Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), K1 = 9.57×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), K2 = 1.46×10−19, what is the equilibrium constant Kfinal for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq) Enter your answer numerically.

The value of for the final 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 final reaction is

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.