Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N, with 0.1000 M HCl solution after the following additions of titrant. 10.00 mL: 21.00 mL: 28.00 mL:

For the titration of 50.0 mL of 0.100-M HCl with 0.100-M NaOH, calculate the pH when these volumes of NaOH have been added: (a) 10.0 mL (b) 25.00 mL (c) 45.0 mL (d) 50.5 mL

Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 106) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 have been added. a. 0.0 mL b. 20.0 mL c. 25.0 mL d. 40.0 mL e. 50.0 mL f. 100.0 mL

Calculate the pH at the following points in a titration of 40 mL (0.040 L) of 0.100 M barbituric acid (Ka=9.8105) with 0.100 M KOH. (a) no KOH added. (b) 20 mL of KOH solution added. (c) 39 mL of KOH solution added. (d) 40 mL of KOH solution added. (e) 41 mL of KOH solution added

For the titration of 50.0 mL of 0.150 M ethylamine. C2H5NH2, with 0.100 M HCl, find the pH at each of the following points, and then use that information to sketch the titration curve and decide on an appropriate indicator. (a) At the beginning, before HCl is added (b) At the halfway point in the titration (c) When 75% of the required acid has been added (d) At the equivalence point (e) When 10.0 mL more HCl has been added than is required (f) Sketch the titration curve. (g) Suggest an appropriate indicator for this titration.

In the titration of 50.0 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 104), with 0.50 M HC1, calculate the pH under the following conditions. a. after 50.0 mL of 0.50 M HCl has been added b. at the stoichiometric point