The following species react in aqueous solution. Predict the...

The following species react in aqueous solution. Predict the products, identify the acids and bases (and their conjugate species), and show the proton transfer in the acidbase reactions. (a) $\mathrm{NH}_{3}$ and $\mathrm{CH}_{3} \mathrm{COOH}$ (b) $\mathrm{N}_{2} \mathrm{H}_{5}^{+}$ and $\mathrm{CO}_{3}^{2-}$ (c) $\mathrm{H}_{3} \mathrm{O}^{+}$ and $\mathrm{OH}^{-}$ (d) $\mathrm{HSO}_{4}^{-}$ and $\mathrm{HCOO}^{-}$

The following species react in aqueous solution. Predict the products, identify the acids and bases (and their conjugate species), and show the proton transfer in the acidbase reactions.
(a) $\mathrm{NH}_{3}$ and $\mathrm{CH}_{3} \mathrm{COOH}$
(b) $\mathrm{N}_{2} \mathrm{H}_{5}^{+}$ and $\mathrm{CO}_{3}^{2-}$
(c) $\mathrm{H}_{3} \mathrm{O}^{+}$ and $\mathrm{OH}^{-}$
(d) $\mathrm{HSO}_{4}^{-}$ and $\mathrm{HCOO}^{-}$

Key Concepts

Proton Transfer

This concept refers to the movement of a proton (H? ion) from one chemical species to another during a reaction. In acid–base reactions, the acid donates a proton while the base accepts it, resulting in the transformation of the original species into its conjugate base or conjugate acid, respectively.

Bronsted-Lowry Acid–Base Theory

This theory defines acids as proton donors and bases as proton acceptors. It provides a framework for understanding a wide range of reactions in solution, emphasizing the importance of the transfer of protons in determining the behavior and reactivity of chemical species.

Conjugate Acid–Base Pairs

In any acid–base reaction, once the proton is transferred, the species that loses the proton becomes the conjugate base, while the species that gains the proton becomes the conjugate acid. These conjugate pairs are crucial for understanding reaction equilibria and the reversibility of acid–base reactions.

Aqueous Acid–Base Reactions

Acid–base reactions in aqueous solutions are governed by the interactions between dissolved ions and molecules, including water, which can both donate and accept protons. This environment allows for the formation of various conjugate pairs and the establishment of equilibrium, making it essential to predict reaction products and identify the species acting as acids or bases.