(B) The equilibrium constant expression for the given reaction is:$K_a = \frac{[H_3O^{+}][HCO_3^-]}{[CO_2]}$Rearranging to find the ratio of $[HCO_3^-

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(B) The equilibrium constant expression for the given reaction is:$K_a = \frac{[H_3O^{+}][HCO_3^-]}{[CO_2]}$Rearranging to find the ratio of $[HCO_3^-]$ to $[CO_2]$:$\frac{[HCO_3^-]}{[CO_2]} = \frac{K_a}{[H_3O^{+}]}$Given $pH = 6.0$,we have $[H_3O^{+}] = 10^{-pH} = 10^{-6} \ M$.Substituting the values:$\frac{[HCO_3^-]}{[CO_2]} = \frac{3.8 \times 10^{-7}}{10^{-6}} = 3.8 \times 10^{-1}$

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Mix Examples-Ionic Equilibrium

Medium

When $CO_2$ dissolves in water,the following equilibrium is established:
$CO_2 + 2H_2O \rightleftharpoons H_3O^{+} + HCO_3^-$
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
$13.4$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Mix Examples-Ionic Equilibrium

Given,$pH$ of a solution $A$ is $3$ and it is mixed with another solution $B$ having $pH$ $2$. If both are mixed in equal volume,then the resultant $pH$ of the solution will be

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What is the $pH$ of the resulting solution when $20 \text{ mL}$ of $\frac{M}{10} \text{ NaOH}$ and $10 \text{ mL}$ of $\frac{M}{10} \text{ H}_2\text{SO}_4$ are mixed together?

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In which of the following acid-base titrations is the $pH$ at the equivalence point greater than $8$?

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In a solution,$0.02 \ M$ acetic acid is $4 \%$ dissociated. The $[OH^{-}]$ in the solution is

DifficultMHT CET 2009

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$BaCO_3 \downarrow + 2HCl \longrightarrow BaCl_2 + CO_2 \uparrow + H_2O$

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When $CO_2$ dissolves in water,the following equilibrium is established:$CO_2 + 2H_2O \rightleftharpoons H_3O^{+} + HCO_3^-$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

Given,$pH$ of a solution $A$ is $3$ and it is mixed with another solution $B$ having $pH$ $2$. If both are mixed in equal volume,then the resultant $pH$ of the solution will be

What is the $pH$ of the resulting solution when $20 \text{ mL}$ of $\frac{M}{10} \text{ NaOH}$ and $10 \text{ mL}$ of $\frac{M}{10} \text{ H}_2\text{SO}_4$ are mixed together?

In which of the following acid-base titrations is the $pH$ at the equivalence point greater than $8$?

In a solution,$0.02 \ M$ acetic acid is $4 \%$ dissociated. The $[OH^{-}]$ in the solution is

Assign $A$,$B$,$C$,$D$ from the given type of reaction.$BaCO_3 \downarrow + 2HCl \longrightarrow BaCl_2 + CO_2 \uparrow + H_2O$

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When $CO_2$ dissolves in water,the following equilibrium is established:
$CO_2 + 2H_2O \rightleftharpoons H_3O^{+} + HCO_3^-$
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:

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$BaCO_3 \downarrow + 2HCl \longrightarrow BaCl_2 + CO_2 \uparrow + H_2O$