Ammonium hydroxide is a weak alkali.

(A) True

(B) False

The statement "Ammonium hydroxide is a weak alkali" is (A) True. Ammonium hydroxide, often represented as NH4OH, is indeed classified as a weak base. Let's delve into why this is the case and what it means in a broader context.

Understanding Ammonium Hydroxide

Ammonium hydroxide is formed when ammonia (NH3) dissolves in water. While ammonia itself is a gas, when it interacts with water, it establishes an equilibrium that produces ammonium ions (NH4+) and hydroxide ions (OH-). This reaction can be represented as follows:

• NH3(g) + H2O(l) ⇌ NH4+(aq) + OH-(aq)

Weak vs. Strong Bases

To classify a base as weak or strong, we look at its ability to dissociate in water. Strong bases, like sodium hydroxide (NaOH), completely dissociate into their ions, resulting in a high concentration of hydroxide ions. In contrast, weak bases only partially dissociate. This partial dissociation is what characterizes ammonium hydroxide as a weak alkali.

Implications of Being a Weak Alkali

The fact that ammonium hydroxide is a weak alkali has several implications:

• pH Level: Solutions of ammonium hydroxide typically have a pH that is higher than 7 but not as high as that of strong bases. This means they are basic but not extremely so.
• Reactivity: Weak bases like ammonium hydroxide can react with acids to form salts and water, but they do so less vigorously than strong bases.
• Applications: Ammonium hydroxide is commonly used in cleaning products and as a fertilizer, where its mild basicity is beneficial.

Real-World Examples

In practical terms, when you use a cleaning product containing ammonium hydroxide, you're leveraging its ability to neutralize acids and break down organic materials without the harshness of stronger alkalis. This makes it safer for various surfaces and materials.

Conclusion

In summary, ammonium hydroxide is indeed a weak alkali due to its partial dissociation in water, which results in a moderate concentration of hydroxide ions. This property influences its behavior in chemical reactions and its applications in everyday products.