I could not find any method to approach this question.. it stumped me.. am I missing something simple?

Using the value of Ksp for Ag_{2}S, the Ka1 and Ka2 for H_{2}S, and the Kf for AgCl_{2}^{-}; calculate the equilibrium constant for the following reaction:

Ag_{2}S_{(aq)}+ 4Cl^{-}_{(aq)} + 2 H^{+}_{(aq)} <---> 2 AgCl_{2}^{-}_{(aq)} + H_{2}S_{(aq)}

I know you can get the molar solubility for Ag_{2}S, and that the Kf for AgCl_{2}^{-} is 1.1 x 10^{5}... but I have no idea how this helps me reach the equilibrium constant???

Any help is greatly appreciated..