Question 1

When sodium chloride is added to a saturated solution of lead(II) chloride, some of the lead(II) chloride precipitates. This phenomenon is called __________

Accepted Answer

A)  the common ion effect. 
B)  selective precipitation. 
C)  supersaturation. 
D)  a solubility anomaly. 
E)  deionization. 
A)  the common ion effect. 
B)  selective precipitation. 
C)  supersaturation. 
D)  a solubility anomaly. 
E)  deionization.

Question 2

Which one of the following would make the best buffer? (Ac = acetate)

Accepted Answer

A)  a solution of hydrochloric acid and sodium chloride, HCl and NaCl 
B)  a solution of acetic acid and ammonia, NaAc and NH3 
C)  a solution of acetic acid and ammonium chloride, HAc and NH4Cl 
D)  a solution of sodium acetate and ammonium chloride, NaAc and NH4Cl 
E)  a solution of ammonia and ammonium chloride, NH3 and NH4Cl 
A)  a solution of hydrochloric acid and sodium chloride, HCl and NaCl 
B)  a solution of acetic acid and ammonia, NaAc and NH3 
C)  a solution of acetic acid and ammonium chloride, HAc and NH4Cl 
D)  a solution of sodium acetate and ammonium chloride, NaAc and NH4Cl 
E)  a solution of ammonia and ammonium chloride, NH3 and NH4Cl

Question 3

The concentration of acetic acid (pKa = 4.75) in vinegar is about 1.0 M. With this information, what do you predict the pH of vinegar to be?

Accepted Answer

A)  4.75 
B)  2.4 
C)  4.0 F1F1F1S1F1F1F10 10-3 
D)  7.0 
E)  5.35 
A)  4.75 
B)  2.4 
C)  4.0 F1F1F1S1F1F1F10 10-3 
D)  7.0 
E)  5.35

Question 4

Sometimes liquid ammonia, NH3, is used as a solvent rather than water. Which expression defines the ammonia autoionization counterpart of Kw?

Accepted Answer

A)  [H3O+][OH-] 
B)  [NH3][NH4+] 
C)  [NH2-][NH4+] 
D)  [H3O+][NH2-] 
E)  [NH4+][OH-] 
A)  [H3O+][OH-] 
B)  [NH3][NH4+] 
C)  [NH2-][NH4+] 
D)  [H3O+][NH2-] 
E)  [NH4+][OH-]

Question 5

The solubility product for an insoluble salt with the formula M3X is written as __________, where s is the molar solubility.

Accepted Answer

A)  Ksp = s2 
B)  Ksp = 4s3 
C)  Ksp = 27s4 
D)  Ksp = 3s3 
E)  Ksp = 3s4 
A)  Ksp = s2 
B)  Ksp = 4s3 
C)  Ksp = 27s4 
D)  Ksp = 3s3 
E)  Ksp = 3s4

Question 6

As the pH decreases, the solubility of __________ would increase.

Accepted Answer

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

Question 7

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 F1F1F1S1F1F1F10 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)  1.4 F1F1F1S1F1F1F10 106 L 
B)  1.5 F1F1F1S1F1F1F10 105 L 
C)  4.5 F1F1F1S1F1F1F10 109 L 
D)  4.5 F1F1F1S1F1F1F10 104 L 
E)  1.5 F1F1F1S1F1F1F10 104 L 
A)  1.4 F1F1F1S1F1F1F10 106 L 
B)  1.5 F1F1F1S1F1F1F10 105 L 
C)  4.5 F1F1F1S1F1F1F10 109 L 
D)  4.5 F1F1F1S1F1F1F10 104 L 
E)  1.5 F1F1F1S1F1F1F10 104 L

Question 8

Which one of the following salts does not produce a basic solution when dissolved in water?

Accepted Answer

A)  Na2S 
B)  NaBr 
C)  NaClO2 
D)  NaNO2 
E)  Na2CO3 
A)  Na2S 
B)  NaBr 
C)  NaClO2 
D)  NaNO2 
E)  Na2CO3

Question 9

A 0.500 g sample of an unknown substance was titrated with a 0.1 M HCl solution. Another 0.500 g sample of it was titrated with a 0.1 M NaOH solution. The resulting titration curves are illustrated here. Given the following possibilities, what is the sample?

Accepted Answer

A)  Na2CO3 
B)  NaHCO3 
C)  H2CO3 
D)  CO2 
E)  There is no way to tell. 
A)  Na2CO3 
B)  NaHCO3 
C)  H2CO3 
D)  CO2 
E)  There is no way to tell.

Question 10

Halfway to the equivalence point in a titration curve of a weak acid with a strong base, __________

Accepted Answer

A)  nothing is happening yet. 
B)  the pH = pKa of the weak acid. 
C)  pH = 3.5 exactly. 
D)  pH = pKa of the indicator. 
E)  the pH has not yet changed. 
A)  nothing is happening yet. 
B)  the pH = pKa of the weak acid. 
C)  pH = 3.5 exactly. 
D)  pH = pKa of the indicator. 
E)  the pH has not yet changed.

Question 11

What is the pH of a buffer solution where [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 12

The solubility product for an insoluble salt with the formula MX2 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 13

A 0.100 M solution of a monoprotic weak acid has a pH of 3.00. What is the pKa of this acid?

Accepted Answer

A)  5.00 
B)  0.999 
C)  3.00 
D)  9.99 
E)  6.00 
A)  5.00 
B)  0.999 
C)  3.00 
D)  9.99 
E)  6.00

Question 14

Bert and Ernie were determining the pH of their goldfish's water. Bert's pH meter was in the fix-it shop, so Ernie used his pOH meter instead. Ernie insists that he can use the reading to calculate the pH by simple addition or subtraction that he learned in second grade, but Bert (showing off as usual) claims that the calculation involves finding an antilogarithm, dividing, and then finding a logarithm. This would make use of all the math he learned in third grade. Who is right?

Accepted Answer

A)  Ernie 
B)  Bert 
C)  both 
D)  neither 
A)  Ernie 
B)  Bert 
C)  both 
D)  neither

Question 15

The pH of an aqueous sodium fluoride (NaF) solution is __________ because __________

Accepted Answer

A)  7; sodium fluoride is a simple salt. 
B)  above 7; fluoride is a weak base. 
C)  below 7; fluoride reacts with water to make hydrofluoric acid. 
D)  about 7; fluoride is a weak base, but produces hydrofluoric acid, and these two neutralize one another. 
E)  0; sodium fluoride is a salt not an acid or a base. 
A)  7; sodium fluoride is a simple salt. 
B)  above 7; fluoride is a weak base. 
C)  below 7; fluoride reacts with water to make hydrofluoric acid. 
D)  about 7; fluoride is a weak base, but produces hydrofluoric acid, and these two neutralize one another. 
E)  0; sodium fluoride is a salt not an acid or a base.

Question 16

Derive the Henderson-Hasselbalch equation from the acid ionization constant expression.

Accepted Answer

The answer of Derive the Henderson-Hasselbalch equation from the acid...

Question 17

Which one of the following salts forms aqueous solutions with pH = 7?

Accepted Answer

A)  Na2S 
B)  NaBr 
C)  NaClO2 
D)  NaNO2 
E)  Na2CO3 
A)  Na2S 
B)  NaBr 
C)  NaClO2 
D)  NaNO2 
E)  Na2CO3

Question 18

A phosphate buffer solution (25.00 mL sample) used for a growth medium was titrated with 0.1000 M hydrochloric acid. The components of the buffer were sodium monohydrogenphosphate and sodium dihydrogenphosphate. The first endpoint occurred at a volume of 10.32 mL, and the second occurred after an additional 18.62 mL was added, for a total volume of 28.94 mL. What was the total concentration of phosphate (in any form) in the buffer?

Accepted Answer

A)  0.03992 M 
B)  0.1198 M 
C)  0.04243 M 
D)  0.07448 M 
E)  0.08382 M 
A)  0.03992 M 
B)  0.1198 M 
C)  0.04243 M 
D)  0.07448 M 
E)  0.08382 M

Question 19

In the following reaction in aqueous solution, the acid reactant is __________, and its conjugate base product is __________. CH3NH2 + HSO4-   CH3NH3+ + SO42-

Accepted Answer

A)  CH3NH2; CH3NH3+ 
B)  CH3NH2; SO42- 
C)  HSO4-; CH3NH3+ 
D)  HSO4-; SO42- 
E)  HSO4-; H3O+ 
A)  CH3NH2; CH3NH3+ 
B)  CH3NH2; SO42- 
C)  HSO4-; CH3NH3+ 
D)  HSO4-; SO42- 
E)  HSO4-; H3O+

Question 20

The solubility product for an insoluble salt with the formula M2X 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

When sodium chloride is added to a saturated solution of lead(II) chloride, some of the lead(II) chloride precipitates. This phenomenon is called __________

Which one of the following would make the best buffer? (Ac = acetate)

The concentration of acetic acid (pK_a = 4.75) in vinegar is about 1.0 M. With this information, what do you predict the pH of vinegar to be?

Sometimes liquid ammonia, NH₃, is used as a solvent rather than water. Which expression defines the ammonia autoionization counterpart of K_w?

