Reveal a copper sulfate message with ammonia!
- Put on protective gloves and eyewear.
- Conduct the experiment on the plastic tray and in a well-ventilated area.
- Avoid inhaling ammonia vapors from the beaker (steps 3–4).
- Do not allow chemicals to come into contact with the eyes or mouth.
- Keep young children, animals and those not wearing eye protection away from the experimental area.
- Store this experimental set out of reach of children under 12 years of age.
- Clean all equipment after use.
- Make sure that all containers are fully closed and properly stored after use.
- Ensure that all empty containers are disposed of properly.
- Do not use any equipment which has not been supplied with the set or recommended in the instructions for use.
- Do not replace foodstuffs in original container. Dispose of immediately.
- In case of eye contact: Wash out eye with plenty of water, holding eye open if necessary. Seek immediate medical advice.
- If swallowed: Wash out mouth with water, drink some fresh water. Do not induce vomiting. Seek immediate medical advice.
- In case of inhalation: Remove person to fresh air.
- In case of skin contact and burns: Wash affected area with plenty of water for at least 10 minutes.
- In case of doubt, seek medical advice without delay. Take the chemical and its container with you.
- In case of injury always seek medical advice.
- The incorrect use of chemicals can cause injury and damage to health. Only carry out those experiments which are listed in the instructions.
- This experimental set is for use only by children over 12 years.
- Because children’s abilities vary so much, even within age groups, supervising adults should exercise discretion as to which experiments are suitable and safe for them. The instructions should enable supervisors to assess any experiment to establish its suitability for a particular child.
- The supervising adult should discuss the warnings and safety information with the child or children before commencing the experiments. Particular attention should be paid to the safe handling of acids, alkalis and flammable liquids.
- The area surrounding the experiment should be kept clear of any obstructions and away from the storage of food. It should be well lit and ventilated and close to a water supply. A solid table with a heat resistant top should be provided
- Substances in non-reclosable packaging should be used up (completely) during the course of one experiment, i.e. after opening the package.
FAQ and troubleshooting
No problem! Continue the experiment.
That’s perfectly fine! You just need to lower the tip of the marker into the solution of copper sulfate so that the cartridge can absorb the solution.
You just need to touch the filter paper a few times for a couple seconds. This should blot away any excess solution.
Try to recall whether the solution was dripping from the other end of the marker when you first filled the cartridge. If it wasn’t, then add copper sulfate solution to the cartridge until the solution starts dripping from the other end.
If you did everything else correctly, is it possible you didn’t dip the tip of the marker into the puddle of copper sulfate in the cup? In this case, lower the tip of the marker into the copper sulfate solution and wait 2 minutes.
In this experiment, it’s best to write your message in the center of the paper so that it gets the best possible exposure to the ammonia vapor. If you wrote your inscription on the edge of the paper, hold it so that the message is positioned over the center of the beaker.
Finally, you can heat the beaker with an ammonia solution to speed up the reaction. To do this, place a candle in the center of the stove and set the flame diffuser on top of it. Center the beaker on the flame diffuser. Take off your protective gloves and light a wooden splint. Use the splint to light the candle. Wait and observe the result!
There is enough paper in the set to repeat the experiment several times. If you really want to use ordinary paper, you can certainly try! Document any differences in your outcomes, and let us know the results of your observations!
Good question! Try figuring out the answer experimentally – test the marker once a day and note when it stops working. Why might the marker stop working? Usually it stops working when it dries out. Just dip the tip of the marker into some more copper sulfate solution. You can even add a few drops of copper sulfate solution directly into the cartridge. Have fun!
Copper sulfate CuSO4 can pass as a decent invisible ink. Fill a marker with it.
Though copper sulfate CuSO4 is blue, the marker leaves almost no trace because very little of it is transferred to the paper. Your message will keep its secrets until the addressee treats it with a fitting chemical.
One such chemical is ammonia NH3, which emerges from a (NH4)2CO3 solution. You could simply apply (NH4)2CO3 solution to the paper, but one wrong move and you'll smear your message away, rendering it illegible! There's a trick, however: emerging ammonia NH3 can leave the solution as a gas.
Your message is now visible!
Ammonia gets inside paper and reacts with copper ions Cu2+. The formed substance has blue-lilac color and we can read the secret message!
Dispose of solid waste together with household garbage. Pour solutions down the sink and wash with an excess of water.
When the ammonia NH3 gas reaches the paper, it reacts with Cu2+ . This forms what’s known as a copper-ammonia complex , and its color is intense enough to make your message clearly visible.
One side effect you may have noticed: NH3 gas has quite a pungent odor , and even a small amount of it in the air is easily noticeable. If you're afraid that somebody might “sniff out” your espionage, you can apply some less smelly chemicals to your message to the same effect.
Why does the secret message appear?
The solution of ammonium carbonate (NH4)2CO3 decomposes into carbon dioxide CO2 and a gas with a rather unpleasant odor — ammonia NH3. Like other gases, ammonia is able to permeate the piece of paper with the secret message, and the ammonia molecules bind with the copper ions on the paper. This chemical reaction turns the light-blue writing a much darker blue-lilac.
How is ammonia produced?
Ammonium carbonate (NH4)2CO3 decomposes, producing ammonia NH3 and carbon dioxide CO2:
(NH4)2CO3 → 2NH3gas↑ + CO2gas↑ + H2O
In addition to being water-soluble, both ammonia and carbon dioxide are highly volatile and therefore vaporize easily. You most likely noticed the distinctly unpleasant smell of ammonia. The carbon dioxide will not react with the paper or the ink, but the ammonia will bind to the ink’s copper ions Cu2+. The change in color indicates that a chemical reaction has taken place.
What else can you do with copper sulfate? Don’t miss your chance to combine it with tannin! See the “Follow-up” section of the “Iron gall ink” experiment for more information.
Copper sulfate CuSO4 is so useful that is produced on a large scale. In particular, anhydrous copper sulfate is an effective dehumidifying agent. Moreover, its aqueous solution is utilized as an antiseptic (poisonous to most living organisms), as an outdoor pesticide, and as a source of copper to be deposited on various metallic surfaces.
For us beginner experimentalists, copper sulfate can serve as an unusual decoration. If we leave an aqueous solution of copper sulfate in an open vessel, the water will gradually evaporate, and the sulfate will precipitate to form beautiful blue crystals. Unfortunately, since these crystals contain water, they dry out and wear away with time. Coating them with a substance like nail polish can help keep them from aging.
Another substance that can serve as a base for invisible inks is cobalt chloride CoCl2. Its aqueous solution is slightly pink, and is almost unnoticeable on white paper (and is totally invisible on a pink background!). However, when heated, this light-pink coloring turns blue, revealing any secret message. The naturally light-pink cobalt chloride CoCl2 turns blue when its Co2+ cations are deprived of water molecules. Interestingly, if such an inscription is exposed to humid air, it will disappear again as water returns to the cobalt cations Co2+. In general, cobalt compounds containing a Co2+ cation easily fluctuate between pink and blue, even with just a slight outside influence.