Homework answers / question archive / University of South Florida CHM 2046 Chapter 16 Aqueous Ionic Equilibrium 1)Which of the following compounds will have the highest molar solubility in pure water? A) PbSO4, Ksp = 1

University of South Florida CHM 2046 Chapter 16 Aqueous Ionic Equilibrium 1)Which of the following compounds will have the highest molar solubility in pure water? A) PbSO4, Ksp = 1

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University of South Florida

CHM 2046

Chapter 16 Aqueous Ionic Equilibrium

1)Which of the following compounds will have the highest molar solubility in pure water? A) PbSO4, Ksp = 1.82 × 10-8

B) MgCO3, Ksp = 6.82 × 10-6

C) AgI, Ksp = 8.51 × 10-17

D) PbS, Ksp = 9.04 × 10-29

E) FeS, Ksp = 3.72 × 10-19

2.            Which of the following compounds solubility will not be affected by a low pH in solution?

A)           AgCl

B)            Mg(OH)2

C)            CaF2

D)           CuS

E)            BaCO3

3.            Which of the following compounds will be more soluble in acidic solution than in pure water?

a.            PbCl2

b.            FeS

c.             Ca(ClO4)2

d.            CuI

e.            None of the above will be more soluble in acidic solution.

 

4.            Identify the salts that are in hard water.

a.            CaCO3 and MgCO3

b.            MgSO4 and CaSO4

c.             NaCl and KBr

d.            NaHSO4 and Na2SO4

e.            NaOCl and HOCl

 

 

5.            Give the expression for the solubility product constant for PbCl2. [Pb2+ ][Cl- ]2

 

A)           [PbCl2 ]

[PbCl2 ]

 

B) [Pb2+ ][Cl-]2

C) [Pb2+][Cl–]2

[Pb2+ ][Cl- ]

 

D)           [PbCl2 ]

E) [Pb2+]2[Cl–]

6.            Give the expression for the solubility product constant for BaF2.

[BaF2 ]

A) [Ba2+ ][F- ]2

 

[Ba2+ ][F- ]2

B)            [BaF2 ]

C) [Ba2+]2[F–]

D) [Ba2+][F–]2

E) [Ba2+][F–]

7.            Give the expression for the solubility product constant for Ca3(PO4)2. [Ca2+ ]3[PO 3-]2

 

A)           Ca3 (PO4 )2

Ca3(PO4 )2

 

[Ca2+]3[PO 3-]2

[Ca2+ ]2[PO 3- ]3

C)            Ca3(PO4 )2

D) [Ca2+]2[PO43–]3

E) [Ca2+]3[PO43–]2

8.            Give the expression for the solubility product constant for Cr2(CO3)3.

A) [Cr3+]2[CO32-]3

[Cr3+ ]2[CO 2- ]3

B)            Cr2 (CO3)3

Cr2 (CO3)3

 

 

C)            [Cr3+ ]2[CO

 

2- 3

3

 

[Cr3+ ]3[CO 2- ]2

D)           Cr2 (CO3)3

E) [Cr3+]3[CO32-]2

9.   Which of the following solubility product expressions is incorrect?

A. Cu2S, Ksp = [Cu+ ][S2- ]

B. Co2S3, Ksp = [Co3+] 2 [S2- ] 3

C.            Ni(CN)2, Ksp = [Ni2+][CN- ] 2

D.            AuI, Ksp = [Au+ ][I- ]

E.            Cr(OH)3, Ksp = [Cr3+][OH- ] 3

 

10.          Which of following substances will increase the molar solubility of nickel(II) phosphate in a saturated solution?

A.            KOH

B.            Na3PO4

C.            AgCl

D.            HNO3

E.            AlPO4

 

11.          The hydroxide-ion concentration of a saturated solution of Fe(OH)2 is 1.16×10^-5M. What is the solubility product constant for Fe(OH)2?

A.2.26×10-2

B.7.80×10-16

C.infinity D.1.56×10-15

 

E.6.24×10-15

 

12.          It is found that the concentration of Pb2+ in a saturated solution of lead (II) chloride is 1.6 x 10^-2 M. What is the Ksp for PbCl2?

