What is the minimum concentration of Ba+2 ions required in order to initiate the precipitation of BaSO4 from a solution containing 0.002molL−1 of SO−24 ions? (Given Ksp for BaSO4=1.4×10−10 )
A
1.7×10−7M
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B
2.7×10−7M
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C
7.0×10−8M
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D
7.0×10−10M
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Solution
The correct option is C7.0×10−8M If ionic product of [Ba+2][SO−24] is greater than Ksp for BaSO4, then the precipitation occur. [Ba+2][SO−24]>1.4×10−10 In a saturated solution [Ba+2]×(2×10−3)=1.4×10−10 [Ba+2]=0.7×10−7molL−1 Thus, minimum concentration of Ba+2 ions required for the precipitation of BaSO4 is 0.7×10−7M.