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<b>Chemistry 12</b>

Examination Booklet

August 2006

<b>Form A</b>

<b>DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.</b>

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<b>PART A: MULTIPLE CHOICE</b>

<b>Suggested Time: 80 minutes</b>
<b>INSTRUCTIONS: For each question, select the best answer and record your choice on the Answer</b>

<b>Sheet provided. Using an HB pencil, completely fill in the bubble that has the letter</b>

corresponding to your answer.

<b>You have Examination Booklet Form A. In the box above #1 on your Answer Sheet, fill in the</b>
bubble as follows.

F

A B C D E G H

Exam Booklet Form/
Cahier d’examen

<b>1. Which of the following would not be units for reaction rate?</b>
A. g s

B. M min
C. kJ mol
D. kPa min

2. Consider the reaction:

2Al s

( )

+ 3CuCl aq₂

( )

Ỉ 2AlCl aq₃

( )

+ 3Cu s

( )

What is the rate of Al consumption in mol min if 0 98. g Cu are produced in 2.5 minutes?
A. 4 1. ¥10-3mol min

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Page 2 Chemistry 12 – 0608 Form A
3. Which of the following describes what happens to the KE and PE as an activated complex

forms products?

KE PE

A. decreases increases

B. decreases decreases

C. increases increases

D. increases decreases

<b>Use the following reaction mechanism to answer questions 4 and 5.</b>

Step 1: 2NO Ỉ N O₂ ₂ (fast)

Step 2: N O₂ ₂ + H₂ Ỉ N O₂ + H O₂ (slow)

Step 3: N O₂ + H₂ Ỉ N₂ + H O₂ (fast)

4. Increasing the concentration of which of the following substances would cause the greatest increase
in the reaction rate?

A. H₂
B. NO
C. N O₂
D. H O₂

5. Which of the following are products in the overall reaction?

I N₂

II N O₂ ₂

III N O₂

IV H O₂

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<b>Use the following diagram to answer questions 6 and 7.</b>

. . . .

Progress of the reaction
PE

(kJ)

300
250
200
150
100
50
0

6. Which of the following are the values for the activation energy

( )

E<i>_a</i> and change in enthalpy

(

DH

)

for the reverse reaction?

E<i>a</i>

( )

kJ DH kJ

( )

A. 300 –50

B. 150 +50

C. 100 –50

D. 100 +50

7. If the above PE diagram represents a reversible reaction that reaches equilibrium, which of the
following must be true for the forward reaction?

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Page 4 Chemistry 12 – 0608 Form A
8. Consider the following:

energy + NH SH s₄

( )

ặ_ă? NH g₃

( )

+ H S g₂

( )

Which of the following describes how enthalpy and entropy change in the forward direction?

Enthalpy Entropy

A. increasing increasing

B. increasing decreasing

C. decreasing decreasing

D. decreasing increasing

9. Consider the following diagram for the equilibrium system:

N O g₂ ₄

( )

+ energy ặ_ă 2NO g₂

( )

Time (min)

Concentrations (M)

t₁

NO₂
N₂O₄

Which of the following stresses was applied at time t₁?
A.

[

NO₂

]

was increased.

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10. Styrene is manufactured as follows:

C H CH CH g kJ C H CHCH g H g

styrene

6 5 2 3

( )

+123 ặă 6 5 2

( )

+ 2

( )

Which of the following describes the temperature and pressure needed for the maximum
yield of styrene?

Temperature Pressure

A. low low

B. low high

C. high low

D. high high

11. Consider the following reactions:

I Na O s₂

( )

_ăặ 2Na

( )

l + ₂1O g₂

( )

K<i>_eq</i> =2 Ơ10-25

II Na O s₂ ₂

( )

ặ_ă 2Na

( )

_l + O g₂

( )

K<i>_eq</i> = 5 ¥10-29

III 2Na O s₂

( )

ặ_ă 4Na

( )

_l + O g₂

( )

K<i>_eq</i> =3 ¥10-14

Which of the following lists the reactions in order, from the greatest

[

O₂

]

at equilibrium, to the
least

[

O₂

]

at equilibrium?

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Page 6 Chemistry 12 – 0608 Form A
12. Consider the equilibrium:

CaCO s₃

( )

ặ_ă CaO s

( )

+ CO g₂

( )

In a 5 0. L container at equilibrium there are 2 42. g CO , 1 00₂ . g CaCO and ₃ 1 00. g CaO.
Which of the following is the value of K<i>_eq</i>?

A. 0 055.
B. 0 011.
C. 0 020.
D. 91

13. Consider the following equilibrium:

CCl g₄

( )

ặ_ă C s

( )

+ 2Cl g₂

( )

Initially, 0 31. mol CCl was placed in a ₄ 1 0. L container. At equilibrium,

[

Cl₂

]

= .0 060M.
Which of the following is the value of K<i>_eq</i>?

A. 3 9. ¥10-4
B. 1 3. ¥10-2
C. 1 4. ¥10-2
D. 7 8. ¥101

14. Consider the following equilibrium:

3NO g₂

( )

_ăặ N O g₂ ₅

( )

+ NO g

( )

K<i>_eq</i> =1 0. ¥10-11

Initially, some NO₂, N O₂ ₅ and NO were placed in a container and allowed to reach equilibrium.
When equilibrium was established, it was found that the pressure had increased. Which of the
following explains what happened?

A. Trial K<i>eq</i> > K<i>eq</i> so the system shifted left.

B. Trial K<i>_eq</i> < K<i>_eq</i> so the system shifted left.
C. Trial K<i>eq</i> > K<i>eq</i> so the system shifted right.

