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Limitations of Arrhenius concept.

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i. If fails to explain the behaviour of acids and bases in non-aqueous solvents.

ii. If fails to explain the neutralisation reactions giving rise to salt formation in absence of solvent.

e.g., CO2 + CaO →CaCO3 ;

NH3(g) + HCI(g) →NH4CI(g) or (s)

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