chemistry

The solubility of silver chloride can be increased by dissolving it in a solution containing ammonia.
AgCl (s) Ag+ (aq) + Cl- (aq) K1 = 1.6 x 10-10
Ag+ (aq) + 2NH3 (aq) Ag(NH3)2+ (aq) K2 = 1.5 x 107

What is the value of the equilibrium constant for the overall reaction?
AgCl (s) + 2NH3 (aq) Ag(NH3)2+ (aq) + Cl- (aq) Knet = ?

A. 1.5 x 107

B. 2.3 x 1014

C. 2.4 x 107

D. 2.4 x 10-3

E. 3.1 x 10-3

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  1. Don't you believe in arrows?
    K for your reaction =
    (Cl^-)[Ag(NH3)2^+]/(NH3)2^2(AgCl)(s)
    which is just k1*k2.

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  2. Bob is right, its k1 times k2 which is D: 2.4x10^-3

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  3. Since K1 and K2 equation are arrange properly to form the overall reaction, you just need to multiply both value of (k1*k2)=2.4*10^-3

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