What osmotic pressure in atmospheres would you expect for a solution of 0.100 M CaCl2 that is separated from pure water by a semipermeable membrane at 310 K? Assume 100% dissociation for CaCl2.

The osmotic pressure is 7.63 atm

Explanation:

We apply the osmotic pressure formula to solve this problem:

π = M . R . T . i

CaCl₂ → Ca²⁺ + 2Cl⁻  (i = 3)

The i refers to the Van't Hoff factor which refers to the amount of ions dissolved.

T is the Absolute T°, for this case 310K

R is the universal constant gase → 0.082 L.atm/mol.K

M is the molarity → 0.1 mol/L

We replace the values → π = 0.1 mol/L . 0.082 L.atm/mol.K . 310K . 3

π = 7.63 atm

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