Weak Electrolyte Definition

Weak Electrolytes are those compounds which partially dissociates into positive and negative ions when dissolved in water.

• These Electrolytes are partially dissolved in water.
• In solution or molten form, these electrolytes are partially ionized.
• Even at higher concentration, interionic interactions are weak.
• Due to partial dissociation in aqueous solution, these electrolytes are bad conductor of electricity.
• Ostwald’s dilution law is applicable on weak electrolytes.

Examples of Weak Electrolytes

Some Categories of Weak Electrolytes are mentioned below :

Weak Acid

Weak Acid dissociates partially in water and are bad conductor of Electricity, so these are weak electrolytes. Some examples of weak acid are Hydrofluoric Acid (HF), Acetic Acid (CH₃COOH), Carbonic Acid (H₂CO₃).

Weak Base

Weak bases partially dissociates in water and are bad conductor of Electricity, so these are weak electrolytes. Some Example of Weak Bases are Aluminium Hydroxide (Al(OH)₃), Ammonia (NH₃) etc.

Characteristic of Weak Electrolytes

• At moderate concentrations, weak electrolytes do not dissociate completely.
• Characteristic of Strong Electrolyte depends on number of parameters such as size of the ion, concentration of ion etc.

Strong Electrolytes are compounds that completely dissociate into their ions when dissolved in water. Whereas Weak Electrolytes are compounds that partially dissociate into their ions when dissolved in water.

In this article, we will learn about, What is Electrolytes, Examples of Weak and Strong Electrolytes, and others in detail.