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 2003 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.. (5) Question 7: 7.. (4) Question 2: 2.. (2) Question 8: 8.. (4) Question 3: 3.. (2) Question 9: 9.. (3) Question 4: 4.. (3) Question 10: 10.. (3) Question 5: 5.. (6) Question 11: 11.. (4) Question 6: 6.. (4)

3 Chemistry 12 APRIL 2003 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 multiplechoice answers must be entered on the Response Form using an HB pencil. Multiplechoice answers entered in this examination booklet will not be marked. 3. For each of the writtenresponse 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 multiplechoice questions PART B: 11 writtenresponse 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 BrønstedLowry Acids and Bases AcidBase Indicators Standard Reduction Potentials of Halfcells No other reference materials or tables are allowed. 3. A calculator is essential for the Chemistry 12 Provincial Examination. The calculator must be a handheld device designed primarily for mathematical computations involving logarithmic and trigonometric functions. The calculator must not be programmable. Computers, calculators with a QWERTY keyboard or symbolic manipulation abilities, and electronic writing pads will not be allowed. Students must not bring any external devices (peripherals) to support calculators such as manuals, printed or electronic cards, printers, memory expansion chips or cards, CDROMS, libraries or external keyboards. 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. Note that some multiplechoice questions are worth 2 marks. 1. Consider the following reaction occurring in an open container: CaCO3( s) + 2HCl( aq) Æ CaCl2( aq) + H2O( l) + CO2( g) The reaction rate could be calculated by using which of the following? (1 mark) A. a change in [ Cl ] B. a decrease in ph value C. a change in gas pressure D. a decrease in the mass of the system 2. Which of the following does not affect both homogeneous and heterogeneous reaction rates? (1 mark) A. addition of a catalyst B. change in temperature C. change in surface area D. change in concentration 3. How do KE and PE change as reactant particles collide with each other? (1 mark) KE PE A. increases increases B. increases decreases C. decreases increases D. decreases decreases 1 OVER

8 4. Under which of the following conditions will the reaction rate decrease for a reaction which goes to completion? (1 mark) A. A catalyst is removed. B. Products are removed. C. Temperature is increased. D. Solid reactants are ground into powders. 5. Consider the following potential energy diagram for a reaction: (2 marks) PE (kj) Progress of the reaction Which of the following represents the correct activation energies? Forward Catalyzed E a Reverse Uncatalyzed E a A. 40 kj 140 kj B. 80 kj 40 kj C. 100 kj 80 kj D. 100 kj 160 kj 2

9 6. What is an important function of the catalyst found in an automobile exhaust system? (1 mark) A. increase fuel economy B. decrease the rate of CO 2 production C. increase the conversion rate of NO 2 to N 2 D. increase the conversion rate of heat into work 7. For the equilibrium system below: Cu( s) + 2Ag ( aq) Æ 2Ag( s) + Cu ( aq) We would know the system is at equilibrium because A. Cu Ag B [ ]= [ ] [ Cu ]= [ Ag ] C. the mass of Cu ( s) remains constant. D. the mass of the entire system remains constant. (1 mark) 8. For the reacting system: (2 marks)? 2Li( s) + 2H2O( ) Æ l 2LiOH( aq) + H2( g) DH = 433kJ What will entropy and enthalpy factors favour? Entropy Enthalpy A. products reactants B. products products C. reactants reactants D. reactants products 3 OVER

10 9. Consider the following equilibrium: N2( g) + 3H2( g) Æ 2NH3 ( g) If some Ne gas is added at a constant volume then how will [ N 2 ], H 2 be affected? [ ] and K eq (2 marks) [ N 2 ] [ H 2 ] K eq A. increases increases decreases B. decreases decreases increases C. decreases increases does not change D. does not change does not change does not change 10. What is the effect of adding a catalyst to an equilibrium system? (1 mark) A. The value of E a increases. B. The value of K eq increases. C. Forward and reverse rates increase. D. The concentration of products increases. 11. Consider the following equilibrium: + 2CrO4 2 ( aq) + 2H ( aq) Æ Cr2O 7 2 ( aq) + H2O l ( ) What is the K eq expression? (1 mark) A. B. C. D. + [ CrO4 ] [ H ] Cr O [ ] Cr2O 7 2 [ ] CrO [ 4 ] [ H ] 2 Cr2O 7 2 [ ] 2 + 2CrO 2H [ 4 ][ ] Cr2O 7 2 [ ][ H2O] CrO [ 4 ] [ H ] 2 4

