0608CH12 Form A - WordPress.com · 2015-08-04 · Page 4 Chemistry 12 – 0608 Form A 8. Consider the following: energy NH SH s NH g H S g+ Æ¨ ()+ 432? Which of the following describes

Contents: 17 pages Examination: 2 hours50 multiple-choice questions Additional Time Permitted: 60 minutes8 written-response questions © Province of British Columbia

Chemistry 12Examination Booklet

August 2006Form A

DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.

FOR FURTHER INSTRUCTIONS REFER TO THE RESPONSE BOOKLET.

Chemistry 12 – 0608 Form A Page 1

PART A: MULTIPLE CHOICE

Suggested Time: 80 minutes

INSTRUCTIONS: For each question, select the best answer and record your choice on the AnswerSheet provided. Using an HB pencil, completely fill in the bubble that has the lettercorresponding to your answer.

You have Examination Booklet Form A. In the box above #1 on your Answer Sheet, fill in thebubble as follows.

FA B C D E HGExam Booklet Form/Cahier d’examen

1. Which of the following would not be units for reaction rate?

A. g sB. M min

C. kJ mol

D. kPa min

2. Consider the reaction:

2 3 2 32 3Al s CuCl aq AlCl aq Cu s( ) + ( ) Æ ( ) + ( )

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 3. min¥ - mol

B. 6 2 10 3. min¥ - mol

C. 9 3 10 3. min¥ - mol

D. 3 9 10 1. min¥ - mol

Page 2 Chemistry 12 – 0608 Form A

3. Which of the following describes what happens to the KE and PE as an activated complexforms products?

KE PE

A. decreases increases

B. decreases decreases

C. increases increases

D. increases decreases

Use the following reaction mechanism to answer questions 4 and 5.

Step 1: 2 2 2NO N OÆ (fast)

Step 2: N O H N O H O2 2 2 2 2+ Æ + (slow)

Step 3: N O H N H O2 2 2 2+ Æ + (fast)

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

A. H2

B. NOC. 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

A. I and II onlyB. I and IV onlyC. II and III onlyD. III and IV only


Use the following diagram to answer questions 6 and 7.

. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .

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 Ea( ) and change in enthalpy DH( )for the reverse reaction?

E kJa ( ) 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 thefollowing must be true for the forward reaction?

A. Enthalpy change favours products and entropy is increasing.B. Enthalpy change favours reactants and entropy is increasing.C. Enthalpy change favours products and entropy is decreasing.D. Enthalpy change favours reactants and entropy is decreasing.


8. Consider the following:

energy NH SH s NH g H S g+ ( ) Æ̈ ( ) + ( )4 3 2

?

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 g energy NO g2 4 22( ) + Æ̈ ( )

Time (min)

Con

cent

ratio

ns (

M)

t1

NO2

N2O4

Which of the following stresses was applied at time t1?

A. NO2[ ] was increased.

B. N O2 4[ ] was decreased.C. Temperature was increased.D. Temperature was decreased.


10. Styrene is manufactured as follows:

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

styrene

6 5 2 3 6 5 2 2123( ) + Æ̈ ( ) + ( )

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

Temperature Pressure

A. low low

B. low high

C. high low

D. high high

11. Consider the following reactions:

I Na O s Na O g212 22( ) Æ̈ ( ) + ( )l Keq = ¥ -2 10 25

II Na O s Na O g2 2 22( ) Æ̈ ( ) + ( )l Keq = ¥ -5 10 29

III 2 42 2Na O s Na O g( ) Æ̈ ( ) + ( )l Keq = ¥ -3 10 14

Which of the following lists the reactions in order, from the greatest O2[ ] at equilibrium, to theleast O2[ ] at equilibrium?

A. I, II, IIIB. I, III, IIC. III, I, IID. III, II, I


12. Consider the equilibrium:

CaCO s CaO s CO g3 2( ) Æ̈ ( ) + ( )

In a 5 0. L container at equilibrium there are 2 42 2. g CO , 1 00 3. g CaCO and 1 00. g CaO.Which of the following is the value of Keq ?

