Question 1

Which of the following would decrease the Ksp for PbI2?

Accepted Answer

A) Lowering the pH of the solution 
B) Adding a solution of Pb(NO3)2 
C) Adding a solution of KI 
D) None of the above-the Ksp of a compound is constant at constant temperature. 
A) Lowering the pH of the solution 
B) Adding a solution of Pb(NO3)2 
C) Adding a solution of KI 
D) None of the above-the Ksp of a compound is constant at constant temperature. D

Question 2

Calculate the percent ionization of cyanic acid, Ka = 2.0 × 10-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

Accepted Answer

A) 0.02% 
B) 0.10% 
C) 0.20% 
D) 2.0% 
E) 20% 
A) 0.02% 
B) 0.10% 
C) 0.20% 
D) 2.0% 
E) 20% C

Question 3

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

Accepted Answer

A) True 
 B)False  False

Question 4

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer.

Accepted Answer

Question 5

At 25 °C, the base ionization constant for NH3 is 1.8 × 10-5.Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Accepted Answer

Question 6

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed?

Accepted Answer

A) 0.10M H2CO3 and 0.050M HCl 
B) 0.10M H2CO3 and 0.10M KOH 
C) 0.10M H2CO3 and 0.10M HCl 
D) 0.10M H2CO3 and 0.050M KOH 
E) 0.10M K2CO3 and 0.050M KOH 
A) 0.10M H2CO3 and 0.050M HCl 
B) 0.10M H2CO3 and 0.10M KOH 
C) 0.10M H2CO3 and 0.10M HCl 
D) 0.10M H2CO3 and 0.050M KOH 
E) 0.10M K2CO3 and 0.050M KOH

Question 7

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L.What is Ksp for this compound?

Accepted Answer

A) 1.8 × 10-4 
B) 3.6 × 10-4 
C) 1.3 × 10-7 
D) 3.2 × 10-8 
E) 2.8 × 10-14 
A) 1.8 × 10-4 
B) 3.6 × 10-4 
C) 1.3 × 10-7 
D) 3.2 × 10-8 
E) 2.8 × 10-14

Question 8

The solubility product for calcium phosphate is Ksp = 1.3 × 10-26.What is the molar solubility of calcium phosphate?

Accepted Answer

A) 1.3 × 10-26 M 
B) 1.5 × 10-7 M 
C) 2.6 × 10-6 M 
D) 4.6 × 10-6 M 
E) 6.6 × 10-6 M 
A) 1.3 × 10-26 M 
B) 1.5 × 10-7 M 
C) 2.6 × 10-6 M 
D) 4.6 × 10-6 M 
E) 6.6 × 10-6 M

Question 9

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4)= 1.1 × 10-12] What is the concentration of the silver ion remaining in solution?

Accepted Answer

A) Yes, [Ag+] = 2.9 × 10-6 M. 
B) Yes, [Ag+] = 0.060 M. 
C) Yes, [Ag+] = 1.3 × 10-4 M. 
D) No, [Ag+] = 0.060 M. 
E) No, [Ag+] = 0.105 M. 
A) Yes, [Ag+] = 2.9 × 10-6 M. 
B) Yes, [Ag+] = 0.060 M. 
C) Yes, [Ag+] = 1.3 × 10-4 M. 
D) No, [Ag+] = 0.060 M. 
E) No, [Ag+] = 0.105 M.

Question 10

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III)fluoride.(For CrF3 , Ksp = 6.6 × 10-11.)

Accepted Answer

A) 0.023 M 
B) 0.032 M 
C) 7.7 × 10-8 M 
D) 2.9 × 10-9 M 
E) 6.9 × 10-10 M 
A) 0.023 M 
B) 0.032 M 
C) 7.7 × 10-8 M 
D) 2.9 × 10-9 M 
E) 6.9 × 10-10 M

Question 11

Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II)iodide to 500.mL of 0.150 M KI.[For PbI2, Ksp = 1.39 × 10-8.]

Accepted Answer

A) 3.04 × 10-4 M 
B) 1.54 × 10-7 M 
C) 6.18 × 10-7 M 
D) 1.52 × 10-4 M 
E) 9.27 × 10-8 M 
A) 3.04 × 10-4 M 
B) 1.54 × 10-7 M 
C) 6.18 × 10-7 M 
D) 1.52 × 10-4 M 
E) 9.27 × 10-8 M

Question 12

Calculate the molar solubility of BaCO3 in a 0.10 M solution of Na2CO3(aq).(Ksp (BaCO3)= 8.1 x 10-9)

Accepted Answer

A) 8.1 x 10-9 M 
B) 9.0 x 10-5 M 
C) 8.1 x 10-8 M 
D) 2.8 x 10-4 M 
E) 0.10 M 
A) 8.1 x 10-9 M 
B) 9.0 x 10-5 M 
C) 8.1 x 10-8 M 
D) 2.8 x 10-4 M 
E) 0.10 M

Question 13

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

Accepted Answer

A) 1.0 
B) 6.0 
C) 7.0 
D) 8.0 
E) 13.0 
A) 1.0 
B) 6.0 
C) 7.0 
D) 8.0 
E) 13.0

Question 14

The Ksp value for lead(II)chloride is 2.4 × 10-4.What is the molar solubility of lead(II)chloride?

Accepted Answer

A) 2.4 × 10-4 mol/L 
B) 6.2 × 10-2 mol/L 
C) 7.7 × 10-3 mol/L 
D) 3.9 × 10-2 mol/L 
E) 6.0 × 10-5 mol/L 
A) 2.4 × 10-4 mol/L 
B) 6.2 × 10-2 mol/L 
C) 7.7 × 10-3 mol/L 
D) 3.9 × 10-2 mol/L 
E) 6.0 × 10-5 mol/L

Question 15

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH3COONa would be classified as a buffer solution.

