The titration of 50.00 mL of 0.150-M HCl with 0.150-M NaOH (the titrant) is carried out in a chemistry labora- tory. Calculate the pH of the solution after these volumes of the titrant have been added: (a) 0.00 mL (d) 50.00 mL Use the results of your calculations to plot a titration curve for this titration. On the curve indicate the position of the equivalence point. (b) 25.00 mL (e) 50.1 mL (c) 49.9 mL (f) 75.00 mL

A 100.0 mL sample of 0.180 M HClO4 is titrated with 0.270 M LiOH.  Determine the pH of the solution at the following points  Initial After 10.00 mL of LiOH is added After 65.00 mL of LiOH is added At equivalent After 70 mL of LiOH is added Sketch a titration curve

Determine the pH during the titration of 69.1 mL of 0.366 M benzoic acid (Ka = 6.3×10-5) by 0.366 M NaOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any NaOH (b) After the addition of 16.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint)  (d) At the equivalence point  (e) After the addition of 104 mL of NaOH

In a titration experiment, 40.0 mL of 0.100 M HCI is titrated with 0.100 M NaOH solution. Determine the pH of the solution: (a) before NaOH is added. (b) after 20.0 mL of NaOH is added.