For an ideal solution,the correct option is

At $27^{\circ} C$,two liquids $A$ and $B$ form an ideal solution with mole fractions $0.67$ and $0.33$ respectively. If the vapour pressure of pure $A$ and $B$ at $27^{\circ} C$ are $300 \ mm$ and $450 \ mm$ respectively,the total vapour pressure of the solution in $mm$ is:

In a binary ideal solution of liquids $A$ and $B$ at a constant temperature,the mole fraction of $A$ in the liquid phase is $0.7$ and in the vapor phase is $0.4$. If $P_A^o + P_B^o = 90 \, mm$,then the vapor pressures of pure liquids $A$ and $B$ at that temperature are respectively:

On mixing $10 \ mL$ of acetone with $40 \ mL$ of chloroform,the total volume of the solution is

When acetone is added to chloroform,then a hydrogen bond is formed between them. These liquids show:

$1 \, \text{mole}$ of liquid $A$ and $2 \, \text{mole}$ of liquid $B$ form a solution with a vapor pressure of $38 \, \text{torr}$. If the vapor pressures of pure $A$ and pure $B$ are $45 \, \text{torr}$ and $36 \, \text{torr}$ respectively,the solution will be: