For AgCl, K_sp = 1.8 x 10^-10, and for Ag+ + 2NH3 leftharpoons [Ag(NH3)2]+, K_f = 1.6 x 10^7. The equilibrium constant of AgCl(s) + 2NH3 leftharpoons [Ag(NH3)2]+ + Cl- is

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For $AgCl$ , $K_{s p} = 1.8 \times 1 0^{- 10}$ , and for $Ag X^{+} + 2 NH X_{3} ⇌ [Ag (NH X_{3}) X_{2}] X^{+}$ , $K_{f} = 1.6 \times 1 0^{7}$ . The equilibrium constant of $AgCl (s) + 2 NH X_{3} ⇌ [Ag (NH X_{3}) X_{2}] X^{+} + Cl X^{-}$ is

The reaction is the sum of dissolution (constant

K_{s p}

) and complex formation (constant

K_{f}

), so

K = K_{s p} K_{f} = 1.8 \times 1 0^{- 10} \times 1.6 \times 1 0^{7} = 2.9 \times 1 0^{- 3}