Chapter 13 & 14 Practice Exam

Size: px
Start display at page:

Download "Chapter 13 & 14 Practice Exam"

Transcription

1 Name: Class: Date: Chapter 13 & 14 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Acids generally release H 2 gas when they react with a. nonmetals. c. active metals. b. semimetals. d. inactive metals. 2. Aqueous solutions of acids a. contain only two different elements. c. have very high boiling points. b. carry electricity. d. cannot be prepared. 3. Bases taste a. soapy. c. sweet. b. sour. d. bitter. 4. Bases react with a. acids to produce salts and water. c. water to produce acids and salts. b. salts to produce acids and water. d. neither acids, salts, nor water. 5. Aqueous solutions of bases a. contain only two different elements. c. have very high boiling points. b. carry electricity. d. cannot be prepared. 6. Which of the following is a binary acid? a. H 2 SO 4 c. HBr b. CH 3 COOH d. NaOH 7. The name of a binary acid a. has no prefix. c. ends with the suffix -ous. b. begins with the prefix bi-. d. begins with the prefix hydro-. 8. An oxyacid contains a. oxygen and hydrogen only. b. oxygen, hydrogen, and one other element. c. oxygen, hydrogen, and two other elements. d. oxygen and an element other than hydrogen. 9. Which of the following is perchloric acid? a. HClO c. HClO 3 b. HClO 2 d. HClO Which of the following is chlorous acid? a. HClO c. HClO 3 b. HClO 2 d. HClO Which of the following is chloric acid? a. HClO c. HClO 3 b. HClO 2 d. HClO 4 1

2 Name: 12. An acid ending with the suffix -ic produces an anion with the a. suffix -ate. c. prefix hydro-. b. suffix -ite. d. suffix -ous. 13. Which acid is produced in the stomach? a. hydrochloric acid c. nitric acid b. phosphoric acid d. sulfuric acid 14. The traditional definition of acids is based on the observations of a. Brønsted and Lowry. c. Arrhenius. b. Lewis. d. Mendeleev. 15. An Arrhenius acid contains a. hydrogen that does not ionize. b. hydrogen that ionizes to form hydrogen ions. c. oxygen that ionizes to form hydroxide ions. d. oxygen that ionizes to form oxygen ions. 16. Arrhenius theorized that an acid is a chemical compound that a. increases the concentration of hydrogen ions when dissolved in water. b. increases the concentration of hydroxide ions when dissolved in water. c. decreases the concentration of hydrogen ions when dissolved in water. d. decreases the concentration of hydroxide ions when dissolved in water. 17. Arrhenius theorized that a base is a chemical compound that a. increases the concentration of hydrogen ions when dissolved in water. b. increases the concentration of hydroxide ions when dissolved in water. c. decreases the concentration of hydrogen ions when dissolved in water. d. decreases the concentration of hydroxide ions when dissolved in water. 18. Which of the following is not a strong acid? a. HNO 3 c. H 2 SO 4 b. CH 3 COOH d. HCl 19. Which of the following is a strong acid? a. HSO 4 c. CH 3 COOH b. H 2 SO 4 d. H 3 PO In water, hydroxides of Group 2 metals a. are all strong bases. c. are all acids. b. are all weak bases. d. are nonelectrolytes. 21. Which of the following is a weak base? a. NH 3 c. NaOH b. KOH d. Ba(OH) Many organic compounds, such as codeine, that contain nitrogen are a. strong bases. c. strong acids. b. weak bases. d. weak acids. 2

3 Name: 23. Which of the following is a diprotic acid? a. H 2 SO 4 c. HCl b. CH 3 COOH d. H 3 PO Whose definition of acids and bases emphasizes the role of protons? a. Brønsted and Lowry c. Arrhenius b. Lewis d. Bohr 25. A Brønsted-Lowry acid is a(n) a. electron-pair acceptor. c. proton acceptor. b. electron-pair donor. d. proton donor. 26. A Lewis acid is a. an electron-pair acceptor. c. a proton acceptor. b. an electron-pair donor. d. a proton donor. 27. Whose acid definition is the broadest? a. Arrhenius c. Brønsted-Lowry b. Lewis d. Faraday 28. A Lewis base is a(n) a. producer of OH ions. c. electron-pair donor. b. proton acceptor. d. electron-pair acceptor. 29. An electron-pair donor is a a. Arrhenius acid. c. Brønsted-Lowry base. b. Brønsted-Lowry acid. d. Lewis base. 30. A base is weak if its tendency to a. attract a proton is great. c. donate a proton is great. b. attract a proton is slight. d. donate a proton is slight. 31. An amphoteric species is one that reacts as a(n) a. acid only. c. acid or base. b. base only. d. None of the above 32. A species that can react as either an acid or a base is a(n) a. Lewis acid. c. oxyacid. b. amphoteric substance. d. salt. 33. The substances produced when KOH(aq) neutralizes HCl(aq) are a. HClO(aq) and KH(aq). c. H 2 O(l) and KCl(aq). b. KH 2 O + (aq) and Cl (aq). d. H 3 O + (aq) and KCl(aq). 34. A salt is not a. an ionic compound composed of a metal cation from a base. b. an ionic compound composed of an anion from an acid. c. a product of neutralization. d. a proton donor. 3

4 Name: 35. Which of the following is not a reactant in a neutralization reaction? a. H 3 O + ion b. OH ion c. an acid and a base in an aqueous solution d. a salt 36. Which compound is produced by a neutralization? a. H 2 O(l) c. Ca(OH) 2 (s) b. HNO 3 (aq) d. H 3 PO 4 (aq) 37. Which of the following gases does not dissolve in atmospheric water to produce acidic solutions? a. NO c. O 2 b. NO 2 d. CO Why is freezing-point depression a colligative property? a. It is inversely proportional to the molal concentration of a solution. b. It is directly proportional to the molal concentration of a solution. c. It does not depend on a molal freezing-point constant for each solvent. d. It depends on the properties of an electrolyte in a solvent. 39. Why is boiling-point elevation a colligative property? a. It is inversely proportional to the molal concentration of a solution. b. It is directly proportional to the molal concentration of a solution. c. It does not depend on a molal boiling-point constant for each solvent. d. It is independent of changes in vapor pressure. 40. A water solution containing an unknown quantity of a nonelectrolyte solute has a freezing point of 0.21 C. What is the molal concentration of the solution if K f = 1.86 C/m? a m c m b m d m 41. A water solution containing an unknown quantity of a nonelectrolyte solute has a freezing point of C. What is the molal concentration of the solution if K f = 1.86 C/m? a m c m b m d m 42. What is the approximate freezing-point depression of a m aqueous NaBr solution? K f = 1.86 C/m. a C c C b C d C 43. What is the approximate freezing-point depression of a m aqueous CaCl 2 solution? K f = 1.86 C/m. a C c C b C d C 44. What is the approximate freezing-point depression of a m aqueous FeCl 3 solution? K f = 1.86 C/m. a C c C b C d C 4

5 Name: 45. What is the approximate freezing-point depression of a m aqueous Na 2 SO 4 solution? K f = 1.86 C/m. a C c C b C d C 46. What is the actual freezing-point depression of a m aqueous NaCl solution? K f = 1.86 C/m. a. slightly less than C c. slightly more than C b. exactly C d. exactly 0 C 47. Actual freezing-point depressions of electrolyte solutions are slightly lower than the calculated values because of a. ion repulsion. b. more complete ionization than is expected. c. ion attraction. d. higher-than-expected effective concentration. 48. Compared with a 0.01 m sugar solution, a 0.01 m KCl solution has a. the same freezing-point depression. b. about twice the freezing-point depression. c. the same freezing-point elevation. d. about six times the freezing-point elevation. 49. Compared with a 0.01 m sugar solution, a 0.01 m MgCl 2 solution has a. the same freezing-point depression. b. about twice the freezing-point depression. c. about three times the freezing-point depression. d. about four times the freezing-point depression. 50. Compared with a 0.01 m sugar solution, a 0.01 m KCl solution has a. the same boiling-point elevation. b. roughly twice the boiling-point elevation. c. the same boiling-point depression. d. about half the boiling-point depression. 51. Compared with the freezing-point depression of a 0.01 m sugar solution, the freezing-point depression of 0.01 m HCl solution is a. exactly the same. c. exactly twice as great. b. slightly lower. d. almost twice as great. 52. Electrolytes have a greater effect on freezing-point depression than nonelectrolytes because electrolytes a. have lower freezing points. b. are volatile. c. produce more moles of solute per mole of solvent. d. are attracted to one another in solution. 5

6 Name: 53. Compared with the actual freezing-point depression for a solution of an electrolyte that dissociates into a 2+ and a 2 ion, the freezing-point depression for an equally concentrated solution of an electrolyte that dissociates into a 1+ and a 1 ion is likely to be a. lower. c. greater. b. the same. d. Not possible to tell with data provided Short Answer 54. What determines the behavior of an amphoteric compound? 55. Explain how industrial processes create acid rain. 56. Use the following equation to explain acid rain: SO 3 (g) + H 2 O(l) H 2 SO 4 (aq) Essay 57. Is the reaction to the left or the reaction to the right more favorable in the following reaction? Explain your answer in terms of acid and base strengths. CH 3 COOH(aq) + H 2 O(l) H 3 O + (aq) + CH 3 COO (aq) Problem 58. Calculate the boiling-point elevation of a solution made from 15.0 g of a nonelectrolyte solute and g of water. The molar mass of the solute is 50.0 g and K b =0.51 C/m g of a nonelectrolyte is dissolved in 1.00 kg of water. The boiling point of the solution is then measured to be C. What is the molar mass of the compound? The K b for water is 0.51 C/m. 60. Consider a solution of 50g KCl, a strong electrolyte, dissolved in 1.5 kg of water. a. Determine the expected freezing point of the solution. The molar mass of KCl is g and K f = 1.86 C/m. b. Would the actual freezing point be higher or lower than your calculated value? Why? 61. What concentration of ethylene glycol is needed to raise the boiling point of water to 105 C? (K b =0.51 C/m) 62. The freezing point of an aqueous solution that contains a nonelectrolyte is 4.0 C. What is the molal concentration of the solution? (K f = 1.86 C/m) 6

