Reporte Para Clase De Ciencia

Got Phenolphthalein?
Purpose- The purpose of this lab is to calculate the actual percentage of the acetic acid by reaching equilibrium such thatit is neutralized with NaOH. This will be done by finding the percent error thus proving whether or not the vinegar is labeled correctly. To findthe percentage one must add NaOH into an Erlenmeyer flask and while adding 10 mL of 5% vinegar solution in a separate flask. Slowly add drop in theNaOH while periodically swirling the flask containing the vinegar solution. Continue adding NaOH until a color change is noted and remains changedfor at least 5 seconds.
Calculations-
1. M NaOH = 1 M
2. N NaOH = 1.0
3. N CH3COOH = Na x 10 mL/7.75 mL = 1.0 N x 7.75 mL/7.75 mL
Na/7.75 =7.75/10 = 1.2
4. M CH3COOH = 1.2 M
5. g CH3COOH/L vinegar solution
60g/.0094 L= 6383.0 mol
6. g CH3COOH/g vinegar solution = 60 g/1000g =0.06 g
7. % CH3COOH = .06 x 100%= 6%
8. % error = [(0.06 – 0.05)/0.05] x 100%
= (0.01/0.05) x 100%
= .2 x 100%
=20%
Conclusion- In conclusion, the percentage of vinegar was more than that stated on the label. By using the normality formula, the normality ofvinegar was found thus resulting in a finding of 6% of the vinegar solution. A 20% error was found, with thus said this lab was performed poorly. Theunavoidable error is knowing the exact point of neutralization due to the fact of the unknown true % of acetic acid in the vinegar solution.