Question

How do you write the chemical equation for the reaction of carbonic acid ${H_2}C{O_3}$ with water ?

Answer 1

$\;{H_2}C{O_3}$ is a powerless acid and is unstable in nature. It goes through incomplete separation within the sight of water to yield ${H^ + }$ and $HC{O_3}^-$ (bicarbonate) ion.

Complete step by step answer:
From the representation given above, it tends to be perceived that the structure of carbonic acid comprises one carbon-oxygen double bond and two carbon-oxygen single bonds. The oxygen particles participating in a single bond with the carbon each have one hydrogen atom attached to them.
Carbonic acid , which is framed by the disintegration and hydrolysis of $\;C{O_2}$ in water, is the significant common filtering specialist in numerous calm biological systems. Carbonic acid is both weak and unsteady and rapidly separates into hydrogen ion $\left( {{H^ + }} \right)$ and bicarbonate ion $\left( {HC{O_3}^-} \right)$
Carbon dioxide, when broken down in water, takes an interest in the following chemical equilibrium.
$C{O_2} + {\text{ }}{H_2}O\; \rightleftharpoons \;H2C{O_3}$
In any case, just a limited quantity of carbon dioxide is changed over into carbonic acid in the synthetic balance depicted previously.
Aqueous carbon dioxide, $C{O_2}$ (aq), responds with water forming carbonic acid,$\;{H_2}C{O_3}$ (aq). Carbonic acid may free protons to shape bicarbonate, $HC{O_3}^ -$ , and carbonate, $C{O_3}^{2 - }$ . For this situation the proton is freed to the water, diminishing pH. The perplexing synthetic equilibria are depicted utilizing two acid equilibrium conditions.
Carbonic acid is a weak Bronsted acid......
${H_2}C{O_3}\left( {aq} \right) + {H_2}O\left( l \right){\text{ }} \to {\text{ }}{H_3}{O^ + } + {\text{ }} - O\left( {O = } \right)C - OH$
Carbonic acid → bicarbonate ions
More often than not we can treat carbonic acid, ${H_2}C{O_3}$ , as hydrated carbon dioxide
: for example ${H_2}C{O_3} \equiv \left( {O = } \right)2C \cdot {H_2}O$ . The oxidation states are the equivalent
${H_2}C{O_3} + {\text{ }}{H_2}O{\text{ }} = {\text{ }}HC{O_3}^ - + {\text{ }}{H_3}{O^ + }$

Note:
$C{O_2}$ enters water through interface with the environment and the natural cycles of natural carbon processing and photosynthesis.
Fluid carbon dioxide, $C{O_2}$ (aq), responds with water forming carbonic acid , ${H_2}C{O_3}$ (aq).
Carbonic acid may free protons to shape bicarbonate, $HC{O_3}^ -$ , and carbonate, $C{O_3}^{2 - }$ . For this situation the proton is freed to the water, diminishing $pH$.