Don't you believe in arrows?
K for your reaction =
(Cl^-)[Ag(NH3)2^+]/(NH3)2^2(AgCl)(s)
which is just k1*k2.
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
3 answers
Bob is right, its k1 times k2 which is D: 2.4x10^-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