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An azeotrope (/ əˈziːəˌtroʊp /) [1] or a constant heating point mixture is a mixture of two or more liquids whose proportions cannot be changed by simple distillation. [2] This happens because when an azeotrope is boiled, the vapour has the same proportions of constituents as the unboiled mixture.
Azeotropes are a mixture of at least two different liquids. Their mixture can either have a higher boiling point than either of the components or they can have a lower boiling point. Azeotropes occur when fraction of the liquids cannot be altered by distillation.
You produce a constant boiling mixture (or azeotropic mixture or azeotrope) and if you distil dilute nitric acid, that's what you will eventually be left with in the distillation flask. You cannot produce pure nitric acid from the dilute acid by distilling it.
An azeotrope is a mixture of two or more liquids with a constant boiling point. The vapor composition and liquid composition are identical, so the components of the mixture cannot be separated by simple distillation. The mixture proportions forming an azeotropic are called the azeotropic composition.
What Is Azeotropic Mixture? An azeotropic mixture is a mixture of substances that has the same concentration of vapour and fluid phases. It is basically a mixture that contains two or more liquids.
Azeotropic mixture refers to a mixture of solvents with different polarities that affects the solubility properties of extractable materials. These mixtures are used to extract large quantities of constituents from crude medications based on their chemical nature.
Definition. An azeotropic mixture is a combination of two or more liquids that has a constant boiling point and composition throughout the distillation process. This unique behavior occurs when the vapor phase of the mixture has the same composition as the liquid phase, making it impossible to separate the components through simple distillation.