A. 1.6 x 10^-5

 

13.          The hydroxide ion concentration of a saturated solution of Cu(OH)2 is 4.58 X 10^-7 M. What is the solubility product constant for Cu(OH)2?

A. 4.80 x 10^-20

 

14.  At 25?C, 1.4 × 10-5 mole of Cd(OH)2 dissolves to give 1.0 liter of saturated aqueous solution. What is the solubility product for Cd(OH)2?

a. 1.7 × 10-5

b. 2.9 × 10-10

c. 1.1 × 10-14

d. 5.8 × 10-15

e. 4.1 × 10-12

 

15. If X = the molar solubility (mol/L) of Ni(OH)2, which of the following represents the correct relationship between the Ksp and X, the molar solubility of Ni(OH)2?

a.            Ksp = 4 X^2

b.            Ksp = 4 X^3

c.             Ksp = 2 X^2

d.            Ksp = X^3

e.            Ksp = X^2

 

16.          The Ksp for magnesium arsenate is 2.1 × 10-20 at 25?C. What is the molar solubility of Mg3(AsO4)2 at 25?C?

a. 6.7 × 10-3 M

b. 3.6 × 10-4 M

c. 4.5 × 10-5 M

d. 7.0 × 10-5 M

e. 1.4 × 10-6 M

 

17.          Which of the following has the lowest molar solubility in water at 25?C? a. Ni(CN)2, Ksp = 3.0 × 10^-23

b. ZnS, Ksp = 1.1 × 10^-21

c. PbS, Ksp = 8.4 × 10^-28

d. Co3(AsO4)2, Ksp = 7.6 × 10^-29

e. CaF2, Ksp = 3.9 × 10^-16

 

18.          Which of the following has the lowest molar solubility in water at 25?C? a. SrCO3 (Ksp = 9.3 x 10^-10)

b. PbI2 (Ksp = 6.5 x 10^-9)

c. AgBr (Ksp = 5.0 x 10^-13)

d. Fe(OH)2 (Ksp = 8 x 10^-16)

e. Ni(OH)2 (Ksp = 2.0 x 10^-15)

 

19.          Calculate the concentration of carbonate ion in a saturated solution of calcium carbonate to which calcium chloride has been added until [Ca2+] = 0.015 M at 25?C. Ksp for CaCO3 = 2.8 × 10-9 .

a. 4.2 × 10-11 M

b. 1.9 × 10-7 M

c. 1.2 × 10-5 M

d. 6.3 × 10-13 M

e. 1.5 × 10-2 M

 

20.          The molar solubility of BaCO3 is 9.0 × 10-5 M at 25?C. What is the solubility product constant for BaCO3?

a. 1.2 × 10-8

b. 8.1 × 10-9

c. 5.3 × 10-12

d. 4.0 × 10-15

e. 6.7 × 10-11

 

21.          A solution contains 0.05 M Au+ , 0.05 M Cu+ , and 0.05 M Ag+ ions. When solid NaCl is added to the solution, what is the order in which the chloride salts will begin to precipitate?

Ksp(AgCl) = 1.8 × 10-10 , Ksp(AuCl) = 2.0 × 10-13 , Ksp(CuCl) = 1.9 × 10-7

a.            AuCl > AgCl > CuCl

b.            AuCl > AgCl > NaCl

c.             AgCl > CuCl > AuCl

d.            CuCl > AgCl > AuCl

e.            NaCl > CuCl > AgCl

 

22.          A solution is 0.0010 M in both Ag+ and Au+ . Some solid NaCl is added slowly until the second solid compound just begins to precipitate. What is the concentration of Au+ ions at this point? Ksp for AgCl = 1.8 × 10-10 and for AuCl is 2.0 × 10-13 .

a. 2.0 × 10-10 M

b. 4.5 × 10-7 M

c. 1.8 × 10-7 M

d. 3.0 × 10-4 M

e. 1.1 × 10-6 M

 

23.          Solid silver nitrate is added slowly to a solution that is 0.0010 M in sodium chloride and 0.0010 M in sodium bromide. What % of the bromide ions remain in solution, i.e., unprecipitated, just before silver chloride begins to precipitate? Ksp for AgCl = 1.8 × 10-10 ,

