Purpose/Introduction What were we trying to accomplish with this experiment? What method did we implement to accomplish the task? What techniques were used to purify and identify the product(s) of the reaction? In this experiment, an acid-base extraction was done to separate a mixture of an unknown acid and fluorene, a neutral compound. The possible unknown acids were 2-chlorobenzoic acid, 3-chlorobenzoic acid, and 3-methylbenzoic acid. The purification of the isolated unknown acid was performed by recrystallization and its identity was established by analyzing the melting point range of the pure product and comparing it to the provided standards. In addition, a mixed melting point experimentation enhanced the fidelity of the unknown's identity when approximately equal amounts of the unknown and one of the standards (at a time) were mixed and the melting point range was recorded. Theory: Explain the theory behind acid base extraction. Why is it possible to separate compounds of different polarity? What establishes the selection of solvents used in an extraction? Briefly comment on how you will recrystallize the unknown acid and how melting point analysis is necessary. A convenient method of separating a mixture of organic compounds is recognized as liquid-liquid extraction, which involves the dispersion of a substance between two immiscible solvents using preferential solubility. Strategically using the differences in solubility of the interested solute, the compound can be transferred from one liquid part to the other during extraction. Organic acids and bases can be separated from each other by using an organic solvent like diethyl ether and a polar solvent such as water. Diethyl ether is an appropriate solvent since it wil... ... middle of paper ... .... Conclusions and Future Experiments: How would you summarize your results and analysis? What questions remain unanswered? What questions were raised by your results and analysis? In summary, acid base extraction is a useful technique when attempting to transfer an organic compound from an organic solvent (ether) to an aqueous solvent after deprotonation with an appropriate base (NaOH). After transferring the unknown acid to the aqueous layer, precipitating it out of solution with a strong acid (HCl--protonation), followed by recrystallization, the unknown acid was able to be identified as 2-chlorobenzoic acid based off of melting point experimentation. A question that remains unanswered may be how many extractions are needed in order to have a plateau for maximum recovery? This is essential in order to have desirable results when testing for identity purposes.
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.
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.).
In this experiment, a mixture of three substances (benzoic acid, 2-naphthol, and 1-4 dimethoxybenzene) will be separated based off acidity strength using the liquid-liquid extraction technique through a separatory funnel. Benzoic acid and 2-napthol will be converted into ionic salts when reacting with their appropriate bases (sodium bicarbonate and sodium hydroxide). Both ionic salts will then form solids through the addition of acidic HCl. Neutral 1,4 – dimethoxybenzene forms a solid through the evaporation of ether. Each compound will then be purified through recrystallization, using the processes of dissolving the solid in either water or methanol, and isolating the solid through vacuum filtration. After a week of evaporation, the compounds will then be examined for both
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.
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
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
This experiment involves performing various techniques, including heating under reflux, separation, drying, distillation, gas chromatography (GC), infrared spectroscopy (IR spectroscopy), and nuclear magnetic resonance (1H NMR). Heating under reflux is important to overcome any activation barrier of energy that may be present in order to complete the reaction.
In this lab had to use acid- base extraction process. Since isopentyl acetate is soluble in diethyl ether, but acetic acid is soluble in both solvents. Therefore, a simple extraction procedure would remove only some of the acetic acid from isopentyl acetate, but it would not completely separate the two compounds.
In order to ensure the most accurate data, a purification was performed by the process of recrystallization. To perform the recrystallization the powder was dissolved in a minimal amount of hot ethanol/H2O solvent that allowed the unknown powder to crystallize properly when cooled. This process allowed for the removal of soluble impurities when suction filtered. A sample of the unknown acid was weighed at 8.24 g, and it was found that 164ml of a 40% ethanol, 60% H20 solvent dissolved the 8.24 g of unknown acid when heated. The beaker containing the dissolved acid was then placed in a beaker containing ice, allowing the unknown acid to recrystallized. After vacuum filtration, the recovered unknown was dried and weighed at 6.92 g. The percent recovery was determined by the following calculation: (8.24--6.92)8.24 x 100% = 16% loss = 84% recovery of unknown.
In this experiment, an acid (Benzoic acid), a base (Ethyl 4- Aminobenzoate) and a neutral compound (9-Fluorenone) were extracted from a mixture. HCl was the acid used to separate the base from the mixture, by forming an organic layer, which contained the acid, the neutral compound, and an aqueous layer that contained the base. NaOH was the base that was used to separate the acid from the neutral compound, which resulted in an organic layer containing the neutral compound and an aqueous layer containing the acid. After this a base was then added to the first aqueous layer containing the base, and an acid added to the second aqueous layer containing the acid. The percent recovery of each compound was then evaluated. The basic component, Ethyl
The purpose of this particular experiment is to acquire the product 4-methylcyclohexene from the reactant 4-methylcyclohexanol by altering the equilibrium and using an elimination (E1) reaction involving dehydration with a strong acid acting as a catalyst. The following techniques and analyses were utilized in this experiment: simple distillation, “salting-out” the crude product, neutralization, unsaturation test, and infrared spectroscopy. Simple distillation is necessary for separating a liquid mixture and collecting the purified product or desired result. “Salting-out” the crude product was employed as a means of an extraction and purification process; that is, the salt would extract the water from the mixture, which leads to a reduction in solubility of the organic compound.
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...
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.
An acid-base indicator is a substance that undergoes a distinct colour change at or near the equivalence point. The point in the titration at which the colour change occurs is called as end point. Obviously, the titration will be accurate only if the end point and the equivalence point coincide fairly closely. For this reason, an acid-base indicator used in this acid-base titration must be selected carefully in order to obtain an accurate result. Thus, the acid-base indicator used in this experiment is the phenolphthalein. Besides, phenolphthalein is also a suitable indicator for titration between a strong base and a weak acid. Phenolphthalein is colourless in an acid solution but pink in base solution. Phenolphthalein was added into both original oxalic acid (C2H2O4) and acetic acid (CH3COO) solution before the acid-base titration was carried out. Phenolphthalein is a weak acid and is represent as Hln in the following chemical
The sample was subjected to steam distillation as illustrated in Figure 1. A total of 50ml of distillate was collected while recording the temperature for every 5.0 ml of distillate. The distillate was transferred into a 250ml Erlenmeyer flask and 3.0 g of NaCl was added. The flask was cooled and the content was transferred into a 250-ml separatory funnel. Then 25.0ml of hexane was added and the mixture was shaken for 5 minutes with occasional venting. The aqueous layer was discarded and the organic layer was left inside. About 25.0ml of 10% NaOH was then added and the mixture was shaken as before. The aqueous layer was collected and then cooled in an ice bath. It was then acidified with enough 6.00 M HCl while the pH is being monitored with red litmus paper. Another 25.0 ml of hexane was added and the mixture was shaken as before. The hexane extract was saved and a small amount of anhydrous sodium sulfate was added. The mixture was then swirled for a couple of minutes then filtered. A small amount of the final extracted was tested separately with 1% FeCl3 and Bayer’s reagent.