Chemistry 12. Examination Booklet 2008/09 Released Exam June 2009 Form A DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO.

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1 Chemistry 1 Examination Booklet 008/09 Released Exam June 009 Form A DO NOT OPEN ANY EXAMINATION MATERIALS UNTIL INSTRUCTED TO DO SO. FOR FURTHER INSTRUCTIONS REFER TO THE RESPONSE BOOKLET. Contents: 18 pages Examination: hours 50 multiple-choice questions Additional Time Permitted: 60 minutes Province of British Columbia

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3 PART A: MULTIPLE CHOICE Value: 6.5% of the examination Suggested Time: 80 minutes INSTRUCTIONS: For each question, select the best answer and record your choice on the Answer Sheet provided. Using an HB pencil, completely fill in the bubble that has the letter corresponding to your answer. You have Examination Booklet Form A. In the box above #1 on your Answer Sheet, fill in the bubble as follows. Exam Booklet Form/ Cahier d examen A B C D E F G H 1. Which of the following would have the highest reaction rate at room temperature? A. H ( g) + I ( g) HI( g) B. H Sg ( ) + Cl ( aq) HCl( aq) + Ss ( ) C. Ca + ( aq) + C O 4 ( aq) CaC O 4 ( s) D. Mg( s) + H O( ) Mg( OH) ( aq) + H ( g). Consider the following experimental results: Experiment 1 Experiment Reactants powdered Cu and HCl chunk of Cu and HNO 3 Temperature 0º C 10º C Concentration of acid 0.6 M HCl 0.4 M HNO 3 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 Chemistry Form A Page 1

4 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: 00 PE (kj) Progress of reaction Which of the following is correct for the reverse reaction? PE (activated complex) (kj) H (kj) A B C D Page Chemistry Form A

5 5. Consider the following reaction mechanism: Step 1: Step : ClO + H O HClO + OH I + HClO HIO + Cl Step 3: HIO + OH IO + H O Which of the following is correct? Reactant for the Overall Reaction Reaction Intermediate A. I OH B. ClO H O C. H O HClO D. HClO HIO 6. Which of the following is correct for all systems at equilibrium? I II III IV The temperature is constant. [Reactants] = [Products] Forward and reverse reactions are occurring. 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 Chemistry Form A Page 3

6 7. In which of the following does entropy increase? A. the electrolysis of Na SO 4 ( aq) B. the reaction of NaCl ( aq) with AgNO 3 ( aq) C. the redox reaction of an Fe nail in CuCl ( aq) D. the neutralization of Sr ( OH) ( aq) by H SO 4 ( aq) 8. Considering enthalpy and entropy factors, in which of the following will equilibrium be established? I Cl ( g)? Cl ( aq) H = 5kJ II CO( g) + H ( g)? CH 3 OH( g) H = 91kJ III Mg( s) + HCl( aq)? MgCl ( aq) + H ( g) H = 45kJ IV 3CO ( g) + 4H Og ( )? C 3 H 8 ( g) + 5O ( g) H =+00 kj A. I and II only B. II and IV only C. III and IV only D. I, II and III only Page 4 Chemistry Form A

7 Use the following equilibrium to answer questions 9 and 10. NO( g) N ( g) + O ( g) H = +181kJ 9. Which of the following pairs of stresses cause the same shift to the above equilibrium? A. adding a catalyst and decreasing volume B. increasing pressure and increasing [ NO] C. decreasing [ N ] and decreasing temperature D. decreasing temperature and increasing volume 10. If some O is injected into the above equilibrium system, which of the following is correct? Equilibrium Shift Net Change [ O ] A. left increase B. left decrease C. right increase D. right decrease 11. Consider the following: SO 3 ( g) + 6HF ( g) SF 6 ( g) + 3H Og ( ) K eq = Which of the following is the value of K eq for: SF 6 ( g) + 6H Og ( ) 1HF ( g) + SO 3 ( g) A B C D Chemistry Form A Page 5

