If a solution containing 35.36 g of mercury(II) acetate is allowed to react completely with a solution containing 5.102 g of sodium sulfide. How many grams of solid precipitate will be formed?

How many grams of the reactant in excess will remain after the reaction?

Assuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter a zero (0) for the number of moles.

Hg2+: ______ mol

C2H3O2:______mol

Na+: ______ mol

S2-:______ mol