Question

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

Answer 1

Hint: \[\;{H_2}C{O_3}\] 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 \[pH\].