MUST KNOW: Henderson Hasselbalch
pH = pKa + log [base/acid] = pKa + log [A-/HA]
if pH < pKa, then the species is more prevalent in the protonated state as there will be a higher concentration of acid (HA) to fit the HH equation
if pH > pKa, then the species will be more prevalent in the deprotonated state as there will be a higher concentration of base (A-) to fit the HH equation
pKa = -log Ka
Ka = 10^-pKa
pH = -log [H+]
[H+] = 10^-pH
For acids/bases:
If it's a strong acid or base, pH = - log[HX]] or pOH = -log[MOH]
If it's weak, pH = 1/2pKa - 1/2log[HA] is the best shortcut to calculate the pH of weak species (Thanks TBR!!!)
For titrations:
pH = pKa at the halfway point for weak species titrated by strong species
and at the equivalence point (where moles acid = moles base) pH = (pKa + pH(of titrant))/ 2
for strong species titrated by strong species, the pH is ALWAYS 7 at the equivalence point.