Final answer:
The statement is true; an ideal solution is one in which all components follow Raoult's law, producing a vapor pressure directly proportional to the mole fraction of each component in the solution.
Step-by-step explanation:
The statement 'An ideal solution is a solution in which all components obeys Raoult's law' is True. Raoult's law quantifies the relationship between the concentrations of components in a solution and the vapor pressures of those components. In an ideal solution, the partial pressure exerted by any component (PA) is equal to the vapor pressure of the pure component (PA⁰) multiplied by its mole fraction (XA) in the solution, expressed as PA = XA*PA⁰.
Real solutions often exhibit deviations from Raoult's law due to differences in intermolecular interactions when mixed, leading to either positive or negative deviations. However, a true ideal solution shows no change in enthalpy on solution formation (AH soln~0), largely because its components have nearly identical intermolecular forces, like mixtures of benzene and toluene that approximate ideal solutions.
The total vapor pressure of an ideal solution (Ptot) is the sum of the partial pressures of its components. When all components in a mixture follow Raoult's law, it is considered an ideal solution.