The pressure that must be applied to a more concentrated solution to prevent the flow of pure solvent into the solution separated by a semipermeable membrane is called the osmotic pressure. This relationship can be expressed as follows:
PV = nRT
Where,
- P = is the pressure (atm),
- V = is the volume (L),
- N = is number of moles of solute,
- R = is the gas constant (0.082 L atm/mol deg), and
- T = is the absolute temperature (°C).
Example:
What is the osmotic pressure of 50 g dextrose in 1,000 mL of water at room temperature (25°C)?
P = [(0.28)(0.082)(298)]/(1)
= 6.84 atm
Where,
- n = (50 g dextrose)/(MW of 180) = 0.28 mol of dextrose,
- T = 273°C + 25°C = 298°C
- V = 1 L
- R = 0.082 L atm/mol deg
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