Odorless Fertilizer from Household Urine

103_9206Using an analysis of urine and  some basic arithmetic,  I realized yesterday how many useful compounds we unfortunately flush down the toilet.  Based on the fact that an individual’s daily output of urine contains about 3 g of potassium ion, 2.5 grams(g)  of phosphate,  16 g of urea, 3 g of amino acids, a gram of ammonia,  a city of 3 million like Montreal, wastes 75 000 kg of potential fertilizer every day, none of which is recovered by sewage treatment.

Luckily there is a solution. At the elevated pH of aged urine, which will also have more ammonium, the latter ion and phosphate will not dissolve in the presence of magnesium ion. If we add more Mg²+ we can create far more of a precipitate known as struvite. The product is odorless, free of heavy metal contaminants and releases ammonium and phosphate ions slowly into the soil, whose pH is lower than that of aged urine.  Over a temperature range of 25 to  35 oC, 169 to 213 mg of struvite dissolve per liter at pH = 7. The Swiss Federal Institute of Aquatic Science is actively involved in building STUN reactors to recover struvite, but I had to try it myself on a small scale.

The easiest way to do it at home is to use Epsom salts. Every 500 L of urine can potentially produce 1 kg of struvite.  The typical trip to the washroom produces 0.150 L  of urine, which proportionally can yield  0.3 g of MgNH4PO4.6H­2O (struvite) or 0.3/245 = 0.00245 moles. Epsom salts are pure hydrated magnesium sulfate MgSO4.7H2O (246g/mole), and a one to one molar ratio, implies that 0.603 g of  the magnesium salt are needed.

With time, the urine’s pH climbs because urea, urine’s 2nd most common ingredient, breaks down into ammonia, which dissolves in urine’s primary ingredient to produce ammonium hydroxide(NH4OH). At an elevated pH, MgNH4PO4.6H­2O  is poorly soluble, which makes recovery possible. Hoping to eventually form larger crystals, I added the Epsom salts while  the urine was fresh so that the struvite would precipitate gradually. As expected no crystals were apparent without the formation of ammonium.

Struvite crystals, six days after the addition of Epsom salts to fresh urine. The white crystals are at the lower edge of the mason jar.
Filtered struvite crystals, seven days after the start of the experiment.

It took between 15 and 34 hours of aging  to get the initial crystals, a time that was probably elongated by the fact that the mason jar of urine was kept in a cold storage room. More crystals formed during the week. I checked the pH of the urine 7 days after first adding the epsom salts, and it had gone alkaline.

To make sure I was not getting magnesium sulfate instead of struvite crystallizing (unlikely since it’s soluble in ocean water), I added baking soda to a magnesium sulfate solution and obtained no precipitate. For an additional control I added baking soda, magnesium sulfate to filtered aged urine and again obtained no crystals.

The cost of Epsom salt is about $ 3.00/kg .  One kg of Epsom salt will produce 0.3/0.603 = 0.5 kg of struvite; so it would cost $6 to make a kilogram of  struvite, which exceeds the cost of commercial fertilizer , and the latter also has the advantage of including plant-required K+. Magnesium carbonate, is cheaper, and can be more easily converted into soluble MgO, but the process releases carbon dioxide into the environment. So the most ecological and economical source of Mg2+  would be bittern, a magnesium-rich liquid that remains after salt (NaCl) is extracted from seawater.

You may be unaware, as I was, that struvite is found in a type of kidney stones. Unlike oxalate or uric acid stones, the struvite -variety sometimes form after frequent urinary infections. The bacteria responsible for the infection hydrolyzes urea to ammonium, raising the pH and mirroring the precipitating effect used in the recovery of struvite from aged urine.


 Other Sources:
  http://oatao.univ-toulouse.fr/4645/1/Hanhoun_4645.pdf ( a detailed study of the solubility and thermodynamics of struvite )


6 thoughts on “Odorless Fertilizer from Household Urine

  1. Very interesting post on a relevant and useful subject, thanks! The post also made me recall myself browsing, as a child, a chemistry book where it was mentioned that some element, maybe potassium, was extracted during medieval times in some middle east city in a place in the desert where the fluids from the public urination toilets discharged, collected and evaporated. These people were indeed ahead in this respect!

    Liked by 1 person

    • That’s a neat connection. I should have also mentioned that Hennig Brand discovered phosphorus by boiling, filtering and processing as many as 60 buckets of urine. The source goes on to say “Thankfully”, phosphorus is now primarily obtained from phosphate rock (Ca3(PO4)2).” Why “thankfully” when ions of the element can be recovered in such an ecological manner?

      Liked by 1 person

    • Use about four grams of Epsom salts for every liter of urine. If you’re a dog owner, a less messy approach for home-made fertilizer is to catch him peeing on the lawn and quickly adding a couple of liters of water on the spot to prevent “burning”.


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