Name ____________________________________ Limiting Reactants
1. Write a balanced equation for the reaction between aqueous solutions of magnesium chloride and sodium
hydroxide.
a.
If 0.0025 moles of magnesium chloride are reacted with 0.003 moles of sodium hydroxide, how many moles
of precipitate should form?
b. If 60.0 mL of 0.20 M magnesium chloride are reacted with 100.0 mL of 0.50 M sodium hydroxide, how many
moles of precipitate can be formed?
2. Write a complete balanced equation for the reaction between aqueous barium chloride and sodium phosphate.
a. If 0.42 grams of barium chloride (208.23 g/mol) are dissolved in water, and 0.35 grams of sodium
phosphate (117.96 g/mol) are dissolved in water, and the two solutions are mixed together and filtered,
how many grams of precipitate can be produced? (Molar mass of barium phosphate is 601.92
g/mol)
3. Write a complete balanced equation for the reaction between aqueous zinc nitrate and aqueous ammonium
carbonate.
a.
If 0.060 moles of zinc nitrate are combined with 0.10 moles of ammonium carbonate, how many grams of
precipitate should be produced? (molar mass of ZnCO3 is 125.42 g/mol)
b.
If 100.0 mL of 0.30 M zinc nitrate are reacted with 40.0 mL of 0.30 M ammonium carbonate, how many
grams of precipitate should be produced?
c. If 2.84 grams of zinc nitrate (189.40 g/mol) are dissolved in water and 2.02 grams of ammonium carbonate
(96.15 g/mol) are dissolved in water, and the two solutions are mixed and filtered, how many grams of
precipitate can be formed? (molar mass of ZnCO3 is 125.42 g/mol)
Answers: 1a) 0.0015 mol Mg(OH)2
1b) 0.012 mol Mg(OH)2
3a) 8 grams ZnCO3
3c) 1.88 g ZnCO3
3b) 1.5 g ZnCO3
2a) 0.40 grams Ba3(PO4)2