[Tunechi]

Calculate the equilibrium constant for the reaction
HS(aq) + H2O(L) ------> H2S(aq) + Oh-(aq)
given that ka1 = 1.3 x 10^-7 and ka2 = 7.1 x 10^-15

Basically i looked at all the equation and concepts that i know and i don't know what approach to use on this question, its given me ka1 and ka2 which are equilibrium constants? How do i find k

k = [H2s][Oh]/[HS]

no concentrations, nothing? I tried finding the pka but idk what to do with the pkas??

Any help would be appreciated

The right answer is 7.7 x 10^-8 but i have no clue how to get it

[ramboacid]

In your equation, HS^- is acting as a base when it converts into H₂S, so you can't go about this using purely K_a values because Ka values describe acid dissociation reactions.

What is the relationship between the equilibrium constants for the reactions
HA H⁺ + A^- and H⁺ + A^-  HA
where HA is a generic acid, and A^- is the conjugate base?