Question 57
Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.
Question 57
Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.
The solutions which obey Raoult's law over the entire range of concentration are known as ideal solutions. For an ideal solution ΔVmix=O and ΔVmix=O. The ideal behaviour of the solutions can be explained by considering two components A and B.
In pure components, the intermolecular attractive interactions will be of A-A type and B-B type, whereas in the binary solutions in addition to these two, A-B type of interaction will also be present. If A-A and B-B intermolecular forces are nearly equal to those between A-B, this leads to the formation of ideal solution e.g., solution of n-hexane and n-heptane. When a solution does not obey-Raoult's law over the entire range of concentration, then it is called non-ideal solution. The vapour pressure of such a solution is either higher or lower, than that predicted by Raoult's law.
If it is higher, the solution exhibits positive deviation and if it is lower it exhibits hegative deviation from Raoult's law. In case of positive deviation, A-B interactions are weaker than those between A-A or B-B i.e., the altractive forces between solute solvent molecules are weaker than those between solute-solute and solvent-solvent molecules e.g., mixture of ethanol and acetone.
For such solutions ΔHmixing=+ve and ΔVmixing=+ ve
On the other hand, in case of negative deviation the internolecular attractive forces between A-A and B-B are weaker than those between A-B molecules. Thus, the escaping tendency of A and B types of molecules from the solution becomes less than from the pure liquids i.e., mixture of chloroform and acetone.
For such solution ΔHmix=− ve and ΔVmix=− ve
The solutions which obey Raoult's law over the entire range of concentration are known as ideal solutions. For an ideal solution ΔVmix=O and ΔVmix=O. The ideal behaviour of the solutions can be explained by considering two components A and B.
In pure components, the intermolecular attractive interactions will be of A-A type and B-B type, whereas in the binary solutions in addition to these two, A-B type of interaction will also be present. If A-A and B-B intermolecular forces are nearly equal to those between A-B, this leads to the formation of ideal solution e.g., solution of n-hexane and n-heptane. When a solution does not obey-Raoult's law over the entire range of concentration, then it is called non-ideal solution. The vapour pressure of such a solution is either higher or lower, than that predicted by Raoult's law.
If it is higher, the solution exhibits positive deviation and if it is lower it exhibits hegative deviation from Raoult's law. In case of positive deviation, A-B interactions are weaker than those between A-A or B-B i.e., the altractive forces between solute solvent molecules are weaker than those between solute-solute and solvent-solvent molecules e.g., mixture of ethanol and acetone.
For such solutions ΔHmixing=+ve and ΔVmixing=+ ve
On the other hand, in case of negative deviation the internolecular attractive forces between A-A and B-B are weaker than those between A-B molecules. Thus, the escaping tendency of A and B types of molecules from the solution becomes less than from the pure liquids i.e., mixture of chloroform and acetone.
For such solution ΔHmix=− ve and ΔVmix=− ve