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

13. Consider the following equilibrium:

CCl g C s Cl g4 22( ) Æ̈ ( ) + ( )

Initially, 0 31 4. mol CCl was placed in a 1 0. L container. At equilibrium, Cl M2 0 060[ ] = . .Which of the following is the value of Keq ?

A. 3 9 10 4. ¥ -

B. 1 3 10 2. ¥ -

C. 1 4 10 2. ¥ -

D. 7 8 101. ¥

14. Consider the following equilibrium:

3 1 0 102 2 511NO g N O g NO g K( ) Æ̈ ( ) + ( ) = ¥ -

eq .

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 thefollowing explains what happened?

A. Trial K Keq eq> so the system shifted left.

B. Trial K Keq eq< so the system shifted left.

C. Trial K Keq eq> so the system shifted right.

D. Trial K Keq eq< so the system shifted right.


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

A. an excess of soluteB. any amount of soluteC. a temperature of 25∞CD. a fixed volume of solvent

16. Which compound will have the greatest solubility?

A. CoSB. CuSC. FeSD. MgS

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

A. Be aq S aq BeS s2 2+ -( ) + ( ) Æ ( )B. Ba aq SO aq BaSO s2

42

4+ -( ) + ( ) Æ ( )

C. BaS aq BeSO aq BaSO s BeS s( ) + ( ) Æ ( ) + ( )4 4

D. Ba aq S aq Be aq SO aq BaSO s Be aq S aq2 2 242

42 2+ - + - + -( ) + ( ) + ( ) + ( ) Æ ( ) + ( ) + ( )

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

A. HI

B. Na S2

C. NaNO3

D. Pb NO3 2( )


19. Which equation has the Ksp expression: K Al SOsp = [ ] [ ]+ -3 242 3

?

A. 2 3342

2 4 3Al aq SO aq Al SO s+ -( ) + ( ) Æ ( ) ( )

B. Al SO s Al aq SO aq2 4 33

42( ) ( ) Æ̈ ( ) + ( )+ -

C. Al SO s Al aq SO aq2 4 33

422 3( ) ( ) Æ̈ ( ) + ( )+ -

D. 3 2342

2 4 3Al aq SO aq Al SO s+ -( ) + ( ) Æ̈ ( ) ( )

20. What is the Ksp for Zn OH( )2 if it has a solubility of 1 3 10 7. ¥ - mol 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+

B. the donation of OH-

C. the acceptance of H+

D. the acceptance of OH-


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

A. 2 2 22 2Na H O NaOH H+ Æ +

B. N H H O N H OH2 4 2 2 5+ Æ̈ ++ -

C. HPO H O H O PO42

2 3 43- + -+ Æ̈ +

D. H C O H O H O HC O2 2 4 2 3 2 4+ Æ̈ ++ -

24. Given the equilibrium:

H BO H PO H BO HPO2 3 2 4 3 3 42- - -+ Æ̈ +

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. NaCNB. Na PO3 4

C. Na CO2 3

D. Na C O2 2 4

26. Which species is not amphiprotic?

A. H O2

B. H BO3 3

C. H PO2 4-

D. H C H O2 6 5 7-


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 OH3+ -[ ] = [ ]

28. Which of the following is a definition of pH?

A. pH H O= [ ]+log 3

B. pH pOH= + 14

C. pH H O= - [ ]+log 3

D. pH pOH pK= + w

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

A. 0 38. g

B. 0 42. g

C. 1 67. g

D. 2 40 10 14. ¥ - g

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

Acid Ka

A. 0 5. M HY 1 0 10 1. ¥ -

B. 1 0. M HA 1 0 10 6. ¥ -

C. 1 0 2. M H B 1 0 10 2. ¥ -

D. 2 0. M HX 1 0 10 3. ¥ -


31. What is the net ionic equation for the hydrolysis of NH Cl4 ?

A. NH Cl aq NH aq Cl aq4 4( ) Æ̈ ( ) + ( )+ -

B. Cl aq H O HCl aq OH aq- -( ) + ( ) Æ̈ ( ) + ( )2 l

C. NH aq H O H O aq NH aq4 2 3 3+ +( ) + ( ) Æ̈ ( ) + ( )l

D. NH aq H O HNH aq OH aq4 2 42+ + -( ) + ( ) Æ̈ ( ) + ( )l

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

( ) + ( ) Æ̈ ( ) + ( )+ -2 3l

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

D. right more blue


34. An indicator has a Ka = ¥ -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 followingdescribes one of its uses in acid-base titrations?

A. bufferB. primary standardC. chemical indicatorD. stoichiometric indicator

36. What is the net ionic equation that describes the reaction of HCl aq with Pb OH s( ) ( ) ( )2 ?

A. H aq OH aq H O+ -( ) + ( ) Æ ( )2 l

B. 2 22 2 2HCl aq Pb OH PbCl s H O( ) + ( ) ( ) Æ ( ) + ( )s l

C. 2 2 22 2 2H aq Cl aq Pb OH s PbCl s H O+ -( ) + ( ) + ( ) ( ) Æ ( ) + ( )l

D. 2 2 2 2 22 22H aq Cl aq Pb aq OH aq Pb aq Cl aq H O+ - + - + -( ) + ( ) + ( ) + ( ) Æ ( ) + ( ) + ( )l

37. Which of the following would be used to prepare an acidic buffer solution?

A. HF and H O3+

B. H S and NaHS2

C. NH and NH Cl3 4

D. HNO and NaNO3 3


38. Four samples of rain are collected from different geographic regions andthe 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. 1 onlyB. 1 and 2C. 1, 2 and 3D. 1, 2, 3 and 4

39. Which of the following best describes the process of oxidation?

A. the process in which oxygen is given offB. the process in which electrons are gainedC. the process in which the oxidation number decreasesD. the process in which the oxidation number increases

40. What is the oxidation number of N in the mercury(II) compound Hg NH Cl3 2 2( ) ?

A. -6B. -4C. -3D. +3

41. Which of the following combinations will react spontaneously under standard conditions?

A. Ag Br+ 2

B. Ni Co+ +2

C. Zn Mg+ +2

D. Au HNO+ 3


42. Which of the following is a correctly balanced reduction half-reaction?

A. 2 2 22 2HCN e C N H+ Æ +- +

B. 2 3 6 62 2 3Sb H O e Sb O H+ + Æ +- +

C. NO H e HNO H O3 2 23 3- + -+ + Æ +

D. Sb O H e Sb OH H O2 5 2 26 4 2+ + Æ ( ) ++ - +

43. Which of the following ion concentrations could be determined by a redox titration usingnitric 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 followingequation:

2 5 6 2 10 84 2 2 42

2 2MnO H C O H Mn CO H O- + ++ + Æ + +

The titration of 0 134. g of oxalic acid required 24 70 4. mL of KMnO solution. What is themolarity of the KMnO4 solution?

A. 5 96 10 4. ¥ - M

B. 1 49 10 3. ¥ - M

C. 2 41 10 2. ¥ - M

D. 6 03 10 2. ¥ - M


Use the following diagram to answer questions 45 to 47.

Volts

1.0

M KNO

3

AnodeCu

CathodePt

(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 Na+ -+ Æ

B. Br e Br2 2 2+ Æ- -

C. 2 22Br Br e- -Æ +

D. H O O H e212 2 2 2Æ + ++ -

46. Which of the following best describes the movement of potassium ions andelectrons as the cell operates?

K+ IonMovement

ElectronMovement

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. VB. +0 62. VC. +0 75. VD. +1 43. V


48. A student constructs three standard electrochemical cells using the metals Pd, Cd and Ga with1 0. M solutions of their ions. The student then records the voltages of Cell 1 and Cell 2 in thefollowing 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. VB. -1 02. VC. +1 02. VD. +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.D. Store the nail wrapped in cobalt wire in a beaker of distilled water.


50. Consider the electrolytic cell shown in the following diagram:

1.0 M AgNO3

DCPowerSource

CuPt(inert)

– +

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

AnionMovement

Mass of PtElectrode

Mass of CuElectrode

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 thatyou have 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.

Bas

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78

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1112

1314

1516

1718

4 Be

Bery

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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

Scan

dium

45.0

22 Ti

Tita

nium

47.9

39 YYt

trium

88.9

40 Zr

Zirc

oniu

m

91.2

57 La

Lant

hanu

m

138.

9

72 Hf

Haf

nium

178.

5

89 Ac

Actin

ium

(227

)

104

Rf

Rut

herfo

rdiu

m

(261

)

23 VVa

nadi

um

50.9

24 Cr

Chr

omiu

m

52.0

41 Nb

Nio

bium

92.9

42 Mo

Mol

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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

58.9

45 Rh

Rho

dium

102.

9

77 IrIri

dium

192.

2

109

Mt

Mei

tner

ium

(266

)

28 Ni

Nick

el

58.7

78 Pt

Plat

inum

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

15 PPh

osph

orus

31.0

33 As

Arse

nic

74.9

51 Sb

Antim

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121.

8

83 Bi

Bism

uth

209.

0

8 OO

xyge

n

16.0

16 SSu

lphu

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34 Se

Sele

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79.0

52 TeTe

lluriu

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

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140.

1

90 Th

Thor

ium

232.

0

59 Pr

Pras

eody

miu

m

140.

9

91 Pa

Prot

actin

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231.

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60 Nd

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dym

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144.

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92 UU

rani

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238.

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61 Pm

Prom

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(145

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93 Np

Nep

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(237

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62 Sm

Sam

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150.

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94 Pu

Plut

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m

(244

)

63 Eu

Euro

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152.

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95 Am

Amer

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m

(243

)

64 Gd

Gad

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157.

3

96 Cm

Cur

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(247

)

65 Tb

Terb

ium

158.

9

97 Bk

Berk

eliu

m

(247

)

66 Dy

Dys

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162.

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98 Cf

Cal

iforn

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(251

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67 Ho

Hol

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164.

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99 Es

Eins

tein

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(252

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68 Er

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100

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69 Tm

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70 Yb

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Nob

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(259

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71 Lu

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175.

0

103

Lr

Law

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(262

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46 Pd

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106.

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38 Sr

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87.6

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28.1

Chemistry 12 Data Page 1

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.

Data Page 2 Chemistry 12

ActiniumAluminumAmericiumAntimonyArgonArsenicAstatineBariumBerkeliumBerylliumBismuthBoronBromineCadmiumCalciumCaliforniumCarbonCeriumCesiumChlorineChromiumCobaltCopperCuriumDubniumDysprosiumEinsteiniumErbiumEuropiumFermiumFluorineFranciumGadoliniumGalliumGermaniumGoldHafniumHeliumHolmiumHydrogenIndiumIodineIridiumIronKryptonLanthanumLawrenciumLeadLithiumLutetiumMagnesiumManganeseMendelevium

AcAlAmSbArAsAtBaBkBeBiBBrCdCaCfCCeCsClCrCoCuCmDbDyEsErEuFmFFrGdGaGeAuHfHeHoHInIIrFeKrLaLrPbLiLuMgMnMd

891395511833855697

483

535482098

658551724272996

10566996863

1009

876431327972

267

1495377263657

10382

3711225

101

(227)27.0

(243)121.8

39.974.9

(210)137.3

(247)9.0

209.010.879.9

112.440.1

(251)12.0

140.1132.9

35.552.058.963.5

(247)(262)162.5

(252)167.3152.0

(257)19.0

(223)157.3

69.772.6

197.0178.5

4.0164.9

1.0114.8126.9192.2

55.883.8

138.9(262)207.2

6.9175.0

24.354.9

(258)

MercuryMolybdenumNeodymiumNeonNeptuniumNickelNiobiumNitrogenNobeliumOsmiumOxygenPalladiumPhosphorusPlatinumPlutoniumPoloniumPotassiumPraseodymiumPromethiumProtactiniumRadiumRadonRheniumRhodiumRubidiumRutheniumRutherfordiumSamariumScandiumSeleniumSiliconSilverSodiumStrontiumSulphurTantalumTechnetiumTelluriumTerbiumThalliumThoriumThuliumTinTitaniumTungstenUraniumVanadiumXenonYtterbiumYttriumZincZirconium

