Acid + base salt + water
An acid donates an H+, and a base accepts an H+.
A Bronsted-Lowry base accepts a proton from something else.
They are both strong acids/weak bases however Br is the stronger acid and by that definition the weaker base.
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-
No, Br- is not a base. Br- is the bromide ion, a conjugate base of hydrobromic acid (HBr). It is a negatively charged ion and can act as a weak base in certain reactions, but it is not considered a base in general chemistry terms.
Br can act as a Lewis base by donating its lone pair of electrons to form a coordinate covalent bond with a Lewis acid.
None of the above. Br- is neutral, with no acidic or basic properties
No, Br- is not an Arrhenius base. It is the conjugate base of hydrobromic acid (HBr) and would act as a base in a Brønsted-Lowry sense by accepting a proton.
yes it is, because HBr is a stronger acid than HCl, therfore, HBr will have a weaker conjugate base, Br, than HCl, Cl
Bromine (Br) is a nonmetal element and is neither an acid nor a base. In its elemental form, bromine does not exhibit typical acidic or basic properties.
No, Br (bromine) is not typically considered a Lewis base. Lewis bases are electron pair donors, while bromine typically does not donate electrons in chemical reactions.
In the reaction, HBr donates a proton (H+) to H2O, making HBr the acid and H2O the base. The resulting products are Br- (conjugate base of HBr) and H3O+ (conjugate acid of H2O).