The $ pH$ of $ 0.1$ $M$ acetic acid is $3$, the dissociation constant of acid will be
$1.0 \times {10^{ - 4}}$
$1.0 \times {10^{ - 5}}$
$1.0 \times {10^{ - 3}}$
$1.0 \times {10^{ - 8}}$
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 $HCl$ ?
Derive the equation of ionization constant $({K_b})$ of weak base.
$p{K_a}$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1\,\,M$ sodium acetate solution will be
Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^+$ ions is $3.4 \times 10^{-4}$. Then find out initial concentration of $CH_3COOH$ Molecules
${K_a}$ of $C{H_3}COOH$ is $1.76 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate dissociation constant of its conjugate base.