Question 1

For the following compound, predict whether the solution is acidic, basic or neutral and why: NH3.

Accepted Answer

A)  acidic because NH3 is a strong acid 
B)  basic because NH3 is a weak base 
C)  neutral because there is no hydrolysis 
D)  basic because NH3 is the salt of a weak acid 
E)  acidic because NH3 is the salt of a weak base 
A)  acidic because NH3 is a strong acid 
B)  basic because NH3 is a weak base 
C)  neutral because there is no hydrolysis 
D)  basic because NH3 is the salt of a weak acid 
E)  acidic because NH3 is the salt of a weak base

Question 2

Which indication of relative acid strengths is INCORRECT?

Accepted Answer

A)  HCl > HF 
B)  HClO2 > HClO 
C)  H2SO4 > H2SO3 
D)  H2SO3 > HNO3 
E)  CH3CO2H > CH3CH2OH 
A)  HCl > HF 
B)  HClO2 > HClO 
C)  H2SO4 > H2SO3 
D)  H2SO3 > HNO3 
E)  CH3CO2H > CH3CH2OH

Question 3

What is the pH of a 0.361 M solution of pyridinium bromide? Kb (pyridine) = 1.5 × 10-9

Accepted Answer

A)  8.38 
B)  5.62 
C)  4.63 
D)  2.81 
E)  11.19 
A)  8.38 
B)  5.62 
C)  4.63 
D)  2.81 
E)  11.19

Question 4

What would be the pH of a solution prepared by dissolving 14.4 g NaOH (Mw = 40.0 g/mol) in enough water to make 1.05 L of solution?

Accepted Answer

A)  13.54 
B)  0.46 
C)  13.58 
D)  13.66 
E)  7.00 
A)  13.54 
B)  0.46 
C)  13.58 
D)  13.66 
E)  7.00

Question 5

In the reaction BF3 + NH3 → F3B:NH3, BF3 acts as a Br∅nsted acid.

Accepted Answer

A) True 
 B)False

Question 6

Determine the pH of 263 ml of solution which has [NH4I] = 0.300 M. Kb = 1.74 × 10-5 for NH3(aq).

Accepted Answer

A)  2.6 
B)  11.4 
C)  4.9 
D)  9.1 
E)  4.6 
A)  2.6 
B)  11.4 
C)  4.9 
D)  9.1 
E)  4.6

Question 7

Choose the INCORRECT statement. The term pH:

Accepted Answer

A)  refers to the "potential" of hydrogen ion 
B)  = -ln [H+] 
C)  = 14 - pOH 
D)  is more convenient than exponential notation 
E)  = -log [H3O+] 
A)  refers to the "potential" of hydrogen ion 
B)  = -ln [H+] 
C)  = 14 - pOH 
D)  is more convenient than exponential notation 
E)  = -log [H3O+]

Question 8

HNO3 is a strong acid.

Accepted Answer

A) True 
 B)False

Question 9

According to the Arrhenius theory, a neutralization reaction involves:

Accepted Answer

A)  the combination of hydrogen ions and hydroxide ions to form water. 
B)  the dissociation of a strong acid to hydrogen ions and an anion. 
C)  the dissociation of a strong base into hydroxide ions and a cation. 
D)  the addition of water to ammonia to make ammonium hydroxide. 
E)  the combination of an acid with a base to make only water. 
A)  the combination of hydrogen ions and hydroxide ions to form water. 
B)  the dissociation of a strong acid to hydrogen ions and an anion. 
C)  the dissociation of a strong base into hydroxide ions and a cation. 
D)  the addition of water to ammonia to make ammonium hydroxide. 
E)  the combination of an acid with a base to make only water.

Question 10

What is the pH of a 0.235 M solution of potassium fluoride? Ka (HF) = 6.6 × 10-4

Accepted Answer

A)  8.28 
B)  11.45 
C)  8.59 
D)  5.41 
E)  5.72 
A)  8.28 
B)  11.45 
C)  8.59 
D)  5.41 
E)  5.72

Question 11

For the following compound, predict whether the solution is acidic, basic or neutral and why: NaCl.