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15. Which condition is essential to prepare a saturated solution of an ionic salt?
A. an excess of solute

B. any amount of solute
C. a temperature of 25∞C
D. a fixed volume of solvent

16. Which compound will have the greatest solubility?
A. CoS

B. CuS
C. FeS
D. MgS

17. What is the net ionic equation for the reaction between equal volumes
of 0 20. M BaS and 0 20. M BeSO ?₄

A. Be2+

( )

aq + S2-

( )

aq Ỉ BeS s

( )

B. Ba2+

( )

aq + SO₄2-

( )

aq Ỉ BaSO s₄

( )

C. BaS aq

( )

+ BeSO aq4

( )

Ỉ BaSO s4

( )

+ BeS s

( )

D. Ba2+

( )

aq + S2-

( )

aq + Be2+

( )

aq + SO₄2-

( )

aq Æ BaSO s₄

( )

+ Be2+

( )

aq + S2-

( )

aq

18. Which of the following substances will have the least effect on the equilibrium in a saturated
solution of PbI s₂( )?

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Page 8 Chemistry 12 – 0608 Form A
19. Which equation has the K<i>_sp</i> expression: K<i>_sp</i> =

[

Al3+

]

2

[

SO₄2-

]

3 ?

A. 2Al3+( )aq + 3SO₄2-( )aq Ỉ Al SO₂( _{4 3}) ( )s
B. Al SO₂( _{4 3}) ( ) ặs _ă Al3+( ) +aq SO₄2-( )aq
C. Al SO₂( _{4 3}) ( ) ặs _ă 2Al3+( ) +aq 3SO₄2-( )aq
D. 3Al3+( ) +aq 2SO₄2-( ) ặaq _ă Al SO₂( _{4 3}) ( )s

20. What is the K<i>_sp</i> for Zn OH( )₂ if it has a solubility of 1 3. ¥10-7mol L ?
A. 2 2. ¥10-21

B. 8 8. ¥10-21
C. 1 7. ¥10-14
D. 3 6. ¥10-4

21. Which compound will have the lowest solubility?
A. AgNO₃

B. AgBrO₃
C. SrSO₄
D. SrCO₃

22. A definition for a Brønsted-Lowry acid should contain which of the following phrases?
A. the donation of H+

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-23. Which equation represents the reaction of a Brønsted-Lowry base with water?

A. 2Na + 2H O₂ Ỉ 2NaOH + H₂

B. N H₂ ₄ + H O₂ ặ_ă N H₂ ₅+ + OH
-C. HPO₄2- + H O₂ _ăặ H O₃ + + PO₄3
-D. H C O₂ ₂ ₄ + H O₂ _ăặ H O₃ + + HC O₂ ₄

-24. Given the equilibrium:

H BO₂ ₃- + H PO₂ ₄- _ăặ H BO₃ ₃ + HPO₄2
-Which is the strongest acid?

A. HPO₄2
-B. H BO₃ ₃
C. H PO₂ ₄
-D. H BO₂ ₃

-25. Which species will result in a solution with the greatest

[

H O₃ +

]

?
A. NaCN

B. Na PO₃ ₄
C. Na CO₂ ₃
D. Na C O₂ ₂ ₄

<b>26. Which species is not amphiprotic?</b>
A. H O₂

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-Page 10 Chemistry 12 – 0608 Form A
27. At a given temperature a sample of pure water has a pH= 7 10. .

Which of the following is true?

Sample Reason

A. acidic pH > 7 00.
B. _basic pH > 7 00.

C. _neutral pOH < pH

D. _neutral _{H O} _OH

3

+

-[

]

=

[

]

28. Which of the following is a definition of pH?
A. pH= log

[

H O₃ +

]

B. pH= pOH + 14
C. pH= -log

[

H O₃ +

]

D. pH= pOH + pK<i>_w</i>

29. What is the mass of NaOH required to prepare 100 0. mL of NaOH aq( ) that
has a pH= 13 62. ?

A. 0 38. g
B. 0 42. g
C. 1 67. g

D. 2 40. ¥10-14g

30. Which of the following hypothetical acids would have the lowest conductivity?

Acid K<i>a</i>

A. _{0 5}_{. M HY} _{1 0}_. _¥₁₀-1

B. 1 0. M HA 1 0. ¥10-6

C. _{1 0}

2

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31. What is the net ionic equation for the hydrolysis of NH Cl₄ ?
A. NH Cl aq₄ ( ) ặ_ă NH₄+( ) +aq Cl aq-( )

B. Cl aq-

( )

+ H O₂

( )

l ặ_ă HCl aq

( )

+ OH-

( )

aq
C. NH₄+

( )

aq + H O₂

( )

_l _ăặ H O aq₃ +

_{( )}

₊ NH₃

_{( )}

aq
D. NH₄+( ) +aq H O₂ ( ) Ỉ_l _ă HNH₄2+( ) +aq OH aq-( )

32. What is the approximate pH of a 0 1. M solution of the salt NH Cl₄ ?
A. 1 0.

B. 5 0.
C. 7 0.
D. 9 0.

33. Consider the following indicator equilibrium:

HIn aq H O H O aq In aq

colourless blue

( )

+

( )

ặ_ă +

( )

+ -

( )

2 l 3

What is the effect of adding HCl to a blue sample of this indicator?
Equilibrium Shift Colour Change

A. left less blue

B. left more blue

C. right less blue

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34. An indicator has a K<i>a</i> = ¥

-4 10 6. Which of the following is true for this indicator?
pH at Transition Point Indicator

A. _{4 0}_. methyl orange

B. _{4 0}_. bromcresol green

C. _{5 4}_. methyl red

D. _{5 4}_. bromcresol green

35. Oxalic acid dihydrate is a pure, stable, crystalline substance. Which of the following
describes one of its uses in acid-base titrations?

A. buffer

B. primary standard
C. chemical indicator
D. stoichiometric indicator

36. What is the net ionic equation that describes the reaction of HCl aq with Pb OH

( )

(

) ( )

₂ s ?
A. H aq+( ) + OH aq-( ) Ỉ H O₂ ( )l

B. 2HCl aq

( )

+ Pb OH

(

) ( )

₂ <i>s</i> Ỉ PbCl s₂

( )

+ 2H O₂

( )

l

C. 2H aq+( ) + 2Cl aq-( ) + Pb OH( ) ( ) Ỉ₂ s PbCl s₂( ) + 2H O₂ ( )_l

D. 2H aq+( ) + 2Cl aq-( ) + Pb2+( ) +aq 2OH aq-( ) Æ Pb2+( ) +aq 2Cl aq-( ) + 2H O₂ ( )l

37. Which of the following would be used to prepare an acidic buffer solution?
A. HF and H O₃ +

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Chemistry 12 – 0608 Form A Page 13
38. Four samples of rain are collected from different geographic regions and

the pH is measured for each sample.

