He M R y CHECK-IN ACTIVITY: Titration Curve 1] A 50.00 mL aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCI. Calculate the pH of the solution after the addition of: a) 0.00 mL HCI b) 10.00 mL HCI c) 25.00 mL HCI d) 40.00 mL HCI e) 45.00 mL HCI f) 49.00 mL HCI g) 50.00 mL HCI h) 51.00 mL HCI i) 55.00 mL HCI j) 60.00 mL HCI

He M R y CHECK-IN ACTIVITY: Titration Curve 1] A 50.00 mL aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCI. Calculate the pH of the solution after the addition of: a) 0.00 mL HCI b) 10.00 mL HCI c) 25.00 mL HCI d) 40.00 mL HCI e) 45.00 mL HCI f) 49.00 mL HCI g) 50.00 mL HCI h) 51.00 mL HCI i) 55.00 mL HCI j) 60.00 mL HCI

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 7P

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When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
Consider die titration of 50.0 mL of 0.10 M H3A (Ka1 = 5.0 104, Ka2 = 1.0 108, Ka3 = 1.0 1012) titrated by 0.10 M KOH. a. Calculate the pH of the resulting solution at 125 mL of KOH added. b. At what volume of KOH added does pH = 3.30? c. At 75.0 mL of KOH added, is the solution acidic or basic?
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105) with 0.100 M HCl.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)