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Question

Calculate the concentration (in mol L1) of hydroxide ion necessary to precipitate Mg(OH)2 from 0.1 M solution of MgSO4.

[Ksp of Mg(OH)2=5.5×1012]

A
7.4×106
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B
6.8×105
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C
7.4×107
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D
6.8×108
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Solution

The correct option is D 7.4×106
The concentration of magnesium ion in 0.1 M solution of magnesium sulphate is 0.1 M.
The solubility product of magnesium hydroxide is 5.5×1012.
Ksp=[Mg2+][OH]2
Substituting values in the above expression, we get
5.5×1012=(0.1)[OH]2

Hence, [OH]2=5.5×10120.1=5.5×1011

[OH]=5.5×1011=7.4×106

Hence, the minimum concentration of hydroxide ion necessary for the precipitation of Mg(OH)2 is 7.4×106 M.

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