The purpose of this experiment was to study the purification of an unknown solution through the process of recrystallization. Recrystallization is a process of the solid organic compound being purified, and impurities soluble at high temperature to form crystals. The identification of an unknown compound was determined through the process of recrystallization. The use of solvent determines the recrystallization process, so the selection of an appropriate solvent is vital for this process since the solubility of the crystals in the hot solvent, is dependent on decreased solubility when the solution is cooling. The solubility test helps in the determination of an appropriate solvent for a specific solute based on whether or not the solute dissolves …show more content…
The temperature of the water was then recorded to the nearest 0.1⁰C. Then the melting points of phenylacetic acid, o-anisic acid, and benzilic acid were determined by the use of a Mel-Temp. The unknown sample was obtained from the chemical stockroom. A small scale of crystals from unknown was placed in a test tube with the following solvents: cyclohexane, hexane, toluene, diethyl ether, ethyl acetate, isopropyl alcohol, methanol, or water, to determine the appropriate solvent for the unknown. If the solute was wholly dissolved in the solvent before heating, it was recorded as a bad solvent. If the solute dissolved after being warmed in a water bath, it was set aside to cool to allow recrystallization; if their recrystallization occurred or not was recorded. If the crystals did not form previous to heating, the solution was placed in ice bath. After the ice bath, if the recrystallization did not occur then it was seeded. After completion of the solubility tests, the appropriate solvent, cyclohexane, was selected for large-scale recrystallization. The unknown was weighed for the large-scale recrystallization then the same process was repeated to test the solubility. The solute dissolved after adding of about 60 mL of solvent, it was set aside to cool to induce crystal reformation. The solution was then seeded and set alone once more. When the process was complete, the crystals …show more content…
Some of the factors are thermometer was calibrated to determine its precision. The actual melting points of water, phenylacetic acid, o-anisic acid, and benzilic acid to their observed melting points were determined by calibrated thermometer. Then the solubility tests were run in order to determine the appropriate solvent for the unknown solute (Table 1). After determination of a solute, a vacuum filtration technique was used to determine the pure form of compound. The melting point of the purified sample was determined and compared to the melting points of other known compounds. The determination of the recrystallized compound’s melting point was used so as to have a better understanding of the purity of the recrystallization
The purpose of this lab was to be able to use physical characteristics to determine the identity of an unknown compound. The data from this experiment classified aluminum as metallic; ascorbic acid, paraffin, palmitic acid, sucrose, graphite, and water as molecular; sodium chloride as ionic. In order to determine this, 3 tests were conducted. The first test was to test the conductivity of each substance at room temperature. In this test, only graphite and aluminum conducted.
Identification of an Unknown Compound using Quantitative and Qualitative Analysis Lauren Tremaglio Chemistry 1011 Lab, Section 16 Instructor: Steven Belina October 3, 2014 Our signatures indicate that this document represents the work completed by our group this semester. Experimental Design and Discussion of Results The objective of this experiment was to identify an unknown compound through quantitative and qualitative analysis. In order to find the identity of the unknown compound, an initial qualitative test for solubility was performed.
Temperature is important, since above 250C° and below 50C virtually no crystallization occurs. Around 14°C is the optimum temperature for rapid crystallization, but also the presence of solid particles (e.g. pollen grains) and slow stirring result in quicker crystallization. Usually, slow crystallization produces bigger and more irregular crystals. During crystallization, water is freed.
There were a few steps in the experiment that may have contributed to impurities in the unknown crystals. In the beginning of the experiment, the column with alumina was used to filter the methanol/unknown mixture into a vial. It was important to add the mixture after methanol was added to the column and was still above the top
3mL of the liquid in each of the vials were added into cuvettes and measured in the spectrophotometer. Before each time point the photo spectrometer was zeroed using a cuvette with 3mL of distilled water. If any of the results were considered unusual the machine was zeroed again and the sample was retested. The results from the spectrophotometer test were recorded in a table. The experiment was repeated six times to gain a sample size of six.
The following lab period the solid was weighed (0.0483 g) and percent yield was calculated (65.5%) with the limiting reagent being tetraphenylcyclopentadienone. The melting point was determined. The first melting point was 204-204.9 °C and the second melting point was 215.6-215.9°C. Finally, an infrared spectroscopy was obtained for the
Pages 96-98 in Chemistry 110 Lab Manual. Wilfrid Laurier University, ON, Canada. Abstract: The purpose of this experiment was to determine the level of purity by using the values for melting point and absorbance and chemically synthesizing aspirin by using phosphoric acid as a catalyst.
Glacial acetic acid and acetic anhydride were added to the mixture while refluxing, which converted the lime colored solution into a clear mixture. The flask was cooled in an ice bath and the solution
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.
Trial #2 and Trial #3 were used to determine the freezing point of an aqueous solution. The “Unknown C” was used to create the aqueous solution. For Trial #2, 2.0019 grams of “Unknown C” were weighed and dissolved into the 11 dram vial. Once dissolved, the 11 dram vial was submerged into the ice bath, and the Vernier temperature probe was immersed into the 11 dram vial as well. Once the temperature of the aqueous solution reached 10°C, the temperature was recorded every 10 seconds.
3. To purify and identify the product, recrystallization is used in order to purify the product, then melting point and TLC techniques are used to identify the product. Theory 4.
The solvent was removed using a rotary evaporator. The melting point was estimated. The obtained mass of caffeine was measured. The percentage yield based on the amount of tea originally used was calculated. 2) Purification of caffeine by sublimation
In Experiment One we will be recrystallizing Benzoic Acid from water. In Experiment Two we will be recrystallizing Benzoic Acid using a solvent pair made up of Methanol and Water. The Seven step process of recrystallization consists of adding a solid organic substance into a solvent, then dissolving the chosen solute, decolorizing the solution, filtering solids, then recrystallize the solute by slowly cooling
Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4
When a solid dissolves in a liquid, it then changes its physical state (from solid to liquid) by melting. Heat is needed to break the bonds holding the molecules in the solid together and at the same time; heat is given off during the formation of new bonds between solute and solvent. Results Table1. Results for titration of benzoic acid with NaOH at 20◦C V(NaOH) ml V(C_6