1. Acids and Bases
Chemistry 1106

2. Definitions Arrhenius Acid Arrhenius BASE
Releases Hydrogen ion (Proton)
Produces H3O+
HNO3 + H2O → H3O+ + NO3-
Arrhenius BASE
Releases OH- ion (Hydroxyl)
NaOH + H2O  Na+ + OH- + H2O

3. Strong vs. Weak Strong Acid/Base Completely Dissociates
Only Few Strong Acids And Bases
No Equilibrium
HNO3 + H2O → H3O+ + NO3-
NaOH + H2O → Na+ + OH- + H2O

4. Strong vs. Weak Weak Acid/Base Partially Dissociates
Reaction Is In Equilibrium
HF + H2O ↔ H3O+ + F-

5. pH Reference is Water In Pure Water (Equilibrium) pH = -log [H3O+]
Water is Amphoteric- Characteristics of both acid and base
H2O + H2O ↔ H3O+ + OH-
In Pure Water (Equilibrium)
[H3O+] = 1.0 x 10-7
[OH-] = 1.0 x 10-7
pH = -log [H3O+]
Most water is not 7
Our is between 4-5

6. Correlations of pH pH Goes Down As [H3O+] Increases
The higher the Ka the higher the Disassociation
Is in -Log scale so… is a 10 fold difference
Since H3O+ and OH- Ions Effect pH, It Can Be Said That:
↓ pH = ↑ Acidic Strength
↑ pH = ↑ Basic Strength

7. pH Electrode
Working principle on current

8. Carefull pH electrode are very sensitive and very easy to break
Never leave a pH electrode out of a solution
Rinse electrode with DI water when introduce to a new solution
Calibrate Electrode
Check calibration curve with solutions pH 4 7 and 10
If valid go to experiment

9. Fill in the blanks Solutions are 1) H2O 2) oxlic acid 3) HCl 4) H2SO4
5) NaOH
6) NH4OH
7) Na2PO 3
8) Unknown A and B

10. Calculations pH = -Log[H3O+] // pOH = -Log[-OH]
10-pH= [H3O+] // 10-pOH= [-OH]
pH + pOH = 14
Only in a strong acid this = the concentration