I have studied that acidic buffer is a type of buffer solution but the definition of buffer solution says that it's a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid whereas the definition of acidic buffer says it's mixture of a weak acid and its SALT with a strong base. I don't understand this one buffer solution is an acid base mixture but acidic buffer is an acid salt mixture
1 Answer
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pH buffers are solutions with low value $\left|\dfrac{\text{d}(\text{pH})}{\text{d}n_\text{base/acid}}\right|$, i.e. their pH does not change much by addition of an acid or base.
How it is achieved is secondary. It is managed by two ways:
- Having a conjugate pair (Broensted-Lawry) acid+base (or several ones). They are usually combination of
- A weak acid and its salt with a strong base, like acetic acid/sodium acetate
- A weak base and its salt with a strong acid, like ammonia/ammonium chloride
- As acids/bases are often are used respective salts of multiprotic acids like phosphoric acid or citric acid.
- Requirements for pH buffers with very low or high pH can be addressed solely by solution of strong acid or base, as high concentrations of $\ce{H+(aq)}$ or $\ce{OH-(aq)}$ have natively high buffering capacity.
Acidic/basic buffers may have several meanings:
- Having acidic/basic pH.
- Using a weak acid/weak base and their salts as conjugate bases/acids.
- Using strong acids/bases as the second buffer type.
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$\begingroup$ So here the salt serves the same purpose that conjugate base does? $\endgroup$– yyzrCommented Dec 14, 2023 at 14:53
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1$\begingroup$ @yyzr The salt IS the conjugate base. More exactly, the anion of the salt - $\ce{CH3COO^}$ - / Or in the other example $\ce{NH4+}$ as the conjugate acid. $\endgroup$– PoutnikCommented Dec 14, 2023 at 14:56