Chapter 6, Problem 6.86P

Interpretation Introduction

Interpretation:

The stability of ${\text{NH}}_{\text{4}}{}^{\text{+}}$ ion in the given solvent is to be explained. The ability of the solvent to solvate cation and anion is to be explained.

Concept introduction:

A protic solvent can solvate both cation and anion, but an aprotic solvent can solvate only cation and not anions. The protic solvent is a compound containing at least one hydrogen atom bonded to an electronegative atom of oxygen, nitrogen, or fluorine and capable of forming a hydrogen bond. The aprotic solvent is a compound which cannot form a hydrogen bond due to the lack of hydrogen atom bonded to an electronegative atom of oxygen, nitrogen, or fluorine. The polar solvent molecule has a partial negative and partial positive charge. The negative ends of the solvent’s dipole solvate the cation strongly, and the positive end of the solvent’s dipole solvate the anion strongly. When two positively charged species are present in the solution, the stronger acid is the one that is less stable.