Question

You have 420 mL of an aqueous solution that is 0.39 M Na₂SO₄ and a separate 185 mL aqueous solution that is 0.45 M BaCl₂.

a). How many moles of each of the four ions are present ?
Na⁺

SO₄^2-

Ba²⁺

Cl^-

b). When these two solutions are mixed together, what is the chemical formula of the solid expected to precipitate from the mixture?

c). If the sulfate ions in the mixed solution react with the barium ions in the mixed solution to form a precipitate, how many moles of Ba²⁺ ions are required to react with all of the SO₄^2- ions present?

d). If the barium ions in the mixed solution react with the sulfate ions in the mixed solution to form a precipitate, how many moles of SO₄^2- ions are required to react with all of the Ba²⁺ ions present?

e). Are barium ions or sulfate ions the limiting reactant in the mixture?

f). How many grams of precipitate will form?
g). Draw chemical symbols of the ions that were spectators of this process. Do the cation first, then the anion.
h). Will the mixture remaining after the precipitate formed be electrolytic?

Answer 1