Indique la base conjugada de los ácidos de BronstedLowry...

Indique la base conjugada de los ácidos de BronstedLowry siguientes: (a) $\mathrm{H}_2 \mathrm{SO}_3$; (b) $\mathrm{HC}_2 \mathrm{H}_3 \mathrm{O}_2$ ' (c) $\mathrm{H}_2 \mathrm{AsO}_4{ }^{-}$; (d) $\mathrm{NH}_4^{+}$.

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Key Concepts

Bronsted-Lowry Acid-Base Theory

The Bronsted-Lowry model defines acids as proton donors and bases as proton acceptors. This theory is fundamental in understanding acid-base reactions, where the transfer of a proton from an acid to a base occurs, forming species that are connected through this proton exchange process.

Conjugate Acid-Base Pair

A conjugate acid-base pair consists of two species that differ by a proton. When an acid donates a proton, the species left behind is its conjugate base. Conversely, when a base accepts a proton, the resulting species is its conjugate acid. Studying these pairs helps in understanding the reversible nature of acid-base reactions and their equilibria.

Deprotonation

Deprotonation is the process by which an acid loses a proton. This event transforms the acid into its conjugate base. The ease and extent of deprotonation depend on the acid’s strength and the molecular environment, which are critical factors in predicting reaction behavior in acid-base chemistry.

Polyprotic Acids

Polyprotic acids contain more than one ionizable hydrogen. Each ionizable proton is lost in a stepwise fashion, forming a series of conjugate bases. This concept is important in systems where multiple equilibria coexist, as the removal of each proton alters the acid’s properties and the equilibrium conditions of the reaction.

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