8 1. Consider the following: I C H 4 ( g) + H ( g) C H 6 ( g) K eq = II III HBr ( g) 0 H ( g) + Br ( g) K eq = Si ()+ s O ( g) SiO () s K eq = 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 K eq. B. Increasing temperature will increase K eq. C. Increasing temperature will decrease K eq. D. Decreasing [ Ni ( CO) 4 ] will decrease K eq. Page 6 Chemistry Form A

9 14. Consider the equilibrium: N ( g) + 3H ( g) NH 3 ( g) K eq = 64 A 1.0 L container is filled with 0.8 mol N, 0.16 mol H and 0.54 mol NH 3. In which direction will the reaction proceed and what will happen to the pressure of the system? Direction Pressure A. left decreases B. left increases C. right decreases D. right increases 15. Which of the following will form a saturated solution? A mol CaSO 4 added to 1.0 L of water B mol Cs SO 4 added to 1.0 L of water C. 0.0 mol MgSO 4 added to.0 L of water D mol Pb( NO 3 ) added to.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) ( aq)? A. Mg + ( aq) + OH ( aq) Mg( OH) () s B. MgS( aq) + Sr( OH) ( aq) SrS( aq) + Mg( OH) () s C. Mg + ( aq) + S ( aq) + Sr + ( aq) + OH ( aq) Mg + ( aq) + OH ( aq) + SrS() s D. Mg + ( aq) + S ( aq) + Sr + ( aq) + OH ( aq) Sr + ( aq) + S ( aq) + Mg( OH) () s Chemistry Form A Page 7

10 18. What is the K sp expression for the low solubility salt formed when K SO 3 ( aq) and AlCl 3 ( aq)are mixed? A. K sp = [ SO 3 ] B. K sp = [ K + ][ Cl ] C. K sp = [ Al 3+ ] [ SO 3 ] 3 D. K sp = [ Al 3+ ] 3 [ SO 3 ] 19. Which compound has the lowest solubility? A. ZnS B. CuS C. AgCl D. SrSO 4 0. What is the solubility of the salt PbCl? A M B M C M D M 1. A solution is found to contain a Pb + this solution before a precipitate forms? [ ] = M [ ] = M [ ] = M [ ] = M A. SO 4 B. SO 4 C. SO 4 D. SO 4 [ ] of 0.10M. What is the maximum SO 4 [ ] that can exist in Page 8 Chemistry Form A

11 . 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 3. Identify the reactant acid and its conjugate base in the equilibrium below. Al( H O) HS H S + Al( H O) 5 ( OH) + Reactant Acid Conjugate Base A. HS H S 3+ B. H S Al ( H O) 6 3+ C. Al ( H O) 6 3+ D. Al ( H O) 6 HS Al ( H O) 5 ( OH) + 4. Which of the following is the weakest acid? A M CH 3 COOH B M HClO 4 C. 1.0 M HIO 3 D. 1.5M HCN Chemistry Form A Page 9

12 5. Which of the following is the correct sequence of relative acid strengths? A. HO > HCO 3 > H O > H CO 3 B. H CO 3 > HCO 3 > H O > HO C. H CO 3 > H O > HCO 3 > HO D. HCO 3 > H O > H CO 3 > HO 6. Water reacts most completely as an acid with which of the following? A. HO B. CO 3 C. C O 4 D. HPO 4 7. Which of the following equations represents the ionization of water? A. H O( ) H ( aq) + 1 O ( aq) B. H O( ) H 3 O + ( aq) + O ( aq) C. H O( ) + H O( ) H + ( aq) + OH ( aq) D. H O( ) + H O( ) H 3 O + ( aq) + OH ( aq) 8. The ionization of water is endothermic. Which of the following is a suitable value of K w if the temperature of water is lower than 5º C? A B C D Page 10 Chemistry Form A

13 9. What is the poh of 0.30 M HI? A B. 0.5 C. 0.5 D What is the equilibrium constant expression for the predominant equilibrium in HCO 3 ( aq)? A. B. H CO 3 OH HCO 3 H 3 O + CO 3 HCO 3 C. HCO 3 ( aq) + H O( ) H CO 3 ( aq) + OH ( aq) D. HCO 3 ( aq) + H O( ) H 3 O + ( aq) + CO 3 ( aq) 31. Which of the following 0.10 M solutions would have the lowest ph? A. HF B. NH 3 C. HNO 3 D. H CO 3 Chemistry Form A Page 11

