Chapter 12, Problem 12.116QP

Interpretation Introduction

Interpretation:

Given the freezing point of the solution of ionic solid in water, the possible molecular formula of the ionic compound that cause the given depression in freezing point when mass of the compound is tripled has to be determined from one of the following - $MX,{\text{ MX}}_2$ or ${\text{MX}}_3$ where M is metal cation and X is an anion with charge $-1.$

Concept Introduction:

Freezing point of a liquid substance is defined as the temperature at which the liquid becomes and solid and both the phases remain in equilibrium.

Depression in freezing point of a solvent due to the addition of non-volatile solute can be determined by the formula,

$\Delta T_f\text{ = i}\times {\text{K}}_f\times \text{m}$.

Where,

$\begin{array}{l}\Delta T_f\text{ = depression in freezing point}\\ {\text{K}}_f\text{ = depression in freezing point constant}\\ \text{m = molality of the solution; i = Van't Hoff factor}\end{array}$