1. Properties of Acids & Bases
Taste
Touch
Reaction with Metals
Sour
Bitter
Like H2O
Slippery
Yes, with most
No, with most

2. Properties of Acids & Bases
Both will conduct electricity when liquid or aqueous (electrolytes).
Both take place in neutralization reactions.

3. Definitions of Acids Arrhenius Definition
When dissolved in water, it separates to give off H+ ions. [

4. H2SO4 (l)  2H+(aq) + SO4-2(aq)[
H2SO4 (l)  2H+(aq) + SO4-2(aq)
HNO3 (l)  H+(aq) + NO3-(aq)

5. Definitions of Acids Br∅nstead-Lowry Definition
Donates H+ ions to other chemicals. [

6. An acid will form the Hydronium Ion (H3O+)
What about in H2O?
An acid will form the Hydronium Ion (H3O+) [

7. Definitions of Bases Arrhenius Definition
When dissolved in water, it separates to give off OH- ions. [

8. Definitions of Bases Br∅nstead-Lowry Def.
Accepts H+ ions from other chemicals. [

9. Water becomes Hydroxide Ion (OH-)
What about in H2O?
Base accepts a H+ ion.
Water becomes Hydroxide Ion (OH-) [

10. These dissociate completely in solution.
Strong Acids & Bases
These dissociate completely in solution. [ [

11. Weak Acids & Bases
These do not break up completely when placed in solution.
Conjugate Acid
Conjugate Base [

12. [

13. Click here for a video clip on strong versus weak acids.[

14. [

15. Weak Acids & Bases
To determine how much an acid dissociates or “breaks-up” use this generic equation:
HA(aq) + H2O(l) ⇆ H3O+(aq) + A-(aq)

16. Weak Acids & Bases
Pg. 610

17. Weak Acids & Bases Example:
If hydrofluoric acid (HF) has a starting concentration of M, what will the concentration of H3O+ be?
Ka for HF is 6.8 x 10-4

18. [H3O+] and [F-] are equal so…
HF (aq) + H2O (l) ⇆
H3O+ (aq)
+ F- (aq)
[H3O+] and [F-] are equal so…
X = [H3O+] = 8.2x10-3 mol/L