* Freezing Point Depression: Salt dissolves in water, forming ions (charged particles). These ions disrupt the regular arrangement of water molecules in the ice crystal structure. This disruption makes it harder for the water molecules to bond together and stay solid, lowering the freezing point (and thus the melting point) of the water.

* Colligative Property: This effect is called "freezing point depression," and it's a colligative property. This means the change in freezing point depends only on the concentration of dissolved particles, not on the specific type of solute (in this case, salt).

* Practical Example: This is why we use salt on icy roads and sidewalks in the winter. The salt lowers the freezing point of water, so the ice melts even at temperatures below 0°C (32°F).

Important Note: The amount of salt needed to lower the freezing point significantly depends on the concentration. A small amount of salt will have a minimal effect.