Trimyristin Synthesis Lab Report
To purify and isolate trimyristin from a nutmeg, the sample of nutmeg was mixed and refluxed with dichloromethane before isolating and purifying the trimyristin through vacuum filtration and recrystallization. After refluxing the solution of dichloromethane and nutmeg, an intense amber colored solution was recovered. Through the process of vacuum filtration and recrystallization, a white, powdery and clumpy sample of solid trimyristin was collected. Of the 8.004 grams of nutmeg utilized in the experiment, 2.399 grams of trimyristin was collected after recrystallization, resulting in a 29.97% recovery in the experiment. By conducting a melting point experiment, the melting point for our extract of trimyristin was most accurately determined to be 50.3℃ - 51.6℃. Additionally, the experimental infrared frequencies for the characteristic functional group in trimyristin (ester) was recorded by utilizing a sample of our extract in the infrared spectrometer (Actual …show more content…
Trimyristin has a melting point of 56℃ - 57℃ and characteristic infrared frequencies seen in Functional Group Frequencies-Table I: Infrared Spectra. Our extract of trimyristin had a melting point range of 50.3℃ - 51.6℃ and infrared spectra frequencies seen in Actual Peka Locations-Table I: Infrared Spectra. Despite attaining a 29.97% recovery of trimyristin in this experiment, we achieved the expected outcome of the experiment, and fairly accurate data. Even though our conduction of the isolation and purification of trimyristin from nutmeg was successful, it was not perfect. Upon initially testing the melting point of our extract of trimyristin, we misread the melting point to be 156℃-157℃. Even though we caught the mistake
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Extract Trimyristin From Nutmeg
920 Words | 4 PagesAs a part of our study on how to completely extract trimyristin from nutmeg, we had to determine the best way to find a solvent that would properly recrystalize it. We used triphenylmethane as a test compound, attempting to find a solvent that would allow it to recrystalize. The most suitable solvent would dissolve the solute when the solvent is hot, not dissolve it when the solvent is cold, and should be fairly volatile and easily removable from the desired product. We tested water as a potential solvent and triphenylmethane would not dissolve when the water was at room temperature or when it was hot, so this was not a good solvent. When we tested methanol, triphenylmethan did not dissolve at room temperature, but did dissove when the methanol was hot, and then recrystalized into a solid when the mehtanol was cooled, so this was a suitable solvent.
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