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How to Make Nitric Acid Download Article Reviewed by Anne Schmidt
Last Updated: April 3, 2025 Fact Checked
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Deriving Nitric Acid from Copper
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Distilling Pure Nitric Acid
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Tips
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Warnings
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Things You'll Need
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This article was reviewed by Anne Schmidt. Anne Schmidt is a Chemistry Instructor in Wisconsin. Anne has been teaching high school chemistry for over 20 years and is passionate about providing accessible and educational chemistry content. She has over 9,000 subscribers to her educational chemistry YouTube channel. She has presented at the American Association of Chemistry Teachers (AATC) and was an Adjunct General Chemistry Instructor at Northeast Wisconsin Technical College. Anne was published in the Journal of Chemical Education as a Co-Author, has an article in ChemEdX, and has presented twice and was published with the AACT. Anne has a BS in Chemistry from the University of Wisconsin, Oshkosh, and an MA in Secondary Education and Teaching from Viterbo University. There are 13 references cited in this article, which can be found at the bottom of the page. This article has been fact-checked, ensuring the accuracy of any cited facts and confirming the authority of its sources. This article has been viewed 144,036 times.
Nitric acid is a type of potent mineral acid used to make things like fertilizers, dyes, and high explosives. The caustic, colorless liquid is typically produced on an industrial scale using highly specialized chemical processes and equipment. However, it’s also possible to make nitric acid in various purities with common laboratory materials, such as nitrate salts, sulfuric acid, and copper. Some of the substances required for this experiment are corrosive, so be sure to don the proper safety gear before handling them. It also won't hurt to brush up on your lab safety procedures so you'll be prepared in the event of an accident.
Steps
Method 1 Method 1 of 2:
Deriving Nitric Acid from Copper
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1 Dissolve 80 grams (2.8 oz) of nitrate salt in 50 millilitres (1.7 fl oz) of water. Start by portioning out your nitrate salt into a small glass mixing container. Then, pour in all of the water at once. Swirl the mixture around inside the container to help it dissolve faster.[1]XResearch source
It’s important to use distilled water rather than ordinary tap water. Most tap water contains traces of other chemicals that can throw off the composition of the acid you produce.[2]XResearch source
For the purposes of this experiment, it will be easiest to use either sodium nitrate, potassium nitrate, or ammonium nitrate. All of these chemicals are readily available at any online chemistry supply store.
Some chemistry supply stores only sell to institutions, not individuals. This may make it hard to get your hands on the items you need unless you have a teacher or supervisor order them on your behalf.
2 Add 100 millilitres (3.4 fl oz) of hydrochloric acid. Measure the acid in a graduated cylinder to ensure that you’re using just the right amount. Transfer the acid to the nitrate salt solution carefully, taking caution not to let it spill or splash. Swirl the contents of the container again to mix your chemical components.[3]XResearch source
You can buy a bottle of concentrated hydrochloric acid for around $1 per ounce (29.57 mL).
It’s a good idea to work under a fume hood or set up your equipment in a well-ventilated open area, as your test materials will emit strong fumes when brought into contact with the acid.
Warning: Always wear gloves and safety goggles when working with acids. Hydrochloric acid in particular is highly corrosive—without proper protection, getting even a small drop on your skin could cause serious burns.[4]XResearch source
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3 Fill a second larger container with 50 millilitres (1.7 fl oz) of water. Pour in just enough water to cover the bottom of the second container. You’ll be using this container to nest your mixing container and prevent spillage or overflow, so make sure that it’s big enough to hold your test materials comfortably.[5]XResearch source
Ideally, your second container will also be slightly taller than your mixing container.
If you’re using a 250 mL beaker as your mixing container, you might place it in a 1,000 mL beaker in order to leave a sufficient amount of space.
