Final answer:
The Van't Hoff factor (i) is the ratio of the number of particles produced in solution to the number of formula units dissolved, which is essential for understanding the behavior of compounds in solution. For instance, the ideal Van't Hoff factor of Sr(OH)2 is 3, accounting for its complete dissociation into three ions in dilute solutions.
Step-by-step explanation:
The Van’t Hoff factor (i) is a critical concept in understanding how ionic and non-ionic compounds behave in solution. Specifically, it is used to calculate the effects of ionization on colligative properties of solutions. The Van’t Hoff factor is the ratio of the number of particles in solution to the number of formula units dissolved. It accounts for the degree of dissociation of a compound in solution.
For example, to predict the Van’t Hoff factor for the compound Sr(OH)2, one must recognize that this compound will dissociate completely in water into three ions: one Sr2+ and two OH−. Hence, the ideal Van’t Hoff factor (i) for Sr(OH)2 is 3, since it produces three particles per formula unit.
However, it is important to note that the ideal Van’t Hoff factor assumes complete dissociation, which is only accurate for dilute solutions (less than 0.001 M). At higher concentrations, due to ion interactions, the actual Van’t Hoff factor may be less than the ideal one.