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

3 CHEMISTRY 12 JUNE 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.

6 THIS PAGE INTENTIONALLY BLANK

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 has the lowest rate of reaction? (1 mark) A. Pb( s) + CuCl2( aq) Cu( s) + PbCl2( aq) B. HCl + NaOH H O + NaCl ( aq) ( aq) 2 ( l) ( aq) C. H SO + Ba( OH) 2H O + BaSO 2 4( aq) 2( aq) 2 ( l) 4( s) ( ) + + D. Pb NO 2NaI PbI 2NaNO 3 2( aq) ( aq) 2( s) 3( aq) 2. Which of the following affects the rate of heterogeneous reactions, but does not affect the rate of homogeneous reactions? (1 mark) A. catalyst B. temperature C. surface area D. concentration 3. As reactant particles approach each other, what changes occur in KE and PE? (1 mark) KE PE A. increases increases B. increases decreases C. decreases increases D. decreases decreases OVER

8 4. Consider the following PE diagram: (1 mark) 500 PE (kj) Progress of the reaction What is the minimum potential energy required to change reactants to the activated complex? A. 200 kj B. 300 kj C. 400 kj D. 500 kj 5. Consider the following reaction mechanism: (1 mark) Step 1 2NO2 NO3 + NO Step 2 NO3 + CO NO2 + CO2 Identify a product in the overall reaction. A. CO B. CO 2 C. NO 2 D. NO 3-2 -

9 6. Consider the following PE diagram for a catalyzed and uncatalyzed reaction: (2 marks) PE (kj) Progress of the reaction Which of the following describes the reverse reaction? Reverse Reaction Activation Energy kj ( ) H kj ( ) A. uncatalyzed B. catalyzed C. uncatalyzed D. catalyzed Consider the following: (1 mark) ( ) ( ) + ( ) 2HBr g H2 g Br2 g Initially, HBr is added to an empty flask. How do the rate of the forward reaction and the HBr [ ] change as the system proceeds to equilibrium? Forward Rate [ HBr] A. decreases decreases B. decreases increases C. increases increases D. increases decreases OVER

10 Use the following equilibrium equation to answer questions 8 and 9. 2SO2( g) + O 2( g) 2SO3 ( g) + energy 8. Which of the following two stresses will each cause the system to shift to the right? (1 mark) [ ] [ ] [ ] [ ] A. decrease temperature, decrease O 2 B. increase temperature, increase SO 3 C. increase temperature, decrease SO 3 D. decrease temperature, increase SO 2 9. Which of the following graphs shows the reverse rate of reaction when a catalyst is added to the equilibrium 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 - 4 -

11 10. Consider the following: (2 marks) 2N2( g) + O2( g) + energy? 2N2O( g) What positions do minimum enthalpy and maximum entropy tend toward? Minimum Enthalpy Maximum Entropy A. products products B. products reactants C. reactants products D. reactants reactants 11. Consider the following: (1 mark) H2( g) + I 2( g) 2HI( g) Initially, some HI is placed into a 1. 0 L container. At equilibrium there is mol H 2, mol I 2 and mol HI present. How many moles of HI were initially added to the container? A mol B mol C mol D mol OVER

12 12. What is the equilibrium expression for the following system? (1 mark) 4Fe( s) + 3O 2( g) 2Fe2O3( s) A. K O eq = [ 2] 3 B. Keq = 1 [ O2] [ Fe O ] C. K eq = Fe O D. K 3 2 [ ] [ 2] [ Fe O eq = 2 ] 2 3 [ 4Fe][ 3O2] What will cause the value of K eq for an endothermic reaction to increase? (1 mark) [ ] [ ] A. increasing products B. decreasing products C. increasing the temperature D. decreasing the temperature 14. Consider the following equilibrium: (2 marks) NO ( g) 2NO ( g) An equilibrium mixture contains mol N2O 4 and mol NO2 in a 1. 0 L flask. What is the value of K eq? A B C D

13 15. In every solubility equilibrium, the rate of dissolving is (1 mark) A. equal to zero. B. equal to the rate of crystallization. C. less than the rate of crystallization. D. greater than the rate of crystallization. 16. A 3. 0 L solution of BaCl 2 has a chloride ion concentration of M. The barium ion concentration in this solution is (1 mark) A M B M C M D M 17. Which of the following has the lowest solubility? (2 marks) A. CaS B. CuS C. FeS D. MgS 18. What is the formula equation for the reaction that occurs when equal volumes of M K3PO 4 and M ZnCl 2 are mixed together? (1 mark) + aq aq ( s) A. K ( ) + Cl ( ) KCl 2+ 3 aq aq 3 4 2( s) B. 3Zn ( ) 2PO4 ( ) Zn PO + ( ) C. 2K PO + 3ZnCl Zn ( PO ) + 6KCl 3 4( aq) 2( aq) 3 4 2( s) ( aq) D. 2K PO + 3ZnCl 3Zn ( PO ) + 6KCl 3 4( aq) 2( aq) 3 4 2( aq) ( s) OVER

14 19. Which of the following could be added to a sample of hard water to remove 2 both 0. 2 M Ca + 2 and 0. 2 M Mg +? (1 mark) A M S B M Cl C M OH 2 D M SO The K sp expression for a saturated solution of Ag2SO3 is (1 mark) sp = + 2 [ 2 ][ 3 ] sp = [ ] [ 3 ] sp = 2+ 2 [ 2 ][ 3 ] sp = [ 2 ] [ 3 ] A. K Ag SO B. K Ag SO C. K Ag SO D. K Ag SO 21. The solubility of CaF 2 is M. Determine the K sp value of CaF 2. (2 marks) A B C D What is the maximum [ Ag + ] that can exist in a solution of M NaIO 3? (1 mark) A B C D M M M M - 8 -

15 23. An Arrhenius base is defined as a substance that (1 mark) A. releases H ( aq) B. releases OH ( aq) C. accepts a proton D. donates a proton The conjugate acid of HAsO 4 2 is (1 mark) A. AsO 4 3 B. AsO 4 2 C. H2AsO4 2 D. H2AsO4 25. Which of the following will have the greatest electrical conductivity? (1 mark) A M HF B M HBr C M HCN D M H2SO3-9 - OVER

16 26. Consider the equilibrium: (2 marks) C H COOH + NO HNO + C H COO Identify the stronger acid and predict whether reactants or products are favoured. Stronger Acid Side Favoured A. HNO 2 reactants B. HNO 2 products C. C H COOH 6 5 reactants D. C H COOH 6 5 products 27. Which of the following represents the equilibrium expression for the ionization of water? w = + [ 3 ][ ] A. K H O OH (1 mark) B. K w = [ 1 HO + ][ OH ] 3 w = + [ 3 ] + [ ] C. K H O OH [ + HO ][ OH ] D. Kw = 3 HO [ 2 ] 28. Determine the ph of 3. 0 M KOH. (2 marks) A B C D

17 29. Four acids are analyzed and their K a values are determined. Which of the following values represents the strongest acid? (1 mark) A. K a = B. K a = C. K a = D. K a = The dissociation of NH4NO3 is represented by (1 mark) A. NH4NO3( s) NH4 ( aq) + NO3 ( aq) + B. NH4 ( aq) + NO3 ( aq) NH4NO3( s) + + C. NH4 ( aq) + H2O( l) H3O ( aq) + NH3 ( aq) D. NO3 ( aq) + H2O( l) HNO3 ( aq) + OH ( aq) A solution of Al( NO 3 ) 3 will be (1 mark) A. basic. B. acidic. C. neutral. D. amphiprotic OVER

18 32. Consider the following equilibrium for the chemical indicator phenol red, HInd, at a ph 73. orange. (2 marks) = ( ) + HInd + H O 2 H3O + Ind yellow red When some NaOH is added, what stress is imposed on the equilibrium and what colour change occurs? Stress Indicator Colour Change + A. increased [ H 3 O ] turns red + B. decreased [ H 3 O ] turns red + C. increased [ H 3 O ] turns yellow + D. decreased [ H 3 O ] turns yellow 33. A chemical indicator has a K a = Determine the ph at the transition point. (1 mark) A B C D

19 34. Consider the following titration curve: ph mol of added base Select a suitable indicator for this titration. (1 mark) A. orange IV B. methyl red C. thymolphthalein D. indigo carmine 35. Calculate the volume of M HNO 3 needed to completely neutralize ml of M Sr OH 2 A ml B ml C ml D ml ( ). (2 marks) 36. Equal moles of which of the following chemicals could be used to make a basic buffer solution? (1 mark) A. HF and NaOH B. HCl and NaCl C. KBr and NaNO 3 D. NH 3 and NH4Cl OVER

20 37. Which reaction occurs when calcium oxide is added to water? (1 mark) A. 2CaO( s) Ca2O2( aq) B. 2CaO( s) 2Ca( aq) + O2( aq) C. CaO( s) H2O( l) Ca OH 2( aq) D. CaO( s) + H2O( l) CaOH( aq) + O2( aq) + ( ) 38. Which of the following is the strongest reducing agent? (1 mark) A. H 2 S B. H 2 O C. H2Se D. H2Te 39. Consider the following unbalanced half-reaction: (2 marks) H SeO 2 3 Se The oxidation number of Se A. increases as it undergoes oxidation. B. increases as it undergoes reduction. C. decreases as it undergoes oxidation. D. decreases as it undergoes reduction

