The electrolyte solutions show abnormal colligative porperties.To account for this effect we define a quantity called the Van't Hoff factor given by
`i=("Actual number of particles in solution after dissociation")/("Number of formula units initially dissolved in solution")`
`i=1 ("for non-electrolytes")`
`igt1 ("for electrolytes, undergoing dissociation")`
`ilt1 ("for solutes, undergoing association")`
Answer the following questions:
For a solution of a non-electrolyte in water, the Van't Hoff factor is

Options

A. `Always equal to 0`
B. ``le1`
C. `Always equal to 2`
D. `ge but lt2`

Answer

To solve the question regarding the Van't Hoff factor for a solution of a non-electrolyte in water, we can follow these steps:

### Step 1: Understand the Definition of Van't Hoff Factor
The Van't Hoff factor (i) is defined as the ratio of the actual number of particles in solution after dissociation to the number of formula units initially dissolved in solution.

### Step 2: Identify the Type of Solute
In this case, we are dealing with a non-electrolyte. Non-electrolytes are substances that do not dissociate into ions when dissolved in a solvent (like water).

### Step 3: Apply the Definition to Non-Electrolytes
For a non-electrolyte:
- The number of formula units initially dissolved in solution is equal to the number of particles in solution after dissolution because non-electrolytes do not dissociate.
- Therefore, the actual number of particles in solution after dissociation is equal to the number of formula units initially dissolved.

### Step 4: Calculate the Van't Hoff Factor
Using the definition:
\[ i = \frac{\text{Actual number of particles in solution after dissociation}}{\text{Number of formula units initially dissolved in solution}} \]
For a non-electrolyte:
\[ i = \frac{n}{n} = 1 \]

### Conclusion
Thus, the Van't Hoff factor (i) for a solution of a non-electrolyte in water is:
\[ i = 1 \]