The osmotic pressure of a solution that contains 0.026g of a hydrocarbon solute is 4.0 torr.
What is osmotic pressure?
The amount of pressure needed to keep a pure solvent from osmosing into a specific solution; this pressure is frequently employed to represent the concentration of the solution.
moles of solute=mass/molar mass =0.026/340g/mol=7.647×10⁻⁵
Molarity=moles/volume in solution
=7.647ₓ10⁻⁵/0.350L=0.000218M
osmotic pressure(Pi)=MRT
Pi=0.000218ₓ0.0821ₓ293
=0.00525atm
now,1 atm= 760 torr
so, 0.00525 atm= (760ₓ0.00525)
=3.99 torr
=4.00 torr
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