freezing-point depression

Freezing-point depression is used by some organisms that live in extreme cold.

The phenomenon of freezing-point depression is analogous to boiling point elevation.

For depression due to the mixture of another compound, see freezing-point depression.

Hydrogen peroxide and water form a eutectic mixture, exhibiting freezing-point depression.

The use of freezing-point depression through "freeze avoidance" has also evolution in some animals that live in very cold environments.

Freezing-point depression can also be used as a purity analysis tool when analysed by differential scanning calorimetry.

The new gene is now capable of noncolligative freezing-point depression, and thus is neofunctionalized.

Chemical (including salt) distribution induces freezing-point depression, causing ice and snow to melt at a lower temperature.

Supercooling is often confused with freezing-point depression.

This is also known as the molal freezing-point depression constant or simply the freezing-point constant.

(This effect is called freezing-point depression.)

In the laboratory, lauric acid is often used to investigate the molar mass of an unknown substance via the freezing-point depression.

Calcium chloride's freezing-point depression properties are used to slow the freezing of the caramel in caramel-filled chocolate bars.

With the formula below, freezing-point depression can be used to measure the degree of dissociation or the molar mass of the solute.

Other compounds such as magnesium chloride or calcium chloride have been used for very cold temperatures since the freezing-point depression of their solutions is lower.

They can also avoid the freezing of their exposed tissues by increasing the amount of solutes in their tissues, known as freezing-point depression.

An antifreeze mixture is used to achieve freezing-point depression for cold environments and also achieves boiling-point elevation ("anti-boil") to allow higher coolant temperature.

Freezing-point depression describes the process in which adding a solute to a solvent produces a decrease in the freezing point of the solvent.

Both the antifreeze and salt work to lower the melting point of the ice in a process called Colligative Properties and specifically, Freezing-point Depression.

Beckmann used the methods of ebullioscopy (boiling-point elevation) and cryoscopy (freezing-point depression) to determine the molecular masses of several substances.

Osmolality can be measured using an osmometer which measures colligative properties, such as Freezing-point depression, Vapor pressure, or Boiling-point elevation.

Due to the freezing-point depression of the electrolyte, as the battery discharges and the concentration of sulfuric acid decreases, the electrolyte is more likely to freeze during winter weather.

Raoult's freezing-point depression method became even more useful after it was improved by Ernst Otto Beckmann and became a standard technique for determining molecular weights of organic substances.

The freezing point of a solution is lower than that of the pure solvent, and the freezing-point depression (ΔT) is directly proportional to the amount concentration for dilute solutions.

The extent of freezing-point depression can be calculated by applying Clausius-Clapeyron relation and Raoult's law together with the assumption of the non-solubility of the solute in the solid solvent.