Hi, so I tried to make some HBr the other day, using NaBr and H2
as precursors. I measured out 2 molar equivalent of NaBr, and 1 molar equivalent of H2
. I then dissolved the NaBr in distilled H2
2O (maybe a bit too much), and then slowly dripped the sulphuric acid into the solution (to keep the temperature below about 60°C.
So far so good...
Next I tried to distill off the excess water, which worked fine at first, but after a while the solution being distilled turned cherry red! Its pH was below 0 and the pH of the clear solution in the collection flask had pH about 1.
At this point I stopped the experiment. I tried to pour the red solution into a bottle for storage, but as I was pouring it immediately crashed out of solution (looking a bit like an orange slushy). Adding more water helped it dissolve the slushy again and made its colour more yellow.
Could anybody help me understand what had happened? (As you can tell I still have much to learn...
My plan for now is this: Distill everything off at about 125°C and collect it (this should be aqueous HBr). The red slushy that will be left over will likely be Na2
has its uses I wouldn't mind collecting it... its soluble in organic solvents so maybe I can rinse it with ether or something, since ether has a lower boiling point than Br2
. That way I could keep some.
Alternatively if people think this isn't a good idea I would also be curious how one can properly get rid of Na2
contaminated with Br2
Any avice would be greatly appreciated, since I certainly don't just want to flush it down the drain