Chapter 14, Problem 116FP

Interpretation Introduction

(a)

Interpretation:

Have to show that two definitions are in Reasonably close agreement.

Concept introduction:

Molality can be calculated by given data.

$$

$\text{Molality = }\frac{\text{Amount of the solute (moles)}}{\text{Mass of the solvent}\left(\text{kilograms}\right)}$

Using the calculated molality value, can find the freezing point depression.

$\begin{array}{l}\Delta {\text{T}}_f={\text{-iK}}_f\text{m}\\ \Delta {\text{T}}_f\text{ = Freezing point depressinon }\\ \text{i = Van't Hoff factor}\\ {\text{K}}_f=\text{ Freezing point depression constant}\\ \text{m = molality of the solution }\end{array}$

$\text{Density = }\frac{\text{Mass}}{\text{Volume }}$

Interpretation Introduction

(b)

Interpretation:

Show that the ORT solution meets the requirement being isotonic.

Concept introduction:

Molality can be calculated by given data.

$$

$\text{Molality = }\frac{\text{Amount of the solute (moles)}}{\text{Mass of the solvent}\left(\text{kilograms}\right)}$

Using the calculated molality value, can find the freezing point depression.

$\begin{array}{l}\Delta {\text{T}}_f={\text{-iK}}_f\text{m}\\ \Delta {\text{T}}_f\text{ = Freezing point depressinon }\\ \text{i = Van't Hoff factor}\\ {\text{K}}_f=\text{ Freezing point depression constant}\\ \text{m = molality of the solution }\end{array}$

$\text{Van't Hoff factor}$ i, is a property of the solute,

Strong electrolytes fully separate into ions in the solution.

When a solute is nonelectrolyte, it does not separate to ions in a solution. Therefore, for nonelectrolyte compounds i = 1