What is the osmotic pressure of a 0.0540 M aqueous sodium sulfate (Na₂SO₄,142 g/mol)solution at 25.0 $\circ$ C?

Question

Quizplus · Accepted Answer

First, we need to calculate the van't Hoff factor (i) of Na2SO4. The compound dissociates into 3 ions in water: Na+ and two SO42-. Therefore, i = 3.
Next, we use the van't Hoff equation: π = iMRT, where π is the osmotic pressure, M is the molarity, R is the gas constant, and T is the temperature in Kelvin.
Converting 25.0°C to Kelvin: 25.0°C + 273.15 = 298.15 K
Plugging in the values: π = 3 x (0.0540 mol/L) x (0.0821 L atm/mol K) x (298.15 K) = 3.96 atm
Therefore, the answer is C) 3.96 atm.

What Is the Osmotic Pressure of a 0 ∘\circ∘ C? A)1

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