Element Collection

Element Collection

Wednesday, September 18, 2013

Potassium Chlorate from Bleach

This post serves as the Video Companion to this video.

This experiment was also featured on Hack a Day!

In this simple experiment you can create potassium chlorate, a powerful oxidizer that finds use in amateur rocketry, a convenient source of oxygen, and the famous "screaming gummy bear" demo (among other things), from common household items with a minimum of effort. The tradeoff is that it's a very inefficient process and yields tend to be very low. Electrolysis is a far superior method, and is something I plan on trying out in the future.

To begin, I measured out 500mL of household bleach. This is about the minimum for this method to produce reasonable (but still quite low) yields. The active ingredient in bleach is sodium hypochlorite, and the higher the concentration in yours the better. Mine was listed as 8.25%.
The good news for chemists is that when shopping for household chemicals to use in experiments, the cheaper the better! The cheapest brands generally do not include extra fancy chemicals like detergents and fragrances, which is desirable for chemistry use.

This solution was then boiled on a hotplate to get rid of most of the water, and to drive the conversion of hypochlorite to chlorate (via a disproportionation reaction, with table salt as a byproduct):
3NaClO == 2NaCl + NaClO3
This only occurs on boiling, so slow evaporation will not work in this experiment. Once crystals start to appear in the liquid, it is time to remove from heat and let cool.
These crystals are the sodium chloride byproduct, and need to be filtered off and can be discarded. The remaining solution contains sodium chlorate, as well as more sodium chloride.
Sodium chlorate is quite soluble, so to recover it and separate it from the sodium chloride it must be converted to potassium chlorate. This can be done with another common household chemical: sodium-free salt alternative. Mine was No Salt brand, which is almost entirely KCl.
For this experiment, we need enough KCl to convert all the sodium chlorate to potassium chlorate. This happens via a simple metathesis reaction:
NaClO3 + KCl == KClO3 + NaCl
Using 500mL of an 8.25% solution of sodium hypochlorite and the two equations above, I calculated that this reaction should only require 13.3g of KCl to go to completion. Other experimenters have recommended using a saturated solution of KCl that is equal in volume to the boiled bleach solution, so that is what I went with this time. Since my bleach ended up at about 200mL, I needed about 75g of KCl to make a saturated solution. The extra ingredients generally leave a solution of No Salt rather cloudy, so I always filter it before use.

Next I combined the solutions together. This should precipitate KClO3 crystals immediately, but I did not see any at all! I think the culprit was using that huge excess of KCl solution. This means that there is a lot of extra water around for the products to dissolve in, so even though potassium chlorate is much less soluble there was still enough solution for it to dissolve in. I believe that if I had used the stoichiometric amount of KCl in the minimum amount of water, 13.3g in about 39mL of water at room temperature, I think I would have seen immediate crystallization. Certainly there is room for future experimentation here.
To get crystallization, I put the solution in the lab fridge over night. When I took the beaker out, there was a nice layer of white, plate-like crystals covering the bottom. I was able to recover 9 grams of product this way.
 22 grams of KClO3 was the theoretical yield here, meaning I had only a 41% recovery. In an attempt to get more yield, I went ahead and boiled the remaining solution down to half its volume and placed it back in the fridge. I ended up with 23.5g of additional product, which by itself is greater than the maximum possible yield! That means that this second crop is very impure; perhaps I shouldn't have reduced the volume quite as much. These crystals looked much different too - they were much more compact, and some were needle-like rather than the nice plates from the first batch. Here is a comparison of the two, with the impure product on the right:
There's still a chance to recover good product from this second batch, and it would require a recrystallization or two. I have yet to try this, but if I do I will update the post. It honestly may not be worth the effort, considering how cheap the reagents were and how simple the process is.

Finally, I wanted to test the product to make sure it was in fact potassium chlorate. There is a simple and exciting test for this - combine some chlorate with half its weight of sugar, and add a drop or two of concentrated sulfuric acid. The mixture crackles and quickly bursts into beautiful lilac flames, making a lot of smoke as well. I tested 1 gram of my pure product combined with 0.5g of sugar, and two drops of acid.
See the video link at the top to see this reaction in action. It appears near the end.


  1. I enjoyed watching this experiment. I am inspired to learn more about chemistry. I think it's fascinating how chemicals react.

  2. Could a solution of 12% sodium dichloro-s-triazinetrione be used instead of bleach?

  3. Is it possible to use calcium hypochorite as found in pool shock? Some products have 75% calcium hypochlorite?

    1. Good question! There's a chance this might be possible, but calcium hypochlorite is unstable in solution. Boiling will likely speed up this decomposition. The solubilities do look promising, though, so if this is your only source of hypochlorite it may be worth a try. I'm leaning towards no, though.

  4. Lowes sells a drain cleaner that is 93% H2SO4 and has some metal inhibitors to help protect plumbing from the acid. Is this form of sulfuric acid strong enough to react with the potassium chlorate? Will the inhibitors interfere with the reaction?

    1. That's actually exactly the type I used! The brand I found is 'Liquid Fire'.

  5. THANKS MAN!!!...I had a "?" moment and was wondering who came up with the idea of "matches"...long story short(I wrote the long story but lost it by going back to this page from the google sign up page before posting it =P), I decided I wanted to make some myself.
    Would you say is more cost-efficient-effective to buy the KClO3 already made, or to make my own?
    How do you know when you have KClO3 in "pure" form?
    What quantity (of chlorine, salt substitute...final yield) would you say is "safe" to begin with?
    I went to school for ME and only had to take CHM for engineers (one class only) and I hated it...THANK YOU for making it interesting my man!!!...lol...I am getting all into home made experiments now...hahaha...Thanks man.

    1. It's probably cheaper to make it yourself, with household bleach and no-salt being cheap (and if you're clever, you can find better versions of both of these). It just takes time. Without a spectrometer you can't really know for sure how pure your chemicals are, but after a few recrystallizations they can be very high purity. Glad you enjoyed it! (and sorry for the slow response!)

  6. sk:

    1. Therefore, the liquid turns pink when it is warm?

    2. it's okay if I do not have 8.25 percent? (2.7)

    3. is what the bleach concentrated in a carton 9.6 percent this is good?

    4. is that a stainless pot of kitchen is good?

    Thank you man good video :D

    1. 1) It shouldn't. Does yours? Sounds like additives - try buying the cheapest brand available.
      2-3) Concentration doesn't matter as long as you account for it in your calculations. Lower concentration just means more water to boil off.
      4) Stainless steel may corrode in the presence of strong oxidizers. Glass is best!

  7. How u calculated the 13.3g of KCl?

    1. Well I started with 500mL of 8.25% bleach, which means it contains roughly 41.25g NaClO (assuming 500mL weighs 500g, which might not be correct but should be pretty close). Then you can use the first orange equation above to calculate how much sodium chlorate will be produced upon boiling. Finally, use the second orange equation to calculate how much KCl needs to be added to fully react this all to potassium chlorate. Stoichiometry!