Fda Vinegar Chemistry 1225 Lab

Procedure: I used a ruler, thermometer, and scale to take measurements. I used a graduated cylinder, short step pipet, scale, and ruler to determine volume and density. I used a volumetric flask, graduated pipet, pipet bulb, scale, and glass beaker to determine concentrations and densities of various dilutions.

Vinegar is a common household product, when mixed with the indicator, phenolphthalein, it turns pink. This indicates that Vinegar is acidic.

For this experiment, we used three different types of vinegar (distilled white, white wine, and champagne) to test the acetic acid within each. Our experiment was aimed to test the amount of acetic acid within each type of vinegar and compare it to the amount listed on each bottle. Our research question was, what type of vinegar contains the most acetic acid? The phenolphthalein indicator turned a light pink color to indicate when the acidic solution turned neutral due to the addition of titrant. The goal of this experiment was to test the acetic acid within each bottle to see if our data matched the value listed on the bottle.

Since Alka Seltzer is swallowed and reacts with stomach acid, the vinegar is in this experiment is substituting as the stomach acid. The principle of limiting reagents relates to this lab because

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.

for percent acetic acid in vinegar, it can be concluded that the percentage of acetic acid in the

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.

The density had to be determined by massing a known volume of the solution and dividing the mass by the volume. The percent by weight of acetic acid in the solution needed to be found by dividing the grams of solute from the grams of total solution. This required manipulation of the equations for density and molarity to reach the desired value. With this information, it was possible to compare both the molarities and the percent composition by weight of the vinegars to store bought

Stoichiometry with Kitchen Chemistry By: Meena Roberts Discussion Section: Wednesday at 8:30 Objective: The purpose of the lab was to see how much carbon dioxide was produced in reaction. Procedure: Measured mass of balloon, mass of NaHCO3 and container, mass of container after NaHCO3 was removed, and mass of NaHCO3 in balloon on digital scale in grams(g).

The purpose of the lab was met. The percent weight and concentration of acetic acid in the vinegar solution and its Ka, the concentration of phosphoric acid in the Unknown 86 container at each equivalent point, and each Ka value at each equivalent point are all listed below

Can red cabbage juice indicator be used to determine the strength of acids and bases? Explain.

In 125-mL Erlenmeyer flask, rinse very well with water. Use distilled or deionized water for a final rinse. Wet flasks can be used for titration. Titration procedure should be repeated 2 more

Experiment to investigate the amount of sodium hydroxide needed to neutralize the solution of vinegar

The purpose of this experiment was to determine how much KMnO4 was needed to titrate approximately 1 mL of an Unknow X101 concentrated solution of Oxalic Acid. A standardized KMnO4 solution was used on a known solution of Oxalic acid to help determine the unknown percent oxalic acid in unknown X101. The unknown sample for this experiment was sample x101 which theoretically was a % Oxalic Acid dehydrate sample but, the average of all three trials determined it to be a 6.7% percent Oxalic acid.

For this experiment, a pH meter was used so this part of the experiment began with the calibration of the pH meter with specified buffers. The buret was then filled with the standard HCl solution and a set-up for titration was prepared. 200g of the carbonate-bicarbonate solid sample was weighed and dissolved in 100 mL of distilled water. The sample solution was then transferred into a 250-ml volumetric flask and was diluted to the 250-mL mark. The flask was inverted several times for uniform mixing. A 50-mL aliquot of the sample solution was measured and placed unto a beaker. 3 drops of the phenolphthalein indicator was added to the solution in the beaker. The electrode of the pH meter was then immersed in the beaker and the solution containing the carbonate-bicarbonate mixture was titrated with the standard HCl solution to the phenolphthalein endpoint. Readings of the pH were taken at an interval of 0.5 mL addition of the titrant. After the first endpoint is obtained, 3 drops of the methyl orange was added to the same solution and was titrated with the standard acid until the formation of an orange-colored solution. Readings of the pH were also taken at 0.5 mL addition of the titrant.