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

Responses

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 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 atoms in the solution to move.
The process of dissolving frees the atoms in the solution to move.

The process of dissolving closely binds the ions in the solution.
The process of dissolving closely binds the ions in the solution.

Answer 1

The correct statement is:

The process of dissolving frees the atoms in the solution to move.

When salt (sodium chloride, NaCl) dissolves in water, it dissociates into its constituent ions (Na⁺ and Cl⁻), which are charged particles. These ions are free to move in the solution, allowing the solution to conduct electricity well. In contrast, pure water and pure salt do not have free ions or charged particles to carry the electrical current, which is why they are poor conductors.