Two liquids $A$ and $B$ form an ideal solution. What will be the vapor pressure of a solution containing a mole ratio of $A$ and $B$ as $3:1$ in $torr$? $(Given: P_A^o = 24 \ torr, P_B^o = 40 \ torr)$

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.

The formation of a binary solution is considered as follows:
$(1)$ Pure solvent enthalpy $\Delta H_1$ (separated)
$(2)$ Pure solute enthalpy $\Delta H_2$ (separated)
$(3)$ Pure solvent + Pure solute $\to$ Solution $\to$ Enthalpy $\Delta H_3$
If $......$ then the resulting solution is ideal.

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

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 :

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