7 Chapter 13 & 14 Practice Exam Answer Section MULTIPLE CHOICE 1. ANS: C PTS: 1 DIF: I REF: 1 2. ANS: B PTS: 1 DIF: I REF: 1 3. ANS: D PTS: 1 DIF: I REF: 1 4. ANS: A PTS: 1 DIF: I REF: 1 5. ANS: B PTS: 1 DIF: I REF: 1 6. ANS: C PTS: 1 DIF: II REF: 1 7. ANS: D PTS: 1 DIF: I REF: 1 8. ANS: B PTS: 1 DIF: I REF: 1 9. ANS: D PTS: 1 DIF: II REF: ANS: B PTS: 1 DIF: II REF: ANS: C PTS: 1 DIF: II REF: ANS: A PTS: 1 DIF: II REF: ANS: A PTS: 1 DIF: I REF: ANS: C PTS: 1 DIF: I REF: 1 OBJ: ANS: B PTS: 1 DIF: I REF: 1 OBJ: ANS: A PTS: 1 DIF: I REF: 1 OBJ: ANS: B PTS: 1 DIF: I REF: 1 OBJ: ANS: B PTS: 1 DIF: II REF: 1 OBJ: ANS: B PTS: 1 DIF: II REF: 1 OBJ: ANS: A PTS: 1 DIF: I OBJ: ANS: A PTS: 1 DIF: I REF: 1 OBJ: 5 1

8 22. ANS: B PTS: 1 DIF: I REF: 1 OBJ: ANS: A PTS: 1 DIF: II REF: 1 OBJ: ANS: A PTS: 1 DIF: I REF: ANS: D PTS: 1 DIF: I REF: ANS: A PTS: 1 DIF: I REF: ANS: B PTS: 1 DIF: I REF: ANS: C PTS: 1 DIF: I REF: ANS: D PTS: 1 DIF: I REF: ANS: B PTS: 1 DIF: I REF: ANS: C PTS: 1 DIF: I REF: ANS: B PTS: 1 DIF: I REF: ANS: C PTS: 1 DIF: II REF: ANS: D PTS: 1 DIF: I REF: ANS: D PTS: 1 DIF: I REF: ANS: A PTS: 1 DIF: I REF: ANS: C PTS: 1 DIF: I REF: ANS: B PTS: 1 DIF: I REF: ANS: B PTS: 1 DIF: I REF: ANS: A PTS: 1 DIF: III REF: ANS: C PTS: 1 DIF: III REF: ANS: D PTS: 1 DIF: III REF: ANS: C PTS: 1 DIF: III REF: ANS: D PTS: 1 DIF: III REF: 2 2

9 45. ANS: B PTS: 1 DIF: III REF: ANS: A PTS: 1 DIF: III REF: ANS: C PTS: 1 DIF: I REF: ANS: B PTS: 1 DIF: II REF: ANS: C PTS: 1 DIF: II REF: ANS: B PTS: 1 DIF: II REF: ANS: D PTS: 1 DIF: II REF: ANS: C PTS: 1 DIF: II REF: ANS: D PTS: 1 DIF: I REF: 2 OBJ: 4 SHORT ANSWER 54. ANS: The behavior of an amphoteric substance is determined by the strength of the acid or base with which it is reacting. PTS: 1 DIF: I REF: ANS: Industrial processes produce compounds that dissolve in the atmospheric water in clouds. This creates acidic solutions that fall to the ground in rain or snow. PTS: 1 DIF: I REF: ANS: Sulfur trioxide gas is produced in industrial processes and released into the atmosphere. It dissolves in atmospheric water in clouds and produces sulfuric acid, which falls to the earth as acid rain or snow. PTS: 1 DIF: II REF: 3 ESSAY 57. ANS: The reaction to the left is more favorable. The H 3 O + ion is a stronger acid than the CH 3 COOH molecule and can donate its proton much more easily. The CH 3 COO ion is a stronger base than the H 2 O molecule and will attract a donated proton much more easily. PTS: 1 DIF: I REF: 3 3

10 PROBLEM 58. ANS: T = 0.61 C Solution: 15.0 g 1 mol = mol 50.0 g m = mol kg mol kg = 1.20m 1.20 m 0.51 C m C = 0.61 C PTS: 1 DIF: III REF: ANS: 68.0g Solution: 1.5 C 1 m 0.51 C = 2.94 m m = mol kg mol kg 200. g = mol 1.00 kg = mol 200. g = 68.0 g/mol mol PTS: 1 DIF: III REF: 2 4

11 60. ANS: a C Solution: 1 mol KCl 0 g KCl = molkcl g KCl m = mol KCl kg mol 1.5 kg = mol KCl kg mol kg 2 molions 1.86 C kg = 1.66 C 1 mol KCl mol ions b. It would be higher (i.e., the magnitude of the freezing-point depression would be less) because the attraction between the K + and Cl ions in solution would lower the effective concentration. PTS: 1 DIF: III REF: ANS: 9.8 m Solution: 5 C 1 m 0.51 C = m = 9.8 m PTS: 1 DIF: III REF: ANS: 2.15 m PTS: 1 DIF: III REF: 2 5

12 Chapter Practice Exam [Answer Strip] _ A 12. _ A 23. _ D 35. _ B 45. _ C 1. _ A 13. _ A 24. _ A 36. _ A 46. _ C 14. _ D 25. _ B 2. _ C 37. _ C 47. _ B 15. _ A 26. _ D 3. _ B 38. _ B 27. _ A 4. _ A 16. _ B 48. _ C 28. _ B 39. _ B 5. _ B 17. _ D 29. _ C 49. _ C 6. _ B 30. _ A 40. _ D 7. _ B 18. _ B 50. _ C 31. _ C 41. _ B 8. _ B 19. _ B 32. _ D 42. _ D 51. _ D 9. _ B 10. _ A 20. _ A 21. _ C 33. _ D 34. _ C 43. _ C 52. _ C 11. _ B 22. _ D 44.

