Question

Which of the following is true of a buffered solution? Group of answer choices All of these are true The solution resists any change in its [H+]. The pH of the solution will not change much even if a concentrated acid is added. Any H+ ions added will react with a conjugate base of a weak acid already in thye solution. The pH of the solution will not change much even if a strong base is added.

Answer 1

Answer:

All of these are true

Explanation:

A buffer solution in chemistry is a solution that resists changes in pH when an acid or base is added to it. It is a solution that contains a weak acid and its conjugate base (anion) or a weak base and its conjugate acid.

A buffer is able to resist a change in pH due to the conjugate base and conjugate acid of the weak acids and bases contained in them respectively. The conjugate base/acid are present in an equilibrium quantity with their acid/base counterparts and help to neutralize or react with any additional H+ or OH- from an acid or base added to their solution.

However, when a strong acid or base is added to the buffer solution, there is only a slight change which practically does not change the pH of the solution.

Hence, all of the above options about a buffered solution is true.

Answer 2

On seeing the given options, it is clear that all the options are correct.

What is a buffer?

A solution, which resists the change in pH upon the supplementation of an acidic or basic components is known as a buffer.

The following are the characteristics of buffer:

• It exhibits a definite pH and it sustains it, that is, it prevents the change in pH or hydrogen ion change.

• A very slight modification in pH takes place at the time of the addition of small concentration of concentrated base or acid.

• When a small concentration of strong acid is added to the buffer solution, then the concentration of hydrogen ions enhances in the solution and will react with the conjugate base of the weak acid to maintain the concentration of hydrogen ion in the weak acid-salt buffer solution.

• When a small concentration of strong base is supplemented to a weak acid-salt buffer then hydrogen ions reacts with the hydroxide ions to produce neutral water and to sustain the equilibrium as per the principle of Le-Cha-telier, the dissociation of weak acid takes place in order to sustain the concentration of hydrogen ions in the buffer solution and thus pH is maintained.

Thus, all the given statements are true.

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