AcidbaseExtraction

The purpose of this laboratory assignment was two-fold, first, we were to demonstrate the extraction of acids and bases, finally, determining what unknowns were present. Second, we were to extract caffeine from tea. These two assignment will be documented in two separate entities. Introduction: Acid/base extraction involves carrying out simple acid/base reactions in order to separate strong organic acids, weak organic acids neutral organic compounds and basic organic substances. The procedure for this laboratory assignment are on the following pages. 3) Separation of Carboxylic Acid, a Phenol and a Neutral Substance The purpose of this acid/base extraction is to separate a mixture of equal parts of benzoic acid(strong acid) and 2-naphthanol(weak base) and 1,4-dimethoxybenzene(neutral) by extracting from tert-butylmethyl ether(very volatile).The goal of this experiment was to identify the three components in the mixture and to determine the percent recovery of each from the mixture. 4) Separation of a Neutral and Basic Substance A mixture of equal parts of a neutral substance containing either naphthalene or benzoin and a basic substance containing either 4-chloroaniline or ethyl 4-aminobenzoate were to be separated by extraction from an ether solution. Once the separation took place, and crystallization was carried out, it became possible to determine what components were in the unknown mixture, by means of a melting point determination. Results Procedure Observations Inference Dissolve 3.05g Phenol Mixture was a golden- Neutral acid in 30ml brown/yellow color t-butyl methyl ether in Erlenmeyer flask and transfer mixture to 125ml separatory funnel using little ether to complete the transfer Add 10 ml of water Organic layer=mixture aqueous layer=water(clear) Add 10 ml saturated aqueous Sodium bicarbonate NaHCO3 dissolves in solution sodium bicarbonate water. to funnel and mix cautiously with stopper on Vent liberated carbon Carbon dioxide gas dioxide and shake the mixture was released three times thoroughly with frequent venting of the funnel Allow layers to separate Layer = H2O +NaHCO3 completely and draw off lower layer into 50ml Erlenmeyer flask 1 Add 10ml of 1.5 aqueous NaOH Flask 2 = H2O + NaHCO3 (5ml of 3M and 5ml H2O) to separatory funnel, shake mixture, allow layers to separate and draw off lower layer into a 25ml Erlenmeyer flask 2. Add additional 5ml of water to funnel, shake as before Add 15 ml NaCl to funnel. Shake Bottom layer is white and NaCl was added to the mixture and allow layers to separate gooey. wash the ether and draw off lower layer, which is layer and to remove discarded organic substances NaOH and NaHCO3 Pour ether layer into 50ml Erlenmeyer flask from the top of the separatory funnel (not allowing any water droplets to be transferred) Flask 3 Add anhydrous NaSO4 to ether extract until it no longer clumps together and set it aside Acidify contents of flask 2 Litmus went from Acidification was now by dropwise addition of blue to pink. Flask complete concentrated HCl while 2 = creamy color testing with litmus paper and cool in ice Acidify contents of flask 1 Litmus went from Acidification was now by adding HCl dropwise blue to pink. Flask complete while testing with litmus 2 = white solution paper and cool in ice Decant ether from flask 3 into a tared flask Boil ether with boiling chips Do a vacuum filtration and Solution turns to a Crystallization is now recrystallize ether by dissolving it solid. complete in 5ml, taking out boiling chips, adding drops of Ligroin until the solution was cloudy and cool it in ice Isolate crystals from flask 2 by Crystals = creamy-white Dried crystals are now vacuum filtration and wash with powder ready for melting point a small amount of ice water determination and recrystallize it from boiling water Repeat the above for flask 1 Crystals = white powder Flasks number 4 and 5 were done by the following diagram. Results: As a result of this acid/base experiment, the following results were obtained: Flask 1: 31.113g -30.223g .890g Flask 2: 36.812g -36.002g .810g Flask 3: 90.789g -90.114g .065g % yield = experimental weight x 100% theoretical weight Flask 1: .890g x 100% = 89% 1.00g Flask 2: .810g x 100% = 81% 1.00g Flask 3: .675g x 100% = 67.5% 1.00g When taking the melting points of the unknowns, flasks 4 and 5, I came to the conclusion that the samples contained, benzoin, melting point of 136-137Degrees(C) and 4-chloroaniline, melting point of 67-80 degrees(C), respectively. Flask 4: 90.912g -89.174g 1.738g % yield = 1.738g x 100% = 90.4% 1.922g Flask 5: 87.833g -86.064g 1.769g % yield = 1.769g x 100% = 87.3% 2.027g Conclusion: After each procedure was complete, it became apparent that flask number 4 and flask number 5 contained benzoin and 4-chloroaniline, respectively. The melting point range that was experimentally determined for each was 136-137 for benzoin and 67-70 for 4-chloroaniline. As you can see, this experiment was not error-free, as my percentage yield was not 100%. This is expected for any experiment; for there is no way that, under the conditions, this experiment can be free of error. This error could have occurred for many reasons. The most prevalent reason, I feel that maybe not all of the substance was transferred from the flask to the vacuum, giving a slight error. Also, some residue could have also been left in the vacuum funnel when transferring the crystal substances. Questions 2) It is necessary because nothing would come out of the stopcock- the reason for this is because of pressure. Leaving the stopper on, would decrease the pressure pushing down on the liquid and the pressure pushing upward would prevail, allowing nothing to escape. 3) I would not expect p-nitrophenol (pka = 7.15) to dissolve NaHCO3(pka = 6.4) because having a weak acid and a weak base, the reaction would favor the products, not the reactants, hence, the reaction would not proceed forward. I would expect 2,5-dinitrophenol(pka = 5.15) to dissolve in NaHCO3 the reaction would proceed forward. 5) a) 1g benzoic acid x 1mol = .00699 mol benzoic acid 143g benzoic acid b) 1ml 10% solution NaHCO3 x 1g_ x 1mol = .00116 mol NaHCO3 4ml 96g NaHCO3 .00699 moles of benzoic acid Introduction: The purpose of the second part of this laboratory assignment was to extract caffeine from tea using dichloromethane and then to confirm the identity of it by preparing a derivative of the extracted caffeine which has a sharp melting point, unlike caffeine itself. Once the extraction was complete, we were to test for melting point and get a HPLC reading for our derivative. Discussion: Tea leaves contain acidic, colored compounds as well as a small amount of undecomposed chlorophyll, which is soluble in dichloromethane. Caffeine can be easily extracted from tea. This procedure can be done using conventional methods. Simply pouring hot water on the tea bags and steeping the bags for about 5-7 minutes would extract most of the caffeine that the tea contains. Pure caffeine itself is a white, bitter, odorless crystalline solid, therefore, it is obvious that more than just caffeine is in the liquid tea solution since tea is a brown color. Because of this, dichloromethane is used to dissolve the caffeine that is in the tea, which leaves the other constituents in the aqueous layer. Using a separatory funnel, it becomes possible to extract the dissolved caffeine from the aqueous layer and the extraction is now ready for further procedure. Results Procedure Observation Inference To a 250ml beaker containing 7 tea bags, add 100ml of boiling water. Allow the mixture to stand Brown aqueous solution for 5-7 minutes while steeping containing caffeine and the tea from the bags other impurities. Decant the mixture into another flask Cool solution to near Dichloromethane = room temperature and water soluble, clear, extract twice with 15ml heavier that water. portions of dichloromethane using a gentle rocking motion and venting. Drain off dichloromethane Dichloromethane Evaporation of the layer on first extraction; organic layer found solvent leaves crude include emulsion layer on on the bottom of the caffeine, which on the second extraction. funnel where the sublimation, yields caffeine is dissolved. a relatively pure Chlorine = top, aqueous product. solution. Drain extraction 1 and 2 back into the funnel Dry combined dichloromethane The solvent layer is solutions and any emulsion yellow. layer with sodium sulfate Wash the drying agent Residue of greenish with further portions of white crystalline weighs solvent and steam bath 50mg(solid) the solvent To 5mg of the Salicylic acid is water sublimed caffeine in water soluble. beaker, add 7.5mg of salicylic acid and .5 ml of dichloromethane. Heat mixture to a boil Petroleum ether is a poor and add a few drops solvent for the product. petroleum ether until the mixture turns cloudy. Insulate beaker and allow it to cool slowly to room temperature and then cool in an ice bath Remove the solvent with Needle-like crystals are Caffeine salicylate is a Pasteur pipette while the isolated(white color) formed. beaker is in the ice bath then vacuum filter. Caffeine beaker: 51.61g -51.56g .05g = 50mg % yield = .05g x 100% = 20% .25g Caffeine salicylate: 17.198g -17.036g .062g % yield = .062g x 100% = 25% .25g Conclusion According to the HPLC graph that follows, my product was very pure. The actual melting point of caffeine salicylate is 137 degree(C), my product was found to have a melting point of 138 degrees (C). As before, of course this experiment was not done completely error-free, the error is due almost entirely on human error.