Preparation and Properties Sodium Carbonate

For thousands of years, people have been aware of and utilised sodium carbonate. The chemical was produced by the ancient Egyptians from natron, a mineral found in the bottoms of dry lakes. Natron is sodium carbonate and sodium bicarbonate mixture. In the mummification of deceased bodies, the Egyptians utilized sodium carbonate. The compound kept the bodies of the dead from decomposing by drying them out. The process was so successful that some 3,000-year-old mummified mummies are still in as good of shape as they were when they died. Sodium carbonate has also been created over the centuries by the combustion of organic waste, particularly seaweed. The compound’s common name, soda ash, comes from this technique of the manufacture (ash containing sodium compounds).

The information about sodium carbonate from various chemistry-related articles is available here. It is found that sodium carbonate (Na₂CO₃) is a chemical compound that is made up of inorganic elements. Students who want to flourish in chemistry need to be well known about sodium carbonate to get deep knowledge about it to do well on their exams. The definition, preparation, properties, and uses are provided here to assist students in effectively understanding the respective topic. Continue to visit our website for additional chemistry help.

Overview

Sodium carbonate (SO-de-um KAR-bun-ate) is a crystalline solid or odourless white powder with an alkaline taste. (Another alkaline-tasting material is baking soda.) It’s hygroscopic, which means it likes to collect moisture from the air. It’s also available as a monohydrate and a decahydrate, both of which have slightly different physical properties than the anhydrous salt. Soda ash refers to the anhydrous form of sodium carbonate, whereas salt soda or washing soda refers to the decahydrate form. One of the most important chemical substances manufactured has traditionally been sodium carbonate. Its main application is in the production of glass and other chemicals.

Sodium Carbonate

Sodium carbonate (Na₂CO₃) is a chemical compound that is made up of inorganic elements. Formerly, it was made from the ashes of plants that grew in sodium-rich soils. Soda ash is sometimes known as sodium carbonate. Trona is used to remove soda ash and it is a double salt that occurs in lakes as a result of evaporation processes. It is made up of sodium carbonate and sodium hydrogen carbonate.

The most significant of the basic heavy chemicals is sodium carbonate, sometimes known as washing soda or soda ash and it has the benefit of not being corrosive, making it safer to handle than sodium hydroxide.

It’s kept on-site in silos or charged into smaller hoppers as needed from bags. Due to the absorption of water and carbon dioxide from the atmosphere during transit and storage, soda ash slowly changes to sodium bicarbonate, and soda ash hydrates, which create a cake on exposed surfaces. This limits the amount of soda ash accessible, making the mechanical transfer more difficult, and making future dissolving more difficult. It is non-corrosive and is batched in the same way that batching lime powder is.

Preparation and Properties Sodium Carbonate

The Solvay Process is presently the only way to make sodium carbonate. In this method, carbon dioxide and ammonia are pumped into a chilled, saturated sodium chloride solution. In the processes that occur, sodium hydrogen carbonate, which is very slightly soluble in the presence of sodium ions, is almost completely precipitated. Filtration removes it, and it is burned to form sodium carbonate.

This procedure’s ingredients are inexpensive and widely available. Salt brine (NaCl), ammonia (NH₃), and limestone are the three (CaCO₃). Here, CaCl₂ is an important by-product of this procedure.

We can write the reactions as:

2NH₃+H₂O+CO₂→NH₄2CO₃

NH4₂CO₃+H₂O+CO₂→2NH₄HCO₃

When adding the common salt to the solution containing NH4+and HCO3– results in precipitation of NaHCO3, which is the least soluble and is then filtered off.

NH₄HCO₃+NaCl→NH₄Cl+NaHCO₃

Now, the sodium bicarbonate is then heated to give Na₂CO₃.

2NaHCO₃→Na₂CO₃+CO₂+H₂O

Finally, the CO₂ gas evolved can be reused again.

When anhydrous sodium carbonate is dissolved in water, it recrystallizes to form washing soda crystals that include ten molecules of water during the crystallisation process.

