chemistry 12 - school district 67old provincial... · experiment 1 experiment 2 reactants powdered...
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Contents: 18 pages Examination: 2 hours 50 multiple-choice questions Additional Time Permitted: 60 minutes © Province of British Columbia
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.
Chemistry 12 – 0906 Form A Page 1
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.
FA B C D E HGExam Booklet Form/Cahier d’examen
1. Which of the following would have the highest reaction rate at room temperature?
A. H2 g( ) + I2 g( ) 2HI g( )
B. H2S g( ) + Cl2 aq( ) 2HCl aq( ) + S s( )
C. Ca2 + aq( ) + C2O42
aq( ) CaC2O4 s( )
D. Mg s( ) + 2H2O( ) Mg OH( )2 aq( ) + H2 g( )
2. Consider the following experimental results:
Experiment 1 Experiment 2
Reactants powdered Cu and HCl chunk of Cu and HNO3
Temperature 20º C 10º C
Concentration of acid 0.6 M HCl 0.4 M HNO3
Rate low high
Which of the following factors would account for the lower rate in Experiment 1? A. temperature B. nature of reactants C. surface area of Cu D. concentration of acid
Page 2 Chemistry 12 – 0906 Form A
3 Which of the following describes “activation energy”? A. the amount of energy that product molecules possess B. the difference between the products PE and the reactants PE C. the amount of energy released when reactant molecules collide D. the minimum amount of energy required to start a chemical reaction 4. Consider the following PE diagram:
Progress of reaction
PE(kJ)
200
100
150
50
Which of the following is correct for the reverse reaction?
PE (activated complex) (kJ) H (kJ)
A. 50 100
B. 50 +100
C. 200 100
D. 200 +100
Chemistry 12 – 0906 Form A Page 3
5. Consider the following reaction mechanism:
Step 1: ClO + H2O HClO + OH
Step 2: I + HClO HIO + Cl
Step 3: HIO + OH IO + H2O
Which of the following is correct?
Reactant for the Overall Reaction Reaction Intermediate
A. I OH
B. ClO H2O
C. H2O HClO
D. HClO HIO
6. Which of the following is correct for all systems at equilibrium?
I The temperature is constant.
II [Reactants] = [Products]
III Forward and reverse reactions are occurring.
IV The forward and reverse reaction rates are equal.
A. I and II only B. I, III and IV only C. II, III and IV only D. III and IV only
Page 4 Chemistry 12 – 0906 Form A
7. In which of the following does entropy increase?
A. the electrolysis of Na2SO4 aq( )
B. the reaction of NaCl aq( ) with AgNO3 aq( )
C. the redox reaction of an Fe nail in CuCl2 aq( )
D. the neutralization of Sr OH( )2 aq( ) by H2SO4 aq( )
8. Considering enthalpy and entropy factors, in which of the following will equilibrium be established?
I Cl2 g( )?
Cl2 aq( ) H = 25kJ
II CO g( ) + 2H2 g( )?
CH3OH g( ) H = 91kJ
III Mg s( ) + 2HCl aq( )?
MgCl2 aq( ) + H2 g( ) H = 425kJ
IV 3CO2 g( ) + 4H2O g( )?
C3H8 g( ) + 5 O2 g( ) H = +2200 kJ
A. I and II only B. II and IV only C. III and IV only D. I, II and III only
Chemistry 12 – 0906 Form A Page 5
Use the following equilibrium to answer questions 9 and 10.
2NO g( ) N2 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 N2[ ] and decreasing temperature
D. decreasing temperature and increasing volume 10. If some O2 is injected into the above equilibrium system, which of the following is correct?
