Acids And Bases
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State the Bronsted-Lowry theory.
An acid is a proton donor and a base is a proton acceptor.
Define conjugate base.
The particle left when the acid has donated its proton.
Define conjugate acid.
The particle formed when a base has accepted a proton.
Define amphoteric.
A substance that acts as either a base or an acid.
Define amphiprotic.
A substance that can both donate or accept protons.
State the Lewis theory.
An acid is an electron pair acceptor and a base is an electron pair donor.
Define acid/base strength.
The tendency of an acid/base to dissociate into ions. The stronger the acid/base, the weaker its conjugate base/acid.
How do Ka and pKa relate to acid/base strength ?
The larger the Ka and the smaller the pKa, the stronger the acid/base and vice versa.
Define polybasic acids.
Acids that have more than 1 dissociable proton.