1. TITRATIONS AND PH CURVES AP CHEM CH 15

2. Review H-H What is the pH of a buffer that is made by dissolving 50.0g of sodium acetate in 500.mL of 0.300M acetic acid? Assume the volume remains constant.

3. STRONG ACID – STRONG BASE TITRATIONS The net ionic equation is: Reaction continues to completion The mole is an inconveniently large unit Stoichiometry, not equilibrium

4. Consider the titration of 50.0mL of 0.200M nitric acid with 0.100M NaOH Amount of NaOH added (mL 0.100M NaOH) pH of resulting solution 0 mL 10 mL 20 mL 50 mL 100 mL 150 mL 200 mL Calculate the pH after: a) No NaOH has been added b)10.0mL of NaOH are added c)20.0mL of NaOH are added d)50.0mL of NaOH are added e)100.0mL of NaOH are added f)150.0mL of NaOH are added g)200.0 mL of NaOH are added

5. pH Curve of Previous Problem

6. WEAK ACID – STRONG BASE TITRATIONS The net ionic equation is: STEP ONE: STOICHIOMETRY STEP TWO: EQUILIBRIUM PROBLEM

7. Consider the titration of 50.0mL of 0.100M acetic acid with 0.100M NaOH Amount of NaOH added (mL 0.100M NaOH) pH of resulting solution 0 mL 10 mL 25 mL 40 mL 50 mL 60 mL 75 mL Calculate the pH after: a) No NaOH has been added b)10.0mL of NaOH are added c)25.0mL of NaOH are added d)40.0mL of NaOH are added e)50.0mL of NaOH are added f)60.0mL of NaOH are added g)75.0 mL of NaOH are added

8. pH Curve of Previous Problem

9. WEAK BASE – STRONG ACD TITRATIONS The net ionic equation is: STEP ONE: STOICHIOMETRY STEP TWO: EQUILIBRIUM PROBLEM

10. Consider the titration of 100.0mL of 0.050M ammonia with 0.100M HCl Amount of HCl added (mL 0.100M HCl) pH of resulting solution 0 mL 10 mL 25 mL 50 mL 60 mL Calculate the pH after: a) No HCl has been added b)10.0mL of HCl are added c)25.0mL of NaOH are added d)50.0mL of NaOH are added e)60.0mL of NaOH are added

11. pH Curve of Previous Problem