Identify the solution type: strong acid, strong base, weak acid, weak base, buffer, or salt
Determine the relevant concentration or amount of H+ or OH-
For strong acids, assume complete dissociation and use [H+] directly
For strong bases, assume complete dissociation and use [OH-] directly
Calculate pH using pH = -log[H+]
Calculate pOH using pOH = -log[OH-]
Use pH + pOH = 14 at 25°C
Convert pOH to pH using pH = 14 – pOH
For weak acids, use the acid dissociation constant Ka and an ICE table
For weak bases, use the base dissociation constant Kb and an ICE table
Solve for equilibrium [H+] or [OH-] from the dissociation expression
Use the approximation x << initial concentration when valid
For buffers, use the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA])
For weak acid salts, calculate hydrolysis using Kb = Kw/Ka
For weak base salts, calculate hydrolysis using Ka = Kw/Kb
For polyprotic acids, calculate pH using the first dissociation step unless otherwise required
For mixtures, combine moles first, then determine the dominant acid-base species
For titrations, find the equivalence point and use the appropriate region formula
Convert moles to concentrations using total solution volume
Check units carefully before calculating
Use significant figures consistent with the given data
Verify the final pH is between 0 and 14 for typical aqueous solutions