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Amino Acids

If K a 1 and ...

Question

If $K_{a 1}$ and $K_{a 2}$ are the ionization constants of $H_{3} N^{+} C H I C O O H$ and $H_{3} N^{+} C H I C O O^{-},$ respectively, the pH of the solution at the isoelectric point is

A

p H = p K_{a 1} + p K_{a 2}

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B

p H = (p K_{a 1} + p K_{a 2})^{1 / 2}

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C

p H = (p K_{a 1} + p K_{a 2})^{1 / 2}

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D

p H = \frac{(p K_{a 1} + p K_{a 2})}{2}

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Solution

The correct option is D $p H = \frac{(p K_{a 1} + p K_{a 2})}{2}$
At isoelectronic point.
$p H = \frac{p K_{a 1} + p K_{a 2}}{2}$

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Similar questions

K_{a 1}

K_{a 2}

are the ionization constants of

H_{3} N^{+} C H I C O O H

H_{3} N^{+} C H I C O O^{-},

respectively, the pH of the solution at the isoelectric point is

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}

.

pH of some solution is given by

p H = \frac{p K_{a_{1}} + p K_{a_{2}}}{2}

. This formula is valid for the compound

N a H_{2} B O_{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)

?

⎛ ⎜ ⎜ ⎝ H O O C - C | H^{\oplus} N H_{3} - C H_{2} C O O H ⎞ ⎟ ⎟ ⎠

The structure of aspartic acid is given.The

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

p K_{a_{3}}

(A)

respectively are:

1.88, 3.65

9.60

p K_{a_{1}}

corresponds to the ionisation of the

C O O H

⎛ ⎜ ⎜ ⎜ ⎜ ⎝ R \oplus N H_{3} | C H - C O O H ⎞ ⎟ ⎟ ⎟ ⎟ ⎠

p K_{a_{2}}

corresponds to the ionisation of

(\oplus N H_{3})

(ammonium ion). What is the

p H

at isoelectric points

(p I)

?

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