13 Chapter Practice Exam [Answer Strip] _ D 53.

Acids and Bases. Chapter 16

Acids and Bases. Chapter 16 Acids and Bases Chapter 16 The Arrhenius Model An acid is any substance that produces hydrogen ions, H +, in an aqueous solution. Example: when hydrogen chloride gas is dissolved in water, the following

More information

Answer the following questions on notebook paper, to be collected and graded for correctness.

Answer the following questions on notebook paper, to be collected and graded for correctness. nswer the following questions on notebook paper, to be collected and graded for correctness. 1. Name the following binary acids: a. HCl hydrochloric acid b. HF hydrofluoric acid c. H 2 S hydrosulfuric

More information

UNIT (6) ACIDS AND BASES

UNIT (6) ACIDS AND BASES UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that

More information

Chapter 14 - Acids and Bases

Chapter 14 - Acids and Bases Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry

More information

If we write these equations in ionic form, in each case the net ionic equation is the same; H 3 O + (aq) + OH - (aq) H 2H 2 O(l)

If we write these equations in ionic form, in each case the net ionic equation is the same; H 3 O + (aq) + OH - (aq) H 2H 2 O(l) CHEM 1105 ACIDS AND BASES 1. Early Definitions Taste: Effect on Indicators: Neutralization: acids - sour; bases - bitter acids turn blue litmus red; bases turn red litmus blue phenolphthalein is colourless

More information

Acids and Bases: A Brief Review

Acids and Bases: A Brief Review Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.

More information

Acids and Bases: A Brief Review, see also pp and pp Brønsted-Lowry Acids and Bases 143. The H + Ion in Water

Acids and Bases: A Brief Review, see also pp and pp Brønsted-Lowry Acids and Bases 143. The H + Ion in Water Quiz number 5 will be given in recitation next week, Feb 26Mar 2 on the first part of Chapter 16, to be covered in lectures this week. 16.1 Acids and Bases: A Brief Review 16.2 BronstedLowry Acids and

More information

Acid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases

Acid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases Acids Identifying Acids and Bases Acid (anhydrides) contains H+ ions as the cation, with and other element as the anion Non-metal oxide H2SO4 HI P2O5 Bases Base (anhydrides) Contains OH- as the anion Combined

More information

stoichiometry = the numerical relationships between chemical amounts in a reaction.

stoichiometry = the numerical relationships between chemical amounts in a reaction. 1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse

More information

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties

More information

1. In which reaction is water acting only as a proton acceptor? 1) H 2 SO 4 (aq) + H 2 O ( ) HSO 4 (aq) + H 3 O + (aq)

1. In which reaction is water acting only as a proton acceptor? 1) H 2 SO 4 (aq) + H 2 O ( ) HSO 4 (aq) + H 3 O + (aq) 1. In which reaction is water acting only as a proton acceptor? 1) H 2 SO 4 (aq) H 2 O ( ) HSO 4 (aq) H 3 O (aq) NH 3 (g) H 2 O ( ) NH 4 (aq) OH (aq) CH 3 COO (aq) H 2 O ( ) CH 3 COOH(aq) OH (aq) H 2 O

More information

Chemical reactions. Classifications Reactions in solution Ionic equations

Chemical reactions. Classifications Reactions in solution Ionic equations Chemical reactions Classifications Reactions in solution Ionic equations Learning objectives Distinguish between chemical and physical change Write and balance chemical equations Describe concepts of oxidation

More information

Chapter 15: Acids, Bases, and Salts. 15.1: Acids and Bases

Chapter 15: Acids, Bases, and Salts. 15.1: Acids and Bases Chapter 15: Acids, Bases, and Salts Name: 15.1: Acids and Bases Define an Acid: Define a Base: Ex of an acid in aqueous solution: Ex of a base in aqueous solution: List some of the properties of acids

More information

Name: Class: Date: 2 4 (aq)

Name: Class: Date: 2 4 (aq) Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of

More information

CHAPTER 9. ANS: a. ANS: d. ANS: c. ANS: a. ANS: c

CHAPTER 9. ANS: a. ANS: d. ANS: c. ANS: a. ANS: c CHAPTER 9 1. Which one of the following is the acid in vinegar? a. acetic acid b. citric acid c. muriatic acid d. ascorbic acid 2. Which is a basic or alkaline substance? a. gastric fluid b. black coffee

More information

I N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS

I N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification

More information

CHAPTER 16: ACIDS AND BASES

CHAPTER 16: ACIDS AND BASES CHAPTER 16: ACIDS AND BASES Active Learning: 4, 6, 14; End-of-Chapter Problems: 2-25, 27-58, 66-68, 70, 75-77, 83, 90-91, 93-104 Chapter 15 End-of-Chapter Problems: 69-74, 125, 129, 133 16.1 ACIDS AND

More information

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g.

