Given that, Ka1=1.0×10−7 and Ka2=1.3×10−13 for H2S.
Find the concentration of S2− and HS− ions (in mol/L) respectively in the solution consisting of 0.1 M H2S and 0.5 M HCl.
For H2S :
Step 1 :
H2S(aq)⇌H+(aq)+ HS−(aq)
at t=0 C1 0 0
at t=teq C(1−α1) (Cα1α2+Cα1) Cα1(1−α2)
Step 2 :
HS−(aq)⇌H+(aq) + S2−(aq)
at t=teq Cα1(1−α2) (Cα1α2+Cα1) Cα1α2
[H+]total=0.5+Cα1+Cα1α2
SInce α1,α2 are very less for weak acid H2S and α1×α2 is even a lesser value than α1. Also, strong acid HCl suppresses the ionization of H2S due to common ion effect. The concentration of H+ can be taken only due to HCl.
∴[H+]total≈0.5 M