11 12. A container is initially filled with pure SO 3. After a period of time, the following equilibrium is established: 2SO2( g) + O2( g) Æ 2SO3 ( g) Keq = What does this equilibrium mixture contain? (1 mark) A. mostly products B. mostly reactants C. 3 5 reactants and 2 5 products D. equal amounts of reactants and products 13. Consider the following equilibrium: 2CO( g) + O2( g) Æ 2CO2( g) Keq = What is the value of K eq for 2CO2( g) Æ 2CO( g) + O2( g)? (1 mark) A B C D Consider the following equilibrium: H2( g) + Br2( g) Æ 2HBr( g) DH =36kJ How could the value of K eq be increased? (1 mark) A. add H 2 B. add HBr C. increase the pressure D. reduce the temperature 5 OVER

12 15. Which of the following is a suitable term for representing solubility? (1 mark) A. grams B. moles C. molarity D. millilitres per second 16. A saturated solution is prepared by dissolving a salt in water. Which of the following graphs could represent the ion concentrations as the temperature is changed? (1 mark) A. Concentration anion cation B. Concentration anion cation Time Time C. Concentration anion cation D. Concentration anion cation Time Time 17. What is the concentration of OH ions in 250 ml of M Sr( OH) 2? (1 mark) A M B M C M D M 6

13 18. What happens when ml of 0. 2 M KOH is added to ml of 0. 2 M CuSO 4? (1 mark) A. No precipitate forms. B. A precipitate of K2SO4 C. A precipitate of Cu( OH) 2 forms. D. Precipitates of K2SO4 and Cu OH ( ) 2 form. 19. Solid NaCl is added to a saturated AgCl solution. How have the Ag + changed when equilibrium has been reestablished? [ ] and [ Cl ] (2 marks) [ Ag + ] [ Cl ] A. increased increased B. decreased increased C. increased decreased D. decreased decreased 20. Which of the following expressions represents Fe 3+ saturated Fe OH [ ] in a ( ) 3 solution? (1 mark) A. B. C. K sp [ ] 3 OH Ksp [ OH ] 3 3 Ksp [ OH ] D. Ksp [ OH ] 3 7 OVER

14 21. What is the value of K sp for Zn( OH) 2 if the solubility of Zn( OH) 2 is equal to M? (2 marks) A B C D What is the maximum number of moles of Cl that can exist in ml of 2. 0 M AgNO 3? (1 mark) A B C D In which of the following is HSO 3 acting as a BrønstedLowry acid? (1 mark) A. HSO + H O Æ H SO + OH B. NH + HSO Æ NH + SO C. HSO + HPO Æ H SO + PO D. H C O + HSO Æ HC O + H SO 24. What is the conjugate base of H PO 2 4? (1 mark) A. OH B. 3 PO 4 C. HPO 4 2 D. H PO 3 4 8

15 25. Which of the following is correct if the four solutions listed are compared to one another? (2 marks) Concentration Relative Conductivity Ionization A. strong acid 050. M highest complete B. weak acid 050. M lowest complete C. strong base 10. M highest complete D. weak base 10. M lowest complete 26. Which of the following is the strongest acid that can exist in an aqueous solution? (1 mark) A. O 2 B. NH 2 C. + H 3 O D. HClO Which of the following household products could have a ph = 12. 0? (1 mark) A. soda pop B. tap water C. lemon juice D. oven cleaner 28. What is the ph of a M KOH solution? (1 mark) A B C D OVER

16 29. What is the value of K b for H PO 2 4? (1 mark) A B C D Which of the following describes the net ionic reaction for the hydrolysis of NH4Cl( s)? (1 mark) + A. NH4 ( aq) + Cl ( aq) Æ NH4Cl( s) B. + NH4Cl( s) Æ NH4 ( aq) + Cl ( aq) C. Cl ( aq) + H2O( l) Æ HCl( aq) + OH ( aq) + D. NH4 ( aq) + H2O( l) Æ NH3 ( aq) + H3O ( aq) Which of the following salts will produce a solution with the highest ph? (2 marks) A M NaNO3 B M NaHSO4 C M NaHCO3 D M NaH2PO4 32. What is true about the transition point of all indicators described by the following equilibrium: + HIn + H O Æ H O + In 2 3 (1 mark) A. ph = K a [ ]= [ ] B. HIn In 7 C. [ H3O + ]= M D. moles of H O 3 + equals moles of OH 10

17 33. A chemical indicator has a K a = What is the ph at the transition point and the identity of the indicator? (2 marks) ph Indicator A. 54. methyl red B. 54. bromcresol green C. 86. phenolphthalein D. 86. thymol blue ( ). 34. A ml sample of HCl is titrated with ml of M Sr OH 2 What is the concentration of the acid? (2 marks) A M B M C M D M 35. Which of the following is the net ionic equation for the neutralization of HNO 3( aq) with Sr( OH) 2( aq )? (1 mark) + A. H ( aq) + OH ( aq) Æ H 2 O l 2+ ( ) + Æ ( ) B. Sr ( aq) 2NO3 ( aq) Sr NO3 2( s) C. 2HNO Sr OH Sr NO 2H O + + ( ) Æ ( ) + l 3( aq) 2( aq) 3 2( aq) 2 ( ) D. 2H ( aq) + 2NO3 ( aq) + Sr ( aq) + 2OH ( aq) Æ Sr ( aq) + 2NO3 ( aq) + 2H2O l ( ) 36. When a strong acid is titrated with a strong base, what will the ph value be at the equivalence point? (1 mark) A B C D OVER

18 37. Which of the following acids could not be present in a buffer solution? (1 mark) A. HF B. HNO 2 C. H2SO3 D. HClO The equation for the decomposition of nitrous acid is 3HNO Æ 2NO + HNO + H O Which of the following is correct? (1 mark) A. This is a redox reaction. B. This is an acidbase reaction. C. This is a reduction half equation. D. This is an oxidation half equation. 39. An equation for the rusting of iron is shown below: 4Fe + 3O Æ 2Fe O Which of the following is false? (1 mark) A. This is a redox reaction. B. O 2 is the oxidizing agent. C. Metallic iron is reduced to Fe 3+. D. Metallic iron is the reducing agent. 40. In which of the following chemical changes will there be an oxidation number change of +3? (1 mark) A. Cr Æ Cr B. ClO Æ ClO Æ 4 C. Cr Æ Cr O D. Mn MnO 12

19 41. Which of the following ions can be reduced by Pb ( s) under standard conditions? (1 mark) A. Cu + B. Cr 3+ C. Sn 2+ D. Ca Consider the following equation for the combustion of ethane: 2CH + 7O Æ 4CO + 6HO The change in oxidation number for carbon is equivalent to (1 mark) A. 1 electron lost. B. 7 electrons lost. C. 1 electron gained. D. 7 electrons gained. 43. Consider the diagram below: Volts H 2(g) 1.0 M KNO3 Co (s) Au (s) 1.0 M HCl 1.0 M Co(NO 3 ) 2 Identify the cathode half reaction. (2 marks) + A. H2 Æ 2H + 2e + B. 2H + 2e Æ H2 3+ C. Au + 3e Æ Au 2+ D. Co + 2e Æ Co 13 OVER

20 44. As a standard Zn / Ag electrochemical cell operates, in which direction do anions move and how does the mass of the cathode change? (2 marks) Anion Direction Mass of Cathode A. towards Zn electrode increases B. towards Ag electrode increases C. towards Zn electrode decreases D. towards Ag electrode decreases 45. What is the standard cell potential for the following reaction: (1 mark) Cr + 3Cu Æ 2Cr + 3Cu ( s) ( s) A V B V C V D V 46. Consider the following: Cr + Tl Æ 2Cr + Tl E = V Identify the standard potential for the halfcell reaction: A V B V C V D V + 3+ Tl Æ Tl + 2 e (1 mark) 14

21 47. The electrolysis of aqueous Rb2SO4 solution using carbon electrodes produces changes in the solution around the electrodes. How will the ph change around the anode and the cathode? (2 marks) ph around the Anode ph around the Cathode A. increase increase B. decrease decrease C. increase decrease D. decrease increase 48. The same amount of electricity (same number of moles of electrons) is used to carry out the electrolysis of PdCl 2( aq) and AgNO 3( aq) solutions in separate cells. The masses of Pd and Ag produced were measured and compared. Which of the following is true about the mass of Pd produced? (1 mark) A. The mass of Pd produced is not related to the mass of Ag. B. The mass of Pd produced is approximately half that of Ag. C. The mass of Pd produced is approximately twice that of Ag. D. The mass of Pd produced is approximately the same as that of Ag. This is the end of the multiplechoice section. Answer the remaining questions directly in this examination booklet. 15 OVER

22 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. 16

23 1. Consider the following reaction: 3Cu( s) + 8HNO3 ( aq) Æ 3Cu( NO3) 2( aq) + 2NO( g) + 4H2O( l) A piece of copper is added to a nitric acid solution in an open beaker, allowing the NO g ( ) to escape. The following data was obtained: TIME (min) MASS OF BEAKER AND CONTENTS (g) Copper a) Calculate the reaction rate for the time period 2. 0 to 6. 0 min. (2 marks) b) Calculate the mass of copper consumed in the first 5 minutes. (3 marks) 17 OVER

24 2. Using collision theory, explain why reactions between two solutions occur more rapidly than reactions between two solids. (2 marks) 3. Consider the following reaction for the Haber Process for ammonia production: N2( g) + 3H2( g) Æ 2NH3 ( g) DH =92kJ The system is normally maintained at a temperature of approximately 500 C. a) Explain why 1000 C is not used. (1 mark) b) Explain why 100 C is not used. (1 mark) 18

25 4. Consider the following equilibrium: SO3 ( g) + NO( g) Æ NO2( g) + SO2( g) In an experiment, moles of SO 3 and moles of NO are placed in a L container. When equilibrium is achieved, [ NO2]= mol L. Calculate the K eq value. (3 marks) 19 OVER

26 5. a) Write the net ionic equation for the reaction between Pb( NO 3 ) 2( aq) and NaCl ( aq). (2 marks) b) Determine, with calculations, whether a precipitate will form when ml of M Pb( NO3) 2 is added to 35. 0mL of M NaCl. (4 marks) 20

27 6. An acidbase reaction occurs between HSO 3 and IO 3. a) Write the equation for the equilibrium that results. (1 mark) b) Identify one conjugate acidbase pair in the reaction. (1 mark) c) State whether reactants or products are favoured, and explain how you arrived at your answer. (2 marks) 21 OVER

28 7. At 10 C, K = w. a) Determine the ph of water at 10 C. (3 marks) b) State whether water at this temperature is acidic, basic or neutral, and explain. (1 mark) 22

29 8. Calculate the ph of M H2S. (4 marks) 23 OVER

30 9. Consider the following experimental results: Ce + Pd Æ Pd + Ce 3+ In + Cd Æno reaction Pd + In Æ In + Pd 2+ Cd + Pd Æno reaction Use these results to complete the table of reduction halfreactions below. (3 marks) WEAKEST STRONGEST Oxidizing Agents Æ Æ Æ Æ Reducing Agents WEAKEST STRONGEST 10. Balance the following equation. (3 marks) Cr O C O Cr CO acidic + Æ + ( ) 2 24

31 11. Consider the following electrolytic cell which contains a porous barrier to prevent general mixing of solutions. Power Supply DC+ e Pt Porous Barrier Cu 1.0 M Sn(NO 3 ) M Cu(NO 3 ) 2 a) Label the anode and cathode in the space provided on the diagram above. (1 mark) b) Write an equation for the overall cell reaction. (2 marks) c) Calculate the minimum theoretical voltage required for this reaction under standard conditions. (1 mark) END OF EXAMINATION 25

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

34 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 BrønstedLowry Acids and Bases 7 Acidbase Indicators 8 Standard Reduction Potentials of Halfcells REFERENCE D.R. Lide, CRC Handbook of Chemistry and Physics, 80 th edition, CRC Press, Boca Raton, 1999.