Ksp for AgBr = 3.3 × 10-13

a. 0.18%

b. 0.018%

c. 0.0010%

d. 0.00010%

e. 0.0018%

 

24.          Calculate the concentration of F- ions in saturated CaF2 solution at 25?C. Ksp = 3.9 × 10-11 . a. 2.1 × 10-4 M

b. 4.3 × 10-4 M

c. 0.016 M

d. 0.032 M

e. 0.10 M

 

25.          AgCl would be least soluble at 25?C in    .

a.            pure water

b.            0.1 M CaCl2

c.             0.1 M HCl

d.            0.1 M HNO3

e.            It is equally soluble in all of these substances.

 

26.          Given the following values of Ksp for four slightly soluble sulfides at 25?C.

 

Sulfide  Ksp         Sulfide  Ksp

CdS        3.6 × 10-29          PbS        8.4 × 10-28

CuS        8.7 × 10-36          MnS       5.1 × 10-15

 

Which one of the following ions exists in the lowest concentration in a solution in which the sulfide ion concentration had been fixed at some (fairly large) constant value at 25?C?

a.            Cd2+

b.            Cu2+

c.             Pb2+

d.            Mn2+

e.            Cannot be answered without knowing the sulfide ion concentration.

 

27.          Ksp for lead fluoride is 3.7 × 10-8 . What is the molar solubility of PbF2 in 0.10 M NaF? a. 4.6 × 10-5 M

b. 1.9 × 10-4 M

c. 3.7 × 10-7 M

d. 3.7 × 10-6 M

e. 8.5 × 10-8 M

 

28.          If a solution is to be made 0.010 M in Mg(NO3)2 and 0.20 M in aqueous NH3, how many mol/L of NH4Cl are required to prevent the precipitation of Mg(OH)2 at 25?C? The Kb for aqueous NH3 is 1.8 × 10-5 and the Ksp for Mg(OH)2 is 1.5 × 10-11 .

a. 0.054

b. 0.56

c. 0.092

d. 1.8

e. 0.86

 

 

 

29.          Determine the molar solubility of PbSO4 in pure water. Ksp (PbSO4) = 1.82 × 10-8. A) 1.82 × 10-8 M

B) 1.35 × 10-4 M

C) 9.1 × 10-9 M

D) 3.31 × 10-16 M

E) 4.48 × 10-4 M

30.          Determine the molar solubility of MgCO3 in pure water. Ksp (MgCO3) = 6.82 × 10-6. A) 6.82 × 10-6 M

B) 3.41 × 10-6 M

C) 4.65 × 10-3 M

D) 2.61 × 10-3 M

E) 3.25 × 10-4 M

31.          Determine the molar solubility of AgI in pure water. Ksp (AgI) = 8.51 × 10-17.

A) 9.22 × 10-9 M

B) 4.26 × 10-17 M

C) 8.51 × 10-17 M

D) 2.77 × 10-6 M

E) 4.40  × 10-6 M

32.          Which of the following compounds will have the highest molar solubility in pure water? A) PbS, Ksp = 9.04 × 10-29

B) CuS, Ksp = 1.27 × 10-36

C) Al(OH)3, Ksp = 3 × 10-34

 

D) ZnS, Ksp = 1.6 × 10-24

E) Ag2S, Ksp = 8 × 10-48

33.          The molar solubility of ZnS is 1.6 × 10-12 M in pure water. Calculate the Ksp for ZnS. A) 8.0 × 10-13

B) 3.2 × 10-12

C) 1.6 × 10-35

D) 2.6 × 10-24

E) 6.80 × 10-5

 

34.          The molar solubility of CuI is 2.26 × 10-6 M in pure water. Calculate the Ksp for CuI.

A) 5.11 × 10-12

B) 4.52 × 10-6

C) 1.50 × 10-3

D) 4.62 × 10-17

E) 1.02 × 10-11

 

35.          Determine the molar solubility of CaSO4 in a solution containing 0.100 M Na2SO4. Ksp (CaSO4) = 2.4 × 10-5.

A) 4.9 × 10-3 M

B) 2.4 × 10-4 M

C) 5.8 × 10-10 M

D) 1.2 × 10-5 M

E) 0.10 M

 

36.          Determine the molar solubility of CuCl in a solution containing 0.050 M KCl. Ksp (CuCl) = 1.0  × 10-6.

A) 1.0 × 10-12 M

B) 5.0 × 10-7 M

C) 2.0 × 10-5 M

D) 1.0 × 10-3 M

E) 0.050 M

 

37.          Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr) = 7.7 × 10-13.

