Predict the products of the following acid–base reactions.
(e) H₂O + NH₃ ⇌

Verified step by step guidance

1. Identify the acid and base in the reaction. In this case, water (H2O) can act as an acid, donating a proton (H⁺), and ammonia (NH3) can act as a base, accepting a proton.
2. Write the chemical equation for the proton transfer. Water donates a proton to ammonia, forming hydroxide ion (OH⁻) and ammonium ion (NH4⁺).
3. Use MathML to represent the chemical equation: ${H2O}_{}+{NH3}_{}\rightleftharpoons {OH-}_{}+{NH4+}_{}$
4. Consider the equilibrium of the reaction. The double arrow (⇌) indicates that the reaction can proceed in both directions, meaning the products can revert to reactants.
5. Understand the concept of conjugate acid-base pairs. In this reaction, NH3 and NH4⁺ are a conjugate acid-base pair, and H2O and OH⁻ are another conjugate acid-base pair.

Key Concepts

Acid-Base Reaction

An acid-base reaction involves the transfer of a proton (H+) from an acid to a base. In the given reaction, water (H2O) acts as an acid, donating a proton to ammonia (NH3), which acts as a base. Understanding the roles of acids and bases is crucial for predicting the products of such reactions.

Bronsted-Lowry Acid and Base

The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. In the reaction H2O + NH3, H2O donates a proton to NH3, forming OH- and NH4+. This concept helps in identifying the conjugate acid-base pairs and predicting the products formed in the reaction.

Conjugate Acid-Base Pair

A conjugate acid-base pair consists of two species that differ by a proton. In the reaction, H2O and OH- form a conjugate acid-base pair, while NH3 and NH4+ form another. Recognizing these pairs is essential for understanding the equilibrium and direction of acid-base reactions.