AzoMittle Posted September 1, 2014 Share Posted September 1, 2014 In compositions that use Boric Acid to control nitrate/Aluminum reactions Sodium bicarbonate will cancel it out, is the same true of the oxalate? or what about other (bi)carbonates such as Strontium carbonate or Barium carbonate? I searched the forums but found nothing, same regarding the Sodium oxalate pH. I also remember seeing somewhere that Boric acid is incompatible with either magnesium or magnalium or something but I can't seem to find anything regarding that now. Does anyone know anything about that? Link to comment Share on other sites More sharing options...
schroedinger Posted September 1, 2014 Share Posted September 1, 2014 Sodium oxalat consist out of NaOH and oxalic acid, so a strong base and weak acid are combined, this results in a salt which reacts basic. But I'm not sure if it will react with boric acid.Bicarb will react with boric acid as every other carbonate should do. Link to comment Share on other sites More sharing options...
Mumbles Posted September 2, 2014 Share Posted September 2, 2014 Sodium oxalat consist out of NaOH and oxalic acid, so a strong base and weak acid are combined, this results in a salt which reacts basic. But I'm not sure if it will react with boric acid.Bicarb will react with boric acid as every other carbonate should do. Bicarbonate is not the same as carbonate. They will react differently. Sodium bicarbonate does not react with boric acid. Try it out. Mix them. No bubbling at ambient conditions. If you heat it, you can drive the reaction though. The pKa's will confirm this. Acid/base reactions want to make the weakest acid and weakest base combo that it can. In this case that combination is bicarbonate and boric acid, not carbonic acid and "B(OH)2O-". Oxalate is the same way. Being a much stronger acid than boric acid, will not be protonated by it. I honestly don't know about carbonate. In general, the carbonate ion will react to bicarbonate at room temperature. However the three we commonly use, copper, strontium, and barium, are very poorly soluble in water. Additionally, their bicarbonates tend to be unstable. I really don't know if the instability and solubility would prevent it from being formed, or drive the reaction forward. Link to comment Share on other sites More sharing options...
AzoMittle Posted September 5, 2014 Author Share Posted September 5, 2014 Bicarbonate is not the same as carbonate. They will react differently. Sodium bicarbonate does not react with boric acid. Try it out. Mix them. No bubbling at ambient conditions. If you heat it, you can drive the reaction though. The pKa's will confirm this. Acid/base reactions want to make the weakest acid and weakest base combo that it can. In this case that combination is bicarbonate and boric acid, not carbonic acid and "B(OH)2O-". Oxalate is the same way. Being a much stronger acid than boric acid, will not be protonated by it. I honestly don't know about carbonate. In general, the carbonate ion will react to bicarbonate at room temperature. However the three we commonly use, copper, strontium, and barium, are very poorly soluble in water. Additionally, their bicarbonates tend to be unstable. I really don't know if the instability and solubility would prevent it from being formed, or drive the reaction forward. I can confirm this. I did not test Sodium oxalate with anything however. Boric acid + Sodium bicarbonate + water = No noticeable reaction Boric acid + Sodium bicarbonate + water + heat = Bubbles, I could not tell if this was from an actual chemical reaction or simply the water boiling however, or both Sodium bicarbonate + Strontium carbonate + water = No noticeable reaction Boric acid + Strontium carbonate + water = No noticeable reaction Link to comment Share on other sites More sharing options...
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