1. 19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1. Lactic acid, HC 3 H 5 O 3, has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate K a. 1.4e-4 Period 1 Day 3 5-7

2. 19.1 Acid-Base Theories> 2 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 3 5-7 1. What is the molarity of a solution of H 3 PO 4 if 15.0 mL is neutralized by 38.5 mL 0.150 M NaOH H 3 PO 4(aq) + 3NaOH (aq)  Na 3 PO 4(aq) + 3H 2 O (l) 0.128 M

3. 19.1 Acid-Base Theories> 3 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. cc Today = lab period 1 Test will be Monday 5-13

4. 19.1 Acid-Base Theories> 4 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. LAB: Standard = Trial # 1 = HCl + NaOH  NaCl + H 2 O HCl = 0.1M 10.2 ml HCl and 10.5 ml NaOH

5. 19.1 Acid-Base Theories> 5 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. B. Buffers Buffer = a solution that resists changes in pH – a solution of a weak acid and one of its salts or a solution of a weak base and one of its salts  a buffer contains one component that can accept hydrogen ions and another component that can donate hydrogen ions, therefore adding hydrogen ions and/or hydroxide ions has little effect on the pH of the solution

6. 19.1 Acid-Base Theories> 6 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. B. Buffers  Example: A solution of carbonic acid and sodium bicarbonate forms a buffer: If you add H + ions: HCO 3 - + H + H 2 CO 3 If you add OH - ions H 2 CO 3 + OH - HCO 3 - + H 2 O

7. 19.1 Acid-Base Theories> 7 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. B. Buffers  Buffer Capacity = the amount of acid or base that can be added to a buffer solution before a significant change in pH occurs (before your H + ion acceptors and/or H + ion donors run out)v

8. 19.1 Acid-Base Theories> 8 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

9. 19.1 Acid-Base Theories> 9 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. B. Buffers  Example Problem: A buffer consists of methanoic acid (HCOOH) and methanoate ion (HCOO - ) Write an equation to show what happens when an acid is added to this buffer. And a base.

10. 19.1 Acid-Base Theories> 10 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Solution ASolution BSolution ASolution B Acid Added 

11. 19.1 Acid-Base Theories> 11 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. page 675 #s 39-43

12. 19.1 Acid-Base Theories> 12 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 5 5-9 1. A buffer consists of carbonic acid (H 2 CO 3 ) and bicarbonate ion (HCO 3 - ) Write an equation to show what happens when an acid is added to this buffer. And a base. HCO 3 - (aq) + H + (aq)  H 2 CO 3(aq) H 2 CO 3(aq) + OH - (aq)  HCO 3 - (aq) + H 2 O (l)

13. 19.1 Acid-Base Theories> 13 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 5 5-9 1. A buffer consists of H 2 PO 4 - ions and HPO 4 -2 ions. Write an equation to show what happens when an acid is added to this buffer. And a base. HPO 4 -2 (aq) + H + (aq)  H 2 PO 4 - (aq) H 2 PO 4 - (aq) + OH - (aq)  HPO 4 -2 (aq) + H 2 O (l)

14. 19.1 Acid-Base Theories> 14 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 5 5-9 1. HNO 3 is a strong acid – assume it completely dissociates in water. Calculate the pH of a solution containing 1.5 grams of HNO 3 in 200 mL of solution. 0.924

15. 19.1 Acid-Base Theories> 15 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 6 5-10 1. Calculate the pH for an aqueous solution in which [OH – ] is 1 × 10 –12 mol/L. Is this solution acidic, basic, or neutral?

16. 19.1 Acid-Base Theories> 16 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 5 5-3 Scheduled tomorrow Friday 5-4 day 6 Test Tuesday 5-8 Day 2  double period NO Double tomorrow Friday 5-4 day 6

17. 19.1 Acid-Base Theories> 17 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 5 5-3 Lab due Friday 5-4 REVIEW!!!

18. 19.1 Acid-Base Theories> 18 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 6 4-26 page 675 #s 39-43 – due tomorrow (Friday 4-27) TEST WILL BE FRIDAY 5-4 DAY 6!!!

19. 19.1 Acid-Base Theories> 19 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Ka =Ka = [H + ] X [NO 3 - ] [HNO 3 ] Ka =Ka = [H + ] X [HSO 3 - ] [H 2 SO 3 ]

20. 19.1 Acid-Base Theories> 20 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. K a = K eq * [H 2 O] = [H 3 O + ] * [CH 3 COO - ] [CH 3 COOH] K b = K eq * [H 2 O] = [NH 4 + ] * [OH - ] [NH 3 ] K b = [conjugate acid] * [OH - ] [base]

21. 19.1 Acid-Base Theories> 21 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. K eq = [NH 4 + ] * [OH - ] [NH 3 ] * [H 2 O]

22. 19.1 Acid-Base Theories> 22 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. The Lewis definition is the broadest. It extends to compounds that the Brønsted-Lowry theory does not classify as acids and bases. Acid-Base Definitions TypeAcidBase ArrheniusH + producerOH – producer Brønsted-LowryH + donorH + acceptor Lewiselectron-pair acceptorelectron-pair donor This table compares the definitions of acids and bases. Interpret Data

23. 19.1 Acid-Base Theories> 23 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Acid-Base Definitions TypeAcidBase Arrhenius Brønsted-Lowry Lewis

24. 19.1 Acid-Base Theories> 24 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day 6 4-26 Arrhenius acid Hydrolysis K w -log[H + ] Lewis base Universal Indicator Titration Bronsted-Lowry acid K a Strong base Concentrated acid Neutralization reaction Standard solution