Assuming ideal behaviour,the enthalpy and volume of mixing of two liquids respectively,are

Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.

An aqueous solution of hydrochloric acid:

At $300 \ K$,the vapour pressure of a pure liquid $A$ is $70 \ mm \ Hg$. It forms an ideal solution with another liquid $B$. The mole fraction of $B$ in the solution is $0.2$ and the total vapour pressure of the solution is $84 \ mm \ Hg$ at the same temperature. What is the vapour pressure (in $mm \ Hg$) of pure liquid $B$ at $300 \ K$?

$A$ solution of two liquids boils at a temperature higher than the boiling point of either of them. Hence,the binary solution shows:

Solution $A$ contains acetone dissolved in chloroform and solution $B$ contains acetone dissolved in carbon disulphide. The type of deviations from Raoult's law shown by solutions $A$ and $B$,respectively,are: