Because ion pairing occurs so often for these, the van't Hoff factor is useful in calculating their effects for electrolytic solutions.
Because ion pairing occurs so often for these, the van't Hoff factor is useful in calculating their effects for electrolytic solutions. The change that they bring about is proportional to the molality of the solute and a simple constant, and examples of them include osmotic pressure, boiling-point elevation, and freezing-point depression. For ten points, name these properties defined as depending only on the number and not the identity of particles in an ideal solution.
Because ion pairing occurs so often for these, the van't Hoff factor is useful in calculating their effects for electrolytic solutions.
{colligative} properties