The equilibrium concentrations of the reactants and products are [ha] = 0.220 m [h3o ] = 2.00 × 10–4 m [a–] = 2.00 × 10–4 m calculate the ka value for the acid ha.

The equilibrium equation showing the dissociation of weak acid is:

is the equilibrium constant for this equation, which is referred to as the acid dissociation constant. value will determine the acidic strength of the acids. Greater the value, more will be the acidity.

Calculating the value from given equilibrium concentrations:

=

=

hi my dude or dudette