Supercooled water

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You can cool water below its stated freezing point and then crystallize it into ice on command. This is known as supercooling.

Supercooling, also known as undercooling, is the process of lowering the temperature of a liquid or a gas below its freezing point without it becoming a solid.
A liquid crossing its standard freezing point will crystalize in the presence of a seed crystal or nucleus around which a crystal structure can form creating a solid. Lacking any such nuclei, the liquid phase can be maintained all the way down to the temperature at which crystal homogeneous nucleation occurs. Homogeneous nucleation can occur above the glass transition temperature, but if homogeneous nucleation has not occurred above that temperature, an amorphous (non-crystalline) solid will form.

Water normally freezes at 273.15 K (0 °C or 32 °F), but it can be "supercooled" at standard pressure down to its crystal homogeneous nucleation at almost 224.8 K (−48.3 °C/−55 °F). The process of supercooling requires that water be pure and free of nucleation sites, which can be achieved by processes like reverse osmosis (I used reverse osmosis water) or chemical demineralization, but the cooling itself does not require any specialised technique.

You can initiate crystallization into ice in several different ways. Three of the most entertaining ways to cause the water to freeze are to shake the bottle, drop the ice into the water or to open the bottle and pour the water onto a piece of ice.