PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS

Transcription

1 INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE APRIL 1999 PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS 1. Insert the stickers with your Student I.D. Number (PEN) in the allotted spaces above and on the back cover of this booklet. Under no circumstance is your name or identification, other than your Student I.D. 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. 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. 5. For each of the written-response questions, write your answer in the space provided in this booklet. 6. 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. 7. 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 Ministry of Education

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3 CHEMISTRY 12 PROVINCIAL EXAMINATION 1. This examination consists of two parts: Value Suggested Time PART A: 48 multiple-choice questions PART B: 11 written-response questions Total: 80 marks 120 minutes 2. Aside from an approved calculator, electronic devices, including dictionaries and pagers, are not permitted in the examination room. 3. 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 Brönsted-Lowry Acids and Bases Acid-Base Indicators Standard Reduction Potentials of Half-cells No other reference materials or tables are allowed. 4. 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 support devices such as manuals, printed or electronic cards, printers, memory expansion chips, or external keyboards. Students may have more than one calculator available during the examination, but calculators may not be shared. Communication between calculators is prohibited and calculators 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. 5. The time allotted for this examination is two hours.

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5 PART A: MULTIPLE CHOICE Value: 48 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. 1. The slowest of the following reactions is + A. Ag ( aq) + B. H 3 O ( aq) 2+ C. 3Ba ( aq) + Cl ( aq) AgCl ( s) + OH ( aq) 2H 2 O () l 3 + 2PO 4 ( aq) Ba 3 ( PO 4 ) 2( s) D. Cu ( s) + 2Ag ( aq) Cu + 2+ ( aq) + 2Ag ( s) 2. The rate of a chemical reaction is equal to the slope of a graph with the axes labelled x-axis y-axis A. time rate B. mass time C. volume of gas time D. time concentration OVER

6 3. Consider the following reaction: CH 4( g) + 2O 2( g) CO 2( g) + 2H 2 O ( g) + heat The diagram which represents the relationship between rate and temperature is: A. B. Rate Rate Temperature Temperature C. D. Rate Rate Temperature Temperature 4. Which of the following describes the energy of colliding particles as reacting molecules approach each other? KE PE A. decreases increases B. increases decreases C. decreases remains constant D. remains constant increases 5. The average kinetic energy of colliding particles can be increased by A. adding a catalyst. B. increasing pressure. C. increasing temperature. D. increasing reactant concentration

7 6. A substance that increases the rate of a chemical reaction and may be recovered unchanged at the end of the reaction is a(n) A. product. B. catalyst. C. activated complex. D. reaction intermediate. 7. Consider the following PE diagram for a reversible reaction: PE (kj) Progress of the reaction Which of the following describes this reaction? DIRECTION ACTIVATION ENERGY (kj) H kj ( ) A. reverse B. forward C. forward D. reverse OVER

8 8. Consider the following equilibrium: 2NO ( g) + Br 2( g) + energy 2NOBr ( g) The equilibrium will shift to the left as a result of A. adding a catalyst. B. removing NOBr. C. increasing the volume. D. increasing the temperature. 9. Consider the following equilibrium: N 2( g) + O 2( g) + energy 2NO ( g) When the temperature is increased, the equilibrium shifts to the A. left and K eq increases. B. left and K eq decreases. C. right and K eq increases. D. right and K eq decreases. 10. Consider the following equilibrium: 2CO ( g) + O 2( g) 2CO 2( g) + energy Some CO 2 is added to the equilibrium system at constant volume and a new equilibrium is established. Compared to the original equilibrium, the rates of the forward and reverse reactions for the new equilibrium have FORWARD RATE REVERSE RATE A. increased increased B. not changed increased C. decreased increased D. not changed not changed - 4 -

9 11. An indication that an equilibrium system favours the products is a A. large K eq. B. positive H. C. one step mechanism. D. low activation energy. 12. The relationship between K eq and the pressure of a gaseous equilibrium at constant temperature can be described by A. B. K eq K eq Pressure Pressure C. D. K eq K eq Pressure Pressure 13. Consider the following equilibrium: 2NO 2( g) N 2 O 4( g) A 1.00 L flask contains mol NO 2 and mol N 2 O 4 at equilibrium. The value of K eq is A B C. 1.3 D OVER

