The ${\rm{p}}{K_b}$ value of ${\rm{N}}{{\rm{H}}_3}$ is 5. Calculate the pH of the buffer solution, ${\rm{1}}\;L$ of which contains $0.01{\rm{ }}M\;{\rm{ }}$ ${\rm{N}}{{\rm{H}}_4}{\rm{Cl}}\,{\rm{ and}}\,0.10\,{\rm{M }}\,{\rm{N}}{{\rm{H}}_4}{\rm{OH}}$

NEET UG CHEMISTRY MCQ: Equilibrium

1 Medium

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Application +4 | -1

The

\mathrm{p}{K_b}

value of

\mathrm{N}{\mathrm{H}_3}

is 5. Calculate the pH of the buffer solution,

\mathrm{1}\;L

of which contains

0.01\mathrm{ }M\;\mathrm{ }

\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}\,\mathrm{ and}\,0.10\,\mathrm{M }\,\mathrm{N}{\mathrm{H}_4}\mathrm{OH}

View answer and explanation

Correct option: D

Option D (10) is correct because it is calculated using the Henderson-Hasselbalch equation for a basic buffer.

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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}