Question 1

Which of the following is the conjugate base of water?

Accepted Answer

A)  H3O+ 
B)  NaOH 
C)  OH− 
D)  O2− 
A)  H3O+ 
B)  NaOH 
C)  OH− 
D)  O2−

Question 2

Which of the following must be increased in order to decrease the pH of a buffer made using acetic acid and sodium acetate?

Accepted Answer

A)  the amount of water present 
B)  [C2H3O2−] 
C)  [HC2H3O2] 
D)  the ratio of [C2H3O2−]/[HC2H3O2] 
A)  the amount of water present 
B)  [C2H3O2−] 
C)  [HC2H3O2] 
D)  the ratio of [C2H3O2−]/[HC2H3O2]

Question 3

Which of the following can be observed when phenolphthalein is added to a sulfuric acid solution?

Accepted Answer

A)  The solution remains colorless. 
B)  The solution turns pink. 
C)  The solution turns blue. 
D)  The solution turns green. 
A)  The solution remains colorless. 
B)  The solution turns pink. 
C)  The solution turns blue. 
D)  The solution turns green.

Question 4

Which of the following pH values corresponds to a slightly acidic solution?

Accepted Answer

A)  2.8 
B)  6.8 
C)  7.2 
D)  11.2 
A)  2.8 
B)  6.8 
C)  7.2 
D)  11.2

Question 5

Examine the following image. Assume the solution in the beaker is a buffer solution.   What will be the pH of the resulting solution when 0.01 mol of NaOH is added to this solution?

Accepted Answer

A)  2.13 
B)  6.14 
C)  4.23 
D)  4.43 
A)  2.13 
B)  6.14 
C)  4.23 
D)  4.43

Question 6

Which of the following is characteristic of a buffer?

Accepted Answer

A)  The pH will go down significantly when OH− is added to a buffer. 
B)  The pH will go down very slightly when OH− is added to a buffer. 
C)  The pH will go up significantly when OH− is added to a buffer. 
D)  The pH will go up very slightly when OH− is added to a buffer. 
A)  The pH will go down significantly when OH− is added to a buffer. 
B)  The pH will go down very slightly when OH− is added to a buffer. 
C)  The pH will go up significantly when OH− is added to a buffer. 
D)  The pH will go up very slightly when OH− is added to a buffer.

Question 7

Why is inducing alkalosis just before a race advantageous to a sprinter?

Accepted Answer

A)  It increases the respiratory rate. 
B)  It strengthens the leg muscles. 
C)  The sprinter can neutralize more lactic acid. 
D)  None of these is true. 
A)  It increases the respiratory rate. 
B)  It strengthens the leg muscles. 
C)  The sprinter can neutralize more lactic acid. 
D)  None of these is true.

Question 8

Which of the following acids produces ions that play an important role in biochemistry?

Accepted Answer

A)  acetic 
B)  boric 
C)  nitric 
D)  phosphoric 
A)  acetic 
B)  boric 
C)  nitric 
D)  phosphoric

Question 9

Which of the following can be characterized as a strong electrolyte?

Accepted Answer

A)  0.001 M KOH 
B)  3.0 M NH3 
C)  both 0.001 M KOH and 3.0 M NH3 
D)  neither 0.001 M KOH or 3.0 M NH3 
A)  0.001 M KOH 
B)  3.0 M NH3 
C)  both 0.001 M KOH and 3.0 M NH3 
D)  neither 0.001 M KOH or 3.0 M NH3

Question 10

Which of the following is the correct set of products formed when an acid reacts with a metal hydroxide?

Accepted Answer

A)  salt and water 
B)  salt and carbon dioxide 
C)  salt and hydrogen 
D)  salt and carbon monoxide 
A)  salt and water 
B)  salt and carbon dioxide 
C)  salt and hydrogen 
D)  salt and carbon monoxide

Question 11

Which of the following is not an acid?

Accepted Answer

A)  H3O+ 
B)  H2CO3 
C)  H2PO4− 
D)  None, they are all acids. 
A)  H3O+ 
B)  H2CO3 
C)  H2PO4− 
D)  None, they are all acids.

Question 12

Which of the following can be characterized as a strong acid?

Accepted Answer

A)  H3BO3 
B)  HCl 
C)  both H3BO3 and HCI 
D)  neither H3BO3 or HCI 
A)  H3BO3 
B)  HCl 
C)  both H3BO3 and HCI 
D)  neither H3BO3 or HCI

Question 13

Examine the following image. Assume the solution in the beaker is a buffer solution.   What is the pOH of the solution in the beaker?

Accepted Answer

A)  9.67 
B)  14.00 
C)  2.13 × 10−10 
D)  4.68 × 10−5 
A)  9.67 
B)  14.00 
C)  2.13 × 10−10 
D)  4.68 × 10−5

Question 14

Which of the following buffers will have the highest pH?

Accepted Answer

A)  A solution containing 0.20 M HC2H3O2 and 0.20 M NaC2H3O2 will have the highest pH. 
B)  A solution containing 0.25 M HC2H3O2 and 0.15 M NaC2H3O2 will have the highest pH. 
C)  A solution containing 0.15 M HC2H3O2 and 0.25 M NaC2H3O2 will have the highest pH. 
D)  They all will have the same pH. 
A)  A solution containing 0.20 M HC2H3O2 and 0.20 M NaC2H3O2 will have the highest pH. 
B)  A solution containing 0.25 M HC2H3O2 and 0.15 M NaC2H3O2 will have the highest pH. 
C)  A solution containing 0.15 M HC2H3O2 and 0.25 M NaC2H3O2 will have the highest pH. 
D)  They all will have the same pH.

