Chemistry 12
Examination Booklet
2008/09 Released Exam
June 2009
Form A
DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.
FOR FURTHER INSTRUCTIONS REFER TO THE RESPONSE BOOKLET.
Contents: 18 pages
50 multiple-choice questions
Examination: 2 hours
Additional Time Permitted: 60 minutes
© Province of British Columbia
PART A: MULTIPLE CHOICE
Value: 62.5% of the examination
Suggested Time: 80 minutes
INSTRUCTIONS: For each question, select the best answer and record your choice on the Answer
Sheet provided. Using an HB pencil, completely fill in the bubble that has the
letter corresponding to your answer.
You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,
fill in the bubble as follows.
Exam Booklet Form/
Cahier d’examen
A
B
C
D
E
F
G
H
1. Which of the following would have the highest reaction rate at room temperature?
A. H2 (g) + I2 (g) 2HI(g)
B.
H2 S(g) + Cl 2 (aq) 2HCl(aq ) + S(s)
C.
2
Ca 2 + (aq) + C2 O4 (aq) CaC 2 O4 (s)
D. Mg(s) + 2H2O( ) Mg(OH )2 (aq) + H2 (g)
2. Consider the following experimental results:
Reactants
Temperature
Concentration of acid
Rate
Experiment 1
Experiment 2
powdered Cu and HCl
chunk of Cu and HNO3
20º C
10º C
0.6 M HCl
0.4 M HNO3
low
high
Which of the following factors would account for the lower rate in Experiment 1?
A.
B.
C.
D.
temperature
nature of reactants
surface area of Cu
concentration of acid
Chemistry 12 – 0906 Form A
Page 1
3
Which of the following describes “activation energy”?
A.
B.
C.
D.
the amount of energy that product molecules possess
the difference between the products PE and the reactants PE
the amount of energy released when reactant molecules collide
the minimum amount of energy required to start a chemical reaction
4. Consider the following PE diagram:
200
PE
(kJ)
150
100
50
Progress of reaction
Which of the following is correct for the reverse reaction?
Page 2
PE (activated complex)
(kJ)
H (kJ)
A.
50
100
B.
50
+100
C.
200
100
D.
200
+100
Chemistry 12 – 0906 Form A
5. Consider the following reaction mechanism:
Step 1:
ClO + H 2 O HClO + OH Step 2:
I + HClO HIO + Cl Step 3:
HIO + OH IO + H 2 O
Which of the following is correct?
Reactant for the
Overall Reaction
Reaction Intermediate
A.
I
OH B.
ClO H 2O
C.
H 2O
HClO
D.
HClO
HIO
6. Which of the following is correct for all systems at equilibrium?
A.
B.
C.
D.
I
The temperature is constant.
II
[Reactants] = [Products]
III
Forward and reverse reactions are occurring.
IV
The forward and reverse reaction rates are equal.
I and II only
I, III and IV only
II, III and IV only
III and IV only
Chemistry 12 – 0906 Form A
Page 3
7. In which of the following does entropy increase?
A. the electrolysis of Na 2SO 4 ( aq )
B. the reaction of NaCl ( aq ) with AgNO3 ( aq )
C. the redox reaction of an Fe nail in CuCl 2 ( aq )
D. the neutralization of Sr ( OH )2 ( aq ) by H 2SO 4 ( aq )
8. Considering enthalpy and entropy factors, in which of the following will equilibrium be established?
A.
B.
C.
D.
Page 4
I
?
Cl 2 (g) Cl2 (aq)
H = 25 kJ
II
?
CO(g) + 2H2 (g) CH3OH (g)
H = 91kJ
III
?
Mg(s) + 2HCl(aq) MgCl2 (aq) + H2 (g)
H = 425 kJ
IV
?
3CO2 (g) + 4H2 O(g) C 3H8 (g) + 5 O2 (g)
H = + 2200 kJ
I and II only
II and IV only
III and IV only
I, II and III only
Chemistry 12 – 0906 Form A
Use the following equilibrium to answer questions 9 and 10.
2NO ( g ) N 2 ( g ) + O2 ( g )
H = +181kJ
9. Which of the following pairs of stresses cause the same shift to the above equilibrium?
A. adding a catalyst and decreasing volume
B. increasing pressure and increasing [ NO ]
C. decreasing [ N 2 ] and decreasing temperature
D. decreasing temperature and increasing volume
10. If some O 2 is injected into the above equilibrium system, which of the following is correct?
Equilibrium Shift
Net Change [ O 2 ]
A.
left
increase
B.
left
decrease
C.
right
increase
D.
right
decrease
11. Consider the following:
SO3 ( g ) + 6HF ( g ) SF6 ( g ) + 3H 2O ( g )
K eq = 6.3 10 3
Which of the following is the value of K eq for:
2SF6 ( g ) + 6H 2O ( g ) 12HF ( g ) + 2SO3 ( g )
A. 1.3 10 1
B. 1.6 10 2
C.
3.2 10 2
D. 2.5 10 4
Chemistry 12 – 0906 Form A
Page 5
12. Consider the following:
I
II
III
C 2H 4 ( g ) + H 2 ( g ) C 2H 6 ( g )
2HBr ( g ) H 2 ( g ) + Br2 ( g )
Si ( s ) + O 2 ( g ) SiO 2 ( s )
K eq = 1.2 10 19
K eq = 7.0 10 20
K eq = 2.0 10 142
Which of the following lists these equilibria from the one that most favours products
to the one that least favours products?
A.
B.
C.
D.
I, II, III
I, III, II
II, III, I
III, I, II
13. Consider the following equilibrium system:
Ni ( s ) + 4CO ( g ) Ni ( CO )4 ( g )
H = 603 kJ
Which of the following statements is correct?
A. Increasing [ CO ] will increase K eq .
B. Increasing temperature will increase K eq .
C. Increasing temperature will decrease K eq .
D. Decreasing [ Ni ( CO )4 ] will decrease K eq .
Page 6
Chemistry 12 – 0906 Form A
14. Consider the equilibrium:
N 2 ( g ) + 3H 2 ( g ) 2NH 3 ( g )
K eq = 64
A 1.0 L container is filled with 0.28 mol N 2 , 0.16 mol H 2 and 0.54 mol NH 3 .
In which direction will the reaction proceed and what will happen to the pressure of the system?
