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Using chromatography for seperating photosynthetic pigments
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Procedure:
Extracting the pigments- Combined five milliliters of spinach in ethanol with five milliliters of cyclohexane in a test tube. Inserted a test tube stopper and shook. Once settled, pipetted the top layer into a small glass container. Added another five milliliters of cyclohexane to the spinach and repeated.
Separating remnants of polar solvents- Added ten milliliters of water to the cyclohexane, carefully stirred and added a solution of brine when an emulsion appeared, then carefully stirred again. Pipetted the top layer into another glass container, added water again, stirred, and pipetted the top layer into an erlenmeyer flask. Used a spatula to scoop anhydrous sodium sulfate into the cyclohexane mixture until it no longer stuck together at the bottom of the flask. Set up and ran the vacuum filter.
Concentrating the sample- Once all of the cyclohexane was filtered into the round bottom flask, removed and connected it to the rotary evaporator and allowed evaporation until the flask fully dried.
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Prepared 20 milliliters of eluent two by combining 10 milliliters of eluent one with 10 milliliters of cyclohexane in a beaker. Prepared 20 milliliters of eluent three by combining 10 milliliters of cyclohexane with 7 milliliters of eluent one and 3 milliliters of acetone in a beaker. Drew the starting point on three TLC plates, then applied one spot of the concentrated sample on each of the three TLC plates. Ran each TLC plate with one of each eluent systems to determine the best eluent, marked the stopping point and eluent used on each plate. Used the UV light to decide which eluent yielded the most spots. Eluent three showed the most spots. Made approximately twenty milliliters of eluent three in a beaker, marked it, covered it with a watchglass and set it aside for
The goal of this two week lab was to examine the stereochemistry of the oxidation-reduction interconversion of 4-tert-butylcyclohexanol and 4-tert-butylcyclohexanone. The purpose of first week was to explore the oxidation of an alcohol to a ketone and see how the reduction of the ketone will affect the stereoselectivity. The purpose of first week is to oxidize the alcohol, 4-tert-butylcyclohexanol, to ketone just so that it can be reduced back into the alcohol to see how OH will react. The purpose of second week was to reduce 4-tert-butylcyclohexanol from first week and determine the effect of the product's diastereoselectivity by performing reduction procedures using sodium borohydride The chemicals for this lab are sodium hypochlorite, 4-tert-butylcyclohexanone
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
Analysis of the Absorption of Green Light Versus Red Light Absorption in Spinach Leaves. The goal of the experiment was to determine if green light had less ability to absorb than red light in spinach leaves. This was done by separating the photosynthetic pigments (chlorophyll a, chlorophyll b, carotene and xanthophylls) from one another using paper chromatography. The separated pigments were then analyzed for their absorption spectrum using a spectrographometer.
Firstly, an amount of 40.90 g of NaCl was weighed using electronic balance (Adventurer™, Ohaus) and later was placed in a 500 ml beaker. Then, 6.05 g of Tris base, followed by 10.00 g of CTAB and 3.70 g of EDTA were added into the beaker. After that, 400 ml of sterilized distilled water, sdH2O was poured into the beaker to dissolve the substances. Then, the solution was stirred using the magnetic stirrer until the solution become crystal clear for about 3 hours on a hotplate stirrer (Lab Tech® LMS-1003). After the solution become clear, it was cool down to room temperature. Later, the solution was poured into 500 ml sterilized bottle. The bottle then was fully wrapped with aluminium foil to avoid from light. Next, 1 mL of 2-mercaptoethanol-β-mercapto was added into fully covered bottle. Lastly, the volume of the solution in the bottle was added with sdH2O until it reaches 500 ml. The bottle was labelled accordingly and was stored on chemical working bench.
Then, I added 8 drops of concentrated phosphoric acid to the mixture. swirling it a few times. Then, I carefully took the flask to the station as I avoided trying to breath the vapors of the acetic anhydride. I put the e-flask into the beaker of water sitting on the hot plate in order to heat it for seven minutes. Once the seven minutes was up, my partner carried the e-flask to the fume hood, and added 3 mL of de-ionized water to the flask. She swirled it for a couple of minutes there. She brought it back tot he station where I gradually added 60 Ml of de-ionozed water to the mixture while my partner stirred the mixture constantly. I was able to see some of the aspirin beginning to form. In order to complete the crystallization process we cooled the flask in an ice-water bath from 4:00 until 4:20. As we waited I began to set up our filtration system. I used a ring stand, right angel clamp, three finger clamp, Buchner funner, filtering flask,rubber tubing, and filter paper in the Buchner funnel. I turned on the aspirator and pored some water over the filtering paper in order to create a good
The objective of this experiment was to perform extraction. This is a separation and purification technique, based on different solubility of compounds in immiscible solvent mixtures. Extraction is conducted by shaking the solution with the solvent, until two layers are formed. One layer can then be separated from the other. If the separation does not happen in one try, multiple attempts may be needed.
