Chapter 8, Problem 8.76E

Interpretation Introduction

Interpretation:

The reason as to why higher-charged ionic compounds demonstrate a greater deviation from the ideal Debye-Hückel limiting law is to be explained.

Concept introduction:

The Debye-Hückel limiting law gives a linear relationship between the natural logarithm activity coefficient of ions and ionic strength of a dilute solution. The Debye-Hückel limiting law is represented as,

$\ln {\gamma }_{\pm }=A\cdot z_{+}\cdot z_{-}\cdot I^{1/2}$

Where,

• $\gamma$ represents the activity coefficient of the ion.

• $A$ represents a constant.

• $z_{+}$ represents the charge on the positive ion.

• $z_{-}$ represents the charge on the negative ion.

• $I$ represents the ionic strength.