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g. Unit 7 Solutions, Acids & Bases Solution mixture + solvent - substance present in the amount solute - in the solvent solvent molecules solute particles ionic substances (separate) based on! Liquid Mixtures

More information

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent 1 Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent % (v/v) = volume of solute x 100 volume of solution filled

More information

Note: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2-

Note: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2- AcidBase Chemistry Arrhenius acid: Substance that dissolves in water and provides H + ions Arrhenius base: Substance that dissolves in water and provides OH ions Examples: HCl H + and Cl Acid NaOH Na +

More information

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Problems: 16.2-16.86 16.1 ACIDS AND BASES: THE BRØNSTED-LOWRY MODEL PROPERTIES OF ACIDS & BASES Acids produce hydrogen ions,

More information

Reactions in solution. A subset of chemical reactions

Reactions in solution. A subset of chemical reactions Reactions in solution A subset of chemical reactions Learning objectives Define solution and its components Distinguish among strong, weak and non-electrolyte Identify strong acids and strong bases Apply

More information

Chem101: General Chemistry Lecture 9 Acids and Bases

Chem101: General Chemistry Lecture 9 Acids and Bases : General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water

More information

BRØNSTED ACIDS & BASES

BRØNSTED ACIDS & BASES ACIDS & BASES BRØNSTED ACIDS & BASES BRØNSTED ACIDS & BASES Brønsted acids are proton donors. Brønsted bases are proton acceptors. Amphoteric species can act as either an acid or a base, depending on the

More information

Review of Basic Concepts, Molarity, Solutions, Dilutions and Beer s Law

Review of Basic Concepts, Molarity, Solutions, Dilutions and Beer s Law Review of Basic Concepts, Molarity, Solutions, Dilutions and Beer s Law Aqueous Solutions In Chemistry, many reactions take place in water. This is also true for Biological processes. Reactions that take

More information

TOPIC 11: Acids and Bases

TOPIC 11: Acids and Bases TOPIC 11: Acids and Bases ELECTROLYTES are substances that when dissolves in water conduct electricity. They conduct electricity because they will break apart into Ex. NaCl(s)! Na + (aq) + Cl - (aq), and

More information

ph of strong acid and base

ph of strong acid and base ph of strong acid and base What does strong mean in terms of acids and bases? Solubility. Basically, if you say an acid or base is strong, then it dissociates 100% in water. These types of situations are

More information

CHEM 101/105 Aqueous Solutions (continued) Lect-07

CHEM 101/105 Aqueous Solutions (continued) Lect-07 CHEM 101/105 Aqueous Solutions (continued) Lect-07 aqueous acid/base reactions a. a little bit more about water Water is a polar substance. This means water is able to "solvate" ions rather well. Another

More information

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions Chapter 4: Solution Stoichiometry Cont. 1 Aqueous Solutions Molarity (dilution calculations, solution stoichiometry); Solubility and Solubility Rules Molecular, Ionic and Net Ionic Equations Precipitation

More information

Lecture 6. Classes of Chemical Reactions

Lecture 6. Classes of Chemical Reactions Lecture 6 Classes of Chemical Reactions Lecture 6 Outline 6.1 The Role of Water as a Solvent 6.2 Precipitation Reactions 6.3 Acid-Base Reactions 1 Electron distribution in molecules of H 2 and H 2 O The

More information

CHEM 12 Acids and Bases 3/22/2016

CHEM 12 Acids and Bases 3/22/2016 Acids and Bases Name: Expected background knowledge from acids and bases introductory reading: Definitions (Arrhenius, BL) of an acid and base Definitions of conjugate acid and base pairs Properties of

More information

Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water.

Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water. Acids and Bases Know the definition of Arrhenius, Bronsted-Lowry, and Lewis acid and base. Autoionization of Water Since we will be dealing with aqueous acid and base solution, first we must examine the

More information

UNIT 14 - Acids & Bases

UNIT 14 - Acids & Bases COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) Practice: 1. hydro- - HF

More information

Chapter 16 Acid-Base Equilibria

Chapter 16 Acid-Base Equilibria Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.

More information

Chapter 7 Chemical Reactions

Chapter 7 Chemical Reactions Chemistry 25 Chapter 7 Chemical Reactions Chemical Reactions Reactions involve chemical changes in matter resulting in new substances. Reactions involve rearrangement and exchange of atoms to produce new

More information

Acids and Bases: Definitions. Brønsted-Lowry Acids and Bases. Brønsted-Lowry Acids and Bases CHEMISTRY THE CENTRAL SCIENCE

Acids and Bases: Definitions. Brønsted-Lowry Acids and Bases. Brønsted-Lowry Acids and Bases CHEMISTRY THE CENTRAL SCIENCE CHEMISTRY THE CENTRAL SCIENCE Professor Angelo R. Rossi Department of Chemistry Spring Semester Acids and Bases: Definitions Arrhenius Definition of Acids and Bases Acids are substances which increase

More information

Table 1. give a slippery feel. produce a piercing pain in a wound. are colorless when placed in phenolphthalein (an indicator).

