Ammonium Chloride

Definition

Ammonium chloride is a chemical compound with the formula NH4Cl. It is a colorless crystalline salt that is highly soluble in water and is commonly used in various industrial and household applications.

5 Must Know Facts For Your Next Test

1. Ammonium chloride is a salt that undergoes hydrolysis in water, resulting in the formation of an acidic solution.
2. The hydrolysis of ammonium chloride produces a solution with a pH less than 7, indicating an acidic environment.
3. The acidic nature of the ammonium chloride solution is due to the presence of the ammonium ion (NH4+), which acts as a weak acid.
4. The hydrolysis of ammonium chloride is an example of a salt hydrolysis reaction, where the cation (NH4+) and the anion (Cl-) interact with water to produce an acidic solution.
5. The strength of the acid or base formed during the hydrolysis of a salt depends on the relative strengths of the conjugate acid-base pairs involved.

Review Questions

• Explain the process of hydrolysis as it relates to ammonium chloride and the formation of an acidic solution.
  • When ammonium chloride (NH4Cl) is dissolved in water, it undergoes hydrolysis, a chemical reaction in which the salt interacts with water. In this case, the ammonium ion (NH4+) acts as a weak acid, accepting a proton (H+) from water, forming an acidic solution with a pH less than 7. The hydrolysis reaction can be represented as: NH4+ + H2O ⇌ NH3 + H3O+. This process results in the formation of a solution that is acidic due to the presence of the hydronium ion (H3O+), which is the conjugate acid of water.
• Describe the relationship between the strength of the acid or base formed during the hydrolysis of a salt and the relative strengths of the conjugate acid-base pairs involved.
  • The strength of the acid or base formed during the hydrolysis of a salt is directly related to the relative strengths of the conjugate acid-base pairs involved. In the case of ammonium chloride, the ammonium ion (NH4+) is a weak acid, and its conjugate base, ammonia (NH3), is a weak base. The strength of the acid or base formed during the hydrolysis depends on the equilibrium between these conjugate acid-base pairs. If the conjugate acid is stronger than the conjugate base, the solution will be acidic, as is the case with ammonium chloride. Conversely, if the conjugate base is stronger than the conjugate acid, the solution will be basic. Understanding this relationship is crucial in predicting the pH of the solution formed during the hydrolysis of a salt.
• Evaluate the role of ammonium chloride in the context of 14.4 Hydrolysis of Salts and explain how its hydrolysis behavior contributes to the understanding of this topic.
  • Ammonium chloride is an important example in the context of 14.4 Hydrolysis of Salts because it demonstrates the principles of how the hydrolysis of a salt can lead to the formation of an acidic or basic solution. The hydrolysis of ammonium chloride, where the ammonium ion (NH4+) acts as a weak acid, produces an acidic solution. This illustrates how the relative strengths of the conjugate acid-base pairs involved in the hydrolysis reaction determine the pH of the resulting solution. By understanding the hydrolysis behavior of ammonium chloride, students can gain insights into the broader topic of salt hydrolysis, including how to predict the acidity or basicity of solutions formed by the hydrolysis of various salts. This knowledge is crucial in comprehending the factors that influence the pH of solutions and the underlying principles of acid-base chemistry.

Related terms

Ammonium Ion: The ammonium ion (NH4+) is a positively charged ion formed when ammonia (NH3) dissolves in water and accepts a proton (H+).

Hydrolysis: Hydrolysis is a chemical reaction in which a molecule is cleaved into two or more parts by the addition of water.

Acid-Base Reactions: Acid-base reactions involve the transfer of protons (H+) between an acid and a base, resulting in the formation of a salt and water.