Which pair from the following will not form an ideal solution?

Liquid $A$ and $B$ form an ideal solution. The vapour pressure of pure liquids $A$ and $B$ are $350 \ mm \ Hg$ and $750 \ mm \ Hg$ respectively at the same temperature. If $x_A$ and $x_B$ are the mole fractions of $A$ and $B$ in the solution,and $y_A$ and $y_B$ are the mole fractions of $A$ and $B$ in the vapour phase,then:

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 $300 \ K$?

$p_A$ and $p_B$ are the vapour pressure of pure liquid components,$A$ and $B,$ respectively of an ideal binary solution. If $x_A$ represents the mole fraction of component $A,$ the total pressure of the solution will be

Which of the following does not belong to an ideal solution?

Assertion $A$: For an ideal solution formed by mixing liquids $P$ and $Q$, $\Delta_{mix} H = 0$ and $\Delta_{mix} V = 0$.
Reason $R$: No interactions occur between $P$ and $Q$.
In the light of the above statements, choose the most appropriate answer from the options given below: