PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS

Transcription

1 INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE JANUARY 2000 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 ENDÊOFÊEXAMINATION. 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: 12 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 Br nsted-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 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. 5. 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. 6. This examination is designed to be completed in two hours. Students may, however, take up toê30 minutes of additional time to finish.

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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. Which of the following is most likely to have the greatest reaction rate at room temperature? A. 2 H + O 2 H O l 2( g) 2( g) 2 ( ) + 2 B. 2Ag ( aq) + CrO4 ( aq) Ag2CrO4( s) C. Pb( s) + 2HCl( aq) PbCl2( aq) + H2( g) D. CH4( g) + 2O2( g) CO2( g) + 2H2O( g) 2. Consider the following reaction involving 1. 0g of powdered zinc: Zn( s) + 2HCl( aq) ZnCl2( aq) + H2( g) Trial Temperature C ( ) Concentration of HCl The rates, in order of fastest to slowest, are A. 1, 2, 3 B. 2, 1, 3 C. 3, 1, 2 D. 3, 2, 1 3. Activation energy can be described as the A. energy of motion. B. energy of the activated complex. C. energy difference between the reactants and the products. D. energy difference between the reactants and the activated complex OVER

6 4. Consider the following potential energy diagram for a reversible reaction: 150 PE (kj) Progress of the reaction Which of the following describes the system above? Reaction Activation Energy ( kj) H ( kj) A. reverse B. reverse C. forward D. forward Increasing the temperature of a reaction increases the reaction rate by I. increasing frequency of collisions II. III. increasing the kinetic energy of collision decreasing the potential energy of collision A. I only. B. I and II only. C. II and III only. D. I, II and III

7 6. What effect does a catalyst have on a reaction? A. It changes the H of a reaction. B. It increases the kinetic energy of the reactants. C. It decreases the potential energy of the products. D. It provides a reaction mechanism with a lower activation energy. 7. Consider the following equilibrium: N2( g) + 2O 2( g) 2NO2( g) Equal moles of N 2 and O 2 are added, under certain conditions, to a closed container. Which of the following describes the changes in the reverse reaction which occur as the system proceeds toward equilibrium? Rate of Reverse Reaction [ NO 2 ] A. increases increases B. decreases increases C. increases decreases D. decreases decreases 8. A chemical equilibrium is described as ÒdynamicÓ because A. maximum randomness has been achieved. B. the pressure and temperature do not change. C. both reactants and products continue to form. D. the concentrations of chemical species remain constant. 9. Which of the following reactions results in an entropy increase? A. 2C( s) + O2( g) 2CO( g) B. N + 2H N H l 2( g) 2( g) 2 4( ) C. 2SO2( g) + O2( g) 2SO3 ( g) + aq aq ( s) D. Ag ( ) + Cl ( ) AgCl OVER

8 10. Consider the following equilibrium: CH3COOH( aq) + H O 2 ( l) CH3COO ( aq) + H3O ( aq) + heat A stress was applied at time t 1 and the data was plotted on the following graph: + [ H 3 O + ] t 1 Time The stress that was imposed at time t 1 is the result of A. the addition of HCl. B. decreasing the temperature. C. the addition of NaCH3 COO. D. increasing the volume of the container. 11. Consider the following potential energy diagram for an equilibrium system: P.E. Progress of the reaction When the temperature of the system is increased, the equilibrium shifts to the A. left and the K eq increases. B. left and the K eq decreases. C. right and the K eq increases. D. right and the K eq decreases

9 12. What is the K eq expression for the following equilibrium? 3Fe( s) + 4H2O ( g) Fe3O4( s) + 4H2( g) eq = 4 [ 2] [ H ] eq = 2 [ HO 2 ] [ H ] 4 eq = 2 [ HO 2 ] A. K H B. K C. K [ Fe O ][ H ] D. K eq = Fe H O 4 [ ] [ 2 ] Consider the following equilibrium: 2O3 ( g) 3O2( g) Keq = 65 Initially, 010. mole of O3 and 010. mole of O2 are placed in a 10. L container. Which of the following describes the changes in concentrations as the reaction proceeds toward equilibrium? [ O 3 ] [ O 2 ] A. decreases decreases B. decreases increases C. increases decreases D. increases increases 14. Which of the following does not define solubility? A. the concentration of solute in a saturated solution B. the moles of solute dissolved in a given volume of solution C. the maximum mass of solute that can dissolve in a given volume of solution D. the minimum moles of solute needed to produce one litre of a saturated solution OVER

10 15. The ion concentrations in 0. 25M Al2( SO4) 3 are [ Al 3+ 2 ] [ SO 4 ] A M 025. M B M 075. M C M 050. M D M 015. M 16. Which of the following will not produce a precipitate when equal volumes of 0. 20Msolutions are combined? A. KOH and CaCl 2 B. Zn( NO3) 2 and K3PO4 C. Sr( OH) 2 and ( NH4) 2S D. Na2SO4 and Pb( NO3) What is observed when H SO 2 4 is added to a saturated solution of CaSO 4? A. the ph increases B. the [ Ca 2+ ] increases C. bubbles of H 2 are given off D. additional CaSO 4 precipitates 18. The solubility of CdS = The value of K sp is A B C D

11 19. How many moles of solute are dissolved in ml of a saturated solution of FeS? A B C D Consider the following ml solutions: AgNO M M M Cl Br IO M BrO 3 Equal moles of AgNO 3 are added to each solution. It is observed that a precipitate forms in all but one solution. Which solution does not form a precipitate? A. Cl B. Br C. IO 3 D. BrO Which of the following could dissolve a precipitate of CaC O a saturated solution ofêcac 2 O 4? A. NaOH B. CaC 2 O 4 C. HCO D. Ca( NO 3 ) in OVER

12 22. Which of the following is a general property of bases? A. taste sour B. turn litmus red C. conduct electric current in solution D. concentration of H 3 O is greater than concentration of OH 23. Water will act as an acid with which of the following? I. HCO 2 3 II. III. HCO 3 CO 3 2 A. I only. B. III only. C. I and II only. D. II and III only. 24. Which of the following 1. 0M solutions will have the greatest electrical conductivity? A. HI B. HS 2 C. HCN D. HPO An acid is added to water and a new equilibrium is established. The new equilibrium can be described by A. ph < poh and Kw = B. ph < poh and Kw < C. ph > poh and Kw = D. ph > poh and Kw >

13 26. Consider the following equilibrium: 2 2 l 3 H O( ) + energy H O ( aq) + OH ( aq) + The [ HO 3 ] will decrease and the K w will remain constant when A. a strong acid is added. B. a strong base is added. C. the temperature is increased. D. the temperature is decreased Which of the following graphs describes the relationship between [ HO 3 ] and ph? A. B. [ H 3 O + ] [ H 3 O + ] ph ph C. D. [ H 3 O + ] [ H 3 O + ] ph ph When the [ HO 3 ] in a solution is increased to twice the original concentration, the change in ph could be from A. 17. to 14. B. 20. to 40. C. 50. to 25. D. 85. to OVER

14 29. The relationship HPO [ ][ HO 3 ] HPO [ ] is the A. Ka for H3P2O 7 B. Kb for H3P2O 7 C. Ka for H2P2O 7 2 D. Kb for H2P2O Which of the following describes the relationship between acid strength and K a value for weakêacids? Acid Strength K a A. increases increases B. increases decreases C. decreases increases D. decreases remains constant 31. The value of K for HPO b 42 is A B C D Which of the following 1. 0M solutions would have a ph greater than 700.? A. HCN B. KNO 3 C. NH4Cl D. NaCH3COO

15 33. What is the ph at the transition point for an indicator with a Ka of A B C D ? 34. What volume of M NaOH is required to completely neutralize ml of M H3PO 4? A ml B ml C ml D ml 35. What is the ph of the solution formed when moles NaOH is addedêtoê1. 00 L of M HCl? A B C D OVER

16 36. Which of the following graphs describes the relationship between the ph of a buffer and the volume of NaOH added to the buffer? A. B. ph ph Volume of NaOH added Volume of NaOH added C. D. ph ph Volume of NaOH added Volume of NaOH added 37. A gas which is produced by internal combustion engines and contributes to the formation of acid rain is A. H 2 B. O 3 C. CH 4 D. NO Which of the following represents a redox reaction? A. CaCO3 CaO + CO2 B. SiCl4 + 2Mg Si + 2MgCl2 C. 2NaOH + H2SO4 2H2O + Na2SO4 D. AgBr + S O Ag( S O ) + Br

17 39. Consider the following reaction: Each oxygen atom is A. reduced and loses 2e B. reduced and gains 2e C. oxidized and loses 2e D. oxidized and gains 2e TiCl + O TiO + 2Cl When NO 2 acts as a reducing agent, a possible product is A. NO B. NO 2 C. NO 2 4 D. NO Which of the following 1. 0M solutions will react spontaneously with lead? A. KCl B. CuCl 2 C. ZnCl 2 D. MgCl Consider the following redox reaction: I + 2S O S O + 2I In a titration, ml of Na2S2O 3 is needed to react completely with mol I 2. What is the concentration of Na2S2O3? A M B M C M D M OVER

18 43. In an operating electrochemical cell the function of a salt bridge is to A. allow hydrolysis to occur. B. allow a non-spontaneous reaction to occur. C. permit the migration of ions within the cell. D. transfer electrons from the cathode to the anode. Use the following diagram to answer questions 44 and 45. Volts Cd anode 1.0 M KNO3 Pb cathode 1.0 M Cd M Pb 2+ E cell = 0.27 V 44. As the cell operates, electrons flow toward A. the Pb electrode, where Pb is oxidized. B. the Cd electrode, where Cd is oxidized. C. the Pb electrode, where Pb 2+ is reduced. D. the Cd electrode, where Cd 2+ is reduced. 45. The E value for the reduction of Cd 2+ is A V B V C V D V

19 46. The following reaction occurs in an electrochemical cell: The E for the cell is A V B V C V D V Cu + 2Cr 2Cr + 3Cu 47. During the corrosion of magnesium, the anode reaction is 2+ A. Mg Mg + 2e 2+ B. Mg + 2e Mg C. 4OH O + 2H O + 4e 2 2 D. O + 2H O + 4e 4OH A molten binary salt, ZnCl 2, undergoes electrolysis. The cathode reaction is 2+ A. Zn Zn + 2e B. 2Cl Cl + 2e C. Cl2 + 2e 2Cl 2+ D. Zn + 2e Zn 2 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. A student wishes to monitor the rate of the following reaction: CaCO3( s) + 2HCl( aq) CaCl2( aq) + CO2( g) + H2O( l) Identify two different properties that could be used to monitor the rate of the reaction. Describe and explain the changes that would occur. (2Êmarks) Property 1: Change and Explanation: Property 2: Change and Explanation:

21 2. Consider the following reaction for the formation of HCl in the presence of light. Cl2 + CHCl3 HCl + CCl4 The following is the proposed reaction mechanism: Step 1 ÊÊÊÊÊÊÊÊÊÊÊ ÊÊÊ Cl2 Cl + Cl Step 2? Step 3 Cl + CCl 3 CCl 4 Determine Step 2 of the reaction mechanism. (2Êmarks) 3. Consider the following equilibrium: + HInd + H O 2 H3O + Ind ( yellow) ( blue) The system is yellow and turns blue on the addition of NaOH. In terms of the forward and reverse reaction rates, explain why this shift occurs. (2Êmarks) OVER

22 4. Consider the following equilibrium: aq aq aq Fe ( ) + SCN ( ) FeSCN ( ) 3 Initially, ml of M Fe + is added to ml of M SCN. At equilibrium, the concentration of FeSCN 2+ is found to be M. Calculate the K eq for the reaction. (4Êmarks) 5. a) Write the balanced formula equation for the reaction between Na3PO4( aq) and CuCl2( aq). (1Êmark) b) Write the net ionic equation for the reaction between Na3PO4( aq) and CuCl2( aq). (1Êmark)

23 6. A saturated solution of nickel carbonate, NiCO 3, contains g in 2. 0 L of solution. Calculate K sp for NiCO 3. (3Êmarks) 7. Define the term amphiprotic. Give an example of an ion which is amphiprotic. (2Êmarks) Definition: Example: OVER

24 8. A M solution of methylamine, CH NH Calculate the K b for methylamine. 3 2, has a ph = (4Êmarks) 9. A titration was performed by adding M NaOH to a ml sample of H2SO 4. Calculate the HSO 2 4 [ ] from the following data. (3Êmarks) Trial #1 Trial #2 Trial #3 Initial volume of NaOH ( ml) Final volume of NaOH ( ml)

25 10. a) Indicate in the blank spaces on the following chart whether or not a reaction will occur when the metals are added to aqueous ions. (1Êmark) ion metal Pd Rh Pt Pd 2+ Rh 2+ no reaction no reaction Pt 2+ reaction reaction b) List the oxidizing agents in order of strongest to weakest. (1Êmark) OVER

26 11. Balance the following redox reaction in basicêsolution: (4Êmarks) ( ) Au + Cl + O2 AuCl4 + OH basic

27 12. Draw and label a simple electrolytic cell capable of electroplating an inert electrode with silver. (2Êmarks) END OF EXAMINATION

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29 Question 1: Question 7: 1.. (2) 7.. (2) INSERT STUDENT I.D. NUMBER (PEN) Question 2: Question 8: STICKER IN THIS SPACE 2.. (2) 8.. (4) batch and sequence number Question 3: Question 9: 3.. (2) Question 4: 4.. (4) Question 5: 5.. (2) 9.. (3) Question 10: 10.. (2) Question 11: 11.. (4) CHEMISTRY 12 January 2000 Course Code = CH Use this space if I.D. sticker is not available. WRITE STUDENT I.D. NUMBER (PEN) Question 6: Question 9: IN THIS SPACE 6.. (3) 12.. (2)

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