sp
[ ]
= [3Ni ] [2 PO ]
4
3
2
3−
2+
D. K sp
4
22. The conjugate base of H 2 PO 4− is
Chemistry 12
Acids and Bases Part One Monster Review
(1 mark)
A. conjugate
PO 43− base of H 2 PO 4− is
22. The
(1 mark)
following are general properties of bases in aqueous solution?
(2 marks)
1. 21. Which of the
B. HPO3−4−
A. PO 4
2−
A. feel
and increase H 3O +
C.
HPOslippery
4−
−
22. The
(1 mark)
B. conjugate
HPO 4 base of H 2 PO 4 is
B.
turn
litmus
red
and
accept
a
proton
D. H 3PO2−
4
C.
HPO
3−
4
C.
conduct
electricity and turn litmus blue
A. PO 4
22. The conjugate base of H 2 PO 4− is
D.
H 3PO
D. feel
slippery
and react with Au to produce H 2( g )
−4
B. HPO
4
OVER
A. PO 43−
7
− 0.10 M solutions of NaCl, HCN and HNO 2 are measured.
C.
HPO 42− conductivities
23. The
The conjugate
electrical
base of H 2 POof
(1 mark)
2. 22.
−
4 is
B.
HPO
The order by conductivity from4 highest to lowest is
(2 marks)
D. H 3PO 4
3−
23. The
electrical
conductivities
of 402−.10 M solutions of NaCl, HCN and HNO2 are measured.
A.
C.HCN
HPO
4 > HNO >
A. PO
NaCl
2
The order by
conductivity from highest to lowest is
(2 marks)
HCN4−> HNO2 >D.NaCl
B. HPO
H 3PO 4
A.
HNO
HCN2
C. NaCl >
HCN2>>HNO
C. electrical
HPO 42− conductivities of 0.10 M solutions of NaCl, HCN and HNO are measured.
3. 23. The
2
B.
D. HCN
HNO2> >HNO
HCN
2 > NaCl
The
order
by
conductivity
from
highest
to
lowest
is
(2 marks)
D. NaCl
H 3PO>4 HCN > HNO2
C.
23. >
electrical conductivities of 0.10 M solutions of NaCl, HCN and HNO2 are meas
D. NaCl
HNO2>>HNO
HCN
>The
NaCl
A.
HCN
2
The order by conductivity from highest to lowest is
(
B. HCN > HNO2 > NaCl
C. NaCl > HCN > A.
HNONaCl
> HNO
2 has
2 > HCN
24. The
Which
of the following
acids
weakest
conjugate
base?
(1 mark)
23.
electrical
conductivities
of 0.the
10 M
solutions
of NaCl
, HCN and HNO2 are measured.
D. HNO2 > HCN >B.NaCl
HNO2to>lowest
NaCl is
The order by conductivityHCN
from >
highest
(2 marks)
A. HIO3
C.
NaCl
>
HCN
>
HNO
2
4. 24. Which of the following acids has the weakest conjugate
base?
(1 mark)
B. NaCl
HNO2> HNO2 >D.HCN
A.
HNO2 > HCN > NaCl
A.
B.
HCN
C. HIO
H 3PO
3 >
4 HNO 2 > NaCl
C.
NaCl
B.
D. HNO
CH COOH
2> HCN > HNO 2
24. Which of3 the following acids has the weakest conjugate base?
(1 mark)
D. H
HNO
C.
3 PO24 > HCN > NaCl
[
5.
25.
24.
25.
25.
6. 26.
25.
]
D. HIO
CH 33COOH
A.
24. Which of the following acids has the weakest conjugate base?
B. HNO2
WhenH 310
.04mL of 0.A.
10 MHIO
HCl is added to 10.0 mL of water, the concentration
C.
PO
3
+
in
the
final
solution
is
(1 mark)
of
H
O
3 3COOH
D. CH
B. acids
HNO
2 the weakest conjugate base?
Which
of the following
has
(1 mark)
When 10.0 mL of 0.10
is added to 10.0 mL26.of water,
concentration
Whichthe
of the
following chemical species are amphip
C. MHHCl
3 PO 4
A. 0.010
M
+
(1 mark)
of
O in
A. H 3HIO
3 the final solution
D. CHis
3COOH
B. 0.050 M
F−
I.
B. HNO2
C. 0.010
10 MM
A.
When
.0 4mL of 0.10 M HCl is added to 10.0 mL of water, the concentration II.
C. H10
3 PO
NH 4+
D. 0.050
20
B.
M
+ M
the final solution is
(1 mark)
of
O in
D. H 3CH
COOH
C. 0.103 M
III.
HPO 42−
25.
When
10
.
0
mL
of
0
.
10
M
HCl
is
added
to
10
.
0
mL
of
water,
the
concentration
Which
of the
species are amphiprotic in aqueous solution?
(2 marks)
D. 0.010
20
MM following chemical
A.
of H 3O + in the final solution is
B. 0.050 M
F−
I.
A. I only.
C.
0
.
10
M
A.
0
.
010
M
When 10.0 mL of 0.10 M HCl is added
to
10
.
0
mL
of
water,
concentration
B. IIthe
only.
+
II.
NH
+
D. H0O
.20 in
M the final solution
B. 0.050
C. III only.
is M 4
(1 mark)
of
3
C. III.
0.10 M HPO 2−
D. II and III only.
4
-8A. 0.010 M
D. 0.20 M
B. 0.050 M
-8C. I0only.
.10 M
A.
B.
D. II0.only.
20 M
27. A solution is prepared by mixing 1.50 × 10 −3 mol H
A.solution
0 molis prepared by mixing 1.50 × 10 −3 mol HCl with 3.00 × 10 −3 mol KOH .
27. A
−3
B. 1.50 the
× 10moles
mol
(1 mark)
Calculate
of OH − present after mixing.
−3
−3
7. 27. A solution is prepared
.
×
mol
HCl
with
3
.
00
×
10
mol
KOH
.
by
mixing
1
50
10
−3
C. 3.00 × 10 mol
A.
0 molthe moles of OH − present after mixing.
(1 mark)
Calculate
D. 4.50 × 10−−33 mol
B. 1.50 × 10 mol
A. 0 mol
C. 3.00 × 10 −−33 mol
B. 1.50 × 10 mol
D. 4.50 × 10 −−33 mol
C. 3.00 × 10 mol
28. Calculate the pH−3in a 0.020 M solution of Sr(OH)2 .
(2 marks)
D. 4.50 × 10 mol
A. 1.40
B.
1.70the pH in a 0.020 M solution of Sr(OH) .
8. 28. Calculate
2
C. 12.30
1.40
28. A.
Calculate
D.
12
60the pH in a 0.020 M solution of Sr(OH)2 .
B.
1.70
A.
40
C. 121..30
B. 121..60
70
D.
C. 12.30
2−
9. 29. The K b value for HPO 4 is
D. 12.60
A. 2.2 × 10 −13
8
29. The
HPO 42− is
B. K
6.b2 value
× 10 −for
C. 1.6 × 10 −−713
29.
The 2K.2of
value
for HPO142−
is salt solutions is acidic?
A.
10following
30. Which
the
.0 M
b ×
−3
D. 7.5 × 10 −8
B. 6.2 × 10 −13
A.
A. BaS
2.2 × 10−7
10. 30. Which
the
1.0 M salt solutions is acidic?
C.
1
.6of×Cl
10 following
B.
B. NH
6.24×
10−−38
D. Ca
7.5 NO
× 10 −7
C.
A.
3 )2
C. BaS
1.6( × 10
−3
B.
NH
D.
COO
-9D. NaCH
7.54×Cl310
C. Ca( NO3 )2
D.
NaCH 3COO
-911. 31. Which of the following represents the hydrolysis reaction that occurs
-9in a solution of K 2 C 2 O 4 ?
(2 marks)
(2 marks)
(1 mark)
(1 mark)
(1mark)
mark)
(1
(1 mark)
OVER
OVER
OVER
(1 mark)
31. Which of the following
represents
2the
− hydrolysis reaction that occurs
+
A. K 2 C 2 O 4 →
← C 2OK ?+ C 2 O 4
(1 mark)
in a solution
of K
2 2 4
21. Which of the following tests c
+
+
→
B. K + 2 H 2 O ← KOH + H 3O
and 1.0 M NaOH?
+
A. K 2 C 22O− 4 →
2 K→
+ C 2 O 42 −−
←
−
C. C 2 O 4 + H 2 O ← HC 2 O 4 + OH
B. K + + 2 H 2 O →
KOH + H 3O +
I.
electrical c
←
→
D. K 2 C 2 O 4 + H 2 O ← K 2 CO3 + CO2 + H 2
−
−
C. C 2 O 42 − + H 2 O →
← HC 2 O 4 + OH
II.
reaction wi
12. 21. Which of the following tests could be used to distinguish between 1.0 M HCl
D. K 2 C 2 O 4 + H 2 O →
← K 2 CO3 + CO2 + H 2
and 1.0 M NaOH?
(1 III.
mark) colour of th
32. When the indicator thymol blue is added to a 0.10 M solution of an unknown acid,
the solutionI.is red.electrical
The acidconductivity
could be
A.
B.
II.
reaction
to produce
hydrogen
gas of an unknown acid,
32. When
the indicator
thymol with
blue zinc
is added
to a 0.10
M solution
A. HF
C.
the
The acid could be
B. solution
H 2S III.is red.colour
of the indicator phenolphthalein
D.
C.
A. HCN
HF
D.
HNO
B. H 2S 3
A. III only
mark)
III (1
only
I and II only
II and III only
(1 mark)
I, II and III
22. An Arrhenius base is defined as a compound that
(1 mark)
−
13. 22. An
A. Arrhenius
accepts OH
base in
is solution.
defined as a compound that
(1 mark)
B.
A.
C.
B.
D.
C.
−
releases OH in solution.
accepts OH − in solution.
accepts protons in solution.
releases OH − in solution.
donates protons in solution.
accepts protons in solution.
D. donates protons in solution.
14. 23. In which one of the following equations are the Brønsted-Lowry acids and bases all
correctly identified? 24. Which of the following statements applies to 1.0 M NH 3( aq ) but
(1 mark)
not to 1.0 M NaO
23. In which one of the following equations are the Brønsted-Lowry acids and bases all
→
Base
Base
+
correctly Acid
identified?+
(1 mark)
Acid
A. partially
← ionizes
24. Which of the following statements
appliesan
to acid
1.0 M NH 3( aq ) but not to 1.0 M NaOH( aq ) ?
B. 2−neutralizes
−
→
+
A.
H
O
HO
SO
HSO3 −
→
2 2
2
Acid
+
Base
Base
C. 3 has a ←
pH
than
7 ++
← greater
Acid
(1 mark)
2−
− NH
D.
turns
bromcresol
green
from
yellow
to
blue
24. Which
of
the
following
statements
applies
to
1
.
0
M
but
not
to
1
.
0
M
NaOH
−
A.
partially
ionizes
→
+
+
B.
3( aq ) HO −
( aq ) ?
H O
HSO−3
SO
←
2
→
+
A. neutralizes
H 22O22 an +acid SO332−
HO
HSO
B.
2
3
←
(1 mark)
2−
−
−
→
+
+
C. partially
C.
has
a
pH
greater
than
7
SO
HO
H
O
HSO
2−
−
−
A.
ionizes
3
2
3
←
→
+
+
B.
SO2 2
2 O 2following statements
← totoHSO
24. Which
ofHthe
applies
1.0 3M NH 3( aq ) HO
but 2not to 1.0 M NaOH( aq ) ?
D. neutralizes
turns
bromcresol
green 3from yellow
blue
B.
2− an acid
−
→
+
+
D.
SO32−
HSO−3
H 2O2
HO2 −−
←
→
+ thanH
+
C. has SO
C.
a pH
7
HO
O
HSO
(1 mark)
2
2
3 greater25.
2
3
In which of←the following are reactants favoured?
A. turns
partially
ionizes green from yellow to blue
D.
bromcresol
− NH
− to 1.0 M NaOH
ofSO
the2−following
applies
toHSO
1.0 M
but not
15. 24. Which
→
+ 3( aq ) HO
D. neutralizes
H 2O2
( aq ) ?
B.
an +acid statements
3
3
←
2
−
− →
+
+
A.
HNO
CN
NO
HCN
←
2
2
(1 mark)
C. has a pH greater than 7
25. In
which
of the
following are reactants favoured?
