1. What we’ve done…. Monday: notes 15.2/16.1 P457 #8-15 p477 #3-6
Tuesday: notes 15.3/16.2
P462 # p486 #16-23
Wednesday: lab separating mixtures
Hmwk: p499 #50-53

2. Acids & Bases

3. Acids 1. Taste sour
Acids taste sour: examples are citric acid in citrus fruits, acetic acid in vinegar…sour pickles

5. 2. Donates Hydrogen ions H+ 3. Forms Hydronium ions H3O+
Products of a chemical reaction will show H3O
Hydrogen proton leaves acid molecule and attaches to a water changing it from H2O to H3O

6. Products of a chemical reaction will show H3O HCl + H2O  H3O+ + Cl-
Hydrogen proton leaves acid molecule and attaches to a water changing it from H2O to H3O

7. 4. Turns Universal Indicator to RED
Blue litmus paper chemically reacts with acid and turns red
Litmus paper made from lichens

8. 5. It Burns skin and tissue
Acid will burn skin and other tissues (eyeballs, etc.) be careful when using strong acid solutions in labs

9. 6. Conducts electricity Only when dissolved in water
Acid disassociates the H+ from the other (such as H+ and Cl- when HCl dissolved in water)
Results in movement of ions (electrons)
Weak acids = conduct less
Strong acids = conduct more
Sulfuric acids in car batteries

10. 7. Crystalline Solid
When undissolved, exists as a crystalline solid

11. Stomach acid Battery acid Examples Citric acid (vitamin c in fruit)
Acetic acid (vinegar)
Gastric juices (stomach acid)
Sulfuric acid (battery)

12. Bases 1. Tastes Bitter Unsweetened chocolate Walnuts Almonds Coffee
Escarole
Squeaky/dry feel in mouth

13. KOH  K+ + OH- NH3 + H2O  NH4+ + OH-
2. Hydroxide ions OH-
KOH  K OH-
NH3 + H2O  NH OH-
2 ways of creating OH- ions in solution:
1. Either by disassociating OH- from the compound in a decomposition reaction or
2. Stealing an H+ from water in a double displacement reaction

14. 3. Turns Universal Indicator to BLUE

15. 4. Corrosive (feels slippery)
Dissolves lipids in your skin and feels slippery

16. 5. Can also conduct electricity

17. Examples Sodium hydroxide pellets
Ammonia = fertilizers, cleaners
Sodium hydroxide (lye) = baking soda, soaps, paper
Calcium hydroxide (lime) = cement
Potassium hydroxide (potash) = bleaching

18. Soap = basic surrounds oily substances allows emulsion in water Whisked away!

19. pH Scale measures hydronium ions (H3O+)
The pH scale is only used to measure concentrations of hydronium ions
Large amounts in acids
Small amounts in bases

20. Comparative concentrations
Hydronium ions (acid)
Hydroxide ions (base)
0 - 6
Acids
A lot
A little 7
neutral =
8 -14
Bases

21. Concentration changes by powers of 10
pH =1 has 10x more acidic (H+) than pH = 2 pH = 1 has 100x more acidic (H+) than pH = 3 More  Less 10
100
1000
10000
100000

22. Acid + Base  water H3O+ + OH-  H2O
Neutralization
Acid + Base  water H3O+ + OH-  H2O

23. KOH + HNO3  H2O + K+ + NO3- Is it balanced?

24. Must have = amounts of hydronium and hydroxide ions to completely neutralize

25. The End Homework--- Due Monday! (from Wednesday) p499 #50-53
(new) p499 #54-55
(new) p501 #78, 81, 82
Don’t forget to turn in Lab: Separating Mixtures today!!!