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| Sodium Hydrogen Carbonate | |
|---|---|
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| IUPAC name | Sodium Hydrogencarbonate |
| Other names | Sodium bicarbonate; bicarbonate of soda; baking soda |
| Identifiers | |
| CAS number | [144-55-8] |
| RTECS number | VZ0950000 |
| Properties | |
| Molecular formula | NaHCO3 |
| Molar mass | 84.007 g/mol |
| Appearance | White crystalline solid. |
| Density | 2.159 g/cm3, solid. |
| Melting point |
Decomposes around 50 °C |
| Solubility in water | 7.8g/100ml water at 18 °C |
| Refractive index (nD) | 1.500 |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | Irritant, esp. to respiratory system |
| NFPA 704 |
 0
1
0
|
| Flash point | Non-flammable. |
| Related compounds | |
| Other anions | Sodium carbonate; carbonic acid |
| Related compounds | Sodium bisulfate; sodium hydrogen phosphate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Sodium bicarbonate or sodium hydrogen carbonate is the chemical compound with the formula NaHCO3. Sodium bicarbonate is a white solid that is crystalline but often appears as a fine powder. It has a slight alkaline taste resembling that of washing soda (sodium carbonate). It is a component of the mineral natron and is found dissolved in many mineral springs. The natural mineral form is known as nahcolite. It is also produced artificially.
Since it has long been known and is widely used, the salt has many related names such as baking soda, bread soda, cooking soda, bicarbonate of soda. Colloquially, its name is shortened to sodium bicarb. The word saleratus, from Latin sal æratus meaning "aerated salt", was widely used in the 19th century for both sodium bicarbonate and potassium bicarbonate. The term has now fallen out of common usage.
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History
The ancient Egyptians used natural deposits of natron, a mixture consisting mostly of sodium carbonate decahydrate and sodium bicarbonate. The natron was used as a cleansing agent like soap.
In 1791 a French chemist produced sodium bicarbonate, as we know it today. But it was only in 1846 that two New York bakers, John Dwight and Austin Church, developed the process of making baking soda from sodium carbonate and carbon dioxide.[1] Each started a company, and the two companies later merged to form Church & Dwight, the makers of Arm & Hammer baking soda.
Production
NaHCO3 is mainly prepared by the Solvay process, which is the reaction of calcium carbonate, sodium chloride, ammonia, and carbon dioxide in water. It is produced on the scale of about 100,000 ton/year (as of 2001).[2]
NaHCO3 may be obtained by the reaction of carbon dioxide with an aqueous solution of sodium hydroxide. The initial reaction produces sodium carbonate:
- CO2 + 2NaOH → Na2CO3 + H2O
Further addition of carbon dioxide produces sodium bicarbonate, which at sufficiently high concentration will precipitate out of solution:
- Na2CO3 + CO2 + H2O → 2NaHCO3
Commercial quantities of baking soda are also produced by a similar method: soda ash, mined in the form of the ore trona, is dissolved in water and treated with carbon dioxide. Sodium bicarbonate precipitates as a solid from this method:
- Na2CO3 + CO2 + H2O → 2NaHCO3
Chemistry
Sodium bicarbonate is an amphoteric compound. It has a pKa of 6.3 in water which causes aqueous solutions to be mildly alkaline:
- HCO3- + H2O → H2CO3 + OH-
Sodium bicarbonate can be used as a wash to remove any acidic impurities from a "crude" liquid, producing a more pure sample. Reaction of sodium bicarbonate and an acid to give a salt and carbonic acid, which readily decomposes to carbon dioxide and water:
- NaHCO3 + HCl → NaCl + H2CO3
- H2CO3 → H2O + CO2 (gas)
Reaction of sodium bicarbonate and acetic acid:
Sodium bicarbonate reacts with bases:
- NaHCO3 + NaOH → Na2CO3 + H2O
Thermal decomposition
Above 60 °C, it gradually decomposes into sodium carbonate, water and carbon dioxide. The conversion is fast at 200 °C:citation needed
- 2NaHCO3 → Na2CO3 + H2O + CO2
Most bicarbonates undergo this dehydration reaction. Further heating converts the carbonate into the oxide (at around 1000°C):
- Na2CO3 → Na2O + CO2
These conversions are relevant to the use of NaHCO3 as a fire-suppression agent ("BC powder") in some dry powder fire extinguishers.
