You have 420 mL of an aqueous solution that is 0.39 MNa2SO4 and a separate 185 mL aqueous solutionthat is 0.45 M BaCl2.
a). How many moles of each of the four ions are present ?
Na+
SO42-
Ba2+
Cl-
b). When these two solutions are mixed together, what is thechemical formula of the solid expected to precipitate from themixture?
c). If the sulfate ions in the mixed solution react with thebarium ions in the mixed solution to form a precipitate, how manymoles of Ba2+ ions are required to react with all of theSO42- ions present?
d). If the barium ions in the mixed solution react with the sulfateions in the mixed solution to form a precipitate, how many moles ofSO42- ions are required to react with all ofthe Ba2+ ions present?
e). Are barium ions or sulfate ions the limiting reactant in themixture?
f). How many grams of precipitate will form?
g). Draw chemical symbols of the ions that were spectators of thisprocess. Do the cation first, then the anion.
h). Will the mixture remaining after the precipitate formed beelectrolytic?
