at a temperature of 5 celsius, 21.5 mg of a non electrolyte is dissolved in enough water to make a 150.0 ml solution. the osmotic pressure of the solution is 0.200 atm. what is the molar mass of the substance dissolved

pi = MRT

Substitute and solve for M.

Then M = mols/L. You know M and L, solve for mols.

Then mols = grams/molar mass. You know mols and grams, solve for molar mass.

To find the molar mass of the substance dissolved, we can use the equation for osmotic pressure:

π = MRT

Where:
π = osmotic pressure
M = molarity of the solution (in moles per liter)
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin

First, we need to convert the temperature from Celsius to Kelvin:

T(K) = T(°C) + 273.15
T = 5°C + 273.15 = 278.15 K

Now, let's calculate the molarity of the solution:

Molarity (M) = moles of solute / liters of solution

We are given that 21.5 mg of the non-electrolyte is dissolved in enough water to make a 150.0 ml solution.

First, we need to convert the mass from milligrams to grams:

mass = 21.5 mg = 0.0215 g

Then, we can calculate the moles of the substance dissolved:

moles = mass / molar mass

Now, we can determine the molarity of the solution:

M = moles / liters of solution

Since the solution volume is given in milliliters, we need to convert it to liters:

liters of solution = 150.0 ml = 0.150 L

Finally, we can substitute the values into the osmotic pressure equation and solve for the molar mass (M):

π = MRT

Rearranging the equation:

M = π / (RT)

Substituting the known values:

M = 0.200 atm / (0.0821 L·atm/(mol·K) * 278.15 K)

Calculating this expression will give you the molar mass of the substance dissolved in grams per mole.