Injectable Glutathione Recipe

[bigMoJo]

The OP did but I think he bailed on using it. Here was someone’s explanation of what was happening.

Did some googling and came across this, kinda interesting.

Sodium bicarbonate NaHCO3 is slightly soluble in water, H2 O. NaHCO3 dissolves in H2 O to yield carbonic acid H2 CO3 and sodium hydroxide NaOH: NaHCO3 + H2 O → H2 CO3 + NaOH. Note that the carbonic acid breaks down further to form water and carbon dioxide CO2 gas: H2 CO3 → H2 O + CO2.

So it looks like you are still making sodium hydroxide when you use sodium bicarbonate.

https://homework.study.com/explanation/does-sodium-bicarbonate-react-with-water.html#:~:text=Answer%20and%20Explanation:,H2%20O%20+%20CO2.

That's partially correct. However, the water becomes "carbonated" from the CO2, it doesn't release into gas unless mixed with something highly acidic or if heated.

I think sodium bicarb may be easier to use and better for the solution, because carbonated water is also found in the bloodstream. Sodium is also in the blood. In fact, that's why saline drips/IVs use NaCl (Sodium Chloride)... water in the blood will rupture blood vessels... in contrast, NaCl helps absorption and closely mimics human blood. NaOH is "kinda" doing the same thing, but it's causing instability in the solution your are "mixing."

I use sodium bicarb to raise pH on my acidic peptides, but I mix with bac and liquid form sod. bic. Additionally, pharma brand Glut. is lypholized with sodium bicarb... I've not seen any with NaOH.

To make it easy... I use 2:1 ratio for bac and sodium bicarb for 200mg Glut. That ratio should get your pH just above 7.

Also, here is an explanation I found on Quora by a PhD regarding water and sodium bicarb... hope all this helps out...
------------------------------------

When you add baking soda (sodium bicarbonate, NaHCO₃) to water, it undergoes a physical dissolution process and a slight chemical reaction:

Dissolution
Baking soda dissolves in water, dissociating into its ionic components:
NaHCO₃ → Na⁺ + HCO₃⁻

Here, sodium ions (Na⁺) and bicarbonate ions (HCO₃⁻) are released into the solution. This is a physical process and does not involve breaking or forming of covalent bonds.

Chemical Reaction (Partial Ionization of Bicarbonate)
In water, bicarbonate ions (HCO₃⁻) can act as a weak base and interact with water molecules. A small fraction reacts to form carbonic acid (H₂CO₃) and hydroxide ions (OH⁻):
HCO₃⁻ + H₂O ⇌ H₂CO₃ + OH⁻

This makes the solution slightly basic, with a pH around 8 to 9 depending on the concentration.

Additional Effects
If the solution is heated or mixed with an acid, bicarbonate ions can further decompose into carbon dioxide (CO₂) gas and water:
HCO₃⁻ → CO₂ + H₂O

This reaction is why baking soda fizzes when combined with acidic substances like vinegar.

Eventually…
When added to water, baking soda primarily dissolves and slightly alters the water's pH, making it mildly alkaline. This property is why sodium bicarbonate is often used as an antacid, water softener, and in household cleaning.

 

[mochul]

The OP did but I think he bailed on using it. Here was someone’s explanation of what was happening.

Did some googling and came across this, kinda interesting.

Sodium bicarbonate NaHCO3 is slightly soluble in water, H2 O. NaHCO3 dissolves in H2 O to yield carbonic acid H2 CO3 and sodium hydroxide NaOH: NaHCO3 + H2 O → H2 CO3 + NaOH. Note that the carbonic acid breaks down further to form water and carbon dioxide CO2 gas: H2 CO3 → H2 O + CO2.

So it looks like you are still making sodium hydroxide when you use sodium bicarbonate.

https://homework.study.com/explanation/does-sodium-bicarbonate-react-with-water.html#:~:text=Answer%20and%20Explanation:,H2%20O%20+%20CO2.

Buddy your are compelrtly wrong. Sodium bicarbonate just disassociates in water not decomposed. Upon heating it turns into sodium carbonate thats why you don’t see it react when mixed with water

 

[LGOP528]

Buddy your are compelrtly wrong. Sodium bicarbonate just disassociates in water not decomposed. Upon heating it turns into sodium carbonate thats why you don’t see it react when mixed with water

I saw the same reaction in several different places but I posted it so people who know more than me would clarify. That was my goal here. @bigMoJo did just that.

We are also mixing in a very acidic solution so I understand that the reaction with water is a completely different situation.

If my original post came across as me making some sort of claim I apologize. I tried to word it in away that did not leave that impression.

Why doesn't sodium bicarbonate dissolved in water spontaneously effervesce when carbonic acid does?

It's well known that if you put carbonic acid $\ce{H2CO3}$ into water it will dehydrate into carbon dioxide $\ce{CO2}$ and water $\ce{H2O}$. Indeed this is how modern fizzy drinks generate their fi...

chemistry.stackexchange.com

 

[bigMoJo]

I saw the same reaction in several different places but I posted it so people who know more than me would clarify. That was my goal here. @bigMoJo did just that.

We are also mixing in a very acidic solution so I understand that the reaction with water is a completely different situation.

If my original post came across as me making some sort of claim I apologize. I tried to word it in away that did not leave that impression.

Why doesn't sodium bicarbonate dissolved in water spontaneously effervesce when carbonic acid does?

