Chemistry 12 June 2002 Provincial Examination
|
|
- Cecily Merry Moody
- 6 years ago
- Views:
Transcription
1 Chemistry 1 June 00 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation Reduction Sub-Organizers A, B, C D, E, F G, H, I J, K, L, M, N, O, P, Q, R S, T, U, V, W Part A: Multiple Choice Q K C S CO PLO Q K C S CO PLO 1. A U 1 1 A1 5. B K 1 4 K1. C K 1 1 A6 6. A U 4 K8 3. C U 1 1 B5 7. A K 1 4 L 4. B U 1 1 B6 8. D U 4 L1 5. B U 1 1 C5 9. D K 1 4 M 6. C H 1 C4, D 30. A K 1 4 N1 7. A U 1 D3 31. B U 1 4 N3 8. D U 1 E 3. B H 4 O3 9. B H 1 E3 33. B U 1 4 O4 10. D U D7 34. C H 1 4 P1 11. D U 1 F1 35. D U 4 P3 1. B K 1 F 36. D K 1 4 Q 13. C U 1 F4 37. C K 1 4 R1 14. A U F5 38. D K 1 5 S5 15. B K 1 3 G 39. D U 5 S 16. B U 1 3 G8 40. C U 1 5 S6 17. B U 3 H1 41. C U 1 5 S6, U9 18. C U 1 3 H3 4. B K 1 5 U3 19. C U 1 3 H7 43. C H 5 U5 0. B K 1 3 I 44. D U 1 5 T1, U 1. B U 3 I3 45. D U 1 5 U. C U 1 3 I6 46. A H 1 5 U9 3. B K 1 4 J4 47. A U 5 U10 4. C U 1 4 J A U 1 5 W4 Multiple Choice = 60 marks (48 questions) 06chk July 9, 00
2 Part B: Written Response Q B C S CO PLO 1. 1 U 3 1 A3. K 1 B K D U 4 F U 3 3 E, H U 3 3 I U 4 4 J8, K U 4 L U 5 4 M U 3 4 Q U 4 5 T 1. 1 U 3 5 W1, W H 5 S6, U9 Written Response = 40 marks Multiple Choice = 60 (48 questions) Written Response = 40 (13 questions) EXAMINATION TOTAL = 100 marks LEGEND: Q = Question Number K = Keyed Response C = Cognitive Level B = Score Box Number S = Score CO = Curriculum Organizer PLO = Prescribed Learning Outcome 06chk - - July 9, 00
3 PART B: WRITTEN RESPONSE Value: 40 marks INSTRUCTIONS: Suggested Time: 50 minutes You will be expected to communicate your knowledge and understanding of chemical principles in a clear and logical manner. Your steps and assumptions leading to a solution must be written in the spaces below the questions. Answers must include units where appropriate and be given to the correct number of significant figures. For questions involving calculations, full marks will NOT be given for providing only an answer. 1. Consider the reaction: (3 marks) Al( s) + 6HCl( aq) AlCl3 ( aq) + 3H( g) A g sample of Al reacts completely in excess HCl in s. What is the rate of production of H in mol s? 1mol mol Al = 10. 0g = mol Al 7. 0g mol H rate = = mol Al = mol H = change in moles time mol H s = mol H s 3 3 mol H mol Al ( Deduct 1 mark for incorrect significant figures. ) 3 marks 06chk July 9, 00
4 . Using collision theory, give two reasons why reactions occur more rapidly at a higher temperature. ( marks) There is a greater fraction of collisions with sufficient energy. There are more frequent collisions. marks 06chk July 9, 00
5 3. Chemical reactions tend toward a position of minimum enthalpy and maximum entropy. a) What is meant by the term enthalpy? (1 mark) Enthalpy is a measure of heat content. b) What is meant by the term entropy? (1 mark) Entropy is a measure of randomness. 06chk July 9, 00
6 4. Consider the following: (4 marks) H( g) + Br ( g) HBr( g) Keq = 1. 0 Initially, mol H and mol Br are placed into a L container. What is the HBr [ ] at equilibrium? H + Br HBr [ I ] [ C] x x + x [ E] x x x K eq HBr x [ H ][ Br ] = ( ) x = [ ] ( x) x ( ) = x = [ HBr]= x = M ( ) 1. 0 = marks 06chk July 9, 00
7 5. Consider the following equilibrium and accompanying graph: ( ) + s aq + 3 aq Zn IO3 ( ) Zn ( ) IO ( ) [ IO 3 ] [ Ions] [ Zn + ] marks t 1 t t 3 a) Identify the stress applied at t 1. (1 mark) + More Zn ( aq) has been added. b) Complete the above graph from t 1 to t 3 for the [ IO 3 ]. ( marks) See graph above. 06chk July 9, 00
8 6. Calculate the solubility of SrSO 4 in grams per litre. (3 marks) SrSO + 4() Sr ( ) + SO K Sr SO s aq 4 aq s s s sp = [ ][ ]=. 7 = Solubility = s = ( ) g Solubility in g L = mol L mol = 011. gl M 3 marks 06chk July 9, 00
9 7. The cyanide ion, CN, is a Brønsted-Lowry base. a) Define Brønsted-Lowry base. (1 mark) A Brønsted-Lowry base is a proton acceptor. b) Write the equation representing the reaction of CN with water. ( marks) CN + H O HCN + OH marks c) Identify a conjugate pair in b) above. (1 mark) CN and HCN OR HO and OH 06chk July 9, 00
10 8. Write an equation to show the ionization of water. ( marks) HO + ( ) HO ( aq) + OH ( aq) marks l 3 06chk July 9, 00
11 9. Calculate the ph of M NH 3. (5 marks) NH + H O NH + OH [] I [ C] x + x + x [ E] 150. x x x marks K K b b = [ + NH ][ OH ] 4 = NH [ 3] = x 150. x = x = [ OH ]= poh = 9. ph = ( Deduct 1 mark for incorrect significant figures. ) 3 5 marks 06chk July 9, 00
12 10. Consider the following buffer equilibrium: (3 marks) + HF( aq) + H O ( l) H3O ( aq) + F ( aq) high concentration low concentration high concentration Using Le Châtelier s Principle, explain what happens to the ph of the buffer solution when a small amount of NaOH is added. + NaOH causes [ H 3 O ] to decrease. The equilibrium shifts right. The ph almost returns to the former value. 06chk July 9, 00
13 11. Balance the following redox equation: (4 marks) + Ag + NO3 Ag + NO (acidic) + + ( ) 3 Ag Ag + 3e 3e + 4H + NO3 NO + HO 3Ag + NO + 4H NO + H O + 3Ag marks (1 mark for each half-reaction) for balancing electrons for addition 06chk July 9, 00
14 1. Draw a diagram of an operating electrolytic cell used to extract pure lead from an impure lead sample. Identify the electrolyte and the material used for the anode. (3 marks) 1 mark DC Power Source + Anode (impure lead) 1.0 M Pb(NO 3 ) 06chk July 9, 00
15 13. A sample of copper is placed in HNO 3( aq) and another sample of copper is placed in HCl ( aq). 1 a) In which acid does the copper react? ( mark) Copper reacts in HNO 3( aq). 1 mark b) Calculate E for the reaction that occurs. ( 1 1 marks ) E is +06. volts 1 1 marks END OF KEY 06chk July 9, 00
Chemistry 12 June 2003 Provincial Examination
Chemistry 12 June 2003 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 April 2004 Provincial Examination
Chemistry 12 April 2004 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 April 2001 Provincial Examination
Chemistry 1 April 001 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 August 2003 Provincial Examination
Chemistry 1 August 003 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 April 2003 Provincial Examination
Chemistry 12 April 2003 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 April 2000 Provincial Examination
Chemistry 12 April 2000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 April 1998 Provincial Examination
Chemistry 12 April 1998 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 January 2002 Provincial Examination
Chemistry 12 January 2002 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 June 1998 Provincial Examination
Chemistry 12 June 1998 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 August 2005 Provincial Examination
Chemistry 12 August 2005 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 January 2000 Provincial Examination
Chemistry 2 January 2000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 August 2000 Provincial Examination
Chemistry August 000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation Ð
More informationChemistry 12 August 2002 Provincial Examination
Chemistry 12 August 2002 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 June 2000 Provincial Examination
Chemistry 1 June 000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 August 2008 Form A Provincial Examination Answer Key
Cognitive Processes K = Knowledge U = Understanding H = Higher Mental Processes Topics 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation Reduction
More informationChemistry 12 JANUARY Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2002 Ministry of Education JANUARY 2002 Course
More informationChemistry 12 August 2006 Form A Provincial Examination Answer Key
Chemistry 12 August 2006 Form A Provincial Examination Answer Key Cognitive Processes K = Knowledge U = Understanding H = Higher Mental Processes Topics 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility
More informationChemistry 12 APRIL Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2002 Ministry of Education APRIL 2002 Course Code
More informationChemistry 12 August 2007 Form A Provincial Examination Multiple-Choice Key
Chemistry 12 August 2007 Form A Provincial Examination Multiple-Choice Key Cognitive Processes K = Knowledge U = Understanding H = Higher Mental Processes Weightings 11% 78% 11% Question Types 50 = Multiple
More informationChemistry 12. Resource Exam B. Exam Booklet
Chemistry 12 Resource Exam B Exam Booklet Contents: 21 pages Examination: 2 hours 50 multiple-choice questions in the Exam Booklet Additional Time Permitted: 60 minutes Province of British Columbia PART
More informationSCH4U: EXAM REVIEW. 2. Which of the following has a standard enthalpy of formation of 0 kj mol -1 at 25ºC and 1.00 atm?
