Chemistry 12 APRIL Course Code = CH. Student Instructions

Transcription

1 MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry Ministry of Education APRIL 2002 Course Code = CH Student Instructions 1. Place the stickers with your Personal Education Number (PEN) in the allotted spaces above. Under no circumstance is your name or identification, other than your Personal Education Number, to appear on this booklet. 2. Ensure that in addition to this examination booklet, you have a Data Booklet and an Examination Response Form. Follow the directions on the front of the Response Form. 3. Disqualification from the examination will result if you bring books, paper, notes or unauthorized electronic devices into the examination room. 4. When instructed to open this booklet, check the numbering of the pages to ensure that they are numbered in sequence from page one to the last page, which is identified by END OF EXAMINATION. 5. At the end of the examination, place your Response Form inside the front cover of this booklet and return the booklet and your Response Form to the supervisor.

2 Question 1: 1.. (3) Question 2: 2.. (2) Question 3: 3.. (2) Question 4: 4.. (4) Question 5: 5.. (5) Question 6: 6.. (3) Question 8: 8.. (2) Question 9: 9.. (5) Question 10: 10.. (3) Question 11: 11.. (4) Question 12: 12.. (2) Question 13: 13.. (3) Question 7: 7.. (2)

3 CHEMISTRY 12 APRIL 2002 COURSE CODE = CH

4 GENERAL INSTRUCTIONS 1. Aside from an approved calculator, electronic devices, including dictionaries and pagers, are not permitted in the examination room. 2. All multiple-choice answers must be entered on the Response Form using an HB pencil. Multiple-choice answers entered in this examination booklet will not be marked. 3. For each of the written-response questions, write your answer in the space provided in this booklet. 4. Ensure that you use language and content appropriate to the purpose and audience of this examination. Failure to comply may result in your paper being awarded a zero. 5. This examination is designed to be completed in two hours. Students may, however, take up to 30 minutes of additional time to finish.

5 CHEMISTRY 12 PROVINCIAL EXAMINATION 1. This examination consists of two parts: Value Suggested Time PART A: 48 multiple-choice questions PART B: 13 written-response questions Total: 100 marks 120 minutes 2. The following tables can be found in the separate Data Booklet: Periodic Table of the Elements Atomic Masses of the Elements Names, Formulae, and Charges of Some Common Ions Solubility of Common Compounds in Water Solubility Product Constants at 25 C Relative Strengths of Brønsted-Lowry Acids and Bases Acid-Base Indicators Standard Reduction Potentials of Half-cells No other reference materials or tables are allowed. 3. A calculator is essential for the Chemistry 12 Provincial Examination. The calculator must be a hand-held device designed primarily for mathematical computations involving logarithmic and trigonometric functions and may also include graphing functions. Computers, calculators with a QWERTY keyboard, and electronic writing pads will not be allowed. Students must not bring any external devices to support calculators such as manuals, printed or electronic cards, printers, memory expansion chips or cards, or external keyboards. Students may have more than one calculator available during the examination. Calculators may not be shared and must not have the ability to either transmit or receive electronic signals. In addition to an approved calculator, students will be allowed to use rulers, compasses, and protractors during the examination.

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7 PART A: MULTIPLE CHOICE Value: 60 marks INSTRUCTIONS: Suggested Time: 70 minutes For each question, select the best answer and record your choice on the Response Form provided. Using an HB pencil, completely fill in the circle that has the letter corresponding to your answer. Selected multiple-choice questions are worth 2 marks. 1. Which of the following could be used to describe the rate of a reaction? (1 mark) A. B. C. D. change in time change in mass change in mass change in volume change in volume change in time change in volume change in mass 2. Consider the following reaction: 2HO 2 2( aq) 2HO 2 ( l) + O2( g) Which factor explains why the above reaction speeds up in the presence of MnO 2( s)? (1 mark) A. temperature B. concentration C. nature of reactants D. presence of catalyst - 1 -

8 3. What happens to the potential energy and the total energy as an activated complex changes into products? (1 mark) PE Total Energy A. increases increases B. decreases decreases C. increases remains constant D. decreases remains constant 4. Consider the following PE diagram: (1 mark) 400 PE (kj) Progress of the reaction Which of the following describes the type of reaction and H for the reverse reaction? Type of Reaction H kj ( ) A. exothermic positive B. endothermic positive C. exothermic negative D. endothermic negative - 2 -

