Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.

Key Concepts

Brønsted–Lowry Acid-Base Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework emphasizes the transfer of protons (H+) in chemical reactions, allowing for a broader understanding of acid-base behavior beyond just the presence of hydroxide ions. This theory is essential for identifying conjugate acid-base pairs.

Conjugate Acid-Base Pairs

A conjugate base is formed when an acid donates a proton. In a conjugate acid-base pair, the acid and its conjugate base differ by one proton. Understanding this relationship is crucial for predicting the products of acid-base reactions and for identifying the conjugate base of a given acid.

Dissociation of Acids

The dissociation of acids involves the release of protons into solution, which is a key step in determining their conjugate bases. For example, when HIO3 dissociates, it loses a proton to form IO3-, while NH4+ dissociates to form NH3. Recognizing how acids dissociate helps in identifying their corresponding conjugate bases.