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) Responses 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 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.

Question

GPT-4o mini · Answer

The correct statement that explains why a salt solution conducts electricity well is: The process of dissolving frees the electrons in the solution to move.

However, it’s important to clarify that when salt (sodium chloride, for example) is dissolved in water, it dissociates into its constituent ions (sodium ions and chloride ions). These free-moving ions allow the solution to conduct electricity, rather than electrons in the traditional sense.

So the best answer from the choices provided should emphasize the mobility of ions rather than electrons. A more precise phrasing would be: The process of dissolving frees the ions in the solution to move. However, since that exact phrasing isn't one of the choices given, the closest option in terms of concept is the one mentioning "freeing electrons," but ideally it should mention "ions" for accuracy.