Calculate the osmotic pressure of a solution that contains 0.0010 mole of KCl and 0.0010 mole of BaCl₂ per liter of solution at 298 K.

Question

Quizplus · Accepted Answer

Osmotic pressure (π) can be calculated using the formula π = iMRT, where i is the van't Hoff factor (the number of particles the solute dissociates into), M is the molarity of the solution, R is the gas constant (0.0821 L·atm/K·mol), and T is the temperature in Kelvin. KCl dissociates into 2 particles (K+ and Cl-), and BaCl2 also dissociates into 3 particles (Ba2+ and 2 Cl-). Therefore, the total number of particles from KCl is 0.0010*2 = 0.0020 moles and from BaCl2 is 0.0010*3 = 0.0030 moles, giving a total of 0.0050 moles of particles per liter. Using the formula π = iMRT with i = 5 (since we have 5 moles of particles per liter), M = 0.0050 mol/L, R = 0.0821 L·atm/K·mol, and T = 298 K, we get π = 5 * 0.0050 * 0.0821 * 298 = 0.12 atm.

Calculate the Osmotic Pressure of a Solution That Contains 0