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Chemistry - Bronsted - Lowry theory

Bronsted - Lowry theory

This is the 'proton transfer' view of acid-base reactions as represented
by the ionisation of hydrogen chloride in aqueous solution.

A proton (the H ion) has been transferred from the acid (HCl) to the base
(H2O).

The acid HCl(aq) is a proton (H) donor.

The base H2O(l) is a proton (H) acceptor.

An acid-base reaction involves two conjugate acid-base pairs.

When the acid HCl(aq) donates a proton it forms its conjugate base:
Cl(aq).

When the base H2O(l) accepts a proton it forms its conjugate acid:
H3O(aq).

The conjugate pairs H3O/H2O and HCl/Cl show that the acid and base differ
by H.

1. H2SO4(aq) + KOH(aq) - KHSO4(aq) + H2O(l)

2. KHSO4(aq) + KOH(aq) - K2SO4(aq) + H2O(l)

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