Considering the following equilibria in an aqueous solution: (1) Ag+ +Cl- <---> AgCl(aq) K=2.0 * 10^3 (2) AgCl(aq) + Cl- <---> AgCl2 - K=93 (3) AgCl(s) <---> Ag+ + Cl- K=1.8*10^-10 (a) Find K for the reaction AgCl(s) <---> AgCl(aq). The species AgCl(aq) is an ion pair consisting of Ag+ and Cl- associated with each other in solution  (b) Find (AgCl(aq)) in equilibrium with excess AgCl(s).  (c) Find K  for AgCl2 - <---> AgCl(s) +Cl-.

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.