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.
A.
B.
C.
D.
I only
I and II only
II and III only
I, II, and III
Consider the following equilibrium for an indicator:
HInd + H2O Ind- + H3O+
When a few drops of indicator methyl red are added to 1.0 M HCl, the colour of
the resulting solution is
A.
B.
C.
D.
3.
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.
4.
10.0 mL
25.0 mL
50.0 mL
100.0 mL
The pOH of 0.050 M HCl is
A.
B.
C.
D.
5.
red and the products are favoured
red and the reactants are favoured
yellow and the products are favoured
yellow and the reactants are favoured
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.
18.0 mL
20.0 mL
40.0 mL
80.0 mL
6.
Consider the following
I
H3PO4
II
H2PO4-
III
HPO42-
IV
Which of the following solutions will have the largest [H30+]?
A.
B.
C.
D.
7.
Which of the following solutions will have the largest [H3O+]?
A.
B.
C.
D.
8.
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.
9.
Normal rainwater has a pH of approximately 6 as a result of dissolved
A.
B.
C.
D.
10.
left and the Kw increases
left and the Kw decreases
right and the Kw increases
right and the Kw decreases
oxygen
carbon dioxide
sulphur dioxide
nitrogen dioxide
A 1.0 M solution of sodium dihydrogen phosphate is
A.
B.
C.
D.
acidic and the pH < 7.00
acidic and the pH > 7.00
basic and the pH < 7.00
basic and the pH > 7.00
PO43-
11.
Consider the following equilibrium for an indicator:
HInd + H2O Ind- + H3O+
When a few drops of indicator chlorophenol red are added to a colourless solution
of pH 4.0, the resulting solution is
A.
B.
C.
D.
12.
A Bronsted-Lowry base is defined as a chemical species that
A.
B.
C.
D.
13.
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.
14.
red as [HInd] < [Ind-]
red as [HInd] > [Ind-]
yellow as [HInd] < [Ind-]
yellow as [HInd] > [Ind-]
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.
15.
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.
shifts left and [H+] decreases
shifts left and [H+] increases
shifts right and [H+] decreases
shifts right and [H+] increases
16.
Which of the following has the highest pH?
A.
B.
C.
D.
17.
In a 100.0 mL sample of 0.0800 M NaOH the [H3O+] is
A.
B.
C.
D.
18.
1.0 M NaIO3
1.0 M Na2CO3
1.0 M Na3PO4
1.0 M Na2SO4
1.25
1.25
8.00
8.00
x
x
x
x
10-13 M
10-12 M
10-3 M
10-2 M
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.
19.
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.
20.
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
The net ionic equation for the hydrolysis of Na2CO3 is
A.
B.
C.
D.
H2O
H2O
H2O
H2 O
+
+
+
+
Na+ NaOH + H+
2Na+ Na2O + 2H+
CO32- H2CO3 + O2CO32- HCO3- + OH-
21.
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.
22.
A basic solution
A.
B.
C.
D.
23.
+
+
+
+
KOH → KSO4 + H2O
KOH → K2SO4 + H2O
2KOH → K2SO4 + H2O
2KOH → K2SO4 + 2H2O
donates protons
donates electrons
produces H+ in solution
produces OH- in solution
Consider the following equilibrium: HS- + H3PO4 H2S + H2PO4The order of Bronsted-Lowry acids and bases is
A.
B.
C.
D.
26.
H2SO4
H2SO4
H2SO4
H2SO4
An Arrhenius base is defined as a substance which
A.
B.
C.
D.
25.
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.
24.
[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
acid, base, acid, base.
acid, base, base, acid
base, acid, acid, base
base, acid, base, acid
The equation representing the reaction of ethanoic acid with water is
A.
B.
C.
D.
CH3COO- + H2O CH3COOH + OHCH3COO- + H2O CH3COO2- + H3O+
CH3COOH + H2O CH3COO- + H3O+
CH3COOH + H2O CH3COOH2+ + OH-
27.
Consider the following equilibrium: 2H2O + 57kJ H3O+ + OHWhen the temperature is decreased, the water
A.
B.
C.
D.
28.
The equation for the reaction of Cl2O with water is
A.
B.
C.
D.
29.
H2O 2HClO
H2O 2ClO + H2
H2O Cl2 + H2O2
H2O Cl2 + O2 + H2
C6H4OC6H5OH
C6H4O2C6H5OH+
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.
32.
+
+
+
+
Which of the following solutions will have the greatest electrical conductivity?
A.
B.
C.
D.
31.
Cl2O
Cl2O
Cl2O
Cl2O
The conjugate acid of C6H50- is
A.
B.
C.
D.
30.
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
33.
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.
34.
3.5
2.9
1.0
3.5
x
x
x
x
10-20 M
10-9 M
10-7 M
10-6 M
1.7
6.0
6.3
1.7
x
x
x
x
10-10 M
10-5 M
10-1 M
104 M
An aqueous solution of NH4CN is
A.
