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(1)Chemistry 12
Examination Booklet August 2006
Form A
DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.
(2)(3)PART A: MULTIPLE CHOICE
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
F
A B C D E G H
Exam Booklet Form/ Cahier d’examen
1 Which of the following would not be units for reaction rate? A g s
B M C kJ mol D kPa
2 Consider the reaction:
2Al s( ) + 3CuCl aq2( ) Ỉ 2AlCl aq3( ) + 3Cu s( )
What is the rate of Al consumption in mol if 98 g Cu are produced in 2.5 minutes? A ¥10-3mol
(4)Page Chemistry 12 – 0608 Form A 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
Use the following reaction mechanism to answer questions and 5.
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
(5)Use the following diagram to answer questions and 7.
Progress of the reaction PE
(kJ) 300 250 200 150 100 50
6 Which of the following are the values for the activation energy ( )Ea and change in enthalpy (DH) for the reverse reaction?
Ea ( )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?
(6)Page Chemistry 12 – 0608 Form A Consider the following:
energy + NH SH s4 ( ) ặă? 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 ặă 2NO g2( )
Time (min)
Concentrations (M)
t1
NO2 N2O4
Which of the following stresses was applied at time t1? A [NO2] was increased
(7)10 Styrene is manufactured as follows:
C H CH CH g kJ C H CHCH g H g styrene
6 3( ) +123 ặă 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( ) Keq =2 Ơ10-25
II Na O s2 2( ) ặă 2Na( )l + O g2( ) Keq = ¥10-29
III 2Na O s2 ( ) ặă 4Na( )l + O g2( ) Keq =3 ¥10-14
Which of the following lists the reactions in order, from the greatest [O2] at equilibrium, to the least [O2] at equilibrium?
(8)Page Chemistry 12 – 0608 Form A 12 Consider the equilibrium:
CaCO s3( ) ặă CaO s( ) + CO g2( )
In a L container at equilibrium there are 42 g CO , 002 g CaCO and 3 00 g CaO Which of the following is the value of Keq?
A 055 B 011 C 020 D 91
13 Consider the following equilibrium:
CCl g4( ) ặă C s( ) + 2Cl g2( )
Initially, 31 mol CCl was placed in a 4 L container At equilibrium, [Cl2]= 060M Which of the following is the value of Keq?
A ¥10-4 B ¥10-2 C ¥10-2 D ¥101
14 Consider the following equilibrium:
3NO g2( ) ăặ N O g2 5( ) + NO g( ) Keq =1 ¥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 Keq > Keq so the system shifted left
B Trial Keq < Keq so the system shifted left C Trial Keq > Keq so the system shifted right
(9)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 20 M BaS and 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 Ỉ 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( )?
(10)Page Chemistry 12 – 0608 Form A 19 Which equation has the Ksp expression: Ksp =[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 Ksp for Zn OH( )2 if it has a solubility of ¥10-7mol L ? A 2 ¥10-21
B 8 ¥10-21 C ¥10-14 D ¥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+
(11)-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 ặă 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
26 Which species is not amphiprotic? A H O2
(12)-Page 10 Chemistry 12 – 0608 Form A 27 At a given temperature a sample of pure water has a pH= 10
Which of the following is true?
Sample Reason
A acidic pH > 00 B basic pH > 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 + pKw
29 What is the mass of NaOH required to prepare 100 mL of NaOH aq( ) that has a pH= 13 62 ?
A 38 g B 42 g C 67 g
D 40 ¥10-14g
30 Which of the following hypothetical acids would have the lowest conductivity?
Acid Ka
A 0 5 M HY 1 0. ¥10-1
B M HA ¥10-6
C 1 0
2
(13)31 What is the net ionic equation for the hydrolysis of NH Cl4 ? A NH Cl aq4 ( ) ặă NH4+( ) +aq Cl aq-( )
B Cl aq-( ) + H O2 ( )l ặă HCl aq( ) + OH-( )aq C NH4+( )aq + H O2 ( )l ăặ H O aq3 +( ) + NH3( )aq D NH4+( ) +aq H O2 ( ) Ỉl ă HNH42+( ) +aq OH aq-( )
32 What is the approximate pH of a M solution of the salt NH Cl4 ? A
B C D
33 Consider the following indicator equilibrium:
HIn aq H O H O aq In aq
colourless blue
( ) + ( ) ặă +( ) + -( )
2 l
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
(14)(15)34 An indicator has a Ka = ¥
-4 10 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 s 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-( ) Ỉ 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 +
(16)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
Which of the above samples would be classified as acid rain? A only
B and C 1, and D 1, 2, and
39 Which of the following best describes the process of oxidation? 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
(17)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 134 g of oxalic acid required 24 70 mL of KMnO solution What is the4 molarity of the KMnO4 solution?
