Chemistry 12 JANUARY 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 JANUARY 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 ENDÊOFÊEXAMINATION. 5. At the end of the examination, place your Response Form inside the front cover of this booklet and return the booklet and your Response Form to the supervisor.

2 Question 1: 1.. (5) Question 6: 6.. (2) Question 2: 2.. (5) Question 7: 7.. (6) Question 3: 3.. (2) Question 8: 8.. (4) Question 4: 4.. (2) Question 9: 9.. (5) Question 5: 5.. (5) Question 10: 10.. (4)

3 CHEMISTRY 12 JANUARY 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 HBÊpencil. 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 toê30 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: 10 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 Br nsted-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 units could be used to express reaction rate? (1Êmark) A. ml s B. ml g C. gml D. ml mol 2. Consider the reaction: (1Êmark) Zn( s) + 2HCl( aq) ZnCl2( aq) + H2( g) The rate of production of ZnCl 2, can be increased by A. decreasing the [ HCl]. B. increasing the temperature. C. increasing the volume of H 2. D. decreasing the surface area of Zn. 3. The statement, the minimum energy needed to achieve a successful collision, defines (1Êmark) A. entropy. B. activation energy. C. the H of reaction. D. the activated complex OVER

8 4. As an activated complex changes to products, (1Êmark) A. potential energy changes to kinetic energy. B. kinetic energy changes to potential energy. C. kinetic energy changes to activation energy. D. potential energy changes to activation energy. 5. Consider the following PE diagram for an uncatalysed and a catalyzed reaction: (2Êmarks) 25 kj PE (kj) 10 kj 15 kj Progress of the reaction Which of the following describes the forward catalyzed reaction? Activation Energy (kj) H (kj) A B C D A substance that increases the rate of a reaction without appearing in the equation for the overallêreactionêis a(n) (1Êmark) A. product. B. catalyst. C. reactant. D. intermediate

9 7. All chemical equilibriums have: (1Êmark) I. rates that are continuing to change II. III. an equilibrium constant expression equal concentrations of products and reactants A. II only B. III only C. I and II only D. I and III only 8. From the following, select the situation where both enthalpy and entropy favour the reaction towardêproducts: (1Êmark) Enthalpy Entropy A. increasing increasing B. increasing decreasing C. decreasing decreasing D. decreasing increasing OVER

10 9. Consider the following equilibrium: (1Êmark) 2NO( g) + Br 2( g) 2NOBr( g) + energy The equilibrium will shift to the left as a result of A. adding a catalyst. B. adding some NO ( g). C. increasing the volume. D. decreasing the temperature. 10. Consider the following equilibrium: (2Êmarks) PCl3 ( g) + 3NH 3( g) P( NH2) 3( g) + 3HCl( g) The volume of the equilibrium system is increased and a new equilibrium is established. How have the rates been affected? Rate (forward) Rate (reverse) A. increased decreased B. decreased increased C. decreased decreased D. did not change did not change 11. Starting with equal moles of reactants, which of the following equilibrium systems most favours the reactants? (1Êmark) A. SO2( g) NO2( g) SO3 ( g) NO( g) K = 34. eq B. CO( g) + H O 2 ( g) CO2( g) + H2( g) K eq = C. H2( g) I2( g) 2HI( g) K = 10 eq D. N2( g) O2( g) 2NO( g) K = eq - 4 -

11 12. Consider the following equilibrium reaction: (2Êmarks) NO ( g) 2NO ( g) Concentration (mol L) N 2 O 4 NO 2 0 t 1 t 2 t 3 Time At time t 1, heat is applied to the system. Which of the following best describes the equilibriumêreaction and the change in K eq? A. exothermic and K eq Êincreases B. exothermic and K eq decreases C. endothermic and K eq increases D. endothermic and K eq decreases 13. Consider the following: (1Êmark) PCl3 ( g) + Cl2( g) PCl5 ( g) Keq = at 227 C Initially, a 1. 00L flask is filled with mol PCl3, mol Cl 2, and mol PCl5 atê 227 C. Use K Trial to predict the change in Cl 2 [ ] as equilibrium is established. K Trial [ Cl 2 ] A. K > K increases Trial eq B. K < K increases Trial eq C. K > K decreases Trial eq D. K < K decreases Trial eq OVER

12 14. A saturated solution forms when a 010. mol of salt is added to 1. 0L of water. The salt is (1Êmark) A. Li 2 S B. CuBr 2 C. Zn( OH) 2 ( ) D. NH CO Consider the following equilibrium: (1Êmark) ( ) 2+ + Ca OH 2( s) Ca ( aq) 2OH ( aq) Adding which of the following could cause the equilibrium [ Ca 2+ ] to increase? A. HO 2 ( l) B. HCl ( aq) C. KOH ( s) ( ) 2( s) D. Ca OH 16. Consider the following solubility equilibrium: (1Êmark) AgCl + ( s) Ag ( aq) + Cl ( aq) Which of the following graphs represents the [ Ag + ] after equilibrium has been established? A. B. [ Ag + ] [ Ag + ] time time C. D. [ Ag + ] [ Ag + ] time time - 6 -

13 17. The concentrations of the cation and anion in 040. M ( NH4) 2Cr2O 7( aq ) are (1Êmark) Cation Anion A M 0. 40M B M 0. 80M C M 0. 40M D M 0. 80M 18. Which of the following will produce a solution with the highest [ OH ]? (1Êmark) A. AgOH B. Sr OH ( ) 2 C. Fe( OH) 3 D. Mg( OH) When equal volumes of 0. 20M ZnSO and 020. M SrS are combined (2Êmarks) A. a precipitate does not form. B. a precipitate of only ZnS forms. C. a precipitate of only SrSO 4 forms. D. precipitates of both ZnS and SrSO 4 form What is the concentration of Pb 2+ in a saturated solution of Pb( IO 3 ) 2? (2Êmarks) A B C D M M M M OVER

14 21. Which of the following tests could be used to distinguish between 1. 0M HCl andê1. 0M NaOH? (1Êmark) I. electrical conductivity II. III. reaction with zinc to produce hydrogen gas colour of the indicator phenolphthalein A. III only B. I and II only C. II and III only D. I, II and III 22. An Arrhenius base is defined as a compound that (1Êmark) A. accepts OH in solution. B. releases OH in solution. C. accepts protons in solution. D. donates protons in solution. 23. In which one of the following equations are the Br nsted-lowry acids and bases all correctly identified? (1Êmark) Acid + Base Base + Acid A. HO SO 3 2 HO 2 + HSO 3 B. HO SO 3 2 HSO 3 + HO 2 C. SO HO 2 2 HO 2 + HSO 3 D. SO HO 2 2 HSO 3 + HO 2-8 -

15 24. Which of the following statements applies to 1. 0M NH3 ( aq) but not to 1. 0M NaOH ( aq)? (1Êmark) A. partially ionizes B. neutralizes an acid C. has a ph greater than 7 D. turns bromcresol green from yellow to blue 25. In which of the following are reactants favoured? (1Êmark) 2 2 A. HNO + CN NO + HCN B. H S + HCO HS + H CO C. H PO + NH H PO + NH D. CH COOH + PO CH COO + HPO 26. What is the poh of a solution prepared by adding 050. mol of NaOH to prepare 050. L of solution? (2Êmarks) A B C D What is the [ HO 3 ] in a solution with a poh = 520.? (2Êmarks) A B C D M M M M OVER

16 28. Which of the following solutions will have a ph = 100.? (1Êmark) A. I only. B. III only. C. I and II only. D. I, II and III. I M HCl II M HNO2 III M NaOH K a for the acid H AsO is What is the value of K b for HAsO 2 4? (1Êmark) A B C D In a titration, which of the following has a ph = 700. at the equivalence point? (1Êmark) A. NH and HNO 3 3 B. KOH and HCN C. NaOH and HCl D. Ca( OH) 2 and CH 3 COOH 31. Which of the following salts dissolves to produce a basic solution? (1Êmark) A. KCl B. NH4Br C. Fe( NO 3 ) 3 D. LiCH COO

17 32. What colour would1. 0M HCl be in an indicator mixture consisting of phenol red and thymolphthalein? (2Êmarks) A. red B. blue C. yellow D. colourless 33. During a titration, what volume of M KOH is necessary to completely neutralize 10. 0mL of 2. 00M CH3COOH? (2Êmarks) A ml B ml C ml D ml 34. Which indicator has a K a = ? (1Êmark) A. neutral red B. thymol blue C. thymolphthalein D. chlorophenol red 35. Acid is added to a buffer solution. When equilibrium is reestablished the buffering + effect has resulted in HO 3 A. increasing slightly. B. decreasing slightly. C. increasing considerably. D. decreasing considerably. [ ] (1Êmark) 36. A buffer solution will form when 010. M NaF is mixed with an equal volume of (1Êmark) A M HF B M HCl C M NaCl D M NaOH OVER

18 37. Which of the following will dissolve in water to produce an acidic solution? (1Êmark) A. CO 2 B. CaO C. MgO D. Na 2 O 38. Which of the following represents a redox reaction? (1Êmark) A. C + O 2 CO 2 B. H2O + SO2 H2SO3 + C. HO 3 + OH 2HO 2 D. NaCl + AgNO AgCl + NaNO The oxidation number of each chromium atom in Cr O is (1Êmark) A. +5 B. +6 C. +7 D List the ions Co, Cu and Zn in order from strongest to weakest oxidizing agents. (1Êmark) A. Zn > Co > Cu B. Co > Cu > Zn C. Cu > Zn > Co D. Cu > Co > Zn

19 41. A piece of Cu reacts spontaneously with 1. 0M Pd + because (2Êmarks) A. Cu is a weaker reducing agent than Pd and E >0. B. Cu is a weaker reducing agent than Pd and E <0. C. Cu is a stronger reducing agent than Pd and E >0. D. Cu is a stronger reducing agent than Pd and E < Which two species will not react spontaneously at standard conditions? (1Êmark) A. Co with Cl 2 B. Cu with Ag + C. Ag with Zn 2+ D. Mg with Cr When a piece of Ag is placed in 1. 0M NiCl 2, (2Êmarks) A. the Cl B. the Ag + C. the Ni 2+ [ ] increases. [ ] decreases. [ ] decreases. D. no change occurs OVER

20 Use the following cell to answer questions 44 and 45. Volts Cu 1.0 M KNO3 Zn 1.0 M Cu( NO 3 ) M Zn( NO 3 ) Which of the following represents the relationship between [ NO 3 ] and the mass of the Cu electrode in the complete cell as it operates? A. B. (1Êmark) [ NO 3 ] [ NO 3 ] Mass of Cu Mass of Cu C. D. [ NO 3 ] [ NO 3 ] Mass of Cu Mass of Cu 45. The E for the above cell is (1Êmark) A Volts B Volts C Volts D Volts

21 46. Which of the following is correct for an electrolytic cell? (1Êmark) Value of E Type of Reaction A. positive non-spontaneous B. positive spontaneous C. negative spontaneous D. negative non-spontaneous 47. Which of the following will inhibit the corrosion of iron? (1Êmark) A. high [ O 2( aq) ] B. wet conditions C. coating with zinc D. increasing the temperature 48. The products of the electrolysis of molten MgCl 2 using inert electrodes are (2Êmarks) A. hydrogen and oxygen. B. hydrogen and chlorine. C. magnesium and oxygen. D. magnesium and chlorine. 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. Consider the following reaction mechanism for the formation of NO 2. Step 1 2NO N2O2 Step 2 Overall 2NO + O 2NO 2 2 a) Complete Step 2. (2Êmarks) b) Define the term reaction intermediate. (2Êmarks) c) Identify a reaction intermediate in the above mechanism. (1Êmark)

23 2. Consider the following equilibrium system: 2COF2( g) CO2( g) + CF4( g) Keq = A 200. L container is filled with mol of COF 2. Calculate the [ COF 2 ] at equilibrium. (5Êmarks) OVER

24 3. Consider the following equilibrium system: 2+ 2 aq aq 4 aq Cu ( ) + 4Br ( ) CuBr blue colourless green ( ) Cooling the equilibrium changes the colour from green to blue. What effect will the decrease in temperature have on K eq? Explain, using Le ChatelierÕs Principle. (2Êmarks) 4. Write the balanced complete ionic equation for the reaction that occurs when 020. M of Ba( NO 3 ) 2 is added to anêequal volume of 0. 20M Na2CO 3. (2Êmarks)

25 ( ) required to start precipitation 5. Calculate the minimum number of moles of Pb NO 3 2 in 50. 0mL of 0. 15M ZnI 2. (5Êmarks) 6. Consider the following Br nsted-lowry equilibrium: 2 aq aq 2 4 aq 3 aq H2SO3 ( ) + HPO 4 ( ) H PO ( ) + HSO a) Identify the two Br nsted-lowry acids in the above equilibrium. (1Êmark) ( ) b) Define the term conjugate acid. (1Êmark) OVER

26 7. A ml sample of HCl with a ph of is completely neutralized withê M NaOH. a) What volume of NaOH is required to reach the stoichiometric point? (4Êmarks) b) Write the net ionic equation for the above neutralization reaction. (1Êmark) c) If the HCl were titrated with a M NH3 ( aq) instead of M NaOH, how would the volume of base required to reach the equivalence point compare with the volume calculated in part a)? Explain your answer. (1Êmark)

27 8. Consider the following equilibrium: energy + H O H O + OH a) Explain how pure water can have a ph = (2Êmarks) b) Calculate the value of K w for the sample of water with a ph = (2Êmarks) OVER

28 9. Balance the following redox reaction in basic solution. (5Êmarks) SO MnO SO MnO basic + + ( )

29 10. Draw and label the parts of an operating electrochemical cell using a zinc anode that will produce an electric current having a voltage of 1. 56V at standard conditions. (4Êmarks) END OF EXAMINATION

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

32 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.

33 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

34 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

35 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

36 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

37 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

38 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

39 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

40 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