Teaching Students About the Acidic and Basic Properties of Aniline


Understanding the chemical nature of compounds is an essential aspect of chemistry education. One intriguing compound that often sparks curiosity in students is aniline (C6H5NH2), a derivative of ammonia where one hydrogen atom is replaced by a phenyl group. This article aims to explore the acidic and basic properties of aniline and provide educators with insights on how to teach their students about this fascinating compound.

Aniline’s Acid-Base Properties

The first step in determining whether aniline is an acid or a base involves examining its molecular structure. Aniline has a  nitrogen atom with a lone pair of electrons, which allows it to act as a Lewis base by donating electron pairs. Conversely, it lacks any functional group capable of donating protons, making it incapable of behaving as an acid in the Brønsted-Lowry sense.

However, aniline’s true nature is revealed when we consider its behavior in different environments:

1. In acidic solutions: In the presence of strong acids like hydrochloric acid (HCl), aniline accepts a proton and forms anilinium ion (C6H5NH3+). This behavior qualifies it as a Brønsted-Lowry base, albeit a weak one due to the electron-withdrawing nature of the benzene ring.

2. In basic solutions: When mixed with strong bases like sodium hydroxide (NaOH), aniline does not exhibit any significant reaction due to its weakness as a base.

Teaching Strategies for Aniline

The following approaches can be employed while teaching students about the acid-base properties of aniline:

1. Introduce foundational concepts: Start by reviewing the concepts of acids, bases, and their properties using Brønsted-Lowry and Lewis theories. Explain how these theories allow us to categorize different compounds based on their proton-donating or accepting abilities.

2. Perform experiments: Allow students to gain a hands-on understanding of aniline by conducting safe, supervised experiments with dilute solutions of the compound. Observe how it interacts with various acidic and basic solutions, concluding that aniline acts as a weak base.

3. Teach resonance structures: To help students visualize aniline’s electronic configuration, illustrate the concept of resonance structures. By drawing out the delocalization of electrons across the molecule, students can better understand why aniline is a weak base.

4. Discuss practical applications: Highlighting aniline’s real-world uses will pique students’ interest in learning more about this compound. For instance, the synthesis of dyes, catalysts, and polymers often involve the use of aniline, emphasizing its importance in industrial chemistry.


Teaching students about aniline takes them on a journey to explore advanced chemical theories and apply them in practical settings. By introducing foundational concepts, engaging students in hands-on experiments, and discussing real-world applications, educators can effectively address whether aniline acts as an acid or a base while fostering their students’ interest in chemistry.

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