Titration of Common Household Products
(Do at least two trials for each part!) Names:________________________________________________
Part I. Titration of vinegar with sodium hydroxide
Vinegar contains acetic acid, so it can be neutralized by adding a base. Use a graduated cylinder to deliver 10.00
mL of vinegar to a clean 250 mL erlenmeyer flask. Add 1-2 drops of phenolphthalein and about 25 mL of distilled
water. Use the 1.00 Molar NaOH solution (in the buret) to titrate the vinegar until the solution is barely pink.
Record volumes on the buret to the nearest 0.1 mL. (or to the nearest 0.01 mL if possible). Discard the titrated
solution in the sink and rinse the flask with distilled water.
Trial #1
Trial#2
Volume of Vinegar Used
Initial Buret Reading
Final Buret Reading
Volume of NaOH delivered from Buret
Color of solution at end point
Part II. Titration of aqueous ammonia (glass cleaner) with hydrochloric acid
Ammonia (NH3) can be neutralized by adding an acid. Use a graduated cylinder to deliver 10.00 mL of ammonia
solution to a clean 250 mL erlenmeyer flask. Add 1 drop of methyl orange and about 25 mL of distilled water. Use
the 1.00 Molar HCl solution (in the buret) to titrate the ammonia until the solution turns from yellow to
peach/light orange (not pink). Record volumes on the buret to the nearest 0.1 mL. (or to the nearest 0.01 mL if
possible). Discard the titrated solution in the sink and rinse the flask with distilled water.
Trial #1
Trial#2
Volume of Ammonia Solution Used
Initial Buret Reading
Final Buret Reading
Volume of HCl delivered from Buret
Color of solution at end point
Part III. Titration of Lysol toilet cleaner with sodium hydroxide!
Lysol contains hydrochloric acid, so it can be neutralized by adding a base. Use YOUR graduated cylinder to deliver
5.00 mL of lysol to a clean 250 mL erlenmeyer flask. Use distilled water to rinse the lysol from your graduated
cylinder into your flask (use at least 20 mL water and make sure all the lysol gets into your flask). Add 1-2 drops of
phenolphthalein. Use the 1.00 Molar NaOH solution (in the buret) to titrate the lysol until the solution is barely
pink. Record volumes on the buret to the nearest 0.1 mL. (or to the nearest 0.01 mL if possible). Discard the
titrated solution in the sink and rinse the flask with distilled water.
Trial #1
Volume of Lysol Used
Initial Buret Reading
Final Buret Reading
Volume of NaOH delivered from Buret
Color of solution at end point
Trial#2
Titration of Common Household Products
Pre Lab Questions
Part I. Titration of vinegar with 1.00 M sodium hydroxide
1. Vinegar is an aqueous solution of acetic acid. What is the formula for acetic acid?
______________________ (Hint: the formula of acetate ion is C2H3O2-1)
2. Write the neutralization reaction that occurs between acetic acid and sodium hydroxide. Include
subscripts.
Part II. Titration of aqueous ammonia with 1.00 M hydrochloric acid
3. When ammonia (NH3) dissolves in water, some of it reacts with water to form ammonium hydoxide,
NH4OH. Write the neutralization reaction that occurs between the ammonium hydroxide and HCl.
Include subscripts.
Part III. Titration of Lysol toilet cleaner with 1.00 M sodium hydroxide!
4. The active ingredient in lysol is hydrochloric acid. Write the neutralization reaction that occurs
between hydrochloric acid and sodium hydroxide. Include subscripts.
CALCULATIONS
Part I
1. Decide what volume of NaOH to use for your calculations: If you had two good (light pink) trials, use
the average volume delivered. If you had one good trial and one bad trial, use the volume from the good
trial. If you didn’t achieve a light pink color in either trial, use the trial with a smaller volume of base
delivered. What volume of NaOH will you use in your calculations? ___________mL
2. Calculate the molarity of acetic acid in the vinegar.
3. Calculate the pH and pOH of the acetic acid.
Part II
4. Decide what volume of HCl to use for your calculations (use the same logic as in part I) What volume
of HCl will you use in your calculations? ___________mL
5. Calculate the molarity of the ammonia solution.
6. Calculate the pH and pOH of the ammonia solution.
7. Decide what volume of NaOH to use for your calculations (use the same logic as in parts I and II)
What volume of NaOH will you use in your calculations? ___________mL
8. Calculate the molarity of the hydrochloric acid in the lysol.
9. Use your molarity from #3 to calculate the pH of lysol.
10. In this lab, you titrated three different household substances: Vinegar, ammonia, and lysol.
a. Which of these substances was the most acidic?_____________________________
b. Which of these substances was the most basic?______________________________
c. Which of these substances had the highest pH?______________________________
11. Which substance was the indicator in part I?_____________________________________
part II?_____________________________________
part III?____________________________________
12. Which substances was the standard solution in part I?______________________________
part II?_______________________________
part III?______________________________