Difference between revisions of "Make Copper Sulfate"
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| − | Copper sulfate is usually encountered as a blue liquid solution, or in blue crystalline form, and is often used in chemistry classes because it is relatively simple to make, and it can be used to demonstrate many interesting reactions, and grow beautiful blue crystals. Copper sulfate also has many practical uses in agriculture, pool maintenance, and the arts and can be readily purchased at many online retailers for these applications.<ref>http://www.copper.org/resources/properties/compounds/table_a.html</ref> You can make copper sulfate at home or in the classroom in a number of ways. Just remember that copper sulfate is a skin irritant that is toxic if ingested. Use caution and appropriate safety gear when handling chemicals, and dispose of them carefully after your experiment. | + | Copper sulfate is usually encountered as a blue liquid solution, or in blue crystalline form, and is often used in chemistry classes because it is relatively simple to make, and it can be used to demonstrate many interesting reactions, and grow beautiful blue crystals. Copper sulfate also has many practical uses in agriculture, pool maintenance, and the arts and can be readily purchased at many online retailers for these applications.<ref name="rf1">http://www.copper.org/resources/properties/compounds/table_a.html</ref> You can make copper sulfate at home or in the classroom in a number of ways. Just remember that copper sulfate is a skin irritant that is toxic if ingested. Use caution and appropriate safety gear when handling chemicals, and dispose of them carefully after your experiment. |
[[Category:Chemistry]] | [[Category:Chemistry]] | ||
==Steps== | ==Steps== | ||
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#*If you get sulfuric acid on your skin, immediately flush your skin with soap and cool water for at least 15 minutes, and seek medical attention. | #*If you get sulfuric acid on your skin, immediately flush your skin with soap and cool water for at least 15 minutes, and seek medical attention. | ||
#*If you splash sulfuric acid in your eyes, flush your eyes for at least 30 minutes with cool water and seek medical attention. WEAR GOGGLES to prevent this from happening! | #*If you splash sulfuric acid in your eyes, flush your eyes for at least 30 minutes with cool water and seek medical attention. WEAR GOGGLES to prevent this from happening! | ||
| − | #*If you spill acid on a surface, cover the spill with baking soda. Wait for the bubbling to stop. Then carefully wipe up all affected surfaces with a sponge or paper towels, and wash all of the material collected down the sink with plenty of water.<ref>https://www.tamut.edu/About/Administration/Environmental-Health-and-Safety/Information%20Folder/Chemical%20disposal.pdf</ref> | + | #*If you spill acid on a surface, cover the spill with baking soda. Wait for the bubbling to stop. Then carefully wipe up all affected surfaces with a sponge or paper towels, and wash all of the material collected down the sink with plenty of water.<ref name="rf2">https://www.tamut.edu/About/Administration/Environmental-Health-and-Safety/Information%20Folder/Chemical%20disposal.pdf</ref> |
#Assemble your equipment. You will need a glass beaker or jar to perform the experiment in, and a glass measuring cup with milliliter gradations, or a glass eyedropper. You may also need a glass stir stick or spatula for retrieving excess copper pieces from the solution, and a scale to weight the copper. | #Assemble your equipment. You will need a glass beaker or jar to perform the experiment in, and a glass measuring cup with milliliter gradations, or a glass eyedropper. You may also need a glass stir stick or spatula for retrieving excess copper pieces from the solution, and a scale to weight the copper. | ||
#*Do '''not''' use metal or plastic measuring spoons, as they will react with the acid. | #*Do '''not''' use metal or plastic measuring spoons, as they will react with the acid. | ||
| − | #Find a suitable workspace. This experiment will put off hydrogen (h<sub>2</sub>) gas, which is extremely combustible, and should only be done outdoors or under a laboratory vent hood, away from any open flames or ignition sources. You should also set up your experiment on an acid resistant surface, preferably one that is glass, or specifically chemical resistant.<ref>https://www.youtube.com/watch?v=L7xr6GqGnrw</ref> | + | #Find a suitable workspace. This experiment will put off hydrogen (h<sub>2</sub>) gas, which is extremely combustible, and should only be done outdoors or under a laboratory vent hood, away from any open flames or ignition sources. You should also set up your experiment on an acid resistant surface, preferably one that is glass, or specifically chemical resistant.<ref name="rf3">https://www.youtube.com/watch?v=L7xr6GqGnrw</ref> |
#*If you don't have a chemical-resistant surface to work on, you should at least put a sheet of thick cardboard under your work area. The sulfuric acid ''will'' dissolve the cardboard, but slowly enough that you can neutralize the spill with baking soda before it eats clear through. | #*If you don't have a chemical-resistant surface to work on, you should at least put a sheet of thick cardboard under your work area. The sulfuric acid ''will'' dissolve the cardboard, but slowly enough that you can neutralize the spill with baking soda before it eats clear through. | ||
| − | #Assemble your materials. For this you will need 30% hydrogen peroxide, and concentrated (98%) sulfuric acid. Both of these can be purchased at a scientific supply company, although the hydrogen peroxide can also be ordered from major online retailers. You will also need a few inches of copper wire, or some chunks of copper pipe, available at any hardware store.<ref>https://www.youtube.com/watch?v=arlYPz3EP7A</ref> | + | #Assemble your materials. For this you will need 30% hydrogen peroxide, and concentrated (98%) sulfuric acid. Both of these can be purchased at a scientific supply company, although the hydrogen peroxide can also be ordered from major online retailers. You will also need a few inches of copper wire, or some chunks of copper pipe, available at any hardware store.<ref name="rf4">https://www.youtube.com/watch?v=arlYPz3EP7A</ref> |
| − | #Create the acid solution. Place 10ml 30% hydrogen peroxide in a beaker. Then add 3ml concentrated sulfuric acid. This is called "Piranha solution" and will heat up quickly, so be extremely careful.<ref>http://www.ch.cam.ac.uk/sites/ch/files/users/meg27/DSO017C%20Acid%20Piranha%20Solution%200911.pdf</ref> | + | #Create the acid solution. Place 10ml 30% hydrogen peroxide in a beaker. Then add 3ml concentrated sulfuric acid. This is called "Piranha solution" and will heat up quickly, so be extremely careful.<ref name="rf5">http://www.ch.cam.ac.uk/sites/ch/files/users/meg27/DSO017C%20Acid%20Piranha%20Solution%200911.pdf</ref> |
#*Never attempt to cover a beaker or vessel containing Piranha solution; it can explode. | #*Never attempt to cover a beaker or vessel containing Piranha solution; it can explode. | ||
#Add the copper. Carefully place about 3g of copper wire or metal chunks into the solution. | #Add the copper. Carefully place about 3g of copper wire or metal chunks into the solution. | ||
| − | #*Do not use pennies for this experiment, as they contain a lot of metals besides copper and may cause unexpected reactions.<ref>http://www.livescience.com/32401-whats-a-penny-made-of.html</ref> | + | #*Do not use pennies for this experiment, as they contain a lot of metals besides copper and may cause unexpected reactions.<ref name="rf6">http://www.livescience.com/32401-whats-a-penny-made-of.html</ref> |
| − | #Watch the reaction take place. Bubbles will begin to form around the copper, and the clear liquid in the jar will begin to turn blue. Leave the copper in the solution until the bubbles stop forming. This can take several minutes, depending on the temperature and concentration of your solution. Carefully lift out any remaining copper with a glass spatula or stirring rod. You should now be left with an aqueous copper sulfate solution.<ref> http://www.nuffieldfoundation.org/practical-chemistry/reacting-copperii-oxide-sulfuric-acid</ref> | + | #Watch the reaction take place. Bubbles will begin to form around the copper, and the clear liquid in the jar will begin to turn blue. Leave the copper in the solution until the bubbles stop forming. This can take several minutes, depending on the temperature and concentration of your solution. Carefully lift out any remaining copper with a glass spatula or stirring rod. You should now be left with an aqueous copper sulfate solution.<ref name="rf7"> http://www.nuffieldfoundation.org/practical-chemistry/reacting-copperii-oxide-sulfuric-acid</ref> |
| − | #Let the solution evaporate. If you wish to collect the copper sulfate crystals, pour the copper sulfate solution into a shallow glass dish and leave it exposed to air for several days while the remaining liquid evaporates. Remember that the solution is still caustic, and use care in handling it.<ref>http://sciencenotes.org/how-to-grow-blue-copper-sulfate-crystals/</ref> You can then use your copper sulfate crystals in various experiments, or to grow larger crystals.<ref | + | #Let the solution evaporate. If you wish to collect the copper sulfate crystals, pour the copper sulfate solution into a shallow glass dish and leave it exposed to air for several days while the remaining liquid evaporates. Remember that the solution is still caustic, and use care in handling it.<ref name="rf8">http://sciencenotes.org/how-to-grow-blue-copper-sulfate-crystals/</ref> You can then use your copper sulfate crystals in various experiments, or to grow larger crystals.<ref name="rf8" /> |
#Dispose of excess copper sulfate solution correctly. Copper sulfate is toxic to fish, plants, and other wildlife and should not be poured into lakes or streams, or rinsed down the storm drain. Copper sulfate is a common ingredient in many drain cleaners, and small quantities, like what this experiment will yield, can be safely diluted with water and rinsed down the sink. | #Dispose of excess copper sulfate solution correctly. Copper sulfate is toxic to fish, plants, and other wildlife and should not be poured into lakes or streams, or rinsed down the storm drain. Copper sulfate is a common ingredient in many drain cleaners, and small quantities, like what this experiment will yield, can be safely diluted with water and rinsed down the sink. | ||
