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Confusing Magnesium Glycinate Label

?

:^)

Greenlighter
Joined
Mar 13, 2014
Messages
29
Hey all, long time lurker here.

I recently got a 1kg bag of magnesium glycinate. The label clearly states that nothing but pure magnesium glycinate is present. However, the label reads:
Serving Size: 2200 milligrams
Servings per container: 454
Amount per serving: Magnesium (as Magnesium Glycinate) 401mg

Would 2200 milligrams of magnesium glycinate not contain 2200mg of Magnesium Glycinate?

I can only assume it's because the 401mg refers to the actual Magnesium and the rest comes from the Glycine, but I can't get the math to work out (though I don't know the subject thoroughly). It seems to leave at least 500mg unaccounted for. Could it be a misprint, or can someone explain the math/science? I'd like to get the dosing right.

Thanks!
 
Because there are 401mg of Magnesium in that Magnesium glycinate.

I don't know how that reaction occurs, maybe someone else can give a formula, but your correct in assuming its referring to the pure mg content before reaction.
 
CloudyFluffy said:
Hi guys,

I think he is a undercover agent or something :sus: :(
Click to expand...

Correct. I'm here to bust anyone who paid attention during chemistry class.

@bob loblaw feel free to answer when you regain consciousness.

Also, it is interesting that although it recommends a dose of about 2200mg of the powder (~tsp), almost every review claims that to be too much and recommends to use 1/8 tsp (~225mg) to 1/4 tsp (~550mg), which would be more on par with the recommended dosage of ~400 mg. You'd expect a full tsp to be necessary if 2200mg really yields 400mg of magnesium.

thanks everyone
 
Anyone want to show of they're math/chemistry skills so I can come to a definite conclusion? Or is the label wrong? I know there are some wicked shmart people here. It'd be much appreciated.
 
It's already been explained, but the discrepancy is because of the sum weight of the glycine groups (well, organic ions). The measure of the magnesium only includes the weight of the magnesium ions, while "magnesium glycinate" accounts for the weight of both ions.

ebola
 
Thanks everyone, though I guess I should have been a little bit clearer. I understand that overall, the discrepancy from the sum weights of the ions.The answer I'm looking for is just a bit more advanced. I'm looking for a bit more of a simplified mathematical "proof" to show me if it is my basic understanding of math/chemistry that is off, or if it is the label. Here's why:

The atomic weight of Magnesium is ~24. The atomic weight of Magnesium Glycinate is ~176. The ratio of the masses, then, is about 1:7.3333... Based on that, you would expect ~2940mg (not 2200mg) of Magnesium Glycinate to contain 401mg of Magnesium. Combine that with the reviews claiming that 2200mg is far too much for this product and that ~225mg - ~550mg of TOTAL weight, which would yield a sub-active dose of Mg according to the above (yes you can 'feel' Mg supplemenation), is necessary, I am at a loss.

Anyone understand what I'm asking?
 
Yeah I understand.
You're saying that according to your calculations, there should be less than 401 mg of Mg in 2200 of Mg Glycinate.
And some people are saying that you need much less than 2200.
The company that makes this product is probably recommending this big dose so that they make more profit. And they may have done wrong calculations. Can you post a pic of the label?
 
@flyhighk Exactly.
ngGA8u7


Can you see the pic?
 
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magnesium + some crap its attached to = overall weight
the magnesium only weight is called elemental magniusm...

for example Magnesium Orotate 654mg = 40mg elemental magnesium................ so u get 614mg of orotate as side effect

minerals are bound with all kinds of shit,the supermarket of the shelf mainstream cheap stuff is horrible.... calcium carbonate,zinc oxide etc
 
@DOB Yeah we got that part, thanks though. I understand the basics very well. The problem is that none of the math comes out correctly. If it did, I would know the correct dose. But since it doesn't (or until someone shows the exact way it does), I have no way of knowing what does I actually am/should be taking and have to assume that the labeling is off in some way. Mods, is there any way this can be put somewhere focused on math/chemistry? The problem lies in a field a bit more 'advanced' than Healthy Living.
Also, if someone could clue me in on the method of posting a picture that works the best, that'd be great (assuming this doesn't work).

http://imgur.com/ngGA8u7
 
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The molar mass of Gly- is 74, the molar mass of Mg2+ is 24.3. If 2200 mg of magnesium glycinate contain 400 mg of magnesium with Mg and Gly as the only ingredients, the molar glycine content as a proportion of molar magnesium content is given by the solution to:

400 = 2200 * 24.3 / (24.3 + x*74) >> x ≈ 1.5, so the natural expectation is that 1.5 moles of glycine are present for every mole of magnesium. Of course Mg(gly)2 has "too much glycine" in this calculation.

Another explanation is that what you are looking at is actually hydrated Mg(gly)OH or similar. The formula Mg(gly)OH*H2O gives exactly 401 mg of Mg per 2200 mg of product. Magnesium salts of this form are probably hygoroscopic, so the use of a hydrate is not all too surprising: this is equivalent to a chelate gly + MgO + H2O. However, as you've seen, it is not too hard to put things into the equation to make the numbers work the way you want, so the only way to get a real answer is to analyze the material itself.
 
It's most likely a hydrated form. Ta da.

No mystery

Edit: I see atara already got there.
 
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