Explain what the hatchet "colligative" means, and also list the colligative properties. Suggest what happens to the boiling suggest and the freezing point of a solvent once a solute is added to it. Calculation boiling point elevations and also freezing allude depressions for a solution.

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People that live in chillier climates have actually seen trucks put salt on the roads once snow or ice cream is forecast. Why is this done? together a result of the information you check out in this section,you will recognize why these occasions occur. You will also learn to calculate precisely how lot of an result a particular solute have the right to have on the boiling allude or freezing allude of a solution.

The example given in the development is an example of a colligative property. Colligative properties room properties that differ based upon the concentration that solute in a solvent, but not on the kind of solute. What this way for the example over is that human being in cooler climates execute notnecessarily require salt to get the same result on the roads—any solute will work. However, the higher the concentration of solute, the more these properties will change.

### Boiling point Elevation

Water boils in ~ $$100^\texto \textC$$ at $$1 \: \textatm$$ the pressure, yet a solution of saltwater does not . As soon as table salt is added to water, the resulting solution has a higher boiling point than the water go by itself. The ions form an attraction through the solvent particles that prevents the water molecules from going right into the gas phase. Therefore, the saltwater solution will not boil in ~ $$100^\texto \textC$$. In order for the saltwater solution to boil, the temperature have to be raised about $$100^\texto \textC$$. This is true for any solute added to a solvent; the boiling point will be higher than the boiling allude of the pure solvent (without the solute). In various other words, as soon as anything is dissolved in water, the equipment will boil at a greater temperature than pure water would.

The boiling suggest elevation because of the existence of a solute is additionally a colligative property. The is, the lot of change in the boiling allude is related to the number of particles that solute in a solution and is not regarded the couchsurfingcook.comical composition of the solute. A $$0.20 \: \textm$$ solution of table salt and also a $$0.20 \: \textm$$ equipment of hydrochloric acid would have the same result on the cook point.

### Freezing allude Depression

The impact of including a solute come a solvent has actually the opposite effect on the freezing allude of a solution as it does on the cook point. A systems will have actually a lower freezing suggest than a pure solvent. The freezing point is the temperature in ~ which the liquid alters to a solid. At a offered temperature, if a problem is included to a solvent (such together water), the solute-solvent interactions stop the solvent from going right into the hard phase. The solute-solvent interactions need the temperature come decrease additional in order come solidify the solution. A usual example is uncovered when salt is used on icy roadways. Salt is put on roads so that the water top top the roadways will not freeze in ~ the normal $$0^\texto \textC$$ however at a lower temperature, together low together $$-9^\texto \textC$$. The de-icing of plane is one more common instance of freezing point depression in action. A variety of solutions space used, yet commonly a equipment such as ethylene glycol, or a much less toxic monopropylene glycol, is offered to de-ice one aircraft. The aircrafts are sprayed through the solution when the temperature is predicted to drop below the freezing point. The freezing allude depression is the distinction in the freezing points of the systems from the pure solvent. This is true for any type of solute included to a solvent; the freezing allude of the equipment will be lower than the freezing point of the pure solvent (without the solute). Thus,when something is liquified in water, the systems will freeze at a reduced temperature 보다 pure water would.

The freezing point depression due to the existence of a solute is also a colligative property. The is, the quantity of readjust in the freezing allude is pertained to the number of particles the solute in a solution and is not concerned the couchsurfingcook.comical ingredient of the solute. A $$0.20 \: \textm$$ systems of table salt and a $$0.20 \: \textm$$ systems of hydrochloric acid would have actually the same effect on the freezing point.

By learning the molality of a solution and also the number of particles a compound will certainly dissolve come form, it is possible to suspect which solution in a team will have actually the lowest freezing point. To compare the boil or freeze points that solutions, follow these basic steps:

label each solute together ionic or covalent. If the solute is ionic, determine the number of ions in the formula. Be mindful to look because that polyatomic ions. Multiply the initial molality ($$\textm$$) the the equipment by the variety of particles developed when the solution dissolves. This will give you the complete concentration of particles dissolved. Compare these values. The greater total concentration will result in a higher boiling point and a reduced freezing point.

Example $$\PageIndex1$$

Rank the complying with solutions in water in bespeak of increasing (lowest to highest) freezing point:

$$0.1 \: \textm \: \ceNaCl$$ $$0.1 \: \textm \: \ceC_6H_12O_6$$ $$0.1 \: \textm \: \ceCaI_2$$

Solution

To to compare freezing points, we require to understand the total concentration of all particles as soon as the solute has been dissolved.

$$0.1 \: \textm \: \ceNaCl$$: This compound is ionic (metal through nonmetal), and also will dissolve right into 2 parts. The full final concentration is: $$\left( 0.1 \: \textm \right) \left( 2 \right) = 0.2 \: \textm$$ $$0.1 \: \textm \: \ceC_6H_12O_6$$: This compound is covalent (nonmetal with nonmetal), and also will continue to be as 1 part. The total final concentration is: $$\left( 0.1 \: \textm \right) \left(1 \right) = 0.1 \: \textm$$ $$0.1 \: \textm \: \ceCaI_2$$: This compound is ionic (metal through nonmetal), and will dissolve into 3 parts. The full final concentration is: $$\left( 0.1 \: \textm \right) \left( 3 \right) = 0.3 \: \textm$$

Remember, the better the concentration the particles, the lower the freezing point will be. $$0.1 \: \textm \: \ceCaI_2$$ will have actually the shortest freezing point, followed by $$0.1 \: \textm \: \ceNaCl$$, and the greatest of the three remedies will it is in $$0.1 \: \textm \: \ceC_6H_12O_6$$, however all three of them will have a lower freezing point than pure water.

The boiling suggest of a systems is higher than the boiling suggest of a pure solvent, and the freezing suggest of a solution is lower than the freezing point of a pure solvent. However, the amount come which the boiling point increases or the freezing point decreases counts on the quantity of solute that is added to the solvent. A mathematics equation is supplied to calculate the boiling allude elevation or the freezing point depression.

The boiling point elevation is the amount the the boiling point temperature increases contrasted to the original solvent. Because that example, the boiling allude of pure water at $$1.0 \: \textatm$$ is $$100^\texto \textC$$ while the boiling allude of a $$2\%$$ saltwater equipment is around $$102^\texto \textC$$. Therefore, the boiling suggest elevation would certainly be $$2^\texto \textC$$. The freezing suggest depression is the amount the the freezing temperature decreases.

Both the boiling allude elevation and also the freezing point depression are related to the molality of the solution. Looking at the formula because that the boiling suggest elevation and also freezing point depression, we view similarities between the two. The equation provided to calculation the increase in the boiling allude is:

\<\Delta T_b = k_b \cdot \textm \cdot i \labelBP\>

Where:

$$\Delta T_b =$$ the quantity the boiling suggest increases. $$k_b =$$ the boiling suggest elevation continuous which depends on the solvent (for water, this number is $$0.515^\texto \textC/m$$). $$\textm =$$ the molality of the solution. $$i =$$ the variety of particles developed when that compound dissolves (for covalent compounds, this number is always 1).

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The adhering to equation is supplied to calculate the to decrease in the freeze point:

\<\Delta T_f = k_f \cdot \textm \cdot ns \labelFP\>

Where:

$$\Delta T_f =$$ the lot the freezing temperature decreases. $$k_f =$$ the freezing allude depression continuous which depends on the solvent (for water, this number is $$1.86^\texto \textC/m$$). $$\textm =$$ the molality the the solution. $$i =$$ the variety of particles created when the compound disappear (for covalent compounds, this number is constantly 1).