Author Topic: Chemistry questions  (Read 2493 times)

Daley

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Chemistry questions
« on: August 09, 2024, 09:20:00 PM »
Okay, I'm gonna readily admit, I'm a bit over my head and I'm having to kinda fly by the seat of my pants with very little help (long story), and it's been about a quarter decade since my last turn at formal chemistry. I need chemists, pharmacists, food science, and hard science types in this thread. I'm primarily posting here because I really don't want to go through the hassle of setting up an account over at StackExchange or Reddit, in hopes of finding a somewhat credible answer given the increasing waves of confident sounding AI generated garbage. I've done my best to ensure I have the proper chemical formulas and CAS#s for the stuff in question to try and ensure there's no question as to what is involved. If further clarification is needed, I'll do my best to try and provide it.

I'm trying to put together a rather unique oral rehydration solution/electrolyte drink to help offset the electroyte imbalances caused by thyroid disorders (sodium/potassium/magnesium deficiency), which can contribute toward high anion gap metabolic acidosis.

The core ingredients:
Sodium Chloride (NaCL) CAS#7647-14-5
Sodium Citrate (Na₃C₆H₅O₇) CAS#6132-04-3
Potassium Citrate (K₃C₆H₅O₇) CAS#866-84-2
Dipotassium Phosphate (K₂HPO₄) CAS#7758-11-4
Glucose (C₆H₁₂O₆)
Citric Acid (C₆H₈O₇) CAS#77-92-9
Water (H₂O)

These core ingredients are all components of LiquidIV and seem to work together and act stable. Where I'm getting hung up, however, is the integration of magnesium into the party... which makes me even more apprehensive on potentially extending over into zinc and calcium. All ingredients involved are obtained from known and trusted providers, and all are food or pharmaceutical grade with independent lab COAs available on product batches.

I'd initially been using Magnesium Malate (C₄H₄MgO₅) CAS#869-06-7 as an option, as a similar electrolyte drink (Re-Lyte) had used it in combination with many of the other ingredients above along with Calcium Carbonate (CaCO₃) CAS#471-34-1 figuring this would be a good path forward, but the pH of the mag malate seems to neutralize the citric acid after a few hours after mixing, which concerns me a bit for longer term stability and pathogen growth suppression, along with raising questions about if there's reactions happening, what's precipitating out if it's not being consumed within 24 hours? Granted, the pathogen concern isn't big given the rate of consumption, but the obvious reaction with the citric acid does raise an eyebrow on what might inadvertently shake out, and I'm not smart enough to potentially figure out what that might be.

...so I went back to the drawing board, and continued researching for the preferred form of magnesium in other existing electrolyte drinks that are actually sold premixed and wet, indicating greater stability. All signs pointed to Magnesium Chloride (Cl₂H₈MgO₄) CAS#22695-80-3, as the primary magnesium source in Pedialyte, Powerade, Vitamin Water, etc. I know it and the potassium phosphate can potentially react and yield magnesium phosphate and potassium chloride, but both are still considered GRAS and medically significant sources for the mineral electrolytes in question, and as far as I can tell, there shouldn't be anything untoward left over. Going this route, I'd also figured Calcium Citrate (Ca₃(C₆H₅O₇)₂) CAS#813-94-5 and Zinc Gluconate (C₁₂H₂₂O₁₄Zn ) CAS#4468-02-4 would be good choices. Given the need to restrict chloride levels for safety, nearly all table salt was eliminated from the recipe, but still included all of the above ingredients. However, sampling a little about an hour later yielded a very bitter and noxious drink... which really freaked me out.

Although I've not found any one electrolyte drink with ALL the above chemicals in the same product, I've found some combination(s) of all the ingredients in various on-market electrolyte beverages and medical IV liquids with and without citric acid. As such, I was operating under the conclusion that all the ingredients involved should be safe to mix without concern to negative reactions/interactions in theory... and yet, reactions are happening that are making me rethink the combos, make me hesitant to use, and leave me wondering how I can realistically add magnesium into this hot mess.

Are these combos of mineral salts safe? Where am I going wrong, or am I going wrong at all and the reactions in question are actually safe but simply unpleasant enough to warrant more stevia and koolaid to help mask the flavor? Should I just stop worrying about the neutralization of the citric acid with the malate? I need magnesium (and realistically calcium and zinc sooner than later) in the mix. Would I be safer going citrated forms of all the minerals in question given the citric acid usage outside of the sodium chloride and potassium phosphate salts? Should I use magnesium chloride in this application, or would another soluble form of magnesium be preferable? Same with the calcium and zinc. Neither the potassium citrate nor the potassium phosphate can be removed from this, as I find the potassium will not uptake into the cells without about a 4:1 ratio with phosphorus. The remaining forms of all the electrolytes in question, I suppose, are negotiable, though it is worth noting that sodium citrate is a known treatment option for acidosis along with the potassium citrate. Taking supplement pills are off the table these days, and I'm finding I'm needing very specific ratios of mineral regularly fed in throughout the day like a traditional oral rehydration solution to keep things in balance.

Thanks in advance!
« Last Edit: August 09, 2024, 09:37:37 PM by Daley »

obstinate

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Re: Chemistry questions
« Reply #1 on: August 11, 2024, 01:39:02 PM »
There are probably forums with a higher concentration of food scientists than this one. I would definitely not do what you're doing to save money, but it sounds like you're trying to make something that cannot be obtained on the market, presumably for important personal reasons. Best of luck.

secondcor521

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Re: Chemistry questions
« Reply #2 on: August 11, 2024, 04:14:11 PM »
I have no idea on the chemistry stuff.

I'm curious why you can't just drink what you need across multiple drinks.  Maybe Liquid IV in the morning and the other minerals later in the day, that sort of thing.

Are you working with a doctor or pharmacist at all?  Maybe a compounding pharmacist would have some ideas.

Daley

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Re: Chemistry questions
« Reply #3 on: August 11, 2024, 06:49:35 PM »
There are probably forums with a higher concentration of food scientists than this one. I would definitely not do what you're doing to save money, but it sounds like you're trying to make something that cannot be obtained on the market, presumably for important personal reasons. Best of luck.

But I'm established here, and there's history with potential responses that helps filter out advice that might be otherwise unqualified or AI generated. I haven't gotten good answers off of any subreddit in years at this point, and have given up the usefulness of the place. And no, this isn't a frugal thing, though the cost does play a factor given the limited budget in play... but yes, what is needed is not a commercial thing, as most commercial things are chock' full-o-chloride, which is the real heart attack machine behind high sodium causing heart disease and arrhythmias.



I'm curious why you can't just drink what you need across multiple drinks.  Maybe Liquid IV in the morning and the other minerals later in the day, that sort of thing.

READ:
Taking supplement pills are off the table these days, and I'm finding I'm needing very specific ratios of mineral regularly fed in throughout the day like a traditional oral rehydration solution to keep things in balance.

Are you working with a doctor or pharmacist at all?  Maybe a compounding pharmacist would have some ideas.

Trying, but it's an uphill battle for reasons that when I start spelling them out in detail, eventually makes me want to throw hands with this community and post fighting words. It's not something I particularly want to or care to do. But since I can't say anything nice right now, I'll stop here and go back to expecting no meaningful help.

Thanks anyway.
« Last Edit: August 11, 2024, 06:51:39 PM by Daley »

neophyte

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Re: Chemistry questions
« Reply #4 on: August 11, 2024, 07:03:33 PM »
I'm not a chemist, but I did watch an extension presentation on hydroponics the other night.

The thing that stuck out to me that might apply to your situation is that you need three different tanks and feeder lines for different sets of (plant) nutrients. If the concentrated solutions are mixed, certain minerals will react and precipitate out and be less bioavailable. I didn't pay attention to exactly what was reacting with what though.

To be clear- there's a lot of overlap here. Potassium, magnesium, and phosphorus were all things they were discussing at this point.
« Last Edit: August 12, 2024, 05:08:06 AM by neophyte »

jim555

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Re: Chemistry questions
« Reply #5 on: August 11, 2024, 08:59:24 PM »
...but it's got electrolytes.  Sounds like plants might crave this.

secondcor521

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Re: Chemistry questions
« Reply #6 on: August 11, 2024, 09:22:24 PM »
READ:

Fair comment.  I tried.  At least I think I understood that you're talking about a human ingesting this and not plants. ;-)

Good luck.

Boll weevil

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Re: Chemistry questions
« Reply #7 on: August 12, 2024, 10:02:05 AM »
1. I recall seeing a table in high school chemistry that listed which combinations would yield precipitates. I don’t recall if it was in the book or a separate worksheet. Finding a version of that may help you out.

2. Are you getting the ingredients in powder form or as a solution? If in powder form, can you create the blend and then add water to it just before consuming (kind of like Metamucil)? That may help you get around the bitterness and pathogen issues. If in powder form, could you just take it as a pill or capsule? You can get a machine to produce your own.



zygote

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Re: Chemistry questions
« Reply #8 on: August 12, 2024, 11:35:41 AM »
I'm a chemist, but not the right kind of chemist. I haven't done these kinds of precipitation and pH calculations since high school/early college. So I can't give you as specific an answer as you're looking for.

You've got a few competing issues at play here:

-ion/electrolyte concentration
-pH of the solution
-precipitation of any reaction products

Are you seeing marked precipitation of solids? If so, the combo is likely incompatible. If not, it's possible you could test the pH and add a buffer compound to get it to where you need it. A bitter taste does mean the solution is likely basic, i.e. the acids have become over neutralized (as you suspect). But depending on what buffer you choose, it may affect your desired cation concentration (and of course you need to make sure it's still safe to consume). Another way to get around this would be to mix multiple solutions and drink some of the electrolytes separately.

As for stability, I agree with the suggestion to premix the powders in the correct ratio and mix with water on demand. Letting it sit over time will change the pH due to the dissolution of atmospheric CO2, and also risk pathogen growth depending on the mixture.

But ultimately, I do think it's best to find an expert here. A pharmacist, a food scientist, someone who more intimately knows the biological ramifications of these electrolyte mixtures. There's probably a reason you haven't found a marketed solution with all these ingredients, because the combinations and the counterions matter. And as a professional chemist, I wouldn't even feel comfortable doing these calculations myself because it's not my area of expertise. It's way above the pay grade of an advice forum.

Raenia

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Re: Chemistry questions
« Reply #9 on: August 13, 2024, 07:16:22 AM »
I'm a chemist, but it's been a long time since I had to do these calculations so you'll want to verify everything. You probably already know some of this but I'll start basic. Most useful point in bold below.

There are basically three questions in your post.
1) What ionic pairings are forming, and are any of them dangerous?
2) Will any of those pairings precipitate out of solution?
3) Will it taste bad?

I'm not in the habit of tasting lab chemicals, so let's ignore 3) and try to work on 1) and 2) :D

1) What ionic pairings are formed in your franken-solution? The short answer is, all of them, but in differing amounts. Solutions exist in an equilibrium where ionic pairs form and break constantly. Which pairings are more prevalent in a solution is governed by the pKa of each component. Any weak acid/base is going to act as a buffering component in some capacity, with different target pH's. With the number of components you're looking at, that calculation is going to be very difficult and messy.

Then there's a secondary risk of reactions happening between the functional groups. Carbonate and Phosphate are both quite stable, but I'm not familiar enough with Malate to know if it might react with either one.

2) A solubility table will help with this. Do you have a pH tester? Knowing the pH of your solution will help a lot. Look up the solubility curves of each ion. Concentration is of course also a factor, but I'm assuming you're dissolving in enough water to eliminate that issue.

Here's a link from Sigma Aldrich: https://www.sigmaaldrich.com/US/en/technical-documents/technical-article/materials-science-and-engineering/solid-state-synthesis/solubility-rules-solubility-of-common-ionic-compounds. A quick look suggests that your precipitate might be Magnesium Carbonate and/or Magnesium Phosphate, both of which are insoluble in water. Zinc is also insoluble with carbonate and phosphate. Malate isn't on that chart, but a quick look suggests that Sodium malate and Potassium malate are both highly soluble in water.

I will say that in the lab, we generally try to keep to a single counter-ion for a buffered solution, to avoid these kinds of calculations. My suggestion would be to keep your Mag Malate separate and mix it up on its own, or together with the zinc if that pairing works, maybe 15 minutes after your other concoction. (I mean, my official suggestion is always talk to your doctor/pharmacist because I'm only a chemist. But you know what I mean.)

Daley

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Re: Chemistry questions
« Reply #10 on: August 13, 2024, 11:17:48 AM »
@Raenia thank you!

It's enough that I'm starting to get a better grasp on it all, especially by giving me the appropriate terminology keywords to help research with. The good news is, it looks like whatever may be interacting and precipitating out on either the mag malate or mag chloride end is mostly harmless and just different GRAS forms of these minerals and are only reacting with the potassim phosphate - they're just no longer water soluble, which means a hearty shake to re-mix before drinking. (I've yet to get to a point where I'd been able to add any sort of calcium, as getting the chloride end in balance has been a bearcat as the goldilocks zone of the chloride levels is proving to be quite a narrow band for me, and the magnesium reactions hadn't helped as they were proving to be a distraction.) Ironically, it also means that if I'm aiming for something larger batch shelf stable, so to speak, using any form of magnesium other than tri-mag citrate is my biggest PITA for random reactions... though nearly all the tri-mag citrate on the market currently is all poorly soluble forms sourced out of China. Wheee!

Not that the results from the other two appear to be dangerous. The mag chloride version actually tasted fine again the next day and I didn't have any adverse reactions - which means that hour sampling was probably just getting the full bitterness of the magnesium salts mid-reaction. The mag malate was just producing stuff that needed shaking back in, and it and the zinc gluconate were just neutralizing the citric acid, as would the calcium carbonate if I'd used any yet.

I literally shot myself in the foot and made things more difficult just trying to use more soluble forms of magnesium from a country that has a better track record of producing this sort of stuff without toxic cross-contamination issues from surprise fillers and poor quality control. Guess this realistically means I need to start looking closer at Aquamin Mg... though the additional trace elements hitching a ride from the Celtic Sea could complicate things further, in theory. Maybe I just need to make peace with the Chinese trimag citrate provided it's at least sourced from a reputable seller like NOW FOODS, and hope for mercy and grace to bridge the gaps while having to shake the crap out of the bottle to get it dissolved.

It also means that the simplest and most stable path forward without dealing with wildcard reactions it looks like and from what I'm beginning to understand is to basically use nothing but the alkalized chelated citrate forms of everything (save the sodium chloride and potassium phosphate) from calcium all the way down to zinc (which the latter is hard to source in raw powder form as a supplement), is likely to result in both the most stable and easiest to balance/buffer out using citric acid since they're basically all already stable precipitates and forms that are already where you need to be. The real art will be tweaking the citric acid quantity just enough to get the liquid to a weak buffering acid level just strong enough to impair rapid microbe growth and maybe a slight tang... and that might be easy enough to calculate out by just using a digital pH tester with a little trial and error. Though, it'll likely continue to be a moving target as I try and dial in each of the remaining electrolytes once I get the chloride levels in check.

The irony with this realization is that this was what my gut was telling me to do from the get-go, but the difficulty in finding quality tri-mag citrate and any sort of un-fillered powdered zinc citrate was a source of difficulty, and I was also just trying to work with what I could source. I mean, I literally asked this in the top post: Would I be safer going citrated forms of all the minerals in question given the citric acid usage outside of the sodium chloride and potassium phosphate salts? The answer, apparently, is yes. Yes, you dumbass... a thousand times yes! D'oh!

...that is, unless I'm still missing something, and I always feel like I know there's something important that I don't know with stuff like this. That's the real handicap of being smart enough to know how little you truly understand, and recognizing the limits of what you do know. I can make educated guesses when I don't know, but bluffing is more a risky art than anything else. Though, given where my health is tapdancing these days, along with the challenges of getting any meaningful help on that front given the general state of American healthcare, complicated by the additional defunding and privatization of social safety net services by certain powers that be, compounded by multiple misdiagnoses and the actual medical conditions that have been sussed out being historically poorly understood and barely researched by medical science... nothing like a good tapdance on the razor's edge of risk and mortality to keep the heart a pumping and keep life spicy, I guess.

*sigh* It also means I've mis-stepped a bit financially with this grand experiment. On one hand, it was only about $65, and I've already saved way more than that given how much knock-off/tweaked Liquid IV I've already made the past few months without the magnesium, never mind the financial and health savings of not giving myself a heart attack continuing to take in the amounts of table salt the real deal would have caused at the quantities I'm needing on the potassium/phosphorous end... but still. When money's tight, money's tight. Now, what to do with all this magnesium chloride, magnesium malate, calcium carbonate and zinc gluconate I probably shouldn't use?



As for stability, I agree with the suggestion to premix the powders in the correct ratio and mix with water on demand. Letting it sit over time will change the pH due to the dissolution of atmospheric CO2, and also risk pathogen growth depending on the mixture.

But ultimately, I do think it's best to find an expert here. A pharmacist, a food scientist, someone who more intimately knows the biological ramifications of these electrolyte mixtures. There's probably a reason you haven't found a marketed solution with all these ingredients, because the combinations and the counterions matter. And as a professional chemist, I wouldn't even feel comfortable doing these calculations myself because it's not my area of expertise. It's way above the pay grade of an advice forum.

Appreciate the help @zygote and some of the thoughts helped a bit, especially when combined with what Raenia posted. As for the quoted part specifically? Making in bulk but portioning out the powder evenly with the right balance/blend for smaller batches doesn't work for a multitude of reasons. First is the distribution problems with all the salts and grain size sorting between the items and not having an industrial mixer to portion smaller batches off with. Second, I don't have the money for a decent milligram accurate scale, let alone one that could handle more than a 50g max limit. Third, is the fact that at the concentrations of the minerals as formulated - I'm going through about 1.5-2L a day, and realistically, that means the batches mixed up only need to be stable for 2-3 days at screaming most. Making in 4L powder batches seems to be the best balance between speed, hassle, and using the best affordable while still functionally useful weight tools available.

And yes, I realistically do need to find an expert... why I posted in hopes that someone of that variety was available in the brain-trust here. Unfortunately, it's harder to get solid information like that off of randos on the internet from what were all the bastions of the most useful information lately, and it's barely better when you are embedded in a known and established community. Unfortunately still, getting that sort of medically relevant expert assistance from the actual experts you're technically supposed to rely on, especially given the need for speed and nimbleness on keeping myself even remotely functional with this stuff while using privatized Medicaid and dealing with CFS/ME? Like it or not, the reality of this situation is when you're actually poor and not just cosplaying poverty to qualify for government benefits one wouldn't actually need if they'd just worked a little longer before leaching off the labor of millions of underpaid people, you don't have the resources to get the help you actually need, let alone in a timely fashion. Nearly all of the progress that I've made the past six months since things finally ran so far off the rails that I hit a crisis point has been from spending money that I didn't have and spending the physical and mental energy I couldn't actually spare researching to get the answers that I've gotten thus far... and taking the risk of guinea pigging myself.

Amazingly enough, I've accidentally stumbled into the solution for the real underlying problems, but it's hard to dial in the electrolyte supplementation levels when all you got to refine it is the occasional complete electrolyte blood test that frequently still gets crucial minerals like phosphorous and magnesium forgotten and dropped from the order by any doctors in question because electrolyte panels don't include those and anion gap calculations now, and trying to piece together the same from self-order labs winds up costing well over $100 a pop... and good luck even getting an anion gap off those self-ordered labs unless you sit down and try to estimate the math yourself off the electrolyte panel. Well, there's also trying to infer what minerals may be too high or too low based on blood pressure readings, types of heart arrythmia caused and detected by an ECG, and listening to what pains the body's giving you and you've experienced from the various extremes encountered... and I'm not gonna sugar coat it. Most of the time? I'm pretty okay, but when things go out of balance, it can get scary fast. I used to brute-force these mineral supplements with pills, but that doesn't work anymore, and I need something a lot more... precise.

