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Here we go again....
Chicken & bat guano is high in Nitrogen because of the Uric acid content, also high in phosphorus and ammonia.
I thought it was the Uric acid bit that was interesting because of the guano being excreted into the water jug...water that comes from the natural source that is also shown in these paintings.
You have to remember that Saint Anthony was a Desert Father in the Natron Valley/Wadi Natrum which has a Subaqueous anoxic environment like the Dead sea and the Red sea areas.The monastic community was formed in the second half of the 4th century in natural or man made caves....recent research shows that, most probably, the initial community was formed around a deserted massive defense tower, built by the Romans, to defend the salt and Natron production of the Wadi.
Saint Anthony decided to follow this tradition and headed out into the alkaline desert region called the Nitra in Latin (Wadi El Natrun today), about 95 km west of Alexandria, some of the most rugged terrain of the Western Desert. Here he remained for some thirteen years.
In the Old Testament rather than Natrum they use the word Neter which is also a common name for the abode of the dead. It means the "divine subterranean place"
Natron (Na2CO3, sodium bicarbonate) was an important material used for mummification, glassmaking, and to preserve food.Used in mummification because it absorbs water and behaves as a drying agent. Moreover, when exposed to moisture the carbonate in natron increases pH, which creates a hostile environment for bacteria. In some cultures natron was thought to enhance spiritual safety for both the living and the dead.
So we have an Alkaline mineral water mixed with a high Nitrate Uric acid....... more later must dash.
I think you mean sodium carbonate not sodium bicarbonate although I'm not very good at chemistry either.
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Sodium carbonate
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Sodium carbonate
other names[hide]Soda ash
Washing soda
Soda crystals
Identifiers
CAS number 497-19-8 Y,
5968-11-6 (monohydrate)
6132-02-1 (dechydrate)
PubChem 10340
ChemSpider ID 9916
EC number 207-838-8
RTECS number VZ4050000
Properties
Molecular formula Na2CO3
Molar mass 105.9884 g/mol (anhydrous)
124.00 g/mol (monohydrate)
286.14 g/mol (decahydrate)
Appearance White solid, hygroscopic
Density 2.54 g/cm3 (anhydrous)
2.25 g/cm3 (monohydrate)
1.46 g/cm3 (decahydrate)
Melting point 851 °C (anhydrous)
100 °C (decomp, monohydrate)
34 °C (decomp, decahydrate)
Boiling point 1600 °C (anhydrous)
Solubility in water 22 g/100 ml (20 °C)
Solubility insoluble in alcohol, ethanol
Basicity (pKb) 3.67
Refractive index (nD) 1.495 (anhydrous)
1.420 (monohydrate)
Structure
Coordination
geometry trigonal bipyramidal
Hazards
MSDS Safety Data Sheet External MSDS
EU Index 011-005-00-2
EU classification Irritant (Xi)
R-phrases R36
S-phrases (S2), S22, S26
NFPA 704 011
Flash point Non-flammable
Related compounds
Other anions Sodium bicarbonate
Other cations Lithium carbonate
Potassium carbonate
Rubidium carbonate
Caesium carbonate
Related compounds Ammonium carbonate
Natron
Sodium percarbonate
Y (what is this?) (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references
Sodium carbonate (also known as washing soda, soda crystals or soda ash), Na2CO3, is a sodium salt of carbonic acid. It most commonly occurs as a crystalline heptahydrate, which readily effloresces to form a white powder, the monohydrate; and is domestically well known for its everyday use as a water softener. It has a cooling alkaline taste, and can be extracted from the ashes of many plants. It is synthetically produced in large quantities from table salt in a process known as the Solvay process.
Contents [hide]
1 Uses
1.1 Other applications
2 Occurrence
3 Production
3.1 Mining
3.2 Barilla and kelp
3.3 Leblanc process
3.4 Solvay process
3.5 Hou's process
4 References
5 External links
[edit] Uses
The manufacture of glass is the most important use of sodium carbonate. When it is combined with sand (SiO2) and calcium carbonate (CaCO3) and heated to very high temperatures, then cooled very rapidly, glass is produced. This type of glass is known as soda lime glass.
Sodium carbonate is also used as a relatively strong base in various settings. For example, sodium carbonate is used as a pH regulator to maintain stable alkaline conditions necessary for the action of the majority of developing agents.[citation needed] It is a common additive in municipal pools used to neutralize the acidic effects of chlorine and raise pH.[1] In cooking, it is sometimes used in place of sodium hydroxide for lying, especially with German pretzels and lye rolls. These dishes are treated with a solution of an alkaline substance in order to change the pH of the surface of the food and thus improve browning.
In taxidermy, sodium carbonate added to boiling water will remove flesh from the skull or bones of trophies to create the "European skull mount" or for educational display in biological and historical studies.
In chemistry, it is often used as an electrolyte. This is because electrolytes are usually salt-based, and sodium carbonate acts as a very good conductor in the process of electrolysis. Additionally, unlike chloride ions which form chlorine gas, carbonate ions are not corrosive to the anodes. It is also used as a primary standard for acid-base titrations because it is solid and air-stable, making it easy to weigh accurately.
Electron Density of Na2CO3 computed with Ghemical/MPQC at the RHF 6-311G** level of theory.