HgMoNdNeNpNiNbNNoOsOPdPPtPuPoKPrPmPaRaRnReRhRbRuRfSmScSeSiAgNaSrSTaTcTeTbTlThTmSnTiWUVXeYbYZnZr

804260109328417

102768

461578948419596191888675453744

10462213414471138167343526581906950227492235470393040

200.695.9

144.220.2

(237)58.792.914.0

(259)190.2

16.0106.4

31.0195.1

(244)(209)

39.1140.9

(145)231.0

(226)(222)186.2102.9

85.5101.1

(261)150.4

45.079.028.1

107.923.087.632.1

180.9(98)127.6158.9204.4232.0168.9118.747.9

183.8238.0

50.9131.3173.0

88.965.491.2

Element Symbol AtomicNumber

AtomicMass Element Symbol Atomic

NumberAtomicMass

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 ive 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–

PO43–

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+

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

¸

˝

ÔÔÔÔ

˛

ÔÔÔÔ

¸

˝

ÔÔÔÔ

˛

ÔÔÔÔ

¸

˝

ÔÔÔÔ

˛

ÔÔÔÔ

¸

˝

ÔÔÔÔ

˛

ÔÔÔÔ

¸

˝

ÔÔÔÔ

˛

ÔÔÔÔ


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+

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)2CuS

Fe(OH)2FeS

Fe(OH)3PbBr2

PbCl2

Pb(IO3)2PbI2

PbSO4

MgCO3

Mg(OH)2AgBrO3

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


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

Æ +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 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

+ +

+ - -

+ - -

+ - -

- + - -

Æ̈ +Æ̈ + ¥Æ̈ + ¥

+( ) Æ̈ + ¥Æ̈ + ¥

.

.

.

.

.

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

Æ̈ + ¥

( ) Æ̈ + ( ) ( ) ¥Æ̈ + ¥Æ̈ + ¥

+ - -

+ + + -

+ - -

+ - -

.

, .

.

.

( )

ÆÆ̈ + ¥+ - -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

, .

, .

.

.

,

( )

Æ̈ + ¥

( ) Æ̈ + ( ) ( ) ¥Æ̈ + ¥Æ̈ + ¥

+ - -

+ + + -

+ - -

- + - -

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 10Æ̈ + ¥+ - -.

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

- + - -

+ + + -

+ - -

- +

Æ̈ + ¥

( ) Æ̈ + ( ) ( ) ¥

+( ) Æ̈ + ¥Æ̈

.

.

.

Hexaaquoaluminum ion, aluminum ion

++ ¥Æ̈ + ¥

- -

- + - -

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

Æ̈ + ¥Æ̈ + ¥Æ̈ + ¥Æ̈ + ¥Æ̈ + ¥

+ - -

- + - -

+ - -

+ + -

+ - -

.

.

.

.

.

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

Æ̈ + ¥Æ̈ + ¥Æ̈ + ¥Æ̈ + ¥Æ̈ + ¥

+ - -

- + - -

+ - -

- + - -

+ - -

-

.

.

.

.

.

¨̈ +

¨ +

+ -

+ -

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

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

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

( ) + Æ̈ +

+ Æ̈ +

+ + Æ̈ +

+ + Æ̈ + +

+ Æ̈ ( ) +

- -

- - -

+ -

- + - +

+ -

.

.

.

.

.

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

- + -

- + - -

- -

- + - +

+ -

+ + Æ̈ ( ) + +

+ + Æ̈ + +( ) + Æ̈ +

+ + Æ̈ + +( ) + + Æ

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

( ) + + Æ̈ + +

+ + Æ̈ ( ) + +( ) + Æ̈ +

+ Æ̈ ( ) + +

+ + Æ̈ ( ) +

+ - +

- + -

- -

- - -

- + -

.

.

.

.

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

+ - +

+ -

- - -

- -

+ -

+ Æ̈ +( ) + + Æ̈ +

+ + Æ̈ ( ) + +( ) + Æ̈ +

+ Æ̈ ( ) +

.

