Question

explain mechanism of basic buffer solution​

Answer 1

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A buffer solution resists large changes of pH upon addition of small amount of acid or base.

Acidic Buffer Solution

It is a solution containing a weak acid and soluble ionic salt of weak acid with a strong base.

For example a solution containing CH3COOH and its salt CH3COONa. In this buffer, the more acidic component (reserve acidity) is CH3COOH and the more basic component (reserve alkalinity) is CH3COO- ions supplied by the salt. The dissociation occurs as follows:

CH3COOH (aq) ←→ CH3COO- (aq) + H+(aq)……partial

CH3COONa (aq) → CH3COO- (aq) + Na+ (aq)……complete

Suppose a small amount of strong acid is added to the buffer solution. The H+ ions of the acid react with the basic component, CH3COO- in the buffer.

CH3COO- (aq) + H+ (aq) → Ch3COOH (aq)

Most of the added H+ ions are consumed because concentration of CH3COO- in the buffer is high. The reaction nearly goes to completion because Ch3COOH is a weak acid and its ions have a strong tendency to form non-ionized CH3COOH molecules. Due to removal of most of the added H+, there is no appreciable decrease in pH

2. If a small quantity of base is added, the OH- ions are consumed by the acidic component CH3COOH

CH3COOH (aq) + OH-(aq) → CH3COO- (aq) + H2O (l)

The effect is the neutralization of most of the added OH- ions by CH3COOH. Therefore, there is no appreciable change in pH

Basic Buffer Solution

An example is the NH4OH/NH4Cl buffer. The acidic component is NH4+ ions and the basic component is NH4OH or OH- ions.

The mechanism is same as that of acidic buffers.

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