Question 1

In a solution prepared by adding excess PbI2 (Ksp = 1.44 $\times$ 10-8)to water,the [I-] at equilibrium is:

Accepted Answer

A)    mol/L 
B)    mol/L 
C)    mol/L 
D)    mol/L 
E)    mol/L 
A)    mol/L 
B)    mol/L 
C)    mol/L 
D)    mol/L 
E)    mol/L

Question 2

Which of the following solid salts is more soluble in 1.0 M H+ than in pure water?

Accepted Answer

A) NaCl 
B) KCl 
C) FePO4 
D) AgCl 
E) KNO3 
A) NaCl 
B) KCl 
C) FePO4 
D) AgCl 
E) KNO3

Question 3

An unknown salt,M3Z,has a Ksp of   .Calculate the solubility in mol/L of M3Z.

Accepted Answer

A)     M 
B)    M 
C)    M 
D)    M 
E) none of the above 
A)     M 
B)    M 
C)    M 
D)    M 
E) none of the above

Question 4

Consider a solution made by mixing 500.0 mL of 4.0 M NHS1U1B13S1U1B0 and 500.0 mL of 0.40 M AgNOS1U1B13S1U1B0.AgS1U1P1+S1S1P0 reacts with NHS1U1B13S1U1B0 to form AgNHS1U1B13S1U1B0S1U1P1+S1S1P0 and Ag(NHS1U1B13S1U1B0)S1U1B12S1U1B0S1U1P1+S1S1P0:
AgS1U1P1+S1S1P0 + NHS1U1B13S1U1B0
S1U1B1 S1U1B0   AgNHS1U1B13S1U1B0S1U1P1+S1S1P0
KS1U1B11S1U1B0 = 2.1 $\times$ 10S1U1P13S1S1P0
AgNHS1U1B13S1U1B0S1U1P1+S1S1P0 + NHS1U1B13S1U1B0
S1U1B1 S1U1B0   Ag(NHS1U1B13S1U1B0)S1U1B12S1U1B0S1U1P1+S1S1P0
KS1U1B12S1U1B0 = 8.2 $\times$10S1U1P13S1S1P0
-The concentration of Ag+ at equilibrium is:

Accepted Answer

A) 2.0 M 
B) 1.2 $\times$0 10-8 M 
C) 4.5 $\times$ 10-9 M 
D) 1.6 M 
E) none of these 
A) 2.0 M 
B) 1.2 $\times$0 10-8 M 
C) 4.5 $\times$ 10-9 M 
D) 1.6 M 
E) none of these

Question 5

You have a solution consisting of 0.10 M Cl- and 0.10 M CrO42-.You add 0.10 M silver nitrate dropwise to this solution.Given that the Ksp for Ag2CrO4 is 9.0 $\times$ 10-12,and that for AgCl is 1.6 $\times$10-10,which of the following will precipitate first?

Accepted Answer

A) silver chloride 
B) silver chromate 
C) silver nitrate 
D) cannot be determined by the information given 
E) none of these 
A) silver chloride 
B) silver chromate 
C) silver nitrate 
D) cannot be determined by the information given 
E) none of these

Question 6

Calculate the concentration of Al3+ in a saturated aqueous solution of Al(OH)3 (Ksp = 2.2 $\times$ 10-32).

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 7

The correct mathematical expression for finding the molar solubility (s)of Sn(OH)2 is:

Accepted Answer

A) 2s2 = Ksp 
B) 2s3 = Ksp 
C) 108s5 = Ksp 
D) 4s3 = Ksp 
E) 8s3 = Ksp 
A) 2s2 = Ksp 
B) 2s3 = Ksp 
C) 108s5 = Ksp 
D) 4s3 = Ksp 
E) 8s3 = Ksp

Question 8

Solubility Products (Ksp)  
Which of the following compounds is the most soluble (in moles/liter)?

Accepted Answer

A) BaSO4 
B) CoS 
C) PbSO4 
D) AgBr 
E) BaCO3 
A) BaSO4 
B) CoS 
C) PbSO4 
D) AgBr 
E) BaCO3

Question 9

The Ksp of PbSO4 is 1.3 $\times$10-8.Calculate the solubility (in mol/L)of PbSO4 in a 0.0037 M solution of Na2SO4.

Accepted Answer

A)    M 
B)    M 
C)    M 
D)    M 
E)    M 
A)    M 
B)    M 
C)    M 
D)    M 
E)    M

Question 10

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+,Ag+,and Au+.The Ksp values for the chloride salts are 1.9 $\times$10-7,1.6 $\times$ 10-10,and 2.0 $\times$ 10-13,respectively.Which compound will precipitate first?

Accepted Answer

A) CuCl 
B) AgCl 
C) AuCl 
D) All will precipitate at the same time. 
E) Cannot be determined. 
A) CuCl 
B) AgCl 
C) AuCl 
D) All will precipitate at the same time. 
E) Cannot be determined.

Question 11

The molar solubility of BaCO3 (Ksp = 1.6 $\times$ 10-9)in 0.10 M BaCl2 solution is:

Accepted Answer

A) 1.6 $\times$10-10 
B) 4.0 $\times$10-5 
C) 7.4 $\times$10-4 
D) 0.10 
E) none of these 
A) 1.6 $\times$10-10 
B) 4.0 $\times$10-5 
C) 7.4 $\times$10-4 
D) 0.10 
E) none of these

Question 12

The solubility of an unknown salt,M3Z2, at 25°C is   mol/L.What is the Ksp for M3Z2 at 25°C?

Accepted Answer

A)    
B)    
C)    
D)    
E) none of these 
A)    
B)    
C)    
D)    
E) none of these

Question 13

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

Accepted Answer

A) greater than 
B) less than 
C) about the same as 
D) cannot be determined 
E) much different from 
A) greater than 
B) less than 
C) about the same as 
D) cannot be determined 
E) much different from

Question 14

The solubility of Cd(OH)2 in water is 1.67 $\times$ 10-5 mol/L.The Ksp value for Cd(OH)2 is

Accepted Answer

A)    
B)    
C)    
D)    
E) none of these 
A)    
B)    
C)    
D)    
E) none of these

Question 15

A 100.-mL sample of solution contains 10.0 mmol of Ca2+ ion.How many mmol of solid Na2SO4 must be added in order to cause precipitation of 99.9% of the calcium as CaSO4? The Ksp of CaSO4 is 6.1 $\times$ 10-5.Assume the volume remains constant.

Accepted Answer

A) 17.4 
B) 10.0 
C) 61.0 
D) 71.0 
E) 6.1 
A) 17.4 
B) 10.0 
C) 61.0 
D) 71.0 
E) 6.1

Question 16

The concentration of Mg2+ in seawater is 0.052 M.At what pH will 99% of the Mg2+ be precipitated as the hydroxide? [Ksp for Mg(OH)2 = 8.9 $\times$10-12]

Accepted Answer

A) 8.35 
B) 9.22 
C) 6.50 
D) 10.12 
E) 4.86 
A) 8.35 
B) 9.22 
C) 6.50 
D) 10.12 
E) 4.86

Question 17

A 50.0-mL sample of 0.100 M Ca(NO3)2 is mixed with 50.00 mL of 0.200 M NaF.When the system has come to equilibrium,which of the following sets of conditions will hold? The Ksp for CaF2 is 4.0 $\times$ 10-11. Moles Solid CaF2

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 18

The solubility of an unknown salt,MZ2, at 25°C is   mol/L.What is the Ksp for MZ2 at 25°C?

Accepted Answer

A)    
B)    
C)    
D)    
E) none of these 
A)    
B)    
C)    
D)    
E) none of these

Question 19

The Ksp of an unknown salt,MZ2,is   .Calculate the solubility (in mol/L)of MZ2 in a 0.0230 M solution of CaZ2.

Accepted Answer

A)    M 
B)    M 
C)    M 
D)    M 
E)    M 
A)    M 
B)    M 
C)    M 
D)    M 
E)    M

Question 20

Which of the following compounds has the lowest solubility in mol/L in water?

Accepted Answer

A) Al(OH)3 Ksp = 2 $\times$ 10-32 
B) CdS Ksp = 1.0 $\times$ 10-28 
C) PbSO4 Ksp = 1.3 $\times$ 10-8 
D) Sn(OH)2 Ksp = 3 $\times$10-27 
E) MgC2O4 Ksp = 8.6 $\times$10-5 
A) Al(OH)3 Ksp = 2 $\times$ 10-32 
B) CdS Ksp = 1.0 $\times$ 10-28 
C) PbSO4 Ksp = 1.3 $\times$ 10-8 
D) Sn(OH)2 Ksp = 3 $\times$10-27 
E) MgC2O4 Ksp = 8.6 $\times$10-5

In a solution prepared by adding excess PbI₂ (K_sp = 1.44 $\times$ 10^-⁸)to water,the [I^-] at equilibrium is:

Which of the following solid salts is more soluble in 1.0 M H⁺ than in pure water?

An unknown salt,M₃Z,has a K_sp of .Calculate the solubility in mol/L of M₃Z.

