Deck 17: Solubility and Complex-Ion Equilibria

Question 1

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

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

Answer 1

4s³ = K_sp

Question 2

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

A)K_sp = [Pb²⁺][IO₃^-]²
B)K_sp = [Pb⁴⁺][2IO₃^2-]²
C)K_sp = [Pb²⁺][2IO₃^-]
D)K_sp = [Pb⁴⁺][IO₃^2-]²
E)K_sp = [Pb²⁺][2IO₃^-]²

Answer 2

K_sp = [Pb²⁺][IO₃^-]²

Question 3

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

A)K_sp = [Zn₃²⁺][(PO₄^3-)₂]
B)K_sp = [3Zn²⁺]³[2PO₄^3-]²
C)K_sp = [Zn²⁺][2PO₄^3-]
D)K_sp = [Zn³⁺]²[PO₄^2-]³
E)K_sp = [Zn²⁺]³[PO₄^3-]²

Answer 3

K_sp = [Zn²⁺]³[PO₄^3-]²

Question 4

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 K_sp = 108s⁵,where s is the molar solubility of the ionic compound.

A)only II
B)both I and II
C)only IV
D)only III
E)only I

Question 5

Cation C and anion A form an ionic compound for which K_sp = 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

Question 6

The concentration of barium carbonate in a saturated aqueous solution of the salt at 25°C is M.What is the K_sp of this sparingly soluble salt?

A)
B)
C)
D)
E)

Question 7

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

A)K_sp = [Al³⁺][3OH^-]
B)K_sp = 3[Al³⁺][OH^-]³
C)K_sp = [Al³⁺][OH^-]³
D)K_sp = [Al³⁺][3OH^-]³
E)K_sp = [Al³⁺][OH^-]

Question 8

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 K_sp for PbCl₂?

A)4.0 × 10^-6
B)1.6 × 10^-5
C)2.5 × 10^-4
D)4.8 × 10^-2
E)1.0 × 10^-6

Question 9

The solubility of calcium carbonate in water at 25°C is g/L.What is the K_sp of this sparingly soluble salt?

A)
B)
C)
D)
E)

Question 10

The solubility of lead(II)sulfate is 4.0 × 10^-2 g/L.What is the solubility product constant for lead(II)sulfate?

A)1.7 × 10^-8
B)1.3 × 10^-4
C)1.6 × 10^-3
D)4.6× 10^-15
E)8.9 × 10^-12

Question 11

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

A)K_sp = [2La³⁺]²[3CO₃^2-]³
B)K_sp = [La²⁺]²[CO₃^2-]³
C)K_sp = [2La³⁺]²[CO₃^2-]³
D)K_sp = [2La³⁺][3CO₃^2-]
E)K_sp = [La³⁺]²[CO₃^2-]³

Question 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 K_sp = s²,where s is the molar solubility of the ionic compound.

A)only I
B)only II
C)only IV
D)only III
E)both I and II

Question 13

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

A)
B)
C)
D)
E)

Question 14

What is the solubility product expression for mercury(I)chloride,Hg₂Cl₂?

A)K_sp = [Hg₂²⁺][2Cl^-]²
B)K_sp = [Hg₂²⁺][Cl^-]²
C)K_sp = [Hg₂²⁺][2Cl^- ]
D)K_sp = [Hg₂][Cl₂]
E)K_sp = [Hg⁺]²[Cl^-]²

Question 15

The solubility of silver(I)carbonate is 3.6 × 10^-2 g/L.What is the solubility product constant for silver(I)carbonate?

A)4.4 × 10^-15
B)
C)1.7 × 10^-8
D)1.3 × 10^-4
E)1.3 × 10^-3

Question 16

What is the solubility product expression for Tb₃(PO₄)₄?

A)K_sp = [Tb³⁺]⁴[PO₄^4-]³
B)K_sp = [3Tb³⁺][4PO₄^3-]
C)K_sp = [3Tb³⁺]³[4PO₄^3-]⁴
D)K_sp = [Tb²⁺]³[PO₄^3-]²
E)K_sp = [Tb⁴⁺]³[PO₄^3-]⁴

Question 17

Cation C and anion A form an ionic compound for which K_sp = 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?

