Intro to Acids and Bases

I would say the part I first struggled with in this unit is the difference between Arrhenius acids/bases versus Bronsted-Lowry acids/bases. Here's the difference!

Arrhenius acids: produces H+ ions in aqueous solutions   

Arrhenius bases: produces OH- ions in aqueous solutions 

Bronsted-Lowry acids: proton (H+) donor

Bronsted-Lowry  bases: proton (H+) acceptor

Key note: Bronsted-Lowry acids/bases are the ONLY ones with conjugate acid/base pairs 

Acids produces conjugate bases and bases produce conjugate acids. 

This basically means that when you have an acid that gives up a proton (H+) the conjugate base is just the remaining substance when a proton is lost from an acid. The conjugate acid of the base is the substance frmed when a proton is added to a base, 

Some important key notes:

-Water is amphoteric substance meaning it can act as an acid or a base. 

-Group 2 metals liberate twice as much OH- for bases 

-Strong acids/bases will have weak conjugate acids/bases

Helpful Links!

Acids and Bases Khan Academy 

Arrhenius acids and bases

Bronsted-Lowry acids and bases theory