14 3. Which of the following describes the predominant hydrolysis reaction that occurs in Na HPO 4 ( aq)? A. Na HPO 4 ( aq) Na + ( aq) + HPO 4 ( aq) B. PO 3 4 ( aq) + H O( ) HPO 4 ( aq) + OH ( aq) C. HPO 4 ( aq) + H O( ) H 3 O + ( aq) + PO 3 4 ( aq) D. HPO 4 ( aq) + H O( ) H PO 4 ( aq) + OH ( aq) 33. Which of the following represents a basic salt solution? A. NaI( aq) B. NH 4 Cl( aq) C. Na CO 3 ( aq) D. NaHSO 4 ( aq) 34. The term equivalence point typically applies to A. buffer solutions. B. titration reactions. C. saturated solutions. D. chemical indicators. Page 1 Chemistry Form A

15 35. A solution is tested with two indicators and the following results are obtained: Indicator chlorophenol red phenolphthalein Colour red colourless What is the approximate ph of the solution? A. 4.0 B. 6.0 C. 7.0 D What is the net ionic equation for the reaction of hydrochloric acid with NaOH ( aq)? A. H + ( aq) + OH ( aq) H O( ) B. HCl ( aq) + NaOH ( aq) NaCl ( aq) + H O( ) C. HCl ( aq) + NaOH ( aq) + H O( ) NaCl ( aq) + H 3 O + ( aq) + OH ( aq) D. H + ( aq) + Cl ( aq) + Na + ( aq) + OH ( aq) Na + ( aq) + Cl ( aq) + H O( ) 37. Consider the following buffer equilibrium system: HCN( aq) + H O( ) H 3 O + ( aq) + CN ( aq) What is the net result of adding a small amount of KOH? A. The ph increases slightly. B. The ph decreases slightly. C. The [ HCN] increases slightly. D. The CN [ ] decreases slightly. Chemistry Form A Page 13

16 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 OasMgO undergoes a reaction in which H O is formed? A. It decreases by 1. B. It increases by 1. C. It increases by. D. It does not change. 41. Consider the following redox equation: K Cr O 7 + 7H SO 4 + 6KBr 3Br + 4K SO 4 + Cr ( SO 4 ) 3 + 7H O Which chemical species is oxidized? A. Br in KBr B. SinH SO 4 C. HinH SO 4 D. Cr in K Cr O 7 Page 14 Chemistry Form A

17 4. Consider the following spontaneous redox reactions: X + Y X + Y Y + Z Y + Z Which of the following describes the relative strengths of the reducing agents? A. X > Y > Z B. Z > Y > X C. X > Y > Z D. Z > Y > X 43. The following half-reaction can be balanced in acidic solution: N O 5 NH 4 + Which of the following appear in the balanced equation? A. 13e B. 14e C. 16e D. 18e 44. Consider the following redox reaction: MnO H I Mn + + 8H O + 5I A 10.0 ml sample of an iodide solution is titrated with 15.7mL of acidified M MnO 4. What is the I A M B M C M D M [ ] of the sample? Chemistry Form A Page 15

18 45. Consider the following diagram of a standard electrochemical cell: e Object 1 e Zn(s) Cu(s) 1.0 M Zn(NO 3 ) 1.0 M Cu(NO 3 ) Which of the following is correct? Object 1 Zn () s A. light bulb cathode B. light bulb anode C. power supply cathode D. power supply anode Page 16 Chemistry Form A

19 Use the following diagram to answer questions 46, 47 and 48. H (g) Volts Pt (inert) Porous Barrier Ag 1.0 M HCl 1.0 M AgNO What is the overall cell reaction? A. Ag + + H + H + Ag B. Ag + H + Ag + + H C. Ag + + H H + + Ag D. Ag + + H Ag + H + + e 47. Which of the following is correct as the cell operates? Direction of NO 3 Migration ph near the Pt Electrode A. towards Pt increases B. towards Pt decreases C. towards Ag increases D. towards Ag decreases 48. Which of the following describes the direction of electron flow and the change in mass of the Ag electrode as the cell operates? Direction of Electron Flow Mass of Ag Electrode A. from Pt to Ag increases B. from Pt to Ag decreases C. from Ag to Pt increases D. from Ag to Pt decreases Chemistry Form A Page 17

