Question 1

Which of the following aqueous mixtures would be a buffer system?

Accepted Answer

A) HCl,NaCl 
B) HNO3,NaNO3 
C) H3PO4,H2PO4- 
D) H2SO4,CH3COOH 
E) NH3,NaOH 
A) HCl,NaCl 
B) HNO3,NaNO3 
C) H3PO4,H2PO4- 
D) H2SO4,CH3COOH 
E) NH3,NaOH

Question 2

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

Accepted Answer

A) HOC6H4OCOOH,Ka = 1.0 $\times$ 10-3 
B) C6H4(COOH)2,Ka = 2.9 $\times$ 10-4 
C) CH3COOH,Ka = 1.8 $\times$ 10-5 
D) C5H5O5COOH-2,Ka = 4.0 $\times$ 10-6 
E) HBrO,Ka = 2.3 $\times$ 10-9 
A) HOC6H4OCOOH,Ka = 1.0 $\times$ 10-3 
B) C6H4(COOH)2,Ka = 2.9 $\times$ 10-4 
C) CH3COOH,Ka = 1.8 $\times$ 10-5 
D) C5H5O5COOH-2,Ka = 4.0 $\times$ 10-6 
E) HBrO,Ka = 2.3 $\times$ 10-9

Question 3

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which
[H2PO4-] = [HPO42-] = 0.35 M?

Accepted Answer

A) The pH will increase slightly. 
B) The pH will increase significantly. 
C) The pH will decrease slightly. 
D) The pH will decrease significantly. 
E) Since it is a buffer solution,the pH will not be affected. 
A) The pH will increase slightly. 
B) The pH will increase significantly. 
C) The pH will decrease slightly. 
D) The pH will decrease significantly. 
E) Since it is a buffer solution,the pH will not be affected.

Question 4

Which of the following has the highest buffer capacity?

Accepted Answer

A) 0.10 M H2PO4-/0.10 M HPO42- 
B) 0.50 M H2PO4-/0.10 M HPO42- 
C) 0.10 M H2PO4-/0.50 M HPO42- 
D) 0.50 M H2PO4-/0.50 M HPO42- 
E) They all have the same buffer capacity. 
A) 0.10 M H2PO4-/0.10 M HPO42- 
B) 0.50 M H2PO4-/0.10 M HPO42- 
C) 0.10 M H2PO4-/0.50 M HPO42- 
D) 0.50 M H2PO4-/0.50 M HPO42- 
E) They all have the same buffer capacity.

Question 5

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO3)2.Which of the following statements is correct? Ksp = 6.44 $\times$ 10-3 for CdF2

Accepted Answer

A) Cadmium fluoride precipitates until the solution is saturated. 
B) The solution is unsaturated and no precipitate forms. 
C) The solubility of cadmium fluoride is increased by the presence of additional fluoride ions. 
D) One must know Ksp for cadmium nitrate to make meaningful predictions on this system. 
E) The presence of NaF will raise the solubility of Cd(NO3)2. 
A) Cadmium fluoride precipitates until the solution is saturated. 
B) The solution is unsaturated and no precipitate forms. 
C) The solubility of cadmium fluoride is increased by the presence of additional fluoride ions. 
D) One must know Ksp for cadmium nitrate to make meaningful predictions on this system. 
E) The presence of NaF will raise the solubility of Cd(NO3)2.

Question 6

When a weak acid is titrated with a strong base,the pH at the equivalence point

Accepted Answer

A) is greater than 7.0. 
B) is equal to 7.0. 
C) is less than 7.0. 
D) is equal to the pKa of the acid. 
E) is equal to 14.0 - pKb ,where pKb is that of the base. 
A) is greater than 7.0. 
B) is equal to 7.0. 
C) is less than 7.0. 
D) is equal to the pKa of the acid. 
E) is equal to 14.0 - pKb ,where pKb is that of the base.

