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Sodium bicarbonate

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Sodium bicarbonate
Sodium Bicarbonate Structure.png
General
Systematic name Sodium Hydrogen Carbonate
Other names

Sodium hydrogen carbonate
Sodium acid carbonate
Baking soda
Bicarbonate of soda
Col-evac
Jusonin
NEUT
Soda mint

Molecular formula NaHCO3
SMILES C(O)(=O)[O-].[Na+]
Molar mass Molar mass::84.01
Appearance White, crystalline powder
CAS number CAS number::144-55-8
Properties
Density and phase [[Density:: 2.16 g/cm-3 solid]]
Solubility in water 7.8g/100g water (18°C)
Melting point Melting point::270°C
Decomposition 50°C (loses CO2)
Acidity (pKa) HCO3- <-> CO32- + H+ pKa = 10.33

CO2 + H2O <-> HCO3- + H+ pKa = 6.33

Structure
Molecular shape Trigonal Planar
Crystal structure Monoclinic-prismatic
Hazards
MSDS Material Safety Data Sheet
Main hazards Slightly hazardous if ingested or inhaled;

mild irritant to eyes and skin.

NFPA 704

NFPA 704 svg.png

0
1
0
Flash point Not applicable
RTECS number VZ0950000
Related compounds
Other anions Sodium carbonate
Other cations Sodium carbonic acid
Related compounds

CH3NaO3
(sodium hydroxymethanone hydrate)
CHNaO2
(sodium hydroxymethanone)
CH3NaO4
(sodium carbonic acid hydroxide)
CHKNaO3+
(potassium sodium hydrogen carbonate)

Except where noted otherwise, data are given for
materials in their standard state (at 25 °C, 100 kPa)
Disclaimer and references

Sodium bicarbonate (NaHCO3), recognized by most as ordinary baking soda, is a compound known for its unusual properties and diverse applications. Found in deposits throughout the globe, natural sodium bicarbonate works to maintain the Earth's balance of carbon dioxide and pH. [1] Baking soda was first used mainly for cooking purposes, but over the last 150 years, its production has grown to include manufacturing of other metals and glass, and as a basic household cleaner. This natural substance has also increased in popularity because it has no adverse effects on the environment.

Properties

Baking soda is commonly used in cooking.

Sodium bicarbonate (most commonly known as baking soda) is classified as an acid salt. This classification results from the combination of the base sodium hydroxide and the acid carbonic, which also gives baking soda the properties of a mild alkali. When heated, sodium bicarbonate releases carbon dioxide and it reacts as a leavening agent for culinary purposes as well as a fire retardant. Carbon dioxide is heavier than the air fueling the fire, so the baking soda smothers the flames. Sodium bicarbonate is capable of precipitating calcium and can absorb acid gas emissions such as sulfur dioxide. [2] Baking soda exists as a solid composed of white, monoclinic crystals and weighs 84.01 g/mol. [3] Because sodium bicarbonate begins to decompose at 50°C, it is difficult to properly determine a boiling or melting point. [4] Its decomposition produces sodium carbonate (Na2CO3), carbon dioxide (CO2), and water (H2O). [5] Baking soda is neither flammable nor explosive. Its chemical attributes also prevent oxidization and make it insoluble (doesn't dissolve) in alcohol. Although it is a mild irritant to the eyes, baking soda remains otherwise non-toxic and safe for general use. [6]

Occurrences

Most sodium bicarbonate is produced through artificial means, but in nature it's found in a mineral called nahcolite. The name Nahcolite is a mnemonic for its chemical formula (Na+H+CO+lite). This mineral, known as an evaporite (“A sedimentary deposit that results from the evaporation of seawater”) [7] , forms in oil shales and lake sediment deposits, and capable of absorbing water. Nahcolite coloring ranges from colorless to brown, and the crystals are monoclinic and transparent. Nahcolite has been found most notably in California, Colorado, Egypt and Kenya. Although the first major find of nahcolite was near Searles Lake, California in 1940 [8] , it was first reported by P. Walther in East Africa. In the oil-shale riverbed of the Green River (Colorado), nahcolite deposits as large as five feet in diameter and other formations with layers four inches thick, have been discovered. Sodium bicarbonate is rarely found in nature because, when exposed, it loses carbon dioxide and passes into another mineral called trona (hydrated sodium bicarbonate carbonate). When water vapor and carbon dioxide react with trona, sodium bicarbonate is a resulting byproduct. Nahcolite only forms when there is excessive and contained carbon dioxide; otherwise, trona will form in its place. [9]

Trona can be a source of hydrated sodium bicarbonate.

Prior to the late 1800s, the Leblanc process was used to manufacture soda ash (sodium carbonate), from which sodium bicarbonate is produced. This process required the creation of sodium sulfate by heating up sodium chloride (table salt) and sulfuric acid. In the late 1800s however, this process was abandoned in favor of the Solvay method in which ammonium and carbon dioxide are exposed to a concentrated solution of sodium chloride. This process creates crude sodium bicarbonate that is refined into pure baking soda. Before being used in food products or for pharmaceutical purposes, the refined baking soda must pass the specifications laid out by the U.S. Food and Drug Administration (FDA) and the United States Pharmacopoeia and Food Chemicals Codex. This ensures the quality and safety of the finished product. [10]

Uses

The reaction of baking soda and vinegar is a favorite science fair project to make a volcano eruption.

Although many people associate baking soda with its role as a cleaner and deodorizer, its chief use is in the food industry. In the United States alone, 33% of baking soda production is consumed in this manner. When used in baking as a key ingredient in baking powder, sodium bicarbonate reacts and releases carbon dioxide. This makes it the most commonly used leavening agent in cooking. Carbonated soda manufacturers have taken advantage of this reaction and frequently add baking soda to drinks to create carbon dioxide bubbles. Much of sodium bicarbonate production goes toward feed supplements for animals, accounting for approximately 25% of its use. For poultry, this valuable supplement enables them to tolerate heat, increases the quality of the eggshell, and keeps up the balance of sodium. Cows need sodium bicarbonate to properly digest fiber and sustain the pH of the rumen. Chemists utilize baking soda as a catalyst, buffer, a blowing agent, and feedstock for chemicals. Other industries that use sodium bicarbonate include pharmaceuticals- as a buffering agent, source of carbon dioxide, and an antacid; leather tanning (maintains pH during the tanning of hides); and the production of sodium carbonate. Because of its weak basicity, baking soda counteracts the effects of nasty smells or odors, and can even act as a fire suppressant. (Myers 248) [11] Baking soda is also employed in the production of glass, laundry detergents, soaps, paper, as well as aluminum refining and other processes of manufacturing various metals. [12]

Baking soda is a popular chemical compound for household purposes because of its versatility, safety, and availability. Its existence as a natural chemical makes it environmentally safe to use and it can even be recycled around the house. [13] The applications of baking soda for everyday use are endless, including, but not limited to: toothpaste, skin irritations (cuts, allergies, etc.), general household cleaner, refrigerator deodorizer, canning, pest and rodent repellant, and stain remover. (Summary of Hughes 1-41) [14]

Household Antacid

One of the most popular and common applications of sodium bicarbonate is a homemade remedy for heartburn. Known as an antacid (a compound that absorbs and neutralizes stomach acid), simple baking soda can temporarily relieve symptoms of indigestion and occasional heartburn. When taken with food, the effects of sodium bicarbonate can last for two to three hours, but at best it is something to be used infrequently and is not a replacement for prescription medication. [15] Heartburn happens when people eat too rapidly or eat certain foods, which causes a small amount of stomach acid to enter the esophagus and produce a burning feeling in the chest. Baking soda can neutralize the acid because of its alkaline properties, and is often used because of its availability and affordability. If a person overdoses on sodium bicarbonate however, it can neutralize too much of the stomach's acid and prevents the proper digestion of food. This can lead to inflammation and allergies throughout the body. [16] Baking soda is not a suitable medication for people suffering from edema, high blood pressure, or heart disease because it increases the level of sodium in the body which aggravates these health conditions. Sodium bicarbonate may also interfere with the effectiveness of other medications like iron supplements or aspirin. If sodium bicarbonate is only administered occasionally and other medications are used an hour or more later, there is rarely any trouble. Overall, baking soda as an antacid provides immediate and temporary relief to heartburn and indigestion, but should not be used in the case of daily symptoms which could indicate a more serious health condition. [17]

References

CAS N°: 144-55-8] Organisation for Economic Co-operation and Development (OECD). Screening Information Data Set (SIDS).