Answered: Describe the difference between a…

Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 7CR: 7. Describe a buffered solution. Give three examples of buffered solutions. For each of your...

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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.

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Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion

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A few small drops of water are left in a burette that is used to titrate a base into an acid solution to determine the concentration of the acid. Will this small amount of water have any effect on the determined value for the concentration of the acid? If so, how is it affected? a. Those extra few drops of acid will cause the calculation for the concentration of the base to be too low. This is because it will seem that it took more acid to neutralize the base than it really did and so it will appear that the base is of stronger concentration than it really was. b. Those extra few drops of acid will cause the calculation for the concentration of the base to be too low. This is because it will seem that it took less acid to neutralize the base than it really did and so it will appear that the base is of stronger concentration than it really was. c. Those extra few drops of acid will cause the calculation for the concentration of the base to be too high. This is because it will seem that…
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Consider the generic dissociation equation... HA + H2O →H3O* + A¯ ..where HA is a weak acid Based on what you know about buffers, explain in detail how this reaction acts as an acid buffer to keep the pH of the solution constant even when a strong acid is added to the solution. Your answer should refer to the reaction above to discuss buffers, how they work, why strong acids/bases cannot be used as buffers, and how Le Chatelier's principle impacts why buffers work.
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Which theory or concept can explain buffer solution precisely? Explain your answer.