Deck 18: Solubility and Simultaneous Equilibria

Question 1

Which of the following is the expression for the solubility product of Ba₃(AsO₄)₂?

A)K_sp = [Ba²⁺]³[AsO₄³]²
B)K_sp = [3 × Ba²⁺]³[2AsO₄³]²
C)K_sp = 3[Ba²⁺] 2[AsO₄³]
D)K_sp = 3[Ba²⁺]³ + 2[AsO₄³]²
E)K_sp = [Ba³⁺]³[AsO₄²]²

Answer 1

K_sp = [Ba²⁺]³[AsO₄³]²

Question 2

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

A)K_sp = [Ca²⁺]³ [PO₄³]²
B)K_sp = [3 × Ca²⁺]³[2PO₄³]²
C)K_sp = 3[Ca²⁺]2[PO₄³]
D)K_sp = 3[Ca²⁺]³ + 2[PO₄³]²
E)K_sp = [Ca²⁺]₃[PO₄³]₂

Answer 2

K_sp = [Ca²⁺]³ [PO₄³]²

Question 3

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

A)K_sp = [Fe²⁺]³[CrO₄³]²
B)K_sp = [2 × Fe²⁺]³[3CrO₄³]²
C)K_sp = 3[Fe²⁺] 2[CrO₄³]
D)K_sp = 2[Fe²⁺]³ + 3[CrO₄³]²
E)K_sp = [Fe³⁺]²[CrO₄²]³

Answer 3

K_sp = [Fe³⁺]²[CrO₄²]³

Question 4

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

A)K_sp = [Cu²⁺][2 OH]
B)K_sp = [Cu²⁺] 2[OH]²
C)K_sp = [Cu²⁺]²[OH]
D)K_sp = [Cu²⁺][OH]²
E)K_sp = [Cu²⁺] ½[OH]²

Question 5

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

A)K_sp = [Ca²⁺][2 × F]
B)K_sp = [Ca²⁺] 2[F]²
C)K_sp = [Ca²⁺]²[F]
D)K_sp = [Ca²⁺][F]²
E)K_sp = [Ca²⁺] ½[F]²

Question 6

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

A)K_sp = [Ag₂²⁺][C₂O₄²]
B)K_sp = [Ag⁺][C₂O₄²]²
C)K_sp = 2[Ag⁺][C₂O₄²]
D)K_sp = [Ag⁺]²[C₂O₄²]
E)K_sp = 2[Ag⁺]²[C₂O₄²]

Question 7

The solubility of magnesium carbonate, MgCO₃, in pure water is 2.6 × 10^-4 moles per liter. Calculate the value of K_sp 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

Question 8

The solubility of calcium oxalate, CaC₂O₄, in pure water is 4.8 × 10^-5 moles per liter. Calculate the value of K_sp 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

Question 9

The solubility of scandium(III)fluoride, ScF₃, in pure water is 2.0 × 10^-5 moles per liter. Calculate the value of K_sp 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

Question 10

The solubility of lead(II)fluoride, PbF₂, in pure water is 2.1 × 10^-3 moles per liter. Calculate the value of K_sp 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

Question 11

The solubility of calcium fluoride, CaF₂, in pure water is 2.15 × 10^-4 moles per liter. Calculate the value of K_sp 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

Question 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 K_sp 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

Question 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 K_sp 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

Question 14

The solubility of silver oxalate, Ag₂C₂O₄, in pure water is 2.06 × 10^-4 moles per liter. Calculate the value of K_sp 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

Question 15

The solubility of silver carbonate, Ag₂CO₃, in pure water is 1.27 × 10^-4 moles per liter. Calculate the value of K_sp 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

Question 16

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

A)PbF₂, K_sp = 3.6 × 10^-8
B)Ag₂CrO₄, K_sp = 1.2 × 10^-12
C)CaF₂, K_sp = 3.9 × 10^-11
D)BaF₂, K_sp = 1.7 × 10^-6
E)PbI₂, K_sp = 7.9 × 10^-9

Question 17

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

A)SrF₂, K_sp = 2.8 × 10^-9
B)Sr(IO₃)₂, K_sp = 3.3 × 10^-7
C)Fe(OH)₂, K_sp = 8.0 × 10^-16
D)PbCl₂, K_sp = 1.6 × 10^-5
E)PbBr₂, K_sp = 3.9 × 10^-5

Question 18

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

A)SrF₂, K_sp = 2.8 × 10^-9
B)Sr(IO₃)₂, K_sp = 3.3 × 10^-7
C)MgF₂, K_sp = 6.5 × 10^-9
D)PbCl₂, K_sp = 1.6 × 10^-5
E)BaF₂, K_sp = 1.7 × 10^-6

Question 19

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

A)SrF₂, K_sp = 2.8 × 10^-9
B)Sr(IO₃)₂, K_sp = 3.3 × 10^-7
C)MgF₂, K_sp = 6.5 × 10^-9
D)PbCl₂, K_sp = 1.6 × 10^-5
E)PbI₂, K_sp = 7.9 × 10^-9

Question 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]

Question 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]

