Search results for query: solubility rules

@palcente #1 calcium nitrate (highly react with CO3) Urea Monopotassium phosphate (can cause issues) Magnesium sulphate (source of So4, also react with CO3) potassium carbonate (source of CO3) #2 calcium nitrate (react with SO4) urea Monopotassium phosphate (can cause issues) potassium...

Darrel and John, I like the solubility chart as well, but it should come with a big disclaimer that says that it is not taking acidity of the target solution into account - neither the size of the body of water it will eventually mix into. For instance, Calcium Carbonate (CaCO3) is pretty much...

To me darrel that chart makes perfect sense, even with my limited knowledge. However... for a noob, or somebody that was kissing the boys/girls behind the bike sheds rather than learning; it doesn't explain that the solubility of calcium sulfate is around 0.26g/l, nor does it explain that...

Hi all, @John q there isn't a specific thread, as such, but the <"solubility rules chart"> (below) is linked into <"numerous threads">. cheers Darrel

Hi all, It maybe a <"zinc (Zn) issue">, I'll copy in @X3NiTH. Have a look at the <"Solubility Rules"> chart. I don't understand why you are using EDTA, if you have FeDTPA as your iron (Fe) source ? cheers Darrel

...as well. Most salts (other than carbonates) are more soluble in warmer water. What @Hufsa and @Hanuman say, have a look at the <"solubility rules chart">, it highlights where problems (the green and pink squares) are likely to occur. If you have <"hard tap water">? Then it is a <"very...

Never understood why people don't use tap water for remineralising, its cheap and delivered to the door. (some will have very soft water and want to keep hard water fish so for them there is a good reason) As for soft water it rains most days. Gave the butt its annual clean out, well it had...

Hi all, You <"are right">. Have a look a the <"solubility rules chart">. If you add salts, where their ions would combine to end up in the green (or pink) boxes, you will get that compound precipitate. You can see that ions with a valency of one ("monovalent") are all soluble, so potassium...

Hi all, Have a look a <"the solubility rules chart">. If you download the <"Fert Calculator V1.8 - New version out! Check Note first/last post!"> it will tell you when you've exceeded the solubility limits for your "all in one mix". You can find the "solubility limits" value for each...

...precipitate will be entirely Calcium Sulphate, any time you dose a Calcium Salt into solution it will precipitate out if it exceeds solubility rules for any other possible calcium compounds from the ingredients present, in this case you exceeded them mightily with sulphate so lots of...

Hi all, It is back to the <"solubility rules chart">, nearly all chlorides are soluble. Whether the ammonium ion (NH4+) remains in solution, or becomes de-ionised to ammonia gas (NH3) <"is dependent on pH">. cheers Darrel

...is quite easy to get a moderate degree of hardness (around 7dKH and 7dGH is what I aimed for) by adding the correct amounts within solubility rules to 1L of Refrigerated Cold Pressurised Carbonated RO/DI thus forming partial Bicarbonate solution over a few hours and when this milky solution...

...that Calcium Nitrate has a tendency to be problematical with other salts and cause the formation of precipitates if you exceed the solubility rules for calcium if you try to make a concentrate (doesn’t have to be a solution CaNO3 will react with other dry salts if placed together in a sachet...

...don't know, <"quite high (several hundred ppm?)"> would be my guess, but it would be a guess. Hard water is also likely to be fairly sulphate rich naturally. Yes, it can do, it is only really calcium (Ca) that is likely to be an issue. Have a look at the <"solubility rules chart">. cheers...

Yes, If you want to store a premixed solution in a bottle that you use at every waterchange you need to be careful not to exceed the solubility rules for Calcium Precipitate formations because of the presence of Sulphate from Magnesium, if it’s all Chlorides then it would all remain in solution...

Hello everyone, Based on its ancestor, the new IFC Aquarium Fertilizer Calculator is completed at last. This has been a long (sometimes fun, sometimes painful) adventure for me. I have spend more time than I care to admit but here it is, ready to roll. Home screenshot here below: Background...