4 Place your mixing container at the bottom of the larger container. Set the mixing container down gently in the shallow water. Check to make sure that at least 1⁄4 inch (0.64 cm) of water is still exposed around all sides of the mixing container. If it’s not, find a larger container to fit it in.[6]XResearch source
5 Add at least 32 grams (1.1 oz) of copper into the acid mixture. If possible, use laboratory-grade 99% pure copper pellets. Weigh the pellets on a precision scale in a lightweight container, making sure to weigh the container itself first and subtract its weight from the final reading. When you have a minimum of 32 grams (1.1 oz), dump the copper into your mixing container.[7]XResearch source
If you can’t find copper pellets for purchase, you can also use copper chips, shavings, wire, or even coins. Keep in mind, however, that the acid mixture will mostly dissolve the copper, so you won’t get it back.
Copper is needed to kickstart the oxidation reaction that will ultimately yield nitric acid.
6 Cover the mixing container with a separate container and wait about 1 hour. The third container will trap the nitrogen dioxide generated as the copper dissolves in the acid mixture. The gas will then flow out of the mixing container and bubble up through the water in the holding container, producing nitric acid.[8]XResearch source
A beaker that’s one or two sizes up should fit perfectly over your mixing container. You could also use a mason jar or other drinking container, provided it’s made of glass.
It may help to rest a small, heavy object, such as a book or piece of scrap wood, over the covering container to hold it down and keep it from bobbing as the escaping gas forces it upwards.
The nitric acid you produce with this method will only be around 40-60% pure. To make higher-purity acid, you’ll need to distill it using nitrate salts and sulfuric acid.
Advertisement Method 2 Method 2 of 2:
Distilling Pure Nitric Acid
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1 Measure out 80 grams (2.8 oz) of pure potassium nitrate in a boiling flask. The mixture of potassium nitrate and sulfuric acid tends to produce nitric acid with the highest degree of purity. Use a precision scale to portion out an exact quantity of nitrate salt. Don’t forget to account for the weight of your measuring container.[9]XResearch source
A round-bottom boiling flask is a must for this experiment. The curved surface and tapered mouth of the flask will prevent the evaporated nitric acid from escaping during the distillation process.
You can also use sodium or ammonium nitrate if you have them, though the purity of the resulting acid may be considerably lower.[10]XResearch source
2 Add 60–65 millilitres (2.0–2.2 fl oz) of concentrated sulfuric acid. Pour the acid into the boiling flask using a plastic funnel. If you don’t have a funnel handy, you can also use a dropper tool, provided it’s labelled with precise increments for liquid measurement.[11]XResearch source
Work under a fume hood or in a well-ventilated outdoor space, and be sure to put on gloves and safety goggles prior to handling any of the required chemicals.[12]XResearch source
The greater the purity of your acid, the better. Using sulfuric acid that’s been diluted with water will result in weaker nitric acid.
Tip: If you happen to come into direct contact with an acid by accident, flush the affected area with cold water for at least 15-20 minutes.
3 Set up an empty glass container and a condenser for distillation. Insert a still head with a glass stopper into the mouth of the boiling flask. Connect the angled stem of the stillhead to a condenser tube. Position the lower end of the condenser over the opening of the empty container.[13]XResearch source
You can pick up a basic distillation kit, complete with everything you need to perform your own chemical distillations at home, from any chemistry supply store.
Double-check that the stoppers on your distillation apparatus are secure. If they're not, it’s possible for harmful fumes to leak out.
4 Heat the acid mixture for about 1 hour. Turn on your burner or hot plate, then sit back and watch the magic happen. As the acid mixture heats up, the nitrate salt and sulfuric acid will react to produce bisulfate and liquid nitric acid. The nitric acid will then be vaporized and move into the condenser, where it will cool into small droplets that will drain little-by-little into the empty container.[14]XResearch source
If you have a thermometer, fit it into the top of the stillhead and keep an eye on it while the acid mixture is on the heat source. The temperature inside the boiling flask will fluctuate somewhat, but it should ideally stay right around the boiling point of the acid, 337 °C (639 °F).[15]XResearch source
You may notice the concentrated nitric acid developing a yellowish hue as it collects. This is a normal side-effect of hydrogen dioxide contamination. The acid will still be pure enough to use for a variety of purposes.