===Making Copper Sulfate Using Nitric Acid=== | ===Making Copper Sulfate Using Nitric Acid=== | ||
| − | #Assemble your safety gear. Nitric acid is considerably more hazardous than sulfuric acid, so be very cautious during this experiment.<ref>http://www.cdc.gov/niosh/npg/npgd0447.html</ref> You will need eye protection, acid-resistant gloves and a lab coat. | + | #Assemble your safety gear. Nitric acid is considerably more hazardous than sulfuric acid, so be very cautious during this experiment.<ref name="rf9">http://www.cdc.gov/niosh/npg/npgd0447.html</ref> You will need eye protection, acid-resistant gloves and a lab coat. |
#Find a suitable work space. Because of the risks involved with using nitric acid, '''this experiment should only done in a laboratory setting.''' As this experiment will put off toxic fumes (NO<sub>2</sub> gas), it must be done under a fume hood. | #Find a suitable work space. Because of the risks involved with using nitric acid, '''this experiment should only done in a laboratory setting.''' As this experiment will put off toxic fumes (NO<sub>2</sub> gas), it must be done under a fume hood. | ||
#Assemble your equipment. You will need a glass beaker or jar to perform the experiment in, a glass measuring cup with milliliter gradations, or a glass eyedropper, and a glass stirring rod or spatula to remove excess copper chunks, and a scale to measure the copper. | #Assemble your equipment. You will need a glass beaker or jar to perform the experiment in, a glass measuring cup with milliliter gradations, or a glass eyedropper, and a glass stirring rod or spatula to remove excess copper chunks, and a scale to measure the copper. | ||
| − | #Assemble your materials. For this you will need water, nitric acid (70%), and concentrated (98%) sulfuric acid. These can be purchased at a scientific supply company. You will also need a few inches of copper wire, or some chunks of copper pipe, available at any hardware store.<ref | + | #Assemble your materials. For this you will need water, nitric acid (70%), and concentrated (98%) sulfuric acid. These can be purchased at a scientific supply company. You will also need a few inches of copper wire, or some chunks of copper pipe, available at any hardware store.<ref name="rf4" /> |
| − | #Create the acid solution. First place 30ml of water in the beaker. Then add 5ml of nitric acid and 3ml concentrated sulfuric acid.<ref> https://www.youtube.com/watch?v=arlYPz3EP7A</ref> | + | #Create the acid solution. First place 30ml of water in the beaker. Then add 5ml of nitric acid and 3ml concentrated sulfuric acid.<ref name="rf10"> https://www.youtube.com/watch?v=arlYPz3EP7A</ref> |
| − | #Add the copper. Carefully drop about 6g of copper wire or metal chunks into the solution. Stand back away from the fumes, and watch the reaction take place. A brown gas will form, bubbles will form as the copper dissolves, and the liquid in the beaker will turn blue. The reaction is complete when the bubbling stops.<ref>http://www.angelo.edu/faculty/kboudrea/demos/copper_HNO3/Cu_HNO3.htm</ref> | + | #Add the copper. Carefully drop about 6g of copper wire or metal chunks into the solution. Stand back away from the fumes, and watch the reaction take place. A brown gas will form, bubbles will form as the copper dissolves, and the liquid in the beaker will turn blue. The reaction is complete when the bubbling stops.<ref name="rf11">http://www.angelo.edu/faculty/kboudrea/demos/copper_HNO3/Cu_HNO3.htm</ref> |
#*The gas that results from the reaction is toxic, and should not be inhaled. | #*The gas that results from the reaction is toxic, and should not be inhaled. | ||
| − | #Let the solution evaporate. If you wish to collect the copper sulfate crystals, pour the copper sulfate solution into a shallow glass dish and leave it exposed to air for several days while the remaining liquid evaporates. Remember that the solution is still caustic, and use care in handling it.<ref | + | #Let the solution evaporate. If you wish to collect the copper sulfate crystals, pour the copper sulfate solution into a shallow glass dish and leave it exposed to air for several days while the remaining liquid evaporates. Remember that the solution is still caustic, and use care in handling it.<ref name="rf8" /> You can then use your copper sulfate crystals in various experiments, or to grow larger crystals.<ref name="rf8" /> |
#Dispose of excess copper sulfate solution correctly. Copper sulfate is toxic to fish, plants, and other wildlife and should not be poured into lakes or streams, or rinsed down the storm drain. Copper sulfate is a common ingredient in many drain cleaners, and small quantities, like what this experiment will yield, can be safely diluted with water and rinsed down the sink. | #Dispose of excess copper sulfate solution correctly. Copper sulfate is toxic to fish, plants, and other wildlife and should not be poured into lakes or streams, or rinsed down the storm drain. Copper sulfate is a common ingredient in many drain cleaners, and small quantities, like what this experiment will yield, can be safely diluted with water and rinsed down the sink. | ||
