Sodium Bicarbonate

Sodium Bicarbonate

Sodium bicarbonate is a chemical compound with the formula NaHCO₃. It is a white crystalline solid that mostly appears as a fine powder. It has a somewhat salty, alkaline taste, like washing soda (sodium carbonate). The natural mineral form is a component of the mineral natron, called nahcolite. It is found dissolved in many mineral springs.

Since it has long been known and is widely used as a food additive, the salt has many related names such as baking or cooking soda, and bicarbonate of soda. Its name comes from the Latin sal æratus meaning aerated salt.

Difference between baking soda and baking powder

Baking powder contains baking soda, plus a powdered acid and cornstarch. Baking powder is a mixture. Baking soda, NaHCO_3, is a pure substance.

Baking soda is alkaline, so acid is used in baking powder to avoid a metallic taste when the chemical change during baking creates sodium carbonate. However, to avoid the over-flavoring of acidic taste, non-acid ingredients like milk or Dutch-processed cocoa must be added.

NaHCO₃ can be obtained by the reaction of carbon dioxide with a water based solution of sodium hydroxide. This reaction produces sodium carbonate:

CO₂ + 2 NaOH → Na₂CO₃ + H₂O

Adding more carbon dioxide produces sodium bicarbonate, which at sufficiently high concentration will accumulate on the bottom. Commercial quantities of baking soda are also produced by a similar method: soda ash, mined as the ore trona, is dissolved in water and treated with carbon dioxide.

The word "trona" comes from the ancient Egyptian word ntry. From deposits found in the Natron Valley, they ground, solvated it, and then used it as paint for hieroglyphics. It precipitates as a solid from this method:

Na₂CO₃ + CO₂ + H₂O → 2 NaHCO₃

Reaction of sodium bicarbonate salt and an acid produce a salt and carbonic acid, which readily decomposes to carbon dioxide and water:

NaHCO₃ + HCl → NaCl + H₂CO₃

H₂CO₃ → H₂O + CO₂

Sodium bicarbonate reacts with acetic acid (in vinegar), producing sodium acetate, water, and carbon dioxide:

NaHCO₃ + CH₃COOH → CH₃COONa + H₂O + CO₂

Sodium bicarbonate reacts with bases such as sodium hydroxide to form sodium carbonates and water:

NaHCO₃ + NaOH → Na₂CO₃ + H₂O

 

Applications:

• As a neutralizer of acids and bases: The salt, NaHCO₃ is reacting with acids and bases. It reacts violently with acids plus releasing CO₂ gas as a reaction,
• As Trona is a common source of soda ash, it is a significant economic commodity because of its applications in manufacturing glass, chemicals, paper, detergents, and textiles,
• As a biopesticide (EPA), an effective way to control fungus growth, 
• As a pest control: kills cockroaches,
• As a paint and corrosion remover,
• As a pH Balancer,
• As a meat tenderizer,
• As a cattle feed supplement,
• As a mild disinfectant: an effective fungus killer,
• As a musty smell absorber,
• As a remover of splinters from the skin,
• As a fire extinguisher,
• With acids: baking soda is primarily used in cooking & baking, as a leavening agent.
  • it reacts with acidic components (Vit-C as L-ascorbic acid, or natural acids in sourdough) in foods like batters, releasing carbon dioxide, which causes expansion of the batter and forms the characteristic texture and grain in pancakes, cakes, quick breads, soda bread, and others.
  • used in breadings to enhance crispness.
  • as baking powder if sufficient acid is added to the recipe.
• Medical uses:
  • as an antacid (mixed with water) to treat acid indigestion and heartburn,
  • intravenously: only when the blood pH is <7.0, and only if there are insufficient sodium or bicarbonate ions in the blood. It raises the pH, thus used in cardiopulmonary resuscitation.
  • Since it can cause alkalosis, it is sometimes used to treat aspirin overdoses. Aspirin requires an acidic environment for proper absorption, and the basic environment diminishes aspirin absorption.
  • used in the treatment of an antidepressant overdose.
  • used topically as a paste, with 3 parts baking soda to one part water, to relieve insect bites and stings (plus their swelling).
  • treat an allergic reaction to plants such as poison -ivy -oak or -sumac to relieve the itching.
  • Adverse reactions to excessive NaHCO₃ can include metabolic alkalosis, edema, congestive heart failure, etc.
• Personal hygiene
  • in toothpaste for better whitening and plaque removal.
  • as an ingredient in mouthwash. It has anti-caries and abrasive properties. It works as a mechanical cleanser on the teeth and gums, neutralizes the production of acid in the mouth and also acts as an antiseptic to help prevent infections.
  • as a dry or wet deodorant or shampoo together with other ingredients.
  • as a buffering agent, combined with table salt, for nasal irrigation.
  • to treat blepharitis, by gently scrubbing the eyelash base.
  • as a body detoxifier, laying in the bathtub.
• In sports: As NaHCO₃ is slightly toxic, only small amounts of it could be used as a 3-7 min. energy kick.
• As cleaning agent:
  • silver,
  • surface rust,
  • washing machines,
  • removes odors from clothes,
  • removing heavy tea and coffee stains,
  • clothing contaminated with uranium (DU) dust.

Bicarbonate

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