Which of the following statements is necessarily true? OA lon-pairing causes the experimentally determined van't Hoff factor to be greater than the predicted van't Hoff factor. OBA0.100 m solution of a weak electrolyte will have a lower boiling point than a 0.100 m solution of a non-electrolyte. OC Osmosis refers to the flow of solvent through a semi-permeable from the more dilute solution side to the more concentrated solution side. OD The freezing point of an aqueous solution containing a non-volatile solute is higher than the freezing point of water. OE The boiling point of all NaCl solutions, regardless of concentration, is the same.

Which of the following statements is necessarily true? OA lon-pairing causes the experimentally determined van't Hoff factor to be greater than the predicted van't Hoff factor. OBA0.100 m solution of a weak electrolyte will have a lower boiling point than a 0.100 m solution of a non-electrolyte. OC Osmosis refers to the flow of solvent through a semi-permeable from the more dilute solution side to the more concentrated solution side. OD The freezing point of an aqueous solution containing a non-volatile solute is higher than the freezing point of water. OE The boiling point of all NaCl solutions, regardless of concentration, is the same.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.103QE

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The freezing point of a 0.031-m solution of copper(II) sulfate in water is 0.075 C. (a) Calculate the vant Hoff factor, i, for this solution. (b) Would the vant Hoff factor be larger, smaller, or the same for a 0.050-m solution of this compound?
Consider two solutions at a certain temperature. Solution X has a nonelectrolyte as a solute and an osmotic pressure of 1.8 atm. Solution Y also has a nonelectrolyte as a solute and an osmotic pressure of 4.2 atm. What is the osmotic pressure of a solution made up of equal volumes of solutions X and Y at the same temperature? Assume that the volumes are additive.
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a. Calculate the freezing-point depression and osmotic pressure at 25C of an aqueous solution containing 1.0 g/L of a protein (molar mass = 9.0 104 g/mol) if the density of the solution is 1.0 g/cm3. b. Considering your answer to part a, which colligative property, freezing-point depression or osmotic pressure, would be better used to determine the molar masses of large molecules? Explain.
The vapor pressure of methanol, CH3OH, is 94 torr at 20 C. The vapor pressure of ethanol, C2H5OH, is 44 torr at the same temperature. (a) Calculate the mole fraction of methanol and of ethanol in a solution of 50.0 g of methanol and 50.0 g of ethanol. (b) Ethanol and methanol form a solution that behaves like an ideal solution. Calculate the vapor pressure of methanol and of ethanol above the solution at 20 C.
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.