Question

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

• A. \(\left(\dfrac{K}{C^{x+y-1}x^x y^y}\right)^{\frac{1}{x+y}}\)
• B. \(\left(\dfrac{K \times C^{x+y-1}}{x^x - y^y}\right)^{\frac{1}{x+y}}\)
• C. \(\left(\dfrac{K \cdot x^x \cdot y^y}{C^{x+y-1}}\right)^{\frac{1}{x+y}}\)
• D. \(\left(\dfrac{K \times C^{x+y-1}}{x^x \times y^y}\right)^{x+y}\)

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.

Answer 1

The Correct Option is A