The osmotic pressure of a solution formed by dissolving 35.0 mg of aspirin (c9h8o4) in 0.250 l of water at 25°c is atm.

The osmotic pressure of aspirin is 0.0190 atm

Explanation:

To calculate the molarity of solution, we use the equation:

We are given:

Mass of solute (aspirin) = 35.0 mg = 0.035 g    (conversion factor: 1 g = 1000 mg)

Molar mass of aspirin = 180.16 g/mol

Volume of solution = 0.250 L

Putting values in above equation, we get:

To calculate the osmotic pressure, we use the equation:

where,

= osmotic pressure of the solution

i = Van't hoff factor = 1 (for non-electrolytes)

M = molarity of aspirin =

R = Gas constant =

T = temperature of the solution =

Putting values in above equation, we get:

Hence, the osmotic pressure of aspirin is 0.0190 atm

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answer: h+ its less than oh

explanation: