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Borax

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(Redirected from Tincal)
For other uses, see Borax (disambiguation).
Not to be confused with Borex, Borox, or Borat.

Borax
Borax crystals
Ball-and-stick model of the unit cell of borax decahydrate
Names
IUPAC name
disodium;3,7-dioxido-2,4,6,8,9-pentaoxa-1,3,5,7-tetraborabicyclo[3.3.1]nonane;decahydrate[1]
Other names
  • Borax decahydrate
  • Sodium borate decahydrate
  • Sodium tetraborate decahydrate
  • Sodium tetrahydroxy tetraborate hexahydrate
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
EC Number
E number E285 (preservatives)
KEGG
RTECS number
  • VZ2275000
UNII
  • InChI=1S/B4O7.2Na.10H2O/c5-1-7-3-9-2(6)10-4(8-1)11-3;;;;;;;;;;;;/h;;;10*1H2/q-2;2*+1;;;;;;;;;;
    Key: CDMADVZSLOHIFP-UHFFFAOYSA-N
  • InChI=1/B4O7.2Na.10H2O/c5-1-7-3-9-2(6)10-4(8-1)11-3;;;;;;;;;;;;/h;;;10*1H2/q-2;2*+1;;;;;;;;;;
    Key: CDMADVZSLOHIFP-UHFFFAOYAP
  • [Na+].[Na+].O0B(O)O[B-]1(O)OB(O)O[B-]0(O)O1.O.O.O.O.O.O.O.O
Properties
Na2B4O5(OH)4·8H2O
Molar mass 381.36 g·mol−1
Appearance White or colorless crystalline solid
Density 1.73 g/cm3 (decahydrate, solid)[2]
Melting point 743 °C (1,369 °F; 1,016 K) (anhydrous)[2]
75 °C (decahydrate, decomposes)[2]
Boiling point 1,575 °C (2,867 °F; 1,848 K) (anhydrous)[2]
31.7 g/L [2]
−85.0·10−6 cm3/mol (anhydrous)[2]: p.4.135 
n1=1.447, n2=1.469, n3=1.472 (decahydrate)[2]: p.4.139 
Structure[3]
Monoclinic, mS92, No. 15
C2/c
2/m
a = 1.1885 nm, b = 1.0654 nm, c = 1.2206 nm
α = 90°, β = 106.623°°, γ = 90°
1.4810 nm3
4
Pharmacology
S01AX07 (WHO)
Hazards
GHS labelling:
GHS08: Health hazard
H360
P201, P308+P313
NFPA 704 (fire diamond)
[7]
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
NIOSH (US health exposure limits):
PEL (Permissible)
 none[4]
REL (Recommended)
 TWA 1 mg/m3 (anhydrous and pentahydrate)[4][5]
TWA 5 mg/m3 (decahydrate)[6]
IDLH (Immediate danger)
 N.D.[4]
Related compounds
Other anions
 Sodium aluminate
Other cations
 Lithium tetraborate
Related compounds
 Boric acid, sodium perborate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Borax (also referred to as sodium borate, tincal (/ˈtɪŋkəl/) and tincar (/ˈtɪŋkər/)) is a salt (ionic compound), a hydrated or anhydrous borate of sodium, with the chemical formula Na2H20B4O17.[1][a]

It is a colorless crystalline solid that dissolves in water to make a basic solution.

It is commonly available in powder or granular form and has many industrial and household uses, including as a pesticide, as a metal soldering flux, as a component of glass, enamel, and pottery glazes, for tanning of skins and hides, for artificial aging of wood, as a preservative against wood fungus, and as a pharmaceutic alkalizer. In chemical laboratories, it is used as a buffering agent.[1][8]

The terms tincal and tincar refer to native borax, historically mined from dry lake beds in various parts of Asia.[9]

History

[edit]

Borax was first discovered in dry lake beds in Tibet. Native tincal from Tibet, Persia, and other parts of Asia was traded via the Silk Road to the Arabian Peninsula in the 8th century AD.[9]