As for why a ready-made product isn't already available? Well, in a way, there is kinda already... but they're IV solutions. I can barely get bloodwork, as is... so that leaves mineral ORS drunk frequently and slowly throughout the day to keep levels balanced, absorbed through a gut that's got malabsorption issues with these very minerals due to scarring from years of undiagnosed celiac disease. Most of the electrolyte solutions on the market are targeted at healthy people tailored for the fitness market, or for people actively suffering from dehydration caused by illness, and both are meant for short term use as it's expected that the cause of the imbalance needing the replenishment is temporary. And the problem is, the cause of my imbalance is chronic and rooted in metabolism malfunction, which means ongoing, likely for the rest of my life. It's already inconvenient enough to take as it is... you can perhaps see why multiplying that out into two or three separate ORS mixes that I have to potentially space out to avoid interaction between not only hampers the need for the regular dosing, but complicates and increases further variation and potentially getting ratios between the target minerals further out of balance. It's why taking supplement pills is the easier path, but that's not an option for me these days given the nature of the hypokalemia and lack of potassium reserves in the body currently. But the thing is, all these minerals should be happy enough to coexist when appropriately buffered, and there are even IV mixes that do just that... after all, if our body can do it...?

Raenia

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Re: Chemistry questions
« Reply #11 on: August 13, 2024, 11:55:25 AM »
@Raenia thank you!

It's enough that I'm starting to get a better grasp on it all, especially by giving me the appropriate terminology keywords to help research with. The good news is, it looks like whatever may be interacting and precipitating out on either the mag malate or mag chloride end is mostly harmless and just different GRAS forms of these minerals and are only reacting with the potassim phosphate - they're just no longer water soluble, which means a hearty shake to re-mix before drinking. (I've yet to get to a point where I'd been able to add any sort of calcium, as getting the chloride end in balance has been a bearcat as the goldilocks zone of the chloride levels is proving to be quite a narrow band for me, and the magnesium reactions hadn't helped as they were proving to be a distraction.) Ironically, it also means that if I'm aiming for something larger batch shelf stable, so to speak, using any form of magnesium other than tri-mag citrate is my biggest PITA for random reactions... though nearly all the tri-mag citrate on the market currently is all poorly soluble forms sourced out of China. Wheee!

Not that the results from the other two appear to be dangerous. The mag chloride version actually tasted fine again the next day and I didn't have any adverse reactions - which means that hour sampling was probably just getting the full bitterness of the magnesium salts mid-reaction. The mag malate was just producing stuff that needed shaking back in, and it and the zinc gluconate were just neutralizing the citric acid, as would the calcium carbonate if I'd used any yet.

I literally shot myself in the foot and made things more difficult just trying to use more soluble forms of magnesium from a country that has a better track record of producing this sort of stuff without toxic cross-contamination issues from surprise fillers and poor quality control. Guess this realistically means I need to start looking closer at Aquamin Mg... though the additional trace elements hitching a ride from the Celtic Sea could complicate things further, in theory. Maybe I just need to make peace with the Chinese trimag citrate provided it's at least sourced from a reputable seller like NOW FOODS, and hope for mercy and grace to bridge the gaps while having to shake the crap out of the bottle to get it dissolved.

It also means that the simplest and most stable path forward without dealing with wildcard reactions it looks like and from what I'm beginning to understand is to basically use nothing but the alkalized chelated citrate forms of everything (save the sodium chloride and potassium phosphate) from calcium all the way down to zinc (which the latter is hard to source in raw powder form as a supplement), is likely to result in both the most stable and easiest to balance/buffer out using citric acid since they're basically all already stable precipitates and forms that are already where you need to be. The real art will be tweaking the citric acid quantity just enough to get the liquid to a weak buffering acid level just strong enough to impair rapid microbe growth and maybe a slight tang... and that might be easy enough to calculate out by just using a digital pH tester with a little trial and error. Though, it'll likely continue to be a moving target as I try and dial in each of the remaining electrolytes once I get the chloride levels in check.

The irony with this realization is that this was what my gut was telling me to do from the get-go, but the difficulty in finding quality tri-mag citrate and any sort of un-fillered powdered zinc citrate was a source of difficulty, and I was also just trying to work with what I could source. I mean, I literally asked this in the top post: Would I be safer going citrated forms of all the minerals in question given the citric acid usage outside of the sodium chloride and potassium phosphate salts? The answer, apparently, is yes. Yes, you dumbass... a thousand times yes! D'oh!

...that is, unless I'm still missing something, and I always feel like I know there's something important that I don't know with stuff like this. That's the real handicap of being smart enough to know how little you truly understand, and recognizing the limits of what you do know. I can make educated guesses when I don't know, but bluffing is more a risky art than anything else. Though, given where my health is tapdancing these days, along with the challenges of getting any meaningful help on that front given the general state of American healthcare, complicated by the additional defunding and privatization of social safety net services by certain powers that be, compounded by multiple misdiagnoses and the actual medical conditions that have been sussed out being historically poorly understood and barely researched by medical science... nothing like a good tapdance on the razor's edge of risk and mortality to keep the heart a pumping and keep life spicy, I guess.

*sigh* It also means I've mis-stepped a bit financially with this grand experiment. On one hand, it was only about $65, and I've already saved way more than that given how much knock-off/tweaked Liquid IV I've already made the past few months without the magnesium, never mind the financial and health savings of not giving myself a heart attack continuing to take in the amounts of table salt the real deal would have caused at the quantities I'm needing on the potassium/phosphorous end... but still. When money's tight, money's tight. Now, what to do with all this magnesium chloride, magnesium malate, calcium carbonate and zinc gluconate I probably shouldn't use?

Glad I could help!

If you want to verify what the precipitate is, you can run a binary study. Just combine two of your ingredients in the approximate concentrations you'd want in your final solution, and see if you get precipitation. Run it on as small a scale as you have the equipment for, no need to waste material. Try the potassium phosphate with one of the Mag pairs, that should confirm if it's Mg phosphate. (Potassium is soluble with just about everything).

If that is the case, you're likely to see similar precipitation with Mg Citrate, since it's the Mg that's the problem, not the paired ion. Especially for the mag chloride, you've already got chloride in the solution from the sodium chloride, plus chloride is soluble with just about everything, it's a very strong acid (in the pKa sense, not the corrosive sense).

Ultimately, though, if you don't mind having to shake vigorously before use, precipitate might not be a big problem for you. I imagine it mostly impacts absorption? Alternately, heat it up and drink it at tea-like temperatures - you'll get a mild bump to solubility (true for most but not all ion pairs - double check solubility curves).

Oh, one more thing! If you're using a batch within a few days, I wouldn't worry much about microbial growth. At my job, aqueous unbuffered solutions are considered good to use for 7 days. Now that's not for human consumption, but that's also at room temp. Refrigerating for 2-3 days? I wouldn't worry.

Daley

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Re: Chemistry questions
« Reply #12 on: August 13, 2024, 01:53:36 PM »
Glad I could help!

If you want to verify what the precipitate is, you can run a binary study. Just combine two of your ingredients in the approximate concentrations you'd want in your final solution, and see if you get precipitation. Run it on as small a scale as you have the equipment for, no need to waste material. Try the potassium phosphate with one of the Mag pairs, that should confirm if it's Mg phosphate. (Potassium is soluble with just about everything).

