1. 1 Some Properties of Acids þ Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) þ Taste sour þ React with metals to produce hydrogen gas þ Electrolytes þ React with bases to form a salt and water þ pH is less than 7 þ Turns blue litmus paper to red

2. 2 What do acids do?

3. 3 Some Common Acids HClhydrochloric acid HNO 3 nitric acid H 2 SO 4 sulfuric acid H 3 PO 4 phosphoric acid H 2 CO 3 carbonic acid

4. 4 Strong Acids Strong acids completely ionize in water. For every mole of acid, there will be 1 mole of H +, so the concentration of H + will be the same as the concentration of the acid. For Example: HCl  H+ + Cl- [0.03 M] [0.03M] [0.03 M]

5. 5 Strong Acids HCl, HI, HBr, HNO 3, H 2 SO 4, HClO 4

6. 6 Weak Acids All weak acids form equilibrium systems in solution. For example: H 2 CO 3 (aq) H+ (aq) + HCO 3 (aq) Since we have an equilibrium system, an equilibrium constant (Ka) can be written: Ka = __[H+] [A-]___ [HA]

7. 7 Some Properties of Bases  Produce OH - ions in water  Taste bitter, chalky  Are electrolytes  Feel soapy, slippery  React with acids to form salts and water  pH greater than 7  Turns red litmus paper to blue “Basic Blue”

8. 8 Some Common Bases NaOHsodium hydroxidelye KOHpotassium hydroxideliquid soap Ba(OH) 2 barium hydroxidestabilizer for plastics Mg(OH) 2 magnesium hydroxide“MOM” Milk of magnesia Al(OH) 3 aluminum hydroxideMaalox (antacid)

9. 9 Strong Bases Strong bases completely ionize in water. For every mole of a base, there will be 1 mole of OH -, so the concentration of OH - will be the same as the concentration of the base. For Example: NaOH  Na+ + OH- [0.03 M] [0.03M] [0.03 M]

10. 10 Strong Bases NaOH, KOH, LiOH, RbOH, CsOH, Ca(OH) 2, Ba(OH) 2, Sr(OH) 2 Strong bases completely ionized in water.

11. 11 HNO 3, HCl, H 2 SO 4 and HClO 4 are among the only known strong acids. Strong versus Weak Acids/Bases The strength of an acid (or base) is determined by the amount of IONIZATION.

12. 12 Categorizing Acids/Bases: Weak versus Strong Weak acids and bases do not completely ionize in water. Strong acids and bases completely ionize in water.

13. 13 Acids and Bases Theories

14. 14 Arrhenius Acids and Bases Acids – produce H + ions (or hydronium ions H 3 O + ) Bases – produce OH - ions (problem: some bases don’t have hydroxide ions!)

15. 15 Arrhenius acid is a substance that produces H + (H 3 O + ) in water Arrhenius base is a substance that produces OH - in water

16. 16 Brønsted – Lowry Acids and Bases Acids – proton donor Bases – proton acceptor A “proton” is really just a hydrogen atom that has lost it’s electron!

17. 17 A Brønsted-Lowry acid is a proton donor A Brønsted-Lowry base is a proton acceptor acid conjugate base base conjugate acid

18. 18 Bronsted-Lowry Definition a. NH 3(g) + H 3 O + (aq) → NH 4 + (aq) + H 2 O b. CH 3 OH (l) + NH 2 - (aq) → CH 3 O - (aq) + NH 3(g) c. OH - (aq) + H 3 O + (aq) → H 2 O + H 2 O

19. 19 Lewis Acids and Bases Lewis acid - a substance that accepts an electron pair Lewis base - a substance that donates an electron pair

20. 20 The pH Scale

21. 21

22. 22 Calculating pH and pOH pH = -log [H + ] pOH = -log [OH - ]

23. 23

24. 24 pH [H + ] [OH - ] pOH

25. 25 Neutralization Acid + Base –Ex: HCl + NaOH  NaCl + H 2 O HNO 3 + KOH  KNO 3 + H 2 O Neutralizations always result in a ________ and __________. salt water

26. 26 Base Ex.

27. Closing Acid, Base, or Both?

28. Slippery

29. Soap

30. Tastes sour

31. Ca(OH) 2

32. Conducts electricity

33. Corrosive to skin

34. Examples include citrus fruits.

35. H 2 SO 4

36. HNO 3

37. Forms the H3O + ion when dissolved in water

38. Ionizes in water.

39. HCl

40. Litmus paper turns red

41. Forms the OH ion when dissolved in water

42. pH < 7

43. pH > 7

44. Baking soda

45. Bitter taste

46. NaOH