Direction
Pressure
A.
left
decreases
B.
left
increases
C.
right
decreases
D.
right
increases
15. Which of the following will form a saturated solution?
A. 0.10 mol CaSO 4 added to 1.0 L of water
B.
0.10 mol Cs 2SO 4 added to 1.0 L of water
C.
0.20 mol MgSO 4 added to 2.0 L of water
D. 0.50 mol Pb ( NO3 )2 added to 2.0 L of water
16. Which of the following would be an appropriate measure of solubility?
A.
B.
C.
D.
moles of solute per volume of solute
mass of solute per volume of solution
volume of solvent per mass of solvent
moles of solute at a specific temperature
17. What is the complete ionic equation for the precipitation reaction between
MgS ( aq ) and Sr ( OH )2 ( aq ) ?
A.
Mg 2 + ( aq ) + 2OH ( aq ) Mg ( OH )2 ( s )
B.
MgS ( aq ) + Sr ( OH ) 2 ( aq ) SrS ( aq ) + Mg ( OH ) 2 ( s )
C.
Mg2 + ( aq ) + S2 ( aq ) + Sr 2 + ( aq ) + 2OH ( aq ) Mg2 + ( aq ) + 2OH ( aq ) + Sr S ( s )
D.
Mg2 + ( aq ) + S2 ( aq ) + Sr 2 + ( aq ) + 2OH ( aq ) Sr 2 + ( aq ) + S2 ( aq ) + Mg ( OH )2 ( s )
Chemistry 12 – 0906 Form A
Page 7
18. What is the K sp expression for the low solubility salt formed when K 2SO3 ( aq )
and AlCl 3 ( aq ) are mixed?
A. K sp = [ SO32 ]
B.
K sp = [ K + ] [ Cl ]
C.
K sp = [ Al 3+ ] [ SO32 ]
2
3
D. K sp = [ Al 3+ ] [ SO32 ]
3
2
19. Which compound has the lowest solubility?
A.
ZnS
B.
CuS
C.
AgCl
D. SrSO 4
20. What is the solubility of the salt PbCl 2 ?
A. 1.4 10 2 M
B.
2.4 10 3 M
C.
3.5 10 3 M
D. 1.2 10 5 M
[
21. A solution is found to contain a [Pb2 + ] of 0.10M . What is the maximum SO 4
2
] that can exist in
this solution before a precipitate forms?
A.
B.
C.
D.
Page 8
[SO
[SO
[SO
[SO
2
4
2
4
2
4
2
4
] = 1.8 10
] = 1.8 10
] = 1.8 10
] = 1.3 10
9
8
7
4
M
M
M
M
Chemistry 12 – 0906 Form A
22. Which of the following represents the results of tests using an acidic solution?
Reaction
with Mg(s)
Colour in
Phenol Red
A.
yes
yellow
B.
yes
red
C.
no
yellow
D.
no
red
23. Identify the reactant acid and its conjugate base in the equilibrium below.
Al ( H 2 O )63+ + HS 2+
H 2S + Al ( H 2 O )5 ( OH )
Reactant Acid
Conjugate Base
A.
HS
H 2S
B.
H 2S
Al ( H 2O )6
3+
C.
Al ( H 2O )6
D.
Al ( H 2 O )6
3+
3+
HS Al ( H 2 O )5 ( OH )
2+
24. Which of the following is the weakest acid?
A. 0.10 M CH 3COOH
B.
0.50 M HClO 4
C. 1.0 M HIO3
D. 1.5 M HCN
Chemistry 12 – 0906 Form A
Page 9
25. Which of the following is the correct sequence of relative acid strengths?
A. HO 2 > HCO3 > H 2O 2 > H 2CO3
B.
H 2CO3 > HCO3 > H 2O 2 > HO 2
C.
H 2CO3 > H 2O 2 > HCO3 > HO 2
D. HCO3 > H 2O 2 > H 2CO3 > HO 2
26. Water reacts most completely as an acid with which of the following?
A. HO 2
B.
CO32 C.
C2O 42 D. HPO 42 27. Which of the following equations represents the ionization of water?
A. H 2O ( ) H 2 ( aq ) +
1
2
O 2 ( aq )
B.
+
2
2H 2O ( ) H 3O ( aq ) + O ( aq )
C.
+
H 2O ( ) + H 2O ( ) H ( aq ) + OH ( aq )
+
D. H 2O ( ) + H 2O ( ) H 3O ( aq ) + OH ( aq )
28. The ionization of water is endothermic. Which of the following is a suitable
value of K w if the temperature of water is lower than 25º C ?
A. 6.8 10 15
B.
2.0 10 14
C. 1.0 10 14
D. 1.6 10 13
Page 10
Chemistry 12 – 0906 Form A
29. What is the pOH of 0.30 M HI ?
A. 3.3 10 14
B.
0.52
C.
0.52
D. 13.48
30. What is the equilibrium constant expression for the predominant equilibrium in HCO3 ( aq ) ?
A.
H CO OH 2 3
HCO3 B.
H 3O + CO32 HCO3 C.
HCO3 ( aq ) + H 2 O ( ) H 2 CO3 ( aq ) + OH ( aq )
2
+
D. HCO3 ( aq ) + H 2 O ( ) H 3O ( aq ) + CO3 ( aq )
31. Which of the following 0.10 M solutions would have the lowest pH?
A. HF
B.
NH 3
C.
HNO3
D. H 2 CO3
Chemistry 12 – 0906 Form A
Page 11
32. Which of the following describes the predominant hydrolysis reaction that occurs in Na 2 HPO 4 ( aq ) ?
A.
B.
2
+
Na 2 HPO 4 ( aq ) 2Na ( aq ) + HPO 4 ( aq )
2
PO 3 ( aq ) + H O ( ) HPO ( aq ) + OH ( aq )
4
2
4
3
+
HPO 42 ( aq ) + H 2 O ( ) H 3O ( aq ) + PO 4 ( aq )
D. HPO 42 ( aq ) + H 2 O ( ) H 2 PO 4 ( aq ) + OH ( aq )
C.
33. Which of the following represents a basic salt solution?
A. NaI(aq)
B.
C.
NH 4 Cl(aq)
Na 2CO 3 (aq)
D. NaHSO 4 (aq)
34. The term “equivalence point” typically applies to
A.
B.
C.
D.
Page 12
buffer solutions.
titration reactions.
saturated solutions.
chemical indicators.
