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Acid and base extraction analysis
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Introduction/Background
Acid- Base Extraction is a method used to separate organic compounds from mixtures. The theory of Acid-Base Extraction states most organic compounds are more soluble in organic solvents than in water. However, if the organic compound is rendered ionic, it becomes more soluble in water than in the organic solvent (Schaller). Because the two solvents are immiscible, they will form two layers which allows for separation of the lower layer using a separatory funnel. The name “Acid-Base Extraction” is given to this technique because by adding an acid or base to a mixture, we can extract a Base or an Acid. In this experiment, a mixture of benzoic acid, 4-chloroaniline and naphthalene will be separated using the extraction
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method. Using the theory of Acid-Base Extraction, Experimental Section Table of Chemicals Benzoic Acid 4-Chloroaniline Naphthalene Table 1 Chemicals Physical Properties Chemical Properties Benzoic Acid(C7 H6 O2 ) Molar mass:122.1g/mol Boiling Point: 249°C Melting point:122 Combustible at high temperature 4-Chloroaniline (C6H8ClN) Molar mass:127.6g/mol Boiling Point:232.2°C Melting point:69-72.5°C Gives off toxic fumes and gasses Naphthalene(C10H8) Molar mass:128.17g/mol Boiling Point:217.9°C Melting point:80.2°C Diethyl Ether (C4H10O) Molar mass:74.12g/mol Boiling Point:34.6°C Melting point:-116.3°C Burning sweet taste Hydrochloric Acid(HCl) Molar mass:36.46g/mol Boiling Point:85.05°C Melting point:114°C Colorless Sodium Hydroxide (NaOH) Molar mass:39.99g/mol Boiling Point:1388°C Melting point:312°C Odorless Anhydrous Sodium Sulfate (Na2SO4) Molar mass:142.04 Boiling Point:1429°C Melting point:884°C White crystalline Results Table 2 Chemicals Mass Recoveries Actual Melting Point Theoretical Melting Point Benzoic Acid .46g 120°C 122°C 4-Chloroaniline 1g 68.5°C 68-71°C Naphthalene 1.1g 83°C 80 °C Percent Recoveries Benzoic Acid %Yield = Actual / Thereotical * 100 = .46g/1.001g *100 = 45.95% 4-Chloroaniline %Yield = Actual / Thereotical * 100 = 1g/1.001g*100 = 99.9% Naphthalene %Yield = Actual / Thereotical * 100 = 1.1/1.001g *100 = 109.9% Total Percent Recovery %Yield = Actual / Thereotical * 100 = 2.56g/3.004g *100 = 85.22% Discussion The results from the experiment showed that actual melting point was very accurate to that of the theoretical melting points of Benzoic Acid, 4-Cloroaniline, and Naphthalene.
This shows that our experiment yielded the correct form of each compound. The percent recovery was accurate for 4-Cloroaniline and Naphthalene yielding 99.9 and 109.9 % respectively while Benzoic Acid only yielded 45.95%. Possible reasons for Benzoic Acid yielding such a low percentage might be because of not capping the separator funnel while working to precipitate 4-chloraniline, also not removing all of the Benzoic Acid from the separatory funnel adds to a recovery less than …show more content…
100% Conclusion In this experiment, Acid- Base Extraction was used in separating an organic mixture containing Benzoic Acid, 4-Cloroaniline, and Naphthalene.
Confirming the Acid- Base extraction theory the acid, base and organic compound making up the organic mixture were separated using a separatory funnel. Techniques performed in this lab can be applied to real life situations such as the extraction or purification of petroleum.. This Acid-Base technique performed remarkable well and separated the organic compounds from the mixture as it set out to do.
References
"Acid-Base Reactions." Science of Everyday Things. 2002, and Melvin D. Joesten. "Acid-Base Reactions." Encyclopedia.com. HighBeam Research, 01 Jan. 2002. Web. 17 Sept. 2015.
Centers for Disease Control and Prevention. Centers for Disease Control and Prevention, 01
July 2014. Web. 17 Sept. 2015.
"Naphthalene." Naphthalene. N.p., n.d. Web. 17 Sept. 2015.
Schaller, Chris P. "Acid-Base Extraction." - Chemwiki. N.p., 02 Oct. 2013. Web. 17 Sept. 2015.
Weldegirma, Solomon. "Simple and Fractional Distillation." Experimental Organic Chemistry. N.p.: 2015, n.d. 1-9.
