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Question

2.5 mL of 25 M weak monoacidic base (Kb=1×1012) at 25o C is titrated with 215 M HCl in water at 25oC. The concentration of H+ at equivalence points is (Kw=1×1014 at 25o C)

A
3.7×1013 M
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B
3.2×107 M
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C
3.2×102 M
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D
2.7×102 M
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Solution

The correct option is C 3.2×102 M
Given, [BOH=25 M, Kb=1×1012, [HCl]=215 M, Kw=1×1014 at 25o C
N1V1Base=N2V2Acid
2.5×25=215×V2
or V2(acid)=152=7.5 mL
BOH+HClBCl+H2O
millimoles of BOH=2.5×25=1 mmol
salt BCl formed = 1 mmol
Total volume of solution =2.5+7.5=10 mL=10×103 L
[BCl] in solution =1×10310×103=0.1 M
For the salt of weak base and the strong acid
[H+]=KwCKb=1014×0.11012
[H+]=3.2×102M

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