20 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 Cl B. H and O C. Na + and Cl D. NaOH and Cl You have Examination Booklet Form A. In the box above #1 on your Answer Sheet, ensure you filled in the bubble as follows. Exam Booklet Form/ Cahier d examen A B C D E F G H This is the end of the multiple-choice section. Answer the remaining questions in the Response Booklet. Page 18 Chemistry Form A

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23 PERIODIC TABLE OF THE ELEMENTS H Hydrogen Li Lithium Be Si Silicon 8.1 Atomic Number Symbol Name Atomic Mass 5 B Boron 6 C Carbon 7 N Nitrogen O Oxygen 9 F Fluorine He Ne Neon 11 Na 1 Mg Sodium Magnesium Aluminum Silicon Phosphorus Sulphur Al 14 Si 15 P S 17 Cl 18 Ar Argon 19 K 0 Ca 1 Sc Ti 3 V Scandium Titanium Vanadium Chromium Manganese 4 Cr Mn 6 Fe 7 Co 8 Ni 9 Cu Cobalt Nickel Copper 30 Zn 31 Ga 3 Ge 33 As Germanium Arsenic Selenium Se 35 Br 36 Kr Krypton 37 Rb Rubidium Strontium Sr 39 Y 40 Zr 41 Nb Zirconium Niobium 4 Mo 43 Tc (98) 44 Ru 45 Rh 46 Pd Technetium Ruthenium Rhodium Palladium 47 Ag 48 Cd In 50 Sn 51 Sb Cadmium Indium Tin Antimony Tellurium Iodine Xenon Te 53 I 54 Xe 55 Cs Cesium 56 Ba 57 La 7 Hf 73 Ta 74 W Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 8 Pb 83 Bi 84 Po 85 At 86 Rn Lead Bismuth Polonium Astatine Radon 09.0 (09) (10) () 87 Fr 88 Ra 89 Ac 104 Rf 105 Db Francium Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium (3) (6) (7) (61) (6) (63) (6) (65) (66) 106 Sg 107 Bh 108 Hs 109 Mt Based on mass of C 1 at Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally. 58 Ce Cerium Th Thorium Pr Praseodymium Pa Protactinium Nd Neodymium U Uranium Pm Promethium (145) 93 Np Neptunium (37) 6 Sm Samarium Pu Plutonium (44) 63 Eu Europium Am Americium (43) 64 Gd Cm Curium (47) 65 Tb Terbium Bk Berkelium (47) 66 Dy Dysprosium 98 Cf Californium 67 Ho Holmium 99 Es Einsteinium 68 Er Erbium Fm Fermium (57) 69 Tm Thulium 101 Md Mendelevium (58) 70 Yb Ytterbium 10 No Nobelium (59) 71 Lu Lutetium 103 Lr (6) Potassium Beryllium Calcium 87.6 Barium Yttrium Molybdenum Silicon Iron Silver Gadolinium Zinc Mercury Gallium Thallium (51) (5) Chlorine 35.5 Bromine Helium Lawrencium Chemistry 1 Data Page 1

24 Data Page Chemistry 1 ATOMIC MASSES OF THE ELEMENTS Based on mass of C 1 at Values in parentheses are the mass number of the most stable or best known isotopes for elements that do not occur naturally. 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 (7) 7.0 (43) (10) (47) (51) (47) (6) 16.5 (5) (57) 19.0 (3) (6) (58) 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 (37) (59) (44) (09) (145) 31.0 (6) () (61) (98) Element Symbol Atomic Number Atomic Mass Element Symbol Atomic Number Atomic Mass