Table 1. give a slippery feel. produce a piercing pain in a wound. are colorless when placed in phenolphthalein (an indicator). Acid/Base Basics How does one define acids and bases? In chemistry, acids and bases have been defined differently by two sets of theories. One is the Arrhenius definition, which revolves around the idea

More information

Aqueous Ions and Reactions

Aqueous Ions and Reactions Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for

More information

Chapter 14: Acids and Bases

Chapter 14: Acids and Bases Ch 14 Page 1 Chapter 14: Acids and Bases Properties of Acids Sour taste React with some metals Turns blue litmus paper red React with bases Some Common Acids HCl, hydrochloric acid H 2 SO 4, sulfuric acid

More information

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base? You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4

More information

Strong Acids (Know These) Announcements & Agenda (02/23/07) Strengths of Acids/Bases - Ionization. Last Time: Last Time: nsted-lowry Acids & Bases

Strong Acids (Know These) Announcements & Agenda (02/23/07) Strengths of Acids/Bases - Ionization. Last Time: Last Time: nsted-lowry Acids & Bases Announcements & Agenda (0//07) You should be reading Ch 0 this weekend! Quiz Today! Open Review Sessions @ pm on Wed. Low attendance this week Last Time: Bronsted nsted-lowry Acids & Bases acids donate

More information

I. Definitions: Name: Period: Date: 1. Arrhenius (1887)- produce in aqueous solutions produce in aqueous solutions

I. Definitions: Name: Period: Date: 1. Arrhenius (1887)- produce in aqueous solutions produce in aqueous solutions Name: Period: Date: I. Definitions: 1. Arrhenius (1887)- produce in aqueous solutions produce in aqueous solutions 2. Bronsted-Lowry (1923) 3. Lewis (1923), so only allows for aqueous solutions only protic

More information

Chapter 16 Acid-Base Equilibria

Chapter 16 Acid-Base Equilibria Chapter 16 AcidBase Equilibria Acids and bases are found in many common substances and are important in life processes. Group Work: Make a list of some common acids and bases. How do we know which is which?

More information

Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution:

Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution: Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution: 1. What are the different types of Intermolecular forces? Define the following terms:

More information

Sample Exercise 13.1 Predicting Solubility Patterns

Sample Exercise 13.1 Predicting Solubility Patterns Sample Exercise 13.1 Predicting Solubility Patterns Predict whether each of the following substances is more likely to dissolve in the nonpolar solvent carbon tetrachloride (CCl 4 ) or in water: C 7 H

More information

Ch 15: Acids and Bases

Ch 15: Acids and Bases Ch 15: Acids and Bases A c i d s a n d B a s e s C h 1 5 P a g e 1 Homework: Read Chapter 15 Work out sample/practice exercises in the sections, Bonus problems: 39, 41, 49, 63, 67, 83, 91, 95, 99, 107,

More information

Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50

Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50 Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs

More information

AP Chemistry- Acids and Bases General Properties of Acids and Bases. Bases- originally defined as any substance that neutralized an acid

AP Chemistry- Acids and Bases General Properties of Acids and Bases. Bases- originally defined as any substance that neutralized an acid AP Chemistry Acids and Bases General Properties of Acids and Bases Acids Electrolyte Taste Litmus Phenolphthalein React with metals to give off H 2 gas H 2 SO 4 (aq) + Mg (s) MgSO 4 (aq) + H 2 (g) Ionize

More information

Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens.

Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens. Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens 2. Binary acids 3. Oxyacids 4. Carboxylic acid 5. Amines Name the following

More information

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical? MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must

More information

CHM1 Review for Exam 12

CHM1 Review for Exam 12 Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and

More information

Chapter 15 Acids and Bases. Fu-Yin Hsu

Chapter 15 Acids and Bases. Fu-Yin Hsu Chapter 15 Acids and Bases Fu-Yin Hsu Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria To help break down food To activate enzymes that break

More information

Unit 6 Water and Its Properties

Unit 6 Water and Its Properties Unit 6 Water and Its Properties 15.1 Water and Its Properties I. Liquid Water A. Surface Tension 1. Surface Tension a. A force that tends to pull adjacent parts of a liquid's surface together, thereby

More information

Acid-Base (Proton-Transfer) Reactions

Acid-Base (Proton-Transfer) Reactions Acid-Base (Proton-Transfer) Reactions Chapter 17 An example of equilibrium: Acid base chemistry What are acids and bases? Every day descriptions Chemical description of acidic and basic solutions by Arrhenius

More information

Talk in. Arrhenius Acid- Base Definition and ph

Talk in. Arrhenius Acid- Base Definition and ph Talk in. Arrhenius Acid Base Definition and ph When we think of acids, we typically think of the Arrhenius definition. Svante Arrhenius (18591927) Arrhenius Acid = Any compound that increases the hydronium

More information

16. What is the H 3 O + concentration of a solution that has an OH concentration of 1 10 3 M? 1) 1 10 4 M 3) 1 10 11 M

16. What is the H 3 O + concentration of a solution that has an OH concentration of 1 10 3 M? 1) 1 10 4 M 3) 1 10 11 M 1. If the [OH ] = 1 10 4 at 298 K for a given solution, the [H + ] of the solution is equal to 1) 1 10 14 3) 1 10 6 2) 1 10 10 4) 1 10 4 2. Based on Reference Table V, which is the strongest base? 1) NO

More information

An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution. Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

More information

Sketch the model representation of the first step in the dissociation of water. H 2. O (l) H + (aq) + OH- (aq) + H 2. OH - (aq) + H 3 O+ (aq)

Sketch the model representation of the first step in the dissociation of water. H 2. O (l) H + (aq) + OH- (aq) + H 2. OH - (aq) + H 3 O+ (aq) Lesson Objectives Students will: Create a physical representation of the autoionization of water using the water kit. Describe and produce a physical representation of the dissociation of a strong acid

