Buffer - 0.50 M HC H,Os/0.50 M NaC;H5O2yellow.1. calculated pH =4.7M: color of solution after thymol blue is added2. Buffer + | drops of 3.0 M NAOH changes pH to 9.6Write a net ionic equation for the neutralization of NaOH by a component of the buffer.HCH, O OHル H6Ous18drops of 3.0 M HCI changes pH to <1.2.3. Buffer +Write a net ionic equation for the neutralization of HCI by a component of the buffer.Compare your results in 2. and 3. Are the base-neutralizing capacity and the acid-neutralizingcapacity of the buffer similar? Explain why or why not.

The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Answered: Compare your results in 2. and 3. Are…

Compare your results in 2. and 3. Are the base-neutralizing capacity and the acid-neutralizing capacity of the buffer similar? Explain why or why not.

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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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

Buffer - 0.50 M HC H,Os/0.50 M NaC;H5O2
yellow.
1. calculated pH =4.7M: color of solution after thymol blue is added
2. Buffer + | drops of 3.0 M NAOH changes pH to 9.6
Write a net ionic equation for the neutralization of NaOH by a component of the buffer.
HCH, O OHル H6Ous
18
drops of 3.0 M HCI changes pH to <1.2.
3. Buffer +
Write a net ionic equation for the neutralization of HCI by a component of the buffer.
Compare your results in 2. and 3. Are the base-neutralizing capacity and the acid-neutralizing
capacity of the buffer similar? Explain why or why not.

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1. According to Table 27.4, if you mix 45.0 mL of a 0.1 M NaH₂PO4 solution with 55.0 mL of a 0.1M Na2HPO4 solution, you will create a buffer with a pH of 6.9.¹ Using the Henderson-Hasselback equation, determine if this pH is based on the concentration ratio of the base/acid or the activity ratio of the base/acid. Show your work to prove your answer. Ionic Strength (μ) 0.001 0.005 0.01 0.05 0.1 0.2 Activity Coefficient for H₂PO4 Activity Coefficient for HPO4²- 0.964 0.867 0.928 0.740 0.902 0.660 0.820 0.445 0.775 0.335 0.750 0.290 2
F.7.
Bonus (2 points) Buffer solutions resist dramatic changes in pH due to the presence of a weak acid-conjugate base pair present in the solution. However, the combination of 20.0mL of 0.30M HC2H3O2 and 10.0mL of 0.30M NaOH also produces an excellent buffer solution. How? Provide a thorough explanation that explains the apparent discrepancy. (Using calculations and reactions to support your explanation is encouraged. Feel free to use another page if additional space in needed.) The Ka of HC2H3O2 is 1.8x 10-5.