The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively. $0.1\,M$, $0.01\, M$ and $0.001\, M$. Which of the following is correct for $pOH$ of $A, B$ and $C$ ?
$pOH (A) < pOH (B) < pOH (C)$
$pOH (A) > pOH (B) > pOH (C)$
$pOH (A) = pOH (B) = pOH (C)$
$pOH (C) < pOh (A) < pOH (B)$
The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$, is
What is the $ pH$ of $0.01\, M$ glycine solution? For glycine, $K{a_1} = 4.5 \times {10^{ - 3}}$ and $K{a_2} = 1.7 \times {10^{ - 10}}$ at $298 \,K$
Write characteristics and uses of ${K_a}$ value.
The solution of $N{a_2}C{O_3}$ has $pH$
The dissociation constant of an acid $HA$ is $1 \times {10^{ - 5}}$. The $pH$ of $0.1$ molar solution of the acid will be