A)only I
B)only III
C)both I and III
D)both I and II
E)only II

Question 18

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 K_sp = 4s³,where s is the molar solubility of the ionic compound.

A)both I and II
B)only II
C)only IV
D)only I
E)only III

Question 19

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

A)K_sp = [Pb⁴⁺][4IO₃^-]⁴
B)K_sp = [Pb⁴⁺][IO₃^-]
C)K_sp = [Pb][IO₃]⁴
D)K_sp = [Pb⁴⁺][IO₃^-]⁴

Question 20

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

I
II
III

A)I only
B)II only
C)III only
D)II and III
E)I,II,and III

Question 21

Which of the following salts has the lowest molar solubility?

A)SrCO₃ (K_sp = 9.3 × 10^-10)
B)MnS (K_sp = 2.5 × 10^-10)
C)BaF₂ (K_sp = 1 × 10^-6)
D)BaSO₄ (K_sp = 1.1 × 10^-10)
E)AgCl (K_sp = 1.8 × 10^-10)

Question 22

What is the molar solubility of lead(II)sulfate at 25°C? The solubility product constant for lead(II)sulfate is 1.7 × 10^-8 at 25°C.

A)1.7 × 10^-8 M
B)5.7 × 10^-3 M
C)8.5 × 10^-9 M
D)1.6 × 10^-3 M
E)1.3 × 10^-4 M

Question 23

Pure water is saturated with slightly soluble calcium fluoride,CaF₂.Which of the following is true concerning the equilibrium concentration of Ca²⁺?

A)
B)[Ca²⁺] = [F^-]
C)
D)
E)[Ca²⁺] = K_sp

Question 24

What is the solubility (in g/L)of barium chromate at 25°C? The solubility product constant for barium chromate is 1.2 × 10^-10 at 25°C.

A)0.41 g/L
B)3.0 × 10^-8 g/L
C)1.5 × 10^-8 g/L
D)0.078 g/L
E)0.0027 g/L

Question 25

A saturated solution of which of the following salts will have the highest molar concentration of chromate ion?

A)CuCrO₄ (K_sp = 3.6 × 10^-6)
B)BaCrO₄ (K_sp = 2.1 × 10^-10)
C)Ag₂CrO₄ (K_sp = 1.2 × 10^-12)
D)Hg₂CrO₄ (K_sp = 2.0 × 10^-9)
E)Tl₂CrO₄ (K_sp = 9.8 × 10^-13)

Question 26

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.

A)3.6 × 10^-31 g/L
B)8.2 × 10^-10 g/L
C)2.8 × 10^-7 g/L
D)5.3 × 10^-15 g/L
E)1.8 × 10^-31 g/L

Question 27

Rank the following salts in order of increasing molar solubility.
Salt
K_sp
BaSO₄
1)1 × 10^-10
AgCl
1)8 × 10^-10
BaCO₃
9)1 × 10^-9
CdS
8 × 10^-27
PbSO₄
1)8 × 10^-8

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

Question 28

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.

A)2.3 × 10^-33 M
B)6.8 × 10^-17 M
C)4.6 × 10^-33 M
D)3.6 × 10^-9 M
E)1.0 × 10^-11 M

Question 29

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

A)CaCO₃ (K_sp = 3.8 × 10^-9)
B)Ni(OH)₂ (K_sp = 2.0 × 10^-15)
C)Fe(OH)₂ (K_sp = 8 × 10^-16)
D)AgBr (K_sp = 5.0 × 10^-13)
E)PbI₂ (K_sp = 6.5 × 10^-9)

Question 30

What is the solubility (in g/L)of silver(I)chloride at 25°C? The solubility product constant for silver(I)chloride is 1.8 × 10^-10 at 25°C.

A)5.1 × 10^-2 g/L
B)2.6 × 10^-8 g/L
C)1.9 × 10^-3 g/L
D)1.3 × 10^-8 g/L
E)2.6 × 10^-1 g/L

Question 31

What is the solubility (in g/L)of calcium fluoride at 25°C? The solubility product constant for calcium fluoride is 3.4 × 10^-11 at 25°C.

