Chemistry
1. Iron (IIII) and copper (II) sulfate solution
Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction.
2 Fe + 3 CuSO4 = 3 Cu + Fe2(SO4)3
The new product is iron (III) sulfate, it contains the Fe 3+ ion which is brown.
Lead (II) nitrate and potassium iodide solutions
Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction. Pb(NO3)2 + 2 KI = 2 KNO3 + PbI2
2. Magnesium metal and hydrochloric acid solution
Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid slowly and observe the reaction. Next, place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas.
We notice one of the products is lead iodide which is insoluble so it precipitates out and indeed its colour is yellow.
3) Mg + 2 HCl = MgCl2 + H2
3. Electrolysis of water
Use a U-tube with electrodes at each end, connected to a battery. Fill the U-tube with water. Turning on the battery, observe the results at each electrode. Next, test for hydrogen and oxygen gas produced at each end of the tube.
Electrolysis of water it splits it up into its constituent elements. Oxygen at te anode, hydrogen at the cathode
4. Burning magnesium
Place magnesium ribbon in a clean crucible (on a clay triangle above a Bunsen burner). Heat until the magnesium begins to burn.
MgO is a white solid.
5.
6.
Data and Observations:
Complete a data table that includes a prediction of reaction type (single replacement, double replacement, synthesis, decomposition, or combustion), observations, and identification of reaction type for each reaction in the lab. (10 points)
Reactants
Prediction of Reaction Type
Observations
Reaction Type
Conclusion:
1. Write a balanced equation for each
Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction.
2 Fe + 3 CuSO4 = 3 Cu + Fe2(SO4)3
The new product is iron (III) sulfate, it contains the Fe 3+ ion which is brown.
Lead (II) nitrate and potassium iodide solutions
Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction. Pb(NO3)2 + 2 KI = 2 KNO3 + PbI2
2. Magnesium metal and hydrochloric acid solution
Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid slowly and observe the reaction. Next, place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas.
We notice one of the products is lead iodide which is insoluble so it precipitates out and indeed its colour is yellow.
3) Mg + 2 HCl = MgCl2 + H2
3. Electrolysis of water
Use a U-tube with electrodes at each end, connected to a battery. Fill the U-tube with water. Turning on the battery, observe the results at each electrode. Next, test for hydrogen and oxygen gas produced at each end of the tube.
Electrolysis of water it splits it up into its constituent elements. Oxygen at te anode, hydrogen at the cathode
4. Burning magnesium
Place magnesium ribbon in a clean crucible (on a clay triangle above a Bunsen burner). Heat until the magnesium begins to burn.
MgO is a white solid.
5.
6.
Data and Observations:
Complete a data table that includes a prediction of reaction type (single replacement, double replacement, synthesis, decomposition, or combustion), observations, and identification of reaction type for each reaction in the lab. (10 points)
Reactants
Prediction of Reaction Type
Observations
Reaction Type
Conclusion:
1. Write a balanced equation for each