Question 1

Silver oxalate,Ag2C2O4,has a molar solubility = 1.1 × 10-4 mol/L.Ag2C2O4 has a solubility product Ksp = ________.

Accepted Answer

Question 2

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid H2X+)are Ka1 = 4.6 × 10-3 and Ka2 = 2.0 × 10-10.What is the pH of 50.00 mL of a 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

Accepted Answer

A) 9)70 
B) 10.69 
C) 11.11 
D) 12.70 
A) 9)70 
B) 10.69 
C) 11.11 
D) 12.70

Question 3

CaF2 has Ksp = 3.5 × 10-11.If 25 mL of 8.0 × 10-4 M Ca(NO3)2 is mixed with 75 mL of
4.0 × 10-4 M KF,a precipitate of CaF2 ________ (will,will not)form.

Accepted Answer

Question 4

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid HS1U1B12S1U1B0A with NaOH.  
-A buffer region is indicated by which point(s)a-d?

Accepted Answer

A) point a 
B) points a and c 
C) point b 
D) points b and d 
A) point a 
B) points a and c 
C) point b 
D) points b and d

Question 5

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid HS1U1B12S1U1B0A with NaOH.  
-Which point a-d represents pKa2?

Accepted Answer

A) point a 
B) point b 
C) point c 
D) point d 
A) point a 
B) point b 
C) point c 
D) point d

Question 6

The following pictures represent solutions at various stages in the titration of a weak diprotic acid HS1U1B12S1U1B0A with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P12-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0 initially present,OHS1U1P1-S1S1P0 initially present and solvent water molecules have been omitted for clarity).  
-Which picture represents the system at the first equivalence point?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4) 
A) (1) 
B) (2) 
C) (3) 
D) (4)

Question 7

Which pair of ions can be separated by the addition of sulfide ion?

Accepted Answer

A) Ag+ and Cu2+ 
B) Cu2+ and Bi3+ 
C) Pb2+ and Ca2+ 
D) Ca2+ and Ba2+ 
A) Ag+ and Cu2+ 
B) Cu2+ and Bi3+ 
C) Pb2+ and Ca2+ 
D) Ca2+ and Ba2+

Question 8

What is the molar solubility of AgCl in 1.0 M K2S2O3 if the complex ion Ag(S2O3)23- forms? The Ksp for AgCl is 1.8 × 10-10 and the Kf for Ag(S2O3)23- is 2.9 × 1013.

Accepted Answer

A) 0)50 M 
B) 1)0 M 
C) 1)5 M 
D) 2)0 M 
A) 0)50 M 
B) 1)0 M 
C) 1)5 M 
D) 2)0 M

Question 9

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H

Accepted Answer

A) 9)43 
B) 9)08 
C) 4)92 
D) 4)57 
A) 9)43 
B) 9)08 
C) 4)92 
D) 4)57

Question 10

A solution may contain the following ions Ag+,Cu2+,Mn2+,Ca2+,and Na+.No precipitate formed when 0.10 M NaCl was added but a dark colored precipitate formed when H2S was added to an acidic portion of the solution.After the removal of the solid the solution was made basic and more H2S was added and a dark precipitate again formed.Treatment of the filtrate with (NH4)2CO3 resulted in a white precipitate.If no further tests were made then what conclusions can you draw?

Accepted Answer

A) possible ions present Cu2+,Mn2+,Na+ 
B) possible ions present Cu2+,Mn2+,Ca2+ 
C) possible ions present Cu2+,Mn2+,Ca2+,Na+ 
D) possible ions present Ag+,Cu2+,Mn2+,Ca2+,Na+ 
A) possible ions present Cu2+,Mn2+,Na+ 
B) possible ions present Cu2+,Mn2+,Ca2+ 
C) possible ions present Cu2+,Mn2+,Ca2+,Na+ 
D) possible ions present Ag+,Cu2+,Mn2+,Ca2+,Na+

Question 11

Sulfurous acid,H2SO3 has acid dissociation constants Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.What is the pH after 10.00 mL of 0.1000 M NaOH is added to 10.00 mL of 0.1000 M H2SO3?

