(D) Solutions which resist the change in the value of $pH$ when a small amount of acid or base is added to them are known as buffer solutions. Since $

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(D) Solutions which resist the change in the value of $pH$ when a small amount of acid or base is added to them are known as buffer solutions. Since $pH = -\log[H_3O^+]$,a constant $pH$ implies that the concentration of $H_3O^+$ remains effectively constant.

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium Buffer solution

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In some solutions,the concentration of $H_3O^{+}$ remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as

JEE MAIN 2014 All JEE MAIN

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Ideal solutions
B
Colloidal solutions
C
True solutions
D
Buffer solutions

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2 Equilibrium: Ionic Equilibrium

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Buffer solution

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For a weak acid $(HA)$,$pK_a = 4.5$. The $pOH$ of a buffer solution of $HA$ in which $50\%$ of the acid is ionized is:

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In a buffer solution containing equal concentration of $B^{-}$ and $HB,$ the $K_b$ for $B^{-}$ is $10^{-10}.$ The $pH$ of the buffer solution is:

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The $pH$ of a buffer solution formed by mixing $30 \text{ mL}$ of $0.1 \text{ M } NH_4OH$ and $30 \text{ mL}$ of $1 \text{ M } NH_4Cl$ solutions is $8.6$. The $pK_b$ of $NH_4OH$ is

MediumAP EAMCET 2018

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Calculate the $pH$ of a $0.10 \,M$ ammonia solution. Calculate the $pH$ after $50.0 \,mL$ of this solution is treated with $25.0 \,mL$ of $0.10 \,M$ $HCl$. The dissociation constant of ammonia,$K_{b} = 1.77 \times 10^{-5}$.

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Which mixture forms a buffer when dissolved in $1 \, L$ of water?

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In some solutions,the concentration of $H_3O^{+}$ remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as

Similar Questions

For a weak acid $(HA)$,$pK_a = 4.5$. The $pOH$ of a buffer solution of $HA$ in which $50\%$ of the acid is ionized is:

In a buffer solution containing equal concentration of $B^{-}$ and $HB,$ the $K_b$ for $B^{-}$ is $10^{-10}.$ The $pH$ of the buffer solution is:

The $pH$ of a buffer solution formed by mixing $30 \text{ mL}$ of $0.1 \text{ M } NH_4OH$ and $30 \text{ mL}$ of $1 \text{ M } NH_4Cl$ solutions is $8.6$. The $pK_b$ of $NH_4OH$ is

Calculate the $pH$ of a $0.10 \,M$ ammonia solution. Calculate the $pH$ after $50.0 \,mL$ of this solution is treated with $25.0 \,mL$ of $0.10 \,M$ $HCl$. The dissociation constant of ammonia,$K_{b} = 1.77 \times 10^{-5}$.

Which mixture forms a buffer when dissolved in $1 \, L$ of water?

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