Carbonic Acid - Structure, Importance, Properties & Uses, FAQs

Carbonic acid has a chemical formula H₂CO₃. There is a small amount of this compound in the solution of carbon dioxide in water. Since the compound contains one carbon-oxygen double bond, its chemical carbonic acid formula is (H₂CO₃). The carbon dioxide chemical formula is CO₂. As the only acid exhaled in its gaseous state by the lungs, carbonic acid is often described as a respiratory acid. Carbonate and bicarbonate salts are formed by it; it is a weak acid.

Carbonic acid structure

Below is an illustration of carbonic acid's structure.

As demonstrated by the illustration above, carbonic acid has a structure that includes a carbon-oxygen double bond and two carbon-oxygen single bonds. One Hydrogen atom is attached to each oxygen atom participating in a single bond with the carbon.

Carin water, and carbon dioxide participate in the following chemical equilibrium :

CO₂ + H₂O ⇌ H₂CO₃

Carbon dioxide in water is converted into carbonic acid in the equilibrium described above, but it is a very small fraction. Carbon dioxide (chemical carbonic acid formula CO₂) is an acidic colorless gas with a density about 53% higher than that of dry air.

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H₂CO₃ properties

Under this subsection, you will find a list of some of the significant physical and chemical properties of carbonic acid.

1. Physical-chemical properties

• Carbonic acid has a molar mass of 62.024 grams per mole.
• 1.668 grams per cubic centimeter is its density in its standard state.
• In chemical terms, H₂CO₃ has a p Ka of 6.35.
• As a conjugate base, bicarbonate corresponds to carbonic acid.
• In most cases, this compound is dissolved in water. There have been reports that NASA scientists have prepared solid H₂CO₃ samples.

2. Chemical Properties

• A weak acid, H₂CO₃ is inherently unstable in nature.
• When water is present, it dissociates partially to give H⁺ and HCO₃^– (bicarbonate) ions.
• A diprotic acid such as carbonic acid can form two types of salts, both of which are bicarbonates.
• Bicarbonate salts are formed by adding a small quantity of a base to H₂CO₃, whereas carbonate salts are formed by adding an excess of a base.
• Interestingly, industrial fermentation processes or the burning of fossil fuels can result in the production of carbonic acid by-products.

Carbonic Acid Uses

With a wide range of uses, H₂CO₃ is a very useful compound. Carbonic acid is also used in the following ways.

• It is carbonic acid that is used to prepare carbonated water, sparkling wine, and other aerated drinks.
• Ammonium persulfate is precipitated from H₂CO₃ powder.
• By transporting carbon dioxide from the body, it helps to eliminate it.
• Ringworm and other dermatitis are treated by protonating certain nitrogenous bases in blood serum and applying a solution of carbonic acid to the area.
• Cleansing contact lenses with these solutions is extremely effective.
• When necessary (such as during drug overdoses), it can be consumed orally to induce vomiting.

Blood Carbonic Acid: Its Importance

By facilitating the process of breathing gas exchange, the bicarbonate ion facilitates the transport of carbon dioxide out of the human body.

It is quite slow for carbon dioxide to undergo hydration reactions, especially without the assistance of a catalyst. the red blood cells contain the enzyme family known as carbonic anhydrases, which contributes to the higher reaction rate.

Catalyzing the dissociation of carbon dioxide and water into carbonic acid is the role of carbonic anhydrase Enzymes. Blood plasma is dissolved in bicarbonate anions created by this process. Upon exhalation, CO₂ is formed from the catalyzed reaction in the lungs.

Importance of Carbonic Acid in Oceans

oceans are believed to have shifted the pH of the ocean water by approximately 0.1 due to the absorption of excess carbon dioxide from the atmosphere (primarily caused by human activities). Ocean water reacts with carbon dioxide to form hydrogen carbonate. Ocean acidification is a common term used to describe this process.

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