Unlike the ideal, most things are not pure in composition. Unfortunately to achieve a specific reaction without any unexpected and possibly unwanted reactions one must purify the desired compounds. To purify a compound one must use the difference of chemical and physical properties. In this lab a analgesic pill is the start of the purification process. In total there are four main steps that are necessary in order to isolate the list of three drugs given. These three drugs are Ibuprofen, Naproxen, and Aspirin. Each pill has a set of impurities other than the drug itself. Those can be grouped into basic soluble fillers and acid soluble fillers. First the pill is crushed and brought into a powder. The next step is to dissolve the powder is a …show more content…
This mixture was very good at separating the mixtures because its dielectric constant is 3.832. This relatively high value for the dielectric constant gives a strong effect towards moving the compounds up the TLC plate. The way that I visualized the spots on the TLC plate is first I placed the plate under a UV light. This showed most but not all the spots. The next way was to dip the TLC plate into bromocresol green. The best mixture was mixture 5 at separating the compounds due to the greatest dielectric constant. The worst mixture being the first mixture this is due to the very low dielectric constant. The general values between the ibuprofen and the aspirin are almost the same most of the time while the naproxen is very low in …show more content…
Since each mixture contained a larger and larger dielectric constant it is fair enough to say that the trend fits to the dielectric constant. I think that the compound I had is aspirin mixed slightly with ibuprofen. I think this due to the fact that the TLC plate has a match on both the aspirin and the unknown as well as the melting point of the unknown and the aspirin are almost exactly the same. My compound is very pure. I think this because of how similar it was to the standard. The standard and the compound were on top of each other and so I think it's fair enough to say that they are of very similar purity. If my drug broke down during a specific condition then it would have resulted in different properties in the melting machine and in the TLC test. In the TLC test I probably would have noticed multiple marks for where the drug traveled. This is due to there being more than one compound. In the melting machine there would have been a greater temperature range for
5. Two or more samples may be applied to each plate if they are kept
...s the change in the temperature of both of these batches, 6°C for the pure, and 13°C for the crude. In this final sub-section of the Characterization of Aspirin, the values of absorbance were recorded. Initially, 0.0566 grams and 0.0590 grams of pure and crude Aspirin respectively were obtained and each individually placed into beakers (400 milliliter) and had 250.0 milliliters of distilled water added to them. From each beaker, a tiny amount of the just dissolved solutions was transferred to a cuvette, one cuvette for each type of aspirin. Each cuvette was placed into the ultraviolent spectroscopy mechanism which was connected to a computer and absorbance spectrum values were obtained at 298 nm (Figure 5) (0.1987 pure aspirin, and 0.9549 crude aspirin).
The analysis is therefore one of the most effective methods of ensuring that each drug being prescribed to patients is safe. It also ensures that all drug components are understood in terms of their structure and chemical behavior. This understanding is very important in the manufacture of drugs and other pharmaceutical products.
Looking at my results, I can see that I only obtained 86.6% of aspirin. this is not the highest percentage that it could be. I probably lost some aspirin when I had to re-filtered the solution multiple times, or when I had to weigh a new beaker and maybe not all of it got transferred over to the new beaker, or maybe I didn’t get all of the aspirin crystals off of the paper towel and into the beaker. Regardless, of where the aspirin sample was lost, I obtained a 86.6% of aspirin from this
Aspirin is also known as Acetylsalicylic acid. It is composed of nine Carbon atoms, eight Hydrogen atoms, and four Oxygen atoms. There are many chemical properties to it. The melting point of aspirin is about one hundred and thirty-five degrees Celsius and the boiling point is one hundred and forty degrees Celsius. It has a density of 1.35 grams per milliliter and the molar mass is 180,160 g/mol (1). This means that the molecule is relatively dense. There is more weight than there is volume. Aspirin is described as odorless and colorless to where the color is white. It looks like a crystal-line powder at room temperature. It is a relatively stable molecule that should be stored at room temperature (2).
