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 Reading 34.56 mL 39.42 mL 44.20 mL

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 Reading 26.05 mL 48.52 mL 33.78 mL

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 Reading 22.92 mL 25.32 mL 41.30 mL

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 Reading 15.7 mL 28.7 mL 42.7 mL

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 Reading 22.92 mL 25.32 mL 41.30 mL

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.