Weak base titration: You are titrating a solution of 0.100 M trimethylamine (pK=4.20) with 0.125 M HCl.Calculate the pH and plot along the titration curve after the addition of the volumes shown below. Make a plot ofthe titration curve.a. 0 mL titrantb. 10.0 mLc.15.0 mLd.20.0 mLe.25.0 mLf. 30.0 mL

I have calculated the pH and plotted the weak base titration curve, and their detailed step-wise…

Answered: Weak base titration: You are titrating…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the titration of 80.0 mL of 0.100 M Ba (OH), by 0.400 M HCI. Calculate the pH of the resulting solution after the following volumes of HCI have been added. a. 0.0 mL pH = b. 20.0 mL pH = c. 30.0 mL pH= d. 40.0 mL PH= e. 90.0 mL pH = Submit Answer Try Another Version 1 item attempt remaining
A. What is the pH of a buffer solution that is composed of 50.0 mL of a 0.25M weak base, Phyllis amine (Ph-NH2) combined with 75.0 mL of 0.23 its salt Phyllis chloride (PHCI)? pKb = 4.65 %3D B. Calculate the new pH of this buffer when 0.301 grams of solid sodium hydroxide is added to the solution. Assume there is no change in volume (MM sodium hydroxide 40.00 g/mol) Show all work on a separate sheet and upload your work. Write your answers in the spaces below: A. The pH of this buffer %3D B. The new pH %3D
= 0.01 x 0.100 = 0.001 001 50.0 X0-250 = 0.0125 0.0123 025 0.06 0.300 x0.01 0.100. X 0.01 B. 9.25 0.06 6A 10.0 mL solution of 0.300 M NH3 is titrated with 0.100 M HCI. Calculate the pH after the addition of 10.0 mL of acid. A. 9.55 0.001 -0.003 0.300 x 0.0 0.001 C. 8.95 0.02 PH = PKG +10g [0.0156 2.67=4.744+ [19165 TI-84 Plus TEXAS INSTRUMENTS D. 9.73 = Pl= 3.68 - 267 28.3. 0:3 0002 0.002 M Plt = -log = .05 U.2 E. 8.77 Pit=Pkg tog 20.015 = 1.01 [A] [HA]
based on the titration curves, compare the three curves and make conclusions based on their shapes.
The molar solubility of PbI2 is 1.46 x 10^-3 M. Calculate the value of Ksp for PbI2. A. 3.11 x 10^-9 B. 4.26 x 10^-6 C. 1.24 x 10^-8 D. 1.46 x 10^-3 E. none of these
25.00 mL sample of 0.08000 M HNO2 (Ka = 4.0 × 10-4) is being titrated with 0.1000 M NaOH. a. Calculate the initial pH of the acid. b. Calculate the pH at 5.00 mL before the equivalence point. c. Calculate the pH at the equivalence point. d. Calculate the pH at 5.00 mL after the equivalence point.
9. Calculate the pH of the solution that results from each mixture. a. 50.0 mL of 0.15 M HCHO₂ with 75.0 mL of 0.13 M NACHO₂ b. What mass of sodium benzoate should you add to 150.0 mL of a 0.15 M benzoic acid solution to obtain a buffer with a pH of 4.25? (Assume no volume change)
Answer using this data for the remaining questions on this page: For 1.0L of an acetic acid solution: Ka = 1.8 x 10-5 and [HA] = 0.250M 2. Calculate the pH of the solution. 3. What is the pka? 4. Calculate the pH of the solution if you make it a buffer by adding enough solid sodium acetate to make the concentration of acetate ion equal to 0.35M. The volume of the solution does not change. 5. What is the new concentration of [HA] if 2.0mL of 5.00M of HCI is added to 1.000L of the solution above? 6. What is the new pH?
The titration on the right was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl. How many buffer regions are present in this titration? 1 3 4 2 The number of buffer regions cannot be determined from the titration curve.

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