Cmc chapter 18

Chapter Menu Acids and Bases Section 18.1 Introduction to Acids and Bases Section 18.2 Strengths of Acids and Bases Section 18.3 Hydrogen Ions and pH Section 18.4 Neutralization Exit Click a hyperlink or folder tab to view the corresponding slides.

Section 18-1 Section 18.1 Introduction to Acids and Bases ,[object Object],Lewis structure: a model that uses electron-dot structures to show how electrons are arranged in molecules ,[object Object],[object Object]

Section 18-1 Section 18.1 Introduction to Acids and Bases (cont.) acidic solution basic solution Arrhenius model Brønsted-Lowry model conjugate acid Different models help describe the behavior of acids and bases. conjugate base conjugate acid-base pair amphoteric Lewis model

Section 18-1 Properties of Acids and Bases ,[object Object],[object Object],[object Object]

Section 18-1 Properties of Acids and Bases (cont.) ,[object Object],[object Object],[object Object],[object Object]

Section 18-1 Properties of Acids and Bases (cont.) ,[object Object],[object Object],[object Object]

Section 18-1 The Arrhenius Model ,[object Object]

Section 18-1 The Arrhenius Model (cont.) ,[object Object],[object Object],[object Object],[object Object],[object Object],[object Object]

Section 18-1 The Brønsted-Lowry Model ,[object Object],[object Object]

Section 18-1 The Brønsted-Lowry Model (cont.) ,[object Object],[object Object],[object Object]

Section 18-1 The Brønsted-Lowry Model (cont.) ,[object Object],[object Object],[object Object],[object Object]

Section 18-1 Monoprotic and Polyprotic Acids ,[object Object],[object Object]

Section 18-1 Monoprotic and Polyprotic Acids (cont.) ,[object Object]

Section 18-1 The Lewis Model ,[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Section 18-1 Section 18.1 Assessment A Lewis acid is a(n) ____. A. electron pair donor B. hydrogen ion donor C. electron pair acceptor D. substance that contains an hydroxide group

[object Object],[object Object],[object Object],[object Object],Section 18-1 Section 18.1 Assessment A conjugate acid is formed when: A. a base accepts a hydrogen ion B. an acid accepts a hydrogen ion C. an acid donates a hydrogen ion D. a base donates a hydrogen ion

Section 18-2 Section 18.2 Strengths of Acids and Bases ,[object Object],electrolyte: an ionic compound whose aqueous solution conducts an electric current ,[object Object],[object Object]

Section 18-2 Section 18.2 Strengths of Acids and Bases (cont.) strong acid weak acid acid ionization constant strong base weak base base ionization constant In solution, strong acids and bases ionize completely, but weak acids and bases ionize only partially.

Section 18-2 Strengths of Acids ,[object Object],[object Object]

Section 18-2 Strengths of Acids (cont.) ,[object Object]

Section 18-2 Strengths of Acids (cont.) ,[object Object],[object Object],[object Object]

Section 18-2 Strengths of Acids (cont.) ,[object Object],[object Object]

Section 18-2 Strengths of Bases ,[object Object],[object Object]

Section 18-2 Strengths of Bases (cont.) ,[object Object]

[object Object],[object Object],[object Object],[object Object],Section 18-2 Section 18.2 Assessment A solution with a small K b is a ____. A. weak acid B. weak base C. strong acid D. strong base

[object Object],[object Object],[object Object],[object Object],Section 18-2 Section 18.2 Assessment Where is the equilibrium point in the ionization equation for a strong acid? A. far right B. far left C. slightly right D. slightly left

Section 18-3 Section 18.3 Hydrogen Ions and pH ,[object Object],Le Châtelier’s principle: states that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress ion product constant for water pH pOH ,[object Object],[object Object],pH and pOH are logarithmic scales that express the concentrations of hydrogen ions and hydroxide ions in aqueous solutions.

Section 18-3 Ion Product Constant for Water ,[object Object],[object Object],[object Object]

Section 18-3 Ion Product Constant for Water (cont.) ,[object Object],[object Object],[object Object]

Section 18-3 pH and pOH ,[object Object],[object Object]

Section 18-3 pH and pOH (cont.) ,[object Object],[object Object],[object Object]

Section 18-3 pH and pOH (cont.) ,[object Object]

[object Object],[object Object],[object Object],[object Object],Section 18-3 Section 18.3 Assessment In dilute aqueous solution, as [H + ] increases: A. pH decreases B. pOH increases C. [OH – ] decreases D. all of the above

