JEE Main 2018 (Offline) | Ionic Equilibrium Question 81 | Chemistry

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

JEE Main 2018 (Offline)

MCQ (Single Correct Answer)

-1

An aqueous solution contains 0.10 M H₂S and 0.20 M HCl. If the equilibrium constants for the formation of HS^– from H₂S is 1.0 $$\times$$ 10^–7 and that of S^2- from HS^– ions is 1.2 $$\times$$ 10^–13 then the concentration of S^2- ions in aqueous solution is :

5 $$\times$$ 10^–19

5 $$\times$$ 10^–8

3 $$\times$$ 10^–20

6 $$\times$$ 10^–21

JEE Main 2018 (Offline)

MCQ (Single Correct Answer)

-1

Which of the following are Lewis acids?

BCl₃ and AlCl₃

PH₃ and BCl₃

AlCl₃ and SiCl₄

PH₃ and SiCl₄