Accepted Answer

A)  acidic because NaCl is a strong acid 
B)  basic because NaCl is a weak base 
C)  neutral because there is no hydrolysis 
D)  basic because NaCl is the salt of a weak acid 
E)  acidic because NaCl is the salt of a weak base 
A)  acidic because NaCl is a strong acid 
B)  basic because NaCl is a weak base 
C)  neutral because there is no hydrolysis 
D)  basic because NaCl is the salt of a weak acid 
E)  acidic because NaCl is the salt of a weak base

Question 12

What is the pH of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10-3; Ka2 = 6.3 × 10-8; Ka3 = 4.2 × 10-13]

Accepted Answer

A)  5.7 
B)  4.3 
C)  3.1 
D)  2.3 
E)  1.6 
A)  5.7 
B)  4.3 
C)  3.1 
D)  2.3 
E)  1.6

Question 13

Which of the following are Lewis bases? 
I. BCl3
II. H-
III. H2O
IV. NH3
V. AlCl3

Accepted Answer

A)  II), III) and IV) 
B)  I), II), and III) 
C)  III), IV) and V) 
D)  I), II), and V) 
E)  I), II), and IV) 
A)  II), III) and IV) 
B)  I), II), and III) 
C)  III), IV) and V) 
D)  I), II), and V) 
E)  I), II), and IV)

Question 14

Hypochlorous acid (HOCl) has an ionization constant of 3.2 × 10-8. What is its percent ionization in 1.0 M and 0.10 M solutions, respectively?

Accepted Answer

A)  0.018% and 0.057% 
B)  0.032% and 0.0032% 
C)  0.57% and 0.18% 
D)  0.57% in both 
E)  0.32% in both 
A)  0.018% and 0.057% 
B)  0.032% and 0.0032% 
C)  0.57% and 0.18% 
D)  0.57% in both 
E)  0.32% in both

Question 15

A 250.0 ml sample of gaseous hydrogen bromide, measured at 22.9°C and 0.930 atm, was dissolved in sufficient pure water to form 250.0 ml of solution. What was the pH of that solution?

Accepted Answer

A)  1.42 
B)  2.58 
C)  3.83 
D)  4.18 
E)  5.68 
A)  1.42 
B)  2.58 
C)  3.83 
D)  4.18 
E)  5.68

Question 16

0.653 g of a monoprotic acid (mm = 157 g/mol) is dissolved in water to produce 50.0 mL of a solution with pH = 2.13. Determine the ionization constant of the acid.

Accepted Answer

A)  7.9 × 10-3 
B)  8.9 × 10-2 
C)  6.6 × 10-4 
D)  3.9 × 10-2 
E)  3.6 × 10-6 
A)  7.9 × 10-3 
B)  8.9 × 10-2 
C)  6.6 × 10-4 
D)  3.9 × 10-2 
E)  3.6 × 10-6

Question 17

What is the [H2AsO4-] for a solution labeled 0.10 M arsenic acid (H3AsO4)? [Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12]

Accepted Answer

A)  1 × 10-7 
B)  6 × 10-3 
C)  0.02 
D)  0.08 
E)  6 × 10-10 
A)  1 × 10-7 
B)  6 × 10-3 
C)  0.02 
D)  0.08 
E)  6 × 10-10

Question 18

Complete the following equation. List the conjugate acid base pairs. Put the base first in each pair. HCl + NH3 ⇌

Accepted Answer

A)  Cl- + NH4+   &emsp;(NH3, NH4+) (Cl-, HCl) 
B)  Cl- + NH4+   &emsp;(NH3, HCl) (Cl-, NH4+) 
C)  H2 + Cl- + NH2-   &emsp;(NH3, NH2-) (Cl-, HCl) 
D)  H2Cl+ + NH2-  &emsp; (NH3, NH2-) (HCl, H2Cl) 
E)  Cl- + NH4+   &emsp; (NH3, Cl-) (NH4+, HCl) 
A)  Cl- + NH4+   &emsp;(NH3, NH4+) (Cl-, HCl) 
B)  Cl- + NH4+   &emsp;(NH3, HCl) (Cl-, NH4+) 
C)  H2 + Cl- + NH2-   &emsp;(NH3, NH2-) (Cl-, HCl) 
D)  H2Cl+ + NH2-  &emsp; (NH3, NH2-) (HCl, H2Cl) 
E)  Cl- + NH4+   &emsp; (NH3, Cl-) (NH4+, HCl)

Question 19

CO2 acts as an acid in the reaction CaO(s) + CO2 ⇌ CaCO3(s) because it ________.

Accepted Answer

A)  turns blue litmus red 
B)  reacts with a metal 
C)  is a proton donor 
D)  is an electron-pair acceptor 
E)  is a gas containing a non-metal 
A)  turns blue litmus red 
B)  reacts with a metal 
C)  is a proton donor 
D)  is an electron-pair acceptor 
E)  is a gas containing a non-metal

Question 20

Which species in the following reaction acts as a Lewis acid? 
CuSO4(s) + 4NH3(aq) ⇌ [Cu(NH3)4]2+(aq) + SO42-(aq)

Accepted Answer

A)  SO42- 
B)  Cu2+ 
C)  [Cu(NH3)4]2+(aq) 
D)  NH3 
E)  [Cu(NH3)4]2+(aq) and SO42- 
A)  SO42- 
B)  Cu2+ 
C)  [Cu(NH3)4]2+(aq) 
D)  NH3 
E)  [Cu(NH3)4]2+(aq) and SO42-

Exam 16: Acids and Bases

For the following compound, predict whether the solution is acidic, basic or neutral and why: NH3.

Which indication of relative acid strengths is INCORRECT?

What is the pH of a 0.361 M solution of pyridinium bromide? Kb (pyridine) = 1.5 × 10-9

What would be the pH of a solution prepared by dissolving 14.4 g NaOH (Mw = 40.0 g/mol) in enough water to make 1.05 L of solution?

In the reaction BF3 + NH3 → F3B:NH3, BF3 acts as a Br∅nsted acid.

Determine the pH of 263 ml of solution which has [NH4I] = 0.300 M. Kb = 1.74 × 10-5 for NH3(aq).

Choose the INCORRECT statement. The term pH:

HNO3 is a strong acid.

According to the Arrhenius theory, a neutralization reaction involves:

What is the pH of a 0.235 M solution of potassium fluoride? Ka (HF) = 6.6 × 10-4

For the following compound, predict whether the solution is acidic, basic or neutral and why: NaCl.

What is the pH of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10-3; Ka2 = 6.3 × 10-8; Ka3 = 4.2 × 10-13]

Which of the following are Lewis bases? I. BCl3 II. H- III. H2O IV. NH3 V. AlCl3

Hypochlorous acid (HOCl) has an ionization constant of 3.2 × 10-8. What is its percent ionization in 1.0 M and 0.10 M solutions, respectively?

A 250.0 ml sample of gaseous hydrogen bromide, measured at 22.9°C and 0.930 atm, was dissolved in sufficient pure water to form 250.0 ml of solution. What was the pH of that solution?

0.653 g of a monoprotic acid (mm = 157 g/mol) is dissolved in water to produce 50.0 mL of a solution with pH = 2.13. Determine the ionization constant of the acid.

What is the [H2AsO4-] for a solution labeled 0.10 M arsenic acid (H3AsO4)? [Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12]

Complete the following equation. List the conjugate acid base pairs. Put the base first in each pair. HCl + NH3 ⇌

CO2 acts as an acid in the reaction CaO(s) + CO2 ⇌ CaCO3(s) because it ________.

Which species in the following reaction acts as a Lewis acid? CuSO4(s) + 4NH3(aq) ⇌ [Cu(NH3)4]2+(aq) + SO42-(aq)

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

For the following compound, predict whether the solution is acidic, basic or neutral and why: NH₃.

What is the pH of a 0.361 M solution of pyridinium bromide? Kb (pyridine) = 1.5 × 10^-9

In the reaction BF₃ + NH₃ → F₃B:NH₃, BF₃ acts as a Br∅nsted acid.

Determine the pH of 263 ml of solution which has [NH₄I] = 0.300 M. Kb = 1.74 × 10^-5 for NH₃(aq).

HNO₃ is a strong acid.

What is the pH of a 0.235 M solution of potassium fluoride? Ka (HF) = 6.6 × 10^-4

What is the pH of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10^-3; Ka2 = 6.3 × 10^-8; Ka3 = 4.2 × 10^-13]

Which of the following are Lewis bases? I. BCl₃ II. H- III. H₂O IV. NH₃ V. AlCl₃

Hypochlorous acid (HOCl) has an ionization constant of 3.2 × 10^-8. What is its percent ionization in 1.0 M and 0.10 M solutions, respectively?

What is the [H₂AsO₄^-] for a solution labeled 0.10 M arsenic acid (H₃AsO₄)? [Ka1 = 6 × 10^-3, Ka2 = 1 × 10^-7, Ka3 = 3 × 10^-12]

Complete the following equation. List the conjugate acid base pairs. Put the base first in each pair. HCl + NH₃ ⇌

CO₂ acts as an acid in the reaction CaO(s) + CO₂ ⇌ CaCO₃(s) because it ________.

Which species in the following reaction acts as a Lewis acid? CuSO₄(s) + 4NH₃(aq) ⇌ [Cu(NH₃)₄]²⁺(aq) + SO₄^2-(aq)