Define
Miscible liquids

Two volatile and miscible liquids can be separated by fractional distillations into pure components under the condition

The following statements is true only under some specific conditions. Write the condition for it "Two volatile and miscible liquids can be separated by fractional distillation into pure components."

Fractional distillation is suitable for separation of miscible liquids with a boiling point difference of about 25 K or less. What part of fractional distillation apparatus makes it efficient and possess an advantage over a simple distillation process. Explain using a diagram.

Chloroform and benzene form a pair of miscible liquids. These can be separated by:

How will you separate a mixture of two miscible liquids benzene and chloroform ?

The boiling points of two miscible liquids, which do not form azeotropic mixture, are close to each other. Their separation is best carried out by :

For a mixture of two volatile , completely miscible liquids A and B , with P_(A)^(@)=500 " torr and " P_(B)^(@)=800 torr , what is the composition of last droplet of liquid remaining in equilibrium with vapour ? Provided the initial ideal solution has a composition of x_(A) = 0.6 and x_(B)=0.4

The solution which boil at constant temperature like a pure liquid and possess same composition in liquid as well as vapour state are called azeotropes. The components of azetropes cannot be separated by fractional distillation. Only non-ideal solutions form azeotropes. Solutions with negative deviation form maximum boiling azeotrope and the solutions with positive deviation form minimum boiling azeotrope. The boiling point of an azeotrope is never equal to the boiling points of any of the components of the azeotrope. Answer the following question: The azeotropic solutions of two miscible liquids 100 mL of liquid A and 50 mL of liquid B are mixed to form 138 mL solution. It is

A mixture of two miscible liquids A and B is distilled under equilibrium conditions at 1 atm pressure. The mole fraction of A in solution and vapour phase are 0.30 and 0.60 respectively. Assuming ideal behaviour of the solution and the vapour, calculate the ratio of the vapour pressure of pure A to that of pure B.

The vapour pressure of two miscible liquids A and B are 300 and 500 mm of Hg respectively.In a flask 2 moles of A are mixed with 6 moles of B.Further to the mixture, 32 g of an ionic non-volatile solute MCl (partically ionised mol.mass =70 u) were also added.Thus, the final vapour pressure of solution was found to be 420 mm of Hg.Then, identify the correct statement(s): (Assume the liquid mixture of A and B to behave ideally ).