Question 1

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

Accepted Answer

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 
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 2

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

Accepted Answer

A) 1.1 × 10-13 
B) 4.7 × 10-5 
C) 8.9 × 1012  
D) 4.9 × 10-5 
E) 2.1 × 104 
A) 1.1 × 10-13 
B) 4.7 × 10-5 
C) 8.9 × 1012  
D) 4.9 × 10-5 
E) 2.1 × 104

Question 3

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.

Accepted Answer

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 
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 4

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.

Accepted Answer

We find that Q = [Mg

Question 5

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.

Accepted Answer

Question 6

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.

Accepted Answer

A) 1.1 g 
B) 0.039 g 
C) 10.9 g 
D) 4.3 g 
E) 1.4 × 10-4 g 
A) 1.1 g 
B) 0.039 g 
C) 10.9 g 
D) 4.3 g 
E) 1.4 × 10-4 g

Question 7

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

Accepted Answer

Question 8

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.

Accepted Answer

Question 9

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

Accepted Answer

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 
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

Question 10

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

Accepted Answer

A) 9.6 × 10-12 
B) 1.3 × 10-1 
C) 1.1 × 1023  
D) 7.7 
E) 9.4 × 10-24 
A) 9.6 × 10-12 
B) 1.3 × 10-1 
C) 1.1 × 1023  
D) 7.7 
E) 9.4 × 10-24

Question 11

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?

Accepted Answer

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 
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 12

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.

Accepted Answer

Question 13

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.

Accepted Answer

Question 14

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-].

Accepted Answer

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 
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 15

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

Accepted Answer

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] 
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]

Question 16

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

Accepted Answer

A) NaCl 
B) MgBr2 
C) LiNO3 
D) CaCO3 
E) AgBr 
A) NaCl 
B) MgBr2 
C) LiNO3 
D) CaCO3 
E) AgBr

Question 17

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

Accepted Answer

No precipi

Question 18

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?

Accepted Answer

The answer of The solubility of lead(II)iodide is 0.064 g/100...

Question 19

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.)

Accepted Answer

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. 
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 20

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.

Accepted Answer

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 
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

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

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.

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 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.

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.

Metal sulfides actually dissolve in water by ________ with water, not by releasing S^2- ions into water.

What is the molar solubility of Ca(OH)₂ in a 0.300 M NaOH solution? The K_sp 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.

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

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.

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?

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.

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

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

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?

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 Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Mixtures at the Molecular Level: Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

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Exam 18: Solubility and Simultaneous Equilibria

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

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

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 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.

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.

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

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.

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

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

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?

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.

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

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

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?

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 Very Brief History of Chemistry

Scientific Measurements

Elements, Compounds, and the Periodic Table

The Mole and Stoichiometry

Molecular View of Reactions in Aqueous Solutions

Oxidation-Reduction Reactions

Energy and Chemical Change

The Quantum Mechanical Atom

The Basics of Chemical Bonding

Theories of Bonding and Structure

Properties of Gases

Intermolecular Attractions and the Properties of Liquids and Solids

Mixtures at the Molecular Level: Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases, a Molecular Look

Acid-Base Equilibria in Aqueous Solutions

Thermodynamics

Electrochemistry

Nuclear Reactions and Their Role in Chemistry

Metal Complexes

Organic Compounds, Polymers, and Biochemicals

Filters

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

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.

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 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.

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.

Metal sulfides actually dissolve in water by ________ with water, not by releasing S^2- ions into water.

What is the molar solubility of Ca(OH)₂ in a 0.300 M NaOH solution? The K_sp 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.

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

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.

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?

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.

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

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.