Answer:
Explanation is in the answer
Explanation:
The pH of the buffer solution does not change appreciably because the strong acid (free H⁺) reacts with conjugate base of buffer producing more weak acid. pH formula of buffers is (Henderson-Hasselbalch formula):
pH = pKa + log ( [A⁻] / [HA] )
The addition of strong acid decreases [A⁻] increasing [HA]. pH change just in the log of the ratio of [A⁻] with [HA], that is a real little effect over pH of the buffer solution.
The addition of small strong acid to buffer the result in negligible change to the buffer solution, as HA has been able to add A in the concentration lower as log A.
The pH of the buffer solution has been given by the amount of hydrogen ion dissociated in the solution. The higher the hydrogen ion, the higher will be the acidic nature of the solution and vice versa.
The addition of strong acid and conjugate base has been producing more weak acid to the solution.
The weak acid production, the solution will make negligible change to the buffer solution, as HA has been able to add A in the concentration of weak log A. It has been thus produced negligible change in the solution.
For more information about pH of the solution, refer to the link:
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