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- 20 ml of a 100 mg/l phenol solution in water is placed in a vial with 20 ml of a fluorocarbon solvent. The organic phase (fluorocarbon solvent) is immiscible with water. The vial is completely filled with the two phases, thus there is no air or contaminant volatilization. After an hour of agitation, the two phase system reaches equilibrium. The two phases are separated and the fluorocarbon is analyzed for total phenol. The resulting phenol concentration in the organic phase is 16.0 mg/l. Compute the unitless partition coefficient (KF-W) for phenol. Compare your calculation with KF-W obtained from an empirical relationship: log10KF-W 0.71 - 0.862log10 CWsat. KF-W means the partition between the fluorocarbon solvent, F, and water, W. Only typed solution.Calculate how many grams of phthalic acid remained in the chilled water (the “mother liquor”) based on the solubility data given (show your work). You will recrystallize phthalic acid, a compound that is used to manufacture synthetic polymers and perfumes. Phthalic acid is very soluble in boiling water, 18 g/100 mL, and is much less soluble in chilled (14°C) water, 0.54 g/100 mL. Thus, water is a very good recrystallization solvent for phthalic acid. 54.8% percent recovery was calculatedSOLUBLE if the first substance is soluble in the second substance and INSOLUBLE if it does not dissolve. 1. Hexane + water SOLUBLE INSOLUBLE 2. Cyclohexene + water SOLUBLE INSOLUBLE 3.Vanillin + sodium hydroxide * SOLUBLE INSOLUBLE 4.Cinnamaldehyde + ethyl alcohol SOLUBLE INSOLUBLE 5.Chloroform + sodium hydroxide * SOLUBLE INSOLUBLE 6.Iodoform + ethyl alcohol * SOLUBLE INSOLUBLE 7.Glycerol + water * SOLUBLE INSOLUBLE
- State whether you would want to use a fractional or simple distillation for each of the cases below. Assume the mixture contains a 1:3 mixture of two components A and B, where component A is the lower boiling point component. Briefly explain each of your answers. 1. You need a really pure sample of component A. 2. You just need each component to be at least 85% pure and want the MAXIMUM amount of distillate out.Students were tasked to conduct a recrystallization experiment to test the ability of the newly discovered solvents in their laboratory to purify and separate a mixture containing compounds X and Y. The solubility of the two compounds in g/50 mL of hot and cold solvents are given by the photo.During the distillation of the Bromobenzene and water mixture which fraction is richer in Bromobenzene: a) First fraction b) Second fraction c) The last fraction d) All fractions have the same composition
- 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-crystallizationSolid-liquid extraction is an effective method to isolate a the desired soluble component in a solid mixture from insoluble materials in the mixture. True FalseA group was given the responsibility of performing a recrystallization experiment in their laboratory to see if the three newly found solvents could purify and separate a mixture including compounds A and B. The following are the solubilities of the two compounds in g/100 mL of hot and cold solvents: Solubility in g/100 mL solvent A B Solvent Hot Cold Hot Cold 1 4.60 1.10 5.30 1.90 2 6.40 5.80 8.40 1.10 3 9.70 3.30 6.80 1.70 What is the %recovery and %purity of A and B in the chosen solvent? Show solutions pls
- Suppose that you have a 1:1 mixture of compounds that is comprised of compound X and compound Y. You desire pure compound X and are planning a recrystallization to enhance the purity. Which solvent below is optimal for your recrystallization? Ethanol (boiling point = 78 °C) Solubility At 0 °C 100 °C Compound X 0.05 g/mL 0.20 g/mL Compound Y 0.02 g/mL 0.40 g/mL Water (boiling point = 100 °C) Solubility At 0 °C 100 °C Compound X 0.02 g/mL 0.05 g/mL Compound Y 0.01 g/mL 0.10 g/mL Methanol (boiling point = 65 °C) Solubility At 0 °C 65 °C Compound X 0.04 g/mL 0.10 g/mL Compound Y 0.02 g/mL 0.30 g/mL Acetone (boiling point = 56 °C) Solubility At 0 °C 56 °C Compound X 0.10 g/mL 0.50 g/mL Compound Y 0.20 g/mL 0.50 g/mL Ethyl Acetate (boiling point = 77 °C) Solubility At 0 °C 77 °C Compound X 0.10 g/mL 0.60 g/mL Compound Y 0.30 g/mL 0.60…Supposed you are in a chemistry laboratory gave you a 500 ml Erlenmeyer flask containing 200 ml of heterogenous liquid mixture. This liquid mixture consists of sodium chloride, water, benzoic acid, is made by combining Mixture A and Mixture B. Mixture A (aqueous mixture): sodium chloride is dissolved in distilled water. Mixture B (organic mixture): benzoic acid, phenol and aniline is dissolved in petroleum ether (a nonpolar solvent). Your task is to separate the components of the heterogenous mixture and identify the components. What wet chemical analysis/qualitative test should be performed to detect the compounds?50.0 mL of a 0.60 M solution of pyridine in ethanol is to be prepared by measuring out a known volume of pure liquid pyridine and diluting to 500 mL with ethanol. The molar mass of pyridine is 79.1 g/mol, and its density at room temperature is 0.982 g/mL. What volume of pyridine is required for this solution?