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Question

An aqueous solution of metal bromide,MBr2(0.05 M) is saturated with H2S. What is the minimum pH at which MS will precipitate? Ksp for MS=6.0×1021, concentration of saturated H2S=0.1 M. K1=107and K2=1.3×1013 for H2S
log 1.04=0.017

A
0.98
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B
0.45
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C
1.2
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D
0.02
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Solution

The correct option is A 0.98
Minimum concentration of S2 ions required to precipitate MS is

[S2]=KspMS[M2+]

=6.0×10210.05=1.2×1019 M

H2S ionizes in solution in following steps

H2SH++HS; K1=107

HSH++S2; K2=1.3×1013

As K1=[H+][HS][H2S]

K2=[H+][S2][HS]

So K1 K2=[H+]2[S2][H2S]

[H+]2=K1K2[H2S][S2]

=107×1.3×1013×0.11.2×1019

=1.08×102

[H+]=1.04×101
pH=log10 [H+]
=log10(1.04×101)
=1log 1.04
=0.98

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