Question 1

The molar solubility of PbI2 is 1.52 $\times$ 10-3 M.Calculate the value of Ksp for PbI2.

Accepted Answer

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

Question 2

Given the following Ksp values,which statement about solubility in mol/L in water is correct?

Accepted Answer

A) PbCrO4,Zn(OH)2,and Pb(OH)2 have equal solubilities in water. 
B) PbCrO4 has the lowest solubility in water. 
C) The solubility of MnS in water will not be pH dependent. 
D) MnS has the highest molar solubility in water. 
E) A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution. 
A) PbCrO4,Zn(OH)2,and Pb(OH)2 have equal solubilities in water. 
B) PbCrO4 has the lowest solubility in water. 
C) The solubility of MnS in water will not be pH dependent. 
D) MnS has the highest molar solubility in water. 
E) A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution. B

Question 3

In the qualitative analysis scheme for metal ions,how are the Analytical Group I cations separated from the other cations?

Accepted Answer

A) by addition of HCl,forming insoluble metal chlorides 
B) by addition of H2SO4,forming insoluble metal sulfates 
C) by addition of H2S in acidic solution,forming insoluble metal sulfides 
D) by addition of H2S in basic solution,forming insoluble metal sulfides or hydroxides 
E) by addition of (NH4)2CO3 or (NH4)3PO4,forming insoluble metal carbonates or phosphates 
A) by addition of HCl,forming insoluble metal chlorides 
B) by addition of H2SO4,forming insoluble metal sulfates 
C) by addition of H2S in acidic solution,forming insoluble metal sulfides 
D) by addition of H2S in basic solution,forming insoluble metal sulfides or hydroxides 
E) by addition of (NH4)2CO3 or (NH4)3PO4,forming insoluble metal carbonates or phosphates A

Question 4

The best explanation for the dissolution of ZnS in dilute HCl is that:

Accepted Answer

A) The zinc ion is amphoteric. 
B) The sulfide-ion concentration is decreased by the formation of H2S. 
C) the sulfide-ion concentration is decreased by oxidation to sulfur. 
D) the zinc-ion concentration is decreased by the formation of a chloro complex. 
E) The solubility product of ZnCl2 is less than that of ZnS. 
A) The zinc ion is amphoteric. 
B) The sulfide-ion concentration is decreased by the formation of H2S. 
C) the sulfide-ion concentration is decreased by oxidation to sulfur. 
D) the zinc-ion concentration is decreased by the formation of a chloro complex. 
E) The solubility product of ZnCl2 is less than that of ZnS.

Question 5

The Ksp for Mn(OH)2 is 2.0 $\times$ 10-13.At what pH will Mn(OH)2 begin to precipitate from a solution in which the initial concentration of Mn2+ is 0.10 M?

Accepted Answer

A) 6.47 
B) 13.3 
C) 5.85 
D) 7.03 
E) 8.15 
A) 6.47 
B) 13.3 
C) 5.85 
D) 7.03 
E) 8.15

Question 6

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NOS1U1B13S1U1B0)S1U1B12S1U1B0 are mixed with 1.0 L of 1.0 M NaS1U1B12S1U1B0CS1U1B12S1U1B0OS1U1B14S1U1B0.The oxalate ion,CS1U1B12S1U1B0OS1U1B14S1U1B0,acts as a ligand to form a complex ion with the MnS1U1P12+S1S1P0 ion with a coordination number of two.
MnS1U1P12+S1S1P0 + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0
S1U1P1 S1S1P0   MnCS1U1B12S1U1B0OS1U1B14S1U1B0
KS1U1B11S1U1B0 = 7.9 $\times$ 10S1U1P13S1S1P0
[Mn(CS1U1B12S1U1B0OS1U1B14S1U1B0)S1U1B12S1U1B0]S1U1P12S1S1P0S1U1P1-S1S1P0
S1U1P1 S1S1P0   MnCS1U1B12S1U1B0OS1U1B14 S1U1B0+ CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0
KS1U1B12S1U1B0 = 1.26 $\times$ 10S1U1P1-S1S1P0S1U1P12S1S1P0
-What is the equilibrium constant for the following formation? Mn2+ + 2C2O42-
    [Mn(C2O4)2]2-

Accepted Answer

A) 1.0 
B) 3.7 $\times$ 102 
C) 2.1 $\times$ 10-1 
D) 6.3 $\times$ 105 
E) none of these 
A) 1.0 
B) 3.7 $\times$ 102 
C) 2.1 $\times$ 10-1 
D) 6.3 $\times$ 105 
E) none of these

Question 7

Determine the equilibrium concentration of the chloride ion.

