Question 1

Which pair of substances does not represent a conjugate acid-base pair?

Accepted Answer

A)  CH3COOH and CH3COO- 
B)  CH3NH3+ and CH3NH2 
C)  H2SO3 and HSO4- 
D)  HPO42- and PO43- 
E)  HCOOH and HCOO- 
A)  CH3COOH and CH3COO- 
B)  CH3NH3+ and CH3NH2 
C)  H2SO3 and HSO4- 
D)  HPO42- and PO43- 
E)  HCOOH and HCOO-

Question 2

A wine sample had a pH of 3.52. This corresponds to [H3O+] =

Accepted Answer

A)  3.3 × 10-11 M. 
B)  3.0 × 10-4 M. 
C)  5.2 × 10-4 M. 
D)  5.2 × 10-3 M. 
E)  3.3 × 10-3 M. 
A)  3.3 × 10-11 M. 
B)  3.0 × 10-4 M. 
C)  5.2 × 10-4 M. 
D)  5.2 × 10-3 M. 
E)  3.3 × 10-3 M.

Question 3

Kw for water

Accepted Answer

A)  decreases as the temperature increases 
B)  increases as the temperature increases 
C)  is equal to 1.0 × 10-14 at all temperatures 
D)  is equal to 1.0 × 1014 at all temperatures 
E)  none of these are correct 
A)  decreases as the temperature increases 
B)  increases as the temperature increases 
C)  is equal to 1.0 × 10-14 at all temperatures 
D)  is equal to 1.0 × 1014 at all temperatures 
E)  none of these are correct

Question 4

A Bronsted-Lowry base must have a(n) ____.

Accepted Answer

A)  atom that does not obey the octet rule 
B)  atom with an unshared pair of electrons 
C)  nitrogen atom 
D)  amphiprotic atom 
E)  oxygen atom 
A)  atom that does not obey the octet rule 
B)  atom with an unshared pair of electrons 
C)  nitrogen atom 
D)  amphiprotic atom 
E)  oxygen atom

Question 5

In terms of base strength, which base does not belong in a category with the others?

Accepted Answer

A)  Ba(OH)2 
B)  NaOH 
C)  Sr(OH)2 
D)  LiOH 
E)  NH4OH 
A)  Ba(OH)2 
B)  NaOH 
C)  Sr(OH)2 
D)  LiOH 
E)  NH4OH

Question 6

The product of the reaction between methylamine, CH3NH2, and hydrochloric acid are

Accepted Answer

A)  CH4NH2+ and Cl- 
B)  CH3NH- and H2Cl+ 
C)  CH3NH3+ and Cl- 
D)  CH3NH3- and Cl+ 
E)  CH3NH42+ and 2Cl- 
A)  CH4NH2+ and Cl- 
B)  CH3NH- and H2Cl+ 
C)  CH3NH3+ and Cl- 
D)  CH3NH3- and Cl+ 
E)  CH3NH42+ and 2Cl-

Question 7

In a 1.2 M solution of KOH, a strong base, [H3O+] = ____, and [OH-] = ____.

Accepted Answer

A)  1.0 × 10-7 M; 1.0 × 10-7 M 
B)  8.3 × 10-15 M; 1.0 × 10-14 M 
C)  8.3 × 10-15 M; 1.2 M 
D)  1.2 M; 8.3 × 10-15 M 
E)  1.2 M; 1.2 M 
A)  1.0 × 10-7 M; 1.0 × 10-7 M 
B)  8.3 × 10-15 M; 1.0 × 10-14 M 
C)  8.3 × 10-15 M; 1.2 M 
D)  1.2 M; 8.3 × 10-15 M 
E)  1.2 M; 1.2 M

Question 8

Which substance is a Lewis acid but not a Bronsted-Lowry acid?

Accepted Answer

A)  acetic acid 
B)  NH4+(aq) 
C)  HCO3-(aq) 
D)  CO2 
E)  CO32- 
A)  acetic acid 
B)  NH4+(aq) 
C)  HCO3-(aq) 
D)  CO2 
E)  CO32-

Question 9

Two common polyprotic acids are

Accepted Answer

A)  sulfuric acid and perchloric acid 
B)  sulfuric acid and nitric acid 
C)  sulfuric acid and phosphoric acid 
D)  perchloric acid and nitric acid 
E)  nitric acid and phosphoric acid 
A)  sulfuric acid and perchloric acid 
B)  sulfuric acid and nitric acid 
C)  sulfuric acid and phosphoric acid 
D)  perchloric acid and nitric acid 
E)  nitric acid and phosphoric acid

Question 10

Which factor does not contribute to the acidity of the hydrogen atom in the carboxylic acid functional group?

