Using 0.100 mol L–1 NaOH, a student titrated 25.0 mL of a 0.100 mol L–1 weak
monoprotic acid, and separately titrated 25.0 mL of a 0.100 mol L–1 strong
monoprotic acid.
Which statement about the volume of base required to reach the equivalence point is correct?
(A) The weak acid will require the same volume of base as the strong acid.
(B) The weak acid will require a larger volume of base than the strong acid.
(C) The weak acid will require a smaller volume of base than the strong acid.
(D) The volume of base required will depend on the molar mass of the acid used.
Which statement correctly describes the pH at each titration equivalence point?
(A) The pH of both solutions will be the same.
(B) One of the solutions will be neutral while the other will have a pH higher than 7.
(C) One of the solutions will be neutral while the other will have a pH lower than 7.
(D) One of the solutions will have a pH higher than 7 while the other will have a pH
lower than 7.
im so confused please help and explain