Sample pH

1 2.8

2 4.0

3 6.2

4 6.8

<i>Which of the above samples would be classified as acid rain?</i>
A. 1 only

B. 1 and 2
C. 1, 2 and 3
D. 1, 2, 3 and 4

<i>39. Which of the following best describes the process of oxidation?</i>
A. the process in which oxygen is given off

B. the process in which electrons are gained

C. the process in which the oxidation number decreases
D. the process in which the oxidation number increases

40. What is the oxidation number of N in the mercury(II) compound Hg NH

(

_{3 2}

)

Cl₂?
A. -6

B. -4
C. -3
D. +3

41. Which of the following combinations will react spontaneously under standard conditions?
A. Ag + Br₂

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42. Which of the following is a correctly balanced reduction half-reaction?
A. 2HCN + 2e- Ỉ C N₂ ₂ + 2H+

B. 2Sb + 3H O₂ + 6e- Ỉ Sb O₂ ₃ + 6H+
C. NO₃- + 3H+ + 3e- Ỉ HNO₂ + H O₂
D. Sb O₂ ₅ + 6H+ + 4e- Ỉ 2Sb OH

(

)

₂+ + H O₂

43. Which of the following ion concentrations could be determined by a redox titration using
nitric acid? Assume the use of a suitable indicator.

A. Br
-B. Ni2+
C. Fe2+
D. Mn2+

44. A solution of KMnO₄ is standardized using oxalic acid

(

H C O₂ ₂ ₄

)

according to the following
equation:

2MnO₄- + 5H C O₂ ₂ ₄ + 6H+ Ỉ 2Mn2+ +10CO₂ + 8H O₂

The titration of 0 134. g of oxalic acid required 24 70. mL of KMnO solution. What is the₄
molarity of the KMnO₄ solution?

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Chemistry 12 – 0608 Form A Page 15

<b>Use the following diagram to answer questions 45 to 47.</b>

Volts

1.0M KNO3 Anode

Cu

Cathode
Pt
(inert)
Layer 1: 1.0 M NaBr(aq)

1.0 M Cu(NO₃)₂
Layer 2: Br₂(l)

45. What is the cathode reaction for this cell?
A. Na+ + e- Ỉ Na

B. Br₂ + 2e- Ỉ 2Br
-C. 2Br- Ỉ Br₂ + 2e

-D. H O₂ Æ ₂1O₂ + 2H+ + 2e

-46. Which of the following best describes the movement of potassium ions and
electrons as the cell operates?

K+ Ion
Movement

Electron
Movement

A. towards the Cu towards the Pt
B. towards the Cu towards the Cu
C. towards the Pt towards the Cu
D. towards the Pt towards the Pt

47. What is the standard cell voltage?
A. -0 75. V

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48. A student constructs three standard electrochemical cells using the metals Pd, Cd and Ga with
1 0. M solutions of their ions. The student then records the voltages of Cell 1 and Cell 2 in the
following table.

Cell Anode Cathode Voltage

1 Ga Pd +1 18. V

2 Ga Cd +0 16. V

3 Cd Pd ?

What voltage should Cell 3 produce?
A. -1 34. V

B. -1 02. V
C. +1 02. V
D. +1 34. V

49. Which of the following would prevent the corrosion of an iron nail?
A. Store the nail inCl g₂

( )

.

B. Store the nail in dry air.

C. Store the nail in a beaker of distilled water.

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Chemistry 12 – 0608 Form A Page 17
50. Consider the electrolytic cell shown in the following diagram:

1.0 M AgNO₃

DC
Power
Source

Cu
Pt

(inert)

–

+

Which of the following describes the anion movement and electrode masses for the above cell?
Anion

Movement

Mass of Pt
Electrode

Mass of Cu
Electrode

A. to the Cu increases increases
B. to the Cu increases decreases
C. to the Pt decreases increases
D. to the Pt decreases decreases

<b>You have Examination Booklet Form A. In the box above #1 on your Answer Sheet, ensure that</b>
you have filled in the bubble as follows.

F

A B C D E G H

Exam Booklet Form/
Cahier d’examen

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<i>12</i> <i> at 12.00.</i>
<i>ally</i>
<i>.</i>

P

ERIODIC

T

ABLE OF
THE

E

LEMENTS
3
4
5
6
7

8
9
10
11
12
13
14
15
16
17
18
21 <b>_Sc</b>
Scandium 45.0
22 <b>_Ti</b>
Titanium 47.9
39 <b>Y</b>
Yttr
ium
88.9
40 <b>_Zr</b>
Zirconium 91.2
57 <b>_La</b>
Lanthan
um
138.9
72 <b>_Hf</b>
Hafnium 178.5
89 <b>_Ac</b>
Actinium (227)
104 <b>Rf</b>

Rutherf
ordium
(261)
23 <b>V</b>
V
anadium 50.9
24 <b>_Cr</b>
Chromium 52.0
41 <b>_Nb</b>
Niobium 92.9
42 <b>_Mo</b>
Molybden
um
95.9
73 <b>_Ta</b>
Tantalum 180.9
74 <b>_W</b>
Tungsten 183.8

105 <b>_Db</b> _Dubnium ₍₂₆₂₎
106 <b>Sg</b>

Seaborgium (263)

25 <b>_Mn</b>

Manganese 54.9

26 <b>_Fe</b> Iron _55.8

43 <b>_Tc</b>
Technetium (98)
44 <b>_Ru</b>
Ruthenium 101.1
75 <b>_Re</b>
Rhenium 186.2
76 <b>_Os</b>
Osmium _190.2

