Briefly explain the laws of osmotic pressure.
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van’t Hoff’s Theory of Osmotic Pressure:
He found that the solute particles in dilute solutions possess kinetic energy and move in a random directions in the solutions. Thus they have similar behaviour as that of gas molecules.
On collision against semipermeable membrane the solute molecules exert osmotic pressure equal to the pressure which the solute molecules would exert if it were gas molecule at the same temperature and occupying the same volume as that of solution.
Thus the gas laws are equally applicable to dilute solutions.
At constant temperature the osmotic pressure (π) of a dilute solution is directly proportional to its molar concentration (C) or inversely proportional to volume (V) of the solution.
He found that the solute particles in dilute solutions possess kinetic energy and move in a random directions in the solutions. Thus they have similar behaviour as that of gas molecules.
On collision against semipermeable membrane the solute molecules exert osmotic pressure equal to the pressure which the solute molecules would exert if it were gas molecule at the same temperature and occupying the same volume as that of solution.
Thus the gas laws are equally applicable to dilute solutions.
At constant temperature the osmotic pressure (π) of a dilute solution is directly proportional to its molar concentration (C) or inversely proportional to volume (V) of the solution.
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These are the types of laws considered in the situation of osmotic pressure ::
the osmotic pressure of a gas is directly proportional to its concentration and inversely proportional to its volume.
Vant Hoff's Charle's law : the osmotic pressure of a gas is directly proportional to absolute temperature.
the osmotic pressure of a gas is directly proportional to its concentration and inversely proportional to its volume.
Vant Hoff's Charle's law : the osmotic pressure of a gas is directly proportional to absolute temperature.
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