2 A student determined the concentration of a weak acid, acetic acid, by a titrimetric method using a standard NaOH solution and a pH meter for end point detection. Table 1.0 below shows the data that was obtained by the student. Table 1.0: Potentiometric titration of acetic acid with 0.100 M standard NaOH solution Burette Reading Volume of NaOH added (mL) pH reading 11.54 0 3.14 12.25 0.71 3.70 13.40 1.86 4.16 16.59 5.05 4.77 17.50 5.96 4.93 19.35 7.81 5.24 20.41 8.87 5.49 21.00 9.46 5.68 21.60 10.06 5.96 21.83 10.29 6.14 22.01 10.47 6.34 22.12 10.58 6.48 22.20 10.66 6.68 22.30 10.76 6.97 22.38 10.84 7.73 22.41 10.87 9.21 22.49 10.95 10.04 22.55 11.01 10.57 22.61 11.07 10.83 23.00 11.46 11.35 23.31 11.77 11.62 23.71 12.17 11.76 24.30 12.76 11.89 25.20 13.66 12.03 Plot the 2nd derivative curve and also determine the end point а b. C.

2 A student determined the concentration of a weak acid, acetic acid, by a titrimetric method using a standard NaOH solution and a pH meter for end point detection. Table 1.0 below shows the data that was obtained by the student. Table 1.0: Potentiometric titration of acetic acid with 0.100 M standard NaOH solution Burette Reading Volume of NaOH added (mL) pH reading 11.54 0 3.14 12.25 0.71 3.70 13.40 1.86 4.16 16.59 5.05 4.77 17.50 5.96 4.93 19.35 7.81 5.24 20.41 8.87 5.49 21.00 9.46 5.68 21.60 10.06 5.96 21.83 10.29 6.14 22.01 10.47 6.34 22.12 10.58 6.48 22.20 10.66 6.68 22.30 10.76 6.97 22.38 10.84 7.73 22.41 10.87 9.21 22.49 10.95 10.04 22.55 11.01 10.57 22.61 11.07 10.83 23.00 11.46 11.35 23.31 11.77 11.62 23.71 12.17 11.76 24.30 12.76 11.89 25.20 13.66 12.03 Plot the 2nd derivative curve and also determine the end point а b. C.

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...

See similar textbooks

Similar questions

Did either buffer F or G reach buffer capacity? How do you know? Explain your reasoning.
4) calculate the pH of the buffer solution after the addition of 0.15 mL of sodium hydroxide based on the known value of Ka for acetic acid? 5) calculate the pH of water after the addition of 0.15 mL of 1 M NaOH? *buffer solution by mixing 20.00 mL of 0.100 M sodium hydroxide and 40.00 mL of 0.100 M acetic acid
Using the graph, identify the half way and equivalence point. Base: NaOH Acid: unknown 11
need both 2 parts soon in detail don't copy I. will downvote
BURETTE READING SAMPLE Pp Mo A 12.4 25.0 6.2 6.2 9.2 16.8 D. 0.0 5.3 Use the table below to identify the basic compound C: *Note that double indicator titration for each compound was done using a standard acid solution with 0.0 mL as initial reading. O NaHCO3 O NaOHANazCO3 O NaOHANaHCO3 O Nazco3
9) Calculate the volume of hydrochloric acid solution that has to be added to reach the equivalence point tibration to another b) The hydrochloric acid solution was added Sodum hydroxide solution (2 5,00md) with unknown Concentration. After addition of 9,18ml hydrochloric acid solution & PH 7.00 was obtamed. Calculate the Concentration of the sodium hydroxide solution.
See image below
For each scenario below, select the color of the solution using the indicator thymol blue during the titration. When you first add indicator to your Na2CO3 solution, the solution is basic (pH ~10), and the color is [Select] At the equivalence point for the titration, the moles of added HCI are equal to the moles of Na2CO3. One drop (or less!) past this is called the endpoint. The added HCI begins to titrate the thymol blue indicator itself. At the endpoint, the indicator color is [Select] When you weren't paying attention and added too much HCI (~12 mL extra), the color is [Select] When you really weren't paying attention and reached the second equivalence point of Na2CO3, the color is ✓ [Select] blue yellow red orange green Question 9
For titration 1,2 and 3 calculate: Moles of Hydrochloric Acid, Moles of hydroxide, Concentration of hydroxide, Concentration of calcium hydroxide
In lab, you measure out 13.20 mL of 1.18M phosphoric acid to titrate with KOH. What volume (in mL) of 0.848 M KOH is required to reach the first equivalence point? Give your answer to one decimal place. Your Answer: Answer
2 A student determined the concentration of a weak acid, acetic acid, by a titrimetric method using a standard NaOH solution and a pH meter for end point detection. Table 1.0 below shows the data that was obtained by the student. Table 1.0: Potentiometric titration of acetic acid with 0.100 M standard NaOH solution Burette Reading Volume of NaOH added (mL) pH reading 11.54 0 3.14 12.25 0.71 3.70 13.40 1.86 4.16 16.59 5.05 4.77 17.50 5.96 4.93 19.35 7.81 5.24 20.41 8.87 5.49 21.00 9.46 5.68 21.60 10.06 5.96 21.83 10.29 6.14 22.01 10.47 6.34 22.12 10.58 6.48 22.20 10.66 6.68 22.30 10.76 6.97 22.38 10.84 7.73 22.41 10.87 9.21 22.49 10.95 10.04 22.55 11.01 10.57 22.61 11.07 10.83 23.00 11.46 11.35 23.31 11.77 11.62 23.71 12.17 11.76 24.30 12.76 11.89 25.20 13.66 12.03 Plot a curve of pH versus the volume of NaOH and determine the end point a.
M of NaOH: 0.100 Volume of HCI 25mL = 0.025L Moles of HCI = 2.5 mol What is the Volume of NaOH equivalence point: What is Moles of NaOH equaivalence point: What is pH at equivalence point? What is calculated pH and experimental pH of NaOH at 0.00 mL , 12.50 mL, 25mL, and 30 mL. Also what is the Error percentage for each one?