Answer: The osmotic pressure of the solution is 3.29 atm
Explanation:
To calculate the concentration of solute, we use the equation for osmotic pressure, which is:
[tex]\pi=iMRT[/tex]
or,
[tex]\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT[/tex]
where,
[tex]\pi[/tex] = osmotic pressure of the solution = ?
i = Van't hoff factor = 1 (for non-electrolytes)
Mass of sucrose = 12.8 grams
Molar mass of sucrose = 342.3 g/mol
Volume of solution = 278 mL
R = Gas constant = [tex]0.082\text{ L atm }mol^{-1}K^{-1}[/tex]
T = temperature of the solution = 298 K
Putting values in above equation, we get:
[tex]\pi=1\times \frac{12.8\times 1000}{342.3\times 278}\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 298K\\\\\pi=3.29atm[/tex]
Hence, the osmotic pressure of the solution is 3.29 atm