Accepted Answer

A) 1)82 
B) 3)60 
C) 4)25 
D) 7)20 
A) 1)82 
B) 3)60 
C) 4)25 
D) 7)20

Question 12

The following pictures represent solutions that contain a weak acid HA (pKS1U1B1aS1U1B0 = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. )  
-Which solution has the largest percent dissociation of HA?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4) 
A) (1) 
B) (2) 
C) (3) 
D) (4)

Question 13

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH.  
-At which point a-d is the pKa of the acid equal to the pH?

Accepted Answer

A) point a 
B) point b 
C) point c 
D) point d 
A) point a 
B) point b 
C) point c 
D) point d

Question 14

At 25°C calcium fluoride has a solubility product constant Ksp = 3.5 × 10-11.The solubility of CaF2 at this temperature is ________ mol/L.

Accepted Answer

Question 15

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH3NH2,with 20.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

Accepted Answer

A) 10.17 
B) 10.57 
C) 10.97 
D) 11.78 
A) 10.17 
B) 10.57 
C) 10.97 
D) 11.78

Question 16

The neutralization constant Kn for the neutralization of phenobarbital (C12H12N2O3)and morphine (C17H19NO3)is 2.9.The acid dissociation constant Ka for phenobarbital is 3.9 × 10-8.What is the base dissociation constant Kb for morphine?

Accepted Answer

A) 1)3 × 10-22 
B) 6)3 × 10-23 
C) 7)4 × 10-7 
D) 1)1 × 107 
A) 1)3 × 10-22 
B) 6)3 × 10-23 
C) 7)4 × 10-7 
D) 1)1 × 107

Question 17

The following pictures represent solutions at various points in the titration of a weak acid HA with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0 initially present,OHS1U1P1-S1S1P0 initially present and solvent water molecules have been omitted for clarity).  
-Which picture represents the solution at the equivalence point?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4) 
A) (1) 
B) (2) 
C) (3) 
D) (4)

Question 18

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

Accepted Answer

A) CH3CO2H(aq)+ NaOH(aq)⇌ H2O(l)+ NaCH3CO2(aq) 
B) HCl(aq)+ C5H5N(aq)⇌ C5H5NHCl(aq) 
C) HCl(aq)+ NaOH(aq)⇌ H2O(l)+ NaCl(aq) 
D) H2SO4(aq)+ 2 KOH(aq)⇌2 H2O(l)+ K2SO4(aq) 
A) CH3CO2H(aq)+ NaOH(aq)⇌ H2O(l)+ NaCH3CO2(aq) 
B) HCl(aq)+ C5H5N(aq)⇌ C5H5NHCl(aq) 
C) HCl(aq)+ NaOH(aq)⇌ H2O(l)+ NaCl(aq) 
D) H2SO4(aq)+ 2 KOH(aq)⇌2 H2O(l)+ K2SO4(aq)

Question 19

Potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2.Describe what happens if the Ksp for Ag2CrO4 is 1.1 × 10-12 and the Ksp of BaCrO4 is 1.2 × 10-10.

Accepted Answer

A) The BaCrO4 precipitates first out of solution. 
B) The Ag2CrO4 precipitates first out of solution and then BaCrO4 precipitates. 
C) Both BaCrO4 and Ag2CrO4 precipitate simultaneously out of solution. 
D) Neither BaCrO4 nor Ag2CrO4 precipitates out of solution. 
A) The BaCrO4 precipitates first out of solution. 
B) The Ag2CrO4 precipitates first out of solution and then BaCrO4 precipitates. 
C) Both BaCrO4 and Ag2CrO4 precipitate simultaneously out of solution. 
D) Neither BaCrO4 nor Ag2CrO4 precipitates out of solution.