5 Blow air on your nitric acid to test its purity. Take a length of rubber tubing or a plastic drinking straw and place one end inside the mouth of the boiling flask. Gently blow into the other end. As you blow, watch for the acid to give off wispy, pale yellow fumes. Substantial fuming will only occur if your nitric acid has a purity greater than about 80%. Because of this unique effect, nitric acid with a high purity is sometimes referred to as “fuming nitric acid.”[16]XResearch source
Be extremely careful not to inhale the fumes. Doing so could cause severe irritation to your airways.
If you’re wearing latex or nitrile gloves, take them off before testing your nitric acid. It may sound counterintuitive, but pure nitric acid can actually cause latex and nitrile to burst into flames!
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Tips
Nitric acid is useful for initiating chemical reactions and producing many other chemical compounds in a laboratory setting. Thanks Helpful 4 Not Helpful 1
Always keep a first aid kit close at hand in your work area in case of unexpected mishaps. Thanks Helpful 4 Not Helpful 1
Copper isn’t cheap, especially if you’re just going to melt it down. Recycle your copper by adding small pieces of aluminum foil to the liquid copper waste, then straining it through a paper towel once it’s had a chance to dissolve. The solid bits left behind will be low-purity copper, which you can use for other experiments. Thanks Helpful 5 Not Helpful 3
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Warnings
Some of the procedures described here can be dangerous if not performed responsibly. For this reason, they’re best left to experienced chemists and lab personnel. If it’s your first time conducting a chemistry experiment, consider a simpler project, like changing the pH of water or neutralizing citric acid. Thanks Helpful 5 Not Helpful 8
Seek immediate medical attention if you notice any burning, swelling, itching, or irritation as a result of exposure to chemicals. If left untreated, chemical burns can lead to more serious symptoms, including shock.[17]XResearch sourceThanks Helpful 0 Not Helpful 1
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Things You’ll Need
Deriving Nitric Acid from Copper
Nitrate salts
Distilled water
Hydrochloric acid
Copper pellets
Assorted laboratory glassware
Graduated cylinder
Precision scale
Fume hood
Rubber gloves
Safety goggles
Copper coins (optional—90% purity or higher)
Distilling Pure Nitric Acid
Potassium nitrate
Concentrated sulfuric acid
Round-bottom boiling flask
Graduated cylinder
Precision scale
Plastic funnel or dropper tool
Distillation equipment
Heat source
Rubber tubing or plastic drinking straw
Fume hood
Rubber gloves
Safety goggles
Thermometer (optional)
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Reviewed by: Anne Schmidt Chemistry Instructor This article was reviewed by Anne Schmidt. Anne Schmidt is a Chemistry Instructor in Wisconsin. Anne has been teaching high school chemistry for over 20 years and is passionate about providing accessible and educational chemistry content. She has over 9,000 subscribers to her educational chemistry YouTube channel. She has presented at the American Association of Chemistry Teachers (AATC) and was an Adjunct General Chemistry Instructor at Northeast Wisconsin Technical College. Anne was published in the Journal of Chemical Education as a Co-Author, has an article in ChemEdX, and has presented twice and was published with the AACT. Anne has a BS in Chemistry from the University of Wisconsin, Oshkosh, and an MA in Secondary Education and Teaching from Viterbo University. This article has been viewed 144,036 times. 93 votes - 92% Co-authors: 10Updated: April 3, 2025 Views: 144,036 Categories: Making Chemicals In other languages Spanish Japanese
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Jun 29, 2021
