log K1 for Ag(NH3)2+ is 3.32 and log K2 is 3.91, what is Kf? Hint: Solve this equation first before solving for the overall equilibrium constant.

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If log K1 for Ag(NH3)2+ is 3.32 and log K2 is 3.91, what is Kf?

Hint: Solve this equation first before solving for the overall equilibrium constant.

Formation of soluble silver-ammonium complex, in an
AgCl solution, occurs in a 3-step process:
AgCI(s)= Ag* (aq) + CH(aq)
Ag*(aq) + NH,(aq) AGNH, (aq)
AGNH, (aq) + NH,(aq) = Ag(NH3)2'(aq) K2
K,
where K, is the solubility product for AgCl and K, & K2
are the equilibrium constants for the complex formation.
The over-all formation constant (K,) for the Ag(NH,),"
complex is equal to K, x K2.
Transcribed Image Text:Formation of soluble silver-ammonium complex, in an AgCl solution, occurs in a 3-step process: AgCI(s)= Ag* (aq) + CH(aq) Ag*(aq) + NH,(aq) AGNH, (aq) AGNH, (aq) + NH,(aq) = Ag(NH3)2'(aq) K2 K, where K, is the solubility product for AgCl and K, & K2 are the equilibrium constants for the complex formation. The over-all formation constant (K,) for the Ag(NH,)," complex is equal to K, x K2.
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