Final answer:
The claim about equilibrium crystallization is false. For true equilibrium to occur during crystallization, the crystallizing material and the liquid must maintain a consistent composition. Solution equilibrium involves equal rates of dissolution and recrystallization, and phase equilibrium involves equal rates of melting and freezing.
Step-by-step explanation:
The statement that equilibrium crystallization occurs when all crystals react continuously and completely with the liquid, so that the adjustment of crystal and melt composition throughout the crystallization interval is perfect, is false. Equilibrium crystallization typically involves a situation where the composition of the residual liquid and the growing crystals remain in equilibrium. This means that any new material crystallizing out will have the same composition as the material being dissolved back into the liquid, maintaining a consistent chemical composition throughout the process.
Solution equilibrium and phase equilibrium are related concepts, and in both cases, it is defined by the rate of a forward process being equal to the rate of the reverse process. For example, solution equilibrium exists when the rate of dissolution equals the rate of recrystallization. Similarly, a phase equilibrium occurs when the rates of melting and freezing are equal, resulting in no net change in the amount of solid or liquid.
A saturated solution must exist for equilibrium crystallization to take place, but that alone is not sufficient for true chemical equilibrium, as all components must be simultaneously present.