(1
mark)
A.
partially
ionizes
− →
−
D. turns bromcresol green
yellow
to blue
B. from
H 2S
+ HCO
HS
+
H
CO
←
2
3
3
B. neutralizes an−acid
−
→
−
+
+ greater
+ HCN
A.
HNO
CN
25. In
following
are
favoured?→
(1 mark)
← C.
2 the
2H PO
C.which
has
aofpH
than
7NOreactants
← H 2 PO 4 + NH 4
3
4 + NH 3
D. turns
green
from
− yellow to blue
→ HS
B.
H 2S +bromcresol
HCO3−− →
← D.
−+ H
2 CO 3 + PO 3 − → CH COO − + HPO 2 −
CH
COOH
←
+
A. HNO
CN
NO
3
4
4
←
2
2 +3 HCN
−
+
which
of
the
following
are
reactants
favoured?
(1 mark)
→
16. 25. In
C. H PO + NH
H 2−PO 4 + NH 4
← HS
B. H 23S +4 HCO3 −3 →
+
H
CO
←
2
3
3− → −
2−
−
− PO
→
D. HNO
CH 3COOH
+
CH
COO
+
+
A.
CN
NO
HCN
←
−
+ + HPO 4
3
4
→
←
2
2
H 3PO
+ NH
H 2reactants
PO 4 + NH
← are
3
4 -825. C.
In which
of4 the
following
favoured?
(1 mark)
− →
−
B.
H
S
+
HCO
HS
+
H
CO
3
−
2
−
−
→
26.
the2COO
pOH
solution prepared by adding 0.50 mol of NaOH to
← What
2 COOH +
3 of
3 PO
D. CH
+ aHPO
← −isCH
3
3
4
4
8
+
A. HNO2 + CN − →
NO
HCN
−.50 L of +solution?
prepare
0
←
→
2
C. H 3PO 4 + NH 3 ← H 2 PO 4 + NH 4
− →
−
B. His2Sthe+ pOH
HCO3of
+00H 2 COby
3 − HS
− mol of NaOH to
26. What
a←
solution
→ prepared
3 −adding 0.250
D. CH
3COOH + PO 4 A. ← 0.CH
3COO + HPO 4
prepare
0.50+L NH
of solution?
(2 marks)
−
+
→
0.30
C. H 3PO
← B.H 2 PO
4
3
4 + NH 4
prepared
by adding 0.50 mol of NaOH to
17. 26. What is the pOH of a solution
C. 14
.00
A.
0.00
D. CH
PO 43− →
CH 3COO − + HPO 42 −
←
prepare
03.COOH
50 L of +solution?
(2 marks)
D. 13.70
B. 0.30
26. What
the pOH of a solution prepared by adding 0.50 mol of NaOH to
A.
0is..00
C. 14
00
prepare
0.50 L of solution?
(2 marks)
D. 13
70
B.
0..30
C. 14.00
26. What
the pOH of a solution prepared by +adding 0.50 mol of NaOH to
A. 0is.00
27. What is the H 3O in a solution with a pOH = 5.20 ?
D.
13
.
70
prepare
0.50 L of solution?
(2 marks)
B. 0.30
C. 14.00
× 10a−14
M = 5.20 ?
A. 1.4with
+
A. 0is.00
the
H
O
in
a
solution
pOH
(2 marks)
18. 27. What
3
D. 13.70
−9
B. 0.30
B. 1.6 × 10 M
+
C. 114
.4.00
× 10H−14
A.
27. What
is
the
(2 marks)
C. 6.3with
× 10a−6pOH
M = 5.20 ?
3OM in a solution
−9
D.
13
.
70
B. 1.6 × 10 M
D. 7.1 × 10 −1 M
−14
..43 ×× 10
A.
−6 M
+
C. 16is
27. What
the10H
OM
in a solution with a pOH = 5.20 ?
(2 marks)
−93
B.
1
6
10
.
×
−1 M
D. 7.1 × 10 M
[
[
]
[
]
[
]
−14
6
−
]
II.
0.10 M HNO2
I.
0.10 M HCl
III.
0.10 M NaOH
II.
0.10 M HNO2
19. 28. Which of the following solutions will have a pH = 1.00 ?
(1 mark)
III.
0.10 M NaOH
A. I only.
B. III only.
I.
0.10 M HCl
C. I and II only.
A. I only.
II.
D. I, II and III.
B. III only.
0.10 M HNO2
C. I and II only.
III.
0.10 M NaOH
D. I, II and III.
21. A hydronium ion has the formula
(1 mark)
A. I only.
2−
−8
21. K
A
ionHhas
the−formula
(1mark)
mark)
+ acid
B.
III
only.
for
?
(1
20. 29.
2 AsO 4 is 5.6 × 10 . What is the value of K b for HAsO 4
A.ahydronium
Hthe
2
C. I and− II only.
B. I,H
OH+and III.
−22
D.
A.
29. K a for the acid H 2 AsO 4− is 5.6 × 10 −8 . What is the
5.6II
2 × 10 ion has the formula
21. A.
A hydronium
(1 mark)
+
−
C. OH
H2O
−14
B.
B. 3.2 × 10
+O++
A. 5.6 × 10 −22
D. H
H23O
−7
A.
C.
1.8 × 10 ion has the formula
21. C.
A hydronium
(1 mark)
−+
B. 3.2 × 10 −14
−
4
B.
OH
D.
H
O
D. 2.43 × 10
−
−8
−7 HAsO 2− ?
+ + acid H 2 AsO 4 is 5.6 × 10 . What is the value
(1 mark)
29. K
C. 1of.8 K
× b10for
4
A.a for
C.
H 2the
O
21. 21. A hydronium
ion has the formula
(1 mark)
−+
D. 2.4 × 10 −4
B.
OH
D.
H
O
−22
3
A. 5.6 × 10
22. C.
The conjugate
(1 mark)
H 2+O + −14acid of C6 H 5NH 2 is
A. 3H
B.
.22 × 10
22. In
The
conjugate
acid of the
C6 Hfollowing
(1mark)
mark)
30.
(1
5 NH 2 is has a pH = 7.00 at the equivalence point?
D.a titration,
H 3O− + which
B.
C.
×510
A. 1OH
C.86 H
NH−7−
+
A.
C.
O
30. In a titration, which of the following has a pH = 7.00
B. NH
C.4626H
H
NH
D.
2H
10 −−43HNO3
3×55and
A.
C
NH
22. The conjugate
acid of C6 H 5NH 2 is
(1 mark)
+
+
D.
H
O
B.
C
B.
and
C. KOH
C636H
H55NH
NH32HCN
A. NH 3 and HNO3
−++
A.
C.
C
H
NH
C.
NaOH
and
HCl
6
5
D.
C
H
NH
23acid of C H NH is
22. 22. The conjugate
(1 mark)
6 5
6 5
2
B. KOH and HCN
+
B.
C
H
NH
5 ) 3and CH 3COOH
Ca
OH
D.a titration,
C66(H
5 NH
3
2which
30. D.
In
of the following has a pH = 7.00 atC.the NaOH
equivalence
point?
(1 mark)
and HCl
A. C6 H 5NH 2−+
C.
22. The
conjugate
acid
of C6 H 5NH 2 is
D. Ca(OH)2 and CH 3COOH (1 mark)
A.
+
B. NH
C6H
H3 5and
NH 3HNO
3
D.
C
NH
23.
31.
23.
23. 23.
23.
31.
23.
24.
24. 24.
24.
24.
24.
6
5
3
− +HCN
Which
is a property of 1.0 M HCl but not a property
B.
KOH
andfollowing
C.
C6of
H 5the
NH
2
A.
C
H
NH
6
5
Which
of
the
following
salts
dissolves to produce a basic solution?
(1
COOH
(1mark)
mark)
of 1.0 M
Which
of CH
theand
+ HCl ? is a property of 1.0 M HCl but not a property
3following
C.
D. NaOH
B.
C66H 55NH
33
(1 mark)
of 1.KCl
0 M CH 3COOH ?
A.
31. Which of the following salts dissolves to produce a ba
+ red
A. Ca
turns
litmus
D.
OH
and
CH
COOH
(
)
3
C.
C
H
NH
6 5 22
B.
Which
of4 Br
the
following
A.
turns
litmus
red is a property of 1.0 M HCl but not a property
B. NH
ionizes
completely
+
A. KCl
D.
C
H
NH
6( NO
5 )3COOH
3
M
CH
?
(1 mark)
of
1.0ionizes
C.
B.
3completely
3 less than 7.0
C. Fe
has
a pH
B. NH 4 Br
+
C.
has
less
7.0a property of 1.0 M HCl but not a property
D.
COO
Which
ofa the
following
is
D. LiCH
produces
H 3red
Othan
in solution
A.
turns
litmus
3pH
C.solution?
Fe( NO3 )3
+
Which
of CH
the 3following
dissolves to produce a basic
(1
COOH
(1mark)
mark)
of
0M
D.
H 3O in? salts
solution
B. 1.produces
ionizes
completely
D. LiCH3COO
C.
a litmus
pH lessred
than 7.0
A.
KCl
A. has
turns
Which
of the
following
is a property of 1.0 M HCl but not a property
+
B.
NH
Br completely
D.
H
O
in
solution
B. 1.0produces
ionizes
M 4CH
COOH
?
(1 mark)
of
3
3
−
−
In
a
1
.
0
M
HF
solution,
the
concentration
of
HF
,
F
,
and
OH
,
C.
Fe( NO
C. has
a pH
3 )3 less than 7.0
A.
red isthe concentration of HF, F − , and OH − ,
In
a 1turns
.highest
0 M litmus
HFtosolution,
from
lowest
(2 marks)
- 10 D.
LiCH3COO
D. produces
H 3O + in solution
from
highestcompletely
to lowest is
(2 marks)
B. ionizes
−
−
> Fless>than
A. has
OH7.0
[HF
C.
a] pH
- 10 −
In
0M
HFF −solution,
the
concentration of HF, F − , and OH − ,
>
>
A. a 1[.HF
OH
]
+
−
−
D.
Hlowest
from
highest
issolution
(2 marks)
B. produces
F > [to
HF
OH
3]O> in
−
B. F −> [HF] > OH −−
C.a 1.OH
> [−solution,
HF] > F−the concentration of HF, F − , and OH − ,
In
0 M− >HF
> >OH
A.
HF
F
[
]
C. highest
OH >to[HF
F−
] is
from
lowest
(2 marks)
−
−
> F > [HF
D. OH
−
−]
10
B. OH
F −> >
[HFF]− > >OH
D.
[HF− ]
−
In
a
1
.
0
M
HF
concentration of HF, F − , and OH − ,
> OHthe
A. [HF]− > Fsolution,
C. OH > [HF] > F −
from highest
to lowest is −
(2 marks)
−
[
[
[
[
[
[[
[
[ ] [
] [ ] [[
]
[
][ ] [ [
]
[
]
[
]
]] [ ][
][ ] [[
]
]]
]
]
]]
]
]]
+
−
++ H 2 O → H 3O ++ Cl
B.
D. 2HCl
NH
+ H22HO2 →
H 24O →
+ OH23O + NH 3
A.
25. In which of the following +reactions− is water behaving as a Brønsted-Lowry acid?
−
C. HCl
NH 3 ++ HH 2OO →
→H
NHO4+ ++ Cl
OH
B.
2
(1 mark)
3
+
+
25. 25. In
D.
NH
H2O
O→
H23O
+ NH
→
+NH
O
A.which
2 H 24O
+reactions
− is
of++
the
following
2H
3 water behaving as a Brønsted-Lowry acid?
2→
C.
NH
H
3
2
4 + OH
+
−
B. HCl ++ H 2 O− → H 3O ++ Cl
+
+OH
H22H
O2 →
O + NH
H the
+ aH
Osolution
A. NH
2is
of
with
= 9.3 × 10 −2 M ?
26. D.
What
3 H 3O
24O →
23 +
−
C. NH + H O → NH + OH
B. HCl3 + H 22O → H 3O4+ + Cl −
+
+
D.
H−16
→aHsolution
+ NH
A. NH
9is.3the
10
+
− 3 H O + = 9.3 × 10 −2 M ?
