Ch.17 Full Test Bank Solubility And Simultaneous Equilibria

Chemistry: Molecular Nature of Matter, 8e (Jespersen)

Chapter 17 Solubility and Simultaneous Equilibria

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

Diff: 1

Section: 17.1

2) Which of the following is the expression for the solubility product of Ca3(PO4)2?

A) Ksp = [Ca2+]3 [PO43]2

B) Ksp = [3 × Ca2+]3[2PO43]2

C) Ksp = 3[Ca2+]2[PO43]

D) Ksp = 3[Ca2+]3 + 2[PO43]2

E) Ksp = [Ca2+]3[PO43]2

Diff: 1

Section: 17.1

3) Which of the following is the expression for the solubility product of Fe2(CrO4)3?

A) Ksp = [Fe2+]3[CrO43]2

B) Ksp = [2 × Fe2+]3[3CrO43]2

C) Ksp = 3[Fe2+] 2[CrO43]

D) Ksp = 2[Fe2+]3 + 3[CrO43]2

E) Ksp = [Fe3+]2[CrO42]3

Diff: 1

Section: 17.1

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

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

Diff: 1

Section: 17.1

5) Which of the following is the expression for the solubility product of calcium fluoride, CaF2?

A) Ksp = [Ca2+][2 × F]

B) Ksp = [Ca2+] 2[F]2

C) Ksp = [Ca2+]2[F]

D) Ksp = [Ca2+][F]2

E) Ksp = [Ca2+] ½[F]2

Diff: 1

Section: 17.1

6) Which of the following is the expression for the solubility product of silver oxalate (Ag2C2O4)?

A) Ksp = [Ag22+][C2O42]

B) Ksp = [Ag+][C2O42]2

C) Ksp = 2[Ag+][C2O42]

D) Ksp = [Ag+]2[C2O42]

E) Ksp = 2[Ag+]2[C2O42]

Diff: 1

Section: 17.1

7) The solubility of magnesium carbonate, MgCO3, in pure water is 2.6 × 10-4 moles per liter. Calculate the value of Ksp for magnesium carbonate from this data.

A) 5.2 × 10-4

B) 6.8 × 10-8

C) 1.4 × 10-7

D) 2.7 × 10-7

E) 4.6 × 10-15

Diff: 1

Section: 17.1

8) The solubility of calcium oxalate, CaC2O4, in pure water is 4.8 × 10-5 moles per liter. Calculate the value of Ksp for calcium oxalate from this data.

A) 2.4 × 10-5

B) 9.6 × 10-5

C) 4.6 × 10-9

D) 2.3 × 10-9

E) 5.3 × 10-18

Diff: 1

Section: 17.1

9) The solubility of scandium(III) fluoride, ScF3, in pure water is 2.0 × 10-5 moles per liter. Calculate the value of Ksp for scandium(III) fluoride from this data.

A) 1.3 × 10-17

B) 1.4 × 10-18

C) 4.3 × 10-18

D) 1.6 × 10-19

E) 4.8 × 10-19

Diff: 1

Section: 17.1

10) 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.

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

Diff: 2

Section: 17.1

11) The solubility of calcium fluoride, CaF2, in pure water is 2.15 × 10-4 moles per liter. Calculate the value of Ksp for calcium fluoride from this data.

A) 1.85 × 10-7

B) 9.28 × 10-8

C) 1.99 × 10-11

D) 3.98 × 10-11

E) 9.94 × 10-12

Diff: 2

Section: 17.1

12) The solubility of copper(II) arsenate, Cu3(AsO4)2, in pure water is 3.7 × 10-8 moles per liter. Calculate the value of Ksp for copper(II) arsenate from this data.

A) 6.9 × 10-38

B) 4.2 × 10-37

C) 2.5 × 10-36

D) 3.7 × 10-36

E) 7.5 × 10-36

Diff: 2

Section: 17.1

13) The solubility of zinc(II) phosphate, Zn3(PO4)2, in pure water is 1.5 × 10-7 moles per liter. Calculate the value of Ksp for zinc(II) phosphate from this data.

A) 2.3 × 10-14

B) 5.1 × 10-28

C) 2.7 × 10-33

D) 8.2 × 10-33

E) 7.6 × 10-35

Diff: 2

Section: 17.1

14) The solubility of silver oxalate, Ag2C2O4, in pure water is 2.06 × 10-4 moles per liter. Calculate the value of Ksp for silver oxalate from this data.

A) 4.24 × 10-8

B) 8.49 × 10-8

C) 1.75 × 10-11

D) 3.50 × 10-11

E) 8.74 × 10-12

Diff: 2

Section: 17.1

15) The solubility of silver carbonate, Ag2CO3, in pure water is 1.27 × 10-4 moles per liter. Calculate the value of Ksp for silver carbonate from this data.

A) 1.64 × 10-11

B) 3.28 × 10-11

C) 2.04 × 10-12

D) 4.10 × 10-12

E) 8.19 × 10-12

Diff: 2

Section: 17.1

16) Which one of the following salts has the highest solubility in water, expressed in moles per liter?