You have a solution consisting of 0.10 M Cl^- and 0.10 M CrO₄²^-.You add 0.10 M silver nitrate dropwise to this solution.Given that the K_sp for Ag₂CrO₄ is 9.0 $\times$ 10^-¹²,and that for AgCl is 1.6 $\times$ 10^-¹⁰,which of the following will precipitate first?

Calculate the concentration of Al³⁺ in a saturated aqueous solution of Al(OH)₃ (K_sp = 2.2 $\times$ 10^-³²).

The correct mathematical expression for finding the molar solubility (s)of Sn(OH)₂ is:

Solubility Products (K_sp) Which of the following compounds is the most soluble (in moles/liter)?

The K_sp of PbSO₄ is 1.3 $\times$ 10^-⁸.Calculate the solubility (in mol/L)of PbSO₄ in a 0.0037 M solution of Na₂SO₄.

Sodium chloride is added slowly to a solution that is 0.010 M in Cu⁺,Ag⁺,and Au⁺.The K_sp values for the chloride salts are 1.9 $\times$ 10^-⁷,1.6 $\times$ 10^-¹⁰,and 2.0 $\times$ 10^-¹³,respectively.Which compound will precipitate first?

The molar solubility of BaCO₃ (K_sp = 1.6 $\times$ 10^-⁹)in 0.10 M BaCl₂ solution is:

The solubility of an unknown salt,M₃Z_2, at 25°C is mol/L.What is the K_sp for M₃Z₂ at 25°C?

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

The solubility of Cd(OH)₂ in water is 1.67 $\times$ 10^-⁵ mol/L.The K_sp value for Cd(OH)₂ is

A 100.-mL sample of solution contains 10.0 mmol of Ca²⁺ ion.How many mmol of solid Na₂SO₄ must be added in order to cause precipitation of 99.9% of the calcium as CaSO₄? The K_sp of CaSO₄ is 6.1 $\times$ 10^-⁵.Assume the volume remains constant.

The concentration of Mg²⁺ in seawater is 0.052 M.At what pH will 99% of the Mg²⁺ be precipitated as the hydroxide? [K_sp for Mg(OH)₂ = 8.9 $\times$ 10^-¹²]

The solubility of an unknown salt,MZ_2, at 25°C is mol/L.What is the K_sp for MZ₂ at 25°C?

The K_sp of an unknown salt,MZ₂,is .Calculate the solubility (in mol/L)of MZ₂ in a 0.0230 M solution of CaZ₂.

Which of the following compounds has the lowest solubility in mol/L in water?

Chemical Foundations

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Chemical Reactions and Solutions Stoichiometry

Gases

Thermochemistry

Atomic Structure and Periodicity

Bonding: General Concepts

Covalent Bonding: Orbitals

Liquids and Solids

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria

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Exam 16: Solubility and Complex Ion Equilibria

In a solution prepared by adding excess PbI2 (Ksp = 1.44 ×\times× 10-8)to water,the [I-] at equilibrium is:

Which of the following solid salts is more soluble in 1.0 M H+ than in pure water?

An unknown salt,M3Z,has a Ksp of .Calculate the solubility in mol/L of M3Z.

Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3.Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: Ag+ + NH3 AgNH3+ K1 = 2.1 ×\times× 103 AgNH3+ + NH3 Ag(NH3)2+ K2 = 8.2 ×\times× 103 -The concentration of Ag+ at equilibrium is:

You have a solution consisting of 0.10 M Cl- and 0.10 M CrO42-.You add 0.10 M silver nitrate dropwise to this solution.Given that the Ksp for Ag2CrO4 is 9.0 ×\times× 10-12,and that for AgCl is 1.6 ×\times× 10-10,which of the following will precipitate first?

Calculate the concentration of Al3+ in a saturated aqueous solution of Al(OH)3 (Ksp = 2.2 ×\times× 10-32).

The correct mathematical expression for finding the molar solubility (s)of Sn(OH)2 is:

Solubility Products (Ksp) Which of the following compounds is the most soluble (in moles/liter)?

The Ksp of PbSO4 is 1.3 ×\times× 10-8.Calculate the solubility (in mol/L)of PbSO4 in a 0.0037 M solution of Na2SO4.

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+,Ag+,and Au+.The Ksp values for the chloride salts are 1.9 ×\times× 10-7,1.6 ×\times× 10-10,and 2.0 ×\times× 10-13,respectively.Which compound will precipitate first?

The molar solubility of BaCO3 (Ksp = 1.6 ×\times× 10-9)in 0.10 M BaCl2 solution is:

The solubility of an unknown salt,M3Z2, at 25°C is mol/L.What is the Ksp for M3Z2 at 25°C?

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

The solubility of Cd(OH)2 in water is 1.67 ×\times× 10-5 mol/L.The Ksp value for Cd(OH)2 is

A 100.-mL sample of solution contains 10.0 mmol of Ca2+ ion.How many mmol of solid Na2SO4 must be added in order to cause precipitation of 99.9% of the calcium as CaSO4? The Ksp of CaSO4 is 6.1 ×\times× 10-5.Assume the volume remains constant.

The concentration of Mg2+ in seawater is 0.052 M.At what pH will 99% of the Mg2+ be precipitated as the hydroxide? [Ksp for Mg(OH)2 = 8.9 ×\times× 10-12]

A 50.0-mL sample of 0.100 M Ca(NO3)2 is mixed with 50.00 mL of 0.200 M NaF.When the system has come to equilibrium,which of the following sets of conditions will hold? The Ksp for CaF2 is 4.0 ×\times× 10-11. Moles Solid CaF2

The solubility of an unknown salt,MZ2, at 25°C is mol/L.What is the Ksp for MZ2 at 25°C?

The Ksp of an unknown salt,MZ2,is .Calculate the solubility (in mol/L)of MZ2 in a 0.0230 M solution of CaZ2.

Which of the following compounds has the lowest solubility in mol/L in water?

Chemical Foundations

Atoms, molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Thermochemistry

Atomic Structure and Periodicity

Bonding: General Concepts

Covalent Bonding: Orbitals

Liquids and Solids

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria

Spontaneity, entropy, and Free Energy

Electrochemistry

The Nucleus: a Chemists View

The Representative Elements

Transition Metals and Coordination Chemistry

Organic and Biological Molecules

Filters

In a solution prepared by adding excess PbI₂ (K_sp = 1.44 $\times$ 10^-⁸)to water,the [I^-] at equilibrium is:

Which of the following solid salts is more soluble in 1.0 M H⁺ than in pure water?

An unknown salt,M₃Z,has a K_sp of .Calculate the solubility in mol/L of M₃Z.

You have a solution consisting of 0.10 M Cl^- and 0.10 M CrO₄²^-.You add 0.10 M silver nitrate dropwise to this solution.Given that the K_sp for Ag₂CrO₄ is 9.0 $\times$ 10^-¹²,and that for AgCl is 1.6 $\times$ 10^-¹⁰,which of the following will precipitate first?

Calculate the concentration of Al³⁺ in a saturated aqueous solution of Al(OH)₃ (K_sp = 2.2 $\times$ 10^-³²).

The correct mathematical expression for finding the molar solubility (s)of Sn(OH)₂ is:

Solubility Products (K_sp) Which of the following compounds is the most soluble (in moles/liter)?

The K_sp of PbSO₄ is 1.3 $\times$ 10^-⁸.Calculate the solubility (in mol/L)of PbSO₄ in a 0.0037 M solution of Na₂SO₄.

Sodium chloride is added slowly to a solution that is 0.010 M in Cu⁺,Ag⁺,and Au⁺.The K_sp values for the chloride salts are 1.9 $\times$ 10^-⁷,1.6 $\times$ 10^-¹⁰,and 2.0 $\times$ 10^-¹³,respectively.Which compound will precipitate first?

The molar solubility of BaCO₃ (K_sp = 1.6 $\times$ 10^-⁹)in 0.10 M BaCl₂ solution is:

The solubility of an unknown salt,M₃Z_2, at 25°C is mol/L.What is the K_sp for M₃Z₂ at 25°C?

The solubility of Cd(OH)₂ in water is 1.67 $\times$ 10^-⁵ mol/L.The K_sp value for Cd(OH)₂ is

A 100.-mL sample of solution contains 10.0 mmol of Ca²⁺ ion.How many mmol of solid Na₂SO₄ must be added in order to cause precipitation of 99.9% of the calcium as CaSO₄? The K_sp of CaSO₄ is 6.1 $\times$ 10^-⁵.Assume the volume remains constant.

The concentration of Mg²⁺ in seawater is 0.052 M.At what pH will 99% of the Mg²⁺ be precipitated as the hydroxide? [K_sp for Mg(OH)₂ = 8.9 $\times$ 10^-¹²]

The solubility of an unknown salt,MZ_2, at 25°C is mol/L.What is the K_sp for MZ₂ at 25°C?

The K_sp of an unknown salt,MZ₂,is .Calculate the solubility (in mol/L)of MZ₂ in a 0.0230 M solution of CaZ₂.