Osmosis and osmotic pressure pdf
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- Osmotic pressure
- 13.7: Osmotic Pressure
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- Osmosis and Osmotic Pressure
Osmotic pressure is a colligative property of solutions that is observed using a semipermeable membrane, a barrier with pores small enough to allow solvent molecules to pass through but not solute molecules or ions. The direction of net solvent flow is always from the side with the lower concentration of solute to the side with the higher concentration. A net flow of water through the membrane occurs until the levels in the arms eventually stop changing, which indicates that equilibrium has been reached. Although the semipermeable membrane allows water molecules to flow through in either direction, the rate of flow is not the same in both directions because the concentration of water is not the same in the two arms.
Osmotic pressure is the minimum pressure which needs to be applied to a solution to prevent the inward flow of its pure solvent across a semipermeable membrane. Potential osmotic pressure is the maximum osmotic pressure that could develop in a solution if it were separated from its pure solvent by a semipermeable membrane. Osmosis occurs when two solutions containing different concentrations of solute are separated by a selectively permeable membrane.
Solvent molecules pass preferentially through the membrane from the low-concentration solution to the solution with higher solute concentration. The transfer of solvent molecules will continue until equilibrium is attained. This formula applies when the solute concentration is sufficiently low that the solution can be treated as an ideal solution.
The proportionality to concentration means that osmotic pressure is a colligative property. Harmon Northrop Morse and Frazer showed that the equation applied to more concentrated solutions if the unit of concentration was molal rather than molar ;  so when the molality is used this equation has been called the Morse equation. To a first approximation,.
The value of the parameter A and of parameters from higher-order approximations can be used to calculate Pitzer parameters.
Empirical parameters are used to quantify the behaviour of solutions of ionic and non-ionic solutes which are not ideal solutions in the thermodynamic sense. The Pfeffer cell was developed for the measurement of osmotic pressure. Osmotic pressure measurement may be used for the determination of molecular weights. Osmotic pressure is an important factor affecting cells. Osmoregulation is the homeostasis mechanism of an organism to reach balance in osmotic pressure.
When a biological cell is in a hypotonic environment, the cell interior accumulates water, water flows across the cell membrane into the cell, causing it to expand.
In plant cells , the cell wall restricts the expansion, resulting in pressure on the cell wall from within called turgor pressure. Turgor pressure allows herbaceous plants to stand upright. It is also the determining factor for how plants regulate the aperture of their stomata.
In animal cells excessive osmotic pressure can result in cytolysis. Osmotic pressure is the basis of filtering " reverse osmosis " , a process commonly used in water purification. The water to be purified is placed in a chamber and put under an amount of pressure greater than the osmotic pressure exerted by the water and the solutes dissolved in it. Part of the chamber opens to a differentially permeable membrane that lets water molecules through, but not the solute particles.
The osmotic pressure of ocean water is about 27 atm. Reverse osmosis desalinates fresh water from ocean salt water. Consider the system at the point when it has reached equilibrium. The condition for this is that the chemical potential of the solvent since only it is free to flow toward equilibrium on both sides of the membrane is equal.
Holding the pressure, the addition of solute decreases the chemical potential an entropic effect. Thus, the pressure of the solution has to be increased in an effort to compensate the loss of the chemical potential.
The addition to the pressure is expressed through the expression for the energy of expansion:. Inserting the expression presented above into the chemical potential equation for the entire system and rearranging will arrive at:. Thus, we get. The activity coefficient is a function of concentration and temperature, but in the case of dilute mixtures, it is often very close to 1.
Combining these gives the following. For aqueous solutions of salts, ionisation must be taken into account. For example, 1 mole of NaCl ionises to 2 moles of ions. From Wikipedia, the free encyclopedia.
Pratt Fundamentals of Biochemistry Rev. New York: Wiley. Oxford University Press. Journal of the American Chemical Society.
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13.7: Osmotic Pressure
Semipermeable Membrane:. A semipermeable membrane is a membrane which allows the solvent molecules, but not the solute molecules through it. The spontaneous and unidirectional flow of solvent molecules through a semipermeable membrane, into a solution OR flow of solvent from a solution of low concentration to a solution of higher concentration through a semipermeable membrane, is called osmosis. Everyday Examples of Osmosis:. A wide-mouthed thistle funnel with a narrow long stem was taken.
Osmotic pressure is the pressure which must be applied to a solution to prevent the inward flow of water across a semipermeable membrane. Osmotic pressure is the pressure which needs to be applied to a solution to prevent the inward flow of water across a semipermeable membrane. It is also defined as the minimum pressure needed to nullify osmosis. The phenomenon of osmotic pressure arises from the tendency of a pure solvent to move through a semi-permeable membrane and into a solution containing a solute to which the membrane is impermeable. Osmosis causes water to flow from an area of low solute concentration to an area of high solute concentration until the two areas have an equal ratio of solute to water. Normally, the solute diffuses toward equilibrium as well; however, all cells are surrounded by a lipid bilayer cell membrane which permits the flow of water in and out of the cell but restricts the flow of solute under many circumstances. As a result, when a cell is placed in a hypotonic solution, water rushes into the membrane, increasing its volume.
PDF | On Mar 26, , Uri Lachish published Osmosis Reverse Osmosis and Osmotic Pressure what they are | Find, read and cite all the.
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Osmosis is one of the most important biological processes in living things for it is the method allowing water to spread around the cells; without water, the cells will die. This Resource Guide on Osmosis will illustrate how important this process is to survival. Osmosis is the passage of water from a low solute concentration area through a semi-permeable membrane to a high solute concentration area to equalize the solute concentrations on both sides.
Osmosis and Osmotic Pressure
Osmotic pressure is the minimum pressure which needs to be applied to a solution to prevent the inward flow of its pure solvent across a semipermeable membrane. Potential osmotic pressure is the maximum osmotic pressure that could develop in a solution if it were separated from its pure solvent by a semipermeable membrane. Osmosis occurs when two solutions containing different concentrations of solute are separated by a selectively permeable membrane. Solvent molecules pass preferentially through the membrane from the low-concentration solution to the solution with higher solute concentration. The transfer of solvent molecules will continue until equilibrium is attained. This formula applies when the solute concentration is sufficiently low that the solution can be treated as an ideal solution.
A solution is defined as a homogeneous mixture of both a solute and solvent. Solutions generally have different properties than the solvent and solute molecules that compose them. Some special properties of solutions are dependent solely on the amount of dissolved solute molecules, regardless of what that solute is; these properties are known as colligative properties. Osmosis is defined as the net flow or movement of solvent molecules through a semipermeable membrane through which solute molecules cannot pass. If a solution consisting of both solute and solvent molecules is placed on one side of a membrane and pure solvent is placed on the other side, there is a net flow of solvent into the solution side of the membrane.
The thistle funnel is lowered into a beaker containing water. The membrane is such that it allows only the molecules of the solvent and not of the solute to pass through it. Thus, there will be movement of water molecules from pure solvent into the solution. As a result, water passes into the thistle funnel and level of solution in the thistle funnel rises gradually. This process is called osmosis. The phenomenon of the flow of solvent through a semipermeable membrane from pure solvent to the solution is called osmosis.
Two other definitions were also found: (5) osmosis is the process by which osmotic pressure is de- veloped and diffusion of solute molecules hindered; (6) osmosis.