107 <b>_Bh</b> _Bohr

ium

(262)

108 <b>Hs</b> _Hassium ₍₂₆₅₎
27 <b>_Co</b> _Cobalt _58.9 45 <b>_Rh</b>

Rhodium 102.9 77 <b>Ir</b> Iridium _192.2 109 <b>Mt</b>

Meitner

ium

(266)

28 <b>_Ni</b> Nicke

l

58.7 78 <b>Pt</b> Platin

um

195.1

29 <b>_Cu</b>

Copper 63.5 47 <b>Ag</b> Silv

er

107.9 79 <b>Au</b> Gold 197.0
30 <b>_Zn</b> Zinc _65.4 48 <b>_Cd</b>

Cadmium 112.4
80 <b>_Hg</b>
Mercur
y
200.6
5 <b>_B</b>

Boron _10.8 13 <b>Al</b>

Alumin

um

27.0 31 <b>Ga</b> Gallium 69.7 49 <b>In</b> Indium _114.8 81 <b>Tl</b> _Thallium _204.4

6 <b>_C</b>

Carbon 12.0 14 <b>Si</b> Silicon 28.1 32 <b>Ge</b>

Ger

manium _72.6 50 <b>_Sn</b> Tin

118.7 82 <b>Pb</b> Lead 207.2
7 <b>_N</b>

Nitrogen 14.0 15 <b>P</b>

Phosphor

us

31.0 33 <b>As</b> Arsenic 74.9 51 <b>Sb</b> _Antimon

y

121.8 83 <b>Bi</b> Bism

uth

209.0

8 <b>_O</b>

Oxygen 16.0 16 <b>S</b> Sulphur 32.1 34 <b>Se</b> _Selenium 79.0 52 <b>Te</b> Tellur

ium

127.6 84 <b>Po</b> Polonium (209)

9 <b>_F</b>

Fluor

ine

19.0 17 <b>Cl</b> Chlor

ine

35.5 35 <b>Br</b> Bromine 79.9 53 <b>I</b> Iodine 126.9 85 <b>At</b> Astatine (210)
10 <b>_Ne</b> Neon _20.2 18 <b>Ar</b> Argon _39.9 36 <b>Kr</b> _Krypton _83.8 54 <b>Xe</b> Xenon _131.3 86 <b>Rn</b> Radon ₍₂₂₂₎

2

<b>He</b> Helium 4.0

58 <b>_Ce</b> _Cerium

140.1 90 <b>Th</b> Thor

ium
232.0
59 <b>_Pr</b>
Pr

aseodymium 140.9
91 <b>_Pa</b>
Protactinium 231.0
60 <b>_Nd</b>
Neodymium 144.2
92 <b>U</b>
Ur
anium
238.0
61 <b>_Pm</b>
Promethium (145)
93 <b>_Np</b>
Neptunium (237)
62 <b>_Sm</b>
Samar
ium

150.4 94 <b>Pu</b> Plutonium (244)

63 <b>_Eu</b>

Europium 152.0 95 <b>Am</b> Amer

icium

(243)

64 <b>_Gd</b>

Gadolinium 157.3

96 <b>_Cm</b> _Curium

(247)

65 <b>_Tb</b>

Terbium _158.9 97 <b>Bk</b> _Berkelium (247)
66 <b>_Dy</b>
Dysprosium 162.5
98 <b>_Cf</b>
Calif
or
nium
(251)
67 <b>_Ho</b>

Holmium 164.9 99 <b>Es</b> _Einsteinium (252)
68 <b>_Er</b> _Erbium

167.3 100 <b>Fm</b> Fe

rmium

(257)

69 <b>_Tm</b>

Thulium _168.9 101 <b>Md</b>

Mendele

vium

(258)

70 <b>_Yb</b>

Ytterbium 173.0 102 <b>No</b> Nobelium (259)

71 <b>_Lu</b>

Lutetium 175.0 103 <b>Lr</b> _Lawrencium ₍₂₆₂₎

46 <b>_Pd</b>

P

alladium _106.4

 _

 


Atomic Number Symbol Name Atomic Mass

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A

TOMIC

M

ASSES OF THE

E

LEMENTS

<i>Based on mass of C12_{at 12.00.}</i>

<i>Values in parentheses are the mass number of the most stable or best</i>
<i>known isotopes for elements that do not occur naturally.</i>

Data Page 2 Chemistry 12

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
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)
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

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

<b>Element</b> <b>Symbol</b> <b>Atomic</b>

<b>Number</b>

<b>Atomic</b>

<b>Mass</b> <b>Element</b> <b>Symbol</b>

<b>Atomic</b>
<b>Number</b>

</div>
<span class='text_page_counter'>(23)</span><div class='page_container' data-page=23>

N

AMES,

F

ORMULAE, AND

C

HARGES OF

S

OME

C

OMMON

I

ONS

<i> * Aqueous solutions are readily oxidized by air.</i>
<i>** Not stable in aqueous solutions.</i>

<b>Negative Ions</b>
<b>(Anions)</b>
<b>P o s i t i v e I o n s</b>

<b>( C a t i o n s )</b>

Aluminum

Ammonium
Barium
Calcium

Chromium(II), chromous
Chromium(III), chromic
Copper(I)*, cuprous
Copper(II), cupric
Hydrogen
Hydronium
Iron(II)*, ferrous
Iron(III), ferric
Lead(II), plumbous
Al3+

NH₄+
Ba2+
Ca2+
Cr2+
Cr3+
Cu+
Cu2+
H+
H₃O+
Fe2+
Fe3+
Pb2+
Hydroxide
Hypochlorite
Iodide

Monohydrogen phosphate
Nitrate
Nitrite
Oxalate
Oxide**
Perchlorate
Permanganate
Phosphate
Sulphate
OH–
ClO–
I–
HPO₄2–
NO₃–
NO₂–
C₂O₄2–
O2–
ClO₄–
MnO₄–
PO₄3–
SO₄2–
S2–
Bromide
Carbonate
Chlorate
Chloride
Chlorite
Chromate
Cyanide
Dichromate

