What Is The Molar Mass Of Acetone

My problem question was, “What happened to the mass and the volume when I dropped an egg in vinegar, corn syrup and water for 24 hours?” To answer this question, you would have to follow the procedures. You need to carefully handle the egg. If you drop it, the the data will be incorrect. Drop the egg in different types of liquids (water, vinegar, and corn syrup) and let them sit there for 24 hours. The next day, record the mass and volume of the egg and different qualitative observations. At the end of this lab, I knew that the procedure did answer my problem because by putting the egg in different liquids, I knew that the results would be different. The answer to the problem question is the mass and the volume changed based on the different

First students obtained 8 graduated cylinders and labeled them. Each one contained a different ratio of vinegar and water. These graduated cylinders with the liquid were weighed and recorded.Then, students obtained an Alka-Seltzer tablet and recorded its mass. Then one alka-seltzer tablet was dropped into each of the graduated cylinders. Students had to

was to determine the percentage by mass of acetic acid in vinegar using acid/base titration. The

After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with the remaining NaOH until the colorless solution remained pink. The final volume was then recorded. While solution #1 was heating the same process was repeated with solution#2 and the second burette

The next step in this lab is to rinse the Erlenmeyer flask with distilled water down the drain and then repeat the experiment, this time adding 10 ml of 0.10M KI and 10 ml of distilled water to the flask instead. The flask should again be swirling to allow the solution to succumb to the same temperature as the water bath and once it has reached the same temperature, 10 ml of 3% H2O2 must then be added and a stopper must be immediately placed on the flask and recording should then begin for experiment two. After recording the times, the Erlenmeyer flask must then be rinsed again with distilled water down the drain. After rinsing the flask, the last part of the lab can now be performed. Experiment three is performed the same way, but instead, 20 ml of 0.10 ml M KI and 5 ml of distilled water will be added and after the swirling of the flask, 5 ml of 3% H2O2 will be added. After the times have been recorded, data collection should now be complete.

In this lab, the molar mass of a volatile liquid is determined based on its physical properties in the vapor state. In order to calculate the molar mass, the mass, temperature, pressure, and volume is measured independently and then converted to the correct units. Sample C was obtained at the beginning of the experiment, which was later informed to be ethanol. Based on the calculations made, the molar mass of the volatile liquid was 95.9 g/mol. However, compared to the known value of 46.1 g of ethanol, the value measured had a 108% error. Unfortunately, this was a very big percent error and may have been caused by incorrectly measuring the volume of the gas. Using the ideal gas law, the molar mass of a volatile compound was calculated in order

Corresponding to the previous experiment, this week’s experiment measures the participants’ ability to conduct basic, fundamental laboratory procedures. These procedures revolve around scientific measurements of volume, mass, and density. Unlike last week’s activity, this week’s experiment had a few modifications. In addition to distilled water, saltwater and an unknown substance were added. There was a total of five substances to choose from; Hexane, Methanol, Ethyl acetate, Ethylene glycol, and Dichloromethane. Part C, the unknown liquid number was four, which the average density was 0.789 gmL-1, and from looking at the chart the unknown identity was methanol. Part A, the temperature of the water was 20 oC, which was in front of the class,

First, all of the equipment was obtained and placed on the table. The necessary equipment was weighed using a top loader balance, which used grams as its unit of measurement. The test tube, which held the samples, was filled with water from a plastic squirt bottle. A piece of filter paper, which had been folded several times, was placed over a funnel over an Erlenmeyer flask to filter the mixture in the test tube. The test tube mixture was poured onto the filter paper.