Accepted Answer

A)  the attraction of the O atoms in the carboxylic acid group for the electrons in the O-H bond 
B)  resonance stabilization of the resulting anion 
C)  the electronegativity of the C atom 
D)  the lack of polarity in the C-H bonds in the rest of the molecule 
E)  the electronegativity of the O that is bonded to the H 
A)  the attraction of the O atoms in the carboxylic acid group for the electrons in the O-H bond 
B)  resonance stabilization of the resulting anion 
C)  the electronegativity of the C atom 
D)  the lack of polarity in the C-H bonds in the rest of the molecule 
E)  the electronegativity of the O that is bonded to the H

Question 11

Which statement is not correct?

Accepted Answer

A)  a Lewis acid is a substance that can accept a pair of electrons to form a new bond 
B)  a Lewis base is a substance that can donate a pair of electrons to form a new bond 
C)  Al(OH)3 is an amphoteric substance that can form either a positive or negative ion 
D)  Neutral molecules cannot act as Lewis acids 
E)  Ag(NH3)2+ is a complex ion, formed from a Ag+ ion (Lewis acid) and two NH3 molecules (Lewis bases) 
A)  a Lewis acid is a substance that can accept a pair of electrons to form a new bond 
B)  a Lewis base is a substance that can donate a pair of electrons to form a new bond 
C)  Al(OH)3 is an amphoteric substance that can form either a positive or negative ion 
D)  Neutral molecules cannot act as Lewis acids 
E)  Ag(NH3)2+ is a complex ion, formed from a Ag+ ion (Lewis acid) and two NH3 molecules (Lewis bases)

Question 12

Amines have the general formula

Accepted Answer

A)  R-CHO 
B)  CH3-(CH2)n-CH3 
C)  R-COOH 
D)  R-NH2 
E)  R-OH 
A)  R-CHO 
B)  CH3-(CH2)n-CH3 
C)  R-COOH 
D)  R-NH2 
E)  R-OH

Question 13

Calculate the pH of a 0.051 M solution of sodium lactate. The Ka for lactic acid is 1.4 × 10-4.

Accepted Answer

A)  1.29 
B)  2.57 
C)  8.28 
D)  11.43 
E)  12.71 
A)  1.29 
B)  2.57 
C)  8.28 
D)  11.43 
E)  12.71

Question 14

Which of the following salts forms a basic solution when dissolved in water?

Accepted Answer

A)  NH4ClO4 
B)  (NH4)2NO3 
C)  NaClO4 
D)  LiCH3COO 
E)  NaCl 
A)  NH4ClO4 
B)  (NH4)2NO3 
C)  NaClO4 
D)  LiCH3COO 
E)  NaCl

Question 15

The conjugate base of NH3 is ____.

Accepted Answer

A)  H2O 
B)  OH- 
C)    
D)  NH4OH 
E)    
A)  H2O 
B)  OH- 
C)    
D)  NH4OH 
E)

Question 16

Bronsted-Lowry acids ____ and Bronsted-Lowry bases ____.

Accepted Answer

A)  generate H3O+ ions in aqueous solution; generate OH- ions in aqueous solutions 
B)  accept protons; generate OH- ions in aqueous solutions 
C)  generate OH- ions in aqueous solution; generate H3O+ ions in aqueous solutions 
D)  generate H3O+ ions in aqueous solution; donate protons in aqueous solutions 
E)  donate protons; accept protons in aqueous solutions 
A)  generate H3O+ ions in aqueous solution; generate OH- ions in aqueous solutions 
B)  accept protons; generate OH- ions in aqueous solutions 
C)  generate OH- ions in aqueous solution; generate H3O+ ions in aqueous solutions 
D)  generate H3O+ ions in aqueous solution; donate protons in aqueous solutions 
E)  donate protons; accept protons in aqueous solutions

Question 17

Which substance can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry acid?