A) PbF2, Ksp = 3.6 × 10-8

B) Ag2CrO4, Ksp = 1.2 × 10-12

C) CaF2, Ksp = 3.9 × 10-11

D) BaF2, Ksp = 1.7 × 10-6

E) PbI2, Ksp = 7.9 × 10-9

Diff: 2

Section: 17.1

17) Which one of the compounds below has the highest molar solubility in water?

A) SrF2, Ksp = 2.8 × 10-9

B) Sr(IO3)2, Ksp = 3.3 × 10-7

C) Fe(OH)2, Ksp = 8.0 × 10-16

D) PbCl2, Ksp = 1.6 × 10-5

E) PbBr2, Ksp = 3.9 × 10-5

Diff: 2

Section: 17.1

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

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

Diff: 2

Section: 17.1

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

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) PbI2, Ksp = 7.9 × 10-9

Diff: 2

Section: 17.1

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

A) solubility = 2[Ag+]

B) solubility = [Ag+]

C) solubility = [2Ag+]

D) solubility = 2[SO42]

E) solubility = [SO42]

Diff: 2

Section: 17.1

21) The solubility of strontium fluoride, SrF2, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

A) solubility = 2[Sr2+]

B) solubility = [Sr2+]

C) solubility = [2 Sr2+]

D) solubility = 2[F]

E) solubility = [F]

Diff: 2

Section: 17.1

22) The solubility of copper(II) iodate, Cu(IO3)2, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

A) solubility = 2[Cu2+]

B) solubility = [Cu2+]

C) solubility = [2 Cu2+]

D) solubility = 2[IO3]

E) solubility = [IO3]2

Diff: 2

Section: 17.1

23) The solubility of silver phosphate, Ag3PO4, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?

A) solubility = 3[Ag+]

B) solubility = [Ag+]

C) solubility = [Ag+]3

D) solubility = [PO43-]

E) solubility = [PO43-]3

Diff: 2

Section: 17.1

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

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

Diff: 2

Section: 17.1

25) The solubility product for Ag3PO4 is: Ksp = 2.8 × 10-18. What is the solubility of Ag3PO4 in water, in grams per liter?

A) 1.2 × 10-15 g/L

B) 7.5 × 10-3 g/L

C) 2.0 × 10-4 g/L

D) 9.9 × 10-3 g/L

E) 1.2 × 10-3 g/L

Diff: 2

Section: 17.1

26) The solubility product for PbBr2 is: Ksp = 6.6 × 10-6. Which of the following represents the solubility of PbBr2?

A) 4.7 × 10-1 g/L

B) 2.4 × 10-3 g/L

C) 6.0 × 10-4 g/L

D) 4.3 g/L

E) 6.1 × 10-4 g/L

Diff: 2

Section: 17.1

27) The solubility product for BaSO4 is 1.1 × 10-10. Calculate the solubility of BaSO4 in pure water.

A) 5.5 × 10-11 mol L-1

B) 1.0 × 10-5 mol L-1

C) 2.1 × 10-5 mol L-1

D) 1.1 × 10-10 mol L-1

E) 2.2 × 10-10 mol L-1

Diff: 2

Section: 17.1

28) The solubility product for PbCl2 is 1.7 × 10-5. What is the solubility of PbCl2 in pure water?

A) 2.4 × 10-4 mol L-1

B) 6.2 × 10-2 mol L-1

C) 7.7 × 10-3 mol L-1

D) 1.6 × 10-2 mol L-1

E) 6.0 × 10-5 mol L-1

Diff: 2

Section: 17.1

29) Calculate the concentration of chloride ions in a saturated solution of lead(II) chloride.

The Ksp = 1.7 × 10-5.

A) 2.4 × 10-4 M

B) 4.8 × 10-4 M

C) 3.9 × 10-2 M

D) 1.2 × 10-1 M

E) 3.2 × 10-2 M

Diff: 2

Section: 17.1

30) Calculate the concentration of bromide ions in a saturated solution of lead(II) bromide.

The Ksp = 6.6 × 10-6.

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

Diff: 2

Section: 17.1

31) Calculate the concentration of iodate ions in a saturated solution of lead(II) iodate, Pb(IO3)2. The Ksp = 2.6 × 10-13.

A) 3.2 × 10-5 M

B) 4.0 × 10-5 M

C) 6.4 × 10-5 M

D) 8.0 × 10-5 M

E) 5.1 × 10-7 M

Diff: 2

Section: 17.1

32) Calculate the concentration of iodate ions in a saturated solution of barium iodate, Ba(IO3)2. The Ksp = 1.5 × 10-9.

A) 1.4 × 10-3 M

B) 2.3 × 10-3 M

C) 7.2 × 10-4 M

D) 3.9 × 10-5 M

E) 7.7 × 10-5 M

Diff: 2

Section: 17.1

33) The solubility product of barium fluoride (BaF2) is 1.7 × 10-6. Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.

A) 7.6 × 10-3 M

B) 1.5 × 10-2 M

C) 3.4 × 10-5 M

D) 1.7 × 10-6 M

E) 3.4 × 10-6 M

Diff: 2

Section: 17.1

34) The solubility product for Mg3(PO4)2 is 6.3 × 10-26. What is the solubility of Mg3(PO4)2 in pure water, in grams per liter?

A) 1.7 × 10-23 g L-1

B) 3.4 × 10-7 g L-1

C) 9.4 × 10-4 g L-1

D) 1.2 × 10-3 g L-1

E) 2.4 × 10-3 g L-1

Diff: 2

Section: 17.1

35) The solubility of lead iodide is 578 mg L-1 at 25 °C. What is the Ksp for PbI2?

A) 7.9 × 10-9

B) 1.6 × 10-6

C) 1.1 × 10-11

D) 2.7 × 10-12

E) 6.3 × 10-6

Diff: 2

Section: 17.1

36) The solubility of barium carbonate is 14.8 mg L-1 at 30 °C. Calculate the Ksp value for BaCO3.

A) 7.5 × 10-5

B) 1.5 × 10-4

C) 5.6 × 10-9

D) 7.5 × 10-6

E) 1.5 × 10-3

Diff: 2

Section: 17.1

37) How many grams of lead(II) chloride would dissolve in 100 mL of water? The Ksp for lead(II) chloride is 2.4 × 10-4 and the molar mass is 278.1 g/mol.

A) 1.1 g

B) 0.039 g

C) 10.9 g

D) 4.3 g

E) 1.4 × 10-4 g

Diff: 2

Section: 17.1

38) What is the solubility, in moles per liter, of Fe(OH)2 (Ksp = 7.9 × 10-16), in 0.0500 molar NaOH 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.

A) 3.16 × 10-13

B) 3.13 × 10-16

C) 1.58 × 10-14

D) 1.14 × 10-14

E) 3.16 × 10-16

Diff: 3

Section: 17.1

39) What is the solubility, in moles per liter, of PbSO4 (Ksp = 6.3 × 10-7) in 0.0230 molar MgSO4 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.

A) 2.14 × 10-5

B) 7.24 × 10-5

C) 2.74 × 10-5

D) 4.72 × 10-5

E) 4.27 × 10-5

Diff: 3

Section: 17.1

40) What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10), in 0.0300 M CaCl2 solution?

Hint: Be sure to account for the presence of a common ion and carefully organize. You should also be able to simplify the math because the solubility is very low.

A) 9.0 × 10-3

B) 9.0 × 10-6

C) 6.0 × 10-9

D) 3.0 × 10-9

E) 6.0 × 10-3

Diff: 3

Section: 17.1

41) What is the solubility, in moles per liter, of BaSO4 (Ksp = 1.1 × 10-10), in 0.0100 M Na2SO4 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.

A) 1.1 × 10-8

B) 1.1 × 10-6

C) 1.1 × 10-7

D) 1.1 × 10-5

E) 1.1 × 10-4

Diff: 3

Section: 17.1

42) 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.

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

Diff: 3

Section: 17.1

43) What is the solubility, in moles per liter, of Ag2CO3 (Ksp = 8.1 × 10-12), in 0.0300 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.

A) 8.2 × 10-6

B) 9.0 × 10-9

C) 3.0 × 10-7

D) 4.0 × 10-10

E) 2.7 × 10-9

Diff: 3

Section: 17.1

44) What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10), in 0.0100 molar aqueous potassium chloride 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.

A) 7.5 × 10-5 mol L-1

B) 1.8 × 10-8 mol L-1

C) 1.3 × 10-6 mol L-1

D) 3.6 × 10-8 mol L-1

E) 1.5 × 10-7 mol L-1

Diff: 3

Section: 17.1

45) The solubility of barium sulfate varies with the composition of the solvent in which it is dissolved. In which solvent mixture would BaSO4 have the lowest solubility? Assume all solutions are at 25 °C.

A) pure water

B) 0.10 M Na2SO4(aq)

C) 1.0 M (NH4)2SO4(aq)

D) 0.5 M Ba(NO3)2(aq)

E) 1.0 M HCl(aq)

Diff: 2

Section: 17.1

46) The solubility of PbI2 (Ksp = 9.8 × 10-9) varies with the composition of the solvent in which it was dissolved. In which solvent mixture would PbI2 have the lowest solubility at identical temperatures?

A) pure water

B) 1.0 M Pb(NO3)2(aq)

C) 1.5 M KI(aq)

D) 0.8 M MgI2(aq)

E) 1.0 M HCl(aq)

Diff: 2

Section: 17.1

47) What is the maximum concentration of Mg2+ ion that can exist in a 0.10 M NaF(aq) solution, without precipitating any magnesium fluoride? The Ksp of MgF2 is 6.6 × 10-9.

A) 1.3 × 10-7 M

B) 6.6 × 10-9 M

C) 6.6 × 10-8 M

D) 1.6 × 10-7 M

E) 6.6 × 10-7 M

Diff: 2

Section: 17.1

48) Calculate the minimum concentration of Ag+ ion that must be added to (or built up in) a 0.140 M Na2CrO4 solution, in order to initiate a precipitation of silver chromate. The Ksp of Ag2CrO4 is 1.2 × 10-12.

Hint: Use an ICE table to help organize your given information and remember to account for the presence of a common ion.

A) 4.8 × 10-9 mol L-1

B) 2.9 × 10-6 mol L-1

C) 2.0 × 10-6 mol L-1

D) 9.5 × 10-7 mol L-1

E) 1.4 × 10-6 mol L-1

Diff: 3

Section: 17.1

49) The solubility product for Ag3PO4 is 2.8 × 10-18. What is the solubility of silver phosphate in a solution which also contains 0.10 moles of silver nitrate per liter?

Hint: Use an ICE table to help organize your given information and remember to account for the presence of a common ion.

A) 4.4 × 10-4 mol L-1

B) 4.4 × 10-15 mol L-1

C) 2.8 × 10-15 mol L-1

D) 3.6 × 10-16 mol L-1

E) 2.8 × 10-13 mol L-1

Diff: 3

Section: 17.1

50) Will a precipitate form when 20.0 mL of 1.8 × 10-3 M Pb(NO3)2 is added to 30.0 mL of

5.0 × 10-4 M Na2SO4? The Ksp of (PbSO4) is 6.3 × 10-7.

Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

A) no, because the ion product, Q < Ksp

B) no, because the ion product, Q > Ksp

C) yes, because the ion product, Q < Ksp

D) yes, because the ion product, Q > Ksp

E) no, because Ksp is less than the ion product

Diff: 3

Section: 17.1

51) 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.

A) yes, because the ion product, Q > Ksp

B) no, because the ion product, Q < Ksp

C) no, because the ion product, Q = Ksp

D) yes, because the ion product, Q < Ksp

E) no, because the ion product, Q > Ksp

Diff: 3

Section: 17.1

52) The pH of a saturated solution of cerium (III) hydroxide in water is 9.20. Use this data to calculate a value for the solubility product constant of cerium(III) hydroxide.

Hint: Use an ICE table to help organize your given information and use pH to find the equilibrium [OH-].

A) 2.5 × 10-10

B) 8.4 × 10-11

C) 4.0 × 10-19

D) 2.1 × 10-20

E) 6.3 × 10-20

Diff: 3

Section: 17.1

53) 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 for

AgI 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.

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

Diff: 3

Section: 17.1

54) For PbCl2, Ksp = 1.7 × 10-5. Will a precipitate of PbCl2 form when 200 mL of 3.0 × 10-2 M Pb(NO3)2 solution is added to 300 mL of 5.0 × 10-2 M KCl?

Hint: Find the concentration of each ion in the insoluble compound, and use those to find Q.

A) yes, the ion product, Q > Ksp

B) no, the ion product, Q < Ksp

C) no, the ion product, Q = Ksp

D) yes, the ion product, Q < Ksp

E) no, because the ion product, Q > Ksp

Diff: 3

Section: 17.1

55) Methylamine, CH3NH2, is a weak molecular base with a value of 4.4 × 10-4 for Kb. An aqueous solution contains 0.200 M CH3NH2 and 0.400 M CH3NH3Cl per liter as the only solutes. If the Ksp of Mg(OH)2 is 7.1 × 10-12, what is the maximum [Mg2+] that can coexist with these solutes in the solution?

Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, and then use that to find [OH-].

A) 8.1 × 10-9

B) 3.2 × 10-8

C) 9.2 × 10-6

D) 1.5 × 10-4

E) 3.7 × 10-1

Diff: 3

Section: 17.1

56) Methylamine, CH3NH2, is a weak molecular base with a value of 4.4 × 10-4 for Kb. An aqueous solution contains 0.200 M CH3NH2 and 0.300 M CH3NH3Cl 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, and then use that to find [OH-].

A) 1.8 × 10-12

B) 9.0 × 10-12

C) 1.8 × 10-9

D) 9.2 × 10-9

E) 9.2 × 10-6

Diff: 3

Section: 17.1

57) Dimethylamine, (CH3)2NH, is a weak molecular base with a value of 9.6 × 10-4.for Kb. An aqueous solution contains 0.350 M (CH3)2NH and 0.250 M (CH3)2NH2Cl per liter as the only solutes. If the Ksp of Mg(OH)2 is 7.1 × 10-12, what is the maximum [Mg2+] that can coexist with these solutes in the solution?

Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, and then use that to find [OH-].

A) 1.7 × 10-7

B) 3.9 × 10-6

C) 7.7 × 10-6

D) 1.5 × 10-5

E) 4.9 × 10-3

Diff: 3

Section: 17.1

58) Which of the following would decrease the concentration of Pb+2 ionized in a solution of PbI2?

A) adding a solution of KI

B) adding a solution of Pb(NO3)2

C) changing the pH of the solution

D) addition of a catalyst

E) adding a solution of NaNO3

Diff: 1

Section: 17.1

59) Zinc carbonate, a slightly soluble substance, is most soluble in which of the following solvents?

A) water

B) 0.1 M ZnCl2(aq)

C) 0.1 M NaOH(aq)

D) 0.1 M HCl(aq)

E) 0.2 M Na2CO3(aq)

Diff: 2

Section: 17.2

60) The value of the solubility product constant for barium carbonate is 5.0 × 10-9 and that of barium chromate is 2.1 × 10-10. From this data, what is the value of Kc for the reaction below?

BaCO3(s) + CrO42-(aq) BaCrO4(s) + CO32-(aq)

Hint: Combine reactions and Ksp values like all other reactions and equilibrium constants.

A) 1.1 × 10-18

B) 4.2 × 10-2

C) 4.8 × 10-9

D) 4.9

E) 24

Diff: 3

Section: 17.2

61) The value of the solubility product constant for silver carbonate is 8.5 × 10-12 and that of silver chromate is 1.1 × 10-12. From this data, what is the value of Kc for the reaction below?

Ag2CO3(s) + CrO42-(aq) Ag2CrO4(s) + CO32-(aq)

Hint: Combine reactions and Ksp values like all other reactions and equilibrium constants.

A) 9.6 × 10-12

B) 1.3 × 10-1

C) 1.1 × 1023

D) 7.7

E) 9.4 × 10-24

Diff: 3

Section: 17.2

62) The value of the solubility product constant for calcium oxalate is 2.3 × 10-9 and that of calcium sulfate is 4.9 × 10-5. From this data, what is the value of Kc for the reaction below?

CaC2O4(s) + SO42-(aq) CaSO4(s) + C2O42-(aq)

Hint: Combine reactions and Ksp values like all other reactions and equilibrium constants.

A) 1.1 × 10-13

B) 4.7 × 10-5

C) 8.9 × 1012

D) 4.9 × 10-5

E) 2.1 × 104

Diff: 3

Section: 17.2

63) Which solid would be more soluble in a strong acid solution than in pure water?

A) KCl

B) MgCl2

C) NaNO3

D) LiBr

E) ZnCO3

Diff: 2

Section: 17.2

64) Which solid would be more soluble in a strong acid solution than in pure water?

A) NaCl

B) MgBr2

C) LiNO3

D) CaCO3

E) AgBr

Diff: 2

Section: 17.2

65) Given the following information:

Ni(OH)2(s) Ni2+(aq) + 2 OH(aq) Ksp = 6.0 × 10-16

H2O(l) H+(aq) + OH(aq) Kw = 1.0 × 10-14

What is the equilibrium constant for the reaction below?

Ni(OH)2(s) + 2 H+(aq) Ni2+(aq) + 2 H2O(l)

A) 1.7 × 1015

B) 6.0 × 10-1

C) 6.0 × 1012

D) 1.7 × 10-13

E) 3.3 × 101

Diff: 1

Section: 17.2

66) Given the following information:

ZnCO3(s) Zn2+(aq) + CO32-(aq) Ksp = 1.5 × 10-10

HCO3-(aq) CO32-(aq) + H+(aq) Ka2 = 5.6 × 10-11

What is the equilibrium constant for the reaction below?

ZnCO3(s) + H+(aq) Zn2+(aq) + HCO3-(aq)

A) 8.4 × 10-21

B) 3.7 × 10-1

C) 1.2 × 1020

D) 2.7

E) 2.1 × 10-10

Diff: 1

Section: 17.2

67) PbCO3, PbCl2, PbI2, and PbS are all only very slightly soluble in pure water. Which one (ones) should be significantly more soluble in acidic solution than in pure water?

A) PbI2, PbS and PbCO3

B) only PbCO3 and PbS

C) only PbCl2 and PbI2

D) only PbCO3

E) All four are significantly more soluble in acidic solution.

Diff: 2

Section: 17.2

68) The group Zn(NO3)2, Zn(CO3)2, ZnCl2, and ZnS contains some salts which are only very slightly soluble in pure water. Of those salts, which one(s) should be significantly more soluble in acidic solution than in pure water?

A) Zn(NO3)2, Zn(CO3)2, and ZnCl2

B) Zn(NO3)2, and Zn(CO3)2

C) ZnCl2, and ZnS

D) Zn(CO3)2, and ZnCl2

E) Zn(CO3)2, and ZnS

Diff: 2

Section: 17.2

69) 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) 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.

Diff: 2

Section: 17.3

70) The acid solubility product, Kspa, for PbS refers to which of the following reactions?

A) PbS(s) + 2H2O(l) H+(aq) + Pb(OH)2(s) + HS-(l)

B) PbS(s) + 2H2O(aq) H+(aq) + Pb(OH)2(s) + HS-(aq)

C) PbS(s) + 2H2O(l) H+(l) + Pb(OH)2(s)

D) PbS(s) + 2H+(aq) Pb2+(aq) + H2S(aq)

E) PbS(s) + 2H+(l) H+(aq) + Pb(OH)2(s) + HS-(aq)

Diff: 1

Section: 17.3

71) A solution contains Ba2+ (1.0 × 10-3 M), Ca2+ (1.0 × 10-3 M) and K+ (1.0 × 10-3 M). Drops of a 5.0 × 10-1 M solution of NaF were added through a microburet until the [F-] in the solution mix reached 1.5 × 10-3 M. Should a precipitate form? If so, what is the precipitate? The Ksp values are BaF2: 1.0 × 10-6, CaF2: 5.3 × 10-9. (Neglect the slight change in volume resulting from the added NaF solution.)

A) a precipitate consisting of BaF2 only should form

B) a precipitate consisting of CaF2 and KF should form

C) a precipitate consisting of BaF2 and CaF2 should form

D) a precipitate consisting of CaF2 only should form

E) No precipitate should form.

Diff: 2

Section: 17.4

72) A solution contains Ba2+ (1.0 × 10-3 M), Ca2+ (1.0 × 10-3 M) and K+ (1.0 × 10-3 M). Drops of a 5.0 10-1 M solution of NaF were added through a microburet until the [F-] in the solution mix reached 3.0 × 10-3 M. Should a precipitate form? If so, what is the precipitate? The Ksp values are BaF2: 1.0 × 10-6, CaF2: 5.3 × 10-9. (Neglect the slight change in volume resulting from the added NaF solution.)