It's well known that if you put carbonic acid $\ce{H2CO3}$ into water it will dehydrate into carbon dioxide $\ce{CO2}$ and water $\ce{H2O}$. Indeed this is how modern fizzy drinks generate their fi...

chemistry.stackexchange.com

I didn't see it that way bro, I don't think you came across that way. I believe we're all trying to be helpful and come up with the best solution.

I also didn't touch on the nuances of the different "buffers"... just saying it's causing "instability in the solution."

It seems OP never went with the NaHCO₃ route, and went with NaOH from the start. I may need a few days to post it, but I have some info saved on the differences of each chemical reaction.

Essentially, one produces bicarbonate ions, the other hydroxyl ions when mixed with water. This difference (and IIRC something else) makes NaOH more "volatile" in the mix versus NaHCO₃. I beleive this is why getting the pH right and the solution clear is difficult when using NaOH. Like I previously mentioned, NaHCO₃ is easier to use.

But, I'll back-up what I'm saying with the info I have. I just have to look through and find it.

Also, after my initial post, I started sourcing raws for this so I can help with the actual hands-on "recipe."

 

[LGOP528]

I didn't see it that way bro, I don't think you came across that way. I believe we're all trying to be helpful and come up with the best solution.

I also didn't touch on the nuances of the different "buffers"... just saying it's causing "instability in the solution."

It seems OP never went with the NaHCO₃ route, and went with NaOH from the start. I may need a few days to post it, but I have some info saved on the differences of each chemical reaction.

Essentially, one produces bicarbonate ions, the other hydroxyl ions when mixed with water. This difference (and IIRC something else) makes NaOH more "volatile" in the mix versus NaHCO₃. I beleive this is why getting the pH right and the solution clear is difficult when using NaOH. Like I previously mentioned, NaHCO₃ is easier to use.

But, I'll back-up what I'm saying with the info I have. I just have to look through and find it.

Also, after my initial post, I started sourcing raws for this so I can help with the actual hands-on "recipe."

That would be much appreciated! I am really getting into brewing these different amino acids.

 

[bigMoJo]

That would be much appreciated! I am really getting into brewing these different amino acids.

We're going down the "rabbit-hole" bro!

 

[Govertical19]

So I tried a couple batches and they both are cloudy. Ph is around 5. Should I trash them or try them?

 

[LGOP528]

So I tried a couple batches and they both are cloudy. Ph is around 5. Should I trash them or try them?

What concentration are you trying to make? What are you using to test the PH?

 

[sinistral]

So I tried a couple batches and they both are cloudy. Ph is around 5. Should I trash them or try them?

If they are cloudy then the pH is too low. Keep adding buffer but more slowly now. I usually shoot for something slightly over 6.

 

[Govertical19]

If they are cloudy then the pH is too low. Keep adding buffer but more slowly now. I usually shoot for something slightly over 6.

Man I can not figure it out. Never got clear and ph is high over 9

 

[sinistral]

Man I can not figure it out. Never got clear and ph is high over 9

Never turned red on you either? You sure you have glutathione base? You can't use any formulation except pure reduced glutathione.

Something like this:

Amazon.com

Also, what are you using for the buffer? You can use something like this:

Amazon.com

 

[Duke309]

I ended up brewing glutathione at 400mg/ml with the belle chem pharm L-Glutathione reduced. I started at a concentration of >500mg/ml and used a 10% sodium hydroxide solution to dilute. I got a little impatient and pH went over 7. Solution cleared up and looked great. I filtered it and put it in the refrigerator. Drawing 1ml with 29g slin pin takes a few minutes, but it is painless and easy to shoot. Next time I would probably go with 500mg/ml and just draw it with a bigger gauge pin and backfill the slin pins.

 

[Govertical19]

Never turned red on you either? You sure you have glutathione base? You can't use any formulation except pure reduced glutathione.

Something like this:

Amazon.com

Also, what are you using for the buffer? You can use something like this:

Amazon.com

I have the bulk supply reduced glutathione

 

[Govertical19]

I ended up brewing glutathione at 400mg/ml with the belle chem pharm L-Glutathione reduced. I started at a concentration of >500mg/ml and used a 10% sodium hydroxide solution to dilute. I got a little impatient and pH went over 7. Solution cleared up and looked great. I filtered it and put it in the refrigerator. Drawing 1ml with 29g slin pin takes a few minutes, but it is painless and easy to shoot. Next time I would probably go with 500mg/ml and just draw it with a bigger gauge pin and backfill the slin pins.

What was the formula you used for this?

 

[LGOP528]

What was the formula you used for this?

What are the weights and volumes that you are using?

 

[Govertical19]

What are the weights and volumes that you are using?

I was following the op post. Is there a update to the recipe

 

[jasonsta]

Do you know a website that sells reduced glutathione powder in Europe?

I ordered from meinarztbedarf.com, but I think I got scammed.
The order status hasn't changed

 

[LGOP528]

I was following the op post. Is there a update to the recipe

No update.

Just a piece of advice, I write down all measurements every time I make a batch. It helps me with the process and I can go back and see if I made a mistake.

 

[sinistral]

Do you know a website that sells reduced glutathione powder in Europe?

I ordered from meinarztbedarf.com, but I think I got scammed.
The order status hasn't changed

Can you buy direct from Belle Chemical from Europe?

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[sinistral]

Do you know a website that sells reduced glutathione powder in Europe?

I ordered from meinarztbedarf.com, but I think I got scammed.
The order status hasn't changed

Actually @Sampei might be able to help here.