If that is the case, you're likely to see similar precipitation with Mg Citrate, since it's the Mg that's the problem, not the paired ion. Especially for the mag chloride, you've already got chloride in the solution from the sodium chloride, plus chloride is soluble with just about everything, it's a very strong acid (in the pKa sense, not the corrosive sense).

Ultimately, though, if you don't mind having to shake vigorously before use, precipitate might not be a big problem for you. I imagine it mostly impacts absorption?
[snip]
Oh, one more thing! If you're using a batch within a few days, I wouldn't worry much about microbial growth. At my job, aqueous unbuffered solutions are considered good to use for 7 days. Now that's not for human consumption, but that's also at room temp. Refrigerating for 2-3 days? I wouldn't worry.

Yeah, I think it mostly just impacts absorption and bioavailability, though they're still medically used forms for both magnesium and phosphorus supplementation. This said, I suspect that given I don't experience much of any difference between the fresh and the stuff with a bit of the white at the bottom of the bottle, given both the phosphorous and the magnesium are kinda critical, at the levels being provided, I doubt it's going to matter too much. I have a habit of shaking pretty much any liquids that aren't water before pouring off a glass to drink, so it doesn't change much realistically.

I'm likely to try and do a couple rounds of testing when I can, but I suspect you're on the right path with it being the magnesium and phosphorous precipitating out. The quicker citric acid neutralization is likely to be explained by the reduction of chloride levels along with the zinc gluconate and the added alkali salts of the magnesium given the quantity of citric acid has remained unchanged with these alterations, now that I'm slightly grokking the reactions a tiny bit more and getting a better grasp on the pH end. Good to know that microbe issues probably aren't a big deal, though. I kinda figured they wouldn't be. After all, juice concentrates and straight sugar-bomb koolaid made with tap water are stable in the fridge for longer than my salty sugar koolaid is.

Now that I'm wrapping my head around things a bit better, I also suspect it's the magnesium addition that's responsible for most of these electrolyte drinks containing both some form of magnesium and potassium phosphate are being sold as powders instead of pre-mixed, and why most are telling you to consume it within 24 hours of mixing. In addition to the B-vitamins breaking down, it probably means the mag phosphate starts precipitating out as the citric acid neutralizes a bit. If the flavor changes enough and you get a white substance on the bottom, even if it's still (mostly) bio-functionally the same, it's likely to freak out and off-put the scientifically illiterate enough to kill sales. I'm reasonably literate, and it still raised enough questions in me and caused me to flounder a bit and order multiple forms of magnesium until I could suss out what was happening and why. This said, I've just found a couple powders with mag citrate listed that doesn't have the 24 hour suggestion.

I've got the trimag citrate, I might as well give it a try to see if it slows down the reaction any or not, given it's supposed to be the most chemically stable form of magnesium salts of the three I have. I don't look forward to the initial mixing, however.

Alternately, heat it up and drink it at tea-like temperatures - you'll get a mild bump to solubility (true for most but not all ion pairs - double check solubility curves).

*shudder* Hot, salty, artificial watermelon lemonade with stevia aftertaste?

...the stuff's barely palatable as is. I'll take my chances with leaving it cold. lol

GuitarStv

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Re: Chemistry questions
« Reply #13 on: August 13, 2024, 01:58:30 PM »
You could always go the college route and dig up a funnel . . .

Fru-Gal

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Re: Chemistry questions
« Reply #14 on: August 13, 2024, 05:45:01 PM »
Interesting thread, not easy for me to understand as I failed chemistry twice LOL.

Therefore allow me to offer some stupid answers… Quick Googling revealed a lemon juice & salt recipe. Perhaps you don’t want the salt, but I was surprised that lemons are so high in potassium. They also have some other beneficial compounds.

https://www.healthline.com/nutrition/foods/lemons#plant-compounds

I wonder if you can get the electrolytes you need from a mixture of whole foods or fresh-squeezed juices?

Here’s another recipe:

https://eatbeautiful.net/homemade-electrolyte-powder-easy-natural-diy-sports-drink/

A lot of the folks who follow Bryan Johnson (longevity guy on YouTube) seem to be hacking their nutrition in similar ways to what you describe for many reasons including specific diseases.

You may be able to find some folks with solutions (ooh, a chemistry joke!) on YouTube.

When I was through-hiking a few weeks ago, electrolytes were important and someone mentioned that some brand had a recipe online that you could use. I can’t remember the brand. (Personally I used Nuun tablets, but I don’t think it was that brand.)
« Last Edit: August 13, 2024, 05:47:08 PM by Fru-Gal »

Daley

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Re: Chemistry questions
« Reply #15 on: August 13, 2024, 07:50:03 PM »
Interesting thread, not easy for me to understand as I failed chemistry twice LOL.

Therefore allow me to offer some stupid answers… Quick Googling revealed a lemon juice & salt recipe. Perhaps you don’t want the salt, but I was surprised that lemons are so high in potassium. They also have some other beneficial compounds.

https://www.healthline.com/nutrition/foods/lemons#plant-compounds

I wonder if you can get the electrolytes you need from a mixture of whole foods or fresh-squeezed juices?

Here’s another recipe:

https://eatbeautiful.net/homemade-electrolyte-powder-easy-natural-diy-sports-drink/

A lot of the folks who follow Bryan Johnson (longevity guy on YouTube) seem to be hacking their nutrition in similar ways to what you describe for many reasons including specific diseases.

You may be able to find some folks with solutions (ooh, a chemistry joke!) on YouTube.

When I was through-hiking a few weeks ago, electrolytes were important and someone mentioned that some brand had a recipe online that you could use. I can’t remember the brand. (Personally I used Nuun tablets, but I don’t think it was that brand.)

Thanks for the effort, @Fru-Gal as your compassion and effort is genuinely appreciated.

Regarding "whole foods" electrolyte drinks... my dietary restrictions and allergies make feeding me expensive enough as is, and given naturally occurring bioavailable phosphorous is a meat-based thing given how non-bioavailable plant-nut-seed based phosphorous is, it's actually cheaper and easier to blend my own playing home pharmacy chemist. More consistent, and easier to track supplement numbers, especially given my need for nearly 2g of elemental potassium a day, which won't uptake into the cells without a large phosphorous kicker.

I've actually been reverse engineering and consulting some of the electrolyte recipes floating around for a few months now while reading dozens of medical papers, and had even successfully fully reverse engineered a couple of commercial models that didn't post recipes online. Regarding the one brand you were thinking of that posted their own recipe, that was LMNT. All these recipes are exercise geared, however, and most of them (like your second link especially) just have way too much damned chloride in them to be safe for long term use for anyone, let alone myself. Heck, I can't even do the official WHO ORS recipe because of that very reason. They use potassium chloride as their potassium vehicle, and I have to use potassium phosphate and potassium citrate to keep from making myself worse.

