Answer:
298K
Step-by-step explanation:
The osmotic pressure (π) of a solution is given by the van 't Hoff equation:
π = iMRT
Where M is the molarity of the solute, i is the van 't Hoff factor (the number of ions or particles the solute dissociates into in solution), R is the gas constant, and T is the temperature in Kelvin.
For a weak electrolyte with a degree of dissociation (α) of 95%, the effective concentration of the solute is:
C_eff = C_total * α
where C_total is the initial concentration of the solution.
Since the concentration of the solution is 0.1 M, the effective concentration of the solute is:
C_eff = 0.1 M * 0.95 = 0.095 M
The van 't Hoff factor for a weak electrolyte is given by:
i = 1 + α
Substituting the value of α into the equation, we get:
i = 1 + 0.95 = 1.95
Substituting the values of i, M, R, and T into the van 't Hoff equation, we get:
π = (1.95)(0.095 M)(0.08206 L·atm/(mol·K))(298 K) = 4.02 atm
Therefore, the osmotic pressure of the solution is 4.02 atm at 298K