Acids, Bases, and Salts
Review for Sections 4.1 – 4.9
1.
Consider the following:
I
II
III
H2CO3 + F-  HCO3- + HF
HCO3- + HC2O4-  H2CO3 + C2O42HCO3- + H2C6H6O7-  H2CO3 + HC6H5O72-
The HCO3- is a base in
A.
B.
C.
D.
2.
The volume of 0.200 M Sr(OH)2 needed to neutralize 50.0 mL of 0.200 M HI is
A.
B.
C.
D.
3.
0.050
1.30
12.70
13.70
The volume of 0.450 M HCl needed to neutralize 40.0 mL of 0.450 M Sr(OH)2 is
A.
B.
C.
D.
5.
10.0 mL
25.0 mL
50.0 mL
100.0 mL
The pOH of 0.050 M HCl is
A.
B.
C.
D.
4.
I only
I and II only
II and III only
I, II, and III
18.0 mL
20.0 mL
40.0 mL
80.0 mL
Consider the following
I
H3PO4
II
H2PO4-
III
HPO42-
IV
PO43-
Which of the following solutions will have the largest [H30+]?
A.
B.
C.
D.
6.
Which of the following solutions will have the largest [H3O+]?
A.
B.
C.
D.
7.
I and II only
II and III only
I, II, and III only
II, III, and IV only
1.0 M HNO2
1.0 M HBO3
1.0 M H2C2O4
1.0 M HCOOH
Consider the following:
H2O + 57 kJ  H3O+ + OH-
When the temperature of the system is increased, the equilibrium shifts
A.
B.
C.
D.
left and the Kw increases
left and the Kw decreases
right and the Kw increases
right and the Kw decreases
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Chemistry 12
Acids, Bases, and Salts
8.
A 1.0 M solution of sodium dihydrogen phosphate is
A.
B.
C.
D.
9.
A Bronsted-Lowry base is defined as a chemical species that
A.
B.
C.
D.
10.
accepts protons
neutralizes acids
donated electrons
produces hydroxides ions in solution
Which of the following solutions will have the greatest electrical conductivity?
A.
B.
C.
D.
11.
acidic and the pH < 7.00
acidic and the pH > 7.00
basic and the pH < 7.00
basic and the pH > 7.00
1.0 M HCN
1.0 M H2SO4
1.0 M H3PO4
1.0 M CH3COOH
Consider the following equilibrium: HC6H5O72- + HIO3  H2C6H5O7- + IO3The order of Bronsted-Lowry acids and bases is
A.
B.
C.
D.
12.
acid, base, acid, base
acid, base, base, acid
base, acid, acid, base
base, acid, base acid
Consider the following: H2O(l)  H+ + OHWhen a small amount of 1.0 M KOH is added to the above system, the equilibrium
A.
B.
C.
D.
13.
Which of the following has the highest pH?
A.
B.
C.
D.
14.
shifts left and [H+] decreases
shifts left and [H+] increases
shifts right and [H+] decreases
shifts right and [H+] increases
1.0 M NaIO3
1.0 M Na2CO3
1.0 M Na3PO4
1.0 M Na2SO4
In a 100.0 mL sample of 0.0800 M NaOH the [H3O+] is
A.
B.
C.
D.
1.25
1.25
8.00
8.00
x
x
x
x
10-13 M
10-12 M
10-3 M
10-2 M
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Chemistry 12
Acids, Bases, and Salts
15.
Consider the following:
I
ammonium nitrate
II
calcium nitrate
III
iron III nitrate
When dissolved in water, which of these salts would form a neutral solution?
A.
B.
C.
D.
16.
II only
III only
I and III only
I, II, and III
Consider the following: SO42- + HNO2  HSO4- + NO2Equilibrium would favour the
A.
B.
C.
D.
17.
The net ionic equation for the hydrolysis of Na2CO3 is
A.
B.
C.
D.
18.
the products since HSO4- is a weaker acid than HNO2
the reactants since HSO4- is a weaker acid than HNO2
the products since HSO4- is a stronger acid than HNO2
the reactants since HSO4- is a stronger acid than HNO2
H2 O
H2 O
H2 O
H2O
+
+
+
+
Na+  NaOH + H+
2Na+  Na2O + 2H+
CO32-  H2CO3 + O2CO32-  HCO3- + OH-
Consider the following equilibrium: 2H2O(l)  H3O+ + OHA few drops of 1.0 M HCl are added to the above system. When equilibrium is
re-established, the
A.
B.
C.
D.
19.
A basic solution
A.
B.
C.
D.
20.
tastes sour
feels slippery
does not conduct electricity
reacts with metals to release oxygen gas
The balanced formula equation for the neutralization of H2SO4 by KOH is
A.
B.
C.
D.
21.
[H3O+] has increased and the [OH-] has decreased
[H3O+] has increased and the [OH-] has increased
[H3O+] has decreased and the [OH-] has increased
[H3O+] has decreased and the [OH-] has decreased
H2SO4
H2SO4
H2SO4
H2SO4
+
+
+
+
KOH → KSO4 + H2O
KOH → K2SO4 + H2O
2KOH → K2SO4 + H2O
2KOH → K2SO4 + 2H2O
An Arrhenius base is defined as a substance which
A.
B.
C.
D.
donates protons
donates electrons
produces H+ in solution
produces OH- in solution
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Chemistry 12
Acids, Bases, and Salts
22.
Consider the following equilibrium: HS- + H3PO4  H2S + H2PO4The order of Bronsted-Lowry acids and bases is
A.
B.
C.
D.
23.
The equation representing the reaction of ethanoic acid with water is
A.
B.
C.
D.
24.
acid, base, acid, base.
acid, base, base, acid
base, acid, acid, base
base, acid, base, acid
CH3COO- + H2O  CH3COOH + OHCH3COO- + H2O  CH3COO2- + H3O+
CH3COOH + H2O  CH3COO- + H3O+
CH3COOH + H2O  CH3COOH2+ + OH-
Consider the following equilibrium: 2H2O + 57kJ  H3O+ + OHWhen the temperature is decreased, the water
A.
B.
C.
D.
25.
The conjugate acid of C6H50- is
A.
B.
C.
D.
26.
1.0 M HCl
1.0 M HNO2
1.0 M H3BO3
1.0 M HCOOH
A solution of 1.0 M HF has
A.
B.
C.
D.
28.
C6H4OC6H5OH
C6H4O2C6H5OH+
Which of the following solutions will have the greatest electrical conductivity?
A.
B.
C.
D.
27.
stays neutral and the [H3O+] increases
stays neutral and the [H3O+] decreases
becomes basic and [H3O+] decreases
becomes acidic and [H3O+] increases
a lower pH than a solution of 1.0 M HCl
a higher pOH than a solution of 1.0 M HCl
a higher [OH-] than a solution of 1.0 M HCl
a higher [H3O+] than a solution of 1.0 M HCl
Which of the following is the weakest acid
A.
B.
C.
D.
HIO3
HCN
HNO3
C6H5COOH
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Chemistry 12
Acids, Bases, and Salts
29.
Considering the following data
Ka = 5.0 x 10-5
Ka = 8.0 x 10-8
Ka = 6.0 x 10-10
H3AsO4
H2AsO4HAsO42-
The Kb value for H2AsO4- is
A.
B.
C.
D.
30.
10-10 M
10-5 M
10-1 M
104 M
x
x
x
x
basic because Ka < Kb
basic because Ka > Kb
acidic because Ka < Kb
acidic because Ka > Kb
HSO4- + H2O  SO42HSO4- + H2O  H2SO4
KHSO4 + H2O  K+ +
KHSO4 + H2O  K+ +
+ H3O+
+ OHSO42- + H3O+
H2SO4 + OH-
The [OH-] in an aqueous solution always equals
A.
B.
C.
D.
35.
1.7
6.0
6.3
1.7
The net ionic equation for the predominant hydrolysis reaction of KHSO4 is
A.
B.
