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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?

Interpretation Introduction

Interpretation:

The buffered solution is to be described. The three examples of the buffered solution are to be stated. The example which shows the components of the buffered solution consume added strong acids or bases is to be explained with equations. The reason corresponding to the fact that the buffering of the solution is important for the biological system is to be stated.

Concept Introduction:

Buffer solution resists the change in pH value when a small amount of base or an acid is added to it. There are two types of buffer solution, basic buffer and acidic buffer solution.

Explanation

Buffer solution has a constant value of pH. It is not affected by the addition of an alkali or an acid.

The examples of the buffer solution are,

  • The solution of acetic acid and sodium acetate makes acid buffer.
  • The solution of ammonium hydroxide and ammonium chloride makes basic buffer.
  • The solution of bicarbonate and carbonic acid makes acidic buffer.

Assume that the acid buffer solution of acetic acid and sodium acetate. The dissociation of sodium acetate is shown below.

CH3COONa(aq)Na+(aq)+CH3COO(aq)

The solution contains the sodium ions, acetate ions and some amount of undissociated acetic acid molecules.

Hydrochloric acid is a strong acid and it dissociates completely.

If some drops of hydrochloric acid is added to this solution. It provides hydrogen ions to the buffer solution

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