25 NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air. ** Not stable in aqueous solutions. Po s i t i v e I o n s ( C a t i o n s ) Al 3+ Aluminum Pb 4+ Lead(IV), plumbic NH 4 + Ammonium Li + Lithium Ba + Barium Mg + Magnesium Ca + Calcium Mn + Manganese(II), manganous Cr + Chromium(II), chromous Mn 4+ Manganese(IV) Cr 3+ Chromium(III), chromic Hg + Mercury(I)*, mercurous Cu + Copper(I)*, cuprous Hg + Mercury(II), mercuric Cu + Copper(II), cupric K + Potassium H + Hydrogen Ag + Silver H 3 O + Hydronium Na + Sodium Fe + Iron(II)*, ferrous Sn + Tin(II)*, stannous Fe 3+ Iron(III), ferric Sn 4+ Tin(IV), stannic Pb + Lead(II), plumbous Zn + Zinc Negative Ions (Anions) Br Bromide OH Hydroxide CO 3 Carbonate ClO Hypochlorite ClO 3 Chlorate I Iodide Cl Chloride HPO 4 Monohydrogen phosphate ClO Chlorite NO 3 Nitrate CrO 4 Chromate NO Nitrite CN Cyanide C O 4 Oxalate Cr O 7 Dichromate O Oxide** H PO 4 Dihydrogen phosphate ClO 4 Perchlorate CH 3 COO Ethanoate, acetate MnO 4 Permanganate F Fluoride PO 4? Phosphate HCO 3 Hydrogen carbonate, bicarbonate SO 4 Sulphate HC O 4 Hydrogen oxalate, binoxalate S Sulphide HSO 4 Hydrogen sulphate, bisulphate SO 3 Sulphite HS Hydrogen sulphide, bisulphide SCN Thiocyanate HSO 3 Hydrogen sulphite, bisulphite Chemistry 1 Data Page

26 SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0.1 mol/l at 5 C. Negative Ions (Anions) Positive Ions (Cations) Solubility of Compounds All Alkali ions: Li +, Na +, K +, Rb +, Cs +, Fr + Soluble All Hydrogen ion: H + Soluble All Ammonium ion: NH 4 + Soluble Nitrate, NO 3 All Soluble or or Chloride, Cl Bromide, Br Iodide, I 1443 All others Ag +, Pb +, Cu + Soluble Low Solubility or or Sulphate, SO All others Alkali ions, H +, NH + Sulphide, S 4, Be +, Mg +, Ca +, Sr +, Ba + All others Alkali ions, H +, NH + Hydroxide, OH 4, Sr +? Phosphate, PO 4 3 Carbonate, CO 3 Sulphite, SO 3 Ag +, Ca +, Sr +, Ba +, Pb + All others Alkali ions, H +, NH 4 + All others Soluble Soluble Soluble Soluble Low Solubility Low Solubility Low Solubility Low Solubility Data Page Chemistry 1

27 SOLUBILITY PRODUCT CONSTANTS AT 5 C Name 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 Formula BaCO 3 BaCrO 4 BaSO 4 CaCO 3 CaC O 4 CaSO 4 CuI Cu(IO 3 ) CuS Fe(OH) FeS Fe(OH) 3 PbBr PbCl Pb(IO 3 ) PbI PbSO 4 MgCO 3 Mg(OH) AgBrO 3 AgBr Ag CO 3 AgCl Ag CrO 4 AgIO 3 AgI SrCO 3 SrF SrSO 4 ZnS K sp Chemistry 1 Data Page

