CHEMISTRY 12 AUGUST 2000 STUDENT INSTRUCTIONS

Transcription

1 Insert Personal Education Number (PEN) here. Insert only pre-printed PEN label here. STUDENT INSTRUCTIONS 1. Insert 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 CHEMISTRY 12 AUGUST 2000 COURSE CODE = CH Insert only hand-printed PEN here. 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. Ministry use only Ministry of Education

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

3 CHEMISTRY 12 AUGUST 2000 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: 80 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: 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. Consider the following reaction: N2( g) + 3H2( g) 2NH3 ( g) If the rate of formation of NH is mol s, then the rate of consumption of H 2 is A mol s B mol s C mol s D mol s Consider the following reaction: Zn( s) + 2HCl( aq) ZnCl2( aq) + H2( g) Which of the following instruments could be used to monitor the rate of the reaction in an open system? A. I and II only. B. I and III only. C. II and III only. D. I, II and III. I. Balance II. III. Pressure gauge ph meter OVER

8 3. Which of the following changes occur when the temperature of a reaction is increased? I. H of the reaction increases II. III. Frequency of the collisions increases Kinetic energy of the reactants increases A. I and II only. B. I and III only. C. II and III only. D. I, II and III. 4. Which of the following is true for an activated complex? A. stable and has low PE B. stable and has high PE C. unstable and has low PE D. unstable and has high PE 5. As you increase the temperature of a reaction, the A. rate increases and the time required for the reaction increases. B. rate increases and the time required for the reaction decreases. C. rate decreases and the time required for the reaction increases. D. rate decreases and the time required for the reaction decreases. 6. Which of the following potential energy curves represents a catalyzed endothermic reaction in the forward direction? I III PE II PE IV Progress of the reaction Progress of the reaction A. I B. II C. III D. IV - 2 -

9 7. Which of the following does not apply to all chemical equilibrium systems? A. They are closed. B. The macroscopic properties are constant. C. Forward and reverse reaction rates are equal. D. There are equal concentrations of reactants and products. 8. Consider the following equilibrium: 2NOCl( g) 2NO( g) + Cl2( g) A flask is filled with NOCl, NO and Cl2. Initially there was a total of 5. 0moles of gases present. When equilibrium is reached, there is a total of 6. 0moles of gases present. Which of the following explains this observation? A. The reaction proceeded left because the Trial K > K B. The reaction proceeded left because the Trial K < K C. The reaction proceeded right because the Trial K > K D. The reaction proceeded right because the Trial K < K eq eq eq eq eq eq eq eq 9. Consider the following reaction: CH 3 8( g) + 5O2 ( g) 3CO2( g) + 4HO 2 ( g) H = 2202 kj Which of the following applies to the forward reaction? Entropy Enthalpy A. increases increases B. increases decreases C. decreases increases D. decreases decreases OVER

10 10. Consider the following equilibrium: NO ( ) N O ( ) + energy 2 2 g 2 4 g The number of moles of NO 2 at equilibrium could be increased by A. adding NO 2 4 B. adding a catalyst. C. decreasing the temperature. D. decreasing the volume by increasing the pressure. 11. What is the K eq expression for [ + H ] 2 A. K eq = 3 Sb Cl + [ ][ ] [ + H ] 2 [ SbOCl ] B. K eq = 3+ Sb Cl C. K 3+ [ ][ ] + 2 [ H ] eq = 3+ [ Sb ][ Cl ][ H2O] [ + H ] 2 [ SbOCl ] D. Keq = 3+ Sb Cl H O [ ][ ][ 2 ] Sb ( aq) + Cl ( aq) + H O 2 ( l) SbOCl( s) + 2H ( aq) Consider the following equilibrium: H2( g) + I 2( g) 2HI( g) Keq = What is the value K eq for the reaction rewritten as: A B C D HI( ) H ( ) + I ( ) K =? 2 g 2 g 2 g eq - 4 -

11 13. Consider the following equilibrium: 2NO2( g) N2O4( g) Keq = The equilibrium concentration of NO 2 is 050. mol L. Calculate the equilibrium concentrationêof NO 2 4( g). A mol L B mol L C mol L D mol L 14. Which of the following forms a molecular solution in water? A. SrSO 4 B. Na3PO4 C. CH 6 12O6 D. NH4CH3COO 15. Which of the following is necessary to form a saturated solution at equilibrium? A. excess solute B. an ionic solute C. solute of low solubility D. trial ion product is less than K sp 16. The net ionic equation that describes a saturated solution of Ag CrO 2 4 is A. Ag CrO 2 4( s) Ag2CrO4( aq) B. Ag CrO ( s) 2Ag ( aq) + CrO4 ( aq) C. Ag CrO ( s) 2Ag ( aq) + Cr ( aq) + 4O ( aq) D Ag ( aq) + CrO4 ( aq) + 2H2O ( l) 2AgOH( s) + H2CrO4( aq) OVER