Applications
Cooking
Sodium bicarbonate is primarily used in cooking (baking) where it reacts with other components to release carbon dioxide, that helps dough "rise". The acidic compounds that induce this reaction include phosphates, cream of tartar, lemon juice, yogurt, buttermilk, cocoa, vinegar, etc., hence sodium bicarbonate can be substituted for baking powder provided sufficient acid reagent is also added to the recipe.[3] Many forms of baking powder contain sodium bicarbonate combined with one or more acidic phosphates or cream of tartar.
Neutralization of acids and bases
Many laboratories keep a bottle of sodium bicarbonate powder within easy reach, because sodium bicarbonate is amphoteric, reacting with acids and bases. (See Chemistry) Furthermore, as it is relatively innocuous in most situations there is no harm in using excess sodium bicarbonate. Lastly, sodium bicarbonate powder may be used to smother a small fire.
A wide variety of applications follow from its neutralization properties including ameliorating the effects of white phosphorus in incendiary bullets from spreading inside an afflicted soldier's wounds.[4] Sodium bicarbonate can be added as a simple solution for raising the pH balance of water that has a high level of chlorine, such as in swimming pools and aquariums.[5]
Medical uses
Sodium bicarbonate is used as an antacid to treat acid indigestion and heartburn[6] An aqueous solution is administered intravenously for cases of acidosis, or when there is insufficient sodium or bicarbonate ions in the blood.[7] This compound has also been used as for patients who have had a ureterosigmoidostomy.citation needed
Adverse reactions to emergency administration include congestive heart failure, with edema secondary to sodium overload, and the metabolic complication of hyperosmolarity, metabolic alkalosis, and hypernatremia.citation needed
As a cleaning agent
- A paste from baking soda can be very effective when used in cleaning and scrubbing.
- For cleaning of aluminium objects it is to be discouraged as it attacks the thin unreactive protective oxide layer of this otherwise very reactive metal.
- A solution in warm water will remove the tarnish from silver when the silver is in contact with a piece of aluminium foil[1].
Miscellanea
- Sodium bicarbonate is used in BC Dry Chemical fire extinguishers as an alternative to the corrosive ammonium phosphate in ABC extinguishers. The alkali nature of sodium bicarbonate makes it the only dry powder agent, besides Purple-K, allowed for use on commercial deep fat fryers. The agent forms a crust over the surface similar to the effects of a wet chemical.citation needed
- It is used in a process for cleaning paint called sodablasting.
- It can be used as a carbon sequestration agent to trap carbon dioxide greenhouse gas emissions in solid form, as one potential tool against global warming.[8]
- It can be administered to garden ponds to raise pH levels.
See also
References
- ^ "Company History". Church & Dwight Co..
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Radiation Cookery Book 45th Edition, Radiation Group Sales Ltd 1954
- ^ "White Phosphorus". GlobalSecurity.org. Retrieved on 2007-09-26.
- ^ "Outdoor Fun: Pool Care". Arm & Hammer Baking Soda (2003). Retrieved on 2007-09-26.
- ^ "Sodium Bicarbonate". Jackson Siegelbaum Gastroenterology (1998).
- ^ "Sodium Bicarbonate Intravenous Infusion". Consumer Medicine Information. Better Health Channel (2004-07-13).
- ^ "Can baking soda curb global warming?". CNet News (2007). Retrieved on 2007-12-30.
Further reading
- Bishop, D., J. Edge, C. Davis, and C. Goodman. Induced Metabolic Alkalosis Affects Muscle Metabolism and Muscle Metabolism and Repeated-Sprint Ability. Medicine and Science in Sports Exercise, Vol. 36, No. 5, pp. 807-813, 2004.
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