Nitration Of Methyl Benzoate Lab Report

A mixture of 0.25 g of camphor (1.64 mmol), 1.5 mL of methanol, and 0.25 g of sodium borohydride (6.60 mmol, NaBH4) was boiled for 2 minutes. Moreover, the addition of 10 mL of ice deionized water resulted in a white solid after the organic solution was vacuum filtered. The organic solid was dissolved in 10 mL of dichloromethane (CH2Cl2) and small amounts of anhydrous sodium sulfate (NaSO4) to dry. The organic solution was decanted and evaporated for melting point (203.3-203.8 °C), NMR, and IR spectroscopy. Product formation and heats of formation (borneol = -1.203675E6 kJ/mol, isoborneol = -1.203687E6 kJ/mol) were analyzed.

We then weighed a filter paper which we will use later in the experiment. We then collected the crystallized acetylsalicylic acid by vacuum filtration in a Buchner funnel and washed the product with a little ice-cold water. We then pre-weighed a clean, empty watch glass and labelled it with our initials and the date, we did this do we could easily identify that it was ours when we go to weigh it with the crystals on. We

Lastly, product was GC traced to obtain the percentage of product and starting material within final product. Observations: Mixture turned yellow as sulfuric acid was added. During reflux condensation, sodium bromide dissolved and brown layer formed on top of solution as it boiled. Brown layer was alkyl bromide while clear, bottom layer was inorganic salts. After simple distillation, product was clear and colorless.

Later on all the observations were compared in order to found out which cation/cations made up the unknown solution. To ensure a safe classroom environment, all four laboratory bottles were cleaned and put away, the paper clip was thrown

To drive the reaction to the amide product, the reaction was performed at 300 ˚C to evaporate the water product, which is an application of Le Chatelier’s principle. Second, the aromatic nitro group was reduced to an amine using sodium dithionite. The reaction is given in Figure 1. Figure 1: Synthesis of luminol from 3-nitrophthalic acid and hydrazine. To verify the synthesis of luminol, the product was mixed with an oxidant (diluted bleach) and was inspected for a blue glow.

Once cool to touch the squeeze out all the tea bags carefully without tearing them apart. Using a separatory funnel extract three times with 15.0ml of dichloromethane gently rocking bath and forth the funnel venting the funnel often each time. Carefully decant into a pre-weighed 125ml flask and add the drying agent-calcium chloride pellets- and the organic layer was evaporated off in a warm water bath. Using aluminum foil as support around the mouth of the flask place test tube in the flask and heat the flask on a hot plate whilst adding water into the tube without letting it boil. Once the caffeine forms crystals around the test tube scrape off all the sublimed product and weigh the dried product 0.1grams of caffeine and had a melting point range of 175-230

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.

Nevertheless, the latter is not used in this experiment since it is very reactive and extremely flammable. On the contrary, NaBH4 is relatively mild and it can be used with protic solvents. In this manner, 1.507 grs of the ketone 9-fluorenone were mixed with 30.0 ml of 95% ethanol in a 125 ml Erlenmeyer flask. The bright yellow mixture was stirred during 7 minutes until all the components were dissolved.

Additionally, I compared IR spectra I obtained to official IR spectra for para-bromoaniline and 4-bromoacetanilide and they had the same important peaks. Between the two weeks, the reaction time was not very different and was about 15 minutes. The combination of data from TLC, IR, and melting point were able to help me asses the identity of my unknown product, and this the importance of characterization in

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.

Abstract: The goals of this experiment were to observe the changes in melting points across different compounds as well as the factors that affect melting point accuracy, which are impurities and amount of compound. The experiment begins by comparing the effectiveness in obtaining the recovery of a solid from a mixture between gravity and vacuum filtration. Which vacuum filtration had 11% loss while gravity had only a 7% loss. It was determined that pure benzoic acid had a melting range of 122.9-124.4 oC while impure benzoic acid had a melting range of 83.4-86.3 oC. The unknown compound 1 was determined to be palmitic acid through mixed melting point theory. Introduction:

Lance Feig CH 128L Experiment Report Purpose The purpose of this lab was to synthesize methyl benzoate from benzoic acid and methanol through Fischer esterification. The identity of the product was verified through IR, GC, and 1H-NMR analysis, where the experimental readings were compared to known readings of methyl benzoate. Furthermore, a percent yield of the product was calculated.

Purpose/Introduction The process of recrystallization is an important method of purifying a solid organic substance using a hot solution as a solvent. This method will allow the separation of impurities. We will analyze Benzoic Acid as it is dissolved and recrystallized in water and in a solvent of Methanol and water. Reaction/Summary

Abstract The unknown concentration of benzoic acid used when titrated with standardized 0.1031M NaOH and the solubility was calculated at two different temperatures (20◦C and 30◦C). With the aid of the Van’t Hoff equation, the enthalpy of solution of benzoic acid at those temperatures was determined as 10.82 KJ. This compares well with the value of 10.27KJ found in the literature.

The solution was warmed to 65oC with constant stirring on the magnetic stirrer till the solid was completely dissolved. Stirring was stopped and 0.4g of charcoal was then added to the solution. After which the solution was transferred to a Buchner funnel with a moist filter paper and the clear filtrate was collected via suction filtration. The residue was washed with warm solution of 10.035g of KI and 15ml of deionized water. 200ml of water was then added to the filtrate in a 500ml beaker with constant stirring.