...mixture has Charge Imbalance then depending on pH and temperature multiple different compounds can form and depending on the solubility rules can precipitate out of solution, in pure water alone oxides and hydroxides can form and even carbonates if the receiving solution is allowed dissolved...

...should be enough) to help mitigate the effect. Ensure full solubility of each salt in the bottle before adding the next salt to the mix, if you keep seeing precipitation then you have a contaminated batch of salts and you need to test to find the culprit. Heres a solubility rules table - :)

Hi all, No, carbonates are less soluble than nitrates. This is the <"solubility rules chart">.It is just like @X3NiTH says as soon as you have ions in solution that form one of the insoluble compounds, that compound will precipitate out. You can see for calcium carbonate it says...

Thanks Darrel - so in there a way of prevent the precipitation in the first place? Presumably by adding an acid? I didn't realise commercially available solutions were so acidic - but what type of acid and in what sort of quantities would I need to look for in a DIY mix?

Hi all, It would be difficult to re-solubilise a lot of the ions, it would depend upon the <"solubility rules">. In the case of carbonates, you could get the cation back into solution by acidifying the solution, the "excess" inorganic carbon would be converted to CO2, and once that buffer had...

My tap water is around 7dKh and 12dGh, but in the tank that drops to around 5dKh - presumably due to some buffering from the soil etc. Out of the tap, the water is around pH 7-7.2 and in the tank varies between pH 7.1 and pH 6.2 with CO2 injection. Am I okay with the standard EDTA chelated Fe...

...in the UK"> there may also be problems with low levels of magnesium (Mg) and a very high Ca++ : Mg++ ratio. If you look at the <"solubility rules chart"> all nitrate (NO3-) and potassium (K+) compounds are soluble, but there are a lot of hydroxide (OH-), carbonate (CO3--), phosphate...

Hi all, I probably should have posted the "Solubility Rules Chart" at some point, because I often talk about solubility and ions, and which combinations of nutrients are likely to go out of solution. cheers Darrel

Hi all, I'd shorten the lighting period a bit. Go for that and ignore the ambient light. It does. I would. It is only really the Seachem Iron (Fe) that is likely to cause issues. Iron (Fe), and to a degree, phosphorus (P), are different from the other plant nutrients in that they are much more...

...all, I should have said that you can use the warm water, and that most salts are more soluble in warmer water. The exception to the solubility rules are the carbonates, and that is because their solubility is dependent upon dissolved CO2, and all gases are less soluble at warmer temperatures...

...I've just found that the stable form of magnesium carbonate <"is the trihydrate"> (MgCO3.3H2O) It is back to the carbonate solubility rules, magnesium carbonate is "sparingly soluble" in water so if you add more than the smallest amount most will remain un-dissolved. Carbonates are soluble in...

Thanks it's alot to take in but in the end I understand it aint good in long run. I will dose about 30-40gr to I find MgSO4 to replace it. It should be rather safe with this small amount

I would say yes, but that depends on you. If you are not using other sources of Cl and your dosis of MgCl2 is not much, then it could be fine, but as many things in life, I think is always better have some safe rules when adding products to the tank. This is, of course, just my point of view...

...can recombine into insoluble compounds (like carbonates & phosphates), which will precipitate out of solution. Have a look at <"Solubility rules">. You also potentially have the "common ion" effect if you make up concentrated solutions. This means that if a solution is saturated with ions...

That is fine. Can you please produce for me some pure NO3 solution in water? If yes I will be very happy. If no why? There is also a picture of what happen after I used the mixed K solution. The white line shows the extended new growth that did not happen before. I do not think that is my faith...

Hi all, Tom and I really aren't trying to be difficult, people are entitled to believe what-ever they like, but if you believe that the source of an ion, from the disassociation of a salt, makes any difference to that ion this is a "faith" position, like homoeopathy, because all of science and...

Hi Gilles, You're very welcome. Generally, I've found that it's better to mount the spraybars along the back wall because the short distance to the front makes better use of the flow energy. I imagine that if the flow is strong enough then mounting it on the side wall would be OK. As with all...