Advantages of the Solvay process:

• The Solvay process is extremely cost-effective
• The raw materials necessary for synthesis are easily available and inexpensive
• The only by-product produced is calcium chloride
• It makes the process pollution-free.
• The Solvay method generates high purity sodium carbonate, and ammonia and carbon dioxide can be recovered and utilised for another cycle.

Physical Properties of Sodium Carbonate:

Colourless or white crystalline powders of sodium carbonate are available. Sodium carbonate in its anhydrous state is hygroscopic. Sodium carbonate has an alkaline flavour and is odourless. Sodium carbonate is water-soluble, ethanol-soluble, and virtually insoluble in acetone. At typical pressures and temperatures, sodium carbonate is stable.

Na2CO3	Sodium Carbonate
Molecular Weight/ Molar Mass	105.9888 g/mol
Density	2.54 g/cm3
Boiling Point	1,600C
Melting Point	851C

Chemical Properties of Sodium Carbonate:

(1) Heat does not affect anhydrous sodium carbonate. At 8520C, it melts without disintegration.

(2) Due to hydrolysis, which produces OH^–( (aq) ions, aqueous sodium carbonate solutions are moderately alkaline.

Na₂CO₃( s)+2H2O(I)→H₂CO₃(aq)+2Na+(aq)+2OH^–(aq)

(3) Sodium carbonate aqueous solutions absorb carbon dioxide from the air and create sodium hydrogen carbonate.

Na₂CO₃(aq)+H₂O+CO₂( g)→2NaHCO₃(aq)

(4) When sodium carbonate combines with weak vegetable acids, such as lime juice, carbon dioxide is released.

Na₂CO₃(aq)+2H+(aq)→2Na+(aq)+H₂O(l)+CO₂( g)

Na₂CO₃(aq)+2HCl(aq)→2NaCl(aq)+H₂O(l)+CO₂( g)

Sodium Carbonate in Water

In general, sodium carbonate is a disodium salt of carbonic acid that has alkalinizing effects. When sodium carbonate is dissolved in water, it produces carbonic acid and sodium hydroxide. In water, sodium carbonate is extremely soluble. It quickly dissociates into sodium ions and carbonate ions, which combine with water to generate bicarbonate ions.

Uses of Sodium Carbonate

The following are some of the applications of sodium carbonate –

• It’s a common ingredient in detergents and soaps.
• It’s a material used in the production of glass.
• It’s a material used to make rayon polymers.
• It is used as an anti-caking agent, raising agent, stabilizer, and other food additives.
• It is used in cuisine, for example, Sodium Carbonate gives ramen noodles their unique flavour.
• It’s a material that’s employed in the brick industry.
• It’s utilized in the tanning and processing of animal hides.
• It is a foaming agent that is found in toothpaste.
• Water glass (Sodium silicate), borax, Sodium phosphate, and a variety of other salt compounds are all made from it.
• It’s a substance that’s used to change the pH of water.
• Carbonate is a water softener that precipitates hard water containing magnesium and calcium ions.
• It could also be used as an analytical reagent and as a laboratory standardization reagent.

Also read: Preparation and Properties of Sodium hydroxide

FAQs

What are the hazards related to Sodium Carbonate?

If handled poorly or if you are accidentally exposed to it, sodium carbonate can be harmful to your health and safety. This drug can cause irritation of the respiratory system, coughing, shortness of breath, and pulmonary edema when inhaled. Contact with the eyes can cause long-term corneal damage, as well as burns. Avoid swallowing or inhaling the dust if you use Sodium Carbonate or Soda Ash in your home. Sodium Carbonate should be handled with caution due to these dangers.

Where and in which form Sodium Carbonate is found?

Sodium carbonate can be created by mixing sodium chloride (salt) and ammonia. Food stores, swimming pool supply stores, and hardware stores all carry sodium carbonate. There is no odour or flavour to the grey-white powder, often known as a solid white powder. It's either a base or an alkali on the pH scale. It's usually safe when it comes into contact with the skin, but solutions made with it can be corrosive. While small dosages aren't dangerous, large amounts can cause poisoning. Sodium carbonate, on the other hand, has a relatively low toxicity risk.

Is sodium carbonate the same as baking soda?

Sodium carbonate is sometimes known as soda ash or washing soda whereas sodium bicarbonate is known as baking soda.