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Bronsted-Lowry Acid-Base Model - Questions

The Bronsted-Lowry Acid-Base Model Concept Builder is comprised of 38 questions. The questions are divided into 18 different Question Groups and spread across three activities. Questions in the same group are rather similar to one another. The Concept Builder is coded to select at random a question from each group until a student is successful with that group of questions.

There are three activities in this Concept Builder. Those three activities are differentiated as follows:
 
  • Fundamental Concepts: Question Groups 1-6 ... Cover fundamental concepts like acid and base as a proton donor and acceptor, hydronium and hydroxide ion, weak acid behavior, and the products of an acid or base dissociation in water.
  • Conjugate Acid-Base Pairs: Question Groups 7-12 ... Given the chemical equation for a dissociation reaction, identify the acid, the base, and the conjugate acid-base pairs.
  • Dissociation Equations: Question Groups 13-18 ... Given the formula for an acid or a base, identify the balanced chemical equation for its dissociation in water.

The questions from each group are shown below. Teachers are encouraged to view the questions in order to judge which activities are most appropriate for their classes. We recommend providing students two or more options. 

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Bronsted-Lowry Acid Base Model


 
Activity 1: Fundamental Concepts
Question Group 1
Question 1
The Bronsted-Lowry model defines acids and bases in terms of their tendency to donate or accept a proton. Which statement below best describes what the model means by “proton”?
 
A proton is a hydrogen ion (H+).
A proton is a hydrogen atom (H).
A proton is a hydroxide ion (OH-).
A proton is a hydronium ion (H3O+).
A proton is a positively-charged electron.
 
 
 
Question Group 2
Question 2
Which statement describes the Bronsted-Lowry definition of an acid and a base?
 
An acid is a proton donor and a base is a proton acceptor.
An acid is a proton acceptor and a base is a proton donor.
An acid is a proton donor and a base is an electron donor.
An acid is a proton acceptor and a base is an electron acceptor.
An acid is a proton donor and a base is an electron acceptor.
 
 
 
Question Group 3
Question 3
Which statement describes the reaction that occurs when a Bronsted-Lowry acid dissolves in water?
 
The acid donates a proton to water to produce the hydronium ion (H3O+).
The acid donates a proton to water to produce the hydroxide ion (H3O+).
The acid donates a proton to water to produce the hydroxide ion (OH-).
The acid accepts a proton from water to produce the hydronium ion (H3O+).
The acid accepts a proton from water to produce the hydroxide ion (OH-).
 
 
 
Question Group 4
Question 4
Which statement describes the hydronium and the hydroxide ions?
 
The hydronium ion is H3O+and the hydroxide ion is OH-.
The hydronium ion is H3O+and the hydroxide ion is H3O-.
The hydronium ion is H+and the hydroxide ion is OH-.
The hydronium ion is OH+and the hydroxide ion is OH-.
The hydronium ion is OH-and the hydroxide ion is H3O+.
 
 
 
 
Question Group 5
Question 5
Which statement describes the reaction that occurs when a Bronsted-Lowry base dissolves in water?
 
The base accepts a proton from water to produce the hydroxide ion (OH-).
The base accepts a proton from water to produce the hydronium ion (H3O+).
The base donates a proton to water to produce the hydroxide ion (OH-).
The base donates a proton to water to produce the hydronium ion (H3O+).
The base donates a proton to water to produce the hydroxide ion (H3O+).
 
 
 

 
Question Group 6
Question 6
Weak acids are different than strong acids. Strong acids completely dissociate in water. Weak acids, having the generic formula HA, only partially dissociate in water. Which bar chart describes this weak acid behavior? (The bar charts represent final amounts of chemicals present in water after dissociation.)
 
 
 
 

 
Question 7
Weak acids are different than strong acids. Strong acids completely dissociate in water. Weak acids, having the generic formula HA, only partially dissociate in water. Which bar chart describes this weak acid behavior? (The bar charts represent final amounts of chemicals present in water after dissociation.)
 
 

 
Question 8
Weak acids are different than strong acids. Strong acids completely dissociate in water. Weak acids, having the generic formula HA, only partially dissociate in water. Which bar chart describes this weak acid behavior? (The bar charts represent final amounts of chemicals present in water after dissociation.)
 
 
 
 

 
Activity 2: Conjugate Acid-Base Pairs
Question Group 7
Question 9
Consider the following acid-base reaction.
 
HBr(aq)   +   H2O(l)   ==>   Br-(aq)   +  H3O+(aq)
 
Which species is acting as the proton donor in this reaction?
HBr
H2O
Br-
H3O+
 
Which species is acting as the proton acceptor in this reaction?
HBr
H2O
Br-
H3O+
 
Idenitfy the two sets of conjugate acid-base pairs.
HBr and H2O
Br- and H3O+
HBr and Br-
H2O and H3O+
HBr and H3O+
H2O and Br-
 
 
 

 
Question 10
Consider the following acid-base reaction.
 
