Sodium bromide: Difference between revisions

{{short description|Inorganic salt: NaBr}}

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| verifiedrevid = 422030388

| Name = Sodium bromide

| ImageFile = Sodium-bromide-3D-ionic.png

| ImageSize = 150px

| ImageName = 3D model of sodium bromide

| ImageFile1 = Sodium bromide.jpg

| ImageSize1 = 200px

| ImageName1 = Sodium bromide powder

| IUPACName = Sodium bromide

| OtherNames =

| SystematicName =

| index_label = anhydrous

| index1_label = dihydrate

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChEMBL_Ref = {{ebicite|correct|EBI}}

| ChEMBL = 1644694

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo1 = 13466-08-5

| CASNo1_Ref = {{cascite|changed|CAS}}

| PubChem = 253881

| RTECS = VZ3150000

}}

| Formula = NaBr

| Na=1 | Br=1

| Appearance = White powder, [[hygroscopic]]

| Density = 3.21 g/cm³ (anhydrous)<br> 2.18 g/cm³ (dihydrate)

| Solubility = 71.35 g/100 mL (−20 °C)<br> 79.52 g/100 mL (0 °C)<br> 94.32 g/100 mL (25 °C)<ref name=chemister>{{cite web | url=http://chemister.ru/Database/properties-en.php?dbid=1&id=714 | title=Sodium bromide}}</ref><br> 104.9 g/100 mL (40 °C)<br> 116.2 g/100 mL (100 °C)<ref name=sioc>{{cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1919|title = Solubilities of Inorganic and Organic Compounds|url = https://archive.org/details/solubilitiesino01seidgoog|publisher = D. Van Nostrand Company|edition = 2nd}}</ref>

| Solubility1 = 17.3 g/100 g (0 °C)<br> 16.8 g/100 g (20 °C)<br> 16.1 g/100 g (40 °C)<br> 15.3 g/100 g (60 °C)<ref name=chemister />

| Solvent1 = methanol

| Solubility2 = 2.45 g/100 g (0 °C)<br> 2.32 g/100 g (20 °C)<br> 2.29 g/100 g (30 °C)<br> 2.35 g/100 g (70 °C)<ref name=chemister />

| Solvent2 = ethanol

| Solubility3 = 19.3 g/100 g (18 °C)<br> 19.4 g/100 g (25 °C)<ref name=chemister />

| Solvent3 = formic acid

| Solubility4 = 38.7 g/100 g (20 °C)<ref name=chemister />

| Solvent4 = glycerol

| Solubility5 = 3.2 g/100 g (10.3 °C)<ref name=chemister />

| Solvent5 = dimethylformamide

| SolubleOther = Soluble in [[ethanol|alcohol]], liquid [[ammonia]], [[pyridine]], [[hydrazine]], [[sulfur dioxide|{{chem2|SO2}}]]<br />Insoluble in [[acetone]], [[acetonitrile]]<ref name=chemister />

| MeltingPtC = 747

| MeltingPt_notes = <br> (anhydrous)<br> {{convert|36|C|F K}}<br> (dihydrate) decomposes<ref name=pphoic>{{cite book|last = Pradyot|first = Patnaik|year = 2003|title = Handbook of Inorganic Chemicals|publisher = The McGraw-Hill Companies, Inc.|isbn = 978-0-07-049439-8}}</ref>

| BoilingPtC = 1390

| BoilingPt_ref = <ref name=pphoic />

| RefractIndex = 1.6428 (24 °C)<br> ''n''_{[[Krypton fluoride laser|KrF]]} = 1.8467 (24 °C)<br> ''n''_{[[Helium–neon laser|He–Ne]]} = 1.6389 (24 °C)<ref>{{cite web|url = http://refractiveindex.info/?shelf=main&book=NaBr&page=Li|title = Refractive index of NaBr (Sodium bromide) - Li|website = refractiveindex.info|first = Mikhail|last = Polyanskiy|access-date = 2014-06-11}}</ref>

| Viscosity = 1.42 cP (762 °C)<br> 1.08 cP (857 °C)<br> 0.96 cP (937 °C)<ref name=chemister />

| VaporPressure = 1 torr (806 °C)<br> 5 torr (903 °C)<ref name=pphoic />

| ThermalConductivity = 5.6 W/(m·K) (150 K)<ref name=korde>{{cite web|url = http://www.korth.de/index.php/162/items/23.html|title = Sodium Bromide (NaBr)|website = korth.de|publisher = Korth Kristalle GmbH|access-date = 2014-06-11|archive-date = 2014-07-14|archive-url = https://web.archive.org/web/20140714185855/http://www.korth.de/index.php/162/items/23.html|url-status = dead}}</ref>

| MagSus = &minus;41.0·10⁻⁶ cm³/mol

}}

| Section3 =

| Section4 = {{Chembox Structure

| CrystalStruct = Cubic

| LattConst_a = 5.97 Å<ref name=korde />

}}

| Section5 = {{Chembox Thermochemistry

| DeltaHf = −361.41 kJ/mol<ref name=chemister />

| DeltaGf = −349.3 kJ/mol<ref name=chemister />

| Entropy = 86.82 J/(mol·K)<ref name=chemister />

| HeatCapacity = 51.4 J/(mol·K)<ref name=chemister />

}}

| Section6 = {{Chembox Pharmacology

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| Legal_AU = S4

| Legal_AU_comment = /S5

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| ExternalSDS = [http://www.sciencelab.com/msds.php?msdsId=9927262 External MSDS]

| FlashPtC = 800

| LD50 = 3500 mg/kg (rats, oral)

| NFPA-H = 2

| NFPA-F = 0

| NFPA-R = 0

| NFPA_ref = <ref name=scl />

}}

| OtherAnions = {{ubl|[[Sodium fluoride]]|[[Sodium chloride]]|[[Sodium iodide]]|[[Sodium astatide]]}}

| OtherCations = {{ubl|[[Lithium bromide]]|[[Potassium bromide]]|[[Rubidium bromide]]|[[Caesium bromide]]|[[Francium bromide]]}}