12 17. Which of the following compounds has the lowest solubility? A. SrS B. CaCl 2 C. Rb CO 2 3 ( ) 2 D. Zn OH 18. Which of the following will form a precipitate when equal volumes of 02. M solutions are combined? A. HI and Na CO 2 3 B. SrS and NH OH 4 C. BaCl and CuSO 2 4 ( ) D. Mg NO and KCl The solute AgBr is least soluble in A. HO 2 B. 10. M FeBr3 C. 10. M CaBr2 D. 10. M AgNO3 20. The magnesium and calcium ions in hard water can be removed by the addition of A. NaI B. NaNO 3 C. Na2CO3 D. Na2SO4 21. The solubility of an AB 2 type salt is M. The salt is A. PbBr 2 B. Fe( OH) 2 ( ) C. Cu IO 3 2 D. Mg( OH) 2-6 -

13 22. Which of the following saturated solutions will have the lowest [ Pb 2+ ]? A. PbI 2 B. PbCl 2 ( ) ( ) C. Pb IO 3 2 D. Pb NO Consider the following equilibrium: HC O + HSO H C O + SO The order of Br nsted-lowry acids and bases in the reaction is A. base, acid, acid, base. B. base, acid, base, acid. C. acid, base, acid, base. D. acid, base, base, acid. 24. Which of the following will have the lowest electrical conductivity? A M HCl B M HNO3 C M H2SO4 D M H3PO4 25. Which of the following represents the ionization of water? A. HO 1 H + O B. 2HO 2 HO 3 + OH + C. 2HO+ O 2HO D. HO O2 + 2H + 2e OVER

14 26. Which of the following are amphiprotic? I. HO 2 II. NH 4 + III. HCO 3 A. I and II only. B. I and III only. C. II and III only. D. I, II and III. 27. Consider the following equilibrium: 2 2 l 3 H O( ) + energy H O ( aq) + OH ( aq) The temperature is increased 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 = What is the ph of a 010. M Sr( OH) 2 solution? A B C D In order to change the ph of a solution from 2. 0 to 40. the H3O + A. increase by a factor of 2. B. decrease by a factor of 2. C. increase by a factor of 100. D. decrease by a factor of 100. [ ] must - 8 -

15 30. The K b expression for HSe is [ HSe ][ OH ] A. Kb = 2 HSe [ ] [ HSe ][ OH ] B. Kb = 2 Se [ ] [ HSe ][ + H O ] b = 3 C. K [ HSe 2 ] [ 2 Se ][ + H O ] D. Kb = 3 HSe [ ] 31. Which of the following graphs describes the relationship between K a and K b for all conjugate pairs? A. B. K a K a K b K b C. D. K a K a K b K b OVER

16 32. The value of K b for HSO 3 is A B C D Which of the following ions will produce an acidic solution when added to water? A. O 2 B. Na + C. + NH 4 D. HCO What is the HO 3 [ ] at the transition point for an indicator with a K a of Ê? A B C D M M M M 35. What is the ph of the solution formed when mol KOH is addedêtoê L of M HCl? A B C D The ph of normal rainwater is a result of the presence of dissolved A. SO 2 B. CO 2 C. NO 2 D. ClO

17 37. A chemical process involving the loss of electrons is a definition of A. oxidation. B. reduction. C. galvanization. D. cathodic protection. 38. Which of the following is not a redox reaction? A. 2Mg + O2 2MgO B. SO3 + H2SO4 H2S2O7 C. CuS + 2 O 2 + C Cu + SO 2 + CO 2 D. 4Ag + 2H S + O 2Ag S + 2H O A reducing agent will cause which of the following changes? A. ClO 3 ClO2 B. NO 2 N2O4 C. HPO 3 3 HPO 3 4 D. HS2O 4 H2SO3 40. The oxidation number of zinc in a reaction increases by 2. This indicates that A. zinc is reduced and loses 2 electrons. B. zinc is reduced and gains 2 electrons. C. zinc is oxidized and loses 2 electrons. D. zinc is oxidized and gains 2 electrons. 41. Which metal will react spontaneously with water? A. Ca B. Ni C. Pb D. Hg OVER

18 42. Consider the following redox reaction which occurs in a lead-acid storage cell: PbO2( s) + Pb( s) + 2H2SO4( aq) 2PbSO4( s) + 2H2O( l) The balanced reduction half-reaction is 2+ A. Pb Pb + 2e B. Pb + SO PbSO + e C. 2H SO 2Pb 2e 2PbSO 2H O D. PbO H SO e PbSO H O 43. Consider the following redox reactions: HClO + I HIO + Cl E = V HClO + Br HBrO + Cl E = V The relative strength of the oxidizing agents from strongest to weakest is A. HIO > HBrO > HClO B. HClO > HIO > HBrO C. HBrO > HIO > HClO D. HClO > HBrO > HIO

