# Chm Lab 5

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Experiment 5: Titration for Acetic Acid in Vinegar Name: Lab Partners: None Date of Experiment: March 25th, 2013 Location: My House Course Number: Chem 112 Abstract: In this experiment the objectives were develop familiarity with the concepts and techniques of titration and to determine the concentration of an acetic acid solution in vinegar. Experiment and Observation: Data Table 1: Quantity of NaOH needed to Neutralize 5 mL of Acetic AcidBrand of Vinegar Used: Heinz White Distilled VinegarLabel Notes: ______________________ | | Initial NaOH reading(Interpolate to 0.1 mL) | Final NaOH reading(Interpolate to 0.1 mL) | Volume of NaOH used | Trial 1 | 9.5 | 1.3 | 8.2 | Trial 2 | 9.7 | 1.4 | 8.3 | Trial 3 | 9.6 | 1.4 | 8.2 | Average volume of NaOH used: | 8.2 | Calculations and Errors: Errors: Calculations: A. Calculate the average number of mL of NaOH used for the 3 trials and record. B. Calculate the Normality of the vinegar using the previously given equation. Na = (Nb)(Volumeb) (Volumea) C. Calculate the mass of the acetic acid in grams using the previously given equation. Massa = (Na)(GMWa) D. Calculate the percentage of acetic acid using the previously given equation. % Acid = Massa(g/L) x 100 1000g/L Discussion and Conclusion: Questions: LabPaq question guidelines: Answer questions A and G in the lab manual. Skip questions B, C, D, E and F in the lab manual, and answer these instead: A. What is the average % acetic acid in your vinegar sample? Standard vinegar is 5% acetic acid.How does your result compare with the standard? G. A 5.0 mL sample of vinegar was titrated with 7.2 mL of 0.55 M NaOH(aq). If the density of the vinegar solution is 1.00 g/mL, what is the mass percent of acetic acid present?