A buffer mixture of acetic acid and potassium acetate has ${\rm{pH}} = 5.24.$ The ratio of $\left[ {{\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }} \right]/\left[ {{\rm{C}}{{\rm{H}}_3}{\rm{COOH}}} \right]$ in this buffer is, $\left( {{\rm{p}}{K_a} = 4.74} \right):$

NEET UG CHEMISTRY MCQ: Equilibrium

1 Easy

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Application +4 | -1

A buffer mixture of acetic acid and potassium acetate has

\mathrm{pH} = 5.24.

The ratio of

\left[ {\mathrm{C}{\mathrm{H}_3}\mathrm{CO}{\mathrm{O}^ - }} \right]/\left[ {\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}} \right]

in this buffer is,

\left( {\mathrm{p}{K_a} = 4.74} \right):

View answer and explanation

Correct option: A

3:1

Option A (

3:1

) is correct because using the Henderson-Hasselbalch equation, the ratio of the conjugate base to the acid is calculated to be approximately 3:1.

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Mg{(HC{O_3})_2}

MgC{O_3}

Mg{(OH)_2}

MgC{O_3}

K_{\mathrm{P}}

\mathrm{CaCO}_3

4.5 \times 10^{-2}

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}),

K_{\mathrm{P}}

2.0 \mathrm{~atm}.

\mathrm{CaO}

\mathrm{CaCO}_3

+

\leftrightharpoons

\mathrm{PC}{\mathrm{l}_5}\leftrightharpoons\mathrm{PC}{\mathrm{l}_3} + \mathrm{C}{\mathrm{l}_2}

{K_{\mathrm{eq}}} = 0.41

\mathrm{p}{K_a}