I put d-ribose into a magnesium bicarbonate solution and it fizzed. So I wondered what could be going on. I used the Chemical Equation Balancer and this is what I got:
https://www.webqc.org/balance.php?react ... BCO2%2BH2O
What is Mg(C9H10O4)2? I can't find it on Google, Bing, or Yandex.
Thanks.
What is the Product of Magnesium Bicarbonate and D-Ribose
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If die Ribose is acidic in Water, then dicarbonate will release CO2 and Water. But the product is wrong, Why should it loose oxygen.
Last edited by ChenBeier on Thu Mar 26, 2020 4:08 am, edited 1 time in total.
I was just surprised that adding d-ribose to my magnesium bicarbonate drink would result in fizz, which signifies CO2 being released from a reaction.
I'm now curious as to what form of magnesium results. There was no precipitation of whatever form it is, it is soluble. Likely an organic acid but I don't know what.
It appears then that the d-ribose was just a catalyst for the magnesium bicarbonate to, for lack of a better word, to self-react and release CO2. The d-ribose seeded the reaction, is that the right way to say it?
I'm now curious as to what form of magnesium results. There was no precipitation of whatever form it is, it is soluble. Likely an organic acid but I don't know what.
It appears then that the d-ribose was just a catalyst for the magnesium bicarbonate to, for lack of a better word, to self-react and release CO2. The d-ribose seeded the reaction, is that the right way to say it?