Pure water and pure salt are poor conductors of electricity. When salt is dissolved in water, the resulting solution conducts electricity well. Which statement explains why this occurs with these substances?(1 point)

Question

The process of dissolving closely binds the ions in the solution. The process of dissolving closely binds the ions in the solution. The process of dissolving more closely binds the electrons in the solution. The process of dissolving more closely binds the electrons in the solution. The process of dissolving frees the electrons in the solution to move. The process of dissolving frees the electrons in the solution to move. The process of dissolving frees the atoms in the solution to move.

Answer 1

The correct statement is: The process of dissolving frees the atoms in the solution to move.

Here's why: When salt (sodium chloride) is dissolved in water, it dissociates into its individual ions (sodium ions and chloride ions). These ions are charged particles that are free to move throughout the solution. This movement of charged ions is what allows the solution to conduct electricity effectively. In pure water, there are very few ions available to carry an electric current, which is why it is a poor conductor. However, in a saltwater solution, the presence of these free-moving ions significantly increases the conductivity of the solution.