Question

A reaction will occur for the following in aqueous solution. This means that an insoluble product will be formed, but only one of the products is insoluble.

Na₂SO_{4 (aq)} + AgNO_{3 (aq)} → ?

If 17.5 g of Na₂SO₄ and 29.4 g of AgNO₃ are reacted, what mass of the insoluble product is formed?

Answer 1

Na₂SO_{4 (aq)} + AgNO_{3 (aq)} → Ag2SO4(s) + 2NaNO3(aq)

no of moles of Na2So4 = W/G.M.Wt

                                       = 17.5/142   = 0.123 moles

no of moles of AgNO3   = W/G.M.Wt

                                      = 29.4/170   = 0.173 moles

1 mole of AgNO3 react with 1 mole of Na2SO4

0.173 moles of AgNO3 react with 0.173 moles of Na2SO4

    Na2SO4 is limiting reactant

1 mole of Na2SO4 react with AgNO3 to gives1 mole Ag2SO4

0.123 moles of Na2SO4 react with AgNO3 to gives = 1*0.123/1 = 0.123 moles of Ag2SO4

mass of Ag2SO4 = no of moles * gram molar mass

                                 = 0.123*311.8   = 38.35g of Ag2SO4 >>>>>answer