9 5. Consider the following diagram for a catalyzed and uncatalyzed reaction: (2 marks) 250 PE (kj) Progress of the reaction Which of the following describes the forward reaction? Reaction Activation Energy kj ( ) H kj ( ) A. catalyzed B. uncatalyzed C. catalyzed D. uncatalyzed Consider the following reaction mechanism: (1 mark) Step 1 NO2 + SO2 SO3 + NO Step 2 NO + 1 O NO Identify the catalyst. A. O 2 B. NO C. SO 2 D. NO OVER

10 7. Consider the following: (1 mark) H2( g) + I 2( g) 2HI( g) Initially, HI is added to an empty flask. How do the rates of the forward and reverse reactions change as the system proceeds to equilibrium? Forward Rate Reverse Rate A. increases increases B. increases decreases C. decreases decreases D. decreases increases 8. Consider the following reaction: (2 marks) 2H2O( l) + energy 2H2( g) + O2( g) Determine the enthalpy and entropy changes for the above reaction? Enthalpy Entropy A. increases decreases B. decreases increases C. increases increases D. decreases decreases - 4 -

11 Use the following equilibrium equation to answer questions 9 and CO( g) + O2( g) 2CO2( g) + energy 9. Which of the following two stresses will each cause the system to shift to the right? (1 mark) A. increase temperature, increase volume B. decrease temperature, increase volume C. increase temperature, decrease volume D. decrease temperature, decrease volume 10. Which of the following shows the forward rate of reaction when the temperature of the system is increased at time = t 1? (1 mark) A. B. rate rate t 1 time t 1 time C. D. rate rate t 1 time t 1 time OVER

12 11. Consider the following: (1 mark) 2SO2( g) + O 2( g) 2SO3 ( g) Initially, mol SO 2 and mol O 2 are placed into a 1. 0 L container. At equilibrium, there is mol O 2 present. What is the SO 2 A mol L B mol L C mol L D mol L [ ] at equilibrium? 12. What is the equilibrium expression for the following system? (1 mark) CaCO3( s) + 2HF ( g) CaF2( s) + H2O( g) + CO2( g) A. K HF HO CO [ 2 ][ 2] eq = [ ] [ HO ][ CO ] B. Keq = HF [ ] [ HO ][ CO ] C. K eq = 2 2 CaCO HF D. K eq 2 [ 3][ ] [ CaF2][ H2O][ CO2] = 2 CaCO HF 2 [ 3][ ] 13. What will cause the K eq for an endothermic reaction to decrease? (1 mark) A. adding a catalyst B. increasing the surface area C. increasing the temperature D. decreasing the temperature - 6 -

13 14. Consider the following equilibrium: (2 marks) N2( g) + O 2( g) 2NO( g) An equilibrium mixture consists of mol N 2, mol O2 and mol NO in a 1. 0 L container. What is the value of K eq? A B C D Which of the following will dissolve in water to form an ionic solution? (1 mark) A. O 2 B. CH 4 C. NH4Cl D. CH3OH 16. The solubility of SrCO 3 is M. How many moles of dissolved solute are present in ml of saturated SrCO 3 solution? (1 mark) A B C D mol mol mol mol OVER

14 17. What are the ion concentrations in M CuCl 2? (1 mark) [ Cu 2+ ] [ Cl ] A M 0. 20M B M 0. 10M C M 0. 30M D M 0. 60M 18. What is the net ionic equation for the reaction that occurs when equal volumes of M Ba( NO3) 2 and M Na2SO 4 are mixed together? (1 mark) 2+ 2 aq aq 4( s) A. Ba ( ) + SO4 ( ) BaSO + aq 3 aq 3( s) B. Na ( ) + NO ( ) NaNO ( ) + + C. Ba NO Na SO BaSO 2NaNO 3 2( aq) 2 4( aq) 4( s) 3( aq) aq aq aq aq 4 s aq 3 aq D. Ba ( ) + 2NO3 ( ) + 2Na ( ) + SO4 ( ) BaSO ( ) + 2Na ( ) + 2NO ( ) 19. Consider the following equilibrium: (2 marks) AgIO + ( ) Ag ( ) + IO 3 s aq 3 aq A few crystals of NaIO 3 are added to the above equilibrium. When equilibrium is re-established, how do the new ion concentrations compare with the original equilibrium concentrations? [ Ag + ] [ IO 3 ] A. decreased decreased B. decreased increased C. increased decreased D. increased increased ( ) - 8 -

