Which of the following solutions behaves nearly as an ideal solution?

Vapour pressures of pure liquids $A$ and $B$ are $300$ and $800 \ torr$ respectively at $25^{\circ}C$. When these two liquids are mixed at this temperature to form a solution in which mole percentage of $B$ is $90$,the total vapour pressure is observed to be $720 \ torr$. Which of the following is true for this solution?

At $88 \, ^\circ C$,the vapor pressure of benzene is $900 \, \text{torr}$ and the vapor pressure of toluene is $360 \, \text{torr}$. What is the mole fraction of benzene in the mixture with toluene at $1 \, \text{atm}$ and $88 \, ^\circ C$? Assume benzene and toluene form an ideal solution.

Consider the following statements about the solutions formed by mixing two liquids.
$A$. An ideal solution thus formed obeys Raoult's law throughout the composition range.
$B$. Mixture of chloroform and acetone shows negative deviation from Raoult's law.
$C$. Mixture of aniline and phenol shows positive deviation from Raoult's law.

At $T(K)$,the vapour pressures of two liquids,heptane and octane are $106 \ kPa$ and $47 \ kPa$ respectively. If $25 \ g$ of heptane and $57 \ g$ of octane form an ideal solution,at $T(K)$ the vapour pressure of solution in $kPa$ is :

$A$ liquid solution is formed by mixing $10 \, moles$ of aniline and $20 \, moles$ of phenol at a temperature where the vapour pressure of pure liquid aniline and phenol are $90 \, mmHg$ and $87 \, mmHg$ respectively. The possible vapour pressure of the solution at that temperature is ............. $mmHg$.