${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.
${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.
$5.9 \times 10^{-10}$
Similar Questions
The solution of $N{a_2}C{O_3}$ has $pH$
The solution of $N{a_2}C{O_3}$ has $pH$
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
The $pH$ of $0.1$ $M$ $HCN$ solution is $5.2$ calculate ${K_a}$ of this solution.
The $pH$ of $0.1$ $M$ $HCN$ solution is $5.2$ calculate ${K_a}$ of this solution.
The $ pH$ of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be
The $ pH$ of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be
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 $H B \left( K _{ a }\right)=1 \times 10^{-8}$ )
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 $H B \left( K _{ a }\right)=1 \times 10^{-8}$ )
- [IIT 2018]