Which of the following is(are) correct for buffer solution?

Acidic buffer will be effective within in the pH range

(p K_{a} \pm 1)

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Basic buffer will be effective within the pH range

(p K_{w} - p K_{b} \pm 1)

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H_{3} P O_{4} + N a H_{2} P O_{4}

is not a buffer solution

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Buffers behave most effectively when the [Salt]/[Acid] ratio equal to 1

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Solution

The correct options are
A Basic buffer will be effective within the pH range $(p K_{w} - p K_{b} \pm 1)$ .
B Buffers behave most effectively when the [Salt]/[Acid] ratio equal to 1
D Acidic buffer will be effective within in the pH range $(p K_{a} \pm 1)$
$p H = p K_{a} + l o g \frac{[s a l t]}{[a c i d]}$
So pH of acidic solution increases if more salt is added.

Buffers behave most effectively when the [Salt]/[Acid] ratio equal to 1 and will be effective within in the pH range $(p K_{a} \pm 1)$

For a basic buffer
$p O H = p K_{b} + l o g \frac{[s a l t]}{[b a s e]}$

and $p H = 14 - p O H$

So basic buffer will be effective within the pH range $(p K_{w} - p K_{b} \pm 1)$ .

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