Materials: 1) Beakers 2) Water 3) Plastic wrap 4) Rubber band 5) Light corn syrup 6) Vinegar 7) 2 raw egg (large) 8) 2 graduated cylinder (100ml, 50ml) 9) Marker for labeling cup 10) Tri Beam scale Procedure: 1) Measure 130ml of vinegar into the beaker. 2) Gently place the egg into the vinegar. Make sure the egg is completely covered by the vinegar. 3) Weigh all of the items o the scale 4) Cover the beaker with plastic and secure it with a rubber band. 5) Label the beaker with your name and period.
Then, six capillary tubes were used to spot the five known solutions and the one unknown. The unknown number and the colors of each solution were recorded. The Chromatography paper was then folded into a cylinder and stapled at the top edge. After that, enough 9:1 acetone: 6 M HCl solution was poured into a 600 mL beaker so that the depth was about 0.5 cm and the chromatography paper was stood up in the beaker, which was then covered with foil. The chromatography paper was removed with tongs
0.1 M silver nitrate was added to the anion solution and a precipitate was formed. Dilute HNO3 was then added dropwise to the precipitate until it became acidic. The supernatant was decanted out and the precipitate remained. 5 mL of distilled water was added to the centrifuge tube with the precipitate. 6 M HNO3 was then added dropwise to the precipitate until the solution was acidic.
The clear gummy bear will dissolve faster because the vinegar won’t have to first break down the color dye that makes the other gummy bear red. Procedure: 1. First we decided what we wanted to do. We could pick from the range of gummy bear colors and solutions
Carbonate could be used to remove silver ions. This is because when carbonate reacts with a cation other the H+ and NH4+, it has a low solubility. Meaning it would form a precipitate with silver and the ions would be removed. Evidence that suggest nitrate compound are soluble is that they didn’t with most compounds, they remained aqueous. Also, there was never a formation of a precipitate when reacting with nitrate ions.
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?
One advantage of my proposed procedure about how to separate the sand from the benzoid acid was a strainer which could have stopped sand particles from entering the benzoic acid or to catch any benzoic solid acid crystals from mixing in with the sand. Since the benzoic acid lifted into the top when I boiled the water, it allowed me to pour it right into the paper cup. Also the benzoic acid was popping a lot along the bottom of the beaker during the heating process so I was able to identify the benzoic acid right away. C. Defiantly benzoic acid crystals could have been left behind during the separation process. I noticed some larger crystals of solid benzoic acid rocks left behind
Grace Murphy 15 September 2015 7th Hour Katelyn Stevens Determine the Density of Aluminum Purpose: To determine the density of aluminum using the water displacement method. Procedure: First, fill a 10 mL-graduated cylinder as close to 5 mL as possible with water and record the volume ( to the nearest 0.01mL) on the data sheet. Next, find the mass of the container with the aluminum using a balance and record it on your sheet. Carefully drop pieces of the aluminum into the graduated cylinder. Drop just enough pieces to rise the water level 0.5 mL.
Manganese dioxide is an inorganic molecule that can achieve this. The catalyst lowers the activation energy of the decomposition which is already noticeable without the addition of a catalyst. In our lab we observed that the Manganse dioxide had no effect on the reaction, however it should have a significant
The color change in the copper sulfate when we heated it indicated that all of the water has evaporated, to be sure, we heated and weighed the crucible and CuSO4 again, and it came out to be .901g again. Finally, before disposing of the CuSO4 we added a little bit of water and observed the changes, the crucible quickly heated up and bonds were formed. Section 2: Results Measurement include: • The initial mass of crucible: 19.071g • The mass of the CuSO4: 1.509 • The mass of CuSO4 after mortar and pestle: 1.424g • The mass of the crucible and the CuSO4: 19.972g Observations: • The color change when the copper sulfate was heated,