Chemistry 12 – 0906 Form A
35. A solution is tested with two indicators and the following results are obtained:
Indicator
Colour
chlorophenol red
red
phenolphthalein
colourless
What is the approximate pH of the solution?
A. 4.0
B. 6.0
C. 7.0
D. 10.0
36. What is the net ionic equation for the reaction of hydrochloric acid with NaOH ( aq ) ?
A. H + ( aq ) + OH ( aq ) H 2 O ( )
B.
HCl ( aq ) + NaOH ( aq ) NaCl ( aq ) + H 2 O ( )
C.
HCl ( aq ) + NaOH ( aq ) + H 2 O ( ) NaCl ( aq ) + H 3O + ( aq ) + OH ( aq )
D. H + ( aq ) + Cl ( aq ) + Na + ( aq ) + OH ( aq ) Na + ( aq ) + Cl ( aq ) + H 2 O ( )
37. Consider the following buffer equilibrium system:
+
HCN ( aq ) + H 2O ( ) H 3O ( aq ) + CN ( aq )
What is the net result of adding a small amount of KOH ?
A. The pH increases slightly.
B. The pH decreases slightly.
C. The [ HCN ] increases slightly.
D. The [ CN ] decreases slightly.
Chemistry 12 – 0906 Form A
Page 13
38. An oxide of which of the following elements will form a basic solution?
A.
B.
C.
D.
P
N
K
C
39. A reducing agent in a chemical reaction can best be described as a substance that
A.
B.
C.
D.
loses electrons and has a decrease in oxidation number.
gains electrons and has a decrease in oxidation number.
loses electrons and has an increase in oxidation number.
gains electrons and has an increase in oxidation number.
40. What happens to the oxidation number of O as MgO 2 undergoes a reaction in which
H 2 O 2 is formed?
A.
B.
C.
D.
It decreases by 1.
It increases by 1.
It increases by 2.
It does not change.
41. Consider the following redox equation:
K 2 Cr2 O 7 + 7H 2SO 4 + 6KBr 3Br2 + 4K 2SO 4 + Cr2 ( SO 4 )3 + 7H 2 O
Which chemical species is oxidized?
A.
Br in KBr
B.
S in H 2SO 4
C.
H in H 2SO 4
D. Cr in K 2 Cr2 O 7
Page 14
Chemistry 12 – 0906 Form A
42. Consider the following spontaneous redox reactions:
X + Y X + Y
Y + Z Y + Z
Which of the following describes the relative strengths of the reducing agents?
A.
X > Y > Z
B.
Z > Y > X
C.
X > Y > Z
D.
Z > Y > X
43. The following half-reaction can be balanced in acidic solution:
N 2O5 NH 4+
Which of the following appear in the balanced equation?
A. 13e B. 14e C. 16e D. 18e 44. Consider the following redox reaction:
2MnO 4 + 16H + + 10 I 2Mn 2 + + 8H 2 O + 5 I 2
A 10.0 mL sample of an iodide solution is titrated with 15.7 mL of acidified 0.0106 M MnO 4 .
What is the [ I ] of the sample?
A. 3.33 10 3 M
B. 1.66 10 2 M
C.
3.24 10 2 M
D. 8.32 10 2 M
Chemistry 12 – 0906 Form A
Page 15
45. Consider the following diagram of a standard electrochemical cell:
e–
Object 1
e–
Cu(s)
Zn(s)
1.0 M Zn(NO3) 2 1.0 M Cu(NO3) 2
Which of the following is correct?
Object 1
Zn ( s )
A.
light bulb
cathode
B.
light bulb
anode
C.
power supply
cathode
D.
power supply
anode
Page 16
Chemistry 12 – 0906 Form A
Use the following diagram to answer questions 46, 47 and 48.
Volts
H2(g)
Porous
Barrier
Pt (inert)
1.0 M HCl
Ag
1.0 M AgNO3
46. What is the overall cell reaction?
A.
Ag+ + H + H 2 + Ag
B.
2Ag + 2H + 2Ag+ + H 2
C.
2Ag+ + H 2 2H + + 2Ag
D.
Ag+ + H 2 Ag + 2H + + e 47. Which of the following is correct as the cell operates?
Direction of NO3 Migration
pH near the Pt Electrode
A.
towards Pt
increases
B.
towards Pt
decreases
C.
towards Ag
increases
D.
towards Ag
decreases
48. Which of the following describes the direction of electron flow and the change in mass of
the Ag electrode as the cell operates?
Direction of Electron Flow
Mass of Ag Electrode
A.
from Pt to Ag
increases
B.
from Pt to Ag
decreases
C.
from Ag to Pt
increases
D.
from Ag to Pt
decreases
Chemistry 12 – 0906 Form A
Page 17
49. An iron pipeline can be protected from rusting by connecting it to a
A.
B.
C.
D.
silver electrode buried beside the pipeline.
copper electrode buried beside the pipeline.
positive terminal of a direct current power supply.
negative terminal of a direct current power supply.
50. The electrolysis of molten NaCl is an industrial process. What does the electrolysis produce?
A. Na and Cl 2
B.
H2 and O2
C.
Na + and Cl D. NaOH and Cl 2
You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,
ensure you filled in the bubble as follows.
Exam Booklet Form/
Cahier d’examen
A
B
C
D
E
F
G
H
This is the end of the multiple-choice section.
Answer the remaining questions in the Response Booklet.
Page 18
Chemistry 12 – 0906 Form A
Chemistry 12
Data Page 39
(226)
(223)
(227)
Actinium
Ac
Yttrium
(261)
Rutherfordium
Rf
104
72
91.2
Zirconium
Values in parentheses
are the masses of the most
stable or best known isotopes for
elements which do not occur naturally.
Based on mass of C12 at 12.00.