A) a precipitate consisting of BaF2 only should form

B) a precipitate consisting of CaF2 and KF should form

C) a precipitate consisting of BaF2 and CaF2 should form

D) a precipitate consisting of CaF2 only should form

E) No precipitate should form.

Diff: 2

Section: 17.4

73) A solution contains Ba2+ (1.0 × 10-3 M), Ca2+ (1.0 × 10-3 M) and K+ (1.0 × 10-3 M). Drops of a 5.0 × 10-1 M solution of NaF were added through a microburet until the [F-] in the solution mix reached 6.0 × 10-3 M. Should a precipitate form? If so, what is the precipitate? The Ksp values are BaF2: 1.0 × 10-6, CaF2: 5.3 × 10-9. (Neglect the slight change in volume resulting from the added NaF solution.)

A) a precipitate consisting of BaF2 only should form

B) a precipitate consisting of CaF2 and KF should form

C) a precipitate consisting of BaF2 and CaF2 should form

D) a precipitate consisting of CaF2 only should form

E) No precipitate should form.

Diff: 2

Section: 17.4

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

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.

Diff: 2

Section: 17.5

75) In an aqueous solution, copper ions can form the complex ion [Cu(H2O)6]+2(aq). In [Cu(H2O)6]+2(aq),

A) [Cu(H2O)6]+2(aq) is a complex ion; H2O is the solvent; Cu+2 is a ligand.

B) [Cu(H2O)6]+2(aq) is a complex ion; H2O is a ligand; Cu+2 is an acceptor.

C) [Cu(H2O)6]+2(aq) is a complex ion; H2O is a donor atom; Cu+2 is a ligand.

D) [Cu(H2O)6]+2(aq) is a ligand; H2O is an acceptor; Cu+2 is a complex ion.

E) [Cu(H2O)6]+2(aq) is a complex ion; H2O is a ligand; Cu+ is an acceptor.

Diff: 1

Section: 17.5

76) Mercury ions (Hg2+) are very difficult to dissolve in a solution of water, or even a dilute solution of NaOH. But if ammonia is added to the water, mercury ions are more readily soluble. Which of the following best explains why this happens?

A) Mercury ions form complex ions with ammonia in solution, which aids the solution process.

B) Ammonia causes the mercury ions to become oxidized.

C) Ammonia causes the mercury ions to lose their charge.

D) Mercury is more soluble in a basic solution than in a neutral solution.

E) This process is still not fully understood by chemist.

Diff: 1

Section: 17.5

77) 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 would be the equilibrium constant for the reaction below?

AgBr(s) + 2 S2O32-(aq) Ag(S2O3)23-(aq) + Br-(aq)

A) 2.0 × 1013

B) 5.0 × 10-1

C) 4.0 × 1025

D) 5.0 × 10-13

E) 10

Diff: 2

Section: 17.6

78) A precipitate will form when a solution containing a cation and a solution containing an anion are mixed if the ________ exceeds the value of the ________.

Diff: 1

Section: 17.1

79) Addition of a common ion to a solution of a slightly soluble salt will ________ the solubility of the slightly soluble salt.

Diff: 1

Section: 17.1

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

Diff: 2

Section: 17.1

81) The pH of a saturated solution of Ca(OH)2 is 12.37. What is the Ksp of Ca(OH)2? ________

Diff: 2

Section: 17.1

82) What is the molar solubility of Ca(OH)2 in a 0.300 M NaOH solution? The Ksp of Ca(OH)2 is 6.5 × 10-6.

Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

Diff: 3

Section: 17.1

83) What is the molar solubility of AgCl in a 0.450 M solution of KCl?

The Ksp of AgCl is 1.8 × 10-10.

Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

Ksp = [Ag] [Cl].

Setting up a concentration table, we have

AgCl(s) Ag+(aq) + (aq)

Initial — 0 0.450

Change — +x +x

Equilibrium — +x 0.450 + x

If we assume that x is small, and substitute into our Ksp expression, we're left with

Ksp = [x] [0.450]. Solving for x gives us a molar solubility of 4.0 × 10-10 mol L-1. Compared to the chloride concentration of 0.450 mol L-1 this is extremely small. Therefore, our assumption is valid.

Diff: 3

Section: 17.1

84) A student mixes 100.00 mL of 0.250 M MgSO4 with 250.00 mL 0.100 M NaOH. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.

Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

Ksp for Mg(OH)2 = 5.6 × 10-12

Diff: 3

Section: 17.1

85) The solubility product for chromium(III) fluoride is Ksp = 6.6 × 10-11. Using this information, what is the molar solubility of chromium(III) fluoride?

Diff: 2

Section: 17.1

86) Calculate the minimum concentration of Cr3+ that must be added to 0.085 M NaF in order to form a precipitate of chromium(III) fluoride. The solubility constant for CrF3 is 6.6 × 10-11.

Diff: 2

Section: 17.1

87) Calculate the concentration of chloride ions in a saturated lead(II) chloride solution.

The Ksp = 2.4 × 10-4 for lead(II) chloride.

Diff: 2

Section: 17.1

88) A student mixes 50.00 mL of 0.500 M NaCl with 75.00 mL of 0.200 M AgNO3. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.

Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq).

We need to find the concentrations of Ag+ and Cl- in solution. The overall volume of the solution is 125.00 mL.

mol Ag+ = 0.200 × 0.07500 L × = 0.120 M Ag+

mol Cl- = 0.500 × 0.05000 L × = 0.200 M Cl-

We find that Q = [Ag+][Cl-] = 2.40 × 10-2. The value of Ksp for AgCl is 1.8 × 10-10. Since Q > Ksp, a precipitate does form.)

Diff: 3

Section: 17.1

89) The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C. What is the solubility product constant for lead(II) iodide at this temperature?

Diff: 2

Section: 17.1

90) 200 mL of an aqueous solution contains 0.030 M concentrations of both Sr2+ and Ca2+. If 100 mL of 2.0 × 10-3 M Na2SO4 is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for SrSO4 and CaSO4 are 2.4 × 10-5 and 3.2 × 10-7.

Hint: Remember that the solutions are diluted.

Diff: 3

Section: 17.1

91) Given the following information:

MgCO3(s) Mg2+(aq) + CO32-(aq) Ksp = 6.8 × 10-8

HCO3-(aq) CO32-(aq) + H+(aq) Ka2 = 5.6 × 10-11

What is the equilibrium constant for the reaction,

MgCO3(s) + H+(aq) Mg2+(aq) + HCO3-(aq)

Diff: 1

Section: 17.2

92) For the H2CO3/ HCO3/CO32- system at room temperature Ka1 = 4.5 × 10-7, while

Ka2 = 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)

Diff: 2

Section: 17.2

93) Many metal sulfides have ________ solubilities.

Diff: 2

Section: 17.3

94) Metal sulfides actually dissolve in water by ________ with water, not by releasing S2- ions into water.

Diff: 2

Section: 17.3

95) Metal cations in the chloride solubility group can be separated from other cations because they form ________ chloride compounds in a solution of HCl.

Diff: 2

Section: 17.4

96) Group II and group III cations (acid-insoluble and base-insoluble sulfides) can be separated out by forming a precipitate of acid-insoluble cations at low ________.

Diff: 1

Section: 17.4

97) 200 mL of an aqueous solution contains 0.030 M concentrations of both Sr2+ and Ca2+. If 100 mL of 2.0 × 10-5 M Na2SO4 is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for SrSO4 and CaSO4 are 2.4 × 10-5 and 3.2 × 10-7.

Hint: Remember that the solutions are being diluted and use the diluted concentrations

Diff: 3

Section: 17.4

98) 200 mL of an aqueous solution contains 0.030 M concentrations of both Sr2+ and Ca2+. If 100 mL of 6.0 × 10-3 M Na2SO4 is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for SrSO4 and CaSO4 are 2.4 × 10-5 and 3.2 × 10-7.

Hint: Remember that the solutions are being diluted and use the diluted concentrations

Diff: 3

Section: 17.4

99) 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag+. If 100 mL of 6.0 × 10-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 × 10-5 and 1.8 × 10-10.

Hint: Remember that the solutions are being diluted and use the diluted concentrations.

Diff: 3

Section: 17.4

100) 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag+. If 100 mL of 0.20 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 × 10-5 and 1.8 × 10-10.

Hint: Remember that the solutions are being diluted and use the diluted concentrations.

Diff: 3

Section: 17.4

101) The formation constant for the diammine silver(I) ion is 1.6 × 107, while the solubility product constant for silver chloride is 1.8 × 1010. What is the equilibrium constant for the reaction,

AgCl(s) + 2 NH3(aq) Ag(NH3)2+(aq) + Cl(aq)?

Diff: 1

Section: 17.5

102) 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.

Diff: 3

Section: 17.5

103) The formation constant for the tris(ethylenediammine)nickel(II) complex ion, [Ni(en)3]2+, is 4.1 × 1017. What is the concentration of the free nickel(II) ion in a solution in which the equilibrium concentration of free ethylenediammine is 0.400 M, and that of the nickel complex above is 0.0100 M?

Diff: 2

Section: 17.5

104) 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?

Diff: 1

Section: 17.5

105) What would be the molar solubility of AgI in a 1.0 M NH3 solution?

The Ksp of AgI is 8.3 × 10-17, and the formation constant of [Ag(NH3)2]+ is 1.6 × 107.

Hint: Combine the formation and solubility reactions to find the overall reaction and its equilibrium constant and account for the presence of a common ion.

Diff: 3

Section: 17.6

106) 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)?

Diff: 2

Section: 17.6

107) The formation constant for the diammine silver(I) ion is 1.6 × 107, while the solubility product constant for silver chloride is 1.8 × 10-10. Given the reaction,

AgCl(s) + 2 NH3(aq) Ag(NH3)2+(aq) + Cl(aq)

What is the solubility, in moles per liter, of silver chloride in 1.00 molar ammonia solution?

Hint: Combine the formation and solubility reactions to find the overall reaction and its equilibrium constant and account for the presence of a common ion.

Diff: 3

Section: 17.6

108) 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. Considering the reaction,

AgBr(s) + 2 S2O32-(aq) Ag(S2O3)23-(aq) + Br(aq)

What is the solubility, in moles per liter, of silver bromide in 0.200 M sodium thiosulfate solution?

Hint: Combine the formation and solubility reactions to find the overall reaction and its equilibrium constant and account for the presence of a common ion.

Diff: 3

Section: 17.6

109) How many grams of AgCl can dissolve in 1.00 L of 1.50 M NH3?

The Ksp of AgCl is 1.80 × 10-10, and the formation constant of [Ag(NH3)2]+ is 1.60 × 107.

Hint: Combine the formation and solubility reactions to find the overall reaction and its equilibrium constant and account for the presence of a common ion.

AgCl(s) Ag+(aq) + Cl-(aq)

Ag+(aq) + 2NH3(aq) [Ag(NH3)2]+(aq)

AgCl(s) + 2NH3(aq) [Ag(NH3)2]+(aq) + Cl-

We arrive at an equilibrium constant for the overall reaction by multiplying the Kform by Ksp, giving 2.88 × 10-3. The overall equilibrium expression then is

Kc =

Setting up a concentration table, we can find out how to express each of the above concentrations.

AgCl(s) + 2NH3(aq) [Ag(NH3)2]+(aq) + Cl-(aq)

Initial — 1.5 0 0

Change — -2x +x +x

Equilibrium — 1.5 - 2x +x +x

Plugging these values into the Kc expression and solving for x, we find x = 0.0727 M. Since there is 1 L of solution, we can express this as 0.0727 mol of AgCl dissolved in 1.0 L. Converting from moles to grams:

massAgCl = 0.0727 mol AgCl × = 10.4 g AgCl

Diff: 3

Section: 17.6

110) The oxide ion can exist in aqueous solutions provided the pH is higher than 11.00.

Diff: 1

Section: 17.3

111) The sulfide ion is too basic to exist as such in aqueous solutions.

Diff: 1

Section: 17.3

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

Diff: 1

Section: 17.3

113) Even though silver chloride is only very slightly soluble in water, addition of a reagent which forms complex ions with silver ions increases this solubility.

Diff: 1

Section: 17.6

114) 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?

A) 1.5 × 10-9 M

B) 4.1 × 10-9 M

C) 0.00024 M

D) 0.00086 M

E) 0.0030 M

Hint: Use the Henderson-Hasselbalch formula to find the pOH of the solution, then use that to find [OH-].

Diff: 3

Section: 17.1

115) NaOH is added to sea water containing 0.050 moles per liter of Mg2+ ion until the pH reaches 12.0. A certain quantity of Mg(OH)2 precipitates. How many parts per billion of magnesium are left behind in the solution? The Ksp of Mg(OH)2 is 7.1 × 10-12.

Hint: Find [Mg2+], then convert to ppb.

A) 1.2 ppb

B) 12 ppb

C) 0.17 ppb

D) 1.7 ppb

E) 173 ppb

Diff: 3

Section: 17.1

116) The Ksp of calcium fluoride is 3.9 × 10-11. A 0.420 g sample of NaF and a 1.110 g sample of calcium chloride were added to a 1.000 liter volumetric flask, and distilled water was added to the mark. After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, how many grams of precipitate, if any, would be formed?

Hint: Find Q and compare to Ksp.

A) 0.00 g

B) 0.039 g

C) 0.39 g

D) 0.41 g

E) 0.77 g

Diff: 3

Section: 17.1

117) The Ksp value for barium chromate is 2.1 × 10-10. A 4.16 g sample of BaCl2 and a 5.83 g sample of potassium chromate were added to a 1.000 liter volumetric flask, and distilled water was added to the mark. After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, what would be the barium ion concentration remaining in solution afterwards? Be mindful that a precipitate may be formed.

Hint: Solving this problem requires comparing Q vs Ksp.

A) 2.5 × 10-8 M

B) 2.1 × 10-8 M

C) 2.5 × 10-7 M

D) 1.5 × 10-6 M

E) 1.5 × 10-5 M

Diff: 3

Section: 17.1

118) The Ksp value for barium chromate is 2.1 × 10-10. A 4.16 g sample of BaCl2 and a 5.83 g sample of potassium chromate were added to a 1.000 liter volumetric flask, and distilled water was added to the mark. After placing the stopper and shaking the flask to dissolve as much chemicals as would dissolve, how many grams of precipitate, if any, would be formed?

Hint: Solving this problem requires comparing Q vs Ksp.

A) 0.00 g

B) 0.0454 g

C) 4.54 g

D) 5.06 g

E) 5.31 g

Diff: 3

Section: 17.1

119) 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.

Diff: 2

Section: 17.2

120) Silver bromide, AgBr, is more soluble in ammonia solution than in pure water. The reaction is,

AgBr(s) + 2 NH3(aq) Ag(NH3)2+ + Br-(aq)

Using Ksp(AgBr) = 5.0 × 10-13 and Kform (Ag(NH3)2+) = 1.60 × 107, calculate the solubility of AgBr in 0.800 M ammonia solution..

Hint: Combine the formation and solubility reactions to find the overall reaction and its equilibrium constant, and make sure to account for the presence of a common ion.

A) 1.6 × 10-3 M

B) 2.3 × 10-3 M

C) 2.8 × 10-3 M

D) 4.2 × 10-3 M

E) 6.1 × 10-2 M

Diff: 3

Section: 17.6

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