Chemistry 12 JUNE 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 JUNE 2001 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.. (4) Question 7: 7.. (5) Question 2: 2.. (2) Question 8: 8.. (4) Question 3: 3.. (4) Question 9: 9.. (2) Question 4: 4.. (4) Question 10: 10.. (3) Question 5: 5.. (4) Question 11: 11.. (2) Question 6: 6.. (2) Question 12: 12.. (4)

3 CHEMISTRY 12 JUNE 2001 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: 12 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 reactions is slowest at room temperature? (1 mark) A. NH + HCl NH Cl 3( g) ( g) 4 ( s) B. MgCl + Ca Mg + CaCl 2( s) ( s) ( s) 2( s) C. HCl + NaOH NaCl + H 2 O l ( aq) ( aq) ( aq) ( ) ( ) + + D. Ba NO Na SO BaSO 2NaNO 3 2( aq) 2 4( aq) 4( s) 3( aq) 2. Consider the following reaction: (1 mark) COCl2( g) CO( g) + Cl2( g) Which of the following could be used to determine reaction rate in a closed system? A. a decrease in gas pressure B. an increase in gas pressure C. a decrease in the mass of the system D. an increase in the mass of the system 3. Activation energy is defined as the (1 mark) A. H. B. average kinetic energy. C. energy of a particle s motion. D. minimum energy needed for a successful collision. 4. Which of the following reactions is endothermic? (1 mark) A. CH + 2O CO + 2H O kJ 4( g) 2( g) 2( g) 2 ( l ). 2 2 s + 2 l. aq + 2 g B. 2Na O ( ) 2H O( ) 287 0kJ 4NaOH( ) O ( ) C. CaO( s) H2O( l ) Ca OH 2( aq) H =65. 2 kj D. CaO( s) + 3C( s) CaC2( s) + CO( g) H = kj + ( ) OVER

8 5. The following diagram shows reactant molecules approaching one another: (2 marks) Cl O N O Cl What is happening to the kinetic energy and the potential energy? Kinetic Energy Potential Energy A. decreasing decreasing B. decreasing increasing C. increasing increasing D. increasing decreasing 6. A proposed mechanism for a reaction is: (1 mark) Step 1 H O + I HI + H O Step 2 H2O2 + HI H2O + HOI Step 3 HOI + H O + I 2H O + I 2 3 Step 4 I + I I In the above mechanism, which of the following is true for the overall reaction? A. HI is a catalyst B. H 3 O is a product C. H 2 O 2 is a reactant D. H 2 O is an intermediate - 2 -

9 7. Consider the following reaction: (2 marks) ( ) ( ) + ( ) 2ICl g I2 g Cl2 g A closed container is initially filled with ICl ( g). What are the changes in the rate of the forward reaction and [ I 2 ], as the system approaches equilibrium? Rate of forward reaction [ I 2 ] A. decreases increases B. decreases decreases C. increases increases D. increases decreases 8. The entropy of a system is a term used to describe (1 mark) A. randomness. B. heat content. C. average kinetic energy. D. stored chemical energy. 9. Consider the following equilibrium: (1 mark) 2+ 2 aq aq 4 aq Cu ( ) + 4Br ( ) + energy CuBr blue colourless green Which of the following will cause this equilibrium to change from blue to green? ( ) A. adding NaBr ( s) B. adding NaNO 3( s) C. adding a catalyst D. decreasing the temperature OVER

10 10. Consider the following equilibrium: (1 mark) Ni( s) 4CO( g) Ni CO 4( l) H kJ Which of the following will cause this equilibrium to shift to the left? A. add some CO B. decrease the volume C. remove some Ni( CO) 4 D. increase the temperature 11. Consider the following equilibrium: (1 mark) N2O4( g) + energy 2NO2( g) Which of the following shows the relationship between concentration and time as a result of adding a catalyst at time = t 1? A. B. NO 2 NO 2 concentration N 2 O 4 concentration N 2 O 4 t 1 time t 1 time C. D. NO 2 NO 2 concentration N 2 O 4 concentration N 2 O 4 t 1 time t 1 time - 4 -

11 12. Consider the following equilibrium: (1 mark) HS + I HI + S 2 ( g) 2( s) 2 ( g) ( s) What is the equilibrium expression for this reaction? A. K HI HS [ 2 ] eq = [ ] [ HS ] B. Keq = 2 2 HI C. K [ ] 2 eq = [ ] 2 [ ] HI S HS I [ 2 ][ 2] [ HS ][ I ] D. K eq = HI S [ ] [ ] 13. Consider the following equilibrium: (1 mark) CO( g) + H O( g) CO ( g) + H ( g) Keq = At equilibrium, the [ CO]= 020. mol L, [ H2O]= 030. mol L, and [ H2]= 090. mol L. Calculate the equilibrium [ CO 2 ]. A mol L B mol L C mol L D. 10. mol L OVER

