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Lab Report on Analysis of Vinegar, Lab Reports of Chemistry

Sioux Falls SeminaryChemistry

Its purpose to standardize a solution of sodium hydroxide to use the standardized sodium hydroxide solution to titrate the acetic acid in vinegar to determine its percent by mass in vinegar

Typology: Lab Reports

2020/2021

Uploaded on 05/11/2021

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E15-1
Experiment 15
FV 9/25/12
ANALYSIS OF VINEGAR
MATERIALS: Four 250 mL Erlenmeyer flasks, two 50 mL burets, liquid funnel, one 150 mL beaker, one
50 mL beaker, 5.00 mL pipet, weighing dish, approximately 0.1 M NaOH,
C6H4(COOH)COOK (potassium hydrogen phthalate), phenolphthalein, grease pencil.
PURPOSE: The purpose of this experiment is two-fold: (1) to standardize a solution of sodium
hydroxide; (2) to use the standardized sodium hydroxide solution to titrate the acetic
acid in vinegar to determine its percent by mass in vinegar.
LEARNING OBJECTIVE: By the end of this experiment, the midshipman should be able to
demonstrate the following proficiencies:
1. Use pipets and burets correctly.
2. Explain the term hygroscopic.
3. Explain the function and necessary qualities of a primary standard.
4. Perform a titration accurately and precisely.
5. Calculate the molarity and the mass of components in a solution from stoichiometry information.
6. Calculate the percent by mass of a component in a solution.
DISCUSSION:
Vinegar is a solution of acetic acid in water. Acetic acid, CH3COOH, is a weak monoprotic acid
with a molar mass of 60.05 g/mole. The percent by mass of acetic acid in vinegar can be determined by
titrating a known amount of vinegar with a standardized solution of sodium hydroxide, i.e., a sodium
hydroxide solution of accurately known concentration. Acetic acid and sodium hydroxide react as shown
below:
CH3COOH (aq) + NaOH (aq) CH3COONa (aq) + H2O (l)
60.05 g/mole
Sodium hydroxide is a hygroscopic solid which means it absorbs water from the air. A weighed
quantity of sodium hydroxide therefore contains an unknown mass of water. Therefore, a solution of
known molarity cannot be made by dissolving a known mass of solid sodium hydroxide in water. The
concentration of a sodium hydroxide solution must be determined experimentally. This is done by
titrating the sodium hydroxide solution against a primary standard. A primary standard is a substance
from which a solution of known concentration can be prepared.
The primary standard used in this experiment is potassium hydrogen phthalate,
C6H4(COOH)COOK, which is referred to by the shorthand notation of "KHP". KHP has several
advantages: it does not absorb moisture readily (i.e., is not hygroscopic); it is easily dried; it can be
accurately weighed; it can be obtained in very pure form; it has a high molar mass of 204.22 g/mole; and
it is very soluble in water. KHP is an acid, which reacts in aqueous solution to neutralize the base, sodium
hydroxide, as shown below:
C6H4(COOH)COOK (aq) + NaOH (aq) C6H4(COONa)COOK (aq) + H2O (l)
204.22 g/mole
KHP
pf3
pf4
pf5

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Download Lab Report on Analysis of Vinegar and more Lab Reports Chemistry in PDF only on Docsity!

Experiment 15

FV 9/25/

ANALYSIS OF VINEGAR

MATERIALS: Four 250 mL Erlenmeyer flasks, two 50 mL burets, liquid funnel, one 150 mL beaker, one 50 mL beaker, 5.00 mL pipet, weighing dish, approximately 0.1 M NaOH, C 6 H4(COOH)COOK (potassium hydrogen phthalate), phenolphthalein, grease pencil.

PURPOSE: The purpose of this experiment is two-fold: (1) to standardize a solution of sodium hydroxide; (2) to use the standardized sodium hydroxide solution to titrate the acetic acid in vinegar to determine its percent by mass in vinegar.

LEARNING OBJECTIVE: By the end of this experiment, the midshipman should be able to demonstrate the following proficiencies:

  1. Use pipets and burets correctly.
  2. Explain the term hygroscopic.
  3. Explain the function and necessary qualities of a primary standard.
  4. Perform a titration accurately and precisely.
  5. Calculate the molarity and the mass of components in a solution from stoichiometry information.
  6. Calculate the percent by mass of a component in a solution.

DISCUSSION:

Vinegar is a solution of acetic acid in water. Acetic acid, CH 3 COOH, is a weak monoprotic acid with a molar mass of 60.05 g/mole. The percent by mass of acetic acid in vinegar can be determined by titrating a known amount of vinegar with a standardized solution of sodium hydroxide, i.e., a sodium hydroxide solution of accurately known concentration. Acetic acid and sodium hydroxide react as shown below:

CH3COOH (aq) + NaOH (aq)  CH3COONa (aq) + H2O (l) 60.05 g/mole

Sodium hydroxide is a hygroscopic solid which means it absorbs water from the air. A weighed quantity of sodium hydroxide therefore contains an unknown mass of water. Therefore, a solution of known molarity cannot be made by dissolving a known mass of solid sodium hydroxide in water. The concentration of a sodium hydroxide solution must be determined experimentally. This is done by titrating the sodium hydroxide solution against a primary standard. A primary standard is a substance from which a solution of known concentration can be prepared. The primary standard used in this experiment is potassium hydrogen phthalate, C6H4(COOH)COOK, which is referred to by the shorthand notation of "KHP". KHP has several advantages: it does not absorb moisture readily (i.e., is not hygroscopic); it is easily dried; it can be accurately weighed; it can be obtained in very pure form; it has a high molar mass of 204.22 g/mole; and it is very soluble in water. KHP is an acid, which reacts in aqueous solution to neutralize the base, sodium hydroxide, as shown below:

C 6 H4(COOH)COOK (aq) + NaOH (aq)  C 6 H4(COONa)COOK (aq) + H2O (l) 204.22 g/mole KHP

PROCEDURE:

Part A. Standardization of the Sodium Hydroxide Solution

  1. Use the top-loading balance to pre-weigh about 0.51 grams of KHP into a weighing dish.
  2. Use the analytical balance to obtain the mass of a clean 250 mL Erlenmeyer flask. Transfer the KHP to the clean 250 mL Erlenmeyer flask. Obtain the mass of the flask and the KHP sample.
  3. Add approximately 100 mL of distilled water to the flask to dissolve the KHP and then add two to three drops of phenolphthalein indicator. Gently swirl the solution.
  4. Add ~50 mL of NaOH solution (approximately 0.1 M) to a 150 mL beaker. Rinse the buret with NaOH and then fill the buret with the NaOH solution from the beaker. Use the small funnel when pouring the NaOH into the buret. Make sure there is no air bubble in the buret tip. Record your initial buret reading with the proper number of significant figures.
  5. Titrate the KHP solution with the NaOH solution to a very pale pink endpoint. Record the final buret reading to the correct number of significant figures.
  6. Repeat steps 1 – 5. After doing your second titration, do a quick calculation to determine whether your precision is acceptable. Divide the volume of NaOH used in each titration by the mass of the KHP sample for each titration. Divide the larger ratio by the smaller ratio. If the resulting number is greater than 1.03, then do a third trial.

Part B. Measurement of Acetic Acid in Vinegar

  1. Use the analytical balance to obtain the mass of a clean, dry 250 mL Erlenmeyer flask. It is okay if the flask is a little wet inside as long as it is only distilled water. It must be dry on the outside.
  2. Add ~15 mL of vinegar to a clean, dry 50 mL beaker. Pre-rinse a 5.00 mL pipet with a small quantity of vinegar. Pipet a 5.00 mL sample of vinegar into the flask. Reweigh the flask containing the 5.00 mL sample.
  3. To the vinegar sample in the 250 mL Erlenmeyer flask, add approximately 100 mL of distilled water and then two or three drops of phenolphthalein indicator.
  4. Refill your buret with the NaOH solution.
  5. Titrate the vinegar solution with the NaOH solution to a very pale pink endpoint.
  6. Repeat steps 1 – 5. If two titrations are not within +/- 0.50 mL of each other, repeat the titration.

Clean up:

  1. Rinse all waste solutions down the drain.
  2. Wash all glassware. Invert the buret and mount it in the buret clamp on the ring stand, with the stopcock open to allow it to drain. Leave the other washed glassware upright. Clean up your area.

DATA TREATMENT

Experiment 15

INCLUDE THE APPROPRIATE SIGNIFICANT FIGURES.

Part A. Standardization of the Sodium Hydroxide Solution

(A.1) Calculate the moles of KHP for:

Sample 1:

Sample 2:

Sample 3:

(A.2) Realizing you titrated to the equivalence point, use your calculations from Part A to calculate the moles of NaOH for:

Sample 1:

Sample 2:

Sample 3:

(A.3) Calculate the concentration (M) of the NaOH solution for each sample, and then obtain the average value:

Sample 1:

Sample 2:

Sample 3:

AVERAGE:

DATA TREATMENT

Experiment 15

Part B. Measurement of Acetic Acid in Vinegar

(B.1) Use your average value of the NaOH molarity to calculate the moles of NaOH for:

Sample 1:

Sample 2:

Sample 3:

(B.2) Realizing you titrated to the equivalence point, calculate the moles of acetic acid in the 5.00 mL sample of vinegar:

Sample 1:

Sample 2:

Sample 3:

(B.3) Calculate the mass % of acetic acid in vinegar, and then obtain the average value:

Sample 1:

Sample 2:

Sample 3:

AVERAGE:

Name ___________________________ Section ___________________________

Date _____________________________

PRE-LAB EXERCISES

Experiment 15

INCLUDE THE APPROPRIATE SIGNIFICANT FIGURES.

1. Write the balanced molecular equation for the neutralization of acetic acid (CH 3 COOH)

with sodium hydroxide.

2. Before the sodium hydroxide can be used in this experiment, it must be standardized (i.e.

the concentration must be measured accurately). This lab will use C 6 H 4 (COOH)COOK

(KHP) to standardize the NaOH solution. Write the balanced molecular equation for the

neutralization of KHP with sodium hydroxide.

3. Calculate the concentration of the sodium hydroxide solution (in M) if it takes 25.00 mL of

sodium hydroxide solution to titrate 0.5000 g of KHP (MM = 204.22 g/mol).

4. Calculate the mass % of acetic acid in vinegar if you found 0.00400 mol of acetic acid in

5.000 mL of vinegar (density = 1.01 g/mL).

Mass % of component X = 100

mass of X total mass of solution (containing X)

×