Explain the protonation (acid-base reaction) of NH3
The Correct Answer and Explanation is:
The protonation of ammonia (NH3) is an acid-base reaction where ammonia acts as a base and accepts a proton (H+) from an acid. In this reaction, ammonia reacts with a proton donor (such as HCl) to form ammonium ion (NH4+). The process can be represented as:NH3+H+→NH4+\text{NH}_3 + \text{H}^+ \rightarrow \text{NH}_4^+NH3+H+→NH4+
Ammonia has a lone pair of electrons on the nitrogen atom, which makes it a good Lewis base. When ammonia encounters a proton (H+), it donates its lone pair to form a new bond with the proton, resulting in the formation of the ammonium ion (NH4+). This protonation reaction increases the positive charge on the nitrogen atom, converting NH3 from a neutral molecule to a positively charged ion (NH4+).
In terms of acid-base theory, ammonia is a weak base. It can accept a proton from an acid, but not as readily as stronger bases like sodium hydroxide (NaOH). The reaction between NH3 and H+ is reversible, meaning that ammonium ion (NH4+) can lose a proton to revert to ammonia (NH3) under certain conditions, such as a decrease in the concentration of hydrogen ions.
The protonation of ammonia also plays a role in various chemical processes. In aqueous solutions, the concentration of H+ ions is often regulated through buffer systems, and ammonia’s ability to become protonated can help maintain the pH balance. For example, in a biological context, ammonium ions are crucial in the regulation of pH in cells and tissues.
Overall, the protonation of ammonia involves a simple yet important acid-base reaction that showcases ammonia’s ability to act as a weak base and accept a proton to form ammonium.