Equilibrium Shift Net Change O2[ ]
A. left increase
B. left decrease
C. right increase
D. right decrease
11. Consider the following:
SO3 g( ) + 6HF g( ) SF6 g( ) + 3H2O g( ) Keq = 6.3 10 3
Which of the following is the value of Keq for:
2SF6 g( ) + 6H2O g( ) 12HF g( ) + 2SO3 g( )
A. 1.3 101
B. 1.6 10 2
C. 3.2 10 2
D. 2.5 10 4
Page 6 Chemistry 12 – 0906 Form A
12. Consider the following:
I C2H4 g( ) + H2 g( ) C2H6 g( ) Keq = 1.2 1019
II 2HBr g( ) H2 g( ) + Br2 g( ) Keq = 7.0 10 20
III Si s( ) + O2 g( ) SiO2 s( ) Keq = 2.0 10142
Which of the following lists these equilibria from the one that most favours products
to the one that least favours products? A. I, II, III B. I, III, II C. II, III, I D. 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 Keq .
B. Increasing temperature will increase Keq .
C. Increasing temperature will decrease Keq .
D. Decreasing Ni CO( )4[ ] will decrease Keq .
Chemistry 12 – 0906 Form A Page 7
14. Consider the equilibrium:
N2 g( ) + 3H2 g( ) 2NH3 g( ) Keq = 64
A 1.0 L container is filled with 0.28 mol N2, 0.16 mol H2 and 0.54 mol NH3 .
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 CaSO4 added to 1.0 L of water
B. 0.10 mol Cs2SO4 added to 1.0 L of water
C. 0.20 mol MgSO4 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. moles of solute per volume of solute B. mass of solute per volume of solution C. volume of solvent per mass of solvent D. 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( ) + Sr2+ aq( ) + 2OH aq( ) Mg2+ aq( ) + 2OH aq( ) + Sr S s( )
D. Mg2+ aq( ) + S2 aq( ) + Sr2+ aq( ) + 2OH aq( ) Sr2+ aq( ) + S2 aq( ) + Mg OH( )2 s( )
Page 8 Chemistry 12 – 0906 Form A
18. What is the Ksp expression for the low solubility salt formed when K2SO3 aq( )
and AlCl3 aq( ) are mixed?
A. Ksp = SO32[ ]
B. Ksp = K+[ ] Cl[ ]
C. Ksp = Al3+[ ]2
SO32[ ]
3
D. Ksp = Al 3+[ ]3
SO32[ ]
2
19. Which compound has the lowest solubility? A. ZnS
B. CuS
C. AgCl
D. SrSO4
20. What is the solubility of the salt PbCl2 ? 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 42
[ ] that can exist in
this solution before a precipitate forms?
A. SO 42
[ ] = 1.8 10 9 M
B. SO 42
[ ] = 1.8 10 8 M
C. SO 42
[ ] = 1.8 10 7 M
D. SO 42
[ ] = 1.3 10 4 M
Chemistry 12 – 0906 Form A Page 9
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 H2O( )63+
+ HS H2S + Al H2O( )5 OH( )2+
Reactant Acid Conjugate Base
A. HS H2S
B. H2S Al H2O( )63+
C. Al H2O( )63+ HS
D. Al H2O( )63+ Al H2O( )5 OH( )
2+
24. Which of the following is the weakest acid? A. 0.10 M CH3COOH
B. 0.50 M HClO4
C. 1.0 M HIO3
D. 1.5M HCN
Page 10 Chemistry 12 – 0906 Form A
25. Which of the following is the correct sequence of relative acid strengths?
A. HO2 > HCO3 > H2O2 > H2CO3
B. H2CO3 > HCO3 > H2O2 > HO2
C. H2CO3 > H2O2 > HCO3 > HO2
D. HCO3 > H2O2 > H2CO3 > HO2
26. Water reacts most completely as an acid with which of the following?
A. HO2
B. CO32
C. C2O42
D. HPO42
27. Which of the following equations represents the ionization of water?
A.
H2O( ) H2 aq( ) + 12 O2 aq( )
B. 2H2O( ) H3O
+ aq( ) + O2 aq( )
C. H2O( ) + H2O( ) H+ aq( ) + OH aq( )
D. H2O( ) + H2O( ) H3O
+ aq( ) + OH aq( )
28. The ionization of water is endothermic. Which of the following is a suitable
value of Kw 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
Chemistry 12 – 0906 Form A Page 11
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. H2CO3 OH
HCO3
B. H3O+ CO3
2
HCO3
C. HCO3 aq( ) + H2O( ) H2CO3 aq( ) + OH aq( )
D. HCO3 aq( ) + H2O( ) H3O+ aq( ) + CO3
2 aq( )
31. Which of the following 0.10 M solutions would have the lowest pH? A. HF
B. NH3
C. HNO3
D. H2CO3
Page 12 Chemistry 12 – 0906 Form A
32. Which of the following describes the predominant hydrolysis reaction that occurs in Na2HPO4 aq( )?
A. Na2HPO4 aq( ) 2Na+ aq( ) + HPO42 aq( )
B. PO4
3 aq( ) + H2O( ) HPO42 aq( ) + OH aq( )
C. HPO4
2 aq( ) + H2O( ) H3O+ aq( ) + PO43 aq( )
D. HPO4
2 aq( ) + H2O( ) H2PO4 aq( ) + OH aq( )
33. Which of the following represents a basic salt solution? A. NaI aq( )
B. NH4Cl aq( )
C. Na2CO 3 aq( )
D. NaHSO4 aq( )
34. The term “equivalence point” typically applies to A. buffer solutions. B. titration reactions. C. saturated solutions. D. chemical indicators.
Chemistry 12 – 0906 Form A Page 13
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( ) H2O( )
B. HCl aq( ) + NaOH aq( ) NaCl aq( ) + H2O( )
C. HCl aq( ) + NaOH aq( ) + H2O( ) NaCl aq( ) + H3O+ aq( ) + OH aq( )
D. H + aq( ) + Cl aq( ) + Na+ aq( ) + OH aq( ) Na+ aq( ) + Cl aq( ) + H2O( )
37. Consider the following buffer equilibrium system:
HCN aq( ) + H2O( ) H3O
+ 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.
Page 14 Chemistry 12 – 0906 Form A
38. An oxide of which of the following elements will form a basic solution? A. P B. N C. K D. C 39. A reducing agent in a chemical reaction can best be described as a substance that A. loses electrons and has a decrease in oxidation number. B. gains electrons and has a decrease in oxidation number. C. loses electrons and has an increase in oxidation number. D. gains electrons and has an increase in oxidation number. 40. What happens to the oxidation number of O as MgO2 undergoes a reaction in which
H2O2 is formed? A. It decreases by 1. B. It increases by 1. C. It increases by 2. D. It does not change. 41. Consider the following redox equation:
K2Cr2O7 + 7H2SO4 + 6KBr 3Br2 + 4K2SO4 + Cr2 SO4( )3 + 7H2O
Which chemical species is oxidized? A. Br in KBr
B. S in H2SO4
C. H in H2SO4
D. Cr in K2Cr2O7
Chemistry 12 – 0906 Form A Page 15
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:
N2O5 NH4+
Which of the following appear in the balanced equation?
A. 13e
B. 14e
C. 16e
D. 18e 44. Consider the following redox reaction:
2MnO4 + 16H++ 10 I 2Mn2+
+ 8H2O + 5 I2
A 10.0 mL sample of an iodide solution is titrated with 15.7mL of acidified 0.0106 M MnO4 .
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
Page 16 Chemistry 12 – 0906 Form A
45. Consider the following diagram of a standard electrochemical cell:
1.0 M Zn(NO3)
Cu(s)Zn(s)
21.0 M Cu(NO3)2
e–Object 1e–
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
Chemistry 12 – 0906 Form A Page 17
Use the following diagram to answer questions 46, 47 and 48.