Radium
Francium
89
88
138.9
Barium
137.3
Cesium
132.9
Ra
Lanthanum
56
Ba
55
Cs
87
Hafnium
178.5
57
La
87.6
Fr
Hf
88.9
Strontium
85.5
40
Zr
Rubidium
Y
38
Sr
37
Rb
47.9
Titanium
45.0
40.1
Scandium
Calcium
39.1
22
Ti
Potassium
21
4
Sc
20
Ca
24.3
23.0
K
Magnesium
Sodium
3
19
12
Mg
9.0
6.9
11
Beryllium
Lithium
Na
4
Be
3
2
Li
1.0
Hydrogen
H
1
1
91
Pa
Protactinium
231.0
90
Thorium
232.0
140.9
Th
Neodymium
Praseodymium
Cerium
140.1
238.0
Uranium
U
92
144.2
60
Nd
59
Pr
58
Ce
Bohrium
Bh
107
186.2
Rhenium
Re
75
(98)
Technetium
Tc
43
54.9
Manganese
Mn
25
28.1
28.1
Silicon
Silicon
Si
Si
14
14
7
(262)
Seaborgium
Sg
106
183.8
Tungsten
W
74
95.9
Molybdenum
Mo
42
52.0
Chromium
Cr
24
6
(263)
(262)
Dubnium
Db
105
180.9
Tantalum
Ta
73
92.9
Niobium
Nb
41
50.9
Vanadium
V
23
5
9
27
93
(237)
Neptunium
Np
(244)
Plutonium
Pu
94
150.4
Samarium
Promethium
(145)
Sm
62
(266)
Meitnerium
Mt
109
192.2
Iridium
Ir
77
102.9
Rhodium
Rh
45
58.9
Cobalt
Co
Pm
61
(265)
Hassium
Hs
108
190.2
Osmium
Os
76
101.1
Ruthenium
Ru
44
55.8
Iron
Fe
26
Atomic Number
Symbol
Name
Atomic Mass
8
(243)
Americium
Am
95
152.0
Europium
Eu
63
195.1
Platinum
Pt
78
106.4
Palladium
Pd
46
58.7
Nickel
Ni
28
10
(247)
Curium
Cm
96
157.3
Gadolinium
Gd
64
197.0
Gold
Au
79
107.9
Silver
Ag
47
63.5
Copper
Cu
29
11
(247)
Berkelium
Bk
97
158.9
Terbium
Tb
65
200.6
Mercury
Hg
80
112.4
Cadmium
Cd
48
65.4
Zinc
Zn
30
12
PERIODIC TABLE OF THE ELEMENTS
(251)
Californium
Cf
98
162.5
Dysprosium
Dy
66
204.4
Thallium
Tl
81
114.8
Indium
In
49
69.7
Gallium
Ga
31
27.0
Aluminum
Al
13
10.8
Boron
B
5
13
(252)
Einsteinium
Es
99
164.9
Holmium
Ho
67
207.2
Lead
Pb
82
118.7
Tin
Sn
50
72.6
Germanium
Ge
32
28.1
Silicon
Si
14
12.0
Carbon
C
6
14
(257)
Fermium
Fm
100
167.3
Erbium
Er
68
209.0
Bismuth
Bi
83
121.8
Antimony
Sb
51
74.9
Arsenic
As
33
31.0
Phosphorus
P
15
14.0
Nitrogen
N
7
15
(258)
Mendelevium
Md
101
168.9
Thulium
Tm
69
(209)
Polonium
Po
84
127.6
Tellurium
Te
52
79.0
Selenium
Se
34
32.1
Sulphur
S
16
16.0
Oxygen
O
8
16
(259)
Nobelium
No
102
173.0
Ytterbium
Yb
70
(210)
Astatine
At
85
126.9
Iodine
I
53
79.9
Bromine
Br
35
35.5
Chlorine
Cl
17
19.0
Fluorine
F
9
17
(262)
Lawrencium
Lr
103
175.0
Lutetium
Lu
71
(222)
Radon
Rn
86
131.3
Xenon
Xe
54
83.8
Krypton
Kr
36
39.9
Argon
Ar
18
20.2
Neon
Ne
10
4.0
Helium
He
2
18
ATOMIC MASSES OF THE ELEMENTS
Based on mass of C12 at 12.00.
Values in parentheses are the mass number of the most stable or best
known isotopes for elements that do not occur naturally.
Element
Actinium
Aluminum
Americium
Antimony
Argon
Arsenic
Astatine
Barium
Berkelium
Beryllium
Bismuth
Boron
Bromine
Cadmium
Calcium
Californium
Carbon
Cerium
Cesium
Chlorine
Chromium
Cobalt
Copper
Curium
Dubnium
Dysprosium
Einsteinium
Erbium
Europium
Fermium
Fluorine
Francium
Gadolinium
Gallium
Germanium
Gold
Hafnium
Helium
Holmium
Hydrogen
Indium
Iodine
Iridium
Iron
Krypton
Lanthanum
Lawrencium
Lead
Lithium
Lutetium
Magnesium
Manganese
Mendelevium
Data Page Symbol
Atomic
Number
Atomic
Mass
Ac
Al
Am
Sb
Ar
As
At
Ba
Bk
Be
Bi
B
Br
Cd
Ca
Cf
C
Ce
Cs
Cl
Cr
Co
Cu
Cm
Db
Dy
Es
Er
Eu
Fm
F
Fr
Gd
Ga
Ge
Au
Hf
He
Ho
H
In
I
Ir
Fe
Kr
La
Lr
Pb
Li
Lu
Mg
Mn
Md
89
13
95
51
18
33
85
56
97
4
83
5
35
48
20
98
6
58
55
17
24
27
29
96
105
66
99
68
63
100
9
87
64
31
32
79
72
2
67
1
49
53
77
26
36
57
103
82
3
71
12
25
101
(227)
27.0
(243)
121.8
39.9
74.9
(210)
137.3
(247)
9.0
209.0
10.8
79.9
112.4
40.1
(251)
12.0
140.1
132.9
35.5
52.0
58.9
63.5
(247)
(262)
162.5
(252)
167.3
152.0
(257)
19.0
(223)
157.3
69.7
72.6
197.0
178.5
4.0
164.9
1.0
114.8
126.9
192.2
55.8
83.8
138.9
(262)
207.2
6.9
175.0
24.3
54.9
(258)
Element
Mercury
Molybdenum
Neodymium
Neon
Neptunium
Nickel
Niobium
Nitrogen
Nobelium
Osmium
Oxygen
Palladium
Phosphorus
Platinum
Plutonium
Polonium
Potassium
Praseodymium
Promethium
Protactinium
Radium
Radon
Rhenium
Rhodium
Rubidium
Ruthenium
Rutherfordium
Samarium
Scandium
Selenium
Silicon
Silver
Sodium
Strontium
Sulphur
Tantalum
Technetium
Tellurium
Terbium
Thallium
Thorium
Thulium
Tin
Titanium
Tungsten
Uranium
Vanadium
Xenon
Ytterbium
Yttrium
Zinc
Zirconium
Symbol
Atomic
Number
Atomic
Mass
Hg
Mo
Nd
Ne
Np
Ni
Nb
N
No
Os
O
Pd
P
Pt
Pu
Po
K
Pr
Pm
Pa
Ra
Rn
Re
Rh
Rb
Ru
Rf
Sm
Sc
Se
Si
Ag
Na
Sr
S
Ta
Tc
Te
Tb
Tl
Th
Tm
Sn
Ti
W
U
V
Xe
Yb
Y
Zn
Zr
80
42
60
10
93
28
41
7
102
76
8
46
15
78
94
84
19
59
61
91
88
86
75
45
37
44
104
62
21
34
14
47
11
38
16
73
43
52
65
81
90
69
50
22
74
92
23
54
70
39
30
40
200.6
95.9
144.2
20.2
(237)
58.7
92.9
14.0
(259)
190.2
16.0
106.4
31.0
195.1
(244)
(209)
39.1
140.9
(145)
231.0
(226)
(222)
186.2
102.9
85.5
101.1
(261)
150.4
45.0
79.0
28.1
107.9
23.0
87.6
32.1
180.9
(98)
127.6
158.9
204.4
232.0
168.9
118.7
47.9
183.8
238.0
50.9
131.3
173.0
88.9
65.4
91.2
Chemistry 12
NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS
* Aqueous solutions are readily oxidized by air.