More information

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure

More information

Test 12: Review questions

Test 12: Review questions Name: Wednesday, April 16, 2008 Test 12: Review questions 1. Which reaction represents the process of neutralization? 1. Mg(s) + 2HCl(aq) MgCl 2(aq) + H 2(g) 2. HCl(aq) + KOH(aq) KCl(aq) + H2O(l) 3. Pb(NO

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

Chapter 12: Solutions

Chapter 12: Solutions Chapter 12: Solutions Problems: 3, 5, 8, 12, 14, 16, 22, 29, 32, 41-58, 61-68, 71-74 solution: homogeneous mixture of a solute dissolved in a solvent solute: solvent: component present in smaller amount

More information

1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is:

1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is: 1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is: a) K = [H+ ][NO 2 ] [HNO 2 ] b) K = [H+ ][N][O] 2 [HNO 2 ] c) K =

More information

5. The ph of a solution is 2. If its ph is increased to 6, how many times greater is the [H + ] of the original solution?

5. The ph of a solution is 2. If its ph is increased to 6, how many times greater is the [H + ] of the original solution? IB Chemistry SL Topic 8 Questions 4. Which substance can be dissolved in water to give a 0.1 mol dm 3 solution with a high ph and a high electrical conductivity? A. HCl B. NaCl C. NH 3 D. NaOH 5. The ph

More information

Types of Reactions. What are Acids &Bases? Chapter 15. Acids & Bases. Definition? a) Arrhenius. b) Bronsted-Lowry. c) Lewis

Types of Reactions. What are Acids &Bases? Chapter 15. Acids & Bases. Definition? a) Arrhenius. b) Bronsted-Lowry. c) Lewis Chapter 15. Acids & Bases Acid/Base Definitions Types of Acids/bases Polyprotic Acids The Ion Product for Water The ph and Other p Scales Aqueous Solutions of Acids and Bases Hydrolysis The Common Ion

More information

Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry

Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry AP Chemistry A. Allan Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen's electronegativity is high (3.5) and hydrogen's

More information

From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116)

From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116) Chem 112 Solutions From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116) 1. Which of the following compounds are nonelectrolytes? A. NaF

More information

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points) CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

More information

Chemistry 52. Reacts with active metals to produce hydrogen gas. Have a slippery, soapy feeling. React with carbonates to produce CO 2

Chemistry 52. Reacts with active metals to produce hydrogen gas. Have a slippery, soapy feeling. React with carbonates to produce CO 2 ACID AND BASE STRENGTH Experiment #2 PURPOSE: 1. To distinguish between acids, bases and neutral substances, by observing their effect on some common indicators. 2. To distinguish between strong and weak

More information

Notes: Acids and Bases

Notes: Acids and Bases Name Chemistry Pre-AP Notes: Acids and Bases Period I. Describing Acids and Bases A. Properties of Acids taste ph 7 Acids change color of an (e.g. blue litmus paper turns in the presence of an acid) React

More information

EOC Review Acids Bases and Salts

EOC Review Acids Bases and Salts EOC Review Acids Bases and Salts 1.Identify the Bronsted-Lowry acid and base in each of the following reactions. 2.The hydroxide ion is 3. The hydronium ion is 4.HCl is a strong/weak acid? 5.CH 3 COOH

More information

Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values

Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values increase or decrease? Q2: The range of values of the ph scale is: Q7: As bases become more alkaline, their ph values increase

More information

Chapter 4: Reaction in Aqueous Solution

Chapter 4: Reaction in Aqueous Solution Chapter 4: Reaction in Aqueous Solution What is a Solution? Solute + substance dissolved typically smaller quantity Solvent! dissolving medium typically larger quantity Solution homogeneous mixture variable

More information

Chemistry Ch 15 (Solutions) Study Guide Introduction

Chemistry Ch 15 (Solutions) Study Guide Introduction Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual

More information

Solutions CHAPTER Specific answers depend on student choices.

Solutions CHAPTER Specific answers depend on student choices. CHAPTER 15 1. Specific answers depend on student choices.. A heterogeneous mixture does not have a uniform composition: the composition varies in different places within the mixture. Examples of non homogeneous

More information

Summary of MQ2 Results: Mean =124 (71 %) Hi = 175. Lo = 32. Your scores will be posted on WebCT

Summary of MQ2 Results: Mean =124 (71 %) Hi = 175. Lo = 32. Your scores will be posted on WebCT Summary of MQ2 Results: Mean =124 (71 %) Hi = 175 Lo = 32 Your scores will be posted on WebCT 16.5 Strong Acids and Bases Strong Acids Strong Bases 16.6 Weak Acids Calculating K a from ph Using K a to

More information

Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water.

Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Ch 15-16 Acids and Bases Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base.

More information

CHEM 10123/10125, Exam 2

CHEM 10123/10125, Exam 2 CHEM 10123/10125, Exam 2 March 7, 2012 (50 minutes) Name (please print) Please box your answers, and remember that significant figures, phases (for chemical equations), and units do count! 1. (13 points)

More information

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride. 1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.

