Question 1

The most suitable acid-base indicator for a titration of acetic acid with NaOH has __________

Accepted Answer

A)  a pKin = pKa of the acid. 
B)  a pKin = pKb of the base. 
C)  pKin = pH of a sodium acetate solution. 
D)  pKin = pH of an acetic acid solution. 
E)  pKin = 7.0 
A)  a pKin = pKa of the acid. 
B)  a pKin = pKb of the base. 
C)  pKin = pH of a sodium acetate solution. 
D)  pKin = pH of an acetic acid solution. 
E)  pKin = 7.0

Question 2

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pKa values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has these acids in order of decreasing acid strength?

Accepted Answer

A)  LA > OA > MA 
B)  LA > MA > OA 
C)  OA > MA > LA 
D)  OA > LA > MA 
E)  MA > LA > OA 
A)  LA > OA > MA 
B)  LA > MA > OA 
C)  OA > MA > LA 
D)  OA > LA > MA 
E)  MA > LA > OA

Question 3

In the Brønsted-Lowry definition of acids and bases, an acid __________

Accepted Answer

A)  is a proton donor. 
B)  is a proton acceptor. 
C)  forms stable hydrogen bonds. 
D)  breaks stable hydrogen bonds. 
E)  corrodes metals. 
A)  is a proton donor. 
B)  is a proton acceptor. 
C)  forms stable hydrogen bonds. 
D)  breaks stable hydrogen bonds. 
E)  corrodes metals.

Question 4

Which one of the following statements is not correct?

Accepted Answer

A)  HIO is a stronger acid than HClO. 
B)  HClO is a stronger acid than HBrO. 
C)  HClO3 is a stronger acid than HClO2. 
D)  HPO42- is a weaker acid than H2PO4-. 
E)  H2SO4 is a stronger acid than H2SO3. 
A)  HIO is a stronger acid than HClO. 
B)  HClO is a stronger acid than HBrO. 
C)  HClO3 is a stronger acid than HClO2. 
D)  HPO42- is a weaker acid than H2PO4-. 
E)  H2SO4 is a stronger acid than H2SO3.

Question 5

What is the actual concentration of molecular NH3 in a 0.200 M solution of ammonia? The Kb value for ammonia is 1.80 F1F1F1S1F1F1F10 10-5.

Accepted Answer

A)  0.200 M 
B)  0.198 M 
C)  1.80 F1F1F1S1F1F1F10 10-5 M 
D)  1.90 F1F1F1S1F1F1F10 10-3 M 
E)  3.6 F1F1F1S1F1F1F10 10-6 M 
A)  0.200 M 
B)  0.198 M 
C)  1.80 F1F1F1S1F1F1F10 10-5 M 
D)  1.90 F1F1F1S1F1F1F10 10-3 M 
E)  3.6 F1F1F1S1F1F1F10 10-6 M

Question 6

The solubility product for an insoluble salt with the formula MX3 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 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 concentration of a saturated calcium carbonate solution?

Accepted Answer

A)  0.00104 M 
B)  4.5 F1F1F1S1F1F1F10 10-9 M 
C)  6.7 F1F1F1S1F1F1F10 10-5 M 
D)  2.25 F1F1F1S1F1F1F10 10-9 M 
E)  4.5 F1F1F1S1F1F1F10 10-5 M 
A)  0.00104 M 
B)  4.5 F1F1F1S1F1F1F10 10-9 M 
C)  6.7 F1F1F1S1F1F1F10 10-5 M 
D)  2.25 F1F1F1S1F1F1F10 10-9 M 
E)  4.5 F1F1F1S1F1F1F10 10-5 M

Question 8

Explain why some salts produce neutral solutions while others produce solutions that are acidic or basic, and give an example for each.

Accepted Answer

Acidic solutions are produced if the cat

Question 9

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 10

Which one of the following is not a conjugate acid-base pair?

Accepted Answer

A)  NH3 and NH2- 
B)  HNO3 and HNO2 
C)  HI and I- 
D)  H2PO4- and HPO42- 
E)  H2O and OH- 
A)  NH3 and NH2- 
B)  HNO3 and HNO2 
C)  HI and I- 
D)  H2PO4- and HPO42- 
E)  H2O and OH-

Question 11

What is the pH of a 0.25 M NH4Cl solution (Ka = 5.68 F1F1F1S1F1F1F10 10-10)?

