What is the silver ion concentration in a solution prepared by mixing 341 mL 0.388 M silver nitrate with 375 mL 0.506 M sodium chromate? The Ksp of silver chromate is 1.2*10^-12

Answer 1

Find the initial concentrations of silver and chromate after dilution from mixing

silver ion: .388 molar (341/(375+341))

chromate: .506 molar(375/(341+375))

The equilibrium is that [Ag⁺]²[CrO₄^2-] = Ksp

The equation for precipitation is 2Ag⁺ + CrO₄^2- → Ag₂CrO₄

Doing an ice diagram where x is the molarity of Ag⁺ precipitated, the final equilibrium is

[[Ag]₀⁺-x]²[[CrO₄^2-]₀ - x/2] = Ksp

You end up with a cubic equation for x (Just plug in (values - Ksp) and plot to find zeroes using Desmos or TI graphing)

answer is [Ag]₀⁺-x