MHT CET202618 April 2026Morning ShiftChemistryIonic EquilibriumActual
The solubility of a sparingly soluble a salt AB ₂ is 1 10⁻⁶ mol/dm ^3 . Calculate its solubility product?
Options
- A1 10⁻¹²
- B2 10⁻¹²
- C3 10⁻¹²
- D4 10⁻¹⁸
Correct answer
D. 4 10⁻¹⁸
Step-by-step solution
The dissociation of the salt AB₂ is given by: AB₂ A²⁺ + 2B^- Let the solubility of the salt be S . The equilibrium concentrations are: [A²⁺] = S [B^-] = 2S The solubility product K_ sp is: K_ sp = [A²⁺][B^-]^2 K_ sp = (S)(2S)^2 = 4S^3 Given S = 1 10⁻⁶ mol/dm ^3 , substituting this value: K_ sp = 4(1 10⁻⁶)^3 K_ sp = 4 10⁻¹⁸ Answer: 4 10⁻¹⁸