chornedsnorkack - 22-3-2014 at 12:42
What are they composed of?
First, note that bromine of course can dissolve molecularly.
Second, note that while chlorine is slightly stronger oxidant than oxygen, bromine should be weaker. The reaction
2Br2+2H2O<->4HBr+O2
should stay on the left side unless somehow driven out of equilibrium.
The first step of bromine hydrolysis should be:
Br2+H2O<->HBr+HBrO
mainly on the left.
But the problem is that hypobromites are more easily dismuted than hypochlorites. The reaction
3HBrO->2HBr+HBrO3
is said to go to right and proceed slowly at 0 Celsius but rapidly in 20 Celsius.
It follows that bromine hydrolysis, in long term, has net result
3Br2+3H2O<->5HBr+HBrO3
Still reversible... but balance rather further to the right than the hydrolysis to hypobromite... meaning correspondingly bigger solubility of
bromine..
Does anyone know what is the total solubility of bromine in water, and what are the concentrations of molecular Br2, HBrO and HBrO3 at the long term
equilibrium?
Assuming that it is a solution of small amount of liquid bromine.
And what is the composition of water bromine?
Bromine, unlike water is nonpolar... and should be a poor solvent for polar substances.
Since HBr is completely dissociated in water, it should partition into water. HBrO3 is also a strong acid.
But how about HBrO? It is a weak acid. Does HBrO dissolve appreciably in bromine?
What is the composition of bromine in equilibrium with a small amount of liquid water? How much hydrogen and oxygen are found in wet bromine?
Texium - 22-3-2014 at 19:20
According to the reference book that I have, bromine's solubility is 41.7g/L at 0˚C, and 35.2g/L at 50˚C. Bromine is much more soluble in
organic solvents.
Also, it makes no note of HBrO being soluble in bromine, although it is highly soluble in water.