Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R). Assertion (A): Ag ₂ CrO ₄ ( K_ sp = 3.2 10⁻¹¹ ) is more soluble in water than AgCl ( K_ sp = 1.0 10⁻¹⁰ ). Reason (R): For sparingly soluble salts, a higher numerical value of K_ sp always implies a higher molar solubility. In the light of the above statements, choose the most appropriate answer from the options g

Step-by-step solution

Let s be the molar solubility. For AgCl (an AB type salt): K_ sp = s^2 s = 1.0 10⁻¹⁰ = 1.0 10⁻⁵ M For Ag ₂ CrO ₄ (an A ₂ B type salt): K_ sp = (2s)^2(s) = 4s^3 4s^3 = 3.2 10⁻¹¹ = 32 10⁻¹² s^3 = 8.0 10⁻¹² s = 2.0 10⁻⁴ M Comparing the solubilities, 2.0 10⁻⁴ M > 1.0 10⁻⁵ M . Thus, Ag ₂ CrO ₄ is more soluble than AgCl , making the Assertion (A) correct. The Reason (R) is incorrect because K_ sp values can only be directly compared to determine relative solubilities if the salts have the same stoichiometry. As shown her