(a) Give the conjugate base of the following BrønstedLowry...

(a) Give the conjugate base of the following BrønstedLowry acids:
(i) $\mathrm{H}_{2} \mathrm{SO}_{3},$ (ii) $\mathrm{HSO}_{3}^{-}$ (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) $\mathrm{CH}_{3} \mathrm{NH}_{2}$,
(ii) $\mathrm{CH}_{3} \mathrm{COO}^{-}$.

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Key Concepts

Brønsted-Lowry Acid-Base Theory

This theory defines acids as proton donors and bases as proton acceptors. It emphasizes the role of proton transfer in acid-base reactions, which helps in predicting the direction of the reaction and determining the properties of the species involved.

Conjugate Acid-Base Pairs

A conjugate acid-base pair consists of two species that transform into each other by the gain or loss of a proton. When an acid donates a proton, it forms its conjugate base, and when a base accepts a proton, it forms its conjugate acid, linking the chemical behavior of the species in equilibrium.

Proton Transfer Mechanism

This concept involves the transfer of a proton (H+) from one molecule to another during a chemical reaction. It is a central process in acid-base chemistry and explains how acids and bases interact to yield their conjugate counterparts.

Amphiprotic Species

Some species can act both as a proton donor and a proton acceptor, depending on the chemical environment. These amphiprotic substances, such as certain anions, illustrate the flexible nature of acid-base chemistry under the Brønsted-Lowry framework.

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