But regarding that Eat Beautiful recipe especially... I don't point this out to be a jerk, but it is a fantastic learning example. Their recipe is potassium chloride, sodium chloride, and magnesium chloride with maple syrup? WOW, 2.25g of elemental chlorine in a 24oz serving (the one electrolyte number she didn't calculate out)! That is literally a heart attack in a bottle for some people, and if she's actually drinking that on the regular? I wouldn't be a bit surprised if she winds up developing heart and kidney problems longer term. I don't even have that much chloride in a full four liter recipe, and that quantity is only half of what eight servings of Liquid IV would give you, which would also make a full four liters! Taking in less than half that amount daily (around 1g) in 2L of ORS was literally still driving my blood chloride levels through the roof.

The thing to understand is that chloride is the electrolyte that actually helps drive some forms of metabolic acidosis, and is actually the high level heart killer component in table salt... not sodium. Hyperchloremia (high chloride levels) can also strip potassium out of cells causing cellular hypokalemia, something I struggle with, and can also impair renal electrolyte balance functions, which can make electrolyte imbalances worse.

That recipe is also a prime example of why folks should be skeptical of random recipes on the internet, especially recipes when dealing with health stuff. There's a lot of bad advice out there.... and that recipe specifically would absolutely crater me and unravel all the progress I've gotten the past few months trying to reign in my own acidosis issues. Given the modern state of scientific literacy in the general population in an era where everything from astrology to flat earth to yoni crystals are roaring back to life and going mainstream again? This is kind of the perfect example of why it's recommended that most people don't do what I'm doing. If you don't know enough, what you don't know can potentially kill you.

If an idiot like me who's stupid enough to play doctor and pharmacist on himself (granted, out of necessity and not hubris), is somehow still smart enough to recognize this and even be acutely aware of the internalized danger and risk of overconfidence? Know it's the tru-tru.
« Last Edit: August 13, 2024, 07:53:22 PM by Daley »

Fru-Gal

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Re: Chemistry questions
« Reply #16 on: August 13, 2024, 09:05:23 PM »
Wow that is a fascinating response. I myself certainly wouldn’t grab a recipe like hers without a lot of cross-checking, but I did find it interesting that she was saying to avoid a certain brand of one of the minerals because of some kind of contamination or other issue — I was wondering what you’d say to that. And of course you pointed out a completely different issue.

Assuming you are careful to check what you’re doing with other experts to avoid cumulative toxicity I’m sure you’ll succeed.

An aside, history is littered with examples of people who fanatically believed in one element or another (e.g. Linus Pauling). Just today I watched an excellent expose of David Sinclair, who has been selling anti-aging supplements based on the now-debunked resveratrol.

Daley

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Re: Chemistry questions
« Reply #17 on: August 13, 2024, 10:14:02 PM »
Wow that is a fascinating response. I myself certainly wouldn’t grab a recipe like hers without a lot of cross-checking, but I did find it interesting that she was saying to avoid a certain brand of one of the minerals because of some kind of contamination or other issue — I was wondering what you’d say to that. And of course you pointed out a completely different issue.

Yeah, I didn't even bother reading the post itself when I banged that response out. Revisiting and skimming over what she actually has to say just reinforces the conclusion that Megan there is a little too confident in the level of understanding that she dispenses her information to her readers with. I'll just focus on a couple really glaring statements, because I could be here all night if I went over it with a fine-tooth comb, especially if I cite, which I'm not this time. It's been a long day, and I'm tired. I do think the first point is what you're referring to above.

1) She's hard-line anti citrate minerals, because of "mold harvested" citric acid and that it totally causes inflammation, supposedly. Is citric acid produced and extracted from black mold? Yes, and in fact 95% of global citric acid is generated from black mold, if I recall correctly. Could it potentially cause problems if the chemical refinement and purification isn't very good? Absolutely. Is the medical study she used to arrive at this conclusion actually saying this? Not really. It's a single limited study, the quality of citric acid and source wasn't documented, the sample size was limited, and the results were inconclusive as it only caused problems in some people. As such, her understanding is dictating that using chloride salts for electrolyte drinks are somehow the smarter, superior and safer choice.

Meanwhile, sodium citrate and potassium citrate are amazing alkalizing electrolytes for treating systemic acidosis, and can help prevent stuff like uric acid crystals in gout and prevent some forms of kidney stones. And yet, the chloride serving size in her electrolyte mix, which she even has a bulk recipe for her readers, has enough chloride in it to cause a form of non-anion gap metabolic acidosis with frequent enough drinking, which if left in that state long enough could snowball into exciting things like CKD, heart disease, and worse in a significant portion of the population that already struggles with some form of acidosis. All because of one small, incomplete study that said some people experienced mild inflammation from large quantities of citric acid, and since citric acid is made from black mold, clearly all citric acid and citrated minerals must be evil roots of inflammation!

2) She's actively anti potassium iodide, claiming it's an "anti-thyroid" supplement, to the point that she advises her readers to avoid all iodized salt usage. I don't even know entirely where to start with this. Iodine deficiency has been on the rise again since the 1970's despite potassium iodide added to table salt reversing thyroid problems and minimizing goiter incidents in the general population for over 30 years. Why? because of processed and fast foods which don't use iodized salt, and the growing popularity of kosher and sea salts in cooking. Sodium intake has grown considerably, but iodide intake with it has dramatically dropped, and thyroiditis is becoming endemic again amongst the American population. It's been shown that yes, potassium iodide in enough quantity, can suppress thyroid hormone production. That quantity is what's usually found in the over-supplementing numbers that come in a lot of flaky alternative medicine cure-all supplements.

The reality is that hypothyroid and goiter, even with autoimmune based versions like Hashimotos can be benefited with age and weight appropriate RDA guideline trace supplementation of potassium iodide, and hyperthyroid conditions including Graves can ALSO benefit from potassium iodide by taking just enough to limit the overproduction of thyroid hormones. Despite the historical documented success of potassium iodide successfully treating an epidemic of thyroid conditions for decades, her takeaway was that potassium iodide was a dangerous anti-thyroid chemical that nobody should ever take in any quantity because it was found to potentially reduce T3/T4 hormone production when you overdose with it in garbage unregulated supplements!

Something, something, correlation does not equal causation.

She's smart enough to be dangerous, like me... but her scientific literacy could use some work.

At least I have the sense to actually know and recognize the limits of what I both know and don't know. Can I bluster and be a confidently pompous ass at times? Absolutely, especially with topics and advice I'm intimately familiar with. But even then? I would caveat. I recognized there's no one-size solution for everyone... but that sort of tempered advice doesn't sell lifestyle brands and books. Overconfidence from a position of authority does. It's why generative AI has suckered so many people. It's a garbage machine, but what it spits out has an unmatched air of authoritarian confidence. And there's no denying that Megan Stevens writes her advice with a level of authority and confidence that I simply do not. This isn't to say that I think she's necessarily ill intentioned, however. Take that observation for what it's worth.

Meanwhile, people flock and love to follow overconfident idiots who promise to think for them, because of the magnetic draw of that confidence. *gestures in the general direction of a certain tangerine septuagenarian who rambles like he has dementia, rapes women, craps his pants, and is the only millionaire who's repeatedly had to file for bankruptcy with businesses selling gambling, football, and beef to the American public* But boy is he confident!

Assuming you are careful to check what you’re doing with other experts to avoid cumulative toxicity I’m sure you’ll succeed.

That's the hope.

An aside, history is littered with examples of people who fanatically believed in one element or another (e.g. Linus Pauling). Just today I watched an excellent expose of David Sinclair, who has been selling anti-aging supplements based on the now-debunked resveratrol.

Yup, it sure is! Some of the smartest people I've found are frequently also people who have some of the largest, most glaring holes in their worldview and understanding that can manifest in some dangerous levels of incompetence, and it frequently gets tangled up in excruciating levels of confidence rooted in how smart they know/think they are. I detect an unexpected theme.
« Last Edit: August 13, 2024, 10:44:38 PM by Daley »

jim555

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Re: Chemistry questions
« Reply #18 on: August 14, 2024, 04:50:51 AM »
Just curious why you prefer the citrate vs. chloride version for potassium?

Daley

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Re: Chemistry questions
« Reply #19 on: August 14, 2024, 08:05:03 PM »
Just curious why you prefer the citrate vs. chloride version for potassium?

metabolic acidosis
Heck, I can't even do the official WHO ORS recipe because of that very reason. They use potassium chloride as their potassium vehicle, and I have to use potassium phosphate and potassium citrate to keep from making myself worse.
[...]
The thing to understand is that chloride is the electrolyte that actually helps drive some forms of metabolic acidosis, and is actually the high level heart killer component in table salt... not sodium. Hyperchloremia (high chloride levels) can also strip potassium out of cells causing cellular hypokalemia, something I struggle with, and can also impair renal electrolyte balance functions, which can make electrolyte imbalances worse.

Daley

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Re: Chemistry questions
« Reply #20 on: August 14, 2024, 09:02:56 PM »
But regarding that Eat Beautiful recipe especially... I don't point this out to be a jerk, but it is a fantastic learning example. Their recipe is potassium chloride, sodium chloride, and magnesium chloride with maple syrup? WOW, 2.25g of elemental chlorine in a 24oz serving (the one electrolyte number she didn't calculate out)! That is literally a heart attack in a bottle for some people, and if she's actually drinking that on the regular? I wouldn't be a bit surprised if she winds up developing heart and kidney problems longer term. I don't even have that much chloride in a full four liter recipe, and that quantity is only half of what eight servings of Liquid IV would give you, which would also make a full four liters! Taking in less than half that amount daily (around 1g) in 2L of ORS was literally still driving my blood chloride levels through the roof.

I'm revisiting this topic briefly, as I feel like I might have been a little harsher than intended on the recipe itself, and perhaps I should explain why given a superficially passing similarity to the WHO ORS recipe. Although the salt and potassium chloride quantities (and subsequently the chloride loads) aren't extremely deviant from the WHO low-osmolar recipe for 1L of ORS, the sodium to chloride ratios are significantly different due to the lack of additional trisodium citrate (or substituted sodium bicarbonate), which can cause problems.

Further, the salts-to-water ratio is not insignificantly stronger ounce-for-ounce as it's using only 2/3rds of the amount of water recommended for the amount of salts used.

Also, the outline of administration of ORS is designed to be a safe, short-term usage for illness related dehydration to prevent mortality in ill people without access to better health care that's administered slowly throughout the day, not to be guzzled.

Real ORS isn't technically designed for regular use in healthy people and should be used sparingly... much like commercial sports drinks. But, it's also not meant to be guzzled, unlike sports drinks.

Given the further information, especially in relation to an electrolyte recipe that has none of those caveats listed, and has alterations that doesn't improve safety or includes warnings despite a slightly incomplete but similar recipe that vaguely echoes the WHO ORS? You can see why given the changes, the context, and the rationalizations, why I was perhaps a bit... harsh about the recipe. That said, it's still a bad electrolyte replenishment recipe, and remains risky for regular and frequent use for the same reasons I mentioned already.

I'm off the soapbox, now.

Zamboni

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Re: Chemistry questions
« Reply #21 on: August 14, 2024, 09:12:55 PM »
A quick look suggests that your precipitate might be Magnesium Carbonate and/or Magnesium Phosphate, both of which are insoluble in water. Zinc is also insoluble with carbonate and phosphate.

I'm also a chemist. This is correct. The higher charges on these cations and anions make them more attractive to each other (opposites attract, the force of attraction can be calculated with Coulomb's Law) which overcome the entropy associated with them being separated in solution.

markbike528CBX

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Re: Chemistry questions
« Reply #22 on: August 15, 2024, 09:47:43 AM »
A quick look suggests that your precipitate might be Magnesium Carbonate and/or Magnesium Phosphate, both of which are insoluble in water. Zinc is also insoluble with carbonate and phosphate.

I'm also a chemist. This is correct. The higher charges on these cations and anions make them more attractive to each other (opposites attract, the force of attraction can be calculated with Coulomb's Law) which overcome the entropy associated with them being separated in solution.
Non-food chemist here.
I concur on the likely precipitates.  I would note that a normal human stomach has a very low pH[1], with acidity that varies between “battery acid” and lemon juice.  So these precipitates should re-dissolve easily.
The stomach acid also has a lot of chloride.
I’m not sure about the source of the abominable taste, but my bet is the general high pH of the preparation, and the magnesium.
 I wouldn’t suggest trying this at home. Daley is correct in searching for some additional info.

Otherwise mostly posting to follow.
[1]https://www.ncbi.nlm.nih.gov/pmc/articles/PMC7684463/

Daley

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Re: Chemistry questions
« Reply #23 on: August 15, 2024, 09:53:00 AM »
A quick look suggests that your precipitate might be Magnesium Carbonate and/or Magnesium Phosphate, both of which are insoluble in water. Zinc is also insoluble with carbonate and phosphate.

I'm also a chemist. This is correct. The higher charges on these cations and anions make them more attractive to each other (opposites attract, the force of attraction can be calculated with Coulomb's Law) which overcome the entropy associated with them being separated in solution.
Non-food chemist here.
I concur on the likely precipitates.  I would note that a normal human stomach has a very low pH[1], with acidity that varies between “battery acid” and lemon juice.  So these precipitates should re-dissolve easily.
The stomach acid also has a lot of chloride.
I’m not sure about the source of the abominable taste, but my bet is the general high pH of the preparation, and the magnesium.
 I wouldn’t suggest trying this at home. Daley is correct in searching for some additional info.

@Raenia @Zamboni @markbike528CBX

Okay... this is odd, and I'm trusting what's being said here by the lot of you. It sounds like the most reactive of any of the ingredients should be magnesium anything and the potassium phosphate, and the precipitate would be insoluble and detectable. Correct? And of the three forms of magnesium salts available to me, it sounded like the mag chloride tetrahydrate should be the most reactive. Correct?