Accepted Answer

Question 12

Phenylephrine (PE, see the structure below) is a nasal decongestant and is the active ingredient in Sudafed, which contains phenylephrine hydrochloride (PEHCl). This conjugate acid of phenylephrine (PEH+) has a pKa = 5.5. At a physiological pH of 7.4. what is the ratio of concentrations, [PE]/[PEH+]?

Accepted Answer

A)  6.7 
B)  0.01 
C)  0.14 
D)  79 
E)  21 
A)  6.7 
B)  0.01 
C)  0.14 
D)  79 
E)  21

Question 13

A solution of sulfuric acid (H2SO4, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the sulfuric acid?

Accepted Answer

A)  0.07048 M 
B)  0.1410 M 
C)  0.2819 M 
D)  0.0353 M 
E)  0.0533 M 
A)  0.07048 M 
B)  0.1410 M 
C)  0.2819 M 
D)  0.0353 M 
E)  0.0533 M

Question 14

Vitamin C is a monoprotic weak acid, which also is called ascorbic acid (C6H8O5, 176 g/mol). A vitamin C tablet weighing 0.75 g was dissolved in 50.0 mL of water and titrated with 0.250 M sodium hydroxide. It took 12.5 mL of the NaOH solution to reach the end point. What is the percentage of vitamin C in the tablet? Only the vitamin C reacted with the NaOH.

Accepted Answer

A)  98.7% 
B)  64.2% 
C)  87.7% 
D)  95.5% 
E)  73.3% 
A)  98.7% 
B)  64.2% 
C)  87.7% 
D)  95.5% 
E)  73.3%

Question 15

The solubility of PbBr2 is 0.427 g per 100 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 F1F1F1S1F1F1F10 10-4 
B)  2.7 F1F1F1S1F1F1F10 10-4 
C)  3.1 F1F1F1S1F1F1F10 10-6 
D)  1.6 F1F1F1S1F1F1F10 10-6 
E)  6.3 F1F1F1S1F1F1F10 10-6 
A)  5.4 F1F1F1S1F1F1F10 10-4 
B)  2.7 F1F1F1S1F1F1F10 10-4 
C)  3.1 F1F1F1S1F1F1F10 10-6 
D)  1.6 F1F1F1S1F1F1F10 10-6 
E)  6.3 F1F1F1S1F1F1F10 10-6

Question 16

The following titration curve is most likely to be associated with

Accepted Answer

A)  the titration of a strong acid with a strong base titrant. 
B)  the titration of a weak acid with a strong base titrant. 
C)  the titration of a strong base with a strong acid titrant. 
D)  the titration of a weak base with a strong acid titrant. 
A)  the titration of a strong acid with a strong base titrant. 
B)  the titration of a weak acid with a strong base titrant. 
C)  the titration of a strong base with a strong acid titrant. 
D)  the titration of a weak base with a strong acid titrant.

Question 17

Which one of the following is a strong acid?

Accepted Answer

A)  nitrous acid, HNO2 
B)  sulfurous acid, H2SO3 
C)  carbonic acid, H2CO3 
D)  hydrofluoric acid, HF 
E)  perchloric acid, HClO4 
A)  nitrous acid, HNO2 
B)  sulfurous acid, H2SO3 
C)  carbonic acid, H2CO3 
D)  hydrofluoric acid, HF 
E)  perchloric acid, HClO4

Question 18

Pure water at any temperature has __________

Accepted Answer

A)  a pH less than 7. 
B)  a pOH more than 7. 
C)  [H3O+] = [OH-]. 
D)  pH = 7. 
E)  no hydronium ions in it. 
A)  a pH less than 7. 
B)  a pOH more than 7. 
C)  [H3O+] = [OH-]. 
D)  pH = 7. 
E)  no hydronium ions in it.

Question 19

Which of the following would be the best choice for preparing a buffer with a pH = 8.0?

