Why does solute depress freezing point

So when you multiply all of these together you get 0. So we can actually like talk about, when you think about when it snows outside and the reason that you put salt on the roads there isn't even salt on the roads that's actually going to lower the freezing point so there's not going to be sheets of ice on your drive way or on the roads or on the side walks.

So that's why they use salt and they actually use calcium chloride typically which is actually better than sodium chloride because this actually breaks up into 3 particles so it'll drop the freezing point 3 times much as another solute would. So this is an example of frizzing point depression.

All Chemistry videos Unit Chemical Solutions. Previous Unit Kinetic-Molecular Theory. Next Unit Chemical Reaction Rates. Kendal Orenstein. Thank you for watching the video. Start Your Free Trial Learn more. Kendal Orenstein Rutger's University M. Explanation Transcript Freezing point depression is a colligative property of solutions. Chemistry Chemical Solutions. When a substance starts to freeze, the molecules slow down due to the decreases in temperature, and the intermolecular forces start to take over.

The molecules will then arrange themselves in a pattern, and thus turn into a solid. In order to achieve a solid, the solution must be cooled to an even lower temperature. The freezing point depression can also be explained in terms of vapor pressure. Considering the fact that the vapor pressure of the solid and liquid forms must be the same at freezing point, because otherwise the system would not be at equilibrium, the lowering of the vapor pressure leads to the lowering of the temperature at which the vapor pressures of the liquid and frozen forms of the solution will be equal.

What is the freezing point of an aqueous solution when enough NaCl has been added to create a 0. The K f value for water is 1. This might seem like the end of the problem, but it is not. How can I calculate the amount of solute in a solution?

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What is solute concentration? How does a solute differ from a solvent? See all questions in Solute.