1. Chapter 13: Acids & Bases “The end is near”

2. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases A. Properties of Acids and Bases –1. Acids Ionize when put into water React with active metals (Group I, II) to produce Hydrogen gas Neutralized with bases Have a sour taste Found in citrus fruits, vinegar, soda pH 0-7

3. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases –2. Bases Ionize when put into water Neutralized with acids Have a bitter taste Feel Slippery Found in soaps, cleaners, antacids, etc. pH 7-14

4. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases B. Arrhenius Definitions of Acids and Bases –1. Acids Produces H + in soln; formula starts with H –2. Bases Produces OH - in soln; formula ends with OH –3. Another definition needed Too many substances that didn’t fit the definition so it needed to be expanded

5. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases C. Bronsted-Lowry Model –1. Definitions Acid = Proton (Hydrogen) Donor Base = Proton (Hydrogen) Acceptor

6. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases –2. Conjugate acid The substance formed from the base –3. Conjugate base The substance formed from the acid

7. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases –4. Acid-Base Pairs Acid and its conjugate base -or- Base and its conjugate acid –5. Generalized equation: H—X + B X -1 + HB +1 Acid Base CB CA

8. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases Example 15L.1 Write the Bronsted Lowry equations for the weak acid HNO 2 and the weak base NH 3, identifying the conjugate acid-base pairs in each equilibrium. (react with water)

9. 13.1 The Arrhenius and Bronsted-Lowry Theories of Acids and Bases Example 15L.2 Write the equilibrium expressions for the interactions between NH 3 and HCO 3 1- and between H 3 PO 4 and H 2 O, identifying the conjugate acid-base pairs in each equation.

10. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases –8. Amphiprotic species Substances that can ionize as either an acid or a base depending on the properties of the other species in soln; can have properties of acid or base

11. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases –9. Acid ionization constant Keq expression for an acid dissociation –10. Base ionization constant Keq expression for a base dissociation

12. 13.1 The Arrhenius and Bronsted- Lowry Theories of Acids and Bases –11. Relative strengths of acids and bases –Strong acids: Br I Cl SO NO ClO (4, 3, 4) –Strong bases: Group I except 1 st one and group II except 1 st two –All other acids and bases are considered weak

13. 13.2 Self-Ionization of Water, The pH Scale A. Water dissociation constant –1. In water solution H 2 O (l) + H 2 O (l)  H 3 O + (aq) + OH - (aq) acid base CB CA OR:H 2 O (l)  H +1 (aq) + OH -1 (aq) –2. For any sample of water molecules: 2 H 2 O (l)  H 3 O + (aq) + OH - (aq)

14. 13.2 Self-Ionization of Water, The pH Scale –3. K eq = [H + ] [OH - ] –4. K w = 1.0x10 -14 –5. Neutral solution [H + ]=[OH - ]=1.0x10 -7

15. –6. Acid solution [H+] > 1x10 -7 7. Basic Solution [H+] < 1x10 -7

16. 13.3 Self-Ionization of Water, The pH Scale Example 15.3 A sample of tap water has a [H + ] = 2.8 x 10 -6 M. What is the [OH - ]?

17. 13.3 The pH scale pH and pOH 1. Definition “The Potential of Hydrogen” pH = -log [H + ]

18. 13.3 Self-Ionization of Water, The pH Scale –2. Size of pH Ranges from 0 to 14 0~7 = ACID 7~14 = BASE 7 = Neutral –3. pOH definition pOH = -log [OH - ] –4. pH and pOH relationship pH + pOH = 14

19. 13.3 Self-Ionization of Water, The pH Scale Example 15.L4 Calculate the pH and pOH of a 0.25 M phosphoric acid solution whose [H + ] is 0.040M. NOTE – the concentration of H + is much lower than the molarity, weak acids don’t completely dissociate

20. 13.3 Self-Ionization of Water, The pH Scale Example 15.L5 Calculate the pH and pOH of a 0.010 M formic acid solution whose [H + ] is 1.8 x 10 -4 M. NOTE – the concentration of H + is much lower than the molarity, weak acids don’t completely dissociate

21. 13.3 The pH Scale –7. pH of strong acids and strong bases a. Strong acids and bases dissociate completely in aqueous solution: HCl (aq)  H +1 (aq) +Cl -1 (aq) over 99% ions Single headed arrow

22. 13.3 Self-Ionization of Water, The pH Scale Example 15L.6 Calculate the [H + ], pH, and [OH - ] of a 0.15M solution of the strong acid, HNO 3.