===Making Copper Sulfate Using Electrolysis=== | ===Making Copper Sulfate Using Electrolysis=== | ||
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#*If you get sulfuric acid on your skin, immediately flush your skin with soap and cool water for at least 15 minutes, and seek medical attention. | #*If you get sulfuric acid on your skin, immediately flush your skin with soap and cool water for at least 15 minutes, and seek medical attention. | ||
#*If you splash sulfuric acid in your eyes, flush your eyes for at least 30 minutes with cool water and seek medical attention. WEAR GOGGLES to prevent this from happening! | #*If you splash sulfuric acid in your eyes, flush your eyes for at least 30 minutes with cool water and seek medical attention. WEAR GOGGLES to prevent this from happening! | ||
| − | #Find a suitable workspace. This experiment will put off hydrogen (h<sub>2</sub>) gas, which is extremely combustible, and should only be done outdoors or under a laboratory vent hood, away from any open flames or ignition sources. You should also set up your experiment on an acid resistant surface, preferably one that is glass, or specifically chemical resistant.<ref | + | #Find a suitable workspace. This experiment will put off hydrogen (h<sub>2</sub>) gas, which is extremely combustible, and should only be done outdoors or under a laboratory vent hood, away from any open flames or ignition sources. You should also set up your experiment on an acid resistant surface, preferably one that is glass, or specifically chemical resistant.<ref name="rf3" /> |
#*If you don't have a chemical-resistant surface to work on, you should at least put a sheet of thick cardboard under your work area. The sulfuric acid ''will'' dissolve the cardboard, but slowly enough that you can neutralize the spill with baking soda before it eats clear through. | #*If you don't have a chemical-resistant surface to work on, you should at least put a sheet of thick cardboard under your work area. The sulfuric acid ''will'' dissolve the cardboard, but slowly enough that you can neutralize the spill with baking soda before it eats clear through. | ||
#Assemble your equipment. You will needs a 6-volt battery, a glass jar or beaker, 2 lengths of copper wire, concentrated sulfuric acid solution (available at scientific supply stores), a glass measuring beaker or eyedropper, and water. | #Assemble your equipment. You will needs a 6-volt battery, a glass jar or beaker, 2 lengths of copper wire, concentrated sulfuric acid solution (available at scientific supply stores), a glass measuring beaker or eyedropper, and water. | ||
#*If you do not have access to concentrated sulfuric acid solution, you can use battery acid, which is 30-35% sulfuric acid and is available at hardware and auto parts stores. | #*If you do not have access to concentrated sulfuric acid solution, you can use battery acid, which is 30-35% sulfuric acid and is available at hardware and auto parts stores. | ||
#Create the sulfuric acid solution. Add 30ml of water to the beaker, and 5ml of concentrated sulfuric acid. If you are using the less concentrated battery solution, add 15ml of acid to 20ml of water. | #Create the sulfuric acid solution. Add 30ml of water to the beaker, and 5ml of concentrated sulfuric acid. If you are using the less concentrated battery solution, add 15ml of acid to 20ml of water. | ||
| − | #Set the two wires in the solution so that they are not touching each other. The wires should be an inch or so apart, depending on the size of your container, and should not be touching each other.<ref | + | #Set the two wires in the solution so that they are not touching each other. The wires should be an inch or so apart, depending on the size of your container, and should not be touching each other.<ref name="rf10" /> |
#Connect the wires to the 6-volt battery. One wire should be wrapped around the positive terminal, and one should be wrapped around the negative terminal. | #Connect the wires to the 6-volt battery. One wire should be wrapped around the positive terminal, and one should be wrapped around the negative terminal. | ||
#Watch the reaction take place. You should see bubble forming at the anode (the wire connected to the negative terminal) but not the cathode, and the solution will begin to turn blue as the copper sulfate is formed. Let the reaction run until the solution is quite blue, and then remove the wires from the solution and disconnect them from the battery. | #Watch the reaction take place. You should see bubble forming at the anode (the wire connected to the negative terminal) but not the cathode, and the solution will begin to turn blue as the copper sulfate is formed. Let the reaction run until the solution is quite blue, and then remove the wires from the solution and disconnect them from the battery. | ||
