For `C' molar solution of weak electrolyte \( A_xB_y \), dissociation constant is \( K \), then degree of dissociation of \( A_xB_y \) at equilibrium is
Show Hint
For a weak electrolyte, always use the approximation \(1-\alpha \approx 1\) because the degree of dissociation is very small. Then substitute equilibrium concentrations carefully in the dissociation constant expression.
Step 1: Write the dissociation of the weak electrolyte.
The weak electrolyte \( A_xB_y \) dissociates as:
\[
A_xB_y \rightleftharpoons xA^{\cdots} + yB^{\cdots}
\]
If the initial concentration of the electrolyte is \( C \) molar and the degree of dissociation is \( \alpha \), then at equilibrium:
\[
[A_xB_y] = C(1-\alpha)
\]
\[
[A] = xC\alpha
\]
\[
[B] = yC\alpha
\]
Step 2: Write the expression for dissociation constant.
The dissociation constant is:
\[
K = \frac{[A]^x[B]^y}{[A_xB_y]}
\]
Substituting the equilibrium concentrations:
\[
K = \frac{(xC\alpha)^x (yC\alpha)^y}{C(1-\alpha)}
\]
Step 3: Simplify the expression.
Expanding the numerator:
\[
K = \frac{x^x y^y C^{x+y}\alpha^{x+y}}{C(1-\alpha)}
\]
\[
K = \frac{x^x y^y C^{x+y-1}\alpha^{x+y}}{(1-\alpha)}
\]
Since \( A_xB_y \) is a weak electrolyte, its degree of dissociation is very small, so:
\[
1-\alpha \approx 1
\]
Therefore:
\[
K = x^x y^y C^{x+y-1}\alpha^{x+y}
\]
Step 4: Solve for degree of dissociation \( \alpha \).
Rearranging the equation:
\[
\alpha^{x+y} = \frac{K}{C^{x+y-1}x^x y^y}
\]
Taking power \( \dfrac{1}{x+y} \) on both sides:
\[
\alpha = \left(\frac{K}{C^{x+y-1}x^x y^y}\right)^{\frac{1}{x+y}}
\]
Step 5: Match with the given options.
This expression matches option (A). Hence, the required degree of dissociation at equilibrium is:
\[
\left(\frac{K}{C^{x+y-1}x^x y^y}\right)^{\frac{1}{x+y}}
\]
Final Answer: (A) \(\left(\dfrac{K}{C^{x+y-1}x^x y^y}\right)^{\frac{1}{x+y}}\)