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Arrhenius theory could not explain the acidic and basic behaviour in non-aqueous solutions.
  • a)
    true
  • b)
    false
Correct answer is option 'A'. Can you explain this answer?
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Arrhenius theory could not explain the acidic and basic behaviour in n...
The major drawback of Arrhenius theory is that it fails to explain the acidic and basic behaviour in non-aqueous solutions. It cannot explain the acidic character of aluminium chloride, Boron fluoride and basic character of NH3 PH3.
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Arrhenius theory could not explain the acidic and basic behaviour in n...
The Arrhenius Theory and Non-Aqueous Solutions

The Arrhenius theory, proposed by Svante Arrhenius in 1884, is a widely accepted theory that explains the behavior of acids and bases in aqueous solutions. According to this theory, acids are substances that release hydrogen ions (H+) in solution, while bases are substances that release hydroxide ions (OH-) in solution. However, the Arrhenius theory is not applicable to non-aqueous solutions and fails to explain their acidic and basic behavior.

Lack of Water Molecules

One of the main reasons why the Arrhenius theory fails in non-aqueous solutions is the absence of water molecules. In aqueous solutions, water molecules play a crucial role in the dissociation of acids and bases. Water molecules can act as a medium for the ions to move around and react with each other. However, in non-aqueous solvents, such as organic solvents like ethanol or acetone, there are no water molecules present to facilitate the ionization process.

Alternative Theories

To explain the acidic and basic behavior in non-aqueous solutions, alternative theories have been proposed. Some of these theories include:

1. Brønsted-Lowry Theory: This theory defines acids as proton (H+) donors and bases as proton acceptors. According to this theory, the solvent plays a crucial role in the behavior of acids and bases. In non-aqueous solvents, the solvent molecules themselves can act as proton acceptors or donors, leading to different acid-base behavior compared to aqueous solutions.

2. Lewis Theory: The Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. This theory is more general and can explain the behavior of acids and bases in both aqueous and non-aqueous solutions. In non-aqueous solvents, Lewis acids and bases can interact through electron transfer, coordination, or complexation reactions.

Conclusion

In summary, the Arrhenius theory, which explains the behavior of acids and bases in aqueous solutions, is not applicable to non-aqueous solutions. The absence of water molecules in non-aqueous solvents prevents the ionization process necessary for the Arrhenius theory. Instead, alternative theories such as the Brønsted-Lowry theory and Lewis theory are more suitable for explaining the acidic and basic behavior in non-aqueous solutions. These theories take into account the different properties and interactions that occur in non-aqueous solvents, leading to a more comprehensive understanding of acid-base behavior in these systems.
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