8. In Activity 2, there were 2 ml of buffer per well. Calculate the final pH of the undiluted buffer after 0.25 mL of 0.1 M NaOH is added. The Ka of CH3COOH = 1.8 x 10-5. Use the CH3COOH buffer concentration calculated in Data Table 2, a balanced CH3COOH + NaOH reaction equation, an ICE table, and a balanced dissociation equilibrium equation to help determine the pH. 9. Calculate the final pH of the second dilution after adding 1 drop of 0.1 M NaOH. Assume that one drop has a volume of 0.05 ml.

8. In Activity 2, there were 2 ml of buffer per well. Calculate the final pH of the undiluted buffer after 0.25 mL of 0.1 M NaOH is added. The Ka of CH3COOH = 1.8 x 10-5. Use the CH3COOH buffer concentration calculated in Data Table 2, a balanced CH3COOH + NaOH reaction equation, an ICE table, and a balanced dissociation equilibrium equation to help determine the pH. 9. Calculate the final pH of the second dilution after adding 1 drop of 0.1 M NaOH. Assume that one drop has a volume of 0.05 ml.

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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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Initial PH 4.7

8. In Activity 2, there were 2 mL of buffer per well. Calculate the final pH of the
undiluted buffer after 0.25 mL of 0.1 M NaOH is added. The Ka of CH3COOH =
1.8 x 10-5. Use the CH3COOH buffer concentration calculated in Data Table
2, a balanced CH3COOH + NaOH reaction equation, an ICE table, and a
balanced dissociation equilibrium equation to help determine the RH.
9. Calculate the final pH of the second dilution after adding 1 drop of 0.1 M
NAOH. Assume that one drop has a volume of 0.05 ml.

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