Concept:The solubility product constant (\( K_{sp} \)) is the equilibrium constant for a solid substance dissolving in an aqueous solution, representing the product of dissolved ion concentrations.
Formula:$$ K_{sp} = [\text{Cation}]^x [\text{Anion}]^y $$
Solution:- For the dissolution of \( \text{AgCl} \), the equilibrium expression is initially \( K_c = \frac{[\text{Ag}^+][\text{Cl}^-]}{[\text{AgCl}]} \).
- Because \( \text{AgCl} \) is a pure solid, its concentration is constant and incorporated into the equilibrium constant.
- This creates the new constant \( K_{sp} = [\text{Ag}^+][\text{Cl}^-] \).
Why other options are incorrect:Solid reactants are never included in the denominator of a \( K_{sp} \) expression, eliminating A and B. Option D ignores the ions completely.
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