.

.

.

.

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

+ + Æ̈ ( ) + +

+ Æ̈ ( ) +

+ + Æ̈ + +

+ Æ̈ +

+ Æ̈ +

+ -

+ -

- + -

+ - +

+ - +

.

.

.

.

.

S s H e H S g

H e H g

Pb e Pb s

Sn e Sn s

Ni e Ni s

( ) + + Æ̈ ( ) +

+ Æ̈ ( ) +

+ Æ̈ ( ) -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

+ -

+ -

+ -

+ -

+ -

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

+ + Æ̈ + -

+ Æ̈ ( ) -( ) + + Æ̈ -

+ Æ̈ -

+ Æ̈ + ( ) -

+ -

+ -

+ -

+ - +

- - -

.

.

.

.

.

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

+ -

- -

+ -

+ -

+ -

+ Æ̈ ( ) -( ) + Æ̈ ( ) + -

+ Æ̈ ( ) -

+ Æ̈ ( ) -( ) + + Æ̈ -

.

.

.

.

.

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

+ Æ̈ ( ) + -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

- -

+ -

+ -

+ -

+ -

.

.

.

.

.

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

+ -

+ -

+ -

+ -

+ -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

.

.

.

.

.

Cs e Cs s

Li e Li s

+ -

+ -

+ Æ̈ ( ) -

+ Æ̈ ( ) -

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

+ -

+ - -

- + -

+ -

+ -

+ Æ̈ ( ) +( ) + ( ) + Æ̈ +

+ + Æ̈ + +

+ Æ̈ ( ) +

+ Æ̈ ( ) +

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

OverpotentialEffect

OverpotentialEffect

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( )


Version 0601.1

D E F G H Exam Booklet Form/

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Examination Rules

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

Question 1

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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)50 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

Course Code = CH 12

Chemistry 12AUGUST 2006

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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)50 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

Course Code = CH 12


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Chemistry 12 – 0608 Response Booklet Page 1

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 clearand logical manner. Your steps and assumptions leading to a solution must be written in this ResponseBooklet. Answers must include units where appropriate and be given to the correct number ofsignificant figures. For questions involving calculations, full marks will NOT be given forproviding only an answer.

1. Consider the reaction: 2 22Zn s O g ZnO s( ) + ( ) Æ ( )

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 g H g CO g H O g K2 2 2 1 60( ) + ( ) Æ̈ ( ) + ( ) = .eq

Initially, 8 2 8 2 2. .mol of CO and mol of H O are placed in a 2 0. L container and allowed to react.Calculate the equilibrium concentrations of CO and CO2 . (4 marks)

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? (4 marks)

4. Given the reactants:

H C O HCOO2 2 4 + Æ̈-

Complete the acid-base equilibrium equation in the box above.Determine whether reactants or products will be favoured and explain why. (3 marks)

Chemistry 12 – 0608 Response Booklet Page 3

5. Calculate the pH of a 0 30 2. M H S solution. Begin by writing the equation for thepredominant reaction. (5 marks)

6. What mass of NaOH s( ) is required to just neutralize 50 0 2 0 2 4. .mL of M H SO ?Begin by writing the balanced equation for the neutralization reaction. (3 marks)

Page 4 Chemistry 12 – 0608 Response Booklet

7. Balance the following in acidic solution.

FeS NO NO SO Fe acidic+ Æ + + ( )- - +2 4

2 3

(4 marks)

8. The electrolysis of copper(II) sulphate solution using copper electrodes is used in the refining ofcopper. Write the anode and cathode half-reactions and describe what would be observed at eachelectrode as the cell operates. (3 marks)

Anode Half-Reaction:

Cathode Half-Reaction:

Observations:

anode:

cathode:

END OF EXAMINATION

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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)50 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

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Documents

0608CH12 Form A - WordPress.com · 2015-08-04 · Page 4 Chemistry 12 – 0608 Form A 8. Consider the following: energy NH SH s NH g H S g+ Æ¨ ()+ 432? Which of the following describes