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Being simultaneously basic and acidic, water undergoes autoprotolysis, also called self-ionization:
The equilibrium constant is
H3O+ in these equations is general simply written H+. In pure water and in solutions that do not give any additional source of H+ or OH- both ions have molar concentrations exact to 10-7. Addition of an acid decreases [OH-] and hence increases [H3O+]; addition of a base has the reverse effect.
The pH scale is defined by
Neutral water has a pH of 7, acidic solutions have lower values of ph (typically 0-7), and basic solutions or alkaline higher values (7-14). In alkaline or basic solutions [OH-] is thus greater than [H+].
Strong and weak behavior
The equilibrium constant of the protolysis reaction
is known as the acid dissociation constant (Ka) of HA or the acidity constant:
It is often expressed as a pKa value, described as
principles and general steps taken
color formation of d-block elements
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The ph of an aqueous solution of Ba(OH)2 is 10 if the ksp of Ba(OH)2 is 1*10^-9 then the concentration of Ba+2 ions in the aqueous solution is Ans) [OH(-)] = 10^(-4) 2.
procedure and curves for radiometric titration
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