35 PERIODIC TABLE OF THE ELEMENTS Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine H He Hydrogen Helium Ne Neon Atomic Number Symbol Name Atomic Mass 3 Li Lithium Si Silicon Na Mg Sodium Magnesium Aluminum Silicon Phosphorus Sulphur Chlorine Argon Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Ni Cu Zn Ga Ge As Se Br Kr Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Nickel Rb Y Zr Nb Mo Tc Ru Rh Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon (98) Sr Pd Ag Cd In Sn Sb Te I Xe Cs Ba Cesium Barium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon (209) (210) (222) Fr Ra La Hf Ac Rf Ta Francium Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium (223) (226) (227) (261) (262) (263) (262) (265) (266) 74 W Db Sg Re Os Bh Hs Ir Mt Pt Au Hg Tl Pb Bi Po At Rn 58 Ce Cerium Based on mass of C 12 at 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) Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally. 1

36 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

37 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

38 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

39 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

40 RELATIVE STRENGTHS OF BRØNSTEDLOWRY 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 H2O H Cr H 6 2O OH Benzoic C6H5COOH H + C6H5COO Hydrogen oxalate ion HC2O 4 H + C2O Ethanoic, acetic CH3COOH H + CH3COO Dihydrogen citrate ion H C H O H + HC H O ( ) + ( ) ( ) Hexaaquoaluminum ion, aluminum ion Al H2O H Al H O OH Carbonic ( CO + HO 2 ) HCO H + HCO Monohydrogen citrate ion HC6H5O 7 H + C6H5O Hydrogen sulphite ion HSO3 H + SO Hydrogen sulphide H2S + H + HS Dihydrogen phosphate ion H2PO4 H + HPO Boric H3BO3 H + H2BO Ammonium ion + + NH4 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 6

41 ACIDBASE 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

42 STANDARD REDUCTION POTENTIALS OF HALFCELLS 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 + 2e 2SO HO + 2H + 2e 2HO MnO + 8H + 5e Mn + 4H O Au + 3e Au( s) + BrO3 + 6H + 5e 1 Br 2 2( l) + 3H2O ClO + + 8H + 8e Cl + 4H O Cl2( g) e Cl O 2 2( g) H e H2O + 2+ MnO2( s) ( s) 2 Br2( l) e Br AuCl4 e Au( s) Cl + 3 ( g) 2 2+ Hg e Hg( l) O 2 2( g) H M e H2O Ag e Ag( s) 1 2+ Hg 2 2 e Hg( l) O ( ) H e 2 g H2O ( s) I2( s) e I + Cu e Cu( s) ( s) + 3 2O 2+ Cu e Cu( s) SO + 4H + 2e H SO + H O Cu + e Cu Sn + 2e Sn S( ) + 2H + 2e s H2S( g) + 2H + 2e H2( g) 2+ Pb + 2e Pb( s) 2+ Sn + 2e Sn( s) Ni + 2e Ni( s) HPO + + 2H + 2e HPO + HO Co e Co( s) + Se( s) H e H2Se Cr + e Cr H Fe e Fe( s) 2 Ag2S( s) e Ag() s S 3+ Cr e Cr( s) 2+ Zn e Zn( s) ( s) Te HO 2 e H2( g) OH 2+ Mn e Mn( s) 3+ Al e Al( s) 2+ Mg e Mg( s) + Na e Na( s) 2+ Ca e Ca( s) 2+ Sr + e Sr( s) 2+ Ba e Ba( s) + K e K( s) + Rb e Rb( s) + Cs e Cs( s) + Li e Li( s) O + 2e H + 2OH ( 10 M) Te H e H Cr O + 14H + 6e 2Cr + 7H O H + 2e Mn + 2H O IO + 6H + 5e I + 3H O NO + 4H + 3e NO + 2H O ( 10 ) NO + 4H + 2e N O + 2H O Fe e Fe MnO + 2H O + 3e MnO + 4OH HSO H e S H Overpotential Effect WEAK STRENGTH OF REDUCING AGENT STRONG