If the Ka of a monoprotic weak acid is 3.3106, what is the pH of a 0.41M solution of this acid? A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq)+H2O(l)H3O+(aq)+A(aq) The equilibrium concentrations of the reactants and products are [HA]=0.160M,[H3O+]=2.00104M, and [A]=2.00104M. Calculate the Ka value for the acid HA Ka= If the Kb of a weak base is 3.9106, what is the pH of a 0.23M solution of this base