1. Acids and Bases

2. Properties of Acids and Bases

3. Properties of Acids and Bases

4. Properties of Acids and Bases
Sour to taste
Reactive
Corrosive
Electrolytes
Bitter to taste
Slippery
Corrosive
Electrolytes

5. Acid Base Nomenclature

6. Acid Nomenclature
Rule 1:
Acids based on anions whose name ends in –ide have associated acids that have the hydro- prefix and –ic ending

7. Acid Nomenclature
Rule 2:
Acids based on anions whose name ends in –ate have associated acids that have an –ic ending

8. Acid Nomenclature
Rule 3:
Acids based on anions whose names end in –ite have associated acids that have an –ous ending

9. Naming Bases
You can already do this
Examples:
Ca(OH)2
NH3

10. 3 Models of Acid- Base Behavior

11. Arrhenius Model
Base
Acid
a substance that increases the concentration of H+ in aqueous solution
HCl(aq)  H+ + Cl-
a substance that increases the concentration of OH- in aqueous solution
NaOH(aq)  Na+ + OH-

12. Bronsted-Lowry Model molecule or ion that donates a proton (H+)
Acid
Base
molecule or ion that donates a proton (H+)
molecule or ion that accepts a proton (H+)

13. Amphoteric (amphiprotic)
Substance that can act as an acid or base

14. Lewis Model atom, ion, or molecule that accepts an electron pair
Acid
Base
atom, ion, or molecule that accepts an electron pair
atom, ion, or molecule that donates an electron pair

15. The pH Scale

16. Self-Ionization of water
Two water molecules produce a hydronium ion and hydroxide ion by transfer of a proton
Kw = [H3O+][OH-] = 1.0x10-14

17. Neutral, Basic, Acidic?
Neutral: when [H3O+] = [OH-]
Basic: [H3O+] < [OH-]
Acidic: [H3O+] > [OH-]

18. Neutral, Basic, Acidic?

19. The pH Scale
Ranges from 0-14
Less than 7 is acidic, 7 is neutral, more than 7 is basic

20. The pH Scale -The lower the pH, the higher the concentration of H+
Ranges from 0-14
pH= -log [H3O+]
pOH = -log [OH-]
pH + pOH= 14

21. The pH Scale
Important Formulas:
pH= -log [H+]
pOH = -log [OH-]
pH + pOH= 14
[H+] = 10-pH
[OH-] = 10-pOH

22. The pH Scale

23. pH of Strong Acids and Bases
Strong Acids completely ionize
Calculate pH from [H+]

24. pH of Strong Acids and Bases
Strong Bases completely ionize
Calculate the pOH from the concentration of [OH-], then calculate pH

25. Titrations

26. Neutralization Reactions
Acid + Base  Salt + Water
Salt = cation of base plus anion of acid

27. Titrations
Titration is the controlled addition and measurement of the amount of solution of known concentration required to react completely with a measured amount of a solution of unknown concentration

28. Titrations
Equivalence point
- the point at which two solutions used in titration are present in chemically equivalent amounts
- In an acid –base titration mole H+ = mole OH-

29. Titrations Acid –Base indicators
- compounds whose colors are sensitive to pH

30. Titrations
End point
= the point in a titration at which an indicator changes color.

31. Titrations
Acid –Base indicators

32. Titrations

33. Titrations

34. Determining the molarity of unknown solution by titration
Titrations
Determining the molarity of unknown solution by titration
1. Write the rxn
2. determine moles neutralized using stoich
3. Divide moles by volume of unknown to calculate molarity

35. Titrations
In a titration 27.4mL of M Ba(OH)2 is added to a 20.0mL sample of HCl solution of unknown concentration. What is the molarity of the acid solution?