Quantitative Analysis: Solution Stoichiometry Demonstration Lab
Purpose: to determine the concentration of an AgNO3(aq)
Cu(s)
+
AgNO3(aq)

Ag(s)
Apparatus and Method:
+
Cu(NO3)2(aq)
100 mL AgNO3 solution
graduated cylinder
copper wire
Observations:
Measurement description
Initial mass of copper
Final mass of copper
Mass of copper reacted
Volume of AgNO3
Molar mass AgNO3
Measurement
Calculations:
Moles of copper reacted
Moles of silver nitrate reacted
Concentration AgNO3(aq)
Conclusions:
n
m
MM
n AgNO3  n Cu 
M
n AgNO3
n Cu
n
V
Solution Stoichiometry Problems
1. Calculate the mass of sodium chloride that would be produced from the complete reaction of 25.0 mL of
0.418 mol/L barium chloride solution.
BaCl2(aq) + Na2SO4(aq)  BaSO4(s) + 2NaCl(aq)
(1.22g)
2.
Calculate the mass of mercury(I) carbonate that could be precipitated by the reaction of 88.9 mL of
0.356 mol/L mercurous nitrate solution according to the following equation.
2HgNO3(aq) + Na2CO3(aq)  Hg2CO3(s) + 2NaNO3(aq)
(7.30g)
3.
Calculate the concentration (mol/L) of potassium chlorate solution that could be made by reacting 34.5 mL
of a 0.0756 mol/L of aluminum chlorate . The final volume of the potassium chlorate solution was
125.0 mL.
Al(ClO3)3(aq) + K3PO4(aq)  AlPO4(s)
+ KClO3(aq)
(0.0626 mol/L)
4.
What mass of PbI2 would be produced by reacting 10.0 mL of 0, 058 mol/L Pb(NO 3)2(aq) with 17.0 mL of
0.067 mol/L KI(aq)?
Pb(NO3)2(aq) + KI(aq)  PbI2(s) + KNO3(aq)
(0.262g)
5.
What mass of ZnCl2 could be produced by completely reacting 356 mL of 0.00576 mol/L of FeCl3(aq)?
FeCl3(aq) + ZnCrO4(aq)  Fe2(CrO4)3(aq) + ZnCl2(aq)
(0.420g)
6.
What mass of CuSO4 can be removed from a sample of water by the addition of 95.0 mL of at 0.0203 mol/L
Li2S solution?
CuSO4(aq) + Li2S(aq)  CuS(s) + Li2SO4(aq)
(0.308g)
7.
Calculate the volume of water that could be produced by completely reacting 45.6 mL of a 0.200 mol/L
NaOH solution.
NH4Cl(s) + NaOH(aq)  NH3(g) + NaCl(aq) + H2O(l)
(0.164mL)
8.
What concentration of ferric acetate could be produced from reacting 26.35 mL of 0.0889 mol/L sodium
acetate with excess ferric chloride? Final volume of Fe(C2H3O2)3(aq) was 27.84 mL.
NaC2H3O2(aq) + FeCl3(aq)  Fe(C2H3O2)3(aq) + NaCl(aq)
(0.02805mol/L)
Acid-Base Stoichiometry Calculations
1.
What mass of MgCO3 would be required to react completely with 125 mL of 0.275 mol/L HCl?
MgCO3(s) + HCl(aq)  MgCl2(aq) + CO(g) + H2O(l)`
(1.45g)
2.
What volume of 0.056 mol/L phosphoric acid would be required to neutralize 1.635 g of sodium
hydroxide?
H3PO4(aq) + NaOH(aq)  Na3PO4(aq) + H2O(l)
(0.243L)
3.
Calculate the mass of aluminum sulphate produced by the complete reaction of 25.0 mL of 3.25 mol/L
sulphuric acid.
Al(s) + H2SO4(aq)  Al2(SO4)3(aq) + H2(g)
(9.27g)
4.
A) Calculate the concentration of a Ba(OH)2(aq) , if 5.67 g of barium hydroxide was dissolved to make
500 mL of solution.
(0.0662mol/L)
B) Calculate the concentration if 85.0 mL of a 2.58 mol/L HC2H3O2 solution was diluted to 500 mL.
(0.439mol/L)
C) Calculate the mass of water produced if the solution from part A was mixed with the solution from
part B.
(1.19g)
5.
75.0 mL of a 0.175 mol/L HCl solution was added to 1.45 g sample of impure calcium carbonate. The
resulting solution then required 11.3 mL of a 0.125 mol/L NaOH solution to neutralize the excess HCl.
Calculate the mass of pure calcium carbonate in the original sample.
(0.587g)
6.
A lake was found to be slightly more acidic ( with H2SO3 ) than it should have been. Scientists attempted to
return the lake to the natural pH by dropping CaCO3 powder in the lake from an airplane. If 3.45 t of
calcium carbonate was required to lower the acidity of the lake, calculate the mass of the H2SO3 that was
consumed.
(2.83 t)
7.
A) An industrial chemical company dissolved 3 567 g of carbon dioxide in 125 000 L of water to make
carbonic acid. Calculate the concentration of the acid.
(6.47x10-4mol/L)
B) Calculate the mass of sodium carbonate that could be made by reacting the acid from part A with
sodium chloride.
(8573 g)
H2CO3(aq) + NaCl(aq)  Na2CO3(aq) + HCl(aq)
8.
A student swallowed a 1.50 g TUMS tablet (calcium carbonate) to consume the excess 6.0 mol/L
hydrochloric acid from his stomach.
A) If the TUMS was 87.3% pure CaCO3, calculate the volume of acid that would be consumed.
(0.0436 L)
B) Calculate the number of calcium ions that would be available from this reaction to be used by the body
for building strong bones.
(7.89x1021 Ca2+)