28 RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASES in aqueous solution at room temperature. Name of Acid Acid Base K a S T R O N G S T R E N G T H O F A C I D W E A K 4 4 Perchloric HClO H + ClO Hydriodic HI H + I Hydrobromic HBr H + Br Hydrochloric HCl H + Cl 3 3 Nitric HNO H + NO very large very large very large very large very large Sulphuric HSO4 H + HSO4 very large + Hydronium Ion H O + 3 H + HO 1. 0 Iodic HIO 3 H + IO Oxalic H C O H + HC O Sulphurous ( SO + HO) H SO 3 H + HSO3 Hydrogen sulphate ion HSO 4 H + SO Phosphoric H PO H + H PO Hexaaquoiron ion iron III ion Fe( HO) + 6 H + Fe( HO) ( OH) +, ( ) 5 Citric H3C6H5O 7 H + HC6H5O7 Nitrous HNO H + NO Hydrofluoric HF H + + F Methanoic, formic HCOOH H + HCOO Hexaaquochromium ion, chromium( III) ion Cr( H O) H + Cr( H O) ( OH) 6 5 Benzoic C H COOH 6 5 H C6H5COO Hydrogen oxalate ion HC O 4 H + CO4 Ethanoic, acetic CH COOH 3 H CH3COO Dihydrogen citrate ion H C H O H + HC H O Hexaaquoaluminum ion, aluminum ion Al( H O) H + Al( H O) ( OH) Carbonic ( CO + HO) H CO 3 H + HCO Monohydrogen citrate ion + HC6H5O 7 H + C6H5O Hydrogen sulphite ion HSO3 H + SO Hydrogen sulphide HS H + HS Dihydrogen phosphate ion H PO + 4 H + HPO Boric H3BO 3 H + HBO Ammonium ion NH + 4 H + NH Hydrocyanic HCN H + CN Phenol C H OH 6 5 H + C6H5O Hydrogen carbonate ion HCO + 3 H + CO Hydrogen peroxide HO H + HO Monohydrogen phosphate ion HPO 4 H + PO4. 10 Water H O H + OH Hydroxide ion OH H + O very small 3 Ammonia NH H + NH very small 14 W E A K S T R E N G T H O F B A S E S T R O N G Data Page Chemistry 1

29 ACID-BASE INDICATORS Indicator 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 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 Chemistry 1 Data Page

30 STANDARD REDUCTION POTENTIALS OF HALF-CELLS Ionic concentrations are at 1M in water at 5 C. Oxidizing Agents Reducing Agents E ( Volts) S T R O N G S T R E N G T H O F O X I D I Z I N G A G E N T F ( g) + e F S O + e SO H O + H + e H O MnO + 8H + 5e Mn + 4H O Au + 3e Au( s) BrO + 6H + 5e Br ( l ) + 3H O ClO + 8H + 8e Cl + 4H O Cl ( g) + e Cl CrO H + 6e Cr + 7HO 1 O( g) + H + e H O MnO ( s) + 4H + e + Mn + H O IO + 6H + 5e I ( s) + 3H O Br ( l) + e Br AuCl + 3e Au( s) + 4Cl NO + 4H + 3e NO( g) + H O Hg + e Hg( l) O ( g) + H ( 10 M) + e H O NO + 4H + e N O + H O Ag + e Ag( s) Hg e Hg l ( ) Fe + e Fe O ( g) + H + e H O MnO + H O + 3e MnO ( s) + 4OH I ( s) + e I Cu + e Cu( s) H SO + 4H + 4e S( s) + 3H O Cu + e Cu( s) SO + 4H + e H SO + H O Cu + e Cu Sn + e Sn S( s) + H + e H S( g) H + e H ( g) Pb + e Pb( s) Sn + e Sn( s) Ni + e Ni( s) H PO + H + e H PO + H O 0. 8 Co + e Co( s) Se( s) + H + e H Se Cr + e Cr H O + e H + OH ( 10 M) Overpotential Effect W E A K S T R E N G T H O F R E D U C I N G A G E N T W E A K Overpotential Effect Fe + e Fe( s) Ag S( s) + e Ag( s) + S Cr + 3e Cr( s) Zn + e Zn( s) ( ) + Te( s) + H + e H Te H O e H g OH Mn + e Mn( s) Al + 3e Al( s) Mg + e Mg( s). 37 Na + e Na( s). 71 Ca + e Ca( s). 87 Sr + e Sr( s). 89 Ba + e Ba( s). 91 K + e K( s). 93 Rb + e Rb( s). 98 Cs + e Cs( s) Li + e Li( s) S T R O N G Data Page Chemistry 1

31 MINISTRY USE ONLY MINISTRY USE ONLY Question (.5) NR Question (.5) NR Place Personal Education Number (PEN) here. Question (.5) NR Question 4 Course Code = CH 008/09 Released Exam JUNE 009 Exam Booklet, Form/ Cahier d examen A B C 1 D E F G H 0 1 Question Question (.5) (.5) NR NR (.5) NR 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. Question Question (.5) (.5) NR NR. Use a pencil to fill in bubbles when answering questions on your Answer Sheet. 3. Use a pencil or blue- or black-ink pen when answering written-response questions in this Booklet. 4. When the examination begins, remove the Data Pages located in the centre of the Examination Booklet. 5. Read the Examination Rules on the back of this Booklet. 814 Version

