PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS

Transcription

1 INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE JUNE 1998 PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS 1. Insert the stickers with your Student I.D. Number (PEN) in the allotted spaces above and on the back cover of this booklet. Under no circumstance is your name or identification, other than your Student I.D. Number, to appear on this booklet. 2. Ensure that in addition to this examination booklet, you have a Data Booklet and an Examination Response Form. Follow the directions on the front of the Response Form. 3. Disqualification from the examination will result if you bring books, paper, notes or unauthorized electronic devices into the examination room. 4. All multiple-choice answers must be entered on the Response Form using an HB pencil. Multiple-choice answers entered in this examination booklet will not be marked. 5. For each of the written-response questions, write your answer in the space provided in this booklet. 6. When instructed to open this booklet, check the numbering of the pages to ensure that they are numbered in sequence from page one to the last page, which is identified by END OF EXAMINATION. 7. At the end of the examination, place your Response Form inside the front cover of this booklet and return the booklet and your Response Form to the supervisor Ministry of Education

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3 CHEMISTRY 12 PROVINCIAL EXAMINATION 1. This examination consists of two parts: Value Suggested Time PART A: 48 multiple-choice questions PART B: 11 written-response questions Total: 80 marks 120 minutes 2. Aside from an approved calculator, electronic devices, including dictionaries and pagers, are not permitted in the examination room. 3. The following tables can be found in the separate Data Booklet. Periodic Table of the Elements Atomic Masses of the Elements Names, Formulae, and Charges of Some Common Ions Solubility of Common Compounds in Water Solubility Product Constants at 25 C Relative Strengths of Brönsted-Lowry Acids and Bases Acid-Base Indicators Standard Reduction Potentials of Half-cells No other reference materials or tables are allowed. 4. A calculator is essential for the Chemistry 12 Provincial Examination. The calculator must be a hand-held device designed primarily for mathematical computations involving logarithmic and trigonometric functions. 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 communication between calculators is prohibited during the examination. In addition to an approved calculator, students will be allowed to use rulers, compasses, and protractors during the examination. 5. The time allotted for this examination is two hours.

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5 PART A: MULTIPLE CHOICE Value: 48 marks INSTRUCTIONS: Suggested Time: 70 minutes For each question, select the best answer and record your choice on the Response Form provided. Using an HB pencil, completely fill in the circle that has the letter corresponding to your answer. 1. Which of the following reactions occurs most rapidly at room temperature? A. H 2( g) +I 2( g) 2HI ( g) B. 2Fe () s +O 2g ( ) 2 FeO () s 2+ C. Cu ( aq) 2 +S ( aq) CuS () s D. C 6 H 12 O 6( aq) +6O 2( g) 6CO 2( g) +6H 2 O ( g) 2. Consider the following reaction: CO + NO 2 CO 2 + NO H =234 kj The activation energy of the forward reaction is 134 kj. What is the activation energy for the reverse reaction? A. 134 kj B. 100 kj C. 234 kj D. 368 kj 3. Which of the following will decrease the number of effective collisions during a chemical reaction? A. Adding a catalyst. B. Increasing the surface area. C. Decreasing the temperature. D. Increasing reactant concentrations OVER

6 4. Consider the following reaction: The rate of reaction is increased by A. adding a catalyst. B. removing some O 2. C. decreasing the temperature. D. increasing the volume of the container. 2N 2 O 5( g) +110 kj 4NO 2( g) +O 2( g) 5. Which of the following apply to all equilibrium systems? I II III Forward and reverse rates are equal Macroscopic properties are constant Mass of reactants equals mass of products A. I and II only B. I and III only C. II and III only D. I, II and III 6. Consider the following equilibrium: The forward reaction is N 2( g) +3H 2( g) 2NH 3( g) +92 kj A. exothermic and entropy is increasing. B. exothermic and entropy is decreasing. C. endothermic and entropy is increasing. D. endothermic and entropy is decreasing

