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Freezing point depression of a solvent resulting from the introduction of a solute?
Wiki User
∙ 14y ago
Yes...With the introduction of a solute, a solvent's freezing point will go down.
The most simple example is during the winter. When people are putting salt on the roads and sidewalks, what that does is lower the ice's freezing point, meaning it will have to be colder before the ice freezes. So, if it's 31 degrees outside, that's cold enough for ice to form, but if you put salt down, the salt will mix with the water trying to freeze and lower it's freezing point to, let's just choose a number, 26 degrees. Since it is not 26 degrees out, the ice will not be able to form. Then the freezing rate is zero, and the melting rate does not change, so eventually all the ice will melt because a solute was introduced to cause freezing point depression.
Wiki User
∙ 14y ago
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Could freezing point depression be used for substances that are not soluble in water?
Substances which are insoluble in a given solvent do not cause a freezing point depression in that solvent.
The change in the freezing point of a solvent by the addition of a solute is called?
freezing point depression ..
Why is the curve for the freezing point of solvent different from the freezing point of solution?
it is increased with the increasing density
What is the depression of freezing point of camphor?
Examples include salt in water, alcohol in water, or the mixing of two solids such as impurities in a finely powdered drug. In such cases, the added compound is the solute, and the original solid can be thought of as the solvent. The resulting solution or solid-solid mixture has a lower freezing point than the pure solvent or solid did. This phenomenon is what causes sea water, (a mixture of salt (and other things) in water) to remain liquid at temperatures below 0 °C (32 °F), the freezing point of pure water.
A solute makes the freezing point of a solution lower than the freezing point of the pure solvent because?
The phenomenon you're describing is generally referred to as freezing-point depression, the lowering of the freeze point of a liquid (or solvent) by adding another compound. Freezing point depression is a phenomenon driven by entropic changes in the system containing solvent and solute. As the system is frozen, the solvent forms crystals of high purity regardless of solute molecules being present while solvent crystallizes. Replacement of any solute in the crystal with a solvent molecule takes place spontaneously, since the inability of solute molecules to fit well into the ordered crystal makes the solute-solvent substitution thermodynamically favorable. As the freezing proceeds, solvent molecules continue to leave the liquid state and incorporate into the solid crystal, with each such occurrence leaving behind a smaller volume of liquid in which solute molecules can occupy. The shrinking of liquid volume occupied by a fixed number of solute molecules reduces the dispersion of solute molecules in the liquid, resulting in a reduction of entropy of the solute molecules. Thus, additional energy is required to match the reduced entropy of the solute molecules with that of the solid solvent crystal. The energy required (versus pure solvent) to gap the entropic difference (thus difference in chemical potential) to establish equilibrium but at a freezing temperature lower than that of the pure substance. Note that at low solute concentrations, freezing point depression is a property that depends solely of the number of solute particles and physical properties of the solute. Such properties are called colligative properties.
Could freezing point depression be used for substances that are not soluble in water?
Substances which are insoluble in a given solvent do not cause a freezing point depression in that solvent.
What does the depression of the freezing point dependent on?
The depression of the freezing point is dependent on the nature of solvent and concentration of solute.
The change in the freezing point of a solvent by the addition of a solute is called?
freezing point depression ..
What will the nonvolatile solute do to the freezing point of a solvent?
This is the property of freezing point depression and boiling point elevation. This is because of the solute absorbing the energy added to the system to heat its own molecules and so it would require more energy to boil the solvent. Likewise for freezing point depression, the molecules retain more energy.
Why is the curve for the freezing point of solvent different from the freezing point of solution?
it is increased with the increasing density
The freezing point of a solution containing 4.12 g of unknown solute in 100 grams of camphor is 166.2 degrees C what is the freezing point depression?
f.p depression = (freezing point of pure solvent)-(freezing point of solution) -------> 178.4-166.2=12.2
How are freezing point depression and boiling point elevation useful?
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.
Why does the freezing point decrease when naphthalene is added in camphor?
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.
How do you solve freezing depression?
You need to know the solute and the solvent and whether the solute is molecular or ionic and how many ions it contains. The formula is the change in freezing point equals the number of ions times the freezing point depression constant times the molality of the solution.
What chemical principle is the deicing procedure based on?
Freezing Point Depression occurs when the freezing point of a liquid is lowered by adding another compound to it. The solution has a lower freezing point than that of the pure solvent.
What Resulting product of a solvent and a solute?
resulting product of a solvent and solute
What is the depression of freezing point of camphor?
Examples include salt in water, alcohol in water, or the mixing of two solids such as impurities in a finely powdered drug. In such cases, the added compound is the solute, and the original solid can be thought of as the solvent. The resulting solution or solid-solid mixture has a lower freezing point than the pure solvent or solid did. This phenomenon is what causes sea water, (a mixture of salt (and other things) in water) to remain liquid at temperatures below 0 °C (32 °F), the freezing point of pure water.