Borax first came into common use in the late 19th century when Francis Marion Smith's Pacific Coast Borax Company began to market and popularize a large variety of applications under the 20 Mule Team Borax trademark, named for the method by which borax was originally hauled out of the California and Nevada deserts.[10][11]

Etymology

[edit]

The English word borax is Latinized: the Middle English form was boras, from Old French boras, bourras.[12] That may have been from Medieval Latin baurach (another English spelling), borac(-/um/em), borax, along with Spanish borrax (> borraj) and Italian borrace, in the 9th century, and from Arabic bawraq, būraq, bōraq[12] (بورق)[13] as mentioned for example in Kitab al-Tabikh of Ibn Sayyar al-Warraq.[citation needed]

The words tincal and tincar were adopted into English in the 17th century from Malay tingkal and from Urdu/Persian/Arabic تنکار‎ tinkār/tankār; thus the two forms in English. These all appear to be related to the Sanskrit टांकण ṭānkaṇa.[14][15]

Chemistry

[edit]
The structure of borax according to X-ray crystallography.

From a chemical perspective, borax contains the [B4O5(OH)4]2− ion. In this structure, there are two four-coordinate boron centers and two three-coordinate boron centers.

It is a proton conductor at temperatures above 21 °C. Conductivity is maximum along the b-axis.[16]

Borax is also easily converted to boric acid and other borates, which have many applications. Its reaction with hydrochloric acid to form boric acid is:

Na2B4O7·10H2O + 2 HCl → 4 H3BO3 + 2 NaCl + 5 H2O

Borax is sufficiently stable to find use as a primary standard for acid-base titrimetry.[17]: p.316 

Molten borax dissolves many metal oxides to form glasses. This property is important for its uses in metallurgy and for the borax bead test of qualitative chemical analysis.

Borax is soluble in a variety of solvents; however, it is notably insoluble in ethanol.[1]

Solubility of borax in some solvents[18]
Organic solvent Temperature
°C (°F) 		Borax % by weight
in saturated solution
Glycerol 98.5% 20 (68) 52.60
Glycerol 86.5% 20 (68) 47.19
Ethylene glycol 25 (77) 41.60
Diethylene glycol 25 (77) 18.60
Methanol 25 (77) 19.90
Aqueous ethanol 46.5% 15.5 (60) 2.48
Acetone 25 (77) 0.60
Ethyl acetate 25 (77) 0.14
Solubility of borax in water[18]
Temperature
°C (°F) 		Borax % by weight in saturated solution
0 (32) 1.99
5 (41) 2.46
10 (50) 3.09
15 (59) 3.79
20 (68) 4.70
25 (77) 5.80
30 (86) 7.20
35 (95) 9.02
40 (104) 11.22
45 (113) 14.21
50 (122) 17.91
55 (131) 23.22
60 (140) 30.32
65 (149) 33.89
70 (158) 36.94
75 (167) 40.18
80 (176) 44.31
85 (185) 48.52
90 (194) 53.18
95 (203) 58.94
100 (212) 65.63

The term borax properly refers to the so-called "decahydrate" Na2B4O7·10H2O, but that name is not consistent with its structure. It is actually octahydrate. The anion is not tetraborate [B4O7]2− but tetrahydroxy tetraborate [B4O5(OH)4]2−,[16] so the more correct formula should be Na2B4O5(OH)4·8H2O. However, the term may be applied also to the related compounds. Borax "pentahydrate" has the formula Na2B4O7·5H2O, which is actually a trihydrate Na2B4O5(OH)4·3H2O. It is a colorless solid with a density of 1.880 kg/m3 that crystallizes from water solutions above 60.8 °C in the rhombohedral crystal system. It occurs naturally as the mineral tinkhanite.[19] It can be obtained by heating the "decahydrate" above 61 °C.[20] Borax "dihydrate" has the formula Na2B4O7·2H2O, which is actually anhydrous, with the correct formula Na2B4O5(OH)4. It can be obtained by heating the "decahydrate" or "pentahydrate" to above 116-120 °C.[20] Anhydrous borax is sodium tetraborate proper, with formula Na2B4O7. It can be obtained by heating any hydrate to 300 °C.[20] It has one amorphous (glassy) form and three crystalline forms – α, β, and γ, with melting points of 1015, 993 and 936 K respectively. α-Na2B4O7 is the stable form.[20]

