**Equilibrium Constant Expression for Silver Chloride Dissociation**When writing the expression for the equilibrium constant for the dissociation of a solid substance into its aqueous ions, it is important to remember that solids are not included in the equilibrium expression. Only the concentrations of aqueous ions are included. Consider the reaction:\[ \text{AgCl} (\text{s}) \rightleftharpoons \text{Ag}^+ (\text{aq}) + \text{Cl}^- (\text{aq}) \]Here, silver chloride (\( \text{AgCl} \)) is a solid, and it dissociates into silver ions (\( \text{Ag}^+ \)) and chloride ions (\( \text{Cl}^- \)) in the aqueous phase.The equilibrium constant expression (K\(_{eq}\) or \( K_{sp} \) for solubility product) for this dissociation is written as:\[ K_{sp} = [\text{Ag}^+][\text{Cl}^-] \]In this expression:- \( [\text{Ag}^+] \) represents the molar concentration of silver ions in solution.- \( [\text{Cl}^-] \) represents the molar concentration of chloride ions in solution.Since \( \text{AgCl} \) is a solid, its concentration does not appear in the equilibrium expression.

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Answered: Write the expression for the…

Write the expression for the equilibrium constant for the reaction represented by the equation: AgCl (s) Ag+ (aq) + Cl¯ (aq)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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