That's what I was understanding, pulling away from everything, and expecting.

On a lark a couple days ago due to banging my head on the extra hassle trying to dial-in a good sodium to chloride ratio between the sodium chloride and sodium citrate when planning to go citrates down nearly the entire line, I tried making one last batch without any table salt but using the mag chloride tetrahydrate instead, as the math and ease worked out easier on the chloride end to just eliminate the table salt, use sodium citrate exclusively for the sodium end and use the mag chloride exclusively for the chloride end. Fewer ingredients, quicker to calculate, easier to make. Mind, the prior effort where the salts turned bitter an hour after before finally settling back down and had a bit of white precipitate at the bottom and a loss of citric acid tang like the mag malate produced involved a quick prototyping using a pre-made LiquidIV drink stick, which basically had everything in it. This batch was 100% custom crafted, and again, the only real change in ingredient list was the deletion of the sodium chloride and increase in sodium citrate with the inclusion of the magnesium chloride. It's also worth noting that I have found more than a couple commercial powder electrolyte mixes similarly crafted with a mix of the potassium phosphate, sodium citrate, and magnesium chloride, but omitting sodium chloride.

My expectation would be that despite using it, there'd be mag phosphate precipitate, which was still safe and reasonably bioavailable and useful towards the end goals.

This batch? Stable, for nearly 48 hours. No precipitate. None. No loss of citric acid as far as I could taste, though I didn't check for pH shift as I don't have the tools to do that yet given using dip strips with colored liquid could skew the results. No changes in flavor at any noticeable point. Weirdest part? Smoothest drinking ORS batch I've made. Ever.

I'm confused. What did or didn't happen feels like it's above my paygrade. On one hand? I'm thankful and relieved that I've stumbled into a stable blend including the magnesium that coincidentally seems to hit the chloride goldilocks zone effortlessly, but the statements made, and the expectations of which of the ingredients were actually supposed to be reactive didn't shake out, especially since it seems like the real reaction was between the sodium chloride and the magnesium chloride on that first batch.

Can this be explained to me like I'm a toddler? I mean, I guess it doesn't matter if I understand why it's stable or not... just that it IS STABLE should be enough. But I feel like understanding why it did turn out stable might better help me understand how to safely move forward with the calcium and zinc additions, as well... though, something in my gut is just telling me to go with citrated versions of both elements on top of this recipe to potentially avoid problems.

Raenia

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Re: Chemistry questions
« Reply #24 on: August 15, 2024, 09:57:00 AM »
Hm. If you share the ingredients and concentrations (mg/mL or mM) I can poke at it a bit. Possibly it's just that the new concoction is at a lower pH than the previous one, which would help solubility of the Mg.

ETA: I know money is tight right now, but if you can manage it, I'd see if you could get a pH tester that doesn't rely on color - they make cheap ones for beer/wine making. I haven't vetted quality, but I'm seeing some on Amazon for $10ish?

Are these lists accurate? Did both 1 and 2 have precipitate, or just 1?

Batch 1: PrecipitateBatch 2: Weird TasteBatch 3: Better?
Sodium CitrateSodium CitrateSodium Citrate
Potassium CitratePotassium CitratePotassium Citrate
Dipotassium PhosphateDipotassium PhosphateDipotassium Phosphate
GlucoseGlucoseGlucose
Citric AcidCitric AcidCitric Acid
Sodium ChlorideSodium ChlorideN/A
Mg MalateMg ClMg Cl
Ca CarbonateCa CitrateCa Citrate
N/AZn GluconateZn Gluconate
« Last Edit: August 15, 2024, 10:13:03 AM by Raenia »

Daley

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Re: Chemistry questions
« Reply #25 on: August 15, 2024, 10:02:12 AM »
Hm. If you share the ingredients and concentrations (mg/mL or mM) I can poke at it a bit. Possibly it's just that the new concoction is at a lower pH than the previous one, which would help solubility of the Mg.

I'll shoot you (and the others - if they want) a PM with the ingredient list. I don't want to publish it publicly to avoid having others blindly recreating what I'm doing to use themselves, given the slightly risky nature of it all, and the fact that the numbers in the recipe are somewhat tailored specifically to my own metabolism defects.

Raenia

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Re: Chemistry questions
« Reply #26 on: August 15, 2024, 10:13:57 AM »
Hm. If you share the ingredients and concentrations (mg/mL or mM) I can poke at it a bit. Possibly it's just that the new concoction is at a lower pH than the previous one, which would help solubility of the Mg.

I'll shoot you (and the others - if they want) a PM with the ingredient list. I don't want to publish it publicly to avoid having others blindly recreating what I'm doing to use themselves, given the slightly risky nature of it all, and the fact that the numbers in the recipe are somewhat tailored specifically to my own metabolism defects.

I can work without numbers for now - just want to make sure I have accurate ingredient lists and what was observed on each batch. I'm not 100% sure I've accurately understood which batches had, e.g. Zinc added, for instance.

Also happy to talk by PM if that works better.
« Last Edit: August 15, 2024, 10:19:52 AM by Raenia »

Daley

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Re: Chemistry questions
« Reply #27 on: August 15, 2024, 06:34:41 PM »
I think I grok it now. I accidentally made a citric acid buffer solution on the last recipe revision. Neat!

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Re: Chemistry questions
« Reply #28 on: August 18, 2024, 01:22:41 PM »
I am not a food chemist. But my grandfather was, he designed food products and baby formula from 1950 -1980 and continued to do research even after he retired well into his 90s. He and lived to be 102 and passed away last year. He shared with me some good advice that seems like I could share it here. Hydrogen Peroxide, in small amounts is very good for you and will kill all sorts of pathogens in the body.  He used it as mouthwash every night and put an eyedropper full in his OJ at breakfast every morning. He said it works as well as any prescription ointment for cold sores, and I have found that to be true.
I'm not sure if that helps with your dilemma but I thought you would find it interesting.

Daley

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Re: Chemistry questions
« Reply #29 on: August 18, 2024, 02:06:39 PM »
I am not a food chemist. But my grandfather was, he designed food products and baby formula from 1950 -1980 and continued to do research even after he retired well into his 90s. He and lived to be 102 and passed away last year. He shared with me some good advice that seems like I could share it here. Hydrogen Peroxide, in small amounts is very good for you and will kill all sorts of pathogens in the body.  He used it as mouthwash every night and put an eyedropper full in his OJ at breakfast every morning. He said it works as well as any prescription ointment for cold sores, and I have found that to be true.
I'm not sure if that helps with your dilemma but I thought you would find it interesting.

Appreciate the effort, Dave. FWIW, I'm familiar with H2O2 therapy... unfortunately, it's a little too risky for folks with autoimmune and/or thyroid disorders, and requires the added hurdle of sourcing actual food grade peroxide off of miserable counterfeit shopping holes like Amazon.