1. Ch. 14
Acids & Bases

2. What's An Acid?
An acid is any substance that increases the H+ ion concentration in water.
This causes the pH to drop
They taste sour.
They react with metals to make H2 gas
These are all the same thing:
H+  H3O+  proton

4. The Six Strong Acids Dissociate completely in H2O
HCl  H+ + Cl- (HCl is an Acid)
Ex: HCl – Hydrochloric Acid
HBr – Hydrobromic Acid
HI – Hydriodic Acid
H2SO4 – Sulfuric Acid
HNO3 – Nitric Acid
HClO4 – Perchloric Acid

5. Be Careful with Strong Acids

6. Weak Acids These don’t completely dissociate in water.
Here is acetic acid, the one in vinegar:
HC2H3O2(aq)  H+ (aq) + C2H3O2-(aq)
about 99% about 1%

7. Some Strong and Weak Acids

8. What’s a Base?
Any substance that makes lots of hydroxide ions, OH-, in water.
They decrease the H+ ion concentration in water and increase the pH.
They taste bitter (ie: soap) and feel slippery

9. Strong Bases They completely dissociate in water:
NaOH  Na+ + OH-
NaOH – Sodium Hydroxide
KOH – Potassium Hydroxide
LiOH – Lithium Hydroxide
Ba(OH)2 – Barium Hydroxide

11. Be Careful with Strong Bases

12. Weak Bases Don’t completely dissociate in water.
Only about 1% to 5% is dissociated.
Here is ammonia, a weak base:
NH3 + H2O  NH OH-

13. Acids & Bases

14. Acid-Base Definitions
Type
Acid
Base
Arrhenius
H+ or H3O+ Producer
OH- Producer
Bronsted-Lowery
Proton (H+) Donor
Proton (H+) Acceptor
Lewis
Electron-Pair Acceptor
Electron-Pair Donor

15. Acid Neutral Base

16. Neutralization Reactions
This is when you mix an acid with a base.
The result is always the same:
Acid + Base  Water + a Salt
The salt can be any number of ionic salts, not just NaCl.

17. Hydrochloric acid reacts with sodium hydroxide. Write the reaction:
HCl + NaOH  H2O + NaCl

18. Before After

19. Another of Neutralization:
Sulfuric acid reacts with potassium hydroxide. Write and balance the reaction.
H2SO4 + 2KOH  2H2O + K2SO4

20. A Break & a Challenge:
Say the color, not the word.