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Sodium bicarbonate
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Sodium bicarbonate
Names
IUPAC name
Sodium hydrogen carbonate
Other names
Baking soda, bicarb (laboratory slang), bicarbonate of soda, nahcolite
Identifiers
CAS Number
144-55-8 Y
3D model (JSmol)
Interactive image
Beilstein Reference
4153970
ChEBI
CHEBI:32139 Y
ChemSpider
8609 Y
DrugBank
DB01390 Y
ECHA InfoCard 100.005.122
EC Number 205-633-8
IUPHAR/BPS
4507
KEGG
C12603 Y
MeSH Sodium+bicarbonate
PubChem CID
516892
RTECS number VZ0950000
UNII
8MDF5V39QO Y
InChI[show]
InChI=1S/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1 Y
Key: UIIMBOGNXHQVGW-UHFFFAOYSA-M Y
InChI=1/CH2O3.Na/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1
Key: UIIMBOGNXHQVGW-REWHXWOFAQ
SMILES[show]
[Na+].OC([O-])=O
Properties
Chemical formula
NaHCO
3
Molar mass 84.0066 g mol−1
Appearance White crystals
Odor Odorless
Density
2.20 g/cm3 as solid[1]
1.1 to 1.3 as powder[2]
Melting point (Decomposes to sodium carbonate starting at 50 °C[7])
Solubility in water
69 g/L (0 °C)[3]
96 g/L (20 °C)[4]
165 g/L (60 °C)[4]
236 g/L (100 °C)[3]
Solubility 0.02 wt% acetone, 2.13 wt% methanol @22 °C.[5] insoluble in ethanol
log P −0.82
Acidity (pKa)
10.329[6]
6.351 (carbonic acid)[6]
Refractive index (nD)
nα = 1.377 nβ = 1.501 nγ = 1.583
Structure
Crystal structure
Monoclinic
Thermochemistry
Specific
heat capacity (C)
87.61 J/mol K
Std molar
entropy (So298)
102 J/mol K
Std enthalpy of
formation (ΔfHo298)
−947.7 kJ/mol
Gibbs free energy (ΔfG˚)
−851.9 kJ/mol
Pharmacology
ATC code
B05CB04 (WHO) B05XA02 (WHO), QG04BQ01 (WHO)
Routes of
administration
Intravenous, oral
Hazards
Main hazards Causes serious eye irritation
Safety data sheet External MSDS
NFPA 704
0
0
1
Flash point Incombustible
Lethal dose or concentration (LD, LC):
LD50 (median dose)
4220 mg/kg (rat, oral)[8]
Related compounds
Other anions
Sodium carbonate
Other cations
Ammonium bicarbonate
Potassium bicarbonate
Related compounds
Sodium bisulfate
Sodium hydrogen phosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y verify (what is Y N ?)
Infobox references
Sodium bicarbonate (IUPAC name: sodium hydrogen carbonate) is a chemical compound with the formula NaHCO3. It is a salt composed of sodium ions and bicarbonate ions. Sodium bicarbonate is a white solid that is crystalline but often appears as a fine powder. It has a slightly salty, alkaline taste resembling that of washing soda (sodium carbonate). The natural mineral form is nahcolite. It is a component of the mineral natron and is found dissolved in many mineral springs. It is among the food additives encoded by the European Union, identified as E 500.
Contents
[hide]
1 Nomenclature
2 Uses
2.1 Cooking
2.1.1 Baking powder
2.2 Pest control
2.3 Alkalinity/pH increase
2.4 Pyrotechnics
2.5 Mild disinfectant
2.6 Fire extinguisher
2.7 Neutralization of acids and bases
2.8 Medical uses and health
2.8.1 Personal hygiene
2.8.2 Veterinary uses
2.9 In sports
2.10 Cleaning agent
3 Chemistry
3.1 Thermal decomposition
4 History
5 Production
5.1 Mining
6 In popular culture
6.1 Film
7 See also
8 References
9 External links
Nomenclature[edit]
Since it has long been known and is widely used, the salt has many related names such as baking soda, bread soda, cooking soda, and bicarbonate of soda. In colloquial usage, the names sodium bicarbonate and bicarbonate of soda are often truncated; forms such as sodium bicarb, bicarb soda, bicarbonate, and bicarb are common. 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 prefix, bi, in bicarbonate comes from an outdated naming system and is based on the observation that there is twice as much carbonate (CO3) per sodium in sodium bicarbonate (NaHCO3) as there is carbonate per sodium in sodium carbonate (Na2CO3) and other carbonates. Modern analyse is based on the exact chemical composition (which was unknown when the name sodium bicarbonate was coined) says this the other way around: there is half as much sodium in NaHCO3 as in Na2CO3 (Na versus Na2).
