If carbonates are weak bases, why is Na2CO3 a strong electrolyte?
The correct answer and explanation is:
Sodium carbonate (Na2CO3) is considered a strong electrolyte because it completely dissociates into its ions when dissolved in water. Despite carbonate ions (CO3^2-) being weak bases, this property does not affect the electrolyte strength of sodium carbonate.
An electrolyte is a substance that conducts electricity when dissolved in water due to the presence of free-moving ions. In the case of Na2CO3, when it dissolves in water, it dissociates completely into two sodium ions (Na+) and one carbonate ion (CO3^2-). This complete dissociation of ions is a key characteristic of strong electrolytes, meaning they can conduct electricity effectively.
The carbonate ion (CO3^2-) is a weak base, which means it can react with water to produce a small amount of hydroxide ions (OH-) through hydrolysis. This reaction results in a slightly basic solution, but it does not affect the dissociation process of sodium carbonate itself. The carbonate’s weak basicity simply indicates its ability to accept protons and not that it impedes its dissociation.
Moreover, the strength of an electrolyte is determined by how completely it dissociates, not by the nature of the ions formed. Sodium carbonate dissociates fully in water, providing a high concentration of ions, which enables it to conduct electricity well. This is why Na2CO3 is classified as a strong electrolyte.
In summary, sodium carbonate is a strong electrolyte because it dissociates completely into ions in solution, allowing it to conduct electricity efficiently. The weak basic nature of carbonate ions does not interfere with this dissociation and does not affect its classification as a strong electrolyte.