Chapter TenOutlineGoalsGoals Contd.10.1 Acids and Bases in Aqueous SolutionSlide 610.2 Some Common Acids and BasesSlide 810.3 The Brønsted-Lowry Definition of Acids and BasesSlide 10Slide 1110.4 Water as Both an Acid and a BaseSlide 1310.5 Acid and Base StrengthSlide 15Slide 1610.6 Acid Dissociated ConstantsSlide 1810.7 Dissociation of Water10.8 Measuring Acidity in Aqueous Solution: pHSlide 2110.9 Working with pH10.10 Laboratory Determination of AciditySlide 2410.11 Buffer SolutionsSlide 2610. 12 Buffers in the BodySlide 28Slide 2910.13 Acid and Base EquivalentsSlide 31Slide 3210.14 Some Common Acid-Base ReactionsSlide 3410.15 TitrationSlide 36Slide 3710.16 Acidity and Basicity of Salt SolutionsSlide 39Chapter SummaryChapter Summary Contd.Slide 42Key WordsKey Words Contd.Slide 45Chapter TenAcids and BasesFundamentals of General, Organic and Biological Chemistry 6th EditionJames E. MayhughCopyright © 2010 Pearson Education, Inc.Copyright © 2010 Pearson Education, Inc.Chapter Ten2Outline►10.1 Acids and Bases in Aqueous Solution►10.2 Some Common Acids and Bases►10.3 The Brønsted–Lowry Definition of Acids and Bases►10.4 Water as Both an Acid and a Base►10.5 Acid and Base Strength►10.6 Acid Dissociation Constants►10.7 Dissociation of Water►10.8 Measuring Acidity in Aqueous Solution: pH►10.9 Working with pH►10.10 Laboratory Determination of Acidity►10.11 Buffer Solutions►10.12 Buffers in the Body►10.13 Acid and Base Equivalents►10.14 Some Common Acid–Base Reactions►10.15 Titration►10.16 Acidity and Basicity of Salt SolutionsCopyright © 2010 Pearson Education, Inc.Chapter Ten3Goals►1. What are acids and bases? Be able to recognize acids and bases and write equations for common acid–base reactions.►2. What effect does the strength of acids and bases have on their reactions? Be able to interpret acid strength using acid dissociation constants Ka and predict the favored direction of acid–base equilibria.►3. What is the ion-product constant for water? Be able to write the equation for this constant and use it to find the concentration of H3O+ or OH- .Copyright © 2010 Pearson Education, Inc.Chapter Ten4Goals Contd.►4. What is the pH scale for measuring acidity? Be able to explain the pH scale and find pH from the H3O+ concentration.►5. What is a buffer? Be able to explain how a buffer maintains pH and how the bicarbonate buffer functions in the body.►6. How is the acid or base concentration of a solution determined? Be able to explain how a titration procedure works and use the results of a titration to calculate acid or base concentration in a solution.Copyright © 2010 Pearson Education, Inc.Chapter Ten510.1 Acids and Bases in Aqueous Solution►An acid is a substance that produces hydrogen ions, H+, when dissolved in water. (Arrhenius definition)►Hydronium ion: The H3O+ ion formed when an acid reacts with water.Copyright © 2010 Pearson Education, Inc.Chapter Ten6►A base is a substance that produces hydroxide ions, OH-, when dissolved in water. (Arrhenius definition) ►Bases can be metal hydroxides that release OH- ions when they dissolve in water or compounds that undergo reactions with water that produce OH- ions.Copyright © 2010 Pearson Education, Inc.Chapter Ten710.2 Some Common Acids and Bases►Sulfuric acid, H2SO4 , is manufactured in greater quantity than any other industrial chemical. It is the acid found in automobile batteries. ►Hydrochloric acid, HCl, is “stomach acid” in the digestive systems of most mammals.►Phosphoric acid, H3PO4 , is used to manufacture phosphate fertilizers. The tart taste of many soft drinks is due to the presence of phosphoric acid.►Nitric acid, HNO3 , is a strong oxidizing agent that is used for many purposes.►Acetic acid, CH3CO2H, is the primary organic constituent of vinegar.Copyright © 2010 Pearson Education, Inc.Chapter Ten8►Sodium hydroxide, NaOH, or lye, is used in the production of aluminum, glass, and soap. Drain cleaners often contain NaOH because it reacts with the fats and proteins found in grease and hair.►Calcium hydroxide, Ca(OH)2 , or slaked lime, is made industrially by treating lime (CaO) with water. It is used in mortars and cements. An aqueous solution of is often called limewater.►Magnesium hydroxide, Mg(OH)2 , or milk of magnesia, is an additive in foods, toothpaste, and many over-the-counter medications. Many antacids contain magnesium hydroxide.►Ammonia, NH3 , is used primarily as a fertilizer. A dilute solution of ammonia is frequently used around the house as a glass cleaner.Copyright © 2010 Pearson Education, Inc.Chapter Ten910.3 The Brønsted-Lowry Definition of Acids and Bases►A Brønsted–Lowry acid can donate H+ ions.►Monoprotic acids can donate 1 H+ ion, diprotic acids can donate 2 H+ ions, and triprotic acids can donate 3 H+ ions.Copyright © 2010 Pearson Education, Inc.Chapter Ten10►A Brønsted–Lowry base accepts H+ ions.►Putting the acid and base definitions together, an acid–base reaction is one in which a proton is transferred. The reaction need not occur in water.Copyright © 2010 Pearson Education, Inc.Chapter Ten11►Conjugate acid–base pair: Two substances whose formulas differ by only a hydrogen ion, H+.►Conjugate base: The substance formed by loss of H+ from an acid. ►Conjugate acid: The substance formed by addition of H+ to a base.Copyright © 2010 Pearson Education, Inc.Chapter Ten1210.4 Water as Both an Acid and a Base►Water is neither an acid nor a base in the Arrhenius sense because it does not produce appreciable concentrations of either H+ or OH- . In the Brønsted–Lowry sense water is both an acid and a base.►In its reaction with ammonia, water donates H+ to ammonia to form the ammonium ion.Copyright © 2010 Pearson Education, Inc.Chapter Ten13►When water reacts as a Brønsted–Lowry base, it accepts H+ from an acid like HCl. ►Substances like water, which can react as either an acid or a base depending on the circumstances, are said to be amphoteric.Copyright © 2010 Pearson Education, Inc.Chapter Ten1410.5 Acid and Base Strength►Strong acid: An acid that gives up H+ easily and is essentially 100% dissociated in water.►Dissociation: The splitting apart of an acid in water to give H+ and an anion.►Weak acid: An acid that gives up H+ with difficulty and is less than 100% dissociated in water.►Weak base: A base that has only a slight affinity for H+ and holds it weakly.