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 $torr$? $(Given: P_A^o = 24 \ torr, P_B^o = 40 \ torr)$

Liquids $A$ and $B$ form an ideal solution over the entire range of composition. At temperature $T$,an equimolar binary solution of liquids $A$ and $B$ has a vapour pressure of $45 \ Torr$. At the same temperature,a new solution of $A$ and $B$ having mole fractions $x_A$ and $x_B$,respectively,has a vapour pressure of $22.5 \ Torr$. The value of $x_A / x_B$ in the new solution is . . . . . (Given that the vapour pressure of pure liquid $A$ is $20 \ Torr$ at temperature $T$)

Which of the following pairs of liquids shows a positive deviation from Raoult's law?

At $27^o C$,the vapor pressure of pure liquid $A$ is $70 \ torr$. It forms an ideal solution with $B$. The mole fraction of $B$ is $0.2$ and the vapor pressure of the solution at $27^o C$ is $84 \ torr$. What is the vapor pressure of pure liquid $B$ at $27^o C$ (in $torr$)?

Which of the following are correct for an ideal solution?
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.

Which of the following mixtures does not show positive deviation from Raoult's law?