Accepted Answer

A)  a solution of formic acid and sodium formate, Ka = 1.8 F1F1F1S1F1F1F10 10-4 
B)  a solution of acetic acid and sodium acetate, Ka = 1.8 F1F1F1S1F1F1F10 10-5 
C)  a solution of hypochlorous acid and sodium hypochlorite, Ka = 3.5 F1F1F1S1F1F1F10 10-8 
D)  a solution of boric acid and sodium borate, Ka = 5.8 F1F1F1S1F1F1F10 10-10 
E)  All of these solutions would be equally good choices for making this buffer. 
A)  a solution of formic acid and sodium formate, Ka = 1.8 F1F1F1S1F1F1F10 10-4 
B)  a solution of acetic acid and sodium acetate, Ka = 1.8 F1F1F1S1F1F1F10 10-5 
C)  a solution of hypochlorous acid and sodium hypochlorite, Ka = 3.5 F1F1F1S1F1F1F10 10-8 
D)  a solution of boric acid and sodium borate, Ka = 5.8 F1F1F1S1F1F1F10 10-10 
E)  All of these solutions would be equally good choices for making this buffer.

Question 20

Which of the following compounds cannot be a Brønsted-Lowry base?

Accepted Answer

A)  OH- 
B)  H2O 
C)  NH3 
D)  NH4+ 
E)  SH- 
A)  OH- 
B)  H2O 
C)  NH3 
D)  NH4+ 
E)  SH-

The most suitable acid-base indicator for a titration of acetic acid with NaOH has __________

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pK_a values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has these acids in order of decreasing acid strength?

In the Brønsted-Lowry definition of acids and bases, an acid __________

Which one of the following statements is not correct?

What is the actual concentration of molecular NH₃ in a 0.200 M solution of ammonia? The K_b value for ammonia is 1.80  10^-⁵.

The solubility product for an insoluble salt with the formula MX₃ is written as __________, where s is the molar solubility.

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?

Explain why some salts produce neutral solutions while others produce solutions that are acidic or basic, and give an example for each.

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

Which one of the following is not a conjugate acid-base pair?

What is the pH of a 0.25 M NH₄Cl solution (K_a = 5.68  10^-¹⁰)?

A solution of sulfuric acid (H₂SO₄, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the sulfuric acid?

The solubility of PbBr₂ is 0.427 g per 100 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.

The following titration curve is most likely to be associated with

Which one of the following is a strong acid?

Pure water at any temperature has __________

Which of the following would be the best choice for preparing a buffer with a pH = 8.0?

Which of the following compounds cannot be a Brønsted-Lowry base?

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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Exam 17: Equilibrium in the Aqueous Phase

The most suitable acid-base indicator for a titration of acetic acid with NaOH has __________

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pKa values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has these acids in order of decreasing acid strength?

In the Brønsted-Lowry definition of acids and bases, an acid __________

Which one of the following statements is not correct?

What is the actual concentration of molecular NH3 in a 0.200 M solution of ammonia? The Kb value for ammonia is 1.80  10-5.

The solubility product for an insoluble salt with the formula MX3 is written as __________, where s is the molar solubility.

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?

Explain why some salts produce neutral solutions while others produce solutions that are acidic or basic, and give an example for each.

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

Which one of the following is not a conjugate acid-base pair?

What is the pH of a 0.25 M NH4Cl solution (Ka = 5.68  10-10)?

A solution of sulfuric acid (H2SO4, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the sulfuric acid?

The solubility of PbBr2 is 0.427 g per 100 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.

The following titration curve is most likely to be associated with

Which one of the following is a strong acid?

Pure water at any temperature has __________

Which of the following would be the best choice for preparing a buffer with a pH = 8.0?

Which of the following compounds cannot be a Brønsted-Lowry base?

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

Filters

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pK_a values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has these acids in order of decreasing acid strength?

What is the actual concentration of molecular NH₃ in a 0.200 M solution of ammonia? The K_b value for ammonia is 1.80  10^-⁵.

The solubility product for an insoluble salt with the formula MX₃ is written as __________, where s is the molar solubility.

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

What is the pH of a 0.25 M NH₄Cl solution (K_a = 5.68  10^-¹⁰)?

A solution of sulfuric acid (H₂SO₄, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the sulfuric acid?

The solubility of PbBr₂ is 0.427 g per 100 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.