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Byju's Answer

Standard XII

Chemistry

Salt of Weak Acid and Weak Base

In a solution...

Question

In a solution of $N a H C O_{3}$ , in amphiprotic anion can undergo ionization to form $H^{+}$ ion and hydrolysis to form $O H^{-}$ ion.
$H C O_{3}^{-} + H_{2} O i o n i z a t i o n ⇋ C O_{3}^{2 -} + H_{3} O^{+}$
$H C O_{3}^{-} + H_{2} O h y d r o l y s i s ⇋ H_{2} C O_{3}^{-} + O H^{-}$ to calculate pH, suitable approximation is :

[C O_{3}^{2 -}] = [H_{2} C O_{3}]

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Degree of ionization = degree of hydrolysis

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both (A) and (B)

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neither 'A' nore 'B'

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Solution

The correct option is D both (A) and (B)
When the following two assumptions are taken,

$[C O_{3}^{2 -}] = [H_{2} C O_{3}]$

$degree of ionization = degree of hydrolysis$

The pH of the solution can be calculated using the expression:

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

Option C is correct.

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Similar questions

Q. In a solution of

N a H C O_{3}

, the amphiprotic anion undergoes ionization to form

H^{+}

ion and hydrolysis to form

O H^{-} i o n

H C O_{3}^{-} + H_{2} O i o n i z a t i o n ⇋ C O_{3}^{2 -} + H_{2} O

H C O_{3}^{-} + H_{2} O i o n i z a t i o n ⇋ H_{2} C O_{3} + O H^{-}

To calculate pH of the above solutions, the suitable approximation is

Q. Choose the right sequential phenomena among the following during the delivery of

O_{2}

from blood tissue.
P : Absorption of

C O_{2}

by the blood.
Q : Reaction of absorbed

C O_{2}

with

H_{2} O

to form

H_{2} C O_{3}

within RBC and its conversion into

H^{+}

and

H C O_{3}^{-}

ions in the presence of carbonic anhydrase enzyme.
R : Reaction of absorbed

C O_{2}

with

H_{2} O

in plasma to form

H_{2} C O_{3}

and its conversion into

H^{+}

and

H C O_{3}^{-}

ions in the presence of carbonic anhydrase enzyme.
S : Combination of

H^{+}

with heme portion of

H b O_{2}

to release

O_{2}

.
T : Combination of

H C O_{3}^{-}

with heme portion

H b O_{2}

to form reduced hemoglobin and release of

O_{2}

Q. The Bronsted acids in the reversible reaction are:

H C O_{3}^{-} (a q .) + O H^{-} (a q .) \to C O_{3}^{2} (a q .) + H_{2} O

N H_{3}

cannot release

O H^{-}

ions. Can it be a base?

Q. What

%

of the carbon in the

H_{2} C O_{3} - H C O_{3}^{-}

buffer should be in the form of

H C O_{3}^{-}

so as to have a neutral solution?

(K_{a} = 4 \times 10^{- 7})

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In a solution of NaHCO3 , in amphiprotic anion can undergo ionization to form H+ ion and hydrolysis to form OH− ion.HCO−3+H2Oionization⇋CO2−3+H3O+HCO−3+H2Ohydrolysis⇋H2CO−3+OH− to calculate pH, suitable approximation is :

The correct option is D both (A) and (B)When the following two assumptions are taken,[CO2−3]=[H2CO3]degree of ionization = degree of hydrolysisThe pH of the solution can be calculated using the expression:pH=pKa1+pKa22Option C is correct.