4× +
2−OMof
3O
with
26. What
OH
C. NH
+
H
O
→
NH
+
OH
3
3
2
4
B. 8.6 +× 10 −13 M
− → H O + + NH
+
−2
D. NH
H−16
4 +OH
2 O of
3
3
26. What
is
the
13
C. 91.31 × 10 M a solution with H 3O = 9.3 × 10 M ?
A.
2
13
D. 89.63 × 10−−16
B.
M
−M
+
A.
9
.
3
×
10
= 9.3 × 10 −2 M ?
26. 26. What is the OH
−13 of a solution with H 3O
C. 1.1 × 10 M
B. 8.6 × 10 −−13
M
2−
+
D. 9is.3the
× 10
= 9.3 × 10 −2 M ?
26. What
OH
−13
16 Mof a solution with H 3O
−
A. 19..13 ×× 10
10 M
M
C.
−−213M
27. D.
The
010
.10
B. pH
MHNO3 is
98..36 of
×× 10
M
A. 9.3 × 10 −−16
M
13
M
C. 1.1 × 10 −13
B.
A. 80..679× 10 −2 M
27. The
.10 MMHNO3 is
D. pH
9.3of× 010
B. 11..100× 10 −13 M
C.
C. pH
26
27. 27. The
of× 010
.10−2MMHNO3 is
D.
901...379
A.
D. 13
00
B.
1..00
01..79
27. A.
The
of 0.10 M HNO3 is
C. pH
26
B.
1
.
00
D. 13.00
27. C.
The
of 0.10 M HNO3 is
10..26
A. pH
79
28. D.
What13is.00
the pOH of a solution made by adding 50.0 mL of 0.50 M NaOH
B. 1.00
to
250.0 mL of water?
A.
C. 01..79
26
B.
1
.
00
is
the pOH of a solution made by adding 50.0 mL of 0.50 M NaOH
28. 28. What
D.
A. 13
0..00
30
C.
to
2501.0.26
mL of water?
B. 131..00
00
D.
28. What
is the pOH of a solution made by adding 50.0 mL of 0.50 M NaOH
C.2500.10..30
08
to
mL of water?
A.
D.
12
.
92
B. is
1.00
28. What
the pOH of a solution made by adding 50.0 mL of 0.50 M NaOH
A.
0
.
30
C.
1
.
08
to 250.0 mL of water?
1is..00
28. B.
What
the pOH of a solution made by adding 50.0 mL of 0.50 M NaOH
D. 12
92
to
mL of water?
C.
A. 25010.0.08
30
29. 29. Which of the following 1.0 M solutions will have the lowest pH ?
D.
B. 121..92
00
A. 0.30
C.
1.08
A. HCl
B.
1of
.00the following 1.0 M solutions will have the lowest pH ?
29. Which
D.
12
.92
B.
HCN
C.
1.08
C. 12
H 3.PO
4 following 1.0 M solutions will have the lowest pH ?
D.
A.
HCl
29. Which
of92the
D. HCN
H 2C2O 4
B.
−
A.
HCl
of4 K
.8 × 10 −7will
. The
value
K a for
30. 30.
C. value
H 3of
POthe
29. The
Which
following
1.0 is
M 4solutions
have
theof
lowest
pHH?2 Te is
b for HTe
B.
HCN
- 10 D. H 2 C 2 O 4
−following
21
29. A.
Which
of
the
1
.
0
M
solutions
will
have the lowest pH ?
C.
H
PO
A. 4HCl
.83 × 10
4
B. H
HCN
D.
B.
.32 C×2 O
104 −13
- 10 A. 2HCl
C. H 3PO 4 −8
C.
2
.
1
×
10
B. HCN
D. H C 2 O 4−7
- 10 C. 4H.832PO
D.
× 10
4
D. H 2 C 2 O 4
- 10 -
[
]
[
]
[
[
]
]
[
[
]
]
[
[
]
]
[
[
]
]
31. In an aqueous solution of NaCl, the pH is
A. less than 7 and the solution is acidic.
- 10 -
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(2 marks)
(2 marks)
(2 marks)
(2 marks)
(2 marks)
(1 mark)
(1 mark)
(1 mark)
(1
(1 mark)
mark)
(1 mark)
(1 mark)
A. 1.4 × 10 − 6 M
B. 3.4 × 10 −5 M
31. 31. In an aqueous−3solution of NaCl, the pH is
C. 2.6 × 10 M
A.
D.
B.
C.
D.
and the solution is acidic.
5less
10 −73 M
.8 ×than
equal to 7 and the solution is neutral.
greater than 7 and the solution is basic.
greater than 7 and the solution is acidic.
32. 21. Which of the following reactions is not a neutralization reaction?
A. KOH + HF → KF + H 2 O
2−
Use
theand
following
for questions
32 and
22. What is the conjugate
acid
what is equation
the conjugate
base of HPO
?33.
4
B. CH 4 + 2 O 2 → CO 2 + 2 H 2 O
C. Ca(OH)2 + 2 HCl → CaCl 2 + 2 H 2 O
Conjugate
Acidthe following
Conjugate Base for the indicator methyl
Consider
22. D.
WhatNa
is 2the
acid and what equation
is the conjugate base of HPO 42− red,
? HInd .
COconjugate
3 + H 2 SO 4 → Na 2 SO 4 + CO 2 + H 2 O
H 2 PO 4−
PO 43−
A.
+
−
HInd + H 2 O →
← H 3O + Ind
2−
33. 22. What isConjugate
3− the
− acid and
Acid
Conjugate
Base
the
conjugate
what
is
conjugate
base
of
HPO
?
4
PO 4
H 2 PO 4
B.
3−
H 2PO
PO 4−
POPO
−
A.
4
H
H
C.
2
3
4
4
Conjugate Acid
Conjugate
Base
3−
−
PO
H
PO
3−
B.
4
PO 44 −
H 32PO
D.
H 2 PO 4
PO 43−4
A.
32. At
be - 7 PO 4− red solutionHwill
C. pH = 4.0H, 2methyl
3 PO
3−4
−
PO 4
H 2 PO 4
B.
3−
−
PO
H
PO
D.
A. red and [3HInd4 −] > Ind
4
H 3PO 4
H 2 PO 4
C.
−
B.
red
and
HInd
<
Ind
[
]
23. Which of the following would be the 3−
same when comparing equal volumes
PO
H
PO
D.
3
4
4
of 1.0 M HBr and 1.0 M CH 3COOH?
C. yellow and [HInd ] > Ind −
[
[
34. 23.
(1 mark)
]
]
[ ]
A.
Which
ofpH
theand
following
D. the
yellow
< [Ind be] the same when comparing equal volumes
[HInd] would
(1 mark)
(2 marks)
(2 marks)
(2 marks)
OVER
(2 marks)
(1 mark)
−
of
0 Melectrical
HBr andconductivity
1.0 M CH 3COOH?
B. 1.the
C. the titration curve for reaction with a base
23. Which of the following would be the same when comparing equal volumes
A. the moles
pH of base required for neutralization
D.
of
1.0 M HBr and
1.0 M CH 3COOH?
B. the electrical conductivity
33. Methyl red is orange in a 0.10 M solution of an acid. The acid could be
C.
curve for reaction with a base
A. the
the titration
pH
D.
of base
required for neutralization
A. the
HI moles
B.
the
electrical
conductivity
B. the
HCl
C.
curve for
reactionthe
with
a base
35. 24. Which
oftitration
the following
represents
predominant
reaction
D.
the
moles
of
base
required
for
neutralization
C. HCN
between
NH 3 and H 2 O ?
D. H 2SO 4
→ represents the predominant reaction
24. Which
of3 the
+ Hfollowing
A. NH
2 O ← NH 3O + H 2
between NH 3 and H 2 O ?
- 11 +
−
B. NH 3 + H 2 O →
← NH 4 + OH
24. Which of the following represents the predominant reaction
→
A. NH
NH33NH
H22O
O H→
NH532O+ ++ H
C.
++ H
NH
O22 −
←
between
←
2O ?
3 and
→
++ + OH − −
B. NH
NH33 ++ H
H22O
O →
NH
D.
← H
←
3O4 + NH 2
→
+ H 22 −
A. NH 3 + H 2 O ← NH 3O
2+
C. NH 3 + H 2 O →
← NH 5 + + O −
B. NH 3 + H 2 O →
← NH 4+ + OH −
D. NH 3 + H 2 O →
H 3O + NH 2
←
2+
2−
C. NH 3 + H 2 O →
← NH 5 + O
−
+
D. NH + H O →
← H O + NH
3
2
3
2
(1 mark)
(1 mark)
(1 mark)
(1 mark)
OVER
(1 mark)
(1 mark)
2
3 ←
2
4
4
3
25. Consider the following reaction:
Strongest acid
Strongest base
What is the strongest
base in the above−system? −
− acid and 2strongest
HPO 4 − HSO
+ H32−SO3 →
Hfollowing
A.
← H 2 PO 4 + HSO3
2 PO 4
25.
Consider
the
reaction:
36. 25. Consider the following reaction:
−
HPO 42−
H 2 PO 4acid
B. is Strongest
Strongest
base
2 −strongest
− system? −
What
the strongest
acid
and
base→
in the
above
2
−
HPO
++ H
H
→
2 SO
3 ←
2 PO
4
4− +
HPO
H
SO
H
PO
+ HSO
HSO33 −
←
2
3
2
4
4
−−
−
HSO33
H 22SO
C.
PO34
A.
Strongest
acid
base
What
is the
strongest
acid andStrongest
strongest2−
base in the above system?
What
strongest
HPO 442−base in the above system?
D.
PO34− acid and strongest
B. is the H
22SO
HSO3−−
H 2 PO 4−
A.
HSO3 base
H 2SO3acid
Strongest
C.
Strongest
Strongest
acid
Strongest
base
2−
HPO 4−2−
H 2 PO 4−−
B.
HSO
H
HPO34−
SO
A.
D.
HSO
H222PO
PO434−
A.
−
HSO332−
H 2SO3−
C.
HPO
H
26. When
, the4 2−OH − is
B.
4 − pOH = 5.30
HPO
H22PO
POhas
B. a solution
4
HPO44−2−
H 2SO3
D.
HSO
H
C.
6 33
HSO33 −
H22−SO
SO
C. 5.0 × 10
A.
M
(2
(2 marks)
marks)
[
]
(1 mark)
[
]
(1 mark)
2−
HPO
H
D.
9 has
26. When
, the442−OH − is
H22−SO
SO
D. 2.a0 solution
B.
× 10
M33 pOH = 5.30HPO
C. 0.72 M − 6
× 10 M
37. 26. A.
When5.a0 solution
has pOH = 5.30 , the OH − is
D. 13.27 M −9
B. 2.0 × 10 M
−
A. 05a..72
0 ×M10 − 6 has
M
26.
C.
26. When
When
a solution
solution has pOH
pOH == 55..30
30,, the
the OH
OH − is
is
−9
B. 13
2.0.27×M
10 M
D.
−−66
A.
5
.
0
×
10
M
A.
10
C. 5many
0..072×M
27. How
molesMof HI are needed to prepare 3.0 L of an HI solution
−−99
B.
..00pH
×× 10
M
with
of
B.
10
M?
D. 2a213
.27
M 1.00
[
]
(1 mark)
[
]
(1
(1 mark)
mark)
C.
C. 00..72
72 M
M
A.
0.030
mol
How13
many
moles of HI are needed to prepare 3.0 L of an HI solution
38. 27. D.
.
27
M
D.
13
.
27
M
B. a0.30
with
pHmol
of 1.00 ?
C. 3.0 mol
27. D.
How many
moles of HI are needed to prepare 3.0 L of an HI solution
molmol
A. 30
0.030
with a pH of 1.00 ?
B. 0.30 mol
27.
many
moles
of HI are needed to prepare 3.0 L of an HI solution
C.
mol
27. How
How
moles
A. 3many
0..0030
mol of HI are needed to prepare 3.0 L of an HI solution
with
a
pH
of
1
.
00
with
of 1.00 ??
D.
mol
B. a30
0.pH
30
mol
C. 3.of
0 mol
the following 1.0 × 10 −3 M solutions has a pH of 3.0 ?
39. 28. Which
A.
A. 00..030
030 mol
mol
D. 030
mol
B.
.
30
mol
B. HCl
0.30 mol
A.
C.
3
..00 mol
C. 3HCN
mol
B.
28. D.
Which
of
the following 1.0 × 10 −3 M solutions has a pH of 3.0 ?
