This solution was diluted with diluents to gae a concentration of 0.1 mg/ml solution each of Amoxicillin trihydrate. The HPLC method was applied to the solutions and the results obtained were shown in table 4.6.11. System suitability solution: 25.0 µg/mL each of of USP Amoxicillin RS in Diluent. Precision
Then percent yield was calculated to be 67.57%. The isolation of less product resulted from using less amount of acetanilide than 0.07g at the beginning of the experiment. In addition, the melting point of the product was measured to be 164.8-168.50c, which is in the range of the normal melting point of 4-bromoacentailide, 165-1690c. This confirmed the formation of 4-bromoacetanilide from the bromination of acetanilide. From the bromination of 0.05g aniline, 0.156g of the product was collected.
Standardization of NaOH solution Accurately weigh out a sample of approximately 0.3-0.4 g of primary standard potassium hydrogen phthalate, KHPh, which has been previously dried at 120°C. Do not use more than 0.4 g. To obtain an accurate mass, weigh the sample on weighing paper, slide it into a clean (but not necessarily dry) 250 mL Erlenmeyer flask and reweigh the paper to account for any KHPh that may remain on it. Dissolve the KHPh sample in about 50 mL of CO2-free water and add 2-3 drops of 0.1% phenolphthalein indicator. Begin adding the approximately 0.1 M sodium hydroxide solution from the buret while continuously swirling the flask contents. Do not open the stopcock completely.
In the experiment 1 of intermolecular forces via evaporation, groups were challenged to gain a better understanding of the molecular forces in alkanes and alcohols while also exploring the impact of molar mass on intermolecular forces. Before starting, it must be understood that evaporation is an endothermic process. Substances with weak intermolecular forces will experience a greater temperature drop. Strong intermolecular forces will not experience a great temperature change. Because of the key statements listed, the group predicted that alcohols would experience little temperature change due to the strong intermolecular forces within them.
Synthesis of 3-[5-(4-substituted) phenyl-1,3,4-oxadiazole-2yl]-2-styrylquinazoline-4(3H)-ones was carried out by following steps: Step 1: Synthesis of 4- substituted benzaldehyde semicarbazon51(2) Semicarbazide Hydrochloride (0.1M) and sodium acetate (0.2M) was added and dissolved in 15-20ml of distilled water placed in flat-bottomed flask. In a separate beaker containing required aromatic aldehyde (1) (0.1M) was dissolved in aldehyde free alcohol. This ethanolic aromatic aldehyde solution was added slowly to the solution of semicarbazide hydrochloride. The precipitate, which gets separated, was filtered, dried and recrystallised from 95% hot ethanol. Table 1: Quantity of aldehydes taken S. No.
A total of 0.1 ml of supernatant was added to cuvette containing 1.9 ml of 50mM phosphate buffer (pH 7). The reaction was started by the addition of 1 ml freshly prepared 30mM H2O2. The rate of decomposition of H2O2 was measured spectrophotometrically at 240 nm. Catalase values were expressed as n moles H2O2 consumed/min/mg protein. Measurement of lipid peroxidation TBARS, a measure of lipid per oxidation, was measured as described by Ohkawa .
The substitution reaction was successful but not fully effective. 19. If the data was inconclusive, then comparing various compounds and the unknown based on physical characteristics would be the first step, titrations would also be a good method. 20. To get a better yield, redoing the experiment would require careful attention in the recrystallization steps: amount of solvent used, how hot solvent is, if the mixture cools to room temperature before placing it in an ice
The reagents used were Diphenylamine reagent which contains concentrated H2SO4. The standard solution used for this test is the deoxyribose standard solution. In the sample, only a faint blue solution appeared, which indicates a small presence of deoxyribose. In test for Phosphate, the standard solution was the Phosphate solution and the reagents used were concentrated H2SO4, concentrated HNO3, 2.5% ammonium molybdate solution. The principle involved in this test is the precipitation of phosphate which bores a yellow-colored solution and yellow precipitate.
This does not show mass being destroyed but what most likely happened was the paper burning and the fumes being released into the air. It also could have been that we could've lost flakes of the paper during the