Accepted Answer

A) 3.9 $\times$ 10-4 
B) 8.0 $\times$ 10-6 
C) 2.8 $\times$ 10-3 
D) 6.1 $\times$ 10-2 
E) none of these 
A) 3.9 $\times$ 10-4 
B) 8.0 $\times$ 10-6 
C) 2.8 $\times$ 10-3 
D) 6.1 $\times$ 10-2 
E) none of these

Question 8

The solubility of La(IO3)3 in a 0.42 M KIO3 solution is   mol/L.Calculate the Ksp for La(IO3)3.

Accepted Answer

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

Question 9

The solubility of silver phosphate,Ag3PO4, at 25°C is 1.60 $\times$10-5 mol/L.What is the Ksp for the silver phosphate at 25°C?

Accepted Answer

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

Question 10

Calculate the solubility of Ca3(PO4)2 (Ksp = 1.3 $\times$ 10-32)in a 0.048 M Ca(NO3)2 solution.

Accepted Answer

A)    mol/L 
B)    mol/L 
C)    mol/L 
D)    mol/L 
E) none of these 
A)    mol/L 
B)    mol/L 
C)    mol/L 
D)    mol/L 
E) none of these

Question 11

An unknown salt,M2Z,has a Ksp of   .Calculate the solubility in mol/L of M2Z.

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 12

Consider a solution containing the following cations: Na+,Hg2+,Mn2+,Al3+ and Ag+.Treatment of the solution with dilute HCl followed by saturation with H2S results in formation of precipitate(s).Which ions still remain in solution (i.e. ,did not precipitate)?

Accepted Answer

A) Ag+ only 
B) Na+,Hg2+,Al3+ 
C) Ag+ and Hg2+ 
D) Na+,Al3+,and Mn2+ 
E) Na+ only 
A) Ag+ only 
B) Na+,Hg2+,Al3+ 
C) Ag+ and Hg2+ 
D) Na+,Al3+,and Mn2+ 
E) Na+ only

Question 13

Calculate the solubility of Ag2CrO4 (Ksp = 9.0 $\times$10-12)in a 0.049 M AgNO3 solution.

Accepted Answer

A)     mol/L 
B)    mol/L 
C)    mol/L 
D)    mol/L 
E) none of these 
A)     mol/L 
B)    mol/L 
C)    mol/L 
D)    mol/L 
E) none of these

Question 14

An industrial plant processes its waste water through a sedimentation tank that removes hazardous metals by precipitating them as insoluble carbonate salts.If sodium carbonate is gradually added to the tank,what would be the order of precipitation of the metals,Pb2+,Cu2+,Hg22+,and Zn2+ if each is $\approx$ 1.0 $\times$ 10-4 M? ( Ksp PbCO3 = 7.4 $\times$10-14,Ksp CuCO3 = 1.4 $\times$10-10,Ksp Hg2CO3 = 8.9 $\times$ 10-17,and Ksp ZnCO3 = 1.4 $\times$ 10-11)

Accepted Answer

A) Pb2+,Hg22+,Zn2+,Cu2+ 
B) Hg22+,Pb2+,Zn2+,Cu2+ 
C) Cu2+,Zn2+,Pb2+,Hg22+ 
D) Cu2+,Zn2+,Hg22+,Pb2+ 
E) All metal ions will precipitate at the same time. 
A) Pb2+,Hg22+,Zn2+,Cu2+ 
B) Hg22+,Pb2+,Zn2+,Cu2+ 
C) Cu2+,Zn2+,Pb2+,Hg22+ 
D) Cu2+,Zn2+,Hg22+,Pb2+ 
E) All metal ions will precipitate at the same time.

Question 15

The solubility of CaSO4 in pure water at 0oC is 1.14 gram(s)per liter.The value of the solubility product is

Accepted Answer

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

Question 16

Given the following values of equilibrium constants: Cu(OH)2(s)   Cu2+(aq)+ 2OH-(aq)
Ksp = 1.60 $\times$10-19
Cu(NH3)42+(aq)   Cu2+(aq)+ 4NH3(aq)
K = 1.0 $\times$10-13
What is the value of the equilibrium constant for the following reaction?
Cu(OH)2(s)+ 4NH3(aq)   Cu(NH3)42+(aq)+ 2OH-(aq)

Accepted Answer

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

Question 17

A solution contains 0.018 moles each of I-,Br-,and Cl-.When the solution is mixed with 200 mL of 0.24 M AgNO3,how much AgCl(s)precipitates out?

Accepted Answer

A) 0.0 g 
B) 1.7 g 
C) 2.6 g 
D) 3.3 g 
E) 5.0 g 
A) 0.0 g 
B) 1.7 g 
C) 2.6 g 
D) 3.3 g 
E) 5.0 g

Question 18

What is the maximum concentration of iodide ions that will precipitate AgI but not PbI2 from a solution that is   M each in Ag+ and Pb2+? For AgI,Ksp = 1.5 $\times$ 10-16 and for PbI2,Ksp = 1.4 $\times$ 10-8.