Dihydrogen phosphate
Ethanoate, acetate
Fluoride

Hydrogen carbonate, bicarbonate
Hydrogen oxalate, binoxalate
Br–

CO₃2–
ClO₃–
Cl–
ClO₂–
CrO₄2–
CN–
Cr₂O₇2–
H₂PO₄–
CH₃COO–
F–
HCO₃–
HCO–

Lead(IV), plumbic
Lithium

Magnesium

Manganese(II), manganous
Manganese(IV)

Mercury(I)*, mercurous

Mercury(II), mercuric
Potassium

Silver
Sodium

</div>
<span class='text_page_counter'>(24)</span><div class='page_container' data-page=24>

S

OLUBILITY OF

C

OMMON

C

OMPOUNDS IN

W

ATER

<i>The term soluble here means</i>> 0.1 mol/L at 25<i>∞C.</i>

<b>Negative Ions</b>
<b>(Anions)</b>
<b>Positive Ions</b>
<b>(Cations)</b>
<b>Solubility of</b>
<b>Compounds</b>
All
All
All
Soluble
Soluble
Soluble
All Soluble
Soluble
Low Solubility
All others
Soluble
Low Solubility
Soluble
Low Solubility

Soluble
Low Solubility
Soluble
Low Solubility
All others
All others
All others
All others
or
or
or
or
¸
˝
Ơ
Ơ
Ơ
Ơ
˛
Ơ
Ơ
Ơ
Ơ
¸
˝
Ơ
Ơ
Ơ
Ơ
˛

Ơ
Ơ
Ơ
Ơ
¸
˝
Ơ
Ơ
Ơ
Ơ
˛
Ơ
Ơ
Ơ
Ơ
¸
˝
Ơ
Ơ
Ơ
Ơ
˛
Ơ
Ơ
Ơ
Ơ
¸
˝
Ơ
Ơ

Ơ
Ơ
˛
Ơ
Ơ
Ơ
Ơ

Data Page 4 Chemistry 12

Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+

Ammonium ion: NH₄+

Chloride, Cl–
Bromide, Br–
Iodide, I–
Nitrate, NO₃–

Hydrogen ion: H+

Ag+, Pb2+, Cu+

Sulphide, S2–

Alkali ions, H+, NH₄+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+
Sulphate, SO₄2–

Hydroxide, OH–

Alkali ions, H+, NH₄+, Sr2+

Sulphite, SO₃2–
Phosphate, PO₄3–
Carbonate, CO₃2–

</div>
<span class='text_page_counter'>(25)</span><div class='page_container' data-page=25>

S

OLUBILITY

P

RODUCT

C

ONSTANTS AT

25

∞C

<b>Name</b> <b>Formula</b>

Barium carbonate
Barium chromate
Barium sulphate
Calcium carbonate
Calcium oxalate
Calcium sulphate
Copper(I) iodide
Copper(II) iodate
Copper(II) sulphide
Iron(II) hydroxide
Iron(II) sulphide
Iron(III) hydroxide
Lead(II) bromide
Lead(II) chloride
Lead(II) iodate
Lead(II) iodide
Lead(II) sulphate
Magnesium carbonate
Magnesium hydroxide
Silver bromate

Silver bromide
Silver carbonate
Silver chloride
Silver chromate
Silver iodate
Silver iodide
Strontium carbonate
Strontium fluoride
Strontium sulphate

BaCO₃
BaCrO₄
BaSO₄
CaCO₃
CaC₂O₄
CaSO₄
CuI
Cu(IO₃)₂
CuS
Fe(OH)₂
FeS
Fe(OH)₃
PbBr₂
PbCl₂
Pb(IO₃)₂
PbI₂
PbSO₄
MgCO₃
Mg(OH)₂
AgBrO₃

AgBr
Ag₂CO₃
AgCl
Ag₂CrO₄
AgIO₃
AgI
SrCO₃
SrF₂
SrSO₄

2.6 ¥ 10–9
1.2 ¥ 10–10
1.1 ¥ 10–10
5.0 ¥ 10–9
2.3 ¥ 10–9
7.1 ¥ 10–5
1.3 ¥ 10–12
6.9 ¥ 10–8
6.0 ¥ 10–37
4.9 ¥ 10–17
6.0 ¥ 10–19
2.6 ¥ 10–39
6.6 ¥ 10–6
1.2 ¥ 10–5
3.7 ¥ 10–13
8.5 ¥ 10–9
1.8 ¥ 10–8
6.8 ¥ 10–6
5.6 ¥ 10–12
5.3 ¥ 10–5

5.4 ¥ 10–13
8.5 ¥ 10–12
1.8 ¥ 10–10
1.1 ¥ 10–12
3.2 ¥ 10–8
8.5 ¥ 10–17
5.6 ¥ 10–10
4.3 ¥ 10–9
3.4 ¥ 10–7

</div>
<span class='text_page_counter'>(26)</span><div class='page_container' data-page=26>

Data Page 6 Chemistry 12

Perchloric HClO H ClO

Hydriodic HI H I

Hydrobromic HBr H Br

Hydrochloric HCl H Cl

Nitric HNO H NO

Sulphuric H SO H HSO

4 4

3 3

2 4 4

Ỉ +
Ỉ +
Ỉ +
Ỉ +
Ỉ +
Ỉ +
+
-+
-+
-+
-+
-+
-very large
very large
very large
very large
very large
very large

Hydronium Ion H O H H O

Iodic HIO H IO

Oxalic H C O H HC O

Sulphurous SO H O H SO H HSO

Hydrogen sulphate ion HSO H SO

3 2

3 3 1

2 2 4 2 4 2

2 2 2 3 3

2

4 4

2 2

1 0
1 7 10
5 9 10
1 5 10
1 2 10

+ +
+ -
-+ -
-+ -
-- + -
-ặ
ă +
ặ
ă + Ơ
ặ
ă + Ơ

+
( ) ặ_ă + Ơ
ặ
ă + Ơ
.
.
.
.
.