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Reviewed by: Anne Schmidt Chemistry Instructor This article was reviewed by Anne Schmidt. Anne Schmidt is a Chemistry Instructor in Wisconsin. Anne has been teaching high school chemistry for over 20 years and is passionate about providing accessible and educational chemistry content. She has over 9,000 subscribers to her educational chemistry YouTube channel. She has presented at the American Association of Chemistry Teachers (AATC) and was an Adjunct General Chemistry Instructor at Northeast Wisconsin Technical College. Anne was published in the Journal of Chemical Education as a Co-Author, has an article in ChemEdX, and has presented twice and was published with the AACT. Anne has a BS in Chemistry from the University of Wisconsin, Oshkosh, and an MA in Secondary Education and Teaching from Viterbo University. This article has been viewed 144,036 times. 93 votes - 92% Co-authors: 10 Updated: April 3, 2025 Views: 144,036 Categories: Making Chemicals In other languages Spanish Japanese 
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1 Dissolve 80 grams (2.8 oz) of nitrate salt in 50 millilitres (1.7 fl oz) of water. Start by portioning out your nitrate salt into a small glass mixing container. Then, pour in all of the water at once. Swirl the mixture around inside the container to help it dissolve faster.[1] 
2 Add 100 millilitres (3.4 fl oz) of hydrochloric acid. Measure the acid in a graduated cylinder to ensure that you’re using just the right amount. Transfer the acid to the nitrate salt solution carefully, taking caution not to let it spill or splash. Swirl the contents of the container again to mix your chemical components.[3] 
3 Fill a second larger container with 50 millilitres (1.7 fl oz) of water. Pour in just enough water to cover the bottom of the second container. You’ll be using this container to nest your mixing container and prevent spillage or overflow, so make sure that it’s big enough to hold your test materials comfortably.[5] 
4 Place your mixing container at the bottom of the larger container. Set the mixing container down gently in the shallow water. Check to make sure that at least 1⁄4 inch (0.64 cm) of water is still exposed around all sides of the mixing container. If it’s not, find a larger container to fit it in.[6] 
5 Add at least 32 grams (1.1 oz) of copper into the acid mixture. If possible, use laboratory-grade 99% pure copper pellets. Weigh the pellets on a precision scale in a lightweight container, making sure to weigh the container itself first and subtract its weight from the final reading. When you have a minimum of 32 grams (1.1 oz), dump the copper into your mixing container.[7] 
6 Cover the mixing container with a separate container and wait about 1 hour. The third container will trap the nitrogen dioxide generated as the copper dissolves in the acid mixture. The gas will then flow out of the mixing container and bubble up through the water in the holding container, producing nitric acid.[8] 
1 Measure out 80 grams (2.8 oz) of pure potassium nitrate in a boiling flask. The mixture of potassium nitrate and sulfuric acid tends to produce nitric acid with the highest degree of purity. Use a precision scale to portion out an exact quantity of nitrate salt. Don’t forget to account for the weight of your measuring container.[9] 
2 Add 60–65 millilitres (2.0–2.2 fl oz) of concentrated sulfuric acid. Pour the acid into the boiling flask using a plastic funnel. If you don’t have a funnel handy, you can also use a dropper tool, provided it’s labelled with precise increments for liquid measurement.[11] 
3 Set up an empty glass container and a condenser for distillation. Insert a still head with a glass stopper into the mouth of the boiling flask. Connect the angled stem of the stillhead to a condenser tube. Position the lower end of the condenser over the opening of the empty container.[13] 
4 Heat the acid mixture for about 1 hour. Turn on your burner or hot plate, then sit back and watch the magic happen. As the acid mixture heats up, the nitrate salt and sulfuric acid will react to produce bisulfate and liquid nitric acid. The nitric acid will then be vaporized and move into the condenser, where it will cool into small droplets that will drain little-by-little into the empty container.[14] 
5 Blow air on your nitric acid to test its purity. Take a length of rubber tubing or a plastic drinking straw and place one end inside the mouth of the boiling flask. Gently blow into the other end. As you blow, watch for the acid to give off wispy, pale yellow fumes. Substantial fuming will only occur if your nitric acid has a purity greater than about 80%. Because of this unique effect, nitric acid with a high purity is sometimes referred to as “fuming nitric acid.”[16]