9.5
Stoichiometry
of Solutions
Stoichiometry in Solution Chemistry
Use the following techniques when solving solution stoichiometry:
A(aq)
+
3B(aq)
→
2C(s) + D(aq)
Step One
Write the quantities given below the reactants they represent in the reaction.
Step Two
Write the operation that will be used to convert the amount in (1) to moles.
Step Three
If necessary, decide which reagent is limiting.
Step Four
Use the moles of limiting reagent to decide the moles of the product, using a stoichiometric
ratio.
Step Five
Use the amount of moles of the desired product, obtained in Step Four, to find the amount in
grams, or a concentration.
EXAMPLES!
Food manufacturers sometimes add calcium acetate to
puddings and sweet sauces as a thickening agent. What
volume of 0.500mol/L calcium acetate, Ca(CH3COO)2(aq),
contains 0.300 mol of acetate ions?
EXAMPLES!
Ammonium phosphate can be used as a fertilizer. 6.0g of
ammonium phosphate is dissolved in sufficient water to
produce 300mL of solution. What are the concentrations
(in mol/L) of the ammonium ions and the phosphate ions
present?
EXAMPLES!
8.76g of sodium sulfide is added to 350mL of 0.250mol/L
lead (II) nitrate solution. Calculate the maximum mass of
precipitate that can form.
EXAMPLES!
Example 1:
 Determine the minimum volume of 0.42
mol/L sodium sulfate, that is required to
react completely with all the barium ions in
500.0 mL of a 0.100 mol/L barium chloride
solution.
Example 2:
 Predict the mass of precipitate expected
when 1.50 L of 0.800 mol/L sodium
carbonate is mixed with 850 mL of a 1.00
mol/L aluminum nitrate solution.
pg 447 # 1, 2
pg 449 # 1, 3, 5, 7