Accepted Answer

A) True 
 B)False

Question 16

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 × 10-8; Ksp (AgI)= 8.3 × 10-17] Calculate the Ag+ concentration when PbI2 just begins to precipitate.

Accepted Answer

Question 17

In which one of the following solutions will acetic acid have the greatest percent ionization?

Accepted Answer

A) 0.1 M CH3COOH 
B) 0.1 M CH3COOH dissolved in 0.1 M HCl 
C) 0.1 M CH3COOH dissolved in 0.2 M HCl 
D) 0.1 M CH3COOH plus 0.1 M CH3COONa 
E) 0.1 M CH3COOH plus 0.2 M CH3COONa 
A) 0.1 M CH3COOH 
B) 0.1 M CH3COOH dissolved in 0.1 M HCl 
C) 0.1 M CH3COOH dissolved in 0.2 M HCl 
D) 0.1 M CH3COOH plus 0.1 M CH3COONa 
E) 0.1 M CH3COOH plus 0.2 M CH3COONa

Question 18

The molar solubility of lead(II)iodate in water is 4.0 × 10-5 mol/L.Calculate Ksp for lead(II)iodate.

Accepted Answer

A) 1.6 × 10-9 
B) 6.4 × 10-14 
C) 2.6 × 10-13 
D) 4.0 × 10-5 
E) 4.0 × 10-15 
A) 1.6 × 10-9 
B) 6.4 × 10-14 
C) 2.6 × 10-13 
D) 4.0 × 10-5 
E) 4.0 × 10-15

Question 19

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [Ka(C6H5COOH)= 6.5 × 10-5]

Accepted Answer

Question 20

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750.mL of 0.125 M NaF.[For CaF2, Ksp = 3.95 × 10-11.]

Accepted Answer

A) 3.16 × 10-10 M 
B) 2.53 × 10-9 M 
C) 4.29 × 10-4 M 
D) 6.32 × 10-10 M 
E) 2.15 × 10-4 M 
A) 3.16 × 10-10 M 
B) 2.53 × 10-9 M 
C) 4.29 × 10-4 M 
D) 6.32 × 10-10 M 
E) 2.15 × 10-4 M

Exam 16: Acid-Base Equilibria and Solubility Equilibria

Which of the following would decrease the Ksp for PbI2?

Calculate the percent ionization of cyanic acid, Ka = 2.0 × 10-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer.

At 25 °C, the base ionization constant for NH3 is 1.8 × 10-5.Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed?

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L.What is Ksp for this compound?

The solubility product for calcium phosphate is Ksp = 1.3 × 10-26.What is the molar solubility of calcium phosphate?

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4)= 1.1 × 10-12] What is the concentration of the silver ion remaining in solution?

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III)fluoride.(For CrF3 , Ksp = 6.6 × 10-11.)

Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II)iodide to 500.mL of 0.150 M KI.[For PbI2, Ksp = 1.39 × 10-8.]

Calculate the molar solubility of BaCO3 in a 0.10 M solution of Na2CO3(aq).(Ksp (BaCO3)= 8.1 x 10-9)

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

The Ksp value for lead(II)chloride is 2.4 × 10-4.What is the molar solubility of lead(II)chloride?

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH3COONa would be classified as a buffer solution.

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 × 10-8; Ksp (AgI)= 8.3 × 10-17] Calculate the Ag+ concentration when PbI2 just begins to precipitate.

In which one of the following solutions will acetic acid have the greatest percent ionization?

The molar solubility of lead(II)iodate in water is 4.0 × 10-5 mol/L.Calculate Ksp for lead(II)iodate.

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [Ka(C6H5COOH)= 6.5 × 10-5]

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750.mL of 0.125 M NaF.[For CaF2, Ksp = 3.95 × 10-11.]

Chemistry: the Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Which of the following would decrease the K_sp for PbI₂?

Calculate the percent ionization of cyanic acid, K_a = 2.0 × 10^-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO₂/HNO₂ buffer.

At 25 °C, the base ionization constant for NH₃ is 1.8 × 10^-5.Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L.What is K_sp for this compound?

The solubility product for calcium phosphate is K_sp = 1.3 × 10^-26.What is the molar solubility of calcium phosphate?

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄)= 1.1 × 10^-12] What is the concentration of the silver ion remaining in solution?

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III)fluoride.(For CrF₃, K_sp = 6.6 × 10^-11.)

Find the concentration of Pb²⁺ ions in a solution made by adding 5.00 g of lead(II)iodide to 500.mL of 0.150 M KI.[For PbI₂, K_sp = 1.39 × 10^-8.]

Calculate the molar solubility of BaCO₃ in a 0.10 M solution of Na₂CO₃(aq).(K_sp (BaCO₃)= 8.1 x 10^-9)

The K_sp value for lead(II)chloride is 2.4 × 10^-4.What is the molar solubility of lead(II)chloride?

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH₃COONa would be classified as a buffer solution.

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 × 10^-8; K_sp (AgI)= 8.3 × 10^-17] Calculate the Ag⁺ concentration when PbI₂ just begins to precipitate.

The molar solubility of lead(II)iodate in water is 4.0 × 10^-5 mol/L.Calculate K_sp for lead(II)iodate.

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [K_a(C₆H₅COOH)= 6.5 × 10^-5]

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750.mL of 0.125 M NaF.[For CaF₂, K_sp = 3.95 × 10^-11.]