The $pH$ of an aqueous solution of ${\rm{C}}{{\rm{H}}_3}{\rm{COONa}}$ of concentration $C\left( {\rm{M}} \right)$ is given by

$7 - \frac{1}{2}p{K_a} - \frac{1}{2}\log C$

$\frac{1}{2}p{K_w} + \frac{1}{2}p{K_b} + \frac{1}{2}\log C$

$\frac{1}{2}p{K_w} - \frac{1}{2}p{K_b} - \frac{1}{2}\log C$

NEET UG CHEMISTRY MCQ: Equilibrium

1 Easy

1 of 1

Application +4 | -1

The

pH

of an aqueous solution of

\mathrm{C}{\mathrm{H}_3}\mathrm{COONa}

of concentration

C\left( \mathrm{M} \right)

is given by

View answer and explanation

Correct option: D

\frac{1}{2}p{K_w} + \frac{1}{2}p{K_a} + \frac{1}{2}\log C

Option D is correct because the pH of a salt of a weak acid and a strong base is given by the formula pH = 1/2 pKw + 1/2 pKa + 1/2 log C.

Practice All Chapter MCQs →

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}