Accepted Answer

A)    M 
B)    M 
C)    M 
D)    M 
E) None of these;PbI2 will always precipitate before AgI. 
A)    M 
B)    M 
C)    M 
D)    M 
E) None of these;PbI2 will always precipitate before AgI.

Question 19

The overall Kf for the complex ion Ag(NH3)2+ is 1.7 $\times$107.The Ksp for AgI is 1.5 $\times$ 10-16.What is the molar solubility of AgI in a solution that is 2.0 M in NH3?

Accepted Answer

A) 1.5 $\times$ 10-9 
B) 1.3 $\times$ 10-3 
C) 1.0 $\times$ 10-4 
D) 5.8 $\times$ 10-12 
E) 8.4 $\times$ 10-5 
A) 1.5 $\times$ 10-9 
B) 1.3 $\times$ 10-3 
C) 1.0 $\times$ 10-4 
D) 5.8 $\times$ 10-12 
E) 8.4 $\times$ 10-5

Question 20

In the qualitative analysis scheme for metal ions,how are the Analytical Group II cations separated from the cations of Analytical Groups III-V?

Accepted Answer

A) by addition of HCl,forming insoluble metal chlorides 
B) by addition of H2SO4,forming insoluble metal sulfates 
C) by addition of H2S in acidic solution,forming insoluble metal sulfides 
D) by addition of H2S in basic solution,forming insoluble metal sulfides or hydroxides 
E) by addition of (NH4)2CO3 or (NH4)3PO4,forming insoluble metal carbonates or phosphates 
A) by addition of HCl,forming insoluble metal chlorides 
B) by addition of H2SO4,forming insoluble metal sulfates 
C) by addition of H2S in acidic solution,forming insoluble metal sulfides 
D) by addition of H2S in basic solution,forming insoluble metal sulfides or hydroxides 
E) by addition of (NH4)2CO3 or (NH4)3PO4,forming insoluble metal carbonates or phosphates

The molar solubility of PbI₂ is 1.52 $\times$ 10^-³M.Calculate the value of K_sp for PbI₂.

Given the following K_sp values,which statement about solubility in mol/L in water is correct?

In the qualitative analysis scheme for metal ions,how are the Analytical Group I cations separated from the other cations?

The best explanation for the dissolution of ZnS in dilute HCl is that:

The K_sp for Mn(OH)₂ is 2.0 $\times$ 10^-¹³.At what pH will Mn(OH)₂ begin to precipitate from a solution in which the initial concentration of Mn²⁺ is 0.10 M?

Determine the equilibrium concentration of the chloride ion.

The solubility of La(IO₃)₃ in a 0.42 M KIO₃ solution is mol/L.Calculate the K_sp for La(IO₃)₃.

The solubility of silver phosphate,Ag₃PO_4, at 25°C is 1.60 $\times$ 10^-⁵ mol/L.What is the K_sp for the silver phosphate at 25°C?

Calculate the solubility of Ca₃(PO₄)₂ (K_sp = 1.3 $\times$ 10^-³²)in a 0.048 M Ca(NO₃)₂ solution.

An unknown salt,M₂Z,has a K_sp of .Calculate the solubility in mol/L of M₂Z.

Consider a solution containing the following cations: Na⁺,Hg²⁺,Mn²⁺,Al³⁺ and Ag⁺.Treatment of the solution with dilute HCl followed by saturation with H₂S results in formation of precipitate(s).Which ions still remain in solution (i.e. ,did not precipitate)?

Calculate the solubility of Ag₂CrO₄ (K_sp = 9.0 $\times$ 10^-¹²)in a 0.049 M AgNO₃ solution.

The solubility of CaSO₄ in pure water at 0^oC is 1.14 gram(s)per liter.The value of the solubility product is

A solution contains 0.018 moles each of I^-,Br^-,and Cl^-.When the solution is mixed with 200 mL of 0.24 M AgNO₃,how much AgCl(s)precipitates out?

The overall K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 $\times$ 10⁷.The K_sp for AgI is 1.5 $\times$ 10^-¹⁶.What is the molar solubility of AgI in a solution that is 2.0 M in NH₃?

In the qualitative analysis scheme for metal ions,how are the Analytical Group II cations separated from the cations of Analytical Groups III-V?

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Exam 16: Solubility and Complex Ion Equilibria

The molar solubility of PbI2 is 1.52 ×\times× 10-3 M.Calculate the value of Ksp for PbI2.

Given the following Ksp values,which statement about solubility in mol/L in water is correct?

