Freezing-Point Depression of Strong and Weak Electrolytes

Freezing-Point Depression of Strong and Weak Electrolytes [Pg.188]

In this experiment, the freezing-point depression of aqueous solutions is used to determine the degree of dissociation of a weak electrolyte and to study the deviation from ideal behavior that occurs with a strong electrolyte. [Pg.188]

Use will be made of the theory developed in Exp. 10 for the freezing-point depression A7 of a given solvent containing a known amount of an ideal solute this material should be reviewed. [Pg.188]

In the case of a dissociating (or associating) solute, the molality given by Eq. (10-11) or (10-20) is ideally the tofaf effective molality—the number of moles of all solute species present, whether ionic or molecular, per 1 kg of solvent. As we shall see, ionic solute species at moderate concentrations do not form ideal solutions and, therefore, do not obey these equations. However, for a weak electrolyte, the ionic concentration is often sufficiently low to permit treatment of the solution as ideal. [Pg.188]

Weak Electrolytes. As an example, let us discuss a weak acid HA with nominal molality m. Owing to the dissociation, [Pg.188]

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