Silver chloride is classified as an insoluble compound because it dissolves only to a small extent in water. Consider the balanced equation and equilibrium constant that shows the partial dissolving of silver chloride in water: AgCl(s) = Ag*(aq) + CI"(aq) Keg = 1.70 x 10-10 a) The reaction AgCl(s) = Ag(ag) + CI (ag) is classified as a (homogeneous or heterogeneous) equilibrium because involves more than one physical state, solid and aqueous. b) Based on the equilibrium constant value and the equilibrium constant expression, the concentration of each ion in a saturated solution of silver chloride is : Concentration of Agt= х 10 Concentration of Cl" = x 10 M

Silver chloride is classified as an insoluble compound because it dissolves only to a small extent in water. Consider the balanced equation and equilibrium constant that shows the partial dissolving of silver chloride in water: AgCl(s) = Ag*(aq) + CI"(aq) Keg = 1.70 x 10-10 a) The reaction AgCl(s) = Ag(ag) + CI (ag) is classified as a (homogeneous or heterogeneous) equilibrium because involves more than one physical state, solid and aqueous. b) Based on the equilibrium constant value and the equilibrium constant expression, the concentration of each ion in a saturated solution of silver chloride is : Concentration of Agt= х 10 Concentration of Cl" = x 10 M

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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