15 20. The K sp expression for Zn( OH) 2 is (1 mark) sp = 2+ 2 [ ][ ] sp = [ 2+ 2 ] [ ] sp = [ 2+ ][ 2 ] sp = [ + ][ 2 ] A. K Zn OH B. K Zn OH C. K Zn OH 2 2 D. K Zn OH 21. The solubility of CdCO 3 is M. Calculate the K sp value for CdCO 3. (1 mark) A B C D At 25 C, what is the [ Cl ] in a saturated solution of PbCl 2? (2 marks) A M B M C M D M 23. The property common to both M HCl and M NaOH is that both solutions (1 mark) A. taste bitter. B. have a ph > 7. C. conduct electricity. D. react with magnesium to produce hydrogen gas OVER

16 24. Consider the following Brønsted-Lowry equilibrium: (1 mark) ( aq) 2 ( l) ( aq) aq C H NH + H O C H NH + OH ( ) The substances acting as acids and bases from left to right are A. acid, base, acid, base. B. acid, base, base, acid. C. base, acid, acid, base. D. base, acid, base, acid. 25. Consider the following equilibrium: (1 mark) In the above equilibrium, a conjugate pair is 2 4 A. HPO and HC O 2 4 B. HPO and H PO 2 aq aq 2 4 aq 2 4 aq H2C2O4( ) + HPO 4 ( ) HC O ( ) + H PO C. H2C2O4 and HPO4 D. H2C2O4 and H2PO4 ( ) 26. The strength of the acids HCl H SO and H PO strongest is A. HCl, H3PO4, H2SO3 B. HCl, H SO, H PO C. H2SO3, H3PO4, HCl D. H3PO4, H2SO3, HCl, from the weakest to (1 mark)

17 27. Consider the following equilibrium at 25 C : (2 marks) HO + ( ) HO ( aq) + OH ( aq) 2 2 l 3 What happens to [ OH ] and ph as 0. 1M HCl is added? A. [ OH ] decreases and ph increases. B. [ OH ] decreases and ph decreases. C. [ OH ] increases and ph increases. D. [ OH ] increases and ph decreases. 28. What is the value of the ionization constant for water at 25 C? (1 mark) A B C D Which of the following equations represents the dissociation of Sr( NO 3 ) 2 in water? (1 mark) 2+ ( ) s aq + aq A. Sr NO3 2( ) Sr ( ) 6NO ( ) ( ) 2+ s aq + 3 ( aq) ( ) 2+ s aq + 3 ( aq) ( ) 2+ 2 s aq + ( 3) 2 aq B. Sr NO3 2( ) Sr ( ) 2NO C. Sr NO3 2( ) 2Sr ( ) NO D. Sr NO3 2( ) Sr ( ) NO ( ) OVER

18 30. What is the equilibrium constant expression representing the predominant reaction for the hydrolysis of NaHCO 3( aq)? (2 marks) w = + [ 3 ][ ] A. K H O OH B. K C. K D. K [ + Na ][ HCO ] eq = 3 [ NaHCO3] [ + HO ][ 2 CO ] a = 3 3 [ HCO3 ] [ HCO ][ OH ] b = 2 3 [ HCO3 ] 31. Which of the following salt solutions will be neutral? (1 mark) A M NH4Cl B M LiClO4 C M K2C2O4 D M NaHCO3 32. The chemical indicator bromthymol blue changes from yellow to blue as a result of the addition of (1 mark) A M HCl B M HNO2 C M K2CO3 D M NH4Cl 33. A chemical indicator has a K a = Determine the identity of this indicator. (1 mark) A. phenol red B. thymol blue C. phenolphthalein D. chlorophenol red

