- #1
Maharg
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Homework Statement
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).
Homework Equations
Ksp = [AgCl] I thinK?
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?