Accepted Answer

A)  HPO42- 
B)  H2O 
C)  NH4+ 
D)  PO43- 
E)  HSO4- 
A)  HPO42- 
B)  H2O 
C)  NH4+ 
D)  PO43- 
E)  HSO4-

Question 18

Which salt forms a neutral solution when dissolved in water?

Accepted Answer

A)  LiF 
B)  K3PO4 
C)  NH4ClO4 
D)  NaOCl 
E)  NaNO3 
A)  LiF 
B)  K3PO4 
C)  NH4ClO4 
D)  NaOCl 
E)  NaNO3

Question 19

Because water can act as a Bronsted-Lowry acid or base, it is said to be ____.

Accepted Answer

A)  amphiphilic 
B)  amphihydrous 
C)  amphiphobic 
D)  amphiprotic 
E)  amphoteric 
A)  amphiphilic 
B)  amphihydrous 
C)  amphiphobic 
D)  amphiprotic 
E)  amphoteric

Question 20

Classify each compound as a carboxylic acid or an amine, in the order given.

Accepted Answer

A)  acid, acid, acid 
B)  acid, amine, acid 
C)  amine, amine, acid 
D)  amine, acid, amine 
E)  acid, acid, amine 
A)  acid, acid, acid 
B)  acid, amine, acid 
C)  amine, amine, acid 
D)  amine, acid, amine 
E)  acid, acid, amine

Which pair of substances does not represent a conjugate acid-base pair?

A wine sample had a pH of 3.52. This corresponds to [H₃O⁺] =

K_w for water

A Bronsted-Lowry base must have a(n) ____.

In terms of base strength, which base does not belong in a category with the others?

The product of the reaction between methylamine, CH₃NH₂, and hydrochloric acid are

In a 1.2 M solution of KOH, a strong base, [H₃O⁺] = , and [OH^-] = .

Which substance is a Lewis acid but not a Bronsted-Lowry acid?

Two common polyprotic acids are

Which factor does not contribute to the acidity of the hydrogen atom in the carboxylic acid functional group?

Which statement is not correct?

Amines have the general formula

Calculate the pH of a 0.051 M solution of sodium lactate. The K_a for lactic acid is 1.4 × 10^-4.

Which of the following salts forms a basic solution when dissolved in water?

The conjugate base of NH₃ is ____.

Bronsted-Lowry acids and Bronsted-Lowry bases .

Which substance can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry acid?

Which salt forms a neutral solution when dissolved in water?

Because water can act as a Bronsted-Lowry acid or base, it is said to be ____.

Classify each compound as a carboxylic acid or an amine, in the order given.

The Nature of Chemistry

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Exam 15: Acids and Bases

Which pair of substances does not represent a conjugate acid-base pair?

A wine sample had a pH of 3.52. This corresponds to [H3O+] =

Kw for water

A Bronsted-Lowry base must have a(n) ____.

In terms of base strength, which base does not belong in a category with the others?

The product of the reaction between methylamine, CH3NH2, and hydrochloric acid are

In a 1.2 M solution of KOH, a strong base, [H3O+] = ____, and [OH-] = ____.

Which substance is a Lewis acid but not a Bronsted-Lowry acid?

Two common polyprotic acids are

Which factor does not contribute to the acidity of the hydrogen atom in the carboxylic acid functional group?

Which statement is not correct?

Amines have the general formula

Calculate the pH of a 0.051 M solution of sodium lactate. The Ka for lactic acid is 1.4 × 10-4.

Which of the following salts forms a basic solution when dissolved in water?

The conjugate base of NH3 is ____.

Bronsted-Lowry acids ____ and Bronsted-Lowry bases ____.

Which substance can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry acid?

Which salt forms a neutral solution when dissolved in water?

Because water can act as a Bronsted-Lowry acid or base, it is said to be ____.

Classify each compound as a carboxylic acid or an amine, in the order given.

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

Filters

A wine sample had a pH of 3.52. This corresponds to [H₃O⁺] =

K_w for water

The product of the reaction between methylamine, CH₃NH₂, and hydrochloric acid are

In a 1.2 M solution of KOH, a strong base, [H₃O⁺] = , and [OH^-] = .

Calculate the pH of a 0.051 M solution of sodium lactate. The K_a for lactic acid is 1.4 × 10^-4.

The conjugate base of NH₃ is ____.

Bronsted-Lowry acids and Bronsted-Lowry bases .