<u>Answer:</u> The osmotic pressure of aspirin is 0.0190 atm
<u>Explanation:</u>
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 = ![25^oC=[273+25]=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B273%2B25%5D%3D298K)
Putting values in above equation, we get:

Hence, the osmotic pressure of aspirin is 0.0190 atm