30
mol
D.
30
mol
C. NaOH
D.
A. K
HCl
2 SO 4
28. Which of the following 1.0 × 10 −3 M solutions has a pH of 3.0 ?
B. HCN
40. 29. Which
of the following expressions shows the relationship
C.
NaOH
between
A. HClK a and K b for a conjugate
−−33 pair? - 9 28.
of
the
following
11..00 ×× 10
M
28. Which
Which
of
the
following
10
M solutions
solutions has
has aa pH
pH of
of 33..00??
D.
K
SO
2
4
B. HCN
A.
a × K b = 14
C. K
NaOH
A.
A. HCl
HCl
B.
+K
= 14
D. K
Ka2SO
-94 b
B.
B. HCN
HCN
C. NaOH
Ka × Kb = Kw
C.
C.
NaOH
D. K
K2aSO
÷ 4K b = K w
D.
-9D.
K
SO
2
(2 marks)
(1 mark)
(1 mark)
(1 mark)
(1
(1 mark)
mark)
(1 mark)
(1 mark)
(1 mark)
OVER
(1 mark)
(1
(1 mark)
mark)
OVER
OVER
4
-- 99 -30. Which of the following will be the most basic?
OVER
OVER
(1 mark)
−
−8 When awill
30. Which
be thecontaining
most basic?
mark)
22.following
solution
Ag + is mixed with a solution containing (1
BrO
3 , the
C. 3.6of×the
10
M
−7
(2 mark
D. 1.3 × 10 − 4 −trial
M ion product is determined to be 2.5 × 10 . What would be observed?
A. 1.0 M NO3
−
+
2containing
−
+ is most
22.
solution
mixed
with since
a solution
A.
A precipitate
would
form
trial containing
ion productBrO
<K
.
30.
Which
will Ag
be the
basic?
(1 mark)
41.
3−sp, the
B. 1.aa0of
Mthe
SOfollowing
22. When
When
solution
4 containing Ag is mixed with a solution containing BrO3 , the
−7
trial
ion product
is
to bewould
2.5 × form
10 −7 since
. What
would
observed?
(2 marks)
marks)
B.determined
A precipitate
trial
ion be
product
>K .
trial
product
(2
C. ion
M NO
CO3 2−is− determined to be 2.5 × 10 . What would be observed?sp
A.
11..00 M
3 C. A precipitate would not form since trial ion product < K .
sp
3 − would form since
−
+
A
precipitate
trial
product
<K
Kcontaining
D.
1
.
0
M
PO
sp ..
22. A.
When
a
solution
containing
Agsince
is mixed
with
a solution
BrO
,
the
A. A
would form
trial ion
ion
product
<
3
B.
1.0precipitate
M SO 442 −D.
sp ion product > K .
A precipitate would not −form
since trial
sp
7
B.
A
precipitate
would
form since
trial
ion
product
> would
K sp . be observed?
trial
ion
product
is
determined
to
be
2
.
5
×
10
.
What
(2 marks)
2
−
B.
A
precipitate
would
form
since
trial
ion
product
>
K
.
sp
C. 1.0 M CO3
C. A precipitate would not form since trial ion product < K sp .
C.
since
product
D.
1.0precipitate
M PO 43− would
A. A
A
precipitate
would not
formform
since
trialtrial
ion ion
product
< K<sp K. sp .
D. A precipitate would not form since trial ion product > K sp .
D.
would not
form
since trial
product
> K. sp .
B. A
A precipitate
precipitate
since
ion ion
product
> Kwhich
42.31. Dissolving
sp
NaCH 3would
COO form
in water
willtrial
produce
a solution
is
(2 marks)
23.
Which
of
the
following
represents
the
complete
neutralization
C. A precipitate would not form since trial ion product < K sp .
(1 mar
of H
A. basic with pH
> 37PO 4 by NaOH?
D. A precipitate would not form since trial ion product > K sp .
B. basic with
pHCOO
< 7 in water will produce a solution which is
31. Dissolving
NaCH
(2 marks)
→ NaH neutralization
A.3 H 3represents
PO 4 + NaOH
PO 4 + H 2 O
23. Which
of
the
following
the
complete
2
C. acidic
with
pH > 7represents the complete neutralization
23. Which
of the
following
(1 mark)
of H 3PO 4 by NaOH?
B.
H 3PO 4 + 3NaOH → Na 3PO 4 + 3H 2 O
A.
basic
with
pH
by
NaOH?
(1 mark)
of
H
PO
D. acidic
3
4 with pH><77
C. < H
B. basic
pH
7 3PO 4 + 2 NaOH → Na 2 HPO 4 + 2 H 2 O
A.
H 3POwith
4 + NaOH → NaH 2 PO 4 + H 2 O
+following
A. acidic
H 3of
POthe
NaOH
NaH
POthe
H 2 ONaH neutralization
C.
pH
73represents
→
+ HPO 4 + H 2 O
D. >H→
PO
4with
4 +complete
43.23. Which
4 +2 NaOH
B.
H
PO
+
3
NaOH
→
Na
PO
+
3
H
O
3
4
3
4
2
(1 mark)
of
PO
B. Hacidic
+NaOH?
3NaOH
3H
4 by
D.
pH < 7→ Na 3PO 4 + 3H 2 O
3 PO
4with
C. H 3PO 4 + 2 NaOH → Na 2 HPO 4 + 2 H 2 O
C. H 3would
PO 4 +produce
Na HPO
O
2 NaOHa →
2 Ha 2pH
4 + at
32. D.
Which
solution
(1 mark)
→yellow
A. H
H33PO
PO44 ++ NaOH
NaOH →
NaH22+
POHPO
NaH
H 2 O = 4.0 ?
4 + 4H+
2O
D. H 3PO 4 + NaOH → NaH + HPO 4 + H 2 O
B.
H 3PO 4 red
+ 3NaOH → Na 3PO 4 + 3H 2 O
A. methyl
2−
conjugate
HBO
is
(1 mar
3O When
C.
H 3PO 424.
NaOH
HPOof
H
+ 2The
→ Na 2base
+
2
25.
equal volumes of 0.10
HNO3 with 0.10 M
B.
methyl
violet
4
32. Which would produce a yellow solution
at a 2pH = 4.0comparing
?
(1 M
mark)
C. indigo
+ NaOH → 2−
D.
H 3PO 4carmine
NaH + HPO 4 + H 2 Owould be observed?
A.
BO
3
2−
D. conjugate
chlorophenol
A.
methyl
redbasered
24. The
of HBO
(1 mark)
3 2− is
3−
A. The pH values would be the same.(1 mark)
base
HBO
is
B. ofBO
B. conjugate
methyl violet
44.24. The
3
3
B. The electrical conductivities would be different.
2− carmine
C.
indigo
C. HBO3 −
A. BO3 2−
The effects on blue litmus paper would be different.
comparing equal D.
volumes
of 0.10 MredHNO3 with 0.10 M HNO2 C.
, what
A.
BO33−
chlorophenol
−
25.
When
comparing
equal
volumes
of
0
10
.
M
HNO
with
10M
M HNO
HNO
what
2−
25.
When
comparing
volumes
0.10 M HNO
..10
,, what
D.33 with
The 00volumes
of 02.210
M NaOH needed
for neutralization
B.
BO
D.
BO
of24.
0.10
M conjugate
HNO
0equal
.10
MHBO
HNO
, of
what
base
ofH
(1 mark)
2volumes
3 3−
3 2 is
dalbevolumes
observed?
(1 HNO
mark)
3 with
25. The
When
comparing
equal
of
0
10
.
M
HNO
with
0
.
10
M
,
what
B.
BO
3
2
would
be
observed?
(1
mark)
would be3 observed?
(1 mark)
−
(1 mark)
C.
HBO
would
be
(1 mark)
3observed?
−
2−
When
comparing
equal volumes of 0.10 M HNO3 with 0.10 M HNO2 , what
45.25.
The pH values
would
beHBO
the
same.
C.
A.
BO
3
−
3
A. H
The
pH values
values would
would be
be the
the same.
same.
A.
The
pH
D.
BO
ouldelectrical
be the same.
2be
3 − values
would
observed?
(1 mark)
The
conductivities
would
be different.
A.
The
pH
would
be
the
same.
3−
B.
The
electrical
conductivities
would be
be26.
different.
D.
H
BO
BO
2 3electrical
3
The
conductivities
would
different.
Consider the equilibrium:
nductivities
be
different.
The
effects onwould
blueB.
litmus
paper
would
be
different.
B.
The
electrical
would
be different.
C. The
The pH
effects
onconductivities
blue litmus
litmus
paper
would
be different.
different.
− values
C.
effects
on
blue
paper
would
be
A.
would
be the
same.
ue
litmus
paper
would
be
different.
C.
HBO
The volumes of 0.10
M
NaOH
needed
for
neutralization
would
be
different.
C.
The
effects
on
blue
litmus
paper
would
be
different.
3
2−
−
D. The
The electrical
volumes of
of
.10
10M
M NaOH
NaOH
needed
for neutralization
neutralization
would be
beHF
different.
→
B.
conductivities
would
be different.
D.
volumes
00.would
needed
for
would
different.
aq ) + HPO 4 ( aq ) ← F ( aq ) + H 2
(
−
0.10 M NaOH needed
for
neutralization
be
different.
D. H
The
volumes
of 0.10 M NaOH needed for
be different.
10different.
-neutralization- 8would
D.
2 BO
3
C. The
effects
on blue litmus paper would-be
D. The volumes of 0.10 M NaOH needed for For
neutralization
would be different.
the above equilibrium,
identify the weaker acid and determ
reactants
or
products
are
favoured.
der the equilibrium:
(2 marks)
26. Consider the equilibrium:
(2 marks)
8 -46.26.
--10
Consider
the
equilibrium:
(2 marks)
um:
(2
marks)
26. Consider the equilibrium:
(2 marks)
-8−
2− − →
−
−
HF( aq ) + HPO 42(−aq ) →
F
+
H
PO
Acid
Side Favoured
←HF( aq( aq
2 42 −( aq
4 ( aq )← F−( aqWeaker
) HPO
4− ( aq )
) +
) + H 2 PO
26. Consider the−equilibrium:
(2 marks)
HF
− )) →
−aq ) + HPO 4 2( aq
→ FF (−aq ) ++ HH2 PO
←
4 (−aq )
(
HF
+
HPO
PO
HF( aq ) + HPO 42(−aq ) →
F
+
H
PO
←
2
←
2
aq
aq
4
aq
4
aq
(
)
(
)
(
)
(
)
aq
4 ( aq )
( )
A.
HF −whether products
− whether
e above equilibrium,
theequilibrium,
weaker acid
and+determine
Foridentify
the above
identify
the 2weaker
-→
8 acid
- F −and determine
HF
HPO
+
H
2 PO 4 whether
aq )
aq )
For
the
above
equilibrium,
acid
and
(identify
( aq ) determine
(whether
( aq ) ←
nts oridentify
productsthe
areweaker
favoured.
reactants
or and
products
are favoured.
For
the acid
above
equilibrium,
identify the
the4weaker
weaker
acid
and
determine
rium,
determine
whether
B.
HF
reactants
reactants
or
products
are
favoured.
reactants or products are favoured.
are favoured.
For the above equilibrium, identify the weaker acid
C. and determine
H 2 PO 4− whether products
Weaker
Acidare favoured.
Side Favoured
Weaker Acid reactants
Side Favoured
or products
Weaker
Side
Weaker Acid
Acid
Side Favoured
Favoured
D.
H 2 PO 4−
reactants
Side Favoured A.
products
HF
productsHF
A.
HF
products
Weaker
Side
Favoured
HFAcid
products
products A.
B.
HF
reactants
HF
reactants
B.
HF
reactants
A.
products
B.
HF −
reactants
reactants
−
C.
H
PO
products
2
4
27. The ionization of water can be represented by
H 2 PO 4
products
−−
C.
H
PO
products
B.
reactants
C.
H22HF
PO44 −
products
products
−
D.
H PO
reactants
A. 2 H 2 O( l ) → 2 H 2( g ) + O2( g )
27. The ionization of water can
be represented by
B. H 2 O( l ) → 2 H +( aq ) + O2(−aq )
47. 27. A.
