Q.2 Answer the following questions on dissolution equilibrium. 2-1) The following ionic compounds are precipitated from aqueous solutions of the ions shown in the parentheses. Give the equations for the equilibria, and show the relationships between the ion concentrations and the solubility products. MnS(Mn2+,S2)Ag2CrO4(Ag+,CrO42)Hg2Cl2(Hg22+,Cl) 2-2) Calculate the solubilities ( gL1 ) of MnS,Ag2CrO4, and Hg2Cl2 using the solubility products listed below. Use the following values if necessary: Ag=107.9,Cl=35.5,Cr= 52.0,Hg=200.6,Mn=54.9,O=16.0,S=32.1 MnS:8.01014mol2L2 Ag2CrO4:1.21012mol3L3 Hg2Cl2:1.21018mol3L3 2-3) An aqueous solution of Mn2+(1.0102molL1) was saturated with H2S. A saturated aqueous solution of H2S has a concentration of [H2S]=1.0101molL1. Calculate the pH range where precipitation occurs. Note that the acid dissociation constants of H2S are K1=9.0108 and K2=1.21015