in this process?

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 metal sulfides is always larger in value than non-sulfides.

Which of the following is the expression for the solubility product of copper(II)hydroxide?

The solubility of lead(II)fluoride, PbF2, in pure water is 2.1 × 10-3 moles per liter. Calculate the value of Ksp for lead(II)fluoride from this data.

In an aqueous solution, silver ions can form Ag(NH3)2+(aq), in the presence of ammonia. In Ag(NH3)2+(aq),

For the formation of Fe(H2O)63+(aq)by Fe+3(aq)+ 6H2O(aq)→ Fe(H2O)63+(aq)Which reactant acts as a Lewis acid, and which acts as a Lewis base?

Which one of the compounds below has the highest solubility in water, expressed in moles per liter?

The solubility of silver sulfate (Ag2SO4), can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

Consider the equilibrium,AgCl(s)+ Br(aq) AgBr(s)+ Cl-(aq)whose equilibrium constant is related to Ksp(AgCl)= 1.8 × 10-10 and Ksp(AgBr)= 5.0 × 10-13. Calculate the equilibrium constant for the reaction and indicate whether AgCl will react with 1.00 M KBr(aq)to a significant extent.

Which of the following is the expression for the solubility product of Ba3(AsO4)2?

The pH of a saturated solution of Mg(OH)2, whose Ksp is 7.1 × 10-12, is ________.

Will a precipitate of MgF2 form when 300 mL of 1.1 × 10-3 M MgCl2 solution is added to 500 mL of 1.2 × 10-3 M NaF? The Ksp of MgF2 is 6.9 × 10-9.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

For the H2CO3/ HCO3/CO32- system at room temperature Ka1 = 4.5 × 10-7, whileKa2 = 4.7 × 10-11. The Ksp for BaCO3 is 5.0 × 10-9.Calculate the equilibrium constant for the reaction,BaCO3(s)+ H+(aq) Ba2+(aq)+ HCO3-(aq)

Calculate the concentration of bromide ions in a saturated solution of lead(II)bromide. The Ksp = 6.6 × 10-6.

The solubility product for Ag3PO4 is: Ksp = 2.8 × 10-18. What is the solubility of Ag3PO4 in water?

What is the solubility, in moles per liter, of MgCO3 (Ksp = 3.5 × 10-8), in 0.0200 M Na2CO3 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 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 is the equilibrium constant for the reaction,AgBr(s)+ 2 S2O32-(aq) Ag(S2O3)23-(aq)+ Br(aq)?

The acid-insoluble sulfides and base-insoluble sulfides can be separated from each other by changing the pH of the aqueous solution that contains them. At low pH, the acid-insoluble sulfides will precipitate out. What role does the acid play in this process?

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 metal sulfides is always larger in value than non-sulfides.

The solubility of lead(II)fluoride, PbF₂, in pure water is 2.1 × 10^-³ moles per liter. Calculate the value of K_sp for lead(II)fluoride from this data.

In an aqueous solution, silver ions can form Ag(NH₃)₂⁺(aq), in the presence of ammonia. In Ag(NH₃)₂⁺(aq),

For the formation of Fe(H₂O)₆³⁺(aq)by Fe⁺³(aq)+ 6H₂O(aq)→ Fe(H₂O)₆³⁺(aq)Which reactant acts as a Lewis acid, and which acts as a Lewis base?

The solubility of silver sulfate (Ag₂SO₄), can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

Consider the equilibrium,AgCl(s)+ Br(aq) AgBr(s)+ Cl^-(aq)whose equilibrium constant is related to K_sp(AgCl)= 1.8 × 10^-10 and K_sp(AgBr)= 5.0 × 10^-13. Calculate the equilibrium constant for the reaction and indicate whether AgCl will react with 1.00 M KBr(aq)to a significant extent.

Which of the following is the expression for the solubility product of Ba₃(AsO₄)₂?

The pH of a saturated solution of Mg(OH)₂, whose K_sp is 7.1 × 10^-¹², is ________.

Will a precipitate of MgF₂ form when 300 mL of 1.1 × 10^-³ M MgCl₂ solution is added to 500 mL of 1.2 × 10^-³ M NaF? The K_sp of MgF₂ is 6.9 × 10^-⁹.Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

For the H₂CO₃/ HCO₃/CO₃^2- system at room temperature K_a1 = 4.5 × 10^-⁷, whileK_a2 = 4.7 × 10^-11. The K_sp for BaCO₃ is 5.0 × 10^-9.Calculate the equilibrium constant for the reaction,BaCO₃(s)+ H⁺(aq) Ba²⁺(aq)+ HCO₃^-(aq)

Calculate the concentration of bromide ions in a saturated solution of lead(II)bromide. The K_sp = 6.6 × 10^-⁶.

The solubility product for Ag₃PO₄ is: K_sp = 2.8 × 10^-¹⁸. What is the solubility of Ag₃PO₄ in water?

What is the solubility, in moles per liter, of MgCO₃ (K_sp = 3.5 × 10^-8), in 0.0200 M Na₂CO₃ 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 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 is the equilibrium constant for the reaction,AgBr(s)+ 2 S₂O₃^2-(aq) Ag(S₂O₃)₂^3-(aq)+ Br(aq)?