AIEEE 2005 | Ionic Equilibrium Question 133 | Chemistry

The solubility product of a salt having general formula MX₂, in water is: 4 $$\times$$ 10^-12 . The concentration of M²⁺ ions in the aqueous solution of the salt is :

2.0 $$\times$$ 10^-6 M

4.0 $$\times$$ 10^-10 M

1.0 $$\times$$ 10^-4 M

1.6 $$\times$$ 10^-4 M

AIEEE 2005

MCQ (Single Correct Answer)

-1

Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be :

3.98 $$\times$$ 10^-6

3.68 $$\times$$ 10^-6

3.88 $$\times$$ 10⁶

3.98 $$\times$$ 10⁸

AIEEE 2004

MCQ (Single Correct Answer)

-1

The molar solubility (in ol L^-1) of a sparingly soluble salt MX₄ is "s". The corresponding solubility product is K_sp. 's' is given in term of K_sp by the relation :

s = (256 K_sp)^1/5

s = (128 K_sp)^1/4

s = ( K_sp / 128)^1/4

s = (K_sp / 256)^1/5

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