1. Analysis of Vinegar by Titration
Lab 10

2. Outline Purpose Potentiometric Titrations Vinegar Titration
Proticity
Equivalence
pKa
Vinegar Titration
Calculations
Waste
Following Lab Reminder
pH Probe Calibration

3. Purpose
Students will use a pH probe to perform potentiometric titrations to determine the mass percent of acetic acid in vinegar and the pKa of acetic acid.

4. Potentiometric Titrations
Potentiometric titrations can be used to determine:
proticity (how many acidic hydrogens are donated to solution)
the amount or concentration of acid or base present (using MaVa= MbVb)
pKa (the “– log” of the acid dissociation constant)

5. Proticity
Acetic acid is a monoprotic weak acid that reacts with NaOH or KOH in a 1:1 ratio and produces a single sigmoidal curve.

6. Equivalence
The equivalence point volume is determined by plotting a derivative curve of the titration curve. The steepest point on the derivative curve corresponds to the equivalence point volume. (Find the exact value on your spreadsheet!)

7. Equivalence Point Volume
The concentration of acetic acid can be determined from:
the equivalence point volume of the base
the concentration of the base
the volume of the acid used in the titration
The equation to use is:
MaVa = MbVb

8. pKa
The pKa of acetic acid is the pH at the half-equivalence point volume of the titration, because:
For a weak acid:
HA H+ + A- and Ka =
At the half-equivalence point, half the acid has been converted to its salt, so:
[HA] = [A-]
Ka = [H+]
pKa = pH

9. Vinegar Titration Make the required dilution of vinegar.
Calibrate your pH probe.
Titrate the specified aliquots to obtain titration curves.
Determine the volume of base delivered at each time point, using the base delivery rate.
Graph the derivative of your titration curves following the instructions in the manual.
Make up a spreadsheet that will allow you to calculate the indicated values.

10. Spreadsheet Time, s pH Vol, mL Deriv 0.01 3.02 0.02 0.001 35.95 4.15
1.97
0.000
60.24
4.65
5.21
0.003
79.47
4.74
10.44
103.54
5.16
13.45
0.002
142.46
5.34
16.11
0.010
151.31
8.50
20.89
18.750
187.66
10.58
21.52
1.960
222.13
11.35
22.95
268.71
11.73
25.36
pKa
Half-equivalence Point Volume
Highest derivative
Equivalence Point Volume

11. moles of base = moles of acid (because they react in a 1:1 ratio)
Calculations
At the equivalence point:
moles of base = moles of acid
(because they react in a 1:1 ratio)
Moles of base = (Eq Pt Vol base, L) x ([base], M)
Mass of acetic acid = (molar mass of acetic acid, g/mol) x (moles of acid, moles)
Mass of vinegar = (density, g/mL) x (Vol vinegar, mL)
Mass % = (mass of acetic acid / mass of vinegar) x 100%

12. Safety Concerns Reagents: Eye Contact: Skin Contact: Inhalation:
Acetic Acid (1 N)
Sodium Hydroxide (0.1 N) / Potassium Hydroxide (0.1 N)
Eye Contact:
Irritation, tearing, redness, pain, impaired vision, severe burns and irreversible eye injury.
Skin Contact:
Severe skin irritation, soreness, redness, destruction of skin (penetrating ulcers) . May cause sensitization and / or allergic reaction.
Inhalation:
May cause coughing, serious burns, pneumonitis, pulmonary edema, and coma.
Ingestion:
Toxic. Corrosive to mucous membranes. May cause perforation of the esophagus and stomach, abdominal pain, nausea, vomiting, diarrhea, general gastro-intestinal upset.

13. Waste Only solutions with a pH between 6 and 8 can go down the drain.
All other solutions need to go in the acid/waste container in the fume hood.

14. Lab 11 Reminder
Lab 11 is next.

15. pH Probe Calibration
Calibrate your pH probe according to the instructions in your lab manual.
Be careful not to break the bulb.
Be careful not to contaminate the buffer solutions.
Ask your instructor if you need help.