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JEE Main20265 April 2026Morning ShiftChemistryIonic EquilibriumActual

M₃ A₂ is a sparingly soluble salt of molar mass y g mol ⁻¹ and solubility x g L ⁻¹ . The ratio of the molar concentration of the anion ( A³⁻ ) to the solubility product of the salt is

Options

  1. A1 54 y^4 x^4
  2. By^5 108 x^4
  3. C108 x^5 y^5
  4. D1 108 y^4 x^4

Correct answer

A. 1 54 y^4 x^4

Step-by-step solution

The molar solubility S of the salt is given by S = x y mol L ⁻¹ . The dissociation of the sparingly soluble salt M₃A₂ is: M₃A₂ 3M²⁺ + 2A³⁻ The molar concentration of the anion A³⁻ is: [A³⁻] = 2S The solubility product K_ sp of the salt is: K_ sp = [M²⁺]^3 [A³⁻]^2 = (3S)^3 (2S)^2 = 27S^3 4S^2 = 108S^5 The ratio of the molar concentration of the anion to the solubility product is: [A³⁻] K_ sp = 2S 108S^5 = 1 54S^4 Substituting S = x y into the expression, we get: Ratio = 1 54 ( x y )^4 = 1 54 y^4 x^4 Answer: 1 54 y^4

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