Ace the ACS Chemistry Challenge 2026 – Ignite Your Inner Scientist!

For a solution to conduct electricity, it is essential that it contains dissolved ions. This is because electrical conductivity in a solution arises from the movement of charged particles. When ionic compounds dissolve in water, they dissociate into their constituent ions, which are free to move throughout the solution. These free-moving ions can carry electric charge, enabling the solution to conduct electricity effectively.

Other conditions mentioned do not facilitate electrical conductivity. For instance, a solution containing only dissolved gases does not have the necessary charged particles to conduct electricity. Similarly, while heating a solution may increase the kinetic energy of the molecules, it does not inherently guarantee the presence of charged particles necessary for conduction. Lastly, a pure solvent without any solute ions will not conduct electricity, as there are no charged species available to facilitate the flow of electrical current. Thus, the presence of dissolved ions plays a crucial role in electrical conductivity in solutions.