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

On mixing,heptane and octane form an ideal solution. At $373 \ K$,the vapour pressures of the two liquid components (heptane and octane) are $105 \ kPa$ and $45 \ kPa$ respectively. Vapour pressure of the solution obtained by mixing $25.0 \ g$ of heptane and $35 \ g$ of octane will be $........ \ kPa$.
(molar mass of heptane $= 100 \ g \ mol^{-1}$ and of octane $= 114 \ g \ mol^{-1}$)

All form ideal solutions except:

For which of the following mixtures is $\Delta_{mix} H > 0$?

An ideal solution has two components $A$ and $B$. If $A$ is more volatile than $B$,then the correct relation between mole fraction of $A$ in liquid $(X_A)$ and vapour phase $(Y_A)$ is:

Which of the following is/are "not correct" for $CH_3OH + CH_3COOH$ mixture solution?
$(a)$ $\Delta H_{\text{mix}} < 0$
$(b)$ Does not obey Raoult's law
$(c)$ $\Delta H_{\text{mix}} > 0$
$(d)$ An example of ideal solution