Fourteen possible chemical reactions are listed below, which you are to carry out in the laboratory.  For each reaction that takes place:

• Write the equation for the reaction in words.
• Write a balanced chemical equation using symbols and formulas.
• Indicate the physical state of both reactants and products.  Remember that all solutions contain water as a solvent.
• Indicate, by means of arrows, when a reaction is reversible.
• If a reaction will not occur, simple write “No Reaction.”
• Classify each reaction as one of the four basic types (S, SD, D, DD)

1. In a test tube, mix 5 mL of barium chloride solution with 5 mL of sulfuric acid.
2. Dissolve a small amount of potassium chloride in about 5 mL of distilled water in a test tube.  Do the same to make 5 mL of sodium nitrate solution in a second test tube.  Mix the two solutions.  (It is the mixing for which an equation is written.  Dissolving the salts in water is not a chemical change - is it?)
3. In a test tube, mix 5 mL of sodium carbonate with one mL of hydrochloric acid.
4. Put 5 mL of sodium hydroxide in an evaporating dish and add one drop of phenolphthalein.  Then add hydrochloric acid drop by drop until the color disappears.  (The phenolphthalein does not take part in the reaction but acts as a color indicator.)
5. Put a one inch square of aluminum foil in a test tube.  Add 2 mL of distilled water and the same amount of hydrochloric acid.  Warm slightly.  Remove from heat after the reaction has begun.
6. Let the test tube in #5 stand until the aluminum has reacted completely.  Pour the resulting solution into a small beaker and add ammonium hydroxide until you can smell the ammonia.
7. Place 2 mL of cupric sulfate solution to a test tube.  Add a few drops of sulfuric acid as a catalyst and carefully drop in an iron wire or nail.  Let it stand a few minutes and pour off the copper solution.  Observe the wire.
8. Repeat the experiment in #7, except use 2 mL of ferrous sulfate and a small length of copper wire.
9. (and 10) Insert the handle of a deflagrating spoon through a small piece of cardboard, and place a small sample of phosphorus (about the size of a pea) in the spoon.  Fill a 250 mL flask with ½ inch of distilled water.  Ignite the phosphorus in the spoon, quickly lower it into the flask, and slide the cardboard down to act as a cover to prevent any gas from escaping.  When the phosphorus has burned out, shake the flask vigorously so the water will dissolve any gases.  Then remove the cover and test the solution you have made with both red and blue litmus paper to see if a reaction has occurred.  Write the equation for the burning of phosphorus.
10. Write the equation for the reaction of the combustion product from #9 with water.
11. Decant 5 mL of calcium hydroxide into the test tube being careful not to disturb the solid particles at the bottom (calcium hydroxide is not very soluble in water).  Bubble the carbon dioxide gas into your test tube until a reaction is noted.
12. Place 5 mL of hydrochloric acid in a test tube.  Drop in a piece of copper wire.
13. Heat 10 mL of distilled water in a test tube and add a very small amount of calcium oxide.  Stir well.  Test with red and blue litmus paper to see if a reaction has occurred.
14. Observe the Hoffman apparatus on the side bench.  It contains water with sulfuric acid as a catalyst, and an electric current is being delivered  into the water.  When you write the equation(s) for what is happening, add a note as to what gases are being produced in the left-hand side and the right-hand side.

1. Aqueous solutions of ammonium carbonate and hydrochloric acid are mixed.
2. Solid sodium oxide is dissolved in water.
3. Tin foil is added to an aqueous solution of ferrous nitrate.
4. Sulfur is burned in air to form gaseous sulfur dioxide, and the gas is then dissolved in water.
5. Aqueous solutions of potassium chromate and mercurous bromide are mixed.
6. An iron nail is added to an aqueous solution of stannous nitrate.

[MHS AP Chem page]