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Question

The solubility product of a sparingly soluble salt Ca(IO3)2 is 6.5×106. Its solubility value in (molL1) is:
(1.63)13=1.17

A
1.2×104
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B
1.63×106
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C
1.2×102
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D
None of the above
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Solution

The correct option is C 1.2×102
Given Ksp=6.5×106
The dissociation equation is Ca(IO3)2(s)Ca2+(aq)+2IO3(aq) 1 0 0 1s s 2s

Ksp=[Ca2+][IO3]2
Ksp=s×(2s)2=4s3
Ksp=4s3=6.5×106
4s3=6.5×106
s3=1.63×106
s=0.017 M


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