Chemistry Forum

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.

If die Ribose is acidic in Water, then dicarbonate will release CO₂ and Water. But the product is wrong, Why should it loose oxygen.

Hmm.
??
That would explain why there is no such product on my search.

But I'm at a loss as to what magnesium compound would result from the reaction.

If d-Ribose is non polar, it should not lose an electron to become an anion, right?

Correct, but why do u want to mix it.

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?

Something must be acidic, otherwise no CO₂ will be released. Which pH is the ribose dissolved in water?

I finally realize what happened.

The magnesium bicarbonate didn't self-destruct. It stayed the same.

The d-ribose seeded (there's a better word for it) the dissolved CO₂ that I failed to mention was in the water. CO₂ started to come out from solution and this caused the fizz.

Thanks ChenBeier!