In the qualitative analysis scheme for metal ions,how are the Analytical Group I cations separated from the other cations?

The best explanation for the dissolution of ZnS in dilute HCl is that:

The Ksp for Mn(OH)2 is 2.0 ×\times× 10-13.At what pH will Mn(OH)2 begin to precipitate from a solution in which the initial concentration of Mn2+ is 0.10 M?

Determine the equilibrium concentration of the chloride ion.

The solubility of La(IO3)3 in a 0.42 M KIO3 solution is mol/L.Calculate the Ksp for La(IO3)3.

The solubility of silver phosphate,Ag3PO4, at 25°C is 1.60 ×\times× 10-5 mol/L.What is the Ksp for the silver phosphate at 25°C?

Calculate the solubility of Ca3(PO4)2 (Ksp = 1.3 ×\times× 10-32)in a 0.048 M Ca(NO3)2 solution.

An unknown salt,M2Z,has a Ksp of .Calculate the solubility in mol/L of M2Z.

Consider a solution containing the following cations: Na+,Hg2+,Mn2+,Al3+ and Ag+.Treatment of the solution with dilute HCl followed by saturation with H2S results in formation of precipitate(s).Which ions still remain in solution (i.e. ,did not precipitate)?

Calculate the solubility of Ag2CrO4 (Ksp = 9.0 ×\times× 10-12)in a 0.049 M AgNO3 solution.

The solubility of CaSO4 in pure water at 0oC is 1.14 gram(s)per liter.The value of the solubility product is

Given the following values of equilibrium constants: Cu(OH)2(s) Cu2+(aq)+ 2OH-(aq) Ksp = 1.60 ×\times× 10-19 Cu(NH3)42+(aq) Cu2+(aq)+ 4NH3(aq) K = 1.0 ×\times× 10-13 What is the value of the equilibrium constant for the following reaction? Cu(OH)2(s)+ 4NH3(aq) Cu(NH3)42+(aq)+ 2OH-(aq)

A solution contains 0.018 moles each of I-,Br-,and Cl-.When the solution is mixed with 200 mL of 0.24 M AgNO3,how much AgCl(s)precipitates out?

What is the maximum concentration of iodide ions that will precipitate AgI but not PbI2 from a solution that is M each in Ag+ and Pb2+? For AgI,Ksp = 1.5 ×\times× 10-16 and for PbI2,Ksp = 1.4 ×\times× 10-8.

The overall Kf for the complex ion Ag(NH3)2+ is 1.7 ×\times× 107.The Ksp for AgI is 1.5 ×\times× 10-16.What is the molar solubility of AgI in a solution that is 2.0 M in NH3?

In the qualitative analysis scheme for metal ions,how are the Analytical Group II cations separated from the cations of Analytical Groups III-V?

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

The molar solubility of PbI₂ is 1.52 $\times$ 10^-³M.Calculate the value of K_sp for PbI₂.

Given the following K_sp values,which statement about solubility in mol/L in water is correct?

The K_sp for Mn(OH)₂ is 2.0 $\times$ 10^-¹³.At what pH will Mn(OH)₂ begin to precipitate from a solution in which the initial concentration of Mn²⁺ is 0.10 M?

The solubility of La(IO₃)₃ in a 0.42 M KIO₃ solution is mol/L.Calculate the K_sp for La(IO₃)₃.

The solubility of silver phosphate,Ag₃PO_4, at 25°C is 1.60 $\times$ 10^-⁵ mol/L.What is the K_sp for the silver phosphate at 25°C?

Calculate the solubility of Ca₃(PO₄)₂ (K_sp = 1.3 $\times$ 10^-³²)in a 0.048 M Ca(NO₃)₂ solution.

An unknown salt,M₂Z,has a K_sp of .Calculate the solubility in mol/L of M₂Z.

Consider a solution containing the following cations: Na⁺,Hg²⁺,Mn²⁺,Al³⁺ and Ag⁺.Treatment of the solution with dilute HCl followed by saturation with H₂S results in formation of precipitate(s).Which ions still remain in solution (i.e. ,did not precipitate)?

Calculate the solubility of Ag₂CrO₄ (K_sp = 9.0 $\times$ 10^-¹²)in a 0.049 M AgNO₃ solution.

The solubility of CaSO₄ in pure water at 0^oC is 1.14 gram(s)per liter.The value of the solubility product is

A solution contains 0.018 moles each of I^-,Br^-,and Cl^-.When the solution is mixed with 200 mL of 0.24 M AgNO₃,how much AgCl(s)precipitates out?

The overall K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 $\times$ 10⁷.The K_sp for AgI is 1.5 $\times$ 10^-¹⁶.What is the molar solubility of AgI in a solution that is 2.0 M in NH₃?