Unit VII
Chemistry 11
Molarity
Worksheets
Molarity Unit Table of Contents
Lesson Day Date Topic
1. Molarity
1
2. Molarity
2
3. Molarity
3
4. Stoichiometry
5. Titrations
1
6. Titrations
2
7. Dilutions
8. Molarity
Review
9. Molarity
and Dilutions
10. Ion
Concentration
11. All
Mole Calculations
12. Molarity
Final Review 2
13. Chemistry
11 Calculations Practice Test # 1
14. Chemistry
11 Calculations Practice Test # 2
15. Chemistry
11 Calculations Practice Test # 3
Molarity Worksheet # 1
1. 15.8 g of
KCl is dissolved in 225 mL of water, calculate the molarity.
2. Calculate
the mass of KCl required to prepare 250. mL of 0.250 M solution.
3. Calculate
the volume of 0.30 M KCl solution that contains 6.00 g of KCl.
4. Calculate
the volume of 0.250 M H2SO4 that contains .250 g H2SO4.
5. 1.50 g of
NaCl is dissolved in 100.0 mL of water, calculate the concentration.
6. How many
moles of NaCl are in 250.0 mL of a 0.200 M solution?
7. How many
litres of a 0.200 M KCl solution contain 0.250 moles?
8. How many millilitres of 0.200 M H2SO4
are required to completely neutralize
250 mL of
0.250 M NaOH?
9. Calculate the mass of CuSO4.5H2O
required to prepare 100.0 mL of 0.100 M solution.
Molarity
Worksheet # 2
1. Calculate the mass of CuSO4.5H2O
required to prepare 100.0 mL of 0.100 M solution.
2. Calculate the mass of CoCl3.6H2O
required to prepare 500.0 mL of a 0.200 M solution.
3. 50.0 g of NaCl is dissolved in 200.0 mL
of water, calculate the molarity.
4. 25.0 g of CuSO4.8H2O
is dissolved in 25.0 mL of water, calculate the molarity.
5. Calculate the mass of NaCl required to
prepare 500.0 mL of a 0.500 M solution.
6. Calculate the volume of 0.500 M NaCl
solution required to contain
0.0500 g of
NaCl.
7. Calculate the volume of 0.200 M NaCl
solution required to contain
0.653 g of
NaCl.
8. Calculate the mass of NaCl required to
prepare 256 mL of a 0.35 M solution.
9. 25.2 g of NaCl is dissolved in 365 mL of
water, calculate the molarity.
10. 56.3 g of CuSO4.8H2O
is dissolved in 30. mL of water, calculate the molarity.
Molarity
Worksheet # 3
1. Calculate the mass of CuSO4.6H2O
required to prepare 200.0 mL of 0.300 M solution.
2. Calculate the mass of CoCl3.8H2O
required to prepare 300.0 mL of a 0.520 M solution.
3. 150.0 g of NaCl is dissolved in 250.0 mL
of water, calculate the molarity.
4. 25.2 g of CuSO4.6H2O
is dissolved in 28.0 mL of water, calculate the molarity.
5. Calculate the mass of NaCl required to
prepare 565.0 mL of a 0.450 M solution.
6. Calculate the volume of 0.250 M NaCl
solution required to contain
0.0300 g of
NaCl.
7. Calculate the volume of 0.500 M NaCl
solution required to contain
0.52 g of
NaCl.
8. Calculate the mass of NaCl required to
prepare 360.0 mL of a 0.35 M solution.
9. 55.6 g of NaCl is dissolved in 562 mL of
water, calculate the molarity.
10. 78.9 g of CuSO4.8H2O
is dissolved in 500.0 mL of water, calculate the molarity.
Stoichiometry Worksheet # 4
1. Excess
sodium hydroxide solution is added to 20.0 mL of 0.184 M ZnCl2, calculate the mass of zinc hydroxide that
will precipitate.
2NaOH(aq) + ZnCl2(aq) → Zn(OH)2(s) + 2NaCl(aq)
2. How many
millilitres of 1.09 M HCl are required to react with a solution formed by dissolving 0.775 g of sodium
carbonate?
Na2CO3(aq) + HCl(aq) → 2NaCl(aq) +
H2O(l)
+ CO2(g)
3. Calculate
the number of grams barium chromate that can be precipitated by adding 50.0 mL of 0.424 MBa(NO3)2.
Ba(NO3)2(aq) +
K2CrO4(aq)
→ BaCrO4(s) +
2KNO3(aq)
4. Determine
the number of millimeters of 0.246 M AgNO3 required to precipitate all the phosphate ion in a solution
containing 2.10 g of sodium phosphate.
3AgNO3(aq) +
Na3PO4(aq)
→ Ag3PO4(s) +
3NaNO3(aq)
5. How many
grams of silver nitrate must be used in the preparation of 150. mL of 0.125 M solution.
6. What volume
of SO2 at STP is generated by the complete reaction of 35.0 mL of 0.924 M Na2SO3?
2HCl + Na2SO3(aq) +
2NaOH(aq) → 2NaCl(aq) + H2O(l) +
SO2(g)
7. How many
milliliters of 6.2 M NaOH must react to liberate 2.4 L of hydrogen at STP?
2Al(s) + 6NaOH(aq) →
2Na3AlO3(aq) + 3H2(g)
8. Calculate
the weight of H2C2O4.2H2O
required to make 750.0 mL of a 0.480 M solution.
9. 25.4 L of
HCL gas at STP are dissolved in 2.5 L of water to produce an acid solution. What volume of 0.200 M Ba (OH)2
will this solution neutralize?
10. 8.25 L at STP
of HCL gas is dissolved in 500.0 ml of water to produce an acid solution. What volume of 0.200 M Ca
(OH)2 will this solution neutralize?
11. 250.0 mL of
water is added to 100.0 mL of 0.0200M H2SO4. What volume
of 0.100M KOH will it
neutralize?
Titration Calculations Worksheet
# 5
1. What volume
of 2.549 M NaOH is needed to fully titrate 50.0 mL of 1.285 M HCl solution ?
2. What volume
of 1.146 M KOH is needed to fully titrate 20.8 mL of 0.557 M H2SO4 solution ?
3. A burette
filled with 1.52 M sodium hydroxide solution reads 2.10 mL initially. After titrating a 25.00 mL sample of acetic
acid the endpoint was reached and the burette
showed 46.30 mL. What is the acetic acid concentration?
4. A burette
filled with 2.557 M sodium hydroxide solution reads 15.62 mL initially. After titrating a 25.00 mL sample of
phosphoric acid the endpoint was reached and
the burette now showed 39.22 mL. What is the [phosphoric acid]?
5. A 10.00 mL
sample of 2.120 M sodium hydroxide solution is placed in a 250.0 mL Erlenmeyer flask. An indicator
called bromothymol blue is added to the solution.
The solution is blue. Hydrochloric acid was added from a burette until there was a green color (endpoint had been
reached).
Determine
the concentration of hydrochloric acid given the following burette readings:
Burette
final = 22.04 mL
Burette
initial = 12.08 mL
6. The
following data was obtained during the titration of 1.0097 M sodium hydroxide with a 25.00 mL aliquot of
hydrofluoric acid:
Trial
1 Trial
2 Trial
3
Burette
Final
Burette
Initial Reading 14.94 mL 19.86 mL 24.66 mL
Vol.
of NaOH Added
Use the above information to determine the concentration of
the acid.
7. The
following data was obtained during the titration of 0.0998 M sodium hydroxide with a 10.00 mL aliquot of
sulphuric acid:
Trial
1 Trial
2 Trial
3
Burette
Final
Burette
Initial Reading 2.46 mL 34.94 mL 20.22 mL
Vol.
of NaOH added
Use the
above information to determine the concentration of the acid.
8. The
following data was obtained during the titration of 2.0554 M hydrochloric acid with a 25.00 mL aliquot of barium
hydroxide:
Trial
1 Trial
2 Trial 3
Burette
Final
Burette
Initial Reading 0.06 mL
2.58 mL 18.54 mL
Volume
of Acid Added
Use the
above information to determine the concentration of the barium hydroxide.
Titrations Worksheet # 6
1. Calculate
the mass of H2C2O4.2H2O
required to prepare 500.0 mL of a 0.200M solution.
2. Calculate
the mass of Cu2SO4.6H2O required to
prepare 200.0 mL of a 0.300M solution.
3. In a
titration 0.200 M NaOH is used to neutralize 10.0 mL of H2SO4.
In three runs the following data
was collected. Calculate the concentration of the acid.
Volume
of 0.20 M NaOH (mL)
Initial Burette Reading 12.90 15.70 18.50
Final Burette Reading 15.70 18.50 21.50
4. In a
titration 0.250 M KOH is used to neutralize 25.0 mL of H3PO4.
In three runs the following data
was collected. Calculate the concentration of the acid.
Volume
of 0.20 M KOH (mL)
Initial Burette Reading 2.90 15.70 28.70
Final Burette Reading 15.70 28.70 42.70
5. Calculate
the volume of 0.500M H3PO4 required to neutralize 25.0 mL
of
0.200M NaOH
6. Calculate
the volume of 0.50 M NaOH required to neutralize 35.0 mL of
0.100M H2C2O4.
7. In a
titration 35.7 mL of 0.250 M H3PO4 is used to neutralize
KOH. Calculate the molarity of the
base.
Trial
1 Trial
2 Trial 3
Burette
Final
Burette
Initial Reading 2.9 mL 15.7 mL 21.50 mL
Volume of
KOH Added
8. In a
titration 35.2 mL of 0.20 M H2C2O4 is used to
neutralize 10.0 mL of NaOH.
Calculate
the molarity of the base.
9. 2
Al + 3
I2 → 2 AlI3
Initial 12.0
mol 15.0 mol 0
Change:
End:
10. C + 2Cl2 → CCl4
Initial 16.0
mol 34.0 mol
0
Changes:
End:
11. 4
Fe
+ 3 O2 → 2 Fe2O3
Initial 12.0
mol 8.0 mol 0
Change:
End:
12. 2
NO
+ O2 → 2 NO2
100g 100g 0
Init:
Change:
End:
Grams:
13. Calculate the
volume of H2 gas produced at STP by the reaction of 300 mL of 0.500 M HCl with excess Zn.
Zn +
2HCl → H2 +
ZnCl2
14. Calculate the
volume of 0.30 M KCl solution that contains 9.00 g of KCl.
Dilutions Worksheet # 7
1. 20.0 mL of
0.200 M NaOH solution is diluted to a final volume of 100.0 mL, calculate the new concentration.
2. 15.0 mL of a
solution of NaOH is diluted to a final volume of 250.0 mL and the new molarity is 0.0500 M. Calculate
the original molarity of the base.
3. 50.0 mL of
0.025 M NaOH solution is added to 150 mL of water. Calculate the new molarity.
4. 45.0 mL of a
solution of NaOH is diluted by adding
250.0 mL of water to produce
a new molarity of 0.0500 M. Calculate the molarity of the base.
5. A 0.125 M
solution is concentrated by evaporation to a reduced final volume of 100.0 mL and a molarity of. 0.150 M.
Calculate the original volume.
6. 850.0 mL of
0.280 M KOH solution is diluted to a final volume of 1000.0 mL, calculate the new concentration.
7. 95.0 mL of a
solution of NaOH is diluted to a final volume of 135 mL and the new molarity is 0.0500 M. Calculate the
original molarity of the base.
Molarity Review # 8
1. Convert 250. g AgNO3 to
formula units and then to atoms of O.
2. Convert 5.9 x1025 H2
molecules to grams.
3. Calculate the percentage composition of
MgSO4.
4. A compound is 42.3 % C, 5.94 % H, 32.9 %
N, and18.8 % O and has a molecular mass
of 425.25 g/mol. Calculate the empirical and molecular formula.
5. How many grams O2 are required
to consume 56.3 g Al?
4Al +
3O2 → 2Al2O3
6. 25.5 mL of
0.100 M HCl reacts with excess Zn to produce 25.3 mL of H2 gas at STP. Calculate the theoretical yield in
mL and the percentage yield of H2 gas.
Zn + 2HCl →
H2 + ZnCl2.
7. Calculate the energy produced by the
complete reaction of 150. g H2.
2H2 + O2 → 2H2O +
130. KJ
8. 84.0 g of Al reacts with 122 g O2
to produce Al2O3.
How many grams of Al2O3 are produced?
Determine the mass of the reactant in excess and the limiting reactant.
9. 15.2 g of Al reacts with 14.3 g O2
to produce Al2O3.
How many grams of Al2O3 are produced?
Determine the mass of the reactant in excess and the limiting reactant.
10. 15.8 g of KCl
is dissolved in 225 mL of water. Calculate the molarity.
11. Calculate the
mass of KCl required to prepare 250.0 mL of 0.250 M solution.
12. Calculate the
volume of 0.30 M KCl solution that contains 6.00 g of KCl.
13. Calculate the
volume of 0.250 M H2SO4 that contains 0.250 g H2SO4.
14. 1.5 g of NaCl
is dissolved in 100.0 mL of water. Calculate the concentration.
15. How many
moles of NaCl are in 250.0 mL of a 0.200 M solution?
16. How many
litres of a 0.200 M KCl solution contain 0.250 moles?
17. Calculate the
volume of H2 gas produced at STP by the reaction of 400.0 mL of 0.800 M HCl with excess Zn.
Zn +
2HCl → H2 +
ZnCl2
18. Calculate the
volume of 0.250 M H3PO4 required to neutralize 25.5 mL of
0.200 M
NaOH.
19. Calculate the
volume of 0.500 M KOH required to neutralize 45.3 mL of
0.320 M H2SO4
.
20. Calculate the mass of CoCl3.6H2O
required to prepare 500.0 mL of a
0.200 M
solution.
Worksheet # 9 Dilutions
and Molarity
1. 40.0 mL of
0.400 M NaOH solution is diluted to a final volume of 200.0 mL, calculate the new concentration.
2. 85.0 mL of a
solution of NaOH is diluted to a final volume of 290.0 mL and the new molarity is 0.0500 M. Calculate
the original molarity of the base.
3. 150.0 mL of
0.025 M NaOH solution is added to 150.0 mL of water. Calculate the new molarity.
4. 220.0 mL of
a solution of NaOH is diluted by adding 250.0 mL of water to produce a new molarity of 0.0500 M.
Calculate the molarity of the base.
5. A 0.350 M
solution is concentrated by evaporation to a reduced final volume of 100.0 mL and a molarity of 0.825 M.
Calculate the original volume.
6. 850.0 mL of
0.280 M KOH solution is diluted to a final volume of 1000.0 mL, calculate the new concentration.
7. 28 g of KCl
is dissolved in 225 mL of water, calculate the molarity.
8. Calculate
the mass of KCl required to prepare 125 mL of 0.450 M solution.
9. Calculate
the volume of 0.40 M KCl solution that contains 8.00 g of KCl.
10. Calculate the
volume of 0.400 M H2SO4 required to neutralize 25.0 mL of
0.200 M
NaOH.
11. Calculate the
volume of H2 gas produced at STP by the reaction of 250.0 mL of 0.600 M HCl with excess Zn. Zn +
2HCl → H2 +
ZnCl2
12. 8.5 L of HCl
gas at STP is dissolved in 325 mL of water, calculate the molarity of the acid solution.
13. How many
moles of NaCl are in 350.0 mL of a 0.400 M solution?
14. How many
litres of a 0.300 M KCl solution contain 0.350 moles?
15. Calculate the
mass of 8.25 x 105 mL of H2 gas at STP.
16. Calculate the
number of formula units of KCl in 200.0 mL of 0.300 M solution.
Worksheet # 10 Ion Concentration
1. What is the
concentration of each ion in a 10.5 M sodium sulphite solution?
2. What is the
concentration of each ion in the solution formed when 94.5 g of
nickel
(III) sulphate is dissolved into 850.0 mL of water ?
3. If 3.78 L of
0.960 M calcium fluoride solution is added to 6.36 L of water, what is the resulting concentration of each ion?
4. What is the
concentration of each ion in a 5.55 M zinc phosphate solution?
5. What is the
concentration of each ion in the solution formed when 94.78 g of
iron (III)
sulphate is dissolved into 550.0 mL of water?
6. If 6.25 L of
0.560 M sodium bromide solution is added to 3.45 L of water, what is the resulting concentration of each ion?
7. What is the
concentration of each ion in a 0.20 M sodium phosphate solution?
8. What is the
concentration of each ion in the solution formed when 16.5 g of Aluminum sulphate is dissolved into 600.0
mL of water?
9. If 1.78 L of
0.420 M barium fluoride solution is added to 2.56 L of water, what is the resulting concentration of each ion?
10. What is the
concentration of each ion in a 1.22 M zinc acetate solution?
11. What is the
concentration of each ion in the solution formed when 94.78 g
of cobalt
(III) sulphate is dissolved into 400.0 mL of water?
12. If the
chloride concentration in 2.00 L of solution is .0900 M, calculate the [Al3+]
and the molarity of the AlCl3
solution.
13. If the [Ga3+]
concentration in 2.00 L of solution is .0300 M, calculate the [SO42-]
and the molarity of the Ga2(SO4)3
solution.
14. In a
titration 12.5 mL of 0.200 M NaOH is needed to neutralize 10.0 mL of H3PO4, calculate the
acid concentration.
15. What volume
of 0.200 M H2SO4 is required to neutralize 25.0 mL of
0.300 M NaOH?
16. The [Cl-] =
0.600 M in 100.0 mL of a AlCl3 solution. How many grams AlCl3
are in the solution?
17. The [SO42-] =
0.600 M in 100.0 mL of a Al2(SO4)3
solution. How many grams Al2(SO4)3
are in the solution?
Worksheet # 11 Mole
Final Review Worksheet
1. 200 mL of
0.200 M H2SO4 reacts with 250 mL of 0.40 M NaOH,
calculate the oncentration of
the excess base.
2. 100.0 mL of
0.100 M H2SO4 reacts with 50.0 mL of 0.20 M NaOH,
calculate the concentration of the
excess acid.
3. 500.0 mL of
0.100 M H2SO4 reacts with 400.0 mL of 0.400 M NaOH,
calculate the concentration of the
excess base.
4. 100.0 mL of
0.200 M H3PO4 reacts with 250.0 mL of 0.40 M NaOH,
calculate the concentration of the
excess base.
5. Change 2.66 moles of H2O to
molecules.
6. Change 9.7x1019 atoms Fe to
moles.
7. Convert 88.3 g AgNO3 to
formula units and then to atoms of O.
8. Convert 3.8 x 1025 H2
molecules to grams.
9. Calculate the empirical formula of a
compound that is 62.2 % Pb,
8.454 % N,
and 28.8 % O. Is this compound ionic or
covalent?
10. A compound is 42.3 % C, 5.94 % H, 32.9 % N,
and 18.8 % O and has a molecular
mass of 425.25 g/mol. Calculate the empirical and molecular formula.
11. How many
moles of Al2O3 are produced by the reaction 200. g Al?
4Al +
302 → 2Al2O3
12. How many
moles Al are required to produce 300. g Al2O3?
4Al +
302 → 2Al2O3
13. 100. g Al
reacts with excess O2 to produce 150. g Al2O3
according to
Calculate
the theoretical and percentage yield. 4Al
+ 302 → 2 Al2O3.
14. Calculate the
energy produced by the complete reaction of 150. g H2.
2H2 + O2
→ 2H2O +
130KJ
15. How many
grams of H2 would be needed to produce 260. KJ of energy?
2H2 +
O2 → 2H2O +
130KJ
16. 20. mol H2
reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O
produced. Identify the limiting reactant.
17. How many
litres of O2 gas at STP are required to produce 100. g Al2O3?
4Al +
302 → 2Al2O3
18. 15.8 g of KCl
is dissolved in 225 mL of water. Calculate the molarity.
19. Calculate the
mass of KCl required to prepare 250.0 mL of 0.250 M solution.
20. Calculate the
volume of 0.30 M KCl solution that contains 6.00 g of KCl.
21. Calculate the volume of 0.250 M H2SO4
required to neutralize 20.0 mL of
0.100 M NaOH.
22. Calculate the volume of H2 gas
produced at STP by the reaction of 150.0 mL of 0.500
M HCl with excess Zn.
Zn +
2HCl → H2 +
ZnCl2
23. 1.5 L of HCl gas at STP is dissolved in
225 mL of water, calculate the molarity of the
acid solution.
24. How many
moles of NaCl are in 250.0 mL of a 0.200 M solution?
25. How many
litres of a .200 M KCl solution contain 0.250 moles?
26. Calculate the
mass of 2.25 x 105 mL of H2 gas at STP.
27. Calculate the
number of formula units of KCl in 100.0 mL of 0.200 M solution.
28. 40.6g of KBr
is dissolved in 500.0 mL of water, calculate the molarity.
29. Calculate the
mass of KBr required to prepare 450.0 mL of 0.350 M solution.
30. Calculate the
volume of 0.50 M KCl solution that contains 3.00 g of KCl.
31. Calculate the
volume of 0.250 M H3PO4 required to neutralize 25.5 mL of
0.200 M
NaOH.
32. In a
titration 22.5 mL of 0.200 M H3PO4 is required to
neutralize 10.0 mL of KOH. What is the
molarity of the base?
Worksheet # 12 All
Mole Calculations
1. Convert 500. g Ca(NO3)2
to formula units and then to atoms of O.
2. Convert 5.9 x1025 CO2
molecules to grams.
3. Calculate the percentage composition of
Al2(SO4)3 to three significant figures.
4.
A compound is 42.3 % C, 5.94
% H, 32.9 % N, and18.8 % O and has a molecular mass
of 850.5g/mol. Calculate the empirical and molecular formula.
5. How many grams of 02 are
required to consume 56.3 g Al?
4Al +
302 → 2Al2O3
6. 15.8 g of
AlCl3 is dissolved in 225 mL of water, calculate the molarity.
7. Calculate
the mass of AlCl3 required to prepare 250.0 mL of 0.250 M solution.
8. Calculate
the volume of 0.30 M AlCl3 solution that contains 6.00 g of AlCl3.
9. Calculate
the volume of 0.450 M H2SO4 required to neutralize 25.0
mL of
0.200 M
NaOH.
10. Calculate the
volume of H2 gas produced at STP by the reaction of 350.0 mL of 0.600 M HCl with excess Zn.
Zn + 2HCl
→ H2 +
ZnCl2
11. 2.9 L of HCl
gas at STP is dissolved in 225 mL of water, calculate the molarity of the acid solution.
12. How many
moles of NaCl are in 500.0 mL of a 0.300 M solution?
13. How many
litres of a 0.2300 M KCl solution contain 0.250 moles?
14. Calculate the
mass of 560. mL of CO2 gas at STP.
15. Calculate the
number of formula units of NaCl in 100.0 mL of 0.200 M solution.
16. 25.5 mL of
0.100 M HCl reacts with excess Zn to produce 25.3 mL of H2 gas at STP. Calculate the theoretical yield in
mL and the percentage yield of H2 gas.
Zn +
2HCl → H2 + ZnCl2.
17. Calculate the energy produced by the
complete reaction of 150. g H2.
2H2+O2 → 2H2O + 130KJ
18. 84.0 g of Al reacts with 122g O2
to produce Al2O3.
How many grams of Al2O3 are produced?
Determine the mass of the reactant in excess and the limiting reactant.
19. Calculate the percentage composition of Na2SO4.
20. How many
litres of O2 gas are required to produce 100. g Al2O3?
4Al +
3O2 → 2Al2O3
21. Calculate the
molar mass of a gas that weighs 19.43 g and has a STP volume of 9.894 L. If the gas is a very funny
one containing nitrogen and used by the dentist, determine the molar mass and molecular formula for the gas.
Write a balanced formula equation, complete ionic equation,
and net ionic equation for each reaction. There are two no reactions.
22. Zn(s) +
AgNO3(aq) →
23. BaS (aq) + KOH(aq) →
24. NaCl(aq) + F2(g) →
25. Sr(OH)2
(aq) + CuSO4 (aq) →
26. NaCl(aq) + Cu(NO3)2(aq)
→
27. NaCl(aq) +
ZnF2(aq) →
28. 100.0 g of an
aqueous compound that is 45.49 % Pb, 12.31 % N, and 42.20 % O reacts with another compound that is 28.16
% N, 8.13 % H, 20.79 % P, and 42.91 %
O. If the actual yield of the product containing lead is 60.0 g, calculate the percentage yield.
29. The following data was obtained during
the titration of 2.0554 M hydrochloric acid
with a 25.00 mL aliquot of barium hydroxide:
Trial
1 Trial
2 Trial
3
Burette
Final
Burette
Initial Reading 0.06 mL
2.58 mL 18.54 mL
Vol.
of Acid Added
Use the
above information to determine the concentration of the barium hydroxide.
30. 20.0 mL of 0.200 M NaOH solution is
diluted to a final volume of 100.0 mL, calculate the new concentration.
31. 15.0 mL of a solution of NaOH is diluted
to a final volume of 250.0 mL and the new molarity is 0.0500 M. Calculate the
original molarity of the base.
32. A burette filled with 2.000 M sodium
hydroxide solution reads 20.20 mL initially. After titrating a 25.00 mL sample
of phosphoric acid the endpoint was
reached and the burette now showed 40.20 mL. What is the [phosphoric acid]?
33. Calculate the volume of 0.500 M KOH
required to neutralize 45.0 mL of
0.320 M H2SO4.
34. 100.0 mL of
0.200 M H2SO4 reacts with 150.0 mL of 0.40 M NaOH, calculate the concentration of the
excess base.
35. 200.0 mL of
0.10 M H2SO4 reacts with 100.0 mL of 0.20 M NaOH, calculate the concentration of the excess
acid.
36. 250.0 mL of
0.100 M H2SO4 reacts with 200.0 mL of 0.400 M NaOH, calculate the concentration of the
excess base.
Worksheet #13 Chemistry
11 Calculations Practice Test # 1
HCl C3H8 SO2 NH4Cl KOH
H2SO4 H2O AgNO3 PbSO4 H3PO4 Ca(OH)2 Al(OH)3 P2O5 Ba(OH)2 CH3COOH
1. Classify the above as ionic or covalent
by making two lists. Describe the difference
between an ionic and covalent compound.
2. Classify the above as acids, bases,
salts and molecular (covalent compounds) by making
four lists.
3. Describe how you can identify each of
the four categories by the formula of the compound.
4. Describe how each of the four categories
would react with litmus and conduct electricity
when aqueous.
5. For each compound that conducts
electricity, write a dissociation equation to show
how it ionizes in water.
6. Calculate the molar mass of FeSO4 •
5H2O and Co3(PO4)2 • 6H2O.
7. 0.300 moles of NaCl is dissolved in
250.0 ml of water, calculate the molarity.
8. 50.0 g of FeSO4 6H2O
is dissolved in 60.0 ml of water, calculate the molarity.
9. How many grams of NaCl are required to
prepare 100.0 ml of a 0.200 M solution?
10. 2.0 g of MgCl2 are dissolved in
25.0 ml of water, calculate the concentration of each ion.
11. How many liters of 0.300 M NaCl
contains10.0 g of NaCl?
12. For
each double replacement reaction write the formula equation, the complete ionic
equation and the net ionic equation.
a) H2SO4(aq) + NaOH(aq) →
b) H3PO4(aq) + Ba(OH)2(aq) →
c) Ca(NO3)2(aq) + Na3PO4(aq) →
d) Zn(s) + HCl(aq) →
13. In
three runs of a titration 22.8, 22.1 and 22.2 mL of .200 M Ba(OH)2
were required to neutralize 10.0 mL of HCl, calculate the acid concentration.
14. In
three runs of a titration 12.1, 12.8, 12.8 mL of.200 M HCl were required to
neutralize 10.0 mL of Ca(OH)2, calculate the base concentration.
15. 35.0
ml of 1.00 M H2SO4 reacts with 175 ml 0.250 M NaOH,
calculate the concentration of the excess acid.
16. 350.0
mL of 0.200 M HCl reacts with 175 mL 0.125 M Ca(OH)2, calculate the
concentration of the excess acid.
17. 25.0
g of sodium reacts with water, how many grams of hydrogen are produced? How
many grams of sodium hydroxide are produced?
18. 25.0
g of calcium reacts with water, how many grams of hydrogen are produced? How
many grams of calcium hydroxide are produced?
19. How
many millilitres of 0.200 M NaOH is required to neutralize 25.0 mL of
0.100
M H2SO4 ?
20. How many millilitres of 0.200M H2SO4
is required to neutralize 25.0 mL of
0.100 M NaOH ?
21. If the [F-] = 0.600 M in an solution, calculate [Al3+]
and the number of grams AlF3 required
to make 1.00 L of the solution.
22. If
the [Na+] = 0.250 M in a Na3P solution,
calculate [P3-] and the number of grams Na3P required to make 1.50 L of the solution.
23. A beaker of mass = 25.36 g contains 2.00 L
of a solution of BaCl2 and is evaporated
to dryness mass = 28.59 g. Calculate the molarity of the solution.
24. A beaker of mass = 55.66 g contains 1.00 L
of a solution of AlF3 and is evaporated
to dryness mass = 62.31 g. Calculate the molarity of the solution.
25. In a titration 0.175 M H2C2O4
was added to a 25.00 mL sample of NaOH. The following
data was collected:
Trial
# 1 Trial # 2 Trial # 3
Final Volume of H2C2O4
(mL) 23.00 20.95 39.05
Initial Volume of H2C2O4
(mL) 4.85 5.00 23.00
26. 2HCl +
Ba(OH)2 → BaCl2 +
2 H2O
When 3.16 g samples of Ba(OH)2
were titrated to the endpoint with HCl solution. 37.80 mL, 35.49 mL, 35.51 mL of HCL was required. Calculate
the HCl concentration.
Worksheet # 14 Chemistry
11 Calculations Practice Test # 2
Match the
following.
1.
Acid a) HCl e)
KOH
2.
Nonacid b)
CH3COOH f)
NH4Cl
3.
Salt c) CH4 g) Ba(OH)2
4.
Base d) HOH h)
AgNO3
5. 200.0 g of NaCl are dissolved in 100. mL
of water, calculate the molarity.
6. How many grams of AgCl are required to
prepare 150.0 mL of 0.200 M solution?
7. How many litres of 0.20 M AgCl are
needed to provide 50.0 g of AgCl?
8. 100. g of AlCl3 is dissolved
in 200.0 mL of water, calculate both ion concentrations.
Write a dissociation equation to show the ionization of the salt in water.
9. In three runs of a titration, 36.9,
34.4, and 34.3 mL of 0.200 M NaOH were used to
neutralize a 25.0 mL sample of H2SO4. Calculate the
molarity of the acid. Begin by
writing a chemical equation for the reaction.
