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Non-ideal solutions exhibit either positive or negative deviations from Raoult’s law. What are these deviations and why are they caused? Explain with one example for each type.

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Non-ideal solutions deviate from Raoult's law, which describes the behavior of ideal solutions. These deviations can be categorized as positive or negative, depending on how they affect the vapor pressure of the components in the solution compared to what is predicted by Raoult's law. Positive Deviation: Positive...
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Non-ideal solutions deviate from Raoult's law, which describes the behavior of ideal solutions. These deviations can be categorized as positive or negative, depending on how they affect the vapor pressure of the components in the solution compared to what is predicted by Raoult's law.

  1. Positive Deviation:

    • Positive deviations occur when the vapor pressure of the components in the solution is higher than what is predicted by Raoult's law. This typically happens when the intermolecular forces between unlike molecules in the mixture are weaker than those between like molecules. As a result, the escaping tendency of the molecules from the solution is higher than expected, leading to a higher vapor pressure.
    • Example: A common example of a positive deviation from Raoult's law is the mixture of acetone (CH3COCH3) and chloroform (CHCl3). Acetone and chloroform have different molecular structures and polarities. When mixed together, the intermolecular forces between acetone and chloroform molecules are weaker than the forces between like molecules. As a result, the vapor pressure of the solution is higher than what would be expected based on Raoult's law.
  2. Negative Deviation:

    • Negative deviations occur when the vapor pressure of the components in the solution is lower than what is predicted by Raoult's law. This typically happens when the intermolecular forces between unlike molecules are stronger than those between like molecules. Consequently, the escaping tendency of the molecules from the solution is lower than expected, resulting in a lower vapor pressure.
    • Example: An example of a negative deviation from Raoult's law is the mixture of ethanol (C2H5OH) and water (H2O). Ethanol and water molecules can form hydrogen bonds with each other due to their polar nature. When mixed together, the intermolecular forces between ethanol and water molecules are stronger than those between like molecules. This results in a lower vapor pressure than what would be expected based on Raoult's law.

In both cases, deviations from Raoult's law are caused by differences in the intermolecular forces between the components of the solution.

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