Which factor primarily influences the conductivity of an aqueous solution?

The conductivity of an aqueous solution is primarily influenced by the concentration of ions present in the solution. When a solute dissolves in water, it can dissociate into ions. These ions are charged particles that are essential for conducting electricity. The greater the concentration of ions in the solution, the higher the number of charge carriers available to facilitate the flow of electric current, which directly increases the conductivity.

In contrast, while temperature can affect the movement of ions and their ability to conduct electricity, it primarily modifies the rate of ion mobility rather than the intrinsic conductivity associated with the ion concentration itself. Non-ionic solutes do not dissociate into ions and therefore do not contribute to conductivity; their presence may not change the conductivity significantly. The pressure applied to the solution rarely has a significant effect on conductivity because conductivity is more directly related to the number of ions in solution than to the physical pressure applied. Thus, the concentration of ions is the most critical factor affecting the conductivity of an aqueous solution.