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Buffer
Solution that has a base and an acid existing at the same time
buffers can only be made with
a weak acid
a buffer resists
changes in ph when limited amounts of acid or base are added to it
henderson hasselbach equation is used
only to calculate ph in buffers
henderson hasselbach equation
pH = pka + log (A)/(HA)
strong acid strong base ph end point
14
weak acid strong base ph end point
ph >7
weak base strong acid ph
ph < 7
ksp
equilibrium constant for the solubility of a slightly soluble salt
molar solubility
moles per liter of the salt dissolved in water
ion product
the product of ion concentrations in asolution, each concentration raised to a power equal to the number of ions in the formula of the ionic compound
Qc < ksp
no precipitate forms, unsaturated solution
Qc > ksp
precipitate will occur, saturated solution
Qc = Ksp
saturated solution, no precipitate formed
salts are more soluble
at a low ph
solubility is affected by
the ph of the solution
complex ion
formed from a metal ion with lewis bases attached to it by coordinate covalent bonds
complex
compound containing complex ions
ligand
lewis base that bonds to a metal ion to form complex ions
formation constant (Kf)
equilibrium constant for the formation of a complex ion
dissociation constant (kd)
1/kF