Suppose: B- is symbol for any (soluble) base.
Equilibrium of a base when diluted in water:
B- + H2O <==> HB + OH-
Equilibrium constant:
Keq = [HB] * [OH-] / [B-] * [H2O]
The base dissociation contant is defined by:
KB = [HB]*[OH-]/[B-]So, KB = Keq*[H2O] = Keq*55.6 mol/L
a base dissociation constant is the rate of the equilibrium that is reached when a weak base is added to water, producing it's conjugate acid and hydroxide ions.
The base that has the smallest base dissociation constant is ammonia. It is a weak base and would ionize the least.
It is a weak base
Ammonia is a weak base
Borax is a weak base.
No, NH3 is a weak base, as it tends to capture free protons.
weak
A weak base is a type of base. This type of base is considered weak because when it is put in an aqueous solution, it cannot ionize.
Weak base
Soap is a weak base.
Ferric hydroxide is insoluble in water so it is a weak base.
no
CoCO3 (Cobalt II carbonate) would be a weak base.
The strength of an acid is expressed by its Ka value (acid 'equilibrium' constant) or its derivative pKa value ( pKa=-log10[Ka] )The relation with the strength of the conjugate base, (Kb , pKb values) is as follows:Ka * Kb = 1.0*10-14 at 25oCpKa + pKb = 14.00 at 25oC