Question

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
A. Less than 1
B. Greater than 1
C. Equivalent to one
D. Zero

Answer 1

Hint: The Van't Hoff factor , \[i\] , indicated variation between the concentration of a material determined by its mass and the concentration of particles actually formed when the substance is diffused. The Van’t Hoff factor is virtually 1 for the majority of non-electrolytes dissolved in water.

Complete step-by-step answer:A solute's impact on dissociation properties, such as osmotic pressure, relative vapour pressure reduction, boiling-point elevation, and freezing-point depression, is measured by the Van 't Hoff factor $i$ . For dissociation, association, and the non-electrolyte solute, the Van't Hoff factor value is more than one, less than one, and equal to one respectively.
The Van't Hoff factor is used to gauge how far a molecule will go in either association or dissociation. The ratio of the quantities of solute particles in associated or dissociated form and in original form is known as the Van't Hoff factor. Only the number of solute particles depends on this value.
The Van't Hoff factor is the ratio of normal molecular weight to experimental molecular weight. It is greater than one which implies that experimental weight is less than the normal calculated molecular weight.

Option ‘B’ is correct

Note: In physics and chemistry, an electrolyte is a substance that conducts electrical current as a result of splitting into positively and negatively charged ions. In this case the number of particles per unit volume increases after ionisation. The mass of individual ions will be less than that of the ionic compound from which it is formed.