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What is the minimum concentration of SO₄^2– required to precipitate BaSO₄ in a solution containing 1.0 × 10^–4 mole/lit of Ba²⁺ ? (K_sp of BaSO₄ = 4 × 10^–10)

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$4\, \times \,{10^{ - 10}}M$

$\large 2\, \times \,{10^{ - 5}}M$

$2\, \times \,{10^{ - 3}}M$

$4\, \times \,{10^{ - 6}}M$

answer is C.

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Detailed Solution

For precipitation, $\large {K_{IP}} \geqslant {K_{sp}}$

$\large OR\left [ {B{a^{ + 2}}} \right] \times \left[ {SO_4^{ - 2}} \right] = 4 \times {10^{ - 10}}$

$\large \Rightarrow {10^{ - 4}} \times \left[ {SO_4^{ - 2}} \right] = 4 \times {10^{ - 6}}$

$\large \Rightarrow \left[ {SO_4^{ - 2}} \right] = 4 \times {10^{ - 6}}$

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