Natural sources

[edit]
Main article: Borax (mineral)
Borax "cottonball"

Borax occurs naturally in evaporite deposits produced by the repeated evaporation of seasonal lakes. The most commercially important deposits are found in: Turkey; Boron, California; and Searles Lake, California. Also, borax has been found at many other locations in the Southwestern United States, the Atacama Desert in Chile, newly discovered deposits in Bolivia, and in Tibet and Romania. Borax can also be produced synthetically from other boron compounds.[21]

Naturally occurring borax (known by the trade name Rasorite–46 in the United States and many other countries) is refined by a process of recrystallization.[22]

Traction steam engine hauling borax, Death Valley National Park, California, 1904

Uses

[edit]
Borax-based laundry detergent

Borax is used in pest control solutions because it is toxic to ants and rats. Because it is slow-acting, worker ants will carry the borax to their nests and poison the rest of the colony.[23]

Borax is used in various household laundry and cleaning products,[24][25] including the 20 Mule Team Borax laundry booster, Boraxo powdered hand soap, and some tooth bleaching formulas.[26][27]

Borate ions (commonly supplied as boric acid) are used in biochemical and chemical laboratories to make buffers, e.g. for polyacrylamide gel electrophoresis of DNA and RNA, such as TBE buffer (borate buffered tris-hydroxymethylaminomethonium)[28][29] or the newer SB buffer or BBS buffer (borate buffered saline) in coating procedures. Borate buffers (usually at pH 8) are also used as preferential equilibration solutions in dimethyl pimelimidate (DMP) based crosslinking reactions.[citation needed]

Borax as a source of borate has been used to take advantage of the co-complexing ability of borate with other agents in water to form complex ions with various substances. Borate and a suitable polymer bed are used to chromatograph non-glycated hemoglobin differentially from glycated hemoglobin (chiefly HbA1c), which is an indicator of long-term hyperglycemia in diabetes mellitus.

Borax alone does not have a high affinity for hardness cations, although it has been used for water-softening. Its chemical equation for water-softening is given below:

Ca2+(aq) + Na2B4O7(aq) → CaB4O7(s)↓ + 2 Na+(aq)
Mg2+(aq) + Na2B4O7(aq) → MgB4O7(s)↓ + 2 Na+(aq)

The sodium ions introduced do not make water "hard". This method is suitable for removing both temporary and permanent types of hardness.

A mixture of borax and ammonium chloride is used as a flux when welding iron and steel. It lowers the melting point of the unwanted iron oxide (scale), allowing it to run off. Borax is also mixed with water as a flux when soldering jewelry metals such as gold or silver, where it allows the molten solder to wet the metal and flow evenly into the joint.[citation needed] Borax is also a good flux for "pre-tinning" tungsten with zinc, making the tungsten soft-solderable.[30] Borax is often used as a flux for forge welding.[31]

Old steam tractor with borax wagons, Death Valley National Park

In artisanal gold mining, borax is sometimes used as part of a process known as the borax method (as a flux) meant to eliminate the need for toxic mercury in the gold extraction process, although it cannot directly replace mercury. Borax was reportedly used by gold miners in parts of the Philippines in the 1900s.[32][33] There is evidence that, in addition to reducing the environmental impact, this method achieves better gold recovery for suitable ores and is less expensive. This borax method is used in northern Luzon in the Philippines, but miners have been reluctant to adopt it elsewhere for reasons that are not well understood.[34] The method has also been promoted in Bolivia[35] and Tanzania.[36]

A rubbery polymer sometimes called Slime, Flubber, 'gluep' or 'glurch' (or erroneously called Silly Putty, which is based on silicone polymers), can be made by cross-linking polyvinyl alcohol with borax. Making flubber from polyvinyl acetate-based glues, such as Elmer's Glue, and borax is a common elementary science demonstration.[37][38]