19 34. Pure sodium hydrogen phthalate is used to standardize a solution of NaOH for use in an acid-base titration. What term is used to describe the sodium hydrogen phthalate? (1 mark) A. titrant base B. standard buffer C. equivalent base D. primary standard 35. Calculate the volume of M NaOH required to completely neutralize ml of M H2SO 4. (2 marks) A ml B ml C ml D ml 36. Which of the following is the net ionic equation for the neutralization of CH COOH 3 with NaOH? (1 mark) A. CH3COO ( aq) + OH ( aq) CH3COOH( aq) + O ( aq) B. CH3COOH( aq) + OH ( aq) H2O( l) + CH3COO ( aq) C. CH3COOH + NaOH NaCH3COO + H2O l 2 ( aq) ( aq) ( aq) ( ) + + D. CH3COO ( aq) + H ( aq) + Na ( aq) + OH ( aq) Na ( aq) + CH3COO ( aq) + H2O l + ( ) 37. The ph of normal rainwater is (2 marks) A. less than 7. 0 due to dissolved SO 2( g) B. less than 7. 0 due to dissolved CO 2( g) C. greater than 7. 0 due to dissolved CO 2( g) D. equal to 7. 0 due to dissolved N 2 and O OVER

20 38. Which of the following describes a strong oxidizing agent? (1 mark) A. a substance which loses electrons readily B. a substance which gains electrons readily C. a substance which has a large increase in oxidation number D. a substance which has a small increase in oxidation number 39. Consider the following unbalanced redox reaction: (2 marks) Sn + MnO Sn + Mn Which of the following describes the change in Sn 2+? A. loses electrons and is reduced B. gains electrons and is reduced C. loses electrons and is oxidized D. gains electrons and is oxidized 40. A solution containing Pd 2+ reacts spontaneously with Ga to produce Pd and Ga 3+. However, a solution containing Pd 2+ does not react with Pt. The metals, in order of increasing strength as reducing agents, are (1 mark) A. Pt < Pd < Ga B. Pt < Ga < Pd C. Ga < Pt < Pd D. Ga < Pd < Pt

21 41. Which of the following can act as an oxidizing agent, but not as a reducing agent? (1 mark) A. Cr B. Cl C. Cu + D. Na Solid copper forms spontaneously in the following reaction: (1 mark) V + Cu Cu + V Based on this observation, Cu 2+ is a A. weaker reducing agent than V 2+ B. weaker oxidizing agent than V 2+ C. stronger reducing agent than V 2+ D. stronger oxidizing agent than V Which of the following could be used to determine the [ Fe 2+ ] by a redox titration? (1 mark) A. I 2 B. Cl C. Cu 2+ D. MnO 4 (acidified) OVER

22 Use the following diagram to answer questions 44, 45 and 46. Volts Lead 1.0 M KNO3 Copper 1.0 M Pb(NO 3 ) M Cu(NO 3 ) What happens to the lead electrode? (2 marks) A. It loses mass as it is reduced. B. It gains mass as it is reduced. C. It loses mass as it is oxidized. D. It gains mass as it is oxidized. 45. As the cell operates, what happens to the ions in the salt bridge? (1 mark) A. K + and NO 3 will both migrate toward the Pb half-cell. B. K + and NO 3 will both migrate toward the Cu half-cell. C. K + will migrate toward the Cu half-cell and NO 3 will migrate toward the Pb half-cell. D. K + will migrate toward the Pb half-cell and NO 3 will migrate toward the Cu half-cell. 46. What is the initial cell voltage? (1 mark) A V B V C V D V

23 47. Consider the following: (2 marks) I. electrolysis of water II. III. electroplating of copper rusting of iron Which of the above involve non-spontaneous redox reactions? A. I and II only B. I and III only C. II and III only D. I, II and III 48. A copper spoon was electroplated with silver. Which of the following reactions occurred at the cathode during electroplating? (1 mark) + A. Ag Ag + e B. + Ag + e Ag C. 2+ Cu Cu + 2e D. 2+ Cu + 2e Cu This is the end of the multiple-choice section. Answer the remaining questions directly in this examination booklet OVER

24 PART B: WRITTEN RESPONSE Value: 40 marks INSTRUCTIONS: Suggested Time: 50 minutes You will be 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 the spaces below the questions. 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: (3 marks) CH 2 4( g) + 3O2( g) 2CO2( g) + 2HO 2 ( g) At certain conditions, mol CO 2 is produced in 2. 0 minutes. What is the rate of consumption of C 2 H 4 in gs? 2. Define the term reaction mechanism. (2 marks)

