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 :-
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 :-
- A
$3.8 \times 10^{-13}$
- B
$3.8 \times 10^{-1}$
- C
$6.0$
- D
$13.4$
Similar Questions
Dissociation constat of weak acid $HA$ is $1.8 \times {10^{ - 4}}$ calculate Dissociation constant of its conjugate base ${A^ - }$
Dissociation constat of weak acid $HA$ is $1.8 \times {10^{ - 4}}$ calculate Dissociation constant of its conjugate base ${A^ - }$
A $0.1\, M$ solution of $HF$ is $1\%$ ionized. What is the $K_a$
A $0.1\, M$ solution of $HF$ is $1\%$ ionized. What is the $K_a$
What is the $pH$ of solution of $7$ $gm$ $N{H_4}OH$ per $500$ $mL$ ? ( ${K_b}$ of $N{H_4}OH 1.8 \times {10^{ - 5}}$, Molecular moles of $N{H_4}OH$ is $35\,g\,mo{l^{ - 1}}$ )
What is the $pH$ of solution of $7$ $gm$ $N{H_4}OH$ per $500$ $mL$ ? ( ${K_b}$ of $N{H_4}OH 1.8 \times {10^{ - 5}}$, Molecular moles of $N{H_4}OH$ is $35\,g\,mo{l^{ - 1}}$ )
Degree of dissociation of $0.1\,N\,\,C{H_3}COOH$ is (Dissociation constant $ = 1 \times {10^{ - 5}}$)
Degree of dissociation of $0.1\,N\,\,C{H_3}COOH$ is (Dissociation constant $ = 1 \times {10^{ - 5}}$)
Which of the following base is weakest
Which of the following base is weakest