10 14. Which of the following produces a molecular solution when dissolved in water? A. RbClO B. CH 3 OH C. NH 4 SCN D. NaCH 3 COO 15. Consider the solubility equilibrium: 2+ CaCO 3( s) Ca ( aq) 2 + CO 3 ( aq) An additional piece of solid CaCO 3 is added to the equilibrium above. The rate of dissolving and rate of crystallization have RATE OF DISSOLVING RATE OF CRYSTALLIZATION A. increased increased B. increased not changed C. not changed increased D. not changed not changed 16. At 25 C, which of the following compounds would dissolve to form a saturated solution with the greatest Pb 2+ [ ]? A. PbI 2 B. PbCl 2 C. PbBr 2 ( ) 2 D. Pb IO When equal volumes of 0.20 M ZnSO 4 and 0.20 M Sr( OH) 2 are combined, A. no precipitate forms. B. a precipitate of only SrSO 4 forms. C. a precipitate of only Zn( OH) 2 forms. D. precipitates of both SrSO 4 and Zn( OH) 2 form

11 18. The solubility of SnS is M. The value of K sp is A B C D Silver chloride, AgCl, would be least soluble in A. 1.0 M HCl B. 1.0 M NaNO 3 C. 1.0 M ZnCl 2 D. 1.0 M AgNO The solubility of SrF 2 is A M B M C M D M 21. Which of the following is a property of sodium hydroxide? A. feels slippery B. releases H 3 O + in aqueous solution C. changes litmus paper from blue to red D. reacts with magnesium to produce hydrogen gas OVER

12 22. The conjugate acid of HAsO 2 4 is A. H 3 O + B. 3 AsO 4 C. H 3 AsO 4 D. H 2 AsO Which of the following 0.10 M solutions has the highest electrical conductivity? A. HF B. HCN C. H 2 CO 3 D. H 3 BO Consider the following acid-base equilibrium: H 2 C 6 H 5 O 7 + HPO 4 2 HC 6 H 5 O H 2 PO 4 In the equilibrium above, A. products are favoured because H 2 PO 4 is the weaker acid. B. reactants are favoured because HPO 2 4 is the weaker acid. C. products are favoured because HC 6 H 5 O 2 7 is the weaker acid. D. reactants are favoured because H 2 C 6 H 5 O 7 is the weaker acid. 25. Which of the following describes the relationship between [ H 3 O + ] and [ OH ]? A. [ H 3 O + ][ OH ]= B. [ H 3 O + ]+ [ OH ]= C. [ H 3 O + ][ OH ]= D. [ H 3 O + ]+ [ OH ]=

13 26. Consider the following equilibrium: 2H 2 O + energy H 3 O + + OH When water has a ph of 7.5, the temperature is A. less than 25 C and the solution is basic. B. less than 25 C and the solution is neutral. C. greater than 25 C and the solution is basic. D. greater than 25 C and the solution is neutral. 27. Calculate the [ H 3 O + ] in a M solution of Sr( OH) 2. A M B M C M D M 28. The value of K b for HCO 3 is A B C D The net ionic equation for the hydrolysis of NH 4 ClO 4 is A. NH 4 ClO 4( s) NH 4 ( aq) + + ClO 4 ( aq) + B. NH 4 ( aq) + H 2 O + () l NH 3( aq) + H 3 O ( aq) C. ClO 4 ( aq) + H 2 O () l HClO 4( aq) + OH ( aq) + D. NH 4 ( aq) + ClO 4 ( aq) NH 3( aq) + HClO 4( aq) OVER

14 30. A sample of an unknown solution is tested with the indicator chlorophenol red. The solution turns yellow on the addition of this indicator. The solution could be A M KF B. 1.0 M NaCl C M Li 2 SO 4 D M NH 4 NO Which of the following indicators has a transition point closest to the equivalence point for the titration of a weak acid by a strong base? A. orange IV B. thymol blue C. methyl orange D. bromcresol green 32. A buffer solution is formed by adding which of the following to water? A. HCl and KOH B. HCN and RbCN C. NaBr and NaOH D. HNO 3 and LiNO A solution of known concentration is the definition of a A. buffer solution. B. neutral solution. C. standard solution. D. saturated solution. 34. Which of the following is responsible for the acidic ph of normal rainwater? A. CO 2 B. NO 2 C. SO 2 D. NH

