When an acid is added to a buffer, does the acid in the buffer turn into base to neutralize the acid? Or is there some other that the buffers maintains constant pH?

Answer 1

The base that comprises the buffer solution is PROTONATED...

The buffer equation can be found using...

#pH=pK_a+log_10{([A^-])/([HA])}#...when a moderate quantity of #H_3O^+# is added, the #[A^-]# is REDUCED, given that it is protonated to give increased #[HA]#. But because the ratio is modified by the logarithmic term, the diminution in #pH# is modified...and likewise if base is added...
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Answer 2

When an acid is added to a buffer, the buffer's base component neutralizes the added acid, maintaining the buffer's pH level. Similarly, when a base is added to a buffer, the buffer's acid component neutralizes the added base, also maintaining the pH level. Buffers work by maintaining a balance between the concentrations of the conjugate acid-base pair within the solution, which allows them to resist changes in pH when acids or bases are added.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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