Acids & Bases

Strong Acids

Hydroiodic acid	HI
Hydrobromic acid	HBr
Hydrochloric acid	HCl
Perchloric acid	HClO4
Sulfuric acid	H2SO4
Nitric acid	HNO3

Strong Bases

Group 1 hydroxides	NaOH, LiOH, KOH
Group 1 oxides	Li2O, etc.
Some group 2 hydroxides	Ba(OH)2, Sr(OH)2, Ca(OH)2
Metal amides	NaNH2, LiNH2, Mg(NH2)2, Ca(NH2)2, etc.

- The conjugate base of a strong acid has no basic properties in water.

- The conjugate base of a weak acid is a weak base.

- The conjugate acid of a strong base has no acidic properties in water. For example, the conjugate acid of LiOH is Li+, which does not act as an acid in water.

- The conjugate acid of a weak base is a weak acid (and the weaker the base, the stronger the conjugate acid). For ex, the conjugate acid of NH3 is NH4+, a weak acid.

Amphoteric: can act as either an ACID or BASE. The conjugate base of a weak polyprotic (more than one H) acid is always amphoteric, because it can either donate or accept another proton.

- ex: H₂CO₃ à HCO₃^- à CO₃^2-