The solubility of Ag(I) in aqueous solutions containing different concentrations of Cl₂ is based on the following equilibria:Ag⁺(aq) + Cl⁻(aq) ⇄ AgCl(s) Ksp=1.8x10⁻¹Ag⁺(aq) + 2Cl⁻(aq) ⇄ AgCl₂⁻(s) Kf=1.8x10⁵When solid AgCl is shaken with a solution containing Cl⁻, Ag(I) is present as both Ag⁺ and AgCl₂⁻. The solubility of AgCl is the sum of the concentrations of Ag⁺ and AgCl₂⁻.(a) Show that [Ag⁺] in solution is given by[Ag⁺] = 1.8x10⁻¹⁰ / [Cl⁻]and that [AgCl₂⁻] in solution is given by[AgCl₂⁻] = (3.2x10⁻⁵) ([Cl⁻])