Analgesic Drugs Lab Report

The purpose of this lab is to investigate the composition of a compound suspected to be Panacetin, a type of pain-killer. Panacetin is typically made up of sucrose, aspirin, and acetaminophen, but the third component in this experiment is unknown. The unknown component is suspected to be a chemical relative of acetaminophen, either acetanilide or phenacetin. Using techniques such as extraction, evaporation, and filtration, the three components will be isolated based on their solubilities and acid-base properties. Then, the percent composition of Panacetin can be deduced based on the masses of the three dried components. The

Prior to beginning the experiment, it is important to understand a few different concepts such as the distinguishing physical properties of a chemical substance and how these physical properties can be analyzed. Physical properties of a chemical substance include water solubility and melting point, both of which are used to pursue identification of the unknown component of Panacetin. Water solubility is a distinct physical feature of chemical substances that can lead to an increase or decrease in product recovered. For example, the water solubility of the two possible unknowns, acetanilide or phenacetin, are different in opposite temperature spectrums. Acetanilide’s cold water solubility is 0.54 grams/100 mL of water, whereas the substance’s boiling water solubility is 5.0 grams/100 mL of water.

Sodium bicarbonate has a molar mass of 84.0 g/mol. It has a melting point of 50°C and can be an irritant.

TLC Analysis Data Table Compound Std. Aspirin Std. Caffeine Rf values 0.38 0.65 Error ---~ 0% 29% 5%

Pre-Lab: Analgesic drugs are known for reducing pain, while antiseptic drugs reduce symptoms such as fevers and swelling. However, some of these drugs can reduce both illnesses. To obtain a pure compound in these drugs, the scientist needs to separate the desired compound by taking advantage of the different physical and chemical properties. Such as; different boiling points, melting points and their solubility properties. To do this a chemist can also asses the differences between acidic and basic substances when they are added to water soluble mixtures. Within this current experiment I will asses the

Substance A and B were weighed; Substance A weighed 0.502 g and substance B weighed 0.503 g. Both substances were put into two different test tube with approximately 8 ml of DI water into the test tub. Substance A and B were stirred and B dissolved while A did not. This shows that B is soluble in water compared to A. Thus, shows that B is soluble in water than A. The reason why B is soluble in water is because it has a higher dipole moment than A. With a higher dipole moment, it shows that it is soluble in water since it is polar and the bonds were easily broken.

aspect to assess the safety and appropriateness of IV acetaminophen use in hospital setting. Several published hospital utilization medication reports showed an increase consumption of intravenous acetaminophen.

Figure 1. The structure of caffeine and benzoic acid with their molecular weights and formulas.

1. Go to http://www.particleandfibretoxicology.com/content/pdf/1743-8977-6-12.pdf (Links to an external site.)Links to an external site. and get a general sense of the article with a focus on the figure. Notice the way that the confidence intervals are graphically portrayed. The histograms (bar graphs) display at the top of each bar the point estimate (mean) and the little ┬ arising from the top of the bar measures the distance between the point estimate and the point estimate + the standard error of the mean (SEM).

I came across interesting information when I was researching material for this assignment. In an article by Nathan I. Cherny, he pointed out the difference between opiates and opioids. Opiate is the term used to describe drugs derived from the juice of the opium poppy (e.g. morphine is an opiate since it is derived from the juice of the opium poppy, but methadone is not because it is synthetic). Opioid is the generic term used to describe naturally occurring, semi-synthetic, and synthetic which produce their effects by combining with opioid receptors. (Cherny, 2012)

The humanity has been using alkaloids-containing extracts since ancient times. For example, there are reports on the use of opium since 3,400 BC. Opium (from Papaver somniferum) exudate is rich in tetrahydrobenzylisoquinoline alkaloids, as (5), codeine (6), and papaverine (7) (ref). Morphine is a potent analgesic and narcotic extensively used to treat both acute and chronic severe pain (Bercovitch et al., 1999). South American Indians have been using coca leaves (Erytrothroxylon coca; Erythroxylaceae) for over 4,000 years (ref), as a stimulant and energy source. Coca is known for its psychoactive alkaloid cocaine (8), whose medicinal use as tonic, for digestive disorders, weakness, aphrodisiac, in the treatment of asthma, alcohol and morphine

“Prescription Painkillers Seen as a Gateway to Heroin” article illustrates the possibility that opiate prescriptions open the door to addictions such as heroin.

Samples of benzophenone, malonic acid, and biphenyl were each tested with water, methyl alcohol, and hexane. Benzophenone was insoluble in water as it is nonpolar while water is highly polar. Benzophenone was soluble in methyl alcohol, dissolving in 15 seconds, because methyl alcohol is intermediately polar as benzophenone is nonpolar. Methyl alcohol is polar but not as much as water. Thus, the nonpolar benzophenone was soluble in methyl alcohol. Benzophenone was partially soluble in hexane because hexane is nonpolar as is benzophenone. Thus, benzophenone was dissolved in hexane. Malonic acid was soluble in water because both malonic acid and water are polar. It took 25 seconds for malonic acid to dissolve in water. Malonic acid was soluble in methyl alcohol because malonic acid is polar and methyl alcohol is intermediately polar, allowing malonic acid to dissolve in the methanol in 15 seconds. Malonic acid was insoluble in hexane because hexane is nonpolar while malonic acid is polar. Biphenyl was insoluble in water as water is highly polar whilst biphenyl is nonpolar. Biphenyl was partially soluble in methanol which is intermediately polar whilst biphenyl is nonpolar, allowing it to dissolve a little. Biphenyl was soluble in hexane because both biphenyl and hexane are nonpolar molecules. Biphenyl dissolved in hexane in 10 seconds.

A polar molecule is a molecule that possesses a negative charge at one end, and a positive charge at another end, caused by the positioning of the electrons due to electronegativity. However, a molecule can have a positive and a negative charged end and still be non-polar. Dipoles are a measure of polarity that are caused by a variation in electronegativity. The difference in electronegativity results in an atom having a greater pull on the shared pair of electrons. If the shape of a molecule causes equal dipole magnitude and an equal distance between the dipole vectors, then the dipoles cancel out and the molecule is considered non-polar .A polar molecule possesses a neutral net charge as the positive and negative sections of the molecule eliminate an imbalance in charge. Polarity is exclusive to covalent bonded compounds, as electron sharing is required in order for partial positivity and partial negativity to occur. The only covalent molecules that don’t contain polar bonds are those including atoms that possess an equal electronegativity, such as H2, or O2, as neither atom possesses a larger attractive force than the other acting upon the electrons .

The presence of characteristic peaks associated with specific structural characteristics of the dug molecule was noted. The IR spectrum of pure Aminexil and Minoxidil presented characteristics signals at: