Glycine/Hydrazine Buffer: Trapping Pyruvate as Hydrazone

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SUMMARY

The discussion centers on the use of a glycine/hydrazine buffer at pH 9.0 for trapping pyruvate as a hydrazone. The initial confusion regarding the pH value was clarified, confirming that the correct pH is indeed 9.0. The participants emphasized the importance of understanding hydrazone formation in this context. This reaction is significant for those studying biochemical pathways involving pyruvate.

PREREQUISITES
  • Understanding of hydrazone chemistry
  • Knowledge of buffer solutions and their pH levels
  • Familiarity with pyruvate and its biochemical roles
  • Basic principles of organic chemistry
NEXT STEPS
  • Research the mechanism of hydrazone formation
  • Study the properties and applications of glycine/hydrazine buffers
  • Explore the role of pyruvate in metabolic pathways
  • Learn about pH control in biochemical reactions
USEFUL FOR

Biochemists, organic chemists, and students involved in metabolic research or buffer chemistry will benefit from this discussion.

nobahar
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Hello!
I think this is going to be one of those unread questions that disappear into the abyss, so I'll shorten in hopes of a reply:
What exactly does this mean: "If the reaction is carried out in a glycine/hydrazine buffer pH0.9, then pyruvate is trapped as the hydrazone and H+ the buffer."?
I can't seem to find any straightforward information concerning this; or not at least I can follow...
Any help appreciated.
Thanks!
 
Last edited:
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First of all - are you sure it is pH 0.9? Not pH 9.0?

Check what hydrazone is.
 
Sorry! Yeah it's pH 9.0. I'll have a look, but I am just about to post a more pressing question that I have.
 

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