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Lab: Determining Ka of Acetic Acid

Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka.

Materials:
25 mL pipet and bulb burette 2x150 mL beaker
125 mL Erlenmeyer flask acetic acid solution sodium hydroxide solution
phenolphthalein pH metre

Procedure:
1. Record the molar concentration of the NaOH solution.
2. Produce a table to record your data. It should have one column for volume of NaOH added and one column for pH.
3. Obtain 50 mL of acetic acid and place it into a beaker.
4. Place 50.0 mL of NaOH into the burette.
5. Pipet 25.0 mL of acetic acid into the Erlenmeyer flask. Add two drops of phenolphthalein to the acid.
6. Record the initial pH of the solution.
7. Add 1.00 mL of NaOH from the burette to the Erlenmeyer until the pH reaches 5.00. Record the volume to two decimal places. Measure the pH of the solution each time you add NaOH.
8. Above pH=5.00, add NaOH in 0.10 or 0.20 mL portions. Record the volume at which the phenolphthalein turns pink.
9. Continue to add NaOH until the pH reaches 11.00. Above pH=11.00, add 0.10 mL portions until the pH reaches 12.00.
Note: All you actually have to do is start the burette running, the values will record as you progress through the lab.



NaOH(ml) pH
0.00 2.52
1.00 3.58
2.00 3.59
3.00 4.92
4.00 4.09
5.00 4.14
6.00 4.55
7.00 4.73
8.00 4.98
9.00 5.07
9.20 5.09
9.40 5.14
9.60 5.19
9.80 5.24
10.00 5.25
10.20 5.37
10.40 5.38
10.60 5.45
10.80 5.59
11.00 5.62
11.20 5.75
11.40 6.18
11.60 6.29
11.80 6.54
12.00 10.68
12.20 11.15
12.30 11.36
12.40 11.43
12.50 11.57
12.60 11.65
12.70 11.67
12.80 11.77
12.90 11.79
13.20 11.83
13.40 11.84
13.60 11.88
14.10 11.92
15.00 12.00

Analysis:
Write the chemical equation for the neutralization reaction you observed.

  • chemistry - ,

    The rest of my lab does not want to post? Why is this?:(

  • chemistry - ,

    My question is found in the Analysis section. Thanks experts!


    Lab: Determining Ka of Acetic Acid

    Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka.

    Materials:
    25 mL pipet and bulb
    burette
    2x150 mL beaker
    125 mL Erlenmeyer flask
    acetic acid solution
    sodium hydroxide solution
    phenolphthalein
    pH metre

    Procedure:
    1. Record the molar concentration of the NaOH solution.
    2. Produce a table to record your data. It should have one column for volume of NaOH added and one column for pH.
    3. Obtain 50 mL of acetic acid and place it into a beaker.
    4. Place 50.0 mL of NaOH into the burette.
    5. Pipet 25.0 mL of acetic acid into the Erlenmeyer flask. Add two drops of phenolphthalein to the acid.
    6. Record the initial pH of the solution.
    7. Add 1.00 mL of NaOH from the burette to the Erlenmeyer until the pH reaches 5.00. Record the volume to two decimal places. Measure the pH of the solution each time you add NaOH.
    8. Above pH=5.00, add NaOH in 0.10 or 0.20 mL portions. Record the volume at which the phenolphthalein turns pink.
    9. Continue to add NaOH until the pH reaches 11.00. Above pH=11.00, add 0.10 mL portions until the pH reaches 12.00.


    NaOH(ml) pH
    0.00 2.52
    1.00 3.58
    2.00 3.59
    3.00 4.92
    4.00 4.09
    5.00 4.14
    6.00 4.55
    7.00 4.73
    8.00 4.98
    9.00 5.07
    9.20 5.09
    9.40 5.14
    9.60 5.19
    9.80 5.24
    10.00 5.25
    10.20 5.37
    10.40 5.38
    10.60 5.45
    10.80 5.59
    11.00 5.62
    11.20 5.75
    11.40 6.18
    11.60 6.29
    11.80 6.54
    12.00 10.68
    12.20 11.15
    12.30 11.36
    12.40 11.43
    12.50 11.57
    12.60 11.65
    12.70 11.67
    12.80 11.77
    12.90 11.79
    13.20 11.83
    13.40 11.84
    13.60 11.88
    14.10 11.92
    15.00 12.00


    Analysis:
    Write the chemical equation for the neutralization reaction you observed

  • chemistry - ,

    Apparently your data doesn't want to copy. I assume that is what you are trying to do. How about just typing in the material. I suggest you start a new post.

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