Borax, given the E number E285, is used as a food additive but this use is banned in some countries, such as Australia, China, Thailand and the United States.[39] As a consequence, certain foods, such as caviar, produced for sale in the United States contain higher levels of salt to assist preservation.[40] In addition to its use as a preservative, borax imparts a firm, rubbery texture to food. In China, borax (Chinese: 硼砂; pinyin: péng shā or Chinese: 月石; pinyin: yuè shí) has been found in foods including wheat and rice noodles named lamian (Chinese: 拉面; pinyin: lāmiàn), shahe fen (Chinese: 沙河粉; pinyin: shāhéfěn), char kway teow (Chinese: 粿條; pinyin: guǒ tiáo), and chee cheong fun (Chinese: 肠粉; pinyin: chángfěn)[clarification needed][41] In Indonesia, it is a common, but forbidden,[42] additive to such foods as noodles, bakso (meatballs), and steamed rice. When consumed with boric acid, numerous studies have demonstrated a negative[clarification needed] association between borax and various types of cancers.[43] Boric acid and borax are low in toxicity for acute oral exposures, at approximately the same acute toxicity as salt. The average dose for asymptomatic ingestion cases, which accounts for 88% of all ingestions, is around 0.9 grams. However, the range of reported asymptomatic doses is wide, from 0.01 to 88.8 g.[44]

Rio Tinto borax mine pit, Boron, California

Other uses include:

Toxicity

[edit]

According to one study, borax is not acutely toxic. Its LD50 (median lethal dose) score is tested at 2.66 g/kg in rats, meaning that a significant dose of the chemical is needed to cause severe symptoms or death. The lethal dose is not necessarily the same for humans. On pesticide information websites it is listed as a non-lethal compound and of no hazardous concerns.[citation needed]

Borax has been in use as an insecticide in the United States with various restrictions since 1946. All restrictions were removed in February 1986 due to the low toxicity of borax, as reported in two EPA documents relating to boric acid and borax.[63][64]

EPA has determined that, because they are of low toxicity and occur naturally, boric acid and its sodium salts should be exempted from the requirement of a tolerance (maximum residue limit) for all raw agricultural commodities.[63]

Although it cited inconclusive data, a re-evaluation in 2006 by the EPA still found that "There were no signs of toxicity observed during the study and no evidence of cytotoxicity to the target organ."[65] In the reevaluation, a study of toxicity due to overexposure was checked and the findings were that "The residential handler inhalation risks due to boric acid and its sodium salts as active ingredients are not a risk concern and do not exceed the level of concern..." but that there could be some risk of irritation to children inhaling it if used as a powder for cleaning rugs.

Overexposure to borax dust can cause respiratory irritation, while no skin irritation is known to exist due to external borax exposure. Ingestion may cause gastrointestinal distress including nausea, persistent vomiting, abdominal pain, and diarrhea. Effects on the vascular system and human brain include headaches and lethargy but are less frequent. In severe cases, a "beefy" red rash affecting the palms, soles, buttocks and scrotum has occurred.[66]

The Indonesian Directorate of Consumer Protection warns of the risk of liver cancer with high consumption of borax over a period of 5–10 years.[60]

Borax was added to the Substance of Very High Concern (SVHC) candidate list on December 16, 2010. The SVHC candidate list is part of the EU Regulations on the Registration, Evaluation, Authorisation and Restriction of Chemicals 2006 (REACH), and the addition was based on the revised classification of borax as toxic for reproduction category 1B under the CLP Regulations. Substances and mixtures imported into the EU which contain borax are now required to be labelled with the warnings "May damage fertility" and "May damage the unborn child".[67] It was proposed for addition to REACH Annex XIV by the ECHA on July 1, 2015.[68] If this recommendation is approved, all imports and uses of borax in the EU will have to be authorized by the ECHA.[needs update]

A review of the boron toxicity (as boric acid and borates) published in 2012 in the Journal of Toxicology and Environmental Health concluded: "It clearly appears that human B [boron] exposures, even in the highest exposed cohorts, are too low to reach the blood (and target tissue) concentrations that would be required to exert adverse effects on reproductive functions."[69] A draft risk assessment released by Health Canada in July 2016 has found that overexposure to boric acid has the potential to cause developmental and reproductive health effects. Since people are already exposed to boric acid naturally through their diets and water, Health Canada advised that exposure from other sources should be reduced as much as possible, especially for children and pregnant women.

