0.100 g sample of phthalic acid was dissolved in 100 mL of water. When 25 ml of diethyl ether was used to extract the phthalic acid, 42 mg of the acid were recovered. What is the distribution coefficient for this extraction? Use IMF to explain your result.
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- 0.750 g of crude acetylsalicylic acid is recrystallized using ethanol as the solvent. The solubility of acetylsalicylic acid in ethanol at 78 oC is 15.45 g per 100 mL. a) How much hot ethanol is needed to dissolve the 0.750 g of acetylsalicylic acid? b) If the solubility of acetylsalicylic acid at 25 oC is 0.100 g per 100 mL, how much acetylsalicylic acid will be obtained after crystallization in ethanol at 25 oC? Use the volume from part A. c) What is the maximum percent recovery for this re-crystallizationA titration experiment required 12.50 ml of standard hydrochloric acid solution to reach the phenolphthalein endpoint. A few drops of methyl orange were added into the analyte, and it consumed 23.60 mL more of the standard acid solution. Which of the following is TRUE about the analysis? The analyte contains only sodium bicarbonate solution. The analyte contains sodium hydroxide and sodium bicarbonate solution. The analyte contains sodium hydroxide only The analyte contains both sodium carbonate and sodium bicarbonate solution. The analyte contains only sodium carbonate solution.A certain lipid sample consists of a wax of unknown molecular weight and composition. It is known, however, that the 2 groups are the same fatty acids. In order to investigate this, saponification and iodine numbers were used. A 3.000 g wax sample was placed under reflux with 20.00 mL of 0.7000 M KOH (56.1056 mg/mmol). It was then back-titrated using a 0.3500 M HCl titrant that required 23.91 mL to the phenolphthalein endpoint. To further characterize this, a 0.100 g sample was titrated for its iodine number. This consumed 3.50 mL of 0.100 N thiosulfate titrant. (Iodine: 126.905 g/eq) a) What is the saponification number of this wax sample? b) What is its Iodine number? c) How would you describe this in terms of unsaturation? d) Given that it is a wax, what is the general structure of this lipid? e) What will be the MW factor for this lipid? f) What is the average MW of the lipid? g) Given the table of molecular weights below, what is the possible identity of the wax? Compound MW…
- a) 0.132g of a pure carboxylic acid (R-COOH) was dissolved in 25.00mL of water and titrated with 0.120M of standardised NaOH solution. A volume of 14.80mL was required to reach the endpoint of the titration.Identify the carboxylic acid.b) A 0.670g sample of barium hydroxide is dissolved and diluted to the calibration mark in a 250.0mL volumetric flask. It was found that 11.56mL of this solution was needed to neutralise 25.00mL of nitric acid solution. Calculate the molarity of the nitric acid solution. Write a chemical equation in your response.c) One student's results are given below:- Concentration of NaOH(aq) = 0.110M- Volume of undiluted vinegar = 10.00mL- total volume of diluted vinegar = 100.00mL- volume of diluted vinegar used in each titration = 20.00mL- Avg. titre of NaOH(aq) = 15.35mLBased on these results, calculate the concentration, in mol L-1, of acetic acid in the undiluted vinegar solution.0.641 g of a semi-synthetic alkaloid was dissolved in 25 ml of 1% w/v acetic acid and wasanalysed directly by HPLC. The solution was found to contain 1.42 mg/100 ml of an impurity.What is the level of impurity in % w/w and ppm? Calculate the pH of a buffer system made by dissolving 1.2 g of acetic acid and 0.82 g ofsodium acetate in 500 ml of distilled water (pKa of acetic acid = 4.7)You have 100 mL of an organic acid solution in water which contains 0.30 g acid. The distribution coefficient of the acid in the ether is close to 10. Calculate the amount of acid that would be left in water after four 20-mL extraction with ether. Do the same calculation using one 80-mL extraction with ether to determine which method is more efficient.
- Tea leaves were boiled and around 1.00 gram of caffeine were extracted using 175.0 ml of water. if three portions of 20.0 ml of dichloromethane were ised to extract the caffeine from the aqueous layer how may caffeine will be extracted by dichloromethane? Solubility of caffeine in water: 2.18 g per 100 ml water Solubility of caffeine in dichloromethane: 18.2 g per 100 ml dichloromethaneFour tablet samples (1.6308 g) which contain acetylsalicylic acid were dissolved in a 100 mL water/ethanol mixture. A 25-mL aliquot was obtained and titrated with standard 0.1273 N NaOH solution using a pH meter. The potentiometric data are given below. Calculate the % acetylsalicylic acid (EW=180.157 g/mol) per tablet. Prove that the active ingredient is indeed acetylsalicylic acid (pKa=3.48).Using the 1 mM solution of p-nitrophenol (PNP) provided, create a series of dilutions. You will make 10, 25, 50, 75, and 100 μM solutions. In making these solutions, use 1x reaction buffer (0.2 M Tris, pH 8.0; 5 mM MgCl2) as the diluent. You will need 1 mL of each of these solutions
- In a test tube with 0.3 mL of N,N-dimethylaniline, 5 mL of 10% NaOH, 0.4 mL of benzene sulfonyl chloride. Add a few drops of 4M KOH to make sure it is alkaline and use a litmus paper. Let it stand for 10 minutes. Pour 6M HCl dropwise until it acidify. Explain what happens to the mixture before and after adding HCl. If a precipitate is formed, collect it by filtration or decantation. Test for solubility of the precipitate in 3 mL of 2.5M NaOH. Heat to 50 OC. Shake the tube well for 3 minutes. Explain what happens to the mixture after adding NAOH. N-methylanilineHow do the reactions of phenol samples with FeCl3compare? Which structural component of the phenols account for the observation? 2. What compound is the precipitate formed in the Bromine water test? 3. Write the reaction formed in the formation of phenolphthalein. Identify the functional group in phenolphthalein, which is responsible for the indicator property. 4. What is the significance of Millon's test?Alkaloids present in 20.0 grams of dried leaves containing 0.20% w/w of alkaloids was completely extracted by boiling the leaves with 250.0 mL of water. The alkaloids were extracted by single extraction using 60.0 mL of dichloromethane. The mass of the alkaloid, after drying was determined to be 35.0 mg. Compute the distribution coefficient of the alkaloid in water and DCM. If three times extraction was done using 20.0 mL of DCM for each extraction. How much alkaloid can be collected?