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Chapter 13: Problem 43

What is osmosis? What is a semipermeable membrane?

Short Answer

Expert verified
Osmosis is the spontaneous net movement of solvent from a region of low solute concentration, through a semipermeable membrane, to an area of high solute concentration. A semipermeable membrane is a type of biological or synthetic, polymeric membrane that will allow certain molecules or ions to pass through it by osmosis. Examples of both can be found in cells within the body.

Step by step solution

01

Define Osmosis

Osmosis is the spontaneous net movement of solvent (most commonly water) from a region of low solute concentration, through a semipermeable membrane, to an area of high solute concentration with the aim to equalize the solute concentrations on the two sides.
02

Give examples of Osmosis

Examples of osmosis can be found in our daily life. When a raisin is placed in a cup of water, it puffs up due to osmosis. In a biological context, osmosis is vitally important for cell survival. Cells are always trying to achieve osmotic balance.
03

Define Semipermeable Membrane

A semipermeable membrane is a type of biological or synthetic, polymeric membrane that will allow certain molecules or ions to pass through it by osmosis.
04

Give examples of Semipermeable Membrane

In biological systems, the most common example of a semipermeable membrane would be the cell membrane. In a synthetic context, it could be a sheet of plastic with small holes in it.

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Most popular questions from this chapter

The density of an aqueous solution containing 10.0 percent ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) by mass is \(0.984 \mathrm{~g} / \mathrm{mL}\). (a) Calculate the molality of this solution. (b) Calculate its molarity. (c) What volume of the solution would contain 0.125 mole of ethanol?

A mixture of liquids \(A\) and \(B\) exhibits ideal behavior. At \(84^{\circ} \mathrm{C},\) the total vapor pressure of a solution containing 1.2 moles of \(A\) and 2,3 moles of \(B\) is 331 \(\mathrm{mmHg}\). Upon the addition of another mole of \(\mathrm{B}\) to the solution, the vapor pressure increases to 347 \(\mathrm{mmHg}\). Calculate the vapor pressures of pure \(\mathrm{A}\) and \(\mathrm{B}\) at \(84^{\circ} \mathrm{C}\)

What is the osmotic pressure (in atmospheres) of a \(12.36 M\) aqueous urea solution at \(22.0^{\circ} \mathrm{C} ?\)

Calculate the percent by mass of the solute in each of these aqueous solutions: (a) \(5.50 \mathrm{~g}\) of \(\mathrm{NaBr}\) in \(78.2 \mathrm{~g}\) of solution, (b) \(31.0 \mathrm{~g}\) of \(\mathrm{KCl}\) in \(152 \mathrm{~g}\) of water, \((\mathrm{c})\) \(4.5 \mathrm{~g}\) of toluene in \(29 \mathrm{~g}\) of benzene.

Write the equation relating osmotic pressure to the concentration of a solution. Define all the terms and give their units.
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