A solution of two miscible liquids (A and B) shows negative deviations, what temperature changes are expected during mixing the liquids?

Explain why a solution of chloroform and aceton shows negative deviation from Raoult's law?

Solution of two volatile liquids A and B obey Roalt's law. At certain temperature, it is found that when the toal pressure above a solution is 0.53 bar. The mol fraction. A in the vapour is 0.45 & other liquid is 0.65. What are the vapour pressures of the two pure liquids at the given temperature?

What is the effect of temperature on the vapour pressure of a liquid?

On mixing liquid X and liquid Y, volume of the resulting solution decreases, what type of deviation from Raoult's law is shown by the resulting solution? What change in temperature would you observe after mixing liquids X and Y.

What is the effect of temperature on the viscosity of liquids?

Non ideal solution 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.

A plot is obtained for two volatile liquids A & B as follows. From the plot answer the following. Which of the liquids have higher boiling point?

An azeotropic solution of two liquids has boiling point lower than either of them when it.

The patient's temperature was the same two times during period given. What were these two times?

A plot is obtained for two volatile liquids A & B as follows. From the plot answer the following. What is the total pressure of the solution phase?