Final answer:
The value of Van't Hoff factor 'i' is less than 1 for an electrolyte, which leads to an experimental molecular weight that is lower than the calculated value, because not all ions behave as independent particles due to interionic attractions. The correct answer is option: A. Less than 1.
Step-by-step explanation:
The experimental molecular weight of an electrolyte will always be less than its calculated value because the value of Van't Hoff factor "i" is less than 1. The Van't Hoff factor, or 'i', is a measure of the deviation from the ideal behavior. When an ionic compound dissolves in water, it tends to dissociate into its constituent ions.
However, due to interionic attractions, not all ions will behave as completely independent particles, especially in solutions that are not extremely dilute. This interaction causes the actual number of particles in solution, and thus the experimental molecular weight, to be less than expected.
As the concentration of the electrolyte increases, the value of 'i' decreases because the ionic compounds do not totally dissociate, leading to fewer effective particles than predicted.