Which of the following pairs will form an ideal solution?

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

Two liquids $X$ and $Y$ form an ideal solution. At $300 \ K,$ vapour pressure of the 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 further added to this solution,vapour pressure of the solution increases by $10 \ mm \ Hg.$ Vapour pressure (in $mm \ Hg$) of $X$ and $Y$ in their pure states will be,respectively:

Which of the following mixtures is a non-ideal solution?

$A$ non-ideal solution was prepared by mixing $30 \ mL$ chloroform and $50 \ mL$ acetone. The volume of the mixture will be

At $300 \ K$,the vapour pressures of $A$ and $B$ liquids are $500 \ mm \ Hg$ and $400 \ mm \ Hg$ respectively. Equal moles of $A$ and $B$ are mixed to form an ideal solution. The mole fraction of $A$ and $B$ in the vapor state is respectively: