Question 1

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

Accepted Answer

Question 2

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 × 10-6F) B) and D)
G) A) and E)

Question 3

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]2F) B) and E)
G) A) and C)

Question 4

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 MF) A) and B)
G) A) and C)

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 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]2F) A) and B)
G) B) and C) D

Question 7

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 > KspF) B) and E)
G) B) and D)

Question 8

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 9

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 × 10-6F) B) and E)
G) A) and C)

Question 10

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 MF) B) and C)
G) B) and E)

Question 11

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 × 10-9F) C) and D)
G) C) and E) C

Question 12

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.F) B) and D)
G) A) and E)

Question 13

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.F) B) and D)
G) B) and C)

Question 14

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

Accepted Answer

A) True 
 B)False  True

Question 15

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)  noF) A) and D)
G) B) and C)

Question 16

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 MF) C) and E)
G) A) and C)

Question 17

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 18

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]F) D) and E)
G) A) and B)

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

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

Exam 18: Solubility and Simultaneous Equilibria

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

Correct Answer
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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.

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

Correct Answer
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Correct Answer
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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?

Correct Answer
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Fe⁺³ acts as a Lewis a...
View Answer

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

Correct Answer
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D

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.

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

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

Correct Answer
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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.

Correct Answer
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C

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?

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified
True

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

Correct Answer
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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.

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

Correct Answer
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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)?

Correct Answer
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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)

Correct Answer
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Exam 18: Solubility and Simultaneous Equilibria

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

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedFe+3 acts as a Lewis a...View AnswerShow Answer

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

Correct AnswerverifiedD

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.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedC

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedTrue

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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)?

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct Answer
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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.

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

Correct Answer
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Correct Answer
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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?

Correct Answer
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Fe⁺³ acts as a Lewis a...
View Answer

Correct Answer
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D

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.

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

Correct Answer
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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.

Correct Answer
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C

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

Correct Answer
verified

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

Correct Answer
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True

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

Correct Answer
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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.

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

Correct Answer
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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)?

Correct Answer
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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)

Correct Answer
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