Which factors promote the formation of solutions? Which two processes are at equilibrium in a saturated sugar solution? Why do solutes lower the freezing point? Why does solution formation require energy? Why do solutes dissolve in solvents? What solvent dissolves silicone? See all questions in Solution Formation. Impact of this question views around the world.
The example given in the introduction is an example of a colligative property. Colligative properties are properties that differ based on the concentration of solute in a solvent, but not on the type of solute. What this means for the example above is that people in colder climates do not necessarily need salt to get the same effect on the roads—any solute will work. However, the higher the concentration of solute, the more these properties will change.
When table salt is added to water, the resulting solution has a higher boiling point than the water did by itself. The ions form an attraction with the solvent particles that prevents the water molecules from going into the gas phase.
This is true for any solute added to a solvent; the boiling point will be higher than the boiling point of the pure solvent without the solute. In other words, when anything is dissolved in water, the solution will boil at a higher temperature than pure water would. The boiling point elevation due to the presence of a solute is also a colligative property.
That is, the amount of change in the boiling point is related to the number of particles of solute in a solution and is not related to the chemical composition of the solute.
The effect of adding a solute to a solvent has the opposite effect on the freezing point of a solution as it does on the boiling point. A solution will have a lower freezing point than a pure solvent. The freezing point is the temperature at which the liquid changes to a solid. At a given temperature, if a substance is added to a solvent such as water , the solute-solvent interactions prevent the solvent from going into the solid phase.
The solute-solvent interactions require the temperature to decrease further in order to solidify the solution. A common example is found when salt is used on icy roadways. The de-icing of planes is another common example of freezing point depression in action. A number of solutions are used, but commonly a solution such as ethylene glycol, or a less toxic monopropylene glycol, is used to de-ice an aircraft.
The aircrafts are sprayed with the solution when the temperature is predicted to drop below the freezing point. The freezing point depression is the difference in the freezing points of the solution from the pure solvent. This is true for any solute added to a solvent; the freezing point of the solution will be lower than the freezing point of the pure solvent without the solute. Thus, when anything is dissolved in water, the solution will freeze at a lower temperature than pure water would.
The freezing point depression due to the presence of a solute is also a colligative property. That is, the amount of change in the freezing point is related to the number of particles of solute in a solution and is not related to the chemical composition of the solute. How does adding a solute to a solvent affect the boiling point of the solvent? Chemistry Solutions Colligative Properties. Jul 29, Explanation: This is an example of a so-called "colligative property" , a property that depends on the NUMBER of particles that you dissolve in the solvent.
Related questions How are colligative properties determined? How do you calculate freezing point depression? How can freezing point depression determine purity?
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