Leah Romero 10/30/2017 Conclusion Lab 3 Chem 102L In lab 3, fundamentals of chromatography, the purpose was to examine how components of mixtures can be separated by taking advantage of different in physical properties. A huge process in this lab was paper chromatography, which was used to isolate food dyes that are found in different drink mixes. The different chromatograms of FD&C dyes were compared to identify which dyes are present in each of the mixes.
Compare the result to the chart on the back of the urinary pH test strips bottle, and record data. Clean the stirring rod with water before moving on to the next test tube. Repeat this process for each increment (2 mL, 3mL, 4mL) Figure #1: Picture of bean solution mixed Figure #2: Picture of materials needed for the with alpha galactosidase experiment Safety considerations: Be careful with the beakers, glass stirring rod, and test tubes, as they could break easily and can cause cuts in the skin. DCP: A scatter plot will be used to display how the amount of alpha galactosidase (measured in mL) in the bean solution affects the glucose concentration (measured in mg/dL) and error bars to show the standard deviation.
Next when the solution is still somewhat warm place a kebab stick into the jar. Secure the stick into place using a close pin or a pen. Allow the solution to sit until the crystals are formed and firmly secured to the stick. Once you are happy with how much the crystals have grown, break the surface sugar in the jar and remove the stick and crystals from the solution. (Davis 2015)
Methylene chloride was added to the TLC chamber until it reaches 0.5 cm depth in order to cover the bottom of the jar; a piece of filter paper was added to the jar allowing the solvent to travel up the paper and the surface area of the solvent increased. Then the plate was placed in the jar containing 100% CH2Cl2 so that the top of the plate rested against the side of the jar opposite the filter paper. When the eluent was near to the top of TLC plate, the plate was removed and then
Insert syringe into ICG powered vial making sure 5ml water contents are carefully distributed in. Take this step slow as the pressure may expel contents out from the rubber topper puncture site. Draw the contents to mix. To fully mix, you may re-insert and re-draw the solution in a back and forth manner.
I will test the experiment to observe the process of osmosis. The membrane of the egg will all that will be left once the egg has been soaked in vinegar for the significant amount of time. After viewing a video over the experiment and reading on the background and science of it, I will understand why everything happens the way it does. This chemistry experiment has many learning experiences behind it that I will
In a small 125ml Erlenmeyer flask, dry the ether solution over anhydrous calcium chloride. Add sufficient calcium chloride so that it no longer clumps to pellets added earlier on the bottom of the flask. Remove the solvent using a rotary evaporator and weigh product. Results 1 mole of benzoic acid (C6H5COOH = 122.12grams) reacts with 1 mole of methanol (CH3OH = 32grams/mole) to produce 1 mole of methyl benzoate (C6H5COOCH3 = 136.15grams) and 1 mole of water.
Pre- lab preparation To perform this investigation, a number of the solutions were needed to be prepared in advance. The following is the preparation process - Preparing the stock solution-The stock solution of Salicylic acid needed to be prepared well in advance before the experiment began. To do so, 1.73g of Salicylic Acid was weighed using the weighing balance. After Salicylic acid was weighed, it was transferred to a standard flask of 100cm3 and, 100cm3 of pure Ethanol (C2H5OH), was poured into the standard flask that contained the Salicylic acid.
Next, addition of starch indicator occurs and then titration of mixture in company with Na2S2O3 is realized until observing of color as blue is obtained. All of these procedure is repeated for solution of blank without adding oil. Consequently, quantity of iodine being used for absorption by oil is
Remove all salt from beaker into a plastic container “g”. Scrape off ALL extra salt to make sure you have everything(If salt isn’t completely dry then spread out and let the rest of the water evaporate on its own. Do not wash out beaker until you know that ALL of the salt is removed from it). Mass all of the separate substances (Beads, Iron, Salt, and Sand). Place plastic container “h” on the digital scale.
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.
The difference in this chemical and physical properties will aid in their separation. Processes like solubility, gravitational filtration and recrystallization will be used to separate the substances present in Panacetin. The melting and boiling point of the substances will help in concluding on which of these compounds will be presented at the end of experiment. Procedure and observation The Panacetin content was weighed approximately 3.0493g and transferred to the Erlenmeyer flask; 75ml of dichloromethane (CH¬2CL2) was added to the content. The dichloromethane (CH2Cl2) dissolved the sucrose, leaving the active unknown agent and aspirin behind.
Divide the mixture into equal halves of 25g weighed using an electronic scale to ensure accuracy, using a different crucible 9. Place the equally divided mixtures next to one another in separate 5L conical flasks 10. Label each conical flask according to the solvent which will be added with a permanent marker, Ethyl acetate and
Experimental Clay-catalyzed dehydration of cyclohexanol Cyclohexanol (10.0336 g, mmol) was added to a 50 mL round bottom flask containing five boiling chips, Montmorillonite K10 clay (1.0430 g) was then added to the cyclohexanol and the mixture was swirled together. The flask was then placed in a sand bath and attached to a simple distillation apparatus. The contents of the flask were then heated at approximately 150 °C to begin refluxing the cyclohexanol. The distillation flask was then loosely covered with aluminum foil and the hood sash was lowered in order to minimize airflow. As the reaction continued, the temperature was adjusted in order to maintain a consistent rate of distillation.