Uses[edit]
Sodium bicarbonate has a wide variety of uses.
Cooking[edit]
Main article: Leavening agent
In cooking, sodium bicarbonate, referred to as baking soda, is primarily used in baking as a leavening agent. It reacts with acidic components in 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 other baked and fried foods. Acidic compounds that induce this reaction include phosphates, cream of tartar, lemon juice, yogurt, buttermilk, cocoa and vinegar. Baking soda may be used together with sourdough, which is acidic, making a lighter product with a less acid taste.[9]
Heat can also by itself cause sodium bicarbonate to act as a raising agent in baking because of thermal decomposition, releasing carbon dioxide. When used this way on its own, without the presence of an acidic component (whether in the batter or by the use of a baking powder containing acid), only half the available CO2 is released. Additionally, in the absence of acid, thermal decomposition of sodium bicarbonate also produces sodium carbonate, which is strongly alkaline and gives the baked product a bitter, "soapy" taste and a yellow color. To avoid an over-acidic taste from added acid, non-acid ingredients such as whole milk or Dutch-processed cocoa are often added to baked foods.[10]
Carbon dioxide production from exposure to heat starts at temperatures above 80 °C.[11]
2 NaHCO3 → Na2CO3 + H2O + CO2
Since the reaction occurs slowly at room temperature, mixtures (cake batter, etc.) can be allowed to stand without rising until they are heated in the oven.
Sodium bicarbonate was sometimes used in cooking green vegetables, as it gives them a bright green colour—which has been described as artificial-looking—due to its reacting with chlorophyll to produce chlorophyllin.[12] However, this tends to affect taste, texture and nutritional content, and is no longer common.[13] Baking soda is still used, though, in the traditional British mushy peas recipe for soaking the peas. It is also used in Asian and Latin American cuisine to tenderize meats. Baking soda may react with acids in food, including vitamin C (L-ascorbic acid). It is also used in breading such as for fried foods to enhance crispness and allow passages for steam to escape, so the breading is not blown off during cooking.
Baking powder[edit]
"Baking powder" is also sold for cooking; it contains around 30% of HCO3 and various acidic ingredients which are activated by the addition of water, without the need for additional acids in the cooking medium.[14][15][16]
Many forms of baking powder contain sodium bicarbonate combined with calcium acid phosphate, sodium aluminium phosphate or cream of tartar.[17] Baking soda is alkaline; the acid used in baking powder avoids a metallic taste when the chemical change during baking creates sodium carbonate.
Pest control[edit]
Sodium bicarbonate can be used to kill cockroaches. Once consumed, it causes internal organs of cockroaches to burst due to gas collection.[18]
Sodium bicarbonate can be an effective way of controlling fungal growth,[19] and in the United States is registered by the Environmental Protection Agency as a biopesticide.[20]
Alkalinity/pH increase[edit]
Sodium bicarbonate can be administered to pools, spas, and garden ponds to raise the total alkalinity. This will also raise the pH level and make maintaining proper pH easier. In the event that the pH is low and the alkalinity is adequate or high, sodium bicarbonate should not be used to adjust the pH.[21]
Pyrotechnics[edit]
Sodium bicarbonate is one of the main components of the common "black snake" firework. The effect is caused by the thermal decomposition, which produces carbon dioxide gas to produce a long snake-like ash as a combustion product of the other main component, sucrose.
