Silver ions are added to a solution with [Br−]=[Cl−]=[CO2−3]=[AsO3−4]=0.1M. Which compound will precipitate with lowest [Ag+]? Silver ions are added to a solution with [Br−]=[Cl−]=[CO2−3]=[AsO3−4]=0.1M. Which compound will precipitate with lowest [Ag+]? November 17, 2020 Category: Chapter 6 - Ionic Equilibrium (Level 1 and Level 2) , Chapter 7 - Equilibrium , N Awasthi Physical Chemistry , Facebook Messenger WhatsApp Share this:TwitterFacebook Related A solution contains 0.1M is Cl− and 10^−4 M CrO2−4. If solid AgNO3 is gradually added to this solution, what will be the concentration of Cl− when Ag2CrO4 begins to precipitate? (Ksp(AgCl)=10^−10M^2, Ksp(Ag2CrO4)=10^−12M^3)AgBr(s)+2S2O2−3(aq)⇔[Ag(S2O3)2]3−(aq)+Br−(aq) [Ksp(AgBr)=5×10^−13, Kf[Ag(S2O3)2]3−=5×10^13] What is the molar solubility of AgBr in 0.1M Na2S2O3?Assertion: Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate AgBr rather than AgCl. Reason : Ksp of AgCl