7 7. Consider the following equilibrium: PCl 5( g) PCl 3( g) +Cl 2( g) The equilibrium concentration of PCl 5 will increase when A. PCl 3 is added. B. Cl 2 is removed. C. a catalyst is added. D. the volume of the container is increased. 8. Consider the following equilibrium: N 2 O 4( g) 2NO 2( g) If the volume of the container is decreased, the A. K eq decreases. [ ] increases. B. N 2 O 4 C. equilibrium does not shift. D. equilibrium shifts to the right. 9. Consider the following equilibrium: For this reaction, A. K eq = [ CO 2 ] B. K eq = C. K eq = 1 [ CO 2 ] [ CaCO 3 ] [ ] CaO CO 2 [ ] [ ] CaO [ ] [ ] D. K eq = CO 2 CaCO 3 CaO () s +CO 2( g) CaCO 3() s OVER

8 10. Which of the following reactions most favours products? REACTION K eq I II III IV 2SO 2( g) +O 2( g) 2SO 3( g) NO ( g) +O 2( g) 2NO 2( g) CO ( g) +O 2( g) 2CO 2( g) H 2( g) +O 2( g) 2H 2 O ( g) A. I B. II C. III D. IV 11. Consider the following: C () s +H 2 O ( g) CO ( g) +H 2( g) At equilibrium in a 1.0 L container, there are mol C, mol H 2 O, mol CO, and mol H 2. The value of K eq is A B C D Consider the following equilibrium: N 2 O 4( g) 2NO 2( g) K eq = At equilibrium, the [ NO 2 ]= mol L and the [ N 2 O 4 ] is A mol L B mol L C mol L D. 25 mol L - 4 -

9 13. Which of the following dissolves in water to form an ionic solution? A. O 2 B. SiO 2 C. KMnO 4 D. C 12 H 22 O A dilute solution of AgNO 3 is added dropwise to each of the following test tubes until a precipitate forms in each tube. 0.2 M NaCl 0.2 M FeCl M CuCl M NH 4 Cl Which solution requires the lowest [ Ag + ] to just begin precipitation? A. NaCl B. FeCl 3 C. CuCl 2 D. NH 4 Cl 15. Which of the following is most soluble? A. Na 2 S B. CaSO 4 C. PbCO 3 D. Zn( OH) OVER

10 16. The solubility of PbI 2 will increase with the addition of A. PbI 2 B. heat. C. water. D. Pb( NO 3 ) Which of the following saturated solutions has the lowest [ SO 4 ] at 25 C? A. SrSO 4 B. PbSO 4 C. CaSO 4 D. BaSO The solubility of MgCO 3 is A M B M C M D M 19. When equal volumes of 0.20 M Pb( NO 3 ) 2 and 0.20 M KI are mixed together, A. a precipitate forms since Trial Ion Product > K sp B. a precipitate forms since Trial Ion Product < K sp C. no precipitate forms since Trial Ion Product > K sp D. no precipitate forms since Trial Ion Product < K sp 20. Bubbles form when Mg () s is added to HCl ( aq). The gas produced is A. O 2 B. H 2 C. Cl 2 D. H 2 O - 6 -

11 21. A substance which produces hydrogen ions in solution is the definition of A. an Arrhenius acid. B. an Arrhenius base. C. a Brönsted-Lowry acid. D. a Brönsted-Lowry base. 22. The number of conjugate pairs in a Brönsted-Lowry acid-base equation is A. 1 B. 2 C. 3 D Which of the following is a stronger base than HPO 4? A. H 2 O B. NO 2 C. 2 CO 3 D. H 2 PO Consider the following equilibria: HTe + HSe HTe + Se 2 H 2 Te + Se 2 HSe + Te 2 Reactants are favoured in both equilibria. The order of acids from strongest to weakest is A. HTe, HSe, H 2 Te B. HSe, H 2 Te, HTe C. H 2 Te, HTe, HSe D. H 2 Te, HSe, HTe OVER

