AIEEE 2010 | Ionic Equilibrium Question 95 | Chemistry

At 25°C, the solubility product of Mg(OH)₂ is 1.0 $$\times$$ 10^–11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001 M Mg²⁺ ions?

AIEEE 2010

MCQ (Single Correct Answer)

-1

Solubility product of silver bromide is 5.0 $$\times$$ 10^–13. The quantity of potassium bromide (molar mass taken as 120g of mol^–1) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is :

1.2 $$\times$$ 10^–10 g

1.2 $$\times$$ 10^–9 g

6.2 $$\times$$ 10^–5 g

5.0 $$\times$$ 10^–8 g

AIEEE 2009

MCQ (Single Correct Answer)

-1

Solid Ba(NO₃)₂ is gradually dissolved in a 1.0 $$\times$$ 10^-4 M Na₂CO₃ solution. At what concentration of Ba²⁺ will a precipitate begin to form ?
(K_sp for BaCO₃ = 5.1 $$\times$$ 10⁻⁹ )

5.1 $$\times$$ 10^-5 M

8.1 $$\times$$ 10^-8 M

8.1 $$\times$$ 10^-7 M

4.1 $$\times$$ 10^-5 M

AIEEE 2008

MCQ (Single Correct Answer)

-1

Four species are listed below
i. $$HCO_3^−$$
ii. $$H_3O^+$$
iii. $$HSO_4^−$$
iv. $$HSO_3F$$
Which one of the following is the correct sequence of their acid strength?

iv < ii < iii < I

ii < iii < i < iv

i < iii < ii < iv

iii < i < iv < ii

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