1.0 M HCl 1.0 M AgNO3
Ag
H2(g)
Pt (inert)
Volts
PorousBarrier
46. What is the overall cell reaction?
A. Ag++ H+ H2 + Ag
B. 2Ag + 2H+ 2Ag++ H2
C. 2Ag++ H2 2H+
+ 2Ag
D. Ag++ H2 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
Page 18 Chemistry 12 – 0906 Form A
49. An iron pipeline can be protected from rusting by connecting it to a A. silver electrode buried beside the pipeline. B. copper electrode buried beside the pipeline. C. positive terminal of a direct current power supply. D. 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 Cl2
B. H2 and O2
C. Na + and Cl
D. NaOH and Cl2 You have Examination Booklet Form A. In the box above #1 on your Answer Sheet,
ensure you filled in the bubble as follows.
FA B C D E HGExam Booklet Form/Cahier d’examen
This is the end of the multiple-choice section. Answer the remaining questions in the Response Booklet.
Chemistry 12 Data Page 1
Bas
ed o
n m
ass
of C
12 a
t 12.
00.
Valu
es in
par
enth
eses
ar
e th
e m
asse
s of
the
mos
t st
able
or
best
kno
wn
isot
opes
for
elem
ents
whi
ch d
o no
t occ
ur n
atur
ally
.
PER
IOD
IC T
AB
LE
OF
TH
E E
LE
ME
NT
S
12
34
56
78
910
1112
1314
1516
1718
4 Be
Bery
llium
9.0
11 Na
Sodi
um
23.0
12 Mg
Mag
nesi
um
24.3
19 KPo
tass
ium
39.1
20 Ca
Cal
cium
40.1
37 Rb
Rub
idiu
m
85.5
55 Cs
Ces
ium
132.
9
56 Ba
Bariu
m
137.
3
87 Fr
Fran
cium
(223
)
88 Ra
Rad
ium
(226
)
21 Sc
S can
dium
45.0
2 2 Ti
Tita
n ium
47.9
39 YYt
trium
88.9
40 Zr
Zirc
o niu
m
91.2
57 La
L ant
hanu
m
1 38.
9
7 2 Hf
Haf
n ium
178.
5
89 Ac
Actin
ium
(227
)
104
Rf
Rut
her fo
rdiu
m
(26 1
)
23 VVa
nadi
um
50.9
24 Cr
Chr
omiu
m
52.0
41 Nb
Nio
bium
92.9
42 Mo
Mol
ybde
num
95.9
73 TaTa
ntal
um
180.
9
74 WTu
ngst
en
183.
8
105
Db
Dub
nium
(262
)
106
Sg
Seab
orgi
um
(263
)
25 Mn
Man
gane
se
54.9
26 Fe
Iron
55.8
43 Tc
Tech
netiu
m
(98)
44 Ru
Rut
heni
um
101.
1
75 Re
Rhe
nium
186.
2
76 Os
Osm
ium
190.
2
107
Bh
Bohr
ium
(262
)
108
Hs
Has
sium
(265
)
27 Co
Cob
alt
5 8.9
45 Rh
Rh o
dium
1 02.
9
77 IrIr i
dium
1 92.
2
1 09
Mt
Me i
tner
ium
(266
)
28 Ni
Nick
e l
58. 7
78 Pt
Plat
inu m
195 .
1
29 Cu
Cop
per
63.5
47 Ag
Silve
r
107.
9
79 Au
Gol
d
197.
0
30 Zn
Zinc
65.4
48 Cd
Cad
miu
m
112.
4
80 Hg
Mer
cury
200.
6
5 B Boro
n
10.8
13 Al
Alum
inum
27.0
31 Ga
Gal
lium
69.7
49 In Indi
um
114.
8
81 Tl
Thal
lium
204.
4
6 CC
arbo
n
12.0
14 Si
Silic
on
28.1
32 Ge
Ger
man
ium
72.6
50 Sn
Tin
118.
7
82 Pb
Lead
207.
2
7 NN
itrog
en
14. 0
1 5 PPh
osp h
orus
31.0
3 3 As
Ars e
nic
74.9
5 1 Sb
Antim
ony
121.
8
8 3 Bi
Bism
uth
209.
0
8 OO
xyge
n
16.0
16 SSu
lphu
r
32.1
34 Se
Sele
nium
79.0
52 TeTe
lluri u
m
127.
6
84 Po
Polo
nium
(209
)
9 FFl
uorin
e
19.0
17 Cl
Chl
orin
e
35.5
35 Br
Brom
ine
79.9
53 IIo
dine
126.
9
85 At
Asta
tine
(210
)
10 Ne
Neo
n
20.2
18 Ar
Argo
n
39.9
36 Kr
Kryp
ton
83.8
54 Xe
Xeno
n
131.
3
86 Rn
Rad
on
(222
)
2 He
Hel
ium
4.0
58 Ce
Cer
i um
140.
1
90 Th
Thor
ium
232.
0
59 Pr
Pras
eody
miu
m
140.
9
91 Pa
Prot
actin
ium
231.
0
60 Nd
Neo
dym
ium
144.
2
92 UU
rani
um
238.
0
61 Pm
Prom
ethi
um
(145
)
93 Np
Nep
tuni
um
(237
)
62 Sm
Sam
ariu
m
1 50.
4
94 Pu
Plu t
oniu
m
(244
)
63 Eu
Euro
pium
152.
0
95 Am
Amer
iciu
m
(243
)
64 Gd
Gad
olin
ium
157.
3
96 Cm
Cur
ium
(247
)
65 Tb
Terb
ium
158.
9
97 Bk
Berk
eliu
m
(247
)
66 Dy
Dys
pros
ium
162.
5
98 Cf
Cal
iforn
ium
(251
)
67 Ho
Hol
miu
m
164.
9
99 Es
E ins
tein
ium
(252
)
6 8 Er
Erb i
u m
167.
3
100
Fm
Ferm
ium
(25 7
)
69 Tm
Thul
ium
168.
9
101
Md
Men
dele
vium
(258
)
70 Yb
Ytte
rbiu
m
173.
0
102
No
Nob
eliu
m
(259
)
71 Lu
Lute
tium
175.
0
103
Lr
Law
renc
ium
(262
)
1 HH
ydro
gen
1.0
46 Pd
Palla
dium
106 .
4
38 Sr
Stro
ntiu
m
87.6
3 Li
Lith
ium
6.9
14
Si
Si
li
co
n
28.1
Ato
mic
Num
ber
Sym
bol
Nam
eA
tom
ic M
ass
14 Si
Silic
on
28.1
Data Page 2 Chemistry 12
ATOMIC MASSES OF THE ELEMENTSBased on mass of C12 at 12.00.
Values in parentheses are the mass number of the most stable or bestknown isotopes for elements that do not occur naturally.
ActiniumAluminumAmericiumAntimonyArgonArsenicAstatineBariumBerkeliumBerylliumBismuthBoronBromineCadmiumCalciumCaliforniumCarbonCeriumCesiumChlorineChromiumCobaltCopperCuriumDubniumDysprosiumEinsteiniumErbiumEuropiumFermiumFluorineFranciumGadoliniumGalliumGermaniumGoldHafniumHeliumHolmiumHydrogenIndiumIodineIridiumIronKryptonLanthanumLawrenciumLeadLithiumLutetiumMagnesiumManganeseMendelevium
AcAlAmSbArAsAtBaBkBeBiBBrCdCaCfCCeCsClCrCoCuCmDbDyEsErEuFmFFrGdGaGeAuHfHeHoHInIIrFeKrLaLrPbLiLuMgMnMd
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)
MercuryMolybdenumNeodymiumNeonNeptuniumNickelNiobiumNitrogenNobeliumOsmiumOxygenPalladiumPhosphorusPlatinumPlutoniumPoloniumPotassiumPraseodymiumPromethiumProtactiniumRadiumRadonRheniumRhodiumRubidiumRutheniumRutherfordiumSamariumScandiumSeleniumSiliconSilverSodiumStrontiumSulphurTantalumTechnetiumTelluriumTerbiumThalliumThoriumThuliumTinTitaniumTungstenUraniumVanadiumXenonYtterbiumYttriumZincZirconium
HgMoNdNeNpNiNbNNoOsOPdPPtPuPoKPrPmPaRaRnReRhRbRuRfSmScSeSiAgNaSrSTaTcTeTbTlThTmSnTiWUVXeYbYZnZr
804260109328417
102768
461578948419596191888675453744
10462213414471138167343526581906950227492235470393040
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
Element Symbol Atomic Number
AtomicMass Element Symbol Atomic
NumberAtomicMass
Chemistry 12 Data Page �
NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air.** Not stable in aqueous solutions.
Negative Ions(Anions)
Po s i t i v e I o n s( C a t i o n s )
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
Sulphide
Sulphite
Thiocyanate
OH–
ClO–
I–
HPO42–
NO3–
NO2–
C2O42–
O2–
ClO4–
MnO4–
PO4?–
SO42–
S2–
SO32–
SCN–
Bromide
Carbonate
Chlorate
Chloride
Chlorite
Chromate
Cyanide
Dichromate
Dihydrogen phosphate
Ethanoate, acetate
Fluoride
Hydrogen carbonate, bicarbonate
Hydrogen oxalate, binoxalate
Hydrogen sulphate, bisulphate
Hydrogen sulphide, bisulphide
Hydrogen sulphite, bisulphite
Br–
CO32–
ClO3–
Cl–
ClO2–
CrO42–
CN–
Cr2O72–
H2PO4–
CH3COO–
F–
HCO3–
HC2O4–
HSO4–
HS–
HSO3–
Lead(IV), plumbic
Lithium
Magnesium
Manganese(II), manganous
Manganese(IV)
Mercury(I)*, mercurous
Mercury(II), mercuric
Potassium
Silver
Sodium
Tin(II)*, stannous
Tin(IV), stannic
Zinc
Pb4+
Li+
Mg2+
Mn2+
Mn4+
Hg22+
Hg2+
K+
Ag+
Na+
Sn2+
Sn4+
Zn2+
Data Page � Chemistry 12
SOLUBILITY OF COMMON COMPOUNDS IN WATER
The term soluble here means > 0.1 mol/L at 25°C.
Negative Ions(Anions)
Positive Ions(Cations)
Solubility ofCompounds
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
14243
14253
123
123
123
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–
Alkali ions, H+, NH4+
Ag+, Ca2+, Sr2+, Ba2+, Pb2+
Chemistry 12 Data Page �
SOLUBILITY PRODUCT CONSTANTS AT 25°C
Name Formula
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
Zinc sulphide
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
ZnS
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
2.0 10–25
K sp
Data Page � 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
→ +
→ +
→ +
→ +
→ +
→ +
+ −
+ −
+ −
+ −
+ −
+ −
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 31
2 2 4 2 42
2 2 2 3 32
4 42 2
1 0
1 7 10
5 9 10
1 5 10
1 2 10
+ +
+ − −
+ − −
+ − −
− + − −
→← +→← + ×→← + ×
+( ) →← + ×→← + ×
.
.
.
.
.
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 43
2 63
2 52 3
3 6 5 7 2 6 5 74
2 24
7 5 10
6 0 10
7 1 10
4 6 10
→← + ×
( ) →← + ( ) ( ) ×→← + ×→← + ×
+ − −
+ + + −
+ − −
+ − −
.
, .
.
.
( )
→→← + ×+ − −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
, .
, .
.
.
,
( )
→← + ×
( ) →← + ( ) ( ) ×→← + ×→← + ×
+ − −
+ + + −
+ − −
− + − −
1 8 10
1 5 10
6 5 10
6 4 10
4
2 63
2 52 4
6 5 6 55
2 4 2 42 5
CHCH COOH H CH COO3 351 8 10→← + ×+ − −.
