Chapter 8.3, Problem 8.6E

Interpretation Introduction

Interpretation:The direction of equilibrium that is favoredshould be identified.

  ${\left({\text{CH}}_{\text{3}}\right)}_3{\text{CO}}^{-}+{\text{CH}}_{\text{3}}\text{OH}\rightleftharpoons {\left({\text{CH}}_{\text{3}}\right)}_3\text{COH}+{\text{CH}}_{\text{3}}{\text{O}}^{-}$

Concept introduction:In accordance with Bronsted definition an acid can act as a proton donor and a base can act as a proton acceptor. Thus in a typical acid-base reaction, the fundamental principle is a lone pair of base reaches out for an acidic proton. Similar curved arrows are used to show the movement of electrons. After deprotonation, the species left with a negative charge is referred as the conjugate base of acid while the other with a positive charge is termed conjugate acid of given base. For example,

  

The strength of various conjugate acid-base pairs varies inversely to one another; the strong acid has a weak conjugate base and the strong base has weak conjugate acid and vice-versa.