A) 8.8 × 10-7 M

B) 3.9 × 10-13 M

C) 5.8 × 10-5 M

D) 5.1 × 10-12 M

E) 0.150 M

 

38.          Determine the molar solubility of Fe(OH)2 in pure water. Ksp (Fe(OH)2) = 4.87 × 10-17. A) 2.44 × 10-17 M

B) 1.62  × 10-17 M

C) 4.03 × 10-9 M

D) 3.65 × 10-6 M

E) 2.30 × 10-6 M

 

39.          Determine the molar solubility of BaF2 in pure water. Ksp (BaF2) = 2.45 × 10-5.

A) 1.83 × 10-2 M

B) 1.23 × 10-5 M

C) 2.90 × 10-2 M

D) 4.95 × 10-3 M

E) 6.13 × 10-6 M

40.          The molar solubility of Ag2S is 1.26 × 10-16 M in pure water. Calculate the Ksp for Ag2S. A) 1.59 × 10-32

B) 1.12 × 10-8

C) 6.81 × 10-63

D) 3.78 × 10-12

E) 8.00 × 10-48

 

41.          Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2)

= 1.7 × 10-6.

A) 2.3 × 10-5 M

B) 8.5 × 10-7 M

C) 1.2 × 10-2 M

D) 0.0750 M

E) 3.0 × 10-4 M

42.          Give the equation for an unsaturated solution in comparing Q with Ksp.

a.            Q > Ksp

b.            Q < Ksp

c.             Q = Ksp

d.            Q ≠ Ksp

e.            None of the above.

 

43.          Which of the following is the correct equation relating Q to Ksp for a saturated solution?

a.            Q > Ksp

b.            Q < Ksp

c.             Q = Ksp

d.            Q ≠ Ksp

e.            Q ≥ Ksp

44.          Which of the following is the correct equation relating Q to Ksp for a supersaturated solution?

a.            Q > Ksp

b.            Q < Ksp

c.             Q = Ksp

d.            Q ≠ Ksp

e.            Q ≥ Ksp

45.          A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 × 10-10.

 

a.            Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations.

b.            Silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl.

c.             Silver chloride will precipitate out of solution, leaving a saturated AgCl solution.

d.            Nothing will happen since NaCl and AgNO3 are both soluble compounds.

e.            There is not enough information to say anything about this solution.

 

46.          A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is

a.            × 10-5 M in calcium ion and 4.75 × 10-5 M in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9.

A)           A precipitate will form since Q > Ksp for calcium oxalate.

B)            Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds.

C)            Nothing will happen since calcium oxalate is extremely soluble.

D)           Nothing will happen since Ksp > Q for all possible precipitants.

E)            There is not enough information to determine.

 

47.          A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is

3.5 × 10-4 M in calcium ion and 2.33 × 10-4 M in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9.

A)           Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds.

B)            Nothing will happen Ksp > Q for all possible precipitants.

C)            A precipitate will form as calcium oxalate is not soluble to any extent.

D)           A precipitate will form since Q > Ksp for calcium oxalate.

E)            There is not enough information to determine.

 

48.          A solution contains 0.021 M Cl? and 0.017 M I?. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl) = 1.0 × 10-6, Ksp(CuI) = 5.1 × 10-12.

A) 3.0 × 10-10 M, CuI

B) 3.0 × 10-10 M, CuCl

C) 4.8 × 10-5 M, CuCl

D) 4.8 × 10-5 M, CuI

E) No precipitate will form at any concentration of copper (I).

 

49.          A solution contains 0.036 M Cu2+ and 0.044 M Fe2+. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuS) = 1.3 × 10-36, Ksp(FeS) = 6.3 × 10-18.

