Question 1

What would happen to the Ag+ and Cl- concentrations if NaCl(s) was added to a saturated solution of AgCl in water?

Accepted Answer

A) [Ag+] and [Cl-] both would increase. 
B) [Ag+] and [Cl-] both would decrease. 
C) [Ag+] would become larger, and [Cl-] would become smaller. 
D) [Ag+] would become smaller, and [Cl-] would become larger. 
E) [Ag+] and [Cl-] would remain the same because the solution is saturated. 
A) [Ag+] and [Cl-] both would increase. 
B) [Ag+] and [Cl-] both would decrease. 
C) [Ag+] would become larger, and [Cl-] would become smaller. 
D) [Ag+] would become smaller, and [Cl-] would become larger. 
E) [Ag+] and [Cl-] would remain the same because the solution is saturated.

Question 2

You are working on a project to recycle nickel and cadmium from old nickel-cadmium batteries that have an iron casing.The batteries are dissolved in aqueous nitric acid, producing a solution containing primarily Ni2+, Cd2+, and Fe3+ cations.One idea is to add sodium hydroxide to neutralize the acid and cause precipitation of Ni(OH)2, Cd(OH)2, and Fe(OH)3.Assume the concentration of each of the cations is 0.100 M before the sodium hydroxide is added.The pH increases as the sodium hydroxide is added.Which compound will precipitate first, and what is the pH at that point?

Accepted Answer

A) Cd(OH)2; pH = 9.16 
B) Fe(OH)3; pH = 4.81 
C) Fe(OH)3; pH = 1.93 
D) Cd(OH)2; pH= 6.42 
E) Ni(OH)2; pH =7.24 
A) Cd(OH)2; pH = 9.16 
B) Fe(OH)3; pH = 4.81 
C) Fe(OH)3; pH = 1.93 
D) Cd(OH)2; pH= 6.42 
E) Ni(OH)2; pH =7.24

Question 3

As the pH decreases, the solubility of _______ increases.

Accepted Answer

A) lead(II) chloride 
B) silver iodate 
C) calcium carbonate 
D) mercury(I) bromide 
E) silver chloride 
A) lead(II) chloride 
B) silver iodate 
C) calcium carbonate 
D) mercury(I) bromide 
E) silver chloride

Question 4

How many moles of sodium acetate must be added to 500.0 mL of 0.250 M acetic acid solution to produce a solution with a pH of 4.94? (The pKa of acetic acid is 4.74.)

Accepted Answer

A) 0.011 moles 
B) 0.021 moles 
C) 0.13 moles 
D) 0.20 moles 
E) 0.21 moles 
A) 0.011 moles 
B) 0.021 moles 
C) 0.13 moles 
D) 0.20 moles 
E) 0.21 moles

Question 5

Ksp for lead iodide is 8.5 *10-9 at 25°C.Will PbI2 precipitate if 250.0 mL of 0.0480 M NaI solution is added to 375.0 mL of 0.0388 M (PbNO3)2 solution?

Accepted Answer

Q_sp= 8.58 *10^-

Question 6

Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl2, 95.21 g/mol, Ksp = 740).How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

Accepted Answer

A) 9.0 kg 
B) 12 kg 
C) 57 kg 
D) 5.4 kg 
E) 7.2 kg 
A) 9.0 kg 
B) 12 kg 
C) 57 kg 
D) 5.4 kg 
E) 7.2 kg

Question 7

Consider the following aqueous equilibrium for a formic acid solution, HCOOH(aq) ⇄ H+(aq) + HCOO-(aq).Suppose solid sodium formate, NaHCOO, is added to the solution.Which of the following statements regarding the resulting solution is NOT correct? Ignore any volume changes.

Accepted Answer

A) The pH decreases. 
B) The H+ concentration decreases. 
C) The system shifts left to reestablish equilibrium. 
D) The HCOOH concentration increases. 
E) The value of Ka does not change. 
A) The pH decreases. 
B) The H+ concentration decreases. 
C) The system shifts left to reestablish equilibrium. 
D) The HCOOH concentration increases. 
E) The value of Ka does not change.

Question 8

A mining operation needs to separate silver and copper.You are to determine whether this separation can be accomplished by oxidizing the metals to Ag+ and Cu+, each one at a concentration of 0.15 M, and then precipitating one as the chloride salt without precipitating the other.What is the concentration of the Ag+ remaining in solution when CuCl begins to precipitate? (For AgCl, pKsp =9.74.and for CuCl, pKsp = 6.76.)

