Final answer:
The osmotic pressure of a 0.100 moles NaCl solution in 14.0 liters of water at 17.0 °C can be calculated using the formula II = MRT. Since NaCl dissociates into two ions, you would use the doubled concentration in the calculation and then convert from atm to kPa for the final answer.
Step-by-step explanation:
The question asks about calculating the osmotic pressure of a solution containing sodium chloride (NaCl) at a given temperature. To find the osmotic pressure (II), we can use the formula II = MRT, where M is the molarity of the solution, R is the ideal gas constant, and T is the temperature in Kelvin. Since NaCl dissociates into two particles (Na+ and Cl-), for every mole of NaCl, we count 2 moles of particles. Therefore, a 0.100 moles NaCl solution in 14.0 liters would have a concentration of (0.100 moles/14.0 liters) * 2 = 0.0143 M. Plug this value into the equation with R = 0.0821 L·atm/K·mol and T = 290.15 K (17.0 °C + 273.15 to convert to Kelvin).
Using these values, the osmotic pressure would be calculated as follows:
II = (0.0143 mol/L) × [0.0821 (L·atm)/(K·mol)] × (290.15 K)
Careful unit conversion from atm to kPa is needed to provide the final answer in the requested units.