A)0.00045 g/L
B)2.7 × 10^-9 g/L
C)0.015 g/L
D)1.3 × 10^-9 g/L
E)0.094 g/L

Question 32

Which salt has the highest molar solubility in pure water?

A)CdCO₃
B)Cd(OH)₂
C)Mn(OH)₂
D)PbCrO₄
E)Fe(OH)₂

Question 33

What is the molar solubility of silver(I)chloride at 25°C? The solubility product constant for silver(I)chloride is 1.8 × 10^-10 at 25°C.

A)1.3 × 10^-5 M
B)9.0 × 10^-11 M
C)1.8 × 10^-3 M
D)3.6 × 10^-4 M
E)1.8 × 10^-10 M

Question 34

The silver-ion concentration in a saturated solution of silver(I)sulfate is 2.9 × 10^-2 M.What is K_sp for silver(I)sulfate?

A)6.9 × 10^-7
B)2.1 × 10^-4
C)9.6 × 10^-5
D)​
E)8.3 × 10^-4

Question 35

Which of the following salts has the lowest molar solubility in water?

A)Ni(OH)₂ (K_sp = 2.0 × 10^-15)
B)Fe(OH)₂ (K_sp = 8 × 10^-16)
C)PbI₂ (K_sp = 6.5 × 10^-9)
D)CaCO₃ (K_sp = 3.8 × 10^-9)
E)AgBr (K_sp = 5.0 × 10^-13)

Question 36

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

A)SrCO₃ (K_sp = 9.3 × 10^-10)
B)BaSO₄ (K_sp = 1.1 × 10^-10 )
C)PbS (K_sp = 2.5 × 10^-27)
D)BaCrO₄ (K_sp = 1.2 × 10^-10)
E)AgCl (K_sp = 1.8 × 10^-10 )

Question 37

Rank the following metal sulfides in order of increasing molar solubility in water.
Salt
K_sp
CoS
4 × 10^-21
CuS
6 × 10^-36
FeS
6 × 10^-18
HgS
1)6 × 10^-52
MnS
2)5 × 10^-10

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

Question 38

What is the molar solubility of lead(II)chloride at 25°C? The solubility product constant for lead(II)chloride is 1.6 × 10^-5 at 25°C.

A)1.6 × 10^-2 M
B)1.6 × 10^-5 M
C)8.0 × 10^-6 M
D)4.0 × 10^-3 M
E)3.2 × 10^-2 M

Question 39

The hydroxide ion concentration of a saturated solution of Cu(OH)₂ is M.What is the solubility product constant for Cu(OH)₂?

A)
B)
C)
D)
E)

Question 40

A saturated solution of which of the following salts will have the greatest molar concentration of silver ion?

A)Ag₂S (K_sp = 8 × 10^-51)
B)AgCl (K_sp = 1.8 × 10^-10)
C)Ag₂CrO₄ (K_sp = 1.2 × 10^-12)
D)Ag₂CO₃ (K_sp = 8.1 × 10^-12)
E)Ag₄Fe(CN)₆ (K_sp = 8.5 × 10^-45)

Question 41

How many moles of CaF₂ will dissolve in 3.0 L of 0.041 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

A)3.3 × 10^-10
B)2.4 × 10^-8
C)7.1 × 10^-8
D)7.9 × 10^-9
E)none of these

Question 42

What is the pH of a saturated solution of Zn(OH)₂? For Zn(OH)₂,K_sp = 2.1 × 10^-16.

A)5.13
B)8.57
C)5.43
D)8.87
E)7.00

Question 43

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

A)Q_c < K_sp
B)Q_c > K_sp
C)Q_c = K_sp
D)K_sp = 1
E)Q_c = 1

Question 44

For which of the following will precipitation be expected?

A)Q_c < K_sp
B)Q_c = 1
C)Q_c = K_sp
D)Q_c > K_sp
E)K_sp = 1

Question 45

What is the concentration of silver(I)ion in a saturated solution of silver(I)carbonate containing 0.0046 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 × 10^-12.

A)6.0 × 10^-4 M
B)2.0 × 10^-9 M
C)8.0 × 10^-9 M
D)4.3 × 10^-5 M
E)8.0 × 10^-4 M

Question 46

To 1.0 L of water,1.5 × 10^-6 mol of Pb(NO₃)₂,6.5 × 10^-6 mol of K₂CrO₄,and 1.0 mol of NaCl are added.What will happen?
Salt
K_sp
PbCrO₄
1)8 × 10^-14
PbCl₂
1)6 × 10^-5

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.

Question 47

Rank the following salts in order of increasing molar solubility.

A)AgSCN < Ag₂CrO₄ < Ag₃PO₄
B)AgSCN < Ag₃PO₄ < Ag₂CrO₄
C)Ag₃PO₄ < Ag₂CrO₄ < AgSCN
D)Ag₃PO₄ < AgSCN < Ag₂CrO₄
E)Ag₂CrO₄ < AgSCN < Ag₃PO₄

Question 48

The solubility of La(IO₃)₃ in a 0.71 M KIO₃ solution is 1.0 ×10^-7 mol/L.Calculate K_sp for La(IO₃)₃.

A)7.1 × 10^-8
B)3.6 × 10^-22
C)3.6 × 10^-1
D)3.6 × 10^-8
E)none of these

Question 49

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 V^1-,W^2-,X^2-,Y^1-,and Z^1-,all have the same K_sp value.Which salt has the highest molar solubility?

A)AV
B)EZ₃
C)DY₂
D)B₂W
E)C₂X₃

Question 50

K_sp for PbF₂ is 4.0 ×10^-8.If a 0.032 M NaF solution is saturated with PbF₂,what is [Pb²⁺] in solution?

A)4.1 × 10^-11 M
B)1.3 × 10^-9 M
C)1.3 × 10^-6 M
D)1.2 × 10^-3 M
E)3.9 × 10^-5 M

Question 51

What is the hydroxide-ion concentration of a saturated solution of Ni(OH)₂? For Ni(OH)₂,K_sp = 2.0 × 10^-15.

A)2.8 × 10^-3 M
B)7.9 × 10^-6 M
C)1.0 × 10^-7 M
D)2.7 × 10^-2 M
E)1.6 × 10^-5 M

Question 52

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,K_sp = 1.0 × 10^-14.

A)A precipitate forms because Q_c > K_sp.
B)A precipitate forms because Q_c < K_sp.
C)No precipitate forms because Q_c < K_sp.
D)No precipitate forms because Q_c = K_sp.
E)No precipitate forms because Q_c > K_sp.

Question 53

What is the molar solubility of MgF₂ in a 0.40 M NaF solution? For MgF₂,K_sp = 8.4 × 10^-8.

A)1.0 × 10^-7 M
B)1.4 × 10^-4 M
C)2.1 × 10^-7 M
D)7.1 × 10^-4 M
E)5.3 × 10^-7 M

Question 54

Which of Figures I-IV represent(s)the result of mixing aqueous solutions of Na₂S and NiCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

A)both I and II
B)only I
C)only II
D)only III
E)only IV

Question 55

Which Figures I-IV represent(s)the result of mixing aqueous solutions of NaOH and CuCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

A)only II
B)both I and II
C)only IV
D)only I
E)only III

Question 56

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)

Question 57

In which of these solutions would silver(I)carbonate have the lowest molar solubility? For silver(I)carbonate,K_sp = 8.5 × 10^-12.

A)0.03 M H₂CO₃
B)0.1 M AgNO₃
C)0.01 M AgNO₃
D)0.1 M Na₂CO₃
E)pure water

Question 58

Which salt has the lowest molar solubility in pure water?

A)PbCrO₄
B)Fe(OH)₂
C)CdCO₃
D)Cd(OH)₂
E)Mn(OH)₂

Question 59

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

A)0.10 M Na₃PO₄
B)0.10 M AgNO₃
C)0.10 M Na₂HPO₄
D)0.10 M HNO₃
E)0.10 M NaH₂PO₄

Question 60

What is the molar solubility of MgF₂ in a 0.36 M Mg(NO₃)₂ solution? For MgF₂,K_sp = 8.4 × 10^-8.

A)8.0 × 10^-8 M
B)2.4 × 10^-4 M
C)2.0 × 10^-8 M
D)4.8 × 10^-4 M
E)3.2 × 10^-3 M

Question 61

A 5.0 × 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,K_sp = 2.0 × 10^-13.

A)4.60
B)9.57
C)4.70
D)9.30
E)9.40

Question 62

For which pair of cations would the addition of dilute hydrobromic acid precipitate one but not the other?

A)Ag⁺ and Ca²⁺
B)Hg₂²⁺ and Ag⁺
C)Ba²⁺ and Na⁺
D)Ca²⁺ and Ba²⁺
E)Pb²⁺ and Ag⁺

Question 63

What is the maximum concentration of carbonate ions that will precipitate BaCO₃ but not MgCO₃ from a solution that is M each in Mg²⁺ and Ba²⁺? For MgCO₃,K_sp = 1.0 × 10^-5 and for BaCO₃,K_sp = 2.6 × 10^-9.

A) M
B) M
C) M
D) M
E)2.6 × 10^-14 M

Question 64

If 275 mL of 1 × 10^-7 M AgNO₃ is mixed with 275 mL of 1 × 10^-8 M NaI,what will occur? For AgI,K_sp = 8.3 × 10^-17.

A)Sodium nitrate will precipitate.
B)Silver(I)nitrate will precipitate.
C)Sodium iodide will precipitate.
D)Silver(I)iodide will precipitate.
E)No precipitate will form.

Question 65

What is the maximum hydroxide-ion concentration that a 0.025 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂,K_sp = 1.8 × 10^-11.

A)4.2 × 10^-6
B)1.7 × 10^-4
C)1.2 × 10^-8
D)7.2 × 10^-9
E)2.7 × 10^-5

Question 66

If 370 mL of 1 × 10^-8 M Al(NO₃)₃ is mixed with 370 mL of 1 × 10^-8 M NaOH,what will occur? For Al(OH)₃,K_sp = 4.6 × 10^-33.

A)Aluminum hydroxide will precipitate.
B)Sodium hydroxide will precipitate.
C)Aluminum nitrate will precipitate.
D)Sodium nitrate will precipitate.
E)No precipitate will form.

Question 67

What is the minimum mass of Na₂CO₃ that must be added to 75.9 mL of a 9.0 × 10^-4 M AgNO₃ solution in order for precipitation to occur? For Ag₂CO₃,K_sp = 8.6 × 10^-12 .

A)7.2 × 10^-3 g
B)3.1 × 10^-4 g
C)3.6 × 10^-3 g
D)7.7 × 10^-8 g
E)8.5 × 10^-5 g

Question 68

Suppose 50.00 mL of a 1 × 10^-7 M solution of lead(II)nitrate is mixed with 50.00 mL of a 1 × 10^-8 solution of sodium phosphate.Which of the following statements is true? For lead(II)phosphate,K_sp = 1 × 10^-44.

A)A precipitate forms because Q_c < K_sp.
B)No precipitate forms because Q_c > K_sp.
C)A precipitate forms because Q_c > K_sp.
D)No precipitate forms because Q_c = K_sp.
E)No precipitate forms because Q_c < K_sp.

Question 69

What is the maximum volume of 8.6 × 10^-5 M K₂CrO₄ that,added to 40.4 mL of a solution that is 5.1 × 10^-5 M Ba(NO₃)₂ and 1.5 × 10^-6 M Pb(NO₃)₂,will precipitate PbCrO₄ but not BaCrO₄? For PbCrO₄,K_sp = 1.8 × 10^-14,and for BaCrO₄,K_sp = 1.2 × 10^-10.

A)40 mL
B)1.1 mL
C)1.0 mL
D)0.0056 mL
E)37 mL

Question 70

A solution contains 0.018 mol 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?
K_sp
AgI
= 1)5 × 10^-16
K_sp
AgBr
= 5)0 × 10^-13
K_sp
AgCl
= 1)6 × 10^-10

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

Question 71

If 430 mL of 1 × 10^-4 M Ca(NO₃)₂ is mixed with 430 mL of 1 × 10^-4 M NaF,what will occur? For CaF₂,K_sp = 3.4 × 10^-11.

