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pinkyjoshi65
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Could someone give and example of a substance that is a Bronsted-Lowry base, but not an Arrhenius base..
astro_kat said:no think about Lewis acids/bases
A Bronsted-Lowry acid is a substance that is capable of donating a proton (H+) in a chemical reaction. This definition is more general than that of an Arrhenius acid, which only refers to substances that produce H+ ions in aqueous solutions. This means that while all Arrhenius acids are also Bronsted-Lowry acids, the reverse is not necessarily true.
One example of a substance that fits this description is ammonia (NH3). While it can act as a Bronsted-Lowry acid by donating a proton in a reaction, it does not produce H+ ions in aqueous solutions and therefore does not meet the criteria for an Arrhenius acid.
One major difference is that Bronsted-Lowry acids can donate protons in non-aqueous solutions, while Arrhenius acids are limited to aqueous solutions. Additionally, Bronsted-Lowry acids do not necessarily have to contain hydrogen, whereas Arrhenius acids must contain hydrogen and produce H+ ions in solution.
Yes, it is possible for a substance to fit both definitions. For example, hydrochloric acid (HCl) can act as a Bronsted-Lowry acid by donating a proton, and it also produces H+ ions in aqueous solutions, meeting the criteria for an Arrhenius acid.
Similar to acids, Bronsted-Lowry bases have a broader definition than Arrhenius bases. They are substances that can accept a proton in a chemical reaction, while Arrhenius bases only refer to substances that produce OH- ions in aqueous solutions. This means that all Arrhenius bases are also Bronsted-Lowry bases, but not all Bronsted-Lowry bases are Arrhenius bases.