1. The problem statement, all variables and given/known data Consider the following equilibria at T = 26 0C, in which all ions are aqueous: Ag+(aq) + Cl-(aq) ----> AgCl(aq) K1 = 2.0E2 AgCl(s) ----> Ag+(aq) + Cl-(aq) K2 = 1.9E-10 Consider the reaction AgCl(s) ----> AgCl(aq) and calculate the concentration of AgCl(aq) in equilibrium with excess undissolved solid AgCl(s). Hint: calculate K3 first and use the equilibration constant expression to find the concentration of AgCl(aq). 2. Relevant equations Ksp = [AgCl] I thinK? 3. The attempt at a solution So I think I'm on the right track but missing something To get k3 is just combining k1 and k2, Since they easily cancel out to make AgCl(s) -> AgCl (aq), I think k3 is just 200 + 1.9E-10 = 200 k3 = 200? That seems odd but then even if that is true I'm not sure which is next as with solubility I've always had problems where it is Ksp=[A], but this one is just Ksp=[A] as solids wouldn't count right?