When CO_2 dissolves in water, the following&n | vedclass

Name: PDF Generator App | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

$\mathrm{Ka}=\frac{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}$

$\frac{\left[\mathrm

Vedclass · Accepted Answer

$3.8 	imes 10^{-1}$

Vedclass · Answer

$\mathrm{Ka}=\frac{\left[\mathrm{H}_{3} \mathrm{O}^{+}ight]\left[\mathrm{HCO}_{3}^{-}ight]}{\left[\mathrm{CO}_{2}ight]}$

$\frac{\left[\mathrm{HCO}_{3}^{-}ight]}{\left[\mathrm{CO}_{2}ight]}=\frac{\mathrm{Ka}}{\left[\mathrm{H}_{3} \mathrm{O}^{+}ight]}$

$=\frac{3.8 	imes 10^{-7}}{10^{-6}}=3.8 	imes 10^{-1}$

When $CO_2$ dissolves in water, the following equilibrium is established

$C{O_2} + 2{H_2}O\, \rightleftharpoons {H_3}{O^ + } + HCO_3^ - $

for which the equilibrium constant is $3.8 \times 10^{-7}$ and $pH = 6.0$. The ratio of $[HCO_3^- ]$ to $[CO_2]$ would be :-

Similar Questions

The ionization constant of propanoic acid is $1.32 \times 10^{-5}$. Calculate the degree of ionization of the acid in its $0.05\, M$ solution and also its $pH$. What will be its degree of ionization if the solution is $0.01$ $M$ in $HCl$ also?

The $pH$ of $ 0.1 \,M$ solution of a weak monoprotic acid $1\%$ ionized is

At $25\,^o C$, the dissociation constant of a base $BOH$ is $1.0 \times {10^{ - 12}}$. The concentration of Hydroxyl ions in $0.01\, M$ aqueous solution of the base would be

Write characteristic and uses of weak base equilibrium constant ${K_b}$.

The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$

When $CO_2$ dissolves in water, the following equilibrium is established $C{O_2} + 2{H_2}O\, \rightleftharpoons {H_3}{O^ + } + HCO_3^ - $ for which the equilibrium constant is $3.8 \times 10^{-7}$ and $pH = 6.0$. The ratio of $[HCO_3^- ]$ to $[CO_2]$ would be :-