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

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.

Answer 1

The correct statement that explains why the solution conducts electricity well when salt is dissolved in water is:

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

However, it's important to clarify that in the case of salt (sodium chloride, NaCl), it is actually the dissociation of salt into its ions (Na⁺ and Cl⁻) that enables the conduction of electricity, as it allows the charged ions to move freely in the solution. The movement of these ions, rather than free electrons, is what facilitates electrical conductivity in the solution. This means the most accurate answer should reflect the concept of ion movement rather than electron movement.