12 25. The equilibrium expression for the ion product constant of water is A. K w = [ H 3 O + ][ ] OH B. K w = C. K w = 1 H 3 O + [ ][ ] OH [ H 2 O] 2 H 3 O + [ ][ ] OH [ ][ ] OH D. K w = H 3 O+ [ H 2 O] Calculate the ph of 0.01 M NaOH. A B C. 2.0 D Consider the following: TEMPERATURE K w 25 C C When water is heated, [ ] [ ] [ ] [ ] A. H 3 O + B. H 3 O + C. H 3 O + D. H 3 O + [ ] [ ] and OH and OH both increase. both decrease. increases and OH decreases and OH [ ] decreases. [ ] increases

13 28. The [ H 3 O + ] of a solution with a poh of 4.60 is A M B M C M D M 29. The K b expression for aniline, C 6 H 5 NH 2, is + A. K b = [ C 6 H 5 NH 3 ][ ] OH B. K b = [ C 6 H 5 NH ][ H 3 ] O+ [ ][ ] OH C. K b = C 6 H 5 NH 3 + [ C 6 H 5 NH 2 ] [ ][ H 3 ] O+ D. K b = C 6 H 5 NH C 6 H 5 NH 2 [ ] 30. A solution of 0.10 M HPO 4 2 is A. acidic because K a < K b B. acidic because K a > K b C. basic because K b < K a D. basic because K b > K a 31. Consider the following equilibrium: HInd + H 2 O H 3 O + + Ind At the transition point for an acid-base indicator, [ ] A. K a = Ind [ ] B. K a = HInd C. K a = H 3 O + D. K a = H 3 O + [ ] [ ][ ] OH OVER

14 32. A solution is amber with neutral red and colourless with phenolphthalein. The approximate ph of the solution is A. 4 B. 6 C. 8 D When a 1.0 M acidic solution is titrated with a 1.0 M basic solution, the ph at the equivalence point is 8.5. The reactants could be A. HBr and KOH B. HNO 3 and NH 3 C. HCl and NaOH D. HNO 2 and NaOH 34. The net ionic equation for the reaction between KOH ( aq) and HBr ( aq) is + A. K ( aq) + B. H ( aq) +Br +OH ( aq) ( aq) KBr () s H 2 O ( l) C. KOH ( aq) +HBr ( aq) KBr ( aq) +H 2 O ( l) + D. K ( aq) +OH ( aq) + +H ( aq) +Br ( aq) + K ( aq) +Br ( aq) +H 2 O ( l) 35. Consider the following equilibrium for a buffer solution: CH 3 COOH + H 2 O CH 3 COO + H 3 O + When a small amount of acid is added to this system, and equilibrium is reestablished, [ ] A. CH 3 COO and ph have both increased. [ ] and ph have both decreased. B. CH 3 COOH [ ] C. CH 3 COO has decreased and ph remains relatively constant. [ ] has decreased and ph remains relatively constant. D. CH 3 COOH

15 36. Which of the following dissolves in water to form a basic solution? A. NO B. SO 3 C. CO 2 D. K 2 O 37. Which of the following is an equation representing a redox reaction? A. 2NO 2( g) N 2 O 4( g) B. Mg () s +Cl 2( g) MgCl 2() s + C. Ag ( aq) +Cl ( aq) AgCl () s + + D. NH 3( aq) +H ( aq) NH 4 ( aq) 38. Consider the following: O 3 + H 2 O + SO 2 SO O2 + 2H + In the redox reaction above, the chemical species oxidized is A. H + B. O 3 C. SO 2 D. 2 SO A product of the oxidation of NO 2 is A. NO B. N 2 O C. NO 2 D. NO OVER

