Question

Assuming ideal solution behavior, what is the osmotic pressure of an aqueous solution of 1.64 g of Ca(NO3)2 in water at 25 °C? The volume of the solution is 275 mL.

a) 0.546 atm
b) 1.56 atm
c) 3.12 atm
d) 0.312 atm

Answer 1

To calculate the osmotic pressure of an aqueous solution, use the formula II = MRT, where II is the osmotic pressure, M is the molarity of the solute, R is the ideal gas constant, and T is the temperature in Kelvin. In this case, the osmotic pressure of the solution is approximately 0.864 atm.

The correct answer is none of all.

Step-by-step explanation:

To calculate the osmotic pressure of an aqueous solution, we need to use the formula II = MRT, where II is the osmotic pressure, M is the molarity of the solute, R is the ideal gas constant (0.0821 L.atm/mol.K), and T is the temperature in Kelvin.

First, we need to determine the molarity of the Ca(NO3)2 solution. To do this, we need to convert the mass of Ca(NO3)2 to moles and then divide by the volume of the solution in liters. The molar mass of Ca(NO3)2 is 164.1 g/mol.

Moles of Ca(NO3)2 = 1.64 g / 164.1 g/mol = 0.01 mol

Molarity of Ca(NO3)2 = 0.01 mol / 0.275 L = 0.0364 M

Plugging the values into the formula, we get:

II = (0.0364 M) * (0.0821 (L.atm)/(K.mol)) * (298 K) = 0.864 atm

Therefore, the osmotic pressure of the solution is approximately 0.864 atm.