More information

Acid-Base Equilibrium

Acid-Base Equilibrium AcidBaseEquil 1 Acid-Base Equilibrium See AqueousIons in Chemistry 1110 online notes for review of acid-base fundamentals! Acid- Base Reaction in Aqueous Salt Solutions Recall that use [ ] to mean concentration

More information

Chapter 4 Three Major Classes of Chemical Reactions. As will likely come as no surprise, chemical reactions can be categorized in a variety of

Chapter 4 Three Major Classes of Chemical Reactions. As will likely come as no surprise, chemical reactions can be categorized in a variety of Chapter 4 Three Major Classes of Chemical Reactions As will likely come as no surprise, chemical reactions can be categorized in a variety of different ways, with nearly all reactions falling into more

More information

Chapter 4 Chemical Reactions and Solution Stoichiometry

Chapter 4 Chemical Reactions and Solution Stoichiometry Chapter 4 In This Chapter The science of chemistry brings three central benefits to society. First, chemistry helps explain how the world works, principally by examining nature on the molecular scale.

More information

Chapter 14 Solutions

Chapter 14 Solutions Chapter 14 Solutions 1 14.1 General properties of solutions solution a system in which one or more substances are homogeneously mixed or dissolved in another substance two components in a solution: solute

More information

14-Jul-12 Chemsheets A

14-Jul-12 Chemsheets A www.chemsheets.co.uk 14-Jul-12 Chemsheets A2 009 1 BRONSTED-LOWRY ACIDS & BASES Bronsted-Lowry acid = proton donor (H + = proton) Bronsted-Lowry base = proton acceptor (H + = proton) Bronsted-Lowry acid-base

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

Chemical Reactions in Water

Chemical Reactions in Water Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Acids, Bases and Salts Acids dissolve in water to give H + ions. These ions attach

More information

3/6/2014. Chapter 15. Acids and Bases. Stomach Acid and Heartburn GERD. Curing Heartburn. Common Acids. Properties of Acids. Lecture Presentation

3/6/2014. Chapter 15. Acids and Bases. Stomach Acid and Heartburn GERD. Curing Heartburn. Common Acids. Properties of Acids. Lecture Presentation Lecture Presentation Chapter 15 Acids and Bases Sherril Soman Grand Valley State University Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria

More information

Name period Unit 9: acid/base equilibrium

Name period Unit 9: acid/base equilibrium Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton

More information

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g) 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

More information

Solutions Review Questions

Solutions Review Questions Name: Thursday, March 06, 2008 Solutions Review Questions 1. Compared to pure water, an aqueous solution of calcium chloride has a 1. higher boiling point and higher freezing point 3. lower boiling point

More information

Topic 8 Acids and bases 6 hours

Topic 8 Acids and bases 6 hours Topic 8 Acids and bases 6 hours Hydronium ion (H3O + ) = more stable form of hydrogen ion (H + ) H + + H2O H3O + 8.1 Theories of acids and bases 2 hours 1. Arrhenius H-X / M-OH ACID a substance that dissociates

More information

Lecture 6: Lec4a Chemical Reactions in solutions

Lecture 6: Lec4a Chemical Reactions in solutions Lecture 6: Lec4a Chemical Reactions in solutions Zumdahl 6 th Ed, Chapter 4 Sections 1-6. 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition

More information

Chapter 4 Chemical Reactions

Chapter 4 Chemical Reactions Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser

More information

CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH

CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides

More information

Lab 9. Colligative Properties an Online Lab Activity

Lab 9. Colligative Properties an Online Lab Activity Prelab Assignment Before coming to lab: Lab 9. Colligative Properties an Online Lab Activity Chemistry 162 - K. Marr Revised Winter 2014 This lab exercise does not require a report in your lab notebook.

More information

1. Identify the Bronsted-Lowry acids and bases and the conjugate acid base pairs in the following reactions.

1. Identify the Bronsted-Lowry acids and bases and the conjugate acid base pairs in the following reactions. Exercise #1 Brønsted-Lowry s and Bases 1. Identify the Bronsted-Lowry acids and bases and the conjugate acid base pairs in the following reactions. (a) HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq) (b) H 2

More information

Acids and Bases. Ch a pt e r Aqueous Equilibria: Chemistry 4th Edition McMurry/Fay. MOH(aq) M + (aq) + OH (aq)

Acids and Bases. Ch a pt e r Aqueous Equilibria: Chemistry 4th Edition McMurry/Fay. MOH(aq) M + (aq) + OH (aq) 15 Ch a pt e r Aqueous Equilibria: Acids and Bases Chemistry th Edition McMurry/Fay Dr. Paul Charlesworth Michigan Technological University AcidBase Concepts 01 Arrhenius Acid: A substance which dissociates

More information

Acid-Base 2/27/2012. Definitions of Acids/Bases. Acid-Base Behavior. Arrhenius Definition. Arrhenius Definition

Acid-Base 2/27/2012. Definitions of Acids/Bases. Acid-Base Behavior. Arrhenius Definition. Arrhenius Definition Acids Taste sour Burn Skin Turn Litmus Red Dissolve metals Citrus fruit Vitamin C (Ascorbic Acid) Vinegar Battery Acid Bases Taste Bitter Behavior Burn Skin/Feel Slippery Turn Litmus Blue Soap Ammonia

More information

CHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

CHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. CHEM 1212 Test II MULTIPLE CHOICE. Choose the one alternative that est completes the statement or answers the question. 1) At 1000 K, the equilirium constant for the reaction is K p = 0.013. 2NO (g) +

More information

4. Acid Base Chemistry

4. Acid Base Chemistry 4. Acid Base Chemistry 4.1. Terminology: 4.1.1. Bronsted / Lowry Acid: "An acid is a substance which can donate a hydrogen ion (H+) or a proton, while a base is a substance that accepts a proton. B + HA

More information