Chapter 2, Problem 2.57P

Interpretation Introduction

Interpretation:

It is to be explained whether $\text{NaCl}$ will be more or less soluble in acetone ${{\text{(CH}}_{\text{3}}\text{)}}_{\text{2}}\text{C = O}$ than in $\text{di-tert-butyl ketone}$${{\text{[(CH}}_{\text{3}}{\text{)}}_{\text{3}}\text{C]}}_{\text{2}}\text{C = O}$.

Concept introduction:

Ionic compounds dissolve in polar solvents. Larger the dipole moment of the polar solvent, better the ions solvated and greater the solubility of the ionic compound.

When an ionic compound dissolves in a polar solvent, the free ions can interact with the solvent molecule through ion-dipole interactions. In such ion-dipole interactions, the positive end of the solvent dipole attracts anions and the negative end attracts cations. Each ion participates in multiple ion-dipole interactions with the solvent, and ions get solvated. The stability of these ion-dipole interactions is greater than that of ion-ion interactions in ionic compounds, which makes the mixture more stable.