Osmosis
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Osmosis is the diffusion of a solvent through a semipermeable membrane from a region of low solute concentration to a region of high solute concentration. The semipermeable membrane is permeable to the solvent, but not to the solute, resulting in a chemical potential difference across the membrane which drives the diffusion. That is, the solvent flows from the side of the membrane where the solution is weakest to the side where it is strongest, until the solution on both sides of the membrane is the same strength (that is, until the chemical potential is equal on both sides).
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Osmosis is an important topic in biology because it provides the primary means by which water is transported into and out of cells.
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Explanation
Consider a semi-permeable membrane that allows water to pass through it, but not larger solutes such as salt. First, suppose such a membrane separates two volumes of pure water. At a macro scale, there will be no flow from one side of the membrane to the other, but at a micro scale, every time a water molecule hits the membrane, it has a certain probability of passing through; individual molecules are passing through the membrane all the time, but the circumstances on both sides are the same so the net flow is zero. Now imagine the same membrane separates a volume of pure water from a volume of a solution. Again, every time a water molecule hits the membrane, it has a certain chance of passing through, but because there are fewer water molecules per volume in the solution, the water molecules on that side will collide with the wall less frequently. As a result, there will be a net flow of fresh water to the side with the solution. Assuming the membrane does not break, this net flow will slow and finally stop as the pressure on the solution side becomes such that the diffusion in each direction is equal.
Example of osmosis
A practical example of this osmosis in cells can be seen in red blood cells. These contain a high concentration of solutes including salts and protein. When the cells are placed in solution, water rushes in to the area of high solute concentration, bursting the cell.
Many plant cells do not burst in the same experiment. This is because the osmotic entry of water is opposed and eventually equalled by the pressure exerted by the cell wall, creating a steady state. In fact, osmotic pressure is the main cause of support in plant leaves.
When a plant cell is placed in a solution higher in solutes than inside the cell osmosis out of the cell occurs. The water in the cell moves to an area higher in solute concentration, and the cell shrinks and so becomes flaccid. This means the cell has become plasmolysed - the cell membrane has completely left the cell wall due to lack of water pressure on it.
In unusual environments, osmosis can be very harmful to organisms. For example, freshwater and saltwater aquarium fish placed in water with an different salt level (than they are adapted to) will die quickly, and in the case of saltwater fish rather dramatically. In addition, the use of table salt to kill leeches and slugs depends on osmosis.
Chemical potential
When a solute is dissolved in a solvent, the random mixing of the two species results in an increase in the entropy of the system, which corresponds to a reduction in the chemical potential. For the case of an ideal solution the reduction in chemical potential corresponds to:
- <math>RT \ln(1 - x_2) \qquad (1)<math>
where <math>R<math> is the gas constant, <math>T<math> is the temperature and <math>x_2<math> is the solute concentration in terms of mole fraction. Most real solutions approximate ideal behavior for low solute concentrations (At higher concentrations interactions between solute and solvent cause deviations from Equation 1). This reduced potential creates a driving force and it is this force which drives diffusion of water through the semipermeable membrane.
Osmotic pressure
As mentioned before, osmosis can be opposed by increasing the pressure in the region of high solute concentration with respect to that in the low solute concentration region. The force per unit area required to prevent the passage of water through a semi-permeable membrane and into a solution of greater concentration is equivalent to the osmotic pressure of the solution, or turgor. Osmotic pressure is a colligative property, meaning that the property depends on the concentration of the solute but not on its identity.
Increasing the pressure increases the chemical potential of the system in proportion to the molar volume (<math>\delta\mu = \delta PV<math>). Therefore, osmosis stops, when the increase in potential due to pressure equals the potential decrease from Equation 1, i.e.:
- <math>\delta PV = -RT \ln(1-x_2)\qquad (2)<math>
Where <math>\delta P<math> is the osmotic pressure and <math>V<math> is the molar volume of the solvent.
For the case of very low solute concentrations, -ln(1-<math>x_2<math>) ≈ <math>x_2<math> and Equation 2 can be rearranged into the following expression for osmotic pressure:
- <math>\delta P = RTx_2/V \qquad (3)<math>
Reverse osmosis
The osmosis process can be driven in reverse with solvent moving from a region of high solute concentration to a region of low solute concentration by applying a pressure in excess of the osmotic pressure. This reverse osmosis technique is commonly applied to purify water. Sometimes the term "forward osmosis" is used for osmosis, particularly when used for rehydrating dried food using contaminated water.
See also
Osmosis Jones is also a term which entered popular parlance after the film of the same name, also the alias of a famed botanist.zh:渗透 da:Osmose de:Osmose es:smosis fr:Osmose it:Osmosi he:אוסמוזה nl:Osmose pl:Osmoza pt:Osmose sl:Osmoza fi:Osmoosi uk:Осмос