The ${\rm{p}}{K_a}$ of a weak acid, $HA$, is 4.80. The ${\rm{p}}{K_b}$ of a weak base, $B{\rm{OH}}$ is 4.78. The pH of an aqueous solution of the corresponding salt, $BA$, will be

NEET UG CHEMISTRY MCQ: Equilibrium

1 Hard

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Application +4 | -1

The

\mathrm{p}{K_a}

of a weak acid,

HA

, is 4.80. The

\mathrm{p}{K_b}

of a weak base,

B\mathrm{OH}

is 4.78. The pH of an aqueous solution of the corresponding salt,

BA

, will be

View answer and explanation

Correct option: C

7.01

Option C is correct because the pH of a salt of a weak acid and a weak base is determined by the difference between the pKa and pKb values.

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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}