Chem 24/10/25 Bronsted Lowry theory

Arrhenius theory

An acid dissociates in water to produce H+ ions

A base disassociates in water to produce OH- ions

Bronsted Lowry acids and bases (theory)

An acid is a proton donor

A base is a proton acceptor

This model allows the classification of both acids and bases

Proton donor

different acids can donate amounts of protons i.e. monoprotic = donate one proton e.g. HCL, HF

Polyprotic acids

Can donate more than one proton in steps e.g. HCL

Diprotic e.g. h2so4

Triprotic e.g. h3po4

Conjugate acid-base pairs

When an acid donates a proton, it forms its conjugate acid

when a base accepts a proton, it forms its conjugate acid

Amphiprotic 

Amphiprotic species are amphoteric (Meaning they can act as either an acid or a base) e.g. Water (Amphiprotic)

HCO3- is amphiprotic

H2PO4 and HPO4 2- are amphiprotic