** Not stable in aqueous solutions.
Positive Ions
(Cations)
Al3+
Aluminum
Pb4+
NH4+
Ammonium
Li+
Lead(IV), plumbic
Lithium
Ba2+
Barium
Mg2+
Magnesium
Ca2+
Calcium
Mn2+
Manganese(II), manganous
Cr2+
Chromium(II), chromous
Mn4+
Manganese(IV)
Cr3+
Chromium(III), chromic
Hg22+
Mercury(I)*, mercurous
Cu+
Copper(I)*, cuprous
Cu2+
Hg2+
K+
Copper(II), cupric
Mercury(II), mercuric
Potassium
Hydrogen
Ag+
Silver
Hydronium
Na+
Sodium
Fe2+
Iron(II)*, ferrous
Sn2+
Tin(II)*, stannous
Fe3+
Iron(III), ferric
Sn4+
Tin(IV), stannic
Pb2+
Lead(II), plumbous
Zn2+
Zinc
Bromide
OH–
Hydroxide
CO32–
Carbonate
ClO–
Hypochlorite
ClO3–
Chlorate
I–
Cl–
Chloride
HPO42–
ClO2–
Chlorite
NO3–
Nitrate
Chromate
NO2–
Nitrite
H+
H3O+
Negative Ions
(Anions)
Br–
CrO42–
CN–
Cr2O72–
Dichromate
H2PO4–
Dihydrogen phosphate
CH3COO –
F–
HCO3–
Ethanoate, acetate
C2O42–
O2–
ClO4–
MnO4–
Monohydrogen phosphate
Oxalate
Oxide**
Perchlorate
Permanganate
Fluoride
PO4?–
Phosphate
Hydrogen carbonate, bicarbonate
SO42–
Sulphate
S2–
Sulphide
HC2O4–
Hydrogen oxalate, binoxalate
HSO4–
Hydrogen sulphate, bisulphate
SO32–
Sulphite
HS–
Hydrogen sulphide, bisulphide
SCN–
Thiocyanate
HSO3–
Chemistry 12
Cyanide
Iodide
Hydrogen sulphite, bisulphite
Data Page SOLUBILITY OF COMMON COMPOUNDS IN WATER
The term soluble here means > 0.1 mol/L at 25°C.
Positive Ions
(Cations)
Solubility of
Compounds
All
Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+
Soluble
All
Hydrogen ion: H+
Soluble
All
Ammonium ion: NH4+
Soluble
Nitrate, NO3–
All
Soluble
All others
Soluble
–
Bromide, Br
Sulphate,
SO42–
123
Iodide, I–
Sulphide, S
123
or
Chloride, Cl–
2–
123
or
14243
Negative Ions
(Anions)
Hydroxide, OH
or
or
Data Page 14253
–
Phosphate, PO43–
2–
Carbonate, CO3
Sulphite, SO32–
Ag+, Pb2+, Cu+
All others
Low Solubility
Soluble
Ag+, Ca2+, Sr2+, Ba2+, Pb2+
Alkali ions, H+, NH4+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+
Low Solubility
Soluble
All others
Alkali ions, H+, NH4+, Sr2+ ?
Low Solubility
Soluble
Low Solubility
All others
Alkali ions, H+, NH4+
All others
Soluble
Low Solubility
Chemistry 12
SOLUBILITY PRODUCT CONSTANTS AT 25°C
Chemistry 12
Name
Formula
K sp
Barium carbonate
BaCO3
2.6 10–9
Barium chromate
BaCrO4
1.2 10–10
Barium sulphate
BaSO4
1.1 10–10
Calcium carbonate
CaCO3
5.0 10–9
Calcium oxalate
CaC2O4
2.3 10–9
Calcium sulphate
CaSO4
7.1 10–5
Copper(I) iodide
CuI
1.3 10–12
Copper(II) iodate
Cu(IO3)2
6.9 10–8
Copper(II) sulphide
CuS
6.0 10–37
Iron(II) hydroxide
Fe(OH)2
4.9 10–17
Iron(II) sulphide
FeS
6.0 10–19
Iron(III) hydroxide
Fe(OH)3
2.6 10–39
Lead(II) bromide
PbBr2
6.6 10–6
Lead(II) chloride
PbCl2
1.2 10–5
Lead(II) iodate
Pb(IO3)2
3.7 10–13
Lead(II) iodide
PbI2
8.5 10–9
Lead(II) sulphate
PbSO4
1.8 10–8
Magnesium carbonate
MgCO3
6.8 10–6
Magnesium hydroxide
Mg(OH)2
5.6 10–12
Silver bromate
AgBrO3
5.3 10–5
Silver bromide
AgBr
5.4 10–13
Silver carbonate
Ag2CO3
8.5 10–12
Silver chloride
AgCl
1.8 10–10
Silver chromate
Ag2CrO4
1.1 10–12
Silver iodate
AgIO3
3.2 10–8
Silver iodide
AgI
8.5 10–17
Strontium carbonate
SrCO3
5.6 10–10
Strontium fluoride
SrF2
4.3 10–9
Strontium sulphate
SrSO4
3.4 10–7
Zinc sulphide
ZnS
2.0 10–25
Data Page RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASES
in aqueous solution at room temperature.