[object Object],[object Object],[object Object],[object Object],Section 18-3 Section 18.3 Assessment What is the pH of a neutral solution such as pure water? A. 0 B. 7 C. 14 D. 1.0 × 10 –14

Section 18-4 Section 18.4 Neutralization ,[object Object],stoichiometry: the study of quantitative relationships between the amounts of reactants used and products formed by a chemical reaction; is based on the law of conservation of mass ,[object Object],[object Object]

Section 18-4 Section 18.4 Neutralization (cont.) neutralization reaction salt titration titrant equivalence point In a neutralization reaction, an acid reacts with a base to produce a salt and water. acid-base indicator end point salt hydrolysis buffer buffer capacity

Section 18-4 Reactions Between Acids and Bases ,[object Object],[object Object],[object Object]

Section 18-4 Reactions Between Acids and Bases (cont.)

Section 18-4 Reactions Between Acids and Bases (cont.) ,[object Object]

Section 18-4 Reactions Between Acids and Bases (cont.) ,[object Object],[object Object]

Section 18-4 Salt Hydrolysis ,[object Object]

Section 18-4 Salt Hydrolysis (cont.) ,[object Object],[object Object],[object Object]

Section 18-4 Salt Hydrolysis (cont.) ,[object Object],[object Object],[object Object],[object Object]

Section 18-4 Buffered Solutions ,[object Object],[object Object]

Section 18-4 Buffered Solutions (cont.) ,[object Object],[object Object],[object Object]

Section 18-4 Buffered Solutions (cont.) ,[object Object],[object Object]

Section 18-4 Buffered Solutions (cont.) ,[object Object]

[object Object],[object Object],[object Object],[object Object],Section 18-4 Section 18.4 Assessment In a neutralization reaction, an acid and base react to form: A. salt and oxygen gas B. salt and ammonia C. salt and water D. precipitate and water

[object Object],[object Object],[object Object],[object Object],Section 18-4 Section 18.4 Assessment Solutions that resist changes in pH are called ____. A. titrants B. salts C. conjugate pairs D. buffers

Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion

Study Guide 1 Section 18.1 Introduction to Acids and Bases Key Concepts ,[object Object],[object Object],[object Object],[object Object]

Study Guide 2 Section 18.2 Strengths of Acids and Bases Key Concepts ,[object Object],[object Object]

Study Guide 3 Section 18.3 Hydrogen Ions and pH Key Concepts ,[object Object],[object Object],[object Object]

Study Guide 4 Section 18.4 Neutralization Key Concepts ,[object Object],[object Object],[object Object],[object Object]

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 1 Which type of acid accepts an electron pair? A. Arrhenius B. Brønsted-Lowry C. Lewis D. Dalton

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 2 What is the conjugate of a weak acid? A. strong acid B. strong base C. weak acid D. weak base

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 3 In a solution with a pH of 4.0, which of the following is true? A. [H + ] > [OH – ] B. [H + ] < [OH – ] C. [H + ] = [OH – ] D. none of the above

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 4 Salt hydrolysis is what type of reaction? A. single-replacement B. double replacement C. synthesis D. decomposition

[object Object],[object Object],[object Object],[object Object],Chapter Assessment 5 The strength of a weak acid is measured by: A. ion product constant B. base ionization constant C. pOH D. acid ionization constant

[object Object],[object Object],[object Object],[object Object],STP 1 What is the pOH of 0.250M HBr, a strong acid? A. 0.60 B. 0.80 C. 13.4 D. 13.2

[object Object],[object Object],[object Object],[object Object],STP 2 Which of the following is a diprotic acid? A. CH 2 COOH B. HCl C. NH 3 + D. H 2 SO 4

[object Object],[object Object],[object Object],[object Object],STP 3 What is the conjugate acid in the following equation? HCl(s) + H 2 O -> H 3 O + (aq) + Cl – (aq) A. Cl – B. H 3 O + C. H 2 O D. HCl

[object Object],[object Object],[object Object],[object Object],STP 4 An increase in concentration of hydrogen ions when hydroxide ions are added to an aqueous solution is an example of: A. an Arrhenius acid B. a Brønsted-Lowry acid C. the equivalence point D. Le Châtelier’s Principle

[object Object],[object Object],[object Object],[object Object],STP 5 Which of the following is a polar molecule? A. CH 4 B. PCl 5 C. H 2 O D. H 2

IB Menu Click on an image to enlarge.

CIM Table 18.2 Three Models for Acids and Bases Table 18.3 Ionization Equations Figure 18.20 A Neutralization Reaction Figure 18.21 Titration Figure 18.22 Neutralization Reactions

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Cmc chapter 18

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Cmc chapter 18