Question

The electrical conductance of two aqueous acidic solutions of the same concentration was measured. The first solution was observed to be a much better conductor than the second. Which statement is correct?

A. The first solution is a stronger acid than the second.

B. The first solution is a weaker electrolyte than the second.

C. The pH is the same for both solutions.

D. The second solution contains a solute that completely ionized when dissolved in water. I know A is the correct answer, but can you explain to me why, so I can answer questions related to this in the future?

Answer 1

Substances which allow electricity to pass through them are known as conductors. Those which undergo decomposition when current is passed through them is known as electrolytic conductors.

Electrolytes are divided into 2- strong & weak electrolytes. Strong electrolytes are sub: like strong acids - HCl dissociate completely in the aqueous solution & conduct electricity .Weak electrolytes like CH3COOH , weak acids have low degree of dissociation & conduct electricity to a small extent.

Strong electrolytes ionize more in a polar solvent. Greater is the polarity of the solvent , greater is the ionization & greater is the conduction. In a strong electrolyte, the dissociation increases on increasing the temperature & the conduction increases. In strong elecrolytes , the interionic attractions that is the interactions between the ions of the solute is higher than the weak electrolyte. So  

A. The 1st solution is a stronger acid than the second.