The $ pH$ of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be
$1.0 \times {10^{ - 4}}$
$1.0 \times {10^{ - 5}}$
$1.0 \times {10^{ - 3}}$
$1.0 \times {10^{ - 8}}$
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 $C$ ?
A solution of sodium borate has a $pH$ of approximately
Degree of dissociation of $0.1\,N\,\,C{H_3}COOH$ is (Dissociation constant $ = 1 \times {10^{ - 5}}$)
The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$, is
The degree of dissociation of $0.1\,M\,HCN$ solution is $0.01\%$ . Its ionisation constant would be