STRONG
Name of Acid
Iodic
Oxalic
H2C2O4
H 2 SO 3
Hydrogen sulphate ion
HSO 4 −
Phosphoric
H 3 PO 4
Citric
Nitrous
Hydrofluoric
Methanoic, formic
Fe(H 2 O)6 3 +
H 3C 6 H 5 O 7
HNO 2
HF
HCOOH
Hexaaquochromium ion, chromium( III ) ion
Cr(H 2 O)6 3 +
Benzoic
C 6 H 5COOH
Hydrogen oxalate ion
Ethanoic, acetic
HC 2 O 4 −
CH 3COOH
Dihydrogen citrate ion
H 2 C 6 H 5O 7 −
Hexaaquoaluminum ion, aluminum ion
Al(H 2 O)6 3 +
Carbonic (CO 2 + H 2 O)
Monohydrogen citrate ion
Hydrogen sulphite ion
Hydrogen sulphide
Dihydrogen phosphate ion
Boric
Ammonium ion
Hydrocyanic
Phenol
Hydrogen carbonate ion
H 2 CO 3
HC 6 H 5O 7 2 −
HSO 3 −
H 2S
H 2 PO 4 −
H 3 BO 3
NH 4 +
HCN
C 6 H 5OH
HCO 3 −
→
→
→
→
→
→
→
←
H+
H+
H+
H+
H+
H+
H+
Ka
+ ClO 4 −
+ I−
+ Br −
+ Cl −
+ NO 3 −
+ HSO 4 −
+ H2O
−
+
→
← H + IO 3
−
+
→
← H + HC 2 O 4
−
+
→
← H + HSO
6.0 × 10 − 3
7.1 × 10 − 4
+
2+
→
← H + Cr(H 2 O)5 (OH)
+
−
→
← H + C 6 H 5COO
2−
+
→
← H +C O
1.5 × 10 − 4
2
3.5 × 10 − 4
1.8 × 10 − 4
4
6.5 × 10 − 5
6.4 × 10 − 5
+
−
→
← H + CH 3COO
2−
+
→
← H + HC 6 H 5O 7
+
2+
→
← H + Al(H O) (OH)
1.8 × 10 − 5
−
+
→
← H + HCO 3
3−
+
→
← H + C 6 H 5O 7
→ H + + SO 2 −
←
3
+
−
→
← H + HS
→ H + + HPO 2 −
←
4
−
+
→
H
+
H
BO
←
2
3
+
→
← H + NH
4.3 × 10 − 7
2
3
−
5
1.7 × 10 − 5
1.4 × 10 − 5
4.1 × 10 − 7
1.0 × 10 − 7
9.1 × 10 − 8
6.2 × 10 − 8
7.3 × 10 −10
5.6 × 10 −10
+
→
← H + CN
+
−
→
← H + C 6 H 5O
2−
+
→
← H + CO
4.9 × 10 −10
2.4 × 10 −12
3
← H + + O2 −
NH 3
+
← H + NH 2
1.3 × 10 −10
5.6 × 10 −11
2.2 × 10 −13
1.0 × 10 −14
very small
−
very small
STRONG
OH −
Data Page 7.5 × 10 − 3
4.6 × 10 − 4
Hydroxide ion
Ammonia
7
1.2 × 10 − 2
→ H + + NO
←
2
+
−
→
H
+
F
←
+
−
→
← H + HCOO
H2O
HPO 4 2 −
1.5 × 10 − 2
6 5
−
Water
Monohydrogen phosphate ion
H2O2
5.9 × 10 − 2
+
→
← H + SO 4
−
+
→
← H + H 2 PO 4
+
2+
→
← H + Fe(H 2 O)5 (OH)
−
+
→
← H +H C H O
2
large
large
large
large
large
large
1.7 × 10 −1
3
2−
→ H + + HO −
←
2
3−
+
→
H
+
PO
←
4
+
−
→
← H + OH
Hydrogen peroxide
very
very
very
very
very
very
1.0
STRENGTH OF BASE
STRENGTH OF ACID
HIO 3
Sulphurous (SO 2 + H 2 O)
Hexaaquoiron ion, iron( III ) ion
WEAK
HClO 4
HI
HBr
HCl
HNO 3
H 2 SO 4
H 3O +
Base
WEAK
Perchloric
Hydriodic
Hydrobromic
Hydrochloric
Nitric
Sulphuric
Hydronium Ion
Acid
Chemistry 12
ACID-BASE INDICATORS
Indicator
Chemistry 12
pH Range in Which
Colour Change Occurs
Colour Change
as pH Increases
Methyl violet
0.0 – 1.6
yellow to blue
Thymol blue
1.2 – 2.8
red to yellow
Orange IV
1.4 – 2.8
red to yellow
Methyl orange
3.2 – 4.4
red to yellow
Bromcresol green
3.8 – 5.4
yellow to blue
Methyl red
4.8 – 6.0
red to yellow
Chlorophenol red
5.2 – 6.8
yellow to red
Bromthymol blue
6.0 – 7.6
yellow to blue
Phenol red
6.6 – 8.0
yellow to red
Neutral red
6.8 – 8.0
red to amber
Thymol blue
8.0 – 9.6
yellow to blue
Phenolphthalein
8.2 – 10.0
colourless to pink
Thymolphthalein
9.4 – 10.6
colourless to blue
Alizarin yellow
10.1 – 12.0
yellow to red
Indigo carmine
11.4 – 13.0
blue to yellow
Data Page STANDARD REDUCTION POTENTIALS OF HALF-CELLS
Ionic concentrations are at 1M in water at 25°C.
Oxidizing Agents
F2 (g) + 2 e −
STRONG
+ 2e
−
H 2 O 2 + 2H + + 2e −
MnO 4 − + 8H + + 5e −
Au 3+ + 3e −
BrO 3 − + 6H + + 5e −
ClO 4 − + 8H + + 8e −
Cl 2 (g) + 2 e −
Cr2 O 7 2 − + 14H + + 6e −
1
2
O 2 (g) + 2 H + + 2 e −
MnO 2 (s) + 4H + + 2 e −
IO 3 − + 6H + + 5e −
Br2 (l) + 2 e −
AuCl 4 − + 3e −
NO 3 − + 4H + + 3e −
Hg 2 + + 2 e −
1
2
O 2 (g) + 2 H + (10 −7 M ) + 2 e −
2 NO 3 − + 4H + + 2 e −
Ag + + e −
1
2
Hg 2 2 + + e −
STRENGTH OF OXIDIZING AGENT
O 2 (g) + 2 H + + 2 e −
MnO 4 − + 2 H 2 O + 3e −
I 2 (s) + 2 e −
Cu + + e −
H 2 SO 3 + 4H + + 4e −
Cu 2 + + 2 e −
SO 4 2 − + 4H + + 2 e −
Cu
2+
+e
−
Sn 4 + + 2 e −
S(s) + 2 H + + 2 e −
2H + + 2e −
Pb 2 + + 2 e −
Sn 2 + + 2 e −
Ni 2 + + 2 e −
H 3 PO 4 + 2 H + + 2 e −
Co 2 + + 2 e −
Se(s) + 2 H + + 2 e −
Cr 3+ + e −
2H 2 O + 2e −
Overpotential
Effect
Fe
2+
+ 2e
−
Ag 2 S(s) + 2 e −
Cr 3+ + 3e −
Zn 2 + + 2 e −
Te(s) + 2 H + + 2 e −
2H 2 O + 2e −
Mn 2 + + 2 e −
Al 3+ + 3e −
Mg 2 + + 2 e −
→ Mn + 4H O
←
2
→
← Au(s)
1
→
Br (l) + 3H O
←
+1.51
+ 2.01
+1.78
2
2+
+1.50
2
+1.48
−
→
← Cl + 4H 2 O
−
→
← 2Cl
3+
→
← 2Cr + 7H O
+1.36
2
2
2
→
← H2O
2+
→
← Mn + 2 H 2 O
1
→
I (s) + 3H O
←
2 2
2
−
→
← 2 Br
→
(
) + 4Cl −
Au
s
←
→
(
) + 2H O
NO
g
←
2
→
← Hg(l)
→
← H2O
→
← N 2 O 4 + 2H 2 O
→ Ag(s)
←
→
← Hg(l)
2+
→
← Fe
+1.39
+1.23
+1.23
+1.22
+1.20
+1.09
+1.00
+ 0.85
+ 0.82
+ 0.80
+ 0.80
+ 0.80
+ 0.77
→
← H2O2
−
→
← MnO 2 (s) + 4OH
−
→
← 2I
+ 0.70
→
← Cu(s)
→
← S(s) + 3H 2 O
→
← Cu(s)
+ 0.52
→
← H 2 SO 3 + H 2 O
+
→
← Cu
2+
→
Sn
←
+ 0.17
+ 0.60
+ 0.54
+ 0.45
+ 0.34
+ 0.15
+ 0.15
→
← H 2 S(g)
→
← H 2 (g)
→
← Pb(s)
+ 0.14
→
← Sn(s)
→
← Ni(s)
→ H PO + H O
←
3
3
2
→
← Co(s)
→
← H Se
− 0.14
2
2+
+ 0.00
− 0.13
− 0.26
− 0.28
− 0.28
− 0.40
→
← Cr
−
−7
→
← H 2 + 2 OH (10 M )
− 0.41
→
← Fe(s)
2−
→
← 2 Ag(s) + S
→
← Cr(s)
− 0.45
→
← Zn(s)
→
← H 2 Te
−
→
← H (g) + 2 OH
− 0.76
→
← Mn(s)
→
← Al(s)
→
← Mg(s)
−1.19
2
− 0.41
− 0.69
− 0.74
− 0.79
− 0.83
−1.66
− 2.37
− 2.93
Cs + + e −
→
← K(s)
→
← Rb(s)
→
← Cs(s)
− 3.03
Li + + e −
→
← Li(s)
− 3.04
2+
+ 2e
−
Ba 2 + + 2 e −
K+ + e−
Rb + + e −
− 2.87
− 2.89
− 2.91
− 2.98
STRONG
Sr 2 + + 2 e −
Overpotential
Effect
+ 0.96
− 2.71
Ca
WEAK
+ 2.87
→
← Na(s)
→
← Ca(s)
→
← Sr(s)
→
← Ba(s)
Na + + e −
Data Page −
→
← 2F
2−
→
← 2SO 4
→
← 2H O
STRENGTH OF REDUCING AGENT
Fe 3+ + e −
E° (Volts)
WEAK
S2 O 8
2−
Reducing Agents
Chemistry 12
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• Students must not possess any book, paper or item that might assist in writing
an examination, including a dictionary or piece of electronic equipment, that is
not specifically authorized for the examination by ministry policy.
• Students must not copy, plagiarize or present as one’s own, work done by any
other person.
• Students must immediately follow the invigilator’s order to stop writing at the end
of the examination time and must not alter an Examination Booklet, Response
Booklet or Answer Sheet after the invigilator has asked students to hand in
examination papers.
• Students must not remove any piece of the examination materials from the
examination room, including work pages.
4. The use of inappropriate language or content may result in a mark of zero
being awarded.
5. Upon completion of the examination, return all examination materials to the
supervising invigilator.
2
Place Personal Education Number (PEN) here.
3. Cheating on an examination will result in a mark of zero. The Ministry of Education
considers cheating to have occurred if students break any of the following rules:
• Students must not communicate with other students during the examination.
1
1
2
Question 4
0
Course Code = CH 12
Chemistry 12
2008/09 Released Exam
JUNE 2009
Response Booklet
Instructions:
Answer the following questions in the space
provided in this Response Booklet. You are
expected to communicate your knowledge
and understanding of chemical principles in
a clear and logical manner. Your steps and
assumptions leading to a solution must be
written in this Response Booklet. Answers
must include units where appropriate
and be given to the correct number of
significant figures. For questions involving
calculations, full marks will NOT be given
for providing only an answer.
A
B
C
D
E
F
2
3
(.5) NR
12
Course Code = CH
2008/09 Released Exam
JUNE 2009
Exam Booklet
Form/
,
Cahier d examen
1
Question 5
0
G
1
2
3
4
5
(.5) NR
H
Question 6
0
Student Instructions
1. Place your Personal Education Number
(PEN) label at the top of this Booklet AND
fill in the bubble (Form A, B, C, D, E, F, G
or H) that corresponds to the letter on your
Examination Booklet.