A) 1.4 × 10-16 M, FeS

B) 3.6 × 10-35 M, CuS

C) 3.6 × 10-35 M, FeS

D) 1.4 × 10-16 M, CuS

E) No precipitate will form at any concentration of sulfide ion.

 

50.          A ligand is a molecule or ion that acts as a

a.            Lewis acid

b.            Bronsted-Lowry acid

c.             Bronsted-Lowry base

d.            Lewis base

 

e.            None of the above.

 

51.          Identify the compound that is acid-insoluble.

a.            PbCl2

b.            As2S3

c.             CoS

d.            Ca3(PO4)2

e.            NaCl

 

52.          Identify the compound that is base-insoluble.

a.            PbCl2

b.            As2S

c.             CoS

d.            Ca3(PO4)2

e.            NaCl

 

53.          A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed upon the addition of 6 mol L-1 HCl.

a.            Ba3(PO4)2

b.            CdS

c.             AgCl

d.            NH4Cl

e.            ZnS

 

54.          A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN. If the Kf for Cu(CN)42- is

1.0 × 1025, how much copper ion remains at equilibrium? A) 3.8 × 10-24 M

B) 1.9 x 10-26 M

C) 6.7 × 10-28 M

D) 2.9 × 10-27 M

E) 4.6 × 10-25 M

55.          A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF. If the Kf for AlF63- is 7 × 1019, how much aluminum ion remains at equilibrium?

A) 1.1 × 10-19 M

B) 3.1 × 10-22 M

C) 9.1 × 10-19 M

D) 1.9 × 10-21 M

E) 4.4 × 10-20 M

56.          A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L-1 HCl followed by the addition of H2S and 0.2 mol L-1 HCl.

a.            Ba3(PO4)2

b.            CdS

c.             AgCl

d.            NH4Cl

e.            ZnS

 

57.          A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed

 

after the addition of 6 mol L-1 HCl, followed by the addition of H2S and 0.2 mol L-1 HCl, and subsequently the addition of OH- to a pH of 8.

a.            Ba3(PO4)2

b.            CdS

c.             AgCl

d.            NH4Cl

e.            ZnS

 

58.          A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 mol L-1 HCl; H2S and 0.2 mol L-1 HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3.

a.            Ba3(PO4)2

b.            CdS

c.             AgCl

d.            NH4Cl

e.            ZnS

 

59.          A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the soluble salt remaining in the solution after the addition of 6 mol L-1 HCl, followed by the addition of H2S and 0.2 mol L-1 HCl, then the addition of OH- to a pH of 8, and finally the addition of (NH4)2HPO4 with NH3.

A)           Ba3(PO4)2

B)            CdS

C)            AgCl

D)           NH4Cl

E)            ZnS

 

60.          Describe the solubility of Al(OH)3 with respect to pH.

A)           soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH

B)            soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH

C)            insoluble at low pH, insoluble in pH-neutral solution, and soluble at high pH

D)           soluble at low pH, in pH-neutral solution, and at high pH

E)            insoluble at low pH, in pH-neutral solution, and at high pH

 

61.          What happens at low pH to aluminum hydroxide precipitate?

A)           Al(H2O)63+ is formed and the Al(OH)3 precipitate dissolves.

B)            Al(H2O)2(OH)4- is formed and the precipitate dissolves.

C)            Al(OH)3 precipitate is still present.

D)           Al precipitates.

E)            Al forms.

 

62.          What happens at neutral pH to aluminum hydroxide precipitate?

A)           Al(H2O)63+ is formed and the precipitate dissolves.

B)            Al(H2O)2(OH)4- is formed and the precipitate dissolves.

C)            Al(OH)3 precipitate is still present.

D)           Al precipitates.

E)            Al is formed.

 

63.          What happens at high pH to aluminum hydroxide precipitate?

A)           Al(H2O)63+ is formed and the precipitate dissolves.

 

B)            Al(H2O)2(OH)4- is formed and the precipitate dissolves.

C)            Al(OH)3 precipitate still remains.

D)           Al precipitates.

E)            Al is formed.

 

A)           Silver(I) iodide will precipitate.

B)            No precipitate will form