2 H 2 O( l ) of
→water
2 H 2can
The ionization
by
2 g
( g ) +beOrepresented
C. H 2 O
→( )H 3O( aq ) + OH( aq )
l
(
)
2−
+
B.
2 OO
(l) → 2H
( 2aqg) ++ OO 2( aqg )
A. H
2H
2
H
2 (l) →
(
)
D. 2 H 2 O( l ) →( ) H 3O +( aq ) + OH −( aq )
C. H 2 O( l ) → H 3O+ ( aq ) + OH
( aq )
B. H 2 O( l ) → 2 H ( aq ) + O2(−aq
)
+
−
D.
2
H
O
→
H
O
+
OH
2 (l) → H O
3
( aq+
) OH ( aq )
C. H O
2
(l)
3
( aq )
( aq )
20. The K sp expression for Zn
(OH)2 is −
Calculate+the pOH
of a 0.050 M HBr solution.
D. 2 H 2 O28.
( l ) → H 3O ( aq ) + OH ( aq )
29.
48. 28.
28.
29.
49. 29.
[
[
[
[
][ ]
][ ]
][
]
][
]
(1 mark)
(1 mark)
(1 mark)
2
−
2+
2−
A. K sp =theZnvalue
A. OH
for M
HPO
.
Calculate
pOH
of 0aK.30
0b.050
HBr
4 solution.
B.
1
.
30
2
B. K sp = Zn−22 + OH −
C. of12a.70
A.
Calculate
0.050 M HBr
40.5.30
10 pOH
×the
2− solution.
Calculate the value
.
2 + of K−b for HPO 4
13.70
C.
Zn
−7 D. 2 OH
B.
B. K
1.16sp.30
×= 10
A. 120..70
30 −−227
C.
2
A.
4
5
.
×= 10
C.
2
2
D.
K
Zn 2 + 2 OH −
sp
B.
1
.
30
D. 13.70 −−722
2−
Calculate
B.
..62.70
××the
10
D.
10value of K b for HPO 4 .
C. 1612
-9D. 213
C.
.2.70
× 10 −27
A. 4.5 × 10 −−222
D. 6.2 × 10
B. 1.6 × 10 −7
-9−6
21. The solubility −of
27 CdCO3 is 2.5 × 10 M . Calculate the K sp value for CdCO3 .
C. 2.2of×the
10following is the net ionic equation describing the
30. Which
22
-912
hydrolysis
of
D. 66..32 ×× 10
10−−KCN
( aq ) ?
A.
−6
is the net ionic equation describing the
B. 2.5of×the
10 following
50. 30. Which
+
+
→
+
A.
K
H
O
6 2 ( l ) ?← KOH ( aq ) + H ( aq )
hydrolysis
( aq )
× )of
C. 5.0( aq
10 −KCN
+
−
→
−3
B. 1KCN
D.
.6+ × (10
aq ) + H 2 O( l ) ← K ( aq ) + CN ( aq )
+
30. Which
the following →
is the net ionic equation describing the
A. K of
( aq ) + H 2 O( l ) ←→ KOH( aq ) + H ( aq−)
C. CN −( aqof) +
H2O
?
hydrolysis
KCN
aq + OH ( aq )
( aq( l)) ← HCN
+ ( )
→
B. KCN
+ H 2 O( l ) ← K +( aq ) + CN −( aq− )
− ( aq )
D. CN ( aq ) + H 2 O( l ) →
← 2 H ( aq ) + CNO
+ −
+ − ( aq )
→
→
+
A.
K
H
O
C. CN( aq( aq
HCN
2 2O
( l )( l ) ←← KOH
) ) + H
( aq( aq
) )++HOH
( aq )( aq )
22. At 25°C , what is the Cl − →in a saturated
solution
of PbCl 2 ?
+
− −
→
B.
++ CN
D. KCN
CN −( aq
H +((aq
CNO
← 2K
aq
( aq) ) ++ HH22OO( l()l ) ←
)
(
)
aq )
( aq )
[ ]
−
−
−2
C. 1CN
H 2 O( l ) →
A.
.4 ×( aq10
← HCN ( aq ) + OH ( aq )
) +M
51. 31. Which of− the −following
1.0 M salt+ solutions will
be acidic?
−
B.
.3 × 10 +2 M
→
D. 2CN
H
O
2
H
+
CNO
2 (l) ←
( aq )
( aq )
( aq )
C.
.9 × 10 −2 M
A. 2NaNO
3
31. Which of the following
1.0 M salt solutions will be acidic?
−2
D.
4
6
10
.
×
B. NaHCO3 M
C. NaNO
NaHSO
A.
3 4
D. NaHCO
NaHPO
31. Which
of the 43following 1.0 M salt solutions will be acidic?
B.
C. NaHSO 4
A. property
NaNO3 common to both 0.10 M HCl and 0.10 M NaOH is that
52. 23. The
D. NaHPO
4
both
B. solutions
NaHCO3
C. pH
NaHSO
32. A.
The
which
an indicator changes colour is known as its
4
tasteatbitter.
D.
NaHPO
4 > 7 .
B. have a pH
A. standard point.
C. pH
conduct
electricity.
32. The
at which
an indicator changes colour is known as its
B. transition
point.
D. react with magnesium to produce hydrogen gas.
C. equivalence point.
A. standard point.
D. stoichiometric point.
B. pH
transition
point.
32. The
at which
an indicator changes colour is known as its
C. equivalence point.
D. standard
stoichiometric
A.
point. point.
(1 mark)
mark)
(1
(1 mark)
(1 mark)
(1 mark)
OVER
(1 mark)
OVER
(1 mark)
(1 mark)
(1 mark)
(2 marks)
(2 marks)
(2 marks)
(2 marks)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 m
6 5
2 (l) ←
2 ( aq )
24. Consider the following Brønsted-Lowry equilibrium:
6
5
3 ( aq )
( aq )
The substances acting as acids and bases from left to right are
+
−
C6 H 5NH 2( aq ) + H 2 O( l ) →
← C6 H 5NH 3 ( aq ) + OH ( aq )
53. 24. Consider the following Brønsted-Lowry
equilibrium:
A. acid, base, acid, base.
B. substances
acid, base, base,
The
actingacid.
asCacids
and bases
from left→
to right are +
−
H NH
2 ( aq ) + H 2 O( l ) ← C 6 H 5 NH 3 ( aq ) + OH ( aq )
C. base, acid, acid, base.6 5
A. base,
acid, base,
acid, base.
D.
acid, base,
acid.
The
actingacid.
as acids and bases from left to right are
B. substances
acid, base, base,
C. base, acid, acid, base.
A. acid, base, acid, base.
D. base, acid, base, acid.
B. acid, base, base, acid.
C. base,the
acid,
acid, base.
25. Consider
following
equilibrium:
D. base, acid, base, acid.
−
−
H 2 C 2 O 4( aq ) + HPO 42(−aq ) →
← HC 2 O 4 ( aq ) + H 2 PO 4 ( aq )
54. 25. Consider the following equilibrium:
In the above equilibrium, a conjugate pair is 2 −
−
−
H 2 C 2 O 4( aq ) + HPO 4 ( aq ) →
← HC 2 O 4 ( aq ) + H 2 PO 4 ( aq )
25. Consider the following equilibrium:
A. HPO 42 − and HC 2 O 4−
In the above
equilibrium, a conjugate pair is 2 −
−
−
→
B. HPO 42 − and H 2 POH4−2 C 2 O 4( aq ) + HPO 4 ( aq ) ← HC 2 O 4 ( aq ) + H 2 PO 4 ( aq )
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
2−−
2−
C.
HPO
A. H
HPO
2 C 24O 4 and HC
44
2O
In the above equilibrium, a conjugate pair is
−−
2−
D.
B. H
HPO
2 C 24O 4 and H 22PO 44
−
2−
A. H
HPO
2 O2−
4
C.
C 4O and
and HC
HPO
2
2
4
4
2−
B. H
HPO
and H 2 PO 4−−
4
D.
2 C 2 O 4 and H 2 PO 4
C. H 2 C 2 O 4 and HPO 42−
, H 2SO3 and H 3PO 4 from the weakest to
55. 26. The strength of the acids HCl
D. H 2 C 2 O 4 and H 2 PO 4−
strongest is
(1 mark)
26. The
acids HCl, H 2SO3 and H 3PO 4 from the weakest to
A. strength
HCl , H 3of
POthe
4 , H 2 SO3
strongest
B. HCl ,isH SO , H PO
(1 mark)
2
3
3
4
26. C.
The
HCl, H 2SO3 and H 3PO 4 from the weakest to
H
H 3the
POacids
2 SO
3 , of
4 , HCl
A. strength
HCl
,H
3 PO 4 , H 2 SO3
strongest
is4 , H 2SO3 , HCl
D.
3 PO
B. H
HCl
,H
2 SO3 , H 3 PO 4
C. H
, HCl3
HCl
,the
PO
2 SO
3H,3H
3 PO
4 , 4H 2 SO
56. 27. A.
Consider
following
equilibrium at 25°C :
D.
H
PO
,
H
SO
,
HCl
B. HCl
3 , 4H 2 SO
23, H
3 3 PO 4
+
−
2 H 2 O( l ) →
C. H 2SO3 , H 3PO 4 , HCl
← H 3O ( aq ) + OH ( aq )
D. H 3PO 4 , H 2SO3 , HCl
What happens to OH − and pH as 0.1 M HCl is added?
[
A.
B.
C.
D.
[OH
[OH
[OH
[OH
−
−
−
−
7.0
(2 marks)
]
] decreases and pH increases.
] decreases and pH decreases.
] increases and pH increases.
] increases and pH decreases.
- 10 - 10 -
- 10 28. What is the value of the ionization constant for water at 25°C ?
A.
(1 mark)
(1 mark)
28. What is the value of the ionization constant for water at 25°C ?
(1 mark)
A. 7.0
57. 28. B.
What14is.0the value of the ionization constant for water at 25°C ?
(1 mark)
−7
C. 1.0 × 10
A. 7.0
D.
.0 .0× 10 −14
B. 114
C. 1.0 × 10 −7
D. 1.0 × 10 −14
58. 29. Which of the following equations represents the dissociation of Sr( NO3 )2
in water?
(1 mark)
30. What is the equilibrium constant expression representing the predominant reaction
(2 marks)
for
the hydrolysis
of NaHCO
−
2 +equations
3( aq ) ?
29. A.
Which
following
represents
the dissociation of Sr( NO3 )2
Sr(of
NOthe
3 )2 ( s ) → Sr ( aq ) + 6 NO ( aq )
30. What is the equilibrium constant expression representing
predominant re
in water?
(1 the
mark)
−
2−+
+
hydrolysis of NaHCO3( aq ) ?
B.
Sr ( aq ) + 2for
NOthe
s ) →OH
A. Sr
K w( NO
= 3H)23(O
3 ( aq )
−
2+
→ 2Sr
A. Sr
Sr(NO
+ ) + 6 NO −( aq )
C.
Sr (2(aq
( NO33))22( s( s) ) →
aq ) + NO3 ( aq )
+
−
+
A. K
OH −
− w = H 3O
+
2
Na
HCO
2−
→
+
2
B.
Sr
NO
Sr
NO
+
2
3
(
)
3
2
s
( aq ) + ( NO3 )3 ( aq )
D.
(NO
B. Sr
K eq
= 3 )2( s( ) ) → Sr ( aq
)
2 ( aq )
NaHCO
2+
3
C. Sr( NO3 )2( s ) → 2Sr ( aq ) + NO3 −( aq )
Na + HCO3 −
59. 30. What is the equilibrium
B.expression
K2 − = representing the predominant reaction
−
2constant
O + ofCO
D. theSrhydrolysis
NOH
Sr32(+aq ) + ( NO?3 )2 eq( aq )
(
NaHCO3
3 )32 ( s ) →
(2 marks)
for
NaHCO
3( aq )
C. K a =
−
HCO3
H 3O + CO3 2 −
A. K w = H 3O + OH − −
C. K a =
H 2 CO3 OH
HCO3 −
D. K b =
−
HCO
3
+
Na HCO3 −
H 2 CO3 OH −
B. K eq =
D. K b =
NaHCO3
HCO −
[
][
]
[ ][ ]
[ ][
]
[
]
[ ][
]
[ ][
]
[
]
[
]
[ ][
]
[[ ][][ ] ]
[
]
[ [ ][ ] ]
[
][ ]
[
]
[
]
O ][CO salt] solutions will be neutral?
