is the osmotic pressure formed by dissolving 50.9 mg of aspirin (C9H8O4) in 0.450 L of water at 24°C

To determine the osmotic pressure formed by dissolving aspirin in water, we can use the following equation:

π = i * M * R * T

Where:
π is the osmotic pressure,
i is the van't Hoff factor (the number of particles into which the solute dissociates),
M is the molarity of the solution,
R is the ideal gas constant (0.0821 L·atm/(mol·K)),
T is the temperature in Kelvin.

First, let's calculate the molarity of the solution:
Molarity (M) = moles of solute / volume of solution (in liters)

To determine the moles of aspirin (C9H8O4), we need to know its molar mass. The molar mass of C9H8O4 is calculated as follows:

(9 * atomic mass of carbon) + (8 * atomic mass of hydrogen) + (4 * atomic mass of oxygen)
= (9 * 12.01 g/mol) + (8 * 1.008 g/mol) + (4 * 16.00 g/mol)
= 180.16 g/mol

Now we can calculate the moles of aspirin:
moles = mass / molar mass
moles = 50.9 mg / 180.16 g/mol

Next, we need to convert the volume from liters to Kelvin:
T = (24°C + 273.15) K

Now we can substitute the values into the osmotic pressure equation:

π = i * (moles / volume) * R * T

Since aspirin does not ionize or dissociate in water, the van't Hoff factor (i) is equal to 1.

Finally, let's plug in the values and calculate the osmotic pressure (π).