1. Weak acid – strong base titrations:
Initial pH:
Acid dissociates partially - ICE, Ka, etc.
Initial pH:
Acid dissociates fully, [acid]=[H3O+]

2. Weak acid – strong base titrations:
Initial pH:
Acid dissociates partially - ICE, Ka, etc.
If 0.1 M NaOH is being used to titrate a 0.1 M solution of acetic acid (Ka = 1.8x10-5), calculate the following:
1. Initial pH: (before titrating)

3. Weak acid – strong base titrations:
pH while adding base:
Stoichiometry first. Buffer zone second.
pH while adding base:
Stoichiometry and LR!

4. Stoichiometry first. Buffer zone second.
pH while adding base:
Stoichiometry first. Buffer zone second.
If 0.1 M NaOH is being used to titrate a 0.1 M solution of acetic acid (Ka = 1.8x10-5), calculate the following:
2. pH while adding base: (before equivalence point)
50 mL of HC2H3O2 is titrated with 10 mL of NaOH

5. Weak acid – strong base titrations:
Equivalence point:
If acid and base are gone, why it slightly basic???
Equivalence point: Point at which all moles of acid have reacted with all moles of base (pH=7)

6. If acid and base are gone, why it slightly basic???
Equivalence point:
If acid and base are gone, why it slightly basic???
If 0.1 M NaOH is being used to titrate a 0.1 M solution of acetic acid (Ka = 1.8x10-5), calculate the following:
3. pH at equivalence point:
50 mL of HC2H3O2 is titrated with NaOH to the equivalence point.

7. Weak acid – strong base titrations:
pH if “over-titrated”:
Stoichiometry and LR!
pH if “over-titrated”:
Excess strong base + conj. Base together

8. 4. pH after equivalence point: (over-titrating)
If 0.1 M NaOH is being used to titrate a 0.1 M solution of acetic acid (Ka = 1.8x10-5), calculate the following:
4. pH after equivalence point: (over-titrating)
50 mL of HC2H3O2 is titrated with 55 mL of NaOH
pH if “over-titrated”:
Excess strong base + conj. Base together

9. Acids and Bases