Question 1

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

Accepted Answer

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 
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

Question 2

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.

Accepted Answer

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 
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 3

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.

Accepted Answer

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 
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 4

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

Accepted Answer

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. 
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 5

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.

Accepted Answer

Question 6

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

Accepted Answer

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 
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 7

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

Accepted Answer

Question 8

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-].

Accepted Answer

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 
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 9

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.

Accepted Answer

A) yes, the ion product, Q > Ksp 
B) no, the ion product, Q sp 
C) no, the ion product, Q = Ksp 
D) yes, the ion product, Q sp 
E) no, because the ion product, Q > Ksp 
A) yes, the ion product, Q > Ksp 
B) no, the ion product, Q sp 
C) no, the ion product, Q = Ksp 
D) yes, the ion product, Q sp 
E) no, because the ion product, Q > Ksp

Question 10

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.

Accepted Answer

Yes, a pre

Question 11

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

Accepted Answer

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 
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 12

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

Accepted Answer

A precipitate will f

Question 13

Calculate the concentration of chloride ions in a saturated solution of lead(II)chloride. The Ksp = 1.7 × 10-5.

Accepted Answer

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 
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 14

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

Accepted Answer

A) KCl 
B) MgCl2 
C) NaNO3 
D) LiBr 
E) ZnCO3 
A) KCl 
B) MgCl2 
C) NaNO3 
D) LiBr 
E) ZnCO3

Question 15

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.

Accepted Answer

The balanced chemical equation is given

Question 16

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

Accepted Answer

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 
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 17

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.

Accepted Answer

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 
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 18

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.

Accepted Answer

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 
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

Question 19

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.

Accepted Answer

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) 
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 20

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?

Accepted Answer

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) 
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)

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

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.

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.

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

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

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

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^-^].

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.

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

Calculate the concentration of chloride ions in a saturated solution of lead(II)chloride. The K_sp = 1.7 × 10^-⁵.

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

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.

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

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.

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.

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 PbI₂have the lowest solubility at identical temperatures?

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

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

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.

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.

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

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

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

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-].

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.

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

Calculate the concentration of chloride ions in a saturated solution of lead(II)chloride. The Ksp = 1.7 × 10-5.

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

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.

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

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.

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.

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 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

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

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.

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.

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

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

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

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^-^].

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.

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

Calculate the concentration of chloride ions in a saturated solution of lead(II)chloride. The K_sp = 1.7 × 10^-⁵.

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.

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

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.

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.

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 PbI₂have the lowest solubility at identical temperatures?