23. 13.3 The pH Scale c. Strong bases completely dissociate in aqueous solution: NaOH (aq)  Na +1 (aq) + OH -1 (aq) over 99% ions Single headed arrow

24. 15.3 The pH Scale Example 15L.7 State the pH, pOH, [H + ], and [OH - ] of a solution made by dissolving 5.00 g of Ba(OH) 2 - a strong base - in 1.00 L of water.

25. 13.4-5 Equilibrium Solutions of Weak Acids and Weak Bases A. Weak Acids and Dissociation Constants –1. Weak acids are partly dissociated in water solution: CH 3 COOH (aq)  H +1 (aq) +CH 3 COO -1 (aq) over 99% molecules Double headed arrow/reversible reaction

26. 13.4-5 Equilibrium Solutions of Weak Acids and Weak Bases –2. K a = Acid dissociation constant CH 3 COOH (aq)  H +1 (aq) + CH 3 COO -1 (aq) –3. Size of K a values Large K a values = lots of protons given off = relatively “strong” acid Small K a values = few protons given off = very little dissociation If K a is smaller than 10 -4, “x” is negligible in an IRE –For quadratic approximations only!

27. 13.4-5 Equilibrium Solutions of Weak Acids and Weak Bases –4. pKa pK a = -log K a

28. 13.4-5 Equilibrium Solutions of Weak Acids and Weak Bases 5. Example 15L.8 Nicotinic acid is a monoprotic acid (only one ionizable H) and another name for the vitamin, niacin. Minute quantities of this substance are found in all living cells. When 0.10 mole of nicotinic acid, HC 6 H 4 NO 2, is dissolved in enough water to make 1.00 L of solution, the pH is found to be 2.92. Calculate the K a for this acid. What is the percent dissociation of this acid?

29. Continued What is the percent dissociation of this acid?

30. 15.4 Equilibrium Solutions of Weak Acids and Weak Bases 6. Example 15L.9 Propionic acid, which occurs in dairy products, is a weak acid often abbreviated Hpro. If 0.10 mole of this acid is mixed with enough water to make 1.00 L of solution, calculate the pH of the solution. K a = 1.3 x 10 -5.

31. 15.4 Equilibrium Solutions of Weak Acids and Weak Bases B. Weak Bases and their Dissociation Constants –1. Two types of substances act like weak bases in aqueous solution: Nitrogen-containing compounds –Ex. NH 3 Anions of acids –Ex. HCO 3 -

32. 15.4 Equilibrium Solutions of Weak Acids and Weak Bases 2. Example 15L.10 Write the dissociation equilibria that show how each of the following acts like a weak base in aqueous solution: CN 1-, PO 4 3-, S 2-.

33. 15.4 Equilibrium Solutions of Weak Acids and Weak Bases –3. Equilibrium constant for a weak base, K b Base dissociation constant Ex. PO 4 -3

34. 15.4 Equilibrium Solutions of Weak Acids and Weak Bases 4. Example 15L.11 Calculate the [OH - ], [H + ] and pH of a 0.75 M solution of carbonate ion which has a K b of 2.1 x 10 -4.

35. 15.4 Equilibrium Solutions of Weak Acids and Weak Bases –5. Relationship between K a and K b K a x K b = K w = 1.0 x 10 -14 pK a x pK b = pK w = 14.0

36. 15.4 Equilibrium Solutions of Weak Acids and Weak Bases 6. Example 15L.12 Propionic acid, HPro, has a K a of 1.3 x 10 -5. Calculate the K b for the propionate ion, Pro -.

37. Polyprotic Acids 1. Definition and examples –Acid that gives off more than 1 H + when put into water 1 st Proton usually given off rapidly Subsequent protons are given off with increasing difficulty (stronger bases at each step) 2. Phosphoric acid H 3 PO 4 = 3 H’s means polyprotic, specifically triprotic

38. 13.6 Neutralization Reactions and Titration Curves for Strong Acids and Bases 1. Definitions –Complete dissociations No need to worry about K a or K b –Strong Acid + Strong Base --> H 2 O + Salt –(JUST LIKE THE TITRATION LAB WE DID THIS WEEK) 2. Equation – (#H + ) M a V a = M b V b (#OH - )

39. 15.10 Neutralization Reactions and Titration Curves for Strong Acids and Bases 3. Curve –Graph of pH versus volume of titrant from a buret –Shows us where the equivalence point of the neutralization reaction is located

40. HOMEWORK: Worksheets from other book: Chapter 19 pages 109-110 and 113 You can use the books on the counter next to ours, this is from that book.