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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

A friend asks the following: “Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution?” How would you explain buffering to this friend?

Interpretation Introduction

Interpretation:

An explanation regarding the concept of the buffering of a solution on basis of the given buffer solution is to be stated.

Concept introduction:

A solution that resists a change in the pH on addition of an acid or an alkali is termed as a buffer solution.

To determine: An explanation regarding the concept of the buffering of a solution on basis of the given buffer solution.

Explanation

Explanation

  • The addition of a strong base to a buffer solution decreases the concentration of the weak acid present. Hence, the value of the pH does not change
  • Given

The buffer solution is made up of a weak acid HA and its salt NaA .

The pH of a solution is calculated by the Henderson-Hassel Balch equation,

pH=pKa+log[salt][acid]

The addition of a strong base to a buffer solution decreases the concentration of the weak acid and increases the concentration of the salt.

Therefore, the ratio [salt][acid] is not much affected. Hence, the value of the pH does not change

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