}}

'''Sodium bromide''' is an [[inorganic compound]] with the formula {{chem2|NaBr|auto=1}}. It is a high-melting white, crystalline solid that resembles [[sodium chloride]]. It is a widely used source of the [[bromide ion]] and has many applications.<ref name=Ullmann>Michael J. Dagani, Henry J. Barda, Theodore J. Benya, David C. Sanders "Bromine Compounds" in ''Ullmann's Encyclopedia of Industrial Chemistry'' Wiley-VCH, Weinheim, 2000. {{doi|10.1002/14356007.a04_405}}</ref>

NaBr crystallizes in the same [[Cubic crystal system|cubic]] motif as [[NaCl]], [[NaF]] and [[NaI]]. The [[anhydrous]] salt crystallizes above 50.7&nbsp;°C.<ref name=Ullmann/> [[wikt:Dihydrate|Dihydrate]] salt ({{chem2|NaBr*2H2O}}) crystallize out of water solution below 50.7&nbsp;°C.<ref name="cec">{{cite book|last=Eagleson|first=Mary (translated by)|title=Concise Encyclopedia Chemistry|url=https://archive.org/details/conciseencyclope00eagl|url-access=registration|date=1994|publisher=Walter De Gruyter|location=Berlin [u.a.]|isbn=9783110114515|pages=996|edition=Illustrated, revised, English language}}</ref>

Sodium bromide can be used as a source of the [[chemical element]] [[bromine]]. This can be accomplished by treating an [[aqueous solution]] of NaBr with [[chlorine]] gas:

:{{chem2|2 NaBr + Cl2 → Br2 + 2 NaCl}}

Sodium bromide is the most useful inorganic bromide in industry.<ref name=Ullmann/> It is also used as a catalyst in TEMPO-mediated oxidation reactions.<ref>{{cite journal | doi=10.1007/s10570-009-9381-2 | volume=17 | issue=2 | title=Water dispersion of cellulose II nanocrystals prepared by TEMPO-mediated oxidation of mercerized cellulose at pH 4.8 | journal=Cellulose | pages=279–288|year = 2010|last1 = Hirota|first1 = Masayuki| last2=Tamura | first2=Naoyuki | last3=Saito | first3=Tsuguyuki | last4=Isogai | first4=Akira | s2cid=97264888}}</ref>

{{see also|Potassium bromide#Applications}}

[[File:Bromo seltzer newspaper.png|thumbnail|left|Bromo-Seltzer newspaper ad (1908)]]

Also known as Sedoneural, sodium bromide has been used as a [[hypnotic]], [[anticonvulsant]], and [[sedative]] in [[medicine]], widely used as an [[anticonvulsant]] and a [[sedative]] in the late 19th and early 20th centuries. Its action is due to the bromide ion, and for this reason [[potassium bromide]] is equally effective. In 1975, bromides were removed from drugs in the U.S. such as [[Bromo-Seltzer]] due to toxicity.<ref>{{cite web|url = http://www.canine-epilepsy.com/Bromide.html|title = Bromide: Potassium & Sodium|website = canine-epilepsy.com|publisher = Canine-Epilepsy Resources|date = 2011-05-31|access-date = 2014-06-11|archive-date = 2014-03-06|archive-url = https://web.archive.org/web/20140306104721/http://www.canine-epilepsy.com/Bromide.html|url-status = dead}}</ref>

:NaBr + RCl → RBr + NaCl (R = [[alkyl]])

Once a large need in [[photography]], but now shrinking, the photosensitive salt [[silver bromide]] is prepared using NaBr.

Sodium bromide is used in conjunction with chlorine as a disinfectant for hot tubs and swimming pools.

Because of its high [[solubility]] in water (943.2 g/L or 9.16 mol/L, at 25 °C) sodium bromide is used to prepare dense [[drilling fluid]]s used in [[oil well]]s to compensate a possible overpressure arising in the fluid column and to counteract the associated trend to [[Blowout (well drilling)|blow out]]. The presence of the sodium [[cation]] also causes the [[bentonite]] added to the drilling fluid to swell, while the high [[ionic strength]] induces bentonite [[flocculation]].

NaBr has a very low toxicity with an oral {{LD50}} estimated at 3.5 g/kg for rats.<ref name=scl>{{cite web|url = http://www.sciencelab.com/msds.php?msdsId=9927262|title = Sodium bromide MSDS|website = sciencelab.com|publisher = Sciencelab.com, Inc.|date = 2013-05-21|access-date = 2014-06-11|format = PDF|archive-date = 2013-10-07|archive-url = https://web.archive.org/web/20131007042442/http://www.sciencelab.com/msds.php?msdsId=9927262|url-status = dead}}</ref> However, this is a single-dose value. Bromide ion is a cumulative toxin with a relatively long [[half-life]] (in excess of a week in humans): see [[potassium bromide]].

{{reflist}}

{{Commons category|Sodium bromide}}

* [https://www.who.int/environmental_health_emergencies/events/Angola%20cause%20finding%20mission%20report%20Exeutive%20Summary%20for%20Web%20V190308.pdf Bromide Poisoning in Angola]

{{bromides}}

{{Hypnotics and sedatives}}

{{Anticonvulsants}}

{{GABAAR PAMs}}

{{Authority control}}

[[Category:GABAA receptor positive allosteric modulators]]

[[Category:Sedatives]]

[[Category:Alkali metal bromides]]

[[Category:Rock salt crystal structure]]