Amonoprotic weak acid, ha, dissociates in water according to the reaction: ha(aq) = h+(aq) + a−(aq). the equilibrium concentrations of the reactants and products are [ha]=0.160 m , [h+]=3.00×10^−4 m , and [a−]=3.00 ×10^−4 m. calculate the value for the acid ha .

Answer : The value of for the acid HA is,

Solution :

The equilibrium reaction for dissociation of weak acid will be,

The expression for dissociation constant will be,

Now put all the given values in this expression, we get:

Therefore, the value of for the acid HA is,

i'm pretty sure its b i might be wrong though!

explanation:

a