What is the colligative property of a solution answer?
Colligative properties of solutions are properties that depend upon the concentration of solute molecules or ions, but not upon the identity of the solute. Colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Colligative property. a property of a solution that depends on the number of particles of solute in a given volume of solvent. o Colligative properties include boiling point, freezing point, vapor pressure, and osmotic pressure.
These colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. This small set of properties is of central importance to many natural phenomena and technological applications, as will be described in this module.
Three important colligative properties of solutions are vapor-pressure lowering, boiling-point elevation, and freezing-point depression.
Colligative properties ⇨ Properties of solutions which depend on the number of solute particles but not on their nature. Examples of colligative properties are: Vapour Pressure lowering of a solution. Boiling Point elevation.
colligative property, in chemistry, any property of a substance that depends on, or varies according to, the number of particles (molecules or atoms) present but does not depend on the nature of the particles.
Hence osmotic pressure is a colligative property.
- Vapor-pressure lowering.
- Boiling-point elevation.
- Freezing-point depression.
Among the options, optical activity is not a colligative property.
Its difference with respect to the vapor pressure of the pure solvent can be calculated as: P∗solvent−Psolution=P∗solvent−xsolventP∗solvent=(1−xsolvent)P∗solvent=xsoluteP∗solvent, which shows that the vapor pressure lowering depends only on the concentration of the solute. As such, it is a colligative property.
What are the properties of a solution?
Properties of a Solution
A solution is a hom*ogeneous mixture. The constituent particles of a solution are smaller than 10-9 metres in diameter. Constituent particles of a solution cannot be seen by naked eyes. Solutions do not scatter a beam of light passing through it.
Colligative property depends just on number of solute particles present in the solution.
Colligative properties are important properties of solutions as they describe how the properties of the solvent will change as solute (or solutes) is (are) added.
Colligative properties include: Relative lowering of vapor pressure (Raoult's law) Elevation of boiling point.
The fundamental cause of all colligative properties is the higher entropy of the solution relative to that of the pure solvent. The presence of solute particles in the solution leads to an increase in the entropy, or the randomness, of the solution, when compared to the pure solvent.
Colligative qualities are those of a solution solely dependent on the concentration of solute molecules. The four colligative properties are vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Colligative Properties Equations
The equations for the four colligative properties are as follows. T f = − i K f m where T is the change in freezing point of the solution, K is a constant, and m is the molality of the solution measured in kg/mol.
Colligative properties of solutions ideally depend only on the number of solute particles per solvent molecule and not on the nature of the solute or solvent. Colligative properties include: vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure.
Colligative properties are those properties which depend on the number of solute particles irrespective of their nature relative to the total number of particles present in the solution. Among the options, optical activity is not a colligative property.
- Vapor-pressure lowering.
- Boiling-point elevation.
- Freezing-point depression.
What is the value of colligative property?
Hence, the values of colligative properties (osmotic pressure, lowering in vapour pressure, depression in freezing point and elevation in boiling point) are of small order as compared to values shown by true solutions at same concentrations.
Colligative property depends just on number of solute particles present in the solution.
In chemistry, the concentration of the solution is how much of the dissoluble substance, known as solute, is mixed with another substance, called a solvent. The standard formula is C = m / V, where C is the concentration, m is the mass of the solute, and V is the total volume of the solution.
The solute particles cannot be separated from the mixture by the process of filtration. The solute particles do not settle down when left undisturbed, that is, a solution is stable. So the statement - ' The particles of a solution can be separated by filtration method. ' is not the property of a solution.
Some examples of solutions are salt water, rubbing alcohol, and sugar dissolved in water. When you look closely, upon mixing salt with water, you can't see the salt particles anymore, making this a hom*ogeneous mixture.
Properties of the true solution
The true solution is completely transparent or colourless. The true solution has solute particles that do not dissolve when mixed with water or other liquids. The true solution does not scatter light as the particles are nearly non-existable in size.
Freezing point depression is one colligative property we use in everyday life. Many antifreezes used in automobile radiators use solutions that have a lower freezing point than normal so that automobile engines can operate at subfreezing temperatures.
