Neel’s unknown solid 1) dissolves in hot ethanol, 2) is essentially insoluble in hexane, and 3) is insoluble in cold water, but sparingly soluble in warm water. Outline a recrystallization procedure
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- Neel’s unknown solid 1) dissolves in hot ethanol, 2) is essentially insoluble in hexane, and 3) is insoluble in cold water, but sparingly soluble in warm water. Outline a recrystallization procedure.
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- O An ideal recrystallization solvent a) Dissolves the solid when hot and insoluble when cold b) Insoluble when hot and dissolves the solid when cold c) Insoluble when hot or cold d) Soluble when hot or cold Which offers the best separation simple distillation or fractional distillation and why?What properties does recrystallization rely on to be an effective method of purification? A) The product is souble in hot solvent. B) The product is insoluble in cold solvent. C) The impurities are soluble in hot solvent. D) The impurities are soluble in cold solvent. E) The product is insoluble in hot solvent. F) The impurities are insoluble in cold solvent. A, B, C, and D A, B, C, and F B, C, D, and E0.750 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-crystallization
- (c) Draw a well labelled suitable diagram/quick sketch to convert [ turbidity containing raw water to de-aerated demineralized turbidity free water.1) Outline the processes you would adopt to purity and test the purity of sodium benzoate, an active ingredient of most cosmetic products in the laboratory.The boiling points for the compounds are 118 °C and 35 °C respectively. The solubility for both compounds is the same (8g/100g water). Explain this observation for (i) boiling point disparity; (ii) solubility similarity H-bonds form in diethyl ether; n-butyl alcohol forms H-bonds in water H-bonds form in n-butyl alcohol; diethyl ether forms H-bonds in water H-bonds in n-butyl alcohol; Both compounds form H-bonds in water O Both compounds form H-bonds; Both compounds form H-bonds in water
- If the solubility of a compound A in ether is 30g/100 ml, and the solubility of A in water is 15 g /100 ml. a) If 100 ml of aqueous solution of 3g of A are extracted twice with 100 ml ether. How much A total is extracted? b) How much A would be extracted if only one extraction, but with a volume of 200 ml of ether were extracted? c) What is your conclusion from the amount of A extracted in problems a and b above?You were given a mixture of two miscible solvent A and B that you are tasked to separate. You know that solvent A has a boiling point of 49 oC while solvent B has a boiling point of 174 oC. Which of the listed method would overall be the most efficient? Fractional distillation Recrystallization Solid-liquid extraction Liquid-liquid extraction Simple distillation Acid-Base extraction2. Is it possible to purify a compound by recrystallization using a mixture of solvents? Why or why not?
- In order to perform a recrystallization using a mixed-solvent system to dissolve your impure solid. Which of the following could not be used as solvent pairs for such a crystallization? Why could you not use that pair? Which pair would you use and why? A) Water and Diethyl ether B) Water and Ethanol C) Hexane and Diethyl Ether19. A liquefied mixture of n-butane, n-pentane, and n-hexane has the following composition: n-C,H10 50%, n-C,H12 30%, and n-C,H14 20%. For this mixture, calculate: a) The weight fraction of each component. b) The mole fraction of each component. c) The mole percent of each component. d) The average molecular weight of the mixture.2)which set up is fractional distillation