Which of the following mixtures forms an ideal solution?

Which of the following is not correct?

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

Two statements are given below:
Statement-$I$: Liquids $A$ and $B$ form a non-ideal solution with positive deviation. The interactions between $A$ and $B$ are weaker than $A-A$ and $B-B$ interactions.
Statement-$II$: For an ideal solution,$\Delta_{mix} H = 0$ and $\Delta_{mix} V = 0$.
The correct answer is:

In a mixture of components $A$ and $B$,the components show negative deviation when:

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 $300 \ K$?