15 35. A solution contains a mixture of methyl orange, phenol red and thymol blue. When this solution is yellow, the ph is A B. 6.0 C. 9.0 D Which of the following represents the reaction between MgO and H 2 O? A. MgO + H 2 O Mg( OH) 2 B. MgO + H 2 O MgH 2 + O 2 C. MgO + H 2 O Mg + H 2 O 2 D. 2MgO + H 2 O 2MgOH O Which of the following represents the formation of a stronger acid as a result of oxidation? A. H 2 SO 3 H 2 S B. HClO 4 HCl C. H 2 SO 3 H 2 SO 4 D. HCO 3 H 2 CO Chlorine has an oxidation number of +5 in A. NaClO B. NaClO 2 C. NaClO 3 D. NaClO OVER

16 39. Consider the following: NO 2 N 2 O 3 The nitrogen atom in each NO 2 A. loses one electron. B. gains one electron. C. loses two electrons. D. gains two electrons. 40. Which of the following is the strongest oxidizing agent? A. BrO 3 B. ClO 4 C. 2 S 2 O 8 D. 2 Cr 2 O Consider the following half-reaction: 1 AsH 3 + H 2 O H 3 AsO 3 +? H + + e When this half-reaction equation is balanced, the coefficient for H + is A. 2 B. 3 C. 6 D When a strip of zinc is placed in a 1.0 M copper( II) chloride solution, A. no change occurs. B. the Cl C. the Cu 2+ D. the Zn 2+ [ ] increases. [ ] increases. [ ] increases

17 43. Consider the following electrochemical cell: Volts H 2(g) 1.0 M KNO3 Copper Platinum 1.0 M HCl 1.0 M Cu(NO 3 ) 2 What changes occur when the cell is in operation? ANODE HALF-CELL CATHODE HALF-CELL A. [ H 3 O + ] increases electrode increases in mass B. [ H 3 O + ] increases electrode decreases in mass C. [ H 3 O + ] decreases electrode increases in mass D. [ H 3 O + ] decreases electrode decreases in mass OVER

18 44. A redox titration is performed in order to determine the [ H 2 O 2 ]. Which of the following would not be a suitable reagent to use? A. acidified IO 3 B. acidified SO 4 2 C. acidified MnO 4 D. acidified Cr 2 O Ethanol, C 2 H 5 OH, is oxidized by an acidified dichromate solution according to the following equation: 2Cr 2 O H + + 3C 2 H 5 OH 4Cr H 2 O + 3CH 3 COOH The E for the reaction above is 2.98 V. The E for the oxidation of ethanol is A V B. 1.23V C V D V 46. Which of the following must be present to produce rust by the corrosion of iron? I. water II. III. oxygen salt A. I only B. II only C. I and II only D. I, II and III

19 47. Why can an object not be plated with magnesium using 1. 0 M MgI 2? A. Water is a stronger reducing agent than I B. Water is a stronger oxidizing agent than I C. Water is a stronger reducing agent than Mg 2+ D. Water is a stronger oxidizing agent than Mg In the electrolysis of 1. 0 M Na 2 SO 4, what is formed at the cathode? A. O 2 B. H 2 C. H 2 SO 3 D. 2 S 2 O 8 This is the end of the multiple-choice section. Answer the remaining questions directly in this examination booklet OVER

20 PART B: WRITTEN RESPONSE Value: 32 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. An experiment is performed by displacement of water to determine the rate of the following reaction: Zn ( s) + 2HCl ( aq) H 2( g) + ZnCl 2( aq) The following data is collected: Time (s) Volume of H 2 (ml) a) Calculate the average rate of formation of H 2 in ml s for the time interval between 20 and 40 seconds. (2 marks) b) How does the rate of this reaction change as the reaction proceeds? Explain why. (2 marks)

21 2. Describe how enthalpy and entropy change, in the forward direction, as an exothermic reaction reaches equilibrium. Explain your reasoning. (2 marks) Enthalpy: Entropy: Explanation: 3. Consider the graph below representing the following equilibrium: CH 3 CH 2 CH 2 CH 3( g) CH 3 CH( CH 3 ) 2( g) n-butane isobutane Data for the graph was obtained from various equilibrium mixtures. 4.0 [ n-butane] ( mol L) [ isobutane] ( mol L) Calculate the value of K eq for the equilibrium. (2 marks) OVER

