Question 1

Which of the following is not a characteristic property of bases?

Accepted Answer

A) Taste bitter 
B) Turn litmus from pink to blue 
C) Neutralize acids 
D) React with carbonates to produce carbon dioxide gas 
E) Feel slippery 
A) Taste bitter 
B) Turn litmus from pink to blue 
C) Neutralize acids 
D) React with carbonates to produce carbon dioxide gas 
E) Feel slippery D

Question 2

The chloride ion, Cl−, is a typical Lewis acid.

Accepted Answer

A) True 
 B)False  False

Question 3

A solution is prepared by adding 0.10 mol of sodium sulfide, Na2S, 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 concentration of sodium ions and sulfide ions will be identical. 
E) The concentration of sulfide 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 concentration of sodium ions and sulfide ions will be identical. 
E) The concentration of sulfide ions will be greater than the concentration of sodium ions. A

Question 4

The ammonium ion, NH4+, is a weak acid.

Accepted Answer

A) True 
 B)False

Question 5

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2) = 1.5 × 10−10

Accepted Answer

A) 0.38 
B) 5.91 
C) 8.09 
D) 9.82 
E) 13.62 
A) 0.38 
B) 5.91 
C) 8.09 
D) 9.82 
E) 13.62

Question 6

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

Accepted Answer

A) H 2O/OH − 
B) H 2O 2/HO 2 − 
C) OH −/O 2− 
D) H 2PO 4 −/HPO 4 2− 
E) HCl/H + 
A) H 2O/OH − 
B) H 2O 2/HO 2 − 
C) OH −/O 2− 
D) H 2PO 4 −/HPO 4 2− 
E) HCl/H +

Question 7

The substance (CH3CH2)2NH is considered

Accepted Answer

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

Question 8

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

Accepted Answer

A) True 
 B)False

Question 9

A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

Accepted Answer

A) 0.64 
B) 0.94 
C) 1.13 
D) 2.16 
E) None of these choices are correct. 
A) 0.64 
B) 0.94 
C) 1.13 
D) 2.16 
E) None of these choices are correct.

Question 10

What is the pH of a 0.20 M HCl solution?

Accepted Answer

A) < 0 
B) 0.70 
C) 1.61 
D) 12.39 
E) 13.30 
A) < 0 
B) 0.70 
C) 1.61 
D) 12.39 
E) 13.30

Question 11

All weak acids have strong conjugate bases.

Accepted Answer

A) True 
 B)False

Question 12

Which, if any, of the following acids is strong?

Accepted Answer

A) Phosphoric 
B) Carbonic 
C) Acetic 
D) Water 
E) None of these choices are correct. 
A) Phosphoric 
B) Carbonic 
C) Acetic 
D) Water 
E) None of these choices are correct.

Question 13

Ammonium chloride is used as an electrolyte in dry cells. Which of the following statements about a 0.10 M solution of NH4Cl, is correct?

Accepted Answer

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

Question 14

Kw = 1.0 × 10−14, regardless of temperature.

Accepted Answer

A) True 
 B)False

Question 15

What is the [H3O+] for a solution at 25°C that has pOH = 5.640?

Accepted Answer

A) 2.34 × 10 −4  M 
B) 2.29 × 10 −6  M 
C) 4.37 × 10 −9  M 
D) 4.27 × 10 −11  M 
E) 8.360 M 
A) 2.34 × 10 −4  M 
B) 2.29 × 10 −6  M 
C) 4.37 × 10 −9  M 
D) 4.27 × 10 −11  M 
E) 8.360 M

Question 16

Phosphoric acid, H3PO4, is a triprotic acid, for which Ka1 = 7.2 × 10−3, Ka2 = 6.3 × 10−8 and Ka3 = 4.2 × 10−13. What is the value of Kb for the hydrogen phosphate anion, HPO4?

