Understanding Electrical Conductivity in Solutions

Electrical conductivity in aqueous solutions depends on the presence of mobile ions. Substances that dissociate or ionize in water to produce ions can conduct electricity. Conversely, substances that remain as neutral molecules in solution do not conduct electricity.

Analyzing Solution Conductivity

• Acids (e.g., HCl) ionize in water to form ions (e.g., $H^+$ and $Cl^-$), making the solution conductive.
• Bases (e.g., NaOH) ionize in water to form ions (e.g., $Na^+$ and $OH^-$), making the solution conductive.
• Alcohol (e.g., Ethanol, $C_2H_5OH$) and Glucose ($C_6H_{12}O_6$) are molecular compounds. They dissolve in water but do not ionize; they exist as neutral molecules. Therefore, their solutions do not conduct electricity.

Evaluating the Options

• Option 1 (Alcohol and acid): Conducts electricity due to the acid.
• Option 2 (Glucose and base): Conducts electricity due to the base.
• Option 3 (Acid and base): Conducts electricity due to both acid and base.
• Option 4 (Alcohol and glucose): Does NOT conduct electricity because both alcohol and glucose remain as neutral molecules in solution.