Given
$(i)$ $\begin{gathered}
HCN\left( {aq} \right) + {H_2}O\left( l \right) \rightleftharpoons {H_3}{O^ + }\left( {aq} \right) + C{N^ - }\left( {aq} \right) \hfill \\
{K_a} = 6.2 \times {10^{ - 10}} \hfill \\
\end{gathered} $
$(ii)$ $\begin{gathered}
C{N^ - }\left( {aq} \right) + {H_2}O\left( l \right) \rightleftharpoons HCN\left( {aq} \right) + O{H^ - }\left( {aq} \right) \hfill \\
{K_b} = 1.6 \times {10^{ - 5}} \hfill \\
\end{gathered} $
These equilibria show the following order of the relative base strength
$O{H^ - } > {H_2}O > C{N^ - }$
$O{H^ - } > C{N^ - } > {H_2}O$
${H_2}O > C{N^ - } > O{H^ - }$
$C{N^ - } > {H_2}O > O{H^ - }$
$25$ $mL$ $0.1$ $M$ $HCl$ solution is diluted till $500$ $mL$. Calculate $pH$ of dilute solution.
Which among the given acids has lowest $pKa$ value
The $pH$ of a $0.1\ M$ aqueous solution of a very weak acid $(HA)$ is $3$. What is its degree of dissociation ?......$\%$
For a weak acid $HA$ with dissociation constant ${10^{ - 9}},\,\,pOH$ of its $0.1 \,M$ solution is
Which oxychloride has maximum $pH$