Sketch a \(\mathrm{pH}\) curve for the titration of a weak acid (HA) with a strong base \((\mathrm{NaOH})\). List the major species and explain how you would go about calculating the \(\mathrm{pH}\) of the solution at various points, including the halfway point and the equivalence point.

To sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH), identify the major species at various points during the titration process and determine the pH using the Ka and Kw expressions. The major species at significant points are: HA (initial point), HA, A-, OH- (before equivalence point), HA, A- (halfway point), A-, H2O (equivalence point), and A-, OH- (after equivalence point). Use stoichiometry and Ka/Kb expressions to calculate the pH at each point: for the initial point and before equivalence point, use Ka; for the halfway point, -log(Ka); for the equivalence point, use Kb; and for after equivalence point, use the concentration of excess OH- ions. Lastly, plot the pH values on the y-axis and the volume of NaOH added on the x-axis to create the pH curve, showing the gradual increase in the buffering region and the steep rise around the equivalence point.