Electrical Conductivity Test

Electrolytes

Substances that produce ions when dissolved in water, which can conduct electricity.

Misconception about Electrolytes

Electrolytes do not generate electricity; they facilitate electricity flow through ions.

Strong Electrolyte

A substance, like sodium chloride (NaCl), that completely dissociates into ions in solution.

Sodium Chloride (NaCl)

A strong electrolyte that dissociates into sodium ions (Na⁺) and chloride ions (Cl⁻) when dissolved in water.

Non-Electrolyte

Substances, like sucrose, that do not dissociate into ions in solution and cannot conduct electricity.

Sucrose

A non-electrolyte that dissolves in water but does not produce ions, so it cannot conduct electricity.

Weak Electrolyte

A substance, like acetic acid (HC₂H₃O₂), that partially dissociates into ions in solution.

Acetic Acid (HC₂H₃O₂)

A weak electrolyte that partially dissociates into hydrogen ions (H⁺) and acetate ions (C₂H₃O₂⁻) in water.

Conductivity of Strong Electrolytes

Exhibit high conductivity due to complete dissociation into a large number of ions.

Conductivity of Weak Electrolytes

Show lower conductivity due to partial dissociation and fewer ions.

Conductivity of Non-Electrolytes

Display no conductivity as they do not dissociate into ions at all.

Demonstration Setup

Uses a light bulb tester connected to electrodes submerged in a solution to test conductivity.

Safety Precautions

Advisable when handling substances like acetic acid to prevent accidents.

Electricity Source in Demonstration

Comes from an external power supply, not from the electrolyte solution itself.

Dissociation

The process of a compound breaking down into ions in solution.