$0.2$ molar solution of formic acid is ionized $3.2\%$. Its ionization constant is
$0.2$ molar solution of formic acid is ionized $3.2\%$. Its ionization constant is
- A
$1 \times {10^{ - 12}}$
- B
$2.1 \times {10^{ - 4}}$
- C
$1.25 \times {10^{ - 6}}$
- D
$1 \times {10^{ - 14}}$
Similar Questions
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.
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.
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is
The dissociation constant of a substituted benzoic acid at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-4}$. The $\mathrm{pH}$ of a $0.01 \ \mathrm{M}$ solution of its sodium salt is
The dissociation constant of a substituted benzoic acid at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-4}$. The $\mathrm{pH}$ of a $0.01 \ \mathrm{M}$ solution of its sodium salt is
- [IIT 2009]
A solution of sodium borate has a $pH$ of approximately
A solution of sodium borate has a $pH$ of approximately
The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$
The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$