Accepted Answer

A) 1.57* 10-2 M 
B) 1.57 * 10-4 M 
C) 2.23 *10-2 M 
D) 2.23 -10-4 M 
E) 3.72* 10-3 M 
A) 1.57* 10-2 M 
B) 1.57 * 10-4 M 
C) 2.23 *10-2 M 
D) 2.23 -10-4 M 
E) 3.72* 10-3 M

Question 9

Ksp for silver sulfate is 1.2 * 10-5 at 25°C.What is the molar solubility of Ag2SO4 in 
A) pure water and 
B) 0.80 M sodium sulfate solution?

Accepted Answer

A) s = 1.4 *10<sup>-

Question 10

The solubility of PbBr2 is 0.427 g per 100.0 mL of solution at 25°C.Determine the value of the solubility product constant for this strong electrolyte.Lead(II) bromide does not react with water.

Accepted Answer

A) 5.4 * 10-4 
B) 2.7 * 10-4 
C) 1.6 * 10-6 
D) 3.1 *10-6 
E) 6.3* 10-6 
A) 5.4 * 10-4 
B) 2.7 * 10-4 
C) 1.6 * 10-6 
D) 3.1 *10-6 
E) 6.3* 10-6

Question 11

When NF3 reacts with BF3 to form F3NBF3,

Accepted Answer

A) a complex ion is formed. 
B) an ionic bond is formed. 
C) the bond is formed by sharing an electron from NF3 and an electron from BF3. 
D) a coordinate covalent bond is formed. 
E) BF3 donates an electron pair to NF3. 
A) a complex ion is formed. 
B) an ionic bond is formed. 
C) the bond is formed by sharing an electron from NF3 and an electron from BF3. 
D) a coordinate covalent bond is formed. 
E) BF3 donates an electron pair to NF3.

Question 12

A solution with a pH of 9.100 is prepared using aqueous ammonia and solid ammonium chloride.What is the ratio of [NH3] to [NH4+] in the solution? The Kb of ammonia is 1.76 * 10-5.

Accepted Answer

A) 0.850 to 1 
B) 1.02 to 1 
C) 0.984 to 1 
D) 1.41 to 1 
E) 0.715 to 1 
A) 0.850 to 1 
B) 1.02 to 1 
C) 0.984 to 1 
D) 1.41 to 1 
E) 0.715 to 1

Question 13

Stalactites-the long, icicle-like formations that hang from the ceilings of caves-are formed from recrystallizing minerals like calcite (calcium carbonate, CaCO3, 100.09/mol).The Ksp of calcium carbonate is 4.5 * 10-9.What is the minimum volume of dripping water saturated with calcium carbonate that would be required to form a small stalactite that had a mass of 1.000 kg?

Accepted Answer

A) 1.5*104 L 
B) 4.5 * 104 L 
C) 1.5 * 105 L 
D) 1.4* 106 L 
E) 4.5 * 109 L 
A) 1.5*104 L 
B) 4.5 * 104 L 
C) 1.5 * 105 L 
D) 1.4* 106 L 
E) 4.5 * 109 L

Question 14

Define the term Lewis acid and provide an example.

Accepted Answer

A Lewis acid is an electron-pa

Question 15

Stalactites-the long, icicle-like formations that hang from the ceilings of caves-are formed from recrystallizing minerals like calcite (calcium carbonate).The Ksp of calcium carbonate is 4.5 *10-9.What is the concentration of a saturated calcium carbonate solution?

Accepted Answer

A) 1.0 * 10-3 M 
B) 4.5 *10-9 M 
C) 6.7 * 10-5 M 
D) 2.3 * 10-9 M 
E) 4.5 * 10-5 M 
A) 1.0 * 10-3 M 
B) 4.5 *10-9 M 
C) 6.7 * 10-5 M 
D) 2.3 * 10-9 M 
E) 4.5 * 10-5 M

Question 16

What is the pH of a buffer solution in which [HA] = [A-]?

Accepted Answer

A) pH =1 
B) pH = Ka 
C) pH = pKa 
D) pH = pOH 
E) pH = 7.0 
A) pH =1 
B) pH = Ka 
C) pH = pKa 
D) pH = pOH 
E) pH = 7.0

Question 17

The solubility product for Ag2S is written as _______, where s is the molar solubility.

Accepted Answer

A) Ksp=s2 
B) Ksp =4S3 
C) Ksp = 4s2 
D) Ksp = 2S3 
E) Ksp = 2s2 
A) Ksp=s2 
B) Ksp =4S3 
C) Ksp = 4s2 
D) Ksp = 2S3 
E) Ksp = 2s2

Question 18

What is the molar solubility of PbF2 in a buffer solution in which the [H+] concentration is roughly constant at 0.080 M? (Ksp of PbF2 is 3.2 *10-8; Ka of HF =6.8 * 10-4.)

