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That’s a Screenshot from the webqc.org, very handy calculator, takes a bit of getting used to though when translating formulas to make it calculate more complex compounds.
Yes less likely but not impossible, any free unchelated Iron in the mix will be mopped up by the PO4, any conditions that degrade the chelate when it’s all in solution will result in increased precipitation.
I always found towards the end of use of a 500ml bottle of DIY AIO that there was always a milky brown precipitate, the things that could affect the mixture in the bottle are storage temperature, exposure to light and evaporation (as the liquid level in the bottle recedes due to dosing the surface area to volume increases, which is why I’ve moved to IV bags).
Right idea, wrong answer, you got a bit carried away with the hydrogen atoms (H), and a lot less carried away with the oxygen.
23.3/18.3 = 1.22 and 6 x 1.22 = 7.33g of CaCl.6H2O.
No, I don't do think so.
That level of Chloride shouldn’t be a problem, I used SaltyShrimp GH+ very successfully to remineralise before I went DIY and that’s made entirely of Magnesium Chloride and Calcium Chloride, at a GH of 6 and 150-200ppm TDS the Chloride is in excess of 100ppm.
As I said you’ve got to be careful with that calculator when translating formulas for it to calculate as Darrel pointed out that it’s easy to miss a few atoms. I should have been more careful when I posted the above solving, it was more a demonstration than the direct calculation.
The main issue is usually the <"water of crystallization">, it can make a lot of difference to the RMM and percentage of the nutrients.
For remineralising RO for use as replacement water you don’t need to add Citric Acid unless you are making a concentrate and using carbonate compounds (CaCO3, MgCO3, KCO3).
I know your trying to make a concentrate but you’ve swapped out using CaSO4 for CaCl alongside MgSO4 and so long as the concentrate is below the solubility threshold for CaSO4 precipitation then it will all stay in solution without the need to acidify.
I started preparing to going down the liquid concentrate remineralisation strategy last year but I got distracted by setting up a marine system which has its own set of challenges related to similar issues when it comes to DIY where a two part brine mixture has the most stability (the concentrate holding the MgSO4 is at the threshold for solubility and the mixture I found needs warmed to 30c to get it all into solution, ATI Absolute Ocean).
The reason I prepared to go liquid remineralisation was because of reactivity between salts.
Part A is usually unreactive though I have seen occasional off white discolouration in the powder here and there but it fully goes into solution for 25L (with help).
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Part B is where the problems arose.
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As you can see it’s turned into an amorphous crystal mass which is insoluble in water, it happened because CaNO3 and MgNO3 are exceptionally hygroscopic and probably absorbed any water vapour in the bag then melting with the phosphate forming an Apatite.
Not quite got round to planning the solution to partB yet but I’ll be putting the Nitrates, Sulphates and Chlorides in one concentrate and keeping the Phosphate separate (probably add it to my liquid bio carbon dose).
My recipe above was to simulate Karst water.
I'm nearly sure CaCl in reaction with citric acid will form HCl and calcium citrate, which could precipitate due to low solubility. But I'm not a chemist, so maybe someone else could shed more light on this.
No the Solubility of CaSO4 is 0.2g/100ml, it’s likely at those ratios in a concentrate that you’ll end up with a MgCl ion solution and CaSO4 precipitation regardless of acidification (I think from what I have read is that you only get a 12% increase in solubility @pH 2.5) Just keep Calcium compounds (Chlorides/Nitrates) away from Sulphate compounds in concentrated solutions.
