Penicillin F is recovered from a dilute aqueous fermentation broth by extraction with amyl acetate, using 6.5 volumes of solvent per 100. volumes of the aqueous phase. At pH = 3.8 the distribution coefficient KD is 74. (a) What fraction of the penicillin would be recovered in a single ideal stage? (b) What would be the recovery with three-stage extraction using fresh solvent in both

Penicillin F is recovered from a dilute aqueous fermentation broth by extraction with amyl acetate, using 6.5 volumes of solvent per 100. volumes of the aqueous phase. At pH = 3.8 the distribution coefficient KD is 74. (a) What fraction of the penicillin would be recovered in a single ideal stage? (b) What would be the recovery with three-stage extraction using fresh solvent in both

Macroscale and Microscale Organic Experiments

7th Edition

ISBN:9781305577190

Author:Kenneth L. Williamson, Katherine M. Masters

Publisher:Kenneth L. Williamson, Katherine M. Masters

Chapter7: Extraction

Section: Chapter Questions

Problem 1Q

See similar textbooks

Similar questions

The mean activity coefficients of KCl in three dilute aqueous solutions at 25 °C are 0.927 (at 5.00 mmol kg−1), 0.902 (at 10.0 mmol kg−1), and 0.816 (at 50.0 mmol kg−1). Estimate the value of B in the Davies equation.
what is the purpose of preparing of a standard sodium hydroxide solution in determination of purity of impure KHP?
The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
Calculate the gravimetric factor of the following. 2 Fe is sought(Analyte), 1Fe2O3 is weighed (Precipitate)
Is there a difference when the needle or metal clip is placed on the surface of distilled water with dilute amounts of liquid detergent? Explain your observations in terms of the strength of IMFA present in each condition.
Calculate the fraction of intact H2PO3 molecules in an aqueous solution of phosphorous acid at (a) pH = 5.0 and (b) pH =9.0.
The molar conductivity of 0.010 M CH3COOH(aq) is 1.65 mS m2 mol-1. What is the acidity constant, Ka, of the acid?
The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
In an experiment to determine the concentration of H2SO4 in a brand of toilet cleanser, 10.0 cm3 of the cleanser was first diluted to 250.0 cm3 with distilled water. 25.0 cm3 of the diluted cleanser were titrated with 0.320 mol dm–3 NaOH solution, using methyl orange as indicator.If 29.2 cm3 of NaOH solution is used, what is the concentration of H2SO4 in the undiluted toilet cleanser?a. 2.30 mol dm–3b. 4.60 mol dm–3 c. 9.20 mol dm–3 d. 11.50 mol dm–3
A sample of an iron ore was prepared for Fe3+ analysis as following: 3.4g of the sample was added anddissolved in acid environment then diluted to 250 mL using volumetric flask. After that, 10 mL of the resultingsolution was transferred by pipet to a 50-mL volumetric flask and continue to be diluted. The scientists foundout that this solution gives the concentration of Fe3+ as 2.3 mg/L. Find the weight percentage of Fe3+ in theoriginal sample.
An acid solution containing 2 per cent by mass of NaNO3, and an unknown concentration of HNO3 is used to regenerate a strong acid resin. After sufficient acid had been passed over the resin for equilibrium to attained, analysis showed that 10 per cent of resin sites were occupied by sodium ions. What was the concentration of HNO3 in the solution, if its density were 1,030 kg/cu.m.?
Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.