Making A Dilution Series

Aim: To make a dilution series to investigate concentration

Equipment:

• A potassium permanganate crystal
• Test tube rack
• 10mL measuring cylinder
• Test tubes
• Safety glasses   
• Dropper

Method

1. Put your safety glasses on.
2. Place the six tubes in the test tube rack.
3. Using the measuring cylinder, fill one test tube with 10mL of water the rest with 5mL of water.
4. Add a single crystal of potassium permanganate to the test tube with 10mL of water.
5. Using your dropper take 5mL of water from the 10mL water and add to the second test tube.
6. Make sure that you rinse your dropper everytime you move 5mL of water.
7. Repeat step 5 with all your test tubes until you have the same result as the photos.

Burning Magnesium

Aim:
I want to find out what happens to Magnesium when you burn it.

Hypothesis:
I predict that when you burn Magnesium it will turn into ashes.

Equipment:
Heat Mat, Bunsen Burner, Scissor Tongs, Magnesium, Lighter and Safety Goggles.

Method:

1. Get equipment
2. Put on safety goggles
3. Put down your heat mat
4. Connect you Bunsen Burn to the gas tap
5. Close the air hole on the Bunsen Burner
6. Ignite the light
7. Turn on the gas
8. Open the air hole on your Bunsen Burner
9. Hold the Magnesium in the Scissor Tongs
10. Put the Magnesium into the blue flame
11. Observe what happens

Results:

When I burned solid, shiny grey Magnesium in the blue Bunsen burner flame it formed a bright, light white and lasted for 5-6 seconds. Then it burned out. Some white powder was left over.









When magnesium is in its metal form it will burn very easily in air. However, in order to start the reaction (the burning) the magnesium metal needs a source of energy. The flame provides a source of heat so that the magnesium metal atoms can overcome their activation energy. Activation energy is the minimum energy required in order for a chemical reaction to proceed. When the magnesium metal burns it reacts with oxygen found in the air to form Magnesium Oxide. A compound is a material in which atoms of different elements are bonded to one another. Oxygen and magnesium combine in a chemical reaction to form this compound. After it burns, it forms a white powder of the magnesium oxide. Magnesium gives up two electrons to oxygen atoms to form this powdery product. This is an exothermic reaction. An exothermic reaction is a term that describes a chemical reaction in which there is a net release of energy (heat).
http://chemwiki.ucdavis.edu/Under_Construction/Demonstrations/Burning_Magnesium

Conclusion

My hypothesis was that it was going to go into black ashes. I was incorrect. It turned into a glowed bright light white.

Evaluation

Other experiments related to this I could do are:

• Do all metals glow brightly?
• How hot did the magnesium get before it reacted?
• Did it make any other chemicals?
• Why did it have a white light and not blue or green?
• What would happen if we used a chunk of Magnesium?
• What would happen if we used powered Magnesium?