Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), H2S(aq)⇌HS−(aq)+H+(aq), K1K1K_1 = 9.39×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), HS−(aq)⇌S2−(aq)+H+(aq), K2K2K_2 = 1.45×10−19, what is the equilibrium constant KfinalKfinalK_final for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq)

The value of for the net reaction is

Explanation:

The given chemical equations follows:

Equation 1:  

Equation 2:  

The net equation follows:

As, the net reaction is the result of the addition of reverse of first equation and the reverse of second equation. So, the equilibrium constant for the net reaction will be the multiplication of inverse of first equilibrium constant and the inverse of second equilibrium constant.

The value of equilibrium constant for net reaction is:

We are given:  

Putting values in above equation, we get:

Hence, the value of for the net reaction is

50.23 i believe is correct but don't quote me on that.