Question 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

Question 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 = [PO₄^3-]
E)solubility = [PO₄^3-]³

Question 24

The solubility product for Ag₃PO₄ is: K_sp = 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

Question 25

The solubility product for Ag₃PO₄ is: K_sp = 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

Question 26

The solubility product for PbBr₂ is: K_sp = 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

Question 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

Question 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

Question 29

Calculate the concentration of chloride ions in a saturated solution of lead(II)chloride. The K_sp = 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

Question 30

Calculate the concentration of bromide ions in a saturated solution of lead(II)bromide. The K_sp = 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

Question 31

Calculate the concentration of iodate ions in a saturated solution of lead(II)iodate, Pb(IO₃)₂. The K_sp = 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

Question 32

Calculate the concentration of iodate ions in a saturated solution of barium iodate, Ba(IO₃)₂. The K_sp = 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

Question 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

Question 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

Question 35

The solubility of lead iodide is 578 mg L^-1 at 25 °C. What is the K_sp 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

Question 36

The solubility of barium carbonate is 14.8 mg L^-1 at 30 °C. Calculate the K_sp value for BaCO_3.

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

Question 37

How many grams of lead(II)chloride would dissolve in 100 mL of water? The K_sp 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

Question 38

What is the solubility, in moles per liter, of Fe(OH)₂ (K_sp = 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

Question 39

What is the solubility, in moles per liter, of PbSO₄ (K_sp = 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

Question 40

What is the solubility, in moles per liter, of AgCl (K_sp = 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

Question 41

What is the solubility, in moles per liter, of BaSO₄ (K_sp = 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

Question 42

What is the solubility, in moles per liter, of MgCO₃ (K_sp = 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

Question 43

What is the solubility, in moles per liter, of Ag₂CO₃ (K_sp = 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

Question 44

What is the solubility, in moles per liter, of AgCl (K_sp = 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

Question 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)

Question 46

The solubility of PbI₂ (K_sp = 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)

Question 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 K_sp 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

Question 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 K_sp 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

Question 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

Question 50

Will a precipitate form when 20.0 mL of 1.8 × 10^-3 M Pb(NO₃)₂ is added to 30.0 mL of5.0 × 10^-4 M Na₂SO₄? The K_sp 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 < K_sp
B)no, because the ion product, Q > K_sp
C)yes, because the ion product, Q < K_sp
D)yes, because the ion product, Q > K_sp
E)no, because K_sp is less than the ion product

Question 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 K_sp 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 > K_sp
B)no, because the ion product, Q < K_sp
C)no, because the ion product, Q = K_sp
D)yes, because the ion product, Q < K_sp
E)no, because the ion product, Q > K_sp

Question 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

Question 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 K_sp forAgI 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

Question 54

For PbCl₂, K_sp = 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 > K_sp
B)no, the ion product, Q < K_sp
C)no, the ion product, Q = K_sp
D)yes, the ion product, Q < K_sp
E)no, because the ion product, Q > K_sp

Question 55

Methylamine, CH₃NH₂, is a weak molecular base with a value of 4.4 × 10^-4 for K_b. An aqueous solution contains 0.200 M CH₃NH₂ and 0.400 M CH₃NH₃Cl per liter as the only solutes. If the K_sp 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

Question 56

Methylamine, CH₃NH₂, is a weak molecular base with a value of 4.4 × 10^-4 for K_b. An aqueous solution contains 0.200 M CH₃NH₂ and 0.300 M CH₃NH₃Cl per liter as the only solutes. If the K_sp 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

Question 57

Dimethylamine, (CH₃)₂NH, is a weak molecular base with a value of 9.6 × 10^-4.for K_b. An aqueous solution contains 0.350 M (CH₃)₂NH and 0.250 M (CH₃)₂NH₂Cl per liter as the only solutes. If the K_sp 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

Question 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

Question 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)

Question 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 K_c for the reaction below? Hint: Combine reactions and K_sp 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

Question 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 K_c for the reaction below? Hint: Combine reactions and K_sp 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

Question 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 K_c for the reaction below? Hint: Combine reactions and K_sp 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

Question 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

Question 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

Question 65

Given the following information: What is the equilibrium constant for the reaction below?

A)1.7 × 10¹⁵
B)6.0 × 10^-1
C)6.0 × 10¹²
D)1.7 × 10^-13
E)3.3 × 10¹

Question 66

Given the following information What is the equilibrium constant for the reaction below?

A)8.4 × 10^-21
B)3.7 × 10^-1
C)1.2 × 10²⁰
D)2.7
E)2.1 × 10^-10

Question 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.

Question 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

Question 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.

Question 70

The acid solubility product, K_spa, 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)

Question 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 K_sp 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.

Question 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 K_sp 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.

Question 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 K_sp 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.

Question 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.

Question 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.

Question 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.

Question 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 S₂O₃^2-(aq) Ag(S₂O₃)₂^3-(aq)+ Br^-(aq)

A)2.0 × 10¹³
B)5.0 × 10^-1
C)4.0 × 10²⁵
D)5.0 × 10^-13
E)10

Question 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 ________.

Question 79

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

Question 80

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