An analysis of a saturated solution of silver chromate, Ag2CrO4, reveals that the concentration of Ag+ is 1.3 x 10-4 Molar. What is the Ksp of Ag2CrO4? A. 2.3 x 10-12 B. 8.8 x 10-12 C. 1.9 x 10-8 D. 1.3 x 10-4 E. 3.1 x 10-4

B. 8.8 x 10⁻¹²

Explanation:

In aqueous solution, silver chromate (Ag₂CrO₄) dissociates into ions as follows:

Ag₂CrO₄(s) ⇄ 2 Ag⁺(aq) + CrO₄²⁻(aq)

                       2s               s

So, the expression of the Ksp of Ag₂CrO₄ is derived from the concentrations of the ions at equilibrium raised by the stoichiometric coefficients:

Ksp = [Ag⁺]²[CrO₄²⁻] = (2s²)s = (4s²)s = 4s³

Since s = [Ag⁺] = 1.3 x 10⁻⁴ M, we calculate the Ksp as follows:

Ksp = 4s³= 4(1.3 x 10⁻⁴)³ = 8.79 x 10⁻¹² M

Therefore, the correct option is B. 8.8 x 10⁻¹²

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