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 63
2 52 5
2 2 2 3 37
6 5 72
1 7 10
1 4 10
4 3 10
− + − −
+ + + −
+ − −
− +
→← + ×
( ) →← + ( ) ( ) ×
+( ) →← + ×→←
.
.
.
Hexaaquoaluminum ion, aluminum ion
++ ×→← + ×
− −
− + − −
C H O
Hydrogen sulphite ion HSO H SO
6 5 73 7
3 32 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
28
2 4 42 8
3 3 2 310
4 310
10
9 1 10
6 2 10
7 3 10
5 6 10
4 9 10
→← + ×→← + ×→← + ×→← + ×→← + ×
+ − −
− + − −
+ − −
+ + −
+ − −
.
.
.
.
.
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 6 510
3 32 11
2 2 212
42
43 13
214
1 3 10
5 6 10
2 4 10
2 2 10
1 0 10
→← + ×→← + ×→← + ×→← + ×→← + ×
+ − −
− + − −
+ − −
− + − −
+ − −
−
.
.
.
.
.
←← +
← +
+ −
+ −
H O very small
Ammonia NH H NH very small
2
3 2
RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASESin aqueous solution at room temperature.
Name of Acid Base Acid Ka
ST
RO
NG
WE
AK
ST
RO
NG
WE
AK
ST
RE
NG
TH
OF
AC
IDS
TR
EN
GT
H O
F B
AS
E
Chemistry 12 Data Page �
ACID-BASE INDICATORS
Indicator
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
pH Range in WhichColour Change Occurs
Colour Changeas pH Increases
0.0 – 1.6
1.2 – 2.8
1.4 – 2.8
3.2 – 4.4
3.8 – 5.4
4.8 – 6.0
5.2 – 6.8
6.0 – 7.6
6.6 – 8.0
6.8 – 8.0
8.0 – 9.6
8.2 – 10.0
9.4 – 10.6
10.1 – 12.0
11.4 – 13.0
Data Page � Chemistry 12
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 82
42
2 2 2
42
23
2 2 2 87
2 2 2 01
2 2 2 1 78
8 5 4 1 51
3 1 50
( ) + →← +
+ →← +
+ + →← +
+ + →← + +
+ →← ( ) +
− −
− − −
+ −
− + − +
+ −
.
.
.
.
.
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
312 2 2
4 2
2
2 72 3
2
12 2
6 5 3 1 48
8 8 4 1 39
2 2 1 36
14 6 2 7 1 23
2 2
− + −
− + − −
− −
− + − +
+ −
+ + →← ( ) + +
+ + →← + +
( ) + →← +
+ + →← + +
( ) + + →
l .
.
.
.
←← +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
22
2
312 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
( ) + + →← + +
+ + →← ( ) + +
( ) + →← +
+ →← ( ) + +
+ + →← ( ) +
+ − +
− + −
− −
− − −
− + −
.
.
.
.
l
OO +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
+ − +
+ −
− − −
− −
+ −
+ →← +
( ) + + →← +
+ + →← ( ) + +
( ) + →← +
+ →← ( ) +
.
.
.
.
.
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 22
42
2 3 22
4 2
4 4 3 0 45
2 0 34
4 2 0 17
0 15
2 0 15
+ + →← ( ) + +
+ →← ( ) +
+ + →← + +
+ →← +
+ →← +
+ −
+ −
− + −
+ − +
+ − +
.
.
.
.
.
S s H e H S g
H e H g
Pb e Pb s
Sn e Sn s
Ni e Ni s
( ) + + →← ( ) +
+ →← ( ) +
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ −
+ −
+ −
+ −
+ −
2 2 0 14
2 2 0 00
2 0 13
2 0 14
2 0 26
2
22
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 22
23 2
2 27
2 2 0 28
2 0 28
2 2 0 40
0 41
2 2 2 10 0 41
+ + →← + −
+ →← ( ) −
( ) + + →← −
+ →← −
+ →← + ( ) −
+ −
+ −
+ −
+ − +
− − −
.
.
.
.
.