The concern is not with any one product, but rather multiple exposures from a variety of sources. With this in mind, the department also announced that certain pesticides that contain boric acid, which are commonly used in homes, will have their registrations cancelled and be phased out of the marketplace. As well, new, more protective label directions are being introduced for other boric acid pesticides that continue to be registered in Canada (for example, enclosed bait stations and spot treatments using gel formulations).[70]

See also

[edit]

Explanatory footnotes

[edit]
  1. ^ It is also written as Na2B4O7·10H2O, which shows that it is a decahydrated tetraborate.

References

[edit]
  1. ^ a b c d e PubChem. "Borax". pubchem.ncbi.nlm.nih.gov. Retrieved December 27, 2021.
  2. ^ a b c d e f g Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. ISBN 978-1439855119.
  3. ^ Levy, H. A.; Lisensky, G. C. (1978). "Crystal structures of sodium sulfate decahydrate (Glauber's salt) and sodium tetraborate decahydrate (borax). Redetermination by neutron diffraction". Acta Crystallographica Section B. 34 (12): 3502–3510. Bibcode:1978AcCrB..34.3502L. doi:10.1107/S0567740878011504.
  4. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0057". National Institute for Occupational Safety and Health (NIOSH).
  5. ^ NIOSH Pocket Guide to Chemical Hazards. "#0059". National Institute for Occupational Safety and Health (NIOSH).
  6. ^ NIOSH Pocket Guide to Chemical Hazards. "#0058". National Institute for Occupational Safety and Health (NIOSH).
  7. ^ "Potential Commodities NFPA 704" (PDF). Archived from the original (PDF) on May 17, 2016. Retrieved December 9, 2018.
  8. ^ "CompTox Chemicals Dashboard". comptox.epa.gov. Retrieved January 1, 2022.
  9. ^ a b "Borax (Na2B4O7·10H2O ) – Sodium Borate – Occurrence, Discovery and Applications". Amoz.com. August 16, 2004.
  10. ^ "American Borax Production". Scientific American. Vol. 37, no. 12. September 22, 1877. pp. 184–185. JSTOR 26062263.. The article states that the distance between Columbus, Nevada and Wadsworth, Nevada is "about 360 miles" whereas today the distance on modern roads is about 160 miles.
  11. ^ Hildebrand, G. H. (1982). Borax Pioneer: Francis Marion Smith. San Diego: Howell-North Books. p. 267. ISBN 0-8310-7148-6.
  12. ^ a b "borax". Oxford English Dictionary (Online ed.). Oxford University Press. (Subscription or participating institution membership required.)
  13. ^ Wehr, Hans (1979). "بورق". In Cowan, J. Milton (ed.). A Dictionary of Modern Written Arabic (4th ed.). Ithaca, NY: Spoken Language Services. p. 100. ISBN 0-87950-003-4.
  14. ^ "Tincal". Oxford English Dictionary (Online ed.). Oxford University Press. (Subscription or participating institution membership required.)
  15. ^ Chemical Age of India, Vol. 37, No.10 & 11 (1976)[full citation needed]
  16. ^ a b Maričić, S.; Pravdić, V.; Veksli, Z. (November 1962). "Proton conductivity in borax, Na2[B4O5(OH)4]-8H2O". Journal of Physics and Chemistry of Solids. 23 (11): 1651–1659. Bibcode:1962JPCS...23.1651M. doi:10.1016/0022-3697(62)90248-2.
  17. ^ Mendham, J.; Denney, R. C.; Barnes, J. D.; Thomas, M. J. K. (2000), Vogel's Quantitative Chemical Analysis (6th ed.), New York: Prentice Hall, ISBN 0-582-22628-7
  18. ^ a b Borax decahydrate. borax.com
  19. ^ Akgül, Mehmet; Çamlıbel, Osman (March 2021). "The use of borax pentahydrate of inorganic filler in medium density fiberboard production". Maderas. Ciencia y tecnología. 23. doi:10.4067/S0718-221X2021000100422. ISSN 0718-221X.
  20. ^ a b c d Şahin, Ömer; Bulutcu, A. Nusret (2002). "Dehydration Behaviour of Borax Pentahydrate to Anhydrous Borax by Multi-Stage Heating in a Fluidized". Turkish Journal of Chemistry. 26 10: 89–96.
  21. ^ "Borax - The Chemical Company". thechemco.com. Retrieved April 8, 2024.
  22. ^ Wizniak, Jaime (July 2005). "Borax, Boric Acid, and Boron – From exotic to commodity" (PDF). Indian Journal of Chemical Technology. 12 (4). ISSN 0975-0991.
  23. ^ Klotz, John H.; Greenberg, Les; Amrhein, Christopher; Rust, Michael K. (August 1, 2000). "Toxicity and Repellency of Borate-Sucrose Water Baits to Argentine Ants (Hymenoptera: Formicidae)". Journal of Economic Entomology. 93 (4): 1256–1258. doi:10.1603/0022-0493-93.4.1256. PMID 10985039. S2CID 17829851.
  24. ^ Sodium borate decahydrate (borax) in the Consumer Product Information Database
  25. ^ "The Many, Many Uses of Borax for Laundry". U.S. Borax. Retrieved June 13, 2022.
  26. ^ Hammond, C. R. (2004). The Elements, in Handbook of Chemistry and Physics 81st edition. CRC press. ISBN 978-0-8493-0485-9.
  27. ^ O'Neil, M.J., ed. (2013). The Merck Index — An Encyclopedia of Chemicals, Drugs, and Biologicals. Cambridge, UK: Royal Society of Chemistry. p. 1595. {{cite encyclopedia}}: Missing or empty |title= (help)
  28. ^ Peacock, Andrew C.; Dingman, C. Wesley (1967). "Resolution of Multiple Ribonucleic Acid Species by Polyacrylamide Gel Electrophoresis". Biochemistry. 6 (6): 1818–1827. doi:10.1021/bi00858a033. PMID 6035921.
  29. ^ Anderson, S. (1981). "Shotgun DNA sequencing using cloned DNase I-generated fragments". Nucleic Acids Research. 9 (13): 3015–27. doi:10.1093/nar/9.13.3015. PMC 327328. PMID 6269069.
  30. ^ Dodd, J.G. (1966). "Soft soldering to tungsten wire". Am. J. Phys. 34 (10): xvi. Bibcode:1966AmJPh..34D..16D. doi:10.1119/1.1972398.
  31. ^ a b Moehring, Jack; Willman, Michael; Pulscher, Isaac; Rowe, Devin (December 2016). "Bladesmithing at South Dakota School of Mines and Technology". JOM. 68 (12): 3186–3192. Bibcode:2016JOM....68l3186M. doi:10.1007/s11837-016-2139-z. ISSN 1047-4838. S2CID 137747858.
  32. ^ "March 2012 ipad ewaste Filipino Borax, Pakistans Pollution, Artisanal Gold Mining". Blacksmithinstitute.org. Archived from the original on October 13, 2016. Retrieved August 7, 2016.
  33. ^ "The borax method" (PDF). Borax replacing mercury in small-scale mining. The Geological Survey of Denmark and Greenland (GEUS). Archived from the original (PDF) on December 6, 2008. Retrieved August 2, 2008.
  34. ^ Appel, Peter W.U.; Na-Oy, Leoncio (June 1, 2012). "The Borax Method of Gold Extraction for Small-Scale Miners". Journal of Health and Pollution. 2 (3): 5–10. doi:10.5696/2156-9614-2.3.5.
  35. ^ Appel, Peter W. U.; Andersen, Astrid; Na-Oy, Leoncio D.; Onos, Rudy (December 1, 2015). "Introduction of Mercury-free Gold Extraction Methods to Medium-Scale Miners and Education of Health Care Providers to Reduce the use of Mercury in Sorata, Bolivia". Journal of Health and Pollution. 5 (9): 12–17. doi:10.5696/2156-9614-5-9.12. PMC 6221499. PMID 30524772.
