Write equations to illustrate the acid-base reaction when...

Write equations to illustrate the acid-base reaction when each of the following pairs of Bronsted acids and bases are combined: Acid Base a. $\mathrm{HOCl} \quad \mathrm{H}_2 \mathrm{O}$ b. $\mathrm{HClO}_4 \quad \mathrm{NH}_3$ c. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_2^{-}$ d. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{OCl}^{-}$ e. $\mathrm{HC}_2 \mathrm{O}_4^{-} \quad \mathrm{H}_2 \mathrm{O}$

Write equations to illustrate the acid-base reaction when each of the following pairs of Bronsted acids and bases are combined:

Acid Base
a. $\mathrm{HOCl} \quad \mathrm{H}_2 \mathrm{O}$
b. $\mathrm{HClO}_4 \quad \mathrm{NH}_3$
c. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{NH}_2^{-}$
d. $\mathrm{H}_2 \mathrm{O} \quad \mathrm{OCl}^{-}$
e. $\mathrm{HC}_2 \mathrm{O}_4^{-} \quad \mathrm{H}_2 \mathrm{O}$

Key Concepts

Bronsted Acid-Base Theory

The Bronsted-Lowry acid-base theory defines acids as proton donors and bases as proton acceptors. This fundamental concept is used to understand the mechanism of many chemical reactions, where the transfer of a hydrogen ion (H?) from the acid to the base results in the formation of a conjugate pair.

Conjugate Acid-Base Pairs

In any acid-base reaction, the acid donates a proton and becomes its conjugate base while the base accepts a proton to become its conjugate acid. These pairs are interrelated, and the strength of an acid is inversely related to the strength of its conjugate base, which helps in predicting the direction of the reaction.

Acid-Base Reaction Equations

Writing acid-base reaction equations involves identifying the species that donate and accept protons, and then representing the proton transfer process. These equations typically indicate the reactants (acid and base) and the resulting conjugate base and conjugate acid, illustrating the fundamental proton transfer step that defines Bronsted acid-base reactions.

Amphiprotic Behavior

Some substances, most notably water, can act as both an acid and a base depending on the reaction context. This property, known as amphiprotism, is essential in balancing acid-base reactions and explains how water participates in a variety of mechanisms as either a proton donor or acceptor.

Transcript

Please give Ace some feedback