Question 1

The substance HOBr is considered

Accepted Answer

A)  a weak Arrhenius acid. 
B)  a weak Arrhenius base. 
C)  a strong Arrhenius acid. 
D)  a strong Arrhenius base. 
E)  a neutral compound. 
A)  a weak Arrhenius acid. 
B)  a weak Arrhenius base. 
C)  a strong Arrhenius acid. 
D)  a strong Arrhenius base. 
E)  a neutral compound.

Question 2

Which of the following is the strongest base?

Accepted Answer

A)  CH3NH2 
B)  NaNO3 
C)  B(OH)3 
D)  Al(OH)3 
E)  LiOH 
A)  CH3NH2 
B)  NaNO3 
C)  B(OH)3 
D)  Al(OH)3 
E)  LiOH

Question 3

Define a base according to the Brønsted-Lowry theory. Write a balanced equation in support of this definition, in which the base is acting as a Brønsted-Lowry base but not as an Arrhenius base.

Accepted Answer

According to Brønsted and Lowr

Question 4

Which one of the following is a Lewis acid but not a Brønsted-Lowry acid?

Accepted Answer

A)  Fe3+ 
B)  H3O+ 
C)  HSO4- 
D)  NH3 
E)  H2O 
A)  Fe3+ 
B)  H3O+ 
C)  HSO4- 
D)  NH3 
E)  H2O

Question 5

If a strong acid such as HCl is diluted sufficiently with water, the pH will be higher than 7.

Accepted Answer

A) True 
 B)False

Question 6

Iodine trichloride, ICl3, will react with a chloride ion to form ICl4-. Which species, if any, acts as a Lewis acid this reaction?

Accepted Answer

A)  ICl4- 
B)  ICl 3 
C)  Cl- 
D)  the solvent 
E)  None of the species acts as a Lewis acid in this reaction. 
A)  ICl4- 
B)  ICl 3 
C)  Cl- 
D)  the solvent 
E)  None of the species acts as a Lewis acid in this reaction.

Question 7

What is the pOH of a 0.0250 M HI solution?

Accepted Answer

A)  0.944 
B)  1.602 
C)  12.398 
D)  13.056 
E)  none of the above 
A)  0.944 
B)  1.602 
C)  12.398 
D)  13.056 
E)  none of the above

Question 8

A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO3, to 1.00 L of water. Which statement about the solution is correct?

Accepted Answer

A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is weakly acidic. 
D)  The solution is strongly acidic. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made. 
A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is weakly acidic. 
D)  The solution is strongly acidic. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made.

Question 9

A solution is prepared by adding 0.10 mol of sodium fluoride, NaF, to 1.00 L of water. Which statement about the solution is correct?

Accepted Answer

A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is acidic. 
D)  The concentrations of fluoride ions and sodium ions will be identical. 
E)  The concentration of fluoride ions will be greater than the concentration of sodium ions. 
A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is acidic. 
D)  The concentrations of fluoride ions and sodium ions will be identical. 
E)  The concentration of fluoride ions will be greater than the concentration of sodium ions.

Question 10

What is the pH of a 0.00200 M HClO4 solution?

Accepted Answer

A)  0.995 
B)  1.378 
C)  2.699 
D)  6.215 
E)  none of the above 
A)  0.995 
B)  1.378 
C)  2.699 
D)  6.215 
E)  none of the above

Question 11

Hydrated metal ions in aqueous solution can act as Brønsted-Lowry acids.

Accepted Answer

A) True 
 B)False

Question 12

Which of the following is the strongest acid?

Accepted Answer

A)  CH3COOH 
B)  HF 
C)  H3PO4 
D)  H2SO3 
E)  H2SO4 
A)  CH3COOH 
B)  HF 
C)  H3PO4 
D)  H2SO3 
E)  H2SO4

Question 13

It is not possible to have a pH lying outside the range 0 to 14.

Accepted Answer

A) True 
 B)False

Question 14

A 0.050 M solution of the weak acid HA has [H3O+] = 3.77 × 10-4 M. What is the Ka for the acid?

Accepted Answer

A)  7.5 × 10-3 M 
B)  2.8 × 10-6 M 
C)  7.0 × 10-7 M 
D)  7.0 × 10-8 M 
E)  2.6 × 10-11 M 
A)  7.5 × 10-3 M 
B)  2.8 × 10-6 M 
C)  7.0 × 10-7 M 
D)  7.0 × 10-8 M 
E)  2.6 × 10-11 M

Question 15

Which of the following aqueous liquids will have the highest pH?

