What is the osmotic pressure of a 0.0540 M aqueous sodium sulfate (Na₂SO₄, 142.04 g/mol) solution at 25.0 $\degree$C?

Question

Quizplus · Accepted Answer

Osmotic pressure (π) can be calculated using the formula π = iMRT, where i is the van't Hoff factor (number of particles the solute dissociates into), M is the molarity, R is the gas constant (0.0821 L·atm/K·mol), and T is the temperature in Kelvin. Sodium sulfate (Na2SO4) dissociates into 3 ions (2 Na+ and 1 SO4^2-), so i = 3. The temperature in Kelvin is 25.0°C + 273.15 = 298.15 K. Therefore, π = 3 * 0.0540 mol/L * 0.0821 L·atm/K·mol * 298.15 K = 3.96 atm.

What Is the Osmotic Pressure of a 0 °\degree° C? A)1

What Is the Osmotic Pressure of a 0 $\degree$ C?
A)1