Bronsted-lowery Acids and Bases
Example compare the relationship between Arrhenius definitions and Bronsted-lowry definitions of acids and bases.
NH3(aq) + H2O(l) <-----> NH4+(aq) + OH-(aq)
| NH3 is an arrhenius base as adding it to water leads to an increase in the concentration of OH- it is Bronsted-Lowry base because it accepts a proton from water. |
H2O acts as Bronsted-lowry acid because it donates a proton to the NH3 molecule. |
an acid and a base work together to transfer a proton to be a Bronsted-Lowry acid, a molecule or ion must have a hydrogen atom that it can lose as an H+ion.
to be a Bronsted-Lowry base, a molecule or ion must have a nonbonding pair of e's that it can use to bind the H+ ion.
Amphoteric substance, is a substance that acts as a base when combined with something more strongly acidic than itself, and as an acid when combined with something more strongly basic than itself.