Experiment #3: The purpose of this experiment to test the chromatography of plant pigments the alcohol test strip test will be used.
In this lab 4-tert-butylcyclohexanone is reduced by sodium borohydride (NaBH4) to produce the cis and trans isomers of 4-tert-butylcyclohexanol. Since the starting material is a ketone, NaBH4 is strong enough to perform a reduction and lithium aluminum hydride is not needed. NaBH4 can attack the carbonyl group at an equatorial (cis) or axial (trans) position, making this reaction stereoselective. After the ketone is reduced by the metal-hydride, hydrochloric acid adds a proton to the negatively charged oxygen to make a hydroxyl group. The trans isomer is more abundant than the cis based on the results found in the experiment and the fact that the trans isomer is more stable; due to having the largest functional groups in equatorial positions.
During this week’s lab, both the cis and trans enantiomers of 2-methylcyclohexanol will be produced through the reduction of 2-methyclcyclohexanone with sodium borohydride. Once the product is formed, NMR signals are used to examine the product of this reduction by observing the cis and trans location of the CH2OH group. The integration of the signal will then be examined and to show the ratio of cis and trans product that is formed through this reaction.
Use glassware as directed by your instructor. Place a test tube placed inside a beaker with ice water to collect the product from the apparatus. Obtain the 10mL round bottom flask from the apparatus. Obtain two graduated cylinders of 10mL. On one graduated cylinder measure 4mL (85% H3PO4) of Phosphoric Acid and pour into the 10mL round bottom flask. On the other graduated cylinder measure 3mL of Cyclohexanol and pour into the flask as well. With a pipet add 5 drops of Sulfuric Acid (H2SO4) into the flask. Attach the round bottom flask to the distillation apparatus. Place thermometer with rubber stopper on the apparatus to obtain the temperature Start with the water flow through the condenser. Turn on and heat the reaction until the product starts to distill. Distill and collect until thermometer temperature rises to 85˚C. Once there is no more product to collect obtain the test tube of product. Two layers should be formed, top layer of cyclohexane and bottom layer with water. Obtain a pipette and remove the bottom layer (water) if any. Add 10% (5mL) of Sodium Bicarbonate (NaHCO3) to nuclearize any acid in the solution. Mix well and remove once again the bottom layer of water with pipette. Add 5mL of water and mix well to wash the top layer. After the two layers form again, remove entirely the bottom layer of water and add a few pellets of Calcium Chloride. Obtain a 50mL or 100mL beaker and weigh.
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
Once the mixture had been completely dissolved, the solution was transferred to a separatory funnel. The solution was then extracted twice using 5.0 mL of 1 M
== § Test tubes X 11 § 0.10 molar dm -3 Copper (II) Sulphate solution § distilled water § egg albumen from 3 eggs. § Syringe X 12 § colorimeter § tripod § 100ml beaker § Bunsen burner § test tube holder § safety glasses § gloves § test tube pen § test tube method = == = =
The working begins with an auto-sampler which picks up a definite amount of sample as programmed from the defined tube and passes in to the pump wherein it is mixed with the mobile phase in definite proportion. This is followed by entry of the mixture into the column under high pressure which aids in separation. The individual analytes in the mixture will interact with the stationary phase and finally be eluted out at a definite retention time. The retention time of each eluting component is recorded and based on this data the output is displayed in the graphical format. Peaks are seen on the graph and each peak corresponds to a particular component in the mixture, while the area under the curve of the peak denotes the concentration of the analyte. The higher the number of peaks, more is the number of analytes present in the
To the first Erlenmeyer flask with the ferrous salt add about 1/3 of the 0.75N sulfuric acid. Dissolve the salt by gently swirling it in the dilute acid. Add about 5mL of the Zimmerman-Reinhardt Reagent (this reagent contains phosphoric acid which complexes yellow ferrous ions into colorless compounds which do not obscure the endpoint; it also contains manganous ions which inhibit the oxidation of any chloride ions in the sample). The use of a white background underneath the flask aids in the detecting of the endpoint. Repeat with second sample.