$A$ mixture of ethanol and acetone shows positive deviation from Raoult's law because:

Explain the terms ideal and non-ideal solutions in the light of forces of interactions operating between molecules in liquid solutions.

Which of the following solutions behaves nearly as an ideal solution?

If liquids $A$ and $B$ form an ideal solution,then which of the following is true?

The vapour pressures of chloroform $(CHCl_3)$ and dichloromethane $(CH_2Cl_2)$ at $298 \ K$ are $200 \ mmHg$ and $415 \ mmHg$,respectively. An ideal solution is prepared by mixing $59.75 \ g$ of $CHCl_3$ and $21.25 \ g$ of $CH_2Cl_2$. The mole fractions of chloroform and dichloromethane in the vapour phase,respectively,are:

The formation of a binary solution is considered as follows:
$(1)$ Pure solvent enthalpy $\Delta H_1$ (separated)
$(2)$ Pure solute enthalpy $\Delta H_2$ (separated)
$(3)$ Pure solvent + Pure solute $\to$ Solution $\to$ Enthalpy $\Delta H_3$
If $......$ then the resulting solution is ideal.