Silver chromate is sparingly soluble in aqueous solutions. The 𝐾sp of Ag2CrO4 is 1.12×10−12 .

Question

What is the solubility (in mol/L) of silver chromate in 1.00 M silver nitrate aqueous solution?

Answer 1

This is a common ion effect problem. The common ion is Ag⁺ (silver ion). We use 1.00 M as the [Ag⁺] in our calculations.

Ag₂CrO₄(s) <==> 2Ag⁺(aq) + CrO4^2-(aq)

Ksp = [Ag⁺]²[CrO₄^2-]

1.12x10^-12 = [1.00]² [CrO₄^2-]

[CrO₄^2-] = 1.12x10^-12 M (moles/L) = solubility of Ag₂CrO₄