Chem II Lab- Titration of Vinegar with NaOH

In summary, the question asked for the calculation of grams of acetic acid per liter of vinegar, using the previous problem's information of diluting the vinegar to an average molarity of 2.7M. The molecular weight of acetic acid was given as 60.06 g and the calculation resulted in 162.16 g. It was noted that this may seem high, but it is possible for vinegar to have a concentration of 16% acetic acid.
  • #1
ChocolateCoke
1
0

Homework Statement



"Calculate the grams of acetic acid per liter of vinegar"


Homework Equations



Previous problem stated the multiply the average molarity of diluted vinegar times 10= 2.7 M

Vinegar (acetic acid)= H(C2H3O2) molecular weight= 60.06 g

The Attempt at a Solution



moles= M x L
2.7M x 1L = 2.7 moles
2.7 moles x 60.06 g= 162.16 g

This seems way too high. and i wasn't given anything really and it is driving me insane!

Thank you in advance for anyone who helps!
 
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  • #2
To the extent that you described your situation, the work and the result look good.

Note that you labeled the topic, "...Titration of Vinegar...". We may assume you were doing calculations to prepare to perform a titration.
 
  • #3
2.7M acetic acid is about 16% - strong for vinegar, but not impossible.

In Germany in grocery stores you can buy Essigessenz which is basically just 70% acetic acid.
 

1. What is the purpose of the "Chem II Lab- Titration of Vinegar with NaOH" experiment?

The purpose of this experiment is to determine the concentration of acetic acid in a sample of vinegar using a titration method with a known concentration of sodium hydroxide (NaOH) solution.

2. What materials are needed for this experiment?

The materials needed for this experiment include: vinegar, sodium hydroxide solution, a burette, a beaker, an Erlenmeyer flask, a funnel, a pipette, phenolphthalein indicator, and a clamp and stand setup.

3. How does titration work in this experiment?

In this experiment, titration is used to find the endpoint of the reaction between acetic acid (in the vinegar) and sodium hydroxide. The NaOH solution is added slowly to the vinegar until the reaction is complete, as indicated by a color change in the solution due to the addition of phenolphthalein indicator. The amount of NaOH solution used is then used to calculate the concentration of acetic acid in the vinegar.

4. Why is phenolphthalein used as an indicator in this experiment?

Phenolphthalein is a colorless indicator that turns pink in the presence of a base, such as sodium hydroxide. It is used in this experiment to indicate the endpoint of the reaction between acetic acid and NaOH, as the solution will turn pink when all of the acetic acid has been neutralized by the base.

5. What are some potential sources of error in this experiment?

Potential sources of error in this experiment include inaccurate measurements of the vinegar or NaOH solution, improper calibration of the burette or pipette, and not properly neutralizing the solution at the endpoint. It is important to take multiple measurements and calculate an average to minimize these errors.

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