19 44. Consider the following diagram of a fuel cell in which H 2 and O 2 combine to produce H O 2 under basic conditions: DC Volts O 2 out H 2 gas in Cathode Electrolyte KOH (aq) Anode O 2 in H 2 gas out The reaction at the anode is + A. 2H + 2e H2 + O + 2H + 2e H O B C. 4OH O + 2H O + 4e D. H + 2OH 2H O + 2e OVER

20 Use the following diagram to answer questions 45 and 46. Volts Ni 1.0 M KNO3 Cu 1.0 M Ni M Cu As the cell operates, observations include Mass of Nickel Electrode Concentration of Copper Ions A. decreases increases B. decreases decreases C. increases increases D. increases decreases 46. What is the cell potential, E, for this cell? A V B V C V D V

21 47. Consider the following electrolytic cell: DC Power Source + Ð Inert electrode Inert electrode Molten NaI (l) In the cell above, A. I migrates to the anode and gains electrons. B. I migrates to the cathode and loses electrons. C. Na + migrates to the anode and loses electrons. D. Na + migrates to the cathode and gains electrons. 48. Which of the following are necessary for electroplating to occur using an electrolytic cell? I. Two electrodes II. III. A metal ion being reduced A direct current power source A. I and II only. B. I and III only. C. II and III only. D. I, II, and III. 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: 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. Consider the following reaction: CaCO3 ( s) + 2HCl( aq) CaCl2( aq) + CO2( g) + H2O( l) A sample of some HCl was added to a sample of CaCO 3 in an open beaker. The total mass was monitored and the following data obtained: HCl (aq) CaCO 3(s) Time (min) Total mass of beaker and contents (g)

23 a) Find the average rate of production of CO in mol s 2 during the first 5 minutes. (2 marks) b) Give one reason why the rate of production of CO 2 would decrease with time. Explain, using collision theory. (1Êmark) Reason: Explanation: OVER

24 2. Consider the following reaction: aq aq aq Fe ( ) + SCN ( ) FeSCN ( ) yellow colourless red When a few drops of 60. M NaOH is added to ml of the above system, a precipitate ofê Fe OH ( ) 3 forms and the solution turns pale yellow. a) Explain this colour change in terms of Le Ch telierõs Principle. (2Êmarks) b) Describe the effect on the rate of the reverse reaction as the colour change occurs. (1Êmark)

25 3. Consider the following equilibrium: 3I2( g) + 3F 2( g) 2IF2( g) + I4F2 ( g) 1 1 Initially, mol of I2 and mol of F 2 are put into a L flask. 3 At equilibrium, I F is M. Calculate the K eq. (4Êmarks) [ 4 2] OVER

26 4. a) Write the complete ionic equation for the reaction between NaBrO and AgNO 3 3. (1Êmark) b) What is the maximum NaBrO 3 [ ] that can exist in equilibrium with M AgNO? (2Êmarks) 5. a) Define the term Br nsted-lowry conjugate acid-base pair. (1Êmark) b) Give an example of a conjugate acid-base pair. (1Êmark) Acid: Base:

27 6. Consider the acids HCl and HF. a) Only one of the following reactions occurs. Complete the equation for the reaction which does occur. (1 mark) i) HCl + F? ii) HF + Cl? b) For the reaction that occurs, are reactants or products favoured? Explain. (1 mark) c) Explain why the other reaction will not occur. (1 mark) OVER

28 + 7. Calculate the [ HO 3 ] of 010. M HNO 2. (3Êmarks)

29 8. Write the formula equation and the net ionic equation for the reaction between 010. M H SO and 010. M Sr OH Formula equation: ( ). (3Êmarks) Net ionic equation: OVER

30 9. During the production of magnesium metal from sea water, magnesium ions are first precipitated from sea water as magnesium hydroxide. a) The magnesium hydroxide is then neutralized by hydrochloric acid, producing magnesium chloride. Write the neutralization reaction. (1 mark) b) The salt produced, magnesium chloride, is dried, melted and undergoes electrolysis. Write the reaction occurring at each electrode. (2Êmarks) Anode: Cathode: c) It is not possible to use electrolysis to remove Mg from a M MgCl solution. Why? (1 mark)

31 10. In the process of extracting tin from a sample of ore, the tin is removed as Sn 2+ ions. A titration requires ml of M K2Cr2O 7 to reach the equivalence point with the Sn 2+ in a g sample of the ore Sn ( aq) + Cr2O 7 ( aq) + 14H ( aq) 3Sn ( aq) + 2Cr ( aq) + 7H2O l ( ) Using the reaction, calculate the percent mass of tin in the ore sample. (4Êmarks) END OF EXAMINATION

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

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 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.

34 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

35 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

36 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

37 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

38 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

39 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

40 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

41 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