As mentioned in the previous post in this blog, in reality there is no liquid mixture that behaves ideally. This time we will have a closer look at real liquid mixtures.
In the case of an ideal solution: The intermolecular forces ( the forces between component X and component Y) in the mixture are more or less equivalently strong as those forces in pure liquid X and in pure liquid X.
There are two different types of deviation. Let us look at the first one first.
1) Positive deviation: This deviation from Raoult's law occurs when the intermolecular forces in the mixture are weaker than those in pure liquids. This also means that the resulting vapour pressure of these mixtures is generally higher than that of ideal mixtures.
Below are the examples of the mixture that exhibit this kind of deviation:
a) Benzene-Water mixture
b) Ethanol-Water mixture
c) Pyridine-Water mixture
P-x diagram for an ideal mixture of X and Y:
P-x diagram for a mixture with positive deviation:
As you can clearly see, the total vapour is higher in the second case than that in an ideal liquid mixture. The second deviation will be dealt in the next post.
In the case of an ideal solution: The intermolecular forces ( the forces between component X and component Y) in the mixture are more or less equivalently strong as those forces in pure liquid X and in pure liquid X.
There are two different types of deviation. Let us look at the first one first.
1) Positive deviation: This deviation from Raoult's law occurs when the intermolecular forces in the mixture are weaker than those in pure liquids. This also means that the resulting vapour pressure of these mixtures is generally higher than that of ideal mixtures.
Below are the examples of the mixture that exhibit this kind of deviation:
a) Benzene-Water mixture
b) Ethanol-Water mixture
c) Pyridine-Water mixture
P-x diagram for an ideal mixture of X and Y:
P-x diagram for a mixture with positive deviation:
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