Talk:Freezing-point depression

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[edit] Mistake???

From the article:

ΔTf = i · Kf · activity

   * activity is in units of mol/kg, and is equal to an activity coefficient times the molality

...

   * i is the i factor or the van 't Hoff factor (see van 't Hoff), accounts for the number of individual ions formed by a compound in solution.

Eehm, isn't i the activity coefficient? I'm a bit puzzled, but it seems to me that it is used twice here.

—The preceding unsigned comment was added by 83.98.253.62 (talk) 09:05, 6 February 2007 (UTC).

[edit] Osmometry

a good addition to this article would be the clinical uses for freezing point depression, such as osmometry!

From the article:

Freezing-point depression is the difference between the freezing points of a pure solvent and a solution of a nonelectrolyte in that solvent.

It is a well-known fact that salt can cause freezing-point depression. The electrolyte article mentions that sodium and chloride are both electrolytes. Maybe the article should mention electrolytes instead of nonelectrolytes?

Freezing-point depression is the difference between the freezing points of the pure solvent and the solution. It occurs in both electrolyte and non electrolyte solutions. However, the van't Hoff factor kicks in when you have an electroyte solution because it takes into account how the ions disassociate. ha ha

[edit] Table of constants?

Anyone willing to compile a table of freezing point depression constants for a variety of solvents? I can do it if no one else does, but right now I'm busy.Quaxmonster 23:23, 22 May 2006 (UTC)