Electrostatic potential of Na2CO3 computed with Ghemical/MPQC at the RHF 6-311G** level of theory.In domestic use, it is used as a water softener during laundry. It competes with the ions magnesium and calcium in hard water and prevents them from bonding with the detergent being used. Without using washing soda, additional detergent is needed to soak up the magnesium and calcium ions. Called Washing Soda, Soda crystals or Sal Soda[2] in the detergent section of stores, it effectively removes oil, grease, and alcohol stains. Sodium carbonate is also used as a descaling agent in boilers such as found in coffee pots, espresso machines, etc.[citation needed]
In dyeing with fiber-reactive dyes, sodium carbonate (often under a name such as soda ash fixative or soda ash activator) is used to ensure proper chemical bonding of the dye with the fibers, typically before dyeing (for tie dyes), mixed with the dye (for dye painting), or after dyeing (for immersion dyeing).[3]
[edit] Other applications
Sodium carbonate is a food additive (E500) used as an acidity regulator, anti-caking agent, raising agent and stabilizer. It is one of the components of kansui, a solution of alkaline salts used to give ramen noodles their characteristic flavor and texture.[4][5] Sodium carbonate is also used in the production of sherbet powder. The cooling and fizzing sensation results from the endothermic reaction between sodium carbonate and a weak acid, commonly citric acid, releasing carbon dioxide gas, which occurs when the sherbet is moistened by saliva.
As a food additive (E500), it is used in the production of snus (Swedish style snuff) to stabilize the pH of the final product. [6] In Sweden, snus is regulated as a food product because it is put into the mouth, requiring pasturization and only ingredents that are approved as food additives.
Sodium carbonate is used by the brick industry as a wetting agent to reduce the amount of water needed to extrude the clay.[citation needed]
In casting, it is referred to as "bonding agent" and is used to allow wet alginate to adhere to gelled alginate.[7]
Sodium carbonate is used in toothpastes, where it acts as a foaming agent, an abrasive, and to temporarily increase mouth pH.
Sodium carbonate may be used for safely cleaning silver. First, aluminium foil is added to a glass or ceramic container, and covered with very hot water and some sodium carbonate. Silver items are dipped into this "bath" to clean them, making sure the silver makes contact with the aluminium foil. Finally, the silver is rinsed in water and let to dry.[8]
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Main article: Solvay process
In 1861, the Belgian industrial chemist Ernest Solvay developed a method to convert sodium chloride to sodium carbonate using ammonia. The Solvay process centered around a large hollow tower. At the bottom, calcium carbonate (limestone) was heated to release carbon dioxide:
CaCO3 → CaO + CO2
At the top, a concentrated solution of sodium chloride and ammonia entered the tower. As the carbon dioxide bubbled up through it, sodium bicarbonate precipitated:
NaCl + NH3 + CO2 + H2O → NaHCO3 + NH4Cl
The sodium bicarbonate was then converted to sodium carbonate by heating it, releasing water and carbon dioxide:
2 NaHCO3 → Na2CO3 + H2O + CO2
Meanwhile, the ammonia was regenerated from the ammonium chloride byproduct by treating it with the lime (calcium hydroxide) left over from carbon dioxide generation:
CaO + H2O → Ca(OH)2
Ca(OH)2 + 2 NH4Cl → CaCl2 + 2 NH3 + 2 H2O
Because the Solvay process recycles its ammonia, it consumes only brine and limestone, and has calcium chloride as its only waste product. This made it substantially more economical than the Leblanc process, and it soon came to dominate world sodium carbonate production. By 1900, 90% of sodium carbonate was produced by the Solvay process, and the last Leblanc process plant closed in the early 1920s.
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Sodium bicarbonate
From Wikipedia, the free encyclopedia
Jump to: navigation, search
Sodium Bicarbonate
IUPAC name [hide]
Sodium hydrogen carbonate
Other names Sodium bicarbonate
Bicarbonate of soda
Baking soda
Sodium hydrogencarbonate
Nahcolite
Identifiers
CAS number 144-55-8 Y
PubChem 516892
ChemSpider ID 8609
RTECS number VZ0950000
Properties
Molecular formula CHNaO3
Molar mass 84.01 g mol−1
Appearance white crystalline solid
Odor odorless
Density 2.173 g/cm3
Melting point decomp: 323.15 K (50 °C) - 543.15 K (270 °C)
Solubility in water 7.8 g/100 mL (18 °C)
10 g/100 mL (20 °C)
Solubility insoluble in alcohol, ether
Acidity (pKa) 10.3
Refractive index (nD) 1.3344
Hazards
MSDS External MSDS
EU Index Not listed
NFPA 704 010
Flash point Non-flammable
LD50 4220 mg/kg
Related compounds
Other anions Sodium carbonate
Other cations Potassium bicarbonate
Ammonium bicarbonate
Related compounds Sodium bisulfate
Sodium hydrogen phosphate
Y (what is this?) (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references
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 can be used to experiment and is not very dangerous. 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 found in its dissolved form in bile, where it serves to neutralize the acidity of the hydrochloric acid produced by the stomach, and is excreted into the duodenum of the small intestine via the bile duct. 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, bicarb soda, or simply 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.
Contents [hide]
1 History
2 Production
3 Mining
4 Chemistry
4.1 Thermal decomposition
5 Applications
5.1 Cooking
5.2 Neutralization of acids and bases
5.3 Medical uses
5.4 Personal hygiene
5.5 Soda loading
5.6 As a cleaning agent
5.7 Miscellaneous
6 See also
7 References
8 Further reading
9 External links
[edit] 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, Nicolas Leblanc, produced sodium bicarbonate as we know it today. In 1846 two New York bakers, John Dwight and Austin Church, established the first factory to develop baking soda from sodium carbonate and carbon dioxide.[1]