22 ( ) 2 is diluted by adding 400.0mL of water. Calculate the concentration of ions in the resulting solution. (2 marks) 4. A ml sample of M Ca NO 3 ( ) 2 can be added to 1.5 L of NaBr aq 5. A maximum of 0.60 g Pb NO 3 ( ) without forming a precipitate. Calculate the [ NaBr]. (4 marks)

23 6. Consider the following amphiprotic anions reacting with each other: HC 6 H 5 O HC 2 O 4? a) Complete the Brönsted-Lowry acid-base equilibrium for the predominant reaction. (1 mark) b) Does the equilibrium above favour reactants or products? Explain. (1 mark) OVER

24 7. Calculate the ph of a 1. 5 M H 2 S solution. (4 marks)

25 8. Consider the following reaction: 2HCl ( aq) + Ba( OH) 2( s) BaCl 2( aq) + 2H 2 O ( l) When 3.16 g samples of Ba( OH) 2 were titrated to the equivalence point with an HClsolution, the following data were recorded: Volume of HCl added Trial 1 Trial 2 Trial ml ml 35.51mL Using the data above, calculate the original [ HCl]. (4 marks) OVER

26 9. Balance the following redox reaction in acid: N 2 O 4 + In HNO 2 + In 3+ ( acid) (3 marks)

27 10. What is an electrolytic cell? (2 marks) OVER

28 11. A solution contains either acidified IO 3 or acidified SO 4 2. Why could the solution be identified using I ( aq)? Provide equations to support your answer. (3 marks) END OF EXAMINATION

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30 INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE CHEMISTRY 12 April 1999 Course Code = CH

31 FOR OFFICE USE ONLY CHEMISTRY 12 April 1999 Course Code = CH Score for Question 1: 1. (4) Score for Question 2: 2. (2) Score for Question 3: 3. (2) Score for Question 8: 8. (4) Score for Question 9: 9. (3) Score for Question 10: 10. (2) Score for Question 4: 4. (2) Score for Question 11: 11. (3) Score for Question 5: 5. (4) Score for Question 6: 6. (2) Score for Question 7: 7. (4)

32 Data Booklet CHEMISTRY 12 Work done in this booklet will not be marked. Ministry of Education Revised November 1994

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 Brönsted-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, 74 edition, CRC Press, Boca Raton, 1993.

34 1 PERIODIC TABLE OF THE ELEMENTS 1 H Hydrogen Li Lithium Be Beryllium Na Sodium Magnesium K Mg 20 Ca Potassium Calcium Sc Ti Scandium Titanium V Cr Vanadium Chromium Mn Manganese Iron Co Cobalt Nickel Ni Cu Zn Copper Zinc Rb Sr Rubidium Strontium Y Zr Yttrium Zirconium Nb Niobium Molybdenum Ru Rh Ruthenium Rhodium Pd Ag Palladium Silver Cd Cadmium Cs Ba Cesium Barium La Hf Lanthanum Hafnium Ta W Tantalum Tungsten Re Os Rhenium Osmium Ir Pt Iridium Platinum Au Hg Gold Mercury Fr Ra Francium Radium (223) (226) 89 Ac Actinium (227) 104 Rf Rutherfordium (261) 59 Pr Praseodymium B C N O F Boron Carbon Al Si Aluminum Silicon Nitrogen Oxygen Fluorine S Cl Sulphur Chlorine Ga Ge Gallium Germanium As Se Arsenic Selenium Br Bromine In Sn Indium Tin Sb Te Antimony Tellurium I Iodine Ne Neon Ar Argon Kr Krypton Xe Xenon Rn Radon 58 (222) Ce Cerium Nd Neodymium Sm Samarium Eu Europium Tb Terbium Ho Er Holmium Erbium Tm Yb Thulium Ytterbium Lu Lutetium Th U Thorium Uranium (145) 93 Np Pu Am Neptunium Plutonium Americium (237) (244) (243) Cm Bk Curium Berkelium (247) (247) 100 Fm Einsteinium Fermium (252) (257) 103 Lr Lawrencium (262) Ha Sg Hahnium Seaborgium (262) (263) 107 Uns Unnilseptium (262) 109 Une 1Unnilennium (266) 2 He Helium Si Silicon 28.1 Atomic number Symbol Name Atomic mass 26 Fe Mo Tc Technetium (98) 108 Uno Unniloctium (265) Based on mass of C 12 at Pm Gd Dy Dysprosium Gadolinium Promethium Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally. Pa Protactinium P Phosphorus Tl Thallium Lead Pb Bi Bismuth Polonium (209) 85 Po At Astatine (210) 98 Cf Californium (251) Es Md No Mendelevium Nobelium (258) (259) - 1 -

