Question

Write the balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous Nal. Include phases. chemical equation: Pb(ClO3)2(aq) + 2Nal(aq) PbL_(s) + 2NaClO2 (aq) What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3)2 is mixed with 0.700 L 0.150 M Nal? Assume the reaction goes to completion. mass of precipitate: g

Answer 1

Page No, I D The balanced chemical reaction of aqueous Pb(ClO3), and aqueous Nal Bor reaction is i Pb(Clos), (aq) + 2 Na I (05) → Pb 12(3)+2 Nallo,y) 2 2) Given : volume of Pb(ClO3) = 1.50L Volume of Nar = 0.700L Concentration of NaI 1.50 M L 0, 700 L X 1.50 mall number of moles of Na I - 1.05 moles. from balanced equation n moles of Pb Iz (3) = 1/2 x moles of Na Ikea) reacting 1 X 1.05 moles 2 0.525 moles Now, molar mass of Pb Iz = H61 g/mal

Page No. 2 mass of Pb I 2 (3) formed molar mass of Polze 0.525 moles = 0.525 moles X 461 g/mal mass of PSI21s) Formed 242 g Hence, mass of precipitate famed assuming reaction goes to completion is 242 g