Ionic Equilibrium

The solubility in water of a sparingly soluble salt AB₂ is 1.0 $\times$ 10⁻⁵ mol L⁻¹. Its solubility product number will be :

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 :

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 :

In a sautrated solution of the sparingly soluble strong electrolyte AgIO₃ (Molecular mass = 283) the equilibrium which sets in is AgIO_3(s) $\leftrightharpoons$ Ag⁺(aq) + $IO_3^-$ If the solubility product constant K_sp of AgIO₃ at a given temperature is 1.0 $\times$10^−8, what is the mass of AgIO₃ contained in 100 ml of its saturated solution?

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 )

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 :

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⁺?

The minimum volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution (K_sp of PbCl₂ = 3.2 $\times$ 10⁻⁸ atomic mass of Pb = 207 u ) is :

If solublity product of Zr₃(PO₄)₄ is denoted by K_sp and its molar solubility is denoted by S, then which of the following relation between S and K_sp is correct ?

The molar solubility of Cd(OH)₂ is 1.84 × 10^–5 M in water. The expected solubility of Cd(OH)₂ in a buffer solution of pH = 12 is :