25 3. State Le Chatelier s Principle. (2 marks) 4. Consider the following: (4 marks) CH4( g) + H2O ( g) CO( g) + 3H2( g) Initially, mol CH 4, mol H2O, mol CO and mol H 2 are placed into a L container. At equilibrium, the [ H2]= mol L. What is the value of K eq? OVER

26 5. A ml sample of a saturated solution of Ag2SO4 was heated in an evaporating dish until all the water was evaporated. The following data were recorded: Volume of solution ml Mass of evaporating dish g Mass of evaporating dish and solid Ag2SO g Calculate the K sp value for Ag SO 2 4. (5 marks)

27 6. The ion H PO 2 4 is an amphiprotic anion. a) Define the term amphiprotic. (1 mark) b) Write the balanced equation for the reaction when H PO 2 4 reacts with HF. (2 marks) 7. Write an equation for a reaction in which H O 2 acts only as a Brønsted-Lowry base. (2 marks) 8. Calculate the ph of M Sr( OH) 2. (2 marks) OVER

28 9. Calculate the ph of M NH4Cl. (5 marks)

29 10. A 0. 1M unknown acid is titrated with M NaOH and the following titration curve results: ph Volume of 0.1M NaOH added a) Choose a suitable indicator (other than phenolphthalein) and give a reason for your choice. (1 mark) Suitable Indicator: Reason: b) Is the unknown acid weak or strong? Explain. (2 marks) Unknown Acid: Explanation: OVER

30 11. Balance the following redox reaction: (4 marks) Ag O + Si Ag + SiO (acidic) 12. Sodium metal is produced commercially by the electrolysis of molten NaCl ( l). Explain why sodium metal, Na ( s), cannot be produced by electrolysis of aqueous NaCl ( aq). (2 marks)

31 13. Blister copper is an impure sample of copper containing small amounts of zinc and gold. Blister copper is purified using electrolysis. + DC Power Source Blister Copper Pure Copper Cu (Zn) (Au) Cu Cu 2+ Sufficient voltage is supplied to oxidize copper at the anode. a) What happens to the zinc at the anode? Explain. (2 marks) b) Write the equation for the half-reaction that occurs at the cathode. (1 mark) END OF EXAMINATION

32 Data Booklet CHEMISTRY 12 Work done in this booklet will not be marked. Ministry of Education Revised January 2000

33 CONTENTS Page Table 1 Periodic Table of the Elements 2 Atomic Masses of the Elements 3 Names, Formulae, and Charges of Some Common Ions 4 Solubility of Common Compounds in Water 5 Solubility Product Constants at 25 C 6 Relative Strengths of Brønsted-Lowry Acids and Bases 7 Acid-base Indicators 8 Standard Reduction Potentials of Half-cells REFERENCE D.R. Lide, CRC Handbook of Chemistry and Physics, 80 th edition, CRC Press, Boca Raton, 1999.

34 PERIODIC TABLE OF THE ELEMENTS H Hydrogen Li Lithium Be Beryllium Si Silicon 28.1 Atomic Number Symbol Name Atomic Mass 5 B Boron C Carbon N Nitrogen O Oxygen F Fluorine He Helium Ne Neon Na Sodium Mg Magnesium Al Aluminum Si Silicon P Phosphorus S Sulphur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenum Tc Technetium (98) 44 Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Fr Francium (223) 56 Ba Barium Ra Radium (226) 57 La Lanthanum Ac Actinium (227) 72 Hf Hafnium Rf Rutherfordium (261) 73 Ta Tantalum Db Dubnium (262) 74 W Tungsten Sg Seaborgium (263) 75 Re Rhenium Bh Bohrium (262) 76 Os Osmium Hs Hassium (265) 77 Ir Iridium Mt Meitnerium (266) 78 Pt Platinum Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth Po Polonium (209) 85 At Astatine (210) 86 Rn Radon (222) Based on mass of C 12 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 (237) 62 Sm Samarium Pu Plutonium (244) 63 Eu Europium Am Americium (243) 64 Gd Gadolinium Cm Curium (247) 65 Tb Terbium Bk Berkelium (247) 66 Dy Dysprosium Cf Californium (251) 67 Ho Holmium Es Einsteinium (252) 68 Er Erbium Fm Fermium (257) 69 Tm Thulium Md Mendelevium (258) 70 Yb Ytterbium No Nobelium (259) 71 Lu Lutetium Lr Lawrencium (262) 1

