Sodium Bicarbonate

Sodium bicarbonate is a chemical compound containing bicarbonate anion (HCO3–) and sodium cation (Na+). Sodium bicarbonate is a salty, alkaline solid found dissolved in several mineral springs and a component of mineral natron.

In 1791, French scientist Nicolas Leblanc created sodium carbonate. Austin Church and John Dwight, bakers from New York, founded the first baking soda factory in 1846. Sodium bicarbonate is a white solid crystalline chemical substance, usually a powder.

Instead of sodium hydroxide, we may use sodium bicarbonate as a wash to eliminate acidic contaminants from a “crude” liquid, providing a purer sample. Sodium bicarbonate reacts with acids to generate salts and carbonic acid, which decompose to CO2 and water:

NaHCO3 + HCl → NaCl + H2CO3

H2CO3 → H2O + CO2(g)

SOD reacts with acetic acid (vinegar) to produce sodium acetate, water, and CO2:

NaHCO3 + CH3COOH → CH3COONa + H2O + CO2(g)

Sodium bicarbonate reacts with bases to generate carbonates:

NaHCO3 + NaOH → Na2CO3 + H2O

NaHCO3 is the molecular formula for sodium bicarbonate.

Uses of sodium bicarbonate

Cooking

Baking soda reacts with an acid to produce carbon dioxide, which expands the batter and gives quick bread, cakes, and other baked and fried foods their unique grain and texture. The following is a general representation of the acid-base reaction:

NaHCO3 + H+ → Na+ + CO2 + H2O

Lemon juice, yoghurt, buttermilk, chocolate and vinegar are all acidic foods that cause this reaction. We can use baking soda with sourdough, which is acidic, to make a lighter, less acidic product.

Heat may also act as a raising agent in baking by decomposing sodium bicarbonate and producing carbon dioxide at temperatures over 80 °C (180 °F), as follows:

2 NaHCO3 → Na2CO3 + H2O + CO2

Without an acidic component, release only half of the available CO2. Aside from producing sodium carbonate (which is very alkaline) without acid, heat decomposition of sodium bicarbonate creates a bitter, “soapy” taste and a yellow colour. Cake batter does not rise until heated in the oven due to the slow reaction rate at room temperature.

Baking powder

There is no need for extra acids in baking powder since it contains 30% bicarbonate and other acidic chemicals activated by water. We may use baking powder with cream of tartar or salt bicarbonate with calcium acid phosphate. Baking powder is acidic, and baking soda is alkaline, avoids a metallic flavour during baking, and creates sodium carbonate.

Pyrotechnics

Black snake fireworks have sodium bicarbonate as a critical ingredient. Sucrose thermal decomposition, creating carbon dioxide and long snake-like ash in this effect. When heated, sodium bicarbonate releases CO2 and H2O, flame retardants.

Mild disinfectant

It is a weak disinfectant and maybe a fungicide for specific organisms. Baking soda absorbs musty odours, making it popular for used book dealers to deodorise books.

Fire extinguisher

Heating sodium bicarbonate creates carbon dioxide, which we can use to extinguish minor grease or electrical fires. We should not use it on deep fryer fires since the sudden gas release may cause grease splatter. BC dry chemical fire extinguishers use sodium bicarbonate instead of diammonium phosphate, which is more corrosive. 

Because sodium bicarbonate is alkaline, it is the only dry chemical agent used in commercial kitchen fire suppression systems. The agent saponified hot grease as an alkali, forming a smothering, soapy foam.

Neutralisation of acids

Sodium bicarbonate spontaneously reacts with acids, generating CO2. We can use it to neutralise undesirable acid solutions or acid spills in laboratories. Although amphoteric reacts with acids and bases, we cannot use sodium bicarbonate to neutralise bases.

Agriculture

Sodium bicarbonate applied to plants prevents fungal growth but does not kill them. A 2% sodium bicarbonate solution may produce fruit discolouration and chlorosis.

Personal hygiene

Some mouthwashes include sodium bicarbonate. It is anticaries and abrasive. It mechanically cleans teeth and gums, neutralises acid production, and acts as an antiseptic to help prevent infections. We can use sodium bicarbonate to manufacture dry or wet deodorants. If you are making a nasal irrigation solution, add a little sodium bicarbonate to it with the table salt.

Doctors use it to treat blepharitis in the eyes by adding a teaspoon of sodium bicarbonate to cold water heated and then gently cleaning the eyelash base with the solution.

Cleaning agent

Soda blasting is a method of removing paint and corrosion using sodium bicarbonate. Sodium bicarbonate is a blasting medium to remove surface contaminants from softer substrates like aluminium, copper, and wood that silica sand abrasive media may harm.

We can use a paste made from baking soda and a small amount of water as a mild scouring powder for eliminating surface rust since rust transforms into a water-soluble compound when exposed to a strongly alkaline solution; we should use cold water; as hot water solutions may damage the steel. Aluminium’s thin protective oxide layer makes sodium bicarbonate unsuitable for cleaning. 

A warm water solution eliminates tarnish from silver when it comes in contact with aluminium foil. We often use baking soda in washing machines to replace water softeners and deodorise clothes. It eliminates thick tea and coffee stains almost as effectively as sodium hydroxide when diluted with warm water.

Conclusion

Sodium bicarbonate is an odourless crystalline white, solid or powder that is stable in dry air but slowly decomposes to generate sodium carbonate when exposed to moist air. The substance is a food additive for humans and animals.

Sodium bicarbonate, also known as sodium hydrogen carbonate or bicarbonate of soda (NaHCO3), is a carbon dioxide source used in effervescent salts, baking powders, beverages, and the main ingredient in dry-chemical fire extinguishers. Due to its mild alkalinity, it is beneficial in treating stomach and urinary hyperacidity and acidosis. Additionally, we can use it in some industrial processes, such as tanning and wool preparation.