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

Question

Which of the following is (are) correct for buffer solution? (A) Acidic buffer will be effective within in the pH range ( p Ka ± 1) (B) Basic buffer will be effective within the pH range ( p Kw- p Kb ± 1) (C) H 3 PO 4+ NaH 2 PO 4 is not a buffer solution (D) Buffers behave most effectively when the [Salt]/[Acid] ratio equal to 1

Tardigrade Admin · Accepted Answer

For acidic buffer, buffer capacity is maximum at

p H = p K_{a}

and for basic buffer, it is maximum at

p H = p K_{w} - p K_{b}

. Buffer is always effective within a

p H

range of

1

with respect to the

p H

at maximum buffer capacity

H_{3} P O_{4} + H_{2} P O_{4}^{⊖}

is a buffer solution

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

Acidic buffer will be effective within in the $p H$ range $(p K_{a} \pm 1)$

Basic buffer will be effective within the $p H$ range $(p K_{w} - p K_{b} \pm 1)$

$H_{3} P O_{4} + N a H_{2} P O_{4}$ is not a buffer solution

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

For acidic buffer, buffer capacity is maximum at
$p H = p K_{a}$ and for basic buffer, it is maximum at
$p H = p K_{w} - p K_{b}$ . Buffer is always effective within a $p H$ range of $1$ with respect to the $p H$ at maximum buffer capacity
$H_{3} P O_{4} + H_{2} P O_{4}^{⊖}$ is a buffer solution

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

Acidic buffer will be effective within in the pH range (pKa​±1)

Basic buffer will be effective within the pH range (pKw​−pKb​±1)

H3​PO4​+NaH2​PO4​ is not a buffer solution

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

For acidic buffer, buffer capacity is maximum at pH=pKa​ and for basic buffer, it is maximum at pH=pKw​−pKb​. Buffer is always effective within a pH range of 1 with respect to the pH at maximum buffer capacity H3​PO4​+H2​PO4⊖​ is a buffer solution

Acidic buffer will be effective within in the $p H$ range $(p K_{a} \pm 1)$

Basic buffer will be effective within the $p H$ range $(p K_{w} - p K_{b} \pm 1)$

$H_{3} P O_{4} + N a H_{2} P O_{4}$ is not a buffer solution

For acidic buffer, buffer capacity is maximum at
$p H = p K_{a}$ and for basic buffer, it is maximum at
$p H = p K_{w} - p K_{b}$ . Buffer is always effective within a $p H$ range of $1$ with respect to the $p H$ at maximum buffer capacity
$H_{3} P O_{4} + H_{2} P O_{4}^{⊖}$ is a buffer solution