Answered: A solute with a partition coefficient…

A solute with a partition coefficient (K-15]s/1S]) of 5 is extracted from 20 mL of phase 1 into phase 2. What volume of phase 2 is needed to extract 90% of the solute in one extraction? (

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter13: Solutions And Their Behavior

Section13.5: Colloids

Problem 2.3ACP

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(1a) Pure benzophenane freezes at 66.6 °C. A solution of 7.75 g of biphenyl (C12H10; molar mass = 154.2g/mol) plus 200.08 g of benzophenane froze at 59.9 °C. Calculate the Kf of benzophenane in °C*kg/mol. (b) An unknown solution with possible cations (Ag+, Hg22+, Pb2+) is treated with 6M HCl and a white precipitate forms. Hot water is added to the precipitate, and a white solid remains after filtration. The white solid is treated with aqueous NH3, and the precipitate turns grey or black. The resulting solution is treated with HNO3 and no precipitate forms. What cations can you determine to be present, absent or maybe present? Explain your reason
Can you please answer number 7 and show all of the steps to the solution
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the molality of the solution.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the mass of potassium chloride present in the salt sample.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate ΔTf for the experiment.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride.1. Calculate ΔTf for the experiment.2. Calculate the molality of the solution.3. Calculate the mass of potassium chloride present in the salt sample.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride.1. Calculate ΔTf for the experiment.2. Calculate the molality of the solution.3. Calculate the mass of potassium nitrate present in the salt sample.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the mass of potassium nitrate present in the salt sample.
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