It is a strong acid.
Hint: if the formula begins with H it is usually an acid.
No. HBr is a strong acid.
HBrO is a weak acid. In solution it partially deprotinates to form BrO- and H+
acid is hbr and the base is h2o
HBr is a strong acid.
Hydrobromic acid has a pKa of −9, making it a stronger acid than hydrochloric acid, but not as strong as hydroiodic acid. Hydrobromic acid is one of the strongest mineral acids known.
No. HBr is a strong acid.
HBrO is a weak acid. In solution it partially deprotinates to form BrO- and H+
acid is hbr and the base is h2o
HBr is a strong acid.
Hydrobromic acid has a pKa of −9, making it a stronger acid than hydrochloric acid, but not as strong as hydroiodic acid. Hydrobromic acid is one of the strongest mineral acids known.
This does not make a buffer because HBr is a STRONG acid, and for a buffer you need a WEAK acid and the salt of the acid.
Bromine itself is not considered an acid. However, it can react with water to a small degree to form hydrobromic acid (HBr), a strong acid and hypobromous acid (HBrO) a weak acid. Br2 + H2O --> HBr + HBrO
HCl is hydrochloric acid HI is hydroiodic acid HF is hydrofluoric acid H2SO4 is sulfuric acid HNO3 is nitric acid HBr is hydrobromic acid HClO4 is perchloric acid
HBr is an acid. It gives hydroxonium ions and bromide ions when dissolving in water.
because it is a strong acid
No, it is a diprotic acid, the first protolysis is strong, the second is (somewhat) weaker, however also this can be regarded as stong. (miscalculation << 0.3 pH unit)
There is no conjugate) base coupled to bromide, Br-, because this Br- can NOT donate (by protolysing) a proton (H+) in water.However Br- itself is the very, very weakest base of the (very, very) strong conjugate acid HBr.This is the only possible conjugate acid/base pair:HBr/Br-