Liquids $A$ and $B$ form an ideal solution for all compositions of $A$ and $B$ at $25^{\circ} C$. Two such solutions with $0.25$ and $0.50$ mole fractions of $A$ have total vapor pressures of $0.3 \ bar$ and $0.4 \ bar$,respectively. What is the vapor pressure of pure liquid $B$ in $bar$?

Which condition is not satisfied by an ideal solution?

Liquids $A$ and $B$ form an ideal solution in the entire composition range. At $350 \ K$,the vapour pressures of pure $A$ and pure $B$ are $7 \times 10^3 \ Pa$ and $12 \times 10^3 \ Pa$,respectively. The composition of the vapour in equilibrium with a solution containing $40 \ \text{mole percent}$ of $A$ at this temperature is

Which from the following liquid mixtures behaves nearly as an ideal solution?

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 $300 \ K$?

Two liquids $A$ and $B$ form an ideal solution at temperature $T \ K$. At $T \ K$, the vapour pressures of pure $A$ and $B$ are $55 \ kNm^{-2}$ and $15 \ kNm^{-2}$ respectively. What is the mole fraction of $A$ in the solution of $A$ and $B$ in equilibrium with a vapour in which the mole fraction of $A$ is $0.8$?