12 14. Consider the following: (2 marks) CO2( g) + CF 4( g) 2COF2( g) Keq = In a reaction container the initial concentrations are: [ 2]= [ 4]= [ 2]= CO 050. mol L, CF 050. mol L, COF 030. mol L To reach equilibrium, the reaction will proceed A. left since Trial K < K eq B. left since Trial K > K eq C. right since Trial K < K eq D. right since Trial K > K eq eq eq eq eq 15. Consider the following equilibrium: (1 mark) BaSO 2+ 4( ) Ba ( ) + SO 2 s aq 4 aq Adding which of the following will cause more solid BaSO 4 to form? ( ) A. CaCl 2( s) B. K2CO3( s) C. Na2SO4( s) D. Mg( NO 3 ) 2 ( s) 16. Which of the following could not be used to represent solubility? (1 mark) A. gml B. ml L C. mol L D. g min - 6 -

13 17. The following three beakers each contain different volumes of a saturated solution of PbI 2 and different masses of solid PbI 2 : (2 marks) Beaker I Beaker II Beaker III What is the relationship for the [ Pb 2+ ] in the solution in the three beakers? A. I = II = III B. I > II > III C. II > III > I D. III > II > I 18. The equation that describes the solubility equilibrium of Ag2CrO4 is (1 mark) A. Ag CrO ( s) Ag2 ( aq) + CrO4 ( aq) B. Ag CrO ( s) 2Ag ( aq) + CrO4 ( aq) C. Ag2CrO4( s) 2Ag( s) Cr( s) 2O2( g) D. Ag CrO ( s) 2Ag ( aq) + Cr ( aq) + 4O ( aq) OVER

14 19. When ml of M Zn NO3 2 ( ) is added to a 10. 0mL sample of 0. 20M unknown. M Ca( NO ) is added to a solution, no precipitate forms. When the same volume of separate ml sample of the unknown solution, a precipitate does form. (2 marks) 0.20 M Zn( NO 3 ) M Ca( NO 3 ) 2 no precipitate forms precipitate forms The identity of the unknown solution could be A. NaCl B. Na 2 S C. Na2SO4 D. Na2CO3 20. The solubility of PbS is A B C D M. The value of K sp is (1 mark) - 8 -

15 21. A hydronium ion has the formula (1 mark) A. H 2 + B. OH C. + H 2 O D. + H 3 O 22. The conjugate acid of C H NH A. C6H5NH B. C6H5NH3 + C. C6H5NH2 + D. C6H5NH3 is (1 mark) 23. Which of the following is a property of 1. 0 M HCl but not a property of 1. 0 M CH3COOH? (1 mark) A. turns litmus red B. ionizes completely C. has a ph less than 7. 0 D. produces H 3 O in solution, 24. In a 1. 0 M HF solution, the concentration of HF, F, and OH from highest to lowest is [ ] > [ ] > [ ] [ ] > [ ] > [ ] [ ] > [ ] > [ ] [ ] > [ ] > [ ] A. HF F OH B. F HF OH C. OH HF F D. OH F HF (2 marks) OVER

16 25. In which of the following reactions is water behaving as a Brønsted-Lowry acid? (1 mark) A. 2HO 2H + O B. HCl H O H O Cl C. NH + H O NH + OH D. NH H O H O NH 26. What is the OH A M B M C M D M + 2 [ ] of a solution with [ H3O ]= M.? (1 mark) 27. The ph of 010. M HNO3 is (1 mark) A B C D What is the poh of a solution made by adding ml of M NaOH to ml of water? (2 marks) A B C D Which of the following 1. 0 M solutions will have the lowest ph? (1 mark) A. HCl B. HCN C. H3PO4 D. H2C2O4-10 -

17 30. The value of K b for HTe is The value of Ka for H2 Te is (1 mark) A B C D In an aqueous solution of NaCl, the ph is (1 mark) A. less than 7 and the solution is acidic. B. equal to 7 and the solution is neutral. C. greater than 7 and the solution is basic. D. greater than 7 and the solution is acidic. Use the following equation for questions 32 and 33. Consider the following equation for the indicator methyl red, HInd. + HInd + H O H O + Ind At ph = 40., methyl red solution will be (2 marks) [ ] > [ ] [ ] < [ ] [ ] > [ ] [ ] < [ ] A. red and HInd Ind B. red and HInd Ind C. yellow and HInd Ind D. yellow and HInd Ind 33. Methyl red is orange in a M solution of an acid. The acid could be (1 mark) A. HI B. HCl C. HCN D. H2SO OVER

18 34. How many moles of KOH are necessary to completely neutralize ml of M HCl? (1 mark) A moles B moles C moles D moles 35. At the equivalence point, the titration of HCl with NH 3 will form a solution which is (2 marks) A. basic with ph > 7. B. acidic with ph < 7. C. acidic with ph > 7. D. neutral with ph = Which of the following could be added to an equal number of moles of NaCH COO 3 to prepare a buffer solution? (1 mark) A. HCl B. HNO 3 C. NaOH D. CH3COOH 37. Which of the following equations describes the reaction that occurs when MgO is added to water? (1 mark) A. MgO H2O Mg OH 2 B. MgO + H2O MgO2 + H2 C. MgO + H2O MgH2 + O2 D. 2MgO + 2H O 2MgOH + H + O + ( ) Which of the following represents a redox reaction? (1 mark) A. H2 + I2 2HI B. HCl + NH 3 NH 4 Cl C. H2O + CO2 H2CO3 D. 2NaI + Pb( NO ) PbI + 2NaNO

