For the definition and description of freezing point lower or freezing point depression
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Freezing point depression isn't a medical term, but a physical process where adding solvents to solutes reduces the freezing point. An example, familiar to all of us, is adding salt to water, such as when we spread rock salt on the road in winter to stop ice forming on them.
Capital delta T subscript f, delta as just a triangle
∆Tfp = Kfp × i × m
f.p depression = (freezing point of pure solvent)-(freezing point of solution) -------> 178.4-166.2=12.2
Salt works by lowering the melting or freezing point of water. The effect is termed 'freezing point depression'.
Salt will reduce the freezing point of water to below 32ºF, thus making it less likely to have slippery roads when temperatures are near the freezing point. This happens because of the colligative property of freezing point depression.
Higher boiling point and a lower freezing point. These are called colligative properties. When a solute is put into solution with the solvent, there is a change in the vapor pressure, osmotic pressure, elevation of the boiling point, and depression of the freezing point.
32 F, 0 C, 273.15 Kelvin. At STP, pure water freezes at the above temperatures. Note that adding some solute (such as table salt or ethanol) will lower the freezing point (see Freezing Point Depression).
The depression of the freezing point is dependent on the nature of solvent and concentration of solute.
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freezing point depression ..
The freezing point depression constant for Naphthalene is 6.9 degrees Celsius/mhttp://en.wikipedia.org/wiki/Freezing-point_depression
f.p depression = (freezing point of pure solvent)-(freezing point of solution) -------> 178.4-166.2=12.2
Substances which are insoluble in a given solvent do not cause a freezing point depression in that solvent.
The freezing is ag gago weak
The maximal freezing point depression for sodium chloride is -18 0C. For the theoretical calculus see the link below.
it is increased with the increasing density
the main applicative use of freezing point depression and boiling point elevation is to calculate the molecular mass of a non volatile solute in a pure solvent.
When adding a solute to a solvent, the freezing point decreases and is also known as freezing-point depression. Hence when naphthalene is added to camphor the freezing point decreases.
-0.37 C