JEE Main 2018 (Offline) | Ionic Equilibrium Question 100 | 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

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MCQ (Single Correct Answer)

-1

Following four solutions are prepared by mixing different volumes of NaOH and HCl of different concentrations, pH of which one of them will be equal to 1 ?

100 mL $${M \over {10}}$$ HCl + 100 mL $${M \over {10}}$$ NaOH

75 mL $${M \over {5}}$$ HCl + 25 mL $${M \over {5}}$$ NaOH

60 mL $${M \over {10}}$$ HCl + 40 mL $${M \over {10}}$$ NaOH

55 mL $${M \over {10}}$$ HCl + 45 mL $${M \over {10}}$$ NaOH

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MCQ (Single Correct Answer)

-1

Which of the following is a Lewis acid?

PH₃

B(CH₃)₃

NaH

NF₃