An aqueous solution contains an unknown concentration of Ba2+. When 50 mL of a 1 M solution of Na2SO4 is added, BaSO4 just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO4 is 1 $\times$ 10–10. What is the original concentration of Ba2+?

Question

An aqueous solution contains an unknown concentration of Ba²⁺. When 50 mL of a 1 M solution of Na₂SO₄ is added, BaSO₄ just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO₄ is 1 $\times$ 10^–10. What is the original concentration of Ba²⁺?

1.0 $\times$ 10^–10 M

5 $\times$ 10^–9 M

2 $\times$ 10^–9 M

1.1 $\times$ 10^–9 M

Solution

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