relationship of ph, poh and pkw
pH + pOH - pH2O = pKw (comes from water dissociation equilibrium);
Here, pH2O = 0 as [H2O] = 1 (since water molecule concentration is infinitely large compared to its dissociated ions)
pH + pOH = pKw
pH= negative logarith to the base 10 of the [H+] in the solution. pOH= negative logarithm to the base 10 of the [OH-] in the solution. A neutral solution is neither acidic nor basic. The values remains constant.
pH + pOH = pKw = 14.
This is the relation between pH and pOH
where pKw = negative logarithm to the base 10 of the degree of ionization of water.
pH= negative logarith to the base 10 of the [H+] in the solution.
pOH = negative logarithm to the base 10 of the [OH-] in the solution.
Value of pKw is 14 at 25 degrees Centigrade.
pH + pOH = 14.00 at 25 degree celsius.
pH+pOH=pKw
as
pH=−log[H3O+]
pOH=−log[OH−]
pKw=−logKw