16 40. Which of the following is the strongest reducing agent? A. Sn 2+ B. Fe 2+ C. Au 3+ D. Mn At standard conditions, a spontaneous reaction will occur between A. Pb and Fe 2+ B. Cu and Sn 2+ C. Cu 2+ and Sn 2+ D. Pb 2+ and Fe Consider the following: 2MnO 4 + 5H2 O 2 + 6H + 5O 2 + 2Mn 2+ +8H 2 O In an experiment, mol of MnO 4 is required to titrate 10.0 ml of H2 O 2 to the equivalence point. The concentration of H 2 O 2 is A M B M C M D M 43. A lead storage battery contains electrochemical cells which involve the following half-reactions: PbO 2 + 4H + +SO e PbSO 4 + 2H 2 O E = V PbSO 4 + 2e Pb + SO 4 2 E = 0.36 V Use the data above to calculate the E for one of these cells. A. E = V B. E = 1.33 V C. E = 2.05 V D. E = V

17 Use the following diagram to answer questions 44, 45 and 46. Volts Cu 1.0 M KNO3 Pb 1.0 M Cu(NO 3 ) M Pb(NO 3 ) In the electrochemical cell above, the half-reaction at the cathode is A. Pb Pb e B. Cu Cu e C. Pb e Pb D. Cu e Cu 45. In the electrochemical cell above, the anode A. loses mass as Pb is oxidized. B. gains mass as Pb is oxidized. C. loses mass as Cu is oxidized. D. gains mass as Cu is oxidized. 46. In the salt bridge in the electrochemical cell above, A. electrons flow into the Pb half-cell. B. electrons flow into the Cu half-cell. C. anions migrate into the Pb half-cell. D. anions migrate into the Cu half-cell OVER

18 Use the following diagram to answer questions 47 and 48. e DC Power Source Inert Electrode A Inert Electrode B 1.0 M CaF 2(aq) 47. The predominant half-reaction occurring at Electrode B is A. 2F F 2 +2e B. Ca e Ca C. 2H 2 O O 2 + 4H + + 4e D. 2H 2 O + 2e H 2 + 2OH 48. In the electrolytic cell above, a suitable substance for Electrode B is A. carbon. B. lithium. C. sodium. D. calcium. This is the end of the multiple-choice section. Answer the remaining questions directly in this examination booklet

19 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 reaction does not always occur when two reactant particles collide. Give two reasons why. (2 marks) i) ii) 2. Consider the following reaction mechanism: Step 1: NO + NO N 2 O 2 Step 2: Step 3: N 2 O 2 + H 2 N 2 O + H 2 O N 2 O + H 2 N 2 + H 2 O a) Write the equation for the overall reaction. (1 mark) b) Identify the reaction intermediate(s). (1 mark) OVER

20 3. Consider the following graph for the reaction: energy + N 2 O 4( g) 2NO 2( g) Concentration (mol L) NO N 2 O 4 0 t 1 t 2 t 3 Time t 4 t 5 a) What is the stress imposed at time t 1? (1 mark) b) What is the stress imposed at time t 3? (1 mark) c) Calculate K eq for the equilibrium between t 2 and t 3. (2 marks)

21 4. Consider the following net ionic equation: + Ag ( aq) +SCN ( aq) AgSCN () s A ml sample of M NH 4 SCN is used to titrate a ml sample containing Ag +. Calculate the Ag + in the original sample. (3 marks) [ ] OVER

22 5. A solution contains M Ba 2+ and an unknown concentration of Sr 2+. When dilute Na 2 CO 3 is slowly added to the mixture, both Ba 2+ and Sr 2+ start to precipitate at the same time. (3 marks) 2 a) Calculate the [ CO 3 ] when BaCO 3 starts to precipitate. b) Calculate the initial [ Sr 2+ ]

23 6. a) Define the term amphiprotic. (1 mark) b) Give an example of an amphiprotic anion. (1 mark) 7. The salt Na 2 CO 3 undergoes hydrolysis to produce a basic solution. Calculate the OH in M Na 2 CO 3. [ ] (4 marks) OVER

