Balanced equation
H₂AsO₄⁻ ⇆ H⁺ + HAsO₄²⁻
Ka = [tex]\frac{(H^+).(HAsO_4^{2-})}{(H_2AsO_4^{-})}[/tex]
The acid dissociation constant determines the difference between strong and weak acids (Ka). The acid dissociates more as Ka increases. Strong acids must therefore dissociate more in water. A weak acid, on the other hand, is less likely to ionise and release a hydrogen ion, which results in a less acidic solution.
The acid dissociation constant, or Ka, is the equilibrium constant of an acid's dissociation reaction. This equilibrium constant serves as a numerical representation of the acidity of a solution. Ka is typically stated in units of mol/L.
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