The degree of dissociation `(alpha)` of a weak electrolyte `A_(x)B_(y)` is related to van't Hoff factor (i) by the expression

Options

A. `alpha=(i-1)/(x+y-1)`
B. `alpha=(i-1)/((x+y+1))`
C. `alpha=((x+y-1))/(i-1)`
D. `alpha=((x+y+1))/(i-1)`

Explanation

To derive the relationship between the degree of dissociation (α) of a weak electrolyte \( A_xB_y \) and the van't Hoff factor (i), we can follow these steps:

### Step 1: Understanding Weak Electrolytes
A weak electrolyte is a substance that does not completely dissociate into ions in solution. Only a fraction of it dissociates.

### Step 2: Writing the Dissociation Reaction
For a weak electrolyte \( A_xB_y \), the dissociation can be represented as:
\[
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