A)No precipitate will form.
B)Sodium nitrate will precipitate.
C)Calcium nitrate will precipitate.
D)Calcium fluoride will precipitate.
E)Sodium fluoride will precipitate.

Question 72

Silver nitrate (AgNO₃)is slowly added to a solution containing 0.100 M Br− and 0.050 M FeCN₆⁴⁻ until a precipitate just forms.What is the molar concentration of Ag⁺ just as the precipitate forms? AgBr K_sp = 5.0 × 10^-13 and Ag₄FeCN₆ K_sp = 8.5 × 10^-45.

A)2.0 × 10^-11 M Ag⁺
B)5.0 × 10^-12 M Ag⁺
C)1.0 × 10^-11 M Ag⁺
D)3.3 × 10^-12 M Ag⁺
E)1.7 × 10^-43 M Ag⁺

Question 73

A solution is 0.010 M in each of Pb(NO₃)₂,Mn(NO₃)₂,and Zn(NO₃)₂.Solid NaOH is added until the pH of the solution is 8.50.Which of the following statements is true?
Salt
K_sp
Pb(OH)₂
1)4 × 10^-20
Mn(OH)₂
2)0 × 10^-13
Zn(OH)₂
2)1 × 10^-16

A)Only Mn(OH)₂ will precipitate.
B)All three hydroxides will precipitate.
C)Only Pb(OH)₂ will precipitate.
D)No precipitate will form.
E)Only Zn(OH)₂ and Pb(OH)₂ will precipitate.

Question 74

If 500 mL of 1.3 × 10^-6 M AgNO₃ is mixed with 500 mL of 1.3 × 10^-6 M NaBr,what will occur? For AgBr,K_sp = 5 × 10^-13.

A)Silver(I)bromide will precipitate.
B)The concentration of Ag⁺ will be 1.3 × 10^-6 M.
C)6.5 × 10^-7 mol of AgBr will form.
D)No precipitation will occur.
E)Sodium bromide will precipitate.

Question 75

Solid KCN is added to a solution composed of 0.10 M Ag⁺ and 0.10 M Zn²⁺ just until a precipitate forms.What is the composition of this initial precipitate? AgCN K_sp = 2.2 × 10^-16 and Zn(CN)₂ K_sp = 3 × 10^-16.

A)The precipitate is pure AgCN(s).
B)The precipitateis pure Zn(CN)₂(s).
C)The precipitate is a mixture of AgCN(s)and Zn(CN)₂(s).
D)The precipitate is a mixture of KCN(s)and AgCN(s).
E)The precipitate is a mixture of KCN(s)and Zn(CN)₂(s).

Question 76

What is the minimum concentration of Pb²⁺ required to begin precipitating Pb(OH)₂(s)in a solution of pH 10.78? For Pb(OH)₂,K_sp = 1.4 × 10^-20.

A)3.0 × 10^-4 M
B)8.4 × 10^-10 M
C)2.3 × 10^-17 M
D)3.9 × 10^-14 M
E)1.2 × 10^-22 M

Question 77

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,K_sp = 2.4 × 10^-12.

A)The AgNO₃ will settle to the bottom without dissolving.
B)The concentration of CrO₄^2- will increase.
C)Some Ag₂CrO₄ will precipitate.
D)Nothing will happen.
E)The concentration of Ag⁺ in solution will not change.

Question 78

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 × 10^-7,1.6 × 10^-10,and 2.0 × 10^-13,respectively.Which compound will precipitate first?

A)AuCl(s)
B)All will precipitate at the same time.
C)It cannot be determined.
D)AgCl(s)
E)CuCl(s)

Question 79

What is the maximum Sr²⁺ concentration possible in a solution that has a M sulfide-ion concentration without precipitating strontium sulfate? For SrSO₄,K_sp = 2.5 × 10^-7.

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

Question 80

Which of the following solutions should be added to a solution containing both copper(II)ions and silver(I)ions in order to precipitate only one of the ions?

A)HCl(aq)
B)H₂S(aq)
C)HNO₃(aq)
D)H₂S(aq)+ HCl(aq)
E)H₂S(aq)+ HNO₃(aq)