What is the Product of Magnesium Bicarbonate and D-Ribose
Post new topic Reply to topic
   Chemical Community Forum Index : Chemistry forum
View previous topic :: View next topic  
Author Message
yerrag
Jr. Member
Jr. Member


Joined: 07 Oct 2018
Posts: 6
Location: Manila
Reply with quoteFind all posts by yerrag

What is the Product of Magnesium Bicarbonate and D-Ribose


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?reaction=Mg%28HCO3%292%2BC9H10O5%3DMg%28C9H10O4%292%2BCO2%2BH2O

What is Mg(C9H10O4)2? I can't find it on Google, Bing, or Yandex.

Thanks.
Back to top
View user's profileSend private message
ChenBeier
Distinguished Member
Distinguished Member


Joined: 27 Sep 2017
Posts: 353
Location: Berlin, Germany
Reply with quoteFind all posts by ChenBeier


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
Back to top
View user's profileSend private message
yerrag
Jr. Member
Jr. Member


Joined: 07 Oct 2018
Posts: 6
Location: Manila
Reply with quoteFind all posts by yerrag


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?
Back to top
View user's profileSend private message
ChenBeier
Distinguished Member
Distinguished Member


Joined: 27 Sep 2017
Posts: 353
Location: Berlin, Germany
Reply with quoteFind all posts by ChenBeier


Correct, but why do u want to mix it.
Back to top
View user's profileSend private message
yerrag
Jr. Member
Jr. Member


Joined: 07 Oct 2018
Posts: 6
Location: Manila
Reply with quoteFind all posts by yerrag


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?
Back to top
View user's profileSend private message
ChenBeier
Distinguished Member
Distinguished Member


Joined: 27 Sep 2017
Posts: 353
Location: Berlin, Germany
Reply with quoteFind all posts by ChenBeier


Something must be acidic, otherwise no CO2 will be released. Which pH is the ribose dissolved in water?
Back to top
View user's profileSend private message
yerrag
Jr. Member
Jr. Member


Joined: 07 Oct 2018
Posts: 6
Location: Manila
Reply with quoteFind all posts by yerrag


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!
Back to top
View user's profileSend private message
Display posts from previous:   
Post new topic Reply to topic
   Chemical Community Forum Index : Chemistry forum Page 1 of 1

 
Jump to:  

Chemical portal