The degree of ionization of a $0.1 \,M$ bromoacetic acid solution is $0.132$ Calculate the $pH$ of the solution and the $p K_{ a }$ of bromoacetic acid.
Degree of ionization, $a=0.132$
Concentration, $c=0.1\, M$
Thus, the concentration of $H _{3} O ^{+}= c$. $a$
$=0.1 \times 0.132$
$=0.0132$
$pH =-\log \left[ H ^{+}\right]$
$=-\log (0.0132)$
$=1.879: 1.88$
Now,
$K_{a}=C \alpha^{2}$
$=0.1 \times(0.132)^{2}$
$K_{a}=.0017$
$p K_{a}=2.75$
Calculate the degree of ionization of $0.05 \,M$ acetic acid if its $p K_{ a }$ value is $4.74$
How is the degree of dissociation affected when its solution also contains $(a)$ $0.01 \,M$ $(b)$ $0.1 \,M$ in $HCl$ ?
The ionization constant of $HF$, $HCOOH$ and $HCN$ at $298\, K$ are $6.8 \times 10^{-4}, 1.8 \times 10^{-4}$ and $4.8 \times 10^{-9}$ respectively. Calculate the ionization constants of the corresponding conjugate base.
In its $0.2\,\, M$ solution, an acid ionises to an extent of $60\%$. Its hydrogen ion concentration is.....$M$
Which oxychloride has maximum $pH$
The solubility of a salt of weak acid $( A B )$ at $pH 3$ is $Y \times 10^{-3} mol L ^{-1}$. The value of $Y$ is
. . . . . (Given that the value of solubility product of $A B \left( K _{ sp }\right)=2 \times 10^{-10}$ and the value of ionization constant of $H B \left( K _{ a }\right)=1 \times 10^{-8}$ )