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Question

Given that, Ka1=1.0×107 and Ka2=1.3×1013 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.

A
5.2×1021 and 2×108
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B
1.0×1018 and 2.3×106
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C
6.5×1019 and 1.3×107
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D
4.6×1020 and 1.3×108
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Solution

The correct option is A 5.2×1021 and 2×108
H2SS2 + 2H+ HClCl+H+ Common ion

For H2S :

Step 1 :

H2S(aq)H+(aq)+ HS(aq)

at t=0 C1 0 0

at t=teq C(1α1) (Cα1α2+Cα1) Cα1(1α2)

Step 2 :

HS(aq)H+(aq) + S2(aq)

at t=teq Cα1(1α2) (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+]total0.5 M


H2SH++HS Ka1=1.0×107HSH++S2 Ka2=1.3×1013

Ka1=[H+][HS][H2S]1.0×107=(0.5)[HS]0.1[HS]=1.0×107×0.10.5=2×108 MKa2=[H+][S2][HS]1.3×1013=(0.5)[S2]2×108[S2]=1.3×1013×2×1080.5[S2]=5.2×1021M

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