B.
C.
D.
37.
10-10
10-8
10-7
10-5
In a solution with a pOH of 4.22, the [OH-] is
A.
B.
C.
D.
36.
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.
35.
2.0
8.0
1.2
1.7
basic because Ka < Kb
basic because Ka > Kb
acidic because Ka < Kb
acidic because Ka > Kb
The net ionic equation for the predominant hydrolysis reaction of KHSO4 is
A.
B.
C.
D.
HSO4- + H2O SO42- + H3O+
HSO4- + H2O H2SO4 + OHKHSO4 + H2O K+ + SO42- + H3O+
KHSO4 + H2O K+ + H2SO4 + OH-
38.
The [OH-] in an aqueous solution always equals
A.
B.
C.
D.
39.
The [H3O+] in a solution with pOH of 0.253 is
A.
B.
C.
D.
40.
41.
x
x
x
x
10-15 M
10-14 M
10-1 M
10-1 M
A.
[H2PO42-][OH-]
[HPO4-]
C.
[K+] [KHPO4-]
[K2HPO4]
B.
D.
[H3PO4][OH-]
[H2PO4-]
[K+]2 [HPO42-]
[K2HPO4]
The solution with the highest pH is
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.
43.
5.58
1.79
5.58
5.97
The equilibrium expression for the hydrolysis reaction of 1.0 M K2HPO4 is
A.
B.
C.
D.
42.
Kw x [H3O+]
Kw - [H3O+]
Kw/[H3O+]
[H3O+]/Kw
2.30
3.30
10.70
11.70
Consider the following equilibrium for an indicator: HInd + H2O Ind- + H3O+
At the transition point,
A.
B.
C.
D.
[HInd] > [Ind-]
[HInd] = [Ind-]
[HInd] < [Ind-]
[HInd] = [H3O+]
Written Response:
1.
a)
NaHC2O4.
Write the net ionic equation for the reaction between NaHSO3 and
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
K+
→
x 0.400 M
0.160 M
[H+][OH-] = 1.0 x 10-14
3.
+
OH0.160 M
[H+] = 6.3 x 10-14 M
A solution of 0.100 M HOCN has a pH of 2.24. Calculate the Ka value for the
acid.
Ka
=
10-2.24
=
H+
HOCN
I
C
E
0.100 M
0.005754 M
0.094245 M
Ka
=
(0.005754 )2
0.094245
0.005754 M
0
0.005754 M
0.005754 M
=
3.5 x 10-4
+
OCN0
0.005754 M
0.005754 M
4.
Calculate the pH in 100.0 mL 0.400 M H3BO3.
I
C
E
H+
H3B03
0.400 M
x
0.400 - x
0
x
x
0
(x)2
0.400
=
+
small Ka approximation
7.3 x 10-10
x
=
1.709 x 10-5 M
pH
=
4.77
H2BO30
x
x
5.
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
→
NaCl
+
+
0.200 L x 0.500 mole
= 0.01000 mole NaOH
L
NaOH
H2 O
= 0.01000 mole HCl
0.300 L x 0.500 mole
L
I
0.0100 mole
0.00900 mole
C
0.00900 mole
0.00900 mole
E
0.0010
0
mole
Note the loss of significant figures!
new volume = 20.0 mL + 30.0 mL = 50.0 mL = 0.0500 L
[H+] = 0.0010 moles =
0.0500 L
Total
0.020 M
pH = 1.70
6.
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.
H2 O
and
F-
7.
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) =
=
1.3 x 10-5
Kw
=
Kb(C3H5O2-)
1.0 x 10-14
7.5 x 10-10
Barbituric acid is a stronger acid because it has a larger Ka.
8.
A solution of 0.0100 M lactic acid, HC3H5O3, has a pH of 2.95. Calculate the Ka
value.
HC3H5O3
C3H5O3-
I
0.0100 M
C
0.001122
0.001122
E
0.008878
0.001122
Ka
9.
=
(0.001122)2
0.008878
H+
0
0.001122
+
0
0.001122
=
1.4 x 10-4
a)
Write equations showing the amphiprotic nature of water as it reacts with
HCO3-.
HCO3- + H2O H3O+ + CO32HCO3- + H2O H2CO3 + OH-
10
-14
10
-7
10.
b)
Calculate the Kb for HCO3-.
=
Kb (HCO3-) =
2.3 x 10-8
Kw
=
Ka(H2CO3)
1.0 x
4.3 x
Calculate the [H3O+] in 0.550 M C6H5COOH.
C6H5COO
-
I
C
E
C6H5COOH
0.550 M
x
0.550 - x
0
x
x
0
(x)2
0.550
x
=
H+
small Ka approximation
=
6.5 x 10-5
[H3O+] =
6.0 x 10-3 M
+
0
x
x