Abstract: The purpose of this experiment was identifying two compounds in an unknown mixture via liquid-liquid extraction and acid-base reactions. The compounds in the unknown mixture isolated by using recrystallization, and then their identity was determined by comparing the experimental melting point values with actual melting points. Unknown mixture 5 contained a carboxylic acid, 4-methylbanzoic acid, and a non-ionizable organic compound, 1,2-diphenylethane-1,2-dione. Purpose: The type of extraction used in this experiment was liquid-liquid extraction, a used technique to separate two liquids in a mixture. In order to do this, the liquids must be immiscible, form distinct layers when mixed. This separation is due to the difference in …show more content…
Also, due to the fact that carboxyilic acids had a lower pKa than the phenols, means that the extraction using NaHCO3 will only ionize a carboxylic acid since they easily donate a proton. Similarly, when extracted using NaOH the aqueous phase will contain the deprotonated phenols as they are weaker acids and require a stronger base. However, if the mixture contains a non-ionizable organic compound, it will not be ionized and thus stay in the organic phase. This is extracted using NaCl and Na¬2SO4 to dry the solution and then using gravity filtration and the rotovap, the solute is …show more content…
The solute in beaker 3 was isolated using gravity filtration and the rotovap and massed 0.283g. Due to the fact that there was originally 0.999g of the unknown mixture, it is assumed that half of the mass should have been in each beaker. However, that was not the case and the following percent recoveries were calculated: the percent recovery for 4-methylbenzoic acid was 55.8% and the percent recovery for 1,2-diphenylethane-1,2- dione was 56.6%. The calculated values for the percent recovery show that not all of the original mixture was recovered; reasons, as to why this may have occurred will be discussed
Three trials were done. All three trials were done the same way. In trial one, the weigh boat was first zeroed on the scale. Five grams of the white unknown mixture was measured on to the weigh boat.
Unknown substance C is sodium carbonate since the molar mass found in the experiment is 110.03 g/mol which is close to the actual molar mass of sodium carbonate that is 105.99 g/mol. Substance A is lithium carbonate since the lab produced 0.33g of CO2 which can be used to calculate the moles of the unknown substance. Since the moles of the unknown are 0.007498 mol, we can divide the original mass used in the experiment (0.50g) by this to get 66.68 g/mol as the molar mass. This then is relatively close to the molar mass of lithium carbonate which is 73.89
In this experiment, extraction was used as a separation technique to separate the acid, base, and neutral compounds. In extraction, two immiscible solvents with different polarities are used to dissolve and separate different solute components, so they form two distinct liquid layers. In this experiment, ethyl acetate, an organic solvent, and an aqueous solution, were used as the two immiscible solvents. The extraction solvent must be capable of dissolving one of the mixture components, without irreversibly reacting with it. While initially it seems as though the organic acid, base, and neutral compounds would never pass into the aqueous layer, the conjugate acid and base of the organic base and acid respectively are soluble in water.
Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.
First, a solid/liquid extraction must take place in order to get the solid natural product into the liquid solvent. This can be done by simply brewing a cup of tea. In order to isolate the desired reaction compounds from the natural product, liquid/liquid extractions are used. (water and DCM) Neutral and acid/base are two forms of liquid/liquid extractions. Because water is present in the pairing, it possible to separate inorganic compounds from organic compounds since organic substances are insoluble in water.
Complex mixtures can be separated and analyze using physical methods. One of it is chromatography. Two components in a mixture are separated by using the different distribution between two non- miscible phases which is stationary phase and mobile phase. The stationary phase exists as liquid or solid and it is fixed in a system. The mobile phase is a fluid which streams through the chromatographic system.
Experiment 2 Report Scaffold (Substitution Reactions, Purification, and Identification) Purpose/Introduction 1. A Sn2 reaction was conducted; this involved benzyl bromide, sodium hydroxide, an unknown compound and ethanol through reflux technique, mel-temp recordings, recrystallization, and analysis of TLC plates. 2. There was one unknown compound in the reaction that was later discovered after a series of techniques described above.
Student’s Name Instructor’s Name Course Date Extraction Aim To separate a mixture of Benzoic acid, 4-t-butylphenol and Biphenyl and to determine the percentage recovery of each Theory Bicarbonate ions, when added to a mixture of the three substances, will convert the carboxylic acid (in this case, benzoic) to ions. Hydroxide ions on the other hand convert Phenols to ions. This makes them soluble in the aqueous layer as ions are soluble in water.
The development of Gas Chromatography (GC) to be an analytical technique to separate the components of a mixture
The results of the study were expressed as gallic acid equivalent (GAE) in μg/ g of dry weight. Single factor experiments Effect of solvent type on extraction of phenolic compounds Selection of extraction solvents is very important as it has important role in the determination of the amount and the type of phenolic compounds that will be extracted. Aqueous alcohols particularly acetone, ethanol and methanol are usually preferred for the extraction of the phenolic compounds from
How to Separate Different Mixtures by Taking Advantage of Their Chemical and Physical Traits Badria Al Hosani Grade 10 Chemistry 21st of October 2014 Mrs. Stewart Research question: What is the effect of chemical and physical traits of a substance have on the way its separated? Background
The aqueous extract was prepared by dissolving 1g of dry extract with 20 ml of sterilized distilled water, so the final concentration of extract would be 0.05 g/ml, from this solution other concentration were prepared (0.1-0.2) g/ml. the solutions were shaken for 30 min. The extract was centrifuged (30,000 rpm; 15 min) and the supernatant was Separated. To hydroalcoholic extract, 80 g of the powder was extracted with aqueous methanol (75%). The other two concentrations were prepared from soaking sixfold aqueous methanol (75%) with different amounts of powder.
Organic chemistry II Experiment 3: chromic acid oxidation reaction Introduction: Camphor is very compact and its molecular structure is symmetrical which gives it the property to change directly from a solid to vapour when heated. Therefore, camphor can easily be purified by sublimation technique. Sublimation is a phase change in which a solid phase passes directly into the vapour without going through an intermediate liquid phase. Solids which have vapour pressure below melting points can be purified by 1) heating the solid to sublime it 2) condensing the vapour on a cold surface 3) scraping off the condensed solid. Sublimation is not a very accurate method as recrystallization or chromatography.
However, this situation may be vice versa due to the relative densities of the two solutions. The extraction process is used to repeat in several times in order to ensure all of the organic compounds are fully drained out. Granular sodium sulfate will act as drying agent to remove the last traces of water from organic
1. INTODUCTION AND BACKGROUND 1.1. Background and Justification Essential oils are aromatic oils found in different parts of plants used for flavors, perfumes, aromatherapy and medicine [1]. These oils are volatile and different from fixed oils which are mainly triglycerides of fatty acids. Essential oils are obtained from thousands of plant species and in different parts of the plant such as flowers, leaves, twigs etc.