Analysis Of Volumetric Analysis

Introduction/purpose:
The purpose of this lab was to find the concentration and mass volume percent of acetic acid in different brands of vinegar solution. In order to find the concentration and mass volume percent of acetic acid we performed a volumetric analysis. This means that the vinegar solution was neutralized by adding a base solution. To view this neutralization process phenolphthalein indicator was added. Phenolphthalein indicator will turn slightly pink when the solution is neutralized.

Materials:
• 0.05 M of Sodium Hydroxide solution (NaOH)
• Vinegar (Acid “A” and Acid ”B”)
• Phenolphthalein indicator
• Two 150ml beakers
• 50ml Burette
• Three 250ml Erlenmeyer flasks
• 10ml pipette and pipette bulb
• Wash bottle
• Funnel
• Retort stand and clamps

Procedure:
1. Clamp the 50ml burette to the retorted stand and add the sodium hydroxide solution (base) using a funnel.
2. Clean one of the Erlenmeyer flasks using a wash bottle and add 10ml of Acid “A” into it. Use the pipette to accurately measure 10ml before adding it to the flask.
3. Add 2-3 drops of phenolphthalein indicator into to the Erlenmeyer flask containing the Acid “A”.
4. Place the Flask under the burette that is filled with the Sodium Hydroxide (base).
5. The Solution inside the burette was unveiled slowly and mixed together with the Acid “A”. The flask was swirled continuously to ensure the Sodium Hydroxide is thoroughly mixed.
6. Stop the flow of the base when the Acid ‘A’ changes it color to light pink.
7. Repeat the process again with the second batch of Acid ‘A’ and record the results.
8. Repeat the process using Acid B and record the results.

Result
To neutralize 10 mL of Acid ‘A’ we used 3.35 mL of Sodium Hydroxide and to neutralize 10 mL of...

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...etic acid than Acid ‘A’. The amount of Base that took to neutralize Acid ‘A’ was 3.9 mL while Acid ‘B’ was 3.5 mL. Finally, the concentration of Acetic acid in Acid ‘A’ was 0.017 mol/L and Acid ‘B’ was 0.19 mol/L
Error Analysis:
Our titration lab went smooth, however there were some errors that can be identified. One such error was that we added too much Sodium Hydroxide during the titration. This could have had a negative effect in the data we gathered and the calculations. Giving us a slightly inaccurate measurements. This can be avoided by getting used to the burettes release mechanism and knowing how to control the flow of the Sodium Hydroxide to the Acid.
Conclusion:
To conclude this lab, we learned how to calculate the mass volume percent of acetic acid in a vinegar solution using stoichiometry learned in unit 2 and how to conduct a proper titration lab.