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

Don't you believe in arrows?

K for your reaction =
(Cl^-)[Ag(NH3)2^+]/(NH3)2^2(AgCl)(s)
which is just k1*k2.

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

To find the value of the equilibrium constant for the overall reaction, we can use the concept of equilibrium constant expressions. The equilibrium constant for the overall reaction is given by the product of the equilibrium constants for the individual steps of the reaction.

The overall reaction is:
AgCl (s) + 2NH3 (aq) ⇌ Ag(NH3)2+ (aq) + Cl- (aq)

First, let's write down the equilibrium constant expressions for the individual steps:

Step 1: AgCl (s) ⇌ Ag+ (aq) + Cl- (aq) (K1 = 1.6 x 10^(-10))

Step 2: Ag+ (aq) + 2NH3 (aq) ⇌ Ag(NH3)2+ (aq) (K2 = 1.5 x 10^7)

Now, multiply the equilibrium constant expressions for the individual steps to get the equilibrium constant expression for the overall reaction:

Knet = K1 * K2

Substituting the given values of K1 and K2:

Knet = (1.6 x 10^(-10)) * (1.5 x 10^7)
= 2.4 x 10^(-3)

Therefore, the value of the equilibrium constant for the overall reaction (Knet) is 2.4 x 10^(-3).

So, the correct answer is D. 2.4 x 10^(-3).