HCl(aq)   +   H2O(l)   ==>    Cl-(aq)   +  H3O+(aq)
 
Which species is acting as the proton donor in this reaction?
HCl
H2O
Cl-
H3O+
 
 
Which species is acting as the proton acceptor in this reaction?
HCl
H2O
Cl-
H3O+
 
 
Idenitfy the two sets of conjugate acid-base pairs.
HCl and H2O
Cl- and H3O+
HCl and Cl-
H2O and H3O+
H2O and Cl-
HCl and H3O+
 
 
 
 

 
Question Group 8
Question 11
Consider the following acid-base reaction.
 
HCN(aq)   +   H2O(l)    ==>    CN-(aq)   +  H3O+(aq)
 
Which species is acting as the proton donor in this reaction?
HCN
H2O
CN-
H3O+
 
 
Which species is acting as the proton acceptor in this reaction?
HCN
H2O
CN-
H3O+
 
 
Idenitfy the two sets of conjugate acid-base pairs.
HCN and H2O
CN- and H3O+
HCN and CN-
H2O and H3O+
HCN and H3O+
H2O and CN-
 
 
 
 

 
Question 12
Consider the following acid-base reaction.
 
HClO3(aq)   +   H2O(l)   ==>    ClO3-(aq)   +  H3O+(aq)
 
Which species is acting as the proton donor in this reaction?
HClO3
H2O
ClO3-
H3O+
 
 
Which species is acting as the proton acceptor in this reaction?
HClO3
H2O
ClO3-
H3O+
 
 
Idenitfy the two sets of conjugate acid-base pairs.
HClO3 and H2O
ClO3- and H3O+
HClO3 and ClO3-
H2O and H3O+
HClO3 and H3O+
H2O and ClO3-
 
 
 
 
 
 

 
Question Group 9
Question 13
Consider the following acid-base reaction.
 
NH3(aq)   +   H2O(l)    ==>   NH4+(aq)   +  OH-(aq)
 
Which species is acting as the proton donor in this reaction?
NH3
H2O
NH4+
OH-
 
 
Which species is acting as the proton acceptor in this reaction?
NH3
H2O
NH4+
OH-
 
 
Idenitfy the two sets of conjugate acid-base pairs.
NH3 and H2O
NH4+ and OH-
NH3 and NH4+
H2O and OH-
NH3 and OH-
H2O and NH4+
 
 
 
 
 
 
 

 
Question 14
Consider the following acid-base reaction.
 
C5H5N(aq)   +   H2O(l)    ==>    C5H5NH+(aq)   +  OH-(aq)
 
Which species is acting as the proton donor in this reaction?
C5H5N
H2O
C5H5NH+
OH-
 
 
Which species is acting as the proton acceptor in this reaction?
C5H5N
H2O
C5H5NH+
OH-
 
 
Idenitfy the two sets of conjugate acid-base pairs.
C5H5N and H2O
C5H5NH+ and OH-
C5H5N and C5H5NH+
H2O and OH-
C5H5N and OH-
H2O and C5H5NH+
 
 
 
 
 
 
 
 

 
Question Group 10
Question 15
When an acid donates a proton to another substance, it turns into its conjugate base. And when a base accepts a proton from another substance, it turns into its conjugate acid.
 
If HC2H3O2 acts as an acid, then what is its conjugate base?
H2O
H3O+
OH-
HC2H3O2+
HC2H3O2-
H2C2H3O2+
H2C2H3O2-
C2H3O2-
C2H3O2+
 
 
If CH3NH2 acts as a base, then what is its conjugate acid?
H2O
H3O+
OH-
CH3NH2+
CH3NH2-
CH3NH+
CH3NH-
CH3NH3-
CH3NH3+
 
 
 
 

 
Question 16
When an acid donates a proton to another substance, it turns into its conjugate base. And when a base accepts a proton from another substance, it turns into its conjugate acid.
 
If HClO2 acts as an acid, then what is its conjugate base?
H2O
H3O+
OH-
HClO2+
HClO2-
H2ClO2+
H2ClO2-
ClO2+
ClO2-
 
 
 
 
If C2H5NH2 acts as a base, then what is its conjugate acid?
H2O
H3O+
OH-
C2H5NH2+
C2H5NH2-
C2H5NH3+
C2H5NH3-
C2H5NH+
C2H5NH-
 
 
 
 

 
Question Group 11
Question 17
When an acid donates a proton to another substance, it turns into its conjugate base. And when a base accepts a proton from another substance, it turns into its conjugate acid.
 