(18)Chemistry 12 – 0608 Form A Page 15
Use the following diagram to answer questions 45 to 47.
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- Æ Na
B Br2 + 2e- Æ 2Br -C 2Br- Ỉ Br2 + 2e
-D H O2 Ỉ 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
(19)48 A student constructs three standard electrochemical cells using the metals Pd, Cd and Ga with M solutions of their ions The student then records the voltages of Cell and Cell 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 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
(20)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
You have Examination Booklet Form A In the box above #1 on your Answer Sheet, ensure that you have filled in the bubble as follows
F
A B C D E G H
Exam Booklet Form/ Cahier d’examen
(21)12 at 12.00. ally . P ERIODIC T ABLE OF THE E LEMENTS 10 11 12 13 14 15 16 17 18 21 Sc Scandium 45.0 22 Ti Titanium 47.9 39 Y Yttr ium 88.9 40 Zr Zirconium 91.2 57 La Lanthan um 138.9 72 Hf Hafnium 178.5 89 Ac Actinium (227) 104 Rf Rutherf ordium (261) 23 V V anadium 50.9 24 Cr Chromium 52.0 41 Nb Niobium 92.9 42 Mo Molybden um 95.9 73 Ta Tantalum 180.9 74 W Tungsten 183.8
105 Db Dubnium (262) 106 Sg
Seaborgium (263)
25 Mn
Manganese 54.9
26 Fe Iron 55.8
43 Tc Technetium (98) 44 Ru Ruthenium 101.1 75 Re Rhenium 186.2 76 Os Osmium 190.2
107 Bh Bohr
ium
(262)
108 Hs Hassium (265) 27 Co Cobalt 58.9 45 Rh
Rhodium 102.9 77 Ir Iridium 192.2 109 Mt
Meitner
ium
(266)
28 Ni Nicke
l
58.7 78 Pt Platin
um
195.1
29 Cu
Copper 63.5 47 Ag Silv
er
107.9 79 Au Gold 197.0 30 Zn Zinc 65.4 48 Cd
Cadmium 112.4 80 Hg Mercur y 200.6 B
Boron 10.8 13 Al
Alumin
um
27.0 31 Ga Gallium 69.7 49 In Indium 114.8 81 Tl Thallium 204.4
6 C
Carbon 12.0 14 Si Silicon 28.1 32 Ge
Ger
manium 72.6 50 Sn Tin
118.7 82 Pb Lead 207.2 N
Nitrogen 14.0 15 P
Phosphor
us
31.0 33 As Arsenic 74.9 51 Sb Antimon
y
121.8 83 Bi Bism
uth
209.0
8 O
Oxygen 16.0 16 S Sulphur 32.1 34 Se Selenium 79.0 52 Te Tellur
ium
127.6 84 Po Polonium (209)
9 F
Fluor
ine
19.0 17 Cl Chlor
ine
35.5 35 Br Bromine 79.9 53 I Iodine 126.9 85 At Astatine (210) 10 Ne Neon 20.2 18 Ar Argon 39.9 36 Kr Krypton 83.8 54 Xe Xenon 131.3 86 Rn Radon (222)
2
He Helium 4.0
58 Ce Cerium
140.1 90 Th Thor
ium 232.0 59 Pr Pr aseodymium 140.9 91 Pa Protactinium 231.0 60 Nd Neodymium 144.2 92 U Ur anium 238.0 61 Pm Promethium (145) 93 Np Neptunium (237) 62 Sm Samar ium
150.4 94 Pu Plutonium (244)
63 Eu
Europium 152.0 95 Am Amer
icium
(243)
64 Gd
Gadolinium 157.3
96 Cm Curium
(247)
65 Tb
Terbium 158.9 97 Bk Berkelium (247) 66 Dy Dysprosium 162.5 98 Cf Calif or nium (251) 67 Ho
Holmium 164.9 99 Es Einsteinium (252) 68 Er Erbium
167.3 100 Fm Fe
rmium
(257)
69 Tm
Thulium 168.9 101 Md
Mendele
vium
(258)
70 Yb
Ytterbium 173.0 102 No Nobelium (259)
71 Lu
Lutetium 175.0 103 Lr Lawrencium (262)
46 Pd
P
alladium 106.4
Atomic Number Symbol Name Atomic Mass
(22)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 not occur naturally.
Data Page 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 83 35 48 20 98 58 55 17 24 27 29 96 105 66 99 68 63 100 87 64 31 32 79 72 67 49 53 77 26 36 57 103 82 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 41 102 76 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
Element Symbol Atomic
Number
Atomic
Mass Element Symbol
Atomic Number
(23)NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS
* Aqueous solutions are readily oxidized by air. ** Not stable in aqueous solutions.
Negative Ions (Anions) P o 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 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
(24)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 of Compounds 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 Ô Ô ˛ Ô Ô Ô Ô ¸ ˝ Ô Ô Ô Ô ˛ Ô Ô Ô Ô ¸ ˝ Ô Ô Ô Ô ˛ Ô Ô Ô Ô ¸ ˝ Ô Ô Ô Ô ˛ Ô Ô Ô Ô ¸ ˝ Ô Ô Ô Ô ˛ Ô Ô Ô Ô
Data Page 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–
(25)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
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
(26)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
3
2 4
Ỉ + Æ + Æ + Æ + Æ + Æ + + -+ -+ -+ -+ -+ -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
3
2 4
2 2 3
2
4
2
1 10 10 10 10
+ + + - -+ - -+ - + - -ặ ă + ặ ă + Ơ ặ ă + Ơ + ( ) ặă + Ơ ặ ă + ¥
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
3
2
3
2
2
3 7
4
2
4
7 10 10 10 10 ặ ă + Ơ ( ) ặă + ( ) ( ) Ơ ặ ă + Ơ ặ ă + Ơ + - -+ + + -+ - -+ - - , ( ) ặ ặ
ă H+ +F- ¥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 ( ) ặă + ( ) ( ) Ơ ặ ă + Ơ ặ ă + ¥ + - -+ + + -+ - + -
-1 10 10 10 10
4
2
3
2
2
6 5
2 42
CH
CH COOH3 ặă H++CH COO3 - ¥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 72
2
3
2
2
2 2 3
6
2
1 10 10 10
- + - -+ + + -+ - + ặ ă + Ơ ( ) ặă + ( ) ( ) Ơ + ( ) ặă + Ơ ặ ă Hexaaquoaluminum ion, aluminum ion
++ Ơ
ặ
ă + Ơ
-
+ -
-C H O
Hydrogen sulphite ion HSO H SO
6
3
3
2
4 10 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
2 4
2
3 3
10
4
10 10
9 10 10 10 10 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 10
3
2 11
2 2 12
4 13 14
1 10 10 10 2 10 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
RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASES
in aqueous solution at room temperature.