Accepted Answer

A) 1.1 * 10-4 
B) 3.2 *10- 
C) 7.4 * 10-3 
D) 8.4* 10-3 
E) 4.8 * 10-2 
A) 1.1 * 10-4 
B) 3.2 *10- 
C) 7.4 * 10-3 
D) 8.4* 10-3 
E) 4.8 * 10-2

Question 19

Which of the statements below about an acid-base buffer solution is/are true?
I.It can be prepared by combining a strong acid with a salt of its conjugate base.
II.It can be prepared by combining a weak acid with a salt of its conjugate base.
III.It can be prepared by combining a weak base with its conjugate acid.
IV.The pH of a buffer solution does not change when the solution is diluted.
V.A buffer solution resists changes in its pH when an acid or base is added to it.

Accepted Answer

A) I, II, and IV 
B) II, III, and V 
C) II, III, IV, and V 
D) I, II, IV, and V 
E) II, III, and IV 
A) I, II, and IV 
B) II, III, and V 
C) II, III, IV, and V 
D) I, II, IV, and V 
E) II, III, and IV

Question 20

Acid-base indicators need to have very intense colors so that a very low concentration is visible.Could there be a problem in using too much indicator?

Accepted Answer

A) No, the colors would just be darker. 
B) No, indicators are inert. 
C) Yes, more indicator requires more extreme pH values to change color. 
D) Yes, the indicator could affect the acid-base chemistry being measured. 
E) No, the colors would just be sharper. 
A) No, the colors would just be darker. 
B) No, indicators are inert. 
C) Yes, more indicator requires more extreme pH values to change color. 
D) Yes, the indicator could affect the acid-base chemistry being measured. 
E) No, the colors would just be sharper.

What would happen to the Ag⁺ and Cl^- concentrations if NaCl(s) was added to a saturated solution of AgCl in water?

As the pH decreases, the solubility of _______ increases.

How many moles of sodium acetate must be added to 500.0 mL of 0.250 M acetic acid solution to produce a solution with a pH of 4.94? (The pK_a of acetic acid is 4.74.)

K_sp for lead iodide is 8.5 *10^-9 at 25°C.Will PbI₂ precipitate if 250.0 mL of 0.0480 M NaI solution is added to 375.0 mL of 0.0388 M (PbNO₃)₂ solution?

Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl₂, 95.21 g/mol, K_sp = 740).How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

Consider the following aqueous equilibrium for a formic acid solution, HCOOH(aq) ⇄ H⁺(aq) + HCOO^-(aq).Suppose solid sodium formate, NaHCOO, is added to the solution.Which of the following statements regarding the resulting solution is NOT correct? Ignore any volume changes.

K_sp for silver sulfate is 1.2 * 10^-5 at 25°C.What is the molar solubility of Ag₂SO₄ in A) pure water and B) 0.80 M sodium sulfate solution?

The solubility of PbBr₂ is 0.427 g per 100.0 mL of solution at 25°C.Determine the value of the solubility product constant for this strong electrolyte.Lead(II) bromide does not react with water.

When NF₃ reacts with BF₃ to form F₃NBF₃,

A solution with a pH of 9.100 is prepared using aqueous ammonia and solid ammonium chloride.What is the ratio of [NH₃] to [NH₄⁺] in the solution? The K_b of ammonia is 1.76 * 10^-5.

Define the term Lewis acid and provide an example.

Stalactites-the long, icicle-like formations that hang from the ceilings of caves-are formed from recrystallizing minerals like calcite (calcium carbonate).The K_sp of calcium carbonate is 4.5 *10^-9.What is the concentration of a saturated calcium carbonate solution?

What is the pH of a buffer solution in which [HA] = [A^-]?

The solubility product for Ag₂S is written as _______, where s is the molar solubility.

What is the molar solubility of PbF₂ in a buffer solution in which the [H⁺] concentration is roughly constant at 0.080 M? (K_sp of PbF₂ is 3.2 10^-8; K_a of HF =6.8 10^-4.)

Acid-base indicators need to have very intense colors so that a very low concentration is visible.Could there be a problem in using too much indicator?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

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Exam 16: Additional Aqueous Equilibria Chemistry and the Oceans

What would happen to the Ag+ and Cl- concentrations if NaCl(s) was added to a saturated solution of AgCl in water?

As the pH decreases, the solubility of _______ increases.