Question 20

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 × 10-12.

Accepted Answer

A) 5)6 × 10-10 M 
B) 5)6 × 10-8 M 
C) 2)4 × 10-6 M 
D) 1)1 × 10-4 M 
A) 5)6 × 10-10 M 
B) 5)6 × 10-8 M 
C) 2)4 × 10-6 M 
D) 1)1 × 10-4 M

Silver oxalate,Ag₂C₂O₄,has a molar solubility = 1.1 × 10^-4 mol/L.Ag₂C₂O₄ has a solubility product K_sp = ________.

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid H₂X⁺)are K_a₁ = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

CaF₂ has K_sp = 3.5 × 10^-11.If 25 mL of 8.0 × 10^-4 M Ca(NO₃)₂ is mixed with 75 mL of 4.0 × 10^-4 M KF,a precipitate of CaF₂ ________ (will,will not)form.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -A buffer region is indicated by which point(s)a-d?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents pK_a2?

Which pair of ions can be separated by the addition of sulfide ion?

What is the molar solubility of AgCl in 1.0 M K₂S₂O₃ if the complex ion Ag(S₂O₃)₂^3- forms? The Ksp for AgCl is 1.8 × 10^-10 and the K_f for Ag(S₂O₃)₂^3- is 2.9 × 10¹³.

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H

Sulfurous acid,H₂SO₃ has acid dissociation constants K_a1 = 1.5 × 10^-2 and K_a2 = 6.3 × 10^-8.What is the pH after 10.00 mL of 0.1000 M NaOH is added to 10.00 mL of 0.1000 M H₂SO₃?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -At which point a-d is the pK_a of the acid equal to the pH?

At 25°C calcium fluoride has a solubility product constant K_sp = 3.5 × 10^-11.The solubility of CaF₂ at this temperature is ________ mol/L.

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 20.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

The neutralization constant K_n for the neutralization of phenobarbital (C₁₂H₁₂N₂O₃)and morphine (C₁₇H₁₉NO₃)is 2.9.The acid dissociation constant K_a for phenobarbital is 3.9 × 10^-8.What is the base dissociation constant K_b for morphine?

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

Potassium chromate is slowly added to a solution containing 0.20 M AgNO₃ and 0.20 M Ba(NO₃)₂.Describe what happens if the K_sp for Ag₂CrO₄ is 1.1 × 10^-12 and the K_sp of BaCrO₄ is 1.2 × 10^-10.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_sp for Mg(OH)₂ is 5.6 × 10^-12.

Chemistry: Matter and Measurement

Atoms, molecules, and Ions

Formulas, equations, and Moles

Reactions in Aqueous Solutions

Periodicity and the Atomic Structure of Atoms

Ionic Bonds and Some Main-Group Chemistry

Covalent Bonds and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

Solutions and Their Properties

Chemical Kinetics

Chemical Equilibrium

Aqueous Equilibria: Acids and Bases

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

Hydrogen, oxygen, and Water

The Main-Group Elements

Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

Nuclear Chemistry

Organic and Biological Chemistry

Filters

Exam 15: Applications of Aqueous Equilibria

Silver oxalate,Ag2C2O4,has a molar solubility = 1.1 × 10-4 mol/L.Ag2C2O4 has a solubility product Ksp = ________.

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid H2X+)are Ka1 = 4.6 × 10-3 and Ka2 = 2.0 × 10-10.What is the pH of 50.00 mL of a 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

CaF2 has Ksp = 3.5 × 10-11.If 25 mL of 8.0 × 10-4 M Ca(NO3)2 is mixed with 75 mL of 4.0 × 10-4 M KF,a precipitate of CaF2 ________ (will,will not)form.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. -A buffer region is indicated by which point(s)a-d?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. -Which point a-d represents pKa2?