Name of Acid Acid Base Ka
STRONG
WEAK
STRONG
WEAK
STRENGTH OF ACID
(27)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 Which Colour Change Occurs
Colour Change as pH Increases
(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
4
2 2
4 2
3
2 2 87
2 2 01
2 2 78
8 51
3 50
( )+ ặă + + ặă + + + ặă + + + ặă + + + 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
4 2 2
6 48
8 39
2 36
14 23
2 - + + - + - + + -+ + ặă ( )+ + + + ặă + + ( )+ ặă + + + 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
3 12 2
2
3
4 2 22
6 20
2 09
3 00
4
( )+ + ặă + + + + ặă ( )+ + ( )+ ặă + + ặă ( )+ + + + 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
4 2
2
0 77
2 70
2 60
2 54
0 52 + - + + - -+ -+ ặă + ( )+ + ặă + + + 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
2
42
2
4
4 45
2 34
4 17
0 15
2 15
+ + ặă ( )+ + + ặă ( ) + + + ặă + + + 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 ( ) + + ặă ( ) + + ặă ( ) -+ ặă ( ) -+ ặă ( ) -+ -+ -+ -+ -+
-2 14
2 00
2 13
2 14
2 26
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 3
2
2
3
2
2 28
2 28
2 40
0 41
2 2 10 41
+ + ặă + -+ 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
3
2
2 45
2 69
3 74
2 76
2 79
+ -+ -+ -+ -+ ặă ( ) -( )+ ặă ( )+ -+ ặă ( ) -+ ặă ( ) -( )+ + ặă -
2 2 83
2 19
3 66
2 37
2 71
2
2
H O e H g OH
Mn e Mn s
Al e Al s
Mg e Mg s
Na e Na s
+ ặă ( )+ -+ ặă ( ) -+ ặă ( ) -+ ặă ( ) -+ ặă ( ) -+ -+ -+ -+ -
Ca e Ca s
Sr e Sr s
Ba e Ba s
K e K s
Rb e Rb s
2 2
2 87
2 89
2 91
2 93 98 + -+ -+ -+ -+ -+ ặă ( ) -+ ặă ( ) -+ ặă ( ) -+ ặă ( ) -+ ặă ( ) -
Cs e Cs s
Li e Li s
+ -+ -+ ặă ( ) -+ ặă ( ) -3 0-3 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
2
3
1 22
2 85
2 10 82
2 2 80
0 80 80 + -+ - + -+ -+ -+ ặă ( ) + ( )+ ( )+ ặă + + + ặă + + + ặă ( ) + + ặă ( ) + l l
STANDARD REDUCTION POTENTIALS OF HALF-CELLS
Ionic concentrations are at 1M in water at 25∞C.
Reducing Agents Oxidizing Agents STRONG WEAK STRONG WEAK Overpotential Effect Overpotential Effect
STRENGTH OF OXIDIZING AGENT
STRENGTH OF REDUCING AGENT
E∞ Volts( )
(29)D E F G H
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Examination Rules
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You may, however, take up to 60 minutes of additional time to finish Answers entered in the Examination Booklet will not be marked
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• 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
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Course Code = CH 12
Chemistry 12
AUGUST 2006 Response Booklet
Course Code = CH 12
AUGUST 2006
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
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
(30)Version 0601.1
D E F G H
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814
© Province of British Columbia Examination Rules
1 The time allotted for this examination is two hours
You may, however, take up to 60 minutes of additional time to finish 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
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Course Code = CH 12
Chemistry 12
AUGUST 2006 Response Booklet
Course Code = CH 12
AUGUST 2006
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
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
(31)PART B: WRITTEN RESPONSE
Suggested Time: 40 minutes 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.
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 (4 marks)
Method 1:
Explanation:
Method 2:
Explanation:
2 Consider the equilibrium: CO g2( ) + H g2( ) ặă CO g( ) + H O g2 ( ) Keq =1 60.
(32)Page Chemistry 12 – 0608 Response Booklet What is the maximum [Pb2+] that can exist in a saturated solution of BaSO4 without causing
precipitate formation? (4 marks)
4 Given the reactants:
H C O2 2 4 + HCOO- ặă
Complete the acid-base equilibrium equation in the box above
(33)5 Calculate the pH of a 30 M H S solution Begin by writing the equation for the2
predominant reaction (5 marks)
6 What mass of NaOH s( ) is required to just neutralize 50 mL of M H SO ?2 4
(34)Page Chemistry 12 – 0608 Response Booklet Balance the following in acidic solution
FeS + NO2- Ỉ NO + SO4 - + Fe + (acidic)
2
(4 marks)
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 (3 marks)
Anode Half-Reaction:
Cathode Half-Reaction:
Observations:
anode:
cathode:
(35)(36)Version 0601.1
D E F G H
Exam Booklet Form/ Cahier d examen
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814
© Province of British Columbia Examination Rules
1 The time allotted for this examination is two hours
You may, however, take up to 60 minutes of additional time to finish 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
MINISTRY USE ONLY MINISTRY USE ONLY
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Course Code = CH 12
Chemistry 12
AUGUST 2006 Response Booklet
Course Code = CH 12
AUGUST 2006
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
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