Question 1

Which statement does NOT correctly describe buffer capacity?

Accepted Answer

A)  Buffer capacity is determined only by the identity of the buffer. 
B)  The addition of amounts of acid or base exceeding the buffer capacity will change the pH of the solution. 
C)  The higher the concentration of weak acid and conjugate base in solution, the higher the buffer capacity. 
D)  The greatest amount of acid or base that a buffer can accept while maintaining pH is called the buffer capacity. 
E)  Once the buffer capacity is exceeded in cells, key functions of the body can be disrupted. 
A)  Buffer capacity is determined only by the identity of the buffer. 
B)  The addition of amounts of acid or base exceeding the buffer capacity will change the pH of the solution. 
C)  The higher the concentration of weak acid and conjugate base in solution, the higher the buffer capacity. 
D)  The greatest amount of acid or base that a buffer can accept while maintaining pH is called the buffer capacity. 
E)  Once the buffer capacity is exceeded in cells, key functions of the body can be disrupted.

Question 2

Which molecule is a base?

Accepted Answer

A)  molecule a 
B)  molecule b 
C)  molecule c 
D)  molecule d 
E)  molecule e 
A)  molecule a 
B)  molecule b 
C)  molecule c 
D)  molecule d 
E)  molecule e

Question 3

Which statement does NOT correctly describe pH?

Accepted Answer

A)  pH is a measure of acidity of a solution. 
B)  pH is a measure of hydronium concentration in a solution. 
C)  The higher the pH, the more acidic a solution. 
D)  A pH of 7 is a neutral solution. 
E)  pH = -log[H3O+]. 
A)  pH is a measure of acidity of a solution. 
B)  pH is a measure of hydronium concentration in a solution. 
C)  The higher the pH, the more acidic a solution. 
D)  A pH of 7 is a neutral solution. 
E)  pH = -log[H3O+].

Question 4

Which of the following statements about bases is FALSE?

Accepted Answer

A)  A base decreases the concentration of hydronium in solution. 
B)  An example of a base is Ca(OH)2. 
C)  A base increases the concentration of hydroxide in solution. 
D)  A base is a proton acceptor. 
E)  A base is always negatively charged. 
A)  A base decreases the concentration of hydronium in solution. 
B)  An example of a base is Ca(OH)2. 
C)  A base increases the concentration of hydroxide in solution. 
D)  A base is a proton acceptor. 
E)  A base is always negatively charged.

Question 5

Which of the following atomic diagrams best represents H+?

Accepted Answer

A)  figure a 
B)  figure b 
C)  figure c 
D)  figure d 
E)  figure e 
A)  figure a 
B)  figure b 
C)  figure c 
D)  figure d 
E)  figure e

Question 6

Which of the following is a buffer system?

Accepted Answer

A)  H2CO3 and HCO3- 
B)  NaCl and NaOH 
C)  HCl and NaOH 
D)  H2O and HCl 
E)  NaCl and NaNO3 
A)  H2CO3 and HCO3- 
B)  NaCl and NaOH 
C)  HCl and NaOH 
D)  H2O and HCl 
E)  NaCl and NaNO3

Question 7

What is the concentration of H3O+ and OH- in pure water at room temperature?

Accepted Answer

A)  1.0 × 10-14 M 
B)  1.0 × 10-7 M 
C)  1.0 M 
D)  1.0 × 107 M 
E)  1.0 × 1014 M 
A)  1.0 × 10-14 M 
B)  1.0 × 10-7 M 
C)  1.0 M 
D)  1.0 × 107 M 
E)  1.0 × 1014 M

Question 8

The neutralization reaction of potassium hydrogen carbonate (KHCO3)and HI produces what spectator ion(s)?

Accepted Answer

A)  CO32- 
B)  K+ and I- 
C)  HCO3- 
D)  H3O+ and OH- 
E)  H+ 
A)  CO32- 
B)  K+ and I- 
C)  HCO3- 
D)  H3O+ and OH- 
E)  H+

Question 9

The boxed species in the following reaction is

Accepted Answer

A)  a hydroxide. 
B)  a hydronium. 
C)  a proton. 
D)  the acid. 
E)  the conjugate base. 
A)  a hydroxide. 
B)  a hydronium. 
C)  a proton. 
D)  the acid. 
E)  the conjugate base.

Question 10

Which of the following compounds is a Brønsted-Lowry base but not an Arrhenius base?

Accepted Answer

A)  HCl 
B)  NaOH 
C)  NH3 
D)  Ca(OH)2 
E)  CH3COOH 
A)  HCl 
B)  NaOH 
C)  NH3 
D)  Ca(OH)2 
E)  CH3COOH

Question 11

Which of the following statements about acids is FALSE?

Accepted Answer

A)  An example of an acid is HBr. 
B)  An acid increases the concentration of hydroxide in solution. 
C)  An acid increases the concentration of protons in solution. 
D)  An acid increases the concentration of hydronium in solution. 
E)  An acid is a proton donor. 
A)  An example of an acid is HBr. 
B)  An acid increases the concentration of hydroxide in solution. 
C)  An acid increases the concentration of protons in solution. 
D)  An acid increases the concentration of hydronium in solution. 
E)  An acid is a proton donor.

Question 12

Which statement about neutralization reactions is FALSE?

Accepted Answer

A)  Neutralization reactions occur between an acid and a base. 
B)  Neutralization reactions are equilibrium reactions. 
C)  Neutralization reactions produce water. 
D)  Neutralization reactions sometimes produce carbon dioxide. 
E)  Neutralization reactions always go to completion. 
A)  Neutralization reactions occur between an acid and a base. 
B)  Neutralization reactions are equilibrium reactions. 
C)  Neutralization reactions produce water. 
D)  Neutralization reactions sometimes produce carbon dioxide. 
E)  Neutralization reactions always go to completion.

Question 13

What is the [H3O+] in a solution that has a [OH-] of 3.2 × 10-4 M?

Accepted Answer

A)  3.2 × 10-10 M 
B)  3.2 × 1010 M 
C)  3.1 × 10-11 M 
D)  3.1 × 1011 M 
E)  1.0 × 10-7 M 
A)  3.2 × 10-10 M 
B)  3.2 × 1010 M 
C)  3.1 × 10-11 M 
D)  3.1 × 1011 M 
E)  1.0 × 10-7 M

Question 14

The boxed species in the following reaction is

Accepted Answer

A)  a hydroxide. 
B)  a hydronium. 
C)  a proton. 
D)  the acid. 
E)  the conjugate base. 
A)  a hydroxide. 
B)  a hydronium. 
C)  a proton. 
D)  the acid. 
E)  the conjugate base.

Question 15

Which of the following statements does NOT describe a pH buffer?

Accepted Answer

A)  A common buffer is a solution of acetic acid and acetate. 
B)  A buffer is a weak acid and the acid's conjugate base in equal concentrations. 
C)  A buffer is a physical barrier that blocks the addition of acid or base to a solution. 
D)  A buffer is a solution that resists change of pH upon addition of small amounts of acid or base. 
E)  Phosphates and bicarbonate are buffering systems in the body. 
A)  A common buffer is a solution of acetic acid and acetate. 
B)  A buffer is a weak acid and the acid's conjugate base in equal concentrations. 
C)  A buffer is a physical barrier that blocks the addition of acid or base to a solution. 
D)  A buffer is a solution that resists change of pH upon addition of small amounts of acid or base. 
E)  Phosphates and bicarbonate are buffering systems in the body.

Question 16

Which statement BEST describe a neutralization reaction?

Accepted Answer

A)  An acid and base react to give a salt and sometimes water. 
B)  Two aqueous molecules react to give a liquid. 
C)  A positively charged ion reacts to give a neutral molecule. 
D)  An anion and a cation react to give a neutral molecule. 
E)  Two neutral molecules react to give a cation and an anion. 
A)  An acid and base react to give a salt and sometimes water. 
B)  Two aqueous molecules react to give a liquid. 
C)  A positively charged ion reacts to give a neutral molecule. 
D)  An anion and a cation react to give a neutral molecule. 
E)  Two neutral molecules react to give a cation and an anion.

Question 17

Which of the following types of molecules and ions is NOT a base?

Accepted Answer

A)  an anion 
B)  a cation 
C)  a neutral molecule containing a nonbonding pair of electrons 
D)  a tertiary nitrogen 
E)  All of these are bases. 
A)  an anion 
B)  a cation 
C)  a neutral molecule containing a nonbonding pair of electrons 
D)  a tertiary nitrogen 
E)  All of these are bases.

Question 18

What do all bases have in common?

Accepted Answer

A)  They contain an OH- group. 
B)  They contain a nitrogen. 
C)  They contain an oxygen. 
D)  They are salts. 
E)  They contain a nonbonding pair of electrons. 
A)  They contain an OH- group. 
B)  They contain a nitrogen. 
C)  They contain an oxygen. 
D)  They are salts. 
E)  They contain a nonbonding pair of electrons.

Question 19

If the concentration of hydronium ion in water is 1 × 10-6 M, the concentration of hydroxide ion is _____ and there is more _____ in the solution.

Accepted Answer

A)  1 × 10-8 M; hydroxide 
B)  1 × 10-8 M; hydronium 
C)  1 × 106 M; hydroxide 
D)  1 × 106 M; hydronium 
A)  1 × 10-8 M; hydroxide 
B)  1 × 10-8 M; hydronium 
C)  1 × 106 M; hydroxide 
D)  1 × 106 M; hydronium

Question 20

Generally, strong bases are hydroxide salts of

Accepted Answer

A)  transition metals. 
B)  the halogens. 
C)  alkali and alkaline earth metals. 
D)  the noble gases. 
E)  any element. 
A)  transition metals. 
B)  the halogens. 
C)  alkali and alkaline earth metals. 
D)  the noble gases. 
E)  any element.

Which statement does NOT correctly describe buffer capacity?

Which molecule is a base?

Which statement does NOT correctly describe pH?

Which of the following statements about bases is FALSE?

Which of the following atomic diagrams best represents H⁺?

Which of the following is a buffer system?

What is the concentration of H₃O⁺ and OH^- in pure water at room temperature?

The neutralization reaction of potassium hydrogen carbonate (KHCO₃)and HI produces what spectator ion(s)?

The boxed species in the following reaction is

Which of the following compounds is a Brønsted-Lowry base but not an Arrhenius base?

Which of the following statements about acids is FALSE?

Which statement about neutralization reactions is FALSE?

What is the [H₃O⁺] in a solution that has a [OH^-] of 3.2 × 10^-4 M?

The boxed species in the following reaction is

Which of the following statements does NOT describe a pH buffer?

Which statement BEST describe a neutralization reaction?

Which of the following types of molecules and ions is NOT a base?

What do all bases have in common?

If the concentration of hydronium ion in water is 1 × 10^-6 M, the concentration of hydroxide ion is _ and there is more _ in the solution.

Generally, strong bases are hydroxide salts of

Matter, Energy, and Measurement

Atomic Structure and Radioisotopes

Ionic and Covalent Compounds

Molecular Geometry, Polarity, and Intermolecular

Chemical Quantities and Introduction to Reactions

Chemical Reactions: Energy, Rates, and Equilibrium

Changes of State and Gas Laws

Mixtures, Solution Concentrations, and Diffusion

Introduction to Organic Chemistry:

Alcohols, Phenols, Thiols, Ethers, and Amines

The Carbonyl Containing Functional Groups

The Common Organic Reactions in Biochemistry

Carbohydrates: Structure and Function

Lipids: Structure and Function

Proteins: Structure and Function

Nucleotides and Nucleic Acids

Energy and Metabolism

Filters

Exam 9: Acids and Bases, Ph, and Buffers

Which statement does NOT correctly describe buffer capacity?

Which molecule is a base?

Which statement does NOT correctly describe pH?

Which of the following statements about bases is FALSE?

Which of the following atomic diagrams best represents H+?

Which of the following is a buffer system?

What is the concentration of H3O+ and OH- in pure water at room temperature?

The neutralization reaction of potassium hydrogen carbonate (KHCO3)and HI produces what spectator ion(s)?

The boxed species in the following reaction is

Which of the following compounds is a Brønsted-Lowry base but not an Arrhenius base?

Which of the following statements about acids is FALSE?

Which statement about neutralization reactions is FALSE?

What is the [H3O+] in a solution that has a [OH-] of 3.2 × 10-4 M?

The boxed species in the following reaction is

Which of the following statements does NOT describe a pH buffer?

Which statement BEST describe a neutralization reaction?

Which of the following types of molecules and ions is NOT a base?

What do all bases have in common?

If the concentration of hydronium ion in water is 1 × 10-6 M, the concentration of hydroxide ion is _____ and there is more _____ in the solution.

Generally, strong bases are hydroxide salts of

Matter, Energy, and Measurement

Atomic Structure and Radioisotopes

Ionic and Covalent Compounds

Molecular Geometry, Polarity, and Intermolecular

Chemical Quantities and Introduction to Reactions

Chemical Reactions: Energy, Rates, and Equilibrium

Changes of State and Gas Laws

Mixtures, Solution Concentrations, and Diffusion

Introduction to Organic Chemistry:

Alcohols, Phenols, Thiols, Ethers, and Amines

The Carbonyl Containing Functional Groups

The Common Organic Reactions in Biochemistry

Carbohydrates: Structure and Function

Lipids: Structure and Function

Proteins: Structure and Function

Nucleotides and Nucleic Acids

Energy and Metabolism

Filters

Which of the following atomic diagrams best represents H⁺?

What is the concentration of H₃O⁺ and OH^- in pure water at room temperature?

The neutralization reaction of potassium hydrogen carbonate (KHCO₃)and HI produces what spectator ion(s)?

What is the [H₃O⁺] in a solution that has a [OH^-] of 3.2 × 10^-4 M?

If the concentration of hydronium ion in water is 1 × 10^-6 M, the concentration of hydroxide ion is _ and there is more _ in the solution.