Question 7

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8(ethylene diamine)and 0.35 C2N2H9Cl?
Kb = 4.7 $\times$ 10-4

Accepted Answer

A) 2.0 $\times$ l0-3 M 
B) 1.1 $\times$ 10-3 M 
C) 6.3 $\times$ 10-9 M 
D) 2.1 $\times$ 10-10 M 
E) 5.0 $\times$ 10-11 M 
A) 2.0 $\times$ l0-3 M 
B) 1.1 $\times$ 10-3 M 
C) 6.3 $\times$ 10-9 M 
D) 2.1 $\times$ 10-10 M 
E) 5.0 $\times$ 10-11 M

Question 8

What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4?
Ka = 6.2 $\times$ 10-8

Accepted Answer

A) 6.51 
B) 6.91 
C) 7.51 
D) 7.90 
E) 8.13 
A) 6.51 
B) 6.91 
C) 7.51 
D) 7.90 
E) 8.13

Question 9

Calculate the solubility of lead(II)iodide,PbI2,in 0.025 M KI.Ksp = 7.9 $\times$ 10-9

Accepted Answer

A) 4.5 $\times$ 10-2 M 
B) 2.8 $\times$ 10-2 M 
C) 8.9 $\times$ 10-5 M 
D) 5.0 $\times$ 10-5 M 
E) 1.3 $\times$ 10-5 M 
A) 4.5 $\times$ 10-2 M 
B) 2.8 $\times$ 10-2 M 
C) 8.9 $\times$ 10-5 M 
D) 5.0 $\times$ 10-5 M 
E) 1.3 $\times$ 10-5 M

Question 10

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77.What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Accepted Answer

A) 3.67 
B) 3.78 
C) 3.81 
D) 3.85 
E) 3.95 
A) 3.67 
B) 3.78 
C) 3.81 
D) 3.85 
E) 3.95

Question 11

The end point in a titration is defined as the point when the indicator changes color.

Accepted Answer

A) True 
 B)False

Question 12

Which of the following substances has the greatest solubility in water?

Accepted Answer

A) Ba(IO3)2,Ksp = 1.5 $\times$ 10-9 
B) PbF2,Ksp = 3.6 $\times$ 10-8 
C) SrSO4,Ksp = 3.2 $\times$ 10-7 
D) CuCl,Ksp = 1.9 $\times$ 10-7 
E) CdS,Ksp = 1.0 $\times$ 10-24 
A) Ba(IO3)2,Ksp = 1.5 $\times$ 10-9 
B) PbF2,Ksp = 3.6 $\times$ 10-8 
C) SrSO4,Ksp = 3.2 $\times$ 10-7 
D) CuCl,Ksp = 1.9 $\times$ 10-7 
E) CdS,Ksp = 1.0 $\times$ 10-24

Question 13

Which of the following substances has the greatest solubility in water?

Accepted Answer

A) PbI2,Ksp = 7.9 $\times$ 10-9 
B) BaF2,Ksp = 1.5 $\times$ 10-6 
C) Ca(OH)2,Ksp = 6.5 $\times$ 10-6 
D) Zn(IO3)2,Ksp = 3.9 $\times$ 10-6 
E) Ag2SO4,Ksp = 1.5 $\times$ 10-5 
A) PbI2,Ksp = 7.9 $\times$ 10-9 
B) BaF2,Ksp = 1.5 $\times$ 10-6 
C) Ca(OH)2,Ksp = 6.5 $\times$ 10-6 
D) Zn(IO3)2,Ksp = 3.9 $\times$ 10-6 
E) Ag2SO4,Ksp = 1.5 $\times$ 10-5

Question 14

At the equivalence point in an acid-base titration

Accepted Answer

A) the [H3O+] equals the Ka of the acid. 
B) the [H3O+] equals the Ka of the indicator. 
C) the amounts of acid and base which have been combined are in their stoichiometric ratio. 
D) the pH is 7.0. 
E) the pH has reached a maximum. 
A) the [H3O+] equals the Ka of the acid. 
B) the [H3O+] equals the Ka of the indicator. 
C) the amounts of acid and base which have been combined are in their stoichiometric ratio. 
D) the pH is 7.0. 
E) the pH has reached a maximum.