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The hypothesis that was formed in this experiment was that decantation and distillation were the techniques that would be successful in separating the three layered substances. The oil on top of the mixture was to be decanted solely, and the salt and sand layers would be distilled and separated together on filter paper on top of boiling hot water. The reason that the oil is decanted is because it doesn’t mingle with the salt and sand layers, and in addition it was the top layer, which was thought to have been easy to separate first. And as for the sand and salt, sand doesn’t mix and dissolve in water compared to salt, which does in fact dissolve, so distillation was thought to be the proper solution to separating the two
The purpose of this experiment was to learn and preform an acid-base extraction technique to separate organic compounds successfully and obtaining amounts of each component in the mixture. In this experiment, the separation will be done by separatory funnel preforming on two liquids that are immiscible from two layers when added together. The individual components of Phensuprin (Acetylsalicylic acid, Acetanilide, and Sucrose as a filler) was separated based upon their solubility and reactivity, and the amount of each component in the mixture was obtained. Also, the purity of each component will be determined by the melting point of the component.
...form 〖PbCrO〗_4 and then process it through a filter. After filtering the 〖PbCrO〗_4 I had to dry the 〖PbCrO〗_4 residue in the drying oven for 30 minutes at 80℃. Then let it cool for 5 minutes and weigh it and finally make a few calculations to obtain the theoretical, actual, and percent yields of 〖PbCrO〗_4. I was able to fulfill the experiment because I obtained all the answers to the equations in an accurate amount. I believe this experiment was a success due to my hypothesis of, If physical methods are used to separate 〖 PbCrO〗_4 precipitate from the reaction mixture then I can successfully calculate the theoretical, actual, and percent yields, being correct.
In order to separate the mixture of fluorene, o-toluic acid, and 1, 4-dibromobenzene, the previously learned techniques of extraction and crystallization are needed to perform the experiment. First, 10.0 mL of diethyl ether would be added to the mixture in a centrifuge tube (1) and shaken until the mixture completely dissolved (2). Diethyl ether is the best solvent for dissolving the mixture, because though it is a polar molecule, its ethyl groups make it a nonpolar solvent. The compounds, fluorene and 1, 4-dibromobenzene, are also nonpolar; therefore, it would be easier for it to be dissolved in this organic solvent.
Felder, M. Richard, Elementary Principles of Chemical Processes, 3rd ed.; Wiley: New Jersey, 2000; p 631.
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.
As shown in Fig. 5, the final pH of the NaClO-NH3 solution after simultaneous removal are 5.4, 6.9, 7.2, 7.5, 8.5, 9.6, 10.7, 11.5 and 12.8 with respect to the initial pH of 5, 6, 7, 8, 9, 10, 11, 12 and 13, from which, an interesting law can be concluded as that if the initial pH is an acidic, the final pH is slightly increased; but if the initial pH is an alkaline, the final pH is declined. NaClO-NH3 is macromolecule compounds with a large inter surface area. It contains abundant functional groups such as hydroxyl (OH), carboxyl (COO), quinone, amino (–NH2), etc, which determines that NaClO-NH3 is a salt of strong base and weak acid, as well the ionization equilibrium and hydrolytic equilibrium would be complicated. When the pH of the NaClO-NH3 solution was acidic, the functional groups such as OH, COO and NH2- would react with H+ to generate the NH3 sediment, resulting in a decrease of inter surface area owing to the block and a great loss of NaClO-NH3, then the NOx removal as well as the duration time was decreased. As for the increase of the final pH in the acidic conditions, this was a result of the consumption of H+ by NaClO. The decrease of the
Performing this experiment, we used the technique called Acid-Base extraction to isolate Eugenol, which is one of the main ingredients of clove oil. Acid-Base extraction is the most efficient method for isolating organic component; it is efficient because it purifies the acid and base mixture based on their chemical identities. We have seen throughout this experiment that acid and base play an important role, when it comes to solubility in water. Our basic knowledge of acid and base is acid is a proton donor and base is a proton acceptor. This ideology helps us to understand why organic compounds are not soluble in water. When compounds tend to be insoluble, we have to use acid and base reaction, to change its solubility. The changes that occurred
acid and water to see how it affects the rate of reaction. I will use
Ensure gloves are worn at all times when handling strong acids and bases within the experiment of the preparation of benzocaine. 4-aminobenzoic acid (3.0g, 0.022 moles) was suspended into a dry round-bottomed flask (100cm3) followed by methylated sprits (20 cm3). Taking extra care the concentrated sulphuric acid of (3.0 cm3, 0.031 moles) was added. Immediately after the condenser was fitted on, and the components in the flask were swirled gently to mix components. It should be ensured that the reactants of the concentrated sulphuric acid and the 4-aminobenzoic acid were not clustered in the ground glass joint between the condenser itself and the flask. In order to heat the mixture to a boiling point, a heating mantle was used and then further left for gently refluxing for a constituent time of forty minutes. After the duration of the consistent forty minutes the rou...
Preparing Benzoic Acid from Benzylalcohol Planning (a) Problem The aim of this experiment is to synthesize benzioc acid, with the highest possible yield, by oxidizing benzylalcohol. Hypothesis We expect the percentage yield to be about 50% due to several processes such as cooling and filtering. Possible Variables - Time - Temperature (of water) - Filter Planning (b) Apparatus/ Materials - Round bottomed flask under reflux - benzylalcohol - HCl - Na2O4 - Büchner funnel - beakers - sodium carbonate Procedure The benzioc acid is synthesized by heating benzylalcohol in a round bottomed flask under reflux. In addition to that, we use Na2O4 as a oxidizing agent. After that, we use HCl to precipitate it.
Extraction of Asphalt from a mix is a common practice in the asphalt laboratories. The extracted asphalt is used for characterization in the laboratories to ensure quality, performance and research. ASTM D2172 is the most accepted procedure for asphalt extraction. This procedure includes five methods such as Method A the centrifuge extraction, Method B the Reflux extraction, Method C first variation of the Reflux method, Method D the second variation of Reflux method and Method E the vacuum extraction. Among them centrifuge method is most popular because the asphalt extracted using Reflux method is subjected to more aging and the vacuum extraction method is not used in a regular basis. There are other methods which are as follows Determination of asphalt binder content from asphalt mixtures using the Asphalt Nuclear Gauge and Determination of Asphalt binder content of Hot Mix Asphalt (HMA) by ignition method. However, in this paper the discussed methods will be limited within chemical based extraction method. Extracted asphalt has to be recovered from the solution. The methods used for recovery are ASTM D1856, Recovery of Asphalt from Solution by Abson method and ASTM D5404, Recovery of Asphalt using Rotovapor apparatus. The solvents used for recovery are trichloroethylene, methylene chloride, 1, 1, 1-trichloroethane, and nitration based benzene etc. Among them benzene is the most toxic solvent. The properties obtained from these test methods were erroneous so it was necessary to develop new methods. Strategic Highway Research Program (SHRP) developed modified extraction and recovery procedures to compensate those errors. The SHRP extraction procedure (AASHTO TP2) is more precise as it uses rotating cylinder with baffled inside wh...
Acid-base chemistry is central to us on a practical level as well, outside of laboratory chemical reactions. Our bodily functions, going from the microscopic transport of ions through nerve cell membranes to the macroscopic acidic digestion of food in the stomach, are all lined by the principles of acid-base chemistry. Homeostasis, the temperature and chemical equilibriums in our bodies, is preserved by acid-base reactions. For example, fluctuations in the pH, or concentration of hydrogen ions, of our blood
For essential oil extraction, dry plant materials of rosemary distilled within 24 h in a steam distiller with an aqueous phase recycling system, using a plant material: water ratio of 2:1. The distillation time was about 2 h, and the oil obtained was separated from the aqueous solution and dried by treating with anhydrous Na2SO4. Each essential oil was transferred into a dark glass flask filled to the top and kept at a temperature of 4 °C until used (Meepagala et al., 2002). Also for mucilage extraction, Cactus stems were removed skin and cubed (1 cm3). Samples were homogenised (20% w/v) in distilled water. The slurry was centrifuge for 10 min at 4,500 rpm and the supernatant precipitated in ethanol and finally dried (Sáenz et al., 1992).
Crude petroleum is separated into its component compounds by fractional distillation. The procedure involves a sample of the petroleum to be heated until the sample is vaporized leaving behind any solid impurities. The resulting steam enters a fractional distillation column in which a temperature gradient had been instilled. The temperature of the column decreases as the steam rises through the column. The idea is that, as the temperature of the column decreases, the vapor temperature will decrease. When the boiling point of a compound is passed, the compound will condense on the sides of the column and be collected in the fraction well at that point. Thus the mixture is separated into fractions of compounds with similar boiling points in a mixture.4 Adamantane’s high boiling point caused it to be one of the initial compounds to condense with the kerosene fraction in the 190o C cut.5