The addition of a strong acid to a weak base will affect the ionization of the weak base by shifting the equilibrium of the weak base's ionization reaction. A weak base, when dissolved in water, undergoes partial ionization to form its conjugate acid and hydroxide ions OH- . The equilibrium constant for this reaction is called the base ionization constant Kb . When a strong acid is added to the solution containing the weak base, the strong acid will donate protons H+ to the solution. These protons will react with the hydroxide ions OH- produced by the weak base, forming water H2O . This reaction can be represented as:H+ + OH- H2OAs the strong acid donates protons to the solution, the concentration of hydroxide ions decreases. This causes the ionization equilibrium of the weak base to shift to the right, in an attempt to re-establish the equilibrium. Consequently, more of the weak base will ionize to produce its conjugate acid and hydroxide ions. However, since the strong acid keeps reacting with the hydroxide ions, the overall ionization of the weak base will be suppressed. The pH of the solution will decrease due to the presence of the strong acid, and the weak base will be less ionized than it would be in the absence of the strong acid.In summary, the addition of a strong acid to a weak base will shift the ionization equilibrium of the weak base, causing it to ionize more. However, the overall ionization of the weak base will be suppressed due to the reaction between the strong acid's protons and the hydroxide ions produced by the weak base.