19 39. In an experiment, Ag + reacts spontaneously with Ru but not with Pd. The relative strength of the metals from strongest to weakest reducing agent is (2 marks) A. Ag > Ru > Pd B. Pd > Ag > Ru C. Ru > Ag > Pd D. Ru > Pd > Ag 40. A piece of Ag does not react spontaneously with 1. 0 M Ti + because (1 mark) A. Ag + is a weaker reducing agent than Ti 2+ B. Ag + is a weaker oxidizing agent than Ti 2+ C. Ag + is a stronger reducing agent than Ti 2+ D. Ag + is a stronger oxidizing agent than Ti Which of the following will react spontaneously with Ag S 2 at standard conditions? (1 mark) A. Al B. Au C. Co D. Pb 42. When a piece of Cu is placed in 1. 0 M HNO 3, (1 mark) A. the H + B. the Cu 2+ C. the NO 3 [ ] increases. [ ] decreases. [ ] decreases. D. no change occurs. 43. When MnO 2 changes to Mn O 2 3 in an alkaline battery, manganese atoms (2 marks) A. lose electrons and are reduced. B. gain electrons and are reduced. C. lose electrons and are oxidized. D. gain electrons and are oxidized OVER

20 Use the following cell to answer questions 44 and 45. Volts Cu 1.0 M KNO3 Ag 1.0 M Cu( NO 3 ) M AgNO Which of the following diagrams represents the relationship between the mass of the Cu electrode and the mass of the Ag electrode as the cell is in operation? (1 mark) A. B. Mass of Cu Mass of Cu Mass of Ag Mass of Ag C. D. Mass of Cu Mass of Cu Mass of Ag Mass of Ag 45. The E for the above cell is (1 mark) A Volts B Volts C Volts D Volts

21 46. The value of E for a cell can be used to determine (1 mark) A. rate. B. spontaneity. C. temperature. D. activation energy. 47. How is the formation of rust on an iron can inhibited by a tin coating? (1 mark) A. The tin is a sacrificial anode. B. The tin cathodically protects the iron. C. The tin is a weaker reducing agent than iron. D. The tin keeps the oxygen away from the iron. 48. The electrolysis of 1. 0 M CuF 2 using inert electrodes will produce (2 marks) A. copper and oxygen. B. copper and fluorine. C. hydrogen and oxygen. D. hydrogen and fluorine. This is the end of the multiple-choice section. Answer the remaining questions directly in this examination booklet 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 calculation, full marks will NOT be given for providing only an answer. 1. The mass of a burning candle is monitored to determine the rate of combustion of paraffin. An accepted reaction for the combustion of paraffin is: 2C28H58( s) + 85O2( g) 56CO2( g) + 58H2O( g) The following data is observed: Time (min) Mass of Candle (g)

23 a) Calculate the average rate of consumption of paraffin in g min for the time interval to minutes. (2 marks) b) Calculate the rate of CO 2 production in mol min for the time interval to minutes. (2 marks) 2. Write four statements that apply to all chemical equilibrium systems. (2 marks) i) ii) iii) iv) OVER

24 3. Consider the following equilibrium system: H2( g) + Br 2( g) 2HBr( g) Keq = A closed container was initially filled with equal moles of H 2 and Br 2. When equilibrium is reached, the [ HBr] is mol L. What was the initial H 2 [ ]? (4 marks)

25 4. Calculate the molar solubility of SrF 2. (4 marks) 5. Does a precipitate form when 3. 0 ml of M NaBr is added to 2. 0 ml of M Pb( NO3) 2? (4 marks) OVER

26 6. Write the equation for the predominant reaction between HSO 4 and H PO 2 4. (2 marks) 7. A M solution of a weak acid, HA, has a ph = Use calculations and the table of Relative Strengths of Brønsted-Lowry Acids and Bases from the Data Booklet to determine the identity of the acid. (5 marks) The acid is:

27 8. Calculate the ph of a solution prepared by mixing ml of M HCl with ml of 1. 0 M NaOH. (4 marks) 9. Identify a gas which causes acid rain, and write an equation showing this gas reacting with water. (2 marks) OVER

28 10. Balance the following redox reaction in acidic solution. (3 marks) ( ) MnO Fe Mn Fe acidic 11. Aluminum is a stronger reducing agent than copper. What is meant by the term stronger reducing agent? (2 marks)

29 12. Consider the electrolysis of water. a) Draw and label the parts of an electrolytic cell capable of decomposing water. (3 marks) b) Identify the gas produced at the anode. (1 mark) END OF EXAMINATION

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

31 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.

32 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

33 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

34 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

35 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

36 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

37 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

38 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

39 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