32 MINISTRY USE ONLY Place Personal Education Number (PEN) here. Course Code = CH 1 Chemistry 1 008/09 Released Exam JUNE 009 Response Booklet Instructions: Answer the following questions in the space provided in this Response Booklet. You are expected to communicate your knowledge and understanding of chemical principles in a clear and logical manner. Your steps and assumptions leading to a solution must be written in this Response Booklet. Answers must include units where appropriate and be given to the correct number of significant figures. For questions involving calculations, full marks will NOT be given for providing only an answer. Province of British Columbia

33 PART B: WRITTEN RESPONSE Value: 37.5% of the examination Suggested Time: 40 minutes 1. (4 marks) A student burned a paraffin candle ( C 5 H 5 ) in an open beaker according to the following equation: C 5 H 5 ()+ s 38 O ( g) 5CO ( g) + 6H Og ( ) The following data was recorded: Time (min) Mass of candle and beaker (g) Calculate the rate of paraffin consumption in moles of C 5 H 5 per minute ( mol C 5 H 5 min); then, calculate how long it would take to produce 0.70 g CO. Chemistry Response Booklet Page 1

34 . (4 marks) Consider the following equilibrium: CO( g) + 3H ( g) CH 4 ( g) + H Og ( ) Initially, 0.00 mol CO and mol H are placed in a.00 L container. At equilibrium, [ H O] = M. Calculate the value of K eq. Page Chemistry Response Booklet

35 3. (4 marks) Consider the following equilibrium: Mg( OH) () s Mg + ( aq) + OH ( aq) What happens to the amount of solid Mg( OH) when some HCl is added? On the graph below, sketch the effect of adding HCl at time t 1. Mg + Concentration (M) OH - t 1 Time (s) Chemistry Response Booklet Page 3

36 4. (3 marks) A solution of Sr ( OH) ( aq) is titrated with H SO 4. Explain what will happen to the electrical conductivity during the titration. Begin by writing the balanced formula equation, including states, to support your answer. Page 4 Chemistry Response Booklet

37 5. (5 marks) Aniline C 6 H 5 NH ( ) is a weak base with a K b = Calculate the concentration of an aniline solution that has a ph = Begin by writing the equation for the predominant equilibrium. Chemistry Response Booklet Page 5

38 6. (3 marks) Calculate the OH [ ] that results when ml of M HCl is mixed with 1.16 g Sr OH (Assume no volume change on mixing.) ( ). Page 6 Chemistry Response Booklet

39 7. (4 marks) Balance the following redox equation in acidic solution: Te O 4 + In In O 3 + Te (acidic) Chemistry Response Booklet Page 7

40 8. (3 marks) Consider the following cell diagram: Power Supply + Pb(s) Cu(s) 1 M K SO 4 Write the overall cell reaction. Write the formula for a precipitate that forms as the cell operates. Page 8 Chemistry Response Booklet

41 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 students break any of the following rules: Students must not be in possession of or have used any secure examination materials prior to the examination session. Students must not communicate with other students during the examination. Students must not give or receive assistance of any kind in answering an examination question during an examination, including allowing one s paper to be viewed by others or copying answers from another student s paper. Students must not possess any book, paper or item that might assist in writing an examination, including a dictionary or piece of electronic equipment, that is not specifically authorized for the examination by ministry policy. Students must not copy, plagiarize or present as one s own, work done by any other person. Students must immediately follow the invigilator s order to stop writing at the end of the examination time and must not alter an Examination Booklet, Response Booklet or Answer Sheet after the invigilator has asked students to hand in examination papers. Students must not remove any piece of the examination materials from the examination room, including work pages. 4. The use of inappropriate language or content may result in a mark of zero being awarded. 5. Upon completion of the examination, return all examination materials to the supervising invigilator.