35 - 2 - ATOMIC MASSES OF THE ELEMENTS Based on mass of C 12 at Values in parentheses are the mass of the most stable or best known isotopes for elements which do not occur naturally. Element Symbol Atomic Number Atomic Mass Element Symbol Atomic Number Atomic Mass Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curium Dysprosium Einsteinium Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Hahnium 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 Dy Es Er Eu Fm F Fr Gd Ga Ge Au Hf Ha He Ho H In I Ir Fe Kr La Lr Pb Li Lu Mg Mn Md (227) 27.0 (243) (210) (247) (251) (247) (252) (257) 19.0 (223) (262) (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)

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

37 SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0.1 mol/ L at 25 ο C. NEGATIVE IONS (Anions) POSITIVE IONS (Cations) SOLUBILITY OF COMPOUNDS All Alkali ions: Soluble Li +, Na +, K +, Rb +, Cs +, Fr + All Hydrogen ion, H + Soluble All Ammonium ion, NH 4 + Soluble Nitrate, NO 3 All Soluble Chloride, Cl or Bromide, Br or 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+ Soluble All others Low Solubility Phosphate, PO 3 4 or Carbonate, CO 2 3 or Sulphite, SO 2 3 Alkali ions, H +, NH 4 + All others Soluble Low Solubility - 4 -

38 SOLUBILITY PRODUCT CONSTANTS AT 25 C Name Formula K sp barium carbonate BaCO barium chromate BaCrO barium sulphate BaSO calcium carbonate CaCO calcium oxalate CaC 2 O calcium sulphate CaSO copper(i) iodide CuI copper(ii) iodate Cu(IO 3 ) copper(ii) sulphide CuS iron(ii) hydroxide Fe(OH) iron(ii) sulphide FeS iron(iii) hydroxide Fe(OH) lead(ii) bromide PbBr lead(ii) chloride PbCl lead(ii) iodate Pb(IO 3 ) lead(ii) iodide PbI lead(ii) sulphate PbSO magnesium carbonate MgCO magnesium hydroxide Mg(OH) silver bromate AgBrO silver bromide AgBr silver carbonate Ag 2 CO silver chloride AgCl silver chromate Ag 2 CrO silver iodate AgIO silver iodide AgI strontium carbonate SrCO strontium fluoride SrF strontium sulphate SrSO zinc sulphide ZnS

39 RELATIVE STRENGTHS OF BRÖNSTED-LOWRY ACIDS AND BASES in aqueous solution at room temperature Strength of Acid Name of Acid Acid Base K a Strength of Base Strong Weak Perchloric HClO 4 H + + ClO 4...very large Hydriodic HI H + + I...very large Hydrobromic HBr H + + Br...very large Hydrochloric HCl H + + Cl...very large Nitric HNO 3 H + + NO 3...very large Sulphuric H 2 SO 4 H + + HSO 4...very large Hydronium Ion H 3 O + H + + H 2 O Iodic HIO 3 H + + IO Oxalic H 2 C 2 O 4 H + + HC 2 O 4 _ ( ) H 2 SO 3 H + + HSO Sulphurous SO 2 + H 2 O Hydrogen sulphate ion HSO 4 H + + SO Phosphoric H 3 PO 4 H + + H 2 PO Hexaaquoiron ion, iron(iii) ion 3+ ( ) 6 H + +Fe( H 2 O) 5 OH Fe H 2 O ( ) Citric H 3 C 6 H 5 O 7 H + + H 2 C 6 H 5 O Nitrous HNO 2 H + + NO Hydrofluoric HF H + + F Methanoic, formic HCOOH H + + HCOO Hexaaquochromium ion, chromium(iii) ion 3 ( ) + 6 H + +Cr( H 2 O) 5 OH Cr H 2 O ( ) Benzoic C 6 H 5 COOH H + + C 6 H 5 COO Hydrogen oxalate ion HC 2 O 4 H + + C 2 O Ethanoic, acetic CH 3 COOH H + + CH 3 COO Dihydrogen citrate ion H 2 C 6 H 5 O 7 H + + HC 6 H 5 O Al( H 2 O) 6 H + +Al( H 2 O) 5 ( OH) ( ) H 2 CO 3 H + + HCO Hexaaquoaluminum ion, aluminum ion Carbonic CO 2 + H 2 O Monohydrogen citrate ion 2 HC 6 H 5 O 7 H + + C 6 H 5 O Hydrogen sulphite ion HSO 3 H + + SO Hydrogen sulphide H 2 S H + + HS Dihydrogen phosphate ion H 2 PO 4 H + + HPO Boric H 3 BO 3 H + + H 2 BO Ammonium ion NH 4+ H + + NH Hydrocyanic HCN H + + CN Phenol C 6 H 5 OH H + + C 6 H 5 O Hydrogen carbonate ion HCO 3 H + + CO Hydrogen peroxide H 2 O 2 H + + HO Monohydrogen phosphate ion 2 HPO 4 H + + PO Water H 2 O H + + OH Hydroxide ion OH H + + O 2... very small Ammonia NH 3 H + + NH 2...very small Weak Strong - 6 -

