Yes, buffers nutralize acids in the medium.
Not necessarily, a buffer solution does maintain a specific pH, but some buffer solutions are acidic or basic.
Buffers
A buffer is supposed to keep the pH of a solution from fluctuating too much. It helps keep the pH more-or-less consistent. Whether it keeps the solution neutral, it doesn't have to be neutral. You can make a solution be whatever pH you want, but different solutions and pHs require different approaches.
Solutions that resist change in pH when added to a strong acid or base are known as buffer solutions.
Neutral solution: pH =7Acidic solution: pH7.
A buffer solution.
it is placed in a buffer solution of 7.0 then it is placed in a buffer having pH 4.0
Buffer Resist and Maintains the PH of the solution if there change in the environment of the solution.
A buffer is supposed to keep the pH of a solution from fluctuating too much. It helps keep the pH more-or-less consistent. Whether it keeps the solution neutral, it doesn't have to be neutral. You can make a solution be whatever pH you want, but different solutions and pHs require different approaches.
The water solution of sodium chloride is neutral.
It maintains the pH of many solutions like medicines.
The water solution of sodium chloride is neutral; any influence on pH.
Solutions that resist change in pH when added to a strong acid or base are known as buffer solutions.
When acid is added to a buffer solution at pH 7, the pH of the buffer solution will decrease. However, due to the presence of a conjugate base in the buffer solution, the buffer will resist the change in pH and try to maintain its original pH value. This is because the conjugate base will react with the acid and prevent a significant decrease in pH.
Neutral in what sense? Guessing pH a neutral solution has a pH of 7.
Pure water has a pH of 7, meaning its neutral. So it helps neutralize acids and bases.
Neutral solution: pH =7Acidic solution: pH7.
Anything with a pH of 7 is neutral
When a pH level is 7.0, it is defined as 'neutral' at 25°C because at this pH the concentration of H3O+ equals the concentration of OH− in pure water. - Wikipedia