Question 15

When a strong acid is titrated with a strong base,the pH at the equivalence point

Accepted Answer

A) is greater than 7.0. 
B) is equal to 7.0. 
C) is less than 7.0,but is not 3.5. 
D) is equal to the pKa of the acid. 
E) is equal to 3.5. 
A) is greater than 7.0. 
B) is equal to 7.0. 
C) is less than 7.0,but is not 3.5. 
D) is equal to the pKa of the acid. 
E) is equal to 3.5.

Question 16

Calculate the solubility of barium carbonate,BaCO3,in pure water.Ksp = 2.0 $\times$ 10-9

Accepted Answer

A) 1.3 $\times$ 10-3 M 
B) 3.2 $\times$ 10-5 M 
C) 2.2 $\times$ 10-5 M 
D) 4.5 $\times$ 10-5 M 
E) 4.0 $\times$ 10-18 M 
A) 1.3 $\times$ 10-3 M 
B) 3.2 $\times$ 10-5 M 
C) 2.2 $\times$ 10-5 M 
D) 4.5 $\times$ 10-5 M 
E) 4.0 $\times$ 10-18 M

Which of the following aqueous mixtures would be a buffer system?

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H₂PO₄^-] = [HPO₄^2-] = 0.35 M?

Which of the following has the highest buffer capacity?

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO₃)₂.Which of the following statements is correct? K_sp = 6.44 $\times$ 10^-3 for CdF₂

When a weak acid is titrated with a strong base,the pH at the equivalence point

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈(ethylene diamine)and 0.35 C₂N₂H₉Cl? K_b = 4.7 $\times$ 10^-4

What is the pH of a buffer that consists of 0.20 M NaH₂PO₄ and 0.40 M Na₂HPO₄? K_a = 6.2 $\times$ 10^-8

Calculate the solubility of lead(II)iodide,PbI₂,in 0.025 M KI.K_sp = 7.9 $\times$ 10^-9

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77.What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

The end point in a titration is defined as the point when the indicator changes color.

Which of the following substances has the greatest solubility in water?

Which of the following substances has the greatest solubility in water?

At the equivalence point in an acid-base titration

When a strong acid is titrated with a strong base,the pH at the equivalence point

Calculate the solubility of barium carbonate,BaCO₃,in pure water.K_sp = 2.0 $\times$ 10^-9

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 19: Ionic Equilibria in Aqueous Systems

Which of the following aqueous mixtures would be a buffer system?

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H2PO4-] = [HPO42-] = 0.35 M?

Which of the following has the highest buffer capacity?

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO3)2.Which of the following statements is correct? Ksp = 6.44 ×\times× 10-3 for CdF2

When a weak acid is titrated with a strong base,the pH at the equivalence point

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8(ethylene diamine)and 0.35 C2N2H9Cl? Kb = 4.7 ×\times× 10-4

What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? Ka = 6.2 ×\times× 10-8

Calculate the solubility of lead(II)iodide,PbI2,in 0.025 M KI.Ksp = 7.9 ×\times× 10-9

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77.What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

The end point in a titration is defined as the point when the indicator changes color.

Which of the following substances has the greatest solubility in water?

Which of the following substances has the greatest solubility in water?

At the equivalence point in an acid-base titration

When a strong acid is titrated with a strong base,the pH at the equivalence point

Calculate the solubility of barium carbonate,BaCO3,in pure water.Ksp = 2.0 ×\times× 10-9

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

What will be the effect of adding 0.5 mL of 0.1 M HCl to 100 mL of a phosphate buffer in which [H₂PO₄^-] = [HPO₄^2-] = 0.35 M?

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate,Cd(NO₃)₂.Which of the following statements is correct? K_sp = 6.44 $\times$ 10^-3 for CdF₂

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈(ethylene diamine)and 0.35 C₂N₂H₉Cl? K_b = 4.7 $\times$ 10^-4

What is the pH of a buffer that consists of 0.20 M NaH₂PO₄ and 0.40 M Na₂HPO₄? K_a = 6.2 $\times$ 10^-8

Calculate the solubility of lead(II)iodide,PbI₂,in 0.025 M KI.K_sp = 7.9 $\times$ 10^-9

Calculate the solubility of barium carbonate,BaCO₃,in pure water.K_sp = 2.0 $\times$ 10^-9