(Solved): Calculate the mass (in grams) of precipitate formed when \( 2.27 \mathrm{~L} \) of \( 0.0820 \math ...

Calculate the mass (in grams) of precipitate formed when \( 2.27 \mathrm{~L} \) of \( 0.0820 \mathrm{M} \) barium nitrate are mixed with \( 3.06 \mathrm{~L} \) of \( 0.0664 \mathrm{M} \) ammonium phosphate. Calculate the concentrations (molarities) of each ion remaining in solution after precipitation is complete. moles of barium nitrate \( = \) moles of ammonium phosphate \( = \) limiting reactant is mass of the precipitate in grams \( = \) molarity of barium ion after precipitation = molarity of nitrate ion after precipitation = molarity of ammonium ion after precipitation \( = \) molarity of phosphate ion after precipitation \( = \)