40 ACID-BASE INDICATORS INDICATOR ph RANGE IN WHICH COLOUR CHANGE OCCURS COLOUR CHANGE AS ph INCREASES 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 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 STRENGTH OF OXIDIZING AGENT strong weak 1 2 Overpotential Effect STANDARD REDUCTION POTENTIALS OF HALF-CELLS Ionic Concentrations are at 1M in Water at 25 C OXIDIZING AGENTS REDUCING AGENTS E (VOLTS) F 2(g) + 2e 2F S 2 O e 2SO H 2 O 2 + 2H + + 2e 2H2 O MnO 4 + 8H + + 5e Mn H 2 O Au e Au (s) BrO 3 + 6H + + 5e 1 Br 2(l) + 3H 2 O ClO 4 + 8H + + 8e Cl + 4H 2 O Cl 2(g) + 2e 2Cl Cr 2 O H + + 6e 2Cr H 2 O O 2(g) + 2H e H 2 O MnO 2(s) + 4H + + 2e Mn H 2 O IO 3 + 6H + + 5e 1 I 2(s) + 3H 2 O Br 2(l) + 2e 2 2Br AuCl 4 + 3e Au (s) + 4Cl NO 3 + 4H + + 3e NO (g) + 2H 2 O Hg e Hg (l) O 2(g) + 2H + (10 7 M)+ 2e H 2 O NO 3 + 4H + + 2e N 2 O 4 + 2H 2 O Ag + + e Ag (s) Hg e Hg (l) Fe 3+ + e Fe O 2(g) + 2H + + 2e H 2 O MnO 4 + 2H2 O+ 3e MnO 2(s) + 4OH I 2(s) + 2e 2I Cu + + e Cu (s) H 2 SO 3 + 4H + + 4e S (s) + 3H 2 O Cu e Cu (s) SO H + + 2e H 2 SO 3 + H 2 O Cu 2+ + e Cu Sn e Sn S (s) + 2H + + 2e H 2 S (g) H + + 2e H 2(g) Pb e Pb (s) Sn e Sn (s) Ni e Ni (s) H 3 PO 4 + 2H + + 2e H 3 PO 3 + H 2 O Co e Co (s) Se (s) + 2H + + 2e H 2 Se Cr 3+ + e Cr H 2 O+ 2e H 2 + 2OH (10 7 M) Fe e Fe (s) Ag 2 S (s) + 2e 2Ag (s) + S Cr e Cr (s) Zn e Zn (s) Te (s) +2H + + 2e H 2 Te H 2 O+ 2e H 2(g) + 2OH Mn e Mn (s) Al e Al (s) Mg e Mg (s) Na + + e Na (s) Ca e Ca (s) Sr e Sr (s) Ba e Ba (s) K + + e K (s) Rb + + e Rb (s) Cs + + e Cs (s) Li + + e Li (s) STRENGTH OF REDUCING AGENT weak Overpotential Effect strong - 8 -