Accepted Answer

A) 6.3 × 10 −8 
B) 4.2 × 10 −13 
C) 1.4 × 10 −12 
D) 1.6 × 10 −7 
E) 2.4 × 10 −2 
A) 6.3 × 10 −8 
B) 4.2 × 10 −13 
C) 1.4 × 10 −12 
D) 1.6 × 10 −7 
E) 2.4 × 10 −2

Question 17

Which one of the following will give a solution with a pH > 7, but is not an Arrhenius base in the strict sense?

Accepted Answer

A) CH 3NH 2 
B) NaOH 
C) CO 2 
D) Ca(OH)2 
E) CH 4 
A) CH 3NH 2 
B) NaOH 
C) CO 2 
D) Ca(OH)2 
E) CH 4

Question 18

Which, if any, of the following is an example of the leveling effect?

Accepted Answer

A) The concentrations of H+ and OH- in pure water are equal. 
B) The number of strong acids equals the number of strong bases. 
C) The number of strong acids equals the number of weak acids. 
D) In water, no acid stronger than H 3O + can exist. 
E) None of these are examples of the leveling effect. 
A) The concentrations of H+ and OH- in pure water are equal. 
B) The number of strong acids equals the number of strong bases. 
C) The number of strong acids equals the number of weak acids. 
D) In water, no acid stronger than H 3O + can exist. 
E) None of these are examples of the leveling effect.

Question 19

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 20

All Lewis acids contain at least one proton.

Accepted Answer

A) True 
 B)False

Exam 18: Acid-Base Equilibria

Which of the following is not a characteristic property of bases?

The chloride ion, Cl−, is a typical Lewis acid.

A solution is prepared by adding 0.10 mol of sodium sulfide, Na2S, to 1.00 L of water. Which statement about the solution is correct?

The ammonium ion, NH4+, is a weak acid.

What is the pH of a 0.0100 M sodium benzoate solution? Kb (C7H5O2) = 1.5 × 10−10

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

The substance (CH3CH2)2NH is considered

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

A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

What is the pH of a 0.20 M HCl solution?

All weak acids have strong conjugate bases.

Which, if any, of the following acids is strong?

Ammonium chloride is used as an electrolyte in dry cells. Which of the following statements about a 0.10 M solution of NH4Cl, is correct?

Kw = 1.0 × 10−14, regardless of temperature.

What is the [H3O+] for a solution at 25°C that has pOH = 5.640?

Phosphoric acid, H3PO4, is a triprotic acid, for which Ka1 = 7.2 × 10−3, Ka2 = 6.3 × 10−8 and Ka3 = 4.2 × 10−13. What is the value of Kb for the hydrogen phosphate anion, HPO4?

Which one of the following will give a solution with a pH > 7, but is not an Arrhenius base in the strict sense?

Which, if any, of the following is an example of the leveling effect?

The substance HOBr is considered

All Lewis acids contain at least one proton.

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three 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

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 Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

The chloride ion, Cl⁻, is a typical Lewis acid.

A solution is prepared by adding 0.10 mol of sodium sulfide, Na₂S, to 1.00 L of water. Which statement about the solution is correct?

The ammonium ion, NH₄⁺, is a weak acid.

What is the pH of a 0.0100 M sodium benzoate solution? K_b (C₇H₅O₂) = 1.5 × 10⁻¹⁰

The substance (CH₃CH₂)₂NH is considered

Ammonium chloride is used as an electrolyte in dry cells. Which of the following statements about a 0.10 M solution of NH₄Cl, is correct?

Kw = 1.0 × 10⁻¹⁴, regardless of temperature.

What is the [H₃O⁺] for a solution at 25°C that has pOH = 5.640?

Phosphoric acid, H₃PO₄, is a triprotic acid, for which K_a1 = 7.2 × 10⁻³, K_a2 = 6.3 × 10⁻⁸ and K_a3 = 4.2 × 10⁻¹³. What is the value of K_b for the hydrogen phosphate anion, HPO₄?