As we know the equation C1V1=C2V2, we can get a set of concentration (g/L) of different ratio of Red #40. Introduction The goal which the experiment designed to achieve is perform a Beer’s law analysis to determine a solution’s concentration, and determine a percent composition. To build the calibration curves for each food dye, we need to measure the absorption of different solutions of known concentration. One rather quick way to make a solution of known concentration is by exact dilution from a more concentrated solution of known concentration. We rinsed a pipette with some of the sample, filled curettes between 2/3 and 3/4 full with the samples, put a curette in the cell holder and make absorbance measurements.
OBJECTIVES In this experiment, you will a. Measure and analyze the visible light absorbance spectrum of a food coloring solution to determine the maximum wavelength(s) of absorbance b. Measure the absorbance of the reaction between a food coloring solution and bleach c. Analyze the absorbance vs. time graphs to determine the order of the reaction d. Write the rate law for the reaction MATERIALS Computer Colorimeter (wavelength = 635 nm) Food coloring (blue) Commercial bleach (5.25% NaOCl) three cuvettes Plastic pipet Kimwipes Procedure 1. Obtain and wear goggles. 2.
While the water was sitting, I put each portion of beet into individual beakers and began to test each portion individually. For tests 1-4 I soaked each piece of beet in water warmed to it’s corresponding temperature for one minute. I then removed the beet from the water and placed it back into its beaker then added 3ml of the room temperature tap water. I then let it sit for 20 minutes. For test 5, I placed the dry beet in its beaker and put it into the refrigerator for 30 minutes, removed it, and added 3ml room temperature tap
I then added 15 mL of distilled water and heated to a boil and removed, then poured the liquid from the beaker into the same paper cup that held the previous liquid. I placed the beaker holding the sand into my oven to dry. Once dried I poured the sand into my weighing dish and measured its mass and calculated and recorded into table 1. While the sand was drying I placed the paper cup into a larger coffee cup filled with crushed ice and water and let it set for about five minutes. I weighed the filter to find out the mass.
Allow the crystals to dry for 1 week then, weigh it, take a MP, and calculate the % yield. * Assemble the apparatus for reflux using the diagram (see figure 1), place boiling chips or a stirring bar in the bottom of the flask. * Weigh 2grams of finely ground nutmeg and combine with 10ml of diethyl ether in a 50ml round bottom flask. * Place a heating mantle under the round bottom, turned on and the heat was slowly adjusted until the mixture starts to boil for 45minutes, then let cool to room temperature by sitting it on the lab bench. * Pour a little ether over the nutmeg residue on the filter paper so that any Diethyl ethanol traces clinging to it is washed down and mixed with the filtered liquid underneath.
Organic Chem. Lab EXPERIMENT 11: ISOLATION OF CAFFEINE FROM TEA LEAVES COMPOUND PROCEDURE Preparation of Tea Solution: We started out experiment by weighing out 5.023g of tealeaves and 2.008g of calcium carbonate powder. These two substances were mixed with 50ml of water and heated under gentle reflux in a round-bottom flask using a condenser apparatus. The hot solution was then filtered and the filtrate was collected and cooled. Extraction and Drying: Using a separatory funnel, the cooled filtrate was extracted with 10ml of methylene chloride.
Experiment Colligative Properties & Osmotic Pressure Karmin Currin 1/19/2014 1:00pm Abstract The purpose of this experiment is to understand and compare the difference of the freezing points between pure solvents in a solution and a non-volatile solute. Secondly, osmosis is demonstrated in a permeable membrane in this case a dialysis tubing and a less permeable membrane with a much harder shell like the egg. Experiment and Observation Starting with Part I of this experiment I gathered together all my items I needed. Small rubber band, salt, tap water, distilled water, 1/8 teaspoon measuring spoon, crushed ice, beaker 100 mL plastic, stopwatch-digital, test tube 13 x 100 mm, digital thermometer, well plate-24. First I made a water bath by filling the 100 mL beaker with cool tap water.
The mixture was decanted again in to the same beaker. Next, we added boiling chips to the liquid and evaporated the solvent over the hot plates under the hood. After the solvent was evaporated and the flask was cooled, we used a spatula to remove a small amount of the crude product and took its melting point. We determined the melting point range of the sample to be 43.0-46.0 degrees Celcius.The crude product was yellow colored when it was warm and orange in color when cooled and sticky. We then recrystallized our sample using 5 ml of warm acetone that was heated on a hot plate under a hood.
Specific Heat of a Metal Michael Diaz Ms. Zhort Performed: October 3, 2013 Due: October 24, 2013 Period: 1 Lab Partner: Rocco & Asha Objective: This lab was meant to teach us how to find the specific heat of a metal sample. Materials: * Specific heat set * Balance * Thermometer * Tap Water * Hot plate * Polystyrene cup and a lid * Stirring rod * 250 mL beaker * String (about 15 cm) Procedure: 1. Fill a 250 mL beaker approximately half full of water. Place the beaker of water on a hot plate. Begin heating the water to the boiling point.
Materials and Methods Materials The compounds used in this lab are listed in the table below: Procedure We boiled 2 NoDoz tablets in grinded form with 60 mL of water in a 100 mL beaker and allowed it to cool to room temperature after it had been sitting on the hot plate for 5-10 minutes. Next, we performed a hot gravity filtration by pouring the hot aqueous solution of water and NoDoz (caffeine and insoluble binder) through a large Buchner funnel into an Erlenmeyer flask. We discarded the collected insoluble binder collected inside of the Buchner funnel and performed an extraction by mixing the aqueous solution collected in the Erlenmeyer flask (aqueous solution of water and caffeine) and 15 mL of methylene chloride in a separatory funnel and swirled until the layers had separated to form an aqueous layer on top and an organic layer containing the solvent and caffeine at the bottom of the funnel. We drained the lower layer into an Erlenmeyer flask and repeated the extraction. Next, we added anhydrous sodium sulfate to the Erlenmeyer flask, which contained the combined organic layers of the 2 extractions,