1. pH In the Laboratory

2. Ionization of Water

3. Equllibrium Constant, K eq

4. Ion Product of Water, K W

5. pH

6. Acidity

7. Measuring pH Indicater Dyes; Methyl Red, Phenol Red, etc. pH Paper (Litmus Paper) pH Meter

8. Voltmeter with electrode Measures electrical potential difference across electrode due to protons 1 pH unit = 60 mV pH also dependent on temperature

9. pH Electrode Filled with reference solution (4 M KCl, sat. AgCl) Glass semi permable (protons cannot cross) Glass protected by plastic sleeve Some are sensitive to Tris buffer

10. pH Standards Color coded 4, 7, and 10 Potassium Hydrogen Pthalate Standardize everyday Bracket pH range

11. pH of Strong Acids HCl H + + Cl - Assume complete dissociation 1 M HCl, pH = -log [H + ] = -log 1 = ? 0.5 M HCl, pH = -log 0.5 = ? 6 M HCl, pH = -log 6 = ?

12. pH of Strong Bases NaOH Na + + OH - Assume complete dissociation pK W = pH + pOH = 14 pH = 14 – (-log [OH - ]) 1 M NaOH, pH = 14 – (-log 1) = ? 0.01 M NaOH, pH = 14 – (-log 0.01) = ? 6 M NaOH, pH = 14 – (-log 6) = ?

13. pH of a Weak Acid