Introduction All of the labs for the past three weeks consisted of the analysis of Aspirin. For the previous three weeks, all of the labs consisted of the analysis of Aspirin. Even though Aspirin is the most common drug used worldwide, it has been known to smell like vinegar. This is because aspirin is considered a salicylate. The formula name for Aspirin is Acetylsalicylic Acid, and the chemical equation is C9H8O4. The background behind Aspirin is that it aids in pain relief and reducing inflammation, swelling, and fever. Also, some benefits of aspirin are that it can treat skin problems such as acne, warts, and psoriasis and treats /helps to prevent a heart attack or stroke and some cancers.
In lab nine spectrophotometry was used in the aspirin analysis. Spectrophotometry is used to measure the ability of how much a chemical substance absorbs light. This was achieved by measuring the light intensity after it was directed through the sample placed in a cuvette. Spectrophotometry is known to be the most useful methods for the analysis of quantitative data.
Beer 's Law is used in the process of spectrophotometry to find the effect of light on the premises of the substance while it is traveling. In other words, Beer 's law is used to indicate how to complete the absorbance of a mixture at a particular wavelength to examine the independent components of a solution. It also shows the relationship between concentration and absorbance. The Beer 's Law formula is Absorbance =
Spectroscopy is the study of light. A spectrophotometer is a machine used to determine the absorbance of light at any given wavelength. It does this by using a source of white light through a prism, which gives multiple wavelengths that can be individually focused (Ayyagari and Nigam, 2007). Substances are put into cuvettes that are glass or quartz containers that light can easily travel through. The light that is being focused travels through the substance gets absorbed by the
This experiment involved three steps: synthesis of aspirin, isolation and purification, and the estimation of purity of the final product. The synthesis involved the reaction of salicylic acid and acetic anhydride in the presence of a catalyst, phosphoric acid, H3PO4. When the aspirin was prepared, it was isolated and filtered. The percentage yield of the synthesis was calculated to be 78.42%. The experimental melting point range of aspirin was determined to be 122 -132°C. Due to its wide range, and lower value than that of the theoretical melting point of 136°C, it was
The goal of this experiment was to synthesize aspirin. In this experiment aspirin, also known as acetylsalicylic acid, was synthesized from salicylic acid and acetic anhydride. In the reaction the hydroxyl group on the benzene ring in salicylic acid reacted with acetic anhydride to form an ester functional group. This method of forming acetylsalicylic acid is an esterification reaction. Since this esterification reaction is not spontaneous, sulfuric acid was used as a catalyst to initiate the reaction. After the reaction was complete some unreacted acetic anhydride and salicylic acid was still be present in the solution as well as some sulfuric acid, aspirin, and acetic acid. Crystallization, which uses the principle of
A spectrophotometer’s purpose is to use colors of the light spectrum to determine the concentration of light absorbing molecules in a solution. (p.59) In this particular lab, our mission was to determine the protein concentration and the standard curve of the unknown sample of BSA. This, by preparing five dilutions of the unknown solution of BSA together with other known concentrations, and then experimenting by observing how the concentrations were passed through the spectrophotometer. The outcome resolved in the absorption levels being decreased, and this
Scientists use an instrument called a spectrometer to quantitatively determine the amount of light absorbed by a solution. The primary inner parts of a typical spectrometer are described below. The spectrometer has a light source that emits white light containing a vast mixture of different wavelengths of electromagnetic radiation. The wavelength of interest is then selected using a monochromator (“mono” meaning one and “chromate” meaning color) and an additional exit slit. The separation of white light into different colors (wavelengths) is known as diffraction. The selected light then reaches the sample and depending on how the light interacts with the chemical compound of interest, some of the light is absorbed and some passes straight through. By comparing the amount of light entering the sample (P0) with the amount of light reaching the detector (P), the spectrometer is able to tell how much light is absorbed by the sample.
Both Aspirin and the Unknown are soluble in dichloromethane, due to their non-polar characteristics. To separate the two components, sodium bicarbonate was added (see figure 3). Sodium bicarbonate reacted with aspirin and converted it to a salt, also forming water and carbon dioxide. It was observed that the solution "fizzed" when this reaction took place, showing the release of carbon dioxide. The newly formed salt then traveled to an aqueous layer where it was soluble, while the unknown remained in the dichloromethane layer. The two layers were then separated. To collect an aspirin solid, the combination of the addition of HCl and the process of vacuum filtration helped to break down the salt and form a solid. Then the solid was placed in the Fisher Scientific Biotemp Oven to dry it to a constant mass of 0.091 g, 32.97% of the total composition. The
Aspirin is one of the most consumed painkillers created up to this date due to its reliability and low expense. It is often used to relieve minor aches and pains, reduce fever and as an anti-inflammatory medication. Due to its wide range of uses, the demand for this pharmaceutical is very high. As a result, manufacturers who produce this drug must be efficient in order to reduce the time taken to produce this drug and produce the in very high quantities.
0.1 gram of commercial aspirin was weighed in a tray and was then added to a second test tube containing 2.0 mL of Iron (III) chloride, which was measured using a 10 mL graduated cylinder, to test for phenols. This was repeated once more to validate results.
5. The degree of precision was to 3 significant figures obtained with the spectrophotometer. The major source of error in our experiment was not calibrating the spectrophotometer with distilled water.
Using the yellow tube, which included everything but starch, as the blank, each group zeroed their spectrophotometer. This was done so that any absorbance observed depends only on the amount of starch present, not on any other reagents (buffer, IKI). To zero the spectrophotometer, the wavelength was first set at 580nm, using knob 3 (45). Next, the groups made sure that the light next to “transmittance” was lit, and the chamber to be tightly closed. Having the chamber empty & closed tightly provides reference for the darkest condition possible. Using knob 1, the transmittance was turned until it read 0.0 (45). Before the groups used their blank test tube to zero the spectrophotometer, each needed to wipe the tube with kimwipes to ensure a clean reading. Turning knob 2, each group was then instructed to zero the absorbance, 0.000. Upon removing the blank, each trial was inserted into the chamber (46). The
Acetaminophen is a worldwide known drug used for aches and pains, but that is all that is thought of when the name is said. Because it is an over the counter medicine, nobody thinks about the effects it can have on you. In fact most people don't even read the warning label. In this paper, it will discuss all of the things nobody even bothers themself to look into. Such as common name/s, what it should be prescribed for, uses, side effects, warnings, drug interactions, and the chemical composition for it. This essay attempts to prove that Acetaminophen is more than just a benign remedy for discomfort.
A spectrophotometer is an instrument which measures the amount of light of a specified wavelength which passes through a medium. This instrument is usually used for the measurement of reflectance of solutions. Light is separate into different wavelengths and is being passed through the sample solution. The sample solution will have its own wavelength and will absorb a certain amount of light. The higher the molecular concentration, the higher the absorbance value.
Spectrophotometry is a routine laboratory test that has the added advantage of being able to
8) Steps 1 - 8 were repeated using the wavelengths of 360 nm to 900
concentration, record the absorbance readings at a fixed wavelength, and plot the absorbance vs. concentration data. The wavelength of 520 nm was selected for experiment Part