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
22
3
2
2
2 0 45
2 2 0 69
3 0 74
2 0 76
2 2 0 79
+ −
− −
+ −
+ −
+ −
+ →← ( ) −
( ) + →← ( ) + −
+ →← ( ) −
+ →← ( ) −
( ) + + →← −
.
.
.
.
.
2 2 2 0 83
2 1 19
3 1 66
2 2 37
2 71
2 22
3
2
H O e H g OH
Mn e Mn s
Al e Al s
Mg e Mg s
Na e Na s
+ →← ( ) + −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
− −
+ −
+ −
+ −
+ −
.
.
.
.
.
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
+ −
+ −
+ −
+ −
+ −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
+ →← ( ) −
.
.
.
.
.
Cs e Cs s
Li e Li s
+ −
+ −
+ →← ( ) −
+ →← ( ) −
3 03
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
12 2
72
3 2 4 2
12 2
2
2 0 85
2 10 2 0 82
2 4 2 2 0 80
0 80
0 80
+ −
+ − −
− + −
+ −
+ −
+ →← ( ) +
( ) + ( ) + →← +
+ + →← + +
+ →← ( ) +
+ →← ( ) +
l
l
.
.
.
.
.
STANDARD REDUCTION POTENTIALS OF HALF-CELLSIonic concentrations are at 1M in water at 25°C.
Reducing AgentsOxidizing AgentsS
TR
ON
GW
EA
KS
TR
ON
GW
EA
K
Overpotential Effect
Overpotential Effect
ST
RE
NG
TH
OF
OX
IDIZ
ING
AG
EN
TS
TR
EN
GT
H O
F R
ED
UC
ING
AG
EN
TE° Volts( )
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Chemistry 12 – 0906 Response Booklet Page 1
PART B: WRITTEN RESPONSE Value: 37.5% of the examination
Suggested Time: 40 minutes
1. (4 marks)
A student burned a paraffin candle C25H52( ) in an open beaker according to the following equation:
C25H52 s( ) + 38 O2 g( ) 25CO2 g( ) + 26H2O 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 C25H52 per minute mol C25H52 min( ) ;
then, calculate how long it would take to produce 0.70 g CO2 .
Page 2 Chemistry 12 – 0906 Response Booklet
2. (4 marks)
Consider the following equilibrium:
CO g( ) + 3H2 g( ) CH4 g( ) + H2O g( )
Initially, 0.200 mol CO and 0.600 mol H2 are placed in a 2.00 L container. At equilibrium, H2O[ ] = 0.039 M. Calculate the value of Keq .
Chemistry 12 – 0906 Response Booklet Page 3
3. (4 marks)
Consider the following equilibrium:
Mg OH( )2 s( ) Mg 2+ 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 t1 .
Time (s)
Concentration(M)
t1
OH-
Mg2+
Page 4 Chemistry 12 – 0906 Response Booklet
4. (3 marks)
A solution of Sr OH( )2 aq( ) is titrated with H2SO4 . Explain what will happen to the electrical conductivity during the titration. Begin by writing the balanced formula equation, including states, to support your answer.
Chemistry 12 – 0906 Response Booklet Page 5
5. (5 marks)
Aniline C6H5NH2( ) is a weak base with a Kb = 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.
Page 6 Chemistry 12 – 0906 Response Booklet
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.)
Chemistry 12 – 0906 Response Booklet Page 7
7. (4 marks)
Balance the following redox equation in acidic solution:
Te O4 + In In2 O3 + Te (acidic)
Page 8 Chemistry 12 – 0906 Response Booklet
8. (3 marks)
Consider the following cell diagram:
PowerSupply
1 M K2SO4
+
Cu(s)Pb(s)
–
Write the overall cell reaction.
Write the formula for a precipitate that forms as the cell operates.
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Course Code = CH 12
Chemistry 122008/09 Released Exam
JUNE 2009
Response Booklet
Course Code = CH 2008/09 Released ExamJUNE 2009
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