(C) The $pH$ of human blood is maintained naturally at $7.36-7.42$ by the $(HCO_3^{-} + H_2CO_3)$ buffer system. This buffer system consists of carbon

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Carbonic acid and salt of carbonic acid

(C) The $pH$ of human blood is maintained naturally at $7.36-7.42$ by the $(HCO_3^{-} + H_2CO_3)$ buffer system. This buffer system consists of carbonic acid $(H_2CO_3)$ and its conjugate base,the bicarbonate ion $(HCO_3^{-})$.

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

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Which of the following buffers is used to maintain the $pH$ of human blood naturally?

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A
Hydrogen cyanide and sodium cyanide
B
Copper hydroxide and copper chloride
C
Carbonic acid and salt of carbonic acid
D
Ammonium hydroxide and ammonium chloride

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6-2.Equilibrium-II (Ionic Equilibrium)

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Buffer solution

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For preparing a buffer solution of $pH = 5$ by mixing sodium acetate and acetic acid,the ratio of the concentration of salt and acid should be $(K_a = 10^{-5})$:-

Medium

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$A$ buffer solution of $100 \ mL$ has a $pH$ value of $4$. When $1 \ mL$ of dilute $HCl$ is added to it,what happens to the $pH$ of the buffer solution?

Easy

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When $NaOH$ is added to a $CH_3COOH$ solution,$60\%$ of the acid is neutralized. If the $pK_a$ is $4.7$,the $pH$ of the resulting solution is:

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Assertion : In a titration of weak acid and $NaOH$,the $pH$ at half equivalence point is $pK_a$.
Reason : At half equivalence point,it forms an acidic buffer and the buffer capacity is maximum where $[acid] = [salt]$.

MediumAIIMS 2009

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$pH$ of a mixture of $1 \ M \ HA$ $(pK_a = 4.2)$ and $1 \ M \ NaA$ is $4.5$. In $300 \ mL$ of buffer,the volume of $HA$ is $....... \ mL$ $[\log \ 2 = 0.3]$

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Which of the following buffers is used to maintain the $pH$ of human blood naturally?

Similar Questions

For preparing a buffer solution of $pH = 5$ by mixing sodium acetate and acetic acid,the ratio of the concentration of salt and acid should be $(K_a = 10^{-5})$:-

$A$ buffer solution of $100 \ mL$ has a $pH$ value of $4$. When $1 \ mL$ of dilute $HCl$ is added to it,what happens to the $pH$ of the buffer solution?

When $NaOH$ is added to a $CH_3COOH$ solution,$60\%$ of the acid is neutralized. If the $pK_a$ is $4.7$,the $pH$ of the resulting solution is:

Assertion : In a titration of weak acid and $NaOH$,the $pH$ at half equivalence point is $pK_a$.Reason : At half equivalence point,it forms an acidic buffer and the buffer capacity is maximum where $[acid] = [salt]$.

$pH$ of a mixture of $1 \ M \ HA$ $(pK_a = 4.2)$ and $1 \ M \ NaA$ is $4.5$. In $300 \ mL$ of buffer,the volume of $HA$ is $....... \ mL$ $[\log \ 2 = 0.3]$

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Assertion : In a titration of weak acid and $NaOH$,the $pH$ at half equivalence point is $pK_a$.
Reason : At half equivalence point,it forms an acidic buffer and the buffer capacity is maximum where $[acid] = [salt]$.