Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), K1 = 9.76×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), K2 = 1.22×10−19, what is the equilib
2 answers:
Answer:
Explanation:
Hello,
In this case, the equilibrium constant is asked for the following reaction:
S2−+2H+⇌H2S
Thus, by means of the given equilibrium constants and reactions, a suitable combination results by:
1. Inverting:
H2S(aq)⇌HS−(aq)+H+(aq)
as
HS−(aq)+H+(aq) ⇌ H2S(aq)
2. Inverting:
HS−(aq)⇌S2−(aq)+H+(aq)
as
S2−(aq)+H+(aq)⇌HS−(aq)
Thus, by adding them we obtain:
HS−(aq)+H+(aq)+S2−(aq)+H+(aq)⇌HS−(aq)+H2S(aq)
Resulting in:
S2−(aq)+2H+(aq)⇌H2S(aq)
Which is simplified but proposing it law of mass action it turns out:
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