Chemical Reaction Lab Report
Writing Practical Reports
Aim:
To observe what happens during and after a chemical reaction.
Equipment:
Concentrated nitric acid in a glass dropping bottle
Small pieces of Copper
250ml Beaker
2 M Lead nitrate in a dropping bottle
2 M Potassium iodide in a dropping bottle
2 M Copper sulfate in a dropping bottle
2 M Sodium hydroxide in a dropping bottle
2 M Hydrochloric acid in a dropping bottle
4 Pyrex test tubes
Test tube rack
Spatula
Bunsen burner, gauze mat
Sandpaper
Magnesium Ribbon
Tongs
Safety glasses
Procedure:
1. This is a teacher-only demonstration.
Place a 250ml Beaker in the fume cupboard. Place the pieces of Copper into the Beaker and add 150ml of concentrated nitric acid …show more content…
From the results in table 1 above, list as many changes as possible that would indicate a chemical reaction is taking place: As soon as the concentrated nitric acid touched the Copper pieces you could see the reaction occur. The liquid started to bubble and dissolve the solid cutlets of Copper, brown smoke was fuming up and once the cutlets were fully dissolved the liquid stopped bubbling and calmed to a green colour.
2. If step 2 in the procedure is reversed (i.e. the potassium iodide is added to the lead nitrate), what do you predict will happen: The reaction would be the same. You would be adding exactly the same amount of chemicals but switching around the order in which what chemical is left waiting in the test tube ready to react with the chemical about to be mixed with it.
3. In step 2 in the procedure, the reactants were potassium iodide and lead nitrate. What do you predict will be the products of this reaction: I predicted they would clash and produce either a heat or bubbles/froff.
4. What do you think was deposited on the Magnesium ribbon when you added it to the copper sulfate solution: Pressure and bubbles because the liquid was slowly dissolving it. The ribbon reacted so much it infact produced a
Aim:
To observe what happens during and after a chemical reaction.
Equipment:
Concentrated nitric acid in a glass dropping bottle
Small pieces of Copper
250ml Beaker
2 M Lead nitrate in a dropping bottle
2 M Potassium iodide in a dropping bottle
2 M Copper sulfate in a dropping bottle
2 M Sodium hydroxide in a dropping bottle
2 M Hydrochloric acid in a dropping bottle
4 Pyrex test tubes
Test tube rack
Spatula
Bunsen burner, gauze mat
Sandpaper
Magnesium Ribbon
Tongs
Safety glasses
Procedure:
1. This is a teacher-only demonstration.
Place a 250ml Beaker in the fume cupboard. Place the pieces of Copper into the Beaker and add 150ml of concentrated nitric acid …show more content…
From the results in table 1 above, list as many changes as possible that would indicate a chemical reaction is taking place: As soon as the concentrated nitric acid touched the Copper pieces you could see the reaction occur. The liquid started to bubble and dissolve the solid cutlets of Copper, brown smoke was fuming up and once the cutlets were fully dissolved the liquid stopped bubbling and calmed to a green colour.
2. If step 2 in the procedure is reversed (i.e. the potassium iodide is added to the lead nitrate), what do you predict will happen: The reaction would be the same. You would be adding exactly the same amount of chemicals but switching around the order in which what chemical is left waiting in the test tube ready to react with the chemical about to be mixed with it.
3. In step 2 in the procedure, the reactants were potassium iodide and lead nitrate. What do you predict will be the products of this reaction: I predicted they would clash and produce either a heat or bubbles/froff.
4. What do you think was deposited on the Magnesium ribbon when you added it to the copper sulfate solution: Pressure and bubbles because the liquid was slowly dissolving it. The ribbon reacted so much it infact produced a