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Chapter 11: Problem 104

Consider the following:What would happen to the level of liquid in the two arms if the semipermeable membrane separating the two liquids were permeable to a. \(\mathrm{H}_{2} \mathrm{O}\) (the solvent) only? b. \(\mathrm{H}_{2} \mathrm{O}\) and solute?

Short Answer

Expert verified
If the semipermeable membrane is permeable to \(\mathrm{H}_{2}\mathrm{O}\) only, water molecules will move from the side of low solute concentration to the side of high solute concentration through osmosis, causing the liquid level to rise on the high solute concentration side and decrease on the other side. If the membrane is permeable to both \(\mathrm{H}_{2}\mathrm{O}\) and solute, the system undergoes diffusion with the solvent and solute molecules moving across the membrane based on concentration gradients. Over time, this process leads to an equilibrium state with equal solute concentrations and liquid levels in each arm.

Step by step solution

01

Semipermeable Membrane Permeable to Water Only

If the semipermeable membrane is permeable to water only (the solvent), then the water molecules will more likely move from the side of low solute concentration to the side of high solute concentration. This process is known as osmosis. It will continue as long as there is a difference in solute concentrations between the two arms. As water molecules move from the side with low solute concentration to the side with high solute concentration, the liquid level on the side with high solute concentration will rise, while the level on the other side will decrease.
02

Semipermeable Membrane Permeable to Both Solvent and Solute

When the semipermeable membrane is permeable to both water and the solute, the system will go through a diffusion process. In this case, both the solvent and solute molecules will move across the membrane based on concentration gradients. The water molecules will still move from the side of low solute concentration to the side with high solute concentration, and the solute molecules will move from the side of high concentration to the side with low solute concentration. Over time, this will create a new equilibrium state in which the concentrations of solute and the liquid levels in each arm will be the same.

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Most popular questions from this chapter

In flushing and cleaning columns used in liquid chromatography to remove adsorbed contaminants, a series of solvents is used. Hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)\), chloroform \(\left(\mathrm{CHCl}_{3}\right)\), methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\), and water are passed through the column in that order. Rationalize the order in terms of intermolecular forces and the mutual solubility (miscibility) of the solvents.

The solubility of benzoic acid \(\left(\mathrm{HC}_{7} \mathrm{H}_{5} \mathrm{O}_{2}\right)\),is \(0.34 \mathrm{~g} / 100 \mathrm{~mL}\) in water at \(25^{\circ} \mathrm{C}\) and is \(10.0 \mathrm{~g} / 100 \mathrm{~mL}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) at \(25^{\circ} \mathrm{C}\). Rationalize this solubility behavior. (Hint: Benzoic acid forms a dimer in benzene.) Would benzoic acid be more or less soluble in a 0.1-M \(\mathrm{NaOH}\) solution than it is in water? Explain.

At \(25^{\circ} \mathrm{C}\), the vapor in equilibrium with a solution containing carbon disulfide and acetonitrile has a total pressure of 263 torr and is \(85.5\) mole percent carbon disulfide. What is the mole fraction of carbon disulfide in the solution? At \(25^{\circ} \mathrm{C}\), the vapor pressure of carbon disulfide is 375 torr. Assume the solution and vapor exhibit ideal behavior.

Consider the following solutions: \(0.010 \mathrm{~m} \mathrm{Na}_{3} \mathrm{PO}_{4}\) in water \(0.020 \mathrm{~m} \mathrm{CaBr}_{2}\) in water \(0.020 \mathrm{~m} \mathrm{KCl}\) in water \(0.020 \mathrm{~m} \mathrm{HF}\) in water \((\mathrm{HF}\) is a weak acid. \()\) a. Assuming complete dissociation of the soluble salts, which solution(s) would have the same boiling point as \(0.040 \mathrm{~m} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) in water? \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) is a nonelectrolyte. b. Which solution would have the highest vapor pressure at \(28^{\circ} \mathrm{C}\) ? c. Which solution would have the largest freezing-point depression?

An aqueous solution is \(1.00 \% \mathrm{NaCl}\) by mass and has a density of \(1.071 \mathrm{~g} / \mathrm{cm}^{3}\) at \(25^{\circ} \mathrm{C}\). The observed osmotic pressure of this solution is \(7.83\) atm at \(25^{\circ} \mathrm{C}\).
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