Mild disinfectant[edit]
It has weak disinfectant properties,[22][23] and it may be an effective fungicide against some organisms.[24] Because baking soda will absorb musty smells, it has become a reliable method for used-book sellers when making books less malodorous.[25]
Fire extinguisher[edit]
Sodium bicarbonate can be used to extinguish small grease or electrical fires by being thrown over the fire, as heating of sodium bicarbonate releases carbon dioxide.[26] However, it should not be applied to fires in deep fryers; the sudden release of gas may cause the grease to splatter.[26] Sodium bicarbonate is used in BC dry chemical fire extinguishers as an alternative to the more corrosive diammonium phosphate in ABC extinguishers. The alkaline nature of sodium bicarbonate makes it the only dry chemical agent, besides Purple-K, that was used in large-scale fire suppression systems installed in commercial kitchens. Because it can act as an alkali, the agent has a mild saponification effect on hot grease, which forms a smothering, soapy foam.
Neutralization of acids and bases[edit]
Sodium bicarbonate is amphoteric, reacting with acids and bases. It reacts violently with acids, releasing CO2 gas as a reaction product. It is commonly used to neutralize unwanted acid solutions or acid spills in chemical laboratories.
Medical uses and health[edit]
See also: Intravenous sodium bicarbonate
Sodium bicarbonate mixed with water can be used as an antacid to treat acid indigestion and heartburn.[27] Its reaction with stomach acid produces salt, water, and carbon dioxide:
NaHCO3 + HCl → NaCl + H2O + CO2(g)
Intravenous sodium bicarbonate is an aqueous solution that is sometimes used for cases of acidosis, or when insufficient sodium or bicarbonate ions are in the blood.[28] In cases of respiratory acidosis, the infused bicarbonate ion drives the carbonic acid/bicarbonate buffer of plasma to the left and, thus, raises the pH. It is for this reason that sodium bicarbonate is used in medically supervised cardiopulmonary resuscitation. Infusion of bicarbonate is indicated only when the blood pH is markedly (<7.1–7.0) low.[29]
HCO3 is used for treatment of hyperkalemia, as it will drive K+ back into cells during periods of acidosis.[30] Since sodium bicarbonate 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 in the case of an overdose.[31] Sodium bicarbonate has also been used in the treatment of tricyclic antidepressant overdose.[32] It can also be applied topically as a paste, with three parts baking soda to one part water, to relieve some kinds of insect bites and stings (as well as accompanying swelling).[33]
Sodium bicarbonate has been found to have no effect on the blood pressure of several types of rat models susceptible to salt-sensitive hypertension, in contrast with sodium chloride. This was ascribed to the high concentration of chloride, rather than the sodium content in dietary salts.[34]
Sodium bicarbonate can be used to treat an allergic reaction to plants such as poison ivy, poison oak, or poison sumac to relieve some of the associated itching.[35][better source needed]
Bicarbonate of soda can also be useful in removing splinters from the skin.[36]
Some alternative practitioners, such as Tullio Simoncini, have promoted baking soda as a cancer cure, which the American Cancer Society has warned against due to both its unproven effectiveness and potential danger in use.[37]
Sodium bicarbonate can be added to local anaesthetics, to speed up the onset of their effects and make their injection less painful.[38] It is also a component of Moffett's solution, used in nasal surgery.
It was discovered as early as the 1920s that bicarbonate caused increase in bone strength in patients who were losing calcium in their urine. In 1968 it was suggested that diets producing too much acid might put bones at risk.[39] Experiments by Anthony Sebastian of the University of California, San Francisco starting in the late twentieth century found that the body was breaking down bones and muscles to release carbonates, phosphates and ammonia, which neutralize acid. Adding bicarbonate to the diet (he used potassium bicarbonate) reduced loss of calcium in post-menopausal women, amounting to the equivalent of "an arm-and-a-leg's worth" of bone if this continued for two decades.
A wide variety of applications follows from its neutralization properties, including reducing the spread of white phosphorus from incendiary bullets inside an afflicted soldier's wounds.[40][medical citation needed]
Antacid (such as baking soda) solutions have been prepared and used by protesters to alleviate the effects of exposure to tear gas during protests.[41][not in citation given][42][dead link]
Personal hygiene[edit]
Toothpaste containing sodium bicarbonate has in several studies been shown to have a better whitening[43][43][44][45] and plaque removal effect[46][47] than toothpastes without it.
Sodium bicarbonate is also used as an ingredient in some mouthwashes. It has anticaries and abrasive properties.[48] 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.[citation needed]
Sodium bicarbonate in combination with other ingredients can be used to make a dry or wet deodorant.[49][50]
Sodium bicarbonate may be used as a buffering agent, combined with table salt, when creating a solution for nasal irrigation.[51]
It is used in eye hygiene to treat blepharitis. This is done by addition of a teaspoon of sodium bicarbonate to cool water that was recently boiled, followed by gentle scrubbing of the eyelash base with a cotton swab dipped in the solution.[52]
Veterinary uses[edit]
Sodium bicarbonate is used as a cattle feed supplement, in particular as a buffering agent for the rumen.[53]
In sports[edit]
Small amounts of sodium bicarbonate have been shown to be useful as a supplement for athletes in speed-based events, such as middle-distance running, lasting from about one to seven minutes.[54][55] However, overdose is a serious risk because sodium bicarbonate is slightly toxic;[56][dead link] and gastrointestinal irritation is of particular concern.[55] Additionally, this practice causes a significant increase in dietary sodium.
Cleaning agent[edit]
Sodium bicarbonate is used in a process for removing paint and corrosion called sodablasting; the process is particularly suitable for cleaning aluminium panels which can be distorted by other types of abrasives.
A paste made from baking soda with minimal water is recommended by a manufacturer as a gentle scouring powder,[26] and is useful in removing surface rust, as the rust forms a water-soluble compound when in a concentrated alkaline solution;[57] cold water should be used, as hot water solutions can corrode steel. [58] Sodium bicarbonate attacks the thin unreactive protective oxide layer that forms on aluminium, making it unsuitable for cleaning this otherwise very reactive metal.[59] A solution in warm water will remove the tarnish from silver when the silver is in contact with a piece of aluminium foil.[59][60] Baking soda is commonly added to washing machines as a replacement for water-softener and to remove odors from clothes. Sodium bicarbonate is also effective in removing heavy tea and coffee stains from cups when diluted with warm water. Also, baking soda can be used as a multi purpose odor remover.[61]
During the Manhattan Project to develop the nuclear bomb in the early 1940s the chemical toxicity of uranium was an issue. It was found that uranium oxides stick very well to cotton cloth, and did not wash out with soap or laundry detergent. However, the uranium would wash out with a 2% solution of sodium bicarbonate. Clothing can become contaminated with toxic dust of depleted uranium (DU), which is very dense, and hence used for counterweights in a civilian context, and in armour-piercing projectiles. DU is not removed by normal laundering; washing with about 6 ounces (170 g) of baking soda in 2 gallons (7.5 l) of water will help to wash it out.[62]
Chemistry[edit]
Sodium bicarbonate is an amphoteric compound. Aqueous solutions are very mildly alkaline due to the formation of carbonic acid and hydroxide ion:
HCO−
3 + H2O → H
2CO
3 + OH−
Sodium bicarbonate can be used as a wash to remove any acidic impurities from a "crude" liquid, producing a purer sample. Reaction of sodium bicarbonate and an acid produces a salt and carbonic acid, which readily decomposes to carbon dioxide and water:
NaHCO3 + HCl → NaCl + H2CO3
H2CO3 → H2O + CO2(g)
Sodium bicarbonate reacts with acetic acid (found in vinegar), producing sodium acetate, water, and carbon dioxide:
NaHCO3 + CH3COOH → CH3COONa + H2O + CO2(g)
Sodium bicarbonate reacts with bases such as sodium hydroxide to form carbonates:
NaHCO3 + NaOH → Na2CO3 + H2O
Sodium bicarbonate reacts with carboxyl groups in proteins to give a brisk effervescence from the formation of CO
2. This reaction is used to test for the presence of carboxylic groups in protein.[citation needed]
Thermal decomposition[edit]
Above 50 °C, sodium bicarbonate gradually decomposes into sodium carbonate, water and carbon dioxide. The conversion is fast at 200 °C:[63]
2 NaHCO3 → Na2CO3 + H2O + CO2
Most bicarbonates undergo this dehydration reaction. Further heating converts the carbonate into the oxide (above 850 °C):[63]
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.
History[edit]
In 1791 French chemist Nicolas Leblanc produced sodium carbonate, also known as soda ash. In 1846 two New York bakers, John Dwight and Austin Church, established the first factory in the United States to produce baking soda from sodium carbonate and carbon dioxide.[64]
Saleratus, potassium or sodium bicarbonate, is mentioned in the novel Captains Courageous by Rudyard Kipling as being used extensively in the 1800s in commercial fishing to prevent freshly caught fish from spoiling.[65]
Production[edit]
Main article: Solvay process
NaHCO3 is mainly prepared by the Solvay process, which is the reaction of sodium chloride, ammonia, and carbon dioxide in water. Calcium carbonate is used as the source of CO2 and the resultant calcium oxide is used to recover the ammonia from the ammonium chloride. The product shows a low purity (75%). Pure product is obtained from sodium carbonate, water, and carbon dioxide as reported in one of the following reactions. It is produced on the scale of about 100,000 tonnes/year (as of 2001).[66]
NaHCO3 may be obtained by the reaction of carbon dioxide with an aqueous solution of sodium hydroxide. The initial reaction produces sodium carbonate:
CO2 + 2 NaOH → Na2CO3 + H2O
Further addition of carbon dioxide produces sodium bicarbonate, which at sufficiently high concentration will precipitate out of solution:
Na2CO3 + CO2 + H2O → 2 NaHCO3
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 → 2 NaHCO3
Mining[edit]
Naturally occurring deposits of nahcolite (NaHCO3) are found in the Eocene-age (55.8–33.9 Mya) Green River Formation, Piceance Basin in Colorado. Nahcolite was deposited as beds during periods of high evaporation in the basin. It is commercially mined using common underground mining techniques such as bore, drum, and longwall mining in a fashion very similar to coal mining. A very small portion is also obtained using in situ leach techniques involving dissolution of the nahcolite by heated water pumped through the nahcolite beds that have previously been mined using the aforementioned techniques. It is then reconstituted through a natural cooling crystallization process. Currently only Tronox (formerly FMC) in the Green River Wyoming basin has successfully commercially solution mined the product.
In popular culture[edit]
Film[edit]
Sodium bicarbonate, as "bicarbonate of soda", was a frequent source of punch lines for Groucho Marx in Marx brothers movies. In Duck Soup, Marx plays the leader of a nation at war. In one scene, he receives a message from the battlefield that his general is reporting a gas attack, and Groucho tells his aide: "Tell him to take a teaspoonful of bicarbonate of soda and a half a glass of water."[67] In A Night at the Opera, Groucho's character addresses the opening night crowd at an opera by saying of the lead tenor: "Signor Lassparri comes from a very famous family. His mother was a well-known bass singer. His father was the first man to stuff spaghetti with bicarbonate of soda, thus causing and curing indigestion at the same time."[68]
See also[edit]
Carbonic acid
Soda bread
List of ineffective cancer treatments
List of minerals
Nahcolite
Natron
Natrona (disambiguation)
Trona
Washing soda
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Jump up ^ Baking soda overdose – All Information. Umm.edu (2009-10-19). Retrieved on 2010-09-24.
Jump up ^ Housecroft, Catherine E.; Sharpe, Alan G. (2008). "Chapter 22: d-block metal chemistry: the first row elements". Inorganic Chemistry, 3rd Edition. Pearson. p. 716. ISBN 978-0-13-175553-6.
Jump up ^ "Science Lab.com". MSDS- Sodium carbonate. sciencelab.com.
^ Jump up to: a b Art, Philadelphia Museum of. "Finishing Techniques in Metalwork".
Jump up ^ "Put a Shine on It". scifun.chem.wisc.edu. Retrieved 2011-03-06.
Jump up ^ Raymond, Jessica (June 10, 2016). "Kitchen Odor Eliminating Candles, Products, and Tricks". cravedujour.com.
Jump up ^ Orcutt, JA. "Depleted Uranium and Health: Facts and Helpful Suggestions". Pharmacology and Toxicology of Uranium Compounds. McGraw-Hill. Retrieved 21 March 2012.
^ Jump up to: a b "Decomposition of Carbonates". General Chemistry Online.
Jump up ^ "Company History". Church & Dwight Co. Archived from the original on 16 October 2011.
Jump up ^ Kipling, Rudyard. Captains Courageous. p. 25.
Jump up ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
Jump up ^ "Duck Soup (1933)". IMDb. Retrieved 4 August 2015.
Jump up ^ "A Night at the Opera (1935)". IMDb. Retrieved 4 August 2015.
External links[edit]
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Sodium compounds
NaAlO2
NaBH4
NaBH3(CN)
NaBO2
NaBiO3
NaBr
NaBrO
NaBrO3
NaCH3COO
NaC6H5CO2
NaC6H4(OH)CO2
NaCN
NaCl
NaClO
NaClO2
NaClO3
NaClO4
NaF
Na2FeO4
NaH
NaHCO3
NaH2PO4
NaHSO3
NaHSO4
NaI
NaIO3
NaIO4
Na5IO6
NaMnO4
NaN3
NaNH2
NaNO2
NaNO3
NaOCN
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NaO3
NaOH
NaPO2H2
NaReO4
NaSCN
NaSH
NaTcO4
NaVO3
Na2CO3
Na2C2O4
Na2CrO4
Na2Cr2O7
Na2GeO3
Na2MnO4
Na3MnO4
Na2MoO4
Na2MoS4
Na2N2O2
Na2O
Na2O2
Na2O(UO3)2
Na2PO3F
Na2S
Na2SO3
Na2SO4
Na2S2O3
Na2S2O4
Na2S2O5
Na2S2O6
Na2S2O7
Na2S2O8
Na2S4O6
Na2Se
Na2SeO3
Na2SeO4
Na2SiO3
Na2Si2O5
Na4SiO4
Na2Te
Na2TeO3
Na2TeO4
Na2Po
Na2Ti3O7
Na2U2O7
NaWO4
Na2Zn(OH)4
Na3N
Na3P
Na3PO4
Na3VO4
Na4Fe(CN)6
Na4P3O7
Na5P3O10
Chemical formulas
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Hydrogen compounds
H3AsO3
H3AsO4
HAt
HSO3F
HBF4
HBr
HBrO
HBrO2
HBrO3
HBrO4
HCl
HClO
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H2CrO4/H2Cr2O7
H2CO3
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HF
HFΟ
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HIO
HIO2
HIO3
HIO4
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HNC
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HNO
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HNO3
H2N2O2
HNO5S
H3NSO3
H2O
H2O2
H2O3
H3PO2
H3PO3
H3PO4
H4P2O7
H5P3O10
H2PtCl6
H2S
H2S2
H2Se
H2SeO3
H2SeO4
H4SiO4
H2SiF6
HSCN
HNSC
H2SO3
H2SO4
H2SO5
H2S2O3
H2S2O6
H2S2O7
H2S2O8
CF3SO3H
H2Te
H2TeO3
H6TeO6
H4TiO4
H2Po
HCo(CO)4
[show]
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Drugs for acid related disorders: Antacids (A02A)
Magnesium (increases motility)
Magnesium carbonate
Magnesium oxide
Magnesium peroxide
Magnesium hydroxide
Magnesium silicate
Aluminium (decreases motility)
Aceglutamide aluminum
Algeldrate
Aluminium phosphate
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Calcium
Calcium carbonate
Calcium silicate
Sodium
Sodium bicarbonate
Combinations and complexes
of aluminium, calcium and magnesium
Almagate
Almasilate
Hydrotalcite
Magaldrate
Authority control
LCCN: sh94006042
GND: 4404786-1
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