A 271-mL of a sugar solution containing 1.79g of the sugar has an osmotic pressure of 30.1 mmHg at 35.1 degrees C. What is the molar maas of the sugar?

pi = MRT

Solve for M
Then M = mols/L of solution.
You have M and L, solve for moles.

Then moles = grams/molar mass
solve for molar mass

168

To find the molar mass of the sugar, we can use the formula for osmotic pressure and rearrange it to solve for the molar mass.

The formula for osmotic pressure (π) is given by:

π = nRT/V

where π is the osmotic pressure, n is the number of moles of solute, R is the ideal gas constant (0.0821 L·atm/(mol·K)), T is the temperature in Kelvin, and V is the volume of the solution in liters.

First, let's convert the given temperature from Celsius to Kelvin:

T = 35.1 + 273.15
T = 308.25 K

Next, let's convert the volume from milliliters to liters:

V = 271 mL / 1000
V = 0.271 L

Now, we can rearrange the formula to solve for the number of moles of solute (n):

n = πV / RT

Substituting the given values:

n = (30.1 mmHg)(0.271 L) / (0.0821 L·atm/(mol·K))(308.25 K)

n = 0.822 mol

Finally, to find the molar mass of the sugar, we divide the mass of the solute (1.79 g) by the number of moles (0.822 mol):

Molar mass = 1.79 g / 0.822 mol

Molar mass = 2.18 g/mol

Therefore, the molar mass of the sugar is approximately 2.18 g/mol.