(C) buffer solution is defined as a solution that resists changes in $pH$ upon the addition of small amounts of acid or base. This property arises bec

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Reacts with the added acid or base

(C) buffer solution is defined as a solution that resists changes in $pH$ upon the addition of small amounts of acid or base. This property arises because a buffer contains components that can neutralize added $H_3O^{+}$ or $OH^{-}$ ions. Specifically,the weak acid component reacts with added base,and the conjugate base component reacts with added acid,thereby maintaining the $pH$ of the solution.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Buffer solution

Medium

The addition of small amounts of either acid or base to a buffer solution causes only small changes in $pH$ because the buffer solution

A
Does not contain either $H_3O^{+}$ or $OH^{-}$
B
Contains large amounts of both $H_3O^{+}$ and $OH^{-}$
C
Reacts with the added acid or base
D
Contains a strong acid and the salt of the same strong acid

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6-2.Equilibrium-II (Ionic Equilibrium)

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Buffer solution

The approximate $pH$ of a solution formed by mixing equal volumes of $0.1 \ M$ sodium propanoate and $0.1 \ M$ propanoic acid (if the dissociation constant of propanoic acid is $1.3 \times 10^{-5}$) will be:

Medium

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The $pH$ of a buffer solution decreases by $0.02$ units when $0.12 \ g$ of acetic acid is added to $250 \ mL$ of a buffer solution of acetic acid and potassium acetate at $27^{\circ} C$. The buffer capacity of the solution is

DifficultTS EAMCET 2009

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The $pH$ of blood does not appreciably change by a small addition of acid or a base because blood

MediumAIPMT 1995

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$20 \ mL$ solution contains $0.1 \ M \ NH_4Cl$ and $0.01 \ M \ NH_4OH$. By adding which one will its $pH$ not change?

Medium

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Assertion : Mixture of $CH_3COOH$ and $CH_3COONH_4$ is an example of acidic buffer.
Reason : Acidic buffer contains equimolar mixture of a weak acid and its salt with weak base.

MediumAIIMS 2007

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The addition of small amounts of either acid or base to a buffer solution causes only small changes in $pH$ because the buffer solution

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The approximate $pH$ of a solution formed by mixing equal volumes of $0.1 \ M$ sodium propanoate and $0.1 \ M$ propanoic acid (if the dissociation constant of propanoic acid is $1.3 \times 10^{-5}$) will be:

The $pH$ of a buffer solution decreases by $0.02$ units when $0.12 \ g$ of acetic acid is added to $250 \ mL$ of a buffer solution of acetic acid and potassium acetate at $27^{\circ} C$. The buffer capacity of the solution is

The $pH$ of blood does not appreciably change by a small addition of acid or a base because blood

$20 \ mL$ solution contains $0.1 \ M \ NH_4Cl$ and $0.01 \ M \ NH_4OH$. By adding which one will its $pH$ not change?

Assertion : Mixture of $CH_3COOH$ and $CH_3COONH_4$ is an example of acidic buffer.Reason : Acidic buffer contains equimolar mixture of a weak acid and its salt with weak base.

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Assertion : Mixture of $CH_3COOH$ and $CH_3COONH_4$ is an example of acidic buffer.
Reason : Acidic buffer contains equimolar mixture of a weak acid and its salt with weak base.