Two liquids $x$ and $y$ form an ideal solution. At $300 \ K$,the vapor pressure of a solution containing $1 \ mol$ of $x$ and $3 \ mol$ of $y$ is $550 \ mm \ Hg$. At the same temperature,if $1 \ mol$ of $y$ is added to the solution,the vapor pressure increases by $10 \ mm \ Hg$. The vapor pressures of pure $x$ and $y$ are respectively:

The total pressure observed by mixing two liquids $A$ and $B$ is $350 \ mm \ Hg$ when their mole fractions are $0.7$ and $0.3$ respectively. The total pressure becomes $410 \ mm \ Hg$ if the mole fractions are changed to $0.2$ and $0.8$ respectively for $A$ and $B$. The vapour pressure of pure $A$ is $........... \ mm \ Hg$. (Nearest integer)
Consider the liquids and solutions behave ideally.

Which property is not found in 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.

Which of the following is not correct for an ideal solution?

Which of the following statements about the composition of the vapour over an ideal $1:1$ molar mixture of benzene and toluene is correct? Assume that the temperature is constant at $25\ ^oC$. (Given,vapour pressure data at $25\ ^oC$,benzene $= 12.8\ kPa,$ toluene $= 3.85\ kPa$)