Electricity in Solutions: What Makes Them Conductive?

What condition is necessary for a solution to conduct electricity?

• A. It must contain dissolved gases
• B. It must contain dissolved ions
• C. It must be heated to a high temperature
• D. It must be a pure solvent

Answer: (B)

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.

When we think about electricity, our minds often jump to batteries, light bulbs, or even the sprawling electrical grids that light up our cities. But have you ever stopped to consider what actually allows certain solutions to conduct electricity? It's not just about having a solid circuit; a little chemistry is at play here!

You know what? To make a solution conductive, it’s as simple as having dissolved ions. That’s right! A solution must contain these charged particles to be able to carry an electric current. This is because electrical conductivity hinges on the mobility of these ions. When ionic compounds break down in water – think table salt (sodium chloride) dissolving – they dissociate into positive and negative ions. These free-moving ions can carry electric charge throughout the solution, making electrical conduction possible.

Let’s consider our other options: What about dissolved gases? While some might think that having oxygen or carbon dioxide dissolved in water could help, that’s not accurate. Dissolved gases don’t provide the necessary charged particles for conductivity the way ions do. And then there's the idea of heating a solution to a high temperature. Sure, heating can increase the kinetic energy of the molecules in the solution, but without those essential ions present, you won't get that conductivity we’re after.

Now, how about pure solvents? Whether it's pristine distilled water or other singular solvent types, without any solute – namely, those essential dissolved ions – you’ve just got a liquid that won’t conduct electricity. No charged species mean no electrical current, plain and simple.

In summary, for a solution to effectively conduct electricity, look for dissolved ions. They’re the real players in this scenario, as they allow the electric charges to flow freely through the liquid. So, the next time you’re mixing solutions or pondering over the mysteries of electrical conductivity, remember: it's all about those ions on the move!