2. Things to Ponder The nicest thing about the future is that it always starts tomorrow.

3. Deal with the faults of others as gently as with your own!

5. Acid-Bases Lesson2

6. Acid Reactions

7. Problem How would you prepare 5.0 L of a 1.5 M solution of glucose? First chemical formula for glucose is ? C 6 H 12 O 6

8. Work Find the molar mass of glucose Molar mass of glucose = 180.18 g C 6 H 12 O 6

9. Work Cont 1.5 mol C 6 H 12 O 6 180.18 g C 6 H 12 O 6 5.0 L solution 1 L solution 1 mol C 6 H 12 O 6 Answer= 1351.35 g C 6 H 12 O 6 Write as Put 1351.35 g C 6 H 12 O 6 in a 5.0 L container and add enough water to get 5.0 L.

10. Properties of Acids and Bases Although taste is not a safe way to classify acids and bases, you probably are familiar with the sour taste of acids.

11. Acid Contain hydrogen ion (H+) pH < 7 Taste sour Electrolyte Reacts with metals that are more reactive than H+. [acidus is latin for sour]

12. Examples of Acids Lemon juice Vinegar (Acetic Acid) Hydrochloric Acid

13. Metal Activity Chart Li K Ba Sr Ca Na Mg Al Mn Zn Cr Most Active Fe Cd Co Ni Sn Pb H Cu Bi Sb Hg Ag Pt Au Least Active

14. Corrosion Oxidation of metals or substances.

15. Bases Contain hydroxide ion (OH - ) pH > 7 Taste bitter Feels slippery Weak electrolyte

16. Examples Soaps Baking soda Sodium Hydroxide

17. Alkaline solutions Another name for basic solutions

18. Hydronium ion H 3 O + Is a H + attached to a water molecule. Results in an acidic hydrogen

19. Monoprotic acids Have only one acidic hydrogen. (Ex: HCl)

20. Diprotic acid Has 2 acidic hydrogens.

21. Triprotic acid Contains 3 acidic hydrogens.

22. ACID-BASE THEORIES The most general theory for common aqueous acids and bases is the BRØNSTED - LOWRY theoryThe most general theory for common aqueous acids and bases is the BRØNSTED - LOWRY theory ACIDS DONATE H + IONSACIDS DONATE H + IONS BASES ACCEPT H + IONSBASES ACCEPT H + IONS

23. Bronsted - Lowrey Came up with a theory that states an acid is a H + donor, a base as a H + acceptor.

24. pH range 0-14

26. Common acids/bases

27. K w - ion - product constant for H 2 O = 1 x 10 -14 (mol / L) 2

28. K w = [H + ] x [OH - ] Remember K w = 1 x 10 -14 (mol / L) 2

29. Problem Find the [ OH - ] if the [ H + ] = 1 x 10 -5 M Work 1 x 10 -14 (mol / L) 2 = 1 x 10 -5 M x [ OH - ] Answer: [ OH - ] = 1 x 10 -9 M

30. Problem Find the [ H + ] if the [OH - ] = 1 x 10 -3 M. Work 1 x 10 -14 (mol / L) 2 = 1 x 10 -3 M x [ H + ] Answer: [ H + ] = 1 x 10 -11 M

31. pH = - log [H +]

32. Note: Must be the hydrogen ion NOT the hydroxide. Number used to denote the hydrogen - ion concentration, of a solution it is the negative logarithm of the H + ion concentration of a solution

33. Problem: Find the pH if the [H + ] = 1 x 10 -10 M. Is this an acid or base. Answer Base

34. Work Using calculator if you have the [H + ] put this number in then hit LOG and multiply by -1. pH = - ( 1 x 10 -10 M) hit LOG Answer= pH = 10 therefore this is a base.