The size of the beaker was recorded in the observation table, while the flame duration time was recorded in the column labeled Trial 1, beside the size of the beaker. 8) Steps 3 to 6 was repeated with the same beaker. The duration time was recorded in the same row as the previous time, but in the column named Trial 2. 9) Steps 3 to 7 was repeated with the rest of the three different sized beakers. 10) Steps 3 to 8 was repeated with the 2 unknown

One milliliter of 6.00-M phosphoric acid was placed into a 125-mL Erlenmeyer flask using a volumetric pipette. Using a slightly larger pipette, six milliliters of 3.00-M sodium hydroxide was transferred into a 50-mL beaker. Then a disposable pipette was used to slowly mix the sodium hydroxide into the phosphoric acid while the solution was swirled around. Then both the beaker and flask were rinsed with 2-mL of deionized water and set aside. A clean and dry evaporating dish was weighed with watch glass on a scale. Then the solution was poured into the dish and the watch glass was placed on top. The solution was then heated with a Bunsen burner to allow for the water to boil off to reveal a dry white solid. After the dish cooled to room temperature it was once again weighed and the new mass was recorded.

To perform the experiment, we had to carry out this experiment in well-ventilated area because the volatile unknown liquid could have been flammable, toxic, or irritant. In addition to that, we also had to wear department safety goggles, avoided skin/clothing contact, and most importantly, tried not to inhale any of the vapor. Now to actually perform the experiment, we placed a boiling stone into a 25 mL Erlenmeyer flask. Using a small piece of aluminum foil and a rubber band we sealed the mouth of the flask. We pinched a small hole in the center of the aluminum foil, and we measured the mass of the dry flask, boiling stone, and foil cap to the nearest 0.001 g. We obtained about 25mL of an unknown volatile liquid using a 10 mL graduated cylinder.

The mass of a piece of filter paper was measured. The paper was folded and placed in a ceramic Buchner funnel. Then, Wet the paper with RO water. The liquid was poured from the beaker into the Calculations funnel using a rubber policeman. The precipitate was carefully transferred to the funnel. Rinse the beaker and a rubber policeman with RO water. Additional water was added to rinse the precipitate. The filter paper was transferred to a beaker using the watch glass and placed the beaker on the Bunsen burner to dry the filter after all the water has passed through the funnel. The mass of the filter paper and precipitate was measured after the precipitate was completely dried.

The lab is about trying to find a neutral potential hydrogen balance (PH) and molarity with following a certain number of steps. In the lab they received material such as, filter paper, vinegar, baking soda, glass rod, water, beaker, graduated cylinder, PH balance meter, and PH strips. After, collecting the material they had to do the first trial with information the teacher had given them to create their own procedure. The first trial was similar to the others except for the amounts would change for each substances. In the first lab the students were told to put fifty milliliters of water in the beaker and mix it in with one gram of sodium bicarbonate. After, mixing the two ingredients the group had to pour the mx into the ring stand. When

First, each graduated cylinder was weighed on the scale individually and labeled as one of the three liquids, so the mass could be recorded. This step helped to keep constant conditions between the different groups, as did using the same scale. Next, 25 mL of each liquid was placed in the compatibly labeled cylinder. The type of liquids used, water, olive oil, and baby oil, were the independent variable of the experiment. Thirdly, each cylinder was weighed again. The mass of the cylinder with the liquid was then recorded. Then, each liquid was poured into the beaker slowly in the order of water, then olive oil, then baby oil. After allowing time for the liquids to settle, the order of the liquids were recorded from bottom to top. Finally, calculations to find the density of each liquid were made by subtracting the mass of each cylinder without the liquid from the mass of the cylinder with the liquid in it, and recording the result. Then the mass of the liquid alone was divided by the 25 mL to find the density, the dependent variable of the experiment. All groups’ densities were averaged

While performing this experiment, I dissected the experiment into two parts, one part for pressure vs volume and the other part for pressure vs temperature. To test the relationship between gas pressure and volume, I started by collecting data of the amount of pressure when the 20mL syringe was moved at 5.0mL, 10.0mL, 12.5mL, 15.0mL, 17.5mL, and 20.0mL while adding 0.8mL to account for the extra volume inside the gas pressure sensor. Lab Quest measured the amount of pressure applied from each volume and graphed it. To test the relationship between gas pressure and temperature, I started by preparing a water bath of cold/ice temperature water into a 1-liter beaker. A temperature probe and the gas pressure sensor will be connected to Lab Quest to collect the data throughout the experiment. A rubber stopper containing a plastic tubing connected to it valve was attached to the gas pressure sensor. I then inserted the glass stir rod into the open valve of the rubber stopper