The standard freezing point depression formula $$\Delta T_f = K_f \cdot m$$ assumes strictly that the solid separating out is pure solvent. What happens if the solute also enters the solid phase (forming a solid solution)?

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The standard freezing point depression formula  $$\Delta T_f = K_f \cdot m$$  assumes strictly that the solid separating out is pure solvent. What happens if the solute also enters the solid phase (forming a solid solution)?

Canvas Classes · Accepted Answer

The standard equation fails/is invalid.    If the solid phase is a mixture (solid solution), the chemical potential of the solvent in the solid phase is lower than that of pure solid solvent. The observed $$\Delta T_f $$ will be **less** than that calculated by $$  K_f \cdot m$$.

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