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 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.

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

When salt (sodium chloride) is dissolved in water, it separates into its constituent ions (sodium ions and chloride ions). These free ions can move throughout the solution, allowing the solution to conduct electricity effectively. Pure water and solid salt do not have these free-moving charged particles, which is why they are poor conductors of electricity.