The solubility product for an insoluble salt with the formula M₃X is written as __________, where s is the molar solubility.

As the pH decreases, the solubility of __________ would increase.

Which one of the following salts does not produce a basic solution when dissolved in water?

A 0.500 g sample of an unknown substance was titrated with a 0.1 M HCl solution. Another 0.500 g sample of it was titrated with a 0.1 M NaOH solution. The resulting titration curves are illustrated here. Given the following possibilities, what is the sample?

Halfway to the equivalence point in a titration curve of a weak acid with a strong base, __________

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

The solubility product for an insoluble salt with the formula MX₂ is written as __________, where s is the molar solubility.

A 0.100 M solution of a monoprotic weak acid has a pH of 3.00. What is the pK_a of this acid?

The pH of an aqueous sodium fluoride (NaF) solution is because

Derive the Henderson-Hasselbalch equation from the acid ionization constant expression.

Which one of the following salts forms aqueous solutions with pH = 7?

In the following reaction in aqueous solution, the acid reactant is , and its conjugate base product is . CH₃NH₂ + HSO₄^- CH₃NH₃⁺ + SO₄²^-

The solubility product for an insoluble salt with the formula M₂X is written as __________, where s is the molar solubility.

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Exam 17: Equilibrium in the Aqueous Phase

When sodium chloride is added to a saturated solution of lead(II) chloride, some of the lead(II) chloride precipitates. This phenomenon is called __________

Which one of the following would make the best buffer? (Ac = acetate)

The concentration of acetic acid (pKa = 4.75) in vinegar is about 1.0 M. With this information, what do you predict the pH of vinegar to be?

Sometimes liquid ammonia, NH3, is used as a solvent rather than water. Which expression defines the ammonia autoionization counterpart of Kw?

The solubility product for an insoluble salt with the formula M3X is written as __________, where s is the molar solubility.

As the pH decreases, the solubility of __________ would increase.

Which one of the following salts does not produce a basic solution when dissolved in water?

A 0.500 g sample of an unknown substance was titrated with a 0.1 M HCl solution. Another 0.500 g sample of it was titrated with a 0.1 M NaOH solution. The resulting titration curves are illustrated here. Given the following possibilities, what is the sample?

Halfway to the equivalence point in a titration curve of a weak acid with a strong base, __________

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

The solubility product for an insoluble salt with the formula MX2 is written as __________, where s is the molar solubility.

A 0.100 M solution of a monoprotic weak acid has a pH of 3.00. What is the pKa of this acid?

The pH of an aqueous sodium fluoride (NaF) solution is __________ because __________

Derive the Henderson-Hasselbalch equation from the acid ionization constant expression.

Which one of the following salts forms aqueous solutions with pH = 7?

In the following reaction in aqueous solution, the acid reactant is __________, and its conjugate base product is __________. CH3NH2 + HSO4- CH3NH3+ + SO42-

The solubility product for an insoluble salt with the formula M2X is written as __________, where s is the molar solubility.

Matter, Energy, and the Origins of the Universe

Atoms, Ions, and Compounds

Chemical Reactions and Earths Composition

Solution Chemistry and the Hydrosphere

Thermochemistry

Properties of Gases: the Air We Breathe

Electrons in Atoms and Periodic Properties

Chemical Bonding and Climate Change

Molecular Geometry and Bonding Theories

Forces Between Ions and Molecules

Solutions and Their Colligative Properties

The Chemistry of Solids

Organic Chemistry: Fuels, Pharmaceuticals, and Materials

Thermodynamics: Spontaneous Processes, Entropy, and Free Energy

Chemical Kinetics

Chemical Equilibrium

The Colorful Chemistry of Metals

Electrochemistry and the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry

Life and the Periodic Table

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The concentration of acetic acid (pK_a = 4.75) in vinegar is about 1.0 M. With this information, what do you predict the pH of vinegar to be?

Sometimes liquid ammonia, NH₃, is used as a solvent rather than water. Which expression defines the ammonia autoionization counterpart of K_w?

The solubility product for an insoluble salt with the formula M₃X is written as __________, where s is the molar solubility.

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

The solubility product for an insoluble salt with the formula MX₂ is written as __________, where s is the molar solubility.

A 0.100 M solution of a monoprotic weak acid has a pH of 3.00. What is the pK_a of this acid?

The pH of an aqueous sodium fluoride (NaF) solution is because

In the following reaction in aqueous solution, the acid reactant is , and its conjugate base product is . CH₃NH₂ + HSO₄^- CH₃NH₃⁺ + SO₄²^-

The solubility product for an insoluble salt with the formula M₂X is written as __________, where s is the molar solubility.