1
2
3
Question 7
0
1
2
3
(.5) NR
4
(.5) NR
Question 8
0
1
2
3
(.5) NR
2. Use a pencil to fill in bubbles when
answering questions on your Answer Sheet.
3. Use a pencil or blue- or black-ink pen when
answering written-response questions in
this Booklet.
4. When the examination begins, remove the
Data Pages located in the centre of the
Examination Booklet.
5. Read the Examination Rules on the back of
this Booklet.
814
© Province of British Columbia
Version 0601.1
PART B: WRITTEN RESPONSE
Value: 37.5% of the examination
Suggested Time: 40 minutes
1. (4 marks)
A student burned a paraffin candle ( C25 H 52 ) in an open beaker according to the following equation:
C25 H 52 ( s ) + 38 O 2 ( g ) 25CO 2 ( g ) + 26 H 2 O ( g )
The following data was recorded:
Time (min)
Mass of candle
and beaker (g)
0.0
175.00
2.0
173.20
Calculate the rate of paraffin consumption in moles of C25 H 52 per minute ( mol C25 H 52 min ) ;
then, calculate how long it would take to produce 0.70 g CO 2 .
Chemistry 12 – 0906 Response Booklet
Page 1
2. (4 marks)
Consider the following equilibrium:
CO ( g ) + 3H 2 ( g ) CH 4 ( g ) + H 2 O ( g )
Initially, 0.200 mol CO and 0.600 mol H 2 are placed in a 2.00 L container. At equilibrium,
[ H 2O ] = 0.039 M . Calculate the value of K eq .
Page 2
Chemistry 12 – 0906 Response Booklet
3. (4 marks)
Consider the following equilibrium:
2+
Mg ( OH )2 ( s ) Mg ( aq ) + 2OH ( aq )
What happens to the amount of solid Mg ( OH ) 2 when some HCl is added?
On the graph below, sketch the effect of adding HCl at time t 1 .
Mg2+
Concentration
(M)
OH-
t1
Chemistry 12 – 0906 Response Booklet
Time (s)
Page 3
4. (3 marks)
A solution of Sr ( OH )2 ( aq ) is titrated with H 2SO 4 .
Explain what will happen to the electrical conductivity during the titration.
Begin by writing the balanced formula equation, including states, to support your answer.
Page 4
Chemistry 12 – 0906 Response Booklet
5. (5 marks)
Aniline ( C6 H 5 NH 2 ) is a weak base with a K b = 4.3 10 10 .
Calculate the concentration of an aniline solution that has a pH = 8.80 .
Begin by writing the equation for the predominant equilibrium.
Chemistry 12 – 0906 Response Booklet
Page 5
6. (3 marks)
Calculate the [ OH ] that results when 800.0 mL of 0.010 M HCl is mixed with 1.216 g Sr ( OH )2 .
(Assume no volume change on mixing.)
Page 6
Chemistry 12 – 0906 Response Booklet
7. (4 marks)
Balance the following redox equation in acidic solution:
Te O 4 + In In 2 O3 + Te
Chemistry 12 – 0906 Response Booklet
(acidic)
Page 7
8. (3 marks)
Consider the following cell diagram:
Power
Supply
–
+
Cu(s)
Pb(s)
1 M K2SO4
Write the overall cell reaction.
Write the formula for a precipitate that forms as the cell operates.
Page 8
Chemistry 12 – 0906 Response Booklet
MINISTRY USE ONLY
MINISTRY USE ONLY
MINISTRY USE ONLY
Question 1
0
1
2
3
4
(.5) NR
3
4
(.5) NR
3
4
(.5) NR
Examination Rules
Question 2
1. The time allotted for this examination is two hours. You may, however, take up to 60 minutes of additional time to finish.
2. Answers entered in the Examination Booklet will not be marked.
0
Place Personal Education Number (PEN) here.
Question 3
0
• Students must not be in possession of or have used any secure examination
materials prior to the examination session.
• Students must not give or receive assistance of any kind in answering an
examination question during an examination, including allowing one’s paper to
be viewed by others or copying answers from another student’s paper.
• Students must not possess any book, paper or item that might assist in writing
an examination, including a dictionary or piece of electronic equipment, that is
not specifically authorized for the examination by ministry policy.
• Students must not copy, plagiarize or present as one’s own, work done by any
other person.
• Students must immediately follow the invigilator’s order to stop writing at the end
of the examination time and must not alter an Examination Booklet, Response
Booklet or Answer Sheet after the invigilator has asked students to hand in
examination papers.
• Students must not remove any piece of the examination materials from the
examination room, including work pages.
4. The use of inappropriate language or content may result in a mark of zero
being awarded.
5. Upon completion of the examination, return all examination materials to the
supervising invigilator.
2
Place Personal Education Number (PEN) here.
3. Cheating on an examination will result in a mark of zero. The Ministry of Education
considers cheating to have occurred if students break any of the following rules:
• Students must not communicate with other students during the examination.
1
1
2
Question 4
0
Course Code = CH 12
Chemistry 12
2008/09 Released Exam
JUNE 2009
Response Booklet
Instructions:
Answer the following questions in the space
provided in this Response Booklet. You are
expected to communicate your knowledge
and understanding of chemical principles in
a clear and logical manner. Your steps and
assumptions leading to a solution must be
written in this Response Booklet. Answers
must include units where appropriate
and be given to the correct number of
significant figures. For questions involving
calculations, full marks will NOT be given
for providing only an answer.
A
B
C
D
E
F
2
3
(.5) NR
12
Course Code = CH
2008/09 Released Exam
JUNE 2009
Exam Booklet
Form/
,
Cahier d examen
1
Question 5
0
G
1
2
3
4
5
(.5) NR
H
Question 6
0
Student Instructions
1. Place your Personal Education Number
(PEN) label at the top of this Booklet AND
fill in the bubble (Form A, B, C, D, E, F, G
or H) that corresponds to the letter on your
Examination Booklet.
1
2
3
Question 7
0
1
2
3
(.5) NR
4
(.5) NR
Question 8
0
1
2
3
(.5) NR
2. Use a pencil to fill in bubbles when
answering questions on your Answer Sheet.
3. Use a pencil or blue- or black-ink pen when
answering written-response questions in
this Booklet.
4. When the examination begins, remove the
Data Pages located in the centre of the
Examination Booklet.
5. Read the Examination Rules on the back of
this Booklet.
814
© Province of British Columbia
Version 0601.1