Originally posted by kmno4
Hehe....
Practical problem:
We have: 0,01 mol/dm3 H2SO4 (let's say there is no HSO4(-) ion dissociation) and 0,01 mol/dm3 HBr.
Let's mix equal volumes of these solutions - what is pH of this mixture ?
ps. on the picture I attached you can see that H2SO4 is more acidic than HCl and even HClO4 (up to concentration ~7 mol/dm3).
Surely H2SO4 is also more acidic than HBr, not because of its volatility ....
In Brauer or IS there is described simple procedure for making HBr:
Dissolve 120g KBr in 200g H2O and cool. Next, slowly add 90 ml conc. H2SO4 keeping temp. below 75 C. Cool it to room temp. and filter off
KHSO4 crystals (solution is distilled to obtain HBr(aq) azeotrope)...
[Edited on 25-2-2009 by kmno4] |