Rinse the Erlenmeyer flask with about 10 ml of solvent and pour the solvent through the funnel, too. Remove the funnel, add two or three boiling chips and reattach the thermometer and adapter to the still pot. • Discard the magnesium sulfate remaining in the Erlenmeyer flask by dissolving it in tap water and pouring the solution down the drain. • Before beginning the distillation, weigh a clean, dry 1 narrow mouth screw cap bottle on a balance. Remove the cap of the bottle, and insert the clean, dry plastic long-stem funnel in the neck of the bottle.
Drops of the Methanol were then added to each flask until the crude caffeine had completely dissolved. 13. The solution was then filtered and the residue collected in a filter paper. It was left to dry and
Formula 2: % Component= 100% component mass (g) sample mass (g) Procedure First, we measured out the evaporating dish to find the mass. Then we added around 3 grams of our sample (2.832g exactly). Next we added the isopropyl alcohol to dissolve the Benzoic Acid.
Then, the pipet was rinsed with distilled water. The bulbs were then attached to the pipette; filling and dispensing water were practiced using both bulbs. Furthermore, the 250-mL beaker was weighed, and its mass was recorded. After that, the Erlenmeyer flask was filled with 100 mL of distilled water. The temperature was recorded.
2.4.1. Tetramethyl glucose acetylation 1gm of tetramethyl glucose was dissolved in 5ml of acetic anhydride and added to fused sodium acetate of 0.375gm and mixed for 10 minutes and allowed to cool. To this mixture 7.5ml of toluene and 5ml of dry ether were added. The whole mixture evaporated to syrup on a water bath at 50 °C. The product dissolved in the dry ether after washing with toluene.
Purpose and Techniques: This experiment has the aim to determine a chemical formula of hydrated compound, which ingrains cupper, chloride and water molecules in its structure. In order to find this hydrated compound, it is necessary to use the law of multiple proportions. In other word, finding the appropriate variables values to this compound (CxCly*zH2O). Additionally, two major steps are required to proceed the experiment.
• Iodine Solution Weigh 7.7g of potassium iodide into a 50cm3 beaker. Use distilled water to help the iodide dissolve. Swirl for a few minutes until the iodide has completely dissolved. Using a funnel to help, pour the potassium iodide into a 500cm3 volumetric flask, make sure all traces of the solution is in the volumetric flask. Using distilled water would be a good method in order to rinse the beaker.
Two chemical reactions are carried by adding sodium hydroxide to the acidic solution from Part I. During the first reaction is the neutralization of the excess of nitric acid in the mixture by sodium hydroxide. The second reaction takes the place after naturalization is a complete and NaOH is in excess. While the liquid inside the beaker is being stirred, with the stirring rod, 10 ml of 6 M NaOH is poured into the solution from Part I at 1 mL at a time. After each 1 mL the solution is tested for acidity with red litmus paper.
Add sodium carbonate (Na2CO3), to the calcium chloride you already have. This will make calcium carbonate ( CaCO3), according to the formula: Na2CO3 + CaCl2 -> CaCO3 + 2NaCl. Afterward, filter this solution to obtain the calcium carbonate. Finally, heat the calcium carbonate at 248 degrees Fahrenheit to dry it out. Heat the calcium carbonate to 1,832 degrees Fahrenheit to get CaO.
On the other hand, white solid paracetamol, 100ml beaker, and 15ml of hot water, 20ml warm water, and water bath were used for the recrystallization purification technique. Evaporating dish, cold water, stirring rod, watch glass, small beaker, oven, cotton wool, and tissue were also employed in the recrystallization purification method. Method Recrystallization purification technique A portion of crude paracetamol sample was transferred into a 100ml beaker. To it, 10ml of hot water was added to dissolve it.
Stoichiometry is a method used in chemistry that involves using relationships between reactants and products in a chemical reaction, to determine a desired quantitative data. The purpose of the lab was to devise a method to determine the percent composition of NaHCO3 in an unknown mixture of compounds NaHCO3 and Na2CO. Heating the mixture of these two compounds will cause a decomposition reaction. Solid NaHCO3 chemically decomposes into gaseous carbon dioxide and water, via the following reaction: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g). The decomposition reaction was performed in a crucible and heated with a Bunsen burner.
Purpose This experiment is to determine the concentration of the solute copper sulfate pentahydrate, and the unknown solution, by passing different wavelengths of light through each solution. Procedure Weigh out approximately 5g of copper sulfate pentahydrate. Record the mass and place the solute into a 50 mL volumetric flask. Fill half of the flask with distilled water, add the stopper for the flask, and lightly shake the flask, until the copper sulfate pentahydrate fully dissolved.
The purpose of this lab was to be able to use physical characteristics to determine the identity of an unknown compound. The data from this experiment classified aluminum as metallic; ascorbic acid, paraffin, palmitic acid, sucrose, graphite, and water as molecular; sodium chloride as ionic. In order to determine this, 3 tests were conducted. The first test was to test the conductivity of each substance at room temperature. In this test, only graphite and aluminum conducted.
The purpose of this laboratory experiment was to identify the molarities of dye present in green Powerade and then create a solution that possessed the same concentrations. This experiment consisted of two parts of experimentation, the first part focused on identifying the dyes present and at what concentration, and the second part focused on the recreation of the stock solution. To successfully complete this experiment, a small cuvette, full of 2 mL of green Powerade, was placed into a UV spectrometer in order to identify which wavelengths were being absorbed and reflected. With this information a complete series of dilutions using yellow #5 and blue #1 dye in ratios of 1:1, 1:2, 1:3, 1:4, and 1:5 were conducted to find the max peak absorbancy