24 8. A student titrated a ml sample of a 0.20 M HX (unknown) acid with 0.20 M NaOH. The following data were collected. Volume of base added (ml) ph a) Describe the acid HX as strong or weak. Support your answer with two observations from the data table. (3 marks) b) Select an appropriate indicator for this titration and identify the colour at the equivalence point. (1 mark)

25 9. Balance the following redox reaction: (3 marks) Ni + ClO 4 Ni 2+ + Cl (acid) 10. Define the term electrolysis. (2 marks) OVER

26 11. Consider the following diagram: tarnished silver spoon Al On a silver spoon, the black tarnish, Ag 2 S, can be removed spontaneously by placing the spoon in contact with aluminum in a conducting solution. a) Write the equations for the two half-reactions. (2 marks) b) Write the equation for the redox reaction. (1 mark) END OF EXAMINATION

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28 INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE CHEMISTRY 12 June 1998 Course Code = CH

29 FOR OFFICE USE ONLY CHEMISTRY 12 June 1998 Course Code = CH Score for Question 1: 1. (2) Score for Question 2: 2. (2) Score for Question 3: 3. (4) Score for Question 8: 8. (4) Score for Question 9: 9. (3) Score for Question 10: 10. (2) Score for Question 4: 4. (3) Score for Question 11: 11. (3) Score for Question 5: 5. (3) Score for Question 6: 6. (2) Score for Question 7: 7. (4)

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

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 Brönsted-Lowry Acids and Bases 7 Acid-Base Indicators 8 Standard Reduction Potentials of Half-Cells REFERENCE D.R. Lide, CRC Handbook of Chemistry and Physics, 74 edition, CRC Press, Boca Raton, 1993.

32 1 PERIODIC TABLE OF THE ELEMENTS 1 H Hydrogen Li Lithium Be Beryllium Na Sodium Magnesium K Mg 20 Ca Potassium Calcium Sc Ti Scandium Titanium V Cr Vanadium Chromium Mn Manganese Iron Co Cobalt Nickel Ni Cu Zn Copper Zinc Rb Sr Rubidium Strontium Y Zr Yttrium Zirconium Nb Niobium Molybdenum Ru Rh Ruthenium Rhodium Pd Ag Palladium Silver Cd Cadmium Cs Ba Cesium Barium La Hf Lanthanum Hafnium Ta W Tantalum Tungsten Re Os Rhenium Osmium Ir Pt Iridium Platinum Au Hg Gold Mercury Fr Ra Francium Radium (223) (226) 89 Ac Actinium (227) 104 Rf Rutherfordium (261) 59 Pr Praseodymium B C N O F Boron Carbon Al Si Aluminum Silicon Nitrogen Oxygen Fluorine S Cl Sulphur Chlorine Ga Ge Gallium Germanium As Se Arsenic Selenium Br Bromine In Sn Indium Tin Sb Te Antimony Tellurium I Iodine Ne Neon Ar Argon Kr Krypton Xe Xenon Rn Radon 58 (222) Ce Cerium Nd Neodymium Sm Samarium Eu Europium Tb Terbium Ho Er Holmium Erbium Tm Yb Thulium Ytterbium Lu Lutetium Th U Thorium Uranium (145) 93 Np Pu Am Neptunium Plutonium Americium (237) (244) (243) Cm Bk Curium Berkelium (247) (247) 100 Fm Einsteinium Fermium (252) (257) 103 Lr Lawrencium (262) Ha Sg Hahnium Seaborgium (262) (263) 107 Uns Unnilseptium (262) 109 Une 1Unnilennium (266) 2 He Helium Si Silicon 28.1 Atomic number Symbol Name Atomic mass 26 Fe Mo Tc Technetium (98) 108 Uno Unniloctium (265) Based on mass of C 12 at Pm Gd Dy Dysprosium Gadolinium Promethium Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally. Pa Protactinium P Phosphorus Tl Thallium Lead Pb Bi Bismuth Polonium (209) 85 Po At Astatine (210) 98 Cf Californium (251) Es Md No Mendelevium Nobelium (258) (259) - 1 -