How many moles of sodium acetate must be added to 500.0 mL of 0.250 M acetic acid solution to produce a solution with a pH of 4.94? (The pKa of acetic acid is 4.74.)

Ksp for lead iodide is 8.5 *10-9 at 25°C.Will PbI2 precipitate if 250.0 mL of 0.0480 M NaI solution is added to 375.0 mL of 0.0388 M (PbNO3)2 solution?

Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl2, 95.21 g/mol, Ksp = 740).How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

Consider the following aqueous equilibrium for a formic acid solution, HCOOH(aq) ⇄ H+(aq) + HCOO-(aq).Suppose solid sodium formate, NaHCOO, is added to the solution.Which of the following statements regarding the resulting solution is NOT correct? Ignore any volume changes.

Ksp for silver sulfate is 1.2 * 10-5 at 25°C.What is the molar solubility of Ag2SO4 in A) pure water and B) 0.80 M sodium sulfate solution?

The solubility of PbBr2 is 0.427 g per 100.0 mL of solution at 25°C.Determine the value of the solubility product constant for this strong electrolyte.Lead(II) bromide does not react with water.

When NF3 reacts with BF3 to form F3NBF3,

A solution with a pH of 9.100 is prepared using aqueous ammonia and solid ammonium chloride.What is the ratio of [NH3] to [NH4+] in the solution? The Kb of ammonia is 1.76 * 10-5.

Define the term Lewis acid and provide an example.

Stalactites-the long, icicle-like formations that hang from the ceilings of caves-are formed from recrystallizing minerals like calcite (calcium carbonate).The Ksp of calcium carbonate is 4.5 *10-9.What is the concentration of a saturated calcium carbonate solution?

What is the pH of a buffer solution in which [HA] = [A-]?

The solubility product for Ag2S is written as _______, where s is the molar solubility.

What is the molar solubility of PbF2 in a buffer solution in which the [H+] concentration is roughly constant at 0.080 M? (Ksp of PbF2 is 3.2 *10-8; Ka of HF =6.8 * 10-4.)

Acid-base indicators need to have very intense colors so that a very low concentration is visible.Could there be a problem in using too much indicator?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

What would happen to the Ag⁺ and Cl^- concentrations if NaCl(s) was added to a saturated solution of AgCl in water?

How many moles of sodium acetate must be added to 500.0 mL of 0.250 M acetic acid solution to produce a solution with a pH of 4.94? (The pK_a of acetic acid is 4.74.)

K_sp for lead iodide is 8.5 *10^-9 at 25°C.Will PbI₂ precipitate if 250.0 mL of 0.0480 M NaI solution is added to 375.0 mL of 0.0388 M (PbNO₃)₂ solution?

Purveyors of salts from the Dead Sea advertise that it is healthy to bathe in a saturated solution of magnesium chloride (MgCl₂, 95.21 g/mol, K_sp = 740).How much magnesium chloride would you have to purchase to make up 10.0 L of bath water saturated with magnesium chloride?

Consider the following aqueous equilibrium for a formic acid solution, HCOOH(aq) ⇄ H⁺(aq) + HCOO^-(aq).Suppose solid sodium formate, NaHCOO, is added to the solution.Which of the following statements regarding the resulting solution is NOT correct? Ignore any volume changes.

K_sp for silver sulfate is 1.2 * 10^-5 at 25°C.What is the molar solubility of Ag₂SO₄ in A) pure water and B) 0.80 M sodium sulfate solution?

The solubility of PbBr₂ is 0.427 g per 100.0 mL of solution at 25°C.Determine the value of the solubility product constant for this strong electrolyte.Lead(II) bromide does not react with water.

When NF₃ reacts with BF₃ to form F₃NBF₃,

A solution with a pH of 9.100 is prepared using aqueous ammonia and solid ammonium chloride.What is the ratio of [NH₃] to [NH₄⁺] in the solution? The K_b of ammonia is 1.76 * 10^-5.

Stalactites-the long, icicle-like formations that hang from the ceilings of caves-are formed from recrystallizing minerals like calcite (calcium carbonate).The K_sp of calcium carbonate is 4.5 *10^-9.What is the concentration of a saturated calcium carbonate solution?

What is the pH of a buffer solution in which [HA] = [A^-]?

The solubility product for Ag₂S is written as _______, where s is the molar solubility.

What is the molar solubility of PbF₂ in a buffer solution in which the [H⁺] concentration is roughly constant at 0.080 M? (K_sp of PbF₂ is 3.2 10^-8; K_a of HF =6.8 10^-4.)