[Hfollowing
OVER
Which of the
(1 mark)
C. K =
11
[HCO
]
Cl An Arrhenius base is defined as a substance that
A. 1.0 M NH23.
31. Which of the following salt solutions will be neutral?
OVER
B. 1.0 M [LiClO
H CO ] [OH ]
D.
K
=
11
A.
releases
H
CHCO
O is defined asA.
C. Arrhenius
1.0 M K base
1( .0)M NH
An
a substance
thatCl
(1 mark)
[
]
D. 1.0 M NaHCO B. releases
B.OH1.0 M LiClO
3
60. 31.
+
3
3
a
3
2−
−
4
43
2
23.
b
2
−
2
4
3
+
3
−
+
aq
−
( aq )
(1
4
4
1.0 M K 2 C 2 O 4
A. releases H ( aq ) C. acceptsC.a proton
23.
An
Arrhenius
base
is
defined
as
a
substance
that
(1 mark)
61.
D. 1.0 M NaHCO
3
B. releases OH −( aqD.
donates
a
proton
)
31. Which of the following
salt solutions will be neutral?
(1 mark)
+
C. releases
accepts aHproton
A.
aq
(
)
32. The chemical indicator bromthymol blue changes from yellow to blue as a result of
−
A.
1.0 M NH
4 Cl
B.
releases
D. addition
donates
aOH
proton
the
of
(1 mark)
( aq )
B. 1.0 M LiClO 4
32. The chemical indicator
bromthymol blue changes from yellow to blue as a re
C.
acceptsHCl
a proton
2−
A.
of HAsO
(1
M K 2 C24.
C. 11..00 M
2 O 4 The conjugate
the acid
addition
of 4 is
D.
donates
a
proton
.
M
HNO
B.
1
0
D. 1.0 M NaHCO
2 3
3−
C. 1.0 M K 2 CO3 A. AsO2−
4 A. 1.0 M HCl
conjugate acid of HAsO
is
(1 mark)
62. 24. The
B. 1.0 M HNO2
D. 1.0 M NH 4 Cl B. AsO4 42−
C. 1.0 M K 2 CO3
C. H 2 AsO 4−
A. AsO 43−
2−D. 1.0 M NH Cl
24.
acid of HAsO
is2− blue changes
(1 mark)
32. The conjugate
chemical
bromthymol
4 from yellow to blue as a result of
2− indicator
4
D.
H
AsO
B. AsO 4
2
4
the addition of
(1 mark)
−
3−
C.chemical
H 2 AsO
A.
AsO
4
33. A
has a K a = 1.0 × 10 −6 . Determine the identity of this
4 indicator
A. 1.0 M2−HCl
indicator.
(1 mark)
D. H 2 AsO 42−
B.
.0 M4 HNO
B. 1AsO
26. Consider the equilibrium:
−
C6 H 5COOH + NO2 − →
← HNO2 + C6 H 5COO
−
63. 25. Which of the following will have the greatest electrical conductivity?
(1
mark)
C6 H 5COOH + NO2 − →
HNO
2 + C 6 H 5COO
Identify the stronger acid and predict whether reactants or products
are favoured. ←
A. 1.0 M HF
Identify the stronger acid and predict whether reactants or products are fav
Acid
Side Favoured
B. 1.0 M Stronger
HBr
C. 1.0 M HCN
Stronger Acid
Side Favoured (2 marks)
reactants
A.
HNO2
26. Consider
the equilibrium:
D. 1.0 M H 2SO3
reactants
A. products HNO2
B.
HNO2
−
+
C6 H 5COOH + NO2 − →
HNO
C
H
COO
←
2
6 5
the equilibrium:
64. 26. Consider
products (2 marks)
B. reactants HNO2
C.
C6 H 5COOH
Identify the stronger acid and predict whether− reactants
or products are favoured.
→
products
HNO2 + C6 H 5COO −reactants
C. + NO
H 5COOH
D.
C6 H 5COOHC6 H 5COOH
2 C 6←
products
D.
C6 H 5COOH
Favoured
Identify theStronger
strongerAcid
acid and predictSide
whether
reactants or products are favoured.
reactants
HNO2
Stronger
Acid
Side Favouredexpression for
27. Which
of the
following
products
B.
HNO2 represents the equilibrium
the ionization of water?
(1 mark)
reactants
A.
HNO2
27. Whichreactants
of the following represents the equilibrium expression for
C.
C6 H 5COOH
the ionization
+
−
productsof water?
A.
OH
B. K w = H 3O
HNO
2
products
D.
C6 H 5COOH
+
C.
C6 H 5COOH
A. Kreactants
OH −
w = H 3O
1
products
B.
D. K w = C6 H 5+COOH−
H 3O OH
1
B. K w =
+
expression
65. 27. Which of the following represents the equilibrium
H 3O OH − for
the
(1 mark)
C. ionization
K w = H 3of
O +water?
+ OH −
OVER
9
+
27. Which
the equilibrium
K w = H 3O +expression
+ OH − for
A. K wof=theHfollowing
OH −representsC.
3O
the ionization
(1 mark)
H 3of
O +water?
OH −
D. K w =
[H+ 12OOH
] −
A. K w = H 3O
H 3O + OH −
B. K w =
D. K w =
H 3O + OH −
[ H 2 O]
A.
[
][
]
[
][
]
[
[
[
[
[
] [ ]
][ ]
][ ]
][ ]
][ ]
[
][
]
[
][
]
[
] [
[
][
]
]
1
B. K w =
−
+
C. K w = the
H 3pH
O of+OH
66. 28. Determine
3.OH
0 M− KOH .
(2 marks)
28. Determine the pH of 3.0 M KOH .
A.
0.48
− −
++
H
O
OH
C.
K
=
H
O
+
OH
w
33
B.
D. 11
K w.00=
A. 0.48
[ H 2 O]
C. 13.52
B. 11.00
D. 14.48 H O + OH −
3
C. 13.52
D. K w =
are analyzed
K a values
67. 29. Four acids
[H2O] and their D.
14.48 are determined. Which of the
following values represents the strongest acid?
28. Determine the pH of 3.0 M KOH .
(1 mark)
(2 marks)
[
]][ [ ] ]
[
]][ [ ] ]
[
][
]
A. K a = 2.2 × 10 −13
A.
0.48
28. Determine
of−83.0 M KOH .
= the
6.2 pH
× 10
B.
K
B. 11a.00
C. 13
= 1.7 × 10 −5
K a.52
A.
0.48
D.
14
48
= 1.2 × 10 −2
D. 11
K a..00
B.
C. 13.52
D. 14.48
(2 marks)
- 10 -
- 10 -
30. The dissociation of NH 4 NO3 is represented by
C. No precipitate forms because the trial ion product > K sp
D.
forms +because the −trial ion product < K sp
A. No
NHprecipitate
4 NO3( s ) → NH 4 ( aq ) + NO3 ( aq )
of NH 4 NO3 is represented by
68. 30. The dissociation
B. NH 4+( aq ) + NO3 −( aq ) → NH 4 NO3( s )
−
→ NH +( aq ) + NO
A. NH 4 NO
)
C. NH 4+( aq )3(+s ) H 2 O( l ) 4→
H 3O +( aq )3 (+aqNH
3( aq )
+
−
B.
NH
+
NO
→
NH
NO
3( s )can −exist in 1.0 L
aq ) maximum
3 ( aq ) [ Na 2 CO43 ] that
22. Determine
D. NO43 −((the
aq ) + H 2 O( l ) → HNO3( aq ) + OH ( aq )
+
of
a precipitate.
C. 0.0010
NH 4+M
+( NO
H 2 O3 ()l2) without
→ H 3Oforming
3( aq )
( aq ) + NH
( aq )Ba
(1 mark)
(1 mark)
(1 mark)
D. NO − ) −+
H O → HNO3( aq ) + OH −( aq )
A. 2.6 3×( aq
10 12 M2 ( l )
B. 2.6 × 10 −9 M
(NO3 )3 will be
69. 31. A solution of −Al
C. 2.6 × 10 6 M
31.
24.
70. 23.
24.
71. 24.
25.
72. 25.
25.
(1 mark)
D.
5.1 × 10 −5 M
A. basic.
A
(1 mark)
B.solution
acidic.of Al( NO3 )3 will be
C. neutral.
A.
D. basic.
amphiprotic.
Which
of the following represents the reaction of H 2 PO 4− acting as an acid?
(1 mark)
B. acidic.
A
acid is defined as a substance that
(1 mark)
C.Brønsted-Lowry
neutral.
−
−
→
D. H
amphiprotic.
A.
2 PO 4 + H 2 O ← H 3 PO 4 + OH
24. Which of the following represents the reaction of H 2 PO 4− acting as an acid?
A. releases− H +( aq )
+
B. H 2 PO 4 + H−2 O →
← H 3O + H 3PO 4
B. releases OH ( aq )
−
+ H PO − 2+− H O → −H PO + OH −
← 4 acting
+ H2O →
+2 HPO
C.
H 2of
PO
HA.
3
4 as an acid?
4 4
Which
the
represents
reaction
of2 H 2 PO
(1 mark)
←
3O the
4 following
C. accepts a proton
−
+
−
− O → H O + H PO
+H
B.4 POH42+PO
←
2H2O →
+ 42OH
D.
2
3
3
4
← H
2 PO 4 − a+proton
D. H
donates
−
→
A. H 2 PO 4 + H 2 O ← H 3PO 4 + OH−
2−
+
→
C. H
2 PO 4 + H 2 O ← −H 3O + HPO 4
Which of the
represents
(1 mark)
− following→
+ the reaction of H 2 PO 4 acting as an acid?
B. H 2 PO 4 + H 2 O ← H 3O + H 3PO
− 4
+
−
→
D. H 2 PO 4 + 2 H 2 O ← H 4 PO 4 + 2OH
−−
2−
+
→
→
+
C.
H
PO
H
O
H
A. H22 PO44 + H22 O ←
OH4−
← H33OPO 4+ +HPO
Consider the−−following equilibrium:
(1 mark)
+ + + 2OH −
→
OVER
D.
B. HH22PO
PO44 ++ 2HH22OO →
← HH34OPO+
4 H 3 PO 4
←
-9−
→
2 −H BO − + H S
+BO
→
+
H
←
3
3
2
2
3
+
C. H 2 PO 4− + H 2 O HS
H
O
HPO
←
3
4
25. Consider the following equilibrium:
−
2 H 2 Oas →
D. two
H 2 PO
H 4 PO 4+ + 2bases
OH − in the above equilibrium are
←
4 + acting
The
species
Brønsted-Lowry
−
HS− + H 3BO3 →
← H 2 BO3 +(1Hmark)
2 S OVER
Consider− the following equilibrium:
- 11 A. HS and H 2S
The two species acting as
− Brønsted-Lowry bases in the above equilibrium are
B. H 3BO3 and H 2S HS− + H 3BO3 →
← H 2 BO3 + H 2S
OVER
− equilibrium: −
− the following
11
Consider
(1
mark)
C. HS and H 2 BO3
A. HS and H 2S
The two species acting as−Brønsted-Lowry bases in the above equilibrium are
D. H 3BO3 and H 2 BO3 − B. H 3BO3→
and HH 2BO
S − +H S
HS + H 3BO3 ←
2
2
3
−
A. HS and H 2S
C. HS− and H 2 BO3 −
The two
species
bases
the− above equilibrium are
B.
H BO
and acting
H S as Brønsted-Lowry
D. H BO and
H in
BO
3
HS−−
3
2
3
3
2
3
−
C.
and
BO
A. the
HSbases
andCHH2O
S 2−3 , NH , and PO 3− in order from strongest to weakest.
(1 mark)
73. 26. List
22 4
3
4
D. H 3BO3 and H 2 BO3 −
B. H 3BO3 and H 2S
3−
> NH
> C− 2 O 42 −
A.
C. PO
HS4− and
H 23BO
3 26. List the bases C O 2− , NH , and PO 3− in order from strongest to weakest.
2 4
3
4
2−
3−
−4
B.
C
O
>
NH
>
PO
2
3
4
D. H 3BO3 and H 2 BO3
−
C. NH 3 > PO 43− 2−
> C 2 O 42 −A. PO 433−
> NH 3 > C 2 O 42 −
26. List the bases C 2 O 4 , NH 3 , and PO 4 in order from strongest to weakest.
(1 mark)
D. PO 43− > C 2 O 42 − > NH 3B. C 2 O 42 − > NH 3 > PO 43−
A. PO 43− > NH 3 > C 2 O 42 −C. NH 3 > PO 43− > C 2 O 42 −
26. List the bases C O 2− , NH , and PO 3− in order from strongest to weakest.
(1 mark)
[ ] in 0.025 M HNO ?
[ ]
[ ]
A.
C. [H
HO
O ] is
is not
lesspresent
than [OH ] A. 4.0 × 10 M
A basic solution
can be defined
in which
B.
[OH[OH
] B.as]one0.025
D. [H
HO
O ] is
is equal
greatertothan
M
C.
than [OH ] C. 1.60 M
A. [H
HO
O ] is
is less
not present
D.
is greater
equal tothan
B. [H
HO
O ] is
[OH[OH] D.] 12.40 M
C. H O is less than [OH ]
What[is the ][H O ] in 0.025
M HNO ?
D. [H O ] is greater than [OH ]
29. Write the base ionization constant expression for
A. 4.0 × 10 M
What is the [H O ] in 0.025 M HNO ?
B. 0.025 M
→
27. A basic solution
can be defined
oneisinthe
which
28. as
What
H 3O
B. H 3O + is equal to OH −
74. 27.
33
33
33
33
28.
3
3
75. 28.
++
−
++
−
−
++
−
3
+
−13
3
−13
−
−
+
−
+
(1 mark)
3
3
NH 3( aq ) + H 2 O( l )
C. 1.60 M
A. 4.0 × 10 −13 M+
28. D.
What12is.40
theM H O in 0.025 M HNO3 ?
B. 0.025 M 3
[
(1 mark)
−
++
+
(1 mark)
3
←
]
[NH3 ]
C. 1.60 M −13
A. K b =
A. 4.0 × 10 M
NH 4+ OH −
D. 12.40 M
B. 0.025 M
76. 29. Write the base ionization constant expression for
C. 1.60 M
NH 4+ OH −
B. K b =
D. 12.40 M
NH 3( aq ) + H 2 O( l ) →
NH3 ]4+ ( aq ) + OH −( aq )
← [ NH
29. Write the base ionization constant expression for
[
][
]
[
][
]
[NH3 ][H2+O]
−
C.
KOb = →
+
NH
H
− ) + OH ( aq )
← +NHOH
2
NH
l
(
)
3( aq )
4 ( aq
[
3]
NH
4
29. A.
WriteKthe
constant expression for
b =base ionization
NH 4+ OH −
[
][
]
[
][
]
[
][
]
+−
−
→
NH 3( aq ) + H 2 O( l ) NH
OH
← 4+NH
4 ( aq ) + OH ( aq )
−
K b = of NH NO can be represented by
D.hydrolysis
A. equation
K b = NH
−
30. The
for4+theOH
predominant
[NH3 ][H4 2O]3
B. K b = NH 4 OH
[NH3 ]
+
−
A. NH 4 NO3( s[)NH→
3 ] NH 4 ( aq ) + NO3 ( aq )
A. equation
K b = for++the←
−−
77. 30. The
predominant
hydrolysis
of NH 4 NO3 can be represented by
NH
OH
44
NH
OH
+
+
NH
H
O
→
[ 3H][2O2(l)] ← H3O ( aq ) + NH3( aq )
B.
NH
b =
4 ( aq ) +NH
C. K
K
b =
[ + →3OH
] − + + NO −
A. NH 4 NO
4) ← NH
− NH
−
s
3
(
4 ( aqHNO
3 ( aq )
)
C. NO3 ( aq ) + +H 2 O( l )− →
←
3( aq ) + OH ( aq )
NH
OH
4
+
→ H O + + + NH
B.
H 2HO2(O
B. NH
K b 4=NO
−
NH
3
[
l ) ]O ← →
3( aq )
( aq )
( aq
) + NH
3+] [+
D.
NH
H
- 11 2− ( l ) ← H 3O ( aq ) + NH 3 NO3 ( aq )
C. K b =4 NH
3( aq
[
]
)
3
OH
+
−
− NH 4
−
→ HNO
K b 3=( aq ) +4 H 2OH
D. NO
C.
O
3( aq ) + OH ( aq )
[NH3 ][H2(Ol) ] ←
−
+
[NH ][H O] →
D.
C. NH
K b 4=NO3( aq+3)+ + H2 2−−O( l ) ← H 3O ( aq ) + NH 3NO3 ( aq )
NH
NH44 OH
OH
D. K b =
] soda (NaHCO3 ) has an amphiprotic anion which is
[NH3from
][H2Obaking
78. 31. A solution made
[[
[NH
3]
+
]][[
]]
[
[
[
[[
][
][
][
]][[
]
]
]
]]
[
][
]
[
][
]
NH 4+ OH −
A.
basic
since
Ka < Kb
D. K b =
NH 3from
] soda (NaHCO3 ) has an amphiprotic anion which is
[
][H Obaking
31. A solution made
B. basic since K a >2 K b
- 11 C.
acidic
since
K
<
K
A. basic since K a a < K b b
D. basic
acidicsince
sinceKK a >>KK b
B.
a
b
- 11 C. acidic since K a < K b
D. acidic since K a > K b
32. A chemical indicator in solution consists of
A. a weak acid and its conjugate acid.
- 11 -
(1 mark)
+ OH −( aq )
NH 4+ ( aq )
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(2 marks)
OVER
(2 marks)
OVER
OVER
(1 mark)
23. Which of the following represents the neutralization reaction
between Ca(OH)2( s ) and HCl( aq ) ?
(1 mark)
79. 23. Which of the following represents the neutralization reaction
+
A.
H 2 OCa
between
OHH)2((saq
HCl( aq ) ?
( l ) ($
) + OH
) and
25.
80. 24.
24.
25.
81. 25.
26.
(1 mark)
B. Ca 2(+aq ) + 2Cl -( aq ) $ CaCl 2( s )
A. H 2 O( l ) $ H +( aq ) + OH -( aq )
Consider
the following equilibrium:
C. Ca(OH)2( s ) + 2 HCl( aq ) $ CaCl 2( aq ) + 25.
2H2O
(l)
B. Ca22+(+aq ) + 2Cl -(-aq ) $ CaCl
2( s )
D. Ca ( aq ) + 2OH ( aq ) + 2 H +( aq ) + 2Cl -( aq ) $ CaCl 2( s ) + 2 H 2 O( l ) HCO - + H O + $ H CO +
®
3
2
3
3
C. Ca(OH) ( s ) + 2 HCl( aq ) $ CaCl 2( aq ) + 2 H 2 O( l )
Consider the 2following
equilibrium:
D. Ca 2(+aq ) + 2OH -( aq ) + 2 H +( aq ) + 2Cl -( aq ) $Which
CaCl 2(of
+ 2following
H 2 O( l ) statements is true?
s ) the
+ $
HCO3 + H 3O ® H 2 CO3 + H 2 O
Considerbecause
the following
A. Products 25.
are favoured
H 2 O isequilibrium:
a stronger acid
Which of the following solutions will have the lowest electrical conductivity?
(1 mark)
Which of the following statements is true?
B. Products are favoured because (2
H 3marks)
O + is
a stronger
ac
HCO
3 + H 3O
A. 1.0 M HI
C. electrical
Reactantsconductivity?
are favoured because (1
HCO
3 is a stronger
Which
of the following
solutions
willHhave
the lowest
mark)
A. Products
are favoured
because
2 O is a stronger acid than H 2 CO3
B. 1.0 M H 2S
Which ofbecause
the following
is tr
D. Reactants
are
favoured
H 3O +statements
is a stronger
ac
+
B.
Products
are
favoured
because
H
O
is
a
stronger
acid
than
H
CO
3
2
3
C.
A. 11..00 M
M NaOH
HI
A. OProducts are favoured because H 2
Consider
theNaNO
equilibrium:
C. 11Reactants
are3favoured
because HCO3 - is a stronger base than H
M
Hfollowing
B.
..00 M
D.
2
2S
+
C.
.0 M NaOH
D. 1Reactants
are favoured because
H+3O is a stronger acid than H 2B.
CO3Products are favoured because H 3
$
HCO
+
H
O
H
CO
+
H
O
®
3
2
3
2
3
D. 1.0 MtheNaNO
C. Reactants
favoured
because
H
3
Consider
following
equilibrium:
26. Which of the following
factors of are
an acidic
solution
would
D. Reactants are
Which of the following statements
is true?
(2favoured
marks) because H
HCO3 - + H 3O + $
® H 2 CO3 + H 2 O
I.
the strength of the acid
A.
Products
are favoured
because
strongerwould
acid than
Which
of the following
factors
of anHacidic
solution
affectHits
pH
(1 mark)
2 O is a
2 CO
3 ?
Which of the following statements is true?
marks)
II.
the (2
concentration
of the a
+
B. Products are favoured because H 3O is a stronger acid than H 2 CO3
I.
the strength
the acidacid than26.
- of
III.
the temperature
A. Reactants
Products are
stronger
H 2 CO
Which
of the following
factors of an ac
2 O is a-is
3O
C.
arefavoured
favouredbecause
because HHCO
base than
H
8 a- stronger
2
3
+
B. Reactants
Products are
II.because
the H
concentration
of theacid
acidthan
D.
arefavoured
favoured
because
H33OO +isisaastronger
stronger
acid
than HH22CO
CO33
I.
the str
-- 8 C. Reactants are favoured
HCO3 is a stronger
base
than H 2 O
A. I and
II only.
III. because
the temperature
II.
the con
B. II acid
and III
only.
D. Reactants are favoured because H 3O + is a stronger
than
H 2 CO3
C. I and III only.
III.
the tem
D.would
I, II and
III.its pH ?
A. I and
II only.
82. 26. Which
of the
following factors of an acidic solution
affect
(1 mark)
B. II and III only.
C. I and III only.
I.
of the acid
26. Which
ofand
the III.
following factors
ofthe
anstrength
acidic solution
would affect its A.
pH ? I and II only. (1 mark)
D. I, II
B. II and III only.
II.
the concentration of the acid
27.
Consider
the
following
C. Iequilibrium:
and III only.
I.
the strength of the acid
D.
I,
II and III.
III.
the temperature
+
II.
the concentration of the acid
2 H 2 O( l ) $
® H 3O ( aq ) + OH ( aq
83. 27. Consider the following equilibrium:
III.
the temperature
A. I and II only.
What-changes occur to H 3O + and pH when NaOH is a
+
2 H 2 O( l ) $
B. II and III only.
® H 3O ( aq ) + OH ( aq )
27. Consider the following equilibrium:
C. I and III only.
+
A. I and II only.
A. H 3O increases and pH increases.
+
D.
I, changes
II and III.
What
occur
to
H
O
and
pH
when
NaOH
is added?
(2 marks)
B. II and III only.
2 H 2 O( l ) $
3
®
B. H 3O + increases and pH decreases.
C. I and III only.
+ III.
D.
and
A. I,HII3O
increases and pH increases.
pH increases.
C. H 3O + decreases
Whatand
changes
occur to H O + and pH
[
[
27.
]
[ ]
B. [H O ] increases and pH decreases.
Consider
the following equilibrium:
C. [H O ] decreases and pH increases.
$
3
3
+
+
D.
[
[
[
[H O
3
H 2 O( l ) ® H 3O +( aq ) + OH -( aq )
+ following 2
27. Consider
the
equilibrium:
D. H O decreases and pH decreases.
]
]
]
]
[ ]
] decreases and pH decreases.
A. [H O ] increases and pH increase
B. [H O ] increases and pH decreas
3
+
3
3
+
+
29.
28.
84. 28.
29.
21.
85. 29.
30.
29.
21.
86. 30.
30.
22.
30.
22.
87. 31.
23.
88. 23.
31.
31.
31.
89. 24.
24.
temperature of water?
(1 mark)
Which
of the following
represents
the dissociation
of the
a salt in water?
(1 mark)
The
ionization
of water is
endothermic.
How is K wequation
related to
A. K w increases as temperature
increases.
29. Which of the following represents the dissociation equation
of a salt in wat
temperature of water?
(1 mark)
+ as temperature
B.
K
decreases
increases.
$
+
A.
KCl
K
Cl
The ionization
of water
How is K w related to the
w (s)
( aq ) is endothermic.