Phosphoric H PO H H PO

Hexaaquoiron ion iron ion Fe H O H Fe H O OH

Citric H C H O H H C H O

Nitrous HNO H NO

Hydrofluoric HF

III

3 4 2 4

3

2 6

3

2 5

2 3

3 6 5 7 2 6 5 7

4

2 2

4

7 5 10
6 0 10
7 1 10
4 6 10
ặ
ă + Ơ
( ) ặ_ă + ( ) ( ) Ơ
ặ
ă + Ơ
ặ
ă + Ơ
+ -
-+ + +
-+ -
-+ -
-.
, .
.

.
( )
ặ
ặ

ă H+ +F- 3 5. ¥10-4

Methanoic formic HCOOH H HCOO

Hexaaquochromium ion chromium ion Cr H O H Cr H O OH

Benzoic C H COOH H C H COO

Hydrogen oxalate ion HC O H C O

Ethanoic acetic
III
, .
, .
.
.
,
( )
ặ
ă + Ơ
( ) ặ_ă + ( ) ( ) Ơ
ặ
ă + Ơ
ặ
ă + Ơ

+ -
-+ + +
-+ -
-- + -

-1 8 10
1 5 10
6 5 10
6 4 10

4

2 6

3

2 5

2 4

6 5 6 5 5

2 4 2 42 5

CH

CH COOH₃ ặ_ă H++CH COO₃ - 1 8. ¥10-5

Dihydrogen citrate ion H C H O H HC H O

Al H O H Al H O OH

Carbonic CO H O H CO H HCO

Monohydrogen citrate ion HC H O H

2 6 5 7 6 5 72 5

2 6

3

2 5

2 5

2 2 2 3 3 7

6 5 7

2

1 7 10
1 4 10
4 3 10

- + -
-+ + +
-+ -
-- +

ặ
ă + Ơ
( ) ặ_ă + ( ) ( ) Ơ
+
( ) ặ_ă + Ơ
ặ
ă
.
.
.
Hexaaquoaluminum ion, aluminum ion

++ Ơ

ặ

ă + Ơ

-

-- + -

-C H O

Hydrogen sulphite ion HSO H SO

6 5 7

3 7

3 3

2 7

4 1 10
1 0 10

.
.

Hydrogen sulphide H S H HS

Dihydrogen phosphate ion H PO H HPO

Boric H BO H H BO

Ammonium ion NH H NH

Hydrocyanic HCN H CN

2 8

2 4 4

2 8

3 3 2 3

10

4 3

10
10

9 1 10
6 2 10
7 3 10
5 6 10
4 9 10
ặ
ă + Ơ
ặ
ă + Ơ
ặ
ă + Ơ
ặ
ă + Ơ
ặ
ă + Ơ
+ -
-- + -
-+ -
-+ +
-+ -
-.
.
.
.
.

Phenol C H OH H C H O

Hydrogen carbonate ion HCO H CO

Hydrogen peroxide H O H HO

Monohydrogen phosphate ion HPO H PO

Water H O H OH

Hydroxide ion OH

6 5 6 5 10

3 3

2 11

2 2 2 12

4
2
4
3 13
2
14

1 3 10
5 6 10

2 4 10
2 2 10
1 0 10
ặ
ă + Ơ
ặ
ă + Ơ
ặ
ă + Ơ
ặ
ă + Ơ
ặ
ă + Ơ
+ -
-- + -
-+ -
-- + -
-+ -

-.
.
.
.
.
ă
ă +
ă +
+
-+

-H O very small

Ammonia NH H NH very small

2

3 2

R

ELATIVE

S

TRENGTHS OF

B

RØNSTED-

L

OWRY

A

CIDS AND

B

ASES

<i>in aqueous solution at room temperature.</i>

<b>Name of Acid</b> <b> Acid</b> <b>Base</b> <b> K</b><i><b>_a</b></i>

<b>STRONG</b>

<b>WEAK</b>

<b>STRONG</b>

<b>WEAK</b>

<b>STRENGTH OF ACID</b>

</div>
<span class='text_page_counter'>(27)</span><div class='page_container' data-page=27>

A

CID-BASE

I

NDICATORS

<b>Indicator</b>

yellow to blue
red to yellow

red to yellow
red to yellow
yellow to blue
red to yellow
yellow to red
yellow to blue
yellow to red
red to amber
yellow to blue
colourless to pink
colourless to blue
yellow to red
blue to yellow
Methyl violet

Thymol blue
Orange IV
Methyl orange
Bromcresol green
Methyl red
Chlorophenol red
Bromthymol blue
Phenol red
Neutral red
Thymol blue
Phenolphthalein
Thymolphthalein
Alizarin yellow
Indigo carmine

<b>pH Range in Which</b>
<b>Colour Change Occurs</b>

<b>Colour Change</b>
<b>as pH Increases</b>

</div>
<span class='text_page_counter'>(28)</span><div class='page_container' data-page=28>

F g e F

S O e SO

H O H e H O

MnO H e Mn H O

Au e Au s

2
2 8

2

4
2

2 2 2

4 2 2

3

2 2 2 87

2 2 2 01

2 2 2 1 78

8 5 4 1 51

3 1 50

( )+ ặă +
+ ặ_ă +
+ + ặă +
+ + ặ_ă + +
+ ặă ( ) +
-
-- -
-+
-- + - +
+
-.
.
.
.
.

BrO H e Br H O

ClO H e Cl H O

Cl g e Cl

Cr O H e Cr H O

O g H e

3 12 2 2

4 2
2
2 7
2 3
2
1
2 2

6 5 3 1 48

8 8 4 1 39

2 2 1 36

14 6 2 7 1 23

2 2
- +
-- + -
--
-- + - +
+

-+ + ặă ( )+ +
+ + ặă + +
( )+ ặ_ă +
+ + ặă + +
( )+ + ặ
l .
.
.
.
ă

ă H O2 +1 23.

