Freezing-point depression

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'''[[Freezing-point depression]]''' describes the phenomenon in which the '''[[freezing point]]''' of a '''[[liquid]]''' (a solvent) is depressed when another compound is added, meaning that a solution has a lower freezing point than a pure solvent. This happens whenever a solute is added to a pure solvent, such as '''[[water]]'''. The phenomenon may be observed in sea water, which due to its '''[[salt]]''' content remains '''[[liquid]]''' at temperatures below 0 °C, the freezing point of pure water. '''[[Freezing-point depression]]''' describes the phenomenon in which the '''[[freezing point]]''' of a '''[[liquid]]''' (a solvent) is depressed when another compound is added, meaning that a solution has a lower freezing point than a pure solvent. This happens whenever a solute is added to a pure solvent, such as '''[[water]]'''. The phenomenon may be observed in sea water, which due to its '''[[salt]]''' content remains '''[[liquid]]''' at temperatures below 0 °C, the freezing point of pure water.
 +----
 +Also See
 +*'''[[Snow]]'''
 +*'''[[Evaporation]]'''
 +*'''[[Water]]'''
 +*'''[[Moisture]]'''
 +*'''[[Sublimation]]'''
 +*'''[[Water Cycle]]'''
 +*'''[[Water Vapor]]'''
 +*'''[[Atmosphere]]'''
Reference Reference

Revision as of 08:55, 1 May 2010

Freezing-point depression describes the phenomenon in which the freezing point of a liquid (a solvent) is depressed when another compound is added, meaning that a solution has a lower freezing point than a pure solvent. This happens whenever a solute is added to a pure solvent, such as water. The phenomenon may be observed in sea water, which due to its salt content remains liquid at temperatures below 0 °C, the freezing point of pure water.


Also See

Reference

  1. Wikipedia Freezing-point depression [1]

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