| 词条 | Ammonium bromide |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 443525663 | Name = Ammonium bromide | IUPACName = Ammonium bromide | ImageFile = Ammonium bromide.png | ImageSize = 90px | ImageFile2 = Ammonium-bromide-3D-balls.png | ImageSize2 = 170px | ImageName2 = ball-and-stick model of an ammonium cation (left) and a bromide anion (right) |Section1={{Chembox Identifiers | UNII_Ref = {{fdacite|correct|FDA}} | UNII = R0JB3224WS | EC_number = 235-183-8 | InChI = 1/BrH.H3N/h1H;1H3 | SMILES = [Br-].[NH4+] | InChIKey = SWLVFNYSXGMGBS-UHFFFAOYAP | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/BrH.H3N/h1H;1H3 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = SWLVFNYSXGMGBS-UHFFFAOYSA-N | CASNo = 12124-97-9 | CASNo_Ref = {{cascite|correct|CAS}} | RTECS = BO9155000liugoiugiu | PubChem = 25514 | ChEBI_Ref = {{ebicite|changed|EBI}} | ChEBI = 85364 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID=23804 |Section2={{Chembox Properties | Formula = NH4Br | MolarMass = 97.94 g/mol | Appearance = white powder, hygroscopic | MeltingPtC = 235 | BoilingPtC = 452 | Density = 2.429 g/cm3 | Solubility = 60.6 g/100 mL (0 °C) 78.3 g/100 mL (25 °C) 145 g/100 mL (100 °C) | RefractIndex = 1.712 | MagSus = −47.0·10−6 cm3/mol |Section3={{Chembox Structure | CrystalStruct = Isometric |Section7={{Chembox Hazards | GHSPictograms = {{GHSp|GHS07}}[1] | GHSSignalWord = Warning | HPhrases = {{H-phrases|315|319|335}}[1] | PPhrases = {{P-phrases|261|264|271|280|302+352|304+340|305+351+338|312|321|332+313|337+313|362|403+233|405|501}} | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 |Section8={{Chembox Related | OtherAnions = Ammonium fluoride Ammonium chloride Ammonium iodide | OtherCations = Sodium bromide Potassium bromide }} Ammonium bromide, NH4Br, is the ammonium salt of hydrobromic acid. The chemical crystallizes in colorless prisms, possessing a saline taste; it sublimes on heating and is easily soluble in water. On exposure to air it gradually assumes a yellow color because of the oxidation of traces of bromide (Br−) to bromine (Br2). PreparationAmmonium bromide can be prepared by the direct action of hydrogen bromide on ammonia. NH3 + HBr → NH4Br It can also be prepared by the reaction of ammonia with iron(II) bromide or iron(III) bromide, which may be obtained by passing aqueous bromine solution over iron filings. 2 NH3 + FeBr2 + 2 H2O → 2 NH4Br + Fe(OH)2 ReactionsAmmonium bromide is a weak acid with a pKa of ~5 in water. It is an acid salt because the ammonium ion hydrolyzes slightly in water. Ammonium Bromide is strong electrolyte when put in water: NH4Br(s) → NH4+(aq) + Br−(aq) Ammonium bromide decomposes to ammonia and hydrogen bromide when heated at elevated temperatures: NH4Br → NH3 + HBr UsesAmmonium bromide is used for photography in films, plates and papers; in fireproofing of wood; in lithography and process engraving; in corrosion inhibitors; and in pharmaceutical preparations.[2] References1. ^1 {{Sigma-Aldrich|id=380008|name=Ammonium bromide|accessdate=2013-07-20}} yu2. ^Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}} 3 : Ammonium compounds|Bromides|Nonmetal halides |
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