Ideal And Non Ideal Solutions

In an ideal solution, the enthalpy of mixing ( ) is zero because intermolecular forces between A–B are equal to those between A–A and B–B. The assertion incorrectly states it is not equal to zero, making it false. The reason correctly describes an ideal solution.

The equilibrium between dichromate ( ) and chromate ( ) ions is pH-dependent. - In an acidic medium, dichromate ions dominate. - In a basic medium, the equilibrium shifts toward chromate ions due to hydroxide ions ( ) removing ions from the solution. The reaction can be expressed as: Thus, chromate ions exist predominantly in a basic medium.

For an ideal solution, the vapour pressure of the solution can be calculated using Raoult's law, which states that the vapour pressure of each component is proportional to its mole fraction in the solution. The total vapour pressure is the sum of the partial pressures of the components:
The partial pressures are calculated as: where and are the vapour pressures of pure components and and are the mole fractions of X and Y. Since equal moles are taken, the mole fraction of each component is 0.5:
Thus, the total vapour pressure of the solution is: