Final answer:
The osmotic pressure of a 0.1M NaCl solution at 25°C, assuming 100% ionization of the solute, is 4.94 atm.
Step-by-step explanation:
The osmotic pressure of a solution can be calculated using the formula π = iCRT, where π is the osmotic pressure, i is the van't Hoff factor (the number of particles into which a compound dissociates in solution), C is the concentration of the solute in moles per liter (M), R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
In the case of 0.1M NaCl, since it fully ionizes in solution, the van't Hoff factor i would be equal to 2, as 1 mole of NaCl produces 2 moles of ions. Plugging the values into the formula, we can calculate the osmotic pressure:
π = (2)(0.1 M)(0.0821 L·atm/mol·K)(298 K) = 4.94 atm.