Synthesis Of Alum From Aluminum Can Pieces

The mixture was heated at 120°C using an aluminum block and was stirred gently. After all of the solid dissolved, it was heated for 20 additional minutes to ensure the reaction was complete.

22.0 mmol (2.93 grams) of anhydrous aluminum chloride was added to a large dry vial and immediately capped. 10 mL dichloromethane,1 mL anisole, and a stir bar were added to the reaction flask. An ice bath was prepared to cool reaction begins to boil. Then the aluminum chloride was added in small portions while stirring between each addition. The adherent aluminum chloride was then mixed with a little amount of dichloromethane and the apparatus was reassembled. Into the addition funnel 1.0 mL (~11 mmol) acetic anhydride was added then stoppered immediately. The acetic anhydride was then slowly added (1 drop every 3 seconds) to the reaction flask while gently boiling in a steam bath with a temperature range of 40°C- 45°C. Once the addition was complete, heat under reflux for ~30 minutes in steam bath. The warm reaction mixture was poured slowly over 10 g of cracked ice with vigorous stirring. Ice water was used to rinse any residue out of the flask into the beaker. The dichloromethane layer was then separated in a seperatory funnel. The CH2Cl2 layer was then washed with 5 mL 3 M NaOH, and then with 5 mL saturated aqueous NaCl. The funnel was shaken to extract two layers. The organic layer was then dried with ~1 gram of anhydrous MgSO4. I think used

The pipet was put into the top of the condenser and leaving no open spaces. The vacuum served to get rid of the nitrogen oxide gases that were formed during the oxidation reaction. The solution was heated for 30 minutes, beginning the time when the first sign of nitrogen oxide fumes were observed. After the 30 minutes, the solution was removed and cooled for a few minutes. The solution turned was a brownish-yellow color and all the crystal were dissolved, leaving a liquid. The solution was then transferred, using a Pasteur pipet, to 3 mL of water in a beaker. The reaction flask was rinsed to remove the remainder of the solution. The solution was stirred with a glass rod until room temperature of the solution was achieved. A yellow solid was to form, but instead the solution remained aqueous in the case of the specific experiment explained here. With additional scraping of the solution with a glass rod, no crystals formed at all. The next procedure, if the crystals had formed was to crush the solid with the glass rod and filter the solid until the crystals were dry. The mass would then be weighed and the crystals were to be recrystallized with 95% ethanol. The crystals were to be cooled in ice water to get full crystallization and then the crystals were to be filtered and air dried, then weighed.

This experiment was performed in order to better increase our chemical lab knowledge in the areas of separation of distinct compounds, and it helped further our ability to observe chemical reactions as compounds are heated and chilled. The class was asked by the ERA to help discover if aluminum from soda cans can be used to

Purpose: The purpose of this lab is to be able to perform four different types of chemical reactions. With the information gained from these reactions, identify the products of the reactants with be identified and balanced equations for the reactions observed will be written. Procedure: Provided by Teacher.

For the Synthesis of Alum lab my lab group and I took 1 gram of aluminum foil and broke it into small pieces. Next we added 25 mL of 3M KOH solution. Once the foil was dissolved we filtered the solution through a Buchner funnel with filter paper sealed inside with water. As the solution was filtering we applied a vacuum filtration to the Buchner funnel to expedite the filtering process. Once it was completely filtered my lab group poured the solution into a beaker and covered the beaker with parafilm. We then waited overnight to allow the crystals to form inside the beaker. Unfortunately, we did not produce any crystals overnight so we borrowed some from another group. Once we obtained the crystals we had to stir them in a beakers to make more form other than just the ones we received. After we rinsed the crystals with half ethanol and half water mixture. Once they were dry we determined the mass of the crystals with a balance.

1 and 2) In this experiment, Sn2 nucelophilic substitution between an unknown nucleophile solution and the known reagents benzyl bromide and NaOH occurred to form a benzyl ether product. 3) Refluxing, recrystallization, melting point, and TLC were used to purify and identify the products of the reaction. 4)

2. Next add both of these reactants to a graduated cylinder containing 30 mL of distilled water

Cold deionized water (20 mL, 1.11 moles) was added into the detached round bottom flask, and the reaction was allowed to crystallize for 2 minutes. The crude product was vacuum filtered, and washed twice with deionized water (50 mL). The filtered crystals were dissolved in ethanol (15 mL, 0.261 moles) in a

Place the filter paper in an Buchner flask. As support, pour a few millimeters of water around the cone-shaped filter paper. At this state, pour in the solution into the filter. Another type of filtration technique is called Vacuum Filtration. The purpose for this method is to collect a desired product from a mixture. To perform a vacuum filtration, the Buchner flask must be securely clamped to a ring stand. After, a Buchner funnel must be placed over the flask. Add a filter paper to the funnel and place a few drops of solvent to hold

The synthesis of alum was carried out adequately as evidenced by the correct changes in the appearances of the mixtures and compounds in various stages of the synthesis process as well as the appearance of the synthesized alum (Table I). Although the weight of the alum placed in both crucibles was similar, the weight of KAl(SO4)2 in the crucibles after heating was unequal relative to the weight of the alum (Table II). A plausible cause for such disparity could be the loss of alum due to the spattering of contents observed during the initial phase of heating. The calculations used to determine the waters of hydration had a limitation because all the difference between the weight of alum and KAl(SO4)2 could only be attributed to the water lost

As you are allowed to attend only one lab make-up session, please contact Prof. Jennifer Chabra for further details. Please also copy me on the

Stirring the mixture gently till is almost at boiling point; drops of silver nitrated were added to check if the mixture was entirely precipitated. After through precipitation, the mixture was placed in drawer to cool down. In the meantime, the sinister glass crucible was weighed on the balance. After the mixture put in the drawer has cooled, the vacuum filtration apparatus was put together and the supernatant liquid was poured into the glass filter leaving the precipitate in the beaker. This process was done again when more amount of 0.01M HNO3 was added to thoroughly filter and transfer the precipitate in the crucible. The flask was cleaned after detaching from the crucible and then reconnected to the crucible to be filtered out one more time with 0.01M HNO3. This time, the aliquot of HNO3 was put in a test tube and given to the TA to test for no turbidity. After the TA’s approval, the apparatus was reconnected and three 5ml portions of acetone washed the

The main objective of this experiment was to use stoichiometry and a variety of other tests to determine the amount of reactants needed, the expected results, percent yield, and compounds present. To achieve this, aluminum extracted from a can was heated in a beaker until the metal dissolved. Solid residue was then removed using vacuum filtration and sulfuric acid was added and placed in an ice bath to create crystals. Vacuum filtration was used again to separate these crystals. The percent yield was then calculated using the found theoretical and actual masses. To assess purity, the melting point was found to be 90-92.5 degrees Celsius, a comparable range to the expected value; using the flame test, it was discovered potassium was present;

20.34mL of diethyl malonate was added to the solution via the separatory funnel over a period of about fifteen minutes. Next, 35mL of EtOH and 14.5mL of n-BuBr were added to the mixture respectively. The solution was refluxed for 10 minutes using a heating mantle and then cooled on ice. The above mixture was later poured into 200ml of water and then transferred to a 500mL separatory funnel.