Chemistry - Types of Reactions Lab
- 1. Materials Magnesium ribbon Sodium Chloride solution (NaCl) Zinc, mossy 1M Silver nitrate (AgNO3) 3 M hydrochloric acid (HCl) 1M lead nitrate (PbNO3) Iron fillings Potassium iodide solution (KI) 1M copper (II) sulfate (CuSO4)
- 2. Procedure Reaction 1 1. Examine a piece of magnesium ribbon. Using crucible tongs, hold the sample in the burner flame until the magnesium starts to burn. CAUTION. DO NOT LOOK DIRECTLY AT THE FLAME. HOLD THE BURNING MAGNESIUM AWAY FROM YOU AND DIRECTLY OVER THE EVAPORATING DISH. When ribbon stops burning, put the remains in the evaporating dish. Examine this product carefully. Write a balanced equation for the reaction for reaction 1 below. What type of chemical reaction is reaction 1? Reaction 2 1. Stand a clean, dry test tube in the test tube rack. Add about 4 mL of 3M hydrochloric acid (HCl) to the tube. CAUTION. Handle acids with care. They can cause painful burns. Do not inhale any HCl fumes. Now carefully drop a small piece of zinc metal (Zn) into the acid in the test tube. Observe and record what happens. 2. Using a test tube holder, invert a second test tube over the mouth of the test tube in which the reaction is taking place. Remove the inverted tube after about 30 seconds and quickly insert a burning wood splint into the mouth of the tube. Observe and record what happens. Write a balanced equation for the reaction that takes place in step 1 of reaction 2. What type or reaction is taking place in step one of reaction 2? Write a balanced equation for the reaction that takes place in step 2 of reaction 2. What type of reaction is taking place in step two of reaction 2?
- 3. Reaction 3 1. Stand a clean, dry test tube in the test tube rack. Add about 4 ml of 1M Copper (II) Sulfate (CuSO4) to the tube. CAUTION. Copper (II) Sulfate is toxic, harmful if inhaled, and may be an irritant. Add a small amount of iron filings and gently shake and swirl to mix well. Observe and record what happens. Write a balanced equation for the reaction that takes place in reaction 3. What type of reaction is taking place in reaction 3? Reaction 4 1. Stand two clean, dry test tubes in the test tube rack. Add about 4 mL of sodium chloride (NaCl) solution in one test tube and 4 mL of silver nitrate (AgNO3) into the other. CAUTION. Silver Nitrate can stain your skin and is and irritant. 2. Mix the two solutions either by using a pipette or slowly pouring one solution into the other. Write a balanced equation for the reaction that takes place in reaction 4. Write the net ionic equation for reaction 4. What type of reaction is taking place in reaction 4. Reaction 5 1. Stand two clean, dry test tubes in the test tube rack. Add about 4 mL of 1M Lead nitrate (PbNO3) in one test tube and 4 mL of Potassium iodide solution (KI) into the other. CAUTION. Lead nitrate is toxic and a possible carcinogen and Potassium iodide is a mild irritant.
- 4. 2. Mix the two solutions either by using a pipette or slowly pouring one solution into the other. Write a balanced equation for the reaction that takes place in reaction 5. Write the net ionic equation for reaction 5. What type of reaction is taking place in reaction 5. Reaction 6 1. Stand two clean, dry test tubes in the test tube rack. Add about 4 mL of 1M Potassium Chromate (K2CrO4) in one test tube and 4 mL of Silver nitrate (AgNO3) into the other. CAUTION. Potassium Chromate is very toxic and a possible carcinogen. Silver Nitrate can stain your skin and is and irritant. 2. Mix the two solutions either by using a pipette or slowly pouring one solution into the other. Write a balanced equation for the reaction that takes place in reaction 6. Write the net ionic equation for reaction 6. What type of reaction is taking place in reaction 6.
- 5. Observations Reactions Observations Reaction 1 Reaction 2 Reaction 3 Reaction 4 Reaction 5 Reaction 6
- 6. Questions 1. In this experiment, what method was used to test for the presence of H2 gas? Why does this test work? 2. What is a precipitate? Why did some compounds precipitate in a few of the reactions? 3. What 3 solid precipitates were formed during this experiment? 4. Balance the equations below and identify the type or reaction represented by each equation. a. AgNO3 (aq) + Cu (s) Cu(NO3)2 (aq) + Ag (s) b. BaCl2 (aq) + Na2(SO4) (aq) Ba(SO4) (s) + NaCl (aq) c. Cl2 (g) + NaBr (aq) NaCl (aq) + O2 (g) d. KClO3 (s) KCl (s) + O2 (g) e. Al Cl3 (aq) + NH4OH (aq) NH4Cl (aq) + Al(OH)3 (s) f. H2 (g) + O2 (g) H2O (g)