Phenylbutyrate and sodium benzoate are orphan drugs approved for the treatment of hyperammonemia in patients with urea cycle disorders, a series of at least 8 rare genetic enzyme deficiencies. I was able to make my predictions based off my knowledge of boiling points, and I understood that the first fraction was taken before the temperature was able to reach the boiling point of toluene. Based on the boiling points of the two cyclohexene products, which isomer, 1-or 3-methylcyclohexene, would be predicted to have the shorter GC retention time? The reason ethylene chloride would from a layer on the bottom is because it has a higher density than the other two (water and 9-Fluorenone) substances in the solution. What effect, if any, did the new drying procedure have on product yield? Even so, it is important to use enough without using way too much. Why was the steam distillate extracted with three portions (3 x 2 mL) of methylene chloride, instead of just one or two portions? Be as complete as possible and show electron flow for all steps. Consult the IR spectrum of 4-methoxyphenol included below, on page 6. Why do the dye compounds have different Rf values? Why or why not? The proper amount is estimated instead. (in other words, it is likely that you did not extract all of the cinnamaldehyde from the cinnamon sticks). If something is more polar, the mobile phase and stationary phase would stick together. The sodium bicarbonate acts as a base in this reaction. Be familiar with how to read IR spectroscopy. In the third fraction, more toluene will be expected because of its higher boiling point. Circle and label the region of the molecule that exhibits polar behavior. This is because the positive charge of Na causes it to bind with the Br molecule from tetrabutylammonium bromide. Some people claim that this man-made additive is … Explain why this condenser was needed for the bromination reaction. The relative peak areas of the borrowed data was 14.25 and 85.75. HINT: What reactant was used in excess(in other words, it was NOT the limiting reactant).Consider also the TLC data reported in question 3. Weak acids and bases will change color with pH, so the dye changes colors depending on whether it is in its acid/base phase or conjugate acid/conjugate base phase. In the organic product drying step (sodium sulfate) in this experiment, a significant procedural difference was followed compared to previous experiments that involved drying of organic phases (the first three experiments of the semester). Since the conical vial had multiple separation steps there is more room for error, whether that is substance residue sticking to the sides of the tubes or in the cotton filter. Another possible error could be when the cotton ball was used to filter, during this part some solution was caught in the cotton and could not be removed even when attempted to be squeezed out using the pipet. For each fraction collected and analyzed by GC, what do the experimental GC data tell you about the progress of the distillation? Also, the solution 2 spot was more faded than solution 1. Comment on the relative solubilities of the organic reactant and product in the diethyl ether phase vs the aqueous phase. Consider the calculated partition coefficients for Experiments 4A and 4B. Report the experimental data here. If substituted for methylene chloride in this partition coefficient experiment, would ethylene chloride form the top or bottom layer? Colors of the spots... which, if any, of the dyes changed color after the eluted TLC plate was immersed in 1 M HCl? Theres evidence that exposure to the substance leads to diseases like cancer, Alzheimers and ADHD in children (1). This chemical reaction should be included in the Reaction Scheme section (hint: review common types of chemical reactions in aqueous solutions from general chemistry, such as precipitation, acid-base, gas-forming, and oxidation-reduction). This situation where the lab materials are not working properly can change what data is collected. It may not be complete in terms of showing ALL electron flow(proton transfers, in particular, are often assumed and not drawn out fully). The product was weighed and then the melting point was obtained. The distillate collected from the steam distillation was cloudy because cinnamaldehyde is not miscible in water. Explain your answer. Ethylene chloride, ClCH2CH2Cl (98.96 g/mol, density = 1.26 g/mL, bp = 83 °C), is an organic solvent with polarity similar to methylene chloride, and is also not miscible with water. By using a redistillation process, we would get even more pure results. List at least one potential problem for each scenario. When the methylene chloride was added, because it does not dissolve with water, it separated the solution into two layers. If there were too much sodium sulfate used it could cause the methylene chloride to harden preventing extraction from the tube, therefore ruining the experiment or making it very inaccurate. Your task is to fill in the rest of the data as directed. The mass of sodium sulfate is not important to the lab because it is not used in any of the calculations to find the partition coefficient of 9-Fluorenone. On the other hand, toluene has a much higher boiling point, which is why more toluene was shown being extracted from the solution as the temperature increased. The substance would have percents closer to 100% with each redistillation. The steam distillate collected in the Hickman still was clear. On a gas chromatogram, what do the peak areas represent? A water-jacketed reflux condenser was used again this week as part of the experimental setup. Sodium benzoate is a preservative added to some sodas, packaged foods, and personal care products to prolong shelf life. Does your data verify that the isolated product was meso-stilbene dibromide? Write a complete and balanced chemical equation for the reaction that occurs during the separation step that you DID NOT performing Experiment 4C (just the separation step, using either 3 M HCl or 3 M NaOH, not the subsequent isolation step).

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