If you make a solution by dissolving 1.0 mol of FeCl3 into 1.0 kg of water, how would the osmotic pressure of this solution compare with the osmotic pressure of a solution that is made from 1.0 mol of glucose in 1.0 kg of water?

Osmotic pressure depends on the number of dissolved particles: at the same temperature and volume, π = iM, where i is the number of particles each solute unit produces. Glucose stays as one particle per molecule, while FeCl₃ dissociates into one Fe³⁺ ion and three Cl⁻ ions, making four particles. Thus, ideally, the FeCl₃ solution has four times the osmotic pressure of the glucose solution, so the answer is “four times as large.”

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