MnO s H e Mn H O

IO H e I s H O

Br e Br

AuCl e Au s Cl

NO H e NO g H

2 2 2

3 12 2 2

2
4

3 2

4 2 2 1 22

6 5 3 1 20

2 2 1 09

3 4 1 00

4 3 2

( )+ + ặă + +
+ + ặ_ă ( )+ +
( )+ ặă +
+ ặ_ă ( )+ +
+ + ặă ( )+
+ - +
- +
--
-- -
-- +
-.
.
.
.
l
O

O +0 96.

Fe e Fe

O g H e H O

MnO H O e MnO s OH

I s e I

Cu e Cu s

3 2

2 2 2

4 2 2

2

0 77

2 2 0 70

2 3 4 0 60

2 2 0 54

0 52
+ - +
+

-- -
--
-+
-+ ặă +
( )+ + ặ_ă +
+ + ặă ( )+ +
( )+ ặă +
+ ặă ( ) +
.
.
.
.
.

H SO H e S s H O

Cu e Cu s

SO H e H SO H O

Cu e Cu

Sn e Sn

2 3 2

2

42 2 3 2

2

4 2

4 4 3 0 45

2 0 34

4 2 0 17

0 15

2 0 15

+ + ặ_ă ( )+ +
+ ặă ( ) +
+ + ặ_ă + +
+ ặă +
+ ặă +
+
-+
-- +
-+ - +
+ - +
.
.
.
.
.

S s H e H S g

H e H g

Pb e Pb s

Sn e Sn s

Ni e Ni s

( )+ + ặă ( ) +
+ ặ_ă ( ) +
+ ặă ( )
-+ ặă ( )
-+ ặ_ă ( )
-+
-+
-+
-+
-+

-2 2 0 14

2 2 0 00

2 0 13

2 0 14

2 0 26

2
2
2
2
2
.
.
.
.
.

H PO H e H PO H O

Co e Co s

Se s H e H Se

Cr e Cr

H O e H OH M

3 4 3 3 2

2

2

3 2

2 2 7

2 2 0 28

2 0 28

2 2 0 40

0 41

2 2 2 10 0 41

+ + ặ_ă +
-+ ặă ( )
-( )+ + ặă
-+ ặă
-+ ặă + ( )
-+
-+
-+
-+ - +
- -
-.
.
.
.
.

Fe e Fe s

Ag S s e Ag s S

Cr e Cr s

Zn e Zn s

Te s H e H Te

2

2 2

3
2

2

2 0 45

2 2 0 69

3 0 74

2 0 76

2 2 0 79

+
--
-+

-+
-+
-+ ặ_ă ( )
-( )+ ặă ( )+
-+ ặă ( )
-+ ặă ( )
-( )+ + ặă
-.
.
.
.
.

2 2 2 0 83

2 1 19

3 1 66

2 2 37

2 71

2 2

2
3
2

H O e H g OH

Mn e Mn s

Al e Al s

Mg e Mg s

Na e Na s

+ ặă ( )+
-+ ặ_ă ( )
-+ ặă ( )
-+ ặă ( )
-+ ặ_ă ( )
--
-+
-+
-+
-+
-.
.
.
.
.

Ca e Ca s

Sr e Sr s

Ba e Ba s

K e K s

Rb e Rb s

2
2
2

2 2 87

2 2 89

2 2 91

2 93
2 98
+
-+
-+
-+
-+
-+ ặ_ă ( )
-+ ặă ( )
-+ ặă ( )
-+ ặ_ă ( )
-+ ặă ( )
-.
.
.

.
.

Cs e Cs s

Li e Li s

+
-+
-+ ặ_ă ( )
-+ ặă ( )
-3 0-3
3 04
.
.

Hg e Hg

O g H M e H O

NO H e N O H O

Ag e Ag s

Hg e Hg

2
1

2 2 7 2

3 2 4 2

1
2 22

2 0 85

2 10 2 0 82

2 4 2 2 0 80

0 80
0 80
+
-+ -
-- +
-+
-+
-+ ặ_ă ( ) +
( )+ ( )+ ặă +
+ + ặ_ă + +
+ ặă ( ) +
+ ặă ( ) +
l
l
.
.
.
.

.

S

TANDARD

R

EDUCTION

P

OTENTIALS OF

H

ALF-CELLS

<i>Ionic concentrations are at 1M in water at 25∞C.</i>

<b> Reducing Agents</b>
<b>Oxidizing Agents</b>
<b>STRONG</b>
<b>WEAK</b>
<b>STRONG</b>
<b>WEAK</b>
Overpotential
Effect
Overpotential
Effect

<b>STRENGTH OF OXIDIZING AGENT</b>

<b>STRENGTH OF REDUCING AGENT</b>

<b>E∞ Volts</b>( )

</div>
<span class='text_page_counter'>(29)</span><div class='page_container' data-page=29>

D E F G H

Exam Booklet Form/
Cahier d examen

A B C

,

<b>Examination Rules</b>

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.

3. Cheating on an examination will result in a mark of zero. The Ministry of Education
considers cheating to have occurred if a student breaks any of the following rules:
• Candidates 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.

• Candidates 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.
• Candidates 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.

• Candidates must not communicate with another student during the
examination.

• Candidates must not remove any piece of the examination materials from

the examination room, including work pages.

• Candidates must not take or knowingly use any secure examination materials
prior to the examination session.

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.

<b>MINISTRY USE ONLY</b> <b>MINISTRY USE ONLY</b>

Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here.

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

0 1 2 3 4

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 NR

(.5)
5

0 1 2 3 4 NR

(.5)

0 1 2 3 NR

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 3 NR

(.5) NR

3

<b>Course Code = CH 12</b>

<b>Chemistry 12</b>

<b>AUGUST 2006</b>

<b>Response Booklet</b>

<b>Course Code = CH </b>

<b>12</b>

<b>AUGUST 2006</b>

<b>Student Instructions</b>

1. Place your Personal Education Number (PEN)
<b>label at the top of this Booklet AND fill in the</b>
bubble (Form A, B, C, D, E, F, G or H) that
corresponds to the letter on your Examination
Booklet.