Accepted Answer

A)  0.1 M CH3COOH, pKa = 4.7 
B)  0.1 M CuCl2, pKa = 7.5 
C)  0.1 M H3C6H5O7, pKa = 3.1 
D)  0.1 M ZnCl2, pKa = 9.0 
E)  pure water 
A)  0.1 M CH3COOH, pKa = 4.7 
B)  0.1 M CuCl2, pKa = 7.5 
C)  0.1 M H3C6H5O7, pKa = 3.1 
D)  0.1 M ZnCl2, pKa = 9.0 
E)  pure water

Question 16

All strong acids have weak conjugate bases.

Accepted Answer

A) True 
 B)False

Question 17

Which of the following is the strongest acid?

Accepted Answer

A)  CH3COOH 
B)  HF 
C)  H3PO4 
D)  H2SO3 
E)  HI 
A)  CH3COOH 
B)  HF 
C)  H3PO4 
D)  H2SO3 
E)  HI

Question 18

What is the pH of a 0.010 M triethanolammonium chloride, (HOC2H2)3NHCl, solution? 
Kb, ((HOC2H2)3N) = 5.9 × 10-7

Accepted Answer

A)  2.75 
B)  4.89 
C)  9.11 
D)  11.25 
E)  none of the above 
A)  2.75 
B)  4.89 
C)  9.11 
D)  11.25 
E)  none of the above

Question 19

Arrhenius bases raise the hydroxide ion concentration when dissolved in water.

Accepted Answer

A) True 
 B)False

Question 20

A solution is prepared by adding 0.10 mol of potassium chloride, KCl, to 1.00 L of water. Which statement about the solution is correct?

Accepted Answer

A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is acidic. 
D)  One needs to know the temperature before any of the above predictions can be made. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made. 
A)  The solution is basic. 
B)  The solution is neutral. 
C)  The solution is acidic. 
D)  One needs to know the temperature before any of the above predictions can be made. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made.

Exam 18: Acid-Base Equilibria

The substance HOBr is considered

Which of the following is the strongest base?

Define a base according to the Brønsted-Lowry theory. Write a balanced equation in support of this definition, in which the base is acting as a Brønsted-Lowry base but not as an Arrhenius base.

Which one of the following is a Lewis acid but not a Brønsted-Lowry acid?

If a strong acid such as HCl is diluted sufficiently with water, the pH will be higher than 7.

Iodine trichloride, ICl3, will react with a chloride ion to form ICl4-. Which species, if any, acts as a Lewis acid this reaction?

What is the pOH of a 0.0250 M HI solution?

A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO3, to 1.00 L of water. Which statement about the solution is correct?

A solution is prepared by adding 0.10 mol of sodium fluoride, NaF, to 1.00 L of water. Which statement about the solution is correct?

What is the pH of a 0.00200 M HClO4 solution?

Hydrated metal ions in aqueous solution can act as Brønsted-Lowry acids.

Which of the following is the strongest acid?

It is not possible to have a pH lying outside the range 0 to 14.

A 0.050 M solution of the weak acid HA has [H3O+] = 3.77 × 10-4 M. What is the Ka for the acid?

Which of the following aqueous liquids will have the highest pH?

All strong acids have weak conjugate bases.

Which of the following is the strongest acid?

What is the pH of a 0.010 M triethanolammonium chloride, (HOC2H2)3NHCl, solution? Kb, ((HOC2H2)3N) = 5.9 × 10-7

Arrhenius bases raise the hydroxide ion concentration when dissolved in water.

A solution is prepared by adding 0.10 mol of potassium chloride, KCl, to 1.00 L of water. Which statement about the solution is correct?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Iodine trichloride, ICl₃, will react with a chloride ion to form ICl₄^-. Which species, if any, acts as a Lewis acid this reaction?

A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO₃, to 1.00 L of water. Which statement about the solution is correct?

What is the pH of a 0.00200 M HClO₄solution?

A 0.050 M solution of the weak acid HA has [H₃O⁺] = 3.77 × 10^-4 M. What is the K_afor the acid?

What is the pH of a 0.010 M triethanolammonium chloride, (HOC₂H₂)₃NHCl, solution? K_b, ((HOC₂H₂)₃N) = 5.9 × 10^-7