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A weak acid is an Acid that does not fully Ionize in Solution ; that is, if the acid was represented by the general formula ''HA'', then in aqueous solution a significant amount of undissolved HA still remains.

\mathrm{ HA_{(aq)} \, \leftrightarrow \, H^+\,_{(aq)} +\, A^-\,_{(aq)} }

The equilibrium concentrations of reactants and products are related by the Acidity Constant expression, (Ka):

\mathrm{ K_a\, =\, rac { {Link without Title} {Link without Title} }{ {Link without Title} } }

The greater the value of Ka, the more the formation of H+ is favored, and the lower the PH of the solution. The Ka of weak acids varies between 1.8×10-16 and 55.5. Acids with a Ka less than 1.8×10-16 are weaker acids than water. Acids with a Ka of greater than 55.5 are strong acids and almost totally dissociate when dissolved in water.

The vast majority of acids are weak acids.


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