21 40. Which of the following will react spontaneously with Br 2 but not with I 2? (1 mark) A. F B. Cr 2+ C. Fe 2+ D. Mn Consider the following: (1 mark) What is true for this reaction? Sn + 2Cl Sn + Cl A. E =+151. V and it is spontaneous. cell B. E =+121. V and it is spontaneous. cell C. E =121. V and it is non-spontaneous. cell D. E =151. V and it is non-spontaneous. cell What is the function of the salt bridge in an electrochemical cell? (1 mark) A. It provides a path for electrons. B. It maintains electrical neutrality in each half cell. C. It allows the anode to become positively charged. D. It allows the cathode to become negatively charged OVER

22 Use the following diagram to answer questions 43, 44 and 45. Volts Sn 1.0 M KNO3 Ag 1.0 M Sn M Ag In the above electrochemical cell, how do the mass of the anode and the [ Ag + ] change as the cell operates? (2 marks) Mass of the Anode [ Ag + ] A. decreases increases B. increases increases C. decreases decreases D. no change decreases 44. What is the overall cell reaction? (1 mark) A. 2Ag + Sn Sn + 2Ag B. 2Ag + Sn Sn + 2Ag + 2+ C. 2Ag + Sn Sn + 2Ag + 2+ D. 2Ag + Sn Sn + 2Ag 45. What is the value of E for the cell? (1 mark) A V B V C V D V

23 46. Consider the following equation: (1 mark) 2+ What is E for the reduction of Cd 2+? A V B V C V D V Cd + 2I Cd + I E =0 94V 2 cell. 47. Which of the following describes an operating electrochemical cell? (2 marks) E Type of Reaction Direction of Electron Flow A. positive spontaneous anode to cathode B. negative spontaneous cathode to anode C. positive non-spontaneous anode to cathode D. negative non-spontaneous cathode to anode OVER

24 48. A copper spoon is plated with silver in an electrolytic cell. + DC Power Source Ag (s) 1.0 M Ag + What is the reaction at the anode? (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

25 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) 2Al( s) + 6HCl( aq) 2AlCl3 ( aq) + 3H2( g) A g sample of Al reacts completely in excess HCl in s. What is the rate of production of H 2 in mol s? OVER

26 2. Using collision theory, give two reasons why reactions occur more rapidly at a higher temperature. (2 marks) i) ii) 3. Chemical reactions tend toward a position of minimum enthalpy and maximum entropy. a) What is meant by the term enthalpy? (1 mark) b) What is meant by the term entropy? (1 mark)

27 4. Consider the following: (4 marks) H2( g) + Br 2( g) 2HBr( g) Keq = Initially, mol H 2 and mol Br 2 are placed into a L container. What is the HBr [ ] at equilibrium? OVER

28 5. Consider the following equilibrium and accompanying graph: 2 ( ) + s aq + 3 aq Zn IO3 2( ) Zn ( ) 2IO ( ) [ Ions] [ IO 3 ] [ Zn 2+ ] t 1 t 2 t 3 a) Identify the stress applied at t 1. (1 mark) b) Complete the above graph from t 1 to t 3 for the [ IO 3 ]. (2 marks) 6. Calculate the solubility of SrSO 4 in grams per litre. (3 marks)

29 7. The cyanide ion, CN, is a Brønsted-Lowry base. a) Define Brønsted-Lowry base. (1 mark) b) Write the equation representing the reaction of CN with water. (2 marks) c) Identify a conjugate pair in b) above. (1 mark) 8. Write an equation to show the ionization of water. (2 marks) OVER

30 9. Calculate the ph of M NH 3. (5 marks)

31 10. Consider the following buffer equilibrium: (3 marks) + HF( aq) + H O 2 ( l) H3O ( aq) + F ( aq) high concentration low concentration high concentration Using Le Châtelier s Principle, explain what happens to the ph of the buffer solution when a small amount of NaOH is added. 11. Balance the following redox equation: (4 marks) + Ag + NO3 Ag + NO (acidic) OVER

32 12. Draw a diagram of an operating electrolytic cell used to extract pure lead from an impure lead sample. Identify the electrolyte and the material used for the anode. (3 marks)

33 13. A sample of copper is placed in HNO 3( aq) and another sample of copper is placed in HCl ( aq). 1 a) In which acid does the copper react? ( 2 mark) b) Calculate E for the reaction that occurs. ( marks ) END OF EXAMINATION

34 THIS PAGE INTENTIONALLY BLANK

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

36 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.

37 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

38 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

39 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

40 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

41 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

42 RELATIVE STRENGTHS OF BRØNSTED-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 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

43 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

44 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 + 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