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

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)

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

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

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)

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.

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

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

Acids and Bases