In the laboratory, a general chemistry student measured the pH of a 0.546 M aqueous solution of caffeine, C3H10N,0, to be 12.160.Use the information she obtaimed to determine the K, for this baseK,(experiment) = In the laboratory, a general chemistry student measured the pH of a 0.455 M aqueous solution of codeine, C13H210,N to be 10.789.Use the mfommation she obtained to determine the K, for this base.K,(experiment) =

In the laboratory, a general chemistry student measured the pH of a 0.546 M aqueous solution of caffeine, C3H10N O2 to be 12.160. Use the information she obtained to determine the K, for this base. K,(experiment) %3D

In the laboratory, a general chemistry student measured the pH of a 0.546 M aqueous solution of caffeine, C3H10N O2 to be 12.160. Use the information she obtained to determine the K, for this base. K,(experiment) %3D

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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This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power = H+ Molarity X OH- Molarity), we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10 to the -4 power 1.0 X 10 to the 10 power. pH= -log…
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