In today’s world, acetaminophen also known as Tylenol, is known to be remarkably popular drug in many countries [1]. This type of drug is known to be an analgesic and antipyretic [1]. In other words, it helps relieve pain associated with many conditions as well as reducing fever [1]. Acetaminophen can be used for many purposes, such as the relief of headaches, muscles aches, toothaches, and etc [1]. On the other hand, this drug may also be used for purposes that are not listed on the medication guide, such as, menstrual cramps [1]. However, acetaminophen ingredients are majorly used for numerous cold and flu medications as well as many prescription analgesics [1]. This drug is widely available in many drug stores/supermarkets and it is provided
Discuss the possible drug and excipient-related constrains of the formulation (no identity of the drug was given to you at this
contamination, toxicity, and side effects. Most people believe these medications are compounded or mixed by a trained and licensed individual. However, this is inaccurate because the pharmacy technician actually compounds a large percentage of a patient’s medications. Compounding involves a techn...
The conical vial was placed in a small beaker and allowed to cool to room temperature. The mixture was Cooled thoroughly in an ice bath for 15-20 minutes and crystals collected by vacuum filtration on a Hirsch funnel. The vial was rinsed with about 5 mL of ice water and transferred into to the Hirsch funnel and again washed with two additional 5mL portions of ice water. Crystals were dried for 5-10 minutes by allowing air to be drawn through them while they remained on the Hirsch funnel. The product was transferred to a watch glass plate and allow the crystals to dry in air. Crude acetaminophen product was weighed and set aside a small sample for a melting point determination and a color comparison after the next step. Calculation of the percentage yield of crude acetaminophen (MW = 151.2). was done and recorded in the lab notebook.
The Graph clearly shows a very distinct curve of best fit, with the curve arcing upwards. The Graph clearly shows there is a trend forming and the trend proves the original theory correct i.e. as temperature increases the higher the kinetic energy transfer to the phosphate and lipids of the cell membrane allowing more activity in its structure allowing bigger gaps to form which allows the pigment in the vacuole to
The ways of analyzing drugs and identifying them are microcrystalline tests, gas chromatography, mass spectrometry, and spectrophotometry. Microcrystalline tests are more specific than the color tests and is uses the polarizing microscope. Gas chromatography is when the sample is separated into its different components based on size and chemical structure. Mass spectrometry fragments the molecules in the sample and that pattern of fragmentation helps with the identification of the substance when compared to a known standard. Spectrophotometry identifies substances by measuring how it absorbs the different wavelengths of light including; UV, visual, and infrared. There are all used to decipher the chemicals compositions of the sample to determine what kind of drug is contained in the substance, including how pure the substance is as well.
HPLC (High Performance Liquid Chromatography) is an analytical technique which separates a complex mixture of components into its specific individual components. It is a powerful tool in analysis, as it combines high speed with extreme sensitivity compared to traditional methods of chromatography because of the use of a pump which creates a high pressure and forces the mobile phase to move with the analyte in high speed. It is been used as a principle technology in various automated analyzers used for diagnostic purpose.
This method can be used to analyse different paracetamol brands and calculate which one contains the greatest quantity of the active ingredient.
Each of these OTC analgesics has different side affects and purposes, but they all share three common elements. These elements are Carbon (atomic number 6, atomic mass 12.011), Hydrogen (atomic number 1, atomic mass 1.0079) and Oxygen (atomic number 8, atomic mass 15.999). By looking at the molecular formulas of each type of OTC analgesic, these three common elements form the base for each chemical compound.
... point, the complete and full separation of the components, as those seen in the first part of the experiment, did not happen. This source of determinate error decreased the Rf values. Furthermore, upon placing my TLC plate into the solution I stumbled and threw the TLC plate in the jar. The solution splashed up on the TLC plate, rushing solution to move up and absorb on the TLC plate without capillary action. Because not all the solution that splashed up was not absorbed, it may have either dragged down some of the ink components or allowed for faster capillary action. This source of indeterminate error skewed the result of the Rf values, either increasing or decreasing the distance traveled of the ink. I don’t believe that this was a great source of error because the components of the unknown ink and the pen #3 still rose to similar values with similar separation.