File - Mr.Matthews` Chemistry

SCH3U - Stoichiometry Involving Solutions Worksheet
1. Calculate the number of mL of 2.00 M HNO3 solution required to react with 216 grams
of Ag according to the equation.
3Ag(s) + 4HNO3(aq) --------->3AgNO3(aq) + NO(g) + 2H2O(l) (1335 mL or 1.34x103 mL)
2. Calculate in mL the volume of 0.500 M NaOH required to react with 3.0 grams of acetic
acid. The equation is:
NaOH(aq) + HC2H3O2(aq) -------> NaC2H3O2(aq) + H2O(l)
(100 mL)
3. Calculate the number of grams of AgCl formed when 0.200 L of 0.200 M AgNO3 reacts
with an excess of CaCl2. The equation is:
2 AgNO3(aq) + CaCl2(aq) -------> 2 AgCl(s) + Ca(NO3)2(aq)
(5.37 g)
4. Calculate the mass of AgCl formed when an excess of 0.100 M solution of NaCl is added
to 0.100 L of 0.200 M AgNO3.
(2.87 g)
5. Calculate:
a) the mass of BaSO4 formed when excess 0.200 M Na2SO4 solution is added to 0.500 L of
0.500 M BaCl2 solution, and
(58.35 g)
b) the minimum volume of the Na2SO4 solution needed to precipitate the Ba2+ ions from
the BaCl2 solution.
(1250 mL or 1.25x103 mL)
6. A sample of impure sodium chloride weighing 1.00 grams is dissolved in water and
completely reacted with silver nitrate solution. The dried precipitate of AgCl has a mass
of 1.48 grams . Calculate the percentage of NaCl in the original impure sample. (60.37%)
7. To neutralize the acid in 10.0 mL of 18.0 M H2SO4 that was accidentally spilled on a
laboratory bench top, solid sodium bicarbonate was used. The container of sodium
bicarbonate was known to weigh 155.0 g before this use and out of curiosity its mass was
measured as 144.5 g afterwards. The reaction that neutralizes sulphuric acid this way is
as follows.
H2SO4 + 2 NaHCO3 --------> Na2SO4 + 2 CO2 + 2 H2O
Was sufficient sodium bicarbonate used? Determine the limiting reactant and the
calculate the maximum yield in grams of sodium sulphate.
(No, 8.52 g)
8. Barium nitrate and potassium sulphate solutions react and form a precipitate. What is
the precipitate? How many mL of 0.40 M Ba(NO3)2 solution are required to precipitate
completely the sulphate ions in 25 mL of 0.80 M K2SO4 solution?
(50.00 mL)
9. What mass of silver chloride can be precipitated from a silver nitrate solution by 200 mL
of a solution of 0.50 M CaCl2?
(28.66 g)
SCH3U - More Stoichiometric Reactions in Solution Worksheet
1. Ammonium sulphate is a "high-nitrogen" fertilizer. It is manufactured by reacting
sulphuric acid with ammonia. In a laboratory study of this process, 50.0 mL of sulphuric
acid reacts with 24.4 mL of a 2.20 M ammonia solution (ammonium hydroxide) to yield
the product ammonium sulphate in solution. Calculate the molar concentration of the
sulphuric acid used.
(0.54 M)
2. Slaked lime is sometimes used in water treatment plants to clarify water for residential
use. The lime is added to an aluminum sulphate solution in the water. Fine particles in
the water stick to the floc precipitate produced, and settle out with it. Calculate the
volume of 0.0250 M calcium hydroxide solution that can be completely reacted with 25.0
mL of 0.25 M aluminum sulphate solution.
(750 mL)
3. In designing a solution stoichiometry experiment for her class to perform, a chemistry
teacher wants 75.0 mL of 0.200 M iron(III) chloride solution to react completely with an
excess of 0.250 M sodium carbonate solution.
a) What is the minimum volume of this sodium carbonate solution needed?
(90 mL)
b) What would be a reasonable volume of this sodium carbonate solution to use in this
experiment? Provide your reasoning.
(100 mL as this 10-15% excess)
4. A student wishes to precipitate all the lead(II) ions from 2.0 L of solution containing,
among other substances, 0.34 M Pb(NO3)2(aq). The purpose of this reaction is to make
the filtrate solution non-toxic. If the student intends to precipitate lead(II) sulphate,
suggest and calculate an appropriate solute, and calculate the required mass of this
(78.70 g of aluminum sulphate)
5. Copper(II) ions can be precipitated from waste solution by adding aqueous sodium
a) What is the minimum volume of 1.25 M Na2CO3(aq) needed to precipitate all the
copper(II) ions in 4.54 L of 0.0875 M CuSO4(aq) solution?
(317.80 mL)
b) Suggest a suitable volume to use for this reaction.
(about 350 mL)
6. A 24.89 piece of zinc is placed into a beaker containing 350 mL of hydrochloric acid. The
next day the remaining zinc is removed, dried, weighed, and found to have a mass of
21.62 grams. Determine the concentration of zinc chloride in the beaker.
(0.14 M)
7. How many millilitres of 0.300 M NiCl2(aq) solution are required to completely react with
25.0 mL of 0.100 M Na2CO3(aq) solution? How many grams of NiCO3(s) will be formed?
(8.33 mL; 0.30 g)
8. How many millilitres of 0.400 M CaCl2(aq) would be needed to react completely with 35.0
mL of 0.600 M AgNO3(aq) solution?
(26.25 mL)
9. Suppose that 30.0 mL of 0.400 M NaCl(aq) is added to 30.0 mL of 0.300 M AgNO3(aq).
a) How many moles and grams of AgCl(s) would precipitate?
(0.009 moles)
b) What would be the concentrations of each of the remaining ions in the solution after
reaction? ([Na+1] = 0.2 M; [Ag+1 ]= 0 M; [Cl-1 ]= 0.05 M; [NO3-1] = 0.15M
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