Which pair of ions can be separated by the addition of sulfide ion?

What is the molar solubility of AgCl in 1.0 M K2S2O3 if the complex ion Ag(S2O3)23- forms? The Ksp for AgCl is 1.8 × 10-10 and the Kf for Ag(S2O3)23- is 2.9 × 1013.

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H

Sulfurous acid,H2SO3 has acid dissociation constants Ka1 = 1.5 × 10-2 and Ka2 = 6.3 × 10-8.What is the pH after 10.00 mL of 0.1000 M NaOH is added to 10.00 mL of 0.1000 M H2SO3?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -At which point a-d is the pKa of the acid equal to the pH?

At 25°C calcium fluoride has a solubility product constant Ksp = 3.5 × 10-11.The solubility of CaF2 at this temperature is ________ mol/L.

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH3NH2,with 20.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

The neutralization constant Kn for the neutralization of phenobarbital (C12H12N2O3)and morphine (C17H19NO3)is 2.9.The acid dissociation constant Ka for phenobarbital is 3.9 × 10-8.What is the base dissociation constant Kb for morphine?

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

Potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2.Describe what happens if the Ksp for Ag2CrO4 is 1.1 × 10-12 and the Ksp of BaCrO4 is 1.2 × 10-10.

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 × 10-12.

Chemistry: Matter and Measurement

Atoms, molecules, and Ions

Formulas, equations, and Moles

Reactions in Aqueous Solutions

Periodicity and the Atomic Structure of Atoms

Ionic Bonds and Some Main-Group Chemistry

Covalent Bonds and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

Solutions and Their Properties

Chemical Kinetics

Chemical Equilibrium

Aqueous Equilibria: Acids and Bases

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

Hydrogen, oxygen, and Water

The Main-Group Elements

Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

Nuclear Chemistry

Organic and Biological Chemistry

Filters

Silver oxalate,Ag₂C₂O₄,has a molar solubility = 1.1 × 10^-4 mol/L.Ag₂C₂O₄ has a solubility product K_sp = ________.

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid H₂X⁺)are K_a₁ = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

CaF₂ has K_sp = 3.5 × 10^-11.If 25 mL of 8.0 × 10^-4 M Ca(NO₃)₂ is mixed with 75 mL of 4.0 × 10^-4 M KF,a precipitate of CaF₂ ________ (will,will not)form.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -A buffer region is indicated by which point(s)a-d?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents pK_a2?

What is the molar solubility of AgCl in 1.0 M K₂S₂O₃ if the complex ion Ag(S₂O₃)₂^3- forms? The Ksp for AgCl is 1.8 × 10^-10 and the K_f for Ag(S₂O₃)₂^3- is 2.9 × 10¹³.

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H

Sulfurous acid,H₂SO₃ has acid dissociation constants K_a1 = 1.5 × 10^-2 and K_a2 = 6.3 × 10^-8.What is the pH after 10.00 mL of 0.1000 M NaOH is added to 10.00 mL of 0.1000 M H₂SO₃?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -At which point a-d is the pK_a of the acid equal to the pH?

At 25°C calcium fluoride has a solubility product constant K_sp = 3.5 × 10^-11.The solubility of CaF₂ at this temperature is ________ mol/L.

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 20.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

The neutralization constant K_n for the neutralization of phenobarbital (C₁₂H₁₂N₂O₃)and morphine (C₁₇H₁₉NO₃)is 2.9.The acid dissociation constant K_a for phenobarbital is 3.9 × 10^-8.What is the base dissociation constant K_b for morphine?

Potassium chromate is slowly added to a solution containing 0.20 M AgNO₃ and 0.20 M Ba(NO₃)₂.Describe what happens if the K_sp for Ag₂CrO₄ is 1.1 × 10^-12 and the K_sp of BaCrO₄ is 1.2 × 10^-10.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_sp for Mg(OH)₂ is 5.6 × 10^-12.