Astarch has a molar mass of 3.20 x 104 g/mol. if 0.759 g of this starch is dissolved in 112 ml of solution, what is the osmotic pressure, in torr, at 25.00 oc?

The osmotic pressure is 3.94 torr.

Explanation:

Osmotic pressure is a colligative property of solution, which can be calculated according to the following expression:

π = M . R. T  [1]

where,

π is the osmotic pressure

M is the molarity of the solution

R is the ideal gas constant (62.36 L . torr/ K . mol)

T is the absolute temperature (in Kelvin scale)

Molarity can be calculated from its definition:

Absolute temperature can be calculated like:

K = °C + 273.15

K = 25.00 + 273.15 = 298.15 K

Replacing this data in equation 1:

chemistry sucks a**

explanation:

the answer is definitely c.