SCH4U_08-09 SCH4U: EXAM REVIEW 1. The heat of a reaction is equal to: a. enthalpy (products) + enthalpy (reactants) b. enthalpy (reactants) enthalpy (products) c. enthalpy (products) enthalpy (reactants)
More informationChemistry 12 AUGUST Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2001 Ministry of Education AUGUST 2001 Course
More informationAcids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
More informationPROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS
INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE APRIL 1996 PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS 1. Insert the stickers with your Student I.D. Number (PEN)
More informationPROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS
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)
More informationIB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any
More informationWhich of the following factors will not alter the position of equilibrium?
86 N( g) + 3H $ ( g) NH3 ( g) Which of the following factors will not alter the position of uilibrium? A a pressure decrease B a temperature increase C the presence of a catalyst D the addition of more
More informationCHM 1046 FINAL REVIEW
CHM 1046 FINAL REVIEW Prepared & Presented By: Marian Ayoub PART II Chapter Description 14 Chemical Equilibrium 15 Acids and Bases 16 Acid-Base Equilibrium 17 Solubility and Complex-Ion Equilibrium 19
More informationSecondary Topics in Equilibrium
Secondary Topics in Equilibrium Outline 1. Common Ions 2. Buffers 3. Titrations Review 1. Common Ions Include the common ion into the equilibrium expression Calculate the molar solubility in mol L -1 when
More informationCHM 2046 Test #3 Review: Chapters , 15, & 16
Chapter 14 1. For the following reaction Kc = 0.513 at 500 K. N 2 O 4 (g) 2 NO 2 (g) If a reaction vessel initially contains an N 2 O 4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations
More informationCHEMISTRY 12 JUNE 2000 STUDENT INSTRUCTIONS
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.
More information-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form
NOTES Acids, Bases & Salts Arrhenius Theory of Acids & Bases: an acid contains hydrogen and ionizes in solutions to produce H+ ions: a base contains an OH group and ionizes in solutions to produce OH ions:
More informationChapter 16. Acids and Bases. Copyright Cengage Learning. All rights reserved 1
Chapter 16 Acids and Bases Copyright Cengage Learning. All rights reserved 1 Section 16.1 Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH ions.
More informationSCH4U: Practice Exam
SCHU_07-08 SCHU: Practice Exam Energy in Chemistry 1. Which of the following correctly describes a reaction that absorbs heat from the surroundings? a. the reaction is endothermic b. H for this reaction
More informationSolutions are aqueous and the temperature is 25 C unless stated otherwise.
Solutions are aqueous and the temperature is 25 C unless stated otherwise. 1. According to the Arrhenius definition, an acid is a substance that produces ions in aqueous solution. A. H C. OH B. H + D.
More information8.1 Explaining the Properties of Acids & Bases. SCH4U - Chemistry, Gr. 12, University Prep
8.1 Explaining the Properties of Acids & Bases SCH4U - Chemistry, Gr. 12, University Prep Equilibrium & Acids & Bases 2 So far, we have looked at equilibrium of general chemical systems: We learned about
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following is the weakest acid? 1) A) HF (Ka = 6.8 10-4) B) HNO2 (Ka
More informationSCH4U Chapter 8 review
Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic
More informationStrong and Weak. Acids and Bases
Strong and Weak Acids and Bases Strength of Acids H2SO4 HSO4 - + H + HNO3 NO3 - + H + Strong Acids HCl Cl - + H + H3PO4 H2PO4 - + H + Phosphoric acid Moderate Acid CH3COOH CH3COO - + H + Acetic acid HF
More informationExample 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates
Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates For Practice 15.1 In each reaction, identify the Brønsted Lowry acid, the Brønsted Lowry base, the conjugate acid, and the conjugate
More informationAcids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.
Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when
More informationChapter 9. Aqueous Solutions and Chemical Equilibria
Chapter 9 Aqueous Solutions and Chemical Equilibria Classifying Solutions of Electrolytes Electrolytes form ions when dissolved in solvent and thus produce solutions that conduct electricity. Strong electrolytesionize
More informationChemistry 12 - Learning Outcomes
Chemistry 12 - Learning Outcomes A: Chapt 1. Reaction Kinetics - (Introduction) A1. give examples of reactions proceeding at different rates A2. describe rate in terms of some quantity (produced or consumed)
More information*In every acid-base reaction, equilibrium favors transfer of a proton from the stronger acid to the stronger base.
16.2 Bronsted-Lowry Acids and Bases An acid is a substance that can transfer a proton to another substance. A base is a substance that can accept a proton. A proton is a hydrogen ion, H +. Proton transfer
More informationph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions?
JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 3 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a
More information11/15/11. Chapter 16. HA(aq) + H 2 O(l) H 3 O + (aq) + A (aq) acid base conjugate conjugate
Chapter 16 Table of Contents Chapter 16 16.1 16.2 16.3 16.4 16.5 16.6 Buffered Solutions Copyright Cengage Learning. All rights reserved 2 Models of Arrhenius: Acids produce H + ions in solution, bases
More informationPart A: Multiple Choice (23 marks total)
Part A: Multiple Choice (23 marks total) Use the answer sheet found at the end of this examination to answer the multiple-choice questions in this section. Shade in the circle that corresponds to your
More informationChemical Equilibrium. What is the standard state for solutes? a) 1.00 b) 1 M c) 100% What is the standard state for gases? a) 1 bar b) 1.
Chemical Equilibrium Equilibrium constant for the reaction: aa + bb + cc + dd + [C ] c [D ] d... equilibrium constant K = [ A] a [B ] b... [] = concentration relative to standard state molarity (M): for
More informationAcids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY
Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationChapter 14. Acids and Bases
Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton
More informationChapters 10 and 11 Practice MC
Chapters 10 and 11 Practice MC Multiple Choice Identify the choice that best completes the statement or answers the question. d 1. Which of the following best describes the rates of chemical reaction?
More informationConcentration 0. 5 M solutions 1. 0 M solutions. Rates Fast Slow. Which factor would account for the faster reaction rate in Experiment 1?
72. Consider the following experimental results: Experiment 1 Experiment 2 2+ - - 4 2 2 4 aq Reactants Fe ( aq) + MnO4 ( aq) MnO ( aq) + H C O ( ) Temperature 20 C 40 C Concentration 0. 5 M solutions 1.
More informationUnit 4-1 Provincial Practice Questions Page 1
Page 1 Page 2 Page 3 Page 4 Page 5 1.00 Page 6 Page 7 Page 8 55. The conjugate base of HAsO 4 2 is A. H 3 O + B. 3 AsO 4 C. H 3 AsO 4 D. H 2 AsO 4 56. Consider the following acidbase equilibrium: HC 6
More informationChapter 17. Additional Aspects of Aqueous Equilibria. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville, MO The Common-Ion Effect Consider a solution of acetic acid: CH 3 COOH(aq) + H 2 O(l)
More informationChem1120pretest2Summeri2015
Name: Class: Date: Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward
More informationCalculations Involving the Equilibrium Constant K eq )
Calculations Involving the Equilibrium Constant K eq ) 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2 ] = 3.45 M, [B 2 ] =
More informationBIOB111_CHBIO - Tutorial activity for Session 6:
BIOB111_CHBIO - Tutorial activity for Session 6: General topics for the week: Acids and Bases ph and buffer Interactive animations are used to reinforce the understanding Instructions- interactive animations:
More informationTake Home Semester 2 Practice Test for Acc Chem MM 15-16
Take Home Semester 2 Practice Test for Acc Chem MM 15-16 Thermochemistry 1. Determine ΔHrxn. 2SO2(g) + O2(g) 2SO3(g) a) 98.9 b) 98.9 c) 197.8 d) 197.8 ΔHf o SO2(g) 296.8 kj/mol SO3(g) 395.7 kj/mol O2(g)
More informationa) Write the expression for the equilibrium constant, K eq
Chemistry 12 K eq Calculations Worksheet Name: Date: Block: 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2] = 3.45 M, [B 2]
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen
More informationUnit 9: Acid and Base Multiple Choice Practice
Unit 9: Acid and Base Multiple Choice Practice Name June 14, 2017 1. Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B.
More informationReview: Acid-Base Chemistry. Title
Review: Acid-Base Chemistry Title Basics General properties of acids & bases Balance neutralization equations SA + SB water + salt Arrhenius vs. Bronsted-Lowry BL plays doubles tennis match with H+) Identify
More informationSalt Hydrolysis Problems
Salt Hydrolysis Problems Page 169 Salt Hydrolysis Problems 1) Write the Brønsted-Lowry reaction between the base CN! and the weak acid H 2 O. CN! + H 2 O W HCN + OH! 2) Write the Brønsted-Lowry reaction
More informationChapter 14 Acid- Base Equilibria Study Guide
Chapter 14 Acid- Base Equilibria Study Guide This chapter will illustrate the chemistry of acid- base reactions and equilibria, and provide you with tools for quantifying the concentrations of acids and
More informationChapter 9 Aqueous Solutions and Chemical Equilibria
Chapter 9 Aqueous Solutions and Chemical Equilibria At equilibrium, the rate of a forward process or reaction and that of the reverse process are equal. 9A The chemical composition of aqueous solutions
More informationSemester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS]
Semester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS] Unit 5: Kinetics How to talk about Reaction Rate rate = Δ[chemical]/Δtime - Common Units: M/s, mol L - s rate of
More informationWe will briefly go over Answer Key
Chem 310 Test 1 12-15 % of Grade (I ll decide later) Tests will be returned no later than 1 week after taken Reminder on regrades We will briefly go over Answer Key Oops forgot to do this!! So answer
More informationEquilibri acido-base ed equilibri di solubilità. Capitolo 16
Equilibri acido-base ed equilibri di solubilità Capitolo 16 The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.
More informationChemistry 3202 Pre-Public Examination May 2012 Name:
Chemistry 3202 Pre-Public Examination May 2012 Name: Section A: Multiple Choice This section contains 40 multiple choice covering concepts from the entire course. Please answer all multiple choice items
More informationChemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria
Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria I. Multiple Choice (for those with an asterisk, you must show work) These multiple choice (MC) are not "Google-proof", but they were so good
More informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationChem1120pretest2Summeri2015
Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward reaction has
More informationSpecific Curriculum Outcomes (updated September 18, 2016)
1 Chemistry 12 Specific Curriculum Outcomes (updated September 18, 2016) Unit A: Thermochemistry Overview: In this unit, students study energy as it relates to chemical changes and quantify the energy
More informationAcids & Bases. Chapter 17
Acids & Bases Chapter 17 Arrhenius Definition: Classic Definition of Acids and Bases Acid: A substance that increases the hydrogen ion concetration, [H + ], (also thought of as hydronium ion, H 3 O + )
More informationEdexcel Chemistry A-level Topic 12 - Acid-Base Equilibria
Edexcel Chemistry A-level Topic 12 - Acid-Base Equilibria Flashcards Define a Bronsted-Lowry acid Define a Bronsted-Lowry acid Proton donor Define a Bronsted-Lowry base Define a Bronsted-Lowry base Proton
More informationChem 106 Thursday, March 10, Chapter 17 Acids and Bases
Chem 106 Thursday, March 10, 2011 Chapter 17 Acids and Bases K a and acid strength Acid + base reactions: Four types (s +s, s + w, w + s, and w + w) Determining K from concentrations and ph ph of aqueous
More informationAcid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
More informationChapter Four: Reactions in Aqueous Solution
Chapter Four: Reactions in Aqueous Solution Learning Outcomes: Identify compounds as acids or bases, and as strong, weak, or nonelectrolytes Recognize reactions by type and be able to predict the products
More informationCH 223 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. Which of the following equations is the solubility
More informationAcid-Base Chemistry & Organic Compounds. Chapter 2
Acid-Base Chemistry & Organic Compounds Chapter 2 Brønsted Lowry Acids & Bases! Brønsted-Lowry Acid: Proton (H + ) Donor! Brønsted-Lowry Base: Proton (H + ) Acceptor! General reaction: HA + B: A - + BH
More information1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O.