Question 15

Which of the following can be characterized as a strong base?

Accepted Answer

A)  Ba(OH)2 
B)  NH3 
C)  both Ba(OH)2 and NH3 
D)  neither Ba(OH)2 or NH3 
A)  Ba(OH)2 
B)  NH3 
C)  both Ba(OH)2 and NH3 
D)  neither Ba(OH)2 or NH3

Question 16

An acetic acid solution has a pH of 5.80. What is its [OH−]?

Accepted Answer

A)  1.6 × 10−20 M 
B)  6.3 × 10−9 M 
C)  1.6 × 10− 6 M 
D)  6.3 × 105 M 
A)  1.6 × 10−20 M 
B)  6.3 × 10−9 M 
C)  1.6 × 10− 6 M 
D)  6.3 × 105 M

Question 17

What is the name of the acid that dissociates to give the nitrite ion, NO2−?

Accepted Answer

A)  hydronitric acid 
B)  nitric acid 
C)  hyponitrous acid 
D)  nitrous acid 
A)  hydronitric acid 
B)  nitric acid 
C)  hyponitrous acid 
D)  nitrous acid

Question 18

Which of the following is formed when a strong acid reacts with methylamine, CH3NH2?

Accepted Answer

A)  CH3NH3 
B)  CH3NH3+ 
C)  (CH3)2NH2+ 
D)  none of these 
A)  CH3NH3 
B)  CH3NH3+ 
C)  (CH3)2NH2+ 
D)  none of these

Question 19

Which of the following is the correct name for the ion H3O+?

Accepted Answer

A)  heavy water 
B)  hydrogen ion 
C)  hydronium ion 
D)  all of these 
A)  heavy water 
B)  hydrogen ion 
C)  hydronium ion 
D)  all of these

Question 20

An ammonia solution has a pH of 8.30. What is its [H3O+]?

Accepted Answer

A)  5.0 × 10−23 M 
B)  2.0 × 10−6 M 
C)  5.0 × 10−9 M 
D)  2.0 × 108 M 
A)  5.0 × 10−23 M 
B)  2.0 × 10−6 M 
C)  5.0 × 10−9 M 
D)  2.0 × 108 M

Exam 8: Acids and Bases

Which of the following is the conjugate base of water?

Which of the following must be increased in order to decrease the pH of a buffer made using acetic acid and sodium acetate?

Which of the following can be observed when phenolphthalein is added to a sulfuric acid solution?

Which of the following pH values corresponds to a slightly acidic solution?

Examine the following image. Assume the solution in the beaker is a buffer solution. What will be the pH of the resulting solution when 0.01 mol of NaOH is added to this solution?

Which of the following is characteristic of a buffer?

Why is inducing alkalosis just before a race advantageous to a sprinter?

Which of the following acids produces ions that play an important role in biochemistry?

Which of the following can be characterized as a strong electrolyte?

Which of the following is the correct set of products formed when an acid reacts with a metal hydroxide?

Which of the following is not an acid?

Which of the following can be characterized as a strong acid?

Examine the following image. Assume the solution in the beaker is a buffer solution. What is the pOH of the solution in the beaker?

Which of the following buffers will have the highest pH?

Which of the following can be characterized as a strong base?

An acetic acid solution has a pH of 5.80. What is its [OH−]?

What is the name of the acid that dissociates to give the nitrite ion, NO2−?

Which of the following is formed when a strong acid reacts with methylamine, CH3NH2?

Which of the following is the correct name for the ion H3O+?

An ammonia solution has a pH of 8.30. What is its [H3O+]?

Matter, Energy, and Measurement

Atoms

Chemical Bonds

Chemical Reactions

Gases, Liquids, and Solids

Solutions and Colloids

Reaction Rates and Chemical Equilibrium

Nuclear Chemistry

Organic Chemistry

Alkanes

Alkenes, Alkynes, and Aromatic Compounds

Alcohols, Ethers, and Thiols

Chirality: the Handedness of Molecules

Amines

Aldehydes and Ketones

Carboxylic Acids

Carboxylic Anhydrides, Esters, and Amides

Carbohydrates

Lipids

Proteins

Enzymes

Chemical Communications: Neurotransmitters and Hormones

Nucleotides, Nucleic Acids, and Heredity

Gene Expression and Protein Synthesis

Bioenergetics: How the Body Converts Food to Energy

Specific Catabolic Pathways: Carbohydrate, Lipid, and Protein Metabolism

Biosynthetic Pathways

Nutrition

Immunochemistry

Body Fluids

Filters

An acetic acid solution has a pH of 5.80. What is its [OH⁻]?

What is the name of the acid that dissociates to give the nitrite ion, NO₂⁻?

Which of the following is formed when a strong acid reacts with methylamine, CH₃NH₂?

Which of the following is the correct name for the ion H₃O⁺?

An ammonia solution has a pH of 8.30. What is its [H₃O⁺]?