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Oxyacids of Phosphorus

H3PO4 is a we...

Question

$H_{3} P O_{4}$ is a weak triprotic acid. The approximate $p H$ of $0.1 M N a_{2} H P O_{4} (a q .)$ is calculated by

A

\frac{1}{2} [p K_{a_{1}} + p K_{a_{2}}]

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B

\frac{1}{2} [p K_{a_{2}} + p K_{a_{3}}]

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C

\frac{1}{2} [p K_{a_{1}} + p K_{a_{3}}]

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D

p K_{a_{1}} + p K_{a_{2}}

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Solution

The correct option is C $\frac{1}{2} [p K_{a_{2}} + p K_{a_{3}}]$
The expression for the pH of $0.1 M N a_{2} H P O_{4} (a q .)$ solution is $\frac{1}{2} [p K_{a_{2}} + p K_{a_{3}}]$
Here, $p K_{a_{2}}$ and $p K_{a_{3}}$ refers to the dissociation of $N a H_{2} P O_{4}$ and $N a_{2} H P O_{4}$ respectively.

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Similar questions

Q. Which of the following relation is correct regarding

p H

of salt of amphiprotic ion,

H_{2} P O_{4}^{-}

K_{a_{1}}

is first acid dissociation constant of

H_{3} P O_{4}

K_{a_{2}}

is second acid dissociation constant of

H_{3} P O_{4}

.

Lysine has p K_{a_{1}} = 2.18, p K_{a_{2}} = 8.95, p K_{a_{3}} = 10.53

In which structure lysine will be present at

p H = 9.7

.

p K_{a_{1}}, p K_{a_{2}} a n d p K_{a_{3}}

H_{3} P O_{4}

are 2.2, 7.2 and 12.3 respectively. The

p H

0.1 M

N a_{2} H P O_{4}

solution will be:

Q. A one litre solution contains

0.04 M

N a_{2} H P O_{4}

0.02 M

N a H_{2} P O_{4}

. The correct statement(s) is/are:

H_{3} P O_{4} :

p K_{a_{1}} = 2.14; p K_{a_{2}} = 6.84; p K_{a_{3}} = 12.3

l o g 2 = 0.3

Q. The structure of a basic amino acid, lysine, is given. The

p K_{a_{1}}, p K_{a_{2}}

p K_{a_{3}}

(A)

2.18, 8.95

10.53

p H

at isoelectric points

(p I)

?

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