10. Calculate the molarity of the excess NaOH
in the solution formed by mixing 100.0
mL of 0.200 M HCl with 100.0 mL of 0.300 M NaOH. Begin by writing a chemical equation for the reaction.
11. A empty beaker has a mass of 29.86 g. The same beaker is filled
with 0.250 L with a solution
of CaCl2 and weighs 87.26 g. The solution is evaporated to dryness and the mass of the beaker and solid
is 62.31 g. Calculate the molarity of the
solution.
12. Complete the formula equation:
AgNO3(aq) +
Na2SO4(aq)
→
Complete the complete ionic
equation:
Complete the net ionic equation:
13. Complete the formula equation:
H3PO4(aq) +
Sr(OH)2(aq) →
Complete the complete ionic
equation:
Complete the net ionic equation:
14. Complete the formula equation:
Fe3(PO4)2(aq) +
Zn(s) -→
Complete the complete ionic
equation:
Complete the net ionic equation:
Worksheet 15 Chemistry 11 Calculations Practice
Test # 3
1. Calculate
the number of formula units in 250. g
CaCl2.
2. Calculate
the mass of 2.35 x 1020
molecules of CO2.
3. Calculate
the STP volume of 10.0 g of CO2 gas.
4. Calculate
the number of grams CaCl2 in 350. mL of a 0.250M solution.
5. Calculate
the volume of 0.250 M NaCl solution that would contain 0.17 g NaCl.
6. 1.26 g of
AlCl3 are dissolved in 160.0 mL of water. Calculate the molarity of
the solution.
7. 12.5 mL of
CO2 gas at STP are dissolved in 250.0 mL of water. Calculate the molarity of the solution.
8. 10.0 g of Al2(SO4)3
is dissolved in 155 mL of water. Calculate the two ion concentrations.
9. 200.0 mL of
0.200M H3PO4 reacts with 200.0 mL of 0.300M KOH. Calculate the molarity of the excess acid in the new
solution formed.
10. 16 g of Ca
react with water. Calculate the volume of H2 gas produced at
STP.
Ca + 2H2O →
H2 + Ca(OH)2
11. In a titration 0.200 M NaOH is used to
neutralize 10.0 mL of H2SO4. In three runs the following data was collected.
Calculate the concentration of the acid.
Volume of
0.200 M NaOH 25.3 mL 25.8 mL 25.6 mL
12. 60.0 g of Al
react with 60.0 g of O2. Calculate the amount of excess
reactant.
4Al
+ 3O2 → 2Al2O3
13. Caculate the
percentage composition of the elements in Ga2(SO4)3
to three significant digits.
14. What volume of
0.300 M solution must be diluted to a final volume of 1200.0 mL and
have a molarity of 0.2500M.
15. Calculate the
number of grams NaCl produced by the complete reaction of
520. g Cl2.
2Na + Cl2 →
2NaCl
16. If the actual
yield of NaCl in the last question was 200. g, calculate the percentage yield of NaCl.
17. 200.0 mL 0.200 M HCl reacts with 400.0
mL 0.150M NaOH. Calculate the molarity of excess base. HCl
+ NaOH → NaCl
+ H2O
18. 100.0 mL of
0.250 M HCl solution is diluted by adding 250.0 mL of water, calculate the new concentration.
19. 65.5 mL of 0.300 M is diluted to a new
molarity of 0.0600 M, how much water was
added?
20. 56.0 mL
of 0.100 M HCl reacts with 0.250 M
Ba(OH)2, calculate the volume of base
required to completely neutralize the acid.
21. Write the
formula, complete, and net ionic equation for each.
H3PO4(aq) and
NaOH(aq).
22. Write the
formula, complete, and net ionic equation for each.
Na3PO4(aq) and
Ca(NO3)2(aq).
23. Write the
formula, complete, and net ionic equation for each.
Cu(NO3)2(aq) and
Ag(s).
24. A empty beaker has a mass of 25.86 g. The same beaker is filled
with 0.250 L with a solution
of CaCl2 and weighs 87.26 g. The solution is evaporated to dryness and the mass of the beaker and solid
is 36.31 g. Calculate the molarity of the
solution.
25. 125.0 g of an
aqueous compound that is 3.091 % H, 31.62
% P, and 65.29 % O reacts
with another compound that is 80.14 % Ba, 18.68 % O, and 1.179 % H. If the actual yield of the solid product is
350. g, calculate the percentage yield of the
solid.