1. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company CHAPTER 2 Water, pH, and Ionic Equilibria to accompany Biochemistry, 2/e by Reginald Garrett and Charles Grisham All rights reserved. Requests for permission to make copies of any part of the work should be mailed to: Permissions Department, Harcourt Brace & Company, 6277 Sea Harbor Drive, Orlando, Florida 32887-6777

2. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Outline 2.1 Properties of Water 2.2 pH 2.3 Buffers 2.4 Water's Unique Role in the Fitness of the Environment

3. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Properties of Water High b.p., m.p., heat of vaporization, surface tension Bent structure makes it polar Non-tetrahedral bond angles H-bond donor and acceptor Potential to form four H-bonds per water

4. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

5. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Comparison of Ice and Water Issues: H-bonds and Motion Ice: 4 H-bonds per water molecule Water: 2.3 H-bonds per water molecule Ice: H-bond lifetime - about 10 microsec Water: H-bond lifetime - about 10 psec (10 psec = 0.00000000001 sec) Thats "one times ten to the minus eleven second"!

6. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

7. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

8. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Solvent Properties of Water Ions are always hydrated in water and carry around a "hydration shell" Water forms H-bonds with polar solutes Hydrophobic interactions - a "secret of life"

9. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

10. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Hydrophobic Interactions A nonpolar solute "organizes" water The H-bond network of water reorganizes to accommodate the nonpolar solute This is an increase in "order" of water This is a decrease in ENTROPY

11. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

12. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Amphiphilic Molecules Also called "amphipathic" Refers to molecules that contain both polar and nonpolar groups Equivalently - to molecules that are attracted to both polar and nonpolar environments Good examples - fatty acids

13. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

14. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

15. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

16. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Acid-base Equilibria The pH Scale A convenient means of writing small concentrations: pH = -log 10 [H + ] Sørensen (Denmark) If [H + ] = 1 x 10 -7 M Then pH = 7

17. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

18. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

19. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

20. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Dissociation of Weak Electrolytes Consider a weak acid, HA The acid dissociation constant is given by: HA  H + + A - K a = [ H + ] [ A - ] ____________________ [HA]

21. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company The Henderson-Hasselbalch Equation Know this! You'll use it constantly. For any acid HA, the relationship between the pK a, the concentrations existing at equilibrium and the solution pH is given by: pH = pK a + log 10 [A ¯ ] ¯¯¯¯¯¯¯¯¯¯ [HA]

22. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

23. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Consider the Dissociation of Acetic Acid Assume 0.1 eq base has been added to a fully protonated solution of acetic acid The Henderson-Hasselbalch equation can be used to calculate the pH of the solution: With 0.1 eq OH ¯ added: pH = pK a + log 10 [0.1 ] ¯¯¯¯¯¯¯¯¯¯ [0.9] pH = 4.76 + (-0.95) pH = 3.81

24. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Consider the Dissociation of Acetic Acid Another case.... What happens if exactly 0.5 eq of base is added to a solution of the fully protonated acetic acid? With 0.5 eq OH¯ added: pH = pK a + log 10 [0.5 ] ¯¯¯¯¯¯¯¯¯¯ [0.5] pH = 4.76 + 0 pH = 4.76 = pK a

25. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Consider the Dissociation of Acetic Acid A final case to consider.... What is the pH if 0.9 eq of base is added to a solution of the fully protonated acid? With 0.9 eq OH¯ added: pH = pK a + log 10 [0.9 ] ¯¯¯¯¯¯¯¯¯¯ [0.1] pH = 4.76 + 0.95 pH = 5.71

26. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

27. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

28. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company Buffers Buffers are solutions that resist changes in pH as acid and base are added Most buffers consist of a weak acid and its conjugate base Note in Figure 2.15 how the plot of pH versus base added is flat near the pK a Buffers can only be used reliably within a pH unit of their pK a

29. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

30. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

31. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company

32. Biochemistry 2/e - Garrett & Grisham Copyright © 1999 by Harcourt Brace & Company