Question

A 30.00 mL solution of 0.235 M CH2NH2 was titrated with 0.150 M H2SO4. a) Calculate the pH of the 30.00 mL solution of 0.235 M CH2NH2 b) Calculate the volume of 0.150 M H2SO4 required to neutralize the 30 mL solution of 0.235 M CH2NH2. c) Calculate the volume of 0.150 M H2SO4 required to neutralize half the mole of CH2NH2 present 30 Ml solution of 0.235 M CH2NH2 d) Calculte the pH of the solution in (c). e) Calculate the pH of the resulting solution after the addition of 100 mL of 0.150 M H2SO4 f) Sketch the pH titration curve by graphing volume of 0.150 M H2SO4 (x-axis) vs pH for: i) pH before the start of titration at V=0 of 0.150 M H2SO4, ii) pH at the halfway point (c), iii) pH at the equivalence point (complete neutralization), iv) pH at (e) the pH of the resulting solution after the addition of the 100 mL of 0.150 M H2SO4.

Answer 1