If HNO3 acts as an acid, then what is its conjugate base?
H2O
H3O+
OH-
HNO3+
HNO3-
H2NO3+
H2NO3-
NO3+
NO3-
 
 
If (CH3)3N acts as a base, then what is its conjugate acid?
H2O
H3O+
OH-
(CH3)3N+
(CH3)3N-
(CH3)2CH2N+
(CH3)2CH2N-
(CH3)3NH-
(CH3)3NH+
 
 
 
 

 
Question 18
When an acid donates a proton to another substance, it turns into its conjugate base. And when a base accepts a proton from another substance, it turns into its conjugate acid.
 
If HClO4 acts as an acid, then what is its conjugate base?
H2O
H3O+
OH-
HClO4+
HClO4-
H2ClO4+
H2ClO4-
ClO4+
ClO4-
 
 
If C6H5NH2 acts as a base, then what is its conjugate acid?
H2O
H3O+
OH-
C6H5NH2+
C6H5NH2-
C6H5NH3+
C6H5NH3-
C6H5NH-
C6H5NH+
 
 
 
 

 
Question Group 12
Question 19
When an acid donates a proton to another substance, it turns into its conjugate base. And when a base accepts a proton from another substance, it turns into its conjugate acid.
 
If HSO4- acts as an acid, then what is its conjugate base?
H2O
H3O+
OH-
HSO4
HSO42-
H2SO4
H2SO42-
SO4
SO42-
 
 
If HSO4- acts as a base, then what is its conjugate acid?
H2O
H3O+
OH-
HSO4
HSO42-
H2SO4
H2SO42-
SO4
SO42-
 
 
 

 
Question 20
When an acid donates a proton to another substance, it turns into its conjugate base. And when a base accepts a proton from another substance, it turns into its conjugate acid.
 
If HC2O4- acts as an acid, then what is its conjugate base?
H2O
H3O+
OH-
HC2O4
HC2O42-
H2C2O4
H2C2O42-
C2O4
C2O42-
 
 
If HC2O4- acts as a base, then what is its conjugate acid?
H2O
H3O+
OH-
HC2O4
HC2O42-
H2C2O4
H2C2O42-
C2O4
C2O42-
 
 
 

 
Activity 3: Acid and Base Dissociation Equations
Question Group 13
Question 21
Identify the dissociation equation for the dissociation of the weak acid hydrofluoric acid (HF) in water.
 
 
 
 
Question 22
Identify the dissociation equation for the dissociation of the weak acid hydrofluoric acid (HF) in water.
 
 
 
 
 
 
Question 23
Identify the dissociation equation for the dissociation of the weak acid hydrofluoric acid (HF) in water.
 
 
 
 
 
Question Group 14
Question 24
Identify the dissociation equation for the dissociation of the weak acid nitrous acid (HNO2) in water.
 
 
 

 
Question 25
Identify the dissociation equation for the dissociation of the weak acid nitrous acid (HNO2) in water.
 
 
 
 
Question 26
Identify the dissociation equation for the dissociation of the weak acid nitrous acid (HNO2) in water.
 
 
 

 
Question Group 15
Question 27
Identify the dissociation equation for the dissociation of the weak acid chlorous acid (HClO2) in water.
 
 
 
 
Question 28
Identify the dissociation equation for the dissociation of the weak acid chlorous acid (HClO2) in water.
 
 
 

 
Question 29
Identify the dissociation equation for the dissociation of the weak acid chlorous acid (HClO2) in water.
 

 
 
 
 
Question Group 16
Question 30
Identify the dissociation equation for the dissociation of the weak acid carbonic acid (H2CO3) in water.
 
 
 
 

 
Question 31
Identify the dissociation equation for the dissociation of the weak acid carbonic acid (H2CO3) in water.
 

 
 
 
Question 32
Identify the dissociation equation for the dissociation of the weak acid carbonic acid (H2CO3) in water.
 
 
 

 
Question Group 17
Question 33
Identify the dissociation equation for the dissociation of the weak base ammonia (NH3) in water.
 
 
 
 
Question 34
Identify the dissociation equation for the dissociation of the weak base ammonia (NH3) in water.
 
 
 

 
Question 35
Identify the dissociation equation for the dissociation of the weak base ammonia (NH3) in water.
 

 
 
 
Question Group 18
Question 36
Identify the dissociation equation for the dissociation of the weak base pyridine (C5H5N) in water.
 
 
 
 

 
Question 37
Identify the dissociation equation for the dissociation of the weak base pyridine (C5H5N) in water.
 
 
 
 
Question 38
Identify the dissociation equation for the dissociation of the weak base pyridine (C5H5N) in water.