Basic Mole Conversions

Complete the chart by calculating the mass or moles of each substance. Show your work on a separate sheet of paper. Indicate the molar mass in the column with its name or formula.

Name or Formula / Mass / Moles
1. / sodium bromide / 50.0 g
2. / FeSO3 / 1.25 mol
3. / magnesium phosphate / 6.4 mol
4. / CaSiO3 / 1.24 x 10-4 g
Name / Formula / Molar Mass / Mass of Given Sample / Moles / Number of Particles
5. / bromine / 40.0 g
6. / carbon dioxide / 17.6 g
7. / helium / 4.2 x 1026 atoms

Balancing Chemical Equations

Write balanced equations for the following word equations.

1.  potassium chloride + silver nitrate potassium nitrate + silver chloride

2.  aluminum hydroxide + sodium nitrate aluminum nitrate + sodium

hydroxide

3.  iron metal + copper (II) sulfate iron (II) sulfate + copper metal

4.  aluminum metal + copper (II) chloride aluminum chloride + copper metal

5. potassium bromide potassium metal + bromine

Concentration of a Solution

Calculate the quantities requested. Show all steps. Remember to use significant digits.

  1. A hydrogen peroxide solution is listed as 3.00% w/v. What volume of this solution would contain 12.0 g of hydrogen peroxide?
  1. What mass of sodium carbonate is required to prepare 3.50 L of a 1.25 g/L sodium carbonate solution in water?
  1. A 50.0 L water sample is found to contain 3.5 ppm of toxic lead. What mass of lead is in the water sample?
  1. A lab sample of sucrose has a concentration of 14.8 mol/L. What amount of sucrose is in a 25.0 mL sample of the solution?
  1. A 1.00 M (Molar = mol/L) nitric acid solution needs to be prepared for a lab. What mass of nitric acid must be measured out to prepare 2.00 L of solution? (HINT: 2 formulas needed)

Naming Chemical Compounds

The following are a good mix of naming and formula writing problems to help you get some practice.

Name the following chemical compounds:

1) NaBr ______

2) Ca(C2H3O2)2 ______

3) P2O5 ______

4) Ti(SO4)2 ______

5) FePO4 ______

6) K3N ______

7) SO2 ______

8) CuOH ______

9) Zn(NO2)2 ______

10) V2S3 ______

Write the formulas for the following chemical compounds:

11) silicon dioxide ______

12) nickel (III) sulfide ______

13) manganese (II) phosphate ______

14) silver acetate ______

15) diboron tetrabromide ______

16) magnesium sulfate heptahydrate ______

17) potassium carbonate ______

18) ammonium oxide ______

19) tin (IV) selenide ______

20) carbon tetrachloride ______

Naming Acids and Bases

Name the following acids and bases:

1) NaOH ______

2) H2SO3 ______

3) H2S ______

4) H3PO4 ______

5) NH3 ______

6) HCN ______

7) Ca(OH)2 ______

8) Fe(OH)3 ______

9) H3P______

Write the formulas of the following acids and bases:

10) hydrofluoric acid ______

11) hydroselenic acid ______

12) carbonic acid ______

13) lithium hydroxide ______

14) nitrous acid ______

15) cobalt (II) hydroxide ______

16) sulfuric acid ______

17) beryllium hydroxide ______

18) hydrobromic acid ______

Boyle’s Law

1.  Correct the following volumes of gas from the indicated pressures to standard pressure. (STP)

  1. 844 ml at 98.6 kPa
  1. 273 cm3 at 59.4 kPa
  1. 116 m3 at 90.0 kPa
  1. 598 ml at 94.4 kPa
  1. 77.0 ml at 105.9 kPa

Charles’ Law

2.  Correct the following volumes of gases for a change from the temperature indicated to standard temperature (pressure remains constant)

  1. 617 ml at 9°C
  1. 609 ml at 83°C
  1. 942 ml at 22°C
  1. 7.12 m3 at 988 K
  1. 213 L at 99°C
  1. 5.93 L at 492 K
  1. 2.27 L at 9°C
  1. 819 cm3 at 21°C
  1. 4.67 ml at 287 K
  1. 5.94 ml at 79°C

Predicting Chemical Reactions

Indicate the reaction type in the blank provided and below predict products and write a balanced chemical equation.

1. Hydrogen and bromine are combined.

REACTION TYPE: ______

BALANCED EQUATION:

2. A drop of copper (II) nitrate is placed on a silver metal strip.

REACTION TYPE: ______

BALANCED EQUATION:

3. Mercury(II) oxide is broken down by heat.

REACTION TYPE: ______

BALANCED EQUATION:

4. Octane is burned in an automobile engine.

REACTION TYPE: ______

BALANCED EQUATION:

Combustion Products

Indicate the chemical formula for the most common oxide of each of the following elements when undergoing combustion reactions with oxygen.

(a) Carbon + oxygen ______

(b) Iron + oxygen ______

(c) Sulfur + oxygen ______

(d) Nitrogen + oxygen ______

(e) Lead + oxygen ______

Solubility

Determine whether the substance indicated is soluble in water (choose “aq”) or insoluble in water (choose one of “s, l, or g”).

(a) glucose, C6H12O6 ______

(b) octane, C8H18 ______

(c) aluminum nitrate, Al(NO3)3 ______

(d) bromine, Br2 ______

(e) ammonium cyanide, NH4CN ______

Calculations

1. A chemist is asked to weigh out 0.100 mol of ammonium nitrate for an experiment. What mass of ammonium nitrate should be placed on the weighing balance?

2. What mass of silver ions is contained in 5.0 L of a 16 ppm silver ion solution?

3. What is the concentration of an ammonia solution (expressed in % w/v) if 30.5 g of ammonia is used to prepare a 1.00 L solution in water?

4. Sodium bicarbonate (baking soda) is the active ingredient in many products used for home treatment of stomach discomfort due to overeating. What volume of a 0.400 mol/L solution would contain 0.125 mol of NaHCO3(aq)?

5. A cleaning solution is prepared by diluting 350. mL of the concentrated commercial reagant to a volume of 1.25 L. What is the concentration of the cleaning solution?

6. A bottle of hydrogen peroxide is labelled 30.0% W/V. If 25.0 mL of the hydrogen peroxide is diluted to 1.00 L by adding water to it, what is the concentration of the diluted solution?

7. An analysis of wine vinegar showed that 24.8 g of acetic acid was present in a 496 mL wine vinegar sample. What is the molar concentration of acetic acid in the wine vinegar? (4 marks)

12