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. Read the Examination Rules on the back of
this Booklet.

</div>
<span class='text_page_counter'>(30)</span><div class='page_container' data-page=30>

Version 0601.1

D E F G H

Exam Booklet Form/
Cahier d examen

A B C

,

814

© Province of British Columbia
<b>Examination Rules</b>

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.

3. Cheating on an examination will result in a mark of zero. The Ministry of Education
considers cheating to have occurred if a student breaks any of the following rules:
• Candidates 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.

• Candidates 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.
• Candidates 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.

• Candidates must not communicate with another student during the
examination.

• Candidates must not remove any piece of the examination materials from
the examination room, including work pages.

• Candidates must not take or knowingly use any secure examination materials
prior to the examination session.

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.

<b>MINISTRY USE ONLY</b> <b>MINISTRY USE ONLY</b>

Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here.

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

0 1 2 3 4

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 NR

(.5)
5

0 1 2 3 4 NR

(.5)

0 1 2 3 NR

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 3 NR

(.5) NR

3

<b>Course Code = CH 12</b>

<b>Chemistry 12</b>

<b>AUGUST 2006</b>

<b>Response Booklet</b>

<b>Course Code = CH </b>

<b>12</b>

<b>AUGUST 2006</b>

<b>Student Instructions</b>

1. Place your Personal Education Number (PEN)
<b>label at the top of this Booklet AND fill in the</b>
bubble (Form A, B, C, D, E, F, G or H) that
corresponds to the letter on your Examination
Booklet.

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. Read the Examination Rules on the back of
this Booklet.

</div>
<span class='text_page_counter'>(31)</span><div class='page_container' data-page=31>

<b>PART B: WRITTEN RESPONSE</b>

<b>Suggested Time: 40 minutes</b>
<b>INSTRUCTIONS: Answer the following questions in the space provided in this Response Booklet.</b>

You are expected to communicate your knowledge and understanding of chemical principles in a clear
<b>and logical manner. Your steps and assumptions leading to a solution must be written in this Response</b>

<b>Booklet. Answers must include units where appropriate and be given to the correct number of</b>

<b>significant figures. For questions involving calculations, full marks will NOT be given for</b>

<b>providing only an answer.</b>

1. Consider the reaction: 2Zn s

( )

+ O g₂

( )

Ỉ 2ZnO s

( )

State two different methods that would increase the rate of this reaction.

Explain each in terms of collision theory. <b>(4 marks)</b>

Method 1:

Explanation:

Method 2:

Explanation:

2. Consider the equilibrium: CO g₂

( )

+ H g₂

( )

ặ_ă CO g

_{( )}

₊ H O g₂

_{( )}

K<i>_eq</i> ₌1 60_.

</div>
<span class='text_page_counter'>(32)</span><div class='page_container' data-page=32>

Page 2 Chemistry 12 – 0608 Response Booklet
3. What is the maximum

[

Pb2+

]

that can exist in a saturated solution of BaSO₄ without causing

precipitate formation? <b>(4 marks)</b>

4. Given the reactants:

H C O₂ ₂ ₄ + HCOO- ặ_ă

Complete the acid-base equilibrium equation in the box above.

</div>
<span class='text_page_counter'>(33)</span><div class='page_container' data-page=33>

5. Calculate the pH of a 0 30. M H S solution. Begin by writing the equation for the₂

predominant reaction. <b>(5 marks)</b>

6. What mass of NaOH s

( )

is required to just neutralize 50 0. mL of 2 0. M H SO ?₂ ₄

</div>
<span class='text_page_counter'>(34)</span><div class='page_container' data-page=34>

Page 4 Chemistry 12 – 0608 Response Booklet
7. Balance the following in acidic solution.

FeS + NO2- Ỉ NO + SO4 - + Fe +

(

acidic

)

2 3

<b>(4 marks)</b>

8. The electrolysis of copper(II) sulphate solution using copper electrodes is used in the refining of
copper. Write the anode and cathode half-reactions and describe what would be observed at each

electrode as the cell operates. <b>(3 marks)</b>

Anode Half-Reaction:

Cathode Half-Reaction:

Observations:

anode:

cathode:

</div>
<span class='text_page_counter'>(35)</span><div class='page_container' data-page=35></div>
<span class='text_page_counter'>(36)</span><div class='page_container' data-page=36>

Version 0601.1

D E F G H

Exam Booklet Form/
Cahier d examen

A B C

,

814

© Province of British Columbia
<b>Examination Rules</b>

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.

3. Cheating on an examination will result in a mark of zero. The Ministry of Education
considers cheating to have occurred if a student breaks any of the following rules:
• Candidates 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.

• Candidates 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.
• Candidates 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.

• Candidates must not communicate with another student during the
examination.

• Candidates must not remove any piece of the examination materials from
the examination room, including work pages.

• Candidates must not take or knowingly use any secure examination materials
prior to the examination session.

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.

<b>MINISTRY USE ONLY</b> <b>MINISTRY USE ONLY</b>

Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here.

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

0 1 2 3 4

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 NR

(.5)
5

0 1 2 3 4 NR

(.5)

0 1 2 3 NR

(.5)

0 1 2 3 4 NR

(.5)

0 1 2 3 NR

(.5) NR

3

<b>Course Code = CH 12</b>

<b>Chemistry 12</b>

<b>AUGUST 2006</b>

<b>Response Booklet</b>

<b>Course Code = CH </b>

<b>12</b>

<b>AUGUST 2006</b>

<b>Student Instructions</b>

1. Place your Personal Education Number (PEN)
<b>label at the top of this Booklet AND fill in the</b>
bubble (Form A, B, C, D, E, F, G or H) that
corresponds to the letter on your Examination
Booklet.

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. Read the Examination Rules on the back of
this Booklet.

</div>

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