1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H O. HCN + H O º H O + + CN ) Write the Brønsted-Lowry reaction for weak base NH reacting with H O NH + H O º OH + NH + ) Using the
More information1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases
Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and
More informationReturn Exam 3 Review for final exam: kinetics, equilibrium, acid-base
Chem 106 Thurs. 5-5-2011 Return Exam 3 Review for final exam: kinetics, equilibrium, acid-base Hour Ex 3; Ave=64, Hi=94 5/5/2011 1 ACS Final exam question types Topic # Calcul n Qualitative Intermol forces
More informationCHEMISTRY 12 SYLLABUS Online 2010
CHEMISTRY 12 SYLLABUS Online 2010 Mr. Lockwood Email: plockwood@sd43.bc.ca Personal: https://my43.sd43.bc.ca/schools/pinetreesecondary/classes/plockwood/default.aspx UserName: Password: WebCT: http://bb.etc.bc.ca/webct/entrypageins.dowebct
More informationChemical Equilibrium. Introduction
Introduction 1.) Equilibria govern diverse phenomena Protein folding, acid rain action on minerals to aqueous reactions 2.) Chemical equilibrium applies to reactions that can occur in both directions:
More informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of AP Chemistry 2014-15 North Nova Education Centre Mr. Gauthier
More informationDougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria
Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria This is a PRACTICE TEST. Complete ALL questions. Answers will be provided so that you may check your work. I strongly
More informationChemical Equilibrium Chapter 6
Chemical Equilibrium Chapter 6 "When a system is in chemical equilibrium, a change in one of the parameters of the equilibrium produces a shift in such a direction that, were no other factors involved
More informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville,
More informationCHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3
CHEMISTRY 123-02 Midterm #2 October 26, 2004 The total number of points in this exam is 100. The total exam time is 50 min. Good luck! PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point
More information2nd Semester Exam Review. C. K eq = [N 2][H 2 ]
Name: ate: 1. Which pair of formulas represents the empirical formula and the molecular formula of a compound?. H 2 O, 4 H 6 O 4. HO, 6 H 12 O 6 8. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g)
More informationAcid-Base Equilibria and Solubility Equilibria Chapter 17
PowerPoint Lecture Presentation by J. David Robertson University of Missouri Acid-Base Equilibria and Solubility Equilibria Chapter 17 The common ion effect is the shift in equilibrium caused by the addition
More informationCHEM Dr. Babb s Sections Exam #3 Review Sheet
CHEM 116 Dr. Babb s Sections Exam #3 Review Sheet Acid/Base Theories and Conjugate AcidBase Pairs 111. Define the following terms: Arrhenius acid, Arrhenius base, Lewis acid, Lewis base, BronstedLowry
More informationEquations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14
Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH
More information2/4/2016. Chapter 15. Chemistry: Atoms First Julia Burdge & Jason Overby. Acid-Base Equilibria and Solubility Equilibria The Common Ion Effect
Chemistry: Atoms First Julia Burdge & Jason Overby 17 Acid-Base Equilibria and Solubility Equilibria Chapter 15 Acid-Base Equilibria and Solubility Equilibria Kent L. McCorkle Cosumnes River College Sacramento,
More informationmol of added base 36. Equal moles of which of the following chemicals could be used to make a basic (1 mark)
59. 34. Consider the following titration curve: 14 13 Consider the following titration curve: 14 1 13 11 14 1 1 13 119 1 18 ph 119 7 18 6 ph 97 5 86 4 ph 75 3 64 53 1 4 31 mol of added base Select a suitable
More informationChemical Equilibrium
Chemical Equilibrium Ch 17 Apr 28 7:40 AM A Reversible reaction is a chemical reaction that can occur in both the forward and the reverse directions N 2 (g) + 3 H 2 (g) 2NH3(g) Apr 16 1:21 PM 1 Equilibrium
More informationAcid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Acid-Ionization Equilibria. Acid-Ionization Equilibria
Acid-Ionization Equilibria Acid-Base Equilibria Acid ionization (or acid dissociation) is the reaction of an acid with water to produce hydronium ion (hydrogen ion) and the conjugate base anion. (See Animation:
More informationChapter 15 - Applications of Aqueous Equilibria
Neutralization: Strong Acid-Strong Base Chapter 15 - Applications of Aqueous Equilibria Molecular: HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) SA-SB rxn goes to completion (one-way ) Write ionic and net ionic
More informationPart One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute)
CHAPTER 16: ACID-BASE EQUILIBRIA Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute) A. Weak Monoprotic Acids. (Section 16.1) 1. Solution of Acetic Acid: 2. See Table
More information