  36. ^ Appel, Peter W.U.; Jønsson, Jesper Bosse (December 31, 1969). "Borax – an alternative to mercury for gold extraction by small-scale miners: introducing the method in Tanzania". Geological Survey of Denmark and Greenland (GEUS) Bulletin. 20: 87–90. doi:10.34194/geusb.v20.4988.
  37. ^ Parratore, Phil (1998). Wacky Science: A Cookbook for Elementary Teachers. Dubuque, IA: Kendall Hunt. p. 26. ISBN 978-0-7872-2741-8.
  38. ^ "Slime Recipe — How to Make Borax and White Glue Slime". Chemistry.about.com. Archived from the original on August 26, 2007. Retrieved August 7, 2016.
  39. ^ Reiley, Laura (April 22, 2019). "After China turned it into a cheap snack, caviar is at risk of losing its status as a luxury good". The Washington Post. Retrieved April 22, 2019.
  40. ^ "Caviar glossary". The Caviar Guide a gourmet review of caviars & fish roe. Hanson Ltd, Geneva, Switzerland. Archived from the original on December 8, 2008. Retrieved July 7, 2008.
  41. ^ "Chinese Ingredients: Borax Powder, Mushroom Extract". Chowhound.chow.com. September 11, 2005. Archived from the original on July 6, 2015. Retrieved August 7, 2016.
  42. ^ "BAHAN BERBAHAYA YANG DILARANG UNTUK PANGAN". www.pom.go.id. Archived from the original on June 26, 2021. Retrieved June 26, 2021.
  43. ^ Wu, Lun; Wei, Ying; Zhou, Wen-Bo; Zhang, You-Shun; Chen, Qin-Hua; Liu, Ming-Xing; Zhu, Zheng-Peng; Zhou, Jiao; Yang, Li-Hua; Wang, Hong-Mei; Wei, Guang-Min; Wang, Sheng; Tang, Zhi-Gang (July 1, 2019). "Gene expression alterations of human liver cancer cells following borax exposure". Oncology Reports. 42 (1): 115–130. doi:10.3892/or.2019.7169. ISSN 1021-335X. PMC 6549072. PMID 31180554.
  44. ^ "Boric Acid Technical Fact Sheet". npic.orst.edu. Retrieved December 13, 2022.
  45. ^ "Alphabetical information on pottery glaze making materials and clay body ingredients". Sheffield Pottery. Retrieved December 4, 2019.
  46. ^ a b Schubert, David M. (2003). "Borates in Industrial Use". In Roesky, Herbert W.; Atwood, David A. (eds.). Group 13 Chemistry III: Industrial Applications. Structure and Bonding 105. Vol. 105. Berlin: Springer Berlin Heidelberg. pp. 1–40. doi:10.1007/3-540-46110-8_1. ISBN 978-3-540-46110-4. OCLC 262687393.
  47. ^ Shen, Kelvin K.; O’Connor, Roderick (1998), Pritchard, Geoffrey (ed.), "Flame retardants: Borates", Plastics Additives: An A-Z reference, Polymer Science and Technology Series, vol. 1, Springer Netherlands, pp. 268–276, doi:10.1007/978-94-011-5862-6_30, ISBN 978-94-011-5862-6
  48. ^ "Centre for Alternative Technology". Cat.org.uk. Archived from the original on August 1, 2012. Retrieved August 7, 2016.
  49. ^ Murray, Lynda M. (1989). "Least toxic pest control: how infestations of termites, ants, fleas, ticks, and beetles can be controlled without causing short- or long-term indoor air quality changes and health risks" (PDF). nepis.epa.gov. United States Environmental Protection Agency. Archived from the original (PDF) on June 26, 2022. Retrieved June 25, 2022.
  50. ^ Suárez, Juan C. (2011), "Bioadhesives", in da Silva, Lucas F. M.; Öchsner, Andreas; Adams, Robert D. (eds.), Handbook of Adhesion Technology, Springer Berlin Heidelberg, pp. 1385–1408, doi:10.1007/978-3-642-01169-6_53, ISBN 978-3-642-01168-9