35 ATOMIC MASSES OF THE ELEMENTS Based on mass of C 12 at Values in parentheses are the mass number of the most stable or best known isotopes for elements that do not occur naturally. 2 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 (227) 27.0 (243) (210) (247) (251) (247) (262) (252) (257) 19.0 (223) (262) (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 (237) (259) (244) (209) (145) (226) (222) (261) (98) Element Symbol Atomic Number Atomic Mass Element Symbol Atomic Number Atomic Mass

36 NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air. ** Not stable in aqueous solutions. Positive Ions (Cations) Al 3+ Aluminum Pb 4+ Lead(IV), plumbic NH 4 + Ammonium Li + Lithium Ba 2+ Barium Mg 2+ Magnesium Ca 2+ Calcium Mn 2+ Manganese(II), manganous Cr 2+ Chromium(II), chromous Mn 4+ Manganese(IV) Cr 3+ Chromium(III), chromic Hg 2 2+ Mercury(I)*, mercurous Cu + Copper(I)*, cuprous Hg 2+ Mercury(II), mercuric Cu 2+ Copper(II), cupric K + Potassium H + Hydrogen Ag + Silver H 3 O + Hydronium Na + Sodium Fe 2+ Iron(II)*, ferrous Sn 2+ Tin(II)*, stannous Fe 3+ Iron(III), ferric Sn 4+ Tin(IV), stannic Pb 2+ Lead(II), plumbous Zn 2+ Zinc Negative Ions (Anions) Br Bromide OH Hydroxide CO 3 2 Carbonate ClO Hypochlorite ClO 3 Chlorate I Iodide Cl Chloride HPO 4 2 Monohydrogen phosphate ClO 2 Chlorite NO 3 Nitrate CrO 4 2 Chromate NO 2 Nitrite CN Cyanide C 2 O 4 2 Oxalate Cr 2 O 7 2 Dichromate O 2 Oxide** H 2 PO 4 Dihydrogen phosphate ClO 4 Perchlorate CH 3 COO Ethanoate, acetate MnO 4 Permanganate F Fluoride PO 4 3 Phosphate HCO 3 Hydrogen carbonate, bicarbonate SO 4 2 Sulphate HC 2 O 4 Hydrogen oxalate, binoxalate S 2 Sulphide HSO 4 Hydrogen sulphate, bisulphate SO 3 2 Sulphite HS Hydrogen sulphide, bisulphide SCN Thiocyanate HSO 3 Hydrogen sulphite, bisulphite 3

37 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 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 All others Ag +, Pb 2+, Cu + Soluble Low Solubility Sulphate, SO 4 2 All others Ag +, Ca 2+, Sr 2+, Ba 2+, Pb 2+ Soluble Low Solubility Sulphide, S 2 Alkali ions, H +, NH 4 +, Be 2+, Mg 2+, Ca 2+, Sr 2+, Ba 2+ All others Soluble Low Solubility Hydroxide, OH Alkali ions, H +, NH 4 +, Sr 2+ All others Soluble Low Solubility or or Phosphate, PO 4 3 Carbonate, CO 3 2 Sulphite, SO 3 2 Alkali ions, H +, NH 4 + All others Soluble Low Solubility 4

38 SOLUBILITY PRODUCT CONSTANTS AT 25 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 2 O 4 CaSO 4 CuI Cu IO 3 CuS FeS ( ) AgBr AgCl AgI ZnS ( ) 2 Fe( OH) 2 Fe OH 3 PbBr 2 PbCl 2 ( ) 2 Pb IO 3 PbI 2 PbSO 4 MgCO 3 ( ) 2 Mg OH AgBrO 3 Ag 2 CO 3 Ag 2 CrO 4 AgIO 3 SrCO 3 SrF 2 SrSO 4 K sp

