HCl and NaOH are both strong electrolytes. When they are dissolved in water, they completely dissociate into ions and conduct electricity effectively.
HCl, also known as hydrochloric acid, is a strong acid. It ionizes completely in water, breaking apart into hydrogen ions (H+) and chloride ions (Cl-). This dissociation is represented by the equation: HCl -> H+ + Cl-. The presence of these ions allows HCl to conduct electricity in solution.
NaOH, on the other hand, is a strong base. It also completely dissociates in water, producing sodium ions (Na+) and hydroxide ions (OH-). The dissociation of NaOH is represented by the equation: NaOH -> Na+ + OH-. The presence of these ions enables NaOH to conduct electricity in solution.
Both HCl and NaOH are highly soluble in water and undergo complete dissociation, resulting in the formation of a large number of ions. This high concentration of ions enhances the electrical conductivity of the solution.
To further illustrate the concept, let’s consider an example. Imagine you have two beakers, one containing a solution of HCl and the other containing a solution of NaOH. If you connect the two beakers with a conductive wire and insert a light bulb into the circuit, the bulb will light up in both cases. This demonstrates that both HCl and NaOH can effectively conduct electricity.
HCl and NaOH are both strong electrolytes as they completely dissociate into ions when dissolved in water. Their ability to conduct electricity is a result of the presence of these ions in solution.