Difference between revisions of "Barium ferrate"
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| − | | | + | | Name = Barium ferrate |
| + | | Reference = | ||
| + | | IUPACName = Barium ferrate | ||
| + | | PIN = | ||
| + | | SystematicName = Barium ferrate (VI) | ||
| + | | OtherNames = Barium ferrate(2-) | ||
| + | <!-- Images --> | ||
| + | | ImageFile = Ferratb.png | ||
| + | | ImageSize = 250 | ||
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| + | | ImageCaption = Dry barium ferrate | ||
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| + | <!-- Sections --> | ||
| + | | Section1 = {{Chembox Identifiers | ||
| + | | 3DMet = | ||
| + | | Abbreviations = | ||
| + | | SMILES = | ||
| + | }} | ||
| + | | Section2 = {{Chembox Properties | ||
| + | | AtmosphericOHRateConstant = | ||
| Appearance = Pinkish-brown powder | | Appearance = Pinkish-brown powder | ||
| − | | | + | | BoilingPt = |
| + | | BoilingPtC = | ||
| + | | BoilingPt_ref = | ||
| + | | BoilingPt_notes = Decomposes | ||
| Density = | | Density = | ||
| − | | | + | | Formula = BaFeO<sub>4</sub> |
| + | | HenryConstant = | ||
| + | | LogP = | ||
| + | | MolarMass = 257.17 g/mol | ||
| + | | MeltingPt = | ||
| MeltingPtC = | | MeltingPtC = | ||
| − | | | + | | MeltingPt_ref = |
| − | | | + | | MeltingPt_notes = Decomposes |
| − | + | | Odor = Odorless | |
| − | | | + | |
| pKa = | | pKa = | ||
| − | | VaporPressure = | + | | pKb = |
| + | | Solubility = Insoluble | ||
| + | | SolubleOther = Slowly reacts with alcohols<br>Insoluble in [[acetone]], [[acetonitrile]], [[dichloromethane]] | ||
| + | | Solvent = | ||
| + | | VaporPressure = ~0 mmHg | ||
| + | }} | ||
| + | | Section3 = {{Chembox Structure | ||
| + | | Coordination = | ||
| + | | CrystalStruct = | ||
| + | | MolShape = | ||
}} | }} | ||
| − | | | + | | Section4 = {{Chembox Thermochemistry |
| + | | DeltaGf = | ||
| + | | DeltaHc = | ||
| DeltaHf = | | DeltaHf = | ||
| − | | Entropy = | + | | Entropy = |
| + | | HeatCapacity = | ||
}} | }} | ||
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| − | | | + | | FrictionSens = |
| + | | DetonationV = | ||
| + | | REFactor = | ||
}} | }} | ||
| − | | | + | | Section6 = {{Chembox Hazards |
| − | | | + | | AutoignitionPt = Non-flammable |
| − | | | + | | ExploLimits = Non-explosive |
| + | | ExternalMSDS = None | ||
| + | | FlashPt = Non-flammable | ||
| + | | LD50 = | ||
| + | | LC50 = | ||
| + | | MainHazards = Oxidizer | ||
| + | | NFPA-F = | ||
| + | | NFPA-H = | ||
| + | | NFPA-R = | ||
| + | | NFPA-S = | ||
| + | }} | ||
| + | | Section7 = {{Chembox Related | ||
| + | | OtherAnions = | ||
| + | | OtherCations = | ||
| + | | OtherFunction = [[Potassium ferrate]]<br>[[Sodium ferrate]] | ||
| OtherFunction_label = ferrates | | OtherFunction_label = ferrates | ||
| − | | | + | | OtherCompounds = |
}} | }} | ||
}} | }} | ||
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=== Chemical === | === Chemical === | ||
It is a very potent oxidizer, but its insolubility makes it extremely stable for a ferrate. It is not known for decomposing just from contact with air, as [[potassium ferrate]] often does. It, however, reacts with acids stronger than ferric acid, such as all strong acids and several mid-strength acids such as phosphoric, liberating the extremely unstable ferric acid which is a powerful oxidizer. | It is a very potent oxidizer, but its insolubility makes it extremely stable for a ferrate. It is not known for decomposing just from contact with air, as [[potassium ferrate]] often does. It, however, reacts with acids stronger than ferric acid, such as all strong acids and several mid-strength acids such as phosphoric, liberating the extremely unstable ferric acid which is a powerful oxidizer. | ||
| + | |||
| + | Barium ferrate and barium sulfate are isomorphic and, for example when coprecipitated, form mixed crystals (solid solution) which are light brown to brick red in appearance.<ref>''Gmelins Handbuch der anorganischen Chemie, Barium,'' Verlag Chemie GmbH, Berlin, 8th edition '''1932''', p. 267</ref> | ||
== Availability == | == Availability == | ||
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== Preparation == | == Preparation == | ||
| − | There are several methods of ferrate synthesis. The most practical are the electrolytic method and the hypochlorite method. In the electrolytic method, a solution of an alkali metal hydroxide is electrolyzed with iron electrodes. In the hypochlorite method, salts of trivalent iron are oxidized with hypochlorites in solution. A weak solution of ferrate can be made by melting [[potassium nitrate]], [[iron (III) oxide]] and [[potassium hydroxide]] together, then grinding the cooled melt in a mortar and dissolving it in water. | + | There are several methods of ferrate synthesis. The most practical are the electrolytic method and the hypochlorite method. In the electrolytic method, a solution of an alkali metal hydroxide is electrolyzed with iron electrodes. In the hypochlorite method, salts of trivalent iron are oxidized with hypochlorites in solution. A weak solution of ferrate can be made by melting [[potassium nitrate]], [[iron(III) oxide]] and [[potassium hydroxide]] together, then grinding the cooled melt in a mortar and dissolving it in water. |
