1. Aims a) To find the molar absorptivity of salicylic acid by plotting a graph of absorbance against the concentration of salicylic acid, using the standard solution. b) To find the concentration of aspirin at the various time intervals using the molar absorptivity value in the previous part, initial concentration of aspirin and the concentration of salicylic acid obtained from the decomposition of the aspirin pill. c) Lastly, to calculate the rate constant of the decomposition of aspirin by plotting a graph of ln[aspirin] against time and making use of the gradient of the best fitted line along with the standard deviation. 2.Data Treatment and Analysis In order to find the molar absorptivity of salicylic acid, a UV spectroscopy is carried
Results: Table 1: Results from the Salicylic acid (g) and the Purity of ASA (g) Experiment Mass of salicylic acid (g) 0.14 g Mass of filter paper (g) 0.47 g Mass of “impure” ASA + filter paper (g) 0.56 g Mass of prepared “impure” ASA (g)
As you can see from my sample that our aspirin sample contains a small amount of pure aspirin and a lot of salicylic acid. Therefore this means that my sample wasn’t pure as it still had remnants of salicylic acid which suggests to me that the reaction hadn’t been fully completed, however my sample did contain a small amount of pure aspirin which means that the reaction is partially had taken place. The sample would have been pure if there was no salicylic acid on the card then my sample would match the pure aspirin sample which means there would have been a fully completed reaction. 2. State what practical techniques used during the procedure and explain how they influence the purity of the sample.
The Rf calculations of aspirin in table 1 shows an Rf value of .491; however, in table 2 the Rf value of aspirin was calculated to be .784. This Rf value is the higher among the other compounds because the Rf values decreases from aspirin to caffeine; therefore, this suggests that the
Aspirin is synthesized through three different steps, the synthesis of the aspirin, the isolation and the purification and finally the purity estimation of the final product. It involves the reaction of acetic anhydride and salicylic acid in the presence of phosphoric acid = H3PO4. After the aspirin is synthesised it then mist be isolated form the reaction solution and purified. This procedure is a possible experiment to execute at a
Thin Layer Chromatography (TLC) Abstract This experiment uses the TLC chromatography technique to identify the presence of acetylsalicylic and Acetaminophen in analgesic drugs (Tylenol and Anacin). It was found that the Anacin and acetylsalicylic had very closer Rf values (0.8 and 0.79). The Tylenol and acetaminophen had closer Rf values (0.54 and 0.58). Hence, Acetylsalicylic acid and acetaminophen were present in Anacin and Tylenol tablets respectively. Introduction Chromatography is the technique of separating of mixtures based on their intermolecular forces.
To do this we have to follow and conduct the experiments given in the BP, such as infrared spectrophotometry, limit testing for p-aminophenol in acetaminophen and running the assay for Acetaminophen and only after these 3 tests can we confidently conclude if the sample is up to standard. Introduction Identification by IR IR is a very specific method for identification of active ingredients in pharmaceutical products. An IR spectrum of the active ingredient should be an exact
Isolation of Ibuprofen: Fifteen 200 mg ibuprofen tablets were used, which was 3.37g (16.34 mmol, 112.3%) ibuprofen. This amount of ibuprofen was submerged in 25 mL of acetone and stirred vigorously for 5 minutes to dissolve. Red coatings of the tablet were separated and vacuum filtration was utilized to dissolve all insoluble components. The melting point range of the crude ibuprofen was 72.4-73.9°C. The major bands from the IR are, FTIR: sp3 O-H stretch, about 3200-2500 cm-1 (b, m); sp3 C-H stretch, 2991-2868 cm-1 (sh, m); sp2 =C-H stretch, 3100-3000 cm-1 (sh, w); sp2 C=O stretch, 1701 cm-1 (sh, s); and sp2-sp2, aromatic, C=C stretch (in ring), 1507 cm-1 (s, m).
Summary Determining the concentration of a liquid can be a tricky process involving complex procedures if it were not for science’s ability to test a substance’s absorbency through spectrophotometry. The experiment was carried out to discover the concentration of Red Dye #40 in several common soft drinks. The samples of the dye were diluted, and tested using a spectrophotometer. The absorbencies of these samples were then recorded, and a standard line curve with the concentration equation and R2 value was created with these results. Using the absorbencies of the dye samples, the concentrations of the soda samples were determined using the slope equation provided by the graphing software.
A table to show the pH of certain solutions Solution Test 1 Test 2 Test 3 Average Distilled water 7.7 7.9 7.8 7.8 2.5 g NaHCO3 (Sodium bicarbonate) 8.1 8.3 8.3 8.2 10ml of 0.85% lactic acid 3.1 3.2 2.9 3.1 5g NaHCO3 (Sodium bicarbonate) 8.1 7.9 8 8 Dry ice 4 4.1 4.2 4.1 Solid NH4Cl 6 6.8 6.5 6.4 0.1M HCl 2.5 2.4 2.3 2.4 Compare the increase or decrease of pH in different solutions to the pH of the distilled water. According to the research done in the Literature Review, acidosis is usually caused by a buildup of lactic acid in the body due to muscle exertion. In comparison to the average pH of the distilled water, the average pH of the lactic acid solution decreased significantly in pH. Similarly, acidosis is caused when there is a buildup