39 RELATIVE STRENGTHS OF BR NSTED-LOWRY ACIDS AND BASES in aqueous solution at room temperature. Name of Acid Acid Base K a STRONG STRENGTH OF ACID WEAK Perchloric HClO H + ClO Hydriodic HI H + I + Hydrobromic HBr H + Br + Hydrochloric HCl H + Cl Nitric HNO H + NO very large very large very large very large very large Sulphuric H2SO4 H + HSO4 very large + Hydronium Ion H O + 3 H + H2O Iodic HIO + 3 H + IO Oxalic H C O + H + HC O ( 2 ) , ( III) 6 + Fe( H2O) ( OH) ( ) + Sulphurous SO H O H SO H HSO Hydrogen sulphate ion HSO H SO Phosphoric H PO H H PO Hexaaquoiron ion iron ion Fe H O H Citric H C H O H H C H O Nitrous HNO H NO Hydrofluoric HF H + F Methanoic, formic HCOOH H + HCOO Hexaaquochromium ion chromium III ion Cr H , ( ) 2O H Cr H 6 2O OH H2C6H5O + H HC H O Al( H2O) H Al H O OH 6 + ( 2 ) ( ) Benzoic C H COOH H C H COO Hydrogen oxalate ion HC O H C O Ethanoic, acetic CH COOH H CH COO. Dihydrogen citrate ion ( ) + ( ) ( ) Hexaaquoaluminum ion, aluminum ion Carbonic ( CO + HO) HCO 2 H + HCO Monohydrogen citrate ion HC H O H C H O Hydrogen sulphite ion HSO H SO 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 Phenol C 6H5OH H + C6H5O Hydrogen carbonate ion HCO3 H + CO Hydrogen peroxide H2O2 H + HO Monohydrogen phosphate ion 2 + HPO4 H + PO Water H O + H + OH Hydroxide ion OH H + O very small Ammonia NH H + NH very small WEAK STRENGTH OF BASE STRONG Ð 6 Ð

40 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 7

41 STANDARD REDUCTION POTENTIALS OF HALF-CELLS Ionic concentrations are at 1M in water at 25 C. Oxidizing Agents Reducing Agents E ( Volts) STRONG STRENGTH OF OXIDIZING AGENT WEAK Overpotential Effect F2( g) + 2e 2F SO e 2SO HO H + 2e 2HO MnO4 + 8H + 5e Mn + 4H2O Au + 3e Au( s) BrO3 + 6H + 5e 1 Br 2 2( l) + 3H2O ClO4 + 8H + 8e Cl + 4H2O Cl2( g) + 2e 2Cl Cr2O H + 6e 2Cr + 7H2O O 2 2( ) + 2H + 2e g H2O MnO2( s) H 2e Mn + 2H2O IO3 6H 5e I ( ) s H2O Br2( l) + 2e 2Br AuCl + 4 3e Au( s) + 4Cl NO H 3e NO( g) + 2H2O Hg + 2e Hg( l) O ( ) + H ( M)+ e g H2O + + 2NO3 + 4H + 2e N2O4 + 2H2O Ag + e Ag( s) Hg e Hg( l) Fe + e 2+ Fe O ( ) + 2H + 2e H O 2 g MnO H2O 3e MnO2( s) + 4OH I2( s) + 2e 2I Cu + e Cu( s) HSO H 4e S( s) + 3H2O Cu + 2e Cu( s) SO4 + 4H + 2e H2SO3 + H2O Cu + e + Cu Sn + 2e 2+ Sn S( ) + 2H + 2e s H2S( g) H + 2e H2( g) Pb + 2e Pb( s) Sn + 2e Sn( s) Ni + 2e Ni( s) HPO H + 2e HPO HO Co + 2e Co( s) Se( ) + 2H + 2e s H2Se Cr + e 2+ Cr H2O + e 7 2 H2 + 2OH ( 10 M) Fe + 2e Fe( s) Ag S + e 2 2 ( s) 2 2Ag() s + S Cr + 3e Cr( s) Zn + 2e Zn( s) Te + H + e ( s) 2 2 H2 Te 079. HO+ e H2( g) + 2OH Mn + 2e Mn( s) Al + 3e Al( s) Mg + 2e Mg( s) Na + e Na( s) Ca + 2e Ca( s) Sr + 2e Sr( s) Ba + 2e Ba( s) K + e K( s) Rb + e Rb( s) Cs + e Cs( s) Li + e Li( s) 304. Ð 8 Ð Overpotential Effect WEAK STRENGTH OF REDUCING AGENT STRONG