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Question

A solution contains 0.1 M H2S and 0.3 M HCl. Given Ka1 and Ka2 for H2S are 107 and 1.8×1013 respectively. If the concentration of HS ions is x×108 M, then what is the value of x? (Give your answer upto two decimal points)

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Solution

H2SH++HSKa1=[H+][HS][H2S]......(i)Further HSH++S2Ka2=[H+][S2][HS].......(ii)
Multiplying both the equation
Ka1×Ka2=[H+]2[S2][H2S]
Due to common ion, the ionisation of H2S is suppresesed and the [H+] in solution is due to the presence of 0.3 M HCl.
[S2]=Ka1×Ka2[H2S][H+]2=1.0×107×1.8×1013×(0.1)(0.3)2 =2×1020M
Putting the value of [S2] in eq. (ii)
1.8×1013=0.3×2×1020[HS]or [HS]=0.3×2×10201.8×1013=3.33×108 M

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