chemistry ch 17 test bank

Example 17.1 TOP: solubility | solubility equilibria KEY: solubility product constant MSC: general chemistry 2.. Example 17.1 TOP: solubility | solubility equilibria KEY: solubility prod

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Chapter 17 - Solubility and Complex-Ion Equilibria

1 Cation C and anion A form an ionic compound for which Ksp = s2, where s is the molar

solubility of the ionic compound Which of Figures I–III represent(s) possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A?

OBJ: Write solubility product expressions (Example 17.1)

TOP: solubility | solubility equilibria KEY: solubility product constant

MSC: general chemistry

2 Cation C and anion A form an ionic compound for which Ksp = 4s3, where s is the molar

solubility of the ionic compound Which of Figures I–III represent(s) possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A?

A) only III

B) only II

C) both I and II

D) only I

E) both I and III

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TOP: solubility | solubility equilibria KEY: solubility product constantMSC: general chemistry

3 Which of the following particulate views is/are consistent with a heterogeneous equilibrium?

E) I, II, and III

TOP: solubility | solubility equilibria

4 What is the solubility product expression for Al(OH)3?

5 What is the solubility product expression for Th(IO3)4?

6 What is the solubility product expression for Zn3(PO4)2?

A) Ksp = [Zn32+][(PO43–)2]

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B) Ksp = [3Zn2+]3[2PO43–]2

C) Ksp = [Zn2+][2PO43–]

D) Ksp = [Zn3+]2[PO42–]3

E) Ksp = [Zn2+]3[PO43–]2

7 What is the solubility product expression for mercury(I) iodide, Hg2I2?

8 What is the solubility product expression for La2(CO3)3?

9 What is the solubility product expression for Pb3(PO4)4?

10 What is the solubility product expression for Sn(IO3)2?

A) Ksp = [Sn2+][IO3 ]2

B) Ksp = [Sn4+][2IO32–]2

C) Ksp = [Sn2+][2IO3 ]

D) Ksp = [Sn4+][IO32–]2

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E) Ksp = [Sn2+][2IO3 ]2

12 Figures I–IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A Identify the figure(s) that

represent(s) products for which Ksp = 4s3, where s is the molar solubility of the ionic

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ANS: A PTS: 1 DIF: moderate REF: 17.1

13 Figures I–IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A Identify the figure(s) that

represent(s) products for which Ksp = 108s5, where s is the molar solubility of the ionic

14 What is the relationship between molar solubility (s) and Ksp for calcium fluoride?

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15 What is the correct mathematical expression for finding the molar solubility (s) of Sn(OH)2?

16 The concentration of calcium carbonate in a saturated aqueous solution of the salt at 25°C is6.71105

M What is the Ksp of this sparingly soluble salt?

OBJ: Calculate Ksp from the solubility (simple example) (Example 17.2)

17 The solubility of strontium carbonate in water at 25°C is 4.50103

OBJ: Calculate Ksp from the solubility (simple example) (Example 17.2)

18 After mixing an excess PbCl2 with a fixed amount of water, it is found that the equilibrium concentration of Pb2+ is 1.6  10–2 M What is Ksp for PbCl2?

OBJ: Calculate Ksp from the solubility (more complicated example).(Example 17.3)TOP: solubility | solubility equilibria KEY: solubility product constant

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19 The solubility of lead(II) sulfate is 4.0  10–2 g/L What is the solubility product constant for lead(II) sulfate?

OBJ: Calculate Ksp from the solubility (more complicated example).(Example 17.3)TOP: solubility | solubility equilibria KEY: solubility product constant

OBJ: Calculate Ksp from the solubility (more complicated example).(Example 17.3)

22 The silver-ion concentration in a saturated solution of silver(I) chromate is 1.3  10–4 M What is Ksp for silver(I) chromate?

OBJ: Calculate Ksp from the solubility (more complicated example).(Example 17.3)

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OBJ: Calculate the solubility from Ksp (Example 17.4)

24 Which of the following salts has the lowest molar solubility?

25 Rank the following salts in order of increasing molar solubility

A) CdS < AgCl < BaSO4 < BaCO3 < PbSO4

B) CdS < AgCl < BaCO3 < BaSO4 < PbSO4

C) CdS < BaSO4 < AgCl < BaCO3 < PbSO4

D) PbSO4 < BaCO3 < AgCl < BaSO4 < CdS

E) PbSO4 < BaCO3 < BaSO4 < AgCl < CdS

26 A saturated solution of which of the following salts will have the lowest molar concentration

of chromate ion?

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27 A saturated solution of which of the following salts will have the greatest molar

concentration of silver ion?

28 What is the solubility (in g/L) of aluminum hydroxide at 25°C? The solubility product constant for aluminum hydroxide is 4.6  10–33 at 25°C

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30 Rank the following metal sulfides in order of increasing molar solubility in water.

A) MnS < FeS < CoS < CuS < HgS

B) FeS < HgS < CoS < CuS < MnS

C) HgS < CuS < CoS < FeS < MnS

D) CuS < CoS < FeS < MnS < HgS

E) CoS < CuS < FeS < HgS < MnS

31 What is the molar solubility of silver(I) bromide at 25°C? The solubility product constant for silver(I) bromide is 5.0  10–13 at 25°C

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33 What is the molar solubility of barium fluoride at 25°C? The solubility product constant for barium fluoride is 1.0  10–6 at 25°C.

34 What is the molar solubility of aluminum hydroxide at 25°C? The solubility product

constant for aluminum hydroxide is 4.6  10–33 at 25°C

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37 Pure water is saturated with slightly soluble calcium fluoride, CaF2 Which of the following

is true concerning the equilibrium concentration of Ca2+?

39 Which of the following salts has the highest molar solubility in water?

TOP: solubility | solubility equilibria KEY: precipitation calculations

40 Which salt has the highest molar solubility in pure water?

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41 Which salt has the lowest molar solubility in pure water?

42 What is the hydroxide-ion concentration of a saturated solution of Ni(OH)2? For Ni(OH)2,

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43 What is the pH of a saturated solution of Ni(OH)2? For Ni(OH)2, Ksp = 2.0  10–15.

45 The insoluble salts AV, B2W, C2X3, DY2, and EZ3, which were formed from the metal ions

A+, B+, C3+, D2+, and E3+ and the nonmetals V1–, W2–, X2–, Y1–, and Z1–, all have the same Ksp

value Which salt has the highest molar solubility?

46 In which of the following solutions would silver(I) phosphate, Ag3PO4, be least soluble?

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ANS: B PTS: 1 DIF: easy REF: 17.2

OBJ: Explain how the solubility of a salt is affected by another salt that has the same

KEY: solubility and the common-ion effect

48 The figure below represents the result of adding which of the following aqueous solutions to

a filtered, saturated solution of AgCl?

A) only NaCl(aq)

B) only HNO3(aq)

C) HCl(aq) or NaCl(aq)

D) only HCl(aq)

E) HCl(aq) or HNO3(aq)

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E) 8.0  10–4 M

OBJ: Calculate the solubility of a slightly soluble salt in a solution of a common ion (Example 17.5) TOP: solubility | solubility equilibria

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53 The solubility of La(IO3)3 in a 0.62 M KIO3 solution is 1.0 10–7 mol/L Calculate Ksp for

55 How many moles of CaF2 will dissolve in 3.0 L of 0.051 M NaF solution? (Ksp for

56 Which of Figures I–IV represent(s) the result of mixing aqueous solutions of Na2S and NiCl2

in which the ion product Qc > Ksp for the insoluble product? (C = cation, A = anion)

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OBJ: State the criterion for precipitation.

57 Which Figures I–IV represent(s) the result of mixing aqueous solutions of NaOH and CuCl2

in which the ion product Qc > Ksp for the insoluble product? (C = cation, A = anion)

OBJ: State the criterion for precipitation

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ANS: D PTS: 1 DIF: easy REF: 17.3

KEY: precipitation calculations | criterion for precipitation MSC: general chemistry

59 Which of the following will apply to a saturated solution of an ionic compound?

60 Suppose 50.00 mL of 2.0  10–6 M Fe(NO3)3 is added to 50.00 mL of 2.0 10–4 M KIO3 Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0  10–14

A) A precipitate forms because Qc > Ksp.

B) A precipitate forms because Qc < Ksp.

C) No precipitate forms because Qc < Ksp.

D) No precipitate forms because Qc = Ksp.

E) No precipitate forms because Qc > Ksp.

OBJ: Predict whether precipitation will occur (given ion concentrations) (Example 17.6)TOP: solubility | solubility equilibria

61 To 1.0 L of water, 3.0  10–6 mol of Pb(NO3)2, 4.0  10–6 mol of K2CrO4, and 1.0 mol of NaCl are added What will happen?

A) A precipitate of KCl will form

B) A precipitate of PbCrO4 will form

C) A precipitate of PbCl2 will form

D) No precipitate will form

E) Both a precipitate of PbCl2 and a precipitate of PbCrO4 will form

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62 What is the maximum Sr2+ concentration possible in a solution that has a 6.3105

63 What will happen if 0.1 mol of solid silver(I) nitrate is added to 1.0 L of a saturated solution

of silver(I) chromate? For Ag2CrO4, Ksp = 2.4  10–12

A) The AgNO3 will settle to the bottom without dissolving

B) The concentration of CrO42– will increase

C) Some Ag2CrO4 will precipitate

D) Nothing will happen

E) The concentration of Ag+ in solution will not change

64 A 4.0  10–4 M solution of MnSO4 is gradually made more basic by adding NaOH At what

pH will manganese(II) hydroxide begin to precipitate? For Mn(OH)2, Ksp = 2.0  10–13.A) 4.70

B) 9.57

C) 4.65

D) 9.35

E) 9.30

65 What is the minimum concentration of Cu2+ required to begin precipitating Cu(OH)2(s) in a

solution of pH 10.77? For Cu(OH)2, Ksp = 2.6  10–19

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