FDA Vinegar / Acetic Acid Analysis
Objective- Determine the Acetic acid level contained within the vinegar sample
Background- Per the FDA regulation which states that consumer vinegar may contain no less than four percent and no more than five percent Acetic Acid, we will determine the Acetic Acid content of a sample of the vinegar in question through titration. After standardization of our titrant, which in this case will be NaOH, we will use this along with the indicator Phenolphthalein, to titrate the vinegar to determine the concentration of Acetic Acid in the sample.
Equipment and reagents- We will use a 50mL beaker, a graduated buret, spatula, droplet applicator, 125mL Erlenmeyer flask, hot plate, and a container of
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M1 NaOH= nNaOHVNaOH= 4.9×10-4mols 4.7mL=10.4×10-5 2. M2 NaOH= nNaOHVNaOH= 4.9×10-4mols 5.0mL=9.8×10-5 3. M3 NaOH= nNaOHVNaOH= 4.9×10-4mols 5.0mL=9.8×10-5
Mavg NaOH= M1×M2×M33=1.0×10-4M
Titration of vinegar nNaOH= Mavg NaOH × VNaOH 1. n1 NaOH= 1.0×10-4M8.8 mL=8.8×10-4m 2. n2 NaOH= 1.0×10-4M8.5 mL=8.5×10-4m 3. n3 NaOH= 1.0×10-4M8.2 mL=8.2×10-4m nCH3COOH= nNaOH Mass of CH3COOH= nCH3COOH ×60gmol 1. Mass of CH3COOH= 8.8×10-4m ×60gmol = 5.28×10-2g 2. Mass of CH3COOH= 8.5×10-4m ×60gmol = 5.08×10-2g 3. Mass of CH3COOH= 8.2×10-4m ×60gmol = 4.9×10-2g
Percent Weight CH3COOH in Vinegar = Mass of CH3COOHMass of Vinegar 1. Mass of CH3COOHMass of Vinegar = 5.28×10-2g1.004gmol ×100=5.26% 2. Mass of CH3COOHMass of Vinegar = 5.10×10-2g1.004gmol ×100=5.08% 3. Mass of CH3COOHMass of Vinegar = 4.9×10-2g1.004gmol ×100=4.91%
Avg % Wght CH3COOH in Vinegar = Mass1+Mass2+Mass33= 5.26+5.08+4.913= 5.08%
Results- The results of this examination is that the content percentage of Acetic Acid in the provided vinegar sample exceeds the FDA standards by .08 percent. While this clearly shows a result outside the provided guidelines, it is possible that the chance of error built into this method of testing could account for the excess. For instance, if there were an air bubble in the tip of the Buret during the titration, this would lead to the assumption of a higher level of NaOH needed to neutralize
Throughout the course of the experiment, the weight of the beaker and liquid, the weight of the Alka-Seltzer tablet, the weight of the beaker with liquid plus the weight of the tablet, and the weight of the beaker with all of the contents after the bubbling ceased remained roughly constant and did not vary widely. However, a trend is able to be seen in Figure 1. It is clear that as the mL of vinegar used in each experiment run increased, the mass percent of NaHCO3 increased as well. During the construction of Figure 1, experiment runs four and six were deleted to create the expected graph which consists of a gradual increase and eventually leveling off into a plateau.
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Three grams of a mixture containing Benzoic Acid and Naphthalene was obtained and placed in 100 ml beaker and added 30 ml of ethyl acetate for dissolving the mixture. A small amount (1-2 drops) of this mixture was separated into a test tube. This test tube was covered and labelled as “M” (mixture). This was set to the side and used the following week for the second part of lab. The content in the beaker was then transferred into separatory funnel. 10 ml of 1 M NaOH added to the content and placed the stopper in the funnel. In the hood separatory funnel was gently shaken for approximately one minute and vent the air out for five seconds. We repeated the same process in the same manner one more time by adding 10ml of 1M NaOH.
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Experiment to investigate the amount of sodium hydroxide needed to neutralize the solution of vinegar
Materials and methods Materials • Vinegar • Baking soda • 9 10cm by 12cm paper towel squares • Film canister • Goggles • Ruler • Scissors • 5 mg measuring cup •
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