( aq )
+
A.
KCl
A.
K
increases
as
temperature
increases.
temperature
of water?
(1 mark)
C.
decreases.( s ) $ K ( aq ) + Cl ( aq )
2w2+
B. Ca ( aq ) + SO 4 ( aq ) $ CaSO 4( s )
22+
B. K w remains
decreasesconstant
as temperature
increases.
D.
as temperature
B.
Cadecreases.
aq ) + SO 4 ( aq ) $ CaSO 4( s )
(O
A. HCl
K w increases
as temperature
increases.
C.
+
KOH
$
KCl
+
H
2 (l)
( aq )
( aq )
( aq
)
C. K w increases
as temperature
decreases.
HCl( aq ) + KOH( aq ) $ KCl( aq ) + H 2 O( l )
B. K w decreases as temperatureC.
increases.
D. K
2 Na
2 NaOH
H 2( g )
D.
temperature
2 O( l ) $as
w remains
( s ) + 2 Hconstant
( aq ) + decreases.
C. K w increases
as temperatureD.
decreases.
2
Na
2 HZn
2 NaOH
21. What is the value of (K
solubility
is equal
)of
2 O(( lOH
s ) sp+ for
) $
2 ( g )Zn(OH
( aqwater?
) + Hof
2 ifa the
Which
of
the
following
represents
the
dissociation
equation
salt
in
(1)2mark)
D. K w remains constant as temperature
decreases.
-6
to 4.2 • 10 M ?
(
+
WhatKCl
is the $
value
K spCl
for Zn(OH)2 if the solubility of Zn(OH)2 is equal
A.
K of
( sthe
) following
( aq ) +represents
( aq ) the
Which
of
equation expression
of a salt in water?
(1 mark)
-2 dissociation
Which
of
the
represents
equilibrium constant
-6followingA.
1.0 • 10the
to 4.2 •2 +10 M ? 2 (2 marks)
30.occurs
Which
the
represents the equilibrium constant
expression
(1 mark)
for the
that
NaF
B.
Cahydrolysis
SO+reaction
CaSO
( aqfollowing
)?
( s )-3 in of
4 ( aq )B.$ ) +following
4.0 • 410
Which
of((aqsthe
represents
the
dissociation
equation
of
a
salt
in
water?
(1
mark)
$
+
A.
KCl
K
Cl
for the hydrolysis reaction that occurs in NaF( aq ) ?
) value
( aq )K for( aq
) (OH
What
of
Zn
if 2the
of Zn(OH)2 is equal
)+2 H
C.
+-2KOH
$1.KCl
O( lsolubility
A. HCl
1is
.0the
•aq10
sp
)
aq
aq
(
)
(
)
(
)-11
C.
8
•
10
2
2 + -6
HF
-3SO
+M
B.
to
10
?+4( aq
(2 marks)
$
A.4.2Ca
KOH
ClCaSO
4( s )-16
aq
( aq) )+$
B.
4KCl
.•0 (=
•( s ))10
) 10
A.
D.
2K
Na
$ 23NaOH
.(0aq •
b ( s ) + 2 H-2 O( l )D.
OH aq ) + H 2 ( gHF
(
)
-11F
C.
HCl
KOH2 -aq ) $ KCl( aq
A.) + KHb2 O
= (l)
C.
1Ca
.8 2•
(+aq10
) +
+
B.
-2 SO 4 (aq
aq
(
)
( ) $ CaSO 4( s )
A. 1.0 • 10 -16
FD.
.0 (•s ) 10
D.
Na
2 NaOH )+ +HHO2( g )
C. 243HCl
KOH
F)+--+23 H
H23OO(+l()aq$
2 (l)
B.
.0 •
( aq10
) $ KCl( aq( aq
)
B. K a = -11
F - H 3O +
HF
[
]
Which
of•the
following
represents
the
equilibrium
C.
10
D. 12.8Na
+
2
H
O
$
2
NaOH
+
H
B.( aq )K a = 2( g ) constant expression
2 (l)
(s)
22.
What
is
the
maximum
500
.0 mL
[
?HF ]of moles of Cl that can exist in (1
mark)
for the hydrolysis
reaction
that
occurs
in NaFnumber
-16
aq
(
)
D. 3.0 • 10
of
2
.
0
M
AgNO
?
+
3
F - represents the equilibrium
Which of theNa
following
constant
expression
+
C. Kiseqthe
= HF
- number of moles of Cl -Na
What
maximum
that
can
exist
in 500.0 mL
F
OH
?
(1 mark)
for
the hydrolysis
reaction
that
occurs
in
NaF
NaF ]
[
-11
( aq )
C.
K
=
A.
4
5
10
.
•
A.
eq
of
2.K
0 bM
?
(1 mark)
Which
of=AgNO
the following
represents
the
equilibrium
constant
expression
[NaF]
F3-11
B. that
9.0 •
10 in NaF( aq ) ?
(1 mark)
for the hydrolysis reaction
occurs
HF-11 OH 10
+
A. K
4is.b5the
What
maximum
number
moles of Cl that can exist in 500.0 mL
A.
=• 10
+ C.
1.8 of
• 10
D.
K
H-3OH
OH
- 3O
w = F
F
11
of
09M
?
(1 mark)
D.-9 K w = H 3O + OH B.
B. 2.K
.a0 =•AgNO
10
HF 3 OH
D. 1.8 • 10
HF
[
]
A. K b = -10 C. 1.8 • 10
F --11FH 3O +
A. 4.5 • 10
-9+
B.
D. K
1.a8 =• 10
Na
F-[11
Which
of
the
following
(1 mark)
- HF ] + salt solutions will be acidic?
B.
9
.
0
•
10
C. K eq = F H 3O
31.
Which
of
the
following
salt
solutions
will
be
acidic?
NaF
[
]
B. 1K.8a •= 10 -10
C.
A. KClO 4 Na[+HF
23.
F] - In which of the following is HSO3 acting as a Brønsted-Lowry acid?
-9
D.
.8eq •=Br
10
A. KClO 4
C.
B. 1K
NH
4
[NaF
++ ] - Br H SO + OH D.
K
O F
OHA. HSO3 -B.-+ HNH
C. which
NaHCO
w = HNa
2 O4&
2
3
33 following
In
is HSO3 acting
as a Brønsted-Lowry
acid?
(1 mark)
C. K eq of
= the
C.
NaHCO
2
+
NaF
[
]
3
D. Na 2 C 2 O 4
B. NH 3 + HSO3 & NH 4 + SO3
+
D.
K
=
H
O
OH
4
3
w
A. HSO
SO3 +-D.
OH -Na 2 C22-O&
3 + H2O &
C.H 2HSO
H 2SO3 + PO 433 -+ HPO 4
In which of the following
is HSO
as10
a Brønsted-Lowry
acid?
(1 mark)
2+
3 acting
-NH
Which
the
salt
solutions
be-acidic?
(1 mark)
B.
+ following
HSO+ - &
SO3will
D. NH
Kof
42 C+
D.
H
HSO
w 3= H 3O 3 OH
- 10 2O4 +
3 & HC 2 O 4 + H 2 SO3
2C. KClO
HSO3-- ++ H
HPO
& H SO + -PO 43A.
HSO
A.
2 O 4& H 2 SO23 + 3OH
34
Which of the following
be acidic?
(1 mark)
-salt solutions
- will
2+- H SO
+
D. NH
H2C
O 4HSO
+ HSO
& HC
OSO
B.
2+
2
2
3
3
4
B.
NH
&
NH
+
43Br
3
4
3
C.
NaHCO
2
3 - acidic?
A.
KClO
Which
of
the
following
salt
solutions
(1 mark)
3
C. HSO34 + HPO 4 & H 2SO3 + will
PO 4be
24. What
is the conjugate
base of H 2 PO 4 ?
D.
B. Na
NH24CBr
2O4
D.
+
HSO
&
HC
O
+
H
SO
A. H
KClO
2C2O
4
2
2
3
3
4
4
C. NaHCO
3
B. NH 4 Br
A. OH
D.
C2O
WhatNa
is 2the
conjugate
base of H3-2 PO 4- ? - 10 (1 mark)
4
C. NaHCO3
B. PO 4
D. Na C O
- 10 C. HPO 42A. OH2- 2 4
3- conjugate base
What
is the
H 2 PO 4 ?
(1 mark)
D. of
H 3PO
B. PO
4
4
- 10 2-4
C. OH
HPO
A.
[ ][ ]
[ ]
[ ][ ]
[ ][
[ ][
[ ]
[ ][
[[ ][[ ][]
[ ][
[ ][[ ]
[ ][
[ ][
[ ][
[ [ ][
[
[
D. PO
H 3PO
3- 4
B.
4
]
]
]
]]
]
]
]
]
]
]]
][ ]
][ ]
[ ][ ]
[ ]
[ ][ ]
[ ][ ]
[
][
]
25. Which
of
the following
is 0correct
solutions listedcomplete
are compared to
A.
strong
acid
.50 M if the fourhighest
Relative
Concentration
Ionization
one another?
Conductivity
B.
weak acid
lowest
complete
0.50 M
90. 25. Which of the following is correct if the four solutions listed are compared to
A.
strong
highest
complete
01.50
M
Relative
C. another?
strong acid
base
highest
complete
one
.0 M
Concentration
Ionization
Conductivity
B.
weak base
acid
lowest
complete
01.50
M
D.
weak
lowest
complete
.0 M
Relative
A.
strong acid
highest
complete
0
.
50
M
Concentration
Ionization
C.
strong base
highest
complete
1.0 M
Conductivity
B.
weak acid
lowest
complete
0.50 M
D.
weak base
lowest
complete
0M
A.
strong
acid
highest
complete
01..50
M
C.
strong base
highest
complete
1.0 M
26. Which
ofweak
the following
is the
acidlowest
that can exist incomplete
an aqueous solution?
B.
acid
0.50strongest
M
D.
weak base
lowest
complete
1.0 M
C. O2-strong base
highest
complete
1.0 M
A.
-the following is the strongest acid that can exist in an aqueous solution?
26. Which
ofweak
B.
D. NH
base
lowest
complete
1.0 M
2
+
C. O
H23O
A.
Which
of-the
D.
HClO
91. 26. B.
4 following is the strongest acid that can exist in an aqueous solution?
NH
2
(2 marks)
(2 marks)
(1 mark)
(1 mark)
(1 mark)
2- +
C.
H
3O
A.
O
26. Which of the following is the strongest acid that can exist in an aqueous solution?
D.
B. HClO
NH -4
(1 mark)
27.
(1 mark)
2
92. 27.
27.
27.
93. 28.
28.
28.
94. 29.
28.
2+
A.
C. O
Hof
Which
3Othe following household products could have a pH = 12.0 ?
B.
2 4
D. NH
HClO
+
A.
soda
C. H 3O pop
B. tapofwater
Which
the following household products could have a pH = 12.0 ?
D. HClO 4
C. lemon juice
A.
D. soda
oven pop
cleaner
B.
tap
water
Which of
the following household products could have a pH = 12.0 ?
C. lemon juice
A. oven
soda cleaner
pop
D.
Which of the following household products could have a pH = 12.0 ?
B. tap water
What
is the juice
pH of a 0.050 M KOH solution?
C. soda
lemon
A.
pop
D. tap
oven
cleaner
B.
water
A.
0.30
C. lemon
What
the juice
pH of a 0.050 M KOH solution?
B. is
1.30
D. oven cleaner
C. 12.70
A.
0.30
D. 13.70
B.
What 1is.30
the pH of a 0.050 M KOH solution?
C. 12.70
What
is0..the
of K for H 2 PO 4- ?
A. 13
30 value
D.
What
is 70
the
pH of a 0.b050 M KOH
solution?
B.
1.30
-12
A.
.03..30
•
C. 112
7010
A.
D. 613
70
B.
.12..30
• 10 -8
B.
-9C. 112
C.
.6.70
• 10 -7
D. 713
D.
.5.70
• 10 -3
-9-
930. Which of the following describes the net ionic- reaction
for the hydrolysis
of NH 4 Cl( s ) ?
A.
B.
NH 4+( aq ) + Cl -( aq ) &
® NH 4 Cl( s )
+
NH 4 Cl( s ) &
® NH 4 aq + Cl aq
-9-
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
(1 mark)
OVER
OVER
OVER
(1 mark)
OVER