When two liquids $A$ and $B$ are mixed,their boiling point becomes greater than both of them. What is the nature of this solution?

The ideal solutions formed by mixing two liquids $A$ and $B$ at $300 \ K$ in the molar ratio of $1:1$ and $1:2$ have vapour pressures of $400 \ mm$ and $350 \ mm$ respectively. At the same temperature,the vapour pressures of pure liquids $A$ and $B$ in $mm$ respectively are:

If vapour pressures of pure liquids $A$ and $B$ are $300$ and $800 \, torr$ respectively at $25 \, ^{\circ}C$. When these two liquids are mixed at this temperature to form a solution in which mole percentage of $B$ is $92$,then the total vapour pressure is observed to be $0.95 \, atm$. Which of the following is true for this solution?

For the ideal solutions, which of the following condition is suitable?

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

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