33 - 2 - ATOMIC MASSES OF THE ELEMENTS Based on mass of C 12 at Values in parentheses are the mass of the most stable or best known isotopes for elements which do not occur naturally. Element Symbol Atomic Number Atomic Mass Element Symbol Atomic Number Atomic Mass Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curium Dysprosium Einsteinium Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Hahnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanum Lawrencium Lead Lithium Lutetium Magnesium Manganese Mendelevium Ac Al Am Sb Ar As At Ba Bk Be Bi B Br Cd Ca Cf C Ce Cs Cl Cr Co Cu Cm Dy Es Er Eu Fm F Fr Gd Ga Ge Au Hf Ha He Ho H In I Ir Fe Kr La Lr Pb Li Lu Mg Mn Md (227) 27.0 (243) (210) (247) (251) (247) (252) (257) 19.0 (223) (262) (262) (258) Mercury Molybdenum Neodymium Neon Neptunium Nickel Niobium Nitrogen Nobelium Osmium Oxygen Palladium Phosphorus Platinum Plutonium Polonium Potassium Praseodymium Promethium Protactinium Radium Radon Rhenium Rhodium Rubidium Ruthenium Rutherfordium Samarium Scandium Selenium Silicon Silver Sodium Strontium Sulphur Tantalum Technetium Tellurium Terbium Thallium Thorium Thulium Tin Titanium Tungsten Uranium Vanadium Xenon Ytterbium Yttrium Zinc Zirconium Hg Mo Nd Ne Np Ni Nb N No Os O Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Rf Sm Sc Se Si Ag Na Sr S Ta Tc Te Tb Tl Th Tm Sn Ti W U V Xe Yb Y Zn Zr (237) (259) (244) (209) (145) (226) (222) (261) (98)

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

35 SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0.1 mol/ L at 25 ο C. NEGATIVE IONS (Anions) POSITIVE IONS (Cations) SOLUBILITY OF COMPOUNDS All Alkali ions: Soluble Li +, Na +, K +, Rb +, Cs +, Fr + All Hydrogen ion, H + Soluble All Ammonium ion, NH 4 + Soluble Nitrate, NO 3 All Soluble Chloride, Cl or Bromide, Br or Iodide, I All others Ag +, Pb 2 +, Cu + Soluble Low Solubility Sulphate, SO 4 2 All others Ag +, Ca 2+, Sr 2+, Ba 2+, Pb 2+ Soluble Low Solubility Sulphide, S 2 Alkali ions, H +, NH 4 +, Be 2+ Mg 2+, Ca 2+, Sr 2+, Ba 2+ All others Soluble Low Solubility Hydroxide, OH Alkali ions, H +, NH + 4, Sr 2+ Soluble All others Low Solubility Phosphate, PO 3 4 or Carbonate, CO 2 3 or Sulphite, SO 2 3 Alkali ions, H +, NH 4 + All others Soluble Low Solubility - 4 -

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

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

38 ACID-BASE INDICATORS INDICATOR ph RANGE IN WHICH COLOUR CHANGE OCCURS COLOUR CHANGE AS ph INCREASES Methyl violet Thymol blue Orange IV Methyl orange Bromcresol green Methyl red Chlorophenol red Bromthymol blue Phenol red Neutral red Thymol blue Phenolphthalein Thymolphthalein Alizarin yellow Indigo carmine yellow to blue red to yellow red to yellow red to yellow yellow to blue red to yellow yellow to red yellow to blue yellow to red red to amber yellow to blue colourless to pink colourless to blue yellow to red blue to yellow - 7 -

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