  51. ^ "Curing eggs for steelhead, steelhead egg cures, Buzz Ramsey, Bill Swann, Andy Martin". wildriversfishing.com. Retrieved April 16, 2021.
  52. ^ [1], "Buffer System for Swimming Pools and Related Structures", issued 2008-11-17 
  53. ^ "Development of Boron-based materials for nuclear applications" (PDF). Archived (PDF) from the original on September 22, 2010.
  54. ^ "Borax". Nature.berkeley.edu. Retrieved August 7, 2016.
  55. ^ "Boron Basics". www.spectrumanalytic.com.
  56. ^ "Learning Taxidermy Fish". Taxidermy Hobbyist | The Art Of Taxidermy. March 17, 2011. Retrieved April 16, 2021.
  57. ^ Marie, Anne. "How To Color Fire – Fun Fireplace Instructions". Chemistry.about.com. Archived from the original on October 21, 2016. Retrieved August 7, 2016.
  58. ^ Nicholls, Walter (November 10, 1991). "THE CUSTOM OF THE COUNTRY HAM". The Washington Post.
  59. ^ "Report of the State Board of Health of the State of New Hampshire ..., Volume 19". 1906. pp. 169–171.
  60. ^ a b "Watch Out For The Food We Consume". Directorate of Consumer Protection, Jakarta, Indonesia. 2006. Archived from the original on December 28, 2008. Retrieved February 10, 2009.
  61. ^ Lattes, C.M.G.; Fowler, R.H.; Cuer, R. (1947). "Range-Energy Relation for Protons and a-Particles in the New Ilford 'Nuclear Research' Emulsions". Nature. 159: 301–302. doi:10.1038/159301a0.
  62. ^ Lattes, C.M.G.; Occhialini, G.P.S. (1947). "Determination of the Energy and Momentum of Fast Neutrons in Cosmic Rays". Nature. 159 (4036): 331–332. Bibcode:1947Natur.159..331L. doi:10.1038/159331a0. PMID 20293532.
  63. ^ a b "Pesticide Reregistration Status" (PDF). Epa.gov. Retrieved August 7, 2016.
  64. ^ "Pesticides" (PDF). Epa.gov. August 20, 2015. Retrieved August 7, 2016.
  65. ^ "Regulations.gov". Archived from the original on May 3, 2015. Retrieved April 27, 2015.
  66. ^ Reigart, J. Routt (2009). Recognition and Management of Pesticide Poisonings (5th Ed. ). DIANE Publishing. p. 76. ISBN 978-1-4379-1452-8. Retrieved June 4, 2020.
  67. ^ Member state committee draft support document for identification of disodium tetraborate, anhydrous as a substance of very high concern because of its CMR properties. Adopted on June 9, 2010. Echa.europa.eu. Retrieved on February 17, 2012.
  68. ^ Recommendation of the European Chemicals Agency of 1 July 2015 for the inclusion of substances in Annex XIV to REACH (List of Substances subject to Authorisation) Archived July 14, 2015, at the Wayback Machine Echa.europa.eu. Retrieved on July 6, 2015.
  69. ^ Bolt, Hermann M.; Başaran, Nurşen; Duydu, Yalçın (2012). "Human Environmental and Occupational Exposures to Boric Acid: Reconciliation with Experimental Reproductive Toxicity Data". Journal of Toxicology and Environmental Health, Part A. 75 (8–10): 508–514. Bibcode:2012JTEHA..75..508B. doi:10.1080/15287394.2012.675301. PMID 22686310. S2CID 31972554.
  70. ^ "Information Update – Health Canada advises Canadians to avoid homemade craft and pesticide recipes using boric acid – Recalls & alerts". Healthycanadians.gc.ca. July 22, 2016. Retrieved August 7, 2016.
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