In any case, if you have '''any''' form of solvated ferrate ion, you can immediately precipitate barium ferrate by adding any soluble barium compound. Barium ferrate does not react with filter paper in neutral and higher pH, so you can use it. | In any case, if you have '''any''' form of solvated ferrate ion, you can immediately precipitate barium ferrate by adding any soluble barium compound. Barium ferrate does not react with filter paper in neutral and higher pH, so you can use it. | ||
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== Projects == | == Projects == | ||
* Make oxygen and chlorine in [[Kipp's apparatus]] or a similar one; | * Make oxygen and chlorine in [[Kipp's apparatus]] or a similar one; | ||
| + | * Make other ferrates | ||
== Handling == | == Handling == | ||
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=== Storage === | === Storage === | ||
| − | Barium ferrate can be stored in any container, such as a jar. | + | Barium ferrate can be stored in any container, such as a jar. However, carbon dioxide and moisture will slowly decompose it, so it's best to seal the container. |
=== Disposal === | === Disposal === | ||
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[[Category:Oxidizing agents]] | [[Category:Oxidizing agents]] | ||
[[Category:Materials unstable in acidic solution]] | [[Category:Materials unstable in acidic solution]] | ||
| + | [[Category:Air-sensitive materials]] | ||
Latest revision as of 16:43, 30 July 2023
 Dry barium ferrate
| |
| Names | |
|---|---|
| IUPAC name
Barium ferrate
| |
| Systematic IUPAC name
Barium ferrate (VI) | |
| Other names
Barium ferrate(2-)
| |
| Properties | |
| BaFeO4 | |
| Molar mass | 257.17 g/mol |
| Appearance | Pinkish-brown powder |
| Odor | Odorless |
| Melting point | Decomposes |
| Boiling point | Decomposes |
| Insoluble | |
| Solubility | Slowly reacts with alcohols Insoluble in acetone, acetonitrile, dichloromethane |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | None |
| Flash point | Non-flammable |
| Related compounds | |
| Related ferrates
|
Potassium ferrate Sodium ferrate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Barium ferrate is a compound with a formula of BaFeO4. This is a stable barium salt of ferric acid, which itself is too unstable to exist in aqueous solution. It is a pinkish-brown crystalline or powder-like solid that is well known as the most stable ferrate and the easiest to synthesize and isolate. It is a strong oxidizer.
Contents
Properties
Physical
It is pinkish-brown powder that does not dissolve in water or other solvents.
Chemical
It is a very potent oxidizer, but its insolubility makes it extremely stable for a ferrate. It is not known for decomposing just from contact with air, as potassium ferrate often does. It, however, reacts with acids stronger than ferric acid, such as all strong acids and several mid-strength acids such as phosphoric, liberating the extremely unstable ferric acid which is a powerful oxidizer.
Barium ferrate and barium sulfate are isomorphic and, for example when coprecipitated, form mixed crystals (solid solution) which are light brown to brick red in appearance.[1]
Availability
Barium ferrate is not used in any household products, and reagent stores rarely sell it. However, it is easy to synthesize and isolate.
Preparation
There are several methods of ferrate synthesis. The most practical are the electrolytic method and the hypochlorite method. In the electrolytic method, a solution of an alkali metal hydroxide is electrolyzed with iron electrodes. In the hypochlorite method, salts of trivalent iron are oxidized with hypochlorites in solution. A weak solution of ferrate can be made by melting potassium nitrate, iron(III) oxide and potassium hydroxide together, then grinding the cooled melt in a mortar and dissolving it in water.
In any case, if you have any form of solvated ferrate ion, you can immediately precipitate barium ferrate by adding any soluble barium compound. Barium ferrate does not react with filter paper in neutral and higher pH, so you can use it.
Projects
- Make oxygen and chlorine in Kipp's apparatus or a similar one;
- Make other ferrates
Handling
Safety
Barium ferrate is mostly non-toxic, being insoluble. The products of its decomposition, however, aren't so safe: it is prone to forming barium hydroxide or salts, which are toxic. Barium ferrate should not come in contact with flammable organic compounds. Do not ingest barium ferrate, because it can be decomposed by your stomach acid and be digested into soluble and toxic barium chloride.
Storage
Barium ferrate can be stored in any container, such as a jar. However, carbon dioxide and moisture will slowly decompose it, so it's best to seal the container.
Disposal
Use sulfuric acid to neutralize barium ferrate. It will release oxygen from the compound and bind the toxic barium into the safe barium sulfate, which can be thrown away with normal garbage.
Heating barium ferrate causes it to decompose. Treating the resulting slag with sulfuric acid will allow to remove the toxic barium ions.
References
- ↑ Gmelins Handbuch der anorganischen Chemie, Barium, Verlag Chemie GmbH, Berlin, 8th edition 1932, p. 267