C.
D.
34.
10-20 M
10-9 M
10-7 M
10-6 M
x
x
x
x
An aqueous solution of NH4CN is
A.
B.
C.
D.
33.
3.5
2.9
1.0
3.5
In a solution with a pOH of 4.22, the [OH-] is
A.
B.
C.
D.
32.
10-10
10-8
10-7
10-5
x
x
x
x
In a solution at 25oC, the [H3O+] is 3.5 x 10-6 M. The [OH-] is
A.
B.
C.
D.
31.
2.0
8.0
1.2
1.7
Kw x [H3O+]
Kw - [H3O+]
Kw/[H3O+]
[H3O+]/Kw
The [H3O+] in a solution with pOH of 0.253 is
A.
B.
C.
D.
5.58
1.79
5.58
5.97
x
x
x
x
10-15 M
10-14 M
10-1 M
10-1 M
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Chemistry 12
Acids, Bases, and Salts
36.
37.
The equilibrium expression for the hydrolysis reaction of 1.0 M K2HPO4 is
A.
[H2PO42-][OH-]
[HPO4-]
C.
[K+] [KHPO4-]
[K2HPO4]
D.
[H3PO4][OH-]
[H2PO4-]
[K+]2 [HPO42-]
[K2HPO4]
The solution with the highest pH is
A.
B.
C.
D.
38.
B.
1.0 M NaCl
1.0 M NaCN
1.0 M NaIO3
1.0 M Na2SO4
The pH of 100.0 mL of 0.0050 M NaOH is
A.
B.
C.
D.
2.30
3.30
10.70
11.70
Written Response Practice
1.
a)
Write the net ionic equation for the reaction between NaHSO3 and NaHC2O4.
HSO3- + HC2O4-  H2SO3 + C2O42-
b)
Explain why the reactants are favoured in the above reaction.
H2SO3 is a stronger acid than HC2O4-
2.
What is the [H3O+] in a solution formed by adding 60.0 mL of water to 40.0 mL of 0.400
M KOH?
KOH
40
100
→
x 0.400 M
[H+][OH-] = 1.0 x 10-14
K+
+
0.160 M
OH0.160 M
[H+] = 6.3 x 10-14 M
3.
Calculate the pH of the solution formed by mixing 20.0 mL of 0.500 M HCl with 30.0
mL of 0.300 M NaOH.
HCl
+
NaOH
→
NaCl
+
H2O
0.200 L x 0.500 mole = 0.01000 mole HCl 0.300 L x 0.300 mole = 0.00900 mole NaOH
L
L
Total new volume = 20.0 mL + 30.0 mL = 50.0 mL = 0.0500 L
[H+] = 0.0010 moles = 0.020 M
0.0500 L
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Chemistry 12
Acids, Bases, and Salts
pH = 1.70
4.
a)
Write the balanced equation representing the reaction of HF with H2O.
HF + H2O  H3O+ + F-
b)
Identify the Bronsted-Lowry bases in the above equation.
H2O
5.
and
F-
Consider the following data:
Barbituric acid
Sodium propanoate
Propanoic acid
Ka = 9.8 x 10-5
Kb = 7.5 x 10-10
Ka = ?
HC4H3N2O3
NaC3H5O2
HC3H5O2
Which is the stronger acid, propanoic acid or babituric acid? Explain using calculations.
Ka (HC4H3N2O3) = Kw
Kb(C3H5O2-)
=
1.0 x 10-14
7.5 x 10-10
=
1.3 x 10-5
Barbituric acid is a stronger acid because it has a larger Ka.
6.
a)
b)
Write equations showing the amphiprotic nature of water as it reacts with HCO3-.
HCO3-
+ H2O 
H3O+ + CO32-
HCO3-
+ H2O 
H2CO3 + OH-
Calculate the Kb for HCO3-.
Kb (HCO3-) = Kw
Ka(H2CO3)
=
1.0 x 10-14
4.3 x 10-7
=
2.3 x 10-8
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Chemistry 12
Acids, Bases, and Salts